HỆ THỐNG BÀI TẬP BẰNG TIẾNG ANH
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Ths Nguyễn Thanh Tú eBook Collection
XÂY DỰNG HỆ THỐNG BÀI TẬP HƯỚNG DẪN HỌC SINH HỌC CÁC MÔN KHOA HỌC TỰ NHIÊN BẰNG TIẾNG ANH TRONG BỘ MÔN HÓA HỌC 10, 11 WORD VERSION | 2021 EDITION ORDER NOW / CHUYỂN GIAO QUA EMAIL TAILIEUCHUANTHAMKHAO@GMAIL.COM
Tài liệu chuẩn tham khảo Phát triển kênh bởi Ths Nguyễn Thanh Tú Đơn vị tài trợ / phát hành / chia sẻ học thuật : Nguyen Thanh Tu Group Hỗ trợ trực tuyến Fb www.facebook.com/DayKemQuyNhon Mobi/Zalo 0905779594
Sáng kiến kinh nghiệm năm học 2018 - 2019
MỤC LỤC THÔNG TIN CHUNG VỀ SÁNG KIẾN......................................................................
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I. Điều kiện, hoàn cảnh tạo ra sáng kiến........................................................................
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II. Mô tả giải pháp.........................................................................................................
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1. Mô tả giải pháp trước khi tạo ra sáng kiến................................................................
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1.1. Vấn đề sử dụng tiếng anh trong việc giảng dạy các môn khoa học trên
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1.2. Vấn đề học Toán và các môn KHTN bằng Tiếng Anh ở Nam Định...........
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2. Mô tả giải pháp sau khi tạo ra sáng kiến...................................................................
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2.1. Giai đoạn 1: Một số thuật ngữ cơ bản.........................................................
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2.1.1 Ngôn ngữ toán học………………………………………………..
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2.1.2. Ngôn ngữ hóa học cơ bản………………………………………
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O
thế giới và tại Việt Nam……………………………………………………….
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2.1.2.2. Tên axit và ion tương ứng................................................
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2.1.2.3. Tên bazo và một số chất hóa học điển hình.......................
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2.1.3. Các thuật ngữ dùng trong phòng thí nghiệm……………………..
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2.1.3.1. Một số dụng cụ hóa học....................................................
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N
H
Ơ
N
2.1.2.1. Tên nguyên tố trong Tiếng Anh.......................................
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2.1.3.3. Các phương pháp thu khí..................................................
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2.1.4. Một số loại phản ứng hay gặp …………………………………..
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2.1.5. Một số khái niệm chung hay dùng ………………………………..
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2.1.6. Một số lời dẫn hay dùng ………………………………………….
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2.2. Giai đoạn 2. Một số ví dụ về cách trình bày lời giải cho bài tập hóa học…….
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2.2.1. Một số ví dụ về bài tập nêu hiện tượng............................................
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KÈ
M
Q
U
Y
2.1.3.2. Một số thao tác thí nghiệm………………………………
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3. Các chuyên đề bài tập……………………………………………………………….
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3.1. Một số chuyên đề thuộc chương trình lớp 10……………………………..
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D
ẠY
2.2.2. Một số ví dụ về bài tập định lượng..................................................
3.1.1. Atoms-The periodic table of chemical element and the periodic law- Chemical bonding (Nguyên tử- Bảng tuần hoàn các nguyên tố hóa học- Liên kết hóa học)…………………………………..
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3.1.2. Oxidation- Reduction reactions; Rates of reaction and Chemical eqilibrium (Phản ứng oxi hóa – khử; Tốc độ phản ứng và Cân bằng hóa học )............................................................................... Trang 2
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Sáng kiến kinh nghiệm năm học 2018 - 2019
3.1.3. Halogen goup – Oxigen,sunfur ( Nhóm halogen; Nhóm oxi39
3.2. Một số chuyên đề thuộc chương trình lớp 11…………………………….
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3.2.1. Chuyên đề: Dissociation ( Sự điện li)…………………………...
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3.2.2. Nitrogen – phosphorus (Nhóm Nito- Photpho)…………………
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3.2.3. Carbon- Silicic (Nhóm Cacbon- silic)…………………………..
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3.2.4. Fudamentals of organic chemistry (Đại cương hóa học hữu cơ)…
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3.3. Một số đề kiểm tra minh họa……………………………………………
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III. Hiệu quả do sáng kiến đem lại:..............................................................................
124
1. So sánh và đối chứng...............................................................................................
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2. Hiệu quả về mặt kinh tế..........................................................................................
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3. Hiệu quả về mặt xã hội……………………………………………………………..
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D
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KÈ
M
Q
U
Y
N
H
Ơ
N
O
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lưu huỳnh)………………………………………………………………
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Sáng kiến kinh nghiệm năm học 2018 - 2019
XÂY DỰNG HỆ THỐNG BÀI TẬP HƯỚNG DẪN HỌC SINH HỌC CÁC MÔN KHOA HỌC TỰ NHIÊN BẰNG TIẾNG ANH TRONG BỘ MÔN HÓA HỌC Giáo viên: Phạm Thị Dung
I. ĐIỀU KIỆN, HOÀN CẢNH TẠO RA SÁNG KIẾN
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Tổ Vật lí –Hóa Học- Công nghệ, trường THPT Nguyễn Khuyến
- Thực hiện Nghị quyết Đại hội Đảng lần thứ XI, đặc biệt là Nghị quyết Trung ương
số 29-NQ/TW ngày 04 tháng 11 năm 2013 về đổi mới căn bản, toàn diện giáo dục và đào tạo, đáp ứng yêu cầu công nghiệp hóa, hiện đại hóa trong điều kiện kinh tế thị trường định
O
hướng xã hội chủ nghĩa và hội nhập quốc tế.
- Theo công văn số 1327/SGDĐT-GDTrH ngày 27/10/2014 của Sở Giáo dục và Đào
N
tạo về việc triển khai dạy các môn khoa học tự nhiên bằng tiếng Anh năm học
2014-
Ơ
2015; công văn số 32/SGDĐT-GDTrH ngày 15/01/2015 của Sở Giáo dục và Đào tạo về việc hướng dẫn Hội thảo các môn khoa học tự nhiên (Toán, Lý, Hóa hoặc Sinh) bằng tiếng
H
Anh năm học 2014-2015. Các giáo viên tham gia phải hoàn thành 2 nội dung: Báo cáo về
N
kinh nghiệm soạn giảng, khai thác tài liệu, sử dụng phần mềm, bồi dưỡng năng lực tiếng
Y
Anh,...và dạy minh họa 01 tiết học (45 phút) bằng tiếng Anh.
U
- Tiếp theo đó, ngày 12/11/2015 Sở Giáo dục và Đào tạo ra công văn số 1304/SGDĐT-GDTrH về việc hướng dẫn giảng dạy, tổ chức Hội giảng và Hội thi Toán và
Q
các môn KHTN bằng tiếng Anh năm học 2015-2016. Và đặc biệt, ngày 04/12/2015 Sở Giáo
M
dục và Đào tạo ra công văn số 1413/SGDĐT-GDTrH về việc triển khai dạy Toán và các môn Khoa học khác bằng tiếng Anh từ năm học 2015-2016 hướng đến phát triển lâu dài và
KÈ
bền vững, các nhà trường và thầy cô giảng dạy có thể thực hiện nâng dần theo từng năm học các mức độ giảng dạy, cụ thể là:
ẠY
+ Mức 1: giáo viên giảng dạy trên lớp, giao tiếp bằng tiếng Việt là chủ yếu;
giao bài tập về nhà hay bài tập nhóm để học sinh thực hành bằng tiếng Anh; giáo viên sửa
D
bài tập, từng bước giao tiếp bằng tiếng Anh. + Mức 2: giáo viên giảng dạy trên lớp kết hợp tiếng Việt với tiếng Anh khi
giao tiếp với học sinh; trao đổi, tổ chức hoạt động bằng tiếng Anh; học sinh dùng tiếng Anh để ghi chép và thực hiện giải các bài tập, giáo viên sửa bài tập bằng tiếng Anh. + Mức 3: thực hiện giảng dạy và tổ chức các hoạt động hoàn toàn bằng tiếng Anh.
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- Theo công văn số 1367/SGDĐT-GDTrH ngày 03/10/2018 về việc tổ chức Hội thảo- Hội thi giải Toán và các môn KHTN bằng tiếng Anh năm học 2018-2019 của Sở GDĐT Nam Định - Như vậy, có thể nói Sở GDĐT Nam Định đã rất quan tâm, hướng dẫn và khuyến khích các trường TH, THCS, THPT trong toàn tỉnh triển khai giảng dạy song ngữ Việt-Anh.
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Tuy vậy, việc thực hiện vẫn còn mang tính đơn lẻ, chuyên biệt ở một số trường trọng điểm. II. MÔ TẢ GIẢI PHÁP 1. Mô tả giải pháp trước khi tạo ra sáng kiến
1.1. Vấn đề sử dụng tiếng anh trong việc giảng dạy các môn khoa học trên thế
O
giới và tại Việt Nam
- Trên thế giới hiện có khoảng 60 nước và vùng lãnh thổ sử dụng tiếng Anh là ngôn
N
ngữ chính thức. Trong đó có nhiều nước sử dụng tiếng Anh cho việc dạy học các môn khoa
Ơ
học ở nhà trường phổ thông như Ấn Độ, Trung Quốc, Hồng Kông, Philippines, Singapore, Ireland, Wales, Scotland, Canada, Jamaica, Mỹ, Peurto Rico, Liberia, Nam Phi, Zimbabwe,
H
New Zealand, Úc, Isarel, Malaysia, Brunei, Costa Rica, Sri Lanka, … Trường Đại học
N
Nanchang (Trung Quốc) đã nghiên cứu sử dụng chiến lược dạy học hoá học hữu cơ bằng
Y
tiếng Anh. Trường Đại học Sydney đã có nhiều nghiên cứu phương pháp dạy học khoa học
U
bằng tiếng Anh.
- Ở Việt Nam, chương trình mục tiêu quốc gia Giáo dục và Đào tạo năm 2012–2015
Q
đã được thực hiện hiệu quả. Việt Nam hiện đang triển khai các chương trình đào tạo tiếng
M
nước ngoài, với mục tiêu đến năm 2020, sinh viên tốt nghiệp đại học có thể giao tiếp và sử dụng ngoại ngữ thành thạo. Điều này sẽ mở thêm cơ hội việc làm cho thanh niên Việt Nam
KÈ
không chỉ ở trong nước mà còn tại các quốc gia cộng đồng ASEAN. - Theo Đề án phát triển hệ thống trường THPT chuyên và Đề án dạy ngoại ngữ các
ẠY
trường trung học của Bộ Giáo dục và Đào tạo, trường THPT chuyên sẽ dạy các môn khoa học tự nhiên bằng tiếng Anh. Bắt đầu năm học 2011–2012, dạy bằng tiếng Anh môn Tin
D
học và Toán học, sau năm 2015 là các môn Vật lí, Hoá học và Sinh học. Mục tiêu đến năm 2020, có 50% học sinh đạt bậc 3 về ngoại ngữ theo tiêu chí của Hiệp hội các tổ chức khảo thí ngoại ngữ châu Âu.
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Sáng kiến kinh nghiệm năm học 2018 - 2019
1.2. Vấn đề học dạy Toán và các môn KHTN bằng Tiếng Anh ở tỉnh Nam Định Ở tỉnh Nam Định, trường THPT chuyên Lê Hồng Phong là một trong những trường tiên phong trong cả nước về việc dạy học các môn khoa học bằng tiếng Anh. Ở đây, có rất nhiều giáo viên có năng lực chuyên môn giỏi, lại có trình độ tiếng Anh chuyên ngành tốt. Đây là một điều kiện thuận lợi để các giáo viên trong tỉnh có thể học tập kinh nghiệm.
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Mặt khác, Sở GD – ĐT Nam Định đã và đang rất quan tâm đến việc thực hiện đề án dạy môn KHTN bằng tiếng Anh. Liên tiếp trong các năm học 2014-2015; 2015-2016 và
2017-2018 Sở GDĐT Nam Định đã tổ chức các Hội thi dạy và học Toán và các môn KHTN bằng Tiếng Anh ở cả giáo viên và học sinh cho trường THPT chuyên và các trường THPT không chuyên trong cả tỉnh. Điều này đã thúc đẩy quá trình nghiên cứu môn tiếng Anh chuyên ngành và áp dụng vào trong thực tiễn giảng dạy và bồi dưỡng chuyên môn của các
O
giáo viên đồng thời thúc đẩy, tạo động lực cho các học sinh giỏi các môn KHTN có nhu
N
cầu, mong muốn học tiếng Anh chuyên nghành, muốn sử dụng tiếng Anh là công cụ để học
Ơ
tập môn học mà mình yêu thích.
Trường THPT Nguyễn Khuyến là một trong những trường có chất lượng học tập
H
môn Tiếng Anh của học sinh tương đối tốt. Ban lãnh đạo nhà trường luôn tạo điều kiện về
N
vật chất và thời gian cho việc nâng cao chuyên môn.
Tuy nhiên, ở thời điểm hiện tại, việc giảng dạy các môn khoa học bằng tiến anh nói
Y
chung và môn hóa học bằng tiến anh nói riêng còn gặp nhiều khó khăn. Khó khăn trước hết là
U
ở tài liệu hướng dẫn. Tính đến thời điểm hiện tại, các tài liệu dùng để dạy học Khoa học nói
Q
chung và Hoá học nói riêng bằng tiếng Anh ở các trường THPT và Đại học, gần như chưa được xuất bản ở Việt Nam. Kiến thức môn Hóa Học ở các trường THPT không chuyên khác với ở
M
trường THPT chuyên nên việc sử dụng các tài liệu của trường chuyên chỉ có tính tham khảo
KÈ
không thể áp dụng được. Các tài liệu trên mạng internet còn rất ít, chủ yếu là sách nước ngoài. Việc tham khảo ý kiến của các giáo viên dạy môn tiếng Anh cũng bị hạn chế vì lĩnh vực
ẠY
chuyên ngành Hóa học có nhiều thuật ngữ khó hiểu và đặc thù riêng. Tiếp theo, trình độ tiếng Anh của giáo viên còn yếu, chưa đáp ứng sự trôi chảy,
D
mạch lạc khi giảng dạy; trình độ tiếng Anh của học sinh cũng không đồng đều. Học sinh và phụ huynh học sinh chỉ có mục đích chính là học để thi đỗ Đại Học nên với các học sinh chọn khối A hay B thì việc học tiếng Anh ít được đầu tư công sức. Hơn nữa việc học các môn KHTN bằng tiếng Anh có tính phức tạp hơn tiếng Anh thông dụng nên đa phần học sinh ngại khó.
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Các giáo viên chưa thật mạnh dạn biên soạn và dạy theo chuyên đề vì e ngại sự không tương thích với chương trình do Bộ Giáo dục và Đào tạo ban hành. Cuối cùng, thời gian giành cho việc dạy học các môn khoa học bằng tiếng Anh chưa có trong chương trình qui định. Việc đảm bảo các kiến thức cơ bản và các kĩ năng cần thiết trong dạy học môn Hóa học bằng tiếng Việt vẫn là yêu cầu cơ bản
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Trước những vấn đề trên và cũng qua 2 đợt hướng dẫn học sinh cùng một số tiết dự
giờ đồng nghiệp tôi xin đưa ra một số nội dung nhằm định hướng và giúp đỡ giáo viên và học sinh có niềm đam mê trong việc học Hóa học bằng tiếng Anh. 2. Mô tả giải pháp sau khi tạo ra sáng kiến
Có thể nói rằng dạy và học các môn khoa học tự nhiên, trong đó có môn hóa là vấn
O
đề cực kì khó khăn đối với cả giáo viên và học sinh, nên cần có một lộ trình rõ ràng, từng giai đoạn, từ những cái đơn giản nhất đến những cái phức tạp. Để làm được điều đó, tôi đã
N
thực hiện qua các giai đoạn.
Ơ
2.1. Giai đoạn một (Làm quen với tiếng Anh trong Hóa học)
Trước hết, giáo viên cung cấp cho học sinh một số nội dung cơ bản như: Ngôn ngữ
H
toán học, các từ vựng trong Hóa học tạo cho các em nền tảng về ngôn ngữ hóa học: cách
N
đọc tên các chất, các thao tác thí nghiệm, các dụng cụ trong phòng thực hành, cách đọc tên
Y
phương trình phản ứng, mô tả các thí nghiệm hóa học và cách giải thích các hiện tượng.
U
Mục đích cho học sinh làm quen với tiếng Anh trong Hóa học. Dưới đây là bảng về các thuật ngữ cơ bản của Hóa học và tên một số chất vô cơ giúp
Q
giáo viên và học sinh dễ tra cứu trong quá trình dạy và học.
M
2.1.1 Ngôn ngữ toán học
KÈ
2.1.1.1 Cách đọc số
a. Cách đọc số đếm twenty - two
131
onehundred and thirty - one
D
ẠY
22
b. Cách đọc năm, tháng 2018
twenty eighteen
30 April, 2018
The thirty of April, twenty eighteen
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c. Cách đọc phân số ½
a half; one half
3/4
three - fourths; three quarters
1/25
a (one) twenty - fifth
7/18
seven - eighteenths
1/100
a (one) hundredth
1/1225
a (one) thousand two hundred and
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twenty - fifth d. Cách đọc các thập phân 0.2
(nought, zero) point two point two nought point nought two zero point zero two
0.02
point nought two
O
point zero two nought point seventy - five
0.75
one point five
Ơ
1.5
N
point seven five twenty - five point three four
H
25.34
N
two five point three four
Y
2.1.1.2. Cách đọc, viết các phép tính cơ bản
Cách diễn đạt
3+5=8
Three plus five equals (to) eight
10 - 7 = 3
Ten minus seven equal (to) three
Nhân (Multiplication)
3 x 5 = 15
Three times five equal (to)/is/make fifteen
M
Cộng (Addition)
Ví dụ
U
Phép tính
21 : 3 = 7
Twenty one divided by three equal (to) seven
Q
Trừ (Substraction)
KÈ
Chia (Division)
Dm3( L)
Cubic decimetre (liter)
Rightward arrow
Cm3 (mL)
Cubic cetimetre (milliliter)
Leftward arrow
<
Less than
Upward arrow
>
More than (greater than)
downward arrow
≤
Less than or equal to
Reversible arrow
≥
More (greater) than or equal to
x>>y
X much greater than y
X<<y
X much less than y
D
ẠY
2.1.1.3. Cách đọc, viết các kí hiệu toán học
A>0 A<0
A is positive number A is negative number
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2.1.2. Ngôn ngữ hóa học cơ bản 2.1.2.1. Tên các nguyên tố trong tiếng anh
Symbol
element
Relative atomic mass
Relative
Atomic
Symbol Name
number
atomic mass
1
H
Hydrogen
1.008
19
K
2
He
Helium
4.003
20
Ca
3
Li
Lithium
6.94
24
Cr
4
Be
Beryllium
9.01
25
Mn
5
B
Boron
10.81
26
Fe
6
C
Carbon
12.01
29
Cu
7
N
Nitrogen
14.01
30
O
number
Name of
FF IC IA L
Atomic
Potassium
39.01
Calcium
40.08
Chromium
52.01
8
O
Oxygen
16.00
35
9
F
Flourine
19.00
38
10
Ne
Neon
20.18
11
Na
Sodium
22.99
12
Mg
Magnesium 24.31
13
Al
14
Manganese 54.94
55.85
Copper
63.54
Zn
Zinc
65.37
Br
Bromine
79.91
Sr
Strontium
87.62
46
Pd
Palladium
105.40
47
Ag
Silver
107.87
48
Cd
Cadmium
112.40
Aluminium 26.98
53
I
Iodine
16.90
Si
Silicon
28.09
56
Ba
Barium
137.34
15
P
Phosphorus 30.97
78
Pt
Plantium
195.09
16
S
Sulfur
32.06
79
Au
Gold
196.97
17
Cl
Chlorine
35.45
80
Hg
Mercury
200.59
Ar
Argon
39.95
82
Pb
Lead
207.20
Ơ
H
N
Y
U
Q
M
KÈ
18
N
Iron
2.1.2.2. Tên các axit và các ion tương ứng.
ẠY
Acid
D
HF
HCl
Name Hydrofluoric acid (aq)
Anion
Name
F-
Flouride ion
Cl-
chloride ion
Br-
bromide ion
Hydrogen fluoride (g) Hydrochloric acid (aq) Hydrogen chloride (g)
HBr
Hydrobromic acid (aq) Hydrogen bromide (g)
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HI
Hydroiodic acid (aq)
I-
iodide ion
Hydrogen iodide (g) Nitric acid
NO3-
Nitrate ion
H2SO4
Sulfuric acid
S O 24
Sulfate ion
H S O 4
Hydrosulfate ion
PO43-
Phosphate ion
H3PO4
Phosphoric acid
H P O 24 H 2 P O 4
Acid
Name
Hydrophosphate ion
Dihydrophosphate ion
Anion
Name
Hydrosunfuric acid (aq)
S2
Hydrogen sulfide (g)
H S
Sulfurous acid
S O 32
Sulfite ion
H SO 3
Hydrosulfite ion
C O 32
Carbonate ion
H C O 3
Hydrocarbonate ion
S iO 32
Silicate ion
H S iO 3
Hydrosilicate ion
NO2-
Nitrite ion
C lO
Hypochlorite ion
Chlorous acid
C lO 2
Chlorite ion
Chloric acid
C lO 3
Chlorate ion
Perchloric acid
C lO 4
Perchlorate ion
CH3COOH
Acetic acid
CH3COO-
Acetate ion
HCOOH
Formic acid
HCOO-
Formate ion
Benzoic acid
C6H5COO- Benzoate ion
H
Silicic acid
Y
H2SiO3
Ơ
Carbonic acid
N
H2CO3
Nitrous acid
HClO
Hypochlorous acid
Q
U
HNO2
HClO3
ẠY
KÈ
HClO4
M
HClO2
C6H5COOH
Hydrosulfide ion
O
H2SO3
Sulfide ion
N
H2S
FF IC IA L
HNO3
D
2.1.2.3. Tên các bazo , các ion tương ứng và một số chất điển hình. Base
Name
Ion
Name
NaOH
Sodium hydroxide
AlO2-
Aluminate ion
KOH
Potassium hydroxide
ZnO22-
Zincate ion
LiOH
Lithium hydroxide
H+(H3O+) Hydronium ion Trang 10
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Rubidium hydroxide
MnO4-
Permanganate ion
CsOH
Cesium hydroxide
CrO42-
Chromate ion
Mg(OH)2
Manganese hydroxide
Cr2O72-
dichromate
Ba(OH)2
Barium hydroxide
O2-
Oxide ion
Ca(OH)2
Calcium hydroxide
O22-
Peroxide
Fe(OH)2
Iron(II) hydroxide
K2SO3
Potatium sulfite
Fe(OH)3
Irom(III) hydroxide
CuS
Copper (II) sulphide
Cu(OH)2
Copper hydroxide
FeO
Iron (II) oxide
Cr(OH)2
Chromium (II) hydroxide
Fe2O3
Iron(III) oxxide
Cr(OH)3
Chromium (III) hydroxide
N2O5
Dinitrogen pentaoxide
Be(OH)2
Berium hydroxide
Na2SO4
Sodium sulfate
Al(OH)3
Aluminum hydroxide
NaH2PO4 Sodium dihidrophophate
Zn(OH)2
Zinc hydroxide
Li3N
AgOH
Silver hydroxide
NH3
Pb(OH)2
Lead hydroxide
O
FF IC IA L
RbOH
N
Litium nitride
Ơ
ammonia
ammonium
H
NH4+
N
2.1.3. Các thuật ngữ trong phòng thí nghiệm hóa học.
Y
2.1.3.1. Một số dụng cụ hóa học hay dùng trong phòng thí nghiệm Test tube
Q
Burette
M
Pipette Beaker
U
Level tube
ống định mức Ống buret Ống pipet Cốc Bình
Level vessel/volumetric flask
Bình định mức
Reaction vessel
Bình phản ứng
KÈ
Flask/vessel
ẠY D
Ống nghiệm
Erlenmeyer flask ( conical)
Bình tam giác
Graduated flask
Bình đong
Graduated cylinder
Ống chia độ
Thermometer
Nhiệt kế
Stirring rod
Que khuấy
Alcohol lamp
Đèn cồn Trang 11
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2.1.3.2. Một số thao tác thí nghiệm Nhận biết
Distinguish
Phân biệt
Separate
Tách
Refine
Tinh chế
Distillation
Chưng cất
Condensate
Ngưng tụ
Pyrolysis/ decompose
Phân hủy
Combust/ burn
Đốt cháy
Absorbed
Hấp thụ
Dry
Làm khô, sấy
Heat up
Đun nóng
Aeration of CO2 into lime water solution
Sục khí CO2 vào dung dịch nước vôi
Slowly pour A solution into B solution
Nhỏ từ từ dung dịch A vào dung dịch B
Ơ
N
O
FF IC IA L
Identify
Q
U
Y
N
H
2.1.3.3. Các phương pháp thu khí
Phương pháp đẩy không khí và để ngửa ống nghiệm dùng để thu những khí tan trong nước và nặng hơn không khí, ví dụ như khí clo, hidroclorua
M
Downward delivery should be used to collect gases that are
KÈ
soluble in water and denser than air, such as chlorine and
D
ẠY
hydrogen chlorine. Phương pháp đẩy không khí và để úp ống nghiệm dùng để thu những khí tan trong nước và nhẹ hơn không khí, ví dụ như khí Upward delivery should be used to collect gases that are
amoniac
soluble in water and less denser than air, such as amonia.
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Phương pháp đẩy nước dùng để thu những khí không ta hoặc ót tan trong nước. Các khí: cacbonic, hidro, oxi được thu bằng
are insoluble of slightly soluble in water. Carbon dioxide, hydrogen or oxygen can be collected by this method. Example Gas
Solubility in waater
Density
phương pháp này
FF IC IA L
Displacement of water is suitable for collecting gases that
The method of collected gases
O
comparred to
N
air Extremely soluble
Less dense
Upward delivery
Carbon dioxide
Slightly soluble
Denser
Displacement of water
Chlorine
Soluble
Denser
Downward delivery
Hydrogen
Not soluble
Less dense
Displacement of water
Denser
Downward delivery
H N
Hydrogen chlorine Very soluble
Ơ
Ammonia
Very slightly soluble
Slightly dense
Displacement of water
Sulphur dioxide
Soluble
Denser
Downward delivery
U
Y
Oxygen
Chemical reaction
Phản ứng trao đổi
exchange reaction
Phản ứng phân hủy
decomposition
Phản ứng hóa hợp
Combination/conjugate reaction
Phản ứng thế
Displacement reaction
Phản ứng oxi hóa khử
Oxidation Reduction Reactions (Redox Reactions)
Phản ứng thuận nghịch
reversible reaction
Phản ứng thuận
Forward reaction
Phản ứng nghịch
Backward/ reverse reaction
Phản ứng một chiều
Irreversible reaction
Phản ứng tỏa nhiệt
exothermic reaction
D
ẠY
M
Phản ứng hóa học
KÈ
Q
2.1.4. Một số loại phản ứng hay gặp
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endothermic reaction
Phản ứng trung hòa
neutralization reaction
Phản ứng axit-bazơ
Acid-base reaction
Phương trình ion thu gọn
Net ionic equation
Phản ứng trao đổi ion
Ion- exchange reaction
FF IC IA L
Phản ứng thu nhiệt
Reactant
Chất sản phẩm
Product
Chất xúc tác
Catalys
Chất lỏng
Liquid
Chất rắn
Solid
Chất khí
Gases
Chất tan
Solute
Ơ
N
Chất phản ứng
Insoluble
H
Chất không tan Chất ít tan
Slightly soluble
Precipitate
N
Chất kết tủa
Q
Phenolphtalein
U
Quỳ tím
Y
Chất chỉ thị axit-bazơ
M
Chất chỉ thị vạn năng
Acid- base indicators litmus Phenolphtalein
Universal indicator Standar temperature and pressure ( STP)
Nồng độ
concentrate
KÈ
Điều kiện tiêu chuẩn
Nồng độ mol/lit
Molar concentration/ molarity
Nồng độ C%
Percent concentration
Dung dịch bão hòa
Saturated solution
Dung dịch chưa bão hòa
Unsaturated solution
Độ tan
Solubility
Dung dịch quá bão hòa
Supersaturated solution
Dung môi
Slovent
Dung dịch đặc
Dilute solution
ẠY D
O
2.1.5. Một số khái niệm chung hay dùng
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Concentrated solution
Hợp chất
Compound
Đơn chất
Element
Hóa chất
chemical
thuốc thử
reagent
Chất điện li yếu/ mạnh
Weak/ strong electrolytes
Chất khí không màu, không mùi, không vị
Colorless, odorless, tasteless gas
mùi xốc
pungent smell
Độc
Toxic /poison
Chất lỏng
Liquid
Chất rắn
Solid
Chất khí
Gas
Tinh thể
Crystal
Suppose that…/asume that…
N
Giả sử…
Thay…vào…, ta được
Replace… in…, we get Hence /we infer On the other hand, we have Therefore Then
Tương tự ta có/tương tự
Similarly (likewise) ,we have
Nhận xét
Remark
Do đó
Thus
Khi và chỉ khi
If and only if
Trường hợp ….
When +clause
Xét thí nghiệm 1
Consider experiment 1
Chuyển đổi hỗn hợp A thành hỗn hợp B
Convert A mixture to B mixture
Giai đoạn 1, 2, 3…
The first/second/… stage
ẠY
KÈ
M
Vậy
Q
Mặt khác, ta có
U
Suy ra
Let the nuber of mole of A be x
Y
Gọi số mol của chất A là x
D
O
N
Ơ H
2.1.6. Một số lời dẫn thường dùng
Khi đó
FF IC IA L
Dung dịch đậm đặc
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Theo định luật bảo toàn khối lượng, ta có
According to the law of mass conservation, we have
Thành phần phần trăm theo khối lượng của
Mass percent of A in X mixture is ( or the
chất A trong hỗn hợp X là
percent by mass of A in X mixture)
2.2.Giai đoạn 2 (Giới thiệu cho học sinh một số bài tập hóa học cơ bản và cách trình bày
FF IC IA L
một bài tập hóa học trong tiếng anh) 2.2.1.Một số ví dụ về bài tập nêu hiện tượng.
Example 1. What phenomenon will happen when aeration of residual CO2 gas into lime solution
Solution: initially, a white precipitate appears, then the precipitate is dissolved CaCO3 + CO2 + H2O Ca(HCO3)2
O
CO2 + Ca(OH)2 CaCO3 + H2O
N
Example 2. What phenomenon will happen when slowly pour NaOH solution into AlCl 3 solution
Ơ
Solution: initially, a white, glue precipitate appears, then the precipitate is dissolved if
H
NaOH is residual
N
AlCl3 + 3NaOH Al(OH)3 + 3NaCl
Al(OH)3 + NaOH NaAlO2 + 2H2O
Y
Example 3. What phenomenon will happen when drop NaOH solution into NH 4Cl solution
U
Solution: A colorless gas with a pungent odor is escaped
Q
NaOH + NH4Cl NH3 + NaCl + H2O 2.2.2.Một số ví dụ về bài tập định lượng.
M
Example 1. For m grams of sodium in water, we obtain 1.5 liters solution which
KÈ
has pH = 13. What is the value of m? Solution:
We have the chemical reaction
ẠY
2Na + 2H2O 2NaOH + H2
D
The after solution has pH =13, hence H = 10-13M OH = 10-1M the number of mole of OH- is: 10-1(mole/l) x 1.5(l)= 0.15mole the number of mole of NaOH is: 0.15 mole the number of mole of Na is: 0.15 mole m = 0.15 (mole) x23 (grams/mole)= 3.45 grams
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Example 2. We mix 200 mL and 0,25M H2SO4 solution with 300 mL and 0,50M NaOH solution, find pH of this mixture? Solution: Mole of H2SO4: nH2SO4=V.M=(0.2)x(0.25)=0,05 mole Since H2SO4 is strong acid it gives 2 x 0.05=0.1mol H+ ion to solution.
FF IC IA L
Mole of NaOH: nNaOH=V.M=(0.3)x(0.5)=0.15 mole
Since NaOH is strong base it gives 0.15mol OH- ion to solution. H + + OH- → H2O (l)
Neutralization reaction becomes
0.1 → 0.15
mole
After reaction there are: 0.15 – 0.10 = 0.05mol OH- ion. V=0.2 + 0.3 =0.5 L
Molar concentration of OH- ion after reaction becomes; nOH V
0.05 0.1 M 0.5
N
[OH-]=
O
Volume of mixture:
H
1014 1014 1013 M pH=-log(10-13) =13 0.1 OH
N
[H+]=
Ơ
Molar concentration of H+ ion after reaction becomes
Example 3. 1 L and 2M NaBr is mixed with 4 L and 0,5 M NaBr. Find final concentration
Y
of this mixture?
U
Solution:
Q
M1.V1 + M2.V2 = Mfinal.Vfinal 2.1 + 0,5.4=Mfinal x 5
M
Mfinal= 0,8 M
KÈ
Example 4. 0.4 mol MgCl2 and 0.6 mol AlCl3 are dissolved in water and 250 mL solution is prepared. Find molar concentration of [Cl-] in this solution. Solution:
ẠY
We write ionization reactions of both salts and find number of moles of ions;
D
MgCl2(s) → Mg+2(aq) + 2Cl-(aq) 0,4mol
0,4mol
0,8mol
AlCl3(s) → Al+3(aq) + 3Cl-(aq) 0,6mol
0,6mol
1,8mol
Mole of Cl- ion = 0,8 + 1,8 =2,6mol Volume of Solution=250mL=0,25L [Cl-]=nCl-/Vsol.=2,6/0,25=10,4 mol/L Trang 17
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Example 5. Solubility of X solid in water vs. temperature graph is given below. When we heat 300 g saturated solution at 15 0C to 35 0C, 0.6 mol X is crystallized, find
FF IC IA L
molar mass of X.
Solution: As you can see from the graph at 15 0C: 100 g water can dissolve 50 g X.
Thus, at this temperature there are 100 g water in 150 g saturated solution. At 15 0C:
O
150 g saturated solution has 100 g water
a=200 g water
300 g saturated solution has a g water
N
According to graph, 100 g water can dissolve 50 g X at 15 0C and 20 g X at 35 0C. Then,
Ơ
when solution prepared by using 100 g water at 15 0C is heated to 35 0C;
H
50 - 20 = 30 g X is crystallized.
N
15 0C → 35 0C; In 100 g water 30 g X is crystallized
Y
In 200 g water b g X is crystallized b=60 g X is crystallized. m 60 100 grams/mole n 0.6
Q
U
Mole of crystallized X is 0,6 so: 0.6 mol X is 60 gMx = The molar mass of X is 100 grams
M
Example 6. A solution of ethanol (C2H5OH) in water is prepared by dissolving 115.0 mL of
KÈ
ethanol (density 0.79 g/cm3) in enough water to make 250.0 mL of solution. What is the molarity of the ethanol in this solution? Solution:
ẠY
Molar mass of C2H5OH: 2x12+5x6+16x1= 46g/mole The mass of ethanol: 75(mL)x0.79(g/mL) = 90.85 grams
D
Mole of ethanol: 90.85:46=1.975mole The molarity of the ethanol in obtained solution is: 1.975 :
250 = 7.9 M 1000
3. Phần hai: Các chuyên đề bài tập Thiết kế bài giảng theo cấp độ song ngữ Việt – Anh (cấp độ 1) theo các bước +) Bước 1: Cung cấp các từ mới trong chuyên đề Trang 18
Sáng kiến kinh nghiệm năm học 2018 - 2019
+) Đưa ra các bài tập đặc trưng của chuyên đề +) Cung cấp hệ thống bài tập trắc nghiệm và tự luận để học sinh ôn tập 3.1. Các chuyên đề thuộc chương trình lớp 10. 3.1.1. Chuyên đề 1. Atoms - The periodic table of chemical element and the periodic hóa học) Bước 1: Cung cấp các từ mới trong chuyên đề
FF IC IA L
law- Chemical bonding (Nguyên tử- Bảng tuần hoàn các nguyên tố hóa học- Liên kết
Nguyên tử
Atom
Bán kinh
Radius
Phân tử
Molecule
Đường kính
Hạt nhân nguyên tử
Atomic nucleus
Bảng tuần hoàn các
The periodic table of
nguển tố hóa học
chemical elements
Diameter
Atomic shell
Định luật tuần hoàn The periodic law
Lớp e
Electron shell
Độ âm điẹn
Phân lớp e
Electron subshell
Hiệu độ âm điện
N
Ơ
Electronegativity
Electronegativity Difference
Ô nguyên tố ( số
Element cell (odinal
thư tự ô nguyên tố)
of Element cell)
H
Nuclear charge
N
Điện tích hạt nhân
O
Vỏ nguyên tử
Atomic number
Chu kì
Period
Số đơn vị điện tích
The number of atomic Nhóm
Group
hạt nhân
nucleu charge
U
Atom symbol/ Atomic Hóa trị
Q
Kí hiệu nguyên tử
Y
Số hiệu nguyên tử
Valence of element
notation Atomic mass
M
Nguyên tử
Hợp chất oxit
KÈ
khối/khối lượng
The oxides compound
nguyên tử
Nguyên tử khối
Average Atomic mass
Hợp chất với hidro
D
ẠY
trung bình
The hydrogen compound
Số khối
Mass number
The hidroxides
Hidroxit
Cấu tạo nguyên tử
Atomic structure
Axit
Acid
Kim loại kiềm thổ
Alkaline earth metals
bazo
base
Kim loại kiềm
Alkaline metals
lưỡng tính
Amphoteric
Điện tích âm
Negative charge/
Phi kim/ Tính phi
Nonmetal element/
minus charge
kim
Nonmetalic property Trang 19
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Điện tích dương
Positive charge/ plus
Kim loại/Tính kim
Metal element
charge
loại
/meltalic property
Hạt mang điện
Charge particle
Khí hiếm
Noble
Cấu hình electron
Electron configuration Trơ, khó pư
Unreactive/ chemically inert
Outermost electron
Hoạt động hóa học
cùng
shell
mạnh
Đồng vị ( đồng vị
Isotope (stable
Kim loại hoạt động
Reactive metal
bền)
isotope)
Nhiệt độ nóng chảy
Melting point
Liên kết hóa học
Chemical bond
Nhiệt độ sôi
Boiling point
Liên kết đôi
Double bond Single bond
O
Liên kết đơn
Reactive chemical
FF IC IA L
Electron lớp ngoài
Neutral molecule
Liên kết ba
Tinh thể nguyên
Atomic/molecular/ion
Liên kết cộng hóa
tử/phân tử/ion
ic crystal
trị
Cộng hóa trị
Covalence
Ơ
N
Phân tử trung hòa
Triple bond Covalent bond Coordinate covalent
trị cho nhận
bond
N
H
Liên kết cộng hóa
Electrovalence
Liên kết ion
Ionic bond
Công thức electron
Electron fomula
qui tắc bát tử
Octet rule
Công thức cấu tạo
Structural formula
Polar covalent bond
U
Polyatomic ion
Liên kết cộng hóa
Nonpolar covalent
trị không cực
bond
Cặp electron dùng
Shared electron pair
Q
Liên kết cộng hóa
M
Ion đanguyên tử
Y
Điện hóa trị
KÈ
Ion đơn nguyên tử
ẠY
Gốc axit
Monatomic ion
trị có cực
chung Acidic radical
Muối ăn
Table salt
Bước 2: Một số bài tập điển hình trong chuyên đề
D
Exercise 1:
An ion with mass number 37 contains one unit of negative charge and 11.1%
more neutrons than electrons. Find the symbol of the ion. Solution Suppose the symbol of atom is X ion of X with one unit negative charge is: X1Let the number of protons in X be Z, the number of notrons be N The number of electrons is Z ( because X atom is neutral) Trang 20
Sáng kiến kinh nghiệm năm học 2018 - 2019
+) The mass number of ion is: N + Z = 37 (1) +) in X1-, 11.1% more neutrons than electrons N- (Z+1)=11,1%(Z+1) (2) From (1) and (2), We have: N= 20; Z = 17 The symbol of X is Cl The symbol of X1- is Cl1Exercise 2: Density of calcium metal is 1.55 gram/cm3. In fact real, volume occupied by calcium is 40.02 gram/mole.
FF IC IA L
atoms only 74% of crystal, the remaining crystals are the empty slots. The molar mass of Calculate the atomic radius of calcium atom.
Solution: We have the fomular
DCa=
M M V1 mole of crystal = (1) V1mole of crystal D
Because, volume occupied by atoms only 74% of crystal
Mx74% 3
4 Dx6.02 x10 x x 3 23
40 x74% 3
4 1.55 x 6.02 x10 x x3,14 3
= 1.96x10-8cm3 = 1.96x10-8 A0
23
N
r =
4 M x π x r3:74%= 3 D
H
From (1), (2), (3) we have 6.02 x 1023 x
N
4 x π x r3 (3) 3
Ơ
V1mole atoms = 6.02 x 1023 x
O
V1 mole of crystal =V1mole atoms : 74% (2)
Y
Exercise 3: In naturally, chrorine exists as two isotopes 1737Cl and 1735Cl . The average
U
atomic mass of chrorine is 35.5 Calculate percent abundance of chrorine isotopes?
Q
Solution:
Let the percent abundance of chrorine- 35 be x%
M
the percent abundance of chrorine- 37 is 100%-x%
KÈ
Applying formula: A
A1 x1 A2 x2 35 x x % 37 x (100% x %) 35.5= x%= 75% x1 x2 100%
ẠY
Therefor, the percent abundance of chrorine- 35 is 75% the percent abundance of chrorine- 37 is 25%
D
+) Bước 3: Bài tập tự luận và trắc nghiệm cho học sinh Question 1. Covalent bond consists of A. a shared electron
B. two different ions.
C. a shared electron pair
D. one or more shared electron pairs
Question 2. A covalent bond in which there is an unequal attraction for the shared electrons is A. nonpolar
B. ionic
C. polar
D. dipolar. Trang 21
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 3. Which of these is an example of a chemical change? A. methane is burned in air B. solid gold is melted to make jewelry C. a bar of copper is stretched into a long copper wire D. Iron is coated with bronze to prevent rusting A. molecules.
B. dipoles.
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Question 4. In a crystal of an ionic compound, each cation is surrounded by a number of C. positive ions.
D. negative ions.
Question 5. What is the number of electrons in an ion with 10 neutrons, a charge of 1-, and an mass number of 19? A. 9
B. 11
C. 29
D. 10
A. anions
B. Cations
C. electrons
D. protons
O
Question 6. Negatively-charged ions are called
Question 7. A neutral atom contains 12 neutrons and 11 electrons. What is the number of B. 23
C. 1
Ơ
A. 12
N
protons in this atom?
D. 11
H
Question 8. What is the mass number of an atom with 20 protons, 20 electrons, and 22 A. 42
N
neutrons? B. 22
C. 2
D. 20
Y
Question 9. What is the symbol of an atom with 11 protons, 11 electrons, and 12 12 11
B.
Na
11 12
Na
Q
A.
U
neutrons?
C.
23 11
D.
Na
11 23
Na
Question 10. The atom has the following parts: B. protons, electrons, molecules
C. protons, electrons, neutrons
D. elements, neutron, protons
KÈ
M
A. ions, protons, electrons
Question 14. The number of electrons in 8O2– anion is A. 6
B. 10
C. 2
D. 8.
ẠY
Question 15. What is the total number of fundamental particles in
D
A. 82
B. 80
C. 52
56 26
Fe 2 ion ?
D. 56
Question 16. The two stable isotopes of boron exist in the following proportions: 19.78% 10 5
B and 80.22%
A. 10
11 5
B . The average atomic mass of boron is
B. 11
C. 10,08
Question 17. An atom has half as many protons as an atom of neutrons than an atom of
28 14
D. 10,8 28 14
Si and also has six fewer
Si . Give the symbol of this atom. Trang 22
Sáng kiến kinh nghiệm năm học 2018 - 2019
A.
34 14
B. 188O
Si
C.
56 28
D. 157 N
Ni
Question 18. If two covalently bonded atoms are identical, the bond is identified as A. dipolar
B. ionic
C. polar covalent
D. nonpolar covalent
Question 20. An atoms' nucleus contains B. protons and electrons
C. neutrons, protons, and electrons
D. protons and neutrons, expect 11H
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A. neutrons only
Question 21. Which combination of particle and charge is correct? A. neutron: negatively charged
B. proton: Positively charged
C. electron: Positively charge
D. electron: no charge
Question 22. When an atom loses electrons, it becomes
B. Neutral atom.
C. No charge.
D. Positively charged.
O
A. Negatively charged.
N
Question 23. The sum of the numbers of the protons and neutrons in the atom of an
Ơ
element is known as A. Atomic Number
B. Isotope Number
An atom of has atomic number of 5, but the mass number is 13 u. How
N
Question 24.
D. Molecular Mass
H
C. Mass Number
many neutrons are present in this atom? B. 21 B. 18
Q
A. 21
C. 8
D. 13
What is the number of electrons in a Cr3+ ion?
U
Question 25.
Y
A. 5
C. 24
D. 27
A. 25 He
M
Question 26. Which of the following atoms has 7 electrons? B. 136C
C. 37 Li
D. 157 N
KÈ
Question 27. The total number of subatomic particles in atom X is 95. electrically neutral particles are 58.33% of charged particles. The mass number of this atom is
ẠY
A. 30
Question 28.
D
A. 40
B. 35
C. 65
The total number of subatomic particles in B. 43
C. 37
D. 25 27 13
Al 3 ion is
D. 27
Question 29: What is the number of electrons in an ion with 30 neutrons, a charge of 3+, and an mass number of 56? A. 21
B. 18
C. 23
D. 66
Question 30. Which of the following conclusions is false? A. The nucleus is posively charged. Trang 23
Sáng kiến kinh nghiệm năm học 2018 - 2019
B. The atom is a dense solid and is indivisible. C. The nucleus is very small and the atom is mostly empty space D. The nucleus is the center of an atom. Question 31. Lithium, the first element in Group 1, has an atomic number of 3. The second element in this group has an atomic number of B. 11
C.10
D. 18
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A. 4
Question 32. In the modern periodic table, elements are ordered. Choose the incorrect answer A. according to decreasing atomic mass. B. according to increasing atomic nuclear charge.
C. elements with the same number of valence electrons are arranged in the same column
O
D. elements with the same number electrons shells in atoms are arranged in the same row Question 33. The most distinctive property of the noble gases is that they are B. nonmetallic
C. radioactive
N
A. metallic
D. largely unreactive.
incorrect? B. Iron – Fe
C. Alumium – Al
D. Helium – He
N
A. Sodium – So
H
Ơ
Question 34: Which of the following element – chemical symbol pairs is matched
Question 35: Which of the following is a nonmetal? B. Potassium
Y
A. Gold
C. Sulfur
D. Copper
U
Question 36: The smallest particle of an element that retains all of the properties of that A. atom
Q
element is called
B. neutron
C. proton
D. electron
M
Question 37: Of the 3 subatomic particles, which one has the lowest mass? B. Electrons
C. Neutrons
D. none, they all have almost the same
KÈ
A. protons
Question 38: An atom of has atomic number of 53, but the mass number is 127 amu. How many neutrons are present in this atom?
ẠY
A. 53
B. 127
C. 74
D. 181
D
Question 39: At 20 degrees c, an atom with density of 7.87 gram/cm3 and the radius of 1.28A0. In fact real, volume occupied by atoms only 74% of the remaining crystals are the empty slots. Element name is A. Coppper (63.54 amu)
B. Iron (56.2 amu)
C. Zinc (65.41 amu)
D. Silver (107.87 amu)
Trang 24
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 40: An atom of element Z has two more protons and two more neutrons than an atom of A.
36 18
34 16 S
. Give the symbol for this atom of Z. B.
Ar
38 18
C.
Ar
30 14
D.
Si
28 14
Si
Bài tập tự luận Exercise 1:
Deduce the average atomic mass of Zirconium. Assume in all cases the
4. (94 – 17.38)
5. (95 – 2.8)
Ơ
Exercise 2:
3. (92 - 17.15)
O
2. (91 – 11.22)
N
1: (90 – 51.45)
FF IC IA L
relative isotopic mass is equal to the mass number.
An ion with mass number 37 contains one unit of negative charge and 11.1% Naturally occurring chrorine exists as two isotopes
N
Exercise 3:
H
more neutrons than electrons. Find the symbol to the ion.
37 17
Cl and
Cl . The
35 17
Y
average atomic mass of chrorine is 35.5 Calculate percent abundance of chrorine isotopes?
U
Exercise 4: Carbon has three naturally occuring isotopes. C-12 has an abundance of x 1 %, C-13 has an abundance of x2, % C-14 has an abundance of x3 %.
Q
With x1 = 100x2 + 90x3 ; x2 = 9x3 . Calculate the average atomic mass of carbon?
M
Exercise 5: An element with mass number 81 contains 31.7% more neutrons as compared to protons. Assign the atomic symbol.
KÈ
Exercise 6: Total particles in X atom are 76; Some more charged particles are electrically neutral particles 20. Assign the symbol to this element.
ẠY
Exercise 7: An ion with mass number 56 contains 3 units of positive charge and 30.4% more neutrons than electrons. Assign the symbol to this ion.
D
Exercise 8. You are given a sample containing 98.9 % carbon-12 and 1.1% carbon-13. What is the average atomic weight for the element? Exercise 9. A sample of element X contains 109 atoms with a mass of 79.00 and 91 atoms with a mass of 81.00. Calculate the the average atomic weight for element X(in amu) Exercise 10. 2x108 atoms of carbon are arranged side by side. Trang 25
Sáng kiến kinh nghiệm năm học 2018 - 2019
Calculate the radius of carbon atom if this e length of this arrangement is 2.4 cm. Exercise 11. An atom with the mass of 196,97 amu; the volume of 1.0210-23 cm3. Calculate the density in grams per cubic centimeter. Exercise 12. Density of calcium metal is 1.55 gram/cm3. In fact real, volume occupied by atoms only 74% of the remaining crystals are the empty slots. The mass number of calcium
FF IC IA L
is 40.02 gram/mole. Calculate the atomic radius of calcium atom.
Exercise 13. Base your answers to questions 1-6 on the following elemental notation. 1. Which element is represented by this ion notation? 2. What is the atomic number of the element? 3. What is the mass number of the element? 4. How many protons does the element have?
X 2
O
5. How many neutrons does the element have?
25 12
N
6. How many electrons does the ion have?
Ơ
Exercise 14. . Base your answers to questions 1-5 on the following electron configurations of neutral atoms. b. 1s22s22p2
d. 1s22s12p3
e. 1s22s22p5
H
c. 1s2
f. 1s22s22p4
N
a. 1s22s22p6s1
1. Which electron configuration represents a noble gas?
Y
2. Which electron configuration shows an atom in the excited state?
U
3. Which electron configuration shows an alkali metal?
Q
4. Which electron configuration represents a halogen? 5. Which ground state configuration shows a total of 4 valence electrons?
M
Exercise 15. Give the electron configuration, and short electron configuration of the
KÈ
ground state of S (Z = 16), Ne (Z = 10), Fe (Z = 56), Cu (Z = 29), Cr (Z = 24) Exercise 16. Two elements in Period 5 are adjacent to one another in the periodic table. The ground state atom of one element has only s electrons in its valence shell; the other has at
ẠY
least one d electron in an unfilled shell. Identify the elements.
D
Exercise 17. In the Natural silver element exists as two stable isotopes, has mass of 107u and percent abundance of 51.8%; has mass of 109u and percent abundance of 48.2%. Calculate the average atomic mass of silver. Exercise 18. Two atoms X and Y have the electronic configuration X: 1s22s22p63s23p63d104s2
Y: 1s22s22p4
Which compound are they likely to form? Trang 26
Sáng kiến kinh nghiệm năm học 2018 - 2019
Exercise 19. Match each set of characteristics on the left with an element in the column at the right. 1.The Sodium(Na)
b. A soft metal; the atom has only one Valence electron
2.chromnium (Cr)
c. A hard metal, the atom has belong to group VIB in period
3.Argon (Ar)
d. A chemically unreactive gas
4.Chlorine (Cl)
FF IC IA L
a. A reactive nonmetal; atom has a large electronegativity
Exercise 20. The ground-state electron configuration of an atom is 1s22s22p63s23p4. What is the valence shell configuration of the atom in the same group, but in Period 5
3.1.2. Chuyên đề 2. Oxidation-Reduction reaction reaction; Rates of reaction and
Chemical eqilibrium ( Phản ứng oxi hóa- khử; Tốc độ phản ứng và cân bằng hóa học) Bước 1: Cung cấp từ mới trong chuyên đề Oxidation Reduction
Phản ứng
Oxi hóa- khử
Reactions
thuận nghịch
N Ơ
(Redox Reactions) Exchange reaction
trao đổi Decomposition
Combination/conjugat
hóa hợp
e reaction
Phản ứng
Displacement reaction
M
thế
KÈ
Hệ số phương
Equation coefficient
trình
Chất oxi hóa =
Oxidizing agent
chất bị khử
(oxidant)= reduced
ẠY D
Dynamic equilibrium
Phản ứng thuận
Forward reaction
Phản ứng nghịch
Backward/ reverse
U
Phản ứng
Q
Y
phân hủy
Chemical equilibrium
Cân băng động
N
Phản ứng
Cân bằng hóa học
H
Phản ứng
Reversible reaction
O
Phản ứng
reaction Sự chuyển dịch cân
The shift of chemical
băng hóa học
equilibrium
Trạng thái cân bằng
Equilibrium state
agent(reduced substance)
Chất khử = chất
Reducing agent
Ảnh hưởng của
The influence of
bị oxi hóa
(reductant)= oxidized
nhiệt độ/nồng độ,
temperature/concentrat
agent (oxidized
áp suất
ion/pressua
substance) Trang 27
Sáng kiến kinh nghiệm năm học 2018 - 2019
Quá trình oxh
Oxidation process =
Ảnh hưởng của
Temperature
oxidation
nhiệt độ đến cân
affects/effects
The oxidation of Fe
bằng hóa học
chemical equilibrium
Nhiệt độ không đổi
Constant temperature
Quá trình khử
Reduction process = reduction . The Reduction of Cu2+ = Cu2+ is reduced
Trạng thái oxi
Oxidation state
Tốc độ phản ứng
reaction
The only redoxing
Hiệu suất phản ứng
Efficiency of reaction
duy nhất
product
Tăng/giảm số
Increases/decreases
Hiệu suất phản ứng
Efficiency
oxi hóa:
Oxidation number
Số oxi hóa
Negative/positive
catalyst
âm/dương
oxidation number
Chuyển electron
Transfer of electron
Mũi tên 1 chiều
Unidirectioral arrow
Thay đổi số oxi
Change the Oxidation
Mũi tên 2 chiều
bidirectioral arrow
hóa của một số
number of some
nguyên tố
elements
Phản ứng hóa học
Chemical reaction
N
O
Sản phẩm khử
Q
U
Y
N
H
Chất xúc tác
Oxidizing agent is the
M
Chất oxi hóa là
Substantce gains
electron
electron
KÈ
chất nhận
( có sự giảm số
(with decreases
oxi hóa)
Oxidation number)
ẠY D
Rate of chemical
Ơ
hóa
FF IC IA L
= Fe is oxidized
Chất khử là chất Reducing agent is the
Chất phản ứng/ chất Reactant/ product
nhường electron Substantce loses
sản phẩm
( có sự tăng số
electron( with
oxi hóa)
increases Oxidation number)
Phương trình
Chemical equation
Phản ứng tỏa nhiệt
Exothermic reaction Trang 28
Sáng kiến kinh nghiệm năm học 2018 - 2019
hóa học Nhường electron Excess ( loses)
Phản ứng thu nhiệt
Endothermic reaction
electrons Nhận electron
Consume/receive/gain
Tổng số oxi hóa của The sum of the
electrons
các nguyên tử
oxidation numbers of
FF IC IA L
atoms
Bước 2: Một số bài tập điển hình trong chuyên đề
Exercise 1: During a classroom experiment copper metal reacts with concentrated nitric acid to produce NO2 gas, which is collected in a gas syringe. When enough gas has
collected in the syringe, the delivery tube is clamped so that no gas can escape. The brown following equation:
∆H <0
N
2NO2(g) N2O4(g)
O
NO2 gas collected reaches an equilibrium with colourless N2O4 gas as represented by the
Ơ
Once this equilibrium has been established, there are 0.01 moles of NO 2 gas and 0.03 moles
H
of N2O4 gas present in the syringe.
(a) A learner, noticing that the colour of the gas mixture in the syringe is no longer
Y
assumption correct? Explain.
N
changing, comments that all chemical reactions in the syringe must have stopped. Is this
U
(b) The gas in the syringe is cooled. The volume of the gas is kept constant during the
Q
cooling process. Will the gas be lighter or darker at the lower temperature? Explain your answer.
M
Solution:
KÈ
(a) This assumption is incorrect. Because, this reaction is reversible reaction, when the reaction has reached equilibrium, the reaction still occurs but the rate of forward reaction is equal to that of the reverse reaction so the colour of the gas mixture in the syringe is no
ẠY
longer changing
D
(b) This reaction has ∆H <0 - exothermic reaction, so when the gas in the syringe is cooled (the volume of the gas is kept constant during the cooling process) chemical equilibrium will move in the right direction, so the gas will be lighter Exercise 2: A number of different reactions take place. The table below shows the number of moles of reactant that are used up in a particular time for each reaction.
Trang 29
Sáng kiến kinh nghiệm năm học 2018 - 2019
Reaction
Mols used up
Time
Reaction rate
1
2
30 secs
2
5
2 mins
3
1
1.5 mins
4
3.2
1.5 mins
5
5.9
30 secs
FF IC IA L
(Mols/sec)
(a) Complete the table by calculating the rate of each reaction. (b) Which is the fastest reaction? (c) Which is the slowest reaction? Solution: Mols used up
Time
Reaction rate
O
Reaction
2
30 secs
2
5
2 mins
3
1
4
3.2
H
U
Y
N
1.5 mins
5.9
Q
5
2 = 0.067 30
Ơ
1
N
(Mols/sec)
5 = 0.042 60 x 2
1 = 0.011 1.5 x60
1.5 mins
3.2 = 0.035 1.5 x60
30 secs
5.9 =0.197 30
slowest reaction
fastest reaction
M
Exercise 3: Two groups of students do experiments: study the rate of reaction when zinc
KÈ
solubles hydrochloric acid solution: -
The first group: Add 1grams of zinc scraps and 200ml of HCl 2M to a beaker.
-
The second group : Add 1grams of zinc powder and 300ml of HCl 2M to a beaker
ẠY
The results showed that bubbles released in the second group were stronger than those in
D
the first group. Please explain that result Solution: In both experiments, there was only reaction Zns + 2HClaq ZnCl2aq + H2 g The faster this reaction occurs, the stronger the gas escape. The rate of reaction depends on temperature, pressure, concentration, surface area and catalyst. In the second group, students used zinc powder so the surface area is larger than Trang 30
Sáng kiến kinh nghiệm năm học 2018 - 2019
that in the first group, so the bubbles released in the second group were stronger than those in the first group Exercise 4: Have a reaction. C2H5Brl + KOHaq C2H5OHaq + KBraq The initial concentration of KOH is 0.07M. After 30 minutes, 10 ml of the solution mixture reacted sufficiently to 12.84 ml of a 0.05
FF IC IA L
M HCl solution. Caculate the average reaction rate of reaction in the period was 30 minutes. Solution: The neutral reaction KOHaq +
KClaq + H2Ol
12.84 x0.05 = 6.42x10-4 mol nKOH = 6.42x10-4 mol 1000
CKOH unreacted= 6.42x10 4 :
10 = 0.0642 mol/l 1000
O
nHCl =
HClaq
CKOH reacted=0.07 - 0.0642= 5.8x10-3mol/l
N
5.8 x10 3 1.933 x104 M/minute 30
Ơ
the average rate of reaction in 30 minutes was:
Bước 3: Cung cấp bài tập tự luận và trắc nghiệm cho học sinh B. favors the reverse reaction.
N
A. favors the forward reaction.
H
Question 1. Raising the temperature of any equilibrium system always C. favors the exothermic reaction.
D. favors the endothermic reaction.
Y
Question 2.Consider the following equilibrium equation:
Q
U
CH3OH(g) 2H2(g) CO(g)Ho 101kJ Increasing [CO] will
M
A. increase [H2]
C. decrease [H2]
B. not change [H2]. D. cause [H2] to fluctuate.
KÈ
Question 3. For equilibrium: 2NO2 N2O4 ∆H = -58.04 kJ. Dip the jar containt mixture of NO2 and N2O4 gas into ice
ẠY
A. The mixture remains the same color as the original
D
C. Brown fades
B. Dark brown
D. The color combination is different
Question 4. A nitrogen and hydrogen mixture, innitially in the mole ratio of 1:3, reached equilibrium with ammonia when 50% of the nitrogen had reacted. What was the partial pressure of ammonia in the equilibrium muxture? A. p/8
B. p/6
C. p/4
D. p/3
Question 5. Consider the following reaction, which takes place in a closed container: A(s) + B(g) → AB(g) ∆H < 0 Trang 31
Sáng kiến kinh nghiệm năm học 2018 - 2019
If you wanted to increase the rate of the reaction, which of the following would you do? A. decrease the concentration of B
B. decrease the temperature of A
C. grind A into a fine powder
D. decrease the pressure
Question 6. Consider the following reaction that has reached equilibrium after some time in a sealed 1 dm3 flask:
FF IC IA L
PCl5(g) PCl3(g) + Cl2(g); ∆H is positive
Which one of the following reaction conditions applied to the system would decrease the rate of the reverse reaction? A. increase the pressure
B. increase the reaction temperature
C. continually remove Cl2(g) from the flask
D. addition of a suitable catalyst
Question 7. Which metal reacts with Cl2 and HCl to produce the same salt? B. Ag
C. Mg
D. Cu
O
A. Fe
question 8. which subtance reacting with concentrated, heated, excess nitric acid solution B. Fe2O3
C. Fe
D. FeCO3
Ơ
A. FeO
N
doesn’t belong to redox reaction?
H
Question 9. Let excess Ba(OH)2 solution react with solution which contains FeCl2, CuSO4
A. FeO, CuO, Al2O3
B. Fe2O3, CuO, BaSO4 D. Fe3O4, CuO, BaSO4
U
C.Fe2O3, CuO
Y
contains:
N
and AlCl3 to produce precipitation A. Heat A in air to constant mass to produce solid X. X
Q
Question 10. Which of the following metals (with excess amounts) can reduce Fe3+ to Fe2+? A. Na
B. Mg
C. Cu
D. Ag
M
Question 11. When pyrolysis 24.5 grams of KClO3 by the reaction: 2KClO3 MnO 2 2KCl
KÈ
+ 3O2. The volume of obtained oxygen (standard conditions) is: A. 4.48liter
B. 6.72 liter
C. 2.24liter
D. 8.96 liter
Question 12. How many moles of FeS2 react with oxygen to obtain 64 grams of SO2
ẠY
according to the following chemical equation: 4FeS2
D
A. 0.4
B. 1.2
C. 0.5
+ 11O2
→ 2Fe2O3+ 8SO2
D. 0.8
Question 13. Have a reaction. C2H5Br + KOH C2H5OH + KBr The initial concentration of KOH is 0.07M. After 30 minutes, 10 ml of the solution mixture was removed and reacted sufficiently to 12.84 ml of a 0.05 M HCl solution. The average reaction rate of reaction in the period was 30 minutes. A. 2.04.10-4 mol / l. minute -1;
B. 1.93.10-4 mol / l. minute -1; Trang 32
Sáng kiến kinh nghiệm năm học 2018 - 2019
C. 1.54.10-4 mol / l. minute -1;
D. 0.95.10-4 mol / l. minute -1
Question 14. The oxidation number of sulfur (S) in H 2S, SO2, SO32-, SO42- in order? A., +4, +6, +8.
B. -2, +4, +4, +6.
C. +2, +4, +8, +10.
D. 0, +4, +3, +8.
Question 15: Oxidized substance is substance:
FF IC IA L
A. get electrons and increase oxidation number B. accept electrons and decrease oxidation number C. give electrons and increasing oxidation number D. lose electrons and decreasing oxidation number
Question 16. Which of the following reaction are not redox reactions? A. 2Fe + 3Cl2 → 2FeCl3
B. 4Fe(OH)2 + O2 → 2Fe2O3 + 4H2O
D. 2NaHCO3 → Na2CO3 + H2O + CO2
O
C. 2Na + 2H2O → 2NaOH + H2
Question 17.For chemical reaction: Cl2 + KOH KCl + KClO3 + H2O
N
The ratio between the chlorine atoms are oxidants and chlorine atoms as a reducing agent in B. 1: 3.
C. 3: 1.
H
A. 5: 1.
Ơ
the chemical equation of reaction gave respectively
D. 1: 5.
N
Question 18. What is the process of Fe2+ → Fe3+ 1e? A. oxidation process.
Y
C. The process of getting a proton.
B. reduction process. D. process of self-oxidation - reduction.
U
Question 19. In the following reaction H2SO4 is not an oxidizer
Q
A. 6H2SO4 + 2Fe Fe2(SO4)3 + 3SO2 + 6H2O B. 2H2SO4 + 2FeSO4 Fe2(SO4)3 + SO2 + 2H2O
M
C. H2SO4 + Fe FeSO4 + H2
KÈ
D. H2SO4 + nSO3 H2SO4.nSO3 Question 20. In the following reactions, the reaction pressure does not affect the reaction
D
ẠY
equilibrium:
A. N2 + 3H2 C. 2NO + O2
2NH3 2NO2.
B. N2 + O2
2NO.
D. 2SO2 + O2 2SO3
Question 21. Two groups of students do experiments: study the rate of reaction when zinc solubles hydrochloric acid solution: -
The first group: 1 g of zinc scraps and 200ml of HCl 2M in a beaker.
-
The second group : Add 1g of zinc powder and add 300ml of HCl 2M to the beaker
Trang 33
Sáng kiến kinh nghiệm năm học 2018 - 2019
The results showed that bubbles released in the second group were stronger than those in The first group, because: A. second group uses more acid. B. the surface area of zinc powder is larger. C. the concentration of zinc powder is greater.
FF IC IA L
D. all three are wrong.
Question 22. In response burn CuFeS2 create products CuO, Fe2O3 and SO2. So a molecule of CuFeS2 will A. receive 12 electrons.
B. give up 13 electrons.
C. get 13 electrons.
D. donated 12 electrons.
Question 23. For chemical reaction: Fe + CuSO4 → FeSO4 + Cu. In the above reaction
O
occurs
B. reduction of Fe2+ and reduction of Cu2+.
C. reduction of Fe2+ and oxidation of Cu.
D. oxidation of Fe and Cu oxidation.
N
A. oxidation of Fe and reduction of Cu2+.
Ơ
Question 24. Consider the reaction:
H
10 FeSO4 + 2KMnO4 + 8H2SO4 → 5Fe2(SO4)3 + 2MnSO4 + K2SO4 + 8H2O. A. K2SO4
B. H2SO4
N
Substances play the role of the environment
Y
Question 25. For equilibrium reactions:
C. H2O
D. MnSO4
A (g) + B (g) C (g) + D (g)
C. decrease [C].
B. decrease [B].
Q
A. increase [B].
U
At constant temperature and pressure, the increase in gas [A] is due to: D. decrease [D].
M
Question 26. Which of the following reaction is an oxidation-reduction reaction? C. N2O5 + H2O → 2HNO3
B. 2HNO3 + 3H2S → 3S + 2NO + 4H2O
D. 2Fe(OH)3 →Fe2O3 + 3H2O
KÈ
A. HNO3 + NaOH → NaNO3 + H2O
Question 27. Completely dissolve 10.8 grams of FeO in solution of HNO3 diluted, hot,
ẠY
residue is obtained V Litter of NO (The only redoxing product – at STP) and solution of
D
Fe(NO3)3 Calculating V: A. 2,24 litters
B. 3,36 litters
C. 4,48 litters
D. 1,12 litters
Question 28. Which of the following substance (or ion) is capable of exhibiting oxidation and is capable of demonstrating reducing properties in chemical reactions? A. Al3+
B. S2-
C. Fe2+
D. Na
Question 29. Indicate wrong content: Trang 34
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. The oxidation number of the element in the compound equal the velence of that element. B. In a molecule, the total oxidation of atoms is zero. C. The oxidation number of a mono ion is equal to the charge of that ion. D. The total oxidation of the elements in the poly ion is equal to the charge of the ion. Question 30. For a system in equilibrium, if the catalyst is added:
FF IC IA L
A. Only increase the speed of the forward reaction. A. Only increase the speed of the reverse reaction.
C. Increases the speed of the forward and reverse reactions equally. D. Do not increase the forward reaction rate and reverse reaction.
Question 31. Calculate the volume of O2 (under standard conditions) required to burn completely 6.8 grams of NH3 to form NO and H2O gas. B. 8.96 liters
C. 13.44 liters
D.16.8 liters
O
A. 11.2 liters
Question 32. Which of the following substances only demonstrate the reduction properties B. SO2
C. S
Ơ
A. NO2
N
in chemical reaction
D. Al
H
Question 33. in the following reactions, the reaction which is not a redox reaction C. H2SO4 + Fe Fe2(SO4)3 + SO2 + H2O
N
B. H2SO4 + Fe FeSO4 + H2
B. H2SO4 + FeSO3 FeSO4 SO2+ H2O
D. H2SO4 + FeO Fe2(SO4)3 + SO2 + H2O
increases:
C. 2NO(g)
2H2O(g).
Q
A. 2H2(g) + O2(g)
U
Y
Question 34. At constant temperature,what the balance will shift to the right if the pressure
N2(g) + O2(g)
B. 2SO3(g)
D. 2CO2(g)
2SO2(g) + O2(g) 2CO(g) + O2(g)
M
Question 35. Dissolve complete 10.8 grams of Fe(OH)2 in a concentrated, hot, residual
KÈ
HNO3 solution, obtained V liters of NO2 gas (The only redoxing product – at STP). The value of V is: A. 1,12 liters
B. 3,36 liters
C. 2,688 liters
D. 4,48 liters
ẠY
Question 36. For the following process: NO3- + 4H + + 3e NO + 2H2O (1).
D
(1) is the process: A. Oxidation
B. Reducing
C. Redox reaction
D. The process of giving, receiving electrons
Question 37. Which of the following reactions is a redox reaction? A. NaOH + HCl NaCl C. KClO3
KCl
+ H2O
+ KClO4
B. CaO + CO2
CaCO3
D. Fe(OH) 3 Fe2O3 + H2O Trang 35
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 38. For the following statements about the oxidation process (1) the process of reducing the oxidation number of the element. (2) the oxidation agent receives electron (3) the process of increasing the oxidation number of the element. The True statements are: A. (1) and (3).
B. (1) and (4).
C. (3) and (4).
FF IC IA L
(4) the process gives up electrons of reduction agent D. (2) and (3).
Question 40. Equilibrium coefficients of Cu2S and HNO3 in reaction: Cu2S + HNO3 Cu(NO3)2 + H2SO4 + NO + H2O A. 3 and 22.
B. 3 and 18.
are:
C. 3 and 10.
D. 3 and 12.
value of n is B. 2.
C. 3.
NO + . H2O. The
D. 4.
N
A. 1.
Mn+ +
O
Question 41. In the following reaction: 3M + 2NO3- + 8H+
Question 42. For the reaction: Al + HNO3 → Al(NO3)3 + N2 + N2O + H2O.
B. 46: 9
C. 46: 6.
D. 44: 9
N
A. 44: 6
H
Determine the molar ratio nAl: nN2O
Ơ
Knowing that when the equation is balanced , molar ratio between N 2O and N2 is 3: 2.
Question 43. Give the following reaction:
Y
KMnO4 + FeSO4 + H2SO4 Fe2(SO4)3 + K2SO4 + MnSO4 + H2O. B. 2 and 10.
C. 4 and 10
Q
A. 10and 4.
U
The coefficients of oxidation and reduction in reaction respectively are D. 10 and 2.
Question 44. For reaction diagram:
M
FeS2 + HNO3 Fe(NO3)3 + H2SO4 + NO + H2O
KÈ
After equilibration, the total coefficients of the substances in the reaction are A. 21.
B. 19.
C. 23.
D. 25.
Question 45. In reaction: 6KI + 2KMnO4 +4H2O 3I2 + 2MnO2 + 8KOH
D
ẠY
What substance is oxidized? A. I-.
B. MnO4-.
C. H2O.
D. KMnO4.
Question 46. For the reaction: M2Ox + HNO3 M(NO3)3 + NO + H2O The reaction is an exchange reaction when: A. x = 1
B. x = 2
C. x = 1 or x = 2
D. x = 3
Trang 36
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 47. The following effect DOES NOT affect the rate of CaCO3 decomposition CaCO3 (s) CaO (s) + CO2 (g)
reaction. A. Heat
B. Add more Limestone
C. use limestone small dam
D. use fine Limestone
Question 48. Using compressed, hot air, blown into the blast furnace to burn coke (in the A. Temperature, pressure.
B. increase the area.
C. Concentration.
D. catalyst.
FF IC IA L
production of cast iron), which factors affect the speed of reaction?
Question 49. Put 5g of zinc in a beaker with 50ml H2SO4 4M solution at normal temperature (25o). In what case the speed of reaction is not change? A. Replace 5g zinc tablets with 5g zinc powder.
O
B. Substitute 4M H2SO4 solution with 2M H2SO4 solution. C. Reaction at 50oC.
N
D. twice as much as the original solution of H2SO4.
Ơ
Question 50. For the following chemical reaction is in equilibrium.
H
2SO2 (g) + O2 (g) 2SO3 (g).
N
As the temperature increases, mass ratio of a mixture gases with hydrogen is decreasing Which of the following statements true about balance
U
temperature increases
Y
A. the reverse reaction is an exothermic reaction , balance shifted forward when
increases
Q
B. the forward reaction is an exothermic reaction, balance shifted reverse as temperature
M
C. the forward reaction is an endothermic reaction, balance shifted in the reverse direction
KÈ
when temperature increases D. the reverse reaction is an endothermic reaction, balance shifted forward when temperature increases
ẠY
Bài tập tự luận
D
Exercise 1. Calculate the average rate of decomposition of N2O5, ∆[N2O5]/∆t, by the
reaction
2N 2 O5(g) 4NO2(g) O 2(g)
during the time interval from t= 600s to t=1200s (regard all time figures as significant).Use the following data: Time
[N2O5]
600 s
1.24 x102M Trang 37
Sáng kiến kinh nghiệm năm học 2018 - 2019
0.93x102M
1200 s
Exercise 2. A nitrogen- hydrogen mixture, initially in the mole ratio of 1:3, reached equilibrium with ammonia when 50% of the nitrogen had reacted. The total final mol of gases at equilibrium state.
N 2(g) 3H2(g) 2NH3(g)
FF IC IA L
Exercise 3. Consider the following equilibrium equation: H2O(g) C(s) CO(g) H2(g) H 0 At equilibrium, which reaction will be favored (forward, reverse, or neither) when a. extra CO gas is introduced? b. a catalyst is introduced? c. the temperature of the system is lowered?
O
d. the pressure on the system is increased due to a decrease in the container volume? Exercise 4. Write chemical equations to complete the following diagram
↓(5)
↓(3)
Fe(OH)3
Fe(OH)2
H
Fe2O3
FeCl2
N
↑(7)
FeCl3
Ơ
Fe
N
Exercise 5. Complete solute 9,84 (grams) solid X containing FeO, Fe2O3 and Fe3O4 by excess chloric acid solution to produce a (grams) FeCl3 and 8,89 (grams) FeCl2.
Y
Measure a?
U
Exercise 6. Identify X in the following diagram:
Q
X + HNO3 đặc
Fe(NO3)3 + NO2↑ + H2O
Exercise 7. Let iron react with:
KÈ
- Iodine
M
- Chlorine gas
- Diluted, cooled sulfuric acid solution - Concentrated, cooled sulfuric acid solution
ẠY
- Concentrated, heated, excess sulfuric acid soluiton
D
- ferric nitrate (iron(III) nitrate)solution - Excess silver nitrate solution a. Which reactions produce ferrous(iron(II)) compounds? Write chemical equations? b. Which reactions produce ferric compounds? Write chemical equations? Exercise 8. Divide m (grams) iron powder into three equal parts:
Trang 38
Sáng kiến kinh nghiệm năm học 2018 - 2019
- Part 1: React with excess chloric acid solution to produce 2,24 liters of gas (at standard condition). - Part 2: Heat for a while to produce m1 (grams) of solid X. Let solid X react with dilute, excess nitric acid solution to produce 1,12 liters of nitrogen monoxide gas (at standard condition)
FF IC IA L
- Part 3: React with excess cupric chloride( copper(II) chloride) solution. After complete
reactions, filter solid from the liquid and dry. Then, the weight of the solid increases m2 (grams) a. Write chemical equations for reactions that occurred b. Determine m, m1, m2?
Exercise 9. For CO gas through the tube containing m gram Fe2O3 heating, after a period of
O
time obtained 13.92 grams of X mixture of Fe, FeO, Fe3O4, Fe2O3. Dissolve all X solids mixture in the residual of HNO3 solution, obtained only 5.824 liters NO 2 in standard
N
conditions. Calculate the value of m
Ơ
3.1.3. Chuyên đề 3: Halogen goup – Oxigen,sunfur ( Nhóm halogen; Nhóm oxi- lưu
H
huỳnh)
N
Bước 1: Cung cấp từ mới trong chuyên đề Chlorine of lime
vôi sữa
Slaked lime
Vôi sống
Quicklime
Đá vôi
Limestone
Xút ăn da
Caustic soda
Diêm tiêu
Sodium salpeter
Steam/ moist
Tinh bột
Starch
Organic solvent
Khắc chữ lên thủy
Etch letters on glass
U Q
Hơi nước
Y
Clorua vôi
M
Dung môi hữu cơ
halide compound
Axit halogen hidric
Hydrohalic acid
H2S
Hydrosulfuric acid
H2SO4
Sunfuric acid
H2SO3
sulfurous acid
Dịch vị dạ dày
Stomach gastric
Màng ngăn xốp
Porous wall/
Ảnh hưởng xấu
Negative effect
KÈ
Hợp chất
tinh
D
ẠY
Halogenua
diaphragm
Tia cực tím
Ultraviolet ray
Thụ động
Passivation
Chất sát trùng
Germicide
Điện phân
Electrolysis
Vật liệu nhạy sáng
light sensitive
Gốc axit
Radicals of axids
material Trang 39
Sáng kiến kinh nghiệm năm học 2018 - 2019
Hơi / áp suất hơi
Phương pháp
vapor /vapor
Hiện tượng thăng
pressure
hoa
Sunfate method
Hơi brom độc
Brom’s vapor is
sunfat
poisonous
hợp ứng dụng thực tế
Practical application
Khai thác
Exploit Matter state
Dissolve infinitely
nước
in water
Chất lỏng màu nâu
Reddish-brown
đỏ
liquid
Tinh thể màu tím
Purplish- black
đen
crystalline
Dung dịch HCl đặc
The concentrated
bốc khói trong
HCl solution
O
Trạng thái tập hợp
Tan vô hạn trong
FF IC IA L
Intergrated method
N
Phương pháp tổng
không khí ẩm
“fumes” in moist air
Ơ
Khí clo nặng gấp 2,5 Chlorine gas is 2,5 lần không khí
time havier than air
Calculate the yield /
Tính hiệu suất của phản ứng nhiệt phân
H
natural occurrence Bleach fiber,
bột giấy
textiles,wood pulp
(The efficiency) of the decomposition
N
Tẩy trắng sợi, vải,
Y
Trạng thái tự nhiên
Diêm
Matche
Pale yellow
Quặng sắt pirit
Pyrite ore
Mùi xốc
Pungent
Sơn
Paint
Rất độc
Poisonous
Chế biến dầu mỏ
Oil refining
KÈ
M
Lục nhạt
Q
U
reaction.
Greenish- yellow
Vàng lục
Nén nước siêu
Compress super-hot- Thuốc
nóng
water
ẠY D
Sublimation
Medicine
Tạp chất
Impurrity
Phẩm nhuộm
Dyes
Khí nhà kính
Greenhouse gas
Trơ, khó pư
Unreactive
Bước 2: Một số bài tập điển hình trong chuyên đề Exercise 1. 69.6 g of MnO2 reacts with an excess concentrated HCl solution. The liberated gas is buddle though 500ml of 4M NaOH solution ( at ambient temperature) a) Write the chemical equation of occurring reactions
Trang 40
Sáng kiến kinh nghiệm năm học 2018 - 2019
b) Determine the molar concentration of compounds in the solution after reaction. Give that the volume of solution after reacting does not change much
The number mole of MnO2 =
69.6 0.8 mole 87
The number mole of NaOH =
500 x 4 2 mole 1000
FF IC IA L
Solution
MnO2s + 4HClaq MnCl2aq + Cl2g + H2Ol
a) The reaction:
b) The number mole of Cl2 = The number mole of MnO2 = 0.8 mole Cl2g + 2NaOHaq NaClaq + NaClOaq + H2O
The number mole of NaCl= The number mole of NaClO = The number mole of Cl 2 = 0.8
O
mole
The number mole of NaOH(reacted) = 2 The number mole of Cl2 = 2x0.8=1.6 mole
N
The number mole of NaOH(residual) = 2 - 1.6 = 0.4 mole
500 0.5 liter 1000
N
the volume of solution =
H
Ơ
NaOH : 0.4 mole In the solution after reaction: NaCl : 0.8 mole ; NaClO :0.8 mole
0.4 0.8 M 0.5
U
Y
the molar concentration of NaOH =
Q
the molar concentration of NaCl = the molar concentration of NaClO =
0.8 1.6 M 0.5
M
Exercise 2. (A) mixture consisting NaI and NaCl. Apply the mixture (A) to the excess solution of AgNO3, the precipitate mixture (B) is obtained. Know that the mass of (B) is
KÈ
equal to the mass of AgNO3 is reacted. Calculate the mass percentage of each substance in (A)
ẠY
Solution
Suppose that the mass of (A) mixture equal 100 grams
D
Let the number mole of NaI be a mole Let the number mole of NaCl be b mole We have: 150a + 58.5b = 100 ( 1) The reactions: NaIaq + AgNO3aq NaNO3aq + AgIs b
b
b
mole Trang 41
Sáng kiến kinh nghiệm năm học 2018 - 2019
NaClaq + AgNO3aq NaNO3aq + AgCls
b
b
b
mole
Because the mass of precipitate mixture (B) is equal to the mass of AgNO3 is reacted 170(x+y) = 235x + 143.5y 65x - 26.5y = 0 (2) 150a 58.5b 100 a 0.341 65a 26.5b 0 b 0.836
Therefor the mass percentage of NaI in (A) is:
FF IC IA L
From (1) and (2), we have
0.341x150 100 51.15% 100
the mass percentage of NaI in (A) is: 100% - 51.15% = 48.85%
Exercise 3. There is a mixture of oxygen and ozone. Some time later, ozone is decomposed completely and we get the only one gas with the volume increasing by 2%
O
a) Explain the increasing the volume of the mixture
b) Determine the percentage by volume of the initial mixture
N
( give that the volume is measured at the same temperature and pressure) 3O2g
H
2O3g
Ơ
Solution: The reaction
a) Because, when O3 is decomposed, the number mole of gas increase so increasing the
N
volume of the mixture
Y
b) Let the number mole of initial mixture be 1 mole
U
the number mole of O3 be a mole
the number mole of O2 be b mole
M
The reaction
Q
a + b = 1 mole (1)
KÈ
2O3g a
3O2g 1.5a
the number mole of O2 after reaction is: b + 1,5a = 1+ 2%x1= 1.02 mole (2) a b 1 a 0.04 1.5a b 1.02 b 0.96
D
ẠY
From (1) and (2), we have
Therefor, in the initial mixture: the percentage by volume of O 3 is:
0.04 100 4% 1
the percentage by volume of O 2 is: 100% - 4% = 96% Exercise 4. A mixture of Fe and FeS reacts with an excess amount of HCl solution to form 2,464 litres of gas mixture at STP. This gas mixture is introduced into an excess Pb(NO 3)2 solution to form 23,9 g of black precipitate Trang 42
Sáng kiến kinh nghiệm năm học 2018 - 2019
a) What gases does the collected gaseous mixture contain? What is the volume of each gas at STP b) Calculate the mass of Fe and FeS on the initial mixture? Solution H2 Fe Pb ( NO3 ) 2 HCl ( residual ) 2.464 L 23.9 gPbS FeS H S 2
Let the number mole of Fe be a mole; FeS be b mole The number mole of the gas mixture is: The number mole of PbS is:
2.464 0.11 mole 22.4
23.9 0.10 mole 239
a
a
mole
b
mole
Ơ
b
N
FeSs + 2HClaq FeCl2aq + H2Sg
O
2HClaq FeCl2aq + H2g
The reactions: Fes +
FF IC IA L
The reaction diagram
a) The collected gaseous mixture contain H2S and H2 a + b = 0.11
H
We have
N
H2Sg + Pb(NO3)2aq HNO3aq + PbSs
b
Y
b b= 0.1 mole a = 0.01 mole
U
the volume of H2S at STP is: 0.1x 22.4 = 2.24 L
Q
the volume of H2 at STP is: 0.1x 22.4 = 0.224 L
M
b) the mass of Fe is: 0.01 x 56 = 0.56 grams the mass of Fe is: 0.1 x 88 = 8.8 grams
KÈ
Exercise 5. 12.8 g of SO2 are absorbed completely into 250 ml of 1M NaOH solution. Calculate the mass of the formed salt after the reaction
ẠY
Solution
D
The number mole of SO2 is:
12.8 0.2 mol 64
The number mole of NaOH is:
250 .1 0.25 mol 1000
The ratio of the number of moles between NaOH and SO2 is
0.25 1.25 1; 2 0.2
So the reaction between NaOH and SO 2 occurs according to two equations NaOH
+
SO2
NaHSO3 Trang 43
Sáng kiến kinh nghiệm năm học 2018 - 2019
a
2NaOH + SO2
a
b
a Na2SO3 + H2O
b
b
Let the number mole of NaHSO3 be a mole; Na2SO3 be b mole According to the above equations, the number mole of SO2 is: a + b = 0.2 mol
FF IC IA L
the number mole of NaOH is: a + 2b = 0.25 mol Therefor, a = 0.15 mol ; b = 0.05 mol So, the mass of NaHSO3 is: 0.15 x 120 = 18.0 grams the mass of Fe is: 0.05 x 126 = 6.3 grams
Exercise 6. A metallic foil with a mass of 50 grams immerged in a HCl solution. After the collection of 336 ml of H2 ( at STP), the mass of this metallic foil decreased by 1.68%.
O
Identify this metal. Solution
N
Suppose, the metal (must found) is M with valence is n
Ơ
The reaction: 2 x 0.015 n
H
2M + 2nHCl 2MCln + nH2
N
Y
336 1 0.015 mol . 1000 22.4
U
The number mol of H2 is:
0.015 mol
2 x0.015 0.03 mol n n
Q
The number mol of M is:
M
The mass of M (reacted) is 1.68% x 50 = 0.84 gram
KÈ
The molecular mass of M is:
0.84 28n 0.03 n
n
1
2
3
M
28
56
84
not accept
Accept
not accept
D
ẠY
We have:
Thus, this metal is iron ( Fe) Exercises 7. Which phenonmenon will be observed when chlorine water is added gradually to potassium iodide solution containing a small amount of starch? Write the chemical equations of occurring reactins that you know. Trang 44
Sáng kiến kinh nghiệm năm học 2018 - 2019
Solution when chlorine water is added gradually to potassium iodide solution, we have reaction: Cl2aq + 2KIaq 2KClaq + I2aq I2 (is formed) make a small amount of starch turn into blue solution I2aq + starch the blue solution
FF IC IA L
Bước 3. Bài tập tự luận và trắc nghiệm Bài tập trắc nghiệm
Question 1. Choose the true statement about fluorine, chlorine, bromine, iodine
A. fluorine has very strong oxidative property and can oxidize water intensiverly B. chlorine has strong oxidative property and can oxidize water.
C. bromine has strong oxidative property. Although weaker than that of chlorine, it still
O
can oxidize water
D. bromine has weaker oxidative property than that of fluorine, chlorine, bromine, but
N
it still can oxidize water
Ơ
Question 2. Which of the following series of acids is arranged in order of decreasing acidic
H
property?
C. HI; HBr; HCl; HF.
N
A. HCl; HBr; HI; HF B. HBr; HI; HCl; HF
D. HF; HCl; HBr; HI
U
The role of bromine is
Y
Question 3. In the following reaction : SO2 + Br2 + H2O H2SO4 + 2HBr
Q
A. A reducing agent
B. an oxidizing agent
M
C. An oxidizing agent and simultaneously a reducing agent
KÈ
D. neither An oxidizing agent, nor A reducing agent Question 4. Which of the following acid solutions cannot be stored in glass bottle? A. HCl
B. H2SO4
C. HNO3
D. HF
ẠY
Question 5. A solution containing 1 g of HBr is poured into a solution containing 1 g of
D
NaOH. A litmus paper is dipped into the obtained solution. Which color will the litmus paper turn? A. Red
B. blue
C. the color does not change
D. cannot be determined
Question 6. Choose the right statement in the following statements: A. Choloride of lime is a salt formed by one metal bonding with anions of a single type of acid Trang 45
Sáng kiến kinh nghiệm năm học 2018 - 2019
B. Choloride of lime is a salt formed by one metal bonding with anions of a two type of acids C. Choloride of lime is a salt formed by two metals bonding with anions of a single type of acid of acids
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D. Choloride of lime is a salt formed by two metals bonding with anions of a two type Question 7. Sunfur dioxide can participare in the following reactions SO2 + Br2 + H2O H2SO4 + 2HBr
(1)
SO2 + 2H2S 3S + 2H2O
(2)
Which of the following statements wrongly expresses the properties of the reactants above?
O
A. Reaction (1): SO2 is a reductant, Br2 is an oxidant
B. Reaction (2): SO2 is an oxidant, H2O is a reductant
N
C. Reaction (2): SO2 is both an oxidant and a reductant
Ơ
D. Reaction (1): HBr is a reductant, H2SO4 is an oxidant
H
Question 8. Match the pairs of substances to their properties properties
N
Substances
1 has oxidative property
B. SO2
2. has reductive property
Y
A. S
3. has oxidative and reductive property
U
C. H2S
4. gas, has oxidative and reductive property
Q
D. H2SO4
5. has neither oxidative nor reductive property
M
A: 3; B: 4; C:2; D:1
KÈ
Question 9. Given the chemical reactions H2S + Cl2 + H2O H2SO4 + HCl Which of the following statements correctly expresses the properties of the reactants ?
ẠY
A. Cl2 is a reductant, H2S is an oxidant
D
B. H2S is a reductant, H2O is an oxidant C. H2O is a reductant, Cl2 is an oxidant D. H2S is a reductant, Cl2 is an oxidant
Question 10. A compound has the mass composition of 35,96% of S; 62,92% of O and 1,12% of H. The chemical formula of this compound is? A. H2SO3
B. H2SO4
C. H2S2O7
D. H2S2O8
Question 11. The oxidation state of sulfur in a type of oleum compound H 2S2O7 is: Trang 46
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. +2
B. +4
C. +6
D. +8
Question 12. Give the chemical equation a) SO2 + Br2 + H2O H2SO4 + 2HBr b) SO2 + H2O H2SO3 d) SO2 + 2H2S 3S + 2H2O e) SO2 + O2 SO3 1. SO2 is the oxidant in the following chemical reactions A. a,d,e
B. b , c
C. d
FF IC IA L
c) SO2 + KMnO4 + H2O K2SO4 + MnSO4 + H2SO4
2. SO2 is the reductant in the following chemical reactions A. bdec
B. ace
C. ade
B. 1s22s22p4
C. 1s22s22p2
Question 14. What bond is oxygen molecular?
B. Ion bond
Ơ
A. Polar covalent bond
D. 1s22s22p63s2
N
A. 1s22s22p6
O
Question 13. Which of the following configuration is the configuration of the oxygen atom:
D. Receiving bond
H
C. Non-polar covalent bond A. O-O
B. O=O
N
Question 15. Which is the true structural formula of oxygen?: D. O ≡ O
C. O→O
Y
Question 16. How many statements is true in the following statementsare?
U
1. Oxygen is a colorless gas and shock smell.
Q
2. Oxygen is a colorless, odorless and tasteless gas. 3. Oxygen is well-dissolved in water. B. 2
C. 3
KÈ
A. 1
M
4. Oxygen is denser than air. D. 4
Question 17. What is basic chemical properties of oxygen ? A. Strongly oxidizing
B. Strongly reducing
ẠY
C. Have both oxidizing and reducing properties
D. Weakly oxidizing
D
Question 18. How many statements are wrong in the following statements? 1. Oxygen maintains the life and the fire. 2. Oxygen is used for welding 3. Oxygen has many applications in the metallurgical industry 4. Liquid oxygen is yellow color
A. 1
B. 2
C. 3
D. 4
Question 19. What is the method of preparing oxygen in the laboratory? Trang 47
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. Electrolysis of water
B. Fractional distillation of liquid air
C. Temperature distribution KMnO4
D. All three ways above
Question 20. What is location of oxygen in the periodic table? B. 10th cell, 2 period, IVA group
C. 8th cell, 3 period, IIA group
D. 10th cell, 3 period, IIA group
Question 21.
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A. 8th cell, 2 period , VIA group
Question 22. The electron configuration of oxygen atom is 1s 22s22p4. After chemical reaction, the electron configuration of O2- ion is: A. 1s22s22p4
B. 1s22s22p43s2
C. 1s22s22p6
D. 1s22s22p63s2
Question 23. O2 mixing a few impurities Cl2. What is the best chemical to remove Cl2? A. H2O.
C. SO2.
B. KOH.
D. KI.
O
Question 24. When pyrolysis 24.5 grams of KClO3 by the reaction: 2KClO3 MnO 2 2KCl + 3O2. B. 6.72 liter
C. 2.24liter
Ơ
A. 4.48liter
N
The volume of obtained oxygen (standard conditions) is:
D. 8.96 liter
H
Question 25. The mass ratio of a mixture of O2 and CO2 with hydrogen is 19. The average
N
mol mass of the mixture and percentage of O 2 by volume is: A. 40 grams and 40%
B. 38 grams and 40%
Y
C. 38 grams and 50%
D. 36 grams and 50%
U
Question 26. How many moles of FeS2 react with oxygen to obtain 64 grams of SO2
Q
according to the following chemical equation: 4FeS2 A. 0.4
B. 1.2
+ 11O2
C. 0.5
→ 2Fe2O3+ 8SO2
D. 0.8
M
Question 27. The mass ratio of a mixture of SO2 and O2 with hydrogen is 24. How many
KÈ
liters of oxygen need added to 20 liters of this mixture to make mass ratio of the new mixture with hydrogen become 22.4. A. 5liters
B. 7.5 liters
C. 8 liters
D. 10 liters
ẠY
Question 28. Burning substance X with sufficient oxygen gas, we obtained only mixture of
D
CO2 and SO2 which has the mass ratio compared with hydrogen gas was 28.667 and the mass ratio of X compared with the air is smaller than 3. What is the formula of X : A. CS
B. CS2O
C. CS2
D. C2S
Question 29. The oxidation number of sulfur (S) in H 2S, SO2, SO32-, SO42- in order? A. +4, +6, +8.
B. -2, +4, +4, +6.
C. +2, +4, +8, +10.
D. 0, +4, +3, +8. Trang 48
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 30. For chemical reaction: Cl2 + KOH KCl + KClO3 + H2O The ratio between the chlorine atoms are oxidants and chlorine atoms as a reducing agent in the chemical equation of reaction gave respectively A. 5: 1.
B. 1: 3.
C. 3: 1.
D. 1: 5.
Question 31. Dissolve completely 2.81 gram mixture of Fe2O3, MgO, ZnO in 500 ml of mixture of anhydrous sulphate. The value of m is
A. 6,81 gam.
B. 4,81 gam.
C. 3,81 gam.
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0.1M H2SO4 acid (barely). After the reaction, evaporated the solution obtained m gram the
D. 5,81 gam.
Question 32. Calculate the volume of O2 (under standard conditions) required to burn completely 6.8 grams of NH3 to form NO and H2O gas. B. 8.96 liters
C. 13.44 liters
D. 16.8 liters
O
A. 11.2 liters
Question 33. Sulfur reacts with hot, concentrated sulfuric acid according to the equation:
N
S + 2H2SO4 3SO2 + 2H2O
Ơ
In this reaction, the ratio of sulfur atoms are reduced and the number of sulfur atoms are
B. 2: 1
C. 1: 2
D. 1: 3
N
A. 3: 1
H
oxidized is
Question 34. in the following reactions, the reaction which is not a redox reaction C. H2SO4 + Fe Fe2(SO4)3 + SO2 + H2O
B. H2SO4 + FeSO3 FeSO4 SO2+ H2O
D. H2SO4 + FeO Fe2(SO4)3 + SO2 + H2O
U
Y
C. H2SO4 + Fe FeSO4 + H2
Q
Question 35. The following diagram is given:
M
(1) (2) (3) (4) ( 5) (6) (7) Cl2. S CuS SO2 SO3 H2SO4 H2 HCl
What reactions are not redox reactions?
KÈ
A. (1), (2), (3), (4), (5)
B. (4), (5), (6), (7)
C. (4), (6)
D. (4)
Question 36. The following diagram is given :
ẠY
(1) ( 2) (3) (4) (5 ) (6) (7 ) H2S S SO2 SO2 SO3 H2SO4 H2. Na2SO3
D
How many reactions are Redox reaction?
A. 4
B. 5
C. 6
D. 7
Một số bài tập tự luận Exercises 1. An amount of a halogen reacts completely with magnesium to form 19 grams of magnesium halide. The same of this halogen reacts completely with aluminum to form 19 grams of aluminum halide. Determine the name of the halogen and the mount of the halogen has been used Trang 49
Sáng kiến kinh nghiệm năm học 2018 - 2019
Exercises 2. Calculate the mass of CaF2 used to synthesize 2,5kg of 40% hydrofluoric acid solution. Give the efficiency of the reaction is 80% Exercises 3. An oxygen gas contains chlorine gas an impurity. How to remove this impurity Exercises 4. 69,6 g of MnO2 reacts with an excess concentrated HCl solution. The c) Write the chemical equation of occurring reactions
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liberated gas is buddle though 500ml of 4M NaOH solution ( at ambient temperature)
d) Determine the molar concentration of compounds in the solution after reaction. Give that the volume of solution after reacting does not change much
Exercises 5. 300 ml of a solution dissolving 5,85 g of NaCl allows to react with 200ml of a solution containing 34 g of dissolved AgNO3 to form a precipitate and filtrate
O
a) Caculate the mass of obtained precipitate.
e) Determine the molar concentration of compounds remained in the filtrate. Give that
N
the volume of solution after reacting does not change much
Ơ
Exercises 6. A solution contains two dissolved NaBr and NaCl salts. The percentage of each salt in the solution is similar and equal C%. Determine the concentration C% of two
H
salts in the solution, give that 50 g of the solution of this two salts reacts completely with
N
50ml of 8% AgNO3 solution with a density of D = 1,0625 g/cm3 Exercises 7. A mixture of 0,65 g of zinc powder and 0,224 g of sunfur powder is heated in
Y
a closed test tube without air. After the reaction, what substances are obtained in the test
U
tube? What are their masses?
Q
Exercises 8. Give the reactions to prove that chlorine has stronger oxidative property than bromine and fluorine
M
Exercises 9. There is a mixture of oxygen and ozone. Some time later, ozone is decomposed completely and we get the only one gas with the volume increasing by 2%
KÈ
c) Explain the increasing the volume of the mixture d) Determine the percentage by volume of the initiate mixture
ẠY
( give that the volume is measured at the same temperature and pressure)
Exercises 10. 1,1 g of mixture of iron and aluminium powder reacts completely with 1,28 g
D
of sulfur powder. Calculate the percentage in mole and mass between iron and aluminium in the initial mixture Exercises 11. How do the reactions of halogen elements with water occur? Write chemical equation of occurring reactions, if any. Exercises 12. Given that NaCl salt contains NaI as impurity a) How is it proved that NaI exists in that sample of NaCl above as impurity Trang 50
Sáng kiến kinh nghiệm năm học 2018 - 2019
b) How is NaCl purified? ( How to remove NaI to obtain pure NaCl) Exercises 13. In STP, a litre of water can dissolve 350 litres of HBr gas. Caculate the percentage of the formed hydrobromic acid solution Exercises 14. 1,03 g of sodium halide (A) react with an excess of AgNO 3 solution to form a precipitate, this precipitate decomposes completely to form 1,08 g of silver. Determine the Exercises 15. a) How to identify NaF and NaCl solution?
FF IC IA L
mane of salt A b) How to remove NaI in the sample of iodine?
Exercises 16. In the laborary there are calcium oxide, water, MnO2, H2SO4 acid 70%
(D = 1,61g/Cm3) and NaCl. Which substances are needed and how much are they needed to synthesize 254 g of chloride of lime 3.2. Các chuyên đề lớp 11.
O
3.2.1. Chuyên đề: Dissociation ( Sự điện li) Amphoteric Acidic salts Neutral salts
Y
Muối trung hòa
Acid anion radicals
Strong electrolyte
li mạnh
solutions
Phương trình ion thu Net ionic equation gọn Môi trường tung
Neutral environment
tính Hòa tan
Dissolve
Axit nhiều nấc
Polyprotic acids
chất điện ly yếu
weak electrolyte
The acid- base
chất điện ly mạnh
Strong electrolyte
M
Monoprotic acids
KÈ
Q
U
Anion gốc axit Axit một nấc
Dung dịch chất điện
N
Muối axit
Conduct electricity
H
hydroxide
Dẫn điện
Ơ
Hidroxit lưỡng tính
N
Bước 1: Các từ mới trong chuyên đề
Phản ứng axit- bazo
reaction
ẠY
Bước 2: Một số bài tập điển hình trong chuyên đề
D
1. In a solution contains Ca2+: a mole, Mg2+: b mol, Cl-: c mol ,NO3- : d mol. a / Making contact expressions a, b, c, d. b / If a = 0.01; c = 0.01; d = 0.03, how much b ? Solution: a / In a solution, the total charge of the cations equals the total charge of the anion, so: 2a + 2b = c + d Trang 51
Sáng kiến kinh nghiệm năm học 2018 - 2019
b/ If a = 0.01; c = 0.01; d = 0.03 b
c d 2a 0.01 0.03 2 x0.01 0.01 2 2
2. For m g of sodium in water, we obtain 1.5 liters solution which has pH = 13. Calculate m. pH 13 H 1013 OH 101 = 0.1M
2Na + 2H2O→ 2Na+ + 2OH- +
H2↑
FF IC IA L
Solution:
The number of moles of OH- in 1.5 liters solution: 0.1x1.5 = 0.15 (mol) number of moles Na = number of moles of OH -= 0.15 (mol) Mass of Na = 0.15 x 23 = 3.45 (g) Bước 3: Một số bài tập
O
Question 1. Which of the following is the Arrhenius definition of a base? B. A base is a substance that accepts protons.
N
A. A base is a substance that donates protons.
Ơ
C. A base is a substance that dissolves in water to form OH- ions.
H
D. A base is a substance that reacts with water to form H + ions.
N
Question 2. Which compound is a strong acid? A. HClO2(aq)
B. H2CO3(aq)
C. HCOOH(aq)
D. HClO4(aq)
B. HClO4(aq)
U
A. CH3COOH(aq)
Y
Question 3. Which one of the following compounds is not a strong electrolyte? C. HI(aq)
D. NaOH(aq)
Q
Question 4. If 22.50 mL of a sodium hydroxide is necessary to neutralize 18.50 mL of a 0.1430 mol/L HNO3 solution, what is the concentration of NaOH?
M
A. 0.1 176 mol/L
B. 0.1430 mol/L
C. 0.1740 mol/L
D. 2.64 mol/L
KÈ
Question 5. If the pH of an unknown solution is 4.25, what is the pOH? A. 10-4.25
B. 10-9.75
C. 9.75
D. 14.0 - 10-9.75
Question 6. A solution contains a hydronium ion concentration of 3.36 x 10-4mol/L.
ẠY
What is the pH of the solution?
D
A. 3.36
B. 3.47
C. 10.53
D. none of the above
Question 1.Which of the following is a weaked electrolyte in water environment? A. H2S, H2SO3, H2SO4, NH3.
B. H2CO3, H3PO4, CH3COOH, Ba(OH)2.
C. H2S, CH3COOH, HClO, NH3.
D. H2CO3, H2SO3, HClO, Al2(SO4)3.
Question 6. There are some solutions that have the same molar concentration: HNO3; CH3COOH; NH3; NaCl; NaOH. The arranged sequence that is in ascending order of pH is: Trang 52
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. HNO3; CH3COOH; NH3; NaCl; NaOH. B. HNO3, CH3COOH; NaCl; NH3; NaOH. C. HNO3; NH3; CH3COOH; NaCl; NaOH. D. CH3COOH; HNO3; NaCl; NH3; NaOH. Question 7. The sequence consisting of substances that all react to Ba(HCO3)2 solution is: B. HNO3, Ca(OH)2, KHSO4
C. NaCl, Na2SO4, Ca(OH)2.
D. HNO3, Ca(OH)2, Mg(NO3)2.
FF IC IA L
A. HNO3, NaCl, Na2SO4.
Question 8. 23.4 grams of amixture of Na, K are dissolved completely in 500 ml of HCl
solution. After that, we obtained 6.72 liters of gas at standard temperature and pressure and an after-reaction solution has pH of 13 . The volume of solids obtained when evaporating completely the after-reaction solution is: B 42,925 grams
C. 43,475 grams
O
A. 43,775 grams
N
Question 9. There are several following reactions:
D. 41,950 grams
(2) Na2CO3 solution + FeCl3solution.
(3) Na2CO3 solution + CaCl2 solution.
(4) NaHCO3 solution + Ba(OH)2 solution. (6) Na2S solution + AlCl3 solution.
H
(5) (NH4)2SO4 solution + Ba(OH)2solution.
Ơ
(1) Na2CO3 solution + H2SO4solution.
A. 3.
B. 6.
N
The number of reactions that produce both precipitate and air are: C. 4.
D. 5.
Y
Question 10: The solubility of NaCl in 100 grams of water at 900C and at 00C are50 grams
U
and 35 grams in order. The process ofcooling 600 grams of saturated NaCl solution at 90 0C A. 45 grams.
Q
to 00C creates the volume of NaCl crystals. How much is this volume? B. 55 grams.
C. 50 grams.
D. 60 grams.
M
Question 11. The X mixture contains K2O, NH4Cl, KHCO3 and BaCl2 that have the same mole.
KÈ
X is heated with the residual amount of water. The solute(s) in the obtained solution is(are): A. KCl, BaCl2
B. KCl, KOH
C. KCl, KHCO3, BaCl2
D. KCl
Question 12. After slowlypouring300 ml a solution containingNaHCO 3 0.1M; K2CO3 0.2M
ẠY
into 100 ml a solution containing HCl 0.2M; NaHSO4 0.6M, we obtain V liter CO 2 at
D
standard temperature and pressureand solution X. 100 mL a solution containing KOH 0.6M ; BaCl2 1.5M is added to X solution. After that,we obtain m grams precipitates. The volume of V and m are: A. 0,448 lít và 11,82g
B. 0,448 lít và 25,8g
C. 1,0752 lít và 23,436g
D. 1,0752 lít và 24,224g
Question 13. X solution contains KNO3 and H2SO4. Each of the following substances: Fe2O3, Trang 53
Sáng kiến kinh nghiệm năm học 2018 - 2019
FeCl2, Cu, FeCl3, Fe3O4, CuO, FeO are reacted to X solution. The number of redox reactions occuring is: A. 5
B. 4
C. 3
D. 2
Question 14. Conduct the followingexperiments: (1) Aerationof H2S into FeSO4 solution.
FF IC IA L
(2) Aerationof H2S into CuSO4 solution. (3) Aerationof CO2 (excess) into Na2SiO3 solution. (4) Aerationof CO2 (residual) into Ca(OH)2solution. (5) Add the excess NH3 solution to Al2(SO4)3 solution. (6) Slowlyadd Ba(OH)2 solution to Al2(SO4)3 solution.
After reactions finish, the number of experiments that create precipitates is: B. 4.
C. 3.
D. 6
O
A. 5.
Question 15.. Choose the correct answer in the following subtances:
N
The solution of electrolyte conducts electricity due to
B. The moving of cations. D. The moving of both cations and anions.
H
C. The moving of dissolved molecules.
Ơ
A. The moving of electrons.
N
Question 16.. Which of the following subtances does not conduct electricity? B. Molten CaCl2
C. Molten NaOH
D. HBr dissolved in water.
Y
A. Dried, solid KCl.
U
Question 17.. Which conclusion is correct according to the Arrhenius theory?
Q
A. A compound which contains hydrogen atoms as its component is an acid. B. A compound which contains OH groups as its component is a base.
M
C. A compound which is able to dissociate into H + cation in water is an acid.
KÈ
D. A base does not have to contain OH groups in its molecules. Question 18.. For the 0.01M of weak CH 3COOH acid solution, if ignoring the dissociation of water, which of the following judgements about the molarity of ions is correct?
ẠY
A. [H+]=0.01M
B. [H+]> [ CH3COO-]
C. [H+] < [CH3COO-]
D. [H+]< 0. 10M
D
Question 19.. For the following of strong HNO3 acid solution, if ignoring the dissociation of water, which of the following judgements about molarity of ions is correct? A. [H+] =0.01M
B. [H+]> [ NO3-]
C. [H+]< [NO3-]
D. [H+]<0. 10M
Question 20.. A solution has [OH-] of 1.5x10-5M. This solution is A. acidic
B. neutral
C. alkaline
D. unknown
Question 21.. A net ionic equation shows: A. What ions exist in the solutions Trang 54
Sáng kiến kinh nghiệm năm học 2018 - 2019
B. Ions with the highest concentration in a solution C. The nature of the reaction in the solution of electrolytes. D. Molecules do not exist in the solution of electrolytes. Question 22.. Which of the following reactions occuring in the solutions form Fe(OH) 3 precipitate? B. Fe2(SO4)3+ KI
C. Fe(NO3)3+Fe
D. Fe(NO3)3+KOH
FF IC IA L
A. FeSO4+ KMnO4+ H2SO4
Question 23. An ion- exchange reaction in the solution of electrolytes occurs only when A. The reactants are well soluble. B. The reactants are strong electrolytes
C. Some ions in the solution combine to reduce their ionic concentration
O
D. The reaction is nonreversible
Question 24.. Which of the following pairs of subtances forms CdS precipitates in the
N
solution?
B. Cd(NO3)2+ H2S
C. Cd( NO3)2+ HCl
D. CdCl2+ Na2SO4
H
Ơ
A. CdCl2+ NaOH
N
Question 25. A solution containing the following ions. Ba 2 ,Ca 2 ,Mg 2 , Na , H , Cl To remove the more cation from the solution without adding new ion to the solution, We
Y
should let that solution react with what the following solution? B. Na2CO3 solution just enough
C. K2CO3 solution just enough
D. NaOH solution just enough
Q
U
A. Na2SO4 solution just enough
Question 26. Add the excess Na2CO3 solution into the HCl solution, the resulting solution
KÈ
A. 7
M
has a pH of
B. <7
C.> 7
D. Not determined
Question 27. Solution X contains a mol NaHCO3 and mol Na2CO3. Perform the following experiments
ẠY
Experiment 1: give (a + b) mol CaCl2. into solution X
D
Experiment 2: Give (a + b) mol Ca(OH)2 into solution X
The mass of precipitation obtained in the each experiments was: A. Equal
B. Experiment 1 is more than experiment 2
C. Experiment 2 is more than experiment 1
D. Not comparable
Question 28. Saline X do turn litmus paper to blue . Salt solution Y does not change the color of litmus paper. Mix X and Y are found precipitate. X and Y are the following pairs A. NaOH ; K2SO4
B. NaOH ; FeCl3
C. Na2CO3 ; BaCl2
D. K2CO3 ; NaCl Trang 55
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 29. Slowly add the solution containing a mole of HCl to the solution containing b mole Na2CO3 and stirring, Obtained V liters of gas (at STP) and solution X. When add the lime water into X, there is a precipitate. The relationship between V and a and b is: A. V = 22.4(a-b)
B. V = 11.2(a-b)
C. V = 11.2(a+b)
D. V = 22.4(a+b)
Question 30: Lead 0.6 mol of CO2 into 250 ml of Ba(OH)2 x mol / l solution to obtain 78.8 precipitation. The value of x and m is A. 4 và 5.
B. 2 và 19,7.
C. 2 và 39,4.
Bài tập tự luận
FF IC IA L
g of precipitate. Remove the precipitate, heat the solution after reaction, we obtain m gram D. 4 và 10.
Exercise 1: Why is it that the solutions of acids such as HCl, bases such as NaOH and salts such as NaCl to conduct electricity, while the solutions such as ethanol, sucrose and glycerol solutions do not?
O
Exercise 2: What is the dissociation? What is an electrolyte?
What types of subtances are electrolytes? What are strong electrolytes? What are weak
N
electrolytes? Give examples and write their dissociation equations.
Ơ
Exercise 3: Write the dissociation equations of the following substances:
H
a. Strong electrolytes : Ba(NO3)2 0. 10M; HNO3 0.020M; KOH 0.01M. Calculate the
N
molarity of each ion in the above solutions. b. Weak electrolytes: HClO, HNO2
Y
Exercise 4: State the definitions of acids, monoprotic acids, polyprotic acids, amphoteric dissociation equation.
U
hydroxides, neutral salts, and acidic salts. Give the illustrative examples and write their
Q
Exercise 5: Write the dissociation equations of the following substances:
M
a. Weak acids: H2S, H2CO3 b. Strong base: LiOH
KÈ
c. Salts: K2CO3, NaClO, NaHS d. Amphoteric hydroxide: Zn(OH)2 Exercise 6: What is the ion product of water? What is its value at 25 ͦ C
ẠY
Exercise 7: State the definitions of acidic, neutral and alkaline ( basic) solutions based on
D
H+ concentration and pH. Exercise 8: What is an acid-base indicator? Give the color of litmus and phenolphatalein in the solutions over different ranges of pH. Exercise 9: Calculate the concentrations of H+, OH- and pH of a 0. 10M HCl solution and a 0.010M NaOH solution.
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Exercise 10: Write the molecular equation and net ionic equation of the reactions ( if any) occuring in the solutions of the following pairs of subtances: a. Fe2(SO4)3+ NaOH
d. MgCl2+ KNO3
b. NH4Cl+ AgNO3
e. FeS+ HCl
c. NaF+ HCl
g. HClO+ KOH
FF IC IA L
Exercise 11: Give the examples and write the molecular and net ionic chemical equations for the following reactions: a. Forming precipitates b. Forming weak electrolytes c. Forming gases
Exercise 12: Write the dissociation reactions of the following subtances: K2S, Na2HPO4,
O
NaH2PO4, Pb(OH)2, HBrO, HF, HClO4
Exercise 13: A solution has the [H+] concentration of 0.01M. Calculate the [OH-] and the
N
pH of the solution. Is this solution acidic, neutral or alkaline? Show the color of purple litmus in this solution.
Ơ
Exercise 14: A solution has the pH of 9.0. Calculate the molarity of H+ and OH- ions in the
H
solution. Show the color of phenolphtalein in this solution.
N
Exercise 15: Write the molecular and net ionic equation of the reactions ( if any) which occur in the solutions of the following subtances:
g. Pb(OH)2+ HNO3
Q
e. K2CO3+ NaCl
d. NaHCO3+ NaOH
U
c. NaHCO3+ HCl
b. FeSO4+ NaOH ( dilute)
Y
a. Na2CO3+ Ca(NO3)2
h. Pb(OH)2+ NaOH
i. CuSO4+ Na2S
M
Exercise 16: Write the ( molecular and net ionic) chemical equations of the ion- exchange reactions in the solutions forming each of the following precipitates: Cr(OH)3, Al(OH)3,
KÈ
Ni(OH)2
3.2.2. Chuyên đề: Nitrogen – phosphorus (Nhóm Nito- Photpho)
D
ẠY
Bước 1: Các từ mới trong chuyên đề Nitrogen fertilizer
Phân đạm
Plant ash
Tro thực vật
Nitrates fertilizer n
phân bón nitrat
Mutinutrient
Phân hỗn hợp
fertilizer
(NH4)2HPO4; KNO3
(containing two or
( nitrophotka)
more basic nutritional elements) Trang 57
Sáng kiến kinh nghiệm năm học 2018 - 2019
Phân đạm amoni
Urea
Complex fertilizer
Phân phức hợp
(is mixture of
Amophos
substances formed
(NH4)2HPO4;
by reaction)
NH4H2PO4
Ure (H2N)2CO
Micronutrient fertilizer
Photphorus fertilizer Phân lân
Fumes/ fume
Single
Supephotphat đơn
The fractional
superphotphat
Ca3(PO4)2 +
distillation of liquid
H2SO4đặc →
air
Supephotphat kép
superphotphat
Ca3(PO4)2 +
Pollutant
N
→ Ca(H2PO4)2
Chất gây ô nhiễm
H
Ca3(PO4)2 + H3PO4
Phân lân nung chảy
Y
Fused phosphate
KÈ
M
Aqua regia
Khí màu nâu đỏ
/brownish-red gas Inert environment:
Môi trường trơ
Phân Kali
Black dynamite/
Thuốc nổ đen/ thuốc
smoke dynamite
nổ khói
Emit light in the
Phát quang trong tối
Q
Potassium fertilizer
Reddish-brown gas
Đất chua
U
Sour soil
đoạn không khí lỏng
Ơ
H2SO4đặc → H3PO4 +CaSO4
Chưng cất phân
N
Double
Khói/ bốc khói
O
Ca(H2PO4)2 +CaSO4
Phân vi lượng
FF IC IA L
Ammonia fertilizer
Nước cường thủy
dark Bột nở NaHCO3
Laughing gas
Khí gây cười
Greenhouse gas
Khí nhà kính
passivation
Thụ động
ẠY
Baking powder
D
Bước 2: Một số bài tập điển hình trong chuyên đề Exercise 1 : A type of phosphate ore contains 35% of Ca3(PO4)2. Calculate the percent content of P2O5 in the above ore. Solution: Suppose we have 100 grams of ore m Ca3(PO4)2 = 35 grams The number mol of P2O5 = the number mol of Ca3(PO4)2 =
35 mol 310 Trang 58
Sáng kiến kinh nghiệm năm học 2018 - 2019
35 x 142 = 16.03 grams 310
the mass of P2O5 =
the percent content of P2O5 in the above ore is:
16.03 x100% 16.03% 100
Exercise 2: When dissolving 30.0g of a mixture of copper and copper (II) oxide in 1.50
FF IC IA L
liters of 1.00 M ( dilute) nitric acid, 6.72liters of nitrogen monoxide ( at STP) are observed to escape from the reaction mixture. Determine the percent content of copper (II) oxide in the mixture, molarity of copper (II) nitrate and nitric acid in the solution after reaction, given that the solution volume is unchanged. Solution: Cu 1.5 L of HNO3 1M 30 g 6.72 L NO CuO
N
Let the number mol: of Cu be a mol, of CuO be b mol
O
We have diagram:
Ơ
64a + 80b = 30 The reactions equation: 8 a 3
a
N
a
H
3Cu(s) + 8HNO3(aq) 3Cu(NO3)2(aq) + 2NO(g) + 4H2O(l) 2 a 3
b
U
2 3
a =
2b
6.72 = 0.3 mol a = 0.45 mol b = 0.015 mol 22.4
Q
b
Y
CuO(s) + 2HNO3(aq) Cu(NO3)2(aq) + H2O(l)
M
a) The percent content of copper (II) oxide in the mixture:
80 x0.015 100% 4% 30
ẠY
KÈ
b) In the solution after reaction has: Cu(NO 3)2: a+b = 0.45 + 0.015 = 0,465 mol
8 3
HNO3(residua): 1.5x1 – ( a + 2b) = 0.27 mol
D
In the solution after reaction has, molarity of copper (II) nitrate: molarity of HNO3 residua :
0.465 0.31M 1.5
0.27 0.18M 1.5
Exercise 3: 6.2 g of phosphorus is burned completely in excess of oxygen. The formed product reacts equivalently with 32% NaOH solution to form Na2HPO4. a. Write the chemical equations of the occurring reactions. Trang 59
Sáng kiến kinh nghiệm năm học 2018 - 2019
b. Calculate the mass of the NaOH solution used. c. Calculate the percent concentration of salts in the obtained solution after the reaction. Solution: a. Write the chemical equations of the occurring reactions. 4P(s) + 5O2(g) 2P2O5(s)
b. The number mol of P is:
FF IC IA L
P2O5(s) + 4NaOH 2Na2HPO4 + H2O 6.2 0.2 mol 31
4P(s) + 5O2(g) 2P2O5(s)
0.2
0.1 mol 0.2 mol 0.4 x 40 50 g 32%
Ơ
the mass of the NaOH solution used is:
N
0.4 mol
0.1
O
P2O5(s) + 4NaOH 2Na2HPO4 + H2O
H
c) the solution after the reaction contain: Na2HPO4: 0.2 mol
N
The mass of the solution after the reaction equal: mP O msolution of NaOH 0.1x142 50 64.2 g 2 5
U
Y
the percent concentration of salts in the obtained solution after the reaction C% Na2HPO4 =
0.2 x142 44.24% 64.2
Q
Bước 3: Một số bài tập tự luyện
Question 1: Nitrogen gas is relatively inert at normal temperature due to:
M
A. Nitrogen has a small atomic radius.
KÈ
B. Nitrogen has a high electronegativity C. In the nitrogen molecule, each nitrogen atom has a pair of non-bonded electron .
ẠY
D. In nitrogen molecular exists triple bond. Question 2: In the laboratory, pure nitrogen is prepared from.
D
A. air
B.NH 3, O2
C.NH4NO2 or mixed solution NaNO2 and NH4Cl
D.Zn and HNO3
Question 3: Nitrogen is oxidized in reaction to what substance A. H2
B. O2
C. Li
D. Mg
Question 4: In compounds, nitrogen has the maximum covalent value: A. 2
B. 3
C. 4
D. 5 Trang 60
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Question 5: In industry, most of the nitrogen is used for A. Creating an inert environment in metallurgy, electronics ... B. synthetic nitrogen fertilizer. C. production of nitric acid. D. ammonia synthesis
FF IC IA L
Question 6: To balance the ammonia synthesis reaction shifted to the right, must A. increase P and increase temperature. B. increase P and decrease temperature C. decrease P and decrease temperature. D. decrease P and increase temperature.
Question 7: Add 100ml of 0.1M NaOH solution to 10 mL of 1M NH4Cl solution (with a
O
few drops of purple litmus) then boil. What color is the solution before drop NaOH solution and after boiling ? Question 8: Has the following properties:
D. colorless, blue
H
1. Dissolves in water
C. red, purple
N
B. red, colorless
Ơ
A. red, blue
3. reacts with alkaline solution
Y
4. Strong basics
N
2. Lighter than air
U
5.Make moist litmus paper turn blue
Q
6. Create white smoke with HCl gas 7. Produced in the industry by the pyrolysis of ammonium salt
M
The properties of NH3 are: B. 1,4,5,6
KÈ
A. 1,2,4,6
C. 1,2,5,6
D. 2,3,4,7
Question 9: In the lab, what method do you use to collect NH3? B. Collection over water
D
ẠY
A. Collection by downward delivery
C. Collection by upward delivery
D. All three can be used Trang 61
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Question 10: In the lab, what method do you use to collect N 2? B. Collection over water delivery
FF IC IA L
A. Collection by downward delivery
D. All three can be used
N
H
Ơ
N
O
C. Collection by upward
Question 11: Give the following statements:
Y
1. The electron configuration of the outermost layer of the nitrogen element is 2s 22p3
U
2. Because there are five electrons in the outermostlayer, in compounds the nitrogen
Q
element can express the oxidation number +5 and the valence V 3. N2 is capable of expressing oxidation and is capable of expressing reduction
KÈ
catalysis
M
4. Because there are triplebonds , all the reactions that N2 involved need temperature, 5. Formula of laughing gas is N2O 6. Most of the amount of N2 is prepared in the industry is used to produce nitrogenous
ẠY
fertilizer.
D
The number of correct statement is: A. 2
B. 3
C. 4
D. 5
Question 12: Give a gas mixture consisting of: H 2; N2; CO2; SO2; H2S; NH3; O2. Conducted gas mixture through concentrated solution of NaOH, obtained gas mixture Y. The composition of mixture Y consists of: A. H2; N2; NH3
B. H2; N2; O2
C. CO2; SO2; H2S
D. H2; N2; O2; NH3 Trang 62
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Question 13: Which of the following gas mixtures can be reacted under appropriate conditions? A. O2 và Cl2
B. Cl2 và N2
C. O2 và CO2
D. N2 và O2
Question 14: Which of the following gas mixture always exists (even when heated) A. Cl2 và HI
B. O2 và N2
C. N2 và Cl2
D. Cl2 và NH3
FF IC IA L
Question 15: in the laboratory, when rearranging chemicals, you accidentally lose a label of chemical vial containing colorless solution.You suspect it is a solution of ammonium sulfate.Choose a reagent to check if the jar is ammonium sulphate A. Ba(OH)2 B. NaOH
C. BaCl2
D. Limut paper
Question 16: Which method use to collect gas is not appropriate to the scope of application A. Collection by downward delivery: This method is used for gases which are soluble in
O
water but more dense than air
N
B. Collection over water: It is the best method of collecting a gas so long as the gas is insoluble or slightly soluble in water
Ơ
C. Collection by upward delivery: This method is used for gases which are soluble in
H
water but less dense than air dense or less dense than air.
N
D. Collection over water: This method can not be used for insoluble gases which are more
Y
Question 17: Which of the following gases are prepared and collected by the following
KÈ
M
Q
U
method?
B. H2; SO2; O2
C. CO2; H2
D. NH3; NO2; SO2
ẠY
A. Cl2; HCl; O2
Question 18: Which of the following gases are prepared and collected by the following
D
method?
Trang 63
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. Cl2; SO2; NO2
B. H2; N2; O2
C. CO2; H2; O2
D. NH3; NO2; HCl
Question 19: Match Column 2 and Column 3 to fit with the keyword in Column 1 Key word
Definitions
Example
1. melting
A. changing from a gas to a liquid
S. sugar disappearing into
2. evaporation
3. dissolving
FF IC IA L
water B. the liquid in which a solid dissolves to T. when molten iron form a solution
solidifies
C. changing from a solid to a liquid
U. water changing to water vapour
D. a solid that dissolves in a liquid to make a solution E. changing from a liquid to a gas
W. when steam forms water
Ơ
N
5. solute
V. salt water
O
4. solution
F. the mixture formed when a solid
H
6. solvent
on a cold surface X. the salt in salt water
N
‘disappears’ into a liquid
G. changing from a liquid to a solid
Y. ice changing to water
8. freezing
H. when a solid is mixed with a liquid
Z. the water in salt water
U
Y
7. condensation
2. –E - U
M
1. – C - T
Q
and seems to disappear 3. H. S
5. D. X
7. A. W
4. F. V
6. B. Z
8. G. Y
KÈ
Question 20: Which of the following substance can dry NH3 gas with moisture vapor? A. P2O5
B. H2SO4 concentration
C. CuO powder
D. NaOH solid
ẠY
Question 21: Dip two glass chopsticks into 2 containers of concentrated HCl and concentrated NH3. Then put two chopsticks close together, what phenomenon appears?
D
A. White smoke.
B. Purple smoke.
C. brownish smoke
Question 22: Has the following properties: (1) molecular lattice; evaporate;
(3) light green in darkness at normal temperature;
D. Yellow smoke. (2) hard to melt, hard to (4) burn only above
250oC. The properties of white phosphorus are: A. (2), (3)
B. (3) , (4)
C. (1), (3)
D. (1), (2)
Trang 64
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 23: In the reaction of phosphorus with: (1) Ca, (2) O2, (3) Cl2, (4) KClO3. The reactions in which phosphorus represents reduction are: A.(1), (2), (4)
B. (1), (3)
C. (2), (3), (4)
D. (1), (2), (3)
Question 24: In the laboratory, the phosphoric acid was prepared according to the following reaction
FF IC IA L
A. 3P + 5HNO3 + 2H2O 3H3PO4 + 5NO B. Ca3(PO4)2 + 3H2SO4 2H3PO4 + 3CaSO4 C. 4P + 5O2 P2O5 và P2O5 + 3H2O 2H3PO4
D. 2P + 5Cl2 2PCl5 và PCl5 + 4H2O H3PO4 + 5HCl
Question 25: Plant ash is also a type of potassium fertilizer because it contains A. KNO3
B. KCl
C. K2CO3
D.K2SO4
O
Question 26: The nutritional value of phosphate fertilizer is determined by the percentage C. PO43-
B.P2O5
D. H3PO4
Ơ
A. P
N
of mass of the what substance
Question 27: Add a piece of phosphorus to the nitric acid solution to obtain gas B and
H
solution C. Apply sufficient NaOH solution into solution C to obtain solution D. Add the
N
AgNO3 solution to solution D we obtain the precipitate E. Aeration of B gas into NaOH solution, B gas absorbed completely. Substances B, C, D, E are B. NO2, H3PO4, Na3PO4, Ag3PO4
C. NH3, H3PO4, Na3PO4, Ag3PO4
D. N2, H3PO4, Na3PO4, Ag3PO4
U
Y
A. NO, H3PO4, Na3PO4, Ag3PO4
was complete?
Q
Question 28: Which of the following experiments was the precipitation after the reaction
M
A. CuCl2 solution reacts with excess NH3 solution
KÈ
B. NaAlO2 solution reacts with excess HCl solution C. AlCl3 solution reacts with excess NaOH solution D. ZnSO4 solution reacts with excess Ba(OH)2 solution
ẠY
Question 29: Completely dissolve 4.8 grams of Mg in HNO3 solution, obtain X solution
D
and 448 ml of NO gas (at STP). Concentrated X solution obtained m grams of anhydrous salt. The value m is A. 29,6.
B. 30,6.
C. 31,6.
D. 33,0.
Question 30: Salt B has the following characteristics: - When pyrolysis salt B only creates one gas - Dissolve B into water then add HCl solution and some copper powder, we see colorless gas Trang 65
Sáng kiến kinh nghiệm năm học 2018 - 2019
then turn to brown in the air escaping. Salt B is A. CaCO3
B. Cu(NO3)2
C. Al(NO3)3
D. NaNO3
Question 30: Give the following experimental diagram:
X gas
In gases: H2, O2, CO2, HCl, Cl2, NH3, N2.
A. 3.
B. 2.
C. 4.
D. 5.
Question 31: There are the following statements
FF IC IA L
The amount of gas that has this properties is
1.Then nutrient content of nitrogen fertilizer is determined by the percentage of N in the 2. Urea nitrogen has the chemical formula (NH4)2CO3.
O
fertilizer
N
3. The nutrient content in phosphate fertilizer is determined by the percentage of phosphorus in the fertilizer
Ơ
4. Urea fertilizer and sodium nitrate fertilizer do not increase soil acidity
H
5. Single supeposphate fertilizer has the formula Ca(H2PO4)2
N
6. Double superphosphate has the formula of Ca(H 2PO4)2 .CaSO4 The number of incorrect statements is B. 3
C. 4
Y
A. 2
D. 5
U
Question 31: There are the following statements
Q
1, Formula of apatite ore is Ca3(PO4)2.3CaF2 2, Formula of phosphorite ore is Ca3(PO4)2
M
3, In industrial H3PO4 is prepared by giving phosphorite or apatite ore effects with
KÈ
concentrated H2SO4
4, In the laboratory, HNO3 is prepared by applying KNO3 solid with concentrated H2SO4 5, In industry HNO3 is prepared from NH3 follow diagram NH3 NO NO2 HNO3
ẠY
The number of correct statements is
D
A. 2
B. 3
C. 4
D. 5
Question 32: There are the following statements 1, In laboratory NH3 gas is collected by water push method 2, In laboratory NH3 gas can be prepared by heating concentrated ammonia solution 3, To dry NH3 gas, gas is passed through concentrated H2SO4 solution Trang 66
Sáng kiến kinh nghiệm năm học 2018 - 2019
4, In industry, NH3 is prepared by reaction of N2 with H2 5, Ammonium salts when pyrolysis produce NH 3 and acid 6, In order for NH3 synthesis reaction turn in the right direction, it is necessary to reduce the temperature or increase pressure or liquefy NH 3 The number of incorrect statements is B. 3
C. 4
D. 5
FF IC IA L
A. 2
Question 33: Solid E was analysed. E was an aluminium salt. The tests on the solid and some of the observations are in the following table. Complete the obser vations in the table.
Observations/ reaction
a. Appearance of solid E
white crystalline solid
b. A little of solid E was heated in a test-
colourless drops of liquid formed at the
tube.
top of the tube
Ơ
water .
N
c A little of solid E was dissolved in distilled
O
Tests on solid E
H
The solution was divided into four test-tubes
N
and the following tests were carried out
..................................
of excess aqueous sodium hydroxide
..................... .............
(ii) To second test-tube was repeated using
..................................
aqueous ammonia solution instead of
. . . . . . . . . . . . . . ………………………...
Q
U
Y
(i) To the first test-tube of solution, drops
aqueous sodium hydroxide.
M
(iii) To the third test-tube of solution, dilute
no reaction
KÈ
hydrochloric acid was added, followed by (iv) To the fourth test-tube of solution,
effervescent pungent gas given off turned
aqueous sodium hydroxide and aluminium
damp litmus paper blue
ẠY
barium chloride solution.
D
powder were added. The mixture was heated. 1. What does test (b) tell you about solid E? 2. Write the equation for the reaction in (c) (i), (ii) 3. Identify the gas given off in test (c)(iv). Solution:
Trang 67
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1. A little of solid E was heated in a test-tube colourless drops of liquid formed at the top of the tubeE is hydrated salt 2. *) In test (c) (i): Originally appeared white, glue precipitate, then the precipitate is dissolved Al(OH)3(s) + OH-(aq) AlO2-(aq) + H2O(l) *) appeared white, glue precipitate, only. Al3+(aq) + 3NH3(aq) +3H2O(l) Al(OH)3(s) + 3NH4+(aq)
FF IC IA L
Al3+(aq) + 3OH-(aq) Al(OH)3(s)
*) To the third test-tube of solution, dilute hydrochloric acid was added, followed by barium chloride solution Solid E hasn’t got SO42- anion
*) To the fourth test-tube of solution, aqueous sodium hydroxide and aluminium powder
O
were added. The mixture was heated effervescent pungent gas given off turned damp
N
litmus paper blue Solid E has got NO3- anion
Ơ
8Al(s) + 5OH-(aq) + 3NO3-(aq) + 2H2O(l) 8AlO2-(aq) + 3NH3(g) 2Al(s) + 2OH-(aq) + 2H2O(l) 2AlO2-(aq) + 3H2(g)
H
Question 33: The following instructions were used to prepare magnesium sulfate
N
crystals, MgSO4.7H2O.
Y
Step 1. Measure 50 cm3 of dilute sulfuric acid into a beaker and warm the solution.
U
Step 2. Using a spatula, add some magnesium oxide and stir the mixture. Continue adding the magnesium oxide until excess is present.
Q
Step 3. Separate the excess magnesium oxide from the solution of magnesium sulfate.
M
Step 4 Heat the solution until crystals form. Obtain the crystals and dry them.
KÈ
a Why is the sulfuric acid warmed? b How would you know when excess magnesium oxide is present in Step 2? c What method is used in Step 3?
ẠY
d Why must care be taken when drying the crystals in Step 4?
D
Question 34: The formula of lithium nitride and alumminum nitride are: A. LiN3 and Al3N
B. Li3N and AlN
C. Li2N3 and Al2N3
D. Li3N2 and Al3N2
Question 35: Choose the correct chemical formula of magnesium phosphide from the followiing formula: A. Mg3(PO4)2
B. Mg(PO3)2
C. Mg3P2
D. Mg2P2O7 Trang 68
Sáng kiến kinh nghiệm năm học 2018 - 2019
The total dissociation equation of H 3PO4 in the solution is : H3PO4
3H+ + PO43-
When adding HCl to the solution, A. The above equilibrium shifts to the forward reaction. C. The above equilibrium does not shift. D. The concentration of PO43- increase. Bài tập tự luận:
FF IC IA L
B. The above equilibrium shifts to the reverse reaction.
Exercise 1: To obtain a neutral phosphate salt, how many liters of 1.00 M NaOH solution are needed to react with 50.0ml of 0.50M H3PO4 solution?
Exercise 2: A type of phosphate ore contains 35% of Ca3(PO4)2. Calculate the percent
O
content of P2O5 in the above ore.
N
Exercise 3: To produce ammophos fertilizer, 6.000x103 mol H3PO4 is used.
Ơ
a. Calculate the volume of ammonia gas ( at STP) needed, given that this type of ammophos has the molar ratio of nNH4H2PO4 : n(NH4)2HPO4= 1: 1
H
b. Calculate the mass of obtained ammophos.
N
Exercise 4: 6.2 g of phosphorus is burned completely in excess of oxygen. The formed product reacts equivalently with 32% NaOH solution to form Na2HPO4.
Y
a. Write the chemical equations of the occurring reactions.
U
b. Calculate the mass of the NaOH solution used.
Q
c. Calculate the percent concentration of salts in the obtained solution after the reaction. Exercise 5: How many tons of ammonia are needed to produce 5.000 tons of 60wt% nitric
M
acid. Given that the loss of ammonia in nitrogen manufacturing is 3.8%
KÈ
Exercise 6: When dissolving 30.0g of a mixture of copper and copper (II) oxide in 1.50 liters of 1.00 M ( dilute) nitric acid, 6.72liters of nitrogen monoxide ( at STP) are observed
ẠY
to escape from the reaction mixture. Determine the percent content of copper (II) in the mixture, molarity of copper (II) nitrate and nitric acid in the solution after reaction, given
D
that the solution volume is unchanged. Exercise 7: Add an excess of a NaOH solution to 150.0 ml of 1.00M (NH4)2SO4 solution, and heat gently. a. Write the chemical equations in the molecular and net ionic forms b. Calculate the obtained gas volume ( at STP)
Trang 69
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Exercise 8: How many liters of nitrogen and hydrogen gases are needed to prepare 62.2 liters of ammonia? Given that the volumes of gases are measured in the same conditions of temperature and pressure,, an the efficiency of the reaction is 25%. Exercise 9: From hydrogen, chlorine, nitrogen and necessary chemicals, write chemical equations (indicate clearly the reaction conditions) to prepare ammonium chloride fertilizer.
FF IC IA L
Exercise 10: a) Write the following chemical equations: NH3+Cl2( excess ) → N2+…
(1)
NH3 (excess ) + Cl2→ NH4Cl+… (2) NH3+ CH3COOH →…
Zn(NO3)2
H3PO4 +… (4) heat
…
(5)
O
(NH4)3PO4
(3)
heat
N
b) Write the molecular and net ionic chemical equations of the reactions between the following substances in the solution:
(1)
Ơ
K3PO4 and Ba (NO3)2
H
Na3PO4 and CaCl2
(2)
N
Ca(H2PO4)2 and Ca(OH)2 with the molar ratio of 1: 1 (3) (NH4)3PO4 + Ba(OH)2
(4)
Y
3.2.3. Chuyên đề: CARBON -SILICIC (Nhóm Cacbon- silic)
Q
KÈ
Ambient
Khí quyển
M
Atmospheric
U
Bước 1: Các từ mới trong chuyên đề
temperatures:
Nhiệt độ
Coke/coal/graphite/amorphorus Than cốc/than/than chì/ carbon/ activated carbon/
cacbon vô định hình/
charcoal
than hoạt tính/Than gỗ
Poisonous gases
Khí độc
Black powders
Thuốc nổ đen
thường
Photosynthesis n Quang hợp
D
ẠY
75%KNO3,10%S,15%C
Allotropes
2KNO3 + S +3C ---> K2S + N2 + 3CO2 Dạng thù
Water glass ( liquid glass)
hình
Thủy tinh lỏng ( Dung dịch đậm đặc của Na2SiO3 và K2SiO3)
Crystalline
Cấu trúc
Water gas/ producer gas
Khí than ướt/ khí than Trang 70
Sáng kiến kinh nghiệm năm học 2018 - 2019
structures
tinh thể
( syngas)
khô
Hardest natural
Chất tự
alloy
Hợp kim
substance/
nhiên cứng
hardness
nhất/ độ Keo dán thủy tinh và sứ
Transparent
Trong suốt
Glues for glass and ceramic
Blackish grey
Tinh thể
Porous material
crysalline
màu xám
Vật liệu xốp
đen structure
lớp
Good conductor
Dẫn điện
/low electrical
tốt/ dẫn
Quartz grains Gaseous fuel
poorly
kém
Ores/minerals
Quặng/
Chất bôi trơn
khoáng vật
N
lubricant
Thuốc pháo
Drill bits
Chế tạo mũi khoan
Glass cutters
Dao cắt thủy tinh
Đầu bút chì
Sharpening pastes
Bột mài
xi đánh
electrodes
Điện cực
U
Protective masks Mặt nạ
Y
fireworks
H
dẫn nhiệt
Nhiên liệu khí
Ơ
conductivity/con điện kém/ ducts heat
Thạch anh
O
Cấu trúc
N
Layered
FF IC IA L
cứng
Pencils lead
Q
phong độc
KÈ
M
Shoe polishes
giày Chất độn
Crucibles for holding heat-
Nồi nấu chảy các hợp
filler in rubber
cao su
resistant metals
kim chịu nhiệt
ẠY
Reinforcing
Bước 2: Một số bài tập điển hình trong chuyên đề
D
Exercise 1. Melting mixture of 3 grams of Mg and 3 grams of SiO 2 in order to react
completely. For the product of Reaction into excess NaOH solution shows V liters of gaseous fly out. Caculate the value of V. Solution: The mole of Mg is:
3 0.125 mol 24 Trang 71
Sáng kiến kinh nghiệm năm học 2018 - 2019
The mole of Mg is:
3 0.05 mol 60
2Mg(s) + SiO2(s) 2MgO + Si (1)
Initial
0.125
Reacted
0.1
After
0.025
0.05
2Mg(s) +
0.05 mol
0.05 0
0.05
Si (s) Mg2Si
Initial
0.025
Reacted
0.0250.0125 0.0125
After
0
FF IC IA L
The reaction:
(2)
0.05 0.0375
After (2) reaction, the solid contain: Mg2Si and Si residua Si(s)
O
Disove this solid into NaOH solution:
+ 2NaOH(aq) + H 2O(l) Na2SiO3(aq) + 2H2↑(g)
N
0.0375
0.075 mol
Ơ
The volume of gas obtained at STP : 0.075 x 22.4 = 1. 68 L solution, the A solution is obtained
H
Exercise 2. Absorb completely 8.96 liters of CO2 gas at STP into 500ml of 1M NaOH
N
a) Please tell me what substances A contains
Y
b) Calculate the molar of substances in A solution
U
c) If solution A is applied into the solution which contain excess BaCl 2, m gram of Solution:
Q
precipitate is obtained. Calculate the value of m
KÈ
M
a) The mole of CO2 is: The mole of NaOH is:
6.72 0.3 mol 22.44
500 x1 0.5 mol 1000
ẠY
Ratio of moles between NaOH and CO2 is
nNaOH 0.5 1.25 1; 2 nCO2 0.4
D
The reaction between NaOH and CO2 occurs in two equations NaOH(aq) + CO2(g) NaHCO3(aq) 2NaOH(aq) + CO2(g) Na2CO3(aq) + H2O(l) A solution contains: NaHCO3 and Na2CO3
b) Let the number mol of NaHCO3 be a mol Let the number mol of Na2CO3 be b mol Trang 72
Sáng kiến kinh nghiệm năm học 2018 - 2019
NaOH(aq) + CO2(g) NaHCO3(aq) a
←
a
← a
2NaOH(aq) + CO2(g) Na2CO3(aq) + H2O(l) 2b
←
b
← b
nCO2 = a+b = 0.4 mol
FF IC IA L
nNaOH = a + 2b = 0.5 mol a = 0.3 mol ; b = 0.1 mol nNaHCO3 = 0.3 mol; nNa2CO3 = 0.1 mol
0.3 C NaHCO3 0.5 0.6M the molar of substances in A solution: 0.1 C 0.2M Na2CO3 0.5
O
c) If solution A is applied into the solution which contain excess BaCl 2; we have reaction:
0.1 mol
Ơ
0.1
N
Na2CO3(aq) + BaCl2(aq) BaCO3(s) + 2NaCl(aq)
the mass of the precipitate is obtained: mBaCO3 = 0.1 x 197 = 19.7 grams
H
Exercise 3. The space shuttle environmental control system handles excess CO 2 (which the
N
astronauts breathe out; it is 4.0% by mass of exhaled air) by reacting it with lithium hydroxide, LiOH, pellets to form lithium carbonate, Li2CO3 , and water. If there are 7
Y
astronauts on board the shuttle, and each exhales 20. L of air per minute, how long could
U
clean air be generated if there were 25,000 g of LiOH pellets available for each shuttle Solution:
Q
mission? Assume the density of air is 0.0010 g/mL.
M
Convert: 0.0010 g/mL = 0.001kg/L
KÈ
Per minute, 7 astronauts on board th shuttle breathe out: 20 x 7 = 140 L The mass of air 7 astronauts on board shuttle breathe out, In one minute:
ẠY
140 x 0.001=0.14 Kg
The mass of CO2 the astronauts breathe out in one minute: 0.14 x103 x 4% = 5.6g
D
The mole of CO2 the astronauts breathe out in one day: CO2(g) 0.13
5.6 0.13 mol 44
+ 2LiOH(aq) Li2CO3(aq) + H2O(l) 0.26
mol
The mass of LiOH is obtained in one minute is: 0.26 x 24 = 6.24 g The period of time the air is cleaned is:
25, 000 4, 006.41 ( minutes) 66.77 hours 6.24 Trang 73
Sáng kiến kinh nghiệm năm học 2018 - 2019
Bước 3: Một số bài tập tự luyện Question 1. The CO2 produced in the laboratory is often with HCl gas. To remove HCl from the mixture, use B. Na2CO3 saturated solution
C. concentrated NaOH solution.
D. concentrated solution of H 2SO4
Question 2. To prevent CO poisoning people use absorbent
FF IC IA L
A. NaHCO3 saturated solution
A. Copper (II) oxide and manganese oxide
B. copper (II) oxide and magnesium oxide
C. Copper (II) oxide and activated carbon
D. activated carbon
Question 3. Which of the following statements about carbonate salts is true: All carbonate salts are regular A. soluble in water
B. pyrolysis produces metal oxide and carbon dioxide
C. pyrolyzed except of carbonate salts of alkaline metals
O
D-insoluble in water
Question 4. The phenomenon occurs when mixing solution of Na2CO3 with FeCl3 solution
N
is
B. There are bubbles escaping from the solution
Ơ
A. Appear red-brown precipitate
D. Appear red- brown precipitate and colorless gas
H
C. Appear light green precipitate
N
escaping from the solution
Question 5. A gas mixture of CO and N2 that has a mass ratio with H2 is 14. If we add 20%
Y
N2 by the volume into the mixture, how the mass ratio with H 2 of the new mixture will? B. Reduce
U
A. No change
C. Increase
D. Not determined
Q
Question 6. The formation of stalactites in limestone caves is due to the following chemical reaction?
M
A. CaCO3 CO 2 H 2 O Ca(HCO3 )2 0
t C. CaCO3 CaO CO2
B. Ca(OH)2 Na 2 CO3 CaCO3 2NaOH
KÈ
D. Ca(HCO3 )2 CaCO3 CO 2 H 2 O
Question 7. Completely dissolve m grams of Na2CO3.10H2O in water to obtain 100 ml of
ẠY
0.1M solution. The value of m is: A. 6.28g
B. 2.68g
C. 28.6g
D. 2.86g
D
Question 8. The oxidation and reduction properties of carbon are expressed in the which following reaction 0
t A. CaO 3C CaC 2 CO 0
t C. C CO2 2CO
0
t B. C 2H 2 CH 4 0
t D. 4Al 3C Al 4 C 3
Question 9. The main component of wet coal gas is Trang 74
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. CO,CO 2 , H 2 , N 2
B. CH 4 ,CO,CO2 , N 2
C. CO,CO2 , H 2 , NO2
D. CO, CO 2 , NH 3 , N 2
Question 10. Which of the following chemical reactions are wrong? A. SiO 2 4HF SiF4 2H 2 O
B. SiO 2 4HCl SiCl 4 2H 2 O
0
0
t D. SiO2 2Mg Si 2MgO
FF IC IA L
t C. SiO2 2C Si 2CO
Question 11. Which of the following pairs of substances do not exist in the same solution: A. NaHCO3vµ BaCl 2
B. Na 2 CO3vµ BaCl 2
C. NaHCO3vµ NaCl
D. NaHCO3vµ CaCl 2
Question 12. Carbon reacts with all substances in the which following sequence? B. Al, HNO3®Æc,KClO3
C. Ba(OH)2 , Na 2 CO3 , CaCO3
D. NH 4 Cl, KOH, AgNO 3
O
A. Na 2 O, NaOH, HCl
N
Question 13. Silic reacts with all substances in the which following sequence? B. F2 , Mg, NaOH
Ơ
A. CuSO 4 ,SiO2 , H 2 SO 4 lo·ng C. HCl, Fe(NO3 )3 , CH 3COOH
D. Na 2SiO3 , Na 3PO 4 , NaCl
H
Question 14. To distinguish between CO2 and SO2 can be used 15.
Apply
C. NaOH solution
the
following
chemical
Y
Question
B. Br2 solution
N
A.Ca (OH)2 solution
Which
of
the
sequence: following
Q
statements is true:
transformation
U
CaCO3 CaO Ca(OH)2 Ca(HCO3 )2 CaCO3 CO 2
D. KNO3 solution
A. There are two oxidation -reduction reactions
M
B. There are three oxidation-reduction reactions
KÈ
C. There is an oxidation-reduction reaction D. There is not oxidation-reduction reaction
Question 16. For 3.12 grams mixture of sodium carbonate and potassium carbonate react
ẠY
with residual HCl solution yields V liters of CO2 and 3.45 grams of chloride salt. The value of V at STP is:
D
A. 6.72 liters
B. 3.36 liters
C. 1.12 liters
D. 0.672 liters
Question 17. Completely absorbed 2,688 liters of CO 2 gas in 2.5 liters of solution of Ba(OH)2 a M, yielded 15.76 g of precipitate. The value of a is A. 0.032
B. 0.048
C. 0.06
D. 0.04
Trang 75
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 18.To completely eliminate FeO, CuO requires 4.48 liters of H 2. If completely eliminate that mixture by CO , CO2 is obtained lead into the residual lime water there are m grams of precipitation. The value of m is: A. 1.0g
B. 2.0g
C. 20g
D. 10g
0.02M to completely precipitate the aluminum ion A. 15ml
B. 10ml
FF IC IA L
Question 19. How many milliliters of 0.12 M Na2CO3 at least add in 25 ml of Al2(SO4)3 C. 30ml
D. 12.5ml
Question 20. For 5 jar contain 5 white powder: NaCl,Na2CO3,Na2SO4,BaCO3,BaSO4. How many substances can identify if only using water and CO 2 A. 2
B. 3
C. 4
D. 5
Question 21. People use sand to make metal molds. To thoroughly clean the sand particles
O
on the metal surface after casting, what solution should we use? B. Dilute solution of H2SO4
C. HF solution.
D. HCl solution
Ơ
Question 22. Liquid glass is:
N
A. NaOH dilution solution
H
A. molten silicon dioxide
N
B. The solution contains Na2SiO3 and K2SiO3 is concentrated C. Solution of saturated silicic acid
Y
D. D. fused quartz
B. HCl solution
C. H2SO4 solution
D. NaOH solution
Q
A. HF solution
U
Question 23. Which of the following solutions to use to engrave on glass? Question 24. Silicon dioxide does not react with the following solution C. Na 2CO3 melted
B. HCl solution
D. HF solution
KÈ
M
A. NaOH solution is concentrated
Question 25. Melting mixture of 3 grams of Mg and 3 grams of SiO2 in order to react completely. For the product of Reaction into excess NaOH solution shows V liters of
ẠY
gaseous fly out. The value of V is?
D
A. 2.24
B. 1.12
C. 1.68
D. 5.6
Question 26. The ion equation 2H+ + SiO32- → H2SiO3↓ corresponds to which molecular
equation A. Carbonic acid and calcium silicate B. Carbonic acid and sodium silicate C. Hydrochloric acid and calcium silicate D. Hydrochloric acid and sodium silicate Trang 76
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 27. When acid oxides react with water, acid will not form. acid oxide which is: A. Carbon dioxide
B. Sulfur dioxide
C. silicon dioxide
D. dinitogen pentaoxide
A. homogeneous mixture
B. heterogeneous mixture
C. compound
D. pure substance
FF IC IA L
Question 28. A combination of sand, salt, and water is an example of a __________.
Question 29. Which one of the following is a pure substance? A. concrete
B. wood
C. salt water
Question 30. What can you say about the reaction below? Fe2O3(s) + 3CO(g) → 2Fe(s) + 3CO2(g) ΔH = -24.8kJ A. it is endothermic and heat is absorbed
O
B. it is exothermic and heat is absorbed
D. elemental copper
C. it is endothermic and heat is released
N
D. it is exothermic and heat is released
Ơ
Question 31. Of the following, only __________ is a chemical reaction. B. dissolving sugar in water
C. tarnishing of silver
D. crushing of stone
N
H
A. melting of lead
Question 32. In the following reaction, what would Le Châtelier’s principle predict to
Y
increase the concentration of CO2?
B. increase O2
Q
A. add a catalyst
U
C(s) + O2(g) CO2(g) ΔH = -393.5 kJ/mol C. increase the pressure
D. increase the temperature
M
Question 33. For the reaction: H2(g) + CO2(g) H2O(g) + CO(g), what would be the effect
KÈ
on the equilibrium system if: (a) the pressure increases ? → no change (b) the volume decreases? → no change
ẠY
Question 34: Which of the following statements is incorrect?
D
A. Liquid glass is a concentrated solution of Na2SiO3 and K2SiO3
B. Gia-ven water is a solution of mixture of sodium chloride and sodium hypochlorite. C. White phosphorus has a molecular lattice structure. D. Complex fertilizer is a product that mixes different types of fertilizer. Question 35: Conducting CO gas through a (hot) mixture Al 2 O3 ,CuO,MgO, Fe 2 O3 . After the reaction occurs completely yields solids are: Trang 77
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. Al 2 O3 ,Cu,MgO, Fe
B. Al,Fe,Cu,Mg
C. Al 2 O3 ,Cu,Mg,Fe
D. Al 2 O3 , Fe2 O3 ,Cu,MgO
Question 36: In the following statements, how many correct statements? (a) For KMnO4 solution reacts with HF solution (concentrate) obtained F 2 gas. (b) Using prepared sulfate to modulation : HF, HCl, HBr, HI.
FF IC IA L
(c) Electrolysis of water are modulation method oxygen gas in industry
(d) Amophot (mixtures of NH4H2PO4 and (NH4)2HPO4) are mixed fertilizers.
(e) In the laboratory, CO is prepared by adding concentrated H 2SO4 to formic acid and heating. (d) Silicic acid is weaker than carbonic acid A. 3
B. 4
C. 2
D. 5
O
Question 37: Melting 6 g of magnesium with 4.5 g of silicon dioxide, Add residual NaOH
N
to the mixture after reaction. What is the volume of hydrogen obtained? Assume the A. 1,68 (liters)
B. 1,12 (liters)
Ơ
reaction is 100% efficient.
C. 0,56 (liters)
D. 0,28 (liters).
H
Question 38: Give the following statements:
N
1. Slicagen is silicic acid takes part water
2. Silicic acid is weaker than carbonic acid
Y
3. Silicon and silicon dioxide react with concentrated, heat alkaline solution
U
4. aeration CO2 in solution Na2SiO3 , appear white, glue precipitated
Q
5. Silicon has both oxidation and reduction properties 6. All carbonate salts are easily decomposed by heating
M
7. Dry ice is solid CO2
KÈ
8. CO2 is the main cause of greenhouse effect
9. In the laboratory, CO is prepared by heating HCOOH with concentrated H 2SO4
ẠY
10. In nature, carbon exists both elements form and compounds 11. In nature, silicon exists both elements form and compounds
D
12. Oxygen is the most abundant element in the earth's crust, then to silicon
How many statements are correct? A. 8
B. 9
C. 10
D. 11
Question 40: the ‘lead’ in a pencil is made of a mixture of graphite and clay. When the percentage of graphite is increased, the pencil slides across the paper more easily. Which statement explains this observation? Trang 78
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. Graphite has a high melting point
C. Graphite is a form of carbon
B. Graphite is a lubricant
D. Graphite is a non-metal
3.2.4. Chuyên đề: FUNDAMENTALS OF ORGANIC CHEMISTRY (Đại cương hóa học hữu cơ) Bước 1: Các từ mới trong chuyên đề Saturated
series
đồng đẳng
hydrocarbon
Isomers
Đồng phân
Unsaturated hydrocarbon
Cis – trans isomerism
Đồng phân cis trans
Uromatic hydrocarbon
Đồng phân lập thể
Hydrocarbon
Hidrocacbon không no
Hidrocacbon thơm
O
Stereo isomers
Hidrocacbon no
FF IC IA L
Homologo/homologous Đồng đẳng/dãy
hidrocacbon
Đồng phân cấu tạo
Halogen derivatives
Empirical formula
Công thức đơn giản
Functional group
nhóm chức
Molecules formula
Công thức phân tử
Qualitative analysis
Phân tích Định tính
Structural formula
Công thức cấu tạo
Quantitative
Phân tích Định
analysis
lượng
N
H
Ơ
Constitutional isomers
ẠY
Branched
Unbranched Inorganic compound
organization names
U
KÈ
Acyclic
- Tên gốc - chức
Common name
Tên thường
Vòng
Nomenclature
danh pháp
Hở
Isomers of
Đồng phân về nhóm
functional groups
chức
Isomers of positions
Đồng phân về vị trí
M
Cyclic
Original
Dẫn xuất halogen
Mạch Cacbon
Q
Carbon chain
Công thức hóa học
Y
Chemical formular
D
N
derivatives
Dẫn xuất
Nhánh
of multiple bonds or liên kết bội hoặc vị Không nhánh
functional groups
trí nhóm chức
Nonpolar liquid n
Chất lỏng không phân cực
Hợp chất vô cơ
Organic compound
Hợp chất hữu cơ
Bước 2: Một số bài tập điển hình trong chuyên đề Exercise 1. Complete combustion of 2.2 g of organic compound A, obtained 4.4 g CO 2 and 1.8 g H2O. Trang 79
Sáng kiến kinh nghiệm năm học 2018 - 2019
a. Determine the empirical formula of A. b. Identification molecular formula of A know that when vaporize 1.1 g of A, the steam volume equal to the volume gain of 0.4 g O2 gas at the same temperature and pressure. Solution
contains C, H maybe contain O
x, y Z ; z Z ) *
Let the molecules formula of A be CxHyOz 0
t CxHyOz CO2 H 2O
nH 2O 0.1 mol nH 0.2 mol nCO2 0.1 mol nC 0.1 mol
O
mO 2.2 0.2 x1 0.1x12 0.8 g nO 0.05 mol
FF IC IA L
a) Complete combustion organic compound A, obtained CO 2 and H2O, so this compound
We have, x:y:z = nC : nH : nO = 0.1 : 0.2 : 0.05 = 2 : 4 : 1
Ơ
b) → molecules formula of A is (C2H4O)n
N
Therefor,the empirical formula of A is C2H4O
1.1 0.4 M A 88 M A 32
Y
VA VO2 n A nO2
N
same temperature and pressure
H
When vaporize 1.1 g of A, the steam volume equal to the volume gain of 0.4 g O2 gas at the
U
44n = 88 n = 2→ molecules formula of A is (C2H4O)2 C4H8O2
Q
Exercise2. An organic compound A has mass ratio with CO2 is 1. Complete combustion A
Solution
M
only collects CO2 and H2O. Find the molecular formula of A
KÈ
Complete combustion organic compound A, obtained CO2 and H2O, so this compound contains C, H maybe contain O
ẠY
Let the molecules formula of A be CxHyOz
x, y Z ; z Z ; y is even number and y 2x+2 *
D
compound A has mass ratio with CO2 is 1 MA = 1x 44= 44 g/mol 12x+y+16z = 44 16z ≤ 44 z ≤ 2.75 z = 0; 1; 2 +) If z = 0 12x + y = 44 12x ≤ 44 x ≤ 3.67 x = 1; 2; 3 x
1
2
3
y
32
20
8
Not accept
Not accept
accept Trang 80
Sáng kiến kinh nghiệm năm học 2018 - 2019
molecules formula of A is C3H8 +) If z = 1 12x + y = 28 12x ≤ 28 x ≤ 2.33 x = 1; 2 x
1
2
y
16
4
Not accept
accept
FF IC IA L
molecules formula of A is C2H4O +) If z = 2 12x + y = 12 x= 1; y =0 (unreasonable) Conclude, the molecules formula of A is C3H8 or C2H4O
Exercise 3. The complete combustion of ethane is given by the following unbalanced equation: C2H6g + O2g → CO2g + H2Og
O
(a) Balance this equation.
N
(b) If one mole of ethane is combusted, how many grams of water vapour are produced? (c) Assume that air contains 20% oxygen gas. What volume of air at STP is needed for the
Ơ
complete combustion of one mole of ethane?
H
Solution
N
(a) Balance this equation
C2H6g + 3.5O2g → 2CO2g + 3H2Og
Y
(b) According to the reaction equation
U
C2H6g + 3.5O2g → 2CO2g + 3H2Og
Q
1 mol → 3.5 mol
→ 3 mol
M
→ The mass of water are produced when one mole of ethane is combusted are: 3 x 18=54 grams
KÈ
(c)According to the reaction equation:
C2H6g + 3.5O2g → 2CO2g + 3H2Og 1 mol → 3.5 mol
ẠY
→ The volume of oxygen are needed when one mole of ethane is combusted is: 3.5 x 22.4 = 78.4 liters
D
Because, air contains 20% oxygen gas so the volume of air are needed is 78.4 : 20% = 392 liters
Bước 3: Một số bài tập tự luận Exercise 1. complete oxidation of 0,6 grams of organic compound A yielded 0,672 liters of CO2 at (STP) and 0,72 grams H2O. Caculate the percent by mass of elements in the molecule of A Trang 81
Sáng kiến kinh nghiệm năm học 2018 - 2019
Exercise 2. 𝛃-carotenne ( an organic compound present in carrot) is orange. Under the action of enzyme in the small intestine, 𝛃-carotenne is converted to vitamin A, hence, it is known as provitamin A. 0,67 grams of 𝛃-carotenne were complete oxidized. The resulting products were led into bottle (1) containing concentrated H 2SO4, sudsequently into bottle (2) containing Ca(OH)2 solution( excess). After the experiment, the mass of bottle (1)
FF IC IA L
increased 0,63 grams; in bottle (2), 5,00 grams of a precipitate were obtained. Caculate the mass of the element in 𝛃-carotenne molecule
Exercise 3. Caculate the molecular weight of the following compounds a) compound has a density of 2,07 compared to the atmosphere
b) The vapor volume of 3,3 grams of compound X is equal to the volume of 1,76 grams of oxygen ( measured at the same temperature and pressua)
O
Exercise 4. Limonene is a flavor isolated from lemon essential oil. The elemental analysis show that it is compound of two elements C and H, in which Cis contributed to 88,235%
Ơ
Caculate the molecular formula of Limonene
N
by mass. The vapor density of Limonene compared to atmosphere is approximately 4,69.
H
Exercise 5. complete oxidation of 0,3 grams of organic compound A( that contains only C,
N
H and O) produces 0,44 grams of CO2 and 0,18 grams of H2O. The vapor volume of 0,3 grams of A is equal to the volume of 0,16 grams of O2 (at the same temperature and
Y
pressua). Caculate the molecular formula of A
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Exercise 6. From the essential oil of anise, anethole, a flavor used in the production of gum,
Q
is isolated ( được tách ra). the molecular weight of anethole is 148,0 g/mol. The elemental analysis show that anethole contains %C = 81,08%; %H= 8,10%, and the rest is oxygen.
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Caculate the empirical formula and molecular formula of anethole.
KÈ
Exercise 7. The percent by mass of C; H; O in compound X is 54,54%, 9,1% and 36,36%,respectively. the molecular weight of X is 88g/mol. Caculate the molecular formula of X Exercise 8. The empirical formula of butane, the fuel used in disposable lighters, is C2H5.
ẠY
In an experiment, the molar mass of butane was determined to be 58 g/mol. What is the
D
molecular formula of butane Exercise 9. A compound’s molar mass is 240 g/mol. Its percentage composition is 75.0% carbon, 5.0% hydrogen, and 20.0% oxygen. What is the compound’s molecular formula? Exercise 10. The empirical formula of codeine is C18H21NO3. If the molar mass of codeine is 299 g/mol, what is its molecular formula?
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Exercise 11. Complete combustion of 4.1 g of organic matter A, obtained 2.65 g Na2CO3,, 1.35 g of water and 1.68 liters of CO2 (STP). Determine the empirical formula of A. Exercise 12. For complete combustion of 4.45 g of compound A has all necessary capacity 4.2 liters O2. Combustion products include 3.15 g H2O and 3.92 liters of gas mixture consisting of CO2 and N2 (STP).
FF IC IA L
Determination of the empirical formula A.
Exercise13. Complete combustion 3.36 liters of methane and ethane obtainded 4.48 liters CO2 (STP). Calculate percent of volume of methane and ethane in the initial mixture?
Exercise14. complete combustible amounts of organic compounds X obtained CO2 and H2O. For the product absorbed into the residual Ca(OH)2 solution, after the reaction was
complete, formed 10 g precipitate and the mass of solution were reduced from the original
O
of 3.8 g. The specific gravity of X at STP is 3.214 g / l. Determine the Molecules formula of X
N
Exercise 15. Organic compounds X has empirical formula C2H5O. Determine the
Ơ
Molecules formula of X. Writing the Structural formula of X, knowing that X has OH
H
functional group in the Molecules
N
Exercise16. Organic compounds X has empirical formula C2H5Cl. Determine the Molecules formula of X. Writing the Structural formula of X
Y
Question 1. Hydrocarbons that contain only single covalent bonds between carbon atoms
U
are called
B. alkenes.
C. alkynes.
D. unsaturated.
Q
A. alkanes. prefix is
B. hex-.
C. hept-.
D. oct-.
KÈ
A. pent-.
M
Question 2. When the longest straight-chain in a hydrocarbon contains seven carbons, its
Question 3. Answer False for the following statements is: A. Organic molecules occur only in nature and cannot be artificially synthesized
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B. Medicines we consume are not derived from natural sources
D
C. Benzene is an example of an aromatic compound D. Propane has one double bond
Question 4. the empirical formula of compound Z is CH3O. its density compared to hydrogen is 31,0. Which of the following molecular formulas corresponds to compound Z? A. CH3O
B. C2H6O2
C. C2H6O
D. C3H9O3
Question 5. A saturated organic compound A. contains all single bonds.
B. contains at least one double or triple bond. Trang 83
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C. contains only carbon and hydrogen atoms.
D. is quite soluble in water.
Question 6. Burning completely 1.68g a hydrocarbon X (M = 84) obtained 5.28g CO 2. Number of carbon atoms in the molecule X are: A. 6
B. 5
C. 4
D. 7
1.8g H2O. The empirical formula of M is A. C3H8
B. C4H8
C. C5H8
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Question 7: Analysis of 1.7 grams of organic compound M, then collected 5.5g CO 2 and D. C5H10
Question 8: Completely burn 7.6 g of a substance X need to use 8.96 liters O2 in STP. Obtained mCO2 - mH2O = 6 g. The molecular formula of X A. C3H8O
B. C3H8O3
C. C3H8
D. C3H8O2
Question 9: Combustion of organic compound Y yields CO2 and H2O with the same
O
number of mole. The molar of oxygen required is four times the number of mole of Y. The molecular formula of Y is: B. C4H8O.
C. C3H6O.
N
A. C2H6O.
D. C3H6O2.
Ơ
Question 10: Combustion 0.1mol organic X requires 7.84 liters of O2 to obtain 5.6 liters of
H
CO2, 4.5g of H2O and 5.3g of Na2CO3. The molecular formula of X is: B. C3H2O4Na2
C. C3H5O2Na
D. C3H7ONa
N
A. C3H5ONa
Question 11: Combustion 0.1 mol of X requires 6.16 liters of O2, yields 13.44 liters
Y
mixture( at STP) of ( CO2, N2 and water vapor). After condensing out of steam, the
U
remaining 5.6 liters of gas (at STP ) has a ratio of mass compared with hydrogen is 20.4
Q
The molecular formula of X is: A. C2H7O2N.
B. C3H7O2N.
C. C3H9O2N.
D. C4H9N.
M
Question 12 To identify the presence of H in an organic compound, We must use the
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following reagent after the inorganic that organic compound. A. concentrated H2SO4
B. CuSO4 anhydrous.
C. NaOH anhydrous
D. CuO
ẠY
Question 13. The molecular formula X is C40H76. Completely hydrogen X obtained saturated
D
compound Y with formula molecules is C40H80. How many pi bonds are there in X? A. 1
B. 3
C. 4
D. 2
Question 14. Which of the following is not the general characteristics of organic compounds? A. Not durable at high temperatures B. Chemical reaction is slow and in many directions C. Mainly contain ionic bonds
D. Volatile and flammable
Question 15. Which of the following statements is not true? Trang 84
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A. In organic molecules, the atoms are bond together with correct valence and in a certain order B. When changing the linking order, the new substance will be formed C. The isomers have chemical properties similar D. The substances in the homologous series has chemical properties similar
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Question 16. Composition of elements in organic compounds are A. necessarily carbon, usually H, often O, N then halogen, S, P ... B. consists of C, H and other elements. C. includes all elements in the periodic table. D. usually C, H often O, N, then to halogen, S, P. 1. The elemental composition mainly C and H. 2. may contain other elements such as Cl, N, P, O.
N
3. chemical bonding mostly covalent bond.
O
Question 17. General characteristics of organic molecules are
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4. Major chemical bonding is ionic bonding.
H
5. volatile, difficult to burn.
N
6. Chemical reactions occur slowly, in many different directions The right idea is: B. 1, 2, 3,6.
Y
A. 2,4, 5, 6.
C. 1, 3, 5,6.
D. 2, 3,4, 6.
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Question 18: Which statement is wrong?
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A chemical bonding in organic compounds is mostly covalent bond. B. Substances which similar structure and properties but different one or more of -CH 2-
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groups in molecular are homologous of each other
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C. Substances of the same molecular weight are the isomers of each other. D. Triple bonds consist of two pi bonds and one xichma bond Question 19: Oxidation of an organic compound X completely with CuO excess , release
ẠY
CO2, H2O and N2. Choose the most accurate conclusion in the following conclusions:
D
A. X contains C, H, N and may contain oxygen. B. X is a compound of three elements C, H, N. C. Substance X contains C, H, possibly N. D. X is a compound of four elements C, H, N, O. Question 20: Metol C10H20O and menton C10H18O are all found in menthol. Know that the
metol molecules do not have double bonds, and the menton molecule has a double bond. So which of the following is true? Trang 85
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A. Metol and menton are all cyclic structures. B. Metol has a ring structure, menton has acyclic structure. C. Metol and menton have acyclic structure. D. Metol has acyclic, menton has cyclic structure. Question 21: Vitamin A has a molecular formula of C20H30O, which contains a hexagonal A. 7.
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cycle and does not contain a triple bond. The double bond in vitamin A molecule is
C. 5.
B. 6.
D. 4.
Question 22: Licopen has a molecular formula of C40H56 that is red compound in tomatoes, containing only double bonds and single bonds in molecules. Hydration fully licopen, C40H82 hydrocarbons was obtained. So licopen contains
B. 1 cicle; 5 double bonds.
C. 4 cicle; 5 double bonds.
D Cacbon acyclic ; 13 double bonds
CH2=CH-C≡CH (1 )
CH3CH=C(CH3)2 (3)
CH2=CHCl (2) ;
What substances have Stereo isomers?
B. 4, 5, 6.
CH3CH=CHBr (5)
C. 2, 4, 6
D. 1, 3, 4
N
A. 2, 4, 5
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CH3CH=CHCH3 (5)
H
CH3CH=CH-CH=CH2(4)
N
Question 23: For the following substances:
O
A. 1 cicle; 12 double bonds.
Question 24: Range of substances that contain substances are isomers of each other?
A. C2H5OH, CH3OCH3.
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B. CH3OCH3, CH3CHO
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C. CH3CH2CH2OH, CH3CH2OH
D. C4H10, C6H6
Q
Question 25: Give the following alkane mixtures: pentane (boiling at 36oC), heptane (boiling at 98oC), octane (boiling at 126oC), nonane (boiling at 151oC). How can we
M
separate these substances? B. Distillation
C. Sublimation.
D. Extract.
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A. Crystallization.
Question 25: The phenomena of chemical compositions and properties are similar, they are more than one or more methylene groups (-CH2-) are called phenomena
ẠY
A. isomerism.
B. isotopes. C. homogeneous
D. Constitutional isomers
D
Question 27: Incorrect statement is: A. The nature of substances depends on molecular composition and chemical structure. B. Substances of the same molecular weight are isomers. C. Substances that are isomers of each other have the same molecular formula. D. Geometric isomers are substances that have the same molecular formula, the same structural formula and differently the distribution of atomic groups in space Question 28: Which of the following range are all derivatives of hydrocarbons? Trang 86
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A. CH2Cl2, CH2Br-CH2Br, NaCl, CH3Br, CH3CH2Br. B. CH2Cl2, CH2Br-CH2Br, CH3Br, CH2=CHCOOH, CH3CH2OH. C. CH2Br-CH2Br, CH2=CHBr, CH3Br, CH3CH3. D. HgCl2, CH2Br-CH2Br, CH2=CHBr, CH3CH2Br. For the following structural formula: CH3CH(OH)CH=C(Cl)CHO. The
oxidation numbers of carbon atoms from right to left are:
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Question 29:
A. +1 ; +1 ; -1 ; 0 ; -3.
B. +1 ; -1 ; -1 ; 0 ; -3.
C. +1 ; +1 ; 0 ; -1 ; +3.
D. +1 ; -1 ; 0 ; -1 ; +3.
Question 30: An organic compound A having M = 74. Burning A with oxygen yields CO 2 and H2O. How many molecular formulas are suitable for A? A. 4.
B. 2.
C. 3.
O
( C6H2; C4H10O; C3H6O2; C2H2O3)
D. 1.
Question 31: An organic compound A has a mass ratio to the air equal to 2. Combustion of B. A. 1.
D. 4.
H
(C4H10; C3H6O; C2H2O)
C. 3.
Ơ
A. 2.
N
A by O2 results in CO2 and H2O. How many molecular formulas are suitable for A?
N
Question 32: Analysis of organic compounds X see that every three parts of the carbon mass have one part of the hydrogen, 7 parts of the nitrogen and 8 parts of the sulfur. In the
Y
molecular formula of X there is only one sulfur atom, so the molecular formula of X is B. C2H2N2S.
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A. CH4NS.
C. C2H6NS.
D. CH4N2S.
Q
Question 33: Compound X empirical formula is CH3O. Which of the following molecular formula applies to X?
B. C2H6O2.
M
A. C3H9O3.
C. C2H6O.
D. CH3O.
KÈ
Question 34: Completely burns 0.6 grams of organic compound X, the product are through Ca(OH)2 excess solution found 2 grams precipitated and the mass of container increased by 1.24 grams. Knowing that the mass of X compared to H 2 by 15. molecular formula of X is:
ẠY
A. C2H6O.
B. CH2O.
C. C2H4O.
D. CH2O2.
D
Question 35: Completely combustible 1.88 grams of organic compound Z (containing C, H, O) required 1,904 liters of O2, yielding CO2 and H2O with a molar ratio of 4: 3. The molecular formula for Z is: A. C4H6O2.
B. C8H12O4.
C. C4H6O3.
D. C8H12O5.
Question 36: Completely burn 1.18 grams of Y (CxHyN) with enough air. Lead the gases mixture obtained into the excessCa(OH)2 solution, obtained 6 grams of precipitate and Trang 87
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9,632 liters of pure gas at standard conditions get out of the jar. Knowing that the air contains 20% oxygen and 80% nitrogen by volume. The molecular formula of Y is B. C3H9N.
C. C4H11N.
D. C4H9N.
D
ẠY
KÈ
M
Q
U
Y
N
H
Ơ
N
O
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A. C2H7N.
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3.3. Một số đề kiểm tra minh họa 3.3.1. Đề số 1 SỞ GIÁO DỤC VÀ ĐÀO TẠO NAM ĐỊNH
HỘI THI TOÁN VÀ CÁC MÔN KHTN BẰNG TIẾNG ANH NĂM HỌC 2017 - 2018 Môn: Hóa học (Thời gian làm bài: 90 phút)
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PART 1: (7.0 marks)
Question 1. A homogeneous mixture is one that is uniform, and where the different components of the mixture cannot be seen. Which of the following substances are homogeneous mixtures? A. concrete.
B. tap water.
C. distilled water.
D. oxygen.
Question 2. Atom A has 5 protons and 5 neutrons, and atom B has 6 protons and 5
O
neutrons. These atoms are...
B. atoms of different elements.
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A. isotopes. C. isomers.
D. allotropes.
B. Ba(HS)2.
C. BaSO3.
D. BaSO4.
H
A. BaS.
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Question 3. Which is the chemical formula of barium sulfite?
N
Question 4. Which gas should not be collected over water due to its high solubility in water?
B. CO2.
C. CO.
Y
A. NH3.
D. N2.
B. Silver chloride.
Q
A. Zinc chloride.
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Question 5. Which solute is the least soluble in water? C. Sodium chloride.
D. Potassium chloride.
Question 6. Sodium metal and chlorine gas react to form sodium chloride. Which one of
M
the following statements concerning this reaction is correct? B. Na+ is the oxidising agent.
C. Cl2 is oxidised.
D. Na is oxidised.
KÈ
A. Cl- is the oxidising agent.
Question 7. Phenolphthalein in acidic solution is
ẠY
A. orange colored.
B. yellow colored.
C. colorless.
D. pink colored.
D
Question 8. Which oxide produces an acidic solution when mixed with water? A. CaO.
B. N2O5.
C. CO.
D. SiO2.
Question 9. Which of the following reactions is a redox reaction? A. Fe(NO3)2 + AgNO3 Ag + Fe(NO3)3.
B. Na2SO3 + H2SO4 Na2SO4 + SO2 + H2O.
C. AgNO3 + KI AgI + KNO3.
D. NaOH + H2SO4 Na2SO4 + H2O.
Question 10. Which element has the greatest electronegativity? Trang 89
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A. Ge.
B. Si.
C. Sn.
D. C.
Question 11. Both CO and CO2 A. burn in air.
B. turn lime water milky.
C. are produced by the combustion of carbon.
D. change the colour of universal
indicator. A. Lose, positive.
B. Lose, negative.
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Question 12. When metals _____ electrons, they become ____ ions. C. Gain, negative.
D. Gain, negative.
Question 13. Which of the following diatomic molecules is joined by a triple covalent bond? A. N2.
B. HCl.
C. O2.
D. H2.
Question 14. Which of the following formula is a hydrocarbon? B. CH4.
C. CH4O.
O
A. CCl4.
D. CH5N.
Question 15. What is the oxidation number of carbon atom in calcium carbide? B. -1.
C. -2.
H
A. potassium iodide with silver nitrate.
Ơ
Question 16. Which will not result in a reaction?
D. 1-.
N
A. 2-.
N
B. potassium iodide with chlorine water.
C. potassium bromide with silver nitrate.
Y
D. potassium bromide with aqueous iodine.
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Question 17. Which test will identify NH4NO3?
Q
A. Reaction with BaCl2 forming a white precipitate. B. Reaction with acid causing effervescence.
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C. Reaction with silver nitrate forming a precipitate.
KÈ
D. Reaction with sodium hydroxide forming a characteristic gas which turns blue litmus red.
Question 18. Which substance will react with dilute sulfuric acid to produce sulfur
ẠY
dioxide?
D
A. zinc metal.
B. sodium sulfite.
C. sulfur trioxide.
D. potassium sulfide.
Question 19. Which gas will react a solution containing potassium iodide and starch to turn it a blue-black color? A. O2.
B. H2S.
C. Cl2.
D. N2.
Question 20. How many grams of Al2(SO4)3 contain 27.36 g of oxygen? A. 48.78.
B. 146.33.
C. 5.12.
D. 15.35. Trang 90
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Question 21. How many other atoms form covalent bonds with each carbon atom in diamond? A. 2.
B. 5.
C. 3.
D. 4.
Question 22. Which substance has the highest melting point? A. H2O.
B. HCl.
C. MgO.
D. CO2.
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Question 23. In which list are the ions arranged in the order of increasing size? A. Na+ < Mg2+ < O2- < F-.
B. F- < O2- < Mg2+ < Na+.
C. Mg2+ < Na+ < F- < O2-.
D. O2- < F- < Na+ < Mg2+.
Question 24. 4.80 g of an element, M, reacts with excess chlorine to produce 13.32 g of the salt. What is the element? A. S.
B. Cr.
C. Se.
D. Ca.
O
Question 25. When the following reaction is balanced, what is the ratio of coefficients of H+(aq) to Fe3+(aq)? B. 1 : 8.
C. 5 : 4.
D. 5 : 1.
Ơ
A. 8 : 5.
N
Fe2+(aq) + MnO4-(aq) + H+(aq) Fe3+(aq) + Mn2+(aq) + H2O.
B. 4.
C. 1.
D. 3.
N
A. 5.
H
Question 26. Ethylene has the formula CH2=CH2. How many sigma bonds does it have? Question 27. What is the molarity of the nitrate ion in 500.0 mL of a solution containing
Y
2.25 g of copper (II) nitrate and 2.52 g of nitric acid? B. 0.091 M.
U
A. 0.280 M.
C. 0.155 M.
D. 0.128 M.
Q
Question 28. Sodium azide is a commonly used compound in airbags. When triggered, it
M
has the following reaction:
2 NaN3 (s) 2Na (s) + 3N2 (g).
KÈ
If 26.0 grams of sodium azide are reacted, how many moles of nitrogen gas would we expect to produce? A. 0.26.
B. 0.40.
C. 0.60.
D. 0.20.
D
ẠY
Question 29. At 400ºC, ammonia decomposes to nitrogen and hydrogen: 2NH3 (g) N2 (g) + 3H2 (g)
In one experiment, the concentration of ammonia decreased from 0.0450 M to 0.0420 M over the course of 100 s. What was the average rate of disappearance of NH3 (g)? A. 1.0 x 10-5 M/s.
B. 6.0 x 10-5 M/s.
C. 3.0 x 10-5 M/s.
D. 1.5 x 10-5 M/s.
Question 30. The mass of a single molecule of an allotrope of sulfur is 3.20×10-22 g. How many sulfur atoms are present in a molecule of this allotrope? Trang 91
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A. 6.
B. 16.
C. 12.
D. 8.
Question 31. What is the molarity of a potassium hydroxide solution if 50.0 mL is exactly neutralized by 38.0 mL of 0.020 M hydrochloric acid solution? A. 0.009 M.
B. 0.015 M.
C. 0.021 M.
Question 32. For the exothermic reaction: N2 (g) + 3H2 (g)
D. 0.038 M.
2NH3 (g).
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Which change will increase the quantity of NH3 in the mixture? A. adding catalyst.
B. decreasing the concentration of N2 (g).
C. increasing temperature.
D. decreasing container volume.
Question 33. What is the pH of a solution prepared by mixing 50.0 mL of 0.12 M NaOH with 30.0 mL of 0.10 M HNO3? A. 1.4.
B. 13.1.
C. 2.7.
D. 12.6.
O
Question 34. The aqueous solubilities of several compounds between temperatures of 0oC and 80oC are shown in this diagram. Which compound can be recovered with the highest
U
Y
N
H
Ơ
N
percent yield by dissolving a sample in water at 80oC and cooling to 0oC?
A. X2.
B. X1.
C. X3.
D. X4.
Q
Question 35. A 1:1 mixture of ethyl alcohol and water is separated by fractional
M
distillation in the apparatus shown. At what temperature does the first drop of condensate
D
ẠY
KÈ
appear on the thermometer?
A. less than 78.4oC.
B. 78.4oC.
C. between 78.4oC and 100.0oC.
D. more than 100.0oC. Trang 92
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PART 2: (3.0 marks) Question 1: White phosphorus consists of a molecule made up of four phosphorus atoms. It burns in pure oxygen to produce tetraphosphorus decaoxide. 1. Write a balanced equation for the reaction that takes place. 2. A 6.20 g piece of white phosphorus is burned in a flask filled with 8.96 liters of SOLUTION: (1.0 marks) 1. Write a balanced equation P4 + 5O2 P4O10.
6.20 g = 0.05 mole 31.0 g/mole x 4
n O2 =
8.96 l = 0.40 mole 22.4 l/mole
N
n P4 =
Ơ
P4 is the limiting reactant. n P = n P O = 0.05 mole 4
H
4 10
4 10
= n P O x M P O = 0.05 mole x (31 g/mole x 4 + 16 g/mole x 10) = 14.2 g 4 10
4 10
N
mP O
O
2. What mass of tetraphosphorus decaoxide is produced?
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oxygen gas at STP. What mass of tetraphosphorus decaoxide is produced?
Question 2: The solubility of highly soluble, thermally unstable salts such as ammonium
Y
chloride may be determined by back titration.
U
In one experiment a 10.0 mL saturated solution of ammonium chloride (X solution),
Q
NH4Cl, at 20.0oC, was diluted with distilled water to 500.0 mL in a standard flask (Y
M
solution). A 10.0 mL aliquot of this solution (Y solution) was added to 10.0 mL of 0.500 M KOH solution. The solution was heated to drive off the ammonia formed by this reaction.
KÈ
After the flask was cooled, the excess hydroxide ions were neutralised by 35.8 mL of 0.100 M HCl solution.
ẠY
1. Write an equation for the neutralisation reaction. 2. Determine the amount, in mole, of KOH that was originally added to the ammonium
D
chloride solution. 3. Determine the amount, in mole, of ammonium chloride in the 10.0 mL aliquot (Y
solution). 4. Calculate the amount, in mole, of ammonium chloride in 10.0 mL of the saturated solution (X solution). 5. Calculate the solubility, in g/L, of ammonium chloride in water at 20.0 oC. Trang 93
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SOLUTION: 1. Write an equation for the neutralisation reaction. KOH + HCl KCl + H2O. 2. Determine the amount, in mole, of KOH that was originally added to the ammonium
n KOH =
10.0 mL x 0.500 mole/L= 5.0 x 10-3 mole 1000
FF IC IA L
chloride solution.
3. Determine the amount, in mole, of ammonium chloride in the 10.0 mL aliquot.
n HCl =
35.8 mL x 0.100 mole/L = 3.6 x 10-3 mole 1000
n KOH(react with ammonium chloride) = 5.0 x 10-3 mole - 3.6 x 10-3 mole = 1.4 x 10-3mole
O
n NH Cl = n KOH = 1.4 x 10-3 mole 4
4. Calculate the amount, in mole, of ammonium chloride in 10.0 mL of the saturated
N
solution.
500.0 mL = 7.1 x 10-2 mole 10.0 mL
H
4
Ơ
n NH Cl(in 500.0 mL Y solution) = 1.4 x 10-3 mole x
n NH Cl(in 10.0 mL X solution) = n NH Cl(in 500.0 mL Y solution) = 7.1 x 102 mole 4
N
4
5. Calculate the solubility, in g/L, of ammonium chloride in water at 20.0 oC.
Y
m NH 4Cl(in 10.0 mL X solution) = n NH 4Cl x M NH 4Cl
U
= 7.1 x 102 mole x (14 g/mole + 4 x 1 g/mole + 35.5 g/mole) = 3.7985 g 1000 = 379.85 g/L 10.0 mL
D
ẠY
KÈ
M
Q
S NH 4Cl = 3.7985 g x
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Sáng kiến kinh nghiệm năm học 2018 - 2019
3.3.2. Đề số 2 SỞ GIÁO DỤC VÀ ĐÀO TẠO NAM ĐỊNH
HỘI THI TOÁN VÀ CÁC MÔN KHOA HỌC BẰNG TIẾNG ANH Năm học 2018-2019 Môn: HÓA HỌC – THPT
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PART 1: (7.0 marks)
Question 1. Metal oxides are typically _______ while nonmetal oxides are typically _______. A. acidic, basic.
B. basic, amphoteric.
C. basic, acidic.
D. amphoteric, basic.
Question 2. Calcium carbonate, CaCO3, decomposes upon heating to calcium oxide and
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carbon dioxide. What mass of solid calcium carbonate is required to produce 5.60 liters of carbon dioxide measured at STP? B. 25.025.
C. 35.035.
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A. 40.04.
D. 30.03.
I-(aq) + IO-(aq) + H2O(l)
H
I2(aq) + 2OH-(aq)
the right?
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Question 3. Which change would move the position of the following equilibrium towards
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A. Adding sulfuric acid.
B. Adding solid potassium hydroxide and stirring to dissolve it.
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C. Increasing the pressure.
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D. Adding solid potassium iodide and stirring to dissolve it.
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Question 4. The correct name for CO is _______. A. carbon dioxide.
B. carbonous.
C. carbon monoxide. D. carbonic.
A. O2, H2 and HCl.
B. H2 and Cl2O.
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Question 5. What are the products of the reaction between chlorine and water? D. HOCl, H2 and Cl2.
C. HCl and HClO.
Question 6. If matter is uniform throughout, cannot be separated into other substances by
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physical processes, but can be decomposed into other substances by chemical processes, it
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is_______ A. a homogeneous mixture.
B. a heterogeneous mixture.
C. an element.
D. a compound.
Question 7. When aqueous solutions of _______ are mixed, a precipitate forms. A. K2SO4 and CrCl3.
B. NaI and KBr.
C. NaBr and AgNO3.
D. Li2CO3 and CsI. Trang 95
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Question 8. One component of gastric (stomach) fluid is hydrochloric acid (HCl). Baking soda (NaHCO3) will neutralize HCl according to the reaction: NaHCO3 (aq) + HCl (aq) → NaCl (aq) + H2O (l) + CO2 (g). How many grams of CO 2 are produced when 200 mL of 0.50 mol L-1 HCl reacts with 100 mL of 0.8 mol L-1 NaHCO3? B. 1.79.
C. 3.52.
D. 2.24.
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A. 4.40.
Question 9. What numerical values of d is required to balance the equation below?
10FeSO4 (aq)+aKMnO4 (aq)+bKHSO4 (aq)→cFe2(SO4)3 (aq)+dK2SO4 (aq)+eMnSO4 (aq)+fH2O (l). A. 9.
B. 15.
C. 24.
D. 1.
Question 10. How many dichlorinated isomers can be formed by the halogenation of A. 5.
B. 3.
C. 4.
Question 11. The major gas in the air is B. trace gases.
C. nitrogen.
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A. oxygen.
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CH3CH2CH2CH3 with Cl2 in the presence of light?
D. 6.
D.carbon dioxide.
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Question 12. Which list represents the halogens in increasing order of oxidizing strength B. I2; Br2; Cl2.
C. Cl2; Br2; I2.
D. I2; Cl2; Br2.
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A. Br2; Cl2; I2.
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(weakest oxidizing agent first)?
Question 13. In chemistry, water of crystallization or water of hydration are water
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molecules that are present inside crystals. Water is often incorporated in the formation of
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crystals from aqueous solutions. Give that you had 9.768 g of zinc oxide. What mass of
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hydrated zinc (II) chloride crystals (ZnCl2.2H2O) could be produced by reaction with excess hydrochloric acid?
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A. 20.460.
B. 25.860.
C. 16.368.
D. 20.688.
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Question 14. Which one of the following types of compound is added to natural gas (methane) in order to detect a leakage of that gas? A. Isopentane.
B. Mercaptans.
C. Nitrogen.
D. Carbonic.
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Question 15. Which of the following elements has the largest number of compounds?
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A. Nitrogen.
B. Carbon.
C. Sodium.
D. Oxygen.
Question 16. The molar concentration of urea [(NH2)2CO] in a solution prepared by
dissolving 18.0 g of urea in enough water to give a final volume of exactly 250 mL: A. 1.2 M.
B. 0.4 M.
C. 1.5 M.
D. 0.7 M.
Question 17. What is physical state of the first four alkanes (at room temperature and atmospheric pressure)? A. Plasma.
B. Solid.
C. Gas.
D. Liquid. Trang 96
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Question 18. Which of the following mixtures cannot be separated by sublimation? A. Ammonium chloride and sand.
B. Ammonium chloride and sodium chloride.
C. Ammonium chloride and iodine.
D. Ammonium chloride and copper sulfate.
Question 19. Which one of the following compounds contains both ionic and covalent bonds? B. NaCl.
C. H2SO4.
D. (NH4)2CO3.
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A. N2.
Question 20. In chemistry, the empirical formula of a chemical compound is the simplest positive integer ratio of atoms present in a compound. Of the following, the only empirical formula is A. C6H6.
B. C12H22O11.
C. C2H4.
D. C6H12O6.
Question 21. Which pair of species is listed in increasing order of the property given? B. Radius: K, Mg.
C. Melting point: I2, Br2.
D. Metallic character: K, Na.
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A. Electronegativity by Pauling scale: O, F.
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Question 22. Vitamin C, a compound of carbon hydrogen and oxygen only, is found in
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many fruits and vegetables. The percentages of carbon, hydrogen, and oxygen in vitamin C
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are determined by burning a sample of vitamin C weighing 2.00 mg. The masses of carbon
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dioxide and water formed are 3.00 mg and 0.818 mg, respectively. By titration its molar mass is found to be about 176. How many are atoms present in a vitamin C molecule? B. 14.
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A. 24.
C. 20.
D. 10.
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Question 23. A solution reacts with crushed egg-shells to release a gas that turns limeA. NaCl.
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water milky. The solution contains
B. KCl.
C. CaCl2.
D. HCl.
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Question 24. Sulfur and fluorine react in a combination reaction to produce sulfur
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hexafluoride:
S (s) + F2 (g) → SF6 (g).
In a particular experiment, the percent yield is 79.0%. This means that a 7.9 g sample of
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fluorine yields _______ g of SF6 in the presence of excess sulfur.
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A. 28.4.
B. 35.9.
C. 10.1.
D. 8.0.
Question 25. What is the name of this compound: CH2=C(CH3)2. A. Isobutylene.
B. α-butylene.
C. Butane
D. 2-methylpropane.
Question 26. Equal masses of powdered calcium carbonate were added to separate solutions of hydrochloric acid. The calcium carbonate was excess. The volume of carbon dioxide produced was measured at regular intervals. Which curves best represent the evolution of carbon dioxide against time for the acid solutions shown in the table below. Trang 97
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B. I - X; III - Y; IV - Z.
C. I - X; IV - Y; III - Z.
D. II - X; I - Y; III - Z.
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Question 27. Consider the following reaction:
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A. I - X; II - Y; IV - Z.
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H+(aq) + Fe2+(aq) + NO2-(aq) → Fe3+(aq) + NO(g) + H2O(l).
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Which statement is correct?
A. NO2- is the reducing agent because it undergoes oxidation.
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B. Fe2+ is the reducing agent because it undergoes reduction.
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C. NO2- is the oxidizing agent because it undergoes oxidation.
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D. Fe2+ is the reducing agent because it undergoes oxidation. Question 28. Which one of the following is a chemical property rather than a physical
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property?
B. Flammability.
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A. Melting point.
C. Viscosity.
D. Brittleness.
Question 29. Which of the following are usually found in the nucleus of an atom? B. Protons and neutrons only.
C. Neutrons only.
D. Protons, neutrons and electrons.
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A. Electrons and neutrons only.
D
Question 30. Elemental silicon is oxidized by O2 to produce a compound which dissolves
in molten Na2CO3. When this solution is treated with aqueous hydrochloric acid, a precipitate forms. What is the precipitate? A. SiH4.
B. NaHSiO3.
C. SiO2.
D. Na2SiO3.
Question 31. The element that does not react with chlorine gas (Cl2) is A. Fe (s).
B. O2 (g).
C. Mg (s).
D. H2 (g). Trang 98
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Question 32. The pH of a solution prepared by mixing 45 mL of 0.183 M KOH and 65 mL of 0.145 M HCl is _______. A. 1.97
B. 0.74
C. 2.92
D. 1.31
Question 33. Which one of the following acids is diprotic? A. H3PO4.
B. HNO3.
C. CH3COOH.
D. H2SO4.
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Question 34. When 100 mL of 1.0M Na3PO4 is mixed with 100 mL of 1.0M AgNO3, a yellow precipitate forms and [Ag+] becomes negligibly small. Which of the following is a correct listing of the ions remaining in solution in order of increasing concentration? A. [NO3-]; [Na+]; [PO43-].
B. [PO43-]; [NO3-]; [Na+].
C. [Na+]; [PO43-]; [NO3-].
D. [PO43-]; [Na+]; [NO3-].
Question 35. When 4.0 g of sulfur is burnt in oxygen, 40 kJ of heat is released. How much A. 320 kJ.
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heat is released when 1.0 mole of sulfur undergoes complete combustion? B. 10 kJ.
C. 160 kJ.
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PART 2: (3.0 marks)
D. 40 kJ.
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Question 1: Each of the five bottles contains one of the following solutions: barium
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nitrate; hydrochloric acid; sodium hydrogen carbonate; sodium carbonate; sulfuric acid. A Reactants
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student mixed pairs of these solutions together and obtained the following results. Observation Bubbles
Solution 2 and solution 3
No reaction
Solution 2 and solution 4
White precipitate
Solution 1 and solution 5
No reaction
Solution 4 and solution 5
No reaction
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Q
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Solution 1 and solution 2
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1. Use the information to identify the five solutions. (Candidates do not need to give an
explanation).
2. Write a correctly balanced equation to represent each of the following reactions:
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a. Between solution 1 and solution 2.
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b. Between solution 2 and solution 4. Answers: (1.0) 1. (0.5) Solution 1: Na2CO3;
Solution 2: H2SO4;
Solution 4: Ba(NO3)2;
Solution 5: NaHCO3.
Solution 3: HCl;
2. (0.5) Trang 99
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a. Na2CO3 + H2SO4 → Na2SO4 + CO2 + H2O. b. H2SO4 + Ba(NO3)2 → BaSO4 + 2HNO3. Question 2: Treatment of alkane X (molecular formula, C7H16) with chlorine molecule (Cl2) in the presence of light or heat produce seven monochlorinated products. Draw structural formula of X. (Candidates do not need to give an explanation).
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Answers: (1.0)
Question 3: Sulfur dioxide is a major air pollutant and has significant impacts upon
human health. Sulfur dioxide emissions are a precursor to acid rain and atmospheric
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particulates. Combustion of fossil fuels contaminated with sulfur compounds produces sulphur dioxide.
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In the European Union, the “Euro IV” standard has been since 2005, which specifies a
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maximum of 50 ppm of sulfur in diesel fuel for most highway vehicles. Calculate the
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ppm of sulfur) is consumed at STP?
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volume of sulfur dioxide produced when a full tank (capacity 60 kg) of diesel (contain 50 Note: ppm (parts per million 10-6) e.g. 10000 ppm = 1%.
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Answers: (1.0)
3.0 g = 0.093 mol 32.1 g/mol
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nS =
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mS = 60.0 kg x 50.10-6 = 3.0 x 10-3 kg = 3.0 g.
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n S = n SO2 = 0.093 mol
D
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VSO2 = 0.093 mol x 22.4 l = 2.09 l
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3.3.1. Đề số 3 TRƯỜNG THPT NGUYỄN KHUYẾN
ĐỀ THI THỬ LẦN 1 TOÁN VÀ CÁC MÔN KHTN BẰNG TIẾNG ANH NĂM HỌC 2018 - 2019 Môn: Hóa học (Thời gian làm bài: 90 phút)
Question 1: Which of the following is a nonmetal? A. Gold
B. Potassium
C. Sulfur
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I. PART 1: (7.0 marks) D. Copper
Question 2: What is the number of electrons in an ion with 24 neutrons, a charge of 3+, and an mass number of 45? A. 21
B. 18
C. 24
D. 66
neutral particles 20. The symbol to this element is 52 24
B.
Cr
81 35
C.
Br
51 25
Mn
D.
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A.
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Question 3: Total particles in X atom are 76; Some more charged particles are electrically 56 26
Fe
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Question 4: At 20 degrees c, an atom with density of 7.87 gram/cm3 and the radius of 1.28A0. In fact real, volume occupied by atoms only 74% of the remaining crystals are the B. Iron (55.85 amu)
D. Silver (107.87 amu)
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C. Zinc (65.41 amu)
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A. Coppper (63.54 amu)
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empty slots. Element name is
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Question 5: Copper has two naturally occuring isotopes. Cu-63 has an abundance of 72.7%. The average atomic weight of copper =63.546 amu. What is the atomic mass of the
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second isotope?
B. 35
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A. 63
C. 65
D. 64
Question 6: Which solute is the least soluble in water? B. barium sulfate.
C. Sodium sulfide.
D. barium sulfide.
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A. Zinc sulfate.
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Question 7: Which of the following reactions is a redox reaction? A. CaCO3 + H2O + CO2 → Ca(HCO3)2.
D
C. 2SO2 + O2 → 2SO3
B. P2O5 + 3H2O → 3 H3PO4. D. BaO + H2O → Ba(OH)2
Question 8: Which of the following formula is an organic compound? A. Na2CO3
B. NH4HCO3
C. KCN
D. (NH2)2CO
Question 9: Which of the following pyrolysis reactions is incorrect? 0
t A. 2KNO3 2KNO2 + O2 0
t C. NH4Cl NH3 + HCl
0
t B. NH4NO3 N2O + 2H2O 0
t D. Cu(NO3)2 Cu + 2NO2 + O2
Trang 101
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Question 10: Which of the following reactions has a reduced ion equation of HCO3- + OH CO32- + H2O?
A. 2NaHCO3 + Ca(OH)2 CaCO3 + Na2CO3 + 2H2O. B. 2NaHCO3 + 2KOH Na2CO3 + K2CO3 + 2H2O D. Ca(HCO3) + 2NaOH CaCO3 + Na2CO3 + 2H2O.
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C. NaHCO3 + HCl NaCl + CO2 + H2O. Question 11: Which gas can be collected over water due to insolube in water? A. NH3
B. HCl
C. SO 2
Question 12: Purple litmus in basic solution is A. blue colored.
B. yellow colored.
D. N2
C. colorless.
D. red colored.
Question 13: What is the oxidation number of sulfur atom in sulfuric acid? B. +4
C. +6
D. 6+
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A. 2A. CH4
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Question 14: Which substance has the highest boiling point? B. C2H6
C. C4H10
D. C5H12
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Question 15: What is the pH of a solution prepared by mixing 500.0 mL of 0.2 M Ba(OH) 2 B. 12
C. 7
D. 1
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A. 13
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with 30.0 mL of 0.20 M HNO3?
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Question 16: Procedure the following experiment:
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glass
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hành
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X crystal
D
X crystal is A. Na2CO3.
B. NH4NO2.
C. NaCl.
D. NH4Cl.
Question 17: What is the molarity of the ammonium ion in 200.0 mL of a solution containing 3.96 g of ammonium sulfate and 8.94 g of ammonium phosphate? A. 1.2 M.
B. 1.8 M.
C. 0.8 M.
D. 0.3 M.
Question 18: When dissolving 3.60 grams of magnesium in 500 ml of 0.80M nitric solution, 0.448 liters of X gas (in the STP) are observed to escape and a Y solution ( the Trang 102
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mass of Y is 3.04 grams greater than the mass of initial nitric solution). The substances in Y react equivalently with V(ml) of 2.00M sodium hydroxide solution. The value of V is A. 230.00.
B. 156.25.
C. 173.75.
D. 167.50.
Question 19: What is the molarity of a barium hydroxide solution if 50.0 mL is exactly neutralized by 80.0 mL of 0.120 M nitric acid solution? B. 0.048 M.
C. 0.096 M.
Question 20: The two gases that can exist in a mixture are A. NH3 and Cl2.
B. H2S and Cl2.
D. 0.192 M.
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A. 0,24 M.
C. HCl and CO2.
D. NH3 and HCl
Question 21: Given X solution is 1M Ca(OH)2 solution. Experiment 1: 3.36 liters of CO 2 gas at STP is absorbed completely in V liter of X solution, obtained 3b mol of precipitate.
Experiment 2: 8.96 liters of CO2 gas at STP is absorbed completely in V liter of X A. 0.25 and 0.05
B. 0.2 and 0.05
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solution, obtained 2b mol of precipitate. Values of V and b are respectively C. 0.3 and 0.1
D. 0.4 and 0.1
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Question 22: When an atom loses electrons, it becomes
B. Neutral atom.
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A. Negatively charged.
D. Positively charged.
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C. No charge.
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Question 23: Of the subatomic particles, which one has the lowest mass? A. protons
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C. neutrons
B. electrons D. none, they all have almost the same
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Question 24: What is the maximum number of electrons of 4th shell? B. 8
C. 18
D. 32
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A. 2
Question 25: Which of the following conclusions is false?
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A. The nucleus is posively charged.
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B. The atom is a dense solid and is indivisible. C. The nucleus is very small and the atom is mostly empty space D. The nucleus is the center of an atom.
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Question 26: When the following reaction is balanced, what is the ratio of coefficients of
D
KMnO4 to SO2? SO2 + KMnO4 + H2O K2SO4 + MnSO4 + H2SO4
A. 2/5.
B. 5/2.
C. 2/3.
D. 3/2.
Question 27: In which list are the ions arranged in the order of increasing size? A. Ca 2+< K+ < Cl−< S2-
B. K+ < Cl−< Ca 2+< S2−
C. S2− < Cl−< K+< Ca2+
D. Cl−< K+ < S2-< Ca2+ Trang 103
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Question 28: When dripping NaOH solution into AlCl3 solution, test results are shown on the following graph (data in molar units): Al(OH)3
0,5a
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a
OH-
0
x
y
Ratio x: y is B. 6:7
C. 5:4
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A. 7: 8 PART 2: (3.0 marks)
D. 4:5
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Question 1: Assemble the apparatus as show in the following figure.Give the observed
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phenomenon in the erlenmeyer flask ; explain and write the chemical reations that occurred
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in the experiment?
X gas
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Y
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HCl solution
KÈ
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CaCO3
Ca(OH)2 solution
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Solution:
D
- Phenomenon: a white precipitate appears in the erlenmeyer flask, the precipitate can dissolve to recreate the transparent solution. - Write the chemical reations : 2HCl(aq) + CaCO3(s) CaCl2(aq) + CO2(g) + H2O(l) X gas is CO2: colorless gas CO2(g) + Ca(OH)2(aq) CaCO3(s) + H2O(l) Trang 104
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White precipitate If CO2 resudal, white precipitate will be dissolved CO2(g) + CaCO3(s) + H2O(l) Ca(HCO3)2 disolve Question 2: An atom with the mass of 196.97 amu;
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Calculate the density in grams per cubic centimeter.
the volume of 1.0210-23 cm3.
Solution:
The atom mass in gram of this atom is: 196.97x1.6605x10-24= 3.27x10-22gram
3.27 x10 22 32.07 g / cm3 1.02 x1023
the density in grams per cubic centimeter of this atom is:
Question 3: Gas mixture X consists of two hydrocarbons A, B at normal conditions. The
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molecular mass of A is smaller than the molecular mass of B. A, B are in the same
homologous series. Hydrocarbon A accounts for 75% of volume in mixture X. The
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complete oxidation reaction of X; the burned products are absorbed by an excess of barium
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hydroxide solution. After the experiment obtained 19.7 grams of precipitate and the mass of
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the base solution decreased by 12.78 grams. Calculate the vapor density of X compared to
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hydrogen. Find the molecular formulas of A, B? Solution:
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Complete combustion X, the combustion products include CO 2 and H2O
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the combustion products absorbed by an excess of barium hydroxide solution obtained 19.7
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grams of precipitate the number mole of BaCO3 is 19.7/197 = 0.1 mol CO2 + Ba(OH)2 BaCO3 + H2O ←
0.1 mol
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0.1
KÈ
mCO2 + mH2O = 19.7 -12.78 = 6.92 grams mH2O = 6.92 - mCO2 = 6.92 – 0.1x44 = 2.52 grams nH2O = 0.14 mol A, B are in the same homologous series and nH2O > nCO2 A and B are ankanes
ẠY
nX = nH2O - nCO2 = 0.14 -0.1 =0.04 mol
D
Hydrocarbon A accounts for 75% of volume in mixture X nA = 0.04 x75% = 0.03 mol
We have : C
nB = 0.04 -0.03= 0.01 mol nC 0.1 2.5 n X 0.04
The molecular mass of A is smaller than the molecular mass of B the number of carbon atom in A < 2.5 , the number of carbon atom in B > 2.5 A has 1 or 2 carbon atoms Trang 105
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+) If A has 1 carbon atom : 0.03 x 1 + 0.01 x (the number of carbon atom in B) = nC( in CO2) = 0.1 the number of carbon atom in B = 7 ( not accept, because A and B are gases at normal conditions) +) If A has 2 carbon atom :
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0.03 x 2 + 0.01 x (the number of carbon atom in B) = nC( in CO2) = 0.1 the number of carbon atom in B = 4 ( accept)
Thus, the molecular formulas of A is C2H6; the molecular formulas of B is C4H10; 3.3.4. Đề số 4
Question 1. Give the following alkane mixtures: pentane (boiling at 36oC), heptane (boiling at 98oC), octane (boiling at 126oC), nonane (boiling at 151oC). How can we separate these A. Crystallization.
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substances? B. Distillation
C. Sublimation.
D. Extract.
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Question 2. The phenomena of chemical compositions and properties are similar, they are
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more than one or more methylene groups (-CH2-) are called phenomena B. isotopes.
C. homogeneous
D. Constitutional isomers
N
H
A. isomerism.
Question 3. Incorrect statement is:
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A. The nature of substances depends on molecular composition and chemical structure.
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B. Substances of the same molecular mass are isomers.
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C. Substances that are isomers of each other have the same molecular formula. D. Geometric isomers are substances that have the same molecular formula, the same
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structural formula and differently the distribution of atomic groups in space
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Question 4. Since ancient times people have known how to separate organic compounds as follows:
1. Crushed indigo leaves, put in water, filter the color solution to dye clothes
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2. Cook the alcohol
D
3. Making sugar from sugarcane juice Which separation method has been used in the above ways A. Crystallization, extraction, distillation
B. Crystallization, distillation, extraction
C. Distillation, extraction, crystallization
D. Extraction, distillation, crystallization
Question 5. Combustion 0.1 mol of X requires 6.16 liters of O 2, yields 13.44 liters mixture( at STP) of ( CO2, N2 and water vapor). After condensing out of steam, the remaining 5.6 Trang 106
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liters of gas (at STP ) has a ratio of mass compared with hydrogen is 20.4 The molecular formula of X is: A. C2H7O2N.
B. C3H7O2N.
C. C3H9O2N.
D. C4H9N.
Question 6. Nitrogen is oxidized in reaction to what substance A. H2
B. O2
C. Li
D. Mg
A. P2O5
B. H2SO4 concentration
C. CuO powder
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Question 7. Which of the following substance can dry NH3 gas with moisture vapor? D. NaOH solid
Question 8. In the laboratory, the phosphoric acid was prepared according to the following reaction A. P + 5HNO3( con.) H3PO4 + 5NO2 + H2O B. Ca3(PO4)2 + 3H2SO4 2H3PO4 + 3CaSO4
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C. 4P + 5O2 P2O5 và P2O5 + 3H2O 2H3PO4
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D. 2P + 5Cl2 2PCl5 và PCl5 + 4H2O H3PO4 + 5HCl
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Question 9. Which of the following experiments was the precipitation after the reaction was complete?
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A. CuCl2 solution reacts with excess NH3 solution
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B. NaAlO2 solution reacts with excess HCl solution
C. AlCl3 solution reacts with excess NaOH solution
Y
D. ZnSO4 solution reacts with excess Ba(OH)2 solution
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Question 10. Salt B has the following characteristics:
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- When pyrolysis salt B creates gas - Dissolve B into water then add HCl solution, we see colorless gas then turn to brown in the
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air escaping. Salt B is
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A. CaCO3
B. Cu(NO3)2
C. Al(NO3)3
D. Fe(NO3)2
Question 11. Which ones of the following properties of pure liquid do not change with
D
ẠY
different amount of matter? A. Boiling point, Melting Point
B. Volume, Density
C. Mass, Volume
D. Density,
Mass
Question 12. Which ones of the following statements are always true related to periodic table? A. s and d block elements are all metal B. p block elements are nonmetal and noble gases C. There are nonmetals before noble gases. Trang 107
Sáng kiến kinh nghiệm năm học 2018 - 2019
D. There are halogens before noble gases Question 13. If number of electrons of X+3, Y-3 and Z are equal, which ones of the following statements are true for them. A. X has largest nuclear charge C. The number of protons of Y is more than that of Z is 3 D. Volume of Y-3 ion is larger than others
FF IC IA L
B. The number of protons of X is more than that of Y is 6
Question 14. Consider the following reaction, which takes place in a closed container: A(s) + B(g) → AB(g) ∆H < 0
If you wanted to increase the rate of the reaction, which of the following would you do? B. decrease the temperature of A
C. grind A into a fine powder
D. decrease the pressure
O
A. decrease the concentration of B
Question 15. Let excess Ba(OH)2 solution react with solution which contains FeCl2, CuSO4
N
and AlCl3 to produce precipitation A. Heat A in air to constant mass to produce solid X. X
Ơ
contains:
B. Fe2O3, CuO, BaSO4
C.Fe2O3, CuO
D. Fe3O4, CuO, BaSO4
N
H
A. FeO, CuO, Al2O3
A. Polar covalent bond
Y
Question 16. What bond is oxygen molecular?
U
C. Non-polar covalent bond
B. Ion bond D. Receiving bond
Q
Question 17. For chemical reaction: Cl2 + KOH KCl + KClO3 + H2O The ratio between the chlorine atoms are oxidized and chlorine atoms as are reduced in the
KÈ
A. 5: 1.
M
chemical equation of reaction gave respectively B. 1: 3.
C. 3: 1.
D. 1: 5.
Question 18. A solution containing 1 g of HBr is poured into a solution containing 1 g of NaOH. A litmus paper is dipped into the obtained solution. Which color will the litmus
ẠY
paper turn?
D
A. Red
B. Blue
C. the color does not change
D. cannot be determined
Question 19. Identify the wrong content when talking about ion: A. Ion was charged particles. B.Ion can be divided into single atomic and poliatomic ions. C.Ion is formed when atoms give up or receive electrons D. negative ion is called a cation, a positive ion called anion. Trang 108
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 20. Which of the following series of substances have only polar covalent bond in the molecule: A. HCl, O3, H2S.
B. O2, H2O, NH3.
D. H2O, HF, H2S
C. HF, Cl2, H2O.
Question 21. In response burn CuFeS2 create products CuO, Fe2O3 and SO2. So a molecule of CuFeS2 will B. give up 13 electrons.
C. get 13 electrons.
D. donated 12 electrons.
FF IC IA L
A. receive 12 electrons.
Question 22. When an ionic bond is formed, the atom that transfers its valence electron out becomes an ion with ? A. positive charge and more protons B. positive charge and no change in the number of protons
O
C. negative charge and more proton
D. negative charge and no change in the number of electrons B. H2SO4
C. NaOH
D. NH3
Ơ
A. MgO
N
Question 23. Which of the following substance has both covalent bond and ionic bond?
H
Question 24. For the following process: NO3- + 4H + + 3e NO + 2H2O (1). (1) is the
N
process:
B. Reducing
C. Redox reaction
D. The process of giving, receiving electrons
Y
A. Oxidation
U
Question 25. Which separation technique is based on differences in the volatility of the A. filtration
Q
substances to be separated?
D. paper chromatography
M
C. solvent extraction
B. distillation
KÈ
Question 26. What is the process of Fe2+ → Fe3+ 1e? A. oxidation process.
B. reduction process.
C. The process of getting a proton.
D. process of self-oxidation - reduction.
ẠY
Question 27. For the following statements about the oxidation process
D
(1) the process of reducing the oxidation number of the element.
(2) the process of increasing the oxidation number of the element.
(3) the process gives up electrons of reduction agent (4) the oxidation agent receives electron The True statements are: A. (1) and (3).
B. (1) and (4).
C. (3) and (4).
D. (2) and (3). Trang 109
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 28. Using compressed, hot air, blown into the blast furnace to burn coke (in the production of cast iron), which factors affect the speed of reaction? A. Temperature, pressure.
B. increase the area.
C. Concentration.
D. catalyst.
part of the reaction is called a A. Reactant.
B. Product.
C. Catalyst.
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Question 29. A substance that is used to speed up a chemical reaction but is not used as D. oxidant agent or rectant agent
Question 30. One of the functions of the catalytic converter in your car is to oxidize carbon monoxide to carbon dioxide. If 15.0 g of carbon monoxide reacts with 9.0 g of oxygen, how many grams of which compound remains unreacted? A. 0.4 g of oxygen remains unreacted
O
B. 8.1 g of oxygen remains unreacted D. 0.8 g of carbon monoxide remains unreacted
N
C. 7.1 g of carbon monoxide remains unreacted
Ơ
Question 31. There are four vial of chemical missing labels, including: sodium
H
hidrocarbonate, sodium chloride, sodium phosphate, sodium nitrate. Using reagents to
N
identify these solutions gives the following results Vials 1 and 4 are not sodium hydrocarbonate
Y
Vials 2 and 3 do not contain sodium phosphate
U
Vial 3 does not contain sodium chloride or sodium hydrocarbonate
Q
Vial 4 is not sodium chloride or sodium nitrate Chemical in vial 2 is:
B. sodium chloride
C. sodium phosphate
D. sodium nitrate
KÈ
M
A. sodium hidrocarbonate
Question 32. Magnesium metal and oxygen gas react to form oxide. Which one of the following statements concerning this reaction is correct? B. O2- is the oxidising agent.
C. Mg is oxidised.
D. Mg2+ is the oxidising agent.
D
ẠY
A. O2 is oxidised.
Question 33. Give following statements 1. alkanes are saturated, acyclic hydrocarbons 2. Hydrogen can be eliminated from alkanes, forming alkenes 3. Heated alkanes forms a mixture which only contain alkanes with smaller molecular mass 4. The reaction of alkanes with chlorine to produce alkyl chlorides is substitution reaction 5. Alkanes are abundant in petroleum Trang 110
Sáng kiến kinh nghiệm năm học 2018 - 2019
How many correct statements: A. 2
B. 3
C. 4
D. 5
Question 34. : 200ml the mixed solution of Ba(OH)2 0,5M and NaOH 0,25M to 300 ml H2SO4 0,3M solution obtain A solution. pH of the A solution and the precipitate obtained A. pH = 2; 2.33 grams
B. pH = 1; 2.33 grams
C. pH = 12; 4,66 grams
D. pH =12; 2.33 grams
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is:
Question 35. Dissolve one divalent metal oxide with a sufficient amount of H2SO4 10% solution, the salt solution obtained was 15.17% concentration. Metal oxides are: A. ZnO.
B. FeO.
C. MgO.
D. CaO.
Exercise 1. Bacterial digestion is an economical method of sewage treatment. The reaction 5CO2(g)+55NH4+(aq) +76O2(g)
O
C5H7O2N(s) +54NO2-(aq) +52H2O(l) +109H+(aq)
N
bacterial tissue
is an intermediate step in the conversion of the nitrogen in organic compounds into nitrate
Ơ
ions. What mass of bacterial tissue is produced in a treatment plant for every 1.0 x104 kg of
Solution:
N
are consumed by the bacteria
H
wastewater containing 3.0% NH4+ ions by mass? Assume that 95% of the ammonium ions
Y
Mass of NH4+ in 1.0 x104 kg of wastewater is: 1.0 x104x3.0%=3.0x102kg
M
3.0x102kg
C5H7O2N(s) + 54NO2-(aq) +52H2O(l)+ 109H+(aq)
113kg
95%
m=
Q
55x18 kg
U
5CO2(g)+55NH4+(aq)+76O2(g)
113 x3.0 x102 x95% 32.53kg 55 x18
KÈ
Exercise 2. Methanol (CH3OH), also called methyl alcohol,is the simplest alcohol. It is used as a fuel in race cars and is a potential replacement for gasoline. Methanol can be manufactured by combination of gaseous carbon monoxide and hydrogen. Suppose 70 kg
ẠY
CO(g) is reacted with 8.60 kg H2 (g).
D
a) Write the chemical reaction occurs b) If 3.84 x 104g CH3OH is actually produced, what is the percent yield of methanol?
Solution: a) Write the chemical reaction occurs:
0C
t ,catalys CO(g) + H2(g) CH3OH(l)
b) Calculate the theoretical yield of methanol. The number mole of CO:
nCO = 70x103 : 28 = 2.5x103 mol Trang 111
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The number mole of H2:
nH2 = 8.60x103 : 2 = 4.3x103 mol
The number mole of CH3OH:
nCH3OH = 3.84 x 104: 32 = 1.2x103 mol
0C
t ,catalys CO(g) + H2(g) CH3OH(l)
We have,
nCO (equation ) nH 2 ( equation )
1 nCO ( reality ) 2.5 1 nH 2 ( reality ) 4
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→ the ef iciency of reaction is calculated according to CO 0C
t ,catalys CO(g) + H2(g) CH3OH(l)
1.2x103 mol
1.2x103 mol
←
→ the percent yield of methanol is H=
nCO ( react ) nCO ( initial )
1.2 x103 x100% x100% 48% 2.5 x103
3.3.5. Đề số 5 B. ionic.
C. nonpolar covalent.
D. polar covalent.
Ơ
A. coordinate covalent.
N
O
Question 1. The silicon-oxygen bonds in SiO2 are best described as
Question 2. A solid can be separated from a liquid by the following means B. distillation
C. filtration
D. hydration
H
A. decantation A. Ba2+
N
Question 3. Which cation forms an insoluble chloride and an insoluble sulfide? B. Cu2+
C. Mn2+
D. Pb2+
Y
Question 4. Which 0.10 M aqueous solution exhibits the lowest electrical conductivity? B. HNO3(aq)
D. Ca(NO3)2(aq)
Q
C. NH4OOCCH3(aq)
U
A. CH3COOH(aq)
Question 5. The diagram above represents the energy profile for the reaction:
M
A + B C + D.
Energy (KJ)
KÈ
85 65
D
ẠY
40
Reaction progress
What is the value of the energy released for the reaction: C + D A + B ? A. -25 kJ
B. 25 kJ
C. 85 kJ
D. -85 kJ
Question 6. . Which of the following alkene has a geometric isomer ? A. CH2=CH-CH3 C. CH3-CH=CH-CH3
B. (CH3)2C=C(CH3)2 D. (CH3)2C=CH-CH3 Trang 112
Sáng kiến kinh nghiệm năm học 2018 - 2019 55 25
Question 7. The ion
Mn 2 contains which combination of protons, neutrons and
Protons
neutrons
electrons
A
25
30
23
B
25
55
23
C
27
30
25
D
30
25
28
FF IC IA L
electrons?
Question 8. In the equation below, which species acts as the oxidizing agent? Pb(s) + PbO2(s) + 2 H+(aq) + 2 HSO4–(aq) 2 PbSO4(s) + 2 H2O(l) A. Pb(s)
C. H+(aq)
B. PbO2(s)
D. HSO4–(aq)
Question 9. Which atom has the highest electronegativity? B .P
C. Cl
D. Br
O
A. Na
N
Question 10. A 5.0 g sample of calcium nitrate (Ca(NO3)2, M = 164) contaminated with
Ơ
silica (SiO2, M = 60.1) is found to contain 1.0 g calcium. What is the mass percent purity of alcium nitrate in the sample? B. 24%
C. 73%
D. 82%
H
A. 20%
N
Question 11. Addition of 6 M HCl to which substance will NOT result in gas evolution? A. Al
B. Fe(NO3)2
C. K2CO3
D. NaNO3
Y
Question 12. A solid has a melting point of 1710 °C, is soluble in water, and does not
U
conduct electricity in the solid state. What is the most likely nature of the bonding in this
Q
solid?
A. Molecular covalent
B. Network covalent
C. Ionic
D. Metallic
KÈ
M
Question 13. The following endothermic reaction is at equilibrium in a sealed container. PCl3(g) + Cl2(g) PCl5(g)
Which of the following changes would result in an increase in the number of moles of
ẠY
PCl5(g) present at equilibrium? I. Increasing the temperature
D
A. I only
B. II only
II. Increasing the volume C. Both I and II
D. Neither I nor II
Question 14. A 1.00 g sample of a hydrogen peroxide (H 2O2) solution is placed in an erlenmeyer flask and diluted with residual sulfuric acid solution. This mixture solution is added to 0.02 M KMnO4 solution via a buret . This requires 22.50 mL of KMnO4 solution.
What is the percent by mass of hydrogen peroxide in the original solution? A. 0.613%
B. 1.53%
C. 3.83%
D. 7.65% Trang 113
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Question 15. What is the electron configuration of the Al3+ion? A. 1s22s22p6
B 1.s22s22p63s23p1
C. 1s22s22p63s23p4
D. 1s22s22p63s23p6
Question 16. Which compound contains both ionic and covalent bonds? A. PF3
B. KF
C. CH3COOH
D. MgSO4
Question 17. A student mixes 10.0 g of KClO3with 45.0 g of H2O and stirs it for a long
FF IC IA L
time at 60 ˚C until the solution is completely clear then allows it to cool slowly to 20 ˚C
Solubility g per 100g where it remains clear. Which statement about the final clearHmixture at 20 ˚C is correct? 2O 60 50 40 30 20 10 0 20
30
40
50
60
70
O
10
80
90
Temperature, 0C
N
A. It is a saturated solution.
Ơ
B. It is an unsaturated solution and can be made saturated by decreasing the temperature.
H
C. It is an unsaturated solution and can be made saturated by increasing the temperature. D. It is a supersaturated solution
N
Question 18. A 65.00 g sample of CuSO4•5H2O (M = 250) is dissolved in enough water to
U
1.00 L of 0.100 M CuSO4?
Y
make 0.800 L of solution. What volume of this solution must be diluted with water to make B. 325 mL
C. 3250 mL
D. 800 mL
Q
A. 3.25 mL
Question 19. A typical polyethylene bag from a grocery store weighs 12.6 g. How many
M
molecules of ethylene, C2H4, must be polymerized to make such a bag? A. 1.35 x 1024
B. 6.02 x 1023
C. 5.33 x 1023
D. 2.71 x 1023
KÈ
Question 20. When 0.10 M solutions of HF, HCl, KF, and KCl are arranged in order of increasing pH which order is correct? B. HCl, HF, KF, KCl
C. HCl, HF, KCl, KF
D. HF, HCl, KCl, KF
ẠY
A. HF, HCl, KF, KCl
D
Question 21. Consider the system at equilibrium: 2SO2(g) + O2(g) 2SO3(g)
∆H < 0.
Which change(s) will increase the yield of SO3(g)? I Increasing the temperature II Increasing the volume of the container A. I only
B. II only
C. Both I and II
D. Neither I nor II Trang 114
Sáng kiến kinh nghiệm năm học 2018 - 2019
Question 22. All of the reactions below represent oxidation-reduction processes EXCEPT A. combustion of tin in chlorine gas.
B. decomposition of potassium chlorate.
C. neutralization of sodium hydroxide.
D. reaction of magnesium with
hydrochloric acid. which of the following? I Atomic radius
II Metallic property
A. I and II only
B. I and III only
FF IC IA L
Question 23. Properties of the alkaline earth metals that increase from Be to Ba include III Nuclear charge C. II and III only
D. I, II, and III
Question 24. How many isomeric compounds have the formula C3H8O? A. 1
B. 2
C. 3
D. 4
Question 25. Which of the compounds below will react readily with chlorine by addition? II. C2H4(ethene)
A. I only
B. I and II only
III. C6H14(hexane)
O
I. C2H2(ethyne)
C. II and III only
D. I, II, and III
N
Question 26. Commercial vinegar is a 5.00% by mass aqueous solution of acetic acid,
Ơ
CH3COOH (M= 60.0). What is the molarity of acetic acid in vinegar? B. 1.00 M
C. 1.20 M
D. 3.00M
N
A. 0.833 M
H
[density of vinegar = 1.00 g/mL]
Question 27. In which reaction at equilibrium will the amount of reactants present increase
Y
with an increase in the container volume? B. H2(g) + F2(g) 2 HF(g)
C. CO(g) + NO2(g) CO2(g) + NO(g)
D. N2(g) + 3 H2(g) 2NH3(g)
Q
U
A. C(s) + CO2(g) 2CO(g)
Question 28. What is the pH of a solution made by mixing 200. mL of 0.0657 M NaOH, B. 2.74
KÈ
A. 3.04
M
140. mL of 0.107 M HCl, and 160. mL of H2O? C. 2.43
D. 2.27
Question 29. Consider the following reactions:
ẠY
X(NO3)2+ Y →X + Y(NO3)2
X(NO3)2+ Z →X + Z(NO3)2 Y(NO3)2+ Z →No reaction
D
What is the correct order ofincreasing activity for the metals; X, Y, Z? A. X < Y < Z
B. X < Z < Y
Question 30. In the reaction
C. Z < Y < X
D. Z < X < Y
ClO3–(aq) + 5Cl–(aq) + 6H+(aq) →3Cl2(g) + 3H2O(l)
the oxidizing and reducing agents are, respectively, A. Cl–(aq) and ClO3–(aq)
B. ClO3–(aq) and Cl–(aq)
C. ClO3–(aq) and H+(aq)
D. Cl–(aq) and H+(aq)
Question 31. What is the IUPAC name for the molecule below? Trang 115
Sáng kiến kinh nghiệm năm học 2018 - 2019
A. heptane
B. 2-ethylpentane
C. 3-methylhexane
D. 4-ethylpentane
Question 32. Which 0.10 M aqueous solution exhibits the lowest electrical conductivity? A. NH4Cl
B. CuBr2
C. Na2CO3
D. C2H5OH
Question 33. Which change(s) is chemical process? A. I only
II. freezing of water
B. III only
C. I and II only
III. sublimation of iodine
FF IC IA L
I. conversion of O2(g) to O3
D. II and III only
Question 34. In which molecule does the chlorine have the most positive partial charge? A. HCl
B. BrCl
C. OCl2
D. SCl2
Question 35. Which must represent an atom in an excited state? A. 1s22s22p1
B. 1s22s22p2
C. 1s22s22p23s1
D. 1s22s22p5
O
Exercise 1. Hydrogen peroxide is used as a cleaning agent in the treatment of cuts and abrasions for several reasons. It is an oxidizing agent that can directly kill many
N
microorganisms; it decomposes upon contact with blood, releasing elemental oxygen gas
Ơ
(which inhibits the growth of anaerobic microorganisms); and it foams upon contact with
H
blood, which provides a cleansing action. In the laboratory, small quantities of hydrogen
N
peroxide can be prepared by the action of an acid on an alkaline earth metal peroxide, such as barium peroxide:
Y
BaO2(s) + HCl(aq) H2O2(aq) + BaCl2(aq)
U
What mass of hydrogen peroxide should result when 1.521 g of barium peroxide is treated
Q
with 25.0 mL of hydrochloric acid solution containing 0.02774 g of HCl per mL? What mass of which reagent is left unreacted? The number mole of BaO2 is nBaO2 =
1.521 = 0.009 mol 169
KÈ
M
Solution:
The mass of HCl is mHCl = 25 x 0.02774 = 0.6935 gram nHCl = 0.019 mol
ẠY
The balance reaction:
D
We have
BaO2(s) + 2HCl(aq) H2O2(aq) + BaCl2(aq)
nBaO2 ( equation ) nHCl ( equation )
1 nBaO2 ( reality ) 0.009 HCl is resudal 2 nHCl ( reality ) 0.019
BaO2(s) + 2HCl(aq) H2O2(aq) + BaCl2(aq) Initially
0.009
0.019
Reacts
0.009 →
0.018
Resudal
0
→ 0.009
0.001
The mass of hydrogen peroxide should result: 0.009 x 34 = 0.306 g Trang 116
Sáng kiến kinh nghiệm năm học 2018 - 2019
The mass of HCl is left unreacted: 0.001 x 36.5 = 0.0365 g Exercise 2. An ionic compound MX3 is prepared according to the following unbalanced chemical equation. M + X2 MX3 A 0.213g sample of X2 contains 1.806x1021 molecules. The compound MX3 consists of
FF IC IA L
65.54% X by mass.
a) What are the identities of M and X, and what is the correct name for MX 3?
b) Starting with 1.00 g each of M and X2, what mass of MX3 can be prepared? Solution a) *) The number mol contain 1.806x1021 molecules is:
0.213 71 g X2 is Cl2 0.003
3 x35.5 x100% 65.54% M M 56 3 x35.5 M M
N
Ơ
3M X x100% 65.54% 3M X M M
H
N
*) The compound MX3 consists of 54.47% X by mass
O
The molecular mass of X2 is: MX2 =
1.806 x10 21 0.003 mol 6.02 x1023
M is Fe. Thus, MX3 is FeCl3 ( iron(III)chloride)
Y
b) We have the balanced reaction
+
U
2Fe 1 56
Reacts
1 2 x ← 71 3
KÈ
M
Q
Initially
3Cl2
2FeCl3
1 71 1 2 x 71 3
mol
1 2 x x 162.5 = 1.53 g 71 3
D
ẠY
Thus, the mass of MX3 can be prepared is:
1 → 71
Trang 117
Sáng kiến kinh nghiệm năm học 2018 - 2019
3.3.6. Đề số 6 TRƯỜNG THPT NGUYỄN KHUYẾN
ĐỀ THI THỬ LẦN 2 TOÁN VÀ CÁC MÔN KHTN BẰNG TIẾNG ANH NĂM HỌC 2018 - 2019 Môn: Hóahọc (Thờigianlàmbài: 90 phút)
I. PART 1: (7.0 marks)
FF IC IA L
Question 1: The properties that are characteristic of non-metalsare A. dull, brittle, non-conductors.
B. shiny, malleable,non-conductors.
C. dull,brittle, conductors.
D. malleable, ductile,conductors.
Question 2: The atomic number of an atom isthe A. sum of the number of protonsand neutrons. B. number of neutronsonly.
O
C. sum of the number of protons, neutrons,and electrons.
N
D. number of protonsonly.
Ơ
Question 3: An element in Group 15, Period 3 of the periodic table will have how many valenceelectrons? B.15
C.1
H
A.5
D.3
N
Question 4: What happens to non-metal atoms in the formation of ioniccompounds? A. They lose electrons and form negative ions.
Y
B. They lose electrons and form positiveions.
U
C. They gain electrons and form negative ions.
Q
D. They gain electrons and form positive ions. Question 5: The chemical formula for hydrosulphuric acidis
M
A. H2SO3(aq)
B.H2S(aq)
C.HS(aq)
D. H2SO4 (aq)
KÈ
Question 6: The chemical equation representing a simple decomposition reactionis B.2C8H18(l)+25O2(g)→16CO2(g)+18H2O(g)
C.NaOH(aq) + HCl(aq) → NaCl(s) + H2O(l)
D. 2 Mg(s) + O2(g) → 2 MgO(s)
ẠY
A.2 NaCl(s) → 2 Na (s) + Cl2(g)
Question 7: The law of conservation of mass predicts thatthe
D
A. initial mass will be equal to the sum of the masses of the reactants and the sum of the
masses of the products. B. sum of the masses of the reactants will be equal to the sum of the masses of theproducts. C. sum of the masses of the products subtracted from the masses of the reactants will be equal to the initialmass. Trang 118
Sáng kiến kinh nghiệm năm học 2018 - 2019
D. initial mass added to the mass of the reactants will be equal to the sum of the masses of theproducts. Question 8: Some observations were recorded for asubstance. 1. The substance is a white crystalline solid. 2. The substance dissolves in water. A. C6H12O6
B. AlCl3
C.CO2
FF IC IA L
3. A solution of the substance conducts electricity. The substance is mostlikely D. CCl4
Question 9: A chemist wishes to make 200 mL of a 0.600 mol/L solution of KOH
(aq).
What volume of 2.00mol/L stock solution will be required for thisdilution? A.670 mL
C.1.67 ×104mL
B.60.0mL
D. 240 mL
II. 0.50 mol of solute in 2.0 L ofsolution
III. 3.0 mol of solute in 15 Lof solution
IV. 1.0 mol of solute in 3.0 L of solution
The most dilute solutionis B.IV
C.I
D.II
Ơ
A.III
O
I. 0.20 mol of solute in 5.0 Lof solution
N
Question 10: A student prepared four aqueous solutions of an ioniccompound.
H
Question 11: Which pair of aqueous solutions would produce a precipitate whenmixed? C. Na2S (aq) andCr(NO3)3(aq)
N
A. MgCl2(aq) andNa2SO4(aq)
B.KF (aq) and NiBr2(aq) D.KCl(aq) and Mg(NO3)2(aq)
Y
Question 12: The concentration of Cl - available in 110 mL of a solution containing 5.55 g
U
of CaCl2 is
B. 0.00550 mol/L
C.0.909mol/L
D. 0.455mol/L
Q
A.0.668 mol/L
Question 13: The new volume of a fixed mass of gas whose pressure is increased from 100
M
kPa to 400 kPa at a constant temperatureis
KÈ
A.four times theoriginalvolume C. one fourth theoriginalvolume
B. one half the originalvolume D. two times the originalvolume
Question 14: How many moles of oxygen are needed to burn 3.00 moles of butane
ẠY
(C4H10(g)) in a butanelighter?
D
A.19.5
B.2.15
C.6.52
D. 13.0
Question 15: Hydrofluoric acid, HF(aq), is not stored in glass containers, SiO2(s), because it reacts with glass.The products of the reaction are SiF4(aq) and water. Calculate the mass of HF(aq) that is needed to react completely with 60.0 g of SiO2(s) A.89.5 g
B.79.9g
C.5.00 g
D. 20.0g
Question 16: A remedy for an upset stomach is produced when a tablet is dissolved in water. The balanced chemical equationis Trang 119
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C6H8O7 (aq) + 3 NaHCO3 (aq) → Na3C6H5O7 (aq) + 3 CO2 (g) + 3 H2O (l) What volume of CO2(g) at STP conditions would result if a tablet containing 16 g of C6H8O7(aq) was used? A.6.8L
B.11L
C.5.6L
D. 1.9L
Question 17: Which one of the following bonds would be described as non-polar? B. C ─ C
C. N ─ O
D. C ─ Cl
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A. H ─ N
Question 18: Inatitration a 20.mL sample of NaOH(aq) was neutralized by 14.9mL of 0.13 mol/L H2SO4(aq).The concentration of the base is A.0.35 mol/L
B.0.048mol/L
C.8.7mol/L
D. 0.19mol/L
Question 19: A solution of sugar in water has a density of 1.05 g/cm3. If you have 75.0 mL of the solution, and if the solution is 8.10% sugar by mass, how many grams of sugar are A.63.8 g
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there in thesolution? B.6.38g
C.60.8 g
D. 6.08 g
B. 922.86
C. 47.46
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A. 461.43
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Question 20: The number of grams in six moles of liquid carbon tetrachloride is D. 153.81
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Question 21: Sulfur is an element that forms a wide range of compounds with oxygen and
A. Sulfur dioxide, SO2
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contain the larger mass of sulfur?
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other elements. In one kilogram of each of the following compounds, which one would
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C. Ammonium persulfate, (NH4)2S2O8
B. Sulfuric acid, H2SO4 D. Sodium trithionate, Na2S3O6
of air is
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Question 22: The gas that could appropriately be collected by the downward displacement B. nitrogen (IV) oxide (NO2)
C. propane (C3H8)
D. hydrogen (H2)
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A. arsine (AsH3)
Question 23: If 2.00 ml of a 0.100 M HCl solution is diluted to 200.0 ml by the addition of pure water, its pH will now be
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A. 3.00
B. 2.00
C. 1.00
D. 0.00100
D
Question 24: In which of the following species is nitrogen in its highest oxidation state? A. NO3-
B. NH4+
C. NH3
D. NO2
Question 25: Which one of the following is the CORRECT semi-structural formula of 2,3dimethylpentane? A. (CH3)2CHCH2CH2CH2CH3
B.CH3C(CH3)2CH2CH2CH3
C.CH3CH(CH3)CH(CH3)CH2CH3
D. CH3CH(CH3)CH(CH3)CH2CH2CH3 Trang 120
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Question 26: Which one of the following electronic configurations represents the uncharged atoms of an element with a maximum oxidation state of +5? A. 1s22s22p5
B. 1s22s22p63s33p1
C. 1s22s22p63s23p3
D. 1s22s22p63s23p63d74s2
NH3? A. 3.30 x 10-3
C. 1.99 x 1021
B. 0.225
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Question 27: How many ammonia molecules are present in 0.0562 g of pure ammonia, D. 7.94 x 1021
Question 28: An ion that has 9 protons, 11 neutrons and 10 electrons would have a net charge of A. +1
B. +2
C. -1
D. -2
Question 29: A certain sulfate has the empirical fomula XSO4, where X represents an
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unknown Group 2 metal. A pure sample of this sulfate is analysed and found to contain 23.55 % by mass of sulfur. Which Group 2 metal does X represent? B. Calcium
C. Strontium
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A. Magnesium
D. Barium
Heat needed (J) = mass of water (g) x 4,2 x temperature
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calculated using the formula:
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Question 30: The amount of energy, in joules, needed to heat a given mass of water can be
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change (oC)
The amount of heat energy released when 1 g of butane burns is 49518 joules. What mass
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of butane would need to be burnt to raisc the temperature of 500 ml (500 g) of water from
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20oC to 100oC?
B. 3,4 g
C. 4,2 g
D. 336 g
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A. 0,85 g
Question 31: Why is water classified as a chemical compound?
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A. It exists on Earth as a solid, liquid, and gas.
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B. It contains hydrogen and oxygen. C. It contains two different elements joined by chemical bonds.
D. It has a higher boiling point than hydrogen or oxygen.
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Question 32: Why is sodium metal a stronger reducing agent than copper metal?
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A. Na atoms only need to lose 1 electron while Cu atoms need to lose 2 to achieve a more
stable electronic configuration. B. Uncharged Na atoms only have 3 occupied electron shells while uncharged Cu atoms have 4 occupied electron shells. C. The attraction between the outermost electron and the nucleus is far weaker in Na atoms than in Cu atoms. D. Na metal is softer and has a lower melting point than Cu metal. Trang 121
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Question 33: Zinc is important to human health because it is an essential trace element that is found in every tissue in the body. Among foods richest in zinc are liver, eggs, and shellfish. Zinc levels in foods are often quoted in parts per million (ppm), which means 1 g in every 1 000 000 g. Some oysters were found to contain 4 mg of zinc per 100 g. A these oysters? A. 4 ppm
B. 40 ppm
C. 400 ppm
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milligram (mg) is one-thousandth of a gram. What is the concentration, in ppm, of zinc in D. 4000 ppm
Question 34:According to the figure to the right, what is the most volatile substance shown? A. benzene B. water
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C. toluene
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N
D. aniline
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Question 35: In an experiment, some hydrochloric acid was added to solid calcium carbonate, The reaction produced carbon dioxide gas that was passed through a clear
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limewater (calcium hydroxide solution). The limewater turned milky as the carbon dioxide
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reacted with the calcium hydroxide forming a white precipitate of calcium carbonate. As
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more carbon dioxide gas was passed into the limewater, it went clear again. What is the most likely explanation for this observation? Carbon dioxide dissolving in the limewater B. forms calcium hydroxide.
C. forms calcium carbonate.
D. turns the solution milky.
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A. turns the solution acidic. PART 2: (3.0 marks)
Question 1: Write a balancedequation for the formation of magnesiumoxide by reaction of
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magnesiumwith a. Oxygen
b. Carbondioxide
Solution : a)
heat 2MgO(s) 2Mg(s) + O2(g)
heat MgO(s) + C(s) b) Mg(s) + CO2(s)
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Question 2: Theconcentration of a solution can be expressed as the mass of solute per liter of solution. Ashwyn dissolved some solid copper sulface in water to make 500 mL of solution. The solution has a copper sulfate concentration of 28 g/L. a. If 100 mL of this solution were evaporated to dryness, what mass of copper sulfate would be recovered?
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b. What volume of Ashwyn’s original solution would contain 2.1 g of copper sulfate?
c. The concentration of another salt solution is 72 g/L. How much water must be added to 250 mL of this solution to change its concentration to 18 g/L? Solution: a) The mass of copper sulfate would be recovered
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28 x100 2.8 grams 1000
mCuSO4 =
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2.1 x1000 75mL 28
72 x 250 18 grams 1000
H
VAshwyn =
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b) The volume of Ashwyn’s original solution would contain 2.1 g of copper sulfate:
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c) The mass of salt in 250mL original solution is:
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Volume of the solution is obtained after dilution is:
18 x1000 1000mL 18
1000 -250 = 750 mL
D
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Q
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→ The volume of water must be added to 250 mL of original solution:
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PHẦN III: HIỆU QUẢ DO SÁNG KIẾN ĐEM LẠI I. So sánh và đối chứng. Từ khi Sở GD-ĐT Nam Định tổ chức hội thi: “ Giải Toán và các môn khoa học bằng tiếng Anh” vào các năm học 2016-2017; 2017-2018; 2018-2019 tôi đều được nhà trường phân công giảng dạy, bồi dưỡng học sinh ở bộ môn Hóa học. Trong năm học
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2016-2017, đề thi là sự tổ hợp của nhiều môn: Toán; Vật lí; Hóa học. Từ năm 2017-2018, ban tổ chức đã tách riêng từng môn nên dấu ấn của giáo viên trong từng bộ môn được thể hiện rõ nét hơn.
Năm học 2017-2018, kết quả bộ môn Hóa đạt được là: 2 giải nhì; 2 giải ba và 1 giải khuyến khích
Năm học 2018-2018, sau khi đã có những rút kinh nghiệm, bổ sung trong giáo án và
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phương pháp tiếp cận thì kết quả đội tuyển môn Hóa học do tôi bồi dưỡng đã đạt được những kết quả khởi sắc hơn, với
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01 giải nhất: Em Trần Thị Ngọc Anh- lớp 11A3 đạt 9,8 điểm ( Đứng số 1 trong tổng số các
Ơ
em dự thi)
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01 giải nhì: Em Nguyễn Huy Hiếu – lớp 11A1 đạt 9,2 điểm
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01 giải ba: Em Đào Trọng Bách – lớp 11A3 đạt 8,5 điểm 02 giải khuyến khích: Em Nguyễn Mạnh Cường – lớp 11A3
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Em Trần Hữu Hiến - lớp 11A1
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Như vậy, với việc lựa chọn nội dung, phương pháp, cách tiếp cận hợp lí và sự rút kinh
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nghiệm, bổ sung qua từng năm tham gia bồi dưỡng tôi đã cùng với các em học sinh đạt được các kết quả ngày càng tiến bộ. Vì vậy tôi mạnh dạn trình bày kinh nghiệm bản thân
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qua sáng kiến này, với mong muốn có thể giúp các thầy cô có thêm hướng tiếp cận và dạy
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học có hiệu quả hơn khi tham gia bồi dưỡng Giải Toán và các môn khoa học bằng tiếng Anh trong những năm học sau.
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II. Hiệu quả do sáng kiến đem lại 1. Hiệu quả kinh tế - Do đây là sáng kiến về mặt khoa học giáo dục, được áp dụng trong quá trình giảng
dạy ở nhà trường nên không tính được hiệu quả về mặt kinh tế. 2. Hiệu quả về mặt xã hội - Các nước đang phát triển nói chung, Việt Nam nói riêng trong giai đoạn mà hội nhập quốc tế ngày càng trở nên sâu rộng càng yêu cầu cao hơn về khả năng sử dụng ngoại ngữ, trong đó đặc biệt là tiếng Anh. Việc giảng dạy các chuyên ngành bằng tiếng Anh tại các trường đại học tại Việt nam đã được triển khai và đạt được những Trang 124
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kết quả hết sức tích cực. Xu thế tất yếu trong bối cảnh đất nước đang phát triển và hòa nhập là tiến đến giảng dạy các môn khoa học bằng tiếng Anh tại các trường chuyên, trường chất lượng cao THPT. - Một trong những điều kiện quan trọng và quyết định đến thành công của việc triển khai giảng dạy các môn khoa học bằng tiếng Anh tại các trường THPT là
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ngoài trình độ tiếng Anh của giáo viên, trình độ tiếng Anh của học sinh thì giáo trình, tài liệu, các phương tiện hỗ trợ cũng như cách khai thác kiến thức trong các tài liệu nước ngoài là rất quan trọng.
- Với SKKN trên, mỗi giáo viên có thể dùng làm cơ sở để xây dựng nên hệ thống bài giảng, bài tập cho riêng mình sao cho phù hợp với trình độ của học sinh, qua đó học sinh vừa tiếp thu kiến thức một cách chủ động, và có thể tự khai thác thêm trên internet.
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- Trong quá trình giảng dạy và viết SKKN này mục đích cung cấp cho giáo viên cách tiếp cận, khai thác tài liệu bằng tiếng Anh, sử dụng các tài liệu để xây dựng và tiến hành bài
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giảng bằng tiếng Anh theo các mức độ khác nhau qua các ví dụ cụ thể. Tài liệu cũng sẽ đưa
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giảng môn Hóa học bằng tiếng Anh
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ra một số kinh nghiệm, kĩ năng trình bày hỗ trợ cho giáo viên nâng cao hiệu quả của giờ
N
- Cũng với cách làm này, các học sinh đã say mê hơn trong việc học tập, sự sáng tạo trong kiến thức làm các em cảm thấy hứng thú hơn và có nhiều quyết tâm hơn trong việc
Y
chiếm lĩnh tri thức nhân loại, nhất là tri thức về khoa học tự nhiên.
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IV. Cam kết không sao chép hoặc vi phạm bản quyền
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Tôi xin cam đoan đây là sáng kiến kinh nghiệm của tôi làm và viết, không sao chép
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nội dung của người khác hoặc vi phạm bản quyền. Nam Định, tháng 05 năm 2019 Tác giả sáng kiến
Phạm Thị Dung
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CƠ QUAN ĐƠN VỊ ÁP DỤNG SÁNG KIẾN ( Xác nhận, đánh giá, xếp loại) ...................................................................................................................................................
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................................................................................................................................................... ................................................................................................................................................... ...................................................................................................................................................
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SỞ GIÁO DỤC – ĐÀO TẠO
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( Xác nhận, đánh giá, xếp loại)
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...................................................................................................................................................
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................................................................................................................................................... ...................................................................................................................................................
Y
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TÀI LIỆU THAM KHẢO 1. Hóa học song ngữ Việt - Anh lớp 10; lớp 11: Nguyễn Xuân Trường ( Chủ biên), Phạm Văn Hoan; Từ Vọng Nghi; Đỗ Đình Rãng; Nguyễn Phú Tuấn- Nhà xuất bản Giáo
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Dục
2. Giáo trình PHƯƠNG PHÁP DẠY HỌC HÓA HỌC BẰNG TIẾNG ANH Ở TRƯỜNG TRUNG HỌC PHỔ THÔNG : Cao Cự Giác ( Tổng chủ biên); Trần Trung Ninh – Nhà xuất bản Đại học Vinh
3. Complete Chemistry for Cambridge IGCSE (Endorsed by CAMBRIDGE international Examinations)
Cambridge-igcse: Chemistry – Third Edition (Endorsed by CAMBRIDGE
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4.
international Examinations)
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Studying the Sciences Chemistry Grades 10 – 12
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5. The Free High School Science Texts: Textbooks for High School Students
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U
Y
N
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6. Chemistry Seventh Edition- Steven S. Zumdahl University of Illinois
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