CP Chemistry: Review packet for Midterm Matching
a. matter b. solid ____
1. definite shape and definite volume
____
2. anything that has mass and takes up space
____
3. neither a definite shape nor volume
____
4. definite volume, takes the shape of its container
a. accuracy
c. liquid d. gas
b. precision
____
5. the closeness of a measurement to the true value of what is being measured.
____
6. the reproducibility, under the same conditions, of a measurement.
a. proton b. neutron c. electron
d. nucleus e. period f. group/family
____
7. subatomic particle with no charge
____
8. central portion of an atom, composed of protons and neutrons
____
9. positively charged subatomic particle
____ 10. negatively charged subatomic particle ____ 11. the vertical columns in the periodic table ____ 12. the horizontal row of blocks in the periodic table
a. John Dalton b. JJ Thomson, cathode ray tube
c. Rutherford, gold foil experiment d. Mendeleev
____ 13. led to the discovery of the electron. ____ 14. proposed an atomic theory based on scientific knowledge. ____ 15. led to the discovery of the nucleus. ____ 16. developed the first successful periodic table.
a. b. c. d. e.
Group 1 Group 2 Group 3-12 Group 13 Group 14
f. g. h. i.
Group 15 Group 16 Group 17 Group 18
____ 17. Oxygen family ____ 18. Alkaline Earth metals ____ 19. Nitrogen family ____ 20. Boron family ____ 21. Alkali metals ____ 22. Transition metals ____ 23. Carbon family ____ 24. Noble Gas family ____ 25. Halogens
a. (aq) b. (s)
d. (g) e. Δ
c. (l) ____ 26. solid ____ 27. dissolved in water ____ 28. heat is added to the reaction ____ 29. liquid ____ 30. gas
a. A + B → AB b. AB → A + B
d. AB + CD → AD + CB e. CH4 + 2O2 → CO2 + 2H2O
c. A + BX → B + AX ____ 31. decomposition ____ 32. single- replacement ____ 33. combustion ____ 34. double-replacement ____ 35. combination
a. wavelength b. speed of light
c. amplitude d. frequency
____ 36. wave’s height from the origin to the crest ____ 37. the distance between two succesive crests on a wave ____ 38. 3.0 x 108 m/s ____ 39. the number of wave cycles to pass a given point per unit time
a. Pauli exclusion principle b. Aufbau principle
c. Hund’s rule
____ 40. an electron occupies the lowest available energy level ____ 41. a maximum of two electrons can occupy each orbital and these electrons must have opposite spin ____ 42. when orbitals of identical energy are available, electrons enter these orbitals singly before any spin pairing takes place
a. atomic radius b. ionization energy
c. electronegativity
____ 43. the energy required to remove an electron from an atom ____ 44. the tendency of an atom to attract electrons to itself when chemically bonded with another element ____ 45. one half of the distance between the nuclei of two like atoms in a diatomic molecule Completion Complete each statement. 46. Determine if the following describe a physical or a chemical property? a) freezing point
________________
c) reactivity ____________________
b) density _________________ d) color __________________
47. Decide if the following statements describe a physical or a chemical change. a) water freezes ____________________
b) silver oxidizes ___________________
c) food grows mold _________________
d) metal is bent ____________________
48. Decide if the following are pure substances (element or compound), heterogeneous mixtures or homogeneous mixtures. a) hydrochloric acid ____________________
b) salt water _____________________
c) vinegar (10% acetic acid) ________________ d) trail mix ____________________
49. Decide if the statement is qualitative or quantitative. a) The freezing point of water is 32°F. _________________________________ b) The liquid is blue in color. _________________________________________
Problem 50. A student measures a temperature as 86°C, whereas the correct temperature is 84°C. What is the percent error?
51. What is the density of 26 g of matter whose volume is 5.3 cm3?
52. A temperature of 450K is __________°C. 53. a) Convert 56 L (liters) to mL (milliliters).
________________
b) Convert 87000 g (grams) to kg (kilograms). ____________________ 54. Convert 180 lbs to kg. (2.2 lbs = 1 kg).
55. The average atomic mass of an element is calculated by multiplying the masses of its isotopes by each isotope’s (circle one-- radioactivity, atomic number, percent (%) abundance or mass number). Other 56. How many significant figures are in the following measurements? a) 2402.5 _____
b) 0.00300 ______
c) 4200 ______
57. Express the following measurements in scientific notation. a) 425,000,000 ____________________
b) 0.000035 ____________________
58. Decide if the following equalities are correct or incorrect. a) 1000 g = 1 kg _________________ b) 1 m = 10 cm __________________ c) 1cm3 = 1mL __________________ d) 1m = 1000 mm ________________ 59. Decide if the following statements about the nucleus are true or false. a) The nucleus is composed of electrons and protons. ________________ b) The nucleus is positively charged.
__________________
c) The nucleus contains most of the volume of the atom. ________________ d) The nucleus is very dense. __________________
60. Isotopes of an element contain the same number of _____________, but a different number of ________________. 61. Decide if the following elements are metals, metalloids or nonmetals. a) Helium ______________
b) Arsenic ____________
c) Calcium ____________
62. a) Which group on the periodic table has the lowest reactivity? ________________ b) Which group on the periodic table has the highest reactivity? ________________ 63. When an electron is removed from an atom which forms: a cation or an anion? 64. How many total electrons does an oxide ion (O2-) have? ___________ 65. Ionic compounds are composed of a metal and a ___________________; molecular/covalent compounds are composed of two ________________________.
66. Give the formula for the following compounds and indicate whether they are ionic or molecular/covalent. a) Calcium chloride ____________________________________________ b) Diphosphorous pentoxide ______________________________________ c) Iron (II) bromide ____________________________________________
67. Determine if the following compounds are ionic or molecular/covalent and give their correct name. a) SF2 ____________________________________________ b) Li2O ___________________________________________ c) Fe2O3 __________________________________________
68. How many atoms are present in one formula unit of the compound Ca3(PO4)2? ______ 69. What are the 7 diatomic molecules? _______________________________________________ 70. Molecules are composed of (circle one-- atoms / formula units), while ionic compounds are made up of (atoms / formula units). 71. Name the following ions: a) N3- ___________________
b) NO3- ____________________
72. Identify the charge for iron in the following compounds. a) FeCl3 ________________
b) FeO _______________
73. Convert 6.5 moles of lithium (Li) to grams.
74. Convert 36.0 grams of carbon to moles.
75. There are ________ oxygen atoms in 20 molecules of CO2. 76. How many moles are in 150.0 grams of potassium hydroxide (KOH)?
b 77. There are ______________ molecules of methane (CH4) in 0.123 moles.
b 78. What is the molar mass of calcium phosphate, Ca3(PO4)2? b 79. What is Avogadro’s number? ______________________ 80. The molar mass of an element is the mass of one __________ of the element. 81. Calculate the percentage composition of ammonium chloride, NH4Cl.
% N = ___________
% H = _____________ % Cl = _______________
82. What is the empirical formula of a compound that is 67.6% Hg, 10.8% S, and 21.6% O.
83. Give the empirical formula for the following compounds. a) C4H10
___________________
b) C6H8O6 ___________________
84. Balance the following equations: a) ____ Au + ____ O2 → ____ Au2O3 b) ____ KI → ____ K + ____ I2 c) ____ Cu + ____ Ag(NO3) → ____ Ag + ____ Cu(NO3)2
85. Label the following chemical compounds as either a reactant or a product in a combustion reaction. a) H2O ________________________ b) C3H6 _________________________ c) O2 _________________________ d) CO2 __________________________
86. What is the equation for the speed of light?
___________________________
87. Is the relationship between wavelength (λ) and frequency (ν) inverse or direct? _______________ 88. The units for frequency (ν) are ________________. 89. a) Give the electron configuration for Phosphorous. ___________________________________ b) Give the noble gas configuration for Aluminum. ___________________________________
90. Periodic law states that the physical and chemical properties of elements are periodic, or repeating functions of their atomic ________________.
91. Fill in the following blanks (*think about the hint elements that we used for each trend) a) Electronegativity tends to _____________ down a group/family and _______________ across a period. b) Atomic radius tends to ______________ down a group/family and ________________ across a period. c) Ionization energy tends to ______________ down a group/family and _______________ across a period.
Review for Midterm Answer Section MATCHING 1. 2. 3. 4.
ANS: ANS: ANS: ANS:
B A D C
5. ANS: A 6. ANS: B
PTS: PTS: PTS: PTS:
1 1 1 1
PTS: 1 PTS: 1
7. 8. 9. 10. 11. 12.
ANS: ANS: ANS: ANS: ANS: ANS:
B D A C F E
PTS: PTS: PTS: PTS: PTS: PTS:
1 1 1 1 1 1
13. 14. 15. 16.
ANS: ANS: ANS: ANS:
B A C D
PTS: PTS: PTS: PTS:
1 1 1 1
17. 18. 19. 20. 21. 22. 23. 24. 25.
ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS: ANS:
G B F D A C E I H
PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS: PTS:
1 1 1 1 1 1 1 1 1
26. 27. 28. 29. 30.
ANS: ANS: ANS: ANS: ANS:
B A E C D
PTS: PTS: PTS: PTS: PTS:
1 1 1 1 1
31. 32. 33. 34. 35.
ANS: ANS: ANS: ANS: ANS:
B C E D A
PTS: PTS: PTS: PTS: PTS:
1 1 1 1 1
36. 37. 38. 39.
ANS: ANS: ANS: ANS:
C A B D
PTS: PTS: PTS: PTS:
1 1 1 1
40. ANS: B 41. ANS: A 42. ANS: C
PTS: 1 PTS: 1 PTS: 1
43. ANS: B 44. ANS: C 45. ANS: A
PTS: 1 PTS: 1 PTS: 1
COMPLETION 46. ANS: a) physical
b) physical
c) chemical
d) physical
PTS: 1 47. ANS: a) physical
b) chemical
c) chemical
d) physical
PTS: 1 48. ANS: a) pure
b) homogeneous
PTS: 1 49. ANS: a) quantitative b) qualitative PTS: 1 PROBLEM 50. ANS: 2.38% PTS: 1 51. ANS: 4.91 g/cm3 PTS: 1 52. ANS: 177 PTS: 1 53. ANS:
c) homogeneous
d) heterogeneous
a) 56000 mL
b) 87 kg
PTS: 1 54. ANS: 81.8 kg PTS: 1 55. ANS: percent (%) abundance PTS: 1 OTHER 56. ANS: a) 5 b) 3
c) 2
PTS: 1 57. ANS: a) 4.25 x 108
b) 3.5 x 10-5
PTS: 1 58. ANS: a) correct
b) incorrect
PTS: 1 59. ANS: a) False, protons and neutrons
c) correct
b) True
d) correct
c) False; contains mass
d) True
PTS: 1 60. ANS: protons(same), neutrons(different) PTS: 1 61. ANS: a) nonmetal
b) metalloid
c) metal
PTS: 1 62. ANS: a) lowest = Group 18 (Noble Gas family)
b) highest = Group 1 (Alkali metals)
PTS: 1 63. ANS: cation PTS: 1 64. ANS: 10 electrons (O atom has 8 electrons, but O2- ion has 10)
PTS: 1 65. ANS: non-metal; non-metals PTS: 1 66. ANS: a) CaCl2 ionic; P2O5 molecular/covalent; FeBr2 ionic PTS: 1 67. ANS: a) molecular/covalent -- sulfur dioxide; ionic -- lithium oxide; ionic -- iron(III) oxide PTS: 1 68. ANS: 13 atoms total (3 Ca, 2 P, 8 O) PTS: 1 69. ANS: Bromine, Iodine, Nitrogen, Chlorine, Hydrogen, Oxygen, Fluorine PTS: 1 70. ANS: molecules = atoms; ionic compounds = formula units PTS: 1 71. ANS: a) nitride ion
b) nitrate ion (polyatomic)
PTS: 1 72. ANS: a) +3
b) +2
PTS: 1 73. ANS: 4.51 g Li PTS: 1 74. ANS: 3 moles PTS: 1 75. ANS: 40 oxygen atoms PTS: 1 76. ANS: 2.67 moles KOH PTS: 1 77. ANS:
7.40 x 1022 molecules PTS: 1 78. ANS: 310.3 g/mol PTS: 1 79. ANS: 6.0 x 1023 PTS: 1 80. ANS: mole PTS: 1 81. ANS: N= 26.19 %
H= 7.48%
Cl= 66.32%
PTS: 1 82. ANS: HgSO4 PTS: 1 83. ANS: a) C2H5
b) C3H4O3
PTS: 1 84. ANS: a) 4, 3, 2
b) 2, 2, 1
c) 1, 2, 1, 2
PTS: 1 85. ANS: a) product
b) reactant
c) reactant
d) product
PTS: 1 86. ANS: c(speed of light) = 位(wavelength) x 谓(frequency) PTS: 1 87. ANS: inverse; as one increases, the other must decrease PTS: 1 88. ANS: hertz or s-1 PTS: 1 89. ANS: a) 1s22s22p63s23p3
b) [Ne]3s23p1
PTS: 1 90. ANS: numbers PTS: 1 91. ANS: a) decrease down a group, increase across a period b) increase down a group, decrease across a period c) decrease down a group, increase across a period PTS: 1