0 welcome to chemistry

welcome to accelerated chemistry!

1

2

+1

2 valence electrons

Group 1

hydrogen 1.008 (H is a nonmetal)

2s

3

Li

Group 2

4

11

12

sodium

5s

K potassium 39.10

55

132.91

7s

Fr

La

francium 223.02

Ra

6d

radium 226.03

atomic number

Ac

44.96 metal metalloid

name average atomic mass (amu) nonmetal

5f

Rf

92.91

Ta

90

Th

thorium 232.04

42

Mo

manganese 54.94

Tc

43

Re

Os

osmium

Sg

186.21 107

seaborgium 171.13

45

Rh

Pr

60

Nd

61

140.91

144.24

U

92

190.20

Bh

Pm

protactinium

231.04

uranium 238.03

(144.91) 93

Ir

Np

Hs

62

Sm

carbon

46

zinc 65.37 48

Ag

palladium

silver

106.40

Cd

cadmium

107.87 79

Pt

platinum

Au gold

195.09

Hg

mercury

196.97

95

Am

americium (243.06)

Ds

281.17 64

65

Gd

Cm

112

(281.16)

gadolinium 157.25 96

Rg

Cn

(285.18)

Tb

Dy

terbium 158.92

dysprosium 162.50

97

4p

gallium 69.72 49

5p

Bk

98

Cf

curium berkelium californium (247.07) (247.07) (251.08)

Ge

32

6p

Tl

Pb

thallium

lead

204.37 113

7p 67

Nh

holmium 164.93 99

207.19 114

Es

einsteinium (252.08)

68

Er

erbium 167.26 100

Mo

flerovium Moscovium (289.19) 289.19)

Fm

fermium (257.10)

Tm

69

thulium 168.93 101

Md

mendelevium (258.10)

70

Po

I

No

71

Kr

36

krypton 83.80

Xe

54

xenon

At

131.30 86

astatine

Ts

Rn radon

(210)

livermorium tennessium (293.20) (294.21)

Yb

argon 39.95

126.90 85

117

Lv

Ar

18

iodine

(210)

ytterbium 173.04 102

53

polonium 116

neon

bromine 79.91

127.60

208.98 115

Fl

nihonium (286.19)

Ho

Bi bismuth

Br

35

tellurium 84

Ne 20.18

chlorine 35.45

Te

121.75 83

Cl

17

selenium 78.96 52

10

19.00

Se

34

Antimony)

118.69 82

F

He helium 4.00

Group 17

sulfur 32.07

As

2

fluorine

S

16

Sb

tin

114.82 81

O

phosphorus 30.97

Sn

indium

9

16.00

germanium arsenic 72.59 74.92 50 51

In

-2 8

oxygen

P

33

-1

halogens

14.01 15

silicon 28.09

Ga

31

200.59

darmstadtium roentgenium copernicium

Eu

111

aluminum 26.98

112.40 80

meitnerium 278.16

europium 151.96

neptunium plutonium (237.05) (244.06)

47

Zn

110

63

Pu

copper 63.55

Pd

78

Cu

Si

14

N

Group 18

7

Group 16

nitrogen

12.01

Al

13

group 12

30

109

Mt

samarium 150.41 94

Ni

192.22

hassium 277.15

group 11

29

nickel 58.71

iridium

108

bohrium 270.13

group 10

28

cobalt 58.93

Ru

rhenium

183.85

Db

Pa

Co

27

iron 55.85 44

praseodymium neodymium promethium

91

group 9

Fe

W

106

dubnium 268.13) 59

Mn

group 8

26

tungsten

180.95 105

group 7

25

molybdenum technetium ruthenium rhodium 95.94 96.91 101.07 102.91 74 75 76 77

tantalum

267.12

cerium 140.12

Cr

chromium 52.00

Nb

73

rutherfordium

Ce

V

niobium

178.49 104

4f

manmade

scandium

Hf

58

solid liquid gas

41

hafnium

actinium 227.03

symbol:

Sc

72

group 6

24

vanadium 50.94

zirconium

138.91 89

Zr

group 5

23

91.22

lanthanum

137.33 88

Ti

titanium 47.90

yttrium

5d

barium

group 4

22

40

Y

88.91 57

Ba

cesium 87

4d

87.62

Sc

scandium 44.96 39

Sr

56

Cs

6s

3d

strontium

rubidium 85.47

group 3

21

calcium 40.08 38

Rb

37

Ca

20

3p

transition metals:

magnesium 24.31

22.99

4s

boron

Group 15

7

C

10.81

Mg

-3

Group 14

6

B

2p

9.012

Na

19

Group 13

beryllium

6.94

+3

0

noble gases

8

valence electrons: 4 5 6

3

5

Be

lithium

3s

metal

1s

alkaline earth metals

H

1

accelerated chemistry 2017-2018

+2

alkali metals

nonmetal

1 valence electron

(220) 118

Og

oganesson (294.21)

Lu

lutetium 174.97 103

Lr

nobelium lawrencium (259.10) 262.11

common ions acetate CH3CO2-

bisulfite HSO3-

chlorite ClO2-

hydroxide OH-

nitrite NO2-

phosphide P3-

ammonium NH4+

bromide Br-

chromate CrO42-

hypochlorite ClO-

oxide O2-

sulfate SO42-

bromide Br-

carbonate CO32-

cyanide CN-

iodide I-

perchlorate ClO4-

sulfide S2-

bicarbonate HCO3-

chlorate ClO3-

dichromate Cr2O72-

nitrate NO3-

permanganate MnO4-

sulfite SO32-

bisulfate HSO4-

chloride Cl-

fluoride F-

nitride N3-

phosphate PO43-

thiosulfate S2O32-

3

chemistry equations 1. introduction to chemistry d = density; m = mass in g; v = volume in mL

m d= V

9. the mole:

is an amount! = 6.02 x 1023

mol-mol conversions:

mol B  mol B mol A mol A mol B gA x x =mol B gA mol A mol A x

gram – mol conversions: mol – g conversions:

mol A x

g– g conversions:

Boyles:

Charles:

actual yield % yield= x 100 theoretical yield error % error= x 100 accepted valued 5 oC = oF −32 x 9

K = OC + 273.15 9o oF = C + 32 5

3. matter, 4. atom: no formulas 5. electrons s = wf

gB mol A mol B x x  gB gA mol A mol B

10. gas laws

P1V1  P2V2

2. data

temperature:

gA x

gB mol B x gB mol A mol B

e = hf

s = the speed of light = 3 x 108 m/s w = wavelength in meters f = frequency, per second. e = energy in joules

h = Plancks constant = 6.626 x 10-34 j sec

Balmer formula : 1 w nm  1   1 0.01097    2 outer 2   inner w = wavelength in nanometers inner = inner shell # outer = outer shell #.

6. periodic table; 7. bonding 8. reactions: no formulas ☺

T1 T2  V1 V2

P = pressure: 1 atm =14.7 psi = 760 mm Hg = 101.3 kPa

Gay-Lussac:

V = volume (L) T = Kelvin Temp (K) n = # of moles (mol) R = 0.0821 L atm/mol K M = molar masses (g/mol)

T1 T2  P1 P2

combined: P1V1 P2V2  T1 T2 ideal gas law:

STP = standard temp and pressure = 1 atm, 273.15 K

PV  nRT

Avogadro’s principle: 22.4 L = 1 mole gas at STP Graham’s law: rate1 = rate2

M2 M1

M = molar mass

11. energy: q = mcDT q = heat, m = mass, c = specific heat (J/gOC), DT = temp change in oC. energy needed to cwater(l) = 4.184 J/g oC melt and boil water: cwater(s) = 2.03 J/goC DH fus water = 334 J/g cwater(g) = 2.01 J/goC DHvap water = 2260 DHvap water = 2260 J/g; DHfus waterJ/g = 334 J/g water boils/condenses at 100oC water melts/freezes at 0oC 1 Nutritional Calorie = 4184 Joules = 4 BTU = 1000 calories = 0.0016 kilowatt hours DG = DH-TDS DG = change in free energy DH = change in enthalpy T = temperature DS = change in entropy 15. acids and bases pH = -log[H+] Ka for example of HCl 10-pH = [H+] = [H+][Cl-]/[HCl] pOH = -log[OH-] Kw = [H+][OH-] = 10-14 10-pOH = [OH-] titration: pH + pOH = 14 molarity unknown  (volume

standard)(molarity volume unknown

14. equilibrium

for:

aA + bB Keq =

cC + dD [C]c[D]d [A]a[B]b

omit liquids and solids

)

standard

13. rates reaction rate = Dconcentration/Dtime collision theory: For 2 molecules to react, they must collide, and with enough force, and in the right locations on the molecules for the reaction to occur.

M = Molarity = moles per liter = moles/liter

12. solutions 1. percent concentration by volume (%v/v) = volume of solute x 100 volume of solution 2. percent concentration by mass (%m/m) = mass of solute x 100 mass of solution 3. Molarity (M) = moles of solute Liters of solution 4. molality (m) = moles of solute Kilograms of solvent 5. mole fraction (X) = moles of solute moles of solution 6. concentration and dilution 6. C1V1 = C2V2 where C1 and C2 are concentrations; and V1 and V2 are volumes 7. Henry’s Law: Solubility is proportional to Pressure S1/P1 = S2/P2 8. pressure and volume units units: 1 atm = 760 mm Hg = 14.7 psi = 101.3 KPa 1 L = 1000 mL 9. boiling point elevation (DTb ) and freezing point depression (DTf) of solutions DTf = Kfm . pm DTb = kbm . pm DTf = change in freezing temp; DTb = change in boiling temperature; Kf = freezing point constant; Kb = boiling point constant; m = molality; pm = particle molality (ion count) (Kf is for the solvent; pm is for the solute)

4

Name (include the first name you’d like to be called in class)___________________________________ Period______

day 1 survey

please always include the period; it helps me keep things in the right folders

welcome to chemistry! please fill out the survey below to get started.

1. What science course did you take last year? Course ___________________Teacher________________ 2. What did you think of the course and/or the teacher?

aristolochic acid

3. What do you think of science?

4. How hard a worker are you?

5. What do you plan to do after high school?

6. Please let me know the names of any brothers or sisters you had that took my course.

8. Tell me a little bit about yourself. Long answers are welcome â˜ş

5

Dr Brielmann

Guilford High School

Student Safety Contract Science is a hands-on laboratory class. However, science activities may have potential hazards.

We will use some equipment and animals that may be dangerous if not handled properly. Safety in the science classroom is an important part of the scientific process. To ensure a safe classroom, a list of rules has been developed and is called the Science Safety Contract. These rules must be followed at all times. Additional safety instructions will be given for each activity. No science student will be allowed to participate in science activities until this contract has been signed by both the student and a parent or guardian.

SAFETY RULES 1. Conduct yourself in a responsible manner at all times in the science room. Horseplay, practical jokes, and pranks will not be tolerated.

2. Follow all written and verbal instructions carefully. Ask your teacher questions if you do not understand the instructions.

3. Do not touch any equipment, supplies, animals, or other materials in the science room without permission from the teacher.

4. Perform only authorized and approved experiments. Do not conduct any experiments when the teacher is out of the room.

5. Never eat, drink, chew gum, or taste anything in the science room.

6. Keep hands away from face, eyes, and mouth while using science materials or when working with either chemicals or animals. Wash your hands with soap and water before leaving the science room.

7. Wear safety glasses or goggles when instructed. Never remove safety glasses or goggles during an experiment. There will be no exceptions to this rule!

8. Keep your work area and the science room neat and clean. Bring only your laboratory instructions, worksheets, and writing instruments to the work area.

9. Clean all work areas and equipment at the end of the experiment. Return all equipment clean and in working order to the proper storage area.

10. Follow your teacher’s instructions to dispose of any waste materials generated in an experiment.

11. Report any accident (fire, spill, breakage, etc.), injury (cut, burn, etc.), or hazardous condition (broken equipment, etc.) to the teacher immediately.

12. Consider all chemicals used in the science room to be dangerous. Do not touch or smell any chemicals unless specifically instructed to do so.

13. Handle all animals with care and respect. a. Open animal cages only with permission. b. Never handle any animals when the teacher is out of the room. c. Do not take animals out of the science room. d. Do not tease or handle animals roughly. e. Keep animals away from students’ faces. f. Wear gloves when handling animals. g. Report any animal bite or scratch to the teacher immediately.

14. Always carry a microscope with both hands. Hold the arm with one hand; place the other hand under the base.

15. Treat all preserved specimens and dissecting supplies with care and respect. a. Do not remove preserved specimens from the science room. b. Use scalpels, scissors, and other sharp instruments only as instructed. c. Never cut any material towards you—always cut away from your body. d. Report any cut or scratch from sharp instruments to the teacher immediately.

16. Never open storage cabinets or enter the prep/storage room without permission from the teacher.

17. Do not remove chemicals, equipment, supplies, or animals from the science room without permission from the teacher.

18. Handle all glassware with care. Never pick up hot or broken glassware with your bare hands.

19. Use extreme caution when using matches, a burner, or hot plate. Only light burners when instructed and do not put anything into a flame unless specifically instructed to do so.

Do not leave a lit burner unattended.

20. Dress properly: long hair must be tied back, no dangling jewelry, and no loose or baggy clothing. Wear aprons when instructed.

21. Learn where the safety equipment is located and how to use it. Know where the exits are located and what to do in case of an emergency or fire drill.

AGREEMENT I, ___________________________ ,(student’s name) have read and understand each of the above safety rules set forth in this contract. I agree to follow them to ensure not only my own safety but also the safety of others in the science classroom or laboratory. I also agree to follow the general rules of appropriate behavior for a classroom at all times to avoid accidents and to provide a safe learning environment for everyone. I understand that if I do not follow all the rules and safety precautions, I will not be allowed to participate in science activities.

Student Signature: ______________________________________Date:_____________ Dear Parent or Guardian: We feel that you should be informed of the school’s effort to create and maintain a safe science classroom/ laboratory environment. Please read the list of safety rules. No student will be permitted to perform science activities unless this contract is signed by both the student and parent/guardian and is on file with the teacher. Your signature on this contract indicates that you have read this Science Safety Contract, reviewed it with your child, and are aware of the measures taken to ensure the safety of your son/daughter in the science classroom.

Parent/Guardian Signature:___________________________________Date:_______ Important questions: Does your child wear contact lenses? Y or N Is your child color blind? Y or N Does your child have any allergies? Y or N If so, please list:_____________________________ __________________________________________

6

Name ______________________________________________

Date ___________________________

score:

SCIENCE SAFETY TEST 1. If a fire erupts, immediately A. notify the teacher.

B. run for the fire extinguisher.

C. throw water on the fire.

D. open the windows.

2. Approved eye protection devices (such as goggles) are worn in the laboratory A. to avoid eye strain.

B. to improve your vision.

C. only if you do not have corrective glasses.

D. any time chemicals, heat, or glassware are used.

3. If you do not understand a direction or part of a laboratory procedure, you should A. figure it out as you do the lab.

B. try several methods until something works.

C. ask the teacher before proceeding.

D. skip it and go on to the next part.

4. After completing an experiment, all chemical wastes should be A. left at your lab station for the next class.

B. disposed of according to your teacher’s directions.

C. dumped in the sink.

D. taken home.

5. You have been injured in the laboratory (cut, burned, etc.). First you should A. visit the school nurse after class.

B. see a doctor after school.

C. tell the teacher at once.

D. apply first aid yourself.

6. Long hair in the laboratory must be A. cut short.

B. held away from the experiment with one hand.

C. always neatly groomed.

D. tied back or kept entirely out of the way with a hair band, etc.

7. Which of the following should NOT be worn during a laboratory activity?

A. loose clothing B. dangling jewelry C. sandals D. All of the above.

8. Horseplay, practical jokes, or pranks in the classroom are A. always against the rules.

B. okay.

C. not dangerous.

D. okay if you are working alone.

9. When handling animals, students should A. open cages only with permission.

B. not tease or handle animals roughly.

C. report bites or scratches to the teacher immediately.

D. All of the above.

10. If a piece of equipment is not working properly, stop, turn it off, and tell A. the principal.

B. your lab partner.

C. your best friend in the class.

D. the teacher.

11. When you finish working with chemicals, biological specimens, and other lab substances, always A. treat your hands with skin lotion.

B. wash your hands thoroughly with soap and water.

C. wipe your hands on a towel.

D. wipe your hands on your clothes.

12. The following activity is permitted in the laboratory: A. chewing gum B. eating C. drinking D. None of the above.

7

13. When using a razor blade or scalpel, always cut material A. away from you.

B. toward you.

C. in your hand.

D. perpendicular.

14. Before you leave the science room, you should A. clean your work area and equipment.

B. return all equipment to the proper storage area.

C. wash your hands with soap and water.

D. All of the above.

15. Draw a diagram of your science room below and label the locations of the following: ■ Fire Blanket ■ Fire Extinguisher(s) ■ Exits ■ Eyewash Station ■ Emergency Shower ■ Waste Disposal Containers ■ Fume Hood ■ Emergency Shut-off (gas)

True—False enter T or F 16. ____ All chemicals in the lab (including foodstuffs and store-bought chemicals) should be treated as if they could be hazardous.

17. ____ Work areas should be kept clean and tidy.

18. ____ Laboratory work may be started immediately upon entering the laboratory even if the teacher is not yet present.

19. ____ Never remove chemicals, specimens, or other equipment from the laboratory.

20. ____ Always carry a microscope using both hands.

21. ____ Read all procedures thoroughly before performing a laboratory investigation.

22. ____ All unauthorized experiments are prohibited.

23. ____ You are allowed to enter the chemical preparation/storage area any time you need to get an item.

24. ____ It is okay to pick up broken glass with your bare hands as long as the glass is placed in the trash can.

25. ____ Do not leave a lit burner unattended.

room c218

8

welcome to L1 and accelerated chemistry

introduction and syllabus checking off each item indicates that you are ready for your first chemistry test 1. Meet your instructor and learn how to use this website. Watch the video here 2. Meet your fellow students 3. Have a look at the class periodic table, available in editable powerpoint (ppt) and pdf format. Watch the video here 4. Take a look at the formulas we will use during the first and second semester ppt pdf screencast 5. Fill out the day 1 survey ppt pdf screencast 6. Sign the safety contract ppt pdf screencast 7. Take the safety quiz ppt pdf screencast 8. Take notes during the “water into wine� demonstration.

Screencast 9. Read the syllabus for this course ppt pdf screencast Complete the 3 labs and activities 10. flame lab ppt pdf screencast 11. molecular model lab ppt pdf screencast 12. botanical art project Watch and take notes on the following screencasted topics: 13. sc1.1: why chemistry is awesome screencast ppt pdf 14. sc1.2: What do chemists do screencast ppt pdf

15. sc1.3: the ohec scientific method screencast ppt pdf 16. sc1.4: classification of matter screencast ppt pdf 17. sc1.5: purification of mixtures screencast ppt pdf 18. sc1.6: physical versus chemical change screencast ppt pdf 19. sc1.7: extensive and intensive properties screencast ppt pdf 20. sc1.8: phase changes screencast ppt pdf 21. sc1.9: organic functional groups screencast ppt pdf 22. read the HONC rules and stereochemistry document.ppt pdf screencast 23. complete worksheet 1.1: balancing chemical equations, structural and skeletal formulas, and isomers ppt pdf screencast 24. complete worksheet 1.2 introduction to chemistry. ppt pdf screencast 25. complete worksheet 1.3: organic functional groups ppt pdf screencast 26. Complete the review worksheet: how to ace the introduction to chemistry unit ppt pdf screencast Once all items are complete you are in a strong position to do well on your first test

9

These videos contain all of the core knowledge for this course.

1. welcome to chemistry 1.1 welcome to chemistry!

1.11 how to got hooked on chemistry 1.2 matter and branches of chem 1.3 chemistry is the central science 1.4chemistry and the scientific method 1.5 what is everything made out of?

2. data 2.1 SI units and derived units 2.2 density 2.3 unit prefixes nano to tera 2.4 temperature for chemists 2.5 scientific notation 2.6 entering scientific notation 2.7 accuracy and precision 2.8 one step unit conversions 2.9 taking a measurement 2.10 significant figures 2.11 percent error 3. matter 3.1 element, molecule, or mixture?

3.2 mixtures 3.3 purification 3.4 physical and chemical properties 3.5 extensive and intensive properties 3.6 phase changes 3.7 states of matter 3.8 liquid crystals and plasmas 3.9 modern separation methods 3.10 identification methods 4. the atom 4.1 the atom: early ideas 4.2 early evidence for the atom 4.3 the electron 4.4 rutherford's gold foil experiment 4.5 history of the atom- a summary 4.6 atomic bookkeeping: p, n and e 4.7 average atomic mass 1 4.8 the band of stability 4.9 what is everything made out of?

4.10 history of the atom

5. the electron accelerated chemistry videos 5.0 valence rules 5.1 gods pattern: aufbau order 5.2 aufbau order on the per. table 9. the mole 5.3 light, waves, and frequency 9.1 what is the mole?

5.4 the electromagnetic spectrum 5.5 bohr's epiphany 1: balmer formula 9.2 mole conversions visualized 9.3 mole conversions 5.6 light and the electron 5.7 it all fits: the hydrogen emission 9.4 gram to gram and molecular spectrum conversions 5.8 atomic orbital theory 9.5 limiting and excess reactants 5.9 orbital notation 9.6 % composition, empirical and 5.10 heisenberg's uncertainty theory molecular formulas 5.11 shorthand notation 9.7 theoretical and actual yield 5.12 electronic rules 9.8 combustion analysis 5.13 valence electrons 9.9 sample combusiton analysis 5.14 electron dot structures problem 6. the periodic table 9.10 sample mixed problem 6.1 history of the periodic table 10. gases 6.2 periodic table features 10.1 gas laws 6.3 periodic table feature quiz 10.2 the three gas laws 6.4 periodic trends 10.3 all the gas formulas 7. bonding 10.4 3 gas law problems: 7.1 how do atoms bond together?

10.5 ideal and combined gas law 7.2 bond types one problems 7.3 bond types two 10.6 avogadro and graham 7.4 ionic bonds 11. solutions 7.5 multiatomic ions 11.1 solutions are everywhere!

7.6 the roman numeral region 11.2 solubility 7.7 metallic bonds 7.8,9 covalent bonds 11.3 how to adjust solubility 7.10 bond formulas 11.4 crystals 7.11 the diatomic elements 11.5 solutions exist in all phases 7.12 naming substances one 11.6 concentration 7.13 naming substances two 11.7 molarity problem 8. chemical reactions 11.8 how to prepare solutions 8.1 what is a chemical reaction?

11.9 adjusting concentrations 8.2 physical vs. chemical change 11.10 colligative properties 8.3 five types of reactions 11.11 solutes elevate boiling points 8.4 chemical recipes 11.12 solutes lower freezing points 8.5 solvents, acids and bases

12. energy 12.1 choose your energy source 12.2 car propulsion systems 12.3 energy and you 12.4 energy units and ice cream 12.5 specific heat 1 12.6 specific heat 2 12.7 enthalpy 12.8 energy of phase changes 12.9 water energy problem 12.10,11 free energy and entropy 12.12 sample free energy problem 12.13 spontaneity and free energy 12.14 bond energies 12.15 fusion: how soon?

13. reaction rates 13.1 introduction to reaction rates 13.2 reaction rate basics 13.3 reaction rate problem 13.4 adjust rate with a STICC 13.5 collision theory 13.6 collisons and energy 13.7 endothermic or exothermic.

14. equilibrium 14.1 equilibrium means reversible 14.2 equilibrium expressions 14.3 an equilibrium problem 14.4,5,6 adjusting equilibrium 15. acids and bases 15.1 common acids and bases 15.2 is water ionic or covalent?

15.3 acids and bases and water 15.4 acids and bases and your calculator 15.5 logarithms and pH 1 15.6 logarithms and pH 2 15.7 logarithms and pH 3 15.8 neutralization 15.9 titration .

10

syllabus for L1 and accelerated chemistry all about this course

Welcome to chemistry! I look forward to working with you this school year. The purpose of this syllabus is to summarize the goals, content, grading policy, and class expectations for this school year.

what is everything made out of?

That is the essential question for this course- the same question that the we all naturally ask as we look at the world around us. It also makes one wonder why some substances are inert, while other substances react violently when mixed. For a few of you, opening your mind to the world of chemistry may change the course of your life (or at least your college major), as it did for me. For all of you this course will help you to understand the world around you.

So, how do we answer this question? Certainly the most enjoyable way is to roll up your sleeves and find out for yourself. Teachers call this inquiry-based learning, and it is very effective (and, hopefully, fun!). We begin each unit by asking a simple question, and you and your lab partner then try to find out on your own. No, not by looking it up on wikipedia- by experiment. What you discover you aren’t likely to forget. It gives you a understanding of things that uses all of your senses. And, best of all, although it usually makes you question your own research, there are those rare occasions your own observations may make you question what the “experts” say, or the way that they say it. The best chemist is a skeptical chemist:

...by having Thus drawn the Chymists Doctrine out of their Dark and Smoakie Laboratories, and both brought it into the open light, and shewn the weakness of their Proofs, that have hitherto been wont to be brought for it, either Judicious Men shall henceforth be allowed calmly and after due information to disbelieve it, or those abler Chymists, that are zealous for the reputation of it, will be Robert Boyle oblig’d to speak plainer then hitherto has been done The Skeptical Chymist (1661)

The best chemist is a skeptical chemist. An original copy of The Skeptical Chymist (1661)from the University of Pennsylvania. Full text is available as is a scanned copy of the 1661 manuscript

Here are the units we will cover. Each chapter will last for 1-2 weeks, and most units will be tested individually. These 15 packets include or will direct you to everything you need to know about chemistry.

Students receive paper copies of each packet, and it is online at the class website (chemistryacademy.org)

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Grading Policy This class uses a “pure points” system: your grade will be determined by the points accumulated from homework, tests, and lab reports. For, example, you might earn 90 points on a 100 point exam, and 5 points on a 10 point quiz. Your average at that point would be 95 points out of a possible 110 total points for an “average” of 86%. Your grade can be accessed on PowerSchool, through the GHS website, also available on the chemistryacademy.com website. Test scores usually incorporate a citizenship component: arriving late to class or being unprepared results in a minor deduction for each occurrence. Assisting others and other meritorious behavior can lead to a small increase in your test score. During any type of testing, there can be no communications in any form with any other student(s). Should such communications take place, the student(s) will receive a grade of zero on the test. Be aware that it is a big deal if your cellphone is out for any reason during a test- this can result in severe consequences.

What to bring to class All parents should receive an email a few days before the first day of class outlining what each student should bring on day 1. Each day students should bring: 1. A laptop or tablet. If you don’t have one a chromebook will be supplied to you in class. Check for updates on this since the school policy is somewhat fluid at this point.

2, A chronologically organized small 3 ring binder that includes the current semester of handouts, all additional handouts , and tests.

3, Loose leaf paper in the binder.

4. A scientific calculator 5. A pen or pencil 6. Your homework 7. Ear buds or Headphones for listening to screencasts.

8. A chromebook or laptop.

On the first day of class you will receive this chapter, and each chapter will be handed out a the end of the previous one..Notebook checks occur during tests (5 points each), mostly to see that you are taking effective notes and completing all worksheets, and staying organized.

The homework for each week is posted in the classroom and on powerschool. Have it out at the beginning of class so it can be collected. Sorry, no credit for Homework late homework.

in this class extensive use will be made of screencasts which include a scored follow-up quiz. Have a look at them at the chemistryacademy.org website; stay tuned for further details.

Absences and Makeup Tests If you missed a class it’s easy to find out what you missed. The weekly schedules and homework are posted in class and on chemistryacademy.org. Rather than asking what you missed when you return from an absence, come in with your homework completed. For extended absences, check in with your instructor to schedule any makeup work. Note that an absence does not excuse you from your work; you will receive a zero until the work is made up. F With the exception of the hands-on labs, this class is fully set up for distance learning. All lectures have screencasts that can be viewed online, and each chapter is available online. Use your packet, go online. Watch the screencasts for each lecture. Complete the worksheets. Email me if you get stuck. Call your friends.

Please try to avoid asking me “What did I miss?”- check powerschool first. Instead, say hello when you return to class and let me know that you are on track. Be aware that you will still have to take the test on the day scheduled, or soon after your return if you for excused absences.

Makeup tests are available for verified absences. Sorry, no retests.

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chemistryacademy 2012-2013

scopolamine

atropine

hyoscamine

anisodamine anisodine

Datura Stramonium

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This course uses a series of chapters which are available online. Students are given a hard copy of each successive chapter during each chapter test Cellphones Please don’t take out your cellphone without permission. If it is impeding your work it may be confiscated.

Media Privacy Occasionally there may be photographs or videos taken of us in the classroom. Although these are usually popular with the students and are good for class morale, it is important for each student to know that their right not to be photographed or videotaped is important and will be respected. Additionally, any photos or videos that are taken in the classroom will never be shared outside the classroom. Each student was mailed a media privacy form at the beginning of the year. Please let me know if you prefer not to be photographed or videotaped.

Welcome to Chemistry! Please email me if you have any questions.

Dr B Common Issues 1. Late to class Students who are late to class without a pass will receive a minor point deduction on their next test. Two tardies results in an email to your parents. Three tardies leads to a detention.

2. Arriving unprepared.

Students who do not have a binder, calculator, and a pencil will receive a minor point deduction on their next test. Daily homework is worth 5 points, and is due at the beginning of class 3. Cellphones visible in class Once class begins, any cellphone seen will result in a 5 point deduction on the next test. Additional consequences such as detentions may follow.

4. Lab Groups of more than 2 To receive credit for a lab experiment your group must be no more than 2 students.

4. Absences and makeup tests Unexcused absences are treated in accordance with the student-parent handbook. Students are responsible for making up lost work and will still have to take each test.

There are no makeups, but students may drop one test per quarter 5. Homework from other classes Will be confiscated if students work on it in class unless specifically instructed otherwise.

6. Students not seated or not in assigned seats Please remain seated in your assigned seat unless instructed otherwise to me marked as present.

7. Unsafe laboratory practices This is a serious offense and will result in immediate removal from class and administrative action.

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