H Chem Text Readings/Assignments/Web links
Unit 0: Introduction to observation and measurement
Web links:
SF calc and diagram quiz with explanations--Only do the diagram problems
Scientific notation back and forth practice with solutions
Scientific notation and how to input to a calculator
Textbook Readings:
1) Observation, measurements, and notations pg 15-17, 51-53, 56, 68-71
Review you answers to the summer assignment and correct them
2) Scientific Notation pgs 50-53
HW: pg 61 #11-12 pg 62 #15 pg 79 #67, 68, 71
Unit 1: Math and Measurement Fundamentals
Text Chapters 3-4
Web links:
Khan academy identifying and calculating with sig figs
SF calculation quiz with explanations
SF calc and diagram quiz with explanations--you should be able to do all of them now
Unit analysis solving with metric and chemistry-type problems
Density Problem solving using label-canceling
Textbook Readings/problems:
1) Significant Figures and calculations pgs 56-62
HW: pg 60 #9,10 pg 62 #14 pg 78 #41, 42, 44, 49 pg 80 #77
2) The Metric system pgs 63-67
HW: pg 67 #19, 21, 22 pg 79 #56, 57, 70
3) Factor-Unit Problem Solving pgs 84-95
HW: pg 93 #9, 10 pg 95 # 16, 17, 19 pg 103 # 36, 39
4) Multi-step Factor-Unit Problems pgs 97-100
HW: pg 97-99 #20, 21, 22, 24 *pg 103 #44, 49, 52
5) Precision, Accuracy and Error pgs 54-55
*Deviation Calculation In-class
HW: pg 62 #13-16 pg 78 #39, 40
6) Density pgs 68-72
HW: pg71 #23, 24 pg 72 #26, 28 pg 79 #61 pg 80 #72, 78
7) Properties of matter, elements, compounds and mixtures pgs 28-40
HW: pg 35 #7-12 pg 47 #27, 30, 32,33
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Unit 2: Atomic Theory and electron configuration
Textbook chapters 5 + 13
Web links:
Dalton's Atomic Theory Summary
JJ Thomson CRT experiment
Rutherford's Gold Foil experiment
1) Early scientists: Dalton, Thompson, and Rutherford
pgs 107-112 Do section 5.1 and 5.2 review
2) Composition of the nucleus, atomic weight/mass calculations
pgs 113-121 Do section 5.3 review
3) Light and atomic spectrum; photoelectric effect
pgs 372-381 Do section 13.3 review
3) Electrons and the quantum mechanical model
pgs 361-366 Do section 13.1 review
4) Electron configuration and quantum numbers
pgs 367-370
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Unit 3: Electron configuration, trends, and the Periodic Table
Text Ch 14
Atomic Trends-Khan academy series of videos
Quantum numbers, the PT, and validity check
Review problems:
-Textbook review pg 409+ #s 17, 21-24, 28, 29, 37, *43
1. Read p 391-396, Do 14.1 section review
2. Read p 398-406, Do 14.2 section review
3. Review Problems Ch 14:
pg 409-410 #21, 24, 26, 28, 29, 30, 37, 43
and pg 411 #13-16
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Unit 4: Matter, formula writing/naming and chemical reactions
Binary Ionic Formula writing (~4mins)
Binary Polyatomic Formula Writing (~10mins)
Transition Metal Formula writing (also vs non transition metals) (~11mins)
Covalent Naming from formulas (~10mins)
Acid Naming classifications (~13mins)
Hydrate naming and formula writing (~5mins)
Ionic Naming/formula writing online quiz
1) Matter, elements, and compounds, properties pg 29-43
HW: pg 43 #19-23 pg 47 # 35, 36, 38, 42
2) Molecules vs Ions pgs 133-148
HW: Review- pg 48 #43, 47 pg 49 #1-14
3) Writing ionic formulas pgs 149-156
HW: pg 148 # 20-23 pg 156 #32-26
4) Writing molecular formulas and naming acids pgs 158-163
HW: pg 163 #43-44 pg 166 #50-54, 56, 58, 61, 62
--------Unit 4b/5 starts here -------
5) Chemical reactions pgs 203-211
HW: Review pg 167 #63-71
6) Classifying Chemical Reactions and Predicting pg 212-224
HW: pg 232 #32, 34, 35, 38, 43, 47, 48, 49, 50, 52
7) No reading
HW: pg 233-234, # 56, 57, 58, 60, 61, 70
8) Net Ionic Equations pg 225-228
HW: pg 228, #28-31
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Unit 6: The Mole
Avogadro's number (what is a mole)-just watch the first 5 minutes until it makes sense
Common mole calculations
#1) read pg 170-180 (moles and molar mass)
pg 181, do section 7.1 review
#2) read pg 180-186 (moles and molar volume)
pg 186, do section 7.2 review
#3) pg 198, do ***46-51, and 55-58
#4) Read pg 188-195 (% composition, Empirical and Molecular formulas)
pg 195 do section 7.3 review
#5) Ch 7 review problems, pg 198-200
#60, 61, 62, 64, 68, 77, 81, 86
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Unit 7: Stoichiometry
Helpful links:
Limiting reactant concept (6mins)
Limiting reactant Calculation--Problem solving starts at 10mins in (16mins total, last 6 mins=problem solving)
Percent yield concept and sample calculation (5mins)
#1) Using chemical equations
Read p236-241 pg 241, do 9.1 review
#2) Stoichiometry problem solving
Read pg 242-250 pg 250, do 9.2 review
#3) Molarity
Read pg 509-513 pg 515 #18, 21, 22, pg 528-529, #50, 52, 73
#4) Limiting Reactants
Read pg 252-259 pg 259, do 9.3 review
#5) Ch 9 Review
pg 262-264 #37, 38, 40, 44-46, 48, 58, 59
#6) Ch 9 Standard test prep
pg 265 #1-12
Stoichio problems missing answers
WS 3 #5 992g limestone
WS 4 #3 0.103 mol excess, 13.8g CO2
WS 5 # 2a PH3=excess, 3.41g left, 2.70g water
WS 6 #1-4 all list LR #5b 52.4g excess #8 1.86g/L (Products of the reaction are CaCl2 + CO2 + H2O #9a 10.9g b 23.3g
Textbook #70 117.2L of air (specific gravity is essentially the same as density for usits)
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Unit 8: Nuclear Chemistry
Chapter 28
Helpful Links
Crash Course Nuclear 1 (10mins)
Crash Course Nuclear 2 (10mins)
Solving half life with Logs
Nuclear energy calculations (3mins)
1) Nuclear radiation, radioactivity, and decay
pgs 841-846
2) Half life...read the CheMath parts too
pg 847-851
3) Fission and medical uses
pgs 853-855, 859-861
4) Fusion and detection of radiation
pgs 856-859
Nuclear Recap answers:
Muliple choice: BDACC ACDDC CACAXXB
18) A-proton b) neutron c) Calcium-43 d) beta (-) e) alpha f) Tin-95
19) beta (-) is emitted
34) 4.12x10^9 years
35) 17200yrs
36) 9.00x10^11 J/mole and 1.50x10^-12 J/nuclide (per nucleus)
Mass and Energy Relationships
1) 4.33x10^6 kg/second
2) -1.92x10^13 J/mole
3) a) 197n + 135p -->X-332
b) 5.55765x10^-22 g/nuclide (per nucleus)
c) mass defect= 4.17391 x 10^-27 kg
d) 3.766519x10^-10 J/nuclide (per nucleus)
e) 2.26142 x10^14 J/mole
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Unit 9: Gas laws and Gas Stoichiometry
Text Ch 10 and 12
Helpful links:
Gas pressure, units, and demonstrations (5mins)
Ideal gas law problem solving, with molar mass (10mins)
1) KMT, pressure, temperatures
Read pg 267-272 (section 10.1) and pg 327-328 (section 12.1)
2) Factors affecting gases
Read pg 330-332
3) Gas laws
Read pg 333-340
4) Ideal gas laws
pg 340-346
5) Avogadro and Graham's law
pg 347-353
WS3 (Dalton's Law WS) Answers:
1) 541mmHg O2, 309mmHg N2
2) 17.8psi Ar, 13.4psi Cl2
3) 137 torr Kr, 318 torr Xe, 319 torr H2
4) 0.0262 moles KClO3 (you need to use stoichiometry, the problem was misplaced)
WS4
#5) 45.9L
10) 1.5 atm
Recap and Integrate: Gases ANSWERS:
1) 74.2g/mol
2) 1.51x10^23 molecules Cl2
3 d=0.980g/L
4) 8.86g Cl2
5) N2 and Cl2=38 torr, O2 and He=152 torr
6) 0.395atm
7) 13.7L
8) 83.9g/mol
9) NH3 is 1.50x faster than F2
10) 14.8 atm
11) a) 36.0L b) 18.75L NO c) 0.196g O2 d) 167g NO
12) a) 32.0g/mol b) N2H4
13) 1.4x10^8L
14) CCl2F2
15) a) Zn + 2HCl--> ZnCl2 + H2 b) 767.2 torr c) 97.74%
16) a) 0.9947g dry air b) 156.71g empty c) 1.37g unknown gas d) 40.29g/mol e) 8.44% err
17) v=1336 m/s
18) CF2Cl2
19) B=H2
20) B=1273K
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Semester 2 START
Unit 10: Bonding (Ch 15 and 16 in text)
Helpful Links:
Lewis Pics, Formal charge, and resonance
1. Read pg 413-419, do 15.1 Section Review problems
2. Read pg 437-446 (covalent bonding)
3. Read pg 449-451(resonance and exceptions to octets) do 15.2 Section Review problems #7-11
4. Read pgs 455-457 (Vsepr theory), and 460-463 (Polarity)
5. Read pg 452-455, 457-459 (molecular and hybridized orbitals)
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Unit 11, Forces of attraction and condensed states of matter (Text ch 10, 15-17)
Helpful Links and Videos:
IMF force types and why (6mins)
Vapor Pressure (2mins)
Solving heating curve problems (6mins)
Complete heating curve problem solving (10min)-uses J/g instead of kJ/mol so problem setup is slightly different
1. Read pg 460-466, Do 16.3 section review problems (IMF types)
2. Read pg 475-478, Do 17.1 Section review problems (water props)
3. Read pg 479-481, Do 17.2 section review problems (Evap and condense)
4. Read pg 274-279 (liquids and evaporation)
Read pg 284-286 (phase diagrams)
5. Read pg 280-283, and Read pg 422-429, Do 15.2 and 15.3 review problems (Props of ionic and metallic)
WS2 H-bonding
1) N-H, O-H or F-H covalent bonds
2) *Just classify each lone O, N or F as a receptor, and each OH, NH, or FH as a donor...don’t double count
a) D1 R0, Total=1 b) D2 R2, T=4 (in reality D2, R4, T=6...but don’t worry)
c) 3/3/T=6 4/3/T=7 2/2/T=4 3/2/T=5
3) SWSWSSW
4) a) by h-bonding b) by LDF
WS3 Vapor pressure and boiling (graph WS)
2) higher temp produces higher VP
3) increased KE means more particles with enough energy to escape IMFs, so more evaporation
4) ~58C
5) VP=AP
6) VP would be the same. If temp and substance are the same, evaporation rate is the same
7) ~127C
8) Cooking time would be shorter bc the water boils at a higher temp, so it is hotter
Attractive Forces Answers
WS4
1) a-0.733atm b-from evaporating alcohol c-P increases d-liquid decreases
2) steam can exist at much higher temperatures, and thus much higher KE; If both at the same temp, steam contains more thermal energy
3) endothermic, it absorbs thermal E from the room
4) depends on external pressure
5) 83.5 kJ
6) 3.96g
7) 2.64 J/gC
8) (2 steps) 31.8kJ
9) 2.15x10 ^23 molecules
10) (4 steps, final temp is -2.0C, not +) 14.0kJ
11) charged particles are allowed to move in a metallic solid
12) their structure is a network of covalent bonds to each atom/molecule nearby that reinforces, like a bed-spring
13) shifting the ionic structure mis-aligns the charges and increases repulsion immensely
14) increasing KE allows IMFs to be reduced more easily due to increased motion and likelihood of particles with enough energy to do so
Notes pt 4: Consider scenarios...
-Rain? yes, FP and MP can change depending on external pressure. (see phase diagram) Higher pressures cause this
-Gas to solid? Yes, incr pressure can cause deposition (phase diagram)
-solid to vapor? yes, increasing temp at a given pressure...or reducing ext pressure at a given temp (phase diagram)
-evap at surface? particles at a boundary are at higher energy due to imbalances attractive forces
Last 3 Diagram pages
VP and Boiling:
1) 40C 2) 72C 3) 102C
4) 380torr 5) 150torr 6) 50torr
7) 54C 8) 82C 9) 111C 10) C
Phase diagram:
1) A=solid 2) C=liquid 3) B=gas 4) d=triple pt
5) e=critical point 6) 60C 7) 100C 8) >110C
9) 45C and 0.5atm 10) solid > liq 11) freeze
Freezing and BP graph
1) 5C 2) 15C 3) 5C 4) a 5) c 6) e
7) b 8) d 9) bd 10) ace 11) d 12) b
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Unit 12: Solutions (Text Ch 17-18)
Helpful Links and Videos
Factors affecting solubility (5mins)
Crash Course dissolving ionic vs covalents (5mins)
Boiling Point elevation concept (4mins)
Freezing point depression concept and quick calc (4mins)
1. Read pg 482-488, do section review problems
2. Read pg 490-493, then read 501-508 (factors affecting solubility)
3. Read pg 509-514 (Molarity and concentration units)
4. Read pg 517-525 (colligative properties)
5. Chapter 18 Review problems (most odd #s are answered in the back of the book)
# 49, 52-55, 58, 60, 61
6. Chapter 18 Review problems
# 72, 73, 76, 79, 86, 91
Summary & Recap: Solutions Answers
1) 0.583M
2) -will not be on our test-
3) 0.208M
4) 30.ml more are needed
5) 131g/mol
6) MF=C4H8O6
7) i=4, +3 charge on the metal
8) 318g/mol
9) *given that 1g vinegar=1ml vinegar*
a-0.833M b-0.88m acetic in vinegar
10) 124g/mol
11) a-100.0662C b-actual=lower because it may not fully dissolve c-lower because only 2 particles would be produced
12) 112g ethanol
13) 0.300g/L (it uses Henry's Law from pg 506 in the text---Just know the concept that higher pressure increases gas solubility)
14) a-decreases b-No effect c-No effect d-decreases e-increases
Other Corrections/Missing Answers:
Notes pt 2 Practice
6) .23 (too many SF) 10) 26.0g 12) 180g/mol
WS2
3) 52 g/mol (too mane SF) 5) 0.114M NO3
POGIL Soln Conc WS
9) 965g solution
WS3
3) EF=C2H3O3 MF=C4H6O6
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Unit 13: Thermochemistry (Text Chapter 10-11)
Helpful Links and Videos
Definitions, vocab, and problems
Calorimetry problem examples and explanation (pdf)
Hess's Law info and worked out problems
Entropy and Gibbs overview (8mins)
Bond Energy WS answers
1. Read pg 292-299, do Section Review 11.1 problems (exo and endothermic, heat capacity) AND
Section review pg 322, #s 47, 42-45.
2. Read pg 300-306, do Section Review 11.2 problems (calorimetry and thermochemical equations)
3. Read pg 314-318, do Section Review 11.4 problems (Hess's Law and heat of formation)
4. Read pg 307-313, do Section Review 11.3 problems (Heat of fusion/vaporization/solution)
5. Read pg 549-556 (entropy and Free Energy)
6. Mixed review problems (some Hess's, some calorimetry, some definitions) pgs 322+ #s 48, 52, 57 (class ex), 58, 64, 70, 72
7. Mixed review problems, pgs 322+ #s 56, 59, 60, 73, 75, 84....pg 497 #58
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Unit 14: Equilibrium
Text Chapter 19
Eq concept and reversible reactions (4min video)
RICE problem examples and workthrough, including assumption (pdf file)
Le'Chatelier's Principle concept and common stresses (4min video)
Le'Chatelier's stresses: temp, catalysts (4min video)
Le'Chat Worksheet Answers
1) Read pg 539-541, 545-548 Reversible reactions and Keq (the problem solving intro as well)
2) Read pg 630-637 Ksp
Problems # 25-32, 34, 35 throughout reading. (answers in the back of the book)
Eq problem Answers/adjustments:
Eq Practice problems-set 2
1) a) 1.00M, 0.50M, and 1.00M c) 2.0
2) b) 0.260 c) It shifts forward to make more products, reactant amounts decrease, K is the same
3) b) sq root of answer (a) c) 1/ answer (a)
4) **If Kp=0.55, it is quadratic to solve. X=0.39, Cl=0.78
5) 0.409M, 0.409M, 0.057M
6) 1.70mol CS2, 3.10mol Cl2, 0.30mol S2Cl2
7) (all values are using torr, not atm....just check your concepts) a) Q=0.0933 b) Not at Eq c) It will shift left to produce more reactants d) quadratic problem solving...if you see that you are fine
8) [BrCl]=0.0900M, 31.1g BrCl
WS2
5) 2.06x10^-10
Unit 16: Acids and Bases (text Ch 20-21)
Unit 17: Acid and bases
Helpful Links and videos
College-level complete notes (ignore anything related to "buffers")
Salt Hydrolysis video (7mins-Kahn Academcy)
1) Read pg 577-579, Do section 20.1 review (properties of acids and bases, simple naming)
2) Read pg 594-5599, Do section 20.3 review (Classifications of acids/bases)
3) Read pg 580-593, Do section 20.2 review (H+ ions and pH, and indicators)
4) Read pg 600-605, Do section 20.4 review (Acid/base strength, dissociation constants)
5) Read pg 613-618, Do section 21.1 review (neutralization, --SKIP--equivalents, and normality)
6) Read pg 626-629. (salt hydrolysis, buffers)
Unit 17: Redox reactions and Electrochemistry (Text Ch 22-23)
Helpful links and videos
Galvanic cell animation video (2mins)
Narrated interactive animation (flash)
Electrochemical and electrolytic cells (8min video)
Determining cell potentials (6 min problem solving)
All worksheet answers (gdoc)
1) Read pg 645-653, Do section review 22.1 (What is Redox, ID it in reactions)
2) Read pg 654-659, Do section review 22.2 (Oxidation numbers)
3) Read pg 660-669, Do section review 22.3 (Balancing redox, half reactions)
4) Read pg 677-684, Do section review 23.1 (Electrochemical cells)
5) Read pg 685-691, Do section review 23.2--Do NOT copy the chart on pg 688, you will be given it (Cell Potentials)
6) Read pg 692-697, Do section review 23.3 (Electrolytic cells)
Unit 18: Kinetics (rates of reactions) Text Ch 19
1. Read pg 533-538, Do 19.1 section review (reaction rates)
2. Read pg 566-569, Do 19.5 section review (Rate laws)
3. Ch 19 review problems:
pg 572+ #64, 62, 65, 67, 74, 75, pg 575 #4
Unit X: Organic Chem Introduction
Helpful links and videos
Make your own naming quiz
Example page and Back page answers