AP chem Assignments
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AP Chemistry Sequencing 2009-2010 Midterm 1 expected oct 8- 9 1. Chapters a. Ch. 1- Math b. Ch. 2 – Atoms, Molecules, and Ions c. Ch. 3 – Stoichiometry d. Ch. 4 – Reactions and solution Stoichiometry Midterm 2 nov 12 and 13 CH 1-4 and 2. Chapters a. Ch. 6 – thermochemistry b. Ch. 7 – Atomic Structure and Periodicity Midterm 3 dec 17 and 18th Chapters 1-9 a. Ch. 8 – Bonding b. Ch. 9 – Orbitals and Geomtry c. Ch. 5 - Gas Laws Midterm 4 expected date jan 28, 29 4. Chapters 1-11 a. Ch. 10 – Liquids and Solids b. Ch. 11 - Solutions Midterm 5 expected Mar 4th and 5th 5. Chapters 1-14 a. Ch. 12 – Kinectics b. Ch. 13 – Equilibrium c. Ch. 14 - Acid/Base Midterm 6 expected april 8th and 9th 6. Chapters 1-17 a. Ch. 15. - Acid Base Equilibria b. Ch. 16. – Thermodynamics c. Ch. 17 – Electrochemistry Chapters covered on your own Ch. 18 - Nuclear- Nuclear Chemistry EC thanksgiving due first day back. 11.28.09 1. Outline of Ch 18 max 2 pages (10 pts) 2. 4 pts Make a table summarizing the different types of decay. a. 2 pts What does each emit? b. 2pts Write one example for each type 3. 2 pts each Ch 18 review # 14, 15, 16, 23, 24, 25, 26, 30, 38, 39, 44, 51, 52, 53, 62, 65 Ch. 21 - Coordination compounds winter break EC due 1.11.2010 1. outline max 2 pages 10 pts 2. 10 pts vocab for ch 21. 3. 4 pts explain why mercury is dangers to you. 4. 2 pts explain the difference between oxidation state and coordination number 5. 2 pts each ch 21 review # 10, 14, 19, 24, 30, 31, 32, 33, 34, 36, 51, 57 Ch. 22 - Organic due 3.14.2010 Optional extra credit may be done ONLY if you did not do the thanksgiving assignment 10 pts-read ch 22 do an outline MINIMUM 2.5 pages, MAX 5 pages AP CHEM REVIEW TEST Test #1 Wed april 21st 330 to 745 pm food will be provided test #2 sat april 24th can be 8-1130 or 1-4 test #3 fri may 7th 4-7 pm or sat april 8th we will take a vote on this one.
Upcoming Assignments
No upcoming assignments.
Past Assignments
Due:
Assignment
AP chemistry HW set 15
Part 1 due fri
Ch 11 review 27, 36, 37, 38
Outline
Read 12.1 and 12.2 do max 2 page outline
Part 2 due wed
1. Write an equation for the dissolving process for ammonium chloride
2. Is dissolving calcium chloride exothermic or endothermic?
3. Assume 1.0 m solution for all the following. With a new freezing point at -5.6 C and a molal freezing constant for water is -1.86 C/m
Findthe von hoff factor
Ch 11 review #40, 42, 50, 57, 64, 70, 92
Part 1 due fri
Ch 11 review 27, 36, 37, 38
Outline
Read 12.1 and 12.2 do max 2 page outline
Part 2 due wed
1. Write an equation for the dissolving process for ammonium chloride
2. Is dissolving calcium chloride exothermic or endothermic?
3. Assume 1.0 m solution for all the following. With a new freezing point at -5.6 C and a molal freezing constant for water is -1.86 C/m
Findthe von hoff factor
Ch 11 review #40, 42, 50, 57, 64, 70, 92
Due:
Assignment
AP chemistry HW set 14
Part 1
NONE
Outline due 1.19.2010
Read ch 11 max 3 page outline
Part 2 due (1.20.2010)
1. Do vocab for ch 11
2. Describe at the molecular what happens when NaCl and Sugar dissolve in water
3. Explain what the difference between molarity and molality
4. What factors affect solubility and explain how they work.
Part 1
NONE
Outline due 1.19.2010
Read ch 11 max 3 page outline
Part 2 due (1.20.2010)
1. Do vocab for ch 11
2. Describe at the molecular what happens when NaCl and Sugar dissolve in water
3. Explain what the difference between molarity and molality
4. What factors affect solubility and explain how they work.
Due:
Assignment
AP chemistry HW set 13 due mon 1.11.2010
Read Ch 10 do outline
• Don’t worry about page 431 to 433
Do vocab for whole chapter
Questions
1. Compare and contrast physical properties for solids and liquids (at least 8)
2. For the following explain how they are caused at the molecular level
a. Viscosity
b. Increase in mp, bp, fp down a group
c. Beading
d. Surface tension
e. Capillary action
f. H-bonding
g. London dispersion
h. Compression
3. Compare and contrast the different types of alloys
4. Explain the impact of ceramics on the production of transistors
5. Compare and contrast ionic and molecular solids
6. During a heating curve, why is there no observed temperature change during a phase change?
7. Draw a basic heating curve for water and label each section and how to calculate the q of each section
8. Draw a phase diagram for water and CO2.
a. Label each diagram.
b. Label the process that occurs as you cross each boundary.
9. Ch 10 review questions # 3, 12, 15, 20, 23, 24, 25, 28, 30, 33, 35, 38, 69, 79, 80, 81, 85, 86,
Read Ch 10 do outline
• Don’t worry about page 431 to 433
Do vocab for whole chapter
Questions
1. Compare and contrast physical properties for solids and liquids (at least 8)
2. For the following explain how they are caused at the molecular level
a. Viscosity
b. Increase in mp, bp, fp down a group
c. Beading
d. Surface tension
e. Capillary action
f. H-bonding
g. London dispersion
h. Compression
3. Compare and contrast the different types of alloys
4. Explain the impact of ceramics on the production of transistors
5. Compare and contrast ionic and molecular solids
6. During a heating curve, why is there no observed temperature change during a phase change?
7. Draw a basic heating curve for water and label each section and how to calculate the q of each section
8. Draw a phase diagram for water and CO2.
a. Label each diagram.
b. Label the process that occurs as you cross each boundary.
9. Ch 10 review questions # 3, 12, 15, 20, 23, 24, 25, 28, 30, 33, 35, 38, 69, 79, 80, 81, 85, 86,
Due:
Assignment
AP chemistry HW set 12
Part 1 due Friday
Ch 5 review #71, 72, 75, 76, 77, 81, 82
Outline
read 10.1 max 1 page
Part 2 due wed
Ch 5 review # 84, 85, 86, 88, 89, 94, 105, 106, 110, 112, 114, 115, 116, 118, 125, 126
Part 1 due Friday
Ch 5 review #71, 72, 75, 76, 77, 81, 82
Outline
read 10.1 max 1 page
Part 2 due wed
Ch 5 review # 84, 85, 86, 88, 89, 94, 105, 106, 110, 112, 114, 115, 116, 118, 125, 126
Due:
Assignment
AP Chemistry HW set 11
Part 1 Due Monday
1. List all the pressure units conversions, all the temperature conversion, and R
2. List all your gas laws (10 total) HINT: B, C, G, C, I, A, D, RMS, G, R
a. For each law what are your conditions
b. What kind of relationship (if applicable)
c. Draw a graph of the relationship (if applicable)
3. Summarize KMT and use KMT to explain what happens when you increase the temperature of a gas inside a balloon.
4. Ch 5 review #20, 25, 26
Outline Due Monday
Read Ch 5 (2nd half) do Max 2 page outline
Part 2 Due Wednesday
Ch 5 review #27, 29, 31, 38, 40, 42, 44, 46, 51, 53, 54, 56, 59, 62, 63, 65, 66, 67,
Part 1 Due Monday
1. List all the pressure units conversions, all the temperature conversion, and R
2. List all your gas laws (10 total) HINT: B, C, G, C, I, A, D, RMS, G, R
a. For each law what are your conditions
b. What kind of relationship (if applicable)
c. Draw a graph of the relationship (if applicable)
3. Summarize KMT and use KMT to explain what happens when you increase the temperature of a gas inside a balloon.
4. Ch 5 review #20, 25, 26
Outline Due Monday
Read Ch 5 (2nd half) do Max 2 page outline
Part 2 Due Wednesday
Ch 5 review #27, 29, 31, 38, 40, 42, 44, 46, 51, 53, 54, 56, 59, 62, 63, 65, 66, 67,
Due:
Assignment
AP Chemistry HW Set 10
Part 1
1. Compare and contrast a C-O bond, a C=O bond and a C=O bond
a. Note bond length, bond enthalpy, and electron density
2. Explain octet expansion. Why can we have SF4 and not OF4
3. What 3 ions are isoelectric with Xe. Arrange them by ionic size
4. Draw the lewis structure for PF5, ClF3, PCl5, NO3-, and Br3-. Why is it ok for some compounds to have more than 8 electrons around them?
5. Ch 8 review # 54, 57, 70
Read Ch 9 do outline
Max 3 page
Part 2 due wed before thanksgiving
1. Draw each hybridization. sp to d2sp3
2. Define bond order
3. How are sigma bonds different from pi bonds?
4. How is diamagnetic different from paramagnetic?
5. Ch 8 review # 86, 91, 92, 96, 100, 102, 118, 123, 125, 128, 130
Part 1
1. Compare and contrast a C-O bond, a C=O bond and a C=O bond
a. Note bond length, bond enthalpy, and electron density
2. Explain octet expansion. Why can we have SF4 and not OF4
3. What 3 ions are isoelectric with Xe. Arrange them by ionic size
4. Draw the lewis structure for PF5, ClF3, PCl5, NO3-, and Br3-. Why is it ok for some compounds to have more than 8 electrons around them?
5. Ch 8 review # 54, 57, 70
Read Ch 9 do outline
Max 3 page
Part 2 due wed before thanksgiving
1. Draw each hybridization. sp to d2sp3
2. Define bond order
3. How are sigma bonds different from pi bonds?
4. How is diamagnetic different from paramagnetic?
5. Ch 8 review # 86, 91, 92, 96, 100, 102, 118, 123, 125, 128, 130
Due:
Assignment
AP Chemsitry Hw Set 9
Part 1 mon week 9
1. What factors determine bond type, bond energy, and bond length?
2. Compare and contrast in a 4 ring venn diagram the 4 types of bonds
a. Include ΔEN, bond length, size, bond strength, Cooulomb’s law, dipole, electron distribution, electron configuration,
3. Explain metallic bonding and how does metallic bonding account for metal properties: conductive, malleable, and ductile?
4. Explain why ions are different sizes then neutral atoms. In which direction does IR increase.
5. Why is a -2 ion bigger than a -1 ion? Is it the same for a +2 ion and a +1 ion?
Outline
Read 8.1 to 8.8 do a max 3 page outline due tues week 9
Part 2 due monday of week 10
1. Make a table summarizing all the VSEPR shapes. Include an example not listed in the table in the book, bond angles, # of lone pairs and # of bonds
2. Given the following bond energies, estimate the enthalpy change (heat of reaction) for the combustion of methane (CH4).
C - C, 347 kJ/mol
C = C, 614 kJ/mol
C - O, 358 kJ/mol
C = O, 799 kJ/mol
C - H, 413 kJ/mol
O - H, 463 kJ/mol
O - O, 146 kJ/mol
O = O, 495 kJ/mol
3. Ch 8 review #22, 24, 26, 30, 40, 46, 47, 67, 68, 81,
Part 1 mon week 9
1. What factors determine bond type, bond energy, and bond length?
2. Compare and contrast in a 4 ring venn diagram the 4 types of bonds
a. Include ΔEN, bond length, size, bond strength, Cooulomb’s law, dipole, electron distribution, electron configuration,
3. Explain metallic bonding and how does metallic bonding account for metal properties: conductive, malleable, and ductile?
4. Explain why ions are different sizes then neutral atoms. In which direction does IR increase.
5. Why is a -2 ion bigger than a -1 ion? Is it the same for a +2 ion and a +1 ion?
Outline
Read 8.1 to 8.8 do a max 3 page outline due tues week 9
Part 2 due monday of week 10
1. Make a table summarizing all the VSEPR shapes. Include an example not listed in the table in the book, bond angles, # of lone pairs and # of bonds
2. Given the following bond energies, estimate the enthalpy change (heat of reaction) for the combustion of methane (CH4).
C - C, 347 kJ/mol
C = C, 614 kJ/mol
C - O, 358 kJ/mol
C = O, 799 kJ/mol
C - H, 413 kJ/mol
O - H, 463 kJ/mol
O - O, 146 kJ/mol
O = O, 495 kJ/mol
3. Ch 8 review #22, 24, 26, 30, 40, 46, 47, 67, 68, 81,
Due:
Assignment
AP chemistry
AP chemistry homework set 8
Part 1
1. For each of the following metals
a. State the flame color
b. Calculate the ΔE of the photon
i. Ca, Cu+1, Fe, Na, K, Mg
2. List ALL possible quantum sets for
a. N, Y, Cr, Al
Outline
Read 7.10 to 7.13 do 1.5 page outline (max)
Part 2
1. If an electron falls from n=4 to n =2
a. What kind of light will be emitted?
b. Calculate the ΔE
2. What is the electron configuration, orbital diagram, and short hand for
a. Ni
b. Se
c. Mg
3. Chapter review
a. Ch 4# 117
b. Ch 6# 105
c. Ch 7# 120, 134, 141
AP chemistry homework set 8
Part 1
1. For each of the following metals
a. State the flame color
b. Calculate the ΔE of the photon
i. Ca, Cu+1, Fe, Na, K, Mg
2. List ALL possible quantum sets for
a. N, Y, Cr, Al
Outline
Read 7.10 to 7.13 do 1.5 page outline (max)
Part 2
1. If an electron falls from n=4 to n =2
a. What kind of light will be emitted?
b. Calculate the ΔE
2. What is the electron configuration, orbital diagram, and short hand for
a. Ni
b. Se
c. Mg
3. Chapter review
a. Ch 4# 117
b. Ch 6# 105
c. Ch 7# 120, 134, 141
Due:
Assignment
AP chemistry HW set 6
Part 1:
1. Explain what the degree symbol and the f mean in ΔH°f
2. Determine the heat of reaction for 3C (s) + 4H2 (g) → CH3CH2CH3
a. Given
CH3CH2CH3 +5O2 (g) → 3CO2 (g) + 4H2O ΔHf = -2044kJ
2H2 (g) + O2 → 2H2O ΔHf = -486.3kJ
C(s) + O2 (g) → CO2 ΔHf = -393.5kJ
3. The thermochemical equation for the combustion of ethyne is:
C2H2(l) + 5O2(g) --> 4CO2(g)+2H2O(g) H=2600kJmol-1
How much energy is produced when 13.0g of ethyne are burnt?
4. Calculate ΔH for the reaction : C2H4(g) + H2(g) → C2H6(g) from the following data.
C2H4(g) + 3 O2(g) → 2 CO2(g) + 2H2O(l) ΔH = -1411 kJ
C2H6(g)+ 3 ½ O2(g) → 2 CO2(g) + 3 H2O(l) ΔH = -1560 kJ
H2(g) + ½ O2(g) → H2O(l) ΔH = -285.8 kJ
Outline
Read 7.1 to 7.4. max 1.5 page outline
Part 2
1. 100 grams of water is heated from 20 C to 30 C. The specific heat of water is 4.184 J/ g x C. Calculate the amount of heat absorbed by the water.
2. Ch 6 review # 54, 62, 63, 72, 84, 94, 95, 97, 101