AP Chemistry Syllabus
Overview of AP Chemistry
AP Program
Our school offers one section of AP Chemistry, which meets five days a week for 45 minutes; averaging three to five days during one of the weeks for each unit as laboratory experiments.The goals with this program are to provide college level chemistry instruction for a diverse student population, provide college level laboratory experiences and prepare students for the AP exam in May 2007.
Student Laboratory Manual (binder)
Even though students work in pairs, they each are required to submit a report for the lab experiments performed. These reports will be kept in a bound notebook and will follow a specific outline included in the laboratory preparation section of the students’ notebook. Laboratory manuals will be graded at the finish of each laboratory experiment. They will be graded on neatness and organization, following specific outline for laboratory notebooks, data, calculations, discussion of theory, questions and possible error occurring in the experiment.
Most experiments listed in this syllabus will require hands-on work in the laboratory. Some are virtual labs which still involve students; with few being teacher led. In collaboration with other students, they will be called upon to collect, process and manipulate data taken from physical observations, both measured and unmeasured, and then develop and formally report their conclusions. The laboratory manual is MANDATORY.
Text
Zumdahl, Zumdahl. Chemistry. 7th ed. New York: Houghton Mifflin Company. 2007
Laboratory Manuals and Websites
We use several sources for our collection of laboratory experiments. These include:
Hall, James F. Experimental Chemistry. 7th ed.
Flinn Scientific Laboratory Kits
http://www.chemcollective.org/vlab/vlab.php
Resource Texts
Thrope, Gary S. Cliffs AP – 5 Chemistry Practice Exams. 2006
Knoespel, Morlan, Ohn-Sabatello. Fast Track to A 5. 2006
Hill, James C. Chemistry: The Central Science. 8th ed.
Lemay, Jr, Robblee, Beall, Brower. Chemistry: Connections to Our Changing World. 2002
Hummel, Zumdahl, Zumdahl, Student Solutions Guide to Accompany Chemistry 7th Ed. 2007
Course Outline
A. Calculation Review from General Chemistry 2.0 week August/September
(used Chemistry I book for review)
1. Chemical Foundations (conversions,, significant digits with calculations) pp. 19-32 C6
2. Atoms, molecules and ions (periodic table, naming compounds) pp. 244-245 C1, C4
3. Stoichiometry (mole-mole, mole-mass, mass-mass, mole-volume, empirical formulas, molecular formulas) pp. 347-353 C6
4. Types of chemical reactions and solution stoichiometry (molarity, molality, and dilutions) pp. 506-529 C2, C6, C3
5. Gases (Boyles Law, Charles Law and Ideal Gas Law) pp. 431-445 C2, C6
6. Thermo chemistry ▲H, ▲Hf, ▲ Hv pp. 392-490 C3, C6
7. Atomic structure and Periodicity electron configuration pp. 147-153 C4
8. Bonding: General Concepts Lewis dot diagrams pp. 230-231 C1
9. Covalent Bonding: Orbitals pp. 141-145 C1
10. Liquids and Solids pp. 456-478 C2
11. Properties and Solutions pp. 500-533 C2
12. Chemical Kinetics pp. 720-747 C3, C6
13. Chemical Equilibrium (Keq) pp. 541-544 C3, C6
C1 – Provides instructions in each of the five content areas outlined in the Course Description the first which is Structure of Matter (Chemical Bonding)
C2 – Provides instruction in each of the five content areas outlined in the Course Description the second which is States of Matter (Solutions)
C3 – This course provides instruction in each of the five content areas outlined in the Course Description, the third which is Reactions (Reaction types: Equilibrium)
C4 – Provides instruction in each of the five content areas outlined in the Course Description, the fourth which is Descriptive Chemistry
C6 –This course emphasizes chemical calculations and the mathematical and formulations of principle
B. Chemical Equilibrium (Ch 13) 2.5 weeks September
1. Laws of mass action C3
2. Equilibrium expressions C3, C6
3. Calculations of K and equilibrium concentrations C3, C6
4. LeChatelier’s principle C3
5. Shifts of equilibrium by temperature, concentration, etc. C3, C6
Assignments:
1. Read pp 611-624. Answer questions 19,21,23,25,27,29,31,35pp. 650-651
2. Read pp 625-640. Answer questions 37, 39, 41, 43,45,47,49,51pp. 651- 652
3. Read pp 640-647. Answer questions 59,61,63,65 pp. 653-654
4. Bonus: Questions 70,72,76,82,83 pp. 654-655
5. Lab: The Analysis of Aspirin
C3 – The course provides instruction in each of the five content areas outlined in
the Course Description, the second of which is State of Matter (gases, Liquids and solids, Solutions)
C6 – Emphasizes chemical calculations and the mathematical formulation of principles in the Course Description
C. Acids, Bases and Equilibria Applications (Ch 14 & 15)4.0 weeks October/November
1. General properties of acidic and basic solutions
2. Define acids and bases according to (a) Arrhenius (b) Bronsted-Lowry (c) Lewis definition C1, C3
3. Identify conjugate acid-base pairs C1, C3
4. Write equilibrium expressions for acid dissociations C1, C3
5. Distinguish among monoprotic, diprotic and triprotic C1
6. Solve problems involving the auto ionization of water C1, C6
7. Define pH and convert between pH, pOH, [H+], [OH-] C6
8. Calculate pH of strong and weak acids and/or bases C6
9. Calculate equilibrium concentrations from percent dissociation C3, C6
10. Explain why certain salts give acidic or basic solutions and show how to calculate the pH of the solutions C1 ,C3,C 6
11. Explain how bond strength and polarity affect acid-base properties C1
12. Predict whether an oxide will produce an acidic or basic solution C1, C 3
13. Explain the effect of a common ion on acid dissociation equilibra and perform calculations on acidic solutions involving common ion C3, C6
14. Explain the characteristics of buffered solutions and calculate the pH of buffer solutions C3, C6
15. Demonstrate how to calculate the pH at any point in an acid-base titration C3, C6
16. Explain how acid-base indicators work C3
17. Select the proper indicator for an acid-base titration C3
Assignments:
1. Read pp 626-654. Answer questions: 29, 37,43,45,47,55,59,63,65,67,77,81,85,95,97
pp. 673-676
2. Read pp 655-660 Answer questions: 99, 101, 105, 109, 111 pp. 676-677
3. Read pp 661-667 Answer questions: 113, 117, 119, 121 pp. 677
4. Read pp 681-696 Answer questions: 21, 23, 27, 33, 37, 41 pp. 740-741
5. Read pp 696-716 Answer questions: 51, 53, 57, 65, 73 pp. 741-743
6. Read pp 717-730 Answer questions: 75, 77, 79, 83, 91, 93, 97, 99 pp. 743-744
7. Read pp 731-736 Answer questions: 103, 105, 111, 113 pp. 744
8. BONUS: 138, 140, 144, 152, 154 pp. 746-747
9. Lab: Analysis of Vinegar Solution and Solid Acid
C1 – Provides instruction in each of the five content areas outlined in the Course Description, the first of which is
Structure of Matter (Chemical Bonding)
C3 – Evidence of Curricular Requirement: The course provides instruction in each of the five content areas outlined
in the Course Description, the third of which is Reactions (Reaction types: Equilibrium)
C6 – Emphasizes chemical calculations and the mathematical formulation of principles
D. Stoichiometry and Types of Chemical Reactions and Solution Stoichiometry (Chapter 3 & 4)
3.0 weeks November/December
1. Describe the modern atomic mass scale and how atomic masses are determined C1, C4
2. Explain the importance of the mole concept
3. Calculate the molar mass of a compound when given a formula C3, C6
4. Interconvert among moles, mass, volume and number of particles in a given sample C3, C6
5. Calculate the mass percent of each element in a compound C6
6. Determine the empirical formula of a compound C1, C6
7. Obtain the molecular formula when given the empirical formula and molar mass C1, C6
8. Identify the characteristics of a chemical reaction and the information given by a chemical equation C1
9. Write a balanced equation to describe a chemical reaction C1
10. Calculate masses of reactants and products using a chemical equation C3, C6
11. Identify the limiting reagents in a reaction C6
12. Solve problems involving limiting reactants C3, C6
13. Calculate the percent yield of a product from a reaction C3 C,6
14. Predict whether a precipitate will form in solution reaction C6
15. State rules of solubility of salts in water C2
16. Write molecular, ionic and net ionic equations to describe reaction in solution C1
17. Solve a variety of problems involving the formation of precipitates C3, C6
18. Solve a variety of problems reacted to acid/base neutralization C3, C6
19. Define oxidation/reduction C2
20. State rules for assigning oxidation states and assign oxidation states to atoms C2
21. Balance oxidation/reduction reactions in both acidic and basic solutions using the half reaction method C3, C6
Assignments:
Chapter 3
1. Read pages 79-88 Answer questions 29, 33,34,36,39,48,53,54,84,89,91 pp. 117-121
2. Read pages 89-96 Answer questions 59,65,68,73,74,79 pp. 119-125
3. Read pages 106-112. Answer questions 97,100,101,105 pp. 121-122
4. BONUS: 145-146 pp 124-125
Chapter 4
1. Read pages 131-147 Answer questions 2, 3,9,11,15,17,19,21,23,25,27 pp. 179-181
2. Read pages 147-157 Answer questions 29,31,33,35,37,39,41,43pp. 181-182
3. Read pages 157-164 Answer questions 45,47,49,51,55pp. 181-182
4. Read pages 164-178 Answer questions 57,59,61,63,65,67 pp. 182-183
5. Lab: Percentage of silver in Alloy
. C1 – The course provides instruction in each of the five content areas outlined in the Course
Description, the first which is Structures of Matter (atomic structure)
C2 –The course provides instruction in each of the five content areas outlined in the Course
Description, the second which is States of Matter (solutions)
C3 – The course provides instruction in each of the five content areas outlined in the Course
Description, the third which is Reactions (Reaction Types and Stoichiometry)
C4 – The course provides instruction in each of the five content areas outlined in the Course
Description, the fourth which is Descriptive Chemistry (including relationships in the periodic
table)
C6 – The course emphasizes chemical calculations and the mathematical formulation of principles
E. Atoms, Molecules and IonsandGases (chapter 2 and 5) 3.0 weeks January/February
1. Describe and solve problems related to the Law of Conservation of Mass, the Law of Definite Proportions and the Law of Multiple Proportions C1, C2 ,C3, C 6
2. State Dalton’s Atomic Theory and apply the theory to specific chemical problems C1, C6
3. State Avogadro’s hypothesis C1
4. Summarize the experiments that characterized the structure of the atom. (Millikan, Thomson, Rutherford) C1
5. Describe features of subatomic particles (mass, charge, location) C1
6. Assign the correct number of protons, neutrons and electrons to an atom, isotope or ion C1
7. Explain the use of nuclear symbols as AXZ to describe an atom C1
8. Determine if a particle is an atom, molecule or ion C1
9. Determine the charge and number of protons, neutrons and electrons in a monatomic ion C1
10. Define: covalent bond, molecule, chemical formula, ion, cation, anion, ionic bond, and polyatomic ion C1
11. Classify elements as metals or nonmetals C4
12. Distinguish among a group and a series on the Periodic Table C4
13. Describe alkali metals, alkali earth metals, transition metals, halogens and noble gases. C4
14. Given information about an element, state what group it belongs to C4
15. Name compounds when given their formulas and write formulas for compounds when given their name C1, C4
16. Given the symbol of any element, provide the name and charge or given the name of the element provide the symbol C4
17. Given the formula for any common polyatomic ion, provide the name and charge, or given the name of any common polyatomic ion, provide the formula and charge C1
18. Define radioactivity, and describe alpha, beta and gamma particles
19. Write equations for nuclear reactions C3
20. Describe how barometers and manometers operate
21. Define and convert among the various units of pressure C6
22. Describe the laws that relate volume, pressure and temperature of a gas and perform calculations involving these laws C2
23. Define the molar volume for an ideal gas C2
24. Define STP C2
25. Perform stoichiometric calculations for reactions involving gases C3, C6
26. Calculate molecular mass of a gas from density data C3, C6
27. State the basic postulates of the kinetic molecular theory C2
28. State the relationship between partial pressure, total pressure ad mole fraction C2
29. Define temperature
30. Calculate and use root mean square velocity C6
31. Describe effusion and diffusion C2
32. Explain the relationship between effusion and molecular mass C2
33. Describe the basic composition of the atmosphere C2
34. Describe the chemistry of air pollution C2
35. Describe how real gases deviate from ideal behavior and why this deviation occurs C2
36. Show how Van der Wails’ equation allows for real gas behavior C2
Assignments:
Chapter 2:
1. Read pages 39-72. Answer questions 10, 13, 26, 28, 33, 35, 36,43,45,47, 49, 55-60, 62, 65, 70
pp. 70-73
2. BONUS: Answer questions 87, 90 pg. 74
Chapter 5:
1. Read pages 181-192. Answer questions 27, 28, 33, 36, 37 pp. 219 - 220
2. Read pages 193-199 Answer questions 40, 44, 45, 47, 51, 54, 57, 61, 66, 72 pp. 220 - 222
3. Read pages 206-214 Answer questions 85, 90 pp. 223
4. LAB: Formula of a Hydrate
Chapter 2 –
C1 – The course provides instruction in each of the five content areas outlined in the Course Description, the first of
which is Structure of Matter ( Atomic theory and atomic structure, chemical bonding)
C4 – The course provides instruction in each of the five content areas outlined in the Course Description, the fourth of
which is Descriptive Chemistry (including relationships in the periodic table)
C6 – The course emphasizes chemical calculations and the mathematical formulation of principles
Chapter 5 –
C2 – The course provides instruction in each of the five content areas outlined in the Course Description, the second
which is States of Matter (Gases, Liquids and Solids, Solutions)
C3 – The course provides instruction in each of the five content areas outlined in the Course Description, the third which
is Reactions (Reaction types, Stoichiometry, Thermodynamics)
C6 – The course emphasizes chemical calculations and the mathematical formulation of principles
F. Electrochemistry (Chapter 17) 2.5 weeks February/March