AP Chemistry Syllabus 2009 - 2010

Course Overview Documents

Three-ring Binder Information
How to Study for AP Chemistry
Lab Safety Rules (RTF file)
Lab Notebook Information
Lab Report Writing Information (html)
Lab Grading Outline (html) How labs are graded
Personal Introduction Essay (doc)

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Goals

The College Board AP Chemistry Course Description states that the “course is designed to be the equivalent of the general chemistry course usually taken during the first college year.” The text goes on to say that, “Students in such a course should attain a depth of understanding of fundamentals and a reasonable competence in dealing with chemical problems. The course should contribute to the development of the students’ abilities to think clearly and to express their ideas, orally and in writing, with clarity and logic.” Therefore I have adopted the following goals for this course:


Instructional Techniques and Assessment

Grades in the course will be broken down as follows:
        Tests: 50% (2 per quarter)
    Quizzes: 25% (6 - 8 per quarter)
          Labs: 25% (6 - 7 2-hr labs per quarter)

The schedule at the end of this introductory material shows what to expect for each unit. Specific dates are not given in the interest of maintaining flexibility. The number of hours of class time for each unit is indicated as a goal. Some degree of strict adherence to the amount of time will be necessary in order to meet the goals of the course. Also in the schedule is recommended Memory Work which are items that you should commit to memory.

For each unit you will be required to complete a brief Outline of the important points in the reading assigned for that unit. This Outline must be separated into the sections used in the chapter. Sometimes one or two entries on the Outline will be sufficient for a given section. For other, more complicated sections you will need to use your judgement as to what the most important ideas and problem-solving techniques are. Keep Outlines brief! This is not meant to be a burden but rather a way to encourage you to prepare thoroughly for class. Outlines should be completed by the first day of a new unit: you must read ahead!

A tip about reading textbooks: they are not novels. In a novel you typically read a passage once with full comprehension. The action carries you forward through the text. Textbooks build sequentially in each chapter and you will at times need to read a section several times—and work through its examples on paper— before you can move on to the next section. Be self-aware and check in with yourself: Did I understand that passage? Could I solve problems based on it?

Each unit has a Problem Set that consists of questions and problems from the ends of the chapters. At times I will assign problems from supplementary material for the Problem Set. These problem sets will be approached in several ways:

  1. You will work independently to solve the problems using only your brain, the text, a calculator and paper and pencil.
  2. You will work in study groups outside of class to help one another to solve the problems. Use this time not to copy another student’s solution but to compare notes about the best way to get to a solution.
  3. You will work in groups during class time with the help of your instructor.

Both Outlines and Problem Sets count as Homework. Homework is not collected, graded, or checked off. Instead, you must keep Outlines and Problem Sets neatly in a dedicated binder. At the end of the quarter you must show this binder to the instructor for a Homework Quiz grade. It will be graded on completeness and organization.

The date of the Homework Quiz will be set whenever we begin a new unit. The Homework Quiz will draw on problems directly from your homework and will be short.

Test dates will be determined as we near completion of a second or third unit in a row. Tests will be offered




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twice each quarter and will be designed to simulate the AP Chemistry Exam as closely as possible. Tests will be comprehensive and will be designed to be completed in one hour. Timed tests will help you to prepare for the AP Exam.

Labs will be offered six to seven times each quarter. Lab assignments will vary in scope but at minimum will require completion of pre-lab work by the first day of work and completion of post-lab questions. Three to four times each quarter you will be required to submit a full formal lab report (format available separately). A portion of your lab grade will depend on your diligence in keeping a good scientific lab notebook. Required for this purpose is a permanently bound ruled notebook. In this notebook you will write your lab procedures, lab notes and data while you work in the lab. By the end of the course you will have accumulated the documentation necessary for colleges to determine whether to give you credit for the lab portion of the AP Chemistry class. A handout is available separately that describes how to make good use of your lab notebook.

Study Groups are required. During the first week of class you will form study groups of 3 - 4 people. Make a regular time to meet and work on AP Chemistry together. Working together makes tackling the difficult material of this course a bit more manageable. These groups will continue to work together during class. Reshuffling of Study Groups will be allowed, if necessary.

Frequently I will ask students to present problems at the board. Presentations will consist in writing out the detailed solution to a problem on the board and explaining how you came to it to the class. The other members of the class are active participants in the process and are expected to ask questions and demand that the presenter justify his or her work. Problem presentations will be a frequent part of this course and will usually precede a Homework Quiz.


Metacognition

In this course our motto is FIO (an acronym that I leave to the reader: you will figure it out if you think about it for a bit).

It is important that you evaluate yourself frequently as you work to find out what you have learned. Try repeating to yourself the contents of class discussions. Even better, go over the concepts and problem-solving techniques with your study group: communicating something you have learned forces you to organize your thoughts about it. When you do so, you learn it better yourself. This is true also about writing in the course. Your lab reports and the answers to lab questions are learning opportunities. When you explain what you have learned in writing you often find that you have not learned it as well as you thought you did. Go back and learn it properly and your writing will improve.

We will spend time in this course developing your mental math skills. The multiple-choice portion of the AP Chemistry Exam must be done without calculators. The multiple-choice problems usually work as follows:

  1. All answers are different by an order of magnitude or more.
  2. All answers are different mathematical manipulations of the given: knowing the kind of operation required will often be enough for you to be able to guess the answer.
  3. Some answers are close and you will need to do some actual calculation: these are designed so as not to be too difficult.
  4. Sometimes answers will be close but a quick calculation with a rounded-off answer will still be enough to select the correct response.
Finally, reviewing the available responses before doing a calculation is often a good way to get through a problem quickly.

Texts

Primary textbook: Chemistry, 6th edition, Zumdahl & Zumdahl, Houghton Mifflin Company, Boston, 2003.
Experimental Chemistry, 6th edition, James F. Hall, Houghton Mifflin Company, Boston, 2003.
Laboratory Experiments for Advanced Placement Chemistry, 2nd edition, Sally Ann Vonderbrink, Ph.D., Flinn Scientific, Inc., Batavia, IL, 2006.
Laboratory Investigations, AP Chemistry, David Hostage and Martin Fossett, The Peoples Publishing Group, Inc., Saddle Brook, NJ, 2006.
Supplementary Materials available on instructor’s web site (http://kaffee.50webs.com/Science/).




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Schedule

First Quarter*
Topic
and Time
Text Information
incl. Problems
Lab(s) Memory Work
Chemical Foundations
Dimensional Analysis, Scientific Notation, Significant Figures, Density, Temperature
1 hour
Chapter 1
Problem Set: 16 19 20 23 25 27 31 33 35 38 41 49 51 55 57 59 67 69 75 77 86
Density Lab
(available online)
Tables 1.1, 1.2 and the Rules for Counting Significant Figures (pg 14)
Atomic Structure I:
Basics of Atomic Theory
3 hours
I. A. 1, 2, 3
Chapter 2: 2.1 - 2.5
Problem Set: 15 18 19 21 23 26 30 31 33 35-38 43-45 47
Pre-lab for Size of a Molecule
Size of a Molecule (all available online)
Z, A, Atomic Symbols, Dalton’s Atomic Theory (pg 46)
Atomic Structure II:
Nucleus, Radioactive Decay, Nuclear Stability, Nuclear Reactions
4 hours
I. C.
Chapter 18: 18.1, 18.2, 18.4 - 18.6
Problem Set:
Supplementary Material:
Alpha and Beta Radiation
Electron Capture and Positron Radiation
Half-life Activity
Mass Defect & Binding Energy Activity
(all available online)
Geiger Counter Demonstration Alpha, Beta, and Positron Decay modes; half-life, E = mc2
Molecules, Ions and Naming Compounds
2 hours
Chapter 2: 2.6 - 2.8
Problem Set: 49 51 53-56 59-67 69-71 77 81
Supplementary Material:
Group Activity: Atomic Structure 1
Group Activity: Atomic Structure 2 (both of the previous are from the Summer Work)
Chemical Formulas and Compounds
Naming Compounds 1
Naming Compounds 2
(all available online)
None Names and formulas for all monatomic cations and anions (easily predictable from the periodic table); names and formulas for these ions: copper, iron, ammonium, carbonate, hydrogen carbonate (bicarbonate), chromate, dichromate, cyanide, phosphate, hydrogen phosphate, sulfate, hydrogen sulfate, nitrate, nitrite, permangnate, and peroxide. Also, learn the acetate ion: C2H3O2-; prefixes in table 2.6; acids in tables 2.7 and 2.8, figure 2.25
Stoichiometry: Atomic Mass, the Mole, Percent Composition, Chemical Equations
5 hours
III. B. 1, 2, 3
Chapter 3
Problem Set: 21 23 28 31 33 35 37 41 49 53 55 69 71 75 76 77 79 83 87 89 93 95 99 101 119
Determination of the Formula of Rust cd 1
Hydrate Lab (both available online) cd 4
Avogadro’s number (6.02 × 1023 particles/mole) and its meaning
pg 120 Solving Stoichiometry problems
Reaction Types & Rxns in Solution: Water, Solutions, Acid/Base, Redox
6 hours
III. A. 1, 2, 3; B. 1, 2, 3 and IV. 1
Chapter 4
Problem Set: 11 15 17 19 21 23 29 35 43 45 47 49 51 55 57 61 63 65 81 84 90 96
Acid-Base Titration (Peoples 8) cd 7
Differences btwn. strong, weak and non-electrolytes; table 4.1 (solubility rules); table 4.2 (oxidation states rules)
Gases: Pressure, Gas Laws, Gas Phase Rxns, Partial Pressures, Kinetic-Molecular Theory
5 hours
II. A. 1 a b, 2 a b c d
Chapter 5
Problem Set: 16 19 20 23-25 29 31 33 37 47 51 54 57 59 63 65 69 73 75 93 105 117
Boyle’s Law (available online) PV = nRT; P1V1/n1T1 = P2V2/n2T2; Dalton’s Law of Partial Pressures; Definition of Mole Fraction; Molar Vol. 22.42 L at STP



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Second Quarter*
Topic
and Time
Text Information
incl. Problems
Lab(s) Memory Work
Thermochemistry: Energy, Enthalpy, Calorimetry, Hess’s Law
4 hours
III. E. 1 2
Chapter 6
Problem Set: 9 11-14 17 21 25 27 31 33 35 37 41 47 53 56 59 63
Molar Volume of a Gas (Flinn 8) cd 5
Calorimetry (H-M 17 I, II, IV) cd 13
ΔE = q + w, w = -PΔV, Hess’s Law
Periodicity: EM Radiation, Atomic Spectra, Quantum Mechanics, Orbitals
7 hours
I. A. 4, 5 IV. 2.
Chapter 7
Problem Set: 15 17 19 23 25 27 29 33 39 41 45 47 51 53 61 63 67 71 73 85 87 89 95 114 117
Flame Test/Atomic Emission Spectroscopy (available online) E=mc2, c = λν, quantum numbers, electron configuration method, trends in ionization energy and atomic radius
Chemical Bonding: Ionic, Covalent, Metallic and Hydrogen Bonds; Lewis Structures, Electronegativity, Hybrid Orbitals; Organic Nomenclature and Structure
10 hours
I. A. 5 I. B. 1 a b c, 2 a b c, 3
Chapter 8, Chapter 9.1 - 9.3, and Chapter 22.1 - 22.5
Problem Set: Ch. 8: 13 14 16-18 20 21 23 25 29 33 35 39 43 47 53 61 63 65 67 70 73 77 79 87 89 91
Ch. 9: 8 9 11 13 15 17 23 31 33
Ch. 22: 23-25 27 31 39 41 52 57
Activity: Lewis Diagrams
Lewis Diagrams: Molecules to draw
Lewis Diagrams and VSEPR Shapes
Qualitative Analysis (Flinn Kit) cd 14
Building Models (hands-on covalent bonding activity)
Lewis Structures method, pg 376 & pg 381
Trends for atomic size, ion size, and electronegativity
VSEPR model method, pg 391 & pg 400
Solids and Liquids: Intermolecular Forces, Types of Solids, Phase Diagrams
3 hours
II. B. 1-4
Chapter 10
Problem Set: 12 14-16 18 19 29 33 35 39 41 43 75 81 83 87-89
Analysis by Gravimetry (Flinn 3) cd 16
Spectrophotometric Analysis: Determining a Mass/Mole Relationship (H-M 11, II) cd 9 and cd 17
 
Solutions: Energy of Solution Formation, Vapor Pressure, Colligative Properties
5 hours
II. B. 1-4 C. 1-4
Chapter 11
Problem Set: 11 13 14 17 19 21 25 27 33 36 37 39 41 45 51 53 54 57 58 61 67 69 71 75 78 84 89
Molar Mass by Vapor Density (Flinn 9) cd 3 Types of intermolecular interaction, Definitions of molarity, molality, percent by mass, mole fraction; Π = MRT



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Third Quarter*
Topic
and Time
Text Information
incl. Problems
Lab(s) Memory Work
Kinetics: Reaction Rates, Rate Laws, Integrated Rate Laws, Reaction Mechanisms
6 hours
III. D. 1-5
Chapter 12
Problem Set: 9-12 14-17 19 21 23 27 29 31 35 37 43 47 49 50 51 53 57 61 63 73
Determination of Reaction Rate/Order (Flinn 12) cd lab 12
Post-lab Questions
Rate Laws Summary, Pg. 563; Table 12.6, pg. 578; Table 12.7, pg. 580
Kinetics Information Sheet
Equilibrium: Equilibrium Constant, Gas Equilibria, Le Châtelier’s Principle
6 hours
III. C. 1 a b, 2 a
Thermodynamic vs. Kinetic Stability
Chapter 13
Problem Set: 9 11 13 15 17-19 21 23 27 31 32 35 37 39 43 47 53 56 57 59 63
Determination of an Equilibrium Constant (Flinn 13) cd 10 and cd 17 Equilibrium Constant Expression, pg. 613;
Kp = K(RT)Δn; Le Châtelier’s Principle
Acids and Bases: Nature, Strength, pH Scale, Polyprotic Acids, Salts, Lewis Acids
6 hours
III. A. 1 B. 1 C. 2 IV. 1
Chapter 14
Problems Set: 17-23 25 31 33 35 37 39 43 47 49-51 55 59 63 67 73 75 77 93 98 99 101 105 107 113 115 119 121 123
Choosing an Appropriate Indicator (Flinn 16) cd 19 Table 14.1, pg.658; Table 14.6, pg. 693; Structure-Acid Strength Connection pg. 694; Table 14.10, pg. 696
More About Equilibria: Common Ion Effects, Buffers, pH Curves, Indicators, Solubility Equilibria
6 hours
III. C. 2 b
Chapter 15
Problem Set: 13-15 21 27 37 39 43 45 49 51 55 59 63 65 66 73 75 83 85 91 95
Qualitative Analysis (Flinn Kit) cd 14
Buffers (Flinn 17) cd 19
Henderson-Hasselbalch Eqn., pg. 722; Summary of Buffer Info, pg. 726
Thermodynamics: Free Energy, Entropy, Spontaneity of Chemical Reactions, Work
5 hours
III. E. 3, 4
Chapter 16
Problem Set: 7-10 14 15 21-23 27 29 33 35 41 43 45 51 55 58 59 71
Electrochemical Series (Walch 16) cd 20
Electrochemical Cells and Electroplating (Flinn Kit) cd 21
Table 16.3, pg. 794; Table 16.5, pg. 797



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Fourth Quarter*
Topic
and Time
Text Information
incl. Problems
Lab(s) Memory Work
Electrochemistry: Galvanic Cells, Reduction Potentials, Thermodynamics of Electrochemistry, Batteries, Corrosion, Electrolysis
6 hours
III. A. 1-3 IV. 1
Chapter 17
Problem Set: 13 14 16-21 25 27 29 31 35 39 47 49 51 55 57 65 69 73 75 77 83 87 93
  ΔG° = -nF E°; Nernst Eqn., pg. 842
Review: Two weeks of review; practice tests, targeted review to be determined none  
Organic Chemistry Chapter 22    
Analytical Chemistry Supplementary Materials    

*The letters ‘cd’ in the syllabus indicate the Course Description Recommended Experiment number. An effort has been made to cover as many of the recommended labs as possible. Also, each unit has a set of letters and numbers associated with it. These refer to the Course Description and indicate which topics in the Topic Outline are to be covered in that unit.

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