AP CHEMISTRY
SYLLABUS
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Course Description
AP Chemistry is designed to be the equivalent of the general chemistry course taken during the first
college year, both conceptually and in the laboratory. The labs serve to supplement the learning in the
lecture section of the course. All labs will be performed after school between 2:45pm and 3:30pm over
the course of a week. There will be some time allowed during the scheduled class time; however, most
labs take two to three hours and cannot be done during that time. Pre-requisite’s to this course include
Advanced Biology, Advanced Math II, College Preparatory Chemistry. Co-requisite’s are Advanced Math
III and College Preparatory Physics.
Chemistry is the study of the composition, structure, and properties of matter and the changes that
matter undergoes. Topics of study include Structure of Matter (20 %), States of Matter (20 %),
Reactions (35-40 %), Descriptive Chemistry (10-15 %), and Laboratory (5-10 %).
AP Class Size: Approximately 14 students; 2 students per lab group
Course Requirements and Grading
All quizzes consist of multiple choice and/or free response only. Chapter Tests consist of Multiple choice
and free response questions. The multiple choice and free response questions come from released AP
Exams. At the end of the 4th Quarter, there will be a lab final exam based on all experiments performed
throughout the year. Each student may use his/her lab notebook on the exam. The Lab Final will count
as a lab grade during the 4th quarter. The grade is a weighted average of the following:
Tests………………………………………………...................60 %
Quizzes………………………………………………………………15 %
Labs…………………………………………………………….........5 %
Mid-Term Benchmark……….………………………………..5 %
Semester Benchmark………………………………………..15%
Instructional Materials
Pen, Pencil, Paper, 1-2” notebook (classroom), 1” notebook (lab),
½ “ notebook, TI-30X Calculator
Make-Policy
1)
2)
3)
4)
All quizzes can be re-taken one time.
Make-up assignments must be completed prior to the next unit assessment.
Projects/Laboratories that have had various progress checks may not be redone.
Tests may not be re-taken.
AP Chemistry Course Sequence
1st Semester
Chapter 5
Chapter 26
Chapter 6
Chapter 7
Chapter 8
Chapter 9
Chapter 4
Chapter 3 & 4
Chapter 2
Chapter 3
Chapter 15
The Structure of Atoms
Nuclear Chemistry
Periodicity
Chemical Bonding
Molecular Structure and Covalent Bonding Theories
Molecular Orbitals in Chemical Bonding
Introduction to Naming Compounds (Acids, Bases, Salts, Oxidation #’s)
Balancing Chemical Equations and Some Types of Chemical Reactions
Chemical Formulas and Composition Stoichiometry
Reaction Stoichiometry
Chemical Thermodynamics
Chapter 10
Chapter 17
Chapter 18
Chapter 19
Chapter 20
Chapter 16
Chapter 21
Reactions in Aqueous Solutions I: Acids, Bases, and Salts
Chemical Equilibrium
Ionic Equilibria I: Acids and Bases
Ionic Equilibria II: Buffers and Titration Curves
Ionic Equilibria III: The Solubility Product Principle
Chemical Kinetics
Electrochemistry
Equations Unit
2nd Semester
Review Weeks
a.
b.
c.
d.
e.
f.
g.
h.
i.
Multiple Choice 1984, 1989, 1994, 2002
Thermodynamics
Kinetics
2000-2005, 2008 Free Response
1989 Multiple Choice
Electrochemistry
1999 Practice AP exam (timed and self-graded)
Free Response 1990-1998
Laboratory
Exams and Lab Final
Required Texts
Whitten, Kenneth, W, Raymond Davis, Larry Peck, and George Stanley. Chemistry. 8th Edition. Prentice
Hall – Pearson.
Supplemental Texts
Vonderbrink, Sally Ann. Laboratory Experiments for Advanced Placement Chemistry. 2nd Edition. Flinn
Scientific.
Davis, RaymondE., Frey, Regina, Sarquis, Mickey, Sarquiz, Jerry L. Modern Chemistry. Holt, Rinehart,
and Winston.
Http://apcentral.collegeboard.com
Laboratory Program
Experiment 1
Lab: Analysis of Alum, AlK(SO4)2*12H2O
Determine the identity of Alum by two techniques, mole ratio and melting point
Experiment 2
Lab: Determination of the Empirical Formula of Silver Oxide
To determine the percent composition and empirical formula of Silver Oxide
Experiment 3
Lab: Gravimetric Analysis of a Metal Carbonate
To determine the identity of a Group 1 metal carbonate compound by gravimetric analysis
Experiment 4
Lab: Finding the Ratio of Moles of Reactants in a Chemical Reaction
To use the method of continuous variations to determine the mole ratio of two reactants.
Experiment 5
Lab : Liquid Chromatography
To separate the components of the mixture, unsweetened grape-flavored Kool-Aid
Experiment 6
Lab: Determination of Molar Mass of Volatile Liquids
To determine the molar masses of various volatile liquids
Experiment 7
Lab: An Activity Series
To determine the activity series for five metals and for three halogens
Experiment 8
Lab: Acid-Base Titrations
To standardize a sodium hydroxide solution and use the standard solution to titrate
an unknown solid acid.
Experiment 9
Lab: Analysis of a Commercial Bleach
To determine the amount of sodium hypochlorite in a commercial bleach by reacting it with
sodium thiosulfate in the presence of iodide ions and starch.
Experiment 10
Lab: Determination of Ka of Weak Acids
To determine the pKa values for ionization of two unknown weak acids.
Experiment 11
Lab: Oxidation-Titrations
To standardize a solution of potassium permanganate by redox titration with a standard
solution of iron (II) ions.
Experiment 12
Lab: Predicting the Products of Chemical Reactions and Writing Chemical Equations
To predict the products of a chemical reaction and to write a balanced chemical equation that
describes the reaction.
Experiment 13
Lab: Molar Mass by Freezing Point Depression
To determine the molar mass of an unknown substance by measuring the freezing point
depression of a solution of the unknown substance and BHT.
Experiment 14
Lab: Solubility and Determination of ΔG0, ΔH0, and ΔS0 of Ca(OH)2
To measure the solubility of calcium hydroxide by titration with hydrochloric acid at two different
temperatures and to use these solubilities to estimate Ksp, ΔG 0, ΔH0, and ΔS0.