AP Chemistry Course Syllabus
Curricular
Scoring Component (CS)
Requirement
1
CS1 – The course provides instruction in Structure of Matter:
atomic theory and structure.
1
CS2 - The course provides instruction in Structure of Matter
: chemical bonding.
1
CS3 – The course provides instruction in States of Matter:
gases.
1
CS4 – The course provides instruction in States of Matter:
liquids.
1
CS5 – The course provides instruction in States of Matter :
solids.
1
CS6 – The course provides instruction in States of Matter :
solutions.
1
CS7 – The course provides instruction in Reactions: reaction
types.
1
CS8 – The course provides instruction in Reactions:
stoichiometry.
1
CS9 – The course provides instruction in Reactions:
equilibrium.
1
CS10 – The course provides instruction in Reactions: kinetics.
1
1
1
1
1
2
3
CS11 – The course provides instruction in Reactions:
thermodynamics
CS12 – The course provides instruction in Descriptive
Chemistry: relationships in the periodic table.
CS13 – The course provides instruction in Laboratory: physical
manipulations.
CS14 – The course provides instruction in Laboratory:
laboratory report
CS15 – The course provides instruction in Laboratory:
collection of laboratory reports in a notebook
or portfolio.
CS16 – The course emphasized chemical calculations and the
mathematical formulation of principles.
CS17 – A minimum of one double period per week or its
equivalent is spent engaged in laboratory work.
AP Chemistry Pacing Guide
Weeks
Topic (Zumdahl Chapter)
Subtopic/Laboratory
Scoring
Component
1st Nine
Wks.
1
2
3
Chemical Foundations (1)
Atoms, Molecules, and Ions (2)
Stoichiometry (3)
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Pre-test
Scientific Method
Units
Uncertainty
Significant Figures
Dimensional Analysis
Temperature
Density
Classification of Matter
Assessment
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Laboratory Safety
Laboratory Notebook/Record Maintenance
Use of Volumetric Glassware (J. F. Hall, Experiment 2,
page 9) – 1 Day
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Pre-test
History of the Model of the Atom
Modern Atomic Theory
Atoms and Ion Formation
Introduction to the Periodic Table
Binary Ionic and Covalent Compounds
Assessment
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Determination of Molar Mass of a Volatile Liquid (J. F.
Hall, Experiment 15, page 159) – 1 Day
Pre-test
Atomic Mass
The Mole
Molar Mass
Percent Composition
Determining Empirical Formula
Balancing Chemical Equations
Stoichiometric Calculations
Limiting Reactant Identification
Yield Calculations
Assessment
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Determination of the Percentage Water in Cu(SO4)2·
13, 14, 16
1, 2, 13
8, 13, 16
H2O (J. F. Hall, Experiment 12, page 117) – 1 Day
4
5
Types of Reactions and
Solution Stoichiometry (4)
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Character of Water
Strong and Weak Electrolytes
Composition of Solutions
Precipitation Reactions
Acid-Base Reactions
Oxidation-Reduction Reactions
Balancing Redox Equations
Oxidation-Reduction Titrations
Assessment
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Analysis of Commercial Bleach (S. A. Vonderbrink,
Experiment 10. page 57) – 1 Day
Finding the Ratio of Moles of Reactants in a Chemical
Reaction (S. A. Vonderbrink, Experiment 2, page 7) – 1
Day
Pressure
Gas Laws
Gas Stoichiometry
Dalton’s Law of Partial Pressure
Kinetic Molecular Theory of Gases
Effusion and Diffusion
Real Gases
Assessment
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6
7
Gases (5)
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8
9
Thermochemistry (6)
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Calcium Carbonate Analysis: Molar Volume of Carbon
Dioxide (J. A. Beran, Experiment 19, page 237) – 1 Day
Energy
Enthalpy and Calorimetry
Hess’s Law
Standard Enthalpies of Formation
Sources of Energy
Assessment
6, 7, 8, 13
3, 13
11, 13, 16
Heat of Metal/Acid Reactions (J. F. Hall, Experiment
17, Choice IV, page 183) – 1 Day
Thermochemistry and Hess’s Law (S. A. Vonderbrink,
Experiment 6, page 31) – 1 Day
2nd Nine
Wks.
10
11
12
Chemical Kinetics (12)
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Reaction Rates
Rate Laws
Determining the Form of the Rate Law
Reaction Mechanisms
10, 13, 16
13
14
Chemical Equilibrium (13)
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Kinetic Model
Catalysis
Assessment
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Rates of Chemical Reactions (J. F. Hall, Experiment 25,
page 303) – 1 Day
Equilibrium Condition
Equilibrium Expressions
Heterogeneous Equilibria
Applications of the Equilibrium Constant
Solving Equilibrium Problems
Le Chatelier’s Principle
Assessment
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14
15
16
17
Acids and Bases (14)
Atomic Structure and
Periodicity (7)
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Determination of the solubility Product of an Ionic
Compound (S. A. Vonderbrink, Experiment 13, page 81) –
1 Day
The Nature of Acids and Bases
Acid Strength
The pH Scale
Calculation of the pH of Strong Acid Solutions
Calculation of the pH of Weak Acid Solutions
Polyprotic Acids
Acid-Base Properties of Oxides
The Lewis Acid-Base Model
Assessment
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Analysis of Stomach Antacid Tablets (J. F. Hall,
Experiment 29, Choice II, page 367) – 1 Day
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Analysis of an Unknown Acid Sample (J. F. Hall,
Experiment 29, Choice I, page 361) – 1 Day
Electromagnetic Radiation
Nature of Matter
Atomic Spectrum of Hydrogen
The Bohr Model
The Quantum Mechanical Model of the Atom
Quantum Numbers
Orbital Shapes and Energies
Pauli Principle
The Aufbau Principle
Periodic Trends in Atomic Properties
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Emission Lines of Some Metallic Elements (J. F. Hall,
Lab 18, Choice III, page 209) – 1 Day
9, 13, 16
9, 13, 16
1, 13
17
18
Bonding Concepts (8)
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Types of Chemical Bonds
Electronegativitiy and Bond Polarity
Formation of Ionic Compounds
Partial Ionic Character of Covalent Bonds
Covalent Chemical bonds Models
Covalent Bond Energies and Reactions
The Localized Electron Bonding Model
Lewis Structures
Exception to the Octet Rule
Resonance
Molecular Structure : The VSEPR Model
Assessment
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Molecular Properties (J. F. Hall, Lab 19, Choice I, page
223) – Day 1
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Midterm
2
3rd Nine
Wks.
19
20
Covalent Bonding (9)
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Hybridization
The Molecular Orbital Model
Homonuclear Diatomic Molecules
Heteronuclear Diatomic Molecules
Combining Localized and Molecular Orbital Models
Assessment
21
22
Liquids and Solids (10)
23
24
Properties of solutions (11)
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Intermolecular Forces
Liquids
Structure and Types of Solids
Structure and Bonding in Metals
Network Atomic Solids
Molecular Solids
Ionic Solids
Vapor Pressure and Changes of State
Phase Diagrams
Assessment
Solution Composition
Energies of Formation
Solubility
Vapor Pressure of Solutions
Boiling-Point Elevation and Freezing-Point Depression
Osmotic Pressure
Colligative Properties of Electrolyte Solutions
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Molecular Mass by Freezing Point Depression (S. A.
Vonderbrink, Experiment 43, page 43) – 1 Day
2
4, 5
6, 13, 16
25
26
27
Applications of Aqueous
Equilibria (15)
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Acid-Base Equilibria: Common Ion Effect, Buffers,
Titration and pH Curves
Solubility Equilbria: Solubility Product and
Precipitation/Qualitative Analysis
Complex Ion Equilibria
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Acids, Bases, and Buffered Systems (J. F. Hall,
Experiment 28, page 345) – 1 Day
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Spontaneity and Entropy
Free Energy
Entropy Changes and Chemical Reactions
Free Energy and Equilibrium
Free Energy and Work
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Vapor Pressure & Enthalpy of Vaporization of Water
(S. A. Vonderbrink, Experiment 9, page 51) – 1 Day
Galvanic Cells
Standard Reduction Potentials
Cell Potential, Electrical Work and Free Energy
Dependence of Cell Potential on Concentration
Chemical Reactions
AP Practice Exam
32
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AP Chemistry Exam - Week of May 15th
33
34
35
36
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Qualitative Analysis of Cations (S. A. Vonderbrink.
Experiment 19, page 123) – 5 Days
Liquid Chromatography (S. A. Vonderbrink, Experiment
21, page 149) – 1 Day
Electrochemical Cells (S. A. Vonderbrink, Experiment
18, page 115) – 1 Day
Synthesis of Alum (S. A. Vonderbrink, Experiment 3,
page 13) – 2 days
Student Lab of Choice – 5 Days
9, 13, 16
4th Nine
Wks.
28
Thermodynamics (16)
29
Electrochemistry (17)
30-31
AP Exam Review
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11, 13, 16
11, 16
All
13