AP CHEMISTRY SYLLABUS
Erich Schneider
Text:
Brown, Theodore E., H. Eugene LeMay, and Bruce E. Bursten. Chemistry: The Central Science. 10th Edition.
Upper Saddle River, NJ: Prentice Hall.
Assessment:
We will cover four units during each academic quarter. Each unit will include:
 Daily homework assignments consisting of a selected reading and questions from the text. Occasionally,
worksheets will be assigned. Assignments can be found on my web page.
 1-2 labs with write-ups. See below for more detail.
 A review packet the will help prepare you for the test. These will include notes, straightforward questions as
well as pertinent multi-step questions from past AP exams.
 In class, we will work together to learn the new material and go over problems. Due to the small class size
in AP Chemistry, students should expect and be prepared to participate daily in our class discussions and to
learn from each other as much as possible.
 A test on each unit. Tests will account for 70% of each quarter grade. (Lab reports: 15%;
Homework/Participation: 15%). Once corrected, we will go over each test thoroughly allowing you to make
corrections. You will be permitted to keep your tests for review.
More on The Lab Component:
Labs are an integral part of the AP curriculum. Every unit will include one or two hands-on labs.
Students will work in pairs to collect data and observations in their notebooks and may collaborate when
assessing their data and planning their calculations. Each lab group will have the opportunity to discuss the
results of the lab informally in class. However, students must work independently when preparing their lab
reports and answering follow-up questions. Lab write-ups will typically include a purpose, a neat and organized
presentation of data and calculations, a conclusion and frequently, answers to follow-up questions. Given the
expectations of the AP curriculum and the constraints of our daily schedule, students may be required to give up
a portion of their lunch break and/or meet after school to complete some of the lab work.
The Importance of your First Year in Chemistry:
The knowledge and lab skills you acquired in your Honors Chemistry course will prove to be essential
to your success in AP Chemistry. In essence, this course is the second part of a two-year Chemistry curriculum.
As you may recall, there were many times throughout your Honors Chemistry curriculum when we went above
and beyond the textbook to cover a topic. Some of these topics included quantum numbers, the HendersonHasselbalch equation, the hydrolysis of salts as well as the memorization of a long list of polyatomic ions. You
completed many hands-on labs that allowed you to develop numerous laboratory skills. Some of these labs were
actually AP level labs. You will come to appreciate the extensive knowledge and skills you mastered during
your first year of chemistry.
Labs Completed During the First Year of Chemistry
1. Observing Physical and Chemical Changes
2. “Centium”: Calculation of % Abundances of Isotopes
3. “Gold Foil Lab”: Using models to calculate the relative size of nuclei
4. “Mendeleev Lab”: Looking at Group and Periodic Trends
5. Polar / Nonpolar Lab
6. Determination of the Empirical Formula of Magnesium Oxide
7. Determination of the Empirical Formula of Zinc Chloride (*time permitting)
8. Stoichiometry: “The Nail Lab”
9. Observing types of Chemical Reactions
10. Determining the Molar Mass of a Gas
11. Determining and Graphing the Solubility of Potassium Nitrate
12. Calculating the Specific Heat of a Metal
13. Using Hess’ Law to Determine the Heat of Combustion of Magnesium Metal.
14. “Iodine Clock”: Factors that Affect the Rate of Reaction
15. Equilibrium: “Le Chatelier’s Lab”
16. Properties of Acids and Bases
17. Acid-Base Titrations
18. Reduction Potentials of Micro-Voltaic Cells (*time permitting)
19. Synthesis of an Ester
20. Saponification (*time permitting)
Syllabus:
Second Quarter
First Quarter
Schedule
Possible Labs & Supplemental
Materials Provided
Unit & Main Topics
Review (Chapters 1-2)
 Classification of Matter
 Properties of Matter
 Measurement and math basics
 Conversions
 Atomic Theory
 Naming inorganic compounds
Stoichiometry (Chapter 3)
 Chemical Equations
 Stoichiometry calculations
 % Composition
 Empirical/Molecular Formula calculations
 Limiting Reactant calculations
 Solution Stoichiometry
Reactions (Chapter 4)
 Classifying Chemical Reactions: Addition,
Decomposition, Displacement, Metathesis,
REDOX, Neutralization, Combustion
 Solubility Rules
Thermochemistry (Chapter 5)
 Energy Basics and the 1st Law of
Thermodynamics
 Enthalpies of Reaction and Formation
 Calorimetry
 Hess’ Law
Electron Structure and Periodic Properties of
the Elements (Chapters 6-7)
 Nature of Light
 Wave Behavior and Quantum Mechanics
 Electron Configurations
 Periodic Trends: Effective Nuclear Charge,
atomic radii, ionic radii, electron affinities,
ionization energies, electronegativities,
metallic character
Bonding and Molecular Geometry
(Chapters 8 & 9)
 Drawing Lewis structures
 Ionic Bonding
 Covalent Bonding
 Resonance structures
 Exceptions to the Octet Rule
 Bond strengths
 VSEPR Model
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Lab: Percent Silver in an Alloy
Lab: Determination of the
Percent by Mass of Water in
Epsom Salt
Polyatomic Ion Table
Lab: Percent Carbonate in an
Egg Shell
Lab: Determination of the
Empirical Formula of Copper
oxide
Stoichiometry Review packet
Lab: Gravimetric Analysis of a
Metal Carbonate
Lab: Qualitative Analysis
Reaction Resource Guide
Solubility Rules Worksheet
Lab: Hess’ Law of Heat
Summation
Thermochemistry Review
packet
Quantum Number Tutorial /
Worksheet
Electrons and Periodic Trends
Review Questions
Lab: Qualitative analysis of
cations and anions
Lab: Molecular Geometry
Model Building
Bonding Review Questions
 Hybridization
 Molecular Geometry
The Gas Laws (Chapter 10)
 Kinetic Molecular Theory (KMT)
 Boyle’s Law, Charles’ Law, Gay-Lussac’s
Law, Combined Gas Law
 Ideal Gases and the Ideal Gas law
 Dalton’s Law of Partial Pressures
 Molecular Effusion and Diffusion
 Real v. Ideal Gases
 Van Der Waal’s equation
Intermolecular Forces of Attraction, Solids and
Liquids (Chapter 11)
 Properties of solids and liquids
 Types of intermolecular attractions
 Vapor Pressure
 Phase diagrams
Third Quarter
MIDTERM EXAMS (December 19-21)
Solutions (Chapter 13)
 The solution process
 Solubility and solubility curves
 Expressing concentration: Mass %, ppm,
ppb, mole fraction, molarity, molality
 Colligative properties: boiling point
elevation, freezing point depression, vapor
pressure lowering, osmosis
 The role of solutions in cell biology
Chemical Kinetics (Chapter 14)
 Factors that affect the rate of reaction
 Reactions Rates
 Rate Laws
 Change of Concentration over time
 Temperature and Rate
 Reaction Mechanisms
 Catalysis
Chemical Equilibrium (Chapter 15)
 The concept of Equilibrium
 The Equilibrium Constant, Keq and Kp
 Applications of Keq / Kp
 Le Chatelier’s Principle
Acids and Bases I (Chapter 16)
 Definitions of Acids and Bases: Arrhenius,
Bronsted-Lowry, Lewis
 Conjugate Acid-Base Pairs
 Self-ionization of water (Kw)
 pH and pOH
 Strong acids v. Weak Acids
 Strong Bases v. Weak Bases
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Lab: Determining the Molar
Volume of a Gas
Gas Laws Review Problems
Lab: Determination of the
Molar Mass of a Volatile
Liquid
IFA’s, Solids and Liquids
Review Problems
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Review Outline
Review questions
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Lab: Determination of Molar
Mass by Freezing Point
Depression
Solutions Review Questions
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Lab: Kinetics of a Reaction
Kinetics Review Problems
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Lab: Determining the Keq for a
reaction
Lab: Le Chatelier Lab
Equilibrium Review Questions
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Lab: Determination of the Ka
for a Weak Acid
Lab: Acid-Base Titration
Acids and Bases I Review
Problems
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Fourth Quarter
Ka and Kb
Hydrolysis of salts
Acid / base strength explained by
molecular structure
Acids and Bases II / Ksp (Chapter 17)
 Acid / Base Titrations
 Buffers and buffer calculations
 Solubility Product constant (Ksp)
 Factors that affect solubility
Thermodynamics (Chapter 19)
 Spontaneous reactions
 Entropy and the 2nd Law of
Thermodynamics
 Gibb’s Free Energy
 Free energy and the equilibrium constant
Electrochemistry (Chapter 20)
 Oxidation numbers
 Balancing REDOX reactions and writing ½
reactions
 Voltaic cells
 Using the Reduction Potential Table to
predict oE
 Electrolysis: electroplating, electrolysis of
a molten salt, electrolysis of an aqueous
salt
 Free energy and REDOX reactions
 EMF under nonstandard conditions
 Batteries and fuel cells
 Corrosion and corrosion prevention
Nuclear Chemistry / Organic Chemistry
(Chapters 21 & 25)
 Types of radioactivity
 Half-lives and half-life calculations
 Writing nuclear reactions for alpha decay,
beta decay, electron capture and positron
emission
 Decay series
 Fission and fusion
 Naming hydrocarbons: alkanes, alkenes,
alkynes, cycloalkanes
 Naming and properties of functional
groups: alcohols, aldehydes, ethers,
carboxylic acids, amines, ketones
 Organic reactions: combustion, addition,
substitution, addition polymerization,
condensation polymerization, esterification,
saponification
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Lab: Determination of the
Solubility Product of an Ionic
Compound
Lab: Preparation and Properties
of Buffers
Acids and Bases II / Ksp
Review Problems
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Thermodynamics Review
Questions
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Lab: Electroplating
Voltaic cells worksheet
Electrochemistry Review
questions
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Lab: Synthesis of a Bio-Fuel
Nuclear Review Questions
Organic Reactions worksheet