AP Chemistry Syllabus
Text used: Chemistry by Zumdahl and Zumdahl, 5th ed., Houghton Mifflin Company, 2000.
ISBN: 0-395-98581-1.
Course Overview
AP Chemistry meets five times per week for 50 minutes. Prerequisites for this course include general level physical and biological
sciences, 2nd year algebra, honors chemistry, as well, pre-calculus or higher math course taken concurrently. This is a second year
chemistry course for motivated students who intend to pursue a career in science. The structure, properties, and behavior of matter are
examined theoretically and in the laboratory. College level text and labs are used. This course poses intellectual and laboratory
challenges to all students and is equivalent rigor of college level general chemistry and chemistry lab, and many college’s honors level
chemistry courses.
Course Goals and Philosophy
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Develop students’ ability to think critically to solve problems in science.
Allow students to attain an in depth knowledge of chemical phenomena.
To produce individuals who have mastered the use of various chemical equipment and techniques.
To gain the ability to make relevant observations and to analyze collected data qualitatively and quantitatively.
Effectively communicate results of various investigations verbally as well as in a formal written report.
To compile evidence of knowledge gain through experimentation and problem solving.
Course Grading Policy
Tests are given at the end of each unit. Quizzes and other formative assessments are given during the units. Labs are assessed mainly
through lab reports while part of the grade depends on technique and obtaining expected result. Select homework problems are
checked and graded for correctness.
Student’s grade is based on the following weighted categories:
Assessments (tests, quizzes) 75%
Labs & Projects 20%
Lab Points 5%
Schedule & Summary of Course Topics:
Unit 1: Foundations of Chemistry (3 days)
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Observations
Uncertainty in measurements
Basic calculations and significant figures (conversions, temperature, density, etc.)
Unit 2: Atom (5 days)
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Atomic theory (from early ideas to new)
Chemical Laws
Modern atomic structure
Isotopes and average atomic mass
Basic organization of the periodic table
Naming all compounds, including
o Simple compounds
o Binary ionic
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Type I
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Type II
o Binary covalent (type III)
o Polyatomic ions
o Acids
Unit 3: Stoichiometry (5 days)
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Mole, molar ratios, atomic masses, % composition
Determining molecular formula of compounds
Components of chemical equations
Balancing reactions
Stoichiometric relations
Limiting reactants
Unit 4: Chemical Reactions (6 days)
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Aqueous solution reactions
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Details on all types of chemical reactions, including special emphasis:
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Acid base reactions
Precipitation reactions
Oxidation reduction reactions
Balancing Redox reactions note: 5 days will be spent later in the course after student have a deeper understanding of
chemical relations
Unit 5: Gases (6 days)
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Gas laws and their originators
Combined gas law
Ideal gas law
Gas stoichiometry
Kinetic Molecular Theory
Diffusion and Effusion
Characteristics of real gases
Unit 6: Intro to Thermochemistry (8 days)
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Nature of energy
Enthalpy and Calorimetry
Hess’s Law
Standard Enthalpies of formation
Unit 7: Quantum Mechanics and Periodicity (7 days)
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Electromagnetic Radiation and Atomic Spectrum
Electron Configurations: Quantum Numbers, orbital shapes, and Aufbau Principle
Pauli exclusion principle, electron spin, and Hund’s rule
Valence electrons, core electrons, and shielding
Discovery of periodic trends
Modern Periodic Trends in atomic properties, including:
o Ionization energies (successive)
o Electron affinities
o Electronegativity
o Atomic radii
o Ionic radii
o Metallic properties
o Densities
Properties of families, including:
o Alkali metals
o Alkaline Earth metals
o Transition metals and varying oxidation numbers
o Lanthanide and actinide series
o Metalloids
o Nonmetals
o Noble Gases
Unit 8: Chemical Bonds (15 days)
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Types of Bonding
Bond Polarity
Lewis-dot Structures
o Octet rule and its exceptions
o Resonance
o Formal Charge
VSEPR Theory – Molecular Shapes
Hybridization of orbitals in bonding
Unit 9: States of Matter (6 days)
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Intermolecular Forces of liquids and solids, including:
o Dipole-Dipole interactions
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Hydrogen bonding
o London Dispersion forces
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Instantaneous dipoles
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polarizability
Liquids and their properties, including:
o Surface tension
o Capillary action
o Viscosity
o Vapor pressure and its relation to temperature
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Enthalpy of vaporization
Phase changes and phase diagrams including allotropic states
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Heating curves
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Enthalpy of fusion
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Supercooling
Molecular and Ionic Solids
o Network solids
o Crystal Structure
o Lattice Energy
Metallic bonding structure
o Packing arrangements and determination of density
o Alloys
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Interstitial
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Substitutional
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Unit 10: Properties of solutions (7 days)
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Solution formation energies
Effects on solubility, including
o Pressure effects
o Temperature effects
o Structural effects
Colligative Properties
o Vapor pressure of solutions and non-ideal solutions
o Boiling point elevation
o Freezing point depression
o Osmotic pressure
o Electrolyte solutions and van’t Hoff factor
Colloids and their properties, including
o Coagulation
o Tyndall effect
Unit 11: Kinetics (9 days)
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Reaction Rates
Rate Law
Integrated Rate Law
o Order of reactions
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Zero order
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First order
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Half-life reactions
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Second order
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Multiple reactant integrated rate law
Catalysts
o Heterogeneous
o Homogeneous
Unit 12: Chemical Equilibrium (24 days)
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Equilibrium Expression and Reaction Quotient
Le Chatelier’s Principle
Gaseous Equilibrium Kc, Kp
Acid-Base Equilibrium – Kw, Ka, Kb
o Calculating pH
o Polyprotic Acids
o Properties of Salts
o Properties of Oxides
o Buffers
o Titrations
Solubility Equilibrium – Ksp
o Qualitative Analysis
o Common ion effect
o Complex Ion formation and equilibrium
Unit 13: Spontaneity, Entropy, and Free Energy (12 days)
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Spontaneous processes and entropy
2nd Law of Thermodynamics
Effect of Temperature
Free Energy and chemical reactions
o Pressure effects
o Temperature effects
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Relation to K
Relation to work
Unit 14: Electrochemistry (11 days)
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Cell Potential
o Nernst Equation
Standard Reduction Potential
Corrosion
Electrolysis
Unit 15: Nuclear Chemistry (if time)
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Types of Decay
Half-Life
Fission
Fusion
Unit 16: Organic Chemistry Basics (if time)
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Hydrocarbons
Functional Groups
Polymers
Review
Additional time before the AP Chemistry Exam is used for reviewing and assessing knowledge
Post Exam
Students develop, initiate, and present a research project in contemporary chemistry topics.
AP Chemistry Labs
This course stresses hands-on laboratory experiments with emphasis on lab safety. At the end of lessons prior to labs, preparatory
instructions and special techniques are explained in detail to the students. This becomes one of the most important safety precautions,
knowledge of intention in the laboratory. A pre-lab assignment is a requirement of each student to complete and understand before
each lab is conducted. This is especially important for safety and also allows the students to foresee and predict potential errors. All of
the experiments conducted in the laboratory require collaboration with other students (typically with a partner). Not only collaboration to
complete the experimental procedure in the allotted time but to also to interpret and analyze data obtained. Following each experiment,
a debrief session is conducted. This is typically conducted in larger groups or as an entire class to share results with others and to aid
in interpreting the data properly. Additionally, each lab is required to have a formal write-up presenting materials, procedure,
data/analysis, and conclusion. The students are required to neatly organize data and manipulate it using Microsoft Excel. Conclusions
should reflect students’ understanding of their results verses expected results, as well as detailed insight and explanation of sources of
error. Lab reports are graded and returned to students in sheet protectors. Major errors or misinterpretations on lab reports are to be
corrected and resubmitted. Students are additionally required to compile the lab reports in a separate lab binder. This binder allows
students to reflect on laboratory experiments conducted as well as serve as evidence of having conducted the experiments.
These labs constitute an average of one class period per week. Labs that require more than one class period are completed by the
students after school or before school on the next day. Some suggested labs for AP chemistry are performed in honors chemistry
(prerequisite). Some of the following labs are from:
Slowinski, Emit J., et al. Chemical Principles in the Laboratory. 5th ed.
Labs Conducted:
1. Determination of the chemical formula of an unknown hydrate.
2. Determination of a chemical formula.
3. Determination of an unknown chloride by AgNO3 titration
4. Determination of the molar mass of a volatile gas (Dumas)
5. Calorimeter Lab (determination of a calorimeter constant – Hess’s Law)
6. Determination of molar mass by freezing point depression
7. Vapor Pressure of water lab
8. Kinetics: Iodination of acetone lab
9. Kinetics: Iodine clock reaction
10. Le Chateleir’s Principle (applying principle to different systems)
11. Determine Equilibrium constant of FeSCN using Beer’s Law and Spec 20
12. Standardization of a base (NaOH)
13. Molar mass of an unknown acid by titration
14. Buffers Lab w/ pH meters (Determining buffer capacity)
15. Determining free energy based on the solubility product of Ksp of Ca(OH)2
16. Electrochemical cells (using Faraday’s Law)
17. Using Nernst Equation with electrode potentials
18. Formation of an Ester (aspirin)