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AP CHEMISTRY SYLLABUS
A. INTRODUCTION
1. This course meets 15, forty-three minute periods every two weeks with eleventh
and twelfth graders.
2. Students are expected to spend one to two hours per night on homework and
studying.
3. Students receive one credit with the grades weighted as follows: A-5, B-4, C-3,
D-1, F-0.
4. The following grading scale is used:
A 100%-92%
B 91%-83%
C 82%-72%
D 71%-61%
F 60%-0%
5. The grades are determined by total points on tests, problem sets and lab reports.
6. The textbook used is Chemistry, 8th edition, by Whitten, Davis, Peck, and Stanley,
Thomson Brooks/Cole Publishing, 2007.
7. The main laboratory manual is Laboratory Experiments for Advanced Placement
Chemistry, 2nd edition, by Sally Ann Vanderbrink, Ph.D., Flinn Scientific, Inc.,
2006.
a. Most of the 26 experiments in this manual are used.
b. Experiments from other manuals are also used as I feel are necessary.
c. Students also do a number of computer generated experiments from the
Pasco set of experiments.
8. An average of two periods out of eight each week are spent by the student on
laboratory experiments. In addition, numerous teacher demonstrations are shown
throughout the year, particularly as an introduction to each unit. Students work in
groups of two in the laboratory. Approximately, fifteen lab reports are submitted
by each student during the year with some reports including two or more related
labs together. Students are encouraged to share their thoughts on the laboratory
experiment during pre and post lab discussions, but are to do their own individual
lab reports. A portfolio of individual lab reports will then be kept by each student
after the reports are graded. The laboratory report includes the following: Title,
Purpose, Theory, Procedure, Data, Graphs, Calculations, Conclusion.
9. Problem Sets for each unit have been set up. These are completed by the students
for every unit, and consist of released Multiple Choice Questions and Free
Response Questions over the last ten years.
10. Before the AP Exam in the spring, I spend five, two hour evening sessions and
one double period day session reviewing with the students taking the test. We
review the problem sets to each unit. Afterwards, the students are given a sample
AP Chemistry Exam, and then we discuss any questions they have.
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B. OBJECTIVES AND EXPERIMENTS
Unit I. Review Basic Information
1. Define chemistry and related terms.
2. Make conversions within the Metric System.
3. Perform calculations on a calculator including scientific notation, logarithms, and
natural logarithms.
4. Express the limitation of an instrument.
5. Assign the correct number of significant figures to a measurement and to a
derived quantity.
6. Construct a graph of best fit manually and on the computer.
7. Interpret information from a graph.
8. Solve problems using the factor label method.
9. Write the Electron Shell Configuration for any atom using various methods.
10. Relate the Electron Shell Configuration and Periodic Table to the properties of
elements.
11. Write the formulas, names, and structural formulas for various inorganic and
organic compounds.
12. Define terms using the mole theory.
13. Solve problems using the mole theory.
14. Prepare a solution of known molarity.
15. Balance equations by trial and error.
16. Observe various redox reactions.
17. Balance redox reactions by the Change in Oxidation Number (CON) and Half
Reaction (HR) Methods.
18. Solve problems using formulas and the derivation of formulas.
19. Write a proper lab report.
Experiments
1. Precision and Accuracy
2. Preparing a Solution of Known Molarity
3. Analysis of Silver in a Metal Alloy
4. Gravimetric Analysis of a Metal Carbonate
Unit II. Atomic Theory, Spectra, Periodic Trends
1. Discuss the Atomic Theories of Dalton, Thomson, Rutherford, Bohr, and BohrSommerfeld.
2. Discuss the Modern Atomic Theory (Quantum Mechanics).
3. Relate the different photons of light to frequency, wavelength, and energy.
4. Relate the atomic spectra and the periodicity of an atom to its electron shell
configuration.
5. Make calculations using c= λν and E=hν.
6. Assign quantum numbers to any electron in an atom.
7. Explain the periodic trends in atoms with respect to atomic radius, ionic radius,
ionization energy, electron affinity, and electronegativity.
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Experiments
1. Flame Tests
2. Measurement of Wavelengths of Light using Spectrum Tubes and a Spectrometer
3. Finding the Ratio of Moles of Reactants in a Chemical Reaction
Unit III. Nuclear Chemistry
1. Identify nuclear stability based on neutron to proton ratio.
2. Explain and calculate the mass defect for an atom as it relates to binding energy
using E=mc2 .
3. Define radioactivity and discuss its causes.
4. Distinguish between alpha, beta, gamma and other types of radiation.
5. Explain induced radioactivity.
6. Discuss uses of radioactive substances and nuclear equipment using an Internet
Survey.
7. Calculate the rate of decay of a radioactive isotope.
Date objects based on their half life.
8. Explain fission and fusion using an Internet Survey.
9. Calculate the energy of a nuclear reaction using E=mc2.
Experiments
1. Demonstration of Radionuclides using a G-M Tube
2. Determination of the Empirical Formula of Silver Oxide
3. Analysis of Alum
Unit IV. Chemical Bonding
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2.
3.
4.
5.
6.
7.
Distinguish between ionic and covalent bonding.
Discuss properties of ionic and covalent compounds.
Illustrate bonding by the Lewis Electron Dot and Atomic Orbital Methods.
Explain and illustrate resonance forms.
Use formal charge to identify the correct Lewis structure.
Show exceptions to the octet rule.
Determine the molecular geometry of a molecule or polyatomic ion using the
VSEPR and Valence Bond (hybridization) Methods.
8. Use the Molecular Orbital Theory to explain exceptions to the octet rule, along
with the bond order, bond strength, and whether a molecule is paramagnetic or
diamagnetic.
9. Identify the number of sigma and pi bonds in a molecule.
Experiments
1. Electrical Conduction of Solutions
2. Chromatography
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Unit V. Mass Relations in Chemistry; Types of Reactions; Stoichiometry
1. Determine the atomic weight and molecular weight of an element and a
compound.
2. Find the atomic mass of an element.
3. Calculate the percent composition of a compound.
4. Determine the empirical and molecular formulas of a compound.
5. Make calculations from a chemical equation.
6. Find the limiting and excess reagent in a reaction.
7. Determine the percent yield of a reaction.
8. List various reaction types.
9. Predict the products of a reaction.
10. Distinguish between strong and weak acids and bases.
11. Write the net ionic reaction for all types of reactions.
12. Determine various calculations for solutions and titrations.
Experiments
1. Demonstration of Various Reaction Types
2. An Activity Series
3. Predicting the Products of Chemical Reactions and Writing Chemical Equations
Unit VI. Gases
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2.
3.
4.
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Define the four variables of a gas and their units.
Solve problems using the combined Gas Law Equation.
Solve problems using the Ideal Gas Equation (PV=nRT).
Find the partial pressure of a gas using Dalton’s Law.
Discuss the Kinetic Molecular Theory.
Solve problems using Graham’s Law of Effusion.
Distinguish between ideal and real gases.
Make calculations using Van der Waals Equation
Explain various environmental problems due to gases based on an Internet Survey.
Experiments
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2.
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Gas Law Demonstrations
Boyle’s Law
Determination of the Molar Mass of Volatile Liquids
Determination of the Molar Volume of a Gas
Unit VII. Solids and Liquids
1. Distinguish between solids and liquids.
2. Explain various types of intermolecular forces of attraction.
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3. Rank the strengths of the different intermolecular forces of attraction.
4. Discuss various properties of liquids and solids, including viscosity, surface
tension, capillary action, vapor pressure, normal melting point, normal boiling
point, and sublimation, based on an Internet Survey.
5. Calculate the amount of heat energy gained or lost in heating or cooling any
substance in any physical state or phase change.
6. Find the vapor pressure or molar heat of vaporization of a liquid using the
Clausius-Clapeyron Equation.
7. Define triple point, critical temperature and critical pressure.
8. Use phase diagrams to identify various states of a substance and other pertinent
information.
Experiments
1. Heat of Vaporization of a Liquid
2. Freezing and Melting of Water
3. Heat of Fusion
Unit VIII. Solutions
1. Define and describe solutions.
2. Express the concentration of a solution in percent composition by mass, molarity,
molality, and mole fraction.
3. Explain how temperature and pressure affect the solubility of various solutions.
4. Define the colligative properties.
5. Make calculations for various colligative properties for electrolytes and
nonelectrolytes.
6. Discuss colloids and their properties.
Experiments
1. Molar Mass by Freezing Point Depression
Unit IX. Thermodynamics and Thermochemistry
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2.
3.
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5.
Define thermodynamics and thermochemistry.
Explain the First Law of Thermodynamics.
Calculate q released or absorbed in a coffee cup calorimeter.
Define the enthalpy or heat of reaction.
Find the standard enthalpy change of a reaction from Hess’s Law using given
reactions, formation reactions and their standard heats of formation, and or bond
energies.
6. Explain the Third Law of Thermodynamics.
7. Define and discuss entropy, S.
8. Identify the possible prediction of the spontaneity of a system based on the standard
enthalpy change and the standard entropy change.
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9. Determine the standard entropy change of a reaction from Hess’s Law.
10. Explain the Second Law of Thermodynamics.
11. Define the Gibbs Free Energy, G, of a system.
12. Define the spontaneity of a system based on the standard free energy change.
13. Calculate the standard free energy change using the Gibbs Free Energy Equation
and from Hess’s Law.
Experiment
1. Thermodynamics---Enthalpy of Reaction and Hess’s Law
Unit X. Rates of Reaction
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2.
3.
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Define reaction rate.
Relate reaction rate to concentration.
Determine the rate law expression for a reaction.
Determine the order of a reactant in a reaction.
Relate reactant concentration and time to the reaction rate.
Discuss the Collision Theory and Transition State Theory for a reaction.
Explain activation energy for a reaction.
Discuss the effect of temperature and a catalyst on the reaction rate.
Define reaction mechanism and relate the rules that qualify it as a successfully
proposed mechanism for a reaction.
10. Explain the different types of catalysts.
Experiments
1. Kinetics of a Reaction
Unit XI. Gaseous Chemical Equilibrium
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3.
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Define an equilibrium reaction.
Write the equilibrium constant expression for an equilibrium reaction.
Determine the equilibrium constant for an equilibrium expression.
Determine the equilibrium partial pressure or concentration for any reactant or
product in an equilibrium reaction.
Use Le Chatelier’s Principle to discuss stresses on equilibrium systems.
Calculate the Keq in a system as it relates to free energy.
Calculate the Keq for an equilibrium system at a new temperature using the van’t
Hoff Equation.
Discuss industrial applications of gaseous equilibria.
Experiments
1. The Determination of Keq for FeSCN+2
2. Le Chatelier’s Principle
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Unit XII. Equilibrium and the Solubility Product Constant
1. Define a slightly soluble compound.
2. Write the equilibrium expression for a slightly soluble compound using the Ksp.
3. Find the Ksp or the concentration of an ion using the equilibrium expression for a
slightly soluble compound.
4. Predict if a precipitate forms using the Ksp.
5. Determine the solubility of a compound using the Ksp.
6. Determine the effect of a common ion on solubility.
Experiment
1. Determination of the Solubility Product of an Ionic Compound
Unit XIII. Acids and Bases
1. Define an acid and base according to the Bronsted-Lowry, Arrhenius, and Lewis
Theories.
2. Derive Kw for water as Kw=[H3O+ ][OH- ].
3. Define an acid and base according to the ratio of the hydronium ion and hydroxide
ion concentrations, and also, the pH vs pOH.
4. Make calculations using various formulas to find the pH, pOH, hydronium or
hydrogen ion concentration, and the hydroxide ion concentration.
5. Distinguish between strong and weak acids and strong and weak bases.
6. Find the concentrations for all species in solution for strong acids, strong bases, and
soluble salts.
7. Find the equilibrium concentrations for all species in solution involving weak acids
or weak bases using expressions for Ka and Kb.
8. Find the pka or pkb and the percent dissociation for a weak acid or base.
9. Make use of the 5% Rule for weak acids, weak bases, and hydrolysis.
10. Determine if a soluble salt is neutral, acidic, or basic.
11. Distinguish between the equivalence point and the end point in a titration.
12. Review the four types of acid-base reactons.
13. Discuss the role of an indicator in a titration.
14. Define a buffer system and explain how one works.
15. Use the Henderson-Hasselbach Equation to find the pH of an acid buffer or pOH of
a base buffer.
16. Decide on choosing the correct buffer and determine its buffering capacity.
17. Define a titration curve.
18. Find the pH at any point in a titration of various types of acid-base reactions using
titration curves.
Experiments
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4.
Determine the Ka for Weak Acids
Acid-Base Titrations
Selecting Indicators for Acid-Base Reactions
Preparation and Properties of Buffer Solutions
Unit XIV. Oxidation and Reduction
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Define electrochemistry
Distinguish between voltaic and electrolytic Electrochemical Cells.
Identify the oxidation and reduction electrodes in an Electrochemical Cell.
Review balancing redox reactions by the half reaction method.
Write the cell notation for a voltaic cell.
Calculate the standard voltage for a voltaic cell from Eocell = Eoox +Eored
Distinguish between strong and weak oxidizing and reducing agents.
Determine the spontaneity of a redox reaction from Eocell.
Find the cell potential (voltage) at nonstandard conditions using the Nernst
Equation.
10. Relate the standard cell voltage, the standard free energy change, and the
equilibrium constant using various equations.
11. Discuss various commercial cells.
Experiments
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2.
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4.
Oxidation-Reduction Titrations
Electrochemical Cells
Electrolysis
Analysis of a Commercial Bleach
Unit XV. Representative Elements
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Discuss the metallurgy of various elements.
Survey various reactions of elements in Groups 1 and 2.
Explain the redox reactions of certain transition elements.
Determine the more stable cation for elements consisting of two or more valence
states.
List the properties of alloys.
Compare the reactivity of various nonmetals.
Discuss the preparation of various nonmetals.
List properties of hydrogen compounds and oxygen compounds of various
nonmetals.
Explain properties of oxoacids and oxoanions.
Experiments
1. Separation and Qualitative Determination of Cations and Anions
2. Preparation and Analysis of Tetraaminocopper II Sulfate Monohydrate
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Unit XVI. Organic Compounds
1. Review names, formulas, structural formulas, and condensed structural formulas for
alkanes, alkenes, alkynes, and the aromatics.
2. Discuss uses for various aromatics.
3. Distinguish between various organic compounds based on their structural groups
(acids, alcohols, ethers, esters, etc.)
4. Name and construct structural and condensed structural formulas for organic
compounds in #3.
5. Discuss the properties of organic compounds in #1 and #3 using an Internet Survey.
6. Discuss synthetic organic polymers.
Experiments
1. Synthesis, Isolation, and Purification of an Ester
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