Commentary from a student who maintained an A+ in AP Chemistry: Having taken the AP Chemistry exam, I can tell you that your nightmarish expectations are true, and that the test is very hard. I didn't work on many sample questions and was therefore ill prepared for the difficulty (I still got a 4; either the graders were on crack or I was very lucky). Do yourselves a favor and pick up a preparation book.
The date for this year's test can be found at College Board Online. Click on "College Board Test Dates" for all SAT and AP tests.
Remember, you can never prepare too much for this exam. Check out the chemistry links to find sites with useful chemistry information. Also, you might want to check out these AP Chemistry preparation books:
AP CHEMISTRY EXAMINATION (3rd edition)
"Multiple choice questions in preparation for the AP Chemistry Examination." Published by D & S Marketing Systems, Inc. Note: These books can only be bought in bulk. Ask your teacher to contact the company about books for the whole class.CRACKING THE AP CHEMISTRY
"Our focus is on the real APs, and on just the things you need to know to score high." Published by Princeton Review $16.00
For your reference, here are the topics that the AP exam covers (thanks to Ziawei for finding and providing this list):
I. Structure of Matter
A. Atomic theory and atomic structure
1. Evidence for the atomic theory
2. Atomic masses; determination by chemical and physical
means
3. Atomic number and mass number; isotopes
4. Electron energy levels: atomic spectra, quantum numbers,
atomic orbitals
5. Periodic relationships including, for example, atomic
radii, ionization energies, electron affinities, oxidation
states
B. Chemical bonding
1.Binding forces
a. Types: ionic, covalent, metallic, hydrogen bonding, van
der Waals
(including London dispersion forces)
b. Relationships to states, structure, and properties of
matter
c. Polarity of bonds, electronegativities
2.Molecular models
a. Lewis structures
b. Valence bond: hybridization of orbitals, resonance,
sigma and pi bonds
c. VSEPR
3.Geometry of molecules and ions, structural isomerism of
simple organic molecules and coordination complexes; dipole
moments of molecules; relation of properties to structure
C. Nuclear chemistry: nuclear equations, half-lives, and
radioactivity; chemical applications
II. States of Matter
A. Gases
1.Laws of ideal gases
a. Equation of state for an ideal gas
b. Partial pressures
2.Kinetic-molecular theory
a. Interpretation of ideal gas laws on the basis of this
theory
b. Avogadro's hypothesis and the mole concept
c. Dependence of kinetic energy of molecules on temperature
d. Deviations from ideal gas laws
B. Liquids and solids
1.Liquids and solids form the kinetic-molecular viewpoint
2.Phase diagrams of one-component systems
3.Changes of state, including critical points and triple
points
4.Structure of solids; lattice energies
C. Solutions
1.Types of solutions and factors affecting solubility
2.Methods of expressing concentration (The use of normalities
is not tested.)
3.Raoult's law and colligative properties (nonvolatile
solutes); osmosis
4.Non-ideal behavior (qualitative aspects)
III. Reactions
A. Reaction types
1.Acid-base reactions; concepts of Arrhenius, Br�nsted-Lowry,
and Lewis; coordination complexes; amphoterism
2.Precipitation reactions
3.Oxidation-reduction reactions
a. Oxidation number
b. The role of the electron in oxidation-reduction
c. Electrochemistry: electrolytic and galvanic cells;
Faraday's laws; standard half-cell potentials; Nernst
equation; prediction of the direction redox reactions
B. Stoichiometry
1.Ionic and molecular species present in chemical systems:
net ionic equations
2.Balancing of equations including those for redox reactions
3.Mass and volume relations with emphasis on the mole
concept, including empirical formulas and limiting
reactants
C. Equilibrium
1.Concept of dynamic equilibrium, physical and chemical; Le
Chatelier's principle; equilibrium constants
2.Quantitative treatment
a. Equilibrium constants for gaseous reactions: Kp, Kc
b. Equilibrium constants for reactions in solution
(1) Constants for acids and bases; pK; pH
(2) Solubility product constants and their application to
precipitation and the dissolution of slightly soluble
compounds
(3) Common ion effect; buffers; hydrolysis
D. Kinetics
1.Concept of rate of reaction
2.Use of differential rate laws to determine order of
reaction and rate constant from experimental data
3.Effect of temperature change on rates
4.Energy of activation; the role of catalysts
5.The relationship between the rate-determining step and a
mechanism
E. Thermodynamics
1.State functions
2.First law: change in enthalpy; heat of formation; heat of
reaction; Hess's law; heats of vaporization and fusion;
calorimetry
3.Second law: entropy; free energy of formation; free energy
of reaction; dependence of change in free energy on
enthalpy and entropy changes
4.Relationship of change in free energy to equilibrium
constants and electrode potentials
IV. Descriptive Chemistry
Knowledge of specific facts of chemistry is essential for an
understanding of principles and concepts. These descriptive facts,
including the chemistry involved in environmental and societal issues,
should not be isolated from the principles being studied but should be
taught throughout the course to illustrate and illuminate the
principles. The following areas should be covered:
1.Chemical reactivity and products of chemical reactions
2.Relationships in the periodic table: horizontal, vertical, and
diagonal with examples from alkali metals, alkaline earth metals,
halogens, and the first series of transition elements
3.Introduction to organic chemistry: hydrocarbons and functional groups
(structure, nomenclature, chemical properties). Physical and chemical
properties of simple organic compounds should also be included as
exemplary material for the study of other areas such as bonding,
equilibria involving weak acids, kinetics, colligative properties, and
stoichiometric determinations of empirical and molecular formulas.
V. Laboratory
The differences between college chemistry and the usual secondary school
chemistry course are especially evident in the laboratory work. The AP
Chemistry Examination includes some questions based on experiences and
skills students acquire in the laboratory: making observations of
chemical reactions and substances; recording data; calculating and
interpreting results based on the quantitative data obtained; and
communicating effectively the results of experimental work.
Colleges have reported that some AP candidates, while doing well on the
examination, have been at a serious disadvantage because of inadequate
laboratory experience. Meaningful laboratory work is important in
fulfilling the requirements of a college-level course of a laboratory
science and in preparing a student for sophomore-level chemistry courses
in college.
Because chemistry professors at some institutions ask to see a record of
the laboratory work done by an AP student before making a decision about
granting credit, placement, or both, in the chemistry program, students
should keep reports of their laboratory work that can be readily
reviewed.
Chemical Calculations
The following list summarizes types of problems either explicitly or
implicitly included in the topic outline. Attention should be given to
significant figures, precision of measured values, and the use of
logarithmic and exponential relationships. Critical analysis of the
reasonableness of results is to be encouraged.
1.Percentage composition
2.Empirical and molecular formulas from experimental data
3.Molar masses from gas density, freezing-point, and boiling-point
measurements
4.Gas laws, including the ideal gas law, Dalton's law, and Graham's law
5.Stoichiometric relations using the concept of the mole; titration
calculations
6.Mole fractions; molar and molal solutions
7.Faraday's law of electrolysis
8.Equilibrium constants and their applications, including their use for
simultaneous equilibria
9.Standard electrode potentials and their use; Nernst equation
10.Thermodynamic and thermochemical calculations
11.Kinetics calculations