Summary of Part A and Part B on the AP Chemistry Exam
(compiled by Steve Haderlie of Springville High School, UT, updated since 2000 by Robert Ause)
YEAR
PART A
PART B
2004 Ksp, solubility equilibrium
(2) Stoichiometry, limiting reactant, thermodynamics
(3) Kinetics, graphical reaction rate
2003
Acid/Base (2) Gas stoichiometry
(3) Kinetics
2002
Acid/Base
(2) Electrochemistry
(3) Stoichiometry of
Combustion Rxn; Structural Isomers
2001
Solution Equilibrium, Ksp
(2) Thermodynamics;
Equilibrium
(3) Acid Base Titration with
Lab components
2000
Gas Equilibrium
(2) Electrochemistry
(3) Stoichiometry; Redox
Titration
1998
Solution Equilibrium, Ksp
(2) Percent Composition,
Freezing Point, Collig Prop.
(3) Thermodynamics; Gas Law
1997
Acid/Base
(2) Electochemistry
(3) Kinetics
1996
Acid/Base
(2) Thermodynamics, bond
energies
(3) Solution concentrations
1995
Gas Equilibrium
(2) Gas stoichiometry, heat
of reaction
(3) Decomposition of solid
carbonates (stoichiometry)
1994
Precipitation
(2) Rate Law, Mechanisms
(3) Gas Laws
1993
Acid/Base
(2) Empirical formula,
colligative prop.
(3) Oxidation-Reduction
Titration
1992
Gas Equilibrium
(2) Electrochemistry,
thermodynamics
(3) Thermodynamics, enthalpy
and entropy
1991
Acid/Base, Buffer
(2) Empirical Formula,
Freezing pt
(3) Rate Law, Mechanisms
1990
Precipitation
(2) Gas Laws, Stoichiometry
(3) Thermodynamics
1989
Acid/Base
(2) Electrolysis
(3) Thermodynamics
1988
Gas Equilibrium
(2) Thermodynamics
(3) Electrolysis
1987
Acid/Base/Precipitation
(2) Rate laws
(3) Acid-base titration
1986
Acid/Base
(2) Redox/electrolysis
(3) Empirical formula
1985
Precipitation
(2) Redox/electrolysis
(3) Freezing pt depression;
Empirical formula
1984
Acid/base
(2) Rates
(3) Thermodynamics
1983
Gas Equilibrium
(2) Thermodynamics
(3) Acid-base titration
1982
Buffer solution
(2) Redox/electrolysis
(3) Empirical formula
1981
Gas Equilibrium
(2) Rates
(3) Redox titration
***Question 4 asks students to write 5 of 8 chemical equations based on the sentence descriptions given.*** (Link to Equation Writing Review)
Summary of Part D Questions (#s 5-8ff.) on the AP Chemistry Exam
YEAR
QUESTION #
DESCRIPTION
2004 5 Qualitative analysis laboratory
experiment (required)
6
Electrochemistry (required)
7
Description of chemical
phenomena using IMFs, solid structure, molecular geometry and polarity.
8
Structural principles, Lewis structures and qualitative gas
laws.
2003 5 Lab based concentration by
colorimeter/spectrophotometer Beer’s Law (required)
6
chemistry of everyday events (colligative properties, gas
ideality, condensation…) (required)
7
Thermodynamics
8
Structural principles around organic molecules.
2002
5 Calorimetry
Experiment (required)
6
Principles of chemical bonding and atomic structure (required)
7
Kinetics
8
Thermodynamics
2001
5 Properties of
Solutions; colligative, pH, precipitation; oxidizing agents; electrolytes (req)
6
Kinetics (required)
7
Electrochemistry
8
Principles of Bonding and intermolecular forces
2000
5 Lab Procedure:
Freezing Point Depression (required)
6 DG,
DH,
DS;
Rate laws (required)
7 Isotopes, electron configurations, IE’s, Lewis
Dots & molecular shapes
8 Acid-Base Titration; Choice of indicator
1999
5 Lab Procedure -
Gas Collection.
6 Thermodynamics.
7 Solution Properties.
8 Bonding and Molecular Structure.
1998
5
Acid-Base titration curves.
6 Reaction
kinetics; reaction orders.
7 LeChatelier’s
Principle.
8 Electrochemical
cells.
9 Altitude and
boiling point; copper-ammonia complex; molecular polarity; redox agents.
1997
5
Molecular geometry and Lewis structures, polarity, group V fluorides.
6 Atomic/molecular
structure related to ionization energies and radii.
7 Thermodynamics,
DS,
DG,
LeChatelier’s Principle.
8 Nuclear decay
process, mass defect, particle properties.
9 Lab process in
determination of mass percent of sulfate in an unknown.
1996
5
Gases, kinetic molecular theory, effusion.
6 Titration of
acid, effects of lab errors.
7 Keq, cell potentials and changes.
8 Kinetics, rate
law, rate constant.
9 Electronic
structure and bonding for differences in boiling point, polarity, bond length,
and group
VI fluorides.
1995
5
Conductivity explanation based on chemical bonding and/or atomic or
molecular structure.
6 Phase diagram
explanation.
7 Explanation in
terms of electronic structure and bonding.
8 Solubility,
thermodynamics explanation.
9 Chemical
reaction potential energy diagram explanation.
1994
5
Provide explanations for various physical and chemical phenomena.
6 Thermodynamics.
DS_,
DG_,
DH_,
and spontaneity.
7 Acid-base
titration curve.
8 Various
chemical principles. Ice melted with salt. Ammonia is a gas, water is a liquid
at room
temperature. Graphite is lubricant, diamond is abrasive. Vinegar in kettle used
for boiling,
fizzes.
9 Atomic
structure and bonding explanations.
1993
5
Explain reactions of H2SO4
using acid/base theory, oxidation-reduction, and bonding and/or
intermolecular forces.
6 Principles of
atomic structure: ionization energy, atomic radii, magnetic fields, and
geometry of
molecules.
7 Galvanic cell
diagram.
8 Thermodynamics.
DS_,
DG_,
DH_,
and spontaneity.
9 Kinetic
Molecular Theory. Atomic
explanations of gas observations.
1992
5
Rate law. LeChatlierÆs Principle, potential energy vs reaction
coordinate, distribution of
molecular energies.
6 Buffer
solutions. Identify buffer pairs,
preparation of buffer, manipulations with buffers.
7 Identification
of four bottles of substances. Describe tests to identify the four from each
other.
8 Physical
properties explained by atomic and molecular forces and/or intermolecular
forces.
9 Lewis dot
structures. Provide bond angles,
hybridization and dimerization.
1991
5
Thermodynamics. Prediction of sign of DS
for a reaction, predict sign of DH,
spontaneity based
on temperature.
6 Laboratory
experiment. Determine molecular
mass of liquid by vapor density method.
7 Electrolysis.
Anode, cathode reactions, explanation for observations on potential
changes as
concentration changes.
8 Physical
properties differences explained by structure and bonding.
9 Nuclear
chemistry. Alpha, beta particles
and fission and fusion.
1990
5
Bond lengths and angle measurements explained by structure and bonding
models.
6 Ionization
energy differences explained by atomic structure.
7 Factors which
affect reaction rates. Collision
theory, temperature, and catalysts.
8 Strength of
acids explanation.
9 Laboratory
experiment. Empirical formula
determined experimentally.
1989
5
Lewis dot structures and VSEPR theory for prediction of geometry, angles
and polarity.
6 Melting point
differences as explained by bonding principles.
7 Descriptive
chemistry. Identification of three
metals by chemical tests.
8 Reaction rates.
Explanation of changes in reaction rates when changes occur in
concentration,
temperature, surface area.
9 Nuclear
chemistry. Alpha, beta particles
and balanced nuclear equations. C-14
dating.
1988
5
Explain physical properties based on bonding and intermolecular forces.
6 LeChatlier's
principle.
7 Acid/Base
titration. Explain shape of
titration curve, how to select indicator, differences in shape
of curve with strong or weak acid and strong or weak base.
8 Phase diagram.
9 Laboratory
experiment. Heat (Enthalpy)
of neutralization for strong acid/strong base.
1987
5
Explanation of periodic properties based on atomic theory.
6 Electrolysis.
Prediction of anode and cathode reactions.
7 Explanation of
ionization of salts in water.
8 Thermodynamics.
Prediction of signs for DS_,
DG_,
DH_.
9 Heisenberg
Uncertainty Principle. Bohr theory of the hydrogen atom.
1986
5
Factors affecting the heat of formation.
6 Rate law and
reaction mechanisms.
7 Strength of
oxyacids.
8 Scientific
explanations for ice melting with salt, graphite conducting while diamond does
not, hot
air balloons must be bigger than helium balloons, carbon dioxide used on oil
fires instead of
water.
9 Explanation of
observation as zinc metal and copper metal are added to acids.
1985
5
Periodic properties explained by atomic structure.
6 Thermodynamics.
Explanation and prediction for enthalpy, entropy and free energy changes.
7 Laboratory
experiment. Preparation of salts.
8 Reaction rate,
rate law.
9 Melting point
trends explained by bonding and intermolecular forces.
1984
4
Scientific explanation for longer time to cook egg in Denver than New
York, burning coal leads
to acid rain, perspiring leads to cooling of body, antifreeze keeps engine from
freezing or
boiling.
5 Discuss role of
indicators in acid/base titrations.
6 Van der Waals
real gas law and explanation of a
and b constants.
7 Physical
differences between metals and non-metals.
Summary
of Multiple Choice Questions on the AP Chemistry Exam
1984
Topic Problem Numbers % of Exam
Stoichiometry/Mole
relationships
44, 45, 52, 73, 85
5.9
Gas Laws/Kinetic Theory
21, 23, 39, 50, 78
5.9
Atomic Theory
19, 22, 58, 66, 70
5.9
Bonding/Intermolecular Forces
8, 9, 18, 40, 41, 51, 60, 80
9.5
Periodic Properties
43
1.2
Solutions/Phase Diagrams
27, 37, 54, 55, 59, 67, 69, 84
9.4
Rates and Equilibrium
25, 26, 28, 36, 76, 82
7.1
Precipitation
68, 74
2.4
Acid/Base/Buffer
33, 48, 49, 53, 63, 64, 75
8.2
Oxidation/Reduction/Electrochemistry
14, 15, 16, 17, 20, 34, 46, 65, 79
10.6
General
1, 2, 3, 4, 5, 6, 7, 24
9.4
Thermodynamics
29, 47, 56, 57, 83
5.9
Qualitative
10, 11, 12, 13, 31, 35
7.1
Reactions
32, 42, 61, 71, 81
5.9
Nuclear
30, 38
2.4
Organic
77
0.9
Laboratory
62, 72
2.4
1989
Topic Problem Numbers % of Exam
Stoichiometry/Mole
relationships
23, 24, 25, 37, 39, 40, 67
9.3
Gas Laws/Kinetic Theory
16, 30, 32, 62
5.3
Atomic Theory
4, 5, 6, 7, 33
5.3
Bonding/Intermolecular Forces
11, 12, 13, 14, 17, 42, 47, 59
10.7
Periodic Properties
1, 2, 3
4.0
Solutions/Phase Diagrams
15, 21, 26, 27, 43, 49, 50, 51, 71, 72
13.3
Rates and Equilibrium
29, 54, 57, 58
5.3
Precipitation
65, 66
2.7
Acid/BaseBuffer
8, 9, 10, 19, 34, 35, 46, 55, 56, 74
13.3
Oxidation/Reduction/Electrochemistry
20, 22, 60, 61, 75
6.7
General
28, 31, 44, 48, 73
6.7
Thermodynamics
41, 53, 70
4.0
Qualitative
63, 64, 69
4.0
Reactions
52
1.3
Nuclear
18, 38, 68
4.0
Organic
0.0
Laboratory
36, 45
2.7
1994
Stoichiometry/Mole
relationships
19, 33, 39, 56, 59, 71
8.0
Gas Laws/Kinetic Theory
24, 37, 40, 45, 64
6.7
Atomic Theory
1, 2, 3, 4, 27, 54
8.0
Bonding/Intermolecular Forces
Periodic Properties
8, 9, 10, 15, 32, 34, 57, 62, 68
12.0
Solutions/Phase Diagrams
5, 6, 7, 14, 26, 28, 44, 47, 53
12.0
Rates and Equilibrium
17, 30, 48, 49, 51, 73
8.0
Precipitation
65
1.3
Acid/BaseBuffer
16, 22, 31, 50, 55, 61, 66, 74
10.7
Oxidation-Reduction/Electrochemistry
18, 20, 36, 63, 75
6.7
General
11, 12, 13, 23
5.3
Thermodynamics
25, 35, 58, 60
5.3
Qualitative/Descriptive
29, 41, 46, 52
5.3
Nuclear
21, 72
2.7
Organic
43
1.3
Laboratory
38, 42, 67, 69, 70
6.7
