Summary of Part A and Part B on the AP Chemistry Exam
YEAR
PART A
PART B
2006
Solution Equilibrium, Ksp
2005
Acid-Base Equilibrium, Ka
2004
Solution Equilibrium, Ksp
2003
Acid-Base Equilibrium, Kb
2002
Acid-Base Equilibrium, Ka
2001
Solution Equilibrium, Ksp
(2) Thermodynamics - Bond Energies
(3) Stoichiometry - Acid-Base titration & pH
2000
Gas Equilibrium
(2) Electrochemical Reactions
(3) Mass Percentage - Gas Stoichiometry - Titration
1999
Acid/Base
(2) Atomic Theory - Light Interactions
(3) Kinetics - Rates - Reaction Orders - Mechanisms
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
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 1
(2)
(3)
(2)
(3)
(2)
(3)
Thermodynamics – calc Ksp
Combustion Analysis – Empirical Formula
Combustion Analysis – Kf – Funct. Groups
Kinetics – Orders & Rates
Stoichiometry - Thermodynamics
Reaction Kinetics
(2)
(3)
(2)
(3)
Gases - Stoichiometry
Kintics – rate laws
Limiting Reagent – EC cell
Gases – Thermo - Structure
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
(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
Summary of Part D Questions on the AP Chemistry Exam
YEAR QUESTION #
2006
2005
2004
2003
2002
DESCRIPTION
5
Analysis of compounds via lab results
6
IMF – Reaction pathways
7
Lewis Structures & geometry
8
Atomic properties of element 119
5
Reactions of Gases – Solution ID from ppt data
6
Lewis structures – sigma and pi bonds
7
IMF and atomic structure on boiling, melting, and ionization
8
Thermodynamics and solutions
5
Qual analysis
6
Electrochemical cell
7
Phases of halogens – melting pt. – molec. shapes - solubilities
8
Lewis structures and prop. of CO and CO2
5
Spectroscopy – Beer’s Law
6
Acid rain – colligative prop. – ideal vs non-ideal gas - condenstation
7
Bond energies – reaction kinetics
8
organic structures – isomers – hybridization – bond types
5
Thermo – Enthalpy of neutralization
6
Atomic size – ionization energy – bond energy – boiling pt.
7
Kinetics of ozone – rate laws
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 2
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
2001
2000
1999
1998
1997
1996
1995
8
Thermo - kinetics
5
Solution Properties
6
Reaction Types - Kinetics - Reaction Rates & Order
7
Electrochemical Cells
8
Intermolecular Forces
5
Molar Mass by Freezing-Point Depression
6
Kinetics - Reaction Rates - Reaction Order
7
Isotopes - Electron Configuration - Ionization Energy - Molecular Structure
8
Acid-Base titration - Indicators
5
Lab Procedure - Gas Collection.
6
Thermodynamics.
7
Solution Properties.
8
Bonding and Molecular Structure.
5
Acid-Base titration curves.
6
Reaction kinetics; reaction orders.
7
LeChâtelier’s Principle.
8
Electrochemical cells.
9
Altitude and boiling point; copper-ammonia complex; molecular polarity; redox agents.
5
Molecular geometry and Lewis structures, polarity, group V fluorides.
6
Atomic/molecular structure related to ionization energies and radii.
7
Thermodynamics, ∆S˚, ∆G˚, LeChatelier’s Principle.
8
Nuclear decay process, mass defect, particle properties.
9
Lab process in determination of mass percent of sulfate in an unknown.
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.
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.
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 3
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
1994
1993
1992
1991
1990
5
Provide explanations for various physical and chemical phenomena.
6
Thermodynamics. ∆S˚, ∆G˚, ∆H˚, 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.
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. ∆S˚, ∆G˚, ∆H˚, and spontaneity.
9
Kinetic Molecular Theory. Atomic explanations of gas observations.
5
Rate law. LeChatlier’s 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.
5
Thermodynamics. Prediction of sign of ∆S for a reaction, predict sign of ∆H, 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.
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.
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 4
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
1989
1988
1987
1986
1985
1984
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.
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.
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 ∆S˚, ∆G˚, ∆H˚,.
9
Heisenberg Uncertainty Principle. Bohr theory of the hydrogen atom.
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.
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.
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.
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 5
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
Summary of Multiple Choice Questions on the AP Chemistry Exam
1984
Topic
Stoichiometry/Mole relationships
Gas Laws/Kinetic Theory
Atomic Theory
Bonding/Intermolecular Forces
Periodic Properties
Solutions/Phase Diagrams
Rates and Equilibrium
Precipitation
Acid/Base/Buffer
Problem Numbers
44, 45, 52, 73, 85
21, 23, 39, 50, 78
19, 22, 58, 66, 70
8, 9, 18, 40, 41, 51, 60, 80
43
27, 37, 54, 55, 59, 67, 69, 84
25, 26, 28, 36, 76, 82
68, 74
33, 48, 49, 53, 63, 64, 75
Oxidation/Reduction/Electrochemistry
14, 15, 16, 17, 20, 34, 46, 65, 79
General
Thermodynamics
Qualitative
Reactions
Nuclear
Organic
Laboratory
1, 2, 3, 4, 5, 6, 7, 24
29, 47, 56, 57, 83
10, 11, 12, 13, 31, 35
32, 42, 61, 71, 81
30, 38
77
62, 72
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 6
% of Exam
5.9
5.9
5.9
9.5
1.2
9.4
7.1
2.4
8.2
10.6
9.4
5.9
7.1
5.9
2.4
0.9
2.4
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
1989
Topic
Stoichiometry/Mole relationships
Gas Laws/Kinetic Theory
Atomic Theory
Bonding/Intermolecular Forces
Periodic Properties
Solutions/Phase Diagrams
Rates and Equilibrium
Precipitation
Acid/BaseBuffer
Oxidation/Reduction/Electrochemistry
Problem Numbers
23, 24, 25, 37, 39, 40, 67
16, 30, 32, 62
4, 5, 6, 7, 33
11, 12, 13, 14, 17, 42, 47, 59
1, 2, 3
15, 21, 26, 27, 43, 49, 50, 51, 71, 72
29, 54, 57, 58
65, 66
8, 9, 10, 19, 34, 35, 46, 55, 56, 74
20, 22, 60, 61, 75
General
28, 31, 44, 48, 73
6.7
Thermodynamics
Qualitative
Reactions
Nuclear
Organic
Laboratory
41, 53, 70
63, 64, 69
52
18, 38, 68
4.0
4.0
1.3
4.0
0.0
2.7
36, 45
% of Exam
9.3
5.3
5.3
10.7
4.0
13.3
5.3
2.7
13.3
6.7
1994
Stoichiometry/Mole relationships
Gas Laws/Kinetic Theory
Atomic Theory
Bonding/Intermolecular Forces
Periodic Properties
Solutions/Phase Diagrams
Rates and Equilibrium
Precipitation
Acid/BaseBuffer
Oxidation-Reduction/Electrochemistry
19, 33, 39, 56, 59, 71
24, 37, 40, 45, 64
1, 2, 3, 4, 27, 54
General
Thermodynamics
Qualitative/Descriptive
Nuclear
Organic
Laboratory
11, 12, 13, 23
25, 35, 58, 60
29, 41, 46, 52
21, 72
43
38, 42, 67, 69, 70
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
8.0
6.7
8.0
8, 9, 10, 15, 32, 34, 57, 62, 68
5, 6, 7, 14, 26, 28, 44, 47, 53
17, 30, 48, 49, 51, 73
65
16, 22, 31, 50, 55, 61, 66, 74
18, 20, 36, 63, 75
page 7
12.0
12.0
8.0
1.3
10.7
6.7
5.3
5.3
5.3
2.7
1.3
6.7
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html
Compiled by: Steve Haderlie
E-mail: hsteven@nebo.edu
page 8
Springville High School, 1205 East 900 South, Springville, UT 84663
WWW site: http://www.shs.nebo.edu/Faculty/Haderlie/apchem/apchem.html