Summary of Part A and Part B on the AP Chemistry Exam



Summary of Part A and Part B on the AP Chemistry Exam

YEAR PART A PART B

2006 Solution Equilibrium, Ksp (2) Thermodynamics – calc Ksp

(3) Combustion Analysis – Empirical Formula

2005 Acid-Base Equilibrium, Ka (2) Combustion Analysis – Kf – Funct. Groups

(3) Kinetics – Orders & Rates

2004 Solution Equilibrium, Ksp (2) Stoichiometry - Thermodynamics

(3) Reaction Kinetics

2003 Acid-Base Equilibrium, Kb (2) Gases - Stoichiometry

(3) Kintics – rate laws

2002 Acid-Base Equilibrium, Ka (2) Limiting Reagent – EC cell

(3) Gases – Thermo - Structure

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

(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 # DESCRIPTION

2006 5 Analysis of compounds via lab results

6 IMF – Reaction pathways

7 Lewis Structures & geometry

8 Atomic properties of element 119

2005 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

2004 5 Qual analysis

6 Electrochemical cell

7 Phases of halogens – melting pt. – molec. shapes - solubilities

8 Lewis structures and prop. of CO and CO2

2003 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

2002 5 Thermo – Enthalpy of neutralization

6 Atomic size – ionization energy – bond energy – boiling pt.

7 Kinetics of ozone – rate laws

8 Thermo - kinetics

2001 5 Solution Properties

6 Reaction Types - Kinetics - Reaction Rates & Order

7 Electrochemical Cells

8 Intermolecular Forces

2000 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

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 LeChâtelier’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, ∆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.

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. ∆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.

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. ∆S˚, ∆G˚, ∆H˚, and spontaneity.

9 Kinetic Molecular Theory. Atomic explanations of gas observations.

1992 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.

1991 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.

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 ∆S˚, ∆G˚, ∆H˚,.

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

................
................

In order to avoid copyright disputes, this page is only a partial summary.

Google Online Preview   Download