Documentation :: Teachers :: Science Standards Alignments :: Alignment with AP® Chemistry Standards
According to the College Board website, “AP® Chemistry is an introductory college-level chemistry course. Students cultivate their understanding of chemistry through inquiry-based investigations as they explore topics like atomic and molecular structure, chemical reactions, kinetics, equilibrium, and thermodynamics.”
The following quizzes at ChemQuiz.net align with the AP® Chemistry Course and Exam Description [PDF]:
Unit 1: Atomic Structure and Properties
1.1 Moles and Molar Mass
Calculate quantities of a substance or its relative number of particles using dimensional analysis and the mole concept.
1.2 Mass Spectra of Elements
Explain the quantitative relationship between the mass spectrum of an element and the masses of the element’s isotopes.
1.3 Elemental Composition of Pure Substances
Explain the quantitative relationship between the elemental composition by mass and the empirical formula of a pure substance.
1.4 Composition of Mixtures
Explain the quantitative relationship between the elemental composition by mass and the composition of substances in a mixture.
1.5 Atomic Structure and Electron Configuration
Represent the ground-state electron configuration of an atom of an element or its ions using the Aufbau principle.
1.6 Photoelectron Spectroscopy
Explain the relationship between the photoelectron spectrum of an atom or ion and:
i. The ground-state electron configuration of the species.
ii. The interactions between the electrons and the nucleus.
1.7 Periodic Trends
Explain the relationship between trends in atomic properties of elements and electronic structure and periodicity.
1.8 Valence Electrons and Ionic Compounds
Explain the relationship between trends in the reactivity of elements and periodicity.
Unit 2: Compound Structure and Properties
2.1 Types of Chemical Bonds
Explain the relationship between trends in the reactivity of elements and periodicity.
2.5 Lewis Diagrams
Represent a molecule with a Lewis diagram.
2.7 VSEPR and Hybridization
Based on the relationship between Lewis diagrams, VSEPR theory, bond orders, and bond polarities:
i. Explain structural properties of molecules.
ii. Explain electron properties of molecules.
Unit 3: Properties of Substances and Mixtures
3.1 Intermolecular and Interparticle Forces
Explain the relationship between the chemical structures of molecules and the relative strength of their intermolecular forces when:
i. The molecules are of the same chemical species.
ii. The molecules are of two different chemical species.
3.3 Solids, Liquids, and Gases
Represent the differences between solid, liquid, and gas phases using a particulate-level model.
3.4 Ideal Gas Law
Explain the relationship between the macroscopic properties of a sample of gas or mixture of gases using the ideal gas law.
3.7 Solutions and Mixtures
Calculate the number of solute particles, volume, or molarity of solutions.
3.10 Solubility
Explain the relationship between the solubility of ionic and molecular compounds in aqueous and nonaqueous solvents, and the intermolecular interactions between particles.
3.12 Properties of Photons
Explain the properties of an absorbed or emitted photon in relationship to an electronic transition in an atom or molecule.
3.13 Beer-Lambert Law
Explain the amount of light absorbed by a solution of molecules or ions in relationship to the concentration, path length, and molar absorptivity.
Unit 4: Chemical Reactions
4.2 Net Ionic Equations
Represent changes in matter with a balanced chemical or net ionic equation:
i. For physical changes.
ii. For given information about the identity of the reactants and/or product.
iii. For ions in a given chemical reaction.
4.3 Representations of Reactions
Represent a given chemical reaction or physical process with a consistent particulate model.
4.5 Stoichiometry
Explain changes in the amounts of reactants and products based on the balanced reaction equation for a chemical process.
4.7 Types of Chemical Reactions
Identify a reaction as acid-base, oxidation-reduction, or precipitation.
4.9 Oxidation-Reduction (Redox) Reactions
Represent a balanced redox reaction equation using half-reactions.
Unit 5: Kinetics
5.1 Reaction Rates
Explain the relationship between the rate of a chemical reaction and experimental parameters.
5.2 Introduction to Rate Law
Represent experimental data with a consistent rate law expression.
5.3 Concentration Changes Over Time
Identify the rate law expression of a chemical reaction using data that show how the concentrations of reaction species change over time.
Unit 6: Thermochemistry
6.4 Heat Capacity and Calorimetry
Calculate the heat q absorbed or released by a system undergoing heating/cooling based on the amount of the substance, the heat capacity, and the change in temperature.
6.5 Energy of Phase Changes
Explain changes in the heat q absorbed or released by a system undergoing a phase transition based on the amount of the substance in moles and the molar enthalpy of the phase transition.
6.6 Introduction to Enthalpy of Reaction
Calculate the heat q absorbed or released by a system undergoing a chemical reaction in relationship to the amount of the reacting substance in moles and the molar enthalpy of reaction.
6.7 Bond Enthalpies
Calculate the enthalpy change of a reaction based on the average bond energies of bonds broken and formed in the reaction.
6.8 Enthalpy of Formation
Calculate the enthalpy change for a chemical or physical process based on the standard enthalpies of formation.
6.9 Hess’s Law
Represent a chemical or physical process as a sequence of steps.
Explain the relationship between the enthalpy of a chemical or physical process and the sum of the enthalpies of the individual steps.
Unit 7: Equilibrium
7.3 Reaction Quotient and Equilibrium Constant
Represent the reaction quotient Qc or Qp, for a reversible reaction, and the corresponding equilibrium expressions Kc = Qc or Kp = Qp.
7.4 Calculating the Equilibrium Constant
Calculate Kc or Kp based on experimental observations of concentrations or pressures at equilibrium.
7.5 Magnitude of the Equilibrium Constant
Explain the relationship between very large or very small values of K and the relative concentrations of chemical species at equilibrium.
7.7 Calculating Equilibrium Concentrations
Identify the concentrations or partial pressures of chemical species at equilibrium based on the initial conditions and the equilibrium constant.
7.9 Introduction to Le Châtelier’s Principle
Identify the response of a system at equilibrium to an external stress, using Le Châtelier’s principle.
7.10 Reaction Quotient and Le Châtelier’s Principle
Explain the relationships between Q, K, and the direction in which a reversible reaction will proceed to reach equilibrium.
7.11 Introduction to Solubility Equilibria
Calculate the solubility of a salt based on the value of Ksp for the salt.
Unit 8: Acids and Bases
8.1 Introduction to Acids and Bases
Calculate the values of pH and pOH, based on Kw and the concentration of all species present in a neutral solution of water.
8.2 pH and pOH of Strong Acids and Bases
Calculate pH and pOH based on concentrations of all species in a solution of a strong acid or a strong base.
8.3 Weak Acid and Base Equilibria
Explain the relationship among pH, pOH, and concentrations of all species in a solution of a monoprotic weak acid or weak base.
8.4 Acid-Base Reactions and Buffers
Explain the relationship among the concentrations of major species in a mixture of weak and strong acids and bases.
Unit 9: Thermodynamics and Electrochemistry
9.1 Introduction to Entropy
Identify the sign and relative magnitude of the entropy change associated with chemical or physical processes.
9.2 Absolute Entropy and Entropy Change
Calculate the standard entropy change for a chemical or physical process based on the absolute entropies (standard molar entropies) of the species involved in the process.
9.3 Gibbs Free Energy and Thermodynamic Favorability
Explain whether a physical or chemical process is thermodynamically favored based on an evaluation of ΔG°.
9.5 Free Energy and Equilibrium
Identify the signExplain whether a process is thermodynamically favored using the relationships between K, ΔG°, and T.
9.8 Galvanic (Voltaic) and Electrolytic Cells
Explain the relationship between the physical components of an electrochemical cell and the overall operational principles of the cell.
9.9 Cell Potential and Free Energy
Explain whether an electrochemical cell is thermodynamically favored, based on its standard cell potential and the constituent half-reactions within the cell.
9.10 Cell Potential Under Nonstandard Conditions
Explain the relationship between deviations from standard cell conditions and changes in the cell potential.
9.11 Electrolysis and Faraday’s Law
Calculate the amount of charge flow based on changes in the amounts of reactants and products in an electrochemical cell.