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AP Chemistry

College-level chemistry covering atomic structure, bonding, reactions, kinetics, thermodynamics, equilibrium, and electrochemistry. Aligned to the College Board AP Chemistry Course and Exam Description.

14 Units

45-60 minutes per unit

What You Will Learn

College Board Aligned

All nine AP Chemistry CED units — from atomic structure through electrochemistry and applications.

Quantitative Rigor

Stoichiometry, equilibrium calculations, thermodynamic analysis, and electrochemistry at college level.

College Credit Potential

A qualifying AP exam score can earn 4-8 college credits at most universities.

All Units

Atomic Structure and Electron Configuration

Explore the quantum mechanical model of the atom, electron configurations, and the periodic trends that emerge from atomic structure.

•Describe the evolution of atomic models from Dalton to the quantum mechanical model
•Write ground-state electron configurations using subshell and orbital notation
•Explain periodic trends (atomic radius, ionization energy, electronegativity) in terms of nuclear charge and shielding
+1 more objectives

Compound Structure and Bonding

Investigate ionic, covalent, and metallic bonding, Lewis structures, VSEPR theory, and how molecular geometry determines molecular properties.

•Distinguish ionic, covalent, and metallic bonding based on electronegativity differences and atomic properties
•Draw Lewis structures including resonance structures and formal charges
•Predict molecular geometries using VSEPR theory
+1 more objectives

Intermolecular Forces and States of Matter

Examine how intermolecular forces govern the properties of solids, liquids, and gases, and how phase diagrams encode the behavior of substances across temperature and pressure.

•Identify and rank intermolecular forces (London dispersion, dipole-dipole, hydrogen bonding, ion-dipole) based on molecular structure
•Explain physical properties (boiling point, viscosity, surface tension, vapor pressure) in terms of IMFs
•Describe the structures of ionic, metallic, molecular, and covalent network solids
+1 more objectives

Chemical Reactions and Net Ionic Equations

Classify and predict chemical reactions, write net ionic equations, and analyze oxidation-reduction reactions through half-reaction methods.

•Classify reactions as combination, decomposition, single-replacement, double-replacement, or combustion
•Write complete and net ionic equations for reactions in aqueous solution
•Assign oxidation states and identify oxidizing and reducing agents in redox reactions
+1 more objectives

Stoichiometry and the Mole Concept

Master the mole as chemistry's central counting unit, and apply stoichiometric reasoning to calculate masses, volumes, yields, and compositions of chemical reactions.

•Use Avogadro's number to convert between moles, mass, particles, and volume of gases
•Determine empirical and molecular formulas from experimental data
•Perform stoichiometric calculations including limiting reagent, theoretical yield, and percent yield
+1 more objectives

Gases and the Ideal Gas Law

Develop a quantitative model of gas behavior through the ideal gas law and kinetic molecular theory, and explore where real gases deviate from ideal predictions.

•Apply the ideal gas law and combined gas law to predict gas behavior under changing conditions
•Use Dalton's law of partial pressures in mixtures of gases
•Explain gas properties using the postulates of kinetic molecular theory
+1 more objectives

Solutions and Colligative Properties

Explore how solutions form, how concentration is measured and manipulated, and how dissolved solutes alter the physical properties of solvents through colligative effects.

•Explain solution formation in terms of intermolecular forces and thermodynamics
•Calculate solution concentrations using molarity, molality, and mole fraction
•Apply Henry's Law, Raoult's Law, and the solubility rules to predict solution behavior
+1 more objectives

Thermochemistry: Energy in Chemical Reactions

Quantify the energy changes in chemical reactions through calorimetry, Hess's Law, standard enthalpies, and bond energy calculations.

•Apply the first law of thermodynamics to chemical systems and distinguish between heat and work
•Calculate heat transfer using q = mcΔT and interpret calorimetry data
•Use Hess's Law and standard enthalpies of formation to calculate reaction enthalpies
+1 more objectives

Thermodynamics: Entropy, Free Energy, and Spontaneity

Investigate why reactions proceed spontaneously by analyzing entropy changes, Gibbs free energy, and the fundamental connection between thermodynamics and equilibrium.

•Explain entropy as a measure of dispersal of energy and matter, and predict the sign of ΔS for physical and chemical processes
•State the second and third laws of thermodynamics and apply them to predict spontaneity
•Calculate Gibbs free energy and use it to predict spontaneity under different conditions
+1 more objectives

Reaction Kinetics: Rates and Mechanisms

Investigate how fast chemical reactions occur and why, through rate laws, reaction mechanisms, collision theory, the Arrhenius equation, and the role of catalysis.

•Determine rate laws from experimental data and calculate rate constants with appropriate units
•Integrate rate laws to find concentration-time relationships for zero-, first-, and second-order reactions
•Explain the molecular basis for reaction rates using collision theory and transition state theory
+2 more objectives

Chemical Equilibrium

Develop a rigorous understanding of dynamic chemical equilibrium, equilibrium constants, the reaction quotient, ICE table calculations, and Le Chatelier's principle.

•Write equilibrium constant expressions (Kc and Kp) from balanced equations and manipulate K for reversed or combined reactions
•Use the reaction quotient Q to predict the direction a system will shift to reach equilibrium
•Solve ICE table problems to find equilibrium concentrations
+1 more objectives

Acids, Bases, and Buffers

Master acid-base theory from Brønsted-Lowry definitions through pH calculations, buffer design, and titration curves — the chemistry that underlies biology, industry, and environmental science.

•Apply Brønsted-Lowry and Lewis acid-base definitions and identify conjugate pairs
•Calculate pH, pOH, [H⁺], and [OH⁻] for strong and weak acids and bases
•Use Ka and Kb values to find equilibrium concentrations and percent ionization in weak acid/base solutions
+2 more objectives

Electrochemistry: Galvanic Cells and Electrolysis

Explore how spontaneous redox reactions generate electrical energy in galvanic cells and how electrical energy drives non-spontaneous reactions in electrolytic cells, with quantitative analysis through the Nernst equation.

•Describe the components and operation of a galvanic cell and predict cell potentials from standard reduction potentials
•Calculate standard cell potential E°cell and relate it to ΔG° and K
•Apply the Nernst equation to calculate cell potential under non-standard conditions
+1 more objectives

Chemistry in Context: Spectroscopy, Chromatography, and Green Chemistry

Connect chemistry concepts to real-world analytical techniques and sustainable practices — spectroscopy, chromatography, and green chemistry principles that define modern scientific and industrial chemistry.

•Explain how spectroscopic techniques (IR, UV-Vis, NMR, mass spectrometry) provide structural and compositional information
•Describe the principles behind chromatographic separation methods and interpret chromatography data
•Evaluate chemical processes against the 12 principles of green chemistry
+1 more objectives

AP Chemistry. College-level course aligned to College Board CED. Replaces standard Chemistry.