AP Chemistry

• The Mole
• Molar Mass
• Grams, Moles and Particles
• Isotopes and Mass Number
• Average Atomic Mass
• Mass Spectra of Elements
• Definite and Multiple Proportions
• Percent Composition
• Empirical Formulas
• Molecular Formulas
• Combustion Analysis
• Composition of Mixtures
• Protons, Neutrons and Electrons
• Electron Configurations
• Orbital Diagrams and Magnetism
• Coulomb's Law in Atoms
• Photoelectron Spectroscopy
• Atomic Radius
• Ionization Energy
• Electronegativity
• Shielding and Effective Nuclear Charge
• Successive Ionization Energies
• Sizes of Ions
• Valence Electrons and Dot Symbols
• Predicting Ion Charges
• Formulas of Ionic Compounds

Covers official topics 1.1–1.8 (moles, mass spectra, composition of pure substances and mixtures, electron configuration, photoelectron spectroscopy, periodic trends, valence electrons and ionic compounds). Quantum numbers, hydrogen's energy levels and the exceptions to the trends are taught too, as college general chemistry does; the Course and Exam Description's exclusion statements say which of these the exam leaves out.

• Ionic Bonds
• Covalent Bonds
• Polar and Nonpolar Bonds
• Potential Energy and Bond Length
• Lattice Energy
• Ionic, Molecular, Network and Metallic Solids
• Metals and Alloys
• Crystal Structures and Unit Cells
• Lewis Structures
• Exceptions to the Octet Rule
• Formal Charge
• Resonance
• Molecular Shapes (VSEPR)
• Polar and Nonpolar Molecules
• Shapes with Five and Six Electron Groups
• Hybrid Orbitals, Sigma and Pi Bonds

Covers official topics 2.1–2.7. Naming compounds (chem.naming-ionic, chem.polyatomic-ions, chem.naming-covalent) is assumed knowledge on the exam and is taught in Chemistry. Molecular orbital diagrams (gchem1.molecular-orbitals) are a general chemistry topic that the AP topic list does not name.

• Intermolecular Forces
• Predicting Boiling Points
• Comparing Intermolecular Forces
• Solids, Liquids and Gases
• Vapor Pressure and Boiling
• Phase Diagrams
• Gas Pressure
• Boyle's Law
• Charles's Law
• Gay-Lussac's Law and the Combined Gas Law
• Avogadro's Law and Molar Volume
• The Ideal Gas Law
• Gas Density and Molar Mass
• Gas Stoichiometry
• Partial Pressures and Mole Fractions
• Kinetic Molecular Theory
• Molecular Speeds and Effusion
• The Maxwell–Boltzmann Distribution
• Real Gases
• Why Things Dissolve
• Molarity
• Dilution
• Electrolytes and Ions in Solution
• Concentrations of Ions
• Separating Mixtures
• Solubility and Solubility Curves
• The Energy of Dissolving
• Gas Solubility and Henry's Law
• Bright-Line Spectra
• Wavelength, Frequency and the Spectrum
• What Light Does to Molecules
• Photons and the Photoelectric Effect
• Hydrogen's Energy Levels
• The Beer–Lambert Law

Covers official topics 3.1–3.13, from intermolecular forces and gases to solutions, separations, spectroscopy, photons and the Beer–Lambert law. Particle drawings of solutions (topic 3.8) are part of the lessons for chem.dissolving and gchem1.ion-concentrations. Colligative properties and the Clausius–Clapeyron equation (gchem1.raoults-law, gchem1.freezing-boiling-points, gchem1.osmotic-pressure, gchem1.molar-mass-colligative, gchem1.clausius-clapeyron) are general chemistry topics that the AP topic list does not name.

• Atoms Are Conserved
• Coefficients and Subscripts
• Balancing Equations
• Net Ionic Equations
• Physical and Chemical Changes
• Mole Ratios
• Mass-to-Mass Stoichiometry
• Limiting Reactant
• Theoretical and Percent Yield
• Solution Stoichiometry
• Titration
• Titration Calculations
• Types of Reactions
• Precipitation and Solubility Rules
• Neutralization
• Acids and Bases
• Proton Donors and Acceptors
• Oxidation Numbers
• Oxidation and Reduction
• Balancing Redox Reactions

Covers official topics 4.1–4.9. Gravimetric analysis and redox titrations (gchem1.gravimetric-analysis, gchem1.redox-titrations) are extra practice in the same skills.

• Collision Theory and Reaction Rate
• Measuring Reaction Rates
• Rate Laws and Reaction Order
• The Method of Initial Rates
• First-Order Reactions
• Zero- and Second-Order Reactions
• Finding the Order from a Graph
• Elementary Steps and Molecularity
• Activation Energy and Catalysts
• Reaction Mechanisms
• The Rate-Determining Step
• A Fast Equilibrium Before a Slow Step
• Energy Profiles for Multistep Reactions
• Catalysis

Covers official topics 5.1–5.11. Calculations with the Arrhenius equation (gchem2.arrhenius) are general chemistry that the AP topic list does not name; its ideas sit in topics 5.5 and 5.6.

• Exothermic and Endothermic Reactions
• Heat and Temperature
• Specific Heat
• Calorimetry
• Calorimetry for Reactions
• Heating Curves and Phase Changes
• Heat for Warming and Phase Changes Together
• Enthalpy and Thermochemical Equations
• Heat from Amounts of Reactant
• Bond Energy and Reaction Energy
• Standard Enthalpies of Formation
• Hess's Law

Covers official topics 6.1–6.9. The first law with work, bomb calorimetry and Born–Haber cycles (gchem1.first-law, gchem1.pv-work, gchem1.bomb-calorimetry, gchem1.born-haber) are general chemistry topics that the AP topic list does not name.

• Dynamic Equilibrium
• The Equilibrium Constant
• The Reaction Quotient
• Calculating K with an ICE Table
• Kp and Kc
• What the Size of K Tells You
• Reversing, Scaling and Adding Reactions
• Finding Equilibrium Concentrations
• The Small-x Approximation
• Le Chatelier's Principle
• Le Chatelier's Principle with Q and K
• The Solubility Product
• Comparing Solubilities
• Will a Precipitate Form?
• The Common-Ion Effect

Covers official topics 7.1–7.12. Particle drawings of equilibrium mixtures (topic 7.8) are part of the lessons for chem.dynamic-equilibrium and gchem2.calculating-k.

• Acids and Bases
• The pH Scale
• pH, pOH and the Ions in Water
• Strong and Weak Acids
• pH of Strong Acids and Bases
• Acid and Base Constants
• pH of a Weak Acid
• Percent Ionization
• pH of a Weak Base
• Neutralization
• Acidic, Basic and Neutral Salts
• How Buffers Work
• Strong Acid–Strong Base Titration Curves
• Weak Acid–Strong Base Titration Curves
• Choosing an Indicator
• Polyprotic Acids
• Molecular Structure and Acid Strength
• pH, pKa and Which Form Dominates
• Adding Acid or Base to a Buffer
• The Henderson–Hasselbalch Equation
• Buffer Capacity and Choosing a Buffer
• pH and Solubility

Covers official topics 8.1–8.11. How Kw and neutral pH change with temperature (part of topic 8.1) is taught inside the lesson for gchem2.strong-acid-ph rather than as its own topic.

• Entropy and Microstates
• Predicting the Sign of ΔS
• Absolute Entropies and ΔS°
• The Second Law
• Gibbs Free Energy
• Temperature and Favorability
• Favored but Slow: Kinetic Control
• Free Energy and Equilibrium
• The Energy of Dissolving
• Coupled Reactions
• Galvanic Cells
• Electrolytic Cells
• Standard Reduction Potentials
• Cell Potential, Free Energy and K
• The Nernst Equation
• Electrolysis Calculations

Covers official topics 9.1–9.11. Topic 9.6 (free energy of dissolution) joins gchem1.dissolution-energy with the entropy and free energy topics. The AP course also asks for hands-on laboratory work, which no website replaces; the Science Lab's Mixing Lab and Gas in a Box help with the ideas.