Atomic Structure and Properties

• 1.1: Moles and Molar Mass
• 1.2: Mass Spectroscopy
• 1.3: Elemental Composition of Pure Substances
• 1.4: Composition of Mixtures
• 1.5: Atomic Structure and Electron Configuration
• 1.6: Photoelectron Spectroscopy
• 1.7: Periodic Trends
• 1.8: Valence Electrons and Ionic Compounds

Molecular and Ionic Compounds

• 2.1: Types of Chemical Bonds
• 2.2: Intramolecular Force and Potential Energy
• 2.3: Structure of Ionic Solids
• 2.4: Structure of Metals and Alloys
• 2.5: Lewis Diagrams
• 2.6: Resonance and Formal Charge
• 2.7: VSEPR and Hybridization

Intermolecular Forces and Properties

• 3.1: Intermolecular and Interparticle Forces
• 3.2: Properties of Solids
• 3.3: Solids, Liquids, and Gases
• 3.4: Ideal Gas Law
• 3.5: Kinetic Molecular Theory
• 3.6: Deviation from Ideal Gas Law
• 3.7: Solutions and Mixtures
• 3.8: Representations of Solutions
• 3.9: Separation of Solutions and Mixtures
• 3.10: Solubility
• 3.11: Spectroscopy and the Electromagnetic Spectrum
• 3.12: Properties of Photons
• 3.13: Beer-Lambert Law

Chemical Reactions

• 4.1: Introduction for Reactions
• 4.2: Net Ionic Equations
• 4.3: Representation of Reactions
• 4.4: Physical and Chemical Changes
• 4.5: Stoichiometry
• 4.6: Introduction to Titration
• 4.7: Types of Chemical Reactions
• 4.8: Introduction to Acid-Base Reactions
• 4.9: Oxidation-Reduction (Redox) Reactions

Kinetics

• 5.1: Reaction Rates
• 5.2: Introduction to Rate Law
• 5.3: Concentration Changes Over Time
• 5.4: Elementary Reactions
• 5.5: Collision Model
• 5.6: Reaction Energy Profile
• 5.7: Introduction to Reaction Mechanisms
• 5.8: Reaction Mechanism and Rate Law
• 5.9: Pre-Equilibrium Approximation
• 5.10: Multistep Reaction Energy Profile
• 5.11: Catalysts

Thermodynamics

• 6.1: Endothermic and Exothermic Processes
• 6.2: Energy Diagrams
• 6.3: Heat Transfer and Thermal Equilibrium
• 6.4: Heat Capacity and Calorimetry
• 6.5: Energy of Phase Changes
• 6.6: Introduction to Enthalpy of Reaction
• 6.7: Bond Enthalpies
• 6.8: Enthalpy of Formation
• 6.9: Hess’s Law

Equilibrium

• 7.1: Introduction to Equilibrium
• 7.2: Direction of Reversible Reactions
• 7.3: Reaction Quotient and Equilibrium Constant
• 7.4: Calculating the Equilibrium Constant
• 7.5: Magnitude of the Equilibrium Constant
• 7.6: Properties of the Equilibrium Constant
• 7.7: Calculating Equilibrium Concentrations
• 7.8: Representations of Equilibrium
• 7.9: Introduction to Le Chatelier’s Principle
• 7.10: Reaction Quotient and Le Chatelier’s Principle
• 7.11: Introduction to Solubility Equilibria
• 7.12: Common-Ion Effect

Acids and Bases

• 8.1: Introduction to Acids and Bases
• 8.2: pH and pOH of Strong Acids and Bases
• 8.3: Weak Acid and Base Equilibria
• 8.4: Acid-Base Reactions and Buffers
• 8.5: Acid-Base Titrations
• 8.6: Molecular Structure of Acids and Bases
• 8.7: pH and pKa
• 8.8: Properties of Buffers
• 8.9: Henderson-Hasselbalch Equation
• 8.10: Buffer Capacity
• 8.11: pH and Solubility

Thermodynamics and Electrochemistry

• 9.1: Introduction to Entropy
• 9.2: Absolute Entropy and Entropy Change
• 9.3: Gibbs Free Energy and Thermodynamic Favorability
• 9.4: Thermodynamic and Kinetic Control
• 9.5: Free Energy and Equilibrium
• 9.6: Free Energy of Dissolution
• 9.7: Coupled Reactions
• 9.8: Galvanic (Voltaic) and Electrolytic Cells
• 9.9: Cell Potential and Free Energy
• 9.10: Cell Potential Under Nonstandard Conditions
• 9.11: Electrolysis and Faraday’s Law