High School Chemistry

AP Chemistry is an advanced high school course and a standardized exam offered by the College Board. It is designed to be the equivalent of a first-year college-level general chemistry course, providing a rigorous and comprehensive introduction to the fundamental principles of chemistry.

Topics are: Introduction to chemistry, Periodic table, Kinetic-molecular theory, Chemical equilibrium, Organic chemistry, Thermochemistry, Matter, Chemical bonds, Chemical solutions, Acids and bases, Biochemistry, Atom, Chemical reaction, Chemical reaction rates, Electrochemistry, Nuclear chemistry.

AP Chemistry Past Papers & Solutions

AP Chemistry 2025 FRQ Solutions

AP Chemistry 2024 FRQ Solutions

AP Chemistry 2023 FRQ Solutions

AP Chemistry 2022 FRQ Solutions

AP Chemistry 2021 FRQ Solutions

AP Chemistry 2020 FRQ Solutions

AP Chemistry 2019 FRQ Solutions

AP Chemistry 2018 FRQ Solutions

AP Chemistry 2017 FRQ Solutions

AP Chemistry 2016 FRQ Solutions

APChemistry Course Content and Structure

The AP Chemistry curriculum is structured into nine units that cover a broad range of topics, emphasizing both conceptual understanding and quantitative problem-solving. The units are:

1. Atomic Structure and Properties: Moles, molar mass, mass spectrometry, electron configuration, periodic trends, and ionic compounds.

2. Molecular and Ionic Compound Structure and Properties: Types of chemical bonds, Lewis diagrams, VSEPR theory, resonance, and hybridization.

3. Intermolecular Forces and Properties: Intermolecular forces, properties of solids, liquids, and gases, the Ideal Gas Law, solutions, and Beer-Lambert’s Law.

4. Chemical Reactions: Types of reactions, stoichiometry, titrations, and redox reactions.

5. Kinetics: Reaction rates, rate laws, reaction mechanisms, and the collision model.

6. Thermodynamics: Endothermic and exothermic processes, calorimetry, enthalpy, and Hess’s Law.

7. Equilibrium: Equilibrium constants, Le Châtelier’s principle, and solubility equilibria.

8. Acids and Bases: Definitions of acids and bases, pH, pOH, buffers, and titrations.

9. Applications of Thermodynamics: Entropy, Gibbs free energy, and electrochemistry (galvanic and electrolytic cells).

High School Chemistry

• Introduction to Chemistry

  Chemistry Definition
  Scientific Method Steps
  Dimensional Analysis
  
  Scientific Units
  Scientific Notation
  Significant Figures

• The Periodic Table

  Periodic Table Overview
  s-Block Elements
  p-Block Elements
  d-Block Elements
  f-Block Elements
  
  Transition Metals
  Inner Transition Metals
  Boron Family - Carbon Family - Nitrogen Family
  Oxygen Family
  Halogens
  Noble Gases
  
  Electronegativity Ionization Energy
  Periodic Trends
  Atomic Radii
  Ionic Radii

• Kinetic-Molecular Theory

  Three States of Matter
  Phase Change
  Phase Diagrams
  Boiling Point
  
  Vapor Pressure
  Gases
  Avogadro’s Principle
  Dalton’s Law
  Graham’s Law
  
  Boyle’s Law
  Charles Law
  Gay Lussac’s Law
  Combined Gas Law
  Ideal Gas Law

• Chemical Equilibrium

  Chemical Equilibrium Definition
  Heterogeneous Equilibrium
  Homgeneous Equilibrium
  Le Chatelier’s Principle
  
  Equilibrium Changes
  Calculating Equilibrium Concentrations
  Solubility Equilibrium

• Organic Chemistry

  Hydrocarbons
  Alkanes
  Naming Alkanes
  Alkenes-Alkynes
  Naming Alkenes-Naming Alkynes
  
  Aromatic Hydrocarbon
  Isomers-Stereoisomers
  Functional Groups

• Thermochemistry

  Specific Heat
  Bomb Calorimeters
  Enthalpy
  Thermochemical Equation
  
  Conservation of Energy
  Second Law of Thermodynamics
  Entropy
  Hess’s Law
  
  Spontaneous Processes
  Heat of Formation
  Gibbs Free Energy
  Heat of Fusion - Heat of Vaporization

• Matter

  Physical Matter Properties
  Chemical Matter Properties
  States of Matter
  Changes in Matter
  
  Conservation of Mass
  Law of Definite Proportions
  Law of Multiple Proportions
  Mixtures
  Elements and Compounds

• Chemical Bonds

  Ionic Bond
  Ionic Compound Properties
  Metallic Bond
  Covalent Bonds
  
  Hydrates
  Lewis Electron Dot Diagram
  Polarity
  
  Naming Covalent Compounds
  Naming Ionic Compounds
  
  Hybridization
  Intermolecular Forces
  VSPER Model

• Chemical Solutions

  Types of Solutions
  Solvation
  Molarity - Molality
  
  Colligative Properties
  Vapor Pressure Lowering
  Boiling Point Elevation
  Freezing Point Depression
  
  Osmosis
  Colloids - Suspensions
  Beer’s Law

• Acids and Bases

  Acid and Base Properties
  Strength of Acids and Bases
  Salts
  Buffered Solutions
  pH and pOH
  
  Bronsted-Lowry Model
  Conjugate Acids and Bases
  Equilibrium Systems
  Naming Acids

• Biochemistry

  Proteins Chemistry Carbohydrates Fats and Lipids Nucleic Acids

• The Atom

  Atomic Structure
  Quantum Numbers
  Atomic Emission Spectra
  Atomic Number - Isotopes
  Atomic Mass
  
  Atomic Orbitals
  Orbital Diagrams
  Electron Configuration
  Exceptions to Electron Configuration
  Valence Electrons
  
  Electromagnetic Spectrum
  Photoelectric Effect
  Planck’s Constant

• Chemical Reactions

  Chemical Equations
  Balancing Chemical Equations
  
  Synthesis Reactions
  Combustion Reactions
  Decomposition Reaction
  Single Replacement Reaction
  
  Double Replacement Reactions
  Net Ionic Equation
  Types of Reactions
  
  Chemistry Mole
  Molar Mass
  Law of Conservation of Mass
  Empirical Formula - Molecular Formula
  
  Stoichiometry
  Percent Yield
  Limiting Reactants

• Chemical Reaction Rates

  Collision Theory
  Reaction Rates Factors
  Reaction Mechanism
  
  Reaction Rate Laws
  Reaction Rate Problems
  Energy Diagrams

• Electrochemistry

  Oxidation Reduction Reactions - Redox
  Half-reactions
  Voltaic Cells
  
  Chemistry Corrosion
  Electrolysis
  Oxidation Number Method

• Nuclear Chemistry

  Nuclear Reactions
  Radioactivity
  Beta Decay
  Alpha Decay
  Electron Capture
  
  Nuclear Stability
  Transmutation
  Half-life
  Fission
  Fusion

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