Course overview

AP Chemistry builds a connected model of matter and change. You move from particle-level structure to macroscopic properties, then use energetics, kinetics, and equilibrium ideas to explain and predict chemical behavior in quantitative terms.

Complete curriculum

Every unit and lesson

36 lessons total

01
Unit 1 · 4 lessons
Atomic Structure and Properties
Model atoms using subatomic particles, electron configurations, and periodic trends, then connect those ideas to measurable properties.
Why it matters
Atomic structure explains why elements behave differently and sets up every later unit on bonding, reactions, and equilibrium.
By the end, you will be able to
- Use atomic number, mass number, and isotopic abundance to calculate average atomic mass.
- Write and interpret electron configurations and orbital diagrams.
- Explain periodic trends in radius, ionization energy, and electron affinity using structure.
1. 1.1
  Subatomic particles and isotopes
  Track protons, neutrons, and electrons to represent nuclides and ions correctly.
2. 1.2
  Electron configuration
  Use Aufbau, Pauli, and Hund principles to place electrons in orbitals.
3. 1.3
  Photoelectron spectroscopy basics
  Relate PES peaks to electron shells and relative binding energy.
4. 1.4
  Periodic trends from structure
  Use effective nuclear charge and shielding to justify periodic patterns.
Study unit 1 in detail
02
Unit 2 · 4 lessons
Molecular and Ionic Compound Structure and Properties
Use bonding models to predict molecular shape, polarity, and intermolecular forces, then connect those to physical behavior.
Why it matters
Structure at the bonding level determines reactivity, phase behavior, solubility, and material properties.
By the end, you will be able to
- Represent ionic and covalent compounds with Lewis structures and formal charge reasoning.
- Use VSEPR and hybridization ideas to predict molecular geometry and bond angles.
- Relate intermolecular forces to boiling point, volatility, and solubility trends.
1. 2.1
  Ionic, covalent, and metallic bonding
  Distinguish bonding types and resulting structural models for solids and molecules.
2. 2.2
  Lewis structures and formal charge
  Build valid electron-dot structures and choose plausible resonance contributors.
3. 2.3
  Molecular geometry and polarity
  Predict shape and net dipole from electron domains and molecular symmetry.
4. 2.4
  Intermolecular forces and properties
  Use LDF, dipole-dipole, and hydrogen bonding to explain property differences.
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03
Unit 3 · 4 lessons
Intermolecular Forces and Properties
Analyze solids, liquids, gases, and solutions using particle models, stoichiometry, and intermolecular interactions.
Why it matters
Many AP Chemistry problems depend on linking particulate reasoning to concentration, gas behavior, and solution properties.
By the end, you will be able to
- Use moles, molar mass, and composition relationships to quantify substances and mixtures.
- Apply the ideal gas law and kinetic molecular theory to explain gas observations.
- Calculate and interpret concentration units such as molarity and mass percent.
1. 3.1
  Structure of solids, liquids, and gases
  Connect particle arrangement and motion to phase-level properties.
2. 3.2
  Gas laws and KMT
  Use PV = nRT and KMT assumptions to interpret pressure, volume, and temperature changes.
3. 3.3
  Solutions and concentration
  Compute molarity, dilution, and composition metrics in context.
4. 3.4
  IMFs in mixtures
  Predict miscibility and boiling-point differences from molecular interactions.
Study unit 3 in detail
04
Unit 4 · 4 lessons
Chemical Reactions
Represent, classify, and quantify reactions using balanced equations, stoichiometric relationships, and net ionic reasoning.
Why it matters
Reaction accounting is the foundation for predicting product amounts and evaluating whether claims are chemically consistent.
By the end, you will be able to
- Balance molecular and net ionic equations while conserving atoms and charge.
- Use stoichiometric ratios to identify limiting reactants and theoretical yield.
- Classify common reaction patterns, including precipitation, acid-base, and redox processes.
1. 4.1
  Balancing and representing reactions
  Translate word descriptions to balanced chemical equations in correct physical states.
2. 4.2
  Net ionic equations
  Separate spectators from reacting species in aqueous systems.
3. 4.3
  Limiting reactant and yield
  Use mole ratios to find which reactant controls product amount.
4. 4.4
  Redox bookkeeping
  Track oxidation states to identify oxidation and reduction in reactions.
Study unit 4 in detail
05
Unit 5 · 4 lessons
Kinetics
Model reaction rates with data, rate laws, and mechanism-level reasoning about collisions and activation energy.
Why it matters
Kinetics explains how fast processes occur and which variables control speed, a core part of scientific prediction.
By the end, you will be able to
- Determine reaction order and rate law from initial-rate data.
- Calculate rate constants and use integrated-rate relationships for simple systems.
- Explain how temperature, concentration, and catalysts influence rate through collision theory and activation energy.
1. 5.1
  Rates from concentration-time data
  Extract average and instantaneous rates with correct sign and units.
2. 5.2
  Rate laws from experiments
  Infer reaction orders using controlled concentration changes.
3. 5.3
  Mechanisms and elementary steps
  Relate proposed mechanisms to observed rate laws and intermediates.
4. 5.4
  Temperature effects and Arrhenius model
  Connect activation energy changes to rate constant behavior.
Study unit 5 in detail
06
Unit 6 · 4 lessons
Thermochemistry
Quantify heat and energy flow in chemical and physical changes using calorimetry, enthalpy, and Hess's law.
Why it matters
Energy accounting links microscopic bond changes to measurable temperature change and process feasibility.
By the end, you will be able to
- Use q = mcDeltaT to calculate heat transfer in a simple calorimetry setup.
- Interpret endothermic and exothermic processes using enthalpy sign conventions.
- Apply Hess's law and standard enthalpies of formation to compute reaction enthalpy.
1. 6.1
  System, surroundings, and energy flow
  Define sign conventions and distinguish heat from temperature.
2. 6.2
  Calorimetry calculations
  Solve heat-transfer problems with mass, specific heat, and DeltaT.
3. 6.3
  Enthalpy and reaction profiles
  Use energy diagrams to classify and compare reaction pathways.
4. 6.4
  Hess's law and formation data
  Combine equations or tabulated values to find $\Delta H$ for target reactions.
Study unit 6 in detail
07
Unit 7 · 4 lessons
Equilibrium
Use equilibrium constants and reaction quotients to predict direction of change and final composition in reversible systems.
Why it matters
Most real chemical systems are dynamic, and equilibrium tools let you predict how they respond to disturbances.
By the end, you will be able to
- Write K expressions from balanced equations and interpret magnitude of K.
- Use Q versus K to determine reaction shift direction.
- Apply Le Chatelier reasoning to concentration, pressure, and temperature changes.
1. 7.1
  Dynamic equilibrium model
  Distinguish static appearance from equal forward and reverse rates.
2. 7.2
  Equilibrium expressions
  Construct Kc or Kp correctly from stoichiometric coefficients.
3. 7.3
  Q versus K reasoning
  Predict spontaneous shift direction before equilibrium is reached.
4. 7.4
  Le Chatelier applications
  Predict and justify shifts due to external changes.
Study unit 7 in detail
08
Unit 8 · 4 lessons
Acids and Bases
Analyze acid-base behavior with Bronsted-Lowry theory, pH relationships, and equilibrium constants for weak acids and bases.
Why it matters
Acid-base systems appear across chemistry, from environmental chemistry to biochemical pathways and industrial processes.
By the end, you will be able to
- Classify acids and bases and identify conjugate pairs in reactions.
- Compute pH, pOH, and related concentrations in strong-acid or strong-base contexts.
- Use Ka, Kb, and pKa ideas to compare weak-acid and weak-base behavior, including buffers.
1. 8.1
  Bronsted-Lowry framework
  Track proton transfer and identify conjugate acid-base pairs.
2. 8.2
  pH and pOH calculations
  Convert among [H+], [OH-], pH, and pOH with logarithmic definitions.
3. 8.3
  Weak-acid and weak-base equilibria
  Use Ka or Kb to estimate dissociation and relative strength.
4. 8.4
  Buffers and titration curves
  Interpret buffer regions, half-equivalence points, and indicator choice.
Study unit 8 in detail
09
Unit 9 · 4 lessons
Applications of Thermodynamics
Connect entropy and free energy to spontaneity, then apply redox and cell-potential models to electrochemical systems.
Why it matters
This unit ties together energy, charge flow, and chemical change, completing the predictive framework for AP Chemistry.
By the end, you will be able to
- Interpret $\Delta S$ and $\Delta G$ to evaluate thermodynamic favorability.
- Use $\Delta G$ = $\Delta H$ - TDeltaS qualitatively and quantitatively in context.
- Analyze galvanic and electrolytic cells using half-reactions and standard cell potential.
1. 9.1
  Entropy and spontaneity
  Use particle distribution and energy dispersal ideas to reason about $\Delta S$ .
2. 9.2
  Free energy relationships
  Link $\Delta G$ sign to spontaneous direction under stated conditions.
3. 9.3
  Galvanic and electrolytic cells
  Identify anode/cathode roles and electron-flow direction.
4. 9.4
  Standard reduction potentials
  Compute $E_{cell}$ and infer whether a redox process is thermodynamically favorable.
Study unit 9 in detail

AP Chemistry

Course overview

Every unit and lesson

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