AP Course

AP Chemistry

Updated for the AP Chemistry framework effective fall 2024, with particle models, quantitative reasoning, labs, quizzes, and practice problems.

Build general chemistry fluency through atomic structure, bonding, reactions, kinetics, equilibrium, acids and bases, thermodynamics, and electrochemistry.

Lessons

Moles and Molar MassMass Spectra of ElementsElemental Composition of Pure SubstancesComposition of MixturesAtomic Structure and Electron ConfigurationPhotoelectron SpectroscopyPeriodic TrendsValence Electrons and Ionic CompoundsTypes of Chemical BondsIntramolecular Force and Potential EnergyStructure of Ionic SolidsStructure of Metals and AlloysLewis DiagramsResonance and Formal ChargeVSEPR and HybridizationIntermolecular and Interparticle ForcesProperties of SolidsSolids, Liquids, and GasesIdeal Gas LawKinetic Molecular TheoryDeviation from Ideal Gas LawSolutions and MixturesRepresentations of SolutionsSeparation of Solutions and MixturesSolubilitySpectroscopy and the Electromagnetic SpectrumProperties of PhotonsBeer-Lambert LawIntroduction for ReactionsNet Ionic EquationsRepresentations of ReactionsPhysical and Chemical ChangesStoichiometryIntroduction to TitrationTypes of Chemical ReactionsIntroduction to Acid-Base ReactionsOxidation-Reduction (Redox) ReactionsReaction RatesIntroduction to Rate LawConcentration Changes over TimeElementary ReactionsCollision ModelReaction Energy ProfileIntroduction to Reaction MechanismsReaction Mechanism and Rate LawPre-Equilibrium ApproximationMultistep Reaction Energy ProfileCatalysisEndothermic and Exothermic ProcessesEnergy DiagramsHeat Transfer and Thermal EquilibriumHeat Capacity and CalorimetryEnergy of Phase ChangesIntroduction to Enthalpy of ReactionBond EnthalpiesEnthalpy of FormationHess’s LawIntroduction to EquilibriumDirection of Reversible ReactionsReaction Quotient and Equilibrium ConstantCalculating the Equilibrium ConstantMagnitude of the Equilibrium ConstantProperties of the Equilibrium ConstantCalculating Equilibrium ConcentrationsRepresentations of EquilibriumIntroduction to Le Châtelier’s PrincipleReaction Quotient and Le Châtelier’s PrincipleIntroduction to Solubility EquilibriaCommon-Ion EffectIntroduction to Acids and BasespH and pOH of Strong Acids and BasesWeak Acid and Base EquilibriaAcid-Base Reactions and BuffersAcid-Base TitrationsMolecular Structure of Acids and BasespH and pK_aProperties of BuffersHenderson-Hasselbalch EquationBuffer CapacitypH and SolubilityIntroduction to EntropyAbsolute Entropy and Entropy ChangeGibbs Free Energy and Thermodynamic FavorabilityThermodynamic and Kinetic ControlFree Energy and EquilibriumFree Energy of DissolutionCoupled ReactionsGalvanic (Voltaic) and Electrolytic CellsCell Potential and Free EnergyCell Potential Under Nonstandard ConditionsElectrolysis and Faraday’s Law

Quizzes

Practice Problems Equation practice, lab analysis, and FRQ-style reasoning resources can be added here.

AP Chemistry · Unit 1 · Topic 1.5

Atomic Structure and Electron Configuration

Particle identity, electron structure, and periodic patterns connect measurable composition to atomic-scale models.

1. Topic Lens

Atomic Structure and Electron Configuration is studied through atomic structure and properties. Connect the system boundary, interacting parts, and measurable evidence before applying a formula.

\[n=\frac{m}{M}\]

Chemical equation or molecular relation

\[2H_2+O_2\rightarrow2H_2O\]

2. Why the Formula Works

The relationship is built from definitions and conservation reasoning:

Molar mass M converts measured mass m into amount n.
One mole contains Avogadro's number N_A of representative particles.
Substitution connects a macroscopic mass to a microscopic particle count.

\[N=\frac{m}{M}N_A\]

3. Detailed Visual Model

Atomic Structure and Electron Configuration: an original pixel-style model. Use it as a schematic, not a literal scale drawing.

4. Worked Example and Lab Link

How many moles are present in 36.0 g of H₂O using M=18.0 g/mol?

Answer: The sample contains 2.00 mol H₂O, or about 1.20×10²⁴ molecules.

Investigation idea: Analyze an original simulated mass spectrum and test whether peak positions and abundances reproduce an average atomic mass.

Common trap: Do not confuse atoms, molecules, formula units, and moles when converting quantities.

Checkpoint · Topic 1.5

Explain how atomic structure and electron configuration supports or limits this conclusion: The sample contains 2.00 mol H₂O, or about 1.20×10²⁴ molecules.

Official curriculum reference: College Board AP Chemistry course page. The explanation and worked example are independently written for this study site.