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Chem

The AP Chemistry class notes cover key topics including atomic structure, bonding, intermolecular forces, chemical reactions, kinetics, thermodynamics, equilibrium, and electrochemistry. Each section outlines fundamental concepts such as electron configurations, reaction types, rate laws, and thermodynamic principles. The notes also address practical applications like titrations, chromatography, and the behavior of acids and bases.

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16 views2 pages

Chem

The AP Chemistry class notes cover key topics including atomic structure, bonding, intermolecular forces, chemical reactions, kinetics, thermodynamics, equilibrium, and electrochemistry. Each section outlines fundamental concepts such as electron configurations, reaction types, rate laws, and thermodynamic principles. The notes also address practical applications like titrations, chromatography, and the behavior of acids and bases.

Uploaded by

jonathan.earp55
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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Download as PDF, TXT or read online on Scribd
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AP Chemistry Class Notes

1. Atomic Structure & Periodicity


Subatomic particles; mass number vs. atomic number; isotopes & mass spectrometry.

Electron configurations: Aufbau, Hund, Pauli; core vs. valence; periodic trends (Z_eff, IE, EA,
EN, atomic radius).

2. Bonding & Molecular Structure


Ionic vs. covalent vs. metallic; lattice energy; Coulomb’s Law.

Lewis structures & exceptions (octet, expanded valence, radicals).

VSEPR geometries, polarity, and IMF strength hierarchy: London < dipole-dipole < H-bonding <
ion-dipole.

Hybridization & molecular orbitals; σ vs. π bonds; resonance; formal charge.

3. Intermolecular Forces & Properties


States of matter, phase changes & diagrams (critical point, triple point).

Solutions: factors affecting solubility; concentration units (M, m, ppm, mole fraction).

Chromatography & distillation as separation techniques.

4. Chemical Reactions
Stoichiometry, limiting reactant, percent yield.

Reaction types: synthesis, decomposition, single-replacement, double-replacement,


combustion, redox.

Titrations: endpoint vs. equivalence; indicators; volumetric analysis; pH curves (strong/weak


combinations).

5. Kinetics
Rate laws (differential / integrated), determining order graphically.

Arrhenius equation; activation energy; catalysis; collision model; reaction mechanisms &
rate-determining step.

6. Thermodynamics
Enthalpy (ΔH): calorimetry (q = m c ΔT), Hess’s Law, bond enthalpies.

Entropy (ΔS) & Gibbs free energy (ΔG = ΔH – TΔS); spontaneity, coupling reactions.
Heat vs. temperature; phase change enthalpies.

7. Equilibrium
K_eq expressions; Le Châtelier shifts (concentration, pressure, temp).

Solubility product (K_sp) and common-ion effect.

Acid–base: Ka, Kb, pKa, pH = –log[H⁺]; polyprotic acids; buffers (Henderson–Hasselbalch).

Indicators and titration curves; hydrolysis of salts.

8. Electrochemistry
Galvanic vs. electrolytic cells: anode/ cathode signage, cell notation.

Nernst equation; ΔG° = –nF E°.

Faraday’s laws (m = ItM/nF); corrosion and prevention.

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