AP Chemistry demands both conceptual understanding and quantitative skill. These notes organize the highest-yield topics by unit so you can review formulas, mechanisms, and reasoning strategies efficiently.
Units 1–3: Atomic Structure, Bonding, and Intermolecular Forces
Electron configuration (aufbau, Hund's rule, Pauli exclusion), periodic trends (ionization energy, electronegativity, atomic radius). VSEPR theory predicts geometry; bond polarity determines molecular polarity. IMFs from weakest to strongest: London dispersion → dipole-dipole → hydrogen bonding → ion-dipole. Hybridization: sp, sp², sp³, sp³d, sp³d².
Units 4–5: Kinetics and Equilibrium
Rate laws: rate = k[A]^m[B]^n — determine m and n from experimental data. Arrhenius equation: k = Ae^(−Ea/RT) — higher Ea = slower reaction. Equilibrium constant K: K > 1 means products favored. Reaction quotient Q vs. K determines direction of shift. Le Chatelier's principle: adding reactant, increasing pressure (gases), or decreasing temperature (exothermic) shifts equilibrium right.
Units 6–7: Acids/Bases and Thermodynamics
Ka and Kb expressions; pH = −log[H⁺]; pKa + pKb = 14. Buffer capacity (Henderson-Hasselbalch: pH = pKa + log([A⁻]/[HA])). Titration curves: strong-strong (equivalence at pH 7), weak-strong (equivalence pH > 7). Thermodynamics: ΔG = ΔH − TΔS; ΔG < 0 = spontaneous. Hess's law and ΔH from bond energies.
Unit 8–9: Electrochemistry and Equilibrium Applications
Galvanic vs. electrolytic cells; cell potential E°cell = E°cathode − E°anode. Nernst equation: E = E° − (RT/nF)lnQ. Faraday's laws of electrolysis. Solubility product Ksp; common ion effect reduces solubility. Complex ion formation and its effect on Ksp.
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