AP Chemistry Comprehensive Review Sheet

AP Chemistry Comprehensive Review Sheet 1. Introduction – Matter & Measurement • • • • • • Classification of matter: elements, compounds, mixtures (homogeneous vs heterogeneous). Physical vs chemical properties and changes. Significant figures rules and dimensional analysis. Density = mass/volume. Temperature conversions (K = °C + 273.15). Scientific notation and metric prefixes. 2. Atoms, Molecules & Ions • • • • • Atomic structure: protons, neutrons, electrons. Atomic number, mass number, isotopes. Ions: cations vs anions. Ionic vs molecular compounds. Nomenclature rules for ionic and covalent compounds. 3. Stoichiometry – Chemical Formulas & Equations • • • • • Balancing chemical equations. Mole concept (6.022 × 10^23 particles/mol). Molar mass calculations. Limiting reactant and percent yield. Empirical vs molecular formulas. 4. Reactions in Aqueous Solutions • • • • • Strong vs weak electrolytes. Solubility rules. Net ionic equations. Acid-base neutralization reactions. Oxidation-reduction basics (OIL RIG). 5. Thermochemistry • • • • • • Heat (q), work (w), internal energy (∆E). First Law: ∆E = q + w. Enthalpy: ∆H = q (at constant pressure). Calorimetry (q = mc∆T). Hess’s Law. Exothermic vs endothermic processes. 6. Electronic Structure of Atoms • • • • • Electromagnetic radiation (c = λν). Photoelectric effect. Quantum numbers (n, l, m_l, m_s). Electron configurations & orbital diagrams. Aufbau principle, Pauli exclusion, Hund’s rule. 7. Periodic Properties of Elements • Effective nuclear charge (Z_eff). • • • • Atomic radius trends. Ionization energy trends. Electron affinity trends. Electronegativity trends. 8. Basic Concepts of Chemical Bonding • • • • Ionic bonding vs covalent bonding. Lattice energy trends. Bond energy and bond length relationships. Polar vs nonpolar bonds. 9. Molecular Geometry & Bonding Theories • • • • • VSEPR theory. Electron domain geometry vs molecular geometry. Hybridization (sp, sp2, sp3). Sigma vs pi bonds. Dipole moments and polarity. 10. Gases • • • • • Gas laws: Boyle, Charles, Avogadro. Ideal Gas Law: PV = nRT. Partial pressures (Dalton’s Law). Kinetic Molecular Theory. RMS speed and Graham’s Law. 11. Liquids & Intermolecular Forces • • • • IMF types: H-bonding, dipole-dipole, London dispersion. Boiling point trends. Surface tension and vapor pressure. Phase changes and heating curves. 12. Solids • • • Types: ionic, metallic, molecular, network covalent. Unit cells and crystal structures. Density of solids using unit cell dimensions. 13. Properties of Solutions • • • • Molarity (M), molality (m). Dilution equation: M1V1 = M2V2. Colligative properties (∆Tb, ∆Tf). Osmotic pressure: π = MRT. 15. Chemical Equilibrium • • • • Equilibrium constant (Kc, Kp). Reaction quotient (Q). Le Châtelier’s Principle. ICE tables. • Relationship between K and ∆G. 19. Chemical Thermodynamics • • • • • Entropy (∆S). Gibbs Free Energy: ∆G = ∆H − T∆S. Spontaneity conditions. ∆G° = −RT ln K. Second Law of Thermodynamics.