AP Chemistry Speed Review

Introduction

• Presented by Jeremy Krug
• Overview of major topics in AP Chemistry in under 20 minutes
• Ultimate Review Packet available with extensive resources

Unit 1: Atoms

• The Mole:
  • A unit to count large numbers of atoms/molecules
  • One mole = atomic mass in grams (e.g., Fe = 55.85g, H2O = 18.02g)
  • Contains 6.022 x 10^23 particles (Avogadro's number)
• Electron Configurations:
  • Example: Neon (Ne) = 1s2, 2s2, 2p6
  • Stable with 8 electrons in valence shell (octet rule)
• Coulomb’s Law & Atomic Properties:
  • Attraction between opposite charges; stronger when closer
  • Photoelectron spectroscopy used to analyze electron sublevels
  • Periodic Table trends: atomic radius, ionization energy, ionic size

Unit 2: Chemical Compounds

• Ionic Bonds:
  • Between metals/nonmetals via electrostatic forces
  • Form a 3D lattice
• Covalent Bonds:
  • Atoms share electrons, can be polar or nonpolar
  • Form discrete molecules
• Metallic Bonds:
  • Free-moving electrons in metals/alloys
• Lewis Dot Diagrams:
  • Visualize molecule shapes and valence electrons

Unit 3: Intermolecular Forces

• Dispersion, Dipole-Dipole, Hydrogen Bonding:
  • Dispersion: weak, stronger with more electrons
  • Dipole-Dipole: stronger, between polar molecules
  • Hydrogen Bonding: strongest, in molecules with O-H, N-H, F-H bonds
• States of Matter & Ideal Gas Law:
  • Solid, liquid, gas dynamics
  • Ideal Gas Law: PV=nRT

Unit 4: Chemical Reactions

• Balancing Equations & Types of Reactions:
  • Net ionic equations omit spectator ions
  • Precipitation, oxidation-reduction, acid-base reactions
• Stoichiometry:
  • Convert quantities to moles, use mole ratios

Unit 5: Kinetics

• Rate Laws & Reaction Mechanisms:
  • Rate = k[Reactant]^order
  • Reaction order affects rate: zero, first, second
  • Use integrated rate laws for time-based calculations
  • Reaction mechanism's slow step determines overall rate

Unit 6: Thermodynamics

• Heat Transfer & Enthalpy:
  • Q = mCΔT for heat calculations
  • Enthalpy changes via bond enthalpies, Hess's Law

Unit 7: Equilibrium

• Equilibrium Concepts:
  • Reaction quotient (Q) compared to equilibrium constant (K)
  • Le Chatelier’s Principle: reaction shifts with concentration changes

Unit 8: Acids and Bases

• pH, pOH, and Equilibrium:
  • pH = -log[H+], pOH = -log[OH-]
  • Strong/weak acids and bases
  • Acid-base titrations and buffer solutions

Unit 9: Applications of Thermodynamics

• Entropy & Gibbs Free Energy:
  • Entropy changes (ΔS) predict reaction favorability
  • ΔG = ΔH - TΔS; negative ΔG indicates favorability
• Electrochemistry:
  • Galvanic cells, oxidation-reduction reactions
  • Nernst Equation for non-standard conditions

Conclusion

• Recap of AP Chemistry major points
• Encouragement to explore further resources at Ultimate Review Packet dot com