AP Chemistry Speed Review Notes

Introduction

• Presenter: Jeremy Krug
• Purpose: Speed review of major AP Chemistry topics
• Ultimate Review Packet:
  • Offers comprehensive AP Chem study guides, review videos, and a full-length exam
  • Price: $24.99 with discounts for class purchases

Unit 1: Atoms

• Mole Concept:
  • Used to count atoms/molecules
  • One mole = atomic mass in grams (e.g., Iron = 55.85g)
  • Avogadro's number: 6.022 x 10^23 particles
• Electron Configurations:
  • Example for Neon: 1s² 2s² 2p⁶
  • Stability with 8 valence electrons (octet rule)
• Coulomb’s Law:
  • Attraction between charges depends on magnitude and distance
  • Valence electrons less tightly held due to distance
• Photoelectron Spectroscopy:
  • Peaks represent sublevels; taller peaks = more electrons
  • Energy required relates to electron binding
• Periodic Table Patterns:
  • Atomic radius: Larger at bottom/left
  • Ionization energy: Higher at top/right
  • Anions larger, cations smaller

Unit 2: Chemical Compounds

• Ionic Bonds:
  • Formed between metals and nonmetals
  • Electrostatic attraction
• Covalent Bonds:
  • Atoms share electrons (can be polar/nonpolar)
  • Form molecules
• Metallic Bonds:
  • Freely moving electrons in metals
• Lewis Structures:
  • Visualize molecule shapes based on valence electrons
  • Aim for octet, double/triple bonds possible

Unit 3: Intermolecular Forces

• Dispersion Forces:
  • Weak; increase with molecule size
• Dipole-Dipole Forces:
  • Attraction between polar molecules
• Hydrogen Bonding:
  • Strong forces in molecules with O-H, N-H, F-H bonds
• States of Matter:
  • Solids: Crystalline, fixed shape
  • Liquids: More space, flow
  • Gases: Independent molecules, compressible
• Ideal Gas Law: PV = nRT

Unit 4: Chemical Reactions

• Net Ionic Equations:
  • Exclude spectator ions
• Balancing Equations:
  • Use coefficients to balance atoms
• Reaction Types:
  • Precipitation, Redox, Acid-Base

Unit 5: Kinetics

• Rate Laws:
  • Determine reaction rates experimentally
  • Order of reaction affects rate
• Reaction Mechanisms:
  • Slow step determines rate
• Factors Affecting Rate:
  • Temperature, concentration, catalysts

Unit 6: Thermodynamics

• Endothermic vs. Exothermic:
  • Endothermic absorbs, exothermic releases heat
• Calculating Heat Transfer: Q = mCΔT
• Enthalpy (ΔH):
  • Use bond enthalpies or Hess's Law

Unit 7: Equilibrium

• Equilibrium Constant (K): Ratio of products to reactants
• Le Chatelier's Principle:
  • Reaction shifts to counter changes

Unit 8: Acids and Bases

• pH and pOH:
  • pH = -log[H⁺]
  • pOH = -log[OH⁻]
• Acid-Base Titrations:
  • Find concentration using endpoint indicator

Unit 9: Applications of Thermodynamics

• Entropy (S): Disorder measure
  • Solids = low, gases = high
• Gibbs Free Energy (ΔG):
  • ΔG = ΔH - TΔS
  • Negative ΔG indicates spontaneity
• Electrochemistry:
  • Galvanic cells, oxidation/reduction
  • Nernst Equation for non-standard conditions

Conclusion

• Comprehensive review of AP Chemistry
• Encouragement to use review packets and additional resources