General Chemistry Lecture Notes

• Contents
• Energetics of Solution Formation
• Gas Solutions
• Colligative Properties
  • Concentration Units
  • Vapor Pressure Lowering
  • Boiling Point Elevation
  • Freezing Point Depression
  • Osmosis
• Kinetics
  • Average Rates
  • Instantaneous Rates
  • The 3 Common Rate Laws
  • Integrated Rate Laws
  • Half-Life
  • The Rate Constant, k
  • Reaction Mechanisms
  • Catalysis
• Dynamic Equilibrium
  • The Equilibrium Constant
  • Manipulating Reactions and K
  • Calculating K_c from Initial Concentrations and 1 Equilibrium Concentration
  • Reaction Quotient, Q
  • Solving for Equilibrium Concentrations using a Known K_c
  • Relearning how to work limiting reactant problems with the RICE method
  • Le Chatelier’s Principle
  • Temperature Dependence of K
  • How to solve *some* problems quickly
• Acids and Bases
  • Arrhenius Definition
  • Brønsted-Lowry Definition
  • Equilibrium
  • p-Scales
  • Substances
  • Adding acids and bases to water
  • Lewis Definition
  • Buffers
  • Titrations
• Solubility
  • Solubility
  • Solubility Product Constant and Molar Solubility
  • Common Ion Effect
  • Acid/Base Considerations
  • Complex Ion Formation
  • Precipitation and Q_sp
• Thermodynamics
  • Entropy, S
  • The 3rd Law of Thermodynamics
  • Standard Molar Entropy, S^∘
  • The 2nd Law of Thermodynamics
  • Gibbs Free Energy, G
  • Gibbs Free Energy of Formation, Δ G_f^∘
  • Equilibrium
  • van’t Hoff equation
• Oxidation-Reduction (Redox) Reactions
  • Balancing Redox Reactions
  • Balancing in basic solution using half-reactions
  • Electrochemical Cells
  • Electrolytic Cells
• Nuclear Chemistry
  • Radiocarbon Dating
  • Uranium-Lead Dating
  • Nuclear binding energy
  • Fission and Fusion
• Transition Metal Complex Ion Chemistry

This document was translated from L^AT_EX by H^EV^EA.