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Chemistry 142. Review. Chapter 13: Chemical Kinetics . Rate Relativ e Rate of Reaction Law of Mass Action and Instantaneous Rate of Reaction Rate Law Reaction order Effect of nature of reactants, temperature, molecular orientation, concentration, catalyst

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chapter 13 chemical kinetics
Chapter 13: Chemical Kinetics
  • Rate
    • Relative Rate of Reaction
      • Law of Mass Action and
    • Instantaneous Rate of Reaction
    • Rate Law
      • Reaction order
      • Effect of nature of reactants, temperature, molecular orientation, concentration, catalyst
      • Zero Order Integrated Rate Law:
      • First Order Integrated Rate Law:
      • Second Order Integrated Rate Law:
      • Half-life
  • Arrhenius Plots
  • Reaction Mechanisms
    • Elementary steps
    • Rate determining step
    • Validating
  • Method of Initial Rates
chapter 14 chemical equilibrium
Chapter 14: Chemical Equilibrium
    • Reversibility of Reactions
    • Equilibrium constants
      • Law of Mass Action
      • Concentration
        • Temperature dependent
      • Pressure
      • Reaction Quotient, Q
      • Relationships
        • Multiplying a reaction by a factor n
        • Reversing a reaction
        • Adding reactions together
    • Le Châtelier’s Principle
      • Effect of concentration changes
      • Effect of volume changes
      • Effect of temperature changes
      • Effect of a catalyst
  • Approximations
chapter 15 acids and bases
Chapter 15: Acids and Bases
  • Properties of Acids and Bases
  • Definitions of Acids and Bases
    • Arrhenius, Brønsted-Lowry, Lewis
  • Ion-product Constant for Water
  • pH Scale and
  • Reactions
    • and
  • Percent Dissociation
  • PolyproticAcids Ka1 > Ka2 > Ka3
  • Acid Strength
    • Bond strength
    • Bond polarity
  • Acid-Base properties of salts
    • acidic, basic, neutral
chapter 16 aqueous ionic equilibrium
Chapter 16: Aqueous Ionic Equilibrium
  • Common Ion
  • Buffers
    • Henderson-Hasselbach equation :
  • Titration Curves
    • Strong acid-strong base
      • Stoichiometric point and pH = 7
    • Weak acid-strong base
      • Half-neutralization and
      • Equivalence point pH > 7
    • Weak base-strong acid
      • Half-neutralization and
      • Equivalence point pH < 7
  • Acid-Base Indicators
  • Complex Ion Equilibrium
  • Solubility Equilibrium, Ksp
    • Effect of common ion, pH, formation of a complex ion
  • Precipitation
  • Qualitative Analysis
chapter 17 free energy and thermodynamics
Chapter 17: Free Energy and Thermodynamics
  • First Law of Thermodynamics
  • Entropy
    • effect of state, molar mass, allotropes, molecular complexity, and dissolution
    • ΔS > 0 system is more disordered, ΔS < 0 system is more ordered
  • Second Law of Thermodynamics
  • Third Law of Thermodynamics (W = 1, S = 0)
  • Gibbs Free Energy
    • exergonic (ΔG < 0), endergonic (ΔG > 0), equilibrium (ΔG = 0)
    • van’t Hoff equation
chapter 18 electrochemistry
Chapter 18: Electrochemistry
  • Oxidation-Reduction Reactions
    • Oxidation vs. reduction
    • Oxidizing agent vs. reducing agent
    • Oxidation numbers
    • Balancing redox reactions
  • Electrodes: anode vs. cathode
  • Voltaic (or Galvanic) Cells (spontaneous)
    • Cell notation
    • Cell potential
    • where
    • The Nernst Equation:
  • Batteries
  • Electrolysis (nonspontaneous)
  • Corrosion
chapter 24 transition metals and coordination compounds
Chapter 24: Transition Metals and Coordination Compounds
  • Properties of Transition Metals
  • Coordination Compounds
    • Ligands: monodentate vs. bidentate vs. polydentate
    • Complex ions
      • Primary valence (oxidation number)
      • Secondary valence (coordination number)
  • Nomenclature
  • Structure and Isomers
    • Structural isomers: coordination isomers vs. linkage isomers
    • Stereoisomers
      • Geometric isomers (diastereomers): cis-trans vs. mer-fac
      • Optical isomers (enantiomers)
  • Bonding
    • Valence Bond Theory: hybridization
    • Crystal Field Theory
  • Applications
chapter 19 radioactivity and nuclear chemistry
Chapter 19: Radioactivity and Nuclear Chemistry
  • Types of Radioactivity
    • Alpha particle(42He), Beta particle (0-1e), Positron (0+1e), Gamma ray (00γ), and Electron Capture
  • Nuclear Equations (Chemical Symbols AZSyc)
    • Valley of Stability
    • Magic Numbers (N or Z = 2, 8, 20, 28, 50, 82 or N = 126)
    • Fission
    • Fusion
  • Radiation Measurements
  • First Order Decay
  • Half-Life
  • Mass Defect and Binding Energy
    • 1 MeV = 1.602 × 10-13 J and 1 amu of mass defect = 931.5 MeV
  • Applications
chapter 20 organic chemistry
Chapter 20: Organic Chemistry
  • Organic Compounds
    • Hydrocarbons
      • alkanes, alkenes, alkynes, arenes
    • Functional Groups
      • organic halide, alcohol, phenol, aldehyde, ketone, carboxylic acid, ester, amine, amide, ether
    • Organic Chemistry Nomenclature
  • Polymers
  • Properties of Organic Compounds
  • Reactions
    • Combustion
    • Addition
    • Substitution
    • Neutralization
    • Dehydration
    • Oxidation
    • Reduction
    • Condensation Reactions
      • Esterification
      • Amidation
lab techniques
Lab Techniques
  • Basic glass working
  • Proper use of standard equipment
    • Balances
      • Electronic and quad-beam
    • Volumetric equipment
      • Beakers, graduated cylinders, Erlenmeyer flasks
      • Volumetric flasks and pipets, burets
  • Use equipment to collect, organize and evaluate experimental data
    • Observe physical and chemical changes
    • Interpret qualitative (non-numerical) and quantitative (numerical) data
  • Use CRC Handbook to look up information
    • Make linear graphs using data