Download Chemistry 3202

Chemistry 3202
Final Exam Review
Unit I: Kinetics & Equilibrium
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Reaction Rates and Measuring Reaction Rates
Kinetic Molecular Theory (KMT)
o Definition
o KMT and Physical States of Matter
o Support of KMT
Collision Theory
Transition State Theory
Activation Energy, EA
Potential Energy Diagrams
Endothermic & Exothermic Processes
Calculations involving Potential Energy Diagrams
Factors that Affect Reaction Rate
o Concentration of a reactant
o Pressure of a reactant
o Surface area of a solid reactant
o Temperature
o Nature of the reactants
o Presence/Absence of a catalyst
Reaction Mechanisms
o Elementary process
o Reaction Intermediates
o Catalyst
o Rate Determining Step
o Overall Reaction Rate
Catalysts
o Homogeneous
o Heterogeneous
Types of Elementary Reactions
o Unimolecular
o Bimolecular
o Termolecular
Reaction Rates Lab
STSE #1: Smog, Catalytic Converters and You
Irreversible vs. Reversible Reactions
Dynamic equilibrium
Conditions necessary for equilibrium
Le Chatelier’s Principle
Equilibrium constant
o Definition
o Interpreting K
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o Calculations involving K
Perturbing Equilibrium Lab
Unit II: Acids and Bases
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Operational Definitions of Acids and Bases
Arrhenius Theory
Modified Arrhenius Theory
Bronsted-Lowry Theory
Conjugate Acid/Base Pairs
Amphoteric
Strong vs. Weak Acids
Strong vs. Weak Bases
Predicting Bronsted-Lowry Acid/Base Reactions
Autoionization of Water
o Kw = [H3O+][OH-]
Types of Acids
o Monoprotic
o Diprotic
o Triprotic
pH and pH Scale
o Calculating pH and pOH
Acid and Base Dilution
pH of a weak acid
o % Reaction
o Acid/Base Dissociation Constants (Ka and Kb)
Calculations Involving Ka and Kb
o ICE tables!
Acid/Base Titrations
o Equivalence Point vs. Endpoint
o Primary standard
o 4 types of Acid/Base Titrations
Acid/Base Stoichiometry
Titration Curves
Indicators
STSE #2: Acids Around Us
Titration Lab
Unit III: Thermochemistry
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Definition of Thermochemistry/Thermodymanics
Energy
Temperature
Potential Energy/ Kinetic Energy/ Thermal Energy
Work and heat
System and surroundings
1st Law of Thermodynamics
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Law of Conservation of Energy
3 types of systems
4 types of energy changes
Heat capacity vs. Specific heat capacity
q = C∆T and q = mc∆T
Phase Change vs. Chemical Change
Enthalpy and Enthalpy change
Molar enthalpy
Representing enthalpy change
o Thermochemical equations
o ∆H notation
o Enthalpy Diagrams
q = n∆H
Heating and Cooling Curves
Total Heat Released or Absorbed by a System
Calorimetry
o Coffee Cup Calorimeter
o Bomb Calorimeter
Hess’s Law
Bond Energy
Lab
STSE #3 – What Fuel’s You
Unit IV: Electrochemistry
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Oxidation and Reduction Reactions
Oxidation vs. Reduction
Half Reactions
Oxidizing Agent vs. Reducing Agent
Balancing Redox Reactions in Neutral solutions
Oxidations Numbers/States
Identifying Redox Reactions
Balancing Redox Reactions
o Acidic
o Basic
Redox Stoichiometry
Electrochemical Cells
Cell Potentials
Electrolytic Cell
o Electrolysis of water
o Electrolysis of molten salts
o Electrolysis of aqueous solutions
Faraday’s Law
Batteries
Hydrogen Fuel Cells
STSE #4: From Minerals to Metal