Connects cell potential with Gibbs free energy, explains standard reduction potentials and redox strength, and derives the Nernst equation for nonstandard conditions and equilibrium.
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MIT 5.111SC: Principles of Chemical Science
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- 01-The Importance of Chemical Principles
01-The Importance of Chemical Principles
- 02-Atomic Structure
- 03-Wave-Particle Duality of Light
- 04-Wave-Particle Duality of Matter; Schrödinger Equation
- 05-Hydrogen Atom Energy Levels
- 06-Hydrogen Atom Wavefunctions (Orbitals)
- 07-Multi-electron Atoms
- 08-The Periodic Table and Periodic Trends
- 09-Periodic Table; Ionic and Covalent Bonds
- 10-Introduction to Lewis Structures
- 11-Lewis Structures: Breakdown of the Octet Rule
- 12-The Shapes of Molecules: VSEPR Theory
- 13-Molecular Orbital Theory
- 14-Valence Bond Theory and Hybridization
- 15-Thermodynamics: Bond and Reaction Enthalpies
- 16-Thermodynamics: Gibbs Free Energy and Entropy
- 17-Thermodynamics: Now What Happens When You Heat It Up?
- 18-Introduction to Chemical Equilibrium
- 19-Chemical Equilibrium: Le Châtelier's Principle
- 20-Solubility and Acid-Base Equilibrium
- 21-Acid-Base Equilibrium: Is MIT Water Safe to Drink?
- 22-Acid-Base Equilibrium: Salt Solutions and Buffers
- 23-Acid-Base Titrations Part I
- 24-Acid-Base Titrations Part II
- 25-Oxidation-Reduction and Electrochemical Cells
- 26-Chemical and Biological Oxidations
- 27-Introduction to Transition Metals
- 28-Transition Metals: Crystal Field Theory Part I
- 29-Transition Metals: Crystal Field Theory Part II
- 30-Kinetics: Rate Laws
- 31-Nuclear Chemistry and Chemical Kinetics
- 32-Kinetics: Reaction Mechanisms
- 33-Kinetics and Temperature
- 34-Kinetics: Catalysts
- 35-Applying Chemical Principles