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The importance of chemical principles
Discovery of electron and nucleus, need for quantum mechanics
Wave-particle duality of light
Wave-particle duality of matter, Schrödinger equation
Hydrogen atom energy levels
Hydrogen atom wavefunctions (orbitals)
p-orbitals
Multielectron atoms and electron configurations
Periodic trends
Periodic trends continued; Covalent bonds
Lewis structures
Exam 1 covering lectures 1-9
Exceptions to Lewis structure rules; Ionic bonds
Polar covalent bonds; VSEPR theory
Molecular orbital theory
Valence bond theory and hybridization
Determining hybridization in complex molecules; Thermochemistry and bond
energies/bond enthalpies
Entropy and disorder
Free energy and control of spontaneity
Exam 2 covering lectures 10-16
Chemical equilibrium
Le Chatelier's principle and applications to blood-oxygen levels
Acid-base equilibrium: Is MIT water safe to drink?
Chemical and biological buffers
Acid-base titrations
Balancing oxidation/reduction equations
Electrochemical cells
Chemical and biological oxidation/reduction reactions
Transition metals and the treatment of lead poisoning
Crystal field theory
Exam 3 covering lectures 17-26
Metals in biology
Magnetism and spectrochemical theory
Rate laws
Nuclear chemistry and elementary reactions
Reaction mechanism
Temperature and kinetics
Enzyme catalysis
Biochemistry
This course provides an introduction to the chemistry of biological, inorganic, and organic molecules. The emphasis is on basic principles of atomic and molecular electronic structure, thermodynamics, acid-base and redox equilibria, chemical kinetics, and catalysis.
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