| L1 |
The importance of chemical principles |
| L2 |
Discovery of electron and nucleus, need for quantum mechanics |
| L3 |
Wave-particle duality of light |
| L4 |
Wave-particle duality of matter, Schrödinger equation |
| L5 |
Hydrogen atom energy levels |
| L6 |
Hydrogen atom wavefunctions (orbitals) |
| L7 |
p-orbitals |
| L8 |
Multielectron atoms and electron configurations |
| L9 |
Periodic trends |
| L10 |
Periodic trends continued; Covalent bonds |
| L11 |
Lewis structures |
| L12 |
Exceptions to Lewis structure rules; Ionic bonds |
| L13 |
Polar covalent bonds; VSEPR theory |
| L14 |
Molecular orbital theory |
| L15 |
Valence bond theory and hybridization |
| L16 |
Determining hybridization in complex molecules; Thermochemistry and bond energies/bond enthalpies |
| L17 |
Entropy and disorder |
| L18 |
Free energy and control of spontaneity |
| L19 |
Chemical equilibrium |
| L20 |
Le Chatelier's principle and applications to blood-oxygen levels |
| L21 |
Acid-base equilibrium: Is MIT water safe to drink? |
| L22 |
Chemical and biological buffers |
| L23 |
Acid-base titrations |
| L24 |
Balancing oxidation/reduction equations |
| L25 |
Electrochemical cells |
| L26 |
Chemical and biological oxidation/reduction reactions |
| L27 |
Transition metals and the treatment of lead poisoning |
| L28 |
Crystal field theory |
| L29 |
Metals in biology |
| L30 |
Magnetism and spectrochemical theory |
| L31 |
Rate laws |
| L32 |
Nuclear chemistry and elementary reactions |
| L33 |
Reaction mechanism |
| L34 |
Temperature and kinetics |
| L35 |
Enzyme catalysis |
| L36 |
Biochemistry |