MIT 5.111 Principles of Chemical Science, Fall 2008 (English)

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Lecture 1: 1. The importance of chemical principles

Lecture 2: 2. Discovery of electron and nucleus, need for quantum mechanics

Lecture 3: 3. Wave-particle duality of light

Lecture 4: 4. Wave-particle duality of matter, Schrödinger equation

Lecture 5: 5. Hydrogen atom energy levels

Lecture 6: 6. Hydrogen atom wavefunctions (orbitals)

Lecture 7: 7. p-orbitals

Lecture 8: 8. Multielectron atoms and electron configurations

Lecture 9: 9. Periodic trends

Lecture 10: 10. Periodic trends continued; Covalent bonds

Lecture 11: 11. Lewis structures

Lecture 12: 12. Exceptions to Lewis structure rules; Ionic bonds

Lecture 13: 13. Polar covalent bonds; VSEPR theory

Lecture 14: 14. Molecular orbital theory

Lecture 15: 15. Valence bond theory and hybridization

Lecture 16: 16. Determining hybridization in complex molecules; Thermochemistry, bond energies/bond enthalpies

Lecture 17: 17. Entropy and disorder

Lecture 18: 18. Free energy and control of spontaneity

Lecture 19: 19. Chemical equilibrium

Lecture 20: 20. Le Chatelier's principle and applications to blood-oxygen levels

Lecture 21: 21. Acid-base equilibrium: Is MIT water safe to drink?

Lecture 22: 22. Chemical and biological buffers

Lecture 23: 23. Acid-base titrations

Lecture 24: 24. Balancing oxidation/reduction equations

Lecture 25: 25. Electrochemical cells

Lecture 26: 26. Chemical and biological oxidation/reduction reactions

Lecture 27: 27. Transition metals and the treatment of lead poisoning

Lecture 28: 28. Crystal field theory

Lecture 29: 29. Metals in biology

Lecture 30: 30. Magnetism and spectrochemical theory

Lecture 31: 31. Rate laws

Lecture 32: 32. Nuclear chemistry and elementary reactions

Lecture 33: 33. Reaction mechanism

Lecture 34: 34. Temperature and kinetics

Lecture 35: 35. Enzyme catalysis

Lecture 36: 36. Biochemistry