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29. Metals in biology
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Classroom Contents
Principles of Chemical Science
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- 1 1. The importance of chemical principles
- 2 2. Discovery of electron and nucleus, need for quantum mechanics
- 3 3. Wave-particle duality of light
- 4 4. Wave-particle duality of matter, Schrödinger equation
- 5 5. Hydrogen atom energy levels
- 6 6. Hydrogen atom wavefunctions (orbitals)
- 7 7. p-orbitals
- 8 8. Multielectron atoms and electron configurations
- 9 9. Periodic trends
- 10 10. Periodic trends continued; Covalent bonds
- 11 11. Lewis structures
- 12 12. Exceptions to Lewis structure rules; Ionic bonds
- 13 13. Polar covalent bonds; VSEPR theory
- 14 14. Molecular orbital theory
- 15 15. Valence bond theory and hybridization
- 16 16. Determining hybridization in complex molecules; Thermochemistry, bond energies/bond enthalpies
- 17 17. Entropy and disorder
- 18 18. Free energy and control of spontaneity
- 19 19. Chemical equilibrium
- 20 20. Le Chatelier's principle and applications to blood-oxygen levels
- 21 21. Acid-base equilibrium: Is MIT water safe to drink?
- 22 22. Chemical and biological buffers
- 23 23. Acid-base titrations
- 24 24. Balancing oxidation/reduction equations
- 25 25. Electrochemical cells
- 26 26. Chemical and biological oxidation/reduction reactions
- 27 27. Transition metals and the treatment of lead poisoning
- 28 28. Crystal field theory
- 29 29. Metals in biology
- 30 30. Magnetism and spectrochemical theory
- 31 31. Rate laws
- 32 32. Nuclear chemistry and elementary reactions
- 33 33. Reaction mechanism
- 34 34. Temperature and kinetics
- 35 35. Enzyme catalysis
- 36 36. Biochemistry
