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  1. CHEMISTRY I. Introduction A. Why study chemistry? B. Definitions 1. Chemistry 2. Matter

  2. 3. Elements

  3. 4. Molecule

  4. 5. Compound

  5. Figure 2.3

  6. Figure 5.3

  7. II. Atomic Chemistry A. Particles / Structure

  8. Figure 2.5

  9. B. Atomic & Mass Number

  10. C. Isotopes & Radioisotopes

  11. Figure 2.7

  12. Isotopes = moreneutrons but stable Radioisotopes = nucleus decay giving off alpha and beta particles, plus gamma rays. Decay = half life Why would this activity be so bad for cells?

  13. E. Electrons

  14. Figure 2.8 Figure 2.6 Figure 2.9

  15. Figure 2.10

  16. www.Ausetute.com.au

  17. Figure 2.9 Valence => number of electrons in the outermost shell

  18. Figure 2.9 Electronegativity degree of attraction for electrons

  19. III. Molecular Chemistry A. Definition B. Chemical Bonds 1. Definition 2. Types a. Electron Sharing

  20. i. Covalent bonds = sharing of valence electrons Figure 2.11

  21. Non-polar covalent bonds Figure 2.12

  22. Polar Figure 2.13

  23. ii. Ionic = giving and receiving electrons Figure 2.14 Figure 2.15

  24. b. Hydrogen Sharing

  25. Hydrogen bonds sharinga hydrogen Figure 2.16

  26. Hydrogen bonds sharinga hydrogen Figure 3.2

  27. c. VanderWalls Forces

  28. VanderWalls Forces sharinga charge

  29. C. Formulas & Models 1. Why Important?

  30. c. Structural Figure 2.18 Figure 2.17 a. Molecular b. Empirical

  31. IV. Chemical Reactions A. Definition B. Types 1. Synthesis, Dehydration, or Anabolic 2. Decomposition, Hydrolytic,or Catabolic 3. Exchange

  32. A(OH) + B(H) AB + H2O AB + H2O  A(OH) + B(H) AB + CD  AC + BD

  33. C. Factors Affecting Rates

  34. V. Inorganic Molecules A. Water 1. Properties

  35. States of Water

  36. Polar

  37. H-Bonding Potential Figure 3.2

  38. Density Figure 3.6

  39. Cohesive Forces Figure 3.4

  40. Cohesive Forces Figure 3.3