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

3. 3. 3. Elements

6. 4. 4. Molecule

7. 5. 5. Compound

8. Figure 2.3

10. Figure 5.3

11. A. A. Particles / Structure II. Atomic Chemistry

12. Figure 2.5

14. B. B. Atomic & Mass Number

16. C. C. Isotopes & Radioisotopes

18. Figure 2.7

19. Isotopes = more neutrons 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?

20. E. E. Electrons

21. Figure 2.8 Figure 2.9 Figure 2.6

22. Figure 2.10

23. AtomNo. ElectronsSub shell Electron ConfigurationIonNo. Electrons Sub shell Electron Configuration H11s 1 H-H- 1 + 1 = 21s 2 He21s 2 Li31s 2 2s 1 Li + 3 - 1 = 21s 2 Be41s 2 2s 2 Be 2+ 4 - 2 = 21s 2 B51s 2 2s 2 2p 1 B 3+ 5 - 3 = 21s 2 C61s 2 2s 2 2p 2 C 4+ 6 - 4 = 21s 2 N71s 2 2s 2 2p 3 N 3- 7 + 3 = 101s 2 2s 2 2p 6 O81s 2 2s 2 2p 4 O 2- 8 + 2 = 101s 2 2s 2 2p 6 F91s 2 2s 2 2p 5 F-F- 9 + 1 = 101s 2 2s 2 2p 6 Ne101s 2 2s 2 2p 6 Na111s 2 2s 2 2p 6 3s 1 Na + 11 - 1 = 101s 2 2s 2 2p 6 Mg121s 2 2s 2 2p 6 3s 2 Mg 2+ 12 - 2 = 101s 2 2s 2 2p 6 Al131s 2 2s 2 2p 6 3s 2 3p 1 Al 3+ 13 - 3 = 101s 2 2s 2 2p 6 Si141s 2 2s 2 2p 6 3s 2 3p 2 Si 4+ 14 - 4 = 101s 2 2s 2 2p 6 P151s 2 2s 2 2p 6 3s 2 3p 3 P 3- 15 + 3 = 181s 2 2s 2 2p 6 3s 2 3p 6 S161s 2 2s 2 2p 6 3s 2 3p 4 S 2- 16 + 2 = 181s 2 2s 2 2p 6 3s 2 3p 6 Cl171s 2 2s 2 2p 6 3s 2 3p 5 Cl - 17 + 1 = 181s 2 2s 2 2p 6 3s 2 3p 6 Ar181s 2 2s 2 2p 6 3s 2 3p 6 www.Ausetute.com.au

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

25. Electronegativity  degree of attraction for electrons Figure 2.9

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

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

28. Non-polar covalent bonds Figure 2.12

29. Polar Figure 2.13

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

31. b. Hydrogen Sharing

32. Hydrogen bonds  sharing a hydrogen Figure 2.16

33. Hydrogen bonds  sharing a hydrogen Figure 3.2

34. c. VanderWalls Forces

35. VanderWalls Forces  sharing a charge

37. 1. 1. Why Important? C. C. Formulas &Models

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

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

41. A (OH) + B (H)  AB + H2OH2O + H 2 O  A (OH) + B (H) AB + CD  AC + BD

43. C. C. Factors Affecting Rates

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

45. States of Water

46. Polar

47. H-Bonding Potential Figure 3.2

48. Density Figure 3.6

49. Cohesive Forces Figure 3.4

50. Cohesive Forces Figure 3.3

51. 2. 2. Uses

52. Solvent Figure 3.6 Figure 3.8

53. Temperature Stabilizer or Regulator

54. C. C. Acids, Acids, Bases, Bases, pH, pH, &Buffers 1. 1. Definitions & Uses

55. An acid  increases the hydrogen ion concentration H 2 CO 3  HCO 3 - + H + (Carbonic) H 2 SO 4  H + + H + + SO 4 2- (Sulfuric) HCl  H + + Cl - (Hydrochloric)

56. A base  decreases the hydrogen ion concentration HCl + NaOH  NaCl + H 2 O (Sodium Hydroxide)

57. pH Scale  measures the hydrogen ion concentration Figure 3.10

58. A buffer  regulates the pH of a solution HCO 3 - + H +  H 2 CO 3 HPO 4 -2 + H +  H 2 PO 4 - NH 3 + H +  NH 4 + How does acid precipitation affect vegetation?

59. Knowledge will always forbear over stupidity.