1. BONDING PICTURES

2. Know what picture to draw for each hybridization

3. sp hybridization: 2 regions of electrons

4. sp 2 hybridization: 3 regions of electrons

5. sp 3 hybridization : 4 regions of electrons

6. sp 3 d hybridization : 5 regions of electrons

7.  and  bonds with sp 2 hybridization  Draw like this:

8. Fluorine F 2  Valence electrons:  7 + 7 = 14  Lewis Dot  Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 13Tetrahedralpaired

9. Fluorine

10. Water H 2 O  Valence electrons:  6 + 1+1 = 8  Lewis Dot Bond angle: <109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 22Tetrahedralbent

11. Water = = H H

12. Ammonia NH 3  Valence electrons:  5 +1+1 +1= 8  Lewis Dot  Bond angle: <109.5  Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 31Tetrahedralpyramidal

13. Ammonia

14. Methane CH 4  Valence electrons:  4 + 4(1) = 8  Lewis Dot  Bond angle: 109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 40Tetrahedral

15. Methane

16. Hydrogen Peroxide H 2 O 2  Valence electrons:  6+6+1+1 = 14  Lewis Dot  Bond angle: <109.5 ° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 22Tetrahedralbent

17. Hydrogen Peroxide =

18. Carbon tetrachloride CCl 4  Valence electrons:  4 + 4(7) = 32  Lewis Dot Bond angle: 109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 40Tetrahedral

19. Carbon tetrachloride = == = = = = = = = = = = == =

20. Hydrogen sulfide H 2 S  Valence electrons:  6 + 1+1 = 8  Lewis Dot  Bond angle: <109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 22Tetrahedralbent

21. Hydrogen sulfide = = = =

22. Hydrogen chloride HCl  Valence electrons:  7 +1= 8  Lewis Dot  Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 13Tetrahedralpaired

23. Hydrogen chloride = = =

24. Oxygen O 2  Valence electrons:  6 + 6 = 12  Lewis Dot  Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 12Trigonal planarpaired

25. Oxygen  Only draw the axes -- not necessary to draw p orbital balloons

26. Nitrogen N 2  Valence electrons:  5 + 5 = 10  Lewis Dot  Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 11Linearpaired

27. Nitrogen = ==

28. Carbon dioxide CO 2  Valence electrons:  4 +6+6 = 16  Lewis Dot Bond angle: 180° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry C: 20Linear O: 12Trigonal planar paired

29. Carbon dioxide

30. Sulfur trioxide SO 3  Valence electrons:  6 + 6 + 6 + 6 = 24  Lewis Dot  Bond angle: 120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry S: 30Trigonal planar O: 13TetrahedralPaired O: 12Trigonal planarpaired

31. Sulfur trioxide

32. Carbon monoxide CO  Valence electrons:  4 + 6 = 10  Lewis Dot  Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 11Linearpaired

33. Carbon monoxide = == CO

34. Ozone O 3  Valence electrons:  6 + 6+6 = 18  Lewis Dot  Bond angle: <120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 21Trigonal planarbent

35. Ozone

36. Phosphorus pentachloride PCl 5  Valence electrons:  5 + 5(7) = 40  Lewis Dot  Bond angle: 90° and 120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 50Trigonal bipyramidal

37. Phosphorus pentachloride

38. Sulfur hexafluoride SF 6  Valence electrons:  6 + 6(7) = 48  Lewis Dot  Bond angle: 90° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 60Octahedraloctahedral

39. Sulfur hexafluoride

40. Nitrate NO 3 -  Valence electrons:  5 + 3(6) +1 = 24  Lewis Dot  Bond angle: 120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 30Trigonal planar

41. nitrate

42. Phosphate PO 4 -3  Valence electrons:  5 + 4(6) + 3 = 32  Lewis Dot -3  Bond angle: 109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 4OTetrahedraltetrahedral

43. Phosphate = = = = = = = = = = = = = == =

44. Sulfate SO 4 -2  Valence electrons:  6 + 4(6) +2 = 32  Lewis Dot  Bond angle: 109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 40Tetrahedraltetrahedral -2

45. Sulfate = = = = = = = = = = = = = == =

46. Chlorate ClO 3 -  Valence electrons:  7 + 3(6)+1 = 26  Lewis Dot  Bond angle: <109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 31Tetrahedralpyramidal

47. Chlorate

48. Ethane C 2 H 6  Valence electrons:  2(4) + 6(1) = 14  Lewis Dot  Bond angle: 109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 40Tetrahedraltetrahedral

49. Ethane

50. Ethene C 2 H 4  Valence electrons:  2(4) + 4(1) = 12  Lewis Dot  Bond angle: 120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 30Trigonal planar

51. Ethene C 2 H 4 = = = = = =

52. Ethyne C 2 H 2  Valence electrons:  2(4) + 2(1) = 10  Lewis Dot  Bond angle: 180° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 20Linearlinear

53. Ethyne C 2 H 2

54. Sulfur Dioxide SO 2  Valence electrons:  6 + 2(6) = 18  Lewis Dot  Bond angle: <120° Bonding regionsNonbonding pairs Central atom geometry Molecular geometry 21Trigonal planarbent

55. Sulfur Dioxide

56. Cyanide CN -  Valence electrons:  4 + 5 + 1= 10  Lewis Dot Bond angle: N/A Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 11Linearpaired

57. Cyanide == =

58. Nitrite NO 2 -  Valence electrons:  5 + 2(6)+1 = 18  Lewis Dot  Bond angle: <120° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 21Trigonal planarbent

59. Nitrite

60. Hydronium H 3 O +  Valence electrons:  6 + 3(1) -1 = 8  Lewis Dot  Bond angle: <109.5° Bonding regions Nonbonding pairs Central atom geometry Molecular geometry 31Tetrahedralpyramidal +

61. Hydronium