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BONDING PICTURES. Know what picture to draw for each hybridization.

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Presentation on theme: "BONDING PICTURES. Know what picture to draw for each hybridization."— Presentation transcript:

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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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:  = 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


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