BONDING PICTURES

Know what picture to draw for each hybridization

sp hybridization: 2 regions of electrons

sp 2 hybridization: 3 regions of electrons

sp 3 hybridization : 4 regions of electrons

sp 3 d hybridization : 5 regions of electrons

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

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

Fluorine

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

Water = = H H

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

Ammonia

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

Methane

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

Hydrogen Peroxide =

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

Carbon tetrachloride = == = = = = = = = = = = == =

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

Hydrogen sulfide = = = =

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

Hydrogen chloride = = =

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

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

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

Nitrogen = ==

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

Carbon dioxide

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

Sulfur trioxide

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

Carbon monoxide = == CO

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

Ozone

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

Phosphorus pentachloride

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

Sulfur hexafluoride

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

nitrate

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

Phosphate = = = = = = = = = = = = = == =

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

Sulfate = = = = = = = = = = = = = == =

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

Chlorate

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

Ethane

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

Ethene C 2 H 4 = = = = = =

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

Ethyne C 2 H 2

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

Sulfur Dioxide

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

Cyanide == =

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

Nitrite

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 +

Hydronium