BONDING PICTURES. Know what picture to draw for each hybridization.
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Transcript of BONDING PICTURES. Know what picture to draw for each hybridization.
BONDING PICTURES
Know what picture to draw for each hybridization
sp hybridization: 2 regions of electrons
sp2 hybridization: 3 regions of electrons
sp3 hybridization : 4 regions of electrons
sp3d hybridization : 5 regions of electrons
and bonds with sp2 hybridization
Draw like this:
Fluorine F2
Valence electrons: 7 + 7 = 14
Lewis Dot
Bond angle: N/A
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
1 3 Tetrahedral paired
Fluorine
Water H2O
Valence electrons: 6 + 1+1 = 8
Lewis Dot
Bond angle: <109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 2 Tetrahedral bent
Water
==
H
H
Ammonia NH3
Valence electrons: 5 +1+1 +1= 8
Lewis Dot
Bond angle: <109.5
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
3 1 Tetrahedral pyramidal
Ammonia
Methane CH4
Valence electrons: 4 + 4(1) = 8
Lewis Dot
Bond angle: 109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
4 0 Tetrahedral Tetrahedral
Methane
Hydrogen Peroxide H2O2
Valence electrons: 6+6+1+1 = 14
Lewis Dot
Bond angle: <109.5 °
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 2 Tetrahedral bent
Hydrogen Peroxide
=
Carbon tetrachloride CCl4
Valence electrons: 4 + 4(7) = 32
Lewis Dot
Bond angle: 109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
4 0 Tetrahedral Tetrahedral
Carbon tetrachloride
===
=
==
==
==
==
=
= =
=
Hydrogen sulfide H2S
Valence electrons: 6 + 1+1 = 8
Lewis Dot
Bond angle: <109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 2 Tetrahedral bent
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
1 3 Tetrahedral paired
Hydrogen chloride
=
==
Oxygen O2
Valence electrons: 6 + 6 = 12
Lewis Dot
Bond angle: N/A
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
1 2 Trigonal planar
paired
Oxygen
Only draw the axes -- not necessary to draw p orbital balloons
Nitrogen N2
Valence electrons: 5 + 5 = 10
Lewis Dot
Bond angle: N/A
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
1 1 Linear paired
Nitrogen
= ==
Carbon dioxide CO2
Valence electrons: 4 +6+6 = 16
Lewis Dot
Bond angle: 180°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
C: 2 0 Linear Linear
O: 1 2 Trigonal planar
paired
Carbon dioxide
Sulfur trioxide SO3
Valence electrons: 6 + 6 + 6 + 6 = 24
Lewis Dot
Bond angle: 120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
S: 3 0 Trigonal planar
Trigonal planar
O: 1 3 Tetrahedral Paired
O: 1 2 Trigonal planar
paired
Sulfur trioxide
Carbon monoxide CO
Valence electrons: 4 + 6 = 10
Lewis Dot
Bond angle: N/A
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
1 1 Linear paired
Carbon monoxide
= ==C O
Ozone O3
Valence electrons: 6 + 6+6 = 18
Lewis Dot
Bond angle: <120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 1 Trigonal planar
bent
Ozone
Phosphorus pentachloride PCl5 Valence electrons:
5 + 5(7) = 40 Lewis Dot
Bond angle: 90° and 120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
5 0 Trigonal bipyramidal
Trigonal bipyramidal
Phosphorus pentachloride
Sulfur hexafluoride SF6
Valence electrons: 6 + 6(7) = 48
Lewis Dot
Bond angle: 90°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
6 0 Octahedral octahedral
Sulfur hexafluoride
Nitrate NO3-
Valence electrons: 5 + 3(6) +1 = 24
Lewis Dot
Bond angle: 120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
3 0 Trigonal planar
Trigonal planar
nitrate
Phosphate PO4-3
Valence electrons: 5 + 4(6) + 3 = 32
Lewis Dot -3
Bond angle: 109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
4 O Tetrahedral tetrahedral
Phosphate =
==
=
==
==
=
=
==
=
= =
=
Sulfate SO4-2
Valence electrons: 6 + 4(6) +2 = 32
Lewis Dot
Bond angle: 109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
4 0 Tetrahedral tetrahedral
-2
Sulfate=
==
=
==
==
=
=
==
=
= =
=
Chlorate ClO3-
Valence electrons: 7 + 3(6)+1 = 26
Lewis Dot
Bond angle: <109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
3 1 Tetrahedral pyramidal
Chlorate
Ethane C2H6
Valence electrons: 2(4) + 6(1) = 14
Lewis Dot
Bond angle: 109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
4 0 Tetrahedral tetrahedral
Ethane
Ethene C2H4
Valence electrons: 2(4) + 4(1) = 12
Lewis Dot
Bond angle: 120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
3 0 Trigonal planar
Trigonal planar
Ethene C2H4
=
=
=
=
=
=
Ethyne C2H2
Valence electrons: 2(4) + 2(1) = 10
Lewis Dot
Bond angle: 180°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 0 Linear linear
Ethyne C2H2
Sulfur Dioxide SO2
Valence electrons: 6 + 2(6) = 18
Lewis Dot
Bond angle: <120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 1 Trigonal planar
bent
Sulfur Dioxide
Cyanide CN-
Valence electrons: 4 + 5 + 1= 10
Lewis Dot
Bond angle: N/A
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
1 1 Linear paired
Cyanide
= ==
Nitrite NO2 -
Valence electrons: 5 + 2(6)+1 = 18
Lewis Dot
Bond angle: <120°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
2 1 Trigonal planar
bent
Nitrite
Hydronium H3O+
Valence electrons: 6 + 3(1) -1 = 8
Lewis Dot
Bond angle: <109.5°
Bonding regions
Nonbonding pairs
Central atom geometry
Molecular geometry
3 1 Tetrahedral pyramidal
+
Hydronium