1. Molecular Shapes
Lewis structures
physical properties
VSEPR
(b.p., solubility)
polarity
separation of charge in molecule
electronegativity HF + -

2. electronegativity larger molecules molecular shape CO2 b.p. = -78oC
SO2
b.p. =
23oC : : : : : : : : : O C O : : : : O S O : : : : 2
valence pairs
linear 3
valence pairs
trigonal + + - - - -
non-polar

3. CHCl3
CCl4
water soluble
insoluble C H Cl C Cl 4
valence pairs
tetrahedral
non-polar
polar

4. Valence Bond Theory
covalent bond
overlap of orbitals
bonding e- pair
opposite spins
CH4
geometry
tetrahedral
[He]
2s2
2p2
shape
tetrahedral
Pauling
valence e- orbitals
in molecules
in atoms
mix 
produce molecular orbitals

5. sp3
mixing
hybridization
depends on
number of atomic orbitals mixed
type of atomic orbitals mixed
CH4
need equivalent orbitals 4
mix atomic orbitals 4
[He]
2s2
2p2
mix s
and 3 p
sp3

6. sp3 CH4 hydrogen sigma bond [He] 2s2 2p2  bond sp3 p energy
hybridization
sp3 s
CH4
hydrogen
sigma bond
[He]
2s2
2p2 s
 bond
sp3

7. sp2
formaldehyde
CH2O C : H O 3
valence pairs on C 3
hybrid orbitals
[He]
2s2
2p2 sp 2

8. sp2  -bond -bond : C H O p p energy hybridization sp2 s p p energy

9. sp CO2 C :: O : 2 hybridized bonds 2 unhybridized bonds s + p sp

10. sp C : :: C O -bond end-to-end -bond side-to-side O p p energy
hybridization C sp s C :: O :
-bond
end-to-end
-bond
side-to-side p p
energy
hybridization O
sp2 s

11. PCl5
trigonal bipyramidal P Cl 5
hybridized orbitals 5
mix s
+ 3p
+ d
dsp3

12. SF6
octahedral S F 6
hybridized orbitals 6
mix s
+ 3p
+ 2d
d2sp3