1. Bonding Thermodynamics: why reactions occur Kinetics:
how reactions occur
Organic chemistry:
chemistry of carbon
chemistry of life
Bonding
Lewis dot structures:
valence e- used in bonding
# valence e- =
group #
“noble gas”
= 8 valence e-

2. Lewis structures CH3OH 1. Determine # valence e-
element group number e- C IV 4 H I 1 O VI 6
2. Place least electronegative element
in center (never H)

3. non-polar covalent  0.4
polar covalent
NaCl =
= 2.1
ionic
Cl-Cl = = covalent
C-O = =
1.0
polar covalent
C-H = =
0.4
covalent

4. Lewis structures 1. Determine # valence e-
2. Place least electronegative element
in center (never H) C
3. Make single bond (2e-) between each
pair of atoms
4. Use remaining e- to satisfy octet rule
5. Use double or triple bonds to reduce
# of unshared e-

5. Lewis structures : : : : : : : CH3OH C H O valence e- 4 4 6 14 e- H H

6. Lewis structures formal charge COCl2 C O Cl valence e- 4 6 14 24 e- ..7
- 4
- 2
= +1 .. .. .. .. O .. ..
6 - 6
- 1
= -1 .. C O Cl 7
- 6
- 1
= 0 ..
6 - 4
- 2
= 0
group number
- unshared e- -
(1/2) shared e-

7. VSEPR Molecular geometries : H2O : : H O H : 4- :
H2O : : H O H + + : 4
pairs of valence e- on O
tetrahedron
bonds angles o
actually 108o
polar bonds
dipole moment
H-bonding
H bound to O, N,
F =
H-bond donor O, .. N, .. .. F
= H-bond acceptor

8. VSEPR Molecular geometries : CH2O : : H C H : : : O : 3+ :
CH2O : : H C H : : : O : - 3
pairs of e- on C
trigonal planar
bonds angles 120o
polar bond
dipole moment
dipole-dipole

9. VSEPR Molecular geometries : : CO2 : : : : : : O C O : :+ :
CO2 : : : : : : O C O : : - -
2 bonding pairs of e- on C
linear
bonds angles 180o
polar bonds
no dipole moment
LDF

10. : H2O : : H O H : O ___ s electrons ___ p electrons 2
4 equivalent orbitals 4
Hybridization
atomic orbitals s p s p 3
-bond
molecular orbitals

11. H : C : H CH2O : : : : O C ___ s electrons ___ p electrons 2
3 equivalent orbitals 2
Hybridization
atomic orbitals s p p
-bond
sp2
-bond
molecular orbitals

12. H : C : H CH2O : : : : O O ___ s electrons ___ p electrons 2
3 equivalent orbitals 4
Hybridization
atomic orbitals s p p
-bond
sp2
-bond
molecular orbitals

13. : : CO2 : : : : O C O : : C ___ s electrons ___ p electrons 2
2 equivalent orbitals 2
Hybridization
atomic orbitals s p p
-bond sp
-bond
molecular orbitals

14. : : CO2 : : : : O C O : : O ___ s electrons ___ p electrons 2
3 equivalent orbitals 4
Hybridization
atomic orbitals s p p
-bond
sp2
-bond
molecular orbitals