Thermodynamics why reactions occur Kinetics how reactions occur

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-

Lewis structures CH 3 OH 1. Determine # valence eelement group number C IV H I O VI e 4 1 6 2. Place least electronegative element in center (never H)

non-polar covalent 0. 4 polar covalent 0. 5 -1. 8 Na. Cl = 3. 0 - 0. 9 = 2. 1 ionic Cl-Cl = 3. 0 - 3. 0 = 0. 0 covalent C-O = 3. 5 - 2. 5 = 1. 0 polar covalent C-H = 2. 5 - 2. 1 = 0. 4 covalent

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

Lewis structures CH 3 OH H 4 O 6 : H H : C : O : H H : : : valence e- C 4 14 e-

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

VSEPR Molecular geometries + H: O: H + : : H 2 O - - on O pairs of valence e tetrahedron 4 bonds angles 109. 5 o actually 108 o polar bonds dipole moment H-bonding . . H bound to O, N, F =H-bond donor. . . O, . . N, F. . = H-bond acceptor

VSEPR Molecular geometries H : C: H : O: : CH 2 O + 3 pairs of e- on C trigonal planar bonds angles 120 o polar bond dipole moment dipole-dipole

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

H: O: H O : : H 2 O ___ 2 s electrons ___ 4 p electrons 4 equivalent orbitals Hybridization p s atomic orbitals sp 3 -bond molecular orbitals

H : C : H : O : C : : CH 2 O ___ 2 s electrons ___ 2 p electrons 3 equivalent orbitals Hybridization p s atomic orbitals p -bond sp 2 -bond molecular orbitals

H : C : H : O : : CH 2 O ___ 2 s electrons ___ 4 p electrons 3 equivalent orbitals Hybridization p -bond p s atomic orbitals sp 2 -bond molecular orbitals

C : : CO 2 : : O : : C: : O ___ 2 s electrons ___ 2 p electrons 2 equivalent orbitals Hybridization p sp s atomic orbitals molecular orbitals p -bond

O : : CO 2 : : O : : C: : O ___ 2 s electrons ___ 4 p electrons 3 equivalent orbitals Hybridization p sp 2 s atomic orbitals molecular orbitals p -bond