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Molecular Geometry and Polarization - PowerPoint PPT Presentation
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Molecular Geometry and Polarization. Shapes of Molecules. Valence Shell Electron Pair Repulsion Theory (VSEPR) a. Bonded electrons b. Lone Pairs. 1. Linear (180 o ) BeH 2 CO 2. 2. Trigonal Planar (120 o ) NO 3 -. 3. Tetrahedral (109.5 o ) CH 4.
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Valence Shell Electron Pair Repulsion Theory (VSEPR)
a. Bonded electrons
b. Lone Pairs
BeH2 CO2
1. Polar molecule – Overall, the electrons are attracted more to one end of an entire molecule
2. Non-Polar Molecule – The electrons are spread out evenly over the entire molecule
-/ + Partial (not full) charges
BH2Cl PH3
- A mixing of the atomic orbitals (s, p, d, f) of the central atom
- Electrons no longer move in the old orbitals, but in a new pattern
Isolated Be 1s22s2 (Note that all Be:
electrons are paired)
To bond Be must unpair some electrons:
Bonded Be 1s22s12p1 •Be•
- Lone pairs do count towards hybridization
- Ex: H2O
Hybrid Orbitals and Multiple Bonds
- sigma () bonds – single bonds formed by hybrid orbitals
- pi () bonds – double or triple bonds, not formed by hybrid orbitals
H H
H – H C=C :N=N:
H H
One bond One bond plus One bond plus
one bond two bonds
- Each C is sp2
- Double bond does not count toward hybridization
- Each C is sp hybridized
- Twobonds do not count toward hybridization
What is the hybridization and bonding types for
H2CO? Also, what are the bond angles?
What is the hybridization and bonding types for
acetonitrile (shown)? Also, what are the bond angles?
H
H - C -C=N:
H
- Adjacent multiple bonds can overlap.
- Benzene (C6H6)
- All bond lengths are equal
Use hybrid orbital theory to explain why all the bonds in the NO3- ion are of equal length
12 a) ~110o b) BF3 flat (no lone pair)
21. a) (lin)lin b) (tetr)tr. Py c) (Trig bi)ss
d) (oh)oh e) (tetr)tetr f) (lin)lin
22 a) (Tetra) Trig. Pyramid b) (Trig planar), Trig pl
c) (Tr. Bipy) T d) (Tetra) Tetra
e) (Trig Bipy) lin f) (Tetra) Bent
- 24 a) i) Octa (sq.planar) ii) Tetrahedral
iii) Trig Bipyr.(see-saw)
b) i) Two ii) O iii) One
c) S or Se
d) Xe
26. a) 104.5o, 120o b) 109.5o, 120o
c) 107o, 104.5o d) 180o, 109.5o
28. 2 LP (NH2-, ~109o), 1 LP (NH3, 107o), 0 LP (NH4+, 109o)
30. a) ClO2- (~109.5o, 2LP) NO2- (120o, 1 LP)
b) XeF2 (4 LP around the center)
32. a) Lone Pair on P b) Lone Pair on center O
- 36. Polar = (b), (c), (e)
- Ortho and meta
- 44. Not enough p suborbitals
46. SF2 = sp3, SF4 = sp3d
48. a) sp3 b) sp c) sp2 d) sp3d
e) sp3d2
52. b) N2H4 (sp3), N2 (sp) c) N2 stronger bond
- 54. a) sp3 (C-H), sp2 (C-O) b) 36 ve c) 26 ve-
d) 2 ve- in double e) 8 ve- in lone pairs
- 56. a) 1, 120o 2, 120o 3, 105o
b) sp2, sp2, sp3
c) 21 bonds
100. In2S (I) [Kr]5s24d10
InS (II) [Kr]5s14d10
In2S3 (III) [Kr]4d10
In(III) is smallest (least mutual electron repul)
In(III) has the highest lattice energy
- a) C2H3Cl3O2 b) C2H3Cl3O2
- c) Structure CCl3CH(OH)2
