04. hybridization 2010
TRANSCRIPT
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1CHEM 212
Nicolas Moitessier
Chemical BondsChemical bonds
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2CHEM 212
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Information
Introduction: What is Organic Chemistry ?
Structures: Ch. 1.3
Alkanes: Ch. 2.1-2.3
Functional groups: Ch. 2.5-2.13
Chemical Bonding & Lewis Structures: Ch. 1.4-1.6
Formal Charges and Resonance: Ch. 1.7-1.8
VSEPR Theory Ch. 1.16
Hybridization Ch. 1.11-1.15
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3CHEM 212
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Chemical Bonding
Bonds can be
Covalent. Ex.: CH4
Atoms achieve octets by sharing of valence electrons
Ionic Ex. NaCl, LiFOctet rule: Lithium loses an electron and becomes positively charged
Fluoride gains an electron and becomes negatively chargedThe charged lithium and fluoride form a strong ionic bond
C
H
H H
HC
H
HH
H
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4CHEM 212
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Valence Bond Theory
The covalent bond results from an overlap of atomic
orbitals containing one unpaired electron each Pauling (Nobel in Chemistry 1954 in Peace 1962)
Aufbau orbitals are filled so that those of lowest energy are filled first
Pauli a maximum of two electrons with paired spins may be placed in each
orbital
Hund With orbitals of equal energy, one electron (unpaired spins) is added to
each until each contains one electron
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5CHEM 212
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The Covalent Bond - Pauling
Sharing of unpaired electrons
H H
1s 1s
1s 1s
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6CHEM 212
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The Covalent Bond - Pauling
Shairing of unpaired electrons
H H
1s 1s
σ bond
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7CHEM 212
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H2
1s + 1s = σ
H H H2
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8CHEM 212
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F2
p-p Overlap
F1s 2s 2p
F
1s 2s 2p
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9CHEM 212
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He2
?
No unpaired electrons
This molecule cannot exist
He He
1s 1s
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10CHEM 212
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HF?
Unpaired electrons
s-p overlap
F
1s 2s 2p
H
1s
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HF
Fluoride is more electronegative than H:
polarized bond
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12CHEM 212
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Single bonds
Carbon atom
4 sp3 electrons
C
1s 2s 2p
C
1s 2s 2p
H
1s
jump
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Hybridization
2s + 2px+ 2py+ 2pz= 4 sp3 e-
C
1s 2s 2p
sp3
Hybri dization
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14CHEM 212
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Methane
Hybridization
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Methane
Bond formation
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Methane
Lewis Structure
Geometry (VSEPR)
Bonding (Valence bond theory): 4
equivalent σ bonds
C H
H
H
H
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Multiple bonds
Ethylene
Lewis structure
VSEPR: 2 trigonal planar carbons
Valence bond theory: 1σ and 1π
C C
H
H
H
H
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18CHEM 212
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Hybridization
C
2s 2p
sp2 p
C
2s 2p
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19CHEM 212 Nicolas Moitessier
Ethylene
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20CHEM 212 Nicolas Moitessier
Ethylene
sp2 p
3 σ bonds 1 π bond
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π bond
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22CHEM 212 Nicolas Moitessier
Triple bond
Acetylene (ethyne)
Lewis structure
VSEPR: 2 linear carbons
Valence bond theory: 1σ and 2π
C C HH
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23CHEM 212 Nicolas Moitessier
Triple Bonds
C
2s 2p
sp p
C
2s 2p
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24CHEM 212 Nicolas Moitessier
Acetylene
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25CHEM 212 Nicolas Moitessier
Acetylene
sp p
sp p
H
s
H
s
σ bond 2 π bonds
σ bond
σ bond
C C HH C C HH C C HH C CC C HH C CC C HH C C
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26CHEM 212 Nicolas Moitessier
The electron configuration shown
below represents
1 2 3 4 5
0% 0% 0%0%0%
1s 2sp3 2sp3 2sp3 2sp3
1. the ground state of boron.
2. the sp3 hybridized state ofcarbon
3. the sp3 hybridized state ofnitrogen
4. the ground state of carbon.5. an excited state of carbon.