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11.18
Cyclobutadiene and Cyclooctatetraene
cyclic conjugation is necessary, but not sufficient
Requirements for Aromaticity
not
aromatic
aromatic
not
aromatic
heat of hydrogenation of benzene is 152 kJ/mol
less than 3 times heat of hydrogenation of
cyclohexene
to give cyclohexane (kJ/mol)
Heats of Hydrogenation
120 231 208
Heats of Hydrogenation
to give cyclooctane (kJ/mol)
heat of hydrogenation of cyclooctatetraene is
more than 4 times heat of hydrogenation of
cyclooctene
97 205 303 410
structure of a stabilized derivative is characterized
by alternating short bonds and long bonds
Structure of Cyclobutadiene
C(CH3)3
(CH3)3C
CO2CH3
(CH3)3C
138 pm
151 pm
Structure of Cyclooctatetraene
cyclooctatetraene is not planar
has alternating long (146 pm)
and short (133 pm) bonds
Conclusion
there must be some factor in addition
to cyclic conjugation that determines
whether a molecule is aromatic or not
11.19
Hückel's Rule:
Annulenes
the additional factor that influences
aromaticity is the number of p electrons
among planar, monocyclic, completely
conjugated polyenes, only those with 4n + 2
p electrons possess special stability (are
aromatic)
n 4n+2
0 2
1 6
2 10
3 14
4 18
Hückel's Rule
among planar, monocyclic, completely
conjugated polyenes, only those with 4n + 2
p electrons possess special stability (are
aromatic)
n 4n+2
0 2
1 6 benzene!
2 10
3 14
4 18
Hückel's Rule
Hückel restricted his analysis to planar,
completely conjugated, monocyclic polyenes
he found that the p molecular orbitals of
these compounds had a distinctive pattern
one p orbital was lowest in energy, another
was highest in energy, and the others
were arranged in pairs between the highest
and the lowest
Hückel's Rule
p-MOs of Benzene
Benzene
Antibonding
Bonding
6 p orbitals give 6 p orbitals
3 orbitals are bonding; 3 are antibonding
Benzene
Antibonding
Bonding
6 p electrons fill all of the bonding orbitals
all p antibonding orbitals are empty
p-MOs of Benzene
Cyclo-
butadiene
Antibonding
Bonding
4 p orbitals give 4p orbitals
1 orbital is bonding, one is antibonding, and 2
are nonbonding
p-MOs of Cyclobutadiene
(square planar)
Cyclo-
butadiene
Antibonding
Bonding
4 p electrons; bonding orbital is filled; other 2
p electrons singly occupy two nonbonding orbitals
p-MOs of Cyclobutadiene
(square planar)
Antibonding
Bonding
8 p orbitals give 8 p orbitals
3 orbitals are bonding, 3 are antibonding, and 2
are nonbonding
p-MOs of Cyclooctatetraene
(square planar)
Cyclo-
octatetraene
Antibonding
Bonding
8 p electrons; 3 bonding orbitals are filled; 2
nonbonding orbitals are each half-filled
p-MOs of Cyclooctatetraene
(square planar)
Cyclo-
octatetraene
p-Electron Requirement for Aromaticity
not
aromatic
aromatic
not
aromatic
4 p electrons 6 p electrons 8 p electrons
Completely Conjugated Polyenes
aromatic
6 p electrons;
completely conjugated
not
aromatic
6 p electrons;
not completely
conjugated
H H
Annulenes are planar, monocyclic, completely
conjugated polyenes. That is, they are the
kind of hydrocarbons treated by Hückel's
rule.
Annulenes
predicted to be aromatic by Hückel's rule,
but too much angle strain when planar and
all double bonds are cis
10-sided regular polygon has angles of 144°
[10]Annulene
incorporating two trans double bonds into
the ring relieves angle strain but introduces
van der Waals strain into the structure and
causes the ring to be distorted from planarity
[10]Annulene
incorporating two trans double bonds into
the ring relieves angle strain but introduces
van der Waals strain into the structure and
causes the ring to be distorted from planarity
[10]Annulene
van der Waals
strain between
these two hydrogens
14 p electrons satisfies Hückel's rule
van der Waals strain between hydrogens inside
the ring
[14]Annulene
H H
H H
16 p electrons does not satisfy Hückel's rule
alternating short (134 pm) and long (146 pm) bonds
not aromatic
[16]Annulene
18 p electrons satisfies Hückel's rule
resonance energy = 418 kJ/mol
bond distances range between 137-143 pm
[18]Annulene
H H
H
H
H
H
11.20
Aromatic Ions
6 p electrons delocalized
over 7 carbons
positive charge dispersed
over 7 carbons
very stable carbocation
also called tropylium cation
Cycloheptatrienyl Cation
H H
H
H
H H
H
+
Cycloheptatrienyl Cation
H H
H
H
H H
H
+
+
H H
H
H
H H
H
Tropylium cation is so stable that tropylium
bromide is ionic rather than covalent.
mp 203 °C; soluble in water; insoluble in
diethyl ether
Cycloheptatrienyl Cation
H Br
+ Br–
Ionic Covalent
Cyclopentadienide Anion
H H
H H
H
••
–
6 p electrons delocalized
over 5 carbons
negative charge dispersed
over 5 carbons
stabilized anion
Cyclopentadienide Anion
H H
H H
H
••
–
H H
H H
H
–
Acidity of Cyclopentadiene
H H
H H
H H
H H
H H
H
••
–
H+ +
pKa = 16
Ka = 10-16
Cyclopentadiene is
unusually acidic for a
hydrocarbon.
Increased acidity is due to
stability of cyclopentadienide
anion.
Electron Delocalization in Cyclopentadienide Anion
H H
H H
H
••
–
Electron Delocalization in Cyclopentadienide Anion
H H
H H
H
••
–
H H
H H
H
••
–
Electron Delocalization in Cyclopentadienide Anion
H H
H H
H
••
–
H H
H H
H
••
–
H H
H H
H
•
• –
Electron Delocalization in Cyclopentadienide Anion
H H
H H
H
••
–
H H
H H
H
••
–
H H
H H
H
•
• –
H H
H H
H
– •
•
Electron Delocalization in Cyclopentadienide Anion
H H
H H
H
••
–
H H
H H
H
••
–
H H
H H
H
H H
H H
H
•
• –
H H
H H
H
– •
•
••
Compare Acidities of
Cyclopentadiene and Cycloheptatriene
H H
H H
H H
pKa = 16
Ka = 10-16
pKa = 36
Ka = 10-36
H H
H
H
H
H H
H H
H H
H H
H
••
–
Compare Acidities of
Cyclopentadiene and Cycloheptatriene
Aromatic anion
6 p electrons
Anion not aromatic
8 p electrons
H H
H
H
H H
H
••
–
n = 0
4n +2 = 2 p electrons
Cyclopropenyl Cation
+
H H
H
H H
H
+
also written as
n = 2
4n +2 = 10 p electrons
Cyclooctatetraene Dianion
H H H H
H
H
H
H
H H H H
H
H
H
H
2–
••
••
–
–
also
written as
11.21
Heterocyclic Aromatic Compounds
Pyridine
N
••
Examples
O
••
••
S
••
••
N
H
••
Pyrrole Furan Thiophene
Quinoline
Examples
N
••
N•
•
Isoquinoline
11.22
Heterocyclic Aromatic Compounds
and
Hückel's Rule
N
••
Pyridine
6 p electrons in ring
lone pair on nitrogen is in an
sp2 hybridized orbital;
not part of p system of ring
Pyrrole
lone pair on nitrogen must be part
of ring p system if ring is to have
6 p electrons
lone pair must be in a p orbital
in order to overlap with ring p
system
N
H
••
Furan
two lone pairs on oxygen
one pair is in a p orbital and is part
of ring p system; other is in an
sp2 hybridized orbital and is not
part of ring p system
O
••
••

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