Download presentation
Presentation is loading. Please wait.
1
11.18 Cyclobutadiene and Cyclooctatetraene
2
Requirements for Aromaticity
cyclic conjugation is necessary, but not sufficient not aromatic not aromatic aromatic 2
3
Heats of Hydrogenation
to give cyclohexane (kJ/mol) 120 231 208 heat of hydrogenation of benzene is 152 kJ/mol less than 3 times heat of hydrogenation of cyclohexene 3
4
Heats of Hydrogenation
to give cyclooctane (kJ/mol) 97 205 303 410 heat of hydrogenation of cyclooctatetraene is more than 4 times heat of hydrogenation of cyclooctene 4
5
Structure of Cyclobutadiene
structure of a stabilized derivative is characterized by alternating short bonds and long bonds C(CH3)3 (CH3)3C CO2CH3 138 pm 151 pm 5
6
Structure of Cyclooctatetraene
cyclooctatetraene is not planar has alternating long (146 pm) and short (133 pm) bonds 5
7
Conclusion there must be some factor in addition to cyclic conjugation that determines whether a molecule is aromatic or not 5
8
11.19 Hückel's Rule: Annulenes
the additional factor that influences aromaticity is the number of p electrons 6
9
Hückel's Rule among planar, monocyclic, completely conjugated polyenes, only those with 4n p electrons possess special stability (are aromatic) n 4n+2 0 2 1 6 2 10 3 14 4 18 7
10
Hückel's Rule among planar, monocyclic, completely conjugated polyenes, only those with 4n p electrons possess special stability (are aromatic) n 4n+2 0 2 1 6 benzene! 2 10 3 14 4 18 7
11
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 7
12
6 p orbitals give 6 p orbitals
p-MOs of Benzene Antibonding Benzene Bonding 6 p orbitals give 6 p orbitals 3 orbitals are bonding; 3 are antibonding 8
13
6 p electrons fill all of the bonding orbitals
p-MOs of Benzene Antibonding Benzene Bonding 6 p electrons fill all of the bonding orbitals all p antibonding orbitals are empty 8
14
p-MOs of Cyclobutadiene (square planar)
Antibonding Cyclo- butadiene Bonding 4 p orbitals give 4p orbitals 1 orbital is bonding, one is antibonding, and 2 are nonbonding 8
15
p-MOs of Cyclobutadiene (square planar)
Antibonding Cyclo- butadiene Bonding 4 p electrons; bonding orbital is filled; other 2 p electrons singly occupy two nonbonding orbitals 8
16
p-MOs of Cyclooctatetraene (square planar)
Antibonding Cyclo- octatetraene Bonding 8 p orbitals give 8 p orbitals 3 orbitals are bonding, 3 are antibonding, and 2 are nonbonding 8
17
p-MOs of Cyclooctatetraene (square planar)
Antibonding Cyclo- octatetraene Bonding 8 p electrons; 3 bonding orbitals are filled; 2 nonbonding orbitals are each half-filled 8
18
p-Electron Requirement for Aromaticity
4 p electrons 6 p electrons 8 p electrons not aromatic not aromatic aromatic 2
19
Completely Conjugated Polyenes
6 p electrons; not completely conjugated 6 p electrons; completely conjugated H not aromatic aromatic 2
20
Annulenes Annulenes are planar, monocyclic, completely conjugated polyenes. That is, they are the kind of hydrocarbons treated by Hückel's rule. 15
21
10-sided regular polygon has angles of 144°
[10]Annulene 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° 16
22
[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 16
![[10]Annulene](http://slideplayer.com./slide/9866917/32/images/22/%5B10%5DAnnulene.jpg "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. 16.")
23
van der Waals strain between these two hydrogens
[10]Annulene van der Waals strain between these two hydrogens 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 16
24
14 p electrons satisfies Hückel's rule
[14]Annulene H H H H 14 p electrons satisfies Hückel's rule van der Waals strain between hydrogens inside the ring 16
25
16 p electrons does not satisfy Hückel's rule
[16]Annulene 16 p electrons does not satisfy Hückel's rule alternating short (134 pm) and long (146 pm) bonds not aromatic 16
26
18 p electrons satisfies Hückel's rule resonance energy = 418 kJ/mol
[18]Annulene H 18 p electrons satisfies Hückel's rule resonance energy = 418 kJ/mol bond distances range between pm 16
27
11.20 Aromatic Ions 21
28
Cycloheptatrienyl Cation
+ 6 p electrons delocalized over 7 carbons positive charge dispersed over 7 carbons very stable carbocation also called tropylium cation 22
29
Cycloheptatrienyl Cation
+ + H 22
30
Cycloheptatrienyl Cation
Br + Br– Ionic Covalent Tropylium cation is so stable that tropylium bromide is ionic rather than covalent. mp 203 °C; soluble in water; insoluble in diethyl ether 23
31
Cyclopentadienide Anion
H •• – 6 p electrons delocalized over 5 carbons negative charge dispersed over 5 carbons stabilized anion 22
32
Cyclopentadienide Anion
H •• – H – 22
33
Acidity of Cyclopentadiene
H H •• – H+ + pKa = 16 Ka = 10-16 Cyclopentadiene is unusually acidic for a hydrocarbon. Increased acidity is due to stability of cyclopentadienide anion. 22
34
Electron Delocalization in Cyclopentadienide Anion
H •• – 26
35
Electron Delocalization in Cyclopentadienide Anion
H H •• – •• – 26
36
Electron Delocalization in Cyclopentadienide Anion
H H •• – •• – H • – 26
37
Electron Delocalization in Cyclopentadienide Anion
H H •• – •• – H H – • • – 26
38
Electron Delocalization in Cyclopentadienide Anion
H H •• – •• – H H H H – • •• • – H H H 26
39
Compare Acidities of Cyclopentadiene and Cycloheptatriene
pKa = 16 Ka = 10-16 pKa = 36 Ka = 10-36 27
40
Compare Acidities of Cyclopentadiene and Cycloheptatriene
•• H •• – – Aromatic anion 6 p electrons Anion not aromatic 8 p electrons 27
41
Cyclopropenyl Cation + H H + also written as n = 0
4n +2 = 2 p electrons 28
42
Cyclooctatetraene Dianion
H H H H – H •• H H H also written as 2– •• H H H H – H H H H n = 2 4n +2 = 10 p electrons 29
43
11.21 Heterocyclic Aromatic Compounds
30
44
Examples N •• N H •• O •• S •• Pyridine Pyrrole Furan Thiophene 31
45
Examples N •• N • Quinoline Isoquinoline 31
46
11.22 Heterocyclic Aromatic Compounds and Hückel's Rule
36
47
Pyridine 6 p electrons in ring
lone pair on nitrogen is in an sp2 hybridized orbital; not part of p system of ring N •• 31
48
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 •• 31
49
two lone pairs on oxygen
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 •• 31
Similar presentations
