H H H C C C C C C H H Benzene and the Concept of Aromaticity H two equivalent resonance forms: other representations: Bond Lengths in Benzene H H H C C C C C C • All carbon-carbon bond lengths in benzene are EQUAL (139 pm) • This.
Download ReportTranscript H H H C C C C C C H H Benzene and the Concept of Aromaticity H two equivalent resonance forms: other representations: Bond Lengths in Benzene H H H C C C C C C • All carbon-carbon bond lengths in benzene are EQUAL (139 pm) • This.
H C H C C H H C C C H
Benzene and
H
the Concept of Aromaticity
two equivalent resonance forms: other representations:
Bond Lengths in Benzene
H C H C H C C C C H H H (We usually draw benzene with alternating single and double bonds for ease of electron counting, but we must remember that the electrons are actually delocalized around the ring) •
All carbon-carbon bond lengths in benzene are EQUAL (139 pm)
•
This is intermediate between a typical C-C (single) bond (154 pm) and a typical C=C (double ) bond (134 pm)
•
This is consistent with
p
electron delocalization
(Un)Reactivity (stability) of Benzene
•
Highly unsaturated (r + db = 4), yet neither Br 2 nor HBr adds across its multiple bonds as with alkenes.
•
Reacts with Br 2 in presence of FeBr 3 catalyst by SUBSTITUTION rather than by addition (which is the way alkenes react with Br 2 ).
H Br 2 Br 2 Br + Br HBr + HBr FeBr 3 FeBr 3
+ H2 -119.7 kJ/mol
Stability of Benzene
Hypothetical ‘cyclohexatriene’ Actual Benzene + 3H2 expect: 3X-119.7= -359.1 kJ/mol + 2H2 -231.8 kJ/mol + 3H2 observe: -208.4 kJ/mol (150.7 kJ/mol more stable!) (same product)
(six 2p orbitals, each w/ 1 electron) Pi Bonding in Benzene
* 6 * 4 * 5 2 3 1
antibonding bonding
Delocalization in Benzene
Note complete delocalization of p electrons!
Hückel Definition of Aromaticity For a system to be aromatic, it must have:
•
4n + 2
p
electrons (for n = any integer: 0, 1, 2, etc.)
•
in the periphery
•
of a monocyclic
•
planar
•
delocalized (conjugated) system (Hückel’s # = (4n+2) = 2, 6, 10, 14, 18, etc. for various integral values of n)
Examples of Aromatic Systems
H H H
#
p
e = 6 2 6 6
Examples of Aromatic Systems
H H H H H H H H H H H H H H H H H H etc.
H H H H etc.
H H H H H etc.
H H H 1 more res. form 3 more res. forms 5 more res. forms
Some Non-Aromatic Systems
H HH
#
p
e = 4 8 4 10 (not planar!)
Some Heteroaromatic Systems
4 5 6 N 1 2 3 5 4 3 N H 1 2 5 4 N 3 N H 1 2
pyridine pyrrole imidazole (has a lp in sp 2 ) (lp is in p orbital) (has a lp in sp 2 hybrid orbital + a lp in p orbital)
Bonding in Pyrrole & Imidazole
H N 4 electrons in p bonds plus 2 lp electrons = 6 p electrons (6 is a Hückel #) lp in p orbital N H
Polycyclic Aromatic Compounds 10
p
e naphthalene 14
p
e anthracene 14
p
e phenanthrene All three are found in coal. Note that in this Kekule resonance form they obey Hückel’s rule; try others!
Spectra of Aromatic Compounds IR: Ar C-H Ar C=C 3030 cm -1 1600, 1500, (1450) cm -1 (2 or 3 sharp bands) 1 H-NMR: 13 C-NMR: UV: Ar H Ar C n -
p
-
p
*
p
* 6.5-8.0
d (
benzene = 7.27
d
) 110-160
d (
benzene = 128.5
d)
205 nm (strong) 255-275 nm (weak)
Summary: Attributes of Aromatics
• • • •
Exceptional Stability
•
Due to extended system of delocalized
p
electrons (conjugation) Special (un)Reactivity
•
Electrophilic substitution rather than addition Bond Length Equalization
•
All C-C bond lengths are equal in benzene; there are NOT single bonds and double bonds.
Magnetic Properties
•
The circulating
p
electrons establish a ‘ring current’ which causes large downfield shifts of aryl protons.