Chapter 21 Flashcards
Benzene Resonance
•We often represent benzene as a hybrid of two equivalent Kekulé structures.
–Each makes an equal contribution to the hybrid and thus the C-C bonds are neither double nor single, but something in between.
•The concepts of hybridization of atomic orbitals and the theory of resonance, developed in the 1930s, provided the first adequate description of benzene’s structure.
–The carbon skeleton is a planar regular hexagon.
–All C-C-C and H-C-C bond angles 120°
•Resonance energy:Resonance energy:The difference in energy between a resonance hybrid and the most stable of its hypothetical contributing structures in which electrons are localized on particular atoms and in particular bonds.
–One way to estimate the resonance energy of benzene is to compare the heats of hydrogenation of benzene and cyclohexene.
pi system of benzene
–(a) The carbon framework with the six 2p orbitals.
–(b) Overlap of the parallel 2p orbitals forms one torus above the plane of the ring and another below it
–this orbital represents the lowest-lying pi-bonding molecular orbital.
Huckel’s rule
- The compound must be cyclic.
- It must have one p orbital on each atom of the ring.
- It should be planar or nearly planar so that there is continuous or nearly continuous overlap of all p orbitals.
- It must have a closed loop of (4n+2) p electrons in the cyclic arrangement of p orbitals.
aromaticity chemical shift
between 6.5 and 9
–The magnetic field induced by circulation of electrons in an aromatic ring deshields the hydrogens of the aromatic ring and shifts their signal to higher frequency.
Aromatic Hydrocarbons
• Cyclobutadiene, Benzene and Cyclooctatetraene are the first members of a family called the annulenes.
–What is remarkable relative to [10]annulene is that if the two hydrogens facing inward toward the center of the ring are replaced by a methylene (CH2) group, the ring is able to assume a conformation close enough to planar that it becomes aromatic.
Annulene
A cyclic hydrocarbon with a continuous alternation of single and double bonds.
Antiaromatic Hydrocarbons
•Antiaromatic hydrocarbon:Antiaromatic hydrocarbon:A monocyclic, planar, fully conjugated hydrocarbon with 4n pi electrons (4, 8, 12, 16, 20…).
–An antiaromatic hydrocarbon is especially unstable relative to an open-chain fully conjugated hydrocarbon of the same number of carbon atoms.
•Cyclobutadiene is antiaromatic.
–In the ground-state electron configuration of this molecule, two electrons fill the 1 bonding MO.
–The remaining two electrons lie in the 2 and 3nonbonding MOs.
Cyclobutadiene
–The ground state of planar cyclobutadiene has two unpaired electrons, which make it highly unstable and reactive.
Cyclooctatetraene
–Cyclooctatetraene, with 8 pi electrons is not aromatic; it shows reactions typical of alkenes.
–X-ray studies show that the most stable conformation is a nonplanar “tub” conformation.
–Although overlap of 2p orbitals occurs to form pi bonds, there is only minimal overlap between sets of 2p orbitals because they are not parallel.
frost circles
•Frost circle:Frost circle: A graphic method for determining the relative order of pi MOs in planar, fully conjugated monocyclic compounds.
–Inscribe in a circle a polygon of the same number of sides as the ring to be examined such that one of the vertices of the polygon is at the bottom of the circle.
–The relative energies of the MOs in the ring are given by where the vertices of the polygon touch the circle.
•Those MOs
–Below the horizontal line through the center of the ring are bonding MOs.
–on the horizontal line are nonbonding MOs.
–above the horizontal line are antibonding MOs.
–Frost circles describing the MOs for monocyclic, planar, fully conjugated four-, five-, and six-membered rings.
Heterocyclic Aromatics
Heterocyclic Aromatics
pyridine
–The nitrogen atom of pyridine is sp2 hybridized.
–The unshared pair of electrons lies in an sp2hybrid orbital and is not a part of the six pi electrons of the aromatic system (the aromatic sextet).
–Resonance energy of pyridine is 134 kJ (32 kcal)/mol.
Furan and Pyrrole
–The oxygen atom of furan is sp2 hybridized.
–one unshared pairs of electrons on oxygen lies in an unhybridized 2p orbital and is a part of the aromatic sextet.
–The other unshared pair lies in an sp2 hybrid orbital and is not a part of the aromatic system
–The resonance energy of furan is 67 kJ (16 kcal)/mol.
Aromatic Hydrocarbon Ions
•Any neutral, monocyclic, unsaturated hydrocarbon with an odd number of carbons must have at least one CH2 group and, therefore, cannot be aromatic.
–Cyclopropene, for example, has the correct number of pi electrons to be aromatic, 4(0) + 2 = 2, but does not have a closed loop of 2p orbitals.
Cyclopropenyl Cation
–If, however, the CH2 group of cyclopropene is transformed into a CH+ group in which carbon is sp2 hybridized and has a vacant 2p orbital, the overlap of orbitals is continuous and the cation is aromatic.
–When 3-chlorocyclopropene is treated with SbCl5, it forms a stable salt.
–If planar cyclopentadienyl cation were to exist, it would have 4 pi electrons and be antiaromatic.
–Note that we can draw five equivalent contributing structures for the cyclopentadienyl cation. Yet this cation is not aromatic because it has only 4 pi electrons.