Benzene and aromaticity
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1 aromaticity The word "benzene" derives historically from "gum benzoin", sometimes called "benjamin" (i.e., benzoin resin), an aromatic resin known to European pharmacists and perfumers since the 15th century as a product of southeast Asia. 1
2 Benzene and aromaticity before 1825 compounds with a distinctive "aromatic" smell 1825 Michael Faraday discovers benzene Aromaticity 2
3 Aromaticity Benzene and aromaticity : high carbon-hydrogen ratios - stable despite considerable unsaturation 1865: benzene structure Kekulé 3
4 Kekulé Something wrong!! Kekulé 4
5 1931 Linus Pauling 5
6 Aromaticity: IUPAC definition Compounds which exhibit significantly exalted diamagnetic susceptibility are aromatic. Cyclic electron delocalization also may result in bond length equalization abnormal chemical shifts magnetic anisotropies chemical and physical properties which reflect energetic stabilization. Aromatic compounds dichloro-dipheynl-tricholoethane, DDT Paul Muller receives a Nobel Prize for his discovery of the insecticidal properties of DDT 6
7 Aromatic compounds Aromatic compounds 7
8 Sources of Aromatic Hydrocarbons From high temperature distillation of coal tar Heating petroleum at high temperature and pressure over a catalyst stability 8
9 Unusual Stability Hydrogenation of just one double bond in benzene is endothermic! Annulenes All cyclic conjugated hydrocarbons were proposed to be aromatic. However, cyclobutadiene is so reactive that it dimerizes before it can be isolated. And cyclooctatetraene adds Br 2 readily. Look at MO s to explain aromaticity. 9
10 MO Rules for Benzene Six overlapping p orbitals must form six molecular orbitals. Three will be bonding, three antibonding. Lowest energy MO will have all bonding interactions, no nodes. As energy of MO increases, the number of nodes increases. MO s for Benzene 10
11 Energy Diagram for Benzene The six electrons fill three bonding pi orbitals. All bonding orbitals are filled ( closed shell ), an extremely stable arrangement. MO s for Cyclobutadiene 11
12 Energy Diagram for Cyclobutadiene Following Hund s rule, two electrons are in separate orbitals. This diradical would be very reactive. Polygon Rule The energy diagram for an annulene has the same shape as the cyclic compound with one vertex at the bottom. 12
13 Aromatic Requirements Structure must be cyclic with conjugated pi bonds. Each atom in the ring must have an unhybridized p orbital. The p orbitals must overlap continuously around the ring. (Usually planar structure) Compound is more stable than its openchain counterpart. Anti- and Nonaromatic Antiaromatic compounds are cyclic, conjugated, with overlapping p orbitals around the ring, but the energy of the compound is greater than its open-chain counterpart. Nonaromatic compounds do not have a continuous ring of overlapping p orbitals and may be nonplanar. 13
14 Hückel s Rule If the compound has a continuous ring of overlapping p orbitals and has 4N + 2 electrons, it is aromatic. If the compound has a continuous ring of overlapping p orbitals and has 4N electrons, it is antiaromatic. [N]Annulenes [4]Annulene is antiaromatic (4N e - s) [8]Annulene would be antiaromatic, but it s not planar, so it s nonaromatic. [10]Annulene is aromatic except for the isomers that are not planar. Larger 4N annulenes are not antiaromatic because they are flexible enough to become nonplanar. 14
15 annulenes MO Derivation of Hückel s Rule Lowest energy MO has 2 electrons. Each filled shell has 4 electrons. 15
16 Cyclobutadiene Cyclobutadiene wasn t prepared until 1965, by Pettit, but it dimerizes (Diels-Alder) even at -78 o C: Compounds With 4n π Electrons Are Not Aromatic (May be Antiaromatic) Planar, cyclic molecules with 4n π electrons are much less stable than expected (anti-aromatic) Cyclobutadiene is so unstable that it dimerizes by a self-diels-alder reaction even at low temperature 16
17 Compounds With 4n π Electrons Are Not Aromatic (May be Antiaromatic) If the ring is larger, it will distort out of planar and behave like an ordinary alkene 8-electron (and higher) compounds are not delocalized (single and double bonds) Cyclooctatetraene has four double bonds, reacting with Br 2, KMnO 4, and HCl as if it were four alkenes cyclooctatetraene Cyclopentadienyl Ions The cation has an empty p orbital, 4 electrons, so antiaromatic. The anion has a nonbonding pair of electrons in a p orbital, 6 e - s, aromatic. 17
18 Acidity of Cyclopentadiene pk a of cyclopentadiene is 16, much more acidic than other hydrocarbons. H H H + _ OC(CH 3 ) 3 + HOC(CH 3 ) 3 pka = 16 pka = 19 Tropylium Ion The cycloheptatrienyl cation has 6 p electrons and an empty p orbital. Aromatic: more stable than open chain ion H OH H +, H 2 O H + 18
19 Dianion of [8]Annulene Cyclooctatetraene easily forms a -2 ion. Ten electrons, continuous overlapping p orbitals, so it is aromatic. + 2 K + 2 K + Pyridine Heterocyclic aromatic compound. Nonbonding pair of electrons in sp 2 orbital, so weak base, pk b =
20 Pyrrole Also aromatic, but lone pair of electrons is delocalized, so much weaker base. Other Heterocyclics 20
21 Fused Ring Hydrocarbons Naphthalene Anthracene Phenanthrene Reactivity of Polynuclear Hydrocarbons As the number of aromatic rings increases, the resonance energy per ring decreases, so larger PAH s will add Br 2. H Br H Br Br H H Br (mixture of cis and trans isomers) 21
22 Fused Heterocyclic Compounds Common in nature, synthesized for drugs. Allotropes of Carbon Amorphous: small particles of graphite; charcoal, soot, coal, carbon black. Diamond: a lattice of tetrahedral C s. Graphite: layers of fused aromatic rings. 22
23 Some New Allotropes Fullerenes: 5- and 6-membered rings arranged to form a soccer ball structure. Nanotubes: half of a C 60 sphere fused to a cylinder of fused aromatic rings. Common Names of Benzene Derivatives OH CH 3 NH2 OCH 3 phenol toluene aniline anisole H C CH 2 O C CH 3 O C H O C OH styrene acetophenone benzaldehyde benzoic acid 23
24 Disubstituted Benzenes The prefixes ortho-, meta-, and para- are commonly used for the 1,2-, 1,3-, and 1,4- positions, respectively. Br NO 2 Br o-dibromobenzene or 1,2-dibromobenzene HO p-nitrophenol or 4-nitrophenol 3 or More Substituents Use the smallest possible numbers, but the carbon with a functional group is #1. OH O 2 N NO 2 O 2 N NO 2 NO 2 1,3,5-trinitrobenzene NO 2 2,4,6-trinitrophenol 24
25 Common Names for Disubstituted Benzenes CH 3 CH 3 O C OH CH 3 OH CH 3 H 3 C CH 3 H 3 C m-xylene mesitylene o-toluic acid p-cresol Phenyl and Benzyl Phenyl indicates the benzene ring attachment. The benzyl group has an additional carbon. Br CH 2 Br phenyl bromide benzyl bromide 25
26 Physical Properties Melting points: More symmetrical than corresponding alkane, pack better into crystals, so higher melting points. Boiling points: Dependent on dipole moment, so ortho > meta > para, for disubstituted benzenes. Density: More dense than nonaromatics, less dense than water. Solubility: Generally insoluble in water. IR and NMR Spectroscopy C=C stretch absorption at 1600 cm -1. sp 2 C-H stretch just above 3000 cm H NMR at δ7-δ8 for H s on aromatic ring. 13 C NMR at δ120-δ150, similar to alkene carbons. 26
27 Mass Spectrometry UV Spectroscopy 27
28 Spectroscopy of Aromatic Compounds IR: Aromatic ring C H stretching at 3030 cm 1 and peaks 1450 to 1600 cm 1 Spectroscopy of Aromatic Compounds UV: Peak near 205 nm and a less intense peak in nm range 1 H NMR: Aromatic H s strongly deshielded by ring and absorb between δ 6.5 and δ
29 Aryl and Benzylic protons: Ring Currents Aromatic ring oriented perpendicular to a strong magnetic field, delocalized π electrons producing a small local magnetic field which opposes the applied field in middle of ring but reinforces the applied field on the perimeter of the ring 29
30 13 C NMR of Aromatic Compounds Carbons in aromatic ring absorb at δ 110 to 140 Shift is distinct from alkane carbons but in same range as alkene carbons 30
31 Summary of Spectroscopy Carey/Useful/aromaticity.html PDF ext/react3.htm 31
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