12Skin Damage12Very high energy radiation (UVC) is currently blocked by the ozone layer (ozone hole issue)High energy radiation (UVB) does the most immediate damage (sunburns)But lower energy radiation (UVA) can penetrate deeper into the skin, leading to long term damageSource: N.A. Shaath. The Chemistry of Sunscreens. In: Lowe NJ, Shaath NA, Pathak MA, editors. Sunscreens, development, evaluation, and regulatory aspects. New York: Marcel Dekker; p
13Sources and Names of Aromatic Hydrocarbons From high temperature distillation of coal tarHeating petroleum at high temperature and pressure over a catalyst
18Polychlorinatedbiphenyls PCB’s Thermally stable, electrically insulating heat transfer liquidCasting wax for lost wax process for making metal things
19dichlorodiphenyltrichloroethane Carson wrote "Dr. DeWitt's now classic experiments [on quail and pheasants] have now established the fact that exposure to DDT, even when doing no observable harm to the birds, may seriously affect reproduction. Quail into whose diet DDT was introduced throughout the breeding season survived and even produced normal numbers of fertile eggs. But few of the eggs hatched." DeWitt's 1956 article (in Journal of Agriculture and Food Chemistry) actually yielded a very different conclusion. Quail were fed 200 parts per million of DDT in all of their food throughout the breeding season. DeWitt reports that 80% of their eggs hatched, compared with the "control"" birds which hatched 83.9% of their eggs. Carson also omitted mention of DeWitt's report that "control" pheasants hatched only 57 percent of their eggs, while those that were fed high levels of DDT in all of their food for an entire year hatched more than 80% of their eggs.Malaria mosquitoMueller 1948 Nobel Prize in Medicine
20Thermodynamic stability of benzene: Heats of Hydrogenation
21Monosubstituted Benzenes Most monosubstituted aromatics are named using benzene as the parent name preceded by the substituent name (as a prefix; all one word):fluoronitroethylfluorobenzenenitrobenzeneethylbenzene
22Alkyl-substituted Benzenes Alkyl substituted benzenes are named according to the length of the carbon chain of the alkyl group.With six carbons or fewer in the alkyl chain, they are named as ‘alkylbenzene.’e.g., propylbenzene:
23Alkyl-substituted Benzenes With more than six carbons in the alkyl chain, they are named as a ‘phenylalkane,’ where the benzene ring is named as a substituent (phenyl) on the alkane chaine.g., 4-phenylnonane4-phenylnonane
24The Benzyl GroupThe benzyl group is a common name for a methyl substituted benzene (toluene) having substitution for one of the hydrogens on the methyl group.the benzyl group benzyl bromide benzyl alcohol
25Common Names of Subs. Benzenes There are a number of nonsystematic (common) names commonly used for certain monosubstituted benzenes (see next slide)These ten common names should be memorized.These common names are used as base names when naming more their more highly substituted derivatives. Examples of these will be given later.
26Mono-substituted Benzene Nomenclature: Common Names
27Disubstituted Benzenes Disubstituted benzenes can be named in one of two ways. Each method describes the relative positions of the two groups on the benzene ring.Systematic numbering of the aromatic ring.Using the prefixes ortho-, meta-, or para-.When numbering the ring carbons, carbon # 1 is always a substituted carbon.The substituents are listed alphabetically.
28Disubstituted Benzenes ortho- (abbreviated o- ) = 1,2-disubstituted(two groups on adjacent carbons on the ring)
29Disubstituted Benzenes meta- (abbreviated m- ) = 1,3-disubstituted(two groups having one unsubstituted carbon between them)
30Disubstituted Benzenes para- (abbreviated p- ) = 1,4-disubstituted(two groups on opposite sides of the ring)
31Disubstituted Benzenes When one of the substituents changes the base name, either o-, m-, and p- or numbers may be used to indicate the position of the other substituent.Carbon # 1 is always the carbon bearing the substituent that changes the base name.413221p-bromoanilineor4-bromoanilineo-chlorophenolor2-chlorophenol
32Common Names of Disubs. Benzenes There are a few nonsystematic (common) names for disubstituted benzenes that you should be familiar with:
33Disubstituted Benzenes Relative positions on a benzene ringortho- (o) on adjacent carbons (1,2)meta- (m) separated by one carbon (1,3)para- (p) separated by two carbons (1,4)Describes reaction patterns (“occurs at the para position”)
34Polysubstituted Benzenes Polysubstituted benzenes must be named by numbering the position of each substituent on the ring (with more than two substituents, o-, m-, and p-can NOT be used.)The numbering is carried out to give the substituents the lowest possible numbers. Carbon #1 always has a substituent.List the substituents alphabetically with their appropriate #s.21342-ethyl-1-fluoro-4-nitrobenzene
35Polysubstituted Aromatics having a Common base name Common names of the monosubstituted benzenes are used as parent names for polysubstituted aromatics when one of the substituents changes the base name.For such rings with common names, the carbon bearing the substituent responsible for the common name is always carbon #1.The substitutents arelisted in alphabeticalorder.toluene1chloro2bromo5345-bromo-2-chlorotoluene
38Naming Benzene as a Substituent A benzene substituent is called a phenyl group, and it can be abbreviated in a structure as “Ph-”.Therefore, benzene can be represented as PhH, and phenol would be PhOH.
39Polycyclic Aromatic Hydrocarbons (PAH) Metabolic byproducts of benzo [a] pyrene react withDNA to form adducts, leading to carcinogenesis (cancer).
40Naphthalene OrbitalsThree resonance forms and delocalized electrons
4113C NMR Absorptions of Dibromobenzenes Figure 17.2The number of signals (lines) in the 13C NMR spectrum of a disubstituted benzene with two identical groups indicates whether they are ortho, meta, or para to each other.
45Pyridine A six-membered heterocycle with a nitrogen atom in its ring electron structure resembles benzene (6 electrons)The nitrogen lone pair electrons are not part of the aromatic system (perpendicular orbital)Pyridine is a relatively weak base compared to normal amines but protonation does not affect aromaticity
47Pyrrole A five-membered heterocycle with one nitrogen electron system similar to that of cyclopentadienyl anionFour sp2-hybridized carbons with 4 p orbitals perpendicular to the ring and 4 p electronsNitrogen atom is sp2-hybridized, and lone pair of electrons occupies a p orbital (6 electrons)Since lone pair electrons are in the aromatic ring, protonation destroys aromaticity, making pyrrole a very weak base
49Structure and Stability of Benzene: Molecular Orbital Theory Benzene reacts slowly with Br2 to give bromobenzene (where Br replaces H)This is substitution rather than the rapid addition reaction common to compounds with C=C, suggesting that in benzene there is a higher barrier
50Heats of Hydrogenation as Indicators of Stability The addition of H2 to C=C normally gives off about 118 kJ/mol – 3 double bonds would give off 356kJ/molTwo conjugated double bonds in cyclohexadiene add 2 H2 to give off 230 kJ/molBenzene has 3 unsaturation sites but gives off only 206 kJ/mol on reacting with 3 H2 moleculesTherefore it has about 150 kJ more “stability” than an isolated set of three double bonds
52Benzene’s Unusual Structure All its C-C bonds are the same length: 139 pm — between single (154 pm) and double (134 pm) bondsElectron density in all six C-C bonds is identicalStructure is planar, hexagonalC–C–C bond angles 120°Each C is sp2 and has a p orbital perpendicular to the plane of the six-membered ring
53The Criteria for Aromaticity Four structural criteria must be satisfied for a compound to be aromatic:1. A molecule must be cyclic.To be aromatic, each p orbital must overlap with p orbitals onadjacent atoms.
54The Criteria for Aromaticity A molecule must be planar.All adjacent p orbitals must be aligned so that the electron density can be delocalized.Since cyclooctatetraene is nonplanar and not aromatic, it undergoes addition reactions just like those of other alkenes.
55The Criteria for Aromaticity A molecule must be completely conjugated.Aromatic compounds must have a p orbital on every atom.
56The Criteria for Aromaticity 4. A molecule must satisfy Hückel’s rule, and contain a particular number of electrons.Hückel's rule:Benzene is aromatic and especially stable because it contains 6 electrons.Cyclobutadiene is antiaromatic and especially unstable because it contains 4 electrons.
57Hückel’s rule refers to the number of electrons, not the number of atoms in a particular ring.
58Why 4n +2?When electrons fill the various molecular orbitals, it takes two electrons (one pair) to fill the lowest-lying orbital and four electrons (two pairs) to fill each of n succeeding energy levelsThis is a total of 4n + 2
59Bonding and Antibonding Orbitals The combination of two p orbitals can be constructive—that is, with like phases interacting—or destructive, that is, with opposite phases interacting.When two p orbitals of similar phase overlap side-by-side, a bonding molecular orbital results.When two p orbitals of opposite phase overlap side-by-side, a * antibonding orbital results.
60Formation of π and π* Molecular Orbitals Two atomic p orbitals combine to form two molecular orbitals.The bonding p MO is lower in energy than the two p orbitals.The * antibonding MO is higher in energy because a destabilizing node results, which pushes nuclei apart when orbitals of opposite phase combine.Figure 17.8
61 Molecular Orbitals for Benzene Since each of the six carbon atoms in benzene has a p orbital, six atomic p orbitals combine to form six MOs.Figure 17.9
62Inscribed Polygon Method of Predicting Aromaticity
63Inscribed Polygon Method of Predicting Aromaticity This method works for all monocyclic completely conjugated systems regardless of ring size.The total number of MOs always equals the number of vertices of the polygon.The inscribed polygon method is consistent with Hückel's 4n + 2 rule—there is always one lowest energy bonding MO that can hold two electrons and the other bonding MOs come in degenerate pairs that can hold a total of four electrons.
64Inscribed Polygon Method of Predicting Aromaticity Figure 17.10
65Buckminsterfullerene—Is it Aromatic? Buckminsterfullerene (C60) is a third elemental form of carbon.Buckminsterfullerene is completely conjugated, but it is not aromatic since it is not planar (CAREFULL!!!)It undergoes addition reactions with electrophiles in much the same way as ordinary alkenes.
66Compounds With 4n Electrons Are Not Aromatic (May be Antiaromatic) Planar, cyclic molecules with 4 n electrons are much less stable than expected (antiaromatic)They will distort out of plane and behave like ordinary alkenes4- and 8-electron compounds are not delocalized (single and double bonds)Cyclobutadiene is so unstable that it dimerizes by a self-Diels-Alder reaction at low temperatureCyclooctatetraene has four double bonds, reacting with Br2, KMnO4, and HCl as if it were four alkenes
67Aromatic IonsThe 4n + 2 rule applies to ions as well as neutral speciesBoth the cyclopentadienyl anion and the cycloheptatrienyl cation are aromaticThe key feature of both is that they contain 6 electrons in a ring of continuous p orbitals
68Aromaticity of the Cyclopentadienyl Anion 1,3-Cyclopentadiene contains conjugated double bonds joined by a CH2 that blocks delocalizationRemoval of H+ at the CH2 produces a cyclic 6-electron system, which is stableRemoval of H- or H• generates nonaromatic 4 and 5 electron systemsRelatively acidic (pKa = 16) because the anion is stable
69CycloheptatrieneCycloheptatriene has 3 conjugated double bonds joined by a CH2Removal of “H-” leaves the cationThe cation has 6 electrons and is aromatic
70NMR and Aromaticity1H NMR spectroscopy readily indicates whether a compound is aromatic.The protons on sp2 hybridized carbons in aromatic hydrocarbons are highly deshielded and absorb at 6.5–8 ppm, whereas hydrocarbons that are not aromatic absorb at 4.5–6 ppm.
71Larger Aromatic RingsCompletely conjugated rings larger than benzene are also aromatic if they are planar and have 4n + 2 electrons.Hydrocarbons containing a single ring with alternating double and single bonds are called annulenes.To name an annulene, indicate the number of atoms in the ring in brackets and add the word annulene.
72Hückel’s Rule and Number of Electrons -Annulene has 10 electrons, which satisfies Hückel's rule, but a planar molecule would place the two H atoms inside the ring too close to each other.Thus, the ring puckers to relieve this strain.Since -annulene is not planar, the 10 electrons cannot delocalize over the entire ring and it is not aromatic.