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Some HistorySome History1825 1825 Michael Faraday isolates a new Michael Faraday isolates a new
hydrocarbon from illuminating gas.hydrocarbon from illuminating gas.1834 1834 EilhardtEilhardt MitscherlichMitscherlich isolates same isolates same
substance and determines its empirical substance and determines its empirical formula to be formula to be CCnnHHnn. Compound comes . Compound comes to be called to be called benzenebenzene..
1845 1845 August W. von Hofmann isolates benzene August W. von Hofmann isolates benzene from coal tar.from coal tar.
1866 1866 August August KekuléKekulé proposes structure of proposes structure of benzene.benzene.
What in the World is What in the World is Benzene??Benzene??
C6H6 discovered by Michael Faraday in 1825– Synthesized in 1834 from benzoic acid– Remarkable chemical stability – Unsaturation number is very high but….
Does not add BromineSubstitutiuon with Br2 / FeBr3Not oxidized by Permanganate or ozoneNo reaction with strong HBr (aq)No reaction with Hydrogen on Pd..??????
Addition vs Substitution…a Mystery
+
Br
Br
AdditionAddition of Bromine to Cyclohexene
Br2
+ Br2
FeBr3
Br
+ HBr
SubstitutionSubstitution of Bromine for Hydrogen in Benzene
C6H6 + Br2 C6H5Br + HBr
∆∆H° of HydrogenationH° of Hydrogenation
Name Structural Formula∆H°
(kcal/mol)
ethylenepropene
1-butenecis-2-butenetrans-2-butene2-methyl-2-butene2,3-dimethyl-2-butene
-32.8-30.1-30.3-28.6-27.6-26.9-26.6
CH2 =CH 2
CH3 CH=CHCH 3
CH3 CH2CH=CH 2
(CH 3 ) 2C=CHCH 3(CH 3 ) 2C=C(CH 3 ) 2
CH3 CH=CHCH 3
CH3CH=CH 2
Friedrich August von Friedrich August von KekuleKekule had a dream of whirling snakes, and the structure of had a dream of whirling snakes, and the structure of benzene. He reported the dream in the following words in 1890, ibenzene. He reported the dream in the following words in 1890, in a speech at a dinner n a speech at a dinner commemorating his discovery that reportedly occurred during a “rcommemorating his discovery that reportedly occurred during a “reverie” on a London everie” on a London bus.bus.
Again the atoms were gamboling before my eyes. This time the smaAgain the atoms were gamboling before my eyes. This time the smaller groups ller groups kept modestly to the background. My mental eye, rendered more ackept modestly to the background. My mental eye, rendered more acute by ute by repeated vision of this kind, could not distinguish larger strucrepeated vision of this kind, could not distinguish larger structures, of manifold tures, of manifold conformation; long rows, sometimes more closely fitted together;conformation; long rows, sometimes more closely fitted together; all twining and all twining and twisting in snakelike motion. But look!twisting in snakelike motion. But look!What was that? One of the snakes had seized hold of its owWhat was that? One of the snakes had seized hold of its own tail, and the form n tail, and the form whirled mockingly before my eyes. As if by a flash of lighting Iwhirled mockingly before my eyes. As if by a flash of lighting I awoke... Let us awoke... Let us learn to dream, gentlemen.learn to dream, gentlemen.
Arthur Arthur KoestlerKoestler (in "The Act of Creation") called this incident "probably the (in "The Act of Creation") called this incident "probably the most most important dream in history since Joseph's seven fat and seven leimportant dream in history since Joseph's seven fat and seven lean cows.an cows.
QUESTION: Can you tell me more about this vision to which you have referred? KEKULÉ: Surely! Let me read to you the remarks I am about to make to the assembly today: During my stay in London I resided in Clapham Road....I frequently, however, spent my evenings with my friend Hugo Mueller....We talked of many things but most often of our beloved chemistry. One fine summer evening I was returning by the last bus, riding outside as usual, through the deserted streets of the city....I fell into a reverie, and lo, the atoms were gamboling before my eyes. Whenever, hitherto, these diminutive beings had appeared to me, they had always been in motion. Now, however, I saw how, frequently, two smaller atoms united to form a pair: how a larger one embraced the two smaller ones; how still larger ones kept hold of three or even four of the smaller: whilst the whole kept whirling in a giddy dance. I saw how the larger ones formed a chain, dragging the smaller ones after them but only at the ends of thechains....The cry of the conductor: "Clapham Road," awakened me from my dreaming; but I spent a part of the night in putting on paper at least sketches of these dream forms.
Contributors to our understanding of Contributors to our understanding of the Structure of Benzenethe Structure of Benzene
1901-19941829-18961791-1867
KekuléKekulé Formulation of BenzeneFormulation of Benzene
Note bond lengthsNote bond lengths
HH
HH
HH
HH
HH
H
H
KekuléKekulé Formulation of BenzeneFormulation of Benzene
Later, Later, KekuléKekulé revised his proposal by suggestingrevised his proposal by suggestinga rapid equilibrium between two equivalenta rapid equilibrium between two equivalentstructures.structures.
HH
HH
HH
HHHH
HH
HH
HH
HH
HHHH
HH
KekuléKekulé Formulation of BenzeneFormulation of Benzene
However, this proposal suggested isomers of theHowever, this proposal suggested isomers of thekind shown were possible. Yet, none were everkind shown were possible. Yet, none were everfound.found.
HH
XX
XX
HHHH
HH
HH
XX
XX
HHHH
HH
All CAll C——C bond distances = 140 pmC bond distances = 140 pm
146 pm146 pm
134 pm134 pm140 pm140 pm 140 pm140 pm
140 pm140 pm 140 pm140 pm
140 pm140 pm140 pm140 pm
140 pm is the average between the C140 pm is the average between the C——C single C single bond distance and the double bond distance in 1,3bond distance and the double bond distance in 1,3--butadiene.butadiene.
KekuléKekulé Formulation of BenzeneFormulation of Benzene
Instead of Instead of Kekulé'sKekulé's suggestion of a rapidsuggestion of a rapidequilibrium between two structures:equilibrium between two structures:
H
H
H
H
H
H
H
HH
HHH
Resonance Formulation of BenzeneResonance Formulation of Benzene
PaulingPauling described the structure of benzene as a described the structure of benzene as a resonanceresonancehybridhybrid of the two Lewis structures. Electrons areof the two Lewis structures. Electrons arenot localized in alternating single and double bonds,not localized in alternating single and double bonds,but are delocalized over all six ring carbons.but are delocalized over all six ring carbons.
HH
HH
HH
HHHH
HH
HH
HH
HH
HHHH
HH
Resonance Formulation of BenzeneResonance Formulation of Benzene
CircleCircle--inin--aa--ring notation stands for resonance ring notation stands for resonance description of benzene (hybrid of two description of benzene (hybrid of two KekuléKekuléstructures)structures)
Unusual Stability of BenzeneUnusual Stability of Benzene
benzene is the best and most familiar example benzene is the best and most familiar example of a substance that possesses "special stability" of a substance that possesses "special stability" or "or "aromaticityaromaticity""
Aromatic molecules have stability that is substantially Aromatic molecules have stability that is substantially greater for a molecule than would be expected on greater for a molecule than would be expected on the basis of any of the Lewis structures written for it the basis of any of the Lewis structures written for it
ThermochemicalThermochemical Measures of StabilityMeasures of Stability
heat of hydrogenation: heat of hydrogenation: compare experimentalcompare experimentalvalue with "expected" value for hypotheticalvalue with "expected" value for hypothetical""cyclohexatrienecyclohexatriene""
PtPt
∆∆H°= H°= –– 208 kJ208 kJ
++ 3H3H22
[ 4.186[ 4.186 kJ / kcal ]kJ / kcal ]
3 x 3 x cyclohexenecyclohexene
120 kJ/mol120 kJ/mol
360 kJ/mol360 kJ/mol
208 kJ/mol
231 kJ/mol231 kJ/mol
3 x 3 x cyclohexenecyclohexene
120 kJ/mol120 kJ/mol
360 kJ/mol360 kJ/mol
"expected" heat "expected" heat of of
hydrogenation hydrogenation of benzene is 3 x of benzene is 3 x
heat of heat of hydrogenation hydrogenation of of cyclohexenecyclohexene
observed heat of observed heat of hydrogenation is hydrogenation is 152 kJ/mol less 152 kJ/mol less than "expected"than "expected"benzene is 152 benzene is 152 kJ/mol more stable kJ/mol more stable thanthanexpectedexpected152 kJ/mol is the 152 kJ/mol is the resonance energy of resonance energy of benzenebenzene
3 x 3 x cyclohexenecyclohexene
360 kJ/mol360 kJ/mol
208 kJ/mol ?!
hydrogenation of hydrogenation of 1,31,3--cyclohexadiene cyclohexadiene (2H(2H22) gives off ) gives off more heat than more heat than hydrogenation of hydrogenation of benzene (3Hbenzene (3H22)!!!)!!!
208 kJ/mol
231 kJ/mol231 kJ/mol
Cyclic Cyclic conjugation versus conjugation versus noncyclicnoncyclic conjugationconjugation
heat of hydrogenation = 208 kJ/molheat of hydrogenation = 208 kJ/mol
heat of hydrogenation = 337 kJ/molheat of hydrogenation = 337 kJ/mol
3H3H22
PtPt
3H3H22
PtPt
Resonance Energy of BenzeneResonance Energy of Benzene
compared to localized 1,3,5compared to localized 1,3,5--cyclohexatrienecyclohexatriene
152 kJ/mol152 kJ/mol
compared to 1,3,5compared to 1,3,5--hexatrienehexatriene
129 kJ/mol129 kJ/mol
exact value of resonance energy of benzene exact value of resonance energy of benzene depends on what it is compared to, but depends on what it is compared to, but regardless of model, benzene is more stable regardless of model, benzene is more stable than expected by a substantial amount than expected by a substantial amount
Molecular Orbital ViewMolecular Orbital Viewof Bonding in Benzeneof Bonding in Benzene
Dr. Dr. AnslynAnslyn will cover this in detailwill cover this in detail
Molecular Orbital Model of Molecular Orbital Model of Bonding in BenzeneBonding in Benzene
High electron density above and below plane of High electron density above and below plane of ringring
Benzene MOsBenzene MOs
AntibondingAntibondingorbitalsorbitals
EnergyEnergy
BondingBondingorbitalsorbitals
6 6 p p AOsAOs combine to give 6 combine to give 6 ππ MOsMOs3 MOs are bonding; 3 are 3 MOs are bonding; 3 are antibondingantibonding
Benzene MOsBenzene MOs
AntibondingAntibondingorbitalsorbitals
EnergyEnergy
BondingBondingorbitalsorbitals
All bonding MOs are filledAll bonding MOs are filledNo electrons in No electrons in antibondingantibonding orbitalsorbitals
The special stability of benzene results from the fact that these three bonding MOs are much lower in energy than the six uncombined 2p atomic orbitals….and the bonding orbitals are “full”…
Frost Circles…a Great TrickFrost Circles…a Great TrickInscribe a polygon of the same number of sides as the ring to be examined such that one of the vertices is at the bottom of the ringThe relative energies of the MOs in the ring are given by where the vertices touch the circleThe 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
ππ--MOs of MOs of CyclobutadieneCyclobutadiene(square planar)(square planar)
AntibondingAntibonding
CycloCyclo--butadienebutadiene BondingBonding
4 4 ππ electrons; bonding orbital is filled; other 2electrons; bonding orbital is filled; other 2ππ electrons singly occupy two nonbonding electrons singly occupy two nonbonding orbitalsorbitals
Structure of Structure of CyclobutadieneCyclobutadiene
structure of a stabilized derivative is characterizedstructure of a stabilized derivative is characterizedby alternating short bonds and long bondsby alternating short bonds and long bonds
C(CHC(CH33))33(CH(CH33))33CC
COCO22CHCH33(CH(CH33))33CC151 pm151 pm
138 pm138 pm
ππ--MOs of MOs of CyclooctatetraeneCyclooctatetraene(square planar)(square planar)
8 8 pp orbitalsorbitals give 8 give 8 ππ orbitalsorbitals3 3 orbitalsorbitals are bonding, 3 are are bonding, 3 are antibondingantibonding, and 2 , and 2 are nonbondingare nonbonding
CycloCyclo--octatetraeneoctatetraene
AntibondingAntibonding
BondingBonding
AntibondingAntibonding
BondingBonding
8 8 ππ electrons; 3 bonding electrons; 3 bonding orbitalsorbitals are filled; 2are filled; 2nonbonding nonbonding orbitalsorbitals are each halfare each half--filledfilled
ππ--MOs of MOs of CyclooctatetraeneCyclooctatetraene(square planar)(square planar)
CycloCyclo--octatetraeneoctatetraene
Structure of Structure of CyclooctatetraeneCyclooctatetraene
cyclooctatetraenecyclooctatetraene is not planaris not planar
has alternating long (146 pm)has alternating long (146 pm)and short (133 pm) bondsand short (133 pm) bonds
Heats of Hydrogenation
to give to give cyclohexanecyclohexane (kJ/mol)(kJ/mol)
Heats of Hydrogenation
heat of hydrogenation of benzene is 152 kJ/mol heat of hydrogenation of benzene is 152 kJ/mol less than 3 times heat of hydrogenation of less than 3 times heat of hydrogenation of cyclohexenecyclohexene
120120 231231 208208
Heats of HydrogenationHeats of Hydrogenation
to give to give cyclooctanecyclooctane (kJ/mol)(kJ/mol)
9797 205205 303303 410410
heat of hydrogenation of heat of hydrogenation of cyclooctatetraenecyclooctatetraene is is more than 4 times the heat of hydrogenation of more than 4 times the heat of hydrogenation of cyclooctenecyclooctene….no special stability here!….no special stability here!
Requirements for Requirements for Aromaticity
cyclic conjugation is necessary, cyclic conjugation is necessary, but not sufficient but not sufficient
Aromaticity
notnotaromatic
notnotaromaticaromaticaromaticaromatic aromatic
ConclusionConclusion
there must be some factor in additionthere must be some factor in additionto cyclic conjugation that determines to cyclic conjugation that determines whether a molecule is aromatic or notwhether a molecule is aromatic or not
Hückel'sHückel's RuleRulethe additional factor that influences the additional factor that influences
aromaticityaromaticity is the number of is the number of ππ electronselectrons
among planar, monocyclic, completely among planar, monocyclic, completely conjugated conjugated polyenespolyenes, only those with 4, only those with 4nn + 2 + 2 ππ electrons possess special stability (are electrons possess special stability (are aromatic)aromatic)
nn 44nn+2+2
0 0 22
1 1 66 benzene!benzene!
22 1010
33 1414
44 1818
Hückel'sHückel's RuleRule
Hückel'sHückel's Rule for Rule for AromaticityAromaticity
To be Aromatic …a compound must :To be Aromatic …a compound must :
1.1. be Cyclicbe Cyclic
2.2. have one P orbital on each atom in the ringhave one P orbital on each atom in the ring
3.3. be planar or nearly so to give orbital overlapbe planar or nearly so to give orbital overlap
4.4. have a closed loop of 4n+2 pi electrons in the have a closed loop of 4n+2 pi electrons in the
cyclic arrangement of p cyclic arrangement of p orbitalsorbitals
Hückel'sHückel's RuleRule
defines a condition for cyclic molecules in whichdefines a condition for cyclic molecules in which
the bonding molecular the bonding molecular orbitalsorbitals are filled and there are filled and there
are no electrons in nonare no electrons in non--bonding or bonding or antibondingantibonding
orbitalsorbitals ….roughly analogous to the “rare gas” ….roughly analogous to the “rare gas”
condition condition fprfpr atomic atomic orbitalsorbitals……
ππ--MOs of BenzeneMOs of Benzene
AntibondingAntibonding
BenzeneBenzene
BondingBonding6 6 ππ electrons fill all of the bonding electrons fill all of the bonding orbitalsorbitalsall all ππ antibondingantibonding orbitalsorbitals are emptyare empty
ππ--MOs of MOs of CyclobutadieneCyclobutadiene(square planar)(square planar)
AntibondingAntibonding
CycloCyclo--butadienebutadiene BondingBonding
4 4 ππ electrons; bonding orbital is filled; other 2electrons; bonding orbital is filled; other 2ππ electrons singly occupy two nonbonding electrons singly occupy two nonbonding orbitalsorbitals
ππ--MOs of MOs of CyclooctatetraeneCyclooctatetraene(square planar)(square planar)
CycloCyclo--octatetraeneoctatetraene
AntibondingAntibonding
BondingBonding
8 8 ππ electrons; 3 bonding electrons; 3 bonding orbitalsorbitals are filled; 2are filled; 2nonbonding nonbonding orbitalsorbitals are each halfare each half--filledfilled
ππ--Electron Requirement for Electron Requirement for AromaticityAromaticity
notnotaromaticaromatic aromaticaromatic notnot
aromaticaromatic
4 4 ππ electronselectrons 6 π electrons6 π electrons 8 8 ππ electronselectrons
Completely Conjugated Completely Conjugated PolyenesPolyenes
6 6 ππ electrons;electrons;not completelynot completely
conjugated
6 π electrons;completely conjugated
6 π electrons;completely conjugated conjugated
notnotaromaticaromatic
HH HH
aromaticaromatic
AnnulenesAnnulenes
AnnulenesAnnulenes are planar, monocyclic, completely are planar, monocyclic, completely conjugated conjugated polyenespolyenes. That is, they are the . That is, they are the kind of hydrocarbons treated by kind of hydrocarbons treated by Hückel'sHückel'srule.rule.
[10]Annulene[10]Annulene
predicted to be aromatic by predicted to be aromatic by Hückel'sHückel's rule,rule,but too much angle strain when planar and but too much angle strain when planar and all double bonds are all double bonds are ciscis
1010--sided regular polygon has angles of 144°sided regular polygon has angles of 144°
[10]Annulene[10]Annulene
strain betweenstrain betweenthese two these two hydrogenshydrogens
incorporating two trans double bonds intoincorporating two trans double bonds intothe ring relieves angle strain but introducesthe ring relieves angle strain but introducesanother kind of strain into the structure andanother kind of strain into the structure andcauses the ring to be distorted from planaritycauses the ring to be distorted from planarity
14 14 ππ electrons satisfies electrons satisfies Hückel'sHückel's rulerule
There is some strain between There is some strain between hydrogenshydrogens insideinsidethe ring the ring
How about [14]Annulene ??How about [14]Annulene ??
HH HH
HH HH
16 16 ππ electrons does not satisfy electrons does not satisfy Hückel'sHückel's rulerule
alternating short (134 pm) and long (146 pm) bondsalternating short (134 pm) and long (146 pm) bonds
not aromatic
[16]Annulene ??[16]Annulene ??
not aromatic
[18]Annulene[18]AnnuleneThe protons resonate at-3.0 and at 9.3δ!!!
18 18 ππ electrons satisfies electrons satisfies Hückel'sHückel's rulerule
resonance energy = 418 kJ/molresonance energy = 418 kJ/mol
bond distances range between 137bond distances range between 137--143 pm143 pm
HH HHHH
HHHHHH