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4/29/12
1
Chapter 7
Aroma,city
The goal of this chapter: • Illustra,ng the mul,faceted defini,on of aroma,city • Quan,fying (an,)aroma,city. • Iden,fying (an,)aroma,c molecules
Il me faut cependant avouer que la chimie proprement dite ne m’a jamais beaucoup intéressé. Pourquoi ? Peut-‐être parce que des no>ons telles que celles de valence, de liaisons chimique etc., m’ont toujours semblé peu claires du point de vue conceptuel. René Thom, 1983. I have to confess that I have never been really interested in chemistry. Why? Maybe because such no>ons as valence, bond lengths etc. have always seemed unclear to me from the conceptual point of view.
A fuzzy chemical concept
Chapter 7 Gonthier, J. Steinmann, S. N.; Wodrich M. D.; Corminboeuf, C. Chem. Soc. Rev. in press. 2012
4/29/12
2
What is Aroma,city?
Aroma,city
Schleyer and Jiao, Pure Appl. Chem. 1996, 68, 209-‐218
aroma1c smell (before 1825)
Hight carbon ra1o (before 1865)
Discovery of benzene Faraday (1825)
Subs1tu1on > addi1on Erlenmeyer (1866)
Benzene structure Kekulé 1865
Exalted diamagne1c suscep1bility Pascal (1910)
Electron sextet Armit-‐Robinson (1925)
4n+2 electron Hückel (1931)
Ring current theory Pauling (1936)
pi electron to contribu1on to magne1c suscep1bilty London (1937)
Ring current effect on NMR chemical shiZ, Pople (1956)
Magne1c sucsep1bility exalta1on Dauben (1969) Flygare (1970)
Nucleus-‐Independent chemical shiZ (NICS) Schleyer (1996)
historically Structure criteria Reac,vity criteria Energy criteria Magne,c criteria
Quantum chemical evalua1on of delocaliza1on energy (2000)
Structural aspects of aroma1city (not discussed here)
Energy evala1on through theromochemiscal data Kis1akowsky (1936)
Chapter 7
Aroma,city
1865 (Kekulé structure)
Chapter 7
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Aroma,city
Defini1on: They are unreac1ve to common double bond transforma1on.
Benzene undergoes subs1tu1ons rather than addi1ons reac1ons (Erlenmeyer, 1866).
Chapter 7
Ek =α + 2β cos kπ(n +1)
Ek =α + 2β cos 2kπ(n)
acyclic chains
cyclic systems (with even number of atoms)
n= number of atoms
Chapter 7
Hückel theory and Aroma,city
Defini1on: Aroma1c compounds are unusually stable!
k = 0, 1, 2…
k = 1, 2, 3…
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Aroma,city
First Defini1on: Aroma1c compounds are unusually stable! Quantum chemical demonstra,on using MO Theory:
Num
ber o
f nod
es =
Ene
rgy
Chapter 7
4n+2 π electrons
E1=α+2β
E2α+β
The stabiliza,on compared to three isolated bonds: 8β-‐ 6β = 2β The stabiliza,on of hexatriene
bonds: 7β-‐6β = β
E1=α+1.8β
E2=α+1.24β
E3=α+0.44β
Aroma,city
First Defini1on: Aroma1c compounds are unusually stable! Quantum chemical demonstra,on using MO Theory:
Chapter 7
4n π electrons
E1=α+2β
E2=E3=α
The stabiliza,on compared to three isolated bonds: 4β-‐ 4β = 0
Num
ber o
f nod
es =
Ene
rgy
E1=α+1.62β
E2=α+0.62β
The stabiliza,on of butadiene bonds: 4.48β-‐4β = 0.48β
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Aroma,city
Defini1on: Aroma1c compounds are unusually stable! Resonance (old terminology=mesomerism): bonding pagern described by mul,ple resonance structures
Conjuga1on effects: Stabiliza,on when double bonds come into conjuga,on
Hyperconjuga1on/anomeric effects: Stabiliza,on when orbitals of the π-‐ and σ frameworks interacts.
Aroma1c effects: Aroma,c stabiliza,on energy
Resonance or delocaliza1on Energy: The Pauling-‐Wheland defini,on of “resonance energy” captures all these “delocaliza,on” effects”.
)()(RE 1 Ψ−= EE ψ
The quan,ty obtained by subtrac,ng the actual energy of the molecule in ques,on from that of the most stable contribu,ng structure.
Wheland, “The Theory of Resonance”, 1944, Page 52. Chapter 7
Aroma,city (RE and ASE)
Conven1onal Evalua1on using a selec,on of reference systems: isodesmic or homodesmo1c reac1ons RE vs. ASE 3 C2H6 + 3 C2H4 + 6 CH4 -65.1 kcal/mol
3 C2H4 + + 3 C2H6 -48.5 kcal/mol
3 + 2 -36.0 kcal/mol
3 + + 3 -28.8 kcal/mol
3 + 3 C2H4 -20.5 kcal/mol
3 + 3 -22.5 kcal/mol
RE
RE
RE (historic but flawed)
ASE value recommended
ASE (from Dewar)
ASE Warning: these equa1ons are not balanced for hyperconjuga1on and branching effects (as discussed earlier in this course) Chapter 7
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Aroma,city (RE)
Kis1akowsky’s seminal evalua1on of the resonance energy of benzene: historically important but flawed.
Chapter 7
Rappel: hyperconjuga1on
Resonance in Benzene (RE)
Direct energy-‐based computa1onal approaches: aroma,c molecules are more stable than their “localized” analogues. One constructs a “localized” resonance structure and compute the delocaliza1on energy by comparing the difference between the energy of the standard molecule and that of the lowest-‐energy resonance structure.
benzenerigid 1,3,5-cyclohexatriene
optimal 1,3,5-cyclohexatriene
VRE
AREΔEc
1.386Å
1.316-‐1.314Å
1.517-‐1.522Å
=Adiaba,c RE= 61.4 kcal mol-‐1
=Ver,cal RE 91.6 kcal mol-‐1
(BLW)-‐B3LYP-‐pVTZ
Chapter 7
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7
Block Localized Wavefunc,on (BLW) Method
BLW: B3LYP/6-‐31G* Y. Mo, S. D. Peyerimhoff, J. Chem. Phys. 1998, 109, 1687–1697. Y. Mo, L. Song, Y. Lin J. Phys. Chem. A 2007, 111, 8291–8301.
• Evaluates resonance energies (RE’s) without reference molecules
• “Disables” selected interac,ons
–
E(BLW)localized π
system
E(DFT)delocalized π
system
RE
= 65.4 kcal/mol
�
ΨIBLW = ˆ A {Φ1Φ2Φk}
)()3()2()1(2
211 iniiiii niβϕαϕβϕαϕ =Φ
∑=
=im
iijij C1µ
µµχϕ
⎩⎨⎧
≠=
=kiski
ikjl
jlklij
δϕϕ
= +61.4 kcal/mol
Chapter 7
Aroma,city in Benzene (ASE)
The ASE evaluates the “extra benzene resonance energy” rela1ve to conjugated but non-‐aroma1c reference molecules:
The recommended value based on chemical equa,ons is 28.8 kcal mol-‐1.
A related aroma,city probe is the “extra cyclic resonance energy” (ECRE) defined as the difference between the resonance energies of a cyclic conjugated compound and an acyclic polyene either with the same number of bonds (ECRE1) or with the same number of diene conjuga1ons (ECRE2).
A third alterna,ve is the “isomeriza1on stabiliza1on energy” (ISE) based on the energy difference between cyclically delocalized and merely conjugated isomers.
Chapter 7
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Extra Cyclic Resonance Energy (ECRE)
ECRE: Energy difference between the resonance energies of a cyclic conjugated compound and its corresponding acyclic polyene
ECRE1: same number of double bonds
= +35.6 kcal/mol
ECRE 2: same number of conjuga1ons
RE – RE
ECRE > 0 Aroma,c ECRE ≈ 0 Non-‐aroma,c ECRE < 0 An,aroma,c Y. Mo, P. v. R. Schleyer Chem. Eur. J.
2006, 12, 2009–2020.
RE – RE = +21.2 kcal/mol3 x
RE – 3 x RE = +25.5 kcal/mol
BLW: B3LYP/6-‐31G*
+28.8 kcal/mol (expt.)
Balanced for hyperconjuga,on, hybridiza,on and protobranchings (as seen later in the course).
Best experimental aroma1c stabiliza1on energy (ASE) es1mate for benzene
3+ 3+
61.4 kcal/mol 25.8 kcal/mol
12.2 kcal/mol
10.5 kcal/mol
= +24.8 kcal/mol
= +29.9 kcal/mol
Chapter 7
An,aroma,city of D2hCyclobutadiene
Es,ma,ng the destabiliza,on imparted by the an,aroma,city of cyclobutadiene is more of a challenge. According to Hückel Theory, the π-‐electronic energy of CBD is twice that of ethene (i.e. RE=0).
ΔHf 37.5 6.7
2
114
ΔH° = 45.7 kcal/mol
How to incorporate the strain effects?
1.588-‐1.595Å
1.317Å
Is the an,aroma,city of CBD really more substan,al than the aroma,city of benzene (~30 kcal/mol)?
Chapter 7
4/29/12
9
BLW: B3LYP/6-‐31G*
CBD Resonance energy (RE)
E(BLW) Localized
E(DFT) Delocalized
= +5.1 kcal/mol
Extra cyclic resonance energy
ECRE= –15.9 kcal/mol
+26.6 kcal/mol+10.1 kcal/mol
RE – RE
+13.3 kcal/mol
RE – RE 2
Antiaromatic species do NOT have negative RE’s, but are net π stabilized!
ECRE2 based on models with two conjugations
CBD is only modestly destabilized by an1aroma1city!
+10.5 kcal/mol"
+5.1 kcal/mol" +21.0 kcal/mol"
Flawed literature es,mates –35 to –45 kcal/mol
ECRE2 for D2h Cyclobutadiene (CBD)
Chapter 7
+ 4 H2C=CH2 4
+ 4 H2C=CH2 4imposed 135 deg
CCC angle
–14.18 kcal/mol
–3.79 kcal/mol
Flawed ASE evaluation
Better ASE evaluation
ECRE2 for D4h Cyclooctatetraene (COT)
(too large due to the 10-11 kcal/mol D4h COT ring strain)
Homodesmo1c Equa1on (nega,ve aroma,c stabiliza,on energy, ASE, based on four conjuga,ons)
Extra cyclic resonance energy (ECRE)
ECRE = –3.2 kcal/mol
ECRE2 based on models with four conjugations
COT is very weakly destabilized by an1aroma1city!
RE RE 4–
+10.5 kcal/mol+38.8 kcal/mol
BLW: B3LYP/6-‐31G*
(B3LYP/6-‐311+G**with ZPE)
Chapter 7
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10
C6H6 + 3H2 C6H12 ΔH1 = -‐49.8 kcal/mol C6H8 + 3H2 C6H14 ΔH2 = -‐81.0 kcal/mol
R1
R2
R3
BLW-‐HF op,miza,on on C6H8:
R1 R2 R3
HF/6-‐311+G(d,p) 1.324 1.463 1.329 BLW/6-‐311+G(d,p) 1.316 1.517 1.312
Basis Set VRE ARE
6-‐311+G(d,p) 23.5 20.8
ECRE of benzene:
Basis Set ECRE1 ECRE2 6-‐311+G(d,p) 36.7 25.7
Isomeriza,on Stabiliza,on Energy (ISE): CH3 CH2
H H ΔH = 33.2 kcal/mol
Schleyer, P. v. R., Puhlhofer, F. Org. Chem. 2002, 4, 2873.
Aroma,city of Benzene (ECRE1)
aR
cR EE1ECRE −=
CC
CX
C
CC
CX
C
cRE
C
C
C
C X
C
C
C
C X
aRE
aR
cR EE2ECRE −=
CC
CX
C
CC
CX
C
cRE
aRE C
C
C
C X
c c
C
C
C
C X
c c
5-‐Membered Rings
Chapter 7
4/29/12
11
X
6-311+G(d,p)
ECRE1 ECRE2 NICS AlH BH CH+ CH- CH2 NH O PH S SiH+ SiH- SiH2
-1.1 -2.7 -28.2 42.8 7.7 34.2 25.8 30.8 21.7 -8.9 34.3 1.4
-3.5 -8.2 -35.4 19.1 3.4 17.9 12.8 17.9 12.7 -15.5 17.2 -0.8
5.4 15.8 46.9 -13.7 -4.1 -14.4 -14.8 -17.2 -15.9 11.2 -14.1 0.3
Table Extra cyclic resonance energies (kcal/mol) and NICS values (ppm) of 5-‐membered rings C4XH4
5-‐Membered Rings
Chapter 7
Op,mal delocalized and localized geometries for C5H5+, C5H5
-‐ and C5H6 with the 6-‐311+G(d,p) basis set
1.331Å
1.449Å
1.317Å
1.509Å
1.405Å
1.405Å
1.325Å
1.533Å
1.329Å
1.505Å
1.314Å
1.547Å
CC
CX
C
CC
CX
C
1.549Å 1.544Å
X=CH+
CC
CX
C
CC
CX
C
1.405Å 1.547Å
X=CH-
CC
CX
C
CC
CX
C
1.477Å 1.539Å
X=CH2
5-‐Membered Rings
Chapter 7
4/29/12
12
1.410Å
1.410Å
1.347Å 1.347Å
X=CH2+
X=CH2-
X=CH3
C
C
C
C X
1.514Å
1.324Å
1.314Å 1.480Å C
C
C
C X
1.409Å
1.409Å
1.364Å 1.364Å C
C
C
C X
1.520Å
1.322Å
1.321Å 1.524Å C
C
C
C X
1.467Å
1.324Å
1.324Å 1.501Å C
C
C
C X
1.518Å
1.313Å
1.316Å 1.534Å C
C
C
C X
Op,mal delocalized and localized geometries for C5H7+, C5H7
-‐ and C5H8 with the 6-‐311+G(d,p) basis set
5-‐Membered Rings
Chapter 7
Es,mate of conjuga,ve and hyperconjuga,ve Stabiliza,ons
Values are in kcal mol-1 BSE=bond separation energy
Molecule Conventional BSE BLW
2.5 5.7 5.4
5.0 7.8 10.5
3.7 14.8 9.9
0.2 15.1 20.1
NA NA 3.3
36.0 64.4 57.5
H3C CH3
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Aroma,city
Altnerna1ve defini1on: Aroma1c compounds exhibits a ring current ! Magne1c Criteria
δ(1H )/ppm 0 7.3
TMS
6.2
Chapter 7
• 1H NMR chemical shiZ: A criterion most o~en used experimentally.
• Due to the ring current induced by an external magne,c field, the inner protons are shi~ed upfield, and the outer protons are downfield-‐shi~ed.
Magne,c Aroma,city
Chapter 7
4/29/12
14
Hydrogens in bridging posi1ons
δ1H [ppm]
E. Vogel, 1983
Magne,c Aroma,city
Chapter 7
But !!!
4-‐5 an,aroma,c H1: 6.10
H2: 7.71 nonaroma,c
H1: 5.78 H2: 6.26 H3: 6.36 4-‐membered ring is an,aroma,c
H1: 8.6 H2: 8.1 H3: 8.5 Nonaroma,c
Magne,c Aroma,city
O
H2
H1
H2 H3
H1 H2
H3
H1
Chapter 7
4/29/12
15
7Li+ NMR Chemical ShiZ
• Lithium bonding is primarily electrosta,c, experimental 7Li chemical shi~s generally shows ligle varia,on among different compounds.
• Lithium ca,ons, typically coordinate to the π faces of aroma,c (or an,-‐aroma,c) systems.
• This complexa,on results in a significant shielding (or deshielding) of the 7Li NMR signal due to ring current effects.
Magne,c Aroma,city
Chapter 7
7Li+ NMR as an Experimental probe
(aroma,c) Paquege, L. A. et al, JACS, 1990, 112, 8776.
(An,aroma,c) Sekiguchi et al, JACS, 1991, 113, 7081.
Magne,c Aroma,city
Chapter 7
4/29/12
16
• Experimental 7Li NMR chemical shi~s can be well reproduced by modern computa,ons.
• The clear advantage of using δ(7Li) as a theore,cal probe lies in the possibility to provide a comparison with 7Li NMR spectrum of experimental Li+ complexes.
• However, the number of Li+ complexes and therefore the u,lity of Li+ as a computa,onal probe are rather limited.
Magne,c Aroma,city
Advantages and limita1ons of 7Li+ NMR Chemical ShiZ
Chapter 7
Why not use the absolute chemical shielding of a virtual nucleus to probe
(the ring current effects of) aroma>city? -‐-‐Schleyer et al, JACS, 1996, 118, 6317.
Magne,c Aroma,city
Chapter 7
4/29/12
17
The twelve outside hydrogens resonate at δ = 9.0 ppm
The six inner hydrogens resonate at δ =-3.0 ppm
Upfield of TMS !!!
Nucleus-‐Independent Chemical Shi~s (-‐14.2 ppm)
1996 Schleyer: Nucleus-‐Independent Chemical Shi~s (NICS): J. Am. Chem. Soc. 1996, 118, 6317.
NMR proper1es of [18]-‐annulenes
HH
HH
HH
HHH
H
H
H
HH H
H
H
H
Magne,c Aroma,city
Chapter 7
-8.6 ppm
+20.9 ppm
-2.0 ppm
NICS are the nega1ve of magne1c shieldings computed at non-‐nucleus posi1ons Nega1ve (diatropic, upfield); posi1ve (paratropic, downfield)
Nucleus-‐Independent Chemical ShiZs = NICS (the most used aroma1city probe).
Magne,c Aroma,city
Chapter 7
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18
benzene cyclohexane cyclobutadiene
Paratropic (B deshielded) Diatropic (B shielded)
Aromatic: long-range magnetic shielding Antiaromatic: long-range magnetic deshielding Non-aromatic:short range magnetic response
PW91/IGLOIII
Magne,c criteria : the nucleus-‐independent chemical shi~
Chapter 7
Grid of NICS points
σ-‐aroma1city
“Cyclopropane should be isoconjugate with benzene and hence σ-‐aroma1c.”
Dewar, J. Am. Chem. Soc. 1984, 106, 669
Dewar at Dyson
Chapter 7
4/29/12
19
σ-‐aroma1city
Dewar, J. Am. Chem. Soc. 1984, 106, 669 Chapter 7
H H
H
H
HH
Walsh sp2 model
σ-‐aroma1city
Chapter 7
4/29/12
20
Why is the strain in cylcopropane ���and cyclobutane so similar?
angle deviation
60°
109.49° tetrahedral value
angle deviation
109.49°- 60°
49.49°
ring size ring strain kcal/mol
3 4 5 6 7
49.44° 19.44°
1.49° -10.56° -19.13°
27.7 26.8
7.1 0.7 6.8
Baeyer Stain (1885)
Chapter 7
Dewar’s original idea of “σ” aroma1city
Dewar, JACS 1984, 106, 669. Cremer and Kraka, JACS, 1985, 107, 3800 and 3811. Cremer and Gauss, JACS, 1986, 108, 7467.
Devia1on due to σ-‐aroma1city
H2C CH2
H2C
6 σ electronsσ-aromatic
Chapter 7
4/29/12
21
Evidence for the σ-‐aroma1city of cyclopropane
Anisotropy of Current Induced Density (ACID) Herges et al. Chem. Rev. 2005, 105, 3758
Diatropic current Negative NICS
The proton chemical shiZ appears upfield as compared to a similar acyclic molecule
1H δ(ppm)
cyclopropane Propane (CH2)
0.22 1.1
-42.8 ppm
NICS Moran, Heine, Manoharan and Schleyer Org. LeZ. 2003, 5, 23.
Chapter 7
Evidence for the σ-‐an1aroma1city of cyclobutane
ACID Herges et al. Chem. Rev. 2005, 105, 3758.
Paratropic current Positive NICSzz
• Dewar first argued that cyclobutane should be considered as σ-‐an1aroma1city but predicted a small destabiliza1on energy.
• The σ-‐an1aroma1city hypothesis is confirmed by magne1c criteria.
NICS Moran, Heine, Manoharan and Schleyer
Org. LeZ. 2003, 5, 23.
+55.1 ppm
Chapter 7
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22
Aroma1city
Chapter 7
Beyond σ and π, beyond organic chemistry
P
P
2.204Å
P P
Super σ-‐aroma,c
NICS ~ -50 ppm
Spherical or 3D aroma1cicy
P4
Chapter 7
closoboranes
4/29/12
23
Science, 2001, Vol. 291, 859.
Prepara,on: Laser vaporiza,on Spectra: Photoelectron spectra Characteriza,on: measured and computed ver,cal electron detachment energies (VDE) agree well
Chapter 7
The Concept of Double Aroma1city
• What is double aroma,city? – The existence of two mutually orthogonal Hückel frameworks
within a single molecule • Stabiliza,on of the structure by a 4n+2 π electron system in the plane
of a molecule in addi,on to the normal 4n+2 π electron system perpendicular to the plane
zx
y
Chandrasekhar, Jemmis, Schleyer Tetrahedron LeZ.1979, 3707. Schleyer, Jiao, Glukhovtsev, Chandrasekhar, Kraka J. Am. Chem. Soc. 1994, 116, 10129.
Radial in-plane
Chapter 7
4/29/12
24
Prototype Double Aroma1c
C6H3+ is stabilized by 6π electrons and 2 in-‐plane radial
electrons
H
H H
+15
3
π MO Radial MO
Chapter 7
Tangen1al σ aroma1city
tangential p-p bonded σ- aromaticity
R. Hoffmann: “A chemist view on bonding in extended structures” 1988.
(CH3)82+
D4h
But pronounced diatropic ring current: NICSzz=-43
Long C-‐C distance=2.361 Å
Chapter 7
4/29/12
25
Mini Quiz 8
1. What is aroma1city? 2. Which isomer is the most stable, which is the stronger acid and why? 3. Iden1fy each of the following molecules as being aroma1c, an1aroma1c or
non-‐aroma1c. How would you verify your predic1on?
HH
orH
H
2-
N
NH N
HN
Chapter 7