noncovalent interactions: electrostatic...
TRANSCRIPT
Charge-charge
Charge-diplol
Dipole-dipol
Charge-induced dipole
Dipol-induced dipole
Dispersion
Van der Waals repulsion
Hydrogen bond
NH3+ -OOC
NH3+ O
H
H
q- q+
OH
H
q- q+ OH
H
q- q+
NH3+ q- q+
OH
H
q- q+ q- q+
q-
q-q+
q+
N H O
1/r
1/r2
1/r3
1/r4
1/r5
1/r6
1/r12
Energydependenceon distance
Noncovalent Interactions
Electrostatic Energy:Israelachvili, J. Intermolecular and Surface Forces, 2nd ed.; Academic Press, London, 1991.
Electrostatic Effect and Bond Energies:Wiberg, K. B. „The Role of Electrostatic Effects in Organic Chemistry“, J. Chem. Edu. 1996, 73, 1089.Wiberg, K. B. „The Interaction of Carbonyl Groups with Substituents“, Acc. Chem. Res. 1999, 32, 922.Kemnitz, C. R.; Loewen, M. J. „Amide Resonance Correlates with a Breadth of C-N Rotation Barriers“,J. Am. Chem. Soc. 2007, 129, 2521.P. R. Rablan „Is the Acetate Anion Stabilized by Resonance or Electrostatics? A Systematic StructuralComparison“, J. Am. Chem. Soc. 2000, 122, 357.
Electrostatics and Conformation:Wiberg, K. B., Wang, Y.-g., Petersson, G. A., Bailey, W. F „Intramolecular Nonbonded AttractiveInteractions: 1-Substituted Propenes“, J. Chem. Theory Comput. 2009, 5, 1033.Gooseman, N. E. J.; O‘Hagan, D.; Peach, M. J. G.; Slawin, A. M. Z., Tozer, D. J.; Young, R. J. „AnElectrostatic Gauche Effect in b-Fluoro- and b-Hydroxy-N-ethylpyridinium Cations“, Angew. Chem.Int. Ed. 2007, 46, 5904.Smith, M. D.; Woerpel, K. A. „Electrostatic interactions in cations and their importance in biology andchemistry“, Org. Bio. Chem. 2006, 4, 1195.
Oxocarbenium Chemistry:Yang, M. T.; Woerpel, K. A. „The Effect of Electrostatic Interactions on Conformational Equilibria ofMultiply Substituted Tetrahydropyran Oxocarbenium Ions“, J. Org. Chem. 2009, 74, 545.Lucero, C. G.; Woerpel, K. A. „Stereoselective C-Glycosylation Reactons of Pyranoses: TheConformational Preference and Reaction of the Mannosyl Cation“, J. Org. Chem. 2006, 71, 2641.
Dipol Controlled Nucleophilic Addition:Wipf, P.; Jung, J.-K. „Nucleophilic Additions to 4,4-Disubstituted 2,5-Cyclohexadienones: CanDipole Effects Control Facial Selectivity?“, Chem. Rev. 1999, 99, 1469.
Inductive Effect: Polarization of electron density in bonds, caused primarily by electronegativity differences.
Electrostatic Effect: Interaction between atomic charges in various parts of a molecule.. The effect is transmitted through space (i. e. a field effect).
Ion-Dipole Interaction:
for r > l: point-dipol approximation (l→0)
Charge-Charge Interaction: Coulomb Law
repulsion between like charges
attraction between unlike charges
between a unit charge (Q = e) anda dipol (u = ql = 1 D) in vacuum (ε = 1)
no interaction energy
Solid line: energy for l = 0.1 nm and l = 0.2 nm
dashed line: energy for l = 0
maximal Interaction Energy for cationswith a H2O molecule at 300 K
Na+: w(r, θ = 0°) = 22.9 kcal/mol (39kT)
Li+: 29.8 kcal/mol
Mg2+: 59 kcal/mol
Charge-Dipol Interaction Energy
Some Examples:
Bond Dissociation Energy (BDE)
Pauling Electronegativities
C2.55
N3.04
O3.44
F3.98
Si1.90
P2.19
S2.58
Cl3.16
difference in electronegativity leads to bond polarisation (charge separation)
coulombic attraction increases bond strength
bond polarisation affects σ and π bonds
H3C X CH3 + X
BDE (kcal/mol)
H3C CH3
H3C NH2
H3C OH
H3C F
89
86
92
110
H3C SiH3
H3C PH2
H3C SH
H3C Cl
90
70
74
83+C F-
-C Si+
+C Cl-
Increasing Electronegativity
π bond strength
C O
C C 64 kcal/mol
84 kcal/mol
K. B. Wiberg et al. J. Chem. Edu. 1996, 73, 1089.
Stabilization in Polyfluorinated Compounds
CF4 + 3 CH4 4 CH3F !H = +53 kcal/mol
C
F
F
C
F+
F-
C
F
Fn(F) !"(CF)
C
F
H
C
F
F
!+
!- !-
!-
2!+
Valence-Bond Theorie MO Theorie
Electrostatic Effect
CH3F
CH2F2
CHF3
CF4
-0.743
-0.744
-0.744
-0.737
-0.429
-0.429
-0.421
-0.405
-0.550
-0.576
-0.576
-0.551
AIM NPA GAPT
Atomic Charges at Fluorine
why is CF4 more stable than CH3F?
F is a poor lone pair donor
Increased positive charge at carbon leadsto stronger electrostatic attraction
C
SiH3
SiH3
!+
2!-
!+
C
F
SiH3
!-
!+
!+
C(SiH3)4 + 3 CH4 4 CH3(SiH3) !H = +13 kcal/mol
FCH2SiH3 + CH4 !H = -7 kcal/molCH3F CH3SiH3+
H3CCNH2
O
H3CCNH2
+
O-
H3CC+
NH2
O-
Amide Resonance and CO-X Interactions
H3C
O
NH2
+ H3C CH3H3C
O
CH3
+ H3C NH2
Group Transfer Reaction
H3C
O
N H3C
O
NH
H
HH
Rotation
Group Separation Energy (GSE)Interaction Energy between CO and C-N
ΔHπ
rotational barrier: ~ 15 kcal/mol
π Electron Interactions
K. B. Wiberg et al. Acc. Chem. Res. 1999, 32, 922.
H3C
O
X
+ H3C CH3H3C
O
CH3
+ H3C X
F
OH
NH2
Cl
+16.7
+22.7
+19.3
+6.8
0.0
+11.5
+13.9
0.0
+16.7
+11.2
+5.4
+6.8
GSE !H" !H#
H
S
X
+ H3C CH3H
S
CH3
+ H3C X
F
OH
NH2
Cl
+4.7
+15.7
+18.4
+0.1
0.0
+12.3
+18.0
0.0
+4.7
+3.5
+0.5
+0.1
GSE !H" !H#
H3CC+
X
O-
Electrostatic Interactions more importantfor electronegativ X (F, OH)
H3CC
X+
O-
C=S bond less polarizedπ bond contributions more important
Me-X BDE (kcal/mol)
°•
planar structure
90° rotated structure (without ΔHπ)
Slope of ~1.5: increased positive charge at carbon leads to stronger CO-bond
negative charge at carbon destabilizes the compound e.g. CO-Si, CO-CF3,…
Ac-X BDE (kcal/mol)
!+H3C
C+
SiH3
O-
!-!-
H3CC+
F
O-
!+H3CC+
CH3
O-
Comparison Ac-X and Me-X Bond Disoziation Energy
H3C CH3
O
H3C NH2
O
H3C OH
O
H3C F
O
1.222 ! 1.220 ! 1.212 ! 1.185 A
CO-bond length
Acidity of Carboxylic Acids
H3CCO-
O
H3CCO
O-
H3CC+
O-
O-
Increasing Polarisation of Ac-X
H3CCOH
O
H3CCO-
O
+ H+
H3C OH + H+H3C O-Methanol: pKa(H2O) = 15.5
Acetic acid: pKa(H2O) = 4.76
stabilisation by resonance electrostatic stabilisation
P. R. Rablan J. Am. Chem. Soc. 2000, 122, 357.
H3C
X
H3C X
E favored by 1.1 kcal/mol Z favored X = OMe
X = Cl
0.53 kcal/mol
0.68 kcal/mol
X = Br 0.45 kcal/mol
Nonbonded Interactions in 1-substituted Propenes
H3C
CH3
H3C CH3
Relative Energies (E→Z) in kcal/mol
HF calculations do not include electroncorrelations (no attractive van der Waals terms)
DFT allows some correction for electron correlationCCSD(T) gives superior correction for this effect.
Energie difference in HF and MP2 calculations for X = Cl, Br, SMe: attractive van der Waals interaction?
calculated Energies independend from used method for X = F, OMe
K. B. Wiberg et al. J. Chem. Theory Comput. 2009, 5, 1033.
H3C CH3
H H
!+ !-H3C F
H H
H3C Br
H H
Steric Repulsion Electrostatic Attraction (X = F, OMe)
Dispersion(X= Cl, Br, OMe)
calculated C=C-CH3 angeles
cis-bond angels larger than trans
difference in bond angles increaseswith size (F→Cl)
contributions to relative energies (kcal/mol)
cis preference is combination ofCoulombic attraction and
dispersion interactions
F
H H
HH
F
H
H F
HH
F
gauche favoured by 0.5-1.0 kcal/mol
Electrostatic Gauche Effect
stereoelectronic effect: σ(CH) → σ*(CF)
1,2-Difluoroethan:
β-Fluoroethylamin
NH2
H H
HH
F
H
H NH2
HH
F
0.9 kcal/mol
H
H NH
HH
FH
-1.0 kcal/mol0.0 kcal/mol
NH3+
H H
HH
F
H
H NH3+
HH
F
-5.8 kcal/mol0.0 kcal/mol
β-Fluoroethylammonium
OH
H H
HH
F
H
H OH
HH
F
H
H O
HH
FH
OH2+
H H
HH
F
H
H OH2+
HH
F
H
H OH+
HH
FH
0.0 kcal/mol -0.3 kcal/mol -2.0 kcal/mol 0.0 kcal/mol -4.4 kcal/mol -7.2 kcal/mol
2-Fluoroethanol protonated 2-Fluoroethanol
gauche preferred in charged system: electrostatic Attraction
D. O‘Hagan et al. Angw. Chem. Int. Ed. 2007, 46, 5904.
N
H H
HH
F
H
H N
HH
F
N+
H H
HH
OH
H
H N+
HH
OH
R = H: 0.0 kcal/mol -3.7 kcal/mol
-3.1 kcal/mol
0.0 kcal/mol -0.05 kcal/mol
0.0 kcal/mol -3.7 kcal/mol
N+
H H
HH
F
R
H
H N+
HH
F
R
R = NMe2: 0.0 kcal/mol
N-(2-fluoroethyl)pyridinium cation
no preference in uncharged system
N-(2-hydroxyethyl)pyridinium cation
C2‘ endo C3‘ endo
NAD+
NH2+
HOHO
OH
OHNH2
+
OH
OH
favored by 4.0 kcal/mol
favored by 0.6 kcal/mol
pKa = 7.5
pKa = 9.5
exo favored by 3.4 kcal/mol
endo favored by 4.1 kcal/mol
N+
Me
Me
F
N+
Me
Me F
Me
Me F
Me
Me
F
NN
CN
F
H
H
O
O
N+N
CN
H
H
O
O
H
F
H+
favored by 0.4 kcal/mol
O
MeO
!+!-
!-
O
MeO
Electrostatic Effects and Conformational Analysis
electrostatic stabilization through space
shorter distance between axial-OMeand carbonyl carbon
K. A. Woerpel et al. Org. Biomol. Chem. 2006, 4, 1195.
O OAc
X
SiMe3
SnBr4
O C3H5
X
O C3H5
X
4
OBn
Me
01:99
94:06
cis/trans
decrease in selectivity from F to I: no anchimeric assistence
O+
4
Nu
Me
O+
4
Nu
OBn!-
Electrostatic Effects in Oxocarbenium Chemistry
O
X+
Nu
F
Cl
05:95
14:86
Br
I
31:69
28:72
pseudoaxial configuration favoured by electrostatic interactions
K. A. Woerpel et al. Org. Biomol. Chem. 2006, 4, 1195.
O+
4
Nu
OBn!-
O+
3
Nu!-BnO
O+
4
Nu
!-
H
BnO 2
O+
Nu
!-OBn
H2
O
BnO
4
O
3
OBn
O
OBn
2
99:01 β-selectivity
O
BnO
OPO(OR)2
4
OBn
OBn
OBn
SiMe3
TMSOTf
O
BnO
OBn
OBn
OBn
!
89:11 β-selectivity 83:17 β-selectivity
α-isomer only
electrostaticstabilisation
no electrostatic preferencehyperconjugation from C2-H-bond
K. A. Woerpel et al. J. Org. Chem. 2009, 74, 545.
Oxocarbenium Chemistry
O
BnO
OPO(OR)2
4
OBn
OBn
OBn
SiMe3
TMSOTf
O
BnO
OBn
OBn
OBn
!
disfavored because ofsyn-pentan interaction
stereoelectronicallydisfavored
stereoelectronically disfavored
α-isomer only
Curtin Hammett scenario possible
O+
4
Nu
OBn
BnO
BnO
OBn
Nu
O+
4OBn
BnO
OBn
OBn
Nu
D-Mannosyl Cation
O
BnO
AcO
TMSCN
EtAlCl2 O
BnO
NC
4
SiMe3
SnBr4
OOAc
Me
O
Me
3
O+BnO
H
O+
H
BnO
!-
Nu
Nu
3
3
OBn
O+
O+
H OBn
H
H
Nu
4
4
Electrostatic stabilisation of oxocarbenium ions
dr = 99:01
dr = 94:06
SiMe3
SnBr4
OOAc
BnO
O
BnO
3
inside attack provides staggered product
favored by 2.5 kcal/moldr = 96:04
K. A. Woerpel et al. Org. Biomol. Chem. 2006, 4, 1195.
OR
O
COOMe
Pb(OAc)3
MeO
pyridineOR
O
COOMeAr
R = Me
R = TBS
80:20
95:05
dr
!+
O-MeOOC
O SiR3
4
Electrostatic stabilisation of an anionic intermediate
electrostatic interaction between enolate andelectropositive silicon stabilizes transition state
J. P. Konopelski et al. Org. Lett. 2002, 4, 4121.
Nucleophilic Additions to 4,4-disubstituted 2,5-Cyclohexadienones
OR'
OR MeMgBr
ORR'
OHMe
Diastereoselectivity?
OO
OMe
OTMS
!
"
OMe
OMe
"'42%
8.6:1 (32%) 17.7:1 (93%) 4.8:1 (81%)
O
O
O
Me
OBz
OMe
OH
5.5:1 (53%) 8.2:1 (85%)7.9:1 (26%)
!'58%!' 39%
OO O
32:1 (79%)
O
O
O
11:1 (27%)
P. Wipf et al. Chem. Rev. 1999, 99, 1469.