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Guillaume Barbe (1979- )
Université de MontréalNovember 11th 2008
From Newton to WoodwardComplete Construction of the Diels-Alder Correlation Diagram
Sir Isaac Newton1642-1727
Robert B. Woodward1917-1979
Theoritical Model forConcerted Reactions
Outlines
• Construction of Schrödinger equation from classical mechanics and routine mathematics
• Hückel Model of molecular orbitals will provide a quantification of the energies and orbital coefficients for polyenes
• Quick excursion in the rational of the symmetry-allowed Diels-Alder Cycloaddition
Classical Mechanics
Sir Isaac Newton1642-1727
First LawEvery object in a state of uniform motion
tends to remain in that state of motion unless an external force is applied to it.
p(t) m (t) mdx(t)
d tconstan t v
Second LawThe relationship between an object's mass m, its acceleration a, and the
applied force F
F md x t
dxm a
d
dxU x
2
2
( )( )
Potential Energy
Em v P
mkin 2 2
2 2
E U x F x dxpo t
x
( ) ( )0
Kinetic Energy
Continuum
Plum-pudding (1904)
Joseph J. Thomson 1856-1940
1906
His sonGeorge Paget Thomson
1856-1940Nobel Prize Physics 1937
Disovery of the Particlelike property of Electron
7 of his students won the Nobel Prize
Planetary Model (1909)
Ernest Rutherford 1871-1937
By emitting radiation, the electron should lose energy and
collapse into the nucleous
Atom is not stable !
1908
Hydrogen Atom
Niels Bohr1885-1962
r
me
mn
m
r
e
r0e
2 2
2
v
Electron on a Stable Orbit
Hydrogen Atom Equilibrium
Em
U xm e
r
m e
rto te e r e
v v v2 2 2
2
2 2
2 2 2( )
Electric Force
Centrifugal Force
Total Energy of the Electron
Ee
rto t 2
2Continuum
1922
Hydrogen SpectraPhotoelectric effect (1905)
Albert Einstein1879-1955
hv hv Epho ton kin elec tron 0
h = Planck Constantphoton = frequency of the incident photonh0 = = Work function = Energy needed
to remove an electron
1921
Wave-Particle DualityPhoton Case
Albert Einstein1879-1955
E pc m c ( ) ( )2 2 2
Special Theory of Relativity
E m c 2
Limit CaseSpeed of object is low
m 0Photon
E pc hv c v
ph
xx t
c
'
v
v1
2
2
tt
cx
c
'
v
v
2
2
21
1921
Wave-Particle DualityElectron Case
Louis de Broglie1892-1987Destructive
r n2
Electron Wave-Particle Duality p
h
Angular momentum l rp rm v
r
phn
r
n
r
2
rm nv
1929
Ultraviolet CatastropheBeginning of quantum theory (1900)
Max Planck1858-1947
Black-body Radiation
d d Density of Energy
8
4
T
Rayleigh-Jeans Law
8
15
hc ehc
T
ehc
T
Planck Distribution
Planck SuggestionE nhvosc
1918
Bohr Model (1913)
Niels Bohr1885-1962
m
r
Z e
r0e
2 2
2
v
Electron on a Stable Orbit
Equilibrium
m Z e
re v 2 2
22
Electric Force
Centrifugal Force
Hydrogen Radius
Ee
rto t 2
2Continuum
rm nv Quantification
rn
Z e m e
2 2
2
EZ e m
nto t 2 4
2 22 QuantumMechanic
1922
Wave Equation
Lieou, C. K. C. Eur. J. Phys. 2007, 28, N17-N19
x t
dx d t 0
dx d t vWave Function
Classical Mechanic
Non-absortive and Non-dispersive medium
x t
1
v
x t t x
Continuously Differentiable
2
2 2
2
2
1 1
x x x x t tv v
2
2 2
2
2
1
x tv
Wave Equation
Stationary Wave
Lieou, C. K. C. Eur. J. Phys. 2007, 28, N17-N19
Wave Equation
Variable Separation ( , ) ( ) ( )x t X x T t
Stationary Wave Function
2
2 2
2
2
1
x tv
( , ) s in 2 sin co s co s sinx tx
v tx
v tx
v t
2
22
2
Trigonomeric Identity
( , ) co s sinx tx
v t
22
sin ax e a ix
Trigonomeric Identity
( , ) ( )x t x e iv t 2
Wave Function
Stationary Wave
Erwin Schrödinger1887-1961
Lieou, C. K. C. Eur. J. Phys. 2007, 28, N17-N19
Wave Equation Wave Function
2
2 2
2
2
1
x tv
Stationary Wave Equation
( , ) ( )x t x e iv t 2
2
22
2
2
( , ) ( )x te
xiv t
x x
1 22
2
2
2
2v v
( , )( )
x t ivx e iv t
t
2
2
220
( )( )
xx
x
2
2
2
0
( )( )
x px
x
1933
Schrödinger Equation
Erwin Schrödinger1887-1961
Stationary Wave Equation
2
2
2
0
( )( )
x px
x E
m v P
mkin 2 2
2 2
Kinetic Energy
EP
mV xto t
2
2( )
Total Energy
P m E V x2 2 ( )
2
2 2
20
( ) ( ( ))
( )x m E V x
xx
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
1933
Free Electron
P = mv > 0P = mv < 0
x
P = momentumm = massv = speed (vector)
E xm
x
( )
( )
2 2
22
x
Schrödinger Equation
( , ) s inx t A ax
Stationary Wave Function
E xm
x
mA a x
( )
( )( )
2 2
2
22
2 2
x
EA a
m
A a h
m
2 2 2 2
22 8
Free Electron Wavefunction
( ) s inx A ax
Particle in a Box
P = mv > 0P = mv < 0
x
P = momentumm = massv = speed (vector)
L
V
0
2 Conditions
( )0 0 ( )L 0
Particle in a Box Wavefunction
( )x A e B eiax iax
A B
( ) s in ( )x A e e A i axiax iax 2
e e
iax
iax iax
2sin ( )
( ) s in ( )x A i aL 2 0
a 2
aL n n 1 2 3, , . . .
an
L
Particle in a Box
n = 1
n = 2
n = 3
LL/20
EA a h
m
2 2
28a
n
L
EA n h
m L
2 2
28
an
L
2
2 L
n
Example: -Carotene
nmXbondschemicalL 8.185.0 21
22 electrons
2
2
2
22
2
22
8
23
8
11
8
12
mL
h
mL
h
mL
hE
nmJs
mkgsm
h
cmL464
)10x626.6(23
)10x8.1)(10x109.9)(/10x998.2(8
23
834
293182
Absorption : blue-greenReflection : yellow-red = orange
E
n = 1
n = 11
n = 12
L0
11:
12:
nHOMO
nLUMO
Quantum Mechanics PostulatesPostulate 1
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
1. Associated with any particle moving in a conservative field of force is a wave function which determines everything that can be known about the system.
( , )x t single value
Quantum Mechanics PostulatesPostulate 2
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
2. With every physical observable q there is associated an operator Q, which when operating upon the wavefunction associated with a definite value of that observable will yield that value times the wavefunction.
E x H x ( ) ( )
Quantum Mechanics PostulatesPostulate 3
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
3. Any operator Q associated with a physically measurable property q will be Hermitian.
Pi
x
EP
mkin 2
2
a b a bH H* ( ) ( ) *
Quantum Mechanics PostulatesPostulate 4
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
4. The set of eigenfunctions of operator Q will form a complete set of linearly independent functions.
c c c ca a 1 1 2 2 3 3 . . .
E Ha a
Quantum Mechanics PostulatesPostulate 5
E xm
xV x x
( )
( )( ) ( )
2 2
22
x
Schrödinger Equation
5. For a system described by a given wavefunction, the expectation value of any property q can be found by performing the expectation value integral with respect to that wavefunction.
a b a bH H* ( ) ( ) *
Hermetian Operator
E H * ( )
Expectation Value
Quantum Mechanics
Erwin Schrödinger1887-1961
Paul Dirac1902-1984
« for the discovery of new productive forms of
atomic theory »
The Nobel Prize in Physics
1933
Werner Heisenberg1901-1976
1932
« for the creation of quantum mechanics… »
Molecular Orbital Theory of Conjugated SystemsHückel Molecular Orbitals
C-2 C-3 C-4
C-5 C-6
Erich Hückel1896-1980
Secular Equations
E H Schrödinger Equation
c a a
Postulate 4
b aa
ac H E 0 c H Ea aa
0
Determination of ca and E
b a abH H* ( )
b a abS *
Overlap Integral
c H Ea b a b aa
* * 0
c H S Ea ab aba
0
Secular Equations
c H S Ea ab aba
0Secular Equations
c H c H c H E c S c S c S1 11 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c H c H E c S c S c S1 2 1 2 2 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c H E c S c S c S1 3 1 2 3 2 3 3 3 1 3 1 2 3 2 3 3 3 0
We want to determine the value and sign of ca and E
Hückel TheoryPlanar/symmetric systems
c H c H c H E c S c S c S1 11 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c H c H E c S c S c S1 2 1 2 2 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c H E c S c S c S1 3 1 2 3 2 3 3 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
4 Approximations for planar and symmetrical polyenes
Erich Hückel1896-1980
Hückel TheoryPlanar/symmetric systems
c H c H c H E c S c S c S1 11 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c H c H E c S c S c S1 2 1 2 2 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c H E c S c S c S1 3 1 2 3 2 3 3 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
C-3
12
3
Mirror Plane of Molecule
x zy
Approximation 1
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 2 H Ha a a a * ( )
c H c H c H E c S c S c S1 11 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c H c H E c S c S c S1 2 1 2 2 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c H E c S c S c S1 3 1 2 3 2 3 3 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
= Coulomb Integral= Energy of bound electron
= Constant
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 2 H Ha a a a * ( )
c c H c H E c S c S c S1 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c c H E c S c S c S1 2 1 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c E c S c S c S1 3 1 2 3 2 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
= Coulomb Integral= Energy of bound electron
= Constant
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 3 H Ha b b a * ( ) a b 1 0:
a b 1 : constant
c c H c H E c S c S c S1 2 1 2 3 1 3 1 11 2 1 2 3 1 3 0
c H c c H E c S c S c S1 2 1 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c H c E c S c S c S1 3 1 2 3 2 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 3 H Ha b b a * ( ) a b 1 0:
a b 1 : constant
c c H E c S c S c S1 2 1 2 1 11 2 1 2 3 1 3 0
c H c c H E c S c S c S1 2 1 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c E c S c S c S2 3 2 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 4Kronecker Symbol
b a ab abS * Overlap Integral
a b ab : 0
a b ab : 1
c c H E c S c S c S1 2 1 2 1 11 2 1 2 3 1 3 0
c H c c H E c S c S c S1 2 1 2 3 2 3 1 2 1 2 2 2 3 2 3 0
c H c E c S c S c S2 3 2 3 1 3 1 2 3 2 3 3 3 0
Secular Equations
Hückel TheoryPlanar/symmetric systems C-3
12
3
Approximation 4
c c c E1 2 1 0
c c c c E1 2 3 2 0
c c c E2 3 3 0
Secular Equations
Kronecker Symbol
b a ab abS * Overlap Integral
a b ab : 0
a b ab : 1
Hückel TheoryPlanar/symmetric systems C-3
12
3
c c c E1 2 1 0
c c c c E1 2 3 2 0
c c c E2 3 3 0
Secular Equations
c E c1 2 0
c c E c1 2 3 0
c c E2 3 0
Secular Equations
E
Secular Determinant
0
E
E
0
0
Hückel TheoryPlanar/symmetric systems C-3
12
3
E
Secular Determinant
0
E
E
0
0
0 2,
E 2
E
E 2
Highest Energy
Lowest Energy3 Molecular Orbitals
is negative
Hückel TheoryPlanar/symmetric systems C-3
12
3
E 2
E
E 2
Highest Energy
Lowest Energy
E
Hückel TheoryPlanar/symmetric systems C-3
12
3
c E c1 2 0 c c E c1 2 3 0
c c E2 3 0
Secular Equations
E 2
E
E 2
Highest Energy
Lowest Energy
c c c1 2 3
1
20
1
2 ; ;
c c c12
22
32 1
Normalization
c c c1 2 3
1
2
1
2
1
2 ; ;
c c c1 2 3
1
2
1
2
1
2 ; ;
Hückel TheoryPlanar/symmetric systems C-3
12
3
E 2
E
E 2
Highest Energy
Lowest Energy
E 0.500
-0.707
0.500
0.707 -0.707
0.500 0.500
0.707
Secular EquationsExample: Butadiene
c H S Ea ab aba
0Secular Equations
c H c H c H c H E c S c S c S c S1 11 2 1 2 3 1 3 4 1 4 1 11 2 1 2 3 1 3 4 1 4 0
C-4
12
34
c H c H c H c H E c S c S c S c S1 2 1 2 2 2 3 2 3 4 2 4 1 2 1 2 2 2 3 2 3 4 2 4 0
c H c H c H c H E c S c S c S c S1 3 1 2 3 2 3 3 3 4 3 4 1 3 1 2 3 2 3 3 3 4 3 4 0
We want to determine the value and sign of ca and E
c H c H c H c H E c S c S c S c S1 4 1 2 4 2 3 4 3 4 4 4 1 4 1 2 4 2 3 4 3 4 4 4 0
Secular EquationsExample: Butadiene C-4
12
34
c c c E1 2 1 0
c c c c E1 2 3 2 0
c c c c E2 3 4 3 0
Secular Equations
c E c1 2 0
c c E c1 2 3 0
c c E c2 3 4 0
Secular Equations
c c c E3 4 4 0 c c E3 4 0
Secular EquationsExample: Butadiene C-4
12
34
c E c1 2 0
c c E c1 2 3 0
c c E c2 3 4 0
Secular Equations
c c E3 4 0
1 2 3 4
Symmetrical
c c1 4 c c2 3
Anti-Symmetrical
c c1 4 c c2 3
Secular EquationsExample: Butadiene C-4
12
34
c E c1 2 0
c c E c1 2 3 0
c c E c2 3 4 0
Secular Equations
c c E3 4 0
1 2 3 4
Symmetrical
c E c1 2 0
c c E c1 2 2 0
E 1 6 2.
E 0 6 2.
Secular EquationsExample: Butadiene C-4
12
34
c E c1 2 0
c c E c1 2 3 0
c c E c2 3 4 0
Secular Equations
c c E3 4 0
1 2 3 4
Anti-Symmetrical
c E c1 2 0
c c E c1 2 2 0
E 1 6 2.
E 0 6 2.
Secular EquationsExample: Butadiene C-4
12
34
Highest Energy
Lowest Energy
E
E 1 6 2.
E 0 6 2.
E 0 6 2.
E 1 6 2.
Secular EquationsExample: Butadiene C-4
12
34
Secular Equations
c c c c12
22
32
42 1
Normalization
c c c c1 2 3 40 3 7 1 0 6 0 0 0 6 0 0 0 3 7 1 . ; . ; . ; .
c E c1 2 0 c c E c1 2 3 0 c c E c2 3 4 0
c c E3 4 0
Highest Energy
Lowest EnergyE 1 6 2.E 0 6 2.E 0 6 2.E 1 6 2.
c c c c1 2 3 40 6 0 0 0 3 7 1 0 3 7 1 0 6 0 0 . ; . ; . ; .
c c c c1 2 3 40 6 0 0 0 3 7 1 0 3 7 1 0 6 0 0 . ; . ; . ; .
c c c c1 2 3 40 3 7 1 0 6 0 0 0 6 0 0 0 3 7 1 . ; . ; . ; .
Secular EquationsExample: Butadiene C-4
12
34
Highest Energy
Lowest Energy
E
0.371
-0.600 0.600
-0.371
0.600
-0.371 -0.371
0.600
0.600
0.371 -0.371
-0.600
0.371
0.600 0.600
0.371E 1 6 2.
E 0 6 2.
E 0 6 2.
E 1 6 2.
Sinusoidal Lobe Alternance
Ethene
Allyle
Butadiene
« Electron in a Box »
Diels-Alder Cycloaddition
Diels-Alder CycloadditionConservation of Orbital Symmetry
Robert B. Woodward1917-1979
Roald Hoffman1937-
Elias J. Corey1928-
?
1965 1981
1990
Diels-Alder CycloadditionSymmetry of Orbitals
plan symmetry
C2 rotation symmetry
plan symmetry
C2 rotation symmetry
Robert B. Woodward1917-1979
Roald Hoffman1937-
Ethylene
Butadiene
1965
1981
Diels-Alder CycloadditionSymmetry of Orbitals
E
SA
AS
SA
AS
Butadiene
SA
AS
Ethylene
, C2
Diels-Alder ReactionReaction Path: Plan Symmetry
Cyclobutene + Ethelyne Cyclohexene
Only a plan symmetry along the reaction path
Diels-Alder ReactionCorrelation Diagrams
LUMO dienophile
HOMO diene
A
A
S
S
A
S
A
S
A
S
A
S
Diels-Alder ReactionCorrelation Diagrams
LUMO dienophile
HOMO diene
A
A
S
S
A
S
A
S
A
S
A
S
[2+2] CycloadditionCorrelation Diagrams
Ethylene + Ethelyne Cyclobutane
Two plan symmetry along the reaction path
[2+2] CycloadditionCorrelation Diagrams
SA
SA
[2+2] CycloadditionCorrelation Diagrams
SA
SS
SA
SS
SA
AS
AA
AS
SA
AA
Diels-Alder CycloadditionFrontier Molecular Orbitals
E
Butadiene EthyleneFMO
Fukui Acc. Chem. Res. 1971, 4, 57.
HOMO
LUMO
HOMO
LUMO Kenichi Fukui1918-1988
1981
Spino et al. Angew. Chem., Int. Ed. 1998, 37, 3262.
Conclusions
• Schrödinger equation can be easily obtained from classical mechanics through routine mathematical procedures
• Application of Hückel Model to polyenes provides an approximate but reliable quantification of energies and orbital coefficients
• Conservation orbital symmetry and FMO are useful in predicting the course of concerted reactions