ch121a atomic level simulations of materials and molecules
DESCRIPTION
Ch121a Atomic Level Simulations of Materials and Molecules. BI 115 Hours: 2:30-3:30 Monday and Wednesday Lecture or Lab: Friday 2-3pm (+3-4pm). Lecture 2, March 30, 2011 QM-2: DFT. William A. Goddard III, [email protected] - PowerPoint PPT PresentationTRANSCRIPT
1Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Ch121a Atomic Level Simulations of Materials and Molecules
William A. Goddard III, [email protected] and Mary Ferkel Professor of Chemistry,
Materials Science, and Applied Physics, California Institute of Technology
BI 115Hours: 2:30-3:30 Monday and Wednesday
Lecture or Lab: Friday 2-3pm (+3-4pm)
Teaching Assistants Wei-Guang Liu, Fan Lu, Jose Mendozq
Lecture 2, March 30, 2011QM-2: DFT
2Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Last Time
3Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Consider the product wavefunction
Ψ(1,2) = ψa(1) ψb(2)
And the Hamiltonian for H2 molecule
H(1,2) = h(1) + h(2) +1/r12 + 1/R
In the details slides next, we derive
E = < Ψ(1,2)| H(1,2)|Ψ(1,2)>/ <Ψ(1,2)|Ψ(1,2)>
E = haa + hbb + Jab + 1/R
where haa =<a|h|a>, hbb =<b|h|b> are just the 1 electron energies
Jab ≡ <ψa(1)ψb(2) |1/r12 |ψa(1)ψb(2)>=ʃ d3r1[ψa(1)]2 ʃd3r2[ψb(2)]2/r12 =
= ʃ [ψa(1)]2 Jb (1) = <ψa(1)| Jb (1)|ψa(1)>
Where Jb (1) = ʃ [ψb(2)]2/r12 is the Coulomb potential at 1 due to the density distribution [ψb(2)]2
Energy for 2-electron product wavefunction
Jab is the Coulomb repulsion between densities a=[ψa(1)]2 and b
4Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The energy for an antisymmetrized product, Aψaψb
The total energy is that of the product wavefunction plus the new terms arising from exchange term which is negative with 4 partsEex=-< ψaψb|h(1)|ψb ψa >-< ψaψb|h(2)|ψb ψa >-< ψaψb|1/R|ψb ψa > - < ψaψb|1/r12|ψb ψa >The first 3 terms lead to < ψa|h(1)|ψb><ψbψa >+ <ψa|ψb><ψb|h(2)|ψa
>+ <ψa|ψb><ψb|ψa>/R But <ψb|ψa>=0Thus all are zeroThus the only nonzero term is the 4th term:-Kab=- < ψaψb|1/r12|ψb ψa > which is called the exchange energy (or the 2-electron exchange) since it arises from the exchange term due to the antisymmetrizer.Summarizing, the energy of the Aψaψb wavefunction for H2 isE = haa + hbb + (Jab –Kab) + 1/R
One new term from the antisymmetrizer
5Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The general case of 2M electronsFor the general case the HF closed shell wavefunction
Ψ(1,2….2M) = A[(φ1)(φ1)(φ2)(φ2)… )(φM)(φM)] leads to
HHFφk = k φk where we solve for k=1,M occupied orbitals
HHF = h + Σj=1,M [2Jj-Kj]
This is the same as the Hamiltonian for a one electron system moving in the average electrostatic and exchange potential, 2Jj-Kj due to the other N-1 = 2M-1 electrons
Problem: sum over 2Jj leads to 2M Coulomb terms, not 2M-1
This is because we added the self Coulomb and exchange terms
But (2Jk-Kk) φk = (Jk) φk so that these self terms cancel.
The HF equations describe each electron moving in the average potential due to all the other electrons.
6Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The Matrix HF equations
The HF equations are actually quite complicated because Kj is an integral operator, Kj φk(1) = φj(1) ʃ d3r2 [φj(2) φk(2)/r12]The practical solution involves expanding the orbitals in terms of a basis set consisting of atomic-like orbitals,
φk(1) = Σ C Xwhere the basis functions, {XMBF} are chosen as atomic like functions on the various centers
As a result the HF equations HHFφk = k φk
Reduce to a set of Matrix equations
ΣjmHjmCmk = ΣjmSjmCmkk
This is still complicated since the Hjm operator includes exchange terms
7Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
New stuff
8Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
HF wavefunctions
Good distances, geometries, vibrational levels
But
breaking bonds is described extremely poorly
energies of virtual orbitals not good description of excitation energies
cost scales as 4th power of the size of the system.
9Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Electron correlation
In fact when the electrons are close (rij small), the electrons correlate their motions to avoid a large electrostatic repulsion, 1/rij
Thus the error in the HF equation is called electron correlation
For He atom
E = - 2.8477 h0 assuming a hydrogenic orbital exp(-r)E = -2.86xx h0 exact HF (TA look up the energy)
E = -2.9037 h0 exact
Thus the elecgtron correlation energy for He atom is 0.04xx h0 = 1.x eV = 24.x kcal/mol.
Thus HF accounts for 98.6% of the total energy
10Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Configuration interaction
Consider a set of N-electron wavefunctions: {i; i=1,2, ..M} where < i|j> = ij {=1 if i=j and 0 if i ≠j)
Write approx = i=1 to M) Ci i
Then E = < approx|H|approx>/< approx|approx>
E= < i Ci i |H| i Cj j >/ < i Ci i | i Cj j >How choose optimum Ci?Require E=0 for all Ci get
j <i |H| Cj j > - Ei< i | Cj j > = 0 ,which we write asHCi = SCiEi in matrix notation, ie ΣjkHjkCki = ΣjkSjkCkiEi
where Hjk = <j|H|k > and Sjk = < j|k > and Ci is a column vector for the ith eigenstate
11Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Configuration interaction upper bound theorm
Consider the M solutions of the CI equationsHCi = SCiEi ordered as i=1 lowest to i=M highest
Then the exact ground state energy of the systemSatisfies Eexact ≤ E1
Also the exact first excited state of the system satisfiesE1st excited ≤ E2 etcThis is called the Hylleraas-Unheim-McDonald Theorem
12Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Alternative to Hartree-Fork, Density Functional Theory
Walter Kohn’s dream:
replace the 3N electronic degrees of freedom needed to define the N-electron wavefunction Ψ(1,2,…N) with
just the 3 degrees of freedom for the electron density (x,y,z).
It is not obvious that this would be possible but
P. Hohenberg and W. Kohn Phys. Rev. B 76, 6062 (1964). Showed that there exists some functional of the density that gives the exact energy of the system
Kohn did not specify the nature or form of this functional, but research over the last 46 years has provided increasingly accurate approximations to it.
Walter Kohn (1923-)Walter Kohn (1923-)Nobel Prize Chemistry 1998
13Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The Hohenberg-Kohn theorem
The Hohenberg-Kohn theorem states that if N interacting electrons move in an external potential, Vext(1..N), the ground-state electron density (xyz)=(r) minimizes the functional
E[= F[+ ʃ (r) Vext(r) d3rwhere F[is a universal functional of and the minimum value of the functional, E, is E0, the exact ground-state electronic energy.
Here we take Vext(1..N) = i=1,..N A=1..Z [-ZA/rAi], which is the electron-nuclear attraction part of our Hamiltonian. HK do NOT tell us what the form of this universal functional, only of its existence
14Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Proof of the Hohenberg-Kohn theorem
Mel Levy provided a particularly simple proof of Hohenberg-Kohn theorem {M. Levy, Proc. Nat. Acad. Sci. 76, 6062 (1979)}. Define the functional O as O[(r)] = min <Ψ|O|Ψ>
|Ψ>(r)
where we consider all wavefunctions Ψ that lead to the same density, (r), and select the one leading to the lowest expectation value for <Ψ|O|Ψ>.F[ is defined as F[(r)] = min <Ψ|F|Ψ>
|Ψ>(r)
where F = i [- ½ i2] + ½ i≠k [1/rik].
Thus the usual Hamiltonian is H = F + Vext
Now consider a trial function Ψapp that leads to the density (r) and which minimizes <Ψ|F|Ψ>
Then E[= F[+ ʃ (r) Vext(r) d3r = <Ψ|F +Vext|Ψ> = <Ψ|H|Ψ> Thus E[≥ E0 the exact ground state energy.
15Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The Kohn-Sham equations
Walter Kohn and Lou J. Sham. Phys. Rev. 140, A1133 (1965).
Provided a practical methodology to calculate DFT wavefunctions
They partitioned the functional E[] into parts
E[] = KE0 + ½ ʃʃd3r1 d3r2 [)/r12 + ʃd3r rVext() + Exc[r
Where
KE0 = i <φi| [- ½ i2 | φi> is the KE of a non-interacting electron
gas having density rThis is NOT the KE of the real system.
The 2nd term is the total electrostatic energy for the density rNote that this includes the self interaction of an electron with itself.
The 3rd term is the total electron-nuclear attraction term
The 4th term contains all the unknown aspects of the Density Functional
16Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Solving the Kohn-Sham equationsRequiring that ʃ d3r (r) = N the total number of electrons and applying the variational principle leads to
[(r)] [E[] – ʃ d3r (r) ] = 0
where the Lagrange multiplier = E[]/ = the chemical potential
Here the notation [(r)] means a functional derivative inside the integral.
To calculate the ground state wavefunction we solve
HKS φi = [- ½ i2 + Veff(r)] φi = i φi
self consistently with (r) = i=1,N <φi|φi>
where Veff (r) = Vext (r) + J(r) + Vxc(r) and Vxc(r) = EXC[]/
Thus HKS looks quite analogous to HHF
17Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
The Local Density Approximation (LDA)
We approximate Exc[ras
ExcLDA[rʃ d3r XC(rr
where XC(r is derived from Quantum Monte Carlo calculations for the uniform electron gas {DM Ceperley and BJ Alder, Phys.Rev.Lett. 45, 566 (1980)}
It is argued that LDA is accurate for simple metals and simple semiconductors, where it generally gives good lattice parameters
It is clearly very poor for molecular complexes (dominated by London attraction), and hydrogen bonding
18Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Generalized gradient approximations
The errors in LDA derive from the assumption that the density varies very slowly with distance.
This is clearly very bad near the nuclei and the error will depend on the interatomic distances
As the basis of improving over LDA a powerful approach has been to consider the scaled Hamiltonian
cxxc EEE drρ(r),...ρ(r)ρ(r),εE xx
19Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
LDA exchange
3
1
xLDAx rρAρε
Here we say that in LDA each electron interacts with all N electrons but should be N-1. The exchange term cancels this extra term. If density is uniform then error is proportional to 1/N. since electron density is = N/V
20Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Generalized gradient approximations
cxxc EEE
drρ(r),...ρ(r)ρ(r),εE xx
sFερρ,ε LDAx
GGAx
3
4
3
12 ρπ24
ρs
Becke 88
X3LYP
PBEPW91
s
F(s) GGA functionals
2
11
232
1188B
sasinhsa1
sasasinhsa1sF
d
521
1
2s100432
1191PW
sasasinhsa1
seaasasinhsa1sF
2
21Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
adiabatic connection formalism
The adiabatic connection formalism provides a rigorous way to define Exc.
It assumes an adiabatic path between the fictitious non-interacting KS system (λ = 0) and the physical system (λ = 1) while holding the electron density r fixed at its physical λ = 1 value for all λ of a family of partially interacting N-electron systems:
1
,0xc xcE U d is the exchange-correlation energy at intermediate coupling strength λ. The only problem is that the exact integrand is unknown.
Becke, A.D. J. Chem. Phys. (1993), 98, 5648-5652.Langreth, D.C. and Perdew, J. P. Phys. Rev. (1977), B 15, 2884-2902.Gunnarsson, O. and Lundqvist, B. Phys. Rev. (1976), B 13, 4274-4298.Kurth, S. and Perdew, J. P. Phys. Rev. (1999), B 59, 10461-10468.Becke, A.D. J. Chem. Phys. (1993), 98, 1372-1377.Perdew, J.P. Ernzerhof, M. and Burke, K. J. Chem. Phys. (1996), 105, 9982-9985.Mori-Sanchez, P., Cohen, A.J. and Yang, W.T. J. Chem. Phys. (2006), 124, 091102-1-4.
22Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Becke half and half functional
assume a linear model ,xcU a b
take , 0
exactxc xU E the exact exchange of the KS orbitals
approximate , 1 , 1
LDAxc xcU U
partition LDA LDA LDAxc x cE E E
set ;exact LDA exactx xc xa E b E E ;exact LDA exact
x xc xa E b E E
Get half-and-half functional 1 1
2 2exact LDA LDA
xc x x cE E E E
Becke, A.D. J. Chem. Phys. (1993), 98, 1372-1377
23Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Becke 3 parameter functional
B31 2 3
LDA exact LDA GGA GGAxc xc x x x cE E c E E c E c E
Empirically modify half-and-half
where GGAxE is the gradient-containing correction terms to the LDA exchange
GGAcE is the gradient-containing correction to the LDA correlation,
1 2 3, ,c c c are constants fitted against selected experimental thermochemical data.
The success of B3LYP in achieving high accuracy demonstrates that errors of for covalent bonding arise principally from the λ 0 or exchange limit, making it important to introduce some portion of exact exchange
DFTxcE
Becke, A.D. J. Chem. Phys. (1993), 98, 5648-5652.Becke, A.D. J. Chem. Phys. (1993), 98, 1372-1377.Perdew, J.P. Ernzerhof, M. and Burke, K. J. Chem. Phys. (1996), 105, 9982-9985.Mori-Sanchez, P., Cohen, A.J. and Yang, W.T. J. Chem. Phys. (2006), 124, 091102-1-4.
24Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
LDA: Slater exchange Vosko-Wilk-Nusair correlation, etc
GGA: Exchange: B88, PW91, PBE, OPTX, HCTH, etc Correlations: LYP, P86, PW91, PBE, HCTH, etc
Hybrid GGA: B3LYP, B3PW91, B3P86, PBE0, B97-1, B97-2, B98, O3LYP, etc
Meta-GGA: VSXC, PKZB, TPSS, etc
Hybrid meta-GGA: HCTHh, TPSSh, BMK, etc
Some popular DFT functionals
25Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Truhlar’s DFT functionals
MPW3LYP, X1B95, MPW1B95, PW6B95, TPSS1KCIS, PBE1KCIS, MPW1KCIS,
BB1K, MPW1K, XB1K, MPWB1K, PWB6K, MPWKCIS1K
MPWLYP1w,PBE1w,PBELYP1w, TPSSLYP1w
G96HLYP, MPWLYP1M , MOHLYP
M05, M05-2xM06, M06-2x, M06-l, M06-HF
Hybrid meta-GGAFPBE + VSXC
26Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
XYG3 approach to include London Dispersion in DFTGörling-Levy coupling-constant perturbation expansion
1
,0xc xcE U d Take initial slope as the 2nd order correlation energy:
, 2
, 0
0
2xc GLxc c
UU E
where
22
2ˆˆˆ1
4
i xi j eeGLc
ij ii j i
fE
where is the electron-electron repulsion operator, is the local exchange operator, and is the Fock-like, non-local exchange operator.
ˆee ˆx
f̂
,xcU a b Substitute into with22 GL
cb E ;exact LDA exactx xc xa E b E E or
Combine both approaches (2 choices for b) 21 2
GL DFT exactc xc xb b E b E E
R5 21 2 3 4
LDA exact LDA GGA PT LDA GGAxc xc x x x c c cE E c E E c E c E E c E
a double hybrid DFT that mixes some exact exchange into while also introducing a certain portion of into
DFTxE2PT
cEDFTcE
contains the double-excitation parts of 2PTcE
22
2ˆˆˆ1
4
i xi j eeGLc
ij ii j i
fE
This is a fifth-rung functional (R5) using information from both occupied and virtual KS orbitals. In principle can now describe dispersion
Sum over virtual orbtials
27Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Final form of XYG3 DFT
R5 21 2 3 4
LDA exact LDA GGA PT LDA GGAxc xc x x x c c cE E c E E c E c E E c E
we adopt the LYP correlation functional but constrain c4 = (1 – c3) to exclude compensation from the LDA correlation term. This constraint is not necessary, but it eliminates one fitting parameter.Determine the final three parameters {c1, c2, c3} empirically by fitting only to the thermochemical experimental data in the G3/99 set of 223 molecules:
Get {c1 = 0.8033, c2 = 0.2107, c3 = 0.3211} and c4 = (1 – c3) = 0.6789
Use 6-311+G(3df,2p) basis set
XYG3 leads to mean absolute deviation (MAD) =1.81 kcal/mol, B3LYP: MAD = 4.74 kcal/mol. M06: MAD = 4.17 kcal/mol M06-2x: MAD = 2.93 kcal/mol M06-L: MAD = 5.82 kcal/mol .G3 ab initio (with one empirical parameter): MAD = 1.05 G2 ab initio (with one empirical parameter): MAD = 1.88 kcal/molbut G2 and G3 involve far higher computational cost.
28Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Thermochemical accuracy with size
G3/99 set has 223 molecules:
G2-1: 56 molecules having up to 3 heavy atoms,
G2-2: 92 additional molecules up to 6 heavy atoms
G3-3: 75 additional molecules up to 10 heavy atoms.
B3LYP: MAD = 2.12 kcal/mol (G2-1), 3.69 (G2-2), and 8.97 (G3-3) leads to errors that increase dramatically with size
B2PLYP MAD = 1.85 kcal/mol (G2-1), 3.70 (G2-2) and 7.83 (G3-3) does not improve over B3LYP
M06-L MAD = 3.76 kcal/mol (G2-1), 5.71 (G2-2) and 7.50 (G3-3).
M06-2x MAD = 1.89 kcal/mol (G2-1), 3.22 (G2-2), and 3.36 (G3-3).
XYG3, MAD = 1.52 kcal/mol (G2-1), 1.79 (G2-2), and 2.06 (G3-3), leading to the best description for larger molecules.
29Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Accuracy (kcal/mol) of various QM methods for predicting standard enthalpies of formation
Functional MAD Max(+) Max(-)
DFT
XYG3 a 1.81 16.67 (SF6) -6.28 (BCl3)
M06-2x a 2.93 20.77 (O3) -17.39 (P4)
M06 a 4.17 11.25 (O3) -25.89 (C2F6)
B2PLYP a 4.63 20.37(n-octane) -8.01(C2F4)
B3LYP a 4.74 19.22 (SF6) -8.03 (BeH)
M06-L a 5.82 14.75 (PF5) -27.13 (C2Cl4)
BLYP b 9.49 41.0 (C8H18) -28.1 (NO2)
PBE b 22.22 10.8 (Si2H6) -79.7 (azulene)
LDA b 121.85 0.4 (Li2) -347.5 (azulene)
Ab initio
HFa 211.48 582.72(n-octane) -0.46 (BeH)
MP2a 10.93 29.21(Si(CH3)4) -48.34 (C2F6)
QCISD(T) c 15.22 42.78(n-octane) -1.44 (Na2)
G2(1 empirical parm)
1.88 7.2 (SiF4) -9.4 (C2F6)
G3(1 empirical parm)
1.05 7.1 (PF5) -4.9 (C2F4)
30Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
-5.00
0.00
5.00
10.00
15.00
20.00
25.00
30.00
-2.00 -1.50 -1.00 -0.50 0.00 0.50 1.00 1.50 2.00 2.50
Reaction coordinate
Ene
rgy
(kca
l/mol
)
HF
HF_PT2
XYG3
CCSD(T)
B3LYP
BLYP
SVWN
HF
HF_PT2 SVWNB3LYP
BLYP
XYG3CCSD(T)
SVWN
H + CH4 H2 + CH3
Reaction Coordinate: R(CH)-R(HH) (in Å)
Ene
rgy
(kca
l/mol
)Comparison of QM methods for reaction surface of
H + CH4 H2 + CH3
31Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Reaction barrier
heights
19 hydrogen transfer (HT) reactions, 6 heavy-atom transfer (HAT) reactions, 8 nucleophilic substitution (NS) reactions and 5 unimolecular and association (UM) reactions.
Functional All (76) HT38 HAT12 NS16 UM10
DFT
XYG3 1.02 0.75 1.38 1.42 0.98
M06-2x a 1.20 1.13 1.61 1.22 0.92
B2PLYP 1.94 1.81 3.06 2.16 0.73
M06 a 2.13 2.00 3.38 1.78 1.69
M06-La 3.88 4.16 5.93 3.58 1.86
B3LYP 4.28 4.23 8.49 3.25 2.02
BLYP a 8.23 7.52 14.66 8.40 3.51
PBEa 8.71 9.32 14.93 6.97 3.35
LDAb 14.88 17.72 23.38 8.50 5.90
Ab initio
HFb 11.28 13.66 16.87 6.67 3.82
MP2 b 4.57 4.14 11.76 0.74 5.44
QCISD(T) b 1.10 1.24 1.21 1.08 0.53
Zhao and Truhlar compiled benchmarks of accurate barrier heights in 2004 includes forward and reverse barrier heights for
Note: no reaction barrier heights used in fitting the 3 parameters in XYG3)
32Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
(A)
-15.00
-10.00
-5.00
0.00
5.00
10.00
15.00
20.00
25.00
30.00
3.0 4.0 5.0 6.0
Intermolecular distance
Ene
rgy
(kca
l/mol
)
BLYP
B3LYP
XYG3
CCSD(T)
SVWN
HF_PT2
(C)
-12.00
-9.00
-6.00
-3.00
0.00
Ec_VWN
Ec_B3LYP
Ec_LYP
Ec_XYG3
Ec_CCSD(T)
Ec_PT2
(B)
-5.00
0.00
5.00
10.00
15.00
20.00
25.00
30.00
3.0 4.0 5.0 6.0
Ex_B
Ex_B3LYP
Ex_XYG3
Ex_HF
Ex_S
HF
HF_PT2
B3LYP
BLYP
CCSD(T)
LDA (SVWN)
A. Total Energy (kcal/mol)
Distance (A)
XYG3
B. Exchange Energy (kcal/mol)
C. Correlation Energy (kcal/mol)
B
S
B3LYP
XYG3
PT2
B3LYP
LYP CCSD(T)
VWN
XYG3
Distance (A)
Conclusion: XYG3 provides excellent accuracy for London dispersion, as good as CCSD(T)
Test for London
Dispersion
33Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Accuracy of QM methods for noncovalent interactions.
Functional Total HB6/04 CT7/04 DI6/04 WI7/05 PPS5/05
DFT
M06-2x b 0.30 0.45 0.36 0.25 0.17 0.26
XYG3 a 0.32 0.38 0.64 0.19 0.12 0.25
M06 b 0.43 0.26 1.11 0.26 0.20 0.21
M06-L b 0.58 0.21 1.80 0.32 0.19 0.17
B2PLYP 0.75 0.35 0.75 0.30 0.12 2.68
B3LYP 0.97 0.60 0.71 0.78 0.31 2.95
PBE c 1.17 0.45 2.95 0.46 0.13 1.86
BLYP c 1.48 1.18 1.67 1.00 0.45 3.58
LDA c 3.12 4.64 6.78 2.93 0.30 0.35
Ab initio
HF 2.08 2.25 3.61 2.17 0.29 2.11
MP2c 0.64 0.99 0.47 0.29 0.08 1.69
QCISD(T) c 0.57 0.90 0.62 0.47 0.07 0.95
HB: 6 hydrogen bond complexes,
CT 7 charge-transfer complexes
DI: 6 dipole interaction complexes, WI:7 weak interaction complexes,
PPS: 5 stacking complexes.
WI and PPS dominated by London dispersion.
Note: no noncovalent complexes used in fitting the 3 parameters in XYG3)
34Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Problem
1
,0xc xcE U d Take initial slope as the 2nd order correlation energy:
, 2
, 0
0
2xc GLxc c
UU E
where
22
2ˆˆˆ1
4
i xi j eeGLc
ij ii j i
fE
where is the electron-electron repulsion operator, is the local exchange operator, and is the Fock-like, non-local exchange operator.
ˆee ˆx
f̂
Sum over virtual orbtials
XYG3 approach to include London Dispersion in DFTGörling-Levy coupling-constant perturbation expansion
EGL2 involves double excitations to virtuals, scales as N5 with size
MP2 has same critical step
Yousung Jung (KAIST) has figured out how to get linear scaling for MP2
XYGJ-OS and XYGJ-OS
35Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
XYGJ-OS method most accurate DFT(including London Dispersion) at modest cost
R5 21 2 3 4
LDA exact LDA GGA PT LDA GGAxc xc x x x c c cE E c E E c E c E E c E
a double hybrid DFT that mixes some exact exchange into while also introducing a certain portion of into
DFTxE2PT
cEDFTcE
contains the double-excitation parts of 2PTcE
22
2ˆˆˆ1
4
i xi j eeGLc
ij ii j i
fE
c4 = (1 – c3) 3 parameters
Ying Zhang , Xin Xu, Goddard; P. Natl. Acad. Sci. 106 (13) 4963-4968 (2009)
Use Görling-Levy coupling-constant perturbation expansion
XYG3 most accurate DFT, but costs too high for large systems
Yousung Jung figured out how to dramatically reduce the costs while retaining the accuracy
XYGJ-OS
Yousung Jung
36Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
0.0
40.0
80.0
120.0
160.0
200.0
0 20 40 60 80 100 120
alkane chain length
CP
U (
hours
)
XYG4-LOS
XYG4-OS
B3LYP
XYG3
Timings XYGJ-OS and XYGJ-LOS for long alkanes
0.0
40.0
80.0
120.0
160.0
200.0
0 20 40 60 80 100 120
XYG4-LOS
XYG4-OS
B3LYP
XYG3
0.0
40.0
80.0
120.0
160.0
200.0
0 20 40 60 80 100 120
XYG4-LOS
XYG4-OS
B3LYP
XYG3
0.0
40.0
80.0
120.0
160.0
200.0
0 20 40 60 80 100 120
XYG4-LOS
XYG4-OS
B3LYP
XYG3
0.0
40.0
80.0
120.0
160.0
200.0
0 20 40 60 80 100 120
XYG4-LOS
XYG4-OS
B3LYP
XYG3
XYGJ-OS
XYGJ-LOS
XYGJ-LOS
XYGJ-OS
37Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Accuracy of Methods (Mean absolute deviations MAD, in eV) HOF IP EA PA BDE NHTBH HTBH NCIE All Time Methods
(223) (38) (25) (8) (92) (38) (38) (31) (493) C100H202 DFT methods SPL (LDA) 5.484 0.255 0.311 0.276 0.754 0.542 0.775 0.140 2.771 BLYP 0.412 0.200 0.105 0.080 0.292 0.376 0.337 0.063 0.322 PBE 0.987 0.161 0.102 0.072 0.177 0.371 0.413 0.052 0.562 TPSS 0.276 0.173 0.104 0.071 0.245 0.391 0.344 0.049 0.250 B3LYP 0.206 0.162 0.106 0.061 0.226 0.202 0.192 0.041 0.187 2.8 PBE0 0.300 0.165 0.128 0.057 0.155 0.154 0.193 0.031 0.213 M06-2X 0.127 0.130 0.103 0.092 0.069 0.056 0.055 0.013 0.096 XYG3 0.078 0.057 0.080 0.070 0.068 0.056 0.033 0.014 0.065 200.0 XYGJ-OS 0.072 0.055 0.084 0.067 0.033 0.049 0.038 0.015 0.056 7.8 MC3BB 0.165 0.120 0.175 0.046 0.111 0.062 0.036 0.023 0.123 B2PLYP 0.201 0.109 0.090 0.067 0.124 0.090 0.078 0.023 0.143 Wavefunction based methods HF 9.171 1.005 1.148 0.133 0.104 0.397 0.582 0.098 4.387 MP2 0.474 0.163 0.166 0.084 0.363 0.249 0.166 0.028 0.338 G2 0.082 0.042 0.057 0.058 0.078 0.042 0.054 0.025 0.068 G3 0.046 0.055 0.049 0.046 0.047 0.042 0.054 0.025 0.046
HOF = heat of formation; IP = ionization potential, EA = electron affinity, PA = proton affinity, BDE = bond dissociation energy, NHTBH, HTBH = barrier heights for reactions, NCIE = the binding in molecular clusters
38Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Comparison of speeds
NCIE All Time (31) (493) C100H202 C100H100
0.140 2.771 0.063 0.322 0.052 0.562 0.049 0.250 0.041 0.187 2.8 12.3 0.031 0.213 0.013 0.096 0.014 0.065 200.0 81.4 0.015 0.056 7.8 46.4 0.023 0.123 0.023 0.143
0.098 4.387 0.028 0.338 0.025 0.068 0.025 0.046
HOF
Methods
(223) DFT methods SPL (LDA) 5.484 BLYP 0.412 PBE 0.987 TPSS 0.276 B3LYP 0.206 PBE0 0.300 M06-2X 0.127 XYG3 0.078 XYGJ-OS 0.072 MC3BB 0.165 B2PLYP 0.201 Wavefunction based methods HF 9.171 MP2 0.474 G2 0.082 G3 0.046
39Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
0. 01. 02. 03. 04. 05. 06. 07. 08. 09. 0
10. 0
B3LY
P
M06
M06-
2x
M06-
L
B2PL
YP
XYG3
XYG4
-OS G2 G3
MAD
(kca
l/mo
l)
G2-1G2-2G3-3
Heats of formation (kcal/mol)
Large molecules
small molecules
40Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
0. 0
5. 0
10. 0
15. 0
20. 0
25. 0
B3LY
P
BLYP PBE
LDA HF MP2
QCIS
D(T)
XYG3
XYG4
-OS
MAD
(kca
l/mo
l)
HAT12NS16UM10HT38
Reaction barrier heights (kcal/mol)
Truhlar NHTBH38/04 set and HTBH38/04 set
41Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
0. 01. 0
2. 03. 0
4. 05. 0
6. 07. 0
8. 0
B3LY
P
BLYP PBE
LDA HF MP2
QCIS
D(T)
XYG3
XYG4
-OS
MAD
(kca
l/mo
l)
HB6CT7DI 6WI 7PPS5
Nonbonded interaction (kcal/mol)
Truhlar NCIE31/05 set
42Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
-5.00
0.00
5.00
10.00
15.00
20.00
25.00
30.00
-2.00 -1.50 -1.00 -0.50 0.00 0.50 1.00 1.50 2.00 2.50
Reaction coordinate
Ene
rgy
(kca
l/mol
)
HF
HF_PT2
XYG3
CCSD(T)
B3LYP
BLYP
SVWN
HF
HF_PT2 SVWNB3LYP
BLYP
XYG3CCSD(T)
SVWN
H + CH4 H2 + CH3
Reaction Coordinate: R(CH)-R(HH) (in Å)
Ene
rgy
(kca
l/mol
)Comparison of QM methods for reaction
surface of H + CH4 H2 + CH3
43Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
DFT-ℓg for accurate Dispersive Interactions for Full Periodic Table
Hyungjun Kim, Jeong-Mo Choi, William A. Goddard, III1Materials and Process Simulation Center, Caltech
2Center for Materials Simulations and Design, KAIST
44Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Current challenge in DFT calculation for energetic Current challenge in DFT calculation for energetic materialsmaterials
• Current implementations of DFT describe well strongly bound geometries and energies, but fail to describe the long range van der Waals (vdW) interactions.
• Get volumes ~ 10% too large• XYGJ-OS solves this problem but much slower than standard
methods• DFT-low gradient (DFT-lg) model accurate description of the long-
range1/R6 attraction of the London dispersion but at same cost as standard DFT
Nlg,
lg 6 6,
- ij
ij i j ij eij
CE
r dR
DFT D DFT dispE E E
C6 single parameter from QM-CCd =1Reik = Rei + Rek (UFF vdW radii)
45Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
PBE-lg for benzene dimerT-shaped Sandwich Parallel-displaced
PBE-lg parameters
Nlg,
lg 6 6,
- ij
ij i j ij eij
CE
r dR
Clg-CC=586.8, Clg-HH=31.14, Clg-HH=8.691
RC = 1.925 (UFF), RH = 1.44 (UFF)
First-Principles-Based Dispersion Augmented Density Functional Theory: From Molecules to Crystals’ Yi Liu and wag; J. Phys. Chem. Lett., 2010, 1 (17), pp 2550–2555
46Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
DFT-lg description for benzene
PBE-lg predicted the EOS of benzene crystal (orthorhombic phase I) in good agreement with corrected experimental EOS at 0 K (dashed line).Pressure at zero K geometry: PBE: 1.43 Gpa; PBE-lg: 0.11 GpaZero pressure volume change: PBE: 35.0%; PBE-lg: 2.8%Heat of sublimation at 0 K: Exp:11.295 kcal/mol; PBE: 0.913; PBE-lg: 6.762
47Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
DFT-lg description for graphite
graphite has AB stacking (also show AA eclipsed graphite)
Exper E 0.8, 1.0, 1.2
Exper c 6.556
PBE-lg
PBE
Bin
din
g e
ne
rgy
(kca
l/mol
)
c lattice constant (A)
48Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Universal PBE-ℓg MethodUFF, a Full Periodic Table Force Field for Molecular Mechanics and Molecular Dynamics Simulations; A. K. Rappé, C. J. Casewit, K. S. Colwell, W. A. Goddard III, and W. M. Skiff; J. Am. Chem. Soc. 114, 10024 (1992)
Derived C6/R6 parameters from scaled atomic polarizabilities for Z=1-103 (H-Lr) and derived Dvdw from combining atomic IP and C6
Universal PBE-lg: use same Re, C6, and De as UFF, add a single new parameter slg
49Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
blg Parameter Modifies Short-range Interactions
blg =1.0 blg =0.7
12-6 LJ potential (UFF parameter)
lg potentiallg potential
When blg =0.6966,ELJ(r=1.1R0) = Elg(r=1.1R0)
50Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Benzene Dimer
T-
shape
d
51Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Benzene Dimer
Sandwi
ch
52Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Benzene Dimer
Parallel-
displac
ed
53Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Parameter OptimizationImplemented in VASP 5.2.11
0.701
2
0.696
6
55Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Hydrocarbon Crystals
• Sublimation energy (kcal/mol/molecule)
• Cell volume (angstrom3/cell)
Molecules PBE PBE-ℓg Exp.
Benzene 1.051 12.808 11.295
Naphthalene 2.723 20.755 20.095
Anthracene 4.308 28.356 27.042
Molecules PBE PBE-ℓg Exp.
Benzene 511.81 452.09 461.11
Naphthalene 380.23 344.41 338.79
Anthracene 515.49 451.55 451.59
56Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Simple Molecular Crystals
• Sublimation energy (kcal/mol/molecule)
Average error: 3.86 (PBE) and 0.96 (PBE-ℓg) Maximal error: 7.10 (PBE) and 1.90 (PBE-ℓg)
Molecules PBE PBE-ℓg Exp.
F2 0.27 1.38 2.19
Cl2 2.05 5.76 7.17
Br2 5.91 10.39 11.07
I2 8.56 14.47 15.66
O2 0.13 1.50 2.07
N2 0.02 1.22 1.78
CO 0.11 1.54 2.08
CO2 1.99 4.37 6.27
57Lecture 1Ch121a-Goddard-L02 © copyright 2011 William A. Goddard III, all rights reserved\
Simple Molecular Crystals
• Cell volume (angstrom3/cell)
Molecules PBE PBE-ℓg Exp.
F2 126.47 126.32 128.24
Cl2 282.48 236.23 231.06
Br2 317.30 270.06 260.74
I2 409.03 345.13 325.03
O2 69.38 69.35 69.47
N2 180.04 179.89 179.91
CO 178.96 178.99 179.53
CO2 218.17 179.93 177.88
Lecture 1Lecture 2 60
Chem 121 - Applied Quantum ChemistryMethod:· Semi-Empirical, used for very big systems, or for rough approximations of geometry (extended Huckel theory, CNDO/INDO, AM1, MNDO)
· HF (Hartree Fock). Simplest Ab Initio method. Very cheap, fairly inaccurate· MP2 (Moeller-Plasset 2). Advanced version of HF. Usually not as cheap or as accurate as B3LYP, but can function as a complement.· CASSCF (Complete Active Space, Self Consisting Field). Advanced version of HF, incorporating excited states. Mainly used for jobs where photochemistry is important. Medium cost, Medium Accuracy. Quite complicated to run… · QCISD (Quadratic Configuration Interaction Singles Doubles). Very advanced version of HF. Very Expensive, Very accurate. Can only be used on systems smaller than 10 heavy atoms. · CCSD (Coupled Cluster Singles Doubles). Very much like QCISD. Density Functional Theory LDA (local density approximation) PW91, PBE· B3LYP (density functional theory). Cheap, Accurate.
Generally, B3LYP is the method of choice. If the system allows it, QCISD or CCSD can be used. HF and/or MP2 can be used to verify the B3LYP results.
Lecture 1Lecture 2 61
Chem 121 - Applied Quantum Chemistry
Basis Set: What mathematical expressions are used to describe orbitals. In general, the more advanced the mathematical expression, the more accurate the wavefunction, but also more expensive calculation.
· STO-3G - The ‘minimal basis set’. Not particularly accurate, but cheap and robust. · 3-21G - Smallest practical Basis Set. · 6-31G - More advanced, i.e. more functions for both core and valence. · 6-31G** - As above, but with ‘polarized functions’ added. Essentially makes the orbitals look more like ‘real’ ones. This is the standard basis set used, as it gives fairly good results with low cost. · 6-31++G - As above, but with ‘diffuse functions’ added. Makes the orbitals stretch out in space. Important to add if there is hydrogen bonding, pi-pi interactions, anions etc present. · 6-311++G** - As above, with even more functions added on… The more stuff, the more accurate… But also more expensive. Seldom used, as the increase in accuracy usually is very small, while the cost increases drastically. · Frozen Core: Basis sets used for higher row elements, where all the core electrons are treated as one big frozen chunk. Only the valence electrons are treated explicitly
Lecture 1Lecture 2 62
Chem 121 - Applied Quantum Chemistry
• Software packages– Jaguar
– GAMESS
– TurboMol
– Gaussian
– Spartan/Titan
– HyperChem
– ADF
Lecture 1Lecture 2 63
Chem 121 - Applied Quantum Chemistry
Running an actual calculation– Determine the starting geometry of the
molecule you wish to study
– Determine what you’d like to find out
– Determine what methods are suitable and/or affordable for the above calculation
– Prepare input file
– Run job
– Evaluate result
Lecture 1Lecture 2 64
Chem 121 - Applied Quantum Chemistry
Example: Good ol’ water
Starting geometry: water is bent, (~104º), a normal O-H bond is ~0.96 Å. For illustration, however, we’ll start with a pretty bad guess.
Simple Z-matrix:O1 H2 O1 1.00H3 O1 1.00 H2 110.00
1.00 Å 1.00 Å
110º
Lecture 1Lecture 2 65
Chem 121 - Applied Quantum Chemistry
What do we wish to find out?
How about the IR spectra?
What is a suitable method for this calculation? Well, any, really, since it is so small. But 99% of the time the answer to this question is “B3LYP/6-31G**” – a variant of density functional theory that is the main workhorse of applied quantum chemistry, with a standard basis set. Let’s go with that.
Lecture 1Lecture 2 66
Chem 121 - Applied Quantum Chemistry
Actual jaguar input:
&genigeopt=1ifreq=1dftname=b3lyp basis=6-31g**&&zmat
O1 H2 O1 0.95H3 O1 0.95 H2 120.00&
Lecture 1Lecture 2 67
Chem 121 - Applied Quantum Chemistry
Running time!
Jaguar calculates the wave function for the atomic coordinates we provided
From the wave function it determines the energy and the forces on the current geometry
Based on this, it determines in what direction it should move the atoms to reach a better geometry, i.e. a geometry with a lower energy
Lecture 1Lecture 2 68
Chem 121 - Applied Quantum Chemistry
1.00 Å 1.00 Å
110º
0.96 Å 0.96 Å
104º
Our horrible guess Target geometry
Think elastic springs: The bonds are too long, so there will be a force towards shorter bonds
Forces
Lecture 1Lecture 2 69
Chem 121 - Applied Quantum Chemistry
Optimization – minimization of the forces. When all forces are zero the energy will not change and we have the resting geometry
O1 H2 O1 0.9500000000 H3 O1 0.9500000000 H2 120.0000000000 SCF energy: -76.41367730925-- O1 H2 O1 0.9566666804 H3 O1 0.9566666820 H2 106.8986301461 SCF energy: -76.41937497895-- O1 H2 O1 0.9653619358 H3 O1 0.9653619375 H2 103.0739287925 SCF energy: -76.41969584939 -- O1 H2 O1 0.9653155294 H3 O1 0.9653155310 H2 103.6688074046 SCF energy: -76.41970381840--
Lecture 1Lecture 2 70
Chem 121 - Applied Quantum Chemistry
0.9653155294 Å
103.6688074046º
Computer accuracy
0.96 Å 0.96 Å
103.7º
“actual” accuracy
Accuracy
0.9653155294 Å
Accuracy is a relative concept
Lecture 1Lecture 2 71
Chem 121 - Applied Quantum Chemistry
frequencies 1666.01 3801.19 3912.97
No negative frequencies!
(Compare IR spectra for gas-phase water)
Lecture 1Lecture 2 72
Chem 121 - Applied Quantum Chemistry
Vibrational levels
“zero” level
Zero Point Energy (ZPE)
Zero Point Energies
Optimized energy is at the zero level, but in reality the molecule has a higher energy due to populated vibrational levels.
At 0 K, all molecules populate the lowest vibrational level, and so the difference between the “zero” level and the first vibrational level is the Zero Point Energy (ZPE)
From our calculation:The zero point energy (ZPE): 13.410 kcal/mol
Lecture 1Lecture 2 73
Chem 121 - Applied Quantum Chemistry
Thermodynamic data at higher temperatures
T = 298.15 K
U Cv S H G --------- --------- --------- --------- --------- trans. 0.889 2.981 34.609 1.481 -8.837 rot. 0.889 2.981 10.503 0.889 -2.243 vib. 0.002 0.041 0.006 0.002 0.000 elec. 0.000 0.000 0.000 0.000 0.000 total 1.779 6.003 45.117 2.371 -11.080
Most thermodynamic data can be computed with very good accuracy in the gas phase. Temperature dependant
Lecture 1Lecture 2 74
Chem 121 - Applied Quantum Chemistry
Transition states
ReactantProduct
Transition State (TS)
CH3Br + Cl- CH3Cl + Br- TS
Reaction coordinate
Line represents the reacting coordinate, in this case the forming C-Cl and breaking C-Br bonds
Stationary points: points on the surface where the derivative of the energy = 0
Lecture 1Lecture 2 75
Chem 121 - Applied Quantum Chemistry
CH3Br + Cl- CH3Cl + Br- TS
Reaction coordinate
Not a hill, but a mountain pass
Transition state = stationary point where all forces except one is at a minimum.
The exception is at its maximum
Lecture 1Lecture 2 76
Chem 121 - Applied Quantum Chemistry
ReactantProduct
TS
Derivative of the energy = 0
Second derivative: For a minimum > 0For a maximum < 0
So a TS should have a negative second derivative of the energy
Second derivative of the energy = force
Lecture 1Lecture 2 77
Chem 121 - Applied Quantum Chemistry
A transition state should have one negative (imaginary) frequency!!!
(and ONLY one)
Lecture 1Lecture 2 78
Chem 121 - Applied Quantum Chemistry
ReactantProduct
TS
Optimizing transition states:
Simultaneously optimize all modes (forces) towards their minimum, except the reacting mode
But for the computer to know which mode is the reacting mode, you must have one imaginary frequency in your starting point
Inflection points
Region with imaginary frequency
Must start with a good guess!!!
Lecture 1Lecture 2 79
Chem 121 - Applied Quantum Chemistry
Example:CH3Br + Cl- CH3Cl + Br-
What do we know about this reaction? It’s an SN2 reaction, so the Cl- must come in from the backside of the CH3Br. The C-Cl forms at the same time as the C-Br forms. The transition state should be five coordinate
Lecture 1Lecture 2 80
Chem 121 - Applied Quantum Chemistry
2.0 2.2Cl Br
H H
H
C
Initial guess: C-Cl = 2.0 Å, C-Br = 2.2 Å
Single point frequency on the above geometry: frequencies 98.64 99.58 109.11 310.66 1339.10 1348.64
frequencies 1349.46 1428.45 1428.73 2838.52 3017.70 3017.93
No negative frequencies! Bad initial guess
Lecture 1Lecture 2 81
Chem 121 - Applied Quantum Chemistry
Refinement :Initial guess most likely wrong because of erronous C-Br and C-Cl bond lengths
Let the computer optimize the five-coordinate structure
Frozen optimizations: Just like a normal optimization, but with one or more geometry parameters frozen
In this case, we optimize the structure with all the H-C-Cl angles frozen at 90º
Lecture 1Lecture 2 82
Chem 121 - Applied Quantum Chemistry
Result:
2.32 2.62Cl Br
C-Cl and C-Br bonds quite a bit longer in the new structure
Frequency calculation: frequencies -286.26 168.54 173.32 173.43 874.16 874.76 frequencies 976.23 1413.99 1414.65 3220.91 3420.84 3421.80
One negative frequency! Good initial guess
Lecture 1Lecture 2 83
Chem 121 - Applied Quantum Chemistry
Time for the actual optimization:
Jaguar follows the negative frequency towards the maximum
Geometry optimization 1: SCF Energy = -513.35042353681Geometry optimization 2: SCF Energy = -513.34995058422Geometry optimization 3: SCF Energy = -513.35001640704Geometry optimization 4: SCF Energy = -513.34970196448Geometry optimization 5: SCF Energy = -513.34968682825Geometry optimization 6: SCF Energy = -513.34968118535
Final energy higher than starting energy (although only 0.5 kcal/mol)
Frequency calculation frequencies -268.67 162.64 174.22 174.31 848.15 848.24 frequencies 960.97 1415.75 1415.96 3220.77 3420.80 3421.15
One negative frequency! We found a true transition state
Lecture 1Lecture 2 84
Chem 121 - Applied Quantum Chemistry
2.46 2.51Cl Br
Final geometry: C-Cl = 2.46 ÅC-Br = 2.51 Å Cl-C-H = 88.7ºBr-C-H = 91.3º
Structure not quite symmetric, the hydrogens are bending a little bit away from the Br.
Lecture 1Lecture 2 85
Chem 121 - Applied Quantum Chemistry
Solvation calculations
Explicit solvents: Calculations where solvent molecules are added as part of the calculation
Implicit solvents: Calculations where solvation effects are added as electrostatic interactions between the molecule and a virtual continuum of “solvent”.
Lecture 1Lecture 2 86
Chem 121 - Applied Quantum Chemistry
Reaction energetics and barrier heights
Collect the absolute energies of the reactants, products and transition states
CH3Br + Cl- TS CH3Cl + Br- -53.078938 + -460.248741 -513.349681 -500.108371 + -13.237607
Sum each term
CH3Br + Cl- TS CH3Cl + Br- -513.327679 -513.349681 -513.345978
Define reactants as “0”, and deduct the reactant energy from all terms
CH3Br + Cl- TS CH3Cl + Br- 0 -.022002 -.018299
Convert to kcal/mol (1 hartree = 627.51 kcal/mol)
Lecture 1Lecture 2 87
Chem 121 - Applied Quantum Chemistry
Reaction energetics and barrier heights
Convert to kcal/mol (1 hartree = 627.51 kcal/mol)
CH3Br + Cl- TS CH3Cl + Br- 0 -13.8 -11.5
But this doesn’t make sense
Lecture 1Lecture 2 88
Chem 121 - Applied Quantum Chemistry
Reaction energetics and barrier heights
CH3Br + Cl- TS CH3Cl + Br- 0 -13.8 -11.5
Solvation not included!
Include solvation corrections!
CH3Br + Cl- TS CH3Cl + Br- 0 9.2 -6.4