c20 JWBS043-Rogers September 13, 2010 11:29 Printer Name: Yet to Come
320 QUANTUM MOLECULAR MODELING
There are many possible values ofR, each of which leads to a unique value of the
electronic energyEelectronic. AlthoughRis constant for any single calculation, the
total energy of the system is a function ofR:
Etotal=Eelectronic+
1
R
This means that a curve ofEtotalvs.Rcan be drawn. From this point on, we shall
drop the subscripts onE, taking the nature ofE, electronic or total, to be clear from
context.
By theLCAOapproximation, a molecular orbital can be expressed as aLinear
Combination of two hydrogenicAtomicOrbitals:
ψ=N 1 e−rA±N 2 e−rB
The atomic orbitals arebasis functionswhich define a vector space that includes the
molecular orbital. The LCAO basis set is not complete, so the molecular orbital we
obtain will not be correct. If functionsN 1 e−rAandN 2 e−rBare normalized hydrogen
1 sorbitals, we call them 1sAand 1sBand the approximate molecular orbital for H+ 2
isψH+ 2 = 1 sA± 1 sB. Physically, one basis function represents hydrogen atom A at
some distance from proton B, while the other basis function represents hydrogen
atom B at some distance from proton A. Neither basis function alone recognizes the
simultaneous interaction of the electron with both nuclei. It is this interaction we seek
because it brings about the chemical bond.
The energy of the positive combinationψH+ 2 = 1 sA+ 1 sBis
E=
∫
ψHˆψdτ=N^2
∫
( 1 sA+ 1 sB)
[
−^12 ∇^2 −
1
rA
−
1
rB
]
( 1 sA+ 1 sB)dτ
whereN^2 is the product of the two normalization constants and the integration is
taken over the entire spaceτ. If we expand and simplify according to the symmetry
of the problem, the energy gives three functions often denotedJ,K, andS:
J=
(
1 +
1
R
)
e−^2 R
K=
(
S
R
− 1 +R
)
e−^2 R
and
S=
(
1 +R+
R^2
3
)
e−R