The Delta Function Model of a Molecule *
The use of two delta functions allows us to see, to some extent,
how atoms bind into molecules.
Our potential is
with attractive delta functions at
This is a parity symmetric potential, so we can assume that our solutions will be parity eigenstates.
For even parity, our solution in the three regions is
Since the solution is designed to be symmetric about
, the boundary conditions at
are the same as at
The boundary conditions determine the constant
A little calculation gives
This is a transcendental equation, but we can limit the energy.
for the single delta function,
is larger than the one for the single
This means that
is more negative and there is more binding energy.
Basically, the electron doesn't have to be a localized with two atoms as it does with just one.
This allows the kinetic energy to be lower.
The figure below shows the two solutions plotted on the same graph as the potential.
Two Hydrogen atoms bind together to form a molecule with a separation of 0.74 Angstroms,
just larger than the Bohr radius of 0.53 Angstroms.
The binding energy (for the two electrons) is about 4.5 eV.
If we approximate the Coulomb potential by with a delta function, setting
our very naive calculation would give 1.48 eV for one electron, which is at least the right order of magnitude.
The odd parity solution has an energy that satisfies the equation
This energy is larger than for one delta function.
This state would be called anti-bonding.