The experimental bond length for Carbon Monoxide is .1128 nm ( http://cccbdb.nist.gov/ ). Carbon Monoxide is a linear molecule. |
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Model of the Electrostatic potential of Carbon Monoxide.
The larger cloud around the molecule on the right
corresponds with a larger electron density. Which is to
be expected because chlorine has more valence electrons
than carbon.
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The HOMO
orbitals are the highest energy molecular orbitals
occupied by electrons. From the model, it is seen that
the HOMO orbitals in Carbon Monoxide are bonding. It is
expected that the orbitals would be bonding because the
bond connecting carbon and chlorine is a triple bond. In
a triple bond the two p- orbitals connect with one
another, which is shown by the model.
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The
LUMO orbitals are the lowest energy molecular orbitals
occupied by electrons. From the model, it is observed
that the LUMO orbitals are non-bonding, and this help
shows how the molecule will react.
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Energy
Level
|
Dipole
Moment (Debye) |
621-G
|
.399197 |
631-G
|
.267398 |
DZV
|
.191372 |
Level 1: s-orbital non-bonding |
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Level
2: s-orbital non-bonding |
|
Level
3: s-orbital bonding |
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Level
4: s-orbital and p-orbital Bonding |
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Level
5: 2 p-orbitals Form a Pi bond |
|
Level
6: 2 p-orbitals (different axis) Form a Pi bond |