Considering a molecular orbital diagram for a diatomic molecule, which of the following bond orders would be impossible to find in a stable molecule? a)4 b)0 c)0.5 d) 0and 4 e) 1.5
Considering a molecular orbital diagram for a diatomic molecule, which of the following bond orders would be impossible to find in a stable molecule?
a)4
b)0
c)0.5
d) 0and 4
e) 1.5
Option d.
According to molecular orbital theory the bond order of a diatomic molecule is given by:
bond order will be 0 when number of electrons in bonding molecular orbital is equal to number of electrons in anti-bonding molecular orbital. This can only take place when the electronic configuration of both the atoms is of noble configuration. If it is so then there won't be any bond between them and they do not exist as a diatomic molecule.
For a diatomic molecule to have 4 as bond order the difference between bonding and anti bonding molecular orbitals should be 8. This cannot take place s and p block elements as the highest number of electrons that can accommodate are 6 in either orbitals.
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