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Question
Use molecular orbital theory to explain why the Be2 molecule does not exist.
Solution
The electronic configuration of Beryllium is `1"s"^2 2"s"^2`.
The molecular orbital electronic configuration for Be2 molecule can be written as:
`sigma_(1"s")^2 sigma_(1"s")^(•2) sigma_(2"s")^2 sigma_(2"s")^(•2)`
Hence, the bond order for Be2 is `1/2 ("N"_"b" - "N"_"a")`
Where,
Nb = Number of electrons in bonding orbitals
Na = Number of electrons in anti-bonding orbitals
∴Bond order of Be2 = `1/2(4-4) =0`
A negative or zero bond order means that the molecule is unstable. Hence, Be2molecule does not exist.
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