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Use molecular orbital theory to explain why the `Be_2` molecule does not exist.

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The atomic no. (Z) or Be is 4. This means that 8 electrons are to be filled in the M.O of `Be_(2).` The configuration is :
`[sigma_(1s)]^(2)"["overset(**)sigma_(1s)"]"^(2)[sigma_(2s)]^(2)"["overset(**)sigma_(2s)"]"^(2) , B.O = 1/2[N_(b)-N_(a)]=1/2[4-4]=0`
As the bond order comes out to be zero, the molecule of `Be_(2)` does not exist.
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L.C.A.O. Principle is involved in the formation of the molecular orbitals according to molecular orbital theory. The energy of the bonding molecular orbital is less than that of the combining atomic orbitals while that of the antibonding molecular orbitals while that of the order (B.O.)=1/2(N_(b)-N_(a)) helps in predicting formation of molecules/molecular ions, bond dissociation energy, stability and bond length. Only the molecules or ions with positive B.O. can be formed. These will be diamagnetic if all molecular orbitals are dilled and paramagnetic if one of more are half filled. The atomic orbitals at the time of overlap must have the same symmetry as well. In the formation of N_(2)^(+) from N_(2), the electron is removed from a