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Question

According to molecular orbital theory, which of the following will not exist?


A
H+2
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B
Be2
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C
B2
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D
C2
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Solution

The correct option is B $$Be_2$$
According to the molecular orbital theory elements which have bond order negative or $$0$$ will not exist.

Formula to calculate bond order $$=\dfrac { Number\ of \ electrons\ in\ BMO -\quad Number\ of\ electrons\ in\ ABMO }{ 2 }$$

where, $$BMO=$$ Bonding molecular orbital
            $$ABMO=$$ Antibonding molecular orbital

Molecular electronic configuation of $$Be_2=\sigma 1s^2 \sigma^* 1s^2 \sigma 2s^2 \sigma^* 2s^2$$

$$Be_2$$ has $$4$$ electrons in $$BMO$$ and $$4$$ in $$ABMO$$ so the bond order will come $$0$$.

So, the correct option is $$[B].$$

Chemistry

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