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Question

According to molecular orbital theory, which of the following will not be a viable molecule?


A
H2
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B
H22
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C
He2+2
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D
He+2
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Solution

The correct option is B $$H_2^{2-}$$


Electronic configuration of $$H_2 {^{2-}} = (\sigma 1s^2)(\sigma ^*1 s^2)$$

Bond order of $$H_2^{2\circleddash} = \dfrac{N_b-N_a}{2} = \dfrac{2-2}{2} = 0$$.

If a bond order of zero is obtained, that means that the molecule is too unstable and so it will not exist.

Hence, $$H_2^{2\circleddash}$$ does not exit, due to zero bond order.

Option B is correct. 

802292_845730_ans_f345a718d64f4a1196febbaa9af6771c.png

Chemistry

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