According to molecular orbital theory, w...

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

`He_(2)^(2-)`

`He_(2)^(+)`

`H_(2)^(-)`

`H_(2)^(2-)`

Text Solution

Verified by Experts

The correct Answer is:

Both `H_(2)^(2+) (2e^(-)) : sigma 1 s^(2) , B.O. 2//2=1`
` H_(2)^(2+) (3e^(-)):sigma 1 s^(2) sigma^(**) 1 s^(1) , B.O. = (2-1)/(2) = 0.5`
`H_(2)^(-) (3e^(-)): sigma 1 s^(2) sigma ^(**)1 s^(1) , B.O. = (2-1)/(2) = 5.0`
`H_(2)^(2-) (4e^(-)): sigma 1 s^(2) sigma ^(**)1 s^(2) , B.O. = (2-2)/(2) = 0`
Thus , `H_(2)^(2-)` connot exist as it has zero bond order

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

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