Correct order of bond length is:

Options

A. `N_(2) gt N_(2)^(+) gt N_(2)^(-) gt N_(2)^(2-)`
B. `N_(2)^(+)gtN_(2)^(-)gtN_(2)^(2-)gtN_(2)`
C. `N_(2)gtN_(2)^(-)=N_(2)^(+)gtN_(2)^(2-)`
D. `N_(2)^(-)gtN_(2)=N_(2)^(+)gtN_(2)^(2-)`

Answer

1

Explanation

Bond order is directly proportional to the bond energy.
Bond order of `N_(2)=3,N_(2)^(+),N_(2)^(-)=2.5" "N_(2)^(2-)=2`
But `N_(2)^(-)` has more electrons in antibonding `MO's` and thus `N_(2)^(+)` is more stable than `N_(2)^(-)` . So correct order of bond energy will be `N_(2) gtN_(2)^(+)gtN_(2)^(-)gtN_(2)^(2-)`
Therefore, `(1)` option is correct.