Using MOT, compare `O_2^(+) and O_2^(-)` species and choose the incorrect option.

Options

A. Both `O_2^(+) and O_2^(-)` are paramagnetic.
B. `O_2^+` is dimagnetic while `O_2^(-)` is paramagnetic.
C. `O_2^(-)` is less stable
D. `O_2^(+)` have higher bond order than `O_2^(-)`

Answer

B

Explanation

Molecular orbital configuration of `O_2^(+)`
`sigma 1S^2 sigma^(**) 1S^2 sigma 2S^2 sigma^(**)S^2 sigma 2P_z^2 = pi 2P_y^2= pi 2 P_y^2 pi^(**) 2 P_x^2 pi 2P_x^2=pi wP_y^2 pi^(**) 2P_y^1`
Bond order ` =1//2 (10 -5) = 2.5`
Number of unpaired electrons = 1, Hence paramagnetic,
Molecular orbital configuration of `O_2^(-)`
`sigma1S^2 sigma^(**)1S^2 sigma2S^2 sigma^(**)2S^2 sigma2P_z^2 = pi 2P_y^2 pi^(**)2P_x^2 = pi 2P_y^1`
Bond order `=1//2 (10-7) = 1.5`
Number of unpaired electron = 1, Hence paramagnetic.
Both `O_2^(+) and O_2^(-)` are paramagnetic
`O_2^(+)` have higher bond order than `O_2^(-)`.
`O_2^(-)` is less stable