Using molelcular orbital theory, compare the bond energy and magnetic character of `O_(2)^(+)` and `O_(2)^(-)` species.

Explanation

According to molecular orbital theory electronic configurations of `O_(2)^(+)` and `O_(2)^(-)` species are as follows:
`O_(2)^(+) : (sigma1s)^(2)(sigma^(star)1s^(2))(sigma2s^(2))(sigma2p_(z))^(2)(pi2p_(x)^(2), pi2p_(y)^(2))(pi^(star)2p_(x)^(1))`
Bond order of `O_(2)^(+) = (10-5)/(2) = (5/2)=2.5`
`O_(2)^(-):(sigma1s)^(2)(sigma^(star)1s^(2))(sigma^(star)1s^(2))(sigma2s^(2))(sigma^(star)2s^(2))(sigma2p_(z))^(2)(pi2p_(x)^(2),pi2p_(y)^(2))(pi^(star)2p_(x)^(2), pi^(star)2p_(y)^(1))`
Bond order of `O_(2)^(-) = (10-7)/(2) = 3/2=1.5`
Higher bond order of `O_(2)^(+)` shows that it is more stable than `O_(2)^(-)`. Both the species have unpaired electrons. So, both are paramagnetic in nature.