The correct order of bond strength is :

Options

A. `O_(2)^(-) lt O_(2) lt O_(2)^(+)`
B. `O_(2)^(-) gt O_(2) gt O_(2)^(+)`
C. `O_(2)^(-) lt O_(2) gt _(2)^(+)`
D. `O_(2)^(-) gt O_(2) gt O_(2)^(+)`

Answer

a

Explanation

Oxygen molecule`(O_(2))`- Total number of electron ` = 16`Electron configuration :
`sigma 1s^(2) lt sigma**1s^(2) lt sigma2s^(2) lt sigma** 2s^(2) lt sigma2p_(x)^(2) lt pi 2p_(y)^(2) = pi 2p_(z)^(2) lt pi **2p_(z)^(1)`
Bond order `= (N_(b) - N_(a))/(2) = (10 - 6)/(2) = (4)/(2) = 2`
`O_(2)^(-)` ion Total number of electron `(16 - 1) = 15` Electronic configuration
`sigma 1s^(2) lt sigma**1s^(2) lt sigma2s^(2) lt sigma** 2s^(2) lt sigma2p_(x)^(2) lt pi 2p_(y)^(2) = pi 2p_(z)^(2) lt pi **2p_(y)^(1) lt pi **2p_(x)^(1)`
Bond order `= ((N_(b) - N_(a)))/(2) = (10 - 5)/(2) = (5)/(2) = 2(1)/(2)`
`O_(2)^(-)` (Super oxide ion )Total number of electron `= (16 + 1) = 17` Electronic configuration
`sigma 1s^(2) lt sigma**1s^(2) lt sigma2s^(2) lt sigma** 2s^(2) lt sigma2p_(x)^(2) lt pi 2p_(y)^(2) = pi 2p_(z)^(2) `
Bond order `= ((N_(b) - N_(a)))/(2) = (10 - 7)/(2) = (3)/(2) = (3)/(2) =1(1)/(2)`