The bond dissociation enthalpy of `N_(2)` is higher than that of `N_(2)^(+)` but the bond dissociation enthalpy of `O_(2)^(+)` is higher than that of `O_(2)`. Explain.

Explanation

`N_(2):K K(sigma_(2s))^(2)(sigma_(2s)^(**))^(2)(pi_(2p_(x)))^(2)(pi_(2p_(y)))^(2)`
`N_(2)^(+):K K(sigma_(2s))^(2)(sigma_(2s)^(**))^(2)(pi_(2p_(x)))^(2)(pi_(2p_(y)))^(2)(sigma_(2p_(z)))^(1)`
`Q_(2): K K(sigma_(2s))^(2)(sigma_(2s)^(**))^(2)(sigma_(2p_(z)))^(2)(pi_(2p_(x)))^(2)(pi_(2p_(y)))^(2)(pi_(2p_(x))^(**))^(1)(pi_(2p_(y))^(**))^(1)`
`Q_(2)^(+):K K(sigma_(2s))^(2)(sigma_(2s)^(**))^(2)(sigma_(2p_(z))^(**))^(2)(sigma_(2p_(z)))^(2)(pi_(2p_(x)))^(2)(pi_(2p_(y)))^(2)(pi_(2p_(x))^(**))^(1)`

Greater the value of bond order, higher will be the value of bond dissociation enthalpy. hence, the bond dissociation enthalpy of `N_(2)` is higher than that of `N_(2)^(+)` but the bond dissociation enthalphy of `O_(2)` is lower than that of `O_(2)^(+)`.