(a) How does bond energy vary from `N_(2)^(+)` and `N_(2)^(-)` and why ?
(b) On the basis of the molecular orbital theory, what is the similarly between :
`(i)F_(2),O_(2)^(2-)" "(ii)CO,N_(2),NO^(+).`
(c ) Like CO why its analong SiO is not so stable ?

Explanation

(a) Both `N_(2)^(+) and N_(2)^(-)` have same bond order (2.5). Hence both have the same energy.
(b) (i) Both `F_(2),O_(2)^(2-)` are isoelectronic. They have the same molecular orbital configuration as well as the bond ordre.
(ii) CO, `N_(2),NO^(+)` have the same bond order (3.0).
(c ) In Co, thereis multiple bonding present. `(Coverset(larr)(=)O":").` As result, it is quite stable. On the other hand, silicon (Si) atom due to is large size linked to oxygen by single bond only (Si-O). Therefore, it is not so stable.