The distribution of electrons among molecular orbitals is called the electronic configuration of the molecule which provides us the following very important informations about the molecule. (A)Stability of molecule : The molecule is stable if number of bonding moleculer orbital electrons `(N_b)` is greater than the number of antibonding molecular orbital electrons `(N_a)`. (B) Bond order : Bond order `=1/2(N_b-N_a)` A positive bond order means a stable molecule while a negative or zero bond order means an unstable molecule. ( C)Nature of the bond : Bond order 1,2 and 3 corresponds to single , double and triple bonds respectively. (D)Bond length: Bond length decreases as bond order increases. (E)Magnetic nature: Molecular orbitals in a molecule are doubly occupied , the substance is diamagnetic and if one or more molecular orbitals are singly occupied, it is paramagnetic. `N_2` has greater dissociation energy than `N_2^+` , where as `O_2` has a lower dissociation energy than `O_2^+` becauseA. Bond order is reduced when `O_2` is ionized to `O_2^(+)` and bond order is increased when `N_2` is ionized to `N_2^+`B. Bond order is increased when `O_2` is ionized to `O_2^(+)` and bond order is decreased when `N_2` is ionized to `N_2^+`C. Bond order is decreased when `O_2` is ionized to `O_2^(+)` and bond order is decreased when `N_2` is ionized to `N_2^+`D. None of these