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^+` because

Options

A. 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

Answer

B

Explanation

`{:(" Species" ,N_2,N_2^+,O_2,O_2^+),("Bond Order",3,2.5,2,2.5):}`