In the following the correct bond order sequence is :
$\mathrm{O}_{2}^{+}>\mathrm{O}_{2}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}^{2-}$
$\mathrm{O}_{2}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}^{2-}>\mathrm{O}_{2}^{+}$
$\mathrm{O}_{2}^{2-}>\mathrm{O}_{2}^{+}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}$
$\mathrm{O}_{2}^{+}>\mathrm{O}_{2}^{-}>\mathrm{O}_{2}^{2-}>\mathrm{O}_{2}$
During change of $O^2$ to $O_2^-$ ion, the electron adds on which one of the following orbitals?
Give difference : Bonding molecular orbital and antibonding molecular orbitals.
The correct order of bound orders of $C _{2}^{2-}, N _{2}^{2-}$ and $O _{2}^{2-}$ is, respectively.
From elementary molecular orbital theory we can give the electronic configuration of the singly positive nitrogen molecular ion $N_2^ + $ as
Select the $CORRECT$ statement if internuclear axis is $y-$ axis