The number of antibonding electron pairs in $O_{2}^{2-}$ molecular ion on the basis of molecular orbital theory is (Atomic number of $O$ is $8$)

The bond order in $NO$ is $2.5$ while that in $NO^{+}$ is $3$. Which of the following statements is true for these two species?

The sum of bond order values of $C_2$ and $O_2^{2+}$ is $x$,which is equal to the sum of bond order values of $a, b$ and $c$. What are $a, b$ and $c$?

Compare the relative stability of the following species and indicate their magnetic properties: $O_2$,$O_2^+$,$O_2^-$ (superoxide),$O_2^{2-}$ (peroxide).

Given below are two statements:
Statement $I$: $A$ hypothetical diatomic molecule with bond order zero is quite stable.
Statement $II$: As bond order increases,the bond length increases.
In the light of the above statements,choose the most appropriate answer from the options given below.

The paramagnetic nature of the oxygen molecule $(O_2)$ is best explained on the basis of: