Arrange $O_2$,$O_2[AsF_6]$,and $KO_2$ in the increasing order of bond length of the $O-O$ bond.

In $O_2^-$,$O_2$,and $O_2^{2-}$ molecular species,the total number of antibonding electrons respectively are

The total number of species from the following in which one unpaired electron is present,is . . . . . . $N_2, O_2, C_2^{-}, O_2^{-}, O_2^{2-}, H_2^{+}, CN^{-}, He_2^{+}$

The correct pair of species with $(A)$ the highest bond order and $(B)$ diamagnetic character is

$CN^-$ and $N_2$ are isoelectronic,but $N_2$ is chemically inert compared to $CN^-$. The reason is:

Select the correct set of statements regarding the molecular orbital theory of $O_2$:
$A$. Addition of an electron to $O_2$ decreases bond order.
$B$. Addition of an electron to $O_2$ increases bond order.
$C$. Removal of an electron from $O_2$ increases bond length.
$D$. Removal of an electron from $O_2$ decreases bond length.