Identify the correct statements from the following.
$(I)$ $SnCl_2$ is ionic,but $SnCl_4$ is covalent in nature.
$(II)$ All linear diatomic molecules have zero dipole moment.
$(III)$ Both $NO$ and $O_2$ are paramagnetic.

Determine the correct $(T)$ and incorrect $(F)$ statements for the permanganate ion $(MnO_4^-)$:
$(a)$ $MnO_4^-$ contains $\sigma$ bonds.
$(b)$ $MnO_4^-$ contains $\pi$ bonds.
$(c)$ $MnO_4^-$ contains both $\sigma$ and $\pi$ bonds.
$(d)$ $MnO_4^-$ is paramagnetic.

Select the incorrect statement about $N_2F_4$ and $N_2H_4$ :
$(I)$ In $N_2F_4$,$d$-orbitals are contracted by electronegative fluorine atoms,but $d$-orbital contraction is not possible by $H$ atoms in $N_2H_4$.
$(II)$ The $N-N$ bond energy in $N_2F_4$ is more than the $N-N$ bond energy in $N_2H_4$.
$(III)$ The $N-N$ bond length in $N_2F_4$ is more than that in $N_2H_4$.
$(IV)$ The $N-N$ bond length in $N_2F_4$ is less than that in $N_2H_4$.
Choose the correct code:

Which molecule does not exist?

The correct formal charges on oxygen atoms numbered $2$, $1$ and $3$ respectively are:

The pairs among $A = [SO_3^{2-}, CO_3^{2-}]$, $B = [O_2^{2-}, F_2]$, $C = [CN^-, CO]$, $D = [NH_3, H_3O^+]$ and $E = [MnO_4^{2-}, CrO_4^{2-}]$ that do not have similar Lewis dot structures are: