Which of the following molecules is theoretically not possible?

Which of the following species has no $p\pi - p\pi$ bond but has a bond order equal to that of $O_2$?

For the ozone molecule,consider the following statements:
$(A)$ It is a linear molecule with a bond angle of $180^{\circ}$.
$(B)$ It is an angular molecule with a bond angle of $117^{\circ}$.
$(C)$ The bond lengths of both $O-O$ bonds are the same.
$(D)$ With respect to oxygen,it is thermodynamically more stable.
The correct options are:

Observe the following structure. The formal charges on the atoms $1, 2, 3$ respectively are:

The number of molecules from the following which contain only two lone pairs of electrons is $........$.
$H_2O, N_2, CO, XeF_4, NH_3, NO, CO_2, F_2$

The incorrect statement among the following is/are: