Element with the following electronic configurations has highest ionisation energy?

We know that Ionization energy is the minimum energy required to remove the most loosely held electron from one mole of gaseous atoms to produce one mole of gaseous atoms and an atom is highly stable when its valence orbital is completely filled or half-filled.

In above options we can see that $\left[\mathrm{Ar}\right]3{ \mathrm{d}}^{10}4{ \mathrm{s}}^{2}4{\mathrm{p}}^3$ and  $\left[\mathrm{Ne}\right]3{ \mathrm{s}}^{2}3{\mathrm{p}}^3$ has half filled p-orbital.

But, In $\left[\mathrm{Ar}\right]3{ \mathrm{d}}^{10}4{ \mathrm{s}}^{2}4{\mathrm{p}}^3$ the presence of $3{\mathrm{d}}^{10}$ electrons offers shielding effect, as a result the $4{\mathrm{p}}^3$ electrons do not experience much nuclear charge and hence the electrons can be removed easily.

Hence, $\left[\mathrm{Ne}\right]3{ \mathrm{s}}^{2}3{\mathrm{p}}^3$is more stable.

Hence, option(A) is the answer.