If four different elements $A, B, C$ and $D$ have electronic configurations as $A = [Ne] 3s^2 3p^4$,$B = [Ne] 3s^2 3p^5$,$C = [Ar] 3d^{10} 4s^2 4p^4$ and $D = [Ar] 3d^{10} 4s^2 4p^5$,identify the element with the largest atomic radius.

Arrange $Na, Na^+, F, F^-$ in the decreasing order of their radii (size).

In $Cl_2$, the van der Waals radius is $180 \ pm$. What is the distance between the two atoms (in $pm$)?

Given below are two statements $ : $
Statement $(I) :$ The metallic radius of $Al$ is less than that of $Ga$.
Statement $(II) :$ The ionic radius of $Al^{3+}$ is less than that of $Ga^{3+}$.
In the light of the above statements, choose the most appropriate answer from the options given below $ : $

Given below are the pairs of group $13$ elements showing their relation in terms of atomic radius: $(B < Al)$, $(Al < Ga)$, $(Ga < In)$ and $(In < Tl)$. Identify the elements present in the incorrect pair and in that pair,find out the element $(X)$ that has a higher ionic radius $(M^{3+})$ than the other one. The atomic number of the element $(X)$ is:

The incorrect decreasing order of atomic radii is: