The decreasing order of size of the isoelectronic series $K^{+}$,$Ca^{2+}$,$Cl^{-}$,and $S^{2-}$ is:

Which of the following is the incorrect order of ionic/atomic radius?

In the isoelectronic species,the ionic radii in $\mathring{A}$ of $N^{3-}$,$O^{2-}$,and $F^{-}$ are respectively given by:

Given below are two statements: one is labelled as Assertion $A$ and the other is labelled as Reason $R$:
Assertion $A$: The ionic radii of $O^{2-}$ and $Mg^{2+}$ are same.
Reason $R$: Both $O^{2-}$ and $Mg^{2+}$ are isoelectronic species.
In the light of the above statements,choose the correct answer from the options given below:

The ionic radii of $F^{-}$ and $O^{2-}$ respectively are $1.33 \ \mathring{A}$ and $1.40 \ \mathring{A}$,while the covalent radius of $N$ is $0.74 \ \mathring{A}$. The correct statement for the ionic radius of $N^{3-}$ from the following is:

Which of the following is the correct increasing order of ionic radii for $N^{3-}$,$Na^+$,$F^-$,$O^{2-}$,and $Mg^{2+}$?