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(D) For set $A$: $F^{-}, Na^{+}, Mg^{+2}$ are isoelectronic species with $10$ electrons. The ionic radius decreases as the nuclear charge $(Z)$ increa

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$Mg^{+2}, Zn, Cs^{+}, Be^{+2}$

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(D) For set $A$: $F^{-}, Na^{+}, Mg^{+2}$ are isoelectronic species with $10$ electrons. The ionic radius decreases as the nuclear charge $(Z)$ increases. Since $Z$ for $Mg$ is $12$,it has the smallest radius.For set $B$: In a period,atomic radius decreases from left to right due to increased effective nuclear charge. Thus,$Zn$ has the smallest radius among $Ni, Cu, Zn$.For set $C$: $N^{-3}$ has $10$ electrons,$Cs^{+}$ has $54$ electrons,and $H^{-}$ has $2$ electrons. $H^{-}$ has the smallest size due to the lowest number of shells and electrons.For set $D$: $Li$ $(Z=3)$,$He$ $(Z=2)$,$Be^{+2}$ $(Z=4)$. $Be^{+2}$ has the smallest radius due to the highest nuclear charge and loss of electrons.Therefore,the correct set is $Mg^{+2}, Zn, H^{-}, Be^{+2}$.

Ion	Radius $(pm)$
$Q^{a+}$	$53$
$X^{b+}$	$66$
$Y^{c+}$	$40$
$Z^{d+}$	$100$

From the given set of species,point out the species from each set having the least atomic radius.
$A. F^{-}, Na^{+}, Mg^{+2}$
$B. Ni, Cu, Zn$
$C. N^{-3}, Cs^{+}, H^{-}$
$D. Li, He, Be^{+2}$

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From the given set of species,point out the species from each set having the least atomic radius.$A. F^{-}, Na^{+}, Mg^{+2}$$B. Ni, Cu, Zn$$C. N^{-3}, Cs^{+}, H^{-}$$D. Li, He, Be^{+2}$