Which of the following has the smallest size?

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(D) The given ions $N^{3-}$,$O^{2-}$,$F^{-}$,and $Na^{+}$ are isoelectronic species,meaning they all have the same number of electrons ($10$ electrons

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$Na^{+}$

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(D) The given ions $N^{3-}$,$O^{2-}$,$F^{-}$,and $Na^{+}$ are isoelectronic species,meaning they all have the same number of electrons ($10$ electrons).For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number,$Z$) increases.The atomic numbers are: $N (Z=7)$,$O (Z=8)$,$F (Z=9)$,and $Na (Z=11)$.Since $Na^{+}$ has the highest nuclear charge $(Z=11)$,it exerts the strongest attraction on the electrons,resulting in the smallest ionic radius.

Similar Questions

Which of the following atoms or ions has the smallest size?

Assertion: The atomic radius of gallium is higher than that of aluminium.
Reason: The presence of additional $d$-electrons offers poor screening effect for the outer electrons from increased nuclear charge.

Identify the element having the smallest atomic radius from the following:

The order of increasing ionic radius of the following is:

The ionic radii of $Na^{+}$,$F^{-}$,$O^{2-}$,and $N^{3-}$ follow the order:

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