The smallest among the following ions is

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(D) The size of an ionic species decreases with an increase in the effective nuclear charge for isoelectronic species or across a period. Among the gi

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$Al^{3+}$

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(D) The size of an ionic species decreases with an increase in the effective nuclear charge for isoelectronic species or across a period. Among the given ions,$Na^{+}$,$Mg^{2+}$,and $Al^{3+}$ are isoelectronic (all have $10$ electrons). For isoelectronic species,the ionic radius decreases as the nuclear charge $(Z)$ increases. Since the atomic number of $Al$ is $13$,$Mg$ is $12$,and $Na$ is $11$,the nuclear charge is highest for $Al^{3+}$. Therefore,$Al^{3+}$ is the smallest among the given ions.

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