Which of the following has the smallest size?

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(D) All the given ions ($Na^{+}$,$Mg^{2+}$,$Al^{3+}$,$Si^{4+}$) are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the i

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$Si^{4+}$

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(D) All the given ions ($Na^{+}$,$Mg^{2+}$,$Al^{3+}$,$Si^{4+}$) are isoelectronic,meaning they all have $10$ electrons.For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.The atomic numbers are: $Na$ $(Z=11)$,$Mg$ $(Z=12)$,$Al$ $(Z=13)$,and $Si$ $(Z=14)$.Since $Si^{4+}$ has the highest nuclear charge $(Z=14)$,it exerts the strongest attraction on the electrons,resulting in the smallest ionic size.Therefore,the correct option is $(D)$.

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