Na^+,Mg^{2+},Al^{3+},and Si^{4+} are isoelect | vedclass

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(C) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.Since all these ions have $10$ electrons,the

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$Na^+ > Mg^{2+} > Al^{3+} > Si^{4+}$

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(C) For isoelectronic species,the ionic radius decreases as the nuclear charge (atomic number) increases.Since all these ions have $10$ electrons,the order of their ionic radii depends on the nuclear charge $(Z)$:$Z$ for $Na = 11$,$Mg = 12$,$Al = 13$,$Si = 14$.As the nuclear charge increases,the attraction between the nucleus and the electrons increases,causing the ionic radius to decrease.Therefore,the correct order is $Na^+ > Mg^{2+} > Al^{3+} > Si^{4+}$.

$Na^+$,$Mg^{2+}$,$Al^{3+}$,and $Si^{4+}$ are isoelectronic. What is the order of their ionic radii?

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