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The order of magnitude of ionic radii of ions ${Na}^{+} {, Mg}^{2 +}, {Al}^{3 +}$ and ${Si}^{4 +}$ is :

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a

\begin{aligned} {Na}^{+} < {Mg}^{2 +} < {Al}^{3 +} < {Si}^{4 +} \end{aligned}

b

\begin{array}{r} {Mg}^{2 +} > {Na}^{+} > {Al}^{3 +} > {Si}^{4 +} \end{array}

c

\begin{array}{r} {Al}^{3 +} > {Na}^{+} > {Si}^{4 +} > {Mg}^{2 +} \end{array}

d

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

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detailed solution

Correct option is D

The order of magnitude of ionic radii of ions ${Na}^{+} > {Mg}^{2 +} > {Al}^{3 +} > {Si}^{4 +}$ . All are isoelectronic, but ${Si}^{4 +}$ has the highest nuclear charge per electron. As a result, ${Na}^{+}$ has the smallest size and nuclear charge per electron.

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