Assertion (A): Na^{+} and Mg^{2+} ions are is | vedclass

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(B) $Na^{+}$ and $Mg^{2+}$ are isoelectronic species having $10 \ e^{-}$ each.However,$Mg^{2+}$ has $12$ protons while $Na^{+}$ has $11$ protons.Due t

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Both $(A)$ and $(R)$ are correct and $(R)$ is correct explanation of $(A)$.

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(B) $Na^{+}$ and $Mg^{2+}$ are isoelectronic species having $10 \ e^{-}$ each.However,$Mg^{2+}$ has $12$ protons while $Na^{+}$ has $11$ protons.Due to a higher number of protons in $Mg^{2+}$,the effective nuclear charge $(Z_{eff})$ is greater for $Mg^{2+}$ than for $Na^{+}$.Since ionic radius is inversely proportional to the effective nuclear charge,the ionic radius of $Na^{+}$ is greater than that of $Mg^{2+}$.Therefore,both $(A)$ and $(R)$ are correct,and $(R)$ is the correct explanation of $(A)$.

Assertion $(A)$: $Na^{+}$ and $Mg^{2+}$ ions are isoelectronic but the ionic radius of $Na^{+}$ is greater than that of $Mg^{2+}$.
Reason $(R)$: The effective nuclear charge of $Na^{+}$ ion is less than that of $Mg^{2+}$ ion.

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Assertion $(A)$: $Na^{+}$ and $Mg^{2+}$ ions are isoelectronic but the ionic radius of $Na^{+}$ is greater than that of $Mg^{2+}$.Reason $(R)$: The effective nuclear charge of $Na^{+}$ ion is less than that of $Mg^{2+}$ ion.