Given below are two statements:Statement I: T | vedclass

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(A) Statement $I$: The electronic configuration of $Na^{+}$ is $1s^{2} 2s^{2} 2p^{6}$, which is a stable noble gas configuration. Removing the second

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Both statement $I$ and statement $II$ are true

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(A) Statement $I$: The electronic configuration of $Na^{+}$ is $1s^{2} 2s^{2} 2p^{6}$, which is a stable noble gas configuration. Removing the second electron from $Na^{+}$ requires a very high amount of energy. In contrast, $Mg^{+}$ has the configuration $1s^{2} 2s^{2} 2p^{6} 3s^{1}$, and removing the second electron results in a stable $Mg^{2+}$ ion $(1s^{2} 2s^{2} 2p^{6})$. Thus, the second ionisation enthalpy of $Na$ is much higher than that of $Mg$. Statement $I$ is true.Statement $II$: Both $O^{2-}$ and $F^{-}$ are isoelectronic species with $10$ electrons. The ionic radius of isoelectronic species decreases as the nuclear charge $(Z)$ increases. Since the atomic number of $O$ $(Z=8)$ is less than that of $F$ $(Z=9)$, the ionic radius of $O^{2-}$ is larger than that of $F^{-}$. Statement $II$ is true.

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