Assertion (A): Mg^{2+} and Al^{3+} are isoele | vedclass

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Question

(A) Isoelectronic species are ions or atoms that have the same number of electrons. Both $Mg^{2+}$ and $Al^{3+}$ have $10$ electrons $(1s^2 2s^2 2p^6)

Vedclass · Accepted Answer

$A$ is true,$R$ is true and $R$ is the correct explanation for $A$.

Vedclass · Answer

(A) Isoelectronic species are ions or atoms that have the same number of electrons. Both $Mg^{2+}$ and $Al^{3+}$ have $10$ electrons $(1s^2 2s^2 2p^6)$.For isoelectronic species,the ionic radius decreases as the atomic number $(Z)$ increases because the effective nuclear charge $(Z_{eff})$ increases,pulling the electrons closer to the nucleus.$Z_{Mg} = 12$ and $Z_{Al} = 13$.Since $Z_{Al} > Z_{Mg}$,the effective nuclear charge on the outermost electrons in $Al^{3+}$ is greater than in $Mg^{2+}$.This higher $Z_{eff}$ results in a smaller ionic radius for $Al^{3+}$ compared to $Mg^{2+}$.Therefore,both $A$ and $R$ are true,and $R$ is the correct explanation for $A$.

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