Al^{3+} has a lower ionic radius than Mg^{2+} | vedclass

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(B) $Al^{3+}$ and $Mg^{2+}$ have an equal number of electrons ($10$ electrons) and are,therefore,isoelectronic.For isoelectronic species,the ionic rad

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$Al^{3+}$ has a higher nuclear charge than $Mg^{2+}$

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(B) $Al^{3+}$ and $Mg^{2+}$ have an equal number of electrons ($10$ electrons) and are,therefore,isoelectronic.For isoelectronic species,the ionic radius depends upon the effective nuclear charge $(Z_{eff})$.Ionic radius is inversely proportional to the effective nuclear charge.Since $Al$ $(Z=13)$ has a higher atomic number than $Mg$ $(Z=12)$,$Al^{3+}$ experiences a greater effective nuclear charge than $Mg^{2+}$.Consequently,the electrons in $Al^{3+}$ are pulled more strongly towards the nucleus,resulting in a smaller ionic radius.

$Al^{3+}$ has a lower ionic radius than $Mg^{2+}$ because

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