Which of the following is the smallest cation | vedclass

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Question

(D) The ionic radii of isoelectronic species decrease as the nuclear charge increases. For the given ions: $Na^{+}$ ($10$ electrons,$Z=11$) $Mg^{+2}$

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$Al^{+3}$

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(D) The ionic radii of isoelectronic species decrease as the nuclear charge increases. For the given ions: $Na^{+}$ ($10$ electrons,$Z=11$) $Mg^{+2}$ ($10$ electrons,$Z=12$) $Al^{+3}$ ($10$ electrons,$Z=13$) $Ca^{+2}$ ($18$ electrons,$Z=20$) Comparing the isoelectronic series $(Na^{+}, Mg^{+2}, Al^{+3})$,the ionic radius decreases as the atomic number increases. Thus,$Al^{+3}$ is the smallest among the isoelectronic ions. $Ca^{+2}$ has a larger shell $(n=3)$ compared to the others $(n=2)$,making it significantly larger. The order of ionic radii is $Ca^{+2} > Na^{+} > Mg^{+2} > Al^{+3}$. Therefore,$Al^{+3}$ is the smallest cation.

Which of the following is the smallest cation?

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