Identify the correct order of ionic radii of | vedclass

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(C) The ionic radii of isoelectronic species decrease as the nuclear charge increases.For the given ions,$K^{+}$ ($18$ electrons),$Li^{+}$ ($2$ electr

Vedclass · Accepted Answer

$K^{+} > Li^{+} > Mg^{2+} > Al^{3+}$

Vedclass · Answer

(C) The ionic radii of isoelectronic species decrease as the nuclear charge increases.For the given ions,$K^{+}$ ($18$ electrons),$Li^{+}$ ($2$ electrons),$Mg^{2+}$ ($10$ electrons),and $Al^{3+}$ ($10$ electrons) have different electronic configurations.Comparing them based on their positions in the periodic table:$K^{+}$ is in the $4^{th}$ period,so it has the largest radius.$Li^{+}$ is in the $2^{nd}$ period.$Mg^{2+}$ and $Al^{3+}$ are isoelectronic ($10$ electrons each) and belong to the $3^{rd}$ period.For isoelectronic species,the ionic radius decreases as the atomic number $(Z)$ increases: $Mg^{2+}$ $(Z=12)$ > $Al^{3+}$ $(Z=13)$.Thus,the correct order is $K^{+} > Li^{+} > Mg^{2+} > Al^{3+}$.

Identify the correct order of ionic radii of the following ions.

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