The order of increasing ionic radius of the f | vedclass

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Question

(A) To determine the ionic radius,we consider the number of shells and the effective nuclear charge.
$Al^{3+}$ has $2$ shells $(1s^2 2s^2 2p^6)$.
$M

Vedclass · Accepted Answer

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

Vedclass · Answer

(A) To determine the ionic radius,we consider the number of shells and the effective nuclear charge.
$Al^{3+}$ has $2$ shells $(1s^2 2s^2 2p^6)$.
$Mg^{2+}$ has $2$ shells $(1s^2 2s^2 2p^6)$.
$Li^{+}$ has $1$ shell $(1s^2)$.
$K^{+}$ has $3$ shells $(1s^2 2s^2 2p^6 3s^2 3p^6)$.
Comparing $Al^{3+}$ and $Mg^{2+}$ (isoelectronic,$10$ electrons): $Mg^{2+}$ has a lower nuclear charge $(Z=12)$ than $Al^{3+}$ $(Z=13)$,so $Mg^{2+} > Al^{3+}$.
Comparing all: $Al^{3+}$ $(0.54 \ \mathring{A})$ $< Mg^{2+}$ $(0.72 \ \mathring{A})$ $< Li^{+}$ $(0.76 \ \mathring{A})$ $< K^{+}$ $(1.38 \ \mathring{A})$.
Therefore,the correct order is $Al^{3+} < Mg^{2+} < Li^{+} < K^{+}$.

The order of increasing ionic radius of the following is:

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