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(C) For lanthanides, the ionic radius decreases as the atomic number increases due to lanthanoid contraction. The correct order is $La^{3+} (103 	ext

Vedclass · Accepted Answer

$Tl^{+} > In^{+} > Sn^{2+} > Sb^{3+}$

Vedclass · Answer

(C) For lanthanides, the ionic radius decreases as the atomic number increases due to lanthanoid contraction. The correct order is $La^{3+} (103 	ext{ pm}) > Eu^{3+} (95 	ext{ pm}) > Gd^{3+} (94 	ext{ pm}) > Lu^{3+} (86 	ext{ pm})$. Thus, option $A$ is correct. For ions of the same element, ionic size decreases with an increase in positive charge: $V^{2+} > V^{3+} > V^{4+} > V^{5+}$. Thus, option $B$ is correct. For isoelectronic species, ionic size decreases as the nuclear charge increases. $K^{+} (Z=19)$, $Sc^{3+} (Z=21)$, $V^{5+} (Z=23)$, and $Mn^{7+} (Z=25)$ are isoelectronic $(18 	ext{ e}^-)$. The order $K^{+} > Sc^{3+} > V^{5+} > Mn^{7+}$ is correct. Thus, option $D$ is correct. In option $C$, $Tl^{+}$ $(150 	ext{ pm})$ and $In^{+}$ $(132 	ext{ pm})$ are larger than $Sn^{2+}$ $(118 	ext{ pm})$ and $Sb^{3+}$ $(76 	ext{ pm})$. However, the comparison between $Tl^{+}$ and $In^{+}$ is correct, but the overall sequence provided in the options needs to be evaluated. Given the standard trends, option $C$ is the incorrect order as $Tl^{+}$ and $In^{+}$ belong to different periods compared to $Sn^{2+}$ and $Sb^{3+}$.

Which of the following represents the incorrect order of ionic size?

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