A) \[{{K}^{+}}\]
B) \[S{{r}^{2+}}\]
C) \[Ar\]
D) \[K\]
Correct Answer: B
Solution :
The radius of the cation is always smaller than that of its parent atom. Thus, size of \[{{K}^{+}}\] ion is smaller than \[K\] atom. As \[{{K}^{+}}\] and \[Ar\] are isoelectronic species and among the isoelectronic species cation has smaller radius than neutral atom. Thus, \[{{K}^{+}}\] has smaller ionic radii than Ar. Moreover, among \[{{K}^{+}}\] and \[S{{r}^{2+}}\] ion, although \[S{{r}^{2+}}\] has gas configuration \[(i.e.,\] has four shells), but \[{{K}^{+}}\] has \[Ar\] gas configuration \[(i.e.,\] has three shells), nevertheless ionic size of \[S{{r}^{2+}}\] is smaller than that of \[{{K}^{+}}\] due to higher nuclear charge which overweighs the effect of an additional shell.
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