Answer:
ClO₄⁻
Explanation:
When an ion is hydrated it is surrounded by water molecules, thus, as small is the ion, more molecules may surround it, and it will be more strongly hydrated. In this case, the Cl is small than the S atom, because Cl is from group 17, and S from group 16, and Cl has more valence electrons, which will be more attracted to the nuclei.
So, ClO₄⁻ will be more strongly hydrated.
From the given pair, [tex]ClO^{-} _{4}[/tex] is more strongly hydrated.
The power of hydration depends on the atomic size. Ionic radii increase as atom size increases, resulting in a decrease in hydration. From the given pair of ions, the size of Cl is smaller than S atom, because ongoing left to right in a periodic table size of the atom decreases. Due to the smaller size of Cl, more water molecules may surround it, and the hydration power will increase as compared to [tex]SO^{-} _{4}[/tex]. Hence, from the given pairs of ions, [tex]ClO^{-} _{4}[/tex] is more strongly hydrated.
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