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Among the following pairs of ions, the lower oxidation state in aqueous solution is more stable than the other, in
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$\mathrm{Tl}^{+}, \mathrm{Tl}^{3+}$
$\mathrm{Tl}^{+}$ions are more stable than $\mathrm{Tl}^{3+}$ and thus, $\mathrm{Tl}^{3+}$ ions change to $\mathrm{Tl}^{+}$ions thereby acting as oxidising agents.
$\mathrm{Tl}^{3+}$ compounds $+2 e^{-} \rightarrow \mathrm{Tl}^{+}$compounds
(less stable, oxidising agent) (more stable, reducing agent)
$\mathrm{Tl}^{3+}$ compounds $+2 e^{-} \rightarrow \mathrm{Tl}^{+}$compounds
(less stable, oxidising agent) (more stable, reducing agent)
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