What is a disproportionation reaction, and which of the...

What is a disproportionation reaction, and which of the following fit the description? (a) $\mathrm{I}_{2}(s)+\mathrm{KI}(a q) \longrightarrow \mathrm{KI}_{3}(a q)$ (b) $2 \mathrm{ClO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HClO}_{3}(a q)+\mathrm{HClO}_{2}(a q)$ (c) $\mathrm{Cl}_{2}(g)+2 \mathrm{NaOH}(a q) \longrightarrow$ NaCl $(a q)+\mathrm{NaClO}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$ (d) $\mathrm{NH}_{4} \mathrm{NO}_{2}(s) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$ (e) $3 \mathrm{MnO}_{4}^{2-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$ $2 \mathrm{MnO}_{4}-(a q)+\mathrm{MnO}_{2}(s)+4 \mathrm{OH}^{-}(a q)$ (f) $3 \mathrm{AuCl}(s) \longrightarrow \operatorname{AuCl}_{3}(s)+2 \mathrm{Au}(s)$

What is a disproportionation reaction, and which of the following fit the description?
(a) $\mathrm{I}_{2}(s)+\mathrm{KI}(a q) \longrightarrow \mathrm{KI}_{3}(a q)$
(b) $2 \mathrm{ClO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \longrightarrow \mathrm{HClO}_{3}(a q)+\mathrm{HClO}_{2}(a q)$
(c) $\mathrm{Cl}_{2}(g)+2 \mathrm{NaOH}(a q) \longrightarrow$
NaCl $(a q)+\mathrm{NaClO}(a q)+\mathrm{H}_{2} \mathrm{O}(l)$
(d) $\mathrm{NH}_{4} \mathrm{NO}_{2}(s) \longrightarrow \mathrm{N}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(g)$
(e) $3 \mathrm{MnO}_{4}^{2-}(a q)+2 \mathrm{H}_{2} \mathrm{O}(l) \longrightarrow$
$2 \mathrm{MnO}_{4}-(a q)+\mathrm{MnO}_{2}(s)+4 \mathrm{OH}^{-}(a q)$
(f) $3 \mathrm{AuCl}(s) \longrightarrow \operatorname{AuCl}_{3}(s)+2 \mathrm{Au}(s)$

Key Concepts

Reaction Analysis Technique

Analyzing reactions through the assignment of oxidation numbers is a key method in identifying disproportionation reactions. This technique helps determine the changes in oxidation states of elements throughout a reaction, thereby revealing whether the same element is simultaneously being oxidized and reduced. Such an analysis is fundamental to classifying a reaction as a disproportionation reaction.

Redox Reaction

Redox reactions, short for reduction-oxidation reactions, involve the transfer of electrons between species. Disproportionation reactions fall under this umbrella category, but they are unique because the same element within a compound is both the donor and acceptor of electrons. Understanding the principles of redox reactions is crucial to identifying and analyzing disproportionation processes.

Disproportionation Reaction

A disproportionation reaction is a type of redox reaction in which a single chemical species undergoes both oxidation and reduction simultaneously. In these reactions, the same element is transformed into two different oxidation states, serving as both the oxidizing and reducing agent, which is a distinctive characteristic setting them apart from other redox processes.

Oxidation State

The concept of oxidation state is essential in understanding redox reactions, including disproportionation. It refers to the hypothetical charge that an atom would have if all bonds to it were completely ionic. By assigning oxidation states to elements, chemists can track electron transfers during reactions, which helps in determining whether a substance is oxidized, reduced, or undergoing both processes in the case of disproportionation.

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