What are disproportionation reactions ? Give example.

A disproportionation reaction is a type of redox reaction where the same chemical species undergoes both oxidation and reduction simultaneously. In such reactions, one atom, ion, or molecule splits into two different products, with one being oxidized and the other being reduced. This process is unique because a single element in a single oxidation state is transformed into two distinct oxidation states.

Key Characteristics of Disproportionation Reactions

• The same element acts as both the reducing agent and the oxidizing agent in the reaction.
• It involves a single species being converted into two different species with varying oxidation states.
• Disproportionation reactions are commonly observed in compounds where the element exists in an intermediate oxidation state, which can further oxidize or reduce.

Example of a Disproportionation Reaction

An example of a disproportionation reaction is the decomposition of hydrogen peroxide (H₂O₂):

Reaction: 2H₂O₂ → 2H₂O + O₂

In this reaction:

• Oxygen in hydrogen peroxide is reduced from an oxidation state of -1 to -2 (forming water).
• Oxygen is also oxidized from an oxidation state of -1 to 0 (forming molecular oxygen).

Applications of Disproportionation Reactions

Disproportionation reactions play an essential role in various chemical and biological processes. For example:

• In biological systems, disproportionation reactions are crucial in metabolic pathways.
• In industrial chemistry, they are used in processes such as the production of oxygen and other chemicals.

Understanding disproportionation reactions helps in studying redox chemistry and the behavior of elements in different oxidation states.