A disproportionation reaction is an oxidation–reduction reaction in which the same substance is oxidized and reduced. Complete and balance the following disproportionation reactions:
(b) MnO₄^2-(aq) → MnO₄^-(aq) + MnO₂(s) (acidic solution)

Verified step by step guidance

1. Identify the oxidation states of manganese in each compound: MnO4^2- has Mn in +6 oxidation state, MnO4^- has Mn in +7 oxidation state, and MnO2 has Mn in +4 oxidation state.
2. Write the half-reactions for the oxidation and reduction processes. For oxidation, Mn in MnO4^2- goes from +6 to +7. For reduction, Mn in MnO4^2- goes from +6 to +4.
3. Balance the manganese atoms in each half-reaction. Since there is one Mn atom on each side of the half-reactions, they are already balanced for Mn.
4. Balance the oxygen atoms by adding water (H2O) molecules. For the oxidation half-reaction, add one water molecule on the right side. For the reduction half-reaction, add two water molecules on the left side.
5. Balance the hydrogen and charge in each half-reaction by adding hydrogen ions (H+) and electrons (e-). For the oxidation half-reaction, add two H+ on the right and one e- on the left. For the reduction half-reaction, add four H+ on the right and two e- on the left.

Key Concepts

Disproportionation Reaction

A disproportionation reaction is a specific type of redox reaction where a single substance undergoes both oxidation and reduction simultaneously. In this process, one part of the molecule loses electrons (is oxidized) while another part gains electrons (is reduced), resulting in the formation of two different products from the same reactant.

Oxidation States

Oxidation states (or oxidation numbers) are a way to keep track of electron transfer in redox reactions. They indicate the degree of oxidation of an atom in a compound, helping to identify which atoms are oxidized and which are reduced. Understanding oxidation states is crucial for balancing redox reactions, including disproportionation reactions.

Balancing Redox Reactions

Balancing redox reactions involves ensuring that the number of electrons lost in oxidation equals the number of electrons gained in reduction. This can be achieved using the half-reaction method, where the oxidation and reduction processes are balanced separately before combining them to form a complete balanced equation. This is essential for accurately representing the stoichiometry of the reaction.