Write unbalanced oxidation and reduction half-reactions for the following processes. (b) Mn³⁺(aq) → MnO₂(s) + Mn²⁺(aq)

Key Concepts

Oxidation and Reduction Reactions

Oxidation and reduction (redox) reactions involve the transfer of electrons between species. Oxidation refers to the loss of electrons, resulting in an increase in oxidation state, while reduction is the gain of electrons, leading to a decrease in oxidation state. Understanding these processes is crucial for balancing half-reactions, as they help identify which species are oxidized and reduced.

Half-Reactions

Half-reactions are the individual oxidation or reduction processes that occur in a redox reaction. Each half-reaction shows the transfer of electrons and the change in oxidation states for the species involved. Writing unbalanced half-reactions allows chemists to focus on the electron transfer and helps in balancing the overall redox reaction by ensuring that the number of electrons lost equals the number gained.

Oxidation States

Oxidation states (or oxidation numbers) are a way to keep track of electron transfer in chemical reactions. They indicate the degree of oxidation of an atom in a compound, with higher oxidation states reflecting a greater loss of electrons. In the given reaction, determining the oxidation states of manganese in Mn³⁺, MnO₂, and Mn²⁺ is essential for identifying the changes that occur during the oxidation and reduction processes.