Disproportionation Reactions
| Formula / Notation | A → B + C where B and C are oxidised and reduced forms of A; e.g., Cl₂ + NaOH |
|---|---|
| Also Known As | Disproportionation reaction, autooxidation-reduction, symproportionation reverse |
What is Disproportionation Reactions?
A redox reaction in which the same element is simultaneously oxidized and reduced, resulting in two different products. For example, copper(I) can disproportionate to copper(0) and copper(II). These reactions are important in catalysis and biochemistry.
Formula & Notation
Other Names / Synonyms: Disproportionation reaction, autooxidation-reduction, symproportionation reverse
Properties & Characteristics
Uses & Applications
Safety Information
Always consult the SDS/MSDS before handling any chemical. This information is for educational purposes only.
Key Facts
Frequently Asked Questions
A redox reaction in which the same element is simultaneously oxidized and reduced, resulting in two different products. For example, copper(I) can disproportionate to copper(0) and copper(II). These reactions are important in catalysis and biochemistry.
Disproportionation reactions are important in production of bleach (Cl₂ + NaOH → NaOCl + NaCl + H₂O), in copper chemistry (Cu⁺ disproportionates to Cu⁰ + Cu²⁺ in aqueous solution), in metal hydride preparation, and in the Cannizzaro reaction (formaldehyde disproportionation).
Disproportionation can generate hazardous products unexpectedly. For example, H₂O₂ disproportionates to H₂O + O₂; at high concentrations or with catalysts (Fe²⁺, MnO₂), this is rapid and generates large volumes of O₂, creating an explosion/fire hazard.
The formula or notation for Disproportionation Reactions is: A → B + C where B and C are oxidised and reduced forms of A; e.g., Cl₂ + NaOH