What is the Difference Between Intramolecular Redox and Disproportionate Redox Reaction?

The key difference between intramolecular redox and disproportionate redox reactions lies in the chemical elements that undergo oxidation and reduction:

• Intramolecular redox reactions involve a single substrate where different elements (or species) within the molecule undergo oxidation and reduction. These reactions occur when molecules containing different elements undergo both oxidation and reduction reactions within the same molecule. Some intramolecular redox reactions involve oxidation and reduction in the same chemical element, which is called disproportionation.
• Disproportionate redox reactions involve a single element undergoing both oxidation and reduction. These reactions occur when the same element in a molecule undergoes oxidation and reduction. A common example of this type of reaction is the disproportionation of the hydrogen peroxide molecule, where oxygen undergoes oxidation to form oxygen gas and reduction to form a water molecule.

In summary, the main difference between intramolecular redox and disproportionate redox reactions is that intramolecular redox reactions involve different elements within a molecule undergoing oxidation and reduction, while disproportionate redox reactions involve the same element undergoing both oxidation and reduction.

Comparative Table: Intramolecular Redox vs Disproportionate Redox Reaction

Intramolecular Redox and Disproportionate Redox Reactions are two types of inorganic chemical reactions where oxidation and reduction occur. Here is a table highlighting the differences between the two:

In summary, the key difference between intramolecular redox and disproportionate redox reactions is that, in intramolecular redox reactions, both oxidation and reduction occur within a single molecule, while in disproportionate redox reactions, the same element undergoes both oxidation and reduction, but not necessarily within a single molecule.