Oxidation-Reduction Reaction

The oxidation states of the substrate change in a chemical reaction known as redox (reduction-oxidation). An increase in the oxidation state or an electron loss is referred to as oxidation, and an electron gain or an electron decrease is referred to as reduction. Redox processes fall into two categories, During an electron transfer, only one electron (typically) moves from the reducing agent to the oxidant. Electrode potentials and redox couples are frequently used to describe this type of redox reaction. An atom moves from one substrate to another through the process of "atom transfer." As an illustration, during the rusting of iron, the oxidation state of the iron atoms increases as it transforms into an oxide, while the oxidation state of oxygen decreases as oxygen accepts the electrons released by iron. Although even though oxidation reactions are frequently linked to the production of oxides, other chemical species can fulfil the same purpose. Transfer of hydrogen atoms reduces C=C (and other) bonds during hydrogenation. Combining the words "reduction" and "oxidation," "redox" is a term. In 1928, the word "redox" made its debut. Oxidation and reduction are interdependent processes that must take place together. The reductant transfers electrons to the oxidant during redox reactions. As a result, in the reaction, the reducing agent (reductant) loses electrons and becomes oxidized, while the oxidising agent (oxidizing agent) gains electrons and becomes reduced. A redox pair is a pair of oxidising and reducing agents that participates in a specific reaction.