Oxidation-Reduction Reaction

Redox (reduction-oxidation) is a type of chemical reaction where the oxidation states of the substrate change. Reduction is the gain of electrons or a decrease in the oxidation state, whereas oxidation is the loss of electrons or an increase in the oxidation state. Redox reactions fall into two categories, Only one electron (typically) moves from the oxidant to the reducing agent during an electron transfer. Redox couples and electrode potentials are frequently used to describe this kind of redox reaction. Atom transfer is the process by which an atom moves from one substrate to another. For instance, when iron rusts, the oxidation state of the iron atoms rises as it transforms into an oxide, while the oxidation state of oxygen falls as oxygen accepts the electrons released by the iron. Other chemical species can perform the same function, despite the fact that oxidation processes are frequently linked to the production of oxides. In hydrogenation, hydrogen atoms are transferred to diminish C=C (and other) bonds. Reduction and oxidation are combined to form the word "redox." In 1928, the word "redox" was first used. Oxidation and reduction are synchronous processes that cannot happen separately. In redox reactions, the reductant gives the oxidant electrons. In this way, the oxidant or oxidising agent obtains electrons and is reduced, whereas the reductant or reducing agent loses electrons and is oxidised. Redox pairs are the pair of oxidising and reducing agents involved in a certain process.