Answer – Oxidation involves the loss of electrons, whereas reduction involves the gain of electrons.
Explanation:
Oxidation and reduction are part of redox reactions, which involve the transfer of electrons between reactant species.
Oxidation is a chemical process in which a substance loses electrons and its oxidation state increases. In a reduction reaction, the substance gains electrons, leading to a decrease in its oxidation state. These two processes are interrelated because when one species undergoes oxidation, another species simultaneously undergoes reduction.
Here is an example:
Oxidation and reduction reactions occur simultaneously wherein there is an exchange of electrons between the oxidized and reduced species Image credit: Grogu60 / Wikimedia Commons (licensed under CC BY-SA 4.0)
The ferrous ion (Fe2+) loses an electron by undergoing oxidation and forms Fe3+ (ferric ion). Therefore, iron is called the oxidized species. Simultaneously, the cerium ion (Ce4+) gains an electron by reduction and forms Ce3+. Therefore, these are called reduced species. Iron’s oxidation state increased from 2+ to 3+, whereas Cerium’s oxidation state reduced from 4+ to 3+.
To sum it up, here’s a table showcasing some differences between oxidation and reduction reactions:
Oxidation
Reduction
Oxidation involves an atom, ion, or molecule losing electrons.
Reduction involves the gaining of electrons by an atom, ion, or molecule.
The chemical substance being oxidized acts as an electron donor.
The chemical substance being reduced acts as an electron acceptor.
Oxidation reactions tend to occur more readily in exothermic processes, releasing energy in the form of heat or light.
Reduction reactions often occur more readily in endothermic processes, requiring an input of energy to proceed.
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