Chemistry

10 Differences between oxidation and reduction reaction

Oxidation and reduction reactions are two types of electrochemical reactions. An electrochemical reaction involves the transfer of electrons between two chemical compounds. In oxidation reactions, there is a loss of electrons, and in reduction reactions, there is a gain of electrons. The electrochemistry of oxidation and reduction is very useful in sensors, chemical synthesis, etc. In this article, we look at 10 differences between oxidation and reduction.

Differences between oxidation and reduction

Basis of differentiation	OXIDATION	REDUCTION
Definition	When one molecule loses an electron, it is termed oxidation.	When one molecule gains an electron, this is termed a reduction.
Meaning of the term	Term reduction means to lead back from the Latin stem.	Term reduction means to lead back comes from Latin stem.
Agents involved	An oxidizing agent oxidizes another substance and itself becomes reduced. It is also known as an electron acceptor.	A reducing agent reduces another substance and itself becomes oxidized. It is also known as an electron donor.
Electron transfer	In this, the electrons are lost.	In this, the electrons are gained
Hydrogen atom	There is the removal of the hydrogen atom.	Here, the oxidation state increases. There is an increase in the oxidation number
Oxygen atom	When oxygen is added, the reaction releases energy.	When oxygen is removed, the reaction stores energy.
Oxidation state	Here, the oxidation state increases. There is an increase in the oxidation number	Here the oxidation state decreases. There is a decrease in oxidation number.
	It occurs in reducing agents.	It occurs in oxidizing agents.
Examples of oxidizing/reducing agents	Oxidizing agents: Ozine, hydrogen peroxide, oxygen, sulfuric acid	Reducing agents: sodium borohydride, lithium aluminum hydride, ascorbic acids
Charges	It causes the increase of positive charges of chemical species.	It causes the increase of negative charges of chemical species.
Real-life application	Electrochemical reactions in batteries, photosynthesis, water splitting, etc	Electrochemical reactions in nanoparticle synthesis by metal salt reduction, electrochemical cells, etc

difference between oxidation and reduction reaction — Difference between oxidation and reduction reaction

What is a redox reaction?

A redox reaction is an electrochemical reaction in which both oxidation and reduction happen simultaneously. For example, water splitting is a redox reaction, in which the release of oxygen gas is an oxidation reaction (because of the loss of hydrogen from water), and the evolution of hydrogen gas is called reduction (due to the loss of oxygen).

H₂O —> H₂ + O₂

Another example would the displacement reactions involving a metal, these types of reactions are widely employed in batteries.

Zn + CuSO₄ —> ZnSO₄ + Cu

Here zinc metal is first 0 oxidation state, after the reaction, the oxidation of zinc increases to +2. This is called an oxidation reaction. For copper, the oxidation state initially is +2. It is decreased to 0 after the reaction. This is called the reduction reaction.

What is the difference between oxidation potential and reduction potential?

The oxidation potential is the value that shows the tendency of the material to lose electrons. In other words, it shows how easily a material can be oxidized. In contrast, the reduction potential shows the tendency of a material to gain electrons. In other words, it shows how easily a material can be reduced.

What is the difference between oxidizing agents and reducing agents?

Oxidizing agents have the ability to oxidize another molecule when they themselves get reduced in the process. Reducing agents have the ability to reduce but they themselves get oxidized in the reaction.

Example: 2NH₂OH + H₂O₂ —> N₂ + 4H₂O

Here, hydrogen peroxide acts as an oxidizing agent. Hydrogen peroxide loses oxygen and gets reduced to water. The hydroxylamine gets oxidized to nitrogen gas.

What are the common examples of oxidation reactions?

2H₂O → 2H₂+ O₂ (release of oxygen is oxidation)
Mg + O2 —> 2MgO (oxidation of magnesium)
Zn + CuSO₄ —> ZnSO₄ + Cu (oxidation of zinc metal)

What are the common examples of reduction reactions?

2H₂O → 2H₂+ O₂ (release of hydrogen is reduction)
Mg + O2 —> 2MgO (reduction of oxygen gas)
Zn + CuSO₄ —> ZnSO₄ + Cu (reduction of copper sulfate)