Difference Between Oxidation and Reduction

Introduction

Oxidation is the process in which the loss of electrons during a reaction occurs or takes place. loss of electrons can be done by either a molecule or by an atom or by any ion. In oxidation the O.S. of the molecule, atom, or ion increases. While the reduction is the process in which the gain of electrons takes place. Gain of electrons can be done by either a molecule or by an atom or by any ions. In the reduction process oxidation state of the molecule, atom, or ion decreases. Redox reaction is a type of reaction that is a combination of oxidation and reduction reactions. In the redox reaction, reactants change their oxidation states. In the redox reaction, both oxidation and reduction reactions occur simultaneously. The agent or element or the compound that itself undergoes reduction is called the oxidizing agent and, the agent that itself undergoes oxidation is called the reducing agent.

What is Oxidation?

Oxidation is a chemical process in which the oxidation states of the chemical substances (reactants) change because of the addition of oxygen molecules. And it can also be defined as the reaction that occurs due to the contact between the substances and the oxygen $\mathrm{(O_{2})}$ molecules. And the substances which are involved in the reaction may be metals and non-metals like living tissues. Oxidation is a process where the loss of one or more electrons during the reaction phase takes place where two or more elements interact. But in the oxidation reaction, the involvement of oxygen is not necessary. One well-known example of oxidation is rusting of iron in the presence of atmospheric air.

What is Reduction?

Reduction is a process that is just opposite to the oxidation reaction. According to the classical concept, a reduction is a process that involves the addition of the hydrogen molecule or any other electropositive element. Reduction reaction also involves the removal of oxygen molecules or any other electronegative element. Reduction is a process where the gain of one or more electrons takes place during the reaction phase where two or more elements interact. In a reduction reaction, the oxidation state of the molecules, atoms, or ions decreases. Again, rusting of iron is an example of a reduction reaction along with the oxidation reaction. In rusting, oxygen gets reduced, while iron gets oxidized. One another example of this is- That iron oxide $\mathrm{Fe_{2}O_{3}}$ undergoes reductions to give iron $\mathrm{(Fe)}$ and carbon monoxide $\mathrm{(CO)}$ undergoes oxidation to form carbon dioxide $\mathrm{(CO_{2})}$.

$$\mathrm{Fe_{2}O_{3}\:+\:3CO\:\rightarrow\:2Fe\:+\:3CO_{2}}$$

What is Redox Reaction?

Redox reaction is nothing but a combination of oxidation (loss of e) and reduction (gain of e) reactions. Since both oxidation (loss of e) and reduction (gain of e) reactions occur simultaneously. In the Redox reaction electrons get transferred between the reactants participating in the reaction. And the reactants in the reaction change in their oxidation states (O.S.). Redox reactions can easily be separated into two distinct processes that are the oxidation process and the reduction process. And the transfer of the electrons $\mathrm{(e)}$ can be observed by observing the change in the O.S of the reacting species. There are various kinds of redox reactions and those are- Combination reaction (𝐴 + 𝐵 → 𝐴𝐵), decomposition reaction $\mathrm{(AB\:\rightarrow\:A\:+\:B)}$, displacement reaction $\mathrm{(X\:+\:YZ\:\rightarrow\:XZ\:+\:Y)}$, and disproportion reactions. Some examples of redox reactions are - the burning of fuel, photosynthesis, etc.

What is an Oxidizing agent?

In a redox reaction, the agent, or the substance that itself gets reduced and oxidized by the other reactant present in the same reaction is called an oxidizing agent. Sometimes oxidizing agents are also called an oxidant or electron acceptors. In other words, an oxidizing agent is a type of chemical species that undergoes a chemical reaction or reaction in which it gains or gets one or more electrons $\mathrm{(e)}$. It is one of the components of the redox reaction. The Oxidizing agent can also be considered a chemical species that transfers or moves its electronegative atoms, generally oxygen atoms to a substrate. One of the examples of oxidizing agents is- ferrocenium ion $\mathrm{(Fe(C_{2}H_{5})\:^{+}_{2})}$. This ion easily accepts an electron (e) to form $\mathrm{Fe(C_{2}H_{5})_{2}}$ . One of the commercially used stronger acceptors is Magic blue.

What is a Reducing agent?

In a redox reaction, the element, or the compound that itself gets oxidized and reduces the other reactant present in the same reaction is called a reducing agent. Sometimes reducing agents are also called reductant or electron donors. In other words, a reducing agent is a type of chemical species that undergoes a chemical reaction or reaction in which it loses or leaves one or more electrons (e). It is one of the important components of the redox reaction. A reducing agent (itself gets oxidized) is typically found in one of its lower or lowest possible oxidation states (O.S.). And, in a redox reaction, the agent or substance whose oxidation state increases is called the reducing agent. Some of the examples of well-known reducing agents are formic acid, earth metals, oxalic acids, etc.

Oxidizing Agent and Reducing Agent in a Redox Reaction

In a redox reaction, an oxidizing agent is an agent or substance that undergoes reduction by taking the electrons, and hence its oxidation state (O.S.) decreases. While the reducing agent is the substance that undergoes oxidation by donating the electrons, and hence its oxidation state (O.S.) increases. An oxidizing agent helps in the oxidation of another reactant present in the same redox reaction and a reducing agent helps in the reduction of another reactant present in the same redox reaction. For example-

$$\mathrm{MnO^{-}_{4}\:+\:SO^{2-}_{3}\:\rightarrow\:Mn^{2+}\:+\:SO^{2-}_{4}}$$

Here, $\mathrm{MnO^{-}}$ is the oxidizing agent because it is being decreased. Its oxidation state (O.S.) is reducing from +7 to +2. And $\mathrm{SO^{2-}}$ is the reducing agent because it is being oxidized or increased. Its oxidation state (O.S.) is exceeding from +4 to +6.

Difference Between Oxidation and Reduction

Oxidation	Reduction
Oxidation is associated with the loss of electrons.	Reduction is associated with the gain of electrons.
Oxidation means an increase or exceedance in the oxidation number (O.N.).	Reduction means a decrease or reduction in the oxidation number (O.N.).
In the process of oxidation, compounds lose their hydrogen atoms.	In the process of reduction, compounds gain hydrogen atoms.
In this oxidation reaction, a definite amount of energy is released.	In this reduction reaction, energy gets stored.
Some examples of oxidizing agents are- Bleach and ferrocenium ion.	Some examples of reducing agents are- earth metals and oxalic acid.

Conclusion

Oxidation is the chemical process that involves the loss of electrons in molecules or compounds. Typically, oxidation is related to the addition of oxygen molecules and the removal of the hydrogen molecule. Reduction is also a chemical process that involves the gain of one or more electrons in the molecules of the compounds. Typically, the reduction is associated with the addition of hydrogen $\mathrm{H_{2}}$ and the removal of oxygen molecules. Redox reaction is a combination of oxidation and reduction reactions. In the redox reaction, both oxidation and reduction take place simultaneously. One of the reactants undergoes oxidation while the other undergoes reduction.

FAQs

1. Define Oxidation

Oxidation is a chemical process where the loss of electrons and gain in the oxidation state of the compound takes place. Oxidation is the component of the redox reaction. Typically, oxidation means the addition of oxygen and the removal of hydrogen.

2. Give some examples of reducing agents?

Some examples of reducing agents are- earth metals $\mathrm{(Mg\:,\:Ca)}$, formic acid, oxalic acid, etc. These metals are capable of being oxidized and reducing others.

3. Define oxidizing agent?

An oxidizing agent is an agent or material that oxidizes the other reactant present with it in the redox reaction and itself gets reduced by accepting the electrons.

4. Give some examples of oxidizing agents?

Some examples of oxidizing agents are- halogens like fluorine and chlorine, bleach, hydrogen peroxide, etc.

5. Give one example of a redox reaction and mention the oxidizing and reducing agent in the reaction?

In the redox reaction-$\mathrm{2Al\:+\:Fe_{2}O_{3}\:\rightarrow\:Al_{2}O_{3}\:+\:2Fe}$ here, Al is a reducing agent because its oxidation state is increasing from 0 to +3 and $\mathrm{Fe_{2}\:O_{3}}$ is an oxidizing agent because its oxidation state is decreasing from +3 to 0.