What is Reduction Reaction?

The concept of reduction can be defined as an gain of electrons. The process of reduction reaction happens in the simultaneity with oxidation reactions. The article is going to focus on the description of the reduction reaction as well as its facts. There are multiple examples of this process such as copper oxide, removal of oxygen, as well as the addition of hydrogen. Examples of reduction reactions are metallurgy, photography, burning, bleaching and batteries. 

Description of Reduction Reaction

A reduction reaction can be described as a method in which an ion, or atom effectively gains electrons. The process effectively happens during a reaction of chemicals when an atom gains electrons. That defines that oxidation number reduces as electrons have negative charges, for example, X2+ to X1+, or X0 to X1-.

The examples of reduction reactions are:

CO2 (g) + H2 (g) → CO (g) + H2O (g)

Na + Cl → NaCl

Zn + CuCl2 → ZnCl2 + Zn

CH₄ (g) + O2 (g) → CO2(g) + H2O (g)

The process is effectively used in producing chemicals, corrosion or rusting, combustion, photosynthesis as well as respiration. Reduction reaction plays a critical role in the respiration system of the human body.  The process of reduction reactions involves enhancing electrons connected with a group of atoms or a single atom. Therefore, a reduced atom receives electrons effectively from another atom. 

In a simple definition, a reduction reaction can be defined as a process of reducing the state of oxidation of a molecule, ion, or atom. In the classical idea of the reduction reaction, the process involves:

• Removal of electronegative element

2FeCl₃ + H2 → 2FeCl2 + 2HCl    (Reduction of ferric chloride)

• Removal of oxygen

ZnO + C → Zn + CO   (reduction of zinc oxide)

• Addition of electropositive element:

SnCl2 + 2HgCl2 → SnCl₄ + Hg2Cl2    (Reduction of mercuric chloride)

•  Addition of hydrogen:

N2 + 3H2 → 2NH₃    (Reduction of nitrogen)

The reducing agent in this process is a substance that effectively brings about reduction. C, H2, and HgCl2 in the above examples are the agents of the process. Oxidation and reduction reactions are effectively interlinked as electrons are neither destroyed nor created in chemical reactions. 

Facts of Reduction Reaction

Reduction reactions are the loss of oxygen and in the present scenario, the process is utilised in different ways. For instance, the method of reduction reaction is used in reducing ores in order to obtain metals, transform ammonia into nitric acid as well as produce electrochemical cells. Some examples of reduction reactions are the copper ion and rusting of iron. This process effectively involves a half-reaction where chemical species reduce their oxidation number by gaining electrons. Oxidation and reduction reactions are commonly known as redox reactions. 

There are multiple types of oxidation and reduction reactions such as combustion, disproportionation, combination, decomposition as well as displacement. The examples of reduction reactions assist in identifying reducing agents and developing certainties regarding the concepts of reduction reactions. Rusting of iron can be defined as an effective example of a reduction reaction. There is an effective importance of oxidation and reduction reactions as they are the main energy sources on this planet. In the function of the human body, the reduction reactions play a critical role in reducing the integer of carbon-heteroatom bonds, as well as enhancing the integer of carbon-hydrogen bonds. In oxidation and reduction reactions electrons are essential. 

Conclusion 

Based on the above discussion, the redox reaction plays a critical role in producing different chemicals. Oxidation and reduction reactions are effectively used in electrochemical cells in order to produce electricity.  The article has discussed the description of the reduction reaction as well as its facts. The application of a reduction reaction can happen without the involvement of oxygen. The application effectively happens throughout a reaction of chemicals when an atom gains electrons. Moreover, it can be stated that, for industrial processes and biochemical reactions, the applications of reduction reactions are common.