Oxidation-Concept of Oxidation

Oxidation-Concept of Oxidation

Introduction

In chemistry, there are various chemical processes and reactions that take place. Of these, oxidation is one of the essential reactions and processes. Rusting that occurs and which we see around us on metallic substances is an outcome of the oxidation reaction.

On a chemical synapse, electron loss represents the oxidation process. Different atom species will absorb those electrons and then become reduced in most cases. In this module, we will learn about the concept of oxidation, oxidation definition, and various other chemical terms associated with the topic of oxidation.

Definition of Oxidation

Oxidation is a chemical process in which the addition of oxygen, loss of an electron, removal of hydrogen, or an increase in the oxidation number takes place.

In simple words, the chemical process of oxidation takes place when an ion, an atom, or a molecule loses one or more than one of its electrons in an occurring or occurring chemical reaction.

When oxidation occurs, the state of oxidation of chemical elements increases, or the oxidation number of a molecule, atom, or ion increases. This is referred to as oxidation. The inverse oxidation process is termed reduction, and the process of reduction happens when electrons are gained when the oxidation number of an atom, molecule, or ion becomes less.

An early definition of oxidation was the addition of oxygen to a substance. This was because oxygen gas (O2) was first recognised as an oxidising agent. Whereas the addition of oxygen to a substance usually results in electron loss. The concept of oxidation has been widened to cover more and different types of chemical reactions and processes.

Elements which are more resistant to shed electrons are more difficult to oxidise. They securely hold onto their electrons. Non-metals such as oxygen, nitrogen, and chlorine are difficult to oxidise.

Examples of Oxidation

The conversion of Ethanol to ethanal is considered an example of oxidation. 

Here, 

CH3CH2OH→CH3CHO. (oxidation due to the loss of Hydrogen)

An oxidising agent is required to remove the Hydrogen from Ethanol in the above-given chemical equation.

The common oxidising agent used in this chemical reaction above is Potassium Dichromate which is acidified with H2SO4dil.

When iron reacts with oxygen to generate iron oxide or rust, this is a typical illustration of the classical concept of oxidation. The iron is believed to have rusted as a result of oxidation.

2Fe + O2 → Fe2O3

Process of the Concept of Oxidation

The characteristics and attributes of an atom or molecule change drastically as it undergoes the chemical oxidation process. For example, when an object made up of iron oxidises, it gets altered because electrons are lost. Unoxidised iron is a dense, structurally sound metal, but oxidised iron is a reddish powder and brittle. 

When iron is oxidised, it acquires a charge. Now, it has a positive electrical charge of three due to the loss of three electrons. The number three and a positive sign (+3) is written on the upper right side of the element, the iron (Fe) symbol to denote this positive three charge.

Because iron is rapidly oxidised, it is essential to minimise its exposure to oxygen and moisture. As long as oxygen is there, iron will continue losing electrons to it.

The ‘OIL RIEG’ Concept of Oxidation

The oil rieg may be utilised to learn about oxidation and reduction in the present day. It only works with electrons and not with oxygen or hydrogen. It is a simple strategy for determining and remembering which elements are oxidised and which are reduced. The oil rieg stands for Oxidation Is Loss and Reduction Is Electron Gain.

This is a useful shorthand for the terms electron loss or gain. If an atom receives or loses an electron, it becomes an ion. This process is defined by whether an atom has shed (oxidation) or acquired (reduction) one electron

Oxidisers in the Concept of Oxidation

Oxidisers are compounds that can lose an electron or electrons from another element and are referred to as oxidising agents. In simple words, the oxidising agent reduces itself by removing electrons from another substance. Because it receives an electron, the oxidising agent is also known as an electron acceptor.

Conclusion

The concept of oxidation and the various other concepts related to oxidation are discussed in the above-given module. 

A student who wishes to pursue a career in the field of Chemistry must know all about oxidation. It is an essential reaction that occurs in the surrounding environment and has its advantages and disadvantages. 

Oxidation is involved in many activities in our daily lives, including combustion, respiration, and photosynthesis in plants. As a result of this process, fats and oils oxidise and become rancid.