Oxidation and Reduction in Terms of Electrons

Chemical reactions constantly keep occurring around us. The oxygen we breathe in is a chemical reaction between two oxygen atoms that have bonded. If we own any iron furniture or things, we notice rust on them after a few days. It is an example of the oxidation of iron. Reduction and oxidation are some of the most common chemical reactions. We can notice the examples of redox reactions in our daily life. But we don’t know what exactly goes on at the electron or atom level during these chemical reactions. Let’s study that.

The reduction and oxidation reactions

Most of the time, the production and oxidation reactions are two reactions. Whenever a reduction reaction takes place, most of the time, it comes with an Oxidation reaction most of the time. Thus, the reduction of oxidation reactions occurs simultaneously; saturation is called the redox reaction in redox reactions, the Oxidation state of atoms changes. Out of the two participating elements, one of the elements gets oxidised by the other elements and gets reduced. Hence the redox reaction takes place simultaneously as these reactions need one reducing agent and one oxidising agent in it. They are known as reducing agents and oxidising agents, respectively. 

Although we might think that an Oxidation reaction would involve oxygen molecules, it is not always the case. This is because the reduction and oxidation reactions are related to the exchange of electrons and not just the exchange of oxygen and hydrogen molecules. 

Let us take an Oxidation reaction example and a reduction reaction example concerning carbon. When a Carbon molecule undergoes oxidation, it gains an oxygen molecule by combining with it, which leads to the formation of the carbon dioxide gas. When the same Carbon atom reacts with hydrogen or gains hydrogen, it leads to methane gas formation.

Measurement of the redox reaction

The extent of the redox reactions, that is, the capability of an element to oxidise at the element or two reduce another element is measured with the help of reduction potential. The unit of reduction potential is Volts or millivolts. The elements with more positive reduction potential values tend to donate electrons and oxidise.

The elements with highly negative reduction potential values usually tend to accept electrons and get reduced. The analysis of ionisation energy and bond energy in water will help calculate the reduction potential of the redox potential. The proper meaning of Oxidation reaction is loss of electrons or increase in the oxidation state of an element.

The definition of reduction is the gain of electrons or decrease in the oxidation state of an element.

The reduction and oxidation reactions in terms of electrons

We know that the oxidation and reduction reactions occur simultaneously in which one element reduces the other element while another element oxidises the first elements.

But let us look at what happens at the atomic level or the electron level during the redox reactions.

When two elements are combined in a chemical process, they are trying to get stabilised by filling their octet. Which means their last shell must contain 8 electrons. The elements either give up the electrons or accept electrons from other elements to achieve this. The elements which have a smaller number of electrons in the outer shells usually tend to donate electrons. The elements that have more number electrons in the outer shells find it is here to accept electrons.

The donation of electrons by an element leads to that element getting oxidised. Since they help the other element get reduced by getting themselves oxidised, they’re called reducing agents. The elements which accept the electrons get reduced. With the help, the other element gets oxidised and gets reduced.

They are termed oxidising agents. Since some other element must have given up its electrons for one element to receive electrons, and for one element to give up its electrons, another element must be ready to receive those electrons. This is why the reduction and oxidation reactions take place simultaneously. However, when an element simply reacts with oxygen or hydrogen, it undergoes only reduction or oxidation.

This is how the reduction and oxidation reactions occur at the atomic or electron level.

Conclusion:

The oxidation and reduction reactions are among the most commonly occurring reactions in nature. They are also used in industries for many manufacturing and processing purposes. A redox reaction is when the reduction and oxidation process takes place simultaneously.

At the electron level, an element donates its electrons to another element at the electron level in a redox reaction. Redox reaction involves an oxidising agent and reducing agent. Lithium is a great reducing agent, and Chlorine is an oxidising agent. The redox reaction happens between one reducing agent and one oxidising agent. However, it could involve hydrogen and oxygen.