Electronic Concepts of Oxidation and Reduction

Introduction

The electronic concepts of oxidation and reduction means that when there is an addition of oxygen or removal of electrons or hydrogen, oxidation occurs. When one substance oxidizes another substance it is known as an oxidizing agent. Oxidizing can also be known by the name oxidant, oxidizer. Whereas, when there is an addition of hydrogen or removal of oxygen or addition of electrons the reduction occurs. When one substance reduces the other substance it is known as a reducing agent. The reducing agent is also known by the name reductant or reducer. The occurrence of oxidation and reduction at the same time is known as a redox reaction. 

Oxidation Reaction:

As per the earlier concept, the procedure that includes the addition of any electronegative elements or oxygen or the removal of an electropositive element or hydrogen is known as oxidation.  

While, as per the electronic concept, a process in which an atom or ion loses one or more electrons is known as oxidation. 

Reduction Chemistry:

As per the earlier concept, the procedure that includes the addition of any electropositive elements or oxygen or the removal of an electronegative element or hydrogen is known as reduction. 

Whereas, as per the electronic concept, a process in which an atom or ion gains one or more electrons is known as reduction. 

Oxidation and reduction:

Mainly in-between reducing substance and oxidising substance a chemical reaction takes place. In this reaction of oxidation and reduction, the reducing substance gains electrons whereas the oxidising substance loses electrons. The oxidation and reduction reaction is also known as the redox reaction. The oxidation and reduction reactions go along with the change of energy in the form of heat, light, and electricity, etc. For example, In the reaction between the oxygen included in water or moist air and iron happens, it forms rust. When in our body fat and glucose are broken down to make energy, oxidation, and reduction occur. 

Example of electronic concepts of oxidation and reduction: 

So, in this case, Fe fluctuates from 0 to +3 which implies that there is the removal of electrons and it is done through the oxidation process. 

As the oxygen state of the oxygen is changing from 0 to -6 that means that there is an addition of electrons and it has gone through the oxidation process. 

Classical idea of oxidation and reduction reactions:

Oxidation Reaction: 

1. The oxidation reaction includes the addition of oxygen:

Formula = C + O2 → CO2

( the oxidation of carbon)

  2. The oxidation reaction includes the addition of an electronegative element:

Formula = Fe + S → FeS

( the oxidation of iron)

  3. The oxidation reaction includes the removal of hydrogen

Formula = H2S + Br2 → 2HBr  + A

( the oxidation of sulphide)

  4. The oxidation reaction includes the removal of 

Formula = 2 KI + H2O2 →  I2 + 2 KOH-

( the oxidation iodide)

The substance that brings about oxidation is oxidising agents. O2, S, Cl2, Br2, and  H2O2 are oxidising agents which are mentioned above. 

Reduction Reaction:

1. The reduction reaction includes the addition of hydrogen 

Formula = N2 + 3H2 → 2NH3  

( the reduction of nitrogen )

  2. The reduction reaction includes the addition of electropositive elements

Formula = SnCl2 + 2HgCl2 → SnCl4 + Hg2Cl2 

( the reduction of mercuric chloride)

  3. The reduction reaction includes the removal of oxygen 

Formula= ZnO  + C  → Zn  + CO 

( the reduction of zinc)

  4. The reduction reaction includes the removal of electronegative elements

Formula = 2FeCl3 + H2 → 2FeCl2 + 2HCl-   

 ( ferric chloride )

The substance that brings about reduction is the reducing agents. H2, HgCl2 and C are reducing agents which are mentioned above. 

The oxidation vs reduction:

A substance losing electrons throughout a reaction is known as oxidation. While a substance gaining electrons throughout a reaction, is known as deduction. Metals reacting with acid is a common happening. The oxidation and reduction is mainly a type of reaction that occurs simultaneously. In this, the reduced one obtains electrons and the oxidised one loses electrons. 

The oxidation and reduction considering electron transfer

• Is the most widely used as
• It is very typically used

Explanation of oxidation and reduction. 

The process of reduction and oxidation are interlinked and they occur simultaneously. It is because of the electrons, as electrons can neither be created nor be destroyed, that is why they occur at the same time. Oxidation and reduction cannot do this without having each other. As we know that both of these reactions appear in a pair and they can’t work individually that’s why they are known by the name the redox reactions. 

Conclusion:

The Reactions where an element combined with oxygen, was used to be the meaning of the word oxidation. And also the substance that oxidises another substance is referred to as an oxidising agent.

Therefore, in learning both the definition of oxidation and reductions in terms of electron transfer, some kind of confusion might occur. That is why we can understand and learn it in a helpful matter and that is: 

• These agents oxidised further substances.
• The process means that the oxidising agent is getting reduced. 
• The loss of electrons equals oxidation
• The gain of electrons refers to reduction.