Oxidation is characterized by a loss of electrons, the gain of oxygen, or the elimination of hydrogen. The concept reduction denotes an electron gain, a hydrogen gain, or the elimination of oxygen. The term LEOGER (Loss of Electron Oxidation Gain of Electron Reduction) is used to understand oxidation and reduction easily.
Oxidation and Reduction are defined by two concepts:
When a reactant loses electrons during a process, this is referred to as oxidation. When a reactant obtains electrons during a reaction, this is referred to as reduction. This is a common occurrence when metals react with acid. When a reactant loses electrons during a process, this is referred to as oxidation.
When a reactant obtains electrons during a reaction, this is referred to as reduction. This is a common occurrence when metals react with acid.
Oxidation reactions include the following:
2Mg+O2→2MgO
HS+Cl2→HCl+S
2KI+H2O2→2KOH+I2
Fe+S→FeS
N2+3H2→2NH3
ZNO+C→Zn+CO
2FeCL3+H2→2FeCl2+2HCl
SnCl2+2HgCl2 →SnCl4+Hg2Cl2
This is the most often used and universally applicable concept of oxidation and reduction.
Oxidation reactions include the following:
Loss of electron:
Mg→ Mg2+2e–
Reduction reactions include the following:
Gain of electrons:
O+2e–→O2-
The processes of oxidation and reduction are inextricably linked. Because electrons are never created or destroyed during a chemical reaction, oxidation and reduction must always take place in pairs; one cannot exist without the other.
A reduction-oxidation reaction, also known as a redox reaction, is a type of chemical reaction in which reduction and oxidation occur simultaneously. The reduced species gains electrons, whereas the oxidized species loses them.
For instance; in the following example Magnesium is oxidized by losing two electrons to oxygen, which is then reduced by getting two electrons from magnesium.
2Mg+O2→2Mg2+O2-
Because oxidation and reduction cannot occur separately, they are referred to together as ‘Redox Reactions.’ The reactant that oxidizes the other reactants is referred to as the Oxidizing agent, whereas the reactant that reduces is referred to as the Reducing agent.
In other words, a material that is oxidized functions as a reducing agent, whereas a substance that is reduced works as an oxidizing agent.
Oxidation is a chemical reaction in which one or more electrons are lost or the element’s valency rises. Reduction is a process in which one or more electrons are acquired or the element’s valency drops. The oxidizing agent is a substance that can receive one or more electrons, resulting in a drop in valency.
A reducing agent is a substance that may lose one or more electrons, causing its valency to rise. A redox reaction consists of two half-reactions, one of which involves the loss of electrons or electrons (oxidation) and the other of which involves the gain of electrons or electrons (reduction).
Oxidation and Reduction are defined by two concepts. The term LEOGER is used to understand oxidation and reduction easily. Oxidation occurs when a reactant loses electrons during a process. Reduction occurs when a reactant acquires electrons during a reaction.
Oxidation occurs when a reactant loses electrons during a process. Reduction occurs when a reactant acquires electrons during a reaction.
Reduction is the process of gaining electrons, whereas oxidation is the process of losing electrons.
The degree of oxidation (loss of electrons) of an atom in a chemical compound is characterized by the oxidation state, often known as the quantity of oxidation.
The importance of oxidation-reduction (redox) processes cannot be overstated because they are the primary natural, biological, and manmade energy sources on this planet. By removing hydrogen and replacing it with oxygen, oxidation of molecules often releases huge quantities of energy.
