Question

Define oxidation and reduction on the basis of electronic concept.
             

Answer 1

Hint: When the number of atoms joined together to form a molecule, these molecules have less energy as compared to individual atoms. When an atom releases electrons and other atoms gain electrons then an ionic bond is formed.

Complete step by step answer:
Metals are electropositive in nature it means metal having the capacity to lose the electrons. When metal loses the electrons they carry a positive charge. Non-Metals are electronegative in nature it means non-metal having the capacity to gain the electrons. When non-metal gains the electrons they carry a negative charge. Then attraction occurs between positive and negative charges and an ionic bond is formed and an ionic compound is formed.
According to electronic concept-Oxidation may be defined as when the element losing the electrons is known as oxidation and Reduction may be defined as when the element gains the electrons is known as Reduction.
During oxidation, the acidic nature of an element increases due to oxidation. And the basic nature of an element increases due to reduction.
The best example of oxidation is rusting of iron.
\[Fe \to F{e^{2 + }} + 2{e^ - }\]
The best example of reduction is Formation of hydrogen gas.
\[2{H^ + } \to {H_2}\]
In it hydrogen gas is present in elemental form so it does not lose the electrons and not gain the electrons.

Note:
Two types of reagents in chemistry: first is Oxidising agent and other is reducing agent.
The oxidising agent may be defined as the element or molecule which reduces itself and helps other elements in oxidising.
The reducing agent may be defined as the element or molecule which oxidises itself and helps other elements in reducing.
During oxidation, the acidic nature of an element increases due to oxidation. And the basic nature of an element increases due to reduction.