Concept of Oxidation

The reaction of compounds coming into touch with oxygen molecules is referred to as oxidation. Metals and non-metals, such as living tissues, are examples of such substances. The process of oxidation is described by the loss of electrons on a chemical level. Typically, the electrons will be taken by another atom species, causing it to be decreased. In many everyday situations, these redox reactions occur. The zinc coating contributes to the nail’s extended life. Nails that have not been galvanised are naked metals that can oxidise. Rain, heat, and other variables might cause the oxidation potential of the nails to increase. Galvanized nails, on the other hand, have a protective coating that prevents the bare metal from fast oxidising. The coating may wear down over time, but it will keep the metal from corroding and oxidising. The oxygen gas is formed once the water is oxidised. Bleach oxidises the electrons in the chemicals that stain textiles. Cleaning garments is made easier by redox reactions.

Oxidation is the loss of one electron during the phase of interaction between two or more atoms. The elements don’t have to include oxygen in this case. In a nutshell, it’s a chemical reaction that results in an atom’s increased oxidation state. Reduction, on the other hand, occurs when the oxidation state of a substance decreases. Formal electron transfers occur in both processes. The process of oxidation is involved in net loss, whereas the state of net gain is the opposite.

Involves the addition of oxygen or any electronegative element

The measure of how quickly an element’s atoms can accept or gain electrons to form anions is known as electronegativity.

When an element (typically a nonmetal) gains electrons, the other element that loses electrons to it is said to be oxidised. As a result, electronegative elements are usually strong oxidizers.

When an element attracts a shared pair of electrons to itself, the process is known as electronegative. Non-metals are always electronegative in nature, and non-metals are strongly polarised and polar in nature due to their nature. The nature of metals, on the other hand, is electropositive. They have the ability and polarised power to bend non-metals, causing non-metals to polarise.

The removal of hydrogen or any electropositive element

The ability of atoms of an element to lose or donate electrons to produce positive ions, also known as cations, is measured by electropositivity.

When an element (typically a metal) loses electrons, the other element that absorbed the electrons is said to be reduced.

As a result, electropositive elements are always powerful reducing agents.

For example, as a very electropositive element, sodium (Na) can attack (push it to receive its electrons) zinc oxide to reduce it to metallic zinc while being oxidised to the oxide.

Atom or ion loses one or more electrons

A cation is a positively charged ion that loses one or even more valence electrons, whereas an anion is a negatively charged ion that obtains electrons.

To generate a cation, which is a positively charged ion, an atom loses electrons (one that is attracted towards the negatively charged terminal, the cathode).

The charge as well as the mass have been preserved.We have to include energy in the equation because the separation of opposite electric charges requires a significant amount of energy.

Chemists use this so-called ionisation energy to explore electronic and atomic structure in the gas phase. The ionisation energy is known to rise over a Period of the Periodic Table (as seen from left to right) and decrease  down a Group.

Conclusion 

The term “oxidation” was first used to denote chemical reactions involving the addition of oxygen to a compound’s element. The earliest known form of oxidation was combustion. Later, the term oxidation was used to represent a wide range of reactions that did not require the use of oxygen. A reducing agent is one that undergoes oxidation, while an oxidising agent is one that undergoes reduction.

One or more electrons are removed or the element’s valency increases during oxidation.

Reduction is a chemical reaction in which an element gains one or even more electrons or loses its valency. The term “oxidising agent” refers to a substance that really can gain one or even more electrons, lowering its valency. A reducing agent is a substance that can lose one or more electrons, resulting in a rise in valency. One side of the redox reaction involves the loss of an electron or electrons (oxidation), while the other involves the gain of an electron or electrons (reduction) (reduction).

The removal of an electropositive element from any chemical species is referred to as oxidation (atom, ion or molecule). The addition of an electronegative element to any chemical species is referred to as oxidation (atom, ion or molecule).