Concept of Oxidation in the Field of Chemistry

In chemistry, various chemical processes and reactions occur, out of which oxidation is one of the essential reactions and processes. Rusting that occurs and which we see around us on metallic substances results from the oxidation reaction.

In chemistry, every element is a pure material made up of atoms with a specific amount of protons in their nucleus. Chemical elements, unlike chemical compounds, cannot be broken down into different substances by any chemical process.

Definition of Oxidation

Oxidation is a Chemical process in which the addition of oxygen, loss of an electron, removal of hydrogen, or an increase in the oxidation number occurs.

In simple words, the chemical process of Oxidation takes place when an ion, an atom or a molecule loses one or more than one of its electrons in an occurring or occurring chemical reaction.

When oxidation occurs, the oxidation state of chemical elements increases or when the oxidation number of a molecule, atom, or ion increases; this is referred to as oxidation. The inverse oxidation process is termed reduction, and the process of reduction happens when electrons are gained when the oxidation number of an atom, molecule, or ion becomes less.

What is an Oxidation Number?

The general charge on the top right side of an atom in a given compound or a chemical ion is called the oxidation level or the number of an element.

In simple words, the oxidation number is the charge of atoms that they would have in a chemical molecule if the electrons are entirely transformed.

Using the concept of oxidation number, a student can determine if a given reaction goes through reduction or not.

Examples of Oxidation

The conversion of Ethanol to ethanol is considered an example of Oxidation. 

Here, 

CH3CH2OH→CH3CHO.

Rules for Calculating Oxidation Number

Rules that are essential to determine the oxidation number of an atom-

Rule 1- The state of oxidation or the number of oxidation of all the elements in chemistry in a free state is considered zero.

For Example-

Br20, Na0, H20, P0, etc.

Rule 2- In a given chemical compound, the more electronegative elements are in negative oxidation states, and the less electronegative elements are assigned the positive oxidation states.

Rule 3- In a neutral body, the additional result of oxidation is zero.

Rule 4- The number of oxygen states in any chemical compound is two (+2). There are a few exceptions.

For Example-

Ca2+ O2-, etc.

Rule 5- The oxidation number of Hydrogen on the combination of hydrogen and non-metal is positive (+1).

When hydrogen is combined with a chemical metal of a lesser electronegativity, then the oxidation state for that element is said to be a negative one (-1).

Rule 6- The state of oxidation or the state of oxidation of the Fluorine Atom is -1 all the time because fluorine is the most electronegative element and cannot form more than one bond. Also, the binary compounds of various other halogens are considered as -1.

Rule 7- The elements of Group l, II and III of the chemical periodic table in chemistry depict a state of oxidation of +1, +2, +3, respectively, in various chemical compounds.

Oxidation Number calculation examples

The Advantages of the Oxidation Number Level or Concept

Oxidation numbers can help us decide whether or not redox is involved in a particular process. Oxidation numbers show that neutralisation and precipitation are not redox reactions, even though they involve ions. This point highlights the importance of oxidation numbers as an electron book-keeping device that allows us to recognise the redox process.

The second advantage in using oxidation numbers is that they allow us to see exactly which part of a molecule or a complexion is reduced or oxidised.

Importance and Application of State of Oxidation

Oxidation state is a strategy for accounting for electrons. The fundamental guideline for oxidation state is the preservation of mass. Since electrons can’t be made or annihilated, appropriate bookkeeping of electrons is fundamental to getting compound responses.

To dole out an oxidation state, we envision that every electron is on precisely one particle – no electron sharing. The oxidation state accepts that all holding is ionic.

Suppose we dole out oxidation states when a response, we can comprehend where the electrons streamed. Electrons are the place where all the activity is in substance responses.

Oxidation states are especially significant for electrochemistry. Electrochemistry includes the coupling of power and compound responses. Oxidation states let us know how electrons stream among synthetic compounds; thus, oxidation states should change for power to be created straightforwardly from a substance response. In the same way, power can be utilised to drive a substance response of electrolysis. Consequently,  that compound response includes changes in oxidation states.

Conclusion

When a component responds with oxygen, the expression “oxidation” is used to portray the response. Hematite oxidation, for instance, is a compound response among hematite metal and oxygen that produces hematite oxide. In short words, the oxidation number is the number relegated to the parts in a synthetic mix. 

The oxidation number can be determined by summarising the consistent oxidation state and likening the all-out oxidation condition of a particle.

The mean oxidation number should be equivalent to the total number decided exclusively. Since oxidation states portray how electrons stream between compounds, they should change for power to be produced straightforwardly from a synthetic response.