Understanding Oxidation With the Help of Example

Oxidation is a chemical reaction which is caused by the contact between materials and oxygen molecules. Such materials can be metals or non-metals.

Furthermore, oxidation may be defined as the loss of single or more electrons throughout the process when two or more elements interact. During the process, elements do not essentially require oxygen, and it can also define  an atom’s enriched oxidation state with the help of chemical reactions. The exact reverse of oxidation is called reduction, which shows a reduction in the oxidation state. Both the reactions involve prescribed electron transfers. Net damage includes oxidation, while the net gain is part of the reduction.

Oxidation Examples

Rust is one of the most common instances of oxidation. Iron components change into brown iron (III) oxide when in contact with oxygen or oxidised. Furthermore, oxidation examples are zinc metal shifting copper or silver in solution, then zinc (II) ion is produced during the oxidation process, and scorching of anything in oxygen, such as sugar or magnesium, is also known as an oxidation reaction. Bleaching hairs, glowing tonic water, and blue jeans are also oxidation-reduction reactions.

Oxidation & Reduction Reaction

Oxidation & reduction reactions are also known as redox reactions, in which the oxidation & reduction takes place, and chemical species change with time. The term shelters a large and diverse body of processes. Numerous oxidation-reduction reactions are common and familiar such as fire, the dissolution and rusting of metals, the browning of fruit, respiration, and photosynthesis, and many more basic life functions.

Examples of Oxidation reduction redox reaction

Some of the examples elaborated on the oxidation and reduction process. Moreover, it can be explained in terms of alteration in oxygen content or hydrogen content, and explanation in terms of electrons is as follows:

Example 1

Magnesium is oxidised and turned into magnesium oxide when contacted or reacted with oxygen. The explanation for the oxidation reaction is as follows:

Magnesium + oxygen → magnesium oxide

2Mg + O2 → 2MgO

Explanation:

Magnesium gains more oxygen, and gaining oxygen is known as oxidation.

or

Magnesium loses electrons, and loss of electrons is also known as oxidation. Which is shown by the equation below :- 

Mg → Mg2+ + 2e-

Example 2

Copper (II) oxide may be reduced to form copper when it comes in contact with hydrogen. Copper (II) oxide is termed as being reduced because

Copper (II) oxide + hydrogen → copper + water

CuO + H2 → Cu + H2O

Explanation:

Copper (II) oxide drops down oxygen, and loss of oxygen is known as reduction.

or

Copper (II) ions increase electrons, and an increase in electrons is known as reduction.

This is shown through the equation below:

Cu2+ + 2e-→ Cu

Example 3

The equation below shows the reaction of nitrogen with hydrogen to make ammonia.

N2 (g) + 3H2 (g) → 2NH3 (g)

Explain why nitrogen is defined as being reduced :-

Explanation:

An increase of hydrogen in nitrogen and an increase in hydrogen is known as reduction.

This cannot be clarified in terms of oxygen (as there is no oxygen in the reaction) and all the materials involved are covalent, and there is no loss or gain of electrons during the reaction. Generally, oxidation and reduction take place concurrently in the reaction. This is commonly called a redox reaction.

Types of Oxidation and Reduction Reactions

Apart from expanding oxidation states to identify redox reactions, there are additional ways to predict when a redox reaction is taking place; specifically, there are a limited number of different forms of reactions in which reduction and oxidation habitually both take place.

• Combination Reactions:

Combination reactions are the type of reaction, which combines elements to make a compound, usually in the form of,

A + B → AB

• Decomposition Reactions:

Decomposition reactions are known as the opposite of combination reactions. A compound decays into its small elemental parts. Normally, it takes place in the form of AB → A + B

• Combustion Reactions:

Combustion reactions contain fuel (mostly organic) and oxygen as reactants and result in water and carbon dioxide and irregularly extra biological products like nitrogen and generally in the form of,

X + O2 → CO2 + H2O

• Displacement Reactions with an Oxidation state change:

This type of reaction can moreover originate in the form of a single replacement, where one component in a compound is swapped by another one, or in the form of a double replacement, where an element in each of the two different reactants gets replaced. The basic form of a single replacement reaction is A + BC → B + AC, and the normally double replacement reaction takes place in the form of

AB + CD → AD + CB.

Conclusions 

Oxidation is a chemical reaction which is caused by the contact between materials and oxygen molecules. Such materials can be metals or non-metals. Oxidation & Reduction or Redox reaction involves the functioning of oxygen and hydrogen. First order reaction is known as the common example of the oxidation reduction reaction.