Uses of Allotropes and Oxides of Carbon

What are Allotropes of Carbon?

Due to its ability to have varied oxidation states or coordination numbers, carbon may have many allotropic forms. Carbon’s ability to catenate is another significant factor. As a result, it leads to the development of diverse allotropes of carbon.

Structure of Carbon Allotrope 

• Graphite:

Graphite’s honeycomb-layered structure is fascinating. Each layer is made up of carbon atoms in planar hexagonal rings with a carbon-carbon bond length of 141.5 picometers. 

Three of the four carbon atoms create sigma bonds, while the fourth forms a pi-bond. Vander Waal forces hold the layers of graphite together.

• Diamond:

It is carbon’s finest crystalline allotrope. It has a tetrahedrally connected number of carbon atoms. Each tetrahedral unit is made up of carbon bound to four carbon atoms, each of which is coupled to another carbon atom. This results in a carbon allotrope with a three-dimensional arrangement of C-atoms.

Some of the Other Allotropes of Carbon

• Buckminsterfullerene

It is another type of allotrope of carbon. Fullerene has a cage-like structure that gives it the appearance of a football.

• Fullerenes

They are spheroidal molecules with the formula C2n, where n is less than 30. These carbon allotropes can be made by laser evaporating graphite.Fullerenes, unlike diamonds, dissolve in organic solvents. Buckminsterfullerene is the name given to the fullerene C60. The carbon atoms have undergone sp2 hybridization.

Properties of Allotropes of Carbon

Carbon atoms can be connected in a variety of ways. Carbon allotropes are formed by them. Allotropes are distinct forms of an element that have different physical qualities but comparable chemical properties. Graphite and diamond are the most popular among them. Their crystalline structures are dissimilar.

Differences Between Graphite and Diamond

• Graphite:

One carbon atom is surrounded by three covalent connections. It is made up of a flat structure. It is made up of a carbon atom that has been sp2 hybridized. It has a 2.3 grams per cubic centimetre relative density. It is opaque and black. It is an excellent electrical conductor. It is a great lubricant, and one of the softest materials on the market, as well as greasy to the touch.

• Diamond:

It can be found in nature in a free condition. It is a particularly stable carbon allotrope made up of four covalent connections forming a ring around one carbon atom. Its cubic crystal structure is face-centered. It is made up of carbon atoms that have been sp3 hybridized. It has a high relative density and is translucent. It also has a refractive index of 2.45, which is quite high.

Both graphite and diamond exist in solid state. They are both fragile. The density of various types of carbon is determined by its origin. There are pure forms of carbon, such as coal, and non-pure forms of carbon, such as hydrogen and carbon mixes.

Chemical Properties of Carbon 

Carbon’s chemical characteristics influence how it reacts with other chemicals and transforms from one form to another. During chemical reactions, the chemical characteristics of carbon are detected. Carbon may be broken down into millions of different chemicals.

Carbon is involved in these major reactions. Let’s discuss them in detail. 

1) Combustion Reaction

When carbon is burned in the presence of oxygen, it produces carbon dioxide, heat, and light. The process of combustion is defined as the generation of heat and light by the burning of carbon more than oxygen.

C (s) + O2 (g) → CO2 (g) + heat + light

The complete combustion of a hydrocarbon occurs when there is an excess of oxygen present, resulting in carbon dioxide and water as the ultimate products. Energy is produced in the form of heat and light. Complete combustion occurs in saturated compounds. 

Incomplete combustion, on the other hand, occurs when there is insufficient amount of oxygen and a surplus of hydrocarbon.

Some of the examples are given below

• Burning of Wood or Coal for household purposes.

• Burning of Petrol or Diesel for using vehicles like cars.

• Combustion of Natural Gas or LPG to cook.

• For the production of energy in thermal power plants.

• Fireworks or burning of Wax candles.

2) Oxidation Reaction

In the presence of allotropes of oxygen, carbon and its compounds are oxidized.

C (s) + O2 (g) →  2CO (g)

Although all combustion reactions are oxidation reactions, they are not all oxidation reactions.

3) Addition Reaction

Carbon may form lengthy atom chains. This is called addition reaction. To become saturated, unsaturated substances go through this process.

CH3CH = CH2 + HCl → CH3C+HCH3 + Cl− → CH3CHClCH3

Uses of Various Allotropes of Carbon

Uses of allotropes

1. Diamond

• Glass-cutting and rock-drilling machines use it.

• It is used as a decorative element.

• In eye surgery, diamond knives are utilised.

• Other diamonds are polished with diamond dust.

• In space and in artificial satellites, it is used to construct windows that guard against radiation.

2. Graphite

• It is used to make lubricants.

• It is used to make carbon electrodes.

• It is used in writing pencils. 

• It is found in paints and polishes.

• Arc lamps, which produce an extremely bright light, use this material.

3. Fullerene ⋅ 

• They are used as insulators.

• They are used in the purification of water as a catalyst.

4. Coal ⋅ 

• It is used as a source of energy in enterprises and houses.

• Coke, coal gas, and coal tar are all made from coal.

• It is used to generate electricity in thermal power plants.

Conclusion 

Hopefully, you have understood the structure, properties and uses of allotropes and oxides of carbon. So Complete combustion of a hydrocarbon occurs when there is an excess of oxygen present, resulting in carbon dioxide and water as the ultimate products and when insufficient oxygen will supply it is called as incomplete combustion. We can understand that all combustion reactions are oxidation reactions, they are not all oxidation reactions.