Graphite is a carbon allotrope that conducts electricity due to electron delocalization above and below the carbon atom planes.
The mineral graphite is a crystalline form of carbon and is made up of graphene layers layered on top of each other.
In Graphite, the atoms of carbon are hybridized and aligned in the same plane, producing hexagonal rings.
There are numerous layers of particles in the rings. The honeycomb layered structure of graphite is distinctive.
Each layer is framed up of planar hexagonal rings of carbon atoms with a carbon-carbon bond length of pm (picometers) within the layer.
Three of the four carbon atoms make sigma bonds, while the fourth one forms a pi-bond. Vander Waal forces grip these layers together.
Figure: ABC type of Graphite
Characteristics of Graphite
It can work as a lubricant as its layers are piled over one other.
It also has a glossy surface, which contributes to its electrical conductivity
It is a fantastic heat as well as electricity passager.
One of the most crucial properties of graphite is that it may be utilized as a parched lubricant in elevated temperature systems where oil cannot be used.
Graphite is dormant to both acids and alkalis.
Applications of Graphite
As dispersion material, graphite powder is used as a lubricant.
In pencils, manufacturing of steel, and mobile phones, graphite can be used.
As it is an excellent conductor of electricity, it is commonly utilized in the fabrication of carbon electrodes for electrolytic cells.
Because of its high melting point and inert nature against acids and alkalis, it is used in the manufacturing of crucibles.