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Graphite is initially used for making the pencils considered as the allotrope of carbon that is opaque and greyish in colour. Properties of Graphite is that it is crystalline solid and enormously slippery to touch. The formation of Graphite is seen when the carbon is highly subjected to high pressure and heat of the upper mantle and earth crust. The properties of Graphite are highly resistible which is used for creating the moderator rods in nuclear power plants. Graphite possesses two-dimensional layers like structure, which is also termed the “Sandwich structure”. In Graphite structure, every atom of carbon is closely linked to the three carbon atoms in a similar plane through the atomic bonds that are covalent.
Properties of Graphite
Alpha graphite and Beta graphite are considered as two types of Graphite classified based on the arrangements of carbon atoms. Graphite is mentioned as the macromolecule which is also termed as macromolecule crystal and this is formed up of the carbon atoms at the point of lattice that of the Diamonds. Graphite possesses a similar composition to Graphite which has the molecular outline that provides every that they are significantly opposite characteristics. The properties of Graphite are mentioned below:
- Graphite are “opaque substances” and the colour of the graphite is “greyish black in colour.”
- In comparison to Diamond, Graphite is lighter in weight, slippery in touch and is very smooth.
- It is represented as a good electricity and heat conductor because of the free electron’s presence in the materials.
- Graphite is enormously soapy, possesses softness due to the weak wall forces of Vander, and is non-inflammable.
Physical properties of Graphite
Graphite is utilised in electrochemistry as the standard stage for describing the heat in the carbon compounds’ formation. The carbon atom in Graphite is SP2 hybridised which creates a structured layer of hexagonal arrangements of the carbon atoms where the layers have relatively weak forces between them. The physical properties of Graphite are:
- Graphite has a relatively high “melting point” of 3650 degrees Celsius near the Diamond melting point due to its layered structure and soft and slippery nature.
- Graphite has the ability and capability in absorbing neutrons of high speed.
- Graphite is regarded as not soluble in water and organic solvents because the force of attraction between the carbon atoms and solvent molecules is not powerful enough. It is not so powerful to overcome the bonds of covalent between the carbon atoms in the Graphite.
- Delocalisation of electrons creates the atomic molecules free to rotate throughout the sheets and makes Graphite the good electricity conductor.
Properties of Diamond and Graphite: comparison
| Basis | Diamond | Graphite |
Properties | The unique nature and trait of Diamond are crystalline. | The structure and nature of Graphite are layered. |
| Every C in the Diamond is SP3 hybridised and forms the covalent bonds of 4 with the neighbouring atoms of C. | In the case of Graphite, it possesses the property where the C atom is SP2 hybridised and creates the sigma bond of 3 with the other C atoms. The fourth electron creates the PI bond in Graphite. | |
| In the context of Diamond, tetrahedral geometry is represented. | Graphite possesses the property where the geometry is represented as planar. | |
| The length of the CC bond is approximately 154 pm. | The length of the CC bond for Graphite is around 141.5 pm. | |
| The covalent bonding is enormously rigid which is extremely hard to break. | The layers of Graphite can be dissected easily due to its softness. | |
| Diamond is regarded as electric insulator that cannot produce electricity. | Graphite is mentioned as a good electricity conductor. |
Conclusion
Based on the above study, it is concluded that Graphite possesses the unique property of producing electricity through the delocalisation of free electrons and carbon atoms. From the thorough understanding, it is comprehended that the carbon atoms of Graphite are negatively charged in the sheet of Graphite, which has the structure of electrons that are highly unusual in carbons through the lone pair of electrons. Softness is the main unique property, which is mostly used for making pencils, papers in comparison to the Diamond.
