Graphene is the term used to denote each layer of the same.

However, the lattice structure of the carbon atoms contributes to the difference in hardness of these two compounds; graphite contains two dimensional lattice bonds, while diamond contains three … The carbon atoms in graphite are arranged in a hexagonal structure where one carbon atom forms covalent bond with three surrounding atoms. By Rudina El Dokani Science 9 (1) Mrs. Nicholl Tuesday December 17th Compare and contrast the properties of diamond and graphite Why do Diamonds and Graphite have such different properties?
The diagram below shows the arrangement of the atoms in each layer, and the way the layers are spaced. Graphite: Graphite has a planar structure. Weight of diamond is expressed in terms of carats.

Diamond has stronger intramolecular bonds than graphite. One carat is equal to 0.2 g or 200 mg. The key difference between diamond graphite and fullerene is that diamond has a diamond cubic crystal structure and graphite has a hexagonal crystal structure, while fullerene occurs as a large spheroidal molecule.. Diamond, graphite and fullerene are different allotropes of the chemical element carbon.

Atomic Structure.

Graphite has a giant covalent structure in which: What is the Structure of Graphite?. Therefore, diamond has a higher boiling point. It can be written C (gr) but is usually written as just C.. Therefore, as carbon had only made 3 bonds, the other free electron floats freely between two layers of carbon plates ( see below ). The crystal structure of diamond is an infinite three-dimensional array of carbon atoms, each of which forms a structure in which each of the bonds makes equal angles with its neighbours.

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Graphite also has a lower density (2.266 grams per cubic centimeter) than diamond. They both have giant structures of carbon atoms , joined together by covalent bonds . All these compounds have only carbon atoms in the composition, but the … Structure and bonding.

Graphite is said to exhibit low electrical conductivity with a low density of about 2.26 g/cm3. Graphite can be converted into diamonds by the action of high temperature (~ 2000 0 C ) and high pressure (100000 atmosphere) in the presence of transition metals (such as platinum).The artificial diamonds, however, are small in size and generally grey in colour and hence cannot be used as gems.

The structure of graphite is as follows: In graphite, unlike diamond, each carbon atom is bonded to three other carbon atoms as shown in the figure. Diamond: Diamond is transparent. Every layer has atoms of carbon arranged in a honeycomb-like a network with the division of 0.142 nm with 0.335 nm distance between planes. In diamond, all the carbon atoms have strong chemical bonds to four other carbon atoms, making perfect tetrahedra on and on throughout the crystal. Diamond and graphite are allotropes of carbon.

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