Diamond and graphite are of carbon?

Answer 1

Diamond and graphite are both composed of carbon, but they are physically different from each other. Diamond is the hardest mineral known, is usually transparent and very abrasive. Graphite on the other hand, is soft, opaque and a very good lubricant.

Answer 2

The atoms are bonded and arranged differently. In graphite, the carbon atoms are sp2 hybridized and each carbon atom is directly bonded to three others. This forms flat sheets of carbon atoms arranged in hexagons (kind of like chicken wire) where the individual layers are fairly strong, but there are only weak interactions between the layers. This gives graphite some interesting properties; it's significantly stronger in some directions than in others and the electrical conductivity is low in the direction perpendicular to the layers but fairly good in the directions parallel to the layers. In diamond, the carbon atoms are sp3 hybridized and each carbon atom is bonded to four others in a tetrahedral lattice. In a perfect crystal of diamond, you could get from any carbon atom to any other carbon atom in the crystal by following a series of covalent bonds; you never have to jump through space like you would to get from one graphite layer to another. This network of covalent bonds makes diamond extremely strong.

Answer 3

Yes, both diamond and graphite are allotropes of carbon, meaning they are different forms of the same element. They have different structures due to the arrangement of carbon atoms, leading to different physical properties despite being composed entirely of carbon. Diamond has a 3D tetrahedral structure, making it hard and transparent, while graphite has a 2D layered structure, making it soft and a good conductor of electricity.

Answer 4

Diamond, Graphite, Soot and Graphene are all different forms of Carbon.

Answer 5

Diamond and graphite are allotropes of carbon.

Answer 6

Yes.