what is the impact of structures on physical properties of two allotropes of carbon
Answers
In a diamond, the carbon atoms are arranged tetrahedrally. Each carbon atom is attached to four other carbon atoms 1.544 x 10-10 meter away with a C-C-C bond angle of 109.5 degrees. It is a strong, rigid three-dimensional structure that results in an infinite network of atoms. This accounts for diamond's hardness, extraordinary strength and durability and gives diamond a higher density than graphite (3.514 grams per cubic centimeter). . It is the best conductor of heat that we know, conducting up to five times the amount that copper does. Diamond also conducts sound, but not electricity; it is an insulator, and its electrical resistance, optical transmissivity and chemical inertness are correspondingly remarkable.
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If it's graphite and diamond...
Graphite has low melting point than that of diamond.
In graphite, every carbon atom is bonded with three other carbon atoms, while, in diamond, every carbon atoms are bonded with four carbon atoms.
This makes diamond more harder in its physical state than that of graphite and is known as the hardest natural substance in the earth.
As graphite has one bond free, i.e., it has three bonds, electrons are able to move within it and this physical property enables it to conduct electricity.
The structure of graphite if that of hexagonal columns, while, the structure of diamond is like that of a tetrahedron.
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