Explain the difference in properties of diamond and graphite on the basis of their structures.

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Solution

The difference between diamond and carbon is given below.
Diamond Graphite
It has crystalline nature
It has layered structure
Each C is $s p^{3}$ hybridzed and forms 4 covalent bonds with neighboring C atoms.
Each C atom is $s p^{2}$ hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
The geometry is tetrahedral.
The geometry is planar
C-C bond length is 154 pm
C-C bond length is 141.5 pm
It has rigid covalent boning which is difficult to break.
It is soft. Its layers can be separated easily.
It is an electrical insulator.
It is good conductor of electricity.

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Explain the difference in properties of diamond and graphite on the basis of their structures.

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Explain the difference between Diamond and graphite.

(a) Write two points of difference in the structures of diamond and graphite.
(b) Explain why graphite can be used as a lubricant but diamond cannot.
(c) Explain why diamond can be used in rock drilling equipment but graphite cannot.
(d) State one use of diamond which depends on its 'extraordinary brilliance' and one use of graphite which depends on its being 'black and quite soft'.

Q. Compare the structures of Diamond and Graphite.

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Diamond	Graphite
It has crystalline nature	It has layered structure
Each C is $s p^{3}$ hybridzed and forms 4 covalent bonds with neighboring C atoms.	Each C atom is $s p^{2}$ hybridized and forms 3 sigma bonds with 3 other C atoms. Fourth electron forms pi bond.
The geometry is tetrahedral.	The geometry is planar
C-C bond length is 154 pm	C-C bond length is 141.5 pm
It has rigid covalent boning which is difficult to break.	It is soft. Its layers can be separated easily.
It is an electrical insulator.	It is good conductor of electricity.