Difference between diamond and graphite
Answers
Hey !!
DIAMOND
Diamond is very hard.
It has high density.
It is a bad conductor of electricity but good conductor of heat than graphite.
It possesses three dimensional net work structure.
Chemical reactivity is low.
Carbon undergoes sp³ hybridisation.
C--C bond length is 154 pm.
GRAPHITE
Graphite is soft.
It has relatively low density.
It is good conductor of heat and electricity.
It possesses a sheet type structure.
Chemical reactivity is high.
Carbon undergoes sp² hybridisation.
C--C bond length 142 pm.
GOOD LUCK !!
Answer:
(A) Hardness : Diamond is very hard, whereas graphite is soft.
(1) Diamond has three dimensional network of sp^3- hybridised carbon atoms joined by extended covalent bonds which are difficult to break.nHence diamond is hard and used as an abrasive.
(2) Graphite has two dimensional sheet like structure, like layers of hexagonal rings from sp^2-hybridised carbon atoms. These layers are held by weak van der Waals forces, which can be broken easily. Hence graphite is soft and slippery and used as lubricant.
(B) Conduction of electricity :
(1) Diamond is a non-conductor of electricity as itndoes not have any mobile, delocalised electronsnin its structure since all electrons are involved inncovalent bonding.
(2) Graphite has delocalised electrons which are mobile all over the sheet like structure of graphite. These electrons conduct electricity. Hence graphite is a good conductor of electricity.