Diamond is hard but graphite is soft. Why?

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Solution

Any carbon atom in a diamond is bound to four other carbon atoms results in the strong tetrahedral arrangement. In graphite, a carbon atom is bound to three other carbon atoms. It forms hexagonal sheets which are comparatively weakly bonded to each other and thus, they can slip a pass to each other. Due to this, diamond is hard but graphite is soft.

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Answer the following questions :

(a) Why is graphite a good conductor of electricity but not diamond ?

(b) Why is diamond very hard ?

(d) What impurity is present in black diamond ?

(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'.

(a) What is the unique property of carbon atom? How is this property helpful to us?
(b) Explain why diamond is hard while graphite is soft (though both are made of carbon atoms).

(a) What is buckminsterfullerene? How is it related to diamond and graphite?
(b) Why is diamond used for making cutting tools (like glass cutters) but graphite is not?
(c) Why is graphite used for making dry cell electrodes but diamond is not?

Q. Graphite is soft but diamond is very hard. why

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