Differentiate between -
Diamond and Graphite

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Solution

Diamond Graphite
In diamond, each Carbon atom is covalently bonded with four Carbon atoms. In graphite, each Carbon atom is covalently bonded with three Carbon atoms.
Due to the absence of free electrons, diamond is a bad conductor of electricity. Due to presence of free electrons, graphite is a good conductor of electricity.
Diamond is a the hardest known natural substance. Graphite is soft and slippery.
Diamond is used to cutting metals and glasses. Graphite is used in making lubricants.

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Diamond	Graphite
In diamond, each Carbon atom is covalently bonded with four Carbon atoms.	In graphite, each Carbon atom is covalently bonded with three Carbon atoms.
Due to the absence of free electrons, diamond is a bad conductor of electricity.	Due to presence of free electrons, graphite is a good conductor of electricity.
Diamond is a the hardest known natural substance.	Graphite is soft and slippery.
Diamond is used to cutting metals and glasses.	Graphite is used in making lubricants.