Question
Diamond is very hard whereas graphite is soft. Explain.
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Answer
Diamond has three$-$dimensional network of $sp^3$ hybridized carbon atoms joined by extended covalent bonds which are difficult to break. Therefore, diamond is hard.
Graphite has two$-$dimensional sheet like structure, like layers of hexagonal rings formed from $sp^2$ hybridized carbon atoms. These layers are held by weak van der Waals forces, which can be broken easily. Therefore, graphite is soft and slippery.
Hence, diamond is very hard whereas graphite is soft.
Graphite has two$-$dimensional sheet like structure, like layers of hexagonal rings formed from $sp^2$ hybridized carbon atoms. These layers are held by weak van der Waals forces, which can be broken easily. Therefore, graphite is soft and slippery.
Hence, diamond is very hard whereas graphite is soft.
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