# data[].attributes.body
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# data[].attributes.body
1. Diamond is strong because each carbon atom is linked to four other carbon atoms by covalent compounds.
In graphite only 3 Valence electrons of each carbon atom in graphite are used in bond formation. The fourth Valence electrons

# data[].attributes.body
1.

# data[].attributes.body
1)diamond is stronger because it has stronger covalent bonds among its carbon atoms while graphite has weaker covalent bonds.
2)the compact and rigid three dimensional arrangements of carbon atoms in diamond give it a high density.
3)

# data[].attributes.body
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# data[].attributes.body
Diamond has strong covalent bonds among its carbon particles. This causes diamond to have a very high density and to be very hard. Graphite carbon structures are weak as they are present as sheets in a hexagonal form with weak bonds between that can be slid over.

Diamond has a higher melting point due to the strong force of attraction between their carbon structures due to their covalent bonds.

Graphite has loose electrons that conduct electricity with ease, while diamond has a strong structure.

# data[].attributes.headline
1.	Explain why, diamond is hard while graphite is soft.                                    2.	Explain why diamond has a high melting point. 3.	Why is graphite a good conductor of electricity but diamond is a non-conductor of electricity?

# data[].attributes.subject
1.	Explain why, diamond is hard while graphite is soft.                                    2.	Explain why diamond has a high melting point. 3.	Why is graphite a good conductor of electricity but diamond is a non-conductor of electricity?