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Diamond and graphite are both covalent structures. Diamond has a tetrahedral arrangement of 5 carbon atoms. Graphite has a hexagonal structure with each carbon atom connected to three others. Diamond is very hard, while graphite is soft. They both have high melting and boiling points. Diamond is an insulator since it has no mobile electrons. Graphite is a conductor due to having valence electrons that are not all used in covalent bonding. This allows them to be delocalized across the planes of carbon atoms.

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