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The difference in properties between diamond and graphite is primarily due to their distinct atomic structures. In diamond, each carbon atom is tetrahedrally bonded to four other carbon atoms, creating a strong three-dimensional network that results in high hardness and a brilliant luster. In contrast, graphite has a planar structure where each carbon atom is bonded to three others in flat sheets, with weaker van der Waals forces between the layers, allowing them to slide over each other. This structural variation accounts for diamond’s rigidity and brilliance compared to graphite’s softness and conductivity.

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