Diamond and graphite
Lesson 7 / 8
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I can describe the properties of diamond and graphite and explain how they result from their giant covalent structures, as well as relate them to their uses.
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In diamond each carbon atom is bonded to four others with strong covalent bonds to form a giant covalent structure.
Diamond is very hard, has a very high melting point and does not conduct electricity (makes it good for cutting tools).
In graphite, each carbon atom is covalently bonded to three others to form layers of hexagonal rings.
There are only weak forces between the layers in graphite which can easily be rubbed apart (makes it a good lubricant).
Graphite conducts electricity because it has delocalised electrons which can move and carry charge/current.
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