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Both diamond and silicon dioxide have a giant covalent structure which is a very large 3D network of atoms held together by strong covalent bonds. Diamond has a giant covalent structure with strong covalent bonds between the atoms which need a lot of energy to break. Diamond is very hard as each carbon atom is held in a rigid tetrahedral arrangement by strong covalent bonds where each carbon atom has 4 covalent bonds. Diamond cannot conduct electricity as has no delocalised electrons or ions which are free to move.

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