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COVALENT NETWORKS - Diamond, Graphite and Silicon Dioxide (Hardness…
COVALENT NETWORKS - Diamond, Graphite and Silicon Dioxide
Hardness
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Graphite
The delocalised electrons between the covalently bonded layers form only a weak force of attraction so when force is applied these weak forces can be broken and the layers can slide over one another
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Conductivity
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Graphite
For any substance to conduct there must be mobile charged particles and in graphite the delocalised electrons (negatively charged) are able to move and therefore graphite can conduct
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Melting Point
Diamond
High melting and boiling point of 3,700 C
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Graphite
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The layers of carbon atoms are bonded by strong covalent bonds and a lot of energy is required to break these
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Diamond is composed of millions of carbon atoms. Each carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral arrangement to form a giant lattice
Graphite is composed of millions of carbon atoms. Each carbon atom in the structure is covalently bonded to 3 other carbon atoms forming layers of covalently bonded carbon atoms. Each carbon has an unbonded valence shell electron and these electrons are delocalised and sit between the layers creating a weak force which holds the layers together.