Graphite conducts electricity while diamond does not because in graphite
Correct answer: D. each carbon uses only three of its four valence electrons in bonding, leaving one delocalised
- A. each carbon forms four single covalent bonds
- B. the carbon atoms are ionised
- C. the layers are held by strong covalent bonds
- D. each carbon uses only three of its four valence electrons in bonding, leaving one delocalised
Explanation
In graphite each carbon is bonded to three others in a flat hexagonal sheet, and the fourth electron is delocalised between the layers, so it can carry current along the sheets. In diamond all four electrons are locked into single bonds, leaving none free. The weak forces between graphite layers also let them slide, which is why graphite is used as a lubricant and in pencils.
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About Crystalline Solids
Crystalline solids contain particles arranged in a regular repeating lattice described by a unit cell. Their study includes coordination number, packing efficiency, density, anisotropy, cleavage, polymorphism and common crystal systems, along with ionic, molecular, covalent network and metallic crystals. Crystalline order differs from the random arrangement of amorphous solids.
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