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Diamonds

Diamonds. Diamond Structure & Bonding Structure : Giant covalent macromolecule Bonding : Each carbon atom has 4 bonding pairs of electrons and 0 lone pairs of electrons. According to VSEPR theory in order to minimize the repulsion the 4 pair of bonding electrons repel each other equally.

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Diamonds

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  1. Diamonds

  2. Diamond Structure & Bonding Structure: Giant covalent macromolecule Bonding: Each carbon atom has 4 bonding pairs of electrons and 0 lone pairs of electrons. According to VSEPR theory in order to minimize the repulsion the 4 pair of bonding electrons repel each other equally. Bond angle: 109.5o Shape: tetrahedral No intermolecular forces of attraction, only intramolecular attractions between the carbon atoms. 

  3. Physical Properties of Diamond  • Hardness: • Hardest substance known • Each carbon atom is held in the lattice by 4 strong covalent bonds, making diamond a strong rigid structure. • The carbon – carbon bonds can only be broken up by another diamond. • Because of their hardness diamonds have many applications in industry. Parts of cars, planes, and other machines are shaped by diamonds.

  4. Solubility in water : The covalent bonds between the carbon atoms are much stronger than the force of attraction exerted by polar water molecules. Diamond is not soluble in water. Melting Point: To break the strong intramolecular covalent bonds requires a large amount of energy, therefore they have very high temperature. M.pt of diamond 4000oC

  5. Conductivity of electricity: All four outer valence electrons in in each C atom are involved in forming covalent bonds with four other C atoms. Therefore the valence electrons are not free to move making diamond a non conductor of electricity.

  6. Physical properties of diamond explained by considering the structure and bonding

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