Diamond structure

• • Diamond and graphite are allotropes of carbon
• Allotropes

  Different atomic or molecular arrangements of the same element in the same physical state.
• • In diamond, each carbon atom bonds with four other carbons atoms, forming a tetrahedron
  • All the covalent bonds are identical, very strong and there are no intermolecular forces

  
• • Diamond does not conduct electricity
  • All the outer shell electrons in carbon are held in the four covalent bonds around each carbon atom
  • As a result, there are no freely moving electrons to carry a charge
• • Diamond has a very high melting point
  • Diamond has a giant covalent structure
  • There are strong covalent bonds between the carbon atoms
  • These need lots of energy to break 
• • It is extremely hard and dense
  • It has strong covalent bonds
  • Diamond's hardness makes it very useful in cutting tools like drills 
• Diamond is the hardest naturally occuring mineral, but it is by no means the strongest.