1(g) Covalent Bonding

properties of diamond + why (2)

hard - tetrahedron structure, each atom is bonded to 4 others

high melting point - strong covalent bonds which require lots of energy to overcome

properties of graphite + why (3)

soft + slippery - layers can easily slide over each other because there are only weak forces between the layers, not covalent bonds

conducts electricity - one electron per carbon atom is delocalised, charged particles that are free to move

high melting point - giant covalent structure, strong covalent bonds require lots of energy to break

properties of graphene + why (3)

high melting point - strong covalent bonds require lots of energy to break

strong - hexagon structure, strong covalent bonds

conducts electricity - delocalised electrons

properties of buckminster fullerene (C₆₀) (2)

slippery + low melting point - weak intermolecular forces, little energy to overcome