1(g) Covalent Bonding
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4 Terms
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
Note 
Flashcards (50)