CARBON STRUCTURES

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  • c.a.r.b.o.n s.tr.uc.tu.re.s
    • d.i.a.m.o.n.d
      • VERY HARD
        • There are many strong covalent bonds
          • Each carbon atom in diamond is bonded to at least 4 other carbon atoms.
            • Creates strong covalent bonds in diamond.
        • Used as a cutting tool for other materials
      • Form of carbon.
      • High Melting Point
        • Lots of energy needed to break strong covalent bonds
          • There are many strong covalent bonds
            • Each carbon atom in diamond is bonded to at least 4 other carbon atoms.
              • Creates strong covalent bonds in diamond.
      • Doesn't Conduct Electricity
        • No delocalised electrons
    • g.r.a.p.h.i.t.e
      • Conducts Electrcity
        • Reason: Each carbon atom forms 3 bonds.
          • 1 electron is delocalised
            • This electron can move freely
              • Conducts Electrcity
                • Reason: Each carbon atom forms 3 bonds.
                  • 1 electron is delocalised
                    • This electron can move freely
        • Soft
          • Carbon atoms=layers of hexagonal rings
            • Held together by weak intermolecular forces
          • Used for pencil lead as it is very lubricant.
        • Covalent Bonds
          • each carbon atom is bonded to 3 other carbon atoms.
            • Creates a giant covalent structure
      • g.r.a.p.h.e.n.e
        • Conducts Electricity
          • Each carbon atom has 1 delocalised electron
          • It is a single layer of graphite
        • Light but Strong
          • One atom thick
          • Strong covalent bonds mean that it is strong
        • u.s.e.s
          • electronics and composite materials.
          • To increase the material's strength without adding more mass
          • Solar panels, batteries etc.

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