C2 bonding

C2 bonding

1. Ionic bonding

   • between metals and non metals
   • Forms + and - ions
     • Forms ionic compounds
       • Giant ionic lattices
         • Strong electrostatic forces of attraction
           • High melting and boiling points
           • Can dissolve in water
             • ions free to move conduct electricity

2. Covalent bonding

   • Between 2 non metals
     • simple molecular substances
       • weak inter molecular forces between molecules
         • Very low melting/ boiling points to separates the molecules
           • don't conduct electricity no ions so no electrical charge
     • Giant covalent structures
       • Examples
         • Graphite
           • good conductor
           • 3 covalent bonds
             • each carbon atom 1 delocalised electron.
             • layers free to slide over each over. week intermolecular forces between layers
         • silicon dioxide
         • Diamond
           • each carbon 4 covalent bonds
             • very rigid and strong
       • Very high melting and boiling points
   • sharing electrons
   • Very strong bonds

3. Metalic structures

   • Alloys harder than pure metals
     • different elements have different sizes.
       • distort layers of metal atoms
   • giant structure
     • electrons delocalise
       • allow the layers to slide over each over
       • electrostatic attraction. positive metal ions + negative electrons
       • conducts heat + electricity

4. Isotopes

   • Different atomic forms of the same element. Same number of PROTONS different number of neutrons

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