Ionic Bonding

Ionic Bonding

1. Why do atoms bond?

   • They want to be stable
   • To have a full outer shell of electrons
     • Metals lose electrons
       • Form positive cations
     • Non-metals gain electrons
       • Form negative anions

2. Making Sodium Chloride

3. Giant Ionic Compounds

   • Held together by lots of strong electrostatic forces between positive and negative ions
     • Lots of energy needed to break these forces
       • High melting point
       • Hard
   • Don't conduct when solid
     • Positions of ions are fixed, no moving charge
   • Conduct when melted or dissolved in water
     • Ions can move, so can carry charge

4. Ionic formula

   • K+1 + Cl-1
     • K1 + Cl1
       • KCl
   • Note: Charges with numbers should be on the top right of the elements
   • Pb+4 + O-2
     • Remove the charges
       • Pb4 + O2
         • Cross and drop when numbers are different
           • Pb2O4
             • Note: Numbers should now be on the bottom right of the elements
             • Can be simplified to PbO2

5. You can get the charge of an element by looking at what group it belongs to

   • Group 1 = +1
   • Group 2 = +2
   • G3 = +3
   • G5 = -3
   • G6 = -2
   • G7 = -1
   • Ignore groups 4 & 8/0 as they don't usually form ionic bonds

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