Bonding

Bonding

1. Ionic Bonding

   • Metals and Non-Metals
   • Electrons go from Metal to Non-Metal
   • Mg + O -->MgO
   • Ions are created, not Atoms
     • Ions are Charged Atoms
       • Metal
         • Posotive
         • Lost Electrons
       • Non-Metal
         • Negative
         • Gained Electrons
   • Opposites Attract
     • So the opposite charge of the Ions attract each other

2. Covelent Bonding

   • Non-Metals only
   • They share electrons
   • Can have single or double bonds
     • Double are stronger
   • Giant Covelent Structures
     • Graphite
       • Each Carbon Atom is only bonded to 3 others
         • Free Electons
       • Layerd in structure
       • Conducts Electrisity
         • Free Electrons
     • Silcone Dioxide
       • Very High melting point
       • Semi-conductor
       • Similar Structure to diamond
     • Diamond
       • Each Carbon is bonded to 4 other Atoms
       • Very high melting point
       • Very hard
         • Due to really strong bonds
       • Does not conduct electrisity
     • Graphite, Diamond and Silicone Dioxide
   • The sharing keeps them bonded
     • Attracted Together

3. Metalic Bonding

   • Metals Only
     • Examples would be Copper
   • De-localised Electons
     • Form a "Sea of Electons"
       • Acts like glue to keep the posotive Metal Ions attracted
       • What makes Metals Shiny
       • This conducts electrisity
         • The de-localised electrons carry the charge
   • Forms layered (lattice) structure
     • Can slide over each other
       • Malleable
       • However, in Alloys, this does not happen
         • An Alloy is a mixture of Metals
         • Makes it more brittle

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