Bonding

Bonding

Ionic Bonding
1. Metals and Non-Metals
2. Electrons go from Metal to Non-Metal
3. Mg + O -->MgO
4. Ions are created, not Atoms
  1. Ions are Charged Atoms
    1. Metal
      1. Posotive
      2. Lost Electrons
    2. Non-Metal
      1. Negative
      2. Gained Electrons
5. Opposites Attract
  1. So the opposite charge of the Ions attract each other
Covelent Bonding
1. Non-Metals only
2. They share electrons
3. Can have single or double bonds
  1. Double are stronger
4. Giant Covelent Structures
  1. Graphite
    1. Each Carbon Atom is only bonded to 3 others
      1. Free Electons
    2. Layerd in structure
    3. Conducts Electrisity
      1. Free Electrons
  2. Silcone Dioxide
    1. Very High melting point
    2. Semi-conductor
    3. Similar Structure to diamond
  3. Diamond
    1. Each Carbon is bonded to 4 other Atoms
    2. Very high melting point
    3. Very hard
      1. Due to really strong bonds
    4. Does not conduct electrisity
  4. Graphite, Diamond and Silicone Dioxide
5. The sharing keeps them bonded
  1. Attracted Together
Metalic Bonding
1. Metals Only
  1. Examples would be Copper
2. De-localised Electons
  1. Form a "Sea of Electons"
    1. Acts like glue to keep the posotive Metal Ions attracted
    2. What makes Metals Shiny
    3. This conducts electrisity
      1. The de-localised electrons carry the charge
3. Forms layered (lattice) structure
  1. Can slide over each other
    1. Malleable
    2. However, in Alloys, this does not happen
      1. An Alloy is a mixture of Metals
      2. Makes it more brittle

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	Created by Alex Maraio over 10 years ago