Metallic bonding

• Do metals exist as single atoms?

  No, they exist as giant metallic lattices
• How do metals exist ?

  As giant metallic lattices
• metallic bond

  The strong electrostatic force of attraction between positive metal ions and the sea of delocalised electrons
• The strength of a metallic bond is based on

  -charge of ion

  -size of ion

  -number of delocalised electrons per atom
• Metallic bond is stronger when

  Ion is more charged, smaller ion, and ion has more delocalised electrons per atom so there is stronger electrostatic forces of attraction between the positive metal ions and sea of delocalised electrons
• Metals atoms become ______ charged ions

  Positively
• How do metal atoms become positively charged ions?

  They lose electrons. These lost electrons form a sea of delocalised electrons
• Properties of metals

  -high melting points (exist as solid at room temperature, except mercury (Hg))

  -conducts electricity

  -insoluble

  -malleable/ductile

  -are good thermal conductors
• Why do metals have high melting points?

  They have a giant metallic lattice structure held together by strong electrostatic forces of attraction between the positively charged metal ions and the sea of delocalised electrons so a lot of energy is required to overcome these bonds
• Why can metals conduct electricity?

  Because delocalised electrons are free to move and carry a current
• Why are metals insoluble?

  Because polar molecules cannot break apart the lattice as the metallic bond is too strong to break
• Why are metals malleable/ductile?

  The layers of positive metal ions can slide over each other without breaking apart
• Why are metals good conductors of heat?

  Because delocalised electrons are free to move and can transfer kinetic energy
• The more electron a metal atom can donate to the delocalised system ...

  The higher the melting point
• Which bond is stronger, ionic or metallic ?

  Ionic