The structure of a metal

Metals consist of giant structures

• Within the metal lattice, the atoms lose their outer electrons and become positively charged metal ions

  • The outer electrons no longer belong to any specific metal atom and are said to be delocalised

  • This means they can move freely between the positive metal ions and act like a “sea of electrons”

• The metallic bond is the strong force of attraction between the positive metal ions and the delocalised electrons

• This type of bonding occurs in metals and metal alloys, which are mixtures of metal

Properties of metals

What are the properties of metals?

Most metals have high melting and boiling points 

• There are strong electrostatic forces of attraction between the positive metal ions and the negative delocalised electrons within the metal lattice structure

• These needs lots o energy to be broken 

• Metals are good conductors of heat and electricity 

  • The delocalised electrons are free to move and carry a charge through the whole structure 

• Most metals are malleable

  • This means they can be hammered into shape

  • This is because the atoms are arranged in layers which can slide over each when force is applied