• Metal atoms are held together strongly by metallic bonding
• Within the?metal lattice, the atoms lose their valence electrons and become positively charged
• The valence electrons no longer belong to any metal atom and are said to be?delocalised
• They move freely between the positive metal ions like a sea of electrons
• Metallic bonds are strong and are a result of the attraction between the positive metal ions and the negatively charged delocalised electrons

Diagram showing metallic lattice structure with delocalised electrons

The link between metallic bonding and the properties of metals

• Metals have?high?melting and boiling points
  • There are many?strong?metallic?bonds?in giant metallic structures
  • A lot of heat energy is needed to overcome forces and break these bonds

   

• Metals?conduct?electricity
  • There are?free?electrons?available to move and carry charge
  • Electrons entering one end of the metal cause a delocalised electron to displace itself from the other end
  • Hence electrons can flow so electricity is conducted

   

• Metals are?malleable?and?ductile
  • Layers of positive ions can?slide?over one another and take up different positions
  • Metallic bonding is not disrupted as the valence electrons do not belong to any particular metal atom so the delocalised electrons will move with them
  • Metallic bonds are thus not broken and as a result metals are strong but?flexible
  • They can be hammered and bent into different shapes without breaking

   

Summary Table of the Physical Properties of Metals

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