Metallic Bonding

• Metallic bonding is represented by a 2-D lattice diagram.
• Metals consist of giant structures of atoms arranged in a regular pattern.
• The electrons in the outer shell of metal atoms are delocalised and so are free to move through the whole structure.
• The sharing of delocalised electrons gives rise to strong metallic bonds.
• Strong electrostatic attraction exists between negatively charged electrons and positive metal ions.
• Metals typically exhibit physical properties such as electrical conductivity and malleability.
• Metals have giant structures of atoms with strong metallic bonding.
• Most metals have high melting and boiling points due to their giant structures of atoms with strong metallic bonding.
• Metals can conduct heat and electricity because of the delocalised electrons in their structures.
• The layers of atoms in metals are able to slide over each other, so metals can be bent and shaped.