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Metallic Bonding (CIE IGCSE Chemistry: Co-ordinated Sciences (Double Award))
Revision Note
Metallic bonding
Extended tier only
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
Diagram to show metallic bonding
Diagram showing metallic lattice structure with delocalised electrons
Properties of metals
Extended tier only
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
Malleability of metals
When a force is applied, the layers of positive ions slide over each other
Exam Tip
When explaining why metals can conduct electricity, be careful of the terminology you use. Don't get confused with ionic compounds.
Metals can conduct electricity as they have free electrons that can carry charge whereas molten or aqueous ionic compounds can conduct electricity because they have free ions that can carry charge.
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