Metallic Bonding (Edexcel IGCSE Chemistry)
Revision Note
Written by: Stewart Hird
Reviewed by: Lucy Kirkham
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Metallic bonding
Metals consist of giant structures of atoms arranged in a regular pattern
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
Metallic bonding
Metallic bonds exist between positive metal ions and delocalised electrons
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 of energy to be broken
Metals conduct electricity
There are delocalised electrons available to move and carry charge
Most metals are malleable
This means they can be hammered into shape
This is because the atoms/ions are arranged in layers which can slide over each other when a force is applied
The malleability of metals
The atoms are able to slide over each other as they are arranged in layers
Examiner Tips and Tricks
It's very important you are able to explain these three properties and use the correct terminology.
For example, you must refer to atoms/ions in your answer for malleability, not just particles.
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