Metallic bonding
Metallic bonding
- Metallic bonding is the attraction between positive metal ions and a "sea" of delocalised electrons.
- The outer electrons are free to move through the whole metal.
- This explains key properties of metals.
Practice
Metallic bonding is the attraction between:
In a metal, positive ions sit in a sea of delocalised electrons that hold the structure together.
The sea of electrons
- The metal's outer electrons leave their atoms and are delocalised — free to move.
- This explains why metals conduct electricity and are strong.
Practice
Metals conduct electricity because:
The delocalised electrons can move through the metal, carrying charge.
Practice
Metallic bonding helps explain why metals are strong.
The strong attraction between the positive ions and the electron sea makes metals strong.
You've got it
Key idea
- metallic bonding = attraction between positive metal ions and a sea of delocalised electrons
- the delocalised electrons are free to move → metals conduct electricity and are strong