- Metallic bonding = electrostatic attraction between positive metal ions and delocalised electrons
- Delocalised electrons = electrons free to move throughout the metal (not fixed to one atom)
- Conducts electricity — delocalised electrons can move and carry charge
- Conducts heat — electrons transfer thermal energy rapidly
- Malleable — can be hammered into shape; layers slide, electrons move to maintain bond
- Ductile — can be drawn into wires; same reason as malleable
- High melting point — strong attraction between ions and electron sea
- Can conduct in solid state — unlike ionic compounds!
This key facts covers Key Facts to Memorise within Metallic Bonding for GCSE Chemistry. Revise Metallic Bonding in Bonding & Structure for GCSE Chemistry with 22 exam-style questions and 21 flashcards. This is a high-frequency topic, so it is worth revising until the explanation feels precise and repeatable. It is section 6 of 12 in this topic. Use this key facts to connect the idea to the wider topic before moving on to questions and flashcards.
Practice questions for Metallic Bonding
In metallic bonding, what are the electrons called that are free to move throughout the metal structure?
Explain why metals are malleable.
Quick recall flashcards
What are delocalised electrons?
Electrons that are free to move throughout the metal structure (not attached to one atom)
What is metallic bonding?
Electrostatic attraction between positive metal ions and a sea of delocalised electrons