This topic summary covers Knowledge Organiser: Metallic Bonding 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 12 of 12 in this topic. Use this topic summary to connect the idea to the wider topic before moving on to questions and flashcards.
Knowledge Organiser: Metallic Bonding
Key Terms
- Metallic bond: attraction between positive metal ions and delocalised electrons
- Delocalised electrons: free electrons not fixed to any atom
- Sea of electrons: the mobile electron cloud in a metal
- Malleable: can be hammered into shape
- Ductile: can be drawn into wire
- Alloy: mixture of metals (or metal + non-metal); harder than pure metal
Must-Know Facts
- Positive metal ions surrounded by sea of delocalised electrons
- Conducts electricity — delocalised electrons carry charge
- Conducts heat — electrons transfer kinetic energy
- Malleable/ductile — layers slide, electrons maintain bond
- High MP — strong attraction between ions and electrons
- Conducts as a SOLID (unlike ionic compounds)
- Alloys harder — different-sized atoms disrupt regular layers, preventing sliding
- Steel (Fe+C), brass (Cu+Zn), bronze (Cu+Sn)
Key Equations
- No calculation equations — descriptive topic
- Metallic bond = electrostatic attraction between positive metal ions and delocalised electrons
- Conductivity: delocalised electrons move freely and carry charge/energy
Common Mistakes
- Saying metals conduct due to free ions: Metals conduct because of DELOCALISED ELECTRONS — not free ions (that is ionic compounds in solution)
- Saying pure metals are harder than alloys: Alloys are harder — different-sized atoms disrupt the regular lattice, preventing layers from sliding
- Forgetting metallic bonds are strong: Students often say metals have weak bonds — metallic bonds are actually strong, giving metals high melting points
- Saying metals are brittle: Metals are malleable and ductile because layers can slide without breaking bonds (unlike ionic compounds which are brittle)
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