🎯 Common Question Types:
- Explain how metals conduct electricity (2 marks)
- Explain why metals are malleable and ductile (2 marks)
- Compare electrical conductivity of metals vs ionic compounds (2-3 marks)
- Predict which of two metals has higher melting point and explain why (2 marks)
📝 Key Command Words:
- Explain: Reference "delocalised electrons free to move" for conductivity
- Explain: Reference "layers of ions slide, electron sea maintains bond" for malleability
- Compare: State the key difference — metals conduct as solids, ionic compounds do not
- Predict: Apply the rules about charge and electron numbers to predict relative MP
⚠️ Common Mistakes to Avoid:
- Saying "free ions" conduct in metals — it's FREE ELECTRONS, not ions
- Saying "metallic bonds break" when a metal deforms — the bond does NOT break, ions slide within the electron sea
- Confusing metallic bonding with covalent bonding — metallic has a sea of electrons, covalent has specific shared pairs
- Not using the word "delocalised" — this is the key exam term for metallic bonding
This exam tips covers Exam Tips for 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 11 of 12 in this topic. Treat this as a marking guide for what examiners are looking for, not just a fact list.
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 is metallic bonding?
Electrostatic attraction between positive metal ions and a sea of delocalised electrons
What are delocalised electrons?
Electrons that are free to move throughout the metal structure (not attached to one atom)