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Paper 1
Bonding, Structure, and Properties
Both
Metallic bonding explains conductivity and malleability.
Key Facts
- Graphite conducts because of delocalised electrons.
- Diamond is hard due to a giant covalent lattice.
Topics Covered
Ionic Bonding
What you need to know
- •Metals lose electrons; non-metals gain electrons.
- •Ions form a giant lattice with strong electrostatic forces.
Exam Tips
- Explain properties using lattice and strong attraction.
Covalent Bonding
What you need to know
- •Non-metals share electrons.
- •Simple molecules have low melting points.
Exam Tips
- Mention weak intermolecular forces for simple molecules.
Metallic Bonding
What you need to know
- •Positive ions in a sea of delocalised electrons.
- •Explains electrical conductivity and malleability.
Exam Tips
- Use the phrase "delocalised electrons."
Key Terms
Ionic bond
Electrostatic attraction between oppositely charged ions.
Covalent bond
A shared pair of electrons between atoms.
Metallic bond
Attraction between positive ions and delocalised electrons.
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Common Exam Questions
Explain why metals conduct electricity.
3 markseasyPaper 1
Model Answer
Metals contain delocalised electrons that are free to move and carry charge.
What examiners want to see
- ✓Mention delocalised electrons.
- ✓Link to charge flow.
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