GCSE Chemistry · AQA 8462 · Topic 4.2
Bonding, structure, and the properties of matter
Key points
- There are three types of strong chemical bond: ionic (metal + non-metal, electrons transferred), covalent (non-metals sharing pairs of electrons) and metallic (positive ions in a sea of delocalised electrons).
- Ionic compounds form giant lattices, have high melting points and conduct electricity when molten or dissolved.
- Simple molecules have low melting and boiling points because only weak intermolecular forces need to be overcome; they do not conduct electricity.
- Giant covalent structures such as diamond, graphite and silicon dioxide have very high melting points.
- Metals conduct electricity and heat and are malleable; alloys are harder because different-sized atoms distort the layers.
- Carbon forms diamond, graphite, graphene and fullerenes, each with different properties.
- Nanoparticles (1–100 nm) have a very high surface area to volume ratio, giving new uses and possible risks.
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Why is salt a hard crystal while water is a liquid and copper bends without breaking? This topic answers that by linking the way particles are bonded to the properties we can see and measure.
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