GCSE Chemistry · Edexcel 1CH0 · Topic 1C
Ionic, covalent and metallic bonding
Key points
- Ionic bonding: a metal transfers electrons to a non-metal, forming oppositely charged ions held by strong electrostatic forces in a giant lattice. High melting points; conduct when molten or dissolved, not when solid.
- Ion names: -ide for simple ions (chloride), -ate for ions with oxygen (sulfate , nitrate ).
- Covalent bonding: non-metal atoms share pairs of electrons. Simple molecules (e.g. water, CO₂) have weak intermolecular forces, so low melting points and no conductivity.
- Giant covalent structures (diamond, graphite, silicon dioxide) have very high melting points. Graphite conducts because it has delocalised electrons; diamond does not. Graphene and fullerenes are other forms of carbon.
- Metallic bonding: positive metal ions in a sea of delocalised electrons. Metals conduct and are malleable because layers can slide.
- Each bonding model has limits, e.g. dot and cross diagrams do not show shape.
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Atoms join together by transferring or sharing electrons, and the type of bonding decides a substance's structure and properties. These notes cover ionic, covalent and metallic bonding, the main structures, and how to explain properties…
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