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Most non-metals exist as simple covalent molecules. In the solid state, the molecules are held together in a simple molecular lattice structure by weak intermolecular bonds.
Carbon and silicon have a different structure. Their atoms are held together in a giant covalent lattice by strong covalent bonds.
Substances with giant covalent lattice structures have high melting and boiling points because a lot of energy is needed to break the strong covalent bonds. They are insoluble in almost all solvents and are non-conductors of electricity.
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Key terms in this lesson
- Covalent bond
- A strong electrostatic attraction between a shared pair of electrons and the nuclei of the bonded atoms.
- Electron pair repulsion theory
- The theory that electron pairs around a central atom arrange themselves as far apart as possible to minimise repulsion, determining the shape of the molecule or ion.
More in Bonding
- Four Pairs of Electrons
- Five Pairs of Electrons
- Six Pairs of Electrons
- Bonding-Pair Lone-Pair Repulsion
- Heating a Solid, Liquid or Gas
- Crystals
- Graphite and Graphene
- Fullerenes
All 30 lessons in Bonding · All AQA AS-level Chemistry topics