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Diamond structure and properties explained

Bonding, structure and the properties of matter • Structure and bonding of carbon

Key concepts

What you'll likely be quizzed about

  • In diamond, each carbon atom forms four single covalent bonds directed towards the corners of a tetrahedron.
  • This arises from the sp3 hybridisation of carbon orbitals.
  • The tetrahedral units become interconnected, forming a large, continuous three-dimensional giant covalent lattice.

Flashcards

Test your knowledge with interactive flashcards

What is the effect of strong directional bonds on mechanical properties?

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Strong directional bonds contribute to extreme hardness but create planes along which the lattice can cleave, resulting in brittleness.

Key notes

Important points to keep in mind

Each carbon atom forms four covalent bonds (sp3), producing a tetrahedral geometry.

Diamond is a giant covalent lattice rather than a molecular substance.

All valence electrons are localised in bonds, making diamond an electrical insulator except when doped.

Strong covalent bonds throughout the lattice result in extreme hardness and a very high melting point.

Directional bonding makes diamond hard but also creates cleavage planes that cause brittleness.

Efficient phonon transfer and light atomic mass contribute to high thermal conductivity.

Diamond remains insoluble because solvents cannot break the extensive covalent network.

Impurities or defects can alter electrical behavior; for example, boron-doped diamond becomes conductive.

Diamond oxidises to carbon dioxide at high temperatures in air.

Gem-quality optical effects arise from transparency, high refractive index, and strong dispersion.

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