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Graphite structure, bonding and physical properties

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

Key concepts

What you'll likely be quizzed about

  • Graphite features a two-dimensional arrangement of carbon atoms in hexagonal rings, forming flat sheets called layers.
  • Layers stack in parallel, creating bulk material with regular repeating hexagons.
  • Each carbon atom resides at a vertex, resulting in a planar lattice with defined spacing between layers.
  • Layer stacking causes anisotropy in physical properties: strong bonding exists within sheets, while weak attractions between sheets produce different behaviors along and across the layers.
  • The layer spacing limits interlayer interactions, facilitating layer sliding during mechanical stress.

Flashcards

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What property of graphite makes it useful in electrodes?

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Electrical conductivity arising from delocalised electrons.

Key notes

Important points to keep in mind

Each carbon in graphite forms three strong in-plane covalent bonds (sp2).

One electron per carbon becomes delocalised across the layer and carries charge.

Weak van der Waals forces between layers allow easy shear and lubrication.

Electrical conductivity in graphite occurs parallel to layers, not perpendicular.

High melting point results from strong covalent bonds within layers.

Graphite is insoluble due to the strong covalent network in each layer.

Properties are anisotropic: different behaviour along and across layers.

Intercalation or impurities modify interlayer spacing and electrical traits.

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