Why does graphite conduct electricity but diamond does not?
Graphite has delocalised electrons between layers; diamond has all four outer electrons in localised covalent bonds. Learn it step by step →
Bonding, Structure & Properties is a core part of GCSE Chemistry. Revise the key concepts and common mistakes below, then lock them in with the free games.
Key concepts
Giant ionic latticeRegular 3D arrangement of alternating ions
Simple molecularSmall molecules with weak intermolecular forces
Giant covalentNetwork of atoms covalently bonded e.g. diamond
Intermolecular forceWeak force between separate molecules
Conductivity ruleCharges must be free to move
Melting pointHigher when bonds or forces broken are stronger
NanoparticleParticle 1-100 nm in size
BuckminsterfullereneC60 hollow cage molecule
Carbon nanotubeRolled-up cylinder of graphene
Surface area to volumeIncreases as size decreases
State symbol(s), (l), (g), (aq) used in equations
Dot-and-crossDiagram showing electrons from each atom
Ionic bondElectrostatic attraction between oppositely charged ions
Covalent bondShared pair of electrons between non-metals
What your exam board covers
Where Bonding, Structure & Properties sits in each exam board's specification. Tap a board to see what it lists.
CCEABondingSpec 1110
Part of: Unit 1 — Structures, trends, chemical reactions, quantitative chemistry and analysis
Questions where students often pick the tempting wrong answer — make sure you know the right one:
Why does graphite conduct electricity but diamond does not?✗ Graphite conducts because it is a metal, while diamond is a non-metal.✓ Graphite has delocalised electrons between layers; diamond has all four outer electrons in localised covalent bonds.
When water boils, what is broken?✗ The covalent bonds between hydrogen and oxygen atoms are broken when water boils.✓ Intermolecular forces (hydrogen bonds) between water molecules are broken — the O-H covalent bonds stay intact.
Why do metals conduct electricity?✗ Metal atoms themselves move to carry the current.✓ Delocalised electrons are free to move through the lattice of positive ions, carrying charge.
Why does NaCl not conduct as a solid but does when molten?✗ ions are charged only when molten✓ ions are free to move when molten
Practise Bonding, Structure & Properties — free games
Test yourself with these quick revision games for this topic:
