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CHEM 121 Studioby Learn4Less · UBC CHEM 121

CHEM 121 glossary

Metallic bonding

The bonding in metals: a lattice of metal cations held together by a "sea" of valence electrons delocalized over the whole crystal. Because the electrons are free to move, metals conduct, and because the bonding has no fixed direction, layers can slide without the solid shattering.

Metallic bonding: cations in a sea of electronsMetal cations sit in a regular array and their valence electrons are delocalized over the whole solid, moving freely between them. The attraction between the cations and the electron sea holds the metal together and lets it conduct electricity.+++++++++++++++metal cations in a sea of delocalized e⁻conducts electricity; malleable and ductile

Metal cations in a sea of mobile electrons.

Example

Sodium contributes one valence electron per atom and melts at 97.8 °C; magnesium contributes two and melts at 650 °C.

See alsoMetallic solidDelocalizationValence electron