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How are electrons shared in a metallic bond?
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In a metallic bond the valence electrons are not tied to any one atom or specific pair of atoms; instead they become delocalized and form a "sea" (or cloud) of electrons that permeates a lattice of positive metal ions. Each metal atom contributes one or more valence electrons to this communal electron pool, and those electrons are shared collectively by all the atoms in the metal.
Key points:
- The electrons are mobile and delocalized (not localized as in covalent bonds).
- The positive metal ions are held together by the electrostatic attraction between them and the delocalized electrons.
- Because the sharing is non-directional and electrons can move freely, metals conduct electricity and heat, are malleable and ductile, and often have a shiny (lustrous) appearance.
More advanced description (band theory): atomic orbitals of many atoms overlap to form broad energy bands; partially filled bands allow electrons to move through the lattice, which is the quantum mechanical basis for the delocalized electron sea.
Key points:
- The electrons are mobile and delocalized (not localized as in covalent bonds).
- The positive metal ions are held together by the electrostatic attraction between them and the delocalized electrons.
- Because the sharing is non-directional and electrons can move freely, metals conduct electricity and heat, are malleable and ductile, and often have a shiny (lustrous) appearance.
More advanced description (band theory): atomic orbitals of many atoms overlap to form broad energy bands; partially filled bands allow electrons to move through the lattice, which is the quantum mechanical basis for the delocalized electron sea.
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