Metallic bonding - PowerPoint PPT Presentation

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Metallic bonding

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  1. Metallic bonding IB Topic 4

  2. valence electrons detach from individual atoms since metals contain only 1-3 valence electrons • no particular electron is confined to a particular metal atom • leaves a close packed lattice of positive ions (cations) in a sea of delocalized negative electrons • the electrostatic attraction between (-) and (+) holds together the metal • electrons act as a "glue" giving the substance a definite structure

  3. the delocalized nature of the bonds, make it possible for the atoms to slide past each other • this means metals are malleable and ductile • hammered into thin sheets or shapes without breaking • drawn into wires • ionic compounds would crack • metals are essential part of the world economy • reinforcement of concrete, wires, cars, pipes… • traded as commodities • most common is iron which is in steel