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Metallic Bonding

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Metallic Bonding and Metallic Properties Explained: Electron Sea Model
In metallic bonding, the valence electrons are not localized to any one particle. They are free to move and occupy the space between the positive ions.
The large attraction of the positive (+) ions for the negative (-) delocalized valence electrons are what holds the crystal together.

Properties of metal
Malleability and ductility: The delocalized electrons are a constant presence, always holding together and shifting (+) ions.
Hard and strong and high melting points: In general, the more delocalized electrons, the tougher the metals. Transition metals have the most delocalized electrons and are the strongest.
Conduct electricity and heat: Delocalized electrons also carry electric current and heat due to their ability to move through the crystal.
Shiny: Delocalized electrons readily absorb and re-emit visible frequency photons, giving metals their characteristic luster.
For more information about metals and their properties:
Properties of Metals and Alloys

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