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Metallic bonding

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Metallic bonding

  1. 1. Metallic BondingStrong forces of attraction are responsiblefor the high melting point of most metals.
  2. 2. CA StandardsStudents know atoms combine to formmolecules by sharing electrons to formcovalent or metallic bonds or byexchanging electrons to form ionicbonds.
  3. 3. Metallic Bonding The chemical bonding that results from the attraction between metal cations and the surrounding sea of electrons Vacant p and d orbitals in metals outer energy levels overlap, and allow outer electrons to move freely throughout the metal Valence electrons do not belong to any one atom
  4. 4. Packing in MetalsModel: Packinguniform, hardspheres to best useavailable space.This is called closestpacking. Each atomhas 12 nearestneighbors.
  5. 5. Metal AlloysSubstitutional Alloy: some metal atoms replaced by others of similar size.
  6. 6. Metal AlloysInterstitial Alloy: Interstices (holes) in closest packed metal structure are occupied by small atoms.
  7. 7. Properties of Metals Metals are goodconductors of heat andelectricity Metals are malleable Metals are ductile Metals have hightensile strength Metals have luster

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