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Metallic Bonds. Metals don’t bond ionically For lattices Don’t share or lose e- like covalent or ionic bonds. Electron Sea Model. All metal atoms in a metallic solid contribute their valence e- to form a “sea” of e-

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Metals don’t bond ionically

    • For lattices
  • Don’t share or lose e- like covalent or ionic bonds
electron sea model
Electron Sea Model
  • All metal atoms in a metallic solid contribute their valence e- to form a “sea” of e-
    • These e- move easily and freely because they are not tied to a specific atom
      • Delocalized electrons
    • Metallic cation is formed

All empty space is evenly distributed v.e-

metallic bonds1
Metallic Bonds
  • The attraction of a metallic cation for delocalized electrons
  • This accounts for a lot of theproperties of metals
    • Range of melting points
    • Malleability
    • Ductile
    • Durable
      • Hard to remove metallic cation because of the strong e- attraction
    • Mobile e-
      • Explains why they are good conductors
metallic bonds2
Metallic Bonds
  • Transition metals tend to be harder due to “d” sublevel electrons
    • More e- = more attraction
  • Alkali metals are softer because they contain only “s” sublevel (1 sublevel)
    • Less e- = less attraction
alloys
Alloys
  • Mixture of elements (usually metals) that has metallic properties
  • Substitutional alloy – atoms of original metallic solid replaced by other metal atoms of similar size
    • Sterling silver  silver is replaced with Cu atoms
  • Interstitial alloy – small holes (interstices) in a metallic crystal that are filled with smaller atoms
    • Like pouring sand in a bucket of gravel
    • Ex. Carbon steel
      • Holes in iron are filled with carbon which strengthens the iron
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