Metal bonding

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Metal bonding

• Metals form organized lattice structures similar
  to ionic cmpds
• adjacent atoms in metal lattice are all same
• close proximity of atoms allows outer electron
  energy levels to overlap
• So

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• electrons in outer valence shell can move freely
  through these overlapping energy levels
  
• results in sea of mobile electrons
• allows () metal cation to form

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Metal Properties
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large amount of energy needed to overcome both
IMF and strong bonding forces of metals in order
to change phase
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• If apply force to structure of metals
• metal atoms shift away from force free
  electrons bond newly overlapping metal cations
  together
• metals shape is deformed but shift doesn't
  separate metal atoms

• If apply force to structure of ionic compounds
• forces like charges to align () to () (-) to
  (-) resulting in shattering due to repulsion
  forces

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Alloys

• mixture of elements with metallic properties
• mixture can be adjusted to get desired properties
• two types
• substitutional and interstitial alloy
• (depends on size of elements same or different
  size)

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Common alloys

• brass Cu Zn
• bronze Cu, Sn Al
• pewter Sn, Pb Cu
• solder Pb Sn
• rose gold Cu Al
• white gold Au Ni, Pd or Pt
• sterling silver Ag Cu
• steel C Fe
• stainless steel Cr Ni