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Metallic Bonding

Metallic Bonding. Metals in the periodic table. Metals Essential for Life. Properties of Metals. Solids (except Hg) – most have high mp & bp Luster Malleable & ductile Good conductor of heat & electricity Metals are losers! (metals lose electrons and form positive ions)

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Metallic Bonding

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  1. Metallic Bonding

  2. Metals in the periodic table

  3. Metals Essential for Life

  4. Properties of Metals • Solids (except Hg) – most have high mp & bp • Luster • Malleable & ductile • Good conductor of heat & electricity • Metals are losers! (metals lose electrons and form positive ions) • Low ionization energy • Low electronegativity

  5. Metallic Bonding Metal atoms form a lattice. The valence levels of the atoms overlap. The valence electrons can roam easily from 1 atom to another throughout the metal. Metallic bonding

  6. Delocalized Electrons • Valence electrons are free to roam throughout crystal • “Sea of Mobile Electrons” • Metallic Bond = attraction between positive metal kernel and electron sea.

  7. Comparison of Metallic & Ionic Bonding Lattice points are all positive. Electrons roam. Lattice points are positive and negative.

  8. Properties of metals • Electrons can move so they conduct a current. • Electron sea holds the metal together when it’s deformed.

  9. Metallic Bonds • Pretty strong. All metals but Hg are solids at room temperature. • Most have moderately high melting points & high boiling points.

  10. Deformation of Metals Deformation of Metals

  11. Why metals are deformable & ionic crystals aren’t:

  12. Deformation of Metals • Applied force moves metal cations. • Cations are held together by electron sea.

  13. Alloys • Mixture of elements that has metallic properties. • Adjust the mixture to get desired properties. • Can be substitutional or interstitial

  14. Substitutional Interstitual Types of Alloys Steel Bronze Brass

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