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METALS

METALS. Bonds and Properties. Alloys Pure Elements. LUSTER. HIGH. DEFORMABILITY. Malleable & Ductile. CONDUCTIVITY OF HEAT AND ELECTRICITY. Good to Excellent. PHASE at STP. Solid (except Hg). Ion FORMATION. Loses e - to form positive ions. IONIZATION ENERGY. Low (lowest is Fr).

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METALS

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  1. METALS Bonds and Properties Alloys Pure Elements

  2. LUSTER HIGH DEFORMABILITY Malleable & Ductile CONDUCTIVITY OF HEAT AND ELECTRICITY Good to Excellent PHASE at STP Solid (except Hg) Ion FORMATION Loses e- to form positive ions IONIZATION ENERGY Low (lowest is Fr) ELECTRONEGATIVITY Low (lowest is Fr) Some Properties of Metals

  3. Many metals have high luster Hmmm…. How much is this shiney Gold worth !? 400 ounces (27.5lbs) $900.00 / ounce $360,000.00 per bar 12 bars = $4,320,000.00

  4. Many Metals have high melting points

  5. Metallic bonding: different from ionic bond Both bond types due to: electrostatic attraction Ionic bond: transfer of electrons from one atom to another Metal bonds: electronsROAM FREELYfrom one metal atom to the next • sea of mobile electrons • accounts for properties of metals Metal bonding

  6. Why can electrons in metals roam freely about?

  7. Metals: organized lattice structures similar to ionic cmpds • adjacent atoms in the metal lattice are all the same • close proximity of atoms allows outer energy levels to overlap So… electrons in the outer valence shell can move freely through these overlapping energy levels = “sea of mobile electrons” Metal bonding

  8. Na 1s1 Na 1s1 Overlapping orbitals

  9. Freely moving electrons: • called “Delocalized” electrons • allows (+) metal cation to form Delocalized electrons move freely throughout the metal from one cation to the next • creates what’s called “the sea • of mobile electrons” This sea of electrons: • binds each metal cation to each neighbor cation • this creates the metal bond Metal bonding

  10. this sea of electrons gives metals some of their unique properties since electrons can move freely from place to place they: • conduct electricity (a flow of electrons) • conduct heat • are malleable and ductile • have luster How do electrons do this? Metal Properties

  11. Electrical Conductivity - + Flow of electrons e-   e- Free flow of electrons through the metal Electrons flow from metal through the metal wire towards the (+) charge; then flow from negative terminal back into the metal originally came from

  12. Metals and non-metals behave very differently when they are hit with a force such as a hammer Metals DEFORM: Non-metals SHATTER Why? Metals have free flowing electrons & nonmetals do not! Malleability

  13. Metal Non-Metal If force is applied to metal: • some metal atoms shift away from force & the free electrons simply bond the newly overlapping metal ions together • metal is deformed but shift doesn't change the metal atoms If force is applied to non-metal: • (+) & (-) charges align • results in fracture due to force of repulsion

  14. Deformation of Metals Deformation of Metals

  15. As number of electrons that can be delocalized ↑ so does: Hardness and Strength Na has one valence electron that can be delocalized so it - is relatively soft ( can be cut with a butter knife) Mg has two electrons that can be delocalized - can still be cut but is much harder than Na Transition metals have varied # of e-'s that can be delocalized - Chromium is very hard and has high strength

  16. Alloys • mixture of elements that have metallic properties • mixture can be adjusted to get desired properties • can be substitutional or interstitial

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