1 metals bonds and properties alloys pure elements
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METALS
Bonds and Properties
Alloys
Pure Elements
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Some Properties of MetalsSome Properties of Metals
Low (lowest: Fr)Low (lowest: Fr)ELECTRONEGATIVITY
Low (lowest: Fr)Low (lowest: Fr)IONIZATION ENERGY
Lose eLose e-- to form (+) ions to form (+) ionsIon FORMATION
Solid (except Hg)Solid (except Hg)PHASE at STP
Good to ExcellentGood to ExcellentCONDUCTIVITY :
HEAT AND ELECTRICITY
Malleable & DuctileMalleable & DuctileDEFORMABILITY
HIGHHIGHLUSTER
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Many metals have high luster
Hmmm….
How much is thisshiney Gold worth !?
400 ounces (27.5lbs)$1660.00 / ounce$664,000.00 per bar
12 bars =$7,968,000.00
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Many Metals have high melting points
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Metallic bonding: different from ionic bond
Both bond types due to: electrostatic attraction
Ionic bond: transfer electrons from one atom to another
Metal bonds: valence electrons ROAM FREELY from one metal atom to next
•sea of mobile electrons•accounts for properties of metals
Metal bondingMetal bonding
66Why can electrons in metals roam freely about?
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Metal bondingMetal bonding
Metals: form organized lattice structures similar to ionic cmpdsadjacent 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 = “sea of mobile electrons”
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Na 3s1 Na 3s1
overlapping valence electron orbitals
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Metal bondingMetal bonding
Freely moving electrons: called “delocalized” electrons allows (+) metal cation to form
Delocalized electrons move freely
throughout metal from one cation to nextcreates what’s called “the sea of mobile
electrons”
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This sea of electrons:• binds each metal cation to each neighbor’s cation • this creates the metal bond
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Metal PropertiesMetal Propertiessea of mobile electrons
givesmetals some unique
properties
since electrons move freelyfrom place to place they:● conduct electricity (flow of electrons)● conduct heatAccounts for metals being● malleable and ductile● and having luster
How do electrons do this?
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Electrical Conductivity
-
Free flow of electrons through the metal
+
e-e-
Flow of electrons
e- flow from metal through metal wire towards (+) charge; then flow from (-) terminal back into metal
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Malleability Malleability Metals & non-metals behave very differently when hit with a force such as hammer
Metals DEFORM whileNon-metals SHATTER
Why?
Metals have free flowing electrons & nonmetals do not!
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If apply force to metal: •metal atoms shift away from force & free electrons bond newly overlapping metal ions together•metal is deformed but shift doesn't change metal atoms
If apply force to non-metal: •like charges align (+) to (+) (-) to (-) which results in shattering due to repulsion
Metal
Non-Metal
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Deformation of MetalsDeformation of Metals
Deformation of MetalsDeformation of Metals
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As # of electrons that can be delocalized ↑ so does: Hardness and Strength
Na has one valence electron that can be delocalized so: - is relatively soft ( can be cut with a butter knife)
Mg has two valence electrons that can be delocalized so:- can still be cut but is much harder than Na
Transition metals have varied # of e-'s that can be delocalized- Chromium (Cr+6) is very hard and has high strength
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AlloysAlloys
mixture of elements that have metallic mixture of elements that have metallic propertiesproperties
mixture can be adjusted to get desired mixture can be adjusted to get desired propertiesproperties
substitutional and interstitial alloy (depends substitutional and interstitial alloy (depends on sizes of elements – same or different size)on sizes of elements – same or different size)
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Common alloysCommon alloysBrass: Cu & ZnBrass: Cu & ZnBronze: Cu, Sn & AlBronze: Cu, Sn & AlPewter: Sn, Pb & CuPewter: Sn, Pb & CuSolder: Pb & SnSolder: Pb & SnRose gold: Cu & AlRose gold: Cu & AlWhite gold: Au & Ni, Pd or PtWhite gold: Au & Ni, Pd or PtSterling silver: Ag & CuSterling silver: Ag & CuSteel: C & FeSteel: C & Fe
Stainless steel: Cr & NiStainless steel: Cr & Ni