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7/30/2019 13Metallurgy_AlloysMJ
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Metals
Metallurgy
How we get metals
Bonding and structure of metals
Alloys, composites
Properties of metals and alloys
Mechanical properties
Electrical properties
Most metals are found in minerals.
1) Elemental Form
e.g. Ag, Au, Pt noble metals.
2) Aluminosilicates and Silicates
Metal + Al, Si, O
e.g. Beryl = Be3Al2Si6O18 Hard to extract metals.
3) Nonsilicate Minerals
Oxides Al2O3, TiO2, Fe2O3 Sulfides PbS, ZnS, CuFeS
2 Carbonates CaCO3
OCCURRENCE OFMETALS
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Steps in MetallurgySteps in Metallurgy
1) Preliminary treatment to concentrate
ore:
Floatation.
Hindered settling
Magnetic separation
2) Further purification and reduction to
obtain the metal in its elementary
state:
Hydrometallurgy leaching.
Pyrometallurgy roasting, smelting.
Electrometallurgy.
3) Final purification and refining of the
metal.
HydrometallurgyHydrometallurgyMetal is extracted from ore using aqueous
reactions
Leaching:
a metal is selectively dissolved
Dissolution agent: acid, base, salt.
Example: Dissolve Au by forming complex ion with CN!
4Au(s) + 8CN!(aq) + O2(g) + 2H2O(l)"4[Au(CN)4]
!(aq) + 4OH!(aq)
Kf[Au(CN)2]! = 2x1038
The gold is then obtained by reduction:
2Au(CN)2!(aq) + Zn(s) " Zn(CN)4
2!(aq) + 2Au(s)
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Hydrometallurgy of AluminumHydrometallurgy of Aluminum
Aluminum is the second most useful metal.
Bauxite: Al2O3.xH2O.
primary ore for Al
impurities: SiO2
Fe2O3
Bayer Process
Bayer process: bauxite (~ 50 % Al2O3) isconcentrated to produce aluminum oxide.
Dissolve bauxite in strong base (NaOH) at
high T, P
Al2O3 dissolves [Al(H2O)2(OH)4]!
hydrated metal complex
Filter out solids
Fe2O3, SiO2 do not dissolve Lower pH, Al(OH)3(s) precipitates
Take advantage of amphoteric nature of Al
Electrometallurgy of Aluminum
Hall process electrolysis cell is used toproduce aluminum.
Problem:Al2O3 melts at 2000C and it is impractical
to perform electrolysis on the molten salt.
Hall: use purified Al2O3 in molten cryolite(Na3AlF6, melting point 1012C).
Anode: C(s) + 2O2!(l) " CO2(g) + 4e!
Cathode: 3e!
+ Al3+
(l) " Al(l) The graphite rods are consumed in the reaction.
ElectrometallurgyElectrometallurgy
Electrometallurgy is the process ofobtaining metals through electrolysis.
Two different starting materials:
molten salt or aqueous solution.
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The Hall ProcessTo produce 1000 kg of Al, we need
4000 kg of bauxite,
70 kg of cryolite,
450 kg of C anodes and
56 # 109J of energy.
ElectrometallurgyElectrometallurgy of Alof Al ElectrometallurgyElectrometallurgyElectrorefining of Copper
Because of its good conductivity, Cu is used to
make electrical wiring.
Impurities reduce conductivity, therefore pure
copper is required in the electronics industry.
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Pyrometallurgy: using high temperatures
to obtain the free metal.
Several steps are employed:
Calcination is heating of ore to cause
decomposition and elimination of a
volatile product:
PbCO3(s) " PbO(s) + CO2(g)Roasting is heating which causes
chemical reactions between the ore
and the furnace atmosphere:
1. Burns off organic matter.
2. Converts carbonates and sulfides to
oxides:
2 ZnS(s)+ 3O2(g) "2ZnO(s) + SO2(g)3. Less active metals are often reduced
HgS(s) + O2(g) " Hg(l) + SO2(g)
PyrometallurgyPyrometallurgysources of iron:
hematite Fe2O3 and magnetite Fe3O4.
Iron Ore: Fe2O3 and SiO2
The Pyrometallurgy of Iron
Add limestone
and coke
Coke is coal
that has been
heated to drive
off the volatile
components.
The blast furnace
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PyrometallurgyPyrometallurgy of Feof Fe
Reactions
2C(s) + O2(g) " 2CO(g) + heat
heat + C(s) + H2O(g) " CO(g) + H2(g)
Fe3O4(s) + 4CO(g) " 3Fe(l) + 4CO2(g)
Fe3O4(s) + 4H2(g) " 3Fe(l) + 4H2O(g)
Coke: 1) heats furnace
2) reduces iron
Why is limestone (CaCO3) added?
PyrometallurgyPyrometallurgy of Feof Fe
At high T
CaCO3" CaO + CO2
CaO + SiO2 " CaSiO3(l)Metal + nonmetal " slag
oxide oxide basic acidic
Limestone (CaCO3)
removes SiO2 (and other)
impurities
slag floats on Fe(l); protects it from
oxidation by O2
Slag: cement
cinder block
building materials
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PyrometallurgyPyrometallurgy of Ironof Iron
Product in blast furnace: pig iron
brittle; not strong
Bessemer Converter
O2 (g) bubbled through molteniron to oxidize remaining
impurities
CaO slag still present to remove
impurities
Alloying elements added as
liquid iron is being removed.
Metals (75% of elements)
Lustrous (reflect light)
(almost) all solids
malleable & ductile
good conductors of heat and electricity
oxides are basic ionic solids
aqueous cations (n+)
reactivity increases downwards in family
Properties of metalsProperties of metals
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Free Electron Model
Metals are positive ions in sea of nearly
free electrons
Electrons bond metal ions together but are
free to roam the crystal lattice.
Explains malleability, ductility , and highelectrical and thermal conductivity.
Bonding in metalsBonding in metals
Important physical properties of pure metals:
malleable, ductile, good conductors of heat
and electricity.
Metals are crystals
every atom has 8 or 12 neighbors.
There are not enough electrons for the
metal atoms to make electron pair bonds
to each neighbor.
STRUCTURE andSTRUCTURE and
PROPERTIES of METALSPROPERTIES of METALS
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Body-centered cubic (bcc)
8 nearest neighbors
Not close packed
Close packed(hexagonal or cubic)
hcp ccp
Metal Crystal StructuresMetal Crystal StructuresMalleability of Metals and Alloys
Some metals are soft and ductile
(Au, Ag, Cu, Al, etc.)
Others are hard (Fe, W, Cr, etc.) Why?
Crystal structure is important.
Two types: body centered cubic (bcc)
- 8-coordinate - hardclose packed (fcc and hcp)
-12-coordinate - soft
Close-packed planes Non-close packed
slip easily - speed bumps
Cu (fcc) CuZn alloy (brass)
Zn (hcp)
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Hypothetical situation:
Upon graduation, you go to work for Boeing.
Your job select a high-strength Al alloy for jet
airplanes.50 tons cargo
Airplane: 500 tons } 150 tons plane structure
300 tons fuel
If you can triple the alloy strength, you can triple cargo
load (to 150 tons).
Material Tensile Yield Stress (psi)
pure (99.45%) annealed Al 4 x 103
pure (99.45%) cold drawn Al 24 x 103
Al alloy - precipitated, hardened 50 x 103
big improvement
But, perfect single crystal Al has a yield
stress of ca. 106 psi!
Mechanical Properties of Metals
and Alloys Defects are responsible for importantmechanical properties of metals:
malleability, yield stress, etc.
Non-directional bonding, large number ofnearest neighbor atoms "metallic
structures readily tolerate mistakes
vacancy dislocation(missing atom) (extra plane of atoms)
point defect line defect
Not important Very important
Defects in Metallic Crystals
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Dislocations Move Under Stress
Key point:
Moving a dislocation
breaks/makes a line
of metal-metal
bonds (easy)
Shearing a perfect
crystal means wehave to break a
plane of bonds
(requires much more
force)
shear force
Hardening of Alloys
Structural alloys - e.g., girders, knife blades,
airplane wings
Need to minimize movement of dislocations.
How?
1. Use annealed single crystals (expensive)
Some specialty applications e.g. jetturbine blade
Impossible for large items (airplane
wings, bridges)
2. Work hardening - moves dislocations to
grain boundaries
planar defect (stronger under stress)
Cold working or drawing of a metal
increases strength and brittleness (e.g.,
iron beams, knives, horseshoes)
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Hardening of Alloys (contd.)
Work HardeningandAnnealinghave
opposite effects
Annealing: crystal grains grow, dislocations
move (metal becomes more malleable)
3. Alloying homogeneous or
heterogeneousImpurity atoms or phases pin
dislocations.
ALLOYSAlloys: Mixtures of metals
- often have improved physical properties
1) Homogeneous (Solution) alloy
Mixed at the atomic level
2) Heterogeneous alloy
non-homogeneous dispersions.(e.g. pearlite steel has two phases: almost pure
Fe and cementite, Fe3C).
3) Intermetallic compounds
compounds of two different metals
having definite compositions:
Examples
Cr3Pt razor blades.
Ni3Al jet engines, lightweight and strong. Co5Sm permanent magnets in headsets.
Au3Bi, Nb3Sn superconductors for low
temperature, high field magnets
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There are two types of solution alloy:
Substitutional alloy when one metal substitutes for
another in the structure.
atoms must have similar atomic radii
elements must have similar bonding
characteristics.
SOLUTION ALLOYS
Interstitial alloy when a non-metal is present in theinterstices of the metal.
Interstitial atoms are smaller
The alloy is much stronger than the pure metal
(increased bonding between nonmetal and metal).
Example steel (contains up to 3 % carbon).
Iron and Steels
Below 900oC, iron has bcc structure
- hard as nails
Above 900oC, iron is close packed
(fcc) - soft
Can be worked into various shapes when hot
Steelmaking:
Carbon steel contains ~ 1% C by weight
(dissolves well in fcc iron but notin bcc)
Slow cooling (tempering):fcc Fe/1%C " mixture of bcc Fe and
Fe3C (pearlite)
Fe3C (cementite) grains stop movement of
dislocation in high carbon steel
- very hardmaterial
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STEELSSTEELS
Steel: Fe (pig iron) + small amounts of C
Mild Steel:
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Band Theory Atomic orbitals (AO) mix to form molecular
orbitals (MO).
Start with 2 AO, end with 2 MO
Start with n AOs, end up with n MOs
In metals energy difference between orbitals in
valence band is small.
Orbital form a continuous band of allowed
energy states.
Bonding in MetalsBonding in MetalsMETAL: ConductorValence electrons do not fill available orbitals
(not enough electrons)
Insulator or semiconductor
Valence band is full (or completely empty).
Energy gap separates valence band from
empty orbitals.
Conduction and InsulationConduction and Insulation
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Insulators: The energy gap is very
large in some solids: these solids will
be poor electrical conductors.
Semiconductors: the energy gap may
be smaller in some solids. The
conductivity of semi-conductors can beincreased with T, or applied fields.
Bonding in MetalsBonding in Metals SEMICONDUCTORS
Add impurities(dopants)to semi-conductorIf impurities donate extra electrons,
then the semiconductor is n-type
e.g. P impurities in Si.
If impurities accept electrons,
then the semiconductor is p-type
e.g. B impurities in Si.
n-type: negative charge carriers (electrons).
p-type: apparent positive charge carriers (holes).
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Properties:
shiny, silvery gray
brittle
Poor thermal conductor
SEMI-METAL
Uses:
alloy (with Al, Mg)
Silicone polymers
Electronic applications
for these applications very pure silicon(
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A diode is a semiconductor with a p-typematerial bonded to an n-type material.
Solar cells (photovoltaics) and lightemitting diodes (LEDs) are both diodedevices.
DiodesDiodes
When no current flows
DiodesDiodes
A diode allows current to flow in only onedirection
Electrons can flow from n-type to p-typeunder forward bias
In a solar cell, light excitation makes currentflow in the opposite direction.
Current flows when the diode is forward biased
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Light Emitting DiodeLight Emitting Diode
When electrons combine with holes, light is
emitted.
The energy of light (E = h$) is the same as theband gap energy Eg
The band gap energy depends on the material
used to make the diode.
LEDs are small light bulbs that produce
useful light from the from the flow of
electrons through a semiconductor
diode.
If the semiconductor used is a silicon
based semiconductor the light
produced is infrared.
Used in TV remote controls
LEDs producing visible light are
typically made from doped Aluminum-
Gallium-Arsenide (AlGaAs) conductor.
Changing the dopants changes the
size of the depletion zone and the color
of visible light produced
LEDsLEDs
::
LL
ightight
EE
mittingmitting
DD
iodesiodes
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LED MaterialsLED Materials
GaP/GaPgreen555
Gap: N/GaPgreen565
GaAs0.15PO.85: N/GaPyellow590
GaAs0.25Po.75: N/GaPorange610
GaAs0.35PO.65: N/GaPred630
GaAI0.35 As/GaAsred660
GaP: Zn-O/GaPred700
Material and structure
of LEDsColor
Wavelength
nm
LEDsLEDs:: LLightight EEmittingmitting DDiodesiodes
More energy efficient than incandescent lighting
LEDs producing visible light are typically madefrom doped Aluminum-Gallium-Arsenide(AlGaAs)
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Where areWhere are LEDsLEDs used?used?Ceramics
Ceramics
inorganic, nonmetallic, solids,
can be covalent network and/or ionic
bonded
Properties:
Crystalline or amorphous (e.g. glass),hard, brittle,
stable to high temperatures,
less dense than metals,
more elastic than metals,
very high melting.
Examples: alumina (Al2O3),
carbides (SiC, Ca2C),Oxides (BeO, ZrO2, Al2O3)
Nitrides (BN).
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SuperconductivitySuperconductivity
Superconductors show no resistance to
flow of electricity.
Superconducting behavior starts below the
superconducting transition temperature, Tc.
Meissner effect: permanent magnets
levitate over superconductors. The
superconductor excludes all magnetic field
lines, so the magnet floats in space.
Superconducting
Ceramic Oxides
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The depletion zone can be removed when
the diode is connected to a battery.
The n-type material is connected to the
negative portion of a battery.
The p-type material is connected to thepositive portion of the battery.
DiodesDiodes
COPPER CONTAININGCOPPER CONTAININGORESORES
Copper containing ore (CuFeS2) is stirred
with aqueous H2SO4 + O2
2CuFeS2(s)+2H+(aq)+SO4
2!(aq)+ 4O2(g) "
2Cu2+(aq) + 2SO42-(aq) + Fe2O3(s) +
\ / + 3S(s) + H2O
2CuSO4(aq) %
Electrolyzed to Cu
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Electrorefining of Copper
Slabs of impure Cu are used as anodes,
thin sheets of pure Cu are the cathodes.
Acidic copper sulfate is used as the
electrolyte.
The voltage across the electrodes is
designed to produce copper at the
cathode.
The metallic impurities do not plate out
on the cathode.
Metal ions are collected in the sludge at
the bottom of the cell.
ElectrometallurgyElectrometallurgy
Metallurgy is the science and
technology of extracting metals from
minerals.
There are five important steps:
Mining
getting the ore out of the ground
Concentrating
preparing it for further treatment
Reduction
to obtain the free metal in the zero
oxidation state
Refining
to obtain the pure metal Mixing with other metals
to form an alloys.
METALLURGYMETALLURGY