ppt slides - 2
TRANSCRIPT
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Crystalline and amorphous materials
Solids can be divided into two categories.
CrystallineAmorphous
Crystalline has long range order
Amorphous materials have short range order
Effect of Crystallinity on Physical properties - ex. Polyethylene
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CrystalType
Particles InterparticleForces
Physical Behaviour Examples
Atomic
Molecular
Metallic
Ionic
Network
Atoms
Molecules
Atoms
Positive andnegative ions
Atoms
Dispersion
DispersionDipole-dipoleH-bonds
Metallic bond
Ion-ionattraction
Covalent
Soft Very low mp Poor thermal and electrical conductors
Fairly softLow to moderate mpPoor thermal and electrical conductors Soft to hardLow to very high mpMellable and ductileExcellent thermal and electrical
conductorsHard and brittle
High mpGood thermal and electrical conductors
in molten condition Very hard Very high mp Poor thermal and electrical conductors
Group 8A
Ne to Rn
O2, P4, H 2O,Sucrose
Na, Cu, Fe
NaCl, CaF 2,MgO
SiO 2(Quartz)
C (Diamond)
TYPES OF CRYSTALLINE SOLIDS
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CRYSTAL STRUCTURE
Crystal structure is the periodic arrangement of atoms in thecrystal. Association of each lattice point with a group of atoms (Basis or Motif) .Lattice : Infinite array of points in space, in which each point hasidentical surroundings to all others.
Space Lattice Arrangements of atoms= Lattice of points onto which the atoms are hung.
Elemental solids (Argon): Basis = single atom.Polyatomic Elements: Basis = two or four atoms .Complex organic compounds: Basis = thousands of atoms .
+
Space Lattice + Basis = Crystal Structure
=
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THREE DIMENTIONAL UNIT CELLS / UNIT CELL SHAPES
1
2
3
4
5
6
7
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Primitive ( P ) Body Centered ( I )
Face Centered ( F ) C-Centered ( C )
LATTICE TYPES
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BRAVAIS LATTICES
7 UNIT CELL TYPES + 4
LATTICE TYPES = 14
BRAVAIS LATTICES
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Close-packing- HEXAGONAL coordination of each sphere
SINGLE LAYER PACKING
SQUARE PACKING CLOSE PACKING
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NON-CLOSE-PACKED STRUCTURES
68% of space is occupied
Coordination number = 8
a) Body centered cubic ( BCC ) b) Primitive cubic ( P)
52% of space is occupiedCoordination number = 6
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6
ABCABC 12Cubic close packed
ABABAB 12Hexagonal
close packed
ABABAB 8Body-centered
Cubic
AAAAA PrimitiveCubic
Stacking pattern
Coordinationnumber
Structure
Non-close
packing
Closepacking
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TETRAHEDRAL HOLES
OCTAHEDRAL HOLES
TYPE OF HOLES IN CLOSE PACKING
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Ionic structures may be derived from the
occupation of holes by oppositely charged
ions (interstitial sites) in the close-packed
arrangements of ions.
IONIC CRYSTAL STRUCTURES
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IONIC CRYSTAL TYPES
Ionic crystaltype
Co-ordinationnumber
A X
Structure type
AX
AX 2
AX 3
6 68 8
6 3
8 4
6 2
NaClCsCl
Rutile(TiO 2)
Fluorite (CaF2)
ReO 3
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Formula Type and fraction of sitesoccupied
CCP HCP
AX All octahedral
Half tetrahedral (T+ or T-)
Rock salt (NaCl)
Zinc Blend (ZnS)
Nickel Arsenide (NiAs)
Wurtzite (ZnS)
AX2
All Tetrahedral
Half octahedral (orderedframework)
Half octahedral (Alternatelayers full/ empty)
Fluorite (CaF2),
Anti-Fluorite (Na 2O)
Anatase (TiO 2)
Cadmium Chloride(CdCl 2)
Not known
Rutile (TiO 2)
Cadmium iodide (CdI 2)
A3X All octahedral & AllTetrahedral
Li3Bi Not known
AX 3 One third octahedral YCl 3 BiI 3
SUMMARY OF IONIC CRYSTAL STRUCTURE TYPES
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Crystallographic notation of atomic planes and directions
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POINT Coordinates
To define a point within a unit cell. Express the coordinates uvw as fractions of unit cell vectors a , b , and c (so that the axes x, y, and z do not have to be orthogonal).
a
b
c
origin
pt. coord.
x ( a ) y ( b ) z ( c )
0 0 0
1 0 0
1 1 1
1/2 0 1/2
pt.
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Self-Assessment Example 1: What is crystallographic direction?
ab
c Along x: 1 a
Along y: 1 b
Along z: 1 c
[1 1 1]DIRECTION =
Magnitude alongX
Y
Z
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Families and Symmetry: Cubic Symmetry
x
y
z
(100)
Rotate 90 o about z-axis
x
y
z
(010)
x
y
z
(001)Rotate 90 o about y-axis
Similarly for other equivalent directions
Symmetry operation cangenerate all the directionswithin in a family.
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How Do We Designate Lattice Planes?
Example 1
Planes intersects axes at: a axis at r= 2 b axis at s= 4/3 c axis at t= 1/2
How do we symbolically designate planes in a lattice?
Possibility #1: Enclose the values of r, s, and t in parentheses (r s t) Advantages:
r, s, and t uniquely specify the plane in the lattice, relative to the origin. Parentheses designate planes, as opposed to directions given by [...]
Disadvantage: What happens if the plane is parallel to --- i.e. does not intersect--- one of the axes? Then we would say that the plane intersects that axis at ! This designation is unwieldy and inconvenient.
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How Do We Designate Lattice Planes?
Planes intersects axes at: a axis at r= 2
b axis at s= 4/3 c axis at t= 1/2
How do we symbolically designate planes in a lattice?
Possibility #2: THE ACCEPTED ONE
1. Take the reciprocal of r, s, and t . Here: 1/r = 1/2 , 1/s = 3/4 , and 1/r = 2
2. Find the least common multipl e that converts all reciprocals to integers . With LCM = 4, h = 4/r = 2 , k= 4/s = 3 , and l= 4/r = 8
3. Enclose the new triple (h,k,l) in parentheses : (238) 4. This notation is called the Miller Index .
* Note: If a plane does not intercept an axes (I.e., it is at ), then you get 0.* Note: All parallel planes at similar staggered distances have the same Miller index.
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Families of Lattice Planes
The Miller indices (hkl) usually refer to the plane thatis nearest to the origin without passing through it.
You must always shift the origin or move the planeparallel, otherwise a Miller index integer is 1/0, i.e.,!
Sometimes (hkl) will be used to refer to any other planein the family, or to the family taken together.
Importantly, the Miller indices (hkl) is the same vector asthe plane normal!
Given any plane in a lattice, there is a infinite set of parallel lattice planes(or family of planes) that are equally spaced from each other.
One of the planes in any family always passes through the origin.
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z
x
y
Look down this direction(perpendicular to the plane)
Crystallographic Planes in FCC: (100)
d 100
aDistance between (100) planes
Distance to (200) plane d 200a
2
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Crystallographic Planes in FCC: (111)
z
x
y
Look down this direction(perpendicular to the plane)
d 111
a 33
Distance between (111) planes
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Note: similar to crystallographic directions, planes that are parallel toeach other, are equivalent
i i i C C l
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Directions in HCP Crystals
1. To emphasize that they are equal, a and b is changed to a 1 and a 2.2. The unit cell is outlined in blue .
3. A fourth axis is introduced (a 3) to show symmetry. Symmetry about c axis makes a 3 equivalent to a 1 and a 2. Vector addition gives a 3 = ( a 1 + a 2).
4. This 4-coordinate system is used: [a 1 a 2 ( a 1 + a 2) c]
Di i i HCP C l d
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Directions in HCP Crystals: 4-index notation
Example What is 4-index notation for vector D?
Projecting the vector onto the basal plane, it liesbetween a 1 and a 2 (vector B is projection).
Vector B = (a 1 + a 2), so the direction is [110] incoordinates of [a 1 a 2 c], where c-intercept is 0.
In 4-index notation, because a 3 = ( a 1 + a 2), thevector B is since it is 3x farther out.
In 4-index notation c = [0001], which must beadded to get D (reduced to integers ) D = [1123]
Self-Assessment Test: What is vector C?
Easiest to remember: Find the coordinate axes that straddle the vector of interest, and follow along those axes (but divide the a 1, a 2 , a 3 part of vector by 3 because you are now three times farther out!) .
13
[112 0]
Check w/ Eq. 3.7
or just use Eq. 3.7
a 2 2a 3 B without 1/3
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Mill I di f HCP Pl
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Miller Indices for HCP Planes
As soon as you see [1100], you will knowthat it is HCP, and not [110] cubic!
4-index notation is more important for planes in HCP, in order to distinguish similar planes rotated by 120 o.
1. Find the intercepts , r and s , of the plane with any two of the basal plane axes ( a 1, a 2, or a 3), as well as theintercept, t , with the c axes.
2. Get reciprocals 1/r, 1/s, and 1/t.3. Convert reciprocals to smallest integers in same ratios .
4. Get h, k, i , l via relation i = - (h +k), where h isassociated with a 1, k with a 2, i with a 3, and l with c .5. Enclose 4-indices in parenthesis: (h k i l ) .
Find Miller Indices for HCP:
r s
t
Mill I di f HCP Pl
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Miller Indices for HCP Planes
What is the Miller Index of the pink plane?
1. The planes intercept a 1, a 3 and c at r=1, s=1 and t= , respectively.
1. The reciprocals are 1/r = 1, 1/s = 1, and 1/t = 0.
2. They are already smallest integers.
3. We can write (h k i l ) = ( 1 ? 1 0 ).
4. Using i = - (h+k) relatio n, k= 2 .
5. Miller Index is (1210)
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Yes, Yes.we can get it without a 3!
1. The planes intercept a 1, a 2 and c at r=1, s= 1/2 and t= , respectively.
2. The reciprocals are 1/r = 1, 1/s = 2, and 1/t = 0.
3. They are already smallest integers.
4. We can write (h k i l ) =
5. Using i = - (h+k ) relation , i=1 .
6. Miller Index is (12 10)
(12 ?0)
But note that the 4- index notation is unique.Consider all 4 intercepts: plane intercept a 1, a 2, a 3 and c at 1, 1/2, 1, and , respectively. Reciprocals are 1, 2, 1, and 0. So, there is only 1 possible Miller Index is (12 10)
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(1 1 1) plane of FCCz
x
y
z
a 1
a 2
a 3
(0 0 0 1) plane of HCPSAME THING!*
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Defects in Solids
There is no such thing as a perfect crystal.
What are these imperfections? Why are they important?
Many of the important properties of materials
are due to the presence of imperfections.
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Vacancy atoms Interstitial atoms Substitutional atoms
Point defects
Types of Imperfections
Dislocations Line defects
Grain Boundaries Area defects
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Vacancies :-vacant atomic sites in a structure.
Self-Interstitials :-"extra" atoms positioned between atomic sites.
Point Defects
Vacancy distortion
of planes
self- interstitial
distortionof planes
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Boltzmann's constant
(1.38 x 10 -23 J/atom-K)(8.62 x 10 -5 eV/atom-K)
N v N
exp Q v k T
No. of defects
No. of potentialdefect sites.
Activation energy
AbsoluteTemperature
Each lattice siteis a potentialvacancy site
Equilibrium concentration varies with temperature!
Equilibrium Concentration:Point Defects
1 eV = 1.6 x 10 -19 J
unitless; probability
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Find the equil. # of vacancies in 1 m 3 of Cu at 1000 C. Given:
A Cu = 63.5 g/mol r = 8.4 g / cm 3
Q v = 0.9 eV/atom N A = 6.02 x 10 23 atoms/mol
Estimating Vacancy Concentration
For 1 m 3 , N = N A A Cu
r x x 1 m 3 = 8.0 x 10 28 sites8.62 x 10 -5 eV/atom-K
0.9 eV/atom
1273K
N v N
exp Q v k T
= 2.7 x 10 -4
Answer:
N v
= (2.7 x 10 -4)(8.0 x 10 28 ) sites = 2.2 x 10 25 vacancies
Cu T m=1083 C, so at T~T m~ 1/10 4 sites are vacant(general rule)
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Imperfections in Solids
Conditions for substitutional solid solution (S.S.) W. Hume Rothery rule
1. r (atomic radius) < 15% 2. Proximity in periodic table
i.e., similar electronegativities 3. Same crystal structure for pure metals 4. Valency
All else being equal, a metal will have a greater tendency to dissolve a metal of higher valency thanone of lower valency.
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Imperfections in Solids
Application of Hume Rothery rules Solid Solutions
1. Would you predictmore Al or Agto dissolve in Zn?
2. More Zn or Al
in Cu?
Element Atomic Crystal Electro- ValenceRadius Structure nega-(nm) tivity
Cu 0.1278 FCC 1.9 +2C 0.071H 0.046O 0.060
Ag 0.1445 FCC 1.9 +1 Al 0.1431 FCC 1.5 +3Co 0.1253 HCP 1.8 +2
Cr 0.1249 BCC 1.6 +3Fe 0.1241 BCC 1.8 +2Ni 0.1246 FCC 1.8 +2Pd 0.1376 FCC 2.2 +2Zn 0.1332 HCP 1.6 +2
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Imperfections in Solids
Specification of composition
weight percent 100x21
11 mm
mC
m 1 = mass of component 1
100x21
1'1
mm
m
nn
nC
nm1 = number of moles of component 1
atom percent
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Line Defects in Solids
Edge Dislocation
One dimensional defect in which atoms are mispositioned.
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Line Defects in Solids
Linear Defects ( Dislocations ) Are one-dimensional defects around which atoms are misaligned
Edge dislocation: extra half-plane of atoms inserted in a crystal structure
b to dislocation line Screw dislocation:
spiral planar ramp resulting from shear deformation b to dislocation line
Burgers vector, b : measure of lattice distortion
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Dislocation motion requires the successive bumping of a half plane of atoms (from left to right here).
Bonds across the slipping planes are broken and remade in succession.
materials can be deformed rather easily
Atomic view of edgedislocation motion fromleft to right as a crystalis sheared.
Motion of Edge Dislocation
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Line Defects in Solids
Screw Dislocation
Burgers vector,b
Dislocationline
b
(a)
(b)
Screw Dislocation
Edge Screw and Mixed
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Edge, Screw, and MixedDislocations
Edge
Screw
Mixed
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Imperfections in Solids
Dislocations are visible in electron micrographs
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Planar Defects in Solids One case is a twin boundary (plane)
Essentially a reflection of atom positions across the twin plane .
Stacking faults For FCC metals an error in ABCABC packing sequence Ex: ABCABABC
Adapted from Fig. 4.9, Callister 7e.
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Polycrystalline Materials
Grain Boundaries regions between crystals transition from lattice of
one region to that of theother
slightly disordered low density in grain
boundaries high mobility high diffusivity high chemical reactivity
Adapted from Fig. 4.7, Callister 7e.
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Microscopic Examination Crystallites (grains) and grain boundaries. Vary
considerably in size. Can be quite large ex: Large single crystal of quartz or diamond or Si ex: Aluminum light post or garbage can - see the
individual grains Crystallites (grains) can be quite small (mm or
less) necessary to observe with a microscope.
O ti l Mi
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Useful up to 2000X magnification.
Polishing removes surface features (e.g., scratches) Etching changes reflectance, depending on crystal orientation.
Micrograph of brass (a Cu-Zn alloy)
0.75mm
Optical Microscopy
Adapted from Fig. 4.13(b) and (c), Callister 7e. (Fig. 4.13(c) is courtesyof J.E. Burke, General Electric Co.
crystallographic planes
O ti l Mi
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Grain boundaries...
are imperfections, are more susceptible
to etching, may be revealed as
dark lines,
change in crystalorientation acrossboundary. Adapted from Fig. 4.14(a)
and (b), Callister 7e. (Fig. 4.14(b) is courtesyof L.C. Smith and C. Brady,
the National Bureau of Standards, Washington, DC[now the National Institute of Standards and Technology,Gaithersburg, MD].)
Optical Microscopy
ASTM grainsize number
N = 2 n -1
number of grains/in 2 at 100x
magnification
Fe-Cr alloy(b)
grain boundary surface groove
polished surface
(a)
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