msep 503 defects, diffusion and transformation slide … · 2019-10-31 · &rxuvh &rqwhqw...
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MSE 553 DEFECTS, DIFFUSION AND TRANSFORMATION IN MATERIALS
E. GIKUNOO
First Semester 2019/2020Wednesdays 2:00 – 5:00 pm 1
Lecturer: Dr. Emmanuel Gikunoo
Office : 321 New Block
Email: [email protected]
Lecture Hours: Tuesdays, 08:00 – 11:00
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Course Information
Website: https://egikunoo.wordpress.com
Objective
This course will provide students with the:
understanding of basic theory of the interaction of defects, general laws of phase transformation and mutual effects between composition, and the microstructure and macroproperties of engineering materials such as metallic alloys and ceramics;
understanding of phase transformations in materials in tailoring the microstructure and properties of various materials;
much needed underlying principles governing materials developments.3
At the end of the course the student should be able to:
discuss the relationship between atomic structure of materials and microstructure evolution on the basis of transport processes.
apply the principles of phase transformation for microstructure design and property improvements.
apply the principles of phase transformation for selection of materials and processes.
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Learning Outcomes
1 2
3 4
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Course Content
This course will introduce students to:
basic crystallography and thermodynamics;
defects classification in different crystals, defects in non-crystalline materials, mechanical, electrical, magnetic and optical properties of defects, defect characterization techniques;
Fick’s first and second laws, Intrinsic and integrated diffusion coefficient, Tracer and growth kinetics, Matano-Boltz analysis, Kirkendall effect, Darken analysis, physico-chemical approach of diffusion;
basic kinetics of transformation, interfacial and homogeneous nucleation, nucleation and growth, coarsening and the Gibbs-Thompson equation, diffusion and diffusionless transformations.
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References
W. D. Callister, Jr., Materials Science and Engineering – An Introduction, 7th Edition, John Wiley & Sons, 2006.
D. R, Askeland and P. P. Phule, The Science and Engineering of Materials, 4th Edition, Thomson Learning Vocational, 2003.
D. A. Porter, K. E. Easterling, M. Sherif, Phase Transformations in Metals and Alloys, 3rd edition, Chapman & Hall, 2009.
P. Haasen, Physical Metallurgy, 3RD edition, Cambridge University Press, 1996.
H. V. Keer, Principles of the Solid State, New Age International (P) Limited, 2005.
Presentation Slides6
7
Grading
Assignments 20
Term Papers 15
Assigned Presentation 15
Final Exam 50
Total 100
Crystal Structure – matter assumes a periodic shape
o Non-crystalline or amorphous “structures” exhibit no long range periodic shapes
o Crystal systems – not structures but potentials
FCC, BCC and HCP – common crystal structures for metals
Point, direction and planer ID’ing in crystals
X-ray diffraction and crystal structure
Crystallography
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5 6
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• Non dense, random packing
• Dense, ordered packing
Dense, ordered packed structures tend to havelower energies & thus are more stable.
Energy and PackingEnergy
r
typical neighbor
bond length
typical neighbor
bond energy
Energy
r
typical neighbor
bond length
typical neighbor
bond energy
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Crystaling Materials
Means: Periodic arrangement of atoms/ions over large atomic distances Leads to structure displaying LONG-
RANGE ORDER that is Measurable and Quantifiable
All metals, many ceramics, and some polymers exhibit this
“High Bond Energy” and a More Closely Packed Structure
STRUCTURES
Materials lacking long range order
Amorphous Materials
These less densely packed lower bond energy
“structures” can be found in some metals and are observed in almost all
ceramics, glass and many “plastics”
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Crystallography
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Crystallography
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11 12
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13
Crystallography
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Crystallography
Crystal Systems
7 crystal systems of varying symmetry are known
These systems are built by changing the lattice parameters:
a, b, and c are the edge lengths, , and are interaxial angles
Unit cell: smallest repetitive volume which contains the complete lattice pattern of a crystal.
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Crystal Systems
13 14
15 16
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Rare due to low packing density (only Polonium (Po) has this structure)
Close-packed directions are cube edges.
Coordination No. = 6(# nearest neighbors) for each atom as seen
Simple Cubic Structure (SC)
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*assume hard spheres
• APF for a simple cubic structure = 0.52
APF = a3
4
3p (0.5a) 31
atoms
unit cellatom
volume
unit cell
volume
Atomic Packing Factor (APF)
close-packed directions
aR=0.5a
contains (8 x 1/8) = 1 atom/unit cell Here: a = 2 × Rat
Where Rat is the atomic radius
𝐴𝑃𝐹 = 𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑎𝑡𝑜𝑚𝑠 𝑖𝑛 𝑢𝑛𝑖𝑡 𝑐𝑒𝑙𝑙
𝑉𝑜𝑙𝑢𝑚𝑒 𝑜𝑓 𝑢𝑛𝑖𝑡 𝑐𝑒𝑙𝑙
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Coordination # = 8
Atoms touch each other along cube diagonals within a unit cell.
- Note: All atoms are identical; the center atom is shaded differently only for ease of viewing.
ex: Cr, W, Fe (), Tantalum, Molybdenum
Body Centered Cubic Structure (BCC)
2 atoms/unit cell: (1 center) + (8 corners x 1/8)19
Atomic Packing Factor: BCC
a
APF =
4
3p ( 3a/4)32
atomsunit cell atom
volume
a3unit cell
volume
length = 4R =Close-packed directions:
3 a
APF for a body-centered cubic structure = 0.68
aR
a2
a3
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Coordination # = 12
Face Centered Cubic Structure (FCC)
4 atoms/unit cell: (6 face x ½) + (8 corners x 1/8)
Atoms touch each other along face diagonals. ABCABC... Stacking Sequence
- Note: All atoms are identical; the face-centered atoms are shaded differently only for ease of viewing.
ex: Al, Cu, Au, Pb, Ni, Pt, Ag
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APF for a face-centered cubic structure = 0.74
Atomic Packing Factor: FCC
The maximum achievable APF!
APF =
4
3p ( 2a/4)34
atomsunit cell atom
volume
a3unit cell
volume
Close-packed directions: length = 4R = a√2
Unit cell contains:6 x 1/2 + 8 x 1/8
= 4 atoms/unit cell
a
2 a
a = 22 R
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Coordination # = 12 APF = 0.74
3D Projection2D Projection
Hexagonal Close-Packed Structure (HCP)
6 atoms/unit cell
c/a = 1.633 (ideal)
c
a
A sites
B sites
A sitesBottom layer
Middle layer
Top layer
Atoms touch each other along face diagonals. ABAB... Stacking Sequence
ex: Cd, Mg, Ti, Zn
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We find that both
FCC & HCP are
highest density
packing schemes
(APF = .74) – this
illustration shows
their differences as
the closest packed
planes are “built-
up”.
HCP and FCC Stalking
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Theoretical Density, r
where n = number of atoms/unit cellA = atomic weight VC = Volume of unit cell = a3 for
cubicNA = Avogadro’s number
= 6.023 x 1023 atoms/mol
Density = r =
r =
aR
r = a3
52.002
atoms
unit cellmol
g
unit cell
volume atoms
mol
6.023x1023
rtheoretical
ractual
= 7.18 g/cm3
= 7.19 g/cm3
Ex: Cr (BCC) A = 52.00 g/mol , R = 0.125 nm,
n = 2
a = √
= 0.2883 nm25 26
Basic Crystallography
Repetition = Symmetry
Types of repetitiono Rotationo Translation
Rotationo What is rotational symmetry
This object is obviously symmetric. Can be rotated 90˚ without detection.o Symmetry is doing something that
looks like nothing has been done!
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Basic Crystallography A figure has rotational symmetry if
it can be rotated by an angle between 0˚ and 360˚ so that the image coincides with the preimage.
The angle of rotational symmetry is the smallest angle for which the figure can be rotated to coincide with itself.
The order of symmetry is the number of times the figure coincides with itself as it rotates through 360˚.28
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Locations in Lattices: Point Coordinates
Point coordinates for unit cell center are
a/2, b/2, c/2 ½ ½ ½
Point coordinates for unit cell (body diagonal) corner are 111
Translation: integer multiple of lattice constants identical position in another unit cell
z
x
ya b
c
000
111
y
z
2c
b
b
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Crystallographic Directions
1. Vector is repositioned (if necessary) to pass through the Unit Cell origin.
2. Read off line projections (to principal axes of unit cell) in terms of unit cell dimensions a, b, and c
3. Adjust to smallest integer values4. Enclose in square brackets, no
commas [uvw]
ex: 1, 0, ½ => 2, 0, 1 => [ 201 ]
-1, 1, 1 [ 111 ]=>
z
x
yx y z
Projections a/2 b 0c
Projections in terms of a, b, and c ½ 1 0
Reduction 1 2 0
Enclosure [brackets] [120]
where ‘overbar’ represents a negative index30
Linear Density – Considers Equivalence and is important in Slip
Linear Density of Atoms = LD =
ex: linear density of Al in [110] direction where a = 0.405 nm
a
[110]
# atoms
length
3.5 nm-1
a22LD ==
# atoms CENTERED on the direction of interest!Length is of the direction of interest within the Unit Cell
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Determining Angles Between Crystallographic Direction:
1 1 2 1 2 1 2
2 2 2 2 2 21 1 1 2 2 2
u u v v w wCos
u v w u v w
Where ui’s , vi’s & wi’s are the “Miller Indices” of the directions in question
– also, if a direction has the same Miller Indices as a plane, it is NORMAL to that plane
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HCP Crystallographic Directions
1. Vector repositioned (if necessary) to pass through origin.
2. Read off projections in terms of unitcell dimensions a1, a2, a3, or c
3. Adjust to smallest integer values4. Enclose in square brackets, no commas
[uvtw]
[ 1120 ]ex: ½, ½, -1, 0 =>
dashed red lines indicate projections onto a1 and a2 axes
a1
a2
a3
-a3
2
a2
2
a1
-a3
a1
a2
zAlgorithm
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HCP Crystallographic Directions Hexagonal Crystals
4 parameter Miller-Bravais lattice coordinates are related to the direction indices (i.e., u'v'w') in the ‘3 space’ Bravais lattice as follows.
'ww
t
v
u
)vu( +-
)'u'v2(3
1-
)'v'u2(3
1-
]uvtw[]'w'v'u[
Fig. 3.8(a), Callister 7e.
-a3
a1
a2
z
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Computing HCP Miller- Bravais Directional Indices (an alternative way):
-a3
a1
a2
z
We confine ourselves to the bravaisparallelopiped in the hexagon: a1-a2-Z and determine: (u’,v’w’)
Here: [1 1 0] - so now apply the models to create Miller Bravis indices
1 1 12 ' ' 2 1 1 13 3 3
1 1 12 ' ' 2 1 1 13 3 3
1 1 2 23 3 3
' 0
M-B Indices: [1120]
u u v
v v u
t u v
w w
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Defining Crystallographic Planes Miller Indices: Reciprocals of the (three) axial
intercepts for a plane, cleared of fractions & common multiples. All parallel planes have same Miller indices.
Algorithm (in cubic lattices this is direct)
1. Read off intercepts of plane with axes in
terms of a, b, c2. Take reciprocals of intercepts
3. Reduce to smallest integer values
4. Enclose in parentheses, no commas i.e.,
(hkl) families {hkl}36
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Crystallographic Planes -- families
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Crystallographic Planesz
x
ya b
c
4. Miller Indices (110)
Examplea b c
z
x
ya b
c
4. Miller Indices (100)
1. Intercepts 1 1 2. Reciprocals 1/1 1/1 1/
1 1 03. Reduction 1 1 0
1. Intercepts 1/2 2. Reciprocals 1/½ 1/ 1/
2 0 03. Reduction 2 0 0
Examplea b c
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Crystallographic Planesz
x
ya b
c
4. Miller Indices (634)
Example
1. Intercepts 1/2 1 3/4a b c
2. Reciprocals 1/½ 1/1 1/¾2 1 4/3
3. Reduction 6 3 4
(001)(010),
Family of Planes {hkl}
(100), (010),(001),Ex: {100} = (100),
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x y zIntercepts Intercept in terms of lattice parametersReciprocals Reductions
Enclosure
a -b c/2 -1 1/20 -1 2
N/A
(012)
Determine the Miller indices for the plane shown in the sketch
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Crystallographic Planes (HCP)
In hexagonal unit cells the same idea is used
Example
a1 a2 a3 c
4. Miller-Bravais Indices (1011)
1. Intercepts 1 -1 12. Reciprocals 1 1/
1 0 -1-1
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3. Reduction 1 0 -1 1 a2
a3
a1
z
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Crystallographic Planes
We want to examine the atomic packing of crystallographic planes – those with the same packing are equivalent and part of families
Iron foil can be used as a catalyst. The atomic packing of the exposed planes is important.
a) Draw (100) and (111) crystallographic planes
for Fe.
b) Calculate the planar density for each of these planes.
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Planar Density of (100) IronSolution: At T < 912C iron has the BCC structure.
(100)
Radius of iron R = 0.1241 nm
R3
34a
2D repeat unit
= Planar Density =a2
1
atoms
2D repeat unit
= (nm)2
atoms12.1
m2
atoms= 1.2 x 1019
12
R3
34area
2D repeat unitAtoms: wholly contained and centered in/on plane within U.C., area of plane in U.C.43
Planar Density of (111) IronSolution (cont): (111) plane 1/2 atom centered on plane/ unit cell
atoms in plane
atoms above plane
atoms below plane
ah2
3
a2
3*1/6= =
nm2
atoms7.0m2
atoms0.70 x 1019Planar Density =
atoms
2D repeat unit
area
2D repeat unit
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3
R
Area 2D Unit: ½ hb = ½*[(3/2)a][(2)a]=1/2(3)a2=8R2/(3)
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CERAMIC AND OTHER UNIT CELLS
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Cesium chloride (CsCl) unit cell showing(a) ion positions and the two ions per lattice point and(b) full-size ions.
Note that the Cs+−Cl− pair associated with a given lattice point is not a molecule because the ionic bonding is nondirectional and because a given Cs+ is equally bonded to eight adjacent Cl−, and vice versa.
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Sodium chloride (NaCl) structure showing (a) ion positions in a unit cell, (b) full-size ions, and (c) many adjacent unit cells.
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Fluorite (CaF2) unit cell showing (a) ion positions and (b) full-size ions.
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SiO4
4
The cristobalite (SiO2) unit cell showing (a) ion positions(b) full-size ions and (c) the connectivity of SiO4
4- tetrahedra.
Each tetrahedron has a Si4+ at its center. In addition, an O2- would be at each corner of each tetrahedron and is shared with an adjacent tetrahedron. 49
Many crystallographic forms of SiO2 are stable as they are heated from room temperature to melting temperature. Each form represents a different way to connect adjacent SiO4
4- tetrahedra
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Polymorphism: Also in Metals Two or more distinct crystal structures for the same
material (allotropy/polymorphism)
titanium (HCP), (BCC)-Ti
carbon:diamond, graphite
BCC
FCC
BCC
1538ºC
1394ºC
912ºC
-Fe
-Fe
-Fe
liquid
iron system:
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The corundum (Al2O3) unit cell is shown superimposed on the repeated stacking of layers of close-packed O2− ions.
The Al3+ ions fill two-thirds of the small (octahedral) interstices between adjacent layers.
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Exploded view of the kaolinite unit cell, 2(OH)4Al2Si2O5.
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(a) An exploded view of the graphite (C) unit cell. (b) A schematic of the nature of graphite’s layered structure.
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(a) C60 molecule, or buckyball.
(b) Cylindrical array of hexagonal rings of carbon atoms, or buckytube.
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Arrangement of polymeric chains in the unit cell of polyethylene. The dark spheres are carbon atoms, and the light spheres are hydrogen atoms. The unit-cell dimensions are 0.255 nm × 0.494 nm × 0.741 nm.
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Diamond cubic unit cell showing
(a) atom positions. There are two atoms per lattice point (note the outlined example). Each atom is tetrahedrally coordinated.
(b) The actual packing of full-size atoms associated with the unit cell.
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Zinc blende (ZnS) unit cell showing
(a) ion positions. There are two ions per lattice point (note the outlined example). Compare this structure with the diamond cubic structure.
(b) The actual packing of full-size ions associated with the unit cell.
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Densities of Material Classesrmetals > rceramics > rpolymers
Why?
Data from Table B1, Callister 7e.
r(g
/cm
)3
Graphite/ Ceramics/ Semicond
Metals/ Alloys
Composites/ fibers
Polymers
1
2
20
30
*GFRE, CFRE, & AFRE are Glass,Carbon, & Aramid Fiber-ReinforcedEpoxy composites (values based on60% volume fraction of aligned fibers
in an epoxy matrix).10
3
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0.30.40.5
Magnesium
Aluminum
Steels
Titanium
Cu,Ni
Tin, Zinc
Silver, Mo
TantalumGold, WPlatinum
Graphite
Silicon
Glass -sodaConcrete
Si nitrideDiamondAl oxide
Zirconia
HDPE, PSPP, LDPE
PC
PTFE
PETPVCSilicone
Wood
AFRE*
CFRE*
GFRE*
Glass fibers
Carbon fibers
Aramid fibers
Metals have...• close-packing
(metallic bonding)• often large atomic masses
Ceramics have...• less dense packing• often lighter elements
Polymers have...• low packing density
(often amorphous)• lighter elements (C,H,O)
Composites have...• intermediate values
In general
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• Some engineering applications require single crystals:
• Properties of crystalline materials often related to crystal structure.Ex: Quartz fractures more easily along some crystal planes than others.
o Diamond single crystals for abrasives o turbine blades
(Courtesy of Pratt and Whitney).
(Courtesy of Martin Deakins, GE Superabrasives.)
Crystals as Building Blocks
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• Most engineering materials are polycrystals.
• Nb-Hf-W plate with an electron beam weld.• Each "grain" is a single crystal.• If grains are randomly oriented, overall component
properties are not directional.• Grain sizes typically ranges from 1 nm to 2 cm
(i.e., from a few to millions of atomic layers).
(Courtesy of Paul E. Danielson, Teledyne Wah Chang Albany)
1 mm
Polycrystals
Isotropic
Anisotropic
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• Single Crystals-Properties vary withdirection: anisotropic.
-Example: the modulusof elasticity (E) in BCC iron:
• Polycrystals
-Properties may/may notvary with direction.
-If grains are randomlyoriented: isotropic.(Epoly iron = 210 GPa)
-If grains are textured,anisotropic.
200 mm
Source of data is R.W. Hertzberg, Deformation and Fracture Mechanics of Engineering Materials, 3rd ed., John Wiley and Sons, 1989.
courtesy of L.C. Smith and C. Brady, the National Bureau of Standards, Washington, DC [now the National Institute of Standards and Technology, Gaithersburg, MD].
Single vs PolycrystalsE (diagonal) = 273 GPa
E (edge) = 125 GPa
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Effects of Anisotropy:
Modulus of Elasticity values for several metals at various crystallographic orientations
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X-Ray Diffraction
Diffraction gratings must have spacings comparable to the wavelength of diffracted radiation.
Can’t resolve spacings Spacing is the distance between parallel planes of
atoms. 64
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Relationship of the Bragg angle (θ) and the experimentally measured diffraction angle (2θ).
X-ray intensity (from detector)
2c
d n2 sinc
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X-Rays to Determine Crystal Structure
X-ray intensity (from detector)
c
d n
2 sinc
Measurement of critical angle, c, allows computation of planar spacing, d.
• Incoming X-rays diffract from crystal planes.
Adapted from Fig. 3.19, Callister 7e.
reflections must be in phase for a detectable signal!
spacing between planes
d
extra distance traveled by wave “2”
2 2 2hkl
ad
h k l
For Cubic Crystals:
h, k, l are Miller Indices 66
Figure 3.34 (a) An x-ray diffractometer. (Courtesy of Scintag, Inc.) (b) A schematic of the experiment.
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X-Ray Diffraction Pattern
Adapted from Fig. 3.20, Callister 5e.
(110)
(200)
(211)
z
x
ya b
c
Diffraction angle 2
Diffraction pattern for polycrystalline -iron (BCC)
Inte
nsity
(re
lativ
e)
z
x
ya b
cz
x
ya b
c
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Diffraction in Cubic Crystals:
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Atoms may assemble into crystalline or amorphous structures.
Common metallic crystal structures are FCC, BCC, and HCP. Coordination number and atomic packing factor are the same for both FCC and HCP crystal structures.
We can predict the density of a material, provided we know the atomic weight, atomic radius, and crystal geometry (e.g., FCC, BCC, HCP)
Crystallographic points, directions and planes are specified in terms of indexing schemes.Crystallographic directions and planes are related to atomic linear densities and planar densities.
SUMMARY
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Materials can be single crystals or polycrystalline. Material properties generally vary with single crystal orientation (i.e., they are anisotropic), but are generally non-directional (i.e., they are isotropic) in polycrystals with randomly oriented grains.
Some materials can have more than one crystal structure. This is referred to as polymorphism (or allotropy).
X-ray diffraction is used for crystal structure and interplanarspacing determinations.
SUMMARY
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