lectures 2 to 5 - crystallography
TRANSCRIPT
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7/23/2019 Lectures 2 to 5 - Crystallography
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ISSUES TO ADDRESS...
How do atoms assemble into solid structures?
(for now, focus on metals)
its structure?
When do material properties vary with the
sample (i.e., part) orientation?
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Energy and Packing
Non dense, random packingEnergy
typical neighbor
r
bond length
typical neighbor
Dense, ordered packing
on energy
Energy
typical neighborbond length
rtypical neighborbond energy
2
,
Materials and Packing
atoms pack in periodic, 3D arraysCrystalline materials...
-metals
-many ceramics
-some ol mers cr stalline SiO2
typical of:
Adapted from Fig. 3.22 (a), Callister 7e.
Si Oxygen
atoms have no periodic packing
oncrys a ne ma er a s...
-complex structures occurs for:
-rapid cooling
noncrystalline SiO2"Amorphous" = Noncrystalline
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Adapted from Fig. 3.22(b ), Callister 7e.
Crystal Structure
Space lattice: Three dimensional network of imagina
lines connectin the atoms is called the s ace latti
(A three dimensional pattern of points in space).
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complete lattice pattern of a crystal (The smallest unit having
the full symmetry of the crystal).
7 crystal systems
The specific unit cell for metal
The edges a, b, and c; and , and
5Fig. 3.4, Callister 7e.
Crystal Systems
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Metallic Crystal Structures
How can we stack metal atoms to minimize
em t s ace?
2-dimensions
vs.
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ow s ac ese - ayers o ma e - s ruc ures
Metallic Crystal Structures
Tend to be densely packed.
- Typically, only one element is present, so all atomic
radii are the same.
- Metallic bonding is not directional.
- Nearest neighbor distances tend to be small in
order to lower bond energy.
- Electron cloud shields cores from each other
Have the simplest crystal structures.
We will examine three such structures...
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Simple Cubic Structure (SC)
Rare due to low packing denisty (only Po has this structure)
Close-packed directions are cube edges.
Coordination # = 6
(# nearest neighbors)
9(Courtesy P.M. Anderson)
Atomic Packing Factor (APF)
APF =Volume of atoms in unit cell*
Volume of unit cell
*assume hard spheres
.
atomsvolume
APF =
4
3 (0.5a) 31unit cella
R=0.5a
a3
unit cell
volume
close-packed directionscontains 8 x 1/8 =
10
Adapted from Fig. 3.23,
Callister 7e.
1 atom/unit cell
Body Centered Cubic Structure (BCC)
Atoms touch each other along cube diagonals.--Note: All atoms are identical; the center atom is shaded
=
eren y ony or ease o v ewng.
ex: Cr, W, Fe (), Tantalum, Molybdenum
Adapted from Fig. 3.2,
Callister 7e.
11(Courtesy P.M. Anderson)
2 atoms/unit cell: 1 center + 8 corners x 1/8
Atomic Packing Factor: BCC APF for a body-centered cubic structure = 0.68
a3
a
-
a2
length = 4R=
3 aa
RAdapted from
Fig. 3.2(a), Callister 7e.
APF =
4
3 ( 3a/4)32unit cell atom
vo ume
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a3
unit cell
volume
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Crystallographic Directions
1. Vector repositioned (if necessary) to pass
z Algorithm
hrough origin.
2. Read off projections in terms of
unit cell dimensions a, b, and c
.
4. Enclose in square brackets, no commas
[uvw]x
y
ex: 1, 0, => 2, 0, 1 => [ 201]
-1, 1, 1 where overbar represents a
negative index
[111]=>
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families of directions
Linear Density
Linear Density of Atoms LD =Unit length of direction vec
Number of atoms
ex: linear density of Al in [110][110]
a = 0.405 nm
a# atoms
2
length
3.5 nma2
LD
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HCP Crystallographic Directionsz
Algorithm
. ec or repos one necessary o pass
through origin.
2. Read off projections in terms of unit
1, 2, 3,
3. Adjust to smallest integer values
4. Enclose in square brackets, no commas-a3
2
Adapted from Fig. 3.8(a), Callister 7e.
a2
-a32
a2
a1
[1120]ex: , , -1, 0 =>
dashed red lines indicate
a3
2
a1
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projections onto a1 and a2 axes a1
HCP Crystallographic Directions Hexagonal Crystals
4 parameter Miller-Bravais lattice coordinates are
' ' 're a e o e rec on n ces .e., u v w as
follows.z
u )'v'u2(1
-
]uvtw[]'w'v'u[
v )'u'v2(1
-a2
'ww
t )vu( +--
a3
a1
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Fig. 3.8(a), Callister 7e.
Crystallographic Planes
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Adapted from Fig. 3.9, Callister 7e.
Crystallographic Planes
Miller Indices: Reciprocals of the (three) axialintercepts for a plane, cleared of fractions &common multiples. All parallel planes have
same Miller indices.
Algorithm.
terms of a, b, c2. Take reciprocals of intercepts
.4. Enclose in parentheses, no
commas i.e., (hkl)
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Planar Density of (111) IronSolution (cont): (111) plane 1 atom in plane/ unit surface cell
atoms in planea2atoms above plane
atoms below plane
ah23
333
2
2
R3
16R
3
42a3ah2area
atoms
1
= =nm2
atoms7.0
m2atoms
0.70 x 1019
316Planar Density =
2D repeat unit
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R32D repeat unit
X-Ray Diffraction
Diffraction ratin s must have s acin s com arable tothe wavelength of diffracted radiation.
Cant resolve spacings
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atoms.
X-Rays to Determine Crystal Structure Incoming X-rays diffract from crystal planes.
Adapted from Fig. 3.19 ,
reflections mustbe in phase fora detectable signal
extradistance
Callister 7e.
spacingbetween
planes
d
travelledby wave 2
X-rayintensit
nMeasurement of
(from
detector)
2 sinc , c,
allows computation of
planar spacing, d.
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c
X-Ray Diffraction Patternz
c
zc
z
c
(110)
x
a b
tive)
x
ya b
x
ya b
ensity(rela
Int
Diffraction angle 2
Diffraction pattern for polycrystalline -iron (BCC)
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Adapted from Fig. 3.20, Callister 5e.
SUMMARY
Atoms may assemble into crystalline or amorphous
.
Common metallic crystal structures are FCC, BCC, and
HCP. Coordination numberand atomic packing factor
We can predict the density of a material, provided we
are the same for both FCC and HCP crystal structures.
, ,
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.
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SUMMARY
Materials can be single crystals orpolycrystalline.
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
Some materials can have more than one crystal
with randomly oriented grains.
s ruc ure. s s re erre o as po ymorp sm or
allotropy).
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interplanar spacing determinations.
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