1. 1
ISSUES TO ADDRESS...
• How do atoms assemble into solid structures?
• How does the density of a material depend on
its structure?
• When do material properties vary with the
sample (i.e., part) orientation?
The Structure of Crystalline Solids
2. 2
• Non dense, random packing
• Dense, ordered packing
Dense, ordered packed structures tend to have
lower energies.
Energy and Packing
Energy
r
typical neighbor
bond length
typical neighbor
bond energy
Energy
r
typical neighbor
bond length
typical neighbor
bond energy
3. 3
• atoms pack in periodic, 3D arrays
Crystalline materials...
-metals
-many ceramics
-some polymers
• atoms have no periodic packing
Noncrystalline materials...
-complex structures
-rapid cooling
crystalline SiO2
noncrystalline SiO2
"Amorphous" = Noncrystalline
Adapted from Fig. 3.23(b),
Callister & Rethwisch 8e.
Adapted from Fig. 3.23(a),
Callister & Rethwisch 8e.
Materials and Packing
Si Oxygen
• typical of:
• occurs for:
4. 4
Metallic Crystal Structures
• How can we stack metal atoms to minimize
empty space?
2-dimensions
vs.
Now stack these 2-D layers to make 3-D structures
5. 5
• Tend to be densely packed.
• Reasons for dense packing:
- 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...
Metallic Crystal Structures
6. 6
• Rare due to low packing density (only Po has this structure)
• Close-packed directions are cube edges.
• Coordination # = 6
(# nearest neighbors)
Simple Cubic Structure (SC)
Click once on image to start animation
(Courtesy P.M. Anderson)
7. 7
• APF for a simple cubic structure = 0.52
APF =
a3
4
3
(0.5a) 3
1
atoms
unit cell
atom
volume
unit cell
volume
Atomic Packing Factor (APF)
APF =
Volume of atoms in unit cell*
Volume of unit cell
*assume hard spheres
Adapted from Fig. 3.24,
Callister & Rethwisch 8e.
close-packed directions
a
R=0.5a
contains 8 x 1/8 =
1 atom/unit cell
8. 8
• Coordination # = 8
Adapted from Fig. 3.2,
Callister & Rethwisch 8e.
• Atoms touch each other along cube diagonals.
--Note: All atoms are identical; the center atom is shaded
differently only for ease of viewing.
Body Centered Cubic Structure (BCC)
ex: Cr, W, Fe (), Tantalum, Molybdenum
2 atoms/unit cell: 1 center + 8 corners x 1/8
Click once on image to start animation
(Courtesy P.M. Anderson)
9. 9
Atomic Packing Factor: BCC
a
APF =
4
3
( 3a/4)3
2
atoms
unit cell atom
volume
a3
unit cell
volume
length = 4R =
Close-packed directions:
3 a
• APF for a body-centered cubic structure = 0.68
a
R
Adapted from
Fig. 3.2(a), Callister &
Rethwisch 8e.
a
2
a
3
10. 10
• Coordination # = 12
Adapted from Fig. 3.1, Callister & Rethwisch 8e.
• Atoms touch each other along face diagonals.
--Note: All atoms are identical; the face-centered atoms are shaded
differently only for ease of viewing.
Face Centered Cubic Structure (FCC)
ex: Al, Cu, Au, Pb, Ni, Pt, Ag
4 atoms/unit cell: 6 face x 1/2 + 8 corners x 1/8
Click once on image to start animation
(Courtesy P.M. Anderson)
11. 11
• APF for a face-centered cubic structure = 0.74
Atomic Packing Factor: FCC
maximum achievable APF
APF =
4
3
( 2a/4)3
4
atoms
unit cell atom
volume
a3
unit cell
volume
Close-packed directions:
length = 4R = 2 a
Unit cell contains:
6 x1/2 + 8 x1/8
= 4 atoms/unit cell
a
2 a
Adapted from
Fig. 3.1(a),
Callister &
Rethwisch 8e.
12. 12
A sites
B B
B
B
B
B B
C sites
C C
C
A
B
B sites
• ABCABC... Stacking Sequence
• 2D Projection
• FCC Unit Cell
FCC Stacking Sequence
B B
B
B
B
B B
B sites
C C
C
A
C C
C
A
A
B
C
13. 13
• Coordination # = 12
• ABAB... Stacking Sequence
• APF = 0.74
• 3D Projection • 2D Projection
Adapted from Fig. 3.3(a),
Callister & Rethwisch 8e.
Hexagonal Close-Packed Structure
(HCP)
6 atoms/unit cell
ex: Cd, Mg, Ti, Zn
• c/a = 1.633
c
a
A sites
B sites
A sites Bottom layer
Middle layer
Top layer
14. 14
Theoretical Density,
where n = number of atoms/unit cell
A = atomic weight
VC = Volume of unit cell = a3
for cubic
NA = Avogadro’s number
= 6.022 x 1023
atoms/mol
Density = =
VC NA
n A
=
Cell
Unit
of
Volume
Total
Cell
Unit
in
Atoms
of
Mass
15. 15
• Ex: Cr (BCC)
A = 52.00 g/mol
R = 0.125 nm
n = 2 atoms/unit cell
theoretical
a = 4R/ 3 = 0.2887 nm
actual
a
R
=
a3
52.00
2
atoms
unit cell
mol
g
unit cell
volume atoms
mol
6.022x1023
Theoretical Density,
= 7.18 g/cm3
= 7.19 g/cm3
Adapted from
Fig. 3.2(a), Callister &
Rethwisch 8e.
16. 16
Densities of Material Classes
metals > ceramics > polymers
Why?
Data from Table B.1, Callister & Rethwisch, 8e.
(g/cm
)
3
Graphite/
Ceramics/
Semicond
Metals/
Alloys
Composites/
fibers
Polymers
1
2
20
30
Based on data in Table B1, Callister
*GFRE, CFRE, & AFRE are Glass,
Carbon, & Aramid Fiber-Reinforced
Epoxy composites (values based on
60% volume fraction of aligned fibers
in an epoxy matrix).
10
3
4
5
0.3
0.4
0.5
Magnesium
Aluminum
Steels
Titanium
Cu,Ni
Tin, Zinc
Silver, Mo
Tantalum
Gold, W
Platinum
Graphite
Silicon
Glass -soda
Concrete
Si nitride
Diamond
Al oxide
Zirconia
HDPE, PS
PP, LDPE
PC
PTFE
PET
PVC
Silicone
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
17. 17
• Some engineering applications require single crystals:
• Properties of crystalline materials
often related to crystal structure.
(Courtesy P.M. Anderson)
-- Ex: Quartz fractures more easily
along some crystal planes than
others.
-- diamond single
crystals for abrasives
-- turbine blades
Fig. 8.33(c), Callister &
Rethwisch 8e. (Fig. 8.33(c)
courtesy of Pratt and
Whitney).
(Courtesy Martin Deakins,
GE Superabrasives,
Worthington, OH. Used with
permission.)
Crystals as Building Blocks
18. 18
• 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 range from 1 nm to 2 cm
(i.e., from a few to millions of atomic layers).
Adapted from Fig. K,
color inset pages of
Callister 5e.
(Fig. K is courtesy of
Paul E. Danielson,
Teledyne Wah Chang
Albany)
1 mm
Polycrystals
Isotropic
Anisotropic
19. 19
• Single Crystals
-Properties vary with
direction: anisotropic.
-Example: the modulus
of elasticity (E) in BCC iron:
Data from Table 3.3,
Callister & Rethwisch
8e. (Source of data is
R.W. Hertzberg,
Deformation and
Fracture Mechanics of
Engineering Materials,
3rd ed., John Wiley and
Sons, 1989.)
• Polycrystals
-Properties may/may not
vary with direction.
-If grains are randomly
oriented: isotropic.
(Epoly iron = 210 GPa)
-If grains are textured,
anisotropic.
200 m Adapted from Fig.
4.14(b), Callister &
Rethwisch 8e.
(Fig. 4.14(b) is 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 Polycrystals
E (diagonal) = 273 GPa
E (edge) = 125 GPa
20. 20
Polymorphism
• Two or more distinct crystal structures for the same
material (allotropy/polymorphism)
titanium
, -Ti
carbon
diamond, graphite
BCC
FCC
BCC
1538ºC
1394ºC
912ºC
-Fe
-Fe
-Fe
liquid
iron system
21. 21
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.
22. 22
X-Ray Diffraction Pattern
Adapted from Fig. 3.22, Callister 8e.
(110)
(200)
(211)
z
x
y
a b
c
Diffraction angle 2
Diffraction pattern for polycrystalline -iron (BCC)
Intensity
(relative)
z
x
y
a b
c
z
x
y
a b
c
23. 23
SUMMARY
• Atoms may assemble into crystalline or
amorphous 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).
• 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.
• 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.
24. 24
• Some materials can have more than one crystal
structure. This is referred to as polymorphism (or
allotropy).
SUMMARY
• 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.
• X-ray diffraction is used for crystal structure and
interplanar spacing determinations.
![19
• Single Crystals
-Properties vary with
direction: anisotropic.
-Example: the modulus
of elasticity (E) in BCC iron:
Data from Table 3.3,
Callister & Rethwisch
8e. (Source of data is
R.W. Hertzberg,
Deformation and
Fracture Mechanics of
Engineering Materials,
3rd ed., John Wiley and
Sons, 1989.)
• Polycrystals
-Properties may/may not
vary with direction.
-If grains are randomly
oriented: isotropic.
(Epoly iron = 210 GPa)
-If grains are textured,
anisotropic.
200 m Adapted from Fig.
4.14(b), Callister &
Rethwisch 8e.
(Fig. 4.14(b) is 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 Polycrystals
E (diagonal) = 273 GPa
E (edge) = 125 GPa](https://image.slidesharecdn.com/week-3-day-1-structure-of-crystalline-solids-250422084027-9f609ab3/85/Week-3-Day-1-Structure-of-Crystalline-Solids-ppt-19-320.jpg)
