LECTURE 18 ENGR 151 Materials of Engineering
LECTURE 18
ENGR 151
Materials of Engineering
2
COORDINATION NUMBER AND IONIC RADII
2
r cation r anion
Coord.
Number
< 0.155
0.155 - 0.225
0.225 - 0.414
0.414 - 0.732
0.732 - 1.0
3
4
6
8
linear
triangular
tetrahedral
octahedral
cubic
3
ROCK SALT STRUCTURE Same concepts can be applied to ionic solids in general.
Example: NaCl (rock salt) structure
rNa = 0.102 nm
rNa/rCl = 0.564
cations (Na+) prefer octahedral sites
Adapted from Fig. 12.2,
Callister & Rethwisch 9e.
rCl = 0.181 nm
• Structure is similar to two intermeshed
FCC lattices
4
MGO AND FEO
O2- rO = 0.140 nm
Mg2+ rMg = 0.072 nm
rMg/rO = 0.514
cations prefer octahedral sites
So each Mg2+ (or Fe2+) has 6 neighbor oxygen atoms
Adapted from Fig. 12.2,
Callister & Rethwisch 9e.
MgO and FeO also have the NaCl structure
5
AX CRYSTAL STRUCTURES
Fig. 12.3, Callister & Rethwisch 9e.
Cesium Chloride structure:
Since 0.732 < 0.939 < 1.0,
cubic sites preferred
So each Cs+ has 8 neighbor Cl-
AX–Type Crystal Structures include NaCl, CsCl, and zinc blende
6
AX2 CRYSTAL STRUCTURES
• Calcium Fluorite (CaF2)
• Cations in cubic sites
• UO2, ThO2, ZrO2, CeO2
• Antifluorite structure –
positions of cations and
anions reversed
• Fluorite is used to
construct elements in high
performance optics
Fig. 12.5, Callister & Rethwisch 9e.
Fluorite structure
7
ABX3 CRYSTAL STRUCTURES
Fig. 12.6, Callister &
Rethwisch 9e.
• Perovskite structure
Ex: complex oxide
BaTiO3
8
• On the basis of ionic radii, what crystal structure
would you predict for FeO?
• Answer:
5500
1400
0770
anion
cation
.
.
.
r
r
=
=
based on this ratio,
-- coord # = 6 because
0.414 < 0.550 < 0.732
-- crystal structure is similar
to NaCl Data from Table 12.3,
Callister & Rethwisch 9e.
EXAMPLE PROBLEM: PREDICTING THE
CRYSTAL STRUCTURE OF FEO
Ionic radius (nm)
0.053
0.077
0.069
0.100
0.140
0.181
0.133
Cation
Anion
Al 3+
Fe 2 +
Fe 3+
Ca 2+
O 2-
Cl -
F -
9
DENSITY COMPUTATIONS FOR
CERAMICS
Number of formula units/unit cell
Volume of unit cell
Avogadro’s number
= sum of atomic weights of all anions in formula unit
= sum of atomic weights of all cations in formula unit
10
DENSITY COMPUTATIONS FOR
CERAMICS – EXAMPLE PROBLEM
11
DENSITY COMPUTATIONS FOR
CERAMICS – EXAMPLE PROBLEM
Most common elements on earth are Si & O
SiO2 (silica) polymorphic forms are quartz,
crystobalite, & tridymite
The strong Si-O bonds lead to a high melting
temperature (1710ºC) for this material
12
SILICATE CERAMICS
Si4+
O2-
Figs. 12.9 & 12.10, Callister &
Rethwisch 9e crystobalite
13
SILICATE CERAMICS
Rather than attempting to characterize silicate
ceramics in terms of crystal structures, we use the
SiO44- tetrahedron.
Negatively-charged entity is characterized by strong
covalent Si-O bonds.
Various silicate structures generated by 1-, 2- and 3-
dimensional arrangements of silicate structures.
Si4+
O2-
14
SILICATE CERAMICS
15
SILICATE CERAMICS
16
Bonding of adjacent SiO44- accomplished by the
sharing of common corners, edges, or faces
SIMPLE SILICATES
Mg2SiO4 Ca2MgSi2O7
Adapted from Fig.
12.12, Callister &
Rethwisch 9e.
Presence of cations such as Ca2+, Mg2+, & Al3+
1. maintain charge neutrality, and
2. ionically bond SiO44- to one another
17
• Quartz is crystalline
SiO2:
• Basic Unit: Glass is noncrystalline (amorphous)
• Fused silica is SiO2 to which no
impurities have been added
• Other common glasses contain
impurity ions such as Na+, Ca2+,
Al3+, and B3+
(soda glass)
Adapted from Fig. 12.11,
Callister & Rethwisch 9e.
GLASS STRUCTURE
Si0 4 tetrahedron 4-
Si 4+
O 2 -
Si 4+
Na +
O 2 -
18
LAYERED SILICATES
Layered silicates (e.g., clays, mica, talc)
SiO4 tetrahedra connected together to form 2-D plane
A net negative charge is associated with each (Si2O5)
2- unit Oxygen ion out of the plane of the page
Negative charge balanced by adjacent plane rich in positively charged cations
Fig. 12.13, Callister
& Rethwisch 9e.
19
Kaolinite clay alternates (Si2O5)2- layer with Al2(OH)4
2+
layer
LAYERED SILICATES (CONT)
Note: Adjacent sheets of this type are loosely bound to one another by van der Waal’s forces.
Fig. 12.14, Callister &
Rethwisch 9e.
20
POLYMORPHIC FORMS OF CARBON
Diamond tetrahedral bonding of
carbon hardest material known
very high thermal conductivity high refractive index
large single crystals – gem stones
small crystals – used to grind/cut other materials
diamond thin films hard surface coatings – used
for cutting tools, medical devices, etc.
Fig. 12.16, Callister &
Rethwisch 9e.
Difficult to initiate slip – no
straightforward slip plane
structure
21
POLYMORPHIC FORMS OF CARBON (CONT)
Graphite layered structure – parallel hexagonal arrays of
carbon atoms
weak van der Waal’s forces between layers
planes slide easily over one another -- good lubricant
Fig. 12.17, Callister
& Rethwisch 9e.
22
• Vacancies
-- vacancies exist in ceramics for both cations and anions
• Interstitials -- interstitials exist for cations
-- interstitials are not normally observed for anions because anions
are large relative to the interstitial sites
Fig. 12.18, Callister & Rethwisch 9e. (From W.G. Moffatt, G.W. Pearsall, and J.
Wulff, The Structure and Properties of
Materials, Vol. 1, Structure, p.78. Copyright
©1964 by John Wiley & Sons, New York.
Reprinted by permission of John Wiley and
Sons, Inc.)
POINT DEFECTS IN CERAMICS (I)
Cation Interstitial
Cation Vacancy
Anion Vacancy
23
• Frenkel Defect -- a cation vacancy-cation interstitial pair.
• Shottky Defect -- a paired set of cation and anion vacancies.
• Equilibrium concentration of defects
POINT DEFECTS IN CERAMICS (II)
Shottky
Defect:
Frenkel
Defect
Fig. 12.19, Callister & Rethwisch 9e. (From W.G. Moffatt, G.W. Pearsall, and J.
Wulff, The Structure and Properties of
Materials, Vol. 1, Structure, p.78. Copyright
©1964 by John Wiley & Sons, New York.
Reprinted by permission of John Wiley and
Sons, Inc.)
24
• Electroneutrality (charge balance) must be maintained
when impurities are present
• Ex: NaCl
IMPERFECTIONS IN CERAMICS
Na + Cl -
• Substitutional cation impurity
without impurity Ca 2+ impurity with impurity
Ca 2+
Na +
Na +
Ca 2+
cation vacancy
• Substitutional anion impurity
without impurity O 2- impurity
O 2-
Cl -
an ion vacancy
Cl -
with impurity
25
EQUILIBRIUM CONCENTRATION OF
FRENKEL DEFECTS
26
EQUILIBRIUM CONCENTRATION OF
SCHOTTKY DEFECTS – AX-TYPE
COMPOUND
27
EXAMPLE PROBLEM
28
EXAMPLE PROBLEM
29
CERAMIC PHASE DIAGRAMS
30
CERAMIC PHASE DIAGRAMS MgO-Al2O3 diagram:
Fig. 12.23, Callister &
Rethwisch 9e. [Adapted from B. Hallstedt,
“Thermodynamic Assessment
of the System MgO–Al2O3,” J.
Am. Ceram. Soc., 75[6], 1502
(1992). Reprinted by
permission of the American
Ceramic Society.]
31
MECHANICAL PROPERTIES
Ceramic materials are more brittle than metals.
Why is this so?
Consider mechanism of deformation
In crystalline, by dislocation motion
In highly ionic solids, dislocation motion is difficult
few slip systems
resistance to motion of ions of like charge (e.g., anions)
past one another
32
REPRESENTATION OF CRACK ORIGINS
Crack interacts with:
Microstructure of
material
Stress
Elastic waves that are
generated
33
MICROSCOPIC CRACK FEATURES
34
MICROSCOPIC CRACK FEATURES
35
STRESS-STRAIN BEHAVIOR
Cannot use tensile testing to predict stress-strain
behavior of ceramics
Difficult to prepare and test specimens with requisite
geometry
Difficult to grip brittle materials without fracturing them
Ceramics fail after only about 0.1% strain – need
precise alignment to avoid bending effects
Transverse bending test employed – flexural
loading
At point of loading, top surface of specimen is in state
of compression, bottom surface of specimen is in state
of tension
36
• Room T behavior is usually elastic, with brittle failure.
• 3-Point Bend Testing often used. -- tensile tests are difficult for brittle materials.
Adapted from Fig. 12.30,
Callister & Rethwisch 9e.
FLEXURAL TESTS – MEASUREMENT OF
ELASTIC MODULUS
F L/2 L/2
δ = midpoint
deflection
cross section
R
b
d
rect. circ.
• Determine elastic modulus according to:
F x
linear-elastic behavior δ
F
δ slope =
(rect. cross section)
(circ. cross section)
37
• 3-point bend test to measure room-T flexural strength.
Adapted from Fig. 12.30,
Callister & Rethwisch 9e.
FLEXURAL TESTS – MEASUREMENT OF
FLEXURAL STRENGTH
F L/2 L/2
δ = midpoint
deflection
cross section
R
b
d
rect. circ.
location of max tension
• Flexural strength: • Typical values:
Data from Table 12.5, Callister & Rethwisch 9e.
Si nitride
Si carbide
Al oxide
glass (soda-lime)
250-1000
100-820
275-700
69
304
345
393
69
Material σ fs (MPa) E(GPa)
(rect. cross section)
(circ. cross section)
38
PLASTIC DEFORMATION IN CERAMICS
Plastic deformation in ceramics is limited – more
of a tendency to fracture
Crystalline ceramics
Ionic structure: Limited number of slip systems for
dislocations due to electrically charged nature of
particles – attractive/repulsive forces resist motion
Covalent structure: Strong covalent bonds limit
dislocation motion, dislocation structures are complex
Noncrystalline ceramics
No dislocation motion; rather plastic deformation
occurs via viscous flow (similar to liquids)
39
SUMMARY
• Interatomic bonding in ceramics is ionic and/or covalent.
• Ceramic crystal structures are based on: -- maintaining charge neutrality
-- cation-anion radii ratios.
• Imperfections
-- Atomic point: vacancy, interstitial (cation), Frenkel, Schottky
-- Impurities: substitutional, interstitial
-- Maintenance of charge neutrality
• Room-temperature mechanical behavior – flexural tests
-- linear-elastic; measurement of elastic modulus
-- brittle fracture; measurement of flexural modulus
40
HOMEWORK
Due Monday, May 8th
12.3, 12.4, 12.5, 12.6
Quiz next Wednesday, April 26th Topic – stress, strain, and Young’s modulus and Poisson’s ratio