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7/17/2019 Amorphous
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Amorphous StructuresCh.
High Temperature Materials
Course KGP003
By
Docent. N. Menad
Dept. of Chemical Engineering
and Geosciences Div. Of
process metallurgy
Luleå University of Technology( Sweden )
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An amorphous solid is a solid in which there is no long-range order of the positions
of the atoms. (Solids in which there is long-range atomic order are called crystalline solids.) Most classes of solid materials can be found or prepared in an amorphous
form. Ex:
common window glass is an amorphous ceramic, many polymers (such as
polystyrene) are amorphous, and even foods such as cotton candy are amorphous
solids.
Amorphous materials are often prepared by rapidly cooling molten material. The
cooling reduces the mobility of the material's molecules before they can pack into a
more thermodynamically favourable crystalline state. Amorphous materials can also
be produced by additives which interfere with the ability of the primary constituent to
crystallize. For example addition of soda to silicon dioxide results in window glass
and the addition of glycols to water results in a vitrified solid.
Some materials, such as metals, are difficult to prepare in an amorphous state. Unlessa material has a high melting temperature (as ceramics do) or a low crystallization
energy (as polymers tend to), cooling must be done extremely rapidly.
Amorphous solids can exist in two distinct states, the 'rubbery' state and the 'glassy'
state. The temperature at which the transition between the glassy and rubbery states is
called their glass transit ion temperature orT
g.
Amorphous Materials
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2. Amorphous Structures
2. Amorphous Structures
Amorphous structures of inorganic glass, even called vitreous state, can bedefined as follows:
An isotropic material that does not have long range 3-dimensional atomicperiodicity (after 20 Å) and has a viscosity greater than 1014 poise.
The difference between a glass and its corresponding liquid
can be demonstrated by the volume/temperature relationship
during cooling shown in the diagram to the right. Duringcooling of a melt to its crystallization temperature (melting
temperature) Tm, the volume follows line “a”. When the
crystallization doesn’t occur the volume follows line “b” and
a super-cooled liquid is formed. After further cooling, line
“b” changes to line “c” with an inflection point at the glasstransition temperature, Tg, resulting in the formation of a
glass. Due to the high viscosity of super-cooled melts,
cooling must occur extremely slowly if the cooling curve is to
show a distinct inflection point. Otherwise, the
volume/temperature relationship follows a curve like line “d”.
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When a crystalline material is heated, the melting temperature
(TM) is well defined. But on cooling, it is often possible to
undercool the liquid so that nucleation and growth do not occur.
At a temperature below TM, the material can become rigid and
act like a solid, while preserving the amorphous atomarrangement.
The Glass Transition Temperature
This is called the glass transition temperature Tg. A plot of volume of density is often used to
illustrate this, since the expansion coefficient of the liquid, crystalline solid, and amorphous solid are
all generally different.
In real materials, Tg depends on cooling rate, and many other
secondary factors, and may not show such a sharp transition
as indicated here
2. Amorphous Structures2. Amorphous Structures
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2. Amorphous Structures2. Amorphous Structures
Glass can be classified as a super-cooled liquid in which
crystallization has not occurred. There are quite many similarities
between glass and liquids.
Glass structure is however much more complicated than crystal
structure. Glass has properties that are difficult or impossible to
simulate in crystalline material. These properties are alsocontinuously variable in a way that is impossible for a crystalline
material as well.
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2. Amorphous Structures2. Amorphous Structures
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2. Amorphous Structures2. Amorphous Structures
A kinetic theory which describes the transition of a melt to a
glass is based on the slow nucleation of crystal grains and
subsequent polycrystalline growth. The rate of nucleation is, as
well as crystal growth rate, temperature dependent but the rate
controlling functions contain conflicting terms that lead to the
different functions having distinct rate maxima, see adjacent
diagram..
Tendency to glass formation increases with:
Increased cooling rate
Increased surface tension melt/crystalline phase
Increased transformation temperatureDecreased melt volume
Decreased grain density
As soon as a nucleation has begun, a crystal will start to grow at
a certain rate depending on the rate of atomic diffusion to the
crystal surface. Crystal growth is therefore dependent on the
viscosity of the melt. Crystal growth rate reaches a maximum,
which for glass, often lies at a different temperature than the
maximum nucleation rate. Also noteworthy, is that the activation
energy for nucleation as well as crystal growth within glass
systems is higher than the Gibbs free activation energy for
viscous flow or self-diffusion
This phenomenon can be explained by the
fact that bonds within a molecular unit
must be broken to allow for crystallization
to occur
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2. Amorphous Structures2. Amorphous Structures
Some amorphous metallic alloys can be prepared under special processing conditions (such as rapidsolidification, thin-film deposition, or ion implantation), but the term "metallic glass" refers only to
rapidly solidified materials.
Even with special equipment, such rapid cooling is required that, for most metals, only a thin wire or
ribbon can be made amorphous. This is enough for many magnetic applications, but thicker sectionsare required for most structural applications such as scalpel blades, golf clubs, and cases for
consumer electronics.
Recent efforts have made it possible to increase the maximum thickness of glassy castings, by
finding alloys where kinetic barriers to crystallization are greater. Such alloy systems tend to have thefollowing inter-related properties:
Metallic Glass
Many different solid phases are present in the equilibrium solid, so that any potential crystal will find that
most of the nearby atoms are of the wrong type to join in crystallization.
The composition is near a deep eutectic, so that low melting temperatures can be achieved without
sacrificing the slow diffusion and high liquid viscosity seen in alloys with high-melting pure
components
Atoms with a wide variety of sizes are present, so that "wrong-sized" atoms interfere with the
crystallization process by binding to atom clusters as they form. One such alloy is thecommercial "Liquidmetal", which can be cast in amorphous sections up to an inch thick
.
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2. Amorphous Structures2. Amorphous Structures
- Si – O – Si- + M2O -Si-O-M+
M+
O- - Si-
With the help of X-ray diffraction studies, the structure of glass
is shown to be based on SiO4 tetrahedral units that are bound toeach other in a random network with so called modified atom
species spread throughout void spaces, as seen in the adjacent
schematic. Here one notices that certain Si-O-Si bonds are
broken and replaced by free O-endings and metal cations
according to the following formula:
A requirement in oxide glass formation is the possibility to
form a 3-dimensional structural network with a comparable
energy to that needed for a corresponding crystalline structural
network. This requires that the primary coordinate number for
every atom in the glass should be nearly identical to those in
the crystalline material. Furthermore, the secondary coordinate
should have only a very small contribution to the total
structural energy. Consider SiO2 for example, the structural
energy difference between Cristobalite and glassy SiO2 (Quartz
glass) is only ~1%
GLASS STRUCTURE
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2. Amorphous Structures2. Amorphous Structures
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Structures found from the glass beads demonstration. A perfect crystal (a),
an amorphous structure (b), and a crystal with a vacancy (c) is shown
2. Amorphous Structures2. Amorphous Structures
2. Amorphous Structures
2 Amorphous Structures
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The amorphous stateobtained by a rapid
quench from a random
start to a temperature
just above T= 0
The crystalline stateobtained after a long
slow cooling with
occasional heating
An intermediate statein the cooling process,
which after reheating
eventually resulted in
a picture similar to B.
A B C
2. Amorphous Structures2. Amorphous Structures
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2. Amorphous Structures2. Amorphous Structures
To fulfill these requirements, Zachariassen has proposed the following
necessities for oxide glass formation.
1. Every oxygen atom should not be bound to more than two cations.
2. The coordinate number for oxygen ions positioned around the
central cation should be small, i.e. less that 4.
3. Oxygen polyhedra can share a corner with each other in order to
form a 3-dimensional network. However, the polyhedra can not share
common edges or surfaces.
4. At least 3 corners of every polyhedron should be shared.
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2. Amorphous Structures2. Amorphous Structures VISCOSITY OF GLASS
The viscosity is a crucial factor in glassformation.
Glass formation is favorable in a material
when:
1. The viscosity is high at the melting point.
2. The viscosity below the melting point
increases with decreasing temperature.
The glass transition temperature, Tg, and the melting temperature, Tm, were
introduced and which are also present in the given diagram. Normally, the
two temperatures have the following relationship
Tg 2/3*TmTg
2/3*Tm
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2. Amorphous Structures2. Amorphous Structures
The viscosity is, as mentioned, also very dependenton composition. In silicate glass, the viscosity
decreases with increasing content of modified
cations. In many cases the change is very
pronounced. For example, for a quartz glass (pure
SiO2) at 1700°C the viscosity decreases 104 poise
with an addition of as little as 2.5 mol% K 2O.
This effect can be attributed to the presence of
oxygen atoms that only have one bond and cause aweak link in the Si-O- network. In the adjacent
diagram, the effect of replacing 8% of SiO2 in a
74SiO2-10CaO-16Na2O glass with different divalent
oxides to the viscosity at 1400°C is shown.
VISCOSITY OF GLASS
For Borsilicate glass, the change in viscosity with an addition of alkali oxides is more
complicated. At high temperatures the viscosity decreases with increased alkali addition,
whilst at lower temperatures, the viscosity increases with increased alkali addition. This phenomenon has yet to be explained theoretic.
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2. Amorphous Structures2. Amorphous Structures
Thermal Stress in Glass
It is understandable that thermal stresses occur between
materials with different thermal expansion behavior during
heating and cooling. When considering glass materials,
thermal stresses can occur when different parts of the glass,having different specific volumes, cool at different rates.
This is the case when a glass product contains segments
with diverse cross sections. Naturally, a thick material will
cool faster than a thin material. A glass material that is
cooled rapidly at the surface will suffer thermal stress
between the surface and interior.
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2. Amorphous Structures2. Amorphous Structures
When reheating the glass the volume curve will
follow the same curve as mentioned above but in
the opposite direction.
2 Amorphous Structures
2 A h S
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2. Amorphous Structures2. Amorphous Structures
The next diagram illustrates the behavior of 3 different
glasses; A, B and C , with different specific volumes (i.e.
different cooling rates) in terms of temperature vs.
physical expansion. Glass A is a rapidly cooled glass, B
a moderately cooled glass, C a slowly cooled glass.
The diagram demonstrates that the thermal expansioncoefficient is the same for all 3 glasses at temperatures
up to 400°C, i.e. the curves are parallel. Above 400°C,
glass A contracts up to roughly 560°C until the glass
structure has reached equilibrium, i.e. the specificvolume of the slowly cooled glass. On the other hand,
glass C follows the “normal” glass cooling curve from
the opposite direction which maintains that the structure
in this glass is in equilibrium during the entire course of
cooling.
Viscosity of glass atdifferent temperature
Annealing temperature
which is a characteristicproperty for every glass
It is through the use of thermal treatment at temperatures near the annealing temperature
that “thermal” stresses in glass can be eliminated. This is a standard practice in
manufacturing of glassware with varying thickness, for example; drinking glass, glassbottles and so on.
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2. Amorphous Structures2. Amorphous Structures
GLASS’ CHEMICAL COMPOSITIONS
(Crystal glass)
SiO2 Al2O3 CaO MgO Na2O K2O PbO B2O3
Type of Glass
Chemical composition , Wt.%
Window glass 72 1.3 8 4 14 0.3
Packing glass 72 0.1 5 4 15
Borsilicate glass 80 2 4 13
Lead glass 54 1 8 37
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2. Amorphous Structures2. Amorphous Structures
TYPES OF COMMERCIAL GLASS
WINDOW GLASS
PLATE GLASS
BOTTLES AND CONTAINERS
OPTICAL GLASS
PHOTOSENSITIVE GLASS
GLASS CERAMICS
GLASS FIBERS
MISCELLANEOUS TYPES OF GLASS
RECYCLING GLASS
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2. Amorphous Structures2. Amorphous Structures
RECYCLING GLASS
Scrap glass taken from the glass manufacturing process, called cullet, has been
internally recycled for years. The scrap glass is economical to use as a raw material because it melts at lower temperatures than other raw materials, thus saving fuel and
operating costs.
Glass that is to be recycled must be relatively free from impurities and sorted by color.
Glass containers such as bottles and jars are the most commonly recycled form of
glass, and their colors are flint (clear), amber (brown), and green. Other types of glass,
such as window glass, pottery, and cooking utensils, are considered contaminants
because they have different compositions than glass used in containers. The recycled
glass is melted in a furnace and formed into new products.
Glass containers make up 90 percent of the total recycled glass used in the United
States. The recycling rate for glass in 2000 was about 23 percent. Other uses for
recycled glass include glass art and decorative tiles. Cullet mixed with asphalt forms a paving material called glassphalt.
2 A h S
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The structural evolution in mechanically
alloyed binary aluminum-iron powder
mixtures containing 1, 4, 7.3, 10.7, and 25 at.
pct Fe has been investigated using x-raydiffraction and electron microscopic
techniques. The constitution (number and
identity of phases present), microstructure
(crystal size, particle size) and transformation behavior of the powders on annealing have
been investigated. The solid solubility of Fe
in Al has been extended up to at least 4.5 at.
pct. compared to the equilibrium value of
0.025 at. pct Fe at room temperature. A fully
amorphous phase plus solid solution in the
Al-10.7 at. pct Fe alloy; agreeing well with
the predictions made using the semi-
empirical Miedema model.
Structural Evolution in Mechanically Al loyed Al-Fe Powder Mixtures
Debkumar Mukhopadhyay
2. Amorphous Structures2. Amorphous Structures Example
2 A h St t
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X-Ray Diffractometry
TS-1 and VS-1 have a good crystallinity and show the
typical reflexes of the orthorhombic MFI-structure
Amorphous cogel with 3% titanium TS-1 with 3% titanium
2. Amorphous Structures2. Amorphous Structures Example
2 A h St t
E l
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2. Amorphous Structures2. Amorphous Structures
Heat flow at heating 10K/min (solid line) and
subsequent cooling with 10K/min
Example