type b -i systems form compounds with congruent melting...
TRANSCRIPT
Chapter I
Introduction
1.1. General aspects
Metal oxides play a very important role in diverse areas of chemistry,
physics and materials science. They have long attracted attention because of
their several unique materials properties, which make them versatile and
useful materials in various industries. They find extensive applications as
structural materials, refractories, adsorbents, insulators and corrosion
resistant materials. Metals are able to form a variety of oxide derivatives,
which can adopt a vast number of structural geometries with electronic
structures that can exhibit either metallic, semiconductor or insulator
characteristics. In technological applications metal oxides are used in the
fabrication of microelectronic circuits, sensors, piezoelectric devices, fuel
cells, coating for the passivation of surfaces against corrosion and as
catalysts. Majority of the catalysts used in chemical and petrochemical
industries involve an oxide as an active phase, promoter or support. Oxide
catalysts fall in to two general categories. They are either electrical insulators
or semiconductors. Insulator oxides are generally those in which the cationic
material has a single valence and have stoichiometric M:O ratios. The simple
oxides MgO, Al2O3 and SiO2 fall in to this category. These materials are not
effective as oxidation catalysts and find more use as solid acids or bases.
Semiconductor oxides are more commonly used in oxidation. They are
materials in which the metallic species are relatively easily cycled between
two valence states as in Fe2O3, V2O5, TiO2 and CuO or the inter-conversion
between the positive ion and the neutral metal as with the more easily
reduced oxides such as ZnO and CdO. In general, the simple semiconductor
2 Chapter 1
oxides are not very good catalysts for synthetic reactions1. The insulator
oxides however, can be used as solid acids and bases for a number of
reactions. Furthermore, the most active areas of the semiconductor industry
involve the use of oxides. Thus, most of the chips used in computers contain
an oxide component. The continued growth in industry and technology leads
to an ever-increasing demand for materials with specific properties. Hence in
the current scenario, further diversification of applications of metal oxides
through modifying their properties has added relevance.
Research interest has shifted from metal oxides to mixed metal
oxides since the properties of the metal oxides can be tuned and modulated
by judicious mixing with suitable other metal oxides. The two metal centers
in a mixed metal oxide can work in a cooperative way catalyzing different
steps of a chemical process, or they can have an enhanced chemical activity
due to effects of metal-metal or metal-oxygen-metal interactions. In
principle, the combination of two metals in an oxide matrix can produce
materials with novel structural or electronic properties that can lead to
superior materials with enhanced properties2. Although the importance of
this class of materials have been known for many years, it is only in the
relatively recent past, with the advancement of analytical techniques, studies
related to their structure and structure property relationship have attained
momentum. The preparation of specific tailor made mixed metal oxide,
which can perform complex functions is one of the main topics of research
today. The intense interest in these materials is driven to a large extent by
their unique properties and potential in various applications relating to high
temperature superconductors, 3
ceramic pigments4
and catalysts5-9
. Mixed
metal oxide thin films offer a strong and versatile material base for the
Introduction 3
development of novel technologies such as ferro-electric memories, 10
infrared detectors, 11
magnetic sensors12
and gas sensors13
.
The large application spectrum of mixed metal oxides requires
tailoring of the properties, such as particle size, morphology and phase
homogeneity. Low temperature route to mixed metal oxides have attracted a
great deal of interest since in the traditional high temperature ceramic
method there is little scope for control over homogeneity of components,
particle size and morphology. In the present work we propose to exploit sol-
gel technology as a route to process mixed metal oxide catalysts. Sol-gel
synthesis of mixed metal oxides provides an approach to control structures at
the nano-scale, thus enabling the formation of highly homogeneous new
materials, generally having improved or entirely new properties14
. Since our
focus is on metal ion doped sol-gel derived alumina, it is worth to mention
some of the relevant details in this area.
1.2. Alumina
One of the well-known metal oxide alumina, Al2O3, which exhibits
diverse phase characteristics, is known for its versatile material properties
and wide applications. It is an important and key material in ceramic industry
because of its unique mechanical, electrical, thermal and chemical properties.
Some of the important applications of alumina are listed below in Table1.1.
4 Chapter 1
Table 1.1. Important applications of alumina
Property Applications
Mechanical Abrasives, wear resistant applications, thread guides,
cermets etc
Thermal Refractory material, substrate for electronic materials,
good thermal conductor
Electrical High temperature insulator, high voltage insulator
Chemical Corrosion resistant applications, coatings on metals
Surface Adsorbents, catalysts
Seven crystalline phases have been reported for alumina which are ,
, , , , and 15
.The transformation between alumina phases strongly
depends on the precursors and the thermal treatment used in their
stabilization. -Alumina is known to have a d- spacing of 2.12Aº and is
probably cubic16
. -Alumina has a cubic spinel structure while -alumina
consists of oxygen anions in fcc lattice with Al ions occupying both
octahedral and tetrahedral sites. The cubic structure resembles a defective
spinel in which both octahedral and tetrahedral cation positions are
occupied17
. -Alumina has been identified as either tetragonal or as pure
amorphous phase18
. It was also suggested that -alumina has a tetragonal
superstructure of the spinel lattice with one unit cell parameter tripled17
. The
-form is an orthorhombic phase and -alumina is monoclinic, 19
its structure
is based on a face centered cubic packing of anions similar to the -phase and
contain both octahedral and tetrahedral Al ions17
. The thermodynamically
stable form of alumina is rhombohedral α-alumina with cell parameters
a = 4.7758Aº and c =12.991Aº. The oxygen positions approximate to
Introduction 5
hexagonal close packing (HCP) with the trivalent cations occupying two-
third of the octahedral interstices. The details of the crystal structure of
various alumina phases and hydroxides of aluminium are given in Table 1.2.
Table 1.2. Crystal structure of aluminium hydroxides and alumina phases
Phase Crystal system
Molecules
per unit
cell
Unit cell parameters Aº
a b c
Bayerite Monoclinic 2 4.72 8.68 5.06
Gibbsite Monoclinic 4 8.64 5.07 9.72
Diaspore Orthorhombic 2 4.40 9.43 2.84
Boehmite Orthorhombic 2 2.87 12.2 3.70
Chi Cubic 10 7.95 - -
Eta Cubic spinel 10 7.90 - -
Gamma Tetragonal - 7.95 7.95 7.79
Delta Tetragonal 32 7.97 7.97 23.5
Theta Monoclinic 4 2.95 2.95 11.9
Kappa Orthorhombic 32 8.49 12.7 13.4
Alpha Rhombohedral 2 4.76 - 12.9
Generally alumina is prepared by calcination of hydroxides of Al,
gibbsite, boehmite, bayerite and diaspore. Among various hydroxides,
boehmite and diaspore are both monohydroxy oxides of aluminium with
different crystal structures. Boehmite is of particular importance because it is
easily dispersible in water around pH 3-3.5. The various hydroxides of Al
6 Chapter 1
can be transformed in to -Al2O3 through different routes by temperature
control as shown below.
300ºC 970ºC 1100ºC
Gibbsite χ κ α
450ºC 750ºC 1000ºC 1200ºC
Boehmite γ δ θ α
230ºC 850ºC 1200ºC
Bayerite η θ α
500ºC
Diaspore α
900ºC 1000ºC
Tohdite κ α
In general, boehmite acts as an important precursor or intermediate for
the synthesis of transition aluminas. Boehmite transforms on heating through
a series of meta-stable transition alumina phases including -, -, -Al2O3,
finally forming thermodynamically stable -Al2O3 as shown above.
Introduction 7
Fig. 1.1. Boehmite polyhedra.
The crystal structure of boehmite (Fig.1.1) consists of Al-O octahedral
double layers, which are connected by hydrogen bonds. The octahedra are
nearly regular and have four of their corners occupied by oxygen atoms and
the other two by hydroxyls20
. The dehydration path inside the boehmite
structure is therefore believed to be along the ac plane. In large crystallite of
boehmite, this path becomes longer and the interlayer spacing is narrow.
Dehydration occurs slowly and suppresses the conversion of boehmite to -
Al2O3, elevating the formation temperature of -Al2O3. The chemical water
of this monohydroxide is made by combination of one terminal OH group on
top of a crystallographic boehmite layer, with one H atom from a
neighboring OH group. Thus the OH groups on the surface of each atomic
boehmite layer combine to produce water molecules, which are expelled.
The oxygen anions, which are not involved in this dehydration basically,
remain unaffected; hence the type of anion crystallographic packing and the
crystal boundaries remains fundamentally unchanged. Such transformations
are known as topotactic transformations. Since the transformation from -
through - to -Al2O3 proceeds topotactically21
it involves only a small
8 Chapter 1
energy difference. The transition of - to -Al2O3 does not require a re-
constructive re-crystallization process because of the similar cubic close
packed oxygen sub lattice. The transformation from - to -Al2O3, however,
requires a reconstruction of the structure involving a change in oxygen sub-
lattice from cubic to hexagonal and hence can occur only with a large energy
difference.
1.3. Alumina based mixed oxides
Incorporation of other metal oxides into alumina is an area of great
interest since it improves the properties of alumina with regards to many
aspects. A scan of literature reveals that many workers have attempted to
modify the properties of alumina by incorporating other metal oxides in its
matrix. Some of the important property modifications achieved by doping
other metal ions in alumina are listed in Table 1.3.
Table 1.3. Property modulation of alumina by incorporating other metal
oxides
System Property
ZrO2/Al2O3 Wear resistance22
Nb2O5/Al2O3 Thermal conductivity23
CeO2/Al2O3 Oxygen storage capacity24
La2O3/Al2O3 Surface area25
B2O3/Al2O3 Surface acidity26
MgO/Al2O3 Creep resistance27
Introduction 9
1.4. MAl2O4 spinels
The spinels are a group of oxides with the general formula
AIIB2
IIIO4. The structure of normal spinel consists of cubic close packing of
anions with the A atoms in tetrahedral sites and the B atoms in octahedral
sites; i.e., A(T)B2(O)O4 (Fig. 1.2). Each AO4 tetrahedron shares corners with
four BO6 octahedra, which are linked to each other through the edges. It is
possible to have various degree of randomization where both types of sites
are occupied partly by A cations and partly by B cations. These are known as
random spinels; i.e., [AxB(1-x)]T[A(1-x)B(1+x)]OO4.
Fig.1.2. Spinel polyhedra
Spinel oxides constitute an important class of advanced ceramic
materials, which exhibit interesting electronic, magnetic and catalytic
properties28-31
. Aluminium based spinels MAl2O4 (M = Cu2+
, Mn2+
, Co2+
and
Ni2+
etc) are also important as ceramic pigments32-
35
since the constituent
transition metal ions can form MO4 and MO6 polyhedra which can exhibit
the d-d transitions within the M2+
ion that get modulated by the ligand field
environment around the metal ion which result in colour modification within
the system.
10 Chapter 1
1.5. General methods of preparation of mixed metal oxides
Multi-component materials exist in various forms and their
preparation involves different protocols with a multitude of possible
preparation schemes. It has long been recognized that the properties of mixed
metal oxides often depend on their method of preparation. The dispersion
and size distribution of metal dopant oxide, their spatial distribution on the
support, homogeneity of components in a multi-component system, porosity,
surface area and pore size distribution of a support are all sensitive functions
of precursors used. The treatment temperature and atmosphere, as well as
other preparation variables such as pH of the preparation solution or the use
of aqueous or organic medium also contribute substantially to their
properties36-38
. In recent years significant progress has been made towards
understanding the relationship between the preparation method and the final
properties of the mixed metal oxides. Some of the most common methods of
preparation of mixed oxide catalysts are described below.
1.5.1. Solid- solid blending
Various methods based on solid-state reaction between powder oxides
are frequently used for the preparation of mixed oxide39
. In high temperature
ceramic method, the mixed oxide phase results from heating intimately
mixed powders at temperatures high enough to allow inter-diffusion and
solid state reactions. A major shortcoming of the high temperature ceramic
method is the lack of homogeneity of the material prepared since the solid-
state reactions between the precursor oxides occur at slow rates. The high
temperature required for completing solid-state reactions between oxides
lead to a drastic decrease in surface area of the resulting catalytic material by
sintering. To overcome this problem, precursor compounds such as
Introduction 11
carbonates and oxalates, which decompose at lower temperatures, have been
used instead of the corresponding oxides.
1.5.2. Co-precipitation method
In the co-precipitation method, the formation of the precipitate from a
homogeneous liquid phase may occur as a result of physical transformations
like change of temperature, solvent or solvent evaporation but most often is
determined by chemical processes like addition of acids or bases and use of
complex forming agents40
. The precipitate is treated in subsequent
preparation stages to form the active catalyst. In a multi-component system,
the composition of the precipitate depends on the difference in solubility
between the components and the chemistry occurring during precipitation.
One possibility is the sequential precipitation of separate chemical
compounds. This occurs whenever there is a large difference in the solubility
products of the compounds involved. The co-precipitates of hydroxides,
hydroxocarbonates, oxalates and formates containing two or more different
metals are generally non-homogeneous in composition and only very seldom
generate a homogeneous mixed oxide41
.
1.5.3. Multi-component complexes as precursors
If preformed complexes are used as precursors in which the desired
ratio of components is already present, it should be possible to prepare a
homogeneous multi-component material with lower temperature treatment.
Only a limited number of examples are available in the literature using this
approach to prepare multi-component oxides. In one example, anhydrous
metal acetate is dissolved in an organic medium in the presence of
isopropoxide of another metal to form a compound. Calcination of this
compound produces a well-mixed multi-component oxide37
. The use of
12 Chapter 1
compound precursors guarantees that the different metal components are
automatically mixed in the precursor. Thus it is expected that homogeneous
multi-component oxides can be obtained subsequently with rather mild
treatments. However, because stochiometric compounds are formed, the
range of composition is limited. Furthermore, the number of compounds that
can be formed readily limits the mixed oxides that can be prepared.
1.5.4. Hydrotalcite oxides as precursors
MgxAl1-x(OH)2(CO3)1-x is the most commonly used hydrotalcite oxide
precursor for other oxides42
. It is made up of layers of MgxAl1-x(OH)2 that carry
a net positive charge when x is greater than 0. This positive charge is balanced
by negatively charged CO32-
ions located between the layers. The Mg and Al
ions can be readily substituted by other cations, which makes hydrotalcite a
convenient precursor for the preparation of homogeneous mixed metal oxides or
samples of metal highly dispersed on an oxide support.
1.5.5. Impregnation method
In the impregnation route, a solid phase preformed in a separate
process is used as a support, and the catalytically active material is mounted
and stabilized on it.43, 44
In this method, a certain volume of solution
containing the precursor of the active element of the catalyst is contacted
with the solid support. If the volume of the solution is either equal or less
than the pore volume of the support, the technique is referred to as incipient
wetness. When the interaction of the active precursor in solution with the
support is weak, the method of incipient wetness impregnation followed by
drying is used to apply high loading of precursors. The maximum loading is
limited by the solubility of the precursors in pore filling liquid. However, in
the absence of sufficiently strong interactions, the drying step usually result
Introduction 13
in severe redistribution of the impregnated species and the support become
non-homogeneously covered by the active material. In the wet impregnation
technique, an excess of solution is used. After a certain time the solid is
separated from the solution and the excess solvent is removed by drying. The
amount of active component introduced onto the support depends on the
equilibrium concentration of the impregnating solution, the pore volume of
the carrier and the binding of precursor on to the support surface45
.
1.5.6. Equilibrium adsorption technique
Equilibrium adsorption is a method used to deposit metal containing
species onto the surface of a porous oxide support. Deposition of species
onto the surface can occur by interaction of protonated or deprotonated
surface hydroxyl with oppositely charged solution species or by
condensation of neutral hydroxyl with hydrolyzed solution cation. Thus, the
pH of the solution is an important parameter that determines the
concentration and the nature of the deposited species, the extent of
hydrolysis of the solution cation, and the extent of protonation and
deprotonation of surface hydroxyls46
.
1.5.7. Chemical vapor deposition method
The chemical vapor deposition method designates any process of
deposition using reaction between surface sites, such as –OH groups on
inorganic supports and vapor of an active material. For preparation of
dispersed metal catalysts, volatile metal chlorides such as SnCl4 or NiCl2
were used to obtain Sn/Al2O3 or Ni/Al2O3 catalysts47
. The method
circumvents the process of impregnation, washing, drying, calcination and
activation, which are involved in solvent-assisted catalyst preparations. Other
complications caused by solvent during liquid phase preparation such as
14 Chapter 1
dissolution, surface poisoning and redistribution of the active material during
drying are also eliminated.
The methods described above however, have limitations with respect
to the chemical compositions, homogeneity, and ease of control of
stoichiometry, porosity and surface area of the final oxide.
1.5.8. Sol-gel processing
Sol-gel process is a very versatile technique, which is used in the
synthesis of nanosized composites, monoliths, thin films, optical ceramics,
fibers and catalysts. 48, 49
One of the most important requirements in the
preparation of multimetallic oxide catalysts is obtaining a good inter-
dispersion of different phases and components, which constitute the catalyst.
Preparation methods based on sol-gel techniques have been well known to
result in highly homogeneous multi-component material of molecular or
atomic levels. Such mixed metal oxides have been widely reported to have
many fold increase in catalytic activity. Table 1.4 provides a summary of
comparison of various methods for the preparation of multi-component
catalysts highlighting both their advantages and disadvantages.
Introduction 15
Table 1.4. A comparison of important methods of preparation of multi-
component oxides
Synthesis methods Advantage Disadvantage
Solid-solid blending Powder of about one
micron or more in size
Aggregation of grains,
no perfect
homogeneity, high
temperature is needed
Co-precipitation
Complex process,
insufficient
homogeneity
From preformed
complexes
Homogeneous multi-
component catalyst
Limited range of
composition
Hydrotalcite method Good stichiometry Medium homogeneity
Impregnation method Poor homogeneity
Equilibrium adsorption
technique
Limited range of
composition
Chemical vapour
deposition High product purity
Limited range of
composition
Sol-gel processing
High homogeneity,
product purity and
flexibility
Simple and requiring no
sophisticated facilities
1.6. Sol-gel processing: An overview
Interest in sol-gel processing of ceramic materials began as early as in
the mid 1800s with Ebelman and Graham’s studies on silica gels. In these
early investigations, the hydrolysis of tetraethyl orthosilicate, under acidic
conditions yielded SiO2 in the form of a glass like material. During late
1800s to the 1920s gels became of considerable interest to chemists
16 Chapter 1
stimulated by the phenomenon of Liesegaing50
rings formed from gels. Many
noted chemists including Ostwald and Lord Raleigh investigated the problem
of the periodic precipitation phenomena that led to the formation of
Liesegaing rings and the growth of crystals from gels. Roy et al51
recognized
the potential for achieving very high levels of chemical homogeneity in
colloidal gels and used the sol-gel method in the 1950s and 1960s to
synthesize a large number of novel ceramic oxide compositions that could
not be made using traditional ceramic powder methods. During the same
period Iler’s52
pioneering work on silica chemistry led to the commercial
development of colloidal silica powder. Stober et al53
extended Iler’s
findings to show that using ammonia as a catalyst for the TEOS hydrolysis
reaction could control both the morphology and size of the powders
Overbeek54
and Sugimoto55
showed that nucleation of particles in a
very short time followed by growth without super saturation will yield
monodispersed colloidal oxide particles. Matijevic et al56-59
employed these
concepts to produce enormous range of colloidal powders with controlled
size and morphologies, including oxides (TiO2, Fe3O4, BaTiO3, CeO2),
hydroxides (AlOOH, FeOOH) and various mixed phases or composites (Ni,
Co, Sr ferrites) and coated particles (Fe3O4 with Al(OH)3).
Sol-gel powder processes have also been applied to fissile elements60
where spray formed sols of UO2 and UO2-PuO2 were formed as rigid gel
spheres during passage through a column of heated liquid. Both glass and
polycrystalline ceramic fibers have been prepared by using the sol-gel
method. Compositions include TiO2-SiO2 and ZrO2-SiO2 glass fibers60, 61
. A
variety of coatings and films have also been developed using sol-gel method.
Of particular importance are the antireflection coatings of indium tin oxide
applied to glass windowpanes to improve insulation characteristics.62, 63
Introduction 17
1.6.1. Sol-gel process: Steps
Sols are dispersions of solid particles in a liquid with particle size of
1-100 nm64
A gel is an interconnected, rigid network with pores of sub
micrometer dimensions and polymeric chains whose average length is
greater than a micrometer. The term gel embraces a diversity of
combinations of substances that can be classified in four categories: (i) well-
ordered lamellar structure, (ii) covalent polymeric net-works completely
disordered, (iii) polymer networks formed through physical aggregation,
predominantly disordered and (iv) particular disordered structure
Generally three approaches are used to make sol-gel monoliths: (I)
gelation of a solution of colloidal powders, (II) hydrolysis and poly-
condensation of alkoxide or nitrate precursors followed by hypercritical
drying of gels and (III) hydrolysis and poly-condensation of alkoxide
precursors followed by aging and drying under ambient atmosphere.
1.6.1.1. Mixing
In method I, a sol is formed by mechanical mixing of substances in
water at a suitable pH. In method II and III, a liquid metal alkoxide precursor
is hydrolyzed by mixing with water65
. The possible reactions are,
2M(OH)4M
OH
O
OH
HO M
OH
OH
OH
+ H2O --------(2)
M(OR)4 + 4H2O M(OH)4 + 4ROH -------(1)
18 Chapter 1
The hydrolysis and poly-condensation reactions eventually result in
M-O-M network. The water/alcohol expelled from the reaction remains in
the pores of the network. Yoldas66
observed that the hydrolysis reaction and
the condensation reaction are not separated in time but takes place
simultaneously. It has been established that the presence of H3O+ in the
solution increases the rate of hydrolysis, whereas OH- increases the
condensation reaction. Orcel et al67
showed that the shape and size of
polymeric structural units are determined by the relative values of the rate
constants for hydrolysis and poly-condensation reactions. Fast hydrolysis
and slow poly-condensation favor formation of linear polymers. On the other
hand, slow hydrolysis and fast condensation result in large, bulkier, and more
ramified polymers68
.
1.6.1.2. Gelation
With time the sol particles link together to become a three
dimensional network. As the sol particles grow and collide, condensation
occurs and macro particles form. The sol becomes a gel when it can support
a stress elastically69
. This is typically defined as the gelation point or gelation
time. One cannot precisely define the point when the sol changes from a
viscous fluid to an elastic gel. The change is gradual as more and more
particles become interconnected. The physical characteristics of the gel
network depend greatly upon the size of the particles and extent of cross-
linking prior to gelation. During gelation, the viscosity increases sharply.
The structure of a gel is established at the time of gelation. The size and the
degree of branching of the inorganic polymer and the extent of cross-linking
have strong influence on porosity of gel, and later on the surface area, pore
volume, pore size distribution, and thermal stability of the final oxide after
calcinations70
.
Introduction 19
In general, if the gel contains polymeric chains with significant
branching and cross-linking (Fig.1.3), it will have large void regions and the
resulting oxide after calcinations will mostly be macro-porous and
mesoporous71
. Conversely, if the gel contains polymeric chains with little
branching and cross-linking, it will have smaller void regions and the
resulting oxide will mostly be micro-porous with low surface area. The
relative rates of hydrolysis and condensation determine the extent of branching
of the inorganic polymer and colloidal aggregation in the gelation mixture.
In general, in the presence of high concentration of metal cation monomer,
Fig. 1.3. Schematic diagram of gels (a) with significant branching and cross-
linking and (b) with little branching and cross-linking
20 Chapter 1
if hydrolysis is slow relative to condensation, long, highly branched and
cross-linked polymeric chains are formed and the resulting oxide can be
macro porous. If condensation and hydrolysis occur at comparable rates,
short polymeric chains with less branching and less cross-linking are formed,
and the final oxide can be micro porous in nature. Since hydrolysis and
condensation are chemical reactions, their relative rates are functions of
many parameters such as pH, temperature, nature and concentration of the
metal ion precursors and concentration of water.
1.6.1.3. Aging
When a gel is maintained in its pore liquid its structure and properties
continue to change long after the gel point. The process is called aging. Four
processes can occur singly or simultaneously during aging poly-
condensation, synersis, 72
coarsening52
and phase transformation. Poly-
condensation reactions continue to occur within the gel network and this
increase the connectivity of the network. Usually in alkoxide-based gels,
chemical hydrolysis reactions are very rapid and are completed in the early
stages of sol preparation, especially when the sol is acid catalyzed. Since the
chemical reactions are faster at high temperature, aging can be accelerated by
hydrothermal treatment, which increases the rate of condensation reaction.
The shrinkage of the gel and the resulting expulsion of liquid from
the pores are called syneresis. Syneresis in alcoholic gel systems is greatly
attributed to formation of new bonds through condensation reactions, which
increases the bridging bonds and causes the interaction of the gel network. In
aqueous gel systems, the structure is controlled by the balance between
electrostatic repulsions and attractive van der waal’s forces. Coarsening or
“Ostwald ripening52
is the irreversible decrease in surface area through
Introduction 21
dissolution and re-precipitation processes. Since the convex surfaces are
more soluble than concave surfaces, if a gel is immersed in a liquid in which
it is soluble, dissolved materials will tend to precipitate on to regions of
negative curvature. Necks between particles will grow and small pores will
get filled in, resulting in an increase in the average pore size of the gel and
decrease in the specific surface area. Washing the pore liquid out of a gel is
also an aging step73
. The pH of the wash water is critical in the case of gels
made from acid catalyzed precursors. The final properties of such gels
depend on both the pH at which the gel was formed and the pH in which it
was washed before drying.
During aging there are changes in most physical properties of the gel.
Since the condensation reaction creates additional bridging bonds, the
stiffness of the gel network increases, as does the elastic modulas74
, the
viscosity and the modulus of rupture. The strength of the gel also increases
with aging. West et al75
. showed that gel strength increased logarithmically
with time ranging between 1 and 32 days. Therefore large monolithic gels
are subjected to aging process before drying to reduce the chance of
cracking. The greater stiffness of the aged gel reduces the shrinkage during
drying, especially if the aging treatment is performed under hydrothermal
conditions.
1.6.1.4. Drying
During drying, the liquid is removed from the interconnected pore
networks. When the pore liquid is removed, shrinkage occurs and the
monolith is termed as xerogel76
(Fig.1.4). If the pore liquid is primarily
alcohol based, the monolith is often termed as an alcogel77
. A gel is defined
as dried when the physically adsorbed water is completely evacuated. This
22 Chapter 1
occurs between 100 and 1800C. Large capillary stresses can develop during
drying and this can cause the gels to crack unless the drying process is
controlled. It has been generally accepted that there are three stages of
drying. During the first stage of drying, the decrease in volume of the gel is
equal to the volume of liquid lost by evaporation. The complete gel network
is deformed by the large capillary forces, which causes the shrinkage of the
material. For large or small pore gels the greatest change in volume, weight,
density, and shrinkage occur during stage 1 drying. Stage 1 drying ends
when shrinkage ceases. Stage 2 begins when the strength of the material has
increased due to the greater packing density of the solid phase, sufficient to
resist further shrinkage. As the network resistance increases the radius of the
meniscus is reduced. Eventually the contact angle approaches zero and the
radius of the meniscus equals to the radius of the pore. This condition creates
the highest capillary pressure, and unable to compress the gel any further, the
pores begin to empty which is the start of stage 2. In stage 2 liquid transport
by flow through the surface films that cover partially empty pores. The liquid
flows to the surface where evaporation takes place. The flow is driven by the
gradient in capillary stress78
. The third stage of drying is reached when the
pores are substantially emptied and surface films along the pores cannot be
sustained. The remaining liquid can escape only by evaporation from within
the pores and diffusion of vapor to the surface. During this stage there are no
further dimensional changes but just a slow progressive loss of weight until
equilibrium is reached, determined by ambient temperature and partial
pressure of water79
. A dried gel still contains a very large concentration of
chemisorbed hydroxyls on the surface of the pores. Thermal treatment in the
range 500-8000C desorbs the hydroxyls and thereby decreases the contact
Introduction 23
angle and the sensitivity of the gels to re-hydration stresses resulting in a
stabilized gel79
.
Fig. 1. 4. Various stages of gel (a) stabilized gel, (b) wet-aged gel and (c)
xerogel
1.6.1.5. Densification
Densification is the increase in bulk density that occurs in a material
as a result of a decrease in volume fraction of pores. Heating the porous gel
at high temperature causes densification. Densification of a gel network
occurs between 10000C and 1700
0C depending up on the radii of the pores,
connectivity of the pores and surface area. Controlling the gel-glass
transition is a difficult problem if it is necessary to retain the initial shape of
the starting material. It is essential to eliminate volatile species prior to pore
closure and to eliminate density gradients due to non-uniform thermal or
atmosphere gradients. The amount of water in the gel has a major role in the
sintering behavior. The viscosity is strongly affected by the concentration of
water, 80
which in turn determines the temperature of the beginning of
densification. For example, a gel prepared in acidic conditions has a high
24 Chapter 1
surface area and water content than a gel prepared in basic conditions and
starts to densify about 2000C sooner than the base catalyzed gel
81. During
sintering, the driving force is a reduction in surface area82
. Most authors
report a diminution of the specific surface area when the densification
temperature increases. However, it was shown that certain samples display
first an increase of surface area until a temperature between 3000C and
4000C and then a decrease with further increase of temperature
83. Several
studies show that despite the complex manner in which the gel evolves
towards a glass its structure and properties become indistinguishable from
those of a melt-derived glass84-87
once the gel has been densified and heated
above the glass transition temperature. Generally the mechanisms
responsible for the shrinkage and densification of gels are capillary
contraction, condensation, structural relaxation and viscous sintering. It is
possible that several mechanisms operate at the same time.
Using different models one can describe the sintering behavior of a
gel. Frenkel’s theory, 88
which is derived for spheres, is valid for the early
stages of sintering, because of the geometrical assumptions. It is based on the
fact that the energy dissipated during viscous flow is provided by the
reduction in surface area. Scherer89
developed a model for describing the
early stages as well as the intermediate stage of sintering. It is assumed that
the microstructure consists of cylinders interacting in a cubic array. To
reduce their surface area, the cylinders become shorter and thicker. The
above models predict reasonably well the behavior of gels upon heating.
1.6.2. Advantages of sol-gel process
The motivation for sol-gel processing is primarily due to higher purity,
homogeneity of the products and the lower processing temperature compared
Introduction 25
with traditional glass melting or ceramic powder methods90
. During the past
decade, there have been enormous growths of interest in sol-gel processing.
This growth has been stimulated by several factors. On the basis of
Kistler’s91
early work, several teams produced very low-density silica
monoliths called aerogels and large monolithic pieces of alumina by sol-gel
methods. These demonstrations of potentially practical route for production
of new materials with unique properties coincided with the growing
recognition that powder processing of materials has inherent limitations in
homogeneity due to difficulty in controlling agglomeration92
.
The goal of sol-gel processing is to control the surface and interfaces
of materials during the early stages of production. Long-term reliability of
materials is usually limited by localized variations in the physical chemistry
of the surface and interfaces within the material. Each step of the process can
be controlled and modified in order to obtain a specific material, with better
characteristics than those obtained by traditional methods of preparation. The
important advantages of sol-gel processing are compositional homogeneity
and the ability to prepare shaped materials such as spherical particles, fibers
and thin films. The sol-gel process presents inherent advantage for the
preparation of porous ceramic oxides, because the nano structure of the
derived materials can be controlled together with their porous structure. At
present sol-gel processing is employed for the preparation of new generation
of advanced materials for structural, electrical, optical, electronic and
catalytic applications.
The sol-gel process is of particular interest for designing catalytically
active materials with specific properties and/or with improved performances
compared to those of classical catalysts. It allows preparation of catalytically
active materials, which can be directly cast in/on supports at the sol stage
26 Chapter 1
itself. This is a great advantage for catalytic membrane development93
. The
classical synthesis methods for conventional catalysts often start from salts
or oxide precursors and involve precipitation, impregnation, or even
solid/solid reactions. These methods are not adapted to a homogeneous
casting of the catalyst on a support and lead to limited specific surface areas
and to a heterogeneous distribution of active species. The sol-gel process
starting from a homogeneous distribution of the precursors at the molecular
level can in many cases improve these specific criteria. Indeed a large range
of methods and precursors can be investigated to obtain the required powders
or films either as pure catalyst or homogeneously doped or dispersed in a
matrix. Further more, the specificity of the process can lead to original
materials which can help in a better understanding of the catalytically active
sites in a specific catalyst.
Since the work embodied in the thesis involves developing various
metal ion doped aluminas through sol-gel route and also the structural
evolution of aluminas and mixed metal oxides including spinels of the type
MAl2O4. We thought it worthwhile to discuss some of the known aspects of
Cu2+
, Mn2+
, Co2+
, Ni2+
, Ce4+
and Ti4+
ions doped aluminas. These are
presented below in separate sections as CuO/Al2O3, MnOx/Al2O3,
CoOx/Al2O3, NiO/Al2O3, CeO2/Al2O3 and TiO2/Al2O3 mixed oxides.
1.7. CuO/Al2O3 mixed oxides
CuO/Al2O3 mixed oxides are widely used in industry as catalysts and
in electronic fields. CuAlO2 is a p-type transparent conducting oxide that has
been proposed for a number of technological applications94
. Another mixed
oxide CuAl2O4, which crystallizes in the spinel form, is a potential catalyst
for the oxidation of phenol in aqueous solutions95
and for the selective
Introduction 27
catalytic reduction of NO with propane96
. The study of CuO/Al2O3 system is
considered to be very important especially in the field of catalysis where the
CuO phase is the most active species for certain catalytic process.
Selim et al97
reported the formation of CuAl2O4 spinel in the
temperature range of 700-8000C, and the decomposition of the spinel to
CuAlO2 at higher temperatures, for a copper-aluminium mixed oxide
prepared by impregnation of -Al2O3 with copper nitrate solution in an
equimolecular ratio. It was also observed that the incorporation of sodium
ions in the mixed oxides stabilized most of the CuAl2O4 spinel in the
crystalline form, and prevented the decomposition to CuAlO2. The rate of
metal aluminate formation in MOx/Al2O3 systems (M = Ni, Co, Cu and Fe)
at 500-10000C in oxygen or nitrogen atmosphere was compared by Boit et
al.98
It was observed that spinel formation rate is higher for CuO/Al2O3
system compared to other systems.
Among the most promising new technologies of power generation
from coal are gasification integrated with combined cycle power generation,
i.e., gas turbine in series with a steam turbine and coal gasification followed
by oxidation in a molten carbonate fuel cell. Both technologies require
removal of H2S from the fuel gas prior to combustion. Patrick et al99
reported
the preparation of copper- aluminium mixed oxide sorbents by the citrate
process, and the resulting product consisted of varying amounts of
compound oxide CuAl2O4 and mixed oxides CuO and Al2O3. The sulfidation
rate was much slower for those sorbents that consisted mainly of the
compound oxide CuAl2O4 compared to those that consisted mostly mixed
oxides CuO and Al2O3. The CuAl2O4 has a partly inverse spinel structure
with Cu2+
occupying both tetrahedral and octahedral sites, the Cu2+
that
28 Chapter 1
occupies tetrahedral sites were responsible for the slow sulfidation kinetics
observed.
Youssef et al100
reported the formation of CuAl2O4 in CuO/Al2O3
system when the sample containing 20 w % of CuO was calcined at 900ºC.
The surface area decreases and means pore radius increases with increase of
Cu loading and rise of calcination temperature. Hydrogenation of
cyclopentadiene to cyclopentane on the reduced catalyst depends on the
efficiency of the dispersion of the metal at the surface of the support. Wang
et al101
prepared sol-gel derived -Al2O3 supported CuO granular sorbents
which exhibited flue gas desulfurization capacity greater than those of the
similar commercial sorbents. Catalytic combustion of methane is one of the
most promising processes for energy production. The high temperature
methane combustion requires thermally stable catalysts. According to
Artizzu et al102
CuO deposited on to high surface area MgAl2O4 spinel
prepared from alumina and magnesium nitrate showed very good activity for
the methane combustion with a selectivity of 100% to carbon dioxide.
Preparation and activity of copper-aluminium mixed oxides from
hydrotalcite like precursors, for the oxidation of phenol aqueous solutions
was reported by Alejandre et al95
. Phenol conversion decreased continuously
over time for the samples calcined at lower temperatures. Samples calcined
at higher temperatures and after HCl treatment (to avoid the CuO phase)
have pure CuAl2O4 spinel phase and showed higher activity for phenol
conversion. In another study, Alejandre et al103
prepared copper-aluminium
hydrotalcite (HT) like compounds from Cu(NO3)26H2O and Al(NO3)39H2O
using trimethylamine and CO2 as precipitants. Pure CuAl2O4 with high
surface area and catalytic property was obtained from the calcination of the
‘HT 0.5’ samples. Contrary to the reports of Shimizu et al104
and Maritisius
Introduction 29
et al105
, they observed that the rate of formation of CuAl2O4 considerably
decreased when the amount of copper in the sample increased. Woelk et al4
reported the formation of brown and blue pigments from Cu-Al-Si-O
systems in the temperature range 800-14000C. The pigment formation was
dependent on the temperature as well as composition of the sample. It was
suggested that the colour is due to two possible reactions: (i) the reaction of
copper ions in a glass matrix that formed during the calcination process and
(ii) the reaction between Al2O3 and Cu2O/CuO or SiO2 and Cu2O/CuO.
Transparent conducting oxides simultaneously exhibit both high
transparency through the visible spectrum and high electrical conductivity.
Transparent conducting oxides are utilized in a variety of commercial
applications, such as flat panel displays, photovoltaic devices and
electrochromic windows, in which they serve as transparent electrodes.
Delafossite type CuAlO2 exhibits both p-type conductivity and transparency.
The interfacial reaction between copper and alumina, which occurs during
the eutectic bonding process was observed by Yi et al106
During eutectic
bonding the compound CuAlO2 is formed at the interface between the copper
and alumina in specimens containing solid copper at temperatures between
1068 and 1072ºC. However, in specimens containing heavily oxidized
copper in which the solid copper phase was not present at the bonding
temperature, CuAlO2 formation was observed at temperatures higher than
10750C. Buijan et al
107 compared the electronic structures of CuAlO2 and
Cu2O, two Cu+
oxides that exhibit weak homoatomic d10
-d10
interactions by
the semiemprical extended Huckel’s method. It revealed the important role
of weak d10
-d10
interactions in the origin of colour and conductivity in this
family of compounds.
30 Chapter 1
A low temperature hydrothermal technique was used to synthesize
CuAlO2 by Shahriari et al108
. In this method, appropriate amounts of
aluminium metal, CuO and Al2O3 were placed along with ground sodium
hydroxide pellets in a Teflon pouch, sealed and placed in an autoclave,
heated to 210ºC and subsequently cooled to room temperature. The
formation of Cu2O, CuAl2O4 and CuO at 700ºC and CuAlO2 at temperature
greater than 800ºC in nitrogen (neutral) atmosphere was reported by Ohashi
et al109
from copper acetate hydrate and aluminium tri-sec-butoxide. Ingram
et al110
reported direct preparation of CuAlO2 by conventional high
temperature solid state reaction. The pellets prepared using high purity
constituent oxides in stoichiometric ratios were heated in air to 1100ºC for
24-36h and quench-cooled in air. This process of firing was repeated until an
X-ray phase-pure sample of CuAlO2 was achieved.
Copper compounds in the environment usually exist in two common
oxidation states Cu+
and Cu2+
. If not properly treated before discharge,
copper-containing wastewater has a great potential to contaminate the soil
and water systems. Thermal treatment has recently been emerging as a
promising environmental technology to stabilize heavy metal-containing
industrial sludge. Aluminosilicate and silica sand are the main inorganic
constituents of the earth’s upper crust, and they are acceptors of heavy metal
contaminants. Wei et al111
reported that copper could be thermally
immobilized with silica or kaolinite, and reported the formation of a less
soluble copper solid phase containing CuO in the copper contaminated
kaolinite heated at 9000C for 1 h. Wei et al
112 reported the formation of
CuAl2O4, while investigating the species distribution of copper in copper
contaminated alumina heated at 900ºC for 1h.
Introduction 31
Nitric oxides (NOx) are commonly produced by various combustion
processes, and contribute largely to a variety of air pollution such as
formation of acid rain, smog, green house effect etc. Strict environmental
regulations necessitates effective after treatments. Abatement is generally
achieved through the selective catalytic reduction. Several authors have
reported the catalytic ability of copper- aluminium mixed oxides for the
selective reduction of NOx. Fernandez-Garcia et al96
reported the reduction
of NO with CO over alumina supported copper oxide catalysts, which is less
expensive than the noble metals (Rh, Pt, Pd etc). From the correlation of
copper surface species present on the catalyst with its catalytic performance
they deduced that a redox type mechanism Cu2+
/Cu+ is working at the
reaction conditions. Shimizu et al104
prepared copper-aluminium mixed
oxide catalysts from hydroxides obtained by co- precipitation of copper
acetate and aluminium nitrate, for the selective reduction of NO with
propane. The UV- vis reflectance spectra showed bands at 1450nm and 750
nm, due to the electronic transitions in Cu2+
in tetrahedral and octahedral
sites of spinel lattice respectively. Low copper samples exhibited a band at
750 nm which indicated that Cu2+
was predominantly in octahedral sites. As
the copper content increased the intensity of band at 1450nm due to the
tetrahedral Cu2+
increased indicating the formation of aluminates. Surface
Cu2+
cations in octahedral sites were responsible for the catalytic activity.
Maritisius et al105
also observed that the amount of copper aluminate
increased with increasing CuO concentration.
Copper aluminate catalysts for abatement of NO with propylene or
ammonia in presence of oxygen was reported by Kim et al113
. The catalysts
were prepared by the incipient wetness impregnation of copper nitrate
solution on commercial alumina. The catalyst calcined at high temperature
32 Chapter 1
showed enhanced activity in the presence of propylene but had no effect on
NO conversion when ammonia was used as the reducing agent. According to
Metelkina et al 114
the catalyst prepared by the above method with 2 %
copper loading showed about 90% NO conversion at 350-400ºC. The
catalytic performance of the system appears to be determined by the degree
of clustering of copper cations. Zhu et al115
prepared copper oxide
supported on alumina by impregnation of copper nitrate on alumina at
different calcination temperatures. The N2O reduction activity increased with
increasing calcination temperature of supports from 450 to 900ºC. However,
further increase in calcination temperature of supports resulted in a reduction
in activity. Several copper species, surface spinel, bulk CuAl2O4 and CuO
were present in the CuO-Al2O3 system. Bennici et al116
reported the surface
properties of deposited CuO phase on silica modified with alumina, titania
and zirconia. All the catalysts possessed high surface area and homogeneous
coverage of the relevant support. The CuO phase deposited on the most
acidic support showed the best activity and selectivity in NOx reduction.
1.8. MnOx/Al2O3 mixed oxides
The increasing stringent environmental regulations limiting emissions
of halogenated hydrocarbons have increased enormously the demand for
technology to remove effectively halogenated compounds from waste
streams. Tseng et al117
reported the decomposition of trichloroethane (TCE)
over an MnOx/γ-Al2O3 catalyst, prepared by the incipient wetness
impregnation method with aqueous solution of manganese nitrate, in a fixed
bed reactor. Einaga et al118
reported the catalytic oxidation of cyclohexane
with ozone at room temperature over alumina supported manganese oxide
catalyst prepared by impregnation of manganese acetate on γ-Al2O3.
Trawezynski et al119
reported the oxidation of ethanol over alumina
Introduction 33
supported MnOx catalyst, prepared by a conventional impregnation of Al2O3
support with aqueous solution of manganese acetate. In another study,
Einaga et al120
reported the oxidation of benzene with ozone at room
temperature over alumina supported manganese oxide catalyst prepared by
the impregnation of γ-Al2O3 with aqueous solution of manganese acetate and
observed a linear correlation between the amount of ozone decomposed and
that of the COx formed. Alumina supported Mn catalysts with Mn loading
ranging from 3.9 to 18.2% were prepared by impregnation of γ-Al2O3
substrate with aqueous solution of manganese nitrate and tested its catalytic
activity in the combustion of formaldehyde/methanol mixture in an air
stream by Arias et al121
and reported that the activity increases with
increasing manganese loadings. Barrio et al122
reported a method for the
preparation of homogeneous coatings of manganese oxide on alumina by a
redox deposition-precipitation method using acetone as solvent and observed
that the catalyst prepared by this method is very active in the complete
oxidation of oxygenated volatile organic compounds.
The adsorption capacity for NO of alumina-supported oxides and
hydroxides of Mn have been studied by Spasova et al123
and reported that the
samples with Mn3+
ions on the surface of the support show enhanced
adsorption capacity. The structural characteristics of manganese oxides
supported on alumina during ozone decomposition reaction in the presence
of water vapour was studied by Einaga et al124
and reported that Mn was
oxidized to higher oxidation state, along with the coordination of water to
Mn. The phase transformation features of MnOx/Al2O3 system, prepared by
impregnation of manganese nitrate on γ-Al2O3 on calcination at 950ºC and
the effect of these phases on the catalytic oxidation of n-pentane was
reported by Tsyrulnikov et al125
. Arena et al126
studied the effect of the oxide
34 Chapter 1
carriers (γ-Al2O3, SiO2, ZrO2 and TiO2) and Mn-precursors (KMnO4,
manganese nitrate and manganese acetate) loading on the structure and
reduction pattern of MnOx based catalysts prepared by incipient wetness
impregnation method by PXRD and temperature programmed reduction
measurements.
Hernandez et al127
reported the synthesis of nano-particles of Mn-
doped alumina from hydrolysis of manganese and aluminium salts at 60ºC in
presence of urea. Sintered density, grain size and microstructure formation of
alumina doped with manganese oxide have been investigated by
Sathiyakumar et al128
and reported that the addition of manganese oxide
produces a relatively uniform dense microstructure at high temperature.
1.9. CoOx/Al2O3 mixed oxides
Liotta et al129
prepared CoOx catalysts supported on alumina and
BeO/Al2O3 by incipient wetness impregnation method and the catalytic
activity was tested in the selective catalytic reduction of NO with C3H6 in the
presence of excess of oxygen, and found that the presence of BeO in the
alumina network is effective in the stabilization of the dispersed Co2+
ions,
which are active and selective for NO reduction and clusters of cobalt oxide
present as Co3O4 in the alumina are active mainly for C3H6 combustion.
Konova et al130
investigated an alumina supported cobalt oxide system with
respect to catalytic decomposition of ozone, complete oxidation of volatile
organic compounds and oxidation of CO in the temperature range –40 to
250ºC in an isothermal reactor. A very high activity of cobalt towards ozone
decomposition at temperatures below -40ºC and significant increase in the
catalytic activity and decrease in the reaction temperature for oxidation of
VOCs and oxidation of CO were observed.
Introduction 35
Wang et al131
prepared a series of Co/Al2O3 catalysts with various
metal loadings by incipient wetness impregnation method and investigated
the reducibility of cobalt oxides in these samples by the temperature
programmed reduction technique and reported that for catalysts with low
cobalt loadings the cobalt phase present is CoAl2O4 and for high Co contents
it is bulk Co3O4. Ji et al132
prepared Co/Al2O3 catalyst with conventional and
sol-gel methods to vary the chemical reactivity of the alumina support and
found that the reactivity of the surface changes the surface structure and
chemical composition of the catalyst. When the metal-support interaction is
weak, Co3O4 was the predominant surface phase and with an increase in
surface reactivity the presence of CoO and CoAl2O4 on the surface were
observed. The performances of some cobalt based catalysts such as mixed
oxides derived from Co-Al hydrotalcite precursor, cobalt supported on
alumina and Co-Mn perovskite in the selective oxidation of toluene to
benzaldehyde were studied by Centi et al133
and reported that the sample
CoOx/Al2O3 mixed oxide derived from hydrotalcite precursor having Co: Al
ratio of 2 was active and selective.
Vakros et al134
modified the equilibrium deposition filtration
technique to allow the deposition via adsorption of a relatively large amount
of Co2+
ions on the γ-Al2O3 surface and prepared CoO/ γ-Al2O3 catalysts
with a very high active surface compared to that achieved by conventional
pore volume impregnation technique. Ataloglou135
prepared CoO/γ-Al2O3
catalysts using three methods. Pore volume impregnation, equilibrium
deposition filtration and pore volume impregnation by adding nitrilotriacetic
acid in the impregnation solution to study the influence of methodology used
for mounting Co(II) species on the γ-Al2O3 surface on the catalytic activity
of the catalyst for complete oxidation of benzene and observed that ‘pvi’
36 Chapter 1
catalysts exhibited the highest activity among the samples with low or
medium Co content, whereas the ‘edf’ catalysts exhibited the highest activity
among the catalysts with the maximum Co content. In another study,
Ataloglou et al136
investigated the influence of the initial concentration of the
impregnating solution used for mounting Co(II) species on γ-Al2O3 surface
by equilibrium deposition filtration method on the catalytic activity of
catalysts for the complete oxidation of benzene and observed higher catalytic
activity for catalysts prepared using high initial concentration of Co(II)
concentration.
1.10. NiO/Al2O3 mixed oxides
Alumina doped with Ni2+
ions is an important system since it
contains a d8 metal ion having interesting electronic, magnetic and catalytic
properties. This system is used in industry as heterogeneous catalysts and
ceramic pigments. Salagre et al137
reported the chemical preparation, surface
areas, pore distributions of several γ-alumina supported nickel samples active
for the catalytic hydrogenation of hexanedinitrile. XPS results showed the
presence of surface Ni2+
in the form of stoichiometric and non-stoichiometric
NiO, and stoichiometric and non-stoichiometric nickel aluminates and
surface reduced nickel. Nickel aluminate is detected at calcination
temperatures greater than 3500C Catalytically active reduced nickel (for
nitrilehydrogenations) either as naked crystallites or as encapsulated nickel
inside voided non-stoichiometric aluminate shells lie on top of the
underlying catalytically inactive NiAl2O4 when precursor calcination
temperatures are higher than 3500C and reduction temperatures of 400
0C.
Dimitrijewits et al138
prepared two series of NiO/γ-alumina catalysts
with Ni content between 3.5% and 14% and their crystalline phases, porous
Introduction 37
microstructure, and methane dry-reforming reaction behavior were studied.
In the case of the impregnated series, the results could be related with the
formation of two kinds of Ni sites: one derived from free-nickel oxide on the
support surface and another produced from NiAl2O4 due to the oxide-support
interaction. The ratio between both types of sites might change from the
beginning of the catalytic reaction to the stationary state (12h of reaction). In
the other series, which had the Ni included in the alumina matrix, an increase
of the specific activity of the sample with the highest Ni content at stationary
state, could indicate changes in the Ni sites during the reaction process. The
conversion values indicated, at both initial and stationary states, the
effectiveness of increasing the Ni-content in the two series.
Goncalves et al139
prepared and characterized various nickel based
catalysts derived through sol–gel method and reported that their surface area
decrease in the sequence Ni-SiO2 > NiAl2O3 > Ni-TiO2. Li et al140
prepared
and characterized three Ni-Al2O3 catalysts, with nickel loadings of 10-13
wt.%, by co-precipitation, impregnation on a sol–gel derived alumina, and
impregnation on a commercial γ-Al2O3 and reported that sol–gel derived
Al2O3 structure was the most stable support up to temperatures of 1000ºC.
Han et al141
investigated the influence of various factors on the existence of
the excess NiO in the sintered sample on preparing spinel from 1:1 mixture
of NiO and Al2O3 and reported that the milling time and starting materials
had an important effect on the excess of NiO while the sintering temperature
and sintering time had little effect on it.
Amini et al142
demonstrated that the coprecipitated mixture of nickel
and aluminum hydroxide precursor absorbs microwave effectively, and that
leads to the formation of nickel aluminate spinel with dominant species are
nickel ions in the tetrahedral coordinated sites. Peelamedu et al143
reported
38 Chapter 1
the simultaneous synthesis and sintering of NiAl2O4 from NiO +Al2O3
powder mixture in just 15 min in a 2.45-GHz microwave field and suggested
that the anisothermal reaction condition that was achieved in a microwave
field appears to be responsible for the observed enhancement in the reaction
kinetics of NiAl2O4 formation. Jeevanandam et al144
reported the synthesis of
nano-sized nickel aluminate spinel particles with the aid of ultrasound
radiation by a precursor approach. Sonicating an aqueous solution of nickel
nitrate, aluminium nitrate and urea yields a precursor, which on heating at
950°C for 14h yields nano-sized NiAl2O4 particles with a size of ca. 13nm
and with a surface area of about 108m2 g
-1. Arean et al
145 prepared NiAl2O4
and Al2O3-NiAl2O4 spinel solid solutions at 500ºC by means of a sol–gel
route, starting from mixed metalalkoxides, with materials having a surface
area greater than 200m2 g
_1 and reported that mixing at the molecular level
between the precursor materials seems to be the key factor allowing spinel
formation at a relatively low temperature
Thermal treatment has recently been emerging as a promising
environmental technology to stabilize heavy metal-containing industrial
sludge. Shih et al146
incorporated Ni-laden waste sludge into kaolinite-based
construction ceramic materials and evaluated incorporation efficiency and
nickel leachability of the products. Results from prolonged leachability tests
of NiO and NiAl2O4 indicate the NiAl2O4 containing samples showed
stronger intrinsic resistance to acidic attack and revealed the superiority of
NiAl2O4 over NiO in stabilizing nickel over long time periods.
1.11. CeO2/Al2O3 mixed oxides
Cerium oxide is an important component of fine grade abrasives for
polishing glass, thin film optical divices, 147
gas sensors148
superconductors, 149
Introduction 39
and heterogeneous catalysts150-152
. Alumina supported ceria forms part of the
classical three-way catalysts used for the elimination of pollutants in
automobile exhausts. Ceria acts as a catalytic activity promoter and this
promoting effect can be classified in two general types. First, it works as a
structure promoting component in the stabilization of the alumina support
toward thermal sintering153
and second as a chemical promoter enhancing the
oxygen storage capacity of the catalysts. The oxygen storage capacity of
CeO2/Al2O3 catalysts is attributed to reversible change in the cerium oxidation
state24.
The change in oxidation state is associated with reversible removal and
addition of oxygen and hence the designation oxygen storage.
Martinez-Arias et al154
characterized and studied the catalytic activity
of Pt/ CeO2/Al2O3 in CO-O2 reaction. The support was prepared by incipient
wetness impregnation of -Al2O3 with an aqueous solution of
Ce(NO3)36H2O. The platinum was incorporated by impregnation of support
with solution of [Pt(NH3)4](OH)2 previously neutralized with nitric acid.
Characterization of the surface sites carried out by means of EPR using
oxygen as the probe molecule indicates that platinum is located on
bidimensional ceria patches present at the alumina surface. The enhancement
of low temperature reduction of platinum by ceria at these sites under
CO+O2 reacting mixture led to the conclusion that the above sites are active
for the CO oxidation reaction. Damyanova et al155
reported that CeO2
loading results in the improvement of catalytic performance of CeO2/Al2O3
supported platinum catalysts for the reforming of methane with CO2.
X-ray absorption spectroscopic studies on CeO2/Al2O3 and
Pd/CeO2/Al2O3 catalysts in the reduction of NO by CO indicated that for
stoichiometric mixtures of NO + CO, the average oxidation state of cerium
was between +3 and
+4and that of Pd was between 0 and
+2
156. Cracium et
40 Chapter 1
al157
reported that the rate of steam reforming of methane was two order of
magnitude higher on Pd/CeO2/Al2O3 than on Pd/Al2O3, which was attributed
to a catalytic synergism between Pd and CeO2. Propane oxidation was
studied on a Pd supported alumina catalyst promoted with ceria, by
Guimaraes et al158
. X-ray photoelectron spectroscopy and temperature
programmed surface reaction were used to characterize the surface sites. It
was observed that the Pd/CeO2/Al2O3 catalyst was less active for oxidation of
propane at low temperatures than the Pd/Al2O3 catalyst, but became very
active at higher temperatures. However, at high temperatures large quantities
of H2 were released, which suggest a drastic change in selectivity. XPS
results showed that the catalyst containing CeO2 form the highest oxidation
state palladium species, PdO after the oxidation of propane. Xiao et al159
reported that the CeO2-MO2 (M = Zr4+
, La3+
, Ca2+
or Mg2+
) solid solution
modified Pd/-Al2O3 catalysts are efficient for the catalytic combustion of
methane and are comparable in activity with other conventional catalysts.
The active sites in the catalyst system are contacts between Pd and the CeO2-
MO2 mixed oxide component.
Kurungot et al160
reported that catalytic reactor system consisting of
integrated micro porous silica with a sand-witched type Rh/-Al2O3 catalyst
layer can give better efficiency for reforming of methane. They found that
promoting the Rh/-Al2O3 catalyst with ceria resulted in significant
improvement in the catalytic stability, possibly due to the kinetic and
oxidative stabilization of the catalyst matrix with ceria.
During a comparative study of Cu/Al2O3 and Cu/CeO2/Al2O3
catalysts with redox processes induced by thermal treatments in CO on
preoxidized samples, Martinez-Arias et al161
observed that the reduction of
copper species is favored when it is in contact with more dispersed two-
Introduction 41
dimensional ceria entities. This easier reduction of copper interacting with
ceria is presumed to favor the catalytic activity of Cu/CeO2/Al2O3 for CO
oxidation. Andreeva et al162
reported that gold-vanadia catalysts supported
on ceria-alumina (1:1) exhibited higher benzene oxidation activity in
comparison with the corresponding ones on ceria-alumina (1:4). It was also
observed that the presence of alumina prevents the agglomeration of gold
and ceria.
Djuricic et al163
reported the preparation and properties of alumina-
ceria nano-nano composites by the calcination of gels obtained by
homogeneous precipitation from dilute chloride and nitrate solutions,
followed by either microwave treatment, autoclave treatment or air drying.
They observed a variety of morphologies depending on the processing route.
The calcined microwave treated gels consisted of nano-size particles of ceria
in nanostructured transition alumina, suitable for catalysis applications.
Decarne et al164
studied the reducibility of Ce-Al-O solids using the H2-TPR
and EPR and found that dispersion of ceria on alumina stabilizes surface
ceria and improve the reducibility of bulk ceria. When ceria content
increases, reduction temperature of bulk ceria increases, whereas reduction
temperature of surface ceria decreases.
Fetter et al165
reported the selective formation of diisopropyl ether
from 2-propanol on alumina- ceria pillared clay catalysts and found that the
reaction depends on the structure and acidity of active sites. The addition of
ceria promotes selectivity and conversion rate of the reaction. Rajiah et al166
reported the synthesis of 3-nitrothphalic acid from 1-nitronaphthalene using
-alumina supported ceria catalyst at 900C with 80 mol% yield and 98%
selectivity.
42 Chapter 1
Saab et al 167
investigated the catalytic oxidation of carbon black in the
presence of CeO2 and Al2O3 catalysts and reported that the rate of carbon
black combustion increases considerably in tight contact conditions. For tight
contact CB-catalyst mixtures, a new EPR signal, designated by S2, is
observed. The appearance of the new signal indicates the formation of new
paramagnetic species consistent with localized paramagnetic spins on the
carbon particles and catalyst interface and can be considered as a fingerprint
of the contact between the two solids. These new species increase the
reactivity of the tight contact CB + CeO2 mixtures in the catalytic reaction of
CB combustion. Sun et al 168
prepared a series of alumina doped ceria
catalysts by citric acid complex combustion method and used for soot
combustion and reported that a strong interaction between CeO2 and Al2O3 in
the mixed oxide developed.
Piras et al169
reported that under oxidizing conditions at 12000C, ceria
is almost ineffective as a stabilizing agent for alumina whereas under
reducing conditions its effects are remarkably enhanced and surface area in
the order of 60 m2/g can be retained after heat treatment at 1200ºC for
several hours. This is directly related to the formation of Ce3+
present mainly
as CeAlO3, which inhibits crystal growth and prevent formation of the -
alumina responsible for reduction in surface area. The ceria entities present
in alumina supported ceria system can be classified according to their
different dispersion degrees: dispersed ceria entities, which include isolated
cerium ions, clusters thereof and or more or less thick CeOx two dimensional
patches (or 2D-Ce entities) and non-dispersed ceria species i.e. ceria
aggregates or 3D-Ce entities. The formation and properties of dispersed ceria
entities depend strongly on the interaction established with underlying
alumina support. The ceria aggregates shows properties close to that of
Introduction 43
unsupported ceria entities. Martinez-Arias et al170
reported that the relative
amounts of each of these species did not show a linear relationship with the
ceria loading. As the ceria loading increased a trend towards formation of
3D-Ce was observed.
1.12. TiO2/Al2O3 mixed oxides
Alumina-titania mixed oxide system is of interest for many
applications such as catalyst, catalyst supports and as an advanced ceramic
material171-174
. It was reported that TiO2/Al2O3 system show high catalytic
activity in the synthesis of aniline from phenol and ammonia and to possess
increased acidity compared to the single oxides175
. Aluminium titanate has
been identified as an important high temperature ceramic in view of its low
thermal expansion coefficient, low thermal conduction, excellent thermal
shock resistance and high melting point.176, 177
A number of investigations have identified alumina-titania
composites as potential catalyst supports for application in coal liquefaction.
Parker et al178
evaluated alumina-titania supported molybdenum
hydrogenation catalysts for coal liquefaction. The catalyst support was
prepared by co-precipitation from aqueous AlCl3 and TiCl4. The optimum
titania loading was found to be 30 mol.%.
Mostafa et al179
reported that TiO2/Al2O3 catalysts, prepared by
calcination of hydro-gels precipitated from the respective chloride solutions
were more active in dehydrating alcohol than the corresponding single oxide
catalysts alumina or titania. Dehydration of alcohols is related to the amount
of surface acidity rather than to the strength of surface acid sites. The
chemical composition and calcination temperature of mixed oxides also
affect the performance of the catalysts in the dehydration of alcohol.
44 Chapter 1
Stringent environmental regulations are exerting pressure to reduce the
maximum allowable sulfur content in diesel. Almost complete removal of 4,6-
dimethyl dibenzothiophene will perhaps be inevitable for reducing the sulfur
content of diesel to a level of 50 wppm and lower. Lecrenay et al180
reported
that the activity of alumina -itania supported Co Mo catalysts were higher than
that of the alumina supported catalysts for hydrodesulfurization of 4,6-
dimethyl dibenzothiophene. It was concluded that the increased acidity caused
the enhancement of activity. Cecilio et al181
observed that sol-gel alumina-
titania supports with TiO2 mol.% between 30 and 50 show good mesoporous
texture and it was particularly valuable for the preparation of well dispersed
MoS2 active phase which leads to a hydrodesulfurization catalyst with higher
activity than that prepared using commercial alumina support.
Effects of titania on the catalytic property of Pd/Al2O3 towards methane
combustion were examined by Wang et al182
. It was observed that the catalytic
activity of Pd/Al2O3 catalysts was considerably improved by pre-coating the
alumina support with titania. Hydrogen chemisorption and BET measurements
revealed that titanium modified alumina could modify the support characteristics
to achieve a high dispersion of Pd. Temperature programmed reduction and
temperature programmed desorption studies demonstrated that the coating of
Pd/Al2O3 with titania can weaken the bond strength of Pd-O and enhance the
catalytic activity towards methane combustion.
Reduction of nitrogen oxides emission has become one of the most
pressing issues to be solved for environmental protection. Catalytic reduction
of nitrogen oxides by hydrocarbon is a promising method for the removal of
dilute nitrogen oxides from engine exhausts. Kawabata et al183
prepared
alumina-titania catalysts from various alumina and titania sources, metal
alkoxides and metal alkoxide modified with organic groups by sol-gel
Introduction 45
method. It was observed that specific surface area, pore size distribution,
solid acidity and catalytic activity of NO reduction for the alumina-titania
catalysts depended on the alumina and titania sources. The catalyst prepared
from metal alkoxide for alumina source and metal alkoxide modified with
organic groups for titania source exhibited higher activity of NO reduction
than other alumina-titania catalysts.
Farias et al184
prepared 1:1 mixed oxides of Al2O3-ZrO2, Al2O3-TiO2,
SiO2-TiO2 and ZrO2-TiO2 at 6000C from sol-gel derived precursors and all
samples had amorphous structures. The oxides are active catalysts in the
epoxidation of cyclooctene with tert-butylhydroperoxide as oxidant. The
titania containing catalysts are the most active and selective ones. Gutierrez-
Alejandre et al185
reported a comparative study of alumina-titania mixed
oxides prepared by sol-gel and impregnation procedures. It was observed that
the samples prepared by sol-gel process showed an increase of surface area
with titania loading, in contrast to their impregnation counterparts, where a
decrease was observed. Better titania dispersion was obtained by the sol-gel
technique than by impregnation technique.
Montoya et al186
reported the effect of temperature on the structural
and textural evolution of sol-gel alumina-titania mixed oxides. Mixed oxides
calcined at 500ºC were amorphous and formed by nanometric particles and
pore sizes of about 2 nm. For these samples the surface area increased as the
titania concentration increased. The sintering process started at 7000C,
resulting in particle and pore size growing from 2nm to about 10 nm and the
powders remained amorphous. At 900ºC both sintering and crystallization
process of TiO2 and Al2O3 were accelerated by the Ti4+
segregation, rutile
and -Al2O3 were present as separate phases.
46 Chapter 1
Linacero et al187
studied a series of xTiO-(1-x)Al2O3 mixed oxides
prepared by sol-gel method with variable amounts of titania, from pure
alumina to pure titania. The textural results showed that at low titania
contents, higher surface area than those of pure alumina were obtained, and
in titania rich samples, higher surface areas than for pure titania were
stabilized. The titanium content also affected the crystallization process. It
was suggested that changing the composition of the mixed oxide might vary
the strength and distribution of the acid sites.
A series of xTiO-(1-x)Al2O3 mixed oxides with different molar ratios
were prepared by a non-alkoxide sol-gel route. It was found that alumina
introduces structure and textural modification to titania and the resultant
properties of the mixed oxides vary with the composition. The anatase to
rutile phase transformation temperature increased with increasing mole
percent of alumina. The surface areas of mixed oxides were about 80%
higher than that of pure alumina 188
. Alumina-titania nano mixtures with
molar ratio 1:0.5 and 1:5 were synthesized by a sol-gel technique. The
precursor powders were characterized by TGA, BET and TEM. The results
showed that as the titania content increases the specific surface area
increased. TEM monographs showed a highly homogeneous distribution of
the constituents with fine needle like particles of ~10nm size189
. In another
report190
they observed a specific surface area as high as 291m2g
-1 for 1:5
Al2O3/TiO2 composite calcined at 400ºC.
I.13. Scope and objectives
The vast majority of catalysts used in modern chemical industry are
based on mixed metal oxides .The preparation of specific tailor made mixed
oxides which can perform complex functions is one of the main topics of
Introduction 47
research in the field of heterogeneous catalysis. Achieving complex catalytic
reactions require a poly-functional catalyst with appropriate morphological
properties. The mixed metal oxide catalyst preparation has focused on a
tuning of the chemical reactivity of the oxide surface to modify the
interaction with adsorbed reacting species. Catalytic activities of oxides have
been associated with surface defects such as surface vacancies. Surface
vacancies are basic or acidic, depending on the type of missing ions. Cation
vacancies can be highly basic while anion vacancies are acidic. Defects in
solid oxides are generally made by doping it with a compound in which the
metal ion has a valence other than the metal in the host oxide. Over the past
decade, research on nano-crystalline materials has been greatly accelerated
by the advances in the ability to manipulate structures on the molecular or
atomic level. Direct synthesis and successful stabilization of nano-crystalline
ceramic materials has only recently been investigated in detail for some
catalytic applications. When a ceramic is fabricated from “nano” powders,
the resulting advanced nano-phase material has dramatically improved
properties; it may conduct electrons, ions and heat more readily than
conventional materials, the features that will have impact on catalyst
efficiency.2 The needs for better catalysts will only increase as environmental
and economic concerns motivate the development of them.
From the discussion made earlier it is clear that in most of the reports
the multi-component oxides were prepared by impregnation of the metal salt
on γ-Al2O3 or solid-solid blending of metal oxide and γ-Al2O3 at high
temperatures. These methods have inherent weakness regarding homogeneity
and surface properties of the products. In these methods the matrix
component used was commercially available γ-Al2O3 and it is likely that this
may considerably affect the reproducibility of the samples prepared. Use of
48 Chapter 1
hydroxides of aluminium as precursor for Al2O3 is fundamental to obtain
pure and reproducible matrix component. Boehmite remains the most
important and versatile precursor for the synthesis of transition aluminas.
Further no study was reported by systematically varying the level of
incorporation of metal ions into the matrix component and calcination
temperature and the influence of these factors on the structural evolution of
various phases and surface characteristics of mixed metal oxides generated.
The present investigation aims to modulate the surface properties of alumina
by doping with Cu2+
, Mn2+
, Co2+
, Ni2+
, Ce4+
and Ti4+
ions using boehmite as
the source of alumina through sol-gel route. For a better understanding of the
properties of the mixed metal oxides developed, it is necessary to know the
structural transformations that occur when the metal ion doped boehmite
xerogels are calcined over a range of temperatures. Therefore we have
focused more on the effect of dopants on the structural evolution of alumina
from boehmite. Thus the main objectives of our study are:
Generation of Cu2+
, Mn2+
, Co2+
, Ni2+
, Ce4+
and Ti4+
ions doped
boehmite xerogels containing varying concentrations of the dopants
and the study of the thermal characteristics of the mixed xerogels to
monitor the chemical processes and phase evolution in them.
Preparation of Cu2+
, Mn2+
, Co2+
, Ni2+
, Ce4+
and Ti4+
ions doped
alumina mixed oxides by the calcination of the above xerogels at
various temperatures.
Investigation of the effect of dopants on the structural evolution of
alumina from boehmite by spectroscopic technique and PXRD
method.
Introduction 49
Monitor the formation characteristics of alumina based spinels
MAl2O4 (M = Cu2+
, Mn2+
, Co2+
and Ni2+
) on calcination of the mixed
xerogels and study the influence of these compounds on the structural
evolution of alumina from boehmite.
Investigation of the influence of the insitu formed MAl2O4 spinels on
the surface characteristics of the alumina mixed oxides.
Investigation of the surface acidity features of the doped and undoped
oxides developed through pyridine adsorption by employing TGA,
FTIR and CHN analysis.
Study of the surface characteristics such as specific surface area, pore
volume and pore size distribution of the selected mixed metal oxides
developed which are relevant for catalytic functions.
50 Chapter 1
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