ORIGINAL PAPER
Very low temperature wet-chemistry colloidal routesfor mono- and polymetallic nanosized crystallineinorganic compounds
Paolo Dolcet • Stefano Diodati • Maurizio Casarin •
Silvia Gross
Received: 13 June 2014 / Accepted: 14 October 2014 / Published online: 26 October 2014
� Springer Science+Business Media New York 2014
Abstract The use of low temperature, sustainable pro-
cesses based on cheap and safe chemicals as well as non-
toxic, easy to handle chemicals and solvents is a
challenging issue in modern inorganic chemistry; moreover
the obtainment of crystalline functional nanostructures at
low or even room temperature is the goal of many synthetic
efforts. Within this framework, in these last years, we have
developed in our group different room or low temperature
(T \ 150 �C) wet chemistry colloidal routes to prepare
different inorganic functional nanomaterials. These com-
pounds range from (1) ferrites to (2) pure and doped metal
oxides, sulphides and halogenides, to (3) metal/metal oxide
nanocomposites. The adopted wet chemistry routes
encompassed (1) miniemulsions, (2) coprecipitation com-
bined with hydrothermal route and (3) more classical col-
loidal routes, though revised in some critical aspects. This
mini-review provides an overview of the main features as
well as the pros and cons of the proposed routes for the
obtainment of targeted inorganic systems for applications
in optical bioimaging or in energy applications. It not only
summarises already published work, but also presents some
exciting perspectives disclosed by performed studies and
past experience as well as comparisons with state-of-the-art
research.
Keywords Wet-chemistry � Colloids � Inorganic
compounds � Low temperature � Room temperature �Colloidal routes
1 Introduction
In the preparation of inorganic nanostructures, the opti-
misation of experimental routes which are based on the use
of mild synthesis conditions, accomplished by most solu-
tion processing methods, is currently an intensively
explored field of research. This field complies with the
precepts of both green chemistry [1, 2] as well as of
resources and energy constraints [1]. In addition, it satisfies
the demands and requirements of the manufacturing
industry. The achievement of nanocrystalline and compo-
sitionally pure materials by using mild conditions (e.g. low
operating temperature and pressure), easy to implement
procedures, safe chemicals and solvents, as well as possibly
avoiding the use of critical raw materials [3, 4] is of par-
amount importance.
In this context, the resort to colloidal-based method
appears one of the most viable choices since, when suitably
optimised from the experimental point of view, this class of
methodologies enables, in the above mentioned mild con-
ditions, a fine control on the very early stages of nano-
structure formation (i.e. nucleation and growth). In this
way, materials with the desired compositional, morpho-
logical and structural features are afforded. These manifold
approaches have already been extensively used for the
synthesis of nanostructured inorganic colloids [5]. Indeed,
controlling the size and shape of inorganic nanostructures
Electronic supplementary material The online version of thisarticle (doi:10.1007/s10971-014-3549-4) contains supplementarymaterial, which is available to authorized users.
P. Dolcet � S. Diodati � M. Casarin � S. Gross (&)
Dipartimento di Scienze Chimiche, Universita degli Studi di
Padova and INSTM, UdR di Padova, Via Marzolo, 1,
35131 Padua, Italy
e-mail: [email protected]
P. Dolcet � S. Gross
Istituto per l’Energetica e le Interfasi, IENI-CNR and INSTM,
UdR di Padova, Via Marzolo, 1, 35131 Padua, Italy
123
J Sol-Gel Sci Technol (2015) 73:591–604
DOI 10.1007/s10971-014-3549-4
in a precise way is a highly fascinating challenge. This
struggle is justified by the improved functional properties
arising when particle size is decreased (to the order of
nanometres) and by the particular nanostructures, shapes
and morphologies which can be obtained. Many different
wet-chemistry methodologies such as (1) sol–gel [6], (2)
solvo/hydrothermal (see Sect. 3) (3) nucleation and growth
in suspension [1, 2, 7] (see Sect. 2) have been developed in
order to achieve these goals. Control over size, shape and
morphology, combined with mild processing parameters
(mainly in terms of temperature and pressure) are favour-
able conditions to be implemented for sustainable and cost-
efficient production of functional inorganic materials.
Further requirements to devise and implement environ-
mentally and economically sustainable synthesis routes are
(1) reproducibility, (2) ease of processing, (3) use of safe,
common chemicals, (4) easy purification steps, (5) high
yields.
In the last years, we have approached different metal
oxides and sulphide systems (pure, mixed and/or doped) by
using classical sol–gel routes [8–12] or colloidal approa-
ches involving the nucleation/growth of the target struc-
tures in suitably optimised solutions/suspensions [13–15].
The former approach involved a post-synthesis thermal
treatment at temperature typically higher than those
addressed in this contribution, and will therefore not be
dealt with further. The latter strategy instead afforded the
formation of crystalline ZnO [15], CuS [13] or ZnS [14]
already at room temperature, without the need of post-
processing, and will therefore be described in greater detail
in the following paragraphs.
2 Nucleation and growth of crystalline colloidal
nanostructures in solution/suspension
2.1 Room temperature synthesis of nanocrystalline
ZnO in different dispersing media: effect of solvent
properties on the morphology of the resulting
nanostructures
ZnO is a very intensively investigated material: its prop-
erties, applications [16–28] and synthesis route have been
extensively reviewed by several authors [29–42], to which
interested readers are referred.
In our case, by implementing and adapting the well-
known procedure reported by Spanhel et al. and Bahne-
mann et al. [32, 33, 42], we developed [15], an easy and
highly reproducible route to nanostructured colloidal ZnO
nanoparticles based on the controlled hydrolysis and con-
densation of zinc acetylacetonate (acac) in alkaline con-
ditions. In detail, by reacting a Zn(acac)2 ethanol solution
with NaOH in a 1:2 molar ratio, ZnO spherical crystalline
nanostructures were obtained after reflux at 80 �C. The
nanostructures displayed a homogeneous size distribution
with particle diameter ranging from 6 to 10 nm, as revealed
by transmission electron microscopy (TEM) micrographs.
Aside from the synthetic purposes, our study was however
also devoted to investigating the influence of the chemistry
of the colloidal system on the final features of the resulting
zinc oxide. In this regard, in order to assess the effect of the
solvent viscosity and dielectric constant on the features of
the obtained material, the same reaction was carried out in
water, glycerol or 1,2-propanediol, characterised by the
chemico-physical properties reported in Table 1 in the ESI,
and yielding nanostructures displaying different size and
morphologies. In all cases, the room temperature crystal-
lisation of hexagonal ZnO was proven by X-ray diffraction
(XRD) analysis, from which, by the Scherrer formula, an
average crystallite size could be calculated (Table 1 in the
ESI). Interestingly, a relevant effect of the chemico-phys-
ical properties of the dispersing media on the morphology
of the resulting nanostructures was highlighted and indeed
different particles sizes and very different morphologies
were obtained. The reflux step was also shown to be a key
factor to avoid the fast precipitation of the oxide and to
achieve a pure compound, since the conversion to the
targeted oxide was complete, and no traces of residual
unreacted Zn(acac)2 could be pointed out, as opposed to
syntheses carried out without heating, where a mixture of
wurtzite, other zinc-based products and organic residue
was obtained [15].
The differences outlined both in size and shape (see
reference 15 for details) could be traced back to the dif-
ferent chemical nature of the different dispersing media.
However, it was not possible to identify a definite corre-
lation between the relevant chemico-physical properties
(pKa, dielectric constant and viscosity at room and final
temperatures) of the four media (Table 1 in the ESI), the
mechanism of hydrolysis and condensation and the
resulting morphologies. In particular, no relationship
between viscosity, acidity, dielectric constant and crystal-
lite size could be rationalised, which would be expected in
the case of an oversimplified growth model based only on
diffusion. The investigation of the kinetics of the process
by time-resolved EXAFS was also very challenging due to
the coexistence of different species and different equilibria
in solution, delivering only an averaged picture of the
whole system. In conclusion, nanocrystalline ZnO nano-
structures displaying different size and shape were
obtained at room temperature by a very easy colloidal route
in four different media, and the effect pKa, dielectric
constant and viscosity on morphology was evidenced,
although not fully rationalised [15].
592 J Sol-Gel Sci Technol (2015) 73:591–604
123
2.2 Room temperature synthesis of nanocrystalline
CuS in carboxylic acids as different dispersing
media: effect of solvent properties
In this study, we addressed the synthesis of colloidal CuS
nanostructures by taking advantage of the peculiar features
of the dispersing media, in this case carboxylic acids [13].
The crystalline hexagonal phase (covellite) of CuS is
often described as a p-type semiconductor (energy gap
1.2–2.0 eV) [43, 44], which shows superconductivity at
1.6 K [45]. Cupric sulphide [46] raises interest as a starting
material for transparent conductive films [47, 48] capable
of transmitting only the visible part of the solar spectrum,
as a catalyst [43] and as a filler to enhance conductivity
[49–51] or wear resistance of polymeric materials. In the
nanosized range, CuS has been used as a cathode for Li-ion
batteries [52], as a photocatalyst for the degradation of
organic dyes [53] and as an additive to improve the tri-
bology properties of polymer composites [54]. Because of
their broad absorption in the near IR range [55], CuS
nanoparticles find also use as IR sensors [56], and, in the
last few years, CuS nanostructures were also tested for
nanomedicine applications [57].
Concerning wet-chemistry approaches to CuS [46], this
system has been prepared via: (1) hydro/solvothermal
methods [58–62], (2) sonochemical methods [63, 64], (3)
colloidal synthesis, (4) microemulsion [65–68], (5)
microwave assisted synthesis [69, 70], (6) surfactant-
assisted templating [71], (7) by using chelating agents [72]
or (8) by organogel-assisted synthesis [73]. The most
generally used precursors are copper (II) inorganic com-
pounds (CuO, CuSO4, CuCl2, etc.) and sulphur sources like
gaseous H2S, thioacetamide, thiourea, dimethylthiourea
carbon disulphide, sodium thiosulfate, sodium sulphide and
elemental sulphur (for further details see [13] and refer-
ences therein).
In our case, we addressed the synthesis by promoting the
controlled nucleation and growth on the CuS nanoparticles
in a carboxylic acid suspension (for synthesis details, see
Scheme 1 in ESI and Ref. 13). Specifically, the optimised
methodology was based on the fast nucleation of the sul-
phide triggered by the reaction of thioacetic acid (acting as
a slowly releasing sulphide source) with water and copper
carboxylates (acetate, propionate) in the corresponding
carboxylic acid (acetic, propionic) solvent. In this regard,
the choice of carboxylic acids as dispersing media was
motivated by several chemical considerations and advan-
tages: (1) hydrolysis of the C–S bond (in thioacetic acid) is
favoured thus producing a fast CuS supersaturation and a
high nucleation rate; (2) the mobility of the precursor
molecules is limited by the high viscosity of the medium,
thus favouring nucleation events with respect to particle
growth; (3) the low dielectric constant of the medium
stabilises the nanoparticles dispersion by reducing the
critical coagulation concentration.
As far as the first and second points are concerned, the
acid environment enhances the nucleation rate and, at the
same time, slows down the growth rate. The former event
arises from the fast CuS supersaturation produced by the
acid catalysed hydrolysis of carbon–sulphur bonds of
thioacetate groups. The growth rate is likely dependent on
the nucleophilic power and acidity of copper hydrosulphide
species that condense with each other to produce the sul-
phide: the nucleophilic power and growth rate would be
enhanced by deprotonation of these molecules, but the
acidity of solvent lowers this effect. Furthermore, the rate
of particle growth is reduced due to the relatively high
viscosities of carboxylic acids with respect to many other
common solvents and the low mobility of the precursor
molecules diminishing the effect of collision between
particles and therefore the supply of material to the
growing particles. As far as the third factor is concerned, as
already mentioned, the low dielectric constant of pure
carboxylic acids stabilises the dispersion by reducing the
critical coagulation concentration.
A mechanism describing the different steps leading to
the formation of CuS, and explaining the role of the pre-
cursors, was proposed and assessed by vibrational spec-
troscopy, which is reported in Ref. [13].
The choice of the precursors was also motivated by
considerations regarding the chemistry of the resulting
system. In fact, one main advantage of using copper
acetate and thioacetic acid as precursors is the formation
of acetic acid as a reaction product, i.e. solvent molecules.
Consequently, the low dielectric constant of the reaction
environment is fully preserved. The prepared nanoparti-
cles were investigated by UV–V is spectroscopy, X-ray
photoelectron spectroscopy (XPS), atomic force micros-
copy and dynamic light scattering. The nanoparticle
suspensions are clear and characterised by a blue-
shifted adsorption edge with respect to bulk CuS. Light
scattering measurements performed on acetic acid sus-
pensions highlighted the formation of monodispersed
nanoparticles with an average diameter of about 5 nm,
thus proving the effectiveness of the adopted procedure in
achieving controlled nucleation and growth of the targeted
nanostructures.
In conclusion, as was the case for ZnO (2.1), the suc-
cessful synthesis of inorganic nanostructures was afforded
by a facile, reproducible, in this case room temperature
wet-chemistry colloidal route, in which the proper choice
of precursors and reaction conditions were proven to play a
major role in directing the systems towards the targeted
materials.
J Sol-Gel Sci Technol (2015) 73:591–604 593
123
3 Hydrothermal synthesis
3.1 Basics of hydrothermal synthesis
and crystallisation under hydrothermal conditions
The term hydrothermal synthesis typically refers to wet
chemistry routes based on an aqueous medium which are
carried out at relatively high pressures and temperatures
[74], either over or under critical conditions. Originally,
this class of synthesis protocols was developed with the
objective of mimicking the conditions in which crystals
grow within the Earth crust [74, 75]; indeed through this
route the rapid growth of large, pure crystals could be
achieved [74–80].
More recently, this method has been applied to the
synthesis of more complex systems, such as binary or
ternary metal compounds, in nanosized crystalline form.
Several works have been published on many different
compounds such as zinc oxide [81, 82], titania [83–85],
ceria [86, 87], metal sulphides [88, 89] as well as several
more complex compounds [90] such as titanates [91, 92],
phosphates [93] and ferrites [94–99]. All these synthetic
protocols take advantage of the particular physical condi-
tions involved. In general, ionic product of the solvent
tends to increase with rising temperature and pressure,
whereas viscosity decreases. In the case of water, the
dielectric constant depends on both pressure and tempera-
ture as it is directly proportional with the former, but
inversely proportional with the latter [74, 100] (vide infra,
Table 1).
Considering that the focus of the present work is on
crystalline inorganic compounds, special consideration
must be given to the processes which may lead to crys-
tallisation in hydrothermal conditions. In this context, if
nanocrystals are to form from an aqueous supersaturated
solution, the precipitation process must occur slowly [101],
in order to avoid the formation of amorphous solids. Due to
the nonstandard conditions in which hydrothermal syn-
thesis takes place [102], it is possible for normally less
soluble compounds to be solvated with greater efficiency
and therefore to react more easily [74, 100]. More specif-
ically, concerning the formation of oxide particles through
hydrothermal conditions, the main topic of our recent
research, many different process mechanisms can be
hypothesised (also depending on the specific synthetic
protocol adopted). In the most widely accepted theory [74,
90, 103, 104], the process takes place in two steps: (1)
in situ transformation followed by (2) precipitation and
growth. During the former phase the precursors are dis-
solved and tiny amounts of the target oxide are able to form
as solvated species (owing to the conditions in which the
process occurs); in the latter phase, the low solubility of the
aforementioned products causes them to nucleate and form
crystals. Depending on the conditions involved (tempera-
ture, pressure, precursors etc.) different products (such as
core–shell intermediates) [90] and/or crystalline forms may
form throughout the synthesis and be progressively con-
verted into more stable forms.
In general, hydrothermal synthesis is attractive, com-
pared to more traditional synthesis protocols, due to the
fact that crystalline products with high purity and compo-
sitional uniformity may be obtained under relatively mild
conditions. Furthermore, due to the fact that by altering the
temperature and pressure of the reaction mixture, several
solvent properties change [100], non-classical crystallisa-
tion pathways may be explored [74, 77]. The changes
underwent by viscosity, density and dielectric constant in
the case of water at different temperatures and pressures
are reported in Table 1.
Recently we have applied hydrothermal synthesis to the
preparation of nanostructured crystalline spinel ferrites, as
outlined in the following paragraphs. The synthesis here-
after presented (Scheme 1) involves the combination of
coprecipitation of metal oxalates from an aqueous solution
with hydrothermal treatment of the resulting suspension at
mild temperatures. In this protocol, hydrothermal condi-
tions, though sub-critical, were achieved through autoge-
nous pressure (by heating the reaction mixture in a closed
vessel); additionally the possible decomposition of oxalate
species to carbon dioxide may have caused a further
increase in pressure. The observed small size of the
nanocrystalline particles obtained (Table 2 in the ESI)
suggests that nucleation occurred relatively rapidly within
the reaction mixture, with particle nucleation being kinet-
ically favoured over growth. The choice of oxalate as a
Table 1 Properties of water and vapour as a function of temperature
and pressure [102, 105]
Temperature/�C State Density/
kg�m-3Viscosity/
lPa�sDielectric
constant
Pressure equal to 0.1 MPa
27 Liquid 996.56 853.82 80.20
52 Liquid 987.19 530.32 69.32
77 Liquid 973.73 368.80 61.79
102 Vapour 0.590 12.339 1.006
135 Vapour 0.543 13.285 1.005
177 Vapour 0.484 15.426 1.004
Pressure equal to 1.0 MPa
20 Liquid 996.96 853.67 77.78
52 Liquid 987.58 530.48 69.36
75 Liquid 974.13 369.02 61.82
102 Liquid 957.43 276.59 55.09
135 Liquid 937.87 218.79 49.06
177 Liquid 890.39 153.00 38.81
594 J Sol-Gel Sci Technol (2015) 73:591–604
123
precipitating counter-ion, as opposed to the more common
hydroxide, was motivated by two reasons: (1) compared to
hydroxides, oxalates of transition metals tend to be less
soluble and have much closer solubility constants [102];
(2) oxalates tend to decompose cleanly, without leaving
undesired organic residue, and yielding formation of
crystalline oxide at temperature much lower than in the
case of hydroxides.
By using this approach, we succeeded in synthesising
four different ferrite spinels (CoFe2O4, MnFe2O4, NiFe2O4
and ZnFe2O4) as pure nanocrystalline compounds at very
low temperatures (75–135 �C) [106], as described more in
detail in the following paragraphs.
3.2 Low temperature hydrothermal synthesis
of nanocrystalline ferrites MFe2O4
The most commonly synthesised ferrites are perovskite fer-
rites, with general formula MFeO3, and spinel ferrites with
general formula MFe2O4. When the hydrothermal method is
taken into consideration, the bismuth ferrite BiFeO3 is the
most commonly synthesised perovskite. Several low tem-
perature routes have been developed for this compound
ranging from the preparation of the pure oxide in crystalline
form [94, 107], to the lanthanum doped species [108]. Low
temperature hydrothermal protocols (60–250 �C) have also
been applied to the synthesis of spinel ferrites, among which
CoFe2O4, NiFe2O4 and ZnFe2O4 [95–99].
As far as our research group is concerned, nanocrystalline
spinel ferrites MFe2O4 (M = Co, Mn, Ni, Zn) were syn-
thesised through a simple route combining coprecipitation of
oxalates and hydrothermal synthesis (Scheme 1) [106, 109].
Previous syntheses, involving the isolation and subsequent
calcination in air of the coprecipitated intermediates at high
temperatures (900–1,300 �C), afforded the nickel, cobalt
and zinc spinels (CoFe2O4, NiFe2O4 and ZnFe2O4) [109–
111] as well as the manganese and strontium perovskites
MnFeO3 [109–111] and SrFeO3-d [109, 112].
However, within the framework of implementing a
greener, more sustainable and milder process, the combi-
nation of coprecipitation with hydrothermal synthesis
appeared as particularly attractive due to several factors:
(1) excellent reproducibility, (2) ease of procedure and
implementation (e.g. scale-up), (3) nontoxic precursors, (4)
mild temperatures, (5) use of water as greenest solvent, (6)
easy and quick purification of products (without the need
for other solvents), (7) high yields, (8) high product purity,
(9) high versatility (numerous different compounds were
synthesised through this method, since oxalates of many
metals can be easily prepared).
Several different syntheses were carried out to explore
the effect of the involved synthetic parameters (nature of
the precursors, nominal ratio between precursors, amount
of peptising agent (tetraethylammonium hydroxide—TE-
NOH), treatment temperature, treatment time, purification
protocol) on the products, which are reported in Supple-
mentary Materials (Table 2 in the ESI). Details on the
synthesis and the protocol specifics are reported in Ref.
[106]. Optimisation of the synthesis protocol led to con-
clude that treatment time and amount of peptising agent
had very limited effect on the characteristics of the
resulting compounds, whereas treatment temperature was
much more influential. Syntheses involving ammonium
hydroxide as a base were unsuccessful and led to impure
products. Finally, suitable choice of precursors and ratio
between them was found to be paramount: excessive oxalic
acid proved to lead to the formation of impure phases.
Concerning this last point, it should be noted that, though
pure samples were obtained for cobalt and manganese
spinels with a nominal M/Fe/acid molar ratio of 1/2/4.5
(Table 2), later syntheses were uniformed for all spinels to
a 1/2/4 nominal molar ratio, to avoid the precipitation of
unidentified impure phases which were occasionally
observed in samples prepared with higher oxalic acid
content. Synthetic attempts were also carried aimed at the
synthesis of other oxides (such as MnFeO3), but they were
unsuccessful (Table 3 in the ESI).
The synthesised oxides were thoroughly characterised
by several different techniques from the structural (X-ray
diffraction—XRD), morphological (transmission electron
microscopy—TEM), compositional (microanalysis, micro-
Raman, X-ray photoelectron spectroscopy—XPS, induc-
tively coupled plasma-atomic emission spectroscopy—
ICP-AES) and functional (superconducting quantum
interference device—SQUID) point of view. In particular
the exact stoichiometry of the samples was assessed by
Scheme 1 Reaction scheme for the synthesis
J Sol-Gel Sci Technol (2015) 73:591–604 595
123
ICP-AES, confirming and completing the information
gained through XRD.
XRD analyses confirmed that the powders were
obtained as nanocrystalline, single phase products, and
allowed to calculate, through Rietveld refinement [113],
the crystallite average sizes for the spinels, which were in
the 17–50 nm range (Table 2).
As can be seen from Table 2, a significant variance in
average crystallite size can be observed between the dif-
ferent spinels in dependence of the M metal, as well as the
other synthesis parameters (Table 2 in the ESI). TEM
analyses further confirmed this data, showing that the
particles were indeed nanosized (Fig. 1).
XPS (Fig. 2) and ICP-AES analyses (Table 1) allowed
to gain insight into the composition of the samples
(respectively on the surface and in bulk).
The gathered data further confirmed sample purity as
well as expected stoichiometry and revealed a slight ten-
dency in the zinc ferrite for iron to segregate on the surface
[106].
Micro Raman analyses carried out on different points in
each sample revealed the obtained products to be compo-
sitionally uniform throughout. Microanalysis detected only
negligible amounts of carbon residue on the samples,
confirming that the decomposition of the oxalate precursor
is complete and clean, as well as that the adopted purifi-
cation protocol is appropriate for the removal of organic
residues.
Finally, from a functional point of view, magnetic
measurements were performed through SQUID on two
spinels (namely the cobalt and the manganese ferrites). In
both cases the compounds behaved as predicted, acting as
Table 2 Synthesis conditions
and experimental results for the
obtained compounds
Compound Nominal Fe/
M/acid ratio
Treatment
temperature
and time
Found
structure
Yield % Crystallite
average
size/nm
M/Fe ratio
(from
ICP-AES)
CoFe2O4 2/1/4.5 135 �C; 24 h CoFe2O4 9,990 172 ± 2 2.01
MnFe2O4 2/1/4.5 135 �C; 24 h MnFe2O4 100 2,049 ± 4 2.05
NiFe2O4 2/1/4 135 �C; 24 h NiFe2O4 95 47 ± 2 2.09
ZnFe2O4 2/1/4 135 �C; 24 h ZnFe2O4 92 6 ± 1 /
Fig. 1 TEM micrographs of the four compounds (a) CoFe2O4, (b) MnFe2O4, (c) NiFe2O4 and (d) ZnFe2O4
596 J Sol-Gel Sci Technol (2015) 73:591–604
123
hard and soft ferrimagnetic materials respectively and
reaching magnetisation values of 67.7 emu/g (CoFe2O4)
and 61.0 emu/g (MnFe2O4) [106].
In conclusion, hydrothermal synthesis was successfully
used to prepare four spinel ferrites (namely CoFe2O4,
MnFe2O4, NiFe2O4 and ZnFe2O4) with extremely high
purity and yields. The nature and nominal ratios between
precursors have shown to be heavily influential on the final
products, as excessive amounts of either metal or oxalic
acid led to the formation of impure phases. The effect of
other parameters (such as temperature, employed base and
treatment time (Table 2 in the ESI)) on the purity, size and
crystallinity of the resulting compounds has also been
investigated. Treatment temperature and time influenced
the products to a lesser degree, though it has to be pointed
out that shorter treatment times and lower temperatures led
to lower crystallinity and yields. As far as the synthetic
protocol is concerned, it combines reasonable speed, high
quality and purity of products, environmentally friendly
conditions and low costs with a good versatility. The actual
effect of pressure was furthermore explored, as syntheses
carried out under reflux, under identical thermal conditions
but at normal pressure, afforded products with lower purity
and yields [106].
4 Miniemulsions: chemistry in nanoreactors
4.1 Principles of the miniemulsion approach
Amidst colloidal methods, that of miniemulsions represents
a very appealing option. Miniemulsions are heterogeneous
systems critically stabilised against diffusion and collision-
induced degradation processes, characterised by an average
droplet size between 30 and 500 nm [114–121]. From a
practical point of view this means that, even though the
system is metastable, the droplets reach the smallest pos-
sible particle size under the applied conditions, which also
means that miniemulsions exploit the surfactant in the most
efficient way.
Unlike the cases of other emulsions (i.e., macro- and
microemulsions), which are usually homogenised by
employing mechanical stirring, the peculiarity of miniemul-
sions arises from the fact that they exploit high intensity
ultrasounds [118]. These generate intense shear forces that
are able to overcome the viscous resistance, which would
otherwise dissipate much of the provided energy as heat.
The highly turbulent flow created by the ultrasounds
induces many simultaneous droplet formation and disrup-
tion events, leading to a strong decrease in the overall
polydispersity. During sonication, therefore, the mean
size of the droplets changes quite rapidly, until a steady
state is achieved, with no further variation in the average
dimensions (Fig. 3). Simultaneously, interfacial tension is
found to increase with decreasing droplet size, since a
constant amount of surfactant has to be distributed
throughout an increasingly larger total interface, until a
plateau is reached. Overall, the droplets forming mini-
emulsions reach the minimal particle size under the applied
conditions, and are at the critical borderline between sta-
bility and instability. On the other hand, the narrow poly-
dispersity achieved ensures that diffusion degradation (the
process known as Ostwald ripening [7]) is strongly hin-
dered, and hence, with a careful choice of surfactant,
miniemulsion stability can reach a timescale of weeks or
even months [114].
Fig. 2 XPS survey spectra of
the four compounds
(a) CoFe2O4, (b) MnFe2O4,
(c) NiFe2O4 and (d) ZnFe2O4
(binding energy values
corrected for surface charge)
J Sol-Gel Sci Technol (2015) 73:591–604 597
123
It is worth highlighting that, together with Ostwald
ripening, chemical exchange processes between mini-
emulsions droplets are also prevented. This means that
each single droplet is independent from the others, thus
acting as a nanometric reactor, able to confine a reaction of
interest, which therefore takes place in a highly parallel
fashion, in 1018–1020 independent nanoreactors. It readily
follows that these systems are extremely attractive for the
opportunity they disclose in achieving a precise control on
the products particle size, since the volume of reaction is
limited to the droplet’s core.
4.2 Application of the miniemulsions approach
to the room temperature synthesis of inorganic
nanostructures
The possibility of generating small, homogenous and sta-
ble monomer droplets that maintain their particular identity
Fig. 3 Homogenisation process in the miniemulsion approach (adapted from [119])
Fig. 4 Schematic
representation of the chemical
processes that can be used for
the synthesis of inorganic
materials via miniemulsion
(adapted from [117])
598 J Sol-Gel Sci Technol (2015) 73:591–604
123
throughout the polymerisation process without any
exchange kinetics involved represents the Holy Grail in
polymer synthesis, and it is indeed in this field that mini-
emulsions were originally developed [118, 119, 122, 123]
and were they find their main applications.
The use of miniemulsion for the direct synthesis of
inorganic materials, on the other hand, is less intensively
explored; nevertheless, it is gaining a growing interest in
the last years [5, 117, 124]. In this regard, a further
advantage in using miniemulsions is their flexibility, since
a wide variety of chemical processes can be exploited in
order to induce the formation of the desired material, as
depicted in Fig. 4.
Some of the first examples found in the literature for the
synthesis of inorganic compounds took advantage of low
melting metals, alloys or salts in order to produce stable
metallic (Wood’s and Rose’s alloys) and inorganic (Fe2O3,
Fe3O4, ZrO2 and CaCO3) nanoparticles. This was achieved
by using the molten precursors as polar phase and inducing
crystallisation by decreasing the temperature below the
melting point, thus exploiting phase transitions [125].
Another widely exploited process, especially for the
preparation of oxide materials, is the sol–gel approach, as
also reviewed by Munoz-Espı et al. and Cao et al. [117,
124]. The popularity of this approach can be traced back to
the high tunability it allows since, by controlling hydrolysis
and condensation rates, the morphology of the nanostruc-
tures can be easily modified, with also the possibility of
introducing further structure-directing agents [126–129].
Through this approach, a variety of different crystalline
materials were prepared, such as mesoporous silica nano-
particles [126], titania and mixed titania/silica and titania/
zirconia nano- [127, 128] and microparticles [129], and
ceria [130] nanoparticles.
In addition, due to its characteristics, the sol–gel process
can be induced to occur at the liquid–liquid interface in the
miniemulsion formulation, generating hollow nanostruc-
tures. This approach was for example exploited for the
synthesis of silica nanocapsules [131], as well as for the
interfacial precipitation of hafnium and zirconium
hydroxides which, upon calcination, maintained their hol-
low morphology and converted in the corresponding oxides
[132].
A further way to influence the morphology of the inor-
ganic materials is using miniemulsion generated polymer
latexes as templates. By tuning not only the dimension of
the latexes, but also their surface functionalities, the
polymer/inorganic interaction can be modified, influencing
the crystallisation process. For further details see refer-
ences [5, 117, 133].
Miniemulsions can also be exploited to generate hybrid
polymer/inorganic nanoparticles that act as precursor and
convert into the desired inorganic material after removal of
the organic component. Through this kind of approach,
either coatings [134] or ordered arrays of metallic nano-
particles [135, 136] might be obtained.
Another common approach for the preparation of inor-
ganic nanostructures exploits precipitation reactions of
metal salts within the droplets core. Among the first
examples in this framework, there is the preparation of
highly stable lanthanide-based phosphors [(Y0.94Eu0.06)2O3,
La0.5Ce0.3Tb0.2PO4, Ba0.9Eu0.1MgAl10O17], which could
also be easily converted to corresponding films [137].
4.3 Synthesis of pure and doped ZnO nanostructures
and of Au/TiO2 nanocomposites by miniemulsion
In this latter framework, i.e. precipitation in confined
space, in recent years we took advantage of these systems
for the controlled preparation of different inorganic nano-
structures, ranging from doped zinc oxide platelets [138,
139] to doped zinc sulphide [140], calcium fluoride [141],
calcium and magnesium hydroxides nanostructures (Table
4 in the ESI) [142], as well as Au/TiO2 nanocomposites
[143].
With the objective of developing materials for optical
bioimaging, the synthesis of ZnO nanostructures was car-
ried out using several surfactants, in order to assess their
influence on miniemulsion stability and final features of the
obtained materials. As expected, non-ionic bulky surfac-
tants performed better in stabilising an inverse miniemul-
sion, thus leading to the formation of nanocrystalline
wurtzite already at room temperature [138, 139]. The
approach used to induce the precipitation of the crystalline
materials was based on the preparation and successive
mixing of two different miniemulsion formulations con-
taining, as the aqueous phase, aqueous solution of the zinc
salt and of a precipitating agent respectively, as depicted in
Scheme 2. The method was then extended to the synthesis,
by coprecipitation, of doped ZnO nanoplatelets (Zn/
M = 50:1 or 20:1; M = AgI, CoII, CuII, EuIII, MgII, MnII)
(Table 5 in the ESI), achieving a very good reproducibility
[138]. The obtained anisotropic nanostructures presented
an average length of ca. 70 nm and thickness of 15 nm; in
particular those with EuIII, showed interesting luminescent
properties (Fig. 5a). Due to the aforementioned lumines-
cence, coupled with the low cytotoxicity of the host matrix,
also assessed in this work, these materials are appealing for
possible future applications in optical bioimaging. Corre-
spondingly, Lactate Dehydrogenase assays were per-
formed, proving that the nanostructures did not induce any
cytotoxic effect on human fibroblast MRC5 cell line. When
the wurtzite platelets were doped with silver ions, the
dopant easily underwent photoreduction, generating an Ag/
ZnO nanocomposite (Fig. 5b). XPS and ICP-AES analyses
allowed to gain insight into the composition of the
J Sol-Gel Sci Technol (2015) 73:591–604 599
123
samples’ surface and assessing the efficiency of the doping
process, highlighting a successful embedding of the ions in
the host matrix.
Due to the high versatility of miniemulsions in terms of
the chemical processes that can take place within their core
(Fig. 4), we also exploited such systems to achieve con-
trolled photodecomposition of a suitable tailored precursor
[144]. Specifically, we used the single-source precursor
AuCl4(NH4)7[Ti2(O2)2(Hcit)(cit)]2�12H2O (Fig. 6), which,
upon UV irradiation, is known to generate the nanocom-
posite Au/TiO2 [143].
This nanocomposite was investigated as photocatalyst in
the oxidation of 2-propanol. By taking advantage of its
properties in combination with the features of miniemul-
sion, a heterogeneous system of nanocrystalline gold
nanoparticles finely dispersed on titania could be easily
obtained (Fig. 7). Due to the chosen photo-triggered
decomposition method [144], gold formed metallic nano-
particles with an average size of 25–40 nm, whereas titania
formed as an amorphous support. XPS analyses evidenced
that almost complete conversion of the precursor into the
nanocomposite could be accomplished with appropriate
irradiation time.
The strong influence of the confinement process induced
by miniemulsion on the final materials was also evidenced
by the catalytic studies. A nanocomposite prepared in
miniemulsion was compared to a sample prepared in sim-
ple water suspension with regard to the catalysis of the
oxidation of 2-propanol. Tests in both gaseous and liquid
phase oxidation evidenced that the former sample is both
mixing A + B
US US
separation, centrifugation
post-functionalisation
characterisation of the suspension
chemical-physical characterisation
cytoxicity assessment
in vivo in vitro testing
metal precursor solution base solution
miniemulsion A miniemulsion B
microwaves
oxide miniemulsion
isolated nanoparticles
bioconjugated nanoparticles
US = ultrasound
US
Scheme 2 Flow chart for the
preparation of inorganic
bioconjugated nanoparticles via
miniemulsion
100 nm
(a) (b)
Fig. 5 (a) PL spectra of Eu doped ZnO nanostructures obtained via miniemulsion; (b) TEM micrograph of Ag/ZnO nanocomposite (adapted
from [138])
600 J Sol-Gel Sci Technol (2015) 73:591–604
123
more active and selective than its counterpart, as evidenced
in Table 3.
We have recently implemented the miniemulsion
approach for the preparation of pure and doped Mg(OH)2,
Ca(OH)2 [142], CaF2 [141], CuS and ZnS [140] nanopar-
ticles and nanostructures. In the case of the halogenide, the
precipitating agent was NaF whereas, in the case of the
sulphides, different sulphide sources were tested in order to
optimise the purity and crystallinity of the obtained
products.
Fig. 6 Crystal structure of the molecular Au/TiO2 single-source precursor AuCl4(NH4)7[Ti2(O2)2(Hcit)(cit)]2�12H2O
Fig. 7 SEM micrograph of Au/TiO2 nanocomposites obtained by
miniemulsion
Table 3 Catalytic tests (oxidation of 2-propanol) of Au/TiO2 nano-
composites prepared in miniemulsion or in suspension
Synthetic route Gaseous phase oxidation Liquid phase
oxidation
Conversion
(%)
Selectivity
(%)
TOF
(mol mg(Cat)-1 h-1)
Miniemulsion 98 80 0.012
Suspension 53 50 0.06
Table 4 Summary of the prepared systems
Compound Synthesis approach References
ZnO Colloidal route [15]
CuS Colloidal route [13]
CoFe2O4 Hydrothermal [106]
MnFe2O4 Hydrothermal [106]
NiFe2O4 Hydrothermal [106]
ZnFe2O4 Hydrothermal [106]
ZnO (pure and doped) Miniemulsion [138, 139]
Au/TiO2 Miniemulsion [143]
ZnS Miniemulsion [140]
CuS Miniemulsion [140]
CaF2 Miniemulsion [141]
Mg(OH)2 Miniemulsion [142]
Ca(OH)2 Miniemulsion [142]
J Sol-Gel Sci Technol (2015) 73:591–604 601
123
In conclusion, droplets formed by miniemulsion showed
to be effective nanoreactors for the controlled preparation
of several inorganic compounds, affording in all cases
crystallisation at room temperature and the formation of
nanosized structures.
5 Conclusions and perspectives
In this paper we have collected the most relevant examples
of our recent activity in the field of low or room temper-
ature synthesis of inorganic colloids. Different wet-chem-
istry approaches were successful in delivering the targeted
systems with desired microstructural and compositional
features. In all cases, the crystallisation of the targeted
nanostructures was pursued at low or room temperature,
and the experimental conditions proved to be determinant
in these cases.
For instance, in the case of miniemulsion, Landfester
and coworkers [5, 114–117, 120, 121] have already pointed
out interesting effects of the confined space on the fate and
structural evolution of the contained inorganic systems. In
particular, the morphosynthetical control of the crystalline
habitus of the formed structures was highlighted: physical
properties of liquids in nanodroplets can be substantially
different from those of the bulk phase and the dynamics of
crystallisation.
In one of our cases, for instance, [139] the confinement
of the precursor formulation in a droplet was proven to be a
key issue in determining the formation of wurtzite instead
of the expected (in the adopted pH range) zinc hydroxide.
In fact, in basic or neutral media (in our case the pH of the
final miniemulsion was determined to be 13.4), ZnII ions
form the amphoteric hydroxide species, ZnOx(OH)g(H2O)z
in a colloidal state, which forms as amorphous or crystal-
line species. This species spontaneously evolves to crys-
talline wurtzite ZnO not only under the action of heating or
irradiation, through a dehydration process, but also upon
prolonged storing and aging in its mother liquor, which in
this case was pursued by their confinement.
Table 4 summarises these efforts by including also the
relevant references.
The very encouraging results achieved have disclosed
several exciting perspectives, and may stimulate many
developments in this field, deriving mainly from:
1. optimisation of the reaction conditions and/or of the
stability of the obtained colloidal systems;
2. implementation of the optimised procedures to differ-
ent chemical systems and complex hierarchical
nanostructures;
3. combination of synthesis and processing methods (e.g.
solvothermal synthesis combined with microwaves
processing, microwaves-triggered decomposition of
single-source precursors in colloidal suspension etc.).
A very fascinating and challenging development in this
field we are now exploring is to establish clear correlations
between the chemico-physical parameters determining the
composition and stability of the colloidal systems and the
observed features (structural, compositional and morpho-
logical) as well as the crystallisation kinetics and
mechanisms.
Colloidal chemistry represents a really bewitching
playground for an inorganic chemist, and surely deserves
further and focussed experimental and theoretical efforts,
for better understanding of structure-properties relation-
ships and of non-classical crystallisation paths.
Acknowledgments The Italian National Research Council (CNR),
the University of Padua, Italy, and the Sabic company are acknowl-
edged for equipment and financial support. S.G. would like to warmly
thank her former master and PhD students Erika Butturini, Daniele
Camozzo, Alessia Famengo, Francesca Latini, Giulia Morgese and
the guest students Julia Migenda, Benjamin Kruner, Antonin Mam-
brini for their valuable contributions to the hereby presented work and
all the colleagues cited in the given references for their appreciated
support in the characterisation of the obtained nanostructures. P.D.
and S.D. acknowledge the PhD School in Molecular Sciences of the
University of Padova for financial support.
References
1. Dahl JA, Maddux BLS, Hutchison JE (2007) Chem Rev
107:2228–2269
2. Cushing BL, Kolesnichenko VL, O’Connor CJ (2004) Chem
Rev 104:3893–3946
3. Critical raw materials for the EU (2010). European Commission.
http://ec.europa.eu/enterprise/policies/rawmaterials/index_en.htm
4. Report on critical raw materials for the EU (May 2014). Euro-
pean Commission. http://ec.europa.eu/enterprise/policies/raw-
materials/critical/index_en.htm
5. Munoz-Espı R, Mastai Y, Gross S, Landfester K (2013) Cryst
Eng Comm 15:2175–2191
6. Brinker C, Scherer G (1990) Sol–gel science: the physics and
chemistry of sol–gel processing. Academic Press, New York
7. Cosgrove T (2010) Colloid science: principles, methods and
applications. Wiley, Hoboken
8. Armelao L, Barreca D, Bottaro G, Gasparotto A, Gross S, Mar-
agno C, Tondello E (2006) Coord Chem Rev 250:1294–1314
9. Armelao L, Bertoncello R, Cattaruzza E, Gialanella S, Gross S,
Mattei G, Mazzoldi P, Tondello E (2002) J Mater Chem
12:2401–2407
10. Armelao L, Colombo P, Fabrizio M, Gross S, Tondello E (1999)
J Mater Chem 9:2893–2898
11. Armelao L, Fabrizio M, Gross S, Martucci A, Tondello E (2000)
J Mater Chem 10:1147–1150
12. Dell’Amico BD, Bertagnolli H, Calderazzo F, D’Arienzo M,
Gross S, Rancan M, Scotti R, Smarsly B, Supplit R, Tondello E,
Wendel E (2009) Chem Eur J 15:4931–4943
13. Armelao L, Camozzo D, Gross S, Tondello E (2006) J Nanosci
Nanotechnol 6:401–408
602 J Sol-Gel Sci Technol (2015) 73:591–604
123
14. Krishnan V, Camozzo D, Armelao L, Bertagnolli H, Tondello E,
Gross S (2008) Z Phys Chem 222:655–669
15. Famengo A, Anantharaman S, Ischia G, Causin V, Natile MM,
Maccato C, Tondello E, Bertagnolli H, Gross S (2009) Eur J
Inorg Chem 2009:5017–5028
16. Morkoc H, Ozgur U (2008) Zinc Oxide: materials preparation,
properties, and devices. Wiley VCH, Weinheim
17. Wang ZL (2004) Mater Today 7:26–33
18. Liu Y, Tong Y (2008) J Nanosci Nanotechnol 8:1101–1109
19. Ellmer K, Klein A (2008) ZnO and Its Applications. In: Ellmer
K, Klein A, Rech B (eds) Transparent Conductive Zinc Oxide,
vol 104. Springer Series in Materials Science, vol 104. Springer,
Berlin
20. Klingshirn C (2007) ChemPhysChem 8:782–803
21. Klingshirn C, Hauschild R, Priller H, Decker M, Zeller J, Kalt H
(2005) Superlattice Microst 38:209–222
22. Fan Z, Lu JG (2005) J Nanosci Nanotechnol 5:1561–1573
23. Ozgur U, Alivov YI, Liu C, Teke A, Reshchikov MA, Dogan S,
Avrutin V, Cho S-J, Morkoc H (2005) J Appl Phys 98:1–103
24. Pearton SJ, Norton DP, Ip K, Heo YW, Steiner T (2005) Prog
Mater Sci 50:293–340
25. Lu Y, Zhong J (2004) Zinc oxide-based nanostructures. In:
Steiner T (ed) Semiconductor nanostructures for optoelectronic
applications. Artech House Publishers, Norwood
26. Wang ZL (2004) J Phys: Condens Matter 16:R829–R858
27. Look DC (2001) Mater Sci Eng B Solid 80:383–387
28. Kwon SG, Hyeon T (2008) Acc Chem Res 41:1696–1709
29. Weller H (2003) Philos T Roy Soc A 361:229–240
30. Loh K, Chua S (2007) Zinc Oxide Nanorod Arrays: Properties
and Hydrothermal Synthesis. In: Mansoori GA, George T,
Assoufid L, Zhang G (eds) Molecular Building Blocks for
Nanotechnology, vol 109. Topics in Applied Physics. Springer,
New York
31. Ehrentraut D, Sato H, Kagamitani Y, Sato H, Yoshikawa A,
Fukuda T (2006) Prog Cryst Growth Ch 52:280–335
32. Spanhel L (2006) J Sol Gel Sci Technol 39:7–24
33. Spanhel L, Anderson MA (1991) J Am Chem Soc
113:2826–2833
34. Bilecka I, Djerdj I, Niederberger M (2008) Chem Commun
2008:886–888
35. Niederberger M, Garnweitner G (2006) Chem Eur J
12:7282–7302
36. Buha J, Djerdj I, Niederberger M (2006) Cryst Growth Des
7:113–116
37. Pinna N, Garnweitner G, Antonietti M, Niederberger M (2005) J
Am Chem Soc 127:5608–5612
38. Clavel G, Willinger MG, Zitoun D, Pinna N (2007) Adv Funct
Mater 17:3159–3169
39. Pinna N, Grancharov S, Beato P, Bonville P, Antonietti M,
Niederberger M (2005) Chem Mater 17:3044–3049
40. Park T-J, Wong SS (2006) Chem Mater 18:5289–5295
41. Zhou H, Wong SS (2008) ACS Nano 2:944–958
42. Bahnemann DW, Kormann C, Hoffmann MR (1987) J Phys
Chem 91:3789–3798
43. Raevskaya AE, Stroyuk AL, Kuchmii SY, Kryukov AI (2004) J
Mol Catal A: Chem 212:259–265
44. Nascu C, Pop I, Ionescu V, Indrea E, Bratu I (1997) Mater Lett
32:73–77
45. Di Benedetto F, Borgheresi M, Caneschi A, Chastanet G, Ci-
priani C, Gatteschi D, Pratesi G, Romanelli M, Sessoli R (2006)
Eur J Mineral 18:283–287
46. Goel S, Chen F, Cai W (2014) Small 10:631–645
47. Grozdanov I, Najdoski M (1995) J Solid State Chem
114:469–475
48. Grijalva H, Inoue M, Boggavarapu S, Calvert P (1996) J Mater
Chem 6:1157–1160
49. Hu H, Campos J, Nair PK (1996) J Mater Res 11:739–745
50. Hu H, Gomez-Daza O, Banos L (1998) Sol Energ Mat Sol C
56:57–65
51. Yamamoto T, Kubota E, Taniguchi A, Dev S, Tanaka K,
Osakada K, Sumita M (1992) Chem Mater 4:570–576
52. Jache B, Mogwitz B, Klein F, Adelhelm P (2014) J. Power
Sources 247:703–711
53. Basu M, Sinha AK, Pradhan M, Sarkar S, Negishi Y, Govind,
Pal T (2010) Environ Sci Technol 44:6313–6318
54. Zhang H-J, Zhang Z-Z, Guo F, Jiang W, Wang K (2010) J
Compos Mater 44:2461–2472
55. Tseng Y-H, He Y, Lakshmanan S, Yang C, Chen W, Que L
(2012) Nanotechnology 23:455708
56. Tseng Y-H, He Y, Que L (2013) Analyst 138:3053–3057
57. Dutta AK, Das S, Samanta S, Samanta PK, Adhikary B, Biswas
P (2013) Talanta 107:361–367
58. Wan SM, Guo F, Peng YY, Shi L, Qian YT (2004) Chem Lett
33:1068–1069
59. Jiang C, Zhang W, Zou G, Xu L, Yu W, Qian Y (2005) Mater
Lett 59:1008–1011
60. Zhang YC, Qiao T (2004) Ya Hu X. J Cryst Growth 268:64–70
61. Zhang YC, Hu XY, Qiao T (2004) Solid State Commun
132:779–782
62. Wang CR, Tang KB, Yang Q, Bin H, Shen GZ, Qian YT (2001).
Chem Lett 30:494–495
63. Kumar RV, Palchik O, Koltypin Y, Diamant Y, Gedanken A
(2002) Ultrason Sonochem 9:65–7064. Wang H, Zhang J-R, Zhao X-N, Xu S, Zhu J-J (2002) Mater Lett
55:253–258
65. Tolia J, Chakraborty M, Murthy ZVP (2012) Cryst Res Technol
47:909–916
66. Biswas S, Hait SK, Bhattacharya SC, Moulik SP (2005) J Dis-
pers Sci Technol 25:801–816
67. Gao L, Wang E, Lian S, Kang Z, Lan Y, Wu D (2004) Solid
State Commun 130:309–312
68. Jiang X, Xie Y, Lu J, He W, Zhu L, Qian Y (2000) J Mater
Chem 10:2193–2196
69. Nafees M, Ali S, Rasheed K, Idrees S (2012) Appl Nanosci
2:157–162
70. Thongtem T, Phuruangrat A, Thongtem S (2007) J Mater Sci
42:9316–9323
71. Zhu L, Xie Y, Zheng X, Liu X, Zhou G (2004) J Cryst Growth
260:494–499
72. Sugimoto T, Chen S, Muramatsu A (1998) Colloid Surf A
135:207–226
73. Xue P, Lu R, Li D, Jin M, Tan C, Bao C, Wang Z, Zhao Y
(2004) Langmuir 20:11234–11239
74. Byrappa K, Yoshimura M (2001) Handbook of hydrothermal
technology. Noyes Publications, Park Ridge
75. Rickard DT, Wickman FE (1981) Chemistry and geochemistry of
solutions at high temperature and pressure. Pergamon, New York
76. Labachev AN (1971) Hydrodrothermal synthesis of crystals.
Nauka, Moscow
77. Labachev AN (1973) Crystallization processes under hydro-
thermal conditions. Consultants Bureau, New York
78. Kuzumina IP, Khaidukov NM (1977) Crystal growth from high
temperature aqueous solutions. Nauka, Moscow
79. Kuznestov VA (1973) Sov Phys Crystallogr 17:775–804
80. Laudise RA (1987) Hydrothermal crystal growth—some recent
results. In: Dryburgh PM, Cockayne B, Barraclough KG (eds)
Advanced crystal growth. Prentice Hall, New York
81. Baruah S, Dutta J (2009) Sci Technol Adv Mater 10:013001
82. Guo Z, Chen X, Li J, Liu J-H, Huang X-J (2011) Langmuir
27:6193–6200
83. Wang J, Zhang T, Wang D, Pan R, Wang Q, Xia H (2013) J
Alloy Compd 551:82–87
J Sol-Gel Sci Technol (2015) 73:591–604 603
123
84. Zheng Y, Shi E, Cui S, Li W, Hu X (2000) J Am Ceram Soc
83:2634–2636
85. Liu J, Wei A, Ge Z, Zhao W (2013) J Mater Sci 24:542–547
86. Hirano M, Kato E (1999) J Am Ceram Soc 82:786–788
87. Mai H-X, Sun L-D, Zhang Y-W, Si R, Feng W, Zhang H-P, Liu
H-C, Yan C-H (2005) J Phys Chem B 109:24380–24385
88. Liu S, Lu X, Xie J, Cao G, Zhu T, Zhao X (2013) ACS Appl
Mater Interface 5:1588–1595
89. Zhang H, Wei B, Zhu L, Yu J, Sun W, Xu L (2013) Appl Surf
Sci 270:133–138
90. Modeshia DR, Walton RI (2010) Chem Soc Rev 39:4303–4325
91. Bacha E, Deniard P, Richard-Plouet M, Brohan L, Gundel HW
(2011) Thin Solid Films 519:5816–5819
92. Li R-J, Wei W-X, Hai J-L, Gao L-X, Gao Z-W, Fan Y-Y (2013)
J Alloy Compd 574:212–216
93. Weiß O, Ihlein G, Schuth F (2000) Micropor Mesopor Mater
35–36:617–620
94. Wei J, Zhang C, Xu Z (2012) Mater Res Bull 47:3513–3517
95. Goh SC, Chia CH, Zakaria S, Yusoff M, Haw CY, Ahmadi S,
Huang NM, Lim HN (2010) Mater Chem Phys 120:31–35
96. Chen L, Shen Y, Bai J (2009) Mater Lett 63:1099–1101
97. Zhang G-Y, Sun Y-Q, Gao D-Z, Xu Y-Y (2010) Mater Res Bull
45:755–760
98. Gyergyek S, Drofenik M, Makovec D (2012) Mater Chem Phys
133:515–522
99. Zhou J, Ma J, Sun C, Xie L, Zhao Z, Tian H, Wang Y, Tao J,
Zhu X (2005) J Am Ceram Soc 88:3535–3537
100. Schubert U, Husing N (2005) Synthesis of inorganic materials,
2nd edn. Wiley-VCH, Weinheim
101. Holden A, Singer P (1971) Crystals and crystal growing. Anchor
Books Doubleday & Company Inc., Garden City
102. Lide DR (2004) Handbook of chemistry and physics, 84th edn.
CRC Press, Boca Raton
103. Chen X, Fan H, Liu L (2005) J Cryst Growth 284:434–439
104. MacLaren I, Ponton CB (2000) J Eur Ceram Soc 20:1267–1275
105. NIST (2011) Thermophysical properties of water. NIST Stan-
dard Reference Data. http://webbook.nist.gov/cgi/fluid.cgi?ID=
C7732185&Action=Page
106. Diodati S, Pandolfo L, Gialanella S, Caneschi A, Gross S (2014)
Nano Res 7:1027–1042
107. Chen X, Tang Y, Fang L, Zhang H, Hu C, Zhou H (2012) J
Mater Sci Mater El 23:1500–1503
108. Chen Z, Hu J, Lu Z, He X (2011) Ceram Int 37:2359–2364
109. Diodati S (2013) Sintesi e caratterizzazione di ferriti nano-
strutturate (Synthesis and characterisation of nanostructured
ferrites). Ph.D. Thesis—Scuola di Dottorato in Scienze
Molecolari [Scienze Chimiche], University of Padova, Italy
110. Diodati S, Gross S (2013) Surf Sci Spectra 20:17–34
111. Diodati S, Nodari L, Natile MM, Caneschi A, de Julian Fern-
andez C, Hoffmann C, Kaskel S, Lieb A, Di Noto V, Mascotto
S, Saini R, Gross S (2014) Eur J Inorg Chem 2014:875–887
112. Diodati S, Nodari L, Natile MM, Russo U, Tondello E,
Lutterotti L, Gross S (2012) Dalton Trans 41:5517–5525
113. Rietveld HM (1969) J Appl Cryst 2:65–71
114. Landfester K, Antonietti M (2004) Miniemulsions for the con-
venient synthesis of organic and inorganic nanoparticles and
‘‘single molecule’’ applications in materials chemistry. In:
Caruso F (ed) Colloids and colloid assemblies: synthesis,
modification, organization and utilization of colloid particles.
Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim
115. Landfester K (2001) Adv Mater 13:765–768
116. Landfester K (2005) Eur Coatings J 12:20–25
117. Munoz-Espı R, Weiss CK, Landfester K (2012) Curr Opin
Colloid Interface Sci 17:212–224
118. Antonietti M, Landfester K (2002) Prog Polym Sci 27:689–757
119. Landfester K (2001) Macromol Rapid Commun 22:896–936
120. Landfester K (2003) Miniemulsions for nanoparticle synthesis.
In: Antonietti M (ed) Colloid chemistry II. Springer Berlin,
Heidelberg
121. Landfester K (2006) Ann Rev Mater Res 36:231–279
122. Bechthold N, Tiarks F, Willert M, Landfester K, Antonietti M
(2000) Macromol Symp 151:549–555
123. Landfester K, Willert M, Antonietti M (2000) Macromolecules
33:2370–2376
124. Cao Z, Ziener U (2013) Nanoscale 5:10093–10107
125. Willert M, Rothe R, Landfester K, Antonietti M (2001) Chem
Mater 13:4681–4685
126. Schiller R, Weiss CK, Geserick J, Husing N, Landfester K
(2009) Chem Mater 21:5088–5098
127. Schiller R, Weiss CK, Landfester K (2010) Nanotechnology
21:405603
128. Rossmanith R, Weiss CK, Geserick J, Husing N, Hormann U,
Kaiser U, Landfester K (2008) Chem Mater 20:5768–5780
129. Collins AM, Spickermann C, Mann S (2003) J Mater Chem
13:1112–1114
130. Nabih N, Schiller R, Lieberwirth I, Kockrick E, Frind R, Kaskel
S, Weiss CK, Landfester K (2011) Nanotechnology 22:135606
131. Peng B, Chen M, Zhou S, Wu L, Ma X (2008) J Colloid
Interface Sci 321:67–73
132. Hajir M, Dolcet P, Fischer V, Holzinger J, Landfester K,
Munoz-Espı R (2012) J Mater Chem 22:5622–5628
133. Ethirajan A, Landfester K (2010) Chem - Eur J 16:9398–9412
134. Munoz-Espı R, Dolcet P, Rossow T, Wagner M, Landfester K,
Crespy D (2011) ACS Appl Mater Interfaces 3:4292–4298
135. Manzke A, Pfahler C, Dubbers O, Plettl A, Ziemann P, Crespy
D, Schreiber E, Ziener U, Landfester K (2007) Adv Mater
19:1337–1341
136. Manzke A, Plettl A, Wiedwald U, Han L, Ziemann P, Schreiber
E, Ziener U, Vogel N, Weiss CK, Landfester K, Fauth K,
Biskupek J, Kaiser U (2012) Chem Mater 24:1048–1054
137. Taden A, Antonietti M, Heilig A, Landfester K (2004) Chem
Mater 16:5081–5087
138. Dolcet P, Latini F, Casarin M, Speghini A, Tondello E, Foss C,
Diodati S, Verin L, Motta A, Gross S (2013) Eur J Inorg Chem
2013:2291–2300
139. Dolcet P, Casarin M, Maccato C, Bovo L, Ischia G, Gialanella
S, Mancin F, Tondello E, Gross S (2012) J Mater Chem
22:1620–1626
140. Dolcet P, Maurizio C, Casarin M, Pandolfo L, Gialanella S,
Badocco D, Pastore P, Gross S, Eur J Inorg Chem (submitted)
141. Dolcet P, Mambrini A, Pedroni M, Speghini A, Gialanella S,
Casarin M, Gross S, RSC Adv (submitted)
142. Butturini E, Dolcet P, Casarin M, Speghini A, Pedroni M,
Benetti F, Motta A, Badocco D, Pastore P, Diodati S, Pandolfo
L, Gross S (2014) J Mater Chem B 2:6639–6651
143. Heutz NA, Dolcet P, Birkner A, Casarin M, Merz K, Gialanella
S, Gross S (2013) Nanoscale 5:10534–10541
144. Rohe M, Loffler E, Muhler M, Birkner A, Woll C, Merz K
(2008) Dalton Trans 864:6106–6109
604 J Sol-Gel Sci Technol (2015) 73:591–604
123