ORIGINAL PAPER
Nano Design of Alumina Supported Monometallic Catalysts:A Promising Way to Improve the Selective Hydrogenationof Poly-Unsaturated Hydrocarbons
Cecile Thomazeau • Tivadar Cseri • Laure Bisson •
Julie Aguilhon • Doan Pham Minh • Cedric Boissiere •
Olivier Durupthy • Clement Sanchez
Published online: 2 August 2012
� Springer Science+Business Media, LLC 2012
Abstract In the field of catalysis by metals, a new insight
for the nanodesign of supported heterogeneous catalysts is
the tailoring of metallic nanoparticles. In this work, well-
faceted monometallic nanoparticles (Pd, Pt, Ni) exposing
mostly the {111} crystallographic facet are obtained in
aqueous solution and are deposited on an alumina support.
The involved mechanisms of nanoparticles formation are
determined and are evidenced to be different as a function
of the nature of the metal. In the case of palladium the
mechanism consists in an oriented attachment of palladium
nanoparticles leading to the energetically most favourable
stacking of nanoparticles, at the origin of the early differ-
entiation of the nanoparticles shapes and of the formation
of the well-faceted palladium nanoparticles. In the case of
platinum, the mechanism seems to be a combination of
aggregation of already reduced nuclei and direct reduction
depending on the experimental conditions. In the case of
the less reductible metal, nickel, well-faceted nanoparticles
are not obtained during the synthesis and only a thermal
activation under hydrogen can engender their formation.
The impact of the {111} crystallographic facet for platinum
and nickel is very important and induces a drastic increase
of selectivity towards olefins formation with a selectivity
close to the one of a palladium catalyst which is the most
selective metal for the selective hydrogenation of poly-
unsaturated hydrocarbons.
Keywords Metallic nanoparticles � Synthesis �Aqueous solution � Morphology � Catalysis �Selective hydrogenation � Selectivity
1 Introduction
In the field of hydrogenation reactions, selective hydroge-
nations are essential and widely used in refining (petroleum
cuts purification) and petrochemistry (production of inter-
mediates for chemical or polymers applications). The main
aim of these reactions is to convert the most unsaturated
hydrocarbons (alkynes, dienes), especially at high conver-
sion level, into the corresponding olefins (the high added
value desired product, with drastic specifications required),
thus avoiding a complete hydrogenation and formation of
the saturated hydrocarbons. The most active and selective
metals used for selective hydrogenations are palladium,
platinum and nickel. Industrial catalysts are usually sup-
ported on alumina with 0.1–0.5 wt% of metal for noble
metals, and with 5–18 wt % of metal in the case of nickel
[1].
C. Thomazeau (&) � T. Cseri � L. Bisson � J. Aguilhon �D. Pham Minh
IFP Energies nouvelles, Rond-point de l’echangeur de Solaize,
BP 3, 69360 Solaize, France
e-mail: [email protected]
L. Bisson � J. Aguilhon � C. Boissiere � O. Durupthy �C. Sanchez
Chimie de la Matiere Condensee de Paris, College de France,
UPMC, Universite Paris VI, UMR 7574, 11 Place Marcelin
Berthelot, 75231 Paris Cedex 05, France
L. Bisson � J. Aguilhon � C. Boissiere � O. Durupthy �C. Sanchez
Chimie de la Matiere Condensee de Paris, College de France,
CNRS, UMR 7574, 11 Place Marcelin Berthelot, 75231 Paris
Cedex 05, France
L. Bisson � J. Aguilhon � C. Boissiere � O. Durupthy �C. Sanchez
College de France, Chaire des Materiaux Hybrides, 11 place
Marcelin Berthelot, 75231 Paris Cedex 05, France
123
Top Catal (2012) 55:690–699
DOI 10.1007/s11244-012-9868-1
In the case of the supported metallic nanoparticles, a
high proportion of exposed atoms is often the key property
to improve catalytic activities. Consequently, catalysis
research efforts were until today essentially focused on
dispersion and particles size effects studies [2] for structure
sensitive reactions such as selective hydrogenation. Con-
ventional selective metallic catalysts used for selective
hydrogenations are made of supported nanoparticles with a
relatively isotropic shape usually represented by a trun-
cated cuboctahedron (Fig. 1e) [3]. These nanoparticles
present several different active sites: {111} and {100}
facets, corners and edges, each one with different catalytic
properties. Indeed, the strong dependence of reactants
adsorption, their activation, and products desorption as a
function of the metallic surface coordination was already
shown on single crystals [4–6], and is now extended to
supported nanoparticles [7]. The improvement of supported
metallic catalysts is now possible by the use of nanopar-
ticles with particular shapes (rods, cubes, tetrahedra…)
(Fig. 1a–d). Indeed, their highly symmetric shapes induce a
precise control of their surface structure: type and amount
of exposed crystallographic planes, proportion between
atoms on corners, edges or facets.
This growing interest for nanostructured metallic
nanoparticles had induced important research efforts and it
is now possible to tune both their size and shape [8]. It has
also recently been established, for a set of reactions, that
both activity and selectivity are highly dependent on the
morphology of nanoparticles and reactions conditions [9].
This approach had already been investigated for reactions
such as water gas shift [10], hydrogenolysis [11], oxidation
[12], reduction [13], and, in our scope of interest, hydro-
genation [14–21] reactions.
Syntheses of well-faceted metallic nanoparticules occur
in aqueous or polyol media and involve the reduction of a
metallic salt precursor using a reducing agent, in the
presence of a surface stabilizer. Since the crystalline
growth rate varies exponentially with the surface energy,
the selective adsorption of such structure-directing agents
induces a preferential stabilization of specific crystallo-
graphic faces and/or inhibits the growth of particles along a
given crystallographic direction [22–30] leading to a
preferential growth along another specific direction.
Recent advances concerning size and shape control of
metallic nanoparticles over nucleation and growth pro-
cesses have been achieved [31–33]. Among the different
methods of synthesis developed in aqueous medium for the
control of nanoparticles shapes, the seed-mediated meth-
ods, based on the decoupling of nucleation and growth
kinetics, are now successfully used for the synthesis of
well-faceted metallic nanoparticles [34–36].
Gold, silver [24, 37], palladium [17, 38] and platinum
[39–42] well-faceted nanoparticles were thus obtained
either with single or mixed morphologies. However,
mechanisms of their formation still remain unclear.
Although the thermodynamic stabilization of given facets
by a preferential adsorption of the capping agent is the
more usually proposed driving force for the growth control,
other parameters could also be critical to achieve the shape
control of the nanoparticle. In the case of gold, the auto-
organization of CTAB molecules in a horizontal bilayer at
the surface of the growing particle is supposed to explain
the uniaxial growth of gold nanorods through an electric
assisted mechanism of molecular growth [43, 44]. A stable
Au(I)-CTAB complex would be formed in solution and
reduced to metallic gold directly on the CTAB-embedded
metallic surfaces [45]. For other metals such as palladium,
platinum and nickel, the involved mechanisms of formation
of metallic nanoparticles with particular shapes seem to be
quite different, as reviewed in this work. Indeed, their
rationalization is of paramount importance for controlling
the formation of one selected type of morphology. The
formation of particles with a unique type of morphology is
essential to establish clear relationships between the nature
of selectively exposed sites and catalytic properties, thus
giving the opportunity to tune the activity and/or the
selectivity of a catalytic system for a given reaction.
In this work, we focus on specific syntheses developed
to obtain well-faceted metallic nanoparticules (Pd, Pt, Ni)
in aqueous medium and deposited on an alumina support,
and on the establishment of the involved mechanisms of
nanoparticles formation. Our aim is, thanks to a real
comprehension of these mechanisms, to obtain one type of
morphology exposing selectively one type of active site.
Then, structure–activity relationships observed for
the supported catalysts would be really accessible and
explained for the selective hydrogenation reaction of
unsaturated hydrocarbons.
ROD TETRAHEDRON CUBE
(100)(100)(111)
(b) (c)(a)[110]
(111)
(111)
POLYHEDRON
(d) (e)(111)
TRUNCATED CUBOCTAHEDRON
(100)
(111)
Fig. 1 Different morphologies and exposed facets observed for
metallic nanoparticles: a Rod, b Cube, c Tetrahedron, d Polyhedron,
e Truncated cuboctahedron
Top Catal (2012) 55:690–699 691
123
2 Experimental
2.1 Preparation of Supported Well-Faceted Metallic
Nanoparticles
Palladium nanoparticles were prepared according to the
following synthesis. First step: reduction of K2PdCl4(12.5 mL, 1 mM) by NaBH4 (3 mL, 0.01 M) in presence
of CTAB (cetyltrimethylammonium bromide, 25 mL,
0.15 M). Second step: stirring of K2PdCl4 (25 mL, 3 mM),
CTAB (25 mL, 0.24 M) and sodium ascorbate (1 mL,
0.08 M), and injection of 90 lL of the first step solution
under argon or hydrogen atmosphere.
Platinum nanoparticles were prepared according to the
following procedure. First step : formation of an aqueous
solution by mixing H2PtCl6 (18 mL, 3 mM) with CTAB
(37.5 mL, 7.5–90 mM) under argon or hydrogen at
323–343 K and one injection per minute of NaBH4
(0.3 mL, 12 mM). Second step: continuation of NaBH4
injections (0.3 mL, 12 mM), total injected volume:
4.5 mL.
Nickel nanoparticles were prepared according to the
following procedure. First step: formation of an aqueous
solution by mixing NiCl2 (40 mL, 16–32 mM) with CTAB
(250 mL, 45–150 mM) under argon atmosphere by a pro-
gressive addition of N2H4 (20 mL, 600–1,200 mM,
343 K). Second step: a reducing step performed at 683 K,
at ambient pressure, under H2 flux (1 l h-1 g-1) during
16 h of the impregnated alumina.
Alumina (d-Al2O3) was added to the different above
prepared solutions, and stirred during 2–10 h. After filtra-
tion, the solid was dried overnight at 303 K.
2.2 Transmission Electron Microscopy
Transmission electron microscopy experiments were per-
formed using a Philips TECNAI F20 apparatus operating at
an acceleration voltage of 200 kV. TEM images were
digitally recorded by a CCD camera. Solutions were
deposited on a perforated carbon film supported by a Cu
grid. The excess of surfactant was removed by rinsing the
grids with ethanol and consecutively drying them under an
IR light before analysis. The catalysts supported on
alumina were crushed in ethanol before deposition on
the grid.
The frequency distribution was defined by the percent-
age of each type of metallic nanoparticle of different
morphology (cubes, polyhedra, etc.) for a given synthesis
procedure. The yield of a type of morphology was calcu-
lated as follow:
Fið%Þ ¼ni
nT
with ni, the number of particles with a given morphology
and nT the number of particles used for the statistical
analysis (on at least two hundred nanoparticles).
2.3 Catalytic Measurements
The selectivity of the supported palladium and platinum
nanoparticles was evaluated for the selective hydrogena-
tion of buta-1,3-diene (model molecule used to represent
the selective hydrogenation of light hydrocarbons cuts such
as C3-propylene or C4-butenes cuts for which an
improvement of the catalysts selectivity is required for
petrochemical applications). With that model molecule,
formation of the intermediates butenes is expected selec-
tively without further hydrogenation towards butane
(Fig. 2). Buta-1,3-diene hydrogenation was performed in
liquid phase using a laboratory scale stainless-steel batch
reactor working under static conditions with variation of
the concentration of reactant and products over time.
Experimental conditions were previously optimized in
order to avoid mass transfer limitations. Buta-1,3-diene and
butenes are hydrogenated following zero order reaction
kinetics. One gram of palladium or platinum catalyst ini-
tially reduced during 2 h under H2 at 323 K was transferred
under Ar in a glove bag into the batch reactor filled with
n-heptane. The catalyst was then put into contact with buta-
1,3-diene at 293 K under 20 bars of H2 and high stirring
velocity. A pressure gauge before the batch reactor main-
tains the pressure constant inside the reactor at 20 bars of
H2. The course of the reaction was followed by the loss of
H2 pressure in the pressure gauge and by analysis of
samples by gas chromatography (plot alumina column
PONA, L = 50 m, split injector; FID detection). The
butenes selectivity is defined according to the following
equation.
*
But-1-ène *
But-2-ènes *
Butane *
k1
k2
k3
k6
k4 k5Buta-1,3-diène
H2
H2
H2
H2
buta-1,3-diene *
1-butene *
2-butenes *
butane **
But-1-ène *
But-2-ènes *
Butane *
k1
k2
k3
k6
k4 k5Buta-1,3-diène
H2
H2
H2
H2
buta-1,3-diene *
1-butene *
2-butenes *
butane *
* = adsorbed product
Fig. 2 Scheme of the selective hydrogenation of buta-1,3-diene
692 Top Catal (2012) 55:690–699
123
Butenes Selectivity ¼ %ðbutenesÞ%ðn� butaneÞ þ
P%ðbutenesÞ
Activity and selectivity of the supported nickel nano-
particles were evaluated for the selective styrene/isoprene
hydrogenation (mix of model molecules used to represent
the selective hydrogenation of a C5–C8 pyrolysis gasoline
cut for which an improvement of both activity and selec-
tivity is required for industrial applications). For this later
catalytic measurement, the interest is the selective hydro-
genation of isoprene towards the corresponding olefins, in
presence of aromatics for which the aim is the selective
hydrogenation of the exo-cyclic olefin, without further
hydrogenation of the aromatic ring. For selective styrene/
isoprene hydrogenation, the formation of olefins interme-
diates (methyl-1-butene, methyl-2-butenes), and ethyl-
benzene are expected without further hydrogenation to the
corresponding alkanes, and ethyl-cyclohexane (Fig. 3).
This reaction was also performed in liquid phase using a
laboratory scale stainless-steel and perfectly stirred batch
reactor. One gram of nickel catalyst initially reduced dur-
ing 16 h under H2 at 683 K was transferred under Ar in a
glove bag into the batch reactor filled with n-heptane. The
catalyst was then put into contact with a styrene/isoprene
solution at 343 K under 35 bars of H2. In this conditions
there is no hydrogenation of the aromatic ring. The rate of
the reaction was followed by the loss of H2 pressure in the
storage bottle. Activity and olefins selectivity are defined
according to the following equations :
Activity ðmol mn�1gðNiÞ�1Þ ¼ VolH2� DPH2
m�%wt Ni � 24
� �
With VolH2 is the H2 volume in the reactor (given in mL),
DPH2 corresponds to the H2 pressure variation over the
time unit (bar min-1), wt% Ni is the metal content of the
catalyst and m is the mass of catalyst (in grams).
Olefins Selectivity ¼ %ðolefinsÞ%ðalcanesÞ þ
P%ðolefinsÞ
3 Results and Discussion
The decoupling of nucleation (with the use of previously
prepared seeds) and growth steps, allows a better control of
each single step and thus leads to better defined morphol-
ogies. However, mechanisms that explain, for each metal,
the formation of a given nanoparticle morphology are far
from being completely known. The direct consequence is
that in most of the proposed syntheses in literature, a
mixture of morphologies (nanorods, nanocubes, nanopo-
lyhedra) is obtained. The study of the preparation of well-
faceted metallic nanoparticles of elements (Pd, Pt, Ni)
belonging to the same column of the periodic table may
give fruitful informations about the evolution of the reac-
tivity in aqueous solution and about the observed mecha-
nisms as function of the intrinsic parameters of these
elements.
3.1 Preparation of Well-Faceted Supported Metallic
Nanoparticles
3.1.1 Well-Faceted Palladium Nanoparticles [36]
During the first step, the fast chemical reduction of
K2PdCl4 palladium salt by sodium borohydride in the
presence of CTAB led to the formation of spherical
5–6 nm palladium seeds (when characterized after 2 h of
reaction). At the beginning of the second step, just after the
introduction of seeds in the growth solution, two distinct
populations of particles were observed: a 7–8 nm popula-
tion attributed to the growth of the initial seeds by
molecular reduction, and a 2–3 nm population assumed to
be nuclei resulting from a secondary homogeneous nucle-
ation process occurring when ascorbate was introduced.
After 5–10 min of reaction, the above described seeds
and nuclei tended to aggregate, leading to the formation of
intermediate particles. This early aggregation of nuclei and
seeds was oriented and stabilized by the adsorption of
CTAB. Considering the high CTAB concentration of the
solution, palladium nanoparticles were assumed to be
covered by a surfactant bilayer, allowing seeds and nuclei
rotation and circulation one on each other. A spontaneous
evolution of the aggregate shape is driven by the free
enthalpy minimization principle (which mechanism could
be described using a very simple geometrical model,
involving spheres stacking [36]). This oriented attachmentFig. 3 Scheme of the selective hydrogenation of isoprene and styrene
Top Catal (2012) 55:690–699 693
123
of seeds and nuclei was proposed to be responsible for the
early differentiation of the palladium nanoparticles shapes.
The different nanoparticles morphologies were found to be
triggered by the energetically most favourable stacking of
spheres. Indeed, the growth of these nanoparticles finally
led to the formation of secondary objects of non random
shapes (Fig. 4a) and to the well-faceted palladium nano-
particles (Fig. 4b) resulting from a dominant molecular
reduction when palladium concentration became too low to
promote homogeneous nucleation. At the end, a wide
variety of palladium nanoparticles with different mor-
phologies (rods, bipyramides, icosahedra, cubes) exposing
{100} and {111} facets was formed in the aqueous
solution.
Considering the known high interaction between CTAB
with the {100} crystallographic facet of palladium [27], it
was assumed that a destabilisation of this interaction could
indirectly have a strong impact on the morphology,
favouring the most stable palladium {111} surface forma-
tion in the absence of the {100} stabilisation by CTAB.
Thus, when argon was replaced by hydrogen bubbling, a
majority of different nanostructures was formed, all exposing
mainly the {111} crystallographic facet (octahedra, prims,
icosahedra). The proportion of {111} exposed crystallo-
graphic facet was above 90 %, as determined elsewhere by a
detailed MET characterization [46].
3.1.2 Well-Faceted Platinum Nanoparticles [68]
Concerning platinum nanoparticles, numerous syntheses
are reported in the literature, even in aqueous medium [13–
16], using strong reducing agents such as sodium borohy-
dride. Structured platinum nanoparticles such as cubes or
cuboctahedra [47–49] could be obtained. Nevertheless,
mechanisms of platinum nanoparticles formation are not
mentioned.
The method of synthesis developed for palladium was
extended to the case of platinum with slight modifications.
The starting aqueous solution prepared by mixing H2PtCl6with CTAB (7.5 mM) under argon at 50 �C contains a Pt
(?IV) precursor rather than a (?II) ion. Numerous
parameters were shown to be critical and had to be pre-
cisely controlled : (i) the nature of the surfactant, (ii) the
control of the hydroxylation of the platinum chloride pre-
cursor, (iii) the temperature and finally (iv) the control of
the reaction atmosphere (under argon or hydrogen).
For this optimized synthesis, during the first step, an
interaction between CTAB and the platinate precursor
could be supposed, leading to {Pt(?IV)-CTAB} moieties
formation, since CTAB probably forms micellar species
(its concentration in solution is higher than its critical
micellar concentration (0.8–1.1 mM) [50]). The Pt(?IV)
cation could thus be surrounded by different coordination
shells with chloride partially substituted by bromide and/or
hydroxide (the ageing of the solution is supposed to lead to
the partial or complete substitution of chloride ligands by
hydroxides ones [41, 42, 51]). The strong reducing agent,
NaBH4, was then injected. At the end of the first step,
spherical platinum nanoparticles of nearly 1–5 nm were
formed after 2 min of reducing agent injections. Theses
nanoparticles were either isolated one from each others or
formed aggregates with a size comprised between 10 and
20 nm.
During the second step, the injections of reducing agent
were maintained leading to the formation of well-faceted
platinum nanoparticles [almost 90 % of well-faceted plat-
inum nanoparticles were observed (Fig. 5)]. When higher
concentrations of CTAB were used (90 mM), platinum
nanoparticles were less faceted, and ill defined morpholo-
gies were preponderantly observed.
These observations led to a proposition of mechanism.
For low surfactant concentrations, well-faceted platinum
nanoparticles were obtained in a large proportion. A direct
molecular reduction of the platinum precursor onto the
growing nanoparticles and/or coalescence of the aggregatesFig. 4 Formation of well-faceted palladium nanoparticles by aggre-
gation after a reaction time of a: 20 min and b 3 h
694 Top Catal (2012) 55:690–699
123
(resulting from the previous aggregation step of the pri-
mary formed platinum nanoparticles) could be proposed as
preponderant. At higher CTAB concentrations, the direct
reduction of the platinum precursor onto the growing
platinum nanoparticles and/or the coalescence of the
aggregates should be disfavoured. As a result, the obtained
platinum nanoparticles were not well-faceted.
Moreover, as already discussed in the case of palladium,
the destabilisation of the CTAB interaction with the {100}
crystallographic plane could indirectly favour the most stable
platinum {111} surface. Thus, even for high CTAB con-
centrations (90 mM), replacing argon by hydrogen allowed
to obtain more than 96 % of well-faceted platinum nano-
particles with predominant {111} crystallographic facet.
3.1.3 Well-Faceted Nickel Nanoparticles
In the case of nickel, the formation of well-faceted nano-
particles is scarcely reported in aqueous solution probably
because of unwanted reoxidation reactions that are more
difficult to avoid with that element. That is why well
defined nickel metallic nanoparticles such as cubes, tetra-
hedra and rods are until now only obtained in organic
solvents [15, 52–56]. Nickel nanosheets could be prepared
either by direct reduction (hydrazine) of a nickel precursor
(nickel chloride) [57] or by an intermediate formation of
nickel hydroxide [58] and its further reduction. Nickel
hexagonal nanosheets exposing the {111} crystallographic
plane are synthesized, with conservation of the morphology
of the previously synthesized nickel hydroxide nanosheets.
Nickel nanoparticles with an urchin morphology are syn-
thesized by reduction of a nickel chloride precursor by
hydrazine in presence of a structure directing agent [59].
The method of synthesis developed in this work for
noble metals was thus finally extended to the case of nickel
with an impregnation of the solutions onto alumina. An
additional reduction at 683 K under H2 atmosphere was
mandatory to obtain nicely-faceted nanoparticles in
the 20–50 nm size range (Fig. 6). From the analysis
Fig. 5 2D-TEM characterization of each type of platinum nanoparticle in solution: a pseudo-cube; b cube; c polyhedron; d tetrahedron;
e cubooctahedron; f rod [68]
Fig. 6 Supported nickel nanoparticles on alumina
Top Catal (2012) 55:690–699 695
123
of frequencies and mean sizes of the different morpholo-
gies of nanoparticles observed by TEM (tetrahedra, ico-
sahedra, rods and decahedra), it appeared that all the
observed morphologies exposed mainly the {111} crys-
tallographic plane and that icosahedra were more often
observed.
The study of the mechanism of formation of these nickel
nanoparticles is still in progress but some elements of
comprehension could already be brought. First of all,
hydrazine (E(N2/N2H4) = -1.16 V/ENH [60]) was chosen
as it is a reductor stronger than NaBH4 (E(B(OH)3)/
BH4-) = -0.481 V/ENH) in order to reduce Ni(II) species
in solution (E(Ni2?/Ni) = -0.257 V/ENH) [61]. More-
over, the reduction had to be performed in basic medium
[62] and the temperature should be increased at 343 K to
kinetically activate the reduction [63]. The two other
drawbacks of NaBH4 are its propensity to decompose in
solution and its ability to form Ni2B species [64] for which
consequences onto catalytic properties are not well known.
Unfortunately, even hydrazine on nickel ratios up to 40 did
not permit to obtain metallic nickel nanoparticles. An
intermediate Ni(II) based structure with a strong interaction
with alumina was detected. This intermediate was charac-
terized as an hydrotalcite type layered structure involving
both Al(III) and Ni(II) cations. The well-faceted metallic
nickel nanoparticles were formed only during treatment
under hydrogen at 683 K, thus during a solid–gas process,
which generate the driving force at the origin of well-
faceted nickel nanoparticles formation.
3.1.4 Comparison of the Different Mechanisms of Well-
Faceted Nanoparticles Formation
When mechanisms of well-faceted metallic nanoparticles
formation are compared for gold, palladium, platinum and
nickel, it appears that they are different, depending on the
metal, and on its reductibility. Indeed, each of the studied
metals possess its own oxidation–reduction thermodynamic
potential [61]: E(Au?/Au) = 1.83 V/ENH, E(Pd2?/
Pd) = 0.83 V/ENH, E (Pt2?/Pt) = 1.2 V/ENH, E(Ni2?/
Ni) = -0.257 V/ENH. This will of course have conse-
quences on the choice of the reductor but no direct rela-
tionship between the oxidation–reduction thermodynamic
potential and mechanisms appears. This points out the fact
that kinetic factors must have to be taken into account and
are determinant for such kind of synthesis.
Direct reduction of a stable Au(I)-CTAB complex on the
CTAB-embedded metallic gold surfaces was proposed in
literature in the case of gold. The mechanism evidenced in
the case of palladium was different from that proposed for
gold, and consisted in an oriented attachment of palladium
nanoparticles leading to the energetically most favourable
stacking of nanoparticles, at the origin of the early
differentiation of the nanoparticles shapes and of the for-
mation of the well-faceted palladium nanoparticles.
Moreover, in the case of platinum, the mechanism seems to
be a combination of aggregation of already reduced nuclei
and direct reduction depending of the experimental con-
ditions. In the case of the less reductible metal, nickel, only
a supplementary reduction step allows the formation of the
well-faceted nickel nanoparticles.
Nevertherless, once the mechanism is understood for a
given metal, it becomes possible to favour the formation of
a given morphology, or of one type of exposed cristallo-
graphic facet, through the control and adjustment of the
experimental parameters. Thus, in the case of palladium
and platinum in solution and even in the case of nickel in a
solid–gas process, the formation of the {111} cristallo-
graphic facet is favoured with hydrogen addition and could
be explained considering a ‘‘surface cleaning’’ by hydrogen
[65]. An adsorption competition of both molecules would
happen in particular on {100} facets, causing their desta-
bilization relatively to {111} facets thus favouring the
{111} facet formation.
We thus obtained metallic nanoparticles with selectively
one type of exposed active site, mainly the {111} crystal-
lographic facet. Consequently, structure–activity relation-
ships could be established for these supported metallic
nanoparticles for the selective hydrogenation reaction of
unsaturated hydrocarbons.
3.2 Catalytic Properties of the Well-Faceted Supported
Metallic Nanoparticules
The supported palladium and platinum nanoparticles
exposing mainly the {111} crystallographic facet were
prepared by deposition of the colloidal solutions on alu-
mina with conservation of the morphologies obtained in
solution. The well-faceted supported nickel nanoparticles
were obtained after the above mentioned supplementary
reduction step. The as prepared catalysts are labelled as
MCat-{111} (M = Pd, Pt, Ni). For each metal, a refer-
ence catalyst, labelled MCat-Ref (M = Pd, Pt, Ni) was
prepared, using conventional well-known methods of syn-
thesis. For the MCat-Ref catalysts, metallic nanoparticles
have a relatively isotropic shape usually represented by a
truncated cuboctahedron [3], thus presenting several dif-
ferent active sites: {111} and {100} facets, corners and
edges. Characterizations, proportions in each type of
crystallographic facets and catalytic properties are reported
Table 1.
Palladium is intrinsically the most selective metal for
selective buta-1,3-diene hydrogenation towards butenes
formation, so a high selectivity is observed for high buta-
1,3-diene conversions, even for PdCat-Ref (olefins selec-
tivity of 96 %, Fig. 7). Nevertheless, thanks to the higher
696 Top Catal (2012) 55:690–699
123
amount of exposed {111} crystallographic plane of PdCat-
{111}, an even higher selectivity of 99 % is reached. This
improvement of selectivity, due to the preferential expo-
sition of the {111} actives sites confirms improvements of
selectivities already observed in literature for the same
reaction for single crystals [67] or for supported well fac-
eted palladium nanoparticles [21] in different experimental
conditions.
In the case of platinum nanoparticles, the influence of
morphology on catalytic properties was already evidenced
for the selective hydrogenation of benzene with a higher
selectivity showed by cubic platinum nanoparticles, thus
exposing mainly the {100} crystallographic facet, in
comparison with cuboctahedric nanoparticles [17]. For
selective hydrogenation of buta-1,3-diene, platinum is
intrinsically less selective than palladium. This is visible
through an olefins selectivity of around 70 % observed for
PtCat-Ref at 85 % conversion of buta-1,3-diene, Fig. 7. A
drastic increase of selectivity towards olefins formation is
observed for PtCat-{111} with a selectivity[90 % at 85 %
conversion of buta-1,3-diene. This could again be associ-
ated with the exposition of the {111} crystallographic
facet. So depending on the type of hydrogenation consid-
ered (aromatic in the literature or dienes in our work), the
nature of the most selective site is different. Moreover, the
impact of platinum nanoparticles morphology on selectiv-
ity is evidenced with a behaviour of the PtCat-{111} cat-
alyst close to that of palladium which is the most selective
metal for such selective hydrogenation reactions.
In the case of nickel, morphologic effects [66] on catalytic
properties are also expected. Indeed, nickel nanoparticles
with specific morphologies such as whiskers, were shown to
display higher activities for benzene hydrogenation when
compared to spherical ones [14]. The evaluation of their
activity in the selective hydrogenation of a representative
Styrene/Isoprene mixture shows a decrease of the activity for
NiCat-{111} (0.15 mol min-1 gNi-1) compared to NiCat-
Ref (2.56 mol min-1 gNi-1), Table 1. However, only one
part of this diminution could be attributed to the higher size
of the NiCat-{111} nanoparticules compared to the reference
catalyst. The following order of activity {111} \{100} \ {110} was already reported in literature for single
crystals [19, 67]. So, the lower activity observed for the
NiCat-{111} catalyst could obviously be explained as a
combination of a diminution of the number of active sites
expressing a lower activity. The evaluation of the NiCat-
{111} catalyst selectivity towards olefins also shows an
Table 1 Characterization and catalytic properties of the palladium, platinum and nickel well-faceted supported nanoparticles
Catalyst wt% (M) % {111} facetsa A (mol min-1 gNi-1) Olefins selectivity (%)b
(M = Pd, Pt, Ni)
PdCat-Ref 0.20 70 – 96
PdCat-{111} 0.19 [90 – 99
PtCat-Ref 0.30 70 – 70
PtCat-{111} 0.16 [96 – 90
NiCat-Ref 15.7 70 2.56 93
NiCat-{111} 8 [85 0.15 96
a The proportion in {111} crystallographic facets is deduced from shape frequencies determined from MET and estimated according to
geometric models presented Fig. 1b The selectivity towards olefins is reported at 85 % buta-1,3-diene conversion for Pd and Pt catalysts, and at 85 % isoprene conversion for Ni
catalysts
6065707580859095
100
20 30 40 50 60 70 80 90 100
Buta-1,3-diene conversion (%)
But
enes
Sel
ectiv
ity (%
)
PtCat-RefPtCat-{111}PdCat-RefPdCat-{111}
Pt
Fig. 7 Butenes selectivity observed for the selective hydrogenation
of buta-1,3-diene
80
85
90
95
100
70 75 80 85 90 95 100
Isoprene Conversion (%)
Ole
fins
Sel
ecti
vity
(%
)
NiCat-Ref
NiCat-{111}
Fig. 8 Olefins selectivity observed for the selective hydrogenation of
a styrene/isoprene mixture
Top Catal (2012) 55:690–699 697
123
improvement due to the {111} crystallographic facet
(Fig. 8). For an isoprene conversion of 85 %, the selectivity
of NiCat-Ref is 93 % while this selectivity increases sig-
nificantly until 96 % for NiCat-{111}.
Moreover, in the case of the platinum and nickel metals,
the improvement of selectivity towards olefins becomes
more and more important for the highest conversions of the
unsaturated hydrocarbon, i.e. in the range of industrial
interest for such reactions.
4 Conclusion
The growing interest for the control of metallic nanoparti-
cules shapes with applications in catalysis, is well illustrated
through many examples of the literature. Well-faceted and
defined nanoparticles can now be obtained through different
syntheses pathways. In this work, different syntheses in
aqueous solution were successfully developed for palladium,
platinum and nickel. Supported catalysts obtained after
deposition of well-faceted nanoparticles on alumina showed
very high selectivity for the hydrogenation of poly-unsatu-
rated compounds. The tailoring of the morphology of these
nanoparticles represents thus an improvement for the nano-
metric scale design of new catalysts generations. The choice
of the appropriate type of active metallic site can then be
done for each targeted reaction in order to obtain the best
catalytic properties.
References
1. Thomazeau C, Boyer C (2011) Tech Ing J5500
2. Boitiaux JP, Cosyns J, Vasudevan S (1983) Appl Catal A 6:41
3. Van Hardeveld R, Hartog F (1969) Surf Sci 15:189
4. Somorjai GA (1996) Chem Rev 96:1223
5. Henry CR (1998) Surf Sci Rep 31:231
6. Tourillon G, Cassuto A, Jugnet Y, Massardier J, Bertolini JC
(1996) J Chem Soc Faraday Trans 92:4835
7. Li Y, Liu Q, Shen W (2011) Dalton Trans 40:5811
8. Cheong S, Warr JD, Tilley RD (2010) Nanoscale 2:2045
9. Somorjai GA, Park PY (2008) Angew Chem Int Ed 47:9212
10. Saaski M, Osada M, Higashimoto N, Yamamoto T, Fukuoka A,
Ichikawa M (1999) J Mol Catal A 141:223
11. Fukuoka A, Higashimoto N, Sakamoto Y, Inagaki S, Fukushima
Y, Ichakawa M (2011) Microporous Mesoporous Mater 68:171
12. Chimentao RJ, Kirm I, Medina F, Rodriguez X, Cesteros Y,
Salagre P, Sueiras JE (2004) Chem Commun 7:846
13. Balint I, Miayazaki A, Aika K (2004) Phys Chem Chem Phys
6:2000
14. Boudjahem AG, Monteverdi S, Mercy M, Bettahar MM (2004)
Catal Lett 97:177
15. Telkar MM, Rode CV, Chaudhari RV, Joshi SS, Nalawade AM
(2004) Appl Catal A 273:11
16. Berhault G, Bisson L, Thomazeau C, Verdon C, Uzio D (2007)
Appl Catal A 327:32
17. Bratlie KM, Lee H, Komvopoulos K, Yang P, Somorjai GA
(2007) Nano Lett 7:3097
18. Silvestre-Albero J, Rupprechter G, Freund HJ (2006) J Catal
240:58
19. Silvestre-Albero J, Rupprechter G, Freund HJ (2005) J Catal
235:52
20. Silvestre-Albero J, Rupprechter G, Freund HJ (2006) Chem
Commun 1:80–82
21. Piccolo L, Valcarcel A, Bausach M, Thomazeau C, Uzio D,
Berhault G (2008) Phys Chem Chem Phys 10:5504
22. Johnson CJ, Dujardin E, Davis SA, Murphy CJ, Mann S (2002)
J Mater Chem 12:1765
23. Sau TK, Murphy CJ (2004) J Am Chem Soc 126:8648
24. Puntes VF, Krishnan KM, Alivisatos AP (2001) Science
291:2115
25. Gomez S, Erades L, Philippot K, Chaudret B, Colliere V, Balmes
O, Bovin JO (2001) Chem Commun 16:1474
26. Kim F, Connor S, Song H, Kuykendall T, Yang P (2004) Angew
Chem Int Ed 43:3673
27. Di Gregorio F, Bisson L, Armaroli T, Verdon C, Lemaitre L,
Thomazeau C (2009) Appl Catal A 352:50
28. Chen J, Herricks T, Geissler M, Xia Y (2004) J Am Chem Soc
126:10854
29. Sun Y, Xia Y (2002) Adv Mater 14:833
30. Giersig M, Pastoriza-Santos I, Liz-Marzan LM (2004) J Mater
Chem 14:607
31. Semagina N, Kiwi-Minsker L (2009) Catal Rev 51:147
32. Xia YN, Xiong XJ, Lim B, Skrabalak SE (2009) Angew Chem Int
Ed 48:60
33. Sau TK, Rogach AL (2019) Adv Mater 22:1781
34. Lim B, Jiang MJ, Tao J, Camargo PHC, Zhu YM, Xia YN (2009)
Adv Funct Mater 19:189
35. Perez-Juste J, Pastoriza-santos I, Liz-Marzan LM, Mulvaney P
(2005) Coord Chem Rev 249:1870
36. Bisson L, Boissiere C, Nicole L, Grosso D, Jolivet JP, Thoma-
zeau C, Uzio D, Berhault G, Sanchez C (2009) Chem Mater
21:2668
37. Jana NR, Gearheart L, Murphy CJ (2001) J Phys Chem B 105:
4065
38. Berhault G, Bausach M, Bisson L, Becerra L, Thomazeau C,
Uzio D (2007) J Phys Chem C 111:5915
39. Balint I, Miyazaki A, Aika K (2002) Appl Catal B 37:217
40. Ahmadi TS, Wang ZL, Green TC, Henglein A, El-Sayed MA
(1996) Science 272:1924
41. Henglein A, Ershov BG, Malow M (1995) J Phys Chem 99:14129
42. Henglein A, Giersing M (2000) J Phys Chem B 104:6767
43. Nikoobakht B, El-Sayed MA (2001) Langmuir 17:6368
44. Perez-Juste J, Liz-Marzan LM, Carnie S, Chan DYC, Mulvaney P
(2004) Adv Funct Mater 14:571
45. Grzelczak M, Perez-Juste J, Mulvaney P, Liz-Marzan LM (2008)
Chem Soc Rev 37:1783
46. Bisson L (2007) PhD, University Pierre Marie Curie
47. Zhao SY, Chen SH, Wang SY, Li DG, Ma HY (2002) Langmuir
18:3315
48. Veisz B, Toth L, Teschner D, Paal Z, Gyorffy N, Wild U, Schlogl
R (2005) J Mol Catal A 238:56
49. Lee H, Habas SE, Kweskin DB, Somorjai GA, Yang P (2006)
Angew Chem Int Ed 45:7824
50. Mukerjee P (1971) Critical Micelle Concentration of aqueous
surfactants systems NSRDS
51. Zhang F, Chen J, Zhang X, Gao W, Jin R, Guan N, Li Y (2004)
Langmuir 20:9329
52. Ely TO, Amiens C, Chaudret B, Snoeck E, Verelst M, Respaud
M, Broto JM (1999) Chem Mater 11:256
53. Cordente N, Respaud M, Senocq F, Casanove M (2001) Nano
Lett 1:565
698 Top Catal (2012) 55:690–699
123
54. Bradley JS, Tesche B, Busser W, Maase M, Reetz MTJ (2000)
J Am Chem Soc 122:4631
55. Leng Y, Li Y, Li X, Takahashi S (2007) J Phys Chem C 111:6630
56. Bai L (2009) J Cryst Growth 311:2474
57. Li J, Qin Y, Kou X, Huang J (2004) Nanotechnology 15:982
58. Xu R, Xie T, Zhao Y, Li Y (2007) J Cryst Growth 7:1904
59. Liu D, Wu H, Zhang Q, Wen LJ (2008) J Mater Sci 43:1974
60. Marecot P, Fakche A, Kellah B, Mabilon G, Prigent M, Barbier J
(1994) Appl Catal B 3:283
61. West RC (1983) Handbook of chemistry and physics, 64th edn.
CRC Press, Boca Raton
62. Park JW, Chae EH, Kim SH, Lee JH, Kim JW, Yoon SM, Choi
JY (2006) Mater Chem Phys 97:371
63. Li YD, Li LQ, Liao HW, Wang HR (1999) J Mater Chem 9:2675
64. Glavee GN, Klabunde KJ, Sorensen CM, Hadjipanayis GC
(1994) Langmuir 10:4726
65. Chaudret B (2006) Materials Congress
66. Grant J, Moyes RB, Oliver RG, Wells PB (1976) J Catal 42:213
67. Bertolini JC, Jugnet Y (2002) Chem Phys Solid Surf 10:404
68. Pham Minh D, Oudart Y, Baubet B, Verdon C, Thomazeau C
(2009) Oil Gas Sci Technol 64:697
Top Catal (2012) 55:690–699 699
123