Ceria-Based Solid Catalysts for Organic Chemistry
Laurence Vivier* and Daniel Duprez[a]
654 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
Ceria is a negative semiconductor oxide in which oxygen va-
cancies can be created at high temperatures in vacuum or in
an inert gas [Equation (1)], or at moderate temperatures in the
presence of a reductor [H2, CO, hydrocarbons; Equation (2) is
written with CO):[1,2]
2 CeO2 ðsÞ ! 2 CeO2Ày ðsÞ þ y O2 ðgÞ ð1Þ
2 CeO2 ðsÞ þ 2y CO ðgÞ ! 2 CeO2Ày ðsÞ þ 2y CO2 ðgÞ ð2Þ
The nonstoichiometric phase CeO2Ày can be better described
2y][O2Ày(VO88)y], where VO88 represents an oxygen
Equation (2) can be rewritten in a more stoichiomet-
ric manner, showing that one O out of four is involved in the
þ 4 OÀII
þ CO ðgÞ ! 2 CeIII
þ 3 OÀII
þ CO2 ðgÞ ð3Þ
Ceria is widely used in catalytic converters for exhaust gases
because of its exceptional redox properties. The material is
able to store oxygen during the lean phase (i.e., excess of
oxygen) and to give oxygen back to metal particles during the
rich phase (when there is virtually no O2 in the gas phase); this
is the so-called oxygen storage capacity (OSC) of ceria. The use
of OSC components was first proposed by Ghandi et al. in
Since the pioneering works of Yao and Yu Yao
Su et al.,[5,6]
many studies have been devoted to improving
knowledge of the kinetics of OSC[7–9]
and of the mechanisms
implicated in surface and bulk oxygen mobility in ceria and re-
with a special insight into CeZrOx
Oxygen diffusivity in these materials can be mea-
sured by 18
O isotopic exchange,[20–22]
while oxygen species
(e.g., superoxides, peroxides) that might be involved in the dif-
fusion process can be investigated by electron spin resonance
ESR studies have shown that the pres-
ence of a metal (Pt, Rh) drastically changes the nature of the
oxygen species; the metal favoring the formation of OÀ
instead of superoxide species.
The presence of certain im-
purities in ceria, such as chloride ions, can also affect the
nature and amounts of surface oxygen species.
species give a sharp IR band at 1126 cmÀ1
, while on reduced
ceria samples surface peroxide species can be recorded at
. OSC measurements are currently carried out by the
dynamic technique, in which CO or H2 pulses are injected over
the preoxidized sample at regular time intervals.[32,33]
tioned above, it is generally accepted that one surface oxygen
atom out of four is involved in the redox process shown in
Equation (2), which represents a theoretical OSC value of
for a mean surface density of
Reduced ceria is able to dissociate
or carbon dioxide[34,36]
according to Equation (4) or
the reverse of Equation (2), respectively.
2 CeO2Ày ðsÞ þ 2y H2O ðgÞ ! 2 CeO2 ðsÞ þ 2y H2 ðgÞ ð4Þ
Ceria also possesses versatile acid–base properties, depend-
ing on the nature and temperature of the pretreatment. Ceria
can chemisorb pyrrole, a proton donor, and CO2, an electron
acceptor, which is characteristic of strong Lewis-base sites.
These properties are relatively insensitive to the state of ceria
(i.e., reduced or unreduced). Reductive pretreatment may how-
ever change the distribution of carbonate species at the ceria
surface (bridged, bidentate, monodentate, polydentate). On
the basis of CO2 chemisorption studies, Martin and Duprez
found the following scale for the density of basic sites of se-
lected oxides (expressed in mmolCO2 mÀ2
): CeO2 (3.23)MgO
(1.77)ZrO2 (1.45)10% CeO2–Al2O3 (0.44)Al2O3 (0.18)
These values were obtained by adsorption at
room temperature. At higher temperatures, the amounts of
chemisorbed CO2 decrease. Li et al. have shown that the
amount of CO2 that remains chemisorbed at 1008C would be
on ceria and 1.40 mmolmÀ2
proves that ceria possesses a high number of basic sites of
weak or medium strength. Binet et al. also observed that ceria
can chemisorb CO or pyridine, but the band positions strongly
suggest that the Lewis acidity of ceria is significantly lower
than that of zirconia or titania.
In constrast to Lewis basicity,
the Lewis acidity would decrease upon reduction of ceria.
Ceria has been the subject of thorough investigations, mainly
because of its use as an active component of catalytic convert-
ers for the treatment of exhaust gases. However, ceria-based
catalysts have also been developed for different applications in
organic chemistry. The redox and acid–base properties of ceria,
either alone or in the presence of transition metals, are impor-
tant parameters that allow to activate complex organic mole-
cules and to selectively orient their transformation. Pure ceria
is used in several organic reactions, such as the dehydration of
alcohols, the alkylation of aromatic compounds, ketone forma-
tion, and aldolization, and in redox reactions. Ceria-supported
metal catalysts allow the hydrogenation of many unsaturated
compounds. They can also be used for coupling or ring-open-
ing reactions. Cerium atoms can be added as dopants to cata-
lytic system or impregnated onto zeolites and mesoporous cat-
alyst materials to improve their performances. This Review
demonstrates that the exceptional surface (and sometimes
bulk) properties of ceria make cerium-based catalysts very ef-
fective for a broad range of organic reactions.
[a] Dr. L. Vivier, Prof. Dr. D. Duprez
LACCO Laboratoire de Catalyse en Chimie Organique
CNRS—UniversitØ de Poitiers
40 Avenue du Recteur Pineau, 86022 Poitiers Cedex (France)
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 655
Ceria-Based Solid Catalysts for Organic Chemistry
All these acid–base or redox surface properties enable ceria
to catalyze numerous organic reactions that require these
types of active centers. Although it is often difficult to ascribe
the catalytic activity to a unique type of site, this Review will
be organized into three parts: reactions preferentially catalyzed
on acid–base sites (dehydration and ketonization), reactions
preferentially catalyzed by redox centers (reduction and oxida-
tion of organic compounds), and finally reactions that may re-
quire both acid–base and redox sites (addition, substitution,
isomerization, or ring opening).
2. Dehydration of Alcohols
2.1. Dehydration of 4-methyl-2-pentanol
The dehydration of 4-methyl-2-pentanol by cerium-based cata-
lysts could represent an alternative route to the preparation of
4-methyl-1-pentene; a monomer for the manufacture of ther-
moplastic polymers of superior technological properties
(Scheme 1). The unsupported mixed oxides CeO2-ZrO2
and CeO2-ZrO2 supported on SiO2
been used for this reaction, in the vapor phase under normal
atmospheric pressure of N2 between 2508C and 4008C. It was
observed that these catalysts exhibit high and stable catalytic
activities. Their acid–base properties govern the competition
between dehydration into the desired 1-alkene, the formation
of other undesired alkenes, and parasitic dehydrogenation. The
product distribution gives a detailed picture of the acid–base
properties of the material.
4-methyl-1-pentene is the most abundant product of 4-
methyl-2-pentanol conversion. By dehydration, 4-methyl-2-pen-
tene and trace amounts of skeletal isomers of C6 alkenes are
also formed. Dehydrogenation leads to 4-methyl-2-pentanone,
and high-molecular-weight ketones are formed only in trace
amounts. A maximum in 4-methyl-1-pentene selectivity is ob-
served with the ceria-rich catalysts, and this selectivity decreas-
es with increasing reaction temperature.
An E1cB mechanism, which needs balanced concentrations
of the acid and base sites, as well as a higher strength of the
latter, is probably operating on these catalysts. The selectivity
in 1-alkene has been already shown during the dehydration of
1-butanol and 2-butanol on CeO2-based catalysts.
2.2. Dehydration of diols
Allylic alcohols can be selectively produced by the vapor-phase
dehydration of 1,3-diols over CeO2 between 3008C and 4258C
1,3-Diols are more reactive than other diols
and monoalcohols over CeO2. 2-Propen-1-ol was produced
from 1,3-propanediol over pure CeO2 with a maximum selectiv-
ity of 98.9% at 3258C. In the dehydration of 1,3-butanediol, 2-
buten-1-ol and 3-buten-2-ol were produced with a sum selec-
tivity 99%. 3-Penten-2-ol was also produced selectively from
2-methyl-1,3-propanediol is less reactive than 1,3-butanediol
or 1,3-propanediol: the methyle group obstructs adsorption on
the surface because of steric hindrance. The corresponding al-
lylic alcohol was produced with lower selectivity: decomposi-
tion proceeds simultaneously.
Theoretical investigations have indicated an interaction be-
tween the oxygen atoms in butan-1,3-diol and cerium cations:
butane-1,3-diol preferentially adsorbs on the oxygen-defect
site of the CeO2 (111) surface and is dehydrated at the defect
site. Indeed, in the dehydration of 1,3-butanediol and of 1,4-
butanediol into unsaturated alcohols, the activity increased
Laurence Vivier obtained her Ph.D. in
chemistry from the University of Poiti-
ers (France) in 1991. Following a post-
doctoral stay at the University of
Swansea (UK), she returned to Poitiers
at the Laboratoire de Catalyse en
Chimie Organique as an Assistant Pro-
fessor. Her research focuses on hydro-
teatment on sulphide catalysts. In
2008, she joined the team of Dr.
Duprez to pursue her research inter-
ests in the use of biomass for renewa-
Daniel Duprez obtained his Ph.D. from
Nancy Polytechnicum (France). After a
two-year stay at the Elf Research
Center at Solaize (near Lyon, France),
he joined the Laboratoire de Catalyse
en Chimie Organique de Poitiers
(France) in 1978. He developed several
projects on the use of isotopic ex-
change for measuring oxygen and hy-
drogen mobilities on supported metal
catalysts, with applications in H2 pro-
duction from biomass resources, H2 purification, oxidation, and
DeNOx reactions and water purification processes (CWAO). Rare-
earth oxides are frequently used in these catalytic applications,
either alone or as “active” supports of metals.
Scheme 1. Transformation of 4-methyl-2-pentanol on ceria-based catalysts.
Scheme 2. Dehydration of 1,3-diols into allylic alcohols.
656 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
with increasing the CeO2 particle size. The CeO2 (111) facets,
more numerous on larger particles, have active sites for the de-
In the dehydration of 1,4-butanediol, 3-buten-1-ol is pro-
duced over CeO2 between 3758C to 4508C.[56–58]
The better se-
lectivity (68.1%) was observed at 4008C. Side reactions, such
as isomerization of the initial product, but-3-en-1-ol, hydroge-
nation, and dehydrogenation proceed, together with the cycli-
zation of 1,4-butanediol to tetrahydrofuran (Scheme 3).
Among the various lanthanide oxides, CeO2 shows proper-
ties that differ from those of the other members of the lantha-
In the reaction of 1,5-pentanediol, CeO2 cata-
lyzed only undesirable side reactions, such as dehydrogena-
tion, as well as dehydration;
d-valerolactone and cyclopenta-
none being the major products. The authors speculated that
the redox cycle of Ce4+
on the surface of CeO2 plays a
key role in the activation of 1,5-pentanediol. Although 1,3-bu-
tanediol is readily activated on CeO2 at 3258C, higher tempera-
tures are needed to activate 1,4-butanediol and 1,5-pentane-
diol on CeO2. Thus, both the reactivity and the selectivity over
CeO2 decrease in the order of 1,3-1,4-1,5-diols.
Triols, such as 1,2,3-propanetriol (glycerol) and 1,2,3- and
1,2,4-butanetriols have been dehydrated to afford the corre-
sponding hydroxyketones, while 1,2-propanediol was dehydro-
genated to form hydroxyacetone over both ceria-supported
and nonsupported Cu-based catalysts.
2.3. Other dehydrations
4-Hydroxy-2-butanone has been converted into 3-buten-2-one
over various oxide catalysts at 1608C. Ceria shows a relatively
high initial activity but is rapidly deactivated. This deactivation
is probably caused by the strong interaction of 3-buten-2-one
with acid sites to form carbon species on the catalyst surface;
however, the results of NH3-temperature programmed desorp-
tion (TPD) could not explain this deactivation; CeO2 showing a
much lower acidity than other oxides such as Al2O3 and SiO2/
Al2O3. In this case, the redox nature of CeO2 may be the cause
of this deactivation.
3.1. Acid condensation
An important route for ketone production is decarboxylative
condensation of two carboxylic acids. Symmetrical, nonsym-
metrical, and arylalkylketones have been obtained by ketoniza-
tion of carboxylic acids in the gas phase over ceria-based cata-
lysts under flowing conditions, proceeding according to the
COOH þ RCOOH ! R0
COR þ CO2 þ H2O ð5Þ
Usually, the ketonization by acid condensation was carried
out in the presence of ceria-based catalysts (10–20% CeO2 sup-
ported on SiO2, TiO2, or Al2O3) between 300 and 4508C.[62–70]
Symmetrical ketones such as 3-pentanone, 6-undecanone,
and 7-tridecanone have been obtained from ketonization of
the appropriate acids.[62,65]
This method was applied to the syn-
thesis of nonsymmetrical ketones used as raw materials for
pesticides and pharmaceutical products.[66–68]
methylcyclopropylketone and methylnonylketone were pro-
duced by the condensation of acetic acid with cyclopropane-
carboxilic acid and decanoic acid, respectively.
In the reac-
tion of propanoic acid, the reactivity of the carboxylic acid
slightly decreased as its chain length was increased, and
branched acids were less reactive than linear ones.
Aromatic ketones were obtained from aromatic carboxylic
acids and acetic acid over CeO2/Al2O3, chosen as an industrial
catalyst for the preparation of the 2-methylacetophenone be-
cause of its higher productivity, longer catalyst life, and the lift-
ing of legal restrictions on catalyst handling. The catalyst
system can also be applied to the preparation of acetophe-
none, nitroacetophenone, and chloroacetophenone.
carboxylic acids were selectively reduced to aldehydes by con-
densation with formic acid.
Moreover, the literature men-
tions some patents relating to the synthesis of nonsymmetrical
ketones from carboxylic acids over CeO2/Al2O3 at 350–
and CeO2/TiO2 at 4408C.
The condensation of acetic acid to acetone
or of propano-
ic acid to 2-pentanone
was also carried out over pure CeO2
from 3008C. The catalytic sites were suggested to be Lewis
acid–base pair sites, with the Lewis acid sites (Ce4+
) being re-
The activity towards acid condensation increased
with increasing particles size, because CeO2 (111) facets are
predominant on larger particles and have active sites for the
condensation reaction of propanoic acid.
Stubenrauch et al.
had shown previously by TPD that acetone is produced during
the decomposition of acetic acid only on the CeO2 (111) sur-
More recently kinetic factors have been investigated for ke-
tonization upgrading processes over a Ce0.5Zr0.5O2 catalyst from
175 to 3508C.
This material showed desirable catalytic prop-
erties for ketonization of carbohydrate-derived carboxylic acids
in the presence of other monofunctional oxygenated species,
such as alcohols or ketones.
Under these conditions two dif-
ferent reactions take place, esterification and ketonization.
Scheme 3. Transformation of 1,4-butanediol over pure CeO2.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 657
Ceria-Based Solid Catalysts for Organic Chemistry
Both consume hexanoic acid, used as model molecule. Direct
ketonization of esters does not take place in the presence of
3.2. Ketonization of esters
Glinski and collaborators have studied the ketonization of vari-
ous aliphatic or aromatic esters over 20 wt% MOx/S, where
M=Mn, Ce, Zr, or Th and S=Al2O3 or SiO2, in the gas phase
between 300 and 4258C.[79–81]
The ketonization of ethyl ester in
the presence of these oxide catalysts proceeds according to
the general equation:
2 RCOOC2H5 ! RCOR þ CO2 þ H2O þ 2 C2H4 ð6Þ
In these studies, the highest yields in ketones were always
obtained with manganese-based catalysts. 3-Pentanone and 7-
tridecanone were formed in ketonization of pure aliphatic
esters, ethyl propanoate and ethyl heptanoate. Unfortunately,
from pure ethyl benzoate, benzene was obtained instead of di-
phenylketone. Dialkyl- and arylalkyl-ketones were obtained
from the cross-ketonization of a mixture of aliphatic and aro-
The reactivity of tert-butyl heptanoate was higher than that
observed for ethyl heptanoate over all MOx/Al2O3 catalysts,
with M=Mn, Ce, or Zr. Thus, various alkyl heptanoates
(C6H13COOR, with R=Me, Et, nPr, iPr, nBu, iBu, sBu, and tBu)
were used in the ketonization reaction in the presence of the
most active catalytic system, MnO2/Al2O3. In the case of n-alkyl
heptanoates, the reactivity increased with the elongation of
the n-alkyl chain.
In the cycloketonization of diethylhexanedioate, only moder-
ate yields of cyclopentanone (35% over MnO2/Al2O3) were
achieved, accompanied by various amounts of byproducts.
Cycloketonization of dimethylhexanedioate was investigated
over pure CeO2 between 350 and 4758C.
The conversion of
diethylhexanedioate increased with increasing reaction tem-
perature whereas the selectivity to cyclopentanone decreased.
This decrease at high conversion was mainly caused by a con-
secutive reaction of cyclopentanone into 2-methylcyclopenta-
none due to alkylation with methanol, produced by the cyclo-
Long-carbon-chain ketones (C17H35COC17H35, C15H31COC15H31,
CH3COC17H35, CH3COC15H31) were also obtained from methyl
esters of fatty acids (essentially C17H35COOCH3 and
C15H31COOCH3), in methanol at atmospheric pressure at 3858C
(optimal temperature), over catalysts containing SnÀCeÀRh
oxides in a molar ratio 90:9:1 (total yield: 63%, conversion:
A similar catalyst was used to transform methyl lau-
rate (C11H23COOCH3) to 12-tricosanone (C11H23COC11H23).
3.3. Dimerization of alcohols
During the alkylation of phenol with 1-propanol over CeO2/
MgO catalysts under atmospheric pressure of helium, Sato
et al. observed that the formation of propanal and 3-penta-
none and the conversion of 1-propanol to 3-pentanone in-
creased with increasing CeO2 content.
Elsewhere, Plint et al.
studied the reaction of a series of primary and secondary alco-
hols containing n carbon atoms under oxidative conditions.
Symmetrical ketones with 2nÀ1 carbon atoms were produced
in the presence of O2 over 40% CeO2/MgO (4508C, 1 atm).
There was no dimerization reaction with 2-methyl-2-propanol.
The yield of ketone increased with chain length from C2–C4
and then reached a maximum for the C4–C7 reactant; the con-
version being consistently high (90%).[86,87]
A reaction mechanism in which alcohol is oxidized to alde-
hyde and then carboxylic acid [Equation (7)] following by the
coupling of two equivalents of acid to give the symmetrical
ketone and CO2 [Equation (8)], is proposed according to the
RCH2OH ! RCHO ! RCO2H ð7Þ
2 RCO2H ! RCOR þ CO2 þ H2O ð8Þ
The reaction of a 1:1 mixture of 1-hexanol and 1-heptanol
produced a statistical yield of the three expected ketones.
Under nonoxidative conditions, 1-propanol was preferentially
converted into 3-pentanone over CeO2-Fe2O3 catalysts at
4508C and propanal, 3-hydroxy-2-methylpentanal, and n-
propyl-propionate were observed as by-products.
tion of Fe2O3 to CeO2 enhances the ability of CeO2 for the cata-
lytic dehydrogenation of 1-propanol to propanal, without
losing the ability to dimerize propanal. The formation of 3-pen-
tanone from 1-propanol over CeO2-Fe2O3 proceeds via aldol
addition of propanal into 3-hydroxy-2-methylpentanal, fol-
lowed by decomposition into 3-pentanone, while n-propylpro-
pionate is formed as a mere by-product [Equation (9)].
2 RCHO ! aldol ! RCOR þ H2 þ CO ðor CO2Þ ð9Þ
This reaction was applied to the cyclization of 1,6-hexanediol
into cyclopentanone, an useful intermediate for medical and
The cyclization of 1,6-hexanediol was se-
lectively catalyzed by CeO2-MnOx with a Mn content of 10–
30 mol%: cyclopentanone was produced with a selectivity of
80 mol% at 4508C. A possible reaction pathway over ceria-
based catalysts is illustrated in Scheme 4.
Elsewhere, SnÀCeÀRh oxides already used in the condensa-
tion of methyl esters of fatty acids have shown high activity
and selectivity at relatively low temperatures in the ketoniza-
tion of n-butanol. At 3508C, 4-heptanone was obtained with
Scheme 4. Probable cyclization reaction pathway over ceria-based catalysts.
658 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
89% selectivity and 88% n-butanol conversion.[90,91]
ing a cerium dopant to the tin basic dioxide structure caused
the appearance of strong acidic centers of Lewis type at the
surface. As the selectivity to 4-heptanone increases with the
presence of cerium, the Lewis acidic sites become more in-
volved in the mechanism of alcohol, aldehyde, or acid conden-
Ceria is able to change reversibly from Ce4+
conditions to Ce3+
under reducing conditions. Oxygen atoms
in CeO2 units are very mobile and easily leave the ceria lattice,
giving rise to a large variety of nonstoichiometric oxides with
the two limiting cases: CeO2 and Ce2O3.
4.1. Hydrogenation of C=C bonds
4.1.1. Hydrogenation of phenol to cyclohexanone
Cyclohexanone is a key raw material in the production of both
caprolactam for Nylon-6 and adipic acid for Nylon-6,6. Industri-
ally, cyclohexanone is produced either by the oxidation of cy-
clohexane or by the hydrogenation of phenol to cyclohexanol,
followed by dehydrogenation of cyclohexanol. Selective hydro-
genation of phenol to cyclohexanone is attractive in terms of
capital cost and energy saving.
The selective hydrogenation of phenol to cyclohexanone
was carried out in gas phase over supported Pd catalysts.[92,93]
The catalytic performance was improved by a modification of
the electronic surroundings of Pd, induced by a promoter or
by a modification of the acid–base characteristics of the sup-
port, leading to a change in the adsorption–desorption equilib-
rium of reactants and products. Similar to La2O3, CeO2 as sup-
port provides a better activity and a good stability to cata-
The high surface area mesoporous oxide support gives rise
to well dispersed and stable metal particles on the surface and
then has some beneficial effect on the catalytic performance.
The vapor-phase hydrogenation of phenol, at atmospheric
pressure, over 3% Pd supported on mesoporous CeO2 (Pd/
CeO2-Ms) at 1808C produced a mixture of cyclohexanone
(about 50%), cyclohexanol (35%), and cyclohexane (15%) with
a phenol conversion of about 80%. The selectivity depended
on the modes of phenol adsorption, which are governed by
the nature of the support. On the Pd/CeO2-Ms catalyst, under
the reported experimental conditions, there was a significant
reduction of the CeO2 surface, which resulted in the formation
of nonstoichiometric CeO2 creating acid and basic sites. Over
basic sites, nonplanar-adsorbed phenol led to the formation of
cyclohexanone, while coplanar-adsorbed phenol led to the for-
mation of cyclohexanol.
More recently, the hydrogenation of phenol to cyclohexa-
none was carried out in the liquid phase with ethanol as sol-
vent in order to improve the selectivity, because the reaction
could be performed at relatively low temperature.[94,95]
maximum phenol selectivity for cyclohexanone over 5.8% Pd-
Ce-B supported on hydrotalcite reached 80%, with a phenol
conversion of 82%.
A similar conversion and selectivity were
obtained by the same authors on Ce-doped Pd-B amorphous
The promoting effect of the Ce-dopant on
the catalytic performance could be attributed to stabilization
of the amorphous structure of the Pd-B alloy by cerium; the
electron-enriched Pd active sites, owing to the electron-dona-
tion from cerium; and the increase of surface basicity resulting
from the formation of Ce2O3.
4.1.2. Hydrogenation of 1,3-butadiene
The hydrogenation of 1,3-butadiene was carried out in the gas
phase at atmospheric pressure between 47 to 1078C. The pres-
ence of CeO2 in Pd-CeO2 supported on Al2O3 catalysts favored
hydrogenation at the 1,2 position of the 1,3-butadiene mole-
cule, increasing the selectivity towards 1-butene.
sence of butane as reaction product indicated that the adsorp-
tion strength of 1,3-butadiene was reduced by the presence of
cerium, which modifies the electronic structure of Pd, thereby
avoiding total hydrogenation.
4.1.3. Hydrogenation of acrylonitrile
Selective gas-phase hydrogenation of acrylonitrile (CH2=CHÀ
CN) over low-loaded Pd (0.05 wt%)/Al2O3 catalysts doped with
various contents of cerium gave propionitrile with a selectivity
nearly 100%. The addition of cerium improved the activity and
the stability of these catalysts.
The sintering of the dispersed
palladium particles was retarded by the addition of cerium and
the catalytic activity was preserved. Elsewhere, the presence of
Pd facilitated the reduction of Ce4+
to form new active
4.1.4. Hydrogenation of mesityl oxide
Mesityl oxide (4-methyl-2-penten-2-one) was selectively hydro-
genated in the gas phase at 1758C over 2CuO-CeO2 and 2Cu-
CeO2 reduced catalysts to produce methyl isobutyl ketone (4-
methylpentan-2-one), an important chemical used at the in-
The reduced sample was more active than the
oxidized one; the selectivities being 93% and 100%, respec-
tively. Binary copper–cerium intermetallic compounds (CeCu2)
are interesting precursors to provide new supported copper
4.1.5. Hydrogenation of sunflower oil
The selective hydrogenation of ethyl esters of traditional sun-
flower oil, a mixture comprising linoleic acid C18:2 (9,12) Z,Z
(60.11%), oleic acid C18:1 (9) Z (27.49%), and stearic acid
C18:0 (3.72%), was carried out at low temperature (408C) in
ethanol as solvent in the presence of supported palladium cat-
alysts (Scheme 5). The aim was to selectively hydrogenate lino-
leic acid C18:2 (9,12) Z,Z towards oleic acid C18:1 (9) Z, avoid-
ing Z–E isomerization, position isomerization, and complete hy-
drogenation. The use of CeO2 as oxide support to deposit pal-
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 659
Ceria-Based Solid Catalysts for Organic Chemistry
ladium did not improve the selectivity toward the C18:1 (9) Z
or (12) Z compared to Pd/SiO2.
4.1.6. Hydrogenation of acetylene
By using Au/CeO2 as catalyst in acetylene hydrogenation in the
gas phase at 3008C, a selectivity of 100% toward ethylene was
obtained with a high conversion, which depended on the H2/
C2H2 ratio. Above 3008C, the only byproduct was methane,
formed by carbene intermediates that also polymerized, giving
rise to deactivation. The high selectivity could be explained by
the difference in the strength of adsorption onto the gold sur-
face between acetylene and ethylene.
4.1.7. Hydrogenation of benzene
The hydrogenation of benzene in the gas phase at atmospher-
ic pressure can be used to characterize the size of metallic par-
ticles of supported ceria-based catalysts.[101–104]
With this reac-
tion it is possible to determine the amount of the accessible
metallic atoms of low-loaded supported rhodium cata-
A Ni/CeO2 catalyst exhibited a different behavior from that
observed with Al2O3 or SiO2 supports. The modification of the
catalytic properties of Ni/CeO2 catalysts with reduction pre-
treatment is correlated to a transformation of the CeO2 sup-
port and to strong interactions between theses species and
In another study, nickel catalysts supported
on ceria, synthesized by g-radiolysis, were tested in the hydro-
genation of benzene. At 1008C, the catalyst completely con-
verted benzene to cyclohexane and remained stable for at
least 20 h. The high catalytic performance of Ni/CeO2 was at-
tributed to the high dispersion of nickel and to the promoter
role of the support, through the formation of NiÀCe phases.
The partial hydrogenation of benzene to cyclohexene is of
great industrial interest: cyclohexene can be used in the syn-
thesis of various organic compounds.[105,106]
are very promising systems for cyclohexene formation through
partial benzene hydrogenation in a three-phase medium, in
the presence of water and TiCl3. The maximum yield in cyclo-
hexene (about 17%) was obtained with Ru/CeO2 catalysts,
noncalcinated and reduced at 5008C or 7508C.
The partial hydrogenation of benzene to cyclohexene was
also carried out over Ru–Ce catalysts supported on siliceous
materials such as SBA-15, in the presence of ZnSO4 in aqueous
solution. The existence of the CeIII
species decreased the
number of exposed Ru atoms, increased the number of elec-
trons on metallic Ru, and enhanced the hydrophilicity of the
catalyst. The maximum yield of cyclohexene (53.8%) was ob-
tained on a RuCe/SBA-15 catalyst, with a molar ratio Ce/Ru
equal to 0.4.
4.1.8. Hydrogenation of biphenyl
Hexagonal mesoporous silica (HMS) was used as support for
the preparation of Au catalysts, and was tested in the liquid-
phase hydrogenation of biphenyl at 5 MPa and 2158C (in a so-
lution of n-tetradecane, with about 10% n-hexadecane). Modi-
fication of HMS by Ce led to Au-supported catalysts that were
more stable with respect to sintering. In the Au/HMS–Ce cata-
lyst, Ce was not incorporated into the framework of HMS, lead-
ing to clusters of Au and CeO2. However, further investigations
on the nature of the Au–CeO2 interaction could yield more ex-
planations with regard to the performance of Au/HMS–Ce cat-
4.2. Hydrogenation of C=O bonds
4.2.1. Hydrogenation of a-b-unsaturated aldehydes
The selective hydrogenation of a-b-unsaturated aldehydes to
unsaturated alcohols is an important reaction in the produc-
tion of many pharmaceutical, agrochemical, and fragrance
compounds. The hydrogenation of the C=C bond is thermody-
namically more favorable than the C=O hydrogenation, and
low yields of the desired product are obtained with the con-
ventional hydrogenation catalysts.
Cerium-based platinum catalysts have been extensively stud-
ied for the hydrogenation of crotonaldehyde (CH3ÀCH=CHÀ
and citral ((CH3)2C=CHÀ(CH2)2ÀC(CH3)=CH-
The activation of the carbonyl bond is induced by
the presence of oxygen vacancies sites located at the interface
between ceria and the platinum particles.
Indeed, the selective hydrogenation of a-b-unsaturated alde-
hydes has been used as probe reaction to study the existence
of a “strong metal–support interaction” (SMSI) effect in ceria-
supported and -promoted noble catalysts. Ceria is able to form
oxygen vacancies and intermetallic compounds after reduction
treatment at relatively high temperatures.
Touroude and collaborators have studied the selective hy-
drogenation of crotonaldehyde on Pt/CeO2 in the gas phase at
On chlorine-free Pt/CeO2, the
crotyl alcohol selectivity increased up to more than 80% (con-
version: 45%) when the reduction temperature of the catalysts
reached 7008C. The presence of chlorine, during the catalyst
synthesis, preserves the catalytic properties of platinum metal
Scheme 5. Hydrogenation and isomerization of linoleic acid C18:2 (9,12) Z,Z.
660 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
for the hydrogenation of C=C bond; chlorine atoms around
platinum particles inhibit the diffusion of cerium atoms inside
the metal particles and prevents the formation of CePt5 alloy.
By controlling the nanostructure, size, and morphology of sup-
ported platinum particles, the authors showed that it is possi-
ble to orientate the selectivity in the hydrogenation of croto-
The presence of zinc facilitated the reduction of surface
ceria, thereby increasing the potential number of Ce3+
metal interface sites, particularly in cases where small Pt parti-
cles were located in ceria rich zones of the support.[113–115]
the case of vapor-phase hydrogenation of crotonaldehyde, the
overall catalytic activity increased significantly after reduction
at 5008C in the zinc-containing catalyst, and furthermore, the
selectivity toward the hydrogenation of carbonyl bond is im-
proved. Pt on mesostructured CeO2 nanoparticles embebbed
within ultrathin layers of highly structured SiO2 binder showed
the highest reported activity, with 80% selectivity for the che-
moselective hydrogenation of crotonaldehyde.
the reduction temperature, the number of Pt-CeO2Àx interfacial
sites, which are responsible for activating the carbonyl bond,
The hydrogenation of citral was carried out in the liquid
phase at 508C in ethanol
or at 708C in isopropanol.
formation of geraniol (E isomer) has been observed as the sole
product on Pt/CeO2 and has been attributed to the influence
of the SMSI state in the selective hydrogenation of C=O
On a Pt/C catalyst promoted with highly dispersed ceria, the
main products of the hydrogenation of citral were citronellal
(hydrogenation of the conjugated C=C bond), the unsaturated
alcohols geraniol and nerol, and the saturated alcohol citronel-
lol (by hydrogenation of the C=O bond of citronellal).
the one hand, the creation of new Pt–CeOx sites at the metal/
support interface act as Lewis acid sites able to activate the C=
O bond of the citral molecule; on the other hand, the exis-
tence of an electronic interaction between the reduced ceria
particles and the active metal leads to an increase in electron
density on the platinum particles, with subsequent weakening
of the adsorption of citral via the C=C bond. Moreover, when
tin is added, the ceria reducibility is increased. The presence of
species, also able to act as Lewis acid sites, on the surface
of platinum particles and/or in their close vicinity could ac-
count for the increase in selectivity to unsaturated alcohols
with reduction temperature. The increase of conversion after
reduction at high temperature in these catalysts could be also
explained by the creation of new PtÀSnn+
sites active for hy-
drogenation of the C=O bond in the citral molecule.
Previously, Barrault et al. have studied the hydrogenation of
cinnamaldehyde (C6H5ÀCH=CH-CHO) in the liquid phase with
propylene carbonate as solvent over cobalt catalysts supported
on activated carbon, and showed that the addition of cerium
to cobalt increased the selectivity to unsaturated alcohol with-
out decreasing of the activity.
Elsewhere, the use of cerium
on Ru-based catalysts supported on alumina and activated
carbon increased the selectivity to the unsaturated alcohols in
hydrogenation of crotonaldehyde (in gas phase) and of citral
(in liquid phase with isopropanol as solvent).
observed activities were very low.
More recently, Campo et al. studied the influence of the spe-
cific surface area of the support on the selective hydrogena-
tion of crotonaldehyde on Au/CeO2.[123–126]
They showed that
the high surface area catalyst (Au/HAS-CeO2, with 240 m2
was active and highly selective towards the hydrogenation of
the C=O bond either at 1208C and atmospheric pressure[123–125]
or at 808C in the liquid phase (solvent: isopropyl alcohol).
Other Au/CeO2 catalysts with lower specific surface areas
showed a rather low selectivity. The high selectivity is an intrin-
sic characteristic of gold particles (particle size lower than
4 nm on Au/HAS-CeO2 and higher than 9 nm on other Au/
CeO2 catalysts), though ceria plays an important role as a
result of its redox and acid–base properties.
The selectivity to the unsaturated alcohol is governed by dif-
ferent factors: the nature of the active metal, metal particles
size, support effects, and presence of promoters or bimetallic
4.2.2. Enantioselective hydrogenation
Mixed nickel–cerium oxides, using tartaric acid as modifier,
were used for studying the enantioselective hydrogenation of
methylacetoacetate in methyl 3-hydroxybutyrate (Scheme 6).
X-ray photoelectron spectroscopy (XPS) and FTIR analysis evi-
denced that the modifying agent reacts with the metallic
nickel to give nickel tartarate. In the presence of this modifier,
the reduction of Ce4+
was improved. The tartarate salt
is stabilized by these Ce3+
species in close vicinity of Ni2+
forming a complex with methyl acetoacetate. Thus, a stable
six-membered ring complex is formed between a hydroxyl
group of tartarate, the reactive C=O bond, and the methylenic
group (acidic H) of methylacetoacetate and gives rise to a
single product, having a specific configuration depending on
the absolute configuration of the modifying agent.
Another, similar reaction concerned the enantioselective hy-
drogenation of 1-phenyl-1,2-propanedione
(Scheme 7). This
reaction was carried out in the liquid phase (cyclohexane was
used as solvent) at 258C and a dihydrogen pressure of 40 bar
over an iridium-supported catalyst promoted by ceria, in the
presence of cinchonidine as modifier. The presence of Ce in
Scheme 6. Hydrogenation of methylacetoacetate.
Scheme 7. Hydrogenation of 1-phenyl-1,2-propanedione.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 661
Ceria-Based Solid Catalysts for Organic Chemistry
the Ir/SiO2 produced a slight increase in both the activity and
the enantioselectivity (formation of (R)-2-hydroxy-1-phenyl-1-
propanone). The cerium oxide species were mainly present on
the silica support and contributed to the formation of Ird+
cies that were responsible for C=O bond polarization and reac-
tion rate enhancement.
4.2.3. Hydrogenation of carboxylic acids to aldehydes
For the hydrogenation of aromatic carboxylic acids, various
metal oxides such as CeO2 have shown high activity and selec-
tivity to corresponding aldehydes.[129–133]
The hydrogenation of
benzoic acid over CeO2 proceeds at up to 3508C in gas phase;
the selectivity to benzaldehyde was more than 95% and the
activity was controlled by the number of oxygen vacancies
that are produced under the reaction conditions. The carboxyl-
ic acid deoxygenates with the help of an oxygen vacancy ac-
cording to the Mars–Van Krevelen mechanism, forming an acy-
lium ion that is hydrogenated to aldehydes. An enhancement
of the catalytic activity of CeO2 at low temperatures could be
achieved by addition of the promoters, as Mn, Zr, In, and Pb
However, ceria catalysts show little deactivation in
stability test owing to coke formation and the valence changes
of Ce over the catalyst.[132,133]
To limit the use of CeO2, owing to its high cost, some au-
thors have used mixed CeO2–Al2O3 oxides for the hydrogena-
tion of benzoic acid to benzaldehyde. To improve their per-
formances, the simultaneous addition of Mn and K to theses
oxides is necessary.
For hydrogenation of aliphatic carboxyl-
ic acids that have two a-hydrogen atoms, CeO2 shows a low
selectivity because undesirable ketonization occurs.
4.2.4. Hydrogenation of aldehydes to alcohols
The reduction of benzaldehyde has been carried out at 3008C
in a helium or dihydrogen atmosphere over simple metal
oxides as CeO2. CeO2 was not proved to be the better catalyst
for either the Cannizzaro reaction (under helium) to produce
benzyl alcohol and benzoate or direct hydrogenation (under
dihydrogen) when compared with other oxides.
Under helium, the bare CeO2 support was more active than
the corresponding copper-supported catalyst, which is due to
the lesser amount of active hydroxyl groups in the surface of
supported catalyst than of bare support.
Indeed, the Canni-
zzaro reaction consumes surface OH groups to form benzyl al-
cohol and benzoate surface species.
Under dihydrogen, a higher activity and a higher selectivity
to benzyl alcohol were obtained on an irreducible support. On
a reducible support such as CeO2, the activity was lower and
could be explained by a strong metal–support interaction.
Indeed, only traces of benzyl alcohol were observed on Cu/
CeO2; the selectivity to toluene being above 90%. More re-
cently, a significant amount of benzyl alcohol was produced
on Ni/CeO2 under atmospheric pressure of H2 at only a low
temperature (708C). The selectivity to toluene increased with
increasing temperature. Toluene is the product of consecutive
benzyl alcohol hydrogenolysis. This mechanism could involve
hydride species, which could be formed on nickel metal sup-
ported on a reducible support such as CeO2.
Elsewhere, Ce-doped NiÀB amorphous alloy catalysts have
exhibited excellent selectivity to furfural alcohol during liquid-
phase hydrogenation of furfural (ethanol used as solvent). The
promoting effect of Ce dopant could be interpreted with a
mechanism of activation and hydrogenation of C=O bond.
The cerium in a low-valent state (Ce3+
) on the surface could
act as Lewis adsorption sites, which have a strong affinity for
the oxygen atom of a carbonyl function and cause a polariza-
tion of the C=O bond. This polarization favors nucleophilic
attack of the carbon atom by hydrogen dissociatively adsorbed
on the neighboring Ni active sites.
4.2.5. Hydrogenation of esters
Diols can be produced from the hydrogenation of esters over
RuSn-based catalysts supported on various oxides in liquid
phase with dioxane as solvent. Unfortunately, CeO2 was not
proved to be the better support. However, an enhancement of
the activity could be attributed to an interaction of the C=O
bond with the exposed cations of the reducible oxide, that is,
an SMSI effect.
4.2.6. Hydrogen transfer reactions
The vapor-phase hydrogen transfer reaction of cyclohexanone
with isopropyl alcohol as hydrogen donor was carried out on
mixed oxides of CeO2 and ZnO with a high surface area, to in-
vestigate the effect of rare earth oxide on the activity of ZnO.
Addition of ceria into zinc oxide was found to increase the cat-
alytic activity. Cyclohexanol was the only product observed in
this reaction, with a selectivity greater than 98%. The CeO2–
ZnO materials exhibited excellent redox and moderate acid–
base properties. The addition of ceria to ZnO influenced the
particle morphology, surface area, and acid–base proper-
4.3. Hydrogenation of CN bonds
Catalytic hydrogenation of nitriles is an important route to pro-
duction of amines, which are of practical importance, in partic-
ular primary amines, as chemicals and intermediates.
The gas-phase hydrogenation of acetonitrile over various
Pd-based catalysts gives a mixture of ethylamine, diethylamine,
and triethylamine. The use of a CeO2 support is significant for
preparing PdZn, PdGa, or PdIn alloy species on its surface. The
activity can then be enhanced while maintaining high selectivi-
ty to ethylamine (97% at 1708C over Pd/ZnO/CeO2). Ceria facil-
itates the reduction of ZnO to Zn, which is then alloyed with
The formation of primary amines from nitriles on copper cat-
alysts is normally followed by the formation of secondary
amines. Therefore, the supported copper–lanthanide oxides
are active and very selective for the propionitrile gas phase hy-
drogenation to n-propylamine; the 2Cu-CeO2 being the more
active. The basicity of the copper–lanthanide oxides seems to
662 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
play a key role in this reaction, and the selective formation of
primary amine is due to the lack of acid sites, which are
known to catalyze condensation reactions that lead to secon-
dary or tertiary amines.[144,145]
4.4. Other hydrogenation reactions
Highly dispersed copper promoted by nickel or cobalt support-
ed on CeO2 catalysts exhibit high conversion (96.6%) for the
gas-phase hydrogenation of ortho-chloronitrobenzene to
ortho-chloroaniline with a high selectivity (98%) and without
The high activity and stability of these bi-
metallic catalysts was attributed to a better dispersion and the
formation of smaller particles as well as to a high specific sur-
face area of the catalyst.
The oxidation of organic compounds is one of the most impor-
tant reactions for synthesis of fine chemicals. They are many
examples of oxidation reactions involving chromium-, manga-
nese-, or vanadium-based compounds that are used in stoi-
chiometric quantities and present serious disadvantages be-
cause they are expensive, toxic, and produce equimolar quanti-
ties of waste that are often difficult to separate from the de-
sired products. Owing to ceria’s high oxygen storage capacity
and good catalytic properties, the use of ceria-based materials
has been intensively investigated and applied in the catalytic
5.1. Aerobic oxidation of alcohols
Oxidation of alcohols to the corresponding carbonyl com-
pounds is an important transformation in organic synthesis; al-
dehydes and ketones being an important class of compounds
in organic chemistry. The oxidation of primary alcohols to alde-
hydes is an interesting process in perfumery industry. The aero-
bic oxidation of ortho- and para-hydroxybenzyl alcohol selec-
tively produced the corresponding aldehydes with good yields,
while the selectivity of meta-hydroxybenzyl alcohol was more
towards the corresponding acid at the expense of aldehyde.
The selectivity was improved by reaction in aqueous methanol
and the addition of CeCl3. The catalytic role of CeCl3 in the cat-
alyst system Pt/C–CeCl3–Bi2(SO4)3 is not clear, but it might pro-
tect the generated aldehyde from further oxidation by acetali-
The reaction of ethanol on unreduced and H2-reduced CeO2
and 1 wt% Pd/CeO2 has been investigated by steady state re-
actions, temperature programmed desorption (TPD), and
in situ FTIR spectroscopy. Steady-state reactions have shown a
zero-reaction-order dependency for dioxygen. The conversion
of ethanol was increased by the addition of Pd, from 15 and
30% on CeO2 and H2-reduced CeO2, to 71 and 63% on Pd/
CeO2 and H2-reduced Pd/CeO2, respectively. Ethanol was con-
verted into acetaldehyde, which in turn can react to give vari-
ous compounds (e.g., acetone, crotonaldehyde, CO, CO2, meth-
ane, benzene). Benzene formation was detected only on Pd/
CeO2 catalysts, with the H2-reduced Pd/CeO2 catalyst decreas-
ing benzene formation to almost negligible amounts. The H2-
reduction of the oxide surface inhibited the b-aldolization
route owing to a considerable decrease of the Lewis-base
sites, oxygen anions.
A catalyst of ruthenium combined with cobalt hydroxide
and cerium oxide (Ru–Co(OH)2–CeO2) exhibited a high activity
for the oxidation of various alcohols in liquid phase with ben-
zotrifluoride as solvent, in the presence of dioxygen. Allylic,
benzylic, and secondary alcohols gave high yields of the corre-
sponding carbonyl compounds.
The oxidation of primary
aliphatic alcohols led to the formation of corresponding car-
boxylic acids. a,w-Primary diols were selectively transformed
into the corresponding lactones. In the case of 1,4-pentanediol
having primary and secondary hydroxyls, methyl-g-butyrolac-
tone was obtained with 87% yield by an intramolecular com-
petitive oxidation (Scheme 8).[149,150]
With Ce-free Ru catalysts, the oxidation of primary alcohols
led to the formation of aldehydes. The oxidation of this inter-
mediate to carboxylic acid was slow. Moreover, when 2,6-di-
tert-butyl-para-cresol was added in the oxidation of 1-octanol
as a radical scavenger, octanal was formed without formation
of octanoic acid. The high activity of the Ru–Co(OH)2–CeO2 cat-
alyst might be due to the high oxidation state of the Ru spe-
), arising from the Co atoms in the vicinity of the CeO2
particles. The radical process of the aldehyde oxidation might
be facilitated by synergism between the Ru, Co, and Ce com-
Au/CeO2 catalysts were also effective for the selective oxida-
tion of primary alcohols (benzyl alcohol) to aldehydes, under
solvent-free conditions at 1008C in the presence of O2. For
more acidic supports, such as Fe2O3, subsequent oxidation of
aldehydes to the corresponding acids occurred.
Gold nanoparticles supported on ceria are excellent general
heterogeneous catalysts for the aerobic oxidation of alco-
The combination of small-crystal-size gold (2–5 nm)
and nanocrystalline ceria (ca. 5 nm) led to a highly active, se-
lective, and recyclable catalyst for the oxidation of alcohols
into aldehydes or ketones using dioxygen at atmospheric pres-
sure as oxidant, in the absence of solvent and base. The nano-
meter-scale ceria surface stabilized the positive oxidation
states of gold by creating Ce3+
and oxygen-deficient sites in
the ceria. Aliphatic primary alcohols were more reluctant to un-
dergo oxidation in the absence of solvent. Notably, they pre-
dominantly gave the corresponding ester with high selectivity.
The esters were directly formed by the hemiacetal intermedi-
ate, which was dehydrogenated (Scheme 9).
Abad et al. proposed a mechanism for the aerobic oxidation
of alcohols over Au/CeO2, where the alcohol is adsorbed on
Scheme 8. Oxidation of 1,4-pentanediol to methyl-g-butyrolactone.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 663
Ceria-Based Solid Catalysts for Organic Chemistry
Lewis-acid sites to give a metal alkoxide that subsequently un-
dergoes a rapid hydride transfer from CÀH to Ce3+
give the ketone and CeÀH and AuÀH. In the presence of dioxy-
gen, cerium-coordinated superoxide (CeÀOO·
) species are
formed and, by hydrogen abstraction from AuÀH, become
cerium hydroperoxide, which is responsible for the formation,
after reduction of CeIV
, of the initial Au+
species. The absence
of gold would render this step impossible and lead to a deple-
tion of CeIII
An allylic alcohol, such as 1-octen-3-ol, undergoes a chemo-
selective oxidation in the presence of Au/CeO2 catalysts to the
corresponding ketone without oxidizing or isomerizing the C=
C double bond. In contrast to this, Pd/CeO2 catalysts promote
a considerable degree of C=C double bond isomerization (1,2-
migration) with the formation of 3-octanone as the final prod-
Au/CeO2 is a good catalyst for the oxidation of allylic
alcohols without solvent or in organic media (toluene as sol-
vent). The chemoselectivity of Pd or AuÀPd for the solventless
oxidation of this family of alcohols is very low when compared
with Au catalysts and this selectivity can be correlated to the
stability and concentration of metal hydrides, AuÀH and PdÀ
Primary aliphatic alcohols are selectively oxidized to the
corresponding aliphatic aldehydes up to moderate conver-
sions. When the conversion increased, the selectivity towards
the aldehyde decreased significantly, owing to overoxidation
of the aldehyde to the corresponding carboxylic acid. The ac-
tivity of a gold catalyst for the aerobic oxidation of alcohols in-
volves the presence of a high density of positive gold atoms
that could act as Lewis acid sites that coordinate with alcohols
to form gold alcoholates and also accept hydrides. In this
regard, the role of the support should be, on the one hand, to
provide stability for positive gold species by interfacial gold–
support interactions, and on the other hand, to facilitate
oxygen activation to promote the reoxidation of metal hy-
The oxidation state of gold particles deposited on different
supports such as CuO-CeO2 and CeO2 was investigated during
the liquid-phase catalytic aerobic oxidation of 1-phenylethanol
(in toluene) using in situ XAFS combined with FTIR for product
analysis. A correlation between the oxidation state of Au and
catalytic activity was observed for Au/CuO–CeO2. The 1-phenyl-
ethanol conversion increased with concomitant reduction of
Au species. Different behaviors were observed for Au/CeO2,
with the activity decreasing simultaneously with the reduction
of Au species. However, this deactivation is not directly related
to reduction of the gold species.
Au/CeO2 catalysts with various gold particle sizes showed a
moderate catalytic activity and high selectivity in the liquid-
phase oxidation of benzyl alcohol to benzaldehyde in mesity-
lene or in toluene. The catalytic behavior of this reaction was
affected by the gold particle sizes, showing highest activity for
the catalyst containing gold particles of 6.9 nm average
The effect of the adsorption of the two thiols, n-octa-
decanethiol (ODT) and mercaptoacetic acid (MAA), has been
studied on CeO2-supported gold catalysts with different Au
particle sizes (2.1 and 6.9 nm). Upon addition of 10 mol%
thiol/Autotal, an almost complete loss of activity in the aerobic
oxidation of benzyl alcohol was observed when the Au cata-
lysts were poisoned by ODT, while at the same concentration,
the MAA adsorption had relatively little influence on activity.
ODT first binds to crystal facets of the Au particles and later
forms reversibly bound species on the surface, likely adsorbing
on edge and corner sites. On the other hand, MAA strongly
binds to the edge and corner sites on the supported Au. The
adsorption of MAA on crystal facets is thermodynamically the
least stable configuration.
A mesoporous CeO2 crystalline film used as support was
loaded with gold particles of about 5 nm. The resulting Au/
CeO2 composite showed a good catalytic activity and stability
for benzyl alcohol aerobic oxidation in absence of solvent and
The catalysts ruthenium hydroxide and manganese oxide
supported on cerium oxide Ru/MnOx/CeO2 show a high catalyt-
ic activity for the oxidation of alcohols to the corresponding
carbonyl compounds in liquid phase with a,a,a-trifluoroto-
luene as solvent. Nonactivated aliphatic alcohols required
longer reaction time for their oxidation than the other activat-
ed benzylic and allylic alcohols. A primary aliphatic alcohol, 1-
octanol, was less reactive than a secondary alcohol, 2-octanol.
The particular advantage of this catalyst is the smooth oxida-
tion of alcohols at 278C under dioxygen atmosphere. Such
high catalytic activities are attributable to cooperative action
among the Ru species, MnOx, and CeO2 in the catalyst.
catalytic activity could significantly be improved by deposition
of the ternary RuMnCe oxidic mixture on redox-active sup-
ports, especially on ceria.
Recently, silver catalysts were proposed as a promising alter-
native, being less expensive than Au or Pt catalysts and appli-
cable to a wide variety of alcohols.
A Ag/SiO2 catalyst that
acts as efficient catalyst (but only in the presence of ceria:
10 wt% Ag/SiO2 mixed with ceria in a ratio of 2:1) gave the
best catalytic performance in the selective liquid-phase oxida-
tion of various benzyl alcohols (solvent: toluene). The negative
effects of electron-withdrawing groups in the benzyl alcohol
oxidation suggest a mechanism where metallic silver acts as
main component for the dehydrogenation via a cationic inter-
mediate. The role of cerium can rather be ascribed to the acti-
vation of molecular oxygen.
5.2. Dehydrogenation of alcohols
An infrared spectroscopy study of the adsorbed species and
the gas-phase products was reported for the transformation of
Scheme 9. Oxidation of aliphatic primary alcohols over Au/CeO2.
664 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
2-propanol over CeO2 catalysts calcined at various tempera-
tures in the gas phase.
The dehydrogenation to give ace-
tone started to take place at 1508C. The acetone, through fur-
ther interaction with the surface, became involved in another
reaction to give isobutene and methane when the reaction
temperature increased to 2508C and the dehydration, which
led to propene, had begun. The increase of the dehydration
activity of ceria, upon calcination, was due to an increase of
the acidity of Brønsted acid sites and an increase of the
number of Lewis acid sites. The alcohol dehydrogenation reac-
tion is controlled by the electronic mobility of the catalyst sur-
face and decrease with calcination. The aldol condensation re-
action can also occur over CeO2 catalysts.
Reactions of ethanol on Cu–Mg5CeOx in the gas phase at
3008C led to the formation of acetaldehyde, n-butyraldehyde,
and acetone as predominant products. The initial rate of etha-
nol dehydrogenation increased linearly with the Cu surface
area. Acetaldehyde concentrations increased rapidly to equilib-
rium levels that became independent of Cu content in
CuyMg5CeOx catalysts. Dehydrogenation and condensation re-
actions occured after binding of ethanol to an acid–base site
pair present in basic oxides. These reactions were influenced
by the presence of Cu metal crystallites. Basic sites may inter-
act with Cu sites via migration of hydrogen atoms.
The conversion of cyclohexanol[39,142,166,167]
or of 2-propa-
allows the characterization of the acid–base surface
properties of the oxides. The dehydration of alcohol leading to
alkene would be catalyzed by the acid centers, whereas its de-
hydrogenation leading to ketone would be catalyzed both by
acid and basic sites. The dehydration activity could be related
to the surface acidity, whereas the ratio between the activity in
dehydrogenation and the activity in dehydration (AONE/AENE)
would represent the surface basicity.
At 3008C, CeO2 presents an acidic activity and on the other
hand a basic activity. At 2008C, the presence of ceria support-
ed on Al2O3 (12% CeO2/Al2O3) decreased the acidity in compar-
ison with Al2O3: the ratio AONE/AENE increased (0.2 to 0.8).
conversion of cyclohexanol increased with the temperature
with increasing selectivity to cyclohexene on pure CeO2.
The addition of a CeO2 component to a ZnO catalyst (up to
40% of CeO2), enhanced the activity of the catalyst with more
than 90% selectivity to cyclohexanone. In CeO2–ZnO, Ce4+
of different degrees of coordination unsaturation will act as
Lewis-acid sites for cyclohexanol dehydrogenation. The ab-
straction of hydride ions is more efficient at the Ce4+
than at the Zn2+
At 3008C, on CeO2, in the presence of helium and dihydro-
gen, propene was formed during the transformation of 2-prop-
anol. The temperature increase favored dehydration, which
occurs on acid–base pair sites that consist of coordinatively un-
ions. At 1508C, 2-propanol undergoes
a dehydrogenation to give acetone. The active sites were
again described as Ce4+
ion pairs, however, the acidic site
is probably different from that involved in the dehydration re-
action. When the temperature increased to up to 3008C, ace-
tone molecules, previously produced, took part in a bimolecu-
lar reaction to give isobutene and methane and an acetate sur-
face species. The surface reactivity was associated with Ce4+
Under air, ceria is more active and the selectivity in acetone
is more important than under helium or dihydrogen.
selectivity of Cu/CeO2/CNF (CNF: carbon nanofiber) was depen-
dent on the fraction of CeO2 and on the temperature. High ac-
tivity and selectivity were achieved with the Cu12Ce5/CNF cata-
lyst. However, excess CeO2 enhanced the dehydration activity
and thereby reduced the selectivity. The presence of CeO2 en-
hanced the reduction and dispersion of Cu.
For a Au/CeO2 catalyst, the good oxidation performances
were explained by a combination of the oxidation capability of
gold atoms with the redox properties of the ceria phase.
fact, the dehydrogenation reaction required redox sites, rather
basic sites. The alcohol transformation cannot be a simple test
of acidity. Particularly, on ceria, its redox property and its high
lability of lattice oxygen contribute to products formations, in-
volving oxygen vacancies.
5.3. Hydrogen transfer reactions
Ceria-supported Cu, Ir, and Pd catalysts have shown a very
high activity for liquid-phase transfer dehydrogenation of cy-
clohexanol and 2-octanol to cyclohexanone and 2-octanone,
respectively, using styrene as the hydrogen acceptor, but for
the primary alcohols, the reaction rates were much lower;
however, with a good selectivity for aldehydes. The Cu/CeO2
and Pd/CeO2 catalysts were more active than the previously re-
ported Cu and Pd catalysts supported on Al2O3, and Ir/CeO2
catalyst exhibited extremely high activity. The synergistic effect
between metals and CeO2 might be responsible for the high
catalytic activity. Pretreatment of the catalysts by hydrogen
caused partial reduction of ceria and thus led to the genera-
tion of Ce3+
species on the catalyst surface. This species would
enhance the adsorption of alcohols through the coordination
between the Ce3+
cation and the hydroxyl group, which favors
the dehydrogenation of alcohols. Meanwhile, the in situ re-
moval of hydrogen would take place on the nearby metal par-
ticles through the hydrogenation of styrene.
5.4. Oxidation of hydrocarbons
Partial oxidation of toluene to benzaldehyde via gas phase
process is one of the current challenges in the field of catalysis.
The oxidation of toluene was carried out on Ag1.2V3CeyO8+x cat-
alysts between 360 and 4608C. The catalytic effect of Ce is
mainly to increase the selectivity to benzaldehyde and benzoic
Series of Ce–Mo catalysts have been prepared for the partial
oxidation of toluene to benzaldehyde. The highest yield of
benzaldehyde is obtained when the composition of the ultra-
fine particles reaches the vicinity of Ce/Ce+Mo=0.5, corre-
sponding to a catalyst comprising both CeO2 and Ce2(MoO4)3.
The excess CeO2 works as a promoter by releasing its lattice
oxygen to the oxygen vacant sites formed on the Ce2(MoO4)3
species during reaction.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 665
Ceria-Based Solid Catalysts for Organic Chemistry
A simple and efficient method for the synthesis of 3-nitro-
phthalic acid by the oxidation of 1-nitronaphthalene has been
reported by Rajiah et al. (Scheme 10). Selective oxidation has
been achieved by the one-step reaction of 1-nitronaphthalene
with 5% CeO2/g-Al2O3 catalyst in acetonitrile in presence of
aqueous acid at 908C producing 3-nitrophthalic acid in
80 mol% yield with 98% selectivity.
Elsewhere, the oxidation products of ethylbenzene are
widely used as intermediates in organic chemistry. Various sup-
ported vanadia catalysts exhibit efficient catalytic activity in
the selective oxidation of ethylbenzene using H2O2 in liquid
phase (solvent: acetonitrile), producing essentially acetophe-
none. The oxidation activity of V2O5/CeO2 catalysts could be
correlated to the amount of the vanadia loaded and the struc-
ture of the species. The CeVO4 formation associated with in-
creased concentration of vanadia on ceria is related to the for-
mation of 2-hydroxyacetophenone.
These catalysts were al-
ready used in the partial oxidation of benzene to phenol.
Selective formation of phenol can be attributed to the pres-
ence of highly dispersed active sites of vanadia over the sup-
The hydroxylation of benzene was used also as test reaction
to characterize catalysts, as MxCe1ÀxVO4 (with M=Li, Ca, and
Fe), for the degradation by photocatalysis of different dyes and
organic compounds. This reaction is associated to the oxida-
tion of cyclohexane to produce cyclohexanol and cyclohexa-
none in liquid phase with chloroform as solvent.
Liquid phase oxidation of cyclohexane to cyclohexanol was
carried out under mild reaction conditions over mesoporous
Ce-MCM-41 catalysts using aqueous hydrogen peroxide (30%)
as oxidant and acetic acid as solvent. MCM-41, without the in-
corporation of Ce as a catalyst under the same conditions with
those used for Ce-MCM-41, did not exhibit any significant ac-
tivity. Furthermore, even incorporating other metal ions, such
as, Fe-MCM-41 exhibited significantly lower activity than Ce-
The Ce present in the framework structure of Ce-
MCM-41 can impart dual catalytic activity to the catalyst and
can form labile oxygen vacancies and the relatively high mobi-
lity of bulk oxygen species. A complex with peroxy acetic acid
was possibly formed in the pores of Ce-MCM-41 which is rela-
tively more hydrophobic and stable than hydrogen peroxide.
The synergistic effects among doped cerium, mesoporous
framework of MCM-41, acetic acid and hydrogen peroxide
make Ce-MCM-41 an effective catalyst for the oxidation of cy-
Previously, the hydroxylation of 1-naphthol was
carried out with aqueous H2O2 on this kind of catalysts.
Elsewhere, in cyclohexene and cyclohexanol oxidation with
H2O2 in acetonitrile, the catalytic activity depends on the
cerium amount in Ce-silica mesoporous SBA-15 materials and
metal atom coordination. Thus, in cyclohexene oxidation the
total yield of oxidative products and selectivity of cyclohexene
oxide (epoxy-) increase with the increase of cerium amount up
to 2 wt% and then tend to decrease. Similar correlation is ob-
served in cyclohexanol oxidation. Probably, the surface OH
groups and state of cerium sites influence the catalytic activity
of Ce-SBA-15. Thus, the sorption value of cyclohexene is high
when content and density of SiÀOH groups are low. Cyclohex-
ene is sorbed on the surface coordinatively with unsaturated
(cus) oxygen or on the surface lattice oxygen anion and is
strongly inhibited if ceria is slightly reduced due to the de-
creasing of available (cus) oxygen and surface oxygen species.
Then the cyclohexene adsorption value decreases with increas-
ing of cerium content in Ce-SBA-15.
Ce-SBA-15 catalysts are also active for the oxidative cleavage
of cyclohexene to adipic acid using aqueous H2O2 as oxidant
under solvent-free conditions.
The coordination of cerium
ions in mesoporous materials can affect the catalytic properties
because the incorporation of cerium atoms into the walls of
mesoporous material allows creation of Lewis and Brønsted
acid sites and preparation of materials with various acidi-
The epoxidation of cyclohexene was carried out also in the
presence of Fe/CeO2 catalysts using aqueous hydrogen perox-
ide (30%) as the oxidizing agent.
Direct oxidation of propane to acrolein could be an interest-
ing alternative to propylene oxidation. Bi-Mo based catalysts
have been heavily studied for the selective oxidation (ammoxi-
dation) of propylene to acrolein via acrylonitrile at 5008C. In Bi-
CeVMoO catalysts, bismuth may be substituted by a low
amount of cerium while the structure of BiVMoO remains un-
changing. With the increasing of Ce (Ce/Ce+Bi0.15), new
phases of CeVO4 and Ce2(MoO4)3 formed. The cerium promotes
the forming of acrolein, and the selectivity to acrolein in-
creased to a maximum at Ce/Ce+Bi atomic ratio equal to 0.15
(45 mol% at about 30 mol% propane conversion). Further in-
creasing Ce content results in further oxidation of acrolein to
COx due to the strong oxidative ability of catalysts.
5.5. Oxidative dehydrogenation of hydrocarbons
5.5.1. Dehydrogenation of light paraffins
The dehydrogenation of light paraffins has acquired more im-
portance owing to the growing demand for light olefins such
of light alkanes to alkenes is a highly endothermic reaction,
and conversion is limited by a thermodynamic equilibrium.
Thus, high operating temperatures (500–7508C) are required
to obtain an acceptable level of alkane conversion. Under
these conditions undesirable side reactions, such as hydroge-
nolysis and isomerization, occur with the formation of byprod-
ucts and coke deposits, thus producing catalyst deactivation.
Scheme 10. Synthesis of 3-nitrophthalic acid by oxidation of 1-nitronaphtha-
666 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
The introduction of Zr4+
in a CeO2 lattice leads to significant
variations in the chemical physical features of ceria, and im-
proves the selectivity to isobutene in the oxidative dehydro-
genation of isobutane between 300 and 4008C. This enhance-
ment has been attributed to an increased oxygen mobility and
to an increased activity for the Ce4+
redox couple, occur-
ring as a consequence of the creation of surface and bulk de-
fects in the solid solution.
The dehydrogenation was carried
out at 4508C over cerium oxide in the presence of tetrachloro-
methane to obtain propene, with a selectivity of up to 80%.
Without tetrachloromethane, carbon dioxide is the principal
product. The enhancement of conversion and selectivity to
propene was shown to be dependent upon the presence of
chlorine, in whatever form, in the surface region of the cata-
The Ce–Ni–O catalytic system is active and selective in oxida-
tive dehydrogenation of propane to propene at 3008C. The
yield of propene increased with the increase in the Ni loading
up to a Ni/Ce atomic ratio equal to 1 and decreased at higher
Ceria was also found to be a good support for
chromium oxide catalysts in the oxidative dehydrogenation of
Recently, chromium oxide was supported on
nanometer-sized Ce0.60Zr0.35Y0.05O2 for the same application.
Elsewhere, platinum catalysts have been widely used for
alkane dehydrogenation. Although a wide variety of catalyst
formulations have been reported in the literature, most plati-
num-based catalysts are characterized by the simultaneous
presence of tin. Pt-Sn/Ce-Al2O3 catalysts, with cerium loadings
in the range of 1.1–3.3 wt%, exhibit a highly efficient perfor-
mance for propane dehydrogenation to propylene at 5768C.
The presence of Ce in the Pt-Sn/Ce-Al2O3 catalysts could not
only stabilize the active states of Pt, Sn, and the support, but
could also suppress the coke accumulation on the catalyst
Pt-Sn/20 wt% CeO2–C catalysts, with different Sn/Pt atomic
ratios, showed good performance in the dehydrogenation of
isobutane at 5008C. Cerium plays an important role in activity,
inhibiting tin reduction and maintaining the amount of alloyed
platinum at an adequate level. A catalyst with Sn/Pt=0.5
showed the best isobutene yield.
5.5.2. Dehydrogenation of ethylbenzene
The industrial demand for styrene is growing, and its produc-
tion via dehydrogenation of ethylbenzene is gaining impor-
tance. The reversible conversion of ethylbenzene to styrene
and dihydrogen is highly endothermic: C6H5CH2CH3!C6H5CH=
CH2+H2; DH=125 kJmolÀ1
. Conversion is favored by low pres-
sures and high temperatures. Industrially, the reaction is carried
out over potassium-promoted iron oxide at temperatures rang-
ing from 550 to 6508C and pressures from sub-atmospheric to
2 atm, with a selectivity of about 90% in styrene at a conver-
sion of 50Æ60%. Ceria is a key component of the catalyst for-
mulation for the dehydrogenation of ethylbenzene to sty-
Activated-carbon-supported cerium catalysts (Ce/AC) exhibit
a high styrene yield (about 40%) with over 80% selectivity at
5508C in the presence of carbon dioxide. The dehydrogenation
of ethylbenzene to styrene proceeds via two reaction paths.
One is the simple dehydrogenation and an oxidation reaction
of dihydrogen formed with carbon dioxide (reverse water–gas
shift reaction; CO2+H2!CO+H2O). The other is the oxidative
dehydrogenation of ethylbenzene through the redox cycle.
V2O5-based catalysts supported on ZrO2–SiO2,
doped with CeO2 exhibit high activities in
oxidative dehydrogenation reaction of ethybenzene. Ceria-con-
taining materials suppress catalyst deactivation by preventing
coke formation during the reaction.
Elsewhere, the activity of CeO2–ZrO2/SBA-15 catalyst for the
dehydrogenation of ethylbenzene to styrene in the presence
of CO2 revealed that mesoporous silica SBA-15 is one of the
promising support materials for the development of highly
active and selective CeO2–ZrO2 mixed metal oxide catalysts.
a-Limonene can be easily dehydrogenated to para-cymene,
which is an important starting material for the production of
intermediates such as para-cresol and can also be used in the
manufacturing of fragrances, herbicides, and pharmaceuticals.
Ce-promoted Pd/ZSM5 catalysts gave higher selectivities than
nonpromoted catalysts for the hydroisomerization of a-limo-
nene to para-cymene at 3008C (Scheme 11).[204,205]
A chemical interaction between CeO2 and Pd particles with
very small size exists inside ZSM5 cavities. A bifonctional mech-
anism had been proposed for the conversion of a-limonene.
An acid-catalyzed shift of the double bond from the isopro-
penyl group into the cyclohexene ring is followed by dehydro-
genation on a palladium site.
5.7. Oxidation of aldehydes to acids
Clean aerobic oxidation of various aldehydes to the corre-
sponding carboxylic acid was carried out over Ru–Co(OH)2–
CeO2 (already used in a previously reported study
) at room
temperature, in liquid phase with benzotrifluoride as sol-
The aliphatic and aromatic aldehydes were rapidly
oxygenated. However for allylic aldehydes such as cinnamalde-
hyde, no conversion was observed even at 608C. The authors
proposed a reaction mechanism via a free-radical process:
there was no conversion of octanal in the presence of a radical
Gold supported on nanocrystalline or on meso-structured
nanocrystalline CeO2 supports was also highly active and selec-
Scheme 11. Hydroisomerization of a-limonene to para-cymene.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 667
Ceria-Based Solid Catalysts for Organic Chemistry
tive for the aerobic oxidation of aliphatic and aromatic alde-
hydes at 258C and 508C in liquid phase with acetonitrile as sol-
With this catalyst, the oxidation of cinammaldehyde at
658C was highly selectivite towards carboxylic acid (77.5%) at
moderate conversion (40.7%). The activity was attributed to
the nanometric particle size of Au and CeO2.
5.8. Other oxidation reactions
5.8.1. Oxidation of 2,3-dimØthylphenol
2,6-dimethyl-1,4-benzoquinone is a key intermediate for the
synthesis of a number of medicines and physiologically active
substances such as 2,3,6-trimethyl-para-benzoquinone, an in-
termediate in the industrial production of Vitamin E. The
liquid-phase oxidation of 2,6-dimethylphenol to 2,6-dimethyl-
1,4-benzoquinone (Scheme 12) was carried out at 208C, using
ethanol as solvent and aqueous hydrogen peroxide as a clean
oxidizing agent in the presence of TiO2–CeO2 mixed xero-
The 2,6-dimethylphenol conversion was 100% in 6 h,
and the yields of 2,6-dimethyl-1,4-benzoquinone achieved
were 85–96% when using the TiO2–CeO2 mixed xerogels as
catalysts, while the yield was 49% when a titania catalyst with-
out cerium was used.
Kanta Rao et al. reported on the use of ceria–titania (rutile and
anatase) catalysts for the ammoxidation of 3-methylpyridine or
4-methylpyridine to their corresponding nitriles in gas phase at
4108C (Scheme 13).
The authors noted a marked steric
effect in their reactivity. The best results were obtained on
20% ceria on anatase, showing a 4-methylpyridine conversion
of 89% (37% for 3-methylpyridine) and a selectivity to 4-meth-
ylpyridine of 77% (45% for 3-methylpyridine). The ammoxida-
tion reaction was highly active when the catalysts were synthe-
sized by dispersing ceria on suitable supports. Indeed, interact-
ed CeO2 species of supported catalysts have shown increased
O2 uptakes as well as increased conversions and selectivities in
the ammoxidation reactions.
5.8.3. Dehydrogenation of amines
Au(OAc)3 preadsorbed onto CeO2 was applied as an effective
catalyst of the selective oxidation of dibenzylamine to dibenzy-
limine using molecular oxygen as the only oxidant in the liquid
phase with toluene as solvent (Scheme 14).[210,211]
developed a very simple route for the synthesis of gold cata-
lysts for the oxidation of amines. The catalyst precursor,
Au(OAc)3, and an oxide support, CeO2, were simply added to
the reaction mixture and the active gold nanoparticles on the
support were formed in situ. During the transformation of di-
benzylamine to dibenzylimine; benzonitrile, benzylamine, and
benzaldehyde were formed in amounts of 0.5%, 0.4% and
7.8%, respectively. The latter two byproducts are the result of
the hydrolysis of dibenzylimine with the coproduct water,
while benzonitrile is formed by oxidative dehydrogenation of
benzylamine. The low benzylamine/benzaldehyde ratio can be
explained the coupling and oxidative dehydrogenation of ben-
zylamine to dibenzylimine. The small amount of benzonitrile
indicates that the direct oxidation of benzylamine to benzoni-
trile is very slow.
5.8.4. Oxidation of oximes
Gold supported on ceria (Au/CeO2), usually used in the oxida-
tion of alcohols[152–156]
is a highly active and
selective catalyst for the liquid phase aerobic oxidation of
oximes to the corresponding carboxylic compounds.
ample, for the aerobic oxidation of keto- and aldoximes
(Scheme 15), Au/CeO2 (with 0.72 wt% of Au) in a mixture of
ethanol water (1:1) or toluene is very efficient to produce ace-
tophenone and benzaldehyde (conversion ca. 85–99% with
100% selectivity, except for benzaldehyde in the presence of
water where there was overoxidation of benzaldehyde to ben-
zoic acid). Another, more elaborate catalyst, a core/shell alloy
of gold and palladium supported on nanoparticulated ceria,
Scheme 12. Oxidation of 2,6-dimethylphenol to 2,6-dimethyl-1,4-benzoqui-
Scheme 13. Ammoxidation of 3-methylpyridine or 4-methylpyridine.
Scheme 14. Selective oxidation of dibenzylamine to dibenzylimine.
Scheme 15. Oxidation of keto- and aldoximes.
668 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
was also efficient in toluene (conversion 99%, with a selectivity
of 99%) but the drawback was a difficult preparation.
6. Addition Reactions
6.1. Synthesis of carbonates
The development of environmental processes based on the
utilization of naturally abundant carbon resources such as
carbon dioxide has gained considerable attention in recent
years. Organic carbonate synthesis using carbon dioxide is one
of the promising reactions in this respect. Organic carbonate
compounds have been used as both a reactive intermediate
and an inert solvent.
Dimethyl carbonate (DMC) can be synthesized from epoxide
compounds such as ethylene oxide or propylene oxide by a
two-step reaction (Scheme 16). In the first step the epoxide
reacts with CO2, producing a corresponding cyclic carbonate.
In the second step, the carbonate is transesterified with metha-
nol to DMC and a corresponding glycol.
CeO2 studied with several metal oxide does not appear to
be a good catalyst for this reaction. The basic metal oxide cata-
lysts give high activity and selectivity for the reaction of epox-
ides and CO2 to the corresponding cyclic carbonates and for
the transesterification with methanol. Among the catalysts ex-
amined, MgO is the best catalyst, active for both these two re-
Corma and collaborators
have shown that ceria nanocrys-
tallites are a moderately active catalyst for the transalkylation
of propylene carbonate by methanol. The presence of gold
nanoparticles on ceria in appropriate loading significantly in-
creases the activity and selectivity towards transalkylation.
DMC can be also synthesized by reaction between methanol
and CO2 in the presence of catalysts with acidic and basic
properties such as ZrO2 and CeO2–ZrO2 solid solutions
(Scheme 17). CeO2–ZrO2 catalyst appear to be very effective for
the selective synthesis of DMC from CH3OH and CO2.
Although the selectivity of DMC syntheses over CeO2–ZrO2
catalysts with Ce/(Ce+Zr)=0.2 was very high (100%) under
the employed reaction conditions, unfortunately the methanol
conversion was very low because the equilibrium of the reac-
tion was largely shifted to the left. However, when H2O is re-
moved from the reaction system, it is possible to drastically en-
hance the methanol conversion. H2O removal can be achieved
by reaction with acetals such as 2,2-dimethoxypropane (DMP;
These catalysts are also effective to the direct
synthesis of cyclic carbonate from CO2 and diols such as ethyl-
ene glycol and propylene glycol.[217,218]
The synthesis of DMC from CH3OH and CO2 was investigated
on CeO2 prepared with various kinds of precursors under vari-
ous calcination temperatures. The formation rate of DMC was
almost proportional to the BET surface area of the catalysts.
This suggests that the active site of this reaction is on a stable
crystal surface of CeO2, such as (111).
CeO2 has been reported to catalyze the direct carboxylation
of methanol to dimethylcarbonate. Nevertheless, the catalyst
lifetime was quite short as after the first cycle the activity de-
creased and went to zero after a few cycles. This deactivation
is mainly due to a surface modification produced by the reduc-
tion of CeIV
during catalysis and to crystal conglomera-
tion. The modification of ceria by loading alumina strongly re-
duces the oxidation of methanol and the consequent reduc-
tion of CeIV
, with increase of both the life of the cata-
lysts and their selectivity.[220,221]
6.2. Aldol condensation
Condensation reactions of aldehydes and ketones are widely
used in organic synthesis, mainly because they lead to CÀC
bond formation. These reactions are generally catalyzed by
bases. The condensation over solid bases leads mainly to aldol
or ketol and/or a,b-unsaturated carbonyl compounds.
The aldol condensation of acetone was studied over solid
base catalysts such as Ca(OH)2, La(OH)3, ZrO2, and CeO2 in the
vapor phase between 200 and 4008C. The condensation of
acetone 1 gives diacetone alcohol 2, which is dehydrated to
mesityl oxide 3. Various secondary products are formed by nu-
merous secondary reactions, such as further aldolization and
Michael condensation (Scheme 19). At 200–4008C, 1 over CeO2
led to 74–97% conversion. CeO2 promoted the formation of
1,3,5-trimethylbenzene 7 with a selectivity of 47% at 4008C,
but also produced large amounts of higher condensation
products (38.9% at 3008C). The formation of 7 is favored with
decreasing basic strength. Indeed, the basicity and basic
strength, respectively, of the catalysts decreased in the order
Ca(OH)2 La(OH)3 CeO2 ZrO2.
Reduced CeO2 was observed to be active for the cross-re-
ductive-coupling reaction between acetaldehyde and benzal-
dehyde to form 1-phenylpropene (C6H5ÀCH=CHÀCH3).
Scheme 16. Two-step synthesis of dimethyl carbonate.
Scheme 17. Synthesis of dimethyl carbonate from CH3OH and CO2.
Scheme 18. Reaction of H2O with 2,2-dimethoxypropane.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 669
Ceria-Based Solid Catalysts for Organic Chemistry
Elsewhere, the reaction of acetaldehyde was studied on
CeO2-based catalysts. CeO2 was chosen as support because its
reducibility and basicity favor aldolization reactions.[224,225]
Three CÀC bond formation reactions from acetaldehyde were
observed: aldolization to crotonaldehyde and crotyl alcohol
(more prominent on CeO2 alone), ketonization to acetone, and
reductive coupling to form butenes and butadiene.
4-Methyl-2-pentanone or methylisobutylketone (MIBK) was
synthesized from 2-propanol in one pot on bifonctional metal/
acid–base catalysts. The synthesis of MIBK from 2-propanol in-
volves the dehydrogenation of 2-propanol to acetone which is
converted to mesityl oxide (3, Scheme 19) via an aldol conden-
sation reaction and consecutive dehydration of the aldol inter-
mediate, diacetone alcohol (2, Scheme 19). MO is hydrogenat-
ed on the metallic site to MIBK by H2 generated during 2-prop-
anol dehydrogenation. One of the most selective catalysts for
the formation of MIBK is CuCe4Ox that presents the higher den-
sity of base sites and lower density of acid sites than CuAl16Ox
The aldol condensation/hydrogenation reaction of 2-hexa-
none was carried out over a Pd/CeZrOx catalyst at tempera-
tures between 300 and 4008C, and pressures of 5–26 bar. The
primary product of aldol condensation/hydrogenation is C12
ketone, with the formation of C9 and C18 ketones as secondary
products. The CeZrOx support was selected because it possess-
es a high lattice oxygen mobility and because of its ability to
interact strongly with supported metals.[228,229]
The retro-aldolization of diacetone alcohol (2, Scheme 19) to
acetone was considered as a test reaction that allowed the
semiquantitative assessment of basic centers.
Ceria (and ti-
tania) were found to exhibit considerable activity in the de-
composition of diacetone alcohol.
6.3. Knoevenagel condensation reaction
The Knoevenagel condensation reaction is a cross-aldol reac-
tion between an aldehyde or ketone and an methylene com-
pound, activated by two electron-withdrawing groups, such as
malononitrile, cyanoesters, b-ketoesters or malonates, in the
presence of base. Ceria–zirconia
shows interesting catalytic per-
formances in the Knoevenagel
condensation between benzal-
dehyde and malononitrile
(Scheme 20) with ethanol as a
solvent at 808C.
The direct correlation between
the concentration of acidic sites
and the yield of the products in-
dicated that a higher concentra-
tion of acidic sites gives more
products in the reaction even if
the presence of basic sites re-
mains obligatory. CexZr1ÀxO2 cat-
alysts can be interesting alterna-
tives to soluble bases in view of the following advantages:
(1) high catalytic activity under mild reaction conditions,
(2) easy separation of the catalyst after the reaction, and (3) re-
usability of the catalyst.
6.4. Synthesis of acetals
Besides the interest of acetals as protecting groups of carbonyl
compounds during organic synthesis, many of them have
found direct applications as fragrances in cosmetics, food and
beverage additives, pharmaceuticals, and polymer chemistry.
The synthesis of dimethyl acetals of carbonyl compounds
such as cyclohexanone (Scheme 21), acetophenone or benzo-
phenone has succefully been carried out by the reaction be-
tween ketones and methanol using different solid acid cata-
Among various rare-earths-exchanged Mg–Y zeolites, CeMg–
Y and Ce-montmorillonite were revealed to be the most effi-
cient catalysts for the acetalization reactions. Acetalization of
cyclohexanone reached equilibrium within 60 min and the
yields of acetal were 66.7% with CeMg–Y zeolite and 69.8%
with Ce–montmorillonite. The yields then slightly increased to
Scheme 20. Knoevenagel condensation reaction between benzaldehyde and
Scheme 19. Condensation of acetone and secondary reactions.
Scheme 21. Acetalization of cyclohexanone with methanol.
670 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
80.5% and 98.8% respectively. The Ce3+
cation acted as a
Lewis-acid site and activated the carbonyl group by coordina-
tion, on the order of 1 kJmolÀ1
as measured by FTIR.
6.5. Synthesis of benzimidazole derivatives
Corma and collaborators
have developed an effective strat-
egy for the rapid and efficient one-pot synthesis of benzimida-
zoles involving a new environmentally friendly catalytic proce-
dure. Benzimidazole derivatives were prepared by a four-step
process with gold and/or palladium catalysts and dioxygen
(Scheme 22). The four steps are (1) oxidation of the benzylalco-
hol to benzaldehyde, (2) cyclocondensation of the aldehyde
with ortho-phenylenediamine, (3) oxidation of carbon–nitrogen
bond, and (4) an N-alkylation reaction. The highest activity and
selectivity were achieved when gold was deposited onto CeO2.
With electron-acceptor substituents on the aromatic diamine
the cyclization/oxidation reaction proceeded more slowly and,
accordingly, lower yields of the desired benzimidazole were
obtained. The same effect was observed when the electron-
withdrawing substituent was at the aromatic alcohol. On the
other hand, 1-butanol afforded very poor yields of the corre-
sponding heterocycle provided this aliphatic alcohol hardly
converted to the corresponding aldehydes. In striking contrast
the conjugated alcohol 2-octen-1-ol converted up to 80% to
the corresponding aldehyde but the latter hardly reacted with
the diamine to afford the desired heterocycle.
6.6. Mannich-type reactions
A Mannich-type reaction is an organic reaction that consists of
an amino alkylation of an acidic proton placed next to a car-
bonyl functional group with aldehyde and ammonia or any pri-
mary or secondary amine to lead a b-amino-carbonyl com-
pound. A sulfated CexZr1ÀxO2 catalyst was found to exhibit
solid-super-acidity and good catalytic activity for synthesis of
b-amino ketones by a three-component Mannich-type reaction
in the liquid phase under solvent-free conditions at ambient
temperature. The reaction between benzaldehyde, aniline, and
cyclohexanone (Scheme 23) proceeded in liquid phase (mixture
of reactants) to afford 82% of product, with a d:l ratio of
82:18. The sulfation of ceria-zirconia mixed oxide can lead to
the formation of super-acidic sites in the catalyst, while the un-
promoted ceria-zirconia mixed oxide possesses only a broad
distribution of weak acid sites.
6.7. Biginelli-type reaction
A Biginelli-type reaction is a multiple-component chemical re-
action that creates 3,4-dihydropyrimidin-2(1H)-ones from b-ke-
toesters, aldehydes, and urea. This reaction is generally cata-
lyzed by Brønsted acids and/or by Lewis acids. Thus, the reac-
tion between benzaldehyde, ethyl acetoacetate, and urea
(Scheme 24) was performed in water at 808C for 4.5 h in the
presence of ceria nanoparticles supported on vinylpyridine
polymer, to give 92% of product. The catalyst was recovered
easily and reused without loss of its activity.
6.8. Coupling reactions
Coupling reactions are of particular interest because they are a
powerful and versatile tool in synthetic organic chemistry for
the formation of carbon–carbon bonds. Gold or palladium sup-
ported on CeO2 are active and extremely selective in perform-
ing the homocoupling of arylboronic acids in liquid phase with
toluene as solvent (Scheme 25),[237–239]
cross-coupling reaction of arylboronic acids and arylbromides
in liquid phase with a mixture ethanol water as solvent
and the Sonogashira cross-coupling reaction
of aryliodides and alkynes in N,N-dimethylformamide (DMF) as
solvent (Scheme 27).
Scheme 24. Biginelli-type reaction.
Scheme 25. Homocoupling reaction of phenylboronic acid.
Scheme 22. Synthesis of benzimidazole.
Scheme 23. Mannich-type reaction.
Scheme 26. Cross-coupling reaction of phenylboronic acid and arylbromide.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 671
Ceria-Based Solid Catalysts for Organic Chemistry
The catalytic activity of Au/CeO2 for the homocoupling of ar-
ylboronic acids is directly proportional to the concentration of
surface species, and nanocrystalline CeO2 is able to stabi-
lize surface AuIII
species on the surface.
Under the same re-
action conditions, supported palladium catalysts are less active
than supported gold catalysts.
The palladium catalysts
showed a selectivity of about 75% towards biphenyl with for-
mation of benzene and phenol as byproducts. When support-
ed gold was used for the reaction, a selectivity of 100% to-
wards biphenyl is obtained.
Pd/CeO2 behaves as an efficient catalyst in the Suzuki–
Miyaura coupling reaction starting from aryl bromides with dif-
ferent electronic substituents at room temperature, in air, in an
environmentally friendly solvent such as ethanol/water mix-
By comparison of isoelectronic PdII
on ceria, the authors have found that the latter selectively pro-
motes homocoupling, while the former catalyzes the cross-
Previously, Corma and collaborators have reported that a
Au/CeO2 catalyst, active for performing the Sonogashira cross-
coupling reaction, contains Au0
, and AuIII
cross-coupling reaction was catalyzed by AuI
, while the homo-
coupling reaction was catalyzed by AuIII
7. Substitution Reactions
7.1. Alkylation of aromatic compounds
The alkylation of aromatic rings, called Friedel–Crafts alkylation,
is a reaction of very broad scope. The most important alkylat-
ing reagents are alkyl halides, alcohols, and olefins. These reac-
tions are usually catalyzed by Lewis acids or also by Brønsted
acids. These conventional catalysts are homogeneous and gen-
erate corrosive and nonrecyclable waste, and are thus not en-
vironmentally friendly. The solid catalysts do not exhibit these
were found to exhibit excellent
catalytic activities for the vapor-phase ortho-alkylation of
phenol with methanol[242,243]
and with 1-propanol.
thors speculated that the reaction mechanism of the ortho-pro-
pylation over the CeO2–MgO catalyst proceeds by the perpen-
dicularly adsorption of phenol on weak basic sites on the cata-
lyst. These species are selectively alkylated in ortho position by
1-propanol, which is possibly activated in the form of 1-hy-
droxypropyl radical rather than propyl cation. The redox prop-
erties of Ce4+
are probably attributed with the activation
of 1-propanol to produce 1-hydroxypropyl radical. Moreover,
neither 2-n-propylphenol nor 2-isopropylphenol is produced
during the alkylation of phenol with 2-propanol in the same
conditions. This fact suggests that isopropyl cation cannot be
produced on the CeO2–MgO at temperatures lower than
Sn–Ce–Rh oxide monophase system, already used in ketoni-
zation of esters[83,84]
was found to be an active
and selective catalyst for the ortho-alkylation of phenol with
Elsewhere, alkylation of aromatics compounds
with alcohols or alkenes was performed over cerium modified
microporous materials such as zeolites or silicoaluminophos-
The impregnation of cerium leads to the
deactivation of external acid sites of H-mordenite: the selectivi-
ty of 2,6-diisopropylnaphthalene in the isopropylation of naph-
thalene was enhanced without significant decrease of catalytic
Ceria thereby prevents non-regio-selective reaction
on external surfaces with improvement of the selectivity. Simi-
lar results were observed over various SAPO for the isopropyla-
tion of biphenyl to produce 4,4’-diisopropylbiphenyl,
H-ZSM-5 zeolite for the ethylation of ethylbenzene to 1,4-di-
and over H-mordenite zeolite for the tert-bu-
tylation of toluene to 4-tert-butyltoluene.[250,251]
Ce–Al–MCM-41-type mesoporous silicate materials was
found to exhibit catalytic activities for isopropylation of naph-
and benzylation of toluene.
Both the density
and the strength of the acid sites were considerably higher in
the samples containing both Ce and Al than in the samples
with only one of these substituents.
7.2. Synthesis of coumarins
The synthesis of coumarins that starts from phenol, called the
Pechmann reaction, requires concentrated sulphuric acid as
catalyst and involves corrosion problems. Reddy et al. reported
an efficient method for the preparation of coumarins using sul-
fated CexZr1ÀxO2 solid catalyst under solvent-free conditions at
1208C (Scheme 28).
With 10 wt% of catalyst, the condensa-
tion between activated phenols with alkyl acetoacetate led to
high yields of products (superior to 70%) within a short period
time (shorter than 143 min).
7.3. Synthesis of anisaldehyde
Hydroxymethylation of anisole has been carried out over
SnO2–CeO2 catalysts in the gas phase in the temperature range
Anisaldehyde (methoxybenzaldehyde) and con-
densation products (Scheme 29) were formed, along with
minor quantities of methoxybenzyl alcohol, ortho-cresol,
phenol, and 2,6-xylenol. A maximum anisaldehyde selectivity
of 64% was obtained at 3508C at an anisole conversion of
Scheme 28. Pechmann condensation.
Scheme 27. Cross-coupling reaction of alkyne and aryliodide.
672 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
46%. Catalytic activity was ascribed to the presence of weak
acid sites and redox metal sites. Stronger acid sites lead to the
formation of condensation products.
7.4. Nitration of aromatic compounds
The liquid-phase nitration of toluene was carried out in the
presence of sulphated titania promoted by a ceria catalyst at
ambient temperature and atmospheric pressure without sol-
It is an attractive method for the environmentally
friendly synthesis of nitroaromatic compounds. Moreover, only
mononitrotoluenes were detected in the products, and the
ratio of para-nitrotoluene and ortho-nitrotoluene was approxi-
mately 1:1. A maximum yield of about 11.4% was achieved for
mononitrotoluenes in 3 h with SO4
/TiO2 doped with CeO2
7.5. Acylation of alcohols, amines, or thiols
The acylation of alcohols, amines, phenols, and thiols is an im-
portant and frequently used organic transformation as it not
only provides an efficient and inexpensive route for protecting
hydroxy, amino, phenolic, and thiol groups, but also produces
important organic intermediates in multistep synthetic pro-
cesses that are widely used in the synthesis of fine chemicals,
pharmaceuticals, perfumes, plasticizers, cosmetics, and chemi-
cal auxiliaries. Some of the solid-acid catalysts have been inves-
tigated as potential replacements for mineral acids in the
and ceria–yttria catalysts
were found to
be good catalysts for the acylation of alcohols, amines, and
thiols with acetic anhydride without solvent
or in the pres-
ence of acetonitrile.
Ceria–yttria catalysts exhibit strong
Lewis acid properties.
/ZrO2 promoted by
were also used as superacid catalysts in the esterifica-
tion reactions. The incorporation of Ce into the catalyst was
beneficial to the formation of sole tetragonal ZrO2 and effec-
tively prevented the formation of monoclinic ZrO2, and re-
strained the loss of sulfated species.
The preparation of monoglycerides from fatty acids or fatty
methyl esters and glycerol can be carried out in the presence
of acidic or basic catalysts. The use of solid basic catalysts
could limit secondary reactions leading to product degrada-
tion. A comparison of various basic oxide solids has shown
that the more significant the intrinsic basicity is, the more
active the catalyst is.
The comparison of the catalytic results
between CeO2 and MgO shows that even if they have similar
intrinsic basicity and surface area, their initial activity in this re-
action are different. MgO is the most active solid which could
be due to the presence of stronger basic sites. But the selectiv-
ities to the monoglycerides are similar and only depend on the
The transesterification of b-keto esters has been also studied
in the presence of Lewis acid catalysts as ceria–yttria based
The authors have previously reported the applica-
tion of this catalyst for the acylation reactions.
is also an efficient catalyst for the transesterification of b-keto
esters by a variety of alcohols.
7.7. Oxidative esterification
5-Hydroxymethyl-2-furfural (HMF) has been selectively convert-
ed into 2,5-dimethylfuroate (DMF) (99 mol% yield) under mild
conditions (65–1308C, 10 bar O2) in the absence of any base,
by using gold nanoparticles on nanoparticulated ceria
usually used in oxidation of alcohols.[152–156]
DMF is a valuable biomass derivative that can be used as poly-
mer precursor to replace terephthalate in PET polymers. The
reaction kinetics show that the oxidative pathway encounters
its limiting step for the oxidation of the alcohol to aldehyde.
Once the aldehyde is formed, the corresponding hemiacetal is
obtained, which is rapidly oxidized into the ester.
8. Isomerization or ring opening
8.1. Isomerization of alkanes
Branched alkanes are very important for high-octane gasolines.
They are produced by isomerization of normal paraffins; an
acid-catalyzed chain reaction that is preferably performed at
low temperatures in order to avoid cracking and aromatization
Isomerization of hexane over WOx/CeO2 catalysts leads to
mono- and dialkylated hydrocarbons and methylcyclopen-
In the absence of dihydrogen, a relatively rapid deacti-
vation of the catalysts occurs. The introduction of hydrogen
improves the stability and modifies the selectivity: the mono-
and dialkylated hydrocarbons predominate. In these condi-
tions, the alkenes are less abundant and, consequently, the ac-
tivity is decreased. These results suggest that the key point is
the formation of alkenes. In a first step, an oxidative hydride
abstraction occurs on Lewis sites associated with W=O species,
followed by isomerization either as a cooperative effect on the
Brønsted acid sites created by tungsten, or even on the same
Lewis site from which the hydride ion was abstracted.
Scheme 30. Oxidative esterification of 5-hydroxymethyl-2-furfural into 2,5-di-
Scheme 29. Synthesis of anisaldehyde.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 673
Ceria-Based Solid Catalysts for Organic Chemistry
8.2. Ring opening
The hydrogenolysis of methylcyclobutane (MCB) is a process
that is well-known to be SMSI-sensitive, and is suited for study-
ing the effect of low- and mid-temperature reduction on skele-
tal hydrocarbon reactions. The hydrogenolytic ring opening of
methylcyclobutane occurs easily at 1008C and below on Pt
and Rh nanoparticles supported on CeO2.
At low tempera-
ture and under dihydrogen excess only the ring opening prod-
ucts n-pentane and isopentane are formed. The progressive
loss of activity observed on ceria-supported Pt and Rh catalysts
with low surface areas upon reduction below 4508C is most
likely due to electronic perturbations at the interface between
the metal nanoparticles and the increasingly reduced ceria
In upgrading highly aromatic fractions such as light cycle oil
(LCO) from FCC, the hydrogenation of aromatic compounds
may not always be sufficient to increase the cetane number
and the opening of at least one of the naphthenic rings is nec-
essary. NylØn et al. have shown that ceria appears to be the
best support among several one as Al2O3, SiO2-Al2O3, ZrO2,
MgO and SiO2.[265,266]
The higher activity and selectivity towards
ring opening of indane are obtained with a 2 wt% Pt5Ir95/CeO2
catalyst. The desired products are 2-ethyltoluene and n-propyl-
benzene, when the naphthenic ring has been cleaved only
once. However, consecutive dealkylation occurs irrevocably
and products such as ortho-xylene, ethylbenzene, toluene, ben-
zene, and light products (C6) are formed. This may be attrib-
uted to the electron-deficient character of the metals when
supported on acid materials. The amphoteric properties may
have impact on limiting secondary cracking reactions promot-
ed by solely acid support materials and therefore increasing
the selectivity towards valuable ring-opening products.
8.3. Isomerization of alkenes
The catalytic isomerization of isoprenol by the shifting of
double bond to prenol (Scheme 31) is a process applied in the
large-scale manufacture of solvents, dyes, surface coatings,
paints, and pesticides. Silica-supported palladium catalyst pro-
moted by selenium and cerium (0.5%Pd-0.05%Se-0.3%Ce/SiO2
catalyst) shows higher performance, among a large variety of
prepared catalysts, in the liquid-phase isomerization of isopre-
nol to prenol in the presence of dihydrogen (45% conversion
with 93% selectivity). Addition of cerium improves the disper-
sion of Pd species affecting catalyst activity. Selenium, being
an electronic modifier, is responsible for stabilization of Pdn+
species. This species determines the formation of p-complexes
upon isoprenol adsorption, manifesting extended performance
in the double bond shift and depressing hydrogenation activi-
9. Conclusion and Perspectives
Over the last decade (more than 75% of the references report-
ed in this Review), ceria-based catalysis has demonstrated high
efficiency in a variety of chemical transformations widely used
for the synthesis of fine chemicals and specialties. Convention-
ally, these reactions are carried out with homogeneous cata-
lysts or with stoichiometric reactants, which are not environ-
mentally benign methods. Heterogeneous catalysts should be
preferred to conventional synthesis methods because they
have the advantages of simple removal from the product and
recyclability. They also provide greater selectivity and en-
hanced reaction rates. For these reasons, cerium-based cata-
lysts can contribute to new attempts to develop “clean and
The redox ability and the acid–base properties of CeO2,
either alone or in the presence of transition metals, are impor-
tant parameters that allow to activate complex organic mole-
cules and to selectively orient their transformation.
Pure ceria is used in the dehydration of alcohols, particularly
in the selective dehydration of diols to allylic alcohols, in the
ortho-selective alkylation of aromatic compounds with alco-
hols, in ketone formation through dimerization of esters and
carboxylic acids, in aldolization, in the reduction of carboxylic
acid to aldehydes and of aldehydes to alcohols and in the re-
verse reaction, the dehydrogenation of alcohols, and it is able
to dehydrogenate isobutane to isobutene or ethylbenzene to
The acid–base or redox properties of ceria can be modified
by involving other oxides (ZrO2, La2O3, MnOx, ZnO, MoO4,
V2O5,…), increasing the scope of the reactions. Ceria can also
be supported on polymers for the Biginelli reaction.
Ceria-supported metal catalysts allow the hydrogenation of
C=C, C=O, or CN bonds, the selective hydrogenation of a-b-
unsaturated aldehydes (to unsaturated alcohols), b-keto esters
(to b-hydroxy esters), and fatty esters. They are also used in
coupling reactions or ring opening, in the synthesis of benzi-
midazole, and in the oxidation of oximes. Cerium atoms have
also been added as promoters to catalytic systems or impreg-
nated onto zeolites and mesoporous materials to improve the
performance of these catalysts.
In the near future, the very rich chemistry of cerium oxides
should boost research on new catalysts with better properties
for organic syntheses. The great variety of cerium-based mixed
oxides allows to adjust acid–base and redox properties and to
modulate both the number and strength of active sites for the
desired reaction. New developments in the synthesis of ceria
nanocrystals of controlled shapes (nanorods, nanocubes, poly-
hedras, and others)[268,269]
should also lead to new catalysts
with higher activities and selectivities in organic chemistry and
Scheme 31. Isomerization of isoprenol to prenol.
674 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
The authors thank Mrs. Danile Mesnard, who began this work.
Keywords: cerium · heterogeneous catalysis · hydrogenation ·
oxidation · synthetic methods
 A. Trovarelli, Catalysis by Ceria and Related Materials, Imperial College
Press, London 2002.
 H. C. Yao, Y. F. Yu Yao, J. Catal. 1984, 86, 254.
 S. Rossignol, C. Descorme, C. Kappenstein, D. Duprez, J. Mater. Chem.
2001, 11, 2587.
 H. S. Ghandi, A. G. Piken, M. Shelef, R. G. Deloch, SAE Paper 76020,
 E. C. Su, C. N. Montreuil, W. G. Rothschild, Appl. Catal. 1985, 17, 75–86.
 E. C. Su, W. G. Rothschild, J. Catal. 1986, 99, 506–510.
 B. Engler, E. Koberstein, P. Schubert, Appl. Catal. 1989, 48, 71–92.
 S. Kacimi, J. Barbier Jr, R. Taha, D. Duprez, Catal. Lett. 1993, 22, 343–
 D. Duprez, C. Descorme, T. Birchem, E. Rohart, Top. Catal. 2001, 16–17,
 A. Trovarelli, G. Dolcetti, C. de Leitenburg, J. Kaspar, P. Finetti, A. Santo-
ni, J. Chem. Soc. Faraday Trans. 1992, 88, 1311–1319.
 A. Trovarelli, Catal. Rev. Sci. Eng. 1996, 38, 439–520.
 E. Aneggi, M. Boaro, C. de Leitenburg, G. Dolcetti, A. Trovarelli, J. Alloys
Compd. 2006, 408–412, 1096–1102.
 A. Holmgren, D. Duprez, B. Andersson, J. Catal. 1999, 182, 441–448 .
 M. Ozawa, M. Hattori, T. Yamaguchi, J. Alloys Compd. 2008, 451, 621–
 M. Ozawa, M. Kimura, A. Isogai, J. Alloys Compd. 1993, 193, 73–75.
 A. Fornasiero, R. Di Monte, G. Ranga Rao, J. Kaspar, S. Meriani, A. Tro-
varelli, M. Graziani, J. Catal. 1995, 151, 168–177.
 S. Rossignol, Y. Madier, D. Duprez, Catal. Today 1999, 50, 261–270.
 S. Rossignol, F. Gerard, D. Duprez, J. Mater. Chem. 1999, 9, 1615–1620.
 M. Boaro, C. de Leitenburg, G. Dolcetti, A. Trovarelli, J. Catal. 2000,
 J. Cunningham, D. Cullinane, F. Farell, J. P. O’Driscoll, M. A. Morris, J.
Mater. Chem. 1995, 5, 1027.
 D. Martin, D. Duprez, J. Phys. Chem. 1996, 100, 9429–9438.
 Y. Madier, C. Descorme, A.-M. Le Govic, D. Duprez, J. Phys. Chem. B
1999, 103, 10999–11006.
 M. Che, J. F. J. Kibblewhite, A. J. Tench, M. Dufaux, C. Naccache, J.
Chem. Soc. Faraday Trans. 1 1973, 69, 857–863.
 J. Soria, A. Martínez-Arias, J. C. Conesa, G. Munuera, A. R. Gonzµlez-
Elipe, Surf. Sci. 1991, 251–252, 990–994.
 X. Zhang, K. J. Klabunde, Inorg. Chem. 1992, 31, 1706–1709.
 A. Martínez-Arias, J. Soria, J. C. Conesa, J. Catal. 1997, 168, 364–373.
 A. N. Il’ichev, A. M. Kuli-zade, V. N. Korchak, Kinet. Catal. 2005, 46, 396–
 C. Li, K. Domen, K. Maruya, T. Onishi, J. Chem. Soc. Chem. Commun.
 C. Li, Y. Sakata, T. Arai, K. Domen, K. Maruya, T. Onishi, J. Am. Chem.
Soc. 1989, 111, 7683–7687.
 C. Binet, M. Daturi, J.-C. Lavalley, Catal. Today 1999, 50, 207–225.
 C. Descorme, Y. Madier, D. Duprez, J. Catal. 2000, 196, 167–173.
 D. Duprez, C. Descorme, in Catalysis by Ceria and Related Materials
(Ed.: A. Trovarelli), Imperial College Press, London 2002, pp. 243–280.
 X. Courtois, N. Bion, P. Marecot, D. Duprez, Stud. Surf. Sci. Catal. 2007,
 K. Otsuka, M. Hatano, A. Morikawa, J. Catal. 1983, 79, 493–496.
 C. Padeste, N. W. Cant, D. L. Trimm, Catal. Lett. 1993, 18, 305–316.
 S. Sharma, S Hilaire, J. M. Vohs, R. J. Gorte, H.-W. Jen, J. Catal. 2000,
 F. Sadi, D. Duprez, F. Gerard, A. Miloudi, J. Catal. 2003, 213, 226–234.
 H. Kaneko, T. Miura, H. Ishihara, S. Taku, T. Yokayama, H. Nakajima, Y.
Tamaura, Energy 2007, 32, 656–663.
 D. Martin, D. Duprez, J. Mol. Catal. A: Chem. 1997, 118, 113–128.
 Y. Li, D. He, Q. Zhu, X. Zhang, B. Xu, J. Catal. 2004, 221, 584–593.
 M. G. Cutrufello, I. Ferino, V. Solinas, A. Primavera, A. Trovarelli, A.
Auroux, C. Picciau, Phys. Chem. Chem. Phys. 1999, 1, 3369–3375.
 M. G. Cutrufello, I. Ferino, R. Monaci, E. Rombi, V. Solinas, Top. Catal.
2002, 19, 225–240.
 V. Solinas, E. Rombi, I. Ferino, M. G. Cutrufello, G. Colón, J. A. Navío, J.
Mol. Catal. A: Chem. 2003, 204–205, 629–635.
 M. G. Cutrufello, I. Ferino, R. Monaci, E. Rombi, G. Colón, J. A. Navío,
Phys. Chem. Chem. Phys. 2001, 3, 2928–2934.
 M. G. Cutrufello, I. Ferino, E. Rombi, V. Solinas, G. Colón, J. A. Navío,
React. Kinet. Catal. Lett. 2003, 79, 93–94.
 B. M. Reddy, P. Lakshmanan, P. Bharali, P. Saikia, J. Mol. Catal. A: Chem.
2006, 258, 355–360.
 B. M. Reddy, G. Thrimurthulu, P. Saikia, P. Bharali, J. Mol. Catal. A: Chem.
2007, 275, 167–173.
 B. M. Reddy, G. K. Reddy, L. Katta, J. Mol. Catal. A: Chem. 2009, 297–
 S. Bernal, J. M. Trillo, J. Catal. 1980, 66, 184–190.
 S. Sato, R. Takahashi, T. Sodesawa, N. Honda, H. Shimizu, Catal.
Commun. 2003, 4, 77–81.
 S. Sato, R. Takahashi, T. Sodesawa, N. Honda, J. Mol. Catal. A: Chem.
2004, 221, 177–183.
 N. Ichikawa, S. Sato, R. Takahashi, T. Sodesawa, J. Mol. Catal. A: Chem.
2005, 231, 181–189.
 A. Igarashi, N. Ichikawa, S. Sato, R. Takahashi, T. Sodesawa, Appl. Catal.
A: Gen. 2006, 300, 50–57.
 N. Ichikawa, S. Sato, R. Takahashi, T. Sodesawa, H. Fujita, T. Atoguchi, A.
Shiga, J. Catal. 2006, 239, 13–22.
 S. Sato, R. Takahashi, T. Sodesawa, A. Igarashi, H. Inoue, Appl. Catal. A:
Gen. 2007, 328, 109–116.
 M. Kobune, S. Sato, R. Takahashi, J. Mol. Catal. A: Chem. 2008, 279, 10–
 S. Sato, R. Takahashi, T. Sodesawa, N. Yamamoto, Catal. Commun.
2004, 5, 397–400.
 S. Sato, R. Takahashi, M. Kobune, H. Inoue, Y. Izawa, H. Ohno, K. Takaha-
shi, Appl. Catal. A: Gen. 2009, 356, 64–71.
 S. Sato, R. Takahashi, N. Yamamoto, E. Kaneko, H. Inoue, Appl. Catal. A:
Gen. 2008, 334, 84–91.
 S. Sato, M. Akiyama, R. Takahashi, T. Hara, K. Inui, M. Yokota, Appl.
Catal. A: Gen. 2008, 347, 186–191.
 N. Ichikawa, S. Sato, R. Takahashi, T. Sodesawa, Catal. Commun. 2005,
 M. Glinski, J. Kijenski , A. Jakubowski, Appl. Catal. A: Gen. 1995, 128,
 I. Furuoya, Catal. Surv. Jpn. 1999, 3, 71–73.
 M. Glinski, J. Kijenski, React. Kinet. Catal. Lett. 2000, 69, 123–128.
 M. Glinski, J. Kijenski, Appl. Catal. A: Gen. 2000, 190, 87–91.
 S. D. Randery, J. S. Warren, K. M. Dooley, Appl. Catal. A: Gen. 2002, 226,
 T. S. Hendren, K. M. Dooley, Catal. Today 2003, 85, 333–351.
 O. Nagashima, S. Sato, R. Takahashi, T. Sodesawa, J. Mol. Catal. A:
Chem. 2005, 227, 231–239.
 K. M. Dooley, A. K. Bhat, C. P. Plaisance, A. D. Roy, Appl. Catal. A: Gen.
2007, 320, 122–133.
 M. Glinski, A. Koziol, D. Lomot, Z. Kaszkur, Appl. Catal. A: Gen. 2007,
 F. Wattimena, Eur. Pat., EP 85996, 1983.
 W. Kleine-Homann, Ger. Offen, DE 3709765, 1988.
 K. Nakaji, Jpn Kokai Tokkyo Koho, JP 01179951, 1989.
 J. Warren, D. Westphal, S. Zoubeck, PTC Int. Appl., WO 2002078447,
 M. A. Hasan, M. I. Zaki, L. Pasupulety, Appl. Catal. A: Gen. 2003, 243,
 J. Stubenrauch, E. Brosha, J. M. Vohs, Catal. Today 1996, 28, 431–441.
 C. A. Gaertner, J. C. Serrano-Ruiz, D. J. Braden, J. A. Dumesic, J. Catal.
2009, 266, 71–78.
 E. L. Kunkes, D. A. Simonetti, R. M. West, J. C. Serrano-Ruiz, C. A. Gärt-
ner, J. A. Dumesic, Science 2008, 322, 417–421.
 M. Glinski, M. Kaszubski, React. Kinet. Catal. Lett. 2000, 70, 271–274.
 M. Glinski, J. Szudybill, React. Kinet. Catal. Lett. 2002, 77, 335–340.
 M. Glinski, W. Szymanski, D. Lomot, Appl. Catal. A: Gen. 2005, 281,
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 675
Ceria-Based Solid Catalysts for Organic Chemistry
 O. Nagashima, S. Sato, R. Takahashi, T. Sodesawa, T. Akashi, Appl. Catal.
A: Gen. 2006, 312, 175–180.
 R. Klimkiewicz, H. Tererycz, H. grabowska, I. Morawski, L. Syper, B. W.
Licnerski, J. Am. Oil Chem. Soc. 2001, 78, 533–535.
 R. Klimkiewicz, H. Teterycza, React. Kinet. Catal. Lett. 2002, 75, 165–
 S. Sato, R. Takahashi, T. Sodesawa, K. Matsumoto, Y. Kamimura, J. Catal.
1999, 184, 180–188.
 N. Plint, D. Ghavalas, T. Vally, V. D. Sokolovski, N. J. Coville, Catal. Today
1999, 49, 71–77.
 N. D. Plint, N. J. Coville, D. Lack, G. L. Nattrass, T. Vallay, J. Mol. Catal. A:
Chem. 2001, 165, 275–281.
 Y. Kamimura, S. Sato, R. Takahashi, T. Sodesawa, T. Akashi, Appl. Catal.
A: Gen. 2003, 252, 399–410.
 T. Akashi, S. Sato, R. Takahashi, T. Sodesawa, K. Inui, Catal. Commun.
2003, 4, 411–416.
 H. Teterycz, R. Klimkiewicz, B. W. Licznerski, Appl. Catal. A: Gen. 2001,
 H. Teterycz, R. Klimkiewicz, M. Laniecki, Appl. Catal. A: Gen. 2004, 274,
 S. Scir, S. Minicò, C. Crisafulli, Appl. Catal. A: Gen. 2002, 235, 21–31.
 M. Watanabe, M. Osada, H. Inomata, K. Arai, A. Kruse, Appl. Catal. A:
Gen. 2003, 245, 333–341.
 J. Liu, H. Li, H. Li, Chin. J. Catal. 2007, 28, 312–316.
 H. Li, J. Liu, H. Li, Mater. Lett. 2008, 62, 297–300.
 R. de Souza Monteiro, F. Bellot Noronha, L. Chaloub Dieguez, M.
Schmal, Appl. Catal. A: Gen. 1995, 131, 89–106.
 X. Shuzhang, L. Zhiying, Z. Guoguang, X. Zuhui, Chem. J. Internet 2004,
6, P3, http://www.chemistrymag.org/cji/2004/.
 J. Badalo Branco, D. Ballivet-Tkatchenko, A. Pires de Matos, J. Alloys
Compd. J. Alloys Compounds 2008, 464, 399–406.
 B. Nohair, C. Especel, G. Lafaye, P. MarØcot, L. C. Hoang, J. Barbier, J.
Mol. Catal. A: Chem. 2005, 229, 117–126.
 Y. Azizi, C. Petit, V. Pitchon, J. Catal. 2008, 256, 338–344.
 J. Barrault, A. Alouche, V. Paul-Boncour, L. Hilaire, A. Percheron-
Guegan, Appl. Catal. 1989, 46, 269–279.
 F. Fajardie, J.-F. Tempre, G. DjØga-Mariadassou, G. Blanchard, J. Catal.
1996, 163, 77–86.
 S. Chettibi, R. Wojcieszak, E. H. Boudjennad, J. Belloni, M. M. Bettahar,
N. Keghouche, Catal. Today 2006, 113, 157–165.
 C. Fontaine-Gautrelet, J.-M. Krafft, G. DjØga-Mariadassou, C. Thomas, J.
Catal. 2007, 247, 34–42.
 P. daCosta Zonetti, R. Landers, A. J. Gomez Cobo, Appl. Surf. Sci. 2008,
 J.-L. Liu, L.- J. Zhu, Y. Pei, J.-H. Zhuang, H. Li, H.-X. Li, M.-H. Qiao, K.-N.
Fan, Appl. Catal. A: Gen. 2009, 353, 282–287.
 P. CastaÇo, T. A. Zepeda, B. Pawelec, M. Makkee, J. L. G. Fierro, J. Catal.
2009, 267, 30–39.
 M. Abid, R. Touroude, Catal. Lett. 2000, 69, 139–144.
 M. Abid, G. Ehret, R. Touroude, Appl. Catal. A: Gen. 2001, 217, 219–
 M. Abid, V. Paul-Boncour, R. Touroude, Appl. Catal. A: Gen. 2006, 297,
 A. Sepﬄlveda-Escribano, F. Coloma, F. Rodríguez-Reinoso, J. Catal. 1998,
 A. Sepﬄlveda-Escribano, J. Silvestre-Albero, F. Coloma, F. Rodríguez-Re-
inoso, Stud. Surf. Sci. Catal. 2000, 130, 1013–1018.
 J. Silvestre-Albero, F. Rodríguez-Reinoso, A. Sepﬄlveda-Escribano, J.
Catal. 2002, 210, 127–136.
 J. Silvestre-Albero, A. Sepﬄlveda-Escribano, F. Rodríguez-Reinoso, J. A.
Anderson, Phys. Chem. Chem. Phys. 2003, 5, 208–216.
 J. Silvestre-Albero, F. Coloma, A. Sepﬄlveda-Escribano, F. Rodríguez-Re-
inoso, Appl. Catal. A: Gen. 2006, 304, 159–167.
 J. C. Serrano-Ruiz, J. Luettich, A. Sepﬄlveda-Escribano, F. Rodríguez-Re-
inoso, J. Catal. 2006, 241, 45–55.
 J. C. Serrano-Ruiz, G. W. Huber, M. A. Sµnchez-Castillo, J. A. Dumesic, F.
Rodríguez-Reinoso, A. Sepﬄlveda-Escribano, J. Catal. 2006, 241, 378–
 P. Concepción, A. Corma, J. Silvestre-Albero, V. Franco, J. Y. Chane-
Ching, J. Am. Chem. Soc. 2004, 126, 5523–5532.
 R. Malathi, R. P. Viswanath, Appl. Catal. A: Gen. 2001, 208, 323–327.
 J. C. Serrano-Ruiz, A. Sepﬄlveda-Escribano, F. Rodríguez-Reinoso, D.
Duprez, J. Mol. Catal. A: Chem. 2007, 268, 227–234.
 J. Barrault, A. Derouault, O. Martin, S. Pronier, C. R. Acad. Sci. Paris, T. 2,
SØrie II c 1999, 507–517.
 B. Bachiller-Baeza, I. Rodríguez-Ramos, A. Guerrero-Ruiz, Appl. Catal. A:
Gen. 2001, 205, 227–237.
 B. Campo, M. Volpe, S. Ivanova, R. Touroude, J. Catal. 2006, 242, 162–
 B. Campo, C. Petit, M. A. Volpe, J. Catal. 2008, 254, 71–78.
 B. C. Campo, S. Ivanova, C. Gigola, C. Petit, M. A. Volpe, Catal. Today
2008, 133–135, 661–666.
 B. Campo, G. Santori, C. Petit, M. Volpe, Appl. Catal. A: Gen. 2009, 359,
 E. Leclercq, A. Rives, E. Payen, R. Hubaut, Appl. Catal. A: Gen. 1998,
 T. Marzialetti, J. L. G. Fierro, P. Reyes, Catal. Today 2005, 107–108, 235–
 Y. Sakata, C. A. van Tol-Koutstaal, V. Ponecz, J. Catal. 1997, 169, 13–21.
 Y. Sakata, V. Ponec, Appl. Catal. A: Gen. 1998, 166, 173–184.
 T. Yokoyama, N. Yamagata, Appl. Catal. A: Gen. 2001, 221, 227–239.
 M. Chong, D.-G. Cheng, L. Liu, F. Chen, X. Zhan, Catal. Lett. 2007, 114
 D.-G. Cheng, M. Chong, F. Chen, X. Zhan, Catal. Lett. 2008, 120, 82–85.
 D.-G. Cheng, C. Hou, F. Chen, X. Zhan, J. Rare Earths 2009, 27, 723–
 D. D. Haffad, U. Kameswari, M. M. Bettahar, A. Chambellan, J. C. Laval-
ley, J. Catal. 1997, 172, 85–92.
 A. Saadi, Z. Rassoul, M. M. Bettahar, J. Mol. Catal. A: Chem. 2000, 164,
 A. Saadi, R. Merabti, Z. Rassoul, M. M. Bettahar, J. Mol. Catal. A: Chem.
2006, 253, 79–85.
 H. Li, S. Zhang, H. Luo, Mater. Lett. 2004, 58, 2741–2746.
 S. M. dos Santos, A. M. Silva, E. Jord¼o, M. A. Fraga, Catal. Today 2005,
 B. Gopal Mishra, G. Ranga Rao, B. Poongodi, Proc. Ind. Acad. Sci. (Chem.
Sci.) 2003, 115, 561–571.
 G. Ranga Rao, H. R. Sahu, B. Gopal Mishra, React. Kinet. Catal. Lett.
2003, 78, 151–159.
 B. Gopal Mishra, G. Ranga Rao, J. Mol. Catal. A: Chem. 2006, 243, 204–
 N. Iwasa, M. Yoshikawa, M. Arai, Phys. Chem. Chem. Phys. 2002, 4,
 J. Badalo Branco, D. Ballivet-Tkatchenko, A. Pires de Matos, J. Phys.
Chem. C 2007, 111, 15084–15088.
 J. Badalo Branco, D. Ballivet-Tkatchenkob, A. Pires de Matosa, J. Mol.
Catal. A: Chem. 2009, 307, 37–42.
 K. N. Rao, B. M. Reddy, S.-E. Park, Catal. Commun. 2009, 11, 142–145.
 R. Oi, S. Takenaka, Chem. Lett. 1988, 1115–1116.
 A. Yee, S. J. Morrison, H. Idriss, J. Catal. 1999, 186, 279–295.
 H. Ji, T. Mizugaki, K. Ebitani, K. Kaneda, Tetrahedron Lett. 2002, 43,
 K. Ebitani, H.-B. Ji, T. Mizugaki, K. Kaneda, J. Mol. Catal. A: Chem. 2004,
 D. I. Enache, D. W. Knight, G. J. Hutchings, Catal. Lett. 2005, 103, 43–
 A. Abad, P. Concepción, A. Corma, H. García, Angew. Chem. 2005, 117,
4134–4137; Angew. Chem. Int. Ed. 2005, 44, 4066–4069.
 A. Abad, C. Almela, A. Corma, H. García, Tetrahedron 2006, 62, 6666–
 A. Abad, C. Almela, A. Corma, H. García, Chem. Commun. 2006, 3178–
 A. Abad, A. Corma, H. García, Pure Appl. Chem. 2007, 79, 1847–1854.
 A. Abad, A. Corma, H. García, Chem. Eur. J. 2008, 14, 212–222.
 P. Haider, J.-D. Grunwaldt, R. Seidel, A. Baiker, J. Catal. 2007, 250, 313–
 P. Haider, B. Kimmerle, F. Krumeich, W. Kleist, J.-D. Grunwaldt, A. Baiker,
Catal. Lett. 2008, 125, 169–176.
 P. Haider, A. Urakawa, E. Schmidt, A. Baiker, J. Mol. Catal. A: Chem.
2009, 305, 161–169.
 S. Miao, Z. Liu, Z. Miao, B. Han, K. Ding, G. An, Y. Xie, Microporous Mes-
oporous Mater. 2009, 117, 386–390.
676 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez
 T. Sato, T. Komanoya, Catal. Commun. 2009, 10, 1095–1098.
 M. P. Che˛cin´ski, A. Brückner, J. Radnik, A. Kçckritz, Appl. Catal. A: Gen.
2009, 366, 212–219.
 M. J. Beier, T. W. Hansen, J.-D. Grunwaldt, J. Catal. 2009, 266, 320–330.
 M. Zaki, N. Sheppard, J. Catal. 1983, 80, 114–122.
 E. Iglesia, D. G. Barton, J. A. Biscardi, M. J. L. Gines, S. L. Soled, Catal.
Today 1997, 38, 339–360.
 B. Gopal Mishra, G. Ranga Rao, Bull. Mater. Sci. 2002, 25, 155–162.
 F. Jose, S. Sugunan, React. Kinet. Catal. Lett. 2006, 89, 261–267.
 M. I. Zaki, G. A. M. Hussein, H. A. El-Ammawy, S. A. A. Mansour, J. Polz,
H. Knçzinger, J. Mol. Catal. 1990, 57, 367–378.
 D. Haffad, A. Chambellan, J. C. Lavalley, J. Mol. Catal. A: Chem. 2001,
 M. Watanabe, T. Iida, Y. Aizawa, H. Ura, H. Inomata, K. Arai, Green
Chem. 2003, 5, 539–544.
 I. Kvande, D. Chen, M. Rønning, H. J. Venvik, A. Holmen, Catal. Today
2005, 100, 391–395.
 N. R. E. Radwan, H. G. El-Shobaky, S. A. El-Molla, Appl. Catal. A: Gen.
2006, 297, 31–39.
 M. I. Domínguez, M. Sµnchez, M. A. Centeno, M. Montes, J. A. Odriozo-
la, J. Mol. Catal. A: Chem. 2007, 277, 145–154.
 J. R. Sohn, S. H. Lee, J. S. Lim, Catal. Today 2006, 116, 143–150.
 J. R. Sohn, D. C. Shin, Bull. Korean Chem. Soc. 2007, 28, 1265–1272.
 S. Wei, S. Ruijuan, L. Junlong, Z. Ensheng, L. Zhanshuang, X. Yide, S.
Wenjie, Chin. J. Catal. 2007, 28, 106–108.
 Z.-G. Yan, S. L. T. Andersson, J. Catal. 1991, 131, 350–368.
 W. Kuang, Y. Fan, Y. Chen, Catal. Today 2001, 68, 75–82.
 T. Rajiah, K. V. R. Chary, K. Sita Rama Rao, R. Nageswara Rao, R. Prasad,
Green Chem. 2002, 4, 210–212.
 T. Radhika, S. Sugunan, Catal. Commun. 2007, 8, 150–156.
 T. Radhika, S. Sugunan, J. Mol. Catal. A: Chem. 2006, 250, 169–176.
 S. Mahapatra, R. Vinu, D. Saha, T. N. Guru Rowa, G. Madras, Appl. Catal.
A: Gen. 2009, 361, 32–41.
 W. Yao, Y. Chen, L. Min, H. Fang, Z. Yan, H. Wang, J. Wang, J. Mol. Catal.
A: Chem. 2006, 246, 162–166.
 S. C. Laha, P. Mukherjee, S. R. Sainkar, R. Kumar, J. Catal. 2002, 207,
 M. N. Timofeeva, S. H. Jhung, Y. K. Hwang, D. K. Kim, V. N. Panchenko,
M. S. Melgunov, Yu. A. Chesalov, J.-S. Chang, Appl. Catal. A: Gen. 2007,
 M. N. Timofeeva, O. A. Kholdeeva, S. H. Jhung, J.-S. Chang, Appl. Catal.
A: Gen. 2008, 345, 195–200.
 A. S. Reddy, C.-Y. Chena, C.-C. Chen, S.-H. Chien, C.-J. Lin, K.-H. Lin, C.-
L. Chene, S.-C. Changa, J. Mol. Catal. A: Chem. 2010, 318, 60–67.
 H. Yang, Y. Fan, J. Wu, Y. Chen, J. Mol. Catal. A: Chem. 2005, 227, 279–
 S. Sugiyama, Y. Iizuka, E. Nitta, H. Hayashi, J. B. Moffat, J. Catal. 2000,
 P. Boizumault-Moriceau, A. Pennequin, B. Grzybowskab, Y. Barbaux,
Appl. Catal. A: Gen. 2003, 45, 55–67.
 C. Yu, Q. Ge, H. Xu, W. Li, Appl. Catal. A: Gen. 2006, 315, 58–67.
 C. de Leitenburg, A. Trovarelli, J. Llorca, F. Cavani, G. Bini, Appl. Catal.
A: Gen. 1996, 139, 161–173.
 P. Moriceau, B. Grzybowskaa, Y. Barbaux, G. Wrobel, G. Hecquet, Appl.
Catal. A: Gen. 1998, 168, 269–277.
 P. Moriceau, B. Grzybowska, L. Gengembre, Y. Barbaux, Appl. Catal. A:
Gen. 2000, 199, 73–82.
 J. C. Serrano-Ruiz, A. Sepﬄlveda-Escribano, F. Rodríguez-Reinoso, J.
Catal. 2007, 246, 158–165.
 G. Wang, H. Dai, L. Zhang, J. Deng, C. Liu, H. He, C. Tong Au, Appl.
Catal. A: Gen. 2010, 375, 272–278.
 A. Trovarelli, C. de Leitenburg, M. Boaro, G. Dolcetti, Catal. Today 1999,
 N. Ikenaga, T. Tsuruda, K. Senma, T. Yamaguchi, Y. Sakurai, T. Suzuki,
Ind. Eng. Chem. Res. 2000, 39, 1228–1234.
 B. M. Reddy, P. Lakshmanan, S. Loridant, Y. Yamada, T. Kobayashi, C.
López-Cartes, T. C. Rojas, A. Fernµndez, J. Phys. Chem. B 2006, 110,
 B. M. Reddy, K. Rao, G. K. Reddy, A. Khan, S.-E. Park, J. Phys. Chem. B
2007, 111, 11546–11553.
 B. M. Reddy, S.-C. Lee, D.-S. Han, S.-E. Park, Appl. Catal. B: Environm.
2009, 87, 230–238.
 K. N. Rao, B. M. Reddy, B. Abhishek, Y.-H. Seob, N. Jiang, S.-E. Park,
Appl. Catal. B: Environm. 2009, 91, 649–656.
 D. Raju Burri, K.-M. Choi, J.-H. Lee, D.-S. Han, S.-E. Park, Catal. Commun.
2007, 8, 43–48.
 P. A. Weyrich, W. F. Hçlderich, Appl. Catal. A: Gen. 1997, 158, 145–162.
 P. A. Weyrich, H. Trevifio, W. F. Hçlderich, W. M. H. Sachtler, Appl. Catal.
A: Gen. 1997, 163, 31–44.
 H. B. Ji, D. G. He, J. Song, Y. Qian, Chin. Chem. Lett. 2004, 15, 1241–
 A. Corma, M. E. Domine, Chem. Commun. 2005, 4042–4044.
 M. Palacio, P. I. Villabrille, G. P. Romanelli, P. G. Vµzquez, C. V. Cµceres,
Appl. Catal. A: Gen. 2009, 359, 62–68.
 P. Kanta Rao, K. S. Rama Rao, S. Khaja Masthan, K. V. Narayana, T.
Rajiah, V. Venkat Rao, Appl. Catal. A: Gen. 1997, 163, 123–127.
 L. Aschwanden, T. Mallat, J.-D. Grunwaldt, F. Krumeich, A. Baiker, J. Mol.
Catal. A: Chem. 2009, 300, 111–115.
 L. Aschwanden, T. Mallat, F. Krumeich, A. Baiker, J. Mol. Catal. A: Chem.
2009, 309, 57–62.
 A. Grirrane, A. Corma, H. Garcia, J. Catal. 2009, 268, 350–355.
 B. M. Bhanage, S.-I. Fujita, Y. Ikushima, M. Arai, Appl. Catal. A: Gen.
2001, 219, 259–266.
 R. Juµrez, A. Corma, H. García, Green Chem. 2009, 11, 949–952.
 K. Tomishige, Y. Furusawa, Y. Ikeda, M. Asadullah, K. Fujimoto, Catal.
Lett. 2001, 76, 71–74.
 K. Tomishige, K. Kunimori, Appl. Catal. A: Gen. 2002, 237, 103–109.
 K. Tomishige, H. Yasuda, Y. Yoshida, M. Nurunnabi, B. Li, K. Kunimori,
Catal. Lett. 2004, 95, 45–49.
 K. Tomishige, H. Yasuda, Y. Yoshida, M. Nurunnabi, B. Li, K. Kunimori,
Green Chem. 2004, 6, 206–214.
 Y. Yoshida, Y. Arai, S. Kado, K. Kunimori, K. Tomishige, Catal. Today
2006, 115, 95–101.
 M. Aresta, A. Dibenedetto, C. Pastore, C. Cuocci, B. Aresta, S. Cometa,
E. De Gigli, Catal. Today 2008, 137, 125–131.
 M. Aresta, A. Dibenedetto, C. Pastore, A. Angelini, B. Aresta, I. Pµpai, J.
Catal. 2010, 269, 44–52.
 S. Lippert, W. Baumann, K. Thomke, J. Mol. Catal. 1991, 69, 199–214.
 H. Idriss, M. Libby, M. A. Barteau, Catal. Lett. 1992, 15, 13–23.
 H. Idriss, C. Diagne, J. P. Hindermann, A. Kiennemann, M. A. Marteau, J.
Catal. 1995, 155, 219–237.
 J. Raskó, J. Kiss, Appl. Catal. A: Gen. 2005, 287, 252–260.
 J. I. Di Cosimo, G. Torres, C. R. Apesteguía, J. Catal. 2002, 208, 114–123.
 G. Torres, C. R. Apesteguıµ, J. I. Di Cosimo, Appl. Catal. A: Gen. 2007,
 E. L. Kunkes, E. I. Gürbüz, J. A. Dumesic, J. Catal. 2009, 266, 236–249.
 E. I. Gürbüz, E. L. Kunkes, J. A. Dumesic, Appl. Catal. B: Environm. 2010,
 P. Haider, J.-D. Grunwaldt, A. Baiker, Catal. Today 2009, 141, 349–354.
 G. Postole, B. Chowdhury, B. Karmakar, K. Pinki, J. Banerji, A. Auroux, J.
Catal. 2010, 269, 110–121.
 B. Thomas, S. Prathapan, S. Sugunan, Microporous Mesoporous Mater.
2005, 80, 65–72.
 J.-I. Tateiwa, H. Horiuchi, S. Uemura, J. Org. Chem. 1995, 60, 4039–
 V. R. Ruiz, A. Corma, M. J. Sabater, Tetrahedron 2010, 66, 730–735.
 B. M. Reddy, P. M. Sreekanth, P. Lakshmanan, A. Khan, J. Mol. Catal. A:
Chem. 2006, 244, 1–7.
 G. Sabitha, K. Baskar Reddy, J. S. Yadav, D. Shailajab, K. Samba Sivudub,
Tetrahedron Lett. 2005, 46, 8221–8224.
 S. Carrettin, J. Guzman, A. Corma, Angew. Chem. 2005, 117, 2282–
2285; Angew. Chem. Int. Ed. 2005, 44, 2242–2245.
 S. Carrettin, A. Corma, M. Iglesias, F. Sµnchez, Appl. Catal. A: Gen. 2005,
 N. G. Willis, J. Guzman, Appl. Catal. A: Gen. 2008, 339, 68–75.
 F. Amoroso, S. Colussi, A. Del Zotto, J. Llorca, A. Trovarelli, J. Mol. Catal.
A: Chem. 2010, 315, 197–204.
 C. Gonzµlez-Arellano, A. Abad, A. Corma, H. García, M. Iglesias, F.
Sµnchez, Angew. Chem. 2007, 119, 1558–1560; Angew. Chem. Int. Ed.
2007, 46, 1536–1538.
 S. Sato, K. Koizumi, F. Nozaki, Appl. Catal. A: Gen. 1995, 133, L7L10.
ChemSusChem 2010, 3, 654 – 678 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim www.chemsuschem.org 677
Ceria-Based Solid Catalysts for Organic Chemistry
 S. Sato, K. Koizumi, F. Nozaki, J. Catal. 1998, 178, 264–274.
 R. Klimkiewicz, H. Grabowskaa, H. Teterycz, Appl. Catal. A: Gen. 2003,
 J.-H. Kim, Y. Sugi, T. Matsuzaki, T. Hanaoka, Y. Kubota, X. Tu, M. Matsu-
moto, S. Nakata, A. Kato, G. Seo, C. Pak, Appl. Catal. A: Gen. 1995, 131,
 S. Tawada, Y. Sugi, Y. Kubota, Y. Imada, T. Hanaoka, T. Matsuzaki, K. Na-
kajima, K. Kunimor, J.-H. Kim, Catal. Today 2000, 60, 243–253.
 M. Bandyopadhyay, R. Bandyopadhyay, S. Tawada, Y. Kubota, Y. Sugi,
Appl. Catal. A: Gen. 2002, 225, 51–62.
 S. Barman, S. K. Maity, N. C. Pradhan, Chem. Eng. J. 2005, 114, 39–45.
 Y. Sugi, Y. Kubota, K. Komura, N. Sugiyama, M. Hayashi, J.-H. Kim, G.
Seo, Appl. Catal. A: Gen. 2006, 299, 157–166.
 G. Kostrab, D. Mravec, M. Bajus, I. Janotka, Y. Sugi, S. J. Cho, J. H. Kim,
Appl. Catal. A: Gen. 2006, 299, 122–130.
 G. Kostrab, M. Lovicˇ, I. Janotka, M. Bajus, D. Mravec, Appl. Catal. A:
Gen. 2007, 323, 210–218.
 M. D. Kadgaonkar, S. C. Laha, R. K. Pandey, P. Kumar, S. P. Mirajkar, R.
Kumar, Catal. Today 2004, 97, 225–231.
 P. Kalita, N. M. Gupta, R. Kumar, J. Catal. 2007, 245, 338–347.
 B. M. Reddy, M. K. Patil, P. Lakshmanan, J. Mol. Catal. A: Chem. 2006,
 T. M. Jyothi, M. B. Talawar, B. S. Rao, Catal. Lett. 2000, 64, 151–155.
 W. Mao, H. Ma, B. Wang, J. Hazard. Mater. 2009, 167, 707–712.
 R. K. Pandey, S. P. Dagade, K. M. Malase, S. B. Songire, P. Kumara, J. Mol.
Catal. A: Chem. 2006, 245, 255–259.
 G. Fan, M. Shen, Z. Zhang, F. Jia, J. Rare Earths 2009, 27, 437–442.
 G. X. Yu, X. L. Zhou, C. L. Li, L. F. Chen, J. A. Wang, Catal. Today 2009,
 S. Bancquart, C. Vanhove, Y. Pouilloux, J. Barrault, Appl. Catal. A: Gen.
2001, 218, 1–11.
 R. K. Pandey, P. Kumar, Catal. Commun. 2007, 8, 1122–1125.
 O. Casanova, S. Iborra, A. Corma, J. Catal. 2009, 265, 109–116.
 A.-S. Mamede, E. Payen, P. Grange, G. Poncelet, A. Ion, M. Alifanti, V. I.
Pârvulescu, J. Catal. 2004, 223, 1–12.
 M. Fuchs, B. Jenewein, S. Penner, K. Hayek, G. Rupprechter, D. Wang, R.
Schlçgl, J. J. Calvino, S. Bernal, Appl. Catal. A: Gen. 2005, 294, 279–289.
 U. NylØn, L. Sassu, S. Melis, S. Järås, M. Boutonnet, Appl. Catal. A: Gen.
2006, 299, 1–13.
 U. NylØn, B. Pawelec, M. Boutonnet, J. L. G. Fierro, Appl. Catal. A: Gen.
2006, 299, 14–29.
 S. B. Kogan, M. Kaliya, N. Froumin, Appl. Catal. A: Gen. 2006, 297, 231–
 H. X. Mai, L. D. Sun, Y. W. Zhang, R. Si, W. Feng, H. P. Zhang, H. C. Liu,
C. H. Yan, J. Phys. Chem. B 2005, 109, 24380–24385.
 R. Si, M. Flytzani-Stephanopoulos, Angew. Chem. 2008, 120, 2926–
2929; Angew. Chem. Int. Ed. 2008, 47, 2884–2887.
Received: February 25, 2010
Published online on May 18, 2010
678 www.chemsuschem.org 2010 Wiley-VCH Verlag GmbH Co. KGaA, Weinheim ChemSusChem 2010, 3, 654 – 678
L. Vivier and D. Duprez