ORIGINAL PAPER
Developments in the Pd Catalyzed Hydrogenation of OxygenatedOrganic Compounds
Charles Sumner Jr. • William Burchett
Published online: 21 June 2012
� Springer Science+Business Media, LLC 2012
Abstract This manuscript briefly reviews some key
developments in hydrogenation catalysis and their appli-
cation from an industrial perspective. The interaction of Pd
(and Pt) with the support material has been previously
reported as a factor that determines the activity and
selectivity of Pd hydrogenation catalysts. Temperature
programmed reduction experiments carried out on
Pd/Al2O3 catalysts in our laboratory showed a correlation
between hydrogen consumption and selectivity for the
hydrogenation of acetophenone.
Keywords TPR � Pd/Al2O3 � Hydrogenation �Selectivity � Acetophenone
1 Introduction
The economic value and impact of hydrogenation catalysts
is tremendous. Each day we consume products derived
from catalyzed hydrogenations ranging from the drugs we
need, the clothes we wear, to the containers that store our
food and beverages. The purpose of this paper is to give a
brief overview of some key developments in hydrogenation
catalysis and how they relate to the industrial manufacture
of chemical products. We will also describe results from
our laboratory pertaining to the interaction of palladium
with an alumina support and the selectivity of the catalyst.
Over the last 30 years, surface chemistry has evolved
into a molecular-level science. The recognition that
chemisorption (and reaction) of a substrate can lead to
reconstruction of a single crystal surface has resulted in the
development of many in situ techniques of spectroscopic
analysis [1, 2]. The characterization of the catalyst surface
during the course of the catalytic reaction (referred to as
Operando techniques) has the obvious advantage of pro-
viding a look at the catalyst while it is in its working form.
Operando measurements and methods are constantly
improving, and many research groups specialize in this
field. Using these techniques, one can potentially identify
reaction intermediate species adsorbed on the surface and
determine other parameters important to the reaction
mechanism. Having a true picture of the reaction mecha-
nism and the structure of the catalyst surface would ulti-
mately lead to the determination of structure–reactivity
relationships. Such insights will greatly aid in the design of
better catalysts and in the improvement of existing com-
mercial catalysts where often a very small increase in
selectivity or rate results in very large economic returns.
2 Catalyst Modeling
Recent advances in the use of density functional theory for
modeling surface reactions have led to the discovery of
several new hydrogenation catalysts. Work published by
Norskov and collaborators described a systematic, com-
putational method to screen potential catalysts for a desired
application [3]. Descriptors (‘‘the most important micro-
scopic materials properties of the catalyst which determine
the macroscopic catalytic performance’’; for example,
reactant heat of adsorption) [4] were identified for the
desired reaction. The descriptors were able to predict trends
in the activity, selectivity, and cost of the catalyst. The
descriptor values were calculated using DFT simulations
and pre-existing computational databases. The materials
that were identified with descriptor values closest to the
C. Sumner Jr. (&) � W. Burchett
Eastman Chemical Company, Kingsport, TN 37662, USA
e-mail: [email protected]
123
Top Catal (2012) 55:480–485
DOI 10.1007/s11244-012-9820-4
optimal values were evaluated experimentally [4]. Several
new catalysts were identified using this approach and
include a Ni–Fe methanation catalyst [5] that is cheaper
and more active than Ni only; a Ni–Zn catalyst [6] for the
selective hydrogenation of ethylene that has selectivity
comparable to the commercial Pd–Ag catalyst but is
cheaper, and a Pt–Bi electrocatalyst [7] for the hydrogen
evolution reaction that is more active than pure Pt. The
advantage of the computational approach to screening
catalysts is that it could save money and time by elimi-
nating most of the experimental screening reactions. A
disadvantage is that it requires access to high performance
computing systems. The approach does not work well with
processes that have several competing reactions, or with
metal oxide surfaces [3]. Improvements to the method
would include the formation of larger databases and
development of better computer code. Computational
methods used to model catalyst surfaces continue to
improve and can be a powerful tool when combined with
experimental work. So, will the day come when experi-
ments are no longer needed? Probably not, since no matter
how good computation becomes, someone will still have to
figure out how to make and then test and scale up the
structures predicted by a computer.
3 Chiral Catalysis
Hydrogenation of prochiral substrates to produce chiral
products is commonly accomplished using homogeneous
catalysts comprised of precious metals complexed with
chiral phosphine ligands. While very good enantiomeric
excess can be achieved with the homogeneous catalysts,
there are many obvious advantages for the use of hetero-
geneous catalysts such as ease of separation, catalyst
recovery and recycle, and handling. These can be particu-
larly important for precious metal catalysts. Advances in
the development and understanding of heterogeneous cat-
alysts for asymmetric hydrogenations have been made
through the combination of surface science techniques and
practical applications [8, 9].
Enantioselective heterogeneous catalysis is generally
thought to involve the formation of a chiral environment at
the catalyst surface [10]. One way chirality can be induced
is by the modification of the surface with adsorbed chiral
molecules to give an ordered array of chiral molecules that
influences the adsorption of a prochiral reactant in a
geometry that favors one of the enantiomeric products. For
example, heterogeneous Pt catalysts modified with chiral
cinchona alkaloids have been found to be effective cata-
lysts for the enantioselective hydrogenation of activated
ketones and a,b-unsaturated carboxylic acids. R,R-tartaric
acid was used as a chiral modifier in the Ni-catalyzed
hydrogenation of b-ketoesters [11, 12].For the case of
acidic modifiers, it is possible that chiral etching of the
metal surface can take place under certain conditions.
Scanning tunneling microscopy (STM) studies have shown
that the adsorption of chiral amino acids onto an achiral
Cu(001) surface can induce restructuring of the surface to
develop intrinsically chiral facets [13]. A similar phe-
nomenon was observed with tartaric acid [14].
The effectiveness of the chiral modifier was reported to
be influenced by the ionicity of the catalyst support mate-
rial for the cinchonidine-modified Pt/Al2O3 system [15].
The enantiomeric excess in the hydrogenation of methyl
benzoyl formate increased with decreasing basicity. The
reason for the effect was thought to be due to the electronic
state of Pt that was dependent on the acidity of the support.
In related work, the diastereoselectivity of cinchonidine
hydrogenation was controlled by tuning the acid–base
properties of the alumina support [16].
4 Metal Support Interaction
Subtle changes in the composition of the catalyst support
material can have a dramatic effect on the performance of
the catalyst. Vannice [17, 18] reported that the reduction
temperature of Pt/TiO2 influenced the selectivity and
activity for the hydrogenation of carbonyl groups to alco-
hols. The catalysts that were reduced at 500 �C were more
selective than catalysts reduced at 200 �C. The origin of
the enhanced selectivity was thought to be the formation of
a Ti3? cation or an oxygen vacancy adjacent to a Pt atom.
The carbonyl oxygen atom was thought to be activated at
the metal-support interfacial region. The Bronsted acidity
or basicity (ionicity) of the support material can have a
great influence on the performance of the catalyst. For
example, Pd supported on high purity silica support was
reported to catalyze the hydrogenation of carbon monoxide
to mainly methane; however, if the silica support contained
as little as 600 ppm of Ca the major product was methanol
[19]. The more acidic silica favored the production of
methane while the more basic silica favored the formation
of methanol.
Mojet and Koningsberger [20] applied a combination of
computational, surface and sorptive characterizations, and
reactivity studies to formulate a model to describe the
metal support interaction for Pt and Pd. In this model, the
ionicity of the support (high ionicity is equivalent to low
acidity) can affect the strength of the metal–oxygen bond
and thus the morphology of the metal particle. A stronger
bond with the support as a result of low ionicity was cal-
culated to cause the metal particles to be flat and raft like,
while a weaker metal oxygen bond caused by high ionicity
caused the particles to be rounder and hemisphere shaped
Top Catal (2012) 55:480–485 481
123
[21]. The ionicity can also affect the bonding modes of
hydrogen and carbon monoxide with the metal particle. For
example, FTIR showed significant l-CO with Pt supported
on basic alumina but not with acidic alumina. The Pt–H
bond strength is higher for ionic supports and the Pt–O
bond strength is higher for acidic supports [22]. The dif-
ference in electron density in the supports affects the
sp/(sp ? d) Pt orbital hybridization and causes the Pt 5d
states to shift to lower binding energy with increased ion-
icity [23]. The hydrogen adsorption energy increases for Pt
on supports with higher ionicity, and thus the ionicity of
the support influences the hydrogen coverage and type of
empty site available for adsorption of reactants. Experi-
mentally, this results in greater activity for hydrogenolysis
reactions on acidic supports [24–26].
5 Experimental Section
5.1 Preparation of Catalysts
The alumina used in this work was 1/16th inch pellets and
had a surface area of 40 m2/g. Solutions (1.0 wt% Pd) of
Pd(NH3)4(OH)2 were prepared by ion exchange of
Pd(NH3)4Cl2 over Amberlyst� A-26(OH) ion exchange
resin. The solutions were analyzed by ICP for Pd and Cl
and stored under an argon atmosphere prior to use. The
concentration of the Pd solution was adjusted by dilution
with deionized water and the resulting solution was added
to the alumina (via incipient wetness technique). The
resulting alumina was vacuum dried first on a rotovap
followed by 12 h at 115 �C in an oven. The dried material
was calcined at 300 �C for 4 h in air, cooled under nitro-
gen, and activated by heating at a rate of 1�/min to 200 �C
under a flow of H2/N2 (1:1). The Pd dispersion as measured
by CO chemisorption (stoichiometry factor of one) ranged
from 33 to 40 %. The average particle size measured by
TEM ranged from 2.3 to 2.5 nm.
5.2 Hydrogenation of Acetophenone
The hydrogenations were carried out in cyclohexane
solution in a 300 mL stainless steel autoclave equipped
with a catalyst basket and a dip tube that enabled sampling
during the reaction. The reaction temperature was 170 �C
and the hydrogen pressure was 1,000 psig. The reactants
were added in one portion to the autoclave at reaction
conditions. The mixture was sampled at time intervals and
analyzed by gas chromatography for 1-phenylethanol,
acetophenone, cyclohexylmethyl ketone (CMK), 1-cyclo-
hexylethanol, ethylbenzene, ethylcyclohexane, and styrene
(no styrene was detected). The initial rate for the formation
of CMK and 1-cyclohexylethanol (the products resulting
from the hydrogenation of the benzene ring) were deter-
mined by taking the slope of the sum of the products
plotted against time at the zero order portion of the curve.
The initial rate for the formation of products resulting from
hydrogenolysis (ethyl benzene and ethyl cyclohexane) was
determined similarly.
6 Results and Discussion
Alumina supported Pd catalysts are used commercially in
continuous processes for the hydrogenation of carbon–
carbon double bonds and for the hydrogenation of aromatic
rings to cyclohexane derivatives. A common problem
encountered during the hydrogenation of compounds that
possess an oxygen-containing functional group is the
hydrogenolysis of the carbon–oxygen bond to give unwanted
Fig. 1 Overlay of H2TPR plots illustrating the variation in H2
consumption for 1 % Pd/Al2O3 catalysts
O OH
O OH
+
+
acetophenone phenylethanol
ethylbenzene
ethylcyclohexane
CMK cyclohexylethanol
ring hydrogenation
hydrogenolysis
Fig. 2 Products from the hydrogenation of acetophenone over 1 %
Pd/Al2O3 at 170 �C and 1,000 psig of H2 in cyclohexane solution
482 Top Catal (2012) 55:480–485
123
byproducts. Research in our laboratory has been focused on
improving the selectivity of the catalyst while at the same
time increasing the activity. The work presented here
involved the characterization and evaluation of catalysts
comprised of alumina supports with differing acidities that
had been decorated with (1 %) Pd.
Temperature programed reduction (TPR) of oxidized Pd
supported on gamma-alumina was reported by Lieske and
Volter [27]to reflect an interaction of Pd with the alumina
support, presumably as the form of a two dimensional
surface species of palladium aluminate. The reduction
temperature of the palladium aluminate was reported to be
around 300 �C, and its formation was thought to be
involved in the redispersion of Pd on alumina by high
temperature calcination. XPS data reported by Otto et al.
[28] were consistent with the presence of two forms of
oxidized Pd. In our labs, we noticed a similar high tem-
perature reduction (at around 300 �C) for alumina sup-
ported Pd hydrogenation catalysts prepared by incipient
wetness using an aqueous solution of Pd(NH3)4(OH)2. The
amount of hydrogen that was consumed at around 300 �C
(250–310 �C) in the TPR experiment varied depending
upon the amount of alkali metal present on the alumina
(that is, the support ionicity). For example, alumina that
had been treated with sodium carbonate (or nitrate) fol-
lowed by calcination at 900 �C prior to impregnation with
Pd gave catalysts that consumed greater amounts of
hydrogen at 300 �C than catalysts prepared from the alu-
mina that had no additive. It was assumed that the supports
with higher ionicity would also have lower acidity. Fig-
ure 1 shows an overlay of TPR plots for five catalysts
comprised of 1 % Pd/alumina that had different hydrogen
consumption amounts. While the hydrogen consumptions
are in the temperature range given by Lieske and Volter for
palladium aluminate, we cannot say with certainty what is
responsible for it. Whether the higher temperature hydro-
gen consumption was due to the presence of palladium
aluminate or the reduction of a surface species in contact
with the metal, the amount of hydrogen that was consumed
at around 300 �C was an indication of the selectivity of the
catalyst when it was applied to the hydrogenation of an
oxygenated organic compound.
The selectivity of the catalysts was evaluated using the
hydrogenation of acetophenone as a model reaction. This
reaction was chosen because of its ability to determine
differences in selectivity that arise as a result of ring
hydrogenation and hydrogenolysis of the carbon–oxygen
bond (Fig. 2). The hydrogenations were carried out in
cyclohexane solution at 170 �C and 1,000 psig H2 in a
stirred autoclave. Saturated products that retained the car-
bon–oxygen bond, cyclohexyl methyl ketone (CMK) and
1-cyclohexylethanol, were grouped as products of ring
hydrogenation, and products that did not contain oxygen,
ethyl benzene and ethyl cyclohexane, were grouped as
Table 1 Hydrogen
consumption and initial rate for
the hydrogenation of
acetophenone for different
1 %Pd/Al2O3 catalysts
Catalyst H2
consumption @
300� (lmol/g)
Initial rate of ring
hydrogenation
(mmol/g/min/gcat)
Initial rate of
hydrogenolysis
(mmol/g/min/gcat)
Total rate
(mmol/g/
min/gcat)
Selectivity
to ring (%)
A 0 0.0013 0.0130 0.0143 9
B 6 0.0027 0.0055 0.0082 33
C 10 0.0017 0.0057 0.0074 23
D 22 0.0023 0.0041 0.0065 36
E 51 0.0016 0.0025 0.0041 39
Fig. 3 Selectivity to ring hydrogenation as a function of hydrogen
consumption Fig. 4 Total initial rate as a function of hydrogen consumption
Top Catal (2012) 55:480–485 483
123
hydrogenolysis products. Under these reaction conditions,
the initial product appeared to be 1-phenylethanol which
was converted to the mixture of final products (similar
kinds of product distributions were obtained when starting
with 1-phenylethanol).
The data for the acetophenone hydrogenations are listed
in the Table 1. The selectivity for ring hydrogenation
appeared to increase with increasing hydrogen consump-
tion measured in the TPR (Fig. 3), while the total rate of
reaction decreased with increasing TPR hydrogen con-
sumption (Fig. 4) at around 300 �C. The selectivity for ring
hydrogenation increased, but the overall activity of the
catalyst with respect to the conversion of acetophenone
decreased. As shown in Fig. 5, the initial rate of hydrog-
enolysis decreased with hydrogen consumption. A plot of
the initial rate of ring hydrogenation against hydrogen
consumption does not appear to show any correlation
(Fig. 6). The hydrogenolysis reaction and ring hydroge-
nation are presumably parallel reactions. The hydrogenol-
ysis reaction appears to be slower on catalysts that have
higher TPR hydrogen consumption. While hydrogenolysis
is slowed, the rate of the ring hydrogenation (in these
examples) does not appear to be affected as much by the
properties of the support, thus the selectivity for ring
hydrogenation increases and the activity as measured by
conversion of acetophenone decreases.
7 Conclusion
Catalysis of industrial hydrogenation processes almost
always involves a balance between activity and selectivity.
Recent progress in the field of surface science has shed
light on some of the properties that are responsible for
both. The interaction of the catalyst metal with the support
material has been recognized as a phenomenon that can
have a great effect on catalyst selectivity, and new models
have been developed to explain how the interaction
operates on a molecular level. In processes where parallel
reactions take place, it is possible that the nature of the
support can favor or inhibit one pathway over the other and
thereby influence the selectivity (and activity) of the cat-
alyst. In the work described here, the observation of a
reduction at 300 �C in the TPR experiment might reflect an
interaction of Pd with the support or be the result of other
factors1. The reduction appears to correlate with the
selectivity of the catalyst for ring hydrogenation, and the
absence of the reduction correlates with a tendency toward
hydrogenolysis.
Acknowledgments We thank Eastman Chemical Company for
permission to publish this work.
References
1. Somorjai GA, Li Y (2011) Proc Nat Acad Sci USA 108:917
2. Yates JT Jr, Campbell CT (2011) Proc Nat Acad Sci USA
108:911
3. Norskov JK, Abild-Pedersen F, Studt F, Bligaard T (2011) Proc
Nat Acad Sci USA 108:937
4. Greeley J, Zapol P, Curtiss L (2008) SciDAC review—nanoscale
materials: recent trends in computational catalysis 2008.
http://scidacreview.org/0804/html/trends.html
5. Anderson M, Bligaard T, Kustov A, Larsen KE, Greeley J,
Johannessen T, Christensen CH, Norskov JK (2006) J Catal
239:501
6. Studt F, Abild-Pedersen F, Bligaard T, Sorensen RZ, Cristensen
CH, Norskov JK (2008) Science 320:1320
7. Greeley J, Jaramillo TF, Bonde J, Chorkendorff I, Norskov JK
(2006) Nat Mater 5:909
8. Mallat T, Orglmeister E, Baiker A (2007) Chem Rev 107:4863
9. Kulkarni A, Torok B (2011) Curr Org Synth 8:187
10. Badderly CJ, Richardson NV (2010) Scanning tunneling
microscopy in surface science. Nanoscience and catalysis. Wiley-
VCH Verlag GmbH & Co., KGaA, Weinheim, pp 1–27
11. Webb G, Wells GB (1992) Catal Today 12:319
12. Izumi Y (1983) Adv Catal 32:215
Fig. 5 Initial rate of hydrogenolysis as a function of hydrogen
consumption
Fig. 6 Rate of ring hydrogenation as a function of hydrogen
consumption
1 The hydrogen consumption at 300 �C could be due to the formation
of a surface species interacting with palladium that is formed as a
result of the basicity of the support
484 Top Catal (2012) 55:480–485
123
13. Zhao X (2000) J Am Chem Soc 122:12584
14. Lorenzo MO, Hag S, Bertrams T, Murray P, Raval R, Badderley
CJ (1999) J Phys Chem B 103:10661
15. Hoxha F, Schimmoeller B, Cakl A, Urakawa A, Mallat T, Prat-
sinis SE, Baiker A (2010) J Catal 271:115
16. Schmidt E, Hoxha F, Mallat T, Baiker A (2010) J Catal 274:117
17. Vannice MA (1990) J Mol Catal 59:165
18. Vannice MA (1997) Top Catal 4:241
19. Fajula F, Anthony RG, Lunsford JH (1982) J Catal 73:237
20. Mojet BL, Miller JT, Ramaker DE, Koningsberger DC (1999) J
Catal 186:373
21. Stakheev AY, Zhang Y, Ivanov AV, Baeva GN, Ramaker DE,
Koningsberger DC (2007) J Phys Chem C 111:3938
22. Ramaker DE, Teliska M, Zhang Y, Stakheev AY, Koningsberger
DC (2003) Phys Chem Chem Phys 5:4492
23. Oudenhuijzen MK, van Bokhoven JA, Ramaker DE, Konings-
berger DC (2004) J Phys Chem B108:20247
24. Oudenhuijzen MK, van Bokhoven JA, Miller JT, Ramaker DE,
Koningsberger DC (2005) J Am Chem Soc 127:1530
25. Ji Y, Koot V, van der Eerden AMJ, Weckhuysen BM, Kon-
ingsberger DC, Ramaker DE (2007) J Catal 245:415
26. Koningsberger DC, Oudenhuijzen MK, de Graaf J, van bokhoven
JA, Ramaker DE (2003) J Catal 216:178
27. Lieske H, Volter J (1985) J Phys Chem 89:1841
28. Otto K, Haack LP, DeVries JE (1992) Appl Cat B Environ 1:1
Top Catal (2012) 55:480–485 485
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