some aspects of electronic interactions in heterogeneous catalysis
TRANSCRIPT
React. Kinet. Gatal. Lett., Vol. 35, No8 1-2, $91-402 (1987)
SOME ASPECTS OF ELECTRONIC INTERACTIONS IN HETEROGENEOUS
CATALYSIS
D.M. Shopov
Institute of Kinetics and Catalysis, BulgarianAcademy
of Sciences, Sofia 1040, Bulgaria
Received February 13, 1987
It is now generally accepted that after the introduction
of the ideas on the existence of active sites, Balandin's theory
about the influence of geometrical and electronic factors on
the mechanism of the reactions is a substantial contribution
to the development of heterogeneous catalysis. In fact, this
was the first attempt to connect the mechanism of heterogeneous
catalytic reactions with the structure of the solid and the
reagents. This idea found numerous applications in further de-
velopment of the theory.
In one of the most recent versions of this idea, Sachtler
and Ponec suggested the therms "ligand" and "ensemble" to de-
scribe the effect of electronic and structural factors on the
adsorption and catalytic properties of bimetallic systems. In
the original version of their approach the authors assign a
secondary role to the ligand effect, which is connected to as-
scribing "independence" to the atoms in the ensemble. The present
ideas about solid state structure give no ground for such arti-
ficial division of electronic and structural factors.
One should note that in the last years the widespread
"local" approach in catalysis contains, or to be more correct,
allows to suggest the existence of "individual" behavior of
the structural elements of the solid body. However, one should
not forget that this is usually made for methodological reasons
with the aim of stressing the chemical nature of catalytic
phenomena. We would like to point out that neglecting the ex-
Akad6miai Kiad6, Budapest
isting collective interactions in the solid body might lead to
rather serious negative consequences.
In the Present lecture, we discuss the basis of the theo-
retical ideas about the nature of chemical bonding, a number of
experimental results concerning the structure and catalytic
properties of bimetallic clusters, the influence of the envi-
ronment on the formation and properties of metal particles, the
role of size effects on the catalytic properties, etc., with
the aim to clarify the role of the electronic and structural
factors.
Theoretical approach
Let us write the following equation for a bulk metal:
HeffT = QT (i)
where Hef f is an effective Hamiltonian with eigenvalue Q. The
latter corresponds to the heat of atomization of the bulk met-
al, defined as the difference between the total energy of the
bulk metal and the sum of the energies of the separate atoms.
The one electron approximation is applied here and the exist-
~nce of fine effects such as electron correlation and magnetic
properties are neglected.
Now let us have two interacting systems with Hamiltoni-
ans H 1 and H 2 and heats of atomization Q1 and Q2" The secular
matrix of the two systems is:
HI1 - E HI2 - ESI2
= O (2) H21 - ES21 H22 - E
The solution of eq.(2) gives the following eigenvalues:
- (2H12S12-Hll-H22) • 2-4 |1-S~2) |HllH22- ~ El, 2= 211_S~2)
One can notice that E 1 or E 2
the original interacting levels Q1
392
(3)
will be higher or lower than
and Q2' respectively, if the
2>I I term HI2 is HI2 HIIH22 .
Therefore, splittting of the levels Q1 and Q2 occurs
and the higher level goes higher, while the lower level shifts
down. This shift of the higher level means that after the in-
teraction the bond strength in the corresponding system is
weakened in general and indicates a tendency of the system to
split into smaller subsystems, e.g. to increase the dispersity.
The opposite is valid for the system with higher heat of atom-
ization, e.g. with the lower energy level. In this case the
effect of the interaction will be strengthening of the chemical
bonds of the system and a tendency to decrease the dispersity. 2
Therefore, if the relation HI2>IHIIH~I is valid, one can
use the heats of atomization to predict the effect of the second
component on the dispersity of the main component in bimetallic
catalysts. We should note that the experimental heats of atom-
ization are measured for bulk metals, where Q does not depend
on the number of atoms. For supported metal clusters, whose
size is often less than 50 A, the heat of atomization differs
from that of the bulk metal. If the functions Q=f(N) for the
two interacting systems do not cross each other, e.g. they do
not form an alloy, then the heats of atomization of the bulk
metal can be used to predict the effect of the second component
on the dispersity of the main, catalytically active component.
The effect of the support on the dispersity can be treat-
ed on the same grounds. The oxide supports, generally used in
catalysis, always have higher heats of atomization than the
supported metals. Therefore, one can expect that the supports
will always favor the dispersity.
Role of the second component in bimetallic catalysts
Table 1 contains the heats of atomization of some metals
and the predicted effect of the second component on the disper-
sity of platinum [I ]. One can note the good agreement between
the predicted and experimental results. Indeed, metals such as
Re, Ir and Ru, which have higher heats of atomization than Pt,
increase its dispersity. And contrary to that, metals such as
393
Bi, Ti, Au, Pb and In, which have lower heats of atomization
than Pt, decrease the dispersity of Pt in full agreement with
the prediction.
For a more detailed understanding of this process we have
carried out quantum-chemical calculations using the extended
H~ckel method [I]. The calculations were carried out for two
model systems Pt-Re and Pt-Ti (Fig. 1). They were chosen be-
cause they represent the two typical cases describing the effect
of the second component on the dispersity of Pt.
Table 1
Effect of the second component on Pt dispersity
("yes" - increase, "nO" - decrease of dispersity)
System:
Main Metal Second Metal
Heat of atomization (kJ/g atom)
Prediction Experiment (Theory)
Pt-566.1 Re-781.6
Pt-566.1 Ir-665.3
Pt-566.1 Ru-648.9
Pt-566.1 Bi-205.7
Pt-566.1 Ti-180.1
Pt-566.1 Au-365.5
Pt-566.1 Pb-195.6
Pt-566.1 In-242.4
yes yes
y e s y e s
yes n o , y e s ?
no no
n o n o
n o n o
n o n o
n o n o i n f l u e n c e
Table 2
Bond populations for the Pt-Re system
System
4Pt atoms linear 4Pt-2Re
4Pt-4Re
Bond population between adjacent atoms, .... 1-2 2-3 3-4 4-5 5-6 13
0.0061 0.1169 0.0061 0.0257 -0.1039 0.0241 0.4032 0.8474 1-2 2-3 3-4 5-6 6-7
0.0768 -0.1144 0.0768 0.5773 0.3809 7-8
0.5778
394
0 0 0 0 0 0 1 2 3 /* 5 6
O - Pt
O - Re Ti
1 2 3 /,
0 0 0 0 0 0 0 0 5 6 7 8
B
Fig. i. Geometries used in the calculation
Table 3
Bond populations for the Pt-Ti system
System Bond population between adjacent atoms P. z3
1-2 2-3 3-4 4-5 5-6
4Pt-2Ti 0,295 0.303 0.162 0.334 0.186
1-2 2-3 3-4 5-6 6-8 7-8
4Pt-4Ti 0.267 0.269 0.267 0.241 0.298 0.241
The calculations indicate (Table 2), that in the presence
of Re the bond population between the Pt atoms is decreased,
while in the presence of Ti it is increased (Table 3). The
bond population values clearly indicate the opposite effects
of Re and Ti on the size of the Pt particles.
The analysis of the computational data allows to explain
this effect in more detail. Charge transfer from Re to Pt
occurs, thus increasing the number of electrons in the antibond,
ing orbitals of Pt. This contributes to the weakening of the
bonds between the Pt atoms and even to breaking of some bonds.
The charge transfer has also been observed experimentally [2].
39,~
The opposite effect is true in the Pt-Ti system. The
transfer of electrons from the antibonding orbitals of Pt to
the empty d-orbitals of Ti results in strengthening of the Pt-
Pt bonds.
Role of the support on the dispersity of supported metal cat-
al[sts
Let us accept as an evaluation of the effective energy of
one bond in the oxide support the value E = Do/n, where D o is
the experimental heat of atomization [3], and n is the number
of ligands surroinding the metal ion in the oxide lattice.
Baker et al. [4] have studied the structure and growth in
hydrogen of very small Pt particles under heating on thin films
of TiO2, AI203 and SiO 2. The following particle sizes (Table 4)
are found. One can notice the good agreement between the par-
ticle size and the E value.
Table 4
Particle size of Pt depending on the carrier and the temperature
Carrier Pt particle size (nm)
825 K 975 K Exi0 -3
(kJ/K moi)
Ti407 0.51 0.56 1270
AI203 0.51 0.67 509.9
SiO 2 0.71 0.96 462.1
The effect of a number of oxides with n=6 o~ the disper-
sity of supported Ni catalysts is investigated in [5]. The
following order has been found:
AI203 > MgO > Cr203 > ReO 3 > CaO > SrO
Ex10 "3 (kJ/K mol) 509.9 166.8 445.2 194.2 176.9 166.9
Again the results are in good agreement with the corresponding
values of E, with the exception of MgO.
396
This is also confirmed in the work of Taghavi et al. [6]
concerning the dispersity of Cu (Table 5). One can again observe
the clear correlation between the particle size and the E value.
Table 5
Particle size of supported Cu depending on the support
S a m p 1 e Mean particle size Ex10 -3 �9 of Cu (nm) (kJ/k mol)
1.93% Cu/AI203 4.5 509.9
1.93% Cu/MgO 10.0 166.8
1.73% Cu/SiO 2 67.0 462.1
In a series of investigations Ioffe et al. [7] have
established that the prior deposition of W, Mo and Re oxides
on the surface of SiO 2 greatly increases the dispersity of
supported Pt. This modification of the surface leads to the
formation of a new solid system, containing W-O, Mo-O and Re-O
bonds of larger bond strength, which interact with the metal
in the above mentioned way.
Our experimental results [8] confirmed the favorable
effect of modifying the surface of silica and alumina by molyb-
denum oxide on the dispersity of supported Pd (Table 6).
Table 6
Disperslty of molybdenum modified palladium samples
Samples Pd Pd3%Mo Pd6%Mo Pd15%Mo Pd20%Mo on SiO 2
Dispersity 0.18 0.62 0.80 0.40 0.39
Samples Pd Pd3%Mo Pd6%Mo Pd15%Mo Pd20%Mo on A1203
Dispersity 0.26 0.49 0.60 0.62 0.55
397
The above examples show that the E value can be used as
a criterion for predicting the effect of the carrier on the
dispersity of supported metals.
Interesting results were also obtained [9] when investi-
gating the formation of palladium particles by reduction in
liquid phase of different polarity of PdCI 2 supported on alumina
or silica (Table 7).
Table 7
Dispersity of Pd particles formed after reduction of PdCI 2
liquid phase
in
Liquid phase dioxane chloroform acetone
SiO 2 0.18 0.27 0.36 Sample
AI203 0.26 0.47 0.84
It is obvious that the dispersity is increased with in-
creasing polarity of the solvent in the order:
acetone > chloroform > dioxane
In the process of formation of the metal particles, interaction
between them and the molecules of the liquid phase takes place.
One can conclude that the role of the liquid phase is similar
to that of the second component in the above discussed cases.
A number of experimental facts related to changes in the
properties of the metal particles caused by interaction with
adsorbed species can be treated on the basis of the above con-
siderations.
Effect of adsorbed species on the electronic structure of metal
clusters
Quantum-chemical calculations carried out by us [10] con-
cerning the effect of adsorbed electron acceptor elements such
as H, O, C1 and S on Pt(111) and Pt(100) clusters indicate that
the adsorption leads to a considerable decrease of the bond
strength between the metal atoms. It is this effect that causes
398
the experimentally observed increased mobility of the surface
metal atoms, the reconstruction of the surface planes or re-
dispersion of metal particles, for example, when treated in oxy-
gen. One cannot but indicate the similarity between the behavior
of these systems and the process taking place in the bimetallic
catalysts under the influence of the second component or the
effect of the support on the dispersity of metal particles.
However, the question arises what is the cause for this de-
stabilization of the metal clusters under the influence of the
above mentioned electron acceptor elements, having in mind e-
lectron transfer from the antibonding metal orbitals to the ad-
sorbate. This electron transfer should lead to stabilization of
the metal particles. However, this stabilizing effect is accom-
panied by shifting of the MO of the metal particles toward higher
energies as a result of interaction with the low lying orbitals
of the adsorbate. This destabilizing effect overcomes the stabi-
lizing effect due to charge transfer, thus resulting in de-
stabilization of the metal particles.
The strong inhibiting effect of sulfur in a number of cat-
alytic reactions can be treated on analogous grounds. For example,
the addition of Cu or Ag to Pt/AI203 catalysts promotes the re-
action of oxidation of CO and C2H 4, while very small amounts of
sulfur strongly inhibit this reaction. The nature of these pro-
moting and inhibiting interactions was studied quantum-chemi-
cally by us [11] and is brought to the above described shifting
of the metal MO up or down under the influence of the inhibitor
or the prmmoter.
All phenomena discussed here have a common feature -- all
of them are the result of electronic interactions, we indicated
that for all systems mentioned the interaction leads to the
formation of a new system, characterized as a whole by a new
local energy minimum and new energy states of the components
of the system. We should note that the changes in the electron
properties sometimes might also cause structural changes, such
as changes in the particle size, in their habitus, the appear-
ance of defects, etc. However, in all cases, the electronic
399
(energetic) factor is the one that dominates and determines the
physical properties of the system.
Effect of metal particle size on the catalytic activity
We have established [12] that the catalytic oxidative cou-
pling of styrene on palladium strongly depends on the particle
size. The catalytic reaction takes place at dispersities above
0.15. A more detailed study shows that catalytic activity is
manifested by particles having sizes less than 1.5 nm. With the
aim of clarifying the influence of the change of the metal sur-
face area we have studied by means of IR spectroscopy the ad-
sorption of CO on metal particles of different size [13]. Only
the bond at 2110 cm -1, characteristic of linearly adsorbed CO
(Fig. 2), was observed for metal particles less than 1.5 nm in
size. For larger particles in polydisperse samples both the
linear (above 2000 cm -I) and the bridged form (below 2000 cm "1 )
o ~ ~i -21~176
I I I I
1900 2100 cm-1
Fig. 2. IR spectra of CO adsorbed on samples of different
dispersities: a - 0.18; b - 0.10
400
of adsorption of CO on the Pd(100) and Pd(111) faces was ob-
served. Correlation between catalytic activity and the integral
intensity of the linear form was found. It could be suggested
that on the large size particles different active sites (in the
sense of geometrical ensembles of particular size) exist. For
smaller particles the surface is unified geometrically; transi-
tion, for example, from cubic lattice into cubooctahedral, or
finally into spherical. These changes in the geometry are caused
by changes in the electronic interactions between the separate
atoms in the metal particle. The essence of these changes is
an increased localization of the wave functions.
An interesting example for the influence of the electronic
factor and of the dispersity is observed in the presence of oxy-
gen. The presence of strongly bound subsurface oxygen in addi-
tion to surface species was established for group VIII metals
such as Pt, Pd, Ir, Ni, etc.
We have studied by quantum-chemical calculations [14] the
changes in the electronic structure of Pt(111), Pd(111), Ir(111)
and Ni(111) clusters that occur in the presence of subsurface
oxygen and its influence on the dissociative chemisorption of
02 . One of the interesting effects of subsurface oxygen is that
it decreases the work function of the above metals, which is
confirmed experimentally [15].
The subsurface oxygen also influences the dissociation of
02 over different size clusters. For small size clusters the
subsurface oxygen enhances the dissociative chemisorption of 02
However, for clusters having more than 18 metal atoms in (111)
configuration, the dissociative chemisorption of 02 is impeded.
For a particular size of the cluster, the destabilizing effect
of subsurface oxygen overcomes the stabilizing effect connected
with the electron transfer from the metal particle to the sub-
surface oxygen. Larger particles are more sensitive to shifting
up of the MO of the cluster. As a result, dissociative chemi-
sorption is impeded.
401
Concluding remarks
The examples we have discussed indicate that it is possible,
on the basis of quantum-chemical description of the interaction
between energy levels, to explain many processes in heteroge-
neous catalysis.
The division into electronic and geometrical factors ap-
peared historically, as an analysis of the processes, with the
aim to simplify their understanding. The present development
of the theory of catalysis shows that achieving of the basic
goal, e.g. explanation and prediction of the properties of cat-
alytic systems necessitate a synthesis between the components
and the mechanism of their action. Undoubtedly, this synthesis
can be carried out successfully only upon recognition of the
decisive role of electron factor.
Acknowledgment. I wish to express my gratitude to Prof. A.
Andreev and Dr. T. Halachev for fruitful discussions.
REFERENCES
I. T. Halachev, A. Andreev, N. Neshev, D. Shopov: Acta Chim. Acad. Sci. Hung., 118, 225 (1985)
2. M.F.L. Johnson, V.M. LeRoy: J. Catal., 35, 434 (1974) 3. Physical and Chemical Properties of Oxides (Res.), Ed. V.G.
Samsonov, p. 93, Metallury, Moscow 1978. 4. R.T.K. Baker, E.B. Prestridge, R.L. Garten: J. Catal., 5_66,
390 (1979) 5. V. Veselov, P. Filipenko Kinet. Katal., 1~7, 491 (1976) 6. M.B. Taghavi, M.G. Pajonk, S.J. Teichner: J. Colloid
Interface Sci., 71 (1979) 7. M.S. Ioffe, B.N. Kuznetsov, Yu.A. Ryndin, Yu.I, Yermakov:
Sixth Intern. Congress on Catalysis, London, paper A5,1976. 8. M. Vassileva, A. Andreev, D. Shopov, M. Gabrovska: Comm.
Dept. Chem. Bulg. Acad. Sci., I-5, 267 (1982) 9. M. Vassileva, A. Andreev: Comm. Dept. Chem. Bulg. Acad. Sci.,
16, 195 (1983) 10. T. Halachev, E. Ruckenstein: Surf. Sci., 108, 292 (1981) 11. T. Halachev, E. Ruckenstein: J. Catal., 73, 171 (1982) 12. A. Andreev, M. Vassileva, K. Tenchev, D. Shopov, G.Saveleva:
React. Kinet. Catal. Lett., 23, 381 (1983). 13. M. Vassileva, G. Kadinov, Ch. Boney, A. Palazov, A. Andreev,
D. Shopov: Heterogeneous Catalysis, Sofia, Proc. V. Intern. Symp., Part I, p. 230, 1983.
14. T. Halachev, E. Ruckenstein: J. Mol. Catal., 16, 149 (1982) 15. W.H. Weinberg, D.R. Monroe, V. Lampton, R.P. Merrill: J.
Vacuum Sci. Teehnol., 14, 444 (1977)
402