Topics In Organometallic Chem - Theorectical Aspects Of Transition Metal Catalysis

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Theorectical Aspects
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Preface
It has been stated in the past that the search for new catalysts has more the 
character of an art than a science discipline. This is because there was usually
more speculation than true knowledge about the reaction mechanisms of
catalytic processes. Even the identity of the catalytically active species was 
frequently not known, which is the reason that systematic testing of all pos-
sibly interesting compounds for catalytic reactions was carried out. This is
costly and time consuming. The situation has changed in the last decade
because much progress has been made in understanding the mechanisms of
many catalytic reactions. Besides sophisticated experimental tools, quantum
chemical calculations of transition states and reaction intermediates played 
a prominent role in gaining much better insight into the fundamentals of
transition metal catalysis. Estimating solvent effects and the calculation of
spectroscopic data are now routinely included in many theoretical studies.
Although the designof new catalytically active species is still largely a trial-
and-error process, modern research is guided by theoretical calculations in
the search for new catalysts, which helps researchers to focus on more promis-
ing compounds. The progress in quantum chemical method development has
led to the present situation where theory and experiment are synergistically
used in an unprecedented manner. In particular, the calculation of transition
metal compounds is no longer a too-difficult task for quantum chemistry
because efficient methods are available for dealing with many-electron atoms
and with relativistic effects.
The seven articles in this volume do not provide a comprehensive view of
theoretical investigations of catalytic reactions, because the field has expanded
already beyond the scope that can be covered in one book. The contributions
written by experts in the field exemplarily demonstrate the strength but also
the present limitations of quantum chemical methods for giving insights into
the mechanism of transition-metal mediated reactions. Because the develop-
ment of new theoretical methods is still a very active research area, much 
progress can be expected in the coming years.
Marburg, Germany, February 2005 Gernot Frenking
Preface
Contents
Transition Metal Catalyzed ss-Bond Activation and Formation Reactions
D. G. Musaev · K. Morokuma . . . . . . . . . . . . . . . . . . . . . . . . . 1
Theoretical Studies of C-H ss-Bond Activation and Related Reactions
by Transition-Metal Complexes
S. Sakaki . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 31
Enantioselectivity in the Dihydroxylation of Alkenes 
by Osmium Complexes
G. Drudis-Solé · G. Ujaque · F. Maseras · A. Lledós . . . . . . . . . . . . . 79
Organometallacycles as Intermediates in Oxygen-Transfer Reactions.
Reality or Fiction?
D. V. Deubel · C.Loschen · G. Frenking . . . . . . . . . . . . . . . . . . . . 109
Late Transition Metals as Homo- and Co-Polymerization Catalysts
A. Michalak · T. Ziegler . . . . . . . . . . . . . . . . . . . . . . . . . . . . 145
Co-Oligomerization of 1,3-Butadiene and Ethylene Promoted 
by Zerovalent ‘Bare’ Nickel Complexes 
S. Tobisch . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 187
The Cluster Approach for the Adsorption of Small Molecules 
on Oxide Surfaces
V. Staemmler . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 219
Author Index Volume 1-14 . . . . . . . . . . . . . . . . . . . . . . . . . . 257
Subject Index . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 263
Transition Metal Catalyzed ss-Bond Activation 
and Formation Reactions
Djamaladdin G. Musaev ( ) · Keiji Morokuma
Cherry L. Emerson Center for Scientific Computation and Department of Chemistry,
Emory University, 1515 Dickey Dr., Atlanta GA 30322, USA 
dmusaev@emory.edu, morokuma@emory.edu
1 Introduction . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 2
2 The Role of the Lower-Lying Electron States of Transition Metal Cations
in Oxidative Addition of the ss-Bonds (such as H-H, C-H and C-C) . . . . . . . 2
3 Role of Cooperative Effects in the Transition Metal Clusters . . . . . . . . . . 6
3.1 Reaction of Pt and Pd Metal Atoms with H2/CH4 Molecules . . . . . . . . . . . 7
3.2 Reaction of Pd2 and Pt2 Dimers with H2/CH4 Molecules . . . . . . . . . . . . . 9
4 ss-Bond Activation via Nucleophilic Mechanism: the Role of Redox Activity 
of the Transition Metal Center – Hydrocarbon Hydroxylation
by Methanemonooxygenase (MMO) . . . . . . . . . . . . . . . . . . . . . . . 10
5 Vinyl-Vinyl Coupling on Late Transition Metals 
Through C-C Reductive Elimination Mechanism . . . . . . . . . . . . . . . . 17
5.1 Reductive Elimination from PtIV Halogen Complexes 
[Pt(CH=CH2)2X4]2– (X=Cl, Br, I) . . . . . . . . . . . . . . . . . . . . . . . . . . 18
5.2 Reductive Elimination from Mixed PtIV Complexes 
[Pt{cis-/trans-(CH=CH2)2(PH3)2}Cl2] . . . . . . . . . . . . . . . . . . . . . . . 19
5.3 Reductive Elimination from PtII Halogen Complexes 
[Pt(CH=CH2)2X2]2– (X=Cl, Br, I) . . . . . . . . . . . . . . . . . . . . . . . . . . 21
5.4 Reductive Elimination from PtII Complexes with Amine 
and Phosphine Ligands [Pt(CH=CH2)2X2] (X=NH3, PH3) . . . . . . . . . . . . 21
5.5 Reductive Elimination from PdIV Complexes [Pd(CH=CH2)2X4]2– (X=Cl, Br, I) 23
5.6 Reductive Elimination from Mixed PdIV Complex 
[Pd{trans-(CH=CH2)2(PH3)2}Cl2] . . . . . . . . . . . . . . . . . . . . . . . . . 23
5.7 Reductive Elimination from PdII Halogen Complexes 
[Pd(CH=CH2)2X2]2– (X=Cl, Br, I) . . . . . . . . . . . . . . . . . . . . . . . . . 23
5.8 Reductive Elimination from PdII Complexes with Nitrogen 
and Phosphine Ligands [Pd(CH=CH2)2X2] (X=NH3, PH3) . . . . . . . . . . . . 23
5.9 Reductive Elimination from RhIII, IrIII, RuII and OsII Complexes . . . . . . . . . 24
5.10 General Discussion . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 24
5.11 Comparison of the Vinyl-Vinyl (Csp2-Csp2) 
and Alkyl-Alkyl (Csp3-Csp3) Reductive Elimination . . . . . . . . . . . . . . . . 26
6 Concluding Remarks . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 27
References . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . 27
Topics Organomet Chem (2005) 12: 1– 30
DOI 10.1007/b104397
© Springer-Verlag Berlin Heidelberg 2005
Abstract The factors controlling the transition metal catalyzed s-bond (including H-H,
C-H and C-C) activation and formation, the fundamental steps of many chemical transfor-
mations, were analyzed. It was demonstrated that in the mono-nuclear transition metal 
systems the (1) availability of the lower lying s1dn–1 and s0dn states of the transition metal
atoms, and (2) nature of the ligands facilitating the reduction of the energy gap between the
different oxidative states of the transition metal centers are very crucial. Meanwhile, in the
transition metal clusters the “cooperative” (or “cluster”) effects play important roles in the
catalytic activities of these clusters. Another important factor affecting the catalytic activity
of the transition metal systems shown to be their redox activity.
Keywords s-Bond activation and formation · Transition metal systems · Catalytic activity
1
Introduction
Sigma-bond (including H-H, C-H and C-C) activation and formation are 
fundamental steps of many chemical transformations and have been subject of
numerous review articles [1]. It is well accepted that certain transition metal
complexes significantly facilitate the s-bond activation/formation steps, which
may occur via various mechanisms, including oxidative addition/reductive
elimination, metathesis and nucleophilic attack. However, the factors affecting
H-H, C-H and C-C activation/formation still need to be clarified in detail. In
this chapter we intend to analyze some factors that control the catalytic activ-
ity of transition metal complexes toward H-H, C-H and C-C bond activation/
formation. Namely, we elucidate the role of (a) lower-lying electronic states of
transition metal cations/atoms, (b) cooperative effects in transition metal clus-
ters, (c) redox activity of the transition metal centers, and (d) the role of metal
and ligand effects in vinyl-vinyl coupling.
2
The Role of the Lower-Lying Electron States of Transition Metal Cations 
in Oxidative Addition of the ss-Bonds (such as H-H, C-H and C-C)
The study of gas-phase activation of H-H, C-H and C-C bonds of the hydro-
gen molecule and saturated hydrocarbons, respectively, by bare transition
metal atoms and cations is very attractive for getting insight to the mecha-
nisms and factors (such as nature of metal atoms and their lower-lying 
electronic states) controlling catalytic activities of transition metal complexes.
Such studies, which are free fromthe ligand and solvent effects, have been 
subject of many experimental [2] and theoretical [3] papers in the past 
10–15 years. Experimental studies indicate that reaction of some transition
metal cations (such as Fe+, Co+, and Rh+) with methane exclusively leads to 
the ion-molecule complex M+(CH4), while others (such as Sc+ and Ir+) pro-
2 D. G. Musaev · K. Morokuma
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 3
Fi
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 o
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 r
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 M
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ceed further via oxidative addition mechanism and leads to hydrido-metal-
methyl and/or MCH2++H2 products. In order to find some insight to the dif-
ference in the reactivity of early and late, as well as first-, second- and third-
row transition metal cations (TMCs), we have studied the mechanism of
the reaction of M+ (M=Sc, Fe, Co, Rh and Ir) with CH4 at the CASSCF and 
MR-SDCI levels of theory in conjunction with large basis sets. The results of
these studies have been published elsewhere [4]. Here we discuss general
trends, factors controlling reactivity of the transition metal cations toward 
s-bonds, and predict the most favorable metal cations that can efficiently 
insert into s-bonds.
As expected, the first step of the reaction M++CH4 is the formation of
ion-molecule complex M+(CH4) (see Fig. 1, which, as an example, includes the
potential energy surface of the reaction Ir++CH4 at the several lower-lying
electronic states of the Ir cation). Our calculations show that these complexes
are structurally non-rigid, where M+ can nearly freely rotate around the CH4
molecule by the pathways (C2v)´(C3v, TS)´(C2v)´… and/or (C3v)´(C2v,
TS)´(C3v)´…, depending on the nature of metal atom and the electronic
state of the complex M+(CH4). These complexes are stable by 21.9 (M=Sc), 15.5
(13.7±0.8) (M=Fe), 21.4 (22.9±0.7) (M=Co), 16.8 (M=Rh), and 20.7 (M=Ir)
kcal/mol relative to the ground state dissociation limit M++CH4 (experimen-
tal values are given in parentheses).
From the resultant M+(CH4) complex the reaction proceeds via the C-H
bond activation transition state (TS) to give the hydrido-metal-methyl cation
complex, HMCH3+. In this step the C-H s-bond is broken and M-H and M-CH3
bonds are formed.Also, the oxidation number of the M-center increases by two.
In order to analyze the reactivity of TMCs toward C-H (as well as H-H and 
C-C) bond, one has to elucidate the factors controlling thermodynamics and 
kinetics of the reaction M+(CH4)ÆHMCH3+.
Our [4] and other [3] studies have shown that thermodynamics of the 
reaction M+(CH4)ÆHMCH3+ is controlled by the two factors. The first factor is
the availability of the s1dn–1 state of the cation M+, which is expected to be the
dominating bonding state in the resultant HMCH3+ complex. The second factor
is the loss of exchange energy (the loss of high-spin coupling (exchange energy)
between valence electrons on the unsaturated transition-metal ion subsequent
to the formation of covalent metal-ligand bonds) upon formation of M-H and
M-CH3 bonds [5]. Upon formation of M-H and M-CH3 bonds, which stabilize
the system, the loss of exchange energy occurs and counteracts the stabilization.
Thus, if the s1dn–1 configuration of the cation M+ is the energetically most favor-
able one (or easily available, i.e. the promotion energy from the ground state to
the excited s1dn–1 state is small) and the loss of exchange energy for formation
of two, M-H and M-CH3, bonds in the s1dn–1 state is small, the reaction M+(CH4)
ÆHMCH3+ is thermodynamically favorable. Taking into account these factors,
one can easily explain the calculated trends in the exothermicity of the reaction
M+(CH4)ÆHMCH3+, and predict thermodynamically the most favorable reac-
tion M+(CH4)ÆHMCH3+.
4 D. G. Musaev · K. Morokuma
Our studies show that the reaction M+(CH4)ÆHMCH3+ is endothermic by
20.3, 32.3, 37.7 and 40.3 kcal/mol for M=Sc, Fe, Co, and Rh, respectively, while
it is exothermic by 8.7 kcal/mol for M=Ir. This trend in the energy of the reac-
tion M+(CH4)ÆHMCH3+ can be qualitatively explained in terms of the energy
gap between the lower lying s0dn and s1dn–1 states of the metal cations and the
necessary exchange energy loss for formation of two covalent bonds to the
s1dn–1 state. Indeed, the s1dn–1 state is a ground state for Ir+, and thus Ir+ can 
easily form two M-L s-bonds.While the ground states of the Sc and Fe cations
are the s1dn–1 states, these cations need 3.7 and 41.4 kcal/mol energy (exchange
energy loss for formation of two covalent bonds to the s1dn–1 state) to form two
M-L bonds. Meanwhile the ground electronic configurations of Co and Rh are
the s0dn states, and the calculated exchange energy loss for formation of two 
covalent bonds to the s1dn–1 state plus s0d8Æs1d7 promotion energy are 39.2 and
77.5 kcal/mol for Co+ and Rh+, respectively. Thus, the calculated trend in the 
energy of the reaction M+(CH4)ÆHMCH3+, Ir (–6.6)<Sc (20.3)<Fe (32.3)<Co
(37.7)<Rh (40.3), is in a qualitatively agreement with the calculated exchange
energy loss for formation of two covalent bonds plus the cost of promotion 
to the s1dn–1 state: Ir<Sc (3.7)<Fe+ (41.4)~Co+ (39.2)<Rh+ (77.5) [5]. As the 
exchange plus promotion costs for formation of two bonds increases via Sc+
(3.7)<Ti+ (13.3)<V+ (32.9)<Cr+ (72.7) and then decreases via Mn+ (51.6)>Ni+
(41.6)~Fe+ (41.4)>Co+ (39.2) (in kcal/mol) [5],we expect that the thermody-
namic stability of insertion product to decrease via M=Sc+>Ti+>V+>Cr+ and
increase Mn+<Ni+~Fe+~Co+. Furthermore, it is well established that the s1dn–1
state becomes the most favorable, and the M-L bond strength significantly in-
creases for the third-row transition metal cations. Therefore, one may expect
that exothermicity of the reaction M+(CH4)ÆHMCH3+ will significantly increase
upon going from the first- and second-row TMCs to the third-row.
Meanwhile, the kinetic stability (existence of the C-H bond activation TS and
the barrier height) of the HMCH3+ complexes is mainly controlled by: (1) the
endothermicity of reaction M+(CH4)ÆHMCH3+. The large endothermicity of
reaction reduces the barrier for the reverse reaction HMCH3+ÆM+(CH4), and
makes HMCH3+ unstable relative to M+(CH4).As noted above, our studies show
that the reaction M+(CH4)ÆHMCH3+ is endothermic by 20.3, 32.3, 37.7 and
40.3 kcal/mol for M=Sc, Fe, Co, and Rh respectively, while it is 8.7 kcal/mol
exothermic for M=Ir. (2) The availability of the s0dn electronic configuration of
the metal center. It is well known that upon oxidative addition of the C-H/H-H
s-bond to transition metal center a charge transfer from the doubly occupied
C-H/H-H s-orbitals to the s (s and ds) orbitals of metal center (called “dona-
tion”) and from metal p-orbitals to the s* antibonding orbital of the C-H/H-H
bond (called “back donation”) takes place (see Scheme 1).
These interactions are efficient when the metal center has empty (or partially
empty) s-type s and ds, orbitals and occupied dp orbitals. Since Fe+, Co+, Rh+,
and Ir+ (and all late transition metal atoms) have double occupied dp orbitals but
Sc+ (and all early transition metal atoms) has none, the “back donation” effect
is expected to be larger for late transition metals compared to the early ones.
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 5
In contrast, transition metal cations such as Co+ and Rh+, have the s0dn ground
state with empty s-orbital as opposed to Sc+, Ir+, and Fe+, and one may expect
the strong s(C-H)Æ(s,ds) (M) donation effects for the former cations. Thus,
availability of the s0dn state (with doubly occupied dp and empty s-orbitals) for
Co+ and Rh+, as well as Fe+, facilitates both “donation” and “back donation”effects and makes the s-bond activation significantly easier for these cations
compared to Sc+ and Ir+. This statement is consistent with the calculated trends;
the reverse reaction HMCH3+ÆM+(CH4) occurs without barrier and is con-
trolled by thermodynamic factors for M=Fe+, Co+ and Rh+. Meanwhile reaction
M+(CH4)ÆHMCH3+ occurs with energetic barrier of 38.5 and 2.1 kcal/mol, for
M=Sc and Ir, and is controlled by both thermodynamic and kinetic factors. The
reverse reaction HMCH3+ÆM+(CH4) occurs with 18.2 and 10.8 kcal/mol barri-
ers for M=Sc and Ir, respectively.
On the basis of these discussions, we conclude that: (1) The s0dn state of the
TMC favors the formation of ion-molecule complexes, while the s1dn–1 state leads
to formation of oxidative addition product, (2) the availability of both s1dn–1 and
s0dn configurations of transition metal cations (and atoms) is absolutely neces-
sary for their reactivity toward s-bonds (such as H-H, C-H, C-C, O-H, and N-H),
and (3) all early first-row (Sc+, Ti+ and V+) transition metals cations, having
empty s or d orbitals with a1 symmetry, as well as many third-row (Hf +, Ta+, W+,
Re+, Os+, Ir+ and Pt+) TMCs, can easily activate s-bonds in the gas phase, and
stabilize the oxidative addition product complexes.
3
Role of Cooperative Effects in the Transition Metal Clusters
In this section we expand the conclusions of the previous section to bare transi-
tion metal clusters in order to test them again and to identify another,“coopera-
tive”(or “cluster”) effect that affects the reactivity of transition metals. In practice,
transition metals are important ingredients of heterogeneous and nano-catalysts,
therefore clear understanding of their reactivity at electronic level is essential to
unravel the secret of their catalytic activities.Diverse classes of experimental and
theoretical studies already have provided a wealth of information concerning the
electronic structure, spectroscopic as well as dynamic properties of variety types
of clusters, including Ptn [6], Pdn [7], Fen+ [8], Con+ [9], and Nbn+ [10].
6 D. G. Musaev · K. Morokuma
Scheme 1 Schematic presentation of “donation” and “back-donation” contributions on 
M-(HX) interaction
In particular, in the experimental work of Cox et al. [6, 7], the measured rate
constants of CH4 and H2 activation by unsupported Pt and Pd clusters (n=6~24)
show a large variation as functions of the cluster size. In the case of Pt clusters,
it was found that dimer through pentamer were the most reactive, while the 
reactivity dropped significantly starting from Pt6. The single Pt atom was less 
reactive compared to Pt2–5 by an order of magnitude, and the bulk was less 
reactive by at least several orders of magnitude. In the case of Pd clusters, it was
found that the activation rate constants for both H-H and C-H bonds show sig-
nificant oscillation in terms of the cluster size. The peak value of the measured
rate constant is around n=8 and 10, and the minimum rate constants have been
observed for n=3 and n=9. Understanding the size-dependence of reactivity of
clusters has become one of the most fascinating and intriguing issues in cluster
chemistry [11].
To unravel the reason behind the observed variation of reactivity as a func-
tion of cluster size [6, 7], we have chosen to study the detailed mechanism of
H2 and CH4 activation on small Ptn and Pdn (n=1–6) clusters. Results of these
studies have already been published [12]. Here, we intend to analyze the factors
controlling the reactivity of these clusters.
3.1
Reaction of Pt and Pd Metal Atoms with H2/CH4 Molecules
First of all, we recall briefly the electronic structure and reactivity of Pd and Pt
atoms, shown in the previous section, since they are the fundamental building
blocks of the clusters and their characteristics have a major influence on the
properties of clusters. According to a large number of theoretical as well as 
experimental studies, Pd and Pt atoms have very different electronic structures
and consequently distinct reactivities. The ground state of Pd atom has a closed-
shell s0d10 configuration, where the open-shell s1d9(3D) state is 21.9 kcal/mol
above [13]. Therefore, based on the conclusions of the previous section, one
may expect that the Pd atom cannot break the H-H or C-H bonds in H2 and CH4
and rather forms molecular complexes Pd(H2) and Pd(CH4), respectively. The 
calculated Pd-H2 bond energy is 16.2 kcal/mol. For the Pt atom, the s1d9(3D)
state is the ground electronic state, while the s0d10 configuration is 11.1 kcal/mol
higher in energy [13]. Consequently, it has been observed that Pt atom breaks
the H-H and C-H bond, in agreement with the conclusions of the previous sec-
tion. Since the ground state of Pt atom is a triplet but resultant HPtH or HPtCH3
is a singlet, a curve crossing from the triplet to the singlet state is required, and
the minimum crossing point can be viewed as the transition state for the acti-
vation process starting from the ground electronic state atom (Fig. 2a). The
binding energy of H2 and CH4 to the Pt atoms is 47.4 kcal/mol and 34.3 kcal/mol,
respectively. Thus, the calculated results for the reactions Pd+H2/CH4 and
Pt+H2/CH4 once again confirm our conclusions from the previous section.
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 7
8 D. G. Musaev · K. Morokuma
Fi
g.
2a
–d
Po
te
nt
ia
l e
ne
rg
y 
pr
of
ile
 o
ft
he
 r
ea
ct
io
ns
:a
Pt
+
H
2/
C
H
4;
b
Pd
2+
H
2;
c
Pd
2+
C
H
4;
d
Pt
2+
C
H
4
3.2
Reaction of Pd2 and Pt2 Dimers with H2/CH4 Molecules
As seen in the potential energy profile of these reactions, shown in Fig. 2b–d,
both Pd2 and Pt2 activate H-H/C-H bonds with very small barrier. In reaction
Pt2+H2/CH4, H-H/C-H activation preferentially takes place on a single metal
atom.Afterwards, one of the H atoms migrates to the other Pt atom over a neg-
ligible isomerization barrier. On both the singlet and the triplet state, H-H 
activation is expected to be barrierless, while C-H activation has a distinct 
barrier on the triplet state for reaction starting from the ground triplet state Pt2.
Nevertheless, since the barrier for C-H activation on the triplet state is small
and lower than the expected minimum of seams of crossing (MSX) between
singlet and triplet in the Pt-CH4 system, it is expected that Pt2 activates the 
C-H bond in CH4 with a faster rate than the Pt atom, which is in accord with the
experimental observation of Cox et al. [6, 7].
Calculations show that the ground state of the reactants Pd2+H2/CH4 is a
triplet state, while the product complexes have a singlet ground state. Therefore,
one may expect that the reaction proceeds either on the excited singlet state
surface or through the minimum of triplet-singlet seams of crossing. On the
singlet state potential energy surface of Pd2+H2/CH4 (see Fig. 2b,c) the reaction
is downhill without activation transition state. Meanwhile, the calculated
triplet-singlet MSX lies lower in energy than the triplet state transition state.
Therefore, the H2/CH4 activation by Pd2 starting from the triplet ground state
dimer is expected to proceed via an intersystem crossing mechanism with very
small barrier. Interestingly, the activation of s-bonds occurs only upon per-
pendicular approach of H-H/C-H bonds to the Pd-Pd bond.
Thus, in contrast to the single atom case where Pd and H2/CH4 form only a
molecular complex and no H-H/C-H bond cleavage occur, two Pd atoms work
“cooperatively” and readily break H2/CH4. This “cooperative” mechanism for
H2/CH4 activation on Pd2 is different from the case of Pt2+H2/CH4. In Pt2 dimer
H2/CH4 activation takes place preferentially on a single atom, while in Pd2 dimer
it occurs on the Pd-Pd bond. Moreover, in the final activation products, H/CH3
groups prefer the bridged sites ofPds, but are localized on metal sites in Pt2.
Those results can be rationalized as the following, as illustrated in Scheme 2. The
singlet state Pd2 consists of mainly two s0d10 Pd atoms, and the LUMO sg has a
correct symmetry to accept electron density effectively from the H2/CH4 s orbital
upon perpendicular approach.As a result, the activation takes place preferentially
in this approach. In the case of Pt2+H2/CH4 reaction, the metal HOMO and LUMO
are of localized metal d character (as established in a number of studies of metal
clusters, the s-s contribution in the metal-metal bonding is dominant, while d-d
interaction is weak). Therefore, the HOMO and LUMO of triplet Pt2 are all of
localized d characters, while the s and s* orbitals that contain large s characters
are much lower and higher in energy, respectively, and therefore activation takes
place preferentially on a single atom (rather than on the Pt-Pt bond, where the
strongest HOMO/LUMO interaction between the metal and H2 is expected.
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 9
10 D. G. Musaev · K. Morokuma
Scheme 2 Orbital diagram of triplet Pd2 and Pt2, MO energies (in hartree) are calculated at
the full valence (20el./12orb.) CASSCF level
In the final singlet products, Pt2(H)2/Pt2(H)(CH3) and Pd2(H)2/Pd2(H)(CH3),
the metal dimers actually are in their triplet configurations. In the case of Pt2,
the metal-metal s bonding orbital is low in energy, and the Pt-H/CH3 bond has
large d character. Therefore, the H/CH3 groups in Pt2(H)2/Pt2(H)(CH3) do not
like the bridged sites, but rather localize on each Pt atom. In the case of Pd2, in
its triplet electronic state, the metal-metal s bonding orbital is the HOMO.
Therefore, both the CH3/H-Pd-Pd bonding and antibonding orbitals have much
metal s component. As a result, the H/CH3 ligands prefer the bridged sites
rather than the localized metal sites.
Thus, our studies of the reactivity of Pd/Pt clusters with H2/CH4 molecules
clearly show a “cooperative” effect that could play a significant role in the re-
activity of the transition metal clusters. Thus, the catalytically inactive metal
atoms could form very active clusters !
4
ss-Bond Activation via Nucleophilic Mechanism: the Role of Redox Activity
of the Transition Metal Center – Hydrocarbon Hydroxylation 
by Methanemonooxygenase (MMO)
Another important factor controlling the reactivity of transition metal cen-
ters toward s-bond is their redox activity. Indeed, it is well established that
transition metal centers with low redox potential can be active catalysts [14].
For example, let us discuss the reactivity in hydrocarbon hydroxylation by
Methanemonooxygenase (MMO).
MMO, one of the members of diiron-containing metalloenzyme family, is 
an enzyme that catalyzes methane oxidation reaction, i.e. conversion of the 
inert methane molecule to methanol [15]. During this reaction two reducing
equivalents from HAD(P)H are utilized to split the O-O bond of O2. One O atom
is reduced to water by 2-electron reduction, while the second is incorporated
into the substrate to yield methanol:
CH4 + O2 + NAD(P)H + H+ Æ CH3OH + NAD(P)+ + H2O
Experimental studies [16] show that the best-characterized forms of the solu-
ble MMO (sMMO) contain three protein components: hydroxylase (MMOH),
so-called B component (MMOB) and reductase (MMOR), each of which is re-
quired for efficient substrate hydroxylation coupled to NADH oxidation. The
hydroxylase, MMOH, which binds O2 and substrate and catalyzes the oxidation,
is a hydroxyl-bridged binuclear iron cluster. In the resting state of MMOH
(MMOHox), the diiron cluster is in the diferric state [FeIII-FeIII], and can accept
one or two electrons to generate the mixed-valence [FeIII-FeII] or diferrous state
[FeII-FeII], respectively. The diferrous state of hydroxylase (MMOHred) is the
only one capable of reacting with dioxygen and initiating the catalytic cycle.
X-ray crystallographic studies of the enzyme from Methylococcus capsula-
tus (Bath) [17] and Methylosinus trichosporium OB3b [18] have unveiled 
the coordination environment of the Fe centers of MMOHox and MMOHred.
According to these studies, in MMOHox each Fe center has six-coordinate 
octahedral environment (see Scheme 3). Fe ions are bridged by a hydroxy ion,
a bidentate Glu g-carboxylate and a water molecule (or another carboxylate).
In addition, each Fe ion is coordinated by one His nitrogen ligand and one
monodentate Glu carboxylate. The two Fe centers are different from each other
in that one of them (Fe2) has an additional monodentate glutamate carboxylate,
while the other Fe (Fe1) has one additional water molecule. Upon reduction, one
of carboxylate ligands undergoes a so-called “1,2-carboxylate shift” from being
a terminal, monodentate ligand bound to Fe2 to a monodentate, bridging 
ligand between the two irons, with the second oxygen of this carboxylate also
coordinated to Fe2. In addition, the hydroxyl bridge is lost, and the other 
hydroxyl/water bridge shifts from serving as a bridge to being terminally
bound to Fe1. Also, the terminal water bound to Fe1 in the oxidized form of
MMOH seems to move out upon reduction of the cluster. Thus, in reduced form
of MMOHred the ligand environment of Fe ions becomes effectively five coor-
dinated, which is reasonable since this is the form of the cluster that activates
dioxygen.
It was established that MMOHred reacts very fast with O2 and forms a
metastable, so-called compound O, which spontaneously converts to another
compound called P (see Scheme 4). Spectroscopic studies [19] indicate that
compound P is a peroxide species, where both oxygens are bound symmetri-
cally to the irons. Compound P spontaneously converts to compound Q, which
was proposed to contain two antiferromagnetically coupled high-spin Fe(IV)
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 11
12 D. G. Musaev · K. Morokuma
Sc
he
m
e
3
St
ru
ct
ur
al
 r
ep
re
se
nt
at
io
n 
of
th
e 
bi
nu
cl
ea
r 
Fe
 c
en
te
r 
of
di
fe
rr
ic
 M
M
O
H
ox
an
d 
di
fe
rr
ou
s 
M
M
O
H
re
d
(s
ee
 [1
5]
)
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 13
Scheme 4 Experimentally proposed catalytic cycle of MMO (see [15])
centers. EXAFS and spectroscopic studies [20, 21] of compound Q, trapped
from M. trichosporium OB3b and M. capsulatus, have demonstrated that com-
pound Q has diamond core, (FeIV)2(m-O)2 structure with one short (1.77 Å) and
one long (2.05 Å) Fe-O bond per Fe atom and a short Fe-Fe distance of 2.46 Å.
Compound Q has been proposed to be the key oxidizing species for MMO.
In the literature there have been several computational attempts [22–25] to
elucidate mechanism of methane oxidation by intermediate Q. Our results [25]
show that reaction proceeds via the mechanism presented in Fig. 3. Later, this
mechanism was validated by several times and currently is well accepted.
As seen in Fig. 3, reaction of compound Q (modeled as structure I) with
methane starts with coordination of CH4. In general, the CH4 molecule could
coordinate to I via two distinct pathways: O-side and N-side. The O-side path-
way corresponds to the coordination of the methane molecule from the side
where the two Glu (carboxylate) located, while the N-side pathway corresponds
to the coordination of CH4 from the two His (imidazole) side. Our calculations
show that both pathways proceed via very similar transition states and inter-
mediates, and the N-side pathway is thermodynamically and kinetically more
favorable than O-side. In spite of this, in this paper we base our discussions only
on the O-side mechanism because it is believe to correspond to the process 
occurring in the protein. The coordination of CH4 to complex I leads to the
methane-Qcomplex, structure II. The interaction between methane and struc-
ture I (compound Q) is extremely weak; the complexation energy is calculated
(relative to the corresponding reactants) to be 0.7 and 0.3 kcal/mol for the 
9A and 11A state, respectively. Because of unfavorable zero point energy and 
entropy factors, it is most likely that the complex II does not exist in reality, and
therefore we will not discuss it.
Results in Table 1 show that the 9A state of structure I very qualitatively is the
Fe(IV)-Fe(IV) complex. On the other hand, in the 11A state it is the Fe(IV)-
Fe(III) mixed valence species, where Fe2 is in the Fe(III) state with five spins that
are heavily delocalized onto O2. The calculated fact that I_9 (here and below in
A_B, A is the structure, while B is the electronic state) is lower in energy than
I_11 suggests that Fe(IV)-Fe(IV) is the preferred state for complex I (and com-
pound Q). This is consistent with the experimental conclusions [21].
The activation of the methane C-H bond takes place on the diamond oxygen
O1. At the TS1, structure III, the C-H bond to be broken is elongated from
1.089 Å in II to 1.271 Å and 1.296 Å in transition states III_9 and III_11. Fur-
thermore, the O-H bond is nearly formed, with distance of 1.250 Å and 1.241 Å
at the TSs, compared to 0.983 Å and 0.978 Å in products IV_9 and IV_11,
respectively. These geometrical changes indicate clearly that III_9 and III_11
are the TSs corresponding to the H abstraction process. The H-abstraction 
barriers are calculated to be 23.2 and 19.0 kcal/mol for the 9A and 11A states,
respectively, relative to the corresponding CH4 complexes II_9 and II_11, re-
spectively. These values of the barrier are in reasonable agreement with avail-
able experimental estimates, 14–18 kcal/mol [23]. The spin densities for TS1, III,
and product IV are found to be similar to each other within their respective 9A
and 11A states (see Scheme 5 and Table 1). Furthermore, the spin densities are
nearly identical between 9A and 11A, except for those on the O2..H..CH3 frag-
14 D. G. Musaev · K. Morokuma
Fig. 3 The potential energy profile (in kcal/mol) for both the 9A state and the 11A state of
the methane activation reaction via O-site pathways: (NH2)(H2O)Fe(m-O)2(h2-COO)2Fe(H2O)-
(NH2)+CH4Æ(NH2)(H2O)Fe(m-O)(HOCH3)(h2-HCOO)2Fe(H2O)(NH2)
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 15
Scheme 5 The spin recoupling scheme in the intermediates of the reaction
Table 1 Relative (in kcal/mol, relative to the 9A reactants) energies, and Mulliken atomic spin
densities (in e) of various intermediates and transition states, for 9A and 11A states, for the 
reaction of the complex I with molecule of methanea. The numbers after slash are relative
to the 11A reactants
Structures DE (in Atomic spin densities (in e)
kcal/mol)
LnFe2 LnFe1 O2 O1 Hb CH3c
9A state
I+CH4 0.0 3.44 3.55 0.44 0.30 – –
II –1.5 3.43 3.52 0.44 0.31 – –
III 23.2 4.59 3.54 0.40 –0.37 0.06 –0.55
IV 11.3 4.64 3.51 0.43 0.08 0.00 –0.99
V 20.6 4.58 3.23 0.38 0.20 0.00 –0.73
VI –41.8 4.54 2.92 0.35 0.00 0.00 0.00
VII –34.3 4.49 2.95 0.38 0.00 0.00 0.00
IVd 23.7 4.52 1.69 0.56 0.07 0.00 0.99
11A state
I 5.4/0.0 4.62 3.47 1.03 0.43 – –
II 4.2/–1.2 4.62 3.47 1.03 0.43 – –
III 24.4/19.0 4.63 3.52 0.43 0.55 –0.07 0.59
IV –11.3/5.9 4.67 3.58 0.43 0.10 0.00 0.98
V 18.6/13.2 4.57 3.97 0.50 0.01 0.01 0.81
VI –53.9/–59.3 4.48 4.59 0.66 0.00 0.00 0.00
VII –46.7/–52.1 4.54 4.54 0.67 0.00 0.00 0.00
IVd –15.5/10.1 4.65 4.54 0.42 0.08 0.00 0.99
a Here, LnFe stands for the (H2O)(NH2)Fe-fragment. This table does not include the portion
of spin densities located on the bridging carboxylate ligands, each of which may have about
0.10–0.15e spin.
b H atom located between O2 and CH3 fragments.
c The number for the entire CH3 fragment.
ment. For the CH3 groupitself, the total Mulliken charge (not given in Table 1)
is at most +0.03e for both the 9A and 11A states and the spin densities on this
group for 9A and 11A are of same magnitude but of opposite sign. One can 
interpret all these values in the following way. In both TSs, III_9 and III_11, a
radical center begins to develop on the CH3 group, with spin densities of –0.46e
and +0.52e, respectively, and in both intermediates, IV_9 and IV_11, the CH3
group is now a real radical with spin densities of –0.98e and 1.00e, respectively.
The spin densities on Fe1 and Fe2 in IV_9 and IV_11, which formally can be
written as L4Fe(m-O)(m-OH)FeL4 with the methyl radical only weakly interact-
ing via a C...HO interaction, can qualitatively be considered to correspond to
Fe(IV) with four spins and Fe(III) with five spins, respectively. In going from
II_9 to III_9, the very qualitative formal oxidation state of Fe2 changes from
Fe(IV) to Fe(III), while from II_11 (which is already Fe(III)) to III_11, no such
change is required. Since the two Fe centers are coupled ferromagnetically in
both 9A and 11A states, the spin of the CH3 radical in both III and IV has to 
couple antiferromagnetically (with negative spin) and ferromagnetically (with
position spin) to make the total spin 2S+1 equal to 9 and 11, respectively. In the
radical complexes IV_9 and IV_11 the interaction of the CH3 radical with the
two iron atoms is very weak and, therefore, their total energies are nearly iden-
tical. It is quite interesting that we find that a mixed valence state is responsible
for the methane oxidation reaction. The present spin density analysis clearly
demonstrates that (1) the methane oxidation proceeds via a bound-radical
mechanism, and (2) the first electron transfer from substrate to Fe-centers occurs
through the TS1 and is completed at the resultant bound-radical complex IV.
The second electron transfer from the substrate to Fe-centers starts with the
recombination of methyl radical with the bridging hydroxyl ligand at the tran-
sition state, TS2, structure V. Indeed, our results show that in the 11A state upon
going from IV_11 to the methanol complex VI_11, Fe1 changes its formal oxi-
dation state from Fe(IV) with four spins to Fe(III) with five spins, while the spin
density on the methyl radical is completely annihilated upon forming a covalent
bond between CH3 and OH. The transition state V_11 has a spin distribution 
between that of IV_11 and VI_11. On the other hand, in the 9A state upon going
from IV_9 to the methanol complex VI_9, the spin density on Fe1 is reduced by
about 0.5, corresponding to the disappearance of roughly one unpaired electron.
Since Fe(V) is not a stable species, it is most likely Fe1 changed its formal oxi-
dation state from Fe(IV) with four spins to Fe(III) with five formal d electrons.
Because of the restriction 2S+1=9, i.e., the total number of unpaired electrons
must be 8 within the Fe(III)-Fe(III) core, Fe1 in VI_9 chose to form one d-lone
pair with only three spins remaining. This complex VI_9 is thus higher in en-
ergy than the corresponding complex VI_11 in violation of the Hund rule.
The barrier heights for the CH3 addition to the hydroxyl ligand calculated
relative to the intermediate IV_9 and IV_11 are 9.3 and 7.3 kcal/mol for the 9A
and 11A states, respectively. Obviously, this step of the reaction is not rate-de-
termining, and can occur rather fast. Overcoming the barriers at TS2 leads to
the complexes methanol-complexes VI, L4Fe(OHCH3)(m-O)FeL4, and completes
16 D. G. Musaev · K. Morokuma
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 17
5
Vinyl-Vinyl Coupling on Late Transition Metals Through C-C Reductive
Elimination Mechanism
Another important s-bond activation/formation process discussed in this 
article is vinyl-vinyl coupling, shown in Scheme 7.Vinyl-vinyl coupling opens
a convenient route to conjugated 1,3-dienes and is widely employed in many
catalytic coupling reactions. The great potential of the field is still undercontinuous development [26, 27] and, therefore, elucidation of the C-C bond
formation mechanism and the factors controlling it are very crucial. In litera-
ture, numerous mechanistic studies on C-C reductive elimination and reverse
process, oxidative addition (C-C bond activation), have been reported for di-
Scheme 6 The redox cycle of Fe-centers during hydrocarbon hydroxylation by MMO
the second electron transfer process. The overall reaction I + CH4ÆVI is 
calculated to be exothermic by 34.3 and 46.8 kcal/mol for the 9Aand 11A states,
respectively. The final step of elimination of the methanol molecule and regen-
eration of the enzyme could be a complex process, and possibilities of different
mechanisms exist but have not yet been studied computationally.
Thus, these results clearly show that the Fe-centers are not directly involved
in methane C-H bond cleavage. However, they play a crucial role in the methane
oxidation process, by accepting two electrons from the substrate. Having low
oxidation potential for Fe-centers is definitely an important factor in this
process and significantly facilitates it. Thus, during the hydrocarbon hydrox-
ylation by MMO, the Fe centers undergo multiple reduction and oxidation
steps; at first, MMOHox [ Fe(III)-Fe(III) state] should be reduced (2-electron 
reduction) to MMOHred [Fe(II)-Fe(II) state], then it should be oxidized (4-elec-
tron oxidation) by O2 molecule to [Fe(IV)-Fe(IV) state], after which it again is
reduced by substrate to Fe(IV)-Fe(III) state and Fe(III)-Fe(III) states (see
Scheme 6). Thus facile oxidation and reduction of Fe-center plays a crucial role
in the hydrocarbon hydroxylation by MMO.
alkyl or mixed complexes of Pt [28–34], Pd [31, 35], Rh [33], Ru [32] and Ir [33].
Also, several theoretical investigations on C-C bond activation by Pt [36–39],
Pd [36–40], Rh [40–43] and Ir [42, 44] have been performed. However, these
studies were made for Csp3-Csp3 and Csp3-Caryl (in most cases methyl-methyl and
methyl-aryl, respectively) bonds, and no theoretical study appears to have been
carried out for reductive elimination of unsaturated vinyl ligands leading to 
a conjugated product. Therefore, we have published [45] two theoretical (DFT
and ONIOM) papers on the mechanism of vinyl-vinyl C-C reductive elimina-
tion reaction on the transition metal complexes, major conclusions of which are
summarized here and compared with other C-C coupling processes. We also 
intend to analyze the factors controlling these reactions.
5.1
Reductive Elimination from PtIV Halogen Complexes [Pt(CH=CH2)2X4]2– (X=Cl, Br, I)
As shown in Fig. 4, our calculations showed that the reaction involving vinyl 
ligands may proceed via two different transition states, 1_TS and 1A_TS, which
possess s-cis and s-trans configuration around the central single bond, respec-
tively. Their corresponding energies are given in Table 2. We note here that at
the B3LYP level of theory, the calculated relative energies of s-trans, s-gauche
and s-cis conformers are 0.0, 3.5 and 4.0 kcal/mol respectively, in agreement
with earlier findings.
Reductive elimination through the s-trans pathway retains C2 symmetry and
has to overcome the activation barrier of 29.4 kcal/mol. On the other hand, ini-
tial complex (1A_Init) and transition state (1A_TS) for s-cis pathway belong to
Cs point group and the activation energy is 4.9 kcal/mol higher than for the for-
mer (Table 2). In the latter process, the product buta-1,3-diene will be released
in the s-gauche (C2) form. Reductive elimination reactions are exothermic by
17.0 and 19.9 kcal/mol for s-cis and s-trans pathways, respectively (Table 2).
Energy difference between the initial bis-s-vinyl complexes 1_Init and
1A_Init is only 0.6 kcal/mol, with the former being more stable. The relative 
order of the transition states (1_TS and 1A_TS) reflects the stability of corre-
sponding buta-1,3-diene isomers in a free form. Thus, s-cis transition states are
expected to lie higher in energy and we will continue the study following the
s-trans pathway only.
18 D. G. Musaev · K. Morokuma
Scheme 7 Vinyl-vinyl coupling reaction on transition metal complexes
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 19
Fig. 4 S-cis and s-trans reductive elimination pathways from octahedral complexes
Upon examination of the C-C reductive elimination reaction from a series
of halogen complexes (PtIV: X=Cl, Br, I; Table 2), a clear trend is observed; the
heavier the ligand, the smaller the activation barrier, and the larger the exother-
micity of the process. Therefore, the easier reductive elimination reaction
should be expected from iodide complexes of PtIV with the activation energy
of only 25.0 kcal/mol and reaction energy of –30.3 kcal/mol.
5.2
Reductive Elimination from Mixed PtIV Complexes [Pt{cis-/trans-
(CH=CH2)2(PH3)2}Cl2]
Introducing phosphine ligand either in cis or trans position to s-vinyl groups
favors C-C bond formation (Table 2). However, in the case trans substitution (4)
the influence is much larger,DE≠=18.5 kcal/mol, compared to DE≠=27.6 kcal/mol
for cis derivative (5) and DE≠=29.4 kcal/mol for the chloride complex (1). It 
is found that lower activation barriers are accompanied by higher reaction
exothermicity (cf. DEfor 1, 4 and 5 in Table 2).
20 D. G. Musaev · K. Morokuma
Ta
bl
e
2
A
ct
iv
at
io
n 
(D
E≠
,D
H
≠ ,
DG
≠ )
 a
nd
 r
ea
ct
io
n 
en
er
gi
es
 (
DE
,D
H
,D
G
) o
ft
he
 C
-C
 r
ed
uc
ti
ve
 e
lim
in
at
io
n 
st
ag
e 
in
 th
e 
ga
s 
ph
as
e 
(i
n 
kc
al
/m
ol
)a
N
o.
Sy
st
em
b
DE
≠
DE
DH
≠
DH
DG
≠
DG
1
Pt
(I
V
),
X
=
C
l
29
.4
–1
9.
9
28
.6
–1
9.
4
29
.2
–3
0.
6
1A
Pt
(I
V
),
X
=
C
l,
s-
ci
sc
34
.3
–1
7.
0
34
.0
–1
6.
0
33
.2
–2
8.
0
2
Pt
(I
V
),
X
=
Br
27
.2
–2
5.
3
26
.4
–2
4.
8
26
.5
–3
5.
9
3
Pt
(I
V
),
X
=
I
25
.0
–3
0.
3
24
.2
–2
9.
9
24
.3
–4
1.
4
4
Pt
(I
V
),
X
1,
X
2=
PH
3;
X
3,
X
4=
C
l;
18
.5
–4
0.
4
17
.5
–3
9.
9
18
.0
–5
2.
2
5
Pt
(I
V
),
X
1,
X
2=
C
l;
X
3,
X
4=
PH
3;
27
.6
–3
3.
2
26
.5
–3
3.
5
27
.6
–4
6.
6
6
Pt
(I
I)
,X
=
C
l
40
.6
–3
.7
/2
6.
1
39
.1
–2
.9
/2
7.
6
39
.0
–3
.0
/1
7.
9
7
Pt
(I
I)
,X
=
Br
35
.4
–8
.3
/2
0.
6
34
.2
–7
.3
/2
1.
9
34
.0
–7
.5
/1
2.
6
8
Pt
(I
I)
,X
=
I
31
.2
–1
2.
3/
13
.0
30
.0
–1
1.
3/
14
.3
29
.9
–1
1.
5/
5.
0
9
Pt
(I
I)
,X
=
N
H
3
35
.2
–8
.5
/0
.9
33
.7
–7
.8
/1
.5
32
.2
–9
.3
/–
10
.0
10
Pt
(I
I)
,X
=
PH
3
19
.3
–2
7.
4/
–1
7.
8
18
.2
–2
6.
4/
–1
7.
5
18
.5
–2
6.
9/
–2
9.
0
11
Pd
(I
V
),
X
=
Br
12
.9
–5
1.
3
12
.5
–5
0.
5
12
.9
–6
1.
2
12
Pd
(I
V
),
X
=
I
11
.4
–5
5.
4
10
.9
–5
4.
6
11
.3
–6
5.
8
13
Pd
(I
V
),
X
1,
X
2=
PH
3;
X
3,
X
4=
C
l;
7.
3
–5
7.
4
6.
6
–5
6.
3
7.
2
–6
7.
4
14
Pd
(I
I)
,X
=
C
l
18
.9
–2
2.
2/
2.
3
17
.8
–2
1.
1/
4.
2
18
.2
–2
1.
2/
–5
.2
15
Pd
(I
I)
,X
=
Br
15
.0
–2
6.
9/
–4
.8
14
.0
–2
5.
6/
–3
.1
14
.2
–2
6.
0/
–1
2.
2
16
Pd
(I
I)
,X
=
I
11
.9
–3
0.
8/
–1
2.
0
11
.0
–29.
5/
–1
0.
4
11
.0
–2
9.
9/
–1
9.
4
17
Pd
(I
I)
,X
=
N
H
3
15
.3
–2
5.
7/
–1
5.
4
14
.3
–2
4.
8/
–1
4.
7
13
.6
–2
6.
0/
–2
5.
5
18
Pd
(I
I)
,X
=
PH
3
6.
8
–4
2.
3/
–3
3.
8
5.
9
–4
1.
0/
–3
3.
3
6.
1
–4
2.
1/
–4
4.
4
19
[R
hI
II
(C
H
=
C
H
2)
2(
PH
3)
3C
l]
17
.8
–2
9.
1
16
.8
–2
8.
8
18
.2
–4
1.
0
20
[I
rI
II
(C
H
=
C
H
2)
2(
PH
3)
3C
l]
28
.5
–1
3.
8
27
.3
–1
3.
7
28
.4
–2
6.
4
21
[R
uI
I (
C
H
=
C
H
2)
2(
PH
3)
3C
l]
28
.1
–4
4.
8/
23
.2
27
.6
–4
2.
8/
21
.9
29
.7
–3
9.
0/
13
.0
22
[O
sI
I (
C
H
=
C
H
2)
2(
PH
3)
3C
l]
34
.1
–4
2.
2/
35
.0
33
.5
–4
0.
1/
34
.2
35
.5
–3
6.
2/
23
.4
a
DE
≠ =
E(
T
S)
–E
(I
ni
t)
;f
or
 M
IV
co
m
pl
ex
es
:D
E=
E(
Pr
od
)–
E(
In
it
);
fo
r 
M
II
co
m
pl
ex
es
:D
E=
E(
p-
C
om
p)
–E
(I
ni
t)
,w
hi
le
 t
he
 v
al
ue
s 
af
te
r/
co
rr
es
po
nd
 t
o
DE
=
E(
Pr
od
)–
E(
In
it
).
T
he
 s
am
e 
is
 a
pp
lic
ab
le
 a
ls
o 
fo
r 
en
th
al
pi
es
 a
nd
 fr
ee
 e
ne
rg
ie
s.
b
Tw
o 
vi
ny
l l
ig
an
ds
 a
re
ci
st
o 
ea
ch
 o
th
er
,X
1 
an
d 
X
2 
ar
e
tr
an
st
o 
vi
ny
l l
ig
an
ds
,a
nd
 X
3 
an
d 
X
4 
ar
e
tr
an
s t
o 
ea
ch
 o
th
er
.
c
R
ed
uc
ti
ve
 e
lim
in
at
io
n 
th
ro
ug
h 
th
e 
s-
ci
s p
at
hw
ay
 (s
ee
 F
ig
.4
);
al
l t
he
 o
th
er
 c
al
cu
la
ti
on
s 
w
er
e 
do
ne
 fo
r 
th
e 
s-
tr
an
s p
at
hw
ay
.
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 21
Reactions of both 4 and 5 lead to the same products, trans-[Pt(PH3)2Cl2] and
buta-1,3-diene. Therefore, the difference in reaction energies (DE) reflects the
relative stability of initial bis-s-vinyl derivatives; 5_Init is thermodynamically
more stable by 7.2 kcal/mol than 4_Init.Very likely, destabilization of 4_Init due
to mutual trans orientation of vinyl and phosphine ligands is responsible for
facilitating the reductive elimination process 4_InitÆÆ4_TSÆÆ4_Prod.
5.3
Reductive Elimination from PtII Halogen Complexes [Pt(CH=CH2)2X2]2– (X=Cl, Br, I)
C-C bond formation initiated from the square planar bis-s-vinyl complexes (6,
7 and 8) also proceeds through the three-centered transition state (Fig. 5). Upon
metal-carbon s-bond breakage and reductive elimination, the coordination 
vacancy becomes available at the metal center and a p-complex of buta-1,3-di-
ene is formed. Double bond coordination (h2-C=C) to the metal atom is 
preferred in this case, while the structure with central C-C bond coordination
has an imaginary frequency corresponding to h2–C–CÆh2–C=C rearrange-
ment.
The same trend as noted above for PtIV is observed for the series of PtII
complexes (6 to 8, Table 2); heavier halogen ligands make C-C bond formation
easier by decreasing the activation energy and favoring the process thermo-
dynamically. However, comparing the C-C reductive elimination reaction from
PtII (6–8, Table 2) complexes with those of PtIV (1–3, Table 2) complexes, one can
deduce a clear preference of the higher oxidation state. For the PtIV derivatives
the activation barriers are lower by 11.2–6.2 kcal/mol and the processes are
more exothermic by 16.2–18.0 kcal/mol than the corresponding PtII species.
5.4
Reductive Elimination from PtII Complexes with Amine and Phosphine Ligands
[Pt(CH=CH2)2X2] (X=NH3, PH3)
The energetics of the C-C bond formation reaction starting from the amine
complex 9 (DE≠=35.2 and DE=–8.5 kcal/mol) are similar to those for the bro-
mide derivatives (DE≠=35.4 and DE=–8.3 kcal/mol, Table 2).
However, reductive elimination reaction from phosphine complex 10 is
much easier with the activation energy of only 19.3 kcal/mol and reaction
exothermicity of –27.4 kcal/mol (Table 2). This barrier is only slightly higher
than that for the corresponding PtIV phosphine complex (4, Table 2). In addi-
tion, Pt(PH3)2 can be considered as a rather stable product in contrast to
Pt(NH3)2 and PtX22– (X=Cl, Br, I). The finding is consistent with the experi-
mental experience that phosphine is often added to reaction mixtures to 
keep the catalyst from decomposing so that the process can take place under
homogeneous conditions [1a, 28, 29, 46]. Obviously, phosphine derivatives are
the best candidates for reductive elimination process among the PtII com-
plexes.
22 D. G. Musaev · K. Morokuma
Fi
g.
5
S-
tr
an
sr
ed
uc
ti
ve
 e
lim
in
at
io
n 
pa
th
w
ay
 fr
om
 s
qu
ar
e 
pl
an
ar
 c
om
pl
ex
es
5.5
Reductive Elimination from PdIV Complexes [Pd(CH=CH2)2X4]2– (X=Cl, Br, I)
In the PdIV complexes, the C-C bond formation takes place rather easily with
very low barriers of 12.9 and 11.4 kcal/mol for 11 (X=Br) and 12 (X=I), respec-
tively (Table 2). These are about 14 kcal/mol lower than for the corresponding
PtIV complexes, while the exothermicity of the reactions is increased by as much
as 26 kcal/mol. The high exothermicity suggests very early transition state struc-
tures. The results (see Table 2) show that reductive elimination from PdIV com-
plexes would proceed most easily among the MII and MIV halogen derivatives
(M=Pt, Pd).
5.6
Reductive Elimination from Mixed PdIV Complex [Pd{trans-(CH=CH2)2(PH3)2}Cl2]
We excluded from consideration the complexes with PH3 ligands located cis to
s-bonded carbon atoms, since this type of PtIV derivatives (5, Table 2) showed
very small effect of PH3 on reaction energetics. Previous PtIV/PtII results (4 and
10, Table 2) suggest that phosphines trans to carbons should significantly 
facilitate the reductive elimination process. This trend seems to be rather gen-
eral and applicable to PdIV complexes as well; the corresponding PdIV complex
13 with phosphines trans to carbons has a low activation barrier for C-C bond
formation of only 7.3 kcal/mol.
5.7
Reductive Elimination from PdII Halogen Complexes [Pd(CH=CH2)2X2]2– (X=Cl, Br, I)
Within the series of PdII halogen complexes 14 (X=Cl), 15 (X=Br) and 16 (X=I),
the expected trends in the energies and geometry changes are again found;
the heavier the halogen, the smaller the activation energy and the earlier the 
transition state. The smallest barrier is calculated for iodide complex DE≠=
11.9 kcal/mol and the largest 18.9 kcal/mol for chloride, with bromide in-be-
tween, 15.0 kcal/mol. Increase in activation energies is accompanied by de-
crease in exothermicity (Table 2).As discussed earlier for the corresponding Pt
compounds, reductive elimination reaction from PdII halogen complexes also
gives anionic Pd0 species [47].
5.8
Reductive Elimination from PdII Complexes with Nitrogen 
and Phosphine Ligands [Pd(CH=CH2)2X2] (X=NH3, PH3)
The activation and reaction energies for the complexes with X=NH3 and X=Br
(17 and 15 in Table 2) are similar: DE≠=15.0 and 15.3 kcal/mol and DE=–26.9
and –25.7 kcal/mol for X=Br and X=NH3, respectively. Thus, both complexes
would show a similar reactivity in the reductive elimination process. However,
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 23
the stability of [Pd0Br2]2– and [Pd0(NH3)2] relative to the corresponding p-com-
plex differs significantly, the former being ca. 11 kcal/mol less stable than the 
latter.For the PdII phosphine complex 18 (X=PH3), vinyl-vinyl coupling reaction
is very easy, with the barrier of only 6.8 kcal/mol, the smallest barrier reported
in this article.
5.9
Reductive Elimination from RhIII, IrIII, RuII and OsII Complexes
We extended the study of C-C reductive elimination reactions to other members
of late transition metals in order to find possible alternatives to Pd/Pt complexes
for catalytic coupling reactions. The calculations were performed only for the
corresponding phosphine complexes, for which experimental precedents for the
reaction were reported. In the case of Rh and Ir derivatives, an extra s-bonded
ligand has to be added to maintain correct oxidation state, because RhII and 
IrII compounds are rarely known [48]. The chloride has been chosen for this 
purpose. Thus the model compounds studied are 19 [RhIII(CH=CH2)2(PH3)3Cl],
20 [IrIII(CH=CH2)2(PH3)3Cl], 21 [RuII(CH=CH2)2(PH3)3],and 22 [OsII(CH=CH2)2-
(PH3)3].
As in the previous cases (Figs. 4 and 5), vinyl-vinyl coupling for these com-
pounds also occurs through the three-centered transition states. The smallest ac-
tivation barrier among these four compounds is found for RhIII19 (17.8 kcal/mol),
while those for the other complexes are considerably higher (28.1–34.1 kcal/mol).
To summarize, the present calculations show that RhIII-based complexes can be
considered as possible catalysts for vinyl-vinyl reductive elimination, while IrIII,
RuII and OsII analogs are likely to be less active. Once again, our calculations
shown that the second raw metals have lower barriers as well as higher exother-
micity than the third row metals within each subgroup RhIII>IrIII and RuII>OsII.
5.10
General Discussion
Thus, our calculations, in an agreement with the available experiments, have
demonstrated that the reactivity of the [M(CH=CH2)2Xn] complexes (for M=Pd
and Pt) in C-C bond formation depends on the nature of the ligand X, and 
decreases in the order: X=PH3>I>Br,NH3>Cl for both MIV and MII oxidation
states. In all the cases, phosphine ligands decrease the activation barriers and
increase the exothermicity of the reaction. The present results also show that
all the second row metals (Ru, Rh and Pd) show the lower barriers and higher
exothermicity than the corresponding third raw metals (Os, Ir and Pt) within
each subgroup (Table 2), i.e. the reactivity of the studied complexes decreases
via PdII>PtII, PdIV>PtIV, RhIII>IrIII, and RuII>OsII. The complexes of PtIV are
more reactive than corresponding complexes of PtII. Similar results have been
obtained for Pd complexes, while for them this effect is less pronounced. Con-
sidering the most reactive phosphine complexes, the following overall relative
24 D. G. Musaev · K. Morokuma
reactivity order in vinyl-vinyl coupling reaction may be suggested for these
metals: PdIV, PdII>PtIV, PtII. Thus, Pd complexes are suggested to be the most 
reactive for this reaction.
Furthermore, these results again demonstrate the importance of the elec-
tronic configuration of the metal for s–bond activation/formation reaction.As
pointed out earlier, the change in the degree of oxidation of metal atoms dur-
ing the oxidative addition/reductive elimination reactions could be described
in terms of the promotion of electronic configuration of metal atoms. In the M0,
MII, and MIV complexes, both Pt and Pd atoms possess d10, s1d9 and s2d8 elec-
tronic configurations, respectively.13 In M0 no covalent bonds are possible, since
all five d orbitals are doubly occupied. In contrast, MII and MIV atoms can make
two and four covalent bonds, respectively, through the hybrid s and d orbitals.
The energy differences between the lower-lying electronic configurations of Pd
and Pt atoms, and the calculated average reaction energies for C-C reductive
elimination reactions of the Pd/Pt-complexes are given in Table 3.
As seen from Tables 3 and 2, the concept of lower lying electronic configu-
rations provides reliable qualitative description of the systems studied. In 
particular, (i) MIVÆMII reductive elimination is always more exothermic than
MIIÆM0, which is consistent with the calculated s2d8Æs1d9 and s1d9Æd10 pro-
motion energies, and (ii) both PdIVÆPdII and PdIIÆPd0 processes are more
exothermic compared to PtIVÆPtII and PtIIÆPt0, which is again agreed with the
calculated s2d8Æs1d9 and s1d9Æd10 promotion energies of Pd and Pt atoms. In
agreement with the Hammond postulate, (i) the activation energies are lower
when the reaction starts from MIV derivatives than from MII, and (ii) C-C bond
formation involving palladium complexes requires significantly smaller bar-
riers than with platinum.
Transition Metal Catalyzed s-Bond Activation and Formation Reactions 25
Table 3 Promotion and average reaction energies (in kcal/mol) for C-C reductive elimina-
tion reactions from platinum and palladium complexesa,b
Reaction Atomic energy DEaverage
differencec
X=Cl, Br, I X=PH3, NH3d
Pd Pt
Pd Pt Pd Pt
MIVÆMII –56.0 –14.8 –53.4 –27.8 –57.4 –40.4
(s2d8Æs1d9) (11,12) (2,3)
MIIÆM0 –21.9 11.1 –4.8 19.9 –33.8 –17.8
(s1d9Æs0d10) (14–16) (6–8) [–15.4] [0.9]
a The compounds used for averaging are given in parentheses (see Table 2 for energies).
b For PtII and PdII, DE with respect to the final products (MX2+diene), rather than to p-com-
plexes is used.
c Experimentally determined.
d Values for X=NH3 are given in brackets.
Similar considerations are also applicable for the reductive elimination 
reactions for the other platinum group metals. Our calculations on reductive
elimination reactions have shown an energetic preference of RhIII com-
pounds to IrIII, RuII and OsII compounds. The fact can be rationalized taking
into account that the only exothermic promotion energy of –37.6 kcal/mol13
is expected for s2d7Æs1d8 (RhIIIÆRhI). In contrast, s2d7Æs1d8(IrIIIÆIrI) and
s1d7Æd8 (RuIIÆRu0) are endothermic by 25.1 and 9.2 kcal/mol respec-
tively [13].
5.11
Comparison of the Vinyl-Vinyl (Csp2-Csp2) and Alkyl-Alkyl (Csp3-Csp3) 
Reductive Elimination
Comparing Csp2-Csp2 reductive elimination with the similar process involving
alkyl groups (Csp3-Csp3), one may clearly note the same qualitative trends.
Experimental studies have shown that dimethyl complexes of Pt(II) eliminate
ethane much easier than their Pt(II) analogs [30, 35], and reactivity of Pt(IV)
methyl complexes is higher than Pt(II) [30]. These results are in line with our
findings (Table 2).
However, the absolute values of activation energies computed for vinyl-vinyl
coupling are significantly lower than that for methyl-methyl coupling. Particu-
larly, DE≠=49.8 kcal/mol (MP4//MP2 level) [39a], DE≠=60.8 kcal/mol (MP4//HF)
[39b,c], and DH≠=41.1 kcal/mol (GVB) [37a] were reported for ethane reductive
elimination from [PtII(CH3)2(PH3)2]. The values are much higher than DE≠=1
9.3 kcal/mol (DH≠=18.2 kcal/mol) calculated in the present work for vinyl-vinyl
coupling from [PtII(CH=CH2)2(PH3)2]. Ethane elimination from [PdII(CH3)2-
(PH3)2] was found to proceed with DH≠=10 kcal/mol (GVB) [37a] and
DE≠=26.3 kcal/mol (MP4//HF) [39c], while our value for [PtII(CH=CH2)2(PH3)2]
is again lower DE≠=6.8 kcal/mol (DH≠=5.9 kcal/mol). Similar relationships are
found for the ethane reductive elimination from [RhIII(CH3)2(PH3)Cp] DE≠=
65.6 kcal/mol (MP2//HF) [43] and [PtIV(CH3)2(PH3)2Cl2] DH≠=34.2 kcal/mol
(GVB) [37a] as compared to [RhIII(CH=CH2)2(PH3)2Cl] DE≠=17.8 kcal/mol and
[PtIV(CH=CH2)2(PH3)2Cl2] DH≠=17.5 kcal/mol given in the present work. In 
addition, vinyl-vinyl coupling is generally much more exothermic than methyl-
methyl coupling [37a, 39, 43].The differences may come from the relative 
stability in the products; D(C-C) in buta-1,3-diene, 115.8 kcal/mol, is consid-
erably larger than in ethane, 90.0 kcal/mol [49]. Thus, the vinyl-vinyl coupling
is energetically more favored than the methyl-methyl reductive elimination.
These theoreticalresults fairly well agree with experimental findings, which
point out that practical implementation of Csp3–Csp3 coupling is rather prob-
lematic due to slow reductive elimination [50], in contrast to the processes 
involving vinyl groups.
26 D. G. Musaev · K. Morokuma
6
Concluding Remarks
Above we have presented four different factors that control the catalytic activ-
ity of transition metals toward s-bonds. In the mono-nuclear transition metal
systems (1) the availability of the lower lying s1dn–1 and s0dn states of the tran-
sition metal atoms, and (2) the nature of the ligands facilitating the reduction
of the energy gap between the different oxidative states of the transition metal
centers are very crucial. Meanwhile, as was demonstrated, in the transition
metal clusters the “cooperative” (or “cluster”) effects play important roles in the
catalytic activities of these clusters. Another factor, which could be very im-
portant for catalytic activity of the transition metal systems is shown to be their
redox activity.
However, those four factors are definitely not the only ones that play crucial
roles in the catalytic activity of transition metal systems with s-bonds. The
transition metal catalyzed s-bond activation and formation are very complex
processes and need more detailed investigations.
Acknowledgment Acknowledgement is made to National Science Foundation for continu-
ous support (presently CHE-0209660) of our homogeneous catalysis project.
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Transition Metal Catalyzed s-Bond Activation and Formation Reactions 27
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28 D. G. Musaev · K. Morokuma
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