Complex Chemistry

195 Pages·1984·8.145 MB·English

by  John Emsley, et al

57
erutcurtS
dna Bonding
Editors:
M. J. Clarke, Chestnut Hill • J. B. Goodenough, Oxford
J. A. Ibers, Evanston • C. K. J~rgensen, Gen~ve
D. M. P. Mingos, Oxford. J. B. Neilands, Berkeley
D. Reinen, Marburg • P. J. Sadler, London
R. Weiss, Strasbourg • R. J. P. Williams, Oxford
xelpmoC yrtsimehC
With Contributions by
J. Emsley R.D. Ernst B.J. Hathaway K.D. Warren
With 58 Figures and 93 Tables
galreV-regnirpS
Berlin Heidelberg New York Tokyo 1984
E ~ Bo~d
Professor Michael .J Clarke
Boston College, Department of Chemistry, Chestnut Hill, Massachusetts
,76120 U.S.A.
Professor John B. Goodenough
Inorganic Chemistry Laboratory, University of Oxford, South Parks
Road, Oxford OX1 3QR, Great Britain
Professor James A. Ibers
Department of Chemistry, Northwestern University Evanston, Illinois
,10206 U.S.A.
Professor naitsirhC K. Jcrgensen
D~pt. de Chimie Min6rale de l'Universit6, 30 quai Ernest Ansermet,
1121-HC Gen~ve 4
Professor David Michael P. Mingos
University of Oxford, Inorganic Chemistry Laboratory, South Parks
Road, Oxford OX1 3QR, Great Britain
Professor Joe B. sdnalieN
Biochemistry Department, University of California, Berkeley, California
,02749 U.S.A.
Professor Dirk Reinen
Fachbereich Chemie der Philipps-Universittit Marburg, Hans-Meerwein-
StraBe, D-3550 Marburg
Professor Peter .J Sadler
Birkbeck College, Department of Chemistry, University of London,
London WC1E 7HX, Great Britain
Professor Raymond ssieW
Institut Le Bel, Laboratoire de CristaUochimie et de Chimie Structurale,
4, rue Blaise Pascal, F-67070 Strasbourg Cedex
Professor Robert Joseph P. Williams
Wadham College, Inorganic Chemistry Laboratory, Oxford OX1 3QR,
Great Britain
ISBN 3-540-13411-5
Springer-Verlag Berlin Heidelberg New York Tokyo
ISBN 0-387-13411-5
Springer Verlag New York Heidelberg Berlin Tokyo
Library of Congress Catalog Card Number 6%11280
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Table of Contents
Structure and Bonding in Metal-Pentadienyl and Related Compounds
R. D. Ernst ...............................
A New Look at the Stereochemistry and Electronic Properties of
Complexes of the Copper(II) Ion
B. J. Hathaway ............................. 55
Calculations of the Jahn-Teller Coupling Constants for d X Systems in
Octahedral Symmetry via the Angular Overlap Model
K. D. Warren. ............................. 119
The Composition, Structure and Hydrogen Bonding of the fl-Diketones
J. Emsley ................................ 147
Author Index Volumes 1-57 ....................... 193
erutcurtS dna Bonding ni lyneidatneP-lateM
dna Related sdnuopmoC
Richard D. Ernst
Department of Chemistry, University of Utah, Salt Lake City, UT 84112, USA
Metal Complexes of the allyl (C3H5) and cyclopentadienyl (C5H5) ligands have played a major role
in the development of organometallic chemistry. Metal allyl complexes are well known fort he many
intricate organic transformations which they may mediate, yet often possess limited stability. Metal
cyclopentadienyl complexes on the other hand possess very high stabilities but only very limited
catalytic chemistry. The pentadienyl ligand (CsH 7 as well as various methylated derivatives) has
similarities to both the allyl and cyclopentadienyl ligands, and it has now been demonstrated that
metal pentadienyl complexes possess not only thermal stability but also chemical and catalytic
reactivities.T his favorable combination then will allow for detailed correlations to be made between
chemical reactivities and the physical natures (structural, spectroscopic, etc.) of these compounds.
In this article the presently available information on metal-pentadienyl compounds is discussed in
order to gain some understanding of their nature compared to the related allyl and cyclopentadienyl
systems, and to anticipate future applications of metal-pentadienyls. Particular emphasis is given to
the bis(pentadienyl)metal complexes, which have been referred to as the "open metallocenes".
A. Introduction ....................................... 2
B. General Electronic and Energetic Considerations .................... 2
I. Physical and Theoretical Data ........................... 2
II. Prospects Regarding Metal Pentadienyl Complex Stability and Reactivity ..... 4
C. Experimental and Theoretical Studies of Pentadienyl Anions, Radicals, and Cations . . 6
I. Preparative Methods ................................ 6
II. Unimolecular Transformations ........................... 7
III. NMR and Conformational Studies ......................... 9
IV. EPR Spectroscopy 41
. . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . . .
V. X-Ray Diffraction Studies ............................. 41
VI. Molecular Orbital Calculations ........................... 20
D. Experimental and Theoretical Studies of Transition Metal-Pentadienyl Compounds . . . 24
I. X-Ray Diffraction Studies ............................. 52
.1 Mono(pentadienyl)metal Complexes ...................... 25
2. Homoleptic Bis(pentadienyl)metal Compounds ................ 29
a. Metal-Ligand Bonding ........................... 29
b. Pentadienyl Ligand Bonding Parameters .................. 37
3. Bis(pentadienyl)metal Complexes with Additional Ligands .......... 39
II. NMR Spectroscopy ................................. 43
III. EPR Spectroscopy ................................. 44
IV. Molecular Orbital Calculations ........................... 44
E. Concluding Remarks ................................... 47
F. Abbreviations ...................................... 48
G. References ........................................ 48
StruCture and Bonding 57
Springer-Verlag @ Berlin Heidelberg 1984
2 R. D. Ernst
A. Introduction
The fields of Inorganic and Organometallic Chemistry experienced a great resurgence in
interest some thirty years ago in large part due to the accidental discovery of the unusu-
ally stable compound ferrocene .)3-1 The subsequent emergence of the cyclopentadienyl
group as one of the most important, versatile, and stabilizing ligands in all of inorganic
chemistry is well known. Fairly detailed theoretical treatments have been published to
account for the great stability of many of these compounds .)7-4 Similarly, the allyl group
was also shown early to form stable z~-complexes with transition metals ,)8 and once again
the initial discovery was rapidly followed by the dedication of a great deal of effort to the
study of such compounds .)11-9 Particularly interesting have been the fascinating applica-
tions of the allylic materials to a wide variety of organic transformations, including the
legendary "naked metal" reactions '9 .)01 A number of bonding schemes and theoretical
treatments have also appeared regarding these systems .)61-°1 It should be noted that while
metal-cyclopentadienyl compounds often possess high stabilities, quite often their reac-
tivities are rather uninteresting, at least when centered at the cyclopentadienyl ligand. Of
course, a notable exception is the organic substitution chemistry of ferrocene and related
molecules .)71 Conversely, the generally reactive metal allyl complexes often (especially in
homoleptic first-row transition metal complexes) possess low thermal stabilities, which
has provided a barrier to obtaining reasonably detailed physical data on these com-
pounds is). Note, however, that despite the disadvantage of low thermal stability, a
number of species such as C0(C3H5) 3 have proven to be useful in a large variety of
interesting transformations .)91
While the first transition metal-pentadienyl compound, Fe(CsH7)(CO)~'C10~, was
reported in %22691 this ligand has been greatly neglected in comparison to the cyclopen-
tadienyl and allyl ligands. Only recently has it become clear that pentadienyl ligands offer
substantial promise for the future of inorganic and organometallic chemistry. In part this
apparent lack of interest may have been due to the greater difficulty associated with
obtaining suitable starting materials for introducing these ligands into metal complexes.
However, now that suitable materials and methods are becoming available (see Sect.
C.I), the field of metal-pentadienyl chemistry is blossoming in many directions. It si the
purpose of this treatment to present a perspective view of some of the more important
physical, structural, and chemical aspects of pentadienyl and metal-pentadienyl chemis-
try as they now appear. Thus, the major focus of this article will be on acyclic pentadienyl
compounds. However, as it is also desired to provide at least a glimpse of how pen-
tadienyl systems compare to their allyl, butadiene, and various cyclic counterparts, a
number of these other relatives will be included where appropriate.
B. General Electronic and Energetic Considerations
L Physical and Theoretical Data
Before treating the structural and spectroscopic data pertaining to various pentadienyl
entities, it is appropriate to examine some physical and theoretical aspects which should
prove helpful to understanding and even predicting some of the features of metal-pen-
Structure and Bonding in Metal-Pentadienyl and Related Compounds 3
+ +
a-1.618 ~ a- 1.732fl
+ a- 1.000/~
a+0.618~ + _
- a+ I,O00B
+~-'~+ a+ 257.1
+ v + a+2.000/~ +
+
Fig. .1 Representations of the :t-molecular orbitals of the cyclopentadienyl (left) and pentadienyl
(right) groups
a-l.414/~
+ +
a--l.0OOB
+ +
a
~+ a+l.414fl
+
A
+/¢~ + a+ 2.000J ~
Fig. 2. Representations of the ralucelom-r~ orbitals of the cyclopropenyl (left) and allyl (right) groups
tadienyl chemistry. The pentadienyl group is a delocatized zt system which commonly
occurs as a cationic, radical, or anionic species. The :t-molecular orbitals appropriate for
this species are depicted in Fig. 1 along with the :t molecular orbitals for the cyclopen-
tadienyl group. It should be noted that the "U" pentadienyl conformation is presented
here (and elsewhere) for convenience, although the more classic treatments have gener-
ally dealt with the "W" conformation ,)12 and an "S" (sickle) conformation also is possi-
ble. For comparison, the :r molecular orbitals for the allyl and cyclopropenyl groups are
U W S
presented in Fig. 2. It can readily be seen from Fig. 1 that the pentadienyl nonbonding
orbital (half-filled for the radical) is localized on the carbon atoms in positions 1, 3 and 5.
Hence, any radical or charge character on this group will be found almost exclusively at
these three positions, as can be seen in resonance hybrids L In comparison, an allyl group
can delocalize any charge or radical character on the 1 and 3 positions, while cyclopen-
tadienyl can delocalize over all 5 positions. In general, therefore, resonance stabilization
for these species will fall in the order cyclopentadienyl > pentadienyl > allyl, although
4 R.D. Ernst
Q •
- <j --- k/
I Ia Ib Ic
the cyclopentadienyl cation is antiaromatic. As will be seen in Sect. B.II, the above MO
diagrams are useful for comparing these three delocalized systems.
A number of pertinent physical parameters which relate to various valence states for
these groups have been measured or estimated. In many cases, the actual values reported
are heavily dependent on the definitions, assumptions, or techniques used, and therefore
ranges of values often result. Nevertheless, these data are still of some use for purposes
of comparison. Thus, allyl radical resonance or stabilization energies have been esti-
mated as being anywhere from 9--25 ,)92-221om/lack with a reasonable value probably
being close to 13-14 kcal/mol .1°3 For the pentadienyl radical, the resonance energy has
been estimated as 15-24 kcal/mol, with a reasonable value probably being around
20 '721om/lack .)s3-13
From appropriate thermochemical data the standard heats of formation of the gas
41,431,
phase '42'321ylla ,/24--93 pentadieny137, and cyclopentadienyl )54'a4 radicals have been
estimated as approximately 40, 48, and 62 kcal/mol, respectively. From these and other
results the C-H bond dissociation energies of propene '32 ,42 ,92 ,164,34-o4 pentadiene37. ,14 ,134
and cyclopentadiene '44 )54 (to yield the allyl, pentadienyl, and cyclopentadienyl radicals),
have been reported to be 88, 75-82, and 82 kcal/mol, respectively. Of course, the values
for allyl and cyclopentadienyl are much better established than that for pentadienyl.
Further, other ¢omplications arise for pentadienyl in that one could deal with either 1,3-
pentadiene or 1,4-pentadiene. In any case, it should be clear that any real difference in
these values could be important in the relative ease of formation or transformation of
allyl, pentadienyl, and cyclopentadienyt ligands on a metal coordination sphere.
Other data have been obtained which reflect on transformations involving charged
ligands. Thus, the electron affinities for ,)74'821ylla pentadieny148/, and cyclopenta-
,941yneid )05 are respectively 0.55, 0.90, and 1.79 eV. The ionization potentials are respec-
tively 8.1, 7.8, and 8.7 eV '93 .)55-15 Of course, the electron affinity and ionization potential
of 5H5C must be expected to be greater than those of 5H3C or 7H5C since in the latter two
species the orbital involved is formally nonbonding, while it is bonding in the C5H5 case.
It is particularly noteworthy that both the ionization potential and the electron affinity of
pentadienyl are lower than the corresponding values for cyclopentadienyl. This suggests
that C5H5 should be more electronegative than its open counterpart (C5H7), all other
things being equal. In fact, relative gas phase acidities of propene, 1,4-pentadiene, and
cyclopentadiene have been determined by competitive measurements .1°6-65 Compared to
cyclopentadiene, 1,4-pentadiene is less acidic by ca. 6.9 kcal/mol. The value for propene
(relative to C5H6) is even larger at 34.3 kcal/mol. The approximate solution pKa values
for propene, 1,4-pentadiene, and cyclopentadiene are 40, 30, and >18, respec-
,95ylevit .)56-16
II. Prospects Regarding Metal Pentadienyl Complex Stability
and Reactivity
Having a wide variety of pertinent data on hand such as the above, it is appropriate to
attempt to anticipate the behavior of a pentadienyl ligand relative to that of the allyl and
Structure and Bonding ni Metal-Pentadienyl and Related Compounds 5
cyclopentadienyl ligands. First, the resonance hybrids of these three ligand systems can
be compared. A r/3-allyl group can be considered to bond to a metal in two hybrid forms,
Ha and Hb, each involving one sigma and one pi attachment. However, one can write
M M
M
H Ha Hb
three resonance hybrids, IIIa-Illc, to indicate the bonding of a r/Lpentadienyl ligand to
a metal. It can readily be seen that a pentadienyl ligand forms an extra :r-attachment to
I
M
III lll a lll b lll c
the metal as compared to the allyl ligand, and this allows an important expectation to be
reached. Since the total metal-ligand interaction is greater for the r/Lpentadienyl ligand
as compared to the r/3-allyl ligand, metal-pentadienyl compounds should possess greater
thermal stability than the often unstable metal-allyl compounds, and this should greatly
facilitate physical studies in this system. Other indications of stability can be gathered by
comparing the :r molecular orbitals of C5H 7 with those of CsHs, each of which can be
considered as 6n electron anions. Referring to Fig. 1, one can notice a very strong
similarity of:r molecular orbitals for the two 6n electron ligands. Thus, all of the bonding
interactions which take place between CsHs and a metal can also take place between
CsH 7 and a metal. Further, it can be seen that the energies of the three filled CsH 7 :r
molecular orbitals are on the average substantially higher than those of the correspond-
ing three filled CsHs orbitals, and the energies of the two empty CsH 7 n-molecular
orbitals are on the average substantially lower than those of the corresponding two empty
CsHs orbitals. On an energetic basis, therefore, the CsH 7 ligand could function as both a
better donor and a better acceptor than the CsHs ligand. Although other considerations
such as overlap may also be important, at least under some conditions it might be
expected that the pentadienyl ligands could actually be more strongly bound than even
the cyclopentadienyl ligand.
Besides expectations of thermal stability, there are also reasons to believe that pen-
tadienyl ligands should be capable of imparting chemical and catalytic reactivity into their
metal complexes. An important reason for the high reactivity of metal allyl complexes
has to do with the ability of the allyl ligand to bond in 3/r (/Va) as well as in r/I (/Vb)
fashion. A pentadienyl ligand should be capable of bonding in r/5, r/3, and ~/r modes
N M
/Va /Vb
(Va-c, respectively), and therefore high reactivity should also be feasible. In fact, as a
model for these important transformations one might compare the energetics of tls-~ 3
isomerizations for the C5H5 and CsH7 anions as well as the energetics of a ~3~1 isomeriza-
tion of a CsHs anion. In particular, the loss in :r-delocalization energy might be one
indicator of the barrier to such processes. Thus, in the conversion of the :r-C3H 5 anion
6 R.D. Ernst
(e = 4a + 2.828fl) to a localized anion (e = 2a) with a free olefinic bond (e = 2a +
2 fl), a loss of 0.828/3 energy units occurs. Similarly, the conversion of a r/5-CsH7 anion (e
= 6 a + 5.464/3) to a r/3-CsH7 anion (e = 4 a + 2.828/3) and a free olefinic bond results in
a loss of 0.636/3 energy units- actually less than that for the allyl ligand. Thus, energeti-
I I M
M M
Va Vb Vc
cally the metal pentadienyl complexes could be even more reactive than metal allyl
complexes, as long as such stepwise processes are involved. Of course, kinetic factors
(e.g., steric) will also make some contribution. It is, however, interesting to note that the
conversion of a r/LCsH5 anion to an r/3-CsH5 anion requires a loss of 1.644/~ units of
energy, which could easily account for the usual lack of such reactivity in these systems.
C. Experimental and Theoretical Studies of Pentadienyl Anions,
Radicals, and Cations
In this section will be included the methods of preparations, selected reactions, spectros-
copy, diffraction studies, and theoretical calculations on pentadienyl anions, radicals,
and cations. Because the anionic species are more readily obtainable and have been
greater utilized than the radical or cationic species, this treatment will naturally
emphasize these anions. Of course, the anionic species generally have a metal counterion
present, which can bring about some covalency due to metal-ligand interactions. Hence,
it can be quite arbitrary as to which metal counterions constitute an ionic compound. This
is particularly evident when one considers that even the replacement of lithium by potas-
sium can bring about major changes in the nature of ionic interactions and pentadienyl
conformation, and that the presence of coordinated Lewis bases (e.g., TMEDA) can
greatly increase ionic character. Strictly for convenience, therefore, the alkali, alkaline
earth, lanthanide and actinide metal ions will be treated here, along with zinc and
aluminum. Transition metal complexes will be considered in Sect. D.
L Preparative Methods
One of the most common routes to pentadienyl anions involves proton abstraction from a
1,4-diene. Lithium alkyls are useful reagents for these deprotonations, and a wide variety
of alkylated, arylated, and siloxylated pentadienyl anions have been prepared in this
fashion .)17-66 Alternatively, (trimethylsilylmethyt)potassium )27 and various metal
amides )37 may be employed. The above reagents have also proven effective in the synth-
eses of resonance stabilized pentadienyl anions from 1,3-dienes such as 1,3,5-triphenyl-
1,3-pentadiene 74), 1-trimethylsilyl-l,3-pentadiene 75'76), 1,5-bis(trimethylsilyl)-l,3-pen-
tadiene ,)67 and 1,3,5-tris(trimethylsilyl)-l,3-pentadiene .MT However, if non-resonance
stabilized 1,3-dienes are to be deprotonated, more reactive metallating agents are
required. One particularly effective medium is a 1 : 1 mixture of butyllithium/potassium