ISOCYANIDE COMPLEXES OF RHENIUMXANDRI SCHOULTZ Submitted in partial fulfilment of the requirements...
Transcript of ISOCYANIDE COMPLEXES OF RHENIUMXANDRI SCHOULTZ Submitted in partial fulfilment of the requirements...
ISOCYANIDE COMPLEXES OF
RHENIUM
X. SCHOULTZ
2013
ISOCYANIDE COMPLEXES OF
RHENIUM
by
XANDRI SCHOULTZ
Submitted in partial fulfilment of the requirements for the
degree of
Magister Scientiae
in the Faculty of Science at the
Nelson Mandela Metropolitan University
December 2013
Supervisor: Prof. T.I.A. Gerber
Table of Contents
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Table of Contents
Contents i
Acknowledgements iii
Abstract iv
Crystallographic Data vi
Abbreviations vii
Chapter 1
Introduction
1.1 Rhenium Background 1
1.2 Aim and Motivation of Research 2
1.3 Rhenium in Nuclear Medicine 3
1.4 Low Valent Rhenium Chemistry 7
1.5 High Valent Rhenium Coordination Chemistry 14
1.6 References 18
Chapter 2
Experimental
2.1 Handling of Rhenium 23
2.2 Materials 23
2.3 Instrumentation 26
2.4 References 27
Table of Contents
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Chapter 3
Complexes of Aniline Derivatives Containing the ReCl3(CNR)
Core
3.1 Introduction 29
3.2 Experimental 32
3.3 Results and Discussion 35
3.4 References 59
Chapter 4
Isolation of Bis-isocyanide Complexes of Re(I)
4.1 Introduction 72
4.2 Experimental 73
4.3 Results and Discussion 74
4.4 References 85
Chapter 5
Reactivity of Re(V) with Isocyanides
5.1 Introduction 92
5.2 Experimental 93
5.3 Results and Discussion 94
5.4 References 102
Chapter 6
Conclusion and Future Work 109
Acknowledgements
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Acknowledgements
I would like to express my very great appreciation to Prof. T.I.A. Gerber for the
opportunity of working under his supervision. All his patient guidance, enthusiastic
encouragement and useful critiques are much appreciated and is truly motivating.
I would like to offer my special thanks to Dr. E. Hosten, Dr. R. Betz and Dr. B.J.A.M van
Brecht for their assistance with the crystallographic analysis.
I am particularly grateful to H. Schalekamp for the exceptional technical assistance he
has given me.
Technical assistance given by E. Bashman, P. Gaika, H. Marchant and V. Maqoko are
also greatly appreciated.
My special thanks are extended to all the rhenium chemistry students and other
colleagues who are so helpful and motivating.
I am grateful toward Nelson Mandela Metropolitan University, National Research
Foundation and NTemBi/NECSA for financial assistance.
I would also like to express my gratitude toward my family and friends for their moral
support and encouragement.
Finally, I would also like to thank God for giving me this amazing opportunity, and for
giving the strength and determination to succeed.
Abstract
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Abstract
This study investigates the synthesis of rhenium(III)-isocyanide complexes with
potentially bidentate ligands, as well as the reactivity of isocyanide ligands toward
rhenium(I) and (V). The crystal structures of all the complexes have been determined by
X-ray diffraction methods.
The coordination behaviour of trans-[ReIIICl3(t-BuNC)(PPh3)2] with aniline and its
derivatives were investigated. The isocyanide-containing rhenium(V) complexes
[ReCl3(t-BuNC)(L)(PPh3)] were isolated, with the ligands H2L (aniline, o-
phenylenediamine and anthranilic acid). In all these complexes the dianionic ligands L
are coordinated monodentately as the imide. However, with 2-aminophenol the
complexes [ReVCl2(t-BuNC)(L)(PPh3)2](ReO4) and [ReIIICl2(t-BuNC)(ibq)(PPh3)2] (ibq- =
2-iminobenzoquinonate) were identified as the products. [ReCl2(t-
BuNC)(L)(PPh3)2](ReO4) is the product of a disproportionation reaction from Re(III) to
Re(VII) and Re(V). All the above complexes show a distorted octahedral geometry
around the rhenium.
The products of the reaction of the Re(I) complex [Re(CO)5Cl] with isocyanides (tert-
butyl- and cyclohexylisocyanide) are reported. Rhenium(I) tricarbonyl complexes of the
form [Re(CO)3(CNR)2Cl] were isolated and they were characterized structurally and
spectroscopically. The tricarbonyls are coordinated in the typical facial-fashion, whereas
the isocyanides are coordinated cis to each other. The reaction of [Re(CO)3(t-BuNC)2Cl]
with H2O led to the formation of the rhenium(I) complex [Re(CO)3(t-BuNC)2(OH2)] in
which the aquo ligand can readily be substituted by a more complex ligand.
Abstract
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The reaction of the rhenium(V) complexes cis-[ReO2I(PPh3)2] and mer-
[ReOCl3(SMe2)(OPPh3)] with isocyanides were studied. The seven-coordinate trigonal
prismatic, square faced monocapped rhenium(III) complex [ReI3(t-BuNC)3(PPh3)] was
surprisingly isolated upon reacting cis-[ReO2I(PPh3)2] with tert-butyl isocyanide. The
dimeric complex (μ-O)[ReOCl2(CNC6H11)2]2 was obtained from the reaction of mer-
[ReOCl3(SMe2)(OPPh3)] with cyclohexyl isocyanide.
Keywords: Rhenium, isocyanides, aniline, derivatives, dimeric
Crystallographic Data
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Crystallographic Data
Additional data and refinement details for all crystal structures analysed in this study are
stored on the compact disk included in this thesis (attached at the back).
These crystallographic data include the following:
All crystal data and details of the structure determinations;
Final coordinates and equivalent isotropic displacement parameters of the non-
hydrogen atoms;
Hydrogen atom positions and isotropic displacement parameters;
Anisotropic and isotropic displacement parameters;
Bond distances;
Bond angles;
Torsion angles;
Contact distances;
Hydrogen bonds.
Abbreviations
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Abbreviations
anal. calcd. elemental analysis calculated
CyNC cyclohexyl isocyanide
d doublet
DMF dimethylformamide
dppe diphosphine
H2aa anthranilic acid
H2an aniline
H2ap 2-aminophenol
H2pd o-phenylenediamine
ibq 2-iminobenzoquinonate
IR infrared
MeCN acetonitrile
m multiplet
NMR nuclear magnetic resonance
Ph phenyl
phen o-phenanthroline
pyr pyridine
s singlet
t triplet
t-BuNC tert-butyl isocyanide
Chapter 1 Introduction
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Chapter 1
Introduction
1.1 Rhenium Background
Rhenium has expansive coordination chemistry due to its characteristics of both early
and late transition metal complexes. It can exist in many oxidation states and binds to
various ligands systems to give stable complexes. Oxo- and imido-ligands are known to
form stable rhenium(V) cores, such as [ReO]3+, [ReO2]+, [ReN]2+ and [ReNR]3+, which
are important constituents of radio-labeled therapeutic agents [1]. Ligands such as
carbonyls with significant π-back bonding capabilities also bind to rhenium in various
oxidation states and is known to be part of the stable Re(I) (d6) core [2].
Due to its extensive coordination chemistry, and the fact that it has two radioactive
isotopes 188Re and 186Re, which are β—emitters, makes this unique metal applicable to
nuclear medicine therapy [3]. Successful employment in nuclear medicine requires
these rhenium compounds to be thermodynamically stable under both thermal and
hydrolytic conditions [4].
The 188Re isotope has up until now been the isotope which shows most promise in the
radiotherapeutic industry, due to its high beta energy. However, 186Re has proved to
also possess exceptional properties, as illustrated in Figure 1.1, giving it wide potential
radiopharmaceutical uses [3, 5]. The 188Re is relatively easy to produce from the
188W/188Re generator; however, it is limited to some extent in radiopharmaceutical uses
due to its relatively short half life [5, 6]. The 186Re radionuclide is generated by the
radioactive decay of 186W or via commercially available generators [5].
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Figure 1.1 - Rhenium radionuclide physical properties
1.2 Aim and Motivation of Research
This project mainly deals with the reactivity of isocyanides towards Re(III) and the more
developed Re(I) and Re(V) oxidation states. The particular interest in isocyanide ligands
are due to their unique physical, chemical and ligation properties. The isocyanide
coordination chemistry towards technetium has been studied quite well and they are
known to form extremely stable complexes with technetium [7]. The technetium
compound used as a radiopharmaceutical in heart-imaging (Tc(MIBI)6+, where MIBI = 2-
methyoxy-2-methylpropyl-isocyanide) is a well known example, and serves as
motivation for this particular interest in isocyanide chemistry.
The chemistry of Re(I) and Re(V) has been investigated quite extensively, leading to the
discovery of the stable cores [Re(CO)3]+ and [ReO]3+ respectively. Limited research has
been done on the +III oxidation state of rhenium and no stable core is yet known. One
0
2
4
6
8
10
12
14
16
Halflife (hr) ( × 10) Max beta energy(MeV)
Range in tissue(mm)
Gamma energy(keV) (× 10)
Re-186
Re-188
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of the main objectives in this study was to investigate the reactivity of rhenium(III)
compounds, with the aim of developing such a stable core.
Rhenium complexes containing multidentate ligands are potential models for
radiotherapeutic agents based on 186Re, especially if they can be coupled to a biological
relevant receptor [8]. Rhenium(III) complexes of the form trans-[ReCl3(CNR)(PPh3)2]
could be a potential precursor for the preparation of rhenium(III) complexes, where the
ligands consist of a multidentate ligand and isocyanide [8]. Considering the stability of
the rhenium-isocyanide bond, reaction of bidentate N-, O-, S-donor ligands should not
affect the rhenium-isocyanide bond, thus leading to a stable [ReIII(CNR)] core.
Re(I) complexes containing the fac-[Re(CO)3]+ core are known to be kinetically and
thermodynamically unreactive, and by adjusting the specific ligand, different
characteristics can be shaped, depending on the complexes of interest [9]. The
combination of the tricarbonyl moiety with isonitriles as a ligand system might give the
metal complex the required properties to be suitable as a therapeutic agent, specifically
in the heart due to its cationic nature. This study thus also deals with the preparation of
such complexes.
Lastly, the reactivity of Re(V), in particular [ReO2I(PPh3)2], with isocyanides were also
investigated. After seeing the interesting coordination of isonitriles with Re(I) and Re(III),
its reactivity with Re(V) was also intriguing.
1.3 Rhenium in Nuclear Medicine
Radiopharmaceuticals have shown to be very effective for diagnostic purposes in
nuclear medicine. The pattern of distribution of radiation in an organ system over a
certain period of time enables one to make an appropriate diagnostic evaluation.
Therapeutic radiopharmaceuticals have also shown very promising applications over
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the last decade, with rhenium being one of the elements possessing radioactive
properties which shows most potential [10].
1.3.1 Rhenium vs. Technetium
Rhenium is a congener of technetium with very similar physical characteristics [11].
99mTc is the ideal radionuclide in diagnosis, but for therapeutic uses the requirements
are complex, since it not only depends on the nuclear, chemical and biological
properties, but also on the nature and localization of the pathological processes [6].
Although technetium and rhenium are so similar in terms of most properties, rhenium is
more easily oxidized and kinetically inert in comparison to technetium. This means that
in vivo oxidation to ReO4- occurs more readily than technetium - thus making it ideal for
therapeutic purposes [12].
The similarities between these two elements is highly advantageous, since extensive
research has been done on the technetium radio isotopes, and approaches to labeling
agents with 99mTc could theoretically be adapted for use with rhenium [6].
1.3.2 Rhenium Nuclides in Therapy
The use of antibody therapy for tumour destruction was based on the natural
mechanism of antibodies to perform different effector functions, such as lysis of tumour
cells by programmed cell death (apoptosis). These antibodies can produce cytotoxic
effects on the tumour cells in addition to the effects of radiation, thus making it highly
advantageous [10].
The ideal radiopharmaceutical would be one that is relatively easy to synthesize, would
have stability as well as selective biodistribution in vivo, after which it is able to clear the
body with minimal side-effects [13]. In radiotherapy, it is necessary to use radiation that
can penetrate the body to the location of the tumour. Thus it is dependent upon the
radionuclide’s radiation properties [14].
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186Re has a half-life of 89.3 hours and upon decaying, a β-particle is emitted with a
maximum energy of 1.1 MeV, as well as a 135 keV gamma particle enabling imaging.
Due to its relatively long half-life, it enables efficient distribution in the body. This nuclide
is produced in a nuclear reactor easily obtainable world-wide, where the choice of
reactor depends on the specific activity requirements. The rhenium radionuclide 188Re
has a half-life of 16.9 hours and its β-particle has a much higher maximum energy of
2.12 MeV with a 135 keV gamma photon, thus also giving it imaging capabilities [15]. Its
half-life is much shorter than that of 186Re, giving it a higher specific activity, and
consequently lower doses are required. It can be disadvantageous in that it decays too
quickly, thus not reaching its final destination before emitting radiation [16]. It can be
produced either using a nuclear reactor, or in a generator – the W188/Re188-generator is
the most common method [17].
Based on the above, it is clear that receptor-targeted radiopharmaceuticals have great
potential in diagnostic imaging and therapy, especially the radioactive rhenium nuclides
due to their exceptional physical properties [18].
1.3.3 Technetium Nuclides for Imaging
The use of 99mTc complexes as imaging agents has been extremely successful in the
past two decades. There has been great success in many regions, including brain,
kidney, liver, heart and bone imaging [5]. The 99mTc complex of particular interest,
especially in this study, is [99mTc(MIBI)6]+ (Figure 1.2), where MIBI represents 2-
methoxy-2-methylpropyl-isocyanide [19]. This positively-charged complex is known to
accumulate in the heart via the Na/K-ATPase pump, with its lipophilicity being an
important physical property enabling this uptake [5, 20]. The overall negative potentials
in the cytosol and mitochondria allows the positively-charged complex to accumulate in
the heart [20]. The isocyanide ligands have great ligation properties and stabilizes the
low oxidation state well [20]. The methoxy group enhances the metabolization of the
untrapped complex by cleavage of the ether to an alcohol, and subsequent excretion by
the kidneys [20].
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The 99mTc-MIBI analogue consisting of aryl bidentate isocyanides have also been
synthesized, showing similar myocardial uptake to Cardiolite (Figure 1.2) [21]. The
bidentate nature of the isocyanide ligands allows better charge distribution and also
increases the lipophilicity [21].
Figure 1.2 - Structure of CardioliteTM (A) and its bidentate analogue (B)
1.3.4 Clinical Applications of 186/188Re
Rhenium radio-isotopes have a broad spectrum of clinical applications due to its
advantageous properties. Both 186Re- and 188Re-hydroxyethylidenediphosphonate
(HEDP) are radiopharmaceuticals that have been used for the palliation of painful bone
metastases in patients [22]. The rhenium radio-isotopes was used to selectively
accumulate in the bone by adsorption to the surface of the hydroxyapatite mediated by
hydroxide bridges [23]. This is metabolically controlled to ensure that hypermetabolic
regions of the bone and joints will receive significant higher radiation than other skeletal
regions with normal metabolism [22]. 186Re-HEDP results in considerable pain relief and
mild toxicity at low doses. More than 50% of the administered activity is cleared through
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the kidneys within 24 hours, thus making the radiation-exposure side-effects minimal.
The 188Re-HEDP have also been synthesized, as well as 188Re-dimercaptosuccinic acid
(DMSA) which is specific to bone metastases from prostate cancer [22, 24].
Due to the effectiveness of rhenium radioactive targeting in bone metastasis, its
applicability to osteosarcoma’s (relatively radio-resistant tumours) have also been
investigated. It was found that it significantly decreased radiation side-effects and
resulted in excellent long-term control [25].
Other common applications include 188Re-perrhenate and 188Re-mercaptoacetyl
triglycine in endovascular radiation therapy, 188Re-peptides in tumour therapy, 188Re-
particles in catheter administration, 188Re-antigranulocyte antibodies in marrow ablation
prior to stem cell rescue, and 186Re-sulphide in synovectomy [6]. Restenosis, which is a
process relatively common in cases of artherosclerotic coronary artery disease, could
possibly be prevented by the use of the β-emitting 188Re isotope [26].
These are just some main indications of successful applications of
radiopharmaceuticals labeled with rhenium radioactive isotopes; however its
applications are much broader. By using rhenium radiopharmaceuticals, it could not
only enhance the therapeutic effectiveness toward cancer cells, but also potentially treat
arthiritis and inhibit arterial restenosis [27].
1.4 Low Valent Rhenium Chemistry
Rhenium is known to exist in many oxidation states, from -I to +VII. The chemistry of the
+I, +V and +VII oxidation states have been investigated most extensively, with the
higher oxidation states being the most common [11]. This is readily seen from the stable
metal cores [ReO]3+, [ReO2]+, [ReN]2+, [ReNR]3+ and [Re(CO)3]+ [1]. The need to
stabilize the metal by pi-acceptors ligands increases as one goes to the lower oxidation
states of rhenium, and thus these classes of ligands will predominate the discussion of
low valent rhenium complexes.
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1.4.1 Ligands for Stabilizing Low Valent Rhenium Complexes
Low oxidation state rhenium metal centers readily accept electron density from electron-
rich ligands, thereby stabilizing the resulting metal complex. Carbonyls is an example of
such a ligand and is known to be part of the stable Re(I) core [Re(CO)3]+ [2].
The Re(I) tricarbonyl core possess a d6 electronic low-spin configuration, making it both
thermodynamically and kinetically inert – more so in comparison to the higher valent
rhenium complexes, such as Re(V). It is synthesized as an aqua-complex, namely
[Re(CO)3(OH2)3]+ via perrhenate reduction. The aqua ligands are easily substituted by
other ligands – ideally tridentate ligands to fill the three vacant coordination sites [27].
Isocyanides are versatile ligands which are isoelectronic with carbon monoxide. The
physical, steric and electronic properties of metal isonitriles can be modified by
changing the substituent on the isocyanide ligand – a characteristic that carbonyls
unfortunately lack [28]. The HOMO of the C=N-R ligand donates electrons from the filled
π-orbital or lone pair orbital to an empty orbital on rhenium (4s/4p) via σ-donation. The
LUMO of the C=N-R ligand is empty and accepts electrons from the 5d orbital of
rhenium. This electron transfer is known as the synergic effect (Figure 1.3). If π-back
bonding is exceptionally strong, the normal linear isocyanide ligand would become bent
at the nitrogen atom (129°-144°), indicating that the metal-carbon bond has a bond
order of two [29].
The coordination chemistry of rhenium with isocyanides is not nearly as developed as
that of rhenium-carbonyl chemistry. Other common ligands that have been found to
efficiently stabilize the lower oxidation states of rhenium are phosphines and polypyridyl
ligands, which are also pi-acids [2].
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Figure 1.3 - Coordination modes of isocyanides and carbonyl to metals
1.4.2 Rhenium(I) Coordination Chemistry
(a) General chemistry of the Re(I)-tricarbonyl core
The chemistry of rhenium(I) has been explored extensively since the discovery of the
rhenium-tricarbonyl core [30]. The fascination with this specific core structure is the
fixed three carbonyls such that three facial positions are unoccupied allowing
multidentate ligands to readily bind to the metal core [31]. As stated earlier, Re(I)-
tricarbonyl complexes are known to be kinetically and thermodynamically stable, and by
varying the ligand coordinated to the metal centre the desired complexes with specific
properties can be fashioned [9]. It was found that even monodentate ligands with low
thermodynamic stability can give stable metal complexes, if the electronic properties of
the ligand allow it [32].
The fac-[Re(CO)3]+ core has been reacted with a variety of multidentate ligands - one of
the earliest studies was with imidazoles and histamine/histidines, as depicted in Figure
1.4 [32]. The ligands that have shown to efficiently bind and stabilize this core contain
amine, aromatic N-heterocycles and carboxylate donors [31].
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Figure 1.4: Early reactivity of fac-[Re(CO)3]+
Rhenium pentacarbonyl chloride [Re(CO)5Cl] has been used as a precursor for many
stable complexes, including the examples illustrated in Figure 1.5 [33]. It is clear from
the Scheme below that the pentacarbonyl rhenium complex can be used as starting
material for various compounds containing the stable tricarbonyl core.
Figure 1.5: Reactivity of Re(CO)5Cl [33]
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(b) Multidentate coordination towards the Re(I) tricarbonyl core
There have been multiple complexes containing bidentate coordinating chelates since
the discovery of the tricarbonyl core. The donor atoms are typically N-, O-, S- or P-
donor ligands. Tridentate chelators containing these donor atoms have shown to
produce stable organometallic compounds, ideal for in vivo conditions [34].
Some of the latest work include complexes with terpyridine (Figure 1.6). The unique
feature of these complexes are that the carbonyls are coordinated in a meridional
fashion, which can be more advantageous than the usual bidentate diimine Re(I)
tricarbonyl complexes [35].
Figure 1.6: Reactivity of terpyridine [35]
The preparation of tridentate chelating systems for coordination with [Re(CO)3]+ usually
requires multiple steps for successful synthesis and its subsequent reactivity under in
vivo conditions can be problematic, and therefore ligands must be carefully considered.
Recent successful work includes the reaction of azide-functionalized compounds with
alkyne prochelators to give a triazole-containing tridentate ligand [34]. Reaction of these
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tridentate chelators to the tricarbonyl core gives a variety of complexes, structurally
different, with unique physical properties, as depicted in Figure 1.7 below [34].
Figure 1.7: Tridentate ligand coordination to [Re(CO)3]+
1.4.3 Rhenium(III) Coordination Chemistry
The chemistry of rhenium in the +III oxidation state have not been studied very
extensively, although a number of stable complexes have been isolated. An interesting
example is its complexes with organohydrazines. These ligands are versatile and
reducing in nature, thus making them ideal for radiopharmaceutical use. They have
shown to prefer Re(III) metal centres, evident from the fact that whether the precursor
compound was in +V or +VII state, it reduced to the +III state yielding an inert, stable
complex as depicted in Figure 1.8 [37].
Figure 1.8: Reactivity of ReOCl3(PPh3)2 with organohydrazines
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Interestingly, very few penta-coordinate Re(III) compounds have been isolated thus far.
An example is the unexpected reduction of oxorhenium((V) upon coordination with a
thiolate ligand (Figure 1.9) [38].
Figure 1.9: Reactivity of [ReOCl3(PPh3)2] with p-methoxybenzyl mercaptan
A similar unexpected reduction of the [ReOCl3(PPh3)2] complex was observed by its
reaction with a Schiff base derivative as illustrated below (Figure 1.10) [39].
Figure 1.10: Reactivity of ReOCl3(PPh3)2 with 2-(2-aminobenzylideneimino)phenol
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1.5 High Valent Rhenium Coordination Chemistry
Extensive research has been done on the +V oxidation of rhenium. The chemistry of
rhenium is thus dominated by this particular oxidation state, due to its unique and stable
physical properties.
1.5.1 Re(V)-oxo chemistry
The +V oxidation state of rhenium is the most diverse and explored oxidation state, and
is known to undergo a variety of reactions, as illustrated below.
(a) Oxidation
A novel cationic rhenium hydrazido complex [ReCl2(NNMePh)2(PPh3)](BPh4) was
isolated by the reaction of trans-[ReOCl3(PPh3)2] with an excess of the unsymmetrically
disubstituted organohydrazine MePhNNH2 in boiling methanol, as illustrated by the
equation below [40]. Upon recrystallization, the highly unstable PF6- salt decomposes to
give a dicationic complex [ReOCl(NNMePh)(PPh3)2](PF6)2 [40].
trans-[ReOCl3(PPh3)2] + MePhNNH2 [ReOCl(NNMePh)(PPh3)2]2+ + 2Cl- + H2O
(b) Reduction
Rhenium(III) complexes can readily be obtained by the reduction of Re(V) by PPh3 in
the presence of suitable ligands such as isonitriles [41].
trans-[ReOCl3(PPh3)2] + CNC(CH3)3 + PPh3 [ReCl3(CNC(CH3)3)(PPh3)2] + OPPh3
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(c) Disproportionation
The reaction of trans-[ReOCl3(PPh3)2] with 1,10-phenanthroline in ethanol gives the
disproportionation products [ReIIICl2(phen)(PPh3)2]+ and perrhenate [42]. Similar
reaction products are obtained when using biimidazole as opposed to the
phenanthronline ligand [42].
trans-[ReOCl3(PPh3)2] + phen [ReCl2(phen)(PPh3)2]+ + [ReO4]-
(d) Ligand Substitution
There are various factors that affect the way in which a ligand coordinates to a metal. It
depends on the structural characteristics, the temperature of the reaction mixture, the
ligand to metal mole ratio and the solvent, to name a few. It is not that common for a
solvent to influence the product, although it has been seen multiple times, as in the
example below with diphosphine [43].
[ReOCl3(OPPh3)(Me2S)] + dppe 𝑇𝐻𝐹→ [ReOCl3(dppe)] + OPPh3 + Me2S
[ReOCl3(OPPh3)(Me2S)] + dppe 𝐸𝑡ℎ𝑎𝑛𝑜𝑙→ [ReOCl2(OEt)(dppe)] + OPPh3 + Me2S + HCl
1.5.2 Re(V)-imido chemistry
The organoimido core M=N-R has proven to be of great use in the radiopharmaceutical
industry, since different organic substituents can be integrated into this stable entity
[44]. The bond between the nitrogen atom and the rhenium metal centre consists of one
sigma and two pi-bonds [43]. Its hybridization depends on whether the bonding mode is
linear or bent, as illustrated in Figure 1.11 below [43].
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Figure 1.11: Organoimido core bonding modes
The linear structure (a) is more common and usually written as M=NR, although
technically speaking it is a triple bond [43]. The nitrogen in structure (a) is a sp-
hybridized nitrogen. The bent structure (b) is fairly uncommon and its nitrogen is sp2-
hybridized. An example of a complex with a bent structure is [Mo(NPh)2(S2CNEt2)2]
where the M-N-C angle is 139° [44].
There have been numerous synthetic methods reported for the preparation of imido
complexes. The synthesis of imido complexes directly from perrhenate is essential for
its feasibility to act as a radiopharmaceutical [44]. Another common method is the use of
aniline or its derivatives with trans-[ReOCl3(PPh3)2], or the reaction of metal chlorides
with primary amines, as depicted below [44, 45].
trans-[ReOCl3(PPh3)2] + H2NC6H5 [ReCl3(NC6H5)(PPh3)2]
[ReCl4(Cp)] + H2NC6H5 [ReCl2(NC6H5)(Cp)] (Cp = cyclopentadienyl)
1.5.3 Re(V) coordination chemistry
Most current studies on the coordination chemistry of rhenium focus on the +V oxidation
state. Numerous complexes in this state have been prepared with a broad class of
ligands typically containing N, S, P and O donor atoms. Re(V) complexes have also
been used multiple times for the preparation of rhenium compounds in other oxidation
states.
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Schiff bases are a versatile class of ligands, and due to its potential multidenticity a
great deal of attention has been paid to these types of ligands [46]. Therefore, the Re(V)
coordination chemistry discussion will focus on Schiff base coordination.
N-(2-amino-3-methylphenyl)salicylideneimine gave a rather interesting complex upon
reaction with ammonium perrhenate, triphenylphosphine and hydrochloric acid in glacial
acetic acid [47]. The ligand acts as a tridentate N,N,O-ligand coordinating through a
doubly deprotonated nitrogen atom (imido), a neutral imino and a phenolate oxygen
[46]. The imido nitrogen and phenolate oxygen lie in the trans axial positions, as
illustrated below (Figure 1.12) [47].
Figure 1.12: Structure of Re(V)-Schiff base complex
Another unusual example of Schiff base coordination is illustrated below, where the
Schiff base undergoes structural changes upon coordination. In the complexes with the
Schiff base in Figure 1.13, structure a shows the product of the reaction of the Re(V)-
oxo precursor [ReOCl3(PPh3)2] with 2-(2-hydroxyphenyl)phenol [46]. In structure b the
product as obtained from the reaction of [ReOCl3(PPh3)2] with 2-
(salicylideneamino)benzenethiol. The resulting complex contained this ligand in two
different forms, thus given a 2+3 ligand system of O,N and S,N,O respectively. This is
very unusual, and quite intriguing [46].
Chapter 1 Introduction
18 | P a g e Nelson Mandela Metropolitan University
Figure 1.13: Re(V) complexes with structurally modified Schiff base ligands
1.6 References
[1] K.C. Potgieter, Complexes of the ReO3+/Re(CO)3+ cores with multidentate N,O-
donor chelates, MSc Dissertation, Nelson Mandela Metropolitan University,
South Africa, 2009, 2.
[2] N.C. Yumata, Reactivity of Rhenium(III) and Rhenium(V) with Multidentate NN-
and NO-Donor Ligands, MSc Dissertation, Nelson Mandela Metropolitan
University, South Africa, 2010.
[3] U. Abram, R. Alberto, J. Braz. Chem. Soc., 2006, 17, 1486.
[4] V. Bertolasi, C. Bianchini, I. de le Rios, A. Marchi, L. Marvelli, M. Peruzzini, R.
Rossi, Inorg. Chim. Acta, 2002, 327, 140.
Chapter 1 Introduction
19 | P a g e Nelson Mandela Metropolitan University
[5] G. Kemp, Mechanistic study of rhenium(I) carbonyl complexes as model
radiophamaceuticals, PhD Thesis, The University of Johannesburg, South Africa,
2008.
[6] D. Lukic, J. Vucina, Physics, Chemistry and Technology, 2002, 2, 236.
[7] R. Alberto, H. Braband, N.I. Gorshkov, V.V. Gurzhiy, S.V. Krivovichev, E.M.
Levitskaya, A.A. Lumpov, A.E. Miroslavov, G.V. Sidorenko, D.N. Suglobov, I.G.
Tananaev, J. Organomet. Chem., 2008, 693, 7.
[8] F.E. Hahn, M. Glaser, T. Lugger, D. Scheller, H. Spies, Inorg. Chim. Acta, 1995,
232, 235.
[9] R. Alberto, R. Schibli, R. Waibel, U. Abram, A.P. Schubiger, Coord. Chem. Rev.,
1999, 190, 901.
[10] S.W. Falen, R.J. Kowalsky, Radiopharmaceuticals in Nuclear Pharmacy and
Nuclear Medicine, 2nd edition, American Pharmacists Association, Washington
DC, 2004, 1; 235; 767-768.
[11] C.S. Cutler, H.M. Hennkens, S. Huclier-Markai, S.S. Jurisson, N. Sisay, Chem.
Rev., 2013, 113, 870.
[12] M.S. Kovacs. The coordination chemistry of rhenium, group 13 and lanthanide
metal complexes: towards new radiotherapeutic agents, PhD Dissertation, The
University of British Columbia, Canada, 2001, 9.
[13] J.B. Arterburn, D.M. Goreham, M.S. Holguin, K.V. Rao, M.V. Valenzuela,
Organomettallics, 2009, 19, 1789.
Chapter 1 Introduction
20 | P a g e Nelson Mandela Metropolitan University
[14] J.C. Kotz, P.M. Treichel, J.R. Townsend, Chemistry and Chemical Reactivity, 7th
edition, Thomson Brooks/Cole, 2008, pp 1086, 1085.
[15] A.L. Beets, F.F. Knapp, J. Krop, W.Y. Lin, J. Pinkert, S.Y. Wang, Rhenium
Radioisotopes for Therapeutic Radiopharmaceutical Development. In:
International Seminar on Therapeutic Applications of Radiopharmaceuticals, pp
1-2. Proceedings of an International Seminar Held in Hyderabad, India 18-22
January 1999. IAEA-SR-209.
[16] J. Wilson, W. Walker, Principles and Techniques of Biochemistry and
Microbiology, 7th edition, Cambridge University Press, New York, 2010.
[17] T. Bandurski, M. Derejko, G. Romanowicz, J. Scheffler, Nucl. Med. Rev., 2003,
6, 55.
[18] J.B. Arterburn, M.C. Perry, K.V. Rao, Angew. Chem. Int. Ed., 2000. 39, 771.
[19] C. Jonsson, H. Jacobsson, Ann. Nucl. Med., 1996, 10, 281.
[20] S. Bouquillon, N, Chemin, A, Du Moulinet D’Hardemarke, D. Fagret, M. Vidal,
Appl. Radiot. Isot., 1996, 47, 479.
[21] B. Das, D. Elmaleh, A. Fischman, L. McIntosh, J. Pitman, T. Shoup, J. Nucl.
Med., 2006, 47, 524.
[22] M. Bangard, H.J. Biersack, C. Menzel, H. Palmedo, J. Risse, J.K. Rockstroh, K.
Schliefer, Radiology, 2001, 221, 257.
[23] P.J. Blower, S. Prakash, Perspective on Bioinorganic Chemistry, 1999, 4, 123.
[24] H.G. van der Poel, EAU-EBU update series, 2007, 5, 117.
Chapter 1 Introduction
21 | P a g e Nelson Mandela Metropolitan University
[25] A.M. Cassoni, E.J. Sawyer, W. Waddington, British J. Radiol., 1999, 72, 1226.
[26] B. Hsieh, J. Hsieh, H. Huang, W. Lin, G. Ting, S. Tsai, S. Wang, Nucl. Med. Biol.,
1999, 26, 967.
[27] M. Andreou, M. Argyrou, M. Lyra, A. Valassi, Intern. Mol. Imag., 2013, 2013, 6.
[28] A.W. Chung, C. Ko, L.T. Lo, C. Ng, S. Yiu, Coord. Chem. Rev., 2012, 256, 1547.
[29] R.H. Crabtree, The Organometallic Chemistry of the Transition Metals, 3rd
edition, Wiley-Interscience Publication, Canada, 2001, 87-88.
[30] U. Abram, R. Alberto, A. Egli, T.A. Kaden, R. Schibli, A.P. Schubiger, J. Am.
Chem. Soc., 1998, 120, 7987.
[31] J. Babich, S.R. Banerjee, M.K. Levadala, L. Wei, J. Zubieta, Inorg. Chem.
Comm., 2003, 6, 1099.
[32] U. Abram, R. Alberto, R. Schibli, A.P. Schubiger, R. Waibel, Coord. Chem. Rev.,
1999, 190, 908.
[33] A. Earnshaw, N.N. Greenwood, Chemistry of the Elements. Butterworth-
Heinemannm Oxford, 1997.
[34] C.A. Kluba, T.L. Mindt, Molecules, 2013, 18, 3207.
[35] D.R. Black., S.E. Hightower, Inorg. Chem. Comm., 2012, 24, 16.
[36] H. Berke, O. Blacque, T. Fox, C.M. Frech, Y. Jiang, Chem. Eur. J., 2010, 16,
2240.
Chapter 1 Introduction
22 | P a g e Nelson Mandela Metropolitan University
[37] W.M. Davis, A. Davison, M. Hirsch-Kuchma, A.G. Jones, T. Nicholson, Inorg.
Chem., 1997, 36, 3237.
[38] P. Bouziotis, E. Chiotellis, M.S. Papadopoulos, I.C. Pirmettis, C.P. Raptopoulou,
A. Terzis, Inorg. Chim. Acta, 1990, 290, 249.
[39] T.I.A. Gerber, K.C. Potgieter, P. Mayer, Polyhedron, 2010, 29, 1424.
[40] M.M. Lynam, J.C. Vites, Coord. Chem. Rev., 1995, 142, 3.
[41] F.E. Hahn, L. Imhoff , T. Lugger, Inorg Chim. Acta, 1998, 269, 347.
[42] M. Jaworska, J. Klak, R. Kruszynski, B. Machura, J. Mrozinski, Polyhedron,
2006, 25, 2538.
[43] A.L. Beauchamp, O. Sigouin, Inorg. Chim. Acta, 2005, 358, 4490.
[44] M.T. Ahmet, B. Coutinho, J.R. Dilworth, J.R. Miller, S.J. Parrott, Y. Zheng,
Polyhedron, 1996, 15, 2041.
[45] R.A. Eikey, M.M. Abu-Omar, Coord. Chem. Rev., 2003, 243, 85.
[46] J.Y. Kim, Y.J. Jon, H.J. Ha, H.K. Chae, Bull. Korean. Chem. Soc., 2003, 24, 504.
[47] I. Booysen, T.I.A. Gerber, E. Hosten, P. Mayer, Bull. Chem. Soc. Ethiop., 2008,
22, 101.
Chapter 2 Experimental
23 | P a g e Nelson Mandela Metropolitan University
Chapter 2
Experimental
2.1 Handling of Rhenium Rhenium occurs naturally as a mixture of two non-radioactive isotopes, namely the
stable 185Re and the unstable 187Re, with natural abundances of 37.40% and 62.60%
respectively. The non-radioactive isotopes were used in this study, thus no special
safety precautions were taken in handling the metal.
2.2 Materials
2.2.1 Chemicals
Ammonium perrhenate (NH4)[ReO4] was obtained commercially from Sigma-Aldrich and
required no further purification. All common laboratory chemicals were of reagent grade
and were used as received from suppliers. Commercially obtained chemicals are
tabulated below (Table 2.1), and were used as received.
Table 2.1: Chemicals obtained commercially.
Chemical Supplier
2-aminophenol >99%, Fluka
2-aminothiophenol 98%, Alfa Aesa
o-phenylenediamine BDH Chem Ltd
anthranilic acid 99.5%, Riedel de Haen
Chapter 2 Experimental
24 | P a g e Nelson Mandela Metropolitan University
2.2.2 Precursor compounds
(a) trans-[ReOCl3(PPh3)2]
A solution of perrhenic acid was prepared by dissolving ammonium perrhenate (1.0 g,
3.7 mmol) in 3 mL concentrated hydrochloric acid. This solution was added to a
suspension of triphenylphosphine (5.0 g, 19.1 mmol) in 50 mL glacial acetic acid under
nitrogen. A green solid was removed by vacuum filtration and washed with glacial acetic
acid and diethyl ether [1]. Yield = 97%, m.p. 252 °C. Anal. Calcd. for C36H30OCl3P2Re
(%): (Mw = 833.16 g/mol) C, 51.90; H, 3.63. Found: C, 52.12; H, 3.69. IR (νmax/cm-1):
ν(Re=O) 998(s).
(b) trans-[ReCl3(MeCN)(PPh3)2]
A mixture of trans-[ReOCl3(PPh3)2] (2.5 g, 3.0 mmol), triphenylphosphine (2.5 g, 9.5
mmol), acetonitrile (17.5 mL) and toluene (20 mL) was stirred for 2 hours at reflux under
nitrogen. After an hour an orange solid formed, which upon cooling to room
temperature, was collected through vacuum filtration and washed with 50 mL ethanol
[2]. Yield = 87%, m.p. 290-296 °C. Anal. Calcd. for C38H33Cl3NP2Re (%): (Mw = 858
g/mol) C, 53.20, H, 3.86, N, 1.63. Found: C, 54.06; H, 3.61; N, 2.25. IR (νmax/cm-1):
ν(Re-N) 501(s).
(c) trans-[ReCl3(CNC(CH3)3)(PPh3)2]
The method obtained from the literature [3] was adapted as follows: trans-
[ReCl3(MeCN)(PPh3)2] (200 mg, 0.233 mmol) was dissolved in 10 mL dry benzene
under nitrogen. tert-Butylisocyanide (29 mg, 0.350 mmol) was added and the reaction
mixture was refluxed under nitrogen for 3 hours. The volume was reduced under
nitrogen and a yellow precipitate was collected. Yield = 58%, m.p. 189 – 192 °C. Anal.
Chapter 2 Experimental
25 | P a g e Nelson Mandela Metropolitan University
Calcd. for C41H39Cl3NP2Re (%):(Mw = 899 g/mol) C, 54.70; H, 4.37; N, 1.56. Found: C,
53.87; H, 4.51; N, 2.30. IR (νmax/cm-1): ν(C≡N) 2144(s).
(d) trans-[ReOI2(OEt)(PPh3)2]
5.0 g of Triphenylphosphine was added to 1.0 g of (NH4)[ReO4] in 30 mL ethanol and 5
mL hydroiodic acid (56%), and the mixture was heated under reflux for 15 minutes.
Upon cooling to room temperature, the green precipitate was filtered, washed with
ethanol and diethyl ether, and dried under vacuum [1]. Yield = 82 %. m.p. 150-154°C.
Anal. Calcd. for C38H35I2O2P2Re (%): (Mw = 1142.8 g/mol) C, 44.50; H, 3.44. Found: C,
43.09; H, 3.44. IR (νmax/cm-1): ν(Re=O) 906(s).
(e) cis-[ReO2I(PPh3)2]
A mass of 1.0 g of trans-[ReOI2(OEt)(PPh3)2] was stirred in a solution of 50 mL acetone
and 2 mL distilled H2O at room temperature for an hour. A purple crystalline product
was isolated, washed with acetone and diethyl ether, and dried under vacuum [1]. Yield
= 75 %. m.p. 169-171°C. Anal. Calcd. for C36H30IO2P2Re (%): (Mw = 869.68 g/mol) C,
49.72; H, 3.48. Found: C, 49.19; H, 2.61. IR (νmax/cm-1): ν(Re=O) 907(s).
(f) mer-[ReOCl3(SMe2)(OPPh3)]
A solution of 1.0 g of trans-[ReOCl3(PPh3)2] and 0.1 mL of Me2SO in 80 mL benzene
was stirred under nitrogen for 2 days at room temperature. The light green precipitate
was filtered under vacuum and washed with diethyl ether. [4] Yield = 70 %. m.p. 222-
227 °C. Anal. Calcd. for C20H19Cl3O2PRe (%): (Mw = 652.01 g/mol) C, 32.86; H, 3.71;
S, 4.92. Found: C, 32.30; H, 3.34; S, 4.06. IR (νmax/cm-1): ν(Re=O) 989(s).
Chapter 2 Experimental
26 | P a g e Nelson Mandela Metropolitan University
2.3 Instrumentation
2.3.1 Analytical Techniques
All infrared spectra were obtained using a Bruker Tensor 27 spectrophotometer.
All NMR spectra were collected at 300K using a 300 MHz Bruker AMX-300
spectrometer with chemical shifts relative to SiMe4.
A Perkin-Elmer Lamda 35 UV/Vis spectrophotometer was used for absorption spectra.
Melting points were determined using a Lasec Stuart SMP30 melting point apparatus.
A BASi Epsilon EC-2000 cyclic voltameter was used for cyclic voltammetry. The three
electrode system consists of a platium working electrode, a platinum wire auxiliary
electrode and a pseudo silver/silver chloride reference electrode. The supporting
electrolyte tetrabutylammoniumtoluene-4-sulfonate had a final concentration of 0.1 M
and the respective compounds analyzed had concentrations of 10-3 M. All the cyclic
voltammetric runs were done at a scan rate of 100 mV/s, scanning between 1500 mV to
-1500 mV and back to 1500 mV. Each sample was deoxygenated before each run by
bubbling nitrogen through the solution for 10-15 minutes.
All conductivity measurements were done on a Hanna HI2300 EC/TDS/NaCl meter. The
conductivity measurements obtained were compared with expected conductivity values
at a concentration of 10-3 M (Table 2.2) [1, 5].
Chapter 2 Experimental
27 | P a g e Nelson Mandela Metropolitan University
Table 2.2: Conductivity ranges expected for electrolyte types in organic solvents.
Solvent Conductivity measurement in
1:1 electrolyte (μS)
Conductivity measurement in
1:2 electrolyte (μS)
Acetonitrile 120-160 220-300
Methanol 80-115 160-220
DMF 65-90 130-170
2.3.2 Crystallography
A Bruker Kappa Apex II diffractometer in the conventional ω-2θ scan mode and
monochromatic Mo-Kα radiation (λ = 0.71073 Å) was used for X-ray crystallographic
analysis.
2.3.3 Computational studies
Density functional theory (DFT) and time-dependent DFT were performed by Dr. P.
Ramasam from the Computational Chemistry Group, Department of Chemistry, Faculty
of Science, University of Mauritius, Réduit, Mauritius.
2.4 References
[1] K.C. Potgieter, Rhenium Complexes with Multidentate Benzazoles and Related
N,X-Donor (X = N, O, S) Ligands, PhD Thesis, Nelson Mandela Metropolitan
University, South Africa, 2012, 28.
[2] N.C. Yumata, Reactivity of Rhenium(III) and Rhenium(V) with Multidentate NN-
and NO-Donor Ligands, MSc Dissertation, Nelson Mandela Metropolitan
University, South Africa, 2009, 29.
Chapter 2 Experimental
28 | P a g e Nelson Mandela Metropolitan University
[3] F.E. Hahn, M. Glaser, T. Lugger, D. Scheller, H. Spies, Inorg. Chim. Acta, 1995,
232, 232.
[4] J.C. Bryan, R.E. Stenkamp, T.H. Tulip, J.M. Mayer, Inorg. Chem., 1987, 26,
2283.
[5] H. Fazilati, H. Golchoubian, Iranica Journal of Energy & Environment, 2012, 3,
266.
Chapter 3 ReCl3(CNR) Core
29 | P a g e Nelson Mandela Metropolitan University
Chapter 3
Complexes of Aniline Derivatives
Containing the ReCl3(CNR) Core
3.1 Introduction
The potential relevance of the 186/188Re radionuclides in nuclear medicine makes the
coordination behaviour of rhenium of particular interest [1]. Although Re(I) complexes of
isocyanides have been studied extensively, not many research efforts focused on their
reactivity towards Re(III) and Re(V). Our initial approach was that the compound trans-
[ReCl3(CNR)(PPh3)2] could be a potential precursor for the synthesis of Re(III)-isonitrile
complexes [2]. In this study, the products of the reaction of trans-[ReCl3(t-
BuNC)(PPh3)2] with aniline and selected potential bidentate derivatives were
investigated. The retainment of the Re(CNR) bond in the +III oxidation state could lead
to a novel core for radiopharmaceutical purposes.
Aniline derivatives have unique chelating abilities, and have therefore attracted a lot of
research interest [3]. The coordination behaviour of rhenium(V) with aniline and its
derivates H2L (H2L = anthranilic acid, o-phenylenediamine, 2-aminophenol) (Figure 3.1)
has been previously studied and leads to complexes in various oxidation states and
results in quite unusual structural properties [4, 5, 6, 7]. These ligands have the ability to
coordinate in a monodentate or a bidentate fashion and are strong enough to bond to
rhenium at low concentration to give a single product in high yield [5, 6, 8].
This study centers on the reaction of trans-[ReCl3(t-BuNC)(PPh3)2] with aniline (H2an)
and its derivatives anthranilic acid (H2aa), o-phenylenediamine (H2pd) and 2-
Chapter 3 ReCl3(CNR) Core
30 | P a g e Nelson Mandela Metropolitan University
aminophenol (H2ap) in an attempt to synthesize complexes of rhenium(III) that contain
an isocyanide ligand. The choice of starting complex was influenced by the reported
higher yields obtained by using [ReCl3(t-BuNC)(PPh3)2] rather than trans-
[ReCl3(MeCN)(PPh3)2] or by the reduction of trans-[ReOCl3(PPh3)2] with an excess of
triphenylphosphine [1].
Figure 3.1: Ligands used in this study
The reaction of trans-[ReCl3(t-BuNC)(PPh3)2] with the potentially bidentate ligands H2L
(H2L = aniline (1), o-phenylenediamine (2), anthranilic acid (3)) surprisingly led to the
isolation of rhenium(V) complexes [ReCl3(t-BuNC)(L)(PPh3)2], in which the ligands L are
coordinated as dianionic monodentate imides (Figure 3.2). Complex 2 was also
synthesized by the reaction of trans-[ReOCl3(PPh3)2] with H2pd in ethanol to form trans-
[ReCl3(pd)(PPh3)2], which was subsequently reacted with t-BuNC in toluene.
By using 2-aminophenol (H2ap) as possible ligand, the rhenium(V) complex salt trans-
[ReCl2(t-BuCN)(ap)(PPh3)2](ReO4) (4) was obtained, with ap also coordinated as an
imide after several recrystallization steps. We can’t offer any explanation for this
anomalous behavior of H2ap. However, the crystals obtained from the mother liquor of
the synthetic solution of 4 led to the formation of the complex trans-[ReCl2(t-
BuCN)(ibq)(PPh3)2] (5) (ibq = 2-iminobenzoquinonate), where ibq coordinates through a
monoanionic imino nitrogen. The oxidation of the ligand is shown in Figure 3.3.
Chapter 3 ReCl3(CNR) Core
31 | P a g e Nelson Mandela Metropolitan University
Figure 3.2: Reaction pathway of trans-[ReCl3(CNC(CH3)3)(PPh3)2] with H2L
Figure 3.3: 2-Aminophenol oxidation and coordination modes for 5
Re
N
Cl
Ph3P
ClN
Y
Re
N
PPh3
Ph3P
Cl
Cl
Cl
N2,
NH2
X
(1) X = H; Y = Cl; Z = H
(2) X = NH2; Y = Cl; Z = NH2
(3) X = COOH; Y = Cl; Z = COOH
(4) X = OH; Y = PPh3; Z = OH
(5) X = OH; Y = PPh3; Z = (=O)
5
4
3
2
6
1
Z
(1)/(2) Acetontrile (3)/(4)/(5) Benzene
Chapter 3 ReCl3(CNR) Core
32 | P a g e Nelson Mandela Metropolitan University
3.2 Experimental
3.2.1 Synthesis of trans-[ReCl3(t-BuNC)(PPh3)(an)] (1)
To a solution of trans-[ReCl3(t-BuNC)(PPh3)2] (75 mg, 0.08 mmol) in 10 mL acetonitrile
was added 15.2 μL of aniline (H2an, 0.17 mmol), and the mixture was heated under
reflux in a nitrogen atmosphere for 3 hours. Cooling to room temperature and removal
of the solvent under vacuum gave a green precipitate, which was filtered off.
Recrystallization from hot ethanol gave dark green crystals. Yield = 47%, m.p. >300°C.
Anal. Calcd. (%): C, 47.78; H, 4.01; N, 3.84. Found: C, 47.71; H, 3.33; N, 3.92. IR
(νmax/cm-1): ν(C≡N) 2187(m); ν(Re=C) 1184(m); ν(Re=N) 1088(m). 1H-NMR (295K, ppm,
CDCl3): 7.80 (d, 3H), 7.52 (d, 3H), 7.33-7.41 (m, 6H, PPh3); 7.19 (m, 9H, PPh3); 1.37 (s,
9H, 3xCH3). UV/Vis (CH3CN, λmax (ε, M-1cm-1)): 390 (1175), 680 (100). Conductivity
(CH3CN, μS): 4.
3.2.2 Synthesis of trans-[ReCl3(t-BuNC)(PPh3)(pd)] (2)
trans-[ReCl3(t-BuNC)(PPh3)2] (75 mg, 0.08 mmol) and o-phenylenediamine (H2pd, 18
mg, 0.17 mmol) were dissolved in 10 mL acetonitrile, and the mixture was heated under
reflux under nitrogen for 2 hours. No precipitate was obtained, but slow evaporation of
the mother liquor gave dark brown crystals suitable for X-ray diffraction after 3 days.
The complex crystallized as the solvate 2∙CH3CN. Yield = 54%, m.p. 125-127°C. Anal.
Calcd. (%): C, 46.80; H, 4.34; N, 7.07. Found: C, 46.56; H, 4.06; N, 6.62. IR (νmax/cm-1):
ν(C≡N) 2196(m); ν(Re=C) 1192(m); ν(Re=N) 1090(m). 1H-NMR (295K, ppm, CDCl3):
7.09 (t, 1H), 6.34 (d, 1H), 7.33-7.75 (m, 9H, PPh3); 7.19 (m, 6H, PPh3 ); 6.08 (d, 1H),
5.95 (d, 1H); 1.18 (s, 9H, 3xCH3). UV/Vis (MeOH, λmax (ε, M-1cm-1)): 346 (740), 480
(550), 669 (370). Conductivity (MeOH, μS): 8.
Complex 2 was also synthesized by dissolving trans-[ReOCl3(PPh3)2] (150 mg, 0.18
mmol) and H2pd (22 mg, 0.20 mmol) in 20 mL ethanol and heated under reflux for an
Chapter 3 ReCl3(CNR) Core
33 | P a g e Nelson Mandela Metropolitan University
hour. A red precipitate [Re(pd)Cl3(PPh3)2] [9] was obtained of which 50 mg (0.05 mmol)
was reacted with tert-butyl isocyanide (12.3 μL, 0.11 mmol) and refluxed for another
hour. Evaporation of the mother liquor gave X-ray quality crystals after 5 days. The
complex did not crystallize with any solvent of crystallization. An X-ray analysis showed
the product to be trans-[ReCl3(t-BuNC)(PPh3)(pd)]. Yield = 33 %, m.p. 124-128 °C. IR
(νmax/cm-1): ν(C≡N) 2190(m); ν(Re=C) 1188(m); ν(Re=N) 1089(m).
3.2.3 Synthesis of trans-[ReCl3(t-BuNC)(PPh3)(aa)] (3)
trans-[ReCl3(t-BuNC)(PPh3)2] (100 mg, 0.11mmol) and anthranilic acid (H2aa, 46 mg,
0.33 mmol) were dissolved in 20 mL benzene and heated under reflux under nitrogen
for 3 hours. A feather-like green precipitate was obtained, which was recrystallized from
dichloromethane:diethyl ether 1:2 v/v using the vapour diffusion crystallization method.
The green crystals isolated after 2 days were suitable for X-ray diffraction studies. Yield
= 39%, m.p. >300°C. Anal. Calcd. (%): C, 47.11; H, 3.78; N, 3.62. Found: C, 46.60; H,
4.26; N, 4.62. IR (νmax/cm-1): ν(C≡N) 2204(m); ν(CO2) 1663(m); ν(Re=C) 1192(m);
ν(Re=N) 1089(m). 1H-NMR (295K, ppm, d6-DMSO): 6.67 (d, 1H), 6.54 (t, 1H), 7.26 (t,
1H), 7.70 (t, 1H), 7.22-7.56 (m, 15H, PPh3), 7.85 (t, 1H), 1.39 (s, 9, 3xCH3). UV/Vis
(DMF, λmax (ε, M-1cm-1)): 384 (2030). Conductivity (DMF, μS): 27.
3.2.4 Synthesis of trans-[ReCl2(t-BuNC)(PPh3)2(ap)](ReO4) (4)
trans-[ReCl3(t-BuNC)(PPh3)2] (100 mg, 0.11 mmol) and 2-aminophenol (H2ap, 36 mg,
0.33 mmol) were dissolved in 20 mL benzene and heated to reflux under nitrogen for an
hour. The solution became red, forming a brown precipitate, which was filtered after
heating was stopped and cooled to room temperature. The material was recrystallized
from methanol to give yellow-brown crystals, suitable for X-ray diffraction. Yield = 30%,
m.p. 163-167°C. Anal. Calcd. (%): C, 45.5; H, 3.7; N, 2.3. Found: C, 47.0; H, 3.5; N,
2.1. IR (νmax/cm-1): ν(O-H) 3225(w), ν(C≡N) 2206(m); ν(Re=C) 1266(m); ν(Re=N)
1089(m), ν(ReO4-) 908(s). 1H-NMR (295K, ppm, CDCl3): 7.57-7.63 (m, 2H), 7.66 (m, 6H,
PPh3); 7.49 (t, 1H), 7.40 (t, 1H), 7.28 (m, 15H, PPh3); 7.19 (m, 9H, PPh3), 2.10 (s, 9H,
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3xCH3). UV/Vis (DMF, λmax (ε, M-1cm-1)): 287 (1810), 408 (446), 499 (186).
Conductivity (DMF, μS): 69.
3.2.5 Synthesis of trans-[ReCl2(t-BuNC)(PPh3)2(ibq)] (5)
trans-[ReCl3(t-BuNC)(PPh3)2] (100 mg, 0.11 mmol) and H2ap (36 mg, 0.33 mmol) were
dissolved in 20 mL benzene and heated to reflux under nitrogen for an hour. The
solution became red, forming a brown precipitate which was filtered. The mother liquor
was evaporated slowly over a period of 3 days to give red-brown crystals, suitable for X-
ray diffraction. Yield = 59%, m.p. 189-183°C. Anal. Calcd. (%): C, 58.31; H, 4.67; N,
2.88. Found: C, 56.98; H, 5.19; N, 2.95. IR (νmax/cm-1): ν(C≡N) 2195(m); ν(Re=C)
1262(m); ν(Re=N) 1071(m), ν(C=O) 1606(m), ν(C=N) 1534(m). 1H-NMR (295K, ppm,
CDCl3): 7.58 (m, 2H), 7.67 (m, 6H, PPh3); 7.43 (d, 1H), 7.32 (t, 1H), 7.26 (m, 15H,
PPh3); 7.19 (m, 9H, PPh3), 2.11 (s, 9H, 3xCH3). UV/Vis (DMF, λmax (ε, M-1cm-1)): 326
(710), 437 (410), 501 (600), 549 (408). Conductivity (DMF, μS): 3.
3.2.6 X-ray crystallography
X-Ray diffraction studies of complexes 1 – 5 were performed at 200 K using a Bruker
Kappa Apex II diffractometer with graphite monochromated Mo Kα radiation (λ =
0.71073 Å). APEX-II was used for data collection and SAINT for cell refinement and
data reduction [10]. The structures were solved by direct methods using SHELXS-2013
[11] and refined by least-squares procedures using SHELXL-2013 [11] with SHELXLE
[12] as a graphical interface. Data were corrected for absorption effects using the
numerical method implemented in SADABS [10].
All non-hydrogen atoms were refined anisotropically. Carbon-bound H atoms were
placed in calculated positions (C-H 0.95 Å for aromatic carbon atoms and C-H 0.99 Å
for methylene groups) and were included in the refinement in the riding model
approximations, with Uiso(H) set to 1.2Ueq(C). The H atoms of the methyl groups were
allowed to rotate with a fixed angle around the C-C bond to best fit the experimental
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electron density (HFIX 137 in SHELXL [BB]), with Uiso(H) set to 1.5Ueq(C). The H atom
of the hydroxyl groups were placed in calculated positions (HFIX 83 in SHELXL [11])
with Uiso(H) set to 1.5Ueq(O). Nitrogen-bound H atoms were located on a difference
Fourier map and refined riding the Uiso(H) set to 1.2Ueq(N).
In complexes 1, 3 and 4 reflections were omitted from the refinement since they were
obscured by the beam-stop. The crystal for 2 was twinned. A .hkl file suitable for twin
refinement was created using the TwinRotMat option in PLATON [13], and refined using
the HKLF 5 option in SHELXL [11] giving a final BASF value of 0.089. Structure 4
contains a solvent accessible void of 206 Å3; the SQUEEZE routine in PLATON [13]
was not used to remove any solvent electron densities. Structures 4 and 5 both have
water molecules where the hydrogen atoms could not be adequately located on the
difference Fourier map.
3.3 Results and Discussion
3.3.1 Synthesis and characterization of trans-[ReCl3(t-BuCN)(PPh3)(an)] (1),
trans-[ReCl3(t-BuCN)(PPh3)(pd)] (2) and trans-[ReCl3(t-BuCN)(PPh3)(aa)] (3)
Complexes 1 – 3 are structurally similar, the major difference being the free functional
group on the phenyl ligand. In complex 1 this is a hydrogen, in complex 2 a secondary
amine, and in complex 3 a carboxylic acid group. Due to their extreme similarities, the
three complexes will be discussed simultaneously.
For complexes 1 and 2, trans-[ReCl3(t-BuNC)(PPh3)2] was reacted with H2an and H2pd
respectively in refluxing acetonitrile with a molar ratio of 1:2 under nitrogen. Complex 3
was isolated by using the same starting material and reacting it with H2aa in a 1:3 molar
ratio in hot benzene under similar conditions as above. In all the above cases, the
ligand acts as a monodentate ligand, coordinating through a doubly deprotonated imido
nitrogen.
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Complexes 1 – 3 are all non-electrolytes. Compound 1 appears as a green solid,
soluble in acetonitrile and dichloromethane, and sparingly soluble in ethanol. It is stable
in solution for weeks as a light green solution. Complex 2 is a brown solid, soluble in
methanol and acetonitrile, but insoluble in ethanol, acetone and dichloromethane.
Compound 3 is also a green solid, but upon dissolving it in an appropriate solvent, a
yellow/orange solution forms, which is stable for several weeks. This complex is soluble
in acetonitrile, dichloromethane and chloroform.
Compounds 1 – 3 have very similar structures, and their respective IR spectra are also
quite similar, as depicted in Figure 3.4 below. The three most important characteristic
bands for these complexes are the C≡N (of the isocyanide), Re=C and Re=N bands,
and they occur at similar frequencies respectively for all three complexes. The
coordinated isocyanide ligand is supported by the C≡N and Re=C absorption at about
2200 cm-1 and 1190 cm-1 respectively. The Re=N bond gave a strong stretching
frequency at approximately 1090 cm-1. The IR spectrum for 2 also shows two peaks at
3401 and 3307 cm-1 [ν(NH)] which signify the free uncoordinated amine group on the
aromatic ring. Complex 3 has a strong COO-H stretch, confirming the carboxylic acid
group to be free on the phenyl ring of the coordinated ligand aa2-.
The 1H NMR spectra for complex 1 is not very informative on the structure of the
complex, due to the fact that the signals of the phenyl protons overlap with that of the
protons on the triphenylphosphine ligand. The 1H NMR spectrum for 2 (Figure 3.5) show
very clear, distinct signals (as to be expected from a diamagnetic complex). The
triphenylphosphine ligand protons have rise to multiple signals in the range 7.19 – 7.75
ppm. The phenyl protons gave rise to two doublets at 6.34 and 6.08 ppm, which are
assigned to H2 and H5 respectively, and two triplets at 7.09 and 5.95 ppm due to H4 and
H3 respectively. The tert-butyl isocyanide protons show an intense signal at the highly
shielded range at about 1.2 ppm – the intensity ascribed to its symmetrical properties.
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Figure 3.4: Infrared spectra of complexes 1–3
Although 1 and 2 are structurally very similar, their respective 1H-NMR spectra are
completely different. The an2- ligand in 1 is a mono-substituted phenyl ring in contrast to
pd2- in 2 being di-substituted. This greatly influences the observed chemical shifts, since
1 doesn’t contain the electron-withdrawing amine.
Complex 3 has a 1H-NMR spectrum very similar to that of 2, ascribed to the fact that the
two complexes are nearly identical – the major difference being the free functional
group on the phenyl ligand, as mentioned earlier. The free secondary amine and free
carboxylic acid on complexes 2 and 3 respectively have similar electronic properties,
explaining why the signals on the two spectra are similar. The proton-NMR spectrum
for 3 shows the presence of the triphenylphosphine ligand by the peaks in the range
7.19 – 7.66 ppm. The phenyl protons gave rise to two doublets at 6.67 (H2) and 7.70
(H5) ppm, and two triplets at 7.26 and 6.54 ppm due to H4 and H3 respectively. The t-
butyl isocyanide protons again resonate as a strong singlet at around 1.4 ppm.
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Figure 3.5: 1H NMR spectrum of 2
Figure 3.6: 1H NMR spectrum of 3
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The UV-Vis spectrum of the green complex 1 only reveals an extremely weak peak at
669 nm ascribed to weak metal-to-ligand charge-transfer. The spectrum of complex 2
shows three peaks. Firstly an intense band is seen at 346 nm, most probably due to the
combined ligand-to-metal charge-transfer transition of [pπ(Cl-) d*π(Re)] and [pπ(N2-)
d*π(Re)]. The less intense peak at about 480 nm is ascribed to being a ligand-to-
metal charge transitions [pπ(CNR) d*π(Re)]. There is also a very weak band at a low
energy (669 nm) due to [d*π(Re) pπ(CNR)] metal-to-ligand charge-transfer
transitions. Complex 3 only exhibits one very weak shoulder band at approximately 384
nm.
The cyclic voltammograms of complexes 1 – 3 show the current response when a
solution of 1 – 3 (0.001M) and 0.1M tetrabutylammonium perchlorate (TBAP) was
subjected to a cyclic excitation signal. The working electrode was a carefully polished
platinum electrode, and the reference electrode was a saturated Ag/AgCl electrode.
Figure 3.7: UV/Vis spectrum of 2
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Consider the voltammogram for 1 (Figure 3.8) and its peak parameters as summarized
in Table 3.1. There is a redox couple observed at A and an irreversible cathodic peak at
B. The process at A is a one-electron quasi-reversible reduction, evident from the
cathodic/anodic current ratio.
Table 3.1: Peak parameters for the cyclic voltammogram of complexes 1 - 3.
1 2 3
Peak A B A B A B
Epc (mV) 1067 -1195 -595 - -825 -1437
Epa (mV) 1144 - - -995 804 -
E1/2 (mV) 1106 - - - -10.5 -
ic (μA) 6.376 14.49 14.1457 - 5.1606 2.7436
ia(μA) 7.111 - - 9.1092 9.4301 -
ia/ic 1.12 - - - 1.82 -
Figure 3.8: Cyclic voltammogram of 1
A
B
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Figure 3.9: Cyclic voltammogram of 2
Figure 3.10: Cyclic voltammogram of 3
A
A B
B
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The cyclic voltammogram for 2 (Figure 3.9) only show two irreversible processes – a
cathodic peak at A and an anodic peak at B. Complex 3 gave two processes upon
subjecting a solution of 3 to an excitation signal. Process A is a two-electron irreversible
process – the irreversibility indicated by the very high anodic to cathodic peak ratio.
Process B only shows an irreversible cathodic peak with a Epc of -1437 mV.
Single crystals for both 1 and 2 were obtained by the evaporation of the mother liquor.
Complex 2 crystallized as the solvate 2·CH3CN. Single crystals for 3 were obtained by
vapour diffusion of diethyl ether into a solution of 3 in dichloromethane. The three
compounds are nearly identical with the free substituent on the phenyl ligand being the
major structural difference. Therefore complexes 1 – 3 will be discussed together,
unless significant differences are applicable.
Perspective views of the asymmetric units of complexes 1 -3 are portrayed in Figures
3.11 – 3.13. The geometry is best described as slightly distorted octahedral around the
central rhenium(V) ion, which is evident from the non-linear bond angles for trans-
ligands Cl(1)-Re(1)-N(1) of 174.9(2)° for 1. Similar trans-angles are observed for 2 and
3 of 175.4(2)° and 170.2(3)° respectively. The basal planes are defined by the two
chlorides Cl(2) and Cl(3), the phosphorus atom P(1) and the carbon atom C(1) of the
isonitrile. The imido nitrogen N(1) and Cl(1) lie in the trans axial positions.
The Re(1)-N(11) bond distance of 1.728(2) Å in complex 2 clearly agrees with the
expected bond length for Re-imido double bonds [1.72(1) – 1.74(1)Å], thus confirming
the coordination mode being linear where the sp2-hybrized nitrogen acts as a 2e- donor
[2]. The analogous Re-N bond in 1 [1.715(2)] Å and 3 [1.728(2) Å] are also within the
expected range for Re(V)-imido bonds [2, 14].
The Re(1)-C(1) bond for 1 - 3 (about 2.03 Å) is significantly shorter than expected for a
Re-C single bond (2.13 Å) and somewhat longer than the distance expected for Re=C
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double bond (1.91 Å), indicating that the Re(1)-C(1) bond has some double bond
character [15]. The Re-Cl and Re-P bond distances for 1 – 3 are as normally found [16].
Figure 3.11 – ORTEP diagram of 1, showing 40% ellipsoid probability
The tert-butyl isocyanide ligand in the complexes are essentially linear, as seen from
the C(1)-N(1)-C(2) angle of 176.8(3)° in 2, indicating the strong σ-donation, weaker π-
accepting nature of the ligand [17]. The isocyanide ligand in complex 3 deviates more
from linearity [169.9(5)°], which may be indicative of stronger pi-back bonding, although
not significantly. The C(1)-N(1) bond length of 2 [1.151(3) Å] is slightly longer than the
average C-N triple bond length, thus showing that is has double bond character [15].
The analogous bonds in complexes 1 and 3 show similar bond lengths. This
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phenomenon is caused by π-back bonding from the metal, resulting in the Re-C bond
being strengthened and the unsaturated C-N bond being weakened [15].
Figure 3.12 – ORTEP diagram of 2∙CH3CN, showing 40% ellipsoid probability
Complex 2 was also synthesized by the reaction of trans-[ReOCl3(PPh3)2] with H2pd in
ethanol to form trans-[ReCl3(pd)(PPh3)2] [9], which was subsequently reacted with t-
BuNC in toluene. The reason behind using this method was to try and explain the
mechanism of the [ReCl3(CNR)]2+ formation. It was found that whether starting with the
Re(III)/Re(V) precursor, the same product will be isolated.
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Figure 3.13: ORTEP diagram of 3, showing 40% ellipsoid probability
The crystal structures of 1 and 2 were superimposed to illustrate the extreme similarities
between these complexes (Figure 3.14). Except for the angles being bent slightly
differently, the only noticeable difference is the substituent on the phenol ring for 2.
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Figure 3.14: Structure overlay of 1 and 2
The intramolecular hydrogen-bonds and interactions in 3 [C(10)-H(13)---O(2) and C(36)-
H(36)---O(1)] are quite strong, and correlates to the crystal packing in the unit cell for
complex 3 (Figure 3.15). As illustrated in Table 3.2, there are more hydrogen
interactions that occur in complex 2 in comparison to complex 1. The difference lies in
the crystal of 2 containing a solvent molecule which participates in hydrogen bonding,
as well as the free primary amine on the phenyl ring of the ligand which is absent in
complex 1. The two hydrogen atoms on the uncoordinated N(12) atom in 2 are involved
in hydrogen-bonds with the chlorides Cl(1) and Cl(3).
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Table 3.2: Hydrogen-bonding and interactions for complexes 1 – 3.
A-H∙∙∙B A-H H∙∙∙B A∙∙∙B A-H∙∙∙B
1
C(36)-H(36)∙∙∙Cl(3) 0.9500 2.8100 3.652(2) 148
C(42)-H(42)∙∙∙Cl(3) 0.9500 2.7000 3.533(19) 146
C(46)-H(46)∙∙∙Cl(1) 0.9500 2.6400 3.249(2) 123
C(46)-H(46)∙∙∙Cl(3) 0.9500 2.7300 3.397(2) 128
2
N(12)-H(12A)∙∙∙Cl(3) 0.87(3) 2.68(3) 3.534(3) 168(3)
N(12)-H(12B)∙∙∙Cl(1) 0.88(2) 2.43(2) 3.300(3) 172(2)
C(3)-H(3A)∙∙∙Cl(3) 0.9800 2.8200 3.657(3) 144
C(5)-H(5C)∙∙∙N(2) 0.9800 2.5300 3.485(4) 166
C(36)-H(36)∙∙∙Cl(2) 0.9500 2.6300 3.481(3) 150
C(46)-H(46)∙∙∙Cl(2) 0.9500 2.7700 2.472(3) 132
3
O(2)-H(2)∙∙∙O(3) 0.8400 1.8400 2.651(6) 163
Cl(3)-H(13)∙∙∙O(2) 0.9500 2.3500 2.696(6) 101
C(26)-H(12B)∙∙∙Cl(3) 0.9500 2.6200 3.406(4) 131
C(36)-H(12B)∙∙∙O(1) 0.9500 2.4400 3.389(6) 172
C(43)-H(12B)∙∙∙Cl(3) 0.9500 2.7600 3.658(6) 157
Geometry optimization was done for all three complexes using the density functional
methods B3LYP and PBE1PBE, the latter being the preferred method for rhenium-
complexes and the former being an old, however very popular and efficient method. The
computational bond lengths and angles for 1 – 3 have quite a lot of similarities; however
there are also some cases in which the predicted structural properties are quite different
from that experimentally obtained. This can be ascribed to a number of reasons, one of
which can be due to the effect of the solvent present. The computational bond lengths
and angles are summarized in Tables 3.8 – 3.10.
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Figure 3.15 - Packing diagram of the unit cell of complex 3
3.3.2 Synthesis and characterization of trans-[ReCl2(t-BuCN)(PPh3)2(ap)](ReO4)
(4)
Complex 4 was synthesized in relatively low yield by heating trans-[ReCl3(t-
BuNC)(PPh3)2] with H2ap in a 1:3 molar ratio in benzene in a nitrogen atmosphere, and
subsequent recrystallization using several solvents. One chloride ion ligand was
substituted by one ap2- unit, which coordinates in a monodentate fashion as an imide.
The reaction is a disproportionation reaction, giving two rhenium atoms in different
oxidation states, namely +V and +VII, in an intricate redox process.
Complex 4 is a 1:1 electrolyte in DMF. It is insoluble in most solvents, the exceptions
being DMF and chloroform. The yellow/orange solution is stable in solution for several
weeks.
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The ligand in complex 4 is coordinated in a similar fashion to the aniline derivatives in
complexes 1 – 3; however the complex is a cation with perrhenate as the counter-ion.
This is confirmed by the strong stretching frequency in its IR spectrum at 908 cm-1
[v(Re=O)] (Figure 3.16). There is also a strong O-H stretch observed around 3600 cm-1,
as to be expected. The characteristic C≡N, Re=C and Re=N bands are observed at
2200 cm-1, 1190 cm-1 and 1090 cm-1 respectively for 4 – similar to that of complexes 1 -
3.
The proton NMR spectrum of 4 was difficult to assign due to the overlapping of the
phenyl protons with that of the triphenylphosphine ligands. The two triphenylphosphine
ligands gave multiplets at 7.66, 7.28 and 7.19 ppm, which integrate for 30 protons. The
other peaks in the aromatic region are assigned to the phenyl protons of the
coordinated ligand, and integrates for 4 protons. The t-butyl isocyanide protons appear
as a singlet integrating for 9 protons at 2.10 ppm.
The absorption spectrum for 4 contains three bands. The low energy, intense peak at
about 287 nm is most probably due to the ligand-to-metal transitions [pπ(Cl-) d*π(Re)]
and [pπ(N2-) d*π(Re)]. The band at 408 nm can be ascribed to the metal-to-ligand
transition from the rhenium metal to the pi-acceptor isocyanide ligand [d*π(Re)
pπ(CNR)]. The low intensity shoulder band at 499 nm can be due to d-d transitions.
The crystal structure of the complex salt 4 is shown in Figure 3.18. The cationic
complex adopts a distorted octahedral geometry around the rhenium(V) centre. The
metal coordinates to two phosphorus atoms, two chlorides, the isocyanide carbon atom
C(1) and the imido nitrogen atom N(2). The O(1)H group is left uncoordinated in the
complex.
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Figure 3.16: Infrared spectrum of complexes 4
Figure 3.17: UV/Vis spectrum of 4
Complex 4 contains the ligand coordinated in a similar fashion to complexes 1 – 3, with
the unanticipated presence of the perrhenate counter ion. The recrystallization process
for 4 is much more complex and contains several more steps than that of 5, and it is
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suspected that during this recrystallization, the perrhenate is somehow introduced. The
C-O bond length of 4 is 1.36(2) Å confirming its single bond character.
Selected bond lengths and angles are given in Table 3.11. Distortion from an ideal
metal-centered octahedron results in a non-linear N(2)-Re-Cl(2) axis of 175.2(4)°, due
to C(1)-Re-Cl(1) and P(1)-Re-P(2) angles of 178.6(4)° and 171.12(8)° respectively.
The rhenium atom is lifted out of the mean equatorial P2ClC plane by 0.160 Å towards
N(2), which is the result of the non-orthogonal angles N(2)-Re-P(1) = 93.74(6)°, N(2)-
Re-P(2) = 93.74(6)° and N(2)-Re-Cl(1) = 91.4(4)°. The N(2)-Re-C(1) angle is orthogonal
at 90.0(6)°.
Figure 3.18: ORTEP diagram of 4, showing 40% ellipsoid probability
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The t-BuNC is coordinated in a linear fashion [Re-C(1)-N(1) = 176.6(1)°; C(1)-N(1)-C(2)
= 178.9(2)°]. The Re-C(1) and Re-N(2) bond lengths are 2.01(1) and 1.75(2) Å
respectively, with the Re-N(2)-C(41) bond angle equal to 178.6(1)°. The Re-P and Re-
Cl bond distances are within the expected ranges for these types of bonds [16]. The
packing diagram of 4 is given in Figure 3.19 which shows that each unit cell contains
four molecules of 4.
Figure 3.19: Packing diagram of 4.
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3.3.3 Synthesis and characterization of trans-[ReCl2(t-BuCN)(PPh3)2(ibq)] (5)
H2ap was reacted with trans-[ReCl3(t-BuNC)(PPh3)2] in a 1:3 molar ratio in refluxing
benzene to form complex 5 in a relatively good yield. Atmospheric conditions were
carefully controlled by working in an inert nitrogen atmosphere. The crystals are not
stable in a solution of DMF, and go from an initial red to a yellow solution within a
couple of days. This compound was confirmed to be a non-electrolyte in DMF. Its
solubility is limited to solvents such as DMF and chloroform.
The IR spectrum of 5 is seen in Figure 3.20, and is overlaid with that of 4 in order to
characterize the spectrum more efficiently. The differences between the two complexes
can easily be identified in this manner. For instance, 5 has no ReVII=O absorption
frequency which is expected approximately at 900 cm-1. Complex 5 has an o-quinone-
imine coordinated to the metal centre, thus one should find a C=O stretching frequency.
The fact that this is not clearly seen can be ascribed to the delocalization of electrons
observed in the ligand (Figure 3.3). Complex 4 has an phenolic group, which explains
the strong signal at 3600 cm-1, which is absent in the spectrum of 5.
Complex 5 is paramagnetic, thus the observed chemical shifts on its proton NMR
spectrum appear over a wide range and the resolution is quite distorted. The protons on
the two triphenylphosphine moieties gave rise to three multiplets at 7.67, 7.26 and 7.19
ppm, integrating for 30 protons. The protons on the coordinated phenyl ligand gave
three signals which integrate for 4 protons at 7.58, 7.43 and 7.32 ppm.
Complex 5 shows two very clear distinct bands of relatively low intensity at 326 and 501
nm, ascribed to charge-transfer transitions [pπ(Cl-) d*π(Re)] and [pπ(N-) d*π(Re)].
There are also two weak shoulder bands observed at about 437 and 549 nm due to d-d
transitions. Their low intensity is a result of the transitions being Laporte forbidden.
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Figure 3.20: IR spectra of 4 and 5
Figure 3.21: 1H NMR spectrum of 5
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Figure 3.22: UV/Vis spectrum of 5
Figure 3.23: Cyclic voltammogram of 5
A
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The cyclic voltammogram of complex 5 is shown in Figure 3.23. There is only one
process seen in the potential region scanned, namely process A. It is an irreversible
anodic peak with Eac = 711 mV and Ia = 4.5869 μA. One would expect to find a more
complex current response due to the intricate redox process which occurred upon
synthesizing complex 5. After a very weak response was obtained when using a
platinum working electrode, it was replaced by a glassy carbon electrode; however
similar results were obtained.
The asymmetric unit of complex 5 is given in Figure 3.24. The rhenium centre is
coordinated to two chlorides in cis positions, two phosphines in trans positions, and the
nitrogen N(1) at a site cis to the isonitrile carbon C(21). The oxygen O(1) is not
coordinated.
The coordination mode of the ap ligand in 5 is different to that in complex 4. The intra-
ligand bond distances of the mono-coordinated 2-aminophenol derivative assist in
determining the formal oxidation state of the rhenium. The O(1)-C(12) bond length of
1.266(6) Å implies that this bond is double compared to the similar bond of 1.36(2)Å in
4. The C(13)-C(14) [1.32(1) Å] and C(15)-C(16) [1.346(7) Å] bonds are double, with the
C(12)-C(13) [1.465(8) Å], C(14)-C(15) [1.412(8) Å], C(11)-C(16) [1.429(7) Å] and C(11)-
C(12) [1.450(7) Å] bonds all single. The N(1)-C(11) length of 1.334(5) Å implies that this
is also a double bond. These results indicate that the ligand is coordinated in the o-
quinone-imine form, as illustrated in Figure 3.25. This shows that the rhenium is in the
formal oxidation state of +III.
The Re-N(1) bond is a double bond [Re-N(1) = 1.748(3) Å], and the Re-N(1)-C(11)
angle of 172.6(3)° confirms the sp hybridization of N(1). The degree of distortion
between N(1) and the donor atoms cis to it differs remarkably from those in complex 4
[N(1)-Re-P(1) = 88.0(1)°, N(1)-Re-P(2) = 87.8(1)°, N91)-Re-C(21) = 94.1(2)°; N(1)-Re-
Cl(2) =104.6(1)°], with the result that the rhenium is lifted out of the mean P2CCl
equatorial plane by 0.098 Å towards N(1), compared to 0.160 Å in 4. The Re-C(21) and
Chapter 3 ReCl3(CNR) Core
57 | P a g e Nelson Mandela Metropolitan University
C(21)-N(2) bond lengths are 2.016(5) and 1.162(6) Å respectively, and the Re-C(21)-
N(2) bond angle is linear [173.4(4)°].
It is clear from the crystal structure of 5 (Figure 3.24) that the phenolic oxygen did not
coordinate to the rhenium metal. There have been many cases in which a phenolic
oxygen coordinated to rhenium, but there is a relatively high energy barrier required for
the 1e- redox reaction which forms such a Re-O species [18]. In the case of 5 it was
more favorable to form the imido-species.
Figure 3.24: ORTEP diagram of 5, showing 40% ellipsoid probability
Chapter 3 ReCl3(CNR) Core
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Figure 3.25: Coordination of the o-quinone-imine form of H2ap to Re(III)
Figure 3.26 illustrates the intramolecular hydrogen-bonding interactions.
Table 3.3: Hydrogen interactions for complex 5
A-H∙∙∙B A-H (Å) H∙∙∙B (Å) A∙∙∙B (Å) A-H∙∙∙B (°)
C(14)-H(14)∙∙∙Cl(2) 0.9500 2.6900 3.576(5) 156
C(15)-H(15)∙∙∙Cl(2) 0.9500 2.8000 3.640(5) 147
C(36)-H(36)∙∙∙Cl(1) 0.9500 2.5600 3.427(5) 152
C(42)-H(42)∙∙∙Cl(2) 0.9500 2.7000 3.513(6) 143
C(56)-H(56)∙∙∙O(1) 0.9500 2.4800 3.339(6) 150
C(62)-H(62)∙∙∙Cl(2) 0.9500 2.7400 3.510(5) 138
C(72)-H(72)∙∙∙Cl(1) 0.9500 2.6300 3.475(5) 148
C(82)-H(82)∙∙∙O(1) 0.9500 2.4600 3.331(6) 152
C(84)-H(84)∙∙∙Cl(1) 0.9500 2.8200 3.705(5) 155
Chapter 3 ReCl3(CNR) Core
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Figure 3.26: Intramolecular hydrogen interactions separated by >5 bonds for 5
3.4 References
[1] R. Alberto, Eur. J. Nucl. Chem. Biol., 2003, 30, 1299; S.S. Jurisson, J.D. Lydon,
Chem. Rev., 1999, 99, 2205.
[2] F.E. Hahn, M. Glaser, T. Lugger, D. Scheller, H Spies, Inorg. Chim. Acta, 1995,
232, 238.
[3] K.C. Potgieter, PhD Thesis, Nelson Mandela Metropolitan Unviersity, 2012, 9.
[4] J.B. Arterburn, M.C. Perry, K.V. Rao, Angew. Chem. Int. Ed., 2000, 39, 771.
Chapter 3 ReCl3(CNR) Core
60 | P a g e Nelson Mandela Metropolitan University
[5] J.B. Arterburn, D.M. Goreham, M.S. Holguin, K.V. Rao, M.V. Valenzuela,
Organomettallics, 2009, 19,1789.
[6] E.J. Sawyer, A.M. Cassoni, W. Waddington, J.B. Bomanji, T.W. Briggs, British J.
Radiol., 1999, 72, 1225.
[7] U. Abram, R. Alberto, G. Artus, A. Egli, W.A. Herrmann, T.A. Kaden, R. Schibli,
A. Schubiger, J. Organomet. Chem., 1995, 492, 217.
[8] U. Abram, R. Alberto, J. Braz. Chem. Soc., 2006, 17, 1486.
[9] I.N. Booysen, Rheniium(I) and (V) Complexes with Potentially Multidentate
Ligands containing the Amino Group, PhD Thesis, Nelson Mandela Metropolitan
University, South Africa, 2009, 32.
[10] APEX2, SADABS and SAINT, Bruker AXS Inc., Madison, Wisconsin, USA, 2010.
[11] G.M. Sheldrick, A short history of SHELX, Acta Cryst., 2008, A64, 112.
[12] C.B. Hübschle, G.M. Sheldrick, B. Dittrich, ShelXle: a Qt graphical user interface
for SHELXL, J. Appl. Cryst., 2011, 44,1281.
[13] A. L. Spek, Acta Cryst., 2009, D65, 148.
[14] M.T. Ahmet, B. Coutinho, J.R. Dilworth, J.R. Miller, S.J. Parrott, Y. Zheng,
Polyhedron,1996, 15, 2042.
[15] M. Fatima, C. Guedes da Silva, R.A. Michelin, A.J.L. Pombeiro, Coord. Chem.
Rev., 2001, 218, 47.
Chapter 3 ReCl3(CNR) Core
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[16] F. Refosco, F. Tisato, C. Bolzati, G. Bandoli, J. Chem. Soc., Dalton Trans., 1993,
605, and references therein.
[17] R.H. Crabtree, The Organometallic Chemistry of the Transition Metals, 3rd
edition, Wiley-Interscience Publication, Canada, 2001, 87.
[18] C.A. Lippert, K.I. Hardcastle, J.D. Soper, Inorg. Chem., 2011, 50, 9864, and
references therein.
Chapter 3 ReCl3(CNR) Core
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Table 3.4 - Selected crystal and data collection details for complexes 1 - 3.
Complex 1 2 3
Formula C29H29Cl3N2PRe C29H29Cl3N2PRe.
C2H3N
C30H29Cl3N2O2PRe.
C4H10O
Formula weight 729.07 785.14 847.20
Crystal System Monoclinic Monoclinic Monoclinic
Space Group P21/c P21/c P21/c
a [Å] 13.5158(2) 9.1212(2) 10.7273(4)
b [Å] 13.9991(2) 16.7180(4) 17.4691(6)
c [Å] 15.6529(3) 21.0649(6) 10.8285(4)
α [°] 90 90 90
β [°] 96.058(1) 94.159(1) 115.866(1)
γ [°] 90 90 90
Volume [Å3] 2945.13(8) 3203.7(1) 1825.9(1)
Z 4 4 2
Dcalc [g/cm3] 1.644 1.628 1.541
Absorption
Coefficient (mm-1) 4.473 4.120 3.625
F(000) 1432 1552 844
Crystal size [mm] 0.13 × 0.17 ×
0.26 0.03 × 0.20 × 0.33 0.08 × 0.09 × 0.10
Theta Min-Max [°] 2.0 – 28.3 2.2 – 28.3 2.1 – 27.5
Index ranges
H -17 : 18 -12 : 12 -13 : 13
K -18 : 17 -22 : 22 -22 : 22
L -19 : 20 -3 : 28 -14 : 10
Goodness-of-fit 1.14 1.05 0.83
Observed data [I >
2.0 σ I] 6675 6976 7107
R 0.0154 0.0233 0.0161
wR2 0.0356 0.0455 0.0329
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Table 3.5 - Selected crystal and data collection details for complexes 4 - 5.
Complex 4 5
Formula C47H44Cl2N2OP2Re, O4Re, O C47H43Cl2N2OP2Re
Formula weight 1238.10 970.88
Crystal System Orthorombic Monoclinic
Space Group Pmna P21/c
a [Å] 15.1070(5) 17.0475(5)
b [Å] 17.3430(6) 10.5682(2)
c [Å] 19.8490(7) 24.4531(6)
α [°] - 90
β [°] - 100.821(1)
γ [°] - 90
Volume [Å3] 5200.5(3) 4327.2(2)
Z 4 4
Dcalc [g/cm3] 1.581 1.490
Absorption Coefficient (mm-1) 4.8959 3.043
F(000) 2408 1944
Crystal size [mm] 0.03 × 0.02 × 0.10 0.05 × 0.06 × 0.30
Theta Min-Max [°] 1.7 – 28.4 1.7 – 28.3
Index ranges
h -20 : 19 -22 : 22
k -23 : 22 -10 : 14
l -21 : 26 -32 : 32
Goodness-of-fit 1.26 1.03
Observed data [I > 2.0 σ I] 5828 7903
R 0.0760 0.0355
wR2 0.1823 0.0930
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Table 3.6 – Selected experimental bond distances [Å] for complexes 1 - 3.
Bond 1 2 3
Re-N(1) 1.715(2) - 1.717(3)
Re-P(1) 2.4438(5) 2.4283(6) 2.447(1)
Re-C(1) 2.032(2) 2.024(4) -
Re-Cl(1) 2.4100(4) 2.4525(6) 2.4203(8)
Re-Cl(2) 2.4194(5) 2.4143(7) 2.419(1)
Re-Cl(3) 2.4026(5) 2.4150(7) 2.415(1)
C(1)-N(2) 1.157(3) - -
N(1)-C(11) 1.376(3) - 1.380(4)
Re-N(11) - 1.728(2) -
C(1)-N(1) - 1.151(3) -
N(11)-C(11) - 1.356(3) -
Re-C(2) - - 2.032(4)
C(2)-N(2) - - 1.146(6)
N(1)-C(11) - - 1.380(4)
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Table 3.7 – Selected experimental bond angles [°] for complexes 1 - 3.
Angle 1 2 3
N(1)-Re-Cl(2) 96.55(5) - 97.9(1)
N(1)-Re-P(1) 93.23(5) - 91.3(1)
N(1)-Re-Cl(1) 170.22(5) - 95.3(1)
N(1)-Re-Cl(3) 97.36(6) - 172.6(1)
N(1)-Re-C(1) 90.85(8) - -
C(1)-N(2)-C(2) 177.1(2) - -
Re-C(1)-N(2) 177.0(2) - -
Cl(1)-Re-Cl(2) 87.30(2) - 87.97(4)
N(11)-Re-Cl(1) - 94.83(7) -
N(11)-Re-P(1) - 92.18(7) -
N(11)-Re-Cl(2) - 170.82(6) -
N(11)-Re-Cl(3) - 97.16(6) -
N(11)-Re-C(1) - 87.43(9) -
C(1)-N(1)-C(2) - 176.8(3) -
Re-C(1)-N(1) - 174.4(2) -
Cl(1)-Re-Cl(3) - 88.20(3) -
Re-N(11)-C(11) - 175.4(2) -
P(1)-Re-Cl(2) - 87.23(2) -
N(1)-Re-C(2) - - 93.9(1)
C(3)-N(2)-C(2) - - 169.9(5)
Re-C(2)-N(2) - - 174.1(4)
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Table 3.8 – Computational bond distances and angles for 1.
Bond PBE1PBE B3LYP
Re-Cl(1) 2.457 2.484
Re-Cl(2) 2.475 2.520
Re-Cl(3) 2.441 2.479
Re-P(1) 2.479 2.529
Re-N(1) 1.709 1.719
Re-C(1) 2.014 2.030
P(1)-C(21) 1.829 1.842
P(1)-C(31) 1.832 1.845
P(1)-C(41) 1.831 1.841
N(1)-C(11) 1.368 1.373
N(2)-C(1) 1.165 1.167
Angle PBE1PBE B3LYP
Cl(1)-Re-Cl(2) 86.7 86.3
Cl(2)-Re-Cl(3) 86.5 86.7
Cl(2)-Re-P(1) 169.8 171.1
Cl(2)-Re-N(1) 95.8 94.4
Cl(2)-Re-C(1) 85.9 86.1
Cl(3)-Re-P(1) 86.9 87.4
Cl(1)-Re-Cl(3) 88.5 87.9
Cl(1)-Re-C(1) 79.8 80.2
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Table 3.9 - Computational bond distances and angles for 2.
Bond PBE1PBE B3LYP
Re-Cl(1) 2.443 2.481
Re-Cl(2) 2.442 2.465
Re-Cl(3) 2.431 2.464
Re-P(1) 2.450 2.505
Re-N(11) 1.720 1.731
Re-C(1) 1.997 2.014
P(1)-C(21) 1.833 1.847
P(1)-C(31) 1.834 1.847
P(1)-C(41) 1.828 1.842
N(1)-C(1) 1.174 1.176
N(11)-C(11) 1.353 1.358
Angle PBE1PBE B3LYP
Cl(1)-Re-Cl(2) 88.2 88.1
Cl(2)-Re-Cl(3) 91.4 91.1
Cl(2)-Re-P(1) 82.3 83.6
Cl(2)-Re-N(11) 170.2 171.4
Cl(2)-Re-C(1) 88.2 79.3
Cl(3)-Re-P(1) 89.8 89.5
Cl(1)-Re-Cl(3) 86.5 86.9
Cl(1)-Re-C(1) 84.3 84.2
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Table 3.10 – Computational bond distances and angles for 3.
Bond PBE1PBE B3LYP
Re-Cl(1) 2.425 2.457
Re-Cl(2) 2.427 2.468
Re-Cl(3) 2.445 2.464
Re-P(1) 2.464 2.519
Re-N(1) 1.714 1.726
Re-C(2) 2.010 2.025
P(1)-C(21) 1.835 1.848
P(1)-C(31) 1.828 1.839
P(1)-C(41) 1.835 1.847
N(1)-C(11) 1.366 1.372
N(2)-C(2) 1.167 1.171
Angle PBE1PBE B3LYP
Cl(1)-Re-Cl(2) 87.1 87.6
Cl(2)-Re-Cl(3) 87.5 87.6
Cl(2)-Re-P(1) 168.4 169.9
Cl(2)-Re-N(1) 94.6 93.2
Cl(3)-Re-P(1) 81.5 83.1
Cl(1)-Re-Cl(3) 91.2 91.0
Cl(1)-Re-N(1) 94.7 94.6
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Table 3.11 – Selected experimental bond distances [Å] for complexes 4 - 5.
Bond 4 5
Re-N(2) 1.75(1) -
Re-P(1) 2.48(3) 2.472(1)
Re-C(1) 2.01(1) -
Re-P(2) 2.48(3) 2.471(1)
Re-N(1) - 1.748(1)
Re-Cl(1) 2.42(3) 2.478(1)
Re-Cl(2) 2.40(3) 2.403(1)
Re-C(21) - 2.016(5)
C(21)-N(2) - 1.162(6)
N(1)-C(11) - 1.334(5)
C(1)-N(1) 1.17(2) -
N(1)-C(2) 1.47(2) -
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Table 3.12 - Experimental bond angles [°] for complexes 4 - 5.
4
N(1)-Re-Cl(1) 168.4(1)
N(1)-Re-P(1) 88.0(1)
N(1)-Re-P(2) 87.8(1)
Re-C(21)-N(2) 173.4(4)
N(1)-Re-Cl(2) 104.6(1)
N(1)-Re-C(21) 94.0(2)
C(21)-N(2)-C(22) 170.1(5)
Cl(1)-Re-Cl(2) 87.05(4)
5
N(2)-Re-Cl(2) 175.2(4)
N(2)-Re-P(1) 93.74(6)
P(1)-Re-P(2) 171.12(8)
C(1)-Re-N(2) 90.0(6)
C(1)-Re-Cl(1) 178.6(4)
C(1)-Re-P(1) 92.39(6)
C(1)-N(1)-C(2) 179(2)
C(1)-Re-Cl(2) 85.2(4)
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Table 3.13 - Experimental intra-ligand bond distances [Å] for complexes 1 - 3.
1 2 3
C(11) – C(12) 1.390(3) 1.416(4) 1.412(5)
C(12) – C(13) 1.384(4) 1.404(4) 1.382(5)
C(13) – C(14) 1.370(4) 1.370(5) 1.380(7)
C(14) – C(15) 1.370(4) 1.401(4) 1.385(6)
C(15) – C(16) 1.385(4) 1.361(4) 1.380(5)
C(11) – C(16) 1.389(3) 1.416(4) 1.391(6)
C(12) – X - 1.344(4) 1.489(6)
X for (1) = H; (2) = N; (3) = C.
Table 3.14 - Experimental intra-ligand bond distances [Å] for complexes 4 - 5.
4 5
C(11) – C(12) 1.41(2) 1.450(7)
C(12) – C(13) 1.41(3) 1.465(8)
C(13) – C(14) 1.31(3) 1.32(1)
C(14) – C(15) 1.34(3) 1.412(8)
C(15) – C(16) 1.38(3) 1.346(7)
C(11) – C(16) 1.36(2) 1.429(7)
C(12) – O 1.36(2) 1.266(6)
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Chapter 4 Isolation of Bis-isocyanide
Complexes of Re(I)
4.1 Introduction
The radionuclides 186Re and 188Re, as well as 99mTc, are of great interest in
radiopharmacy, due to their highly favourable properties as therapeutic and diagnostic
agents respectively [1]. The coordination requirements of the relevant metal in a certain
oxidation state containing a specific ligand system are used as basis for radiolabeling
[2]. These requirements are usually characterized by chemically robust cores which are
used as foundation for the synthesis of radiopharmaceuticals [2].
The core of specific interest in this particular study is the [Re(CO)3]+ core. The Re(I)
tricarbonyl core is a small, kinetically inert moiety, which readily allows low molecular
weight biomolecules to bind without the loss of biological activity or specificity [2].
The reaction of [Re(CO)5Cl] with isocyanides have been investigated to some extent [3].
The isocyanide coordination chemistry of technetium has, however, been studied quite
well and they are known to form extremely stable complexes with technetium due to
their electronic properties [4]. The technetium compound used as a radiopharmaceutical
in heart-imaging [99mTc(MIBI)6]+ (MIBI = 2-methoxy-2-methylpropyl-isocyanide) is well
known and serves as motivation for the further study and expansion of Re(I)-isocyanide
coordination chemistry.
Chapter 4 Bis-isocyanide Complexes
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This chapter focuses on the reaction of [Re(CO)5Cl] with isocyanides and subsequent
reaction with aquo ligands to give a mixed ligand system with the tricarbonyl core.
These aquo ligands are very labile, and can readily be replaced by a desired ligand.
The reactions of the rhenium(I) complex [Re(CO)5Cl] with tert-butyl isocyanide (t-BuNC)
and cyclohexyl isocyanide (CyNC) led to the formation of [Re(CO)3(t-BuNC)2Cl] (1) and
[Re(CO)3(CyNC)2Cl] (2) respectively. The Re(I) precursor was first stirred in boiling
tetrahydrofuran for two days to remove two carbonyls, after which it was reacted with
the respective isocyanides at room temperature. Reaction of 1 with AgOTf (silver
trifluoromethanesulfonate) and subsequently with water, gave [Re(CO)3(t-
BuNC)2(OH2)](OTf) (3).
4.2 Experimental
4.2.1 Synthesis of fac-[Re(CO)3(t-BuNC)2Cl] (1)
A previously reported method [3] was adapted as follows: [Re(CO)5Cl] (424 mg, 1.2
mmol) was dissolved in 60 mL THF and refluxed under nitrogen for 12 hours. t-BuNC
(200 mg, 2.4 mmol) was added to the reaction mixture and it was stirred for an
additional 24 hours. After removal of the solvent under vacuum, a white precipitate
formed which was filtered and recrystallized from a dichloromethane-n-hexane (2:1 v/v)
mixture. The white crystals were washed with diethyl ether and dried. Yield = 20%, m.p.
160-163 °C. Anal. Calcd. (%): C, 33.08; H, 5.94; N, 3.84. Found: C, 33.47; H, 5.35; N,
4.63. IR (νmax/cm-1): ν(C≡O) 1890 (s), 1954 (s), 2030 (s) ; ν(C≡N) 2183 (s), 2207 (s).
1H-NMR (CDCl3) (ppm): 1.58 (s, 18H, C(CH3)3).
4.2.2 Synthesis of fac-[Re(CO)3(CyNC)2Cl] (2) (CyNC = Cyclohexyl isocyanide)
A mixture of [Re(CO)5Cl] (424 mg, 1.2 mmol) and CyNC (262 mg, 2.4 mmol) in 60 mL
THF was heated under reflux for 24 hours. The solvent was evaporated under vacuum
and formed a white precipitate, which was filtered off and recrystallized from a
Chapter 4 Bis-isocyanide Complexes
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dichloromethane-n-hexane (1:1 v/v) mixture. The white crystals were washed with
diethyl ether and were suitable for X-ray diffraction studies. Yield = 45%, m.p. 119-122
°C. Anal. Calcd. (%): C, 38.86; H, 4.19; N, 5.41. Found: C, 38.97; H, 4.23; N, 5.35. IR
(νmax/cm-1): ν(C≡O) 1892 (s), 1957 (s), 2030 (s) ; ν(C≡N) 2192 (s), 2210 (s). 1H-NMR
(CDCl3) (ppm): 1.49 (s, 2H, (CNCH-C5H10)), 1.40 (d, 8H, (m-H)), 1.73 (s, 8H, (o-H)),
1.86 (s, 4H, (p-H)). Conductivity (10-3 M, CH2Cl2): 1 μS.
4.2.3 Synthesis of fac-[Re(CO)3(t-BuNC)2(H2O)](OTf) (3)
(OTf = trifluoromethanesulfonate)
Complex 1 (27 mg, 0.058 mmol) was dissolved in 7 mL of dichloromethane and 0.017 g
AgOTf (0.066 mmol) was added. The reaction mixture was stirred for 30 minutes at
room temperature and the AgCl precipitate was filtered off. Four μL of distilled water
was then added to the filtrate, and stirred overnight. The solvent was partially removed
under vacuum, and the residue was filtered off, and recrystallized from ethanol to give
colourless crystals, suitable for X-ray diffraction studies. Yield = 57 %, m.p. 106-109 °C.
Anal. Calcd. (%): C, 28.22; H, 3.20; N, 4.41; S, 4.50. Found: C, 27.86; H, 3.34; N, 4.64;
S, 5.31. IR (νmax/cm-1): ν(C≡O) 1895 (s), 1931 (s), 2040 (s) ; ν(C≡N) 2199 (s), 2219 (s).
1H-NMR (DMSO) (ppm): 2.15 (s, 2H, H2O); 2.56 (s, 18H, C(CH3)3). Conductivity (10-
3M, MeCN): 100 μS.
4.3 Results and Discussion
4.3.1 Synthesis and characterization of fac-[Re(CO)3(t-BuNC)2Cl] (1) and fac-
[Re(CO)3(CyNC)2Cl] (2)
The neutral complexes fac-[Re(CO)3(t-BuNC)2Cl] (1) and fac-[Re(CO)3(CyNC)2Cl] (2)
were formed by the reaction of [Re(CO)5Cl] with tert-butyl isocyanide and cyclohexyl
isocyanide respectively. Two isocyanide ligands bind to the rhenium atom, substituting
two carbonyl groups in the process, as depicted below.
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[Re(CO)5Cl] + 2CNR [Re(CO)3(CNR)2Cl] + 2CO
For both reactions no solid was isolated after refluxing for several hours. In both cases,
crystals of excellent quality were isolated upon removal of the solvent and
recrystallization of the residues in a suitable solvent. Both complexes 1 and 2 are
insoluble in acetonitrile, methanol and DMF, and soluble in ethanol as well as
dichloromethane.
Complex 1 and 2 contain three carbonyl groups centered around a central rhenium
atom, as well as two isonitrile ligands. The former is characterized by three intense
stretching frequencies in the IR spectrum (Figure 4.1), typical of fac-[Re(CO)3]+, at 1890,
1954 and 2030 cm-1. Nearly identical bands are observed for 2. The two isonitrile
ligands are also clearly distinguished from one another at frequencies of 2183 and 2207
cm-1 for 1, with similar bands seen for 2.
Figure 4.1: IR spectrum of 1 in the range 900 – 2400 cm-1
Chapter 4 Bis-isocyanide Complexes
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Figure 4.2: IR spectrum of 2 in the range 400 – 3500 cm-1
The simple 1H-NMR spectrum for 1 is quite useful in its characterization, since the only
protons present are those of the t-butyl isocyanide ligand which is highly symmetrical
and magnetically equivalent. These protons were assigned to the singlet at 1.58 ppm,
integrating for 18 protons. Complex 2 doesn’t contain these highly symmetrical
properties, and thus it was more difficult to assign their respective protons. The proton
next to the isonitrile functional group (CNCH-C5H10) is assigned to the singlet at 1.49
ppm, due to the shielding effects experienced by this particular proton. The peaks at
1.73, 1.40 and 1.86 were assigned to the ortho-, meta-, and para-hydrogens on the
cyclohexyl ring. The UV-Vis spectrum of both complexes 1 and 2 revealed no
observable transitions.
The cyclic voltammogram for 2 only shows one anodic peak at 1338 mV with an anodic
peak current of 19.8 μA. This is an irreversible process, since no corresponding
cathodic peak is observed, as can be seen from Figure 4.3. Complexes 1 and 2 are
structurally similar – the only difference being the type of isocyanide coordinated to the
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rhenium. They are expected to behave similarly upon subjecting them to an excitation
signal, thus only the current response for 2 was analysed.
Figure 4.3: Cyclic voltammogram of 2
A perspective view of the asymmetric units of complexes 1 - 2 are portrayed in Figures
4.4 and 4.5 respectively. Complexes 1 and 2 are structurally similar, the major
difference being the type of isocyanide ligands bonded to the central rhenium atom.
Complexes 1 – 2 are typical tricarbonyl rhenium complexes, as indicated by the average
Re-CO bond length of 1.950 Å, which corresponds to the range normally observed
[1.900(2)-1.928(2) Å] for similar complexes [5]. A chloro ligand and a carbonyl ligand
occupy the axial sites, with two isocyanides and two carbonyls in the equatorial plane.
The three carbonyls are coordinated in a facial orientation to the rhenium(I) central atom
– characteristic of the chemically robust fac-[Re(CO)3]+ core [5].
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Figure 4.4: ORTEP diagram of 1, showing 40% ellipsoid probability. Hydrogen atoms
have been omitted for clarity
The Re-CNR bonds all have some double bond character, as can be seen from their
average bond lengths of 2.096(5) Å (Tables 4.6 and 4.7), which are intermediate to that
normally found for typical rhenium(I)-carbon single and double bonds [6]. There is a
slight distortion from an ideal octahedral geometry, evident from the trans angles. This
distortion is not significant, due to the absence of multidentate ligands imposing further
constraints to the geometry. The Cl-Re-C(3) bond angle [89.9(2)° in 1] is extremely
close to orthogonality, which is not surprising at all. The tert-butyl isocyanides are
linear, deviating slightly from linearity, as seen from the C(1)-N(1)-C(11) [173.0(5)°] and
C(2)-N(2)-C(21) [177.(5)°] for complex 1. The cyclohexyl isocyanide ligands in complex
2 are more linear, with an average C-N-C angle of 176.3(2)°.
The central rhenium atom is not lifted out of the mean equatorial plane of the complexes
to any significant extent. This is probably due to the absence of multidentate ligands, as
mentioned above.
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Figure 4.5: ORTEP diagram of 2, showing 40% ellipsoid probability. Hydrogen atoms
have been omitted for clarity
Figure 4.6: Unit cell of 2 showing short van der Waals intramolecular contact distances
Chapter 4 Bis-isocyanide Complexes
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The unit cell of 2 contains two complexes and is shown in Figure 4.6, which illustrates
intramolecular contact distances larger than three bonds. Only one was found between
N(1) and H(15B) at a distance of 2.72 Å. This contact distance is relatively short,
indicating that there are only van der Waals forces present in this particular complex [5].
4.3.2 Synthesis and characterization of fac-[Re(CO)3(t-BuNC)2(H2O)](OTf) (3)
The reaction of a mixture of [Re(CO)3(t-BuNC)2Cl] and AgOTf gave the intermediate
product [Re(CO)3(t-BuNC)2(OTf)], as well as AgCl. The AgCl was filtered off and
[Re(CO)3(t-BuNC)2(OTf)] was reacted with water to give fac-[Re(CO)3(t-
BuNC)2(H2O)](OTf) (3). The axial chloro ligand is substituted for an aquo ligand, as
illustrated below.
[Re(CO)3(t-BuNC)2Cl] + AgOTf [Re(CO)3(t-BuNC)2(OTf)] + AgCl
[Re(CO)3(t-BuNC)2(OTf)] + H2O [Re(CO)3(t-BuNC)2(OH2)]+ + OTf-
Recrystallization of the precipitate obtained from the mother liquor in ethanol gave white
crystals suitable for X-ray diffraction studies. Complex 3 is soluble in acetonitrile and
methanol. Its conductivity measurement confirms it being a 1:1 electrolyte in acetonitrle
(100 μS).
The IR spectrum of 3 is characterized by three intense stretching frequencies at 1895,
1931 and 2040 cm-1, which is the result of the v(C≡O) of its three carbonyl groups
(Figure 4.7). The isocyanide C≡N stretching frequencies are also observed at 2199 and
2219 cm-1. The presence of the aquo ligand is evident from the broad peak at 3000-
3400 cm-1, ascribed to the O-H stretching frequency bands.
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Figure 4.7: IR spectrum for 3 in the range 1500 – 3500 cm-1
The proton NMR spectrum for 3 quite useful in characterization, due to the symmetrical
properties of the tert-butyl isocyanide ligand. The protons on the latter ligand are
assigned to the singlet resonating at 2.56 ppm, which integrates for 18 protons. The
protons on the aquo ligand resonate at 2.15 ppm.
Table 4.1: Peak parameters for the cyclic voltammogram of 3.
Peak A B
Epc (mV) -376 -1315
Epa (mV) - 1211
E1/2 (mV) - -52
ic (μA) 0.949 8.896
ia(μA) - 3.937
ia/ic - 0.45
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Figure 4.8: Cyclic voltammogram of 3
The cyclic voltammogram of complex 3 shows the current response when a solution of
3 (0.001M) was subjected to a cyclic excitation signal. The working electrode was a
carefully polished glassy carbon electrode. From the summarized cyclic voltammetric
parameters in Table 4.1 and the cyclic voltammogram in Figure 4.8, it is clear that there
are two processes observed for 3. Process A is an irreversible process, whereas B is a
quasi-reversible two-electron redox couple.
A perspective view of the assymmetric unit of 3 is shown in Figure 4.9. An aquo ligand
and a carbonyl ligand occupy the axial sites, with two isocyanides and two carbonyls in
the equatorial plane. Overall, the structure is only slightly distorted. The trans axial
angle O(6)-Re-C(4) is extremely close to orthogonality [178.1(1)°]. The fact that there is
not a great deal of distortion from an ideal octahedral geometry is most probably due to
the relatively small, monodentate ligands present. Complex 3 is structurally similar to 1,
the axial substituent being the major difference. Complex 1 has a chloro ligand in the
axial site, whereas complex 3 has a labile aquo ligand, which can readily be substituted
with a ligand of interest. The structural similarities are clearly depicted in Figure 4.10.
A
B
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Figure 4.9: ORTEP diagram of 3, showing 40% ellipsoid probability. The hydrogen
atoms have been omitted for clarity
Figure 4.10: Structure overlay of complexes 1 and 3
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Table 4.8 shows the experimental bond lengths and angles for 3. Complex 3 also
contains the fac-[Re(CO)3]+ core, with an average Re-CO bond length of 1.943 Å, which
is concordant with expected values [1.900(2)-1.928(2) Å] [5]. The rhenium-carbonyl
bond [1.897(3) Å] trans to the aquo ligand is somewhat shorter than the corresponding
rhenium-carbonyl bond trans to the chloride in complex 1 [1.915(5) Å]. The rhenium-
isocyanide bond shows double bond character, as seen from the average value of
2.095(3) Å, identical to that of complex 1. The Re-O bond [2.22(2) Å] of H2O is typical of
rhenium-aquo bond distances and is significantly longer than other typical Re-O bonds
such as phenolic oxygens [1.84-1.97Å], which indicates that it is more weakly bound
and neutral, and thus easily replaceable [7, 8].
The hydrogens on the aquo ligand in 3 connects to the anion OTf- via two hydrogen-
bonds (Figure 4.11). These intramolecular hydrogen-bonds O(6)-H(6A)∙∙∙O(71) [1.87(2)
Å] and O(6)-H(6B)∙∙∙O(73) [1.81(2) Å] are relatively strong, and agree with other [O-
H∙∙∙O] hydrogen-bonds found in the literature [9].
Figure 4.11: Intra- and intermolecular hydrogen-bonding for 3
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Table 4.2: Hydrogen-bond parameters for complex 3.
A-H∙∙∙B A-H H∙∙∙B A∙∙∙B A-H∙∙∙B
O(6)-H(6A)∙∙∙O(71) 0.84(2) 1.87(2) 2.687(4) 166
O(6)-H(6B)∙∙∙O(73) 0.83(2) 1.81(2) 2.642(4) 177
4.4 References
[1] U. Abram, R. Alberto, R. Schibli, A.P. Schubiger, R. Waibel, Coord. Chem. Rev.,
1999, 190-192, 903.
[2] J. Babich, S.R. Banerjee, M.K. Levadala, L. Wei, J. Zubieta, Inorg. Chem.
Commun., 2003, 6, 1099.
[3] K.K. Cheung, A. Mayer, L. Yang, J. Organomet. Chem., 1999, 585, 26.
[4] R. Alberto, H. Braband, N.I. Gorshkov, V.V. Gurzhiy, S.V. Krivovichev, E.M.
Levitskaya, A.A. Lumpov, A.E. Miroslavov, G.V. Sidorenko, D.N. Suglobov, I.G.
Tananaev, J. Organomet. Chem., 2008, 693, 7.
[5] I. Booysen, T.I.A. Gerber, E. Hosten, P. Mayer, J. Iran. Chem. Soc., 2008, 5, 93.
[6] M. Fatima, C. Guedes da Silva, R.A. Michelin, A.J.L. Pombeiro, Coord. Chem.
Rev., 2001, 218, 47.
[7] R. Mahfouz, E. Al-Frag, R.H. Siddiqui, W.Z. Al-kiali, O. Karama, Arab. J. Chem.,
2011, 4, 119.
[8] T.N. Mtshali, W. Purcell, H.G. Visser, S.S. Basson, Transition Met. Chem. 2008,
33, 711.
[9] W. Noh, G.S. Girolami, Dalton Trans., 2007, 674.
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Table 4.3 - Selected crystal and data collection details for 1.
Complex 1
Formula C13H18ClN2O3Re
Formula weight 471.95
Crystal System Orthorhombic
Space Group P212121
a [Å] 5.9620(2)
b [Å] 9.8999(3)
c [Å] 28.8810(9)
Volume [Å3] 1704.65(9)
Z 4
Dcalc [g/cm3] 1.839
Absorption Coefficient (mm-1) 7.292
F(000) 904
Crystal size [mm] 0.06 × 0.06 × 0.56
Theta Min-Max [°] 2.2 – 28.4
Index ranges
h -7 : 7
k -13 : 10
l -38 : 38
Goodness-of-fit 1.17
Observed data [I > 2.0 σ I] 4141
R 0.0205
wR2 0.0418
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Table 4.4 - Selected crystal and data collection details for 2.
Complex 2
Formula C17H22ClN2O3Re
Formula weight 524.03
Crystal System Triclinic
Space Group P-1
a [Å] 6.0170(2)
b [Å] 10.4477(3)
c [Å] 15.4208(5)
α [°] 98.801(1)
β [°] 99.740(1)
γ [°] 95.696(1)
Volume [Å3] 936.36(5)
Z 2
Dcalc [g/cm3] 1.859
Absorption Coefficient (mm-1) 6.648
F(000) 508
Crystal size [mm] 0.06 × 0.06 × 0.43
Theta Min-Max [°] 2.0 – 28.3
Index ranges
h -8 : 7
k -13 : 13
l -20 : 20
Goodness-of-fit 1.03
Observed data [I > 2.0 σ I] 4304
R 0.0147
wR2 0.0309
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Table 4.5 - Selected crystal and data collection details for 3.
Complex 3
Formula C13H20N2O4Re. CF3O3S
Formula weight 603.60
Crystal System Triclinic
Space Group P-1
a [Å] 9.1575(4)
b [Å] 111.5182(5)
c [Å] 12.2140(6)
α [°] 67.073(2)
β [°] 70.216(2)
γ [°] 85.534(2)
Volume [Å3] 1114.33(9)
Z 2
Dcalc [g/cm3] 1.799
Absorption Coefficient (mm-1) 5.605
F(000) 584
Crystal size [mm] 0.13 × 0.66 × 0.72
Theta Min-Max [°] 1.9 – 28.3
Index ranges
h -12 : 12
k -15 : 15
l -16 : 16
Goodness-of-fit 1.10
Observed data [I > 2.0 σ I] 5141
R 0.0196
wR2 0.0458
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Table 4.6 – Experimental bond distances and angles for 1.
Bond Bond length [Å]
Re-Cl(1) 2.494(1)
Re-C(1) 2.096(5)
Re-C(2) 2.095(5)
Re-C(3) 1.972(5)
Re-C(4) 1.950(6)
Re-C(5) 1,915(5)
C(1)-N(1) 1.144(7)
C(2)-N(2) 1.150(6)
C(3)-O(3) 1.132(7)
Angle Bond angle [°]
Cl(1)-Re-C(5) 177.5(2)
Cl(1)-Re-C(4) 92.3(2)
Cl(1)-Re-C(3) 89.9(2)
Re-C(1)-N(1) 173.0(5)
Re-C(2)-N(2) 173.8(4)
C(1)-N(1)-C(11) 173.0(5)
C(2)-N(2)-C(21) 177.(5)
C(3)-Re-C(5) 92.0(2)
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Table 4.7 – Experimental bond distances and angles for 2.
Bond Bond length [Å]
Re-Cl(1) 2.4969(5)
Re-C(1) 2.099(2)
Re-C(2) 2.093(2)
Re-C(3) 1.956(2)
Re-C(4) 1.917(2)
Re-C(5) 1.957(2)
C(1)-N(1) 1.147(3)
C(2)-N(2) 1.143(3)
C(3)-O(3) 1.138(3)
Angle Bond angle [°]
Cl(1)-Re-C(4) 176.95(7)
Cl(1)-Re-C(3) 92.56(7)
Cl(1)-Re-C(5) 88.77(6)
Re-C(1)-N(1) 177.2(2)
Re-C(2)-N(2) 177.0(2)
C(1)-N(1)-C(11) 177.5(2)
C(2)-N(2)-C(21) 175.0(2)
C(4)-Re-C(5) 91.36(9)
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Table 4.8 – Experimental bond distances and angles for 3.
Bond Bond length [Å]
Re-O(6) 2.220(2)
Re-C(11) 2.100(3)
Re-C(21) 2.090(3)
Re-C(3) 1.961(3)
Re-C(4) 1.897(3)
Re-C(5) 1.971(3)
C(11)-N(1) 1.140(4)
C(21)-N(2) 1.144(4)
C(3)-O(3) 1.134(5)
Angle Bond angle [°]
O(6)-Re-C(4) 178.1(1)
O(6)-Re-C(3) 92.2(1)
O(6)-Re-C(5) 92.9(1)
Re-C(11)-N(1) 176.6(3)
Re-C(21)-N(2) 173.3(3)
C(11)-N(1)-C(12) 178.7(3)
C(21)-N(2)-C(22) 173.4(3)
C(4)-Re-C(5) 88.8(1)
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Chapter 5 Reactivity of Re(V) with Isocyanides
5.1 Introduction
The previous chapters deal with the chemistry of rhenium(I) and (III) and their reactivity
towards isocyanides. This chapter focuses on the reactivity of rhenium(V), since this
particular oxidation state is of great significance in radiopharmaceuticals due to its easy
accessibility from perrhenate. The reactivity of [ReVOCl3(PPh3)2] with isocyanides have
been investigated and led to the isolation of the rhenium(III) complex
[Re(CNR)Cl3(PPh3)2] [1]. However the reactivity of [ReVO2I(PPh3)2] with isocyanides has
not been studied.
The fac-[Re(CO)3]+ core has been proven to be effective in radiolabelling due to the
kinetic and thermodynamic stability of the d6 configuration. Isocyanides possess similar
electronic properties to that of carbonyls, and can therefore potentially also display the
necessary properties for application in radiopharmaceutical use. They have great
ligation properties and have been used in diagnostics, as seen from technetium
complexes of the form [Tc(CNR)6]+ [2].
This study describes the reactivity of [ReVO2I(PPh3)2] and [ReVOCl3(OPPh3)(SMe2)] with
the ligands tert-butyl isocyanide and cyclohexyl isocyanide respectively. The reaction of
tert-butyl isocyanide with [ReO2I(PPh3)2] surprisingly gave the seven-coordinated
rhenium(III) complex cis-[Re(t-BuNC)3I3(PPh3)] (1) - a triisocyanide complex containing
three bulky iodo-ligands. From the reaction of cyclohexyl isocyanide with
[ReOCl3(OPPh3)(SMe2)], the rhenium(V) complex (μ-O)[ReOCl2(CNC6H11)2]2 (2) was
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isolated. A similar reaction has been previously reported and gave a different complex,
as depicted in Figure 5.1, but no crystal structure was reported to confirm the result [3].
Figure 5.1: Previously reported reaction of [ReVOCl3(OPPh3)(SMe2)] with cyclohexyl
isocyanide
5.2 Experimental
5.2.1 Synthesis of cis-[Re(t-BuNC)3I3(PPh3)] (1)
27.8 μL (0.25 mmol) of t-BuNC was added to a stirred suspension of 0.097 g (0.11
mmol) of [ReO2I(PPh3)2] in 20 mL benzene. The reaction mixture was heated under
reflux for an hour. After cooling to room temperature, the solvent was removed under
vacuum to produce a yellow residue. Recrystallization from ethanol gave yellow
crystals. Yield = 21 %, m.p. 194-196 °C. IR (νmax/cm-1): ν(C=N) 2121 (s), 2158 (s). 1H-
NMR (CDCl3) (ppm): 7.45 (m, 15H, PPh3), 2.16 (s, 27H, C(CH3)3). UV/Vis (CH2Cl2, λmax
(ε, M-1cm-1)): 544 (270).
5.2.2 Synthesis of (μ-O)[ReOCl2(CNC6H11)2]2 (2)
A suspension of 0.21 g (0.32 mmol) of [ReVOCl3(OPPh3)(SMe2)] in 10 mL
dichloromethane was mixed with 0.17 g of cyclohexyl isocyanide in a nitrogen
atmosphere and stirred for 2 hours at room temperature. The solution instantly changed
to a bright blue colour. The solvent was evaporated under vacuum and a blue
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precipitate was filtered off. Recrystallization from acetonitrile produced blue crystals
suitable for X-ray diffraction studies. Yield = 52 %, m.p. 171-172 °C. IR (νmax/cm-1):
ν(C=N) 2224 (s), 2238 (s); ν(Re=O) 894 (s); ν(Re-O-Re) 720. 1H-NMR (CDCl3) (ppm):
2.18 (m, 8H, p-H); 2.00 (m, 16H, m-H); 1.52 (m, 16H, o-H); 1.28 (s, 4H, CNCH(C5H10).
UV/Vis (CH2Cl2, λmax (ε, M-1cm-1)): 583 (335), 664 (280).
5.3 Results and Discussion
5.3.1 Synthesis and characterization of cis-[Re(t-BuNC)3I3(PPh3)] (1)
The seven-coordinated Re(III) complex cis-[Re(t-BuCN)3I3(PPh3)] was isolated by the
reaction of [ReO2I(PPh3)2] with tert-butyl isocyanide in a 1:2 molar ratio in benzene. The
two cis-oxo ligands were substituted, giving three isocyanides and three iodides cis
relative to one another. This reaction thus involves the reduction of Re(V) to Re(III).
Recrystallization of 1 from ethanol gave yellow crystals which were suitable for X-ray
diffraction studies. It is insoluble in acetonitrile, methanol and ethanol, and soluble in
chlorinated solvents to give yellow solutions. The complex decomposes after a few days
in solution.
The infrared spectrum of 1 (Figure 5.2) is characterized by the intense C≡N stretching
frequencies of the three isocyanide ligands bonded to the central rhenium atom. One
intense band appears at 2121 cm-1, with a shoulder at 2158 cm-1. It is possible that the
stronger band obscured the peaks for the other two isocyanide ligands. A similar effect
is normally observed for the three C≡O ligands of the rhenium(I) tricarbonyl core.
The 1H-NMR spectrum for 1 is not very useful in its characterization, since the protons
on the tert-butyl isocyanide ligands are all highly symmetrical in nature, and thus they
are observed as one intense 27 proton singlet. The aromatic region contains a multiplet
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integrating for 15 protons in the range 7.25 – 7.90 ppm. In the UV-Vis spectrum,
obtained in dichloromethane solution, there is only one weak peak at 544 nm. Ligand-
to-metal and metal-to-ligand charge transfer transitions are normally very intense, so
this peak of relatively low intensity is ascribed to d-d transitions.
Figure 5.2: IR spectrum of 1 in the range 700 – 3300 cm-1
The asymmetric unit of 1 is shown in Figure 5.3, showing the seven-coordinate Re(III)
complex. The geometry is best described as trigonal prismatic, square face
monocapped, with angles I(1)-Re-I(1i) = 86.70(2)°, P(1)-Re-C(1) = 75.88(8)°, I(1)-Re-
P(1) = 127.57(1) and C(1)-Re-C(1i) = 144.2(2)°. There is an isocyanide slightly trans to
each iodo-ligand, with an average angle of 156.55(8)°, instead of 180° for an ideal
octahedral arrangement. The isocyanides are all linear, as seen from the Re-C(1)-N(1)
angle of 178.1(2)°, while the C(1)-N(1)-C(2) angle deviates more from linearity by an
angle of 167.8(3)°. The Re-C bond lengths [2.013 Å] are as expected for rhenium-
isocyanides, as are the average isonitrile C≡N bond of 1.151(4) Å illustrating triple bond
character [4].
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Figure 5.3: ORTEP diagram of 1, showing 40% ellipsoid probability. The hydrogen
atoms have been omitted for clarity
Figure 5.4 illustrates the very complex packing of the crystals of 1 in its unit cell. There
are six molecules of 1 per unit cell; however, no significant hydrogen-bonding is
observed in this complex.
Complexes of seven-coordinate rhenium(III) are scarce in the literature. The oxidative
addition of Br2 to [Re(CO)L4Br] (L = CNMe, p-CNC6H4Me) produced the complex
[ReL4Br3], a rhenium(III) complex containing four isocyanides. In this complex the metal
is seven-coordinated, with three isocyanides and three bromides in a fac-octahedral
arrangement, with the fourth isocyanide coordinated on the face formed by the three
isocyanides in a capped-octahedral geometry. The average C-Re-Br angle is 158°,
compared to the C-Re-I angles of average 156.55(8)° in complex 1 [5].
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The reaction of two equivalents of tert-butyl isocyanide with [ReCl3(PMePh2)3] in toluene
led to the isolation of the seven-coordinae [ReCl3(t-BuNC)2(PMePh2)2]. However, with a
large excess of t-BuNC the complex salt [ReCl2(t-BuNC)3(PMePh2)2]Cl was isolated [6].
Figure 5.4: Packing diagram for 1
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5.2.2. Synthesis and characterization of (μ-O)[ReOCl2(CNC6H11)2]2 (2)
Compound 2 was prepared by stirring [ReVOCl3(OPPh3)(SMe2)] and cyclohexyl
isocyanide in dichloromethane at room temperature for two hours. A similar reaction has
been reported previously, but the solvent used was tetrahydrofuran and the product
isolated was speculated to be [ReOCl3(CNC6H11)2], but was not confirmed since no
crystal structure was reported [3]. At first the reaction was done in tetrahydrofuran;
however, the [ReVOCl3(OPPh3)(SMe2)] did not react efficiently and no blue powder was
isolated as stated in literature [3]. The solvent was changed in an attempt to synthesize
[ReOCl3(CNC6H11)2], but upon recrystallization from acetonitrile complex 2 was
surprisingly isolated.
Complex 2 is stable in air for several days, and it is insoluble in alcohols, acetonitrile
and chloroform, but soluble in dichloromethane, DMF and DMSO.
The IR spectrum for 2 (Figure 5.5) shows two C≡N stretching frequencies at 2238 and
2224 cm-1. Only one Re=O band is seen at 893 cm-1, typical of rhenium-oxo bonds.
There is a strong absorption at 720 cm-1, which is ascribed to the bridging oxo species
[v(Re-O-Re)].
The 1H-NMR spectrum for 2 is not very informative on the structure due to the
symmetrical nature of the complex. The multiplets in the range 1.2 – 2.2 ppm are
assigned to the cyclohexyl protons, which integrate for 44 protons of the four ligands.
The electronic spectrum of the blue solution of 2 shows two bands at high energy range.
The more intense band at 583 nm in the electronic spectrum of 2 can be ascribed to the
ligand-to-metal charge transfer transition [pπ(Cl-) d*π(Re)]. The less intense shoulder
at 664 nm is assigned to a (dxy)2 (dxy)1 (dπ*)1
transition.
The cyclic voltammogram for 2 (Figure 5.7) shows both oxidative and reductive waves.
The negative sweep potentials show a one-electron reversible oxidation at peak A, the
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reversibility indicated by the anodic to cathodic peak ratio which is extremely close to 1
(Table 5.1). The reductions at B and C are all irreversible, and as well as the oxidation
at peak D.
Figure 5.5: IR spectrum for 2
Figure 5.6: UV-Vis spectrum for 2
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Table 5.1: Peak parameters for the cyclic voltammogram of complex 2.
Peak A B C D
Epc (mV) -802 -1281 -1497 -
Epa (mV) -721 - - 202
E1/2 (mV) -761 - - -
ic (μA) 2.5879 4.0589 2.4629 -
ia(μA) 2.5635 - - 0.9461
ia/ic 0.99 - - -
Figure 5.7: Cyclic voltammogram for complex 2
A perspective view of the crystal structure of 2 is shown in Figure 5.8. The dinuclear
molecule is symmetrical around the Re(1)-O(1)-Re(1i) centre, with the bridging O(1)
lying on a crystallographic inversion centre. The bond lengths between rhenium and the
bridging oxo are exactly equal at 1.9119(3) Å and it has a Re(1)-O(1)-Re(1i) angle of
exactly 180.0°. This Re-O-Re angle is precisely linear, which is not so common when
considering other complexes of this form [7]. This Re=O distance [1.702(3) Å] as well
as the Re-O bond lengths lie within the expected range for similar complexes containing
A
B
C
D
Chapter 5 Re(V) Reactivity
101 | P a g e Nelson Mandela Metropolitan University
the O=Re-O-Re=O moiety [8-11]. This O=Re-O-Re=O moiety is commonly found in
rhenium(V) chemistry and bond distances and angles are consistent with those normally
found [7]. [Re2O3(S2CN(C2H5)2)4] is an example of a similar dinuclear Re(V) species, in
which the bridging species is essentially linear [12]. The bond distances also correlate
well with the mononuclear complex [ReOCl3(CN(CH3)3)(PPh3)] [7].
Each rhenium is centered in a distorted octahedral geometry. The basal plane is defined
by the two chloride and two isocyanide ligands, with the terminal and bridging oxo
ligands coordinated in the trans axial positions. The distortion is due to the non-linear
angles O(1)-Re-O(2) = 168.45(9)°, Cl(2)-Re-C(2) = 171.78(1)° and Cl(1)-Re-C(1) =
175.5(1)°. The angles Cl(1)-Re-Cl(2) = 88.67(3)°, Cl(1)-Re-O(1) = 90.37(3)° and Cl(1)-
Re-C(2) = 90.11(9)° are very close to orthogonality.
The isocyanides are all linear, evident from the angles Re-C(1)-N(1) and Re-C(2)-N(2)
of 174.7(3)° and 177.7(3)° respectively. Similarly, the intra-ligand angles C(1)-N(1)-
C(11) and C(2)-N(2)-C(21) of 174.3(4)° and 175.8(3)° respectively are also linear. The
bond lengths Re-C(1) [2.090(4) Å] and Re-C(2) [2.079(3) Å] are as expected for
rhenium-isocyanides [4]. The average Re-Cl bond distance of 2.39 Å is as normally
found for similar Re(V) complexes [3, 7, 13].
The hydrogen interactions for complex 2 are summarized in Table 5.2. It is evident from
this table that there are strong hydrogen interactions between C(25)-H(25b)∙∙∙O(2) and
C(26)-H(26a)∙∙∙O(2).
Table 5.2: Hydrogen interactions for complex 2
A-H∙∙∙B A-H (Å) H∙∙∙B (Å) A∙∙∙B (Å) A-H∙∙∙B (°)
C(25)-H(25b)∙∙∙O(2) 0.9900 2.5600 3.253(5) 127
C(26)-H(26a)∙∙∙O(2) 0.9900 2.5700 3.151(5) 118
Chapter 5 Re(V) Reactivity
102 | P a g e Nelson Mandela Metropolitan University
Figure 5.8: ORTEP diagram of complex 2. Hydrogen atoms were omitted for clarity
Although dimeric complexes of rhenium(V) containing the Re2O34+ core are quite
common, most examples contain tetradentate N2O2-donor ligands. For example, with
the tetradentate ligands (1,2-ethylenebis(salicylideneimine) [H2sal2en] the complex
[Re2O3(sal2en)2] was isolated from its reaction with [ReOCl3(PPh3)2]. It was determined
that these type of μ-oxo dimers are usually formed if the reactions are carried out in air
and wet solvents [13].
5.4 References
[1] H. Spies, M. Glaser, F.E. Hahn, T. Lügger, D. Scheller, Inorg. Chim. Acta, 1995,
232, 235.
Chapter 5 Re(V) Reactivity
103 | P a g e Nelson Mandela Metropolitan University
[2] F.E. Hahn, Angew. Chem. Int. Ed., 1993, 32, 650.
[3] J.C. Bryan, R.E. Stenkamp, T.H. Tulip, J.M. Mayer, Inorg. Chem., 1987, 26,
2283.
[4] P. Schaffer, J.F. Britten, A. Davison, A.G. Jones, J.F. Valliant, J. Organomet.
Chem., 2003, 680, 323.
[5] P.M. Treichel, J.P. Williams, W.A. Freeman, J.I. Gelder, J. Orgmet. Chem., 1979,
170, 247.
[6] S. Warner, L.K. Cheatham, T.H. Tulip, I.D. Williams, S.J. Lippard, Inorg. Chem.,
1991, 30, 1221.
[7] F.E. Hahn, T. Lügger, Inorg. Chim. Acta, 1998, 269, 347.
[8] B. Machura, R. Kruszynski, J. Kusz, Polyhedron, 2007, 26, 3054.
[9] B. Machura, Coord. Chem. Rev., 2005, 249, 591.
[10] N.H. Huy, U. Abram, Inorg. Chem., 2007, 46, 5310.
[11] S.R. Fletcher, A.C. Skapski, J. Chem. Soc., Dalton Trans., 1972, 10, 1073.
[12] R. Shandles, E.O. Schlemper, R.K. Murmann, Inorg. Chem., 1971, 10, 2785.
[13] F. Refosco, F. Tisato, C. Bolzati, G. Bandoli, J. Chem. Soc., Dalton Trans., 1993,
605, and references therein.
[14] T.I.A. Gerber, D. Luzipo, P. Mayer, J. Coord. Chem., 2005, 58, 1505.
Chapter 5 Re(V) Reactivity
104 | P a g e Nelson Mandela Metropolitan University
Table 5.3 - Selected crystal and data collection details for 1.
Complex 1
Formula C33H42I3N3PRe
Formula weight 1078.58
Crystal System Trigonal
Space Group R-3
a [Å] 16.8432(3)
b [Å] 16.8431(3)
c [Å] 23.5562(3)
α [°] 90
β [°] 90
γ [°] 120
Volume [Å3] 5787.4(3)
Z 6
Dcalc [g/cm3] 1.857
Absorption Coefficient (mm-1) 5.615
F(000) 3060
Crystal size [mm] 0.24 × 0.28 × 0.34
Theta Min-Max [°] 2.2, 28.3
Index ranges
h -22 : 22
k -22 : 22
l -31 : 29
Goodness-of-fit 1.23
Observed data [I > 2.0 σ I] 3037
R 0.0180
wR2 0.0522
Chapter 5 Re(V) Reactivity
105 | P a g e Nelson Mandela Metropolitan University
Table 5.4 - Selected crystal and data collection details for 2.
Complex 2
Formula C28H44Cl4N4O3Re2
Formula weight 998.89
Crystal System Monoclinic
Space Group P21/n
a [Å] 12.1765(6)
b [Å] 9.8302(5)
c [Å] 14.3784(7)
α [°] 90
β [°] 99.695(2)
γ [°] 90
Volume [Å3] 1696.5(2)
Z 2
Dcalc [g/cm3] 1.956
Absorption Coefficient (mm-1) 7.479
F(000) 964
Crystal size [mm] 0.05 × 0.46 × 0.52
Theta Min-Max [°] 2.5, 28.3
Index ranges
h -15 : 16
k -13 : 13
l -19 : 19
Goodness-of-fit 1.06
Observed data [I > 2.0 σ I] 3797
R 0.0221
wR2 0.0643
Chapter 5 Re(V) Reactivity
106 | P a g e Nelson Mandela Metropolitan University
Table 5.5 – Experimental bond distances and angles for 1.
Bond Bond length [Å]
Re-I(1) 2.8402(5)
Re-C(1) 2.013(3)
Re-P(1) 2.391(1)
N(1)-C(1) 1.151(4)
N(1)-C(2) 1.459(4)
Angle Bond angle [°]
I(1)-Re-P(1) 127.57(1)
I(1)-Re-I(1i) 86.70(2)
I(1)-Re-C(1i) 156.55(8)
P(1)-Re-C(1) 75.88(8)
C(1)-Re-C(1i) 144.2(2)
I(1i)-Re-C(1ii) 156.55(8)
C(1ii)-Re-C(1) 156.55(8)
Re-C(1)-N(1) 178.1(2)
C(1)-N(1)-C(2) 167.8(3)
Chapter 5 Re(V) Reactivity
107 | P a g e Nelson Mandela Metropolitan University
Table 5.6 – Experimental bond distances and angles for 2.
Bond Bond length [Å]
Re-Cl(1) 2.392(1)
Re-Cl(2) 2.3953(9)
Re-O(1) 1.9119(3)
Re-O(3) 1.702(3)
Re-C(1) 2.090(4)
Re-C(2) 2.079(3)
N(1)-C(1) 1.137(5)
N(1)-C(11) 1.455(5)
N(2)-C(2) 1.142(4)
N(2)-C(21) 1.446(4)
Angle Bond angle [°]
Cl(1)-Re-Cl(2) 88.67(3)
Cl(1)-Re-O(1) 90.37(3)
Cl(1)-Re-O(2) 97.00(9)
Cl(1)-Re-C(1) 175.5(1)
Cl(1)-Re-C(2) 90.11(9)
Cl(2)-Re-C(2) 171.8(1)
Re(1)-O(1)-Re(1a) 180.00
O(1)-Re-O(2) 168.45(9)
C(1)-N(1)-C(11) 174.3(4)
C(2)-N(2)-C(21) 175.8(3)
Re-C(1)-N(1) 174.7(3)
Re-C(2)-N(2) 177.7(3)
Chapter 6 Conclusion
108 | P a g e Nelson Mandela Metropolitan University
Chapter 6 Conclusion and Future Work
This study deals with the preparation of rhenium complexes in different oxidation states
containing isocyanide ligands. All of the complexes were analysed spectroscopically
and were structurally characterized.
The complexes synthesized in Chapter 3 contain potentially bidentate derivatives of
aniline and can be extended to include multifunctional ligands such as 3-nitrobenzene-
1,2-diamine (A) and 2-[(4-methylphenyl)sulfanyl]aniline (B), as depicted in Figure 6.1. It
has also been proposed that [Re(t-BuNC)Cl3(PPh3)2] can be reacted with tripodal
tetradentate ligands, in which the rhenium-isocyanide bond is retained [1].
Figure 6.1: Structure of multifunctional aniline derivates
Chapter 4 dealt with the preparation of rhenium-tricarbonyl complexes containing
isocyanide ligands. These complexes can be reacted with different aromatic,
multidentate ligands to stabilize the complexes. This is especially true for the positively
Chapter 6 Conclusion
109 | P a g e Nelson Mandela Metropolitan University
charged complex [Re(CO)3(t-BuNC)2(OH2)]+ which contains the labile aquo ligand,
which can be substituted very easily.
Different rhenium(V) precursors were reacted with isocyanides in Chapter 5 to give
large, complex molecules. An unusual seven-coordinate trigonal prismatic, square face
monocapped rhenium complex was isolated containing three isocyanides coordinated in
a cis-fashion. The class of isocyanides can be varied to see whether it reacts similarly.
Reactivity of more bulky isocyanides would be particularly interesting, since the complex
already contains three bulky iodides.
In vivo cytotoxicity screening can be performed on the complexes synthesized against a
variety of cell lines. A particularly interesting complex to screen would be [Re(CO)3(t-
BuNC)2(OH2)]+ due to its cationic nature. Cationic complexes are known to be readily
taken up by the heart, thus its in vivo behavior is something to explore in the future.
Multidentate isocyanide ligands have more favorable properties compared to the
monodentate analogues and have been successful in diagnostic applications with
technetium [2, 3]. A logical extension to this study would be the synthesis of Re(I) and
(V) complexes containing bidentate isocyanides.
References
[1] H. Spies, M. Glaser, F.E. Hahn, T. Lügger, D. Scheller, Inorg. Chim. Acta, 1995,
232, 235.
[2] F.E. Hahn, M. Tamm, L. Imhof, T. Lügger, J. Organom. Chem., 1996, 526, 149.
[3] R.J. Angelici, M.H. Quick, G.A. Kraus, D.T. Plummer, Inorg. Chem., 1982, 21,
2178.