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Gomathy Chakkaradhari
DissertationsDepartment of ChemistryUniversity of Eastern Finland
No. 151 (2019)
121/2014 KEKÄLÄINEN Timo: Characterization of petroleum and bio-oil samples by ultrahigh-resolution Fourier transform ion cyclotron resonance mass spectrometry122/2014 BAZHENOV Andrey: Towards deeper atomic-level understanding of the structure of magnesium dichloride and its performance as a support in the Ziegler-Natta catalytic system123/2014 PIRINEN Sami: Studies on MgCl2/ether supports in Ziegler–Natta catalysts for ethylene polymerization124/2014 KORPELA Tarmo: Friction and wear of micro-structured polymer surfaces125/2014 HUOVINEN Eero: Fabrication of hierarchically structured polymer surfaces126/2014 EROLA Markus: Synthesis of colloidal gold and polymer particles and use of the particles in preparation of hierarchical structures with self-assembly127/2015 KOSKINEN Laura: Structural and computational studies on the coordinative nature of halogen bonding128/2015 TUIKKA Matti: Crystal engineering studies of barium bisphosphonates, iodine bridged ruthenium complexes, and copper chlorides129/2015JIANGYu:Modificationandapplicationsofmicro-structuredpolymersurfaces130/2015 TABERMAN Helena: Structure and function of carbohydrate-modifying enzymes 131/2015KUKLINMikhailS.:Towardsoptimizationofmetaloceneolefinpolymerizationcatalystsvia structuralmodifications:acomputationalapproach132/2015SALSTELAJanne:Influenceofsurfacestructuringonphysicalandmechanicalpropertiesof polymer-cellulosefibercompositesandmetal-polymercompositejoints133/2015 CHAUDRI Adil Maqsood: Tribological behavior of the polymers used in drug delivery devices134/2015 HILLI Yulia: The structure-activity relationship of Pd-Ni three-way catalysts for H2S suppression135/2016 SUN Linlin: The effects of structural and environmental factors on the swelling behavior of Montmorillonite-Beidellite smectics: a molecular dynamics approach136/2016 OFORI Albert: Inter- and intramolecular interactions in the stabilization and coordination of palladium and silver complexes: DFT and QTAIM studies137/2016 LAVIKAINEN Lasse: The structure and surfaces of 2:1 phyllosilicate clay minerals138/2016 MYLLER Antti T.: The effect of a coupling agent on the formation of area-selective monolayers of iron a-octabutoxy phthalocyanine on a nano-patterned titanium dioxide carrier139/2016KIRVESLAHTIAnna:Polymerwettabilityproperties:theirmodificationandinfluencesupon water movement140/2016 LAITAOJA Mikko: Structure-function studies of zinc proteins141/2017 NISSINEN Ville: The roles of multidentate ether and amine electron donors in the crystal structure formation of magnesium chloride supports 142/2017 SAFDAR Muhammad: Manganese oxide based catalyzed micromotors: synthesis, characterization and applications143/2017 DAU Thuy Minh: Luminescent coinage metal complexes based on multidentate phosphine ligands144/2017AMMOSOVALena:Selectivemodificationandcontrolleddepositiononpolymersurfaces145/2017 PHILIP Anish: PEI-mediated synthesis of gold nanoparticles and their deposition on silicon oxide supports for SERS and catalysis applications146/2017 RAHMAN Muhammad Rubinur: Structure and function of iron-sulfur cluster containing pentonate dehydratases147/2018 ANKUDZE Bright: Syntheses of gold and silver nanoparticles on support materials for trace analyses using surface-enhanced Raman spectroscopy148/2018 PENTTINEN Leena: Structure determination of enzymes with potential in processing of cell wall compounds149/2018 SIVCHIK Vasily: Tuning the photoluminescence of cyclometalated platinum(II) compounds via axial and non-axial interactions150/2019 MIELONEN Kati: Hierarchically structured polymer surfaces: Curved surfaces and sliding behavior on ice
Tuning the emission properties of oligophosphine copper and silver complexes with ancillary ligands
Gom
athy Chakkaradhari: Tuning the em
ission properties of oligophosphine copper and silver complexes w
ith ancillary ligands
151
Tuning the emission properties of oligophosphine
copper and silver complexes with ancillary ligands
Gomathy Chakkaradhari
Department of Chemistry
University of Eastern Finland
Finland
Joensuu 2019
2
Gomathy Chakkaradhari
Department of Chemistry, University of Eastern Finland
Supervisor
Prof. Igor O Koshevoy, University of Eastern Finland
Referees
Prof. Axel Klein, University of Cologne, Germany
Dr. Christophe Lescop, Institute of Chemical Sciences of Rennes, France
Opponent
Doc. Raija Oilunkaniemi, University of Oulu, Finland
To be presented with the permission of the Faculty of Science and Forestry of the
University of Eastern Finland for public criticism in Auditorium M101, Yliopistokatu 7,
Joensuu, on May 3rd 2019 at 12 o’ clock noon.
Copyright © 2019 Gomathy Chakkaradhari
ISBN: 978-952-61-3055-2 (Print)
ISBN: 978-952-61-3056-9 (PDF)
ISSN: 2242-1033
Grano Oy Jyväskylä
Jyväskylä 2019
ABSTRACT
Coinage metal complexes, which form light emitting materials, have attracted a great
deal of research attention due to their versatile chemistry, natural abundance, and many
potential applications. These compounds are used as emitters in solid state lighting, a
variety of sensors, cell imaging, and photocatalysis. In the early days, significant
progress in the field of photofunctional metal-containing molecular materials was
associated with the derivatives of noble metals, which are often expensive and toxic. The
past two decades clearly demonstrate that further scientific developments in metal-based
chromophores have significantly shifted to environmentally friendly compounds of
copper and silver. As one might expect, the physical properties of these species are
primarily defined by the constituting organic fragments, which form the coordination
environment around the metal centers. Thus, it is not surprising that noticeable evolution
of inorganic and organometallic luminescent complexes occurs upon introducing new
ligands or ligand combinations, and upon adjusting their electronic and stereochemical
characteristics.
In examining the nearly 50-year history of copper luminophores, it is easy to track how
extensive experimental and theoretical investigations gradually improved our
understanding of structure-property relationships and of the processes occurring in the
excited state, on the molecular level. Consequently, this knowledge has allowed for a
remarkable advance from the first weakly luminescent diimine and phosphine-halide
copper complexes to highly efficient emitters with vastly improved quantum yields and
widely variable colors. Nevertheless, we are currently far from utilizing the entire
potential of coordination complexes of copper, and particularly of silver, d10 ions; the
utilization of the latter has been largely underestimated until recently due to frequently
encountered photodegradation. Moreover, our ability to predict and rationally
manipulate the photophysical characteristics of the transition metal luminophores in the
solid state, and therefore to develop next generation photofunctional materials, remains
at an early stage.
In this thesis, a series of copper(I) and silver(I) luminescent compounds was synthesized
with the aid of sterically demanding tri- and tetradentate organophosphorus ligands as
primary building blocks, which have rarely been utilized in the coordination chemistry
of d10 complexes prior to this work. The chosen molecular design complies with a
general strategy established for copper emitters, according to which bulkier ligands
suppress the radiationless relaxation of the excited state. Following this concept, very
efficient luminescence was attained; in particular, one of the highest quantum yield for
silver complex, that had been reported at the time, was realized. Although the metal-
phosphine framework plays a pivotal role in the observed emission, the ancillary ligands
proved to have an important influence on the electronic transitions, which occur during
the excitation and emission processes. In addition to the molecular features, which can
be tuned synthetically, it was demonstrated that the solid-state luminescence crucially
depends on the intermolecular arrangement in the bulk solid. As a result, a delicate
interplay of molecular and crystal engineering can produce novel materials with
interesting optical functionalities.
4
LIST OF ORGINAL PUBLICATIONS
This dissertation is a summary of original publications I-V.
I Chakkaradhari, G.; Belyaev, A. A.; Karttunen, A. J.; Sivchik, V.; Tunik, S. P.;
Koshevoy, I. O., Alkynyl triphosphine copper complexes: synthesis and
photophysical studies, Dalton Trans., 2015, 44, 13294-13304.
II Chakkaradhari, G.; Chen, Y-T.; Karttunen, A. J.; Dau, M. T.; Janis, J.; Tunik,
S. P.; Chou, P-T.; Ho, M-L.; Koshevoy, I. O., Luminescent Triphosphine
Cyanide d10 Metal Complexes. Inorg. Chem., 2016, 55 (5), 2174-2184.
III Dau, M. T.; Asamoah, B. D.; Belyaev, A. A.; Chakkaradhari, G.; Hirva, P.;
Janis, J.; Grachova, E. V.; Tunik, S. P.; Koshevoy, I. O., Adjustable
coordination of a hybrid phosphine-phosphine oxide ligand in luminescent Cu,
Ag and Au complexes. Dalton Trans., 2016, 45, 14160-14173.
IV Chakkaradhari, G.; Eskelinen, T.; Degbe, C.; Belyaev, A. A.; Melnikov, A. S.;
Grachova, E. V.; Tunik, S. P.; Hirva, P.; Koshevoy, I. O., Oligophhosphine-
thiocyante copper(I) and silver(I) complexes and their borane derivatives
showing delayed fluorescence. Inorg. Chem., 2019, 58, 3646-3660.
V Pan, Z-B.; Wang, Y-C.; Chakkaradhari, G.; Zhu, J. F.; He, R-Y.; Koshevoy, I.
O., Chou, P-T.; Pand, S-W.; Ho, M-L., Silver Metal Complex as a Luminescent
Probe for Enzymatic Sensing of Blood Glucose and Urine, Dalton Trans., 2018,
47, 8346-8355.
AUTHOR’S CONTRIBUTION
The results presented in the publications I, II, IV are based on the ideas proposed by the
authors and the supervisor. The author designed and prepared all complexes in these
works (except terminal di- and trialkynes in I, compounds 11 and 12 in IV). The joint
publications III and V include the materials provided by the author (compounds 11–16
in III and Ag3 in V). The author carried out the X-ray diffraction analysis, IR and NMR
spectroscopic measurements (except 19F and low temperature NMR experiments).
Theoretical analysis and photophysical investigations were performed by the
collaborating groups, the author took part in the interpretation of these data. The author
has co-written the publications in collaboration with the supervisor and co-authors.
5
CONTENTS
Abstract ......................................................................................................................... 3
List of original publications ......................................................................................... 4
Contents ......................................................................................................................... 5
Abbreviations ................................................................................................................ 6
1. Introduction .............................................................................................................. 7
1.1. Selection of phosphine and ancillary ligands ...................................................... 9
1.2. Evolution of Cu(I) luminescent compounds ...................................................... 10
1.3. Silver(I) complexes: an alternative class of luminophore ................................. 16
1.4. Applications ....................................................................................................... 19
1.4.1. Oxygen gas sensing ................................................................................ 19
1.4.2. Cu(I) complexes in photocatalysis ......................................................... 22
1.5. Aims of the study ............................................................................................... 24
2. Experimental ........................................................................................................... 25
2.1. Phosphine ligands .............................................................................................. 25
2.2. Synthesis of metal complexes ............................................................................ 25
2.3. Purification and characterization ....................................................................... 27
3. Results and discussion ............................................................................................ 28
3.1. Mononuclear tri- and tetraphosphine d10 complexes ......................................... 28
3.1.1. Triphosphine cyanide complexes ............................................................. 29
3.1.2. Tri- and tetraphosphine thiocyanate complexes ....................................... 31
3.1.3. Triphosphine halide complexes ................................................................ 32
3.1.4. Tri and tetraphosphine isothiocyantoborate complexes............................ 33
3.1.5. Triphosphine alkyne complexes ............................................................... 35
3.2. Photophysical properties of mononuclear complexes ........................................ 36
3.2.1. [Cu(P3)X] halides and pseudohalides ....................................................... 36
3.2.2. [Ag(P3)X] halides, pseudohalides, and [Au(P3)CN] ................................ 39
3.2.3. [M(P4)X] thiocyanate and isothiocyanatoborate complexes .................... 41
3.3. Dinuclear bi- and triphosphine d10 complexes .................................................... 43
3.3.1. Thiocyanate bridged dinuclear complexes .............................................. 43
3.3.2. Cyanide bridged di- and trinuclear complexes ........................................ 45
3.3.3. Alkynyl bridged di-and trinuclear complexes ......................................... 47
3.4. Photophysical properties of di- and trinuclear complexes ................................... 49
4. Conclusions ............................................................................................................. 53
Acknowledgements ..................................................................................................... 55
5. References ............................................................................................................... 56
6
ABBREVIATIONS
FTIR Fourier Transformation Infra-red
NMR Nuclear Magnetic Resonance
MS Mass spectra
EA Elemental analysis
P3 bis(2-diphenylphosphinophenyl) phenylphosphine
P4 Tris(2-diphenylphosphino) phenylphosphine
SCN Thiocyanate anion
CN Cyanide anion
NCS Isothiocyanate ligand
NC Isocyanide ligand
OLEDs Organic light emitting diodes
LEECs Light emitting electrochemical cells
EQE External quantum yield
TADF Thermally activated delayed fluorescence
ISC Intersystem crossing
RISC Reverse intersystem crossing
HOMO Highest occupied molecular orbital
MLCT Metal to ligand charge transfer
LLCT Ligand to ligand charge transfer
LMCT Ligand to metal charge transfer
LC Ligand center
DFT Density functional theory
PMMA Polymethylmethacrylate
THF Tetrahydrofuran
KBr Potassium bromide
tfpb tetrakis(bis-3,5-trifluoromethyl phenyl) borate
pftpb tetrakis(pentafluorophenyl) borate
PF6 Hexafluoro phosphate
BF4 Tetrafluoro borate
PPh3 Triphenyl phosphine
tBu Tertiary butyl
2-MeTHF 2-Methyl tetrahydrofuran
TEA Triethyl amine
NHC N-heterocyclic carbene
PS Photosensitizer
Ksv Stern-Volmer constant
Im Imidazole
7
1. INTRODUCTION
To what extent are we conscious of the importance of the copper, silver, and gold metals,
which constitute the group 11 d-block elements in the periodic table? Olympic medals
for first, second, and third place have been awarded in the order of gold (yellow), silver
(white) and bronze (red-brown) since 1904 (Figure 1).1 The sequence of the winners runs
from gold to bronze (which is an alloy principally containing copper) according to the
natural abundance of these metals. They have a relatively stable nd10(n+1)s1 electronic
configuration with a completely filled d-shell and are called coinage metals, since they
were used to make coins due to their noticeable inertness (particularly silver and gold).
Figure 1. Olympic medals for first, second, and third place.1
Organometallic compounds of late transition metals often demonstrate advantageous
optoelectronic properties and therefore play an important role in the development of new
chromophores. In this respect, the coinage metal series has attracted a great deal of
attention in diverse fields such as organic light emitting diodes (OLEDs),2-8 light-
emitting electrochemical cells (LEECs),9-10 sensing applications,11-14 and
photocatalysis.15-19 In this respect, silver and, to a greater extent, copper compounds have
been extensively investigated due to their high natural abundance and low toxicity.
In general, the applications of compounds of silver and copper are extremely diverse.
Thus, copper (II) salts efficiently control the algae in water reservoirs (including lakes,
ponds, etc.).20 Copper (I) oxide is used as an antifouling paint, as a catalyst for numerous
organic reactions, and as a powerful absorbent for carbon monoxide.20 Copper plays an
important role in human growth; the average requirement for this micronutrient in the
human body is 1.5–3 mg per day.21 It is used in medicines and food products.21 The
appearance of the tetraamine copper (II) complex [Cu(NH3)4]2+ was the first
scientifically documented observation of a coordination compound (1597), although it
could not be properly formulated at that time.22 The application of silver halides in
photography has been known since the beginning of the nineteenth century, when the
first images were produced by J. Herschel, J. N. Nicepce, and L. Daguerre,23 using an
AgBr suspension in gelatin to produce a black and white photographic film. The
antibacterial nature of silver is extensively exploited in different kinds of healthcare
products (creams and ointments). The Ag-NHC (NHC = N-heterocyclic carbene)
compounds are widely used in medicinal applications, as the strong Ag-C bonds produce
stable compounds.24 The various fields of practical applications of Cu(I) and Ag(I) metal
complexes are summarized in Figure 2.
8
Figure 2. The use of Cu(I) and Ag(I) compounds in different fields.
The peculiar behavior of Cu(I) and Ag(I) compounds largely results from a variable
coordination number, and, therefore, a variety of accessible structural arrangements,
which dramatically influence the optoelectronic behavior of these species. The
photophysical and photochemical properties of Cu(I) complexes have been actively
investigated since the early 1970s.25 The first luminescent coinage metal complexes, of
the general formula LmCunXn (L = P/AsPh3), X = Br or Cl), were reported by Dori and
co-workers in 1970.26 McMillin et al. documented the first observation of room
temperature phosphorescence in solution for the [Cu(dmp)2]+ (dmp = 2,9-dimethyl-1,10-
phenanthroline) complex.27
In early 1960, Allison et al. studied the effect of metal atoms on the luminescence spectra
of porphyrins28 and noted that the silver derivatives did not show any emission. Later, in
1970, the influence of temperature on the luminescence of the silver halides AgCl and
AgBr was described by Marinchik.29 Despite the photo-instability of many Ag(I)
derivatives, the last two decades have seen a steady growth in the number of articles
dealing with silver luminescent materials (30–50 articles per year, according to the
Scopus search results for “silver luminescent compound”).
Although many early Cu(I) compounds were unstable to vacuum sublimation and
solution processing, the impressive progress in molecular design and understanding of
structure-property relationships has led to a number of highly stable, luminescent
complexes of Cu(I) and Ag(I) being reported since 2000. Furthermore, optoelectronic
devices, developed on their basis, have comparable performances to those utilizing the
noble metals (see the discussion in sections 1.2 and 1.3). This makes the copper(I) and
silver(I) luminophores attractive and affordable candidates for photophysical study.
9
1.1 SELECTION OF PHOSPHINE AND ANCILLARY LIGANDS
The use of different ligands containing the heteroatoms P or S (soft donors) and N or O
(hard donors) combined with transition metals allows tuning of the optical properties of
the resultant complexes. The phosphine ligands show high affinities for the late transition
group 11 metals, Cu, Ag, and Au, in the +1 oxidation state. The stereochemistry, bonding
nature, and steric and electronic properties of polyphosphine chelating ligands result in
different coordination modes, providing diverse opportunities for formation of stable
coordination complexes, the emission properties of which are typically tuned by
changing the ligands.
Special interest has been focused on the sterically demanding tri- and tetradentate
phosphine ligands, as they produce a robust structural arrangement around the metal
centers that improves the rigidity of the resulting complexes, required for efficient
luminescence.
Representative examples of reported tri- and tetradentate chelating phosphine ligands
are depicted in Figure 3 (A30-33, B30, 34-37, C38-40, D41, E42-43, F44, G45, H45, I46), many of
which (A, C, E, and similar ) have been used for the preparation of d10 metal complexes.
Figure 3. Reported tri- and tetradentate ligands.
In addition to the phosphine ligand, the selection of ancillary ligands is highly important
for adjusting the spectroscopic characteristics of the metal complexes. The coordination
number of the Cu(I) and Ag(I) ions depends on the joint effect of the donor properties
of the ligand environment. Different stoichiometries of metals and ligands can produce
10
mono-, di-, and multinuclear complexes.47 Several types of ancillary ligand are typically
combined with polyphosphines in coinage metal complexes:
(i) halides,
(ii) pseudohalides (CN, SCN, NCS, NC),
(iii) alkynyls,
(iv) thiolates,
(v) carbenes
An interesting characteristic of the halides, pseudohalides, and alkynes is that they can
act as bridges between two or more metal atoms. The first luminescent Cu(I) compounds
with bridging halides, [CuI(Py-X)]4 (X = I or Br), were reported by Hardt and co-
workers.48-49 Subsequently, many research groups have studied phosphine coinage metal
complexes with alkyne,50-51 halide51 and pseudohalide25 ancillary ligands.
1.2 EVOLUTION OF Cu(I) LUMINESCENT COMPOUNDS
The development of energy efficient light emitting devices based on metal complexes is
primarily associated with Ir(III), Pt(II), and Os(II) noble metal compounds. Generally,
phosphorescent emitters undergo radiative relaxation of the triplet excited states, which
is characterized by a longer lifetime, whereas in fluorescent materials the emission
occurs only from the singlet excited state. An inexpensive alternative to materials
containing high-cost heavy metals is offered by the compounds of more abundant and
cheaper metals such as Cu(I) and Ag(I) derivatives.52-54 In contrast to the noble metal-
based phosphors, copper and silver species often demonstrate the thermally activated
delayed fluorescence (TADF) phenomenon. In the TADF process, the conversion
between the first excited singlet state (S1) and the triplet excited state (T1), termed as an
intersystem crossing (ISC), is reversible under ambient conditions and is followed by
the reverse intersystem crossing (RISC) from T1 to S1, due to the small energy difference
between the lowest excited singlet and triplet states (which is ideally less than 1000 cm-
1 and therefore the thermal energy at 298 K is sufficient to overcome this barrier). As a
result of this process, the system radiatively returns to the ground state (S0) from the first
singlet excited state (S1), although with a delay in the order of microseconds.
Numerous Cu(I) complexes have been found to behave as TADF materials due to a low
activation energy ΔE(S1-T1), which facilitates fast RISC.55 During the last 20 years, the
number of publications devoted to Cu(I) compounds showing delayed fluorescence has
dramatically increased,55 thanks to facile tuning of their physical properties by changing
the ancillary ligands and to their successful application in the fabrication of efficient
electroluminescent devices.56-59
The dawn of investigations into Cu(I) chromophores is associated with the pioneering
research of McMillin, who studied the electronic properties of [Cu(NN)2]+ mononuclear
homoleptic complexes (Figure 4). These compounds show rich absorption and emission
behavior, which principally depends on the nature of the phenanthroline system and the
substituents within it.60-64 It has been shown that the tetrahedral geometry of the ground
11
state is distorted to a flattened, planar-like arrangement in the excited state, significantly
affecting the electronic structure. In general, these complexes are weakly emissive
(quantum yields are typically less than 1%) in solution due to the structural
reorganization in the excited state, which may lead to the formation of Cu(II) complexes.
Furthermore, the formation of an exciplex in the excited state (from the association of
pentacoordinate transition complexes with the solvent molecules or counter ions) can
induce ultra-fast non-radiative transitions and emission quenching in [Cu(NN)2]+
compounds.64
Reducing the possibility of exciplex formation can increase the lifetime and the quantum
yield of the emission. According to a general trend observed for a series of
phenanthroline [Cu(NN)2]+ complexes, the substituents in the 2 and 9 positions of the
NN ligand dramatically influence the lifetime, which varies from 90 to 920 ns for
aliphatic groups of variable bulkiness (Figure 4). The major factors causing the lifetime
increase are related to the growing number of substituents in the phenanthroline system
and particularly to the sizes of the substituents in the 2 and 9 positions.65
Figure 4. Reported [Cu(NN)2]+ complexes and their excited state lifetimes.65
In order to achieve better emission properties, heteroleptic [Cu(PP)(NN)]+ complexes
were introduced by McMillin in the late 1970s.66-67 This type of N, P- mixed ligand
compound started to receive considerable attention in the 21st century. McMillin and
coworkers were the first to report the highly emissive [Cu(POP)(dmp)]+ complex (τ =
14.3 µs and Φ = 0.15, in oxygen-free dichloromethane solution).68 Tailoring the
chelating ligands (PP) and (NN) to tune the electronic and steric features strongly
influences the emissive properties of the resulting copper(I) coordination compounds.
The quantum yields depend on the structural rigidity of the complexes; bulkier
substituents induce a higher intensity of luminescence. Nevertheless, manipulating the
excited state lifetimes of these complexes, in a rational manner, on the molecular level
12
still presents a substantial puzzle. Many [Cu(PP)(NN)]+ species69-72 have since been
synthesized and subsequently applied in electroluminescent devices (OLEDs5, 7, 73 and
LEECs).74
The following examples, 9–11 (Figure 5), illustrate the significant changes in
photophysical properties achieved by varying the ligand environment in [Cu(PP)(NN)]
type complexes.75 These compounds have a small energy gap ΔE(S1-T1), and, as
powders, exhibit fast TADF (blue-green emission) with quantum yields from 70% to
90% at 300 K (Figure 5).
Figure 5. Schematic structures of 9–11 (left); luminescence decay time versus temperature for
powder samples of 9–11 (right).
The importance of steric bulkiness in [Cu(PP)(NN)] complexes was clearly shown by
inserting additional methyl groups into the bipyridyl moiety.76 The weak solid state
emission of 13 (Φ = 9%) increased dramatically, up to 74% for 12, with increasing
molecular rigidity, due to the higher repulsion between bipyridine and the diphosphine
ligands (Figure 6). This interaction inhibited the non-radiative transitions and thus
enhanced the quantum yield.
Figure 6. Schematic structures of copper complexes 12 and13.
Aside from the diphosphine-diimine [Cu(PP)(NN)]+ family of copper(I) luminophores,
other types of ligand sphere have been introduced in order to alter the optical
characteristics. For instance, combining phosphines, halides, and N-heterocyclic ligands
(L) resulted in a series of compounds of the general formula [Cu2(µ-X)2(PPh3)(L)],
13
which possess halide-bridged bimetallic units77 and which exhibit emission colors
ranging from blue to red.77 Simple mononuclear Cu(I) compounds [CuX(PPh3)2(4-
methylpyridine)] (X = Cl (14), Br (15), I (16), Figure 7), synthesized from commercially
available starting materials, demonstrated intense blue emission at room temperature, in
the solid-state, and reached 100% quantum efficiency.78
Figure 7. Schematic structure of copper complexes 14–16.
Tsuboyama and coworkers described halide-bridged dinuclear complexes, supported by
the bidentate P-donor ligand 1,2-bis(diphenylphosphino)benzene (17–19), which
showed solid-state room temperature luminescence with quantum yields of 80%, 60%,
and 60% respectively (Figure 8). Specifically, compound 17 was used to prepare an
electroluminescent device with an external quantum efficiency (EQE) of 4.8%.79
Furthermore, strongly emissive dicopper complexes Cu2I2(PyrPhos)(PR3)2 (20a–c)
(Figure 8), stabilized by the bridging pyridyl-phosphine and comprised of monodentate
phosphines and phosphites have been developed.80
Figure 8. Schematic structures of compounds 17–24.
14
These materials demonstrated delayed fluorescence due to a small energy separation
ΔE(S1-T1), with high emission quantum yields reaching 99% in powdered samples (85%
in thin films), under ambient conditions, which makes them suitable for OLED
fabrication. In the case of heterodentate N, P donor ligands, quantum yields of nearly
100%, in the solid state at 77 K, and of up to 65% at 298 K, were attained for compounds
21–24 (Figure 8). These complexes show thermally activated delayed fluorescence,
which is highly attractive for electroluminescent applications.81
Active progress in organometallic carbene chemistry, particularly of Ag(I)- and Au(I)-
NHC (NHC = N-heterocyclic carbenes) complexes, stimulated the synthesis of Cu(I)-
NHCs, which were unknown until 2009.82 Using heterodentate imine-carbene ligands as
NC chelating analogues of common diimines, four-coordinate tetrahedral Cu(I)
complexes of the general formula [Cu(PP)(NC)]+ can be readily generated (Figure 9).
Photophysical study of NHC derivatives 25 and 26 revealed their TADF behavior (λem
= 520 and 570 nm, respectively) with moderate solid-state quantum yields (56% and
35% respectively).83 In the recently reported congeners 27a–c, the decoration of the
pyridine-moiety of the py-NHC ligand with electron donating and withdrawing groups
resulted in the shift of the emission energy to shorter and longer wavelengths,
respectively (489, 518, 539 nm). In contrast, the strength of these substituents does not
correlate in the same way with the emission wavelength, probably due to the contribution
of the py-NHCs ligands to both the HOMOs and LUMOs.84
Figure 9. Schematic structures of complexes 25–27.
Compared with complexes with conventional four coordinate geometry, two- and three-
coordinate Cu(I) complexes are expected to undergo less structural distortion in the
excited state. A new series of 2-coordinate copper complexes with cyclic alkyl(amino)
carbene ligands (28–31) (Figure 10) was introduced by Stefen and coworkers. The
phosphoresence emission of these compounds varied from violet, at 398 nm (31), to
green, at 512 nm (28–30), in the solid state, with quantum yields of up to 65%.85 Recently
the same group reported a family of linear Cu(I) complexes of the general formula
[Cu2{tBuIm(CH2)3tBuIm}X2] (X = PF6, n = 3), (X = BF4, n = 3), (X = BF4, n = 1)
[Cu(tBu2Im)2]PF6 (Im = imidazole), which showed mechanochromic phosphoresecence.
Their solid state quantum efficiencies varied between 4% and 51%.86
15
Figure 10. Schematic structures of complexes 28–31.
Peters et al. reported three-coordinate amidophosphine complexes, 32–34, which
demonstrate a significant alteration of the emission color from blue to yellow (Figure
11).87
Figure 11. Schematic structures of complexes 32–34.
For the purpose of stabilizing low coordination number compounds, bulky NHC ligands
are particularly attractive due to their strong bonding to transition metal ions and high
steric demand, which lead to robust complexes. Thompson and coworkers prepared the
trigonal planar three-coordinate Cu(I) NHC complexes, 35 and 36 (Figure 12), which
are phosphorescent in solution (maximum Ф = 1.4%) and in the solid state (maximum
Ф = 58%).88 In a continuation of this work, modification of the chelating pyridyl-azolate
(NN) ligands of the NHC complexes 37a–d (Figure 12) was carried out. A systematic
investigation of the physical properties of the resulting complexes revealed a significant
change in the quantum yields of compound 37a (in soution, Ф = 17%) and 37c (as a neat
crystalline material, Ф = 62%).89
16
Figure 12. Schematic structures of the three-coordinate complexes 35–37.
Taking into account the wide range of ligands suitable for binding to the Cu(I) ion, it is
evidently possible to generate an extensive library of compounds with readily tunable
optoelectronic properties, the photophysical performance of which would be comparable
to that of d6 metal chromophores. As a result of impressive synthetic effort and
comprehensive analysis of structure-property relationships, Cu(I) complexes have
developed from weakly emissive [Cu(NN)2+] species to excellent emitters with nearly
100% quantum efficiencies by means of rational design of the ligand environment. In
general, the optical properties of these luminophores can be influenced by modulating
the steric and electronic factors of the constituent ligands. In addition to the dramatically
improved quantum yields, a color variation from red to green-blue has been achieved by
tuning the nature of the emissive excited state, which can be comprised of different
contributions from MLCT (metal-to-ligand charge transfer), LLCT, and ligand centered
origins.
1.3 SILVER(I) COMPLEXES: AN ALTERNATIVE CLASS OF LUMINOPHORE
Luminescent organometallic silver complexes often occur as polynuclear assemblies and
their emission properties strongly depend on the metal-metal interactions and the
geometry of the metal core. This type of interaction induces the combination of metal
centered and ligand-to-metal charge transfer (LMCT) electronic transitions.90-91 In
contrast, in the absence of metal-metal bonding, the luminescence of silver(I) complexes
typically originates from ligand-centered (LC) or LLCT excited states, as the low energy
17
metal-to-ligand charge transfer is less favorable for the Ag(I) ion due to its higher
oxidation potential compared to that of Cu(I).90, 92-95
This is exemplified by complex 38 (Figure 13), the emission of which is associated with
ligand-to-ligand charge transfer (LLCT) transitions.96 Osawa et al. studied the
luminescence and photochemistry of a homoleptic mononuclear Ag(I) compound
containing diphosphine ligands (39, Figure 13). Interestingly, at 298 K, orange
luminescence was observed with a maximum at 670 nm, while at 77 K the luminescence
was hypsochromically shifted to 456 nm, in degassed 2-MeTHF. The large red shift (220
nm) of the emission and low quantum yield at 298 K indicate that the excited state was
MLCT in origin, with charge transfer occuring from the Ag(I) ion to the diphosphine.
This indicates that the structural modification from a tetrahedral to a planar arrangement
in the relaxed excited state results in orange luminescence at 298 K.97 For 39 and the
related mononuclear diphosphine complex 40 (Figure 13) it was suggested that, in the
excited state, they are attacked by the nucleophilic solvent molecules to a lesser extent
than are Cu(I) congeners, which decreases the possibility of non-radiative deactivation.
These results indicate that better quantum efficiently might be realized for Ag(I)
complexes in comparison to those of Cu(I).98
It is worth noting that investigations of thermally activated delayed fluorescence in Ag(I)
complexes are less frequently reported with respect to those of Cu(I) metal complexes.58,
99
Figure 13. Schematic structures of complexes 38–41.
As mentioned above, Cu(I) complexes tend to undergo MLCT electronic transitions due
to the low oxidation potential of the Cu(I) metal ion.23, 100 On the contrary, stabilization
of 4d silver orbitals frequently leads to ligand-centered emission. Thus, it is challenging
to optimize the TADF properties of Ag(I) compounds. To develop silver complexes with
delayed fluorescence, electron-donating phosphine ligands have been introduced to
destabilize the low-lying 4d metal orbitals.52 For instance, the dichloro bridged Ag(I)
18
dimer with a dppd ligand (41, Figure 13) shows blue emission at room temperature,
ascribed to TADF, with an impressive quantum yield of 93%; and an energy gap ΔE(S1-
T1) between the lowest singlet and triplet excited states of 980 cm-1.100
Yersin and coworkers have recently reported highly efficient TADF emitters of the
general Ag(NN)(PP) type (42–44, Figure 14).101 The nido-carborane-bis-
(diphenylphosphine)(P2-nCB), with a negatively charged backbone, serves as strong
electron donor. These compounds reach 100% quantum yields with short decay times of
1.4 µs, which is even shorter than the reported lifetime of 1.5 µs for the strongly
phosphorescent Ir(ppy)3 complex.102 It is important to note that, so far, this is the shortest
radiative lifetime determined for Ag(I) and Cu(I) luminophores. Introducing the methyl
and n-butyl groups into the 2 and 9 positions of the 1,10-phenanthroline ligand
influenced the optical properties of these Ag(I) complexes. An increase in the structural
robustness of these species reduces the non-radiative decay and leads to the maximum
quantum efficiency.
Figure 14. Schematic structures of silver complexes 42–44.
The combination of the tetradentate phosphine ligand, tpbz, with a terminal halide and
ancillary phosphine produces dinuclear silver complexes with the general formula
[(Ag(PPh3)(X)]2(tpbz) (X = Cl 45, Br 46, I 47) (Figure 15). Solid-state light-blue to green
emissions (TADF), with maxima between 471 nm and 495 nm, and quantum yields of
up to 98%, were observed for these compounds. The tetraphosphine ligand serves as a
bis-bidentate bridge between the two silver atoms. Its phenylene spacer is a major
contributor to the LUMO; the HOMO is primarily distributed among Ag, P, and the
halides, as predicted by the DFT calculations.54 The same tetradentate ligand, utilized
together with the strongly electron-donating carborane-diphosphine (P2-nCB), produced
the dinuclear Ag(I) complex 48 (Figure 15), which showed highly efficient TADF with
a 1.9 µs decay time and a low energy gap ΔE(S1-T1) = 480 cm-1, as a result of
(M+L)L´CT transitions, which lead to the excited states.103
19
Figure 15. Schematic structures of silver complexes 45–47 (left) and complex 48 (right).
1.4 APPLICATIONS
In addition to the abovementioned application of copper(I) emitters for the fabrication
of light-emitting devices (OLEDs and LEECs), it is worth highlighting two notable areas
where these molecular materials could be successfully utilized.
1.4.1 OXYGEN GAS SENSING
Solid state oxygen sensors can be made with the help of supporting materials16, 104-105 or
with pure porous phosphorescent compounds.105-107 A limitation of the supporting
materials is possible degradation of the polymer matrix, which stimulated the
development of pure compounds as oxygen sensors. Early progress in this direction
involved the expensive d-block noble metals Ru108, Pt109, and Ir110-111, due to their long-
lived triplet excited states, induced by high spin-orbit coupling. To reduce the production
cost, the focus moved to the search for oxygen sensing materials based on
environmentally friendly elements. In this respect, complexes of highly abundant Cu
metal, capable of forming metal-to-ligand charge transfer (MLCT) emissive states with
long lifetimes, have drawn considerable attention as potential oxygen sensors.104
The photoluminescent sensing of oxygen is based on collisional non-radiative quenching
of the triplet excited state of the probe (i.e. complex) via collisional interaction with an
oxygen molecule in its triplet ground state. In inert (non-aerated) conditions, these
phosphorescent compounds are emissive, but in contact with air, weak to negligible
emission is observed. The oxygen concentration can be measured by estimating the
degree of the decrease in emission intensity. For the favorable cases, when the material
is uniform and the emission occurs from only one site, linear fitting of the intensity
change (I0/I) vs O2 concentration (Stern–Volmer plot) can be performed for analytical
purposes. Otherwise, a non-linear dependence suggests that the emission is generated by
the two different sites, which have different susceptibilities to quenching.104
The supported sensing materials containing copper luminophores are exemplified by
compounds of the [Cu(PP)(NN)]+ type (49–51) and by the neutral [Cu(PP)(NN)]
molecule, 52 (Figure 16), embedded into polymeric matrices such as polystyrene,104, 112
PMMA13, and MCM-41.113
The crystal engineering approach to obtain efficient, non-supported sensing materials
aims to increase the void space in the crystal structure using ionic compounds. The most
common anions are BF4- (tetrafluoroborate) and tfpb (sodium tetrakis [3,5-
20
bis(trifluoromethyl)phenyl] borate. The void space plays a crucial role in oxygen
diffusion into the crystal lattice and in regulating the collisional interactions with the
emitter molecules. Additionally, it is necessary to consider not only the void space (i.e.
porosity) of the compounds, but the emission lifetime, brightness, and stability of the
compounds, and the reproducibility, which are important factors, essential for efficient
sensing.11
Figure 16. Schematic structures of copper complexes, 49–52, used with supporting materials
for oxygen gas sensing.
Selected properties (void space, KSV, and quantum yield in both aerated (O2) and non-
aerated conditions) of the prominent crystalline copper(I) sensors 53–58 (Figure 17),
prepared by Mann and coworkers, are listed in Table 1.12, 107 These compounds show
better quantum yields and sensitivities (approximately 10 times greater) than reported
homoleptic [Cu(NN)2]+ derivatives (NN = 1,10-phenanthroline (phen), 2,9-dimethyl-
1,10-phenanthroline (dmp), 2,9-dimethyl-4,7-diphenyl-1,10-phenanthroline (bdmp),
2,9-diisopropyl-1,10-phenanthroline (dipp), and 2,9-di-tert-butyl-1,10-phenanthroline
(dbp)).11 In particular, compound 54 has an excellent quantum yield of 0.66(5)% (under
N2) and Stern–Volmer constant (KSV = 5.65 atm-1), compared to the previously published
pure crystalline system [Ru(4,7-Me2Phen)3](tfpb)2] (Φ = 0.11(2)% (under N2), KSV =
4.76 atm-1).106 Furthermore, compounds 57 and 58 are almost non-emissive in aerated
conditions and brightly emissive in un-aerated conditions (Figure 18).
21
Figure 17. Schematic structures of copper complexes 53–58, reported as crystalline oxygen gas
sensors.
Table 1. Void spaces and quantum yields (aerated and non-aerated) for compounds 53–58.12, 107
a The estimated detection limit is 5 x 10-3atm-1.
Compound
Number
Void
space %
Quantum
yield (N2)
Quantum
yield (O2)
KSV atm-1
53 4.6 0.88 (9) 0.19 (2) 3.60(2)a
54 3.3 0.66 (5) 0.084 (3) 5.65(8)a
55 2.0 0.95 (5) 0.22 (1) 3.41(9)a
56 2.0 0.47 (4) 0.31 (3) 0.153(2)a
57 2.3 0.228 (5) 0.0029 (2) 96(1)
58 3.7 0.226 (9) 0.0021 (5) 91.9(3)
22
Figure 18. Emission spectra (uncorrected) of 57 and 58 at different O2 concentrations. Pure
nitrogen (blue) and oxygen (red) and oxygen to nitrogen mole fractions of 0.095, 0.241, and
0.467 (black), from top to bottom.107
A rare example of oxygen gas sensing by a silver compound is demonstrated by a metal
organic framework constructed from the silver-chalcogenolate cluster 59,
(Ag12(StBu)8(CF3COO)4(bpy)4]n.14 The quantum yields of this silver cluster under
vacuum and air are 61% and 12.1%, respectively; the homogeneous crystalline material
has a reproducible KSV of 0.639 kPa-1.
1.4.2 Cu(I) COMPLEXES IN PHOTOCATALYSIS
A photocatalyst is a compound or material that accelerates a photochemical reaction
without itself undergoing a permanent chemical change. The photocatalytic process
requires the use of a specific photosensitizer (PS) which absorbs light energy.
[Ru(bipy)3]2+ was the first complex used as a photosensitizer, in the 1970s.114 A number
of photocatalytic systems involving complexes of noble metals (platinum,115-117
rhenium,118-119 and ruthenium120) have been reported. The development of low-cost metal
PSs has been limited compared to that of noble metals and in this respect Cu(I)-based
photosensitizers offer an attractive alternative.
Generation of H2 gas from water is considered a prospective way to source renewable
energy. A series of Cu(I) complexes, 59–63 (Figure 19), with diphosphine and different
NN ligands, was used as photosensitizers with [Fe3(CO)12] as a water reduction catalyst,
in presence of TEA as a sacrificial reductant. Among the series, photosensitizer 63
showed the best results (TON (turn over number) (Cu) = 804, in the shorter time of 6 h),
which might be due to the bulkier and more robust PP ligand (with a larger bite angle),
which reduces the nonradiative quenching and thus provides a longer lifetime.121
Complex 64 [Cu(dpp)(binc)]BF4 (Figure 19) was successfully used as a photo-redox
catalyst under mild visible-light conditions in atom transfer radical addition and
allylation reactions.122
23
Figure 19. Schematic structures of copper catalyst complexes, 59–64, reported in the literature.
The water reduction process has been significantly enhanced by employing electron
transfer from the [Cu(NN)(PP)] sensitizer, upon visible light excitation, to the water
reduction catalyst [Rh(NN)2Cl2]+, in the presence of an electron donor. The absence of
the Cu(I) photosensitizer completely suppressed hydrogen production and shows the
importance of this component. The comparison of photosensitizers 65 and 65a (Figure
20), which differ in substituents on the biquinoline ligand, shows how careful
modification of the ligand can affect the electronic properties of the complex and
subsequently impact the sensitizing activity.123
Figure 20. Schematic representation of the hydrogen generation reaction.123
24
1.5 AIMS OF THE STUDY
Copper (I) and Ag(I) heteroleptic phosphine complexes have been extensively utilized
as photofunctional molecular materials. Their success has largely been defined by the
tunability of the optical behavior via facile modulation of the ligand environment, which
is often comprised of diphosphine, PP, and diimine, NN, or halide ligands. However,
chelating tri- and tetradentate phosphines have rarely been employed in the preparation
of luminescent coinage metal complexes.124-126 In particular, the joint effect of
polydentate phosphine and pseudo-halide ligands on the emission properties of copper
and silver luminophores has been virtually overlooked prior to this work.
In view of the literature data, the overall goal of my research project was to prepare a
series of photoluminescent copper and silver compounds supported by oligophosphine
ligands. The utilization of different coordinating pseudohalides (cyanide and
thiocyanide) and terminal alkynyl groups was aimed at the study of the effect of the
ancillary ligand on the optical behavior of the resulting compounds. Consequently, the
potentially ambidentate character of the anionic fragments was intended to be utilized
for the construction of di- and trinuclear assemblies.
25
2. EXPERIMENTAL
2.1 PHOSPHINE LIGANDS
The preparation of commercially unavailable tri- and tetradentate phosphine ligands was
carried out by adopting the method published by Hartley et al.42 These reactions are air-
and temperature- sensitive, therefore all solvents were distilled under an inert atmosphere
prior to use. All other reagents, including the diphosphines (Figure 21) were used as
received. All reactions were performed under a nitrogen atmosphere.
Scheme 1. Preparation of the phosphine ligands.
The phosphines were prepared in a two-step process; the first step is common to both tri-
and tetradentate ligands. In accordance with the literature procedure,42 1,2-
dibromobenzene was used as a starting material to obtain intermediate 1-bromo-2-
diphenylphosphinobenzene, which was subsequently lithiated and reacted with Cl2PPh
and PCl3 to afford tri- (P3) and tetradentate (P4) phosphine ligands, respectively (Scheme
1). In addition, commercially available diphosphine ligands (Figure 21) were used to
prepare heteroleptic dinuclear coinage metal complexes.
Figure 21. Diphosphine ligands used in this work.
2.2 SYNTHESIS OF THE METAL COMPLEXES
The copper subgroup metal precursors MX (X = (pseudo)halide type ligand) were treated
with a phosphine ligand to produce mono-, di-, and trinuclear complexes, 1–38 (Table
26
2). The starting terminal di- and tri-alkynes were prepared according to the reported
procedures127-129 using a standard protocol for Sonogashira cross-coupling reactions.
Table 2. The list of compounds 1-38 synthesized in the course of this work.
The listed metal complexes correspond to the following publications
Publication I - 1-3, 30-33
Publication II - 19-23, 34-38
Publication III - 8-13
Publication IV – 4-7, 14-18, 24-29
Publication V - 31a
Mononuclear
1 (P3)Cu(CN)
2 (P3)Ag(CN)
3 (P3)Au(CN)
4 (P3)Cu(SCN)
5 (P3)Ag(SCN)
6 (P4)Cu(SCN)
7 (P4)Ag(SCN)
8 (P3)Cu(Cl)
9 (P3)Ag(Cl)
10 (P3)Cu(Br)
11 (P3)Ag(Br)
12 (P3)Cu(I)
13 (P3)Ag(I)
14 [(P3)Cu{NCS:B(C6F5)3}]
15 [(P3)Ag{NCS:B(C6F5)3}]
16 [(P3S)Cu{NCS:B(C6F5)3}]
17 [(P4)Cu{NCS:B(C6F5)3}]
18 [(P4)Ag{NCS:B(C6F5)3}]
19 (P3)Cu(C2Ph)
20 (P3)Cu(C2-4-OCH3C6H4)
21 (P3)Cu(C2-4- NO2C6H4)
22 (P3)Cu(C2-4- CF3C6H4)
23 (P3)Cu(C2-2-C6H5N)
Dinuclear
24 [Cu(SCN)dppb]2
25 [Cu(SCN)DPEphos]2
26 [Cu(SCN)Xantphos]2
27 [Ag(SCN)dppb]2
28 [Ag(SCN)DPEphos]2
29 [Ag(SCN)Xantphos]2
30 [(P3)Cu(CN)Cu(P3)](CF3SO3)
30a [(P3)Cu(CN)Cu(P3)](BF4)
31 [(P3)Ag(CN)Ag(P3)](BF4)
31a [(P3)Ag(CN)Ag(P3)](tfpb)
32 [(P3)Au(CN)Ag(P3)](CF3SO3)
34 Cu2(P3)2(1,4-C2C6H4C2)
35 Cu2(P3)2(4,4´-C2(C6H4)2C2)
36 Cu2(P3)2(4,4´´-C2(C6H4)3C2)
Trinuclear
33 [{Cu(P3)NC}2Au](CF3SO3)
37 Cu3(P3)3(1,3,5-(C2C6H4)3C6H3)
38 Cu3(P3)3(1,3,5-(C2C6H4C2C6H4)3C6H3)
27
2.3. PURIFICATION AND CHARACTERIZATION
The polyphosphine ligands and their intermediates were purified by column
chromatography and/or recrystallization. The metal complexes were generally
recrystallized via slow evaporation or gas-phase diffusion techniques. The FTIR
measurements were performed on a KBr disc using a Bruker Vertex 70 FTIR instrument.
Structural studies were carried out by single-crystal diffraction analysis; the
corresponding data were collected with a Bruker SMART Apex II, Kappa Apex II, or
Kappa Apex II Duo diffractometer using Mo Kα radiation (λ = 0.71073 Å). The
multinuclear (1H, 31P, 19F) NMR spectroscopic investigations in solution were carried out
on a Bruker Avance 400, 500, or AMX 400 instrument. The electrospray ionization mass
spectra were measured on a Bruker APEX-QeQh-FT-ICR mass spectrometer in positive
ion mode.
Collaborators at the National Taiwan University (Taiwan), Soochow University
(Taiwan), St.-Petersburg State University (Russia), and Aalto University (Finland)
carried out computational and photophysical investigations of the compounds and
materials prepared by the author.
28
3. RESULTS AND DISCUSSION
3.1. MONONUCLEAR TRI- AND TETRAPHOSPHINE d10 COMPLEXES
The development of coinage metal complexes exhibiting efficient luminescence requires
rational molecular design in order to decrease structural flexibility and consequently
suppress geometrical distortions in the excited state that, in turn, block the non-radiative
relaxation pathways. Following the chosen general strategy, a series of copper subgroup
metal complexes was obtained utilizing stereochemically rigid tri- and tetradentate
phosphine ligands, which have previously been sparsely employed in the preparation of
photofunctional d10 compounds.124-125, 130-131
The families of structurally related species [(P3)M(CN)] (M = Cu, Ag, Au; 1–3),
[(P3)M(SCN)] (M = Cu, Ag; 4 and 5), [(P4)M(SCN)] (M = Cu, Ag; 6 and 7),
[(P3)M(Hal)] (Hal = Cl, Br, I; M = Cu, 8, 10, 12; M = Ag 9, 11, 13) were obtained and
investigated (Scheme 2). Furthermore, the boronated thiocyanate derivates
[(P3)M{SCN:B(C6F5)3}] (M = Cu, Ag; 14 and 15), [(P3S)Cu{SCN:B(C6F5)3}] (16),
[(P4M{SCN:B(C6F5)3}] (M = Cu, Ag; 17 and 18) and the alkynyl compounds
[(P3)Cu(C2R)] (19–23) [R=Ph 19, 4-OCH3-C6H4 20, 4-NO2-C6H4 21, 4-CF3-C6H4 22, 2-
NC6H5 23) were synthesized. By means of variation of the metal centers (Cu, Ag, Au)
and of the auxiliary halide/pseudo-halide ligands, it was possible to study their influence
on the formation and structural and photophysical characteristics of the target complexes.
Scheme 2. Preparation of the mononuclear, neutral complexes 1–23.
29
3.1.1 TRIPHOSPHINE CYANIDE COMPLEXES
Neutral tetracoordinate complexes of the general formula [(P3)M(CN)] (M = Cu 1, Ag 2,
Au 3) were conventionally synthesized by reacting the P3 ligand with an equimolar
quantity of the metal cyanide MCN (M = Cu, Ag, or Au) at ambient temperature (Scheme
2). The products were isolated as crystalline materials in good yields. Complexes 1–3
crystallized in the P21/n space group and afforded isomorphous crystals with nearly
identical unit cell dimensions. Selected structural parameters are listed in Table 3 and
indicate that the main deviations of the bond distances and angles are associated with the
different sizes and coordination preferences of the metal centers.
Table 3. Selected bond lengths and angles for complexes 1–3.
1 (M = Cu) 2 (M = Ag) 3 (M = Au)
Bond lengths, Å
P(1)-M(1) 2.294(4) 2.527(3) 2.401(4)
P(2)-M(1) 2.272(5) 2.516(4) 2.409(5)
P(3)-M(1) 2.289(5) 2.484(4) 2.413(5)
C(1)-M(1) 1.937(2) 2.123(1) 2.064(2)
Bond angles, deg
N(1)-C(1)-M(1) 178.0(2) 173.4(1) 175.6(2)
C(1)-M(1)-P(1) 120.04(5) 118.37(3) 118.80(5)
C(1)-M(1)-P(2) 123.05(5) 128.16(4) 128.84(5)
C(1)-M(1)-P(3) 117.42(5) 126.41(3) 119.30(5)
P(1)-M(1)-P(3) 114.04(2) 108.89(1) 112.91(2)
P(2)-M(1)-P(3) 87.35(2) 81.81(1) 84.20(2)
P(2)-M(1)-P(1) 87.14(2) 80.32(1) 84.44(2)
Figure 22. Crystal structures of complexes 1–3.
Unsurprisingly, the larger van der Waals radius for Ag compared to those of Cu and Au
metals results in systematically longer M–CN and M–P bond distances for the silver
complex, 2. The central metal ions in compounds 1–3 adopt pseudo-tetrahedral geometry
in the ligand sphere (Figure 22), which is composed of the phosphine coordinated in a
30
tridentate mode, and of the carbon-bound cyanide group. The P–M separations in 1
somewhat exceed those reported for other tetracoordinated Cu complexes.132 Structural
parameters of compounds 2 and 3 are very close to the values found for their chloride
congeners M(P3)Cl.124 Furthermore, the M–CN contacts in these species are comparable
to those of previously characterized coinage metal complexes.132-133
The C≡N stretching frequencies in the IR spectra of compounds 1–3 revealed
characteristic strong bands at 2108, 2116 and 2112 cm-1, respectively; these values are
similar to those of previously reported cyanide compounds.132 The solution behavior of
1–3 was studied by NMR spectroscopy; the corresponding data are in good agreement
with the solid-state structures. The 1H and 1H-1H COSY spectra of these compounds
demonstrate well-resolved patterns generated by the aromatic protons of the phosphine
ligands (Figure 23).
Figure 23. (Top) the 31P{1H} NMR spectra of 1–3, CD2Cl2, 298 K. (Bottom) the 400 MHz 1H-1H COSY NMR spectrum of 1, CD2Cl2, 298 K (assignment of the rings A and B is arbitrary).
The 31P{1H} NMR spectra of complexes 1 and 3 illustrate splitting patterns typical for
the A2B spin system. In contrast, the silver congener, 2, shows two resonances, the
31
multiplicity of which is compatible with the first-order A2X system of 31P atoms,
additionally split by coupling with Ag nuclei (the isotopomers with 107,109Ag atoms
remain unresolved, Figure 23).
3.1.2 TRI- AND TETRAPHOSPHINE THIOCYANATE COMPLEXES
Mononuclear compounds 4–7 [(P3/P4)M(SCN)] [P3 (M = Cu 4, Ag 5), P4 (M = Cu 6, Ag
7)] were prepared by complexation of metal thiocyanates, MSCN, with phosphine
ligands P3/P4, using dichloromethane as a solvent, at ambient temperature (Scheme 2).
The IR spectra of these compounds exhibit characteristic C≡N vibrations in the range of
2080 to 2097 cm-1; these values are in line with those of similar, previously reported
species.134-135 The silver complexes (5 and 7) have higher C≡N stretching frequencies
than the copper (4 and 6) analogues, which could be attributed to the different bonding
modes of the ambidentate SCN ligand in these compounds.
Figure 24. Crystal structures showing molecular views of 5, 6, 7a, and 7n.
In the Ag complexes, the thiocyanate group is predominantly attached to the metal center
through the S atom, which leads to a bent Ag–SCN motif, similar to the reported
complexes,14, 16-17 as confirmed by X-ray crystallographic analysis. In contrast, a linear
Cu–NCS arrangement is observed for 4 and 6 (Figure 24). The central metal atoms in
these compounds are supported by three phosphorous atoms from the P3/P4 ligands and
the fourth coordination site is occupied by the terminal SCN ion, resulting in a distorted
tetrahedral shape. In complexes 6 and 7, containing the P4 ligand, one of the terminal
PPh2 groups is not bound to the metal (Cu/Ag) ions.
The tetraphosphine complexes adopt multiple forms depending on the solvents used for
crystallization. Thus, in addition to the yellow-green diethyl ether solvate 6, this
compound was obtained as a yellow solvate 6a (containing highly disordered solvent),
32
and a solvent-free yellow-orange minor form derivative, 6b. The silver analog, 7,
crystallizes in two solvent free forms (minor, poorly reproducible, pale green 7 and
yellow 7a; pseudo-polymorphs) and as two solvates (THF and methanol containing 7b
and 7c, respectively). Furthermore, a linkage isomer with N-bonded thiocyanate (7n) has
been isolated (Figure 24). It is noteworthy that coinage metal complexes with the P4
ligand remain scarce.136-137
The bond distances between the metal and phosphorous atoms are similar to those of
[M(P3)CN] congeners 1–3 and their close relatives in the [M(P3)Cl] series.124 The
separations between the free PPh2 groups and the metal centers are 4.101 Å (M = Cu, 6)
and 3.848 Å (Ag, 7), which are similar to those in their alkynyl congeners.136 The Ag–S
bond length (2.49–2.50 Å) is comparable to the values reported for other mono134 and
dinuclear138-139 complexes.
In the 31P NMR spectra recorded in solution, broad peaks were observed for the Cu(I)
complexes, 4 and 6, at 193 K. In contrast, Ag(I) complexes, 5 and 7, demonstrate well-
resolved patterns corresponding to the AX2 and AX3 spin systems and further splitting
due to the P–Ag magnetic interactions (1JP-107Ag = 179 and 112 Hz, 1JP-109Ag = 203 and 129
Hz, Figure 25). The high symmetry of the tetraphosphine coordination in 7, observed in
solution even at low temperature, suggests the dissociation of the SCN anion to produce
a [Ag(P4)]+ cation. This hypothesis is also in line with the crystallization of two linkage
isomers of this complex. The proton NMR spectra for 4–7 are consistent with the 31P data
and support the symmetric arrangement of the phosphine ligands around the metal ion.
Figure 25. Experimental (top, 193 K, CD2Cl2) and simulated (bottom) 400 MHz 31P{1H} NMR
spectra of 7.
3.1.3 TRIPHOSPHINE HALIDE COMPLEXES
In order to compare the photophysical properties of [M(P3)X] compounds with different
X type ligands, the corresponding copper and silver halide derivatives were synthesized.
The coordination of triphosphine ligand P3 to the CuX halide salts readily leads to
mononuclear complexes [Cu(P3)X] (X = Cl 8, Br 10, I 12) in high yields. The [Ag(P3)X]
complexes (X = Cl 9, Br 11, I 13) can be conveniently prepared by treating AgPF6 with
NBu4X, followed by P3 ligand (Scheme 2). The compounds (8, 9, 11, and 13) had
33
previously been reported for electroluminescence applications.125-126 Among them, the
crystal structure of 9 had previously been described.124
Figure 26. Crystal structures of complexes 8 and 11.
The single crystal structures of compounds 8, 10, 11, and 13 have molecular skeletons
and M–P bond distances which are close to those for the reported structure of 9 as well
as to those of the cyanide (1 and 2) and thiocyanate (4 and 5) congeners (Figure 26).
Similar to the pseudohalide derivatives, the central metal ions in complexes 8, 10, 11,
and 13 adopt a tetrahedral arrangement with the chelating tridentate phosphine P3 and the
halide ligands. As expected, the M–X bond distance increases with the size of the
ancillary halogens (Cu–Cl 2.2748 Å, Cu–Br 2.3986 Å; Ag–Br 2.57221 Å, Ag–I 2.7050
Å).
The solution 1H, 1H-1H COSY and 31P NMR spectra for the halide complexes are
consistent with the solid-state structures. In particular, the 31P NMR data confirm that all
the phosphorus atoms are coordinated to the metal ions; the resonances of compounds 8–
13 are moderately shifted to higher field compared to those of the cyanides [M(P3)CN]
(1 and 2), which may reflect the effect of the ancillary X ligand on the electronic features
of the metal center.
3.1.4 TRI- AND TETRAPHOSPHINE ISOTHIOCYANATOBORATE
COMPLEXES
The ambidentate nature of the terminal SCN groups was utilized to initiate an additional
donor-acceptor interaction with the Lewis acid B(C6F5)3 in order to produce
isothiocyanatoborate complexes [(P3/P4)M{NCS:B(C6F5)3}] [P3 (M = Cu 14, Ag 15), P4
(M = Cu 17, Ag 18)] (Scheme 2), which were isolated as crystalline materials in high
yields. These compounds are formed upon the reaction of neutral compounds 4–7 with
B(C6F5)3, in an equimolar ratio, in dry THF, under a nitrogen atmosphere. In all these
species the SCN:B(C6F5)3 ligand is S-bound to the metal centers, thus forming bent M–
SCN fragments even though a linear Cu–NCS skeleton is found in the parent complexes
4 and 6. This rearrangement can be explained in terms of hard-soft acid-base theory. The
hard B(C6F5)3 acid shows a clear preference for binding to a hard donor, which is the N
atom in the ambidentate SCN ligand; thus, the copper and silver metal ions invariably
bind to the sulfur functions, leading to bent M–SCN products.
34
Remarkably, the crystallization of compound 14 from an acetone/diethyl ether mixture
results in the formation of derivative 16, [(P3S)Cu{NCS:B(C6F5)3}], in which the P3
ligand has one sulfidated PPh2 group, evidently due to decomposition of thiocyanate
(Figure 27). It is important to note that this is the first example of a hetero-tridentate
diphosphine-phosphine sulfide ligand (PPP=S).
Figure 27. Crystal structures of complexes 16 and 17.
The X-ray structural analysis of isothiocyantoborate complexes, 16–18, confirmed the S-
coordination of the thiocyanate to the metal atoms and N-bonding to the boron. The
distorted tetrahedral environment of copper and silver ions is completed by P3/P4 ligands.
The linear arrangement of SCN:B motifs and the corresponding structural parameters for
14–18 are comparable to those of the published compound [K(18-crown-
6)][SCN:BR3].140 Due to the B-NCS interaction, the C≡N bond distances in 16–18
(1.136–1.152 Å) are shorter than in the parent compounds 4–7 (1.152–1.160 Å); this
structural observation is consistent with the changes in C≡N stretching frequencies,
which are significantly increased in 16–18 (2189–2181 cm-1) with respect to 4–7 (2080–
2097 cm-1) and which are similar to the values reported for cyano-boronated
complexes.141-142
In 16, the pseudo-tetrahedral geometry is achieved by coordinating two of the P-donor
atoms of the heterodentate P3S ligand and the two sulfur atoms from P3S and the
SCN:BR3 ion (Figure 28). Despite the anionic nature of the latter, the S–Cu distance
involving the PPh2=S group (2.304 Å), is slightly shorter than that with the SCN:
B(C6F5)3 function (2.346 Å); both values agree with the reported data for copper
thiocyanate47, 143-144 and phosphine sulfide145-147 compounds.
The attachment of the B(C6F5)3 group causes a shift in the 31P NMR signals for the
isothiocyanatoborate complexes compared to the those of the parent complexes, which
confirms the formation of products 14–18. The silver compounds 15 and 18 produce 31P
spectroscopic profiles corresponding to the A2B and A3X spin systems, respectively,
which are similar to those of the parent complexes 5 and 7 (Figure 28).
35
Figure 28. The 31P NMR spectrum of 16 at 298 K (top); the 31P NMR spectrum of 18 at 210 K,
400 MHz (black) and its simulation (red), assuming the AX3 spin system (bottom).
The copper isocyanotoborate complex, 14, showed two broad signals (2:1 ratio) in the 31P NMR spectrum at 298 K, whereas 17 displayed one resonance, at room temperature,
and proved to be less rigid than its precursor, 6. The 31P NMR spectrum of compound 16
is consistent with its solid-state structure and displayed three doublets with a 1:1:1 ratio
of their relative intensities; the low field signal evidently originates from the Ph2P=S
group (Figure 28). Additionally, a characteristic set of resonances with a 2:2:1 ratio,
corresponding to the ortho-, meta-, and para-F atoms, was observed in the 19F NMR
spectra of isothiocyanatoborate complexes.
3.1.5 TRIPHOSPHINE ALKYNE COMPLEXES
Neutral alkyne coinage metal complexes of the general formula [CuP3(C2R)] (19–23) [R
= Ph 19, 4-OCH3-C6H4 20, 4-NO2-C6H4 21, 4-CF3-C6H4 22, 2-NC6H5 23) were
synthesized by the reaction of a stoichiometric amount of [Cu(P3)]+ cationic precursor
prepared in situ and an alkyne, in the presence of a base (Scheme 2). The products were
obtained as yellow solids, which are somewhat unstable in chlorinated solvents.
A nearly identical set of multiplets appeared in the 31P NMR spectra of compounds 19–
23, which is assigned to an A2B spin system. The downfield shift of the resonances
relative to those of the free ligand confirms that all three phosphorus atoms of the P3
ligand are coordinated to the metal ion. The similarity of the 31P NMR chemical shifts
within this series indicates that the electronic properties of the alkynyl groups have a
small influence on the copper, and consequently the P atoms. The complete assignment
36
of the 1H NMR spectra for 19–23 is in line with the composition [CuP3(C2R)] and the
symmetrical structural arrangement of these complexes in solution.
Figure 29. Crystal structures of complexes 19, 21, and 23.
The structural characterization of compounds 19, 21, and 23 (Figure 29) proved the
tridentate character of the triphosphine coordination to the copper center, accompanied
by the terminal alkynyl group, thus providing pseudo tetrahedral ligand arrangement,
with observed M–P and M–C≡C distances which were quite similar to those of the
reported congener complexes.131, 148-149 It is important to note that these compounds were
the first monomeric alkynyl complexes of Cu(I), which typically aggregate via a σ–π
bridging mode of the –C≡CR groups.130, 149-152
3.2 PHOTOPHYSICAL PROPERTIES OF MONONUCLEAR COMPLEXES
The photophysical investigations of complexes 1–23 focused on their solid-state
behavior, due to the weak or even negligible luminescence of these species in solution;
where measurements were performed for selected compounds only (1–3, 7, 14–15, 17–
18).
3.2.1 [Cu(P3)X] HALIDES AND PSEUDOHALIDES
Table 4 summarizes the photophysical data for mononuclear triphosphine copper
compounds in the solid state at 298 K and 77 K. Compounds 1 and 4 show strong green
emission with high quantum yields of 70% and 57%, respectively. From quantum
chemical calculations, the lowest excited state for compound 1 corresponds to MLCT
(metal-to-ligand charge transfer, L = triphosphine ligand) along with ligand-to-ligand
CN → P3 charge transfer (Figure 30), whereas for compound 4, mainly L´LCT transitions
(L´ = SCN), with some MLCT character, were predicted. Among the mononuclear Cu(I)
complexes, 1 shows the highest quantum yield and the longest observed lifetime (τ = 15
μs at 298 K) compared to those of other reported Cu(I) complexes.58, 76, 153 In contrast, 4
has the shortest lifetime, at 5 μs, at room temperature, in comparison with those of
[Cu(P3)X] (X = Cl 8, Br 10, I 12, and CN 1, Table 4). Furthermore, there was a drastic
change in the lifetime of 4 (694 μs) when frozen at 77 K. The dependence of lifetime on
temperature for 4 (Figure 30) confirms the presence of TADF, which implies that
37
different excited states are responsible for the emission at low (T1) and ambient (S1)
temperatures.
The addition of the B(C6F5)3 group to 4, which converts it into 14, results in a slight blue
shift of the emission wavelength from 520 nm to 505 nm (Δν = 571 cm-1) with respect to
that of the parent compound, 4. The S1 and T1 excited states of 14 are assigned as
(L+M)LCT type (L = phosphine) with a less than 2% contribution from the SCN:
B(C6F5)3 ligand, which is different from the transitions found for 4. The gradual increase
in the lifetime upon cooling (174 fold) suggests TADF properties (Figure 30). It is
noteworthy that the longest lifetime (3067 μs) among the reported compounds is
observed for 14 at 77 K.
Figure 30. Electron density difference plots for the lowest energy triplet emission (T1 → S0) of
the Cu(I) complex, 1 (left). During the electronic transition, the electron density increases in the
blue areas and decreases in the red areas. Temperature dependencies of the average decay times
of 4 and 14 (right).
Strong blue-green emissions with maxima between 504 and 517 nm were observed for
halide derivatives 8, 10, and 12; these bands are slightly blue-shifted relative to those of
the pseudohalide congeners, 1 and 4. Among the halide series (8, 10, and 12), the
emission energy increases from [Cu(P3)Cl] (517 nm) to [Cu(P3)I] (504 nm). In the same
order, the room temperature quantum yields (21–37%) show substantial growth (Table
4). The drastic increase (up to 66 fold) in the decay time at low temperature, together
with the bathochromic shift, indicate that these compounds demonstrate delayed
fluorescence behavior.99, 154 The emission of these compounds originated mainly from a
MXLCT type excited state.
The series of compounds, 19–23, bearing terminal alkynyl ligands, revealed a significant
red-shift of the emission maxima, up to 722 nm (21) (Table 4 and Figure 31). However,
quantum yields for those complexes were substantially lower compared to those of the
halides (8, 10, and 12) and pseudohalides (1 and 4). The triplet excited state of
compounds 19–23 was largely determined by the alkynyl ligands, with a small
contribution from the metal ions, i.e. they can be classified as having intra-ligand origin
mixed with some MLCT character (Figure 31). The T1 state in this case is different from
those for of the pseudohalide derivatives, 1 and 4, in which MLCT and a mixture of
38
MLCT+L´LCT transitions make major contributions, according to quantum mechanical
calculations.
Table 4 The photophysical properties of neutral mononuclear copper complexes 1, 4, 8, 10, 12,
14, and 19–23, at 298 and 77 K, in the solid state.
298K 77K
No Ancillary
ligands
λex,
nm
λem,
nm
Ф,
%
τav,a
μs
λex,
nm
λem,
nm
τobs,a
μs
1 CN 415 530 70 15
4 SCN 295,367 520 57 5 370 520 694
8 Cl 370 517 21 9 363, 397 520 566
10 Br 370 507 36 12 363, 397 523 794
12 I 370 504 37 11 311 512 137
14 NCS:
B(C6F5)3 316, 365 505 39 18 323, 364 515 3067
19 415 602 6 2 415 612 246a
20 415 602 8 2 415 612 73a
21 580 722 0.1 - 415 717 -
22 340, 415 573 11 3 370 579 59a
23 415 573 19 4 415 579 149a a The average emission lifetime for the two exponential decay was calculated using τav = (A1τ12 +
A2τ22)/(A1τ1 + A2τ2); Ai = weight of the i exponent.
Similar to halide compounds 8, 10, and 12, complexes 19–23 are likely to exhibit TADF
properties, which is indicated by the lifetime values measured at 298 K and 77 K. Upon
cooling, the lifetime increased up to 130-fold compared to its magnitude at room
temperature (Table 4).
Figure 31. a) Electron density difference plots for the lowest energy triplet emission (T1 → S0)
of the Cu(I) complex, 19, (isovalue 0.002 a.u.). During the electronic transition, the electron
density increases in the blue areas and decreases in the red areas. b) Normalized solid-state
excitation (left) and emission (right) spectra of 19 and 23 at 298 K (dashed line) and 77 K (solid
line).
39
3.2.2 [Ag(P3)X] HALIDES, PSEUDOHALIDES AND [Au(P3)CN]
Intense green emission maximized at 525 nm with 87% quantum yield is observed for
silver compound 2, which has the longest observed lifetime (29 µs) and highest quantum
yield at room temperature among the mononuclear series (Tables 4 and 5). Gold
compound 3 shows red-shifted luminescence (λem = 640 nm) and a lower quantum yield
of 8%, which is different from the performance of 1 and 2 (Figure 32). Notably, the
ancillary ligand in 3 has a significant influence on the emission intensity, as [Au(P3)I]155
emits at the same wavelength as 3 but with 4-times greater intensity (λem = 640 nm and
Ф = 35%). A similar trend in emission colors was reported for M(PP)(PS) (M = Cu, Ag
and Au) [PP = (1,2-bis(diphenylphosphino)benzene; PS = 2-diphenylphosphine
benzenethiolate] complexes.153
Table 5 The photophysical properties of neutral mononuclear silver complexes 2, 3, 5, 9, 11, 13,
and 15, at 298 K and 77 K, in the solid state.
298K 77K
No Ancillary
ligands
λex,
nm
λem,
nm
Ф,
%
τav, a
μs
λex,
nm
λem,
nm
τobs, a
μs
2 CN 400 525 87 29
3 CN 459 640 8 1
5 SCN 320, 365 538 32 15 314, 365 548 1121
9 Cl 347, 441 521 40 27 329, 375 535 596
11 Br 393 521 41 26 329, 375 535 538
13 I 312, 483 513 39 14 329, 375 525 180
15 NCS:
B(C6F5)3 356 482 12 23 350 478 1480
a The average emission lifetime for the two exponential decay was calculated using τav = (A1τ12 +
A2τ22)/(A1τ1 + A2τ2); Ai = weight of the i exponent.
Figure 32. Normalized solid-state excitation (solid line) and emission (solid line with symbol)
spectra of 1–3 at 298 K. λex = 406 nm for emission(left). Temperature dependencies of the
average decay times of 5 and 15 (right).
It is noteworthy that the emission spectra of complexes 1–3 were measured in solution
(degassed dichloromethane, 298 K). Compounds 1 and 2 show red-shifted emission at
665 nm and 675 nm, with low quantum yields of 7×10-4 and 8×10-4%, respectively, while
3 is virtually nonemissive. This is typically attributed to the geometrical distortion
40
(planarization) of the excited state geometry, which can then undergo non-radiative
relaxation.97, 156-157
A slight red shift in the emission wavelength is observed for silver thiocyanate, 5, (538
nm) compared with that of its cyanide relative, 2 (525 nm, Δν = 460 cm-1, Table 4), which
is opposite to the behavior observed for the copper analogues (for which a blue shift is
detected). Introducing the borane group, B(C6F5)3, into 5 shifts the emission of resulting
compound 15 by approximately 56 nm (Δν = 2160 cm-1) towards the blue region, to 482
nm. Similar to the Cu (I) thiocyanate pair, 4 and 14, in the case of Ag(I) congeners, 5 and
15, a lower quantum yield (5 = 32%, 15 = 12%, Table 5) and an increase in the lifetimes
(at 298 K and 77 K) were observed for the boronated compound. Computational analysis
indicates that the lowest excited states correspond to a mixture of L’LCT (SCN → P3),
with some MLCT character, in 5; however, (L+M)LCT transitions are predicted to
control the excitation of 15. Temperature-dependent analysis of the decay time clearly
demonstrated the TADF phenomenon in 5 and 15 (ΔE = 838 and 1608 cm-1, respectively,
Figure 32). The boronated complex, 15, showed a longer phosphorescent decay time
τ(T1) = 1466 µs compared to parent compound 5 (1117 µs) tentatively assigned to the
differences in the electronic structures (Figure 33).
Figure 33. The appearance of the highest occupied molecular orbitals in the singlet ground
states (S0) and the first excited states (T1) of 5 and 15.
The emission wavelengths for silver halide derivatives 9, 11, and 13 are observed
between 513 and 521 nm, which are slightly red-shifted relative to the Cu(I) compounds
8, 10, and 12. Quantum yields of the silver halide compounds (9, 11, and 13) fall in the
range of 38–40%, which are higher than those of the copper analogues, however, they
are lower than that of the cyanide complex, 2. The emission of these compounds was
ascribed to MXLCT type. The room temperature lifetimes (14–27 µs) of silver halide
41
derivatives 9, 11, and 13 are significantly increased upon cooling (77 K), which suggests
TADF behavior (Tables 4 and 5).
3.2.3 [M(P4)X] THIOCYANATE AND ISOTHIOCYANATOBORATE
COMPLEXES
The pertinent photophysical data for mononuclear tri and tetraphosphine Cu(I) (6 and 17)
and Ag(I) (7 and 18) compounds at 298 K and 77 K are listed in Table 6. Complex 16
did not show appreciable emission and was therefore not investigated.
Table 6 The photophysical properties of homometallic complexes 6, 6a, 7, 7a, 7c, 7n, 17, 17a,
and 18, at 298 K and 77 K, in the solid state.
a The average emission lifetime for the two exponential decay was calculated using τav = (A1τ12 +
A2τ22)/(A1τ1 + A2τ2); Ai = weight of the i exponent.
Figure 34. a) Normalized solid-state excitation and emission spectra at 298 K (dotted) and 77 K
(solid) of 7a–c, 7n (inset picture shows appearance of 7a–c, 7n under UV light at 298 K). b)
Normalized solid-state emission spectra at 298 K of 17 and 17a (inset picture shows appearance
of 17 and 17a under UV light at 298 K).
298K 77K
No λex,
nm λem,
nm Ф,
% τav, a
μs λex,
nm λem,
nm
τobs, a
μs
6 360 543 27 5 360 552 1387
6a 400 575 23 4 396 575 1045
7a 367 552 27 10 367 507 747
7c 368 630 19 7 365 645 890
7n 366 525 44 10 365 518 598
17 395 505 17 2 380 500 1984
17a 370 625 11 4 370 666 1276
18 310, 365 575 9 8 375 630 1018
42
As mentioned in Section 3.1.2, compounds 6 and 7 [Cu/AgNCS(P4)] crystallized in
different pseudopolymorphs; the optical properties were studied for two solvates, 6 and
6a, and for three forms of 7 (solvates 7 and 7c, solvent free 7a, and the linkage isomer
7n). For the THF solvate, 7b, only the emission spectra were recorded due to the presence
of at least two crystalline forms. Compared to that of triphosphine complex 4 (λem = 520
nm, Ф = 56%), significant red shifts in the emissions were observed for the solvated
forms 6 and 6a (λ = 543 and 573 nm, Δν = 814 and 1779 cm-1, respectively) and quantum
yields for the tetraphosphine species were lower, at 27% and 23%. The emissions of the
different crystalline forms of compound 7 cover a wide range of the visible spectrum
(Figure 34a). The emission maxima of solvent-free forms 7n and 7a were observed in
the green to yellow region (λem = 525 and 552 nm, respectively). In contrast, a
bathochromic shift was observed for the THF solvate 7b (605 nm) and the emission
maximum reached 630 nm for methanol solvate 7c (Table 6).
Substantially blue-shifted emissions were observed for borane-containing complexes 17
and 18 in comparison to those of parent compounds 6 and 7 (solvated form). Two
crystalline forms of 17 emit at the dramatically different wavelengths of 505 nm and 625
nm (Figure 34b), similar to materials 6 and 6a. Complex 18, obtained in one form,
exhibits an emission band at 575 nm. The presence of the B(C6F5)3 group in 17 and 18
affects the quantum yields (9–17%), which are smaller than those of 6, 6a, 7, and 7a
(Table 6). Furthermore, grinding compound 7 produces a uniform material with yellow-
orange luminescence, which is converted into a solid with strong green luminescence
upon addition of acetonitrile (Figure 35a).
Figure 35. Changes in the emission spectra of 7 upon grinding (dotted orange line) and upon the
addition of acetonitrile (solid green line) (left). Temperature dependencies of the average decay
times for compounds 7, 7a, 15, and 18 (right).
Similar to the case in triphosphine complexes, a mixture of MLCT (d → P4) and L´LCT
(SCN → P4) transitions contribute to the excited state for compound 6–7. For compound
6, the temperature dependence of the decay time increased continuously at 77 K and
therefore could not be treated using the two-state model. However, it is consistent with
the TADF character of the emission, pointing to a low energy difference (less than 500
cm-1) between the S1 and T1 levels. In the case of 7, the profile of the dependence of
43
lifetime on temperature clearly shows the TADF behavior of this luminophore (Figure
35b).
The composition of the excited states for complexes 17 and 18 is principally of
(L+M)LCT (d,p(M,P)→πP4) character with a small involvement of the SCN:B(C6F5)3
ligand, which is in contrast with those of the respective precursor compounds, 6 and 7.
One specific trend is perceived for boronated compounds 17 and 18, which exhibit
systematically longer lifetimes at 77 K. The TADF behavior of 17 and 18 was confirmed
by variable temperature studies of their lifetimes (Figure 35b).
The luminescence of compounds 7, 17, and 18 was also measured in degassed THF
solution. Remarkably, the emission bands are observed in the red region, ranging from
620 to 690 nm with 0.9–2.4% quantum yields. The lowered quantum yields are
presumably due to structural distortions occurring in the excited state, which lead to non-
radiative deactivation.101 Among the investigated compounds, compound 7 exhibits the
longest emission wavelength, 690 nm at 298 K, with a quantum efficiency of 2.1%.
3.3 DINUCLEAR BI- AND TRIPHOSPHINE d10 COMPLEXES
The ambidentate nature of thiocyanate and cyanide pseudohalides allowed the
preparation of a series of bimetallic complexes, which is comprised of neutral compounds
[M(SCN)P2]2 (dppb, DPEphos, Xantphos, M = Cu 24–26; M = Ag 27–29) and ionic
species [(MP3)CN(P3M)]+ (M = Cu 30; Ag 31; Au, Ag 32). Hetero-trinuclear complex
[(P3)Cu-NC-Au-CN-Cu(P3)]+ 33 was also synthesized to extend this approach, where the
pseudo-halides act as bridges between the two metal centers. Alternatively, neutral
copper compounds were obtained using di- and tri alkynyl spacers along with P3 ligand;
the number of terminal alkyne groups determines the complex nuclearity affording linear
[{(P3)CuC2}2R)] (R = -(C6H4)-n; n = 1 34, n = 2 35, n = 3 36) and star shaped
[{(P3)CuC2}3R)] (R= 1,3,5-(C6H4)3-C6H3 37, 1,3,5-(C6H4-4-C2C6H4)3-C6H3 38)
complexes.
3.3.1 THIOCYANATE-BRIDGED DINUCLEAR COMPLEXES
The bidentate P2 ligands (Figure 21) were reacted with copper and silver thiocyanates
according to the reported protocol139, 158 to generate neutral homo-bimetallic complexes
with the molecular formula [M(SCN)P2]2 (M = Cu, P2 = dppb 24, DPEphos 25, Xantphos
26; M = Ag, P2 = dppb 27, DPEphos 28, Xantphos 29) in moderate to high yields of 50–
88% (Scheme 3). The Cu complexes 24–26 were obtained as yellow crystals, with lower
yields compared to the Ag analogues 27–29, due to the formation of insoluble
unidentified side products.
The C≡N stretching vibrations of 24–29 were observed at frequencies between 2088 and
2108 cm-1 as sharp peaks (Figure 36) and these values were consistent with those of the
previously synthesized thiocyanate Ag(I) and Cu(I) compounds.139, 158 Generally,
according to Nakamoto theory,159 the wavenumber of C≡N stretches for SCN bridges
falls above 2100 cm-1. However, many complexes have been reported which do not obey
44
this theory.47, 160 Except for those of 24, the IR data for complexes 25–29 were not in the
Nakamoto range but were similar to those of other reported thiocyanate bridged
complexes.161-162 The 31P NMR spectra of copper compounds 24–26 show broad singlet
peaks, evidently due to structural flexibility of the complexes in solution. In the case of
Ag(I) compounds 27 and 28, sharp doublets were observed due to the silver-phosphorous
magnetic interactions, with coupling constants, JP-107Ag/109Ag, of 366 and 374 Hz. These
values are comparable with those of published compounds.160, 163
Figure 36. Solid state infrared spectra of compounds 24–29.
Scheme 3. Preparation of the di- and trimetallic complexes.
To evaluate the structural arrangements, the X-ray single crystallographic analysis was
carried out for compounds 24–29 (Figure 37). The dinuclear complexes 24–27, and 29
formed 8-membered rings composed of thiocyanate anions coordinated in µ2,κ2-mode
and metal ions. The metal centers adopted distorted tetrahedral geometries and the
phosphines were found in trans-positions in the centrosymmetric molecules (except 26);
a similar framework was observed in previously reported Cu(I) and Ag(I) dinuclear
45
complexes.139, 160-161, 164-165 In 26, probably as a result of the steric properties of Xantphos
and repulsion between the phenyl rings, there was a decrease in the molecular symmetry,
resulting in a cis-disposition of the phosphines. Disparately, compound 28 consists of a
4-membered ring formed by two metals and two SCN anions, bound in μ2,k1-mode
through the S atoms; Nicola et al. reported an analogous framework for AgSCN:dpph
(1:1)2 (dpph = Ph2P(CH2)5PPh2) and AgSCN:dppf (1:1)2 (dppf =
bis(diphenylphosphino)ferrocene) complexes.135, 166
Among these compounds, the M–S bond distances are longer in the Ag(I) than in the
Cu(I) species; the longest one is 2.6817(9) Å, which was observed in 27, and the shortest
is 2.3630(9) Å in 24. The CN bond distances (1.153(4)–1.164(2) Å) were comparable to
those in cyanide complexes 1–3, which confirms that the C-N motif is of multiple order
(Figure 37).
Figure 37. Crystal structures of complexes 26–28.
3.3.2 CYANIDE-BRIDGED DI AND TRINUCLEAR COMPLEXES
The cyanide ligand was used to form bridged metal compounds with higher nuclearities.
Monometallic compounds with free terminal cyanide functions were used to build
dinuclear homo-bimetallic coinage metal compounds [(MP3)CN(P3M)]+X- (M = Cu; X
= -CF3SO3 30, BF4 30a) (M = Ag; X- = BF4 31, B[C6H3(CF3)2]4 31a). These compounds
were constructed by reacting equimolar amounts of mononuclear compounds 1–3 with
corresponding metal salts at ambient temperature, using dichloromethane as a solvent.
In general, attempts to produce heteronuclear compounds were unsuccessful, only for
the combination of Au(I) and Ag(I) was the complex [(AuP3)CN(P3Ag)]+ (32)
synthesized. Furthermore, the hetero-trimetallic compound [(P3)Cu-NC-Au-CN-
Cu(P3)]+ 33 was obtained in good yield by treating the [Cu(P3)]+ ion, generated in situ
from P3 and [Cu(NCMe)4]+, with K[Au(CN)2] (Scheme 3).
Intense IR vibrational bands observed between 2126 and 2172 cm-1 in the spectra of
compounds 30–33 confirm the presence of cyanide C≡N groups. The stretching
46
frequencies of the bridging cyanides C≡N display higher wavenumbers than the terminal
ones in 1–3 (2108–2116 cm-1). The C≡N stretch of 33 at 2172 cm-1, clearly indicates the
coordination of the Au[CN]2 motif to the Cu metal ions. These IR frequencies were in
good agreement with those of reported cyanide compounds.166-168
X-ray crystallographic analysis was performed to characterize compounds 30 and 31.
Unfortunately, 32 and 33 did not produce crystals suitable for X-ray measurements. In
compounds 30 and 31, two MP3 moieties were connected through the CN linker resulting
in a linear arrangement. The coordination geometries of the metal centers in 30 and 31
were generally similar to their precursor compounds, 1 and 2, respectively. No
significant differences were observed between the MP3 fragments in 1 and in bimetallic
complex 30. In the case of dinuclear Ag(I) compound 31, the central Ag–P bond is
significantly longer than the terminal ones and the corresponding bond in the
mononuclear complex, 2. In structures 30 and 31, the counterions behave as bridges
connecting the neighboring cationic units through a system of hydrogen bonds (Figure
38).
Figure 38. Molecular view of complex 31 with BF4– counter ions.
In the 31P NMR spectrum of the dinuclear Cu(I) compound in solution, two different sets
of signals were observed. This is possibly due to the unequal electronic properties of the
C and N atoms of the cyanide ligand, which affect the shielding of the phosphorus nuclei
and differentiate the Cu(P3)-C and Cu(P3)–N moieties (Figure 39). In contrast, the 31P
NMR spectrum of the dinuclear Ag(I) complex is an example of a single A2B spin system
with a well resolved splitting pattern due to the presence of the two silver isotopes, 107Ag
and 109Ag, with characteristic coupling constant values J(PB–107Ag) 245 Hz, J(PB–109Ag)
282 Hz; J(PA–107Ag) 138 Hz, J(PA–109Ag) 160 Hz). This spectral pattern indicates a small
difference in the shielding of P atoms within the Ag(P3) units by the C and N functions.
Two broad signals were detected for the trimetallic complex 33, their JPP values are
similar to those of dinuclear copper compound 30.
47
Figure 39. 31P{1H} NMR spectrum of 30, CD2Cl2, 298 K.
The 31P NMR spectrum of 32 shows that several species exist in a dynamic equilibrium
in solution. The phase purity of crystalline compound 32 was confirmed by
photophysical data, which were completely different from those of compounds 2 and 31.
Additionally, the complete assignment of the 1H NMR data for compounds 30, 31, and
33 is consistent with the solid-state structures.
Figure 40. ESI-MS of the complexes 30–33.
In the ESI-MS spectra, signals at m/z 1412.23, 1500.18, 1635.20, and 1590.24 correspond
to singly charged cations of compounds 30–33, respectively, and provide clear evidence
of the existence of these species in solution (Figure 40).
3.3.3 ALKYNYL-BRIDGED DI AND TRINUCLEAR COMPLEXES
In this study, di and tridentate alkynyl ligands were used to assemble the homo bi- and
trimetallic compounds [{(P3)CuC2}2R)] (R = -(C6H4)-n; n = 1 34, n = 2 35, n = 3 36),
[{(P3)CuC2}3R)] (R = 1,3,5-(C6H4)3-C6H3 37, 1,3,5-(C6H4-4-C2C6H4)3-C6H3 38)
(Scheme 3), which were prepared in a similar manner to the mononuclear alkynyl series.
The stereochemistry of the alkynyl spacers resulted in the formation of linear and star-
shaped neutral complexes.
48
The 31P NMR spectra of compounds 34–38 display one set of resonances, which
indicates a symmetrical arrangement of the complexes in solution, and therefore the
equivalence of the CuP3 fragments. The A2B spin system pattern and the values of
chemical shifts were similar to those of the mononuclear complexes 19–23. The 1H NMR
signals of the alkynyl spacers and tridentate phosphine ligand are clearly separated and
were assigned in agreement with the suggested stereochemistry. For example, the proton
spectrum for compound 38 (Figure 41) is consistent with the C3v symmetry point group
of the idealized geometric arrangement. Overall, the NMR data analyses for the alkynyl
series, 34–38, were in good agreement with the proposed structures.
Figure 41 31P{1H} (top) and 400 MHz 1H-1H COSY (bottom) NMR spectra of
complex 38 (CD2Cl2, 298 K).
49
3.4 PHOTOPHYSICAL PROPERTIES OF DI- AND TRINUCLEAR COMPLEXES
This section first describes the photophysical properties of bimetallic thiocyanate
complexes 24, 25, and 27, secondly, those of bi- and trimetallic cyanide complexes 30–
33, and finally, those of bi- and trimetallic alkynyl complexes 34–38, in the solid state.
The others were not measured due to their weak emission, both in the solid state and in
solution. Furthermore, the optical properties of compounds 30–33 were studied in
degassed solution, at 298 K.
The bimetallic compounds 24, 25, and 27 exhibit broad emission bands from blue (448
nm) to yellow-orange (571 nm) in color, which thus cover a wide range of the energies
of the visible spectrum (Figure 42a). The excited states for 24 and 25 were assigned as
(M+L´)LCT in character using computational analysis; the charge transfer involved a
mixture of d(Cu) → phosphine and SCN → phosphine transitions. The L´LCT
contribution is higher in comparison to that of the MLCT in silver complex 27. The
dependencies of lifetime on temperature confirm the TADF properties of these
compounds (Figure 42b). In particular, compound 27 has the longest lifetime (12 µs), at
298 K, among the bimetallic compounds (Table 7).
Figure 42. a) Normalized solid-state excitation and emission spectra of 24, 25, and 27 at 298 K
(solid line) 77 K (dashed line) (appearance of these compounds under UV light depicted in the
inset picture). b) Temperature dependence of decay times for 24, 25, and 27.
A small hypsochromic shift in the emissions of 30 and 31 and a significant bathochromic
shift in the emission of 33 were observed compared with those of mononuclear
compounds 1 and 2. The emission maximum of heterobimetallic compound 32 (λem =
590 nm) was positioned between those of Ag (λem = 525 nm) and Au (λem = 640 nm)
monomeric compounds 2 and 3 (Table 7). The different emission maximum and decay
time of 32 compared with those of 2 and 31 suggested that the crystalline sample of 32
contains only the Au–Ag heterometallic compound without appreciable quantities of
admixtures 2 and 31. A significant decrease in the quantum yields and lifetimes for 30–
33 was observed, compared to those of monomeric compounds 1–3. As was the case for
the mononuclear complexes, MLCT character was assigned to the excited states of 30–
33.
50
Table 7 The photophysical properties of homometallic complexes 24, 25, 27, and 30–38, at 298
K and 77 K, in the solid state.
298K 77K
No λex,
nm
λem,
nm
Ф,
%
τav, a
μs
λex,
nm
λem,
nm
τobs, a
μs
24 370 571 14 2 340, 400 571 118
25 310, 365 448 15 3 341 452 628
27 332 505 35 12 323 472 1701
30 405 520 0 1 ns
31 405 510 15 6
32 450 590 28 3
33 415 545 21 6
34 424 603 3 2 401 540sh, 581, 635 50
35 341, 441 616 1 2 426 556, 642 13
36 347, 441 629 0.6 2 426 574, 622, 683 -
37 393 638 2 1 426 530, 575sh, 640 166
38 313, 483 560 ~0.1 0.3 442 524, 570, 607,
647sh -
a The average emission lifetime for the two exponential decay was calculated using τav = (A1τ12 +
A2τ22)/(A1τ1 + A2τ2); Ai = weight of the i exponent.
Remarkably, crystalline 30 showed an appreciable sensitivity to O2, which caused strong
emission quenching; when exposed to O2 (1 atm), the emission intensity decreased by
99.05% (Figure 43). This behavior can be explained by the presence of void space in the
crystalline material, which allows O2 to penetrate into the bulk solid and collisionally
quench the luminescence.11, 105 As this sensing ability depends on the morphology of the
solid, sample 30a, with BF4– as the counterion, was synthesized analogously to 30, which
contains the CF3SO3– anion.
Both crystalline compounds are strong emitters under an inert atmosphere or under
vacuum (λ = 520 nm, τobs = 6 µs for 30 and 9 µs for 30a). In contrast, they are very
weakly luminescent in air, with lower lifetimes of 45 ns and 1 ns for 30 and 2 µs and 58
ns for 30a. The emission behavior was monitored under repeated variation of the
concentration of O2 in N2 to determine the reversibility of the oxygen sensing response
and the stability of the materials (Figure 43).
51
Figure 43. Emission spectra of complexes 30 (a) and 30a (b) under different concentrations of
O2. (c and d) Corresponding SV plots of 30 and 30a. (e and f) Intensity-response during
variation between 1 atm of N2 and 1 atm of O2.
The emission intensity of 30 is quenched by up to 99.05% at an O2 pressure of 1 atm,
which is higher compared to the value reported for [Cu(CN-xylyl)2(dmp)]tfpb, (dmp =
2,9-dimethyl-1,10-phenanthroline; CN-xylyl = 2,6-dimethylphenylisocyanide) copper
compound107 but lower than that of the copper azolate system.13 The Stern–Volmer plot
of the intensity versus the molar concentration of oxygen is not linear, presumably due
to the heterogeneity of the sample, and can be fitted using a two-site model. The
sensitivity of compound 30 to O2 (Ksv = 319 atm-1) is three times better than those
previously reported for mononuclear copper complexes (Ksv = 96 atm-1).107 The
sensitivity of 30a (Ksv = 639 cm-1) is twice that of compound 30 (Figure 43).
Similar to 30 and 30a, emission quenching by O2 was observed for disilver compound
31a, with the [B(C6H3(CF3)2]4 counter ion (Figure 44). The bulkier counter ion was
selected to prepare non-crystalline material with improved uniformity, significant
porosity, and low density. The quenching constant of 31a, Ksv1 = 47.6 atm-1, is higher
compared to those of silver nanoparticles containing Pd-porphyrin169 and Ru170
complexes, but lower than that reported for a silver cluster based metal-organic
framework.14 The large quenching constant and significant stability of 31a allowed this
complex to be employed in the fabrication of a low-cost, paper-based glucose sensor,
which permits its the detection of Glucose at physiologically important concentrations
in human blood and urine samples, with a fast response time (10 s) and good selectivity.
52
Figure 44. The effect of different O2(g) mole fractions in nitrogen on the responses of 31a on
paper (solid line). λex = 405 nm (left). Stern–Volmer plot for the oxygen quenching of 31a
(right).
In degassed solution, compounds 30–33 have higher quantum yields, between 1.0 and
2.3 x 10-3 %, with a hypsochromic shift compared to those of homometallic series 1–3.
By extending the alkynyl ligands in the di- and trinuclear series of compounds, 34–38,
the emission bands were shifted towards the red region of 560–638 nm and the intensity
was varied between approximately 0.1 and 2.6% (Table 7). The lowered quantum
efficiencies, compared to those of the mononuclear analogues, are tentatively explained
by the increasing size of the alkynyl backbone, which reduced the rate of radiative decay.
The lowest lying triplet excited states for compounds 34–38 were assigned as ILCT type
with mixed MLCT/LLCT character; the largest contributions from the copper metal
atom and the phosphine ligand were predicted for dinuclear compound 34 (Figure 45).
Figure 45. a) Electron density difference plots for the lowest energy triplet emission (T1 → S0)
of the Cu(I) complexes 34 and 37 (isovalue 0.002 a.u.). During the electronic transition, the
electron density increases in the blue areas and decreases in the red areas.
53
4. CONCLUSIONS
The research presented in this thesis focused on the synthesis and photophysical studies
of novel series of copper and silver coordination complexes 1–38, based on
oligophosphine ligands.
With the aim of developing new luminophores, sterically demanding organophosphorus
ligands were employed for molecular construction. This approach, in general, allowed
the preparation of stereochemically rigid compounds, which were capable of efficient
room temperature solid state emission. Chelating tri- and tetradentate ligands P3/P4,
rarely previously encountered in the coordination chemistry of coinage metals, were
successfully used as key building blocks to generate a family of mononuclear complexes
[(P3/P4)M(X)] (X = halides, CN, SCN, alkynyls), which were synthesized using
straightforward one step process utilizing commercially available metal salts, MX, or
terminal alkynes. Notably, the latter species included the first examples of monometallic
alkynyl Cu(I) species.
The variation of the anionic ligands, X, proved to have an substantial effect on the
photophysical behavior of these luminophores. Thus, in the case of the copper alkynyl
compounds, the different localizations of the lowest excited singlet and triplet states, as
predicted by computational analysis, might be responsible for the low quantum yields
(Ф = 0.1–19%, 19–23) and a considerable red-shift of the emission (λem = 573–722 nm).
In contrast, changing the alkynyl group for cyanide dramatically improved the
efficiency of the luminescence, to 70% for copper and 87% for silver complexes; the
latter value was one of the highest among the silver emitters at the time of reporting. In
contrast, the comparison of the thiocyanate compounds and their isocyanoborate
SCN:B(C6F5)3 derivatives illustrated how the nature of the excited states and decay
times can be manipulated by altering the electronic properties of the ancillary groups.
Furthermore, the tetraphosphine derivatives, [(P4)M(SCN)], showed a pronounced
tendency to provide a diversity of solid forms, with a remarkable variation in emission
wavelengths achieved in 7 (λem = 525–630 nm) and 17 (λem = 505–625 nm).
Taking the advantage of the ambidentate nature of cyanide and thiocyanate groups, and
increasing the number of alkynyl groups in the organic ligands allowed the engineering
of bi- and trimetallic systems, which include [M(SCN)P2]2 dimers with [MSCN]2
metallacycles, linearly arranged cyanide [(MP3)2CN]+ and [{(MP3)2CN}2Au]+ species,
alkynyl-bridged linear [{(P3)CuC2}2R], and star-shaped [{(P3)CuC2}2R] complexes.
Importantly, the emission characteristics of cationic cyanide-bridged [(MP3)2CN]+
compounds exhibited significant sensitivity to molecular oxygen, which depended on
the morphology of the solid sample and reached a maximum in porous crystalline solids.
In addition, satisfactory sensitivity was realized in amorphous materials containing
bulky counter ions; this behavior was successfully employed in the fabrication of a
simple-to-prepare and cost-effective sensor to determine the glucose level in blood and
urine samples.
54
Overall, the described affordable luminescent metal complexes, which were easily
prepared from multidentate phosphines and readily available copper and silver
precursors, contribute to a promising approach to molecular materials, the optical
functionality of which can be effectively modulated on both the molecular and
macroscopic levels.
55
ACKNOWLEDGEMENTS
This research work was carried out at the Department of Chemistry, University of
Eastern Finland between 2014-2019. The financial support provided by the University
of Eastern Finland and the Academy of Finland is gratefully acknowledged. The author
also acknowledged the ERKO funding for the personal financial support.
First and foremost, I would like to express my sincere gratitude to my supervisor, Prof.
Igor Koshevoy for giving me the opportunity to work with his guidance and for his
invaluable advice, patience throughout my research life at UEF.
This thesis would not have been completed without additional support from the
collaborative research groups: Prof. Sergey Tunik (St. Petersburg State University),
Prof. Pi-Tai Chou (National Taiwan University), Prof. Antti Karttunen (Aalto
University). I would like to express my special thanks to Docent. Pipsa Hirva, Prof.
Janne Jänis making their contribution to the publications. I owe to my deepest gratitude
to Emeritus prof. Tapani Pakkanen for his advice to select my research area at UEF.
I would like to offer my sincere thanks to Prof. Axel Klein and Dr. Christope Lescop
for their reviews and permission to defend the thesis. I am grateful to Doc. Raija
Oilunkaniemi for accepting her role as an opponent.
I would particularly like to thank inorganic group members Andrey, Vasily, Minni, Toni
and Cecilia (master student, UEF) for their contribution to the publications. Also, I
would like to thank Ilya and others for their support and being for helpful during the
years. I am grateful to several persons at the department of chemistry, who helped me
during my studies. Especially, I thank Taina for assisting in the lab and microanalysis,
together with Päivi Inkinen, Tarja Virrantalo for supporting in chemical supply. I
appreciate Sirpa Jääskeläinen for the opportunity to meet the visitors from school. I am
also thankful to Mari Heiskanen, Sari Suvanto, Eija Faari-Kapanen, Katri Mustonen and
Leila Tiihonen for their administrative support. A special mention goes to Anish, Lin,
Mubin, Chiara, Paulina, Kristina and Muthu for their lively chatting and discussions.
I would like to convey my special thanks to all my friends for their invaluable bond
during my stay in Joensuu.
I would like to express my heartfelt thanks to my parents Chakkaradhari, Thayammal,
and family members: Madhavapriya, Janani, Bhavishya, Sathish, Raghavendran,
Chandra for their unfaltering source of love, encouragement and constant support every
step in my life. Finally, I must express my deepest gratitude to my beloved husband
Senthil, our prince Nikhilan and the little one who is yet to be born for their immense
support, no matter what. You have given me the courage and strength that have led my
accomplishments.
Gomathy Chakkaradhari
Joensuu 2019
56
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Gomathy Chakkaradhari
DissertationsDepartment of ChemistryUniversity of Eastern Finland
No. 151 (2019)
121/2014 KEKÄLÄINEN Timo: Characterization of petroleum and bio-oil samples by ultrahigh-resolution Fourier transform ion cyclotron resonance mass spectrometry122/2014 BAZHENOV Andrey: Towards deeper atomic-level understanding of the structure of magnesium dichloride and its performance as a support in the Ziegler-Natta catalytic system123/2014 PIRINEN Sami: Studies on MgCl2/ether supports in Ziegler–Natta catalysts for ethylene polymerization124/2014 KORPELA Tarmo: Friction and wear of micro-structured polymer surfaces125/2014 HUOVINEN Eero: Fabrication of hierarchically structured polymer surfaces126/2014 EROLA Markus: Synthesis of colloidal gold and polymer particles and use of the particles in preparation of hierarchical structures with self-assembly127/2015 KOSKINEN Laura: Structural and computational studies on the coordinative nature of halogen bonding128/2015 TUIKKA Matti: Crystal engineering studies of barium bisphosphonates, iodine bridged ruthenium complexes, and copper chlorides129/2015JIANGYu:Modificationandapplicationsofmicro-structuredpolymersurfaces130/2015 TABERMAN Helena: Structure and function of carbohydrate-modifying enzymes 131/2015KUKLINMikhailS.:Towardsoptimizationofmetaloceneolefinpolymerizationcatalystsvia structuralmodifications:acomputationalapproach132/2015SALSTELAJanne:Influenceofsurfacestructuringonphysicalandmechanicalpropertiesof polymer-cellulosefibercompositesandmetal-polymercompositejoints133/2015 CHAUDRI Adil Maqsood: Tribological behavior of the polymers used in drug delivery devices134/2015 HILLI Yulia: The structure-activity relationship of Pd-Ni three-way catalysts for H2S suppression135/2016 SUN Linlin: The effects of structural and environmental factors on the swelling behavior of Montmorillonite-Beidellite smectics: a molecular dynamics approach136/2016 OFORI Albert: Inter- and intramolecular interactions in the stabilization and coordination of palladium and silver complexes: DFT and QTAIM studies137/2016 LAVIKAINEN Lasse: The structure and surfaces of 2:1 phyllosilicate clay minerals138/2016 MYLLER Antti T.: The effect of a coupling agent on the formation of area-selective monolayers of iron a-octabutoxy phthalocyanine on a nano-patterned titanium dioxide carrier139/2016KIRVESLAHTIAnna:Polymerwettabilityproperties:theirmodificationandinfluencesupon water movement140/2016 LAITAOJA Mikko: Structure-function studies of zinc proteins141/2017 NISSINEN Ville: The roles of multidentate ether and amine electron donors in the crystal structure formation of magnesium chloride supports 142/2017 SAFDAR Muhammad: Manganese oxide based catalyzed micromotors: synthesis, characterization and applications143/2017 DAU Thuy Minh: Luminescent coinage metal complexes based on multidentate phosphine ligands144/2017AMMOSOVALena:Selectivemodificationandcontrolleddepositiononpolymersurfaces145/2017 PHILIP Anish: PEI-mediated synthesis of gold nanoparticles and their deposition on silicon oxide supports for SERS and catalysis applications146/2017 RAHMAN Muhammad Rubinur: Structure and function of iron-sulfur cluster containing pentonate dehydratases147/2018 ANKUDZE Bright: Syntheses of gold and silver nanoparticles on support materials for trace analyses using surface-enhanced Raman spectroscopy148/2018 PENTTINEN Leena: Structure determination of enzymes with potential in processing of cell wall compounds149/2018 SIVCHIK Vasily: Tuning the photoluminescence of cyclometalated platinum(II) compounds via axial and non-axial interactions150/2019 MIELONEN Kati: Hierarchically structured polymer surfaces: Curved surfaces and sliding behavior on ice
Tuning the emission properties of oligophosphine copper and silver complexes with ancillary ligands
Gom
athy Chakkaradhari: Tuning the em
ission properties of oligophosphine copper and silver complexes w
ith ancillary ligands
151