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Chapter 1
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Chapter 1
Introduction
1. INTRODUCTION
Coordination chemistry, the science concerned with the interaction of
organic / inorganic ligands with metal centers has remained one of the most
active research areas in inorganic chemistry.
The study of coordination chemistry in the modern day perspective was
initiated due to the significant contributions of two notable scientists; Alfred
Werner and Sorphus Mads Jorgenson. The pioneering contribution of
Werner to the study of coordination chemistry was well recognized by the
Nobel Prize awarded to him in the year 1913. Many of the basic ideas
related to the stereochemistry of metal complexes and the mechanism of
isomerization given by Werner has remained unchanged even today. The
nature of the metal-ligand bond, stability, structure and stereochemistry of
metal complexes are now better understood with the help of advanced
sophisticated physicochemical techniques of high precision and capability.
Subsequent to the pioneering work by Werner and Jorgenson, the research in
chemistry has progressed a lot. The stepping stone provided by Werner and
Jorgenson has led the modern inorganic chemistry in the direction of
becoming truly a multidisciplinary subject in the present day context [1].
Coordination chemistry is found to be applicable in the fields of wide
diversity such as dyes, colors, nuclear fuels, catalysis, photography,
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toxicology, bioinorganic chemistry, medicine, ceramics, materials science
and toxicology [2-4].
Progress of the industries dealing with organic chemicals, pharmaceuticals,
petrochemicals and plastics depends a lot on the findings in the field of
coordination chemistry.
Nature makes extensive use of coordination compounds and the study of
such compounds is becoming increasingly popular in biology as well as in
chemistry. Inclusion of a variety of ligands in complexes has enabled their
applications as biocides, catalysts, NMR shift reagents and DNA binders [5].
The study of interaction of small molecules and metal complexes with DNA
is an active area of research at the interface of chemistry and biology [6].
Many of the biologically active compounds are transition metal complexes
and even the simpler types of metal complexes have served as model
compounds in investigating natural processes. The living system is also
partially supported by coordination compounds. Hemoglobin, an iron
complex, carries oxygen to the animal cells [1, 7].
In coordination chemistry, the search for molecular magnets with specific
properties is a challenging field for a synthetic chemist. The suitable designs
of new compounds with the improved features of magnetic properties are of
great interest for technological applications [8, 9].
Development of sophisticated analytical instruments and a synthesis of a
wide variety of coordination compounds have encouraged many researchers
to revisit the chemical reactions. This study has enabled the inorganic
chemists to make significant progress in the modification of the concept of
chemical bonding.
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1. 1 Ligand
In coordination chemistry, a ligand is an atom, an ion or a molecule attached
to a central atom / ion which are usually a metal to form a coordination
complex [10].
The atoms and molecules used as ligands are capable of functioning as
donors of electron-pair in the bond formed with the central metal atom / ion.
Ligands contain at least one donor atom with a lone pair of electrons used to
form covalent bonds with the central metal ion or atom with which they are
attached. Thus, the ligands act as Lewis bases and the central metals act as
Lewis acids. The central metal usually has a positive charge which is
stabilized by donation of electrons from the ligands. The nature of metal –
ligand bonding can be covalent or ionic. Ligands can be anions, cations or
neutral molecules. Examples of common ligands are the neutral molecules
like water (H2O), ammonia (NH3) and carbon monoxide (CO) and the anions
like cyanide (CN-), chloride (Cl
-), and hydroxide (OH
-). Cations like NO
+
and N2H5+ are also capable of acting as ligands [11].
Ligands are classified in different ways based on their charge, size, identity
of the coordinating atom(s), and the number of electrons donated to the
metal [12].
Ligands that bind the central atom through only one site are known as
monodentate ligands. Monodentate ligands are sometimes referred to as "one
toothed" because they bind to the central metal atom at one point. Some
examples of monodentate ligands are chloride ions (referred to as chloro
when it is a ligand), water (referred to as aquo / aqua when it is a ligand),
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hydroxide ions (referred to as hydroxo when it is a ligand) and ammonia
(referred to as ammine when it is a ligand).
When ligands have two donor atoms which allow them to bind the central
metal atom or ion at two points are called bidentate ligands. Common
examples of bidentate ligands are ethylenediamine (en), and the oxalate ion
(ox) as shown in figure 1.
Figure 1: Bidentate ligands.
Some ligand molecules containing many atoms capable of donating lone pair
of electrons are able to bind the metal ion through multiple sites. These
ligands are called polydentate ligands [13].
Diethylene triamine (dien) is an example of a tridentate ligand. Tridentate
ligands are also known as ‘scorpionate ligands’. EDTA
(ethylenediaminetetraacetate) has six sites available for bonding. Hence, it is
an example of hexadentate ligand as shown in figure 2.
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Figure 2: Polydentate ligands.
Most of the complexes of polydentate ligands are chelated complexes; they
tend to be more stable than the complexes of monodentate ligands as it is
necessary to break all of the bonds to the central atom for the ligand to be
displaced [14].
1. 2 Schiff base ligands
The condensation of primary amines with aldehyde and ketones gives
compound with a functional group that contain a carbon-nitrogen double
bond with the nitrogen connected to an alkyl group called Schiff bases, since
their synthesis reported by Hugo Schiff (1864) [15].
The general formula in the broadest sense of the Schiff base is R1R2C=NR3,
where R is an organic side chain. The Schiff base is synonymous with
azomethine. The presence of a lone pair of electron in sp2 hybridized orbital
of nitrogen atom of azomethine group is of considerable chemical
importance [16, 17]. This lone pair imparts an excellent chelating ability
especially when used in combination with one or more donor atoms close to
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azomethine group. So, Schiff bases are capable of forming coordinate
covalent bonds with many of the metal ions through azomethine and
phenolic group or other group present on the ligand [18, 19].
Chromatographic purification of Schiff bases on silica gel is not
recommended as they undergo hydrolysis. Examples of few such ligands are
shown in figure 3. A large number of Schiff base complexes have been
extensively investigated for their catalytic and biological activity [20].
Figure 3: Schiff base ligands.
1. 3 Chelation
Chelation is a process in which a polydentate ligand bonds to a metal ion
forming a ring. The complexes involving a ring in which metal ion is an
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integral part is called a chelate and the polydentate ligand is referred to as a
chelating agent.
Chelates are generally more stable than complexes derived from
monodentate ligands. This enhanced stability known as chelate effect is
usually accredited to effects of entropy which favors the displacement of
many ligands by one polydentate ligand [12]. When the chelating ligand
forms a large ring that at least partially surrounds the central atom and bonds
to it leaving the central atom at the centre of a large ring, the complexes are
called macrocyclic complexes [21]. These complexes are generally more
rigid and involve higher ligand denticity. These complexes are more inert.
Hemoglobin is an example of macrocyclic complex. Hemoglobin is a
complex with a porphyrin macrocycle and an iron atom at the center bound
to four nitrogen atoms of the tetrapyrrole macrocycle. A very stable
dimethylglyoximate complex of nickel is a synthetic macrocycle derived
from the anion of dimethylglyoxime ligand [22].
Ethylenediaminetetraacetic acid (EDTA), with four carboxylic acid groups
along with two amine groups can form six bonds with a metal ion and is a
popular hexadentate ligand in coordination chemistry. Under suitable
conditions, EDTA forms chelates with a wide variety of metal ions. These
chelates contain five 5-membered rings in their structure. The
hexacoordinated complexes from EDTA are octahedral in geometry as
shown in the figure 4.
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Figure 4: Chelated complex of EDTA.
1. 4 Transition metal complexes
The transition metals are known to form a wide variety of complexes with
different ligands. The formation of M-L bond requires the metal to possess
vacant orbitals known as secondary valency in coordination chemistry.
These orbitals must have suitable orientation in the space with reasonably
low energy. Since, the transition metal ions generally meet these
requirements best, they form complexes readily. Almost all the transition
elements form coordination complexes due to the availability of their vacant
d-orbitals [10].
Following characteristics make the transition metals particularly interesting
to coordination chemist:
Variable oxidation states (electron transfer properties),
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Spectral and magnetic features, ligand field effects, unpaired d-
electrons,
Formation of chelated complexes,
Coordination geometries (tetrahedral, octahedral, square planar,
pyramidal etc.)
Most M2+
and higher oxidation states are borderline or hard acids and
generally prefers borderline or hard base such as O- and N-donor
groups, whereas lower oxidation states bind soft bases.
Metal coordination complexes have a wide diversity of technological and
industrial applications from catalysis to anticancer drugs [23].
1. 5 Applications of metal complexes
Metal complexes plays essential role in pharmaceutical, petrochemical,
plastic and agricultural industries. Particularly, the Schiff base complexes
are widely applicable in various biological systems, catalysts, polymers,
dyes as well as enzymatic agents [20].
I. Catalysis
Many Schiff base metal complexes show excellent catalytic activity in
various reactions at temperatures above 100oC in the presence of moisture.
These types of applications have been reported both in homogeneous and
heterogeneous catalysis [24]. The Schiff base metal complexes are capable
of catalyzing reactions like hydrolysis, oxygenation, electro-reduction and
decomposition [25]. The production of commercially important branched
and linear polyethylenes is increased by the catalytic activity of Schiff base
metal complexes in polymerization of olefins [26]. The transition metals like
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tungsten, molybdenum and ruthenium in the presence of alkylating agents
such as R4Sn or RAlCl2 catalyzed the ring opening polymerization of
cycloalkenes at high temperature without any control on the molecular
weight of polymers [27]. Schiff base metal complexes showed important
applications in the reduction of ketones to alcohols and alkylation of allylic
substrates [28]. The oxidation of hydrocarbon using Schiff base metal
complexes has been a field of academic and industrial interest to analyze the
catalytic activity of various metal complexes. Schiff base metal complexes
also show catalytic activity in the carbonylation of alcohols and alkenes at
low pressure to produce α-arylpropionic acid and their esters [29].
In addition to monometallic, the bimetallic Schiff base complexes also show
catalytic activity in carbonylation reaction. The Heck reaction, an
industrially useful process to synthesize fine chemicals and pharmaceuticals
has been catalyzed successfully using Schiff base complexes [30]. The
Schiff base complexes of nickel(II) and copper(II) ions have increased
enantioselectivity in the alkylation of enolates [31]. The Schiff base
complexes of copper(II) and manganese(III) moderately improved the
enantiomeric synthesis of aziridines and amides with chiral
metalloporphirins [32]. The isomerization of norbornadiene to quadricyclane
was considerably catalyzed using diimine complexes of rhodium. These
types of interconversions were useful for the storage of solar energy [33].
The aluminium-salen Schiff base complexes when used in catalyzing the
addition of hydrogen cyanide to N-allylbenzaldimine showed enantiomeric
excess [34]. The optically active cyanohydrins are extensively used in the
synthesis of drugs and pesticides. These cyanohydrins were synthesized
successfully reacting trimethyl silylcyanide with aldehydes in the presence
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of transition metal Schiff base complexes [35]. Schiff base complexes are
also useful in desymmetrization of meso compounds with significant yield
and enantiomeric excess [36]. The homogeneous chiral lanthanum(III)
Schiff base complexes showed catalytic activity in asymmetric Diels–Alder
reactions [37]. These studies point out that the Schiff base metal complexes
are potential catalysts to influence the yield and selectivity in chemical
transformations.
Dinuclear Schiff base complexes of transition metal ions are more efficient
catalysts than mononuclear complexes probably due to the synergic effect of
two metal ions. A variety of homo and hetero dinuclear Schiff base
complexes of transition metal ions are used as catalysts in various reactions
[38]. The dinuclear Schiff base complexes of copper (II) are used as
catalysts in oxygen activation [39]. Dinuclear Schiff base complexes of
copper (II) ions prepared from 2-hydroxyisopthalaldehyde and 2-(pyridine-
2-yl)ethanamine as shown in figure 5(b), are used successfully in
hydroxylation of phenol [40]. The homo and hetero dinuclear complexes of
transition metal ions are effective catalysts in direct oxygenation of
unfunctionalized hydrocarbons and phenols. The dinuclear complexes
formed from the palladium ion as shown in figure 5(a) are also useful in
oxidation reactions.
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(a) Dinuclear palladium complex (b) Dinuclear copper complex
Figure 5: Dinuclear complexes used as catalyst.
II. Materials science
The magnetic properties of solids are very important and attempts to
understand them have provided a deep insight into the fundamental structure
of many coordination complexes [41]. Nowadays, magnetic materials are
being used in biomedical applications like contrast agent in magnetic
resonance imaging (MRI), targeted drug delivery and magnetic separation of
cell, DNA, protein etc.
Magnets are also used for storage of information in various devices like
tapes, hard discs and other memory devices [42]. Reduction the size of
particles can permit the size reduction of several hardwares used in computer
related applications. A type of magnetism known as superparamagnetism is
observed in some ferromagnetic and ferrimagnetic nanoparticles. Under the
influence of temperature, the magnetization in some small nanoparticles is
known to flip the directions randomly. The time gap between two such
consecutive flips is called Neel relaxation time [9]. In absence of the
external magnetic field if the time used to measure magnetization is greater
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than the Neel relaxation time, the average magnetization appears as zero and
the material is said to be in superparamagnetic state. Under such conditions,
the behavior of the materials in external magnetic field becomes similar to a
paramagnetic material with a very high magnetic susceptibility [43, 44]. The
usage of such small nanoparticles has facilitated the size reduction in
hardware. However, there is a lower limit to the size of the particle provided
by superparamagnetic size below which the information cannot be
permanently stored due to the free fluctuation of the magnetization.
Recently, it has been discovered that molecules containing transition metal
ions show a slow relaxation of magnetization at low temperature and
behaving like superparamagnets [45]. This is a very interesting property,
because they give rise to the magnetic hysteresis effect and become bistable.
Thus, there is a possibility to open a storage of information in a single
molecule.
Slow relaxation of magnetism in some higher nuclearity polynuclear
complexes is known to occur via quantum tunneling mechanism [46, 47].
When the magnetization returns to the ground state it does not follow the
rules laid down by the classical mechanics which involves going over the
energy barrier (Figure 6, route 1) [48]. A single molecular magnet (SMM)
with the spin state of Ms = 10 at the ground state when placed in the
magnetic field so that the spin state becomes Ms = -10. When the field is
removed, it does not return to Ms = 10 by going from Ms = -10 → Ms = -9
→ Ms = -8 …. Ms = 0 →….Ms = 9 → Ms = 10. Instead, the spins states are
tunneled from one spin state to another so that it does not go through all the
levels (route 1, route 2, route 3). This occurs only if the two spin states are
equal in energy or may be observed by steps in the hysteresis curve. The
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quantum tunneling mechanism enables the use of these complexes in the
study of quantum effects or in the quantum computing as quantum bits [49].
The polynuclear complexes are equivalent to binary units in classical
computing [50]. The advantage of the quantum computers is that they have
the potential to perform the same functions as conventional computers but
on a smaller scale.
Figure 6: Quantum tunneling in single molecular magnets.
( Route 1: No quantum tunnelling. Route 2: Thermally assisted quantum
tunnelling. Route 3: Pure quantum tunnelling.)
The magnetic properties of poly- and dinuclear transition metal complexes
are characterized by (a) the exchange coupling between the transition metal
cations, given by the exchange integral J (direct exchange, super exchange,
double exchange), (b) the electronic g-factor, describing the splitting of
degenerate electronic levels in an external magnetic field, and (c) the zero-
field splitting parameter D which contains information on local geometrical
distortions and spin orbit interactions.
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The quantum tunneling is observed generally in the inorganic metal
complexes having more than one metal centers. The magnetic interaction
between two nonequivalent paramagnetic centers may lead to situations
which cannot be encountered in species containing only one kind of metal
center. The polynuclear complexes of transition metals can act as single
molecular magnet. Especially in the polynuclear complexes, there is
increasing interest in dinuclear complexes, which contain ligand structures
capable of holding two metal centers in close proximity. These dinuclear
complexes have formed the basis for a detailed understanding of magnetic
exchange interactions and provide fundamental insights into the geometrical
and electronic properties of the bridged group [51, 52]. The field of
molecular magnetism has developed rapidly in the last two decades and
particular emphasis has been placed on hetero bimetallic complexes. In
physicochemical aspects these dinuclear complexes have noteworthy
significance as new inorganic materials. They show various magnetic
properties with antiferromagnetic coupling depending upon the bridge angle
and degree of distortion. The dinuclear complexes also show redox
properties based on the macrocyclic ring size and show redox driven
translocation mechanism [53].
The presence of two metals in the same molecule largely affects both the
physical properties and the reactivity of the complexes. This is either due to
the significant modifications in the individual properties of two metals are in
the development of new characteristics not observed in mononuclear
complexes. The physical properties of these dinuclear metal complexes
(redox properties, florescence etc.) vary to a great extent [54]. In the case of
polymetallic complexes, it is possible to study the effects of chemical,
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electrochemical or photochemical modification of one metallic center on the
properties of the other. The reciprocal interaction between the active centers
often brings amazing results. A great interest for transition metal complexes
arises not only from the above mentioned particularities but also from the
wide range of arrangements, which can be created due to the huge flexibility
in their structures [55]. Besides the availability of a large number of
transition metals it is often sufficient through simple reactions to vary either
the nature of the auxiliary ligands bound to the metals or the oxidation state
of the metals themselves in order to induce particular chemical and physical
properties in the system [56].
III. Biology
The metal complexes exhibit a lot of bioactivities such as antimicrobial
activity, antiviral activity, antifungal activity, analgesics, HIV protease and
anticonvulsants [20].
a. Antimicrobial activity
Schiff bases and their complexes exhibit antimicrobial activity according to
types of metals and ligands. Schiff bases prepared from indane-1, 3-dione-2-
imine-N-acetic acid and 2-imino-N-2-propionic acid and ninhydrin, glycine
/L-alanine and their metal(II) chelates shows unique geometries and good
antimicrobial activities against E. coli, P. mirabilis, S. aureus and P.
faecalis. Various metal complexes with aniline exhibit different behavior
with different types of bacteria. Some aldimines, pyrazines, aminoacids
derived Schiff base and heterocyclic ketones derived Schiff bases and their
complexes also exhibit antimicrobial activity [57]. Schiff bases and metal
complexes derived from benzimidazole, toluidinones, furaldehydes,
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thiazoles, pyridine, pyrazolone, hydrazine and imidazolinones exhibits
antibacterial activity. Salicylidine derivatives and metal complexes exhibit
antibacterial activity against S. typhi, S. aureus, B. subtilis and S. flexneri
[58, 59].
b. Antifungal activity
Thiazole and benzothiazole Schiff bases show effective antifungal activity
[60]. Presence of methoxy, halogen and napthyl groups enhance fungicidal
activity towards Curvularia. Furfurglidene nictoinamide Schiff base
exhibits antifungal activity against A. niger, Alternaria solani and
Collectotricum capsici. Pyrandione Schiff bases exhibits physiological
activity against A. niger. Some Schiff bases of quinazolinones show
antifungal activity against Candida albicans, Trichophyton rubrum, T.
mentagrophytes, A. niger and Micosporum gypseum [61, 62].
Schiff bases and their metal complexes formed between furan or
furylglycoxal with different amines show antifungal activity against
Helminthosporium gramineum (causing stripe disease in barely),
Syncephalostrum racemosus (causing fruit rot in tomato) and C. capsici
(causing die back disease in chillies). Moreover, hydrazine and
carbothioamide as well as their metal complexes exhibit antifungal activity
against A. alternata and H. graminicum. Molybdenum and manganese
complexes control disease (caused by A.alternata) in brinjal crop. Schiff
bases derived from benzothiazole or phenyl-azo-thiazole and its metal
complexes show microbiological activity against A. niger and A. alternata.
The salicyladmine Schiff base complex of ruthenium(II), thalium(I)
complexes with benzothiazolines, copper(II) complexes of the
benzoylpyridine Schiff base show antifungal activities [63].
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Oxovanadium(IV) complexes with triazole exhibits antifungal activity [64].
As(III), Sb(III), and Bi(III) complexes with o- tolylammonium di-
thiocarbamate are antifungal against A. niger and A. alternata. Some novel
Schiff bases derived from cephalexin and their metal complexes show
antifungal activities. Schiff bases derived from salicylaldehydes and
boronate esters exhibited antifungal activities against A. niger and A. flaves.
The Schiff base prepared from salicylaldehyde and di-methyl
thiophosphoramide and their complexes with Cu(II), Ni(II), and Zn(II) are
effective chemicals to kill Tetranychus bimaculatus [65, 66].
c. Antiviral activity
Schiff bases of gossypol shows high antiviral activity. Silver complexes in
oxidation state (I) exhibited inhibition against Cucumber mosaic virus;
glycine salicylaldehyde Schiff base Ag (I), gave effective results up to
74.7% towards C. mosaic virus [67].
d. Anti – tumor and cytotoxic activity
Salicylidiene anthranilic acid possesses antiulcer activity and complexation
behaviour with copper complexes, which exhibit an increase in antiulcer
activity. Some Schiff bases and their metal complexes containing Cu, Ni, Zn
and Co were prepared from salicylaldehyde, 2,4 dihydroxy- benzaldehyde,
glycine and L-alanine possess antitumor activity and their order of reactivity
with metal complexes is Ni˃Cu˃Zn˃Co [68].
The mononuclear complex of platinum cisplatin as shown in figure 7(A) is
currently used in the treatment of testicular, ovarian, head and neck, neck
and cervical cancers. However, a large percentage of human cancers have a
natural resistance to treatment with cisplatin. Nowadays, there is good
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development in the multinuclear platinum complexes shown in figure 7(B),
that can used as anticancer drugs. Multinuclear platinum complexes contain
two or more linked platinum centers that can each covalently bind to DNA.
Hence these are capable of forming a completely different range of DNA
adducts compared to cisplatin. These multinuclear complexes have great
potential as new anticancer agents [69].
(A): Cisplatin (B): Dinuclear linked cisplatin complex.
Figure 7: Anticancer platinum complexes.
Transition metals have an important place within medicinal biochemistry.
There is significant progress in the utilization of transition metal complexes
as drugs to take care of several human diseases. Transition metals exhibit
different oxidation states and can interact with a number of negative charged
molecules. This activity of transition metals has started the development of
metal based drugs showing potential pharmacological applications [70].
IV. Medical therapy
The carbon monoxide (CO) and nitric oxide (NO) affects the biological
cycle can be appropriately described by the general observation of
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Paracelsus in the early 16th
century that “the dose makes the poison”. These
diatomic molecules are odorless, colorless gases that were long known only
as toxic poisons until the discovery in the 1980s of NO as the endothelium-
derived relaxing factor [71]. The nitric oxide (NO) is now known as an
important signaling molecule that impacts a wide range of physiological
responses, including blood pressure regulation, neurotransmission, immune
response and cell death. The information on the biological roles of CO is
about 15 years behind that of NO. But, it appears to play a role in some of
the same pathways as NO in addition to other important processes.
The concentration dictates the biological effect in both the cases, with low
concentrations being critical for signaling events and high concentrations
being toxic. These gas molecules also have the common importance in the
transition metal coordination chemistry which increases their biological
impact. Also, their biosynthesis is metal-dependent, and in many cases their
biological targets are metal centers, typically heme iron. These reactions
notify that transition metal complexes in biological environments can
liberate and sequester NO and CO by breaking or forming metal-nitrosyl
(M-NO) and metal-carbonyl (M-CO) bonds. Therefore, it is possible to
develop artificial small molecule coordination complexes that can detect NO
and CO in order to study their biological roles and also act as therapeutic
agents [3].
2. POLYTOPIC LIGANDS
Dinuclear and polynuclear transition metal complexes bridged by
polyatomic ligands have gained much concentration in the recent years
towards synthesis, characterization and applications. Transition metal
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complexes of such type have become subject of methodical investigation
due to their applications in the study of intermetallic interactions, magnetic
exchange, catalysis and binuclear metal reactivity. Polynuclear complexes
are interesting both from the magnetochemical point of view as well as
potential model of biological systems [72].
The behavior of single metal ions embraced by a monodentate as well as the
chelating ligand environment has been studied extensively till date [19, 73].
In such systems individual metal centers are usually too far from each other
which restricts the possibility of spin-spin coupling between paramagnetic
metal ions. Polynucleating ligands, on the other hand, have structural
attributes that combine separate coordination pockets. They are continuously
arranged, metal ions are bound at a smaller distance and can be linked
directly by endogenous or exogenous ligand fragments which can lead to
spin communication between metals [74].
Polytopic ligands can be designed in such a way that the synthesis becomes
convenient. Such ligands range from ditopic to hexatopic displaying
different geometry and length. They may also contain a variety of functional
groups. Such a rich library of ligands gives an opportunity to systematically
study the relationship between the geometry of the ligand and the
functionality of the product obtained. The increasing interest for hybrid
ligands (hard and soft type) has induced new chemical and physical
properties in their complexes. Some examples of the polytopic ligands with
hard coordination functions containing oxygen, nitrogen as donor atoms are
discussed here [75].
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2. 1 Diketones
Classical β-diketones and related ligands have been studied for more than a
century. Their ability to give rise to rich and interesting coordination
chemistry is well recognized. They act under appropriate conditions as
nonnegative O2-chelating donors, capable of stabilizing mononuclear or
polynuclear complexes. In particular, their keto-enol tautomerism has been
studied in solution by IR and NMR spectroscopy and in the solid state by X-
ray single crystal diffraction as shown in figure 8 [76].
Figure 8: Keto-enol tautomerism in diketones.
There is a growing amount of literature which especially deals with the
possible applications of these complexes as components of molecular
devices or as precursors in the formation of new materials. The application
of the complexes as phosphors for lighting and high efficiency
electroluminescent devices for light emitting diodes, contrast agents for
medical magnetic resonance imaging, NMR shift reagents, luminescent
probes for proteins and amino acids, magnetically addressable liquid
crystals, magnetic alloys for refrigeration and superconducting materials
give good reason for the efforts made to control the metallic sites and to
selectively introduce specific metal ions into organized assemblies [77].
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Here, the increasing of carbonyl groups with the consequent formation of tri-
or tetraketones and bis-β-diketones as shown in the figure 9 allows the
formation of well-defined homo- and /or heteropolynuclear complexes [78].
Figure 9: Poly-diketones.
These complexes have unusual physico-chemical properties, arising due to
the coordination of equal or different metal ions in close connection and
interacting with each other through the carbonyl bridges. Moreover, these
ligands generally coordinate in the equatorial plane of metal ions like
copper(II), nickel(II), cobalt(II).
Furthermore, the insertion of phenol groups at the end or between the
carbonyl moieties generates an interesting series of β-ketophenolate systems
as shown in figure 10, capable of securing up to eight metal ions in close
proximity. The metal ion assembly is mainly governed by the presence or the
release of the phenol protons [79].
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Figure 10: Keto-phenol derivatives
2. 2 Dicarboxylates
The dicarboxylate anion is capable of generating homo- and
heteropolynuclear complexes. The wide structural diversity of the oxalato-
bridged complexes (binuclear species to high-nuclearity compounds and to
two and three dimensional coordination polymers) is due to the outstanding
flexibility of the oxalato ligand as shown in figure 11 [80]. The oxalate
ligand is the simplest dicarboxylate. The oxalato bridge can powerfully
mediate the exchange interactions between the paramagnetic metal ions
shows interesting magnetic properties.
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Figure 11: Modes of coordinations of dicarboxylates.
Numerous oxalato-bridged homopolynuclear complexes have been
synthesized and characterized till date. These compounds are generally
obtained through the reaction between a cationic complex having potentially
free coordination sites and the oxalate anion [81].
2. 3 Phenolic ligands
In 1970, Robson defined a class of ligands able to simultaneously bind two
or more metal ions thus forming di- or polynuclear metal complexes [82].
From amongst the many different types of dinucleating ligands and
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polynucleating ligands, the phenol-based molecules have involved the
attention of a great number of researchers. This is due to the key role played
by the phenolic group which has many useful electronic and structural
characteristics such as:
(i) Charge as a function of pH: The charge in such complexes ranges
from 0 at low pH to −1 at high pH values;
(ii) Bridging capability: The phenolic donor atom is capable of binding
two metal centres in close proximity;
(iii) Effect of aromatic ring: The benzene ring present allows a great
synthetic flexibility.
Regarding the first point, the acid–base properties of the phenol in aqueous
solution depends on the ligand topology in which it is inserted; in fact,
although the phenol loses its acidic proton at pH > 10 giving the phenolate
H−1L− anionic species, this process can occur also at lower pH values when
the phenol takes part of an amino-phenolic ligand. Often, it is the H−1L
species involved in the second point, which is the phenolate oxygen atom to
bridge two metal centres [83].
I. Ligands containing one phenolic unit:
The ligand with one phenol unit has appeared as an important class of
acyclic ligands capable of binding two metal ions close to each other in
addition to bridging abilities of the phenolate oxygen atom towards metal
ions. Some of the phenolic ligands containing amine or polyamine side arms
as shown in figure 12. The basicity behavior and coordination properties in
aqueous solution of these types of ligands are reported [84].
Chapter 1
Page 27
Figure 12: Ligand containing one phenolic unit.
Some of the phenolic ligands bearing the imine and pyridine side arms as
shown in figure 13.
Figure 13: Phenolic ligand with imine and pyridine side arms.
Chapter 1
Page 28
II. Ligands containing two phenolic units:
The ligands containing two phenolic ligands can form the dinuclear as well
as polynuclear complexes. The symmetrical biphenolic N5O2 donor ligand
(2,6-bis(2-hydroxyphenyl) pyridine) forming µ-phenoxo bridge complexes,
whereas some tetradentate amino diphenolic ligands such as (N,N’-bis[(2
hydroxyphenyl] methyl)-1,3-propylendiamine) forming complexes without a
bridge is shown in figure 14 [85].
Figure 14: Ligands containing two phenolic units.
Some ligands containing one phenolic unit with reactive group (aldehyde)
can react with diamines to form the Schiff base ligands with polynucleating
atoms. Bis (o-vanillin) benzidine prepared by the Schiff base reaction of o-
vanillin and benzidine is shown in figure 15. These types of ligands
generally used for the formation of homonuclear complexes.
Figure 15: Phenolic Schiff base ligand.
Chapter 1
Page 29
Different oximes and metal oximates are established to be versatile ligands
in polynuclear complexes due to their ambidentate character with potential
for oxygen and nitrogen coordination. Since 1905, when Tschugaeff first
introduced dimethylglyoxime as a reagent for detection of nickel, oximes as
ligands have played an important role for the long-term progress in
coordination chemistry. Due to the flexibility in bonding, oximes are
excellent bridging units in modular synthesis [86]. Modular preparation with
oximate ligands enables the synthesis of linear symmetrical and
asymmetrical cores containing two different metal ions [87]. Some oximes
which have been used for synthesizing polynuclear complexes are listed
below as shown in figure 16.
Figure 16: Different types of oxime ligands.
Chapter 1
Page 30
2. 4 Bridging ligands
Bridging ligands have received much interest recently due to their ability to
couple metal centers in a covalent manner resulting in polymetallic
complexes that frequently possess new and interesting properties. Bridging
ligands of the type discussed here bind to each metal through one or more
donor atoms forming a coordinate covalent σ-bond. Due to the presence of
π-systems on the ligands, commonly π- backbonding or less commonly π-
bonding, can lead to enhanced stability of the metal-ligand bonds. The
denticity of a ligand is commonly used to describe its bonding [88].
Herein, monodentate bridging ligands include the class of ligands that bind
to each metal center through only one donor atom. These monodentate
bridging ligands are historically significant, thus some of their chemistry is
also included in the discussion. The monodentate bridging ligands
containing primarily nitrogen-donor atoms such as cyanide, linked pyridines
and fused pyrazine ring systems as shown in figure 17. The fused pyrazine
have two donor atoms but the each donor atom can bridge only one metal
centre [89].
Figure 17: Monodentate bridging ligand.
Bidentate bridging ligands encompass the broad and rapidly expanding field
of ligands which bind to each metal center through two donor atoms. Such
bidentate ligands have generated a lot of recent research in this field and lead
Chapter 1
Page 31
to the study of a wide assortment of supramolecular complexes using these
ligands as the connectors. Bidentate bridging ligands bind to each metal by
two donor atoms. This gives added stability through the chelating effect.
Ligands such as 1,10-phenanthroline and 2,2′ bipyridine as shown in figure
18, are the bidentate bridging ligands [90].
Figure 18: Bidentate bridging ligands.
Tridentate bridging ligands include bridging ligands that bind to multiple
metal centers using three donor atoms per metal center as shown in figure
19.
Figure 19: Tridentate bridging ligand.
Tridentate bridging ligands bind two or more metal centers through three
donor atoms per metal center. The pyridine based bridging ligands and
phenanthroline based bridging ligamds are tridentate bridging ligands. The
function of such bridging ligands is also to prevent undesired
oligomerization processes. The bridging ligands including di-, tri- and tetra-
Chapter 1
Page 32
amines, 2,2′-bipyridine, 1,10-phenanthroline, 2,2′,6′,2′′-terpyridine have
been used as end-cap ligands [75].
3. METAL ORGANIC LIGANDS (MOLS)
In the last twenty five years, complexes of transition metals with higher
nuclearity has attracted the attention of many coordination chemists. This
class of compounds is found in the literature with several names such as
oligomeric complexes, polynuclear complexes, cages and clusters [91]. A
central question for the synthesis of polynuclear complexes is that ‘Are there
any general methodologies for the template synthesis of polynuclear
complexes ?’ In general the answer is ‘No’. In contrast to the predictive
synthetic schemes applied in organic chemistry, the reaction in polynuclear
transition metal chemistry cannot be described as operator controlled. In
order to enable the tailor making of polynuclear complexes, the greatest
concern is the development of synthetic routes that can provide metal
complexes with high nuclearity, particularly heterometallic systems in a
controlled manner [92]. Over the last 15 - 20 years several groups (Escuer
and Vicente, Decurtins, Christou, Thompson, Verdaguer etc.) have
commendably attempted the development of route to the synthesis of such
compounds.
From amongst the variety of methodologies applied to synthesize
polymetallic coordination compounds, the use of ‘metalloligands’, i.e. metal
complexes as ligands, in which the ligands already bounds to one metal have
free coordination sites that can bind a second metal of the same or a different
kind has proven to be very successful [93]. Different complexes containing
one or more metal centers are able to react further with other complexes
Chapter 1
Page 33
through available appropriate donor atoms. One should begin with
monometallic precursors which can then be assembled by chemical reaction
to form polymetallic complexes. These types of complex precursors
considered as ligand named as metal organic ligands (MOLs) [94, 95]. The
well recognized approach ‘metal complexes as ligands’ involving
multinucleating ligands offers many potential advantages over the self-
assembly route and it enables greater control over the route of the reaction
and the products [96]. The MOL approach allows the synthesis of larger
molecules by reaction of mono or binuclear complexes of appropriate
ligands. These approach containing polynucleating ligands proceeds step by
step and provide a route to gain control of the nuclearity in addition to the
preparation of species containing different metal ions, i.e. heterometallic
complexes. Thus, in this manner, it is possible to build polymetallic systems
in a stepwise fashion having both homo and hetero-variants [97].
3.1 Homopolynuclear complexes
The homopolynuclear complexes synthesized by polytopic ligands allows
the coordination of metal ions through the reactive groups having donor
atoms such as nitrogen, oxygen or sulfur. This self-assembly approach
allows the rational preparation of linear double- and triple-stranded
oligonuclear complexes from mono- to di- and trinuclear species depending
on the molecular symmetry, coordination mode of the polytopic ligands and
the preferred coordination geometry of the metal ions as shown in figure 20
[98].
Chapter 1
Page 34
Figure 20: Homopolynuclear complexes.
The polynuclear complexes are prepared for different purposes. The pursuit
of the molecular magnetic materials requires an intelligent design of the
ligand which can organize the paramagnetic metal ions in a desired topology
and efficiently transmit electron exchange interactions between the metal
ions. This basic principle is remarkably supported by the work on the
magnetic properties of oxamato – bridged multimetallic coordination
compounds which was initiated by Kahn and coworkers in the late 1980’s
and then extended to the oxamidato – bridged analogues by Journaux and
Lioret in the late 1990’s. In this work, as discussed earlier, aliphatic or
aromatic group substituted bis(oxamato)- and related bis(oxamidato) –
copper(II) complexes were used as ligands, referred to as metal-organic
ligands (MOLs) for the preparation of multimetallic compounds [9, 94, 95].
Chapter 1
Page 35
The study of polynuclear complexes was initiated using the ligands like
oxalates which formed the homopolynuclear complexes. After 1990’s, a
great number of oxalate-bridged homopolynuclear complexes have been
synthesized and characterized till date [99]. These compounds are generally
obtained during the reaction between cationic complexes having potentially
free coordination sites and the oxalate anion. These types of polynuclear
complexes have general formula M(C2O4).nH2O where, M is a divalent
metal ion. These types of homopolynuclear compounds can be formed using
the polytopic ligands [100]. But, as discussed earlier, one of the challenges
in the field of polynuclear self – assembly of molecular organic – inorganic
material is the controlled and on the spot generation of well defined
molecular structures [101]. A high degree of structural organization can be
achieved through the multiple one- to three- binding of transition metals
[102]. Therefore, it is important to design the organic ligand together with
the proper choice of the metal ion, since the overall topology of the network
is influenced by match or mismatch of coordination of the linking metal ions
in addition to the binding properties of the bridging ligands [103, 104].
The oxalate – type ligands can be modified to bis – chelating coordination
ability which makes them a versatile choice for interconnecting metal ions
with different spins. The self – assembly of inorganic structures
encompassing bridging oxalate-type units have produced different types of
frameworks, which include 1D-chains, 2D-layer and 3D-networks bearing
the same types of metal ions [105].
Chapter 1
Page 36
3.2 Heteropolynuclear complexes
The synthesis of heterometallic complexes is known to be complicated. A
one-pot procedure involving the reaction of two different metal ions with the
ligand anion produces a mixture of compounds [106]. In order to overcome
this difficulty, an alternative synthetic strategy (MOL) has been developed
which consists the use of mononuclear complexes as ligands towards the
second metal ion.
Plenty of work on the well – recognized ‘metal complex as ligands’
approach has been done till date [51]. F. Lioret and coworkers reported the
homo- and heteroleptic anionic complexes of chromium(III) with one or
more potentially bridging groups such as [Cr(salen)(C2O4)]-
,[Cr(acac)2(C2O4)]- and [Cr(C2O4)3]
3- which are particularly useful designing
heterometallic complexes with interesting magnetic properties [107].
M.C. Dul and coworkers explained the molecular–programmed self-
assembly of metal-organic ligands with the free carbonyl oxygen which
allows self-assembled mono-,di-,and trinuclear square planar or octahedral
complexes to be used as MOLs toward other metal ions (M(II) = Cu, Ni, Co,
Mn, Fe, Zn) as shown in figure 21. This molecular self-assembly approach
allows the rational preparation of polynuclear complexes as well as
coordination polymers of varying nuclearity, topology, and dimensionality,
depending on the coordination mode of MOLs and coordinated metal ions
[72].
Chapter 1
Page 37
Figure 21: Heteropolynuclear complexes.
H. Adams and coworkers synthesized the homodinuclear complexes from
ligand (L) by the reaction of sodium 2,6-diformyl-4-methylphenolate and
1,3-diamine propane as shown in figure 22 [108]. The Schiff base complex
[Na2(L)] formed readily underwent transmetallation by Zn(ClO4)2.6H2O to
produce Zn2(L) (ClO4)2.2H2O.
Figure 22: Polydentate ligand used for polynuclear complexes.
Whereas, the heterodinuclear complexes [MAMB(L)]2+
, where MA = Ni2+
, MB
= Mn2+
, Fe2+
, Co2+
, Cu2+
, Zn2+
were prepared by two step synthesis, based on
Chapter 1
Page 38
the reaction of metal acetates with mononuclear nickel complex. In the first
step, the mononuclear nickel complex was formed, one of the coordination
compartments was blocked by protonation of inner penalty groups. In the
second step acetate ions deprotonated the phenolate groups and made it
available for the further coordination. So, by the modification of the
synthetic method the homodinuclear and heterodinuclear complexes from
same Schiff base ligands can be formed.
E.Q. Gao and coworkers also used ‘complex as ligand’ approach with an
intention to prepare polynuclear species. Many oxamido-bridged
polynuclear complexes were prepared by using mononuclear Cu(II)
complexes of some N,N- bis(coordinating group substituted) oxamides such
as [Cu(oxpn)] and [Cu(obze)]2 as ligands as shown in figure 23. The
diamines and dioxalates are used for the preparation of the mononuclear
complexes. The mononuclear complexes with free coordinating sites were
used as MOLs for the preparation of the dinuclear complexes [109].
Figure 23: Mononuclear complexes used as MOLs.
The mononuclear complexes as given in figure 23 have free oxalate sites for
the further coordination. The mononuclear complexes with variation of
Chapter 1
Page 39
different ligands with the substitutions give different types of dinuclear
complexes [110]. The dinuclear complexes prepared from the above method
are different from which they reported the dinuclear Cu(II)-M(II) (M=Cu,
Ni, Mn) complexes as shown in figure 24 [111].
Figure 24: Dinuclear complexes of MOLs
Some other types of metal organic ligands have been designed using a ligand
containing number of potential sites from which all cannot contribute in the
coordination, the monotopic complexes formed from these types of ligands
can act as precursors. The mononuclear complexes of transition metals
prepared from 6-amino-2-thiouracil containing the amine group as unutilized
functionality is shown in figure 25. These types of mononuclear complexes
can be modified for further reaction to form the polynuclear complexes
[112].
Chapter 1
Page 40
M(II)-(6-amino-2-thiouracil)
Figure 25: Mononuclear with active sites.
From amongst many methods for the preparation of polynuclear complexes,
Y. Sunatsuki and coworkers implemented two methods. The first method (1)
in which, one kind of metal complex contains simultaneous donor and the
acceptor ability for the further reaction and construct the assembly structure.
The second method (2) in which, two kinds of metal complexes contain
simultaneous donor and the acceptor ability for the further reaction. The
second method is successfully used in the preparation of molecular magnetic
materials [113].
The representative example of first method is given as Cu(II) complexes
with multidentate Schiff-base ligands containing imidazole groups with both
donor and acceptor abilities in the formation of coordination bonding. Under
the acidic condition condensation of 4-formylimidazole and N,N-
dimethyldiethylenetriamine form compound 1 as shown in figure 26.
Chapter 1
Page 41
Figure 26: Mononuclear MOL.
Compound 1 reacts with itself in the presence of the base to give imidazolate
bridge species 2 as shown in figure 27. Here the compound 1 acts as metal
organic ligand and react itself to form the homodinuclear complex [114].
Figure 27: Homodinuclear complex from MOLs.
Brewer and coworkers isolated a mono-deprotonated species 3 which is the
mononuclear complex with the free amine of the ring skeleton [115]. This
complex functions as monodentate ligand complex i.e. metal complex as
ligand and react with the other mononuclear complex,
tetraphenylporphyrinato Fe(III) to give linear trinuclear complex 4 [116].
Chapter 1
Page 42
Figure 28: Heterotrinuclear complex from mononuclear MOLs.
The same concept was used to synthesize the trinuclear complex as shown in
figure 29. The mononuclear complex of Cu(II) ion of unsymmetrical
tetradentate ligands containing an imidazole group per molecule were
synthesized [117]. The mononuclear complex of Cu(II) was self – assembled
to the mononuclear complex of iron to form various polynuclear complexes
such as compound 5.
Figure 29: Heterotrinuclear complex.
Here, Y. Sunatsuki have used precursor complexes which act as MOLs and
form a variety of the heteropolynuclear complexes with metal variants [118].
A. Jana and coworkers reported the solvent dependent reaction of
mononuclear complexes of Cu(II) and N,N’-ethylenebis(3-
ethoxysalicylaldimine) with nickel(II) perchlorate in 1:1 ratio in acetone
produces the trinuclear copound [(CuIIL)2Ni
II(H2O)2](ClO4)2. On the other
Chapter 1
Page 43
hand, reaction with same reactants in the same ratio with the methanol
produces the pentanuclear compound [(CuIIL)2Ni
II(H2O)2](ClO4)2
.2[(CuIIL(H2O)][103].
The new concept of the coordinated amine reacts with the free aldehyde
group of the mononuclear complex that form the trinuclear complexes by the
Schiff base reaction between the two mononuclear complexes was reported
by S.Deeplathaand coworkers. The copper(II) complex of 3,4-dihydroxy
benzaldehyde as the ligand system in which the aldehyde group could be
modified to attach additional nitrogen donor sites through Schiff base
condensation has been attempted by S. Deeplatha and coworkers [119]. They
formed the trinuclear complexes using the method (2); the two kinds of
metal complexes having reactive sites. In first step 2,2’-bipyridyl 3,4-
dihydroxo benzaldehyde monometallic cupric(II) complex was allowed to
react with diethylenetriamine complexes of Cu(II), Zn(II) and Ni(II) to
afford trinuclear complexes as shown in figure 30.
Figure 30: Heterotrinuclear complex.
Chapter 1
Page 44
4. MAGNETIC INTERACTION IN POLYNUCLEAR
COMPLEXES
Magnetic properties of materials have been utilized over years in mechanical
applications such as electric motors, electric generators as well as in
communication technologies such as television and telephones. More
recently, magnetism has found extensive application in the area of data
storage and processing, from magnetic tape to floppy discs and computer
hard drives [120].
The most usable types of magnets are either ferro- or ferrimagnets, each of
which has a characteristic Curie temperature, below the Curie temperature it
shows its magnetic properties. Such magnets can be pure metals, alloys,
metal oxides or molecular magnets [121]. The spins on the magnetic centers
are interacting with their neighbors in the three dimensional lattice of a
conventional magnet and their spontaneous magnetization relies on the
alignment of a very large number of spin centres in the bulk material. The
bulk magnetic structure is divided into many magnetic domains within each
of which the spins are aligned in ferromagnetic materials. When the different
domains having different alignment directions such that their overall
magnetic moments cancels out, the materials are classified as
antiferromagnetic materials [122].
Traditional magnetic materials consist of two- and three-dimensional
structures of transition metal or lanthanide metal containing spin units.
These types of materials are generally prepared at very high temperatures
using metallurgical methods. In contrast to traditional magnetic materials,
molecular magnets are organic or inorganic / organic hybrid materials
consisting either metal with spin units or organic radical containing spin
Chapter 1
Page 45
units [123]. These magnetic materials are conveniently prepared at low
temperatures. In addition to this, such materials can possess better optical
properties and the combination of magnetic properties with other properties
like mechanical, electrical and / or optical properties makes them easily
processable.
In the last two decades, an increasing interest in polynuclear complexes
containing ligand structures capable of holding two or more metal centers in
close proximity and act as single molecular magnets has been observed. The
field of molecular magnetism exhibited a rapid development in the last two
decades with a particular emphasis on heteropolymetallic complexes. The
magnetic interaction between two nonequivalent paramagnetic centers may
lead to situations which cannot be encountered in species containing only
one kind of center [124].
The occurrence of magnetic interactions in coordination compounds is
because of the incompletely filled d-orbitals in addition to the arrangement
of electrons. An electron acts as a tiny bar magnet with a negative charge. If
the magnetic fields of two or more electrons in the atoms of a molecule are
parallel then that molecule becomes magnetic.
Normally, the magnetic fields of electrons in atoms cancel each other and the
atom cluster appears as non-magnetic. But in some molecules, because of
some special type of bonding between its atoms (i.e. bridge between atoms),
the magnetic fields of two or more electrons in the molecule becomes
parallel and these types of molecules exhibit molecular magnetism. The field
strength of a molecular magnet depends on the number parallel electron
magnetic fields in the molecule [125, 126].
Chapter 1
Page 46
4.1 Types of Magnetic behavior
The origin of magnetism lies in the orbital and spin motion of electrons and
their interactions with each other. Atoms, ions, molecules and solids having
unpaired electrons when brought under the influence of a magnetic field,
develop a net magnetization because of very strong interaction between the
moments of neighboring atoms [127, 128]. In some materials there is no
collective interaction between the atomic magnetic moments. The magnetic
behavior can be classified as follows:
I. Diamagnetism
Systems having only paired electrons are described as diamagnetic. Most
organic molecules are diamagnetic. In this case, magnetic susceptibility is
usually independent of the temperature and the strength of the applied field.
These substances when exposed to a magnetic field, a negative
magnetization is produced and the susceptibility will also negative so, they
will be weakly repelled by the field [129].
II. Paramagnetism
Systems having one or more unpaired electrons are called paramagnetic. The
paramagnetic substance possesses a net magnetic moment and gets attracted
to a magnetic field due to a partial alignment of the atomic magnetic
moments in the direction of the field as shown in figure 31. Such substances
have a net positive magnetization and positive susceptibility [130]. The
individual magnetic moments do not retain any magnetization in the absence
of an externally applied magnetic field [131].
Chapter 1
Page 47
Figure 31: Spin alignments in paramagnets.
III. Ferromagnetism
The ferromagnetic substance are type of paramagnetic substances which
have magnetic interactions between neighboring paramagnetic centers such
that the individual moments are aligned parallel to each other as shown in
figure 32 and there will be a net increase in the magnetic moment. The
ferromagnetic substance is usually divided into domains to minimize its total
free energy leading to spontaneous magnetization arises in each domain
even in the absence of a magnetic field. Its magnetic susceptibility is
positive and very large. However, above its Curie temperature the interaction
is no longer strong enough to maintain the moments in alignment, and the
substances then behave as simple paramagnetic material [132].
Figure 32: Spin alignments in ferromagnets.
Chapter 1
Page 48
IV. Antiferromagnetism
When the magnetic interactions between paramagnetic centers lead to an
antiparallel alignment of the moments, the paramagnetic substance is said to
exhibit antiferromagnetism as shown in figure 33. Because of the complete
compensation of the magnetic moments, the substance does not show any
spontaneous magnetization. Above its Neel temperature, an antiferromagnet
behaves as a paramagnet [132].
Figure 33: Spin alignments in antiferromagnets.
V. Ferrimagnetism
Substances where the magnetic moments are aligned antiparallel as shown in
figure 34, but there is an incomplete compensation of the spins are termed
ferrimagnets. This usually results either from unequal numbers of spins
being oriented in the two directions, or when the two types of spin centers
have different numbers of unpaired electrons. Ferrimagnets exhibit
spontaneous magnetization as in the case of ferrromagnets [74, 133].
Chapter 1
Page 49
Figure 34: Spin alignments in ferrimagnets.
A detailed description of the magnetic properties and behavior of different
materials will be provided in chapter 3.
4.2 History of magnetism in polynuclear complexes
In 1704, a new blue pigment useful for paints and fabrics was discovered by
Berlin Draper. This discovery was reported anonymously in 1710 [134] and
the method was described in 1724 by Woodward and Brown [135, 136]. This
pigment, now called Prussian blue (or Berlin Blue) was the first synthetic
coordination compound. The history of its discovery and the various theories
about its nature and the origin of its bright color were reviewed recently in
the context of the development of chemical ideas in the 18th
and 19th
centuries [137, 138]. The crystal structure of Prussian Blue
FeIII
4[FeII(CN)6]3.14H2O was determined by Buser, Ludi and Gudel in 1972
[139].
In 1928, Davidson and Welo published the first magnetic investigation of the
parent species Prussian Blue. They measured the magnetic susceptibility at
three temperatures in the range of 200 to 300 K [140]. An extension of this
Chapter 1
Page 50
early work on magnetic properties of Prussian Blue was done in 1940. In
1968, Prussian Blue was shown to be a ferromagnet with Tc = 5.6 K [141].
The polynuclear complexes exhibit many interesting magnetic properties
owing to bridging ligands as well as the intermetallic bonding. The magnetic
properties of dinuclear complexes have been studied over many years [142].
E.F. Hasty and coworkers reported the binuclear copper(II) Schiff base
compounds of salicylaldehyde with aromatic polyamines in 1978. The
binuclear complexes have the iminobenzene moiety bridging between the
two metal ions. The compound Cu2(sal-m-phenylinediamine) had an
antiferromagnetic interaction (J= -1.5 cm-1
). The compound with nickel
metal also showed an antiferromagnetic interaction [124].
O’ Conner and coworkers also reported a series of dinuclear complexes
based on new binucleating ligands derived from the condensation of
salicylaldehyde, pyridine-2-carboxaldehyde. The first example of
ferromagnetic coupling in dinuclear complexes was observed for compound
shown in figure 35, with J value of about +17 and +80 cm-1
[143].
Figure 35: Homodinuclear complex with ferromagnetism.
In 1987, Mallahi and coworkers reported the binuclear complexes of copper
with ligands having various exogenous donors (OH, N3, OCN). These
Chapter 1
Page 51
dinuclear complexes exhibit strong antiferromagnetic nature with OH bridge
while the species with OCN bridge show a weak antiferromagnetic coupling.
The magnetic properties of the homonuclear complexes are studied
extensively since a long but, interest in magnetic properties of
heterodinuclear complexes has increased in the recent times. Many reviews
on the magnetic properties of dinuclear and polynuclear complexes of
transition metal complexes are well documented [99, 144]. The interest in
magnetic properties of coordination polymers and clusters is also emerging
these days. The magnetic properties of asymmetric heterodinuclear
complexes containing the µ-Oxo-bis(p-acetato)dimetal was reported in 1992
by Hotzelmann and coworkers. Bulk magnetic properties of all the
compounds have been studied in the temperature range 4.2 – 298 K. It was
found that the spins of the two paramagnetic metal ions are either
intramolecularly antiferromagnetically or ferromagnetically coupled [142].
The oxalate-bridged dinuclear complexes of Cr(III)-M(II) (M=Cu, Ni, Co,
Fe, Mn) complexes as shown in figure 36 were synthesized and the magnetic
properties were investigated by Ohba and coworkers. The magnetic
investigations of these compounds in the temperature range 4.2–300 K
reveal a ferromagnetic interactions between the Cr(III) and M(II) ions for all
the complexes [145].
Chapter 1
Page 52
Cr(III)-M(II) (M=Cu, Ni, Co, Fe, Mn)
Figure 36: Heterodinuclear complex with ferromagnetism.
The polynuclear complexes of different transition metals and ligands have
generated interesting magnetic properties [146]. The dinuclear complexes of
nickel(II) containing triethylenetetramine and tricyanomethanide exhibits a
ferromagnetic coupling. But, the dinuclear complexes synthesized from
polytopic ligands like 2-[N-bis-(2-pyridylmethyl) aminomethyl]-4-methyl-6-
[N-(2 pyridylmethyl) aminomethyl]phenol as shown in figure 37 exhibited
the antiferromagnetic coupling [147].
Figure 37: Homodinuclear complex with antiferromagnetism.
Chapter 1
Page 53
The synthesis, structure and magnetic properties of a dinuclear Co(II)
complex of a tridentate verdazyl radical was reported by M. T. Lemaire and
others. The magnetic susceptibility data of the dinuclear complexes
suggested ferromagnetic interactions at low and high temperatures with
J= +20 cm-1
. Rodriguez-Dieguez and coworkers reported the
antiferromagnetic interaction occurs in dinuclear complexes of Co(II) with
pyrimidine-2-carboxylato bis bidentate ligands [99, 148].
The dinuclear complexes of iron(II) and iron(III) are also synthesized and
well characterized. The dinuclear complexes of iron(II) with dicarboxylate
and 2,3-lutidine was reported by Sidorov and others. These homodinuclear
complexes of iron(II) are found to be antiferromagnetic as shown in figure
38 [149].
Figure 38: Homodinuclear complex with antiferromagnetism.
The dinuclear complexes of iron(II) with pyrimidine-2-dicarboxylato bis
bidentate ligands also exhibits the antiferromagnetism. Kil Sik Min and
coworkers reported the ferromagnetic interactions at low temperatures in
dinuclear complexes of Iron(II) with tris(2-pyridylmethyl)amine and 2,3,5,6-
tetrahydroxy-1,4-benzoquinonate [150].
The magnetic properties of mononuclear as well as dinuclear complexes of
manganese are found to be much interesting. Sujin Han reported a weak
Chapter 1
Page 54
ferromagnetism in mononuclear manganese complex [151]. The structure
and magnetic properties of manganese(III) complexes with pentaanioc
pentadentate ligands including alkoxo, amido and phenoxo donors were
reported by Stoicescu and coworkers [152]. All the complexes exhibit the
antiferromagnetism at low temperatures with J value -3.6 cm-1
. Ribas and
coworkers reported the trinuclear complexes with oxo-manganese center
exhibits the antiferromagnetism at lower temperature [153].
Ferromagnetic CuII
4, CoII
4, NiII
6 azido complexes derived from di-2,6-(2
pyridylcarbonyl) pyridine was reported by Georgopoulou and others. The
polynuclear complexes prepared from all these three transition metals
exhibited the ferromagnetic interactions. Hence, the magnetic interaction is
different according to the transition metals and ligands used [154].
5. LITERATURE SURVEY
The polynuclear complexes of transition metals are synthesized and
extensively characterized till date. Many excellent papers have been
published during the last three decades on the preparation and properties of
polynuclear complexes and the most relevant results are reviewed here [155,
156]. The applications of the polynuclear complexes and dinuclear
complexes are also found in different fields. The preparation of the
polynuclear complexes with different methodologies are also well
documented [157, 158]. A brief literature survey according to the application
in different fields and the methodologies for the preparation of dinuclear
complexes is reported here. The dinuclear complexes with bridged and
aliphatic ligands started from the late ninteenth century. A good deal of work
was done on binuclear complexes in the late nineteenth century including,
Chapter 1
Page 55
Fremy (1852), Gibbs (1876), Vortmann (1898), Jorgensen (1894) and
Mascetti (1900). A number of papers by Werner (1898-1918) greatly
expanded the scope of the field. The first mention of trinuclear complex was
in 1908 by the German chemist Weinland. In 1970, the first homodinuclear
complexes with macrocyclic ligands were prepared by Robson with template
reaction so, called Robson type complexes [82]. From that time Robson type
complexes have been synthesized and characterized. The preparation of
dinuclear iron(III) complexes with aromatic and aliphatic ligands were
reported by K. S. Murray in 1974 [156].
The dinuclear complexes with different metal ions prepared by ‘metal
complexes as ligand’ stretagy are the most successful. F. Lioret and
coworkers reported the homo- and heteroleptic anionic complexes of
chromium(III) with one or more potentially bridging groups such as
[Cr(salen)(C2O4)]-
,[Cr(acac)2(C2O4)]- and [Cr(C2O4)3]
3- are particularly
useful for the design of heterometallic complexes of interest in magnetism
[159]. M.C. Dul and coworkers explained the molecular–programmed self-
assembly of metal-organic ligands with the free carbonyl-oxygen which
allows self-assembled mono-, di-, and trinuclear square planar or octahedral
complexes to be used as MOLs toward other metal ions (M(II) = Cu, Ni, Co,
Mn, Fe, Zn) [72]. The heterodinuclear complexes [MAMB(L)]2+
, where MA =
Ni2+
, MB = Mn2+
, Fe2+
, Co2+
, Cu2+
, Zn2+
have been prepared by two step
synthesis, based on the reaction of metal acetates with mononuclear nickel
complex by J. Lisowski in 1999. Brewer and coworkers synthesized the
tinuclear complexes of unsymmetrical tetradentate ligands containing an
imidazole group per molecule by using the mononuclear precursor [115].
Chapter 1
Page 56
A variety of homo and heterodinuclear Schiff base complexes of transition
metal ions were used as catalysts by B. Carbezon and coworkers. Ligtenbarg
and others reported the dinuclear complexes of copper(II) ions used
successfully in hydroxylation of phenol in 1998. A review on visible light
promoted reactions catalysed by tansition metal complexes by A. Inagaki
and coworkers [160]. Daniel Seidel reported the dinuclear copper complexes
as asymmetric catalyst. Simon-Manso and Kubiak reported the dinuclear
nickel complexes as catalyst for electrochemical reduction of carbondioxide
[161]. V. Lozan and coworker reported the dinuclear nickel(II) and
palladium(II) complexes in combination with co-catalyst as highly active
catalyst for the vinyl / addition polymerization of norbornene.
The synthesis and magnetic properties of dinuclear as well as polynuclear
complexes of oxamato-bridged coordination compounds was initiated by
Kahn and coworkers in the late 1980s and then extended to the
oxamidatobridged analogues by Journaux and Lioret in the late 1990s [94].
In this work, aliphatic or aromatic group substituted bis(oxamato)- and
related bis(oxamidato)-copper(II) complexes were used as ligands [162]. In
1987, Mallahi and coworkers reported the binuclear complexes of copper
with ligands with various exogeneous donors (OH, N3, OCN). The magnetic
properties of asymmetric heterodinuclear complexes containing the µ-Oxo-
bis(p-acetato)dimetal was reported in 1992 by Hotzelmann and coworkers.
O’ Conner and others have reported a series of dinuclear complexes based
on new binucleating ligands derived from the condensation of
salicylaldehyde, pyridine-2-carboxaldehyde [163]. This was the first
example of ferromagnetic coupling in dinuclear complexes observed for
compound with J value of about +17 and +80 cm-1
. The oxalate-bridged
Chapter 1
Page 57
dinuclear complexes of Cr(III)-M(II) (M=Cu, Ni, Co, Fe, Mn) complexes
were synthesized and the magnetic properties were investigated by Ohba and
coworkers [145]. The synthesis, structure and magnetic properties of a
dinuclear Co(II) complex of a tridentate verdazyl radical was reported by M.
T. Lemaire and coworkers [92]. Rodriguez-Dieguez and others reported the
antiferromagnetic interaction occurring in dinuclear complexes of Co(II)
with pyrimidine-2-carboxylato bis bidentate ligands. Nishida and coworkers
have reported the copper (II) complex shows weak anti ferromagnetic
coupling [164]. The heptadentate polybenzimidazole ligand 2,6
bis[benzimidazoylmethyl) aminomethyl]-p-cresol and its copper(II)
complexes with pyridine and pyrazole bridges have been reported by McKee
and coworkers [165].
5.1 Present work
I. Scope and interest
The chemistry of metal complexes including ordinary complexes, chelates
and mixed ligand complexes has been extensively studied till date for their
roles as biological models as well as a wide range of physicochemical
properties. In order to fiddle with the properties of the complexes originating
due to metal ions, polynuclear complexes with inclusion of different metals
is imperative. Mixed-metal complexes are a class of compounds which can
have properties that are not present in ordinary complexes. Interest in these
kind of complexes stems from their bioinorganic relevance and magnetic
properties. Numerous homopolynuclear complexes have been prepared
using polydentate ligands in which some of the donor atoms are unable to
coordinate with the same metal ions due to steric factors and form the
Chapter 1
Page 58
multinuclear complexes of the same metal ion. Synthetic routes leading to
heteropolynuclear complexes with pre-established structures and properties
has remained a challenge for synthetic chemists. A one - pot procedure for
template synthesis of heteromettallic complexes has not been well
established yet. This difficulty has been overcome to some extent using a
well-recognized approach ‘Complexes as Ligands’. We report here the
synthesis of dinuclear complexes via novel route the inter – complex
reaction is capable of opening a new era in the preparation of complexes
with a lot more variations. The magnetic interactions in these types of
polynuclear complexes are quite interesting and can be used as magnetic
materials.
II. Overview
The present work is to study the mixed metal complexes prepared by the
novel method i.e. ‘complexes as ligands’. A series of complexes were
synthesized by this method and then characterized by analytical techniques.
The work is divided into five chapters.
The first chapter of the thesis includes an extensive literature survey. This
chapter describes the general introduction and background of transition
metal complexes, polytopic ligands and polynuclear complexes, metal
organic ligands (MOL’s) as well as the magnetic interactions in metal
organic ligands based complexes.
Chapter 2: Synthesis and characterization of dinuclear complexes of
salicylaldehyde and 2–aminophenolwith Zn(II), Mn(II) and Fe(II).
This chapter will deal with the general information of the complexes of the
particular ligands. Synthetic method for the all the nine dinuclear complexes
Chapter 1
Page 59
and various characterization techniques and methods employed to
characterize the synthesized compounds will be discussed here.
Physicochemical data and results from various techniques like infrared
spectra, TGA, electronic spectra, magnetic properties, 13
C NMR spectra, 1H
NMR spectra, mass spectra and powder X – ray diffraction data will also be
discussed. A brief explanation of absorption and emission spectrometry are
reported here.
Chapter 3: Synthesis and characterization of dinuclear complexes of
salicylaldehyde and 2 – aminophenol with Co(II), Ni(II) and Cu(II).
This chapter contains general synthetic method for nine dinuclear complexes
of transition metals viz. Co(II), Ni(II), Cu(II). The physicochemical data and
results from various techniques like infrared spectra, thermogravimetric
analysis, electronic spectra, mass spectra and detailed study of magnetic
properties of all the synthesized compounds will be discussed. The
molecular magnetic theory and the methods used to study the magnetic
properties for the interpretations of the nature of compounds either
ferromagnetic or antiferromagnetic is described.
Chapter 4: Synthesis and characterization of dinuclear complexes of
o–vanillin and 2–aminophenol with Z (II), Mn(II) and Fe(II).
This comprises general information on complexes of o–vanillin. The general
synthetic method for homo and hetero dinuclear complexes of transition
metals Zn(II), Mn(II) and Fe(II) with o-vanillin and 2-aminophenol. The
chapter includes study similar that of the second chapter carried out with a
new series. Theories of various methods of the mass spectrometry which can
be used for structure elucidation is described here.
Chapter 1
Page 60
Chapter 5: Synthesis and characterization of dinuclear complexes of
o–vanillin and 2–aminophenol with Co(II), Ni(II) and Cu(II).
In this chapter the general methods for the preparation of dinuclear
complexes and characterization data are discussed as like that of the third
chapter. The molecular mechanical methods used to identify the most stable
structure is described.
Chapter 1
Page 61
6. REFERENCES
[1] P. Atkins, T. Overton, J. Rourke, M. Weller, F. Armstron, Shriver &
Atkins Inorganic chemistry, Freeman and Company, New York, 2006.
[2] K.C. Gupta, A.K. Sutar, Coordination Chemistry Reviews, 252 (2008)
1420-1450.
[3] L. Kathryn, Haas, K.J. Franz, Chem.Rev., 109 (2007) 4921-4960.
[4] S. Kumar, D.N. Dhar, P.N. Saxena, Journal of Scientific & Industrial
Research, 68 (2009) 181-187.
[5] V. D. Bhatt, S.R. Ram, Chemical Sciences Journals, 63 (2012) 1-11.
[6] E .Keskioglu, A.B. Gunduzalp, S. Cete, Spectrochim.Acta, 70A (2008)
634-640.
[7] S.J. Lippard, J.M. Berg, Principles of Bioinorganic Chemistry, University
Science Books, Mill Valley, 1994.
[8] D. Zhao, D.J. Timmons, D. Yuan, H. Zhou, Accounts of chemical
research, 44 (2010) 123–133.
[9] O. Kahn, Molecular Magnetism, VCH Weinheim, 1993.
[10] W. U. Malik, R.D. Madan, G.D. Tuli, Selected topics in inorganic
chemistry, S.Chand group, India, 1999.
[11] S. Prakash, G.D. Tuli, S.K. Basu, R.D. Madan, Advanced Inorganic
Chemistry, S.Chand, India, 2006.
[12] R. Gopalan, Concise coordination chemistry, Vikas Publishing Pvt.
Ltd., India, 1996.
[13] T.J. Meyer, T. J. Pure Appl. Chem. , 58 (1986) 1193–1206.
[14] J.E. Hurrey, E.A. Keiter, R.L. Keiter, O.K. Medhi, Inorganic chemistry:
Principle of stucture and reactivity, Durling Kinderaley, India, 2008.
[15] H. Schiff, Annalen, 131 (1864) 118-126.
[16] S.A. Sadeek, M.S. Refat, J. Korean, Chem. Soc., 50 (2006) 107-113.
[17] A. Bigotto, V. Galasso, G. Dealti, Spectrochim. Acta, 28A (1972) 1581-
1593.
[18] N. Chitrapriya, V. Mahalingam, L.C. Channels, M. Zeller, F.R.
Fronczek, K. Natarajan, Inorg. Chim. Acta, 361 (2008) 2841-2851.
[19] V.D. Bhatt, A. Ray, Intern. J. Polymeric Mater, 49 (2001) 355-366.
Chapter 1
Page 62
[20] S. Kumar, D. N. Dhar, P.N. Saxena, Journal of Scientific & Industrial
Research 68 (2009) 181-187.
[21] M.P. Suh, H.J. Park, T.K. Prasad, D.-W. Lim, Chem. Rev. , 112 (2012)
782–835.
[22] A.I. Vogel, A Text Book of Quantitative inorganic Analysis, Longmans,
London, 1989.
[23] S. Wang, Coordination Chemistry Reviews, 215 (2001) 79–98.
[24] Z. Guan, P.M. Cotts, E.F. McCord, S.J. McLain, Science, 283 (1999)
2059-2071.
[25] K.C. Gupta, A.K. Sutar, Coordination Chemistry Reviews 252 (2008)
1420–1450.
[26] B.L. Small, M. Brookhart, A.M.A. Bennett, J. Am. Chem. Soc., 120
(1998) 4049-4052.
[27] T.M. Trnka, R.H. Grubbs, Acc. Chem. Res., 34 (2001) 18-29.
[28] Z. Xi, H. Wang, Y. Sun, N. Zhou, G. Cao, M. Li, J. Mol. Catal. A
Chem., 168 (2001) 299-309.
[29] H.Y. Zhou, J. Cheng, S.J. Lu, H.X. Fu, H.Q.Wang, J. Organomet.
Chem., 556 (1998) 239-248.
[30] J. Tsuji, Palladium Reagents and Catalysts, Wiley, New York, 1996.
[31] E.J. Carey, Y. Bo, J.B. Peterson, J. Am. Chem. Soc., 120 (1998) 13000.
[32] Y. Kolmura, T. Katsuki, Tetrahedron Lett., 42 (2001) 3339.
[33] C. Tarro, S. Kato, A. Evenzahav, S.H. Bossrnam, J.K. Barton, M.J.
Turro, J. Inorg. Chim. Acta., 243 (1996) 101-113.
[34] M.S. Sigman, E.N. Jacobson, J. Am. Chem. Soc., 120 (1998) 5315.
[35] T.L. Terry, A. Yeung, S.C. Albert, Coordination Chemistry Reviews
248 (2004) 2151–2164.
[36] Y.Z. Hang, L.Z. Gong, X.M. Feng, W.H. Hu, Z. Li, A.Q. Mi,
Tetrahedron, 53 (1997) 14327.
[37] K. Mikani, M. Terada, H. Matsuzawa, Angew. Chem. Int., 41 (2002)
3554.
[38] N.O. Komatsuzaki, R. Katoh, Y. Himeda, H. Sugihara, H. Arakawa,
K.Kasuga, Bull. Chem. Soc. Jpn., 76 (2003) 977-988.
Chapter 1
Page 63
[39] M. Lubben, R. Hage, A. Meetsma, K. Bijma, B.L. Feringa, Inorg.
Chem., 34 (1995) 2217.
[40] A.G.J. Ligtenbarg, E.K. Beuken, A. Meetsma, N. Veldman,
W.J.J.Smeets, A.L. Spek, B.L. Feringa, J. Chem. Soc., (1998) 163.
[41] R. J. Kupplera, D. J. Timmonsb, Q.-R. Fanga, J.-R. Li, T. A. Makala, M.
D. Younga, D. Yuana, D. Zhaoa, W. Zhuanga, H.-C. Zhoua, Coordination
Chemistry Reviews 253 (2009) 3042–3066.
[42] D. Gatteschi, Journal of Alloys and Compounds 317-318 (2001) 8-12.
[43] L.V. Azaroff, J.J. Brophy, Electronic Processes in Materials, McGraw-
Hill Book Company, New York, 1963.
[44] R.M. Bozorth, Ferromagnetism, Wiley-IEEE Press, New York, 1993.
[45] G. Aromía, L. A. Barriosa, O. Roubeaub, P. Gameza, Coordination
Chemistry Reviews, 255 (2011) 485-546.
[46] J. Taylor, The high temperature synthesis of transition metal oxo-
carboxylate polynuclear complexes, in, Victoria University of Wellington,
Wellington, 2007.
[47] L. Thomas, F. Lionti, R. Ballou, D. Gatteschi, R. Sessoli, B. Barbara,
Nature, 383 (1996) 145.
[48] G. Christou, A Molecular Approach to Nanoscale Materials, in: Single-
Molecule Magnets, Tasmania, Hobart, 2007.
[49] M. Affronte, F. Troiani, A. Ghirri, A. Candini, M. Evangelisti, S.
Carretta, P. Santini, G. Amoretti, S. Piligkos, G. Timco, R.E.P. Winpenny,
Polyhedron, 24 (2005) 2562.
[50] M. N. Leuenberger, D. Loss, Nature, 410 (2004) 789.
[51] D. Venegas-Yazigi, D. Aravena, E. Spodine, E. Ruiz, S. Alvarez,
Coordination Chemistry Reviews, , 254 (2010) 2086-2095.
[52] A.R. Paital, W.T. Wong, G. Aromı, D. Ray, Inorg. Chem., 46 (2007)
5727-5733.
[53] D. J. Evans, C.J. Pickett, Chem. Soc. Rev, 32 (2003) 268-275.
[54] M. Ruben, Synthesis of Molecular Magnets, in: Institute of
Nanotechnology, Germany, 2007.
[55] S. Blundell, A of Magnetism in Condensed Matter, Oxford University
Press, London, 2001.
Chapter 1
Page 64
[56] E.W. Lee, Magnetism, An Introductory Survey, Dover Publications,
New York, 1970.
[57] H.L. Singh, M. Sharma, A.K. Varshney, Chem Res Commun, 131
(1998) 110376.
[58] V. Mishra, D. K. Saksena, M. C. Jain, Synth React Inorg Met Org
Chem, 17 (1987) 987-1002.
[59] S. Gaur, Asian J Chem, 15 (2003) 250-254.
[60] B. Dash, P. K. Mahapatra, D. panda, J Indian ChemSoc, 61 (1984)
1061-1064.
[61] C.N.R. Rao, P.V. Rao, G.V. Reddy, M.C. Ganorkar, Indian J Chem, 26A
(1987) 887-890.
[62] P. Mishra, P.N. Gupta, A.K. Shakya, J Indian Chem Soc, 68 (1991) 539-
541.
[63] R. Ramesh, M. Sivagamsundari, Synth React Inorg Met Org Chem, 33
(2003) 899-910.
[64] N.C. Bhardwaj, R.V.Singh, Indian J Chem, 33A (1994) 423-425.
[65] Z.H. Chohan, H. Prevez, K.M. Khan, A. Rauf, G.M. Maharvi, C.T.
Supuran, JEnzy Inhib Med Chem, 19 (2004) 85-89.
[66] H. Zhang, D.W. Norman, T. M. Wentzell, A.M. Irving, J.P. Edwards,
Trans Met Chem, 30 (2005) 63-68.
[67] K.S. Siddiqi, R.I. Kureshy, N.H. Khan, S. Tabassum, S. Zaidi, Inorg
Chem Acta, 151 (1988) 95-100.
[68] K.P. Sharma, V.S. Jolly, P. Pathak, Ultra Sci Phys Sci, 10 (1998) 263-
266.
[69] Nial J. Wheate, J.G. Collins, Coordination Chemistry Reviews, 241
(2003) 133-145.
[70] S. Rafique, M. Idrees, A. Nasim, H. Akbar, A. Athar, Biotechnology and
Molecular Biology Reviews, 5 (2010) 38-45.
[71] L.J. Ignarro, Nitric Oxide: Biology and Pathobiology, Academic Press,
San Diego, 2000.
[72] M.C. Dul, E. Pardo, R. Lescouezec, Y. Journaux, J. Ferrando-Soria, R.
Ruiz-García, J. Cano, M. Julve, F. Lloret, D. Cangussu, C.L.M. Pereira,
H.O. Stumpf, J. Pusan, C. Ruiz-Perez, Coordination Chemistry Reviews,
254 (2010) 2281-2296.
Chapter 1
Page 65
[73] V.D. Bhatt, ICAIJ, 3 (2008) 60-64.
[74] K.C. Mondal, Syntheses, Structures and Properties of f and d-f
Complexes using O-vanillin-derived Schiff base Ligands, in: Karlsruher
Institut für Technologie, Universitätsbereich, vorgelegte, 2010.
[75] A.B.P. Lever, comprehensive coordination chemistry, 1-9 (2010) 1-819.
[76] T. Jüstel, H. Nikol, Adv. Mater., 12 (2000) 527.
[77] T. Gross, F. Chevalier, J.S. Lindsey, Inorg. Chem., 40 (2001) 4762.
[78] P. A. Vigato, V. Peruzzo, S. Tamburini, Coordination Chemistry
Reviews 253 (2009) 1099–1201.
[79] N. YuKozitsyna, A.E. Gekhman, S.E.Nefedov, M.N. Vargaftik, I.I.
Moiseev, Inorg. Chem. Commun., 10 (2007) 956.
[80] B.-H. Ye, M.-L. Tong, X.-M. Chen, Coordination Chemistry Reviews
249 (2005) 545-565.
[81] M. Yuan, E.B. Wang, Y. Lu, S.T. Wang, Y.G. Li, L. Wang, C.W. Hu,
Inorg. Chim. Acta 344 (2003) 257.
[82] N.H. Pilkington, R. Robson, Aust. J. Chem., 23 (1970) 2225.
[83] G. Ambrosi, M. Formica, V. Fusi, L. Giorgi, M. Micheloni,
Coordination Chemistry Reviews 252 (2008) 1121–1152.
[84] N. Ceccanti, M. Formica, V. Fusi, L. Giorgi, M. Micheloni, R. Pardini,
R. Pontellini, M.R. Tin`e, Inorg. Chim. Acta, 321 (2001) 153.
[85] I.A. Koval, M. Sgobba, M. Huisman, M. Lueken, E. Saint-Aman, P.
Gamez, B. Krebs, J. Reedijk, Inorg. Chim. Acta, 359 (2006) 4071.
[86] P. Chaudhuri, Coordination Chemistry Reviews, 243 (2003) 143-190.
[87] W.E. Hatfield, Inorg. Chem., 11 (1972) 216.
[88] H.A. Goodwin, F. Lions, J. Am. Chem. Soc., 82 (1960) 5013–5023.
[89] V.Gutmann, Electrochim. Acta, 21 (1976) 661-670.
[90] B. A. Shaw, E.H. Ibrahim, Angew. Chem. Int., 6 (1967) 556.
[91] R. J. Deeth, A. Anastasi, C. Diedrich, K. Randell, Coordination
Chemistry Reviews, 253 (2009) 795-816.
[92] M.T. Lemaire, T.M. Barclay, L.K. Thompson, R.G. Hicks, Inorganica
Chimica Acta, 359 (2006) 2616-2621.
Chapter 1
Page 66
[93] E. Pardo, R. Ruiz-Garc, J. Cano, X. Ottenwaelder, R. Lescou¨ezec, Y.
Journaux, F. Lloret, M. Julve, Dalton Transactions, (2008) 2780–2805.
[94] O. Kahn, Struct. Bond., 68 (1987) 89.
[95] O. Kahn, Acc. Chem. Res., 33 (2000) 647.
[96] Y. Journaux, R. Ruiz, A. Aukauloo, Y. Pei, Mol. Cryst. Liq. Cryst., 305
(1997) 193.
[97] E. Pardo, R. Ruiz-García, F. Lloret, J. Faus, M. Julve, Y. Journaux,
M.A. Novak, F.S. Delgado, C. Ruiz-Pérez, Chem. Eur. J., 13 (2007) 2054.
[98] G. Blay, I. Fernández, J.R. Pedro, R. Ruiz-García, M.C. Mu˜noz, J.
Cano, R. Carrasco, Eur. J. Org. Chem., (2003) 1627.
[99] M.T. Lemaire, T.M. Barclay, L.K. Thompson, R.G. Hicks, Inorganica
Chimica Acta, 359 (2006) 2616–2621.
[100] G. Blay, I. Fernández, J.R. Pedro, R. Ruiz-García, M.C. Mu˜noz, J.
Cano, R. Carrasco, Eur. J. Org. Chem., 63 (2003) 1627.
[101] S. Hikichi, M. Akita, Y. Moro-oka, Coord. Chem. Rev., 198 (2000) 61-
87.
[102] W. Kaim, Coord. Chem. Rev., 219-221 (2001) 463-488.
[103] A. Jana, R. Koner, M. Nayak, P. Lemoine, S. Dutta, M. Ghosh, S.
Mohanta, Inorganica Chimica Acta, 365 (2011) 71-77.
[104] Miessler, L. Gary, D.A. Tarr, Inorg. Chem., 9 (1999) 315.
[105] S. Decurtins, R. Pellaux, G. Antorrena, F. Palacio, Coord. Chem. Rev.,
190-192 (1999) 881.
[106] O. Kahn, B. Briat, J. Chem. Soc. Trans., 72 (1976) 268.
[107] G. Marinescua, M. Andruhb, F. Lloret, M. Julvec, Coordination
Chemistry Reviews, 255 (2011) 161-185.
[108] M. Ohba, H. Okawa, Coordination Chemistry Reviews, 198 (2000)
313-328.
[109] J.K.Tang, L.Y.Wang, L.Zhang, E.Q.Gao, D.Z.Liao, P.Cheng, Dalton
Transactions, (2002) 1607-1612.
[110] H. Ojima, K. Nonoyama, Coord. Chem. Rev., 92 (1988) 1069.
[111] E.-Q. Gao, D. Liao, Z. Jiang, S. Yan, Polyhedron 20 (2001) 923-927.
[112] M.S. Masoud, E.A. Khalil, A.M. Hindawy, A.M. Ramadan, Canadian
Journal of Analytical Sciences and Spectroscopy, 50 (2005) 297-310.
Chapter 1
Page 67
[113] C. Brewer, G. Brewer, W.R. Scheidt, M. Shang, E.E. Carpenter,
Inorganica Chimica Acta, 313 (2001) 65-70.
[114] R.N. Katz, G. Kolks, S.J. Lippard, Inorg. Chem., 19 (1980) 3845.
[115] C.T. Brewer, G. Brewer, J. Chem. Soc. Dalton Trans., (1992) 1669.
[116] C.T. Brewer, G. Brewer, L. Mat, J. Sitar, R. Wang, J. Chem. Soc.
Dalton Trans., (1993) 151.
[117] C.A. Koch, C.A. Reed, G.A. Brewer, N.P. Rath, W.R. Scheidt, G.
Gupta, G. Lang, J. Am. Chem. Soc., 111 (1989) 7645.
[118] Y. Sunatsuki, Y. Motoda, N. Matsumoto, Coordination Chemistry
Reviews 226 (2002) 199-209.
[119] S. Deepalatha, P.S. Rao, R. Venkatesan, SpectroChimica Acta part A,
64 (2006) 178-187.
[120] R.L. Carlin, Magnetochemistry, Springer-Verlag, Berlin, 1986.
[121] K. Awaga, H. Okamoto, T. Mitani, Y. Maruyama, T. Sugano, M.
Kinoshita, Solid State Communications, 71 (1989) 1173-1177.
[122] C.M. Hurd, Contemporary Physics 23 (1982) 469-493.
[123] B. Bleaney, K.D. Bowers, Prod. Phys. Soc., 65 (1952) 667.
[124] R. Paschke, S. Liebsch, C. Tschierske, Inorganic Chemistry, 42 (2003)
8230-8240.
[125] M. Dua, Q. Wanga, Y. Wanga, X. Zhaoa, J. Ribas, Journal of Solid
State Chemistry, 179 (2006) 3926–3936.
[126] M.B. Bushuev, E.V. Peresypkina, V.P. Krivopalov, A.V. Virovets, L.G.
Lavrenova, Inorganica Chimica Acta, 365 (2011) 384–390.
[127] C.J. O’Connor, Prog. Inorg. Chem. , 29 (1982) 203.
[128] E.K. Brechin, Chem. Commun., (2005) 1541.
[129] M. Pilkington, S. Decurtins, J. S. Miller, M. Drillon, Magnetism: From
Molecules to Materials, Wiley-VCH, Weinheim, 2001.
[130] D. Gatteschi, R. Sessoli, J.Villain, Molecular Nanomagnets, Oxford
University Press, New York, 2006.
[131] F. E. Mabbs, D.J. Machin, Magnetism and Transition Metal
Complexes, Chapman and Hall, 1973.
[132] D. Maspoch, D. Ruiz-Molina, J. Veciana 2007, 770, Chem. Soc. Rev.,
36 (2007) 736.
Chapter 1
Page 68
[133] M. Kurmoo, Chem. Soc. Rev., 38 (2009) 1353.
[134] Anonymous, Miscellanea Berolinensia and Incrementum Scientiarum,
1 (1710) 377–378.
[135] J. Woodward, Phil. Trans., 33 (1724) 15–17.
[136] J. Brown, Phil. Trans., 33 (1724).
[137] A.G. Sharpe, The Chemistry of Cyano Complexes of the Transition
Metals, Academic Press, New York, 1976.
[138] F. Palacio, Introduction to Physical Techniques in Molecular
Magnetism, University of Zaragoza, Zaragoza, 1999.
[139] H.U. Güdel, H. Stucki, A. Ludi, Inorg. Chim. Acta, 7 (1974) 121.
[140] D. Davidson, L.A. Welo, J. Phys. Chem., 32 (1928) 1191.
[141] A. Ito, M. Suenaga, K. Ono, J. Chem. Phys., 48 (1968) 3597–3599.
[142] R. zelmann, K. Wieghard, U. Florke, H. Haup, D.C. Weatherburn, J.
Am. Chem. Soc., 114 (1992) 1681-1696.
[143] F.A. Mautner, M. Mikuriya, H. Ishida, H. Sakiyama, F.R. Louka, J.W.
Humphrey, S.S. Massoud, Inorganica Chimica Acta 362 (2009) 4073–4080.
[144] M. Dua, Q. Wanga, Y. Wanga, X. Zhaoa, J. Ribas, Journal of Solid
State Chemistry 179 (2006) 3926–3936.
[145] M. Ohba, H. Tamaki, N. Matsumoto, H. Okawa, Inorg. Chem. , 32
(1993) 5385-5390.
[146] A.R. Paital, W. Wong, G. Aromı, D. Ray, Inorganic Chemistry, 14
(2007) 5727-5736.
[147] A. Greatti, M. Scarpellini, R. A. Peralta, A. Casellato, Inorganic
Chemistry 47 (2008) 1107-1116.
[148] M. James, J. Horvat, Journal of physics and chemistry of solid, 63
(2002) 657-663.
[149] A. A. Sidorov, I. G. Fomina, G. G. Aleksandrov, Yu. V. Rakitin, V. M.
Novotortsev, V. N. Ikorskii, M. A. Kiskin, I.L. Eremenkoa, Russian
Chemical Bulletin, 53 (2004) 483—485.
[150] K.S. Min, K.Swierczek, A.G. DiPasquale, A.L. Rheingold, W.M.
Reiff, A.M. Arifa, J.S. Miller, Chem. Commun. , (2008) 317–319.
[151] S. Han, J.L. Manson, J. Kim, J.S. Miller, Inorg. Chem. , 39 (2000)
4182-4185.
Chapter 1
Page 69
[152] L. Stoicescu, A. Jeanson, C. Duhayon, A.T. Vallina, A.K. Boudalis, J.
Costes, J. Tuchagues, Inorganic Chemistry, 17 (2007) 6902-6910.
[153] J. Ribas, B. Albela, H. Stoeckli-Evans, G. Christou, Inorg. Chem. , 36
(1997) 2352-2360.
[154] A.N. Georgopoulou, C.P. Raptopoulou, V. Psycharis, R. Ballesteros, B.
Abarca, A.K. Boudalis, Inorganic Chemistry 48 (2009) 3167-3176.
[155] M. Gruselle, C. Train, K. Boubekeur, P. Gredin, N. Ovanesyan,
Coordination Chemistry Reviews, 250 (2006) 2491-2500.
[156] K.S. Murrey, Coord. Chem. Rev., 12 (1974) 1-35.
[157] L.K. Thompsona, O. Waldmann, Z. Xua, Coordination Chemistry
Reviews, 249 (2005) 2677–2690.
[158] R. Ruiz, J. Faus, F. Lloret, M. Julve, Y. Journaux, Coordination
Chemistry Reviews 193-195 (1999) 1069–1117.
[159] S. Triki, F. Berezovsky, J.S. Pala, C. J. Gomez-Garcı, E. Coronado, K.
Costuas, J. Halet, Inorg. Chem. , 40 (2001) 5127-5132.
[160] A. Inagakia, M. Akitaa, Coordination Chemistry Reviews, 254 (2010)
1220–1239.
[161] K.M. Smith, Coordination Chemistry Reviews 250 (2006) 1023-1031.
[162] Y. Pei, O. Kahn, J. Sletten, J.P. Renard, R. Georges, J.C. Gianduzzo, J.
Cure´ly, Inorg. Chem. Commun., 27 (1988) 4-14.
[163] P.J. Steel, Coordination Chemistry Reviews, 106 (1990) 227-265.
[164] X.-Y. Wang, L. Wang, Z.-M. Wang, G. Su, S. Gao, Chem. Mater., 17
(2005) 6369.
[165] N. Matsumoto, H. Murakami, T. Akui, J. Honbo, H.O. kawa, A.
Ohyoshi, Bull. Chem. Soc. Jpn., 59 (1986) 1609.