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CHAPTER - I
INTRODUCTION
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1 INTRODUCTION
1.1 INTRODUCTION TO CO-ORDINATION CHEMISTRY.
1.2 LIGANDS CONTAINING OXYGEN AND NITROGEN AS
DONOR ATOMS AND THEIR METAL COMPLEXES.
1.3 LITERATURE SURVEY ON PREVIOUS STUDIES ON METAL
CHELATES WITH LIGANDS CONTAINING OXYGEN-
NITROGEN AND OXYGEN-OXYGEN DONORS.
1.4 AIM OF THE PRESENT INVESTIGATION.
1.5 REFERENCES.
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1 INTRODUCTION
Chemistry is an active evolving science that has vital importance to our world
in both realm of nature and the realm of society. Its roots are ancient but at every
beat it is modern science. Therefore, chemistry is a modern science of 21st century1.
1.1 Introduction to Co-ordination chemistry:
Co-ordination chemistry is a branch of Inorganic chemistry which involves the
study of the molecular compounds known to be formed by the union of stoichiometric
ratio and capable of independent existence. These compounds have been
designated as complex compounds or co-ordination compounds. Therefore addition
or molecular compounds which retain their identity even in solution and the properties
of which are different from their constituents are termed as complex salts or co-
ordination compounds2. In other words, a co-ordination compound or complex is
formed when the Lewis base (donor) is attached to a Lewis acid (acceptor) by means
of “lone pair” of electrons3.
In recent days large area of Inorganic Chemistry research is acquired by co-
ordination chemistry due to its interesting and significant properties Co-ordination
chemistry has always been a challenge to researchers. Majority of biologically active
compounds are co-ordination compounds4.
The knowledge about coordination compounds has been developed from
pioneer work of A. Werner5 in 1893. Werner was the first who could able to explain
the nature of bonding in complexes. He proposed that in co-ordination compounds
the central metal exhibits two types of valencies that are primary and secondary. The
primary valency is ionisable and non-directional while secondary valency is non-
ionisable and directional. For this revolutionary work Alfred Werner was awarded a
Noble prize in 1913. Brown6 classified the complexes, Tambe-Blomstrand7 and
Jorgensen8 pointed out the relation between different classes and the structure of
complex compounds.
Werner’s work was elaborated by Lewis9, Kossel10. Sidgwick11, and Fajans12.
Linus Pauling13 and others finally developed the work into ‘Valence Bond Theory”
(VBT) in 1931.
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In the complex the metal ion or metal atom is present at the centre and
has the capacity to accept lone pair of electrons resulting into coordinate bond or
dative bond. The number of bonds formed by donor atoms with central metal species
is termed as “Co-ordination Number” which exhibits the specific characteristic of
central metal ion, related to the positions of metal ions or atoms in periodic table. Co-
ordination chemistry deals with the large number of metallic elements belonging to s-
block, d-block, f-block and higher members of p-block of the periodic table. The
stability of complexes have explained by Sidgwick with the help of EAN rule which is
nothing but the fact that central metal ion or atom acquires the same effective atomic
number of next inert gas. In fact some compounds obey EAN rule while some do not.
In 1931 Pauling gave VBT which is based on the unique and revolutionary
idea regarding the concept of hybridization. According to VBT, the central metal ion
or atom makes available number of empty or vacant orbitals equal to its co-ordination
number. These empty metal orbitals undergo pearticular types of hybridization such
as sp, sp2, sp3, dsp2, dsp3, sp3d. d2sp3 or sp3d2 and sp3d3 with moleculer shapes or
geometries like linear, trigonal, tetrahedral, square planer, trigonal bipyramidal,
square pyramidal, octahedral or square bipyramidal and pentagonal bipyramidal
respectively. The filled ligand orbitals overlap with vacant hybrid metal orbitals with
the formation of co-ordinate covalent bond. This theory explains mainly electronic
structure of central metal ion or atom, geometries of complexes, concept of inner
orbital and outer orbital complexes, magnetic moments and stereochemistry.
However, it does not give proper explanation of maximum pairing, complex spectra
and quantitative interpretation of magnetic properties.
Crystal Field Theory (CFT) developed by Bethe14 and Van Vleck15 is another
advanced approach in the study of complexes. According to CFT, the bond between
metal and ligand is purely electrostatic and it is neither due to sharing of electrons nor
due to interaction of atomic orbitals. The effect of interaction of metal d-orbitals with
the surrounding ligands is the formation of crystal field which removes the
degeneracy of metal d-orbitals resulting into crystal field splitting. The energies of the
sublevels of orbitals depend upon the type of geometry. e.g. in octahedral or oh
complex, five metal d-orbitals get splitted into t2g-triplet with lower energy and eg
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(doublet) with higher energy splitting mode is basically related to the orientation of
metal d-orbitals and direction of the ligand approach in specific geometry. The energy
difference between t2g and eg levels in octahedral complex is the Crystal Field
Stabilization Energy (CSFE) which is denoted as l0Dq or ∆o.
For tetrahedral and square planer complexes it is designated as ∆t and ∆sq
respectively. The magnitude of 10Dq depends mainly upon nature of ligand (e.g.
position in ECS) and charge on the central metal. CFT gives quantitative
interpretation of magnetic and spectral properties of co-ordination compounds.
Van Vleck15 and Mulliken16,17 developed (MOT) i.e. molecular orbital theory
which provides quantitative interpretation for all the properties of coordination
compounds. In MOT the bonding between central metal species and ligand is
considered as ionic, covalent and intermediate. The energy level diagram for a metal
complex18 includes bonding orbitals, non-bonding d-orbitals on metals and
antibonding orbitals formed by overlap of the orbitals of metal ion and orbitals of
ligands with appropriate symmetries. MOT satisfactorily accounts for the spectral and
magnetic properties of metal complexes including those of the π-type, like metal
carbonyls and metal olefins19.
Ligand Field Theory20-22, (LFT) is developed in recent years which is the
modern extension of CFT. LFT correlates the physical properties of co-ordination
compounds with the nature and position of the ligand in ECS which reflect change in
ligand surrounding which can be divided in three categories e.g. thermodynamic,
spectral and magnetic. In the first category the splitting of the d-orbitals under the
influence of ligand field is disscussed23. The second category gives the electronic
transitions taking place between ground and excited levels of co-ordination
compounds 24, 25. The spin and angular moments of electrons in the filled shell give
rise to magnetic properties.
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1.1.1 Chelates:
Rossotti26 has defined the co-ordination complex as a chemical species
formed by two or more species one of which is metal ion and others are ligands.
Ligands are able to form either one bond with central metal (monodentate) or more
than one bond with central metal (polydentate). Interaction of polydentate ligand with
metal ion results into a cyclic structure consisting heteroatoms. The term “Chelate”
was first introduced by Morgan and Drew27 to describe such cyclic structures arising
from the combination of metallic species with polydentate organic or inorganic ligand
species. The heterocyclic rings are termed as ‘chelate rings’ and the phenomenon is
known as ‘Chelation’. The term ‘Chelate’ was taken from the Greek word ‘chela’
meaning crabs claw. The analogy is obvious because donor atoms from ligand may
hold an object (central metal) through more than one point of attachment and form
heterocylic ring. More recent treatment is observed in the book written by Martell and
Calvin29.
Out of the most striking properties of chelates is their unusual stability pointed
out by Feitter29.Therefore they resemble the aromatic rings encountered in organic
chemistry. The stability of chelate depends upon the size and number of atoms
involved in the ring. Generally co-ordination compounds formed by five membered
rings are more stable than unsaturated five membered ring. However, a greater
stability is achieved with the formation of six membered rings. The co-ordination
numbers of metal are generally four and six. The well known example of chelate in
animal kingdom is haemoglobin. i.e. red pigment present in the blood which is Fe-
phorphyrine chelate and in plant kingdom is chlorophill i.e. green pigment needed for
photosynthesis which is Mg-porphyrine chelate. This suggests a need for the study of
metal-chemistry involved in biological systems30 which may be tittled as bio-
inorganic chemistry.
The formation of co-ordinate covalent bond with central metal ion or atom and
donor atom of ligand may proceed with or without replacement of hydrogen atom
from organic functional groups. Majority of chelating agents i.e. ligands involved in
chelate formation belong to organic chemistry. With this point of view co-ordination
chemistry, may be considered as inter-disciplinary branch or bridge between
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Inorganic chemistry and Organic chemistry because it involves the combination of
metal ions or atoms with donor groups of chelating agents.
Following are the type of functional groups observed in chelating agents-
(A) Functional groups which combine with metal ions by replacement of hydrogen –
-COOH (Carboxylic) -OH (Phenolic)
-SO3H (Salphonic) -SH (Thiophenolic)
>C=N–OH (Oxime) >C-N–H (Imine) etc.
(B) Functional groups which combine with metal ions without replacement of
hydrogen –
- OH (Alcoholic) -NH2 (Primary amine)
- SH (Mercapto) -NHR (Secondary amine)
- O – (Ether) -NR2 (Tertiary amine)
> C = S (Thiocarbonyl) - CH = CH – N< (Enamine)
> C = N- R (Alkylimine) - S – (Thioether )
O
NEnamino Ketone etc.
1.1.2 Application of co-ordination compounds:
Co-ordination chemistry has found many more applications in various
branches of science such as-
a) Analytical chemistry31
b) Biology32
c) Catalysis33, 34
d) Pharmacology35
e) Metabolic activities36-38
6) Medicines39, 40
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1.1.3 Importance of co-ordination compounds in biol ogical systems:
Co-ordination compounds possess the ability to influence many of the reactions
upon which number of vital processes of living organisms depend. Excellent theories
are available on some of the naturally occurring co-ordination compounds.41,42
It may be observed that many of the capitalized compounds are biological
catalysts known as enzymes. .Enzymes generally consist of a protein part which
account for the bulk weight of the molecule and a non-protein part i.e. prosthetic
group.
The participation of complex compound in nearly every phase of biological
activity is classified as –
1. Bond formation and cleavage
2. Exchange of functional groups
3. Blocking of functional groups
4. Influence upon stereochemistry
5. Oxidation reduction reactions
6. Storage and transfer
7. Transmission of energy
Metal ions play an important role in many of the bond making and bond
breaking reactions in natural processes. The acceleration of bond cleavage as a
result of co-ordination may be attributed to the polarisation of electrons towards metal
and therefore away from organic molecule. Thus the activation energy necessary is
considerably lowered43.
e.g. Zn forms an essential part of a number of enzymes including carbon
anhydrase, alcohol dehydrogenase, alkaline phosphatase, glutamic dehydrogenase
and lactic dehydrogenase. Zn is also playing an important role in the biological action
of insulin. Nickel, Cobalt and Cadmium also react with insulin polypeptides44,45. A
calcium protein complex known as enterokinase aids in the conversion of
chymotrypsin into trypsin46,47.
In addition to bond forming and rupturing reactions, metal ions participate in
group transfer reaction. eg. Enzyme Transaminase which contains chelating
substance pyridoxal. Transmutation provides link between carbohydrate and protein
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metabolism through the transfer of amino group from amino acid to keto acids. The
requirement of vitamin gave that amino acids initially form schiff‘s bases with
pyridoxal. Haemoglobin and chlorophyll are porphyrin chelates while vit. B12 is corrin
chelate observed in biosystems.
Redox reactions are of fundamental importance in biochemical processes in which
metal ions play an important role in the form of complexes.
1.1.4 Importance of Co-ordination compounds in medi cine or as drugs:
Many drugs become biologically active by forming complexes with important
biological metabolites or enzymes. Hence, number of studies appeared in literature
concerning with drugs.
(I) ANTIMICROBIAL AGENTS-
The activities of certain antimicrobial agents (i.e antibiotics) depend in part
upon their ability to form chelates. e.g.
a) Tetracycline s – It is suggested that chelation is involved in the mechanism
of tetracyclines. Attempts have been made to prepare chelates for the theorapeutic
purposes with Fe3+, Co3+
, Al3+, Sn 2+, Cd2+, Pb2+, Cr3+, Mo5+ and rare earths48, 49.
Tetracycline complexes are also prepared with Be2+, Co3+, Ni3+ 50,51, Ransmeir52
prepared complexes with Ca & Al while Benet & Goyan53 used Cu for complexation.
Oxytetraycline complexes are prepared54 with Co3+, Fe3+, Mn2+, Ni2+, Ca2+, Zn2+, Al3+,
Cr3+, Cu2+ & Mg2+
b) 8- Hydroxyquinoline (oxine ) – This is well known chelating agent which
exhibits antimicrobial, amoebicidal and fungicidal properties55,56. The effect of oxine
upon gram positive bacteria is more than upon gram-negative bacteria, 8-
hydroxyquinoline appears to penetrate cell membranes, as a fat- soluble complex
with metals. The Cu2+ complex easily pass into parasite body, liberate Cu & kill the
invader57.
The antimicrobial properties of penicillin58, Bacitracin59, Cycloserine60,61, Kojic
acid62, Morin59, α-nitroso-β-naphthol, polymyxin62 and α-Picolinic acid59 are evidently
related to their chelating ability as their activity is affected by certain metals.
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(II) Antituberculotic agents
Streptomycin is a good chelating agent. Chelates of streptomycin with Fe3+ 63
have been reported. Mixed complexes of dihydro-streptomycin and Penicillin- G with
Fe3+, Cu2+, Co3+, Ni2+ and Th4+ have been studied64. The activity of streptomycin has
been reported to be inhibited by addition of Cu2+, Co2+, Ni2+ 65, Ca 2+ and Mg2+ 66.
Other antituberculotic agents are p-aminosalicylic acid, thiosemicarbazone
and aspergellic acid67. p-aminosalicylic acid and alcoholic gold salt react to form gold
complex which is useful antitubercular68.
(III) Analgesics in rheumatoid diseases and fever:
The antirheumatic action of orthohydrobenzoic acid (salicylic acid) is due to its
ability to form complex with heavy metals69, while meta and para forms are ten times
less effective than orthoforms.
Gold derivatives used in rheumatoid arthritis are sanocrysine, myochrysine,
solganal auranofin, sodium p-hydroxybenzoate and gold thioglucolanalide (Leuron)70.
(iv) Diuretics –
The effectiveness of organomercurial diuretics is attributed to their ability of
inhibition by complex formation. Recent studies have demonstrated that mercury
remains bound as the organo-mercurial complex R-Hg–X71,72 in kidney. ‘X’ may be a
protein which is exchangable for cysteine or acetyl cysteine complex73.
(V) Antithyroids –
Thiourea and thiouracil are known to react with copper and have marked
antithyroid activity. In the thiouracil series of compounds, there is a positive
relationship between chelating ability and antithyroid activity74.
(VI) Disinfectants and antiseptics –
Copper bis-(marphonylamino) sulphathiazole is useful as bactericide and
antiseptic75. Copper complexes of o-hydroxyazonaphthols and phenanthrols supress
the growth of Microbacterium tuberculosis, both in vitro and vivo76.
Silver nitrate and protein complexes are used as antiseptic and germicide. Silver
picrate is an antiseptic used in gonorrheal and trichomonal infections. Unstable silver
complex of cesin could cure infections and helps to attain higher curative power of
silver complexes of arphenamine77 as silver-bismethyl (2,3-dihydroxy p-phenethyl)
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amino sulphadiazine, Ag-diaminosulphadiazine, Ag-Bis(marphoxylamino) sulpha-
anilamide, Ag-Bis(benzylamine)–sulphadiazine etc. Silver complexes are useful as
bactericide and antiseptic and can be incorporated for external application78.
Organomercurials are used as antiseptics. The inactivation of bacteria by
mercurial may be caused due to their ability of form inactive complexes with
sulphydral enzymes79 without cell injury.
The antibacterial activity of organic compounds of arsenic80 and antimony81 is
brought about by a similar mechanism.
(VII) Antimalerials-
Poludrine one of the antimalerials is reported to act through the formation of
chelate with copper82. Quinoline and p-toluence sulphonamide have been used as
drugs for diseases like maleria,tuberculosis etc.Tewari and Mishra83 prepared metal
chelates of Fe(III ), Co(II ), Ni(II ), Cu(II ) and Zn(II ) with 5-iodo-7-chloro-8-hydroxy-
quinolino-4-(p-tolyl)-sulphonamide and found that the metal chelates were more
active than ligands against several types of bacteria.
(VIII) Vasodepressar and Bronchodilator 84-95-
Such as catechol, amines like adrenaline, nor-adrenaline, dopamine and
isopranaline.
(IX) Anticancer drug-
Like folic acid antagonists, thiogunine adenine etc.96-109 acts as anticancer drug.
(X) Complexes as antidotes or antimetal poisoning d rugs.
Some of the metals are extremely toxic. The treatment of metallic toxicity till a
few years back was considered to be quite difficult due to lack of specific antidotes or
antitoxic species. The development of antagonists to the biological actions is
important in modern pharmacology. The antagonists are valuable drugs. Heavy
metals have toxic effects as they combine with reactive110 groups, essential for
normal cell functions and thereby they block the reactive sites. A number of chelating
agents are developed which show remarkable degree of specificity and hence used
in various intoxification.
Dimercapral, BAL (2,3 dimercapto propanol) form a stable, non-toxic chelate
with arsenic and lead-atoms in Lewisite . Dimercaprol has been used successfully in
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the treatment of poisoning or toxic reactions of mercurials and gold salts111,112,
trivalent antimony113, trivaleut arsenic114, chromium115 and copper116.
Anorther reagent EDTA (Ethylenediaminetetraacetic acid) forms a chelate with
calcium ions in blood and has been used in the treatment of hypercalcimia 117,118 for
dissolving calcified corneal opacities119.
Pericillamine, a degradation product of penicillin is used as a chelating agent
in the case of Cu, Hg, Zn and Pb Poisoning120,121. It is an effective drug for Wilson’s
disease which is caused by deposition of copper in various tissues, in toxic
amounts122-124.
Desferrioxamine is a chelating agent which is used in the treatment of excess
iron storage diseases and hence acute iron poisoning. Desferrioxamine has been
found to have a remarkable affinity for ferric iron.
From the above paragraphs it would be clear that there is a continuous search
for newer and newer metal complexes of novel ligands which would possess
applications in variety of fields.
In 1965 Rosenberg125-127 discovered the anticaner activity of cis-platin which is
platinum complex. Since then platinum complexes of different ligands have been
investigated and found to possess antitumour activity and are used in cancer
chemotherapy and are known as anticancer agents128,129.
The antileukemia properties of many130,131 organoplatinum complexes have
been reported .
Celave et al.132,133 Studied a series of Co(II). Cr(III) Complexes from which only
[Co(NH3)4Cl2] Cl and [Co(NH3)3CO3] NO3 showed anticancer activity.
Therefore a number of organic compounds possessing physiological activity
and ability to act as ligands are being synthesized of which some of the examples are
carboxylic acids134, aldehydes, phenols136, ketones137, nitrocompounds138, amino
acids139, alkaloids140, thiozines141,142,3 β-diketones143, schiff’s bases19,4,2 and
enaminoketones144-147.
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1.2 Ligands containing Oxygen and Nitrogen as dono r atoms and
their metal complexes
1.2.1 Schiff’s bases - Schiff’s bases are condensation products of amines with active
carbonyl compounds. They are also known as imines148, anils and azomethines.
They contain azomethine (>C=N-) group and hence act as effective ligands. It was
first synthesized by Schiff149.
R'
RO
HN
HR"
R'
RN
H2OR" +
Active Carbonyls Pri-amine Schiff's base
The Schiff’s bases are more effective when they bear supporting and
stabillizing group like- OH in the vicinity of >C=N group. Therefore the chemistry of
Schiff base metal complexes attracted many researchers and has been developed
rapidly in recent years150. Hydrazones, carbazones semicarbazones,
thiosemicarbazones, thiocarbazones, oximes etc. are some of the important classes
of Schiff bases that have been studied extensively151.
Mane153 has synthesized complexes of Cu(II ), Ni(II), Co(II ), Fe(III ) and Mn (II ) metal
ions with Schiff bases derived from dehydroacid (DHA) and primary aromatic amine
like m-chloroaniline, m-aminophenol, m-anisidine, m-toluidine, m-bromoaniline, 3,4
dichloroaniline m-amino benzoic acid and o-phenitidine and characterized.
Pachling152 reported the synthesis and characterisation of Fe(III ), Cr(III ), Cd(II ),
Hg(II ) & Pb(II ) complexes of schiff base derived from DHA and semicarbazide like
amines. Pandhare19 reported the synthesis and characterization of complexes of
schiff’s bases derived from o-aminophenol and substituted aldehydes.
Maurya et al.154 reported the synthesis, magnetic and spectral studies of some
novel binuclear-dioxo molybdenum VI chelates involving Schiff bases derived from
sulpha drugs and 4-benzoyl-3-methyl-1-phenyl-2-pyrazolin-5-one.
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1.2.2 ββββ-Diketones -
β-Diketones comprises a class of compounds characterized by the presence
of two –OXO- groups –(-CO-CH2-CO-). β-diketones possess good chelating ability
and they show enhanced biological activities. Khot2 reported synthesis and
characterization of complexes of transition metals with β-diketones. Mathews
Cheriyan155 synthesized and characterized the complexes of Co(II ), Ni(II ), Cu(II ) and
Zn(II ) with 2-(2-carboxyphenylazo)-1,3-diketones.
Ismail Patel156 synthesized Mn(II ) complexes with Schiff bases derived from
heterocyclic β-diketones and some diamines.
1.2.3 Chalcones-
Chalcones are the condensation product of acetophenone with aromatic
aldehydes in the presence of strong base. Chelcones and their metal complexes
show significant biological activities. Chalcones are nothing but α, β-unsaturated
ketones. Patange3 reported the synthesis and characterization of complexes of
Mn(II ), Fe(III ), Co(II ), Ni(II) and Cu(II ) metal ions with chalcones derived from
dehydroacetic acid (DHA) with hetetrocyclic aldehydes.
General structure of ligand used in above work is-
O
Ar
OH3C
OH O
α
β
1.2.4 Enamines or Enaminoketones-
The term “enamine’ was first introduced in 1927 to emphasis the structural
similarity between the α,β-unsaturated amine system and the α,β-unsaturated
alcohol moiety present in enols157. Isolated reports concerning the reactions of
enamines date back to the early nineteen hundreds. Indeed in 1916 Robinson
correctly interpreted. The course of the reaction between an alkyl halide and ethyl β-
amino-crotonate158, 159. However, it was not until 1954, when Stork and his associates
described alkylation and acylation reactions, and demonstrated the ease of
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preparation of a number of enamines160, that general interest was arose. Since then
a considerable amount of work has been reported on a variety of enamines,
expanding the scope of the original observations.
Preparation and some properties-
The most common procedure for enamine formation, which was first used by
Herr and Heyl in 1952, then exploited by Stork160 et. al. involved heating under reflux
an equimolar mixture of carbonyl compound and the amine in a solvent such as
anhydrous benzene, toluene or xylene with azeotropic removal of water.
Preparation from aldehydes and ketones:
The most versatile and most often used method of formation of enamine
involes the condensation between aldehyde or ketone and a secondary amine.
a) C C
O
H
HN CC
N H2O
The mechanism of the reaction is usually expressed as follows.
C C
O
H
HN
R'
R"
H
OH
NR'R"
(I)
H
NR'R"
(II)
NR'R"
(III)
H
O+H2
NR'R"
(III)
OR
In the acid catalyzed reaction presumably the N-hemiacetal (I) is protonated to
(III ). The actual rate of enamine formation depends upon the several factors in a
complex way such as-
i) The basicity of amine.
ii) The degree of steric hindrance in either the amine or ketone, which affects
the rate of formation of (I)
iii) The rate of loss of the hydroxyl group from (I) or (III ) and
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iv) The rate of loss of a proton from (II)
The enamine once formed may be isolated by distillation.
The most commonly used compounds have been the cyclic amines.
N Hi.e. a) Pyrrolidine
b) Piperidine
c) Morpholine
NH
NHO
If a molecule contains both aldehyde and ketonic functions like 2-oxocyclohexane-
carbaldehyde reaction with secondary amine occurs as follows-
O
CHO
2-oxocyclohexanecarbaldehyde
NHR'R"
O
CH-NR'R"
One of the properties of enamine is protonation. And basically the structure of
enamine system may be regarded as a resonance hybrid to which following canonical
forms (a) and (b) are important contributors157.
CCH
N CCH
N
Hence electrophilic reagents include protons, may attach the system at either the
nitrogen atom to give ammonium salt –
CC
NR
Or more importantly, at that carbon atom β to the nitrogen to yield an iminium salt-
αβ
R
CC
N
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Joshi et. al.161 reported the reactions of thiosemicarbazide with 3-formylchromone
and synthesized some pyrazole and enamine containing organosphorous162 compounds
in view of activities associated with heterocyclic compounds163.
3-Formylchromones when treated with thiosemicarbazide in alcoholic KOH gave
compound (I) which when treated with sodium metal in dry THF followed by treatment
with O,O-diethylphosphorochloroido thiolate yielded compounds (II) and (III) 163.
Formylchromones when heated with piperidine in ethanol yielded compound (III ) termed
as enaminoketone.
O
O
CHO
R1
R2
R3
Thiosemicarbazide/ Alc. KOH
Heat 3 hrs
O
R1
R2
R3
N
NH
(I)
Na/ THF
POC2H5
S
OC2H5
OH
O
R1
R2
R3
N
(III)
Enaminoketones
R1
R2
R3
N NH
(II)
OH
O
Piperidine/Ethanol
P OC2H5
S
OC2H5
Cl
O
Among the different functionalized chromones 3-formylchromones occupy a
unique position because they can be transformed into various heterocycles163-165.
The reactivity of 3-formylchromone towards several nucleophiles such as hydrazine,
phenyl hydrazine and particularly two functional nucleophiles, e.g amidines,
derivatives of guanindine and isothiourea was investigated166.
3-Formylchromone when treated with piperidine167 under reflux gives 1-(2-
hydroxy-phenyl)-3-piperidin-1-yl-propenone, which is enamine function.
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O
O
CHO
R1
R2
R3
OH
O
R1
R2
R3
NEthanol
RefluxN
H
Iminoketones or ketoenamines are versatile synthones which can be
converted to variety of heterocyclic compounds168. The compound 1-(2-hydroxy-
phenyl)-3-piperidin-1-yl-propenones were utilized for synthesis of bioactive
organophosphorous compounds163.
Dalvi et.al.169 synthesized different 1-(2-hydroxy-phenyl)-3-piperidin-1-yl-
propenones by ultrasonic activation from differently substituted 3-formylchromones
and piperidine. For the method of ultrasonic irradiation the time required for
completion of the reaction is less and yields are better than conventional method.
Piperidine reacts with 3-formylchromones by attacking the electron deficient centre of
C2 carbon and the probable mechanism is as follows-
O
O
CHO
R1
R2
R3
OH
O
R1
R2
R3
N
N
H
O
O-
CHO
R1
R2
R3
N+HO
O
R1
R2
R3
N
O
H
N
H
O-
O
R1
R2
R3
N
N+H
O
H
The required 3-formylchromones are synthesized by Vilsmeier-Haack reaction
on variously substituted 2-hydroxyacetophenones derived from phenols by Bechman
rearrangement.
Karale170 described the syntheses of a series of organic compounds of varied
classes such as chromones, aminopyrimidines, thiopyrimidines, pyrazoles,
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benzothiazepines, dihydrobezothiazepines, fused amino and thiopyrimidines,
coumarins etc.
While referring the literature servey of the above classes of compounds it was
found that they are associated with various physiological and biological properties
and thus find importance in medicine.
A number of scientists in the past have tried to find out some relationship
between chemical structure and physiological or biological properties. It is now well
established fact that the activity of a compound depends upon three factors. The first
and perhaps most important is the heterocyclic moiety present in the particular
compound. The second factor is the nature of the substituents and the third factor is
the position of the substituents in these compounds.
4-Oxo-4H-[1]benzopyran-3-carboxaldehyde is a versatile synthone171 and can
be converted into large no. of heterocyclic compounds such as pyrimidines,
pyrazoles, oxazoles upon condensation with different nucleophiles. These 3-
formylchromones give important intermediates, which can be used in the synthesis of
some important heterocyclic compounds e.g. 4-heteryl coumarins172.
The effective and facile method for the synthesis of 3-formylchromones was
developed by Nohara et. al.173 They have synthesized a number of 3-
formylchromones by formylating various 2-hydroxy acetophenones by the application
of Vilsmeier-Haack reaction. The most suitable formylating reagent was a complex of
dimethylformamide and phosphorousoxychloride. The reaction can be represented
as follows.
R1
R2
R3
OH
O
DMF/POCl3
R1
R2
R3
O
CHO
OR4 R4
4-Oxo-4H-[1]benzopyran-3-carboxaldehydes when condensed with primary
aromatic amines gives 3-(aryliminomethyl)-chromones i.e. schiffs bases or anils. The
reaction between equimolar quantities of 3-formylchromones and primary aromatic
amine invariably lead to a mixture of the anil (a) and 1,4-adduct (b)173.
20
R3
O
CHO
O
NH2
R5
R6
R7
R1
R2
R4
R3
O
OH
N
R5
R6
R7
R1
R2
R4
R3
O
O
HN
R5
R6
R7
R1
R2
R4
NH
R5
R6
R7
(a)
(b)
Pyrazoles are associated with bactericidal174, antiinflamatory175 and
hepatoprotective176 activities. Chalcones are associated with bacteriostatic177,
tuberculostatic178and insecticidal179 activities.
Chandrakanta Ghosh180 gave that 3-acetyl-4-oxo-4H-[1]benzopyran gives(1a)
gives enaminoketons(2) with piperidine.
R1
R2
R3
OH
O
R1
R2
R3
O
COMe
O
R
1a
N
2
Of the 3-acetyl-4-oxo-4H-[1]benzopyran (trivial name: 3-acylchromenone) the
reactions of 3-formylchromones have been extensively studied171.
Zagorevskii181 et al. studied the mechanism of the opening of the pyron ring of
chromone during the action of amines.
Ghosh182 et al. reported the base catalyzed reaction of EtOH with α-Cyno-
acrylic esters (I-R=OH, R1=CN, R2=H, Me) which gives the pyranobenzopyrans (II -
R3=CO2Et, R4=OEt). Similar reaction of EtOH, MeCOCH2COMe, EtO2CCH2CO2Et,
MeCOCH2CO2Et with azalactones (I; R, R1= N:CPhO) produces the fused pyrans [II-
R3=NHCOPh, R4=OEt,CH(COMe)2CH(CO2Et)2CH(COMe)CO2Et]. Piperidine
converts chromone derivatives (I; R=CO2Et, COMe, CN; R1=OEt) into the
21
transenaminoketone (E)-(III ). The pyranobenzopyrans [II ; R3=NHCOPh; R4=CH
(COMe)2, CH(CO2Et)2, CH(COMe)CO2Et] react with pyridine-acetic anhydride to form
the acetates (IV ; R5, R6=me, OEt) corresponding to open the chain tautomers of the
former.
R2
O
CH:CRCOR
O
R
IR2
O R4
II OR3
O
R2
OH
O
NR2
OAc
O
CH:C(COR5)COR6
NHCOPhIII IV
Ghosh et al.183 reported the study of defunctionalization of acids and various
substituted aldehydes to the respective chromones (II) via o-hydroxy acrylphenones
(III). A mixture of substituted chromones (I) and piperidine in ethanol was refluxed to
yield enaminoketones (III), while heated with conc. H2SO4 in ethanol to give (II)
Me
OH
O
Me
O
CO2H
O
N
I IIIMe
O
OII
Zagorevskii184 et al. reported the structure of products from the opening of the
pyran ring of 4-pyrones by amines.
Yong-Ming-Wu185 reported synthesis of 2-bromodifluoromethyl quinoline
derivatives and difluoromethylene thioether by cyclization of β-bromo difluoromethyl
β-enaminoketones.
22
N OH
Ph
1
R
BrF2CN OF2Br
2
PPA
120oC
Ph
R-XH/ Base R-XH/ Base
OH
NO
H
Ph
4
MeO
R-X
FF
N
Ph
HOOC
3
XR
FF
R
23
1.3 Literature survey on previous studies on metal chelates with
ligands containing Oxygen, Nitrogen and Oxygen-Oxyg en
donors-
The literature survey gives that the scope of co-ordination chemistry is vast.
The new horizons of this chemistry extends its tendencies to various interdisciplinary
fields. The development of numerous newer organic chelating agents that can
coordinate with metal ions has opened up a broad scope to a research scientist in
synthetic field. In the last few decades a lot of work has been done on metal
complexes in solution as well as in solid state.
Transition metal ions in particular form stable complexes having variety of
applications in different fields. Therefore the synthetic study of transition metal
chelates has become the remarkable flowering of inorganic chemistry which has
enriched the chemical science to a high degree.
1.3.1 Brief account of Manganese [ II] Complexes-
Manganese is the twelth most abundant element by weight in the earth’s crust.
It is biologically important in photosynthesis; it shows 2+ as most stable state in
complexes.
Mn(II ) with d5 configuration corresponding to half filled ‘d’ shell is more stable
than other divalent transition metal ions. Most of the complexes are six co-ordinated
and have high spin arrangement of five unpaired electrons186. Some complexes have
square plane and tetrahedral geometries with Coordination Number 4.
Chondhekar187 reported Mn (II) chelates with Schiff bases derived from 5-
hydroxy acetophenone and aromatic amines. The complexes are reported, possess
dimetric tetrahedral geometry on the basis of their spectral and magnetic
susceptibility measurements. Magnetic moments were found to be in the range 4.86-
5.85 B. M. and complexes show M: L ratio 1:1.
Kuntebommana halli et al.188 reported Mn (II) complexes of vanillin
thiosemicabazone(VTSC).
Rao et al.189 reported Mn(II) complexes of Schiff bases derived from 1-tyrosine
hydrazide and o-hydroxy acetophenone.
24
Singh et al.190 reported Mn(II) complexes of Schiff bases derived from
salicylaldehyde and 2-aminobenzophenone-2-thionylhydrazone191.
S
O
HN
N C
NHC
OM
Syamal and Mourya191 have studied Mn(II), Ni(II), Cu(II) and Zn(II)
dioxouranium(VI) and dioxomolybdenum(VI) complexes of tridentate dibasic ONO
donor Schiff base derived from 2-benzothiazole.
Shukla P R192 reported complexes of Mn(II), Fe(II), Co(II) and Ni(II) with some
tri, tetra and hexadentate Schiff bases.
Jojo Joseph et al.193 reported spectral and lattice parameters of transition
metal complexes of polydentate Schiff bases derived from 3-formyl-4-hydroxy
coumarin and 4-amino phenol/2 amino benzoic acid with Mn(II), Co(II), Ni(II) and
Cu(II).
Patel et al.156 reported Mn(II) complexes with Schiff bases derived from β-
diketones and some amines.
Mandlik et al.194 reported synthesis and characterization of Mn(II), Cr (III), Fe
(III), VO(IV), Zr(IV) and VO2(VI) Schiff base complexes.
Aswale et al.195 synthesized Mn(III),Fe(III), Ti(III) etc polychelates derived from
bis-bidentate salicyaldimine.
Hankare et al.196 reported synthesis and characterization of complexes of
Mn(II), Co(II), Ni(II), Cu(II), Zn(II), Cd(II) and Hg(II) with Schiff bases derived from 5-
(2’-thiazolylazo) salicylaldehyde and p-methoxy aniline.
Mitu et al.197 reported synthesis and characterization of Mn(II), Co(II), Ni(II),
Cu(II), Zn(II), Cd(II) complexes of Isonicotinoylhydrazone-1-methyl-2-aldehyde-
pyrrole.
25
Sivakolunthu et al.198 reported synthesis and characterization of Mn(II), Co(II),
Ni(II), Cu(II) and Zn(II) complexes with 8-quinolinyloxyacetic acid.
Khan199 reported complexes of Mn(II), Co(II), Ni(II), Cu(II), Fe(III), Cr(III), Zn
(III) etc with 1,1-(2,6-pyrimidyl-bis-benzothiazole)-2-thione.
Maurya et al.200 reported the synthesis ans characterization of Mn(I)
complexes of biologically active oxygen donor 2 or 3 pyrazoline-5-one derivatives.
NC
NC
OH2
O
NH2
N
Mn
O
C
C NN
C
CH3
CH3
Shakir Mohammad201,202 reported synthesis and physicochemical studies of
complexes with Mn (II), Co(II), Ni(II), Cu(II) and Zn(II) with macrocyclic ligands
derived from 2, 6-diacetylpyridine dihydrazone.
Verkey and Jacob 203 reported synthesis and characterization of zeolite
encapsulated Mn (III) salen complexes.
O
R'
R N
MnO
RN
Cl
R'
Mitu et al.204 synthesized and characterized the complexes of Mn(II), Co(II),
Ni(II) and Cu(II) with Aroylhydrazone ligand.
Hankare et al.205 reported synthesis and characterization of Mn(II), Co(II),
Ni(II) and Zn(II) azo coumarin complexes as follows:
S
N NN
OH
CH
N
OCH3
i) Structure of ligand
26
S
N
NN
O
CH
N
H3CO
S
N
N
N
O
HC N
OCH3
M
M
Cl
Cl
ii) Structure of Complex
M= Mn(II), Co(II), Ni(II), Cu(II), Zn(II), Cd(II) and Hg(II)
Nakamura et al.206 reported the method for stabilizing β-diketone metal
complexes and their compositions for metallographic CVD by selecting metals like
Cu, Fe, Mn, Zn, Al, etc. using R-1COCH2COR2 (R, R2= alkyl groups) in organic
solvent.
Structure of the square planer Cu-L2 complex.
O
O
N
MO
OH
O
N
HO
O
O
Chondhekar et al.207 reported the synthesis of transition metal complexes of
Mn(II), Fe(II) etc with 2-hydroxy / 5’-chlorophenyl acetophenones and p-nitromethyl
benzoic acid and benzaldehyde.
Irudayasamy208 reported the synthesis of complexes of Mn, Fe with 2’-
hydroxychalcone and characterized on the basis of elemental analysis, conductance,
magnetic, electronic and IR studies and found that the complexes are monomeric low
spin and square planer.
27
Peng and yanging et al.209 reported ionic-liquid grafted mn(II) Schiff base complex
prepared with imidazoline and employed as an efficient and recyclable catalyst for
the epoxin.
Swamy210 reported formation constants of metal chelates of
2’hydroxychalcone and 2’hydroxy-5’ methyl chalcone with bivalent metals like Mn(II),
Ni(II), Zn(II), Cd(II) etc
Booth et al. 211 reported reactions between methyl, acetyl and
phenylpentacarbonyl Manganese and acytylenes. The reactions undergo Cis
additions, The PMR and IR Spectra are described.
Nesmeyanov et al.212 reported anisotropic rearrangement of tertiary α-
acetylene alcohols by cyclopentadienyl tricarbonyl manganese and concluded that
the stabilisation of the carbonium ion by C5H4Mn(CO3)3 is probably due to Mn or M-
C5H4 ring electrons.
Abrahams et al.213 reported in situ synthesis of trisubstituted methanol ligands
and their potential as one pot generators of cubane like metal complexes. When
excess Na Sulphite was used, the monoanionic complexes M3Na{(C5H4N)2SO3C(O)-
4} M= Mn, Co, Zn with an M3NaO4 cubane core are formed directly from 2,2’ dipyridyl
ketones.
Nair et al.214 reported synthesis of crosslinked divinylbenzene Me-
methacrylate co-polymer supported β-diketone linked complexes of Mn(II), Fe(III),
Co(II), Ni(II) and Cu(II) and studied the influence of degree of cross-linking of the
polymer support, structural environment of ligand and nature of metals on the rate of
reactions.
Pike et al.215 reported synthesis of dioxyanthraquinone-bridged bimetallic β-
diketonate complexes of Mn(III), Fe(III), Al(III), Cr(III), V(III) and characterized for Uv-
Vis, IR, NMR and fluorescence studies.
Taft et al.216 reported the preparation and characterization of Mn and Fe
alkoxide cubes and found that in [Mn4(OEt)4(EtOH)2(DPM)4] the 4 metal ions and
bridging alkoxides ligands are located at alternating vertices of a cube with either
alcoholic or alkoxide and β-diketonate or benzoate ligands on the exterior of the core.
28
Patel et al.217 reported physiochemical studies of metal β-diketonates. V.
spectral and magnetic properties of Mn(III), Fe(III), Co (III), Al(III) and Cr(III)
complexes of 1-(2-thienyl)-1,3-butanedione and 4, 4, 4-trifluoro-1-(2-thienyl)-1,3-
butanedione.
Patel et al.218 reported physiochemical studies of Mn(II), Fe(III), Co(II), Ni(II),
Cu(II), Zn(II) and Pd(II) complexes of 1-(3-pyridyl)-1,3-butanedione and 4, 4, 4-
trifluoro-1-(3-pyridyl -1,3-butanedione with respect to magnetic and spectral
properties at 83-300K.
Batyr et al.219 prepared the adducts of heterocyclic amines with bis-β-
diketonates of 3d elements i.e. Mn, Fe, Cu, Ni, Co, Zn etc. and their thermal stability
are studied. Ligands are 2,2’-bipyrine, 1,10-phenanthroline and HФ=acetylacetone
etc.
1.3.2 Brief Account of Iron (III) Complexes-
Iron is the fourth most abundant element in the earth’s crust. It is biologically
the most important transition metal in plants and animals functioning as electron
carrier, oxygen carrier and oxygen storage and forms several unusual complexes186.
Iron (III) ion with its d5 configuration has 3+ oxidation state and forms
octahedral complexes with various ligands in general. The tetrahedral and square
planer complexes of Fe (III) are less reported as compared to its octahedral
complexes. The affinity of Fe (III) for amine ligands is very less. No simple amine
complexes exist in aqueous solution as addition of aqueous ammonia to Fe (III) ions
leads to precipitate it as hydroxide4.
Iron (III) has affinity towards ligands which co-ordinate via oxygen. Octahedral
complexes of Fe (III) like [Fe(CN)6]3- are low spin with one unpaired electron having a
magnetic moment of 1.9 B. M. while the complexes [Fe(H2O)6)+3[FeF6]
-3 etc. are high
spin with five unpaired electrons having a magnetic moment of 5.9 B. M.
The affinity of Fe (III) towards oxygen donor is greater than nitrogen donor220.
It has been observed that urea co-ordinates with Fe (III) via oxygen forming stable
complexes. The unidentate ligands with nitrogen donor do not form stable complexes
in aqueous solution. The complexes of the type [Fe(NH3)6]+3 are formed with gaseous
ammonia but they are decomposed immediately, by water at room temperature with
29
release of ammonia4. Ligands such as bipyridil, 1,10-phenanthroline have chelating
nitrogen donor atoms and form stable complexes with Fe(III). The substitution of
metal ion is difficult in such low spin complexes yielded by strong field ligands. A
large number of stable chelates of Fe (III) with many bidentate, tridentate,
tetradentate and polydentate Schiff base ligands are reported 221-223.
Some dimeric complexes such as [Fe(SAL)2en]2 are reported to have
magnetic moment about 1.9 B. M. at 298oK. These complexes are believed to have a
linear Fe-O-Fe system through which magnetic interaction seem to occur224.
Debey et al.226 studied the Fe (III) complexes of Schiff bases derived from
salicylaldehyde and some amines for their composition and abilities.
Manganese (II) and Iron (III) complexes of 2-hydroxy,2-carboxy-phenyl-azo-β-
diketonses are reported to be dimeric225.
Costamagna227 systematically surveyed the literature on Cu(II), Ni(II), Fe(III)
chelates of 2-hydroxy-1-naphthaldehyde and salicylaldehyde.
Abdula et al.228 synthesized and analyzed Mn (II) and Fe (III) complexes of
Schiff bases derived from salicylaldehyde 2-hydroxy acetophenone and ethylene
diamine and found to posses 1:1 (A)and 1:2 (B) metal to ligand ratio respectively.
O
MNR1
O
N R1
Cl
Cl
(A)
R=-H, -CH3M=Fe (III), Mn(II) (B)
OM
N
C
N
C
O
N
R
O
N
R
O
R
R
Vankat Reddy228 has synthesized and characterized the Fe (III) and
Mn(II) complexes of schiff bases derived from 2-hydroxy acetophenone, 2-hydroxy-4-
methyl acetophenone, salicyaldehyde, 3,5 dichloro salicyaldehyde, benzoxazole
hydrazide and benzimidazole and found to possess octahedral geometry.
Mehta et al.229 reported some six co-ordinated Iron (III) schiff base complexes.
30
Palaniandvar et al.230 have reported Fe(III) complex of tridentate ligand
derived from pyridine-2,6-dicarboxylic acid and catechol with structure-C.
O
Fe
O
X
X
N
SOl(C)
X= O or N
Kenaway et al.231 prepared Fe (III) chelates with 4-(-2-hydroxy)-1-
(2,4dihydroxy
benzaldehyde)-3-thiosemicarbazone.
Patange et. al.3 reported synthesis and characterization of solid complexes of
Mn(II), Fe(III), Co(II), Ni(II) & Cu(II) metal ions with chalcones derived from
dehydroacetic acid aromatic and heterocyclic aldehydes.
Mane et. al.4 reported synthesis and characterization of Mn(II), Fe(III), Co(II),
Ni(II) and Cu(II) complexes with ligands derived from dehydroacetic acid and primary
aromatic amines.
Surya Rao et al.232 synthesized Mn(II), Fe(III), Co(II), Ni(II), Zn(II) chelates of
physiologically active schiff bases derived dehydroacetic acid and thiosemicarbazide,
salicylhydrazide and benzoyl hydrazides. The insecticidal activities of some of the
chelates were good.
O
OM
N
O
H3C
CH3
X
N
M=Zn(II), Fe(III), Co(II), Ni(II), Cu(II) and Mn(II)
X= O or S.
Salunke233 reported the synthesis and characterization of Fe(III), Co(II), Ni(II)
Cu(II) and Mn(II) complexes of azo schiff bases derived from dehydroacetic acid and
p-toluidine, p-anisidine, p-bromoanline, o-toluidine, o-anisidine and β-
naphthylamines. The complexes were characterized by UV, IR, NMR conductance,
XRD and antimicrobial analysis and proposed octahedral structure with dimetric
nature as follows-
31
O
OM
N
N
NM
O CH3
O N
O
ArAr
H3C
Ar
CH3
O
N
N
Ar
Cl Cl
Cl
Radhakrishan et al.234 reported complexes of 1,2 dihydro-1,5-dimethyl 1-2-
phenyl-4-formyl (Benzhydrazide)-3H-pyrazol-3-one with structure-
NN
O
Fe
NHCH3C
H3C
Ph
N CH
O
HN
C
Ph
O
NH
Ph
O
NN
CH3
CH3
Ph
XX
X
X= SCN, Cl or Br.
Shetti et al.235 reported synthesis and characterization of schiff bases derived
from 2,6-diformyl, p-cresol and anilines and obtained binuclear complexes with Fe
(III) as-
Fe
O
Fe
O N
N
N
N
Cl
Cl
Cl
Cl
Dubey et al.236 reported the synthesis, reactions and physicochemical
characterization of Iron (III) complexes containing substituted benzoxazole and
various schiff bases moieties.
Dash237 reported interaction of N, N’ ethylene bis (salicylamide) with Fe (III): A
magneto structural electrochemical and mechanistic investigation.
32
Structure of ligand-
OH
O
HN
HN O
HO
Dash and Rath 238 reported phenol amide chelates of Fe (III) i.e. interaction of
1,5-bis-(2-hydroxybenzamido)-3-azo pentane in aqueous methanol medium.
Structure of the complexe= HLFe(OH)23+.
OH
FeNHO
O
NH
O
OH2
Sureshan et al.239 reported epoxidation of olefins by using Mn (III) and Fe
(III) amide complexes with structure-
O
MO
O
O
NH (CH2)n
NH
HN (CH2)n
nH2OCl
Syamal et al.240 reported synthesis of polystyrene supported chelating resin
containing Schiff’s base derived from salicyladshyde and triethylene tetramine and its
Fe (III), Cu (II), Ni (II), Co(II), Mo (II), Zn (II), Cd (II) and Zr (IV) complexes.
Ajaily et al.241 reported the synthesis and characterization of Fe (III), benzoin
complex with structure having 1:1 M-L ratio.
33
O
Fe
OOH
OH
OH2
OH2
Mitu et al.242 reported synthesis and characterization of Cu (II), Ni (II), Co(II),
Mn (II), Zn (II) and Cd (II) complexes of isonicotinoylhydrazone-1-methyl-2-aldehyde
pyrrole.
Heerdt et al.243 reported the study of single-ion and molecular contributions to
the zero splitting in an Fe (III)-oxodimer by single crystal w-band EPR.
Clegg244 reported the study of dinuclear bis-β-diketonato ligand derivatives of
Fe (III) and Cu (II) and use of the latter as components for assembly of extended
metallo supramolcular structures.
Zutin245 reported the synthesis, electrochemical behavior and X-ray crystal and
molecular structures of [Fe (diene) (CO)2 PPh3] diene=chalcone or Sorbic acid.
Constable246 reported control of Fe (II) spin states in 2,2’,:6’.2”-terpyridine
complexes through ligand substitution.
Singh and Kamaluddin247 reported epoxidation of some α, β-unsaturated
carbonyl systems with tert-butyl hydro-peroxide in the presence of Fe (III) Schiff base
complexe (Fe-salen) 20, as catalyst. Presence of electron withdrawing groups in
Phenyl ring of chalcone and high dielectric constant medium favored the yield of
epoxide.
Galkina248 reported reactions of hydrophosphoryl compounds with iron
carbonyl π−complexes of α-enones.
Hemalatha249 reported the synthesis of Fe (III) complexes with two new
bichalcones i.e. 2’, 4’-dihydroxy-5’-(2-hydroxy) cinnamoyl-2-hydroxychalcone and
2’.4’ dihydroxy-5’-(4-hydroxy-3-methoxy) cinnamoyl-4-hydroxy-3-methoxy chalcone
and characterized by elemental analysis, IR, magnetic and conductance
measurements.
34
Gupta250 reported epoxidation of chalcone with tertiary butyl droperoxide in
presence of Fe(III) Schiff base complex i.e. N,N’-ethylenebis(salicylideniminato) Fe
(II) -µ-oxio-N,N’-ethylenebis (Salicyclideniminato) Fe (III) as a catalyst.
Narawade251 reported stability constants of Fe (III) chelates with some
substituted chalcones like 2’-hydroxy-4-methoxy -5’-methylchalcone.
Daniel et al.252 reported regio- and stereoselective addition of carbon
disulphide Fe-complexes to α, β unsaturated carbonyl in the presence of strong
acids.
Nesmeyanov et al.253 reported preparation and molecular structure of chelates
π-allyl-σ carbamoyliron tricarbonyl complexes.
Syamasunder et al.254 reported spectrometric investigation of iron -2’4’-
dihydroxychalcone complex and predicted that chalcones to be used as analytical
reagents.
Misra et al.255 reported the studies on chalcone complexes of Fe (III) with
HL=RCOCH:CH ph and R=8-hydroxy-5-quinolinyl.
Yu, Zhi-gang et al. 256 reported the synthesis and characterization of diphenyl
benzoylpyrazolone and its metallic complexes with Fe (III). HL synthesized is 1-(p-
chloro –phenyl)-3-phenyl-4-benzoyl-pyrazolone-5.
Prasad et al.257 reported synthesis and spectral characterization of Fe (III)
complexes of dioxadiaza macrocycles derived from α-diketones and 1,8 diamino-3,6-
dioxaoctane.
Nowicki et al.258 reported synthesis, spectroscopic and magnetic properties of
Fe (III) complexes with N’N’ ethylene bis (Salicylaldimide) and β-diketones.
35
1.3.3 Brief Account of Cobalt (II) Complexes-
Cobalt is another important element from first transition series of
d-block of the periodic table. Cobalt belongs to VIII group with atomic number
27. Obviously cobalt has low abundance of only 23 ppm by weight in earth’s
crust due to odd atomic number with d7 configuration. Out of the common 2+
and 3+ oxidation states, 2+ state is more stable than 3+. However 3+ state is
stable considerably and is important in complexes. Co (II) ion forms tetrahedral
or octahedral complexes. Less commonly it forms square planer complexes
with bidentate and tetradentate ligands. Formation of both octahedral and
tetrahedral complexes with the same cobalt salt and ligand is common due to
small difference between the stabilities of these geometries. Sometimes these
two geometries are found to be in equilibrium as reported in compounds of
[CoX2(Py)2] type259. Square planer complexes are formed by tetradentate
ligand such as bis (salicylaldehyde ethylene diaminato) ion and porphyrins.
The Co (II) chelates derived from Schiff bases of bromosalicylaldehyde
and sulphamethoxy pyridazine, sulphamethazole, sulphafurazol have been
reported as six co-ordinated260.
Chondehekar187 reported Co (II) complexes of bidentate Schiff bases
derived from 5-chloro-2-hydroxy acetophenone and aromatic amines. They
observed magnetic moments and electronic bands of the chelates with Schiff
bases of p-bromoaniline and 1-naphthylamine are suggested dimeric nature
and further suggested that one nucleus exist as square and other tetrahedral
e.g. (A) and (B).
36
O
Co
N
H3C Ar
N
O
CH3
Cl
Cl
(A)
O
Co
O
Co
N
NCl
Cl
R
R
CH3
H3C
Cl
Cl
(B)
R=
Br
Pereiro et al.261 reported the influence of cobalt complex on thermal properties
of poly(ethylene terphthalate) / polycarbonate. They denoted the effects of
processing time and concentration of cobalt acetyacetonate complex in polyethylene
terphthalate in thermogravimetric (TG) analysis.
Khot 2 reported cobalt complexes of substituted acrylophenone as examples of
complexes of β-diketone ligands as
OCo
O
CH3
OH
NO2
(a)
OCo
O
N(CH3)2
NO2
(b)
O O
O2N
CH3
Mohammad Shakir et al.262 reported 14 and 16-membered
hexaazamacrocyclic Co (II) complexes bearing pendant amine group with octahedral
geometry as-
NN
Co
N
N
N
N
NH2H2N ClCl
37
Syamal263 synthesized new ligands from salicylaldehyde and 5-methyl
pyrazole-3-carbohydrazide and reported Co(II) complexes with octahedral geometry
and dimeric structure.
Co
O
Co
O
O
NO
N
OH2
OH2
OH2
OH2
Prasad et al.264 also reported chalcone complexes with mixed ligands as
O
Co
O
O
OOH2
OH2
R1
R2
R1= H / MeR2= Et / Me
Venkateswar Rao265 reported the synthesis of tetradentated Schiff bases
derived from dehydroacetic acid (DHA and carbohybrazide and their complexes with
various transition metals like Co (II).
N
M
O
N
OOH2
OH2
O O
H3C CH3
O O
HN NH
O
CH3H3C
Venketeswer Rao266 have also reported the Schiff base complexes of
dehydroacetic acid and DL-Histadine with Co(II), V(IV), Ni(II), Mn (II), Fe (II) Cu (II)
etc.
Prasad et al.267 reported synthesis of mixed ligand complexes of Co (II)
containing 5-bromosalicyldehyde and β-diketone, hydroxyl aldehydes or ketones.
Structures obtained are as follows-
38
O
CoO
O
OOH2H
RBr
(a)
R=H,CH3, C2H5, C6H5
O
CoO
O
OOH2H
HBr
(b)OH2
O
CoO
O
O
RH
RBr
(c)
R= CH3, C6H5
Mathew et al.268 reported the synthesis and characterization of Co (II)
complexes of Chromen-2-one-3-carboxyhydrazide and 2-(chromen-2’-only)-5-
(aryl)1,3,4-oxodiazole derivatives.
Structure of metal complex of 1,3,4-oxodiazole-
N
Co
O
O
N
O
OX
Cl
ON
ON
NO2
O2N
X= Cl-/ Br-/ NO3/ CH3COO-/ ClO4-, CNS-/ SO4
Banergy et al.269 reported the synthesis and electrochemistry and single
crystal structure of [Co(α-NaiEt)2(N3)2] Where α-NaiEt=1-ethyl-2(naphthyl-α-
azo)imidazole.
Reaction:
Co(OAc)2+2α-NaiR+2NaN3NaOH
Stir, 298oK[Co(N3)2(α-NaiR)2] + NaOAc
Where R= Me, Et or Bz
Structure of complex –
39
N'
Co
N
N
N'N3
N3
Baranwal et al.270 reported the synthesis and characterization of novel mixed
ligands like ternary carboxylato complexes of Co (II) with Schiff bases HSB having
general formula [Co(OOCR)SB], where R= C11H23, C13H27, C15H31 or C17H35 etc.
Co Co
O O
OO
O N
N O
C6H4
H4C6
R
R
Ar
Ar
O
O
H
Et
Et
H
Ar=Ph / p-Cl-C6H4R=C11H23/ C13H27/ C15H31/ C17H35
Demirhan et al.271 reported the synthesis and characterization of a new vic-
dioxime ligand and its complexes with Co (II). Systematic studies of substituted
derivatives of 1, 10 phenanthroline (Phen) and other α-diimines have been
successfully undertaken272. Nebahat gave the synthesis of a new Vic-dioxime (I) and
its reaction with various metal ions like Co (II).
e.g. synthesis of 5,6-diamino-1,10 phenanthrolino-5-6-bis(2,3-dihydroxyimino-1-aza)
propane prepared, from anti-chloro-methyl dioxime and 5,6 diamino-1,10
phenanthroline to give the Co (II) complex.
40
N
N
NH2
NH2
C
C
H3C
H3C
N
N
OH
OH
NaHCO3N
N
NH
NH
C
C
N
N
CH3
OH
NN
OH
CH3
NOH
NHO
vic-dioxine
2
Co (II) structure obtained is a dimeric species of the polymeric compound as-
N
N
HN
HNN
N
Co
NH
NHCl
Cl
N
Co
N
N
NCl
Cl
CH3H3C
OH
OH
OH
OH
N
Co
N
N
N Cl
Cl
H3CCH3
HO
OH
HO
OH
Khatavkar et al.273 reported the structural investigations of Co (II), Cu (II) and
Ni (II) complexes of phenylazobenzoylacetone.
Awadallah et al.274 reported the synthesis and biocidal activity studies on solid
complexes of Co (II), Fe (II) and Ni (II) with Violuric acid and dinitrosoresorcinol. It
was found that most of the compounds possessed fairly good antibacterial and
antifungal activities.
Panda et al.275 reported the synthesis and characterization of Co (II) with [16]
1,5,6,8,9,13,14,16-octaaza-2.4,10,12-tetraoxo-7,15-dithia-
1,3,3,5,6,8,9,11,11,13,14,16 dodecahydrocyclohexadecane.
41
HN
HN NH
Co
NH
NH NH
NHNH
SS
OO
OO
x-
x-=Cl-/ Br-/ NO3-/ SO4
2-
Singh et al.276 reported synthetic and spectroscopic studies of Co (II)
complexes of pyridine-2-carboxaldehyde thiobenzoyl hydrazone denoted as 2-PTBH.
HN N
S
N
Structure of complexes
N
S N
SM
N
N
N
N
b) [Co(2-PTB)2
S
N S
N
CoNH
HN
N
N
x
x
a) Co (2 PTBH)2 X2, where X =Cl, Br, NCS
HC
CH
Binzet et al.277 reported the synthesis and thermal behavior of Co (II) Ni (II)
and Cu (II) complexes of N, N-di-n-propyl-N’-(2-chlorobenzoyl) thiourea.
Mathews et al.278 reported synthesis and characterization of the complexes of
Co (II) Ni (II), Cu (II) anf Zn (II) with 2-(2-carboxyphenylazo)-1,3-diketones like
acetylacetone, benzoylacetone and dibenzolmethane. The ligand exist entirely as
intromolecularly hydrogen bonded 2-aryl hydrozones and this form persists in metal
chelate in which the hydrogen bonded and deprotonated hydrazeno nitrogen atom
42
and one of the carboxylate oxygen atom bonds with metal ion leaving one of the
carbonyl groups free.
N OCo
O
NOH2
H3C
O CH3
O
Fahiman279 reported substituent effects on the volatility of metal β-diketones.
Volatile trends are established for a series of M (β-diketonate)n complexes , where
M= Cu (II), Co (II), etc and β-diketonate are i) (acac) i.e. acetylacetonate, ii) (tfac) i.e.
trifluoroacetylacetonate, iii) (hfac) i.e. hexafluoroacetylacetonate, etc.
Golding280, Hill et al.281, Abeles282 and Wilkinson283 reported preparation of the
models for vitamin B-12 or Cobaloximes.
e.g. Bis(dimethylglyoxime) ethyl-pyridine Co (III).
e.g. Dibromo(dimethylglyoxime) dimethylglyoxomatocabalt III.
CoBr2
N
N
CH3
CH3
OH
OH
2
O
N
Co
N
OH
N
OH
O
N
CH3
CH3H3C
H3C Br
Br
H
1.3.4 Brief account of nickel (II) complexes
Nickel is moderately abundant and is twenty second most abundant element in
the earth’s crust. Nickel is the member of‘d’ block of the periodic table having atomic
No-28, which is placed in I series of transition metals. The common oxidation state of
Nickel is (II) associated with d8 configuration. Though the chemistry of Ni (II) is simple
but complexes are quite complicated. Square planer and octahedral geometries are
commonly observed. Lee186 has given the account of few tetrahedral, trigonal
bipyramidal structures in his book named as “Concise Inorganic Chemistry”.
43
The square planer complexes with dsp2 hybridization are diamagnetic under
strong field forcing the electrons to pair up. Octahedral and tetrahedral Ni (II)
complexes are paramagnetic due to two unpaired electrons and are associated with
octahedral (sp3d2) and tetrahedral (sp3) geometries respectively.
Chondekar187 reported mononuclear Ni (II) complexes of Schiff bases derived
from 5-chloro-2-hydroxy-acetophenone and aromatic amines.
N
NiO
O
N
CH3
Ar
Ar
CH3
Cl
Cl
Baranwal et al.284 reported the synthesis and characterization of substituted
derivatives of Ni (II) carboxylates with Schiff bases. The complex is reported to
possess linear trimeric structure with each Ni (II) centre having octahedral geometry.
o o
o o
Nio
o
o
o
Ni
Ni o
o
o
o
oo = bidentate ligand
Shivakumaraiah et al.285 reported monochelates and bischelates of Ni (II) with
bis-benzimidazolyl derivatives.
The intention behind above study is the report of the binding of histidine
imidazole to Ni (II) in various biological centres given by Cammack286.
Nickel is an essential trace element present in many hydrogenases which is
reported by Van Der Zwaan et al.287. Sorell288 reported metal complexes of
44
multidentate Nickel-heterocycles containing imidazole moiety for metalloenzymes
and metalloproteins.
Brajesh Kumar et al.289 reported the physico-chemical and spectral studies of
Ni (II) complexes of 2-subtituted benzaldehyde semicarbazone and
thiosemicarbazones the chemistry of which is receiving considerable attention due to
their pharmacological properties. Padhye et al.290 reported a wide range of medicinal
properties of semicarbazones and thiosemicarbazones and their metal complexes.
Hussain Reddy291 reported the synthesis and characterization of Ni (II)
complexes of some heterodonor ligands like 2,4-dihydroxyacetophenone-2-imino-
ethanethiol (DAET) etc.
C
CH3
N
SHOHHO
Structure of complex (binuclear)
N
X X
X
N
X
Ni Ni
OH2
OH2
OH2
OH2
X= O or S
Manimekalai et al.292 reported the studies on Ni (II) complexes of
benzoylhyrazones, They synthesized Ni (II) complexes of the type [NiLOH.
2H2O]2.nH2O, where L is either Cis-2,6 diphenyltetrahydrothiopyran-4-one benzoyl-
hydrazone. i.e. DTTBH
Structure of DTTBH-
S
NNH
O
Ph
Ph
Or trans-3-methyl-cis-2,6 diphenyl piperidine-4-one benzoylhydrazone i.e.
MDPBH.
Structure of MDPBH-
45
HN
NNH
O
Ph
Ph
CH3
Metal complexes of aroylhydrazone have broad application in biological
processes, such as in the treatment of tumour, tuberculosis, leprosy and mental
disorder293, 294.
Ligands DTTBH and MDPBH react in the enol form with metal ions. For Ni (II)
complexes enolic oxide bridged dimeric strucuture has been proposed.
Ni
O
Ni
ON
N C
N
NC
S
S
OH2
OH2
HOOH2
OH2
OHPh
PH
H
H
Ph
Ph
4 H2O
Waldemar Adam et al.295 reported a convenient synthesis of Ni (II) and Co (II)
complexes of unsymmetrical salen-type ligands and their application as catalysts.
Salen-type ligands with N and O atoms are important as their metal complexes find
widespread applications as homogenous catalysis in variety of reactions296 e.g. use
of Ni (II) complexes as highly active for polymerization of olefins297.
Structure of complex
46
O
Ni
NHC
O
CHN
Xiaoyan et al.298 reported α, β unsaturated carbonyl compounds as Hard/ soft
chelating ligands in methyl Nickel phenolates and investigated the structure of trans-
methyl-2-(3-phenyl-2, 3-η-2-propenoyl) phenolato bis (trimethylphosphine) Nickel (II)
complex.
Biradar299 reported synthesis and characterization of complexes of Ni (II) with
O,O’ dihydroxychalcones.
Chaston300 et al. reported thioderivatives of β-diketones and their Nickel (II)
chelates.
1.3.5 Brief account of copper (II) complexes
Copper is one of the ancient metals used by human being in his evolution. It is
one of the most transition element from first row of d-block of the periodic table. It is
moderately abundant and is the twenty fifth most abundant elements in the earth’s
crust. Copper is extensively studied for complexation with its most stable oxidation
state259 as 2+.
Cu (II) ion with d9 configuration provides an opportunity for observation of the
Jahn-Teller effect associated with additional stabilization besides crystal field
stabilization energy (CFSE). Number of Cu (II) complexes with bidentate ligands
containing O and Nickel donor atoms has been reported by Tan301 and
Chondhekar302.
They found to have square planer, tetrahedral and octahedral geometries.
In our laboratory Chondhekar302 reported both mononuclear and binuclear
Copper (II) complexes of Schiff bases derived from 5-chloro-2-hydroxy
acetophenones and aromatic amines e.g. A and B.
47
O N
Cu
ON
R
R'
R'
R
Cl
Cl
(A)
Cu
OCu
O
N
NR'
R
R'
R
Cl
Cl(B)
BrBr
Parashar et al.303 reported the Cu (II) complexes of salicyldahyde Schiff bases
with 2 substitutes aniline with square plane geometry.
O NCu
ON
R
R' R'
R'
Carugo et al.304 synthesized Cu (II) complexes of 4-hydroxy-6-methyl-3[3-
dimethylacryloyl]-2H-pyran-2-one. This complex is reported to have
pentacoordination with square pyramidal stereochemistry having pyridine in the
apical position.
O O
O OCu
N
O
O
O
O
CH3N
N
H3C
48
Djedouni et al.305 reported Cu (II) complexes of Bis[3-acetyl-6-methyl-2-H-
pyran-2,4(3H)-dionato]bis(dimethyl suphoxide) i.e. [Cu (C8H7O4)2(C2H6OS)2].
The complex shows Cu (II) ion octahedrally co-ordinated with the type MO6.
The bidentate dehydroacetic acid ligands occupy the equatorial plane of the complex
structure in trans configuration and DMSO is co-ordinated through O at apical
positions.
O
Cu
O
O
O
OMe2
OSMe2
O
O
H3C
CH3
O
O
CH3
H3C
Mishra et al.306 reported synthesis, spectroscopic studies, molecular, structure
optimization and superoxide dismutase of Cu (II) and Zn (II) bipyridyl assisted
supramolecular motifs containing octadentate Schiff base. Structure of [ Cu2
(bipyridine)2. tsdb] complex , where tsdb=N, N’, N”,N’”-tetrasalicylidene-3,3’-
diaminobenzidine.
N N
N NCu
O
ONN
NN
O
O
Cu
Salunke-Gawali et al.307 reported thermal magnetic and electro-chemical
properties of polymeric copper complexes of 2-hydroxy-1-4-naphthalo-quinone and
its methyl derivative.
Shahada et al.308 reported synthesis, characterization and thermal studies of
new chelating Fulven monomers, polymers and their metal complexes e. g. Cu (II).
49
Mokerrem Kurtoglu et al.309 reported synthesis , characterization and biological
evaluation of Cu (II), Co (II) and Ni (II) complexes of Schiff base-b m b H i.e. 4-[{4-
(benzyloxy) phenyl]-imino} methyl] benzene-1, 3-diol.
Structure of the complex-
O
Cu
N
N O
OH
OH
O
O
Gulnur Keser Karaoglan310 reported synthesis and characterization of a new
Schiff bases namely-2-(6-(E)-1-(2-hetadecylcarbonyl-oxyphenyl)
methylideneamino)[1, 10] phenanthrolin-5-yl-imino methylphenyl sterate with Cu (II),
Ni (II) and Co (II) salts.
Structure of the complex-
O
Cu
N
ON
OO
C17H35
C17H35
H
H
N
N
50
Shriver311 denoted the use of Cu (acac)2 complexe in the method of chemical
vapour deposition (CVD) in order to prepare thin films needed for the
superconductors in electronic devices.
Nakamura312 reported the method stabilizing β-diketone metal
complexes and their compositions for metalorganic CVD.
O
O
M
R1
R2 n
M= Cu, Mn, Zn, Co, Mg etc.
R1 & R2=alkyl group
n>0
Devi et al.313 reported the synthesis, characterization and chemical vapor
deposition of a novel Cu (II) chemical vapor precursor.
Fahiman et al.279 reported substituent effects on volatility of metal β-diketones.
Volatile trends are established for a series of M (β-diketonate) n complexes, where
M=Cu (II), Co (II), While β-diketonates are acetyacetonate (acac);
trifluoroacetylacetonate (tfac) or hexafluoroacetylacetonate (hfac).
Teghil et al.314 reported the thermodynamic study of the sublimation processes
of Cu and Al acetylacetonate.
51
1.3.6 Literature Survey of Emine Complexes with Metals
Literature survey revealed that enamines or ketoenamines can be subjected to
different reactions and substituted products are obtained.
Fanshawe et al.315 reported substituted enaminoketones. They claimed for
substituted enaminoketones of the formulae.
O
NH2
R
and
NH2
O
R
Where R is selected from the group consisting of pyridyl and pyrazinyl.
Yong-Ming et al.185 reported the transformation of β-bromodifluoromethyl β-
enaminoketones.
Endo Kohel et al.316 reported addition of Zn salts of stabilized cabanion
species to isolated olefins. They described the deprotonation reaction of
enaminoketones, which were available from 1, 3dicarbonyl compounds was
foundwith an equimolar amount of dialkylzinc under mild conditions. The resulting
organozinc reagents react with a cyclopropenone acetal to afford a carbometalation
product in high yield.
Gerhard et al.317 reported the synthesis of enaminoketone sulphides of the
formula-
O N
R1
SPh (Y)y
R2
R3
R4
Where R1, R2, R3 and R4 = alkyl or hydrogen.
Y= halogen, alkoxy, alkyl, nitro or cyano group
y = integer ranging from 0-3.
Larina et al.318 reported the use of enaminoketones and enhydrazides in the
synthesis of phosphorus-nitrogen containing heterocycles and Phosphorylated
enamines.
52
The scheme given by Larina can be established that 4-arylamino-3-penten-2-
ones react with phosphorus pentachloride to form 4-Nickel-aryl, Nickel-
dichlorophosphyrylamino-2-chloro-1,3-
pentadienyltrichlorophosphoniumhexachlorophosphorates I. Compound I as well as
diphosphoric acid chloroanhydride II readily prepared from compound I undergo
heterocyclisation to 1,2, azophosphine III and IV with cleavage of phosphorous
chloride.
NH
R O
Ar3PCl53HCl N
Cl3P
R Cl
Ar
POCl2(I)
PCl6-
-POCl3
NP+
RCl
Ar
(III)Cl Cl
2 HCOOH
-POCl3-4HCl
-2CO
N POCl2
RCl
Ar
POCl2(II)
-POCl3
NP
RCl
Ar
(IV)O Cl
Ar= Ph, p-MeC6H4 p-NO2C6H4R= H, Me
No references cited for enamines enaminoketones complexes with metals.
53
1.4 AIM OF THE PRESENT INVESTIGATION
Bacon F. in 1620 stated that “Those who aspire not to guess and divine, but to
discover and know, who propose not to devise mimic and fabulous worlds of their own, but
to examine and dissect the nature of this very world itself, must go facts themselves for
everything”319.
-
-
-
-
“What is Chemistry?” The answer lies in the significance of each letter forming
the word ‘CHEMISTRY”-
Such as:
C - Curiosity
H - Honesty
E - Enthusiastic efforts
M - Magnificent
I - Infinity / Intelegence
S - Search
T - Truth
R - Real
Y - Yearn
Therefore “Chemistry can be defined as an intelegent efforts and honest yearn
originating from curiosity for better understanding of infinite journey of nature, which
results in the search for real truth lieing at the very root of the universe”.
� � �
54
“Where is Chemistry?”. Answer is ‘Chemistry is everywhere, right from atom
to universe. Therefore, it can be given that “chemistry is omnipresent similar to vital
force of universe (Vishva-Chaitanya) or God. There is no place without chemistry. The
concept of earth, fire, water, wood and sky (Panch Mahabhute) is full of chemistry
which is composed of elements and uncountable number of their compounds.
Inorganic chemistry is the important basic branch of chemistry, which has
experienced and impressive renaissance. Academic and industrial research in
inorganic chemistry is flourishing and the output of research papers and reviewers is
growing exponentially320.
Large areas of inorganic chemistry remain unexplored, so new and often
unusual inorganic compounds are constantly being synthesized in laboratories. Such
exploratory inorganic syntheses, especially in co-ordination chemistry continue to
enrich the field with compounds that give us new perspectives on structure, bonding,
reactivity and biological activities. In addition to its intellectual attractions, we can
learn that inorganic chemistry has considerable practical impact and touches on all
other branches of science. e.g. In industrial field, eight of the top ten industrial
chemicals by weight are inorganic. Inorganic chemistry is also essential to the
formulation and improvement of modern materials such as catalysts, semiconductors,
superconductors, light guides, non-linear optical devices and advanced ceramic
materials. The environmental impact of inorganic chemistry is huge. In this
connection the extensive role of metal ions (especially transition metals such as Fe,
Co, Ni, Cu, Mn, Cr, Zn, Mo etc) led to the triving area of bioinorganic chemistry which
may be extended upto biotechnology and genetic engineering311.
Bioinorganic chemistry is a leading discipline in which many critical processes
require metal ions including respiration, metabolism, nitrogen fixation,
photosynthesis, nerve transmission, muscle contraction, signal transduction and
protection against toxic and multigenic agents. Unnatural metals have been
introduced into human biology as diagnostic probes and drugs. Numbers of
biomolecules are co-ordination compounds formed from metal ions with organic
groups321.
55
This inspired for the search for the synthesis of organic ligands and
their transition metal chelates. Among the different functionalized chromones, 3-
formylchromones occupy an unique position because they can be transformed into
various heterocycles169.
Studies on co-ordination chemistry behavior of potentially important
ligands containing various organic functional groups with transition metals are a
subject of interest. The development of numerous organic chelating ligands that can
co.ordinate with transition metal ions has opened up a broad scope to research. The
transition metal complexes of bidentate to polydentate organic chelating ligands
containing oxygen-oxygen (e.g. chalcones, β-diketones etc.), oxygen-nitrogen (Schiff
bases) or Nitrogen-sulpher–(thiosemicarbazides)-oxygen etc. are proved to be the
potential donor sites have been reported.
3-Formyl chromones i.e. 4-OXO-4H-[1]-benzopyran-3-carboxaldehyde is a
versatile synthone i.e. precursor for number of compounds like pyrazoles oxazoles,
pyrimidines enamones etc. Upon condensation with different nucleophiles.
These 3-formylchromones give important intermediates, which can be used for
the synthesis of some important heterocyclic compounds of metal complexes.
Compounds having chromone moiety are associated with interesting biological
activities170 associated with this nucleus are antibacterial, antifungal, antidiabetics. In
chromone, substituents at 2 and 3 positions have been reported to possess coronary
dilatory relaxation activity, muscular relaxation effect, antimicrobial and analgesic
activity.
When 3-formylchromones are refluxed with piperidine in ethanol, gave 1-(2-
hydroxyl-phenyl)-3-piperidin-1-yl-propenone i.e enaminoketones.
OH
O
N
It is planned to undertake comprehensive investigation of transition
metal complexes of enaminoketones. The work includes synthesis of variously
substituted ligands derived from 3-formylchromones and piperidine as-
56
[1]-1-(2-hydroxy-5-chloro-phenyl)-3-piperidine-1-yl-propenone-L1.
OH
O
NCl
[2]-1-(2-hydroxy-5-methylphenyl)-3-(piperidin-1-yl)prop-2-en-1-one-L2
OH
O
NH3C
[3] 1-(2-hydroxy-3,5-dimethylphenyl)-3-(piperidin-1-yl)prop-2-en-1-one-L3
OH
O
NH3C
CH3
[4]1-(3-chloro-2-hydroxy-5-methylphenyl)-3-(piperidin-1-yl)prop-2-en-1-one-L4
OH
O
NH3C
Cl
[5] 1-(3,5-dichloro-2-hydroxyphenyl)-3-(piperidin-1-yl)prop-2-en-1-one-L5
OH
O
NCl
Cl
With this aim in view, the present study deals with the synthesis of complexes
in solid state using transition metal ions like Mn (II), Fe (II), Co (II), Ni (II) and Cu (II),
with synthesized enaminoketones designated as L1, L2, L3, L4 and L5. The
characterization of ligands have been proposed to carry out using elemental analysis,
57
M.P., conductivity, IR, NMR and UV/ Visible spectral study. The characterization of
metal complexes of enaminoketone ligands have been proposed to carry out using
elemental analysis, M.P., conductivity, IR, NMR and UV/ Visible spectra, magnetic
susceptibility, TGA / DTA and X-ray powder diffraction study.
Ligands as well as complexes are also proposed for the study of the
biological activity, so as to confirm whether there is enhancement in this property of
ligands due to metal Co-ordination.
All these investigations are to be used for structural prediction of transition
metals complexes.
58
1.5 REFERENCES
1. “Chemistry” –Raymond Chang, Mc-grow hill publication, New Yark. 7th
International edition.
2. Khot B R – Ph.D. Thesis, Department of Chemistry, Shivaji University,
Kolhapur (Jan 1990).
3. Patange V N– Ph.D. Thesis, Department of Chemistry, Dr. BAMU,
Aurangabad (June 2007).
4. Mane V G– Ph.D. Thesis, Department of Chemistry, Dr. BAMU,
Aurangabad (May 2007).
5. Werner A Z, Inorganic Chem, 3, 1893, 267.
6. Brown W Z, Inorganic Chem, 164, 1927, 345.
7. Blomstrand ‘Chemier der’ Jetztzeit Heidelberg, 1869 & Ber, 4, 1871, 40.
8. Jorgensen C K, J Prakt Chem, 18(2), 1978, 209.
9. Lewis G W, J Amer Chem Soc, 38, 1916, 762.
10. Kossel, Ann phys, 49, 1916, 229.
11. Sidgwick J, J Chem Soc, 123, 1923, 725.
12. Fajans, Naturedissenchaflen, 11, 1923, 165.
13. Pauling L, J Amer Chem Soc, 53, 1931, 1367 and 54, 1932, 988.
14. Bethe H, Ann-physik, 3, 1929, 133.
15. Van Vleck J H, Phys Rev, 41, 1960, 208.
16. Mulliken R S, J Chem Physique, 46, 1940, 497.
17. Balhausen C J & Cray, ”Introductory notes on moleculer orbitial theory”,
Benzamin (N Y) 1965.
18. Langmuir I L, J Amer Chem Soc, 41, 1919, 868, 1543.
19. Pandhare G R– Ph.D. Thesis, Department of Chemistry, Dr. BAMU,
Aurangabad (Mar 2004).
20. Orgal L E, “An Introduction to Transition Metal Chemistry”, Mathuen,
London 2nd Ed, 1966.
21. Poulet H J, J Chimie Physique, 54, 1967, 258.
22. Griffith J S, Trans Faraday Soc, 56, 1960, 193.
23. Dun T M, “Modern Co-ordination chemistry” (Ed Lewis & Wilkins) Inter
59
Science, 234, 1960.
24. Dun T M, Ibid, 239.
25. Jorgensen C K, “Absorption spectra & bonding in complexes “, Permon
Press, N Y, 1962.
26. Rossoti F J & Rossoti H, “The determination of stability constants”, MC
Graw Hill Book Co, N Y, 1961.
27. Morgan K C & Drew, J Chem Soc, 117, 1920, 1456.
28. Martell A. E.& Calvin M. “Chemistry of the Metal Chelate Compounds”
N Y, prentice Hall, Inc, 1952.
29. Feiffer Z P, Anorge Allegen Chem, 97, 1936, 230.
30. Yatsimirsky K B, “Medical Aspects of Bio-inorganic Chemistry”, 1983.
31. Flaschka H A & Bernard A J “Chelates in Analytical Chemistry” Vol-I,
Marcell Dekker, N Y, 1967.
32. Dwyer F P & Mellor D P “Chelating agents & Chelates”, Acdemic Press,
N Y, 1964.
33. Swift H E, Bozik T G & Wu Complexes Y, J Catalysis, 17, 1970, 331.
34. Harkal S D- Ph.D. Thesis, Department of Chemistry, Rostock
University, Germany (2005).
35. Tiwari S K & Sharma L M, J Indian Chem Soc, 73, 1996.
36. Williams D, “An Introduction to Bioinorganic chemistry, spring field II
linois, Thomas, 1976.
37. Eichnorm G L “Advances in Chemistry series No 37, Am Chem Soc,
Washigton, D C, 1963, 19.
38. M. N. Hughes,”The Inorganic chemistry of Biological process London,
wiley, 1972.
39. Seven M J & Johnson L A,”Metal binding in Medicine” J B Lippicott
Co.Philadelphia, 1960.
40. Lippard S J & Berg J M, “Principles of Bioinorganic chemistry”
University Science Books, Mill Valley, California 1994.
41. Lemberg & Lagge. ”Hematin compounds and Bile Pigments” New York,
Interscience Publishers, Inc. 1949.
60
42. Martell & Calvin, chemistry of metal Chelate compounds, Chapter 8,
New York, Pretice Hall, Inc. 1952.
43. Eichhorn G L, ‘Co-ordination Compounds in natural product’ and Bailer
J C, ‘The Chemistry of the Co-ordination compounds’ Reinhold, New
York, 1956.
44. Shukla J P, Pai S A ,Khopkar P K & Subramnian M S, J Inorg Nucl
Chem, 36, 1974, 3862.
45. Taneja A D, J Inorg Nucl Chem, 35(10), 1973, 3617.
46. Mc Donald M R & Kunitz M, J Gen Physiol, 25, 1941, 53.
47. Green M M, Glaner J A, Cumningham L M & Neurath H, J Amer Chem
Soc, 74, 1952, 2122.
48. Rilter L, Chemical Abstract, 50, 1956, 10348.
49. Tubes M & Morrison D C, Chemical Abstract 17, 1966, 603 & 66, 1967,
16132.
50. Gale L F, Chemical abstract, 72, 1967, 35830.
51. Baker W A (Junior) & Brown P M, J Amer Chem Soc, 88, 1966, 1314.
52. Ransmeir J C, J Clin-Invest, 28, 1949, 977.
53. Benet L Z & Goyam J E J Pharma Sci Eng, 54(7) 1965, 983.
54. Albert A, Nature, 172, 1953, 201.
55. Albert A, Rubbo S D, Goldacre R J & Balfour B G, Brit J Exp Pathol, 28,
1947, 69.
56. Rubbo S D, Albert A & Gibson M I, Brit J Exp Pathol, 31, 1950, 425.
57. Rubbo S D, Ibid, 34, 1953, 19.
58. Trace J C & Edds G T, Am J Vet Res, 15, 1955 639.
59. Weinberg E D, Cook E A & Wisner C A, Proc soc Am Bacteriologists,
42, 1956.
60. Stoves J L, Mfg Chemists, 25, 1954, 148.
61. Weinberg E D, Bacteriol Revs, 21, 1947, 46.
62. Newton B A, Nature, 172, 1953, 160.
63. Ofye W M & Lange W E, J Amer Pharm Assoc, 44, 1955, 261.
61
64. Ishidate M & Kanao, Anal Chim Acta, 22, 1960, 452 and C A, 54, 1960,
14205.
65. Donovick R, Bayan A P, Canales P & Pansy F, J Bacteriol, 56, 1948,
125.
66. Pramer D, Arch Biochem and Biophys, 62, 1956, 265.
67. Weinberg E D, Bacteriol Revs, 21, 1957, 46.
68. Albert A, Experientia, 9, 1953, 370.
69. Bergel M, Semana Med (Bucnos Aires), 100, 1952, 807.
70. Batterman R C, J Amer Med Assoc, 152, 1953, 1053.
71. Grief R L & Pitts R F, J Clin Invest, 35, 1956, 38.
72. Handley C A & Seibert R A, J Pharmacol Exp Therap, 116, 1956, 27.
73. Weiner I M & Miller O H, J Pharmacol Expert. Therap, 113, 1955, 241.
74. Libbermann D, Nature, 164, 1949, 142.
75. Rosenzweig S, Chemical Abstract, 45, 1951, 5186.
76. Idem, J Amer Pharm Assoc, 44, 1955, 261.
77. Danysz, Compt Rend, 164, 1917, 746, Ibid, 1955, 644.
78. Rosenzweig S & Fuchs W M, Chemical abstract, 45, 1951, 5186.
79. Cook E S, Kreke C W, McDevitt M & Bart M D, Lett J Biol Chem, 164,
1946, 43.
80. Eagle H & Doak G O, Pharmacol Rev, 3, 1951, 107.
81. Schubert M. first symposium on Chem, Biological Correlation Natl Acad
Sci Natl Res council, Washington D C, 269, 1951.
82. Albert A & Magrath, Biochem J, 41, 1947, 534.
83. Tewari G D& Mishra M N, Br Med J , 2, 1962, 325.
84. Andrews A C, Lyone T D & Brein T D O, J Chem Soc, 1962, 1776.
85. Murukami Y, Nakamura K & Tokunara M, Bull Chem Soc Japan, 36(6),
1963, 669.
86. Halmekoski J, Soum Kemistrilehti, 35, 209, B-35, 1962, 238.
87. Jameson R F & Neillei W F S, J Inorg Nucl Chem , 31(12), 1966, 3809.
88. Smith T D, Carr & Pilbro J R, J Chem Soc, 16A, 1971, 2569.
62
89. Muro I, Morishina & Yonezawa T, Chem Biol Interaction, 3(3), 1971,
213.
90. Sinsteri S, Villa L & Ferri V, Pharmacol, Ed Sci, 23(2), 1971, 210.
91. Vijayvargia B L, Chakrawarti P B & Sharma H N, J Indian Chem Soc, 57,
1980, 471.
92. Chakrawarti P B, Vijayvargia B L & Sharma H N, J Indian Chem Soc, 59,
1982, 734.
93. Chakrawarti P B, Vijayvargia B L & Sharma H N, J Indian Chem Soc, 60,
1983, 89.
94. Chakrawarti P B, Vijayvargia B L & Sharma H N, J Indian Chem Soc, 63,
1986, 1036.
95. Chakrawarti P B, Vijayvargia B L & Sharma H N, J Indian Chem Soc, 64,
1987.
96. Bag S P, Fernando O & Freiser, Archiv Biochem Biophys, 106, 1964,
379.
97. Nayan R & Dey A K, Indian J Chem, 10, 1972.
98. Cheney G E, Freiser H & Fernando O, J Amer Chem Soc, 81, 1959,
2611.
99. Nayan R & Dey A K, Z Natur Forsch, 27b, 1972, 688.
100. Nayan R & Dey A K, J Indian Chem Soc, 50, 1973, 98.
101. Nayan R & Dey A K, Z Natur Forsch, 25b, 1970, 1453.
102. Chakrawarti P B & Shrivastva S, Nat Acad Sci Letts (Ind), 4(6), 1981,
243.
103. Chakrawarti P B & Shrivastva S, J Indian Chem Soc, 62, 1985, 265.
104. Chakrawarti P B & Shrivastva S, J Indian Chem Soc, 63, 1986, 688.
105. Frust A, “Chemistry of chelation in cancer,” Thomas Springfield, Illinois,
1963.
106. Brown D A & Chidambaram M V, “Metal Ions in Biological Systems,” Ed.
H. Sigel, Marcell, Dekkar, New York, 14, 1982, 5.
107. Dash K C & Schimidbaur H, “Metal Ions in Biological Systems,” Ed. H.
Sigel, Marcell, Dekkar, New York, 14, 1982, 6.
63
108. Rosenberg B, “Metal Ions in Biological Systems,” Ed. H. Sigel, Marcell,
Dekkar, New York, 10, 1982, 8.
109. Kanopkaite S & Brazenas G,“Metal Ions in Biological Systems,” Ed. H.
Sigel, Marcell, Dekkar, New York, 10, 1982, 8.
110. Passov H, Rothstain A & Clarkson T W, Pharmac Rev, 13, 1961, 185-
224.
111. Gilman A, Phillips F S & Roberta P, J Pharmac Exptl Therap, 87, 1946,
85.
112. Hurch J B, U S Atomic Energy Comm Anal, 50, 1956, 9268(b).
113. Nichimura H, Nagasaki Igakkai Zassi, 31, 1956, 153 &. Chemical Abstact,
50, 1956, 9268(b).
114. Peters R A, Stocken L A & Thompson R H S, Nature, 156, 1945, 616.
115. Stocken L A & Thompson R H S, Physiol Revs, 29, 1949, 168.
116. Matthews W B, Milne M D & Bell M, Quart J Med, 21, 1952, 425.
117. Popovic A, Chickter C Reinovsky A & Rubin M, Proc Soc Expl Biol Med,
74, 1950, 415.
118. Spencer H, Vankinscott V, Lewin I & Laszlo D, J Clin Invest, 31, 1957,
1023.
119. Grant M M, Arch Opthol (Chicago), 48, 1952, 681.
120. Aposhian H V, Fedn Proc Am Soc Expl Bio, 20, 1961, 85.
121. Goldberg S, Br Med J, 1, 1963, 1270.
122. Seven M J, Scheinberg I H, Ibid CH, 38.
123. Harris C E, Can Med Assos J, 79, 1958, 664.
124. Bannerman R M & Sheilla T, Br Med, J 2, 1962, 1573.
125. Rosenberg B, Plat Inet Rev, 15, 1971, 42.
126. Broomfield R J, Nature (London), 223, 1969,735.
127. Cleave M J & Hoeschale J D, Bio Inorg Chem, 2, 1973, 187, Plat Met
Rev, 17, 1973, 2.
128. Williams D R, Chem Rev, 72, 1972, 203.
129. Cleave M J, & Hides P C,’ Metal ions in Biochemical systems’ Vol II Ed H
Sigel Marcel Dekkar, New York and Besel, 1980.
64
130. Gandolfi C, & Bium J, Inorg ChemActa, 80, 1983, 103.
131. Giraldi T, Cancer Res, 37, 1977, 262.
132. Das M & Livingstone, Brit J Cancer, 38, 1968, 325.
133. Cleave M J, Co ord Chem. Rev, 12, 1974, 349.
134. Das B & Aditya S, J of Indian chemical society, 36, 1959, 473.
135. Schwarzenbach G & Willi H, Helv chem. Acta, 134, 1951, 528.
136. “Stability constants” supplement No. 1 special publication 25, The
Chimical Society London, 359.
137. Freedman N J & Plane R M, Inorg Chem, 2, 1963, 11.
138. Jabalpurwala K E & Milburn R M, J Am Chem Soc,88, 1966, 3224.
139. Kulkarni V D Ph. D. Thesis, Marathwada University, Aurangabad.
140. Mehrotra R C, Bohra R & Gaor D P,”Metal diketones and allied
derivatives, Academic press, New York, 1978.
141. Dasgupta H C & Sing V, J Indian chem Soc, 55, 1978, 853.
142. Yamada S, Co Ord Chem Reves, 1, 1966.
143. Bhosale S B Ph D Thesis, Dr. BAMU, Aurangabad, 1995.
144. Ghosh C K & Khan Smriti, J Synthesis, 9, 1981, 719.
145. Ghosh C, Pal C & Bhattacharya A, Indian Journal of chemistry, 24B,
1985, 914.
146. Joshi N S, Karale B K, Jagtap A P, Shinde S M, Bhirud S B, Gill C H
Indian J Heterocycl chem, 13(2), 2003, 151.
147. Dalavi N R, Ph. D. Thesis – University of Pune, 2006.
148. Medola R, Kuntzen H S & Brightman R, J Chem Soc,97, 1910, 456.
149. Sciff H, Ann Supp, 3, 1964.
150. Rajaram & Trans V, Metal chem.(Weinheim Ger) 9(2), 1984, 48-51.
151. Lions F & Barry, Aust J chem., 22, 1969, 17-87.
152. Pachling S Ph D Thesis, Dr BAMU Aurangabad, July, 2001.
153. Mane P S Ph D Thesis, Dr BAMU Aurangabad, May, 2001.
154. Maurya R Complexes, Pandey A & Sutradhar D, Indian J Chem, 43A,
2004, 763.
155. Ceriyan M & Mohanan K, Asia J Chem, 19 (4), 2007, 2831-2838.
65
156. Patel I A, Thaker B T & Thaker P B, Indian J Chem, 37A, 1998, 429.
157. Dyke S F, “The chemistry of enamines”, Cambrige University Press.
158. Robinson R, J Chem Soc,109, 1916, 1038.
159. Hamilton E E P, & Robinson R, ibid, 1029.
160. Stork G, Brizzolara A, Landesman H, Szmuszkovicz J & Terell R, J Am
Chem Soc, 85, 1963, 207.
161. Joshi N S, Karale B K, Jagtap A P, Shinde S M, Bhirud S B & Gill C H,
Indian J of Heterocycl Chem, 13, 2003, 151.
162. Kumar A & Malhotra E S et al., Indian J Chem, 41B, 2002.
163. Eomuodson R S, Dictionary of organo-phosphorous compounds
(chapman and Hall), London.1988.
164. Lowe W, Synthesis, 1976, 274.
165. Lowe W, Ann Chem, 1977, 1050
166. Basinski W, Jerzmawska Z & Pol, J Chem, 57, 1983, 471.
167. Gosh C K & Khan S J, Synthesis, 9, 1981, 719.
168. Mousawi S A, john E & Kandery N A, J Hetrocyclic Chem, 41(3), 2004,
381.
169. Dalvi N R, Shelke S N, Karale B K, & Gill C H, Syn Commun, 37,2006,
1421.
170. Karale B K, Ph. D. Thesis ‘A search for some potentially active
heterocyclic compounds’ BAMU, A’bad, 2000.
171. Ghosh C K, J Hetrocyclic chem, 20, 1983, 1437.
172. Szent-Gyorgyi A, Biokhikiya, 2, 1937, 151.
173. Nohara A, Umetani T & Sanno Y, Terahedron Lett, 30 (19), 1974, 3553.
174. Reddy K R S, Shrimannarayana G, Rao NVS, Proceedings of Indian
Academic Sci sect A, 81(5), 1976, 197.
175. Benard M, Hulley E, Molenda H & Stochla K, Pharmazine, 41 (8), 1986,
560.
176. Cekavicius B, Odynets A G, Sausins A, Berzina D & ZOlotoyabko R M,
Khim Pharm Zh, 21 (8), 1987, 959.
177. Buu Hoi N B, Xyon N D & Symo, Bull Soc Chim, 1956, 1946.
66
178. Kuhn R & Hensel H, Ber, 86, 1953, 1333.
179. Ariyon R & Suschitzky H, J Chem Soc, 1961, 2242.
180. Chadrakanta Ghosh, Chandana Pal & Atanu Bhattacharyya, Indian
Journal of Chem, 24, 1985, 914.
181. Zagorevskii VA, Orlova EK & Tsvetkova ID, Inst Farmakol Moscow &
USSR, Khimiya Gaterotsiklicheskikh Soedineii,4, 1972, 457.
182. Ghosh, Chandrakanta, Bandyopadhyay, Biswas C & Subhabrata, Ind J
Chem, 29 B (9), 1990, 814.
183. Ghosh, Chandrakanta & Khan Smriti, Synthesis, 9, 1981, 719.
184. Zagorevskii VA, Orlova EK, Tsvetkova I D, Vinokurov VG, Troitskaya VS
& Rozenberg SG, Khimiya Geterotsiklicheskikh Soedineii, 7 (6), 1971,
723.
185. Yong-Ming Wu, Ya Li & Juan Deng, Key laboratory of organofluorine
Chemistry, Shanghai Institute of Organic Chemistry, Chinese Academy of
Science, 354, Fenglin Rd, Shanghai 200032, China, 2005
186. Lee J D., “Concise Inorganic chemistry “ELBS 4th Edn Chapman and Hall
Ltd. London, SEI 8 HN, 1995.
187. Chondhekar T K, Acta Ciencia Indica, 14 C (4) 1988, 297.
188. Kuntebommanahalli N T, Gujjarhalli T Complexes, Winston D L & Cyril P,
Trans Met Chem, 10, 1985, 299.
189. Rao T R, Sahay M & Agrawal R C, Ind J Chem, 24A, 1985, 649.
190. Singh B & Shrivastav A K, Proc Ind Acad Sci (Chem Sci), 103, 1991, 691.
191. Syamal A & Mourya M, Trans Met Chem, 11, 1986, 201.
192. Shulka P R, Ahmed N, Chandra S, Mishra S & Rastogi R, J Indian Chem
Soc, LXV, 1988.
193. Joseph J & Mehta B H, Asian J Chem, 19 (1), 2007, 401.
194. Madlik P R, More M B & Aswar A S, Indian J Chem, 42A, 2003, 1064.
195. Aswale S R, Mandilk P R, Aswale S S & Aswar A S, Indian J Chem, 42A,
2003, 322.
196. Hankare P P, Gavali L V, Bhuse V M, Delekar S D & Rohade R S, Indian
J Chem, 43 (A), 2004, 2578.
67
197. Mitu L, Kriza A & Dianu M, Asian J Chem, 19 (7), 2007, 5666.
198. Sivakolunthu S, Saroja B & Sivasubramanian S, Indian J Chem, 37(A),
1998, 357.
199. Khan T A, Shahajahan & Zaidi S A, Indian J Chem, 37 (A), 1998,161.
200. Maurya R C, Verma R, Indian J Chem, 37 (A), 1998, 147.
201. Mohammad S, Chingsubam P, Chisti H T N, Azim Y & Begum N, Indian
J Chem, 43 (A), 2004, 556.
202. Sureshan C A, Bhattacharya P K, Indian J Chem, 37 (A), 1998, 897.
203. Varkey S P & Jacob C R, Indian J Chem, 37 (A), 1998, 407.
204. Mitu L & Kriza A, Asian J Chem, 19, 2007, 658.
205. Hankare P P, Naravane S R, Bhuse V M, Delekar S D & Jagatap A H,
Indian J Chem, 43, 2004, 1464.
206. Keiichi N, Tani, Takashi, Ueda, Takashi, Saito, Makato, JPN Kokai
Tokkyo Koho, 2005, 17.
207. Akuskar S K, Chondhekar T K, Dhuley D G, Asian J Chem, 9(3), 1997,
336.
208. Irudayasamy M, Nagarajan S, Asian J Chem, 1 (3), 1989, 214.
209. Peng, Yanging, Cai, Yueguin, Song, Gonghua, Chen, Jing, Synlett, 14,
2005, 2147.
210. Swamy S, Jaganna T, Lingaiah P, Indian J Chem, 16A (8), 1978, 723.
211. Booth, Brian L, Hargreaves R G, J Chem Soc (A), 2, 1970, 308.
212. Nesmeyanov A N, Anisimov K N, Kolobova N E, Magomedov G K,
Zhurnal Organicheskoi Khimii, 3 (7), 1967, 1149.
213. Abrahams, Brendan F, Hudson, Timothy A, Robson, Chem- A Europian J,
12 (27), 2006, 7095.
214. Nair V A, Sreekumar K, J Poly Mat, 19 (2), 2002, 155.
215. Pike, Robert D, Choy, Jaso L, Fletcher, Gary M, Guy, Kathryn A, J Am
Chem Soc, 168, 1998, 23.
216. Taft, Kingsley L, Caneschi, Andrea Pence, Laura E, Delfs, Christopher D,
Papaefthymiou, Georgia C, Lippard S, J Amer Chem Soc, 115 (25),
1993, 11753.
68
217. Patel K S & Adimado A A, J Inorg and Nucle Chem, 42 (9), 1980, 1241.
218. Patel K S & Feniran J A, J Inorg and Nucle Chem, 39 (7), 1977, 1143.
219. Batyr D G, Balan V T, Marchenko G N USSR , Biologicheskie
Khimicheskie Nauki, 1973, 61.
220. Abdula, El-Wafa & Moustafa H M, Rev Roum Chim, 38(7), 1993, 837.
221. Cotton F A & Wilkinson G.,”Advanced Inorganic Chemistry”, 1972, 890.
222. Figgis B N & Lewis J, Progr Inorg Chem, 6, 1969, 107.
223. Swamy S J & Reddy A D, J Indian Chem Soc, 77, 2000, 336.
224. Cotton F A, Coordin Chem Rev, 8, 1972, 185.
225. Dissouki, Hassan A I, Moustafa R & Moustafa M, Inorg Chemica Acta,
1990, 1265.
226. Dubey K P & Wasil B L, Proc Nat Acad Sci Sec-A, 55 (4), 1985, 297.
227. Costamagna, J Coord Chem Rev, 119, 1992, 67.
228. Venkatreddy G, Ph.D. Thesis, Department of Chemistry, Osmaniya
University, Hyderabad, A P, India, (1982).
229. Mehta B H & Purandare K V, Oriental J Chem, 14, 1998, 71.
230. Palaniandvar M, Dhanalakshmi T, Bhuvaneshwari M, J Inorg Biochem,
100, 2006, 1527.
231. Kenaway M M, Gaber M, Abu, Usama El-Ayaan & Khattab M A, Indian J
Chem, 33 (A), 1994, 914.
232. Rao D S & Ganorkar M C, Curr Sci, 49 (13), 1980, 511.
233. Salunke S D–Ph.D. Thesis, Dr. BAMU, Aurangabad, (July 2001).
234. Radhakrishnan P K & Raju K C, Indian J Chem, 44A, 2005, 1812.
235. Shetti U N, Revankar V K & Mahale V B, Indian J Chem, 37 A, 1998, 540.
236. Debey R K, Dubey V K & Mishra C M, Indian J Chem, 45 A, 2006, 2637.
237. Dash A C, Mishra A , Indian J Chem, 37A, 1998, 961.
238. Dash A C & Rath R K, Indian J Chem, 43 A, 2004, 310.
239. Sureshan C A, & BhattacharyaP K, Indian J Chem, 37A, 1998, 897.
240. Syamal A & Singh M M, Indian J Chem, 37 A, 1998, 350.
241. EL-Ajaily M M, Maihub A A, Abuzwida M A, Aboukrishna M M, Amar A A
& Asaih E A, Asian J Chem, 19 (1), 2007, 281
69
242. Mitu L, Kriza A & Niadu M, Asian J Chem, 19 (7), 2007, 5666.
243. Heerdt T, Stefen P, Goovaerts M, Etienne, Caneschi, Andrea, Cornia,
Anddrea, J Magnetic resonance, 179 (1), 2006, 29.
244. Clegg, Jack K, Leonard F, McMurtrie, John C & David S, ??? check it??,
5, 2005, 857.
245. Zutin K, Nogueira V M, Mauro A E, Melnikov P, Lluykhin A, Polyhedron,
20, 2001, 1011.
246. Constable, Edwin C, Gerhard B, Eckhard, Dyson, Raylene, Eldik V, Rudi,
Fenske, Dieter, Karderli, Susan, Morris, Darrell, Neubrand, Anton, Markus
N, Smith D R, Karl W, Margareta Z, Zuberbuhler, Andreas D, Chem-A
European J , 5 (2), 1999, 498.
247. Kamaluddin, Singh H V, Oxidation Commun, 18 (3), 1995, 275.
248. Gaikina I V, Saakyan G M, Galkin V I, Cherkasov R A & Kazan, Zhurnal
Obshchei Khimii, 63 (10), 1993, 2221.
249. Hemalatha G, John M A, Venkatraman V R & Nagarajan S, Asian J
Chem, 3 (3), 1991, 342.
250. Gupta D R, Kamaluddin, Shobha N, Indian Curr Sci, 50 (18), 1989, 1016.
251. Narwade M L, Chincholkar M M & Sathe S W, J Indian Chem Soc, 62 (3),
1985, 194.
252. Daniel P & Pierre D, Organometallics, 1 (10), 1982, 1401.
253. Nesmeyanov A N, Rybinskaya M I, Rybin L V, Gubenko N T, Bokii N G,
Batsanov A S & Struchkov Y T, J organometallic Chem, 149 (2), 1978,
177.
254. Syamasundar K S V, Indian Academic Sci, 59A (4), 1964, 241.
255. Misra, Dwivedi P C, Upadhyaya R K, Singh V P, Gupta D R, J Indian
Chem Soc, 57 (1), 1980, 107.
256. Zhi-gang Y, Liu Bo, You, Zhao-di Yang, Cheng-bin C, Huaxue Shiji, 29
(12), 2007, 708.
257. Prasad R N, Amita J, J Indian Chem Soc, 84 (9), 2007, 850.
258. Nowicki & Waldmar, Transition Metal Chem, 21 (5), 1996, 469.
70
259. Gill N S, Nylhom R S, Barclay C H, Christie T L and Pauiling P J, Inorg
Nucl Chem, 18, 1961, 88.
260. Lehtnin & Marie, Acta Pharm Fenn, 2, 1981, 90.
261. Pereira P S Complexes, Mendes L Complexes, Dias M L & Sirelli L, J
Thermal Analysis and Calorimetry, 2007.
262. Shakir M, Azim Y, Christi T N, Begum N, Chingsuban P and , Siddiqui, J
Braz Chem Soc, 17, 2006, 272.
263. Syamal A, Trans Met Chem, 11, 1986, 172.
264. Prasad R N, Agrawal A A & Sharma K M, J Indian Chem Soc, 83, 2006.
265. Rao V P & Narasaih V, Indian J Chem, 42 A, 2003, 1899.
266. Rao V P, Ashiwini K & Fatima K, National Academy Sci india, LXXV (A),
2005.
267. Prasad R N, Sharma K & Agrawal A, Indian J Chem, 46 A, 2007, 600.
268. Mathew G, Suseelan M S & Krishna R, Indian J Chem, 45 A, 2006, 2040.
269. Banergee D & Sinha C, Indian J Chem, 45 A, 2006, 2224.
270. Barawal B P, Singh A K, Fatima T & Gupta T, Indian J Chem, 45 A, 2006,
2006.
271. Nebahat D, Erden I & Aviciata U, Inorg Chem, 43 A, 2004, 782.
272. Mossod A & Hodgson D J, Inorg Chem, 32, 1993, 4839.
273. Khatavkar S B, Sadana G S & Deshmukh A A, J Indian Chem Soc, LXV,
1988, 529.
274. Awadallah R M, Mohamed A E & Ramdan A M, J Indian Chem Soc, LXV,
1988, 532.
275. Panda A K, Dash D C, panda A & Mishra P, Indian J Chem, 37 A, 1998,
67.
276. Singh N K & Agrawal N R, Indian J Chem, 37 A, 1998, 276.
277. Binzet G, Arslan H & Kulco N, Asian J Chem, 19 (7), 2007, 5711.
278. Mathews C, Mohnan K, Indian J Chem, 19 (4), 2007, 2831.
279. Fahman, Bradley D, Barron & Andrew R, Advanced Mat optics &
electrnics, 10, 2000, 223.
280. Golding B T, Chem In Britain, 26, 1990, 950.
71
281. Hill, J Chem Soc A, 1969, 554.
282. Abeles R H & Dolphin D, Account Chem, 9, 1976, 114.
283. Wilkinson G, Comprehensive Organometallic Chem, 5, 1984.
284. Barnawal B P, Das S S & Singh P, Indian J Chem, 37 A, 1998, 826.
285. Shivakumaraiah & Nanje Gowda N M, Indian J Chem, 42 A, 2003, 1856.
286. Cammack R, Adv Inorg Chem, 32, 1988, 297.
287. Zwaanjw V D, Albracht S P J, Fontijn R D & Roelofs Y B M, Biochim
Biophys Acta , 872, 1986, 208.
288. Sorell T N, Tetrahedron, 45, 1989, 3.
289. Kumar B, Sangal & Kumar A, Asian J Chem, 19 (1), 2007, 647.
290. Padhye S B, Kauffman G B, Coord Chem Rev, 12, 1985, 63.
291. Hussain R K & Lingappa Y, Indian J Chem, 36 A, 1998, 1130.
292. Manimekalai A & Senthil S B, Indian J Chem, 43 A, 2004, 2568.
293. Cymerman C J, Willis D, Rubbo S D & Edgar , J nature, 176, 1955, 34.
294. Chohan Z H & Rauf A, Inorg Met-Org Chem, 26 (4), 1996, 591.
295. Waldemar A & Chantu R S, Indian J Chem, 43 A, 2004, 56.
296. Wilkinson G, Comprehensive Co-ordination chemistry, Pergamon press,
New York, 2 (6), 1987.
297. Ittel S D, Johnson L K & Brookhart M, Chem Rev, 100, 2000, 1169.
298. Xiaoyan Li, Hongiian, Sun, Floerke, Ulrich, Klein & Hans F,
Organometallics, 24 (18), 2005, 4347.
299. Biradar N S, Patil B R & Kulkarni V H, Inorganica Chimica Acta, 15 (1),
1975, 33.
300. Chaston S H H, Livingstone S E, Lockyer T N, Pickles V A & Shannon J
S, Australian J Chem, 18 (5), 1965, 673.
301. Tan S F, Ang K P, Jayachandran H L, Transition Met Chem, 9, 1984, 390.
302. Chondhekar T K, Khanolkar D D, Indian J Chem, 25, 1986, 868.
303. Parashar R K & Sharma R C, Inorg chemica Acta, 157, 1988, 201.
304. Carugo O, Bisi C & Rizzi M, Polyhedron, 9 (17), 1990, 2061.
305. Djedonai A, Abderrahem B, Soflane B, Adel B & Tahar D, Acta Cryst, 62
E, 2006, 33.
72
306. Mishtra L, Bindu & Bhattacharya S, Indian J Chem, 43 A, 2004, 315.
307. Salunke-Gavali S, Rane S, Boukheddaden K, Codjovi E, Linares J, Varret
F & Bakare P, Indian J Chem, 43 A, 2004, 2563.
308. Shahada L A & Amin R R, Asian J Chem, 19 (2), 2007, 1153.
309. Mokerrem K & Ispir E, Asian J Chem, 19 (2), 2007, 1239.
310. Karaoglan G K, Aciata V & Gul A, Indian J Chem, 46 A, 2007, 1273.
311. Shriver D F, Atkins P W & Lanford C M, “Inorganic chemistry” IInd Ed,
Oxford University Press, Oxford, 1994.
312. Keiichi N, Takashi T, Ueda T & Makoto S, Jpn Kokai Tokkyo Koho, 2005,
17.
313. Devi A, Goswami J, Lakshmi R & Shivshankar S A, J Mat Research, 13
(3), 1998, 687.
314. Teghil R, Ferro D, Bencivenni L & Pelino M, Thermochimica Acta, 44 (2),
1981, 213.
315. Joseph F W, Stephen C L & Robert S, U S Pat, 1976, 3997, 530.
316. Kohel E, Masaharu N & Eiichi N, Nippon Kagakkai Koen Yokoshu, 81 (2),
2002, 1132.
317. Gehard H, Alt & Speziale, Coeve C, MO Patent, 1969, 3, 452, 001.
318. Larina L I, Bozhenkov G V, Abramova E V, Borisov & Rozinov V G,
Russian Pat.
319. Cotton F A & Wilkinson G, “Basic Inorganic chemistry “Wiley Eastern
Pvt”, 4835/24 Ansari Road, Daryaganj, New Delhi-11002, 1986.
320. Cotton F A & Wilkinson G, “Advanced Inorganic chemistry “A
comprehersive text, Wiley Eastern Pvt”, J, 41, South extension 1, New
Delhi-49, 1972.
321. Lippard S J, Berg J M, ”Principles Of Bioinorganic chemistry” Unversity
Science books, Mill Valley C A 94941 California-U S A.