Search tips
Search criteria 


Logo of bioinorgchemapplJournal's HomeManuscript SubmissionAims and ScopeAuthor GuidelinesEditorial BoardHome
Bioinorg Chem Appl. 2010; 2010: 960571.
Published online 2010 July 4. doi:  10.1155/2010/960571
PMCID: PMC2910486

Mononuclear and Dinuclear Manganese(II) Complexes from the Use of Methyl(2-pyridyl)ketone Oxime


The reactions of methyl(2-pyridyl)ketone oxime, (py)C(Me)NOH, with manganese(II) sulfate monohydrate have been investigated. The reaction between equimolar quantities of MnSO4 · H2O and (py)C(Me)NOH in H2O lead to the dinuclear complex [Mn2(SO4)2{(py)C(Me)NOH}4] · (py)C(Me)NOH, 1 · (py)C(Me)NOH, while employment of NaOMe as base affords the compound [Mn(HCO2)2{(py)C(Me)NOH}2] (2). The structures of both compounds have been determined by single crystal X-ray diffraction. In both complexes, the organic ligand chelates through its nitrogen atoms. The IR data are discussed in terms of the nature of bonding and the structures of the two complexes.

1. Introduction

There is currently a renewed interest in the coordination chemistry of oximes [1]. The research efforts are driven by a number of considerations. One of these is that they are considered to be reasonable models for the biologically significant imidazole donor group of the amino acid histidine [2]. Thus, they potentially can be used for the synthesis of various nuclearity metal clusters to model Mx sites in biomolecules, including elucidating the structure and mechanism of action of the CaMn4 core of the water oxidizing complex within the photosynthetic apparatus of green plants and cyanobacteria [3, 4]. In addition, metal complexes of oximes can be used in several other applications, that is, the solution of pure chemical problems [5, 6], the development of new oxygen activation catalysts based on nickel(II) polyoximate complexes [7] and the application of metal ion/oxime systems as efficient catalysts for the hydrolysis of organonitriles [8]. In the latter, metal ions can behave as extremely strong activators of RCN molecules towards nucleophilic attack by OH/H2O. Other applications of metal complexes of oximes include the design of Ca2+- and Ba2+-selective receptors based on site-selective transmetallation of polynuclear zinc (II)/polyoxime complexes [9], the study of metal-ion assisted organic transformations [10], and the mechanistic investigation of corrosion inhibition by Acorga P5000 (a modern corrosion inhibitor comprising 5-nonylsalicylaldoxime as a mixture of carbon-chain isomers) on iron surfaces [11]. Note also that oximate ligands are employed in the synthesis of homo- and heterometallic [1, 12] clusters and coordination polymers [13] with interesting magnetic properties, including single-molecule magnetism [1416], and single-chain magnetism [17] behavior.

Ligands containing one oxime group and one pyridyl group, without other donor sites, are popular in coordination chemistry. Metal-free pyridine oximes exhibit a plethora of biological properties including action on the cardiovascular system, sedative, antidepressant, antispasmodic, cytotoxic, antiviral, and bactericidal activities, while they are good antidotes for poisoning by organophosphorus compounds [18]. Most of these ligands contain a 2-pyridyl group, and thus are named 2-pyridyl oximes, (py)C(R)NOH (Scheme 1). The anionic forms of these molecules, (py)C(R)NO, are versatile ligands for a variety of research objectives, including μ2 and μ3 behaviour; the activation of 2-pyridyl oximes by 3d-metal centers towards further reactions is also becoming a fruitful area of research. The majority of the metal complexes of these ligands have been prepared in the last 15 years and much of their chemistry remains to be explored in more detail [1].

Scheme 1
General structural formula and abbreviations of simple 2-pyridyl oximes, including methyl(2-pyridyl)ketone oxime [(py)C(Me)NOH].

With only few exceptions [19, 20], the hitherto structurally characterized metal complexes containing neutral 2-pyridyl oximes as ligands are mononuclear. The donor atoms of the neutral 2-pyridyl oximes in metal complexes are the nitrogen atom of the oxime group and the nitrogen atom of the pyridyl group. Thus, (py)C(R)NOH behave as N,N'-chelating ligands (see Scheme 2) making necessary the employment of additional inorganic or organic anions to complete the coordination sphere of the metal centre or to balance the charge of the complex cation. A variety of monoanions have been used for this reason, for example, PhCO2 [21], Cl [22, 23], Br [24], and NO3 [25]. Recently, we have started a research program to explore the use of the sulfate ion, SO42−, in 3d-metal/2-pyridyl oxime chemistry, instead of the abovementioned monoanionic ligands. The possible advantages of using SO42− include (i) the possibility of triggering aggregation of preformed smaller species into new products, and (ii) the possible diversion of known reaction systems developed using inorganic monoanions to new species as a result of the higher charge and higher denticity of the sulfate ligand.

Scheme 2
The common coordination mode of the neutral 2-pyridyl oximes and the Harris notation [26] which describes this mode.

The sulfate ion [27] is currently a ligand of intense interest. The μ2, μ3, μ4, μ5, μ8,  or μ10 potential of SO42− (Scheme 3) prompted as to combine 2-pyridyloximes with the sulfate ligand to aim at new types of compounds.

Scheme 3
The up to now crystallographically established coordination modes of the sulfato ligand and the Harris notation [26] which describes these modes.

In this paper, we report the synthesis and the X-ray structural characterization of the two new Mn(II) complexes [Mn2(SO4) 2 {(py)C(Me)NOH}4]·(py)C(Me)NOH (1·(py)C(Me)NOH) and [Mn(HCO2)2 {(py)C(Me)NOH}2] (2) which contain the neutral methyl(2-pyridyl)ketone oxime as organic ligand. The IR data are discussed in terms of the nature of bonding and the structures of the two complexes.

2. Experiments

All manipulations were performed under aerobic conditions using materials and solvents as received. IR spectra were recorded on a Perkin-Elmer PC16 FT-IR spectrometer with samples prepared as KBr pellets.

[Mn2 (SO4)2 {(py)C(Me)NOH}4 ]·(py)C(Me)NOH (1·(py)C(Me)NOH) —

Solid MnSO4 · H2O (0.067 g, 0.40 mmol) was added to a slurry of (py)C(Me)NOH (0.054 g, 0.40 mmol) in H2O (15 cm3); the solid soon dissolved and the solution was stirred for 1 hour at room temperature. The resultant solution was left for slow evaporation. After one week, yellow crystals appeared which were collected by filtration, washed with cold H2O (1 cm3), cold MeOH (1 cm3) and ice-cold Et2O (2 cm3), and dried in air. The yield was 79% (based on the metal). Found %: C, 42.94; H, 3.89; N, 14.51. Calc % for C35H40O13N10S2Mn2: C, 42.78; H, 4.10; and N, 14.25. Selected IR data (KBr, cm−1): 3420 (wb), 3150 (m), 3069 (m), 2843 (m), 2363 (w), 2343 (w), 1654 (w), 1593 (s), 1561 (m), 1476 (s), 1437 (m), 1327 (m), 1285 (w), 1215 (m), 1124 (s), 1080 (s), 1030 (s), 1010 (s), 989 (s), 781 (s), 748 (m), 683 (m), 631 (m), 592 (m), 561 (w), 494 (w), 452 (w), and 447 (w).

[Mn(HCO2 )2 {(py)C(Me)NOH}2 ](2) —

Solid NaOMe (0.090 g, 1.50 mmol) was added to a colourless solution of (py)C(Me)NOH (0.204 g, 1.50 mmol) in CH2Cl2 (20 cm3); the solid soon dissolved. Solid MnSO4·H2O (0.250 g, 1.50 mmol) was then added and the resulting solution was stirred for 24 hours at room temperature. A small quantity of undissolved material was removed by filtration and the dark brown filtrate layered with Et2O (40 cm3). Slow mixing gave X-ray quality yellow crystals of the product. The crystals were collected by filtration, washed with cold H2O (1 cm3), cold MeOH (2 cm3), and ice-cold Et2O (2 × 3 cm3), and dried in air. The yield was 45% (based on the metal). Found %: C, 46.95; H, 4.26; N, 13.43. Calc % for C16H18O6N4Mn: C, 46.82; H, 4.13; N, 13.98. Selected IR data (KBr, cm−1): 3412 (mb), 3073 (w), 2362 (m), 1846 (m), 1597 (s), 1562 (s), 1475 (s), 1436 (m), 1365 (s), 1348 (s), 1326 (m), 1250 (w), 1165 (w), 1137 (m), 1042 (s), 961 (m), 782 (s), 751 (s), 683 (m), 562 (w), and 458 (w).

2.1. X-Ray Crystallography

For 1·(py)C(Me)NOH, X-Ray data were collected at 298 K using a Crystal Logic Dual Goniometer diffractometer with graphite-monochromated Mo-Ka radiation (λ = 0.71073 Å). Lorentz, polarization, and Ψ-scan absorption corrections were applied using Crystal Logic software. Symmetry equivalent data were averaged with Rint = 0.0084, to give 3727 independent reflections from a total 3964 collected. The structure was solved by direct methods and refined by full-matrix least-squares on F2, using 3727 reflections and refining 325 parameters. All nonhydrogen atoms were refined anisotropically. Hydrogen atoms were either located by difference maps and were refined isotropically or were introduced at calculated positions as riding on bonded atoms.

For 2, X-ray data were collected at 100 K using a Oxford Diffraction diffractometer with graphite-monochromated Mo-Ka radiation (λ = 0.71073 Å). Symmetry equivalent data were averaged with Rint = 0.0160, to give 9343 independent reflections from a total of 13039 collected. The structure was solved by direct methods and refined by full-matrix least-squares on F2, using 9343 reflections and refining 258 parameters. All non-hydrogen atoms were refined anisotropically. Hydrogen atoms were either located by difference maps and were refined isotropically or were introduced at calculated positions as riding on bonded atoms.

Details of the data collection and refinement for 1·(py)C(Me)NOH and 2 are given in Table 1.

Table 1
Crystal data and structure refinement for 1· (py)C(Me)NOH and 2.

3. Results and Discussion

3.1. Synthetic Comments

Treatment of MnSO4·H2O with one equivalent of (py)C(Me)NOH in H2O gave a colorless solution from which the new dinuclear compound [Mn2 (SO4 )2 {(py)C(Me)NOH}4 ]·(py)C(Me)NOH (1·(py)C(Me)NOH) was obtained in ~80% yield. Its formation can be summarized in (1).

equation M1

The nonstoichiometric MnSO4·H2O to (py)C(Me)NOH reaction ratio (1 : 1) employed for the preparation of 1·(py)C(Me)NOH (Section 2) did not prove detrimental to the formation of the complex. With the identity of 1·(py)C(Me)NOH established by single-crystal X-ray crystallography, the “correct” stoichiometry (1 : 2.5) was employed and led to the pure compound in high yield.

As a next step, we decided to add base in the reaction mixture targeting the deprotonation of the organic ligand. Thus, treatment of MnSO4·H2O with one equivalent of (py)C(Me)NOH and one equivalent of NaOMe in CH2Cl2 gave a dark brown solution from which the mononuclear compound [Mn(HCO2)2{(py)C(Me)NOH}2] (2) was obtained. Its formation can be summarized in(2)

equation M2

To our surprise, an amount of the methoxide ions did not act as proton acceptors but they got oxidized to formates (HCO2) during the aerial aggregation process [28]. Thus, the organic ligand in 2 is neutral. As expected, the nature of the base is crucial for the identity of the product; employment of NEt3, NMe4OH, NEt4OH, LiOH·H2O etc. leads to dark brown oily materials that have not been characterized. Also, note that: (i) The color of 2 (yellow) is different than the color of the reaction mixture (dark brown, this colour is characteristic of MnIII or MnII/III species), and (ii) a similar reaction, but with (py)C(ph)NOH instead of (py)C(Me)NOH, yields the octanuclear mixed-valent cluster [MnII4 MnIII4O4(NO3)2{(py)C(ph)NO}8(HCOO)2 (MeOH)2] [29] whose core consists of two butterfly subunits. These observations indicate that compound 2 is not the only product of the reaction and that, presumably, a higher nuclearity cluster, with the metals at higher oxidation states, is present in solution. Work is in progress to isolate the second product from the reaction mixture.

3.2. Description of Structures

Selected interatomic distances and angles for complexes 1·(py)C(Me)NOH and 2 are listed in Tables Tables2 and2 and and4,4, respectively. The molecular structures of the two compounds are shown in Figures Figures1 and1 and and22.

Figure 1
The dinuclear molecule present in 1·(py)C(Me)NOH. Primes are used for the symmetry-related atoms.
Figure 2
The molecular structure of compound 2.
Table 2
Selected dond lengths (Å) and angles (°) for 1·(py)C(Me) NOH.a
Table 4
Selected dond lengths (Å) and angles (°) for 2.

Complex 1·(py)C(Me)NOH crystallizes in the triclinic space group P-1. Its structure consists of dinuclear [Mn2(SO4)2{(py)C(Me)NOH}4] molecules and (py)C(Me)NOH molecules in the crystal lattice. The dinuclear molecules lie on a crystallographic inversion center. The two MnII atoms are bridged by two η1: η1: μ2 or 2.1100 (Harris notation [26]) sulfato ligands; two N,N ′-chelating (py)C(Me)NOH ligands complete six coordination at each metal center. The ligating atoms of (py)C(Me)NOH are the nitrogen atoms of the neutral oxime and 2-pyridyl groups. Thus, adopting the Harris notation, (py)C(Me)NOH behaves as an 1.011 ligand.

The coordination sphere of the MnII ion in 1·(py)C(Me)NOH exhibits a slightly distorted octahedral geometry as a consequence of the relatively small bite angles of the chelating ligands [N1–Mn–N2=70.11(10), N11–Mn–N12=70.19(10)°]. Both sulfato oxygen atoms O(31) and O(32′) are trans to the pyridyl nitrogen atoms N(1) and N(11), respectively. Each metal center adopts the cis-cis-trans configuration considering the position of the coordinated SO42− oxygen, pyridyl nitrogen and oxime nitrogen atoms, respectively. The cis arrangement of the oxime groups seems unfavourable, probably due to the steric hindrance arising from the methyl group upon oxime coordination. The long Mn (...) Mn' distance [5.040(2) Å] is a consequence of the presence of the two syn, anti sulfato bridges.

The molecular structure of 1·(py)C(Me)NOH is stabilized by intramolecular hydrogen bonds (Table 3). Each coordinated (py)C(Me)NOH oxime group is strongly hydrogen bonded to an uncoordinated O atom of the sulfato ligand (O33 or O33′). Thus, O33 (and its symmetry equivalent) participates in two hydrogen bonds.

Table 3
Dimensions of the hydrogen bonds in complex 1·(py)C(Me) NOH.a

Complex 2 crystallizes in the monoclinic space group P21/n and its structure consists of mononuclear [Mn(HCO2)2{(py)C(Me)NOH}2] molecules. Two bidentate chelating (py)C(Me)NOH molecules (1.011 [26], see Scheme 2) and two monodentate HCO2 ions create six-coordination at the MnII ion. The coordination geometry of the metal ion is distorted octahedral. As 1·(py)C(Me)NOH, complex 2 is the cis-cis-trans isomer considering the positions of the coordinated HCO2 oxygen, pyridyl nitrogen and oxime nitrogen atoms, respectively.

Intramolecular hydrogen bonds are present in the structure of 2 (Table 5). The oximic oxygen atom of each (py)C(Me)NOH ligand is very strongly intramolecularly hydrogen bonded to one uncoordinated formate oxygen atom.

Table 5
Dimensions of the hydrogen bonds in complex 2.a

Complexes 1·(py)C(Me)NOH and 2 join a small but growing family of structurally characterized metal complexes containing the neutral or anionic forms of methyl(2-pyridyl)ketone oxime as ligands. The 1.011 ligation mode is the exclusive one for the metal complexes containing the neutral ligand [22, 24, 30].

The structurally characterized Mn complexes of (py)C(Me)NOH and/or (py)C(Me)NO [14, 3133] are collected in Table 6, together with the cores of the polynuclear complexes and the ligands' coordination modes for convenient comparison. Closer inspection of Table 6 reveals that compound 1 is the first member of this subfamily in which the MnII ions are linked by the SO42− ion. Complex 2 can be compared with the compound [MnII(O2CPh)2{(py)C(Me)NOH}2] [33] which contains terminal PhCO2 ions, instead of HCO2 in 2; the HCO2 versus PhCO2 change has little structural effect.

Table 6
Formulae, coordination modes of the ligands, and cores of the structurally characterized Mn complexes of (py)C(Me)NOH and/or (py)C(Me)NO.

3.3. IR Spectra

Complexes 1 and 2 exhibit medium to strong intensity IR bands at ~3400 cm−1, assignable to ν(ΟH) vibrations of the (py)C(Me)NOH molecules. The broadness and relatively low frequency of these bands are both indicative of hydrogen bonding.

The ν(C=N)oxime and ν(N–O)oxime vibrations for the free ligand appear as medium intensity bands at 1566 and 1116 cm−1, respectively [34, 35]. The 1116 cm−1 band is shifted to a lower wavenumber in 1 and 2 (1, 1080; 2, 1042 cm−1). This shift is attributed to the coordination of the neutral oxime nitrogen [22]. The strong band at 1124 cm−1 in the spectrum of 1·(py)C(Me)NOH should also have a ν(N–O)oxime character resulting from the presence of lattice (py)C(Me)NOH molecules in the structure. Several bonds appear in the 1655-1400 cm−1 region for both complexes; contribution from the ν(C=N)oxime and δ(OH) modes (>1580 cm−1) are expected in this region, but overlap with the stretching vibrations of the aromatic rings and the carboxylate groups (for 2) renders assignments and discussion of the coordination shifts difficult.

The in-plane deformation band of the 2-pyridyl ring of free (py)C(Me)NOH at 637 cm−1 shifts upwards in 1 (683 cm−1) and 2 (683 cm−1), confirming the involvement of the ring-N atom in coordination [36]. The appearance of a medium intensity band at 631 cm−1 in the spectrum of 1·(py)C(Me)NOH is indicative of the presence of lattice (py)C(Me)NOH molecules in this complex.

The IR spectrum of the free, that is, ionic, sulfate (the SO42− ion belongs to the Td point group) consists of two bands at ~1105 and ~615 cm−1, assigned to the ν3(F2) stretching [νd(SO)] and ν4(F2) bending [δd (OSO)] modes, respectively [27, 37, 38]. The ν1(A1) stretching [νs(SO)] and ν2(E) bending [δd(OSO)] modes are not IR-active (these are Raman-active). The coordination of SO42− to metal ions decreases the symmetry of the group and the ν3 and ν4 modes are split [27, 37, 38]. In the case, the SO42−-site symmetry is lowered from Td to C3v (monodentate coordination), both ν1 and ν2 appear in the IR spectrum with weak to medium intensity, while ν3 and ν4 each splits into two bands in both IR and Raman spectra [37]. When the SO42−-site symmetry is lowered from Td to C2v (bidentate chelating or bridging coordination), again ν1 and ν2 appear in the IR spectrum (ν2 splits into two Raman modes), while ν3 and ν4 each splits into three IR-active and Raman-active vibrations [37]. The crystallographically established symmetry of the sulfato groups in 1·(py)C(Me)NOH is C2v. The bands at 1215, 1124 and 1080 (overlapping with the N–Ooxime stretch) cm−1 are attributed to the ν3 modes [37, 39], while the bands at 592, 631 and 683 cm−1 (the latter two overlapping with the in-plane 2-pyridyl deformations) are assigned to the ν4 modes [37, 38]. The band at 1010 cm−1 and the two weak features at 494 and 452 cm−1 can be assigned to the ν1 and ν2 modes, respectively. The appearance of two ν2 bands is consistent with a symmetry at the sulfato groups lower than C2v [37, 39]. Thus, from the vibrational spectroscopy viewpoint, the sulfato ligands of 1·(py)C(Me)NOH appear to have Ci symmetry (and not C2v as deduced from their bidentate character). When the SO42−-site symmetry is lowered from Td to Ci, ν3 and ν4 each splits into three IR-active vibrations, ν2 splits into two ones, while ν1 appears as a single band [37, 39]. This spectroscopic feature in 1·(py)C(Me)NOH is attributed to the fact that one uncoordinated oxygen atom of each bidentate bridging sulfate is hydrogen bonded to the oxygen atoms of the neutral oxime groups (see Table 3) resulting in a further lowering of the sulphate symmetry [39].

The ν(CO2) bands are difficult to assign in the spectrum of 2 due to the appearance of various stretching vibrations in the 1600–1400 cm−1 region and thus the application of the spectroscopic criterion of Deacon and Phillips [40] is very difficult.

4. Conclusions

The use of the sulfate ligand in combination with neutral (py)C(Me)NOH in Mn(II) chemistry has provided access to the two new neutral complexes [Mn2 (SO4)2 {(py)C(Me)NOH}4 ]·(py)C(Me)NOH (1·(py)C(Me)NOH) and [Mn(HCO2)2{(py)C(Me)NOH}2] (2), the latter being sulphate-free. In both complexes, the organic ligand chelates through its nitrogen atoms. The sulfate anion bridges the two MnII atoms in 1. Compounds 1 · (py)C(Me)NOH and 2 join a small family of structurally characterized manganese complexes containing the neutral or anionic forms of methyl(2-pyridyl)ketone oxime as ligands, while they are new examples of structurally characterized compounds in which (py)C(Me)NOH exists exclusively in its neutral form.

Analogues of 1·(py)C(Me)NOH and 2 with phenyl(2-pyridyl)ketone oxime, (py)C(ph)NOH, are not known to date, and it is currently not evident whether the stability of these species is dependent on the particular nature of the 2-pyridyl oxime ligand. We are studying this matter. Synthetic efforts are also in progress to “activate” the μ3 to μ6 bridging potential of the sulfate ligand in Mn complexes containing 2-pyridyl oximes and/or their anions as a means to get access to clusters and polymers with interesting structural and magnetic properties. Studies on the biological activity of 1·(py)C(Me)NOH and 2 are also planned.

5. Supplementary Information

CCDC 757892 and 757893 contain the supplementary crystallographic data for 1·(py)C(Me)NOH and 2. These data can be obtained free of charge via, or from the Cambridge Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: (+44)1223-336033; or e-mail: deposit/at/


This work was supported by the Cyprus Research Promotion Foundation (Grant DIETHNIS/STOXOS/0308/14). In dedication to Professor Nick Hadjiliadis for his retirement and for his important contributions to Bioinorganic Chemistry.


1. Milios CJ, Stamatatos TC, Perlepes SP. The coordination chemistry of pyridyl oximes. Polyhedron. 2006;25(1):134–194.
2. Rosa DT, Krause Baue JA, Baldwin MJ. Structural and spectroscopic studies of the versatile coordination chemistry of the chiral ligand N,N-bis(1-propan-2-onyl oxime)-L-methionine N′-methylamide with NiII and ZnII. Inorganic Chemistry. 2001;40(7):1606–1613. [PubMed]
3. Sauer K, Yano J, Yachandra VK. X-ray spectroscopy of the photosynthetic oxygen-evolving complex. Coordination Chemistry Reviews. 2008;252(3-4):318–335. [PMC free article] [PubMed]
4. Mishra A, Yano J, Pushkar Y, Yachandra VK, Abboud KA, Christou G. Heteronuclear Mn-Ca/Sr complexes, and Ca/Sr EXAFS spectral comparisons with the Oxygen-Evolving Complex of Photosystem II. Chemical Communications. 2007;(15):1538–1540. [PubMed]
5. Burdinski D, Birkelbach F, Weyhermüller T, et al. Encapsulation by a chromium(III)-containing bicyclic ligand cage. synthesis, structures, and physical properties of heterometal complexes CrIIIMCrIII [M = (H+)2, Li(I), Mg(II), Cu(II), Ni(II), Ni(IV), Co(III), Fe(II), Fe(III), Mn(II)] Inorganic Chemistry. 1998;37(5):1009–1020.
6. Kukushkin VYu, Pombeiro AJL. Oxime and oximate metal complexes: unconventional synthesis and reactivity. Coordination Chemistry Reviews. 1999;181(1):147–175.
7. Goldcamp MJ, Robison SE, Krause Bauer JA, Baldwin MJ. Oxygen reactivity of a nickel(II)-polyoximate complex. Inorganic Chemistry. 2002;41(9):2307–2309. [PubMed]
8. Kopylovich MN, Kukushkin VYu, Haukka M, Fraústo da Silva JJR, Pombeiro AJL. Zinc(II)/ketoxime system as a simple and efficient catalyst for hydrolysis of organonitriles. Inorganic Chemistry. 2002;41(18):4798–4804. [PubMed]
9. Akine S, Taniguchi T, Saiki T, Nabeshima T. Ca2+- and Ba2+-selective receptors based on site-selective transmetalation of multinuclear polyoxime-zinc(II) complexes. Journal of the American Chemical Society. 2005;127(2):540–541. [PubMed]
10. Pombeiro AJL, Kukushkin VYu. Reactivity of coordinated oximes. In: McCleverty JA, Meyer TJ, editors. Comprehensive Coordination Chemistry II. Vol. 1. Amsterdam, The Netherlands: Elsevier; 2004. pp. 631–637.
11. Thorpe JM, Beddoes RL, Collison D, et al. Surface coordination chemistry: corrosion inhibition by tetranuclear cluster formation of iron with salicylaldoxime. Angewandte Chemie: International Edition. 1999;38(8):1119–1121.
12. Khanra S, Weyhermüller T, Bill E, Chaudhuri P. Deliberate synthesis for magnetostructural study of linear tetranuclear complexes BIIIMnIIMnIIBIII, MnIIIMnIIMnIIMnIII, MnIVMnIIMnIIMnIV, FeIIIMnIIMnIIFeIIICrIIIMnIIMnIICrIII. Influence of terminal ions on the exchange coupling. Inorganic Chemistry. 2006;45(15):5911–5923. [PubMed]
13. Robertson D, Cannon JF, Gerasimchuk N. Double-stranded metal-organic networks for one-dimensional mixed valence coordination polymers. Inorganic Chemistry. 2005;44(23):8326–8342. [PubMed]
14. Stamatatos TC, Foguet-Albiol D, Stoumpos CC, et al. Initial example of a triangular single-molecule magnet from ligand-induced structural distortion of a [MnIII3O]7+  complex. Journal of the American Chemical Society. 2005;127(44):15380–15381. [PubMed]
15. Milios CJ, Raptopoulou CP, Terzis A, et al. Hexanuclear manganese(III) single-molecule magnets. Angewandte Chemie: International Edition. 2003;43(2):210–212. [PubMed]
16. Milios CJ, Vinslava A, Whittaker AG, et al. Microwave-assisted synthesis of a hexanuclear MnIII single-molecule magnet. Inorganic Chemistry. 2006;45(14):5272–5274. [PubMed]
17. Miyasaka H, Clérac R, Mizushima K, et al. [Mn2(saltmen)2Ni(pao)2(L)2](A)2 with L = pyridine, 4-picoline, 4-tert-butylpyridine, N-methylimidazole and A = ClO4, BF4, PF6, ReO4: a family of single-chain magnets. Inorganic Chemistry. 2003;42(25):8203–8213. [PubMed]
18. Abele E, Abele R, Lukevics E. Pyridine oximes: synthesis, reactions, and biological activity. Chemistry of Heterocyclic Compounds. 2003;39(7):825–865.
19. Alexiou M, Tsivikas I, Dendrinou-Samara C, et al. High nuclearity nickel compounds with three, four or five metal atoms showing antibacterial activity. Journal of Inorganic Biochemistry. 2003;93(3-4):256–264. [PubMed]
20. Papatriantafyllopoulou C, Kostakis GE, Raptopoulou CP, Terzis A, Perlepes SP, Plakatouras JC. Investigation of the MSO4 · xH2O(M = Zn, x = 7; M = Cd, x = 8/3)/methyl 2-pyridyl ketone oxime reaction systemml: a novel Cd(II) coordination polymer versus mononuclear and dinuclear Zn(II) complexes. Inorganica Chimica Acta. 2009;362(7):2361–2370.
21. Milios CJ, Kyritsis P, Raptopoulou CP, et al. Di-2-pyridyl ketone oxime [(py)2CNOH] in manganese carboxylate chemistry: mononuclear, dinuclear and tetranuclear complexes, and partial transformation of (py)2CNOH to the gem-diolate(2−) derivative of di-2-pyridyl ketone leading to the formation of NO3 Dalton Transactions. 2005;(3):501–511. [PubMed]
22. Papatriantafyllopoulou C, Raptopoulou CP, Terzis A, Manessi-Zoupa E, Perlepes SP. Investigation of the zinc chloride/methyl(2-pyridyl)ketone oxime reaction systemml: a mononuclear complex and an inverse 12-metallacrown-4 cluster. Zeitschrift für Naturforschung. 2006;61(1):37–46.
23. Alexiou M, Dendrinou-Samara C, Raptopoulou CP, Terzis A, Kessissoglou DP. From monomer zinc-oxamato complexes to tetranuclear inverse 12-membered and octanuclear 12-membered metallacrowns. Inorganic Chemistry. 2002;41(18):4732–4738. [PubMed]
24. Riggle K, Lynde-Kernell T, Schlemper EO. Synthesis and X-ray structures of Ni(II) complexes of 1-(2-pyridinyl)ethanone oxime. Journal of Coordination Chemistry Chemistry. 1992;25:117–125.
25. Cibulka R, Císařová I, Ondráček J, Liška F, Ludvík J. Electrochemical reductions of Ni2+, Cu2+ and Zn2+ complexes of azinyl methyl ketoximes on mercury. Collection of Czechoslovak Chemical Communications. 2001;66(1):170–184.
26. Coxall RA, Harris SG, Henderson DK, Parsons S, Tasker PA, Winpenny REP. Inter-ligand reactions: in situ formation of new polydentate ligands. Journal of the Chemical Society, Dalton Transactions. 2000;(14):2349–2356.
27. Papatriantafyllopoulou C, Manessi-Zoupa E, Escuer A, Perlepes SP. The sulfate ligand as a promising ‘player’ in 3d-metal cluster chemistry. Inorganica Chimica Acta. 2009;362(3):634–650.
28. Nurova SY, Turevskaya EP, Kessler VG, Yanovskaya MI. The Chemistry of Metal Alkoxides. Dordrecht, The Netherlands: Kluwer Academic Publishers; 2002.
29. Papatriantafyllopoulou C, Tasiopoulos A, Perlepes SP. unpublished results. [PubMed]
30. Papatriantafyllopoulou C, Raptopoulou CP, Terzis A, Janssens JF, Perlepes SP, Manessi-Zoupa E. Reactions of nickel(II) sulfate hexahydrate with methyl(2-pyridyl)ketone oxime: two mononuclear sulfato complexes containing the neutral ligand. Zeitschrift für Naturforschung. 2007;62(9):1123–1132.
31. Stoumpos CC, Stamatatos TC, Sartzi H, et al. Employment of methyl 2-pyridyl ketone oxime in manganese non-carboxylate chemistry: MnII2MnIV and MnII2MnIII6 complexes. Dalton Transactions. 2009;(6):1004–1015. [PubMed]
32. Zuo J, Dou J, Li D, Wang D, Sun Y. Dichlorido[1-(2-pyrid-yl)ethanone oximato][1-(2-pyrid-yl)ethanone oxime]manganese(III) Acta Crystallographica E. 2007;63(12):m3183–m3184.
33. Stoumpos CC, Stamatatos TC, Psycharis V, Raptopoulou CP, Christou G, Perlepes SP. A new MnII4MnIII4 cluster from the use of methyl 2-pyridyl ketone oxime in manganese carboxylate chemistry: synthetic, structural and magnetic studies. Polyhedron. 2008;27(18):3703–3709.
34. Papatriantafyllopoulou C, Aromi G, Tasiopoulos AJ, et al. Use of the sulfato ligand in 3d-metal cluster chemistry: a family of hexanuclear nickel(II) complexes with 2-pyridyl-substituted oxime ligands. European Journal of Inorganic Chemistry. 2007;(18):2761–2774.
35. Chaudhuri P, Winter M, Flörke U, Haupt H-J. An effectively diamagnetic oximato-bridged asymmetric dinuclear copper(II) complex with a Cu(II)I bond. Inorganica Chimica Acta. 1995;232(1-2):125–130.
36. Lever ABP, Mantovani E. The far-infrared and electronic spectra of some bis-ethylenediamine and related complexes of copper(II) and the relevance of these data to tetragonal distortion and bond strengths. Inorganic Chemistry. 1971;10(4):817–826.
37. Nakamoto K. Infrared and Raman Spectra of Inorganic and Coordination Compounds. 4th edition. New York, NY, USA: Wiley; 1986.
38. Papatriantafyllopoulou C, Efthymiou CG, Raptopoulou CP, et al. Initial use of the di-2-pyridyl ketone/sulfate ‘blend’ in 3d-metal cluster chemistry: preparation, X-ray structures and physical studies of zinc(II) and nickel(II) cubanes. Journal of Molecular Structure. 2007;829(1–3):176–188.
39. Papatriantafyllopoulou C, Efthymiou CG, Raptopoulou CP, Terzis A, Manessi-Zoupa E, Perlepes SP. Mononuclear versus dinuclear complex formation in nickel(II) sulfate/phenyl(2-pyridyl)ketone oxime chemistry depending on the ligand to metal reaction ratio: synthetic, spectral and structural studies. Spectrochimica Acta A. 2008;70(4):718–728. [PubMed]
40. Deacon GB, Phillips RJ. Relationships between the carbon-oxygen stretching frequencies of carboxylato complexes and the type of carboxylate coordination. Coordination Chemistry Reviews. 1980;33:227–250.

Articles from Bioinorganic Chemistry and Applications are provided here courtesy of Hindawi Publishing Corporation