# Use of the 2-Pyridinealdoxime/N,N′-Donor Ligand Combination in Cobalt(III) Chemistry: Synthesis and Characterization of Two Cationic Mononuclear Cobalt(III) Complexes

Authors: Konstantis F. Konidaris; Catherine P. Raptopoulou; Vassilis Psycharis; Spyros P. Perlepes; Evy Manessi-Zoupa; Theocharis C. Stamatatos
Journal: Bioinorganic Chemistry and Applications
 (2010)

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## Abstract

The use of 2-pyridinealdoxime (paoH)/N,N′-donor ligand (L-L) “blend” in cobalt chemistry has afforded two cationic mononuclear cobalt(III) complexes of the general type [Co(pao)2(L-L)]+, where L-L = 1,10-phenanthroline (phen) and 2,2′-bipyridine (bpy). The CoCl2/paoH/L-L (1 : 2 : 1) reaction system in MeOH gives complexes [CoIII(pao)2(phen)]Cl·2H2O (1·2H2O) and [CoIII(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH). The structures of the complexes were determined by single-crystal X-ray crystallography. The CoIII ions are six-coordinate, surrounded by three bidentate chelating ligands, that is, two pao- and one phen or bpy. The deprotonated oxygen atom of the pao- ligand remains uncoordinated and participates in hydrogen bonding with the solvate molecules. IR data of the complexes are discussed in terms of the nature of bonding and the known structures.


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## Body

## 1. Introduction

Oximes and their metal complexes are of current interest because of their rich physicochemical properties, reactivity patterns, and potential applications in many important chemical processes in the fields of medicine [1, 2], bioorganic chemistry [3], catalysis [4], and electrochemical and electrooptical sensors [5].In the treatment of organophosphate insecticide toxicity in man and animals, the use of acetylcholinesterase reactivators in conjunction with atropine has been found to be the most effective treatment [6]. Among various acetylcholinesterase reactivators, 2-pyridinealdoxime (paoH) is routinely used in human and veterinary practices. It is furthermore known that metal complexes of active drugs as ligands can have important pharmaceutical activities because of several factors. In fact, the field of medicinal inorganic chemistry emerged a long time ago [7], and it is based on certain principles that can be summarized as follows. Complexation with the metal protects the drug against enzymatic degradations because of the inertness of certain metal-ligand linkages. The metal complex can have better hydrophobicity/hydrophilicity properties than the free ligand and, through this, it can improve the transport processes in the tissues. In addition, the metal complex can release the active drug(s) in a specific organ, and its activity can be reinforced by the combination of effects from the ligands and from the metal residue. The application of these principles has already resulted in the design of successful metal-based drugs [8, 9].Since 1905, when Tschugaeff introduced dimethylglyoxime as a reagent for the analysis of nickel, oxime ligands have played an important role in the continuing progress of coordination chemistry [10]. Furthermore, the ability of the oximate(-1) group (>C=N–O-) to stabilize oxidized forms of metal ions, for example, NiIII or NiIV, has a vital importance in their role in the areas of technological applications [11]. In contrast to the great number of studies dealing with metal complexes of simple oximes and salicylaldoximes [12], relatively little is known about complexes of 2-pyridyloximes [13–15] although this class of compounds could offer unique features in terms of structural and physical properties.Few years ago our group explored the influence of these ligands on the Co cluster chemistry by reacting cobalt carboxylate salts with neutral 2-pyridyloximes; the main objectives were the access to new structural types of clusters with interesting magnetic and spectroscopic properties and the study of Co-mediated reactions of the oxime group. Reaction schemes involving di-2-pyridyl ketone oxime, dpkoxH (Figure1), and various Co carboxylate sources led [16] to the first mixed-valence Co(II,III), inverse 12-metallacrown-4 complexes, namely, [Co2IICo2III(OR)2(O2CR′)2(dpkox)4S2]X2 (R = H, CH3; R′=CH3, C6H5, (CH3)3; S = solvent; X = ClO4, PF6). The use of phenyl 2-pyridyl ketone oxime, phpkoxH (Figure 1), methyl 2-pyridyl ketone oxime, MepaoH (Figure 1), and 2-pyridinealdoxime, paoH (Figure 1) in Co carboxylate chemistry yielded [17] the trinuclear, mixed-valence, carboxylate-free Co(II,III) complexes  [Co3(phpkox)6](PF6)2, [Co3(Mepao)6](ClO4)2, and [Co3(pao)6](ClO4)2. The core of these complexes has an open-topology comprising one CoII center and two CoIII ions. Recently [18] two of us reported complexes [Co3IIIO(O2CPh)3(pao)3]2[Co3II(O2CPh)8], [Co3IIIO(O2CPh)3(pao)3](O2CPh), [Co3IIIO(O2CPh)3(pao)3]2(O2CPh)(NO3), and  [Co2IIICoII(OH)Cl3(pao)4]. The above prior results encouraged us to proceed to the amalgamation of 2-pyridyl oximes with N,N′-donor ligands, that is, 1,10-phenanthroline (phen) and  2,2′-bipyridine (bpy) (Figure 1), in cobalt chemistry. The primary aim of this project was the synthesis and structural characterization of a series of cobalt building blocks that could act as “metalloligands” for the construction of one-dimensional heterometallic assemblies with various transition metal ions (e.g., MnIII, CrIII, FeII) or lanthanides; the latter chains would probably provide interesting magnetic, optical, and spectroscopic properties. A secondary goal was the study of the biological properties of the resulting mixed-ligand complexes. Herein, we concentrate on the synthetic investigation of the general CoCl2/paoH/phen or bpy reaction system and describe the preparation and characterization of the cationic mononuclear complexes [Co(pao)2(phen)]Cl and [Co(pao)2(bpy)]Cl.Figure 1
Structural formulae and abbreviations of the ligands discussed in the text.


## 2. Experiments

### 2.1. Starting Materials and Physical Measurements

All manipulations were performed under aerobic conditions using reagents and solvents as received. Cobalt(II) chloride, 2-pyridinealdoxime (paoH), 1,10-phenanthroline hydrate (phen·H2O), and 2,2′-bipyridine (bpy) were purchased from Aldrich Co. Elemental analyses (C, H, N) were performed by the University of Ioannina (Greece) Microanalytical Laboratory using an EA 1108 Carlo Erba analyzer. Ir spectra (4000–450 cm-1) were recorded on a Perkin-Elmer 16 PC FT-IR spectrometer with samples prepared as KBr pellets. Solid-state (diffuse reflectance, 28.5–12.5 kK) electronic spectra were recorder on a Varian Cary 100 instrument. Magnetic susceptibility measurements were carried out at 25°C by the Faraday method using a Cahn-Ventron RM-2 balance standardized with [HgCo(NCS)4]n.


### 2.2. Compound Preparation

#### 2.2.1. Preparation of [Co(pao)2(phen)]Cl·2H2O (1·2H2O)

To a pale yellow, stirred solution of paoH (0.12 g, 1.0 mmol) in MeOH (20 cm3) was added a colourless solution of phen·H2O (0.10 g, 0.5 mmol) in the same solvent (5 cm3). To the resulting, almost colourless solution, a pink solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (10 cm3) was added. The deep orange solution obtained was stirred at ambient temperature for 30 min and allowed to very slowly evaporate at 6–8°C for one week. Well-formed, X-ray quality crystals of the product slowly appeared. The orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×4 cm3), and dried in air. Yields as high as 70% were obtained (found: C, 51.9; H, 3.8; N, 15.6. C24H22CoN6O4Cl calcd.: C, 52.1; H, 4.0; N, 15.2%).


#### 2.2.2. Preparation of [Co(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH)

To a pink, stirred solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (15 cm3) was added solid paoH (0.12 g, 1.0 mmol). To the resulting deep orange solution a colourless solution of bpy (0.08 g, 0.5 mmol) in the same solvent (5 cm3) was added. The solution was stirred at ambient temperature for 25 min, filtered, and the filtrate was layered with Et2O/n-hexane (40 cm3, 1:1v/v). Slow mixing gave well-formed, X-ray quality crystals of the product. The reddish orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×3 cm3), and dried in air. Yields as high as 75% were obtained. The crystals were found to lose solvent readily; the dried sample analysed for [Co(pao)2(bpy)]Cl, that is, 2 (found: C, 53.3; H, 3.4; N, 17.2. C22H18CoN6O2Cl calcd.: C, 53.6; H, 3.7; N, 17.1%).


### 2.3. X-Ray Crystallographic Studies [1]

Suitable crystals of1·2H2O were sealed in capillary filled with drops of the mother liquor, while crystals of 2·1.5MeOH were mounted in air and covered with epoxy glou. Diffraction measurements of 1·2H2O and 2·1.5MeOH were made on a Crystal Logic dual goniometer diffractometer using graphite-monochromated Mo radiation. Crystal data and full details of the data collection and data processing are listed in Table 1. Unit cell dimensions were determined and refined by using three angular settings of 25 automatically centred reflections in the range 11°<2θ<23° for both complexes. Three standard reflections, monitored every 97 reflections, showed less than 3% intensity variation and no decay. Lorentz-polarisation corrections were applied for 1·2H2O and 2·1.5MeOH using Crystal Logic software.Table 1
Crystallographic data for complexes1·2H2O and 2·1.5MeOH.
Parameter1·2H2O2·1.5MeOHColor (habit)Red/orange prismsRed prismsCrystal size (mm)0.33× 0.08 × 0.050.50× 0.35 × 0.30Chemical formulaC24H22CoN6O4ClC23.5H19CoN6O3.5ClM552.86535.83Crystal systemTetragonalOrthorhombicSpace groupI41/acdIc2mUnit cell dimensionsa (Å)17.098(5)13.134(6)b (Å)17.098(5)8.900(4)c (Å)31.903(9)21.293(8)V (Å3)9327(5)2489(2)Z164Dcalc (g cm-3)1.5751.430μ (mm-1)0.8960.836Radiation (Å)MoKα (0.71073)MoKα (0.71073)Temperature (K)298298Scan mode/speed (°min-1)θ-2θ/2.6θ-2θ/3.5Scan range (°)2.1 +α1α2 separation2.3 +α1α2 separationθ range (°)2.1–23.01.8–25.0Reflections collected31573561Unique reflections1627 (Rint=  0.0276)2253 (Rint=  0.0240)Reflections used[I>2σ(I)]12371882Parameters refined164204[Δ/σ]max0.0000.014[Δρ]max/[Δρ]min (e Å-3)0.712/−0.4440.695/−0.244GoF (onF2)1.1011.079R1(a) [I> 2σ(I)]0.05430.0424wR2(b) [I> 2σ(I)]0.14530.1097R1(a)= Σ(|‌Fo|‌-|‌Fc|‌)/Σ(|‌Fo|‌); wR2(b)= {Σ[w(Fo2-Fc2)2]/Σ[w(Fo2)2]}1/2, w=1/[σ2(Fo2)+(aP)2+bP] where P= (max(Fo2,0)+2Fc2)/3.The structures were solved by direct methods using SHELXS-97 [19] and refined by full matrix least-squares on F2 with SHELXL-97 [20]. For both structures, all non-H atoms were refined using anisotropic thermal parameters. Some H-atoms were located by difference maps and refined isotropically. No H-atoms for the solvate molecules of 1·2H2O were included in the refinement.Reference [1] CCDC codes are 771333 and 771334 for complexes 1·2H2O and 2·1.5MeOH, respectively.


## 2.1. Starting Materials and Physical Measurements

All manipulations were performed under aerobic conditions using reagents and solvents as received. Cobalt(II) chloride, 2-pyridinealdoxime (paoH), 1,10-phenanthroline hydrate (phen·H2O), and 2,2′-bipyridine (bpy) were purchased from Aldrich Co. Elemental analyses (C, H, N) were performed by the University of Ioannina (Greece) Microanalytical Laboratory using an EA 1108 Carlo Erba analyzer. Ir spectra (4000–450 cm-1) were recorded on a Perkin-Elmer 16 PC FT-IR spectrometer with samples prepared as KBr pellets. Solid-state (diffuse reflectance, 28.5–12.5 kK) electronic spectra were recorder on a Varian Cary 100 instrument. Magnetic susceptibility measurements were carried out at 25°C by the Faraday method using a Cahn-Ventron RM-2 balance standardized with [HgCo(NCS)4]n.


## 2.2. Compound Preparation

### 2.2.1. Preparation of [Co(pao)2(phen)]Cl·2H2O (1·2H2O)

To a pale yellow, stirred solution of paoH (0.12 g, 1.0 mmol) in MeOH (20 cm3) was added a colourless solution of phen·H2O (0.10 g, 0.5 mmol) in the same solvent (5 cm3). To the resulting, almost colourless solution, a pink solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (10 cm3) was added. The deep orange solution obtained was stirred at ambient temperature for 30 min and allowed to very slowly evaporate at 6–8°C for one week. Well-formed, X-ray quality crystals of the product slowly appeared. The orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×4 cm3), and dried in air. Yields as high as 70% were obtained (found: C, 51.9; H, 3.8; N, 15.6. C24H22CoN6O4Cl calcd.: C, 52.1; H, 4.0; N, 15.2%).


### 2.2.2. Preparation of [Co(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH)

To a pink, stirred solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (15 cm3) was added solid paoH (0.12 g, 1.0 mmol). To the resulting deep orange solution a colourless solution of bpy (0.08 g, 0.5 mmol) in the same solvent (5 cm3) was added. The solution was stirred at ambient temperature for 25 min, filtered, and the filtrate was layered with Et2O/n-hexane (40 cm3, 1:1v/v). Slow mixing gave well-formed, X-ray quality crystals of the product. The reddish orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×3 cm3), and dried in air. Yields as high as 75% were obtained. The crystals were found to lose solvent readily; the dried sample analysed for [Co(pao)2(bpy)]Cl, that is, 2 (found: C, 53.3; H, 3.4; N, 17.2. C22H18CoN6O2Cl calcd.: C, 53.6; H, 3.7; N, 17.1%).


## 2.2.1. Preparation of [Co(pao)2(phen)]Cl·2H2O (1·2H2O)

To a pale yellow, stirred solution of paoH (0.12 g, 1.0 mmol) in MeOH (20 cm3) was added a colourless solution of phen·H2O (0.10 g, 0.5 mmol) in the same solvent (5 cm3). To the resulting, almost colourless solution, a pink solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (10 cm3) was added. The deep orange solution obtained was stirred at ambient temperature for 30 min and allowed to very slowly evaporate at 6–8°C for one week. Well-formed, X-ray quality crystals of the product slowly appeared. The orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×4 cm3), and dried in air. Yields as high as 70% were obtained (found: C, 51.9; H, 3.8; N, 15.6. C24H22CoN6O4Cl calcd.: C, 52.1; H, 4.0; N, 15.2%).


## 2.2.2. Preparation of [Co(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH)

To a pink, stirred solution of CoCl2 (0.07 g, 0.5 mmol) in MeOH (15 cm3) was added solid paoH (0.12 g, 1.0 mmol). To the resulting deep orange solution a colourless solution of bpy (0.08 g, 0.5 mmol) in the same solvent (5 cm3) was added. The solution was stirred at ambient temperature for 25 min, filtered, and the filtrate was layered with Et2O/n-hexane (40 cm3, 1:1v/v). Slow mixing gave well-formed, X-ray quality crystals of the product. The reddish orange prismatic crystals were collected by filtration, washed with cold MeOH (2×3 cm3) and Et2O (2×3 cm3), and dried in air. Yields as high as 75% were obtained. The crystals were found to lose solvent readily; the dried sample analysed for [Co(pao)2(bpy)]Cl, that is, 2 (found: C, 53.3; H, 3.4; N, 17.2. C22H18CoN6O2Cl calcd.: C, 53.6; H, 3.7; N, 17.1%).


## 2.3. X-Ray Crystallographic Studies [1]

Suitable crystals of1·2H2O were sealed in capillary filled with drops of the mother liquor, while crystals of 2·1.5MeOH were mounted in air and covered with epoxy glou. Diffraction measurements of 1·2H2O and 2·1.5MeOH were made on a Crystal Logic dual goniometer diffractometer using graphite-monochromated Mo radiation. Crystal data and full details of the data collection and data processing are listed in Table 1. Unit cell dimensions were determined and refined by using three angular settings of 25 automatically centred reflections in the range 11°<2θ<23° for both complexes. Three standard reflections, monitored every 97 reflections, showed less than 3% intensity variation and no decay. Lorentz-polarisation corrections were applied for 1·2H2O and 2·1.5MeOH using Crystal Logic software.Table 1
Crystallographic data for complexes1·2H2O and 2·1.5MeOH.
Parameter1·2H2O2·1.5MeOHColor (habit)Red/orange prismsRed prismsCrystal size (mm)0.33× 0.08 × 0.050.50× 0.35 × 0.30Chemical formulaC24H22CoN6O4ClC23.5H19CoN6O3.5ClM552.86535.83Crystal systemTetragonalOrthorhombicSpace groupI41/acdIc2mUnit cell dimensionsa (Å)17.098(5)13.134(6)b (Å)17.098(5)8.900(4)c (Å)31.903(9)21.293(8)V (Å3)9327(5)2489(2)Z164Dcalc (g cm-3)1.5751.430μ (mm-1)0.8960.836Radiation (Å)MoKα (0.71073)MoKα (0.71073)Temperature (K)298298Scan mode/speed (°min-1)θ-2θ/2.6θ-2θ/3.5Scan range (°)2.1 +α1α2 separation2.3 +α1α2 separationθ range (°)2.1–23.01.8–25.0Reflections collected31573561Unique reflections1627 (Rint=  0.0276)2253 (Rint=  0.0240)Reflections used[I>2σ(I)]12371882Parameters refined164204[Δ/σ]max0.0000.014[Δρ]max/[Δρ]min (e Å-3)0.712/−0.4440.695/−0.244GoF (onF2)1.1011.079R1(a) [I> 2σ(I)]0.05430.0424wR2(b) [I> 2σ(I)]0.14530.1097R1(a)= Σ(|‌Fo|‌-|‌Fc|‌)/Σ(|‌Fo|‌); wR2(b)= {Σ[w(Fo2-Fc2)2]/Σ[w(Fo2)2]}1/2, w=1/[σ2(Fo2)+(aP)2+bP] where P= (max(Fo2,0)+2Fc2)/3.The structures were solved by direct methods using SHELXS-97 [19] and refined by full matrix least-squares on F2 with SHELXL-97 [20]. For both structures, all non-H atoms were refined using anisotropic thermal parameters. Some H-atoms were located by difference maps and refined isotropically. No H-atoms for the solvate molecules of 1·2H2O were included in the refinement.Reference [1] CCDC codes are 771333 and 771334 for complexes 1·2H2O and 2·1.5MeOH, respectively.


## 3. Experiments

### 3.1. Synthetic Comments

The reaction system that we investigated was the CoCl2/paoH/phen or bpy one. Treatment of a solution of CoCl2 with two equivalents of paoH and one equivalent of 1,10-phenanthroline (phen) in MeOH, under aerobic conditions, followed by slow evaporation of the resulting solution allowed orange crystals of the product to be obtained in a form suitable for crystallography. The product was identified as the cationic mononuclear complex [Co(pao)2(phen)]Cl·2H2O (1·2H2O). Following a similar reaction scheme and replacing only the corresponding bidentate ligand with 2,2′-bipyridine (bpy), we were able to obtain red crystals suitable for crystallography. The new product was identified as [Co(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH).The most noticeable feature of this reaction scheme is the deprotonation of the oximato group without the presence of a strong base in the reaction system. Reduction products of the atmospheric oxygen, which is responsible forCoII → CoIII oxidation, are possible agents for the former deprotonation. The formation of 1 and 2 can be summarized by the stoichiometric equations (1) and (2), respectively,(1)2CoCl2+4paoH+2phen·H2O+1/2O2→MeOH2[Co(pao)2(phen)]Cl+2HCl+3H2O(2)2CoCl2+4paoH+2bpy+1/2O2→MeOH2[Co(pao)2(bpy)]Cl+2HCl+H2OThe following experimental points should be mentioned at this point. (a) The reactions between CoCl2, paoH and N,N′-donor ligands in MeOH are [OH-]-independent. Addition of one equivalent of LiOH·H2O in the above described reaction mixtures leads to complexes 1·2H2O and 2·1.5MeOH as well as to unidentified noncrystalline, hydroxo compounds. (b) A number of attempts were made for the isolation of new products by increasing or decreasing the paoH/Co reaction ratio, keeping constant (1 : 1) the phen or bpy : Co ratio. Increasing the former ratio, that is, to 3:1 or 4 : 1, complexes 1 and 2 remained the main products; however, these were contaminated with variable amounts of the known product [CoIII(pao)3] [21] (analytical evidence, unit cell determination of the isolated dark orange crystals). Reducing the above reaction ratio (1 : 1 and/or 0.5/1), paoH-“free” products were isolated containing only bpy or phen and chloride ions. We have not yet found evidence for the existence of the mixed-ligand species [Co(pao)(phen)2]Cl2 and [Co(pao)(bpy)2]Cl2. (c) Both complexes are soluble in water, dimethylformamide, dimethylsulfoxide, and acetonitrile, less soluble in nitromethane and ethanol, and insoluble in benzene, chloroform and dichloromethane.


### 3.2. Description of Structures

Labeled ORTEP plots of complexes1·2H2O and 2·1.5MeOH are shown in Figures 2 and 4, respectively. Selected bond distances and angles for complexes 1·2H2O and 2·1.5MeOH are listed in Table 2.Table 2
Selected bond distances (Å) and angles (°) for complexes1·2H2O and 2·1.5MeOH,a with the estimated standard deviations in parentheses.
1·2H2O2·1.5MeOHBond distancesCo–N(1)1.928(4)1.937(3)Co–N(2)1.904(4)1.909(4)Co–N(3)1.986(4)1.977(4)Co–N(1′)1.928(4)1.937(3)Co–N(2′)1.904(4)1.909(4)Co–N(3′)1.986(4)1.977(4)N(2)–O/O(1)1.294(6)1.273(5)N(3)–C(7)1.322(7)1.343(6)N(1)–C(1)1.343(7)1.340(6)N(2)–C(6)1.298(7)1.309(7)Bond anglesN(3)–Co–N(3′)82.7(2)82.2(2)N(1)–Co–N(3)88.6(2)93.6(2)N(1)–Co–N(2)83.7(2)83.7(2)N(2)–Co–N(2′)89.9(3)89.8(2)N(1)–Co–N(3′)96.1(2)90.7(2)Co–N(2)–O/O(1)122.7(4)123.3(3)aUnprimed and primed atoms are related by symmetry.Figure 2
Partially labeled plot of the molecular structure of the cation that is present in1·2H2O. Primes are used for symmetry related atoms. H atoms have been omitted for clarity.Disregarding the different nature of the N,N′-donor ligands, compounds1·2H2O and 2·1.5MeOH display strikingly similar molecular structures. Thus, only the structure of the former will be described in detail.Complex1·2H2O crystallizes in the tetragonal space group I41/acd. Its structure consists of the mononuclear [Co(pao)2(phen)]+ cation, one chloride ion, and two solvate water molecules; the latter three will not be further discussed. The metal ion lies on a crystallographic 2-fold axis. The CoIII center is in a six-coordinate ligand environment comprising the two nitrogens from two chelating, anionic pao-ligands, [N(1)/N(2) and their symmetry-related partners] and two aromatic nitrogens from the chelating phen molecule [N(3) and N(3′)]. The metal coordination geometry is well described as distorted octahedral, its chromophore being CoIIIN6. Two transpositions of the octahedron are occupied by the pyridyl nitrogen atoms of the two pao- ligands [N(1)–Co–N(1′) = 173.8(3)°]; thus, the two oximate nitrogen atoms [N(2), N(2′)] are in cis position. Angular distortions from perfect octahedral geometry are primarily a consequence of the chelating rings and their restricted bite angles. The Co–N bond lengths agree well with values expected for low-spin CoIII in octahedral environments [21].In the crystal lattice of1·2H2O, the molecules interact through hydrogen bonds forming 1D zig-zag chains (Figure 3). These include the water lattice molecules, the oximate oxygen atom, and the Cl- counteranion; their dimensions are presented in Table 3.Table 3
Hydrogen bonding interactions in1·2H2O.
Interaction D–H⋯AD⋯A (Å)H⋯A (Å)D–H⋯A (°)Symmetry operation of AOW-HWA⋯O2.854(7)1.740(4)161.7(3)x, y, zOW-HWB⋯Cl3.124(6)1.978(2)163.5(3)x, y, zFigure 3
A part of the 1D structure of1·2H2O due to H-bonding interactions (dashed lines) along the a axis. Chlorides (green) are emphasized using space filling models.Figure 4
Partially labeled plot of the molecular structure of the cation that is present in2·1.5MeOH. H atoms have been omitted for clarity. Primes are used for symmetry related atoms.Complex2·1.5MeOH crystallizes in the orthorhombic space group Ic2m; the metal ion lies on a crystallographic twofold axis. One half of the molecule comprises the asymmetric unit of the structure. The three ligands are N,N′-bidentate chelating. Again the pyridyl nitrogen atoms of the two pao- ligands are in trans positions. A packing diagram of the complex is shown in Figure 5.Figure 5
Packing diagram of complex2·1.5MeOH along the c axis. The metal coordination spheres are polyhedron designed (purple). The chloride counteranions and the methanol solvate molecules have been omitted.Since the space group of1·2H2O is centrosymmetric and the space group of 2·1.5MeOH involves a mirror plane, both complexes are racemic mixtures of their Δ and Λ enantiomorphs.Complexes1 and 2 join a small family of structurally characterized homo- [17, 18, 21] and heterometallic [22, 23] Co complexes featuring pao- as ligand. Many years ago Blackmore and Magee [24, 25] and Grant and Magee [26] studied the reactions between 2-pyridinealdoxime and various CoII sources under a variety of reaction conditions. Structural assignments of the solid products [24, 26] were based on spectroscopic data; no X-ray structures were reported. The authors did not prepare mixed-ligand complexes.


### 3.3. Physical and Spectroscopic Characterization

Complexes1 and 2 are diamagnetic, in accordance with their low-spin 3d6 character.The solid-state (diffuse reflectance) UV-Vis spectra of the two complexes are almost identical and typical for low-spinCoIIIN6 chromophores [27]. The low-spin octahedral ground term is A1g1, and there are two relatively low lying spin allowed transitions, with lower lying spin triplet partners, all derived from (t2g)5(eg). Under this scheme, the bands in the spectra of 1 and 2 at ~29.0, 21.5, 17.0, and 13.5 kK are assigned [27] to the A1g1→T2g1, T1g1, T2g3, and T1g3 transitions, respectively, although a superposition of the highest energy d-d transition and a charge transfer band should not be ruled out.Two bands, one of medium intensity at~1015 cm-1 assigned to ν(N–O) and one strong at 1599 cm-1 assigned to ν(C=N)_oximate are common in the IR spectra of the two complexes [21]; the higher-wavenumber band most probably overlaps with an aromatic stretch. The in-plane deformation of the 2-pyridyl ring of the free paoH at 627 cm-1 shifts upward on coordination in the spectra of 1 (643 cm-1) and 2 (645 cm-1) [28].


## 3.1. Synthetic Comments

The reaction system that we investigated was the CoCl2/paoH/phen or bpy one. Treatment of a solution of CoCl2 with two equivalents of paoH and one equivalent of 1,10-phenanthroline (phen) in MeOH, under aerobic conditions, followed by slow evaporation of the resulting solution allowed orange crystals of the product to be obtained in a form suitable for crystallography. The product was identified as the cationic mononuclear complex [Co(pao)2(phen)]Cl·2H2O (1·2H2O). Following a similar reaction scheme and replacing only the corresponding bidentate ligand with 2,2′-bipyridine (bpy), we were able to obtain red crystals suitable for crystallography. The new product was identified as [Co(pao)2(bpy)]Cl·1.5MeOH (2·1.5MeOH).The most noticeable feature of this reaction scheme is the deprotonation of the oximato group without the presence of a strong base in the reaction system. Reduction products of the atmospheric oxygen, which is responsible forCoII → CoIII oxidation, are possible agents for the former deprotonation. The formation of 1 and 2 can be summarized by the stoichiometric equations (1) and (2), respectively,(1)2CoCl2+4paoH+2phen·H2O+1/2O2→MeOH2[Co(pao)2(phen)]Cl+2HCl+3H2O(2)2CoCl2+4paoH+2bpy+1/2O2→MeOH2[Co(pao)2(bpy)]Cl+2HCl+H2OThe following experimental points should be mentioned at this point. (a) The reactions between CoCl2, paoH and N,N′-donor ligands in MeOH are [OH-]-independent. Addition of one equivalent of LiOH·H2O in the above described reaction mixtures leads to complexes 1·2H2O and 2·1.5MeOH as well as to unidentified noncrystalline, hydroxo compounds. (b) A number of attempts were made for the isolation of new products by increasing or decreasing the paoH/Co reaction ratio, keeping constant (1 : 1) the phen or bpy : Co ratio. Increasing the former ratio, that is, to 3:1 or 4 : 1, complexes 1 and 2 remained the main products; however, these were contaminated with variable amounts of the known product [CoIII(pao)3] [21] (analytical evidence, unit cell determination of the isolated dark orange crystals). Reducing the above reaction ratio (1 : 1 and/or 0.5/1), paoH-“free” products were isolated containing only bpy or phen and chloride ions. We have not yet found evidence for the existence of the mixed-ligand species [Co(pao)(phen)2]Cl2 and [Co(pao)(bpy)2]Cl2. (c) Both complexes are soluble in water, dimethylformamide, dimethylsulfoxide, and acetonitrile, less soluble in nitromethane and ethanol, and insoluble in benzene, chloroform and dichloromethane.


## 3.2. Description of Structures

Labeled ORTEP plots of complexes1·2H2O and 2·1.5MeOH are shown in Figures 2 and 4, respectively. Selected bond distances and angles for complexes 1·2H2O and 2·1.5MeOH are listed in Table 2.Table 2
Selected bond distances (Å) and angles (°) for complexes1·2H2O and 2·1.5MeOH,a with the estimated standard deviations in parentheses.
1·2H2O2·1.5MeOHBond distancesCo–N(1)1.928(4)1.937(3)Co–N(2)1.904(4)1.909(4)Co–N(3)1.986(4)1.977(4)Co–N(1′)1.928(4)1.937(3)Co–N(2′)1.904(4)1.909(4)Co–N(3′)1.986(4)1.977(4)N(2)–O/O(1)1.294(6)1.273(5)N(3)–C(7)1.322(7)1.343(6)N(1)–C(1)1.343(7)1.340(6)N(2)–C(6)1.298(7)1.309(7)Bond anglesN(3)–Co–N(3′)82.7(2)82.2(2)N(1)–Co–N(3)88.6(2)93.6(2)N(1)–Co–N(2)83.7(2)83.7(2)N(2)–Co–N(2′)89.9(3)89.8(2)N(1)–Co–N(3′)96.1(2)90.7(2)Co–N(2)–O/O(1)122.7(4)123.3(3)aUnprimed and primed atoms are related by symmetry.Figure 2
Partially labeled plot of the molecular structure of the cation that is present in1·2H2O. Primes are used for symmetry related atoms. H atoms have been omitted for clarity.Disregarding the different nature of the N,N′-donor ligands, compounds1·2H2O and 2·1.5MeOH display strikingly similar molecular structures. Thus, only the structure of the former will be described in detail.Complex1·2H2O crystallizes in the tetragonal space group I41/acd. Its structure consists of the mononuclear [Co(pao)2(phen)]+ cation, one chloride ion, and two solvate water molecules; the latter three will not be further discussed. The metal ion lies on a crystallographic 2-fold axis. The CoIII center is in a six-coordinate ligand environment comprising the two nitrogens from two chelating, anionic pao-ligands, [N(1)/N(2) and their symmetry-related partners] and two aromatic nitrogens from the chelating phen molecule [N(3) and N(3′)]. The metal coordination geometry is well described as distorted octahedral, its chromophore being CoIIIN6. Two transpositions of the octahedron are occupied by the pyridyl nitrogen atoms of the two pao- ligands [N(1)–Co–N(1′) = 173.8(3)°]; thus, the two oximate nitrogen atoms [N(2), N(2′)] are in cis position. Angular distortions from perfect octahedral geometry are primarily a consequence of the chelating rings and their restricted bite angles. The Co–N bond lengths agree well with values expected for low-spin CoIII in octahedral environments [21].In the crystal lattice of1·2H2O, the molecules interact through hydrogen bonds forming 1D zig-zag chains (Figure 3). These include the water lattice molecules, the oximate oxygen atom, and the Cl- counteranion; their dimensions are presented in Table 3.Table 3
Hydrogen bonding interactions in1·2H2O.
Interaction D–H⋯AD⋯A (Å)H⋯A (Å)D–H⋯A (°)Symmetry operation of AOW-HWA⋯O2.854(7)1.740(4)161.7(3)x, y, zOW-HWB⋯Cl3.124(6)1.978(2)163.5(3)x, y, zFigure 3
A part of the 1D structure of1·2H2O due to H-bonding interactions (dashed lines) along the a axis. Chlorides (green) are emphasized using space filling models.Figure 4
Partially labeled plot of the molecular structure of the cation that is present in2·1.5MeOH. H atoms have been omitted for clarity. Primes are used for symmetry related atoms.Complex2·1.5MeOH crystallizes in the orthorhombic space group Ic2m; the metal ion lies on a crystallographic twofold axis. One half of the molecule comprises the asymmetric unit of the structure. The three ligands are N,N′-bidentate chelating. Again the pyridyl nitrogen atoms of the two pao- ligands are in trans positions. A packing diagram of the complex is shown in Figure 5.Figure 5
Packing diagram of complex2·1.5MeOH along the c axis. The metal coordination spheres are polyhedron designed (purple). The chloride counteranions and the methanol solvate molecules have been omitted.Since the space group of1·2H2O is centrosymmetric and the space group of 2·1.5MeOH involves a mirror plane, both complexes are racemic mixtures of their Δ and Λ enantiomorphs.Complexes1 and 2 join a small family of structurally characterized homo- [17, 18, 21] and heterometallic [22, 23] Co complexes featuring pao- as ligand. Many years ago Blackmore and Magee [24, 25] and Grant and Magee [26] studied the reactions between 2-pyridinealdoxime and various CoII sources under a variety of reaction conditions. Structural assignments of the solid products [24, 26] were based on spectroscopic data; no X-ray structures were reported. The authors did not prepare mixed-ligand complexes.


## 3.3. Physical and Spectroscopic Characterization

Complexes1 and 2 are diamagnetic, in accordance with their low-spin 3d6 character.The solid-state (diffuse reflectance) UV-Vis spectra of the two complexes are almost identical and typical for low-spinCoIIIN6 chromophores [27]. The low-spin octahedral ground term is A1g1, and there are two relatively low lying spin allowed transitions, with lower lying spin triplet partners, all derived from (t2g)5(eg). Under this scheme, the bands in the spectra of 1 and 2 at ~29.0, 21.5, 17.0, and 13.5 kK are assigned [27] to the A1g1→T2g1, T1g1, T2g3, and T1g3 transitions, respectively, although a superposition of the highest energy d-d transition and a charge transfer band should not be ruled out.Two bands, one of medium intensity at~1015 cm-1 assigned to ν(N–O) and one strong at 1599 cm-1 assigned to ν(C=N)_oximate are common in the IR spectra of the two complexes [21]; the higher-wavenumber band most probably overlaps with an aromatic stretch. The in-plane deformation of the 2-pyridyl ring of the free paoH at 627 cm-1 shifts upward on coordination in the spectra of 1 (643 cm-1) and 2 (645 cm-1) [28].


## 4. Conclusions

The present work extends the body of results that emphasizes the ability of the monoanionic ligand pao- to form interesting structural types in 3d metal chemistry. The use of both paoH and phen or bpy in reactions with CoII sources has led to products 1 and 2, the first mixed-ligand CoIII noncarboxylate complexes involving paoH/pao-. Of interest is the nonparticipation of the deprotonated oximate oxygen atom in coordination; this is due to the involvement of the negatively charged oxygen in hydrogen bonding.Complexes of trivalent 3d metals (e.g.,CrIII, MnIII, FeIII) other than CoIII with the pao-/phen or bpy ligand combinations are not known to date, and it is currently not evident whether the structures of such compounds are dependent on the particular nature of the metal ion. We are studying this matter. Synthetic efforts are also in progress to use 1 and 2 as “metalloligands” for the preparation of heterometallic CoIII/MIII complexes (M = Fe, Mn, lanthanides).



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