# Synthesis, Spectroscopic, and Magnetic Studies of Mono- and Polynuclear Schiff Base Metal Complexes Containing Salicylidene-Cefotaxime Ligand

Authors: J. R. Anacona; Johan Calvo; Ovidio A. Almanza
Journal: International Journal of Inorganic Chemistry
 (2013)

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## Abstract

Metal complexes of a Schiff base ligand derived from cefotaxime and salicylaldehyde were prepared. The salicilydene-cefotaxime ligand (H2L) and mononuclear [M(L)] (M(II) = Co, Ni and Cu), dinuclear [Ag2(L)(OAc)2], and tetranuclear metal complexes [M4(L)(OH)6] (M(II) = Ni, Cu) were characterized on the basis of analytical, thermal, magnetic, and spectral studies (IR, UV-visible, 1H NMR, 13C NMR, and EPR). The electronic spectra of the complexes and their magnetic moments suggesttetrahedral geometry for the isolated complexes. The complexes are nonelectrolytes and insoluble in water and common organic solvents but soluble in DMSO.


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## Body

## 1. Introduction

Interaction between transition metals and proteins is ubiquitous in biochemistry [1]. The fundamental intrinsic nature of these interactions can be studied in metal complexes with amino acid Schiff bases [2], which has led to the suggestion that Schiff bases act as a tridentate ligand containing an azomethine nitrogen atom and the terminal two oxygen atoms of the carboxylate group as well as the hydroxyl group [3]. The field of Schiff base complexes has been fast developing on account of the wide variety of possible structures for the ligands depending upon the aldehydes and amines considered, and various Schiff bases were reported to possess genotoxicity [4–6], antibacterial [7, 8], and antifungal activities [9]. The increasing interest in transition metal complexes containing a Schiff base ligand is derived from their well-established role in biological systems as well as their catalytic and pharmaceutical applications [10, 11].Although the chemistry and spectroscopy of metal complexes of Schiff bases derived from aldehydes and/or ketones and amino acids have been widely studied, rather less is known about their antibiotic analogues. A literature survey revealed that little work involving metal-based antibiotics has been reported so far. Cefotaxime is a third generation cephalosporin antibiotic; like otherβ-lactam antibiotics, it has a broad-spectrum antimicrobial activity [12]. Since the coordination environments of metals in metal-based antibiotics is not well-known and continuing with our studies in order to shed more light on the nature of mono- and polynuclear Schiff base complexes containing antibiotics [13–18], we report here the isolation and characterization of metal(II) complexes containing a Schiff base ligand derived from cefotaxime antibiotic and salicylaldehyde.


## 2. Experimental

### 2.1. Materials and Methods

All necessary precautions were taken to exclude oxygen and moisture during the synthesis and handling of the compounds. Analytical grade chemicals were used as received for all experiments. Fourier transform infrared (FTIR) spectra of the ligand and its metal complexes as KBr pellets were recorded in the spectral range 4,000–400 cm−1 with a Perkin-Elmer Series 2000 apparatus. Measurements of d-d transitions in the visible and near infrared region were taken with a Cary Recording Spectrophotometer Model 17D, while a Perkin-Elmer Spectrophotometer was used for recording the visible and u.v. regions. The contents of C, H, N, and S were analysed on a LECO CHNS 932 model microanalytical instrument. The complexes were analyzed for their metal content with a Perkin-Elmer atomic absorption analyzer, after decomposition with a mixture of HNO3 and HCl followed by H2SO4. Thermograms were recorded on a simultaneous thermal analyzer, STA-6000 (Perkin-Elmer) instrument in air and a heating rate of 4°C min−1 up to 200°C. Magnetic susceptibilities were measured on a Johnson Matthey Susceptibility Balance at room temperature using Hg[Co(NCS)4] as calibrant. EPR spectra were recorded on a Bruker ECS 106 spectrometer by the X-band. 1H and 13C NMR spectra were measured in deuterated DMSO on a Jeol 400 MHz spectrometer. All NMR studies were performed at room temperature, and the chemical shift values were determined in relation to SiMe4.


### 2.2.  Synthesis of Salicilydene-Cefotaxime Ligand (H2L)

To 1 mmol of cefotaxime in 250 mL of hot ethanol was added 1 mmol of salicylaldehyde. The solution was refluxed under nitrogen atmosphere at 50°C for 30 min to give a dark yellow precipitate. This material was filtered off and washed with ethanol and ether and dried under reduced pressure. The product was purified by recrystallization from the same solvent (yield 65%), m.p. 150–152°C.1H NMR (DMSO-d6, δ, ppm): 7.2–7.7 (m, 4H, –phenyl), 10.2 (s, 1H, –OH), 8.7 (s, 1H, HC=N), 11.0 (s, 1H, –COOH), 7.6 (s, 1H, thiazole), 9.1 (s, 1H, –NH–CO–), 6.1 (d, 1H, J=7.2, β-lactam), 6.3 (d, 1H, J=7.4, β-lactam), 4.8 (s, 2H, CH2O), 2.1 (s, 2H, six-membered thiazole ring), 1.9 (s, 6H, CH3); 13C NMR (DMSO-d6, δ, ppm): 170.45 (C15, five-membered thiazole ring), 168.39 (C12, –C=N), 163.62 (C17, –CH=N), 163.43 (C11, –HN–CO), 163.02 (C2, β-lactam), 161.50 (C7, –COOH), 157.82 (C19, –OH–ph), 142.61 (C5), 132.24, 130.46, 121.25, 118.45, 115.82 (C18, C20–C23 phenyl), 58.12 (C3, β-lactam ring), 57.33 (C1, β-lactam ring), 49.23 (C8, –CH2). Anal. Calcd. for (H2L) (C23H21N5O8S2) (%): C, 49.4; N, 12.5; H, 3.8; S, 11.4. Found: C, 49.3; N, 12.3; H, 3.8; S, 11.2.


### 2.3. Synthesis of Mono-[M(L)] (M(II)= Co, Ni, and Cu) and Tetranuclear Schiff Base Complexes [M4(L)(OH)6] (M(II) = Ni, Cu)

Cobalt, nickel, and copper complexes were prepared by the same general method. To a hot solution of 1 mmol (or 4 mmol) of the appropriate M(OAc)2 metal salt in 20 mL of MeOH was slowly added with stirring a solution of 1 mmol of H2L in 10 mL of the same solvent. To this KOH 0.1% of methanol was added to adjust the pH of the solution at 7-8 and the mixture was refluxed for 2 hours. The metal complexes of H2L were separated from the reaction mixture as amorphous solids and washed several times with MeOH and ether and dried under reduced pressure at room temperature (yield 35–45%), m.p. > 250°C. Anal. Calcd. for Co(L):  Co(C23H19N5O8S2) (%): C, 44.8; N, 11.4; H, 3.1; S, 10.4; Co, 9.6. Found: C, 44.5; N, 11.0; H, 3.5; S, 10.1; Co, 9.5. Anal. Calcd. for NiL: Ni(C23H19N5O8S2) (%): C, 44.8; N, 9.5; H, 3.1 S, 10.4; Ni, 9.5. Found: C, 44.6; N, 9.8; H, 3.4; S, 10.6; Ni, 9.2. Anal. Calcd. for Cu(L): Cu(C23H19N5O8S2) (%): C, 44.5; N, 11.3; H, 3.1; S, 10.3; Cu, 10.2. Found: C, 44.1; N, 10.9; H, 2.7; S, 9.8; Cu, 10.1. Anal. Calcd. for Ni4L(OH)6: Ni4(C23H25N5O14S2) (%): C, 30.9; N, 7.8; H, 2.8 S, 7.2; Ni, 26.3. Found: C, 31.2; N, 8.1; H, 2.9; S, 7.5; Ni, 26.6. Anal. Calcd. for Cu4(L)(OH)6: Cu4(C23H25N5O14S2) (%): C, 30.2; N, 7.7; H, 2.8; S, 7.0; Cu, 27.8. Found: C, 29.9; N, 7.5; H, 3.1; S, 6.8; Cu, 27.9.


### 2.4. Synthesis of Dinuclear Schiff Base Complex [Ag2(L)(OAc)2]

To a hot solution of 2 mmol of Ag (OAc) metal salt in 10 mL of dry MeOH was slowly added with stirring a solution of 1 mmol of H2L in 10 mL of the same solvent, under nitrogen atmosphere. The metal(II) complex of H2L was separated from the reaction mixture as amorphous solids and washed several times with MeOH and ether and dried under reduced pressure at room temperature (yield 50–55%), m.p. > 250°C. Anal. Calcd. for Ag2(L)(OAc)2: Ag2(C27H25N5O12S2) (%): C, 36.4; N, 7.9; H, 2.8; S, 7.2; Ag, 24.2. Found: C, 36.5; N, 8.1; H, 3.2; S, 7.1; Ag, 24.1.


## 2.1. Materials and Methods

All necessary precautions were taken to exclude oxygen and moisture during the synthesis and handling of the compounds. Analytical grade chemicals were used as received for all experiments. Fourier transform infrared (FTIR) spectra of the ligand and its metal complexes as KBr pellets were recorded in the spectral range 4,000–400 cm−1 with a Perkin-Elmer Series 2000 apparatus. Measurements of d-d transitions in the visible and near infrared region were taken with a Cary Recording Spectrophotometer Model 17D, while a Perkin-Elmer Spectrophotometer was used for recording the visible and u.v. regions. The contents of C, H, N, and S were analysed on a LECO CHNS 932 model microanalytical instrument. The complexes were analyzed for their metal content with a Perkin-Elmer atomic absorption analyzer, after decomposition with a mixture of HNO3 and HCl followed by H2SO4. Thermograms were recorded on a simultaneous thermal analyzer, STA-6000 (Perkin-Elmer) instrument in air and a heating rate of 4°C min−1 up to 200°C. Magnetic susceptibilities were measured on a Johnson Matthey Susceptibility Balance at room temperature using Hg[Co(NCS)4] as calibrant. EPR spectra were recorded on a Bruker ECS 106 spectrometer by the X-band. 1H and 13C NMR spectra were measured in deuterated DMSO on a Jeol 400 MHz spectrometer. All NMR studies were performed at room temperature, and the chemical shift values were determined in relation to SiMe4.


## 2.2.  Synthesis of Salicilydene-Cefotaxime Ligand (H2L)

To 1 mmol of cefotaxime in 250 mL of hot ethanol was added 1 mmol of salicylaldehyde. The solution was refluxed under nitrogen atmosphere at 50°C for 30 min to give a dark yellow precipitate. This material was filtered off and washed with ethanol and ether and dried under reduced pressure. The product was purified by recrystallization from the same solvent (yield 65%), m.p. 150–152°C.1H NMR (DMSO-d6, δ, ppm): 7.2–7.7 (m, 4H, –phenyl), 10.2 (s, 1H, –OH), 8.7 (s, 1H, HC=N), 11.0 (s, 1H, –COOH), 7.6 (s, 1H, thiazole), 9.1 (s, 1H, –NH–CO–), 6.1 (d, 1H, J=7.2, β-lactam), 6.3 (d, 1H, J=7.4, β-lactam), 4.8 (s, 2H, CH2O), 2.1 (s, 2H, six-membered thiazole ring), 1.9 (s, 6H, CH3); 13C NMR (DMSO-d6, δ, ppm): 170.45 (C15, five-membered thiazole ring), 168.39 (C12, –C=N), 163.62 (C17, –CH=N), 163.43 (C11, –HN–CO), 163.02 (C2, β-lactam), 161.50 (C7, –COOH), 157.82 (C19, –OH–ph), 142.61 (C5), 132.24, 130.46, 121.25, 118.45, 115.82 (C18, C20–C23 phenyl), 58.12 (C3, β-lactam ring), 57.33 (C1, β-lactam ring), 49.23 (C8, –CH2). Anal. Calcd. for (H2L) (C23H21N5O8S2) (%): C, 49.4; N, 12.5; H, 3.8; S, 11.4. Found: C, 49.3; N, 12.3; H, 3.8; S, 11.2.


## 2.3. Synthesis of Mono-[M(L)] (M(II)= Co, Ni, and Cu) and Tetranuclear Schiff Base Complexes [M4(L)(OH)6] (M(II) = Ni, Cu)

Cobalt, nickel, and copper complexes were prepared by the same general method. To a hot solution of 1 mmol (or 4 mmol) of the appropriate M(OAc)2 metal salt in 20 mL of MeOH was slowly added with stirring a solution of 1 mmol of H2L in 10 mL of the same solvent. To this KOH 0.1% of methanol was added to adjust the pH of the solution at 7-8 and the mixture was refluxed for 2 hours. The metal complexes of H2L were separated from the reaction mixture as amorphous solids and washed several times with MeOH and ether and dried under reduced pressure at room temperature (yield 35–45%), m.p. > 250°C. Anal. Calcd. for Co(L):  Co(C23H19N5O8S2) (%): C, 44.8; N, 11.4; H, 3.1; S, 10.4; Co, 9.6. Found: C, 44.5; N, 11.0; H, 3.5; S, 10.1; Co, 9.5. Anal. Calcd. for NiL: Ni(C23H19N5O8S2) (%): C, 44.8; N, 9.5; H, 3.1 S, 10.4; Ni, 9.5. Found: C, 44.6; N, 9.8; H, 3.4; S, 10.6; Ni, 9.2. Anal. Calcd. for Cu(L): Cu(C23H19N5O8S2) (%): C, 44.5; N, 11.3; H, 3.1; S, 10.3; Cu, 10.2. Found: C, 44.1; N, 10.9; H, 2.7; S, 9.8; Cu, 10.1. Anal. Calcd. for Ni4L(OH)6: Ni4(C23H25N5O14S2) (%): C, 30.9; N, 7.8; H, 2.8 S, 7.2; Ni, 26.3. Found: C, 31.2; N, 8.1; H, 2.9; S, 7.5; Ni, 26.6. Anal. Calcd. for Cu4(L)(OH)6: Cu4(C23H25N5O14S2) (%): C, 30.2; N, 7.7; H, 2.8; S, 7.0; Cu, 27.8. Found: C, 29.9; N, 7.5; H, 3.1; S, 6.8; Cu, 27.9.


## 2.4. Synthesis of Dinuclear Schiff Base Complex [Ag2(L)(OAc)2]

To a hot solution of 2 mmol of Ag (OAc) metal salt in 10 mL of dry MeOH was slowly added with stirring a solution of 1 mmol of H2L in 10 mL of the same solvent, under nitrogen atmosphere. The metal(II) complex of H2L was separated from the reaction mixture as amorphous solids and washed several times with MeOH and ether and dried under reduced pressure at room temperature (yield 50–55%), m.p. > 250°C. Anal. Calcd. for Ag2(L)(OAc)2: Ag2(C27H25N5O12S2) (%): C, 36.4; N, 7.9; H, 2.8; S, 7.2; Ag, 24.2. Found: C, 36.5; N, 8.1; H, 3.2; S, 7.1; Ag, 24.1.


## 3. Results and Discussion

Through a condensation reaction an amino group available in the drug substance cefotaxime was allowed to react with salicylaldehyde to form a Schiff base ligand H2L which was, subsequently, reacted with metal ions to form mono- and polynuclear Schiff base metal complexes. The synthetic route of H2L ligand and the [ML] complexes is given in Scheme 1. The ligand and the metal(II) complexes were isolated pure from MeOH in very good yields and they are of various colors. The ligand is yellow; iron and nickel are green while silver and cobalt are dark red complexes in color. All the complexes did not melt/decompose when heated up to 250°C. The analytical data of the complexes correspond well with 1 : 1, 2 : 1, or 4 : 1 metal : ligand stoichiometries. Thus, the general formulae [M(L)] (M(II) = Co, Ni, Cu), [Ag2(L)(OAc)2], and [M4(L)(OH)6] (M(II) = Ni, Cu) have been assigned to the mono- and polynuclear complexes, respectively, and they are very air stable solids at room temperature without decomposition for a long time. The complexes are insoluble in water and other common organic solvents such as ethanol, chloroform, benzene, acetone, dichloromethane, DMF, acetonitrile, and diethyl ether but soluble in DMSO. Thermograms of the metal complexes indicate that the complexes are stable with no hydration water and solvent molecules. The molar conductance values measured in DMSO at room temperature vary from 7.0 to 16.7 S cm2 mol−1, revealing the nonelectrolytic nature of the complexes [19].Scheme 1


### 3.1.1H and 13C NMR Spectra

The NMR spectra of free ligand are reported along with possible assignments in the experimental section.1H NMR spectrum of the Schiff base ligand was recorded in DMSO-d6. All the protons were found as to be in their expected region [20]. The number of protons and carbons calculated from the integration curves and those obtained from the values of the expected elemental analyses agree well with each other. The paramagnetic nature of the complexes produced precluded detailed studies of the products by NMR spectroscopy. 13C NMR spectrum of salicylidene-cefotaxime ligand was also recorded in DMSO-d6. All assignments of the carbon atoms due to heteroatomic and/or aromatic groups were found in their expected region [20, 21] and are well supported by their IR and 1H NMR spectra. The results also indicate that the presence of number of carbons agrees well with the expected number of carbons.


### 3.2. FT-IR Spectra

Infrared spectroscopy provides valuable information as to whether or not condensation to form imine bonds has occurred. The salicylaldehyde produces band close to 1700 cm−1 while the terminal NH2 group of the cefotaxime gives N–H stretching vibrations at 3200 and 3300 cm−1. The C=N imine band, at 1650 cm−1, does not overlap with the above bands and simple observation of the 1600–1700 cm−1 region indicates the success or failure of a reaction. The spectra of the studied metal(II) complexes show significant bands from 1600 to 1640 cm−1 which may be assigned to ν(C=N) stretching modes of the coordinated ligand H2L. The shift of this band on complexation towards lower wave numbers indicates coordination of the azomethine nitrogen to the metal center [22, 23]. The main IR wavenumbers can be seen in Table 1.Table 1
Main IR wavenumbers (cm−1).
Compound
ν(C=O)
ν(C=N)
ν(COO)
ν(COO)
Δν
lactam
imine
asymm.
sym.
Schiff base
1740
1650
[Co(L)]
1730
1630
1550
1340
210
[Ni(L)]
1730
1630
1580
1360
220
[Cu(L)]
1730
1630
1580
1360
220
[Ag2(L)(OAc)2]
1750
1640
1590
1380
210
[Ni4(L)(OH)6]
1750
1640
1580
1370
210
[Cu4(L)(OH)6]
1750
1640
1570
1360
210The infrared spectrum of the Schiff base ligand shows a strong absorption band at 1730 cm−1 which can be assigned to lactam ν(C=O) vibrational mode. This band shifted in the metal complexes. The shifts of this band toward higher wavenumbers for polynuclear complexes rather strange but they have been observed in cephalosporin metal complexes of cefazolin [16], ceftriaxone [17], and cephalosporin Schiff base metal complexes [24]. Probably, the absorption band of the lactam carbonyl moiety of the Ag2, Ni4, and Cu4 complexes was shifted to higher frequency due to greater rigidity shown by this group when coordinated.The amide (C=O) band is unshifted in the complexes compared to the free ligands. Furthermore, the C–N–C stretching and the N–H stretching vibrations of the CONH residues observed in free Schiff base at 1180 and 3240 cm−1, respectively, either do not shift or show a slight shift in all the metal complexes indicating that these N atoms were not involved in coordination. Given the significant shifts in the lactam C=O band in the complexes, we suggest that coordination of the Schiff base ligand occurs through the oxygen atom from the lactam rather than the amide carbonyl group [22].Theν(C–OH) phenolic stretching frequency of ligand is seen at 1345 cm−1 which gets shifted to a lower frequency region in the complexes in the range of 1332–1326 cm−1, and this is indicative of bonding through phenolic oxygen [25]. Also, disappearance of the stretching frequency at 1710 cm−1 assigned to ν(C=O) from COOH moiety in the ligand and appearance in the complexes of new νas and νs modes of the (−COO−) group at 1550–1580 and 1340–1370 cm−1 ranges, respectively, indicate that the Schiff base has reacted. These and the Δν value (νas-νs) > 200 cm−1 are consistent with carboxylate monodentate coordination with the metal atoms. These overall data suggest that the azomethine-N, phenolic-O, carboxylate-O, and lactam C=O moieties are involved in coordination with the metal(II) ion in complexes and that the Schiff base behaves as a tetradentate ligand.Furthermore, the appearance of new bands in the 540–490 cm−1 ranges attributed to ν(M–N) stretching vibrations, observed in the spectra of the complexes (absent in the free ligand), provides evidence that the C=N moiety could be bonded to the metal ion through the nitrogen atom. The complexes also show bands in the 1430–1460, 1070–1100, and 720–740 cm−1 ranges which can be assigned to phenyl ring vibrations. Medium intensity band appearing in the 2850–2950 cm−1 region corresponds to aliphatic ν(C–H), while aromatic ν(C–H) stretches appear in the 3000–3100 cm−1 region. Lastly, the bands in the 460–410 cm−1 region observed in all complexes, and absent in the free ligands, could be tentatively assigned to ν(M–O) vibrations. A broad band at 3430 cm−1 observed in the [M4(L)(OH)6] complexes is assigned to ν(OH).


### 3.3. Electronic Spectra

The electronic spectra of the Schiff base ligand as well as the complexes in 10−3 M DMSO solutions showed two broad bands in the regions 230–280 nm and 300–335 nm. The former band is assigned to the absorption of (Lb1→A11) of the benzene ring, while the second band is assigned to π-π* (C=N–) transition of the azomethine group, which is shifted to lower wavelength on coordination [26].As is known, the electronic spectra of the complexes show that the absorptions around 400–900 nm are due to ligand to metal charge-transfer and/or d-d transition bands of the metal in the complexes. The electronic spectra of the complexes exhibit two bands atca. 570–670 nm (ε = 148–180 L mol−1 cm−1) and at ca. 420–440 nm (ε = 1.16–3.65 × 103 L mol−1 cm−1). The first band is probably due to the A24→T14 (P) for [Co(L)], A23→T23 (F) for [Ni(L)], and T22→E22 (G) for [Cu(L)] transition, and the second due to the charge transfer transition of tetrahedral geometry [27–32]. The [Ag2(L)(OAc)2] and [M4(L)(OH)6] complexes exhibit a band at 420~430 nm which may be attributed to the d-d transition of the metal in a tetrahedral environment [33]. In addition, they show a strong absorption in the short wavelength range, 385–395 nm, which may be attributed to the charge-transfer absorption bands, due to the spin-exchange interaction between the metalII ions [33].


### 3.4. Magnetic Measurements

All the complexes are paramagnetic. From the molar magnetic susceptibility values, corrected magnetic moments were calculated using Pascal’s constants. The [Co(L)] complex has a magnetic moment of 4.50 B.M. typical for high spin d7 systems with three unpaired electrons. The value observed for this complex is higher than the value expected for square-planar geometry (2.1–2.8) and consistent with the value expected for high spin tetrahedral geometry [34]. The [Ni(L)] complex has a magnetic moment of 3.72 B.M. as predicted for high spin d8 systems with two unpaired electrons and in agreement with the values reported for tetrahedral geometry around the nickel(II) ion [34]. The [Cu(L)] complex has a magnetic moment of 1.75 B.M. at room temperature, in the range associated with d9 systems with one unpaired electron.The room temperature EPR spectrum of a powder sample of the [Cu(L)] complex showed a single signal with poorly resolved hyperfine structure. The EPR spectrum of the [Cu4(L)(OH)6] complex also shows a single broad signal with poor resolution of the hyperfine structure on both sides of the main signal and the g values, g∥=2.17 and g⊥=2.05, and the calculated axial symmetry parameter, G=3.4, supports [35] the suggestion that there is no considerable exchange interaction between the copper centers (G < 4). In general, polynuclear Cu(II) complexes give broad EPR peaks and the broadening is assigned to a dipolar interaction [36]. The greater value of g∥ compared to g⊥ proposes a distorted tetrahedral-square pyramidal structure and rules out the possibility of a trigonal bipyramidal structure which is expected to have g⊥>g∥. Also, the observed g∥ values of less than 2.3 provide evidence for the covalent character of bonding between Cu(II) ion and the ligand [37, 38].For the complex [Ni4(L)(OH)6] the χMT product at 300 K is equal to 4.161 cm3 mol−1 K which corresponds to an effective magnetic moment of 5.8 M.B.; this value is similar to the theoretical value expected for four uncoupled nickel(II) ions. For the complex [Cu4(L)(OH)6] the χMT product is 1.335 cm3 mol−1 K at room temperature which corresponds to an effective magnetic moment of 3.3 M.B.; this value is very close to the theoretical value expected for four independent copperII ions. Thus, these complexes with noninteracting metal centres have magnetic properties that are the same as seen in the mononuclear complex of the same metal.Notwithstanding that the synthesis of silver complex was carried out under nitrogen atmosphere, presumably air oxidation occurs and the Schiff base ligand having delocalizedπ-orbital system is able to coordinate to the central silver ion under the form of semiquinone allowing to obtain a paramagnetic complex compound. During the course of our research we observed that addition of silver acetate to an aqueous suspension of a 50% MeOH solution of H2L resulted in the disproportionation of silverI to the free metal and the silver complex at an observable and rather rapid rate, depending on conditions of concentration and temperature. The silver complex, isolated as [Ag2(L)(OAc)2], is a dark red solid which can be conveniently recrystallized from water/dimethylsulphoxide.The X-band EPR spectrum of a powdered sample of the [Ag2(L)(OAc)2] complex at room temperature revealed the existence of two paramagnetic centres. The first is a semiquinone radical which exhibits a sharp but not so intense one line EPR spectrum centered at 3330 G, g=1.99, and a line width of 70 G. This calculated electronic g factor, which is close to that of the free electron value (2.0023), as well as the relatively small width of the line as compared with the spectra of other complexes, suggests a more pronounced electron density delocalization on the Schiff base ligand, through the silver ion which is large in size and hence more polarizable.The second paramagnetic centre shows the features of an intense signal centered at 3200 G and total width of 960 G, for anS=1, dinuclear silver product, with a g value of 2.08 which coincides with those reported earlier [39, 40]. The spectrum exhibits a dissymmetric broad band which indicates a magnetic spin-exchange interaction between the two spins, SAg(II)=1/2 [41]. Thus, the appearance of this EPR signal shows that the silver complex has unpaired electrons with a high density on the silver nuclei, that is, must contains Ag(II).The hyperfine doublet structure characteristic of the nuclear spins of107Ag (I=1/2, 51.82%, and 109Ag (I=1/2, 48.18%) could not be resolved due to the fact that the centres are not diluted and the magnetic moments of each isotope differ by less than 20%. Also, the superhyperfine coupling due to 14N nucleus was not observed. The obtained signals are a proof of the Schiff base radical character and are in agreement with ascribing the complex structure of a free radical stabilized through the cation. The formation of this novel complex illustrates further the effect of the exceptionally strong ligand field exerted by the salicylidene-cefotaxime ligand. This serves to raise antibonding levels (d orbitals) in the species of lower oxidation state to such a high energy that electrons are easily removed.For the complex [Ag2(L)(OAc)2] the χMT product at 300 K is equal to 2.880 cm3 mol−1 K which corresponds to an effective magnetic moment of 4.8 M.B.; this value is higher than the theoretical value expected for two uncoupled silver(II) ions. The electron spins on two metal centres in an oxocarboxylate complex can have two interactions—a ferromagnetic interaction where both the spins are parallel or an antiferromagnetic interaction where the electron spins are opposite to each other. The different interactions between the spins can be determined by the bond angle between the two metal centres and the bridging oxygen. Studies of hydroxide bridged copper dimers [42] have shown that when the metal centres are close together, the spins will have a ferromagnetic interaction and this would be the case of the Schiff base silver complex.We have attempted to grow single crystals of the metal chelates but in no case have we had any success, due to their insolubility in common organic solvents. These studies represent a contribution to future crystallographic analyses, which are complicated by the difficulties in obtaining X-ray quality crystals of cephalosporins complexes. Based on the composition of these complexes, their IR, EPR, electronic spectra, conductivity measurements, and magnetic characterization, we propose that polynuclear complexes would have the coordination environment as shown in Figure1. Similarly, the isolation and characterization of metal(II) complexes containing a Schiff base ligand derived from cefixime antibiotic and salicylaldehyde were carried out [24]. Analytical data indicated the formation of M : Schiff base (1 : 2) complexes, in which ligand is bidentate via azomethine-N and deprotonated salicyl-O moiety.Figure 1
Suggested structures for [Ag2(L)(OAc)2] and [M4(L)(OH)6] complexes.


## 3.1.1H and 13C NMR Spectra

The NMR spectra of free ligand are reported along with possible assignments in the experimental section.1H NMR spectrum of the Schiff base ligand was recorded in DMSO-d6. All the protons were found as to be in their expected region [20]. The number of protons and carbons calculated from the integration curves and those obtained from the values of the expected elemental analyses agree well with each other. The paramagnetic nature of the complexes produced precluded detailed studies of the products by NMR spectroscopy. 13C NMR spectrum of salicylidene-cefotaxime ligand was also recorded in DMSO-d6. All assignments of the carbon atoms due to heteroatomic and/or aromatic groups were found in their expected region [20, 21] and are well supported by their IR and 1H NMR spectra. The results also indicate that the presence of number of carbons agrees well with the expected number of carbons.


## 3.2. FT-IR Spectra

Infrared spectroscopy provides valuable information as to whether or not condensation to form imine bonds has occurred. The salicylaldehyde produces band close to 1700 cm−1 while the terminal NH2 group of the cefotaxime gives N–H stretching vibrations at 3200 and 3300 cm−1. The C=N imine band, at 1650 cm−1, does not overlap with the above bands and simple observation of the 1600–1700 cm−1 region indicates the success or failure of a reaction. The spectra of the studied metal(II) complexes show significant bands from 1600 to 1640 cm−1 which may be assigned to ν(C=N) stretching modes of the coordinated ligand H2L. The shift of this band on complexation towards lower wave numbers indicates coordination of the azomethine nitrogen to the metal center [22, 23]. The main IR wavenumbers can be seen in Table 1.Table 1
Main IR wavenumbers (cm−1).
Compound
ν(C=O)
ν(C=N)
ν(COO)
ν(COO)
Δν
lactam
imine
asymm.
sym.
Schiff base
1740
1650
[Co(L)]
1730
1630
1550
1340
210
[Ni(L)]
1730
1630
1580
1360
220
[Cu(L)]
1730
1630
1580
1360
220
[Ag2(L)(OAc)2]
1750
1640
1590
1380
210
[Ni4(L)(OH)6]
1750
1640
1580
1370
210
[Cu4(L)(OH)6]
1750
1640
1570
1360
210The infrared spectrum of the Schiff base ligand shows a strong absorption band at 1730 cm−1 which can be assigned to lactam ν(C=O) vibrational mode. This band shifted in the metal complexes. The shifts of this band toward higher wavenumbers for polynuclear complexes rather strange but they have been observed in cephalosporin metal complexes of cefazolin [16], ceftriaxone [17], and cephalosporin Schiff base metal complexes [24]. Probably, the absorption band of the lactam carbonyl moiety of the Ag2, Ni4, and Cu4 complexes was shifted to higher frequency due to greater rigidity shown by this group when coordinated.The amide (C=O) band is unshifted in the complexes compared to the free ligands. Furthermore, the C–N–C stretching and the N–H stretching vibrations of the CONH residues observed in free Schiff base at 1180 and 3240 cm−1, respectively, either do not shift or show a slight shift in all the metal complexes indicating that these N atoms were not involved in coordination. Given the significant shifts in the lactam C=O band in the complexes, we suggest that coordination of the Schiff base ligand occurs through the oxygen atom from the lactam rather than the amide carbonyl group [22].Theν(C–OH) phenolic stretching frequency of ligand is seen at 1345 cm−1 which gets shifted to a lower frequency region in the complexes in the range of 1332–1326 cm−1, and this is indicative of bonding through phenolic oxygen [25]. Also, disappearance of the stretching frequency at 1710 cm−1 assigned to ν(C=O) from COOH moiety in the ligand and appearance in the complexes of new νas and νs modes of the (−COO−) group at 1550–1580 and 1340–1370 cm−1 ranges, respectively, indicate that the Schiff base has reacted. These and the Δν value (νas-νs) > 200 cm−1 are consistent with carboxylate monodentate coordination with the metal atoms. These overall data suggest that the azomethine-N, phenolic-O, carboxylate-O, and lactam C=O moieties are involved in coordination with the metal(II) ion in complexes and that the Schiff base behaves as a tetradentate ligand.Furthermore, the appearance of new bands in the 540–490 cm−1 ranges attributed to ν(M–N) stretching vibrations, observed in the spectra of the complexes (absent in the free ligand), provides evidence that the C=N moiety could be bonded to the metal ion through the nitrogen atom. The complexes also show bands in the 1430–1460, 1070–1100, and 720–740 cm−1 ranges which can be assigned to phenyl ring vibrations. Medium intensity band appearing in the 2850–2950 cm−1 region corresponds to aliphatic ν(C–H), while aromatic ν(C–H) stretches appear in the 3000–3100 cm−1 region. Lastly, the bands in the 460–410 cm−1 region observed in all complexes, and absent in the free ligands, could be tentatively assigned to ν(M–O) vibrations. A broad band at 3430 cm−1 observed in the [M4(L)(OH)6] complexes is assigned to ν(OH).


## 3.3. Electronic Spectra

The electronic spectra of the Schiff base ligand as well as the complexes in 10−3 M DMSO solutions showed two broad bands in the regions 230–280 nm and 300–335 nm. The former band is assigned to the absorption of (Lb1→A11) of the benzene ring, while the second band is assigned to π-π* (C=N–) transition of the azomethine group, which is shifted to lower wavelength on coordination [26].As is known, the electronic spectra of the complexes show that the absorptions around 400–900 nm are due to ligand to metal charge-transfer and/or d-d transition bands of the metal in the complexes. The electronic spectra of the complexes exhibit two bands atca. 570–670 nm (ε = 148–180 L mol−1 cm−1) and at ca. 420–440 nm (ε = 1.16–3.65 × 103 L mol−1 cm−1). The first band is probably due to the A24→T14 (P) for [Co(L)], A23→T23 (F) for [Ni(L)], and T22→E22 (G) for [Cu(L)] transition, and the second due to the charge transfer transition of tetrahedral geometry [27–32]. The [Ag2(L)(OAc)2] and [M4(L)(OH)6] complexes exhibit a band at 420~430 nm which may be attributed to the d-d transition of the metal in a tetrahedral environment [33]. In addition, they show a strong absorption in the short wavelength range, 385–395 nm, which may be attributed to the charge-transfer absorption bands, due to the spin-exchange interaction between the metalII ions [33].


## 3.4. Magnetic Measurements

All the complexes are paramagnetic. From the molar magnetic susceptibility values, corrected magnetic moments were calculated using Pascal’s constants. The [Co(L)] complex has a magnetic moment of 4.50 B.M. typical for high spin d7 systems with three unpaired electrons. The value observed for this complex is higher than the value expected for square-planar geometry (2.1–2.8) and consistent with the value expected for high spin tetrahedral geometry [34]. The [Ni(L)] complex has a magnetic moment of 3.72 B.M. as predicted for high spin d8 systems with two unpaired electrons and in agreement with the values reported for tetrahedral geometry around the nickel(II) ion [34]. The [Cu(L)] complex has a magnetic moment of 1.75 B.M. at room temperature, in the range associated with d9 systems with one unpaired electron.The room temperature EPR spectrum of a powder sample of the [Cu(L)] complex showed a single signal with poorly resolved hyperfine structure. The EPR spectrum of the [Cu4(L)(OH)6] complex also shows a single broad signal with poor resolution of the hyperfine structure on both sides of the main signal and the g values, g∥=2.17 and g⊥=2.05, and the calculated axial symmetry parameter, G=3.4, supports [35] the suggestion that there is no considerable exchange interaction between the copper centers (G < 4). In general, polynuclear Cu(II) complexes give broad EPR peaks and the broadening is assigned to a dipolar interaction [36]. The greater value of g∥ compared to g⊥ proposes a distorted tetrahedral-square pyramidal structure and rules out the possibility of a trigonal bipyramidal structure which is expected to have g⊥>g∥. Also, the observed g∥ values of less than 2.3 provide evidence for the covalent character of bonding between Cu(II) ion and the ligand [37, 38].For the complex [Ni4(L)(OH)6] the χMT product at 300 K is equal to 4.161 cm3 mol−1 K which corresponds to an effective magnetic moment of 5.8 M.B.; this value is similar to the theoretical value expected for four uncoupled nickel(II) ions. For the complex [Cu4(L)(OH)6] the χMT product is 1.335 cm3 mol−1 K at room temperature which corresponds to an effective magnetic moment of 3.3 M.B.; this value is very close to the theoretical value expected for four independent copperII ions. Thus, these complexes with noninteracting metal centres have magnetic properties that are the same as seen in the mononuclear complex of the same metal.Notwithstanding that the synthesis of silver complex was carried out under nitrogen atmosphere, presumably air oxidation occurs and the Schiff base ligand having delocalizedπ-orbital system is able to coordinate to the central silver ion under the form of semiquinone allowing to obtain a paramagnetic complex compound. During the course of our research we observed that addition of silver acetate to an aqueous suspension of a 50% MeOH solution of H2L resulted in the disproportionation of silverI to the free metal and the silver complex at an observable and rather rapid rate, depending on conditions of concentration and temperature. The silver complex, isolated as [Ag2(L)(OAc)2], is a dark red solid which can be conveniently recrystallized from water/dimethylsulphoxide.The X-band EPR spectrum of a powdered sample of the [Ag2(L)(OAc)2] complex at room temperature revealed the existence of two paramagnetic centres. The first is a semiquinone radical which exhibits a sharp but not so intense one line EPR spectrum centered at 3330 G, g=1.99, and a line width of 70 G. This calculated electronic g factor, which is close to that of the free electron value (2.0023), as well as the relatively small width of the line as compared with the spectra of other complexes, suggests a more pronounced electron density delocalization on the Schiff base ligand, through the silver ion which is large in size and hence more polarizable.The second paramagnetic centre shows the features of an intense signal centered at 3200 G and total width of 960 G, for anS=1, dinuclear silver product, with a g value of 2.08 which coincides with those reported earlier [39, 40]. The spectrum exhibits a dissymmetric broad band which indicates a magnetic spin-exchange interaction between the two spins, SAg(II)=1/2 [41]. Thus, the appearance of this EPR signal shows that the silver complex has unpaired electrons with a high density on the silver nuclei, that is, must contains Ag(II).The hyperfine doublet structure characteristic of the nuclear spins of107Ag (I=1/2, 51.82%, and 109Ag (I=1/2, 48.18%) could not be resolved due to the fact that the centres are not diluted and the magnetic moments of each isotope differ by less than 20%. Also, the superhyperfine coupling due to 14N nucleus was not observed. The obtained signals are a proof of the Schiff base radical character and are in agreement with ascribing the complex structure of a free radical stabilized through the cation. The formation of this novel complex illustrates further the effect of the exceptionally strong ligand field exerted by the salicylidene-cefotaxime ligand. This serves to raise antibonding levels (d orbitals) in the species of lower oxidation state to such a high energy that electrons are easily removed.For the complex [Ag2(L)(OAc)2] the χMT product at 300 K is equal to 2.880 cm3 mol−1 K which corresponds to an effective magnetic moment of 4.8 M.B.; this value is higher than the theoretical value expected for two uncoupled silver(II) ions. The electron spins on two metal centres in an oxocarboxylate complex can have two interactions—a ferromagnetic interaction where both the spins are parallel or an antiferromagnetic interaction where the electron spins are opposite to each other. The different interactions between the spins can be determined by the bond angle between the two metal centres and the bridging oxygen. Studies of hydroxide bridged copper dimers [42] have shown that when the metal centres are close together, the spins will have a ferromagnetic interaction and this would be the case of the Schiff base silver complex.We have attempted to grow single crystals of the metal chelates but in no case have we had any success, due to their insolubility in common organic solvents. These studies represent a contribution to future crystallographic analyses, which are complicated by the difficulties in obtaining X-ray quality crystals of cephalosporins complexes. Based on the composition of these complexes, their IR, EPR, electronic spectra, conductivity measurements, and magnetic characterization, we propose that polynuclear complexes would have the coordination environment as shown in Figure1. Similarly, the isolation and characterization of metal(II) complexes containing a Schiff base ligand derived from cefixime antibiotic and salicylaldehyde were carried out [24]. Analytical data indicated the formation of M : Schiff base (1 : 2) complexes, in which ligand is bidentate via azomethine-N and deprotonated salicyl-O moiety.Figure 1
Suggested structures for [Ag2(L)(OAc)2] and [M4(L)(OH)6] complexes.



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*Source: 108740-2013-04-30.xml*