# Mixed-Ligand Nickel(II) Complexes Containing Sulfathiazole and

Authors: J. R. Anacona; Maried Lopez
Journal: International Journal of Inorganic Chemistry
 (2012)

---

## Abstract

Nickel(II) reacts with cephalosporins plus sulfathiazole (Hstz) to form the following mixed-ligand complexes of general formulae  [Ni(L)(stz)(H2O)x]n
(L1,4, x=1; L2,3, x=0; L = monoanion of cefazolin HL1, cephalothin HL2, cefotaxime HL3, ceftriaxone HL4) and [Ni(L5)(stz)]Cl (cefepime L5), which were characterized by physicochemical and spectroscopic methods. Their spectra indicated that cephalosporins are acting as multidentate chelating agents, via the lactam carbonyl and carboxylate and N-azomoieties. The complexes are insoluble in water and common organic solvents but soluble in DMSO, where the [Ni(L5)(stz)]Cl complex is 1 : 1 electrolyte. They probably have polymeric structures. They have been screened for antibacterial activity, and the results are compared with the activity of commercial cephalosporins.


---

## Body

## 1. Introduction

Cephalosporins are classed asβ-lactam antibiotics, and they are widely used in clinical therapy for the treatment of severe infections, because of their antibacterial activity [1, 2]. Most common among several mechanisms by which bacteria develop resistance to β-lactam antibiotics is by elaboration of the enzyme β-lactamase, which hydrolyzes the β-lactam ring. A second mechanism is through alteration of penicillin-binding proteins (PBPs), which are found as both membrane-bound and cytoplasmic enzymes that catalyze cross-linking reactions in bacterial cell wall synthesis [3, 4]. PBPs are targets of β-lactam antibiotics, which interfere with cell wall synthesis by binding covalently to the catalytic site. Most bacterial species produce several PBPs, differing in molecular weight, affinity for binding β-lactam antibiotics, and enzymatic function (e.g., transpeptidase, carboxypeptidase, or endopeptidase). The PBPs are usually broadly classified into high-molecular-weight and low-molecular-weight categories [3, 4].Prior to the availability and application of antibiotics for the control of diseases, sulfonamides were employed as effective chemotherapeutic agents for the prevention and cure of bacterial infections in humans [5, 6]. Certain microbes require p-aminobenzoic acid (PABA) in order to synthesize dihydrofolic acid, which is required to produce purines and ultimately nucleic acids. Sulfonamides, chemical analogs of PABA, are competitive inhibitors of dihydropteroate synthetase. The complex formation between metal ions and sulfa drugs has also been extensively studied with a view to establish the relationship and importance of metal-drug interactions [7–10].The interaction of antibiotics with main and transition metal ions has attracted our attention and compelled us to combine their chemistry in order to establish whether complexation affects the pharmacological properties of the ligand and to derive additional fundamental knowledge about antibiotic action [11–16]. We report here the synthesis, characterization, and antibacterial activity of nickel(II) complexes containing both sulfathiazole and cephalosporins ligands, in order to combine their antibacterial activities. The chemical structures of the ligands studied in this paper are shown in Figure 1.Figure 1
The structure of the ligands.


## 2. Experimental

### 2.1. Physical Methods

All chemicals of reagent grade were commercially obtained from either Aldrich or Sigma and used without further purification. Solvents were redistilled by standard techniques before use. IR spectra were recorded as KBr pellets in the 4000–400 cm−1 range with a Perkin-Elmer Series 2000 FT-IR spectrophotometer. The electronic spectra of 1 × 10−3 M in DMSO solution of the ligand and its complex were recorded in the UV-Vis. region using a Shimadzu UV-240 spectrophotometer. The diffuse reflectance spectra of all the complexes in the 360–850 nm region were recorded on the same instrument equipped with a spherical reflectance assembly using BaSO4 as reference. C, H, N, and S were analyzed on a LECO CHNS 932 model microanalytical instrument. Nickel contents were estimated with a Perkin-Elmer atomic absorption spectrophotometer. The halogen content was determined by combustion of the solid complex (30 mg) in an oxygen flask in the presence of a KOH–H2O2 mixture. The halide content was then determined by titration with a standard Hg(NO3)2 solution using diphenyl carbazone as an indicator. Thermograms were recorded on a simultaneous thermal analyzer, STA-6000 (Perkin Elmer) instrument at a heating rate of 4°C min−1. Magnetic susceptibilities were measured on a Johnson Matthey Susceptibility Balance at 298 K. The effective magnetic moments were calculated from the expression μeff=2.828 (χMT)1/2 B.M., where χM is the molar susceptibility corrected using Pascal’s constants for diamagnetism of all atoms in the compounds. ESR spectra of the copper complexes were recorded on a JEOL microwave unit, JES-FE2XG Spectrophotometer. The magnetic field was calibrated with 2,2-diphenyl-1-picrylhydrazyl.


### 2.2. Antibacterial Activity Tests

Antibacterial activities of cephalosporins and their complexes were tested using the paper disc diffusion method [17]. The chosen strains were G(+) Staphylococcus aureus ATCC 25923 and G(−) Escherichia coli ATCC 11775, Pseudomonas aeruginosa ATCC 27853, Klebsiella pneumoniae ATCC 23357, Salmonella enteritidis CDC 64, and Bacillus subtilis ATCC 6051. The liquid medium containing the bacterial subcultures was autoclaved for 20 min at 121°C before inoculation. The bacteria were then cultured for 24 h at 36°C in an incubator. Muller Hinton broth was used for preparing basal media for the bioassay of the organisms. Nutrient agar was poured onto a plate and allowed to solidify. The test compounds in DMSO solutions (5 × 10−2 M) were added dropwise (10 μL) to a 5 mm diameter filter paper disc placed at the centre of each agar plate. The plates were then kept at 5°C for 1 h then transferred to an incubator maintained at 36°C. The width of the growth inhibition zone around the disc was measured after 24 h incubation. Four replicates were made for each treatment and the values recorded are the mean average.


### 2.3. Preparation of the Complexes

The complexes were prepared by mixing clear solutions of the appropriate cephalosporin sodium salt (1 mmol) andNiCl2·6H2O metal salt: (1 mmol) in distilled water (10 cm3) and sulfathiazole (1 mmol) in EtOH (10 cm3). The reaction mixture was then stirred at room temperature for 4 h. and green precipitates formed. The precipitated complexes were filtered off, washed with water, MeOH and ether, and dried under reduced pressure at room temperature. Complexes were purified by recrystallization from dimethylsulfoxide/water mixture. The purity of the compounds was checked by TLC using silica gel-G as an adsorbent. Yields: 65–70%.


## 2.1. Physical Methods

All chemicals of reagent grade were commercially obtained from either Aldrich or Sigma and used without further purification. Solvents were redistilled by standard techniques before use. IR spectra were recorded as KBr pellets in the 4000–400 cm−1 range with a Perkin-Elmer Series 2000 FT-IR spectrophotometer. The electronic spectra of 1 × 10−3 M in DMSO solution of the ligand and its complex were recorded in the UV-Vis. region using a Shimadzu UV-240 spectrophotometer. The diffuse reflectance spectra of all the complexes in the 360–850 nm region were recorded on the same instrument equipped with a spherical reflectance assembly using BaSO4 as reference. C, H, N, and S were analyzed on a LECO CHNS 932 model microanalytical instrument. Nickel contents were estimated with a Perkin-Elmer atomic absorption spectrophotometer. The halogen content was determined by combustion of the solid complex (30 mg) in an oxygen flask in the presence of a KOH–H2O2 mixture. The halide content was then determined by titration with a standard Hg(NO3)2 solution using diphenyl carbazone as an indicator. Thermograms were recorded on a simultaneous thermal analyzer, STA-6000 (Perkin Elmer) instrument at a heating rate of 4°C min−1. Magnetic susceptibilities were measured on a Johnson Matthey Susceptibility Balance at 298 K. The effective magnetic moments were calculated from the expression μeff=2.828 (χMT)1/2 B.M., where χM is the molar susceptibility corrected using Pascal’s constants for diamagnetism of all atoms in the compounds. ESR spectra of the copper complexes were recorded on a JEOL microwave unit, JES-FE2XG Spectrophotometer. The magnetic field was calibrated with 2,2-diphenyl-1-picrylhydrazyl.


## 2.2. Antibacterial Activity Tests

Antibacterial activities of cephalosporins and their complexes were tested using the paper disc diffusion method [17]. The chosen strains were G(+) Staphylococcus aureus ATCC 25923 and G(−) Escherichia coli ATCC 11775, Pseudomonas aeruginosa ATCC 27853, Klebsiella pneumoniae ATCC 23357, Salmonella enteritidis CDC 64, and Bacillus subtilis ATCC 6051. The liquid medium containing the bacterial subcultures was autoclaved for 20 min at 121°C before inoculation. The bacteria were then cultured for 24 h at 36°C in an incubator. Muller Hinton broth was used for preparing basal media for the bioassay of the organisms. Nutrient agar was poured onto a plate and allowed to solidify. The test compounds in DMSO solutions (5 × 10−2 M) were added dropwise (10 μL) to a 5 mm diameter filter paper disc placed at the centre of each agar plate. The plates were then kept at 5°C for 1 h then transferred to an incubator maintained at 36°C. The width of the growth inhibition zone around the disc was measured after 24 h incubation. Four replicates were made for each treatment and the values recorded are the mean average.


## 2.3. Preparation of the Complexes

The complexes were prepared by mixing clear solutions of the appropriate cephalosporin sodium salt (1 mmol) andNiCl2·6H2O metal salt: (1 mmol) in distilled water (10 cm3) and sulfathiazole (1 mmol) in EtOH (10 cm3). The reaction mixture was then stirred at room temperature for 4 h. and green precipitates formed. The precipitated complexes were filtered off, washed with water, MeOH and ether, and dried under reduced pressure at room temperature. Complexes were purified by recrystallization from dimethylsulfoxide/water mixture. The purity of the compounds was checked by TLC using silica gel-G as an adsorbent. Yields: 65–70%.


## 3. Results and Discussion

The results of elemental analyses (C, H, N, S, Cl, and Ni content) are in good agreement with those calculated for the molecular formula of the prepared complexes (Table1). All the complexes are green colored, air, and moisture stable amorphous solids, which decompose without melting. They are almost insoluble in water and other common organic solvents such as MeOH, EtOH, benzene, hexane, acetone, chloroform, acetonitrile, and ether but soluble in DMSO. The insolubility of the complexes suggests that they are polymeric compounds [18].Table 1
Elemental analyses for the nickel(II) complexes.
CompoundFound (Calcd.) %CNHSClNi[Ni(L1)(stz)(H2O)]35.519.52.320.17.2[Ni(C23H24N11O7S5)](35.2)(19.6)(3.1)(20.4)(7.5)[Ni(L2)(stz)]40.19.73.017.58.1[Ni(C25H28N5O10S4)](40.3)(9.4)(3.8)(17.2)(7.9)[Ni(L3)(stz)]39.514.23.317.17.5[Ni(C25H25N8O9S4](39.1)(14.6)(3.3)(16.7)(7.6)[Ni(L4)(stz)(H2O)]37.317.72.818.16.4[Ni(C27H25N11O9S5)](37.4)(17.8)(2.9)(18.5)(6.8)[Ni(L5)(stz)]Cl40.815.03.715.84.77.3[Ni(C28H34N9O7S4)]Cl(40.5)(15.2)(4.1)(15.4)(4.3)(7.1)Thermograms of the hydrated metal complexes, [Ni(L1)(stz)(H2O)] and [Ni(L4)(stz)(H2O)], indicate endothermic decompositions in the 150–180°C range due to the loss of one molecule of coordinated water with a found mass loss of 2.46 and 2.34% (calcd. 2.29 and 2.08%), respectively [18, 19]. Thermal analysis for the cefepime complex [Ni(L5)(stz)]Cl displays two stages of weight loss. The first decomposition process that occurs at about 387°C could be assigned to the loss of one chlorine atom with a found mass loss of 4.62% (calcd. 4.27%). It can be seen that the complex began to decompose exothermically at ca. 420°C, and the decomposition was completed at ca. 520°C leaving out NiO as a residue with a found mass loss of 9,52% (calcd. 8.99%).Molar conductance values measured in DMSO at room temperature (10−3 M solution) indicated that the complexes have lower values (13–17 Ω-1 cm−2 mol−1) indicating their nonelectrolyte nature of these chelates [20] and that the sulfathiazole anion is coordinated to the metal. The only exception was [Ni(L5)(stz)]Cl, which showed higher value (38 Ω-1 cm−2 mol−1) acting as 1 : 1 electrolyte in this solvent indicating the ionic nature of this chelate. According to elemental analysis, there is one chlorine atom for each nickel ion. The complex is slightly soluble in water. In order to decide whether the chlorine was bounded ionically or covalently, a small amount of a complex sample was dispersed in distilled hot water and filtered. AgNO3 testing of the filtrates gave a precipitate of AgCl. This qualitative chlorine test implies that in [Ni(L5)(stz)]Cl complex, chlorine is bounded to the metal ionically. Hence, complexation gives a cationic complex with accompanying chloride ion in the form of counter anion.


### 3.1. Infrared Spectra

The IR spectra of cephalosporins and their complexes are similar, and the main features are recorded in Table2. Generally the ring carbonyl absorption frequency will be shifted to higher wavenumbers as the ring becomes more strained. The cephalosporins showed a strong absorption at 1730–1780 cm−1 lactam (C=O) stretching. This band shifted to lower frequency in the metal complexes. The amide (C=O) band is unshifted in the complexes compared to the free ligands (Figure 2). Given the significant shifts in the lactam C=O bands in the complexes, we suggest that coordination of the cephalosporin ligands occurs through the oxygen atom from the lactam rather than the amide carbonyl groups.Table 2
IR spectral data of the drugs and the complexes (cm−1).
νC=OνC=OνCOOνCOOΔννC=NνNi–NCompoundLactamAmideAsymm.SymmCefazolin1765165016001380220[Ni(L1)(stz)(H2O)]1749165015801370210425Cephalothin1730165016201400220[Ni(L2)(stz)]1715165016101390220430Cefotaxime17801640160013752251610[Ni(L3)(stz)]17501640159013702201605426Ceftriaxone17741667161014002101610[Ni(L4)(stz)(H2O)]17551661160013852151610430Cefepime17701650160013902101600[Ni(L5)(stz)]Cl17401650159013802101590415Figure 2
Infrared spectra of cephalothin (A) and [Ni(L2)(stz)] (B) in the solid state. Stretching CO lactam (a), stretching CO amide (b), asymmetric COO stretching (c), and symmetric COO stretching (d).The band at 1600–1620 cm−1 corresponding to the carboxylate asymmetrical stretching of the free ligands is shifted (10–20 cm−1) to lower wavenumbers in the spectra of the complexes, indicating coordination through that group. The remaining carboxylate band, namely, νsym(COO), formerly at around 1400 cm−1, also changes as a result of coordination. A carboxylate ligand can bind to the metal atom either as a monodentate or a bidentate ligand, giving changes in the relative positions of the asymmetric and symmetric stretching vibrations [21, 22]. The IR spectra of the complexes give a separation value of >200 cm−1 suggesting monodentate bonding for the carboxylate group.The presence ofν(Ni–N) stretching vibrations in the 410–430 cm−1 range for the complexes (absent in the free ligands) provides evidence that the sulfathiazole and cephalosporin moieties are bonded to the metal through the nitrogen atoms. Evidence of the N-thiazole interaction arises from the red shifts of the band assigned in the free sulfa drug to the thiazole ring vibrations (from 1550 cm−1 in the sulfathiazole to 1500 cm−1 in the complex) together with a marked intensity reduction. The bands at 3320 and 3280 cm−1, assigned to the νas(N–H) and νs(N–H) vibrations, respectively, of the NH2 group are slightly shifted in the cefotaxime, ceftriaxone, and cefepime nickel(II) complexes.The coordination of the tetrazole or-NH2 groups to the metal are not the only explanation of these absorption bands; alternatively, the N atom of the CONH and C=N–OCH3 groups (when corresponding) could coordinate to the metal; however, steric constraints would probably prevent coordination of these N atoms along with the COO and lactam CO groups. Furthermore, the C=N stretching vibration of the C=N–OCH3 residue, observed in free cefotaxime, ceftriaxone, and cefepime at 1600–1610 cm−1, either does not shift or shows a slight shift in all complexes, indicating that these groups are not involved in coordination. The usual modes of Hstz ligand are also present. As expected, the bands at 1310, 1150, and 560 cm−1 attributed to an O=S=O remain unchanged with respect to those of the ligand.


### 3.2. Magnetic Measurements

From the molar magnetic susceptibility values, corrected magnetic moments were calculated using Pascal’s constants. The cefazolin and ceftriaxone nickel(II) complexes have magnetic moment values in the 3.02–3.12 BM range, which are expected for systems with two unpaired electrons with no metal-metal interactions. They are within the range 2.9–3.3 consistent with their octahedral configuration around the Ni(II) ion. Nickel(II) (d8) ion, being a non-Krammer’s ion, EPR spectra, is observable, generally at low temperatures. However, there are very few reports in the literature about the study of this d8 ion at room temperature. The g value is isotropic and close to 2.2 [23–25]. EPR spectra of powdered samples of above-mentioned complexes were obtained at room temperature. They showed the same signals, a broad strong one at 3280 G with g = 2.14 and a linewidth of 200–430 G and a weak one at 2460 G with g = 2.85 and a linewidth of 110 G suggesting that the mentioned complexes have similar structure. There was no evidence of fine structure due to 61Ni nuclei (1.19% natural abundance, I = 3/2). On the other hand, the cephalothin, cefotaxime, and cefepime nickel(II) complexes have magnetic moments in the 3.6–3.8 BM range, which are higher than the values expected for octahedral geometry and consistent with the values expected for nickel(II) high spin pseudotetrahedral complexes [23].


### 3.3. Electronic Spectra

The UV-Vis spectra of the complexes in DMSO solutions present absorption maxima attributable to the ligands. A band at 250–270 nm is assigned toπ→π* transitions, while an intraligand band at 290–320 nm is related to the π→π* transitions within the heterocyclic moieties [26, 27]. The band in the 360–380 nm region is ascribed to an intraligand transition of the n→π* type in accordance with the literature data for transitions due to sulphur atoms [26, 28]. The fact that the bands due to sulphur atoms are not shifted suggests that this atom is not involved in coordination. A long-term UV-Vis study was carried out to verify the stability of new complexes in DMSO solution. Compared with ligands, it is significant to note that the absorption wavelengths of new complexes hardly varied for up to 1 month, meaning that new complexes were stable in DMSO solution.Different geometries of nickel(II) have quite different spectra in the visible and near-infrared portions of the spectrum. The absorptions in this region are due to d-d transitions and are quite weak compared to typical ultraviolet spectra. The electronic spectra of the complexes in solid state show almost similar features as in DMSO solution. The electronic spectra of [Ni(L1)(stz)(H2O)] and [Ni(L4)(stz)(H2O)] showed d-d bands in the region 10,417–10,526, 15,500–16,010 and 24,100–25,000 cm−1, assigned to 3A2g(F) → 3T2g(F) (ν1), 3A2g(F) → 3T1g(F) (ν2) and 3A2g(F) → 3T1g(P) (ν3) transitions, respectively. The calculated molar absorptivities of these absorptions are typically less than 10. The values of magnetic moments (3.02 and 3.12 B.M.), the spin-orbit coupling constants (λ = −175 and −267 cm−1), and the calculated ligand field parameters of Dq = 1,042 and 1,053 cm−1, B = 557 and 629 cm−1, and β = 0.53 and 0.60 indicating covalent complexes are also consistent with the octahedral geometry. The bands observed at ca. 12,500 cm−1 can be assigned to spin forbidden transitions to singlet levels originated by 1D and 1G splitting.Tetrahedral nickel(II) typically has a similar spectrum but shifted to lower energies. The electronic spectra of the light green nickel(II) complexes [Ni(L2)(stz)], [Ni(L3)(stz)], and [Ni(L5)(stz)]Cl are consistent with tetrahedral geometry showing one band at about 13,900–14,000 cm−1 assignable to 3T1(F) →3T1(P) (ν3) transition and a band at 22,222 cm−1 assignable to charge-transfer [28, 29]. The calculated molar absorptivities are of about 100.


### 3.4. Coordination Sites

In our case, the antibiotics have several potential donor atoms that might be involved in coordination with the nickel ions forming polymers. The assumption that the coordination of cephalothin, cefotaxime, and cefepime occurs through the carboxylate, lactam carbonyl group, and aminothiazolyl moiety (or S—thiophene group in the cephalothin ligand) seems likely that they behave as tridentate ligands. The multidentate chelation would require some kind of polymeric structure in which the ligand bridges different metal centres, since these atoms would be incapable of chelating a single metal due to geometric constraints. For instance, it is feasible that the nickel ions in the [Ni(L5)(stz)]+ cation complex containing coordinated stz anion are four-coordinate. Although, it would not be appropriate to predict precisely the structure of these complexes, a structure may tentatively be proposed. Figure 3 shows a suggested structure of [Ni(cefepime)(stz)]+ cation complex.Figure 3
Suggested structure of [Ni(L5)(stz)]+ cation complex.On the other hand, the coordination of cefazolin and ceftriaxone may occur through the carboxylate, lactam carbonyl, and two N-heterocyclic moieties; thus it is possible that they behave as monoanionic tetradentate ligands [13, 15]. It has been reported that deprotonated sulfathiazole, stz, coordinates through the N-thiazole moiety [7–10]. 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.


### 3.5. Microbiological Screening

Preliminary screening for antimicrobial activities of the stock solutions of the ligand and metal complexes was performed qualitatively using the disc diffusion assay.In vitro antimicrobial activities were measured from the diameter of clear inhibition zones caused by samples against the same bacteria and under the identical experimental conditions. As assessed by colour, the complexes remain intact during biological testing. In order to clarify role of In order to clarify role of DMSO, sulfathiazole and nickel(II) chloride salt in the biological screening, separate studies were carried out with the solutions alone of DMSO, sulfathiazole, and the free metal salt, and they showed no significant activity against any bacterial strains. The antibacterial activities of the complexes were better than those of both the Hstz and the starting metal salt. These provided reasons to believe that antibacterial activities of the complexes synthesized do not correlate with the toxicity of them against the bacterial tested.The results are shown in Table3, where it can be appreciated that except cefepime complex in most cases the antimicrobial activity of complexes was similar or less than the activity of pure antibiotics. The cefazolin [Ni(L1)(stz)H2O] complex showed lower bactericidal activity than the free ligand against all tested bacteria. The complexed cefotaxime [Ni(L3)(stz)] showed better activity against Salmonella enteritidis and Bacillus subtilis than the uncomplexed cefotaxime, while ceftriaxone and cephalothin complexes showed better activity against Escherichia coli and Staphylococcus aureus than the free antibiotics, respectively.Table 3
Antibacterial activity of the drugs and the complexes.
CompoundZone of inhibition (mm)E.C.S.E.P.A.S.AK.P.B.S.Cefazolin33.0±1.536.0±1.00.0±0.034.0±1.535.0±0.557.0±2.0[Ni(L1)(stz)(H2O)]20.0±2.518.0±0.00.0±0.027.0±1.023.0±1.037.0±1.0Cephalothin19.0±0.529.0±1.00.0±0.025.0±1.033.0±1.560.0±0.5[Ni(L2)(stz)]10.0±0.021.0±0.50.0±0.027.0±0.520.0±1.033.0±1.0Cefotaxime40.0±1.534.0±0.023.0±1.018.0±2.039.0±0.535.0±1.0[Ni(L3)(stz)]31.0±1.037.0±0.517.0±0.013.0±0.524.0±0.537.0±0.5Ceftriaxone33.0±0.538.0±1.035.0±2.025.0±1.040.0±1.043.0±0.5[Ni(L4)(stz)(H2O)]35.0±1.032.0±0.022.0±0.515.0±0.528.0±1.035.0±1.5Cefepime13.0±2.025.0±1.50.0±0.00.0±0.025.0±2.030.0±1.0[Ni(L5)(stz)]Cl30.0±1.533.0±0.519.0±1.015.0±1.028.0±0.035.0±0.5Sulfathiazole8.0±1.07.0±0.57.0±0.56.0±0.07.0±1.08.0±1.5E.C.,Escherichia coli ATCC 35939; S.E., Salmonella enteritidis ATCC 497; P.A., Pseudomonas aeruginosa ATCC 10145; S.A., Staphylococcus aureus ATCC 25923; K.P., Klebsiella pneumoniaATCC 10031; B.S., Bacillus subtilis ATCC 6051. Values are the mean ± Standard deviation of the mean.The cefepime adduct, at difference of all the others, shows better antibacterial activity than that of the free ligand against all tested bacteria. The cefepime [Ni(L5)(stz)]Cl complex is only electrolyte that showed better activity than free cefepime against all bacteria strains, including against P. aeruginosa and S. aureus where cefepime is inactive. The cefepime complex activity could be slightly higher because of the different structure of cefepime compared to other cephalosporins tested (it has a zwitterionic structure possessing the pyrrolidinium ring). Antibacterial activity of mixed-ligand nickel ion complexes depends mainly on the type of cephalosporin used, the metal ion, and the type of microorganism.It is known that chelation tends to make the ligand to act as more powerful and potent bacterial agent [29–35]. However, when using β-lactam ligands, the complexation significantly reduces the antimicrobial activity of the ligands. Considering that metal coordination generally involves the β-lactam C=O, a significant increase in the lability of the β-lactam ring could be anticipated; however, as sometimes happens the antimicrobial activity of β-lactam complexes is higher. The results in Table 3 can be understood considering that the enzyme probably serves primarily to hold catalytic groups or the substrate in the proper positions and is possible to expect that metal complexes of β-lactam antibiotics may change the stereochemistry required in solvolytic reactions on an enzyme surface. The results may highlight that the activity of the compounds is most probably related to their conformational adaptability, depending on the size and nature of the metal complexes and the geometrical constraints induced by intramolecular H bonds. Thus, the activity of β-lactam complexes compared to β-lactams (Table 3) may reflect a different mechanistic pathway by which the various metal complexes and the β-lactams react with the PBP active sites to achieve formation of a stable PBP-inhibitor adduct. The level of resistance to β-lactam complexes is determined by the amount, nature, and kinetic properties of the PBPs.


## 3.1. Infrared Spectra

The IR spectra of cephalosporins and their complexes are similar, and the main features are recorded in Table2. Generally the ring carbonyl absorption frequency will be shifted to higher wavenumbers as the ring becomes more strained. The cephalosporins showed a strong absorption at 1730–1780 cm−1 lactam (C=O) stretching. This band shifted to lower frequency in the metal complexes. The amide (C=O) band is unshifted in the complexes compared to the free ligands (Figure 2). Given the significant shifts in the lactam C=O bands in the complexes, we suggest that coordination of the cephalosporin ligands occurs through the oxygen atom from the lactam rather than the amide carbonyl groups.Table 2
IR spectral data of the drugs and the complexes (cm−1).
νC=OνC=OνCOOνCOOΔννC=NνNi–NCompoundLactamAmideAsymm.SymmCefazolin1765165016001380220[Ni(L1)(stz)(H2O)]1749165015801370210425Cephalothin1730165016201400220[Ni(L2)(stz)]1715165016101390220430Cefotaxime17801640160013752251610[Ni(L3)(stz)]17501640159013702201605426Ceftriaxone17741667161014002101610[Ni(L4)(stz)(H2O)]17551661160013852151610430Cefepime17701650160013902101600[Ni(L5)(stz)]Cl17401650159013802101590415Figure 2
Infrared spectra of cephalothin (A) and [Ni(L2)(stz)] (B) in the solid state. Stretching CO lactam (a), stretching CO amide (b), asymmetric COO stretching (c), and symmetric COO stretching (d).The band at 1600–1620 cm−1 corresponding to the carboxylate asymmetrical stretching of the free ligands is shifted (10–20 cm−1) to lower wavenumbers in the spectra of the complexes, indicating coordination through that group. The remaining carboxylate band, namely, νsym(COO), formerly at around 1400 cm−1, also changes as a result of coordination. A carboxylate ligand can bind to the metal atom either as a monodentate or a bidentate ligand, giving changes in the relative positions of the asymmetric and symmetric stretching vibrations [21, 22]. The IR spectra of the complexes give a separation value of >200 cm−1 suggesting monodentate bonding for the carboxylate group.The presence ofν(Ni–N) stretching vibrations in the 410–430 cm−1 range for the complexes (absent in the free ligands) provides evidence that the sulfathiazole and cephalosporin moieties are bonded to the metal through the nitrogen atoms. Evidence of the N-thiazole interaction arises from the red shifts of the band assigned in the free sulfa drug to the thiazole ring vibrations (from 1550 cm−1 in the sulfathiazole to 1500 cm−1 in the complex) together with a marked intensity reduction. The bands at 3320 and 3280 cm−1, assigned to the νas(N–H) and νs(N–H) vibrations, respectively, of the NH2 group are slightly shifted in the cefotaxime, ceftriaxone, and cefepime nickel(II) complexes.The coordination of the tetrazole or-NH2 groups to the metal are not the only explanation of these absorption bands; alternatively, the N atom of the CONH and C=N–OCH3 groups (when corresponding) could coordinate to the metal; however, steric constraints would probably prevent coordination of these N atoms along with the COO and lactam CO groups. Furthermore, the C=N stretching vibration of the C=N–OCH3 residue, observed in free cefotaxime, ceftriaxone, and cefepime at 1600–1610 cm−1, either does not shift or shows a slight shift in all complexes, indicating that these groups are not involved in coordination. The usual modes of Hstz ligand are also present. As expected, the bands at 1310, 1150, and 560 cm−1 attributed to an O=S=O remain unchanged with respect to those of the ligand.


## 3.2. Magnetic Measurements

From the molar magnetic susceptibility values, corrected magnetic moments were calculated using Pascal’s constants. The cefazolin and ceftriaxone nickel(II) complexes have magnetic moment values in the 3.02–3.12 BM range, which are expected for systems with two unpaired electrons with no metal-metal interactions. They are within the range 2.9–3.3 consistent with their octahedral configuration around the Ni(II) ion. Nickel(II) (d8) ion, being a non-Krammer’s ion, EPR spectra, is observable, generally at low temperatures. However, there are very few reports in the literature about the study of this d8 ion at room temperature. The g value is isotropic and close to 2.2 [23–25]. EPR spectra of powdered samples of above-mentioned complexes were obtained at room temperature. They showed the same signals, a broad strong one at 3280 G with g = 2.14 and a linewidth of 200–430 G and a weak one at 2460 G with g = 2.85 and a linewidth of 110 G suggesting that the mentioned complexes have similar structure. There was no evidence of fine structure due to 61Ni nuclei (1.19% natural abundance, I = 3/2). On the other hand, the cephalothin, cefotaxime, and cefepime nickel(II) complexes have magnetic moments in the 3.6–3.8 BM range, which are higher than the values expected for octahedral geometry and consistent with the values expected for nickel(II) high spin pseudotetrahedral complexes [23].


## 3.3. Electronic Spectra

The UV-Vis spectra of the complexes in DMSO solutions present absorption maxima attributable to the ligands. A band at 250–270 nm is assigned toπ→π* transitions, while an intraligand band at 290–320 nm is related to the π→π* transitions within the heterocyclic moieties [26, 27]. The band in the 360–380 nm region is ascribed to an intraligand transition of the n→π* type in accordance with the literature data for transitions due to sulphur atoms [26, 28]. The fact that the bands due to sulphur atoms are not shifted suggests that this atom is not involved in coordination. A long-term UV-Vis study was carried out to verify the stability of new complexes in DMSO solution. Compared with ligands, it is significant to note that the absorption wavelengths of new complexes hardly varied for up to 1 month, meaning that new complexes were stable in DMSO solution.Different geometries of nickel(II) have quite different spectra in the visible and near-infrared portions of the spectrum. The absorptions in this region are due to d-d transitions and are quite weak compared to typical ultraviolet spectra. The electronic spectra of the complexes in solid state show almost similar features as in DMSO solution. The electronic spectra of [Ni(L1)(stz)(H2O)] and [Ni(L4)(stz)(H2O)] showed d-d bands in the region 10,417–10,526, 15,500–16,010 and 24,100–25,000 cm−1, assigned to 3A2g(F) → 3T2g(F) (ν1), 3A2g(F) → 3T1g(F) (ν2) and 3A2g(F) → 3T1g(P) (ν3) transitions, respectively. The calculated molar absorptivities of these absorptions are typically less than 10. The values of magnetic moments (3.02 and 3.12 B.M.), the spin-orbit coupling constants (λ = −175 and −267 cm−1), and the calculated ligand field parameters of Dq = 1,042 and 1,053 cm−1, B = 557 and 629 cm−1, and β = 0.53 and 0.60 indicating covalent complexes are also consistent with the octahedral geometry. The bands observed at ca. 12,500 cm−1 can be assigned to spin forbidden transitions to singlet levels originated by 1D and 1G splitting.Tetrahedral nickel(II) typically has a similar spectrum but shifted to lower energies. The electronic spectra of the light green nickel(II) complexes [Ni(L2)(stz)], [Ni(L3)(stz)], and [Ni(L5)(stz)]Cl are consistent with tetrahedral geometry showing one band at about 13,900–14,000 cm−1 assignable to 3T1(F) →3T1(P) (ν3) transition and a band at 22,222 cm−1 assignable to charge-transfer [28, 29]. The calculated molar absorptivities are of about 100.


## 3.4. Coordination Sites

In our case, the antibiotics have several potential donor atoms that might be involved in coordination with the nickel ions forming polymers. The assumption that the coordination of cephalothin, cefotaxime, and cefepime occurs through the carboxylate, lactam carbonyl group, and aminothiazolyl moiety (or S—thiophene group in the cephalothin ligand) seems likely that they behave as tridentate ligands. The multidentate chelation would require some kind of polymeric structure in which the ligand bridges different metal centres, since these atoms would be incapable of chelating a single metal due to geometric constraints. For instance, it is feasible that the nickel ions in the [Ni(L5)(stz)]+ cation complex containing coordinated stz anion are four-coordinate. Although, it would not be appropriate to predict precisely the structure of these complexes, a structure may tentatively be proposed. Figure 3 shows a suggested structure of [Ni(cefepime)(stz)]+ cation complex.Figure 3
Suggested structure of [Ni(L5)(stz)]+ cation complex.On the other hand, the coordination of cefazolin and ceftriaxone may occur through the carboxylate, lactam carbonyl, and two N-heterocyclic moieties; thus it is possible that they behave as monoanionic tetradentate ligands [13, 15]. It has been reported that deprotonated sulfathiazole, stz, coordinates through the N-thiazole moiety [7–10]. 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.


## 3.5. Microbiological Screening

Preliminary screening for antimicrobial activities of the stock solutions of the ligand and metal complexes was performed qualitatively using the disc diffusion assay.In vitro antimicrobial activities were measured from the diameter of clear inhibition zones caused by samples against the same bacteria and under the identical experimental conditions. As assessed by colour, the complexes remain intact during biological testing. In order to clarify role of In order to clarify role of DMSO, sulfathiazole and nickel(II) chloride salt in the biological screening, separate studies were carried out with the solutions alone of DMSO, sulfathiazole, and the free metal salt, and they showed no significant activity against any bacterial strains. The antibacterial activities of the complexes were better than those of both the Hstz and the starting metal salt. These provided reasons to believe that antibacterial activities of the complexes synthesized do not correlate with the toxicity of them against the bacterial tested.The results are shown in Table3, where it can be appreciated that except cefepime complex in most cases the antimicrobial activity of complexes was similar or less than the activity of pure antibiotics. The cefazolin [Ni(L1)(stz)H2O] complex showed lower bactericidal activity than the free ligand against all tested bacteria. The complexed cefotaxime [Ni(L3)(stz)] showed better activity against Salmonella enteritidis and Bacillus subtilis than the uncomplexed cefotaxime, while ceftriaxone and cephalothin complexes showed better activity against Escherichia coli and Staphylococcus aureus than the free antibiotics, respectively.Table 3
Antibacterial activity of the drugs and the complexes.
CompoundZone of inhibition (mm)E.C.S.E.P.A.S.AK.P.B.S.Cefazolin33.0±1.536.0±1.00.0±0.034.0±1.535.0±0.557.0±2.0[Ni(L1)(stz)(H2O)]20.0±2.518.0±0.00.0±0.027.0±1.023.0±1.037.0±1.0Cephalothin19.0±0.529.0±1.00.0±0.025.0±1.033.0±1.560.0±0.5[Ni(L2)(stz)]10.0±0.021.0±0.50.0±0.027.0±0.520.0±1.033.0±1.0Cefotaxime40.0±1.534.0±0.023.0±1.018.0±2.039.0±0.535.0±1.0[Ni(L3)(stz)]31.0±1.037.0±0.517.0±0.013.0±0.524.0±0.537.0±0.5Ceftriaxone33.0±0.538.0±1.035.0±2.025.0±1.040.0±1.043.0±0.5[Ni(L4)(stz)(H2O)]35.0±1.032.0±0.022.0±0.515.0±0.528.0±1.035.0±1.5Cefepime13.0±2.025.0±1.50.0±0.00.0±0.025.0±2.030.0±1.0[Ni(L5)(stz)]Cl30.0±1.533.0±0.519.0±1.015.0±1.028.0±0.035.0±0.5Sulfathiazole8.0±1.07.0±0.57.0±0.56.0±0.07.0±1.08.0±1.5E.C.,Escherichia coli ATCC 35939; S.E., Salmonella enteritidis ATCC 497; P.A., Pseudomonas aeruginosa ATCC 10145; S.A., Staphylococcus aureus ATCC 25923; K.P., Klebsiella pneumoniaATCC 10031; B.S., Bacillus subtilis ATCC 6051. Values are the mean ± Standard deviation of the mean.The cefepime adduct, at difference of all the others, shows better antibacterial activity than that of the free ligand against all tested bacteria. The cefepime [Ni(L5)(stz)]Cl complex is only electrolyte that showed better activity than free cefepime against all bacteria strains, including against P. aeruginosa and S. aureus where cefepime is inactive. The cefepime complex activity could be slightly higher because of the different structure of cefepime compared to other cephalosporins tested (it has a zwitterionic structure possessing the pyrrolidinium ring). Antibacterial activity of mixed-ligand nickel ion complexes depends mainly on the type of cephalosporin used, the metal ion, and the type of microorganism.It is known that chelation tends to make the ligand to act as more powerful and potent bacterial agent [29–35]. However, when using β-lactam ligands, the complexation significantly reduces the antimicrobial activity of the ligands. Considering that metal coordination generally involves the β-lactam C=O, a significant increase in the lability of the β-lactam ring could be anticipated; however, as sometimes happens the antimicrobial activity of β-lactam complexes is higher. The results in Table 3 can be understood considering that the enzyme probably serves primarily to hold catalytic groups or the substrate in the proper positions and is possible to expect that metal complexes of β-lactam antibiotics may change the stereochemistry required in solvolytic reactions on an enzyme surface. The results may highlight that the activity of the compounds is most probably related to their conformational adaptability, depending on the size and nature of the metal complexes and the geometrical constraints induced by intramolecular H bonds. Thus, the activity of β-lactam complexes compared to β-lactams (Table 3) may reflect a different mechanistic pathway by which the various metal complexes and the β-lactams react with the PBP active sites to achieve formation of a stable PBP-inhibitor adduct. The level of resistance to β-lactam complexes is determined by the amount, nature, and kinetic properties of the PBPs.



---

*Source: 106187-2012-05-09.xml*