# Thermal, Spectral, Fluorescence, and Antimicrobial Studies of Cobalt, Nickel, Copper, and Zinc Complexes Derived from 4-[(5-Bromo-thiophen-2-ylmethylene)-amino]-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine

Authors: Kiran Singh; Yogender Kumar; Parvesh Puri; Chetan Sharma; Kamal Rai Aneja
Journal: International Journal of Inorganic Chemistry
 (2012)

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## Abstract

A new series of cobalt, nickel, copper, and zinc complexes of bidentate Schiff base derived from the condensation of 5-bromothiophene-2-carboxaldehyde with 4-amino-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine were synthesized. Physical (magnetic measurements, molar conductance, TG), spectral (UV-Vis, IR,1HNMR, fluorescence, ESR), and analytical data have established the structures of synthesized Schiff base and its metal complexes. The presence of coordinated water in metal complexes was confirmed by IR and TG studies. The Schiff base exhibits a strong fluorescence emission, contrast to this partial fluorescence quenching phenomena is observed in its metal complexes. A square planar geometry for Cu(II) and octahedral geometry for Co(II), Ni(II) and Zn(II) complexes have been proposed. The Schiff base and its metal complexes have been screened for antibacterial (Staphylococcus aureus, Bacillus subtilis, Escherichia coli, Pseudomonas aeruginosa) and antifungal activities (Aspergillus niger, A. flavus).


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## Body

## 1. Introduction

Triazine chemistry has attracted attention due to the utility of melamine derivatives as starting material for a variety of polymers [1], as scavenging resins in organic manipulations [2] and in medicinal chemistry [3]. They provide a wide range of applications in the field of optics [4], herbicides [5], and pharmaceuticals [6]. These are valuable bases for estrogen receptor modulators and are also used as bridging agents to synthesize herbicides and in the production of drugs or polymers [7, 8]. Many derivatives of 1,2,4-triazine form colored complexes with different metal ions and can be used as analytical reagent for their determination [9]. A range of polymer-supported triazines and their metal-bound analogues were screened for use in catalysis and organic synthesis [10, 11]. Goodman et al. reported that triazine-derived copper complexes have superoxide radical scavenging activity in pathological processes [12]. In our last publication, we have reported that Schiff base derived from 4-amino-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine shows antibacterial and antifungal activity and enhanced antimicrobial activity is observed, when the Schiff base is combined to transition metal ions [13].Encouraged by above-mentioned finding, we found it is to investigate the thermal, spectral, fluorescence, and antimicrobial studies of cobalt, nickel, copper, and zinc complexes derived from 4-[(5-bromo-thiophen-2-ylmethylene)-amino]-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine.


## 2. Experimental

### 2.1. Materials

All the chemicals used in the present study were of analytical grade and used without further purification. 4-Amino-3-mercapto-6-methyl-5-oxo-1,2,4-triazine [14] was prepared by reported literature method.


### 2.2. Syntheses

#### 2.2.1.4-[(5-Bromo-thiophen-2-ylmethylene)-amino]-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine [HL]

A solution of 4-amino-3-mercapto-6-methyl-5-oxo-1,2,4-triazine (2.12 g, 13.5 mmol) in ethanol (40 mL) was treated with 5-bromothiophene-2-carboxaldehyde   (2.69 g, 13.5 mmol). The reaction mixture was refluxed for 7 h and kept overnight at room temperature. The bluish white-colored solid crude so obtained was filtered off and washed with cold ethanol, dried, and recrystallized in ethanol.Bluish white; yield (76%); m.p. 234–236°C; anal. calcd. for C9H7BrN4OS2: C, 32.64; H, 2.13; N, 16.92; found: C, 32.42; H, 2.08; N, 16.92%.


#### 2.2.2. Metal Complexes of HL (1 : 1)

The solid complexes were prepared by mixing hot ethanolic solutions of theHL  (0.18 g, 0.54 mmol) with aqueous ethanolic solution of acetates of Co(II) (0.14 g, 0.54 mmol), Ni(II) (0.14 g, 0.54 mmol), Cu(II) (0.11 g, 0.54 mmol), and Zn(II) (0.12 g, 0.54 mmol), which resulted in the immediate precipitation of metal complexes. The solid complexes were filtered off, washed thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone, and vacuo dried.Co(L)OAc·3H2O: anal. calcd. for C11H15BrCoN4O6S2: C, 26.31; H, 3.01; N, 11.16; Co, 11.73; found: C, 26.13; H, 2.85; N, 11.12; Co, 11.30%.Ni(L)OAc·3H2O: anal. calcd. for C11H15BrN4NiO6S2: C, 26.32; H, 3.01; N, 11.16; Ni, 11.69; found: C, 26.10; H, 3.00; N, 11.03; Ni, 11.22%.Cu(L)OAc·H2O: anal. calcd. for C11H11BrCuN4O4S2: C, 28.06; H, 2.35; N, 11.90; Cu, 13.50; found: C, 28.00; H, 2.15; N, 11.82; Cu, 13.10%.Zn(L)OAc·3H2O: anal. calcd. for C11H15BrN4O6S2Zn: C, 25.97; H, 2.97; N, 11.01; Zn, 12.85; found: C, 25.65; H, 2.97; N, 11.01; Zn, 12.87%.


#### 2.2.3. Metal Complexes of HL (1 : 2)

The aqueous ethanolic solutions of acetates of Co(II) (0.17 g, 0.68 mmol), Ni(II) (0.17 g, 0.68 mmol), Cu(II) (0.14 g, 0.68 mmol), and Zn(II) (0.15 g, 0.68 mmol) were treated with the hot ethanolic solutions of the HL (0.45 g, 1.3 mmol). The products formed were filtered and purified by washing thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone and dried.Co(L)2·2H2O: anal. calcd. for C18H16Br2CoN8O4S4: C, 28.62; H, 2.13; N, 14.83; Co, 7.80; found: C, 28.18; H, 2.01; N, 14.83; Co, 7.53%.Ni(L)2·2H2O: anal. calcd. for C18H16Br2N8NiO4S4: C, 28.63; H, 2.14; N, 14.84; Ni, 7.77; found: C, 28.63; H, 2.12; N, 14.80; Ni, 7.72%.Cu(L)2: anal. calcd. for C18H12Br2CuN8O2S4: C, 29.86; H, 1.67; N, 15.48; Cu, 8.78; found: C, 29.85; H, 1.65; N, 15.80; Cu, 8.38%.Zn(L)2·2H2O: anal. calcd. for C18H16Br2N8O4S4Zn: C, 28.38; H, 2.12; N, 14.71; Zn, 8.58; found: C, 28.37; H, 2.10; N, 14.53; Zn, 8.23%.


### 2.3. Analyses and Instrumentation

The elemental analyses (C, H, and N) were carried out at SAIF, Punjab University, Chandigarh, by using Perkin-Elmer 2400 Elemental Analyzer. The metal contents were determined gravimetrically by a literature procedure [15] after digesting the organic matter with aqua regia and evaporating the residue to dryness. IR spectra of neat samples of the ligand and its metal complexes were performed in the range 4000–250 cm−1 on a MB-3000 ABB Spectrometer. The electronic spectra of solid complexes were recorded on T 90 (PG Instruments ltd) UV/Vis spectrometer in the region 1100–200 nm. 1H NMR spectra were recorded in DMSO-d6 on a Bruker ACF 300 spectrometer at 300 MHz using tetramethylsilane as the internal standard. Magnetic moments were measured at Institute Instrumentation Centre, IIT Roorkee, on vibrating sample magnetometer (Model 155). The Perkin Elmer (Pyris Diamond) instrument was used to carry out thermal analysis of metal complex in atmospheric air (50–800°C) at a heating rate of 10°C Min−1 using a reference to alumina powder. The fluorescence studies of Schiff base and its metal complexes were recorded on SHIMADZU RF-5301PC spectrophotometer. The solutions of 10−3M concentration were prepared in HPLC grade DMF and the experiment was carried out at room temperature. ESR spectra were recorded on X-Band at frequency of 9.1 GHz under the magnetic field 3000 Guass on a Varian E-112 ESR spectrometer at SAIF IIT Bombay.


### 2.4. Pharmacology

#### 2.4.1. Antibacterial Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antibacterial activity against two Gram-positive (Staphylococcus aureusMTCC 96, Bacillus subtilisMTCC 121) and two Gram-negative (Escherichia coliMTCC 1652, Pseudomonas aeruginosaMTCC 741) bacterial strains by agar well-diffusion method as reported in our previous paper [13]. DMSO was used as a negative control whereas ciprofloxacin was used as positive control. All the bacterial cultures were procured from Microbial Type Culture Collection (MTCC), IMTECH, Chandigarh, and subcultured on nutrient agar.


#### 2.4.2. Antifungal Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antifungal activity against two fungi, Aspergillus nigerandA. flavus, the ear pathogens isolated from the patients of Kurukshetra [16] and evaluated by poisoned food technique [13]. The molds were grown on Sabouraud dextrose agar (SDA) at 25°C for 7 days and used as inocula. DMSO was used as the negative control whereas fluconazole was used as the positive control. The experiments were performed in triplicates. Diameters of fungal colonies were measured and expressed as percent mycelial inhibition. 										(1)Percentinhibitionofmycelialgrowth=(dc-dt)/dc×100,
where dc average diameter of fungal colony in negative control sets and dt average diameter fungal colony in experimental sets.


#### 2.4.3. Determination of Minimum Inhibitory Concentration (MIC)

MIC is the lowest concentration of an antimicrobial compound that will inhibit the visible growth of a microorganism after overnight incubation.MIC of the various compounds against bacterial strains was tested through a modified agar well-diffusion method [17]. In this method, a twofold serial dilution of each synthesized compound was prepared by first reconstituting the compound in DMSO followed by dilution in sterile distilled water to achieve a decreasing concentration range 512 to 1 μg mL−1. A 100 μL volume of each dilution was introduced into wells (in triplicate) in the agar plates already seeded with 100 μL of standardized inoculum (106 cfu mL−1) of the test microbial strain. All test plates were incubated aerobically at 37°C for 24 h and observed for the inhibition zones. Ciprofloxacin was used as positive control.


## 2.1. Materials

All the chemicals used in the present study were of analytical grade and used without further purification. 4-Amino-3-mercapto-6-methyl-5-oxo-1,2,4-triazine [14] was prepared by reported literature method.


## 2.2. Syntheses

### 2.2.1.4-[(5-Bromo-thiophen-2-ylmethylene)-amino]-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine [HL]

A solution of 4-amino-3-mercapto-6-methyl-5-oxo-1,2,4-triazine (2.12 g, 13.5 mmol) in ethanol (40 mL) was treated with 5-bromothiophene-2-carboxaldehyde   (2.69 g, 13.5 mmol). The reaction mixture was refluxed for 7 h and kept overnight at room temperature. The bluish white-colored solid crude so obtained was filtered off and washed with cold ethanol, dried, and recrystallized in ethanol.Bluish white; yield (76%); m.p. 234–236°C; anal. calcd. for C9H7BrN4OS2: C, 32.64; H, 2.13; N, 16.92; found: C, 32.42; H, 2.08; N, 16.92%.


### 2.2.2. Metal Complexes of HL (1 : 1)

The solid complexes were prepared by mixing hot ethanolic solutions of theHL  (0.18 g, 0.54 mmol) with aqueous ethanolic solution of acetates of Co(II) (0.14 g, 0.54 mmol), Ni(II) (0.14 g, 0.54 mmol), Cu(II) (0.11 g, 0.54 mmol), and Zn(II) (0.12 g, 0.54 mmol), which resulted in the immediate precipitation of metal complexes. The solid complexes were filtered off, washed thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone, and vacuo dried.Co(L)OAc·3H2O: anal. calcd. for C11H15BrCoN4O6S2: C, 26.31; H, 3.01; N, 11.16; Co, 11.73; found: C, 26.13; H, 2.85; N, 11.12; Co, 11.30%.Ni(L)OAc·3H2O: anal. calcd. for C11H15BrN4NiO6S2: C, 26.32; H, 3.01; N, 11.16; Ni, 11.69; found: C, 26.10; H, 3.00; N, 11.03; Ni, 11.22%.Cu(L)OAc·H2O: anal. calcd. for C11H11BrCuN4O4S2: C, 28.06; H, 2.35; N, 11.90; Cu, 13.50; found: C, 28.00; H, 2.15; N, 11.82; Cu, 13.10%.Zn(L)OAc·3H2O: anal. calcd. for C11H15BrN4O6S2Zn: C, 25.97; H, 2.97; N, 11.01; Zn, 12.85; found: C, 25.65; H, 2.97; N, 11.01; Zn, 12.87%.


### 2.2.3. Metal Complexes of HL (1 : 2)

The aqueous ethanolic solutions of acetates of Co(II) (0.17 g, 0.68 mmol), Ni(II) (0.17 g, 0.68 mmol), Cu(II) (0.14 g, 0.68 mmol), and Zn(II) (0.15 g, 0.68 mmol) were treated with the hot ethanolic solutions of the HL (0.45 g, 1.3 mmol). The products formed were filtered and purified by washing thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone and dried.Co(L)2·2H2O: anal. calcd. for C18H16Br2CoN8O4S4: C, 28.62; H, 2.13; N, 14.83; Co, 7.80; found: C, 28.18; H, 2.01; N, 14.83; Co, 7.53%.Ni(L)2·2H2O: anal. calcd. for C18H16Br2N8NiO4S4: C, 28.63; H, 2.14; N, 14.84; Ni, 7.77; found: C, 28.63; H, 2.12; N, 14.80; Ni, 7.72%.Cu(L)2: anal. calcd. for C18H12Br2CuN8O2S4: C, 29.86; H, 1.67; N, 15.48; Cu, 8.78; found: C, 29.85; H, 1.65; N, 15.80; Cu, 8.38%.Zn(L)2·2H2O: anal. calcd. for C18H16Br2N8O4S4Zn: C, 28.38; H, 2.12; N, 14.71; Zn, 8.58; found: C, 28.37; H, 2.10; N, 14.53; Zn, 8.23%.


## 2.2.1.4-[(5-Bromo-thiophen-2-ylmethylene)-amino]-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine [HL]

A solution of 4-amino-3-mercapto-6-methyl-5-oxo-1,2,4-triazine (2.12 g, 13.5 mmol) in ethanol (40 mL) was treated with 5-bromothiophene-2-carboxaldehyde   (2.69 g, 13.5 mmol). The reaction mixture was refluxed for 7 h and kept overnight at room temperature. The bluish white-colored solid crude so obtained was filtered off and washed with cold ethanol, dried, and recrystallized in ethanol.Bluish white; yield (76%); m.p. 234–236°C; anal. calcd. for C9H7BrN4OS2: C, 32.64; H, 2.13; N, 16.92; found: C, 32.42; H, 2.08; N, 16.92%.


## 2.2.2. Metal Complexes of HL (1 : 1)

The solid complexes were prepared by mixing hot ethanolic solutions of theHL  (0.18 g, 0.54 mmol) with aqueous ethanolic solution of acetates of Co(II) (0.14 g, 0.54 mmol), Ni(II) (0.14 g, 0.54 mmol), Cu(II) (0.11 g, 0.54 mmol), and Zn(II) (0.12 g, 0.54 mmol), which resulted in the immediate precipitation of metal complexes. The solid complexes were filtered off, washed thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone, and vacuo dried.Co(L)OAc·3H2O: anal. calcd. for C11H15BrCoN4O6S2: C, 26.31; H, 3.01; N, 11.16; Co, 11.73; found: C, 26.13; H, 2.85; N, 11.12; Co, 11.30%.Ni(L)OAc·3H2O: anal. calcd. for C11H15BrN4NiO6S2: C, 26.32; H, 3.01; N, 11.16; Ni, 11.69; found: C, 26.10; H, 3.00; N, 11.03; Ni, 11.22%.Cu(L)OAc·H2O: anal. calcd. for C11H11BrCuN4O4S2: C, 28.06; H, 2.35; N, 11.90; Cu, 13.50; found: C, 28.00; H, 2.15; N, 11.82; Cu, 13.10%.Zn(L)OAc·3H2O: anal. calcd. for C11H15BrN4O6S2Zn: C, 25.97; H, 2.97; N, 11.01; Zn, 12.85; found: C, 25.65; H, 2.97; N, 11.01; Zn, 12.87%.


## 2.2.3. Metal Complexes of HL (1 : 2)

The aqueous ethanolic solutions of acetates of Co(II) (0.17 g, 0.68 mmol), Ni(II) (0.17 g, 0.68 mmol), Cu(II) (0.14 g, 0.68 mmol), and Zn(II) (0.15 g, 0.68 mmol) were treated with the hot ethanolic solutions of the HL (0.45 g, 1.3 mmol). The products formed were filtered and purified by washing thoroughly with warm water, with aqueous ethanol to remove unreacted metal acetates or ligands, and finally with acetone and dried.Co(L)2·2H2O: anal. calcd. for C18H16Br2CoN8O4S4: C, 28.62; H, 2.13; N, 14.83; Co, 7.80; found: C, 28.18; H, 2.01; N, 14.83; Co, 7.53%.Ni(L)2·2H2O: anal. calcd. for C18H16Br2N8NiO4S4: C, 28.63; H, 2.14; N, 14.84; Ni, 7.77; found: C, 28.63; H, 2.12; N, 14.80; Ni, 7.72%.Cu(L)2: anal. calcd. for C18H12Br2CuN8O2S4: C, 29.86; H, 1.67; N, 15.48; Cu, 8.78; found: C, 29.85; H, 1.65; N, 15.80; Cu, 8.38%.Zn(L)2·2H2O: anal. calcd. for C18H16Br2N8O4S4Zn: C, 28.38; H, 2.12; N, 14.71; Zn, 8.58; found: C, 28.37; H, 2.10; N, 14.53; Zn, 8.23%.


## 2.3. Analyses and Instrumentation

The elemental analyses (C, H, and N) were carried out at SAIF, Punjab University, Chandigarh, by using Perkin-Elmer 2400 Elemental Analyzer. The metal contents were determined gravimetrically by a literature procedure [15] after digesting the organic matter with aqua regia and evaporating the residue to dryness. IR spectra of neat samples of the ligand and its metal complexes were performed in the range 4000–250 cm−1 on a MB-3000 ABB Spectrometer. The electronic spectra of solid complexes were recorded on T 90 (PG Instruments ltd) UV/Vis spectrometer in the region 1100–200 nm. 1H NMR spectra were recorded in DMSO-d6 on a Bruker ACF 300 spectrometer at 300 MHz using tetramethylsilane as the internal standard. Magnetic moments were measured at Institute Instrumentation Centre, IIT Roorkee, on vibrating sample magnetometer (Model 155). The Perkin Elmer (Pyris Diamond) instrument was used to carry out thermal analysis of metal complex in atmospheric air (50–800°C) at a heating rate of 10°C Min−1 using a reference to alumina powder. The fluorescence studies of Schiff base and its metal complexes were recorded on SHIMADZU RF-5301PC spectrophotometer. The solutions of 10−3M concentration were prepared in HPLC grade DMF and the experiment was carried out at room temperature. ESR spectra were recorded on X-Band at frequency of 9.1 GHz under the magnetic field 3000 Guass on a Varian E-112 ESR spectrometer at SAIF IIT Bombay.


## 2.4. Pharmacology

### 2.4.1. Antibacterial Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antibacterial activity against two Gram-positive (Staphylococcus aureusMTCC 96, Bacillus subtilisMTCC 121) and two Gram-negative (Escherichia coliMTCC 1652, Pseudomonas aeruginosaMTCC 741) bacterial strains by agar well-diffusion method as reported in our previous paper [13]. DMSO was used as a negative control whereas ciprofloxacin was used as positive control. All the bacterial cultures were procured from Microbial Type Culture Collection (MTCC), IMTECH, Chandigarh, and subcultured on nutrient agar.


### 2.4.2. Antifungal Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antifungal activity against two fungi, Aspergillus nigerandA. flavus, the ear pathogens isolated from the patients of Kurukshetra [16] and evaluated by poisoned food technique [13]. The molds were grown on Sabouraud dextrose agar (SDA) at 25°C for 7 days and used as inocula. DMSO was used as the negative control whereas fluconazole was used as the positive control. The experiments were performed in triplicates. Diameters of fungal colonies were measured and expressed as percent mycelial inhibition. 										(1)Percentinhibitionofmycelialgrowth=(dc-dt)/dc×100,
where dc average diameter of fungal colony in negative control sets and dt average diameter fungal colony in experimental sets.


### 2.4.3. Determination of Minimum Inhibitory Concentration (MIC)

MIC is the lowest concentration of an antimicrobial compound that will inhibit the visible growth of a microorganism after overnight incubation.MIC of the various compounds against bacterial strains was tested through a modified agar well-diffusion method [17]. In this method, a twofold serial dilution of each synthesized compound was prepared by first reconstituting the compound in DMSO followed by dilution in sterile distilled water to achieve a decreasing concentration range 512 to 1 μg mL−1. A 100 μL volume of each dilution was introduced into wells (in triplicate) in the agar plates already seeded with 100 μL of standardized inoculum (106 cfu mL−1) of the test microbial strain. All test plates were incubated aerobically at 37°C for 24 h and observed for the inhibition zones. Ciprofloxacin was used as positive control.


## 2.4.1. Antibacterial Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antibacterial activity against two Gram-positive (Staphylococcus aureusMTCC 96, Bacillus subtilisMTCC 121) and two Gram-negative (Escherichia coliMTCC 1652, Pseudomonas aeruginosaMTCC 741) bacterial strains by agar well-diffusion method as reported in our previous paper [13]. DMSO was used as a negative control whereas ciprofloxacin was used as positive control. All the bacterial cultures were procured from Microbial Type Culture Collection (MTCC), IMTECH, Chandigarh, and subcultured on nutrient agar.


## 2.4.2. Antifungal Activity (In Vitro)

The newly synthesized Schiff base (HL) and its metal complexes were screenedin vitro for their antifungal activity against two fungi, Aspergillus nigerandA. flavus, the ear pathogens isolated from the patients of Kurukshetra [16] and evaluated by poisoned food technique [13]. The molds were grown on Sabouraud dextrose agar (SDA) at 25°C for 7 days and used as inocula. DMSO was used as the negative control whereas fluconazole was used as the positive control. The experiments were performed in triplicates. Diameters of fungal colonies were measured and expressed as percent mycelial inhibition. 										(1)Percentinhibitionofmycelialgrowth=(dc-dt)/dc×100,
where dc average diameter of fungal colony in negative control sets and dt average diameter fungal colony in experimental sets.


## 2.4.3. Determination of Minimum Inhibitory Concentration (MIC)

MIC is the lowest concentration of an antimicrobial compound that will inhibit the visible growth of a microorganism after overnight incubation.MIC of the various compounds against bacterial strains was tested through a modified agar well-diffusion method [17]. In this method, a twofold serial dilution of each synthesized compound was prepared by first reconstituting the compound in DMSO followed by dilution in sterile distilled water to achieve a decreasing concentration range 512 to 1 μg mL−1. A 100 μL volume of each dilution was introduced into wells (in triplicate) in the agar plates already seeded with 100 μL of standardized inoculum (106 cfu mL−1) of the test microbial strain. All test plates were incubated aerobically at 37°C for 24 h and observed for the inhibition zones. Ciprofloxacin was used as positive control.


## 3. Results and Discussion

The synthesis of Schiff base (HL) is schematically represented in Figure1. Elemental analyses indicated the formation of 1 : 1 and 1 : 2 metal complexes of HL with Co(II), Ni(II), Cu(II), and Zn(II) metal ions. All the complexes are dark green, brown to dark brown in color and nonhygroscopic in nature. The molar conductance values of the complexes (measured in 10-3M DMF) are in the range 8.1–10.3 ohm-1cm2 mol−1 indicating the nonelectrolytic nature [18, 19]. The low conductivity values are in agreement with low solubility of metal complexes in water, ethanol, chloroform, acetone, and most organic solvents. On the other hand, they are soluble in DMSO and DMF and decomposed at higher temperature. The purity of ligands and their metal complexes has been checked by TLC.Figure 1
Scheme for the synthesis of Schiff base.


### 3.1. IR Spectra

The comparative analysis of the IR spectra of the complexes and of the free ligand (Table1) revealed that the absorption band characteristic of the stretching vibrations of -C=N- (azomethine group) is shifted towards lower wave number from 1599 cm−1 in the spectrum of the ligand to 1575–1589 cm−1 in the complexes [19, 20]. This indicates the coordination of the nitrogen of this group with the metal ions. Further coordination of metal to azomethine nitrogen is confirmed by a new band at 488–498 cm−1 due to ν(M–N). The ν(C=O) stretching frequency of the ligand at 1690 cm−1 is not altered in almost all of the complexes, indicating that the oxygen of C=O is not involved in bonding with metal ion [13]. A characteristic strong band at 2476 cm−1 is ascribed to ν(SH), which disappeared in the spectra of metal complexes, confirming deprotonation and coordination of thiol group [13, 19]. This is further supported by the lower frequency band appeared at 733–756 cm−1 in the metal complexes due to ν(C–S). The new band in the region of 371–382 cm−1 in the metal complexes is assigned to vibrations of ν(M–S) bond [21, 22]. The broad band around 3305 cm−1, corresponding to ν(O–H) indicates the presence of coordinated water molecules. In addition, a strong band around 1745 cm−1 has been assigned to ν(OOCCH3) in 1 : 1 metal complexes. Further, the absorptions corresponding to asymmetric and symmetric stretching of the acetate groups at ~1617 and 1420 cm−1, respectively confirms the monodentate nature of the acetate ion in complexes [23, 24].Table 1
IR spectral data of the ligand and its metal complexes.
Compound
ν(C=O)
ν(N=CH)
ν(C–S)
ν(S–H)
ν(OOCCH3)
ν(H2O/OH)
ν(M–S)
ν(M–N)
HL
1690
1599
—
2476
—
—
—
—
Co(L)(OAc)·3H2O
1685
1582
748
—
1744
3310
376
498
Co(L)2·2H2O
1688
1575
750
—
—
3318
378
493
Ni(L)(OAc)·3H2O
1686
1587
756
—
1744
3298
382
488
Ni(L)2·2H2O
1686
1589
756
—
—
3298
381
488
Cu(L)(OAc)·H2O
1687
1582
748
—
1745
3307
371
490
Cu(L)2
1686
1583
752
—
—
—
373
495
Zn(L)(OAc)·3H2O
1689
1580
737
—
1743
3313
372
492
Zn(L)2·2H2O
1690
1582
733
—
—
3315
373
490


### 3.2.1H NMR Spectra

In the1H-NMR spectra (Table 2), the signal of the azomethine proton is shifted from 8.52 ppm in the spectrum of the ligand to 8.80 and 8.73 ppm, in the spectra of 1 : 1 and 1 : 2 metal complexes, respectively. This shows that the most probable binding of the ligand with the metal ion is realized through the nitrogen atom of the azomethine group [13, 17]. The peak corresponding to −SH at 10.30 ppm in the free ligand is not observed in the spectra of the metal complexes. This clearly shows deprotonation of −SH during complex formation. In the spectrum of the ligand, signals due to aromatic protons appeared as two doublets at δ 7.16 and 7.33 ppm. These resonance signals remain almost unaltered in the spectra of the complexes. The methyl group protons of triazine appeared as singlet at δ 2.35 ppm in the spectrum of ligand and slightly shielded in the spectra of metal complexes. In the spectra of 1 : 1 Zn complex singlet at δ 1.85 is due to methyl group of acetate ion [20].Table 2
1H NMR spectral data of Schiff base and Zn(II) metal complexes.
Compound
1H NMR (ppm)
HL  [C9H7BrN4OS2]
CDCl3, 2.35 (s, 3H, –CH3), 7.16 (d, 1H, Ar–H), 7.33 (d, 1H, Ar–H),  8.52 (s, 1H, –N=CH–), 10.30 (s, 1H, –SH)
Zn(L)(OAc)·3H2O [C11H15BrN4O6S2Zn]
DMSO d6, 2.18 (s, 3H, –CH3), 7.22 (d, 1H, Ar–H), 7.38 (d, 1H, Ar–H),  8.80 (s, 1H, –N=CH–), 1.85 (s, 3H, CH3COO)
Zn(L)2·2H2O [C18H16Br2N8O4S4Zn]
DMSO d6, 2.20 (s, 6H, –CH3), 7.38 (d, 2H, Ar–H), 7.59 (d, 2H, Ar–H),  8.73 (s, 2H, –N=CH–)


### 3.3. Electronic and Magnetic Moments Measurements

In order to obtain further structural information, the electronic spectra and magnetic moments of the complexes have been measured (Table3). At room temperature Co(II) complexes show magnetic moments 4.13 and 4.20 BM, indicating three unpaired electrons. The electronic spectra of Co(II) complexes exhibit absorption in the region 11560–12004, and 22258–22779 cm−1. These bands may be assigned to T1g4(F)→4T2g(F) (ν1) and 4T1g(F)→4T1g(P) (ν3) transitions respectively. The position of these bands is consistent with octahedral geometry around the Co(II) ion [25]. With these values the ligand field parameters (Dq), the Racah parameter (B) and nephelauxetic ratio (β) have been calculated [26]. The value of B, which is lower than the free ion value of 971 cm−1, indicates overlapping of ligand-metal orbitals.Table 3
Electronic spectra, magnetic data, and ligand field parameters of metal complexes.
Compound
Transitions (cm-1)
Dq cm-1
B cm-1
ν
2/ν1
β
β%
μ
eff (BM)
ν
1
ν
2
ν
3
Co(L)(OAc)·3H2O
12004
25348*
22779
1334.4
807.6
2.11
0.831
16.9
4.13
Co(L)2·2H2O
11560
24431*
22258
1287.1
800.6
2.11
0.824
17.6
4.20
Ni(L)(OAc)·3H2O
11261
16200
26115
1126.1
568.8
1.43
0.546
45.4
3.78
Ni(L)2·2H2O
11376
16345
26238
1137.6
563.6
1.43
0.541
45.9
3.76
Cu(L)(OAc)·H2O
20123
—
—
—
—
—
1.75
Cu(L)2
19998
—
—
—
—
—
1.75
*Calculated value.The Ni(II) complexes reported herein are found to have room temperature magnetic moment values 3.78 and 3.76 BM, corresponding to two unpaired electrons. The electronic spectra of Ni(II) complexes display three absorption bands in the range 11261–11376, 16200–16345, and 26115–26238 cm−1. These bands may be assigned to three spin allowed transitions  3A2g(F)→3T2g(F) (ν1), 3A2g(F)→3T1g(F) (ν2), and 3A2g(F)→3T1g(P) (ν3), respectively. The position of these bands indicates that the complexes have an octahedral geometry around the Ni(II) complexes [13, 19, 27–31]. The ligand field parameters (Dq, B, β, β%) have also been calculated (Table 3) for Ni(II) complexes by using band-fitting equation [26]. These parameters indicated significant covalent character of the metal-ligand bonds and an overlapping of ligand-metal orbitals. At room temperature Cu(II) complexes show magnetic moments 1.75 BM corresponding to one unpaired electron. The electronic spectra of Cu(II) complexes showed absorption band in the region 19998–20123 cm−1 attributed to 2B1g→2A1g transition indicative of square planar geometry [20, 22].


### 3.4. Photoluminescence Emission Spectra

The photoluminescence emission spectra of the Schiff base (HL) and its 1 : 2 metal complexes are recorded in DMF at room temperature (Figure2). HL exhibits a strong fluorescence emission at 376 nm with excitation at 265 nm. In contrast with fluorescence spectra of HL, partial fluorescence quenching phenomena are observed in its metal complexes with weak fluorescence emission at 389, 379, 381, and 374 nm for Co(II), Ni(II), Cu(II), and Zn(II) complexes, respectively with excitation at 265 nm. The fluorescence spectra results revealed that fluorescence emission intensity of Schiff bases decreased dramatically on complex formation with transition metal ions. The reason for the weak fluorescence intensity with formation of metal complexes is due to decrease in electron density on Schiff base [32, 33]. The decrease in emission maxima was in the order of HL > Zn(II) > Co(II) > Cu(II) > Ni(II).Figure 2
Fluorescence emission spectra of Schiff base and its metal complexes.


### 3.5. Electron Paramagnetic Resonance Spectra

ESR spectra (Figure3) of copper complexes in powder form at LNT were recorded in the X band using 9.1 GHz field modulation with g factor quoted relative to the standard marker TCNE (g=2.0027). The ESR spectra of Cu(II) complexes show typical axial behavior with slightly different g|| and g⊥ values. From the observed g values for Cu(L)(OAc)·H2O at room temperature (g||=2.11, g⊥=2.04, gav=2.06, G=2.84) and for Cu(L)2 at room temperature (g||=2.14, g⊥=2.06, gav=2.08, G=2.37), it is evident that unpaired electron is localized in the dx2-y2 orbital and corresponds to square planar geometry of the complexes. The g||<2.3 value confirms the covalent character of the metal ligand bond. The axial symmetry parameter G is less than 4.0 and indicates considerable exchange interaction in the solid complex [32, 34]. No signal at half field was observed in the spectrum, ruling out the possibility of a dimeric form [35].Figure 3
X-band ESR spectra of Cu(L)(OAc)·H2O.


### 3.6. Thermal Studies

Thermal studies of Zn(L)2·2H2O and Ni(L)2·2H2O (Figure 4) indicate that the complexes decompose in three major steps from 50 to 800°C. The TG curves gives information on the thermal stability and the product formed on heating [21, 22, 36]. The TG curve of Zn(L)2·2H2O consists mainly of three steps in the temperature range 50–198, 198–430, and 430–800°C. The first step seems to be consistent with the evolution of two water molecules (calcd. 4.75%, found 4.54%). The second TG step represents a mass loss (calcd. 45.9%, found 45.7%) corresponding to expulsion of organic moiety (C10H6Br2S2). The final steps corresponds to decomposition of triazine molecules at 430–800°C with mass loss of 40.8% (calcd. 40.9) of the ligand leaving zinc oxide as residue.Figure 4
Thermogravimetric curves of Zn(L)2·2H2O and Ni(L)2·2H2O.TGA studies of Ni(L)2·2H2O indicated first weight loss (4.3%) in the range of 50–235°C, attributed to the loss of two water molecules (calcd. 4.8%). The second weight loss of 49.9% (calcd. 50.0%) from 235–300°C corresponds to loss of organic moiety (C10H6Br2N2S2). In the last step of decomposition triazine moiety comes out in the range 300–800°C with mass loss of 37.1% (Calcd. 37.5%). The final residual weight is 9.1% (calcd. 9.8%) corresponding to NiO.


### 3.7. Antimicrobial Discussion

The ligand (HL), metal complexes, standard drugs, and DMSO solvent were screened separately for their antibacterial activity against Gram-positive (Staphylococcus aureus, Bacillus subtilis) and Gram-negative (Escherichia coli, Pseudomonas aeruginosa) bacteria and antifungal activity against Aspergillus niger and Aspergillus flavus.The microbial results are summarized in Tables 4, 5, and 6. The antimicrobial studies suggested that the Schiff bases are biologically active and their metal complexes showed significantly enhanced antibacterial and antifungal activity against microbial strains in comparison to the free ligands. Positive controls (standard drug) produced significantly sized inhibition zones against the tested bacteria and fungi; however, negative control (DMSO) produced no observable inhibitory effect against any of the test organisms.Table 4
Antibacterial activity of synthesized compounds through agar well diffusion method.
Compound
Diameter of growth of inhibition zone (mm)a
Staphylococcus  aureus
Bacillus  subtilis
Escherichia  coli
Pseudomonas  aeruginosa
HL
16.3
18.3
—
—
Co(L)(OAc)·3H2O
18.3
18.3
—
—
Co(L)2·2H2O
16.3
19.6
—
—
Ni(L)(OAc)·3H2O
17.3
18.0
—
—
Ni(L)2·2H2O
17.3
19.6
—
—
Cu(L)(OAc)·H2O
16.3
18.3
—
—
Cu(L)2
20.6
22.6
—
—
Zn(L)(OAc)·3H2O
19.3
21.3
—
—
Zn(L)2·2H2O
17.3
19.6
—
—
Ciprofloxacin
26.6
24.0
25.0
22.0
—No activity.
aValues, including diameter of the well (8 mm), are means of three replicates.Table 5
Minimum inhibitory concentration (MIC) (μg/mL) of compounds.
Compound
Staphylococcus  aureus
Bacillus  subtilis
HL
128
64
Co(L)(OAc)·3H2O
128
64
Co(L)2·2H2O
128
64
Ni(L)(OAc)·3H2O
128
64
Ni(L)2·2H2O
128
64
Cu(L)(OAc)·H2O
128
64
Cu(L)2
64
32
Zn(L)(OAc)·3H2O
64
32
Zn(L)2·2H2O
128
64
Ciprofloxacin
6.25
6.25Table 6
Antifungal activity of Schiff base and metal complexes.
Compound
Mycelial growth inhibition (%)
Aspergillus  niger
Aspergillus  flavus
HL
45.2
46.6
Co(L)(OAc)·3H2O
47.7
51.1
Co(L)2·2H2O
48.8
52.2
Ni(L)(OAc)·3H2O
45.5
48.8
Ni(L)2·2H2O
43.3
46.6
Cu(L)(OAc)·H2O
45.5
48.8
Cu(L)2
58.8
63.3
Zn(L)(OAc)·3H2O
56.6
61.1
Zn(L)2·2H2O
51.1
56.6
Fluconazole
81.1
77.7Tested chemical compounds showed zone of inhibition ranging between 16 mm and 22 mm against the Gram-positive bacteria. On the basis of zone of inhibition produced against the test bacterium, Cu(L)2 was found to be most effective against B. subtilisand S. aureus, with zone of inhibition of 20.6 mm and 22.6 mm, respectively. However other tested compounds showed moderate antibacterial activity (Table 4). Tested chemical compounds did not exhibit any activity against Gram-negative (Escherichia coliand Pseudomonas aeruginosa) bacteria. In the whole series, the MIC of chemical compounds ranged between 32 and 128 μg/mL against Gram-positive bacteria. Two compounds Cu(L)2 and Zn(L)(OAc)·3H2O were found to be best as they exhibit the lowest MIC of 32 μg/mL against B. subtilisand 64 μg/mL againstS. aureus (Table 5). The results of our study are in accordance with the reports of earlier workers [13, 19, 21, 24], which also showed that the antibacterial activity of ligands is greatly enhanced when it is coordinated to metal ions. The Schiff base is found to show antifungal activity, and its metal complexes show enhanced activity as compared to the uncoordinated compound. Of the nine chemical compounds screened for their antifungal activity, three compounds Cu(L)2, Zn(L)(OAc)·3H2O, and Zn(L)2·2H2O showed more than 50% inhibition of mycelial growth against Aspergillus flavus whereas three compounds namely Cu(L)2, Zn(L)(OAc)·3H2O, and Zn(L)2·2H2O, showed more than 55% inhibition of mycelial growth against A. niger(Table 6). The overtone’s concept [37] and Tweedy’s chelation theory [38] can be used to explain the enhancement in antimicrobial activity of the metal complexes.


## 3.1. IR Spectra

The comparative analysis of the IR spectra of the complexes and of the free ligand (Table1) revealed that the absorption band characteristic of the stretching vibrations of -C=N- (azomethine group) is shifted towards lower wave number from 1599 cm−1 in the spectrum of the ligand to 1575–1589 cm−1 in the complexes [19, 20]. This indicates the coordination of the nitrogen of this group with the metal ions. Further coordination of metal to azomethine nitrogen is confirmed by a new band at 488–498 cm−1 due to ν(M–N). The ν(C=O) stretching frequency of the ligand at 1690 cm−1 is not altered in almost all of the complexes, indicating that the oxygen of C=O is not involved in bonding with metal ion [13]. A characteristic strong band at 2476 cm−1 is ascribed to ν(SH), which disappeared in the spectra of metal complexes, confirming deprotonation and coordination of thiol group [13, 19]. This is further supported by the lower frequency band appeared at 733–756 cm−1 in the metal complexes due to ν(C–S). The new band in the region of 371–382 cm−1 in the metal complexes is assigned to vibrations of ν(M–S) bond [21, 22]. The broad band around 3305 cm−1, corresponding to ν(O–H) indicates the presence of coordinated water molecules. In addition, a strong band around 1745 cm−1 has been assigned to ν(OOCCH3) in 1 : 1 metal complexes. Further, the absorptions corresponding to asymmetric and symmetric stretching of the acetate groups at ~1617 and 1420 cm−1, respectively confirms the monodentate nature of the acetate ion in complexes [23, 24].Table 1
IR spectral data of the ligand and its metal complexes.
Compound
ν(C=O)
ν(N=CH)
ν(C–S)
ν(S–H)
ν(OOCCH3)
ν(H2O/OH)
ν(M–S)
ν(M–N)
HL
1690
1599
—
2476
—
—
—
—
Co(L)(OAc)·3H2O
1685
1582
748
—
1744
3310
376
498
Co(L)2·2H2O
1688
1575
750
—
—
3318
378
493
Ni(L)(OAc)·3H2O
1686
1587
756
—
1744
3298
382
488
Ni(L)2·2H2O
1686
1589
756
—
—
3298
381
488
Cu(L)(OAc)·H2O
1687
1582
748
—
1745
3307
371
490
Cu(L)2
1686
1583
752
—
—
—
373
495
Zn(L)(OAc)·3H2O
1689
1580
737
—
1743
3313
372
492
Zn(L)2·2H2O
1690
1582
733
—
—
3315
373
490


## 3.2.1H NMR Spectra

In the1H-NMR spectra (Table 2), the signal of the azomethine proton is shifted from 8.52 ppm in the spectrum of the ligand to 8.80 and 8.73 ppm, in the spectra of 1 : 1 and 1 : 2 metal complexes, respectively. This shows that the most probable binding of the ligand with the metal ion is realized through the nitrogen atom of the azomethine group [13, 17]. The peak corresponding to −SH at 10.30 ppm in the free ligand is not observed in the spectra of the metal complexes. This clearly shows deprotonation of −SH during complex formation. In the spectrum of the ligand, signals due to aromatic protons appeared as two doublets at δ 7.16 and 7.33 ppm. These resonance signals remain almost unaltered in the spectra of the complexes. The methyl group protons of triazine appeared as singlet at δ 2.35 ppm in the spectrum of ligand and slightly shielded in the spectra of metal complexes. In the spectra of 1 : 1 Zn complex singlet at δ 1.85 is due to methyl group of acetate ion [20].Table 2
1H NMR spectral data of Schiff base and Zn(II) metal complexes.
Compound
1H NMR (ppm)
HL  [C9H7BrN4OS2]
CDCl3, 2.35 (s, 3H, –CH3), 7.16 (d, 1H, Ar–H), 7.33 (d, 1H, Ar–H),  8.52 (s, 1H, –N=CH–), 10.30 (s, 1H, –SH)
Zn(L)(OAc)·3H2O [C11H15BrN4O6S2Zn]
DMSO d6, 2.18 (s, 3H, –CH3), 7.22 (d, 1H, Ar–H), 7.38 (d, 1H, Ar–H),  8.80 (s, 1H, –N=CH–), 1.85 (s, 3H, CH3COO)
Zn(L)2·2H2O [C18H16Br2N8O4S4Zn]
DMSO d6, 2.20 (s, 6H, –CH3), 7.38 (d, 2H, Ar–H), 7.59 (d, 2H, Ar–H),  8.73 (s, 2H, –N=CH–)


## 3.3. Electronic and Magnetic Moments Measurements

In order to obtain further structural information, the electronic spectra and magnetic moments of the complexes have been measured (Table3). At room temperature Co(II) complexes show magnetic moments 4.13 and 4.20 BM, indicating three unpaired electrons. The electronic spectra of Co(II) complexes exhibit absorption in the region 11560–12004, and 22258–22779 cm−1. These bands may be assigned to T1g4(F)→4T2g(F) (ν1) and 4T1g(F)→4T1g(P) (ν3) transitions respectively. The position of these bands is consistent with octahedral geometry around the Co(II) ion [25]. With these values the ligand field parameters (Dq), the Racah parameter (B) and nephelauxetic ratio (β) have been calculated [26]. The value of B, which is lower than the free ion value of 971 cm−1, indicates overlapping of ligand-metal orbitals.Table 3
Electronic spectra, magnetic data, and ligand field parameters of metal complexes.
Compound
Transitions (cm-1)
Dq cm-1
B cm-1
ν
2/ν1
β
β%
μ
eff (BM)
ν
1
ν
2
ν
3
Co(L)(OAc)·3H2O
12004
25348*
22779
1334.4
807.6
2.11
0.831
16.9
4.13
Co(L)2·2H2O
11560
24431*
22258
1287.1
800.6
2.11
0.824
17.6
4.20
Ni(L)(OAc)·3H2O
11261
16200
26115
1126.1
568.8
1.43
0.546
45.4
3.78
Ni(L)2·2H2O
11376
16345
26238
1137.6
563.6
1.43
0.541
45.9
3.76
Cu(L)(OAc)·H2O
20123
—
—
—
—
—
1.75
Cu(L)2
19998
—
—
—
—
—
1.75
*Calculated value.The Ni(II) complexes reported herein are found to have room temperature magnetic moment values 3.78 and 3.76 BM, corresponding to two unpaired electrons. The electronic spectra of Ni(II) complexes display three absorption bands in the range 11261–11376, 16200–16345, and 26115–26238 cm−1. These bands may be assigned to three spin allowed transitions  3A2g(F)→3T2g(F) (ν1), 3A2g(F)→3T1g(F) (ν2), and 3A2g(F)→3T1g(P) (ν3), respectively. The position of these bands indicates that the complexes have an octahedral geometry around the Ni(II) complexes [13, 19, 27–31]. The ligand field parameters (Dq, B, β, β%) have also been calculated (Table 3) for Ni(II) complexes by using band-fitting equation [26]. These parameters indicated significant covalent character of the metal-ligand bonds and an overlapping of ligand-metal orbitals. At room temperature Cu(II) complexes show magnetic moments 1.75 BM corresponding to one unpaired electron. The electronic spectra of Cu(II) complexes showed absorption band in the region 19998–20123 cm−1 attributed to 2B1g→2A1g transition indicative of square planar geometry [20, 22].


## 3.4. Photoluminescence Emission Spectra

The photoluminescence emission spectra of the Schiff base (HL) and its 1 : 2 metal complexes are recorded in DMF at room temperature (Figure2). HL exhibits a strong fluorescence emission at 376 nm with excitation at 265 nm. In contrast with fluorescence spectra of HL, partial fluorescence quenching phenomena are observed in its metal complexes with weak fluorescence emission at 389, 379, 381, and 374 nm for Co(II), Ni(II), Cu(II), and Zn(II) complexes, respectively with excitation at 265 nm. The fluorescence spectra results revealed that fluorescence emission intensity of Schiff bases decreased dramatically on complex formation with transition metal ions. The reason for the weak fluorescence intensity with formation of metal complexes is due to decrease in electron density on Schiff base [32, 33]. The decrease in emission maxima was in the order of HL > Zn(II) > Co(II) > Cu(II) > Ni(II).Figure 2
Fluorescence emission spectra of Schiff base and its metal complexes.


## 3.5. Electron Paramagnetic Resonance Spectra

ESR spectra (Figure3) of copper complexes in powder form at LNT were recorded in the X band using 9.1 GHz field modulation with g factor quoted relative to the standard marker TCNE (g=2.0027). The ESR spectra of Cu(II) complexes show typical axial behavior with slightly different g|| and g⊥ values. From the observed g values for Cu(L)(OAc)·H2O at room temperature (g||=2.11, g⊥=2.04, gav=2.06, G=2.84) and for Cu(L)2 at room temperature (g||=2.14, g⊥=2.06, gav=2.08, G=2.37), it is evident that unpaired electron is localized in the dx2-y2 orbital and corresponds to square planar geometry of the complexes. The g||<2.3 value confirms the covalent character of the metal ligand bond. The axial symmetry parameter G is less than 4.0 and indicates considerable exchange interaction in the solid complex [32, 34]. No signal at half field was observed in the spectrum, ruling out the possibility of a dimeric form [35].Figure 3
X-band ESR spectra of Cu(L)(OAc)·H2O.


## 3.6. Thermal Studies

Thermal studies of Zn(L)2·2H2O and Ni(L)2·2H2O (Figure 4) indicate that the complexes decompose in three major steps from 50 to 800°C. The TG curves gives information on the thermal stability and the product formed on heating [21, 22, 36]. The TG curve of Zn(L)2·2H2O consists mainly of three steps in the temperature range 50–198, 198–430, and 430–800°C. The first step seems to be consistent with the evolution of two water molecules (calcd. 4.75%, found 4.54%). The second TG step represents a mass loss (calcd. 45.9%, found 45.7%) corresponding to expulsion of organic moiety (C10H6Br2S2). The final steps corresponds to decomposition of triazine molecules at 430–800°C with mass loss of 40.8% (calcd. 40.9) of the ligand leaving zinc oxide as residue.Figure 4
Thermogravimetric curves of Zn(L)2·2H2O and Ni(L)2·2H2O.TGA studies of Ni(L)2·2H2O indicated first weight loss (4.3%) in the range of 50–235°C, attributed to the loss of two water molecules (calcd. 4.8%). The second weight loss of 49.9% (calcd. 50.0%) from 235–300°C corresponds to loss of organic moiety (C10H6Br2N2S2). In the last step of decomposition triazine moiety comes out in the range 300–800°C with mass loss of 37.1% (Calcd. 37.5%). The final residual weight is 9.1% (calcd. 9.8%) corresponding to NiO.


## 3.7. Antimicrobial Discussion

The ligand (HL), metal complexes, standard drugs, and DMSO solvent were screened separately for their antibacterial activity against Gram-positive (Staphylococcus aureus, Bacillus subtilis) and Gram-negative (Escherichia coli, Pseudomonas aeruginosa) bacteria and antifungal activity against Aspergillus niger and Aspergillus flavus.The microbial results are summarized in Tables 4, 5, and 6. The antimicrobial studies suggested that the Schiff bases are biologically active and their metal complexes showed significantly enhanced antibacterial and antifungal activity against microbial strains in comparison to the free ligands. Positive controls (standard drug) produced significantly sized inhibition zones against the tested bacteria and fungi; however, negative control (DMSO) produced no observable inhibitory effect against any of the test organisms.Table 4
Antibacterial activity of synthesized compounds through agar well diffusion method.
Compound
Diameter of growth of inhibition zone (mm)a
Staphylococcus  aureus
Bacillus  subtilis
Escherichia  coli
Pseudomonas  aeruginosa
HL
16.3
18.3
—
—
Co(L)(OAc)·3H2O
18.3
18.3
—
—
Co(L)2·2H2O
16.3
19.6
—
—
Ni(L)(OAc)·3H2O
17.3
18.0
—
—
Ni(L)2·2H2O
17.3
19.6
—
—
Cu(L)(OAc)·H2O
16.3
18.3
—
—
Cu(L)2
20.6
22.6
—
—
Zn(L)(OAc)·3H2O
19.3
21.3
—
—
Zn(L)2·2H2O
17.3
19.6
—
—
Ciprofloxacin
26.6
24.0
25.0
22.0
—No activity.
aValues, including diameter of the well (8 mm), are means of three replicates.Table 5
Minimum inhibitory concentration (MIC) (μg/mL) of compounds.
Compound
Staphylococcus  aureus
Bacillus  subtilis
HL
128
64
Co(L)(OAc)·3H2O
128
64
Co(L)2·2H2O
128
64
Ni(L)(OAc)·3H2O
128
64
Ni(L)2·2H2O
128
64
Cu(L)(OAc)·H2O
128
64
Cu(L)2
64
32
Zn(L)(OAc)·3H2O
64
32
Zn(L)2·2H2O
128
64
Ciprofloxacin
6.25
6.25Table 6
Antifungal activity of Schiff base and metal complexes.
Compound
Mycelial growth inhibition (%)
Aspergillus  niger
Aspergillus  flavus
HL
45.2
46.6
Co(L)(OAc)·3H2O
47.7
51.1
Co(L)2·2H2O
48.8
52.2
Ni(L)(OAc)·3H2O
45.5
48.8
Ni(L)2·2H2O
43.3
46.6
Cu(L)(OAc)·H2O
45.5
48.8
Cu(L)2
58.8
63.3
Zn(L)(OAc)·3H2O
56.6
61.1
Zn(L)2·2H2O
51.1
56.6
Fluconazole
81.1
77.7Tested chemical compounds showed zone of inhibition ranging between 16 mm and 22 mm against the Gram-positive bacteria. On the basis of zone of inhibition produced against the test bacterium, Cu(L)2 was found to be most effective against B. subtilisand S. aureus, with zone of inhibition of 20.6 mm and 22.6 mm, respectively. However other tested compounds showed moderate antibacterial activity (Table 4). Tested chemical compounds did not exhibit any activity against Gram-negative (Escherichia coliand Pseudomonas aeruginosa) bacteria. In the whole series, the MIC of chemical compounds ranged between 32 and 128 μg/mL against Gram-positive bacteria. Two compounds Cu(L)2 and Zn(L)(OAc)·3H2O were found to be best as they exhibit the lowest MIC of 32 μg/mL against B. subtilisand 64 μg/mL againstS. aureus (Table 5). The results of our study are in accordance with the reports of earlier workers [13, 19, 21, 24], which also showed that the antibacterial activity of ligands is greatly enhanced when it is coordinated to metal ions. The Schiff base is found to show antifungal activity, and its metal complexes show enhanced activity as compared to the uncoordinated compound. Of the nine chemical compounds screened for their antifungal activity, three compounds Cu(L)2, Zn(L)(OAc)·3H2O, and Zn(L)2·2H2O showed more than 50% inhibition of mycelial growth against Aspergillus flavus whereas three compounds namely Cu(L)2, Zn(L)(OAc)·3H2O, and Zn(L)2·2H2O, showed more than 55% inhibition of mycelial growth against A. niger(Table 6). The overtone’s concept [37] and Tweedy’s chelation theory [38] can be used to explain the enhancement in antimicrobial activity of the metal complexes.


## 4. Conclusions

The present work describes the synthesis of cobalt, nickel, copper, and zinc complexes of bidentate Schiff base derived from the condensation reaction of 5-bromothiophene-2-carboxaldehyde with 4-amino-3-mercapto-6-methyl-5-oxo-[1,2,4]triazine. The physical (magnetic measurements, molar conductance, TG), spectral (UV-Vis, IR, 1HNMR, fluorescence, ESR), and analytical data for these complexes clearly suggest that the Schiff base is coordinated to metal ions through its azomethine nitrogen and sulphur. The presence of coordinated water in metal complexes was confirmed by IR and TG studies. The Schiff base exhibits a strong fluorescence emission contrast to this partial fluorescence quenching phenomena is observed in its metal complexes. The proposed structures of metal complexes are presented in Figure 5. The antimicrobial studies suggested that the Schiff bases were found to be biologically active and their metal complexes show significantly enhanced antibacterial and antifungal activity against microbial strains in comparison to the free ligands, thus, exhibiting their broad spectrum nature and can become a new antimicrobial agent, after further biological studies.Figure 5
Proposed structures of metal complexes.



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*Source: 873232-2012-08-02.xml*