# Synthesis, Characterization, and Biological Evaluation of Some 3d-Metal Complexes of Schiff Base Derived from Xipamide Drug

Authors: Suman Malik; Suparna Ghosh; Bharti Jain; Archana Singh; Mamta Bhattacharya
Journal: International Journal of Inorganic Chemistry
 (2013)

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## Abstract

The present paper deals with the synthesis and characterization of metal complexes of Schiff base derived from xipamide, a diuretic drug. The bidentate ligand is derived from the inserted condensation of 5-aminosulfonyl-4-chloro-N-2,6-dimethyl phenyl-2-hydroxybenzamide (Xipamide) with salicylaldehyde in a 1 : 1 molar ratio. Using this bidentate ligand, complexes of Hg(II), Zn(II), and VO(IV) with general formula ML2 have been synthesized. The synthesized complexes were characterized by several techniques using molar conductance, elemental analysis, magnetic susceptibility, FT-IR spectroscopy, electronic spectra, mass spectra, and particle size analysis. The elemental analysis data suggest the stoichiometry to be 1 : 2 [M : L]. All the complexes are nonelectrolytic in nature as suggested by molar conductance measurements. Infrared spectral data indicate the coordination between the ligand and the central metal ion through deprotonated phenolic oxygen and azomethine nitrogen atoms. Spectral studies suggest tetrahedral geometry for Hg(II), Zn(II) complexes, and square pyramidal geometry for VO(IV) complex. The pure drug, synthesized ligand, and metal complexes were screened for their antifungal activities against Aspergillus niger and Aspergillus flavus. The ligand and its Hg(II) and VO(IV) complexes were screened for their diuretic activity too.


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## Body

## 1. Introduction

Coordination complexes are gaining importance in recent years especially in the designing of long acting drugs in metabolism. The metal complexes from bidentate ligands have often been studied recently because of their technical applications [1, 2] and applications in enhancement of drug action [3, 4]. Transition metals are essential for normal functioning of living organism and are, therefore, of great interest as potential drugs [5]. The coordination chemistry of nitrogen donor ligands is an active area of research. A great deal of attention in this area has been focused on the complexes formed by 3d metals with bidentate ligands using both sulfur and nitrogen [6, 7]. The Schiff bases are an important class of ligands in coordination chemistry. The study of structural and binding features of various Schiff base complexes can play an important role in better understanding of the complex biological process. Schiff bases derived from salicylaldehyde are well known for their interesting ligational properties and exclusive applications in different fields [8–10]. It is well known from the literature that Schiff bases derived from thiazide drugs have a strong ability to form metal complexes [11]. The interaction of these donor ligands and metal ions gives complexes of different geometries, and literature survey reveals that these complexes are potentially more biologically active. Thus, in recent years Schiff bases and their metal complexes have attained much attraction because of their extensive biological activities [12, 13]. Keeping the above fact in our mind and in continuation of our earlier work on transition metal complexes with Schiff bases [14, 15], the ligand xipamide-salicylaldimine Schiff base (L) has been synthesized. In the present paper, the synthesis and characterization of the ligand and its complexes with Hg(II), Zn(II), and VO(IV) are being reported.


## 2. Experimental

All the chemicals used were of AR/GR grade and purchased from E-Merck (USA). Chemicals were used without any purification. Xipamide drug was provided by Dishman Pharmaceuticals which was used as such for the synthesis of ligand.Elemental analyses were carried out on model 240 PerkinElmer elemental analyzer at CDRI, Lucknow. Metal contents were determined gravimetrically using standard methods [16]. Conductivity measurements were made in anhydrous DMF on a Systronics model 305 (India) Conductivity Bridge. Magnetic susceptibility measurements of the complexes in the solid state were determined by vibrating sample magnetometer at Centre for Advance Technology, Indore at room temperature. The electronic spectra of the metal complexes in DMF were recorded on a Perkin-Elmer UV WinLab Spectrophotometer at School of Studies in Chemistry and Biochemistry, Vikram University, Ujjain, India. The infrared spectra of the ligand and complexes were recorded in KBr pellets using Perkin-Elmer FT-IR spectrophotometer in the range 4000–400 cm−1 at School of Studies in Chemistry and Biochemistry, Vikram University, Ujjain, India. Particle size analysis was carried out at SICART, Gujarat using, laser diffraction particle size analyzer. The instrument used was CILAS 1064L/D model in the range of 0.04–500 μm. The melting points of the ligand and complexes were recorded in open capillaries on a capillary melting point apparatus.The antifungal activities of both the ligands and their complexes were testedin vitro for growth inhibitory against Aspergillus niger andAspergillus flavusby agar growth food poison technique [17] at different concentrations compared with Grisofulvin as appositive control.The diuretic activity of Hg(II) and VO(IV) complexes were tested on white albino mice at Jawaharlal Nehru Cancer Hospital and Research Centre, Bhopal, India. Mice were fed with standard rodent pellet diet and acidified double-distilled water. The selected test compound, ligand, and standard drug xipamide (XM) at a dose of 0.24 mg suspended in 0.5% gum acacia were administrated to animals of respective group. One group of animal was taken as control. For the measurement of weight of urine, Whatman no. 1 filter paper was used. The urine weight was recorded after two hours.


### 2.1. Synthesis of the Ligand (Xipamide Salicylaldimine)

Equimolar (0.01 M) solutions of pure drug (0.22 gm) and salicylaldehyde (0.14 mL) were separately dissolved in methanol-water mixture (1 : 1) and refluxed for four hours and kept for a day. Peach colour crystals of xipamide Schiff base were formed in the reaction mixture and were filtered and washed thoroughly with 50% methanol-water mixture, dried over vacuum, and weighed. Melting point of Schiff base was recorded. The structure of the synthesized ligand is shown in Figure1.Figure 1
Structure of ligand.


### 2.2. Synthesis of Complexes

For the synthesis of complexes, 0.006 M ligand solution was prepared in 50% acetone-water solvent and refluxed for four hours with  0.003 M solution of metal salts separately. The refluxed solutions were kept for some days. Solid crystalline compounds appeared in the solution, which were filtered, washed with 50% acetone-water mixture, dried, and weighed. Melting points of the complexes were recorded.


## 2.1. Synthesis of the Ligand (Xipamide Salicylaldimine)

Equimolar (0.01 M) solutions of pure drug (0.22 gm) and salicylaldehyde (0.14 mL) were separately dissolved in methanol-water mixture (1 : 1) and refluxed for four hours and kept for a day. Peach colour crystals of xipamide Schiff base were formed in the reaction mixture and were filtered and washed thoroughly with 50% methanol-water mixture, dried over vacuum, and weighed. Melting point of Schiff base was recorded. The structure of the synthesized ligand is shown in Figure1.Figure 1
Structure of ligand.


## 2.2. Synthesis of Complexes

For the synthesis of complexes, 0.006 M ligand solution was prepared in 50% acetone-water solvent and refluxed for four hours with  0.003 M solution of metal salts separately. The refluxed solutions were kept for some days. Solid crystalline compounds appeared in the solution, which were filtered, washed with 50% acetone-water mixture, dried, and weighed. Melting points of the complexes were recorded.


## 3. Results and Discussion

The analytical data of the complexes and their molar conductance values are given in   Table1. All these complexes are analyzed for 1 : 2 stoichiometry of the type ML2. On the basis of these characterizations it has been found that all the complexes are nonhygroscopic, stable at room temperature, insoluble in water, but fairly soluble in DMSO. The molar conductance values of these complexes are too low to account for their electrolytic behavior [18, 19].Table 1
Analytical data and molar conductance values for ligand and metal complexes.
S. number
Ligand/complexes
Elemental analysis (%): found (Calcd.)
M.pt. (°C)
Color
Molar conductance Ω−1 cm2 mol−1
C
N
S
Cl
M
1
L
56.87 (57.57)
5.84 (5.96)
6.91 (6.97)
7.50 (7.61)
—
250
Peach
—
2
HgL2
47.08 (47.32)
4.97 (5.01)
5.48 (5.73)
6.34 (6.36)
17.70 (17.98)
241
Off-White
13.2
3
ZnL2
53.48 (53.85)
5.64 (5.71)
6.38 (6.52)
7.01 (7.14)
6.51 (6.67)
218
White
12.8
4
VOL2
52.87 (53.17)
5.79 (5.70)
6.67 (6.52)
7.09 (7.25)
5.27 (5.18)
242
Yellow
11.8


### 3.1. Spectral Studies of Ligand and Its Complexes

#### 3.1.1. IR Spectra

The characteristic vibrations and assignments of ligand and its complexes are described in Table2. The IR spectra of the complexes indicate that the ligand behaves as bidentate and coordinates with metals via azomethine nitrogen and phenolic –OH groups. The shift of vC=N to lower wave number by 30–40 cm−1 in the complexes indicates that these groups are involved in complexation [20, 21]. The ligand shows strong band at 3386 cm−1 due to phenolic –OH group [22]. This band is absent in all the metal complexes indicating the involvement of this group in complex formation [23]. Moreover, the shift of the vC–O phenolic bands from 1282 cm−1 in ligand to 1282–1312 cm−1 in the spectra of metal complexes supports the coordination of the phenolic oxygen atom to the metal ion [24]. The bands for vM–O modes appeared in the range of 580 cm−1–615 cm−1 in all the complexes [25]. The presence of sharp band in the region 503–514 cm−1 in the spectra of all the complexes assigned to vM–N mode [26] further support the involvement of azomethine nitrogen atom in coordination. In addition to these bands VO(IV) complex exhibits the characteristic stretching frequency [27, 28] for V=O at 952 cm−1.Table 2
IR spectral data (cm−1) of ligand and its complexes.
S. number
Ligand/complexes
V
N
–
H
v
C=N
V
C
–
O
v
C=O
v
M
–
N
v
M
–
O
1
C22H19N2O5ClS
3302
1639
1282
1671
—
—
2
C44H36N4O10Cl2S2Hg
3301
1598
1312
1669
514
615
3
C44H36N4O10Cl2S2Zn
3300
1623
1288
1681
514
580
4
C44H36N4O10Cl2S2VO
3300
1620
1281
1680
505
608


#### 3.1.2. Magnetic Susceptibility and Electronic Spectra

The magnetic moment obtained for the oxovanadium (IV) complex at room temperature is 1.77 B.M, and its electronic spectra displayed bands at 13986, 17094, and 21740 cm−1 assigned for 2B2 → 2E, 2B2 → 2B1, and 2B2 → 2A1 transitions, respectively. These values suggest the square pyramidal geometry for VO(IV) complex [29]. The Hg(II) and Zn(II) complexes are found to be diamagnetic as expected for d10 systems and may have tetrahedral geometry [30].


#### 3.1.3. Mass Spectra

The mass spectrum of [Zn(C22H18ClN2O5S)2] as shown in Figure 2 shows a molecular ion peak at m/z 980 (I) due to [Zn(L)2]⨥ which is in accordance with the proposed formula of the complex. The other peaks at m/z values 151 and 271 may be due to the fragments (C9H11NO)⨥ and [Zn(ClC6H4COH)SO2NH]⨥. The base peak at m/z 117 may be due to the zinc metal linked to the donor atoms of the ligand. Such type of fragmentation pattern has been reported by many workers [31, 32].Figure 2
Mass spectrum of ZnL2.


#### 3.1.4. Particle Size Analysis

To find out the maximum efficiency of the drugs and their metal complexes, studies on    the particle size analysis are being considered very helpful [33]. The bioavailability of   low-solubility drug is often intrinsically related to the drug particle size. Smaller particle size of the complexes is responsible for the enhanced solubility of the drug [34]. The results of the particle size analysis carried out for the pure drug, ligand, and its Hg(II) and VO(IV) complexes have been recorded in Table 3. These results reveal that, after complexation, the size of the ligand and complexes got reduced to a considerable extent as compared to their parent drug xipamide (XM). It is well known that smaller size leads to better absorption, so it is concluded from our result that complexation enhanced the absorption and potency of the drug [35].Table 3
Particle size measurement of pure drug, ligand and its metal complexes.
S. number
Sample code
Particle size (μm)
1
XM
112
2
L
95.6
3
HgL2
67.5
4
VOL2
64.5


#### 3.1.5. Antimicrobial Activity

For antifungal activity the ligand and its metal complexes were screened againstAspergillus niger,and the findings are given in Table 4. These complexes showed higher activity with 12–17 mm inhibition than the ligand which showed only 11.48 mm inhibition at the same concentration as that of the test drug. However, ligand and their complexes showed lower activity as compared to standard drug griseofulvin with 19.38 mm inhibition at the same concentration.Table 4
Antimicrobial screening data of the ligand L and its metal complexes.
S. number
Compound/complex
Antifungal zone of inhibition (in mm)
A.  niger
A.  flavous
1
L
11.48
10.38
2
HgL2
15.76
16.41
3
ZnL2
13.45
14.33
4
VOL2
17.00
21.22
5
Grisofulvin
19.38
18.22Antifungal activity studies of ligand and its complexes againstAspergillus flavusshowed that all the complexes with 11.47–21.22 mm inhibition showed higher activity than the ligand which showed only 10.38 mm inhibition only. VO(IV) complex showed higher activity than standard drug which showed 18.22 mm inhibition at the same concentration as that of the test drug. It is known that chelation tends to make the ligand act as more powerful and potent antimicrobial agent, thus inhibiting more of the microbes than the parent ligand [36].


#### 3.1.6. Diuretic Activity

The diuretic activity of the Hg(II) and VO(IV) complexes was tested on white albino mice and recorded in Table5. The selected test compound, ligand, and standard drug xipamide at a dose of 0.24 mg suspended in 0.5% gum acacia were administrated to animals of the respective group. The result revealed that metal complexes have more diuretic activity as compared to the respective ligand and pure drug. Thus it is revealed that complexation can increase the pharmaceutical activity of the parent drug [37].Table 5
Diuretic screening data of the pure drug, ligand, and its metal complexes.
Group
Ligand/complexes
Average volume of urine (μL)
Final average (μL)
1:00 PM
3:00 PM
5:00 PM
I
Control
113.94
167.22
118.01
133.06
±
29.656
II
Xipamide
155.66
208.09
266.91
210.22
±
55.656
III
L
175.75
235.48
289.10
233.44
±
56.702
IV
HgL2
265.54
283.12
343.12
297.26
±
40.6777
V
VOL2
386.66
375.29
378.57
380.17
±
5.852Statistical analyses were performed by using one-way analysis of variance ANOVA followed by GraphPad InStat 3. Statistical significance was accepted at the 5% level (P<0.05). The VO(IV) complex is found to be more significant with P<0.001 whereas Hg(II) complex is also found to be significant with P<0.05.


## 3.1. Spectral Studies of Ligand and Its Complexes

### 3.1.1. IR Spectra

The characteristic vibrations and assignments of ligand and its complexes are described in Table2. The IR spectra of the complexes indicate that the ligand behaves as bidentate and coordinates with metals via azomethine nitrogen and phenolic –OH groups. The shift of vC=N to lower wave number by 30–40 cm−1 in the complexes indicates that these groups are involved in complexation [20, 21]. The ligand shows strong band at 3386 cm−1 due to phenolic –OH group [22]. This band is absent in all the metal complexes indicating the involvement of this group in complex formation [23]. Moreover, the shift of the vC–O phenolic bands from 1282 cm−1 in ligand to 1282–1312 cm−1 in the spectra of metal complexes supports the coordination of the phenolic oxygen atom to the metal ion [24]. The bands for vM–O modes appeared in the range of 580 cm−1–615 cm−1 in all the complexes [25]. The presence of sharp band in the region 503–514 cm−1 in the spectra of all the complexes assigned to vM–N mode [26] further support the involvement of azomethine nitrogen atom in coordination. In addition to these bands VO(IV) complex exhibits the characteristic stretching frequency [27, 28] for V=O at 952 cm−1.Table 2
IR spectral data (cm−1) of ligand and its complexes.
S. number
Ligand/complexes
V
N
–
H
v
C=N
V
C
–
O
v
C=O
v
M
–
N
v
M
–
O
1
C22H19N2O5ClS
3302
1639
1282
1671
—
—
2
C44H36N4O10Cl2S2Hg
3301
1598
1312
1669
514
615
3
C44H36N4O10Cl2S2Zn
3300
1623
1288
1681
514
580
4
C44H36N4O10Cl2S2VO
3300
1620
1281
1680
505
608


### 3.1.2. Magnetic Susceptibility and Electronic Spectra

The magnetic moment obtained for the oxovanadium (IV) complex at room temperature is 1.77 B.M, and its electronic spectra displayed bands at 13986, 17094, and 21740 cm−1 assigned for 2B2 → 2E, 2B2 → 2B1, and 2B2 → 2A1 transitions, respectively. These values suggest the square pyramidal geometry for VO(IV) complex [29]. The Hg(II) and Zn(II) complexes are found to be diamagnetic as expected for d10 systems and may have tetrahedral geometry [30].


### 3.1.3. Mass Spectra

The mass spectrum of [Zn(C22H18ClN2O5S)2] as shown in Figure 2 shows a molecular ion peak at m/z 980 (I) due to [Zn(L)2]⨥ which is in accordance with the proposed formula of the complex. The other peaks at m/z values 151 and 271 may be due to the fragments (C9H11NO)⨥ and [Zn(ClC6H4COH)SO2NH]⨥. The base peak at m/z 117 may be due to the zinc metal linked to the donor atoms of the ligand. Such type of fragmentation pattern has been reported by many workers [31, 32].Figure 2
Mass spectrum of ZnL2.


### 3.1.4. Particle Size Analysis

To find out the maximum efficiency of the drugs and their metal complexes, studies on    the particle size analysis are being considered very helpful [33]. The bioavailability of   low-solubility drug is often intrinsically related to the drug particle size. Smaller particle size of the complexes is responsible for the enhanced solubility of the drug [34]. The results of the particle size analysis carried out for the pure drug, ligand, and its Hg(II) and VO(IV) complexes have been recorded in Table 3. These results reveal that, after complexation, the size of the ligand and complexes got reduced to a considerable extent as compared to their parent drug xipamide (XM). It is well known that smaller size leads to better absorption, so it is concluded from our result that complexation enhanced the absorption and potency of the drug [35].Table 3
Particle size measurement of pure drug, ligand and its metal complexes.
S. number
Sample code
Particle size (μm)
1
XM
112
2
L
95.6
3
HgL2
67.5
4
VOL2
64.5


### 3.1.5. Antimicrobial Activity

For antifungal activity the ligand and its metal complexes were screened againstAspergillus niger,and the findings are given in Table 4. These complexes showed higher activity with 12–17 mm inhibition than the ligand which showed only 11.48 mm inhibition at the same concentration as that of the test drug. However, ligand and their complexes showed lower activity as compared to standard drug griseofulvin with 19.38 mm inhibition at the same concentration.Table 4
Antimicrobial screening data of the ligand L and its metal complexes.
S. number
Compound/complex
Antifungal zone of inhibition (in mm)
A.  niger
A.  flavous
1
L
11.48
10.38
2
HgL2
15.76
16.41
3
ZnL2
13.45
14.33
4
VOL2
17.00
21.22
5
Grisofulvin
19.38
18.22Antifungal activity studies of ligand and its complexes againstAspergillus flavusshowed that all the complexes with 11.47–21.22 mm inhibition showed higher activity than the ligand which showed only 10.38 mm inhibition only. VO(IV) complex showed higher activity than standard drug which showed 18.22 mm inhibition at the same concentration as that of the test drug. It is known that chelation tends to make the ligand act as more powerful and potent antimicrobial agent, thus inhibiting more of the microbes than the parent ligand [36].


### 3.1.6. Diuretic Activity

The diuretic activity of the Hg(II) and VO(IV) complexes was tested on white albino mice and recorded in Table5. The selected test compound, ligand, and standard drug xipamide at a dose of 0.24 mg suspended in 0.5% gum acacia were administrated to animals of the respective group. The result revealed that metal complexes have more diuretic activity as compared to the respective ligand and pure drug. Thus it is revealed that complexation can increase the pharmaceutical activity of the parent drug [37].Table 5
Diuretic screening data of the pure drug, ligand, and its metal complexes.
Group
Ligand/complexes
Average volume of urine (μL)
Final average (μL)
1:00 PM
3:00 PM
5:00 PM
I
Control
113.94
167.22
118.01
133.06
±
29.656
II
Xipamide
155.66
208.09
266.91
210.22
±
55.656
III
L
175.75
235.48
289.10
233.44
±
56.702
IV
HgL2
265.54
283.12
343.12
297.26
±
40.6777
V
VOL2
386.66
375.29
378.57
380.17
±
5.852Statistical analyses were performed by using one-way analysis of variance ANOVA followed by GraphPad InStat 3. Statistical significance was accepted at the 5% level (P<0.05). The VO(IV) complex is found to be more significant with P<0.001 whereas Hg(II) complex is also found to be significant with P<0.05.


## 3.1.1. IR Spectra

The characteristic vibrations and assignments of ligand and its complexes are described in Table2. The IR spectra of the complexes indicate that the ligand behaves as bidentate and coordinates with metals via azomethine nitrogen and phenolic –OH groups. The shift of vC=N to lower wave number by 30–40 cm−1 in the complexes indicates that these groups are involved in complexation [20, 21]. The ligand shows strong band at 3386 cm−1 due to phenolic –OH group [22]. This band is absent in all the metal complexes indicating the involvement of this group in complex formation [23]. Moreover, the shift of the vC–O phenolic bands from 1282 cm−1 in ligand to 1282–1312 cm−1 in the spectra of metal complexes supports the coordination of the phenolic oxygen atom to the metal ion [24]. The bands for vM–O modes appeared in the range of 580 cm−1–615 cm−1 in all the complexes [25]. The presence of sharp band in the region 503–514 cm−1 in the spectra of all the complexes assigned to vM–N mode [26] further support the involvement of azomethine nitrogen atom in coordination. In addition to these bands VO(IV) complex exhibits the characteristic stretching frequency [27, 28] for V=O at 952 cm−1.Table 2
IR spectral data (cm−1) of ligand and its complexes.
S. number
Ligand/complexes
V
N
–
H
v
C=N
V
C
–
O
v
C=O
v
M
–
N
v
M
–
O
1
C22H19N2O5ClS
3302
1639
1282
1671
—
—
2
C44H36N4O10Cl2S2Hg
3301
1598
1312
1669
514
615
3
C44H36N4O10Cl2S2Zn
3300
1623
1288
1681
514
580
4
C44H36N4O10Cl2S2VO
3300
1620
1281
1680
505
608


## 3.1.2. Magnetic Susceptibility and Electronic Spectra

The magnetic moment obtained for the oxovanadium (IV) complex at room temperature is 1.77 B.M, and its electronic spectra displayed bands at 13986, 17094, and 21740 cm−1 assigned for 2B2 → 2E, 2B2 → 2B1, and 2B2 → 2A1 transitions, respectively. These values suggest the square pyramidal geometry for VO(IV) complex [29]. The Hg(II) and Zn(II) complexes are found to be diamagnetic as expected for d10 systems and may have tetrahedral geometry [30].


## 3.1.3. Mass Spectra

The mass spectrum of [Zn(C22H18ClN2O5S)2] as shown in Figure 2 shows a molecular ion peak at m/z 980 (I) due to [Zn(L)2]⨥ which is in accordance with the proposed formula of the complex. The other peaks at m/z values 151 and 271 may be due to the fragments (C9H11NO)⨥ and [Zn(ClC6H4COH)SO2NH]⨥. The base peak at m/z 117 may be due to the zinc metal linked to the donor atoms of the ligand. Such type of fragmentation pattern has been reported by many workers [31, 32].Figure 2
Mass spectrum of ZnL2.


## 3.1.4. Particle Size Analysis

To find out the maximum efficiency of the drugs and their metal complexes, studies on    the particle size analysis are being considered very helpful [33]. The bioavailability of   low-solubility drug is often intrinsically related to the drug particle size. Smaller particle size of the complexes is responsible for the enhanced solubility of the drug [34]. The results of the particle size analysis carried out for the pure drug, ligand, and its Hg(II) and VO(IV) complexes have been recorded in Table 3. These results reveal that, after complexation, the size of the ligand and complexes got reduced to a considerable extent as compared to their parent drug xipamide (XM). It is well known that smaller size leads to better absorption, so it is concluded from our result that complexation enhanced the absorption and potency of the drug [35].Table 3
Particle size measurement of pure drug, ligand and its metal complexes.
S. number
Sample code
Particle size (μm)
1
XM
112
2
L
95.6
3
HgL2
67.5
4
VOL2
64.5


## 3.1.5. Antimicrobial Activity

For antifungal activity the ligand and its metal complexes were screened againstAspergillus niger,and the findings are given in Table 4. These complexes showed higher activity with 12–17 mm inhibition than the ligand which showed only 11.48 mm inhibition at the same concentration as that of the test drug. However, ligand and their complexes showed lower activity as compared to standard drug griseofulvin with 19.38 mm inhibition at the same concentration.Table 4
Antimicrobial screening data of the ligand L and its metal complexes.
S. number
Compound/complex
Antifungal zone of inhibition (in mm)
A.  niger
A.  flavous
1
L
11.48
10.38
2
HgL2
15.76
16.41
3
ZnL2
13.45
14.33
4
VOL2
17.00
21.22
5
Grisofulvin
19.38
18.22Antifungal activity studies of ligand and its complexes againstAspergillus flavusshowed that all the complexes with 11.47–21.22 mm inhibition showed higher activity than the ligand which showed only 10.38 mm inhibition only. VO(IV) complex showed higher activity than standard drug which showed 18.22 mm inhibition at the same concentration as that of the test drug. It is known that chelation tends to make the ligand act as more powerful and potent antimicrobial agent, thus inhibiting more of the microbes than the parent ligand [36].


## 3.1.6. Diuretic Activity

The diuretic activity of the Hg(II) and VO(IV) complexes was tested on white albino mice and recorded in Table5. The selected test compound, ligand, and standard drug xipamide at a dose of 0.24 mg suspended in 0.5% gum acacia were administrated to animals of the respective group. The result revealed that metal complexes have more diuretic activity as compared to the respective ligand and pure drug. Thus it is revealed that complexation can increase the pharmaceutical activity of the parent drug [37].Table 5
Diuretic screening data of the pure drug, ligand, and its metal complexes.
Group
Ligand/complexes
Average volume of urine (μL)
Final average (μL)
1:00 PM
3:00 PM
5:00 PM
I
Control
113.94
167.22
118.01
133.06
±
29.656
II
Xipamide
155.66
208.09
266.91
210.22
±
55.656
III
L
175.75
235.48
289.10
233.44
±
56.702
IV
HgL2
265.54
283.12
343.12
297.26
±
40.6777
V
VOL2
386.66
375.29
378.57
380.17
±
5.852Statistical analyses were performed by using one-way analysis of variance ANOVA followed by GraphPad InStat 3. Statistical significance was accepted at the 5% level (P<0.05). The VO(IV) complex is found to be more significant with P<0.001 whereas Hg(II) complex is also found to be significant with P<0.05.


## 4. Conclusion

The outcome of the above results confirms the stoichiometry of the complexes to be 1 : 2 [M : L] as indicated by elemental analysis and conductometric measurements. IR spectra suggest that the ligand behaves as bidentate and coordinates to the central metal ion through azomethine nitrogen and phenolic –OH group. This has been further confirmed on the basis of NMR spectral studies. Mass spectra further support the above stoichiometry on the basis of respective molecular masses and fragmentation patterns. Thus, on the basis of above physicochemical and spectral studies, the assigned structures for the metal complexes are shown in Figures3(a) and 3(b). The complexes are found to have higher biological activities as compared to the respective ligand and the parent drug that, somehow, justifies the purpose of the research work. The present work will be further extended to the synthesis of metal complexes using other biologically active metals and evaluation of their biological activities.Structure of metal complexes.
(a)
(b)



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*Source: 549805-2013-02-18.xml*