# Synthesis, Characterization, and Biological Activity of Mn(II), Fe(II), Co(II), Ni(II), Cu(II), Zn(II), and Cd(II) Complexes of N-Thiophenoyl-N′-Phenylthiocarbohydrazide

Authors: M. Yadav; Debasis Behera
Journal: Journal of Chemistry
 (2013)

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## Abstract

Mn(II), Fe(II), Co(II), Ni(II), Cu(II), Zn(II), and Cd(II) complex of N-thiophenoyl -N′-phenylthiocarbohydrazide (H2 TPTH) have been synthesized and characterized by elemental analysis, magnetic susceptibility measurements, infrared, NMR, electronic, and ESR spectral studies. The complexes were found to have compositions [Mn(H TPTH)2], [Co(TPTH) (H2O)2], [Ni(TPTH) (H2O)2], [Cu(TPTH)], [Zn(H TPTH)], [Cd(H TPTH)2], and [Fe(H TPTH)2(EtOH)]. The magnetic and electronic spectral studies suggest square planar geometry for [Cu(TPTH)], tetrahedral geometry for [Zn(TPTH)] and [Cd(H TPTH)2], and octahedral geometry for rest of the complexes. The infrared spectral studies of the 1 : 1 deprotonated complexes suggest bonding through enolic oxygen, thiolato sulfur, and both the hydrazinic nitrogens. Thus, H2TPTH acts as a binegative tetradentate ligand. H2 TPTH and its metal complexes have been screened against several bacteria and fungi.


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## Body

## 1. Introduction

The expansion of research in the coordination chemistry of nitrogen-sulphur donor ligands such as substituted thiosemicarbazides [1], thiosemicarbazones [2–4], and dithiocarbazates [5], during the recent years has been due to their remarkable antineoplastic activity against a variety of tumors [6] in addition to their applicable antifungal [7] and antibacterial [8] activities. Sulphur and nitrogen containing ligands and their transition metal complexes are also used as corrosion inhibitors [9, 10] and extreme pressure lubricant additives [11]. Keeping in view the above biological activity of the ligands, we planned to undertake the synthesis, characterization, antibacterial, and antifungal activity of the 3d-metal complexes of N-thiophenoyl-N′-phenylthiocarbohydrazide (H2 TPTH) (Figure 1), having oxygen and sulphur as donors. This legand is expected to form addition complexes without loss of protons and deprotonated complexes by loss of one or both the hydrazinic protons.Figure 1
H2 TPTH.


## 2. Experimental

### 2.1. Starting Materials

All the chemicals used were of analytical grade. Ammonium polysulphide [12] and carboxymethyldithiobenzoate [13] were prepared by literature methods.


### 2.2. Preparation of N-Thiophenoyl-N′-Phenylthiocarbohydrazide (H2 TPTH)

N-thiophenoyl-N′-phenylthiocarbohydrazide (H2 TPTH) was prepared by mixing solutions of 2-thiophene carboxylic acid hydrazide (20 mmol) and carboxymethyldithiobenzoate (20 mmol) each dissolved separately in 50 mL of 0.5 N NaOH and allowing the mixture to stand at room temperature for 2 hrs. The product precipitated by adding dilute AcOH dropwise to the above ice-cold mixture, was filtered off, washed with H2O, dried, and recrystallized from EtOH.


### 2.3. Preparation of the Complexes

#### 2.3.1. [M(H TPTH)2]

The complexes of the type [M(H TPTH)2] [M = Mn(II), Cd(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (2 mmol) for 1 h under reflux. The precipitated complexes were filtered, washed with methanol and dried in vacuo.


#### 2.3.2.  [M(TPTH)(H2O)2] and [M(TPTH)]

The complexes of the type [M(TPTH)(H2O)2] [M = Co(II), Ni(II)] and [M(TPTH)] [M = Cu(II), Zn(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (1 mmol) for about 1 h under reflux. The precipitated complexes were filtered, washed with methanol, and dried in vacuo.


#### 2.3.3. [Fe(H TPTH)2(EtOH)]

[Fe(H TPTH)2(EtOH)] was prepared by boiling together an aqueous-methanolic solution (25 mL) of (NH4)2SO4·FeSO4·6H2O (1 mmol) which was prepared in the presence of a small amount of ascorbic acid and H2 TPTH (2 mmol) in ethanol (25 mL) for about 1 h. The precipitated complex was filtered, washed with water, ethanol, and dried in vacuo.


### 2.4. Instrumentation

Complexes were analysed for their metal content, following a standard procedure [14] by decomposing the complexes with a mixture of HNO3 and HCl followed by H2SO4. Sulphur and chloride were determined as BaSO4 and AgCl, respectively. Carbon, hydrogen, and nitrogen were estimated on a EA 1108 CHN Elemental Analyser. Magnetic susceptibility measurements were made at room temperature on a Cahn-Faraday balance using Hg[Co(NCS)4] as calibrant. Electronic spectra were recorded on a CARY-2390 UV-Visible Spectrophotometer as Nujol mulls [15]. IR Spectra were recorded in the 4000–400 cm−1 region (KBr disc) on a JA SCO FT/FR-5300 spectrophotometer. The 1H and 13C NMR spectra were obtained in DMSO-D6 on a JEOL FX-300 Q FT/NMR spectrometer using TMS as internal reference. ESR spectra were recorded on a X-band spectrometer model EPR-112 using DPPH as a 〈g〉 marker. The electrical conductivity of the pressed pellets of the complexes was obtained by a conventional two-probe method in the 303–383 K range with contact made on the pellet surfaces using graphite paint. A Keith ley 236 SMU was used to measure the resistance.


### 2.5. Bactericidal Screening

The antibacterial activity of the ligand and the complexes was evaluated using the disc diffusion technique [16]. A stock solution of 2000 μg cm−3 was made by dissolving 2 mg cm−3 of each compound in DMSO and it was serially doubled diluted upto five dilutions, giving the concentrations of 1000, 250, 125, and 62.5 μg cm−3. Filter paper (Whattman No. 42) discs (6 mm dia) were soaked in these solutions of different concentrations and placed on nutrient agar plates. The plates were then incubated for 24 hrs at 37°C. The inhibition zones around the discs were measured after 24 hrs. Cotrimoxazole was used as a standard drug in the form of disc, containing trimethoprim—1.25 μg and sulfamethoxazole = 23.75 μg per disc. The zones of inhibition were found to be 20, 32, and 18 mm against Staph aureus, Escherichia coli, and Pseudomonas aeruginosa, respectively, in agreement with the sensitive zone reported in the literature.


### 2.6. Fungicidal Screening

The antifungal activity was evaluated by a drug dilution technique. The solution of the test compounds was prepared as described earlier to which Sabouraud’s dextrose broth and slightly turbid suspension of fungus in normal saline (10μL) were added and placed in an incubator for 48–72 hrs. A turbidity in the solution indicated the growth of fungus, which is represented as − sign, however, a clear solution showed that there was no growth of fungus and is represented as + sign. The cases where compounds showed antifungal activity, no growth was observed in the solution. Amphotericin B was used as a standard drug.


## 2.1. Starting Materials

All the chemicals used were of analytical grade. Ammonium polysulphide [12] and carboxymethyldithiobenzoate [13] were prepared by literature methods.


## 2.2. Preparation of N-Thiophenoyl-N′-Phenylthiocarbohydrazide (H2 TPTH)

N-thiophenoyl-N′-phenylthiocarbohydrazide (H2 TPTH) was prepared by mixing solutions of 2-thiophene carboxylic acid hydrazide (20 mmol) and carboxymethyldithiobenzoate (20 mmol) each dissolved separately in 50 mL of 0.5 N NaOH and allowing the mixture to stand at room temperature for 2 hrs. The product precipitated by adding dilute AcOH dropwise to the above ice-cold mixture, was filtered off, washed with H2O, dried, and recrystallized from EtOH.


## 2.3. Preparation of the Complexes

### 2.3.1. [M(H TPTH)2]

The complexes of the type [M(H TPTH)2] [M = Mn(II), Cd(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (2 mmol) for 1 h under reflux. The precipitated complexes were filtered, washed with methanol and dried in vacuo.


### 2.3.2.  [M(TPTH)(H2O)2] and [M(TPTH)]

The complexes of the type [M(TPTH)(H2O)2] [M = Co(II), Ni(II)] and [M(TPTH)] [M = Cu(II), Zn(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (1 mmol) for about 1 h under reflux. The precipitated complexes were filtered, washed with methanol, and dried in vacuo.


### 2.3.3. [Fe(H TPTH)2(EtOH)]

[Fe(H TPTH)2(EtOH)] was prepared by boiling together an aqueous-methanolic solution (25 mL) of (NH4)2SO4·FeSO4·6H2O (1 mmol) which was prepared in the presence of a small amount of ascorbic acid and H2 TPTH (2 mmol) in ethanol (25 mL) for about 1 h. The precipitated complex was filtered, washed with water, ethanol, and dried in vacuo.


## 2.3.1. [M(H TPTH)2]

The complexes of the type [M(H TPTH)2] [M = Mn(II), Cd(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (2 mmol) for 1 h under reflux. The precipitated complexes were filtered, washed with methanol and dried in vacuo.


## 2.3.2.  [M(TPTH)(H2O)2] and [M(TPTH)]

The complexes of the type [M(TPTH)(H2O)2] [M = Co(II), Ni(II)] and [M(TPTH)] [M = Cu(II), Zn(II)] were prepared by boiling together the methanolic solutions (25 mL) of the respective M(OAc)2·nH2O (1 mmol) and H2 TPTH (1 mmol) for about 1 h under reflux. The precipitated complexes were filtered, washed with methanol, and dried in vacuo.


## 2.3.3. [Fe(H TPTH)2(EtOH)]

[Fe(H TPTH)2(EtOH)] was prepared by boiling together an aqueous-methanolic solution (25 mL) of (NH4)2SO4·FeSO4·6H2O (1 mmol) which was prepared in the presence of a small amount of ascorbic acid and H2 TPTH (2 mmol) in ethanol (25 mL) for about 1 h. The precipitated complex was filtered, washed with water, ethanol, and dried in vacuo.


## 2.4. Instrumentation

Complexes were analysed for their metal content, following a standard procedure [14] by decomposing the complexes with a mixture of HNO3 and HCl followed by H2SO4. Sulphur and chloride were determined as BaSO4 and AgCl, respectively. Carbon, hydrogen, and nitrogen were estimated on a EA 1108 CHN Elemental Analyser. Magnetic susceptibility measurements were made at room temperature on a Cahn-Faraday balance using Hg[Co(NCS)4] as calibrant. Electronic spectra were recorded on a CARY-2390 UV-Visible Spectrophotometer as Nujol mulls [15]. IR Spectra were recorded in the 4000–400 cm−1 region (KBr disc) on a JA SCO FT/FR-5300 spectrophotometer. The 1H and 13C NMR spectra were obtained in DMSO-D6 on a JEOL FX-300 Q FT/NMR spectrometer using TMS as internal reference. ESR spectra were recorded on a X-band spectrometer model EPR-112 using DPPH as a 〈g〉 marker. The electrical conductivity of the pressed pellets of the complexes was obtained by a conventional two-probe method in the 303–383 K range with contact made on the pellet surfaces using graphite paint. A Keith ley 236 SMU was used to measure the resistance.


## 2.5. Bactericidal Screening

The antibacterial activity of the ligand and the complexes was evaluated using the disc diffusion technique [16]. A stock solution of 2000 μg cm−3 was made by dissolving 2 mg cm−3 of each compound in DMSO and it was serially doubled diluted upto five dilutions, giving the concentrations of 1000, 250, 125, and 62.5 μg cm−3. Filter paper (Whattman No. 42) discs (6 mm dia) were soaked in these solutions of different concentrations and placed on nutrient agar plates. The plates were then incubated for 24 hrs at 37°C. The inhibition zones around the discs were measured after 24 hrs. Cotrimoxazole was used as a standard drug in the form of disc, containing trimethoprim—1.25 μg and sulfamethoxazole = 23.75 μg per disc. The zones of inhibition were found to be 20, 32, and 18 mm against Staph aureus, Escherichia coli, and Pseudomonas aeruginosa, respectively, in agreement with the sensitive zone reported in the literature.


## 2.6. Fungicidal Screening

The antifungal activity was evaluated by a drug dilution technique. The solution of the test compounds was prepared as described earlier to which Sabouraud’s dextrose broth and slightly turbid suspension of fungus in normal saline (10μL) were added and placed in an incubator for 48–72 hrs. A turbidity in the solution indicated the growth of fungus, which is represented as − sign, however, a clear solution showed that there was no growth of fungus and is represented as + sign. The cases where compounds showed antifungal activity, no growth was observed in the solution. Amphotericin B was used as a standard drug.


## 3. Results and Discussion

All the complexes are insoluble in water, methanol, and ethanol but are soluble in polar organic solvents such as DMSO and DMF. [Mn(H TPTH)2] and [Co(TPTH)(H2O)2] are more soluble in DMSO than other complexes. The complexes having 1 : 1 metal-ligand stoichiometry (Table 1) are formed by loss of two protons from the legend, generating a conjugated system. Because of steric considerations, all the four potential sites cannot be attached to a single metal and, therefore, the ligand binds in a polymeric fashion. Accordingly, the 1 : 1 complexes show high-melting points. The following equations represent the formation of the ligand and the complexes:
(1)(C6H5)CSSCH2COOH+C4H3SCONHNH22222→NaOHAcOHC6H5CSNHNHCOC4H3S(H2TPTH)2222→NaOHaCOH+HSCH2COOH(2)M(OAc)2·nH2O+2H2TPTH2222→MeOH[M(HTPTH)2]+nH2O+2AcOH
M = Mn(II), Cd(II); n=4, 2
(3)M(OAc)2·4H2O+H2TPTH2222→MeOH[M(TPTH)(H2O)2]+2H2O+2AcOH
M = Co(II), Ni(II)
(4)M(OAc)2·nH2O+H2TPTH2222→MeOH[M(TPTH)]+nH2O+2AcOH
M = Cu(II), Zn(II); n=1, 2
(5)(NH4)2SO4·FeSO4·6H2O+2H2TPTH2222→H2OEtOH[Fe(HTPTH)2(EtOH)](NH4)2SO4+H2SO42222→H2OEtOH+6H2O.Table 1
Analytical data and physical properties of the complexes N-thiophenoyl-N′-phenylthiocarbohydrazide (H2 TPTH).
Compound empirical formula
Colour/Yield   (%)
Found   (Calcd.) %
M.P.   (°C)
μ
eff  (B.M.)
M
C
H
N
S
N2H4
H2 TPTH C12H10N2S2O
Cream  (60)
—
54.9 (55.0)
3.7  (3.8)
10.5 (10.7)
24.3 (24.4)
12.9 (13.0)
125
Diamag
[Mn(H TPTH)2]  C24H18N4S3O3Mn
Yellow  (55)
9.7 (9.8)
51.2 (51.3)
3.1 (3.2)
9.9 (10.0)
17.0 (17.1)
11.6 (11.7)
276
5.76
[Fe(H TPTH)2  (Et)] C26H24N4S3O4Fe
Dirty yellow (45)
9.1 (9.2)
51.1 (51.3)
3.8 (3.9)
9.0 (9.2)
15.6 (15.8)
10.8 (10.8)
238
5.31
[Co(TPTH) (H2O)] C12H12N2S2O3Co
Brick red (60)
16.4 (16.6)
40.4   (40.6)
3.3 (3.5)
7.7   (7.9)
17.8 (18.0)
9.3 (9.4)
>322
4.94
[Ni(TPTH) (H2O)2] C12H12N2S2O3Ni
Dark green 55)
16.4 (16.5)
40.5 (40.6)
3.3 (3.4)
7.8 (7.9)
17.9 (18.0)
9.3 (9.4)
>364
3.06
[Cu(TPTH)] C12H8N2S2OCu
Black (60)
19.5   (19.6)
44.4 (44.5)
2.3 (2.5)
8.6 (8.7)
19.7 (19.8)
10.3 (10.4)
282
1.98
[Zn(TPTH)] C12H8N2S2OZn
White (45)
19.9 (20.1)
44.2 (44.3)
2.4 (2.5)
8.4 (8.6)
19.5 (19.7)
10.2 (10.3)
>363
Diamag
[Cd(H TPTH)2]C24H18N4S3O3Cd
White (50)
18.1 (18.2)
46.5 (46.6)
2.8 (2.9)
9.0 (9.1)
15.3 (15.5)
10.5   (10.6)
256
Diamag


### 3.1. Magnetic Moments and Electronic Spectra

The magnetic moments and electronic spectral data of the complexes are given in Tables1 and 2, respectively. [Mn(H TPTH)2] shows a magnetic moment, 5.76 B.M. and exhibits a band at 16140 cm−1 assigned to the A61g→T41g transition for the octahedral geometry [17]. The magnetic moment 5.31 B.M. and presence of bands at 11770 and 20840 cm−1 owing to the T25→B15 and charge-transfer transitions, respectively, suggests a high-spin square pyramidal geometry for [Fe(H TPTH)2(EtOH)]·[Co(TPTH)(H2O)2] shows a magnetic moment of 4.92 B.M. and exhibits a d–d band at 16675 cm−1, assigned to the T41g(F)→T41g(P) (ν3) transition for a distorted octahedral geometry. Ni(TPTH)(H2O)2] exhibits a magnetic moment of 3.06 B.M. and shows a band at 16140 cm−1 attributed to the A32g(F)→T31g(F) (ν2) transition for a distorted octahedral geometry around Ni(II). [Cu(TPTH)] shows a magnetic moment of 1.98 B.M. indicating the presence of one unpaired electron. The complex shows a d–d band at 15635 cm−1 due to the envelope of the B21g→A21g,B22g and E2g transitions, usually observed for square planar Cu(II) complexes [17].Table 2
Electronic spectral bands and their assignments.
Compound
Band maxima (cm−1)
Assignments
H2TPTH
30495, 35220
L
[Mn(H TPTH)2]
16140, 24620
6
A
1g
→
4
T
1g, C.T.
[Fe(H TPTH)2(Et(OH)]
11770, 20840, 24380
5T2→5B1, C.T.
[Co(TPTH)(H2O)2]
16675, 24080
4
T
1g (F) →4T1g (P) (v3), C.T.
[Ni(TPTH)(H2O)2]
16140, 25000
3
A
2g (F) →3T1g (F) (v2), C.T.
[Cu(TPTH)]
15635, 21560, 27790
Envelope of2B1g→2A1g, 2B2g, 2Eg, C.T.
[Zn(TPTH)]
25650
C.T.
[Cd(H TPTH)2]
27035
C.T.
C.T.: charge-transfer; L: intraligand transition.


### 3.2. IR Spectra

The important IR spectral bands and their assignments are given in Table3. The IR spectrum of H2 TPTH shows bands at 3125 and 3100 cm−1 due to the presence of two NH groups. The bands at 1640, 1460, 1325, 1000, and 835 cm−1 are assigned to ν(C=O), thioamide I [β(NH) + ν(CN)], thioamide II [ν(CN) + β(NH)], ν(N–N), and ν(C=S), respectively. The spectra of [Mn(H TPTH)2] and [Fe(H TPH)2(EtOH)] show only one peak at 3125 cm−1 due to ν(NH), suggesting loss of one hydrazinic proton via enolisation/thioenolisation. A strong band at 1640 cm−1 in the ligand due to ν(C=O) is found to be absent in these complexes, and in place of this a new band due to ν(N=C) of NCO appears, suggesting that enolic oxygen is involved in bonding. [Mn(H TPTH)2] shows a negative shift of 15 cm−1 in ν(C=S), suggesting an additional bonding through thione sulfur. Furthermore, the spectra of these complexes show a positive shift of 20 cm−1 in ν(N–N) indicating that one hydrazinic nitrogen is also involved in bonding. The presence of ν(NH) at 3180 cm−1 and ν(C=O) at 1625 cm−1 in [Cd(H TPTH)2] indicates loss of NH proton via thioenolisation. Further, the band at 1460, 1325, and 1000 cm−1 due to thioamide I, II and ν(N–N) undergo positive shifts of 25, 15, and 20 cm−1, respectively, showing the involvement of thiolato sulfur [18] and one hydrazinic nitrogen in bonding.Table 3
Important IR spectral bands (cm−1) and their assignments.
Compound
v(OH)
v(N–H)
v(C=O)/v(NCO)
Thioamide I[β(NH) + v(CN)]
Thioamide II[v(CN) + β(NH)]
Thioamide IVv(C=S)/v(C–S)
v
(N–N)
H2 TPTH
—
3125, 3100
1640
1460
1325
835
1000
[Mn(H TPTH)2]
—
3125
1605
1485
1340
820
1020
[Fe(H TPTH)2(EtOH)]
—
3120
1605
1485
1340
835
1020
[Co(TPTH)(H2O)2]
3425
—
1580
1490
1395
745
1070
[Ni(TPTH)(H2O)2]
3420
—
1580
1490
1395
740
1070
[Cu(TPTH)]
—
—
1585
1490
1400
745
1070
[Zn(TPTH)]
—
—
1585
1490
1395
760
1070
[Cd(H TPTH)2]
—
3180
1625
1485
1340
740
1020The IR spectra of [M(TPTH)(H2O)2] (M = Co(II), Ni(II)) and [M(TPTH)] (M = Cu(II) and Zn(II)) show the absence of both the ν(NH), ν(C=O), and ν(C=S) bands and in place of these two new bands appear at 1580 and 745 cm−1, due to ν(N=C) of NCO and ν(C–S) modes, respectively, suggesting that both –NH–NH protons are lost via enolisation and thioenolisation and bonding of the resulting enolic oxygen and thiolato sulfur takes place with the metal ion. Further, the thioamide I, II, and ν(N–N) bands at 1460, 1325, and 1000 in the free ligand undergo a positive shift of 33, 65, and 70 cm−1, respectively, in the spectra of the complexes [19] suggesting the involvement of these groups as bonding sites. These observations show the involvement of thiolato sulfur and both the hydrazinic nitrogens, in addition to the enolic oxygen in bonding. Thus, H2 TPTH acts as a binegative tetradentate ligand in the 1 : 1 complexes.


### 3.3. NMR Spectra

The1H NMR spectrum of H2 TPTH (Table 4) in DMSO-d6 shows a signal at δ 9.86 and 9.72 ppm due to the presence of –NH–NH– protons which are lost on D2O exchange. The protons due to the thiophene ring appear at δ 7.12 (s, 1H), 7.32 (d, 1H), and 7.56 (s, 1H) ppm and the benzene ring protons appear as a multiplet at at δ 6.64 −6.92(m, 5H) ppm [20].Table 4
1H-NMR data of H2 TPTH and the complexes (δ, ppm).
Compound
Benzene ring
Thiophene ring
NH
H2 TPTH
6.64–6.92 (m, 5H)
7.12 (q, 1H), 7.32 (d, 1H), 7.56 (s, 1H)
9.86 (1H), 9.72 (1H)
[Ni(TPTH)(H2O)2]
6.61–6.88 (m, 5H)
7.08 (s, 1H), 7.28 (d, 1H), 7.52 (s, 1H)
—
[Mn(H TPTH)2]
6.62–6.90 (m, 5H)
7.04 (s, 1H), 7.30 (d, 1H), 7.51 (s, 1H)
9.66The NH signals are absent in the1H NMR spectrum of [Ni(TPTH)(H2O)2], suggesting loss of both NH protons via enolization and thioenolization. The thiophene ring protons show three separate signals at δ 7.08 (q, 1H), 7.28 (d, 1H), and 7.52 (s, 1H) ppm and the benzene ring protons are observed at δ 6.61–6.88 (m,5H) ppm.The1H NMR spectrum of [Mn(H TPTH)2] shows separate signals for the thiophene ring protons at δ 7.04 (s, 1H), 7.30 (d, 1H), and 7.51 (s, 1H) ppm and for benzene ring protons at δ 6.62–6.90 (m, 5H) ppm. The two signals appearing at δ 9.66 and 4.16 ppm are due to the presence of –NH–C(O) and –N=C(SH) protons, respectively. The latter is formed due to the thioenolization of the ligand. All the thiophene and benzene ring protons are observed nearly at the same position in the complex as compared to those of the H2 TPTH, suggesting noninvolvement of the ring sulphur in bonding.The13C NMR spectrum of (H2 TPTH) (Table 5) shows eleven signals, of which two signals at δ 181 and 163 ppm are due to the C=S and C=O carbons, respectively. The chemical shifts for the benzene and thiophene ring carbons in H2 TPTH are (δ, ppm) C′ (2, 6) 151, 146, C′ (4) 136, C′ (3, 5) 126, 122, C (2) 150, C (3) 116, C (4) 112, and C (5) 144.Table 5
13C-NMR data (δ, ppm).
Compound
>C=S
>C=O
C (2, 6)
C (4)
C (3, 5)
C′ (2)
C′ (3)
C′ (4)
C′ (5)
H2 TPTH
181
163
151, 146
136
126, 122
150
116
112
144
[Ni(TPTH)(H2O)2]
188
171
150, 147
134
130, 122
150
116
112
144
[Mn(TPTH)2]
181
174
152, 148
135
128, 123
150
117
112
146The13C-NMR spectrum of [Ni(TPTH)(H2O)2] also shows eleven signals. The chemical shifts for the ring carbons are (δ, ppm) C′ (2, 6) 150, 147, C′ (4) 134, C′ (3, 5) 130, 122, C (2) 150, C (3) 116, C (4) 112, and C (5) 144. The signals at δ 188 and 171 ppm in [Ni(TPTH)(H2O)2] shows downfield shift of 7 and 8 ppm, respectively, as compared to the ligand, suggesting the formation of C–S and C–O groups from the ligand on thioenolization and enolization, respectively.The13C-NMR spectrum of [Mn(H TPTH)2] shows separate signals for all eleven carbons. The chemical shifts for the ring carbons are (δ, ppm) C′ (2, 6) 152, 148 C′ (4) 135, C′ (3, 5) 128, 123, C (2) 150, C (3) 117, C (4) 112, and C (5) 146. The signal at 181 ppm due to C=S carbons show nearly the same chemical shifts as for the ligand, suggesting that the double bond character is retained in the complex. The signals at δ 174 ppm in the complex shows downfield shift of 11 ppm as compared to the ligand, suggesting the the involvement of C=S in bonding.


### 3.4. ESR Spectra

The room temperature solid state ESR spectrum of [Cu(TPTH)] yields a broad signal with〈g〉 value of 2.072 characteristic of square planar geometry around Cu(II).


### 3.5. Bactericidal Screening

The antibacterial activity of H2 TPTH (Table 6) and its complexes have been tested against S. aureus, E. coli, and P. aeruginosa. H2 TPTH shows antibacterial activity starting from 62.5 to 2000 μg cm−3 against S. aureus and the activity increases with an increase in the concentration. The ligand is found to be active at a concentration of 1000 μg cm−3 against E. coli. [Mn(H TPTH)2], and [Cu(TPTH)] show the activity at higher concentration namely 500, 1000, and 2000 μg cm−3 against S. aureus. [Mn(H TPTH)2], [Zn(TPTH)], and [Cu(TPTH)] also show activity against E. coliat 2000 μg cm−3. Only [Cu(TPTH)] has been found active against P. aeruginosa at 500 μg cm−3. [Zn(TPTH)] shows activity against E. coli but is inactive against S. aureus and P. aeruginosa at 2000 μg cm−1.Table 6
Antibacterial activity of H2 TPTH and its complexes.
Compound
Bacteria*
Concentration (μg cm−3)
62.5
125
250
500
1000
2000
H2 TPTH
a
(16)+
(27)+
(22)+
(24)+
(23)+
(24)+
b
(9)−
(11)−
(14)−
(16)−
(17)+
(18)+
c
—
—
—
—
—
—
[Mn(H TPTH)2]
a
(9)−
(11)−
(15)−
(17)+
(17)+
(18)+
b
—
—
(9)−
(14)−
(16)−
(18)+
c
—
—
—
—
—
—
[Zn(TPTH)].
a
—
—
—
—
—
—
b
—
—
(10)−
(13)−
(16)−
(17)+
c
—
—
—
—
—
—
[Cu(TPTH)]
a
—
(11)−
(15)−
(16)−
(17)+
(18)+
b
—
(10)−
(12)−
(15)−
(17)+
(17)+
c
(13)−
(14)−
(16)−
(17)+
(18)+
(18)+
*a:  Staph aureus; b: Escherichia coli, c: Pseudomonas aeruginosa. Control: cotrimoxazole. + and −, over the parentheses indicate the zone of inhibition and no zone of inhibition, respectively.


### 3.6. Fungicidal Screening

The antifungal screening results (Table7) show that free H2 TPTH is active from 125 to 2000 μg cm−3 against C. kefri. However, [Mn(H TPTH)2], [Cu(TPTH)], and [Zn(TPTH)] are found to be active even at a lower concentration of 62.5 μg cm−3 against C. kefri. [Zn(TPTH)], [Mn(H TPTH)2] and [Cu(TPTH)] does not show activity at any concentration against  C. albicans.Table 7
Antifungal activity of H2 TPTH and its complexes.
Compound
Fungus*
Concentration (μg cm−3)
62.5
125
250
500
1000
2000
H2 TPTH
a
−
+
+
+
+
+
b
−
−
−
−
−
−
[Mn(H TPTH)2]
a
+
+
+
+
+
+
b
−
−
−
−
−
−
[Zn(TPTH)].
a
−
−
−
−
−
−
b
−
−
−
−
−
−
[Cu(TPTH)]
a
+
+
+
+
+
+
b
−
−
−
−
−
−
*a: Candida kefri; b: Candida albicans. Control: amphotericin B. Growth and  no growth of fungi are represented by  – and + sign, respectively.On the basis of physicochemical studies and the foregoing discussion, the proposed structures of the complexes are shown in Figure2.Figure 2
Proposed structure of the complexes.


## 3.1. Magnetic Moments and Electronic Spectra

The magnetic moments and electronic spectral data of the complexes are given in Tables1 and 2, respectively. [Mn(H TPTH)2] shows a magnetic moment, 5.76 B.M. and exhibits a band at 16140 cm−1 assigned to the A61g→T41g transition for the octahedral geometry [17]. The magnetic moment 5.31 B.M. and presence of bands at 11770 and 20840 cm−1 owing to the T25→B15 and charge-transfer transitions, respectively, suggests a high-spin square pyramidal geometry for [Fe(H TPTH)2(EtOH)]·[Co(TPTH)(H2O)2] shows a magnetic moment of 4.92 B.M. and exhibits a d–d band at 16675 cm−1, assigned to the T41g(F)→T41g(P) (ν3) transition for a distorted octahedral geometry. Ni(TPTH)(H2O)2] exhibits a magnetic moment of 3.06 B.M. and shows a band at 16140 cm−1 attributed to the A32g(F)→T31g(F) (ν2) transition for a distorted octahedral geometry around Ni(II). [Cu(TPTH)] shows a magnetic moment of 1.98 B.M. indicating the presence of one unpaired electron. The complex shows a d–d band at 15635 cm−1 due to the envelope of the B21g→A21g,B22g and E2g transitions, usually observed for square planar Cu(II) complexes [17].Table 2
Electronic spectral bands and their assignments.
Compound
Band maxima (cm−1)
Assignments
H2TPTH
30495, 35220
L
[Mn(H TPTH)2]
16140, 24620
6
A
1g
→
4
T
1g, C.T.
[Fe(H TPTH)2(Et(OH)]
11770, 20840, 24380
5T2→5B1, C.T.
[Co(TPTH)(H2O)2]
16675, 24080
4
T
1g (F) →4T1g (P) (v3), C.T.
[Ni(TPTH)(H2O)2]
16140, 25000
3
A
2g (F) →3T1g (F) (v2), C.T.
[Cu(TPTH)]
15635, 21560, 27790
Envelope of2B1g→2A1g, 2B2g, 2Eg, C.T.
[Zn(TPTH)]
25650
C.T.
[Cd(H TPTH)2]
27035
C.T.
C.T.: charge-transfer; L: intraligand transition.


## 3.2. IR Spectra

The important IR spectral bands and their assignments are given in Table3. The IR spectrum of H2 TPTH shows bands at 3125 and 3100 cm−1 due to the presence of two NH groups. The bands at 1640, 1460, 1325, 1000, and 835 cm−1 are assigned to ν(C=O), thioamide I [β(NH) + ν(CN)], thioamide II [ν(CN) + β(NH)], ν(N–N), and ν(C=S), respectively. The spectra of [Mn(H TPTH)2] and [Fe(H TPH)2(EtOH)] show only one peak at 3125 cm−1 due to ν(NH), suggesting loss of one hydrazinic proton via enolisation/thioenolisation. A strong band at 1640 cm−1 in the ligand due to ν(C=O) is found to be absent in these complexes, and in place of this a new band due to ν(N=C) of NCO appears, suggesting that enolic oxygen is involved in bonding. [Mn(H TPTH)2] shows a negative shift of 15 cm−1 in ν(C=S), suggesting an additional bonding through thione sulfur. Furthermore, the spectra of these complexes show a positive shift of 20 cm−1 in ν(N–N) indicating that one hydrazinic nitrogen is also involved in bonding. The presence of ν(NH) at 3180 cm−1 and ν(C=O) at 1625 cm−1 in [Cd(H TPTH)2] indicates loss of NH proton via thioenolisation. Further, the band at 1460, 1325, and 1000 cm−1 due to thioamide I, II and ν(N–N) undergo positive shifts of 25, 15, and 20 cm−1, respectively, showing the involvement of thiolato sulfur [18] and one hydrazinic nitrogen in bonding.Table 3
Important IR spectral bands (cm−1) and their assignments.
Compound
v(OH)
v(N–H)
v(C=O)/v(NCO)
Thioamide I[β(NH) + v(CN)]
Thioamide II[v(CN) + β(NH)]
Thioamide IVv(C=S)/v(C–S)
v
(N–N)
H2 TPTH
—
3125, 3100
1640
1460
1325
835
1000
[Mn(H TPTH)2]
—
3125
1605
1485
1340
820
1020
[Fe(H TPTH)2(EtOH)]
—
3120
1605
1485
1340
835
1020
[Co(TPTH)(H2O)2]
3425
—
1580
1490
1395
745
1070
[Ni(TPTH)(H2O)2]
3420
—
1580
1490
1395
740
1070
[Cu(TPTH)]
—
—
1585
1490
1400
745
1070
[Zn(TPTH)]
—
—
1585
1490
1395
760
1070
[Cd(H TPTH)2]
—
3180
1625
1485
1340
740
1020The IR spectra of [M(TPTH)(H2O)2] (M = Co(II), Ni(II)) and [M(TPTH)] (M = Cu(II) and Zn(II)) show the absence of both the ν(NH), ν(C=O), and ν(C=S) bands and in place of these two new bands appear at 1580 and 745 cm−1, due to ν(N=C) of NCO and ν(C–S) modes, respectively, suggesting that both –NH–NH protons are lost via enolisation and thioenolisation and bonding of the resulting enolic oxygen and thiolato sulfur takes place with the metal ion. Further, the thioamide I, II, and ν(N–N) bands at 1460, 1325, and 1000 in the free ligand undergo a positive shift of 33, 65, and 70 cm−1, respectively, in the spectra of the complexes [19] suggesting the involvement of these groups as bonding sites. These observations show the involvement of thiolato sulfur and both the hydrazinic nitrogens, in addition to the enolic oxygen in bonding. Thus, H2 TPTH acts as a binegative tetradentate ligand in the 1 : 1 complexes.


## 3.3. NMR Spectra

The1H NMR spectrum of H2 TPTH (Table 4) in DMSO-d6 shows a signal at δ 9.86 and 9.72 ppm due to the presence of –NH–NH– protons which are lost on D2O exchange. The protons due to the thiophene ring appear at δ 7.12 (s, 1H), 7.32 (d, 1H), and 7.56 (s, 1H) ppm and the benzene ring protons appear as a multiplet at at δ 6.64 −6.92(m, 5H) ppm [20].Table 4
1H-NMR data of H2 TPTH and the complexes (δ, ppm).
Compound
Benzene ring
Thiophene ring
NH
H2 TPTH
6.64–6.92 (m, 5H)
7.12 (q, 1H), 7.32 (d, 1H), 7.56 (s, 1H)
9.86 (1H), 9.72 (1H)
[Ni(TPTH)(H2O)2]
6.61–6.88 (m, 5H)
7.08 (s, 1H), 7.28 (d, 1H), 7.52 (s, 1H)
—
[Mn(H TPTH)2]
6.62–6.90 (m, 5H)
7.04 (s, 1H), 7.30 (d, 1H), 7.51 (s, 1H)
9.66The NH signals are absent in the1H NMR spectrum of [Ni(TPTH)(H2O)2], suggesting loss of both NH protons via enolization and thioenolization. The thiophene ring protons show three separate signals at δ 7.08 (q, 1H), 7.28 (d, 1H), and 7.52 (s, 1H) ppm and the benzene ring protons are observed at δ 6.61–6.88 (m,5H) ppm.The1H NMR spectrum of [Mn(H TPTH)2] shows separate signals for the thiophene ring protons at δ 7.04 (s, 1H), 7.30 (d, 1H), and 7.51 (s, 1H) ppm and for benzene ring protons at δ 6.62–6.90 (m, 5H) ppm. The two signals appearing at δ 9.66 and 4.16 ppm are due to the presence of –NH–C(O) and –N=C(SH) protons, respectively. The latter is formed due to the thioenolization of the ligand. All the thiophene and benzene ring protons are observed nearly at the same position in the complex as compared to those of the H2 TPTH, suggesting noninvolvement of the ring sulphur in bonding.The13C NMR spectrum of (H2 TPTH) (Table 5) shows eleven signals, of which two signals at δ 181 and 163 ppm are due to the C=S and C=O carbons, respectively. The chemical shifts for the benzene and thiophene ring carbons in H2 TPTH are (δ, ppm) C′ (2, 6) 151, 146, C′ (4) 136, C′ (3, 5) 126, 122, C (2) 150, C (3) 116, C (4) 112, and C (5) 144.Table 5
13C-NMR data (δ, ppm).
Compound
>C=S
>C=O
C (2, 6)
C (4)
C (3, 5)
C′ (2)
C′ (3)
C′ (4)
C′ (5)
H2 TPTH
181
163
151, 146
136
126, 122
150
116
112
144
[Ni(TPTH)(H2O)2]
188
171
150, 147
134
130, 122
150
116
112
144
[Mn(TPTH)2]
181
174
152, 148
135
128, 123
150
117
112
146The13C-NMR spectrum of [Ni(TPTH)(H2O)2] also shows eleven signals. The chemical shifts for the ring carbons are (δ, ppm) C′ (2, 6) 150, 147, C′ (4) 134, C′ (3, 5) 130, 122, C (2) 150, C (3) 116, C (4) 112, and C (5) 144. The signals at δ 188 and 171 ppm in [Ni(TPTH)(H2O)2] shows downfield shift of 7 and 8 ppm, respectively, as compared to the ligand, suggesting the formation of C–S and C–O groups from the ligand on thioenolization and enolization, respectively.The13C-NMR spectrum of [Mn(H TPTH)2] shows separate signals for all eleven carbons. The chemical shifts for the ring carbons are (δ, ppm) C′ (2, 6) 152, 148 C′ (4) 135, C′ (3, 5) 128, 123, C (2) 150, C (3) 117, C (4) 112, and C (5) 146. The signal at 181 ppm due to C=S carbons show nearly the same chemical shifts as for the ligand, suggesting that the double bond character is retained in the complex. The signals at δ 174 ppm in the complex shows downfield shift of 11 ppm as compared to the ligand, suggesting the the involvement of C=S in bonding.


## 3.4. ESR Spectra

The room temperature solid state ESR spectrum of [Cu(TPTH)] yields a broad signal with〈g〉 value of 2.072 characteristic of square planar geometry around Cu(II).


## 3.5. Bactericidal Screening

The antibacterial activity of H2 TPTH (Table 6) and its complexes have been tested against S. aureus, E. coli, and P. aeruginosa. H2 TPTH shows antibacterial activity starting from 62.5 to 2000 μg cm−3 against S. aureus and the activity increases with an increase in the concentration. The ligand is found to be active at a concentration of 1000 μg cm−3 against E. coli. [Mn(H TPTH)2], and [Cu(TPTH)] show the activity at higher concentration namely 500, 1000, and 2000 μg cm−3 against S. aureus. [Mn(H TPTH)2], [Zn(TPTH)], and [Cu(TPTH)] also show activity against E. coliat 2000 μg cm−3. Only [Cu(TPTH)] has been found active against P. aeruginosa at 500 μg cm−3. [Zn(TPTH)] shows activity against E. coli but is inactive against S. aureus and P. aeruginosa at 2000 μg cm−1.Table 6
Antibacterial activity of H2 TPTH and its complexes.
Compound
Bacteria*
Concentration (μg cm−3)
62.5
125
250
500
1000
2000
H2 TPTH
a
(16)+
(27)+
(22)+
(24)+
(23)+
(24)+
b
(9)−
(11)−
(14)−
(16)−
(17)+
(18)+
c
—
—
—
—
—
—
[Mn(H TPTH)2]
a
(9)−
(11)−
(15)−
(17)+
(17)+
(18)+
b
—
—
(9)−
(14)−
(16)−
(18)+
c
—
—
—
—
—
—
[Zn(TPTH)].
a
—
—
—
—
—
—
b
—
—
(10)−
(13)−
(16)−
(17)+
c
—
—
—
—
—
—
[Cu(TPTH)]
a
—
(11)−
(15)−
(16)−
(17)+
(18)+
b
—
(10)−
(12)−
(15)−
(17)+
(17)+
c
(13)−
(14)−
(16)−
(17)+
(18)+
(18)+
*a:  Staph aureus; b: Escherichia coli, c: Pseudomonas aeruginosa. Control: cotrimoxazole. + and −, over the parentheses indicate the zone of inhibition and no zone of inhibition, respectively.


## 3.6. Fungicidal Screening

The antifungal screening results (Table7) show that free H2 TPTH is active from 125 to 2000 μg cm−3 against C. kefri. However, [Mn(H TPTH)2], [Cu(TPTH)], and [Zn(TPTH)] are found to be active even at a lower concentration of 62.5 μg cm−3 against C. kefri. [Zn(TPTH)], [Mn(H TPTH)2] and [Cu(TPTH)] does not show activity at any concentration against  C. albicans.Table 7
Antifungal activity of H2 TPTH and its complexes.
Compound
Fungus*
Concentration (μg cm−3)
62.5
125
250
500
1000
2000
H2 TPTH
a
−
+
+
+
+
+
b
−
−
−
−
−
−
[Mn(H TPTH)2]
a
+
+
+
+
+
+
b
−
−
−
−
−
−
[Zn(TPTH)].
a
−
−
−
−
−
−
b
−
−
−
−
−
−
[Cu(TPTH)]
a
+
+
+
+
+
+
b
−
−
−
−
−
−
*a: Candida kefri; b: Candida albicans. Control: amphotericin B. Growth and  no growth of fungi are represented by  – and + sign, respectively.On the basis of physicochemical studies and the foregoing discussion, the proposed structures of the complexes are shown in Figure2.Figure 2
Proposed structure of the complexes.


## 4. Conclusion

The magnetic and electronic spectral studies suggest square planar geometry for [Cu(TPTH)], tetrahedral geometry for [Zn(TPTH)] and [Cd(H TPTH)2], and octahedral geometry for the rest of the complexes. The infrared spectral studies of the 1 : 1 deprotonated complexes suggest bonding through enolic oxygen, thiolato sulfur, and both the hydrazinic nitrogens. The ESR spectrum of [Cu(TPTH)] shows that the unpaired electron is present in the dx2-y2 orbital of Cu(II). The ligand H2 TPTH shows antibacterial activity against S. aureus, E. coliandP. aeruginosaand antifungal activity against C. kefriandC. albicans. The complexes Mn(H TPTH)2], [Cu(TPTH)] and [Zn(TPTH)] also show antibacterial activity against the bacteria S. aureus, E. coli, andP. aeruginosaand antifungal activity against the  C. kefriandC. albicans.



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*Source: 721397-2012-10-21.xml*