Journal of Applied ChemistryVolume 2014 (2014), Article ID 529764, 5 pageshttp://dx.doi.org/10.1155/2014/529764

Research Article

Synthesis of Triphenyltin (IV) and Dibutyltin (IV) Complexes of 1-Aryl-2,5-dithiohydrazodicarbonamides and Their Characterization

Rashmi B. Rastogi, Karuna Singh, and Vinay Jaiswal

Department of Chemistry, Indian Institute of Technology (Banaras Hindu University), Varanasi 221005, India

Received 28 October 2013; Accepted 3 February 2014; Published 5 March 2014

Academic Editor: Guennadi E. Zaikov

Copyright © 2014 Rashmi B. Rastogi et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract.

Organotin complexes of the types Ph₃SnL and Bu₂SnL [where Ph = phenyl and Bu = butyl; HL = 1-phenyl-2,5-dithiohydrazodicarbonamide (HPhthc), 1-benzyl-2,5-dithiohydrazodicarbonamide (Hbzthc), 1-(4-ethoxyphenyl)-2,5-dithiohydrazodicarbonamide (HEtOPhthc)] have been prepared. Molar conductance studies demonstrate the nonionic behavior of the complexes. The ¹H and ¹³C nuclear magnetic resonance and FAB mass spectra of the complexes are consistent with the proposed stoichiometry. Infrared spectra suggest an anionic bidentate coordinating behavior of the ligands.

1. Introduction

Dithiohydrazodicarbonamides have proved to be compounds of versatile behavior. This particular ligand system and its 3d metal complexes have been shown to possess high antimicrobial activity [1, 2]. Anticorrosion properties of these ligands have also been recognized for the corrosion of copper in aqueous chloride solutions [3]. Some 1-aryl-2,5-dithiohydrazodicarbonamides and their molybdenum and tungsten complexes have been found to act as excellent extreme-pressure lubrication additives [4] and corrosion inhibitors for mild steel in 1.0 N sulfuric acid [5]. Biocidal activity of organotins is well recognized [6–8]. These have been enormously used as antifouling paints [9, 10]. Organotins derived from carboxylic acid, phosphoric group, N, S donating groups have been studied as corrosion inhibitors [11–22]. Organotins are known for their friction and wear reducing properties [23–25]. Organotin derivatives of alkylphenols have been successfully used as antiwear additives for lubricating oils [26]. Since organotins and dithiohydrazodicarbonamides both are well known for their biocidal behavior, friction and wear reducing properties and anticorrosive properties, synthesis of organotin complexes with dithiohydrazodicarbonamides was undertaken with intent to explore their applicability as corrosion inhibitors. The present communication, therefore, describes the synthesis of some triphenyltin and dibutyltin dithiohydrazodicarbonamides and their characterization by infrared, proton, and ¹³C nuclear magnetic resonance spectroscopy and FAB mass spectrometry.

2. Experimental

2.1. Materials

Analytical grade reagents were used in the present investigation. The ligands were prepared by refluxing thiosemicarbazide with appropriate aryl isothiocyanates in 50% ethanol using previously reported methods [27]. In a representative experiment 1-phenyl-2,5-dithiohydrazodicarbonamide was synthesized as given below.

Thiosemicarbazide (0.05 moL) and phenyl isothiocyanate (0.05 moL) were mixed with 50 mL of 50% ethanol and the mixture was refluxed for one hour. The solid that appeared was filtered, washed with water, and crystallized from ethanol, m.pt. 174°C.

The structures of dithiohydrazodicarbonamides used for preparation of complexes are given in Figure 1.

Figure 1: Structures and acronyms of the various dithiohydrazodicarbonamides.

2.2. Preparation of the Complexes

2.2.1. Triphenyltin Complexes

To an ethanolic solution of triphenyltin chloride (3.8 g, 10 mmoL), an ethanolic solution of the corresponding ligand (10 mmoL) was added with constant stirring. The reaction mixture was stirred at solvent reflux for 4 hrs and excess solvent was removed by distillation at reduced pressure. On addition of excess of petroleum ether to the residual liquid, a dirty-white solid precipitated. The solvent was removed by evaporation and the residual solid was dried at reduced pressure. It was then recrystallized from acetone.

2.2.2. Dibutyltin Complexes

Dibutyltin complexes were synthesized by adding dropwise an ethanolic solution of dibutyltin dichloride (3.04 g, 10 mmoL) to a stirred ethanolic solution of the corresponding ligand (20 mmoL). The reaction mixture was stirred at solvent reflux for 3 hrs and the excess solvent was removed by distillation at reduced pressure. The residual liquid was allowed to cool to room temperature. Upon the addition of excess petroleum ether (b.p. 60–80°C), a solid product formed. The solid was collected by filtration, washed with ethanol, and dried at reduced pressure. It was then recrystallized from acetone.

3. Instrumentation

Electrical conductance of 10−3 M solutions of the complexes in DMSO was measured at room temperature using an inversion-type special conductivity cell with a bright platinum electrode (WTW model LBR/B). Infrared spectra were obtained using a Perkin Elmer 983 spectrophotometer. ¹H and ¹³C NMR spectra were recorded using a Jeol FX Fourier Transform Multinuclear NMR spectrometer and solutions in DMSO-d₆ using tetramethylsilane as internal reference. FAB mass spectra were recorded using a Jeol SX 6000 mass spectrometer and xenon/6 KV/10 mA as the FAB gas and NBA m-nitrobenzyl alcohol as matrix. Powder X-ray diffraction (XRD) data of the complexes were recorded at room temperature using a Rigaku Cu-rotating anode (Japan) X-ray diffractometer operating at 40 KV and 100 mA at 1.5406 Å wavelength (Cu-K radiation).

4. Result and Discussion

The complexes were analyzed for their tin, sulfur, hydrogen, carbon, and nitrogen contents. Tin and sulfur were determined gravimetrically as SnO₂ and BaSO₄, respectively [28]. Carbon, hydrogen, and nitrogen were determined microanalytically. The analytical data together with molar conductance values are given in Table 1. As indicated by analytical data, the complexes of the types Ph₃SnL and Bu₂SnL₂ where [LH = HPhthc, Hbzthc, HEtOPhthc] are formed. All the complexes are soluble in common organic solvents. The molar conductance values of all the complexes are in the range 9–15.5 ohm−1 moL−1 cm² which shows them to be nonionic [29].

Table 1: Analytical data and behavior of organotin (IV) dithiohydrazodicarbonamide complexes.

Complex empirical formula
Color
Anal. %
Found (calculated)
Molar conductance 10⁻³ M in DMSO (ohm⁻¹ mol⁻¹ cm²)

C
H
N
S
Sn

Ph₃Sn(Phthc)C₂₆H₂₄N₄S₂Sn
Pale white
54.73 (54.35)
4.21 (4.18)
9.82 (9.75)
11.22 (11.14)
20.70 (20.55)
10.90

Bu₂Sn(Phthc)₂ C₂₄H₃₆N₈S₄Sn
Pinkish white
42.35 (42.22)
5.29 (5.27)
16.47 (16.42)
18.82 (18.76)
17.35 (17.30)
15.50

Ph₃Sn(Bzthc)C₂₇H₂₆N₄S₂Sn
White
55.91 (55.10)
4.40 (4.42)
9.49 (9.52)
10.84 (10.88)
20.01 (20.06)
9.63

Bu₂Sn(Bzthc)₂EtC₂₆H₄₀N₈S₄Sn
Dirty white
44.08 (43.94)
5.64 (5.63)
15.81 (15.77)
18.07 (18.02)
16.66 (16.61)
14.70

Ph₃Sn(EtOPhthc)C₂₈H₂₈N₄OS₂Sn
Cream
54.45 (54.19)
4.86 (4.83)
9.07 (9.03)
10.37 (10.32)
19.12 (19.03)
6.15

Bu₂Sn(EtOPhthc)₂ C₂₈H₄₄N₈O₂S₄Sn
White
43.86 (43.63)
5.74 (5.71)
14.62 (14.54)
16.71 (16.62)
15.40 (13.32)
9.61

4.1. Infrared Spectra

Prominent IR spectral bands and the corresponding assignments are displayed in Table 2. The IR spectrum of the ligand 1-phenyl-2,5-dithiohydrazodicarbonamide (HPhthc) exhibits four bands at 3420, 3390, 3210, and 3150 cm⁻¹ which are assigned to (N–H), (NH₂), (NH) (ArNH₂) and (N–H) (–NH–NH–), respectively [1]. These bands appear at 3400, 3380, 3220, and 3140 cm⁻¹, respectively, in HEtOPhthc and at 3410, 3370, 3250, and 3180 cm⁻¹, respectively, in Hbzthc. The position of the first two bands is almost unaffected by complexation indicating that the primary amino (–NH₂) nitrogen is not involved in the coordination. Upon complexation, the third band of the ligands becomes broad and the fourth band is absent suggesting that at least one of the >NH groups is involved in coordination and formation of the complexes. The β(NH₂) and (N–N) absorption bands of strong intensity in the spectra of the ligand appearing at 1600–1640 and 980 cm⁻¹, respectively, show lower and higher energy shifts of 10–20 and 20–40 cm⁻¹, respectively, on complexation indicating that one of the hydrazinic nitrogen atoms is involved in coordination [1]. The thioamide band I [β(NH) + (CN)] and thioamide band II [(CN) + β(NH)] appearing for the ligands at approximately 1500 and 1300 cm⁻¹, respectively, undergo shifts of higher energy 20–90 cm⁻¹ upon complexation due to the reduction of the >C=S bond order from two to one and an increase in the >C–N bond order from one to two as a result of thioenolisation.

Table 2: IR spectral bands (cm⁻¹) and their assignments.

Complex
(N–H)
(NH₂)
[(N–H) + (CN)] Thiomide I
[ (CN) + (N–H)] Thiomide II
[ (C=S)/C–S)] Thiomide IV
(NH₂)
(Sn–C)
(Sn–S)
(Sn–N)
ν (N–N)

HPhthc
34203390
32103150
1500
1300
840
1640
—
—
—
980

Ph₃Sn(Phthc)
34103380
32003150
1555
1385
770
1650
600
384
354
1005

Bu₂Sn((Phthc))₂
34003364
31803140
1560
1390
760
1645
590
370
360
1010

HEtOPhthc
34003380
32203140
1520
1300
810
1610
—
—
—
960

Ph₃Sn(EtOPhthc)
33903370
32103120
1570
1365
720
1605
585
380
340
980

Bu₂Sn(EtOPhthc)₂
34003360
32203110
1580
1360
710
1610
610
397
350
985

HBzthc
34103370
32503180
1510
1320
880
1600
—
—
—
900

Ph₃Sn(Bzthc)
34003365
32403160
1535
1380
805
1590
617
390
310
940

Bu₂Sn(Bzthc)₂
34003360
32503150
1540
1370
810
1580
605
380
315
950

The position of absorption for the thioamide IV bands appearing at 880–840 cm⁻¹ in the ligands remains almost unchanged in the spectra of the complexes and a new band around 810–770 cm⁻¹ due to the (C–S) stretching vibration is present, suggesting that one of the >C=S groups is not involved in the coordination. The appearance of a new band in the region 810–770 cm⁻¹ in the spectra of the complexes indicates that coordination of the metal through the “thiolo” sulfur has occurred.

New bands appearing in the far-IR spectra of all the complexes in the region 580–620, 310–360, and 370–390 cm⁻¹ may be tentatively assigned to (Sn–C), (Sn–N), and (Sn–S) modes, respectively [28].

4.2. ¹H NMR Spectra

¹H NMR spectrum of the ligand HPhthc recorded in DMSO-d₆ exhibits D₂O exchangeable resonance signals at δ 9.93 (–NH–NH) and δ 2.36 (s, –NH₂) ppm. Aromatic protons, together with the –NH proton, are observed as a multiplet between δ 7.74 and 7.06 ppm. However, the complexes of the ligand HPhthc show a –NH–NH proton signal at δ 9.70 ppm due to one proton only, supporting the view that one proton has undergone deprotonation after thioenolisation to form the complex. Other proton signals of the ligand appear at more deshielded positions in the complexes. The electronic environment around these protons has changed to some extent as a consequence of complexation.

4.3. ¹³C NMR Spectra

The ¹³C NMR spectrum of HBzthc displays resonance signals between δ 120.0 and 131.8 ppm corresponding to the carbon atoms of the benzyl group and a single peak at δ 170.6 and δ 171.3 ppm due to >C=S carbon atoms. The spectra of Ph₃SnPhthc and Bu₂Sn(Phthc)₂ indicate greater deshielding of the >C=S carbon as compared to the ligand which may arise due to the presence of –N=C–S from –HN–C=S after the removal of proton upon thioenolisation.

4.4. FAB Mass Spectra

The FAB mass spectrum of Ph₃SnPhthc shows several peaks due to various fragments resulting from its ionization. The presence of a prominent peak at m/z = 226 for the ligand HPhthc and an intense molecular ion peak at m/z = 570 (−4H⁺), (59) reflects its monomeric nature. The spectrum of Bu₂Sn(EtOPhthc)₂ contains a low intensity peak at m/z = 766 (−4H⁺), (11) which corresponds to the molecular ion peak of complex.

Based on analytical data and the physicochemical studies noted, structures for the proposed complexes have been proposed. These structures are shown in Figure 2.

Figure 2: Proposed structure of organotin (IV) complexes.

Conflict of Interests

The authors declare that there is no conflict of interests regarding the publication of this paper.

Acknowledgments

The financial assistance from All India Council of Technical Education, New Delhi, is gratefully acknowledged. The authors are thankful to Head, Department of Chemistry, Faculty of Science, Banaras Hindu University, for providing IR and NMR facilities.

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