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American Journal of Applied Sciences
Year: 2009  |  Volume: 6  |  Issue: 4  |  Page No.: 582 - 585

Complexes of 2-Thioacetic Acid Benzothiazole with Some Metal Ions

Emad Yousif, Yang Farina, Khawla Kasar, Abdualbasit Graisa and Kumail Ayid    

Abstract: New metal complexes of the ligand 2-thioacetic acid benzothiazole with the metal ions Ni(II), Cu(II), Zn(II), Cd(II) and Sn(II) were prepared in alcoholic medium. The prepared complexes were characterized by FTIR Spectroscopy, electronic spectroscopy, 1HNMR, 13CNMR, magnetic susceptibility and conductivity measurements. From the spectral measurements, monomer structures for the complexes were proposed. Square planar geometry was proposed for the copper complex. The other complexes were proposed to be tetrahedral.

Preparation of complexes: Addition of ethanol solution of the suitable metal salt (Nickel acetate tetrahydrate, Tin chloride, Copper acetate, Cadmium acetate dihydrate and Zinc acetate dihydrate) to an ethanol solution of 2-thioacetic acid benzothiazole in 2:1 (ligand: metal) molar ratios was carried out. After reflux for half an hour, crystalline colored precipitates formed at room temperature. The rustling solids were filtered off, washed with distilled water, dried and recrystallized from ethanol and dried at 50°C. Table 1 shows the melting point of the prepared compounds.

Instrumentation: Elemental C, H, N and S analysis were carried out on a Fison EA 1108 analyzer, the FTIR spectra in the range (4000-200) cm-1 cut were recorded as CsI disc on FTIR.8300 Shimadzu Spectrophotometer, uv-visible spectra were measured using Shimadzu Uv-vis. 160 A-Ultra-violet Spectrophotometer in the range (200-1000) nm. The magnetic susceptibility values of the prepared complexes were obtained at room temperature using Magnetic Susceptibility Balance of Bruke Magnet B.M.6, Atomic absorption measurements of the prepared complexes were obtained using Shimadzu 680cc-flame.

Table 1: Physical data for preparation ligand and the complexes

The 1H and 13C nuclear magnetic resonance spectra were recorded on a jeol 400 MHz spectrometer in dueteated DMSO, relative to the internal standard Tetramethylsilane (TMS). Melting points were recorded on a hot stage Gallen Kamp melting point apparatus.


Infra-red spectroscopy: The ligand was prepared by the reaction of one mole of 2-mercapto benzothiazole with one mole of chloroacetic acid in presence of KOH.

Table 1 shows the physical data for the ligand and the prepared complexes. The data of CHNS and metal analysis were obtained using flame atomic absorption technique. The calculated values were in a good agreement with the experimental values.

The FTIR spectrum of the ligand, shows a characteristic stretching absorption bands at 3435, 1710, 1573 and 694 cm-1 assigned to hydroxyl, carbonyl, C = N of the thiazole ring and the stretching of C-S group respectively.

The reaction between this ligand with Ni (II), Cu (II), Zn (II), Cd (II) and Sn (II) gave different types of complexes. In the free ligand, the bands at 1710 and 1033 cm-1 were assigned to the stretching of C = O and C-O of the hydroxyl in the carboxylate group. On complexation these bands were shifted to a lower frequency region.

This shift is probably due to the complexation of the metal to the ligand through oxygen of the carbonyl group, the disappearance of the hydrogen from hydroxyl group on complexation indicate the complexation is through the oxygen atom. Stretching of metal-oxygen bands of the complexes appeared in low frequency region (412-440) cm-1[10].

The IR data of the complexes are shown in Table 2. The Table 1ists the stretching frequency (υ) for some of the characteristics groups exhibited by the ligand and complexes.

Table 2: Characteristic absorption bands of 2-thioacetic acid benzothiazole and its complexes

Table 3: Electronic spectra for 2-thioacetic acid benzothiazole and its complexes in DMSO solvent

Ultraviolet-visible spectroscopy: The ultraviolet visible electronic spectrum of the 2-thioacetic acid benzothiazole (LH) in DMSO solvent is recorded in Table 3. Bands at the wavelengths (282, 301 and 328 nm) This transition may be attributed to π→p* electronic transition[11].

The electronic spectra of 2-thioacetic acid benzothiazole complexes showed, as expected, different absorptions from that of the free ligand. In the complexes these bands were shifted to different wavelength than the corresponding bands in the ligand as shown in Table 3, which appears in the wavelength range between 280-381 nm.

The ligand field electronic transitions between the metal d orbital’s appear in Ni (II) and Cu (II) bands located in the visible region at 460 nm for Ni (L)2 assigned to the transition 3A23T1 (p) and 610 nm for Cu (L)2 assigned to the transitions 2B1g→2A1g. The other complexes were diamagnetic as expected for d10 ions so that no (d-d) transition can be expected in the visible region

Magnetic susceptibility and conductivity measurements: The experimental magnetic moment for each metal complexes is listed in Table 4.

Table 4: Magnetic Moment, Conductivity measurements in DMF solvent

Magnetic measurements are widely used in studying transition metal complexes. The magnetic properties are due to the presence of unpaired electrons in the partially filled d-orbital in the outer shell of these elements. These magnetic measurements give an idea about the electronic state of the metal ion in the complex.

The magnetic moment for Ni (II) in any complex is approximately 3.11 B.M., this value refers to a high spin tetrahedral structure, while the value of Cu (II) is approximately 1.44 led to suggest the square planar structure which can become in a good agreement with the data of electronic transitions. Other complexes have no magnetic moment because its diamagnetic. Molar conductivity measurement in DMF solvent at 25ºC showed that the complexes were non-electrolyte[11] Table 4.

NMR spectroscopy: The data of proton NMR of the 2-thioacetic acid benzothiazol and its complexes displayed good solubility in DMSO. The proton nuclear magnetic resonance spectral data gave additional support for the composition of the complexes, Table 5 .The observed changes are evidences of complexion had happened because the chemical shift of a compound is heavily depended on its electronic environment.

The 1HNMR spectrum of the complexes confirmed the disappearance of OH signal at 12.22 ppm in the free ligand. The δ 7.35-8.14 ppm resonance signal protons of the aromatic ring shifted to the higher field upon complexation, while the proton of the -CH2 aliphatic group shifted to higher field also[12].

The 13CNMR of the ligand and its complexes are presented in Table 6. The C = O resonance group of the complexes at 158.46-159.6 ppm where shifted downfield compared with the position in the free ligand which appeared at 196.51 ppm. It is most likely that shift is due to the decrease of electron density at carbon atoms when oxygen is bonded to metalion[12].

Study of complex formation in solution: Complexes of (L) with metal ions were studied in solution using ethanol as a solvent, in order to determine [M/L] ratio in the complex follow Molar ratio method[13].

A series of solutions were prepared having a constant concentration (10-3M) of the metal ion and (L).

Table 5: 1HNMR spectral data(δ,ppm) of the ligand and complexes

Table 6: 13CNMR spectral data (δ,ppm) of the ligand and complexes

The [M/L] ratio was determined from the relationship between the absorption of the absorbed light and the mole ratio of [M/L].The results of complexes formation in solution.

The results of complexes in ethanol, suggest that the metal to ligand ratio was [1/2] for all complexes which were similar to that obtained from solid state Study.

On the basis of the preceding discussion, the structure of the complexes suggested as follows:


The ligand 2-thioacetic acid benzothiazole were successfully synthesized by condensation method. The ligand was treated to different metal salts to afford the corresponding complexes. Square planar geometry was proposed for the copper complex. The other complexes were proposed to be tetrahedral.

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