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Journal of the Brazilian Chemical Society

versão impressa ISSN 0103-5053

J. Braz. Chem. Soc. v.10 n.3 São Paulo  1999

http://dx.doi.org/10.1590/S0103-50531999000300005 

Article

 

Nickel(II), Copper(I) and Copper(II) Complexes of Bidentate Heterocyclic Thiosemicarbazones

 

Rejane Lúcia de Lima, Letícia Regina de Souza Teixeira, Tania M. Gomes Carneiro, and Heloisa Beraldo*

Departamento de Química, Universidade Federal de Minas, 31270-901 Belo Horizonte - MG, Brazil

 

 

Complexos de tiossemicarbazonas derivadas de 3- e 4-formilpiridina (H3FPT e H4FPT) e 3- e 4-acetilpiridina (H3APT e H4APT) com níquel(II) e cobre(I) ou cobre(II) foram preparados e caracterizados através de microanálises, medidas de condutividade molar e susceptibilidade magnética e por meio de seus espectros de infravermelho e de R.M.N., no caso dos complexos de cobre(I) e dos complexos diamagnéticos de níquel(II).

 

Nickel(II) and copper(I) or copper(II) complexes of thiosemicarbazones derived from 3- and 4-formylpyridine (H3FPT and H4FPT) and 3- and 4-acetylpyridine (H3APT and H4APT) have been prepared and characterized by microanalyses, molar conductivity and magnetic susceptibility measurements and by their NMR (in the case of copper(I) and diamagnetic nickel(II) complexes) and IR spectra.

Keywords: heterocyclic thiosemicarbazones, bidentate thiosemicarbazones, nickel(II), copper(I), copper(II)

 

 

Introduction

Thiosemicarbazones and their metal complexes are a broad class of biologically active compounds1. Metal complexes of N-heterocyclic thiosemicarbazones derived from 2-formylpyridine (H2FPT) and 2-acetylpyridine (H2APT) were extensively described in the literature2, but very few works deal with those derived from 3- and 4-formylpyridine (H3FPT, H4FPT, Fig. 1) and 3- and 4-acetylpyridine (H3APT, H4APT, Fig. 1). In some cases, lowering of the thiosemicarbazone’s denticity leads to a decrease of activity2 but the literature reports examples of biologically significant bidentate thiosemicarbazones. The compound p-acetamidobenzaldehyde thiosemicarbazone, for example, known as thioacetazone, is employed in the clinical treatment of tuberculosis3 and functions as a potential N-S bidentate ligand. In previous works we studied the iron(II), iron(III), copper(II) and zinc(II) complexes of H2FPT and H2APT4-7. In the present article we report the syntheses and characterization of complexes of H3FPT, H4FPT, H3APT and H4APT with nickel(II), and copper(I) or copper(II).

 

 

Experimental

IR spectra were recorded by means of a Perkin Elmer 283B spectrometer using Nujol mulls between CsI plates and NMR spectra with a Brucker DRX-400 Avance (400 MHz) spectrometer. The thermogravimetric data were obtained in dynamic air atmosphere at 10 °C/min in the 25 - 750 °C range, by using a Mettler TA 4000 TG50 analyzer. A YSI model 31 conductivity bridge was employed for molar conductivity measurements. The magnetic susceptibilities of the solids were measured at room temperature with a Johnson Matthey Magnetic Susceptibility balance. Partial elemental analyses were performed using a Perkin Elmer 240 equipment.

H3FPT, H4FPT, H3APT and H4APT were obtained by refluxing an ethanolic solution of 3- or 4-formylpyridine and 3- or 4-acetylpyridine with thiosemicarbazide (all purchased from Aldrich Chemical Company and used without purification) as described in the literature8. The complexes were prepared by refluxing ethanolic solutions of the thiosemicarbazone and the metal(II) perchlorate in molar ratio M:L 1:2 during 5-6 h. In the case of H3APT and H4APT the reaction with copper(II) perchlorate gave the copper(I) complexes (vide infra). The solids that formed on cooling were filtered off, washed with ethanol then ether and dried. The yields were 50 - 65% in the case of the nickel(II) complexes, 66 - 70% in the case of the copper(I) complexes and 56% in that of the copper(II) complexes.

 

Results and Discussion

Table 1 lists the colors, partial elemental analyses and molar conductivities of the nickel(II), copper(I) and copper(II) complexes. Thiosemicarbazones can coordinate metal ions as neutral ligands (HTSC) or as anionic species (TSC) upon deprotonation at the N(2’)4,5,7.

 

 

The C, H, N data indicate that the copper(II) complexes of H3FPT and H4FPT present two anionic bidentate ligands per metal ion, as supported by their behavior as non-electrolytes, and their geometry is probably square planar. In contrast, both H3APT and H4APT form copper complexes in which only one neutral ligand is coordinated to the metal ion and the other coordination positions are occupied by water molecules, as confirmed by the IR spectra of the complexes (vide infra). However, in these cases the compounds are diamagnetic, suggesting reduction of copper(II) to copper(I), consistent with their yellow color and with the presence of one perchlorate as counterion in both complexes. In previous works we demonstrated that H2FPT acts as a reducing agent of its own iron(III) complex6. The occurrence of a similar effect may now be suggested. The protonation of the ligand in the complexes was confirmed by the presence of 1H-NMR signals at d = 10.503 and d = 11.967, assigned to the N(2’)-H protons hydrogen-bonded to the DMSO solvent molecules9 (see Table 2). Also, the acetyl protons which give a signal at d = 2.313 and d = 2.329 in the spectra of H3APT and H4APT respectively are shifted to higher frequency (d = 2.391 and d = 2.484 respectively) in the spectra of the copper(I) complexes due to coordination through N(1’), as observed in the literature10. Microanalyses indicate that the copper(I) complex with H3APT presents two coordinated water molecules, whereas that with H4APT presents a total of six water molecules, which are coordinated and crystallization water, as confirmed by the infrared data (vide infra), but it is not possible to determine the number of water molecules of each type in that complex. Although the loss of water does not appear separately in the thermograms of both complexes, thermogravimetric data show a residue of CuO corresponding to 18.8% (calcd. 20.3%) and to 18.3% (calcd. 17.1%) for the copper(I) complexes of H3APT and H4APT respectively, in agreement with the proposed formulations. In this case, reoxidation of copper(I) to copper(II) during the thermogravimetric measurements probably occurs.

 

 

C,H,N analyses suggest that H3FPT and H4FPT form 2:1 ligand-to-metal complexes with nickel(II), in which one of the ligands is neutral and the other anionic, similar to an iron(III) complex of 2-acetylpyridine thiosemicarbazone obtained by us in a previous work11. The molar conductivity measurements indicate that both complexes are 1:1 electrolytes, consistent with the presence of the perchlorate bands in the infrared spectrum (vide infra). The complex [Ni(H4FPT)(4FPT)]ClO4 is diamagnetic, suggesting square planar geometry but in the case of [Ni(H3FPT)(3FPT)]ClO4 the measured magnetic susceptibility of 3.0 BM is close to the theoretical value of 2.83 BM of tetrahedral arrangement. The 1H-NMR spectrum of the former shows a peak at d = 11.398, assigned to the protonated ligand’s N(2’)-H hydrogen bonded to DMSO9. Also, the signal at d = 7.992 in the spectrum of H4FPT, assigned to the formyl proton, is shifted to higher frequency (d = 7.998) upon coordination of the azomethine nitrogen N(1’). H3APT and H4APT form 3:1 ligand-to-metal complexes with nickel(II), of octahedral geometry. Microanalyses of these complexes suggest the presence of two protonated and one deprotonated bidentate ligands, which was also confirmed by the 1:1 electrolyte behavior of both complexes and by the presence of perchlorate absorptions in the IR spectrum. Although the NMR signals are broad for the paramagnetic nickel(II) complexes preventing reliable integration, the presence of resonances at d = 11 - 12 (data not shown), characteristic of the N(2’)-H protons hydrogen bonded to DMSO9 confirms that at least one of the ligands is protonated.

The assignments of the IR bands useful for determining the ligand’s mode of coordination are listed in Table 3. The bands in the region 3160 - 3440 cm-1, attributed to the symmetrical stretching mode n(NH2) in the spectra of the ligands, shift to 3460 - 3210 cm-1 in those of the complexes, as a consequence of the coordination of the sulfur from the C=S(NH2) group, as observed by other authors12. The n(C=N) bands of the thiosemicarbazones at ca. 1590 cm-1 shift to 1625 - 1565 cm-1 in the spectra of the complexes, indicating coordination of the azomethine nitrogen N(1’) in agreement with previous studies13. The uncomplexed thiosemicarbazones show the thioamide IV band, which possesses considerable contribution from n(CS), in the 800 - 825 cm-1 range. This band shifts 45 to 110 cm-1 to lower energy when coordination occurs with deprotonation at N(2’) and formation of a single C-S bond11. The shift is 5 to 25 cm-1 to lower frequencies when the thiosemicarbazones coordinate the metal in the neutral form11. Bands in the 355 - 395 cm-1 region are assigned to n(M-S) and those at 435 - 485 cm-1 region to n(M-N) vibrations13, supporting the coordination of all ligands as bidentate N-S chelating agents. In the spectra of [Cu(H3APT)(H2O)2]ClO4 and [Cu(H4APT)(H2O)n]ClO4.(6-n)H2O there are bands at 3315, 1630, 605 and 420 cm-1 and at 3420, 1625, 595 and 430 cm-1 respectively, attributable to n(OH), d(OH2), pw(OH2) and nCu-O of coordinated water13. Furthermore, the IR spectrum of [Cu(H4APT)(H2O)n]ClO4.(6-n)H2O shows broad absorptions in the region 3600 - 3200 cm-1 characteristic of crystallization water14. Finally, a strong, broad absorption band, which is characteristic of n3 of ionic perchlorate15 is observable in the spectra of [Cu(H3APT)(H2O)2]ClO4, [Ni(H3FPT)(3FPT)]ClO4 and [Ni(H4FPT)(4FPT)]ClO4 at about 1070 cm-1. Also, n4(ClO4) is present as a sharp shoulder at 620 cm-1 and a weak band at 946 cm-1 may be due to n1(ClO4), suggesting that the ionic perchlorate is distorted from tetrahedral symmetry due to lattice effects or hydrogen bonding by the coordinated ligand’s NH functions. In contrast, [Cu(H4APT)(H2O)n]ClO4.(6-n)H2O, [Ni(H3APT)2(3APT)]ClO4 and [Ni(H4APT)2(4APT)]ClO4 show a much sharper band for n3(ClO4), a sharp band for n4(ClO4) and no indication of n1(ClO4) suggesting minimal distortion from tetrahedral symmetry.

 

 

In the present work a variety of metal complexes of heterocyclic bidentate thiosemicarbazones were prepared and characterized. Copper(II) complexes of 3- and 4-formylpyridine thiosemicarbazone present two deprotonated ligand molecules per metal ion. The reaction of 3- and 4-acetylpyridine thiosemicarbazone with the copper(II) salt leads to the formation of copper(I) complexes in which the thiosemicarbazones coordinate as protonated neutral ligands, in accordance with the lower acidity constant of the acetyl derivatives, due to the electron donor inductive effect of their methyl group7. Moreover, 3- and 4-formylpyridine thiosemicarbazone coordinate nickel(II) forming 2:1 ligand-to-metal complexes having one protonated and one deprotonated ligand, of tetrahedral geometry in the first case and of square planar geometry in the latter. The thiosemicarbazones derived from 3- and 4-acetylpyridine form octahedral nickel(II) complexes of the ML3 type, in which two ligand molecules are protonated and one is deprotonated. At this stage it is worth comparing the structures of the metal complexes of 2-formyl and 2-acetylpyridine thiosemicarbazone with those of the corresponding 3- and 4- analogs. In the former the presence of the tridentate chelating N-N-S system normally favors the formation of 1:1 complexes with copper(II) of approximately square planar geometry2. In contrast, the bidentate (3- and 4-) thiosemicarbazones form copper(II) complexes with 2:1 ligand-to-metal ratios. The 2-formyl and 2-acetylpyridine thiosemicarbazones, as well as their 3- and 4- analogs form nickel(II) complexes with a variety of geometries and different ligand-to-metal ratios but only the 2- (i.e. a) thiosemicarbazones can form ML2 complexes of octahedral geometry upon coordination of the tridentate N-N-S ligand1. To our knowledge the literature does not report many examples of copper(I) complexes of 2-formyl and 2-acetylpyridine thiosemicarbazone for us to establish comparisons with the 3- and 4- analogs.

In conclusion, changing the point of attachment of the lateral chain in relation to the heteroaromatic nitrogen from the 2- (i.e. a) to the 3- or 4- (i.e. b or g) positions and the nature of the pyridine starting reagent (formyl or acetyl) may have influence in the structure of the metal complexes obtained and the structural differences probably affect the biological activity of these compounds.

 

Acknowledgements

The authors acknowledge support for their work from CNPq, Capes and Fapemig. Helpful suggestions from professor Douglas X. West are acknowledged.

 

References

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2. West, D.X.; Padhye, S.B.; Sonawane, P.S. Structure and Bonding 1991, 76, 1 and references therein.         [ Links ]

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4. Beraldo, H.; Tosi, L. Inorg.Chim.Acta 1983, 75, 249.         [ Links ]

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9. West, D.X.; Stark, A.M.; Bain, G.; Liberta, A .E. Trans.Met.Chem. 1996, 21, 289.         [ Links ]

10. Kovala-Demertzi, D.; Domopoulou, A.; Demetzis, A.; Valdez-Martinez, J.; Hernadez-Ortega, S.; Espinosa-Perez, G.; West, D.X.; Salberg, M.; Bain, G.; Bloom, P.D. Polyhedron 1996, 15, 2587.         [ Links ]

11. Borges, R.H.U.; Beraldo, H.; Abras, A . J. Braz. Chem. Soc. 1997, 8, 33.         [ Links ]

12. El-Sawaf, A.K.; West, D.X.; El-Saied, F.A.; El-Bahnasawy, R.M. Inorg. Met.-Org. Chem. 1997, 27, 1127.         [ Links ]

13. Beraldo, H.; Boyd, L.P.; West, D.X. Trans.Met.Chem. 1988, 23, 67 and references therein.         [ Links ]

14. Chasan, D.E.; Pytlewski, L.L.; Karyannis, N.M.; Owens, C. J. Inorg. Nuclear Chem. 1978, 40, 1019.         [ Links ]

15. Nakamoto, K. In Infrared and Raman Spectra of Inorganic and Coordination Compounds, Wiley Interscience Publication, John Wiley & Sons, Inc.; New York, p. 251, 1986.         [ Links ]

 

Received: November 13, 1998