Synthesis, Spectroscopy, Theoretical, and Electrochemical Studies of Zn(II), Cd(II), and Hg(II) Azide and Thiocyanate Complexes of a New Symmetric Schiff-Base Ligand

Montazerozohori, Morteza; Nozarian, Kimia; Ebrahimi, Hamid Reza

doi:https://doi.org/10.1155/2013/718149

Journal of Spectroscopy

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Research Article | Open Access

Volume 2013 | Article ID 718149 | https://doi.org/10.1155/2013/718149

Synthesis, Spectroscopy, Theoretical, and Electrochemical Studies of Zn(II), Cd(II), and Hg(II) Azide and Thiocyanate Complexes of a New Symmetric Schiff-Base Ligand

Morteza Montazerozohori,¹Kimia Nozarian,¹and Hamid Reza Ebrahimi²

Academic Editor: Feride Severcan

Received19 Jun 2012

Revised18 Sept 2012

Accepted19 Sept 2012

Published10 Nov 2012

Abstract

Synthesis of zinc(II)/cadmium(II)/mercury(II) thiocyanate and azide complexes of a new bidentate Schiff-base ligand (L) with general formula of MLX₂ (M = Zn(II), Cd(II), and Hg(II)) in ethanol solution at room temperature is reported. The ligand and metal complexes were characterized by using ultraviolet-visible (UV-visible), Fourier transform infrared (FT-IR), ¹H- and ¹³C-NMR spectroscopy and physical characterization, CHN analysis, and molar conductivity. ¹H- and ¹³C-NMR spectra have been studied in DMSO-d₆. The reasonable shifts of FT-IR and NMR spectral signals of the complexes with respect to the free ligand confirm well coordination of Schiff-base ligand and anions in an inner sphere coordination space. The conductivity measurements as well as spectral data indicated that the complexes are nonelectrolyte. Theoretical optimization on the structure of ligand and its complexes was performed at the Becke’s three-parameter hybrid functional (B3) with the nonlocal correlation of Lee-Yang-Parr (LYP) level of theory with double-zeta valence (LANL2DZ) basis set using GAUSSIAN 03 suite of program, and then some theoretical structural parameters such as bond lengths, bond angles, and torsion angles were obtained. Finally, electrochemical behavior of ligand and its complexes was investigated. Cyclic voltammograms of metal complexes showed considerable changes with respect to free ligand.

1. Introduction

Schiff bases are very important class of ligands in coordination chemistry due to the wide applications of them in synthesis of a large variety of transition-metal complexes with various structural architectures [1–5]. These ligands are often prepared in suitable yields and purity during direct reaction between aldehyde or ketone and primary aromatic and/or aliphatic amines. In situ complexation reaction is another common method for synthesis of these compounds [6, 7]. Schiff-base transition metal complexes have been found to show attractive properties and applications. For example, some salen-type complexes have been found as interesting catalyst in organic synthesis [8–11]. Also some Schiff-base coordination compounds have shown interesting magnetic properties [12], a DNA-hydrolytic character [13], antibacterial behavior [14], nonlinear optical [15], and fluorescence properties [16]. In addition, in recent years, some transition metal complexes of Schiff bases have also been presented as building blocks in supramolecular assemblies [17]. Furthermore, a special literature survey on zinc, cadmium, and mercury complexes well confirms the wide utility of them in various fields of chemistry and biochemistry. Some complexes of above metal ion showed antibacterial activities [18–20]; antifungal activities [21]; antitumor and cytotoxic activities [22]. Several zinc enzymes have been found in which geometry around the zinc ion as active site is tetrahedral [23]. Some zinc(II) and cadmium Schiff-base complexes have been known as effective emitting layers, luminescent, fluorescent, and electroluminescent materials [24–27]. Zinc complexes can be used as Lewis-acid catalyst in organic synthesis [28]. A report has shown that cadmium and mercury Schiff-base complexes have an acceptable potential for inhibition of corrosion [29]. Recently in analytical chemistry point of view, we reported the utility of zinc, cadmium, and mercury Schiff-base complexes for construction of some ion selective electrodes [30, 31]. This variety of possible applications of IIB metal complexes especially with various Schiff-base ligands and geometries conducted us to develop the synthesis of new coordination compound of zinc group. As a part of our continuing studies on symmetric bidentate Schiff bases including N-atom donors and their IIB metal ions complexes [30–37] and due to the importance of Zn Cd and Hg complexes in chemistry and biochemistry as mentioned above, herein our aim is the synthesis and characterization of new zinc(II), cadmium(II), and mercury complexes of a novel -Schiff-base ligand; N,N′-bis((E)-3-(2-nitrophenyl)allylidene)propane-1,3-diamine. Then, theoretical modeling and electrochemical behavior of the ligand and its new complexes are described with respect to each other.

2. Experimental

2.1. Materials and Methods

All solvents and chemicals used in synthesis and analysis were provided from Aldrich, Merck, and/or BDH companies. Metal thiocyanate and azide salts were freshly prepared according to our previous report [32]. IR spectra were recorded on a JASCO FT/IR-680 spectrometer in the range of 4000–400 cm⁻¹ as KBr pellets. ¹H- and ¹³C-NMR spectra were recorded on a Bruker DPX FT-NMR spectrometer at 500 MHz in DMSO-d₆ solvent. Chemical shifts (δ) are reported in part per million (ppm) relative to an internal standard of TMS. Elemental analyses for carbon, hydrogen, and nitrogen were carried out on a CHN elemental analyzer. Molar conductivities of the Schiff-base complexes were measured in DMSO (10⁻³ M) at room temperature by the use of Metrohm 712 conductometer with dip-type conductivity cell made of platinum black. Melting points (°C) were recorded on a BUCHI melting point B-545 instrument in open capillary tubes. Electronic spectra were recorded in DMF solution on a JASCO-V570 model spectrometer in the range of 200–800 nm. All cyclic voltammograms were obtained by a SAMA500 CV instrument including a cell containing three electrodes: glassy carbon as working, platinum disk as supporting, and silver wire as reference electrodes. Scan rate was of 0.1 V/S. Cyclic voltammetry recording was performed on the solutions of ligand and its complexes in dry acetonitrile as well as tetrabutylammonium hexafluorophosphate as supporting electrolyte at room temperature.

2.2. Synthesis of the Schiff-Base Ligand (L)

The ligand of N,N′-bis((E)-3-(2-nitrophenyl)allylidene)propane-1,3-diamine has been synthesized by the reaction between 2-nitrocinnamaldehyde (2 mmol, 0.354 g) and propane-1,3-diamine (1 mmol, 0.074 g) in ethanol under severe stirring for 4 h. The yellowish solution so obtained was subjected to evaporation for obtaining yellowish white precipitate. Then, the product was recrystallized from dichloromethane to afford the pure Schiff base in 76% yield. %C₂₁H₂₀N₄O₄: calc. C, 64.28%; H, 5.14%; N, 14.28%; found: C, 63.7%; H, 5.3%; N, 14.6%. Characteristic FT-IR and UV-visible spectral data have been summarized in Table 1. ¹H NMR (DMSO-d₆): 8.17 (d, 2H, J = 8.40 Hz), 8.02 (d, 2H, J = 8.40 Hz), 7.96 (d, 2H, J = 7.60 Hz), 7.45 (t, 2H, J = 7.60, J = 7.20 Hz), 7.61 (t, 2H, J = 8.00 Hz, J = 7.60 Hz), 7.38 (d, 2H, J = 15.60 Hz), 6.98 (dd, 2H, J = 16.00 Hz, J = 8.80 Hz), 3.56 (t, 4H, J = 6.80 Hz), 1.90 (q, 2H, J = 6.80 Hz) ppm. ¹³C NMR (DMSO-d₆): 162.85, 148.44, 135.70, 134.07, 133.00, 130.70, 130.32, 128.92, 125.00, 59.04, 32.24 ppm. m.p. = 163°C; (DMF) = 2.53 cm² Ω⁻¹ M⁻¹.

2.3. Synthesis of Metal Complexes

All Schiff-base complexes were synthesized by gradual addition of ethanolic solution of ligand (0.5 mmol) to solution of metal (II) thiocyanate or azide salts in ethanol. The mixture was stirred for 2-3 hours severely at room temperature. The complexes as precipitate were filtered, washed with ethanol twice, dried under vacuum and finally recrystallized from dichloromethane/methanol or chloroform/ethanol. Characteristic FT-IR and UV-visible spectral data were summarized in Table 1 and other physical and spectral data are as follows.

(1) . Yield: 58%; yellowish white precipitate, %C₂₃H₂₀ZnS₂N₆O₄: calc. C, 48.13%; H, 3.51%; N, 14.46%; found: C, 47.9%; H, 3.6%; N, 14.1%. ¹H NMR (DMSO-d₆): 8.24 (d, 2H, J = 8.40 Hz), 8.04 (d, 2H, J = 8.00 Hz), 7.96 (d, 2H, J = 7.6 Hz), 7.76 (t, 2H, J = 7.2 Hz, J = 6.80 Hz), 7.63 (t, 2H, J = 7.6 Hz, J = 6.80 Hz), 7.45 (dd, 2H, J = 16.00 Hz, J = 4.80 Hz), 7.03 (dd, 2H, J = 15.20 Hz, J = 8.40 Hz), 3.62 (t, 4H, J = 5.6 Hz), 1.92 (q, 2H, J = 6.00 Hz) ppm. ¹³C NMR (DMSO-d₆): 164.24, 148.46, 137.16, 135.79, 134.16, 132.16, 130.60, 128.90, 125.08, 59.25, 31.91 ppm. m.p. = 196°C (dec.). (DMF) = 36.22 cm² Ω⁻¹ M⁻¹.

(2) . Yield: 84%; white precipitate, %C₂₁H₂₀ZnN₁₀O₄: calc. C, 46.55%; H, 3.72%; N, 25.85%; found: C, 47.4%; H, 3.5%; N, 25.2%. ¹H NMR (DMSO-d₆): 8.29 (d, 2H, J = 8.80 Hz), 8.05 (d, 2H, J = 8.00 Hz), 7.94 (d, 2H, J = 7.6 Hz), 7.78 (t, 2H, J = 7.20 Hz, J = 7.60 Hz), 7.64 (t, 2H, J = 8.00 Hz, J = 7.2 Hz), 7.51 (d, 2H, J = 16.00 Hz), 7.03 (dd, 2H, J = 16.00 Hz, J = 8.80 Hz), 3.66 (t, 4H, J = 6.00 Hz), 1.93 (q, 2H, J = 6.40 Hz) ppm.¹³C NMR (DMSO-d₆): 165.06, 148.50, 138.03, 134.22, 131.67, 130.67, 130.52, 128.94, 125.13, 59.38, 31.64 ppm. m.p. = 180°C (dec.). (DMF) = 25.47 cm² Ω⁻¹ M⁻¹.

(3) [CdL(SCN)(NCS)]. Yield: 58%; yellowish white precipitate, %C₂₃H₂₀Cd S₂N₆O₄: calc. C, 44.49%; H, 3.25%; N, 13.53%; found: C, 44.9%; H, 3.4%; N, 13.7%. ¹H NMR (DMSO-d₆): 8.21 (d, 2H, J = 8.80 Hz), 8.03 (d, 2H, J = 8.00 Hz), 7.98 (d, 2H, J = 7.60 Hz), 7.77 (t, 2H, J = 7.60 Hz), 7.62 (t, 2H, J = 7.60 Hz), 7.42 (d, 2H, J = 15.60 Hz), 7.08 (dd, 2H, J = 15.60 Hz, J = 8.40 Hz), 3.60 (t, 4H, J = 5.60 Hz), 1.91 (q, 2H, J = 6.40 Hz) ppm.¹³C NMR (DMSO-d₆): 163.90, 148.45, 136.55, 134.15, 133.56, 132.67, 130.66, 130.50, 129.01, 125.05, 59.14, 32.25 ppm. m.p. = 179°C (dec.). (DMF) = 46.67 cm² Ω⁻¹ M⁻¹.

(4) . Yield: 39%; white precipitate, %C₂₁H₂₀CdN₁₀O₄: calc. C, 42.83%; H, 3.42%; N, 23.79%; found: C, 42.4%; H, 3.6%; N, 24.2%. ¹H NMR (DMSO-d₆): 8.22 (d, 2H, J = 8.40 Hz), 8.04 (d, 2H, J = 8.00 Hz), 7.98 (d, 2H, J = 7.60 Hz), 7.71 (t, 2H, J = 7.60 Hz, J = 7.20 Hz), 7.63 (t, 2H, J = 7.60 Hz), 7.42 (d, 2H, J = 16.00 Hz), 7.14 (m, 2H), 3.62 (bs, 4H), 1.89 (q, 2H, J = 6.40 Hz) ppm.¹³C NMR (DMSO-d₆): 164.08, 148.48, 136.54, 134.12, 132.71, 130.69, 130.50, 128.98, 125.05, 59.10, 32.25 ppm. m.p. = 179°C (dec.). (DMF) = 17.72 cm² Ω⁻¹ M⁻¹.

(5) . Yield: 62%; yellowish white precipitate, %C₂₃H₂₀Hg S₂N₆O₄: calc. C, 38.95%; H, 2.84%; N, 11.85%; found: C, 39.2%; H, 2.9%; N, 11.6%. ¹H NMR (DMSO-d₆): 8.48 (d, 2H, J = 8.00 Hz), 8.08 (d, 2H, J = 8.00 Hz), 7.96 (d, 2H, J = 7.60 Hz), 7.81 (t, 2H, J = 7.60 Hz), 7.67 (t, 2H, J = 8.00 Hz, J = 7.60 Hz), 7.60 (d, 2H, J = 15.60 Hz), 7.13 (dd, 2H, J = 15.20 Hz, J = 8.80 Hz), 3.80 (bs, 4H), 2.01 (m, 2H) ppm.¹³C NMR (DMSO-d₆): 166.12, 148.56, 139.39, 134.27, 131.19, 131.06, 130.35, 129.08, 125.21, 117.80, 60.04, 31.65 ppm. m.p. = 123°C (dec.). (DMF) = 19.90 cm² Ω⁻¹ M⁻¹.

(6) . Yield: 62%; yellowish white precipitate, %C₂₁H₂₀HgN₁₀O₄: calc. C, 37.25%; H, 2.98%; N, 20.69%; found: C, 37.6%; H, 3.2%; N, 20.3%. ¹H NMR (DMSO-d₆): 8.29 (d, 2H, J = 8.40 Hz), 8.14 (d, 2H, J = 8.40 Hz), 7.95 (d, 2H, J = 8.40 Hz), 7.86 (t, 2H, J = 7.60 Hz), 7.63 (t, 2H, J = 10.0 Hz, J = 7.20 Hz), 7.07 (dd, 2H, J = 15.6 Hz, J = 8.60 Hz), 6.62 (d, 2H, J = 16.40 Hz), 3.46 (bd, 4H), 2.07 (m, 2H) ppm.¹³C NMR (DMSO-d₆): 167.5, 156.3, 136.33, 134.78, 134.16, 131.97, 129.46, 125.40, 125.07, 17.98 ppm. m.p. = 110°C (dec.). (DMF) = 20.43 cm² Ω⁻¹ M⁻¹.

3. Results and Discussion

3.1. Physical Measurements and Microanalysis Data

Herein, the synthesis and spectral identification of a new symmetrical bidentate Schiff-base ligand of N,N′-bis((E)-3-(2-nitrophenyl)allylidene)propane-1,3-diamine and its complexes with zinc, cadmium, and mercury ions in general formula of MLX₂ (X = SCN⁻, ) are reported as shown in Figure 1. The elemental analysis data are in accordance to the calculated values confirming molar ratio of 1 : 1 between MX₂ and Schiff-base ligand at all complexes. The ligand is melted at 163°C and is soluble in common organic solvents. The complexes were found to be decomposed in the range of 110–196°C. Solubility test showed that the titled complexes are soluble in organic solvents such as dichloromethane, chloroform, acetonitrile, and ethylacetate and insoluble in alcohols such as ethanol and methanol. The compounds were stable under ordinary laboratory conditions.

3.2. Molar Conductivity

The low molar conductivities of 10⁻³ M solutions of ligand and its complexes in DMF solvent were in the range of 2.53–46.67 cm² Ω⁻¹ M⁻¹ at room temperature indicate that all of them are nonelectrolytes [38, 39]. Molar conductance of mercury complexes was smoothly lower than zinc and cadmium analogues that state more stability of them toward dissociation in DMF solution.

3.3. FT-IR Spectra

Some important FT-IR absorption frequencies of the bidentate Schiff-base ligand and its zinc, cadmium, and mercury complexes have been collected in Table 1. In infrared spectrum of the ligand, lack of characteristic absorption frequencies of the starting aldehyde and amine at wave numbers of 1682 cm⁻¹ and 3150–3300 cm⁻¹ and then appearance of strong absorption frequencies at wave numbers of 1635 and 1615 cm⁻¹, assigned to asymmetric and symmetric stretching of C=N bonds, confirm the synthesis of ligand. The asymmetric and symmetric stretching vibrations of C=N bonds in the IR spectrum of the free ligand are enhanced in intensity while smoothly shift to lower wave numbers in the complexes spectra by 2–9 cm⁻¹ and 1–5 cm⁻¹, respectively, and this is in consistency with coordination of the ligand to the metal ion centers via the azomethine nitrogen atoms [34, 35, 40]. Furthermore, in the case of mercury(II) complexes, the symmetric vibration of azomethine is vanished or probably unified with the asymmetric one. In the IR spectrum of Schiff-base ligand, several weak absorptions are observed at 3067, 2935, and 2843 cm⁻¹ that are assignable to aromatic, aliphatic, and iminic C–H stretching vibrations, respectively, and also two strong absorption frequencies related to NO₂ groups are found at 1522 and 1345 cm⁻¹, that are nearly unchanged or shifted after coordination of ligand. In the IR spectrum of zinc thiocyanate complex, appearance of a very strong characteristic vibration at 2065 cm⁻¹ may confirm coordination of N-bonded thiocyanate [41, 42]. Two absorption frequencies at 2097 and 2058 cm⁻¹ in cadmium complex IR spectrum maybe attributed to both S- and N-bonded mode of thiocyanates, respectively. This suggestion is in accordance to some previous reports on thiocyanate complexes [41]. Also mercury thiocyanate complex spectrum shows a strong sharp absorption at 2117 cm⁻¹ that may be related to S-coordination of thiocyanate ions [41–43]. The absorptions appeared at 2062, 2046, and 2034 cm⁻¹ in azide complexes spectra are attributable to the υ(N=N=N) of coordinated azides based on the literature reports [44–46].

3.4. Electronic Spectra

UV-visible spectra of the free ligand and complexes were recorded in DMF (Table 1). Two bands that appeared at 298 nm and 326 nm (as a shoulder) in the UV-visible spectrum of ligand maybe attributed to transitions within aromatic rings and azomethine groups, respectively (Table 1). In zinc thiocyanate and azide complexes, these two band are observed at 303 nm (as shoulder), 323 nm, 293 nm, and 330 (as shoulder). In cadmium and mercury complexes, these bands are unified and appeared at red shifted wavelengths, 331–339 nm. Therefore, the coordination of the ligand and other anions to the metal ions is well confirmed by noticeable difference of the complexes spectral data with respect to the free ligand.

3.5. ¹H- and ¹³C-NMR Spectra

The ¹H NMR spectroscopy has been used for confirmation of the binding of ligand to metal ions for all complexes. The ¹H and ¹³C NMR spectral data have been summarized in Section 2. The ¹H and ¹³C NMR spectra of ligand and zinc azide complex are illustrated in Figure 2. Regarding Figure 1, the ¹H NMR spectrum of Schiff-base ligand in DMSO-d₆ exhibits a doublet peak with coupling constant of 8.40 Hz, at 8.17 ppm assigned to imine (–HC=N–) protons that is shifted to the downfield region at 8.21–8.48 ppm in the complexes, except for mercury azide complex (i.e., smoothly upfielded to 8.14 ppm), indicating coordination of ligand to metal ions. In the ligand spectrum, the aromatic hydrogens of split by are seen as a doublet at 8.02 ppm with coupling constant 8.40 Hz. This signal shifts to 8.03–8.14 ppm in the complexes. Hydrogens of in ligand are observed as a doublet at 7.96 ppm with coupling constant of 7.60 Hz due to coupling with . In complexes, this doublet appeared in the range of 7.94–7.98 ppm. Hydrogens of that are split by and have been appeared as triplet at 7.45 pm with coupling constants of 7.60 and 7.20 Hz. This ligand signal has been shifted to 7.71–7.86 ppm in the complexes. Hydrogens of are exhibited as a triplet signal at 7.61 ppm with coupling constants of 8.00 and 7.60 Hz, that are seen at 7.62–7.67 ppm in titled coordination compounds. Olefin hydrogens of split by appeared as a doublet at 7.38 ppm with coupling constant of 15.60 Hz. In all complexes, the related signal is downfielded to 7.42–7.60 ppm except for mercury azide that is upfielded to 6.60 ppm. hydrogens appeared as a doublet of doublet at 6.98 ppm with coupling constants of 16.00 and 8.80 Hz that shift to weaker fields at 7.03–7.14 ppm in coordinated ligand of complexes. The ¹³C-NMR spectrum of the ligand shows azomethine carbons C (9, 9′) resonances at 162.85 ppm [32–35]. This peak is shifted to the downfield regions at 163.90–167.5 ppm in its complexes indicating well coordination of the iminc nitrogens to metal ions. The other assigned signals are observed at 148.44 (), 135.70 (), 134.07 (), 133.00 (), 130.70 (), 130.32 (), 128.92 (), 125.00 (), 59.04 (), and 32.24 (C₁₁) ppm; these signals have been shifted to the up- or downfields in all of complexes indicating coordination of the ligand to metal ions. The additional signals at 135.79, 133.56, and 117.80 in thiocyanate complexes may be assigned to coordinated thiocyanate ions in zinc, cadmium, and mercury thiocyanate complexes, respectively.

(a)

(b)

(c)

(d)

3.6. Theoretical Modeling of Ligand and Its Complexes

The initial structures of ligand and its complexes were sketched with HyperChem 8.0.8 software and PM3 semiempirical method. All geometries were optimized at the Becke’s three-parameter hybride functional (B3) with the nonlocal correlation of Lee-Yang-Parr (LYP) level of theory with double-zeta valence (LANL2DZ) basis set using GAUSSIAN 03 suite of program, working on 2.3 GHz dual processors. Calculations were followed in the gas phase. Density functional theory (DFT) calculations were done in order to find the optimized geometry of the ligand and its complexes. For instance, the optimized structures of ligand, zinc thiocyanate, and azide complexes have been shown in Figure 3. Some selected structural parameters including bond lengths, bond angles, and torsion angles based on Figure 1 are summarized in Table 2. As seen in Table 2, M–N (imine) and M–X are increased from zinc to mercury complexes. N′–M–N angles are decreased as N′–Hg–N > N′–Cd–N > N′–Zn–N while X–M–X′ are nearly increased with going from zinc to mercury complexes. N–C₉–C₈–C₇ and torsional angles are placed in the ranges of −176.6223 to −179.7008(°) and 178.3640 to 179.0566(°), respectively indicating nearly planer status around the C₉–C₈ and . and torsional angles are found to be at the ranges: 66.41 to 71.63(°) and −66.39 to −73.23(°), respectively that suggest gauche conformation around the C₁₀–C₁₁ and bonds. Torsional angles around the bonds of C₇–C₆ and are in the range of −149.97 to 155.17(°) and 149.98 to −154.52(°), confirming out of plane torsion of aromatic rings with respect to suggestible molecular plane.

(a)

(b)

(c)

3.7. Electrochemical Behavior

The electrochemical properties of a substance in solution are investigated by cyclic voltammetry technique. In this paper, cyclic voltammograms of ligand and its zinc, cadmium, and mercury complexes were obtained in dry acetonitrile solutions on glassy carbon electrode with a scan rate of 0.1 V/S and are depicted in Figure 4. The redox potential data have been summarized in Table 3. The ligand is redox active in the potential window of (−2)–(+1.5) volt. Cyclic voltammogram of ligand shows its reduction in two negative potentials of −0.78 and −1.54 V. These reductive processes may be attributed to reduction of nitro groups [47]. In positive direction, the ligand is oxidized only at −0.63 V. In zinc complexes, again two reduction and one oxidation waves are recorded but with an observable shift to more positive values in first waves in two complex and only second wave in zinc azide complex. Meanwhile, the second reduction wave of zinc thiocyanate shifts to less positive value. In contrast to zinc complexes, cadmium and mercury analogues are reduced and oxidized via reversible processes at the voltage range of (−0.77)–(−0.93) V and (−.57)–(−0.72) V, respectively. As shown in Figure 4, thiocyanate complexes are nearly reduced harder than ligand except in the case of zinc complex so that the second reduction peak does not appear at (−2)–(+1.5) and furthermore the first reduction wave shifts to more negative values. Anodic oxidation of thiocyanate complexes also becomes harder than free ligand except about mercury complex so that they are oxidized in more positive values. A comparison between azide and thiocyanate complexes reveals that the former are reduced and/or oxidized easier than the latter. This can be due to more π-back bonding from metal to ligand in thiocyanate complex with respect to azide analogues because of softness character of thiocyanate that leads to more electron density on ligand structure in thiocyanate complex explaining the observed trend. On the other hand, the azide ion indirectly induces more positive character on the structure of coordinated ligand with respect to thiocyanate. Furthermore, it also reduces tendency of metal ion for π-back bonding to ligand. The ease of reduction in azide and thiocyanate complexes is ZnL(N₃)₂ > CdL(N₃)₂ > HgL(N₃)₂ and ZnL(NCS)₂ > CdL(SCN)(NCS) > HgL(SCN)₂, respectively. Opposite order is deduced for oxidation peak in the azide and thiocyanate complexes. These trends can also be deduced based on π-back bonding phenomenon that is increased as mercury > cadmium > zinc in consistency with an increase in softness character of three ions.

(a)

(b)

3.8. Conclusion

In this work, we reported the synthesis, full spectroscopic characterization, electrochemical and theoretical investigation of a new symmetric bidentate Schiff-base ligand and its new zinc(II), cadmium(II), and mercury(II) azide and thiocyanate four coordinated compounds. The physical, spectral, and theoretical results predict pseudotetrahedral geometry for all coordination compounds. The ligand and its complexes structures were optimized at the nonlocal correlation of Lee-Yang-Parr (LYP) level of theory with double-zeta valence (LANL2DZ) basis set using Gaussian 03 suite of program, and finally some theoretical structural parameters such as bond lengths, bond angles, and torsional angles were extracted. Electrochemical behavior of ligand and its complexes was investigated by cyclic voltammetry technique. The cyclic voltammogram of ligand illustrated two reduction and one oxidation peaks. The zinc complexes exhibited a similar behavior with respect to ligand, but cadmium and mercury complexes showed a reversible electrochemical process.

Acknowledgments

Partial support of this research by Yasouj University is acknowledged. The authors do not have a direct financial relation with the commercial identity companies mentioned in this work.

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Copyright © 2013 Morteza Montazerozohori 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.

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Journal of Spectroscopy

Synthesis, Spectroscopy, Theoretical, and Electrochemical Studies of Zn(II), Cd(II), and Hg(II) Azide and Thiocyanate Complexes of a New Symmetric Schiff-Base Ligand

Abstract

1. Introduction

2. Experimental

2.1. Materials and Methods

2.2. Synthesis of the Schiff-Base Ligand (L)

2.3. Synthesis of Metal Complexes

3. Results and Discussion

3.1. Physical Measurements and Microanalysis Data

3.2. Molar Conductivity

3.3. FT-IR Spectra

3.4. Electronic Spectra

3.5. 1H- and 13C-NMR Spectra

3.6. Theoretical Modeling of Ligand and Its Complexes

3.7. Electrochemical Behavior

3.8. Conclusion

Acknowledgments

References

Copyright

3.5. ¹H- and ¹³C-NMR Spectra