# Synthesis and Antimicrobial Studies of Tridentate Schiff Base Ligands with Pyrazolone Moiety and Their Metal Complexes

Authors: Ramasamy Jayarajan; Gnanasambandam Vasuki; Pillutla Sambasiva Rao
Journal: Organic Chemistry International
 (2010)

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## Abstract

Synthesis, characterization, and antimicrobial activity of tridentate Schiffbase ligands containing pyrazolone moiety (3a and 3b) and their transition metal complexes of VO(II), Cu(II), Fe(III), and Co(II) 4a–h have been investigated. The complexes show enhanced antibacterial activity against S. aureus, E. coli, and S. typhi and antifungal activity against C. albicans, Rhizopus sp., and A. niger compared to the ligands.


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## Body

## 1. Introduction

Developing metal-based drugs is emerging as an active area of research. Many organic ligands particularly tridentate Schiff base ligands show enhanced antibacterial, antifungal, and carcinostatic activity when complexed to transition metal ions [1–7]. Heterocyclic systems bearing the pyrazolyl moiety show antibacterial, antifungal, anti-inflammatory and enzyme-inhibitory activity [8–11]. 4-acylpyrazolones are good chelating ligands. Synthesis and characterization of metal complexes of 4-acylpyrazoles are well documented [12–14]. However, biological activity of tridentate Schiff base ligands containing pyrazolone moiety and their transition metal complexes is not explored. Therefore, in the present paper we report the synthesis, characterization, and antimicrobial activity of tridentate Schiff bases of the type ONN (3a)and ONO (3b)containing the pyrazolone moiety and their VO(II), Cu(II), Fe(III), and Co(II) complexes.


## 2. Results and Discussion

3-Methyl-1-phenylpyrazol-5-one(1) and 4-acetyl-3-methyl-1-phenylpyrazol-5-one were prepared by following the literatures procedure. 4-acetyl-3-methyl-1-phenylpyrazol-5-ones mainly exists as the 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol tautomer (2). Condensing (2) with 1,2-diaminobenzene, and 2-aminophenol resulted in ONN-and ONO-type tridentate ligands (3aand3b), respectively. Ligands 3a and 3b were complexed with metal salts viz vanadyl sulphate monohydrate, copper(II) nitrate trihydrate, ferric chloride hexahydrate, and cobalt(II) nitrate hexahydrate to obtain, their corresponding complexes (4a–h). Compounds 3aand 3b were characterized by IR, 1H NMR, 13C NMR, and elemental analysis. In addition to these spectral techniques LC-MS was also used for characterization of 3a. 13C NMR and LC-MS data (m/e 307) of 3a indicates the formation of tridentate ligand resulting from condensation of 2 with one amino group of 1,2-diaminobenzene. Though there is a possibility for biscondensation repeated experiments resulted in tridentate ligand (3a) only. Complexes (4a–h)were characterized by IR, UV-Visible, mass, and EPR spectral studies. However, from the data available the structure of complexes could not be fully characterized. The proposed structures of the complexes are given in Table 1. The coordination of methanol in VO(II) complexes (4aand4e) was verified by thermal analysis. Thermogram of complexes showed a weight loss around 70–130°C ascribable to loss of methanol in the complexes. Further conclusive evidence of the coordination of methanol in these complexes was shown by the appearance of ν(OH) around 3400 cm−1 in IR spectra.Table 1
Proposed structure of complexes.
CompoundStructureCompoundStructure4a4e4b4f4c4g4d4h


### 2.1. Antibacterial Studies

The ligands(3a-b) and complexes (4a–h) synthesized were screened for their antibacterial activity by disc-diffusion method [15, 16] against Staphylococcus aureus (Gram positive), Pseudomonas aeruginosa(Gram negative), and Salmonella typhi (Gram negative). The test compounds were prepared at a concentration of 200 μg/mL. Solvent control that is, DMSO was also maintained throughout the experiment simultaneously. Nutrient agar plates were prepared under sterile conditions and incubated overnight to detect contamination. About 0.2 mL of working stock culture was transferred into separate nutrient agar plates and spread thoroughly using a glass spreader. Whatman No. 1 discs (6 mm in diameter) were impregnated in the test compounds and dissolved in DMSO (200 μg/mL) for about half an hour. Commercially available drug disc (Ciprofloxacin 10 μg/disc) was used as positive reference standard. Negative controls were also prepared by impregnating disc of same size in DMSO solvent. The discs were placed on the inoculated agar plates and incubated at 37±1°C for about 18–24 h. Antibacterial activity was evaluated by measuring the zone of inhibition (mm) against the test organism Figure 1.Antibacterial activity of(3a-b)and(4a-h).
(a)(b)It is observed that, in general, metal complexes show enhanced antibacterial activity than the corresponding ligands. No general trend in the activity of the ligands or the metal complexes against the bacterial strain is observed. Iron complex4cshowed enhanced activity against all bacterial strains. 4c also showed very low minimum inhibitory concentration (MIC) value (12.5 μg/mL) of S. aureus. The activity of iron complex 4gis less compared to 4c for all bacterial strains.Among the cobalt complexes4d and 4h, 4his more effective against S. typhi with low MIC value (25 μg/mL) compared to the standard ciprofloxacin (50 μg/mL) as well as its corresponding iron complex.


### 2.2. Antifungal Studies

The antifungal activity of3a-band their complexes(4a–h) were examined with three fungal strains namely Candida albicans, Rhizopus sp., andAspergillus niger. Drug amphotericin B was used as standard. Sabouraud’s dextrose agar (SDA) medium was used for the growth of fungi, and testing was done in Sabouraud’s dextrose broth (SDB) medium. The subculture and the viable count were carried out by the same procedure as done in antibacterial studies except the temperature was maintained at 28±1°C for about 72 h. Similarly for disc diffusion method, the petri dishes were incubated at 28±1°C for about 72 h. The diameters of zone of inhibition (mm) of all the compounds are given in Figure 2.Antifungal activity of(3a-b) and (4a-h).
(a)(b)It is observed that the diameter of zone of inhibition (mm) of cobalt complex4h shows very high activity with very low MIC value (12.5 μg/mL) against the fungal strain A. niger (MIC of standard amphotericin B is 50 μg/mL).


## 2.1. Antibacterial Studies

The ligands(3a-b) and complexes (4a–h) synthesized were screened for their antibacterial activity by disc-diffusion method [15, 16] against Staphylococcus aureus (Gram positive), Pseudomonas aeruginosa(Gram negative), and Salmonella typhi (Gram negative). The test compounds were prepared at a concentration of 200 μg/mL. Solvent control that is, DMSO was also maintained throughout the experiment simultaneously. Nutrient agar plates were prepared under sterile conditions and incubated overnight to detect contamination. About 0.2 mL of working stock culture was transferred into separate nutrient agar plates and spread thoroughly using a glass spreader. Whatman No. 1 discs (6 mm in diameter) were impregnated in the test compounds and dissolved in DMSO (200 μg/mL) for about half an hour. Commercially available drug disc (Ciprofloxacin 10 μg/disc) was used as positive reference standard. Negative controls were also prepared by impregnating disc of same size in DMSO solvent. The discs were placed on the inoculated agar plates and incubated at 37±1°C for about 18–24 h. Antibacterial activity was evaluated by measuring the zone of inhibition (mm) against the test organism Figure 1.Antibacterial activity of(3a-b)and(4a-h).
(a)(b)It is observed that, in general, metal complexes show enhanced antibacterial activity than the corresponding ligands. No general trend in the activity of the ligands or the metal complexes against the bacterial strain is observed. Iron complex4cshowed enhanced activity against all bacterial strains. 4c also showed very low minimum inhibitory concentration (MIC) value (12.5 μg/mL) of S. aureus. The activity of iron complex 4gis less compared to 4c for all bacterial strains.Among the cobalt complexes4d and 4h, 4his more effective against S. typhi with low MIC value (25 μg/mL) compared to the standard ciprofloxacin (50 μg/mL) as well as its corresponding iron complex.


## 2.2. Antifungal Studies

The antifungal activity of3a-band their complexes(4a–h) were examined with three fungal strains namely Candida albicans, Rhizopus sp., andAspergillus niger. Drug amphotericin B was used as standard. Sabouraud’s dextrose agar (SDA) medium was used for the growth of fungi, and testing was done in Sabouraud’s dextrose broth (SDB) medium. The subculture and the viable count were carried out by the same procedure as done in antibacterial studies except the temperature was maintained at 28±1°C for about 72 h. Similarly for disc diffusion method, the petri dishes were incubated at 28±1°C for about 72 h. The diameters of zone of inhibition (mm) of all the compounds are given in Figure 2.Antifungal activity of(3a-b) and (4a-h).
(a)(b)It is observed that the diameter of zone of inhibition (mm) of cobalt complex4h shows very high activity with very low MIC value (12.5 μg/mL) against the fungal strain A. niger (MIC of standard amphotericin B is 50 μg/mL).


## 3. Conclusions

4-Acetylpyrazolone predominantly exists as 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol tautomer. The 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol readily condenses with 1,2-diaminobenzene and 2-aminophenol forming tridentate Schiff base ligands of ONN and ONO type. The metal complexes of these ligands with VO(II), Cu(II), Fe(III), and Co(II) show varying geometries. The ligands and metal complexes exhibit varying degree of antibacterial and antifungal activity. In general Fe(III) and Co(II) complexes are more potent than other complexes and ligands.


## 4. Experimental Section

### 4.1. General Procedures

1H NMR and 13C NMR spectra were recorded on a Bruker 400 instrument using tetramethylsilane (TMS) as internal standard and CDCl3, or DMSO-d6 as solvent. Chemical shifts are given in parts per million (ppm). IR spectra were recorded on a Nicolet 6700 FT-IR Spectrophotometer in KBr pellet method in the range of 400–4000 cm−1. UV-Vis spectra were obtained from Ocean Optics HR 4000 Spectrophotometer and using DMF as a solvent in a 1 cm quartz cell. Elemental analyses were carried out on a Perkin-Elmer 2400 Series CHNS/O analyzer. The ESI-mass spectra were recorded in QTOF-Micromass-UK by using DMF as solvent, and the LC-MS was taken in Shimadzu LC-MS using acetonitrile as solvent. Thermogravimetric analyses were recorded on TA Instruments Q 600 SDT. The EPR spectra of complexes were recorded in JEOL JES-TE 100 EPR Spectrometer operating at X-band frequency.3-Methyl-1-phenylpyrazoline-5-one  (1)
3-Methyl-1-phenylpyrazoline-5-one was prepared by following the literatures procedure [17].3-Methyl-1-phenyl-4-acetylpyrazoline-5-ol  (2)
3-Methyl-1-phenyl-4-acetylpyrazoline-5-ol was prepared by following the literatures procedure [18].


### 4.2. General Procedure for the Synthesis of Tridentate Schiff Base Ligands (3a-b)

Ethanolic solution of 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol (2 mmoL) and 1,2-diaminobenzene (2 mmoL) was taken in a round-bottom flask and refluxed for 3 h. The solid product was filtered, washed with cold ethanol and recrystallized from ethanol, and dried under vacuum. A similar procedure was adopted for the reaction between 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol (2 mmoL) and 2-aminophenol (2 mmoL) to synthesize3b, but the reaction mixture was refluxed for 8 h and the product was recrystallized from acetonitrile.4-(1-(2-aminophenylimino)  ethyl)-3-methyl-1-phenylpyrazol-5-ol (3a)
Yellow. Yield (75%); m.p. 192°C; IR (KBr, cm−1): 3437 (OH stretch), 3350 (NH stretch), 3036 (aromatic CH stretch), 1621 (azomethine C=N stretch), 1538 (cyclic C=N stretch) and 1393 (C–O stretch), 1H NMR (CDCl3) ppm: δ2.29 (s, 3H, CH3), 2.42 (s, 3H, CH3), 3.9 (s, 2H, NH2), 6.77–8.02 (m, 9H, CH aromatic), and 12.58 (s, 1H, OH); 13C NMR (CDCl3) ppm: δ16.6, 17.5, 100.54, 116.31, 118.66, 119.32, 122.17, 124.44, 127.68, 128.75, 129.32, 138.97, 142.6, 147.36, 165.56, and 165.85; LC-MS m/z 307 [M+H]+; analytical calculation for C18H18N4O: C, 70.57; H, 5.92; and N, 18.29 found C, 70.52; H, 5.86; and N, 18.20.4-(1-(2-hydroxyphenylimino)  ethyl)-3-methyl-1-phenylpyrazol-5-ol  (3b)
Pale yellow. Yield (70%); m.p. 220°C; IR (KBr, cm−1): ~3163( OH stretch), 2982 (aromatic CH stretch), 1623 (azomethine C=N stretch), 1532 (cyclic C=N stretch) and 1388 (C–O stretch), 1H NMR (DMSO-d6) ppm; δ2.37 (s, 3H, CH3), 2.38 (s, 3H, CH3), 6.82–8.03 (m, 9H, CH aromatic), and 10.0 (s, 1H, phenolic OH); 13C NMR (DMSO-d6) ppm: δ21.75, 22.38, 104.75, 121.63, 123.15, 124.11, 128.31, 128.86, 131.75, 133.30, 133.43, 144.50, 151.81, 157.17, 169.18, and 170.43; analytical calculation for C18H17N3O2: C, 70.34; H, 5.58; and N, 13.67 found C, 70.27; H, 5.55; and N, 13.58.


### 4.3. General Procedure for the preparation of VO(II), Cu(II), Fe(III), and Co(II) complexes (4a–h)

The solution of Schiff base ligand3a/3b(10 mmoL) in ethanol/methanol and metal salts (10 mmoL) (vanadyl sulphate monohydrate (1.8 g), copper(II) nitrate trihydrate (2.41 g), cobalt(II) nitrate hexahydrate (2.91 g), and ferric chloride hexahydrate (2.7 g) in minimum quantity of ethanol/methanol were heated separately and mixed. The resultant solution was refluxed for 5-6 h. The solution was then concentrated to half of its volume, filtered and washed several times with hot water and finally with hot alcohol. The product was dried under vacuum and recrystallized from DMF. All the metal complexes have a melting point above 250°C.


### 4.4. IR Spectra

The FT-IR (KBr) spectra of all complexes(4a–h) were recorded, and values are given in Table 2. The IR of the Schiff base (3a) exhibits strong bands at ~3350 cm−1  due to the presence of ν(NH2) varies in the complexes (4a–d) shows the coordination of amine group with metal ions. The band at 1621 cm−1 due to ν(C=N) (azomethine) group is shifted to lower values indicating that the ligands are coordinated to the metal ions through the nitrogen of the azomethine group. Moreover, the presence of ν(C=N) stretching in 3balso varies in the complexes compared to the ligand indicating the formation of the complexes. The band at 1300–1400 assignable to pyrazolone ν(C–O) stretching in ligand varies in complexes. Further conclusive evidence of the coordination of these Schiff base ligands (3a-b)with metals was shown by the appearance of weak low-frequency new bands at 400–530 cm−1 corresponding to ν(M–N) and ν(M–O) stretching modes.Table 2
FT-IR and UV-Vis spectral data of complexes (3a-b and 4a–h).
S No.CodeIR (KBr) cm−1λmax (nm)C=NC–OM–L13a16211393—331, 28224a16011383511, 478413, 26134b16091384507, 435617, 399, 29844c16001382501, 453415, 28554d15941383514, 460531, 364, 29163b16231388—31574e16361355513, 455601, 399, 29484f15971377511, 482606, 483, 29194g16001382507, 455442, 291104h15931369511, 461541, 376, 301


### 4.5. UV-Visible Spectra

The electronic spectra (Table2) of the Schiff base ligands (3a-b)show absorption bands around 200–350 nm due to π-π* and n-π* transitions for the benzene ring and azomethine group. In the spectra of the complexes, the absorption band of the azomethine chromophore n-π* transition is shifted compared to the ligand indicating that the imine nitrogen is involved in the coordination with metal ions. The spectra of the metal complexes (4a–h) shows that the absorption around 400–800 nm is due to ligand to metal charge transfer and d–d transition band of the metal in the complexes.


### 4.6. EPR Spectra

The powder and solution state EPR spectra for4a,4b,4c,4e,4f, and 4g have been recorded at X-band frequencies at room temperature and also in 77 K (LNT), and a typical spectra are shown in Figure 3. The calculated g and hyperfine (A) values are given in Table 3. As expected, the Co(II) complexes (4dand4h) do not give rise to any EPR spectra down to 77 K due to relaxations, but formation of the complex was confirmed by mass spectra (m/z 669), and an octahedral structure has been proposed.Table 3
g and A values for complexes. A values are in units of mT.
CompoundsRecorded conditiong11g⊥A11A⊥4aLNTSolution1.9371.9818.736.494bRTPowder2.262.06**LNTPowder2.242.06LNTSolutiong1=2.31,g2=2.06,15.08*g3=2.034cRTPowderg1=20.44,g2=5.1,**g3=2.34,g4=1.69,g5=1.294eLNTSolution1.9381.9818.706.514fRTPowder2.262.06**LNTSolutiong1=2.31,g2=2.06,14.84*g3=2.044gRTPowderg1=20.4,g2=5.24,**g3=2.37,g4=1.7,g5=1.31*unresolved.(a)
EPR spectrum of4a solution at LNT (Freq=9.06597GHz)(b)
EPR spectrum of4b solution at LNT (Freq=9.06786 GHz)(c)
EPR spectrum of4c powder at RT (Freq=9.38540 GHz)The EPR spectrum of complexes4aand4e indicates that the paramagnetic ion responsible is VO(II) having S=1/2 and I=7/2. A close look at the spectrum indicates a shoulder on hyperfine lines suggesting that the symmetry of the complex is lower than distorted octahedron. This is not a common observation, as the deviation from axial symmetry is not reported in powder spectrum. The room temperature powder spectrum of 4ewas also recorded. The calculated g and A values of 4e matched with the values of 4a. This suggests that the coordination around vanadyl ion is nearly the same in both 4aand4e except for a slight change in distortion [19].Powder EPR spectrum of4b was recorded at room temperature and 77 K. The hyperfine lines from copper nucleus are not resolved at room temperature spectrum due to dipole-dipole broadening. In order to obtain the hyperfine values, the complex was dissolved in DMF, and EPR spectrum was recorded at 77 K. The spectrum clearly indicates resonances from copper nucleus (63Cu/65Cu). The symmetry around the copper is lower than distorted octahedral as reflected from the three g values [20]. Also the three g values suggest that the coordination around the copper is six, which was confirmed by mass spectra (m/z 665).The powder EPR spectrum of4c at room temperature shows a number of resonances indicating that iron is under the influence of a strong tetragonal distortion. The range of g-values suggests that all the three Kramers’ doublets are populated at room temperature. The ESI-Mass of 4c complex (m/z 740) suggests that the complex is oxygen bridged bimetallic iron complex. Moreover oxobridged iron complexes are well known in many literatures [21]. The recorded solution EPR spectrum shows a single resonance at g=2. This kind of observation suggests that the dimeric iron complex might have become monomer after dissolution, hence a single line is observed [22]. The complex 4g behaves similar to 4c.


## 4.1. General Procedures

1H NMR and 13C NMR spectra were recorded on a Bruker 400 instrument using tetramethylsilane (TMS) as internal standard and CDCl3, or DMSO-d6 as solvent. Chemical shifts are given in parts per million (ppm). IR spectra were recorded on a Nicolet 6700 FT-IR Spectrophotometer in KBr pellet method in the range of 400–4000 cm−1. UV-Vis spectra were obtained from Ocean Optics HR 4000 Spectrophotometer and using DMF as a solvent in a 1 cm quartz cell. Elemental analyses were carried out on a Perkin-Elmer 2400 Series CHNS/O analyzer. The ESI-mass spectra were recorded in QTOF-Micromass-UK by using DMF as solvent, and the LC-MS was taken in Shimadzu LC-MS using acetonitrile as solvent. Thermogravimetric analyses were recorded on TA Instruments Q 600 SDT. The EPR spectra of complexes were recorded in JEOL JES-TE 100 EPR Spectrometer operating at X-band frequency.3-Methyl-1-phenylpyrazoline-5-one  (1)
3-Methyl-1-phenylpyrazoline-5-one was prepared by following the literatures procedure [17].3-Methyl-1-phenyl-4-acetylpyrazoline-5-ol  (2)
3-Methyl-1-phenyl-4-acetylpyrazoline-5-ol was prepared by following the literatures procedure [18].


## 4.2. General Procedure for the Synthesis of Tridentate Schiff Base Ligands (3a-b)

Ethanolic solution of 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol (2 mmoL) and 1,2-diaminobenzene (2 mmoL) was taken in a round-bottom flask and refluxed for 3 h. The solid product was filtered, washed with cold ethanol and recrystallized from ethanol, and dried under vacuum. A similar procedure was adopted for the reaction between 3-methyl-1-phenyl-4-acetylpyrazolin-5-ol (2 mmoL) and 2-aminophenol (2 mmoL) to synthesize3b, but the reaction mixture was refluxed for 8 h and the product was recrystallized from acetonitrile.4-(1-(2-aminophenylimino)  ethyl)-3-methyl-1-phenylpyrazol-5-ol (3a)
Yellow. Yield (75%); m.p. 192°C; IR (KBr, cm−1): 3437 (OH stretch), 3350 (NH stretch), 3036 (aromatic CH stretch), 1621 (azomethine C=N stretch), 1538 (cyclic C=N stretch) and 1393 (C–O stretch), 1H NMR (CDCl3) ppm: δ2.29 (s, 3H, CH3), 2.42 (s, 3H, CH3), 3.9 (s, 2H, NH2), 6.77–8.02 (m, 9H, CH aromatic), and 12.58 (s, 1H, OH); 13C NMR (CDCl3) ppm: δ16.6, 17.5, 100.54, 116.31, 118.66, 119.32, 122.17, 124.44, 127.68, 128.75, 129.32, 138.97, 142.6, 147.36, 165.56, and 165.85; LC-MS m/z 307 [M+H]+; analytical calculation for C18H18N4O: C, 70.57; H, 5.92; and N, 18.29 found C, 70.52; H, 5.86; and N, 18.20.4-(1-(2-hydroxyphenylimino)  ethyl)-3-methyl-1-phenylpyrazol-5-ol  (3b)
Pale yellow. Yield (70%); m.p. 220°C; IR (KBr, cm−1): ~3163( OH stretch), 2982 (aromatic CH stretch), 1623 (azomethine C=N stretch), 1532 (cyclic C=N stretch) and 1388 (C–O stretch), 1H NMR (DMSO-d6) ppm; δ2.37 (s, 3H, CH3), 2.38 (s, 3H, CH3), 6.82–8.03 (m, 9H, CH aromatic), and 10.0 (s, 1H, phenolic OH); 13C NMR (DMSO-d6) ppm: δ21.75, 22.38, 104.75, 121.63, 123.15, 124.11, 128.31, 128.86, 131.75, 133.30, 133.43, 144.50, 151.81, 157.17, 169.18, and 170.43; analytical calculation for C18H17N3O2: C, 70.34; H, 5.58; and N, 13.67 found C, 70.27; H, 5.55; and N, 13.58.


## 4.3. General Procedure for the preparation of VO(II), Cu(II), Fe(III), and Co(II) complexes (4a–h)

The solution of Schiff base ligand3a/3b(10 mmoL) in ethanol/methanol and metal salts (10 mmoL) (vanadyl sulphate monohydrate (1.8 g), copper(II) nitrate trihydrate (2.41 g), cobalt(II) nitrate hexahydrate (2.91 g), and ferric chloride hexahydrate (2.7 g) in minimum quantity of ethanol/methanol were heated separately and mixed. The resultant solution was refluxed for 5-6 h. The solution was then concentrated to half of its volume, filtered and washed several times with hot water and finally with hot alcohol. The product was dried under vacuum and recrystallized from DMF. All the metal complexes have a melting point above 250°C.


## 4.4. IR Spectra

The FT-IR (KBr) spectra of all complexes(4a–h) were recorded, and values are given in Table 2. The IR of the Schiff base (3a) exhibits strong bands at ~3350 cm−1  due to the presence of ν(NH2) varies in the complexes (4a–d) shows the coordination of amine group with metal ions. The band at 1621 cm−1 due to ν(C=N) (azomethine) group is shifted to lower values indicating that the ligands are coordinated to the metal ions through the nitrogen of the azomethine group. Moreover, the presence of ν(C=N) stretching in 3balso varies in the complexes compared to the ligand indicating the formation of the complexes. The band at 1300–1400 assignable to pyrazolone ν(C–O) stretching in ligand varies in complexes. Further conclusive evidence of the coordination of these Schiff base ligands (3a-b)with metals was shown by the appearance of weak low-frequency new bands at 400–530 cm−1 corresponding to ν(M–N) and ν(M–O) stretching modes.Table 2
FT-IR and UV-Vis spectral data of complexes (3a-b and 4a–h).
S No.CodeIR (KBr) cm−1λmax (nm)C=NC–OM–L13a16211393—331, 28224a16011383511, 478413, 26134b16091384507, 435617, 399, 29844c16001382501, 453415, 28554d15941383514, 460531, 364, 29163b16231388—31574e16361355513, 455601, 399, 29484f15971377511, 482606, 483, 29194g16001382507, 455442, 291104h15931369511, 461541, 376, 301


## 4.5. UV-Visible Spectra

The electronic spectra (Table2) of the Schiff base ligands (3a-b)show absorption bands around 200–350 nm due to π-π* and n-π* transitions for the benzene ring and azomethine group. In the spectra of the complexes, the absorption band of the azomethine chromophore n-π* transition is shifted compared to the ligand indicating that the imine nitrogen is involved in the coordination with metal ions. The spectra of the metal complexes (4a–h) shows that the absorption around 400–800 nm is due to ligand to metal charge transfer and d–d transition band of the metal in the complexes.


## 4.6. EPR Spectra

The powder and solution state EPR spectra for4a,4b,4c,4e,4f, and 4g have been recorded at X-band frequencies at room temperature and also in 77 K (LNT), and a typical spectra are shown in Figure 3. The calculated g and hyperfine (A) values are given in Table 3. As expected, the Co(II) complexes (4dand4h) do not give rise to any EPR spectra down to 77 K due to relaxations, but formation of the complex was confirmed by mass spectra (m/z 669), and an octahedral structure has been proposed.Table 3
g and A values for complexes. A values are in units of mT.
CompoundsRecorded conditiong11g⊥A11A⊥4aLNTSolution1.9371.9818.736.494bRTPowder2.262.06**LNTPowder2.242.06LNTSolutiong1=2.31,g2=2.06,15.08*g3=2.034cRTPowderg1=20.44,g2=5.1,**g3=2.34,g4=1.69,g5=1.294eLNTSolution1.9381.9818.706.514fRTPowder2.262.06**LNTSolutiong1=2.31,g2=2.06,14.84*g3=2.044gRTPowderg1=20.4,g2=5.24,**g3=2.37,g4=1.7,g5=1.31*unresolved.(a)
EPR spectrum of4a solution at LNT (Freq=9.06597GHz)(b)
EPR spectrum of4b solution at LNT (Freq=9.06786 GHz)(c)
EPR spectrum of4c powder at RT (Freq=9.38540 GHz)The EPR spectrum of complexes4aand4e indicates that the paramagnetic ion responsible is VO(II) having S=1/2 and I=7/2. A close look at the spectrum indicates a shoulder on hyperfine lines suggesting that the symmetry of the complex is lower than distorted octahedron. This is not a common observation, as the deviation from axial symmetry is not reported in powder spectrum. The room temperature powder spectrum of 4ewas also recorded. The calculated g and A values of 4e matched with the values of 4a. This suggests that the coordination around vanadyl ion is nearly the same in both 4aand4e except for a slight change in distortion [19].Powder EPR spectrum of4b was recorded at room temperature and 77 K. The hyperfine lines from copper nucleus are not resolved at room temperature spectrum due to dipole-dipole broadening. In order to obtain the hyperfine values, the complex was dissolved in DMF, and EPR spectrum was recorded at 77 K. The spectrum clearly indicates resonances from copper nucleus (63Cu/65Cu). The symmetry around the copper is lower than distorted octahedral as reflected from the three g values [20]. Also the three g values suggest that the coordination around the copper is six, which was confirmed by mass spectra (m/z 665).The powder EPR spectrum of4c at room temperature shows a number of resonances indicating that iron is under the influence of a strong tetragonal distortion. The range of g-values suggests that all the three Kramers’ doublets are populated at room temperature. The ESI-Mass of 4c complex (m/z 740) suggests that the complex is oxygen bridged bimetallic iron complex. Moreover oxobridged iron complexes are well known in many literatures [21]. The recorded solution EPR spectrum shows a single resonance at g=2. This kind of observation suggests that the dimeric iron complex might have become monomer after dissolution, hence a single line is observed [22]. The complex 4g behaves similar to 4c.



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*Source: 648589-2010-12-26.xml*