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. 2013 Oct 3;2013:981764. doi: 10.1155/2013/981764

Syntheses, Spectral Characterization, and Antimicrobial Studies on the Coordination Compounds of Metal Ions with Schiff Base Containing Both Aliphatic and Aromatic Hydrazide Moieties

Dinesh Kumar 1,*, Silky Chadda 1, Jyoti Sharma 1, Parveen Surain 2
PMCID: PMC3808720  PMID: 24198736

Abstract

An EtOH solution of 3-ketobutanehydrazide and salicylhydrazide on refluxing in equimolar ratio forms the corresponding Schiff base, LH3 (1). The latter reacts with Mn(II), Co(II), Ni(II), Cu(II), Zn(II), Cd(II), Zr(OH)2(IV), MoO2(VI), and UO2(VI) ions in equimolar ratio and forms the corresponding coordination compounds, [M(LH)(MeOH)3] (2, M = Mn, Co, Ni), [Cu(LH)]2 (3), [M′(LH)(MeOH)] (4, M′ = Zn, Cd), [Zr(OH)2(LH)(MeOH)2] (5), [MoO2(LH)(MeOH)] (6), and [UO2(LH)(MeOH)] (7). The coordination compounds have been characterized on the basis of elemental analyses, molar conductance, spectral (IR, reflectance, 1H NMR, ESR) studies, and magnetic susceptibility measurements. They are nonelectrolytes in DMSO. The coordination compounds, except 3, are monomers in diphenyl. They are active against gram-positive bacteria (S. aureus, B. subtilis), gram-negative bacteria (E. coli, P. aeruginosa), and yeast (S. cerevisiae, C. albicans). 1 acts as a dibasic tridentate ONO donor ligand in 2–7 coordinating through its both enolic O and azomethine N atoms. The coordination compounds 2 and 3 are paramagnetic, while rest of the compounds are diamagnetic. A square-planar structure to 3, a tetrahedral structure to 4, an octahedral structure to 2, 6, and 7, and a pentagonal bipyramidal structure to 5 are proposed.

1. Introduction

Aroyl hydrazones and their coordination compounds are known to possess the biological activities and inhibit many enzymatic reactions in the cell. Owing to their biological activities such as antifungal, antibacterial, antimycobacterial, antitumor, anti-inflammatory, anti-HIV, leishmanicidal, trypanocidal, inhibitor of anthrax lethal factor, antidiabetic, antimalarial, and antipyretic, there has been an increasing interest towards the studies of the coordination compounds of the Schiff bases containing the hydrazone moiety during the past few decades [1–12]. The coordination compounds containing hydrazone moiety have been reported to act as analytical reagents, such as polymer coatings, fluorescent materials [13, 14], enzymes inhibitors, antifungal/antibacterial agents [15, 16], and corrosion inhibitors [17]. A perusal of the literature reveals that much work has been carried out towards the coordination compounds of Schiff bases containing salicylhydrazide moiety [18–27]; however, no work seems to be reported on the coordination compounds of Schiff base derived from 3-ketobutanehydrazide and salicylhydrazide. Novel noncytotoxic salicylhydrazide-containing 1N inhibitors have been developed through substructure database search methods [28]. The developmental progress of the salicylhydrazide class of 1N inhibitors was halted due to cytotoxicity issues. The salicyloylhydrazide moiety has been reported to be the minimally required substructure for 1N inhibitory potency of the compounds [29]. The salicylhydrazides have also been proposed to inhibit 1N catalytic activity through chelation of the active site Mg2+, and they exhibit cytotoxicity in the nanomolar range. The replacement of one of the two phenols in N,N′-bis-salicylhydrazide with an optimally substituted heterocyclic group (heavily substituted triazole groups) renders a novel class of noncytotoxic salicylhydrazides, greatly enhancing the therapeutic potential of this class of 1N inhibitors. Keeping in view the above importance of the compounds possessing hydrazone moiety, we thought it worthwhile to synthesize and characterize the Schiff base, LH3 (1) and its coordination compounds with Mn(II), Co(II), Ni(II), Cu(II), Zn(II), Cd(II), Zr(OH)2(IV), MoO2(VI), and UO2(VI) ions. The Schiff base and its coordination compounds have also been studied for their antimicrobial activities.

2. Experimental

2.1. Materials

Manganese(II) acetate tetrahydrate, cobalt(II) acetate tetrahydrate, nickel(II) acetate tetrahydrate, copper(II) acetate monohydrate, ethyl acetoacetate, methyl salicylate [Loba Chemie], hydrazine hydrate [Fisher Scientific], ammonium molybdate tetrahydrate, cadmium(II) acetate dihydrate, zinc(II) acetate dihydrate, hexadecaaquaoctahydroxotetrazirconium(IV) chloride [BDH], dioxouranium(VI) acetate dihydrate [Hopkins and Williams (UK)], DMSO, DMF, MeOH, EtOH, 1,4-dioxane, and THF [Ranbaxy] were used as received for the syntheses. Bis(acetylacetonato)dioxomolybdenum(VI) and hexadecaaquaoctahydroxotetrazirconium(IV) acetate were synthesized according to the literature procedures [30, 31]. All the microbial cultures were procured from microbial type culture collection (MTCC), IMTECH, Chandigarh. The bacteria were subcultured on nutrient agar, whereas yeast was subcultured on malt yeast agar.

2.2. Analytical and Physical Measurements

The estimation of metal contents, spectral studies (IR, reflectance, 1H NMR, ESR), and the magnetic susceptibility measurements were carried out by the methods reported earlier [32]. The melting points of the compounds were determined on digital melting point apparatus (Stuart SMP-40). For the purification of KBHz, SHz and 1–7 chromatographic separations were carried out using silica gel columns (160–200 mesh) of varying length. Thin-layer chromatography (TLC) was performed on commercial Merck plates coated with a 0.20 mm layer of silica gel. The molar conductances of the coordination compounds in DMSO were carried out using Toshniwal conductivity bridge (Model CL01-02A) and a dip type cell calibrated with KCl solution. Carbon, hydrogen, and nitrogen contents of the compounds were determined on a FLASH EA 1112 CHNS (O) analyzer. The IR spectra of 1–7 were recorded in KBr (4000–250 cm−1) on a Fourier Transform Infrared spectrometer (Model RZX, Perkin Elmer). The reflectance spectra were recorded on a Hitachi-330 UV-vis-NIR spectrophotometer. 1H NMR spectra of 3-ketobutanehydrazide, 1, 4–7 were recorded on an Avance-II (Bruker) FT NMR spectrometer at 400 MHz using DMSO as a solvent and TMS as an internal standard. The mass spectrum of 1 was recorded on Waters Micromass Q-Tof Micro-mass spectrometer. The ESR spectrum of 3 was recorded at LNT in solid on a Varian E-112 ESR spectrometer with X-band microwave frequency (9.1 GHz) using tetracyanoethylene (TCNE) as a g-marker and monitoring the frequency with a frequency meter. The magnetic measurements were carried out at room temperature by Lakeshore VSM 7410 instrument. The antimicrobial studies of 1–7 were performed by agar well diffusion method [33–35].

2.3. Antibacterial Activity

A total of six microbial strains, that is, two gram-positive bacteria (S. aureus, B. subtilis), two gram-negative bacteria (E. coli, P. aeruginosa), and two yeasts (S. cerevisiae, C. albicans), were screened for evaluation of antibacterial and antifungal activities of 1–7. All the microbial cultures were adjusted to 0.5 McFarland standard, which were visually comparable to a microbial suspension of approximately 1.5 × 108 cfu/mL. 20 mL of agar medium was poured into each Petri plate, and the agar plates were swabbed with 100 μL inocula of each test microorganism and kept for 15 min for adsorption. Using sterile cork borer of 8 mm diameter, wells were bored into the seeded agar plates and these were loaded with a 100 μL volume with concentration of 2.0 mg/mL of each compound reconstituted in DMSO. All the plates were incubated at 37°C for 24 h. The antimicrobial activity of each compound was evaluated by measuring the zone of growth inhibition against the test microorganisms with zone reader (Hi antibiotic zone scale). DMSO was used as a negative control, whereas ciprofloxacin and amphotericin B were used as positive controls for bacteria and yeasts, respectively.

2.3.1. Determination of Minimum Inhibitory Concentration (MIC)

The minimum inhibitory concentration (MIC) is the lowest concentration of an antimicrobial compound that inhibits the visible growth of a microorganism after overnight incubation. MIC of the various compounds against bacterial and yeast strains was tested through a modified agar well diffusion method [36]. In this method, a two-fold serial dilution of each compound was prepared by first reconstituting the compound in DMSO followed by dilution in sterile distilled water to achieve a decreasing concentration range of 512 to 1 μg/mL. 100 μL of each dilution was introduced into wells (in triplicate) in the agar plates already seeded with 100 μL of standardized inoculums (106 cfu/mL) of the test microbial strain. All test plates were incubated aerobically at 37°C for 24 h, and the inhibition zones were observed. MIC was recorded for each test organism.

2.4. Synthesis and Characterization

2.4.1. Synthesis of 3-Ketobutanehydrazide (KBHz)

Hydrazine hydrate (5.0 g, 100 mmol) was added slowly with continuous stirring to an ice-cooled EtOH solution (20 mL) of ethyl acetoacetate (13.0 g, 100 mmol) during a period of 0.5 h. The reaction mixture was refluxed on a water bath for 2 h. The white compound separated out was suction filtered, washed with EtOH and recrystallised from EtOH, and dried in vacuo over silica gel at room temperature. The progress of the reaction was monitored on TLC using hexane and Et2O (1 : 1 v/v) as eluent. Color: white. M. p. = 188°C. Yield: 10.4 g (90%). Anal. Calcd. for C4H8N2O2: C, 41.38; H, 6.90; N, 24.06; Found: C, 41.24; H, 6.94; N, 24.14. IR bands (cm−1): 3298 ν(OH) (intramolecular H-bond), 2899 ν(N–H) (intramolecular H-bond), 1677 ν(C=O) (keto), 1618 δ(NH2), and 1041 ν(N–N) (hydrazide). 1H NMR (400 MHz; DMSO-d6; δ, ppm): 1.27 (s, 3H, –CH3), 2.58 (s, 2H, –CH2), 5.26 (br, 2H, –NH2) and 7.84 (br, 1H, –CONH).

2.4.2. Synthesis of Salicylhydrazide (SHz)

The title compound was synthesized according to the literature procedure [37]. The progress of the reaction was monitored on TLC using hexane and Et2O (1 : 1 v/v) as eluent. Color: white shining crystals. M. p. = 147°C. Yield: 11.4 g (75%). Anal. Calcd. for C7H8N2O2: C, 55.26; H, 5.26; N, 18.42; Found: C, 55.29; H, 5.21; N, 18.43. IR bands (cm−1): 3434 ν(OH) (intramolecular H-bond), 3320 ν(N–H) (intramolecular H-bond), 1735 ν(C=O) (keto), 1643 ν(C=N), 1607 δ(NH2), 1532 ν(C–O) (ϕ), 1252 ν(C–O) (enolic), 1035 ν(N–N) (hydrazide). 1H NMR (400 MHz; DMSO-d6; δ, ppm): 4.18 (s, 2H, –NH2), 6.80–8.04 (m, 4H, ArH), 9.90 (br, 1H, phenolic-OH) and 12.33 (br, 1H, enolic-OH).

2.4.3. Synthesis of 1

3-Ketobutanehydrazide (11.6 g, 100 mmol) and salicylhydrazide (15.2 g, 100 mmol) were refluxed in EtOH (50 mL) on a water bath for 2 h. The excess of solvent was distilled off, and the yellow compound separated out was allowed to stand at room temperature. The compound was suction filtered, washed with EtOH and recrystallized from EtOH, and dried as mentioned above. The progress of the reaction was monitored on TLC using hexane and Et2O (1 : 1 v/v) as eluent. Color: yellow. M. p. = 109°C. Yield: 22.5 g (90%). Anal. Calcd. for C11H14N4O3: C, 52.80; H, 5.60; N, 22.36; Found: C, 52.69; H, 5.71; N, 22.40. IR bands (cm−1): 3267 ν(OH) (intramolecular H-bond), 2720 ν(N–H) (intramolecular H-bond), 1619 ν(C=N) (azomethine), 1532 ν(C–O)ϕ, 1239 ν(C–O) (enol) and 1012 ν(N–N). 1H NMR (400 MHz; DMSO-d6; δ, ppm): 2.14 (s, 3H, –CH3), 2.56 (s, 2H, –CH2), 5.24 (d, 2H, –NH2), 6.84–7.80 (m, 4H, –ArH), 8.01 (s, 1H, –N=COH) (adjacent to aliphatic moiety), 9.87 (br, 1H, –OH) (phenolic), 12.24 (s, 1H, –N=COH) (adjacent to aromatic moiety).

2.4.4. Syntheses of 2–7

A MeOH solution (~30 mL) of appropriate metal acetate (5 mmol) was added to a MeOH solution (~100 mL) of 1 (1.25 g, 5 mmol) with constant stirring. The solution was refluxed on a water bath for 3-4 h, and the solid residue obtained was suction filtered, washed with MeOH, and dried as mentioned above. The resulting solids were recrystallized from dimethyl sulfoxide (DMSO). The progress of the reaction was monitored on TLC using hexane and Et2O (1 : 1 v/v) as eluent. Color: mentioned in Table 1. Yield: 50–75%. The compounds are stable up to 250°C, and they get decomposed above this temperature. 1H NMR spectral data of these coordination compounds are given in Table 3. We were unable to get the compounds (1–7) in crystalline forms; therefore, their studies related with X-ray structural determinations could not be carried out.

Table 1.

Analytical, colour, molar conductance (Ω−1 cm2 mol−1), mass spectral, and molecular weight data of compounds.

S. no. Compound Stoichiometry Colour Yield
g (%)		 ΛM (Ω−1 cm2 mol−1) Found (calcd)
M. Wt. M% C% H% N%
(1) 1 C11H14N4O3 Yellow 22.5 (90) — 250.1a (250) — 52.69 (52.80) 5.71 (5.60) 22.36 (22.40)
(2) 2 (M = Mn) MnC14H24N4O6 Grey 1.14 (57) 11.7 352.6b (398.9) 13.63 (13.76) 42.08 (42.12) 6.11 (6.02) 14.17 (14.04)
(3) 2 (M = Co) CoC14H24N4O6 Brown 1.25 (62) 10.3 423.4b (402.9) 14.43 (14.62) 41.82 (41.70) 5.88 (5.96) 13.72 (13.90)
(4) 2 (M = Ni) NiC14H24N4O6 Purple 1.37 (68) 9.2 392.6b (402.7) 14.67 (14.58) 41.79 (41.72) 5.87 (5.96) 13.73 (13.91)
(5) 3 Cu2C22H24N8O6 Dark Green 1.12 (72) 6.8 618.4b (623.0) 20.52 (20.39) 42.46 (42.38) 3.73 (3.85) 17.82 (17.98)
(6) 4 (M′ = Zn) ZnC12H16N4O4 Yellow 0.86 (50) 5.6 363.9b (345.4) 18.65 (18.93) 41.52 (41.69) 4.73 (4.63) 16.08 (16.21)
(7) 4 (M′ = Cd) CdC12H16N4O4 White 1.18 (60) 5.2 387.3b (392.4) 28.52 (28.64) 36.82 (36.70) 4.13 (4.08) 14.31 (14.27)
(8) 5 ZrC13H22N4O7 Yellow 1.64 (75) 5.0 425.8b (437.2) 20.93 (20.86) 35.63 (35.68) 5.08 (5.03) 12.72 (12.81)
(9) 6 MoC12H16N4O6 Yellow 1.18 (58) 4.7 419.6b (407.9) 23.48 (23.51) 35.23 (35.30) 3.84 (3.92) 13.52 (13.73)
(10) 7 UC12H16N4O6 Orange 1.79 (65) 3.6 541.7b (550.0) 43.44 (43.27) 26.36 (26.18) 2.88 (2.91) 10.02 (10.18)
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Abbreviations: amass spectral data and bRast method data.

Table 3.

NMR spectral data of the coordination compounds.

S. no. Compound Stoichiometry 1H NMR (400 MHz; DMSO-d6) δ (ppm)
(1) 4 (M′ = Zn) ZnC12H16N4O4 1.27 (t, 3H, –CH3), 2.06 (s, 3H, –CH3) (MeOH),
2.56 (s, 1H, –CH), 3.53 (br, 1H, –OH) (MeOH), 5.14 (d, 2H, –NH2), 6.94–7.80 (m, 4H, Ar–H), 8.50 (br, 1H, –NH), 9.87 (br, 1H, –OH) (phenolic)
(2) 4 (M′ = Cd) CdC12H16N4O4 1.25 (t, 3H, –CH3), 2.15 (s, 3H, –CH3) (MeOH),
2.58 (s, 1H, –CH), 3.16 (br, 1H, –OH) (MeOH),
5.14 (d, 2H, –NH2), 6.74–7.88 (m, 4H, Ar–H), 8.56 (br, 1H, –NH), 9.87 (br, 1H, –OH) (phenolic)
(3) 5 ZrC13H22N4O7 1.30 (t, 3H, –CH3), 2.15 (s, 3H, –CH3) (MeOH), 2.50 (s, 3H, –CH3) (MeOH), 2.58 (s, 1H, –CH), 3.16 (br, 2H, –OH), 3.26 (br, 2H, –OH) (MeOH), 5.14 (d, 2H, –NH2), 6.74–7.88 (m, 4H, Ar–H), 8.72 (br, 1H, –NH), 9.87 (br, 1H, –OH) (phenolic)
(4) 6 MoC12H16N4O6 1.25 (t, 3H, –CH3), 2.25 (s, 3H, –CH3) (MeOH),
2.56 (s, 1H, –CH), 3.45 (br, 1H, –OH) (MeOH),
5.11 (d, 2H, –NH2), 6.53–7.50 (m, 4H, Ar–H), 8.87 (br, 1H, –CONH), 9.90 (br, 1H, –OH) (phenolic)
(5) 7 UC12H16N4O6 1.25 (t, 3H, –CH3), 2.35 (s, 3H, –CH3) (MeOH),
2.56 (s, 1H, –CH), 3.52 (br, 1H, –OH) (MeOH),
5.14 (d, 2H, –NH2), 6.66–7.52 (m, 4H, Ar–H), 8.87 (br, 1H, –CONH), 9.90 (br, 1H, –OH) (phenolic)
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3. Results and Discussion

The nucleophilic addition reaction between 3-ketobutanehydrazide and salicylhydrazide in equimolar ratio in EtOH followed by the elimination of one water molecule results in the formation of the Schiff base, LH3 (1) (Scheme 1).

Scheme 1.

Scheme 1

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Synthesis of the Schiff base.

A MeOH solution of 1 reacts with a MeOH solution of Mn(II), Co(II), Ni(II), Cu(II), Zn(II), Cd(II), Zr(OH)2(IV), MoO2(VI), and UO2(VI) ions and forms the corresponding coordination compounds, 2–7 (Scheme 2).

Scheme 2.

Scheme 2

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Synthesis of complexes 2-7.

The coordination compounds are insoluble in H2O, EtOH, dioxane, and THF, but they were soluble in DMF and DMSO. Their molar conductance data (3.6–11.7 Ω−1 cm2 mol−1 in DMSO) reveal their nonelectrolytic nature. They are stable up to 250°C and get decomposed above this temperature. Attempts to obtain single crystal suitable for X-ray determination were unsuccessful. The structures of the synthesized ligand and metal complexes (Schemes 1 and 2) were established with the help of elemental analyses data, IR and NMR spectra.

3.1. Infrared Spectral Studies

The IR spectra of KBHz and 1–7 were recorded in KBr. The ν(C=N) (azomethine) stretch of 1 shifts to lower energy by 7–24 cm−1 indicating coordination through its azomethine N atom [38]. The ν(C–O)ϕ stretch of 1 occurring at 1532 cm−1 remains unaltered in 2–7 indicating the noninvolvement of phenolic O atom towards coordination [39]. The ν(C–O) (enolic) stretch of the Schiff base shifts from 1239 cm−1 to higher energy by 8–18 cm−1 in 2–7 indicating coordination through its enolic O atom [39]. Thus, 1 behaves as a dibasic tridentate ONO donor ligand in 2–7 coordinating through its azomethine N and both enolic O atoms. The involvement of enolic O and azomethine N atoms towards coordination is further supported by the appearance of new nonligand bands between 571–594 and 478–483 cm−1 due to the ν(M–O) and ν(M–N) vibrations in 2–7. These bands are in the expected order of increasing energy: ν(M–N) < ν(M–O) [40] as expected due to the greater dipole moment change in the M–O vibration, greater electronegativity of the O atom than N atom, and shorter M–O bond length than the M–N bond length [41]. The absence of a band, between 835–955 cm−1, characteristic of the ν(Zr=O) stretch [42] and the appearance of a new band at 1125 cm−1 due to δ(Zr–OH) bending mode in 5 suggests the structure of 5 structure as [Zr(OH)2(LH)(MeOH)2] and not as [ZrO(H2O)(LH)(MeOH)2]. The ν s(O=Mo=O) and ν as(O=Mo=O) stretches occur at 925 and 900 cm−1, respectively in 6, and these bands occur in the usual range (892–964 cm−1; 840–925 cm−1) reported for the majority of MoO2(VI) compounds [43]. The presence of the ν s(O=Mo=O) and ν as(O=Mo=O) bands indicates a cis-MoO2 structure as the compounds with a trans-MoO2 structure exhibit only the ν as(O=Mo=O) stretch since the ν s(O=Mo=O) stretch is IR inactive [44]. The absence of a band at ~770 cm−1 in the present MoO2(VI) coordination compound indicates the absence of an oligomeric structure with ⋯Mo=O⋯Mo=O⋯ interaction [43]. The ν as(O=U=O) stretch in 7 occurs at 930 cm−1. This band occurs in the usual range (870–950 cm−1) observed for the majority of trans-UO2 compounds [45].

3.2. Reflectance Spectral Studies

The coordination compound 2 (M = Mn) shows three bands at 15860, 21275, and 25850 cm−1 due to the 6 A 1g → 4 T 1g(G)(ν 1), 6 A 1g → 4 T 2g(G)(ν 2) and 6 A 1g → 4 A 1g(G) (ν 3) transitions, respectively, in an octahedral environment [46]. The coordination compound 2 (M = Co) shows three bands at 9091, 13698 and 19820 cm−1 due to the 4 T 1g(F) → 4 T 2g(F)(ν 1), 4 T 1g(F) → 4 A 2g(F)(ν 2) and 4 T 1g(F) → 4 T 1g(P)(ν 3) transitions, respectively, in an octahedral environment [46]. Using the free ion value of B = 971 cm−1, the values of spectral parameters [46] in 2 (M = Co) are as follows: 10Dq = 10253 cm−1, B′ = 792.74 cm−1, β = B′/B = 0.82, β 0 = 18% and CFSE = –98.20 kJ mol−1. The value of ν 3/ν 1 is 2.18, and this value falls in the usual range (2.00–2.80) observed for the majority of octahedral Co(II) coordination compounds [46]. The coordination compound 2 (M = Ni) shows three bands at 9250, 15360, and 24095 cm−1 due to the 3 A 2g(F) → 3 T 2g(F)(ν 1), 3 A 2g(F) → 3 T 1g(F)(ν 2) and 3 A 2g(F) → 3 T 1g(P)(ν 3) transitions, respectively, suggesting an octahedral geometry around the metal ion [46]. Using the free ion value of B = 1030 cm−1, the values of spectral parameters in 2 (M = Ni) are as follows: 10Dq = 9250 cm−1, B′ = 743.74 cm−1, β = 0.72, β 0 = 28%, and CFSE = –132.79 kJ mol−1. The value of the ν 2/ν 1 is 1.66, and this value lies in the usual range (1.6–1.8) reported for the majority of octahedral Ni(II) coordination compounds [46]. The 10Dq value of the Co(II) coordination compound is greater than that of the corresponding Ni(II) coordination compound 10253 cm−1 > 9250 cm−1. This is in line with the spectrochemical series of metal ions for a given ligand, given stoichiometry, and a given stereochemistry: Co(II) > Ni(II) [46]. The β 0 value of the Co(II) coordination compound is less as compared to that of the corresponding Ni(II) coordination compound: 18% < 28%. This is in line with the nephelauxetic metal ion series in terms of β and β 0 for a given ligand, a given stoichiometry, and a given stereochemistry [46]. The coordination compound 3 shows two bands: one at 14750 cm−1 and the other at 20150 cm−1 due to the 2 B 1g → 2 A 1g and 2 B 1g → 2 E g transitions, respectively, indicating a square-planar configuration around the metal ion [46] (Table 2).

Table 2.

IR, reflectance spectral data (cm−1), and magnetic moments of the coordination compounds.

S. no. Compound ν (C=N) (azomethine) ν (C–O) (enolic)
 ν max⁡ (cm−1) Magnetic moment (B.M.)
(1) 1 1619 1239 — —
(2) 2 (M = Mn) 1604 1256 15860, 21275, 25850 5.86
(3) 2 (M = Co) 1601 1247 9091, 13698, 19820 4.78
(4) 2 (M = Ni) 1605 1257 9250, 15360, 24095 3.17
(5) 3 1605 1248 14750, 20150 1.76
(6) 4 (M′ = Zn) 1606 1257 — Diamagnetic
(7) 4 (M′ = Cd) 1608 1254 — Diamagnetic
(8) 5 1612 1250 — Diamagnetic
(9) 6 1598 1252 — Diamagnetic
(10) 7 1595 1248 — Diamagnetic
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3.3. 1H NMR Studies

The 1H NMR spectra of KBHz, 1 and 4–7 were recorded in DMSO-d6. The chemical shifts (δ) are expressed in ppm downfield from TMS [47]. The Schiff base (1) exhibits a singlet at δ 2.14 ppm due to the methyl protons, a singlet at δ 2.56 ppm due to the methylene proton, a doublet at δ 5.24 ppm due to the –NH2 protons, a broad signal at δ 9.87 ppm due to the phenolic proton, a multiplet at δ 6.84–7.80 ppm due to the aromatic protons, a singlet at δ 8.01 ppm due to –N=COH (adjacent to aliphatic moiety) proton, and a singlet at δ 12.24 ppm due to –N=COH (adjacent to aromatic moiety) proton. The absence of the resonance signals at δ 8.01 ppm and δ 12.24 ppm due to the enolic protons (adjacent to aliphatic and aromatic moieties, resp.) in 4–7 indicates the deprotonation of the enolic protons followed by the involvement of both enolic O atoms towards coordination.

3.4. ESR Spectral Studies

The ESR spectrum of 3 in DMSO at liquid nitrogen temperature was recorded in X-band, using 100 kHz field modulation, and the g values are relative to the standard marker, tetracyanoethylene (TCNE) (g = 2.0023). The observed values of g ||, g ⊥, g av, and G are 2.15, 2.08, 2.11, and 1.84, respectively. From the observed values of various parameters, it is concluded that the unpaired electron lies in d x 2 − y 2 orbital giving 2 B 1 as the ground state with g || > g ⊥ > 2, indicating square planar geometry around the copper(II) ion [48, 49].

3.5. Magnetic Measurements

The magnetic moments of 2 (M = Mn, Co, Ni) are 5.86, 4.78, and 3.17 B.M., respectively. These values lie in the normal ranges reported for the majority of magnetically dilute octahedral compounds of Mn(II), Co(II), and Ni(II) ions [46]. The magnetic moment of 3 (M = Cu) is 1.76 B.M. indicating square planar geometry around the Cu(II) ion [46]. The coordination compounds 4–7 are diamagnetic.

3.6. Antimicrobial Studies

The newly synthesized compounds (1–7) were screened for their antibacterial and antifungal activities (Tables 4 and 5). The compounds 1, 2 (M = Co, Ni) and 3–7 possessed variable antibacterial activities against the gram-positive bacteria (S. aureus, B. subtilis). The compounds 3 and 4 (M′  = Zn) displayed activities against gram-negative bacteria (E. coli). The compound 2 (M = Mn) displayed antifungal activities against yeasts (S. cerevisiae, C. albicans). Positive controls produced significantly sized inhibition zones against the tested bacteria and fungi; however, negative control produced no observable inhibitory effect against any of the test organisms (Figures 1 and 2). On the basis of maximum inhibitory activities shown against gram-positive bacteria, the compounds 3 and 4 (M′  = Zn) were found to be most effective against S. aureus with zone of inhibition of 22.6 mm and 21.3 mm. The compound 3 was found to be most effective against B. subtilis showing the zone of inhibition of 25.3 mm. Among gram-negative bacteria, the compounds 3 and 4 (M′  = Zn) displayed antibacterial activities with zone of inhibition of 15.3 mm and 12.6 mm against E. coli. The compound 2 (M = Mn) showed zone of inhibition ranging between 13.0 mm against S. cerevisiae and 15.3 mm against C. albicans. The MIC of various compounds ranged between 16 μg/mL and 256 μg/mL against gram-positive bacteria, while it ranged between 128 μg/mL and 512 μg/mL against gram-negative bacteria. The compounds 3 and 4 (M′ = Zn) were found to be the best as they exhibit the lowest MIC of 32 μg/mL against S. aureus. The compound 3 showed lowest MIC of 16 μg/mL against B. subtilis. However, in case of yeasts, the compound 2 (M = Mn) showed MIC value of 128 μg/mL. The compound 3 was found to be the best in inhibiting the growth of bacteria; thus, it can be further used as an antibacterial agent in pharmaceutical industry for mankind, after testing its toxicity to human beings. It is worth to mention that the antimicrobial activity of the ligand (1) is greatly enhanced after coordination [50–52]. The lipid membrane surrounding the cell favours the passage of only lipid-soluble materials; therefore, the liposolubility is an important factor which controls the antimicrobial activity [53, 54]. On chelation, the polarity of the metal ion is reduced to a greater extent due the overlapping of the ligand orbital and partial sharing of the positive charge of the metal ion with donor groups. Moreover, delocalization of the π-electrons over the whole chelate ring is increased and the lipophilicity of the coordination compounds is enhanced. The increased lipophilicity enhances the penetration of the coordination compounds into the lipid membranes and blocks the metal binding sites in the enzymes of microorganisms. These coordination compounds also disturb the respiration process of the cell and thus block the synthesis of proteins, which restricts further growth of the microorganisms. In general, coordination compounds are more active than ligand.

Table 4.

In  vitro antimicrobial activity of synthetic chemical compounds through agar well diffusion method.

Compound
no.		 Diameter of growth of inhibition zone (mm)a
S.  aureus B.  subtilis E.  coli P.  aeruginosa S.  cerevisiae C.  albicans
1 19.3 21.6 — — — —
2 (M = Mn) — — — — 13.0 15.3
2 (M = Co) 15.3 17.3 — — — —
2 (M = Ni) 13.6 15.6 — — — —
3 22.6 25.3 15.3 — — —
4 (M′ = Zn) 21.3 22.6 12.6 — — —
4 (M′ = Cd) 18.6 20.3 — — — —
5 14.6 19.3 — — — —
6 16.3 22.3 — — — —
7 17.6 20.6 — — — —
Ciprofloxacin 26.6 24.0 25.0 22.0 — —
Amphotericin B — — — — 19.3 16.6
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—: no activity, avalues, including diameter of the well (8 mm), are means of three replicates.

Table 5.

Minimum inhibitory concentration (MIC) (µg/mL) of compounds by using modified agar well diffusion method.

Compound no. S.  aureus B.  subtilis E.  coli P.  aeruginosa S.  cerevisiae C.  albicans
1 64 32 — — — —
2 (M = Mn) — — — — 128 128
2 (M = Co) 128 128 — — — —
2 (M = Ni) 256 128 — — — —
3 32 16 128 — — —
4 (M′ = Zn) 32 32 512 — — —
4 (M′ = Cd) 64 64 — — — —
5 64 64 — — — —
6 64 32 — — — —
7 128 128 — — — —
Ciprofloxacin 6.25 6.25 6.25 6.25 — —
Amphotericin B — — — — 12.5 12.5
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—: no activity.

Figure 1.

Figure 1

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Bar Chart indicating the diameter of growth of inhibition zone for compounds/standard against various microbes.

Figure 2.

Figure 2

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Bar Chart indicating minimum inhibitory concentration (MIC) (μg/mL) for compounds/standard against various microbes. Abbreviations: Sa: S. aureus, Bs: B. subtilis, Ec: E. coli, Pa: P. aeruginosa, Sc: S. cerevisiae, Ca: C. albicans.

4. Conclusions

On the basis of the analytical data, valence requirements, conductance, spectral studies, and magnetic susceptibility measurements, it is proposed that 1 acts as a monobasic tridentate ONO donor ligand in 2–7 coordinating through its azomethine N and both enolic O atoms. 2 and 3 are paramagnetic, while 4–7 are diamagnetic. The data suggest a square-planar structure to 3, a tetrahedral structure to 4, an octahedral structure to 2, 6, and 7, and a pentagonal bipyramidal structure to 5. The coordination compounds show significant enhanced antimicrobial activities as compared to the free Schiff base (Scheme 3). Therefore, these compounds can be further used in pharmaceutical industry as antimicrobial agents for mankind, after testing its toxicity to human beings.

Scheme 3.

Scheme 3

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Acknowledgment

Silky Chadda is highly thankful to the authorities of the National Institute of Technology, Kurukshetra, Haryana, India, for providing an institutional fellowship to carry out the above work.

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