# Spectral Investigation andIn Vitro Antibacterial Evaluation of NiII and CuII Complexes of Schiff Base Derived from Amoxicillin and α-Formylthiophene (αft)

Authors: Narendra Kumar Chaudhary; Parashuram Mishra
Journal: Journal of Chemistry
 (2015)

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## Abstract

Two new metal complexes of general formula M(Haαft)2 [M = NiII and CuII] of asymmetrical Schiff base ligand (HL = Haαft) derived from amoxicillin and α-formylthiophene have been prepared and characterized by various physicochemical and spectral techniques. Molar conductance measurement indicates nonelectrolytic nature of the metal complexes. FT-IR spectral study reveals the ligation of metal ions at two different nitrogen [NN] donor sites of Haαft. FT-IR and electronic absorption spectral evidences suggest distorted tetrahedral and square planar geometry for CuII and NiII complexes, respectively. The structure optimization by molecular mechanics (MM) force field calculation through ArgusLab 4.0.1 version software also supports the concerned geometry of the complexes. The cell dimensions as suggested by XRPD study, a (6.753 Å), b (13.904 Å), c (20.122 Å), α (142.76°), β (106.580°), and γ (72.4343°) for CuII and a (24.2547 Å), b (6.6371 Å), c (5.5047 Å) (α = β = γ = 90°) for NiII complexes, are in good agreement with their triclinic and orthorhombic crystal systems. Particle size calculation by Scherrer’s formula indicates nanocrystalline nature of the complexes. The antibacterial sensitivity study suggests promising activities of Haαft (Ligand) and M(Haαft)2 complexes against four clinical pathogenic bacteria, namely,E. coli,P. vulgaris,P. aeruginosa, andS. aureus, though being less active than the standard drug amikacin.


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## Body

## 1. Introduction

Increasing threat of drug resistance caused by several microorganisms is today’s most debated public health concern. The development and modifications in the design of previous antibiotics, with new modes of action, requires intensive research to overcome these infections [1]. Schiff bases are the chemical compounds prepared by the condensation of active carbonyl groups with primary amines and have active azomethine linkage. Due to simplicity in preparation and wide range of applications in medical, biochemical, and industrial fields, Schiff bases are gaining much popularity in the recent years [2]. Presence of various coordination sites makes them as privileged ligands in the coordination chemistry of transition metals [3]. Schiff bases have important applications in the medical science as a potent antibacterial [4], antitumor [5], antiviral [6], and anti-inflammatory drugs [7]. The pharmacological activity of this class of compounds is often enhanced by complexation with metal ions. Serendipitous finding of cisplatin as a potent anticancer drug opened the gate of unexplored world of metal based chemotherapeutic agents [8, 9]. Recently, metal based drugs are gaining significant importance in medical sciences, due to their increased potentiality that actively interrupts the growth eager mechanism of microorganisms. The central metal ion in metal based drugs is usually the key feature of the mechanism of action. Several medical problems that arise due to free metal ion toxicity may be ameliorated by chelating agents like Schiff bases [10]. Amoxicillin is a very important class of β-lactamic antibiotic used in clinical therapy due to its specific toxicity towards bacterial pathogens [11]. Broad spectrum activity of amoxicillin is related to better oral absorption and high concentrations in blood compared to ampicillin which effectively works against bacteria. However, the failure in its antibacterial activity has been attributed to the formation of β-lactamase enzyme which hydrolyzes the β-lactam ring of the molecule [12]. Several research findings in the medical science put amoxicillin as an abortive drug and require modifications, either by changing the ligand property or by complexation with metal ions. With this expectation, metal complexes of amoxicillin derived Schiff base will be the new hope for better drug substance in clinical practices. In the present investigation, we report here the synthesis, spectral characterization, coordination behavior, X-ray powder diffraction study, and antibacterial evaluation of NiII and CuII complexes of Schiff base ligand (Haαft) derived from amoxicillin and α-formylthiophene. The work has been extended to assure the correct geometry by MM2 calculations supported in CsChemOffice 3D ultra and ArgusLab 4.0.1 version software.


## 2. Experimental Section

### 2.1. Materials

All the chemicals and solvents used in the experiment were of analytical reagent grade (AR). They included amoxicillin trihydrate (Duchefa Biochemie, Netherland),α-formylthiophene (Spectrochem, Mumbai, India), and metal salts, namely, NiCl2·6H2O and CuCl2·2H2O (Merck). Distilled methanol (Qualigen) was used as solvent for the synthesis. All the glassware used in the research was of high grade borosilicate glass and was cleaned by triple distilled water. For the antibacterial sensitivity study, the bacterial cultures were prepared in Muller Hinton’s nutrient agar media (Himedia Co.).


### 2.2. Measurements

The elemental microanalysis (C, H, and N) of the complexes was analyzed on Elementar vario EL III (Germany) model Analyzer. Double-check method was done to get the accuracy of the data. The pH measurement was done in Elico-16 pH meter. The electronic absorption spectra that reveal d-d andπ-πand  n-π transitions of the ligand and its complexes were recorded in single beam microprocessor Labtronics UV-Vis. spectrophotometer (LT-290 model) using DMSO as the solvent and internal reference chemical in 200–800 nm range. Characteristic shifts in IR band positions had been analyzed by intimate observations of infrared spectra of ligand and metal complexes that were run as KBr discs in the range 4000–400 cm−1 on a Perkin Elmer 783 FT-IR spectrophotometer. 1H NMR spectra were recorded in DMSO-d6 solvent on a Bruker advance 400 MHz instrument using TMS as internal reference. ESI-MS spectra were accomplished on Agilent 6520 Q-TOF mass spectrometer equipped with an electron spray ionization source in the mass range of 200 to 1100. The XRD powder pattern was recorded on a vertical type Philips PW 1130/00 X-ray diffractometer, operated at 40 kV and 50 Ma generator using the monochromatised Cu-Kα line at wavelength 1.54056 Å as the radiation source and measurements were taken over the range of 2θ (10 to 80°). Crystallographic data were analyzed by X′Pert High Score, CRYSFIRE, and CHECKCELL software programme. The powder XRD pattern of the ligand and metal complexes was recorded in Xpowder software. The possible geometries of the metal complexes were evaluated by using the molecular modeling calculation, optimized by CsChem 3D Utra-11 programme and ArgusLab 4.0.1 version software.


### 2.3. Synthesis of Ligand (HL = Haαft)

To the hot and homogenously stirred solution of amoxicillin trihydrate (5 mmol, 2.097 gm) in distilled methanol (30 mL),α-formylthiophene (5 mmol, 0.47 mL) was added dropwise with constant stirring and the resulting solution was refluxed for about 6 h. The pH of the amoxicillin trihydrate solution had been adjusted to 8 by dropwise addition of alcoholic NaOH solution [13]. The solution was concentrated and allowed to cool. The bright yellow solid product was separated by slow diffusion process, purified by recrystallization from hot methanol and dried under vacuum. The synthetic design for the preparation of ligand (HL) is presented in Scheme 1.Scheme 1
Proposed route for the synthesis of ligand (HL).


### 2.4. Synthesis of Metal Complexes

In hot 30 mL methanolic solution of ligand (L) (4 mmol, 1.89 gm), 10 mL methanolic solution of the metal salts (2 mmol, 0.4752 gm NiCl2·6H2O, and 0.34 gm CuCl2·2H2O) was added dropwise under constant stirring over magnetic stirrer. The reaction mixture was refluxed for several hours under water bath and alternate stirring of the mixture was also done to facilitate the easy approach of ligand for coordination with metal ion. Colored solid complexes were formed on cooling the solution slowly at room temperature. The solid was filtered, washed with methanol, and dried under vacuum [14, 15]. The general structure of metal complex is presented in Figure 1:(1)MX2+2HL→RefluxML2where MX2 is NiII&CuII chloride salts. HL is Ligand. NiII-complex is Ni(Haαft)2. CuII-complex is Cu(Haαft)2.Figure 1
Structure of metal complex (M = Ni & Cu).


### 2.5. Antibacterial Assay

The experimental portion of antibacterial study was carried out in microbiology laboratory of MMAM campus Biratnagar. The ligand (HL) and its metal complexes were screenedin vitro for antibacterial sensitivity study against three Gram-negative and one Gram-positive bacterial strains using modified Kirby-Bauer paper disc diffusion method [16]. Mueller-Hinton’s nutrient agar media were applied for the bacterial growth. Fresh cultures of standard bacteria, namely,Escherichia coli,Proteus vulgaris,Pseudomonas aeruginosa, andStaphylococcus aureus, were inoculated separately in five mL of tryptone soya broth, maintaining pH at 7.4 for better growth. The broth was incubated for 8 h at 37°C until visible growth changes to opaqueness. The broth was spread over nutrient agar media, prepared as usual in Petri plates using sterile stick swab and the well-sterilized paper discs of five mm diameter (Whatman number 1) impregnated with test compounds at two different concentrations, 1 and 0.1 μg/μL, in DMSO were stuck on the previously seeded bacterial culture [17]. The growth inhibition was compared with the standard drug amikacin of 30 μg per disc of six mm size (Himedia Co.). DMSO, which exhibited no antimicrobial activity against the test bacterial pathogens, was used as negative control. Afterwards, the Petri plates were incubated at 37°C and the inhibition of the growth of organisms, evidenced by clearing zone surrounding each disc, was measured by using antibiogram zone measuring scale, after 36 h of incubation [18].


## 2.1. Materials

All the chemicals and solvents used in the experiment were of analytical reagent grade (AR). They included amoxicillin trihydrate (Duchefa Biochemie, Netherland),α-formylthiophene (Spectrochem, Mumbai, India), and metal salts, namely, NiCl2·6H2O and CuCl2·2H2O (Merck). Distilled methanol (Qualigen) was used as solvent for the synthesis. All the glassware used in the research was of high grade borosilicate glass and was cleaned by triple distilled water. For the antibacterial sensitivity study, the bacterial cultures were prepared in Muller Hinton’s nutrient agar media (Himedia Co.).


## 2.2. Measurements

The elemental microanalysis (C, H, and N) of the complexes was analyzed on Elementar vario EL III (Germany) model Analyzer. Double-check method was done to get the accuracy of the data. The pH measurement was done in Elico-16 pH meter. The electronic absorption spectra that reveal d-d andπ-πand  n-π transitions of the ligand and its complexes were recorded in single beam microprocessor Labtronics UV-Vis. spectrophotometer (LT-290 model) using DMSO as the solvent and internal reference chemical in 200–800 nm range. Characteristic shifts in IR band positions had been analyzed by intimate observations of infrared spectra of ligand and metal complexes that were run as KBr discs in the range 4000–400 cm−1 on a Perkin Elmer 783 FT-IR spectrophotometer. 1H NMR spectra were recorded in DMSO-d6 solvent on a Bruker advance 400 MHz instrument using TMS as internal reference. ESI-MS spectra were accomplished on Agilent 6520 Q-TOF mass spectrometer equipped with an electron spray ionization source in the mass range of 200 to 1100. The XRD powder pattern was recorded on a vertical type Philips PW 1130/00 X-ray diffractometer, operated at 40 kV and 50 Ma generator using the monochromatised Cu-Kα line at wavelength 1.54056 Å as the radiation source and measurements were taken over the range of 2θ (10 to 80°). Crystallographic data were analyzed by X′Pert High Score, CRYSFIRE, and CHECKCELL software programme. The powder XRD pattern of the ligand and metal complexes was recorded in Xpowder software. The possible geometries of the metal complexes were evaluated by using the molecular modeling calculation, optimized by CsChem 3D Utra-11 programme and ArgusLab 4.0.1 version software.


## 2.3. Synthesis of Ligand (HL = Haαft)

To the hot and homogenously stirred solution of amoxicillin trihydrate (5 mmol, 2.097 gm) in distilled methanol (30 mL),α-formylthiophene (5 mmol, 0.47 mL) was added dropwise with constant stirring and the resulting solution was refluxed for about 6 h. The pH of the amoxicillin trihydrate solution had been adjusted to 8 by dropwise addition of alcoholic NaOH solution [13]. The solution was concentrated and allowed to cool. The bright yellow solid product was separated by slow diffusion process, purified by recrystallization from hot methanol and dried under vacuum. The synthetic design for the preparation of ligand (HL) is presented in Scheme 1.Scheme 1
Proposed route for the synthesis of ligand (HL).


## 2.4. Synthesis of Metal Complexes

In hot 30 mL methanolic solution of ligand (L) (4 mmol, 1.89 gm), 10 mL methanolic solution of the metal salts (2 mmol, 0.4752 gm NiCl2·6H2O, and 0.34 gm CuCl2·2H2O) was added dropwise under constant stirring over magnetic stirrer. The reaction mixture was refluxed for several hours under water bath and alternate stirring of the mixture was also done to facilitate the easy approach of ligand for coordination with metal ion. Colored solid complexes were formed on cooling the solution slowly at room temperature. The solid was filtered, washed with methanol, and dried under vacuum [14, 15]. The general structure of metal complex is presented in Figure 1:(1)MX2+2HL→RefluxML2where MX2 is NiII&CuII chloride salts. HL is Ligand. NiII-complex is Ni(Haαft)2. CuII-complex is Cu(Haαft)2.Figure 1
Structure of metal complex (M = Ni & Cu).


## 2.5. Antibacterial Assay

The experimental portion of antibacterial study was carried out in microbiology laboratory of MMAM campus Biratnagar. The ligand (HL) and its metal complexes were screenedin vitro for antibacterial sensitivity study against three Gram-negative and one Gram-positive bacterial strains using modified Kirby-Bauer paper disc diffusion method [16]. Mueller-Hinton’s nutrient agar media were applied for the bacterial growth. Fresh cultures of standard bacteria, namely,Escherichia coli,Proteus vulgaris,Pseudomonas aeruginosa, andStaphylococcus aureus, were inoculated separately in five mL of tryptone soya broth, maintaining pH at 7.4 for better growth. The broth was incubated for 8 h at 37°C until visible growth changes to opaqueness. The broth was spread over nutrient agar media, prepared as usual in Petri plates using sterile stick swab and the well-sterilized paper discs of five mm diameter (Whatman number 1) impregnated with test compounds at two different concentrations, 1 and 0.1 μg/μL, in DMSO were stuck on the previously seeded bacterial culture [17]. The growth inhibition was compared with the standard drug amikacin of 30 μg per disc of six mm size (Himedia Co.). DMSO, which exhibited no antimicrobial activity against the test bacterial pathogens, was used as negative control. Afterwards, the Petri plates were incubated at 37°C and the inhibition of the growth of organisms, evidenced by clearing zone surrounding each disc, was measured by using antibiogram zone measuring scale, after 36 h of incubation [18].


## 3. Results and Discussion

The carboxylic acid group (-COOH) of amoxicillin undergoes esterification with methanol. Esterified amoxicillin now interacts withα-formylthiophene for the formation of ligand. The ligand was soluble in methanol and polar solvents like DMSO and DMF. The melting points of ligand (195°C) and metal complexes (>210°C) suggested that the complexes are more stable than the ligand and all of them are air and moisture stable. IR spectral measurements are completely consistent with the proposed formulation of the ligand and complexes.


### 3.1. Physical Data and Microelemental Analysis

The Schiff base ligand and its metal complexes were subjected to elemental analysis. The results of elemental analysis with molecular formula and other physical data like melting points and color change of the compounds are presented in Table1. The results are in good agreement with suggested molecular formula. Sharp melting point of compounds indicates the purity of the prepared compounds [19].Table 1
Elemental analysis and physical properties measurement data.
Compound
Mol. formula
Mol. wt.
Colour
m. pt. (°C)
Calculated (found) (%)
pH
C
H
N
O
S
M
HL
C22H23N3O5S2
473.57
Bright yellow
195
55.80 (55.68)
4.90 (4.91)
8.87 (8.82)
16.89 (16.75)
13.54 (13.59)
—
4.97
Ni(Haαft)2
C44H44N6NiO10S4
1003.81
Brown
230
52.65 (52.67)
4.42 (4.421)
8.37 (8.29)
15.94 (15.87)
12.78 (12.75)
5.85 (5.94)
2.98
Cu(Haαft)2
C44H44CuN6O10S4
1008.66
Black
220
52.39 (52.50)
4.45 (4.55)
8.33 (8.21)
15.86 (15.81)
12.72 (12.80)
6.30 (6.15)
2.5The change in color of the ligand and its metal complexes from the parent compounds used for their preparation is the good indication of formation via chemical reaction [20]. Complexation with metal ions exhibited drop down of pH values due to deprotonation of ligands. In our work, decrease in pH values from ligand to metal complexes also confirms complexation [21].


### 3.2. Spectral Analysis

#### 3.2.1. FT-IR Analysis

The most significant IR spectral bands are presented in Table2. The IR spectral data comparison of the reported complexes with those of the uncomplexed ligand provides valuable information about the coordination sites of the ligand. Shift in the positions of strong intensity band at 1661.56 cm−1 characteristic for azomethine (HC=N) stretch for ligand to lower wave numbers 1652.09 and 1651.25 cm−1 for CuII and NiII complexes, respectively, support the coordination of the azomethine nitrogen to the metal centre [22]. This fact is further substantiated by the appearance of new bands below 500 cm−1 assignable for metal-nitrogen coordination. The medium intensity band at 448.82 cm−1 is assignable for Cu-N stretch and similar band for NiII complex appears at 470.18 cm−1. There was no shift in band positions observed for the stretch of carboxylate group (-COO-), which appeared at 1515.18, 1514.20, and 1514.98 cm−1 characteristic for ligand, CuII, and NiII complexes, respectively [23]. This indicates no involvement of carboxylate group for the coordination with metal ions. The negative band shift from 3485.12 cm−1 assignable for N-H stretch in ligand provides good conformity for the coordination of metal ions with deprotonated nitrogen (NH) group of substituted amide [24]. M-N coordination mode is further ensured by the appearance of bands at 3423.36 and 3432.69 cm−1 for CuII and NiII complexes, respectively. A weak sharp band observed at 1599.85 cm−1 assignable for ν(C=O) lactam is restored in the metal complexes [25]. Lactam (C=O) stretch band in CuII and NiII complexes appeared at 1602.88 and 1601.89 cm−1, respectively [26]. The bands in the range of 2961–2965 cm−1 in all the synthesized compounds could be assigned for the C-H stretch of methyl group [27].Table 2
Characteristic IR band positions (cm−1) of ligand and metal complexes.
Compound
ν(NH)
ν(C=N)
ν(C=O) lactam
ν(CH3)
ν(COO)
ν(M-N)
HL
3485.12 (br)
1661.56 (s)
1599.85
2965.69 (s)
1515.18
—
Ni(Haαft)2
3432.69 (br)
1651.25 (s)
1601.89
2963.51 (s)
1514.98
470.18
Cu(Haαft)2
3423.36 (br)
1652.09 (s)
1602.88
2961.96 (s)
1514.20
448.82


#### 3.2.2.1H NMR Analysis

1H NMR spectral comparison of novel ligand and its metal complexes was made to confirm the binding mode of ligand with metal ions. The 1H NMR spectra of the ligand are shown in Figure 2 and the spectral data are summarized in Table 3. The 1H NMR spectral peak at 2.5 ppm in the spectra of ligand is assignable to DMSO solvent protons. The peaks in the region of 0.9–1.4 ppm are suggesting the peak for methyl protons present in the amoxicillin moiety, near the lactam ring [28]. Although NiII complex is diamagnetic, having square planar geometry, it offers nominal changes in the chemical shift values of different types of protons compared to the ligand. The azomethine proton appears as a singlet at 9.95 ppm for the ligand and at 10.038 ppm for NiII complex [29]. All four aromatic protons as a set of two doublets appear in the range of 6.6–7.3 ppm. In addition to this, methyl protons of ester group produced by esterification of carboxylic acid group of amoxicillin with methanol show singlet in the region of 3.3–4.7 ppm [30]. Thiophene ring has three protons which appear as a multiplet in the region of 7.1–8.7 ppm in the spectrum of the ligand. The ligand showed a singlet peak at 8.5 ppm assignable to NH proton [31]. It is important to mention here that no clear appreciable changes in 1H NMR spectrum had been reported for CuII complex due to paramagnetic effects [32]. All these results indicated the participation of NH proton in the coordination process with metal ions.Table 3
The1H NMR spectral data (δ, ppm) of ligand.
Compound
Chemical shiftδ ppm
Assignment
HL
6.7–7.0
2d, 4H, aromatic protons
9.95
s, 1H, azomethine protons
7.1–8.0
m, 3H, thiophene ring protons
0.9–1.4
s, 6H, methyl protons
3.4–4.1
s, 3H, CH3 of ester group
8.5
s, 1H, NH protonFigure 2
1H NMR spectrum of HL.


#### 3.2.3.13C NMR Analysis

The13C NMR spectral data for novel ligand has been recorded in DMSO. The measured chemical shifts of all the carbon atoms, as numbered in the structure of novel ligand, are listed in Table 4. As given in Figure 3, the azomethine carbon signal for the ligand appears at 157.594 ppm [33]. The signal for the carbon of carbonyl group (C-3) appears at 172.668 ppm in the spectrum of ligand [34]. Aromatic carbons showed signals in the range of 115–145 ppm. The carbon signal at 170.8 ppm is attributed to lactam carbonyl carbon. Due to resonance effect in diamagnetic and paramagnetic nature of the mentioned metal complexes, there was no marked change in their 13C NMR spectra, compared to the ligand.Table 4
The13C NMR spectral data (δ, ppm) of the free ligand and metal complexes.
Ligand (HL)
Assignment
Chemical shiftδ ppm
C-1
157.594
C-3
172.668
C-5
170.8
C-7
26.909
C-8
26.909
C-9
73.378
C-10
178.399
C-11
39.928
Ar-C
115.652, 121.217, 128.318, 129.44, 136.56, 138.423, 145.635
DMSO
39.65Figure 3
13C NMR spectrum of HL.


#### 3.2.4. ESI-MS Analysis

The ESI mass spectrum of ligand (HL) offered a peak atm/z 473 amu corresponding to its molecular ion peak [M∙+] and it confirms the proposed molecular formula of the ligand. Other peaks in the mass spectrum of HL atm/z 459, 445, 353, 187, and 168 amu are the fragment peaks. Their intensities provide the idea of stability of the fragments. ESI mass spectrum of the complexes indicated the molecular ion peaks atm/z 1003 and 1008 amu characteristic for NiII and CuII complexes, respectively. The mass spectrum of ligand is presented in Figure 4.Figure 4
Mass spectrum of ligand (HL).


#### 3.2.5. X-Ray Powder Diffraction Study

The X-ray powder diffraction technique was carried to get useful crystal data information to deduce accurate cell parameters, crystal system, and the cell volume. Powder diffraction patterns of the ligand and metal complexes were recorded and crystallographic data are listed in Table5. X-ray diffraction powder pattern of CuII complex is shown in Figure 5. The crystallite size of the ligand and its metal complexes was calculated from Scherrer’s formula, dXRD=0.9λ/βcos⁡θ, where λ is the wavelength, β is the full-width half maximum of the characteristic peak, and θ is the diffraction angle for the hkl plane [35, 36]. The diffractogram of ligand gave 13 reflection peaks with 100% intensity at 2θ = 26.7349°. Associated with this, the interplanar distance was d = 3.3348 Å. The 26 reflections have been recorded for CuII complex with maxima at 2θ = 26.0048° and interplanar distance d = 3.4265 Å. Unit cell dimensions of ligand a (15.009 Å), b (20.077 Å), c (20.060 Å), α (55.910°), β (65.330°), and γ (59.920°) confirm its triclinic crystal system. a (6.753 Å), b (13.904 Å), c (20.122 Å), α (142.76°), β (106.580°), and γ (72.4343°) data for the CuII complex also confirms triclinic crystal system. NiII complex has unit cell dimensions a (24.2547 Å), b (6.6371 Å), and c (5.5047 Å) (α = β = γ = 90°) and this confirms orthorhombic crystal system (Table 5). Particle size calculation data, 55.325, 85.451, and 75.231 nm for the ligand, CuII, and NiII complexes, respectively, revealed their nanocrystalline nature.Table 5
Crystal data and structure refinement.
Compounds
HL
Ni(Haαft)2
Cu(Haαft)2
Formula
C22H23N3O5S2
C44H44N6NiO10S4
C44H44CuN6O10S4
FW
473.57
1003.81
1008.66
Temp (K)
298
298
298
Wavelength
1.54056
1.54056
1.54056
Crystal system
Triclinic
Tetragonal
Triclinic
Space group
P1
P/4 mm
P1
Unit cell dimension
a (Å)
15.009
24.2547
6.753
b (Å)
20.077
6.6371
13.904
c (Å)
20.060
5.5047
20.122
α
°
55.910
90
142.76
β
°
65.330
90
106.580
γ
°
59.920
90
72.4343
Volume (A3)
4295.95
859.4463
1047.72
θ range (°)
5–75
5–75
5–75
Limiting indices
−1≤h≤6 0≤k≤2 1≤l≤0
-
2
≤
h
≤
3 0≤k≤3 1≤l≤-2
1
≤
h
≤
0 0≤k≤2 -2≤l≤0
Particle size (nm)
55.325
75.231
85.451Figure 5
Powder XRD pattern of Cu(Haαft)2.


#### 3.2.6. Molar Conductance and Magnetic Properties of the Complexes

Molar conductance values of the soluble complexes in DMSO (1 × 10−3 M) at room temperature vary from 5.1 to 20.1 Ω−1 cm2 mol−1 revealing their nonelectrolytic nature. The observed range is below 50 Ω−1 cm2 mol−1 characteristic for nonelectrolytes [37]. The room temperature magnetic moments for tetra coordinated NiII and CuII complexes indicate their respective diamagnetic and paramagnetic nature. NiII complex has observed magnetic moment value 0 BM, which is consistent with its square planar geometry, using dsp2 hybridization in the coordination process. CuII complex in a distorted tetrahedral geometry has observed magnetic moment value μeff = 1.84 BM, which is greater than the theoretical spin only magnetic moment value, μSO = 1.73 BM. This is considered possibly due to orbital contribution that sum up in the spin interaction magnetic momentum [38]. The Jahn-Teller distortion effect in the CuII complex forced it to acquire distorted tetrahedral geometry.


#### 3.2.7. Electronic Absorption Spectra

The electronic spectra of the Schiff base ligand and its metal complexes were recorded in DMSO solution and are presented in Table6. The absorption peaks at the region of 361 and 391 nm of high intensity for ligand are attributable to intraligand n→π∗ transitions of azomethine and lactam carbonyl group [39, 40]. Similar peaks at 268 and 310 nm for the ligand are assignable to intraligand π→π∗ transitions. These peaks are still present in NiII and CuII complexes, but slightly shifted from the ligand peaks. The complexes of NiII and CuII show the low intensity bands in the visible region at 465 and 450 nm, respectively, which are assignable to the A11g→B11g and B21g→E2g transitions for ligand metal charge transfer band [41]. The electronic spectrum of the NiII complex exhibits a single band at 520 nm which may be assignable to the A11g→B12g, d-d transition typical for the square planar geometry [42]. As this d-d transition is a high energy process, it may probably confirm its square planar geometry. The lack of any electronic transitions at higher wavelengths indicates large crystal field splitting and is consistent with the said geometry for the NiII complex [43]. Absence of d-d transition band in the spectra of CuII complex probably indicates distorted tetrahedral geometry, which is also supported by other spectral studies.Table 6
The relative peak positions (λmax) of the free ligand and metal complexes.
Compound
Peak positions (λmax) in nm
π
→
π
∗ transitions
n
→
π
∗ transitions
LMCT band
d-d transition
HL
310–268
391, 361
—
—
Ni(Haαft)2
307, 272
391,  370
465
520
Cu(Haαft)2
285
370
450
—


### 3.3. Antibacterial Sensitivity Study

The pure metals are considered biologically inactive. However, the activity of metal cations depends on their bioavailability and the presence of bioligands [44]. It was, therefore, of great interest to investigate antibacterial activity of Schiff base and its transition metal complexes against some bacterial pathogens. Here, four clinical bacterial pathogens, namely,Escherichia coli,Proteus vulgaris,Pseudomonas aeruginosa (Gram-negative), andStaphylococcus aureus (Gram-positive), have been focused on for the microbiological interaction with the synthesized compounds.In the present work, the antibacterial activity results presented in Table7 show that the ligand (HL) and its two metal complexes exhibit potential biological activity. Two different concentrations of the compounds have been selected for the biological interactions with bacterial pathogens. They show increased bactericidal effect at higher concentrations. The graphical charts of the comparable antibacterial sensitivity study of the synthesized compounds are presented in Figures 6 and 7. The results demonstrate better antibacterial activity of metal complexes compared to the free ligand. The azomethine group present in the ligand may be the cause for its remarkable activity. The enhancement in the activity of metal complexes is considered due to coordination of metal ions with the donor sites of ligand that might inhibit the enzyme production, which is suitable for the bacterial growth. The chelation makes the compound lipophilic due to partial sharing of positive charge and π-electrons delocalization within the whole chelate ring [45–47]. This increased lipophilicity enhances the ability of complexes for permeation through the lipid layer of the cell membrane and blocks the metal binding sites in enzymes of the microorganisms. These complexes also disturb the respiration process of the cell and this freezes the synthesis of proteins, which restricts further growth of the organisms [48]. The data also reveals that the activity of free ligand and metal complexes is lesser than standard drug amikacin. Overall comparison of observed data gave information that metal complexes are more active than the free ligand against all bacteria. However, they show better inhibitory effect withS. aureus compared to other bacterial pathogens. The variation in the effectiveness of different compounds against different bacterial pathogens depends on the impermeability through the cell membrane of microorganisms.Table 7
Antibacterial sensitivity of synthesized compounds.
Compounds
Conc.
Diameter of zone of inhibition in (mm)
(μg/μL)
E. coli
P. vulgaris
P. aeruginosa
S. aureus
L
10.5
98
108
109
1210
Ni(Haαft)2
10.5
129
1210
1411
1512
Cu(Haαft)2
10.5
119
1412
1311
1411
DMSO
0
0
0
0
Standard
19
18
18
20Figure 6
Antibacterial sensitivity at the concentration of 1μg/μL.Figure 7
Antibacterial sensitivity at the concentration of 0.5μg/μL.


### 3.4. Molecular Modeling Analysis

To provide clear and deep perception of the geometry of the ligand and metal complexes, molecular modeling has been carried out by using molecular mechanics and Hartree-Fock (HF) quantum mechanics calculations. The geometry optimization was done by Universal Force Field (UFF) with minimum RMS gradient 0.100, supported in ArgusLab programme [49]. Single point energy calculation of the ligand through Hartree-Fock SCF computation with maximum iteration 200 and convergence rate 10−10 kcal/mol reveals the final SCF energy −121796.5370 kcal/mol and heat of formation −78.0985 kcal/mol. After the geometry optimization by UFF (molecular mechanics) technique, the final geometrical energy of the ligand has been computed to 161.2699 kcal/mol and this provides stability of the molecule [50, 51]. The surface structure of the ligand has been computed through HOMO and LUMO plot. Similar study with the NiII and CuII complexes has assured their final geometrical energy 449.0564 and 752.1825 kcal/mol, respectively. The optimized structures of the metal complexes are presented in Figures 8 and 9 and they reveal square planar geometry for NiII and tetrahedral geometry for CuII complexes. The computational findings are in good support of the proposed structures of the complexes. The selected bond lengths, bond angles, and bond energies of the ligand and metal complexes are given in Tables 8(a)–8(f).Table 8
(a) Selected bond lengths and bond energies of ligand (HL). (b) Selected bond angles and bond energies of ligand (HL). (c) Selected bond lengths and bond energies of NiII-complex. (d) Selected bond angles and bond energies of NiII-complex. (e) Selected bond lengths and bond energies of CuII-complex. (f) Selected bond angles and bond energies of CuII-complex.
(a)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
C8-N15
1.447
532.154
N15-C16
1.291
749.036
C16-C17
1.464
386.878
C8-C22
1.489
367.716
C22-N23
1.437
543.390
N23-C24
1.462
515.889
(b)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
C8-N15-C16
120.00
226.230
N15-C8-C22
109.47
312.267
N15-C16-C17
120.00
295.502
N15-C8-H14
109.47
169.990
C22-N23-C24
106.70
261.205
N23-C22-O25
120.00
378.598
(c)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
Ni1-N2
1.885
306.275
Ni1-N3
1.885
306.275
Ni1-N4
1.870
313.824
Ni1-N5
1.870
313.824
(d)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
N2-Ni1-N3
90.00
340.090
N2-Ni1-N4
90.00
344.228
N2-Ni1-N5
90.00
344.228
Ni1-N2-C9
106.00
212.735
Ni1-N2-C24
106.00
208.934
N3-Ni1-N4
90.00
344.228
N3-Ni1-N5
90.00
344.228
N4-Ni1-N5
90.00
348.473
(e)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
Cu1-N2
2.031
176.938
Cu1-N3
2.031
176.938
Cu1-N4
2.016
181.007
Cu1-N5
2.016
181.007
(f)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
N2-Cu1-N3
109.47
156.977
N2-Cu1-N4
109.47
158.764
N2-Cu1-N5
109.47
158.764
Cu1-N2-C9
106.70
132.072
Cu1-N2-C24
106.70
129.991
N3-Cu1-N4
109.47
158.764
N3-Cu1-N5
109.47
158.764
N4-Cu1-N5
109.47
160.587Figure 8
Molecular modeling structure of Ni(Haαft)2.Figure 9
Molecular modeling structure of Cu(Haαft)2.


## 3.1. Physical Data and Microelemental Analysis

The Schiff base ligand and its metal complexes were subjected to elemental analysis. The results of elemental analysis with molecular formula and other physical data like melting points and color change of the compounds are presented in Table1. The results are in good agreement with suggested molecular formula. Sharp melting point of compounds indicates the purity of the prepared compounds [19].Table 1
Elemental analysis and physical properties measurement data.
Compound
Mol. formula
Mol. wt.
Colour
m. pt. (°C)
Calculated (found) (%)
pH
C
H
N
O
S
M
HL
C22H23N3O5S2
473.57
Bright yellow
195
55.80 (55.68)
4.90 (4.91)
8.87 (8.82)
16.89 (16.75)
13.54 (13.59)
—
4.97
Ni(Haαft)2
C44H44N6NiO10S4
1003.81
Brown
230
52.65 (52.67)
4.42 (4.421)
8.37 (8.29)
15.94 (15.87)
12.78 (12.75)
5.85 (5.94)
2.98
Cu(Haαft)2
C44H44CuN6O10S4
1008.66
Black
220
52.39 (52.50)
4.45 (4.55)
8.33 (8.21)
15.86 (15.81)
12.72 (12.80)
6.30 (6.15)
2.5The change in color of the ligand and its metal complexes from the parent compounds used for their preparation is the good indication of formation via chemical reaction [20]. Complexation with metal ions exhibited drop down of pH values due to deprotonation of ligands. In our work, decrease in pH values from ligand to metal complexes also confirms complexation [21].


## 3.2. Spectral Analysis

### 3.2.1. FT-IR Analysis

The most significant IR spectral bands are presented in Table2. The IR spectral data comparison of the reported complexes with those of the uncomplexed ligand provides valuable information about the coordination sites of the ligand. Shift in the positions of strong intensity band at 1661.56 cm−1 characteristic for azomethine (HC=N) stretch for ligand to lower wave numbers 1652.09 and 1651.25 cm−1 for CuII and NiII complexes, respectively, support the coordination of the azomethine nitrogen to the metal centre [22]. This fact is further substantiated by the appearance of new bands below 500 cm−1 assignable for metal-nitrogen coordination. The medium intensity band at 448.82 cm−1 is assignable for Cu-N stretch and similar band for NiII complex appears at 470.18 cm−1. There was no shift in band positions observed for the stretch of carboxylate group (-COO-), which appeared at 1515.18, 1514.20, and 1514.98 cm−1 characteristic for ligand, CuII, and NiII complexes, respectively [23]. This indicates no involvement of carboxylate group for the coordination with metal ions. The negative band shift from 3485.12 cm−1 assignable for N-H stretch in ligand provides good conformity for the coordination of metal ions with deprotonated nitrogen (NH) group of substituted amide [24]. M-N coordination mode is further ensured by the appearance of bands at 3423.36 and 3432.69 cm−1 for CuII and NiII complexes, respectively. A weak sharp band observed at 1599.85 cm−1 assignable for ν(C=O) lactam is restored in the metal complexes [25]. Lactam (C=O) stretch band in CuII and NiII complexes appeared at 1602.88 and 1601.89 cm−1, respectively [26]. The bands in the range of 2961–2965 cm−1 in all the synthesized compounds could be assigned for the C-H stretch of methyl group [27].Table 2
Characteristic IR band positions (cm−1) of ligand and metal complexes.
Compound
ν(NH)
ν(C=N)
ν(C=O) lactam
ν(CH3)
ν(COO)
ν(M-N)
HL
3485.12 (br)
1661.56 (s)
1599.85
2965.69 (s)
1515.18
—
Ni(Haαft)2
3432.69 (br)
1651.25 (s)
1601.89
2963.51 (s)
1514.98
470.18
Cu(Haαft)2
3423.36 (br)
1652.09 (s)
1602.88
2961.96 (s)
1514.20
448.82


### 3.2.2.1H NMR Analysis

1H NMR spectral comparison of novel ligand and its metal complexes was made to confirm the binding mode of ligand with metal ions. The 1H NMR spectra of the ligand are shown in Figure 2 and the spectral data are summarized in Table 3. The 1H NMR spectral peak at 2.5 ppm in the spectra of ligand is assignable to DMSO solvent protons. The peaks in the region of 0.9–1.4 ppm are suggesting the peak for methyl protons present in the amoxicillin moiety, near the lactam ring [28]. Although NiII complex is diamagnetic, having square planar geometry, it offers nominal changes in the chemical shift values of different types of protons compared to the ligand. The azomethine proton appears as a singlet at 9.95 ppm for the ligand and at 10.038 ppm for NiII complex [29]. All four aromatic protons as a set of two doublets appear in the range of 6.6–7.3 ppm. In addition to this, methyl protons of ester group produced by esterification of carboxylic acid group of amoxicillin with methanol show singlet in the region of 3.3–4.7 ppm [30]. Thiophene ring has three protons which appear as a multiplet in the region of 7.1–8.7 ppm in the spectrum of the ligand. The ligand showed a singlet peak at 8.5 ppm assignable to NH proton [31]. It is important to mention here that no clear appreciable changes in 1H NMR spectrum had been reported for CuII complex due to paramagnetic effects [32]. All these results indicated the participation of NH proton in the coordination process with metal ions.Table 3
The1H NMR spectral data (δ, ppm) of ligand.
Compound
Chemical shiftδ ppm
Assignment
HL
6.7–7.0
2d, 4H, aromatic protons
9.95
s, 1H, azomethine protons
7.1–8.0
m, 3H, thiophene ring protons
0.9–1.4
s, 6H, methyl protons
3.4–4.1
s, 3H, CH3 of ester group
8.5
s, 1H, NH protonFigure 2
1H NMR spectrum of HL.


### 3.2.3.13C NMR Analysis

The13C NMR spectral data for novel ligand has been recorded in DMSO. The measured chemical shifts of all the carbon atoms, as numbered in the structure of novel ligand, are listed in Table 4. As given in Figure 3, the azomethine carbon signal for the ligand appears at 157.594 ppm [33]. The signal for the carbon of carbonyl group (C-3) appears at 172.668 ppm in the spectrum of ligand [34]. Aromatic carbons showed signals in the range of 115–145 ppm. The carbon signal at 170.8 ppm is attributed to lactam carbonyl carbon. Due to resonance effect in diamagnetic and paramagnetic nature of the mentioned metal complexes, there was no marked change in their 13C NMR spectra, compared to the ligand.Table 4
The13C NMR spectral data (δ, ppm) of the free ligand and metal complexes.
Ligand (HL)
Assignment
Chemical shiftδ ppm
C-1
157.594
C-3
172.668
C-5
170.8
C-7
26.909
C-8
26.909
C-9
73.378
C-10
178.399
C-11
39.928
Ar-C
115.652, 121.217, 128.318, 129.44, 136.56, 138.423, 145.635
DMSO
39.65Figure 3
13C NMR spectrum of HL.


### 3.2.4. ESI-MS Analysis

The ESI mass spectrum of ligand (HL) offered a peak atm/z 473 amu corresponding to its molecular ion peak [M∙+] and it confirms the proposed molecular formula of the ligand. Other peaks in the mass spectrum of HL atm/z 459, 445, 353, 187, and 168 amu are the fragment peaks. Their intensities provide the idea of stability of the fragments. ESI mass spectrum of the complexes indicated the molecular ion peaks atm/z 1003 and 1008 amu characteristic for NiII and CuII complexes, respectively. The mass spectrum of ligand is presented in Figure 4.Figure 4
Mass spectrum of ligand (HL).


### 3.2.5. X-Ray Powder Diffraction Study

The X-ray powder diffraction technique was carried to get useful crystal data information to deduce accurate cell parameters, crystal system, and the cell volume. Powder diffraction patterns of the ligand and metal complexes were recorded and crystallographic data are listed in Table5. X-ray diffraction powder pattern of CuII complex is shown in Figure 5. The crystallite size of the ligand and its metal complexes was calculated from Scherrer’s formula, dXRD=0.9λ/βcos⁡θ, where λ is the wavelength, β is the full-width half maximum of the characteristic peak, and θ is the diffraction angle for the hkl plane [35, 36]. The diffractogram of ligand gave 13 reflection peaks with 100% intensity at 2θ = 26.7349°. Associated with this, the interplanar distance was d = 3.3348 Å. The 26 reflections have been recorded for CuII complex with maxima at 2θ = 26.0048° and interplanar distance d = 3.4265 Å. Unit cell dimensions of ligand a (15.009 Å), b (20.077 Å), c (20.060 Å), α (55.910°), β (65.330°), and γ (59.920°) confirm its triclinic crystal system. a (6.753 Å), b (13.904 Å), c (20.122 Å), α (142.76°), β (106.580°), and γ (72.4343°) data for the CuII complex also confirms triclinic crystal system. NiII complex has unit cell dimensions a (24.2547 Å), b (6.6371 Å), and c (5.5047 Å) (α = β = γ = 90°) and this confirms orthorhombic crystal system (Table 5). Particle size calculation data, 55.325, 85.451, and 75.231 nm for the ligand, CuII, and NiII complexes, respectively, revealed their nanocrystalline nature.Table 5
Crystal data and structure refinement.
Compounds
HL
Ni(Haαft)2
Cu(Haαft)2
Formula
C22H23N3O5S2
C44H44N6NiO10S4
C44H44CuN6O10S4
FW
473.57
1003.81
1008.66
Temp (K)
298
298
298
Wavelength
1.54056
1.54056
1.54056
Crystal system
Triclinic
Tetragonal
Triclinic
Space group
P1
P/4 mm
P1
Unit cell dimension
a (Å)
15.009
24.2547
6.753
b (Å)
20.077
6.6371
13.904
c (Å)
20.060
5.5047
20.122
α
°
55.910
90
142.76
β
°
65.330
90
106.580
γ
°
59.920
90
72.4343
Volume (A3)
4295.95
859.4463
1047.72
θ range (°)
5–75
5–75
5–75
Limiting indices
−1≤h≤6 0≤k≤2 1≤l≤0
-
2
≤
h
≤
3 0≤k≤3 1≤l≤-2
1
≤
h
≤
0 0≤k≤2 -2≤l≤0
Particle size (nm)
55.325
75.231
85.451Figure 5
Powder XRD pattern of Cu(Haαft)2.


### 3.2.6. Molar Conductance and Magnetic Properties of the Complexes

Molar conductance values of the soluble complexes in DMSO (1 × 10−3 M) at room temperature vary from 5.1 to 20.1 Ω−1 cm2 mol−1 revealing their nonelectrolytic nature. The observed range is below 50 Ω−1 cm2 mol−1 characteristic for nonelectrolytes [37]. The room temperature magnetic moments for tetra coordinated NiII and CuII complexes indicate their respective diamagnetic and paramagnetic nature. NiII complex has observed magnetic moment value 0 BM, which is consistent with its square planar geometry, using dsp2 hybridization in the coordination process. CuII complex in a distorted tetrahedral geometry has observed magnetic moment value μeff = 1.84 BM, which is greater than the theoretical spin only magnetic moment value, μSO = 1.73 BM. This is considered possibly due to orbital contribution that sum up in the spin interaction magnetic momentum [38]. The Jahn-Teller distortion effect in the CuII complex forced it to acquire distorted tetrahedral geometry.


### 3.2.7. Electronic Absorption Spectra

The electronic spectra of the Schiff base ligand and its metal complexes were recorded in DMSO solution and are presented in Table6. The absorption peaks at the region of 361 and 391 nm of high intensity for ligand are attributable to intraligand n→π∗ transitions of azomethine and lactam carbonyl group [39, 40]. Similar peaks at 268 and 310 nm for the ligand are assignable to intraligand π→π∗ transitions. These peaks are still present in NiII and CuII complexes, but slightly shifted from the ligand peaks. The complexes of NiII and CuII show the low intensity bands in the visible region at 465 and 450 nm, respectively, which are assignable to the A11g→B11g and B21g→E2g transitions for ligand metal charge transfer band [41]. The electronic spectrum of the NiII complex exhibits a single band at 520 nm which may be assignable to the A11g→B12g, d-d transition typical for the square planar geometry [42]. As this d-d transition is a high energy process, it may probably confirm its square planar geometry. The lack of any electronic transitions at higher wavelengths indicates large crystal field splitting and is consistent with the said geometry for the NiII complex [43]. Absence of d-d transition band in the spectra of CuII complex probably indicates distorted tetrahedral geometry, which is also supported by other spectral studies.Table 6
The relative peak positions (λmax) of the free ligand and metal complexes.
Compound
Peak positions (λmax) in nm
π
→
π
∗ transitions
n
→
π
∗ transitions
LMCT band
d-d transition
HL
310–268
391, 361
—
—
Ni(Haαft)2
307, 272
391,  370
465
520
Cu(Haαft)2
285
370
450
—


## 3.2.1. FT-IR Analysis

The most significant IR spectral bands are presented in Table2. The IR spectral data comparison of the reported complexes with those of the uncomplexed ligand provides valuable information about the coordination sites of the ligand. Shift in the positions of strong intensity band at 1661.56 cm−1 characteristic for azomethine (HC=N) stretch for ligand to lower wave numbers 1652.09 and 1651.25 cm−1 for CuII and NiII complexes, respectively, support the coordination of the azomethine nitrogen to the metal centre [22]. This fact is further substantiated by the appearance of new bands below 500 cm−1 assignable for metal-nitrogen coordination. The medium intensity band at 448.82 cm−1 is assignable for Cu-N stretch and similar band for NiII complex appears at 470.18 cm−1. There was no shift in band positions observed for the stretch of carboxylate group (-COO-), which appeared at 1515.18, 1514.20, and 1514.98 cm−1 characteristic for ligand, CuII, and NiII complexes, respectively [23]. This indicates no involvement of carboxylate group for the coordination with metal ions. The negative band shift from 3485.12 cm−1 assignable for N-H stretch in ligand provides good conformity for the coordination of metal ions with deprotonated nitrogen (NH) group of substituted amide [24]. M-N coordination mode is further ensured by the appearance of bands at 3423.36 and 3432.69 cm−1 for CuII and NiII complexes, respectively. A weak sharp band observed at 1599.85 cm−1 assignable for ν(C=O) lactam is restored in the metal complexes [25]. Lactam (C=O) stretch band in CuII and NiII complexes appeared at 1602.88 and 1601.89 cm−1, respectively [26]. The bands in the range of 2961–2965 cm−1 in all the synthesized compounds could be assigned for the C-H stretch of methyl group [27].Table 2
Characteristic IR band positions (cm−1) of ligand and metal complexes.
Compound
ν(NH)
ν(C=N)
ν(C=O) lactam
ν(CH3)
ν(COO)
ν(M-N)
HL
3485.12 (br)
1661.56 (s)
1599.85
2965.69 (s)
1515.18
—
Ni(Haαft)2
3432.69 (br)
1651.25 (s)
1601.89
2963.51 (s)
1514.98
470.18
Cu(Haαft)2
3423.36 (br)
1652.09 (s)
1602.88
2961.96 (s)
1514.20
448.82


## 3.2.2.1H NMR Analysis

1H NMR spectral comparison of novel ligand and its metal complexes was made to confirm the binding mode of ligand with metal ions. The 1H NMR spectra of the ligand are shown in Figure 2 and the spectral data are summarized in Table 3. The 1H NMR spectral peak at 2.5 ppm in the spectra of ligand is assignable to DMSO solvent protons. The peaks in the region of 0.9–1.4 ppm are suggesting the peak for methyl protons present in the amoxicillin moiety, near the lactam ring [28]. Although NiII complex is diamagnetic, having square planar geometry, it offers nominal changes in the chemical shift values of different types of protons compared to the ligand. The azomethine proton appears as a singlet at 9.95 ppm for the ligand and at 10.038 ppm for NiII complex [29]. All four aromatic protons as a set of two doublets appear in the range of 6.6–7.3 ppm. In addition to this, methyl protons of ester group produced by esterification of carboxylic acid group of amoxicillin with methanol show singlet in the region of 3.3–4.7 ppm [30]. Thiophene ring has three protons which appear as a multiplet in the region of 7.1–8.7 ppm in the spectrum of the ligand. The ligand showed a singlet peak at 8.5 ppm assignable to NH proton [31]. It is important to mention here that no clear appreciable changes in 1H NMR spectrum had been reported for CuII complex due to paramagnetic effects [32]. All these results indicated the participation of NH proton in the coordination process with metal ions.Table 3
The1H NMR spectral data (δ, ppm) of ligand.
Compound
Chemical shiftδ ppm
Assignment
HL
6.7–7.0
2d, 4H, aromatic protons
9.95
s, 1H, azomethine protons
7.1–8.0
m, 3H, thiophene ring protons
0.9–1.4
s, 6H, methyl protons
3.4–4.1
s, 3H, CH3 of ester group
8.5
s, 1H, NH protonFigure 2
1H NMR spectrum of HL.


## 3.2.3.13C NMR Analysis

The13C NMR spectral data for novel ligand has been recorded in DMSO. The measured chemical shifts of all the carbon atoms, as numbered in the structure of novel ligand, are listed in Table 4. As given in Figure 3, the azomethine carbon signal for the ligand appears at 157.594 ppm [33]. The signal for the carbon of carbonyl group (C-3) appears at 172.668 ppm in the spectrum of ligand [34]. Aromatic carbons showed signals in the range of 115–145 ppm. The carbon signal at 170.8 ppm is attributed to lactam carbonyl carbon. Due to resonance effect in diamagnetic and paramagnetic nature of the mentioned metal complexes, there was no marked change in their 13C NMR spectra, compared to the ligand.Table 4
The13C NMR spectral data (δ, ppm) of the free ligand and metal complexes.
Ligand (HL)
Assignment
Chemical shiftδ ppm
C-1
157.594
C-3
172.668
C-5
170.8
C-7
26.909
C-8
26.909
C-9
73.378
C-10
178.399
C-11
39.928
Ar-C
115.652, 121.217, 128.318, 129.44, 136.56, 138.423, 145.635
DMSO
39.65Figure 3
13C NMR spectrum of HL.


## 3.2.4. ESI-MS Analysis

The ESI mass spectrum of ligand (HL) offered a peak atm/z 473 amu corresponding to its molecular ion peak [M∙+] and it confirms the proposed molecular formula of the ligand. Other peaks in the mass spectrum of HL atm/z 459, 445, 353, 187, and 168 amu are the fragment peaks. Their intensities provide the idea of stability of the fragments. ESI mass spectrum of the complexes indicated the molecular ion peaks atm/z 1003 and 1008 amu characteristic for NiII and CuII complexes, respectively. The mass spectrum of ligand is presented in Figure 4.Figure 4
Mass spectrum of ligand (HL).


## 3.2.5. X-Ray Powder Diffraction Study

The X-ray powder diffraction technique was carried to get useful crystal data information to deduce accurate cell parameters, crystal system, and the cell volume. Powder diffraction patterns of the ligand and metal complexes were recorded and crystallographic data are listed in Table5. X-ray diffraction powder pattern of CuII complex is shown in Figure 5. The crystallite size of the ligand and its metal complexes was calculated from Scherrer’s formula, dXRD=0.9λ/βcos⁡θ, where λ is the wavelength, β is the full-width half maximum of the characteristic peak, and θ is the diffraction angle for the hkl plane [35, 36]. The diffractogram of ligand gave 13 reflection peaks with 100% intensity at 2θ = 26.7349°. Associated with this, the interplanar distance was d = 3.3348 Å. The 26 reflections have been recorded for CuII complex with maxima at 2θ = 26.0048° and interplanar distance d = 3.4265 Å. Unit cell dimensions of ligand a (15.009 Å), b (20.077 Å), c (20.060 Å), α (55.910°), β (65.330°), and γ (59.920°) confirm its triclinic crystal system. a (6.753 Å), b (13.904 Å), c (20.122 Å), α (142.76°), β (106.580°), and γ (72.4343°) data for the CuII complex also confirms triclinic crystal system. NiII complex has unit cell dimensions a (24.2547 Å), b (6.6371 Å), and c (5.5047 Å) (α = β = γ = 90°) and this confirms orthorhombic crystal system (Table 5). Particle size calculation data, 55.325, 85.451, and 75.231 nm for the ligand, CuII, and NiII complexes, respectively, revealed their nanocrystalline nature.Table 5
Crystal data and structure refinement.
Compounds
HL
Ni(Haαft)2
Cu(Haαft)2
Formula
C22H23N3O5S2
C44H44N6NiO10S4
C44H44CuN6O10S4
FW
473.57
1003.81
1008.66
Temp (K)
298
298
298
Wavelength
1.54056
1.54056
1.54056
Crystal system
Triclinic
Tetragonal
Triclinic
Space group
P1
P/4 mm
P1
Unit cell dimension
a (Å)
15.009
24.2547
6.753
b (Å)
20.077
6.6371
13.904
c (Å)
20.060
5.5047
20.122
α
°
55.910
90
142.76
β
°
65.330
90
106.580
γ
°
59.920
90
72.4343
Volume (A3)
4295.95
859.4463
1047.72
θ range (°)
5–75
5–75
5–75
Limiting indices
−1≤h≤6 0≤k≤2 1≤l≤0
-
2
≤
h
≤
3 0≤k≤3 1≤l≤-2
1
≤
h
≤
0 0≤k≤2 -2≤l≤0
Particle size (nm)
55.325
75.231
85.451Figure 5
Powder XRD pattern of Cu(Haαft)2.


## 3.2.6. Molar Conductance and Magnetic Properties of the Complexes

Molar conductance values of the soluble complexes in DMSO (1 × 10−3 M) at room temperature vary from 5.1 to 20.1 Ω−1 cm2 mol−1 revealing their nonelectrolytic nature. The observed range is below 50 Ω−1 cm2 mol−1 characteristic for nonelectrolytes [37]. The room temperature magnetic moments for tetra coordinated NiII and CuII complexes indicate their respective diamagnetic and paramagnetic nature. NiII complex has observed magnetic moment value 0 BM, which is consistent with its square planar geometry, using dsp2 hybridization in the coordination process. CuII complex in a distorted tetrahedral geometry has observed magnetic moment value μeff = 1.84 BM, which is greater than the theoretical spin only magnetic moment value, μSO = 1.73 BM. This is considered possibly due to orbital contribution that sum up in the spin interaction magnetic momentum [38]. The Jahn-Teller distortion effect in the CuII complex forced it to acquire distorted tetrahedral geometry.


## 3.2.7. Electronic Absorption Spectra

The electronic spectra of the Schiff base ligand and its metal complexes were recorded in DMSO solution and are presented in Table6. The absorption peaks at the region of 361 and 391 nm of high intensity for ligand are attributable to intraligand n→π∗ transitions of azomethine and lactam carbonyl group [39, 40]. Similar peaks at 268 and 310 nm for the ligand are assignable to intraligand π→π∗ transitions. These peaks are still present in NiII and CuII complexes, but slightly shifted from the ligand peaks. The complexes of NiII and CuII show the low intensity bands in the visible region at 465 and 450 nm, respectively, which are assignable to the A11g→B11g and B21g→E2g transitions for ligand metal charge transfer band [41]. The electronic spectrum of the NiII complex exhibits a single band at 520 nm which may be assignable to the A11g→B12g, d-d transition typical for the square planar geometry [42]. As this d-d transition is a high energy process, it may probably confirm its square planar geometry. The lack of any electronic transitions at higher wavelengths indicates large crystal field splitting and is consistent with the said geometry for the NiII complex [43]. Absence of d-d transition band in the spectra of CuII complex probably indicates distorted tetrahedral geometry, which is also supported by other spectral studies.Table 6
The relative peak positions (λmax) of the free ligand and metal complexes.
Compound
Peak positions (λmax) in nm
π
→
π
∗ transitions
n
→
π
∗ transitions
LMCT band
d-d transition
HL
310–268
391, 361
—
—
Ni(Haαft)2
307, 272
391,  370
465
520
Cu(Haαft)2
285
370
450
—


## 3.3. Antibacterial Sensitivity Study

The pure metals are considered biologically inactive. However, the activity of metal cations depends on their bioavailability and the presence of bioligands [44]. It was, therefore, of great interest to investigate antibacterial activity of Schiff base and its transition metal complexes against some bacterial pathogens. Here, four clinical bacterial pathogens, namely,Escherichia coli,Proteus vulgaris,Pseudomonas aeruginosa (Gram-negative), andStaphylococcus aureus (Gram-positive), have been focused on for the microbiological interaction with the synthesized compounds.In the present work, the antibacterial activity results presented in Table7 show that the ligand (HL) and its two metal complexes exhibit potential biological activity. Two different concentrations of the compounds have been selected for the biological interactions with bacterial pathogens. They show increased bactericidal effect at higher concentrations. The graphical charts of the comparable antibacterial sensitivity study of the synthesized compounds are presented in Figures 6 and 7. The results demonstrate better antibacterial activity of metal complexes compared to the free ligand. The azomethine group present in the ligand may be the cause for its remarkable activity. The enhancement in the activity of metal complexes is considered due to coordination of metal ions with the donor sites of ligand that might inhibit the enzyme production, which is suitable for the bacterial growth. The chelation makes the compound lipophilic due to partial sharing of positive charge and π-electrons delocalization within the whole chelate ring [45–47]. This increased lipophilicity enhances the ability of complexes for permeation through the lipid layer of the cell membrane and blocks the metal binding sites in enzymes of the microorganisms. These complexes also disturb the respiration process of the cell and this freezes the synthesis of proteins, which restricts further growth of the organisms [48]. The data also reveals that the activity of free ligand and metal complexes is lesser than standard drug amikacin. Overall comparison of observed data gave information that metal complexes are more active than the free ligand against all bacteria. However, they show better inhibitory effect withS. aureus compared to other bacterial pathogens. The variation in the effectiveness of different compounds against different bacterial pathogens depends on the impermeability through the cell membrane of microorganisms.Table 7
Antibacterial sensitivity of synthesized compounds.
Compounds
Conc.
Diameter of zone of inhibition in (mm)
(μg/μL)
E. coli
P. vulgaris
P. aeruginosa
S. aureus
L
10.5
98
108
109
1210
Ni(Haαft)2
10.5
129
1210
1411
1512
Cu(Haαft)2
10.5
119
1412
1311
1411
DMSO
0
0
0
0
Standard
19
18
18
20Figure 6
Antibacterial sensitivity at the concentration of 1μg/μL.Figure 7
Antibacterial sensitivity at the concentration of 0.5μg/μL.


## 3.4. Molecular Modeling Analysis

To provide clear and deep perception of the geometry of the ligand and metal complexes, molecular modeling has been carried out by using molecular mechanics and Hartree-Fock (HF) quantum mechanics calculations. The geometry optimization was done by Universal Force Field (UFF) with minimum RMS gradient 0.100, supported in ArgusLab programme [49]. Single point energy calculation of the ligand through Hartree-Fock SCF computation with maximum iteration 200 and convergence rate 10−10 kcal/mol reveals the final SCF energy −121796.5370 kcal/mol and heat of formation −78.0985 kcal/mol. After the geometry optimization by UFF (molecular mechanics) technique, the final geometrical energy of the ligand has been computed to 161.2699 kcal/mol and this provides stability of the molecule [50, 51]. The surface structure of the ligand has been computed through HOMO and LUMO plot. Similar study with the NiII and CuII complexes has assured their final geometrical energy 449.0564 and 752.1825 kcal/mol, respectively. The optimized structures of the metal complexes are presented in Figures 8 and 9 and they reveal square planar geometry for NiII and tetrahedral geometry for CuII complexes. The computational findings are in good support of the proposed structures of the complexes. The selected bond lengths, bond angles, and bond energies of the ligand and metal complexes are given in Tables 8(a)–8(f).Table 8
(a) Selected bond lengths and bond energies of ligand (HL). (b) Selected bond angles and bond energies of ligand (HL). (c) Selected bond lengths and bond energies of NiII-complex. (d) Selected bond angles and bond energies of NiII-complex. (e) Selected bond lengths and bond energies of CuII-complex. (f) Selected bond angles and bond energies of CuII-complex.
(a)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
C8-N15
1.447
532.154
N15-C16
1.291
749.036
C16-C17
1.464
386.878
C8-C22
1.489
367.716
C22-N23
1.437
543.390
N23-C24
1.462
515.889
(b)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
C8-N15-C16
120.00
226.230
N15-C8-C22
109.47
312.267
N15-C16-C17
120.00
295.502
N15-C8-H14
109.47
169.990
C22-N23-C24
106.70
261.205
N23-C22-O25
120.00
378.598
(c)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
Ni1-N2
1.885
306.275
Ni1-N3
1.885
306.275
Ni1-N4
1.870
313.824
Ni1-N5
1.870
313.824
(d)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
N2-Ni1-N3
90.00
340.090
N2-Ni1-N4
90.00
344.228
N2-Ni1-N5
90.00
344.228
Ni1-N2-C9
106.00
212.735
Ni1-N2-C24
106.00
208.934
N3-Ni1-N4
90.00
344.228
N3-Ni1-N5
90.00
344.228
N4-Ni1-N5
90.00
348.473
(e)
Bond type
Bond lengths (Å)
Bond energy (kcal/mol)
Cu1-N2
2.031
176.938
Cu1-N3
2.031
176.938
Cu1-N4
2.016
181.007
Cu1-N5
2.016
181.007
(f)
Bond type
Bond angle (°)
Bond energy (kcal/mol)
N2-Cu1-N3
109.47
156.977
N2-Cu1-N4
109.47
158.764
N2-Cu1-N5
109.47
158.764
Cu1-N2-C9
106.70
132.072
Cu1-N2-C24
106.70
129.991
N3-Cu1-N4
109.47
158.764
N3-Cu1-N5
109.47
158.764
N4-Cu1-N5
109.47
160.587Figure 8
Molecular modeling structure of Ni(Haαft)2.Figure 9
Molecular modeling structure of Cu(Haαft)2.


## 4. Conclusion

The present study focuses the microbiological interaction of prepared compounds against clinically important bacterial pathogens. The antibacterial sensitivity data of the compounds presented in this report allowed us to state that the metal complexes have generally better antibacterial activity than uncomplexed ligand, but less active than control drug. The electronic absorption spectral study reveals d-d transition band at 520 nm forNiII complex and this high energy process suggests its square planar geometry. The charge transfer band for CuII complex at 450 nm indicates its tetrahedral geometry. X-ray powder diffraction study reveals triclinic crystal system for the ligand and CuII complex, while it is trigonal crystal system for NiII complex. The particle size calculation by Scherrer’s formula indicates their nanocrystalline nature. The ESI-MS study that provided molecular mass of the ligand and metal complexes truly confirms the ML2 type of complexes. The FT-IR, 1H NMR, and 13C NMR spectral results are also in good agreement with the proposed molecular and structural formula of the ligand and its metal complexes. The change in pH value occurring in the reaction process greatly supports the deprotonation during complex formation which is further supported by the change in their colors. The sharp melting point of the compounds gives the evidence of purity of the synthesized compounds.



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*Source: 136285-2015-12-08.xml*