# Synthesis and Characterization of Cobalt(III) and Copper(II) Complexes of 2-((E)-(6-Fluorobenzo[d]thiazol-2-ylimino) methyl)-4-chlorophenol: DNA Binding and Nuclease Studies—SOD and Antimicrobial Activities

Authors: K. Savithri; B. C. Vasantha Kumar; H. K. Vivek; H. D. Revanasiddappa
Journal: International Journal of Spectroscopy
 (2018)

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## Abstract

A bidentate (N- and O-) imine-based ligand(L1) and its metal complexes of types [CuII(L1)2](C1), [CuII(L1)(Phen)](C2), [CoIII(L1)2](C3), and [CoIII(L1)(Phen)](C4) (L1 = 2-((E)-(6-fluorobenzo[d]thiazol-2-ylimino)methyl)-4-chlorophenol and phen = 1,10-phenanthroline) were synthesized as potential chemotherapeutic drug candidates. The prepared complexes were structurally characterized by spectral techniques (NMR, FT-IR, LC-MS, EPR, and electronic absorption), thermogravimetric analysis (TGA/DTA), magnetic moment, and CHNO elemental analysis. Spectroscopic studies suggested the distorted octahedral structure for all complexes.In vitro bioassay studies include binding and nuclease activities of the ligand and its complexes with target calf thymus- (CT-) DNA were carried out by employing UV-Vis, fluorescence spectroscopy, viscosity, and gel electrophoresis techniques. The extent of binding propensity was determined quantitatively by Kb and Ksv values which revealed a higher binding affinity for C2 and C4 as compared to C1 and C3. In addition, the scavenging superoxide anion free radical (O∙-2) activity of metal complexes was determined by nitroblue tetrazolium (NBT) light reduction assay. Molecular docking studies with DNA and SOD enzyme were also carried out on these compounds. The antimicrobial study has shown that all the compounds are potential antibacterial agents against Gram-negative bacterial strains and better antifungal agents with respect to standard drugs used.


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## Body

## 1. Introduction

Imine-based ligands coordinated to transition metal ions have several advantages, are also very popular now, and are being used at the forefront of the development of DNA molecular probes (DNA-binding metal complexes) and therapeutic agents [1, 2]. Transition metal complexes that are suitable for binding and cleaving nucleic acids are of significant interest due to their various applications in nucleic acid chemistry, like foot-printing studies and sequence-specific binding agents and also as a putative anticancer drug.DNA executes an imperative constituent for many biochemical progressions that rise in the cellular system as in various regulatory processes/gene expressions. These processes can be modified by the interaction of chemical compounds with specific regions of DNA. Some of the d-block metal complexes activate endonucleolytic cleavage reaction in DNA photolytically or with the aid of external agents [3]. DNA is an attractive motif for the design of novel chemotherapeutics of cancer as the process involves DNA replication during the S phase of cell cycle [4]. The covalent and noncovalent interactions of transition metal complexes with DNA lead to biological activity [5, 6]. The DNA cleavage is an important enzymatic reaction involved in several biological processes as well as in biotechnological manipulation of genetic material. Artificial DNA cleaving agents could find applications in several fields, in nucleic acids structural studies, natural process as biotechnological manipulation of genetic material, or drug development [7]. Medicinal inorganic chemistry covers broad applications of metals in pharmaceuticals [8]. Chemically, Lewis acidic metal centers are well opting to influence fundamental cellular processes due to their affinity for basic N- and O- donor ligands, large aromatic manners capable of π-interactions with nucleic acid building blocks.A bicyclic heteronuclear compound comprises benzothiazole—a unique synthon in synthetic therapeutic chemistry [9]. 2-Amino benzothiazole derivatives have received considerable attention owing to their unique structures and exquisite pharmacophores observed in many diagnostic and therapeutic agents. A literature review has illustrated that the substitution at 4, 5, and 6th positions of 2-aminobenzothiazole improves biological activities. Moreover, imine bases derived from 2-aminobenzothiazole are of great importance due to their wide applications as antimicrobial, anti-inflammatory, antidegenerative, and anti-HIV agents [10–12]. Fluorobenzothiazole derivatives possess exquisite potency and selectivity in cytotoxicity with a broad spectrum of action than their parent nonfluorinated counterparts and have been therefore comprehensively explored for chemotherapeutic applications in drug design [13, 14].Recently, metal complexes have shown biological activity in many mammalian cell systemsin vitro andin vivo[15]. Metal complexes of imine bases derived from substituted aldehydes and heterocyclic compounds containing nitrogen, sulfur, and/or oxygen as ligand atoms are of interest as simple structural models of more complicated biological systems [16]. Hence, much attention has been given on the design of metal-based complexes. Copper is an essential endogenously biocompatible metal ion found in the living system which may be less toxic than the other nonessential metal ions. Cu(II) complexes are preferred candidates for various pharmacostudies due to the presence of its biorelevant ligands which can bind and cleave DNA [17]. The biological behavior of Cu(II) complexes has been subjected to intense investigation for DNA binding and cleavage activities [18] for novel chemotherapeutics and highly sensitive diagnostic agents [19]. Structural features and donor atoms of the complex may influence significant factors such as the lipophilic/hydrophilic nature of the compound, the favoured oxidation state of the copper center, and the observed biological reactivity of the complexes [20]. Cobalt involves itself in the regulation of DNA synthesis indirectly and in cobalt-dependent proteins which make it an essential biological element [21]. Cobalt(III) complexes have been widely investigated in coordination chemistry and biochemistry [22] owing to their therapeutic activities [23]. Copper and cobalt are bioessential metals in all living systems which show antifungal and antibacterial properties against several pathogenic fungi and bacteria depending on the reaction with the central DNA system [24]. The binding of fluorescent polycyclic molecules to DNA can be conveniently investigated by a variety of techniques, including absorption and fluorescence spectroscopic methods because their absorption and emission properties significantly change on complex formation [25].Superoxide dismutase (SOD) is found in many organisms, and there still exist some shortcomings in a wide range of clinical applications of SOD [26]. Hence, special attention is paid to the artificial mimics of SOD. Developing highly efficient and stable SOD mimics is one of the crucial projects in biochemistry [27]. Copper complexes of salicylic acid are potent SOD mimetic as transition metal ion complexes have generally been used as antioxidants to eliminate noxious reactive oxygen species. Among the reported mimics, the highest SOD-like activity is only 20% of the bovine erythrocyte Cu, Zn-SOD [28]. Along with copper, some of the metals such as iron [29], manganese [29, 30], ruthenium [31], and cobalt [32] show a marked SOD activity and seem to retain it in living cells which has been reported [33]. Molecular dynamics in computational chemistry track precise dynamics in atomic detail. They allow for the simulation to be extended to larger molecular systems, like proteins and nucleic acids as their approach accurately and efficiently explores conformational space with improved sampling and converges to the correct canonical probability distribution [34].In continuation of our previous research work [35] on the detailed study of L1, the present research paper describes the synthesis of imine-based complexes of essential transition metals involving Co(III) and Cu(II) and mixed ligand complexes in presence of 1,10-phenanthroline. The prepared complexes were subjected to spectroscopic structural elucidation. The interaction of complexes with DNA has also been investigated using electronic absorption, fluorescence spectroscopy, viscosity measurement, and gel electrophoresis. The SOD mimic activity was determined using a nonenzymatic NBT system. Molecular docking studies were to unravel the mode of binding of the compounds with DNA and SOD. With investigation of the antimicrobial (against pathogenic strains of bacteria and fungi), a minimum concentration of the compounds sufficient to inhibit the microbial growth (MIC) was obtained with a focus on potential new and unique and versatile scaffolds for pharmaceutical efficacy profile.


## 2. Experimental Section

### 2.1. Materials

CuCl2·2H2O, CoCl2·6H2O, DMSO, superoxide dismutase (SOD), methyl green, ascorbic acid, sodium azide (NaN3), Tris(hydroxymethyl)aminomethane, disodium salt of calf thymus DNA (highly polymerized, stored at 4°C), 4,6-diamino-phenylindole (DAPI), H2O2 (Merck), NBT, pUC18 supercoiled plasmid DNA (Genei), and ethidium bromide (EB) were purchased from Sigma Corp. and they were used as supplied.


### 2.2. Methods and Instrumentation

The melting point determination in an open capillary tube using a precision digi melting point apparatus and was uncorrected. Mass spectra of synthesized compounds were recorded using a 2010 EV LC-MS Shimadzu spectrometer. Microanalysis (C, H, N, O, and M) was performed on a Perkin-Elmer elemental analyzer. Magnetic susceptibility measurements were performed by the Gouy technique in the solid state at room temperature and Hg[Co(NCS)4] is the standard used. Electronic spectra were recorded (200–800 nm) in DMSO using a UV-Vis spectrophotometer (DU 730 “Life Science” M/S, Beckman Coulter, USA). IR spectra were recorded on a Perkin-Elmer 783 spectrophotometer via attenuated total reflection (FT-ATR) in the range of 4000–400 cm−1. TGA analysis was performed on Shimadzu AT-50 thermal analyzer from 25 to 700°C with a heating rate at 10°C/min under N2 atmosphere. Electron paramagnetic resonance (EPR) spectra were recorded using a JEOL JES-TE100 EPR spectrometer in DMSO solution at LNT in the solid state on X-band at a frequency of 9.13 GHz under the magnetic field of 300 mT. Fluorescence measurements were performed on RF-5301P spectrofluorophotometer (Shimadzu) equipped with a 150-W Xenon lamp, using a quartz cell path length of 1 cm at a slit width of 5.0 nm.


#### 2.2.1. Synthesis of Metal Complexes (C1 and C3)

A synthetic scheme (Figure1) of metal complexes and mixed ligand complexes is described as follows.Figure 1
General scheme for the synthesis of L1 and its metal complexes.The ligand, L1 (2 mmol), was dissolved in ethanol by heating and intensive stirring. To the warm suspension, a warm ethanol solution of CuCl2·2H2O and/or CoCl2·6H2O (1 mmol) was added dropwise. The resulting mixture was kept under reflux over a water bath for 4 h at 80°C. The solvent was evaporated in vacuo, and the obtained solid was directly used for further processing.


#### 2.2.2. Synthesis of Mixed Ligand Complexes (C2 and C4) with 1,10-Phenanthroline

An ethanolic solution of 1,10-phenanthroline (1 mmol) was added to hot ethanolic solution of CuCl2·2H2O/CoCl2·6H2O (1 mmol) with constant stirring, followed by dropwise addition of ethanolic L1 (1 mmol). The reaction mixture was then refluxed for 4.5 h at 60°C. Later, the obtained precipitate was filtered and washed with cold ethanol twice. The solid product was dried under desiccator and weighed.C1: [Cu(L1)2(H2O)2] (H2O)2.  Yield = 70%, brown color,Anal. (%) for C28H22Cl2CuF2N4O6S2: Found (Calc.): C 45.03 (45.02), H 2.95 (2.97), Cu 8.52 (8.51), N 7.48 (7.50), O 12.82 (12.85);mp = >300°C. m/z: 747.07, 749.21, 750.14;IR (υmax/cm−1): (HC=N) azomethine 1639; M-O 568; M-N 445; H2O 3392, 862.C2: [Cu(L1)(phen)(H2O)(Cl)]. Yield = 68%, inchworm green color,Anal. (%) C27H20Cl2CuFN4O2S: Found (Calc.) C 54.81 (52.47), H 3.27 (3.26), Cu 10.26 (10.28), N 9.06 (9.07), O 75.14 (5.18);mp = 286–288°C. m/z: 617.98, 620.32;IR (υmax/cm−1); (HC=N) azomethine 1638; M-O 576; M-N 442; M-Cl 371; H2O 3382, 851.C3: [Co(L1)2(H2O)2]Cl. Yield = 72%, brown color,Anal. (%)for C28H18Cl3CoF2N4O4S2-; Found (Calc.) C 45.33 (45.31), H 2.45 (2.44), Co 7.94 (7.90), N 7.55 (7.54), O 8.63 (8.61);mp = 294–296°C. m/z: 741.88, 744.32, 745.26;IR (υmax/cm−1); (HC=N) azomethine 1640; M-O 542; M-N 463; M-Cl 362, H2O 3387, 856.C4: [Co(L1)(phen)(Cl)2]. Yield = 63%, bottle green color,Anal.(%) for C26H15Cl3CoFN4OS: Found (Calc.) C 50.70 (50.71), H 2.45 (2.46), Co 9.54 (9.57), N 9.08 (9.10), O 2.59 (2.60);mp ≥ 300°C. m/z: 615.77, 618.36; IR (υmax/cm−1); (HC=N) azomethine 1633; M-O 576; M-N 468; M-Cl 372.


### 2.3. Bioassay Studies

#### 2.3.1. DNA-Binding Experiments

Electronic Absorption Spectral Titration.The stock solution of CT-DNA was prepared in 5 mM Tris-HCl/50 mM NaCl buffer at pH 7, which gave A260/A280nm ofca. 1.8–1.9, indicating that the DNA was sufficiently devoid of protein [36], and the concentration of DNA was determined from its absorption intensity at 260 nm (ε260 = 6600 M−1 cm−1) [37]. All the stock solutions were stored at 4°C and used within four days. The intrinsic binding constant (Kb) values of the complexes to CT-DNA were obtained by monitoring the change in the absorption intensity of the spectral bands with increasing concentration of DNA. After equilibrium had been reached, the spectra were recorded at 200–500 nm against an analogous solution of DNA as a reference. UV spectral data were fitted into Wolfe-Shimer equation (1) [38] to obtain the intrinsic binding association constant (Kb):(1)DNAεa-εb=DNAεb-εf+1Kbεb-εf,where [DNA] is the concentration of DNA in base pairs, εa is apparent extinction coefficient (Aobs/[MC]), εb is the extinction coefficient of the metal complex in the fully bound form, and the extinction coefficient for free metal complex [MC] is εf. The value of Kb was calculated as the ratio of the slope to intercept.Fluorimetric Studies.Ethidium bromide (EB) emits intense fluorescence light in the presence of DNA at λex 600 nm (546 nm) due to strong intercalation between adjacent DNA base pairs. The fluorescence emission intensity can be quenched when the second molecule was added to the CT-DNA bound EB solution. In the fluorescence quenching study, [DNA]/[EB]=1.13 is kept constant and varied with the concentration of the compounds. The fluorescence spectra of the reaction mixture were recorded between 500 and 850 nm at excitation wavelength 515 nm. The fluorescence quenching efficiency is evaluated according to the classical Stern-Volmer equation (2). The binding constant (Kb) and number of binding sites (n) can be determined from emission spectra with (3).(2)FoF=1+KsvQ(3)logFo-FF=log⁡Kb+nlog⁡Q.The fluorescence intensities in absence and presence of the quencher (complexes) are termed Fo and F as, respectively, “Q” is the concentration of the quencher and Ksv is the Stern-Volmer quenching constant.Viscosity Measurements.Viscosity experiments were carried out on an Ostwald microviscometer, immersed in a thermostat water bath maintained at a constant temperature at 26°C. Compounds were added to DNA solution (10 μmolL−1) with a micropipette. The concentration of the compounds was maintained in the range of 0–10 μML−1. Data were graphically presented as η/ηo1/3 versus the ratio of the concentration of compounds to DNA (r), where η was the viscosity of DNA in the presence of compound and ηo was the viscosity of DNA alone. The relative viscosity η was calculated using [39](4)η=t-toto,where to and t represent the flow time of buffer solution through the capillary and observed flow time for DNA in the absence and presence of the complex, respectively. The mean of three replicate measurements was used to evaluate the viscosity of the samples.


#### 2.3.2. DNA Cleavage Assay

Agarose-gel electrophoresis monitored the ability of transition metal complexes to cleave plasmid DNA. The experiment was accomplished with supercoiled pUC18 (200 ng, 1μL) which was treated with varying concentrations of compounds (10–50 μM) in Tris-boric acid-buffer with NaCl (50 mM, pH 7.2) by agarose-gel electrophoresis method. The samples (5 μL in Tris-buffer) were incubated at 37°C for 45 min in water bath; to this solution, 1 μL loading buffer (0.25% bromophenol blue and 30% glycerol) was added. This mixture was loaded in the 1% agarose gel and electrophoresis was carried out at 60 V for an hour. The agarose gel was prestained with 0.5 μg/mL ethidium bromide (EtBr) and visualized under UV light and photographed for further analysis. The cleavage properties were determined based on the ability of compounds to convert the supercoiled form (Form I) into nicked (Form II) and linear form (Form III) [23].


#### 2.3.3. Superoxide Dismutase (SOD) Assay

The superoxide dismutase activities of the synthesized metal complexes were assessed by colorimetric-based assay with xanthine/xanthine oxidase system as the source ofO2∙- due to their conducive solubility. The quantitative reduction of nitroblue tetrazolium (NBT) to monoformazan (MF+) by the O2∙- changes the color from yellow to blue which was followed spectrophotometrically at 560 nm. The suppression ratio was calculated using standard equation [Acontrol-Asample/Acontrol] × 100. In the SOD-like activity test, the metal complexes compete with NBT for oxidation of the generated superoxide ions. Plotting the results as the percentage of inhibiting NBT for comparative concentrations of complexes was determined by absorption changes. Tabulated results were derived from linear regression analysis and are given as the concentration (μM) equivalent to 1 unit of native Cu Zn-SOD activity (IC50 = 0.04 μM dm−3) [40]. A unit SOD activity is the concentration of the complex or enzyme which causes 50% inhibition in the reduction of NBT.


#### 2.3.4. Molecular Docking

Crystal structure of DNA dodecamer (1BNA.pdb) with the sequence of d(CpGpCpGpApApTpTpCpGpCpG) and Cu, Zn-SOD (1CB4) was downloaded from the protein data bank (http://www.rcsb.org) and used for docking studies. Compounds were drawn using Maestro 2D sketcher and energy minimization was computed by OPLS 2005, while, for the preparation of the DNA or Cu, Zn-SOD, hydrogen was added to the polar atoms and the valency of the metal ions was optimized [41]. Meanwhile, the water molecules and the substrate were deleted. The DNA was minimized to some extent after hydrogen was added. Finally, a grid for DNA [with the dimension (10 Å × 10 Å × 10 Å)] and Cu, Zn-SOD [with the dimension (20 Å × 20 Å × 20 Å)] were prepared. The dimension of the grid was in such a manner that the grid covers the complete DNA. Using Extraprecision (XP) docking protocol, compounds were evaluated based on glide scoring which was docking into the receptor grid of radii as mentioned above [42].


#### 2.3.5. Antimicrobial Activity

All the synthesized compounds were screenedin vitro for their antimicrobial activity against Gram -ve bacteria asEscherichia coli(MTCC 443) andPseudomonas aeruginosa(MTCC 2453) and Gram +ve bacterial strains asBacillus subtilis (MTCC 121) andStaphylococcus aureus(MTCC 3160), and fungal strains areCandida albicans(ATCC 10231) andAspergillus niger(ATCC 6275), and standard antibiotic ciprofloxacin (25 mg) and antifungal fluconazole (25 mg) served as the positive control. The impact was tested in terms of minimum inhibitory concentration (MIC) using a serial plate dilution assay [43]. Microbial cultures were incubated at 37°C for a day in case of bacteria and 72 h for fungi, respectively. 100 μL of Mueller-Hinton broth of bacteria was pipetted into each well; to this, a 10 μL suspension of the test pathogens was then added. 4% DMSO was used as a solvent for solution preparation and served as a negative control in order to monitor sample sterility and to determine any antimicrobial influence of the solvent. Inhibition zone was measured, and MIC was determined using double-fold serial dilution in liquid media containing varying concentrations of test compounds from 1 to 1000 μg/mL. Bacterial growth was measured by the turbidity of the culture after 18 h. Turbidity standard as McFarland Standard 0.5 solution was used. If particular concentration of compound inhibits bacterial growth, half the concentration of the compound was tested. This procedure was carried on to a concentration at which bacteria grow normally. The lowest concentration that inhibits the bacterial growth was determined as MIC value. Three replicates were maintained per test microbe. The resultant MIC values were determined as the mean of these replicate experiments.


## 2.1. Materials

CuCl2·2H2O, CoCl2·6H2O, DMSO, superoxide dismutase (SOD), methyl green, ascorbic acid, sodium azide (NaN3), Tris(hydroxymethyl)aminomethane, disodium salt of calf thymus DNA (highly polymerized, stored at 4°C), 4,6-diamino-phenylindole (DAPI), H2O2 (Merck), NBT, pUC18 supercoiled plasmid DNA (Genei), and ethidium bromide (EB) were purchased from Sigma Corp. and they were used as supplied.


## 2.2. Methods and Instrumentation

The melting point determination in an open capillary tube using a precision digi melting point apparatus and was uncorrected. Mass spectra of synthesized compounds were recorded using a 2010 EV LC-MS Shimadzu spectrometer. Microanalysis (C, H, N, O, and M) was performed on a Perkin-Elmer elemental analyzer. Magnetic susceptibility measurements were performed by the Gouy technique in the solid state at room temperature and Hg[Co(NCS)4] is the standard used. Electronic spectra were recorded (200–800 nm) in DMSO using a UV-Vis spectrophotometer (DU 730 “Life Science” M/S, Beckman Coulter, USA). IR spectra were recorded on a Perkin-Elmer 783 spectrophotometer via attenuated total reflection (FT-ATR) in the range of 4000–400 cm−1. TGA analysis was performed on Shimadzu AT-50 thermal analyzer from 25 to 700°C with a heating rate at 10°C/min under N2 atmosphere. Electron paramagnetic resonance (EPR) spectra were recorded using a JEOL JES-TE100 EPR spectrometer in DMSO solution at LNT in the solid state on X-band at a frequency of 9.13 GHz under the magnetic field of 300 mT. Fluorescence measurements were performed on RF-5301P spectrofluorophotometer (Shimadzu) equipped with a 150-W Xenon lamp, using a quartz cell path length of 1 cm at a slit width of 5.0 nm.


### 2.2.1. Synthesis of Metal Complexes (C1 and C3)

A synthetic scheme (Figure1) of metal complexes and mixed ligand complexes is described as follows.Figure 1
General scheme for the synthesis of L1 and its metal complexes.The ligand, L1 (2 mmol), was dissolved in ethanol by heating and intensive stirring. To the warm suspension, a warm ethanol solution of CuCl2·2H2O and/or CoCl2·6H2O (1 mmol) was added dropwise. The resulting mixture was kept under reflux over a water bath for 4 h at 80°C. The solvent was evaporated in vacuo, and the obtained solid was directly used for further processing.


### 2.2.2. Synthesis of Mixed Ligand Complexes (C2 and C4) with 1,10-Phenanthroline

An ethanolic solution of 1,10-phenanthroline (1 mmol) was added to hot ethanolic solution of CuCl2·2H2O/CoCl2·6H2O (1 mmol) with constant stirring, followed by dropwise addition of ethanolic L1 (1 mmol). The reaction mixture was then refluxed for 4.5 h at 60°C. Later, the obtained precipitate was filtered and washed with cold ethanol twice. The solid product was dried under desiccator and weighed.C1: [Cu(L1)2(H2O)2] (H2O)2.  Yield = 70%, brown color,Anal. (%) for C28H22Cl2CuF2N4O6S2: Found (Calc.): C 45.03 (45.02), H 2.95 (2.97), Cu 8.52 (8.51), N 7.48 (7.50), O 12.82 (12.85);mp = >300°C. m/z: 747.07, 749.21, 750.14;IR (υmax/cm−1): (HC=N) azomethine 1639; M-O 568; M-N 445; H2O 3392, 862.C2: [Cu(L1)(phen)(H2O)(Cl)]. Yield = 68%, inchworm green color,Anal. (%) C27H20Cl2CuFN4O2S: Found (Calc.) C 54.81 (52.47), H 3.27 (3.26), Cu 10.26 (10.28), N 9.06 (9.07), O 75.14 (5.18);mp = 286–288°C. m/z: 617.98, 620.32;IR (υmax/cm−1); (HC=N) azomethine 1638; M-O 576; M-N 442; M-Cl 371; H2O 3382, 851.C3: [Co(L1)2(H2O)2]Cl. Yield = 72%, brown color,Anal. (%)for C28H18Cl3CoF2N4O4S2-; Found (Calc.) C 45.33 (45.31), H 2.45 (2.44), Co 7.94 (7.90), N 7.55 (7.54), O 8.63 (8.61);mp = 294–296°C. m/z: 741.88, 744.32, 745.26;IR (υmax/cm−1); (HC=N) azomethine 1640; M-O 542; M-N 463; M-Cl 362, H2O 3387, 856.C4: [Co(L1)(phen)(Cl)2]. Yield = 63%, bottle green color,Anal.(%) for C26H15Cl3CoFN4OS: Found (Calc.) C 50.70 (50.71), H 2.45 (2.46), Co 9.54 (9.57), N 9.08 (9.10), O 2.59 (2.60);mp ≥ 300°C. m/z: 615.77, 618.36; IR (υmax/cm−1); (HC=N) azomethine 1633; M-O 576; M-N 468; M-Cl 372.


## 2.2.1. Synthesis of Metal Complexes (C1 and C3)

A synthetic scheme (Figure1) of metal complexes and mixed ligand complexes is described as follows.Figure 1
General scheme for the synthesis of L1 and its metal complexes.The ligand, L1 (2 mmol), was dissolved in ethanol by heating and intensive stirring. To the warm suspension, a warm ethanol solution of CuCl2·2H2O and/or CoCl2·6H2O (1 mmol) was added dropwise. The resulting mixture was kept under reflux over a water bath for 4 h at 80°C. The solvent was evaporated in vacuo, and the obtained solid was directly used for further processing.


## 2.2.2. Synthesis of Mixed Ligand Complexes (C2 and C4) with 1,10-Phenanthroline

An ethanolic solution of 1,10-phenanthroline (1 mmol) was added to hot ethanolic solution of CuCl2·2H2O/CoCl2·6H2O (1 mmol) with constant stirring, followed by dropwise addition of ethanolic L1 (1 mmol). The reaction mixture was then refluxed for 4.5 h at 60°C. Later, the obtained precipitate was filtered and washed with cold ethanol twice. The solid product was dried under desiccator and weighed.C1: [Cu(L1)2(H2O)2] (H2O)2.  Yield = 70%, brown color,Anal. (%) for C28H22Cl2CuF2N4O6S2: Found (Calc.): C 45.03 (45.02), H 2.95 (2.97), Cu 8.52 (8.51), N 7.48 (7.50), O 12.82 (12.85);mp = >300°C. m/z: 747.07, 749.21, 750.14;IR (υmax/cm−1): (HC=N) azomethine 1639; M-O 568; M-N 445; H2O 3392, 862.C2: [Cu(L1)(phen)(H2O)(Cl)]. Yield = 68%, inchworm green color,Anal. (%) C27H20Cl2CuFN4O2S: Found (Calc.) C 54.81 (52.47), H 3.27 (3.26), Cu 10.26 (10.28), N 9.06 (9.07), O 75.14 (5.18);mp = 286–288°C. m/z: 617.98, 620.32;IR (υmax/cm−1); (HC=N) azomethine 1638; M-O 576; M-N 442; M-Cl 371; H2O 3382, 851.C3: [Co(L1)2(H2O)2]Cl. Yield = 72%, brown color,Anal. (%)for C28H18Cl3CoF2N4O4S2-; Found (Calc.) C 45.33 (45.31), H 2.45 (2.44), Co 7.94 (7.90), N 7.55 (7.54), O 8.63 (8.61);mp = 294–296°C. m/z: 741.88, 744.32, 745.26;IR (υmax/cm−1); (HC=N) azomethine 1640; M-O 542; M-N 463; M-Cl 362, H2O 3387, 856.C4: [Co(L1)(phen)(Cl)2]. Yield = 63%, bottle green color,Anal.(%) for C26H15Cl3CoFN4OS: Found (Calc.) C 50.70 (50.71), H 2.45 (2.46), Co 9.54 (9.57), N 9.08 (9.10), O 2.59 (2.60);mp ≥ 300°C. m/z: 615.77, 618.36; IR (υmax/cm−1); (HC=N) azomethine 1633; M-O 576; M-N 468; M-Cl 372.


## 2.3. Bioassay Studies

### 2.3.1. DNA-Binding Experiments

Electronic Absorption Spectral Titration.The stock solution of CT-DNA was prepared in 5 mM Tris-HCl/50 mM NaCl buffer at pH 7, which gave A260/A280nm ofca. 1.8–1.9, indicating that the DNA was sufficiently devoid of protein [36], and the concentration of DNA was determined from its absorption intensity at 260 nm (ε260 = 6600 M−1 cm−1) [37]. All the stock solutions were stored at 4°C and used within four days. The intrinsic binding constant (Kb) values of the complexes to CT-DNA were obtained by monitoring the change in the absorption intensity of the spectral bands with increasing concentration of DNA. After equilibrium had been reached, the spectra were recorded at 200–500 nm against an analogous solution of DNA as a reference. UV spectral data were fitted into Wolfe-Shimer equation (1) [38] to obtain the intrinsic binding association constant (Kb):(1)DNAεa-εb=DNAεb-εf+1Kbεb-εf,where [DNA] is the concentration of DNA in base pairs, εa is apparent extinction coefficient (Aobs/[MC]), εb is the extinction coefficient of the metal complex in the fully bound form, and the extinction coefficient for free metal complex [MC] is εf. The value of Kb was calculated as the ratio of the slope to intercept.Fluorimetric Studies.Ethidium bromide (EB) emits intense fluorescence light in the presence of DNA at λex 600 nm (546 nm) due to strong intercalation between adjacent DNA base pairs. The fluorescence emission intensity can be quenched when the second molecule was added to the CT-DNA bound EB solution. In the fluorescence quenching study, [DNA]/[EB]=1.13 is kept constant and varied with the concentration of the compounds. The fluorescence spectra of the reaction mixture were recorded between 500 and 850 nm at excitation wavelength 515 nm. The fluorescence quenching efficiency is evaluated according to the classical Stern-Volmer equation (2). The binding constant (Kb) and number of binding sites (n) can be determined from emission spectra with (3).(2)FoF=1+KsvQ(3)logFo-FF=log⁡Kb+nlog⁡Q.The fluorescence intensities in absence and presence of the quencher (complexes) are termed Fo and F as, respectively, “Q” is the concentration of the quencher and Ksv is the Stern-Volmer quenching constant.Viscosity Measurements.Viscosity experiments were carried out on an Ostwald microviscometer, immersed in a thermostat water bath maintained at a constant temperature at 26°C. Compounds were added to DNA solution (10 μmolL−1) with a micropipette. The concentration of the compounds was maintained in the range of 0–10 μML−1. Data were graphically presented as η/ηo1/3 versus the ratio of the concentration of compounds to DNA (r), where η was the viscosity of DNA in the presence of compound and ηo was the viscosity of DNA alone. The relative viscosity η was calculated using [39](4)η=t-toto,where to and t represent the flow time of buffer solution through the capillary and observed flow time for DNA in the absence and presence of the complex, respectively. The mean of three replicate measurements was used to evaluate the viscosity of the samples.


### 2.3.2. DNA Cleavage Assay

Agarose-gel electrophoresis monitored the ability of transition metal complexes to cleave plasmid DNA. The experiment was accomplished with supercoiled pUC18 (200 ng, 1μL) which was treated with varying concentrations of compounds (10–50 μM) in Tris-boric acid-buffer with NaCl (50 mM, pH 7.2) by agarose-gel electrophoresis method. The samples (5 μL in Tris-buffer) were incubated at 37°C for 45 min in water bath; to this solution, 1 μL loading buffer (0.25% bromophenol blue and 30% glycerol) was added. This mixture was loaded in the 1% agarose gel and electrophoresis was carried out at 60 V for an hour. The agarose gel was prestained with 0.5 μg/mL ethidium bromide (EtBr) and visualized under UV light and photographed for further analysis. The cleavage properties were determined based on the ability of compounds to convert the supercoiled form (Form I) into nicked (Form II) and linear form (Form III) [23].


### 2.3.3. Superoxide Dismutase (SOD) Assay

The superoxide dismutase activities of the synthesized metal complexes were assessed by colorimetric-based assay with xanthine/xanthine oxidase system as the source ofO2∙- due to their conducive solubility. The quantitative reduction of nitroblue tetrazolium (NBT) to monoformazan (MF+) by the O2∙- changes the color from yellow to blue which was followed spectrophotometrically at 560 nm. The suppression ratio was calculated using standard equation [Acontrol-Asample/Acontrol] × 100. In the SOD-like activity test, the metal complexes compete with NBT for oxidation of the generated superoxide ions. Plotting the results as the percentage of inhibiting NBT for comparative concentrations of complexes was determined by absorption changes. Tabulated results were derived from linear regression analysis and are given as the concentration (μM) equivalent to 1 unit of native Cu Zn-SOD activity (IC50 = 0.04 μM dm−3) [40]. A unit SOD activity is the concentration of the complex or enzyme which causes 50% inhibition in the reduction of NBT.


### 2.3.4. Molecular Docking

Crystal structure of DNA dodecamer (1BNA.pdb) with the sequence of d(CpGpCpGpApApTpTpCpGpCpG) and Cu, Zn-SOD (1CB4) was downloaded from the protein data bank (http://www.rcsb.org) and used for docking studies. Compounds were drawn using Maestro 2D sketcher and energy minimization was computed by OPLS 2005, while, for the preparation of the DNA or Cu, Zn-SOD, hydrogen was added to the polar atoms and the valency of the metal ions was optimized [41]. Meanwhile, the water molecules and the substrate were deleted. The DNA was minimized to some extent after hydrogen was added. Finally, a grid for DNA [with the dimension (10 Å × 10 Å × 10 Å)] and Cu, Zn-SOD [with the dimension (20 Å × 20 Å × 20 Å)] were prepared. The dimension of the grid was in such a manner that the grid covers the complete DNA. Using Extraprecision (XP) docking protocol, compounds were evaluated based on glide scoring which was docking into the receptor grid of radii as mentioned above [42].


### 2.3.5. Antimicrobial Activity

All the synthesized compounds were screenedin vitro for their antimicrobial activity against Gram -ve bacteria asEscherichia coli(MTCC 443) andPseudomonas aeruginosa(MTCC 2453) and Gram +ve bacterial strains asBacillus subtilis (MTCC 121) andStaphylococcus aureus(MTCC 3160), and fungal strains areCandida albicans(ATCC 10231) andAspergillus niger(ATCC 6275), and standard antibiotic ciprofloxacin (25 mg) and antifungal fluconazole (25 mg) served as the positive control. The impact was tested in terms of minimum inhibitory concentration (MIC) using a serial plate dilution assay [43]. Microbial cultures were incubated at 37°C for a day in case of bacteria and 72 h for fungi, respectively. 100 μL of Mueller-Hinton broth of bacteria was pipetted into each well; to this, a 10 μL suspension of the test pathogens was then added. 4% DMSO was used as a solvent for solution preparation and served as a negative control in order to monitor sample sterility and to determine any antimicrobial influence of the solvent. Inhibition zone was measured, and MIC was determined using double-fold serial dilution in liquid media containing varying concentrations of test compounds from 1 to 1000 μg/mL. Bacterial growth was measured by the turbidity of the culture after 18 h. Turbidity standard as McFarland Standard 0.5 solution was used. If particular concentration of compound inhibits bacterial growth, half the concentration of the compound was tested. This procedure was carried on to a concentration at which bacteria grow normally. The lowest concentration that inhibits the bacterial growth was determined as MIC value. Three replicates were maintained per test microbe. The resultant MIC values were determined as the mean of these replicate experiments.


## 2.3.1. DNA-Binding Experiments

Electronic Absorption Spectral Titration.The stock solution of CT-DNA was prepared in 5 mM Tris-HCl/50 mM NaCl buffer at pH 7, which gave A260/A280nm ofca. 1.8–1.9, indicating that the DNA was sufficiently devoid of protein [36], and the concentration of DNA was determined from its absorption intensity at 260 nm (ε260 = 6600 M−1 cm−1) [37]. All the stock solutions were stored at 4°C and used within four days. The intrinsic binding constant (Kb) values of the complexes to CT-DNA were obtained by monitoring the change in the absorption intensity of the spectral bands with increasing concentration of DNA. After equilibrium had been reached, the spectra were recorded at 200–500 nm against an analogous solution of DNA as a reference. UV spectral data were fitted into Wolfe-Shimer equation (1) [38] to obtain the intrinsic binding association constant (Kb):(1)DNAεa-εb=DNAεb-εf+1Kbεb-εf,where [DNA] is the concentration of DNA in base pairs, εa is apparent extinction coefficient (Aobs/[MC]), εb is the extinction coefficient of the metal complex in the fully bound form, and the extinction coefficient for free metal complex [MC] is εf. The value of Kb was calculated as the ratio of the slope to intercept.Fluorimetric Studies.Ethidium bromide (EB) emits intense fluorescence light in the presence of DNA at λex 600 nm (546 nm) due to strong intercalation between adjacent DNA base pairs. The fluorescence emission intensity can be quenched when the second molecule was added to the CT-DNA bound EB solution. In the fluorescence quenching study, [DNA]/[EB]=1.13 is kept constant and varied with the concentration of the compounds. The fluorescence spectra of the reaction mixture were recorded between 500 and 850 nm at excitation wavelength 515 nm. The fluorescence quenching efficiency is evaluated according to the classical Stern-Volmer equation (2). The binding constant (Kb) and number of binding sites (n) can be determined from emission spectra with (3).(2)FoF=1+KsvQ(3)logFo-FF=log⁡Kb+nlog⁡Q.The fluorescence intensities in absence and presence of the quencher (complexes) are termed Fo and F as, respectively, “Q” is the concentration of the quencher and Ksv is the Stern-Volmer quenching constant.Viscosity Measurements.Viscosity experiments were carried out on an Ostwald microviscometer, immersed in a thermostat water bath maintained at a constant temperature at 26°C. Compounds were added to DNA solution (10 μmolL−1) with a micropipette. The concentration of the compounds was maintained in the range of 0–10 μML−1. Data were graphically presented as η/ηo1/3 versus the ratio of the concentration of compounds to DNA (r), where η was the viscosity of DNA in the presence of compound and ηo was the viscosity of DNA alone. The relative viscosity η was calculated using [39](4)η=t-toto,where to and t represent the flow time of buffer solution through the capillary and observed flow time for DNA in the absence and presence of the complex, respectively. The mean of three replicate measurements was used to evaluate the viscosity of the samples.


## 2.3.2. DNA Cleavage Assay

Agarose-gel electrophoresis monitored the ability of transition metal complexes to cleave plasmid DNA. The experiment was accomplished with supercoiled pUC18 (200 ng, 1μL) which was treated with varying concentrations of compounds (10–50 μM) in Tris-boric acid-buffer with NaCl (50 mM, pH 7.2) by agarose-gel electrophoresis method. The samples (5 μL in Tris-buffer) were incubated at 37°C for 45 min in water bath; to this solution, 1 μL loading buffer (0.25% bromophenol blue and 30% glycerol) was added. This mixture was loaded in the 1% agarose gel and electrophoresis was carried out at 60 V for an hour. The agarose gel was prestained with 0.5 μg/mL ethidium bromide (EtBr) and visualized under UV light and photographed for further analysis. The cleavage properties were determined based on the ability of compounds to convert the supercoiled form (Form I) into nicked (Form II) and linear form (Form III) [23].


## 2.3.3. Superoxide Dismutase (SOD) Assay

The superoxide dismutase activities of the synthesized metal complexes were assessed by colorimetric-based assay with xanthine/xanthine oxidase system as the source ofO2∙- due to their conducive solubility. The quantitative reduction of nitroblue tetrazolium (NBT) to monoformazan (MF+) by the O2∙- changes the color from yellow to blue which was followed spectrophotometrically at 560 nm. The suppression ratio was calculated using standard equation [Acontrol-Asample/Acontrol] × 100. In the SOD-like activity test, the metal complexes compete with NBT for oxidation of the generated superoxide ions. Plotting the results as the percentage of inhibiting NBT for comparative concentrations of complexes was determined by absorption changes. Tabulated results were derived from linear regression analysis and are given as the concentration (μM) equivalent to 1 unit of native Cu Zn-SOD activity (IC50 = 0.04 μM dm−3) [40]. A unit SOD activity is the concentration of the complex or enzyme which causes 50% inhibition in the reduction of NBT.


## 2.3.4. Molecular Docking

Crystal structure of DNA dodecamer (1BNA.pdb) with the sequence of d(CpGpCpGpApApTpTpCpGpCpG) and Cu, Zn-SOD (1CB4) was downloaded from the protein data bank (http://www.rcsb.org) and used for docking studies. Compounds were drawn using Maestro 2D sketcher and energy minimization was computed by OPLS 2005, while, for the preparation of the DNA or Cu, Zn-SOD, hydrogen was added to the polar atoms and the valency of the metal ions was optimized [41]. Meanwhile, the water molecules and the substrate were deleted. The DNA was minimized to some extent after hydrogen was added. Finally, a grid for DNA [with the dimension (10 Å × 10 Å × 10 Å)] and Cu, Zn-SOD [with the dimension (20 Å × 20 Å × 20 Å)] were prepared. The dimension of the grid was in such a manner that the grid covers the complete DNA. Using Extraprecision (XP) docking protocol, compounds were evaluated based on glide scoring which was docking into the receptor grid of radii as mentioned above [42].


## 2.3.5. Antimicrobial Activity

All the synthesized compounds were screenedin vitro for their antimicrobial activity against Gram -ve bacteria asEscherichia coli(MTCC 443) andPseudomonas aeruginosa(MTCC 2453) and Gram +ve bacterial strains asBacillus subtilis (MTCC 121) andStaphylococcus aureus(MTCC 3160), and fungal strains areCandida albicans(ATCC 10231) andAspergillus niger(ATCC 6275), and standard antibiotic ciprofloxacin (25 mg) and antifungal fluconazole (25 mg) served as the positive control. The impact was tested in terms of minimum inhibitory concentration (MIC) using a serial plate dilution assay [43]. Microbial cultures were incubated at 37°C for a day in case of bacteria and 72 h for fungi, respectively. 100 μL of Mueller-Hinton broth of bacteria was pipetted into each well; to this, a 10 μL suspension of the test pathogens was then added. 4% DMSO was used as a solvent for solution preparation and served as a negative control in order to monitor sample sterility and to determine any antimicrobial influence of the solvent. Inhibition zone was measured, and MIC was determined using double-fold serial dilution in liquid media containing varying concentrations of test compounds from 1 to 1000 μg/mL. Bacterial growth was measured by the turbidity of the culture after 18 h. Turbidity standard as McFarland Standard 0.5 solution was used. If particular concentration of compound inhibits bacterial growth, half the concentration of the compound was tested. This procedure was carried on to a concentration at which bacteria grow normally. The lowest concentration that inhibits the bacterial growth was determined as MIC value. Three replicates were maintained per test microbe. The resultant MIC values were determined as the mean of these replicate experiments.


## 3. Results and Discussion

### 3.1. Chemistry

A new potential N and O-bidentate imine-based ligand (L1) and its Co(III) and Cu(II) complexes were prepared by usual literature protocol, and a microanalysis checked the purity for C, H, O, and N. Cobalt(III) complexes were obtained by aerobic/chemical oxidation of mixtures of Co(II) salts and the ligand [44, 45]. Analytical data of all the complexes (C1–C4) are summarized above and the results obtained are reliable with those calculated for the proposed formulae. All the compounds were stable at atmospheric conditions, nonhygroscopic, and highly soluble in organic solvents such as DMF and DMSO. The molar conductivity of the complexes in DMSO (10−3 M) at 26°C is commensurate with their nonelectrolytic nature (13–18 Ω−1cm2 mol−1), but the cobalt(III) complex (C3) tends to be in an electrolytic environment with their ionic behavior at higher conductivity (38 Ω−1cm2 mol−1). However, the analytical, spectroscopic, and magnetic data do enable us to predict the possible structure of the synthesized complexes.


### 3.2. Spectral Characterization

#### 3.2.1. Vibrational Spectroscopy

IR spectra of the complexes were studied concerning the spectrum of the free ligand to characterize the binding mode of the imine-based ligand to the metal ion in complexes. The IR spectrum (FigureS1) of free ligand exhibits a sharp band at 1662 cm−1 due to azomethine group vibration. This band is shifted to longer wavelength (lower wavenumber) in the range 1650–1634 cm−1 of the complexes and confirms the coordination of the imine nitrogen to the metal ion. L1 has the characteristic band at 1562 cm−1 for C=N, thiazole ring. Spectra of complexes exhibited a new broad band in the range “3500–3400” cm−1 which may be attributed to stretching vibration υ(OH) of hydrated water, which is ensured by thermal analysis. The phenolic -OH stretching frequency at 1267 cm−1 found in the spectrum of the Schiff base was absent in the spectra of metal complexes and might be due to the coordination of the phenol oxygen atom involved in complexation as C-O-M at ~1224 cm−1 [46]. In the spectra of all the metal complexes, a very broadband at 3500 cm−1 is observed signifying the presence of coordinated/lattice held water. The bands due to M-O and M-N (coordination of azomethine nitrogen vibrational modes) appeared in the range of 565–490 and 470–435 cm−1, respectively [47].


#### 3.2.2. Electronic Spectra and Magnetic Moment

The electronic spectral measurements used to assign the possible geometry of the complexes are based on d-d transition peaks. Electronic spectra of the ligand and its metal complexes were measured in DMSO, and the numerical data are listed in TableS1. In Figure S2, a very strong band is below 400 nm for Schiff base (303 nm) and at 344 nm for complexes, due to ligand-centered π→π∗/n→π∗ (most probably from phenolate oxygen donor atom) transitions (LLCT). The absorption band observed at around 330–350 nm is attributed to ligand-centered charge transfer including n→π∗ transitions of phenanthroline. Besides a moderate broadband found at 385–410 nm with absorption maxima (λmax) at 406 nm (C1), 400–410 nm (C2), 385 nm (C3), and 405 nm (C4) were attributed to the metal ligand charge transfer (MLCT) transitions in complexes. The spectra further display a broadband in the region 460–580 nm with an absorption maximum at 520 nm which is due to several metal-centered d-d transitions which may be assigned to d-d transitions of a distorted octahedral copper(II) chromophore and it may be assigned to Eg2→T2g2 transition [48]. Lower energy band at λmax 502–550 nm is attributed to A1g1→T2g1 (ν1) ligand field transitions in an octahedral Co(III) complexes [49].The Cu(II) complexes exhibited a magnetic moment of 1.88–1.91 B.M which is higher than that of the spin-only value (1.73 BM) [50]. The strong and weak field complexes of some transition metal ions differ in the number of unpaired electrons in the complex, when this number can be ascertained readily from a comparison of the measured magnetic moment and that calculated from the spin paired and spin-free complexes. Determination of the number of unpaired electrons can also give information regarding the oxidation state of a metal ion in a complex. It is also useful in establishing a structure of many complexes [51]. Octahedral geometry around the Cu(II) ion is supported by the magnetic susceptibility value (1.83 BM).On the other hand, the magnetic moment was not found for the Co(III) complexes, which reveals low-spin d6 diamagnetic environment of the complexes [52]. Thus, magnetic moment values and spectral data support octahedral geometry for both the Cu(II) and Co(III) complexes.


#### 3.2.3. Thermogravimetric (DTA-TG) Studies

To give more insight into the thermal stability and compositional analysis of the metal complexes, the thermogravimetric analysis is carried out from ambient temperature to 700°C. Thermograms of complexes (C1–C4) are presented in Figure S3. The first phase corresponds to the loss of a lattice/coordinated water molecule at 82–120°C. The second step refers to the decomposition of a ligand molecule to an endothermic process that leads to the formation of a metal oxide above 560°C as a final product. Complexes (C2 and C4) containing phenanthroline showed decomposition at temperatures lower than that of the ligand. The percentage of metal oxide content was calculated from the weight of the ash obtained.Thermogravimetric details of the synthesized compounds are presented in TableS2. Generalized thermal degradation pattern of the complexes is represented as follows:(5)The preceding observations further support the composition of the complexes, which is compatible with the results obtained by other methods.


#### 3.2.4. EPR Spectra

X-band EPR spectra of copper complexes C1 and C2 exhibited axial patterns of four lines due to the hyperfine coupling of the unpaired electrons with the copper nucleus (63Cu, I=3/2). The g and A values were calculated from the spectra of the Cu(II) complexes (Figure 2). The trend g∥>g⊥ (Table S3) observed in these complexes indicates that the Cu(II) is in a distorted octahedral coordination environment, and the unpaired electron most likely resides predominantly in the dx2-y2 orbital (g∥>g⊥>2.0) of the Cu(II) ion and is the characteristic feature for the axial symmetry. The deviation of “g” values from the free electron value (2.0023) is by angular momentum contribution in the complexes. The average “g” value for overall distortion is calculated using the equation: gavg=(1/3)(2g⊥+g∥) [53].Figure 2
EPR spectrum of complexes C1 and C2.Molecular orbital coefficients in-planeσ-bonding (α2), in-plane π-bonding (β2), and out-of- plane π-bonding (γ2) are the covalency parameters for the metal to ligand bond which were evaluated using the following expressions:(6)α2=A∥0.036+g∥-2.0027+37g⊥-2.0023+0.04β2=g∥-2.0023E-8λα2γ2=g∥-2.0023E-2λα2,where λ = −829 cm−1 for the free copper ion and E is the electronic transition energy.The observed values ofα2 and β2 indicate that the complex has covalent bonding character. The smaller the β2, the larger the covalency of the bonding. Furthermore, it has appeared that the covalency of the out-of-plane is greater than of the in-plane π-bonding.The octahedral Co(III) complexes have diamagnetic ground state and the electronic configuration ist2g6 and the spin state is S=0; for this state, no EPR signal is obtained.


### 3.3. Combining Capacity of Metal Complexes with CT-DNA

#### 3.3.1. Electronic Absorption Spectral Features of DNA Binding

The binding behavior of double-stranded CT-DNA helix with Cu(II) and Co(III) complexes was studied using spectral absorption titration followed by the changes in the absorbance and shift in wavelength. The absorption intensity of the complexes was affected resulting in the tendency of hyperchromism (in the range of 224–270 nm) and no red shift (small shift ~2 nm for C2) and no sharp isosbestic points on the concomitant addition of DNA to the fixed concentration of complexes were observed. The absorption band was observed at λmax 266, 270, 224, and 268 nm for C1, C2, C3, and C4, respectively (Figure 3).Figure 3
Electronic absorption spectrum of complex C2 (20 μM) in the absence and presence of DNA in Tris/NaCl buffer (pH = 7.2). The arrows show the absorbance changes upon increasing concentration of DNA (0–25 μM) at RT. Inset: plot of [DNA]/(εa-εf) × 10−5 versus [DNA].The complex can be anticipated to engage bases in the grooves byπ-π interactions (through the planar, aromatic phen moiety) and, meanwhile, form hydrogen bonding and/or electrostatic interactions with the negatively charged phosphate backbone [54]. These spectroscopic changes assured that the complexes have greater binding propensity with DNA helices. Such surface contact was substantiated by quantitative calculations from (1) for their intrinsic binding constant (Kb) and the obtained values are 6.01 × 104, 8.16 × 105, 5.95 × 104, and 7.86 × 104 for complexes C1, C2, C3, and C4, respectively, which is comparable to a potential intercalator (for EB whose Kb have been found to be in the order of 106–107 M−1) [55, 56]. These results suggest an intimate association of the compounds with CT-DNA and it is also likely that compounds bind to the duplex helix via external contact (surface binding). The relative Kb value and pronounced hyperchromism of complexes C2 and C4 in comparison to C1 and C3, with respect to CT-DNA, were because the planar and larger surface area of the 1,10-phenanthroline ring appended in the complex causes enlargement of size of the DNA [57].


#### 3.3.2. Investigation on Quenching Mechanism

Fluorescence quenching propensity further examined the relative binding of compounds to CT-DNA due to high sensitivity and selectivity of this method. A significant decrease in fluorescence intensity of EB-DNA upon gradual addition of compounds atλem 626 nm was observed. Figure 4 confirms this trend. The fluorescence quenching of the EB-DNA solution could be due to relative complexes accepting excited state electron from EB. In addition, it was found that the interaction between complexes and double-stranded DNA in a groove binding mode causes a strong fluorescence quenching.Figure 4
Fluorescence quenching curves of EB-DNA in presence of complex (C2 and C4) at the concentration 0–35 μM at the interval of 5 in Tris-HCl/NaCl buffer (pH 7.2). The arrow indicates the effect of increasing the complex concentration on the fluorescence emission of ethidium bromide bound CT-DNA. The inset shows the linear fit of Fo/F versus [complex].
(a) (b)The Stern-Volmer quenching constant (Ksv) and Scatchard analysis were accomplished using corrected fluorescence data taking into account the effect of dilution. Deducing from the slope of the quenching plot of relative fluorescence intensity for CT-DNA as a function of the compounds of different concentrations (Figure 4 inset graph), DNA-binding tendency can be reflected in the relative order: Copper complexes (Ksv = C1 2.55 × 104, C2 3.83 × 105) > cobalt complexes (Ksv = C3 1.12 × 104, C4 3.61 × 104). This observation suggests that the complexes bind to DNA in a different degree which coincides with their solid structure where complex C2 has the largest plane coordinated to an ancillary phenanthroline ligand. Higher Ksv value of C2 complex suggests its stronger quenching ability than other complexes.The linear fitting plots oflog⁡[(F0-F)/F] versus log⁡[Q] (Figure 5) from (3) furnished the values of intrinsic binding constant (Kb) in the magnitude of 104–105, suggesting that the compounds bind strongly to DNA and the binding sites (n) were found to be 0.8–1.9±0.15. Comparable association of complexes to the DNA base with classical intercalator, EB (Kb = 107 M−1), assisted for the hypothesis of compounds to be minor groove binding which is almost similar to reported benzothiazole complexes [58]. The significant superior binding of C2 and C4 compared to other complexes is possibly owing to the 1,10-phenanthroline ring analogue as coligand in the respective complexes, which favours the interaction with the DNA through π-π∗ interaction and H-bonding [59].Figure 5
Plot oflog⁡[(F0-F)/F] versus log⁡Q for (a) DNA-C2 complex and (b) DNA-C3 complex at 298 K.
(a) (b)


#### 3.3.3. Viscosity Measurements

The most rigorous mean of testing the binding mode between DNA and compounds is viscometry technique in solution in the absence of crystallographic structural data. A classical intercalation probe demands that the DNA helix must be lengthened as base pairs are separated to accommodate the binding ligand, which leads to an increase in DNA viscosity [60]. EB, a well-known DNA intercalator, increases the relative viscosity strongly by lengthening the DNA double helix through intercalation, while DAPI, a popular groove binding agent under the same conditions, typically causes less pronounced (positive or negative) or no change in DNA solution which leads to quenching its effective length and concomitantly its viscosity [61, 62]. Herein, the relative thickness of compounds inapparently increases upon increasing concentration of compounds unlike the behavior of EB [2]. Interestingly, for C1 and C3 complexes there is an increase in specific viscosity of DNA, which is not as pronounced as the classical EB and the mixed ligand complexes. The degree of viscosity depends on the binding affinity to DNA which is calculated by (3) which follows the order EB > C2 > C4 > C1 > C3 > DAPI. The results suggest that the complexes could bind to DNA primarily groove binding nature which is consistent with preceding electronic and fluorescence spectroscopic results. The effects of relative viscosity of CT-DNA under the influence of increasing amounts of the complexes at 27±0.1°C are depicted in Figure 6.Figure 6
Effects of relative viscosity of CT-DNA under the influence of increasing amount of the complexes at27±0.1°C.


### 3.4. Chemical Nucleus Activity

Plasmid DNA strand scission was achieved by monitoring the gel electrophoresis for naturally occurring, covalently supercoiled conformation (Form I, SC) of pUC18 DNA transition to the open circular (Form II, OC) and linear conformation (Form III, LC). Different DNA nuclease capacity of complexes may occur due to different binding affinities of the complexes to DNA. The DNA cleaving abilities of all the compounds were investigated by reaction changes with supercoiled (SC) pUC18 DNA and the relative mobility of the products on agarose gel. At first, the concentration-dependent DNA cleavage by the complexes was performed on plasmid pUC18 DNA in Tris pH 7.1 buffer solutions in the absence of any reducing agents. The electrophoretic pattern of the DNA cleavage (Figure7) shows that the gradual cleavage observed by the complexes in the range of 10–50 μM. Meanwhile, the complex acts as chemical nucleases by cleaving the DNA Form I into Form II and the intensity of Form II increases as the compound concentration increases. Enhanced concentration of compound induces DNA cleavage more efficiently, which was monitored by the appearance of Form II with the disappearance of Form I.Figure 7
Gel electrophoresis assay for the cleavage of pUC18 plasmid DNA (200 ng) by C2 in 50 mM Tris-HCl/NaCl buffer (pH, 7.3) after 45 min incubation time at different concentration; Lane 1, DNA control; Lane 2, DNA + C2 (10 μM); Lane 3: DNA + C2 (20 μM); Lane 4: DNA + C2 (30 μM); Lane 5: DNA + C2 (40 μM); Lane 6: DNA + C2 (50 μM).Mechanistic Pathway of DNA Cleavage by Reactive Oxygen Species.Copper and cobalt complexes can cleave DNA through an oxidative or hydrolytic mechanism. In the process of oxidative DNA scission, it may lead to the formation of reactive species like hydroxyl radical (HO∙), superoxide anion radical (O2-∙), and/or singlet oxygen (1O2) which cause damage to the base or/and sugar of DNA. To establish the effect of reactive species on cleavage efficiency of pUC18 DNA induced by metal complexes, comparative DNA nicking ability of all the complexes was evaluated in the presence of H2O2, 3-mercaptopropionic acid (MPA), and ascorbic acid (Asc) (Figure 8, Lanes 2–4). DNA nuclease activity was significantly increased in presence of oxidative reagents which follows the order MPA > H2O2 > Asc. Thus, complexes with MPA showed effective cleavage activity, thus by producing SH radical leads complete degradation of Form I to Form II was noticed which suggests that these activators play a crucial role in assisting complexes in DNA cleavage.Figure 8
(a) Agarose-gel electrophoresis diagram showing cleavage of pBR322 supercoiled DNA (200 ng) by complex 2 in presence of activators and reactive oxygen species at 310 K after incubation for 45 min. Lane 1: DNA control; Lane 2: DNA + C2 + Asc (0.4 M); Lane 3: DNA + C2 + H2O2 (0.4 M); Lane 4: DNA + C2 + MPA (0.4 M); Lane 5: DNA + C2 + DMSO (0.4 M); Lane 6: DNA + C2 + EtOH (0.4 M); Lane 7: DNA + C2 + NaN3 (0.4 M); Lane 8: DNA + C2 + SOD (15 units); Lane 9: DNA + C2 + methyl green (2.5 μL of 0.01 mg/ml solution); Lane 10: DNA + C2 + DAPI (8 μM). (b) A graph of percentage cleavage of DNA determined using image analyzer.
(a) (b)Gel electrophoretic study was carried out with some standard diffusible radical scavengers such as hydroxyl radical scavengers DMSO, EtOH, singlet oxygen quencher-sodium azide, and superoxide radical scavenger as SOD which were used prior to the addition of complex to DNA solution under the aforesaid identical conditions. The addition of DMSO/EtOH to complex solution inhibited the DNA cleavage efficiency (Lanes 5 and 6) which is an indicative of the involvement of diffusible (HO.) hydroxyl radicals as one of the ROS accountable for DNA nicking, while the addition of SOD decreased the cleavage efficiencies (Lane 7) which revealed that superoxide radical was likely to be the cleaving agent. However, there was an enhancement of DNA cleavage in case of NaN3 (Lane 8) followed by the appearance of NC (Form II) which demonstrated the noninvolvement of sodium azide suggestive nonactivated oxygen intermediate in DNA scission process. The complexes C2 and C4 can convert SC into NC and LC efficiently compared to C1 and C3 which implies that the metal complexes induced intensively the plasmid DNA cleavage where SOD anion, as well as oxidative mechanistic pathways, can play a significant role in the cleavage pattern. The observed cleavage efficiency follows the order of complex 2 > 4 > 1 > 3, depending upon the coligand. It is also noticed that the hydrophobicity of mixed ligand complex (strong interaction of the extended aromatic rings of the phen moiety) induces efficient cleavage.DNA Cleavage in the Presence of Recognition Elements.The groove binding preference of the complexes was studied using DNA minor groove-binder 4′-6-diamidino-2-phenylindole (DAPI) and major groove-binder methyl green (MG). The supercoiled pUC18 DNA was treated with DAPI or methyl green before complexes addition.The electrophoresis results obtained with DAPI (Lane 10, Figure8) are followed by concomitant conversion of Form I to Form II/III in all the complexes. However, no apparent inhibition of DNA damage was observed in presence of major groove-binder MG (Lane 9, Figure 8). This further strengthens the hypothesis of minor groove preference for the complexes. These results are of significance as majority of the oxidative cleavage reagents usually bind in the minor groove mode [61].The complexes exhibit moderate cleavage activity in the following order: 2 > 4 > 1 > 3.


### 3.5. SOD Assay

One of the essential biological properties of metal complexes is radical scavenging activity. There is a linear relationship between DNA binding and antioxidant properties of the compounds. Radical scavenging activity of prepared compounds was determined indirectly by the nitroblue tetrazolium (NBT) assay. Generation of superoxide radicals is determined by the percentage of inhibition of the reduction of NBT (IC50). It has been revealed (Table S4) that the synthesized copper complexes exhibited quite a strong antioxidant activity in the range of 0.13–1.02 μmol dm−3 with reference to the standard used. The significant IC50 values are determined by UV-Vis spectroscopy. The scavenging effect of the Co(III) complexes may be ascribed to the chelating function of a ligand with the metal ion to achieve significantly selective effect of radical scavenging activity in biological system [63]. It has been proposed that only complexes with IC50 values below 20 μM may become clinically interesting [28]. Table S4 reveals the superoxide radical suppression efficacies of the complexes. It was observed that the radical scavenging activities of complexes increased with the increment of the complex concentrations.


### 3.6. Evaluation of Antimicrobial Activity

MIC data (Table1) display varying degrees of biocidal effects of L1 and its complexes on the growth of tested species. This study highly encourages that all the metal complexes have higher inhibitory effects than free ligand, and in particular mixed ligand complexes exhibited prominent antimicrobial activity, observed in the order of C2 > C4 > C1 > C3 > L1. All of these synthesized compounds showed MIC values in micromolar range (3.02–19.23 μg/mL). Out of these, C2 is the most bioactive (MIC 3.025 μg/mL) in the series and it was found to be more potent than the standard drug (MIC 3.12 μg/mL). The augmented toxicity of all the metal complexes could be explained on the light of Overtone’s concept [64] and Tweedy’s chelation theory [65]. As per these theories, the mode of action of the metal complexes may involve the formation of hydrogen bond formation through the azomethine group (HC=N-) with the active centers of cell constituents [66] resulting in interferences with the normal cell process. Structural activity relationship (SAR) study of the benzothiazole compounds shows that electron withdrawing groups (EWD) like fluorine exerts more potent antibacterial activity than electron donating groups (ER) is reported [67].Table 1
Antimicrobial activities of synthesized compounds.
Sl. number Compounds(30 µg/disk) MIC (zone of inhibition ± SD) inµg/mL E. coli P. aeruginosa B. subtilis S. aureus C. albicans A. niger ( 1 ) L1 11.0 (15 ± 0.6) 12.6 (17 ± 0.3) 12.3 (18 ± 0.9) 11.9 (17 ± 0.1) 19.6 (12 ± 0.2) 19.2 (16 ± 0.4) ( 2 ) C1 4.7 (22 ± 0.7) 4.8 (22 ± 0.9) 4.8 (23 ± 0.6) 4.6 (22 ± 0.7) 11.3 (20 ± 0.4) 11.5 (20 ± 0.6) ( 3 ) C2 3.02 (24 ± 0.4) 3.45 (24 ± 0.5) 3.31 (24 ± 0.4) 3.39 (21 ± 0.9) 8.84 (26 ± 0.2) 8.92 (26 ± 0.5) ( 4 ) C3 4.4 (22 ± 0.6) 4.6 (21 ± 0.6) 4.46 (24 ± 0.6) 3.91 (22 ± 0.6) 10.6 (23 ± 0.6) 9.37 (25 ± 0.6) ( 5 ) C4 3.73 (22 ± 0.8) 3.71 (23 ± 0.8) 3.13 (25 ± 0.1) 3.64 (26 ± 0.8) 9.16 (24 ± 0.5) 9.42 (24 ± 0.4) ( 6 ) Ciprofloxacin 3.12 (20 ± 0.6) 3.12 (20 ± 0.6) 3.0 (27 ± 0.6) 3.12 (19 ± 0.6) - - ( 7 ) Fluconazole - - - - 6.25 (16 ± 0.6) 6.31 (17 ± 0.6) Each value was replicated thrice.


### 3.7. Molecular Docking Studies

All the compounds were subjected to molecular docking with DNA and Cu, Zn-SOD using glide module of Schrödinger software to explore the binding of compounds with DNA. The virtual predicted top-ranking conformation with minimum energy glide score of compounds suggests best possible geometrical oriental binding with the target DNA double helix, which implies the highest binding affinity of DNA. The order of binding of compounds is as follows: L1 (−3.157), C2 (−3.564), C4 (−3.624), C1 (−4.288), and C3 (−4.195), whereas, with Cu, it is Zn-SOD C1 (−2.474), C2 (−1.478), C3 (−3.013), and C4 (−3.469). The other associated parameter calculated during docking studies is van der Waals interactions (kcal/mol) for DNA [L1 (−25.097), C2 (−21.049), C4 (−22.156), C1 (−27.888), and C3 (−28.739)] as well as Cu, Zn-SOD [C1 (−25.833), C2 (−12.897), C3 (−35.912), and C4 (−33.996)]. The determined 3D structure of C1 plays a significant role in exploring its structural consequences and conformational behavior during interactions with DNA [68]. C1 and C3 stacked with A-T-rich regions, whereas C2, C4, and L1 bind with G-C residues of groove wall of DNA by surface binding interactions (Figure 9). Geometrical oriental binding of L1 and C2 appears to be the same (Figure 9). Ligand L1 interacts with guanine and adenine through π-π interaction (Figure 10(a)). Complex C1 interacts with adenine via salt bridge and hydrogen bond (Figure 10(b)), whereas C2 interacts with adenine via salt bridge along with π-π interaction and hydrogen bond (Figure 10(c)); thus it shows maximum affinity with adenine. Thus, these confer the highest binding affinities of complexes C2 and C4 with DNA. Hence, these docked complexes, intra- and intermolecular hydrogen bond, and hydrophobic interactions (C2, C4, and L1) significantly participated in maintaining the stacked position of the complexes with DNA [68]. Therefore, it is suggested that there is a mutual complement between spectroscopic data and molecular docked model, which can be authenticated with spectroscopic results and it also provides the indication of groove mode.Figure 9
Binding mode of CT-DNA with compounds (L1, C1, and C2). DNA is represented in ribbon structure wherein the nucleoside is colored as yellow-guanine, maroon-thymine, blue-cytosine, and light green as adenine. Compounds are represented and highlighted in the figure.Figure 10
Two-dimensional views of docked complexes.
(a) (b) (c)Docked structures of DNA with L1(Figure 10(a)), C1(Figure 10(b)), and C2(Figure 10(c)) showing the molecular interactions like inter- and intrahydrogen bonds, π-π stacking, and salt bridges.Binding of compound at Cu Zn domain of SOD results in an increase in an antioxidant activity of SOD and decrease in oxidative stress [69]. All the compounds were found near active site of Cu, Zn-SOD (Figure 11), and C4 interacted with Tyr108 via π-π stacking, whereas C1 formed hydrogen bond with Ser109, C2 with Arg113, and C3 interacted with Glu107 via salt bridge. Hence, the data suggest that these compounds have potent binding with Arg113 and Glu107 which are resided near active site of Cu, Zn-SOD, thereby regulating the generation of free radicals.Figure 11
Active center forO2∙- scavenging of metal complexes.


## 3.1. Chemistry

A new potential N and O-bidentate imine-based ligand (L1) and its Co(III) and Cu(II) complexes were prepared by usual literature protocol, and a microanalysis checked the purity for C, H, O, and N. Cobalt(III) complexes were obtained by aerobic/chemical oxidation of mixtures of Co(II) salts and the ligand [44, 45]. Analytical data of all the complexes (C1–C4) are summarized above and the results obtained are reliable with those calculated for the proposed formulae. All the compounds were stable at atmospheric conditions, nonhygroscopic, and highly soluble in organic solvents such as DMF and DMSO. The molar conductivity of the complexes in DMSO (10−3 M) at 26°C is commensurate with their nonelectrolytic nature (13–18 Ω−1cm2 mol−1), but the cobalt(III) complex (C3) tends to be in an electrolytic environment with their ionic behavior at higher conductivity (38 Ω−1cm2 mol−1). However, the analytical, spectroscopic, and magnetic data do enable us to predict the possible structure of the synthesized complexes.


## 3.2. Spectral Characterization

### 3.2.1. Vibrational Spectroscopy

IR spectra of the complexes were studied concerning the spectrum of the free ligand to characterize the binding mode of the imine-based ligand to the metal ion in complexes. The IR spectrum (FigureS1) of free ligand exhibits a sharp band at 1662 cm−1 due to azomethine group vibration. This band is shifted to longer wavelength (lower wavenumber) in the range 1650–1634 cm−1 of the complexes and confirms the coordination of the imine nitrogen to the metal ion. L1 has the characteristic band at 1562 cm−1 for C=N, thiazole ring. Spectra of complexes exhibited a new broad band in the range “3500–3400” cm−1 which may be attributed to stretching vibration υ(OH) of hydrated water, which is ensured by thermal analysis. The phenolic -OH stretching frequency at 1267 cm−1 found in the spectrum of the Schiff base was absent in the spectra of metal complexes and might be due to the coordination of the phenol oxygen atom involved in complexation as C-O-M at ~1224 cm−1 [46]. In the spectra of all the metal complexes, a very broadband at 3500 cm−1 is observed signifying the presence of coordinated/lattice held water. The bands due to M-O and M-N (coordination of azomethine nitrogen vibrational modes) appeared in the range of 565–490 and 470–435 cm−1, respectively [47].


### 3.2.2. Electronic Spectra and Magnetic Moment

The electronic spectral measurements used to assign the possible geometry of the complexes are based on d-d transition peaks. Electronic spectra of the ligand and its metal complexes were measured in DMSO, and the numerical data are listed in TableS1. In Figure S2, a very strong band is below 400 nm for Schiff base (303 nm) and at 344 nm for complexes, due to ligand-centered π→π∗/n→π∗ (most probably from phenolate oxygen donor atom) transitions (LLCT). The absorption band observed at around 330–350 nm is attributed to ligand-centered charge transfer including n→π∗ transitions of phenanthroline. Besides a moderate broadband found at 385–410 nm with absorption maxima (λmax) at 406 nm (C1), 400–410 nm (C2), 385 nm (C3), and 405 nm (C4) were attributed to the metal ligand charge transfer (MLCT) transitions in complexes. The spectra further display a broadband in the region 460–580 nm with an absorption maximum at 520 nm which is due to several metal-centered d-d transitions which may be assigned to d-d transitions of a distorted octahedral copper(II) chromophore and it may be assigned to Eg2→T2g2 transition [48]. Lower energy band at λmax 502–550 nm is attributed to A1g1→T2g1 (ν1) ligand field transitions in an octahedral Co(III) complexes [49].The Cu(II) complexes exhibited a magnetic moment of 1.88–1.91 B.M which is higher than that of the spin-only value (1.73 BM) [50]. The strong and weak field complexes of some transition metal ions differ in the number of unpaired electrons in the complex, when this number can be ascertained readily from a comparison of the measured magnetic moment and that calculated from the spin paired and spin-free complexes. Determination of the number of unpaired electrons can also give information regarding the oxidation state of a metal ion in a complex. It is also useful in establishing a structure of many complexes [51]. Octahedral geometry around the Cu(II) ion is supported by the magnetic susceptibility value (1.83 BM).On the other hand, the magnetic moment was not found for the Co(III) complexes, which reveals low-spin d6 diamagnetic environment of the complexes [52]. Thus, magnetic moment values and spectral data support octahedral geometry for both the Cu(II) and Co(III) complexes.


### 3.2.3. Thermogravimetric (DTA-TG) Studies

To give more insight into the thermal stability and compositional analysis of the metal complexes, the thermogravimetric analysis is carried out from ambient temperature to 700°C. Thermograms of complexes (C1–C4) are presented in Figure S3. The first phase corresponds to the loss of a lattice/coordinated water molecule at 82–120°C. The second step refers to the decomposition of a ligand molecule to an endothermic process that leads to the formation of a metal oxide above 560°C as a final product. Complexes (C2 and C4) containing phenanthroline showed decomposition at temperatures lower than that of the ligand. The percentage of metal oxide content was calculated from the weight of the ash obtained.Thermogravimetric details of the synthesized compounds are presented in TableS2. Generalized thermal degradation pattern of the complexes is represented as follows:(5)The preceding observations further support the composition of the complexes, which is compatible with the results obtained by other methods.


### 3.2.4. EPR Spectra

X-band EPR spectra of copper complexes C1 and C2 exhibited axial patterns of four lines due to the hyperfine coupling of the unpaired electrons with the copper nucleus (63Cu, I=3/2). The g and A values were calculated from the spectra of the Cu(II) complexes (Figure 2). The trend g∥>g⊥ (Table S3) observed in these complexes indicates that the Cu(II) is in a distorted octahedral coordination environment, and the unpaired electron most likely resides predominantly in the dx2-y2 orbital (g∥>g⊥>2.0) of the Cu(II) ion and is the characteristic feature for the axial symmetry. The deviation of “g” values from the free electron value (2.0023) is by angular momentum contribution in the complexes. The average “g” value for overall distortion is calculated using the equation: gavg=(1/3)(2g⊥+g∥) [53].Figure 2
EPR spectrum of complexes C1 and C2.Molecular orbital coefficients in-planeσ-bonding (α2), in-plane π-bonding (β2), and out-of- plane π-bonding (γ2) are the covalency parameters for the metal to ligand bond which were evaluated using the following expressions:(6)α2=A∥0.036+g∥-2.0027+37g⊥-2.0023+0.04β2=g∥-2.0023E-8λα2γ2=g∥-2.0023E-2λα2,where λ = −829 cm−1 for the free copper ion and E is the electronic transition energy.The observed values ofα2 and β2 indicate that the complex has covalent bonding character. The smaller the β2, the larger the covalency of the bonding. Furthermore, it has appeared that the covalency of the out-of-plane is greater than of the in-plane π-bonding.The octahedral Co(III) complexes have diamagnetic ground state and the electronic configuration ist2g6 and the spin state is S=0; for this state, no EPR signal is obtained.


## 3.2.1. Vibrational Spectroscopy

IR spectra of the complexes were studied concerning the spectrum of the free ligand to characterize the binding mode of the imine-based ligand to the metal ion in complexes. The IR spectrum (FigureS1) of free ligand exhibits a sharp band at 1662 cm−1 due to azomethine group vibration. This band is shifted to longer wavelength (lower wavenumber) in the range 1650–1634 cm−1 of the complexes and confirms the coordination of the imine nitrogen to the metal ion. L1 has the characteristic band at 1562 cm−1 for C=N, thiazole ring. Spectra of complexes exhibited a new broad band in the range “3500–3400” cm−1 which may be attributed to stretching vibration υ(OH) of hydrated water, which is ensured by thermal analysis. The phenolic -OH stretching frequency at 1267 cm−1 found in the spectrum of the Schiff base was absent in the spectra of metal complexes and might be due to the coordination of the phenol oxygen atom involved in complexation as C-O-M at ~1224 cm−1 [46]. In the spectra of all the metal complexes, a very broadband at 3500 cm−1 is observed signifying the presence of coordinated/lattice held water. The bands due to M-O and M-N (coordination of azomethine nitrogen vibrational modes) appeared in the range of 565–490 and 470–435 cm−1, respectively [47].


## 3.2.2. Electronic Spectra and Magnetic Moment

The electronic spectral measurements used to assign the possible geometry of the complexes are based on d-d transition peaks. Electronic spectra of the ligand and its metal complexes were measured in DMSO, and the numerical data are listed in TableS1. In Figure S2, a very strong band is below 400 nm for Schiff base (303 nm) and at 344 nm for complexes, due to ligand-centered π→π∗/n→π∗ (most probably from phenolate oxygen donor atom) transitions (LLCT). The absorption band observed at around 330–350 nm is attributed to ligand-centered charge transfer including n→π∗ transitions of phenanthroline. Besides a moderate broadband found at 385–410 nm with absorption maxima (λmax) at 406 nm (C1), 400–410 nm (C2), 385 nm (C3), and 405 nm (C4) were attributed to the metal ligand charge transfer (MLCT) transitions in complexes. The spectra further display a broadband in the region 460–580 nm with an absorption maximum at 520 nm which is due to several metal-centered d-d transitions which may be assigned to d-d transitions of a distorted octahedral copper(II) chromophore and it may be assigned to Eg2→T2g2 transition [48]. Lower energy band at λmax 502–550 nm is attributed to A1g1→T2g1 (ν1) ligand field transitions in an octahedral Co(III) complexes [49].The Cu(II) complexes exhibited a magnetic moment of 1.88–1.91 B.M which is higher than that of the spin-only value (1.73 BM) [50]. The strong and weak field complexes of some transition metal ions differ in the number of unpaired electrons in the complex, when this number can be ascertained readily from a comparison of the measured magnetic moment and that calculated from the spin paired and spin-free complexes. Determination of the number of unpaired electrons can also give information regarding the oxidation state of a metal ion in a complex. It is also useful in establishing a structure of many complexes [51]. Octahedral geometry around the Cu(II) ion is supported by the magnetic susceptibility value (1.83 BM).On the other hand, the magnetic moment was not found for the Co(III) complexes, which reveals low-spin d6 diamagnetic environment of the complexes [52]. Thus, magnetic moment values and spectral data support octahedral geometry for both the Cu(II) and Co(III) complexes.


## 3.2.3. Thermogravimetric (DTA-TG) Studies

To give more insight into the thermal stability and compositional analysis of the metal complexes, the thermogravimetric analysis is carried out from ambient temperature to 700°C. Thermograms of complexes (C1–C4) are presented in Figure S3. The first phase corresponds to the loss of a lattice/coordinated water molecule at 82–120°C. The second step refers to the decomposition of a ligand molecule to an endothermic process that leads to the formation of a metal oxide above 560°C as a final product. Complexes (C2 and C4) containing phenanthroline showed decomposition at temperatures lower than that of the ligand. The percentage of metal oxide content was calculated from the weight of the ash obtained.Thermogravimetric details of the synthesized compounds are presented in TableS2. Generalized thermal degradation pattern of the complexes is represented as follows:(5)The preceding observations further support the composition of the complexes, which is compatible with the results obtained by other methods.


## 3.2.4. EPR Spectra

X-band EPR spectra of copper complexes C1 and C2 exhibited axial patterns of four lines due to the hyperfine coupling of the unpaired electrons with the copper nucleus (63Cu, I=3/2). The g and A values were calculated from the spectra of the Cu(II) complexes (Figure 2). The trend g∥>g⊥ (Table S3) observed in these complexes indicates that the Cu(II) is in a distorted octahedral coordination environment, and the unpaired electron most likely resides predominantly in the dx2-y2 orbital (g∥>g⊥>2.0) of the Cu(II) ion and is the characteristic feature for the axial symmetry. The deviation of “g” values from the free electron value (2.0023) is by angular momentum contribution in the complexes. The average “g” value for overall distortion is calculated using the equation: gavg=(1/3)(2g⊥+g∥) [53].Figure 2
EPR spectrum of complexes C1 and C2.Molecular orbital coefficients in-planeσ-bonding (α2), in-plane π-bonding (β2), and out-of- plane π-bonding (γ2) are the covalency parameters for the metal to ligand bond which were evaluated using the following expressions:(6)α2=A∥0.036+g∥-2.0027+37g⊥-2.0023+0.04β2=g∥-2.0023E-8λα2γ2=g∥-2.0023E-2λα2,where λ = −829 cm−1 for the free copper ion and E is the electronic transition energy.The observed values ofα2 and β2 indicate that the complex has covalent bonding character. The smaller the β2, the larger the covalency of the bonding. Furthermore, it has appeared that the covalency of the out-of-plane is greater than of the in-plane π-bonding.The octahedral Co(III) complexes have diamagnetic ground state and the electronic configuration ist2g6 and the spin state is S=0; for this state, no EPR signal is obtained.


## 3.3. Combining Capacity of Metal Complexes with CT-DNA

### 3.3.1. Electronic Absorption Spectral Features of DNA Binding

The binding behavior of double-stranded CT-DNA helix with Cu(II) and Co(III) complexes was studied using spectral absorption titration followed by the changes in the absorbance and shift in wavelength. The absorption intensity of the complexes was affected resulting in the tendency of hyperchromism (in the range of 224–270 nm) and no red shift (small shift ~2 nm for C2) and no sharp isosbestic points on the concomitant addition of DNA to the fixed concentration of complexes were observed. The absorption band was observed at λmax 266, 270, 224, and 268 nm for C1, C2, C3, and C4, respectively (Figure 3).Figure 3
Electronic absorption spectrum of complex C2 (20 μM) in the absence and presence of DNA in Tris/NaCl buffer (pH = 7.2). The arrows show the absorbance changes upon increasing concentration of DNA (0–25 μM) at RT. Inset: plot of [DNA]/(εa-εf) × 10−5 versus [DNA].The complex can be anticipated to engage bases in the grooves byπ-π interactions (through the planar, aromatic phen moiety) and, meanwhile, form hydrogen bonding and/or electrostatic interactions with the negatively charged phosphate backbone [54]. These spectroscopic changes assured that the complexes have greater binding propensity with DNA helices. Such surface contact was substantiated by quantitative calculations from (1) for their intrinsic binding constant (Kb) and the obtained values are 6.01 × 104, 8.16 × 105, 5.95 × 104, and 7.86 × 104 for complexes C1, C2, C3, and C4, respectively, which is comparable to a potential intercalator (for EB whose Kb have been found to be in the order of 106–107 M−1) [55, 56]. These results suggest an intimate association of the compounds with CT-DNA and it is also likely that compounds bind to the duplex helix via external contact (surface binding). The relative Kb value and pronounced hyperchromism of complexes C2 and C4 in comparison to C1 and C3, with respect to CT-DNA, were because the planar and larger surface area of the 1,10-phenanthroline ring appended in the complex causes enlargement of size of the DNA [57].


### 3.3.2. Investigation on Quenching Mechanism

Fluorescence quenching propensity further examined the relative binding of compounds to CT-DNA due to high sensitivity and selectivity of this method. A significant decrease in fluorescence intensity of EB-DNA upon gradual addition of compounds atλem 626 nm was observed. Figure 4 confirms this trend. The fluorescence quenching of the EB-DNA solution could be due to relative complexes accepting excited state electron from EB. In addition, it was found that the interaction between complexes and double-stranded DNA in a groove binding mode causes a strong fluorescence quenching.Figure 4
Fluorescence quenching curves of EB-DNA in presence of complex (C2 and C4) at the concentration 0–35 μM at the interval of 5 in Tris-HCl/NaCl buffer (pH 7.2). The arrow indicates the effect of increasing the complex concentration on the fluorescence emission of ethidium bromide bound CT-DNA. The inset shows the linear fit of Fo/F versus [complex].
(a) (b)The Stern-Volmer quenching constant (Ksv) and Scatchard analysis were accomplished using corrected fluorescence data taking into account the effect of dilution. Deducing from the slope of the quenching plot of relative fluorescence intensity for CT-DNA as a function of the compounds of different concentrations (Figure 4 inset graph), DNA-binding tendency can be reflected in the relative order: Copper complexes (Ksv = C1 2.55 × 104, C2 3.83 × 105) > cobalt complexes (Ksv = C3 1.12 × 104, C4 3.61 × 104). This observation suggests that the complexes bind to DNA in a different degree which coincides with their solid structure where complex C2 has the largest plane coordinated to an ancillary phenanthroline ligand. Higher Ksv value of C2 complex suggests its stronger quenching ability than other complexes.The linear fitting plots oflog⁡[(F0-F)/F] versus log⁡[Q] (Figure 5) from (3) furnished the values of intrinsic binding constant (Kb) in the magnitude of 104–105, suggesting that the compounds bind strongly to DNA and the binding sites (n) were found to be 0.8–1.9±0.15. Comparable association of complexes to the DNA base with classical intercalator, EB (Kb = 107 M−1), assisted for the hypothesis of compounds to be minor groove binding which is almost similar to reported benzothiazole complexes [58]. The significant superior binding of C2 and C4 compared to other complexes is possibly owing to the 1,10-phenanthroline ring analogue as coligand in the respective complexes, which favours the interaction with the DNA through π-π∗ interaction and H-bonding [59].Figure 5
Plot oflog⁡[(F0-F)/F] versus log⁡Q for (a) DNA-C2 complex and (b) DNA-C3 complex at 298 K.
(a) (b)


### 3.3.3. Viscosity Measurements

The most rigorous mean of testing the binding mode between DNA and compounds is viscometry technique in solution in the absence of crystallographic structural data. A classical intercalation probe demands that the DNA helix must be lengthened as base pairs are separated to accommodate the binding ligand, which leads to an increase in DNA viscosity [60]. EB, a well-known DNA intercalator, increases the relative viscosity strongly by lengthening the DNA double helix through intercalation, while DAPI, a popular groove binding agent under the same conditions, typically causes less pronounced (positive or negative) or no change in DNA solution which leads to quenching its effective length and concomitantly its viscosity [61, 62]. Herein, the relative thickness of compounds inapparently increases upon increasing concentration of compounds unlike the behavior of EB [2]. Interestingly, for C1 and C3 complexes there is an increase in specific viscosity of DNA, which is not as pronounced as the classical EB and the mixed ligand complexes. The degree of viscosity depends on the binding affinity to DNA which is calculated by (3) which follows the order EB > C2 > C4 > C1 > C3 > DAPI. The results suggest that the complexes could bind to DNA primarily groove binding nature which is consistent with preceding electronic and fluorescence spectroscopic results. The effects of relative viscosity of CT-DNA under the influence of increasing amounts of the complexes at 27±0.1°C are depicted in Figure 6.Figure 6
Effects of relative viscosity of CT-DNA under the influence of increasing amount of the complexes at27±0.1°C.


## 3.3.1. Electronic Absorption Spectral Features of DNA Binding

The binding behavior of double-stranded CT-DNA helix with Cu(II) and Co(III) complexes was studied using spectral absorption titration followed by the changes in the absorbance and shift in wavelength. The absorption intensity of the complexes was affected resulting in the tendency of hyperchromism (in the range of 224–270 nm) and no red shift (small shift ~2 nm for C2) and no sharp isosbestic points on the concomitant addition of DNA to the fixed concentration of complexes were observed. The absorption band was observed at λmax 266, 270, 224, and 268 nm for C1, C2, C3, and C4, respectively (Figure 3).Figure 3
Electronic absorption spectrum of complex C2 (20 μM) in the absence and presence of DNA in Tris/NaCl buffer (pH = 7.2). The arrows show the absorbance changes upon increasing concentration of DNA (0–25 μM) at RT. Inset: plot of [DNA]/(εa-εf) × 10−5 versus [DNA].The complex can be anticipated to engage bases in the grooves byπ-π interactions (through the planar, aromatic phen moiety) and, meanwhile, form hydrogen bonding and/or electrostatic interactions with the negatively charged phosphate backbone [54]. These spectroscopic changes assured that the complexes have greater binding propensity with DNA helices. Such surface contact was substantiated by quantitative calculations from (1) for their intrinsic binding constant (Kb) and the obtained values are 6.01 × 104, 8.16 × 105, 5.95 × 104, and 7.86 × 104 for complexes C1, C2, C3, and C4, respectively, which is comparable to a potential intercalator (for EB whose Kb have been found to be in the order of 106–107 M−1) [55, 56]. These results suggest an intimate association of the compounds with CT-DNA and it is also likely that compounds bind to the duplex helix via external contact (surface binding). The relative Kb value and pronounced hyperchromism of complexes C2 and C4 in comparison to C1 and C3, with respect to CT-DNA, were because the planar and larger surface area of the 1,10-phenanthroline ring appended in the complex causes enlargement of size of the DNA [57].


## 3.3.2. Investigation on Quenching Mechanism

Fluorescence quenching propensity further examined the relative binding of compounds to CT-DNA due to high sensitivity and selectivity of this method. A significant decrease in fluorescence intensity of EB-DNA upon gradual addition of compounds atλem 626 nm was observed. Figure 4 confirms this trend. The fluorescence quenching of the EB-DNA solution could be due to relative complexes accepting excited state electron from EB. In addition, it was found that the interaction between complexes and double-stranded DNA in a groove binding mode causes a strong fluorescence quenching.Figure 4
Fluorescence quenching curves of EB-DNA in presence of complex (C2 and C4) at the concentration 0–35 μM at the interval of 5 in Tris-HCl/NaCl buffer (pH 7.2). The arrow indicates the effect of increasing the complex concentration on the fluorescence emission of ethidium bromide bound CT-DNA. The inset shows the linear fit of Fo/F versus [complex].
(a) (b)The Stern-Volmer quenching constant (Ksv) and Scatchard analysis were accomplished using corrected fluorescence data taking into account the effect of dilution. Deducing from the slope of the quenching plot of relative fluorescence intensity for CT-DNA as a function of the compounds of different concentrations (Figure 4 inset graph), DNA-binding tendency can be reflected in the relative order: Copper complexes (Ksv = C1 2.55 × 104, C2 3.83 × 105) > cobalt complexes (Ksv = C3 1.12 × 104, C4 3.61 × 104). This observation suggests that the complexes bind to DNA in a different degree which coincides with their solid structure where complex C2 has the largest plane coordinated to an ancillary phenanthroline ligand. Higher Ksv value of C2 complex suggests its stronger quenching ability than other complexes.The linear fitting plots oflog⁡[(F0-F)/F] versus log⁡[Q] (Figure 5) from (3) furnished the values of intrinsic binding constant (Kb) in the magnitude of 104–105, suggesting that the compounds bind strongly to DNA and the binding sites (n) were found to be 0.8–1.9±0.15. Comparable association of complexes to the DNA base with classical intercalator, EB (Kb = 107 M−1), assisted for the hypothesis of compounds to be minor groove binding which is almost similar to reported benzothiazole complexes [58]. The significant superior binding of C2 and C4 compared to other complexes is possibly owing to the 1,10-phenanthroline ring analogue as coligand in the respective complexes, which favours the interaction with the DNA through π-π∗ interaction and H-bonding [59].Figure 5
Plot oflog⁡[(F0-F)/F] versus log⁡Q for (a) DNA-C2 complex and (b) DNA-C3 complex at 298 K.
(a) (b)


## 3.3.3. Viscosity Measurements

The most rigorous mean of testing the binding mode between DNA and compounds is viscometry technique in solution in the absence of crystallographic structural data. A classical intercalation probe demands that the DNA helix must be lengthened as base pairs are separated to accommodate the binding ligand, which leads to an increase in DNA viscosity [60]. EB, a well-known DNA intercalator, increases the relative viscosity strongly by lengthening the DNA double helix through intercalation, while DAPI, a popular groove binding agent under the same conditions, typically causes less pronounced (positive or negative) or no change in DNA solution which leads to quenching its effective length and concomitantly its viscosity [61, 62]. Herein, the relative thickness of compounds inapparently increases upon increasing concentration of compounds unlike the behavior of EB [2]. Interestingly, for C1 and C3 complexes there is an increase in specific viscosity of DNA, which is not as pronounced as the classical EB and the mixed ligand complexes. The degree of viscosity depends on the binding affinity to DNA which is calculated by (3) which follows the order EB > C2 > C4 > C1 > C3 > DAPI. The results suggest that the complexes could bind to DNA primarily groove binding nature which is consistent with preceding electronic and fluorescence spectroscopic results. The effects of relative viscosity of CT-DNA under the influence of increasing amounts of the complexes at 27±0.1°C are depicted in Figure 6.Figure 6
Effects of relative viscosity of CT-DNA under the influence of increasing amount of the complexes at27±0.1°C.


## 3.4. Chemical Nucleus Activity

Plasmid DNA strand scission was achieved by monitoring the gel electrophoresis for naturally occurring, covalently supercoiled conformation (Form I, SC) of pUC18 DNA transition to the open circular (Form II, OC) and linear conformation (Form III, LC). Different DNA nuclease capacity of complexes may occur due to different binding affinities of the complexes to DNA. The DNA cleaving abilities of all the compounds were investigated by reaction changes with supercoiled (SC) pUC18 DNA and the relative mobility of the products on agarose gel. At first, the concentration-dependent DNA cleavage by the complexes was performed on plasmid pUC18 DNA in Tris pH 7.1 buffer solutions in the absence of any reducing agents. The electrophoretic pattern of the DNA cleavage (Figure7) shows that the gradual cleavage observed by the complexes in the range of 10–50 μM. Meanwhile, the complex acts as chemical nucleases by cleaving the DNA Form I into Form II and the intensity of Form II increases as the compound concentration increases. Enhanced concentration of compound induces DNA cleavage more efficiently, which was monitored by the appearance of Form II with the disappearance of Form I.Figure 7
Gel electrophoresis assay for the cleavage of pUC18 plasmid DNA (200 ng) by C2 in 50 mM Tris-HCl/NaCl buffer (pH, 7.3) after 45 min incubation time at different concentration; Lane 1, DNA control; Lane 2, DNA + C2 (10 μM); Lane 3: DNA + C2 (20 μM); Lane 4: DNA + C2 (30 μM); Lane 5: DNA + C2 (40 μM); Lane 6: DNA + C2 (50 μM).Mechanistic Pathway of DNA Cleavage by Reactive Oxygen Species.Copper and cobalt complexes can cleave DNA through an oxidative or hydrolytic mechanism. In the process of oxidative DNA scission, it may lead to the formation of reactive species like hydroxyl radical (HO∙), superoxide anion radical (O2-∙), and/or singlet oxygen (1O2) which cause damage to the base or/and sugar of DNA. To establish the effect of reactive species on cleavage efficiency of pUC18 DNA induced by metal complexes, comparative DNA nicking ability of all the complexes was evaluated in the presence of H2O2, 3-mercaptopropionic acid (MPA), and ascorbic acid (Asc) (Figure 8, Lanes 2–4). DNA nuclease activity was significantly increased in presence of oxidative reagents which follows the order MPA > H2O2 > Asc. Thus, complexes with MPA showed effective cleavage activity, thus by producing SH radical leads complete degradation of Form I to Form II was noticed which suggests that these activators play a crucial role in assisting complexes in DNA cleavage.Figure 8
(a) Agarose-gel electrophoresis diagram showing cleavage of pBR322 supercoiled DNA (200 ng) by complex 2 in presence of activators and reactive oxygen species at 310 K after incubation for 45 min. Lane 1: DNA control; Lane 2: DNA + C2 + Asc (0.4 M); Lane 3: DNA + C2 + H2O2 (0.4 M); Lane 4: DNA + C2 + MPA (0.4 M); Lane 5: DNA + C2 + DMSO (0.4 M); Lane 6: DNA + C2 + EtOH (0.4 M); Lane 7: DNA + C2 + NaN3 (0.4 M); Lane 8: DNA + C2 + SOD (15 units); Lane 9: DNA + C2 + methyl green (2.5 μL of 0.01 mg/ml solution); Lane 10: DNA + C2 + DAPI (8 μM). (b) A graph of percentage cleavage of DNA determined using image analyzer.
(a) (b)Gel electrophoretic study was carried out with some standard diffusible radical scavengers such as hydroxyl radical scavengers DMSO, EtOH, singlet oxygen quencher-sodium azide, and superoxide radical scavenger as SOD which were used prior to the addition of complex to DNA solution under the aforesaid identical conditions. The addition of DMSO/EtOH to complex solution inhibited the DNA cleavage efficiency (Lanes 5 and 6) which is an indicative of the involvement of diffusible (HO.) hydroxyl radicals as one of the ROS accountable for DNA nicking, while the addition of SOD decreased the cleavage efficiencies (Lane 7) which revealed that superoxide radical was likely to be the cleaving agent. However, there was an enhancement of DNA cleavage in case of NaN3 (Lane 8) followed by the appearance of NC (Form II) which demonstrated the noninvolvement of sodium azide suggestive nonactivated oxygen intermediate in DNA scission process. The complexes C2 and C4 can convert SC into NC and LC efficiently compared to C1 and C3 which implies that the metal complexes induced intensively the plasmid DNA cleavage where SOD anion, as well as oxidative mechanistic pathways, can play a significant role in the cleavage pattern. The observed cleavage efficiency follows the order of complex 2 > 4 > 1 > 3, depending upon the coligand. It is also noticed that the hydrophobicity of mixed ligand complex (strong interaction of the extended aromatic rings of the phen moiety) induces efficient cleavage.DNA Cleavage in the Presence of Recognition Elements.The groove binding preference of the complexes was studied using DNA minor groove-binder 4′-6-diamidino-2-phenylindole (DAPI) and major groove-binder methyl green (MG). The supercoiled pUC18 DNA was treated with DAPI or methyl green before complexes addition.The electrophoresis results obtained with DAPI (Lane 10, Figure8) are followed by concomitant conversion of Form I to Form II/III in all the complexes. However, no apparent inhibition of DNA damage was observed in presence of major groove-binder MG (Lane 9, Figure 8). This further strengthens the hypothesis of minor groove preference for the complexes. These results are of significance as majority of the oxidative cleavage reagents usually bind in the minor groove mode [61].The complexes exhibit moderate cleavage activity in the following order: 2 > 4 > 1 > 3.


## 3.5. SOD Assay

One of the essential biological properties of metal complexes is radical scavenging activity. There is a linear relationship between DNA binding and antioxidant properties of the compounds. Radical scavenging activity of prepared compounds was determined indirectly by the nitroblue tetrazolium (NBT) assay. Generation of superoxide radicals is determined by the percentage of inhibition of the reduction of NBT (IC50). It has been revealed (Table S4) that the synthesized copper complexes exhibited quite a strong antioxidant activity in the range of 0.13–1.02 μmol dm−3 with reference to the standard used. The significant IC50 values are determined by UV-Vis spectroscopy. The scavenging effect of the Co(III) complexes may be ascribed to the chelating function of a ligand with the metal ion to achieve significantly selective effect of radical scavenging activity in biological system [63]. It has been proposed that only complexes with IC50 values below 20 μM may become clinically interesting [28]. Table S4 reveals the superoxide radical suppression efficacies of the complexes. It was observed that the radical scavenging activities of complexes increased with the increment of the complex concentrations.


## 3.6. Evaluation of Antimicrobial Activity

MIC data (Table1) display varying degrees of biocidal effects of L1 and its complexes on the growth of tested species. This study highly encourages that all the metal complexes have higher inhibitory effects than free ligand, and in particular mixed ligand complexes exhibited prominent antimicrobial activity, observed in the order of C2 > C4 > C1 > C3 > L1. All of these synthesized compounds showed MIC values in micromolar range (3.02–19.23 μg/mL). Out of these, C2 is the most bioactive (MIC 3.025 μg/mL) in the series and it was found to be more potent than the standard drug (MIC 3.12 μg/mL). The augmented toxicity of all the metal complexes could be explained on the light of Overtone’s concept [64] and Tweedy’s chelation theory [65]. As per these theories, the mode of action of the metal complexes may involve the formation of hydrogen bond formation through the azomethine group (HC=N-) with the active centers of cell constituents [66] resulting in interferences with the normal cell process. Structural activity relationship (SAR) study of the benzothiazole compounds shows that electron withdrawing groups (EWD) like fluorine exerts more potent antibacterial activity than electron donating groups (ER) is reported [67].Table 1
Antimicrobial activities of synthesized compounds.
Sl. number Compounds(30 µg/disk) MIC (zone of inhibition ± SD) inµg/mL E. coli P. aeruginosa B. subtilis S. aureus C. albicans A. niger ( 1 ) L1 11.0 (15 ± 0.6) 12.6 (17 ± 0.3) 12.3 (18 ± 0.9) 11.9 (17 ± 0.1) 19.6 (12 ± 0.2) 19.2 (16 ± 0.4) ( 2 ) C1 4.7 (22 ± 0.7) 4.8 (22 ± 0.9) 4.8 (23 ± 0.6) 4.6 (22 ± 0.7) 11.3 (20 ± 0.4) 11.5 (20 ± 0.6) ( 3 ) C2 3.02 (24 ± 0.4) 3.45 (24 ± 0.5) 3.31 (24 ± 0.4) 3.39 (21 ± 0.9) 8.84 (26 ± 0.2) 8.92 (26 ± 0.5) ( 4 ) C3 4.4 (22 ± 0.6) 4.6 (21 ± 0.6) 4.46 (24 ± 0.6) 3.91 (22 ± 0.6) 10.6 (23 ± 0.6) 9.37 (25 ± 0.6) ( 5 ) C4 3.73 (22 ± 0.8) 3.71 (23 ± 0.8) 3.13 (25 ± 0.1) 3.64 (26 ± 0.8) 9.16 (24 ± 0.5) 9.42 (24 ± 0.4) ( 6 ) Ciprofloxacin 3.12 (20 ± 0.6) 3.12 (20 ± 0.6) 3.0 (27 ± 0.6) 3.12 (19 ± 0.6) - - ( 7 ) Fluconazole - - - - 6.25 (16 ± 0.6) 6.31 (17 ± 0.6) Each value was replicated thrice.


## 3.7. Molecular Docking Studies

All the compounds were subjected to molecular docking with DNA and Cu, Zn-SOD using glide module of Schrödinger software to explore the binding of compounds with DNA. The virtual predicted top-ranking conformation with minimum energy glide score of compounds suggests best possible geometrical oriental binding with the target DNA double helix, which implies the highest binding affinity of DNA. The order of binding of compounds is as follows: L1 (−3.157), C2 (−3.564), C4 (−3.624), C1 (−4.288), and C3 (−4.195), whereas, with Cu, it is Zn-SOD C1 (−2.474), C2 (−1.478), C3 (−3.013), and C4 (−3.469). The other associated parameter calculated during docking studies is van der Waals interactions (kcal/mol) for DNA [L1 (−25.097), C2 (−21.049), C4 (−22.156), C1 (−27.888), and C3 (−28.739)] as well as Cu, Zn-SOD [C1 (−25.833), C2 (−12.897), C3 (−35.912), and C4 (−33.996)]. The determined 3D structure of C1 plays a significant role in exploring its structural consequences and conformational behavior during interactions with DNA [68]. C1 and C3 stacked with A-T-rich regions, whereas C2, C4, and L1 bind with G-C residues of groove wall of DNA by surface binding interactions (Figure 9). Geometrical oriental binding of L1 and C2 appears to be the same (Figure 9). Ligand L1 interacts with guanine and adenine through π-π interaction (Figure 10(a)). Complex C1 interacts with adenine via salt bridge and hydrogen bond (Figure 10(b)), whereas C2 interacts with adenine via salt bridge along with π-π interaction and hydrogen bond (Figure 10(c)); thus it shows maximum affinity with adenine. Thus, these confer the highest binding affinities of complexes C2 and C4 with DNA. Hence, these docked complexes, intra- and intermolecular hydrogen bond, and hydrophobic interactions (C2, C4, and L1) significantly participated in maintaining the stacked position of the complexes with DNA [68]. Therefore, it is suggested that there is a mutual complement between spectroscopic data and molecular docked model, which can be authenticated with spectroscopic results and it also provides the indication of groove mode.Figure 9
Binding mode of CT-DNA with compounds (L1, C1, and C2). DNA is represented in ribbon structure wherein the nucleoside is colored as yellow-guanine, maroon-thymine, blue-cytosine, and light green as adenine. Compounds are represented and highlighted in the figure.Figure 10
Two-dimensional views of docked complexes.
(a) (b) (c)Docked structures of DNA with L1(Figure 10(a)), C1(Figure 10(b)), and C2(Figure 10(c)) showing the molecular interactions like inter- and intrahydrogen bonds, π-π stacking, and salt bridges.Binding of compound at Cu Zn domain of SOD results in an increase in an antioxidant activity of SOD and decrease in oxidative stress [69]. All the compounds were found near active site of Cu, Zn-SOD (Figure 11), and C4 interacted with Tyr108 via π-π stacking, whereas C1 formed hydrogen bond with Ser109, C2 with Arg113, and C3 interacted with Glu107 via salt bridge. Hence, the data suggest that these compounds have potent binding with Arg113 and Glu107 which are resided near active site of Cu, Zn-SOD, thereby regulating the generation of free radicals.Figure 11
Active center forO2∙- scavenging of metal complexes.


## 4. Conclusions

The newly synthesized four mononuclear copper and cobalt complexes of imine-based ligand (L1) were analyzed with spectral techniques and screenedin vitrofor their binding efficacy towards DNA. Taking into account the analytical and spectral studies, an octahedral geometry is assigned to all these complexes. TGA revealed that the synthesized compounds were thermally stable. Spectral titration assessed the relative noncovalent binding of metal complexes to DNA and the results are corroborated with each other techniques. Observed DNA cleavage results demonstrated that their effective interactions with DNA in groove mode depend on ligand architecture. The antioxidant activity of compounds was measured by NBT assay. After binding with metal ions, the scavenging of superoxide anion free radical (O2∙-) activity of metal complexes obviously increased. The copper complexes exhibited the remarkable capacity for scavenging O2∙-. This is further fortified by molecular docking study where all the compounds are preferential selective for the groove of DNA. Antimicrobial results in higher antibacterial and antifungal potency of metal complexes than free ligand. The presence of a planar heterocyclic ligand in Cu(II) and Co(III) drug based mixed-ligand complexes which changes the interaction of complex in biological systems is noticed.



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*Source: 8759372-2018-03-01.xml*