Synthesis, Spectroscopic Characterization and Biological Studies of Mn(II), Cu(II), Ni(II), Co(II) and Zn(II) Complexes with New Schiff Base of 2-((Pyrazine-2-ylimino)methyl)phenol

: In the search for novel anticancer complex, transition metal complexes of Schiff base derived from 2-aminopyrazine and salicylaldehyde were successfully synthesized and characterized based on elemental analyses, spectroscopic and thermal analysis. The IR spectra showed the ligand is a tridentate chelator with O, N and N atoms. donor sites in the Zn(II), Co(II), Ni(II), and Mn(II) complexes. Contrary, it behaved a bidentate chelator in the Cu complex by O and N. Molar ratio data revealed that the ligand to metal ratio was 1:2 for Co(II) Cu(II) and Zn(II) while it was 1:1 for Mn(II) and Ni(II) complexes. The obtained complexes have the formulae [M(L) 2 ] (where M = Co(II) and Zn(II), [M(L)Cl(2H 2 O)] · H 2 O (where M = Ni(II) and Mn(II) were octahedral geometry). The computational studies were performed by DFT calculations to compare the optimized geometries with the experimental values. The interaction of these complexes with calf thymus DNA (CT-DNA) was investigated by UV-Vis spectroscopic technique. Molecular docking studies were against three protein cancer to investigate the binding ability of the new compounds. The anticancer activity was studied with different cell lines and the IC 50 of the Cu(II) complex for (HOP-62) showed a practical result. The LD 50 values of Zn(II) and Co(II) complexes showed that they are non-toxic at doses up to 370 mg/kg.


Introduction
The importance of the heterocyclic compounds came from the diversity usage in industries, biological fields [1,2] and in analytical chemistry as analytical reagents for metal ion detection [3] or dyes synthesis, cosmetics, plastics and pharmaceutical products. Moreover, they play a practical role in the drug industry by designing and developing medicines and their wide applications [4]. One of the essential chemical structure classes is nitrogen heterocycles which are particularly well represented between natural products, biologically active structures, and medical-related compounds [3]. Among the most distinguished types, phenanthridine, indole, pyrazine, quinoline, and isoquinoline compounds which have gained significant interest in organic synthesis, medical chemistry, and materials science [5]. Schiff bases are an important class of organic compounds especially the ones synthesized from heterocyclic compounds, due to their chelating properties and ability to coordinate with a wide range of actinide, lanthanide and transition ions in various oxidation states using oxygen and nitrogen or other atoms to form stable complexes [6]. Several Schiff bases were prepared to contain nitrogen atoms with crucial biological activity such as antimicrobial, antioxidant, anticancer, anti-HIV activity, analgesic, anti-inflammatory [3,7].
It was reported when metal ions are introducing into the molecules of the compound it could improve their biological properties by decreasing their toxicity and enhancing their lipophilicity, absorbance, and stability [7]. Additionally, the presence of an imine (-C=N-) or azomethine (-HC=N-) group in Schiff bases contributes to linkage provides much flexibility in the design ligands for metal ion coordination [3,8]. Interestingly, most of the studies confirmed complexes of Schiff bases with transition metals are showed higher biological activities than their corresponding ligand [8]. Akmal S. Gaballa et al. synthesized Pt(II) complexes with Schiff bases derived from salicylaldehyde. The Schiff base ligand and its Pt(II)complexes have been tested in vitro to evaluate their antibacterial activity against eight types of bacteria. The activity data show that the Pt(II) complexes are more potent antimicrobials than the parent Schiff base ligands against one or more microorganisms [9]. Xueguang Ran et al. synthesized three salicylaldehyde derivatives Schiff base ligand and their Zn(II), Cu(II), and Co(II) complexes. These compounds were screened and evaluated by antibacterial and antifungal bioassay and showed that the metal complexes have more active than the free ligan. Among these complexes, the Cu(II) complex was the most effective compared to other complexes [10]. Another reported work presented eight vanadium complexes derived from Schiff bases and tested their inhibition toward human recombinant PTP1B by selected complexes, glucose consumption and cytotoxicity tests in adipocytes in 3T3-L1 cell line. All vanadium complexes were noncytotoxic and three complexes were found to be active in the inhibition of human recombinant PTP1B [11].
In this study, Schiff bases and their transition metal complexes Mn(II), Cu(II), Ni(II), Co(II), and Zn(II) were synthesis and characterization by various techniques. The interaction of Schiff bases and their transition metal complexes with biological targets were tested with CT-DNA. Molecular docking was used to simulate the binding of the investigated complexes with three types of cancer proteins. Finally, we tested the complexes in vitro activity against three cancer cell lines via (Ovar3), (M14), and (NSCLC).

Materials and Instruments
All starting materials and reagents were purchased from Alfa Aesar. The ACROS. Calf thymus (CT-DNA) and all solvents were purchased from Sigma-Aldrich. IR spectra were recorded in Bruker Alpha in the range of 400-4000 cm −1 . UV-Vis spectra in the range of 200-800 nm were collected using a MultiSpec-1501 with a solution of 10 −3 M in DMSO at room temperature using matched 1.0 cm quartz cells. The 1 H NMR spectra in DMSO-d 6 solution were recorded on Bruker Avance 600 MHz. Thermal analysis was carried out on a PerkinElmer TGA system until 1000 • C in the air with a heating rate of 10 • C/min. The solid sample EPR analysis was obtained using the continuous wave Bruker EMX PLUS spectrometer (Bruker BioSpin, Rheinstetten, Germany) and collected with Bruker Xenon software.

Synthesis of Metal Complexes
The Schiff base ligand that prepared by previous work [12]. Briefly, 2 mmol or 1 mmol of ligand was dissolved in absolute ethanol in 25 mL and adjusted with a drop of NaOH. The solution of 1 mmol of the chloride salts of Co(II), Cu(II), and Zn(II) ions in absolute ethanol was added to the ligand solution and refluxed for 2-3 h. The complex was then filtered, washed with diethyl ether, and dried at room temperature, Scheme 1.

Computational Calculation
Gaussian 09 software package [13] is used to optimize the free Schiff base ligand and its metal complexes. Gauss View software [14] was used to visualize the output files and prepare the figures showing the molecular orbitals (MOs). The DFT method by the hybrid density functional theory, B3LYP, is used with 6-311G for the ligand while the metal complexes were optimized by the LAND base site in the gas phase. The obtained vibrational frequencies have indicted the optimized geometry corresponds to valid energy minimum and is scaled by 0.966 and 0.961 factors for 6-31G and LAND base site,

Computational Calculation
Gaussian 09 software package [13] is used to optimize the free Schiff base ligand and its metal complexes. Gauss View software [14] was used to visualize the output files and prepare the figures showing the molecular orbitals (MOs). The DFT method by the hybrid density functional theory, B3LYP, is used with 6-311G for the ligand while the metal complexes were optimized by the LAND base site in the gas phase. The obtained vibrational frequencies have indicted the optimized geometry corresponds to valid energy minimum and is scaled by 0.966 and 0.961 factors for 6-31G and LAND base site, respectively. The obtain HOMO and LUMO energies were used to calculate the essential quantum parameters by the following equation: energy gap (Egap = ELUMO − EHOMO), absolute electronegativities (χ = −EHOMO + ELUMO/2), absolute hardness (ɳ = ELUMO − EHOMO/2), chemical potentials (μ = −χ), global softness (S = 1/2ɳ), global electrophilicity (ω = π2/2ɳ) [15].

DNA Binding Studies
The DNA-binding abilities of the ligand and its metal complexes were studied by the UV-Vis spectroscopic method. The CT-DNA solution was confirmed to be protein-free by the U.V. absorbance ratio of 1.8 at 260 and 280 nm. All experiments were conducted at a pH value of 7.4 using Tris-HCl buffer and carried out by procedure described earlier [16,17]. The Benassi-Hildebrand equation (Equation (1)) was used to calculate the binding constants (Kb) [17].

DNA Binding Studies
The DNA-binding abilities of the ligand and its metal complexes were studied by the UV-Vis spectroscopic method. The CT-DNA solution was confirmed to be protein-free by the U.V. absorbance ratio of 1.8 at 260 and 280 nm. All experiments were conducted at a pH value of 7.4 using Tris-HCl buffer and carried out by procedure described earlier [16,17]. The Benassi-Hildebrand equation (Equation (1)) was used to calculate the binding constants (K b ) [17].
A 0   [20]. We used the docking protocol that has been described in our previous work [21]. After the crystal structure has been downloaded from the PDB www.rcsb.org (accessed on 1 July 2021), the water molecules, co-ligand, and metal ions have been removed. The final form was obtained after 3D protonation and the correction process. The MOE site finder generated the active binding sites to create the dummy sites as the binding pocket. The default docking parameters were as follows: triangle matcher for replacing the molecule and London dG for rescoring the docking scores. The DFT optimized structures of the compounds have been used to generate the best five binding poses with flexible molecules rotation. The hydrogen bonds formed between elastase and investigated compound were used to rank the binding affinity and presented as the free binding energy (S, kcal/mol). The higher negative values of the docking scores were presented along with 2D and 3D structures [22].

Anticancer and Toxicological Studies
The cells were supplied by the Egyptian Holding Company for Biological Products and Vaccines (VACSERA) and then kept in the tissue culture unit. The growth of the cells was proceeded in RPMI-1640 medium, supplemented with FBS (10% heat inactivated), penicillin (50 units/mL), and streptomycin (50 mg/mL), and kept in a humidified atmosphere with 5% carbon dioxide [23,24]. The cells were kept as monolayer cultures by serial sub-culturing, obtaining cell culture reagents from Lonza (Basel, Switzerland). The antitumor activities of the complexes were assessed against Ovcar-3 (overian) NSCLC (lung), and M-14 (Melanoma) cell lines. The sulforhodamine B (SRB) assay method was applied to determine the cytotoxicity, as described in the literature [25]. Exponentially growing cells were gathered using 0.25% Trypsin-EDTA and seeded in 96-well plates at 1000-2000 cells/well in RBMI-1640 supplemented medium. The cells were maintained in the medium for 1 day and then they were incubated for 3 days with various concentrations of the tested complexes. Following 3 days treatments, the cells were fixed with 10% trichloroethanoic acid for 1 h at 4 • C. Wells were stained for 10 min at room temperature with 0.4% SRBC dissolved in 1% acetic acid. The plates were air dried for 24 h and the dye was dissolved in Tris-HCl for 5 min with shaking at 1600 rpm. The optical density (OD) of each well was assessed spectrophotometrically at 564 nm with an ELISA microplate reader (ChroMate-4300, Palm City, FL, USA). The IC 50 values were calculated from a Boltzmann sigmoidal concentration response curve using the nonlinear regression fitting models (Graph Pad, Prism Version 9).

Determination of Acute Toxicity (LD 50 )
The median lethal dose (LD 50 ) of the test compounds was determined in mice. A group of male albino mice of five animals (25-30 g) was injected (i.p.) at a specific grade. The percentage of mortality was determined 72 h after injection for each drug under investigation. A prism-9 processed computation of LD 50

Infrared Analysis
A sharp (C=N) band of the azomethine group was observed 1602 cm −1 in the free ligand [12]. After complexation, the vibration band of the azomethine group was decreased in intensity and shifted toward a lower frequency about 16-60 cm −1 in the metal complexes, except the Cu(II) complex that has low intensity band and shifted toward higher frequency about 2 cm −1 . This shift or disappearance of the peaks support complex formations [26]. The observed sharp band of the pyrazine ring (C=N) in the ligand at 1561 cm −1 was shifted more than 5 cm −1 in the metal complexes, except the Cu(II), Table S1. This indicates that the pyrazine ring is involved in coordinating to the metal ions [12]. New broadband in three metal complexes Cu(II), Mn(II) and Ni(II) at 3334, 3315 and 3457 cm −1 could assign to ν(H 2 O) [22].
A new band of ν(M-O) band have appeared in the wavenumber range 522-575 cm −1 and ν(M-N) band in range 424-444 cm −1 [22]. Figure S1 showed the comparison of the IR spectra of the free ligand and the metal complexes. 1 H-NMR Spectra for Ligand and Zn(II) Complex The 1 HNMR spectrum of the Schiff base has discussed in detail in our previous work [12]. The signal at 12.38 ppm in the free ligand indicated the presence of phenolic-OH proton has disappeared in the Zn(II) complex spectrum and confirmed the coordination by phenolic oxygen to the zinc ion. In addition, the Schiff base shows another signal at 9.52 ppm which can be ascribed to the azomethine proton (-CH=N). This signal was shifted to 10.22 ppm after complexing to Zn(II) ion and reveals the involvement of azomethine nitrogen in the coordination of the zinc complex [12]. The 1 H NMR data for the ligand and Zn(II) are shown in Figure S2 and summarized in Table S2.

Conductance Measurements
The observed molar conductance of the transition metal complexes at range Λ M = 26-58 ohm −1 cm 2 mol −1 in 10 −3 M DMSO solutions, which suggest the nonelectrolytic nature of these compounds.

Molar Ratio
To determine the molar ratio of the metal ion to the ligand molecule. The metal ion standard solution 1 × 10 −4 M was pipetted into seven volumetric flasks (0, 1, 2, . . . , 6 mL), and a solution of 1 × 10 −4 M ligand (6, 5, 4, . . . , 0 mL) was added, respectively. All the measurements were carried by a spectroscopic method in a 200-500 nm range. The absorbance measurements were performed by keeping the metal ion concentration constant at 0.72 × 10 −3 M, while the ligand varied, as shown in Table S3. The absorbance of the sample solution was measured against blank at the maximum wavelength, and the values were then plotted against the ratio of [M])/([M] + [L]) [27]. From the results, we found the inflection was at 0.33 for Co(II) Cu(II) and Zn(II), as shown in Figure 1, while the inflection at 0.5 indicated to 1:1 for Mn(II) and Ni(II) complexes and 1:2 for the other metals.

The Electronic Spectra
Electronic spectral studies for all these complexes were carried out in DMSO M concentration. The spectrum of the Schiff base free ligand has observed bands at

The Electronic Spectra
Electronic spectral studies for all these complexes were carried out in DMSO at 10 −3 M concentration. The spectrum of the Schiff base free ligand has observed bands at 264.28, 321.93, and 357.31 nm assigned to π-π* and n-π* transition, respectively [12]. The metal complexes showed a shift towards lower frequencies of the absorption bands and confirmed the coordination of the ligand to the metallic ions [28]. The electronic spectra of the complexes are shown in Figure S3. Since they are dark-colored complexes, the electronic spectra of d-d transitions are interred with the broad peak of the high excitation coefficient of ligand contribution. Therefore, they are an expression that is forbidden as the Laporte rule of electronic absorptions; this is because the extinction coefficient for these complexes is low compared with the ligand's contribution in the electronic spectra, and it is not easy to see the peaks of these complexes next to the ligand peak.

EPR Spectra for Cu(II) Complex
Electronic paramagnetic resonance spectroscopy is a reliable method to obtain information on the structure of materials with unpaired electrons of complexes [29]. The EPR spectrum of solid Cu(II) complex was obtained at room temperature showed values of g|| = (2.40) and g⊥ = (2.19) as shown in Figure 2. The g|| is greater than the g⊥ value (g|| > g⊥ > 2.0023) and assumed the octahedral, tetrahedral and square planer structure and indicate the ground state of the Cu(II) ion will be dx 2 − y 2 [30]. Further, calculating the value of g av by this equation g av = (g||+(2g⊥) 3 was 2.24 and suggests the covalent character of the metal-ligand bond [17].

Thermal Analysis
Studying the results of the thermal analysis of the metal complexes can expect the number of water molecules, decomposing of the organic molecule in the complexes and metal oxides [31]. The thermogravimetric analysis was measured at room temperature to 800 °C, Figure 3, and the results were summarized in Table S4.
The TG curves of the Mn(II), Ni(II), Cu(II), and Zn(II) complexes showed four decomposition steps while Co(II) complex showed a two-decomposition step; we will discuss them in detail.

•
The Mn(II) curve showed four decomposition steps within the temperature ranges of 38.76-821. 43

Thermal Analysis
Studying the results of the thermal analysis of the metal complexes can expect the number of water molecules, decomposing of the organic molecule in the complexes and metal oxides [31]. The thermogravimetric analysis was measured at room temperature to 800 • C, Figure 3, and the results were summarized in Table S4.

Kinetic Studies
Thermodynamic parameters for the complexes were calculated by employing tw methods, the Coast-Redfern integral [32] and the approximation of Horowitz-Metzg [33] methods, to obtain the activation energy (Ea). Thermodynamic activation paramete of decomposition processes of the complexes, ΔH (enthalpy), ΔS (entropy), ΔG (Gibbs fr energy change of the decomposition), and E (thermal activation energy) are evaluate graphically, and calculated from the thesis in Equations (2)-(4).

ΔH = E + PV
where KB and h are Boltzmann and Plank's constants, respectively [34,35]. The results a shown in Table S5. Moreover, the general thermal behaviors of the prepared complex in terms of stability ranges, peak temperatures, and values of kinetic parameters are plo ted for Mn(II) complex in Figures 4 and 5.
The negative values of ΔS indicate pointed to high randomness-degree in non-spo taneous reaction. The positive values of ΔG showed the reaction is non-spontaneous t wards products and spontaneous towards the reactants and the positive values of Δ means the reaction is endothermic [35,36]. The TG curves of the Mn(II), Ni(II), Cu(II), and Zn(II) complexes showed four decomposition steps while Co(II) complex showed a two-decomposition step; we will discuss them in detail.

•
The

Kinetic Studies
Thermodynamic parameters for the complexes were calculated by employing two methods, the Coast-Redfern integral [32] and the approximation of Horowitz-Metzger [33] methods, to obtain the activation energy (E a ). Thermodynamic activation parameters of decomposition processes of the complexes, ∆H (enthalpy), ∆S (entropy), ∆G (Gibbs free energy change of the decomposition), and E (thermal activation energy) are evaluated graphically, and calculated from the thesis in Equations (2)-(4).
where K B and h are Boltzmann and Plank's constants, respectively [34,35]. The results are shown in Table S5. Moreover, the general thermal behaviors of the prepared complexes in terms of stability ranges, peak temperatures, and values of kinetic parameters are plotted for Mn(II) complex in Figures 4 and 5.
Appl. Sci. 2021, 11, x FOR PEER REVIEW 9 of 20  The negative values of ∆S indicate pointed to high randomness-degree in non-spontaneous reaction. The positive values of ∆G showed the reaction is non-spontaneous towards products and spontaneous towards the reactants and the positive values of ∆H means the reaction is endothermic [35,36].

Structural Interpretation
From the above analyses, the suggested structures of these complexes are given in Figure 6 and are matched with previous research. The Schiff base ligand coordinated to metal ions Mn(II), Ni(II) through the N, N, O system [11,37] while Co(II) and Zn(II) [38] was bidentate and bonded through the N, N, O atoms. For Cu(II), the structure is presented in Figure 6.

Structural Interpretation
From the above analyses, the suggested structures of these complexes are given in Figure 6 and are matched with previous research. The Schiff base ligand coordinated to metal ions Mn(II), Ni(II) through the N, N, O system [11,37] while Co(II) and Zn(II) [38] was bidentate and bonded through the N, N, O atoms. For Cu(II), the structure is presented in Figure 6.

Geometry of the Complexes
We used the obtained results from the spectroscopic analysis (IR, NMR, UV-VIS, and EPR) we proceeded with a computational study to optimize the complex's geometry by the DFT approach. The optimized geometries optimized in the gas-phase of the ligand and its metal (Π) complexes were presented with the number and labels of the atoms in Figure 7.

Geometry of the Complexes
We used the obtained results from the spectroscopic analysis (IR, NMR, UV-VIS, and EPR) we proceeded with a computational study to optimize the complex's geometry by the DFT approach. The optimized geometries optimized in the gas-phase of the ligand and its metal (Π) complexes were presented with the number and labels of the atoms in Figure 7.

Geometry of the Complexes
We used the obtained results from the spectroscopic analysis (IR, NMR, UV-VIS, and EPR) we proceeded with a computational study to optimize the complex's geometry by the DFT approach. The optimized geometries optimized in the gas-phase of the ligand and its metal (Π) complexes were presented with the number and labels of the atoms in Figure 7. A selected geometric parameter around the coordination sphere such as bond length and bond angles for the free ligand and its metal complexes were extracted and tabulated it in Table 1.
The bond length of the free Schiff base showed different characters after bind to the metal ions. The bond length C20-N22 became longer than the free ligand after complexation, whether O18-C4 became shorter by 0.04 and 0.06 Å, respectively. There was a slight change in the C14-N22 and C14-N23 bond lengths around 0.01or 0.02 Å. In the metal complexes, the primary ligand is coordinated in a bidentate to all metal except Co(II) and Zn(II) that bonded via tridentate from the organic ligand.
The new bonds with the Mn(II) ion, M-O18, and M-N22, were in the reported range of the ionic character of these bonds [39]. Moreover, the other new bonds between the Mn(II) and HO 2 or Cl ion are presented in a covalent bond. Interestingly, all the bonds around Cu(II) ion, M-O, and M-N were ionic bonds with an average length of 1.97 Å. In contrast, the bidentate Ni(II) complexes and tridentate Co(II) and Zn(II) compounds have covalent bonds or medium ionic atmosphere with bond length average = 2 Å.
The importance of bond angles in the coordination complexes comes from the ability to describe the geometric structure of the prepared compounds. Generally, the selected angles around the coordination site in the free ligand, C3-C4-O18 and C3-C20-N22, became bigger after binding to metal ions, while the bond angle between N22-C14-N23 has decreased.  The frontier orbital energies are important theoretical parameters that contest the highest occupied and the lowest unoccupied molecular orbital energies (HOMO and LUMO, respectively) and the difference between them is called the energy gap (E HOMO − E LUMO = E gap ) [17]. The calculated energy values for the ligand and its metal complexes were extracted and tabulated with the quantum parameters in Table 2. Figure 8 presents the HOMO and LUMO electron densities calculated by the B3LYP method using the 6-31G basis set for Schiff base and LAND for the metal complexes. For the free ligand, E gap was 4.09 eV decreased after complexing with metal ions. The small E g indicates the softtness and reactivity of the complexes. We can arrange the complexes in the following order, Cu(II) > Mn(II) > Co(II) > Ni(II) > Zn(II). Therefore, the Cu(II) complex presents good reactivity and reveals good toxicity and inhibition activity [40]. Absolute electronegativities (χ), absolute hardness (η), absolute softness (σ), chemical potentials (Pi), global softness (S), global electrophilicity (ω), and additional electronic charge (∆Nmax) are listed in Table 2. softtness and reactivity of the complexes. We can arrange the complexes in the followi order, Cu(II) > Mn(II) > Co(II) > Ni(II) > Zn(II). Therefore, the Cu(II) complex presents go reactivity and reveals good toxicity and inhibition activity [40]. Absolute electronegati ties (χ), absolute hardness (η), absolute softness (σ), chemical potentials (Pi), global so ness (S), global electrophilicity (ω), and additional electronic charge (ΔNmax) are listed

DNA-Binding Studies
Electronic absorption titration is one of the easiest methods that helps to predict th type of binding mode of compounds with CT-DNA [41]. In this experiment, the concen tration of the metal compounds has been maintained with the variation of the DNA con centration in the range of 2 × 10 −6 -7 × 10 −6 M.
The free Schiff base ligand spectrum did not show any observed shift after the add tion of the DNA nevertheless it showed a reduction in the absorption intensity (hype chromic), suggesting a weak interaction between the ligand and DNA [42]. The intrins binding constant (Kb) for the ligand with CT-DNA was 1 × 10 6 M −1 .
In general, for the metal complexes, the experiments showed two performances fo the metal complexes with increasing CT-DNA concentration, hyperchromic with blu shift or hypochromic with redshift. The complexes of Zn(II) and Mn(II) showed a shi

DNA-Binding Studies
Electronic absorption titration is one of the easiest methods that helps to predict the type of binding mode of compounds with CT-DNA [41]. In this experiment, the concentration of the metal compounds has been maintained with the variation of the DNA concentration in the range of 2 × 10 −6 -7 × 10 −6 M.
The free Schiff base ligand spectrum did not show any observed shift after the addition of the DNA nevertheless it showed a reduction in the absorption intensity (hyperchromic), suggesting a weak interaction between the ligand and DNA [42]. The intrinsic binding constant (K b ) for the ligand with CT-DNA was 1 × 10 6 M −1 .
In general, for the metal complexes, the experiments showed two performances for the metal complexes with increasing CT-DNA concentration, hyperchromic with blue shift or hypochromic with redshift. The complexes of Zn(II) and Mn(II) showed a shift from the λ max to more than 5 nm. This could indicate the change of the distance between the two helix structures in DNA [41], Figure S4a. The absorption spectra of Ni(II), Cu(II), and Co(II) complexes showed a hypochromic mode with a blue shift which indicated the change in the DNA confirmation or the damage that occurred to the DNA structure [37] Figure S4b.
The binding constant (K b ) for the complexes were presented in Table 3. Interestingly, all the complexes gave (k b ) values ranging from 8 × 10 5 to 3.33 × 10 5 . Comparing these values with Ru (III) complexes [43], we found that the values were assumed to be intercalation binding types. As observed from Table 3, the Ni(II) complex had the highest binding constant value, followed by the Zn(II) complex.

Molecular Docking
Molecular docking is a computational software regularly used to understanding protein-receptor interaction with complexes [17,44]. The docking process was carried out by simulating the interaction of the Schiff base and their metal complexes with three types of protein-receptors; (M14) melanoma cancer (PDB = 2OPZ), (Ovar3) ovarian cancer (PDB = 3W2S), and (HOP-62) (NSCLC) cancer (PDB = 1S9J) which have selected according to the literature and previous studies . The docking study results of the complexes are summarized in Table 4. We found that the compounds obtained a high negative value indicating practical bound to the protein. Obviously, Cu(II), Zn(II), and Co(II) complexes gave better results than the ligand. Both Cu(II) and Zn(II) complexes showed the best value compared to the rest of the complexes. We can discuss this binding by way of the following points: • Cu(II) complex was associated with three hydrogen bonds (π-H) with 2OPZ protein, through the carbon 20 in the complex with the hexagonal ring of the TRP 323, and the five-pointed ring of the TRP 323 amino acid residue, and the benzene ring in the copper complex also associated with the LEU 307 amino acid residue, Table 5 shows the best possible conformation inside the Melanoma cancer 2OPZ protein both the ligand and their metal complexes. • Cu(II) complex was associated with four hydrogen bonds with 3W2S protein, through the carbon 27 in the complex with the ASP 855 amino acid residue by H-donor bond, nitrogen 19 in the complex with a nitrogen atom in MET 793 amino acid residue by H-acceptor bond, and the benzene ring in the copper complex also associated with the LEU 718 and GLY 796 amino acid residues by π-H bond, are tabulated in Table 5. • Zn(II) complex was associated with two hydrogen bonds (π-H) with 1S9J protein, through the benzene ring in the complex with the ALA 220 and ASN 221 amino acid residues by π-H bond, are tabulated in Table 5 shows the best possible conformation inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes. residues by π-H bond, are tabulated in Table 5 shows the best possible conformati inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes residues by π-H bond, are tabulated in Table 5 shows the best possible conformation inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes. residues by π-H bond, are tabulated in Table 5 shows the best possible conformatio inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes residues by π-H bond, are tabulated in Table 5 shows the best possible conformation inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes. residues by π-H bond, are tabulated in Table 5 shows the best possible conformati inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes residues by π-H bond, are tabulated in Table 5 shows the best possible conformation inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes.  Ligand residues by π-H bond, are tabulated in Table 5 shows the best possible conformati inside the (NSCLC) cancer 1S9J protein both the ligand and their metal complexes

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand.

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand.

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand.

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand.

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand.

Anticancer and Toxicological Studies
The Schiff base ligand and their metal complexes were examined against three types of cancer cells. The results are presented in Table 6. The results clarified that metal complexes have better anticancer activities compared to the ligand. Observing the Cu(II) complex has higher activity towards all cancer lines due the pyrazine ring's role which raising the complex's efficiency [46,47]. Hopeful a drug's safety used in vivo can be examined, which means more studies in the laboratory.
The median lethal dose (LD 50 ) of the most active anticancer metal complexes for HOP-62 complexes (Zn(II) and Co(II)) in addition these complexes were determined (i.p.) in mice according to reported procedures [48]. The animals got an injection (i.p.) of a specific grade. The results showed that the (LD 50 ) of tested compounds were non-toxic at doses up to 370 mg/kg

Conclusions
The present work describes the synthesized and characterized of a Schiff base and their metal complexes by analytical and spectroscopic studies. The IR spectra showed a new band at 400 for M-O and 500 M-N indicating that the ligand successfully coordinated to Cu ions through the N, O system and by tridentate system (N, N, O) with other metals ions. The molar ratio data reveal that the ligand to metal ratio is 1:2 for Co(II) Cu(II) and Zn(II), and 1:1 for Mn(II) and Ni(II) complexes. The thermal analysis explained the number of water molecules in the metal complexes. The proposed structures of metal complexes were confirmed by optimizing the geometry of the complexes by the DFT method. The energy gap, E GAP , for the complexes was lower than that of the ligand, which indicated high activity for the metal complexes. The DNA binding, molecular docking analysis, and anticancer studies suggested that the Schiff base metal complexes were found to be biologically active. The metal complexes showed efficient activity of three cell lines cancer (Ovra3), (M14), and (HOP-62); notably, Cu complex for (HOP-62) showed great results for the safety of the drug used in vivo.

Supplementary Materials:
The following are available online at https://www.mdpi.com/article/ 10.3390/app11199067/s1, Table S1: comparison between characteristic IR bands experimental and theoretical values, Table S2: major 1H NMR data for ligand and Zn(II) complex, Table S3: experimental data of Cu(II) complex by molar ratio, Table S4: thermoanalytical result of the ligands and their complexes, Table S5: thermodynamic data of thermal decomposition of ligands and its uranyl complexes. Figure S1. IR spectra for ligand and their metal complexes, Figure S2. 1H NMR spectra of Schiff base ligands (a) and Zn(II)complex (b), Figure S3. The electronic spectra of ligand and their complexes, Figure S4. Absorption spectra of (a) Zn(II) complex and (b) the Ni(II) complex in a Tris-HCl buffer upon addition of DNA. The change in the absorbance upon increasing the concentration of DNA is indicated with arrows.