INTRODUCTION
Schiff bases play a pivotal role in inorganic chemistry [1] due to their ability to form stable complexes with most transition metal ions in the periodic Table. These complexes are of great importance in the medical field [2], where they are widely used in the pharmaceutical industry and exhibit high biological activity against many types of bacteria and cancer cells [3]. They are also widely used as intermediates in the synthesis of many medically and biologically important heterocyclic compounds [4]. Schiff bases can catalyze a variety of synthetic chemical processes and biologically active [5]. The emergence of inorganic biochemistry has led to increased research interest in these compounds. Metal compounds with chelating bonds to sulfur, nitrogen, and oxygen have received increasing attention due to their distinctive physical and chemical properties, especially if these compounds are heterocyclic and contain nitrogen [6,7], for their ability to act as reagents for studying DNA structure, as well as their use as chemotherapy 
agents and diagnostic drugs [8]. The high electron density on the nitrogen atom in the azomethine group enhances the biological potential of these bases. Therefore, metal complexes with Schiff bases act as antioxidants, antibacterial agents, antifungals, anticancer agents, antituberculosis agents, and anti-inflammatories [9]. In this study, a diamine compound with a heterocyclic aldehyde derived from pyridine was used. Pyridine (a heterocyclic nitrogen compound) and its derivatives exhibit a wide range of biological activities [10][11] to form a Schiff base, and then the formation of complexes with cobalt(II), nickel(II), copper(II), zinc(II), platinum(III), and gold(IV). Analyses were performed to determine the structure and geometry of the compound [12]. Furthermore, the antimicrobial activity of these metal compounds was evaluated using the paper disk diffusion method [13] (for qualitative determination) and the liquid broth serial dilution method [14] (to determine the minimum inhibitory concentration). The antiproliferative activity of these compounds was investigated against various cancer cell lines [15]. Molecular docking analysis was performed to elucidate the mechanism of action of these compounds and to support the efficient binding of the molecules to the protein’s active site. This study aimed to design and synthesize a novel pyridine-based Schiff base ligand and to investigate its coordination behavior with selected transition metal ions. The synthesized ligand was fully characterized using a range of physical, chemical, and spectroscopic techniques, including elemental analysis, Fourier transform infrared spectroscopy (FTIR), UV-Vis spectroscopy, mass spectrometry, and nuclear magnetic resonance spectroscopy (NMR), to confirm its structure and binding sites. A series of metal complexes with cobalt(II), nickel(II), copper(II), zinc(II), platinum(IV), and gold(III) were prepared, and their geometric structures were elucidated based on spectroscopic and magnetic studies. In addition to structural characterization, the biological potential of the ligands and their complexes was evaluated through antibacterial assays against both Gram-positive and Gram-negative bacteria, as well as in vitro anticancer studies. This work also focuses on understanding the role of metal coordination in enhancing biological activity, highlighting the synergistic effect between Schiff base ligands and metal ions.

MATERIALS AND METHODS
Instrumentation
Using the Bruker D.R.X. nuclear magnetic resonance spectrometer (NMR spectrometer). (DMSO-d6, 125 MHz, 500 MHz), a 5975 mass spectrometer, a Euro Vectro-3000A trace element analyzer, a Jena atomic absorption spectrometer (VARIO 6, AG), a Shimadzu 1700 UV-Vis spectrometer (wavelength 200-1100 nm), and a Shimadzu Fourier-transformed infrared spectrometer (wavelength 400-4000 cm⁻¹). Scanning electron microscopy (FE-SEM) images of the compounds were also acquired using a Zeiss EM3200 microscope. X-ray diffraction (XRD) was also recorded using a Philips diffraction spectrometer with a graphite crucible as the single component. The instrument used Cu kα radiation (wavelength= 1.54 angstroms) as the X-ray source at 45 kV and 50 mA. Using AgNO3 solutions, the chloride content of Co(II), Ni(II), Cu(II), Zn(II), Pt(IV) and Au(III) complexes was measured. Thin-layer chromatography (TLC) was used to determine the overall composition of the materials. Selected samples were also subjected to biological activity assessments at the Al-Amin Center for Advanced Research and Biotechnology. The Beckman Model J2-21 refrigerated centrifuge and Marubeni freezer (-800°C) were manufactured in the USA. The distillation apparatus, drying apparatus, and sterilization apparatus were manufactured by Hermle (Germany) and Ogawa Seiki (USA). Organon Teknika designed the incubators and reading devices. A Leica inverted microscope was used, and the microplates, multi-well plates, and 96-well plates—microporous membranes capable of passing through a 0.22 µm filter—were manufactured in the USA. Sterile flasks for tissue culture (25.75 cm²), water bath, and water pump.

Materials
6-methoxypicolinaldehyde,1,2-phenylenediamine,metal chlorides (CoCl₂·6H₂O), (NiCl2.6H2O, CuCl2.2H2O, ZnCl2, (H2PtCl6.6H2O) and (HAuCl4.3H2O) as well as Müller-Hinton agar, absolute ethanol, glacial acetic acid, acetone, acetonitrile, diethyl ether, dimethylsulfoxide (DMSO), hexane, N,N-Dimethylformamide (DMF), ethyl acetate. All chemicals and solvents were of the highest quality and were sourced from Sigma-Aldrich. BDH and Fluka were employed without additional manipulation.

Synthesis of New ligand (MMAPM)
The synthesis of the (1Z,1’Z)-N,N’-(1,2-phenylene)bis(1-(6-methoxypyridin-2-yl)methanimine) (MMAPM): 2.4 mL (0.02 mol) of 6-methoxypicolinaldehyde and 0.108 g (0.01 mol) of 1,2-phenylenediamine,dissolved in 20 mL of hot absolute ethanol were reacted to produce the molecule (MMAPM), with the addition of three drops of glacial acetic acid [16]. The reaction mixture was heated under reflux at 78 °C with continuous magnetic stirring to ensure complete homogeneity and successful formation. After the reaction, which lasted 270 minutes and was detected by thin-layer chromatography (TLC) using a 2:4 (v/v) mixture of hexane and ethanol as a solvent, the resulting mixture was allowed to cool gradually to room temperature and left undisturbed for 8 hours to allow crystallization and prevent agglomeration [17]. Over time, a brown crystalline substance was observed to form. The material was then washed with cold, dry ether, and the product was filtered. The solids content after oven drying was 75%. Fig. 1 illustrates the formation reaction of MMAPM.

Preparation of Metal Salts Standard Solutions
Standard solutions of metal salts were prepared by dissolving a weight of (0.0001 mol) of each of the following salts to obtain a basic solution of 1×10⁻³ M each of CoCl₂·6H₂O, NiCl₂.6H₂O, CuCl₂.2H₂O, ZnCl2, H2PtCl6.6H2O and HAuCl4.3H2O in 100 mL of absolute ethanol. These solutions were used to prepare a number of concentrations between 1×10⁻⁴ and 1×10⁻⁶ M [18].

Mole Ratio Method 
The absorption spectra of 1 mL of metal ions at the optimal concentration were measured against different volumes of the bonding solution at the same concentration. A relationship was plotted between the absorption and the mole ratio, and the M:L ratio was found to be 1:1 for all the complexes under study.

Synthesis metal complexes
The Schiff base ligand (MMAPM) was coordinated with the corresponding metal chlorides of Ni(II), Co(II), Cu(II), Zn(II), Pt(IV), and Au(III) to create the metal complexes. Under constant stirring, approximately 1 mmol of the Schiff base ligand (MMAPM) was fully dissolved in 35–30 mL of hot absolute ethanol. Separately, 20–25 mL of ethanol solution was used to dissolve approximately 1 mmol of the appropriate metal chloride salt, such as CoCl₂·6H₂O, NiCl₂·6H₂O, CuCl₂·2H₂O, ZnCl₂, H2PtCl6.6H2O, or HAuCl4.3H2O. To guarantee full complex formation, the ligand solution was added dropwise to the metal salt solution while being continuously stirred. The mixture was then refluxed for one to three hours. The successful coordination between the ligand and metallic ions was demonstrated by the appearance of coloured precipitate [19]. The mixture was left to cool to room temperature. and the resulting solid complexes were filtered, repeatedly cleaned with cold ethanol and then diethyl ether to eliminate any materials that had not yet reacted, and oven-dried until the formation of corresponding metal (II/III/IV) Schiff base complexes, then each compound was dissolved in absolute ethanol and ultrasonically treated at a frequency of 20–40 kHz for 20 minutes while maintaining a temperature below 40 °C to reduce agglomeration and improve nanodispersion without affecting the coordination structure. The compounds were then separated, washed, and dried [14]. The different quantities of ligand as well as the per cent composition of all forming complexes are shown below in the Table 1 and Fig. 2.

Antimicrobial Study
All recently synthesised ligands and complexes were evaluated for their antibacterial efficacy against S. aureus (a gram-positive bacterium) and E. coli (a gram-negative bacterium) utilising the agar diffusion method[20,21]. Each chemical demonstrated the ability to fight germs. The test organisms were cultivated in Mueller-Hinton broth. Chemical solutions utilised for biological study were dissolved in dimethyl sulfoxide (DMSO) at a concentration of 1x10-3 M [22]. The plates spent a day at 37°C in a heated incubator. The size of the inhibitory zone the compounds created against the corresponding test bacterium was used to assess the antibacterial efficacy of the compounds synthesised in this way. To arrive at a conclusion, the volume of the area of growth limitation for each sample was computed using the average of three independent replicates [23].

Anti-cancer studies
Using a cell viability assay against specific human cancer cell lines, the anticancer activity of the chosen compounds was evaluated in vitro [24]. The cancer cells were kept at 37°C, 5% CO₂, and humid conditions in either DMEM or RPMI-1640 with 10% FBS and 1% antibiotic-antimycotic. Trypsin-EDTA solution was used for subculturing at a confluency of roughly 70–80%. The cells were then seeded into 96-well microplates at a suitable seeding density of roughly 1× l0⁴ cells/well. To enable attachment, the plates were subsequently incubated for a full day. To obtain different concentrations, the chosen compounds were diluted with culture medium after being dissolved in dimethyl sulfoxide (DMSO). Fresh medium containing varying concentrations of the test compounds, untreated cells as a negative control, and a standard anticancer medication as a positive control were used to replace the culture medium after incubation. Under typical cultural conditions, the treated plates were incubated for 72 hours. Following treatment, the MTT assay—which involves adding MTT reagent to each well and then incubating for four hours was used to measure cell viability. The formed formazan crystals must be dissolved in DMSO or another suitable solubilizing solution, and a microplate reader must be used to measure the absorbance at 570 nm. In order to calculate the percentage of cell viability and inhibition, the tested compounds’ IC₅₀ values are derived from dose-response curves. To ensure accuracy and reproducibility, every experiment was carried out in triplicate.

Molecular Docking
The molecular docking study was conducted using the Molecular Operating Environment (MOE). The chemical structures for the ligands of interest (MMAPM, and MIMPM-Pt complex) were drawn in MOE and energy minimized with the default force field to arrive at Table three-dimensional conformations. The crystal structure of the target protein (PDB ID: 4JPS) was obtained from the Protein Data Bank, and prepared by removing water molecules and all co-crystallized ligands before adding hydrogen atoms and partial charges. The active site was obtained using the Site Finder module in MOE and docking simulations were performed with the default docking protocol, whereby ligand conformations were generated and ranked by binding free energy scores (S-score). The best binding poses were selected by choosing poses with the lowest energy according to the RMSD < 1 Å and lowest energy criteria. The interactions between the ligands and the amino acid residues at the binding site were visualized and analyzed using the MOE tools. The hydrogen bonds as well as π–π interactions and hydrophobic contacts between the ligand and the amino acid residues were easily identified, and bond distance and interaction energy could be measured.

RESULTS AND DISCUSSION
Physical features and elemental analysis
The ligand utilized in this investigation (MMAPM) is brown in colour. During the coordination process, this ligand consented with the metal ions to give complexes of varied colours. The compounds are soluble in polar organic solvents such as ethanol, methanol, acetone, diethyl ether, dimethyl sulfoxide, and carbon tetrachloride but insoluble in water. Table 2 shows the physical properties and elemental analysis (C, H, N, O) of the compound, where the analytical data for the compounds match the experimental results. The values show a 1:1 ratio between the metal and the ligand in Co(II), Ni(II), Cu(II), Zn(II) and Pt(IV), which corresponds to an octahedral geometry. Except for the Au(III) complex, which is square planar and has the same metal-to-ligand ratio.

NMR Spectra for the (MMAPM) ligand and Pt(IV) complex
NMR spectral data were recorded for MMAPM and its complexes in DMSO-d6 solvent. The MMAPM spectrum showed a signal at 8.84 ppm attributed to the azomethine proton (-CH=N), indicating the formation of a Schiff base bond. Aromatic ring protons appeared between 7.20 and 7.57 ppm, while a signal between 7.63 and 7.67 ppm was attributed to the pyridine ring protons. A signal of 3.87 ppm was found for the methoxy group protons (-OCH3) [25].
The non-magnetic Pt4+-MMAPM complex showed a single azomethine proton (-N=CH-) signal at 8.95 ppm. Similarly, the aromatic ring protons showed a shift at (δ=7.24–7.61) ppm, and the pyridine ring protons showed a shift at (7.63–7.74) ppm. A signal at (δ=3.84) ppm was attributed to the methoxy protons directly bonded to the benzaldehyde ring in the Pt⁴⁺ complex, and single signals at (δ=2.31) ppm were attributed to the methyl protons directly bonded to the pyrene ring. The peaks of the Pt-MAPM complex shifted toward the lower end of the spectrum, which is attributed to the contribution of free electron pairs in the central ion and the formation of the bond between nitrogen and Pt⁴⁺[26], as shown in Fig. 3.
The13C-NMR spectra of the compound (MMAPM) in d6-dimethyl sulfoxide showed a signal at 162.03 ppm attributed to the carbon atoms in the azomethine group. The signal at 165.45 ppm was attributed to carbon atoms C16 and C19 in the pyridine ring. The shift at δ(42.53 and 42.44 ppm) was attributed to the methoxy group (CH3-O) in carbon atoms C25 and C26. The signals at (137.85), (127.64), and (123.45) ppm were attributed to the benzene diamine ring [27]. The 13C-NMR spectrum of Pt+4 (Fig. 4) showed a slight difference in chemical shifts from the ligand spectrum. A chemical shift at δ(166.74 ppm) is attributed to the C9 atom in azomethine [28]. A shift at δ(166.74 ppm) is attributed to the CH3O-C19 atoms in the pyridine rings. Chemical shifts at δ(137.42), 128.80, and 124.42 ppm are attributed to the carbon atoms of the aromatic phenyl ring [29].
The mass spectra of the ligand (MMAPM) and its Pt4+-L complex were obtained in order to compare their stoichiometric composition. The base peak at (m/z+=347) in the mass spectrum of (MMAPM) Fig. 5, a parent ion peak linked to (M.+), is believed to be a reliable indicator of the newly formed ligand. The remaining pieces, along with their respective abundances and fragmentation routes, are shown in Fig. 6. The [PtC20H18N4O2Cl2]Cl2.H2O, similarly produced the [M+] peaks at m/z+ 701, which is consistent with the proposed chemical formula. The predicted chemical formula of the compounds is supported by all of these mass spectrum peak values for ligand and its investigated metal complex. Fig. 6 displays the remaining fragments, their respective abundances, and the Pt-complex’s fragmentation pathways. 

FTIR Spectra of (MMAPM) and its metal Complexes
Infrared spectral data for the Schiff base ligand (MMAPM) were collected and compared with those of its complexes for potential coordination sites in the formation of these complexes, as shown in Figs. 7 and 8. The data included in Table 3 represent the identification of characteristic bands. The ligand spectrum shows the characteristic -C=N band at 1590 cm⁻¹, and this band shifts to lower frequencies in the spectra of the complexes and is observed at 1579, 1578, 1577, 1575, 1581, and 1581 cm⁻¹ in the spectra of the complexes with Co⁺², Ni⁺², Cu⁺², Zn⁺², Pt⁺⁴ and Au⁺³, respectively [30]. This indicates the participation of azomethine nitrogen in the formation of the bond with the metal ions [31].The binding of nitrogen to metal ions reduces the electron density on the azomethine bond, leading to a decrease in the absorption of –C=N-. The bands at 3412 cm⁻¹ for the platinum complex, 3389 cm⁻¹ for the zinc complex, and 3385 cm⁻¹ for the gold complex indicate the presence of water of crystallization molecules [32]. Furthermore, the infrared spectra of these complexes reveal new bands in the 507, 503, 511, 518, 509, and 526 cm⁻¹ regions, which suggest (M-N) binding, respectively [33]. The appearance of (M-N) supports the involvement of a nitrogen atom in the formation of these complexes under study.

Electronic spectra and magnetic measurements
The UV-Vis spectrum of the methyl phosphate group (MMAPM) in Table 4 shows a high-intensity absorption peak at 223, 240, and 291 nm, attributed to (π→π*) transitions. A band at 443 nm is also present, attributed to n→π* transitions of the azomethine nitrogen electron pair to the Schiff base [34]. As these bands shift to higher wavelengths, the azomethine nitrogen binds to the central metal ion during the formation process. Physical evidence for all these observations is found in the red color of the Cobalt ion’s complex. Both bands appearing in Fig. 9 at 596 nm and 672 nm are caused by the 4T1g(F)→4T1g(p) (υ3) and 4T1g(F)→4A2g(F) (υ2) transitions, respectively, with octahedral structures. The Nickel(II) complex has a magnetic moment of 2.950 B.M. These results can be attributed to two visible bands at 749 nm and 634 nm, which indicate the presence of the 3A2g→3T2g(F)(υ1) and 3A2g→3T1g(F) (υ2) electron transitions associated with the octahedral nickel(II) complex [35]. The broad absorption band of Cupper(II) at 685 nm has been attributed to the 2B1g→2A1g, 2B1g→2B2g, and 2B1g→2B2g transitions, with a magnetic moment value of 1.852 B.M, consistent with distorted octahedral structures. The blue-shifted bands in the Zn(II) complex’s spectrum 439 nm indicate that the azomethine group coordinates or is assigned to the dπ(Zn) 2+→ π*(L)(C.T) transition. Electronic spectrum data for the Zn(II) complex shows a octahedral, diamagnetic configuration[26]. Electron spectral data for Platinum(IV) in ethanol were also collected, and when compared to the spectrum of the free ligand, bands at 698 and 582 nm were associated with the 1A1g→1T2g(F) (υ2) and 1A1g→1T1g(p) (υ3) transitions, while the bands at 405 nm confirm the (n→π*) transition. This also confirms the regular octahedral geometry of platinum(IV) [36]. The electronic spectrum of Au(III) complexes shows a band at 794 nm for the 1A1g→1T1g(F) (υ1) transition and a band at 681 nm for the 1A1g→1B1g(υ2) transition. A band at 508 nm indicates the 1A1g→1Eg (υ3) transition, while bands at 402–223 nm indicate intrabond transitions (n→π*). The study shows that the Au(III) complex is non-magnetic and has a planar square shape [37]. With a blue shift in the ligand spectrum (MMAPM) and the appearance of new bands, these complexes exhibit bright colors, indicating symmetry between the ligand and the metal ion. Table 4 shows the basic electronic transitions of the MMAPM ligand and metal complexes.

Conductivity measurements 
The molar conductivity of the studied metal complexes was investigated using absolute ethanol as a solvent at room temperature, as shown in Table 5. The conductivity ratio of the metal complexes with the MMAPM ligand was found to be 0:0, while it was 1:2 with platinum (IV), and 1:3 with gold (III). The values for the other compounds were found to be similar to those obtained for many non-ionic metal compounds [38].

X-ray diffraction study (XRD)
Using X-ray diffraction in the solid state, the ligand (MMAPM) as well as their metal complexes under investigation were examined in the angular range of 2 (5-80°) to ascertain certain structural characteristics, including crystal sizes and structure. To ascertain their purity and the flaws in the crystal structure that arose when the ligands under investigation were transformed into metal complexes, microstrains and dislocation density were also computed. Certain diffraction peaks arise for the reasons listed in : First, microstrain (like lattice deformation); second, faulting due to crystal distortions; Third: The crystal’s domain size; fourth: The domain size distribution [28]. The distance (d spacing) between the crystal planes for the ligand as well as their metal complexes was determined using Bragg’s law [39]. For the ligands and their prepared metal complexes, the X-ray diffraction (XRD) spectra showed a distinct difference in the previously mentioned data of the density of solutes (δ), micro-ductility (Ψ), crystal size (D), and the spacing between the crystal planes (d). We observed an inverse relationship between the crystal size (D), micro-ductility (Ψ), and the density of solutes (δ); as the crystal size increases, the micro-ductility decreases, the density of solutes decreases, and consequently the defects in the crystal decrease. This confirms the occurrence of the coordination process between the ligands and the metal ions under study. Because of micro-tension and crystalline cracking, the lack of sharp peaks suggests the absence of a crystalline network. In X-ray spectroscopy, amorphous structures are indicated by broad peaks, whereas crystalline or semi-crystalline structures are indicated by sharp peaks. The crystalline arrangement, the characteristics of the crystalline network, and the crystalline planes all affect how sharp these peaks are. Furthermore, it was demonstrated to us that all of the ligand and their metal complexes under investigation are in the nano range because their grain sizes are less than 100 nm. The diffraction angles, observed d values, relative intensity, crystal size, crystal intensity, peak widths at mid-intensity, micro-resistance, and dissolution density for each ligand. Displayed in the X-ray spectrum in Table 6 and the metal complexes that are being investigated. The X-ray diffraction spectra of the ligand and their prepared metal complexes are shown in Fig. 10.

FE-SEM analysis
The ligand (MMAPM) and its metal complexes’ surface characteristics, including particle size, shape, aggregates, and distribution, were examined Fig. 11. The irregular fragments particles with an average particle size of 36.41 nm were visible in the FESEM image of the ligand. The Zn(II) complex FESEM image revealed clumped with an average particle size of 40.83 nm and the largest percentage of clusters. The Au(III) complex’s FESEM image revealed heterogeneous crystals with a lower proportion of aggregates particles with an average particle size of 45.62 nm, whereas the Pt(IV) complex’s FESEM image revealed irregular with an average particle size of 380.07 nm [40]. 

Suggested configurations for prepared compounds 
All complexes are octahedral in geometry, with the exception of the gold, palladium, and silver complexes, which are square planar and tetrahedral, respectively, according to the literature on the available coordination sites in the ligand and its relationship with different metal ions [41].These findings were obtained using spectroscopic and analytical methods such as molar ratio diagnostic measurements, elemental analysis, metal content, magnetic measurements, molar conductivity, and UV-visible and Fourier transform infrared spectroscopy. The coordination was established through the nitrogen atoms of the azomethine groups, resulting in five-membered chelate rings that add stability to the formed metal complexes. In all complexes, the ligand uses a bidentate coordination mechanism [42]. The interactions mentioned above are shown in Fig. 12, which was created with Chem. Sketch 2020. These structures exhibit metal to ligand ratios of 1:2 and 1:1, as predicted by our approach.

Antibacterial activity
Pyridine and its derivatives exhibit significant activity in inhibiting numerous pathogenic bacteria and fungi [43]. This is attributed to the ability of its solutions to dissolve the outer cell wall, leading to leakage of cell fluids and cell death. Furthermore, this biologically active ligand contains functional groups within its structure, such as two hybridized nitrogen atoms, enabling it to bind to various elements present in the cell body [44], such as copper, cobalt, iron, zinc, divalent manganese, and monovalent potassium ions, which are essential for bacterial cell function. This results in the formation of complexes with these elements, which in turn cause cell death due to the loss of these elements [45]. The biological activity of the ligand and its metallic compounds under investigation was studied against two different types of pathogenic bacteria, one Gram-positive (S. aureus) and the other Gram-negative (E. coli). Platinum (IV), zinc (I), and gold (III) complexes demonstrated high activity against both Gram-positive and Gram-negative bacteria. The biological activity results showed high inhibitory activity against both types of bacteria used. Inhibition zones (in millimeters) were recorded to study the effects of the ligand and its prepared metal compounds dissolved in 0.1 mg/ml dimethyl sulfoxide (DMSO) on Staphylococcus aureus and Escherichia coli. Table 7 and Fig. 13 show the results.

Molecular docking
The theoretical study used the (MOE) Molecular Operating Environment program to show the molecular docking mechanism of the ligand (MMAPM) Schiff base and its complexes [PtLCl2] Cl2.H2O with lung cancer protein (4JPS). Following molecular docking with the (4JPS) protein, the two compounds showed strong binding affinities with varying degrees of stability in the active pocket. The strongest binding -5.0084 kcal/mol, was achieved with the standard ligand, indicating a stable and well-fitted complex inside the receptor cavity. The other two compounds had less negative values, indicating weaker but still favorable binding interactions.

Docking results for ligand (MMAPM)
Compound (MMAPM) (pose 1) achieved a moderate affinity (-6.90783 kcal/mol) but had the lowest RMSD (1.795422 Å), indicating a highly stable conformation even if the total binding energy was slightly weaker. This suggests a precise geometric fit that could be optimized further to strengthen polar interactions. Moreover it can make hydrogen bond with TYR 836, TRP 780, TRP 780, GLN 859 as displayed in Table 8.

Molecular docking of the compound [PtC20H18N4O2Cl2]Cl2.H2O
The complex [Pt(MMAPM)Cl2]Cl2.H2O exhibited the best docking performance, with a binding affinity of -5.0084 kcal/mol and an excellent RMSD value of 1.643115 Å angstrom, reflecting high stability within the binding pocket. Its interactions included strong hydrogen bonds with the amino acid residues VAL 851 and MET 922, which enhances its stability [46]. The polar and nonpolar interactions make compound the most promising candidate, as it approaches the standard drug-binding efficiency. This good binding pattern with the protein (4JPS) supports its strong inhibitory activity, with an IC50 value of 150 μg/ml [47]. Table 9 and Fig. 14 below illustrate this interaction.

Effect of the ligand (HDF)
The ligand (MMAPM) and its combination with [Pt(MMAPM)Cl2]Cl2.H2O were tested for their anticancer activity against A549 lung cancer cells. Novel bioactive compounds with selective cytotoxicity are important for cancer treatment. Cell viability and the anticancer activity of these compounds were measured using the MTT assay [48]. The results showed that (MMAPM) possesses high inhibitory energy against cancer cells. The inhibition was highest at the highest concentration (400 µg/ml). The inhibition percentage of the ligand and its combination with platinum was 61.04% and 71.38%, respectively, at this dose. At the lowest concentration (25µg/ml), the A549 cell line showed only slight inhibition, at percentages of 25.17% and 24.12%, respectively. The IC₅₀ values also confirmed the selective toxicity of A549 lung cancer cells at 150 µg/ml for (MMAPM) and 197 µg/ml for platinum. For normal (BEAS-2B) cells, the IC₅₀ values were 220 µg/ml.These results indicate that platinum(IV) selectively damages lung cancer cells without affecting normal cells, supporting its potential as a novel anticancer therapy. Table 10 and Fig. 15 illustrate the dose-dependent effects on A549 prostate cancer cells compared to normal (BEAS-2B) cells using the 24-hour MTT assay at 37°C.

CONCLUSION
The complexes in this study were characterized using proton (1H) and (13C) nuclear magnetic resonance, elemental analysis, mineral composition analysis, Fourier transform infrared (FT-IR) and ultraviolet-visible (UV-Vis) mass spectrometry, X-ray diffraction (XRD), and field emission scanning electron microscopy (FE-SEM). Magnetic susceptibility measurements indicated that the octahedral configuration was correct for all complexes except for the gold(III) complex, which exhibited a planar square geometry. The M:L ratio in these structures was 1:1. The bioactivity data for the compounds showed antibacterial and anti-lung cancer properties.

CONFLICT OF INTEREST
The authors declare that there is no conflict of interests regarding the publication of this manuscript.