Antiproliferative Copper(II) Complexes Bearing Mixed Chelating Ligands: Structural Characterization, ROS Scavenging, In Silico Studies, and Anti-Melanoma Activity

Melanoma is a skin cancer characterized by rapid growth and spread for which current therapies produce both resistance and increased risk of infection. To develop new anti-melanoma biocompatible species, the series of complexes Cu(N-N)(bzac)(X)⋅nH2O (N-N: 1,10-phenanthroline/2,2′-bipyridine, Hbzac: 1-phenyl-1,3-butanedione, X: NO3/ClO4, and n = 0, 1) was studied. Single-crystal X-ray diffraction revealed a mononuclear structure for all complexes. The ability of the complexes to scavenge or trap reactive oxygen species such as O2⋅− and HO⋅ was proved by EPR spectroscopy experiments. All complexes inhibited B16 murine melanoma cells in a dose-dependent and nanomolar range, but the complexes with 1,10-phenanthroline were more active. Moreover, comparative activity on B16 and healthy BJ cells revealed a therapeutic index of 1.27–2.24. Bioinformatic methods were used to calculate the drug-likeness, pharmacokinetic, pharmacogenomic, and pharmacodynamic profiles of the compounds. The results showed that all compounds exhibit drug-likeness features, as well as promising absorption, distribution, metabolism, and excretion (ADME) properties, and no toxicity. The pharmacodynamics results showed that the neutral species appear to be good candidates for antitumor molecular targets (Tyrosyl-DNA phosphodiesterase 1, DNA-(apurinic or apyrimidinic site) lyase or Kruppel-like factor 5). Furthermore, the pharmacogenomic results showed a good affinity of the copper(II) complexes for the human cytochrome. These results recommend complexes bearing 1,10-phenanthroline as good candidates for developing drugs to melanoma alternative treatment.


Introduction
Cancer is a difficult disease to treat because both organic and inorganic drugs must have low toxicity and reduced side effects besides efficacy. Among various types of cancers, melanoma is less common than other types of skin cancer, such as keratinocyte carcinomas, but it is more likely to grow and spread [1]. The main environmental risk factor for melanoma development is UV light exposure, which causes genetic mutations in melanocytes [2]. Chemotherapeutic treatment of melanoma includes dacarbazine as a single agent and carboplatin in combination with paclitaxel as combinatory drug therapy [1,3]. These therapies lead to severe side effects, including acquired resistance along with an increased risk of infection. Consequently, challenges and opportunities remain around developing new chemotherapeutics species for melanoma treatment that can overcome the observed deficiencies of current drugs.
Hence, in the constant search for new drugs with lower toxicity and reduced side effects, Cu(II) complexes are preferred, considering their reduced systemic toxicity due to the essential character of this ion [4][5][6][7][8]. Thus, several Cu(II) species with multidentate ligands have been designed as non-toxic species for healthy tissues, but with high activity and selectivity in melanoma cells.
The first Cu(II) complex with such activity arose from the observation that the mechanism of action of elesclomol (esl), a compound active in metastatic melanoma, comprises its complexation with Cu(II) in both extracellular and intracellular fluids. Therefore, the [Cu(esl)] 2+ species is considered to be the active form, and assays against MDA-MB435 melanoma cells yielded a value of half-maximal inhibitory concentration (IC 50 ) of less than 100 nM. Thus, the indirect inhibitory effect of esl is related to Cu(II)-mediated oxidative stress in tumor cells by producing a high level of hydrogen peroxide [9].
In addition, bioinformatic tools [27] were used to predict the drug-like profile, absorption, distribution, metabolism, and elimination (ADME) profiles of the studied compounds [28], with an emphasis on predicting the affinities of molecular targets. Based on our experience in the bioinformatics of new drug candidates [29], we aimed to evaluate the Cu(II) complexes interactions with human antitumor targets.
The C, N, and H chemical analyses were carried out with a EuroEA elemental analyzer. Fourier Transform Infrared spectroscopy (FTIR) spectra were recorded with a Tensor 37 spectrometer (Bruker, Billerica, MA, USA) in the 400-4000 cm −1 range. A Jasco V 670 spectrophotometer (Jasco, Easton, MD, USA) with Spectralon as a standard in the 200-1500 nm range was used to record the UV-Vis spectra in solid-state. A continuous wave X-Band Bruker EMX plus EPR spectrometer (Bruker, Karlsruhe, Germany) equipped with a Bruker X-SHQ 4119HS-W1 X-Band resonator was used for the X-band EPR measurements. The parameters for the X-Band measurements were set as follows: microwave frequency 9.879 GHz, microwave power 6.325 mW, modulation amplitude 0.2 mT, conversion time 74.17 ms, and time constant 40.96 ms at 35 scans. All measurements were carried out at room temperature. Simultaneous Thermogravimetric/Differential Scanning Calorimetry-Mass spectroscopy (TG-DSC/MS) measurements were performed on a TGA/DSC1 Thermal Analyser (Mettler Toledo, Schwarzenbach, Switzerland), coupled to a Vacuum Thermostar Mass Spectrometer (Pfeiffer, Asslar, Germany) under the following conditions: isothermal conditioning at 25 • C, temperature range from 25 to 800 • C, heating rate 5 • C/min, dynamic air atmosphere with a flow rate of 100 mL/min, sample masses of 2-4 mg, 150 µL platinum crucible; empty crucible served as reference. The blank curve was subtracted. Evolved gasses were introduced into the Mass Spectrometer via a 75 cm heated capillary.

Synthesis of Complexes
The complexes (1), (3), and (4) were synthesized as reported [25,26]. The complex [Cu(bzac)(phen)NO 3 ]·H 2 O (2) was prepared as follows: to a solution containing copper(II) nitrate hexahydrate (0.244 g, 1 mmol) in 25 mL ethanol, a solution containing phen (0.180 g, 1 mmol) was added in 10 mL ethanol. The reaction mixture was magnetically stirred at 50 • C for 1 h, and then a solution obtained by dissolving Hbzac (0.162 g, 1 mmol) in 10 mL ethanol was added. The dark green single crystals obtained after the solution stood at room temperature for several days were isolated. The resulting solution was further concentrated, and the obtained microcrystals were filtered off, washed several times with cold ethanol, and dried in air. Yield 86%. Anal. Calcd. for C 22

Crystal Structural Analysis
The structure was solved by direct methods and refined using full-matrix least-squares techniques based on F2. The non-H atoms were refined using anisotropic displacement parameters. The calculations were performed using the crystallographic software package SHELX-2018 [30]. The crystallographic data (excluding structure factors) have been deposited with the Cambridge Crystallographic Data Centre with CCDC reference number 2184808. These data can be obtained free of charge from http://www. USA) were grown in DMEM (Dulbecco's Modified Eagle Medium) supplemented with reagents like MEM. All cell cultivation media and reagents were purchased from Biochrom AG (Berlin, Germany) and Sigma-Aldrich (Darmstadt, Germany).

Cell Viability Assay
Cell viability was evaluated using the MTT assay (3-(4,5-dimethylthiazol-2-yl)-2,5diphenyltetrazolium bromide) as previously described [14]. Briefly, BJ and B16 cells were seeded in 96-well plates at densities of 10,000 cells/well and 7000 cells/well and further cultured in the medium for 24 h. The next day, the investigated compounds were added at a concentration of 1 to 25 µM for 24 and 48 h. The cells cultivated in medium without the studied samples served as negative controls. After incubation for the desired times, the medium was replaced with MTT solution (1 mg/mL) and incubated for an additional 4 h at 37 • C. Finally, the medium was collected, and DMSO was used to dissolve the insoluble formazan product. A Mithras 940 (Berthold, Bad Wildbad, Germany) plate reader was used to measure the absorbance of the samples at 570 nm. The data were corrected for background, and the percentage of viable cells was obtained using the following equation: Half-maximal inhibitory concentration (IC 50 ) was determined by fitting the data with a sigmoidal logistic function using Origin 8.1 (Microcal Inc., Northampton, MA, USA) software.

Cell Cycle Analysis
Twenty-four hours after treatment of B16 cells with concentrations of 1 and 5 µM of each compound, cells were harvested and fixed with pre-chilled 70% ethanol solution at −20 • C. Cells were incubated with 0.2 mg/mL RNAse and 20 µg/mL propidium iodide (PI) in a 0.1% Triton TX-100 solution, in the dark, for 30 min at 37 • C. Cell cycle distribution was analyzed using a Beckman Coulter Cell Lab Quanta SC Flow Cytometer (Indianapolis, IN, USA), and the data were analyzed using the Quanta Analysis software.

Molecular Modeling of Complexes
Starting from the 3D structures of the compounds downloaded as pdb files in the Molecular Operating Environment (MOE) software [31], the Simplified Molecular Input Line Entry (SMILES) file of the compounds for further bioinformatics and cheminformatics analysis was obtained. In addition, the optimized energies of the compounds were determined using the MOE software. The energies of the structures were minimized using Forcefield MMFF94x with a gradient of 0.05. After minimization, the Gasteiger partial charges were applied to all compounds.
Under these rules, bioactive drugs are not expected to violate more than one of the criteria: (i) Lipinski filter-The molecular weight should not exceed 500 g/mol, the partition coefficient between octanol and water (Log P(o/w)) should not exceed 5, the number of hydrogen bond acceptors should not exceed 10, and the number of hydrogen bond donors should not exceed 5; (ii) Ghose filter-The molecular weight should be between 160 and 480 g/mol, the Log P(o/w) should be between −0.4 and 5.6, the molar refractivity should be between 40 and 130 m 3 /mol, and the number of atoms should be between 20 and 70; (iii) Veber rule-the number of rotatable bonds should not be more than 10 and the total polar surface area should not be greater than 140Ǻ 2 , and (iv) Egan filter-The Log P(o/w) should not be more than 5.88 and the total polar surface area should not be greater than 131Ǻ 2 .

Computational Pharmacokinetics and Pharmacogenomics Profiles of Copper(II) Complexes
The SMILES files of copper(II) complexes were used to predict their absorption, distribution, excretion, and toxicity (ADE-Tox) profiles using the pkCSM database [37]. The following criteria were selected for our research: (i) intestinal absorption (percentage)-A molecule with an absorption rate of less than 30% is considered poorly absorbed; (ii) bloodbrain barrier (BBB) permeability represented as log BBB (logarithm of brain-to-plasma drug concentration ratio)-A value greater than 0.3 indicates high BBB permeability, while a value less than 1 indicates low BBB permeability and (iii) substrate of renal organic cation transporter 2 (OCT2), the primary renal uptake transporter expressed on the basolateral side of the proximal tubule. The predicted toxic profile of the compounds was a significant aspect of our research. We assessed AMES toxicity, hepatotoxicity, cardiotoxicity, and median lethal dose (LD 50 ).
Considering the Pharmacogenomics Profiles of molecular complexes, we investigated the potential of the compounds to serve as inhibitors or substrates for cytochromes involved in the metabolism of many antitumor drugs, such as CYP2D6, CYP3A4, CYP1A2, CYP2C19, and CYP2C9, to predict their pharmacogenomic profile.

Compounds' Computational Pharmacodynamic Profiles
The pharmacodynamic features and possible molecular mechanisms by which copper(II) complexes modulate human enzymes involved in cancer are less represented in bioinformatics and pharmaceutical databases. In this context, the SuperPred database [38] was used to establish the probability of binding copper(II) complexes to enzymes involved in antitumor treatments based on logistic regression machine learning models. The binding data and resulting model accuracy are based on 646 human targets. In addition, therapeutic indications of the predicted targets [39] were identified.

Results and Discussion
The stepwise reaction of copper perchlorate or nitrate with 1,10-phenanthroline (phen)/2,2 -bipyridine (bpy) and 1-phenyl-1,3-butanedione (Hbzac) in a molar ratio of 1:1:1 gave the complexes [Cu(bzac)(phen)X]·nH 2 O (X: ClO 4 , n = 0 (1); X: NO 3 , n = 1 (2) (1) (2) All complexes are mononuclear species in which both organic ligands act as a chelate. In all complexes, the oxyanion behaves unidentate, except for complex (3), where perchlorate is present as a free ion. As a result, except for complex (3), which is an ionic species, the other ones are neutral. The Cu(II) adopts a distorted square pyramidal stereochemis- The compound [Cu(bzac)(phen)NO 3 ]·H 2 O (2) was fully characterized as a mononuclear species by single-crystal X-ray diffraction. On the other hand, elemental analysis, IR spectra, and single-crystal X-ray data confirmed the identity of the other complexes with the species reported in the literature [25,26].
All complexes are mononuclear species in which both organic ligands act as a chelate. In all complexes, the oxyanion behaves unidentate, except for complex (3), where perchlorate is present as a free ion. As a result, except for complex (3), which is an ionic species, the other ones are neutral. The Cu(II) adopts a distorted square pyramidal stereochemistry, except for complex (3), where the surrounding is square planar ( Figure 1).
We further characterized the compounds by solid-state IR, UV-Vis, EPR spectroscopy, and TGA/DSC MS analysis, and tested their antiproliferative activity. (2) X-ray diffraction on single crystals for compound (2) reveals the presence of a mononuclear unit that crystalizes with one water molecule ( Figure 2). A summary of the crystallographic data and the structure refinement are given in Table 1. The [Cu(bzac)(phen)NO 3 ] mononuclear species contain the metal ion in a square pyramid surrounding, with the two oxygen atoms from the benzoylacetonato ligand, and the two nitrogen atoms from 1,10-phenanthroline in the basal plane, at distances similar to the ones encountered in other mononuclear units [Cu1-O1 = 1.901(3); Cu1-O2 = 1.909(3); Cu1-N1 = 1.997(4); Cu1-N2 = 2.000(3) Å] [40,41]. The nitrate ligand is coordinated, through its oxygen atom as a terminal ligand, into the apical position [Cu1-O3 = 2.370(4) Å]. Selected bond distances are collected in Table 2.   (2)

Physico-Chemical Characterization of Complexes
The IR spectra of the compounds are very complex in the 400-1700 cm −1 range due to the overlapping of the bands of the three ligands, Hbzac, phen/bpy, and ClO4/NO3 oxyanions. Interestingly, the neutral species are linked through hydrogen bonds between the water molecule hydrogen and noncoordinated oxygen atom from nitrate anion, [O1w···O5 = 2.968 Å], leading to a supramolecular dimer (Figure 3b). The copper-copper separation within the dimer is Cu···Cu = 12.541 Å.

FT-IR Spectra
The IR spectra of the compounds are very complex in the 400-1700 cm −1 range due to the overlapping of the bands of the three ligands, Hbzac, phen/bpy, and ClO 4 /NO 3 oxyanions.
Compared to the spectra of the two ligands, the spectra of the complexes exhibit multiple bands assigned to overlapping (C=N) and (C=C) stretching vibrations in the 1560-1590 and 1425-1485 cm −1 ranges (Table S1). In the spectra of the complexes, the band associated with the delocalized keto-enol bonds appears in the range of 1600 cm −1 [42]. The spectrum of (1) displays the pattern of unidentate coordination of perchlorate with bands assigned to stretching vibrations ν 3 and ν 4 split in two components and the appearance of a band characteristic for ν 1 vibration at 960 cm −1 . The perchlorate function of a free ion in compound (3) is confirmed by the presence of the characteristic bands at 1090 and 620 cm −1 , arising from the ν 3 and ν 4 stretching vibrations, respectively [43].
Instead, the spectra of both nitrate species exhibit the pattern characteristic of unidentate behavior. Thus, two components appear in the region characteristic of ν 1 vibration and only one for the other three, but these are shifted compared to the ionic species [43].
The supplementary band at 3475 cm −1 in the spectrum of (2) was assigned to a hydrated water molecule. In addition, the low-intensity bands in the 430-460 cm −1 range were assigned to the (Cu-N) and (Cu-O) stretching vibrations, respectively [42].

UV-Vis Spectra
The solid-state UV-Vis spectra of the complexes overlapped with those of the corresponding ligands are presented in In addition, the spectra of both organic ligands exhibit two or three bands below 350 nm in the UV region assigned to n→π* and π→π* transitions. In all complexes, these appear as superimposed bands between Hbzac and phen or bpy and are shifted to either lower or higher wavelengths due to coordination.

EPR Spectroscopy Solid State EPR Spectroscopy
The powder Cu(II) complexes were studied using EPR spectroscopy. The measured EPR spectra are presented in Figure 5. All spectra present similar characteristics, with an axial g tensors g around 2.44 and g ⊥ = 2.07 values characteristic of Cu(II) ions either in a square pyramidal (complexes (1), (2), and (4)) or a square-planar stereochemistry (complex (3)) as already reported in the literature [46][47][48]. Due to a strong spin-spin exchange interaction, no hyperfine structure is observed at room temperature, which disappears in the relatively broad line width.  In addition, the spectra of both organic ligands exhibit two or three bands below 350 nm in the UV region assigned to n→π* and π→π* transitions. In all complexes, these appear as superimposed bands between Hbzac and phen or bpy and are shifted to either lower or higher wavelengths due to coordination.

Solid State EPR Spectroscopy
The powder Cu(II) complexes were studied using EPR spectroscopy. The measured EPR spectra are presented in Figure 5. All spectra present similar characteristics, with an axial g tensors g‖ around 2.44 and g⊥ = 2.07 values characteristic of Cu(II) ions either in a square pyramidal (complexes (1), (2), and (4)) or a square-planar stereochemistry (complex (3)) as already reported in the literature [46][47][48]. Due to a strong spin-spin exchange interaction, no hyperfine structure is observed at room temperature, which disappears in the relatively broad line width.

Solution EPR Spectroscopy
The Cu(II) complexes were dissolved in DMSO at a final concentration of 1 mM. Figure 6 shows the EPR spectra of the complexes in solution after one week. All four complexes show excellent stability in solution, which is essential for measurements on cells where the complexes are incubated for two days or longer. All four compounds show relatively broad spectra in solution due to the already mentioned spin-spin exchange interaction between the Cu(II) centers, with an axial g-value of g = 2.12 and g ⊥ = 2.06. Compared with the g-values determined with EPR on the compounds in solid-state, they stay almost unchanged, indicating that the complexes structure is preserved in solution.
The small shifts in the g-values are due to the changes in the correlation times, which are strongly influenced by the mobility of the molecules. The four normally visible hyperfine lines that should arise from the hyperfine interaction of the Cu(II)-paramagnetic centers with the copper nuclear spin ICu = 3/2 are not observable due to the broadening of the spectra. Pharmaceutics 2022, 14, 10 of 22

Solution EPR Spectroscopy
The Cu(II) complexes were dissolved in DMSO at a final concentration of 1 mM. Figure 6 shows the EPR spectra of the complexes in solution after one week. All four complexes show excellent stability in solution, which is essential for measurements on cells where the complexes are incubated for two days or longer. All four compounds show relatively broad spectra in solution due to the already mentioned spin-spin exchange interaction between the Cu(II) centers, with an axial g-value of g‖ = 2.12 and g⊥ = 2.06. Compared with the g-values determined with EPR on the compounds in solid-state, they stay almost unchanged, indicating that the complexes structure is preserved in solution.

Solution EPR Spectroscopy
The Cu(II) complexes were dissolved in DMSO at a final concentration of 1 mM. Figure 6 shows the EPR spectra of the complexes in solution after one week. All four complexes show excellent stability in solution, which is essential for measurements on cells where the complexes are incubated for two days or longer. All four compounds show relatively broad spectra in solution due to the already mentioned spin-spin exchange interaction between the Cu(II) centers, with an axial g-value of g‖ = 2.12 and g⊥ = 2.06. Compared with the g-values determined with EPR on the compounds in solid-state, they stay almost unchanged, indicating that the complexes structure is preserved in solution.

Thermal Behavior
The thermal behavior of the complexes was studied using the simultaneous TGA/DSC technique in air coupled with MS analysis to detect the evolved gases. The data are summarized in Table S2.
From the measured curves of all complexes in Figure 7, it is evident that the thermal decomposition process and its pattern are determined by the inorganic ligands, the perchlorate, and the nitrate anion. The decomposition of the complexes containing the perchlorate ion is shifted toward higher temperatures, and the shape of the exothermic peak in the first stage corresponds to an intense and explosive breakdown. The nitrate anion complexes follow a different pattern (Figure S1a,b). The organic ligands are released before the inorganic ions; they decompose exothermically in the last step. The residue of all decomposition pathways in air is an inorganic CuO.
TGA/DSC technique in air coupled with MS analysis to detect the evolved gases. The data are summarized in Table S2.
From the measured curves of all complexes in Figure 7, it is evident that the thermal decomposition process and its pattern are determined by the inorganic ligands, the perchlorate, and the nitrate anion. The decomposition of the complexes containing the perchlorate ion is shifted toward higher temperatures, and the shape of the exothermic peak in the first stage corresponds to an intense and explosive breakdown. The nitrate anion complexes follow a different pattern ( Figure S1a,b). The organic ligands are released before the inorganic ions; they decompose exothermically in the last step. The residue of all decomposition pathways in air is an inorganic CuO. The most thermally stable is complex (3), in which perchlorate is present as a free ion that initiates its explosive exothermic decomposition at an onset temperature of 292 °C and ends it in a narrow temperature range at 320 °C. The MS spectra show ( Figure S2c  The most thermally stable is complex (3), in which perchlorate is present as a free ion that initiates its explosive exothermic decomposition at an onset temperature of 292 • C and ends it in a narrow temperature range at 320 • C. The MS spectra show ( Figure S2c, Table S2) the exuberant mass fragmentation characteristic of both organic ligands; moieties from bzac (C 4 H 5 O (m/z 68), C 6 H 5 (m/z 77, 78), (m/z 105, 85, 43), (m/z 51, 50), and moieties from bpy (C 5 H 6 N (m/z 78, 79), (m/z 51, 52, 50), whose combustion is accompanied by released water (m/z 17, 18) and carbon dioxide (m/z 44). In the subsequent exothermic process up to 600 • C, the mass peaks typical of the perchlorate ion Cl (m/z 35), CHCl (m/z 49), ClO (m/z 51, 52), and Cl 2 (m/z 70) are strongly pronounced, and also carbon dioxide without water, indicating that the organic matter was burned to carbon black in the first step. The mass peak m/z 35, present in both decomposition stages, confirms the presence of perchlorate decomposition in the first step, as it is not characteristic of organic ligands.
Complex (1), thermally stable up to 125 • C, follows the pattern of perchlorate combustion and rapidly loses its mass up to 292 • C (Figure 7 and Figure S1a). The moiety of the organic ligands bzac and phen (C 6 H 13 N 2 (m/z 112, 113, 63, 50)) is slowly released over a further 60 • C ( Figure S2a) as m/z 78, 77, 51, and 50 peaks are formed when exothermic decomposition of the remaining organic matter occurs at 352 • C, releasing water and carbon dioxide as by-products as well as perchlorate decomposition, ending at 569 • C.
The multi-step decomposition of the nitrate complex (2) (Figure 7) starts at 155 • C and is accelerated at 214 • C by the decomposition of the organic ligands. Characteristic mass peaks (Table S2, Figure S2b) correspond to the moieties of bzac and phen and the release of nitrogen dioxide (m/z 30, 46), water, and carbon dioxide. The transformation at 304 • C shows the onset of exothermic decomposition of the nitrate anion and the remaining organic moieties, completed at 509 • C.
However, the nitrate species (4) (Figure 7) is the first to undergo exothermic decomposition at 150 • C, with mass peaks ( Figure S2d) corresponding to the moieties of bzac, which are further overlaid by peaks of bpy (Table S2). Mass peaks above 304 • C indicate exothermic decomposition of the remaining organic moieties, completed at 538 • C. In all decomposition steps, water and carbon dioxide are released.

Antiproliferative Activity
Cell viability was evaluated for all compounds at 24 and 48 h against BJ normal skin and murine B16 melanoma cells. The viability curves for all experimental conditions are presented in Figure 8.
However, the nitrate species (4) (Figure 7) is the first to undergo exothermic decomposition at 150 °C, with mass peaks ( Figure S2d) corresponding to the moieties of bzac, which are further overlaid by peaks of bpy (Table S2). Mass peaks above 304 °C indicate exothermic decomposition of the remaining organic moieties, completed at 538 °C. In all decomposition steps, water and carbon dioxide are released.

Antiproliferative Activity
Cell viability was evaluated for all compounds at 24 and 48 h against BJ normal skin and murine B16 melanoma cells. The viability curves for all experimental conditions are presented in Figure 8. The results show that all compounds have slightly enhanced cytotoxicity towards the cancer cell line compared to the normal cell line, but these affect the cells differently. Thus, complexes (1) and (2) containing 1,10-phenanthroline as a ligand behave similarly ( Figure  8A, B). As can be seen, cell viability rapidly decreases to 20% in BJ cells and 10% in B16 cells treated with a concentration of 10 μM of the complexes. Exposure to higher concentrations, up to 25 μM, induces minor changes in cell viability, reaching about 15% for BJ cells and about 5% for B16 cells for both compounds. Furthermore, IC50 values were determined for the two compounds, as indicated in Table 3. Table 3. The half-maximal inhibitory concentration (IC50) and therapeutic index (TI) of the studied complexes. The results show that all compounds have slightly enhanced cytotoxicity towards the cancer cell line compared to the normal cell line, but these affect the cells differently. Thus, complexes (1) and (2) containing 1,10-phenanthroline as a ligand behave similarly ( Figure 8A,B). As can be seen, cell viability rapidly decreases to 20% in BJ cells and 10% in B16 cells treated with a concentration of 10 µM of the complexes. Exposure to higher concentrations, up to 25 µM, induces minor changes in cell viability, reaching about 15% for BJ cells and about 5% for B16 cells for both compounds. Furthermore, IC 50 values were determined for the two compounds, as indicated in Table 3.  (1) is somewhat more toxic to melanoma cells than to normal skin cells.
This aspect can also be observed from the therapeutic index (TI) calculated and presented in Table 3. The TI was 1.13 after 24 h and 1.27 after 48 h for compound (1). Considering the similarities between compounds (1) and (2), the TI values for compound (2) are close to those found for compound (1 (Table 3).
Compounds (3) and (4) containing bpy have a different effect on cell lines BJ and B16 than compounds (1) and (2). These compounds affect the cells' viability in a dosedependent manner, with a slight decrease with increasing concentrations (Figure 8C,D). For both compounds, the viability of B16 cells was more affected than that of BJ cells.
IC 50 (Table 3). These values are close to those found for compound (3). Calculating the TI values, we found that compound (4) also had higher efficiency after 48 h of treatment. TI calculated values were 1.82 after 24 h and 2.19 after 48 h.
Various studies on copper(II) complexes with N-N heterocycle ligands have indicated their potential antitumor activity in the micromolar range [16,18,[49][50][51]. Similar results were reported for complexes with both N-N heterocycle and Hbzac, such as (1) and (3), which were significantly more cytotoxic against MKN-45 cells than 5-fluorouracil after 48 h of incubation [25]. Moreover, Cu(II) species with other β-diketonates proved activity against the chronic myelogenous leukemia cell line [52].
Based on these results, it is evident that Cu(II) complexes with 1,10-phenanthroline are more active than 2,2'-bipyridine complexes, and these results agree with other reported data [16][17][18]49,52,53]. These data have been associated with the enhanced intercalation abilities of this aromatic system.

Effect of Copper(II) Complexes on Cell Cycle Distribution
Considering that the copper(II) complexes can interact with DNA, as mentioned earlier [54], we were interested in verifying whether and how the compounds can interfere with the cell cycle progression. Based on the viability results and the IC 50 values reported above, we were interested in examining the effect of the compounds at concentrations less than 5 µM values to keep enough cells alive. Cell cycle analysis was performed for tumor cells. Figure 9 shows the results for B16 cells treated with concentrations of 1 µM and 5 µM of each of the four compounds. The untreated cells, shown as the percentage of cells in each phase, have a distribution of 49.70% in the G0/G1 phase, 25.65% in the S phase, 15.53% in the G2/M phase, and 9.11% in the sub-G1 phase. When treated with compounds (1) and (2), we see that the cell cycle distribution of B16 cells is affected ( Figure 9A,B).
For both compounds, the lower concentration of 1 µM did not significantly alter the cell cycle distribution. However, when B16 cells were treated with 5 µM, we found that both compounds induced cell cycle arrest in the G0/G1 phase and increased the cells in the sub-G1 phase.
Compound (1) showed a significant increase (60.14%) of cells in the G0/G1 phase (p < 0.001) when treated with 5 µM (Figure 9A). This increase was followed by a significant decrease in the S (15.82%) and G2/M phase (5.59%) (p < 0.001) compared to the control cells. In addition, a significant increase (18.43%) in the sub-G1 populations was also observed (p < 0.001). The results indicate that compound (1) induced G0/G1 cell cycle arrest at a concentration of 5 µM and that the cells also underwent apoptosis. 15.53% in the G2/M phase, and 9.11% in the sub-G1 phase. When treated with compo (1) and (2), we see that the cell cycle distribution of B16 cells is affected ( Figure 9A,B For both compounds, the lower concentration of 1 μM did not significantly alt cell cycle distribution. However, when B16 cells were treated with 5 μM, we found both compounds induced cell cycle arrest in the G0/G1 phase and increased the ce the sub-G1 phase. Compound (1) showed a significant increase (60.14%) of cells in the G0/G1 ph < 0.001) when treated with 5 μM ( Figure 9A). This increase was followed by a signi decrease in the S (15.82%) and G2/M phase (5.59%) (p < 0.001) compared to the co cells. In addition, a significant increase (18.43%) in the sub-G1 populations was als served (p < 0.001). The results indicate that compound (1) induced G0/G1 cell cycle at a concentration of 5 μM and that the cells also underwent apoptosis.
It is known from previous studies that the cell cycle progression is regulated series of checkpoints that assess whether a cell can progress with division [46,47]. Th most essential checkpoints are the G1 checkpoint, which allows cells to transition fro G1 to S phase, where DNA synthesis occurs, and the G2 checkpoint, which allows c For compound (2), when cells were treated with 5 µM, the percentage of cells that were in the G0/G1 phase significantly increased to 54.90% (p < 0.05), while cells in the S and G2/M phase significantly decreased to 13.81% (p < 0.001) and 10.78% (p < 0.05), respectively. Like compound (1), after treating B16 cells with compound (2), the percentage of cells that were in the sub-G1 phase significantly increased to 24.49% (p < 0.001).
It is known from previous studies that the cell cycle progression is regulated by a series of checkpoints that assess whether a cell can progress with division [46,47]. The two most essential checkpoints are the G1 checkpoint, which allows cells to transition from the G1 to S phase, where DNA synthesis occurs, and the G2 checkpoint, which allows cells to transition from the G2 to M phase, where daughter cell formation by mitosis occurs [55,56].
The G1 checkpoint is activated after detecting DNA damage, among other events, and prevents these cells from transitioning to the S phase. An increase in the number of cells in the sub-G1 phase indicates cells with damaged DNA that have been unable to repair it and have undergone apoptosis. Based on the reported results, we can say that compounds (1) and (2) can induce DNA fragmentation followed by cell cycle arrest in G0/G1 phase, which eventually leads B16 melanoma cells into apoptosis. Similar findings were previously reported for other copper(II) complexes that caused both G0/G1 cell cycle arrest and apoptosis in various cells [49,54,57,58].
Surprisingly, no changes in the cell cycle were observed for compounds (3) and (4), or when B16 cells were treated with 1 µM or 5 µM. Figure 10 shows the EPR spectra of the compounds dissolved in DMSO at 100 µM before and after adding KO 2 and H 2 O 2 as ROS O 2 · − and HO· donors, respectively. The measurements show that compounds (1), (2), and (3) exhibit a scavenging response in the presence of O 2 · − radicals by changing the oxidation state of the copper centers, while compound (4) shows no changes in its EPR spectrum, indicating that this compound has neither scavenging nor a trapping ability toward superoxide radicals. In contrast, all compounds in the presence of HO· radicals show the trapping ability of these radicals, as indicated by the additional EPR signals in all four EPR spectra.

Complexes Interaction with ROS
repair it and have undergone apoptosis. Based on the reported results, we can say that compounds (1) and (2) can induce DNA fragmentation followed by cell cycle arrest in G0/G1 phase, which eventually leads B16 melanoma cells into apoptosis. Similar findings were previously reported for other copper(II) complexes that caused both G0/G1 cell cycle arrest and apoptosis in various cells [49,54,57,58].
Surprisingly, no changes in the cell cycle were observed for compounds (3) and (4), or when B16 cells were treated with 1 μM or 5 μM. Figure 10 shows the EPR spectra of the compounds dissolved in DMSO at 100 µ M before and after adding KO2 and H2O2 as ROS O2 -and HO donors, respectively. The measurements show that compounds (1), (2), and (3) exhibit a scavenging response in the presence of O2 -radicals by changing the oxidation state of the copper centers, while compound (4) shows no changes in its EPR spectrum, indicating that this compound has neither scavenging nor a trapping ability toward superoxide radicals. In contrast, all compounds in the presence of HO radicals show the trapping ability of these radicals, as indicated by the additional EPR signals in all four EPR spectra. The Cu(II) complexes (1)-(3), which exhibit superoxide scavenging abilities, can be reduced inside of the tumor cells by this anion to corresponding Cu(I) species (reaction 1) [59,60]. These Cu(I) complexes can be involved further either in hydrogen peroxide generation (reaction 2) or in its reduction to hydroxyl radical (reaction 3, Fenton-like reaction).

Complexes Interaction with ROS
[Cu(II) (N-N) On the other hand, the highly reactive hydroxyl radical can induce the DNA cleavage, thus triggering the tumor cell apoptosis.

Drug-Likeness, Pharmacokinetics, and Pharmacogenomics Profiles of the Compounds
The results generated from the medicinal chemistry filtering (Lipinski, Ghose, Veber, and Egan) and ADME-Tox analyses are represented in Table 4. Our results show that compounds (2)-(4) comply with the drug-likeness rules, indicating that these compounds have a possible drug effect and good bioavailability. Even though compound (1) has a molecular weight greater than 500 and the Ghose filter does not apply to compound (1), we believe that compound (1) can also be included in the analysis. Furthermore, the ADME-predictable properties of the Cu(II)-based complexes were evaluated (Table 5). We evaluated the ADME-Tox characteristics, with emphasis on (i) intestinal absorption, (ii) BBB and CNS permeability, considering that these compounds are planned to be used in antitumor therapies, and (iii) the type of cytochrome for which these compounds are substrates/inhibitors and a renal organic cation transporter 2 (OCT2) substrate. Table 5 also quantifies the predicted toxicity of the complexes. The results revealed that (i) all compounds (1)-(4) exhibited excellent intestinal absorption, with compounds (2) and (4) exhibiting outstanding intestinal absorption.
For the BBB permeability considered, we noticed that the complexes recorded good BBB permeability values (log BBB varied from −0.988 to −0.714). All complexes have a reasonable CNS permeability, varying from −3.118 to −1.976. Among the compounds analyzed, compound (2) showed suitable permeability for BBB and good permeability in the nervous system. Significant results were recorded for the elimination rate, demonstrating that compounds (3) and (4) are not renal OCT2 substrates.
In this study, great importance was given to the prediction of the toxicity of the compounds. The results revealed that: (i) none of the compounds (2)-(4) exhibited AMES toxicity, (ii) compounds (1), (3), and (4) did not induce immunotoxicity, but compounds (2)-(4) appeared as hepatotoxic species. Very important, the LD 50 was predicted, the values being in the range 2.968 and 2.672. Hence, a pharmacogenomic profile of the active compounds was generated ( Table 6). The results regarding metabolic pathways showed that Cu(II) complexes are not CYP2D6 substrates/inhibitors, but all compounds are CYP3A4 substrates except CYP3A4 inhibitors (except compound (4)). Regarding the affinities of compounds (1)-(4) to CYP1A2, CYP2C19, or CYP2C9, we mentioned that compound (2) inhibits all three cytochromes, but compounds (3) and (4) have no inhibitory activities of these targets. From the SuperPred database, we extracted the most significant molecular targets for compounds (1)-(4). We selected the molecular targets with model accuracy greater than 70% and a probability of interaction of at least 90% (Table 7).
We note that the common molecular targets for all compounds were Transcription intermediary factor 1-alpha and Kruppel-like factor 5, whereas Monoamine oxidase A was predicted to be the target for compounds (1), (2), and (4); Tyrosyl-DNA phosphodiesterase 1 was the target for compounds (1), (3), and (4). Literature data mentioned that the Transcription intermediate factor 1-alpha is critically involved in the tumorigenic process [61][62][63]. Additionally, recent studies have mentioned the role and regulation of Kruppel-like factor 5 (KLF5 transcription factor) in cancers [64,65].
From the database SuperPred, the most significant important molecular targets for all complexes were extracted. The molecular targets with more than 70% model accuracy and a probability of interaction not less than 90% were selected (Table 7).

Conclusions
A series of copper perchlorate or nitrate complexes with mixed ligands 1,10-phenanthroline/2,2bipyridine and 1-phenyl-1,3-butanedionate were developed as biologically active species. These were characterized as mononuclear, neutral, or ionic species based on single-crystal X-ray diffraction data. The EPR studies evidenced the complexes' ability to scavenge ROS species, O 2 − and HO. Compounds with 1,10-phenanthroline have the potential to be developed as antitumor agents, considering their efficacy at concentrations around 5 µM and their ability to induce apoptosis in treated cells. Furthermore, compounds (1) and (2) could be considered in further pharmacological and pharmacokinetic studies due to their lower cytotoxic on the healthy cell line. As more information is needed regarding their efficacy against various other cancers, a new study involving a larger number of healthy and cancerous cell lines can be considered. Bioinformatic tools elucidated the pharmacological profile of the compounds, including important criteria of pharmacokinetic/pharmacodynamics profiles, and important pieces of information about molecular target affinities of compounds were collected. Our results showed that all Cu(II) complexes presented drug-like features, representing an important step when a new compound is proposed as a therapeutic species. Pharmacokinetic properties conclude that studied complexes are not significantly toxic, have a good BBB permeability, and, very importantly, present a good intestinal absorption. Regarding the predicted pharmacodynamic profile of compounds, we concluded that all complexes presented affinities for Transcription intermediary factor 1-alpha, and Kruppel-like factor 5 (KLF5 transcription factor), both critically involved in cancer evolution.