Bioinorganic Chemistry and Applications

Bioinorganic Chemistry and Applications / 2018 / Article

Research Article | Open Access

Volume 2018 |Article ID 7176040 | 22 pages |

Synthesis of Novel VO(II)-Perimidine Complexes: Spectral, Computational, and Antitumor Studies

Academic Editor: Spyros P. Perlepes
Received12 Jan 2018
Accepted26 Apr 2018
Published06 Sep 2018


A series of perimidine derivatives (L1–5) were prepared and characterized by IR, 1H·NMR, mass spectroscopy, UV-Vis, XRD, thermal, and SEM analysis. Five VO(II) complexes were synthesized and investigated by most previous tools besides the theoretical usage. A neutral tetradentate mode of bonding is the general approach for all binding ligands towards bi-vanadyl atoms. A square-pyramidal is the configuration proposed for all complexes. XRD analysis introduces the nanocrystalline nature of the ligand while the amorphous appearance of its metal ion complexes. The rocky shape is the observable surface morphology from SEM images. Thermal analysis verifies the presence of water of crystallization with all coordination spheres. The optimization process was accomplished using the Gaussian 09 software by different methods. The most stable configurations were extracted and displayed. Essential parameters were computed based on frontier energy gaps with all compounds. QSAR parameters were also obtained to give another side of view about the biological approach with the priority of the L3 ligand. Applying AutoDockTools 4.2 program over all perimidine derivatives introduces efficiency against 4c3p protein of breast cancer. Antitumor activity was screened for all compounds by a comparative view over breast, colon, and liver carcinoma cell lines. IC50 values represent promising efficiency of the L4-VO(II) complex against breast, colon, and liver carcinoma cell lines. The binding efficiency of ligands towards CT-DNA was tested. Binding constant (Kb) values are in agreement with the electron-drawing character of the p-substituent which offers high Kb values. Also, variable Hammett’s relations were drawn.

1. Introduction

Vanadium was widely used as a therapeutic agent in the late eighteenth century, treating a variety of ailments including anemia, tuberculosis, rheumatism, and diabetes [1, 2]. Vanadium compounds exhibit various biological and physiological effects in the human body. Vanadium compounds have been extensively studied for their diverse biological activities such as antitumor, antibacterial, and insulin-enhancing effects and potential capabilities as DNA structural probes [3, 4]. The coordination chemistry of oxovanadium is highly ligand dependent and more important in biological systems [5] as well as catalytic systems [6, 7]. Due to the d1 configuration, vanadium(IV) ionic species are easily identified by EPR spectroscopy. Due to less toxicity [8, 9], the Schiff base complexes of the vanadyl ion are topic of many research reports [10, 11]. In Europe, vanadium is often used as a natural treatment for diabetes. Vanadium has been found in human studies to imitate the effects of insulin in our bodies. This ability may be useful for some of those with diabetes, a natural method to help lower blood sugar, take less insulin, or in some instances stop taking insulin altogether [12, 13]. It is noticeable that complexation of vanadium with organic ligands minimizes unfavorable effects of its inorganic salts such as vanadyl sulfate while even maintains its potential benefits [14]. Furthermore, mimicking the biological activities in natural systems can be achieved by vanadium complexes which contain oxygen and nitrogen donor ligands; so identification of the structure of these complexes is regarded important [1517]. Bioinorganic chemistry is a fast developing field of modern chemistry that uses Schiff bases and their transition metal complexes for a variety of applications, e.g., in biological, medical, and environmental sciences. This work is interested in preparation of a series of perimidine derivatives by various substituents. New vanadyl complexes will be prepared and well characterized by using different techniques. CT-DNA binding will be tested along the organic series. Theoretical implementation will be accomplished over all prepared compounds by different standard programs. Antitumor activity will be scanned over all new prepared compounds for comparison.

2. Experimental Work

2.1. Chemicals Used

Chemicals essential for preparation of perimidine derivatives such as 1,8-diaminonaphthalene, ethylbenzoyl acetate, 4-methoxyaniline, aniline, 4-chloroaniline, 3-chloroaniline, 4-nitroaniline, NaNO2, NaOH, HCl, and dioxane were purchased from Fluka and used without previous treatments. Also, VOSO4·xH2O salt used for the complexation process was commercially available from Sigma-Aldrich. All handled solvents were from Merck and used without previous purification.

2.2. Synthesis
2.2.1. Synthesis of Compounds 3a–e (Perimidine Derivatives)

Ligands 3a–e were synthesized as reported in the literature [18] from coupling reaction of compound 1 (2.5 mmol) in ethanol (20 mL) with the appropriate arenediazonium chloride 2 in the presence of sodium hydroxide (2.5 mmol) in the ice bath at 0–5°C. The whole mixture was then left in a refrigerator overnight. The precipitated solid was filtered off, washed with water, and finally crystallized from dioxane/EtOH to give the respective hydrazones 3a–e (Scheme 1). 1H·NMR and mass spectra are displayed in Figures 1, 2, S1, and S2. The analysis is matching completely with that reported in the literature [16]. The structural forms of new perimidine compounds are displayed in Figures 3(a) and 3(b).

(1)2-[N-phenyl-2-oxo-2-phenylethanehydrazonoyl]-1H-perimidine ( 3a ) (L1). IR υ: 3402, 3194 (2NH), and 1616 (CO) cm−1. 1H·NMR (DMSO-d6) d: 6.72–7.80 (m, 16H, Ar–H) and 13.62 (s, 2H, 2NH). MS m/z (%): 390 (M, 22), 285 (2), 166 (5), 140 (7), 127 (1), 105 (100), 93 (8), and 77 (35). Anal. calcd. for C25H18N4O (390.42).(2)2-[N-(4-methoxyphenyl)-2-oxo-2-phenylethanehydrazonoyl]-1H-perimidine ( 3b ) (L2). IR υ: 3333, 3167 (2NH), and 1680 (CO) cm−1. 1H·NMR (DMSO-d6) δ: 3.58 (s, 3H, OCH3), 7.59–7.97 (m, 15H, ArH), and 12.20 (br s, 2H, 2NH). MS m/z (%): 420 (M, 5), 419 (9), 193 (12), 166 (12), 126 (14), 107(17), 105 (100), 92 (31), and 77 (75). Anal. calcd. for C26H20N4O2 (420.47).(3)2-[N-(4-chlorophenyl)-2-oxo-2-phenylethanehydrazonoyl]-1H-perimidine ( 3c ) (L3). IR υ: 3422, 3206 (2NH), and 1612 (CO) cm−1. 1H·NMR (DMSO-d6) d: 6.73–7.77 (m, 15H, Ar–H) and 13.27 (s, 2H, 2NH). MS m/z (%): 426 (M 2, 5), 425 (M 1, 6), 424 (M, 14), 140 (4), 127 (5), 111 (2), 105 (100), and 77 (37). Anal. calcd. for C25H17ClN4O (435.44).(4)2-[N-(4-nitrophenyl)-2-oxo-2-phenylethanehydrazonoyl]-1H-perimidine ( 3d ) (L4). IR υ: 3356, 3198 (2NH), and 1670 (CO) cm−1. 1H·NMR (DMSO-d6) d: 6.64–8.21 (m, 15H, Ar–H) and 12.60 (s, 2H, 2NH). MS m/z (%): 435 (M, 8), 238 (34), 138 (13), 167 (11), 106 (45), 105 (58), 93 (100), 77 (44), and 66 (76). Anal. calcd. for C25H17N5O3 (424.88).(5)2-[N-(3-chlorophenyl)-2-oxo-2-phenylethanehydrazonoyl]-1H-perimidine ( 3e ) (L5). IR υ: 3229, 3167 (2NH), and 1622 (CO) cm−1. 1H·NMR (DMSO-d6) d: 6.70–7.91 (m, 15H, Ar–H) and 13.02 (s, 2H, 2NH). MS m/z (%): 426 (M2, 7), 425 (M1, 9), 424 (M, 16), 194 (7), 166 (7), 140 (5), 127 (4), 105 (100), 111 (4), and 77 (36). Anal. calcd. for C25H17ClN4O (424.88).
2.2.2. Synthesis of VO(II) Complexes

New VO(II) complex series was synthesized by using variable derivatives from perimidine ligands. Equimolar (3 mmol) values were used from the perimidine ligand and dissolved fully in dioxane; after that, it was mixed with VOSO4·xH2O which dissolves in the dioxane/H2O mixture. The weighted molar ratio value from vanadyl salt was calculated attributing to its anhydrous weight. After ≈5 h reflux, 0.5  sodium acetate was added after dissolving in a little amount of bi-distilled water to precipitate the complexes. Each precipitate was separated out on hot, filtered off, washed several times with ethanol and diethyl ether, and finally dried in a vacuum desiccator.

2.3. DNA Binding Study

The binding attitudes of perimidine derivatives towards calf thymus DNA (CT-DNA) will be studied by using the spectroscopy method. CT-DNA (50 mg) was dissolved by stirring overnight in double deionized water (pH = 7.0) and must be kept at 4°C. Bi-distilled water was used to prepare the buffer (5.0 mM tris(hydroxymethyl)-aminomethane and 50 mM NaCl, pH = 7.2). Tris-HCl buffer was prepared in deionized water. DNA buffering solution gave absorbance ratio at 260/280 nm by 1.8–1.9, and this indicates the absence of protein from DNA [19, 20]. Applying the UV-Vis technique, the DNA concentration was determined (5.10 × 10−4 M) using its known molar absorptivity coefficient value (6600 M−1·cm−1 at 260 nm). At room temperature, 200–900 nm is the wavelength range used, and in 1 cm quartz cuvette, a fixed concentration (2.0 × 10−5 M in dioxane) from each ligand was utilized. A scanning process was done after adding CT-DNA by a gradual way from 0.00 to ≈2.18 × 0−4 mol·L−1. The same DNA amount added to the ligand solution was added also to the reference cell to delete the absorbance of free DNA. A significant binding constant (Kb) for interaction between ligands towards CT-DNA was determined by using the following equation: [DNA]/(єa − єf) = [DNA]/(єb − єf) + 1/Kb (єa − єf) [21], where [DNA] is the concentration of CT-DNA in base pairs, єa is the extinction coefficient observed for A/[compound] at the used DNA concentration, and єf is the extinction coefficient for each free compound (HL1−5) in the solution. Moreover, єb is the extinction coefficient of the compound when fully bond to DNA. In plots of [DNA]/(єa − єf) vs. [DNA], Kb is given by the following ratio: slope/intercept.

2.4. Antitumor Influence

The evaluation of cytotoxicity of candidate anticancer drugs will be performed using the most effective, available SRB method. All molecules and their derivatives will be tested for their toxicity on different cancer cell lines. In an attempt to evaluate the impact, the samples were prepared with different concentrations: 0.01, 0.1, 1, 10, and 100 µg/ml, respectively. The cells were cultured in the mixture of samples and media (RPMI-FBS + samples) for 72 h; after that, cytotoxicity impact was evaluated compared to the response of doxorubicin as a positive control.

The cytotoxic effect of the composites and ligands will be tested against different cancer cell lines (HepG2, MCF-7, and HCT116) as donor cancer cell lines by means of the SRB cytotoxicity test. To avoid the contamination, the RPMI media of the cells were supplemented with 100 µg/ml streptomycin and 100 units/ml penicillin with 10% FBS and incubated at a 5% CO2 incubator. Growing cells were collected using the trypsin enzyme and then counted using the cell counter in order to distribute equally the number of cells to each well of 69-well plates. The cells will incubate under sterile conditions with different concentrations of both ligands and composites for 72 hours, and subsequently, treated cells and untreated cells and the positive control were fixed with 10% TCA (trichloroacetic acid) and kept at 4°C for 1 h. After washing few times, fixed and washed cells were stained with 0.4% SRB stain solution for ten minutes, and subsequently, the cells were washed with 1% glacial acetic acid. To dissolve SRB-stained cells, Tris-HCl was used. To detect the density of remaining colors, a plate reader will be used at 540 nm wavelength. In order to determine the IC50 value, statistical analysis was accomplished through SigmaPlot version 14.0. The advantage of prepared compounds as potential drugs against different cancer cells was investigated.

2.5. Physical Techniques
2.5.1. Elemental Analysis

The element contents (carbon, hydrogen, and nitrogen) were determined at the Micro-Analytical Unit of Cairo University. Vanadium, sulfate, and chloride contents were evaluated by known standard methods [22] through complexometric and precipitation methods.

2.5.2. Conductivity Measurements

Applying the Jenway 4010 conductivity meter, the molar conductivity of freshly prepared 1.0 × 10−3 mol/cm3 in DMSO solutions was estimated.

2.5.3. X-Ray Diffraction and SEM

X-ray diffraction manners were recorded on the Rigaku diffractometer using Cu/Kα radiation. Scanning electron microscopy (SEM) images were obtained by using Joel JSM-6390 equipment.

2.5.4. IR, 1H·NMR, and 13CNMR Spectra

IR spectra were obtained using the JASCO FT/IR-4100 spectrophotometer from 400 to 4000 cm−1 in the KBr disc, while 1H·NMR spectra were recorded in deuterated dimethyl sulfoxide using the Varian Gemini 300 NMR spectrometer.

2.5.5. Mass spectra

Mass spectra were recorded on GCMS-QP1000 EX (Shimadzu) and GCMS 5988-A.

2.5.6. ESR Analysis

ESR spectra of VO(II)-powdered complexes were obtained on the Bruker EMX spectrometer working in the X-band (9.60 GHz) with 100 kHz modulation frequency. The microwave power was set at 1 mW, and modulation amplitude was set at 4 Gauss. The low field signal was obtained after 4 scans with a 10-fold increase in the receiver gain. A powder spectrum was obtained in a 2 mm quartz capillary at ordinary temperature.

2.5.7. UV-Vis Spectra and Magnetic Measurements

Electronic spectra for all compounds were recorded using the UV2 Unicam UV/Vis spectrophotometer in the DMSO solvent. Magnetic susceptibility values for VO(II) complexes were conducted by the Johnson Matthey magnetic susceptibility balance at room temperature.

2.5.8. Thermal Analysis

The Shimadzu thermogravimetric analyzer (20–900°C) at 10°C·min−1 heating rate under nitrogen was used for thermal analysis. Theoretical treatments (modeling and docking) were accomplished by known standard programs.

2.5.9. Antitumor Activity

Antitumor activity was conducted at the Regional Center for Mycology and Biotechnology.

2.6. Computational
2.6.1. DFT/Hartree–Fock Study

Implementing the Gaussian 09 software [23], the structural optimization process was accomplished over pyrimidine ligands and their VO(II) complexes in the gas phase. Two known methods were found as the most suitable one for the optimization process. The output files were visualized by the GaussView program [24]. According to the numbering scheme, DFT parameters were extracted using frontier energy gaps (EHOMO and ELUMO) for all investigated compounds. Moreover, other significant computations were taken from log files as oscillator strength, excitation energy, charges assigned for coordinating atoms, and some bond lengths.

2.6.2. QSAR Computation

New perimidine compounds were treated for the optimization process to give the best structural forms. HyperChem (v8.1) software is the tool used for such a purpose. The preoptimization process was executed by molecular mechanics force field (MM+) accompanied by semiempirical AM1 for the soft adjustment procedure. This process was accomplished without fixing any parameter till the equilibrium state for geometric structures. A system for minimizing energy was employed the Polak–Ribiere conjugated gradient algorithm. The QSAR process leads to computing essential parameters including the partition coefficient (log P). Log value is considered the essential indicator used to predict the biological activity for optimized compounds [25].

2.6.3. Docking Computation

Applying AutoDockTools 4.2 by using Gasteiger partial charges which added over the elements of pyrimidine ligands, the simulation procedure was executed to give a view on the biological behavior of compounds. Rotatable bonds were cleared, and nonpolar hydrogen atoms were conjoined. Interaction occurred between inhibitors (ligands) and protein receptors (4c3p, 3bch, and 4zdr) for breast, colon, and liver cancer proteins. The docking process was accomplished after addition of fundamental hydrogen atoms, Kollman united atom-type charges, and salvation parameters [26]. Affinity (grid) maps of ×× Å grid points and 0.375 Å spacing were generated applying the AutoGrid program [27]. Van der Waals forces and electrostatic terms were obtained. This is done by applying autodock parameter set-dependent and distance-dependent dielectric functions, respectively. The docking process was executed using the Solis and Wets local search method and Lamarckian genetic algorithm (LGA) [28]. Initial position, orientation, and torsions of the inhibitor molecule were set indiscriminately. All rotatable torsions were expelled during the docking process. Each experiment is the mean value of 10 different runs that are set close after the maximum of 250000 energy assessments. 150 is the used population size. During the process, the translational step of 0.2 Å, quaternion, and torsion steps of 5 were applied.

3. Results and Discussion

3.1. Physical Properties

Essential analytical and physical data for ligands and their VO(II) complexes are summarized in Table 1. All investigated complexes are nonhygroscopic in nature, having high melting point (>300°C). The elemental analysis proposes 1 : 2 (HL : M) molar ratio as the general formula for all complexes. All complexes are completely soluble in DMSO or DMF solvents. The conductivity measured is 5.66–14.22 Ω−1·cm2·mol−1. Such conductivity values are attributed to the nonconducting character of tested complexes [29]. This coincides with sulfate anion which favors covalent attachment with metal ions inside the coordination sphere.

Compounds (formula weight) (calcd./found)ColorElemental analysis (%) calcd. (found)

(1) (C25H18N4O) (L1) (390.44/390.42)Dark brown76.91 (76.90)4.65 (4.66)14.35 (14.35)
(2) [(VO)2 (SO4)2 (L1)]H2O (734.46)Dark brown40.88 (40.88)2.74 (2.73)7.63 (7.65)26.16 (26.16)13.87 (13.88)
(3) (C26H20N4O2) (L2) (420.47/420.44)Dark brown74.27 (74.27)4.79 (4.79)13.32 (13.31)
(4) [(VO)2 (SO4)2 (L2)]2H2O (782.51)Dark green39.91 (39.90)3.09 (3.10)7.16 (7.17)24.55 (24.54)13.02 (13.03)
(5) (C25H17N5O3) (L3) (435.44/435.42)Dark brown68.96 (68.95)3.93 (3.93)16.08 (16.09)
(6) [(VO)2 (SO4)2 (L3)]H2O (779.46)Dark green38.52 (38.52)2.46 (2.46)8.99 (8.97)24.65 (24.66)13.07 (13.05)
(7) (C25H17N4OCl) (L4) (424.88/424.86)Dark brown70.67 (70.66)4.03 (4.02)13.19 (13.18)8.34 (8.35)
(8) [(VO)2 (SO4)2 (L4)]H2O (768.90)Dark green39.05 (39.05)2.49 (2.48)7.29 (7.28)24.99 (25.02)/4.61 (4.63)13.25 (13.26)
(9) (C25H17N4OCl) (L5) (424.88/424.86)Dark brown70.67 (70.68)4.03 (4.05)13.19 (13.18)8.34 (8.35)
(10) [(VO)2 (SO4)2 (L5)]3H2O (804.93)Dark brown37.30 (37.31)2.88 (2.88)6.96 (6.95)23.87 (23.88)/4.40 (4.41)12.66 (12.67)

3.2. Comparative IR Study

The assignments of all characteristic bands for five perimidine ligands and their VO(II) complexes are summarized in Table 2. ν(NH), δ(NH), ν(C=N), and ν(C=O) are the significant functional bands for coordinating groups which appear in narrow regions observed in all derivatives. This may refer to the far effect of the aromatic substituent on bond movement inside such groups. A comparative study of ligands and their VO(II) complexes reveals the following observations: (1) lower-shifted appearance of former bands is considered a strong evidence for contribution of C=O, NH, and C=N groups in coordination towards two central atoms. (2) New bands appeared at 1368–1434 and 1140–1179 cm−1 assigned for νas(SO4) and νs(SO4), respectively, through bidentate attachment [30]. (3) Other bands appearing at ≈760 and ≈690 cm−1 are attributed to δr(H2O) and δw(H2O), respectively, for crystal water molecules. (4) ν(M-L) bands appeared at the low wavenumber region belonging to M-O and M-N bonds. These spectral observations suggest a tetradentate mod of coordination towards two vanadyl atoms. Also, the band observed at 966–1074 cm−1 range assigns for ν(V = O), significantly pointing to the square-pyramidal configuration [31].

CompoundsνNH,νOHδNHυC=OνC=Nνas(SO4)νs(SO4)δr(H2O), δw(H2O)νV=OνM-OνM-N

(1) (C25H18N4O) (L1)3155147316181518
(2) [(VO)2 (SO4)2 (L1)]H2O3110, 335014701596151414201142765, 670966588476
(3) (C26H20N4O2) (L2)3177147015971508—-
(4) [(VO)2 (SO4)2 (L2)]2H2O3100, 337214471592150214111146765, 6971074572515
(5) (C25H17N5O3) (L3)3150147316201538
(6) [(VO)2 (SO4)2 (L3)]H2O3105, 338214471616151714111179743, 697966600508
(7) (C25H17N4OCl) (L4)3160147416141518
(8) [(VO)2 (SO4)2 (L4)]H2O3100, 342014711624151014341150755, 637985610550
(9) (C25H17N4OCl) (L5)3150147316201518
(10) [(VO)2 (SO4)2 (L5)]3H2O3054, 338414461616151213681140754, 6891074589508

3.3. Electronic Spectra and Magnetic Measurements

Electronic transition bands and magnetic moment values are aggregated in Table 3. UV-Vis spectra were recorded qualitatively in the DMSO solvent to gain smoothly absorption curves. Intraligand transition bands appearing at 31,250–38,168, 25,974–30,769, and 17,544–19,157 cm−1 are attributed to n ⟶ , π ⟶ , and n ⟶  transitions, respectively, inside variable groups [32]. A structural condensed conjugation of chromophores leads to appearance of deep colors for all perimidine ligands. This is accompanied with the appearance of the n ⟶  band in the middle of the visible region. VO(II) complex spectra display intraligand transitions suffer shift due to coordination. The appearance of charge transfer bands attributes to O ⟶ V and N ⟶ V transitions. Also, new significant d-d transition bands were observed at ≈15,300 and 12,800 cm−1 assigned for 2B2g ⟶ 2B1g (E2, υ2) and 2B1g ⟶ 2Eg (E1, υ1), respectively. These bands are attributed to transition inside the square-pyramidal configuration (Figure 4). Reduced magnetic moment values (μeff = 1.65–1.68 BM) recorded for all complexes support the proposal of binuclear complexes [33].

Compoundsμeff (BM)d-d transition bands (cm−1)Intraligand and charge transfer (cm−1)

(1) (C25H18N4O) (L1)31,746; 26,316; 23,923; 18,868
(2) [(VO)2 (SO4)2 (L1)]H2O1.6615,290; 1280035,714; 29,412; 25,641; 24,272; 17,857
(3) (C26H20N4O2) (L2)38,168; 28,249; 23,810; 19,048
(4) [(VO)2 (SO4)2 (L2)]2H2O1.6815,393; 1275037,037; 30,769; 26,316; 23,256; 17,544
(5) (C25H17N5O3) (L3)36,364; 30,303; 26,316; 23,810; 19,157
(6) [(VO)2 (SO4)2 (L3)]H2O1.6615,873; 1283037,037; 28,571; 26,667; 18,182
(7) (C25H17N4OCl) (L4)31,746; 25,974; 18,587
(8) [(VO)2 (SO4)2 (L4)]H2O1.6715,385; 12,80035,714; 30,303; 25,974; 24,390; 17,857
(9) (C25H17N4OCl) (L5)31,250; 26,316; 24,390; 18,182
(10) [(VO)2 (SO4)2 (L5)]3H2O1.6515,873; 1278035,714; 30,769; 25,000; 23,256; 18,868

3.4. ESR Spectra

ESR spectra (Figure 5, for example) of VO(II) solid complexes were obtained and investigated to verify the structural forms of them. All spectra demonstrated an eight-line pattern, which attributes to the analogous and vertical ingredients -tensors and hyperfine (hf) A-tensors. Spin Hamiltonian parameters and molecular orbital values were calculated and are represented in Table 4. The analogous and vertical ingredients are well resolved. Nitrogen super-hyperfine splitting is not observed, which points to the presence of single electron in the dxy orbital. The pattern suggests that and A are axially symmetric in nature. The factors A and appear to be in covenant with the values commonly known for vanadyl complex in the square-pyramidal geometry. factor, which is expressed by  = (− 2.0023)/(⊥ − 2.0023) = 4, measures the exchange interaction between metal centers. In agreement with Hathaway [34, 35],  > 4 shows negligible exchange interaction, while  < 4 is the vice versa. An observable reduction of the values calculated (1.71–2.79) proposes strong interaction inside binuclear complexes [36, 37]. This interaction affects the magnetic moment value of complexes which suffers observable reduction. The tendency of to decrease with increasing is an index for tetrahedral distortion () [3840]. The molecular orbital coefficients and are calculated by



The hyperfine conjunction disciplinarians were calculated by taking A// and A as negative, which gave positive values of and . The calculated and values introduce the highly ionic character of in-plane σ- and π-bonding. The electronic transition spectra display two significant bands at ≈15,300 and 12,800 cm−1 assigned for 2B2g ⟶ 2B1g (E2, υ2) and 2B1g ⟶ 2Eg (E1, υ1), respectively. Assume pure d-orbitals by using first- and second-order perturbation theories. The parameters attributing to transition energy are called the spin Hamiltonian parameters and calculated by the following expression:  =  − (2λ/E2), where is the free-electron value (2.0023). Using E2 value, the spin-orbital coupling constant (λ) was evaluated (138.18). A value for λ of 250 cm−1 is reported [41] for free V+4 ion. The high reduction in the magnitude of λ for the double-bonded oxovanadium complex (V=O)+2 is attributed to substantial π-bonding. However, the value falls inside the logical borders announced. The orbital reduction factors, namely, K// and K, are also calculated using 2K// = (// − 2.00277) E/8 λ and 2K = ( − 2.00277) E/2 λ. For pure σ-bonding, K// ≈ K ≈ −0.77, while 2K// > 2K signifies in-plane σ-bonding, with 2K⊥ < 2K// accounting for out-of-plane π-bonding [42].

3.4.1. Calculation of Dipole Term (p)

Dipolar term values can be determined by

If is taken to be negative and positive, the value of will be more than 270 G, which is far from the expected value. Thus, the signs of both and are used as negative and are indicated in the form of the isotropic hf constant (Ao). McGarvey theoretically accomplished the p value as +136 G for vanadyl complexes which does not deviate much from the expected value.

3.4.2. Calculation of MO Coefficients and Bonding Parameters

The values observed are different from the electronic value (2.0023). This assigns to spin-orbit interaction of the dxy ground state level. The isotropic and anisotropic and A parameters were calculated using the following equations: Ao = (A// + 2A)/3 and  = (// + 2)/3. Taking A11 and A to be negative values, the K expression is K = −(Ao/p) − (− ).

Thus, K (Fermi contact term) can be determined. The Fermi contact term, k, is a sense of polarization exerted by the uneven apportionment of d-electron density on the inner core s-electron.

3.5. X-Ray Diffraction

X-ray diffraction patterns were executed over 10° < 2θ < 90° range (Figures 6 and S3) for ligands under study. This technique gives a considerable view about dynamics of the crystal lattice in solid compounds. Using standard methods, a comparative study of patterns with reactants reflects the purity of isolated compounds [43]. Also, significant parameters related to crystalline compounds can be calculated using the high-intense peak (full width at half maximum (FWHM)). The crystallinity appearing with the LH ligand reflects the isolation of a strictly known irregular crystallite, while the amorphous appearance of others reflects the indiscriminate orientation of atoms inside the 3D space. 2θ (21.18), d spacing (4.1910), FWHM (0.2454), relative intensity (%) (857), and particle size (6.003 Ε) were calculated for LH compounds. The crystallite size was computed by utilizing the Debye–Scherrer equation: β = 0.94 λ/(S cos θ), where S is the crystallite size, θ is the diffraction angle, β is FWHM, and Cu/Kα (λ) = 1.5406 Å. The d-spacing between inner crystal planes was extracted from the Bragg equation:  = 2dsin(θ) at n = 1. The size calculated falls in the nanometer range (nm) which expects a widespread application especially for the biological field. Also, crystal strain (ε, 5.027) was calculated by β = , while dislocation density (δ, 0.0277) was computed by δ = 1/S2 [44]. The dislocation density and strain are the aspects for network dislocation in compounds. The lower values of them indicate high quality of compounds. The SEM tool is used to give a clear view about the habit and surface morphology of all studied compounds (Figure S4). The images of paramagnetic compounds are not strictly resolved because an insufficient electron beam can meet the surface to provide well resolution. Subsequently, the determination of particle size in an accurate way is strongly absent. It was known about this study that the crystals were grown up from just a single one to several accumulated distributables with particle sizes starting with few nanometers to many hundreds. The formation of extended crystals over a rocky shape may happen by two nucleation processes: by distribution and by piling up of layers which are grown. It was pointed to that if the rate of growth along the C-axis is fast and a great number of grown nuclei are active across the axis in comparison with vertical to the C-axis, the crystals will be extended over patches [45]. The attitude displayed on different crystals may be due to the growth along the strongest bond through anisotropy included in crystal structures. When the amount exceeds to a certain limit, the result is evolution of plates and rock shapes. It is credible to assume that the environmental conditions change the nature and shape of the morphology. Moreover, the rock and plates shaping compounds may have excellent activity towards different applications due to their broad surface area [46]. The homogeneous morphology observed indicates the obtained strict-defined crystals are free from metal ions on the external surface.

3.6. Thermal Study

The degradation behaviors of all perimidine compounds and their VO(II) complexes were tested. The proposed degradation insights corresponding to all decomposition stages are tabulated (Table 5). The treated perimidine compounds start their successive decomposition at low temperature (≈60°C) in three stages. A sequenced complete degradation of the organic compound was recorded with or without carbon atoms residue. VO(II)-perimidine complexes display an observable thermal stability for the organic compounds coordinated. The degradation stages varied in between three and four stages. The first degradation process starts at 40–80°C temperature range which starts with the removal of water molecules and is followed by decomposition of the coordinating ligand. Variable residue was proposed with the complexes degradation process but all agree with the presence of biatomic metals. An acceptable conformity between calculated and found weight losses percentage may reflect the exact determination of stage borders.

CompoundStepsTemp. range (°C)DecomposedWeight loss; calcd. (found %)

L11st45.1–120.5-[C6H6 + N2]27.18 (27.16)
2nd122.2–410.1-[C6H5 + CO]26.92 (26.95)
3rd410.3–670.2-[C8H7N2]33.59 (33.54)
Residue4C12.31 (12.35)
[(VO)2 (SO4)2 (L1)]H2O1st80.3–120.3-[H2O + SO4]15.53 (15.55)
2nd120.6–391.7-[SO4 + C6H6 + N2]27.53 (27.55)
3rd391.9–798.8-[C19H12N2]36.53 (36.50)
ResidueV2O320.41 (20.40)
L21st65.6–156.1-[C6H5OCH3]25.72 (25.71)
2nd156.6–299.9-[C6H5 + CO + N2]31.66 (31.69)
3rd301.0–663.2-[C9H7N2]34.05 (33.89)
Residue3C8.57 (8.71)
[(VO)2 (SO4)2 (L2)]2H2O1st42.1–135.1-[2H2O + 2SO4]29.16 (29.16)
2nd136.1–270.1-[C6H5OCH3 + N2]17.40 (17.29)
3rd271.0–485.4-[C6H5]9.85 (9.94)
4th485.6–797.9-[C13H7N2]24.43 (24.45)
ResidueV2O319.15 (19.16)
L31st63.66–230.51-[C6H6 + NO2]28.50 (27.90)
2nd231.21–410.11-[C7H5 + CO + N2]33.33 (33.31)
3rd410.52–650.64-[C11H6N2]38.16 (38.79)
[(VO)2 (SO4)2 (L3)]H2O1st79.2–140.6-[H2O + SO4]14.63 (14.62)
2nd141.9–278.9-[SO4 + C6H5 + CO]25.81 (25.78)
3rd279.1–479.5-[NO2 + C6H6 + N2]19.52 (19.53)
4th480.11–798.8-[C12H6N2]22.86 (22.90)
ResidueV2O217.18 (17.17)
L41st64.65–145.46-[C6H5Cl + CO + N2]39.68 (39.68)
2nd145.68–326.78-[C6H5 + N2]24.74 (24.75)
3rd330.12–680.23-[C12H7]35.58 (35.57)
[(VO)2 (SO4)2 (L4)]H2O1st69.1–256.1-[H2O + C6H5Cl + SO4]29.48 (29.65)
2nd256.9–484.1-[SO4 + CON2 + C6H5]29.80 (29.81)
3rd484.6–789.4-[C10H7N2]20.18 (19.98)
ResidueV2O2 + 2C20.54 (20.56)
L51st62.3–169.6-[C6H5 + N2]24.74 (24.71)
2nd160.1–371.9-[C6H5Cl + CO + N2]39.68 (39.59)
3rd372.6–666.8-[C9H7]27.10 (27.19)
Residue3C8.48 (8.51)
[(VO)2 (SO4)2 (L5)]3H2O1st42.1–266.3-[3H2O + C6H5Cl]20.70 (20.71)
2nd266.38–482.5-[2SO4 + CON2 + C6H5]40.41 (40.61)
3rd482.9–793.5-[C8H7N2]16.29 (16.36)
ResidueV2O2 + 4C22.60 (22.32)

3.7. DNA Binding

Appling the spectrophotometric titration method, the binding mod of perimidine derivatives towards CT-DNA was investigated. Electronic absorption of freshly prepared solutions was obtained at 25°C over 200–800 nm range, with a reference solution for each concentration. Scanned solutions include fixed ligand concentration (2 × 10−5 M) with a regular increase of DNA added. The effective binding constant for the interaction of the organic derivatives with DNA was obtained based on observable changes in absorption at 418, 420, 420, 385, and 410 nm for LH, LOMe, LNO2, L4, and L5, respectively. A regular increase of DNA amount added to the ligand solution leads to the bathochromic effect for the significant ligand band assigned for transition inside interacting groups. This band is minimized gradually as appeared clearly with the aggregated spectra for each derivative. This minimization is followed by appearance of the slightly shifted peak (1-2 nm) from the free ligand peak, which assigns for the binding complex and suffers a gradual increase in absorbance. This is considered as a sufficient indicator of coupled DNA helix stabilization, after the interaction process. Such an investigation suggests the coupling for binding sites through electrostatic attraction or occluded in major and minor grooves inside DNA. Also, the bathochromic effect can be investigated and explained based on two bases: broad surface area of perimidine molecules and the presence of planar aromatic chromophore, which facilitate well binding towards CT-DNA. This groove binding leads to structural reorganization of CT-DNA. This requires a partial disassembling or deterioration of double helix at the exterior phosphate, which leads to formation of cavity suitable for entering compounds [47]. The bathochromic feature observed is directly proportional to electron withdrawing character for substituents and their position. The binding constants (Kb) for the five derivatives were calculated by known spectral relationships [19] for L1, L2, L3, L4, and L5 as 6.10 × 104, 6.07 × 104, 6.75 × 104, 7.99 × 104, and 8.80 × 104 M−1. According to Hammett’s constants (σR), essential correlation against intrinsic constants will be conducted (Figure 7), and the relation verifies the direct relation in between [48].

3.8. Computational
3.8.1. DFT/Hartree–Fock Study

Applying the Gaussian 09 software, the optimization process was executed over all new compounds till reaching the best configuration. A known standard method was used for this purpose. Essential parameters will be extracted from the energy levels of frontiers (HOMO and LUMO). The energy gap between EHOMO and ELUMO will give an excellent view about the character of the tested compound. The biological behavior and the ligational mode are most significant features concluded. The frontier images of perimidine ligands and their VO(II) complexes are shown in Figures 8(a) and 8(b), respectively. HOMO-level images display the concentration over the perimidine ring which includes two donor centers, while the LUMO-level images display the concentration over the other side in molecules including the other two coordination sites. This view introduces a good electron relocation between donor atoms which smoothens the donation of coordinating centers. On the other side, the two levels in VO(II) complexes represent the concentration around the two central atoms mainly. This may offer the good role of VO atoms in the application feature interested in this research. This may happen through the smooth charge transfer process that includes the complexes. Electronegativity (χ), chemical potential (μ), global hardness (η), global softness (S), global electrophilicity index (ω), and absolute softness (ϭ) were calculated by using known standard equations [49, 50]. Toxicity and reactivity of compounds can be clarified by using the electrophilicity index (ω) value. This index gives a clear insight about the expected biological attitude of tested perimidine compounds in comparison with their VO(II) complexes and, also, measures the firmness of the compound which takes an extra negative charge from the environment. Also, the firmness and reactivity of compounds can be tested from two opposite indexes (η and ϭ) [42, 51].

(1) Some Quantum Parameters. Some important quantum parameters are calculated for all treated compounds attributing to frontier energy gaps and are displayed in Table 6. The computed results of ligands introduce the following notices: (i) the degree of converged softness recorded for perimidines offers their compatible flexibility towards the coordination. (ii) Electrophilicity index (χ) and electronic chemical potential index (μ) have two different signs. This is evidence for the ability of compounds to acquire electrons from the surrounding by the following order: L4 > L3 > L5 > L1 > L2 ligands. This arrangement agrees by an excellent way with the priority of electron withdrawing substituents (Cl and NO2) in para position which facilitates the compound electron affinity.

CompoundEHEL(EH − EL)EL − EHxµηS (eV-1)ωϭ

L1 + VO(II)−0.20433−0.19545−0.00890.008880.19989−0.199890.004440.002224.499551225.2252252
L2 + VO(II)−0.20163−0.19237−0.00930.009260.197−0.1970.004630.0023154.191037215.9827214
L3 + VO(II)−0.21881−0.21008−0.00870.008730.214445−0.214450.0043650.0021835.267658229.0950745
L4 + VO(II)−0.20433−0.19545−0.00890.008880.19989−0.199890.004440.002224.499551225.2252252
L5 + VO(II)−0.19719−0.16607−0.03110.031120.18163−0.181630.015560.007781.06007364.26735219

Whenever, the extracted data assigning for VO(II) complexes introduce the following observations: (i) frontier energy gaps are completely minimized from original perimidines leading to red shift inside electronic transitions. Such a behavior may clarify the effect of metal atoms (vanadyl) in stabilizing the compounds. This reduction is preferable in biological attitude of compounds [52]. (ii) The absolute softness values in complexes were enhanced than the ligand values which predicated their high biological activity. From calculated energy gaps, Hammett’s relation displays a significant effect of the p-substituent on δE values of ligands or their complexes by two reverse features (Figure 9).

(2) Some Log File Parameters. Essential log file data are summarized and presented in Table 7. The allowed data are varied in between the free ligands and their complexes, due to the difference in methods used for the treatment. A suitable method used for the organic ligand appeared unsuitable for its VO(II) complex. A comparative investigation introduced the following notices: (i) a general reduction in the charges computed for coordinating atoms (O19, N11, N15, and N16). This is due to their participation in coordination with VO(II) atoms. (ii) The computed bond lengths appearing with four perimidine derivatives are comparable with each other except for the L3 ligand. This displays the inductive effect of the p-substituent (nitro group) on the elongation of bond lengths attributing to the affected function groups. (iii) Oscillator strength values (range 0–1) of complexes are commonly minimized than those of their corresponding ligands. This may indicate the effect of the metal atom (vanadyl) in facilitating the absorption or reemission of electromagnetic radiations inside complex molecules [53]. The values are close to zero and not 1; this may suggest low excitation energy values needed for electronic transitions. (iv) Also, an increase in dipole moment values of complexes over ligands indicates high polarity of covalent bonds surrounding two central atoms except for the L2 complex. This may refer to the significant difference between all substituents from the methoxy group which has electron-donating feature in opposite with the others [54].

CompoundO19N11N15N16C18–O19C12–N11C14–N15N15–N16V1V2D (Debye)E (nm)ʄ

L1 + VO(II)−0.410181−0.282766−0.316313−0.2484290.9332010.92933111.566716513.70.003
L2 + VO(II)−0.420038−0.397120−0.322648−0.2502610.9275520.9150693.550431387.70.0008
L3 + VO(II)−0.414856−0.387699−0.320321−0.2549470.9551240.95254416.689917266.30.0032
L4 + VO(II)−0.410181−0.282766−0.316313−0.2484290.9332010.92933111.566716513.70.003
L5 + VO(II)−0.405024−0.408894−0.304735−0.2105730.9052450.7306018.970620988.60.002

3.8.2. QSAR Calculations

Using the HyperChem (v8.1) program, essential QSAR parameters are calculated and tabulated (Table 8). This computation gives a clear view about some statistics belonging to coordinating agents. Log  value is an indication for the biological feature of the tested compound by a reverse relation [55]. The values are arranged by the following order: L1 (2.53) > L4 = L5 (2.31) > L2 (1.53) > L3 (−1.64). Partition coefficient (log ) values introduce a distinguish biological activity may appear with the L3 ligand.


Surface area (approx.) (Å2)425.73488.36496.79464.04465.53
Surface area (grid) (Å2)623.02661.15661.91644.29642.82
Volume (Å3)1060.571138.871134.041105.991105.72
Hydration energy (kcal/mol)−8.29−9.97−17.83−8.00−8.02
Log P2.531.53−1.642.312.31
Reactivity (Å3)132.87139.25138.92137.59137.59
Polarizability (Å3)45.3247.8047.6247.2547.25
Mass (amu)390.44420.47436.45424.89424.89

3.8.3. Docking Computation

Simulation technique is a new revolution process served in different applications. Drug design is a complicated process that needs significant facilities to establish a view about the expected efficiency of proposed drugs. In last decades, the docking computation process between the proposed drug (inhibitor) and the infected cell proteins is the concern in drug industrial research. AutoDockTools 4.2 software was used for this approach. 4c3p, 3bch, and 4zdr are the BDP files for breast, colon, and liver cancer cell proteins which are used for the docking process with five perimidine derivatives. The extracted energies over PDB files (a format using the Gaussian 09 software) are presented in Table 9. Scanning for the energy values introduces the following observations: (i) there is no interaction observed with the five inhibitors towards 3bch colon cancer protein. (ii) The degree of interaction towards breast colon protein (4c3p) is arranged as L5 > L1 > L2 > L4, while the arrangement towards 4zdr (liver cancer protein) is as L5 > L1 > L4 > L3 > L2. This result displays the priority of L5 and L1 ligands in the inhibition process towards breast and liver carcinoma cell lines through a strong interaction (Figures 10 and S5) [55]. Dissociation constant (pKa) calculated is considered the biopharmaceutical measure of drug-likeness compounds. This constant helps in understanding the ionic form of the drug along the pH range. High pKa values (>10) reflect their ionization which facilitates their diffusion across the cell membrane to give a well inhibition process. Also, highly reduced energies were recorded for 4c3p and 4zdr receptors. Positive sign of electrostatic energy recorded clarifies high stability of interacting complexes. HP plots (Figures 11 and S6) as well as 2D plots (Figure S7) display prolonged H-bonding appearing with L5 and LH ligands. This verifies the degree of interaction proposed on extracted energies. Also, high surface area recorded with breast or liver cancer protein complexes introduces a good degree of H-interaction. And hp, 2D, and surface area data verify the absence of interaction recorded with colon cancer protein.

LigandspKaReceptorEst. free energy of bindingEst. inhibition constant (Ki) (µM)vdW + bond + desolving energyElectrostatic energyTotal intercooled energyFrequencyInteracting surface


3.9. Antitumor Efficiency

The results obtained by screening all prepared compounds for comparison confirmed that the complexes exhibit more cytotoxicity against HepG2, MCF-7, and HCT116 in vitro. The IC50 values are displayed in Table 10 and in Figures 12 and S8. Cells were treated with various concentrations of compounds and incubated for 48 h [56]. Cytotoxicity is considered as a good anticancer parameter if the influence induced apoptotic pathways inside the cell. Apoptotic may be detected by many parameters like the activation of caspase family, DNA fragmentation, or morphology of the cell. The sample L4 + VO(II) was the best impacted complex on liver, breast, and colon cancer cell lines with IC50 values of 1.66, 3.42, and 1.27, respectively, while its relative ligand (L4) impact was moderate at all cancer types. Hence, these results showed that the present study’s effort to improve and enhance the effect of new complexes has achieved a clear, acceptable, and respectable success because the effect was enhanced for 15, 7, and 22 times, respectively, compared to the ligand with clear signs that it is going to be very close to the positive control. On the contrary, unfortunately, the same results were not detected in other complexes; they went in the contrary way: instead, they increased the impact they decreased it dramatically. What our results tell us clearly is that neither VO(II) nor ligands alone can act as an anticancer candidate drug, while only one complex can present that effect. So, the mechanism of action is not related to the ligand or to VO(II) itself, as far as related to the complex itself.

Cell typeIC50 (µg/ml)


4. Conclusion

This paper presents new VO(II) complexes derived from a series of perimidine ligands. This study focuses on the effect of substituents on the chemistry and applicability of complexes. All the new compounds were well characterized by all possible tools. The complexes were found in a nanoscale comfortably. The different theoretical implementations gave a view about the biological feature of the investigated compounds in a comparative way. The docking process displays the high interaction of organic derivatives against breast cancer, while the experimental investigation displays the priority of the L4-VO(II) complex against all carcinomas tested. The binding efficiency of ligands towards CT-DNA was tested. Binding constant (Kb) values are in agreement with the electron-drawing character of the p-substituent which displayed high Kb values.

Data Availability

The data used to support the findings of this study are available from the corresponding author upon request.

Conflicts of Interest

The authors declare that they have no conflicts of interest regarding the publication of this paper.


The authors extend their appreciation to the Deanship of Scientific Research at King Khalid University for funding this work through General Research project under grant number (G.R.P-124-38).

Supplementary Materials

Figure S1: 1H·NMR spectra of L4 and L5 perimidine ligands. Figure S2: mass spectra of L3 and L4 ligands. Figure S3: X-ray patterns of four perimidine ligands. Figure S4: SEM images of perimidine ligands and their VO(II) complexes. Figure S5: interacting protein-inhibitor complexes for L1, L2, L3, L4, and L5 with 4c3p (1) and 3bch (2) receptors (A–E, respectively). Figure S6: interacting hp plot: LH, LOMe, LNO2, LClP, and LClM with 4c3p(1) and 3bch(2) receptors (A–E, respectively). Figure S7: 2D plot forms: L1, L2, L3, L4, and L5 with 4c3p (1), 3bch (2), and 4zdr (3) receptors (A–E, respectively). Figure S8: dose response curves of perimidine-VO(II) complexes against MCF-7, HCT116, and HepG2 cancer cells. (Supplementary Materials)


  1. M. S. Refat, “Synthesis, characterization, thermal and antimicrobial studies of diabetic drug models: complexes of vanadyl(II) sulfate with ascorbic acid (vitamin C), riboflavin (vitamin B2) and nicotinamide (vitamin B3),” Journal of Molecular Structure, vol. 969, no. 1–3, pp. 163–171, 2010. View at: Publisher Site | Google Scholar
  2. G. R. illsky, “Synthesis, characterization, thermal and antimicrobial studies of diabetic drug models: complexes of vanadyl(II) sulfate with ascorbic acid (vitamin C), riboflavin (vitamin B2) and nicotinamide (vitamin B3),” in Vanadium in Biological Systems Physiology and Biochemistry, N. D. Chasteen, Ed., Kluwer Academic Publishers, Dordrect, Netherlands, 1990. View at: Google Scholar
  3. Z. Ye, G. Yan, J. Tang, Q. Fu, J. Lu, and N. Yang, “Synthesis and biological evaluation of two oxidovanadium (IV) complexes as DNA-binding and apoptosis-inducing agents,” American Journal of Biological Chemistry, vol. 4, no. 1, pp. 6–13, 2016. View at: Google Scholar
  4. J. Farzanfar, K. Ghasemi, A. R. Rezvani et al., “Synthesis, characterization, X-ray crystal structure, DFT calculation and antibacterial activities of new vanadium(IV, V) complexes containing chelidamic acid and novel thiourea derivatives,” Journal of Inorganic Biochemistry, vol. 147, pp. 54–64, 2015. View at: Publisher Site | Google Scholar
  5. K. Kanmani Raja, L. Lekha, R. Hariharan, D. Easwaramoorthy, and G. Rajagopal, “Synthesis, structural, spectral, electrochemical and catalytic properties of VO (IV) complexes containing N, O donors,” Journal of Molecular Structure, vol. 1075, pp. 227–233, 2014. View at: Publisher Site | Google Scholar
  6. D. M. Boghaei and S. Mohebi, “Synthesis, characterization and study of vanadyl tetradentate Schiff base complexes as catalyst in aerobic selective oxidation of olefins,” Journal of Molecular Catalysis A: Chemical, vol. 179, no. 1-2, pp. 41–51, 2002. View at: Publisher Site | Google Scholar
  7. J.-Q. Wu and Y.-S. Li, “Well-defined vanadium complexes as the catalysts for olefin polymerization,” Coordination Chemistry Reviews, vol. 255, no. 19-20, pp. 2303–2314, 2011. View at: Publisher Site | Google Scholar
  8. G. Micera and D. Sanna, in Vanadium in the Environment, Part One: Chemistry and Biochemistry, J. O. Nriagu, Ed., John Wiley & Sons, New York, NY, USA, 1998.
  9. F. T. G. Hudson, Vanadium Toxicology and Biological Significance, Elsevier, NewYork, NY, USA, 1996.
  10. R. C. Maurya and S. Rajput, “Oxovanadium(IV) complexes of bioinorganic and medicinal relevance: synthesis, characterization and 3D molecular modeling and analysis of some oxovanadium(IV) complexes involving the O, N-donor environment of pyrazolone-based sulfa drug Schiff bases,” Journal of Molecular Structure, vol. 794, no. 1–3, pp. 24–34, 2006. View at: Publisher Site | Google Scholar
  11. D. M. Boghaei, A. Bezaatpour, and M. Behzad, “Synthesis, characterization and catalytic activity of novel monomeric and polymeric vanadyl Schiff base complexes,” Journal of Molecular Catalysis A: Chemical, vol. 245, no. 1-2, pp. 12–16, 2006. View at: Publisher Site | Google Scholar
  12. M. S. Refat, M. A. A. Moussa, and S. F. Mohamed, “Synthesis, spectroscopic characterization, thermal analysis and electrical conductivity studies of Mg(II), Ca(II), Sr(II) and Ba(II) vitamin B2 complexes,” Journal of Molecular Structure, vol. 994, no. 1–3, pp. 194–201, 2011. View at: Publisher Site | Google Scholar
  13. M. S. Refat and S. A. El-Shazly, “Identification of a new anti-diabetic agent by combining VOSO4 and vitamin E in a single molecule: studies on its spectral, thermal and pharmacological properties,” European Journal of Medicinal Chemistry, vol. 45, no. 7, pp. 3070–3079, 2010. View at: Publisher Site | Google Scholar
  14. R. Takjoo, A. Akbari, S. Yousef Ebrahimipour, M. Kubicki, M. Mohamadi, and N. Mollania, “Synthesis, spectral characterization, DFT calculations, antimicrobial activity and molecular docking of 4-bromo-2-((2-hydroxy-5-methylphenylimino)methyl)phenol and its V(V) complex,” Inorganica Chimica Acta, vol. 455, pp. 173–182, 2017. View at: Publisher Site | Google Scholar
  15. V. Kraehmer and D. Rehder, “Modelling the site of bromide binding in vanadate-dependent bromoperoxidases,” Dalton Transactions, vol. 41, no. 17, pp. 5225–5234, 2012. View at: Publisher Site | Google Scholar
  16. P. Sathyadevi, P. Krishnamoorthy, R. R. Butorac, A. H. Cowley, and N. Dharmaraj, “Synthesis of novel heterobimetallic copper(I) hydrazone Schiff base complexes: a comparative study on the effect of heterocyclic hydrazides towards interaction with DNA/protein, free radical scavenging and cytotoxicity,” Metallomics, vol. 4, no. 5, pp. 498–511, 2012. View at: Publisher Site | Google Scholar
  17. R. Pradhan, M. Banik, D. B. Cordes, A. M. Z. Slawin, and N. C. Saha, “Synthesis, characterization, X-ray crystallography and DNA binding activities of Co(III) and Cu(II) complexes with a pyrimidine-based Schiff base ligand,” Inorganica Chimica Acta, vol. 442, pp. 70–80, 2016. View at: Publisher Site | Google Scholar
  18. T. A. Farghaly and H. K. Mahmoud, “Synthesis, tautomeric structures, and antitumor activity of new perimidines,” Archiv der Pharmazie, vol. 346, no. 5, pp. 392–402, 2013. View at: Publisher Site | Google Scholar
  19. M. E. Reichmann, S. A. Rice, C. A. Thomos, and P. Doty, “A further examination of the molecular weight and size of desoxypentose nucleic acid,” Journal of the American Chemical Society, vol. 76, no. 11, pp. 3047–3053, 1954. View at: Publisher Site | Google Scholar
  20. J. Marmur, “A procedure for the isolation of deoxyribonucleic acid from micro-organisms,” Journal of Molecular Biology, vol. 3, no. 2, pp. 208–218, 1961. View at: Publisher Site | Google Scholar
  21. A. Wolfe, G. H. Shimer, and T. Meehan, “Polycyclic aromatic hydrocarbons physically intercalate into duplex regions of denatured DNA,” Biochemistry, vol. 26, no. 20, pp. 6392–6396, 1987. View at: Publisher Site | Google Scholar
  22. A. I. Vogel, Text Book of Quantitative Inorganic Analysis, Longman, London, UK, 1986.
  23. M. J. Frisch, G. W. Trucks, H. B. Schlegel et al., Gaussian 09, Revision D, Gaussian, Inc., Wallingford, CT, USA, 2010.
  24. R. Dennington II, T. Keith, and J. Millam, Gauss View, Version 4.1.2, Semichem, Inc., Shawnee, KS, USA, 2007.
  25. M. M. Al-Iede, J. Karpelowsky, and D. A. Fitzgerald, “Recurrent diaphragmatic hernia: modifiable and non-modifiable risk factors,” Pediatric Pulmonology, vol. 51, no. 4, pp. 394–401, 2015. View at: Publisher Site | Google Scholar
  26. T. A. Halgren, “Merck molecular force field. I. Basis, form, scope, parametrization, and performance of MMFF94,” Journal of Computational Chemistry, vol. 17, no. 5-6, pp. 490–519, 1998. View at: Publisher Site | Google Scholar
  27. G. M. Morris, D. S. Goodsell, R. S. Halliday et al., “Automated docking using a Lamarckian genetic algorithm and an empirical binding free energy function,” Journal of Computational Chemistry, vol. 19, no. 14, pp. 1639–1662, 1998. View at: Publisher Site | Google Scholar
  28. F. J. Solis and R. J. B. Wets, “Minimization by random search techniques,” Mathematics of Operations Research, vol. 6, no. 1, pp. 19–30, 1981. View at: Publisher Site | Google Scholar
  29. W. J. Geary, “The use of conductivity measurements in organic solvents for the characterisation of coordination compounds,” Coordination Chemistry Reviews, vol. 7, no. 1, pp. 81–122, 1971. View at: Publisher Site | Google Scholar
  30. N. M. El-Metwaly, R. M. El-shazly, I. M. Gabr, and A. A. El-Asmy, “Physical and spectroscopic studies on novel vanadyl complexes of some substituted thiosemicarbazides,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 61, no. 16, pp. 1113–1119, 2005. View at: Publisher Site | Google Scholar
  31. K. S. Abu-Melha and N. M. El-Metwally, “Spectral and thermal studies for some transition metal complexes of bis(benzylthiocarbohydrazone) focusing on EPR study for Cu(II) and VO2+,” Spectrochimica Acta Part A: Molecular and Biomolecular Spectroscopy, vol. 70, no. 2, pp. 277–283, 2008. View at: Publisher Site | Google Scholar
  32. A. A. Abou-Hussen, N. M. El-Metwaly, E. M. Saad, and A. A. El-Asmy, “Spectral, magnetic, thermal and electrochemical studies on phthaloyl bis(thiosemicarbazide) complexes,” Journal of Coordination Chemistry, vol. 58, no. 18, pp. 1735–1749, 2005. View at: Publisher Site | Google Scholar
  33. A. B. P. Lever, Inorganic Electronic Spectroscopy, Elsevier, Amsterdam, Netherlands, 1986.
  34. B. J. Hathaway and D. E. Billing, “The electronic properties and stereochemistry of mono-nuclear complexes of the copper(II) ion,” Coordination Chemistry Reviews, vol. 5, no. 2, pp. 143–207, 1970. View at: Publisher Site | Google Scholar
  35. B. J. Hathaway, “A new look at the stereochemistry and electronic properties of complexes of the copper(II) ion,” Structure and Bonding, vol. 57, pp. 55–118, 1984. View at: Publisher Site | Google Scholar
  36. H. Montgomery and E. C. Lingefetter, “The crystal structure of Tutton’s salts. IV. Cadmium ammonium sulfate hexahydrate,” Acta Crystallographica, vol. 20, no. 6, pp. 728–730, 1966. View at: Publisher Site | Google Scholar
  37. D. Kivelson and R. Neiman, “ESR studies on the bonding in copper complexes,” Journal of Chemical Physics, vol. 35, no. 1, pp. 149–155, 1961. View at: Publisher Site | Google Scholar
  38. J. A. Wellman, F. B. Hulsbergen, J. Verbiest, and J. Reedijk, “Influence of alkyl chain length in N-alkyl imidazoles upon the complex formation with transition-metal salts,” Journal of Inorganic and Nuclear Chemistry, vol. 40, pp. 143–147, 1978. View at: Google Scholar
  39. U. Sagakuchi and A. W. Addison, “Spectroscopic and redox studies of some copper(II) complexes with biomimetic donor atoms: implications for protein copper centres,” Journal of the Chemical Society, Dalton Transactions, p. 600, 1979. View at: Publisher Site | Google Scholar
  40. H. Yokoi and A. W. Addison, “Spectroscopic and redox properties of pseudotetrahedralcopper(II) complexes. Their relation to copper proteins,” Inorganic Chemistry, vol. 16, no. 6, pp. 1341–1349, 1977. View at: Publisher Site | Google Scholar
  41. B. R. Mc Garvey, “The isotropic hyperfine interaction,” Journal of Physical Chemistry, vol. 71, no. 1, pp. 51–66, 1967. View at: Publisher Site | Google Scholar
  42. R. C. Chikate and S. B. padhye, “Transition metal quinone–thiosemicarbazone complexes 2: magnetism, ESR and redox behavior of iron (II), iron (III), cobalt (II) and copper (II) complexes of 2-thiosemicarbazido-1, 4-naphthoquinone,” Polyhedron, vol. 24, no. 13, pp. 1689–1700, 2005. View at: Publisher Site | Google Scholar
  43. B. D. Cullity, Elements of X-Ray Diffraction, Addison–Wesley Inc., Boston, MA, USA, 2nd edition, 1993.
  44. S. Velumani, X. Mathew, P. J. Sebastian, S. K. Narayandass, and D. Mangalaraj, “Structural and optical properties of hot wall deposited CdSe thin films,” Solar Energy Materials and Solar Cells, vol. 76, no. 3, pp. 347–358, 2003. View at: Publisher Site | Google Scholar
  45. F. A. Saad, N. M. El-Metwaly, T. A. Farghaly et al., “Illustration for series of new metal ion complexes extracted from pyrazolone derivative, spectral, thermal, QSAR, DFT/B3LYP, docking and antitumor investigations,” Journal of Molecular Liquids, vol. 229, pp. 614–627, 2017. View at: Publisher Site | Google Scholar
  46. J. H. Al-Fahemi, F. A. Saad, N. M. El-Metwaly et al., “Synthesis of Co(II), Cu(II), Hg(II), UO2(II) and Pb(II) binuclear nanometric complexes from multi-donor ligand: spectral, modeling, quantitative structure–activity relationship, docking and antitumor studies,” Applied Organometallic Chemistry, vol. 31, no. 11, p. e3787, 2017. View at: Publisher Site | Google Scholar
  47. J. M. Chen, W. Wei, W. X. L. Feng, and T. B. Lu, “CO2 fixation and transformation by a dinuclear copper cryptate under acidic conditions,” Chemistry–An Asian Journal, vol. 2, no. 6, pp. 710–714, 2007. View at: Publisher Site | Google Scholar
  48. A. Z. El-Sonbati, M. A. Diab, A. A. El-Bindary, M. M. Ghoneim, M. T. Mohesien, and M. K. Abd El-Kader, “Polymeric complexes—LXI. Supramolecular structure, thermal properties, SS-DNA binding activity and antimicrobial activities of polymeric complexes of rhodanine hydrazone compounds,” Journal of Molecular Liquids, vol. 215, pp. 711–739, 2016. View at: Publisher Site | Google Scholar
  49. U. El-Ayaan, N. M. El-Metwally, M. M. Youssef, and S. A. A. El Bialy, “Perchlorate mixed–ligand copper(II) complexes of β-diketone and ethylene diamine derivatives: thermal, spectroscopic and biochemical studies,” SpectrochimicaActa Part A, vol. 68, no. 5, pp. 1278–1286, 2007. View at: Publisher Site | Google Scholar
  50. R. K. Ray and G. R. Kauffman, “EPR spectra and covalency of bis(amidinourea/o-alkyl-1-amidinourea)copper (II) complexes. Part II. Properties of the CuN 42-chromophore,” Inorganica Chimica Acta, vol. 173, no. 12, pp. 207–214, 1990. View at: Publisher Site | Google Scholar
  51. S. Sagdinc, B. Köksoy, F. Kandemirli, and S. H. Bayari, “Theoretical and spectroscopic studies of 5-fluoro-isatin-3-(N-benzylthiosemicarbazone) and its zinc(II) complex,” Journal of Molecular Structure, vol. 917, no. 2-3, pp. 63–70, 2009. View at: Publisher Site | Google Scholar
  52. I. Fleming, Frontier Orbital’s and Organic Chemical Reactions, Wiley, London, UK, 1976.
  53. S. K. Tripathi, R. Muttineni, and S. K. Singh, “Extra precision docking, free energy calculation and molecular dynamics simulation studies of CDK2 inhibitors,” Journal of Theoretical Biology, vol. 334, pp. 87–100, 2013. View at: Publisher Site | Google Scholar
  54. M. M. Al-Iede, J. Karpelowsky, and D. A. Fitzgerald, “Recurrent diaphragmatic hernia: modifiable and non-modifiable risk factors,” Pediatric Pulmonology, vol. 51, no. 4, pp. 394–401, 2015. View at: Publisher Site | Google Scholar
  55. N. Terakado, S. Shintani, and Y. Nakahara, “Expression of Cu, Zn-SOD, Mn-SOD and GST-pi in oral cancer treated with preoperative radiation therapy,” Oncology Reports, vol. 7, no. 5, pp. 1113–1120, 2000. View at: Publisher Site | Google Scholar
  56. C. Fosset, B. A. McGaw, and M. D. Reid, “A non-radioactive method for measuring Cu uptake in HepG2 cells,” Journal of Inorganic Biochemistry, vol. 99, no. 5, pp. 1018–1022, 2005. View at: Publisher Site | Google Scholar

Copyright © 2018 Gamil A. Al-Hazmi et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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