# Synthesis, Spectral Characterization, and Thermal and Cytotoxicity Studies of Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) Complexes of Schiff Base Derived from 5-Hydroxymethylfuran-2-carbaldehyde

Authors: Amani S. Alturiqi; Abdel-Nasser M. A. Alaghaz; Reda A. Ammar; Mohamed E. Zayed
Journal: Journal of Chemistry
 (2018)

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## Abstract

Coordination compounds of Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) ions were synthesized from the furan ligand [5-hydroxymethylfuran-2-yl-methyleneaminoquinolin-2-one] (H-MFMAQ) derived from the condensation of 5-hydroxymethylfuran-2-carbaldehyde and 1-aminoquinolin-2(1H)-one. Elemental analytical data, IR, NMR (1H, 13C, and 15N), EPR, XRD, SEM, TEM, EDX, TGA, mass, molar conductance, magnetic moment, and UV-Visible spectra techniques were used to confirm the structure of the synthesized chelates. According to the data obtained, the composition of the 1 : 1 metal ions : furan Schiff base ligand was found to be [M(MFMAQ)Cl2] (M = Cr(III) and Ru(III)) and [M(MFMAQ)Cl(H2O)]·nH2O in which (M = Mn(II); n=1, Co(II); n=0, Ni(II); n=2, Cu(II); n=0 and Zn(II); n=2.5). The measurements of magnetic susceptibility, ligand field parameter, and reflectance spectra suggested an octahedral geometry for the complexes. Central metals ions and furan Schiff base coordinated via O3 and N donor sites which was observed from IR spectra. The cytotoxic activities of all inspected compounds were evaluated towardshuman breast(MCF-7)and lung cancer(A549)cell lines.


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## Body

## 1. Introduction

Transition metal complexes derived from the Schiff base ligands with biological potency have been broadly studied. Schiff bases appear to be an important intermediate in a number of enzymatic reactions including interaction of an enzyme with an amino or a carbonyl group of the substrate. The biochemical process which involves the condensation of a primary amine in an enzyme may be one of the most important catalytic mechanisms kinds [1]. Transition metal complexes with different oxidation states have a strong role in bioinorganic chemistry and may give the models basis for active sites of biological systems [2–4]. For a long time, it had been identified as a serious cofactor in biological compounds, either as a compositional template in protein folding or as a Lewis acid catalyst which can readily adopt the coordination numbers 4, 5, or 6 [5, 6]. Coordination chemistry of cobalt complexes was a substantial importance as a result of the toxic environmental effect of cobalt. The cobalt mobilization and immobilization in the climate, organisms, and approximately technical systems (such as in ligand exchange chromatography) have been presented manifestly to depend on the complexation of the metal center by chelating nitrogen donor ligands [7]. The size and shape of the nanomaterials are considered the key factors for shaping their characteristics such as electrical, optical, magnetic, antimicrobial, and catalytic potency. Metal and metal oxide nanoparticles have found a wide range of uses, including heterogeneous catalysts, environmental remediation, electronics, chemical sensing devices, medicinal fields, separations, thin films, inks, disinfection, and antimicrobial activity [8]. These different applications altered with morphology and size of those metal and metal oxide nanoparticles [9]. Detection of metal ions of biological importance has attracted much attention. Like Zn2+ ion fluorescent probes or sensors have achieved special interest. Zn2+ is an essential trace element and the second (after Cu2+) most abundant metal ion in humans [10, 11]. In our present work, novel [M(MFMAQ)Cl2] (M = Cr(III) and Ru(III)) and [M(MFMAQ)Cl(H2O)]·nH2O (M = Mn(II); n=1, Co(II); n=0, Ni(II); n=2, Cu(II); n=0 and Zn(II); n=2.5) complexes were discussed using different studding techniques such as elemental analyses, molar conductance, magnetic moment, and UV–Vis., IR, NMR (1H, 13C and 15N), mass, EPR, XRD, SEM, TEM, EDX, and TGA behavior. Also, the ligand (H-MFMAQ) and its complexes show remarkable cytotoxicity againsthuman breast (MCF-7) andlung cancer (A549) cell lines.


## 2. Experimental

### 2.1. Materials and Methods

All the metal salts were gained from E-Merck and used without further purification. Solvents MeOH, EtOH, DMF, DMSO, and agar were procured from Hi-media chemicals. However, the solvents were purified by the standard procedures. Elemental analyses were performed on a Perkin Elmer 2400 CH/N Analyzer. Metal contents were determined complexometrically by standard EDTA titration and the Cl was tested gravimetrically using AgNO3. Electronic spectra of the complexes were recorded on a Shimadzu Model 1601 UV-Visible Spectrophotometer. Infrared spectroscopy measurements were performed on an Agilent Cary 630 FTIR spectrometer, using the Attenuated Total Reflectance (ATR) method, with a diamond cell. Spectra were recorded from 4000 to 400 cm–1, with 64 scans and resolution of 4 cm–1. The 1H and N15,H1 correlation NMR spectra of samples were recorded in a Bruker Avance III 500 MHz (11.7 T) spectrometer. The 1H NMR spectrum of samples was recorded in a Bruker Avance III 600 MHz (14 T) spectrometer. The N15,H1 NMR correlation spectrum of samples was recorded in a Bruker Avance III 400 MHz (9.4 T) spectrometer. The samples were analyzed in a d6-DMSO solution and the chemical shifts were given relative to tetramethylsilane (TMS). The 13C and 15N solid state NMR (SSNMR) spectra were recorded in a Bruker 300 MHz spectrometer, using the combination of cross-polarization, proton decoupling, and magic angle spinning (CP/MAS) at 10 kHz. Electrospray ionization mass spectrometry (ESI-MS) measurements were carried out using a Waters Quattro Micro API. Samples were evaluated in the positive mode. Ligand was analyzed in a 1 : 1 methanol : water solution with addition of 0.10% (v/v) formic acid; Cu(II) complex was analyzed in a 1 : 1 acetonitrile : water with 0.10% (v/v) formic acid; Co(II) and Ru(III) complexes were dissolved in a minimum amount of DMF and further dissolved in a 1 : 1 methanol : water solution with addition of 0.10% (v/v) formic acid immediately before the experiments. Each solution was directly infused into the instrument’s ESI source and analyzed in the positive mode, with capillary potential of 3.00 kV, trap potential of 2 kV, source temperature of 150°C, and nitrogen gas for desolvation. Room temperature magnetic susceptibility measurements were carried out on a modified Gouy-type magnetic balance, Hertz SG8-5HJ. The room temperature molar conductivity of the complexes in MeOH, EtOH, and DMSO solutions (0,001 mol·L−1) was measured using a deep vision 601 model digital conductometer. The X-band EPR spectrum was performed at LNT (77 K) using TCNE as the g-marker. Powder X-ray diffraction patterns were recorded with a X’Pert PRO Diffractometer using CuKα1 radiation (λ = 1.54060 Å) with operating voltage 40 kV and a current of 30 mA. Thermal studies were carried out using Q 600SDT and Q 20 DSC thermal analyzer. SEM images were recorded in a Hitachi SEM analyzer and transmission electron microscopy (TEM) images were taken by Zeiss-EM10C-100 KV. Energy Dispersive X-Ray Analysis (EDX) (EDAX Falcon System) was conducted to analyze the presence of elements in the specimens that have been sputtered with carbon black. The cytotoxic activity of the inspected free ligand and complexes (1–7) was studied towardshuman breast (MCF-7) andlung cancer (A549) cell lines at the Regional Center for Microbiology and Biotechnology, Al-Azhar University as well as the other biological activities.


### 2.2. Synthesis of Schiff Base Ligand (H-MFMAQ)

New Schiff base ligand (H-MFMAQ) (Scheme1) was prepared when 5-hydroxymethylfuran-2-carbaldehyde (1.24 g, 11.23 mmol) was added to 1-aminoquinolin-2(1H)-one (1.79 g, 11.23 mmol), both dissolved in absolute ethanol (50 ml). Mixture was heated under reflux for 3 h to be a pale-yellow precipitate and was formed upon cooling the solution to room temperature. The product was filtered off and washed with few amounts of ethanol then diethyl ether, air-dried, and recrystallized from ethanol. The yield was 2.77 g (91%). The physical properties and analytical data of the furan Schiff base ligand and its metal complexes are scheduled in Table 1.Table 1
Analytical and physical data of the ligand H-MFMAQ and complexes 1–7.
Number Compound(formula wt.) [M.Wt.] Color M.P.  °C Yield% Elemental analysis calc. (found) C% H% N% Cl% M% H-MFMAQ(C15H12N2O3)  [268.3] Pale yellow 146 91 67.16 (67.13) 4.51 (4.49) 10.44 (10.42) -- -- 1 [Cr(MFMAQ)Cl2] (C15H11Cl2CrN2O3) [390.2] Dark brown 211 78 46.18 (46.12) 2.84 (2.82) 7.18 (7.14) 18.17 (18.11) 13.33 (13.32) 2 [Ru(MFMAQ)Cl2] (C15H12Cl2N2O3Ru) [439.2] Black 219 83 41.02 (40.97) 2.52 (2.50) 6.38 (6.34) 16.14 (16.10) 23.01 (23.00) 3 [Mn(MFMAQ)Cl(H2O)]·H2O (C15H15ClMnN2O5) [393.7] Wine red 224 82 45.76 (45.73) 3.84 (3.83) 7.12 (7.11) 9.00 (8.98) 13.95 (13.91) 4 [Co(MFMAQ)Cl(H2O)] (C15H13ClCoN2O4) [379.7] Olive 218 84 47.45 (47.42) 3.45 (3.43) 7.38 (7.33) 9.34 (9.32) 15.52 (15.50) 5 [Ni(MFMAQ)Cl(H2O)]2H2O (C15H17ClN2NiO6) [415.5] Brown 226 77 43.37 (43.34) 4.12 (4.10) 6.74 (6.72) 8.53 (8.51) 14.13 (14.10) 6 [Cu(MFMAQ)Cl(H2O)] (C15H13ClCuN2O4) [384.3] Grass green 233 86 46.88 (46.83) 3.41 (3.38) 7.29 (7.23) 9.23 (9.20) 16.54 (16.51) 7 [Zn(MFMAQ)Cl(H2O)]·2.5H2O (C15H18ClN2O6.5Zn) [431.1] Yellow 208 73 41.79 (41.72) 4.21 (4.18) 6.50 (6.48) 8.22 (8.19) 15.16 (15.12)Scheme 1
Synthetic route of ligand H-MFMAQ.


### 2.3. Synthesis of Schiff Base Metal(II/III) Complexes

A mixture of furan Schiff base ligand H-MFMAQ (6.76 mmol; 1.81 g) dissolved in an ethanol (20 ml) and chloride salt of Cr (III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), or Zn (II) (6.76 mmol) dissolved in the same solvent (20 ml) was heated for two hours under reflux on a water bath. The formed precipitate was filtered off, washed with ethanol and diethylether, and finally dried to give [Cr(MFMAQ)Cl2] (1), [Ru(MFMAQ)Cl2] (2), [Mn(MFMAQ)Cl(H2O)]·H2O (3), [Co(MFMAQ)Cl(H2O)] (4), [Ni(MFMAQ)Cl(H2O)]·2H2O (5), [Cu(MFMAQ)Cl(H2O)] (6), and [Zn(MFMAQ)Cl(H2O)]·2.5H2O (7) complexes.


## 2.1. Materials and Methods

All the metal salts were gained from E-Merck and used without further purification. Solvents MeOH, EtOH, DMF, DMSO, and agar were procured from Hi-media chemicals. However, the solvents were purified by the standard procedures. Elemental analyses were performed on a Perkin Elmer 2400 CH/N Analyzer. Metal contents were determined complexometrically by standard EDTA titration and the Cl was tested gravimetrically using AgNO3. Electronic spectra of the complexes were recorded on a Shimadzu Model 1601 UV-Visible Spectrophotometer. Infrared spectroscopy measurements were performed on an Agilent Cary 630 FTIR spectrometer, using the Attenuated Total Reflectance (ATR) method, with a diamond cell. Spectra were recorded from 4000 to 400 cm–1, with 64 scans and resolution of 4 cm–1. The 1H and N15,H1 correlation NMR spectra of samples were recorded in a Bruker Avance III 500 MHz (11.7 T) spectrometer. The 1H NMR spectrum of samples was recorded in a Bruker Avance III 600 MHz (14 T) spectrometer. The N15,H1 NMR correlation spectrum of samples was recorded in a Bruker Avance III 400 MHz (9.4 T) spectrometer. The samples were analyzed in a d6-DMSO solution and the chemical shifts were given relative to tetramethylsilane (TMS). The 13C and 15N solid state NMR (SSNMR) spectra were recorded in a Bruker 300 MHz spectrometer, using the combination of cross-polarization, proton decoupling, and magic angle spinning (CP/MAS) at 10 kHz. Electrospray ionization mass spectrometry (ESI-MS) measurements were carried out using a Waters Quattro Micro API. Samples were evaluated in the positive mode. Ligand was analyzed in a 1 : 1 methanol : water solution with addition of 0.10% (v/v) formic acid; Cu(II) complex was analyzed in a 1 : 1 acetonitrile : water with 0.10% (v/v) formic acid; Co(II) and Ru(III) complexes were dissolved in a minimum amount of DMF and further dissolved in a 1 : 1 methanol : water solution with addition of 0.10% (v/v) formic acid immediately before the experiments. Each solution was directly infused into the instrument’s ESI source and analyzed in the positive mode, with capillary potential of 3.00 kV, trap potential of 2 kV, source temperature of 150°C, and nitrogen gas for desolvation. Room temperature magnetic susceptibility measurements were carried out on a modified Gouy-type magnetic balance, Hertz SG8-5HJ. The room temperature molar conductivity of the complexes in MeOH, EtOH, and DMSO solutions (0,001 mol·L−1) was measured using a deep vision 601 model digital conductometer. The X-band EPR spectrum was performed at LNT (77 K) using TCNE as the g-marker. Powder X-ray diffraction patterns were recorded with a X’Pert PRO Diffractometer using CuKα1 radiation (λ = 1.54060 Å) with operating voltage 40 kV and a current of 30 mA. Thermal studies were carried out using Q 600SDT and Q 20 DSC thermal analyzer. SEM images were recorded in a Hitachi SEM analyzer and transmission electron microscopy (TEM) images were taken by Zeiss-EM10C-100 KV. Energy Dispersive X-Ray Analysis (EDX) (EDAX Falcon System) was conducted to analyze the presence of elements in the specimens that have been sputtered with carbon black. The cytotoxic activity of the inspected free ligand and complexes (1–7) was studied towardshuman breast (MCF-7) andlung cancer (A549) cell lines at the Regional Center for Microbiology and Biotechnology, Al-Azhar University as well as the other biological activities.


## 2.2. Synthesis of Schiff Base Ligand (H-MFMAQ)

New Schiff base ligand (H-MFMAQ) (Scheme1) was prepared when 5-hydroxymethylfuran-2-carbaldehyde (1.24 g, 11.23 mmol) was added to 1-aminoquinolin-2(1H)-one (1.79 g, 11.23 mmol), both dissolved in absolute ethanol (50 ml). Mixture was heated under reflux for 3 h to be a pale-yellow precipitate and was formed upon cooling the solution to room temperature. The product was filtered off and washed with few amounts of ethanol then diethyl ether, air-dried, and recrystallized from ethanol. The yield was 2.77 g (91%). The physical properties and analytical data of the furan Schiff base ligand and its metal complexes are scheduled in Table 1.Table 1
Analytical and physical data of the ligand H-MFMAQ and complexes 1–7.
Number Compound(formula wt.) [M.Wt.] Color M.P.  °C Yield% Elemental analysis calc. (found) C% H% N% Cl% M% H-MFMAQ(C15H12N2O3)  [268.3] Pale yellow 146 91 67.16 (67.13) 4.51 (4.49) 10.44 (10.42) -- -- 1 [Cr(MFMAQ)Cl2] (C15H11Cl2CrN2O3) [390.2] Dark brown 211 78 46.18 (46.12) 2.84 (2.82) 7.18 (7.14) 18.17 (18.11) 13.33 (13.32) 2 [Ru(MFMAQ)Cl2] (C15H12Cl2N2O3Ru) [439.2] Black 219 83 41.02 (40.97) 2.52 (2.50) 6.38 (6.34) 16.14 (16.10) 23.01 (23.00) 3 [Mn(MFMAQ)Cl(H2O)]·H2O (C15H15ClMnN2O5) [393.7] Wine red 224 82 45.76 (45.73) 3.84 (3.83) 7.12 (7.11) 9.00 (8.98) 13.95 (13.91) 4 [Co(MFMAQ)Cl(H2O)] (C15H13ClCoN2O4) [379.7] Olive 218 84 47.45 (47.42) 3.45 (3.43) 7.38 (7.33) 9.34 (9.32) 15.52 (15.50) 5 [Ni(MFMAQ)Cl(H2O)]2H2O (C15H17ClN2NiO6) [415.5] Brown 226 77 43.37 (43.34) 4.12 (4.10) 6.74 (6.72) 8.53 (8.51) 14.13 (14.10) 6 [Cu(MFMAQ)Cl(H2O)] (C15H13ClCuN2O4) [384.3] Grass green 233 86 46.88 (46.83) 3.41 (3.38) 7.29 (7.23) 9.23 (9.20) 16.54 (16.51) 7 [Zn(MFMAQ)Cl(H2O)]·2.5H2O (C15H18ClN2O6.5Zn) [431.1] Yellow 208 73 41.79 (41.72) 4.21 (4.18) 6.50 (6.48) 8.22 (8.19) 15.16 (15.12)Scheme 1
Synthetic route of ligand H-MFMAQ.


## 2.3. Synthesis of Schiff Base Metal(II/III) Complexes

A mixture of furan Schiff base ligand H-MFMAQ (6.76 mmol; 1.81 g) dissolved in an ethanol (20 ml) and chloride salt of Cr (III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), or Zn (II) (6.76 mmol) dissolved in the same solvent (20 ml) was heated for two hours under reflux on a water bath. The formed precipitate was filtered off, washed with ethanol and diethylether, and finally dried to give [Cr(MFMAQ)Cl2] (1), [Ru(MFMAQ)Cl2] (2), [Mn(MFMAQ)Cl(H2O)]·H2O (3), [Co(MFMAQ)Cl(H2O)] (4), [Ni(MFMAQ)Cl(H2O)]·2H2O (5), [Cu(MFMAQ)Cl(H2O)] (6), and [Zn(MFMAQ)Cl(H2O)]·2.5H2O (7) complexes.


## 3. Results and Discussions

### 3.1. Ligand (H-MFMAQ)

H-MFMAQ percentage of purity was 99.97%; it has been measured by HPLC. Mass spectrum of the furan Schiff base ligand (H-MFMAQ) (Figure1(a)) has final peak at 268 amu corresponding to the furan Schiff base ligand moiety [C15H12N2O3] (atomic mass 268 amu) (Scheme 2). Other peaks like 52, 82, 148, 152, 208, and 227 amu were suggested according to diverse fragments. From this study, it was found that the intensity of the peaks gave information on the stability of fragmentation. The electronic spectrum of furan Schiff base ligand (H-MFMAQ) in ethanol exhibited five absorption bands (Figure 2(a)) at 233–338 nm regions which is due to π→π∗ and n→π∗ transitions utilizing molecular orbital of the quinoline and furan rings, C=N and C=O groups. Nevertheless, the IR spectrum of furan Schiff base ligand (H-MFMAQ) (Figure 3(a)) does not show any band at 1700 cm–1, 3380 cm–1, and 3250 cm–1 corresponding to the carbonyl groups and free primary amino groups; this confirms the complete condensation between keto and amino groups. The band at 1637 cm–1 is corresponding to ν (CH=N) stretching vibration. The IR spectrum of furan Schiff base ligand (H-MFMAQ) displays a broad band at 3483 cm–1, which can be assigned to ν(OH) group. The 1H-NMR spectra of the furan Schiff base ligand (H-MFMAQ) (Figure 4(a)) exhibit signals due to aromatic protons as multiplet at δ 6.80–7.23 (8H) and a broad signal at δ (11.35) ppm is assigned for O–H proton, which disappeared with addition of D2O due to the proton exchange. In 13C NMR of ligand (H-MFMAQ) (Figure 5(a)) (–C=O) carbonyl carbon showed signal at 166.47 ppm, (–C=N–) azomethine carbon at 162.12 ppm, (–C–O) phenolic group carbon at 158.27 ppm, and (C–O) furan ring at 170.12. The spectrum 15N-NMR of the ligand (H-MFMAQ) (Figure 6(a)) shows two signals centered 244.3 and 163.3 ppm, which were assigned to N12 (azomethine) and N1 (quinoline), respectively.Scheme 2
Mass fragmentation pattern of furan Schiff base ligand (H-MFMAQ).Figure 1
Mass spectrum of (a) ligand, (b) Co(II) complex, (c) Cu(II) complex, and (d) Ru(III) complex.
(a) (b) (c) (d)Figure 2
Electronic spectrum of (a) ligand and (b) Ru(III) complex.
(a) (b)Figure 3
(a) IR spectrum of ligand, (b) IR spectrum of Cr(III) complex, and (c) IR spectrum of Zn(II) complex.
(a)
H-MFMAQ (b)
[Cr(MFMAQ)Cl2] (c)
[Co(MFMAQ)Cl(H2O)]Figure 4
1H NMR spectra of (a) Schiff base ligand and (b) Zn(II) complex.Figure 5
13C NMR spectra of (a) Schiff base ligand and (b) Zn(II) complex.Figure 6
15N NMR spectra of (a) Schiff base ligand and (b) Zn (II) complex.


### 3.2. Complexes

The empirical formulae of complexes showing number of water molecules are presented in Table1. All synthesized solid complexes are stable in air. They are practically insoluble in water, but on the contrary quite soluble in polar organic solvents (e.g., EtOH, MeOH, DMF, and DMSO). The structures of the complexes could not be determined because single crystals were not obtained. The molar conductivity data (Table 2) clearly indicate that all complexes in MeOH and DMSO as well as Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes in MeOH, DMF, and DMSO are in the range 7.58–15.24 Ω–1cm2mol–1 indicating the nonelectrolytic nature of all complexes [12]. This finding is consistent with the infrared spectral data that showed the coordinated nature of chloride anions.Table 2
Molar conductivity of complexes Λ M/Ω−1 cm2 mol−1 for 0,001 mol·L−1 solutions in MeOH, DMF, and DMSO at 25°C.
Complex Λ M  [Ω−1 cm2 mol−1] MeOH DMF DMSO [Cr(MFMAQ)Cl2] 14.36 15.24 7.58 [Ru(MFMAQ)Cl2] 12.87 14.25 9.77 [Mn(MFMAQ)Cl(H2O)]·H2O 12.42 14.85 8.56 [Co(MFMAQ)Cl(H2O)] 11.57 13.93 8.45 [Ni(MFMAQ)Cl(H2O)]·2H2O 12.84 14.47 9.27 [Cu(MFMAQ)Cl(H2O)] 10.75 13.74 7.89 [Zn(MFMAQ)Cl(H2O)]·2.5H2O 11.59 14.66 8.98


#### 3.2.1. Mass Spectra of Complexes

The ESI mass spectrum of the Co(II) complex [Co(MFMAQ)Cl(H2O)] (Figure 1(b)) shows the parental ion peak at m/z = 379 corresponding to (CoC15H13ClN2O4)+. The other fragments of the complex give the peak with various intensities at different m/z values like at 74 (CoO)+, 77 (C6H5)+, 144 (CoC4H7NO)+, and 326 (CoC15H11N2O3)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 3.Scheme 3
Mass fragmentation pattern of Co(II) complex [Co(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Cu(II) complex [Cu(MFMAQ)Cl(H2O)] (Figure 1(c)) shows the parental ion peak at m/z = 384 corresponding to (CoC15H13ClN2O4)+. The different fragments of the complex with different m/z values are present at 97 (C5H7NO)+, 120 (C7H8N2)+, 202 (CuC6H7N2O2)+, and 326 (CuC13H11ClN2O2). This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 4.Scheme 4
Mass fragmentation pattern of Cu(II) complex [Cu(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Ru(III) complex [Ru(MFMAQ)Cl2] (Figure 1(d)) shows the molecular ion peak at m/z = 439 corresponding to (RuC15H11Cl2N2O3)+. The other fragments of the complex show the peaks at different m/z values like at 56 (C4H8)+, 210 (RuC6H7NO)+, 158 (C10H10N2)+, 263 (RuC8H6N2O2)+, and 326 (RuC11H14N2OCl)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 5. These facts were matched to the suggested molecular formula for these complexes, that is, [Co(MFMAQ)Cl(H2O)], [Cu(MFMAQ)Cl(H2O)], and [Ru(MFMAQ)Cl2], where MFMAQ is the ligand. This confirms the Schiff base frame formation. Elemental analysis values were appropriate with those values calculated from the molecular formulae assigned to these complexes which are further supported by mass studies.Scheme 5
Mass fragmentation pattern of Ru(II) complex [Cu(MFMAQ)Cl2].


#### 3.2.2. Electronic Absorption, Magnetic Measurements, and Ligand Field Parameter

The electronic absorption spectra of the free Schiff base ligand and its complexes (Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II)) were studied in Nujol mull.Two bands were showed at 18,995 (ε = 46 Lmol−1 cm−1) and 16,238 cm–1 (ε = 34 Lmol−1 cm−1); for Cr(III) complex [Cr(MFMAQ)Cl2] electronic spectrum, those may be consigned to 4A2g(F)→4T1g(F) and 4A2g(F)→4T2g(F) transitions, respectively, in an octahedral geometry [13], whereas the third band, which is due to 4A2g (F)→4T1g (P) transition, lies in the range of the ligand transitions that were predicted at 34,264 cm–1 (ε = 132 Lmol−1 cm−1). The ligand field parameters of the current Cr(III) complex have been calculated using Tanabe-Sugano diagrams B (583 cm–1), 10Dq (1742 cm–1), and β (0.53). The effective magnetic moment of the complex is 3.92 BM, which is consistent with the spin-only value for three unpaired electrons (3.87 BM) [14].Electronic spectrum of Mn(II) complex [Mn(MFMAQ)Cl(H2O)]·H2O exhibits four weak intensity absorption bands at 17,943 (ε = 30 Lmol-1cm−1), 22,806 (ε = 36 Lmol−1 cm−1), 27,216 (ε = 64 mol−1 cm−1), and 37,489 cm−1 (ε = 138 Lmol−1 cm−1). These bands may be assigned to the transitions: 6A1g→4T1g (4G), 6A1g→ 4Eg, 4A1g (4G) (10B + 5C), 6A1g→4Eg (4D) (17B + 5C), and 6A1g→ 4T1g (4P) (7B + 7C), respectively. The ligand parameters B and C were calculated from the second and third electronic transitions because these electronic transitions are free from the crystal field splitting and depend on B and C parameters [13, 14]. The calculated values of the ligand field parameters are given in Table 3. Room temperature magnetic moment of the Mn(II) complex lies at 5.94 BM; this value is in tune with a high-spin octahedral configuration.Table 3
Ligand field parameters of the complexes.
Complex Dq (cm−1) B (cm−1) β LFSE (kJmol−1) [Cr(MFMAQ)Cl2] 1674 792 0.88 208.68 [Ru(MFMAQ)Cl2] – – – – [Mn(MFMAQ)(H2O)Cl]·H2O 1168 808 0.73 100.47 [Co(MFMAQ)(H2O)Cl] 792 – 0.95 114.23 [Ni(MFMQ)(H2O)Cl]·2H2O – – – – [Cu(MFMAQ)Cl(H2O)]  492 0.81 – [Zn(MFMAQ)Cl(H2O)]2.5H2O – – – –The electronic spectrum of cobalt (II) complex [Co(MFMAQ)Cl(H2O)] recorded in Nujol mulls exhibits three absorption peaks at 13,897 (ε = 24 Lmol−1 cm−1), 15,368 (ε = 27 Lmol−1 cm−1), and 25,157 (ε = 53 Lmol−1 cm−1) cm–1, respectively. These bands can be assigned to 4T1g→4T2g (F)(ν1), 4T1g→4A2g (F)(ν2), and 4T1g→4T1g (P)(ν3) transitions, respectively, suggesting an octahedral geometry around Co(II) ion [13, 14]. Octahedral cobalt(II) complex, however, preserves a large orbital contribution to magnetic moment on account of 4T1g (F) ground term and exhibits μeff in the range 4.8–5.6 B.M [15]. The magnetic measurements reported here lie at 5.18 BM and demonstrate that the Co(II) complex was paramagnetic and has a high-spin octahedral configuration with 4T1g(F) ground state.The ligand field parameters (Table3) B (interelectronic repulsion of the d-electrons in complex), β (The Nephelauxetic effect), and 10Dq are calculated according to the equation reported for the octahedral Co(II) complex.(1)μeff=4.981-4λ=10Dq,λ=-178cm-1B=4ν3-15Dq2-10Dq260ν3-15Dq-180Dqν1=10Dqβ=BcomplexBfree  ion,where B (free ion) for Co(II) is 996 cm−1. The 10Dq, B, and β values are 7032 cm−1, 698 cm−1, and 0.68, respectively. These results show that the interelectronic repulsion of d-electrons in a complex is less than in the free ion. The value of B in a complex is 78% of the free ion value. The β value is related directly to covalence.The reduction ofB is caused by complex formation by the delocalization of the d-electron cloud on the ligand, which in turn causes the covalent bond formation. The data shows the Co(II) complex has covalent character in the metal ligand “σ” bond [15].Electronic spectrum of [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows bands at 15,053 (ε = 23 Lmol−1 cm−1), 17,892 (ε = 28 Lmol−1 cm−1), and 22,111 cm–1 (ε = 43 Lmol−1 cm−1). These bands may be specified to A32g(F)→3T2g(F)(ν1), 3A2g(F)→3T1g(F)(ν2), and 3A2g(F)→3T1g(P)(ν3) transitions, respectively. It proposes octahedral geometry of [Ni(MFMAQ)Cl(H2O)]·2H2O complex [13, 14]. The magnetic moment was evaluated which gave 3.08 μB, for [Ni(MFMAQ)Cl(H2O)]·2H2O complex which lies in the extent (2.9–3.3 μB) of the Ni(II) octahedral complexes [15]. The Nephelauxetic parameter β (Table 3) was readily obtained by utilizing the correlation β = B (complex)/B (free ion), where B (free ion) for Ni(II) is 1041 cm–1 [15]. The value of β lies at 0.27. These values indicated the covalent character in metal ligand “σ” bond [13].The Cu(II) complex [Cu(MFMAQ)Cl(H2O)] spectrum displayed a band at 22,137 cm−1 (ε = 41 Lmol−1 cm−1) assigned to 2Eg→2T2g transition assuming octahedral geometry around the central Cu(II) ion [15]. The emulated magnetic moment of the Cu(II) complex is 1.98 BM, which assures the octahedral structure of this complex [15].The electronic spectrum of ruthenium(III) complex [Ru(MFMAQ)Cl2] records three bands at 15,167 (ν1) (ε = 22 Lmol−1 cm−1), 17,353 (ν2) (ε = 27 Lmol−1 cm−1), and 25,158 cm−1 (ν3) (ε = 61 Lmol−1 cm−1) (Figure 2(b)). These bands may be assigned to 2T2g→ 4T1g, 2T2g→ 4T2g, and 2T2g→4A1g transitions in order of increasing energy. The position of bands is in tune with the prediction for octahedral complexes of the metal ions [13]. The ligand field parameters Δ,B, and β have been calculated by using the relation(2)ν1=Δ-4B+86B2Δν2=Δ+12B+2B2Δσ.The value of B in free ion is 638 cm−1. The value of β indicates that there is low covalency in the metal ligand σ-band [16]. The Ru(III) complex shows magnetic moments at room temperature 1.76 BM, which is lower than the predicted value of 2.17 BM. The lowering in μeff values may be due to lower symmetry ligand fields, metal-metal interaction, or extensive electron delocalization [14].The Zn(II) complex [Zn(MFMAQ)Cl(H2O)]·2.5H2O is diamagnetic as predictable and its geometry is most likely octahedral likewise Mn(II), Cu(II), Ni(II), and Co(II) complexes of H-MFMAQ ligand [15].


#### 3.2.3. Infrared Spectra of Complexes

The study of infrared spectra of the furan Schiff base H-MFMAQ comparing to their metal complexes (1–7) (Table4; Figure 3) foremost revealed that the ligand is tetradentately coordinated to the metal ions. The bands were symbolized at 1712 and 1637 cm–1 due to the carbonyl and azomethine stretching vibration which was shifted to lower frequency by 14–19 and 12–16 cm–1, suggesting oxygen carbonyl and nitrogen azomethine involvements in complexity. At 1618 cm–1, the band was assigned to the furan ring ν(C–O–C) vibrations which is also shifted to lower frequency by 13–18 cm–1, which is suggestive to involvement of the furan ring in chelation. Also, at 3483 cm–1, the band was attributed to νOH in the ligand (H-MFMAQ) which disappeared in its metal complexes indicating deprotonation of the OH moiety during coordination [17]. The new bands at 543–552, 433–438, and 412–416 cm−1 were assigned to M–O (carbonyl), M–O (phenol), M–N (azomethine) and (M–Cl) in the metal complexes spectra were observed [15, 17]. The IR results showed that the metal was harmonized through one nitrogen atom (azomethine group) and three oxygen atoms (deprotonated hydroxyl group, carbonyl group, and furan ring) besides chlorine atoms.Table 4
IR spectral data (cm−1) of the H-MFMAQ ligand and its metal complexes.
Number ν O H ν ( O H ) w a t e r ν C = O ν C = N ν ( C - O – C ) f u r a n ν M – O ν M – N ν M – C l H-MFMAQ 3483br – 1712m 1637m 1618m – – – 1 – – 1693w 1621m 1600m 543m 433w 416m 2 – – 1698m 1622m 1600w 548s 434w 412w 3 – 3320br 1695s 1622m 1605w 552m 438m 414m 4 – 3300r 1693m 1625sh 1602m 547m 434m 41 m 5 – 3320br 1697m 1624m 1605m 552m 437m 413m 6 – 3300r 1696m 1625m 1604m 549m 435m 414m 7 – 3318br 1698m 1623m 1603m 547m 438m 415m sh: sharp, m: medium, br: broad, s: small, and w: weak.


#### 3.2.4. NMR Spectra Investigation

The proton NMR spectroscopy of H-MFMAQ ligand (Figure4(a)) and its [Zn(MFMAQ)Cl(H2O)]2.5H2O complex (Figure 4(b)) was evident in DMSO-d6 solution employing tetramethylsilane (TMS) as internal standard. OH signal was found at 11.35 ppm in the spectrum of the ligand H-MFMAQ which completely disappeared in the spectrum of the [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. This suggests the sharing of the OH group in chelation with Zn(II) through isolation of the OH proton. The azomethine proton signal was shifted to high field in the spectrum of [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. It was looked at 8.13 ppm as compared to 8.67 ppm in the Schiff’s base H-MFMAQ. This refers to the complexity of the zinc atom through nitrogen atom azomethine. However, multiple bands assigned to the aromatic protons were found at 6.92–7.97 and 6.98–7.96 ppm in the free Schiff 22 base ligand and Zn(II) complex, respectively. The signal observed at 3.2 ppm with an integration corresponding to seven protons in the case of Zn(II) complex was assigned one coordinate water molecule and half past two hydrate water molecules.In13C NMR of ligand (Figure 5(a)) (–C=O) carbonyl carbon showed signal at 166.47 ppm, (–C=N–) azomethine carbon at 162.12 ppm, (–C–O) phenolic group carbon at 158.27 ppm, and (C–O) furan ring at 170.12. The signals due to (–C=N–) azomethine, (–C–O) phenolic, and (C–O) furan carbons were slightly shifted downfield in comparison to the corresponding signals of these groups in the ligand thereby confirming the complexation (Figure 5(b)) with zinc metal ion.The15N NMR spectra of the free ligand (Figure 6(a)) and the Zn(II) complex (Figure 6(b)) were also obtained. The spectrum of the ligand shows two signals centered at 244.3 and 163.3 ppm, which were assigned to N12 (azomethine) and N1 (quinoline), respectively. In the spectrum of Zn(II) complex only one broad signal is observed for the nitrogen atoms at 162.7 ppm. This behavior led us to assign the broad signal in the spectra of the complexes as both N12 and N1 atoms. With this assignment, N12 shifted 81.6 ppm downfield upon coordination to Zn(II). On the other hand, the nitrogen N1 shifts only 0.6 ppm upon coordination with Zn(II). This minor shift indicates that this atom is not involved in coordination as already evidenced by other techniques.


#### 3.2.5. ESR Spectra

The ESR spectrum of the [Cr(MFMAQ)Cl2] complex (Table 5) has been recorded as polycrystalline sample at room temperature. No hyperfine interaction was observed in the ESR spectra of the [Cr(MFMAQ)Cl2] complex at room temperature. The g-values are calculated by using the expression, g = 2.0023(1-4λ/10Dq), whereλis the spin–orbit coupling constant for the metal ion in the complex. Owen [18] gives the reduction of the spin–orbit coupling constant from the free ion value; 90 cm−1 for chromium(III) can be employed as a measure of metal ligand covalency (Figure 7(a)). It is possible to define a covalency parameter analogues to the Nephelauxetic parameter which is the ratio of the spin–orbit coupling constant for the complex and the free Cr(III) ions.Table 5
The spin-Hamiltonian parameters of Cr(III) and Cu(II) Schiff base complexes in DMSO at 300 and 77 K.
Complex Hyperfine constant × 10−4cm−1 A A ⊥ A i s o g g ⊥ g i s o [Cr(MFMAQ)Cl2] – – 84 – – 1.97 [Cu(MFMAQ)Cl(H2O)] 163 47 106 2.34 2.04 2.11Figure 7
EPR spectra of (a) Cr(III) complex and (b) Cu(II) complex as polycrystalline sample.
(a) (b)The solid state ESR spectrum of [Cu(MFMAQ)Cl] complex (Figure7(b)) is displayed at room temperature. The shape of the spectrum is consistent with octahedral environment around Cu(II) ion and the higher g value for the investigated [Cu(MFMAQ)Cl] complex (Table 5), when compared to that of free electron (g = 2.24) revealing an appreciable covalency of metal ligand bonding with dx2-y2 as the ground-state characteristic of octahedral stereochemistry [19]. Also, the g/A value 143 for the [Cu(MFMAQ)Cl] complex lies just within the range expected for octahedral complex [19]. The decrease of the g-value by 9 compared to that of the free-electron value (2.07) is an approximate measure of the ligand field strength; the stronger the furan Schiff’s base ligand field, the smaller the decrease in the g value and vice versa.


#### 3.2.6. XRD, EDX, SEM, and TEM Morphological Studies

In Figure8, XRD patterns of the [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)] complexes are depicted. The indexing procedures were performed using (CCP4, UK) CRYSFIRE program [20, 21] giving triclinic crystal system for [Cr(MFMAQ)Cl2] (Figure 8(a)) having M(9) = 7, F(6) = 8, [Co(MFMAQ)Cl(H2O)] orthorhombic crystal system (Figure 8(b)) having M(9) = 8, F(6) = 8, and tetragonal crystal system for [Cu(MFMAQ)Cl(H2O)] (Figure 8(c)) having M(6) = 14, F(6) = 6, as the superior solutions. Their cell parameters are interpreted in Table 6.Table 6
Crystallographic data for the Schiff base complexes [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)].
Data [Cr(MFMAQ)Cl2] [Co(MFMAQ)Cl(H2O)] [Cu(MFMAQ)Cl(H2O)] Empirical formula C 1 5 H 1 1Cl2N10O3Cr C 1 5 H 1 3Cl2N2O4Co C 1 5 H 1 3Cl2N2O4Cu Formula weight (g/mol) 390.2 379.7 384.3 Radiation Cu-Kα1 Cu-Kα1 Cu-Kα1 2θ range 5–60 5–60 5–60 Wavelength (Å) 1.501189 1.49997 1.52153 Crystal system Triclinic Orthorhombic Tetragonal Space group P4/m P4/m P4/m Unit cell dimensions (Å, °) a (Å) 7.986878 17.2354 7.315829 b (Å) 8.000534 17.2362 7. 315829 c (°) 17.23584 16.2358 7. 315829 α (°) 90 90 90 β (°) 90 90 90 γ (°) 90 90 90 Volume (Å3) 1010.47 5234.35 698.74 (Calc.) density (g/cm−3) 1.89785 1.34 1.89 Limiting indices 0 ≤h ≤ 3, 0 ≤ k ≤ 1, 1 ≤ l ≤ 7 3 ≤h ≤ 10, 1 ≤ k ≤ 6, 3 ≤ l ≤ 10 2 ≤h ≤ 8, 1 ≤ k ≤ 8, 0 ≤ l ≤ 2 Z 2 6 6 Rf 0.0000901 0.000027 0.0000783 Temperature (K) 298 298 298Figure 8
Powder XRD spectra of (a) Cr(III), (b) Co(II), and (c) Cu(II) complexes.
(a) (b) (c)The images SEM of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes were showed in Figures 9(a)–9(c), respectively. The micrograph of [Cr(MFMAQ)Cl2] complex shows peel shaped particles. The [Ni(MFMAQ)Cl(H2O)]·2H2O complex mentions ice rock structure. The [Cu(DPPMHQ)Cl(H2O)] complex grain-structure of ice was existent. The chemical composition of Schiff base complexes was determined using energy dispersive X-ray diffraction (EDX). In EDX profile of Cr(III), Ni(II), and Cu(II) complexes (Figures 9(a)–9(c)) the peaks of essential elements like C, N, O and respective Cr(III), Ni(II), and Cu(II) elements which constitute the molecules of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes are clearly identified supporting the proposed structures. All positions contain predictable elements, and different elements such as impurity were not detected.Figure 9
The SEM/EDX images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)Figures10(a)–10(c) show the TEM images of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes, respectively. The consistency and resemblance in between the particle forms of synthesized dimeric complexes suggest that structural phases have a similar template. The particles diameter is found in nano range as follows: Cr(II), 62–224 nm; Ni(II), 18–23 nm; Cu(II), 12–32 nm. Nanoparticle-size complexes may act strong in different application areas in a biological one.Figure 10
TEM images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)


#### 3.2.7. Thermal Decomposition

To evaluate the thermal behavior of metal complexes, the thermogravimetric (TG/DTG) curves for the complexes are represented in Figure11 and weight loss at different decomposition stages, temperatures ranges with DTG peaks, assignments, and the final pyrolysis product observed in the present studies are summarized in Table 7.Table 7
Thermal decomposition steps of the Cr(III), Ni(II), and Cu(II) complexes in TG plots.
Complex Temperaturerange (°C) Weight loss (%) DTG peaks(°C) Assignments Residue found%(calc.%) Obs. Cal. [Cr(MFMAQ)Cl2] 372–423 45.59 45.62 418 −C6H5NOCl2 1/2Cr2O3  19.71 (19.73) 473–798 34.88 34.90 544 −C9H6NO0.5  [Ni(MFMAQ)Cl(H2O)]·2H2O 92–194 12.87 12.99 122, 163 −2H2O (hydrated) + H2O (coordinated) NiO17.92 (17.97) 313–444 43.18 43.22 398 −C9H6NOCl 462–799 25.72 25.77 722 −C6H5NO  [Cu(MFMAQ)Cl(H2O)] 192–273 4.62 4.68 249 −H2O (coordinated) CuO20.63 (20.68) 293–484 46.95 46.99 326 −C9H7NOCl 506–798 27.58 27.61 565 −C6H4NOFigure 11
TG and DTG 3D-plots of Cr(III), Ni(II), and Cu(II) complexes up to 800°C.In TGA curve of the [Cr(MFMAQ)Cl2] complex does not show any weight loss up to 385°C; this indicates the absence of lattice and coordinated water molecules in it. The [Cr(MFMAQ)Cl2] complex shows two-step decomposition process in the range of 372–423°C and 473–798°C, respectively; the first step is relatively fast and a total of 26.84% weight loss has been observed which corresponds to the nonchelated part of the ligand moiety. The remaining chelated part of the ligand is decomposed in the second step which is 39.64% (calc. 38.46%). The final pyrolysis product, projected as chromium(III) oxide, and some unreacted residue had an observed mass of 33.52% (calc. 33.34%).The TG curve of the [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows the three-step decomposition process; in the first step 4.52% (calc. 4.23%) weight loss has been observed in the range of 92–124°C, which indicates the presence of one lattice water molecule in the complex. Another 4.86% (calc. 4.23%) weight loss corresponds to one coordinated water molecule which has been observed in the range of 124–173°C. In the second step of decomposition starting from 313°C to 442°C, nonchelated part of the ligand is eliminated which has been found to be 24.82% (calc. 26.04%). In the last step starting from 462°C to the final temperature, 46.84% (calc. 46.28%) weight loss corresponds to the remaining part of the ligand which has been noticed and the ultimate pyrolysis product is obtained as nickel(II) oxide of mass 18.96% (calc. 18.03%).Quite similar results have been recorded for [Cu(MFMAQ)Cl(H2O)] where decomposition takes place in three steps in the range of 192–273°C, 293–484°C, and 506–798°C, respectively, and copper (II) oxide; mass of 21.19% (calc. 19.78%) seems to be the final product. The only difference is that no lattice water molecule is presented in [Cu(MFMAQ)Cl(H2O)] complex. On the basis of TG analysis the increasing order of the stability of complexes is as follows: [Ni(MFMAQ)Cl(H2O)]·2H2O < [Cu(MFMAQ)Cl(H2O)] < [Cr(MFMAQ)Cl2]. Thus, the Co(II) complex shows excellent thermal stability in all the complexes when subjected to higher temperature; hence it is used in such types of applications.


#### 3.2.8. Structure of the Complexes

Based on the above studies, the following structure (Scheme6) may suggest these complexes.Scheme 6
The proposed structures of H-MFMAQ complexes.


#### 3.2.9. Cytotoxicity Studies

The anticancer activities of the H-MFMAQ Schiff base ligand and its metal(II/III) complexes against thehuman breast (MCF-7) andlung cancer (A549) cell lines were screened using MTT assay. The results were analyzed by cell viability curves and expressed as IC50 values. The maximal inhibition concentrations (IC50) given in Table 8 showed that the cytotoxicity efficiencies of the compounds under investigation follow the order: Cr(III) complex > Ru(III) complex > H-MFMAQ > Mn(II) complex > Co(II) complex > Ni(II) complex > Cu(II) complex > Zn(II) complex. From the results, it is evident that the Cr(III) and Ru(III) complexes exhibited higherin vitro cytotoxicity against both the selected cell lines when compared to the Schiff base ligand. Also, the cytotoxicity efficiency of the Cr(III) and Ru(III) complexes is comparable with that of the standard drug, cis-platin, while the Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes showed lower anticancer activities when compared to that of the ligand. The cytotoxicity of metal complexes is depending on their ability to bind DNA and damage its structure resulting in the impairment of its function, which is followed by replication and transcription processes inhibition and eventually cell death that is what we can suppose [22–26]. Thus, the relatively higher cytotoxicity exhibited by the Cr(III) and Ru(III) complexes may be due to the relatively stronger binding ability of the complexes with DNA as shown in the DNA binding studies.Table 8
Cytotoxicities (IC50, μM) of the Schiff base ligand and its complexesa.
Compound MCF-7 A-549 Ligand 25 ± 1.2 28 ± 1.4 Cr(III) complex 17 ± 1.6 2 0 ± 1.7 Ru(III) complex 18 ± 1.5 2 1 ± 1.7 Mn(II) complex 21 ± 1.6 2 4 ± 1.6 Co(II) complex 19 ± 1.7 2 2 ± 1.9 Ni(II) complex 21 ± 1.7 2 8 ± 1.4 Cu(II) complex 26 ± 1.5 3 7 ± 0.8 Zn(II) complex 29 ± 1.7 3 8 ± 1.2 Cisplatin 13 ± 0.5 1 2 ± 0.9 aIC50: concentration of the drug required to inhibit growth of 50% of the cancer cells (μM). The data are mean ± SD of three replicates each.


## 3.1. Ligand (H-MFMAQ)

H-MFMAQ percentage of purity was 99.97%; it has been measured by HPLC. Mass spectrum of the furan Schiff base ligand (H-MFMAQ) (Figure1(a)) has final peak at 268 amu corresponding to the furan Schiff base ligand moiety [C15H12N2O3] (atomic mass 268 amu) (Scheme 2). Other peaks like 52, 82, 148, 152, 208, and 227 amu were suggested according to diverse fragments. From this study, it was found that the intensity of the peaks gave information on the stability of fragmentation. The electronic spectrum of furan Schiff base ligand (H-MFMAQ) in ethanol exhibited five absorption bands (Figure 2(a)) at 233–338 nm regions which is due to π→π∗ and n→π∗ transitions utilizing molecular orbital of the quinoline and furan rings, C=N and C=O groups. Nevertheless, the IR spectrum of furan Schiff base ligand (H-MFMAQ) (Figure 3(a)) does not show any band at 1700 cm–1, 3380 cm–1, and 3250 cm–1 corresponding to the carbonyl groups and free primary amino groups; this confirms the complete condensation between keto and amino groups. The band at 1637 cm–1 is corresponding to ν (CH=N) stretching vibration. The IR spectrum of furan Schiff base ligand (H-MFMAQ) displays a broad band at 3483 cm–1, which can be assigned to ν(OH) group. The 1H-NMR spectra of the furan Schiff base ligand (H-MFMAQ) (Figure 4(a)) exhibit signals due to aromatic protons as multiplet at δ 6.80–7.23 (8H) and a broad signal at δ (11.35) ppm is assigned for O–H proton, which disappeared with addition of D2O due to the proton exchange. In 13C NMR of ligand (H-MFMAQ) (Figure 5(a)) (–C=O) carbonyl carbon showed signal at 166.47 ppm, (–C=N–) azomethine carbon at 162.12 ppm, (–C–O) phenolic group carbon at 158.27 ppm, and (C–O) furan ring at 170.12. The spectrum 15N-NMR of the ligand (H-MFMAQ) (Figure 6(a)) shows two signals centered 244.3 and 163.3 ppm, which were assigned to N12 (azomethine) and N1 (quinoline), respectively.Scheme 2
Mass fragmentation pattern of furan Schiff base ligand (H-MFMAQ).Figure 1
Mass spectrum of (a) ligand, (b) Co(II) complex, (c) Cu(II) complex, and (d) Ru(III) complex.
(a) (b) (c) (d)Figure 2
Electronic spectrum of (a) ligand and (b) Ru(III) complex.
(a) (b)Figure 3
(a) IR spectrum of ligand, (b) IR spectrum of Cr(III) complex, and (c) IR spectrum of Zn(II) complex.
(a)
H-MFMAQ (b)
[Cr(MFMAQ)Cl2] (c)
[Co(MFMAQ)Cl(H2O)]Figure 4
1H NMR spectra of (a) Schiff base ligand and (b) Zn(II) complex.Figure 5
13C NMR spectra of (a) Schiff base ligand and (b) Zn(II) complex.Figure 6
15N NMR spectra of (a) Schiff base ligand and (b) Zn (II) complex.


## 3.2. Complexes

The empirical formulae of complexes showing number of water molecules are presented in Table1. All synthesized solid complexes are stable in air. They are practically insoluble in water, but on the contrary quite soluble in polar organic solvents (e.g., EtOH, MeOH, DMF, and DMSO). The structures of the complexes could not be determined because single crystals were not obtained. The molar conductivity data (Table 2) clearly indicate that all complexes in MeOH and DMSO as well as Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes in MeOH, DMF, and DMSO are in the range 7.58–15.24 Ω–1cm2mol–1 indicating the nonelectrolytic nature of all complexes [12]. This finding is consistent with the infrared spectral data that showed the coordinated nature of chloride anions.Table 2
Molar conductivity of complexes Λ M/Ω−1 cm2 mol−1 for 0,001 mol·L−1 solutions in MeOH, DMF, and DMSO at 25°C.
Complex Λ M  [Ω−1 cm2 mol−1] MeOH DMF DMSO [Cr(MFMAQ)Cl2] 14.36 15.24 7.58 [Ru(MFMAQ)Cl2] 12.87 14.25 9.77 [Mn(MFMAQ)Cl(H2O)]·H2O 12.42 14.85 8.56 [Co(MFMAQ)Cl(H2O)] 11.57 13.93 8.45 [Ni(MFMAQ)Cl(H2O)]·2H2O 12.84 14.47 9.27 [Cu(MFMAQ)Cl(H2O)] 10.75 13.74 7.89 [Zn(MFMAQ)Cl(H2O)]·2.5H2O 11.59 14.66 8.98


### 3.2.1. Mass Spectra of Complexes

The ESI mass spectrum of the Co(II) complex [Co(MFMAQ)Cl(H2O)] (Figure 1(b)) shows the parental ion peak at m/z = 379 corresponding to (CoC15H13ClN2O4)+. The other fragments of the complex give the peak with various intensities at different m/z values like at 74 (CoO)+, 77 (C6H5)+, 144 (CoC4H7NO)+, and 326 (CoC15H11N2O3)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 3.Scheme 3
Mass fragmentation pattern of Co(II) complex [Co(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Cu(II) complex [Cu(MFMAQ)Cl(H2O)] (Figure 1(c)) shows the parental ion peak at m/z = 384 corresponding to (CoC15H13ClN2O4)+. The different fragments of the complex with different m/z values are present at 97 (C5H7NO)+, 120 (C7H8N2)+, 202 (CuC6H7N2O2)+, and 326 (CuC13H11ClN2O2). This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 4.Scheme 4
Mass fragmentation pattern of Cu(II) complex [Cu(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Ru(III) complex [Ru(MFMAQ)Cl2] (Figure 1(d)) shows the molecular ion peak at m/z = 439 corresponding to (RuC15H11Cl2N2O3)+. The other fragments of the complex show the peaks at different m/z values like at 56 (C4H8)+, 210 (RuC6H7NO)+, 158 (C10H10N2)+, 263 (RuC8H6N2O2)+, and 326 (RuC11H14N2OCl)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 5. These facts were matched to the suggested molecular formula for these complexes, that is, [Co(MFMAQ)Cl(H2O)], [Cu(MFMAQ)Cl(H2O)], and [Ru(MFMAQ)Cl2], where MFMAQ is the ligand. This confirms the Schiff base frame formation. Elemental analysis values were appropriate with those values calculated from the molecular formulae assigned to these complexes which are further supported by mass studies.Scheme 5
Mass fragmentation pattern of Ru(II) complex [Cu(MFMAQ)Cl2].


### 3.2.2. Electronic Absorption, Magnetic Measurements, and Ligand Field Parameter

The electronic absorption spectra of the free Schiff base ligand and its complexes (Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II)) were studied in Nujol mull.Two bands were showed at 18,995 (ε = 46 Lmol−1 cm−1) and 16,238 cm–1 (ε = 34 Lmol−1 cm−1); for Cr(III) complex [Cr(MFMAQ)Cl2] electronic spectrum, those may be consigned to 4A2g(F)→4T1g(F) and 4A2g(F)→4T2g(F) transitions, respectively, in an octahedral geometry [13], whereas the third band, which is due to 4A2g (F)→4T1g (P) transition, lies in the range of the ligand transitions that were predicted at 34,264 cm–1 (ε = 132 Lmol−1 cm−1). The ligand field parameters of the current Cr(III) complex have been calculated using Tanabe-Sugano diagrams B (583 cm–1), 10Dq (1742 cm–1), and β (0.53). The effective magnetic moment of the complex is 3.92 BM, which is consistent with the spin-only value for three unpaired electrons (3.87 BM) [14].Electronic spectrum of Mn(II) complex [Mn(MFMAQ)Cl(H2O)]·H2O exhibits four weak intensity absorption bands at 17,943 (ε = 30 Lmol-1cm−1), 22,806 (ε = 36 Lmol−1 cm−1), 27,216 (ε = 64 mol−1 cm−1), and 37,489 cm−1 (ε = 138 Lmol−1 cm−1). These bands may be assigned to the transitions: 6A1g→4T1g (4G), 6A1g→ 4Eg, 4A1g (4G) (10B + 5C), 6A1g→4Eg (4D) (17B + 5C), and 6A1g→ 4T1g (4P) (7B + 7C), respectively. The ligand parameters B and C were calculated from the second and third electronic transitions because these electronic transitions are free from the crystal field splitting and depend on B and C parameters [13, 14]. The calculated values of the ligand field parameters are given in Table 3. Room temperature magnetic moment of the Mn(II) complex lies at 5.94 BM; this value is in tune with a high-spin octahedral configuration.Table 3
Ligand field parameters of the complexes.
Complex Dq (cm−1) B (cm−1) β LFSE (kJmol−1) [Cr(MFMAQ)Cl2] 1674 792 0.88 208.68 [Ru(MFMAQ)Cl2] – – – – [Mn(MFMAQ)(H2O)Cl]·H2O 1168 808 0.73 100.47 [Co(MFMAQ)(H2O)Cl] 792 – 0.95 114.23 [Ni(MFMQ)(H2O)Cl]·2H2O – – – – [Cu(MFMAQ)Cl(H2O)]  492 0.81 – [Zn(MFMAQ)Cl(H2O)]2.5H2O – – – –The electronic spectrum of cobalt (II) complex [Co(MFMAQ)Cl(H2O)] recorded in Nujol mulls exhibits three absorption peaks at 13,897 (ε = 24 Lmol−1 cm−1), 15,368 (ε = 27 Lmol−1 cm−1), and 25,157 (ε = 53 Lmol−1 cm−1) cm–1, respectively. These bands can be assigned to 4T1g→4T2g (F)(ν1), 4T1g→4A2g (F)(ν2), and 4T1g→4T1g (P)(ν3) transitions, respectively, suggesting an octahedral geometry around Co(II) ion [13, 14]. Octahedral cobalt(II) complex, however, preserves a large orbital contribution to magnetic moment on account of 4T1g (F) ground term and exhibits μeff in the range 4.8–5.6 B.M [15]. The magnetic measurements reported here lie at 5.18 BM and demonstrate that the Co(II) complex was paramagnetic and has a high-spin octahedral configuration with 4T1g(F) ground state.The ligand field parameters (Table3) B (interelectronic repulsion of the d-electrons in complex), β (The Nephelauxetic effect), and 10Dq are calculated according to the equation reported for the octahedral Co(II) complex.(1)μeff=4.981-4λ=10Dq,λ=-178cm-1B=4ν3-15Dq2-10Dq260ν3-15Dq-180Dqν1=10Dqβ=BcomplexBfree  ion,where B (free ion) for Co(II) is 996 cm−1. The 10Dq, B, and β values are 7032 cm−1, 698 cm−1, and 0.68, respectively. These results show that the interelectronic repulsion of d-electrons in a complex is less than in the free ion. The value of B in a complex is 78% of the free ion value. The β value is related directly to covalence.The reduction ofB is caused by complex formation by the delocalization of the d-electron cloud on the ligand, which in turn causes the covalent bond formation. The data shows the Co(II) complex has covalent character in the metal ligand “σ” bond [15].Electronic spectrum of [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows bands at 15,053 (ε = 23 Lmol−1 cm−1), 17,892 (ε = 28 Lmol−1 cm−1), and 22,111 cm–1 (ε = 43 Lmol−1 cm−1). These bands may be specified to A32g(F)→3T2g(F)(ν1), 3A2g(F)→3T1g(F)(ν2), and 3A2g(F)→3T1g(P)(ν3) transitions, respectively. It proposes octahedral geometry of [Ni(MFMAQ)Cl(H2O)]·2H2O complex [13, 14]. The magnetic moment was evaluated which gave 3.08 μB, for [Ni(MFMAQ)Cl(H2O)]·2H2O complex which lies in the extent (2.9–3.3 μB) of the Ni(II) octahedral complexes [15]. The Nephelauxetic parameter β (Table 3) was readily obtained by utilizing the correlation β = B (complex)/B (free ion), where B (free ion) for Ni(II) is 1041 cm–1 [15]. The value of β lies at 0.27. These values indicated the covalent character in metal ligand “σ” bond [13].The Cu(II) complex [Cu(MFMAQ)Cl(H2O)] spectrum displayed a band at 22,137 cm−1 (ε = 41 Lmol−1 cm−1) assigned to 2Eg→2T2g transition assuming octahedral geometry around the central Cu(II) ion [15]. The emulated magnetic moment of the Cu(II) complex is 1.98 BM, which assures the octahedral structure of this complex [15].The electronic spectrum of ruthenium(III) complex [Ru(MFMAQ)Cl2] records three bands at 15,167 (ν1) (ε = 22 Lmol−1 cm−1), 17,353 (ν2) (ε = 27 Lmol−1 cm−1), and 25,158 cm−1 (ν3) (ε = 61 Lmol−1 cm−1) (Figure 2(b)). These bands may be assigned to 2T2g→ 4T1g, 2T2g→ 4T2g, and 2T2g→4A1g transitions in order of increasing energy. The position of bands is in tune with the prediction for octahedral complexes of the metal ions [13]. The ligand field parameters Δ,B, and β have been calculated by using the relation(2)ν1=Δ-4B+86B2Δν2=Δ+12B+2B2Δσ.The value of B in free ion is 638 cm−1. The value of β indicates that there is low covalency in the metal ligand σ-band [16]. The Ru(III) complex shows magnetic moments at room temperature 1.76 BM, which is lower than the predicted value of 2.17 BM. The lowering in μeff values may be due to lower symmetry ligand fields, metal-metal interaction, or extensive electron delocalization [14].The Zn(II) complex [Zn(MFMAQ)Cl(H2O)]·2.5H2O is diamagnetic as predictable and its geometry is most likely octahedral likewise Mn(II), Cu(II), Ni(II), and Co(II) complexes of H-MFMAQ ligand [15].


### 3.2.3. Infrared Spectra of Complexes

The study of infrared spectra of the furan Schiff base H-MFMAQ comparing to their metal complexes (1–7) (Table4; Figure 3) foremost revealed that the ligand is tetradentately coordinated to the metal ions. The bands were symbolized at 1712 and 1637 cm–1 due to the carbonyl and azomethine stretching vibration which was shifted to lower frequency by 14–19 and 12–16 cm–1, suggesting oxygen carbonyl and nitrogen azomethine involvements in complexity. At 1618 cm–1, the band was assigned to the furan ring ν(C–O–C) vibrations which is also shifted to lower frequency by 13–18 cm–1, which is suggestive to involvement of the furan ring in chelation. Also, at 3483 cm–1, the band was attributed to νOH in the ligand (H-MFMAQ) which disappeared in its metal complexes indicating deprotonation of the OH moiety during coordination [17]. The new bands at 543–552, 433–438, and 412–416 cm−1 were assigned to M–O (carbonyl), M–O (phenol), M–N (azomethine) and (M–Cl) in the metal complexes spectra were observed [15, 17]. The IR results showed that the metal was harmonized through one nitrogen atom (azomethine group) and three oxygen atoms (deprotonated hydroxyl group, carbonyl group, and furan ring) besides chlorine atoms.Table 4
IR spectral data (cm−1) of the H-MFMAQ ligand and its metal complexes.
Number ν O H ν ( O H ) w a t e r ν C = O ν C = N ν ( C - O – C ) f u r a n ν M – O ν M – N ν M – C l H-MFMAQ 3483br – 1712m 1637m 1618m – – – 1 – – 1693w 1621m 1600m 543m 433w 416m 2 – – 1698m 1622m 1600w 548s 434w 412w 3 – 3320br 1695s 1622m 1605w 552m 438m 414m 4 – 3300r 1693m 1625sh 1602m 547m 434m 41 m 5 – 3320br 1697m 1624m 1605m 552m 437m 413m 6 – 3300r 1696m 1625m 1604m 549m 435m 414m 7 – 3318br 1698m 1623m 1603m 547m 438m 415m sh: sharp, m: medium, br: broad, s: small, and w: weak.


### 3.2.4. NMR Spectra Investigation

The proton NMR spectroscopy of H-MFMAQ ligand (Figure4(a)) and its [Zn(MFMAQ)Cl(H2O)]2.5H2O complex (Figure 4(b)) was evident in DMSO-d6 solution employing tetramethylsilane (TMS) as internal standard. OH signal was found at 11.35 ppm in the spectrum of the ligand H-MFMAQ which completely disappeared in the spectrum of the [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. This suggests the sharing of the OH group in chelation with Zn(II) through isolation of the OH proton. The azomethine proton signal was shifted to high field in the spectrum of [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. It was looked at 8.13 ppm as compared to 8.67 ppm in the Schiff’s base H-MFMAQ. This refers to the complexity of the zinc atom through nitrogen atom azomethine. However, multiple bands assigned to the aromatic protons were found at 6.92–7.97 and 6.98–7.96 ppm in the free Schiff 22 base ligand and Zn(II) complex, respectively. The signal observed at 3.2 ppm with an integration corresponding to seven protons in the case of Zn(II) complex was assigned one coordinate water molecule and half past two hydrate water molecules.In13C NMR of ligand (Figure 5(a)) (–C=O) carbonyl carbon showed signal at 166.47 ppm, (–C=N–) azomethine carbon at 162.12 ppm, (–C–O) phenolic group carbon at 158.27 ppm, and (C–O) furan ring at 170.12. The signals due to (–C=N–) azomethine, (–C–O) phenolic, and (C–O) furan carbons were slightly shifted downfield in comparison to the corresponding signals of these groups in the ligand thereby confirming the complexation (Figure 5(b)) with zinc metal ion.The15N NMR spectra of the free ligand (Figure 6(a)) and the Zn(II) complex (Figure 6(b)) were also obtained. The spectrum of the ligand shows two signals centered at 244.3 and 163.3 ppm, which were assigned to N12 (azomethine) and N1 (quinoline), respectively. In the spectrum of Zn(II) complex only one broad signal is observed for the nitrogen atoms at 162.7 ppm. This behavior led us to assign the broad signal in the spectra of the complexes as both N12 and N1 atoms. With this assignment, N12 shifted 81.6 ppm downfield upon coordination to Zn(II). On the other hand, the nitrogen N1 shifts only 0.6 ppm upon coordination with Zn(II). This minor shift indicates that this atom is not involved in coordination as already evidenced by other techniques.


### 3.2.5. ESR Spectra

The ESR spectrum of the [Cr(MFMAQ)Cl2] complex (Table 5) has been recorded as polycrystalline sample at room temperature. No hyperfine interaction was observed in the ESR spectra of the [Cr(MFMAQ)Cl2] complex at room temperature. The g-values are calculated by using the expression, g = 2.0023(1-4λ/10Dq), whereλis the spin–orbit coupling constant for the metal ion in the complex. Owen [18] gives the reduction of the spin–orbit coupling constant from the free ion value; 90 cm−1 for chromium(III) can be employed as a measure of metal ligand covalency (Figure 7(a)). It is possible to define a covalency parameter analogues to the Nephelauxetic parameter which is the ratio of the spin–orbit coupling constant for the complex and the free Cr(III) ions.Table 5
The spin-Hamiltonian parameters of Cr(III) and Cu(II) Schiff base complexes in DMSO at 300 and 77 K.
Complex Hyperfine constant × 10−4cm−1 A A ⊥ A i s o g g ⊥ g i s o [Cr(MFMAQ)Cl2] – – 84 – – 1.97 [Cu(MFMAQ)Cl(H2O)] 163 47 106 2.34 2.04 2.11Figure 7
EPR spectra of (a) Cr(III) complex and (b) Cu(II) complex as polycrystalline sample.
(a) (b)The solid state ESR spectrum of [Cu(MFMAQ)Cl] complex (Figure7(b)) is displayed at room temperature. The shape of the spectrum is consistent with octahedral environment around Cu(II) ion and the higher g value for the investigated [Cu(MFMAQ)Cl] complex (Table 5), when compared to that of free electron (g = 2.24) revealing an appreciable covalency of metal ligand bonding with dx2-y2 as the ground-state characteristic of octahedral stereochemistry [19]. Also, the g/A value 143 for the [Cu(MFMAQ)Cl] complex lies just within the range expected for octahedral complex [19]. The decrease of the g-value by 9 compared to that of the free-electron value (2.07) is an approximate measure of the ligand field strength; the stronger the furan Schiff’s base ligand field, the smaller the decrease in the g value and vice versa.


### 3.2.6. XRD, EDX, SEM, and TEM Morphological Studies

In Figure8, XRD patterns of the [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)] complexes are depicted. The indexing procedures were performed using (CCP4, UK) CRYSFIRE program [20, 21] giving triclinic crystal system for [Cr(MFMAQ)Cl2] (Figure 8(a)) having M(9) = 7, F(6) = 8, [Co(MFMAQ)Cl(H2O)] orthorhombic crystal system (Figure 8(b)) having M(9) = 8, F(6) = 8, and tetragonal crystal system for [Cu(MFMAQ)Cl(H2O)] (Figure 8(c)) having M(6) = 14, F(6) = 6, as the superior solutions. Their cell parameters are interpreted in Table 6.Table 6
Crystallographic data for the Schiff base complexes [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)].
Data [Cr(MFMAQ)Cl2] [Co(MFMAQ)Cl(H2O)] [Cu(MFMAQ)Cl(H2O)] Empirical formula C 1 5 H 1 1Cl2N10O3Cr C 1 5 H 1 3Cl2N2O4Co C 1 5 H 1 3Cl2N2O4Cu Formula weight (g/mol) 390.2 379.7 384.3 Radiation Cu-Kα1 Cu-Kα1 Cu-Kα1 2θ range 5–60 5–60 5–60 Wavelength (Å) 1.501189 1.49997 1.52153 Crystal system Triclinic Orthorhombic Tetragonal Space group P4/m P4/m P4/m Unit cell dimensions (Å, °) a (Å) 7.986878 17.2354 7.315829 b (Å) 8.000534 17.2362 7. 315829 c (°) 17.23584 16.2358 7. 315829 α (°) 90 90 90 β (°) 90 90 90 γ (°) 90 90 90 Volume (Å3) 1010.47 5234.35 698.74 (Calc.) density (g/cm−3) 1.89785 1.34 1.89 Limiting indices 0 ≤h ≤ 3, 0 ≤ k ≤ 1, 1 ≤ l ≤ 7 3 ≤h ≤ 10, 1 ≤ k ≤ 6, 3 ≤ l ≤ 10 2 ≤h ≤ 8, 1 ≤ k ≤ 8, 0 ≤ l ≤ 2 Z 2 6 6 Rf 0.0000901 0.000027 0.0000783 Temperature (K) 298 298 298Figure 8
Powder XRD spectra of (a) Cr(III), (b) Co(II), and (c) Cu(II) complexes.
(a) (b) (c)The images SEM of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes were showed in Figures 9(a)–9(c), respectively. The micrograph of [Cr(MFMAQ)Cl2] complex shows peel shaped particles. The [Ni(MFMAQ)Cl(H2O)]·2H2O complex mentions ice rock structure. The [Cu(DPPMHQ)Cl(H2O)] complex grain-structure of ice was existent. The chemical composition of Schiff base complexes was determined using energy dispersive X-ray diffraction (EDX). In EDX profile of Cr(III), Ni(II), and Cu(II) complexes (Figures 9(a)–9(c)) the peaks of essential elements like C, N, O and respective Cr(III), Ni(II), and Cu(II) elements which constitute the molecules of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes are clearly identified supporting the proposed structures. All positions contain predictable elements, and different elements such as impurity were not detected.Figure 9
The SEM/EDX images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)Figures10(a)–10(c) show the TEM images of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes, respectively. The consistency and resemblance in between the particle forms of synthesized dimeric complexes suggest that structural phases have a similar template. The particles diameter is found in nano range as follows: Cr(II), 62–224 nm; Ni(II), 18–23 nm; Cu(II), 12–32 nm. Nanoparticle-size complexes may act strong in different application areas in a biological one.Figure 10
TEM images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)


### 3.2.7. Thermal Decomposition

To evaluate the thermal behavior of metal complexes, the thermogravimetric (TG/DTG) curves for the complexes are represented in Figure11 and weight loss at different decomposition stages, temperatures ranges with DTG peaks, assignments, and the final pyrolysis product observed in the present studies are summarized in Table 7.Table 7
Thermal decomposition steps of the Cr(III), Ni(II), and Cu(II) complexes in TG plots.
Complex Temperaturerange (°C) Weight loss (%) DTG peaks(°C) Assignments Residue found%(calc.%) Obs. Cal. [Cr(MFMAQ)Cl2] 372–423 45.59 45.62 418 −C6H5NOCl2 1/2Cr2O3  19.71 (19.73) 473–798 34.88 34.90 544 −C9H6NO0.5  [Ni(MFMAQ)Cl(H2O)]·2H2O 92–194 12.87 12.99 122, 163 −2H2O (hydrated) + H2O (coordinated) NiO17.92 (17.97) 313–444 43.18 43.22 398 −C9H6NOCl 462–799 25.72 25.77 722 −C6H5NO  [Cu(MFMAQ)Cl(H2O)] 192–273 4.62 4.68 249 −H2O (coordinated) CuO20.63 (20.68) 293–484 46.95 46.99 326 −C9H7NOCl 506–798 27.58 27.61 565 −C6H4NOFigure 11
TG and DTG 3D-plots of Cr(III), Ni(II), and Cu(II) complexes up to 800°C.In TGA curve of the [Cr(MFMAQ)Cl2] complex does not show any weight loss up to 385°C; this indicates the absence of lattice and coordinated water molecules in it. The [Cr(MFMAQ)Cl2] complex shows two-step decomposition process in the range of 372–423°C and 473–798°C, respectively; the first step is relatively fast and a total of 26.84% weight loss has been observed which corresponds to the nonchelated part of the ligand moiety. The remaining chelated part of the ligand is decomposed in the second step which is 39.64% (calc. 38.46%). The final pyrolysis product, projected as chromium(III) oxide, and some unreacted residue had an observed mass of 33.52% (calc. 33.34%).The TG curve of the [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows the three-step decomposition process; in the first step 4.52% (calc. 4.23%) weight loss has been observed in the range of 92–124°C, which indicates the presence of one lattice water molecule in the complex. Another 4.86% (calc. 4.23%) weight loss corresponds to one coordinated water molecule which has been observed in the range of 124–173°C. In the second step of decomposition starting from 313°C to 442°C, nonchelated part of the ligand is eliminated which has been found to be 24.82% (calc. 26.04%). In the last step starting from 462°C to the final temperature, 46.84% (calc. 46.28%) weight loss corresponds to the remaining part of the ligand which has been noticed and the ultimate pyrolysis product is obtained as nickel(II) oxide of mass 18.96% (calc. 18.03%).Quite similar results have been recorded for [Cu(MFMAQ)Cl(H2O)] where decomposition takes place in three steps in the range of 192–273°C, 293–484°C, and 506–798°C, respectively, and copper (II) oxide; mass of 21.19% (calc. 19.78%) seems to be the final product. The only difference is that no lattice water molecule is presented in [Cu(MFMAQ)Cl(H2O)] complex. On the basis of TG analysis the increasing order of the stability of complexes is as follows: [Ni(MFMAQ)Cl(H2O)]·2H2O < [Cu(MFMAQ)Cl(H2O)] < [Cr(MFMAQ)Cl2]. Thus, the Co(II) complex shows excellent thermal stability in all the complexes when subjected to higher temperature; hence it is used in such types of applications.


### 3.2.8. Structure of the Complexes

Based on the above studies, the following structure (Scheme6) may suggest these complexes.Scheme 6
The proposed structures of H-MFMAQ complexes.


### 3.2.9. Cytotoxicity Studies

The anticancer activities of the H-MFMAQ Schiff base ligand and its metal(II/III) complexes against thehuman breast (MCF-7) andlung cancer (A549) cell lines were screened using MTT assay. The results were analyzed by cell viability curves and expressed as IC50 values. The maximal inhibition concentrations (IC50) given in Table 8 showed that the cytotoxicity efficiencies of the compounds under investigation follow the order: Cr(III) complex > Ru(III) complex > H-MFMAQ > Mn(II) complex > Co(II) complex > Ni(II) complex > Cu(II) complex > Zn(II) complex. From the results, it is evident that the Cr(III) and Ru(III) complexes exhibited higherin vitro cytotoxicity against both the selected cell lines when compared to the Schiff base ligand. Also, the cytotoxicity efficiency of the Cr(III) and Ru(III) complexes is comparable with that of the standard drug, cis-platin, while the Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes showed lower anticancer activities when compared to that of the ligand. The cytotoxicity of metal complexes is depending on their ability to bind DNA and damage its structure resulting in the impairment of its function, which is followed by replication and transcription processes inhibition and eventually cell death that is what we can suppose [22–26]. Thus, the relatively higher cytotoxicity exhibited by the Cr(III) and Ru(III) complexes may be due to the relatively stronger binding ability of the complexes with DNA as shown in the DNA binding studies.Table 8
Cytotoxicities (IC50, μM) of the Schiff base ligand and its complexesa.
Compound MCF-7 A-549 Ligand 25 ± 1.2 28 ± 1.4 Cr(III) complex 17 ± 1.6 2 0 ± 1.7 Ru(III) complex 18 ± 1.5 2 1 ± 1.7 Mn(II) complex 21 ± 1.6 2 4 ± 1.6 Co(II) complex 19 ± 1.7 2 2 ± 1.9 Ni(II) complex 21 ± 1.7 2 8 ± 1.4 Cu(II) complex 26 ± 1.5 3 7 ± 0.8 Zn(II) complex 29 ± 1.7 3 8 ± 1.2 Cisplatin 13 ± 0.5 1 2 ± 0.9 aIC50: concentration of the drug required to inhibit growth of 50% of the cancer cells (μM). The data are mean ± SD of three replicates each.


## 3.2.1. Mass Spectra of Complexes

The ESI mass spectrum of the Co(II) complex [Co(MFMAQ)Cl(H2O)] (Figure 1(b)) shows the parental ion peak at m/z = 379 corresponding to (CoC15H13ClN2O4)+. The other fragments of the complex give the peak with various intensities at different m/z values like at 74 (CoO)+, 77 (C6H5)+, 144 (CoC4H7NO)+, and 326 (CoC15H11N2O3)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 3.Scheme 3
Mass fragmentation pattern of Co(II) complex [Co(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Cu(II) complex [Cu(MFMAQ)Cl(H2O)] (Figure 1(c)) shows the parental ion peak at m/z = 384 corresponding to (CoC15H13ClN2O4)+. The different fragments of the complex with different m/z values are present at 97 (C5H7NO)+, 120 (C7H8N2)+, 202 (CuC6H7N2O2)+, and 326 (CuC13H11ClN2O2). This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 4.Scheme 4
Mass fragmentation pattern of Cu(II) complex [Cu(MFMAQ)(H2O)Cl].The ESI mass spectrum of the Ru(III) complex [Ru(MFMAQ)Cl2] (Figure 1(d)) shows the molecular ion peak at m/z = 439 corresponding to (RuC15H11Cl2N2O3)+. The other fragments of the complex show the peaks at different m/z values like at 56 (C4H8)+, 210 (RuC6H7NO)+, 158 (C10H10N2)+, 263 (RuC8H6N2O2)+, and 326 (RuC11H14N2OCl)+. This schematic mass spectral fragmentation pattern of ligand is consistent with its structure which is depicted in Scheme 5. These facts were matched to the suggested molecular formula for these complexes, that is, [Co(MFMAQ)Cl(H2O)], [Cu(MFMAQ)Cl(H2O)], and [Ru(MFMAQ)Cl2], where MFMAQ is the ligand. This confirms the Schiff base frame formation. Elemental analysis values were appropriate with those values calculated from the molecular formulae assigned to these complexes which are further supported by mass studies.Scheme 5
Mass fragmentation pattern of Ru(II) complex [Cu(MFMAQ)Cl2].


## 3.2.2. Electronic Absorption, Magnetic Measurements, and Ligand Field Parameter

The electronic absorption spectra of the free Schiff base ligand and its complexes (Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II)) were studied in Nujol mull.Two bands were showed at 18,995 (ε = 46 Lmol−1 cm−1) and 16,238 cm–1 (ε = 34 Lmol−1 cm−1); for Cr(III) complex [Cr(MFMAQ)Cl2] electronic spectrum, those may be consigned to 4A2g(F)→4T1g(F) and 4A2g(F)→4T2g(F) transitions, respectively, in an octahedral geometry [13], whereas the third band, which is due to 4A2g (F)→4T1g (P) transition, lies in the range of the ligand transitions that were predicted at 34,264 cm–1 (ε = 132 Lmol−1 cm−1). The ligand field parameters of the current Cr(III) complex have been calculated using Tanabe-Sugano diagrams B (583 cm–1), 10Dq (1742 cm–1), and β (0.53). The effective magnetic moment of the complex is 3.92 BM, which is consistent with the spin-only value for three unpaired electrons (3.87 BM) [14].Electronic spectrum of Mn(II) complex [Mn(MFMAQ)Cl(H2O)]·H2O exhibits four weak intensity absorption bands at 17,943 (ε = 30 Lmol-1cm−1), 22,806 (ε = 36 Lmol−1 cm−1), 27,216 (ε = 64 mol−1 cm−1), and 37,489 cm−1 (ε = 138 Lmol−1 cm−1). These bands may be assigned to the transitions: 6A1g→4T1g (4G), 6A1g→ 4Eg, 4A1g (4G) (10B + 5C), 6A1g→4Eg (4D) (17B + 5C), and 6A1g→ 4T1g (4P) (7B + 7C), respectively. The ligand parameters B and C were calculated from the second and third electronic transitions because these electronic transitions are free from the crystal field splitting and depend on B and C parameters [13, 14]. The calculated values of the ligand field parameters are given in Table 3. Room temperature magnetic moment of the Mn(II) complex lies at 5.94 BM; this value is in tune with a high-spin octahedral configuration.Table 3
Ligand field parameters of the complexes.
Complex Dq (cm−1) B (cm−1) β LFSE (kJmol−1) [Cr(MFMAQ)Cl2] 1674 792 0.88 208.68 [Ru(MFMAQ)Cl2] – – – – [Mn(MFMAQ)(H2O)Cl]·H2O 1168 808 0.73 100.47 [Co(MFMAQ)(H2O)Cl] 792 – 0.95 114.23 [Ni(MFMQ)(H2O)Cl]·2H2O – – – – [Cu(MFMAQ)Cl(H2O)]  492 0.81 – [Zn(MFMAQ)Cl(H2O)]2.5H2O – – – –The electronic spectrum of cobalt (II) complex [Co(MFMAQ)Cl(H2O)] recorded in Nujol mulls exhibits three absorption peaks at 13,897 (ε = 24 Lmol−1 cm−1), 15,368 (ε = 27 Lmol−1 cm−1), and 25,157 (ε = 53 Lmol−1 cm−1) cm–1, respectively. These bands can be assigned to 4T1g→4T2g (F)(ν1), 4T1g→4A2g (F)(ν2), and 4T1g→4T1g (P)(ν3) transitions, respectively, suggesting an octahedral geometry around Co(II) ion [13, 14]. Octahedral cobalt(II) complex, however, preserves a large orbital contribution to magnetic moment on account of 4T1g (F) ground term and exhibits μeff in the range 4.8–5.6 B.M [15]. The magnetic measurements reported here lie at 5.18 BM and demonstrate that the Co(II) complex was paramagnetic and has a high-spin octahedral configuration with 4T1g(F) ground state.The ligand field parameters (Table3) B (interelectronic repulsion of the d-electrons in complex), β (The Nephelauxetic effect), and 10Dq are calculated according to the equation reported for the octahedral Co(II) complex.(1)μeff=4.981-4λ=10Dq,λ=-178cm-1B=4ν3-15Dq2-10Dq260ν3-15Dq-180Dqν1=10Dqβ=BcomplexBfree  ion,where B (free ion) for Co(II) is 996 cm−1. The 10Dq, B, and β values are 7032 cm−1, 698 cm−1, and 0.68, respectively. These results show that the interelectronic repulsion of d-electrons in a complex is less than in the free ion. The value of B in a complex is 78% of the free ion value. The β value is related directly to covalence.The reduction ofB is caused by complex formation by the delocalization of the d-electron cloud on the ligand, which in turn causes the covalent bond formation. The data shows the Co(II) complex has covalent character in the metal ligand “σ” bond [15].Electronic spectrum of [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows bands at 15,053 (ε = 23 Lmol−1 cm−1), 17,892 (ε = 28 Lmol−1 cm−1), and 22,111 cm–1 (ε = 43 Lmol−1 cm−1). These bands may be specified to A32g(F)→3T2g(F)(ν1), 3A2g(F)→3T1g(F)(ν2), and 3A2g(F)→3T1g(P)(ν3) transitions, respectively. It proposes octahedral geometry of [Ni(MFMAQ)Cl(H2O)]·2H2O complex [13, 14]. The magnetic moment was evaluated which gave 3.08 μB, for [Ni(MFMAQ)Cl(H2O)]·2H2O complex which lies in the extent (2.9–3.3 μB) of the Ni(II) octahedral complexes [15]. The Nephelauxetic parameter β (Table 3) was readily obtained by utilizing the correlation β = B (complex)/B (free ion), where B (free ion) for Ni(II) is 1041 cm–1 [15]. The value of β lies at 0.27. These values indicated the covalent character in metal ligand “σ” bond [13].The Cu(II) complex [Cu(MFMAQ)Cl(H2O)] spectrum displayed a band at 22,137 cm−1 (ε = 41 Lmol−1 cm−1) assigned to 2Eg→2T2g transition assuming octahedral geometry around the central Cu(II) ion [15]. The emulated magnetic moment of the Cu(II) complex is 1.98 BM, which assures the octahedral structure of this complex [15].The electronic spectrum of ruthenium(III) complex [Ru(MFMAQ)Cl2] records three bands at 15,167 (ν1) (ε = 22 Lmol−1 cm−1), 17,353 (ν2) (ε = 27 Lmol−1 cm−1), and 25,158 cm−1 (ν3) (ε = 61 Lmol−1 cm−1) (Figure 2(b)). These bands may be assigned to 2T2g→ 4T1g, 2T2g→ 4T2g, and 2T2g→4A1g transitions in order of increasing energy. The position of bands is in tune with the prediction for octahedral complexes of the metal ions [13]. The ligand field parameters Δ,B, and β have been calculated by using the relation(2)ν1=Δ-4B+86B2Δν2=Δ+12B+2B2Δσ.The value of B in free ion is 638 cm−1. The value of β indicates that there is low covalency in the metal ligand σ-band [16]. The Ru(III) complex shows magnetic moments at room temperature 1.76 BM, which is lower than the predicted value of 2.17 BM. The lowering in μeff values may be due to lower symmetry ligand fields, metal-metal interaction, or extensive electron delocalization [14].The Zn(II) complex [Zn(MFMAQ)Cl(H2O)]·2.5H2O is diamagnetic as predictable and its geometry is most likely octahedral likewise Mn(II), Cu(II), Ni(II), and Co(II) complexes of H-MFMAQ ligand [15].


## 3.2.3. Infrared Spectra of Complexes

The study of infrared spectra of the furan Schiff base H-MFMAQ comparing to their metal complexes (1–7) (Table4; Figure 3) foremost revealed that the ligand is tetradentately coordinated to the metal ions. The bands were symbolized at 1712 and 1637 cm–1 due to the carbonyl and azomethine stretching vibration which was shifted to lower frequency by 14–19 and 12–16 cm–1, suggesting oxygen carbonyl and nitrogen azomethine involvements in complexity. At 1618 cm–1, the band was assigned to the furan ring ν(C–O–C) vibrations which is also shifted to lower frequency by 13–18 cm–1, which is suggestive to involvement of the furan ring in chelation. Also, at 3483 cm–1, the band was attributed to νOH in the ligand (H-MFMAQ) which disappeared in its metal complexes indicating deprotonation of the OH moiety during coordination [17]. The new bands at 543–552, 433–438, and 412–416 cm−1 were assigned to M–O (carbonyl), M–O (phenol), M–N (azomethine) and (M–Cl) in the metal complexes spectra were observed [15, 17]. The IR results showed that the metal was harmonized through one nitrogen atom (azomethine group) and three oxygen atoms (deprotonated hydroxyl group, carbonyl group, and furan ring) besides chlorine atoms.Table 4
IR spectral data (cm−1) of the H-MFMAQ ligand and its metal complexes.
Number ν O H ν ( O H ) w a t e r ν C = O ν C = N ν ( C - O – C ) f u r a n ν M – O ν M – N ν M – C l H-MFMAQ 3483br – 1712m 1637m 1618m – – – 1 – – 1693w 1621m 1600m 543m 433w 416m 2 – – 1698m 1622m 1600w 548s 434w 412w 3 – 3320br 1695s 1622m 1605w 552m 438m 414m 4 – 3300r 1693m 1625sh 1602m 547m 434m 41 m 5 – 3320br 1697m 1624m 1605m 552m 437m 413m 6 – 3300r 1696m 1625m 1604m 549m 435m 414m 7 – 3318br 1698m 1623m 1603m 547m 438m 415m sh: sharp, m: medium, br: broad, s: small, and w: weak.


## 3.2.4. NMR Spectra Investigation

The proton NMR spectroscopy of H-MFMAQ ligand (Figure4(a)) and its [Zn(MFMAQ)Cl(H2O)]2.5H2O complex (Figure 4(b)) was evident in DMSO-d6 solution employing tetramethylsilane (TMS) as internal standard. OH signal was found at 11.35 ppm in the spectrum of the ligand H-MFMAQ which completely disappeared in the spectrum of the [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. This suggests the sharing of the OH group in chelation with Zn(II) through isolation of the OH proton. The azomethine proton signal was shifted to high field in the spectrum of [Zn(MFMAQ)Cl(H2O)]2.5H2O complex. It was looked at 8.13 ppm as compared to 8.67 ppm in the Schiff’s base H-MFMAQ. This refers to the complexity of the zinc atom through nitrogen atom azomethine. However, multiple bands assigned to the aromatic protons were found at 6.92–7.97 and 6.98–7.96 ppm in the free Schiff 22 base ligand and Zn(II) complex, respectively. The signal observed at 3.2 ppm with an integration corresponding to seven protons in the case of Zn(II) complex was assigned one coordinate water molecule and half past two hydrate water molecules.In13C NMR of ligand (Figure 5(a)) (–C=O) carbonyl carbon showed signal at 166.47 ppm, (–C=N–) azomethine carbon at 162.12 ppm, (–C–O) phenolic group carbon at 158.27 ppm, and (C–O) furan ring at 170.12. The signals due to (–C=N–) azomethine, (–C–O) phenolic, and (C–O) furan carbons were slightly shifted downfield in comparison to the corresponding signals of these groups in the ligand thereby confirming the complexation (Figure 5(b)) with zinc metal ion.The15N NMR spectra of the free ligand (Figure 6(a)) and the Zn(II) complex (Figure 6(b)) were also obtained. The spectrum of the ligand shows two signals centered at 244.3 and 163.3 ppm, which were assigned to N12 (azomethine) and N1 (quinoline), respectively. In the spectrum of Zn(II) complex only one broad signal is observed for the nitrogen atoms at 162.7 ppm. This behavior led us to assign the broad signal in the spectra of the complexes as both N12 and N1 atoms. With this assignment, N12 shifted 81.6 ppm downfield upon coordination to Zn(II). On the other hand, the nitrogen N1 shifts only 0.6 ppm upon coordination with Zn(II). This minor shift indicates that this atom is not involved in coordination as already evidenced by other techniques.


## 3.2.5. ESR Spectra

The ESR spectrum of the [Cr(MFMAQ)Cl2] complex (Table 5) has been recorded as polycrystalline sample at room temperature. No hyperfine interaction was observed in the ESR spectra of the [Cr(MFMAQ)Cl2] complex at room temperature. The g-values are calculated by using the expression, g = 2.0023(1-4λ/10Dq), whereλis the spin–orbit coupling constant for the metal ion in the complex. Owen [18] gives the reduction of the spin–orbit coupling constant from the free ion value; 90 cm−1 for chromium(III) can be employed as a measure of metal ligand covalency (Figure 7(a)). It is possible to define a covalency parameter analogues to the Nephelauxetic parameter which is the ratio of the spin–orbit coupling constant for the complex and the free Cr(III) ions.Table 5
The spin-Hamiltonian parameters of Cr(III) and Cu(II) Schiff base complexes in DMSO at 300 and 77 K.
Complex Hyperfine constant × 10−4cm−1 A A ⊥ A i s o g g ⊥ g i s o [Cr(MFMAQ)Cl2] – – 84 – – 1.97 [Cu(MFMAQ)Cl(H2O)] 163 47 106 2.34 2.04 2.11Figure 7
EPR spectra of (a) Cr(III) complex and (b) Cu(II) complex as polycrystalline sample.
(a) (b)The solid state ESR spectrum of [Cu(MFMAQ)Cl] complex (Figure7(b)) is displayed at room temperature. The shape of the spectrum is consistent with octahedral environment around Cu(II) ion and the higher g value for the investigated [Cu(MFMAQ)Cl] complex (Table 5), when compared to that of free electron (g = 2.24) revealing an appreciable covalency of metal ligand bonding with dx2-y2 as the ground-state characteristic of octahedral stereochemistry [19]. Also, the g/A value 143 for the [Cu(MFMAQ)Cl] complex lies just within the range expected for octahedral complex [19]. The decrease of the g-value by 9 compared to that of the free-electron value (2.07) is an approximate measure of the ligand field strength; the stronger the furan Schiff’s base ligand field, the smaller the decrease in the g value and vice versa.


## 3.2.6. XRD, EDX, SEM, and TEM Morphological Studies

In Figure8, XRD patterns of the [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)] complexes are depicted. The indexing procedures were performed using (CCP4, UK) CRYSFIRE program [20, 21] giving triclinic crystal system for [Cr(MFMAQ)Cl2] (Figure 8(a)) having M(9) = 7, F(6) = 8, [Co(MFMAQ)Cl(H2O)] orthorhombic crystal system (Figure 8(b)) having M(9) = 8, F(6) = 8, and tetragonal crystal system for [Cu(MFMAQ)Cl(H2O)] (Figure 8(c)) having M(6) = 14, F(6) = 6, as the superior solutions. Their cell parameters are interpreted in Table 6.Table 6
Crystallographic data for the Schiff base complexes [Cr(MFMAQ)Cl2], [Co(MFMAQ)Cl(H2O)], and [Cu(MFMAQ)Cl(H2O)].
Data [Cr(MFMAQ)Cl2] [Co(MFMAQ)Cl(H2O)] [Cu(MFMAQ)Cl(H2O)] Empirical formula C 1 5 H 1 1Cl2N10O3Cr C 1 5 H 1 3Cl2N2O4Co C 1 5 H 1 3Cl2N2O4Cu Formula weight (g/mol) 390.2 379.7 384.3 Radiation Cu-Kα1 Cu-Kα1 Cu-Kα1 2θ range 5–60 5–60 5–60 Wavelength (Å) 1.501189 1.49997 1.52153 Crystal system Triclinic Orthorhombic Tetragonal Space group P4/m P4/m P4/m Unit cell dimensions (Å, °) a (Å) 7.986878 17.2354 7.315829 b (Å) 8.000534 17.2362 7. 315829 c (°) 17.23584 16.2358 7. 315829 α (°) 90 90 90 β (°) 90 90 90 γ (°) 90 90 90 Volume (Å3) 1010.47 5234.35 698.74 (Calc.) density (g/cm−3) 1.89785 1.34 1.89 Limiting indices 0 ≤h ≤ 3, 0 ≤ k ≤ 1, 1 ≤ l ≤ 7 3 ≤h ≤ 10, 1 ≤ k ≤ 6, 3 ≤ l ≤ 10 2 ≤h ≤ 8, 1 ≤ k ≤ 8, 0 ≤ l ≤ 2 Z 2 6 6 Rf 0.0000901 0.000027 0.0000783 Temperature (K) 298 298 298Figure 8
Powder XRD spectra of (a) Cr(III), (b) Co(II), and (c) Cu(II) complexes.
(a) (b) (c)The images SEM of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes were showed in Figures 9(a)–9(c), respectively. The micrograph of [Cr(MFMAQ)Cl2] complex shows peel shaped particles. The [Ni(MFMAQ)Cl(H2O)]·2H2O complex mentions ice rock structure. The [Cu(DPPMHQ)Cl(H2O)] complex grain-structure of ice was existent. The chemical composition of Schiff base complexes was determined using energy dispersive X-ray diffraction (EDX). In EDX profile of Cr(III), Ni(II), and Cu(II) complexes (Figures 9(a)–9(c)) the peaks of essential elements like C, N, O and respective Cr(III), Ni(II), and Cu(II) elements which constitute the molecules of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes are clearly identified supporting the proposed structures. All positions contain predictable elements, and different elements such as impurity were not detected.Figure 9
The SEM/EDX images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)Figures10(a)–10(c) show the TEM images of [Cr(MFMAQ)Cl2], [Ni(MFMAQ)Cl(H2O)]·2H2O, and [Cu(MFMAQ)Cl(H2O)] complexes, respectively. The consistency and resemblance in between the particle forms of synthesized dimeric complexes suggest that structural phases have a similar template. The particles diameter is found in nano range as follows: Cr(II), 62–224 nm; Ni(II), 18–23 nm; Cu(II), 12–32 nm. Nanoparticle-size complexes may act strong in different application areas in a biological one.Figure 10
TEM images of (a): Cr(III), (b): Ni(II), and (c): Cu(II) complexes.
(a) (b) (c)


## 3.2.7. Thermal Decomposition

To evaluate the thermal behavior of metal complexes, the thermogravimetric (TG/DTG) curves for the complexes are represented in Figure11 and weight loss at different decomposition stages, temperatures ranges with DTG peaks, assignments, and the final pyrolysis product observed in the present studies are summarized in Table 7.Table 7
Thermal decomposition steps of the Cr(III), Ni(II), and Cu(II) complexes in TG plots.
Complex Temperaturerange (°C) Weight loss (%) DTG peaks(°C) Assignments Residue found%(calc.%) Obs. Cal. [Cr(MFMAQ)Cl2] 372–423 45.59 45.62 418 −C6H5NOCl2 1/2Cr2O3  19.71 (19.73) 473–798 34.88 34.90 544 −C9H6NO0.5  [Ni(MFMAQ)Cl(H2O)]·2H2O 92–194 12.87 12.99 122, 163 −2H2O (hydrated) + H2O (coordinated) NiO17.92 (17.97) 313–444 43.18 43.22 398 −C9H6NOCl 462–799 25.72 25.77 722 −C6H5NO  [Cu(MFMAQ)Cl(H2O)] 192–273 4.62 4.68 249 −H2O (coordinated) CuO20.63 (20.68) 293–484 46.95 46.99 326 −C9H7NOCl 506–798 27.58 27.61 565 −C6H4NOFigure 11
TG and DTG 3D-plots of Cr(III), Ni(II), and Cu(II) complexes up to 800°C.In TGA curve of the [Cr(MFMAQ)Cl2] complex does not show any weight loss up to 385°C; this indicates the absence of lattice and coordinated water molecules in it. The [Cr(MFMAQ)Cl2] complex shows two-step decomposition process in the range of 372–423°C and 473–798°C, respectively; the first step is relatively fast and a total of 26.84% weight loss has been observed which corresponds to the nonchelated part of the ligand moiety. The remaining chelated part of the ligand is decomposed in the second step which is 39.64% (calc. 38.46%). The final pyrolysis product, projected as chromium(III) oxide, and some unreacted residue had an observed mass of 33.52% (calc. 33.34%).The TG curve of the [Ni(MFMAQ)Cl(H2O)]·2H2O complex shows the three-step decomposition process; in the first step 4.52% (calc. 4.23%) weight loss has been observed in the range of 92–124°C, which indicates the presence of one lattice water molecule in the complex. Another 4.86% (calc. 4.23%) weight loss corresponds to one coordinated water molecule which has been observed in the range of 124–173°C. In the second step of decomposition starting from 313°C to 442°C, nonchelated part of the ligand is eliminated which has been found to be 24.82% (calc. 26.04%). In the last step starting from 462°C to the final temperature, 46.84% (calc. 46.28%) weight loss corresponds to the remaining part of the ligand which has been noticed and the ultimate pyrolysis product is obtained as nickel(II) oxide of mass 18.96% (calc. 18.03%).Quite similar results have been recorded for [Cu(MFMAQ)Cl(H2O)] where decomposition takes place in three steps in the range of 192–273°C, 293–484°C, and 506–798°C, respectively, and copper (II) oxide; mass of 21.19% (calc. 19.78%) seems to be the final product. The only difference is that no lattice water molecule is presented in [Cu(MFMAQ)Cl(H2O)] complex. On the basis of TG analysis the increasing order of the stability of complexes is as follows: [Ni(MFMAQ)Cl(H2O)]·2H2O < [Cu(MFMAQ)Cl(H2O)] < [Cr(MFMAQ)Cl2]. Thus, the Co(II) complex shows excellent thermal stability in all the complexes when subjected to higher temperature; hence it is used in such types of applications.


## 3.2.8. Structure of the Complexes

Based on the above studies, the following structure (Scheme6) may suggest these complexes.Scheme 6
The proposed structures of H-MFMAQ complexes.


## 3.2.9. Cytotoxicity Studies

The anticancer activities of the H-MFMAQ Schiff base ligand and its metal(II/III) complexes against thehuman breast (MCF-7) andlung cancer (A549) cell lines were screened using MTT assay. The results were analyzed by cell viability curves and expressed as IC50 values. The maximal inhibition concentrations (IC50) given in Table 8 showed that the cytotoxicity efficiencies of the compounds under investigation follow the order: Cr(III) complex > Ru(III) complex > H-MFMAQ > Mn(II) complex > Co(II) complex > Ni(II) complex > Cu(II) complex > Zn(II) complex. From the results, it is evident that the Cr(III) and Ru(III) complexes exhibited higherin vitro cytotoxicity against both the selected cell lines when compared to the Schiff base ligand. Also, the cytotoxicity efficiency of the Cr(III) and Ru(III) complexes is comparable with that of the standard drug, cis-platin, while the Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes showed lower anticancer activities when compared to that of the ligand. The cytotoxicity of metal complexes is depending on their ability to bind DNA and damage its structure resulting in the impairment of its function, which is followed by replication and transcription processes inhibition and eventually cell death that is what we can suppose [22–26]. Thus, the relatively higher cytotoxicity exhibited by the Cr(III) and Ru(III) complexes may be due to the relatively stronger binding ability of the complexes with DNA as shown in the DNA binding studies.Table 8
Cytotoxicities (IC50, μM) of the Schiff base ligand and its complexesa.
Compound MCF-7 A-549 Ligand 25 ± 1.2 28 ± 1.4 Cr(III) complex 17 ± 1.6 2 0 ± 1.7 Ru(III) complex 18 ± 1.5 2 1 ± 1.7 Mn(II) complex 21 ± 1.6 2 4 ± 1.6 Co(II) complex 19 ± 1.7 2 2 ± 1.9 Ni(II) complex 21 ± 1.7 2 8 ± 1.4 Cu(II) complex 26 ± 1.5 3 7 ± 0.8 Zn(II) complex 29 ± 1.7 3 8 ± 1.2 Cisplatin 13 ± 0.5 1 2 ± 0.9 aIC50: concentration of the drug required to inhibit growth of 50% of the cancer cells (μM). The data are mean ± SD of three replicates each.


## 4. Conclusion

The structures of the complexes of H-MFMAQ with Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) ions are confirmed by the elemental analyses, IR, NMR (1H, 13C, and 15N) NMR, molar conductance, magnetic moment, UV–Vis., mass, ESR, SEM, EDX, TEM, and thermal analyses data. Therefore, from the IR spectra, it is concluded that H-MFMAQ behaves as a Schiff’s base tetradentate ligand with O3N sites coordinating to the metal ions via the azomethine N group, furan O ring, carbonyl O group, and deprotonated hydroxyl-O group. From the molar conductance data of the complexes (Λm), it is concluded that the complexes of H-MFMAQ ligand are considered as nonelectrolytes. Octahedral geometry was proposed to the Cr(III), Ru(III), Mn(II), Co(II), Ni(II), Cu(II), and Zn(II) complexes. The 1H NMR spectra of the free ligand show that the –OH signal which appeared in the spectrum of H-MFMAQ ligand at 11.35 ppm completely disappeared in the spectra of its Zn(II) complex indicating that the –OH proton is removed by the chelation with Zn(II) ion. The antitumor activities of all inspected compounds were evaluated towardshuman breast (MCF-7) andlung cancer (A549) cell lines.



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