# DNA Cleavage, Cytotoxic Activities, and Antimicrobial Studies of Ternary Copper(II) Complexes of Isoxazole Schiff Base and Heterocyclic Compounds

Authors: Vijay Kumar Chityala; K. Sathish Kumar; Ramesh Macha; Parthasarathy Tigulla; Shivaraj
Journal: Bioinorganic Chemistry and Applications
 (2014)

---

## Abstract

Novel mixed ligand bivalent copper complexes [Cu. L. A. ClO
4] and [Cu. L. A] where “L” is Schiff bases, namely 2-((3,4-dimethylisoxazol-5-ylimino)methyl)-4-bromophenol (DMIIMBP)/2-((3,4-dimethylisoxazol-5-ylimino)methyl)-4-chlorophenol (DMIIMCP), and “A” is heterocyclic compound, such as 1,10-phenanthroline (phen)/2,21-bipyridyl (bipy)/8-hydroxyquinoline (oxine)/5-chloro-8-hydroxyquinoline (5-Cl-oxine), have been synthesized. These complexes have been characterized by IR, UV-Vis, ESR, elemental analysis, magnetic moments, TG, and DTA. On the basis of spectral studies and analytical data, five-coordinated square pyramidal/four-coordinated square planar geometry is assigned to all complexes. The ligands and their ternary complexes with Cu(II) have been screened for antimicrobial activity against bacteria and fungi by paper disc method. The antimicrobial studies of Schiff bases and their metal complexes showed significant activity and further it is observed that the metal complexes showed more activity than corresponding Schiff bases. In vitro antitumor activity of Cu(II) complexes was assayed against human cervical carcinoma (HeLa) cancer cells and it was observed that few complexes exhibit good antitumor activity on HeLa cell lines. The DNA cleavage studies have also been carried out on pBR 322 and it is observed that these Cu(II) complexes are capable of cleaving supercoiled plasmid DNA in the presence of H2O2 and UV light.


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## Body

## 1. Introduction

Heterocyclic moieties, found in large number of compounds, play an important role in several biological processes. The biological activity of these compounds is mainly dependent on their molecular structures [1–3]. The azomethine group in Schiff bases (–N=CH–) is a significant feature that makes them important compounds owing to their wide range of biological activities [4–7]. Schiff bases are able to inhibit the growth of several animal tumors which can be altered depending upon the type of substituent present on the aromatic rings. Copper plays an essential role in the human organs and the function of copper in the human body is complex and not fully understood [8–11]. The role of Copper is a biocatalyst in the redox reactions. The Cu(II) complexes have demonstrated a wide variety of coordination geometries around Cu(II) atom with N,N and N,O donor ligands and the structure of complex depending on the number, type, and arrangement of ligands about the copper center. The ligands form stable five- or six-membered rings after complexation with the metal ion [12–15]. 8-Hydroxyquinoline and some of its derivatives are monoprotic N,O donor bidentate chelating agents and exhibited substantial cytotoxic activity against cancer cells. The planar nature of “phen” is its ability to participate as either an intercalating or groove-binding agent with DNA [16–19].The Cu(II) metal complexes may interact with DNA by covalent or noncovalent bindings. The labile part of these complexes is replaced by a nitrogen base of DNA such as guanine via its N7 donor atom. On other hand, the noncovalent DNA interactions include intercalative, electrostatic, and groove binding of cationic metal complexes along the outside of DNA helix. Intercalation involves the partial insertion of aromatic heterocyclic rings between the DNA base pairs. Copper has high Lewis acidity which eventually facilitates the DNA cleavage.The interesting biological activities associated with Schiff bases and their mixed ligand complexes promoted us to investigate their DNA interactions. The present paper describes the synthesis, characterization, antimicrobial and antitumor activity, and DNA cleavage activity of novel ternary Cu(II) complexes [Cu(DMIIMBP)(phen)ClO4](1), [Cu(DMIIMBP)(bipy)ClO4](2), [Cu(DMIIMBP)(oxine)](3), [Cu(DMIIMBP)(5-Cl-oxine)](4), [Cu(DMIIMCP)(phen)ClO4](5), [Cu(DMIIMCP)(bipy)ClO4](6), [Cu(DMIIMCP)(oxine)](7), and [Cu(DMIIMCP)(5-Cl-oxine)](8).


## 2. Material and Methods

### 2.1. Physical Measurements

1H- NMR and 13C- NMR spectra of the ligands were recorded on Bruker 400 MHz NMR instrument and using TMS as internal standard. The EI mass spectra were recorded on a VG micromass 7070-H instrument; ESI mass spectra were recorded on VG AUTOSPEC mass spectrometer. Digital conductivity meter of model DI-909 having a dip-type cell was calibrated with KCl solution. Electronic spectra of metal complexes in DMSO were recorded on Schimadzu UV-VIS 1601 spectrophotometer. Magnetic susceptibilities of the complexes were determined on Gouy balance model 7550 using Hg[Co(NCS)4] as standard. The diamagnetic corrections of the complexes were computed using Pascal’s constants. TG of complexes was carried on Mettler Toledo Star system in the temperature range of 0–1000°C. Melting points of the ligands and decomposition temperature of complexes were determined on Polmon instrument (model number MP-96). IR spectra of the compounds were recorded using KBr pellets in the range (4000–400 cm−1) on Perkin-Elmer Infrared model 337. The percentage composition of C, H, and N of the compounds was determined by using microanalytical techniques on Perkin Elmer 240C (USA) elemental analyzer. The EPR spectra of the copper complexes were recorded on EPR Varian-E-112 at room temperature. The percentage composition of metal ions in solid metal complexes was determined by EDTA titration procedure. All the chemicals used were of analytical reagent grade. Solvents such as water, methanol, acetone, petroleum ether, and chloroform were purified by standard procedures [20].


### 2.2. General Procedure for the Synthesis of Isoxazole Schiff Bases

3,4-Dimethyl-5-aminoisoxazole (1.0 mmol) was dissolved in hot methanol to which 5-bromosalicylaldehyde/5-chlorosalicylaldehyde (1.0 mmol) was added and the mixture was refluxed for 2 hours under nitrogen atmosphere. The dark yellow product formed was filtered and washed with petroleum ether and recrystallized from methanol. Purity of the compounds checked by TLC showed single spot in petroleum ether and ethyl acetate (6 : 4) solvent mixture. Yield was 80–85%.


### 2.3. Synthesis of Ternary Cu(II) Metal Complexes

The synthesis of copper complexes1–8 was described in Scheme 1. In the preparation of metal complexes, metal to ligands ratio was maintained at 1 : 1 : 1. Hot methanol solution of ligand (1.0 mmol), hot methanol solution of copper acetate monohydrate [Cu(CH3COO)2
·H2O] (1.0 mmol), and methanol solution of 1,10-phenanthroline/2,21-bipyridine/8-hydroxyquinoline/5-chloro-8-hydroxyquinoline (1.0 mmol) were mixed together with constant stirring. The mixture was refluxed for 2-3 hours at 70–80°C on water bath. After cooling slowly, a few drops of 0.1 M NaClO4 were added for complexes1,2,5, and6 with constant stirring over a period of 1 h and on cooling, the dark green/brown coloured metal complexes were precipitated. The products were filtered, washed with cold methanol, and dried under vacuum over P4O10.Scheme 1
Schematic routes of the synthesis of the complexes.


### 2.4. Cell Culture

The human cervical carcinoma cell lines (HeLa) were cultured as a monolayer with Roswell Park Memorial Institute medium (RPMI-1640), supplemented with 10% (v/v) fetal bovine serum (FBS), 2 mM L-glutamine, 4.5 g/L glucose, 1× nonessential amino acids, and 1 × antibiotics consisting of penicillin/streptomycin, gentamycin, amphotericin B, and nystatin at 37°C, in a humidified atmosphere of 5% CO2, in a CO2 incubator.


#### 2.4.1. Cytotoxicity Assay (MTT Assay)

The MTT assay was used to assess cytotoxicity [21]. The human cervical carcinoma cell lines (HeLa) were obtained from National Center for Cell Science (NCCS), Pune, India. Briefly, the copper complexes (1,2,5, and6) were dissolved in DMSO, diluted in culture medium, and used to treat the cancer cell, with the complex in the concentration range of 2 to 10 μg/mL, for a period of 72 h. DMSO diluted in the culture medium was used as the solvent control. A miniaturized viability assay using 3-[4,5-dimethylthiazol-2-yl]-2,5-diphenyltetrazolium bromide (MTT) was carried out according to the method described earlier [22]. HeLa cells growing exponentially were added to 96-well plates (Orange Scientific) at a density of 3 x 103 per well after counting on Bright Line Haemocytometer (Sigma Ltd.). Compounds (2–10 μg/mL) were then added to the wells, ensuring an equal volume of 200 μL across the plates. Cytotoxicity/proliferation was measured at 72 h using a standard methyl thiazol tetrazolium (MTT) based assay without modifications. Briefly, MTT (Hi Media Ltd.) was added to each well to yield a working concentration of 0.4 mg mL−1, and the plates were returned to the incubator for a further 2 h. After this time, the medium was aspirated, 200 μL of DMSO (Sigma Ltd.) was then added to each well, and the plates were agitated gently for 5 min before measuring the optical density at 600 nm in each well using Thermo Scientific Multiskan EX Elisa reader. The IC50 value was determined as concentration of the complex that is required to reduce the absorbance to half that of the control.


## 2.1. Physical Measurements

1H- NMR and 13C- NMR spectra of the ligands were recorded on Bruker 400 MHz NMR instrument and using TMS as internal standard. The EI mass spectra were recorded on a VG micromass 7070-H instrument; ESI mass spectra were recorded on VG AUTOSPEC mass spectrometer. Digital conductivity meter of model DI-909 having a dip-type cell was calibrated with KCl solution. Electronic spectra of metal complexes in DMSO were recorded on Schimadzu UV-VIS 1601 spectrophotometer. Magnetic susceptibilities of the complexes were determined on Gouy balance model 7550 using Hg[Co(NCS)4] as standard. The diamagnetic corrections of the complexes were computed using Pascal’s constants. TG of complexes was carried on Mettler Toledo Star system in the temperature range of 0–1000°C. Melting points of the ligands and decomposition temperature of complexes were determined on Polmon instrument (model number MP-96). IR spectra of the compounds were recorded using KBr pellets in the range (4000–400 cm−1) on Perkin-Elmer Infrared model 337. The percentage composition of C, H, and N of the compounds was determined by using microanalytical techniques on Perkin Elmer 240C (USA) elemental analyzer. The EPR spectra of the copper complexes were recorded on EPR Varian-E-112 at room temperature. The percentage composition of metal ions in solid metal complexes was determined by EDTA titration procedure. All the chemicals used were of analytical reagent grade. Solvents such as water, methanol, acetone, petroleum ether, and chloroform were purified by standard procedures [20].


## 2.2. General Procedure for the Synthesis of Isoxazole Schiff Bases

3,4-Dimethyl-5-aminoisoxazole (1.0 mmol) was dissolved in hot methanol to which 5-bromosalicylaldehyde/5-chlorosalicylaldehyde (1.0 mmol) was added and the mixture was refluxed for 2 hours under nitrogen atmosphere. The dark yellow product formed was filtered and washed with petroleum ether and recrystallized from methanol. Purity of the compounds checked by TLC showed single spot in petroleum ether and ethyl acetate (6 : 4) solvent mixture. Yield was 80–85%.


## 2.3. Synthesis of Ternary Cu(II) Metal Complexes

The synthesis of copper complexes1–8 was described in Scheme 1. In the preparation of metal complexes, metal to ligands ratio was maintained at 1 : 1 : 1. Hot methanol solution of ligand (1.0 mmol), hot methanol solution of copper acetate monohydrate [Cu(CH3COO)2
·H2O] (1.0 mmol), and methanol solution of 1,10-phenanthroline/2,21-bipyridine/8-hydroxyquinoline/5-chloro-8-hydroxyquinoline (1.0 mmol) were mixed together with constant stirring. The mixture was refluxed for 2-3 hours at 70–80°C on water bath. After cooling slowly, a few drops of 0.1 M NaClO4 were added for complexes1,2,5, and6 with constant stirring over a period of 1 h and on cooling, the dark green/brown coloured metal complexes were precipitated. The products were filtered, washed with cold methanol, and dried under vacuum over P4O10.Scheme 1
Schematic routes of the synthesis of the complexes.


## 2.4. Cell Culture

The human cervical carcinoma cell lines (HeLa) were cultured as a monolayer with Roswell Park Memorial Institute medium (RPMI-1640), supplemented with 10% (v/v) fetal bovine serum (FBS), 2 mM L-glutamine, 4.5 g/L glucose, 1× nonessential amino acids, and 1 × antibiotics consisting of penicillin/streptomycin, gentamycin, amphotericin B, and nystatin at 37°C, in a humidified atmosphere of 5% CO2, in a CO2 incubator.


### 2.4.1. Cytotoxicity Assay (MTT Assay)

The MTT assay was used to assess cytotoxicity [21]. The human cervical carcinoma cell lines (HeLa) were obtained from National Center for Cell Science (NCCS), Pune, India. Briefly, the copper complexes (1,2,5, and6) were dissolved in DMSO, diluted in culture medium, and used to treat the cancer cell, with the complex in the concentration range of 2 to 10 μg/mL, for a period of 72 h. DMSO diluted in the culture medium was used as the solvent control. A miniaturized viability assay using 3-[4,5-dimethylthiazol-2-yl]-2,5-diphenyltetrazolium bromide (MTT) was carried out according to the method described earlier [22]. HeLa cells growing exponentially were added to 96-well plates (Orange Scientific) at a density of 3 x 103 per well after counting on Bright Line Haemocytometer (Sigma Ltd.). Compounds (2–10 μg/mL) were then added to the wells, ensuring an equal volume of 200 μL across the plates. Cytotoxicity/proliferation was measured at 72 h using a standard methyl thiazol tetrazolium (MTT) based assay without modifications. Briefly, MTT (Hi Media Ltd.) was added to each well to yield a working concentration of 0.4 mg mL−1, and the plates were returned to the incubator for a further 2 h. After this time, the medium was aspirated, 200 μL of DMSO (Sigma Ltd.) was then added to each well, and the plates were agitated gently for 5 min before measuring the optical density at 600 nm in each well using Thermo Scientific Multiskan EX Elisa reader. The IC50 value was determined as concentration of the complex that is required to reduce the absorbance to half that of the control.


## 2.4.1. Cytotoxicity Assay (MTT Assay)

The MTT assay was used to assess cytotoxicity [21]. The human cervical carcinoma cell lines (HeLa) were obtained from National Center for Cell Science (NCCS), Pune, India. Briefly, the copper complexes (1,2,5, and6) were dissolved in DMSO, diluted in culture medium, and used to treat the cancer cell, with the complex in the concentration range of 2 to 10 μg/mL, for a period of 72 h. DMSO diluted in the culture medium was used as the solvent control. A miniaturized viability assay using 3-[4,5-dimethylthiazol-2-yl]-2,5-diphenyltetrazolium bromide (MTT) was carried out according to the method described earlier [22]. HeLa cells growing exponentially were added to 96-well plates (Orange Scientific) at a density of 3 x 103 per well after counting on Bright Line Haemocytometer (Sigma Ltd.). Compounds (2–10 μg/mL) were then added to the wells, ensuring an equal volume of 200 μL across the plates. Cytotoxicity/proliferation was measured at 72 h using a standard methyl thiazol tetrazolium (MTT) based assay without modifications. Briefly, MTT (Hi Media Ltd.) was added to each well to yield a working concentration of 0.4 mg mL−1, and the plates were returned to the incubator for a further 2 h. After this time, the medium was aspirated, 200 μL of DMSO (Sigma Ltd.) was then added to each well, and the plates were agitated gently for 5 min before measuring the optical density at 600 nm in each well using Thermo Scientific Multiskan EX Elisa reader. The IC50 value was determined as concentration of the complex that is required to reduce the absorbance to half that of the control.


## 3. Results and Discussion

### 3.1. Characterization of Ligands

The two ligands DMIIMBP and DMIIMCP reported earlier were yellow in colour and stable to air and moisture. The physical and spectral data, such as IR, mass,1H-NMR, and 13C-NMR, obtained for these ligands were in good agreement with the literature data [22].


### 3.2. Characterization of Metal Complexes

All the complexes were stable at room temperature and nonhygroscopic. On heating, they were decomposed at high temperatures. The complexes were insoluble in water but were soluble in DMSO. The composition of the complexes was deduced from the elemental analysis. From the data it was clear that the experimental values shown for each of the complexes were in good agreement with the theoretical values calculated for 1 : 1 : 1 ratio (see Section2.3 of materials and methods). Analytical data of Schiff bases and their metal complexes were presented in Table 1.Table 1
Analytical data of Schiff bases and their metal complexes.
Compound
Formula
M.Wt.
C
H
N
O
M
DMIIMBP
C12H11BrN2O2
296
48.76 (48.84)
3.58 (3.76)
9.34 (9.49)
10.54 (10.84)
—
[Cu(DMIIMBP)(phen)ClO4
]
C24H20BrClCuN4O6
637
44.69 (45.09)
3.11 (3.15)
8.46 (8.76)
14.81 (15.01)
9.89 (9.94)
[Cu(DMIIMBP)(bipy)ClO4
]
C22H20BrClCuN4O6
613
42.33 (42.94)
3.17 (3.28)
8.94 (9.11)
15.14 (15.60)
10.18 (10.33)
[Cu(DMIIMBP)(oxine)]
C21H18BrCuN3O3
502
49.25 (50.06)
3.34 (3.60)
8.27 (8.34)
9.24 (9.53)
12.53 (12.61)
[Cu(DMIIMBP)(5-Cl-oxine)]
C21H17BrClCuN3O3
536
46.01 (46.86)
3.09 (3.18)
7.92 (7.81)
8.65 (8.92)
11.02 (11.81)
DMIIMCP
C12H11ClN2O2
250
57.05 (57.49)
4.34 (4.42)
11.07 (11.17)
12.24 (12.76)
—
[Cu(DMIIMCP)(phen)ClO4
]
C24H20Cl2CuN4O6
593
55.10 (55.46)
3.21 (3.39)
8.99 (9.42)
15.26 (16.14)
10.13 (10.68)
[Cu(DMIIMCP)(bipy)ClO4
]
C22H20Cl2CuN4O6
569
41.98 (46.29)
3.05 (3.53)
9.14 (9.81)
15.95 (16.82)
10.82 (11.13)
[Cu(DMIIMCP)(oxine)]
C21H18ClCuN3O3
458
54.89 (54.90)
3.85 (3.95)
9.10 (9.15)
10.26 (10.45)
12.99 (13.83)
[Cu(DMIIMCP)(5-Cl-oxine)]
C21H17Cl2CuN3O3
492
50.99 (51.08)
3.19 (3.47)
8.14 (8.51)
9.11 (9.72)
12.67 (12.87)


### 3.3. IR Spectra

The important infrared spectral bands and their assignments for the synthesized ligands and complexes were recorded as KBr pellets and were presented in Table2. The IR data of the free ligands and its metal complexes were carried out within the IR range 4000–400 cm−1. In all the Schiff bases, azomethine stretching vibrations appear in the 1633–1605 cm−1 range. These bands were shifted to lower frequency region to the extent of 10–35 cm−1 in complexes, indicating the nitrogen of azomethine is coordinated with the metal ion [23–26]. A broad band around 3453 to 3446 cm−1 in ligands due to the phenolic OH group has disappeared in their complexes indicating coordination through phenolic hydroxyl group [27]. A medium intensity band around 1189 to 1159 cm−1 due to phenolic νC–O group of the ligands shifted to higher or lower frequency region in their complexes, suggesting the participation of the oxygen of the hydroxyl group in bonding with the metal ion [28, 29]. These facts suggest that these shifts are due to coordination of ligand with the metal atom by the azomethine nitrogen and phenolic oxygen. This fact is also supported by the appearance of nonligand bands at appropriate positions in the far infrared region (528–563 cm−1 and 410–454 cm−1) due to νM–O and νM–N vibrations, respectively [30–33]. The peaks corresponding to the ring stretching frequencies (ν(C=C) and ν(C=N)) at 1505, 1421 cm−1 of free phen and at 1509, 1423 cm−1 of free bipy were shifted to higher frequencies upon complexation (1518, 1430 cm−1 for1, 1514, 1446 cm−1 for2, 1516, 1431 cm−1 for5, and 1516, 1447 cm−1 for6), indicating the coordination of the heterocyclic nitrogen atoms of phen and bipy with the metal ion. The characteristic out-of-plane hydrogen bending modes of free phen observed at 851 and 735 cm−1 and for bipy at 848, 740 cm−1 were shifted to 849, 722 cm−1 for1, 841, 731 cm−1 for2, 849, 720 cm−1 for5, and 830, 30 cm−1 for6 upon metal complexation [34]. The peaks around 1112, 1104, and 1034 cm−1 (ν(ClO4)) confirm the presence of a coordinated perchlorate ion [35, 36]. A strong ν(C–O) band observed in the range between 1105 and 1135 cm−1 indicates the presence of oxine moiety in the complexes coordinated through its nitrogen and oxygen atoms as mononegative bidentate ligand [37–40].Table 2
Some important IR absorption frequencies (cm−1) of Schiff bases and metal complexes.
Compound
v(OH)
v(HC=N)
v(C–O)
v(M–O)
v(M–N)
Other bands
DMIIMBP
3446
1641
1182
—
—
v(C–Br) 779
[Cu(DMIIMBP)(phen)ClO4
]
—
1620
1164
550
448
v(Cl–O) 1070, 1104, 1148
[Cu(DMIIMBP)(bipy)ClO4
]
—
1614
1162
548
445
v(Cl–O) 1034, 1058, 1110
[Cu(DMIIMBP)(oxine)]
—
1607
1167 and 1113
550
410
—
[Cu(DMIIMBP)(5-Cl-oxine)]
—
1618
1159 and 1133
543
454
v(C–Cl) 780
DMIIMCP
3453
1605
1183
—
—
v(C–Cl) 778
[Cu(DMIIMCP)(phen)ClO4
]
—
1622
1164
552
434
v(Cl–O) 1071, 1104, 1148
[Cu(DMIIMCP)(bipy)ClO4
]
—
1618
1162
550
419
v(Cl–O) 1036, 1059, 1112
[Cu(DMIIMCP)(oxine)]
—
1609
1189 and 1109
521
414
—
[Cu(DMIIMCP)(5-Cl-oxine)]
—
1633
1183 and 1128
549
421
v(C–Cl) 776


### 3.4. Thermal Analysis

The thermograms of [Cu(DMIIMBP)(phen)ClO4] and [Cu(DMIIMCP)(oxine)] were given in Figures 1(a) and 1(b). From the Figures 1(a) and 1(b) it was found that the heating rates were suitably controlled at 10°C min−1 under nitrogen atmosphere, and the weight loss was measured from the ambient temperature up to 1000°C. The [Cu(DMIIMBP)(phen)ClO4] complex undergoes 1 step of decomposition with the temperature range from 100°C to 370°C with an estimated mass loss of 70.52% (70.91% calculated). In the thermogram it is observed that an exothermic peak appeared at 310°C due to perchlorate. This mass loss corresponds to the pyrolysis of the DMIIMBP and 1,10-phenanthroline ligand molecules leaving CuO as a residue. The [Cu(DMIIMCP)(oxine)] complex undergoes 2 steps of decomposition with the temperature range from 100°C to 370°C with an estimated mass loss of 44.85% (45.01% calculated). This mass loss corresponds to the pyrolysis of the DMIIMCP and oxine ligand molecules leaving CuO as a residue.(a) The TGA spectrum of [Cu(DMIIMBP)(phen)ClO4]. (b) The TGA spectrum of [Cu(DMIIMCP)(oxine)].
(a)
(b)


### 3.5. Magnetic Susceptibility and Electronic Spectra

The electronic spectral data, molar extension coefficient values, and magnetic susceptibility values of the metal complexes are presented in Table3 and from the data it is observed that the magnetic moment values of all Cu(II) complexes were in the range of 1.85–1.96 B.M. which is in accordance with one unpaired electron. In the present studies, all Cu(II) complexes show a single broad band in the range from 14,989 to 16,920 cm−1 due to transition between 2
B
1
g
→
2
E
g suggesting square pyramidal geometry and square planner geometry. Square pyramidal and square planar Cu(II) complexes were expected to give three bands. However, these three bands usually overlap in these complexes to give only one broad absorption band. The electronic spectral and magnetic moment data of all Cu(II) complexes suggest the square pyramidal geometry for complexes1,2,5, and6and square planar geometry for3,4,7, and8 Cu(II) complexes.Table 3
Electronic spectral data and magnetic susceptibility values of the Cu(II) complexes.
Complex
Wave number(
v
) cm−1 (nm)
ε
=
10
2 M−1 cm−1
μ
eff  (BM)
[Cu(DMIIMBP)(phen)ClO4
]
15,545 (646)
0.044
1.85
[Cu(DMIIMBP)(bipy)ClO4
]
16,323 (615)
0.059
1.95
[Cu(DMIIMBP)(oxine)]
16,891 (592)
0.061
1.92
[Cu(DMIIMBP)(5-Cl-oxine)]
15,954 (627)
0.072
1.89
[Cu(DMIIMCP)(phen)ClO4
]
15,210 (662)
0.056
1.93
[Cu(DMIIMCP)(bipy)ClO4
]
14,989 (665)
0.063
1.89
[Cu(DMIIMCP)(oxine)]
16,273 (614)
0.049
1.96
[Cu(DMIIMCP)(5-Cl-oxine)]
16,920 (591)
0.045
1.87


### 3.6. ESR Spectra

ESR spectra of all Cu(II) complexes were recorded as polycrystalline sample on X band at frequency 9.3 GHz under the magnetic field strength 3400 G. The ESR data of copper metal complexes1–8 are presented in Table 4. A representative ESR spectrum of [Cu(DMIIMBP)(phen)ClO4] is shown in Figure 2. According to the data g
∥ and g
⊥ values for all Cu(II) complexes are found to be in the range of 2.149–2.171 and 2.039–2.061, respectively. From the data, it is clear that g
∥
>
g
⊥
>
2.0023
(
g
e
) which suggest the unpaired electron present in d
x
2
-
y
2 orbital giving 2
B
1
g as the ground state and all the complexes are in square planar geometry [41]. Further it was observed that the g
∥ values for all Cu(II) complexes were less than 2.3 in agreement with the covalent character of the metal ligand bond. The g values are related to axial symmetry parameter G by the Hathway expression, that is, G
=
(
g
∥
-
2.0023
)
/
(
g
⊥
-
2.0023
).Table 4
ESR data of copper metal complexes1–8.
Compound
Temperature
g
ll
g
⊥
Δg
G
[Cu(DMIIMBP)(phen)ClO4
]
300 K
2.1539
2.0402
0.1137
3.8279
[Cu(DMIIMBP)(bipy)ClO4
]
300 K
2.1523
2.0536
0.0987
2.9238
[Cu(DMIIMBP)(oxine)]
300 K
2.1510
2.0391
0.1119
3.8624
[Cu(DMIIMBP)(5-Cl-oxine)]
300 K
2.1497
2.0411
0.1086
3.6437
[Cu(DMIIMCP)(phen)ClO4
]
300 K
2.1594
2.0431
0.1162
3.6928
[Cu(DMIIMCP)(bipy)ClO4
]
300 K
2.1710
2.0616
0.1093
2.841
[Cu(DMIIMCP)(oxine)]
300 K
2.1498
2.0423
0.1075
3.5416
[Cu(DMIIMCP)(5-Cl-oxine)]
300 K
2.1526
2.0426
0.1099
3.5807Figure 2
The ESR spectrum of [Cu(DMIIMBP)(phen)ClO4].According to the data, theG values for all Cu(II) complexes were found to be less than 4 indicating the ligands were strong field and the metal ligand bonding in these complexes is covalent [42, 43].


## 3.1. Characterization of Ligands

The two ligands DMIIMBP and DMIIMCP reported earlier were yellow in colour and stable to air and moisture. The physical and spectral data, such as IR, mass,1H-NMR, and 13C-NMR, obtained for these ligands were in good agreement with the literature data [22].


## 3.2. Characterization of Metal Complexes

All the complexes were stable at room temperature and nonhygroscopic. On heating, they were decomposed at high temperatures. The complexes were insoluble in water but were soluble in DMSO. The composition of the complexes was deduced from the elemental analysis. From the data it was clear that the experimental values shown for each of the complexes were in good agreement with the theoretical values calculated for 1 : 1 : 1 ratio (see Section2.3 of materials and methods). Analytical data of Schiff bases and their metal complexes were presented in Table 1.Table 1
Analytical data of Schiff bases and their metal complexes.
Compound
Formula
M.Wt.
C
H
N
O
M
DMIIMBP
C12H11BrN2O2
296
48.76 (48.84)
3.58 (3.76)
9.34 (9.49)
10.54 (10.84)
—
[Cu(DMIIMBP)(phen)ClO4
]
C24H20BrClCuN4O6
637
44.69 (45.09)
3.11 (3.15)
8.46 (8.76)
14.81 (15.01)
9.89 (9.94)
[Cu(DMIIMBP)(bipy)ClO4
]
C22H20BrClCuN4O6
613
42.33 (42.94)
3.17 (3.28)
8.94 (9.11)
15.14 (15.60)
10.18 (10.33)
[Cu(DMIIMBP)(oxine)]
C21H18BrCuN3O3
502
49.25 (50.06)
3.34 (3.60)
8.27 (8.34)
9.24 (9.53)
12.53 (12.61)
[Cu(DMIIMBP)(5-Cl-oxine)]
C21H17BrClCuN3O3
536
46.01 (46.86)
3.09 (3.18)
7.92 (7.81)
8.65 (8.92)
11.02 (11.81)
DMIIMCP
C12H11ClN2O2
250
57.05 (57.49)
4.34 (4.42)
11.07 (11.17)
12.24 (12.76)
—
[Cu(DMIIMCP)(phen)ClO4
]
C24H20Cl2CuN4O6
593
55.10 (55.46)
3.21 (3.39)
8.99 (9.42)
15.26 (16.14)
10.13 (10.68)
[Cu(DMIIMCP)(bipy)ClO4
]
C22H20Cl2CuN4O6
569
41.98 (46.29)
3.05 (3.53)
9.14 (9.81)
15.95 (16.82)
10.82 (11.13)
[Cu(DMIIMCP)(oxine)]
C21H18ClCuN3O3
458
54.89 (54.90)
3.85 (3.95)
9.10 (9.15)
10.26 (10.45)
12.99 (13.83)
[Cu(DMIIMCP)(5-Cl-oxine)]
C21H17Cl2CuN3O3
492
50.99 (51.08)
3.19 (3.47)
8.14 (8.51)
9.11 (9.72)
12.67 (12.87)


## 3.3. IR Spectra

The important infrared spectral bands and their assignments for the synthesized ligands and complexes were recorded as KBr pellets and were presented in Table2. The IR data of the free ligands and its metal complexes were carried out within the IR range 4000–400 cm−1. In all the Schiff bases, azomethine stretching vibrations appear in the 1633–1605 cm−1 range. These bands were shifted to lower frequency region to the extent of 10–35 cm−1 in complexes, indicating the nitrogen of azomethine is coordinated with the metal ion [23–26]. A broad band around 3453 to 3446 cm−1 in ligands due to the phenolic OH group has disappeared in their complexes indicating coordination through phenolic hydroxyl group [27]. A medium intensity band around 1189 to 1159 cm−1 due to phenolic νC–O group of the ligands shifted to higher or lower frequency region in their complexes, suggesting the participation of the oxygen of the hydroxyl group in bonding with the metal ion [28, 29]. These facts suggest that these shifts are due to coordination of ligand with the metal atom by the azomethine nitrogen and phenolic oxygen. This fact is also supported by the appearance of nonligand bands at appropriate positions in the far infrared region (528–563 cm−1 and 410–454 cm−1) due to νM–O and νM–N vibrations, respectively [30–33]. The peaks corresponding to the ring stretching frequencies (ν(C=C) and ν(C=N)) at 1505, 1421 cm−1 of free phen and at 1509, 1423 cm−1 of free bipy were shifted to higher frequencies upon complexation (1518, 1430 cm−1 for1, 1514, 1446 cm−1 for2, 1516, 1431 cm−1 for5, and 1516, 1447 cm−1 for6), indicating the coordination of the heterocyclic nitrogen atoms of phen and bipy with the metal ion. The characteristic out-of-plane hydrogen bending modes of free phen observed at 851 and 735 cm−1 and for bipy at 848, 740 cm−1 were shifted to 849, 722 cm−1 for1, 841, 731 cm−1 for2, 849, 720 cm−1 for5, and 830, 30 cm−1 for6 upon metal complexation [34]. The peaks around 1112, 1104, and 1034 cm−1 (ν(ClO4)) confirm the presence of a coordinated perchlorate ion [35, 36]. A strong ν(C–O) band observed in the range between 1105 and 1135 cm−1 indicates the presence of oxine moiety in the complexes coordinated through its nitrogen and oxygen atoms as mononegative bidentate ligand [37–40].Table 2
Some important IR absorption frequencies (cm−1) of Schiff bases and metal complexes.
Compound
v(OH)
v(HC=N)
v(C–O)
v(M–O)
v(M–N)
Other bands
DMIIMBP
3446
1641
1182
—
—
v(C–Br) 779
[Cu(DMIIMBP)(phen)ClO4
]
—
1620
1164
550
448
v(Cl–O) 1070, 1104, 1148
[Cu(DMIIMBP)(bipy)ClO4
]
—
1614
1162
548
445
v(Cl–O) 1034, 1058, 1110
[Cu(DMIIMBP)(oxine)]
—
1607
1167 and 1113
550
410
—
[Cu(DMIIMBP)(5-Cl-oxine)]
—
1618
1159 and 1133
543
454
v(C–Cl) 780
DMIIMCP
3453
1605
1183
—
—
v(C–Cl) 778
[Cu(DMIIMCP)(phen)ClO4
]
—
1622
1164
552
434
v(Cl–O) 1071, 1104, 1148
[Cu(DMIIMCP)(bipy)ClO4
]
—
1618
1162
550
419
v(Cl–O) 1036, 1059, 1112
[Cu(DMIIMCP)(oxine)]
—
1609
1189 and 1109
521
414
—
[Cu(DMIIMCP)(5-Cl-oxine)]
—
1633
1183 and 1128
549
421
v(C–Cl) 776


## 3.4. Thermal Analysis

The thermograms of [Cu(DMIIMBP)(phen)ClO4] and [Cu(DMIIMCP)(oxine)] were given in Figures 1(a) and 1(b). From the Figures 1(a) and 1(b) it was found that the heating rates were suitably controlled at 10°C min−1 under nitrogen atmosphere, and the weight loss was measured from the ambient temperature up to 1000°C. The [Cu(DMIIMBP)(phen)ClO4] complex undergoes 1 step of decomposition with the temperature range from 100°C to 370°C with an estimated mass loss of 70.52% (70.91% calculated). In the thermogram it is observed that an exothermic peak appeared at 310°C due to perchlorate. This mass loss corresponds to the pyrolysis of the DMIIMBP and 1,10-phenanthroline ligand molecules leaving CuO as a residue. The [Cu(DMIIMCP)(oxine)] complex undergoes 2 steps of decomposition with the temperature range from 100°C to 370°C with an estimated mass loss of 44.85% (45.01% calculated). This mass loss corresponds to the pyrolysis of the DMIIMCP and oxine ligand molecules leaving CuO as a residue.(a) The TGA spectrum of [Cu(DMIIMBP)(phen)ClO4]. (b) The TGA spectrum of [Cu(DMIIMCP)(oxine)].
(a)
(b)


## 3.5. Magnetic Susceptibility and Electronic Spectra

The electronic spectral data, molar extension coefficient values, and magnetic susceptibility values of the metal complexes are presented in Table3 and from the data it is observed that the magnetic moment values of all Cu(II) complexes were in the range of 1.85–1.96 B.M. which is in accordance with one unpaired electron. In the present studies, all Cu(II) complexes show a single broad band in the range from 14,989 to 16,920 cm−1 due to transition between 2
B
1
g
→
2
E
g suggesting square pyramidal geometry and square planner geometry. Square pyramidal and square planar Cu(II) complexes were expected to give three bands. However, these three bands usually overlap in these complexes to give only one broad absorption band. The electronic spectral and magnetic moment data of all Cu(II) complexes suggest the square pyramidal geometry for complexes1,2,5, and6and square planar geometry for3,4,7, and8 Cu(II) complexes.Table 3
Electronic spectral data and magnetic susceptibility values of the Cu(II) complexes.
Complex
Wave number(
v
) cm−1 (nm)
ε
=
10
2 M−1 cm−1
μ
eff  (BM)
[Cu(DMIIMBP)(phen)ClO4
]
15,545 (646)
0.044
1.85
[Cu(DMIIMBP)(bipy)ClO4
]
16,323 (615)
0.059
1.95
[Cu(DMIIMBP)(oxine)]
16,891 (592)
0.061
1.92
[Cu(DMIIMBP)(5-Cl-oxine)]
15,954 (627)
0.072
1.89
[Cu(DMIIMCP)(phen)ClO4
]
15,210 (662)
0.056
1.93
[Cu(DMIIMCP)(bipy)ClO4
]
14,989 (665)
0.063
1.89
[Cu(DMIIMCP)(oxine)]
16,273 (614)
0.049
1.96
[Cu(DMIIMCP)(5-Cl-oxine)]
16,920 (591)
0.045
1.87


## 3.6. ESR Spectra

ESR spectra of all Cu(II) complexes were recorded as polycrystalline sample on X band at frequency 9.3 GHz under the magnetic field strength 3400 G. The ESR data of copper metal complexes1–8 are presented in Table 4. A representative ESR spectrum of [Cu(DMIIMBP)(phen)ClO4] is shown in Figure 2. According to the data g
∥ and g
⊥ values for all Cu(II) complexes are found to be in the range of 2.149–2.171 and 2.039–2.061, respectively. From the data, it is clear that g
∥
>
g
⊥
>
2.0023
(
g
e
) which suggest the unpaired electron present in d
x
2
-
y
2 orbital giving 2
B
1
g as the ground state and all the complexes are in square planar geometry [41]. Further it was observed that the g
∥ values for all Cu(II) complexes were less than 2.3 in agreement with the covalent character of the metal ligand bond. The g values are related to axial symmetry parameter G by the Hathway expression, that is, G
=
(
g
∥
-
2.0023
)
/
(
g
⊥
-
2.0023
).Table 4
ESR data of copper metal complexes1–8.
Compound
Temperature
g
ll
g
⊥
Δg
G
[Cu(DMIIMBP)(phen)ClO4
]
300 K
2.1539
2.0402
0.1137
3.8279
[Cu(DMIIMBP)(bipy)ClO4
]
300 K
2.1523
2.0536
0.0987
2.9238
[Cu(DMIIMBP)(oxine)]
300 K
2.1510
2.0391
0.1119
3.8624
[Cu(DMIIMBP)(5-Cl-oxine)]
300 K
2.1497
2.0411
0.1086
3.6437
[Cu(DMIIMCP)(phen)ClO4
]
300 K
2.1594
2.0431
0.1162
3.6928
[Cu(DMIIMCP)(bipy)ClO4
]
300 K
2.1710
2.0616
0.1093
2.841
[Cu(DMIIMCP)(oxine)]
300 K
2.1498
2.0423
0.1075
3.5416
[Cu(DMIIMCP)(5-Cl-oxine)]
300 K
2.1526
2.0426
0.1099
3.5807Figure 2
The ESR spectrum of [Cu(DMIIMBP)(phen)ClO4].According to the data, theG values for all Cu(II) complexes were found to be less than 4 indicating the ligands were strong field and the metal ligand bonding in these complexes is covalent [42, 43].


## 4. Molecular Modeling

Successful docking was performed for the selected DMIIMBP and DMIIMCP compounds and their corresponding Gold Fitness score and Chem scores were given in Tables5
(
a
) and 5
(
b
). The interactions of DMIIMBP and DMIIMCP with protein were shown in Figures 3(a) and 3(b).Table 5
(a) Gold Fitness values of the ligands DMIIMBP and DMIIMCP. (b) Chem score values of the ligands DMIIMBP and DMIIMCP.
(a)
S. number
Compound
Gold Fitness
S(hb_ext)
S(vdw_ext)
S(hb_int)
S(vdw_int)
1
DMIIMBP
57.67
4.67
41.97
0.00
−4.71
2
DMIIMCP
57.70
4.55
41.52
0.00
−3.94
(b)
S. number
Compound
Chem score
DG
S(hbond)
S(metal)
S(lipo)
DE(clash)
DE(int)
1
DMIIMBP
19.16
−19.44
1.88
0.00
87.41
0.03
0.25
2
DMIIMCP
19.03
−19.23
1.90
0.00
85.10
0.01
0.18(a) Interactions between TYR and LYS-DMIIMBP crystal ligand (yellow) and target protein (pale green). The TYR residue (gray) and LYS residue (pink) interactions are shown in CPK model. Hydrogen bonding interactions were represented as line (red). (b) Interactions between ASN-DMIIMCP crystal ligand (green) and target protein (pale green). The ASN residue (pink) interactions are shown in CPK model. Hydrogen bonding interactions were represented as line (red).
(a)
(b)For any docked pose [44], the Gold score is calculated generally as the sum of the electrostatic, van der Waals, and hydrophobic interactions and hydrogen bonding interactions. Chem score function includes metal-binding and solvation terms. The Gold Fitness ranges from 57.67 to 57.70 and Chem score ranges from 19.16 to 19.03. Docking results revealed that DMIIMBP and DMIIMCP ligands are involved in hydrogen bonding and van der Waals interactions with the active site residues of DNA topoisomerase I. Among these ligands, DMIIMBP was the best inhibitor of DNA topoisomerase I. The binding energy and the total energy of DMIIMBP and DMIIMCP were listed in Table 6. The LUMO and HOMO structures of DMIIMBP and DMIIMCP were shown in Figures 4(a) and 4(b). The energy levels of LUMO and HOMO reveal that the DMIIMBP was very potential in antimicrobial activity.Table 6
The energy values of the ligands DMIIMBP and DMIIMCP.
Molecule
HOMO (eV)
LUMO (eV)
Binding energy (kcal/mol)
Total energy (kcal/mol)
DMIIMBP
−8.96
−1.09
−7.36
−2959.70
DMIIMCP
−8.89
−1.06
−7.49
−2976.18(a) LUMO and HOMO structures for DMIIMBP. (b) LUMO and HOMO structures for DMIIMCP.
(a)
(b)


## 5. Antimicrobial Activity

In the present investigation, biological activity of the ligands, namely, DMIIMBP, DMIIMCP and their ternary complexes with Cu(II), has been screened for antimicrobial activity against bacteria (E. coli andP. aeruginosa) and fungi (A. niger andR. oryzae) by paper disc method. The concentration for these samples was maintained as 1 mg/mL in DMSO. The results thus obtained were explained on the basis of Overtone’s concept and Chelation theory [45, 46]. The mode of action of the compounds may involve formation of a hydrogen bond through the azomethine group with the active centers of cell constituents, resulting in an interference with the normal cell process [47].The variation in the activity of different complexes against different organisms depends either on the impermeability of the cells of the microbes or difference in ribosome of microbial cells. A comparison of the biological activity of the synthesized compounds with some known antibiotics (ciprofloxacin and ketoconazole) is presented in Table7. It is observed that some of Schiff base metal complexes exhibit better activity than the corresponding ligands.Table 7
Antimicrobial activity of the Schiff bases and metal complexes.
Complex
E. Coli
P. aeruginosa
R. oryzae
A. niger
DMIIMBP
17
14
11
8
[Cu(DMIIMBP)(phen)ClO4
]
19
16
13
10
[Cu(DMIIMBP)(bipy)ClO4
]
18
15
12
9
[Cu(DMIIMBP)(oxine)]
16
14
10
8
[Cu(DMIIMBP)(5-Cl-oxine)]
18
17
9
9
DMIIMCP
16
13
10
10
[Cu(DMIIMCP)(phen)ClO4
]
17
16
11
12
[Cu(DMIIMCP)(bipy)ClO4
]
18
15
11
11
[Cu(DMIIMCP)(oxine)]
15
14
8
8
[Cu(DMIIMCP)(5-Cl-oxine)]
16
15
9
10
Ciprofloxacin
20
18
—
—
Ketoconazole
—
—
15
13


## 6. Cytotoxic Activity

The cytotoxic activity of Cu(II) complexes was assayed on cultured human cervical carcinoma cell lines (HeLa) for 72 h to the medium containing the respective complexes at 2 to 10μg/mL concentration and adopting MTT assay and results were given in Table 8.Table 8
In vitro cytotoxicity (HeLa cell line) of Cu (II) complexes.
Concentration (μg/mL)
Absorbance
Cell viability (%)
Toxicities (%)
Concentration (μg/mL)
Absorbance
Cell viability (%)
Toxicities (%)
Control
0.1165
100
0
Control
0.1165
100
0
[Cu(DMIIMBP)(phen)ClO4
]
[Cu(DMIIMBP)(bipy)ClO4
]
2
0.1011
86.90
13.10
2
0.0800
68.66
31.34
4
0.0751
64.35
35.65
4
0.0625
53.64
46.36
6
0.0732
63.05
36.95
6
0.0534
45.83
54.17
8
0.0611
52.50
47.50
8
0.0502
43.09
56.91
10
0.0532
45.59
54.41
10
0.0495
42.49
57.51
[Cu(DMIIMCP)(phen)ClO4
]
[Cu(DMIIMCP)(bipy)ClO4
]
2
0.0880
75.53
24.47
2
0.1120
96.13
3.87
4
0.0833
71.50
28.50
4
0.0985
84.54
15.46
6
0.0605
51.93
48.07
6
0.0726
62.31
37.69
8
0.0580
49.78
50.22
8
0.0696
59.74
40.26
10
0.0550
47.21
52.79
10
0.0580
49.78
50.22The cytotoxic activity determined according to the dose values of the exposure of the complex required to reduce survival of the cell was given in Figure5. The toxicities of 10 μg/mL of [Cu(DMIIMBP)(phen)ClO4](1), [Cu(DMIIMBP)(bipy)ClO4](2), [Cu(DMIIMCP)(phen)ClO4](5), and [Cu(DMIIMCP)(bipy)ClO4](6) complexes were found to be 54.41%, 57.51%, 52.79%, and 50.22%, respectively. According to these results, [Cu(DMIIMBP)(bipy)ClO4](2) complex was found to behave as a good antitumor agent on HeLa cell lines. The IC50 values obtained in this study were given in Table 9. The IC50 value of the [Cu(DMIIMBP)(phen)ClO4](1), [Cu(DMIIMBP)(bipy)ClO4](2), [Cu(DMIIMCP)(phen)ClO4](5), and [Cu(DMIIMCP)(bipy)ClO4](6) complexes was higher for the 72 h treatment groups, that is, 10
±
0.09 μg/mL, whereas for [Cu(DMIIMBP)(bipy)ClO4] the IC50 value is 5
±
0.06 μg/mL.Table 9
IC50 range of Cu (II) complexes for HeLa cells.
Complex
IC50 (μg/mL)
[Cu(DMIIMBP)(phen)ClO4
]
9 ± 0.03
[Cu(DMIIMBP)(bipy)ClO4
]
5 ± 0.06
[Cu(DMIIMCP)(phen)ClO4
]
8 ± 0.03
[Cu(DMIIMCP)(bipy)ClO4
]
10 ± 0.09Figure 5
Percentage of cell viability versus different concentrations for HeLa cells exposed to the metal complexes after 72 h incubation.


## 7. DNA Cleavage Studies

The cleavage activity was demonstrated by gel-electrophoresis experiments using supercoiled (SC) plasmid pBR 322 DNA in a medium TAE buffer. These experiments were monitored by the addition of varying concentrations of the complex (40–200μM). When DNA was incubated with increasing concentrations of the complexes, SC DNA was degraded to nicked circular (NC) form. The catalytic activities of complexes1and2 were depicted in Figure 6. The activity of1 starts at a concentration as low as 40 μM. At 40 μM, 80 μM, and 120 μM, a complete conversion of SC plasmid DNA into the NC form was observed, and the DNA completely smeared is shown in Figure 6(a) (lanes 2, 3, and 4). In contrast, only 63% cleavage was achieved with2as shown in Figure 6(a) (lanes 6, 7 and 8). This may be due to the efficient binding of1 with DNA compared to that of2. To ensure that the Cu complexes were solely responsible for the cleavage, several control experiments were performed under identical conditions. No cleavage of DNA was observed with free Cu (100 mm) and free ligands (100 mm). In a control experiment with DMSO (1 mm), a known radical scavenger, only slight inhibition (ca. 2%) of DNA cleavage was observed, ruling out the possibility of DNA cleavage via OH-based depurination pathway and also a possible oxidative cleavage [48, 49]. When circular plasmid DNA is subjected to electrophoresis, relatively fast migration will be observed for the intact supercoil form (Form-I). If scission occurs on one strand (nicking), the supercoil will relax to generate a slower-moving open circular form (Form-II). If both strands were cleaved, a linear form (Form-III) that migrates between Form-I and Form-II will be generated [50]. The cleavage effect upon irradiation of the plasmid pBR322 DNA in the presence of different concentrations of complexes1and2has been tested and is shown in Figure 6(b): Lane 1 DNA alone, Lanes 2–4 DNA + complex (1), and Lanes 6–8 DNA + complex (2) with increasing concentration (40 μM, 80 μM, and 120 μM) of complex. Form-II increases and Form-I decreases gradually as the concentration of complex increases. The results suggest concentration-dependent single-strand cleavage of supercoiled Form-I to the nicked Form-II. Under comparable experimental conditions, complex1 exhibits more effective DNA cleavage activity than complex2. The different cleaving efficiency may be ascribed to the different binding affinity of complexes to DNA.Agarose gel electrophoresis patterns for the oxidative cleavage of pBR 322 DNA by 1 and 2(a) and photolytic cleavage of pBR 322 DNA by 1 and 2(b). (a) Lane 1, DNA control; Lane 2, DNA+1 (40 μM) + H2O2 (1 mM); Lane 3, DNA+1 (80 μM) + H2O2 (1 mM); Lane 4, DNA+1 (120 μM) + H2O2 (1 mM); Lane 5, DNA + H2O2 (1 mM) + DMSO (1 mM). Lane 6, DNA+2 (40 μM) + H2O2 (1 mM); Lane 7, DNA+2 (80 μM) + H2O2 (1 mM); Lane 8, DNA+2 (120 μM) + H2O2 (1 mM); (b) Lane 1, DNA control; Lane 2, DNA+1 (40 μM) + H2O2 (1 mM); Lane 3, DNA+1 (80 μM) + H2O2 (1 mM); Lane 4, DNA+1 (120 μM) + H2O2 (1 mM); Lane 5, DNA + DMSO (1 mM). Lane 6, DNA+2 (40 μM) + H2O2 (1 mM); Lane 7, DNA+2 (80 μM) + H2O2 (1 mM); Lane 8, DNA+2 (120 μM) + H2O2 (1 mM).
(a)
(b)


## 8. Conclusions

Mixed ligand metal chelates of Cu(II) with DMIIMBP/DMIIMCP and phen/bipy/oxine/5-Cl-oxine have been synthesized and characterized. The metal ligand stoichiometry in all complexes was found to be 1 : 1 : 1. The Schiff bases act as monobasic bidentate coordinating through nitrogen of azomethine and phenolic oxygen atom. Based on analytical, conductance, IR, magnetic moments, electronic, and ESR spectral data for the complexes1,2,5, and6 and for complexes3,4,7, and8, five-coordinated square pyramidal geometry and four-coordinated square planar geometry are assigned, respectively. Docking studies of the Schiff bases reveal that DMIIMBP Schiff base was more potential for antimicrobial activity. Further it is observed that metal complexes showed higher activity than corresponding Schiff bases and some complexes showed comparable activity with standard drug. The cytotoxicity of all the Cu(II) complexes was assayed and it was found that the cytotoxicity of the [Cu(DMIIMBP)(bipy)ClO4] complex at 10 μg/mL concentration shows 57.51% toxicity suggesting good antitumor agent on human cervical carcinoma cell lines. In the DNA cleavage studies it is observed that the [Cu(DMIIMBP)(phen)ClO4](1) shows more potential activity than the other complexes due to its higher planarity nature.



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*Source: 691260-2014-05-08.xml*