# DNA Binding Test, X-Ray Crystal Structure, Spectral Studies, TG-DTA, and Electrochemistry of [CoX2(dmdphphen)] (Dmdphphen Is 2,9-Dimethyl-4,7-diphenyl-1,10-phenanthroline, X = Cl, and NCS) Complexes

Authors: Mousa Al-Noaimi; Mohammed Suleiman; Hany W. Darwish; Ahmed H. Bakheit; Muneer Abdoh; Iyad Saadeddin; Naveen Shivalingegowda; Neartur Krishnappagowda Lokanath; Odey Bsharat; Assem Barakat; Ismail Warad
Journal: Bioinorganic Chemistry and Applications
 (2014)

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## Abstract

Two new neutral mixed-ligand cobalt(II) complexes, [CoCl2(dmdphphen)] 1 and [Co(NCS)2(dmdphphen)]  2, where dmdphphen is 2,9-dimethyl-4,7-diphenyl-1,10-phenanthroline, were synthesized and characterized by an elemental analysis, UV-Vis, IR, TG/DTA, cyclic voltammetry CV, and single X-ray diffraction. Complex 2 crystallized as monoclinic with a space group P21/c. Co(II) ions are located in a distorted tetrahedral environment. TG/DTA result shows that these complexes are very stable and decomposed through one-step reaction. The two complexes exhibit a quasireversible one-electron response at −550 and 580 mV versus Cp2Fe/Cp2Fe+, which has been assigned to Co(I)/Co(II) and Co(II)/Co(III) couples. Absorption spectral studies reveal that such complexes exhibit hypochromicity during their interaction with CT-DNA.


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## Body

## 1. Introduction

1,10-Phenanthroline ligands and their derivatives are very attractive in metal complexes [1–3]. In addition, their metal complexes are frequently used as catalyst for the enantioselective hydrolysis of N-protected amino acid esters, allylic substitutions, reduction of acetophenone [3–6], and oxidation of olefins [7]. Also, cobalt(II) complexes with a reversible Co(II)/Co(III) are a good oxygen carrier and can oxidize the double bond of the olefins [8–10].The ability of the cobalt phenanthroline complexes to bind and to cleave DNA under physiological conditions is of current interest because of their potential applications in nucleic acids chemistry [11]. Also, these complexes are useful in footprinting studies [12–17]. The cleavage of DNA usually occurs through the heterocyclic bases, deoxyribose sugar moiety, or phosphodiester linkage [18–20]. For the mixed-ligand complexes to interact efficiently with DNA, the ligands need to be flat, have large surface area, and have a spatial geometry to interact with the base pairs in DNA [15–23]. By changing the ligands or the metal ions, it is possible to modify the interaction with nucleic acids [23–26].Previously, a series of several mixed-ligand mononuclear [27, 28] and dinuclear [29, 30] metal complexes have a general formula MX2(dmphen) (2,9-dimethyl-1,10-phenanthroline, X = Cl, NCS) prepared in our lab. These complexes were found to be suitable precursors for spherical shape metal oxide nanoparticles [31]. Herein, two new neutral mixed-ligand cobalt(II) complexes, [CoCl2(dmdphphen)]1 and [Co(NCS)2(dmdphphen)]2, where dmdphphen is (2,9-dimethyl-4,7-diphenyl-1,10-phenanthroline), were synthesized and characterized by different spectroscopic methods. Also, the DNA binding and the catalytic oxidation of styrene in the presence of H2O2 for the complexes were investigated.


## 2. Experimental Section

### 2.1. Materials and Instrumentation

2,9-Dimethyl-4,7-diphenyl-1,10-phenanthroline ligand, CoCl2·6H2O, and Co(NCS)2 were purchased from Acros Organics. Elemental analyses were carried out on an Elementar vario EL analyzer. The IR spectra for samples were recorded using PerkinElmer Spectrum 1000 FT-IR Spectrometer. The UV-Vis spectra were measured by using a TU-1901 double-beam UV-Vis spectrophotometer. TG/DTA spectra were measured by using a TGA-7 PerkinElmer thermogravimetric analyzer. The cyclic voltammograms for the complexes were measured in CH3CN and 0.1 M tetrabutylammonium hexafluorophosphate (TBAHF) using BAS 100 B/W electrochemical workstation (Bioanalytical Systems, West Lafayette, IN, USA) and controlled by a standard 80486 personal computer (BAS control program version 2.0). All electrochemical experiments were carried out at room temperature under argon with a three-electrode cell. Voltalab 80 potentiostat PGZ402 with Pt-disk electrode (Metrohm, A = 0.0064 cm2) was used as working electrode. Platinum wire (£ 1 mm) spiral with diameter 7 mm was used as a counter electrode. Haber-Luggin double reference electrode was used as a reference one. All potentials in this paper are reported to an external Cp2Fe0/+ standard [32].


### 2.2. General Procedure for the Preparation of the Desired Complexes

A mixture of CoX2 salt (2 mmol) in distilled ethanol (15 mL) and free ligand (2.1 mmol) in methanol (10 mL) is stirred for around 0.5 h at room temperature until the precipitation appeared which was filtered, washed with ethanol, and dried. Suitable crystals for X-ray diffraction analysis were growing up by slow diffusion of ethanol into a solution of the complex in CH2Cl2 after two days (yield 88%).


#### 2.2.1. Complex1

Yield: 0.76 g (90%). Anal. Calc. for C26H20Cl2CoN2: C, 63.69; H, 4.11; N, 5.71.Found. C, 63.43; H, 4.21; N, 5.48. UV-Vis (nm) bands in dichloromethane: 655, 572, 360, 240, 280 and 304. M.p 320°C. Conductivity in CH3CN: 10.28 (µS/cm).


#### 2.2.2. Complex2

Yield: 0.94 g (88%). C28H20CoN4S2: Cal. C, 62.80; H, 3.76; N, 10.46; S, 11.97. Found. C, 62.92; H, 3.85; N, 10.33; S, 11.86. UV-Vis (nm) bands in dichloromethane: 645, 566, 358, 242, 282 and 305. M.p 290°C. Conductivity in CH3CN: 9.52 (µS/cm).


### 2.3. Crystallography

A suitable single-crystal complex2 with dimensions of 0.23 × 0.22 × 0.21 mm was chosen for an X-ray diffraction measurement. X-ray intensity data were collected at 296 K on a Bruker CCD diffractometer equipped with Cu Kα radiation (l = 1.54178 Å). Data were collected with the φ and ω scan method. The final unit cell parameters were based on all reflections. Data reduction of all the collected reflections and absorption correction were carried out using the APEX 2 [33] package. The structure was solved by direct methods using SHELXS [34]. The structure was then refined by a full-matrix least-squares method with anisotropic temperature factors for nonhydrogen atoms using SHELXL [34]. All the nonhydrogen atoms were revealed in the first Fourier map itself. After several cycles of refinement, the final difference Fourier map showed peaks of no chemical significance and the residual saturated to 0.0671. Details of data collection and refinement are given in Table 1. The geometrical calculations were carried out using the programPLATON [35]. The molecular and packing diagrams were generated using the softwareMERCURY [36].Table 1
Crystal data and structure refinement for ligand and complex2.
Complex2
Empirical formula
C28H20N4S2Co
Formula weight
535.55
Temperature
293(2) K
Wavelength
1.54178 Å
Crystal system
Monoclinic
Space group
P
2
1
/
c
Unit cell dimensions
a = 14.8373(12) Å α = 90°  b = 21.0942(11) Å  β = 100.191(4)°c = 8.2470(6) Å γ = 90°
Volume
2540.4(3) Å3
Z
4
Density (calculated)
1.400 Mg/m3
Absorption coefficient
7.017 mm−1
F
(
000
)
1100
Crystal size
0.30 × 0.25 × 0.15 mm3
Theta range for data collection
3.03° to 63.94°
Index ranges
−15 ≤h ≤ 17, −21 ≤ k ≤ 24, −9 ≤ l ≤ 6
Reflections collected
8247
Independent reflections
3934[R(int) = 0.0671]
Refinement method
Full-matrix least-squares onF2
Data/restraints/parameters
3934/0/318
Goodness-of-fit onF2
1.047
FinalR indices [I > 2sigma(I)]
R
1 = 0.0671, wR2 = 0.1910
R indices (all data)
R
1 = 0.1715, wR2 = 0.2661
Largest diff. peak and hole
0.641 and −0.870 e⋅Å−3


### 2.4. DNA Binding and Cleavage Experiments

Absorbance measurement was performed to clarify the binding affinity of cobalt(II) complexes by emissive titration at room temperature. The complexes were dissolved in mixed solvent of Tris-HCl buffer (5 mM Tris-HCl/50 mM NaCl buffer for pH = 7.2) for all the experiments and stored at 4°C for further use and used within 2 days. Tris-HCl buffer was subtracted through baseline correction. The absorption experiments were performed by keeping the concentration of cobalt(II) complexes constant (1.5×10-4 mol/L) and increasing the concentration of DNA gradually (1.0×10-4–1×10-3 mol/L).


## 2.1. Materials and Instrumentation

2,9-Dimethyl-4,7-diphenyl-1,10-phenanthroline ligand, CoCl2·6H2O, and Co(NCS)2 were purchased from Acros Organics. Elemental analyses were carried out on an Elementar vario EL analyzer. The IR spectra for samples were recorded using PerkinElmer Spectrum 1000 FT-IR Spectrometer. The UV-Vis spectra were measured by using a TU-1901 double-beam UV-Vis spectrophotometer. TG/DTA spectra were measured by using a TGA-7 PerkinElmer thermogravimetric analyzer. The cyclic voltammograms for the complexes were measured in CH3CN and 0.1 M tetrabutylammonium hexafluorophosphate (TBAHF) using BAS 100 B/W electrochemical workstation (Bioanalytical Systems, West Lafayette, IN, USA) and controlled by a standard 80486 personal computer (BAS control program version 2.0). All electrochemical experiments were carried out at room temperature under argon with a three-electrode cell. Voltalab 80 potentiostat PGZ402 with Pt-disk electrode (Metrohm, A = 0.0064 cm2) was used as working electrode. Platinum wire (£ 1 mm) spiral with diameter 7 mm was used as a counter electrode. Haber-Luggin double reference electrode was used as a reference one. All potentials in this paper are reported to an external Cp2Fe0/+ standard [32].


## 2.2. General Procedure for the Preparation of the Desired Complexes

A mixture of CoX2 salt (2 mmol) in distilled ethanol (15 mL) and free ligand (2.1 mmol) in methanol (10 mL) is stirred for around 0.5 h at room temperature until the precipitation appeared which was filtered, washed with ethanol, and dried. Suitable crystals for X-ray diffraction analysis were growing up by slow diffusion of ethanol into a solution of the complex in CH2Cl2 after two days (yield 88%).


### 2.2.1. Complex1

Yield: 0.76 g (90%). Anal. Calc. for C26H20Cl2CoN2: C, 63.69; H, 4.11; N, 5.71.Found. C, 63.43; H, 4.21; N, 5.48. UV-Vis (nm) bands in dichloromethane: 655, 572, 360, 240, 280 and 304. M.p 320°C. Conductivity in CH3CN: 10.28 (µS/cm).


### 2.2.2. Complex2

Yield: 0.94 g (88%). C28H20CoN4S2: Cal. C, 62.80; H, 3.76; N, 10.46; S, 11.97. Found. C, 62.92; H, 3.85; N, 10.33; S, 11.86. UV-Vis (nm) bands in dichloromethane: 645, 566, 358, 242, 282 and 305. M.p 290°C. Conductivity in CH3CN: 9.52 (µS/cm).


## 2.2.1. Complex1

Yield: 0.76 g (90%). Anal. Calc. for C26H20Cl2CoN2: C, 63.69; H, 4.11; N, 5.71.Found. C, 63.43; H, 4.21; N, 5.48. UV-Vis (nm) bands in dichloromethane: 655, 572, 360, 240, 280 and 304. M.p 320°C. Conductivity in CH3CN: 10.28 (µS/cm).


## 2.2.2. Complex2

Yield: 0.94 g (88%). C28H20CoN4S2: Cal. C, 62.80; H, 3.76; N, 10.46; S, 11.97. Found. C, 62.92; H, 3.85; N, 10.33; S, 11.86. UV-Vis (nm) bands in dichloromethane: 645, 566, 358, 242, 282 and 305. M.p 290°C. Conductivity in CH3CN: 9.52 (µS/cm).


## 2.3. Crystallography

A suitable single-crystal complex2 with dimensions of 0.23 × 0.22 × 0.21 mm was chosen for an X-ray diffraction measurement. X-ray intensity data were collected at 296 K on a Bruker CCD diffractometer equipped with Cu Kα radiation (l = 1.54178 Å). Data were collected with the φ and ω scan method. The final unit cell parameters were based on all reflections. Data reduction of all the collected reflections and absorption correction were carried out using the APEX 2 [33] package. The structure was solved by direct methods using SHELXS [34]. The structure was then refined by a full-matrix least-squares method with anisotropic temperature factors for nonhydrogen atoms using SHELXL [34]. All the nonhydrogen atoms were revealed in the first Fourier map itself. After several cycles of refinement, the final difference Fourier map showed peaks of no chemical significance and the residual saturated to 0.0671. Details of data collection and refinement are given in Table 1. The geometrical calculations were carried out using the programPLATON [35]. The molecular and packing diagrams were generated using the softwareMERCURY [36].Table 1
Crystal data and structure refinement for ligand and complex2.
Complex2
Empirical formula
C28H20N4S2Co
Formula weight
535.55
Temperature
293(2) K
Wavelength
1.54178 Å
Crystal system
Monoclinic
Space group
P
2
1
/
c
Unit cell dimensions
a = 14.8373(12) Å α = 90°  b = 21.0942(11) Å  β = 100.191(4)°c = 8.2470(6) Å γ = 90°
Volume
2540.4(3) Å3
Z
4
Density (calculated)
1.400 Mg/m3
Absorption coefficient
7.017 mm−1
F
(
000
)
1100
Crystal size
0.30 × 0.25 × 0.15 mm3
Theta range for data collection
3.03° to 63.94°
Index ranges
−15 ≤h ≤ 17, −21 ≤ k ≤ 24, −9 ≤ l ≤ 6
Reflections collected
8247
Independent reflections
3934[R(int) = 0.0671]
Refinement method
Full-matrix least-squares onF2
Data/restraints/parameters
3934/0/318
Goodness-of-fit onF2
1.047
FinalR indices [I > 2sigma(I)]
R
1 = 0.0671, wR2 = 0.1910
R indices (all data)
R
1 = 0.1715, wR2 = 0.2661
Largest diff. peak and hole
0.641 and −0.870 e⋅Å−3


## 2.4. DNA Binding and Cleavage Experiments

Absorbance measurement was performed to clarify the binding affinity of cobalt(II) complexes by emissive titration at room temperature. The complexes were dissolved in mixed solvent of Tris-HCl buffer (5 mM Tris-HCl/50 mM NaCl buffer for pH = 7.2) for all the experiments and stored at 4°C for further use and used within 2 days. Tris-HCl buffer was subtracted through baseline correction. The absorption experiments were performed by keeping the concentration of cobalt(II) complexes constant (1.5×10-4 mol/L) and increasing the concentration of DNA gradually (1.0×10-4–1×10-3 mol/L).


## 3. Results and Discussion

### 3.1. Synthesis of the Desired Complexes

The mononuclear CoCl2(dmdphphen) complex1 and Co(NCS)2(dmdphphen) complex2were isolated in a good yield without side product as seen in Scheme 1.Scheme 1
Synthesis of the Co(II) complexes1and2.The structures of the desired complexes were confirmed by using elemental analysis, IR, UV-Vis, TG/DTA, and X-ray single-crystal measurement for complex2. The analytical data of the complexes show the formation of [1 : 1 : 2] [M : dmdphphen : 2X] ratio in a good agreement with the suggested formula [CoX2(dmdphphen)] of the isolated complexes. The isolated solid complexes are insoluble in water, ethanol, n-hexane, and ethers but soluble in chlorinated solvents as CHCl3 and CH2Cl2. The solubility and molar conductance showed that the two complexes are nonelectrolytic in their nature.


### 3.2. X-Ray Crystal Structure

Crystal structure data and selected bonds length for complex2 are compiled in Tables 1 and 2, respectively. ORTEP drawing of the complex is shown in Figure 1. The central cobalt metal ion is coordinated to the two nitrogen atoms (N2 and N13) of the dmdphphen ligand and to two nitrogen atoms (N30 and N33) of the isothiocyanate ligand in a tetrahedral symmetry. The phenanthroline ring in the dmdphphen moiety is essentially planar with an rms deviation of 0.0752 Å. The phenyl rings (C8–C13 and C24–C29) are twisted out of the plane of the dmdphphen moiety as indicated by the dihedral angle values of 43.2(4)° and 47.2(4)°, respectively. All coordination distances and bond angles are similar to those found in similar compounds [37]. No classic hydrogen bonds were observed. In the crystal structure there is a π-π stacking interaction between adjacent dmdphphen and distances 3.7109(17) Å and 3.8070(17) Å, which may account for stabilizing the crystal structure (Figure 2). The packing of the molecules when viewed down along the a axis indicates that the molecules are interlinked by weak hydrogen bonds to form one dimensional chain.Table 2
Selected bond distances (Å) and bond angles (°) of the complex 2.
Bond angles (°)
Bond distances (Å)
N2–Co1–N13
82.11(18)
Co1–N13
2.035(4)
N2–Co1–N30
108.7(2)
Co1–N2
2.032(4)
N2–Co1–N33
122.3(2)
Co1–N30
1.923(7)
N13–Co1–N30
109.3(2)
Co1–N33
1.905(5)
N13–Co1–N33
122.8(2)
N2–C15
1.374(6)
N30–Co1–N33
109.0(2)
N13–C14
1.360(6)Figure 1
ORTEP of the complex2 with atom labelling. Thermal ellipsoids are drawn at the 50% probability level.Figure 2
A crystal packing of complex2 viewed (perspective) along crystallographic a direction.


### 3.3. IR Spectrum

The IR spectrum of complex1 (Figure 3(b)) showed four characteristic absorptions peaks in the range of 3060, 2950, 550, and 350 cm−1 [7–10] which was assigned to H–Ph, H–CH3, Co–N, and Co–Cl stretching vibrations, respectively. New band at 2150 cm−1 which was assigned to NCS vibrations was observed in IR spectrum of complex2 (Figure 3(c)). The H–Ph, H of CH3 in dmdphphen bands appeared in their expected areas (Figure 3(a)).Figure 3
IR-KBr disk spectra of free ligand (a) and their desired complexes1and2.


### 3.4. Electronic Absorption Spectral Study

The experimental absorption spectra (UV-Vis) of the [CoX2(dmphen)] complexes1,2 in dichloromethane solution presented three dominant bands in the regions 200–800 nm (Figure 4). The bands in the UV region centered at around 240, 280, and 300 nm were assigned ligand-centered π-π* transitions (in both complexes). The bands at 360, 572, and 655 nm for complex1 (above) and at 365, 560, and 645 nm for complex1 (down) can be assigned to the d→d transition and MLCT, respectively [14–20].UV-Vis spectrum of the desired complexes (1 and2) in dichloromethane at RT.
(a)
(b)


### 3.5. Thermal Decomposition Analysis of Complexes1

The thermal analysis of complex1 (Figure 5) was investigated in the range of 0–600°C and heating rate of 10°C/min. Figure 5 shows that there is no uncoordinated or coordinated water in the range of 0–150°C and 150–180°C, respectively. Also, it shows that there are no decomposition intermediate steps of the coordinated chloride and dmdphphen ligands; both inorganic and organic ligands were destructured away from the Co metal with one-step broad decomposition in 200–330°C with weight loss ~81% and an exothermic DTA signal at ~315°C; the final residue was confirmed by IR to be CoO.Figure 5
TG/DTA thermal curves of the desired complex1.


### 3.6. Electrochemistry

The electron-transfer behavior of the complexes in acetonitrile solution was examined by cyclic voltammetry. As a representative example, the cyclic voltammogram for complex2is shown in Figure 6. Complex2 exhibited two single electron reversible oxidative responses at −550 and 580 mV versus Cp2Fe/Cp2Fe+, which has been assigned to Co(I)/Co(II) and Co(II)/Co(III) couples, respectively. The dmdphphen ligand is electroinactive over the studied range of +1.5 to −1.5 V. Both complexes exhibit the similar behavior during the cyclic voltammetry experiments.Figure 6
Voltammogram diagram of complex2 (c=1×10-3 M, in acetonitrile solution, 0.1 M TBAHF, scan rate 100 mV/s at RT).


### 3.7. DNA-Complex1 Binding Test

The affinity of Co(II) complexes for double-stranded CT-DNA was explored using UV-Vis titrations in deionised water. The results of representative titrations are shown in Figure7. Complex1 showed good DNA binding affinity. Complex1 has three characteristic absorption peaks at 360 nm, 572 nm, and 655 nm, respectively. There is a decrease in an intensity for all peaks for complex1 by adding several concentrations of DNA. This suggests that the cobalt complex might be bind to DNA by an intercalative mode [38]. However, by comparing the small shift for complex1 with 7 nm red-shift values for Os(phen)2(dppz)2+ [39] and 9 nm for [Co(phen)2(pdtp)]3+ [40], this demonstrates that the intercalative strength of such complexes into DNA is not very strong.Figure 7
Visible spectra of 1.5 × 10−4 mol/L of complex1interacting with (a)—0, (b)—1.0 × 10−4, (c)—5 × 10−4, and (d)—1 × 10−3 mol/L CT-DNA at RT.


## 3.1. Synthesis of the Desired Complexes

The mononuclear CoCl2(dmdphphen) complex1 and Co(NCS)2(dmdphphen) complex2were isolated in a good yield without side product as seen in Scheme 1.Scheme 1
Synthesis of the Co(II) complexes1and2.The structures of the desired complexes were confirmed by using elemental analysis, IR, UV-Vis, TG/DTA, and X-ray single-crystal measurement for complex2. The analytical data of the complexes show the formation of [1 : 1 : 2] [M : dmdphphen : 2X] ratio in a good agreement with the suggested formula [CoX2(dmdphphen)] of the isolated complexes. The isolated solid complexes are insoluble in water, ethanol, n-hexane, and ethers but soluble in chlorinated solvents as CHCl3 and CH2Cl2. The solubility and molar conductance showed that the two complexes are nonelectrolytic in their nature.


## 3.2. X-Ray Crystal Structure

Crystal structure data and selected bonds length for complex2 are compiled in Tables 1 and 2, respectively. ORTEP drawing of the complex is shown in Figure 1. The central cobalt metal ion is coordinated to the two nitrogen atoms (N2 and N13) of the dmdphphen ligand and to two nitrogen atoms (N30 and N33) of the isothiocyanate ligand in a tetrahedral symmetry. The phenanthroline ring in the dmdphphen moiety is essentially planar with an rms deviation of 0.0752 Å. The phenyl rings (C8–C13 and C24–C29) are twisted out of the plane of the dmdphphen moiety as indicated by the dihedral angle values of 43.2(4)° and 47.2(4)°, respectively. All coordination distances and bond angles are similar to those found in similar compounds [37]. No classic hydrogen bonds were observed. In the crystal structure there is a π-π stacking interaction between adjacent dmdphphen and distances 3.7109(17) Å and 3.8070(17) Å, which may account for stabilizing the crystal structure (Figure 2). The packing of the molecules when viewed down along the a axis indicates that the molecules are interlinked by weak hydrogen bonds to form one dimensional chain.Table 2
Selected bond distances (Å) and bond angles (°) of the complex 2.
Bond angles (°)
Bond distances (Å)
N2–Co1–N13
82.11(18)
Co1–N13
2.035(4)
N2–Co1–N30
108.7(2)
Co1–N2
2.032(4)
N2–Co1–N33
122.3(2)
Co1–N30
1.923(7)
N13–Co1–N30
109.3(2)
Co1–N33
1.905(5)
N13–Co1–N33
122.8(2)
N2–C15
1.374(6)
N30–Co1–N33
109.0(2)
N13–C14
1.360(6)Figure 1
ORTEP of the complex2 with atom labelling. Thermal ellipsoids are drawn at the 50% probability level.Figure 2
A crystal packing of complex2 viewed (perspective) along crystallographic a direction.


## 3.3. IR Spectrum

The IR spectrum of complex1 (Figure 3(b)) showed four characteristic absorptions peaks in the range of 3060, 2950, 550, and 350 cm−1 [7–10] which was assigned to H–Ph, H–CH3, Co–N, and Co–Cl stretching vibrations, respectively. New band at 2150 cm−1 which was assigned to NCS vibrations was observed in IR spectrum of complex2 (Figure 3(c)). The H–Ph, H of CH3 in dmdphphen bands appeared in their expected areas (Figure 3(a)).Figure 3
IR-KBr disk spectra of free ligand (a) and their desired complexes1and2.


## 3.4. Electronic Absorption Spectral Study

The experimental absorption spectra (UV-Vis) of the [CoX2(dmphen)] complexes1,2 in dichloromethane solution presented three dominant bands in the regions 200–800 nm (Figure 4). The bands in the UV region centered at around 240, 280, and 300 nm were assigned ligand-centered π-π* transitions (in both complexes). The bands at 360, 572, and 655 nm for complex1 (above) and at 365, 560, and 645 nm for complex1 (down) can be assigned to the d→d transition and MLCT, respectively [14–20].UV-Vis spectrum of the desired complexes (1 and2) in dichloromethane at RT.
(a)
(b)


## 3.5. Thermal Decomposition Analysis of Complexes1

The thermal analysis of complex1 (Figure 5) was investigated in the range of 0–600°C and heating rate of 10°C/min. Figure 5 shows that there is no uncoordinated or coordinated water in the range of 0–150°C and 150–180°C, respectively. Also, it shows that there are no decomposition intermediate steps of the coordinated chloride and dmdphphen ligands; both inorganic and organic ligands were destructured away from the Co metal with one-step broad decomposition in 200–330°C with weight loss ~81% and an exothermic DTA signal at ~315°C; the final residue was confirmed by IR to be CoO.Figure 5
TG/DTA thermal curves of the desired complex1.


## 3.6. Electrochemistry

The electron-transfer behavior of the complexes in acetonitrile solution was examined by cyclic voltammetry. As a representative example, the cyclic voltammogram for complex2is shown in Figure 6. Complex2 exhibited two single electron reversible oxidative responses at −550 and 580 mV versus Cp2Fe/Cp2Fe+, which has been assigned to Co(I)/Co(II) and Co(II)/Co(III) couples, respectively. The dmdphphen ligand is electroinactive over the studied range of +1.5 to −1.5 V. Both complexes exhibit the similar behavior during the cyclic voltammetry experiments.Figure 6
Voltammogram diagram of complex2 (c=1×10-3 M, in acetonitrile solution, 0.1 M TBAHF, scan rate 100 mV/s at RT).


## 3.7. DNA-Complex1 Binding Test

The affinity of Co(II) complexes for double-stranded CT-DNA was explored using UV-Vis titrations in deionised water. The results of representative titrations are shown in Figure7. Complex1 showed good DNA binding affinity. Complex1 has three characteristic absorption peaks at 360 nm, 572 nm, and 655 nm, respectively. There is a decrease in an intensity for all peaks for complex1 by adding several concentrations of DNA. This suggests that the cobalt complex might be bind to DNA by an intercalative mode [38]. However, by comparing the small shift for complex1 with 7 nm red-shift values for Os(phen)2(dppz)2+ [39] and 9 nm for [Co(phen)2(pdtp)]3+ [40], this demonstrates that the intercalative strength of such complexes into DNA is not very strong.Figure 7
Visible spectra of 1.5 × 10−4 mol/L of complex1interacting with (a)—0, (b)—1.0 × 10−4, (c)—5 × 10−4, and (d)—1 × 10−3 mol/L CT-DNA at RT.


## 4. Conclusions

Tetrahedral cobalt(II) complexes [CoCl2(dmdphphen)]1and [Co(NCS)2(dmdphphen)]2 were made available in good yield. Complex2was solved by XRD as monoclinic with a space group P21/c. Co(II) ions are located in a distorted tetrahedral environment. TG/DTA result shows that these complexes are very stable and decomposed through one-step reaction; the complexes exhibit a quasireversible one-electron response at ~−550 mV assigned to Co(I)/Co(II) and ~580 mV assigned to Co(II)/Co(III) versus Cp2Fe/Cp2Fe+. Absorption spectral studies reveal that such complexes exhibit good DNA binding.



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*Source: 914241-2014-12-29.xml*