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Crystals 2017, 7(9), 277; doi:10.3390/cryst7090277

Article
Synthesis, Crystal Structure, Luminescence, Electrochemical and Antimicrobial Properties of Bis(salamo)-Based Co(II) Complex
Li Wang, Jing Hao, Li-Xiang Zhai, Yang Zhang and Wen-Kui Dong *Orcid
School of Chemical and Biological Engineering, Lanzhou Jiaotong University, Lanzhou 730070, China
*
Correspondence: Tel.: +86-931-493-8703
Academic Editor: Shujun Zhang
Received: 5 September 2017 / Accepted: 10 September 2017 / Published: 12 September 2017

Abstract

:
A newly designed Co(II) complex, [Co3(L)(OAc)2(CH3OH)2]·CH3OH, by the reaction of a bis(salamo)-type tetraoxime ligand (H4L) with Co(II) acetate tetrahydrate was synthesized and characterized by elemental analyses, IR, UV-vis spectra and single-crystal X-ray crystallography. The UV-vis titration experiment manifested that a trinuclear (L:M = 1:3) complex was formed. It is worth noting that the two terminal Co(II) (Co1 and Co3) atoms of the Co(II) complex have different coordination modes and geometries unreported earlier. Furthermore, through intermolecular interactions (C–H···O, C–H···π and O–H···O), a 2D layer-like network is constructed. In addition, the fluorescence behaviors, antimicrobial activities and electrochemical properties of H4L and its Co(II) complex were investigated.
Keywords:
complex; crystal structure; supramolecular interaction; luminescent study; cyclic voltammetry; antimicrobial activity

1. Introduction

N2O2 salen-type ligands and their analogues have been the focus of increasing attention because their metal complexes are used as catalysts of organic reactions [1,2,3,4,5,6,7], nonlinear optical materials [8,9,10,11,12,13,14,15,16,17,18], electrochemical fields [19,20,21,22], ion recognition [23,24,25], supramolecular architectures [26,27,28,29,30,31,32,33,34,35,36,37], biological fields [38,39,40,41,42], magnetic materials [43,44,45,46] and so forth. With respect to these complexes, phenoxo bridging plays a key role in assembling metal ions and salen-type ligands.
To date, a novel salen-type analogue, salamo, has been studied originally [47,48,49,50,51,52,53,54]. Salamo-type ligands and their metal complexes can resist the C=N exchange reaction. They are also useful as a building block for larger supramolecules. In addition, if hydroxyl and naphthaleneol groups are introduced to the salamo-type ligands, a highly versatile coordination ability and preferable practical property are expected. Taking these factors into account, a new complex [Co3(L)(OAc)2(CH3OH)2]·CH3OH containing naphthaleneol-based bis(salamo)-type tetraoxime ligand (H4L) was synthesized and characterized by elemental analyses, IR, single-crystal X-ray crystallography and UV-vis titration. Meanwhile, the electrochemical properties of the Co(II) complex were investigated by cyclic voltammetry, and the fluorescent and antibacterial properties of H4L and its Co(II) complex were also studied.

2. Experimental

Crystallographic data have been deposited with the Cambridge Crystallographic Data Centre (CCDC) as supplementary publication, No. CCDC 1572529. Copies of the data can be obtained free of charge on application to CCDC, 12 Union Road, Cambridge CB21EZ, UK (Telephone: +(44)-01223-762910; Fax: +44-1223-336033; E-mail: deposit@ccdc.cam.ac.uk). These data can be also obtained free of charge at www.ccdc.cam. Ac.uk/conts/retrieving.html.

2.1. Materials and Methods

2-Hydroxy-3-methoxybenzaldehyde (99%), methyl trioctyl ammonium chloride (90%), pyridinium chlorochromate (98%) and boron tribromide (99.9%) were purchased from Alfa Aesar (New York, NY, USA). Hydrobromic acid 33 wt% solution in acetic acid was purchased from J&K Scientific Ltd. (Beijing, China). The other reagents and solvents were analytical grade reagents from Tianjin Chemical Reagent Factory (Tianjin, China) and used as received.
C, H, and N analyses were obtained using a GmbH VarioEL V3.00 automatic elemental analysis instrument (Berlin, Germany). Elemental analysis for Co(II) was detected by an IRIS ER/S·WP-1 ICP atomic emission spectrometer (Berlin, Germany). 1H NMR spectra were determined by a German Bruker AVANCE DRX-400 spectrometer (Bruker, Billerica, MA, USA). UV-vis titration was recorded on a Shimadzu UV-2550 spectrophotometer (Shimadzu, Kyoto, Japan) in mixed solvent (DMF/CH3OH = 1:1, v/v). IR spectra were recorded on a Vertex 70 FT-IR spectrophotometer (Bruker, Billerica, MA, USA), with samples prepared as KBr (400–4000 cm−1) pellets. X-ray single crystal structure was determined on a Agilent SuperNova Eos diffractometer (Bruker, Billerica, MA, USA). Melting points were measured by the use of a microscopic melting point apparatus made in Beijing Taike Instrument Limited Company (Beijing, China), and the thermometer was uncorrected. Fluorescence spectra were recorded on a Hitachi F-7000 FL spectrophotometer (Hitachi, Tokyo, Japan). Cyclic voltammetry measurements were performed using Chi 660 voltammetric analyzer (CH Instruments, Austin, TX, USA) in DMF containing 0.05 mol L−1 tetrabutylammonium perchlorate.

2.2. Synthesis of H4L

1,2-Bis(aminooxy)ethane, 2-hydroxy-1-naphthaldehyde and 2,3-dihydroxynaphthalene-1,4-dicarbaldehyde were synthesized according an analogous procedure reported earlier [55,56]. The major reaction steps of H4L and its Co(II) complex are given in Scheme 1.
2,3-Dihydroxynaphthalene-1,4-dicarbaldehyde (216.0 mg, 1.0 mmol) was added to an ethanol solution (60 mL) of 2-[O-(1-ethyloxyamide)]oxime-2-naphthol (492.5 mg, 2 mmol). The suspension solution was stirred at 40 °C for 15 h. After cooling to room temperature, the precipitate was filtered and washed successively with ethanol and ethanol-hexane (1:4). The product was dried in vacuo, and 355.3 mg of a yellow crystalline solid was obtained. Yield: 570.0 mg (85.1%), m.p. 201–203 °C. Anal. Calcd for C38H32N4O8 (%): C, 67.85; H, 4.79; N, 8.33. Found: C, 67.83; H, 4.80; N, 8.36. 1H NMR (400 MHz, DMSO) δ 10.72 (s, 4H), 9.14 (s, 2H), 9.05 (s, 2H), 8.67 (d, J = 8.5 Hz, 2H), 8.51 (dd, J = 6.5, 3.3 Hz, 2H), 7.85 (dd, J = 15.7, 8.4 Hz, 4H), 7.50 (s, 2H), 7.36 (s, 4H), 7.21 (d, J = 8.9 Hz, 2H), 4.62 (s, 8H).

2.3. Synthesis of the Co(II) Complex

A solution of cobalt(II) acetate tetrahydrate (14.95 mg, 0.06 mmol) in methanol (3 mL) was added dropwise to a solution of H4L (13.44 mg, 0.02 mmol) in chloroform (4 mL) at room temperature. After stirring for 20 min, the color of the mixed solution turned to brown; the solvent was allowed to partially evaporate for two weeks at room temperature, after which nigger-brown block-shaped single crystals suitable for X-ray diffraction studies were obtained. Anal. Calcd for C45H46Co3N4O15 (%): C, 51.00; H, 4.38; N, 5.29; Co, 16.68. Found: C, 50.79; H, 4.33; N, 5.37; Co, 16.48.

2.4. Crystal Structure Determination of the Co(II) Complex

Intensity data of the Co(II) complex was recorded at 293(2) K employing a Agilent SuperNova Eos diffractometer with a monochromated Mo- radiation (λ = 0.71073 Å) source. Crystal decay was not observed during the data collections. Multiscan absorption corrections were applied using the SADABS software (Bruker, Billerica, MA, USA). The structure was solved by using Fourier difference method and refined by the full-matrix least-squares method on F2 using the SHELXTL [57] crystallographic software package (Bruker, Billerica, MA, USA). The non-hydrogen atoms were generated anisotropically. All hydrogen atoms were positioned geometrically. A summary of the crystal data and final details relevant to the structure determination is listed in Table 1.

3. Results and Discussion

3.1. IR Spectra

The FT–IR spectra of the free ligand H4L and its corresponding Co(II) complex are given in Figure 1. The ligand H4L and its Co(II) complex show various bands in the region of 400–4000 cm−1. The ligand H4L has a broad absorption band at 3419 cm−1, which is the stretching vibration absorption band of phenol hydroxyl group. The ligand H4L shows a characteristic band of C=N group at 1609 cm−1, which is shifted by 14 cm−1 in the Co(II) complex indicating that the Co(II) ions are coordinated by oxime nitrogen atoms of completely deprotonated (L)4− units [58], which is similar to previously reported Co(II) complexes. The Ar–O stretching vibration of the ligand appears at 1235 cm−1 while the Co(II) complex is observed at 1231 cm−1 implying that the Co(II) ions are coordinated by oxygen atoms of phenolic groups of the (L)4− units [59]. In addition, a O–H stretching band can be found at 3411 cm1 in the Co(II) complex, which indicates the presence of methanol molecules, which is in accordance with the results determined by X-ray diffraction.

3.2. UV-Vis Titration

In the UV-vis titration experiment of the Co(II) complex, the solution of H4L in mixed solvent (DMF/CH3OH = 1:1, v/v) was changed from near colorless to light brown during the Co(II) acetate titration process. It can be seen from Figure 2 that the ligand H4L has two strong absorption peaks at 313 and 355 nm, which can be assigned to π→π* type transition and indicates that the ligand H4L contains a large conjugation system. The former can be assigned to the π-π* transition of the naphthalene rings and the latter one to the π-π* transition of the oxime groups [60]. Upon coordination of the ligand, the intraligand π-π* transition of the naphthalene rings of the salicylaldehyde group appears at ca. 317 nm in the Co(II) complex. Compared with the free ligand H4L, the absorption band at ca. 355 nm disappears from the UV-vis spectrum of the Co(II) complex, which indicates that the oxime nitrogen atoms are involved in coordination to the Co(II) atoms. Moreover, the new absorption band is observed at ca. 385 nm for the Co(II) complex, and assigned to L→M charge-transfer (LMCT) transition which is characteristic of the transition metal complexes with N2O2 coordination sphere [61].
The H4L contains two salamo cavities and one O4 coordination environment and it is assumed that the coordination ratio of the Co(II) complex is 1:3. After the addition of 3.0 equiv of Co(II) acetate tetrahydrate, changes in UV-vis absorption intensity ceased. The result is consistent with the result of the elemental analyses mentioned above.

3.3. Crystal Structure

The analysis of the crystal structure of the Co(II) complex indicates that the H4L to Co(II) ratio is 3:1. The molecule structure and coordination configuration of the Co(II) complex are illustrated in Figure 3. The parameter values of bond distances and angles are listed in Table 2.
Single-crystal X-ray diffraction analysis reveals that the Co(II) complex crystallizes in the monoclinic system in the P 1 n 1 space group with Z = 2. The Co(II) complex is composed of three Co(II) ions, one completely deprotonated (L)4− unit, two μ2-acetate ions, two methanol molecules participating in coordination and one uncoordinated methanol molecule. Three coordination environments of the (L)4− unit are occupied by three Co(II) atoms. From the coordination polyhedra of the Co(II) complex, it can be seen that the geometrical configuration of Co1 and Co2 atoms are different from the Co3 atom. The three Co(II) atoms were bridged by the two μ2-acetate groups. Terminal Co3 atom is penta-coordinated by two oxime nitrogen (N3 and N4) atoms, two deprotonated phenoxo-oxygen (O5 and O8) atoms of the (L)4− unit and one oxygen (O11) atom of one μ2-acetate ion. The coordination geometry of Co3 atom is best described as a tetragonal pyramid coordination motif (τ = 0.095) [62], as shown in Figure 3b. Co1 and Co2 atoms are hexa-coordinated with distorted octahedral geometries. The hexa-coordination of terminal Co1 atom is maintained by the N2O2 coordination sphere of the (L)4− unit and one oxygen (O10) atom from the μ2-acetato bridge and another oxygen (O15) atom from the coordinated methanol molecule. While the central Co(II) (Co2) atom possesses three phenoxo-oxygen (O1, O5 and O4) atoms from the (L)4− unit and double μ2-acetato oxygen (O9 and O12) atoms and another oxygen (O13) atom from the coordinated methanol molecule. It is worth noting that the two terminal Co(II) (Co1 and Co3) atoms of the Co(II) complex have different coordination modes and geometries, which isn’t observed in the bis(salamo)-type complexes reported earlier [63].
The intramolecular and intermolecular hydrogen bonds are shown in Figure 4, Figure 5 and Figure 6. The relevant values of the hydrogen bonds are listed in Table 3 [64]. With the help of intermolecular C–H···O, C–H···π and O–H···O interactions [65], adjacent Co(II) complex moleculars can be linked into an infinite 2D layer-like network. Moreover, the Co(II) complex is stabilized further by two C−H···π weak hydrogen bonds [66,67,68,69,70,71,72] (Figure 4). The coordination entities are assembled via π···π stacking interactions (Cg···Cg distances in range 4.627(4)−4.860(4) Å) to the supramolecular chain extending along crystallographic [010] axis [73].

3.4. Fluorescence Properties

The excitation and emission spectra of H4L and its Co(II) complex in mixed solvent (DMF/CH3OH = 1:1, v/v) at room temperature are shown in Figure 7. The ligand shows an intense photoluminescence. The Co(II) complex shows a slightly weak photoluminescence, manifesting that fluorescent property has been influenced by the introduction of the Co(II) ions [74,75,76], which also give rise to the variation in IR and UV-vis spectra of the Co(II) complex.

3.5. Antimicobial Activities

Inhibitory bacterial experiments on commonly-used bacteria, namely E. coli and S. aureus, were performed using the punch method. A small amount (0.1 mL) of a fresh overnight bacterial suspension was added into autoclaved lysogeny broth (LB) agar, then the agar was poured into sterile dishes. The concentration of the test compounds were 0.625, 1.25 and 2.5 mg/mL. 70 μL of samples were added into a burrowed hole measuring 5 mm in diameter with transfer liquid gun when the medium underwent solidification. Ampicillin was used as a reference standard with different concentrations. After 6 h of incubation at 37 °C, the clear zones of inhibition were photographed.
The zones of DMF, complex, H4L and cobalt acetate also had apparent differences in antibacterial activity among the two kinds of bacteria. The complex demonstrated more enhanced antimicrobial activities than the ligand under the same conditions (2.5 mg/mL) and the ligand has a weak biological activity; cobalt acetate also displayed little antimicrobial activity. Moreover, S. aureus exhibits stronger antibacterial activity, whereas E. coli has weaker antibacterial activity (Figure 8a,b). The diameter of inhibition zones of test compounds are illustrated in Figure 8c,d. As shown in Figure 8, this increase in the antibacterial activities of the Co(II) complex was accompanied with an increase in concentration.

3.6. Electrochemistry Studies

The voltammogram of the Co(II) complex is shown in Figure 9. The electrochemical measurement was carried out in a standard three-electrode cell, consisting of a glassy carbon (GC) disc (U = 5 mm) as working electrode, a platinum wire as auxiliary and a Ag/AgNO3 as reference with the scanning rate of 50 mV s−1. There are two pairs of redox peaks during the electrolysis of the Co(II) complex resulting from the redox reaction of Co(III)/Co(II) and Co(II)/Co(I), respectively. The first pair of redox peaks are due to the electron transfer [77] between Co(III) and Co(II) during the electrolysis of the Co(II) complex with potential Epa1 value of −0.769 V, Epc1 value of −0.865 V and current iPa1 = 49.522 μA, iPc1 = −88.807 μA, the average potential E1/2 = −0.817 V, the potential difference between oxidation peak and reduction peak were 0.096 V and current ratio were −0.557. Another pair of redox peaks are because the electron transfer between Co(II) and Co(I) during the electrolysis of the Co(II) complex with potential Epa2 value of −0.865 V, Epc2 value of −1.258 V, current iPa2 = −3.340 μA, iPc1 = −90.056 μA and the average potential E1/2 = −1.062 V, the potential difference between oxidation peak and reduction peak were 0.393 V and current ratio were 0.0371. In short, the experimental data reveal that electrolysis progress of the Co(II) complex is irreversible.

4. Conclusions

In this investigation, the Co(II) complex with a bis(salamo)-type ligand has been synthesized and characterized by IR, UV-vis spectra and X-ray crystallography. The Co(II) complex forms a 2D layer-like network by different intermolecular interactions. Hence, intermolecular non-classical hydrogen-bonding interactions play a key role in the construction of supramolecular frameworks. In addition, the luminance properties reveal that the Co(II) complex has a quality of fluorescent quenching. Furthermore, antimicrobial and electrochemical properties of H4L and its Co(II) complex were also studied.

Acknowledgments

This work was supported by the National Natural Science Foundation of China (21361015, 21761018) and the Outstanding Research Platform (Team) of Lanzhou Jiaotong University, which are gratefully acknowledged.

Author Contributions

Wen-Kui Dong and Jing Hao conceived and designed the experiments; Li-Xiang Zhai performed the experiments; Yang Zhang analyzed the data; Li Wang wrote the paper.

Conflicts of Interest

The authors declare no conflict of interest.

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Scheme 1. Syntheses route to H4L and its complex.
Scheme 1. Syntheses route to H4L and its complex.
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Figure 1. Infrared spectra of H4L and its Co(II) complex.
Figure 1. Infrared spectra of H4L and its Co(II) complex.
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Figure 2. (a) UV-vis spectra of H4L and corresponding Co(II) complex; (b) Absorption spectra of the Co(II) complex in the presence of different concentrations of Co(II) ion (0–3 equiv.) in (DMF/CH3OH = 1:1, v/v).
Figure 2. (a) UV-vis spectra of H4L and corresponding Co(II) complex; (b) Absorption spectra of the Co(II) complex in the presence of different concentrations of Co(II) ion (0–3 equiv.) in (DMF/CH3OH = 1:1, v/v).
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Figure 3. (a) Molecular structure and atom numbering of the Co(II) complex with 30% probability displacement ellipsoids (hydrogen atoms are omitted for clarity); (b) Coordination polyhedra for Co(II) ions.
Figure 3. (a) Molecular structure and atom numbering of the Co(II) complex with 30% probability displacement ellipsoids (hydrogen atoms are omitted for clarity); (b) Coordination polyhedra for Co(II) ions.
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Figure 4. View of intermolecular C–H···π interactions of the Co(II) complex.
Figure 4. View of intermolecular C–H···π interactions of the Co(II) complex.
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Figure 5. View of the intramolecular hydrogen-bonding interactions of the Co(II) complex.
Figure 5. View of the intramolecular hydrogen-bonding interactions of the Co(II) complex.
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Figure 6. (a) View of the 1D chain structure of the Co(II) complex; (b) View of the 2D layer-like network of the Co(II) complex; (c) Packing diagram of the Co(II) complex.
Figure 6. (a) View of the 1D chain structure of the Co(II) complex; (b) View of the 2D layer-like network of the Co(II) complex; (c) Packing diagram of the Co(II) complex.
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Figure 7. (a) The excitation and emission spectra of H4L; (b) The excitation and emission spectra of the Co(II) complex.
Figure 7. (a) The excitation and emission spectra of H4L; (b) The excitation and emission spectra of the Co(II) complex.
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Figure 8. Inhibition of H4L and its Co(II) complex on E. coli and S. aureus. (a,b) represent the inhibition effect of H4L and its Co(II) complex on E. coli and S. aureus, respectively; (c) the diameter of inhibition zones of E. coli in different concentrations; (d) the diameter of inhibition zones of S. aureus in different concentrations)
Figure 8. Inhibition of H4L and its Co(II) complex on E. coli and S. aureus. (a,b) represent the inhibition effect of H4L and its Co(II) complex on E. coli and S. aureus, respectively; (c) the diameter of inhibition zones of E. coli in different concentrations; (d) the diameter of inhibition zones of S. aureus in different concentrations)
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Figure 9. Cyclic voltammogram of the Co(II) complex in DMF at 298 K, c = 5 × 104 M, scan rate = 50 mV s1.
Figure 9. Cyclic voltammogram of the Co(II) complex in DMF at 298 K, c = 5 × 104 M, scan rate = 50 mV s1.
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Table 1. Crystal data and structure refinement parameters for the Co(II) complex.
Table 1. Crystal data and structure refinement parameters for the Co(II) complex.
FormulaC45H46Co3N4O15
Formula weight1059.65
Temperature (K)293(2)
Wavelength (Å)0.71073
Crystal systemMonoclinic
Space groupP 1 n 1
a (Å)8.9831(3)
b (Å)13.4177(4)
c (Å)21.4815(7)
α (°)90.00
β (°)90.561(3)
γ (°)90.00
V (Å3)2589.10(15)
Z, Dc (g cm−3)2, 1.359
μ (mm−1)1.015
θ Range (°)3.336–24.999
F(000)1090
Crystal size (mm)0.14 × 0.11 × 0.04
–10 ≤ h ≤ 10
Index ranges–15 ≤ k ≤ 15
–18 ≤ l ≤ 25
Reflections collected/unique8775/5819 [Rint = 0.0350]
Completeness to θ = 24.99999.7%
GOF0.982
Data/restraints/parameters5819/21/615
Final R1, wR2 indices0.0362/0.0750
R1, wR2 indices (all data)0.0405/0.0773
Largest differences peak and hole (e Å−3)0.412/−0.339
Table 2. Selected bond lengths (Å) and angles (°) of the Co(II) complex.
Table 2. Selected bond lengths (Å) and angles (°) of the Co(II) complex.
BondLengthsBondLengths
Co1–O12.075(4)Co2–O52.107(4)
Co1–O42.029(4)Co2–O92.086(4)
Co1–O102.070(4)Co2–O122.018(4)
Co1–O152.143(4)Co2–O132.142(5)
Co1–N12.068(4)Co3–O52.022(4)
Co1–N22.155(4)Co3–O81.950(4)
Co2–O12.123(4)Co3–O111.997(4)
Co2–O42.066(4)Co3–N32.042(4)
BondAnglesBondAngles
O1–Co1–O483.33(15)O1–Co1–N185.63(16)
O9–Co2–O13175.45(16)O5–Co3–O1194.83(16)
O1–Co1–O1091.26(15)O1–Co1–N2165.68(16)
O12–Co2–O1390.19(18)O5–Co3–N384.87(17)
O1–Co1–O1592.68(15)O4–Co1–O1089.68(15)
O5–Co3–O891.62(15)O5–Co3–N4174.98(16
O4–Co1–O1590.20(15)O10–Co1–O15176.02(16)
O8–Co3–O11109.57(17)O11–Co3–N3123.21(18)
O4–Co1–N1168.95(16)O10–Co1–N191.04(17)
O8–Co3–N3127.22(17)O11–Co3–N490.18(17)
O4–Co1–N282.36(15)O10–Co1–N289.24(16)
O8–Co3–N486.48(17)N3–Co3–N492.58(17)
O15–Co1–N189.84(17)O1–Co2–O481.28(15)
Co1–O1–Co293.70(16)O1–Co2–O5158.08(15)
O15–Co1–N286.80(16)N2–O3–C13110.1(4)
Co1–O1–C1129.6(4)O1–Co2–O989.69(15)
N1–Co1–N2108.68(16)Co1–O4–Co296.82(17)
Co2–O1–C1136.5(4)O1–Co2–O12105.68(16)
Co1–O4–C16128.3(4)Co2–O5–C17111.6(3)
O1–Co2–O1394.82(16)O4–Co2–O12172.71(17)
Co2–O4–C16113.2(3)Co3–O5–C17128.5(3)
O4–Co2–O576.85(15)O4–Co2–O1391.40(16)
Co2–O5–Co3119.50(18)O5–Co2–O988.35(15)
O4–Co2–O988.62(15)O5–Co2–O1296.12(15)
Co3–O8–C29133.6(3)Co2–O12–C40134.1(4)
O5–Co2–O1387.22(15)Co2–O13–C42128.4(4)
Co2–O9–C38129.2(3)Co2–O13–C1A124.7(17)
O9–Co2–O1289.24(17)Co1–O15–C44135.1(4)
Co1–O10–C38128.7(4)Co1–N1–O2124.9(3)
Co3–O11–C40136.1(4)Co1–N1–C11126.7(4)
Co1–N2–O3126.3(3)Co3–N3–O6118.7(3)
Co1–N2–C14126.4(4)Co3–N3–C24126.5(4)
Co1–O15–C44135.5(4)Co1–O15–H15114(2)
Co3–N4–O7123.2(3)Co2–O13–H13116(3)
Co3–N4–C27127.6(4)Co1–O15–H15115(2)
Table 3. Hydrogen bonding interactions (Å, °) of the complex.
Table 3. Hydrogen bonding interactions (Å, °) of the complex.
D–XX···AD···AD–X···ASymmetry Codes
C6–H6–O80.93002.59003.382(9)144.00(x, 1 + y, z)
C12–H12A–O100.97002.45003.292(7)145.00
C12–H12A–N20.97002.47002.871(7)105.00
C12–H12B–O110.97002.47003.400(8)160.00(1/2 + x, 1 − y, 1/2 + z)
C13–H13A–N10.97002.55002.919(7)102.00
C22–H22–O70.93002.53003.213(8)130.00(1/2 + x, −y, 1/2 + z)
C26–H26B–O110.97002.42003.262(8)145.00
O13–H13–O80.87(2)1.94(3)2.723(6)149(5)
O14–H14A–O90.82001.91002.715(6)168.00
O15–H15–O140.86(3)1.80(3)2.637(7)164(3)(1 + x, y, z)
C13–H13B–Cg1 2.87
C13–H13B–Cg2 2.99
Symmetry codes: Cg1 and Cg2 for the Co(II) complex are the centroids of Co3, O8, N4, C27–C29 and C28–C32, C37 atoms, respectively.
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