Synthesis, Crystal Structure, Magnetic Property and Photo-induced Coloration of a One-dimensional Chain Complex

A novel photoactive complex was constructed from two non-photoactive ligands and cobalt (II) ions. Upon ultra violet (UV) irradiation (365 nm), the color of complex 1 changes from orange to violet. The ESR spectrum indicates that the photoactive phenomenon of complex 1 originates from an intermolecular energy transfer between the H 5 DDCPBA ligand and phenanthroline ligand. This photoactive complex shows high thermal stability according to the investigation of thermogravimetric analyses. In addition, the temperature dependence of magnetic susceptibilities for the orange complex 1 was also investigated systematically.


Introduction
In the past two decades, metal organic coordination polymers, as a class of complexes constructed by metal ions and organic bridging ligands through coordination bonds, have attracted great research interest due to their intriguing structural topologies and potential applications in catalysis, separation, electronics, luminescence, drug delivery and gas storage, etc. [1][2][3][4][5][6][7][8][9][10][11].In all kinds of applications, photo properties of metal organic coordination polymers have attracted increasing attention, especially for their development of photoresponsive materials based on metal-ligand complexes, due to their value and importance to the development of advanced molecular electronic and photonic devices.For example, Fu and coworkers have reported a series of new types of photochromic molecular systems based on the viologen ligand [12][13][14].Champness's group has reported a metal-bearing coordination network synthesized from Re(2,2 -bipyridine-5,5 -dicarboxylate)(CO) 3 Cl bridging ligands and Cu(II) nodes, which undergoes an irreversible photoinduced charge transfer process [15].Compared to the traditional pure organic and inorganic molecular systems, the photoresponsive materials based on metal-ligand complexes can be perturbed and tuned by the connection of different metal centers and photochromic ligands.It is worth pointing out that although quite a number of classes of metal complexes with different photochromic ligands have been developed in recent years, the photoresponsive frameworks constructed from non-photochromic ligands are still rare to the best of our knowledge.Only Fu reported a photoactive Zn(II) complex using two non-photoactive components [16].
In the present paper, one novel photoactive complex was constructed from two non-photoactive ligands and cobalt (II) ions, [Co(HDDCPBA) 0.5 (Phen)(H 2 O) 2 ]•2H 2 O [1, H 5 DDCPBA = 3,5-di(3 5dicarboxyl-phenyl) benzoic acid, Phen = 1,10-phenanthroline].Upon ultra violet (UV) irradiation A single crystal of the complex 1 with appropriate dimensions was chosen under an optical microscope and quickly coated with high vacuum grease (Dow Corning Corporation) before being mounted on a glass fiber for data collection.Data were collected on a Bruker Apex II Image Plate single-crystal diffractometer with a graphite-monochromated Cu Kα radiation source (λ = 1.54184Å) operating at 50 kV and 30 mA for complex 1.All absorption corrections were applied using the multi-scan program SADABS [17].In all cases, the highest possible space group was chosen.The structure was solved by direct methods using SHELXS-97 [18] and refined on F 2 by full-matrix least-squares procedures with SHELXL-97 [19].Atoms were located from iterative examination of difference F-maps following least squares refinements of the earlier models.Hydrogen atoms were placed in calculated positions and included as riding atoms with isotropic displacement parameters 1.2 times Ueq of the attached C atoms.All structures were examined using the Addsym subroutine of PLATON [20] to ensure that no additional symmetry could be applied to the models.The crystallographic details of complex 1 are summarized in Table 1.Selected bond lengths and angles for complex 1 are collected in Table 2.

Descriptions of the Crystal Structures
Complex 1 was prepared by a hydrothermal reaction of H 5 DDCPBA, Co(NO 3 ) 2 •6H 2 O and Phen in mixed solvents of DMF/DMA/H 2 O at 60 • C for two weeks and characterized by single-crystal X-ray crystallography, powder X-ray diffraction (PXRD), thermogravimetric analysis (TGA), and elemental analysis.Single-crystal X-ray analysis reveals that the photoresponsive molecular system is constructed by the connections of DDCPBA and Phen mixed ligands with a cobalt ion as node (Figure 1A).The Co( II ) center has a distorted {CoN 2 O 4 } octahedral coordination sphere with two nitrogen atoms from one phen ligand, two oxygen atoms from two different DDCPBA ligands and two oxygen atoms from two different coordinated water molecules.The Co-N distances are 2.118(3) Å and 2.141(3) Å, the distances of Co-Ow are 2.103(3) Å and 2.127(3) Å, and Co-O distances are 2.066(2) Å and 2.138(2), respectively.It is worth pointing out that the coordination arrangements make the distances between the oxygen atoms of the carboxyl groups and the N atom of the phen ligand as follows: 3.0261(37), 3.0615(39), 3.0428(37) and 4.1927(37) Å, respectively.According to the previous reports [13,21], the distance (smaller than 3.7 Å) satisfies the requirements for an inter-ligand charge transfer.The carboxylate group in complex 1 adopts µ 1 -η 1 -η 0 bridging modes to link two Co(II) ions to form a 16-membered-ring (Figure 1B), and then the 16-membered-rings were connected to each other to furnish a 1D chain by the DDCPBA ligand (Figure 1C).inter-ligand charge transfer.The carboxylate group in complex 1 adopts μ1-η 1 -η 0 bridging modes to link two Co(II) ions to form a 16-membered-ring (Figure 1B), and then the 16-membered-rings were connected to each other to furnish a 1D chain by the DDCPBA ligand (Figure 1C).

The Diffuse-Reflectance Spectra and ESR Spectra
The diffuse-reflectance spectra of the initial state and radical form of the complex 1 are shown in Figure 2. As shown in Figure 2, the diffuse-reflectance spectra of the orange crystal show absorption bands at 473 nm and 507 nm, which can be ascribed to the π-π* and n-π* transitions of the aromatic rings.However, upon UV irradiation (365 nm), the color of complex 1 changes to violet from orange, with new absorption bands appearing at about 572 nm and its intensity increases with extending the irradiation time.After about 1 hour, the diffuse-reflectance spectra of complex 1 do not change any more.When complex 1 changed from orange to violet under UV irradiation, whether it be exposed to light irradiation or heating, the color of the sample will not change back.ESR measurement indicates that the coloration process is due to the generation of radicals (g = 2.003) (Figure 3), which is close to previous reports for free organic radicals [22].

The Diffuse-Reflectance Spectra and ESR Spectra
The diffuse-reflectance spectra of the initial state and radical form of the complex 1 are shown in Figure 2. As shown in Figure 2, the diffuse-reflectance spectra of the orange crystal show absorption bands at 473 nm and 507 nm, which can be ascribed to the π-π* and n-π* transitions of the aromatic rings.However, upon UV irradiation (365 nm), the color of complex 1 changes to violet from orange, with new absorption bands appearing at about 572 nm and its intensity increases with extending the irradiation time.After about 1 h, the diffuse-reflectance spectra of complex 1 do not change any more.When complex 1 changed from orange to violet under UV irradiation, whether it be exposed to light irradiation or heating, the color of the sample will not change back.ESR measurement indicates that the coloration process is due to the generation of radicals (g = 2.003) (Figure 3), which is close to previous reports for free organic radicals [22].
Crystals 2017, 7, 77 4 of 8 inter-ligand charge transfer.The carboxylate group in complex 1 adopts μ1-η 1 -η 0 bridging modes to link two Co(II) ions to form a 16-membered-ring (Figure 1B), and then the 16-membered-rings were connected to each other to furnish a 1D chain by the DDCPBA ligand (Figure 1C).

The Diffuse-Reflectance Spectra and ESR Spectra
The diffuse-reflectance spectra of the initial state and radical form of the complex 1 are shown in Figure 2. As shown in Figure 2, the diffuse-reflectance spectra of the orange crystal show absorption bands at 473 nm and 507 nm, which can be ascribed to the π-π* and n-π* transitions of the aromatic rings.However, upon UV irradiation (365 nm), the color of complex 1 changes to violet from orange, with new absorption bands appearing at about 572 nm and its intensity increases with extending the irradiation time.After about 1 hour, the diffuse-reflectance spectra of complex 1 do not change any more.When complex 1 changed from orange to violet under UV irradiation, whether it be exposed to light irradiation or heating, the color of the sample will not change back.ESR measurement indicates that the coloration process is due to the generation of radicals (g = 2.003) (Figure 3), which is close to previous reports for free organic radicals [22].

X-Ray Powder Diffraction Analysis
The phase purity of pink complex 1 is sustained by the powder X-ray diffraction pattern, Figure 4. Most of the peak positions of simulated and experimental patterns are in good agreement with each other; the differences in intensity may be due to the preferred orientation of the powder samples.

IR Spectra
The FT-IR spectrum of pink compound 1 was also investigated, Figure 5.The sharp bands at about 1557 cm −1 and 1423 cm −1 are attributed to asymmetric and symmetric stretching vibrations of the carboxylic group, respectively [22,23].

Thermogravimetric Analyses
To assess the thermal stability and its structural variation with the temperature, thermogravimetric analysis (TGA) of orange complex 1 was performed under a N2 atmosphere, Figure 6.Complex 1 has two identifiable weight loss steps: The first one is consistent with the removal of two uncoordinated and two coordinated water molecules (obsd 14.53%, calcd 14.11%), which

X-Ray Powder Diffraction Analysis
The phase purity of pink complex 1 is sustained by the powder X-ray diffraction pattern, Figure 4. Most of the peak positions of simulated and experimental patterns are in good agreement with each other; the differences in intensity may be due to the preferred orientation of the powder samples.

X-Ray Powder Diffraction Analysis
The phase purity of pink complex 1 is sustained by the powder X-ray diffraction pattern, Figure 4. Most of the peak positions of simulated and experimental patterns are in good agreement with each other; the differences in intensity may be due to the preferred orientation of the powder samples.

IR Spectra
The FT-IR spectrum of pink compound 1 was also investigated, Figure 5.The sharp bands at about 1557 cm −1 and 1423 cm −1 are attributed to asymmetric and symmetric stretching vibrations of the carboxylic group, respectively [22,23].

Thermogravimetric Analyses
To assess the thermal stability and its structural variation with the temperature, thermogravimetric analysis (TGA) of orange complex 1 was performed under a N2 atmosphere, Figure 6.Complex 1 has two identifiable weight loss steps: The first one is consistent with the removal of two uncoordinated and two coordinated water molecules (obsd 14.53%, calcd 14.11%), which

IR Spectra
The FT-IR spectrum of pink compound 1 was also investigated, Figure 5.The sharp bands at about 1557 cm −1 and 1423 cm −1 are attributed to asymmetric and symmetric stretching vibrations of the carboxylic group, respectively [22,23].

X-Ray Powder Diffraction Analysis
The phase purity of pink complex 1 is sustained by the powder X-ray diffraction pattern, Figure 4. Most of the peak positions of simulated and experimental patterns are in good agreement with each other; the differences in intensity may be due to the preferred orientation of the powder samples.

IR Spectra
The FT-IR spectrum of pink compound 1 was also investigated, Figure 5.The sharp bands at about 1557 cm −1 and 1423 cm −1 are attributed to asymmetric and symmetric stretching vibrations of the carboxylic group, respectively [22,23].

Thermogravimetric Analyses
To assess the thermal stability and its structural variation with the temperature, thermogravimetric analysis (TGA) of orange complex 1 was performed under a N2 atmosphere, Figure 6.Complex 1 has two identifiable weight loss steps: The first one is consistent with the removal of two uncoordinated and two coordinated water molecules (obsd 14.53%, calcd 14.11%), which

Thermogravimetric Analyses
To assess the thermal stability and its structural variation with the temperature, thermogravimetric analysis (TGA) of orange complex 1 was performed under a N 2 atmosphere, Figure 6.Complex 1 has two identifiable weight loss steps: The first one is consistent with the removal of two uncoordinated and two coordinated water molecules (obsd 14.53%, calcd 14.11%), which appears between 90 and 172 • C. The second one is attributed to the collapse of the framework, which is in the range of 345 to 445 • C. It is worth pointing out that the present complex 1 has better thermal stability than that of the pure organic photoresponsive materials, suggesting an effective way to develop photoresponsive materials based on metal-ligand complexes [24].
Crystals 2017, 7, 77 6 of 8 appears between 90 and 172 °C.The second one is attributed to the collapse of the framework, which is in the range of 345 to 445 °C.It is worth pointing out that the present complex 1 has better thermal stability than that of the pure organic photoresponsive materials, suggesting an effective way to develop photoresponsive materials based on metal-ligand complexes [24].

Magnetic Properties
The temperature dependence of magnetic susceptibilities for the orange complex 1 measured in the range of 2-300 K under the external magnetic field of 1000 Oe is shown in Figure 7.The χmT value at room temperature is 2.68 emu•K•mol −1 , which is higher than the spin only value of 1.875 emu•K•mol −1 for the isolated high spin Co(II) (S = 3/2); this can be ascribed to the effects of the Spin-orbit coupling of the octahedral Co(II) ion [25] with the temperature decreasing; the χmT value remains almost constant from 300 to about 100 K.After this, the χmT value starts to decrease rapidly and reaches its lowest peak with the value of 1.55 emu•K•mol −1 at 2 K.The magnetic susceptibility for the orange complex 1 conforms well to the Curie-Weiss law in a range of 2-300 K and gives the negative Weiss constant θ = −7.21K and the Curie constant C = 2.78 emu•K•mol −1 .
The field-dependent magnetizations measured up to 70 kOe at 2 K for complex 1, as shown in Figure 8.The magnetization increases with a relatively fast speed with increasing field until 20 kOe, then increases smoothly up to about 2.6 M/emμ•g −1 until 70 kOe.This data is only slightly lower than the saturated value of 3.0 M/emμ•g −1 for an isolated Co(II) ion based on g = 2.0, indicating further that there no obvious magnetic coupling exists between the Co(II) ions due to the long distance separated by the flexible organic ligands.

Magnetic Properties
The temperature dependence of magnetic susceptibilities for the orange complex 1 measured in the range of 2-300 K under the external magnetic field of 1000 Oe is shown in Figure 7.The χmT value at room temperature is 2.68 emu•K•mol −1 , which is higher than the spin only value of 1.875 emu•K•mol −1 for the isolated high spin Co(II) (S = 3/2); this can be ascribed to the effects of the Spin-orbit coupling of the octahedral Co(II) ion [25] with the temperature decreasing; the χmT value remains almost constant from 300 to about 100 K.After this, the χmT value starts to decrease rapidly and reaches its lowest peak with the value of 1.55 emu•K•mol −1 at 2 K.The magnetic susceptibility for the orange complex 1 conforms well to the Curie-Weiss law in a range of 2-300 K and gives the negative Weiss constant θ = −7.21K and the Curie constant C = 2.78 emu•K•mol −1 .
appears between 90 and 172 °C.The second one is attributed to the collapse of the framework, which is in the range of 345 to 445 °C.It is worth pointing out that the present complex 1 has better thermal stability than that of the pure organic photoresponsive materials, suggesting an effective way to develop photoresponsive materials based on metal-ligand complexes [24].

Magnetic Properties
The temperature dependence of magnetic susceptibilities for the orange complex 1 measured in the range of 2-300 K under the external magnetic field of 1000 Oe is shown in Figure 7.The χmT value at room temperature is 2.68 emu•K•mol −1 , which is higher than the spin only value of 1.875 emu•K•mol −1 for the isolated high spin Co(II) (S = 3/2); this can be ascribed to the effects of the Spin-orbit coupling of the octahedral Co(II) ion [25] with the temperature decreasing; the χmT value remains almost constant from 300 to about 100 K.After this, the χmT value starts to decrease rapidly and reaches its lowest peak with the value of 1.55 emu•K•mol −1 at 2 K.The magnetic susceptibility for the orange complex 1 conforms well to the Curie-Weiss law in a range of 2-300 K and gives the negative Weiss constant θ = −7.21K and the Curie constant C = 2.78 emu•K•mol −1 .
The field-dependent magnetizations measured up to 70 kOe at 2 K for complex 1, as shown in Figure 8.The magnetization increases with a relatively fast speed with increasing field until 20 kOe, then increases smoothly up to about 2.6 M/emμ•g −1 until 70 kOe.This data is only slightly lower than the saturated value of 3.0 M/emμ•g −1 for an isolated Co(II) ion based on g = 2.0, indicating further that there no obvious magnetic coupling exists between the Co(II) ions due to the long distance separated by the flexible organic ligands.The field-dependent magnetizations measured up to 70 kOe at 2 K for complex 1, as shown in Figure 8.The magnetization increases with a relatively fast speed with increasing field until 20 kOe, then increases smoothly up to about 2.6 M/emµ•g −1 until 70 kOe.This data is only slightly lower than the saturated value of 3.0 M/emµ•g −1 for an isolated Co(II) ion based on g = 2.0, indicating further that there no obvious magnetic coupling exists between the Co(II) ions due to the long distance separated by the flexible organic ligands.

Conclusions
In conclusion, a novel photoactive system was constructed from two non-photoactive ligands and cobalt (II) ions.Upon UV irradiation (365 nm), orange crystal of 1 becomes violet.The ESR spectrum indicates that the photoactive phenomenon of complex 1 originates from an intermolecular energy transfer between the DDCPBA ligand and phenanthroline ligand.

Conclusions
In conclusion, a novel photoactive system was constructed from two non-photoactive ligands and cobalt (II) ions.Upon UV irradiation (365 nm), orange crystal of 1 becomes violet.The ESR spectrum indicates that the photoactive phenomenon of complex 1 originates from an intermolecular energy transfer between the DDCPBA ligand and phenanthroline ligand.

Figure 3 .
Figure 3.The ESR spectrum of the violet crystal 1.

Figure 4 .
Figure 4.The powder XRD patterns and the simulated one from the single-crystal diffraction data for the complex 1.

Figure 3 .
Figure 3.The ESR spectrum of the violet crystal 1.

Figure 3 .
Figure 3.The ESR spectrum of the violet crystal 1.

Figure 4 .
Figure 4.The powder XRD patterns and the simulated one from the single-crystal diffraction data for the complex 1.

Figure 4 .
Figure 4.The powder XRD patterns and the simulated one from the single-crystal diffraction data for the complex 1.

Figure 3 .
Figure 3.The ESR spectrum of the violet crystal 1.

Figure 4 .
Figure 4.The powder XRD patterns and the simulated one from the single-crystal diffraction data for the complex 1.

Figure 7 .
Figure 7. Temperature dependence of χmT for the complex 1.The blue solid lines represent the best fitting in the temperature range of 2-300 K.

Figure 7 .
Figure 7. Temperature dependence of χmT for the complex 1.The blue solid lines represent the best fitting in the temperature range of 2-300 K.

Figure 7 .
Figure 7. Temperature dependence of χ m T for the complex 1.The blue solid lines represent the best fitting in the temperature range of 2-300 K.

Figure 8 .
Figure 8. Plot of magnetization for the complex 1 at 2 K.

Figure 8 .
Figure 8. Plot of magnetization for the complex 1 at 2 K.

Table 1 .
Crystal data for complex 1.