Advances in Materials Science and Engineering

Advances in Materials Science and Engineering / 2017 / Article

Research Article | Open Access

Volume 2017 |Article ID 3237247 |

Il-Ju Ko, Hyun-Chang Oh, Yong-Jun Cha, Chae Hyeok Han, Eun-Young Choi, "Ionothermal Synthesis of a Novel 3D Cobalt Coordination Polymer with a Uniquely Reported Framework: [BMI]2[Co2(BTC)2(H2O)2]", Advances in Materials Science and Engineering, vol. 2017, Article ID 3237247, 6 pages, 2017.

Ionothermal Synthesis of a Novel 3D Cobalt Coordination Polymer with a Uniquely Reported Framework: [BMI]2[Co2(BTC)2(H2O)2]

Academic Editor: Peter Majewski
Received06 Apr 2017
Revised17 Jul 2017
Accepted26 Jul 2017
Published28 Aug 2017


The framework of [RMI]2[Co2(BTC)2(H2O)2] (RMI = 1-alkyl-3-methylimidazolium, alkyl; ethyl (EMI); propyl (PMI); butyl (BMI)), which has uniquely occurred in ionothermal reactions of metal salts and H3BTC (1,3,5-benzenetricarboxylic acid), an organic ligand, reappeared in this work. Ionothermal reaction of cobalt acetate and H3BTC with [BMI]Br ionic liquid as the reaction medium yielded the novel coordination polymer [BMI]2[Co2(BTC)2(H2O)2] (compound B2). Similar ionothermal reactions with different [EMI]Br and [PMI]Br as the reaction media have been previously reported to produce [EMI]2[Co3(BTC)2(OAc)2] (compound A1) and [PMI]2[Co2(BTC)2(H2O)2] (compound B1), respectively. In contrast with the trinuclear secondary building unit of A1, the framework structure of B1 and B2 consists of dinuclear secondary building units in common, but with subtle distinction posed by the different size of the incorporated cations. These structural differences amidst the frameworks showed interesting aspects, including guest and void volume, and were used to explain the chemical trend observed in the system. Moreover, the physicochemical properties of the newly synthesized compound have been briefly discussed.

1. Introduction

The rising demands for new materials with befitted properties for applications in numerous fields of science and industry [13] have led to development and advancements of novel synthesis methods [410]. Ionothermal synthesis, where ionic liquids are used both as solvents and templates [11], has been recently deployed for preparation of novel structures [12, 13] amidst a great attention attributed to its unique and pragmatic physicochemical properties [11], namely, those discussed hereafter and many more [1416]: high thermal stability [17], negligible vapor pressure [18], environmentally friendliness [19], and, most interestingly, its ability to finely tune the reaction environment by changing the cation and anion of the ionic liquid and ultimately enabling systematic approach to the final product [20, 21]. Despite such attractiveness of ionothermal synthesis and its expandability that has already been demonstrated with novel structures of various classes including zeolites [12, 13], zeotype frameworks [12, 2224], and metal-organic frameworks or MOFs [20, 21, 25], the methodology has not been extensively employed [21], leaving a vast number of different reaction conditions for future research. The unique advantages of ionothermal synthesis may be fully practiced only when enough experiments have been carried out with various circumstances to produce a sizable number of frameworks.

We herein report a novel 3D cobalt coordination polymer [BMI]2[Co2(BTC)2(H2O)2] (compound B2), which has been ionothermally prepared with [BMI]Br as the solvent. Its framework is very rare in literature, previously being only uniquely exemplified by [PMI]2[Co2(BTC)2(H2O)2] (compound B1), a polymer obtained from a reaction analogous to ours, but with [PMI]Br as the solvent [26]. On the contrary, another analogous reaction with [EMI]Br as the solvent yielded a polymer with a notably different framework, [EMI]2[Co3(BTC)2(OAc)2] (compound A1) [27]. Moreover, attempts have been made to synthesize novel polymers with [PEMI]Br and [HMI]Br and acquired pink amorphous solids. In order to provide explanations to the trend introduced above, the framework of the novel compound [BMI]2[Co2(BTC)2(H2O)2] (compound B2) will be thenceforth examined from various aspects in relation to that of [EMI]2[Co3(BTC)2(OAc)2] (compound A1) and [PMI]2[Co2(BTC)2(H2O)2] (compound B1).

2. Experimental

2.1. Crystal Preparation

For the preparation of [BMI]2[Co2(BTC)2(H2O)2] (compound B2), Co(OAc)2·4H2O (3.0 mmol, 0.7472 g) and H3BTC (2.0 mmol, 0.4203 g) were placed altogether in a 23 mL Teflon-lined stainless-steel autoclave with [BMI]Br (20 mmol, 4.3824 g). The mixture was gradually heated in a furnace for 3 hours to reach the reaction temperature of 150°C. The temperature was held still for 3 days and slowly cooled to room temperature for 5 hours. The obtained deep blue crystals (Figure 1(a)) were filtered, washed with ethanol, and naturally dried for purification. All chemicals including ionic liquids (ILs) were commercially purchased from Chem. Tech. Research Incorporation (C-TRI) and Sigma-Aldrich Chemical Company and used without further purification.

2.2. Crystal Structure Analysis

Crystallographic data of obtained crystals were collected at −100°C on Bruker Smart Breeze diffractometer in different locations including Pusan National University. Summary of crystallographic data for compound B2 are given in Table 1 and further details of the crystal structure have been deposited at the Cambridge Crystallographic Data Center as supplementary publication (CCDC-1525180). For crystallographic comparison, summarized data for compound A1 and compound B1 are also given in Table 1.


Empirical formulaC22H12Co3O16C16H18CoN2O7C17H20CoN2O7
Space groupPbcaP2(1)/nP2(1)/n
Crystal systemOrthorhombicMonoclinicMonoclinic
α (deg)90.0090.0090.00
β (deg)90.0095.276(14)95.3550(10)
γ (deg)90.0090.0090.00
Cell volume3797.9(2)1850.4061840.52(15)
Reference[27][26]This work

The reference in the article.

Powder X-ray diffraction (PXRD) data were recorded on a Rigaku Miniflex 600 diffractometer at 40 kV, 15 mA for Cu-Kα radiation (λ = 1.5406 Å) with a scan speed of 5°/min, and a step size of 0.01° in 2θ.

3. Result and Discussion

The framework of compound B2 imputes its understructure to the dinuclear unit built by connecting two cobalt atoms with six BTC3− ligands as illustrated in Figure 1(b). The fundamental asymmetric unit of compound B2 contains one cobalt (II) atom, one BTC3− ligand, one [BMI] cation, and a water molecule (Table 1). Each cobalt (II) atom is five-coordinated with four oxygen atoms from carboxylate groups of BTC3− ligands and one from a water molecule in a distorted trigonal bipyramid geometry. BTC3− ligands exhibit µ4 coordination modes: two of the carboxylates exhibit monodentate coordination fashion and the remaining bidentate coordination fashion. Two symmetric cobalt (II) atoms are linked by two carboxylate groups exhibiting bidentate coordination mode, each from different BTC3− ligands and form the [Co2(µ2-COO)2] core as in compound B1 [26] (Figure 1(b)). Nevertheless, the distance between two neighboring cobalt (II) atoms is 3.53 Å, which is slightly shorter than that of compound B1, 3.56 Å [26], but such an arrangement with a long distance of 3.53 Å still eradicates the possibility of direct interaction between them. The range of Co-O distance was measured to span from 1.9830(13) Å to 2.1314(14) Å (see Table 2), exhibiting the similar range of compound B1 [26]. The 3D framework of compound B2, given by connecting cobalt (II) core with six BTC3− ligands, has rhombic channels parallel to the crystallographic axe (Figure 2). [BMI] cations of ionic liquids residing in the open channels as shown in Figure 2 behave as charge balancing species for the anionic framework.


Symmetry transformations: #1: , , ; #2: , , ; #3: , , .

The difference between type A framework, a trinuclear system, and type B frameworks, dinuclear system, becomes evident at their secondary building units, visually depicted at Figure S1 in Supplementary Material available online at, along with the subtleness in distinction between compound B1 and compound B2 [26, 27]. However, the [RMI] molecules were present as guests in all frameworks, suggesting a role played by the alkyl chains of differing lengths in determination of framework types.

To further account for the effect of guest molecules, Connolly surfaces and volumes have been calculated for their in situ conformations and for the cation pairs in the form of which the guests occur [28] (Figure 3). Note that the [EMI] cations are so severely disordered in compound A1 that reliable conformation data could not be obtained and therefore, data for [EMI] have been imported from isoreticular correspondent prepared with nickel in place of cobalt (CCDC number 719778) for better depiction of the trend. It has been discovered that the butyl chain of [BMI] molecule is considerably bent, making the volume of the molecule only slightly larger than [PMI] molecule compared to the increase in volume from [EMI] to [PMI]; the distance from the first carbon of the alkyl chain to the final carbon was 2.918 Å in compound B2, which is only slightly larger than 2.567 Å of compound B1. This indicates that the type B framework is stable for the cobalt-BTC system strong enough to cause the severe bending in the butyl chain of the guest molecule whilst the increase of guest volume from [EMI] to [PMI] posed the boundary between framework A and B. Nevertheless, the scarcity of the framework in systems of other metal elements suggests such a favor is limited specifically to the cobalt system (see Table S1).

It is apparent that increasing guest volume will exert a pressure on the framework to the direction of expanding its free volume. Occupied volume and free volume have been calculated for the three compounds and yielded a result corresponding to the expectation, but only partially (Figure S2). The free volume ratio was determined to be nearly the same for compounds B1 and B2, suggesting the rigidness of the framework with respect to the change of free volume ratio. This result accords with the bent conformation of the [BMI] cation in compound B2 and the failure to produce crystalline frameworks in reactions using [PEMI]Br and [HMI] in place of [BMI], respectively; this framework remains invariant over a range of synthesizing environment and such invariance may at minimum be partially attributed to the absence of any other framework that could rise from this range of synthesizing environment. Figure 4 summarizes the data regarding the occupied volume, the free volume, the guest volume, and the volume of the cation pairs that the guests found in structure.

Lastly, physicochemical properties of compound B2 have been explored from a variety of scopes including those that have not been practiced for compound B1 upon its synthesis. Several analyses were additionally performed to confirm the incorporation of ligands and metals. Infrared absorption spectroscopy has been practiced for the crystals and compared with H3BTC to provide additional proof for the incorporation of BTC3− ligands in the framework (Figure S3). The carboxylic C=O peak in Figure S3 is shifted from 1691 cm−1 of H3BTC to 1616 cm−1 of compound B2, which supports the coordination of H3BTC ligands to the cobalt (II) atoms. Powder X-ray diffraction pattern of the remnants of the crystals after thermogravimetric analysis (TGA) exactly matches that of cobalt oxide (Co3O4), proving that the incorporated metal is indeed cobalt (Figure S4). Moreover, the crystals of compound B2 have been applied to various solvents including water, DMF, ethanol, and acetone, to further test its properties (Figure S5). The crystals remained stable under all solvents, except for water, in which a framework change was observed along with immediate color change to pink (Figure S6). The SEM image confirmed the complete change in framework structure of compound B2 upon treatment with water (Figure S7). Additionally, powder X-ray diffraction pattern of the crystals after application of water has been compared with that of the prior state, which was discovered to be considerably different and strongly supported the change of framework in compound B2 under water (Figure S8). To trace the direct cause of the framework change, energy dispersive spectroscopy has been performed for the crystals treated with water and the nitrogen atoms was revealed to be absent after addition of water. Since the nitrogen atoms are only included in the [BMI] cations, the framework change has been suggested to be accompanied by the evacuation of [BMI] guest molecules (Figure S9). Conceding further research taken, presumably along with the relative stability observed under other common solvents, this phenomenon, the evacuation of cation molecules out of the framework structure, may open a possibility for the ionothermal methodology in preparing coordination polymers with a cation exchange property. Lastly, thermogravimetric analysis (TGA) of compound B2 has confirmed the framework stable up to 352°C as shown in Figure S4(a), raising the potential of the compound for industrial applications.

4. Conclusions

We have reported a novel coordination polymer [BMI]2[Co2(BTC)2(H2O)2] (compound B2) and compared it within the system of polymers arising from ionothermal reaction of Co(OAc)2 and BTC mediated by the ionic solvent [RMI]Br. Resident inside the cavities, the cations have been expected to directly relate their sizes to the volume of the cavities. However, the accuracy of this assumption was curtailed by structural analysis of compound B2 along with the discovery of significant bending in the alkyl chain of the BMI cations. Moreover, thermal stability and removability of the incorporated cations exhibited by compound B2 further open the feasibility of implementing the ionothermal methodology for production of new materials with demanded properties.

Conflicts of Interest

There are no conflicts of interest regarding the publication of this paper.


This work has been supported by the Korea Science Academy of KAIST from the Ministry of Science, ICT and Future Planning. The authors also acknowledge Busan Metropolitan Office of Education for financial support.

Supplementary Materials

Supporting Information: Information is available regarding powder X-ray diffraction patterns, Energy Dispersive Spectroscopy data, photographs of crystals, and TGA thermodiagrams.

  1. Supplementary Material


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Copyright © 2017 Il-Ju Ko et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

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