Synthesis of an Adduct-Type Organic Ionic Crystal with Solid-State Ionic Conductivity from A Thiocyanate-Based Ionic Liquid and B(C₆F₅)₃

Abstract

We synthesized the novel adduct-type organic ionic crystal [C3mim][SCN·B(C₆F₅)₃] (1) by the reaction of 1–methyl–3–propylimidazolium thiocyanate ([C3mim][SCN]), which is a room temperature ionic liquid, and B(C₆F₅)₃, a bulky Lewis acid. The formation of a coordinative B–N bond between the SCN anion and the B(C₆F₅)₃ in 1 was revealed by single-crystal X-ray diffractometry. We showed that 1 displays ionic conductivity in the crystalline state and that doping 1 with sodium thiocyanate and B(C₆F₅)₃ results in a dramatic increase in ionic conductivity compared to that of 1.

1. Introduction

Ionic liquid crystals (ILCs) [1,2,3] and organic ionic plastic crystals (OIPCs) [4,5,6] have attracted considerable attention as matrix materials for the development of innovative solid electrolytes. Both liquid crystals and plastic crystals are intermediate phases that lie between crystals and liquids; hence, ILCs and OIPCs undergo phase transitions to organic ionic crystals (OICs), as low-temperature phases, upon cooling in a similar manner to ionic liquids (ILs). Interestingly, studies into solid-state ion diffusion through OICs are quite limited despite the applications of ILCs and OIPCs as electrolyte materials being vigorously studied.

On the other hand, we have reported ionic conduction through lithium-based OICs composed of lithium salts with organic anions and small molecules [7,8,9,10,11]. We found the formation of an ordered arrangement of lithium ions has been reported to be a key factor for lithium–ion diffusion in the crystal lattices of these lithium-based OICs. These results suggest that OICs composed of similar component units to ILs also have potential as matrix materials. Furthermore, such OICs are expected to exhibit favorable solid–electrolyte features, namely flame retardancy, non-volatility, and a wide potential window, such as those shown by ILs.

In order to synthesize such ion-conductive OICs, anions that are steric bulky compared to the cation are desirable. For example, we reported the phase-transition behavior of OIPCs composed of tetraalkylammonium or pyrrolidinium cations and the cyclic perfluorosulfonylamide anion, [N(SO₂CF₂)₂CF₂]⁻ (CPFSA) [12,13]. In this study, we showed that CPFSA-based OIPCs exhibit considerably high melting points compared to those of the analogous OIPCs that contain bis(trifluoromethanesulfonyl)amide ([N(SO₂CF₃)₂]⁻, TFSA) because of the bulkiness of CPFSA. Moreover, the use of a large counter anion in an OIC is also expected to provide void structures that enhance ion diffusion in the crystal lattice.

In order to synthesize such ion-conductive OICs, anions that are steric bulky compared to the cation are desirable. For example, we reported the phase-transition behavior of OIPCs composed of tetraalkylammonium or pyrrolidinium cations and the cyclic perfluorosulfonylamide anion, [N(SO₂CF₂)₂CF₂]⁻ (CPFSA) [12,13]. In this study, we showed that CPFSA-based OIPCs exhibit considerably high melting points compared to those of the analogous OIPCs that contain bis(trifluoromethanesulfonyl)amide ([N(SO₂CF₃)₂]⁻, TFSA) because of the bulkiness of CPFSA. Moreover, the use of a large counter anion in an OIC is also expected to provide void structures that enhance ion diffusion in the crystal lattice.

One of the most useful techniques for increasing the size of an anion involves the formation of coordinative interactions between the coordinating anion and a bulky Lewis acid [14,15,16]. Previously, such adduct-type anions were prepared by the addition of the bulky B(C₆F₅)₃ Lewis acid to anions containing cyano groups [16]. With this in mind, we synthesized ion conductive OICs using the 1–methyl–3–propylimidazolium thiocyanate ([C3mim][SCN]) IL and B(C₆F₅)₃ (Figure 1). Herein, we report the synthesis and crystal structure of [C3mim][SCN·B(C₆F₅)₃] (1), a novel adduct-type OIC that exhibits ionic conductivity in the crystalline state. We also fabricated a solid-state ion-conductive OIC-based solid electrolyte by doping 1 with NaSCN and B(C₆F₅)₃.

2. Materials and Methods

All experiments were carried out under an argon atmosphere using Schlenk techniques or argon-filled glovebox (MBraun, UNIlab2000). Dehydrated THF, dehydrated pentane, and NaSCN were purchased from Kanto Chemical Co. (Tokyo, Japan) Tris(pentafluorophenyl) borane was purchased from Tokyo Chemical Industry Co. or gifted from Kanto Denka Kogyo Co., Ltd. (Tokyo, Japan) [C3mim][SCN] was prepared as reported [17]. The measurement of ion conductivity was performed using a disc of electrolyte sealed in a closed vessel. The disc was placed between two Au plates in a two-electrode cell. The temperature of cells was controlled by using a bench-top-type chamber (ESPEC, SU-241) and all cells were equilibrated at the operating temperature for at least 3 h before performing any measurements. Conductivity data were collected using a VMP3 (Biologic SAS, Seyssinet-Pariset, France) by AC impedance measurements over the frequency range between 1 Hz and 1MHz. Differential scanning calorimetry (DSC) analysis was performed by DSC60 instrument operated at a heating rate of 10 °C min⁻¹ under a nitrogen atmosphere using Al₂O₃ (Shimadzu Corporation, Kyoto, Japan) as reference material. Elemental analysis was performed on a Perkin Elmer 2400II CHNO/S elemental analyzer (Perkin Elmer Inc., MA, USA). Powder X-ray diffraction patterns were collected at room temperature with Rigaku Smart-Lab diffractometer (CuKα radiation) (Rigaku Corporation, Tokyo, Japan).

Synthesis of 1: [C3mim][SCN] (0.4930 g, 2.69 mmol) was charged in a 50 mL reaction flask. Then, B(C₆F₅)₃ (1.3810g, 2.70 mmol) dissolved in dehydrated THF was added to the flask. The reaction mixture was vigorously stirred at room temperature for 5 min to give a colorless homogeneous solution. Then, the solution was concentrated under reduced pressure. The obtained highly viscous liquid crystallized gradually to give colorless single crystals at room temperature. The OIC 1 was obtained in 44% yield (0.815 g) by washing the crystals with dehydrated pentane followed by drying under reduced pressure at room temperature. Anal. calcd for C₂₆H₁₃BF₁₅N₃S: C, 44.92; H, 1.88; N, 6.04. Found: C, 44.77; H, 1.67; N, 5.49. Melting point: 99.8 °C.

Fabrication of 1–0.1 and 1–0.2: OIC 1 and 0.1 or 0.2 molar equivalents of NaSCN and B(C₆F₅)₃ were charged in a 50 mL reaction flask. Then, the solid mixture was heated at 110 °C for 10 min to give colorless viscous liquid followed by cooling at room temperature to yield 1–0.1 or 1–0.2 as white solids.

Crystallographic Structural Determination. Data collections were carried out on a Rigaku VariMax Saturn (MoKα radiation, 1.2 kW rotating anode) (Rigaku Corporation, Tokyo, Japan). Crystal Data for C₂₆H₁₃BF₁₅N₃S (MW: 695.25): orthorhombic, Space Group P2₁2₁2₁ (no. 19), a = 10.5887(12) Å, b = 13.1964(16) Å, c = 19.541(2) Å, V = 2730.5(5) ų, Z = 4, T = −120.0°C, μ(MoKα) = 2.454 cm⁻¹, Dcalc = 1.691 g/cm³, reflections collected/unique reflections/parameters refined: 31262/6244/417, Rint = 0.0173, final R₁ = 0.0317 (I > 2σ(I)), wR₂ = 0.0844 (all data), GOF = 1.057. CCDC 1955625 contains the supplementary crystallographic data for this paper. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html (or from the CCDC, 12 Union Road, Cambridge CB2 1EZ, UK; Fax: +44 1223 336033; E-mail: [email protected]).

3. Results and Discussion

Compound 1 was synthesized by the addition of [C3mim][SCN] to B(C₆F₅)₃∙THF dissolved in dry THF under argon. The reaction proceeded at room temperature to give a colorless solution, which was evaporated under reduced pressure and cooled to give the 1 as colorless single crystals. [C3mim][SCN·B(C₆F₅)₃] (1) was subjected to differential scanning calorimetry (DSC), which revealed only one peak attributed to melting at 99.8 °C (Figure 2).

The crystal structure of 1 was revealed by single-crystal X-ray diffractometry (XRD) at −120 °C (Figure 3), which showed that the [C3mim][SCN] and B(C₆F₅)₃ moieties are located in the crystal lattice of 1 in a 1:1 molar ratio. The formation of a coordinative interaction between the N atom of the thiocyanate anion and the B atom of B(C₆F₅)₃ was also confirmed, since the boron center exhibits a tetrahedral structure with an average N–B–C bond angle of 107.5°. Furthermore, the B–N bond distance in 1 was determined to be 1.54 Å, while the B-N-C bond angle was found to be 165.23°. These values are comparable to those reported for compounds with B–N bonds between cyano groups and B(C₆F₅)₃ [16,18]. The packing view of 1 reveals a one-dimensional arrangement of imidazolium ions and adduct-type anions along the b-axis (Figure 4).

The ion conductivity of 1 was evaluated by the ac impedance method. A disk of 1 was fabricated by grinding single crystals to a white powder followed by pressure molding; this disk was used in the conductivity experiments. Crystals of 1 exhibit a linear Arrhenius relationship between the logarithm of solid-state ion conductivity and reciprocal temperature in the 75–95 °C range (Figure 5), from which the activation energy for 1 was calculated to be 258 kJ mol⁻¹. This value is quite large compared to those for lithium ion conduction in previously reported lithium-salt based OICs [8,9,10,11].

Based on the above result, we investigated the use of 1 as a matrix material for a solid electrolyte with sodium–ion conductivity. We expected the in situ formation of Na[SCN·BCF] when 0.1 or 0.2 molar equivalents of NaSCN and B(C₆F₅)₃ were added to 1, these materials are referred to as “1–0.1” and “1–0.2”, respectively. DSC curves of 1–0.1 and 1–0.2 gave the behavior corresponding to the melting point depression in comparison with 1 (Figure 2). Solid electrolytes 1–0.1 and 1–0.2 were obtained by heating a solid mixture of 1 and the appropriate amounts of NaSCN and B(C₆F₅)₃ at 120 °C under argon in the absence of any solvent to give colorless viscous liquids followed by cooling to room temperature. Both 1–0.1 and 1–0.2 were obtained as white powders that exhibit solid-state ionic conductivity. The ionic conductivity of 1–0.2 was determined to be 2.9 × 10⁻⁵ S cm⁻¹ at 80 °C, which is 100 times higher than that of 1.

Interestingly, the observed powder XRD patterns of 1 at room temperature were almost identical to the simulated pattern based on the crystal structure of 1 revealed by single crystal X-ray diffraction study at −120 °C (Figure 6). This result shows that the crystal structure of 1 shown in Figure 3 is maintained at room temperature. Moreover, it is shown that the ordered arrangements of the imidazolium cations and the adduct-type anions in 1 depicted in Figure 4 are maintained in both 1–0.1 and 1–0.2 since the XRD patterns of 1, 1–0.1, and 1–0.2 are quite similar. It strongly suggests that the sodium ions in 1–0.1 and 1–0.2 occupy cationic sites or interstitial positions in the packing structure of 1. Since the imidazolium cation and the adduct-type anion are sterically quite large compared to the sodium ion, we expect that the sodium ions diffuse through the crystal lattices of 1–0.1 and 1–0.2.

4. Conclusions

We synthesized the adduct-type anion-containing OIC 1 by the addition of B(C₆F₅)₃ to an SCN-anion-containing IL. Single crystal X-ray diffractometry revealed that 1 forms coordinative B–N bonds between the SCN anions and B(C₆F₅)₃ moieties. We also confirmed that 1 shows solid-state ionic conductivity in the crystalline state. We also investigated doping 1 with sodium thiocyanate and B(C₆F₅)₃ to evaluate the suitability of the obtained OIC as a matrix material. Both 1–0.1 and 1–0.2 exhibited increased ionic conductivity compared to that of 1. These results indicate that OICs formed by the addition of bulky Lewis acids to ILs have great potential as matrix materials for the development of innovative solid electrolytes.