Journal Information
Vol. 8. Issue 5.
Pages 4387-4398 (September - October 2019)
Download PDF
More article options
Vol. 8. Issue 5.
Pages 4387-4398 (September - October 2019)
Original Article
DOI: 10.1016/j.jmrt.2019.07.050
Open Access
Composite nanomaterials based on 1-butyl-3-methylimidazolium dicianamide and clays
E.P. Grishinaa,b, L.M. Ramenskayaa,
Corresponding author

Corresponding author.
, N.O. Kudryakovaa, K.V. Vagina,b, A.S. Kraeva, A.V. Agafonova
a G.A. Krestov Institute of Solution Chemistry of the Russian Academy of Sciences, Ivanovo, 1 Akademicheskaya St., Russia
b Ivanovo State University of Chemistry and Technology, Ivanovo, 7 Sheremetevsky Prospekt, Russia
This item has received

Under a Creative Commons license
Article information
Full Text
Download PDF
Figures (10)
Show moreShow less
Tables (2)
Table 1. Physicochemical characteristics of the materials used.
Table 2. Physicochemical properties of the BMImDCA ionic liquid and nanocomposites.
Show moreShow less

Nanocomposites of ionic liquids with layered aluminosilicates represent a new class of functional materials that are promising when creating electrochemical devices, in environmental protection, in biomedicine, etc. Such nanocomposites contain environmentally friendly (clay) and easily regenerable components (ionic liquids), which makes them promising objects of green chemistry. In this paper, the interaction of 1-butyl-3-methylimidazolium dicyanamide ionic liquid with clays such as montmorillonite K10 (MMT K10), bentonite (Bent) and halloysite (Hal), which have a different molecular and mesoporous structure, as well as particles of different size and shape, was studied for the first time. Physicochemical methods such as FT-IR, TG, DSC, electron microscopy, viscosimetry and conductometry were used. The effect of the confinement of ionic liquid in the pores and immobilization on the surface of clays on the physicochemical properties of nanocomposites has been revealed. It was found that the interaction of ionic liquid with clays depends on the type of nanoclay, and the interaction strength changes in the following order: MMT K10 ≈ Bent >> Hal. The resulting materials have the properties of pseudoplasticity, high ionic conductivity, which is promising when creating electrochemical devices. At low temperature, the electrical conductivity of the halloysite-based composite is higher than that of a pure ionic liquid. The conductivity of the studied materials obeys to a general trend, which depends on the specific interactions and the properties of the clay-filled ionic liquid.

Composite nanomaterials
Ionic liquid
Decomposition temperature
Glass transition
Full Text

Currently, the use of new types of high-performance materials and technologies is necessary to meet the requirements of modern green development. For example, promising developments are nanostructured catalysts for the photodegradation of water pollutants and air purification, new classes of highly porous materials, including covalently bonded stable porous structures, as well as biosimilar materials that combine environmentally friendly components in their structure [1–4]. Natural clays and ionic liquids are promising compounds in the field of green chemistry.

Ionic liquids (ILs) or room temperature ionic liquids (RTILs) are studied as a possible substitute for conventional molecular solvents for catalytic and organic reactions; their application allows sufficiently reducing the amount of water used in different technological processes. These compounds represent a relatively new and constantly widening class of salts with N- or P-containing organic cations and large inorganic or organic anions. These salts are in the molten (liquid) state at room temperatures. The unique combination of properties of ionic liquids – high ionic conductivity values, a wide temperature range of liquid state, low vapour pressure, high electrochemical and thermal stability – makes these RTILs quite attractive materials for creating new electrolytes for electrochemical energy storage units – electrochemical capacitors, lithium-ion batteries, photogalvanic cells, etc. [5–8]. The growing interest in ionic liquids is also caused by the prospects for their use in devices that work at elevated temperatures for a long time. Ionic liquids based on an N,N′-dialkylimidazolium cation and a bis(trifluoromethylsulfonyl)imide, (Tf)2N anion are the most claimed. That is why their properties have been studied well [9–20]. However, a promising alternative to the above-mentioned salts for the use in electrochemical devices is the ILs with a dicyanamide, (CN)2N (DCA) anion because they, as a rule, have lower viscosity and, consequently, better ionic conductivity than other ILs, and remain stable for a long time under heating [21–28].

At the same time, an urgent problem to be solved in electrochemical power engineering is developing, based on ionic liquids, highly-efficient solid state devices that have improved functional characteristics and are safe-to-use, especially at elevated temperatures [29–31]. Therefore, the creation of quasi-solid electrolytes (ionogels, nanocomposites) through IL immobilization or confinement into various inorganic porous matrices is relevant. In such materials, when ILs are introduced into the nanopores or adsorbed on the surface of a porous material, some of their confinement effects can change the properties of ILs, although the ions retain their liquid-like dynamics and mobility [32]. Ionic liquids have been quite successfully introduced into a 3D-network made up by silica [29–43], without reducing the composite conductivity or electrochemical stability window in comparison with the pure ionic liquid [36,44–46].

In addition to silica, it is possible to use nanoparticles of other inorganic oxides – SnO2[47,48], ZrO2[49] or TiO2[50,51] – as the inorganic matrix for creating ionogels. The last few years have seen a growing interest in the development of hybrid materials based on ionic liquids and natural alluminosilicates – bentonite [52], montmorillonite [53–58], kaolinite [59], and halloysite [60]. Immobilization of ionic liquids by the surface of nanoparticles of minerals and intercalation of cations into the inter-layer space of the minerals can ensure high (of the order of 10−3 S cm−1) ionic conductivity [60], excellent thermal stability [52,58], which makes them potentially suitable for the use in high-temperature electrochemical devices maintaining their high capacity and a large number of charge cycles [56].

There are so far only a limited number of works devoted to creating ion-conducting composites using clay minerals. In this work, new nanocomposites based on ionic liquid of 1-butyl-3-methylimidazolium dicyanamide (BMImDCA) immobilized in the inorganic matrix of bentonite, halloysite or montmorillonite К10 were obtained; their physicochemical characteristics were studied compared to those of pure components. The present data are useful in creating environmentally safe operating electrolytes for high-performance electrochemical devices.

2Materials and methods2.1Materials

The following materials were used in the work:

  • -

    Ionic liquid 1-butyl-3-methylimidazolium dicyanamide (BMImDCA, Sigma-Aldrich, CAS Number: 448245-52-1), the structural formula is given in Fig. 1;

    Fig. 1.

    Structural formula of 1-butyl-3-methylimidazolium dicyanamide.

  • -

    Montmorillonite К10 (MMT K10, Acros organics, Catalog No. AC456071000);

  • -

    Nanoclay, hydrophilic bentonite (Bent, Sigma-Aldrich, CAS Number 1302-78-9);

  • -

    Halloysite nanoclay (Hal, Sigma-Aldrich, CAS Number 1332-58-7).

2.2Preparation of IL-clay nanocomposites

The BMImDCA–clay nanocomposites were obtained through direct mixing of the components with a vibration shaker IKA VORTEX 4 basic (IKA-Werke GmbH & Co. KG, Germany). The mixture was kept in a vacuum drying oven LT-VO/20 (Labtex, Russia) at a temperature of 80 °C for 8 h. The obtained mechanical dispersions of clay mineral particles in the ILs were additionally treated in hermetically sealed capsules in an ultrasonic cleaner CT-431D2 (CTbrand Wahluen Electronic TOOL Co. Ltd., China) for 8 h. The obtained mixtures had the following molar ratios of the IL components: clay 2:1 (with Hal and with MMT K10) and 1:1 (with Bent), which corresponded to 60.4 wt.%, 53.5 wt.% and 53.3 wt.% of 1-butyl-3-methylimidazolium dicyanamide in the composite material.

2.3Methods of study

The visualization of the clay minerals and ionic liquid-clay composites was made by the scanning electron spectroscopy method using an NVision 40 microscope (Carl Zeiss, Inc., Germany).

The specific surface area of the clay samples was measured using the BET method, while the pore size distribution was obtained by the Dubinin–Astakhov method with low-temperature nitrogen adsorption-desorption Quantachrome Nova 1200 equipment. All the samples had been degassed in advance in a vacuum drying oven at 105 °C for 7 h.

The particle size distribution of the clay minerals and Z-potential were determined in distilled water with a particle size and Z-potential analyzer Zetasizer Nano (Malvern Instruments Ltd., UK).

A TG 209 F1 Iris calorimeter (NETZSCH, Germany) was used for thermal studies. A sample of about 10 mg in a platinum crucible was heated in an argon flow at a rate of 10 °C min−1 to a temperature of 800 °C. The accuracy of measuring the mass and temperature was ±10−6 g and ±0.1 °C, respectively.

A DSC 204 F1 Phoenix calorimeter (NETZSCH, Germany) was used to study the phase behavior of the pure ionic liquid and composites. A sample of approximately 10 mg in a hermetically sealed platinum pan was cooled with liquid nitrogen to −120 °C at a rate of 10 °C min−1 and then heated to 200 °C at a rate of 10 °C min−1. The measurements were carried out in an argon atmosphere. The accuracy of the mass and temperature measurements was ±10−5 g and ±0.1 °C, respectively.

An infrared Fourier spectrometer VERTEX 80v (Bruker, Germany) was used for spectrophotometric measurements. The FT-IR reflection spectra were recorded in the region from 500 to 4000 cm−1 at room temperature using a diamond crystal. The spectral resolution was 2 cm−1.

A Brookfield Programmable Viscometer Model DV2T (Brookfield, USA) was used to measure the dynamic viscosity (η). The measurement accuracy was ±1%. The temperature was varied from 10 to 80 °C.

A Solartron SI 1260A Impedance/Gain-Phase analyzer (Solartron analytical, UK) was used to determine the specific conductivity (κ). The measurement was carried out in a designed hermetic cell using platinum electrodes. The frequency range of the alternating current was from 1 to 100 kHz, the cell voltage was 10 mV. The value of the cell constant was determined using a 0.01 mol·dm−3 KCl solution. The measurements were carried out in the range from −20 to 80 °C. The cell temperature was maintained using a liquid cryothermostat LIOP FT-316-40 (LOIP, Russia) with the accuracy of ±0.2 °C.

3Results and discussion3.1Structural characteristics of clays

In this work, nanocomposites based on the ionic liquid BMImDCA were obtained using three types of clay minerals as structure-forming fillers with nano-size pores: hydrophilic bentonite, montmorillonite К10 and halloysite nanoclay. Several characteristics of these materials are presented in Fig.2 and Table 1 in comparison with the available literature data [61–65].

Fig. 2.

SEM-images of clay minerals used (on the left) and their mixtures with BMImDCA (on the right): a – MMT K10, mixture with IL, b – Bent, mixture with IL, c – Hal, mixture with IL.

Table 1.

Physicochemical characteristics of the materials used.

Parameter  Ionic liquid  Montmorillonite К10  Hydrophilic bentonite  Halloysite nanoclay 
Molecular formula  C10H15N5  Al2H2O12Si4  H2Al2O6Si  Al2Si2O5(OH)4 × 2H2
Chemical composition (for clays)a, wt.%  IL ≥ 97 Watera ˜ 0.11 (K.Fisher method)  O – 62.85  O – 58.12  O – 63.65 
    Na – 0.15  Na – 1.43  Al – 18.20 
    Mg – 0.80  Mg – 3.05  Si – 17.51 
    Al – 5.81  Al – 8.67  Cl – 0.12 
    Si – 27.66  Si – 24.12  Ca – 0.11 
    Cl – 0.19  Cl – 0.32  Fe – 0.13 
    K – 0.63  Ca – 1.50  Mg – 0.28 
    Ca – 0.14  Ti – 0.24   
    Ti – 0.16  Fe – 2.55   
    Fe – 1.62     
Molecular weight, g mol−1  205.26  360.307  180.1  294.19 
Density, g cm−3  1.06  0.370  0.6–1.1  2.53 
Pore volume, ml g−1  –  0–80 nm: 0.36  0.004a  1.26–1.34 
    0–24 nm: 0.30    0.13* 
    0–14 nm: 0.26     
Average pore size, nm  –  4.1a  4.0a  7.8a 
Particle size, nm  Cation volume, nm3  >63,000 (<25%)  ≤25,000  Diameter: 30–70 
  0.150 [61]  220–430a  150–560a  Length: 1000–3000 
  0.198 [62]      90–280a 
  Anion volume, nm3       
  0.056 [63]       
  0.089 [64]       
  0.069 [65]       
Surface area, m2  g−1  –  240  1.9a  57a 
Z-potentiala, mV  –  −28  −28  −13 

This work.

The hydrophilic bentonite (Nanoclay) used in this work is an untreated hydrophilic clay (without organic modifications). It mainly consists of montmorillonite and different amounts of other minerals, such as quartz (SiO2), calcium and sodium feldspar [(CaAl2Si2O8), (NaAl3Si2O8)] and represents aggregates of plates packed together via electrostatic forces and containing interlayer water in their structure [66]. The surface of bentonite aggregates has a negative charge which is compensated by the cations intercalated between the structural plates [67].

Montmorillonite K10 is an acid-activated and thermally treated montmorillonite. Untreated montmorillonite is a clay mineral, 2:1 silicate, a member of the smectite group (Fig. 2). Its original structure consists of two SiO4 tetrahedral layers, with their tops directed to each other and forming a sandwich with the central octahedral layer of aluminum hydroxide [68]. Montmorillonite contains a large number of mobile cations capable of ionic exchange, which is used for exchange of inorganic cations with organic cations and formation of an organically modified clay mineral [69,70]. During the acidic treatment, the crystal structure of the montmorillonite becomes partially destroyed, which leads to the formation of a highly porous substance with a larger surface area and nanopores [68]. As a result of the thermal treatment, montmorillonite K10 almost loses its ability to swell [71,72].

Halloysite is a hydrated tubular form of kaolinite [73,74]. The crystal structure of halloysite consists of aluminosilicate plates folded into nanoscrolls (Fig. 2). The crystallization water and OH groups of the kaolinite are in the gap between the layers [75]. On average, halloysite nanotubes have the external diameter of 50–100 nm, and the pore space diameters are about 12–15 nm at the length of about 1 μм. The internal surface of the kaolinite plates in the rolls has a positive charge, while the external one is charged negatively. The surface area can reach 50–500 m2  g−1 depending on the treatment method [76,77].

The structural characteristics of the clays used in this work to prepare nanocomposites are given in Table 1. The experimental data show that the specific surface area of MMT K10 is much larger than that of the other clay samples used, the Z-potential is negative in all the studied samples and is the least in the halloysite particles.

By comparing the average pore sizes of the clay minerals with the ionic liquids anion and cation volumes (Table 1), we can suppose that a large asymmetric cation and a rather large anion can easily penetrate into the pore or inter-layer space of the clay particles. In fact, it has been shown that cations of different ILs under certain conditions can be intercalated into inter-layer spaces of clay minerals and make them larger [57,58]. It is noteworthy that in all the prepared composites, the IL volume is more than 3 times bigger than the free volume of the pores of the mineral filler. That is why most of the IL is immobilized by the clay particle surface.

3.2FT-IR spectra

Figs. 3–5 show the FT-IR reflection spectra for the BMImDCA–MMT K10, BMImDCA–Hal and BMImDCA–Bent composites, the pure ionic liquid BMImDCA and the original clay MMT K10, Hal and Bent in the region of 4000–400 cm−1. The spectra of all the composites are similar to those of pure IL and include bands of the inorganic matrix. One or two peaks at ca. 3700 and 3600 cm−1 belong to the stretching modes of the SiOH group; the broad band of about 3600–3300 cm−1 and the slight peak at 1650 cm−1, are assigned to the νOH stretching mode and δOH bending mode from absorbed water, respectively [58,78,79]. Several peaks in the range of 3200–3000 cm−1 and 3000–2800 cm−1 are related to the νCH modes of the ring and aliphatic chains of the BMIm+ cation, respectively [19,80]. The strong peaks between 2400 and 2000 cm−1 are associated with the vibration of the N≡C bond of the DCA anion [81]. The peaks observed below 1600 cm−1 are due to the stretching and bending vibrations of various groups from the cation, such as νCH2(N) and νCH3(N) at ca. 1570 cm−1, ring CH3 and νCN at ca. 1460 cm−1, νCCCC at ca. 1427 and 1380 cm−1, δasip ring and δCCCC at ca. 1307 cm−1, δCH3(N)CN at ca. 1166 cm−1[80]. The bands from Si–O, Al–O and Mg–O are observed around 1030 cm−1, 620 and 470–530 cm−1, respectively [58,79].

Fig. 3.

FTIR spectra of BMImDCA–MMT K10 (black trace), BMImDCA (red trace) and MMT K10 (blue trace) and in the region of 4000–400 cm−1; insert – Extended FTIR spectra in the regions (a) NC (anion), (b) νCH2(N), νCH3(N), ring CH3, νCN, νCCCC (cation), and (c) MgO (MMT K10).

Fig. 4.

FTIR spectra of BMImDCA–Hal (black trace), BMImDCA (red trace) and Hal (blue trace) and in the region of 4000–400 cm−1; insert – Extended FTIR spectra in the regions (a) NC (anion), (b) δasip ring and δCCCC cm−1 (cation) and (c) MgO (Hal).

Fig. 5.

FTIR spectra of BMImDCA–Bent (black trace), BMImDCA (red trace) and Bent (blue trace) and in the region of 4000–400 cm−1; insert – Extended FTIR spectra in the regions (a) NC (anion), (b) δasip ring and δCCCC cm−1 (cation) and (c) MgO (Bent).


In contrast to the BMImBF4 ionic liquid confined in silica matrix [82], noticeable changes in the infrared spectrum can be observed in the studied systems. For example, the νSi–OH modes of pure MMT K10 (˜3670 and 3622 cm−1) and pure Bent (3625 cm−1) disappear in the spectra of the composites, and the bands of absorbed water shift by 10 and 6 cm−1 to the higher frequency range (Figs. 3 and 5). However, there are no applicable changes in the spectrum of the Hal composite: two silanol peaks at 3697 and 3622 cm−1 of pure Hal are observed at the same frequencies at 3697 and 3625 cm−1 (Fig. 4). The ν(Si–O) and ν(Mg–O) modes show red shifts (Δν) increasing from Hal to MMT K10 and Bent (Fig. 3–5 and inserts (c) in Fig. 3–5). For example, the value of Δν(Si–O) is 6, 26 and about 40 cm−1 for the Hal, MMT K10 and Bent composites, respectively.

The ionic liquid confined in MMT K10 and Hal shows a minor blue shift (–Δν) of about 3–4 cm−1 in the frequency range of the DCA anion relative to the pure IL (insert (a) in Figs. 3,4). At the same time, the shift of about 9–15 cm−1 and a new band at ca.2153 cm−1 are observed in the spectrum of the Bent composite (insert (a) in Fig. 5). As for the BMIm+ cation, more significant changes are observed in the range of 1700–1200 cm−1: new bands appear in the spectrum of the MMT K10 composite at 1410 and 1507 cm−1 (insert (b) in Fig. 3), and the peak at 1302 cm−1 is blue-shifted by 5 and 3 cm−1 in the spectra of the Hal and Bent composites, respectively (insert (b) in Figs. 4 and 5). In the range of 3200–2800 cm−1, the νCH modes exhibit a slight blue shift of about 1–4 cm−1, with the largest value for the Bent composite (Figs. 3–5).

Thus, it has been found that some of the characteristic frequencies of both the ionic liquid and the clay are shifted in the spectra of their nanocomposites by a distance exceeding the instrumental resolution (2 cm−1). This phenomenon is associated with the interaction of these compounds, mainly due to Coulomb and van der Waals forces. Apparently, the anion DCA also partially interacts with the silanol groups of the inner layer through hydrogen boning SiOH···N. In accordance with the values of the observed shifts, these interactions become weaker in the series MMT K10 ≈ Bent >> Hal. Apparently, the water absorbed by the clay is partially desorbed and replaced by an ionic liquid, mainly an anion, and this ability decreases in the order mentioned above.

3.3TG and DCS studies

Fig. 6 shows the DTA traces of the three composites and pure components. In all cases, a peak at a temperature below 100 °C corresponds to the departure of physically adsorbed water. For pure clay, a peak at a temperature above 400 °C is associated with the dehydroxylation of the aluminosilicate layers [53,78]. Pure ionic liquid shows the peaks at 314 and 393 °C corresponding to the decomposition of the DCA anion (Tan) and more stable BMIm+ cation (Tcat), respectively [18,83], followed by a small peak from the destruction of the residual IL fragments.

Fig. 6.

DTGA curves of (a) MMT K10, (b) Bent, (c) Hal, (d) BMImDCA, (e) BMImDCA–MMT K10, (f) BMImDCA–Bent and BMImDCA–Hal (g).


All the modified clay minerals exhibit lower temperatures for both the dehydroxylation and destruction of the ionic liquid (Fig. 6). This phenomenon is attributed to the lower crystallinity of the grafted materials [84]. It should be noted that the ionic liquid confined in MMT K10 and Bent shows a more significant depression of the temperatures Tan and/or Tcat in relation to the pure ionic liquid than when it is enclosed in Hal. This thermal response is the result of different arrangements of the cation and anion, for example, on the surface, in the pores or inside the aluminosilicate layers. It was found that the BMImBr ionic liquid entrapped within silica nonporous has a higher crystallinity than the same IL absorbed on the surface [85]. This result is confirmed by our data in Fig. 7, which shows DSC curves for the pure and confined ionic liquid.

Fig. 7.

DSC traces of BMImDCA (1), BMImDCA–Hal (2), BMImDCA–MMT K10 (3) and BMImDCA–Bent (4).


All of the samples exhibit a wide endothermic wave at temperatures above 60 °C caused by water removal, as well as a glass transition (Tg) at low temperatures. Our Tg value for pure BMImDCA appeared to be slightly below −90 °C [86] due to the presence of water, which is known to lead to the salt amorphization [87]. It may be clearly seen from Fig. 7 that the IL entrapped in MMT K10 and Bent has the higher Tg values, and IL entrapped in Hal has a lower Tg value in comparison with the pure ionic liquid.

Thus, the thermal behavior of the BMImDCA ionic liquid in MMT K10 and Bent composites is similar, but different from that in the Hal composite. It is known that the properties of a confined ionic liquid differ from the properties of both adsorbed and bulk salts [53,88,89]. Based on the presented data, it can be supposed that the confined BMImDCA is located mainly on the surface of the Hal and in the pores of MMT K10 and Bent. In addition, the DCA anion partially intercalates into the aluminosilicate layers depending on the properties of the clay in the following order MMT K10 ≈ Bent >> Hal. This result is consistent with the above IR data.

3.4Viscosity η and Ionic conductivity κ

When nanoporous fillers are introduced into an ionic liquid, an important problem to be solved is maintaining high ionic conductivity in the quasi-solid state of the composite, and this problem is solved quite successfully, for example, when nanoporous silica are used [38,41,90]. In this work, at the predetermined ratio of components, the obtained composites represent pastes of different consistency that do not segregate for a long time (Fig. 2). For the studied systems, we have obtained dependences of shear stress (τr) on shear rate (Dr) (Fig. 8). Pure BMImDCA, just like BMImBr that was investigated by us earlier [91], has properties of Bingham (or plastic) fluids: τr = τ0 + ηDr, here τ0 is the yield stress, below which the liquid does not flow, η is the Bingham viscosity. The composites based on IL behave in a similar way. Values η, obtained for the systems under study, are given in Table 2.

Fig. 8.

Dependences of shear stress τr on shear rate Dr for BMImDCA (1) and its mixtures with MMT K10 (2), Bent (3) and Hal (4) at 20 °C.

Table 2.

Physicochemical properties of the BMImDCA ionic liquid and nanocomposites.

Parameter  BMImDCA  BMImDCA –MMT K10  BMImDCA –Bent  BMImDCA –Hal 
Td, °C  314  280  310  300 
Tg, °C  −94.4  −90.6  −88.1  −98.5 
Ηa, Pa s  0.031  18.67  4.42  0.86 
Κa, S m−1  0.964  0.398  0.554  0.840 
Walden producta, Pa s S m−1  0.029  7.431  2.449  0.722 
Eab, kJ mol−1  22  21  20  20 
T0, °C  −115.9  −120.1  −128.8  −138.9 

Temperature 20 °C.


The values are calculated for the temperature range of 20–80 °C, R2 ≥ 0.998.

The temperature dependence of the BMImDCA ionic conductivity in the bulk state and in immobilized state in clay minerals is shown in Fig. 9a,b. As it shows, despite the fact that the viscosity grew by 1–2 orders of magnitude when nanoporous aluminosilicate thickeners were introduced into the IL and the bulk concentration of ions decreased, the conductivity in the composites remained high. For example, in the considered temperature range, value κ of the solid-state composite with the lowest conductivity among the objects in question (BMImDCA–MMT K10) exceeds that of the pure N,N′-dialkylimidazolium ILs with a (Tf)2N anion that we studied earlier [19,20]. The temperature behaviour of all the ion-conducting composites studied in this work in the range from 30 to 80 °C can be described by the Arrhenius equation (R2 ≥ 0.998) with similar values of effective energy of activation of specific electric conductivity (Table 2). Widening of the temperature range leads to a deviation from linear behaviour, and the dependence κ(T) can be described by the Vogel–Fulcher–Tammann (VFT) equation related to the ordinary en masse diffusion (vehicle mechanism) [9,92]:

where κ0 is the limiting electric conductivity, kκ is a constant related to the Arrhenius activation energy, and T0 is the ideal glass transition temperature. The values of T0 depend on the chosen temperature range but are always lower than the experimentally determined glass transition point Tg[20,93] and, according to the literature data, in most cases T0/Tg ≈ 0.75 (T0, K; Tg, K). For the studied IL and nanocomposites based on it, the ratio T0/Tg equals 0.87 (BMImDCA), 0.84 (BMImDCA–MMT K10), 0.78 (BMImDCA–Bent) and 0.76 (BMImDCA–Hal) in the temperature range (253–353 К).

Fig. 9.

Plot of the ionic conductivity (κ) as a function of temperature (a) and Arrhenius conductivity plots (b) for BMImDCA (1) and composites BMImDCA–MMT K10 (2), BMImDCA–Bent (3) and BMImDCA–Hal (4).


As Fig. 9 shows, the obtained values of specific electric conductivity essentially depend on the nature of the clay material. Despite a very big (about two orders of magnitude) difference in the specific surface areas and pore volume, as well as an almost four-time difference in the viscosity values (Table 2), the nanocomposites with MMT K10 and Bent at the same IL content (wt.%) have quite similar κ values (0.40 and 0.55 S m−1 at 20 °C, respectively), which are much lower than in the pure IL. In contrast to these systems, the conductivity of the BMImDCA–Hal composite is slightly lower in the region of positive temperatures, compared to the pure IL, and is even higher than that in the region of negative temperatures (0.84 and 0.92 S m–1 at 20 °C; 0.15 and 0.11 S m–1 at −20 °C, respectively). The nanocomposites with MMT K10 and Hal at the same molar ratio of the components are, however, very different from each other in their ionic conductivity. This may be caused by the electrostatic binding of a relatively larger number of cations with the highly developed surface of MMT K10 than in the composite with Hal. Besides, the lower negative charge of the surface and the larger pore size of Hal (Table 1) are not favorable for confinement ions, ion pairs and self-assembly complexes of the IL. That is why the higher conductivity of BMImDCA–Hal in comparison with BMImDCA–MMT K10 is associated with the effect of two structural factors – smaller specific surface and porosity and larger pore size.

It is worth mentioning that when plotted in the logκ – logη−1 coordinates (Walden plot), the points corresponding to different composites lie on the same straight line (Fig. 10, R2 = 0.9997). And the slope corresponds to the power index in the fractional Walden rule κηα = const, that can be applied to ionic liquids. Value α characterizes the degree of IL “ionicity”, and the value α < 1 is the result of formation of ionic associates in them [94,95]. For the composites with different clay minerals, we have obtained the value α = 0.24, which indicates that the degree of binding of conductivity ions with the surface is also high in the pores of the clay minerals.

Fig. 10.

Walden plot for nanocomposites; the temperature is 20 °C.


The effect of the interaction of ionic liquid 1-butyl-3-methylimidazolium dicyanamide with layered aluminosilicates (montmorillonite K10, bentonite and halloysite), which have different particle shape and porous mesostructure, on the physicochemical properties of gel-like materials was studied. It has been established that the properties of the inorganic host matrix (porous structure, negative surface charge and the functional groups on the surface and inside the layer) affect the physicochemical properties of their composites with the ionic liquid used. The infrared spectra of composites revealed noticeable changes in the characteristic frequencies both clay (νSiO, νSiOH) and ionic liquid (νNC, νCH2(N), νCH3(N), ring CH3, etc.). Thermodynamic studies of a nanocomposites ionic liquid–clay showed lower temperatures for the processes of clay dehydroxylation and destruction of the ionic liquid, as well as a change in the glass transition temperature compared to the initial components. Based on the data obtained, a model of interaction and location of the ionic liquid in nanoclay was proposed. According to this model, the ionic liquid is located mainly on the surface of Hal and in the pores of MMT K10 and Bent. The immobilization of ionic liquid by the clay is apparently due mainly to the Coulomb interactions of the BMIm+ cation and the SiO groups, which provide a negative charge of the clay surface. The dicyanamide anion is introduced into the interlayer space of the clay due to the formation of the hydrogen bond SiOH···N. According to IR spectroscopy, the interaction of ionic liquids with clay weakens in the order MMT K10 ≈ Bent >> Hal. Studies of viscometry have shown that both the composites under study and the pure BMImDCA have the property of pseudoplasticity (Bingham fluid). Compared to pure ionic liquid, the obtained nanocomposites have lower ionic conductivity due to a decrease in the number of free ions involved in the transfer process, owing to the interaction of the ionic liquid with the inorganic matrix. It was found that "ionicity" is equal to 0.24, and the fractional Walden rule is valid. At the same time, a quasi-solid electrolyte retains the properties of an ionic liquid with a high value of ionic conductivity.

Conflicts of interest

The authors declare no conflicts of interest.


This work was funded by Russian Foundation for Basic Research grant № 18-29-12012 mk. The authors gratefully acknowledge to the center for joint use of scientific equipment “The upper Volga region centre of physico-chemical research”.

Z. Wang, M. Chen, D. Huang, G. Zeng, P. Xu, C. Zhou, et al.
Multiply structural optimized strategies for bismuth oxyhalide photocatalysis and their environmental application.
Chem Eng J, 374 (2019), pp. 1025-1045
H. Yi, M. Yana, D. Huang, G. Zeng, C. Lai, M. Li, et al.
Synergistic effect of artificial enzyme and 2D nano–structured Bi2WO6 for eco–friendly and efficient biomimetic photocatalysis.
Appl Catalysis B: Environ, 250 (2019), pp. 52-62
H. Wang, Z. Zeng, P. Xu, L. Li, G. Zeng, R. Xiao, et al.
Recent progress in covalent organic framework thin films: fabrications, applications and perspectives.
Chem Soc Rev, 48 (2019), pp. 488-516
M.B. Zakaria, T. Chikyow.
Recent advances in Prussian blue and Prussian blue analogues: synthesis and thermal treatments.
Coordination Chem Rev, 352 (2017), pp. 328-345
H. Olivier–Bourbigou, L. Magna.
Ionic liquids: perspectives for organic and catalytic reactions.
J Molec Catal A: Chem, 182–183 (2002), pp. 419-437
T. Sato, S. Marukane, T. Morinaga.
Ionic liquids for the electric double layer capacitor applications.
pp. 109-134
H. Srour, L. Chancelier, E. Bolimowska, T. Gutel, S. Mailley, H. Rouault, et al.
Ionic liquid–based electrolytes for lithium–ion batteries: review of performances of various electrode systems.
J Appl Electrochem, 46 (2016), pp. 149-155
Y. Zhao, T. Bostrom.
Application of ionic liquids in solar cells and batteries: a review.
Curr Org Chem, 19 (2015), pp. 556-566
P. Wasserheid, T. Welton.
Ionic liquids in synthesis.
Wiley–VCH Verlag, (2003),
H. Tokuda, K. Hayamizu, K. Ishii, Susan MdABH, M. Watanabe.
Physicochemical properties and structures of room temperature ionic liquids. 2. Variation of alkyl chain length in imidazolium cation.
J Phys Chem B, 109 (2005), pp. 6103-6110
H. Tokuda, S. Tsuzuki, Md A.B.H. Susan, K. Hayamizu, M. Watanabe.
How ionic are room–Temperature ionic liquids? An Indicator of the physicochemical properties.
J Phys Chem B, 110 (2006), pp. 19593-19600
H. Tokuda, K. Hayamizu, K. Ishii, Md A.B.H. Susan, M. Watanabe.
Physicochemical properties and structures of room temperature ionic liquids. 1. Variation of anionic species.
J Phys Chem B, 108 (2004), pp. 16593-16600
L. Ramesh, M.G.F. Gardas, P.J. Carvalho, I.M. Marrucho, I.M.A. Fonseca, A.G.M. Ferreira, et al.
P T measurements of imidazolium–based ionic liquids.
J Chem Eng Data, 52 (2007), pp. 1881-1888
H.A. Every, A.G. Bishop, D.R. MacFarlane, G. Orädd, M. Forsyth.
Transport properties in a family of dialkylimidazolium ionic liquids.
Phys Chem Chem Phys, 6 (2004), pp. 1758-1765
P. Bonhôte, A.P. Dias, N. Papageorgiou, K. Kalyanasundaram, M. Grätzel.
Hydrophobic, highly conductive ambient–temperature molten salts.
Inorg Chem, 35 (1996), pp. 1168-1178
J.G. Huddleston, A.E. Visser, W.M. Reichert, H.D. Willauer, G.A. Broker, R.D. Rogers.
Characterization and comparison of hydrophilic and hydrophobic room temperature ionic liquids incorporating the imidazolium cation.
Green Chem, 3 (2001), pp. 156-164
J. Vila, L.M. Varela, O. Cabeza.
Cation and anion sizes influence in the temperature dependence of the electrical conductivity in nine imidazolium based ionic liquids.
Electrochim Acta, 52 (2007), pp. 7413-7417
E.P. Grishina, L.M. Ramenskaya, M.S. Gruzdev, O.V. Kraeva.
Water effect on physicochemical properties of 1–butyl–3–methylimidazolium based ionic liquids with inorganic anions.
J Mol Liquids, 177 (2013), pp. 267-272
L.M. Ramenskaya, E.P. Grishina, N.O. Kudryakova.
Physicochemical features of short–chain 1–alkyl–3–methylimidazolium bis(trifluoromethylsulfonyl)–imide ionic liquids containing equilibrium water absorbed from air.
J Mol Liquids, 272 (2018), pp. 759-765
E.P. Grishina, N.O. Kudryakova, L.M. Ramenskaya, Yu A. Fadeeva.
The temperature effect on the transport properties of 1–Alkyl–3–methylimidazolium bis(trifluoromethylsulfonyl)imide ionic liquids.
Russ J Phys Chem A, 92 (2018), pp. 724-729
D.R. MacFarlane, J. Golding, S. Forsyth, M. Forsyth, G.B. Deacon.
Low viscosity ionic liquids based on organic salts of the dicyanamide anion.
Chem Commun (Camb), 16 (2001), pp. 1430-1431
D.R. MacFarlane, S.A. Forsyth, J. Golding, G.B. Deacon.
Ionic liquids based on imidazolium, ammonium and pyrrolidinium salts of the dicyanamide anion.
Green Chem, 4 (2002), pp. 444-448
Y. Yoshida, O. Baba, G. Saito.
Ionic liquids based on dicyanamide anion: influence of structural variations in cationic structures on ionic conductivity.
J Phys Chem B, 111 (2007), pp. 4742-4749
Yuan W–L, X. Yang, L. He, Y. Xue, S. Qin, G.-H. Tao.
Viscosity, conductivity, and electrochemical property of dicyanamide ionic liquids.
Front Chem, 6 (2018), pp. 1-12
L. Rui, Y. Meirong, X. Xiaopeng.
Thermal stability and thermal decomposition kinetics of 1–Butyl–3–methylimidazolium dicyanamide.
Chinese J Chem Eng, 18 (2010), pp. 736-741
H. Yoon, G.H. Lane, Y. Shekibi, P.C. Howlett, M. Forsyth, A.S. Best, et al.
Lithium electrochemistry and cycling behaviour – of ionic liquids using cyano based anions.
Energy Environ Sci, 6 (2013), pp. 979-986
Y. Bai, J. Zhang, Y. Wang, M. Zhang, P. Wang.
Lithium–modulated conduction band edge shifts and charge–transfer dynamics in dye–sensitized solar cells based on a dicyanamide ionic liquid.
Langmuir, 27 (2011), pp. 4749-4755
C. Wolff, S. Jeong, E. Paillard, A. Balducci, S. Passerini.
High power, solvent–free electrochemical double layer capacitors based on pyrrolidinium dicyanamide ionic liquids.
J Power Sources, 293 (2015), pp. 65-70
C.-C. Chen, C.-Y. Chiang, T.-Y. Wu, I.-W. Sun.
Improved electrochromic properties of poly(3,4–ethylenedioxythiophene) in 1–butyl–3–methylimidazolium dicyanamide.
ECS Electrochem Lett, 2 (2013), pp. H43-H45
S. Wang, B. Hsia, J.P. Alper, C. Carraro, Z. Wang, R. Maboudian.
Comparative studies on electrochemical cycling behavior of two different silica–based ionogels.
J Power Sources, 301 (2016), pp. 299-305
K.-M. Lee, P.-Y. Chen, C.-P. Lee, K.-C. Ho.
Binary room–temperature ionic liquids based electrolytes solidified with SiO2 nanoparticles for dye–sensitized solar cells.
J Power Sources, 190 (2009), pp. 573-577
J.L. Bideau, L. Viau, A. Vioux.
Ionogels, ionic liquid based hybrid materials.
Chem Soc Rev, 40 (2011), pp. 907-925
P. Wang, S.M. Zakeeruddin, P. Comte, I. Exnar, M. Grätzel.
Gelation of ionic liquid–based electrolytes with silica nanoparticles for quasi–solid–state dye–sensitized solar cells.
J Am Chem Soc, 125 (2003), pp. 1166-1167
S. Shimano, H. Zhou, I. Honma.
Preparation of nanohybrid solid–state electrolytes with liquidlike mobilities by solidifying ionic liquids with silica particles.
Chem Mater, 19 (2007), pp. 5216-5221
K. Ueno, K. Hata, T. Katakabe, M. Kondoh, M. Watanabe.
Nanocomposite ion gels based on silica nanoparticles and an ionic liquid: ionic transport, viscoelastic properties, and microstructure.
J Phys Chem B, 112 (2008), pp. 9013-9019
K. Ueno, M. Watanabe.
From colloidal stability in ionic liquids to advanced Soft materials using unique media.
Langmuir, 27 (2011), pp. 9105-9115
M.-A. Néouze, J.L. Bideau, P. Gaveau, S. Bellayer, A.I. Vioux.
New materials arising from the confinement of ionic liquids within silica–derived networks.
Chem Mater, 18 (2006), pp. 3931-3936
S.A.M. Noor, P.M. Bayley, M. Forsyth, D.R. MacFarlane.
Ionogels based on ionic liquids as potential highly conductive solid state electrolytes.
Electrochim Acta, 91 (2013), pp. 219-226
A.I. Horowitz, M.J. Panzer.
High–performance, mechanically compliant silica–based ionogels for electrical energy storage applications.
Mater Chem, 22 (2012), pp. 16534-16539
L. Negrea, B. Daffosa, V. Turq, P.L. Taberna, P. Simon.
Ionogel–based solid–state supercapacitor operating over a wide range of temperature.
Electrochim Acta, 206 (2016), pp. 490-495
A. Vioux, L. Viau, S. Volland, J.L. Bideau.
Use of ionic liquids in sol–gel; ionogels and applications.
C R Chimie, 13 (2010), pp. 242-255
M.P. Singh, R.K. Singh, S. Chandra.
Properties of ionic liquid confined in porous silica matrix.
ChemPhysChem, 11 (2010), pp. 2036-2043
A.I. Horowitz, K. Westerman, M.J. Panzer.
Formulation influence on the sol–gel formation of silica–supported ionogels.
J Solgel Sci Technol, 78 (2016), pp. 34-39
D. Deb, S. Bhattacharya.
Role of different nanoparticulate cores on the thermal, mechanical and electrochemical cycling behaviour of nanoscale hybrid ionic fluids.
Electrochim Acta, 245 (2017), pp. 438-447
Y. Li, K.-W. Wong, K.-M. Ng.
Ionic liquid decorated mesoporous silica nanoparticles: a new high–performance hybrid electrolyte for lithium batteries.
Chem Commun, 52 (2016), pp. 4369-4372
A.I. Horowitz, M.J. Panzer.
High–performance, mechanically compliant silica–based ionogels for electrical energy storage applications.
J Mater Chem, 22 (2012), pp. 16534-16539
B. Dutta, D. Deb, S. Bhattacharya.
Ionic liquid–SnO2 nanoparticle hybrid electrolytes for secondary charge storage devices: physicochemical and electrochemical studies.
Int J Hydrogen Energy, 43 (2018), pp. 4081-4089
S. Bellayer, L. Viau, Z. Tebby, T. Toupance, J.L. Bideau, A. Vioux.
Immobilization of ionic liquids in translucent tin dioxide monoliths by sol–gel processing.
Dalton Trans, (2009), pp. 1307-1313
P. Bose, S. Bhattacharya.
Influence of anion structure on thermal, mechanical, dielectric and electrochemical properties of ZrO2 nanoparticle–pyrrolidinium ionic liquid hybrid electrolytes for the application in energy storage devices.
Int J Hydrogen Energy, 43 (2017), pp. 1-11
U.-H. Lee, T. Kudo, I. Honma.
High–ion conducting solidified hybrid electrolytes by the self–assembly of ionic liquids and TiO2.
Chem Commun, (2009), pp. 3068-3070
Y.L. Verma, A.K. Tripathi, V.K. Shalu Singh, L. Balo, H. Gupta, S.K. Singh, et al.
Preparation and properties of titania based ionogels synthesized using ionic liquid 1–ethyl–3–methyl imidazolium thiocyanate.
Mat Sci Eng B, 220 (2017), pp. 37-43
B. Haddad, D. Villemin, K. Dahamni, H. Belarbi, T. Moumene, S. Bresson, et al.
Preparation and thermal properties of organically modified bentonite with ionic liquids.
ChemXpress, 9 (2016), pp. 295-302
J.P. Fontana, F.F. Camilo, M.A. Bizeto, R. Faez.
Evaluation of the role of an ionic liquid as organophilization agent into montmorillonite for NBR rubber nanocomposite production.
Appl Clay Sci, 83–84 (2013), pp. 203-209
L. Reinert, K. Batouche, J.-M. Lévêque, F. Muller, J.-M. Bény, B. Kebabi, et al.
Adsorption of imidazolium and pyridinium ionic liquids onto montmorillonite: characterization and thermodynamic calculations.
Chem Eng J, 209 (2012), pp. 13-19
L. Wu, L. Liao, G. Lv, F. Qin, Z. Li.
Microstructure and process of intercalation of imidazolium ionic liquids into montmorillonite.
Chem Eng J, 236 (2014), pp. 306-313
S. Maiti, A. Pramanik, S. Chattopadhyay, G. De, S. Mahanty.
Electrochemical energy storage in montmorillonite K10 clay based composite as supercapacitor using ionic liquid electrolyte.
J. Colloid Interface Sci, 464 (2016), pp. 73-82
N.H. Kim, S.V. Malhotra, M. Xanthos.
Modification of cationic nanoclays with ionic liquids.
Microporous Mesoporous Mater, 96 (2006), pp. 29-35
C. Takahashi, T. Shirai, M. Fuji.
Study on intercalation of ionic liquid into montmorillonite and its property evaluation.
Mater Chem Phys, 135 (2012), pp. 681-686
G.K. Dedzo, C. Detellier.
Clay minerals-ionic liquids, nanoarchitectures, and applications.
Adv Funct Mater, 28 (2017), pp. 1703845
N. Zhao, Y. Liu, X. Zhao, H. Song.
Liquid crystal self–assembly of halloysite nanotubes in ionic liquids: a novel soft nanocomposite ionogel electrolyte with high anisotropic ionic conductivity and thermal stability.
Nanoscale, 8 (2016), pp. 1545-1554
H. Tokuda, K. Ishii, M.A.B.H. Susan, S. Tsuzuki, K. Hayamizu, M. Watanabe.
Physicochemical properties and structures of room–temperature ionic liquids. 3. variation of cationic structures.
J Phys Chem B, 110 (2006), pp. 2833-2839
Y. Marcus.
Ionic and molar volumes of room temperature ionic liquids.
J Mol Liquids, 209 (2015), pp. 289-293
P. Li, D.R. Paul, T.-S. Chung.
Supporting information for high performance membranes based on ionic liquid polymers for CO2 separation from the flue gas.
Green Chem, 14 (2012), pp. 1052-1063
W. Beichel, U.P. Preiss, S.P. Verevkin, T. Koslowsli, I. Krossing.
Empirical description and prediction of ionic liquids’ properties with augmented volume–based thermodynamics.
J Mol Liquids, 192 (2014), pp. 3-8
K. Bica, M. Deetlefs, C. Schröder, K.R. Seddon.
Polarisabilities of alkylimidazolium ionic liquids.
PhysChemChemPhys, 15 (2013), pp. 2703-2711
Q.H. Hu, S.Z. Qiao, F. Haghseresht, M.A. Wilson, G.Q. Lu.
Adsorption study for removal of basic red dye using bentonite.
Ind Eng Chem Res, 45 (2006), pp. 733-738
E. Ferrage, B. Lanson, N. Malikova, A. Plançon, B.A. Sakharov, V.A. Drits.
New insights on the distribution of interlayer water in bi–hydrated smectite from X ray diffraction profile modeling of 00l reflections.
Chem Mater, 17 (2005), pp. 3499-3512
M.F. Brigatti, E. Galan, B.K.G. Theng.
Structure and mineralogy of clay minerals.
2nd ed., pp. 21-81
F. Bergaya, M. Jaber, J.-F. Lambert.
Organophilic clay minerals.
pp. 45-86
H. He, J. Guo, X. Xie, H. Lin, L. Li.
A microstructural study of acid–activated montmorillonite from Choushan, China.
Clay Miner, 37 (2002), pp. 337-344
S. Maiti, A. Pramanik, S. Chattopadhyay, G. De, S. Mahanty.
Electrochemical energy storage in montmorillonite K10 clay based composite as supercapacitor using ionic liquid electrolyte.
J Colloid Interface Sci, 464 (2016), pp. 73-82
A. Jha, A.C. Garade, M. Shirai, C.V. Rode.
Metal cation–exchanged montmorillonite clay as catalysts for hydroxyalkylation reaction.
Appl Clay Sci, 74 (2013), pp. 141-146
E. Joussein, S. Petit, J. Churchman, B. Theng, D. Righi, B. Delvaux.
Halloysite clay minerals – a review.
Clay Miner, 40 (2005), pp. 383-426
N. Kohyama, K. Fukushima, A. Fukami.
Observation of the hydrated form of tubular halloysite by an electron microscope equipped with an environmental cell.
Clays Clay Miner, 26 (1978), pp. 25-40
P. Yuan, P.D. Southon, Z. Liu, C.J. Kepert.
Organosilane functionalization of halloysite nanotubes for enhanced loading and controlle drelease.
Nanotechnology, 23 (2012), pp. 375705
C.S. Yelleswarapu, G. Gu, E. Abdullayev, Y. Lvov, D.V.G.L.N. Rao.
Nonlinear optics of nontoxic nanomaterials.
Opt Commun, 283 (2010), pp. 438-441
R.D. White, D.V. Bavykin, F.C. Walsh.
The stability of halloysite nanotubes in acidic and alkaline aqueous suspensions.
Nanotechnology, 23 (2012),
I.K. Tonle, S. Letaief, E. Ngamenic, C. Detellier.
Nanohybrid materials from the grafting of imidazolium cations on the interlayer surfaces of kaolinite. Application as electrode modifier.
J Mater Chem, 19 (2009), pp. 5996-6003
A. Ahmed, Y. Chaker, El H. Belarbi, O. Abbas, J.N. Chotard, et al.
XRD and ATR/FTIR investigations of various montmorillonite clays modified by monocationic and dicationic imidazolium ionic liquids.
J Mol Struct, 1173 (2018), pp. 653-664
N.E. Heimer, R.E. Del Sesto, Z. Meng, J.S. Wilkes, W.R. Carper.
Vibrational spectra of imidazolium tetrafluoroborate ionic liquids.
J Mol Liq, 124 (2006), pp. 84-95
A. Ferry, L. Edman, M. Forsyth, D.R. MacFarlane, J. Sun.
NMR and Raman studies of a novel fast–ion–conducting polymer–in–salt electrolyte based on LiCF3SO3 and PAN.
Electrochim Acta, 45 (2000), pp. 1237-1242
T.-H. Wang, E.-Y. Lin, H.-C. Chang.
Pressure–dependent confinement effect of ionic liquids in porous silica.
Nanomaterials, 9 (2019), pp. 620
H.L. Ngo, K. Lecompte, L. Hargens, A.B. McEwen.
Thermal properties of imidazolium ionic liquids.
Thermochim Acta, 357–358 (2000), pp. 97-102
G.K. Dedzo, C. Detellier.
Characterization and applications of kaolinite robustly grafted by an ionic liquid with naphthyl functionality.
Materials, 10 (2017), pp. 1006
Y. Wang, C. Li, X. Guo, G. Wu.
The influence of silica nanoparticles on ionic liquid behavior: a clear difference between adsorption and confinement.
Int J Mol Sci, 14 (2013), pp. 21045-21052
C.P. Fredlake, J.M. Crosthwaite, D.G. Hert, S.N.V.K. Aki, J.F. Brennecke.
Thermophysical properties of imidazolium–based ionic liquids.
J Chem Eng Data, 49 (2004), pp. 954-964
E.P. Grishina, L.M. Ramenskaya, A.M. Pimenova, M.S. Gruzdev.
The influence of water on the physicochemical characteristics of 1–Butyl–3–methylimidazole bromide ionic liquid.
Russ J Phys Chem A, 82 (2008), pp. 1098-1103
L.M. Ramenskaya, E.P. Grishina.
Intensification phenomenon of weak ionic interactions of 1–butyl–3–methylimidazolium hexafluorophosphate ionic liquid macro–dispersed in poly(methyl methacrylate): FTIR spectroscopic evidence.
J Mol Liq, 218 (2016), pp. 133-137
C. Li, X. Guo, Y. He, Z. Jiang, Y. Wang, S. Chen, et al.
Compression of ionic liquid when confined in porous silica nanoparticles.
RSC Adv, 3 (2013), pp. 9618-9621
D. Membreno, L. Smith, B. Dunn.
Silica sol–gel chemistry: creating materials and architectures for energy generation and storage.
J Solgel Sci Technol, 70 (2014), pp. 203-215
E.P. Grishina, L.M. Ramenskaya, A.M. Pimenova.
The physicochemical properties of the low–Temperature ionic liquid silver bromide–1–Butyl–3–methylimidazolium bromide.
Russ J Phys Chem A, 83 (2009), pp. 1883-1886
M.N. Garaga, L. Aguilera, N. Yaghini, A. Matic, M. Perssonc, A. Martinelli.
Achieving enhanced ionic mobility in nanoporous silica by controlled surface interactions.
PhysChemChem Phys, 19 (2017), pp. 5727-5736
M. Galińnski, A. Lewandowski, I. Stępniak.
Ionic liquids as electrolytes.
Electrochim Acta, 51 (2006), pp. 5567-5580
W. Xu, E.I. Cooper, C.A. Angell.
Ionic liquids: ion mobilities, glass temperatures, and fragilities.
J Phys Chem B, 107 (2003), pp. 6170-6178
E.P. Grishina, A.M. Pimenova, L.M. Ramenskaya, O.V. Kraeva.
Electrochemical properties of 1–Butyl–3–Methylimidazolium bromide melt containing water impurities.
Russ J Electrochem, 44 (2008), pp. 1257-1262
Copyright © 2019. The Authors
Journal of Materials Research and Technology

Subscribe to our newsletter

Article options
Cookies policy
To improve our services and products, we use cookies (own or third parties authorized) to show advertising related to client preferences through the analyses of navigation customer behavior. Continuing navigation will be considered as acceptance of this use. You can change the settings or obtain more information by clicking here.