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Energy Material Advances / 2021 / Article

Research Article | Open Access

Volume 2021 |Article ID 7368420 | https://doi.org/10.34133/2021/7368420

Xinyi Liu, Zhou Yu, Erik Sarnello, Kun Qian, Soenke Seifert, Randall E. Winans, Lei Cheng, Tao Li, "Microscopic Understanding of the Ionic Networks of “Water-in-Salt” Electrolytes", Energy Material Advances, vol. 2021, Article ID 7368420, 9 pages, 2021. https://doi.org/10.34133/2021/7368420

Microscopic Understanding of the Ionic Networks of “Water-in-Salt” Electrolytes

Received09 Nov 2020
Accepted29 Dec 2020
Published28 Jan 2021

Abstract

“Water-in-salt” electrolytes with excellent electrochemical and physical properties have been extensively investigated. However, the structural understanding of the lithium bis(trifluoromethane sulfonyl)imide (LiTFSI) in water is still lacking. Here, we perform synchrotron X-ray scattering to systemically study the structural variation of TFSI anions in an aqueous solution under a variety of concentrations and temperatures. There are two different solvation structures in the solution: TFSI- solvated structure and TFSI- network. As the concentration increases, the TFSI- solvated structure gradually disappears while the TFSI- network gradually forms. Even at relatively low concentrations, the TFSI- network can be observed. Our experimental results show that these two structures can coexist at a particular concentration, and temperature changes will lead to one structure’s formation or disappearance. Also, the TFSI- network is the key to obtain a stable electrochemical window under relatively high temperatures.

1. Introduction

One key component of the Lithium-ion batteries (LIBs) is the electrolyte, which works as an indispensable ion conductor and an electron-insular between the anode and cathode [1, 2]. Conventional electrolytes usually consist of organic carbonate solvents that are highly volatile and flammable, and LiPF6 salt is chemically unstable [3]. These drawbacks hinder the development of next-generation batteries, requiring higher energy densities, wider operating temperatures, and better safety performance [4]. Compared with the traditional organic electrolytes, nonvolatile and nonflammable aqueous electrolytes could be a promising alternative electrolyte for the next-generation LIBs [5, 6]. However, the electrochemical stability window of aqueous electrolytes is narrow, and they cannot be used for most of the electrochemical couples in LIBs. Suo et al.’s group [7] reported a new aqueous electrolyte called “water-in-salt” (WIS) containing 21 m LiTFSI. The WIS electrolyte has a larger electrochemical stability window (~3.0 V), comparable to the organic electrolytes used in commercial LIBs.

This new finding facilitated the studies on WIS’s solvation structure and the transport properties in electrolytes, such as ionic conductivity [8] and transference number [9]. Combining infrared spectroscopy (IR) and molecular dynamics (MD), Lim et al. [8] found that even when the concentration of LiTFSI salt in water is as high as 21 m, there are still bulk-like water molecules acting as a medium for lithium-ion transport. Hydrated lithium ions move through those bulk-like water channels proposed as the lithium-ion conduction mechanism. Borodin et al. [9] investigated the ion solvation and transport in LiTFSI aqueous system with combined MD simulation, small-angle neutron scattering (SANS), and a variety of spectroscopic techniques. They found the disproportionation of cation solvation leads to a heterogeneous liquid structure, and the Li+(H2O)4 domain serves as a percolating channel for fast Li+ transports with a high lithium-transference number. With FTIR and MD simulation, Lewis et al. [10] revealed that Li cations contact with TFSI anions directly in the form of contact ion pairs that have a significant population at relatively high concentrations (larger than 3 m). Simultaneously, many anions are contacted directly in the interconnected ion network mediated by the Li cations.

However, the techniques employed in previous studies, such as NMR [11], Raman [12], and IR spectroscopy [13], are sensitive to the local molecular bonding and orientations and are a challenge to capture the whole structure of the forming clusters and aggregates. Small-angle X-ray scattering (SAXS) provides information about molecules’ size and shape and assemblies from 1 to 150 nm in solution [1417]. Recently, we investigated the solvation structure and dynamics of highly concentrated LiTFSI aqueous electrolyte combining SAXS with MD simulations [18]. We discovered heterogeneous structure features in 20 m LiTFSI aqueous solution. Because of this heterogeneous structure, the small number of anions present in the water domain causes a weak overall connection between ions. Such a weak connection promises the movement of Li+ in the water domain which is relatively free and results in high correlated transference numbers despite the high viscosity. Although many recent reports have investigated the structures of highly concentrated LiTFSI aqueous electrolytes, the solvation behaviors at different concentrations and temperatures are not entirely understood.

In this work, we conducted a SAXS study to investigate the solvation behavior of LiTFSI aqueous solutions in a wide range of concentration regime of 1 to 20 m. Also, the stability of these samples under different temperatures was studied by in situ SAXS measurements. TFSI anions can form two different structures, TFSI- solvated structure and TFSI- network. At low concentrations, the TFSI- solvated structure is the main solvated structure. TFSI- solvated structure and TFSI- network coexist as the concentration increases to the medium concentration. At high concentrations, only the TFSI- network remains. Also, we found that increasing temperature may promote the conversion between bulk water and interfacial water. The structural changes caused by the temperature are the reversible process. The electrochemical performance of different concentration LiTFSI aqueous solutions under different temperatures was also investigated. The temperature effect was more evident in the oxygen evolution reaction than that in the hydrogen evolution reaction. High concentration of LiTFSI solution is stable at high temperatures.

2. Materials and Methods

2.1. Sample Preparation

The electrolytes were prepared by dissolving the lithium bis(trifluoromethane sulfonyl)imide (LiTFSI, >99%, Sigma-Aldrich), and sodium bis(trifluoromethane sulfonyl)imide (NaTFSI, >97%, Sigma-Aldrich) in high purity water which conductivity is 18.2 MΩ × cm at 25°C. All the electrolytes were prepared by molality (mole-salt in kg-solvent) used by abbreviated concentrations (1 m, 2 m, 3 m, 5 m, 10 m, 15 m, and 20 m).

2.2. Small-Angle X-Ray Scattering

SAXS experiments were performed at the Advanced Photon Source (APS) 12ID-B and C station of Argonne National Laboratory. The 2D SAXS data were collected on a Pilatus 2 M area detector (DECTRIS Ltd.) and incident energy of 12 keV. The two-dimensional scattering images were radially averaged over all orientations to produce plots of scattered intensity versus scattering vector , where . The scattering vector, , was calibrated using silver behenate. The samples were loaded into 1.5 mm diameter quartz capillary tubes and sealed with epoxy for the SAXS measurement. To investigate the LiTFSI and NaTFSI aqueous solution structures under different temperatures, SAXS was investigated in situ. The samples were put in a multisample heater for capillary, which was designed by 12ID-B and C station of Argonne National Laboratory, and the gap between each capillary was 10 mm. This heater was set to change the sample temperature at 10°C/min.

2.3. Electrochemical Measurements

Cyclic voltammetry (CV) was carried out using CHI 600E electrochemical working station at a scanning rate of 10 mV/s. 316 stainless steel grid (200-mesh sieve), as working and counter electrodes, was cleaned ultrasonically in alcohol and then washed with high purity water several times and dried before measurement. The electrolytic cell was heated in a water bath, and a thermometer is used to measure the temperature.

2.4. MD Simulation Systems and Methods

MD simulations were performed on 1, 5, and 20 m LiTFSI aqueous solutions to investigate the transition of the solvation structure of TFSI- ion. The details of the MD system setups are listed in Table 1. The initial configurations of the MD simulations were packed using the PACKMOL code [19]. The simulation box is periodic in all three directions. The force fields of Li+ and TFSI- ion were taken from some recent works [20]. The TIP3P model was employed for the water molecules [21]. MD simulations were performed using the GROMACS package [22]. The simulations were first equilibrated under the NPT ensemble to stabilize the system density and energy for 30 ns. Then, a 100 ns trajectory was generated for each simulation under the NVT ensemble [23]. The last 50 ns trajectory was used for the related analysis. More simulation details were archived in our recent publications.


Nominal concentration ()MD concentration ()LiTFSI numberWater number

10.991005600
55.055005500
2019.8220005600

m = mol/kg.

3. Results

3.1. The Evolution of Electrolyte Structure with Varying LiTFSI Concentration

It should be noted that Li+ cannot be observed directly through SAXS measurement due to its small scattering factor [15]. Therefore, all information obtained from SAXS measurement is related to the structure of the large TFSI-. To fully understand the solvation structure, we systemically changed the LiTFSI concentrations and measured them with SAXS. The SAXS profiles of different LiTFSI concentrations at room temperature are shown in Figure 1(a). We observe two peaks: one is marked as Peak a in the low part, and the other is labeled as Peak b in the vicinity of 0.99 Å-1. As the concentration gradually increases, Peak a position shifts to a higher , which indicates the average distance or spacing between TFSI ions becomes shorter. Also, the intensity of this peak decreases with increasing concentration. At a high concentration of 20 m, the peak disappears. However, Peak b begins to appear at a relatively low concentration of 2 m and its position shifts slightly to a higher below 10 m and then remains unchanged as the concentrations increase to a high concentration of 20 m. This suggests that the average spacing between TFSI- networks becomes smaller, and then, there is no change.

The spacing of the two peaks can be calculated using , and its relationship with concentrations is shown in Figure 1(b). There are three concentration regimes, (I) low concentration regime, (II) medium concentration regime, and (III) high concentration regime. At regime I (<2 m), only Peak a can be observed and spacing is around 18.5 Å. At regime II (2 m~15 m), Peak a and Peak b coexist. The spacing of Peak a gradually decreases from 16.2 to 12.0 Å, while the spacing of Peak b remains at 6.4 Å. At regime III (>15 m), only Peak b can be observed. The two peaks represent two different TFSI- solvation structures.

Initially, we assigned Peak b to the charge-ordering of LiTFSI (TFSI- and Li+), which is widely used for ionic liquid and molten salt [13]. However, we found Peak b position for NaTFSI solution is the same as LiTFSI (in the later section), which means the cation does not play an essential role for the Peak b. Otherwise, it should be shifted to a lower , considering that the radius of Na+ is larger than that of Li+. This result indicates that other TFSI- structures may contribute to this peak. Other possible structures are as follows: (1) TFSI- and TFSI- are directly in contact, and (2) TFSI- is connected to water molecules (i.e., TFSI-···HOH···TFSI-). The spacing between TFSI- network is 6.4 Å, which is larger than that of the pure TFSI-Li-TFSI distance [14], as shown in Figure 1(b) ( is the spacing of pure LiTFSI obtained from reference, which is 5.3 Å [24]). Therefore, we attribute the formation of this peak to the TFSI- network formed by the bridging of water molecules.

As shown in Figure 1(b), the spacing of Peak a is much larger than pure TFSI-TFSI distance and TFSI- networks, indicating the solvation structures are different. We named this solvation structure as the TFSI- solvated structure. Interestingly, we did not observe Peak a when we dissolved LiTFSI in different concentrations of organic solvents (including acetonitrile and propylene carbonate) (Figure S1). The reason is that the water molecules are bipolar while other solvents are not. In an aqueous solution, both cations and anions can be well solvated by water. However, in organic solvents we studied, only cations can be solvated well while anions remain unsolvated and remain relatively free [2527].

Unlike only one peak is observed at low (1 m) and high concentration (20 m), we can observe both Peak a and Peak b at medium concentrations (2 m ~15 m), indicating both the TFSI- solvated structure and TFSI- network coexist. As the concentration of LiTFSI increases, more TFSI anions will extract free water molecules from the outermost layer, resulting in a shorter distance between TFSI-. As a result, Peak a starts to move to a higher . Also, as the concentration increases, TFSI anions begin to form TFSI- networks leading to the appearance of Peak b, and the intensity increases because of the increased number of TFSI anions in the TFSI- networks. The number of TFSI- solvated structure becomes less, resulting in a decrease in the intensity and disappearance of Peak a. Eventually, only Peak b exists at high concentrations, which indicates that only the TFSI- network exists.

The driving forces for the formation of these two different solvated structures are further investigated. Combining our current SAXS work and Lim et al.’s [8] previous IR work, we believe that these two solvated structures are driven by two different hydrogen bonds caused by two different types of water. They have demonstrated two different kinds of water in LiTFSI aqueous solutions: one is bulk water that has hydrogen bonding with each other, and the other is interfacial water, which can form another hydrogen bonding with TFSI ions. From IR spectra, it can be seen that as the LiTFSI concentration gradually increases from 1 to 21 m, the intensity of the bulk water peak decreases and the intensity of interfacial water increases. Meanwhile, the bulk water peak has a significantly blue shift, while the interfacial water peak position remains almost unchanged. These results are consistent with our SAXS study. As the concentration increases, Peak a shifts to a high until it entirely disappears, while the position of Peak b remains unchanged. Therefore, we believe that the TFSI- solvated structure is due to the solvation of bulk water, while the formation of TFSI- networks is due to the interfacial water and TFSI-. These two structures have been captured with MD simulation, which is shown in Figures 2(a) and 2(b). The concept of interfacial water and bulk water has been well studied in the protein/water system, where the interfacial water forms a strong hydrogen bonding with protein [28].

3.2. Effect of Changing Temperature

TFSI- solvated structures are mainly caused by the hydrogen bonding between the bulk water, and TFSI- networks are formed through the hydrogen bonding between the TFSI- and the interfacial water. Therefore, we should be able to observe the change in these two structures if the solution is exposed to external stimuli such as temperature because it has been reported that the hydrogen bonding between the bulk water molecules can be destroyed with increasing temperature [29]. To verify this hypothesis, we conduct in situ SAXS studies of LiTFSI at different concentrations and temperatures in aqueous solutions. At low, medium, and high concentrations, we observe three different results. At high concentration, Peak b remains unchanged as temperature varies (Figure 3(a)), indicating that the spacing has no change (Figure 3(b)).

However, at medium concentrations of 5 m, we observe a different phenomenon, as shown in Figure 3(c). As the temperature gradually increases, Peak a shifts to high , and the intensity decreases, and Peak b shifts to low with an increase in intensity. The spacing from both structures is shown in Figure 3(d). Increasing the temperature will break the hydrogen bonding of bulk water molecules. These new water molecules may move into three-dimension TFSI- networks and to reorganize with the existing interfacial water to form a new type of interfacial water, which causes Peak b to move to low and increase in intensity. Conversely, because of the bulk water the solvated TFSI- structures becomes less, Peak a shifts to a high and the intensity decreases. We found the same trend for another medium concentration of 10 m, as shown in Figure S2.

At low concentration (1 m), the SAXS profiles from 25 to 65°C are presented in Figure 3(e), and two peaks can be observed. This means that even at relatively low concentrations, the TFSI- networks could form through hydrogen bonding between interfacial water and TFSI-. As the temperature gradually increases, the intensity of Peak a decreases while the intensity of Peak b increases, which is the result of the relative population of the two TFSI- species gradually changing with increasing temperature. Heating will break the hydrogen bonding from bulk water and may promote the formation of new interfacial hydrogen bonding. As a result, the TFSI- solvated structures become less and more TFSI- interacts with interfacial water to form TFSI- network. The reduced number of solvated TFSI- causes Peak a shifts slightly to the low [28], and the value is shown in Figure 3(f).

It should be noted that this temperature effect is entirely reversible regardless of the concentration of LiTFSI. As shown in Figures 3(b), 3(d), and 3(f), the value of the LiTFSI aqueous solutions under different temperatures is reversible. For example, at a medium concentration of 5 m as shown in Figure 3(d), the values of Peak a and Peak b are 13.6 Å and 6.3 Å at 25°C, respectively, and they change to 12.8 Å and 6.6 Å as the temperature rises to 65°C. When the temperature is lowered to 25°C, the value returns to 13.6 Å and 6.3 Å. We can observe the same phenomenon for the low (1 m), medium (10 m) (Figure S2), and high concentration (20 m) LiTFSI aqueous solutions.

Next, we tested NaTFSI in an aqueous solution and found similar phenomena as LiTFSI aqueous solutions. From Figure 4(a), we can observe the two peaks coexist. As the concentration increases, Peak a moves to high and its intensity decreases while Peak b appears at a concentration of 3 m and its position ( Å-1) remains almost no change. Unlike LiTFSI solution, it only shows low and medium concentration regimes (Figure 4(b)) because of the lower solubility of NaTFSI. At a medium concentration of 5 m (Figure 4(c)), Peak a shifts to higher with a decreased intensity and Peak b shifts to lower with an increase in intensity as temperature increases. A similar trend is observed for other medium concentrations of 3 m and 7 m (Figure S3 and S4). For the low concentration NaTFSI aqueous electrolyte (1 m), as shown in Figure 4(e), the intensity of Peak a decreases while the intensity of Peak b increases. We also can observe that Peak a shifts to a lower with the temperature increasing, which is the same as 1 m LiTFSI aqueous solution. This temperature effect is also completely reversible regardless of the concentration of NaTFSI. As shown in Figures 4(d) and 4(f), the variation of the value of the NaTFSI aqueous solutions under different temperatures is reversible. Based on the SAXS profiles of LiTFSI and NaTFSI aqueous solutions, we find that TFSI- salts with cations in the same group have the same behavior as a function of concentration and temperature.

3.3. Electrochemical Stability Test under Different Temperatures

From SAXS results at different temperatures, we can observe the structural changes of LiTFSI aqueous solutions at different concentrations. We believe that this structural change may lead to different electrochemical performances. Therefore, we investigated the electrochemical stability window of low (1 m), medium (5 m), and high (20 m) LiTFSI aqueous electrolytes under different temperatures, as shown in Figure 5. The electrochemical window was evaluated on the stainless steel electrode by cyclic voltammetry (CV). Compared with 1 m LiTFSI aqueous electrolyte, the overall stability window of 20 m LiTFSI aqueous electrolytes has been expanded to ca. 3.0 V. The onset potential of the hydrogen evolution reaction (HER) and oxygen evolution reaction (OER) shifts to more negative and positive values, respectively. The phenomenon is consistent with previous finding by Suo et al. [7]. With increasing the temperature, the electrochemical stability windows for 1 m, 5 m, and 20 m LiTFSI aqueous electrolytes were narrow. Since the positively charged electrode in the OER will contact an excess of TFSI anions, the temperature effect will be more pronounced on the anode side. We can observe from Figure 5 that the change of current on the OER of the 1 m LiTFSI aqueous electrolytes is more significant than that of 5 m and 20 m LiTFSI solutions. For a 20 m LiTFSI aqueous electrolyte, the current changes from 0.002 A/cm2 to 0.003 A/cm2 under 1.8 V as the temperature increases from 25°C to 65°C, but for 1 m LiTFSI aqueous electrolyte, the current changes from 0.02 A/cm2 to 0.07 A/cm2. The rate of change of 1 m LiTFSI aqueous electrolytes is 2.5 times that of 20 m LiTFSI aqueous electrolytes (the current changes from 0.02 A/cm2 to 0.04 A/cm2) and 5 times of 20 m LiTFSI aqueous electrolytes (Table S1). This phenomenon can be ascribed to the gradual formation of hydrogen bonding between water molecules and TFSI anions with the concentration increases.

Water molecules forming the hydration sphere of lithium ions present at the electrode surface can be stripped off and reduced to form hydrogen. From Table S1, the current change rates of 1 m, 5 m, 10 m, 15 m, and 20 m LiTFSI aqueous solutions under -1.8 V HER onset potential are almost the same (150%), which means there are many free water molecules which solvated Li+ in the high concentration LiTFSI aqueous electrolyte at the cathode electrode. A schematic presentation of the species presents negatively and positively charged electrodes in low and high concentration shown in Figure S5.

4. Discussion

In summary, we studied LiTFSI solutions with synchrotron X-ray scattering technique by systemically varying the LiTFSI concentration and temperature. According to SAXS results, LiTFSI aqueous solutions can be divided into three concentration regimes: low concentration, medium concentration, and high concentration. At a low concentration solution regime, only TFSI- solvated structures exist at room temperature. However, the TFSI- networks can be formed with increasing temperature. For a medium concentration solution regime, two structures (TFSI- solvated structure and TFSI- network) coexist. There is only one structure at room temperature at a high concentration solution regime, TFSI- network, where all TFSI- have been involved in forming TFSI- networks. TFSI- network structure at high temperature even improves the electrochemical high-temperature stability.

Data Availability

All data needed to evaluate the conclusions in the paper are presented in the paper and/or the Supplementary Materials. Additional data related to this paper may be requested from the authors T. L.

Conflicts of Interest

The authors declare that there is no conflict of interest regarding the publication of this article.

Acknowledgments

This work was supported as part of the Joint Center for Energy Storage Research, an Energy Innovation Hub, funded by the U.S. Department of Energy, Office of Science, Basic Energy Sciences. This research used resources of the Advanced Photon Source, a U.S. Department of Energy (DOE) Office of Science User Facility operated for the DOE Office of Science by Argonne National Laboratory under Contract No. AC02-06CH11357.

Supplementary Materials

Figure S1: SAXS profile for the (a) acetonitrile and (b) propylene carbonate at different concentrations under room temperature. Figure S2: (a) SAXS profile for the 10 m LiTFSI aqueous solutions at different temperatures. SAXS curves for the 10 m LiTFSI aqueous solution at various temperatures shown in (b) during heating/cooling cycles. Figure S3: (a) SAXS profile for the 7 m NaTFSI aqueous solutions at different temperatures. SAXS curves for the 7 m NaTFSI aqueous solution at various temperatures shown in (b) during heating/cooling cycles. Figure S4: (a) SAXS profile for the 3 m NaTFSI aqueous solutions at different temperatures. SAXS curves for the 3 m NaTFSI aqueous solution at various temperatures shown in (b) during heating/cooling cycles. Figure S5: schematic representation of the ionic environment close to the electrode surface under polarization for the low and high concentration LiTFSI aqueous electrolytes. Table S1: current density of 1 m, 5 m, 10 m, 15 m, and 20 m aqueous electrolytes on nonactive electrolytes under different temperatures. (Supplementary Materials)

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