Performance Evaluation of Composite Electrolyte with GQD for All-Solid-State Lithium Batteries

1  Introduction

Recently, the demand for high-performance batteries has exploded, and all-solid-state lithium metal batteries are receiving great attention to satisfy the demand for high density energy systems. All-solid-state lithium batteries are replacing liquid electrolytes. Because there is no risk of battery explosion, and because high energy density is possible, such solid-state batteries represent a new generation of battery technology [1–3]. The capacity of a battery is determined by the quantity of Li+ ions that move, and the Li+ ion conductivity of the electrolyte affects the charging and discharging rates of the battery [4–6]. To achieve high energy density, it is important to develop a battery with high voltage and large capacity; for high output, it is necessary to increase the quantity of Li+ ions and electrons that move [7–10]. Conventional rechargeable lithium-ion batteries have revolutionized powertrains for electric vehicles. Additional innovations include small energy storage devices and eco-friendly wearable devices. However, with the move toward usage of solid materials, the current level of lithium-ion battery structure has limitations in energy storage capacity and stability.

A modified metal electrode in which the lithium (Li) to host material ratio is extended is capable of more than doubling the theoretical energy density at the heterogeneous interface. Among anode materials, Li metal has high theoretical specific capacity and low electrochemical potential. Nevertheless, the heterogeneous reaction properties at the heterogeneous interface lead to the spontaneous formation of inhomogeneous and brittle solid electrolyte interfaces (SEIs), also known as dendrites, and electrical short-circuit reactions upon rupture [11–14]. This issue not only poses a safety risk due to side reactions caused by Li dendrites, but also creates a vicious cycle of low coulombic efficiency and shortened lifespan. Existing studies on Li metal stabilization have suggested using additives to improve Li+ ion transport and control the metal surface, or the development of solid electrolytes that can act as physical barriers to dendrite propagation [15–20].

Here, we use a low-dimensional quantum dot structure to control the Li+ ion flux and Li deposition; this structure suppresses dendrite formation and forms Li diffusion interfaces based on lithiated graphene quantum dots (Li-GQDs). The use of graphite and carbon nanotubes for Li dendrite suppression has been explored, but less attention has been paid to the role that a modified interface between Li and carbon can contribute to battery structure stabilization. A positively charged, low-dimensional GQD matrix structure was obtained through a chemical exfoliation process; this structure has fewer defects than the bulk structure and the active site are reactive. Here, by exploring the heterojunction between Li and GQDs, in-depth study of the Li–carbon hetero-structure was conducted to promote dendrite inhibition. The spontaneous reaction of Li metal and the dissimilar materials when no electric potential is applied indicates the potential for passivation of the Li anode. Li can form an alloy upon contact with a non-metal or intercalated Li+ ions, maintaining charge properties and reducing stacking defects. Because it is only activated at high potentials, the carbon structure as a hetero-interfacial layer enables selective conversion of Li+ ions by preventing reaction of the layer with larger anions [21–24].

In this work, we formed a passivation structure for the Li anode metal layer using GQD-based Li+ ion control. Because the contact between particles is not smooth due to pores between the defects present inside the electrode and the solid electrolyte, the effective contact area through which lithium ions move is low, making it difficult to realize high battery performance. However, this new technology designed using a low-dimensional structure maximizes the effective contact area between cathode material and solid electrolyte so that lithium ions can move smoothly; a low-defect GQD layer is formed. By using a solid electrolyte coated with GQD layer to fill in defects and pores inside the electrode during device fabrication, the interfacial resistance during lithium ion movement was effectively improved [25–27]. We have demonstrated a heterointerface design that incorporates a low-dimensional GQD layer into a heterostructure matrix to provide robust interfacial stabilization. The Li metal structure is shown in Fig. 1b, in which it can be seen that the GQD layer with high mass density was wetted with a highly concentrated electrolyte. Li dendrite growth was effectively suppressed due to the Li+ flux of the modified Li metal interface and the excellent mechanical strength of the homogeneous GQD layer.

Figure 1: Schematic of Lithium (Li)-Ion battery mechanism, lithium dendrite in all-solid-state batteries: growth mechanisms

Physical contact between Li and GQD layers resulted in spontaneous reduction of the modified GQD layers, which was balanced by the control of Li+ ions. It was hypothesized that the Li-GQD hetero-interface acts as a mediator to control Li diffusion and prevent the growth of dendrites. During battery charging, Li+ ions of the Li-GQD layer were deposited on the Li metal surface and then replaced with Li+ ions of the electrolyte. The reduction change of the GQD layer was confirmed only in the region in close contact with the Li metal; spontaneous lithiation proceeded due to the generation of an electrochemical potential at the heterogeneous interface and the Fermi level difference. The heterostructure of the Li-GQD layer did not change under potential-induced lithiation, and no bulk deposits or leakage defects were observed, indicating the formation of uniform SEI-layer Li-GQD thin film. To our knowledge, this is the first report of a low-dimensional GQD-based all-solid-state battery operating stably at room temperature.

2  Experiment

2.1 Preparation of Graphene Quantum Dots (GQDs)

Graphene was synthesized on Cu foil in a thermal furnace at 950°C for 7 min under Argon (Ar): Hydrogen 2 (H2): methane (CH4) mixed-gas flow. Subsequently, a pre-prepared poly (methyl methacrylate) (PMMA, Sigma Aldrich) solution was dropped all over the graphene surface, spin-coated at 5000 rpm for 45 s, and then heat treated on a hot plate at 160°C for 3 min. The PMMA solution was prepared by adding 0.5 g PMMA powder to 15 mL chlorobenzene (Sigma Aldrich) and stirring the mixture at 65°C for 8 h. The Cu was removed by dipping the PMMA/graphene/Cu foil stack in 1 mole (M) Iron (III) chloride (FeCl3) solution (Sigma Aldrich). The PMMA/graphene stack was then transferred onto glass or polyethylene terephthalate (PET) substrate and heat-treated at 110°C for 3 h. Finally, the PMMA was dissolved by acetone. The following processes were used to fabricate GQDs. Graphene oxide (GO) was prepared from graphite powder using the Hummers method. GO was deoxidized in a horizontal furnace at 350°C–450°C for four hours under Ar to produce reduced graphene oxide powder. About 5.0–6.5 g of graphene oxide powder was oxidized by ultrasonication in concentrated 15 mL sulfuric acid (H2SO4) and 40 mL nitric acid (HNO3) for 20 h. In addition, 350 mL deionized water was used to dilute the mixture. After cooling to room temperature, the resulting powder was redispersed in 35-mL DI water for two hours under ultrasonication. Then, by filtering the resulting suspension through a 200 nanometer (nm) nano-porous membrane, a brown solution was separated. Since the colloidal solution still contained some large graphene nanoparticles (<200 nm) emitting weak blue fluorescence, it was further filtered overnight in a dialysis bag with a cutoff of 3500 dalton (Da) molecular weight, thereby producing strongly fluorescent GQDs. The GQDs were separated into different sizes using several dialysis bags of 1000–50,000 Da and a 20-nm nano-porous membrane.

2.2 Cell Fabrication

To fabricate solid-state Li batteries (SSLBs)-based nano-structure devices, after the direct synthesis of the extracted graphene, graphene quantum dots (GQDs) of each shape were directly grown on patterned Li electrodes on a copper (Cu) thin films through a modified chemical vapour deposition (CVD) method. After washing the composite GQD layer in a deionized water cleaning process, heat treatment was performed. Coin cells were assembled in glove box using CR2032 type shells. The modified PEO electrolyte membrane was prepared by drying a mixture of polyethylene oxide (PEO), Lithium bis(trifluoromethanesulphonyl) imide (LiTFSI) powders, and acetonitrile in a vacuum oven at 50°C for 24 h [28–30]. The symmetrical cells with GQD-PEO-LiTFSI hybrid paste were fabricated with two Li disks (thickness of 200 µm) and a donut spacer (thickness of 25 µm). GQD-PEO-LiTFSI hybrid paste was placed in the middle of spacer. The interlayer was built with 10 µL commercial LE (1 m LiPF6 in ethylene carbonate/diethyl carbonate mixture solvent) or 15 mg paste hybrid on each side of pellet. The interlayer in full cells was built in the same way for symmetric cells [31–33].

2.3 Characterization

Plane- and cross-sectional-view images of the materials and devices were obtained by field emission scanning electron microscopy (FE-SEM, Carl Zeiss, model LEO SUPRA 55). Morphologies of GQDs were analyzed using an High-resolution Transmission Microscopy (HRTEM) (FEI Tecnai F30 S-Twin). To make the HRTEM specimens, the GQDs were dispersed in DI water, drops of which were then put on C- or SiO-coated Cu grids (Tedpella, Inc., Redding, CA, USA) and mica substrate, respectively. The current-voltage (I–V) curve of the device was analyzed using an electrical and electronic workstation (Keithley 2400). Current density-voltage (J-V) characteristics were monitored by forward/reverse scans at 200 ms and 10 mV under standard conditions. The ionic conductivity of the electrolytes was measured on a dielectric spectrometer in the temperature range from −20°C to 100°C in a gold-plated cell with Teflon spacer. Lithium samples were transferred from glovebox to the chamber in a vessel without explosion in air. Raman spectra were observed from a Bruker IFS66 Fourier Transform spectrometer with a FRA106 Raman module. All the heating tests were carried out in Ar-filled glove box. Electrochemical impedance spectroscopy was performed on a Reference 600 (Gamry Instruments) over a frequency range of 0.01 to 1 MHz and the perturbation amplitude was 10 mV.

3  Results and Discussion

3.1 Li-Ion Battery Mechanism and Lithium Dendrite in Solid-State Batteries

As shown in Fig. 1, a lithium secondary battery consists of a positive electrode, an electrolyte, and a gold electrode, a polymer separator with thickness of tens to hundreds of micrometers is positioned inside a liquid electrolyte comprising organic solvent and lithium salt. Movements of lithium ions are in opposite directions during charging and discharging. In other words, during discharge, Li+ ions move from the negative to the positive electrode, and electrons generated as lithium ionizes also transfer in the same direction. The cause of this Li+ ion migration is the system’s pursuit of chemical stability against the potential difference between the two electrodes. Li dendrite growth, which unexpectedly penetrates the separator during charge/discharge operation and causes battery failure and fire, has severely limited the use of next-generation devices as well as various high-performance system applications. Therefore, next-generation batteries require a transition from the existing layered structure to a modified electrode structure that can control the intercalation of lithium between graphite layers.

The electrical properties of the sample according to the I2 content of the modified poly (ethylene oxide) (PEO) structure are shown in Fig. 2a. For ionic modulation of the PEO structure, the ionic conductivities of electrolytes with different GQD-I2 contents (1, 1.5 and 2 wt% of PEO-LiTFSI) were measured. It was found that the ionic conductivity of the sample structures depends on the temperature [34]. Compared with pristine PEO-LiTFSI, when 1.5 wt% I2 was added to the PEO-LiTFSI electrolyte at 50°C, the resulting electrolyte saw its ionic conductivity increase from 9.34 × 10−6 to 6.28 × 10−5 S cm−1. The ionic conductivity tends to increase with increasing temperature of the modified PEO-GQD based electrolyte.

Figure 2: (a) Ionic conductivities of the GQD-PEO-based electrolyte with Iodine (I2) contents. (b) Raman spectra of pristine PEO and GQD-modified PEO- Lithium bis(trifluoromethanesulphonyl) imide (LiTFSI)-1.5 weight (wt) %

In Fig. 2b, Raman spectroscopy was performed to investigate the effect of I2 on the ionic conductivity. The characteristic band at 190 cm−1 belongs to I2, but this characteristic peak was not observed in the GQD-modified PEO-LiTFSI-1 wt % I2 sample. In contrast, in the GQD-modified PEO-LiTFSI-1.5 wt % I2 sample, a significant band between 130 and 200 cm−1 was observed due to the activation of symmetric stretching mode of the I3-atomic structural unit. This indicates that iodine exists in I3 rather than I2 form in the GQD-modified PEO polymer structure. Through spectroscopic analysis of I2 dissolved in acetonitrile, the properties of I3− were confirmed. Unlike the 145 cm−1 peak, related to I3, the characteristic 190 cm−1 peak of I2 was dominant. According to this result, I3− is mainly generated by interaction between I2 and PEO, in a reaction controlled by GQD.

When I2 was dissolved in acetonitrile, it received electrons from the modified PEO, an electron donating structure, and generated I− through a reduction reaction. As a result, I− ions generated I3, an anion, through a chemical reaction with I2. The interaction between PEO and I2, as well as the donor-acceptor relationship between iodine species and acceptor, is widely known through the results of previous studies on organic molecular phenomena in water-insoluble solvents. The chemical movement of hydrogen atoms according to different amounts of I2 in the modified PEO structure (PEO-x wt % I2, x = 2, 4, 6) is smaller than that in the original PEO structure, and results show that chemical movement increases as the density of I2 increases. This indicates the complex action at the interface produced by GQDs between I3-units and PEO molecules.

As a result, the I2 surface structure modified by GQD reduces the crystallinity of PEO and promotes electron transfer in the PEO hetero-interface structure. GQD-modified I3− interacts with the carbon-oxygen of the electron-donating substitutes to effectively weaken the bonding force between Li+ ions and other oxygen groups, promoting efficient transport of Li+. As a result, this process contributes to the enhancement of the ionic conductivity of the GQD-modified electrolyte. Compared with that of the pristine PEO structure, the diffraction intensity of modified PEO-LiTFSI decreased, indicating that there was a change in crystallinity. It was confirmed that I2 doping can significantly reduce the effective contact resistance of the modified GQD-PEO, and can control the crystallinity through the action of GQD. In addition, GQD-based I2 doping does not affect the electrochemical behavior of the composite electrolyte. We investigate the electrochemical properties of various hetero-interfaces used to stabilize Li metal anodes of Li batteries with symmetric structure. All devices are rated at a fixed capacity of 0.2 mAh cm−2 and a current density of 0.2 mA cm−2.

3.2 Solid-State Lithium Batteries based on Nanocomposite Electrolyte with GQD

Fig. 3 shows the cell using pristine PEO-LiTFSI electrolyte had an average overpotential of 120 mV and exhibited a limited cycle life of 385 h. Further analysis of the micro-surface morphology of the Li layer by scanning electron microscopy (SEM) revealed that a sharp drop in overpotential occurred during repeated charge/discharge cycles, indicating a short circuit. A porous Li metal surface can be observed in Fig. 3d. The void defects inhibit Li+ ion diffusion and accelerate formation of Li dendrites in the hetero-interface structure [35]. As a result, device performance such as lifetime and durability deteriorated. In contrast, devices using GQD-modified PEO-LiTFSI-x wt% I2 (x = 1 and 1.5) electrolytes had improved cycling stability. Through the interfacial Li plating and stripping process, dense structural defects were improved at the interface between the GQD-modified PEO-LiTFSI-1.5 wt% I2 electrolyte and Li metal.

Figure 3: (a and c) Voltage profiles of symmetric cells with different electrolytes interlayer operated at a current density of 0.1 mA cm−2 and 45°C. (b and d) Morphology of cycled Li metal anodes. Top view SEM images of cycled Li anode using pristine and GQD-PEO-LiTFSI-1.5 wt% I2 electrolyte in low-magnification. Scale bar, 500 nm

In particular, the GQD-modified PEO-LiTFSI-1.5 wt % I2 electrolyte had a long lifetime of more than 550 h and a rather low average overpotential of 55 mV, leading to negligible polarization. The Li metal anode showed a generally uniform surface and stable cycling performance without serious defects on the surface or at the interface. The GQD-modified PEO-LiTFSI-1.5 wt% I2 electrolyte presents a low polarization of 0.2 mA cm−2. Moreover, the battery performance of devices composed of electrolytes containing 1.5 wt % I2 ions was superior to those containing I2 ions at percentages of 0.5, 1.0, and 3 wt %. However, I3- reacted chemically with the unstable Li structure, composed disproportionately of Li interfaces and GQD-Li2O. The unstable structure of the I3-ion caused corrosion of the active Li structure, indicating contact issues between Li layer and GQD and poor battery performance.

Likewise, a moderate reaction of GQD-modified iodine to reduce overpotential is confirmed with different current densities. This indicates a significant enhancement effect of GQD-modified I2-ion on the interfacial stability between the GQD-electrolyte and the Li layer.

To confirm the mechanism of GQD-modified I2 doping on the surface and interfacial stability, observed the morphology and composition of the interface at atomic scale by measuring (transmission electron microscopy) TEM. The low-magnification TEM image in Fig. 4a shows the interface observed without I2 doping. In the high-resolution-TEM (HR-TEM) images of the blue and yellow square region in Fig. 4b, crystalline Li layer and GQD-Li2O regions are visible. In addition, the high oxygen content and oxygen atoms at the interface between the pristine PEO-LiTFSI electrolyte and the Li anode formed a Lithium oxide (Li2O) structure [36]. Compared with the case without I2 doping, it did not change the defect structure at the interface. In the HR-TEM images in Figs. 4c and 4d, Li2O and GQD nanocrystal regions and an amorphous layer can be seen to be mixed, and an I-doped organic-inorganic layer can be observed.

Figure 4: (a and b) TEM images of the distribution of the SEI components with GQD-PEO-LiTFSI-1.5 wt % I2 electrolyte. Scale bar, 500 nm, 20 nm, respectively. (c and d) corresponding high-resolution transmission electron microscopy (HR-TEM) images obtained in the blue and yellow rectangular region of (b), respectively. Scale bar, 2 nm

Crystal structures and grid spacing corresponding to Li, Li2O, Lithium iodide (LiI), and Lithium iodide oxide (LiIO3) were can be observed in Figs. 4c and 4d. An Li layer with lattice spacing of 2.48 Å. The lattice spacings of 2.71 and 2.46 Å corresponded to the Li2O (111) and GQD planes. The LiI layer distributed on the surface of the Li2O structure and Li2O domains has been recognized as a solid polymer electrolytes (SPEs) interfacial reactant with Li. The LiI structure forms due to the rapid reaction between I3- and Li/GQD-Li2O. In addition, the formation of LiIO3 took place via different interfacial reactions according to the I3-doping and Li2O content. This can be confirmed by the contents of the various nanostructure at the interface after Li formation. The TEM results indicate that GQD-based I2 doping can achieve uniform formation of Li layer by construction of modified SEI interfacial layer (LiI/GQD-LiIO3). Controlled I3 reacts with Li and Li2O at the interface to generate activated Li+ ions and this leads to a defect-free stable interface, which can enhance Li+ ion conduction at the heterostructure.

The solid-state batteries with GQD-PEO-LiTFSI-1.5 wt% I2 electrolyte also indicate a good rate capability, as shown in Fig. 5a, High capacities of 152, 148, and 146 mAh g−1 are delivered at, respectively, 50, 100, and 200 μA cm−2. The capacity recovers to 149 mAh g−1 when the current returns to 100 μA cm−2. Further evaluation of the electrochemical stability of the GQD-PEO layer was conducted with a cycling test in an GQD-PEO-LiTFSI-1.5 wt% Li cell at 150 μA cm−2, a stabilized capacity of 149 mAh g−1 is delivered after an activation reaction in the first several cycles.

Figure 5: Electrochemical performance of solid-state batteries with GQD-PEO-LiTFSI-1.5 wt% I2 electrolyte. (a) cycling stability, and (b) Raman characterization of the interphase between GQD-PEO electrolyte and Li metal

In Fig. 5b, Raman spectra results show the composition of the modified atomic layer interface and the chemical reaction of the iodine species. The components of the intermediate phase appearing in the PEO-based device structure are Li2O and an amorphous composite polymer; this intermediate phase becomes a large source of resistance to ion conduction. With GQD-modified I2 doping, there was no significant change in oxygen content at the heterostructure interface, and the oxygen content of Li2O, compared to that of Li6.4La3Zr1.4Ta0.6O12, decreased. As a result, the composition of the GQD-based I-doped hetero-interface, which can control defects between the GQD-modified electrolyte and Li structure.

The properties of elemental iodine on the electrolyte interface before and after the repeated operation indicated that the structure of I2 deteriorated and the amount of I- component increased, indicating that the LiI3 moiety was reduced to an LiI layer by Li atoms [37]. The change of the I3-structure in the modified GQD-PEO-LiTFSI-1.5 wt% I electrolyte was measured by Raman spectra analysis during charge/discharge cycles of transparent LiFePO4/PEO-LiTFSI-1 wt% I2 GQD/Li devices. A pathway to stabilize Li was realized by spontaneous formation of a modified LiI layer between the composite polymer/GQD/Li hetero-interface. In the signal range of 0 to 200 cm−1, a peak appeared at 128 cm−1, which corresponds to the symmetric stretching mode of the I3-structure. The peak at 128 cm−1 decreases during the charge/discharge cycle, indicating that modified I3− reacts with Li and Li2O to form a hetero-interfacial passivation layer of LiI and LiIO3. The reduction of modified I3− by Li and Li2O can be described by the Li+ and IO3-ion reactions.

To design a hetero-interface with improved structural reliability between the Li metal anode and the GQD-modified PEO-LiTFSI-1.5 wt% I2 electrolyte, a modified transparent LiFePO4 anode, Li metal anode, and electrolyte were fabricated at 50°C and evaluated via SSLB. The LiFePO4/Li device to which the pristine PEO-LiTFSI electrolyte was applied showed rapid capacity deterioration, with a capacity retention rate of 43.6% after 100 cycles. In contrast, by applying the GQD-modified electrolyte, the LiFePO4/Li device showed moderate capacity retention and stable movement at 0.5 C, as can be seen in Fig. 6a. After 100 cycles, the GQD-modified device provides a specific capacity of 148 mAh g−1 and a capacity retention of 94.8%. Moreover, batteries using modified electrolytes with GQDs have capacities higher than those of pristine devices. As a result, the GQD-controlled iodine matrix significantly increased the effective area of Li+ ion transport because the hetero-interface and electrolyte inside contribute to battery capacity enhancement [38].

Figure 6: Electrochemical performances of solid-state Li battery. (a) Charge curves of GQD-PEO-LiTFSI-1.5 wt% I2/Li cells. (b) Impedance spectrum at various electrolytes before and after 50 cycles

The pristine electrolyte and the GQD-based I-doped electrolyte showed typical charge/discharge characteristics of transparent LiFePO4 devices, as shown in Fig. 6a. In addition to the voltage of 3.25 and 3.40 V corresponding to LiFePO4, SSLB containing GQD-PEO-LiTFSI-1.5 wt % I2 electrolyte modified with GQD also has a 3.14 V discharge characteristic, caused by the state change of modified I3. This is consistent with the nanostructure properties. The control made possible by use of 1.5 wt % I2 modified with GQDs revealed the reversible redox properties of LiFePO4, indicating a reduction of I3− to I− and oxidation of I- to I3-due to GQD. This suggests that the GQD-modified iodine structure is involved in the electrochemical change of the device. In addition, the SSLB using the modified GQD-PEO-LiTFSI-1.5 wt % I2 electrolyte showed superior rate characteristics compared to those of the pristine electrolyte.

Subsequently, using EIS measurement, changes of SSLB interface impedance (Rct) after repeated cycles were analyzed to determine the hetero-interfacial structural stability between the GQD-modified PEO electrolyte and the Li interface. As shown in Fig. 6b, Rct showed a tendency to increase after continuously changing cycle of the SSLB containing modified PEO-LiTFSI electrolyte. And, the Rct of the device using the modified GQD-PEO-LiTFSI-1.5 wt % I2 electrolyte was smaller than that of the device using the pristine PEO-LiTFSI electrolyte. After 10, 50, and 100 cycles, the Rcts of the devices were 254, 102, and 86 Ω, respectively. These results indicate that GQD-based modified I2 doping is responsible for the structuring of the highly conductive modified SEI layer with GQDs, and is related to the formation of the Li/Li2O structure by iodine redox reaction. The hetero-interface impedance between Li anode and GQD-PEO electrolyte decreased.

4  Conclusion

A modified structure of I2 was applied to a GQD-PEO-based hetero-structured electrolyte. During the SPEs structuring process, iodine underwent I2 to I3− conversion and reacted with the carbon–oxygen bond of the modified PEO, improving the ionic conductivity of the hetero-composite electrolyte by a factor of 5. In addition, changes of position of I-doped LiI and the LiIO3 structure at the Li metal anode interface are attributed to the stable diffusion of iodine in the GQD-modified electrolyte. An SEI layer comprised of iodide and Li2O hetero-interfaces in the amorphous Li structure was formed, inhibiting the growth of Li dendrites through a reaction between GQD-modified electrolyte and Li metal anode. In addition, GQD-modified I3− reacts with Li and Li2O structures allowing control of the Li metal anode hetero-interface. Due to the effect of GQD-modified I2 doping, the GQD/PEO LiTFSI-1.5 wt % I2/Li device exhibited stable rate capacity and good cycling performance. These aspects of heterostructure control and electrolyte design based on halogen-related reactions suggest an effective strategy for an optimal SSLBs system, and can be used to design low-dimensional structure-based halide applications for complex electrolytes.

Funding Statement: This research was funded by a 2020 research Grant from Sangmyung University.

Conflicts of Interest: The authors declare that they have no conflicts of interest to report regarding the present study.