Developments of electrolyte systems for lithium–sulfur batteries: a review
- 1College of Chemical and Biological Engineering, Zhejiang University, Hangzhou, Zhejiang, China
- 2Anhui Academy for Environmental Science Research, Hefei, Anhui, China
With a theoretical specific energy five times higher than that of lithium–ion batteries (2,600 vs. ~500 Wh kg−1), lithium–sulfur (Li–S) batteries have been considered as one of the most promising energy storage systems for the electrification of vehicles. However, both the polysulfide shuttle effects of the sulfur cathode and dendrite formation of the lithium anode are still key limitations to practical use of traditional Li–S batteries. In this review, we focus on the recent developments in electrolyte systems. First, we start with a brief discussion on fundamentals of Li–S batteries and key challenges associated with traditional liquid cells. We then introduce the most recent progresses in liquid systems, including ether-based, carbonate-based, and ionic liquid-based electrolytes. And then we move on to the advances in solid systems, including polymer and non-polymer electrolytes. Finally, the opportunities and perspectives for future research in both the liquid and solid Li–S batteries are presented.
With the development of modern society and the boost of the electronics industry, energy storage systems have attracted considerable attention during the past few decades. Among them, lithium–ion (Li-ion) batteries have been intensely studied on their stable electrochemistry and long lifespan for applications in portable electronic devices. However, Li-ion batteries are still suffering approaching limiting capacity and high cost with safety concerns. This makes them inferior to support emerging industrial applications, including military power supplies, electric vehicles, and stationary electrical grids, which need higher capacity, lower cost, and more secured operation (Tarascon and Armand, 2001; Li et al., 2009; Ellis et al., 2010; Goodenough and Kim, 2010; Etacheri et al., 2011).
Recently, lithium–sulfur (Li–S) batteries attract considerable attentions due to high theoretically gravimetric and volumetric energy densities of 2,600 Wh kg−1 and 2,800 Wh L−1, respectively. Based on the complete reaction between the metallic lithium and elemental sulfur to form lithium sulfide (Li2S) as shown in Eq. 1:
Lithium–sulfur batteries can supply the energy density three to fivefolds higher than Li-ion batteries. Combined with other advantages of sulfur such as the natural abundance, cheapness, and non-toxic, Li–S batteries have been considered as one of the most promising energy storage devices for next generation high-energy power systems.
A typical Li–S cell is shown in Figure 1, which include carbon–sulfur composites as the cathode and metallic lithium as the anode with organic liquid electrolyte in between. During discharge, sulfur is electrochemically reduced into Li2S on the electrode through a complex process with a series of polysulfide intermediates.
Figure 1. Schematic configuration of Li–S battery based on organic liquid electrolyte (Mikhaylik et al., 2010).
A typical discharge profile of sulfur cathode in the liquid electrolyte is shown in Figure 2. The active sulfur is electrochemically reduced through a stepwise sequence of a series of intermediates in formula as Li2Sx (x = 2~8) on the electrode surface, among which the long-chain polysulfide Li2Sx (x = 4~8) is demonstrated highly soluble in the electrolyte while the short-chain Li2Sx (x = 2~4) is less soluble (Ji and Nazar, 2010; Yang et al., 2013).
The lithiation of sulfur can briefly described as four processes below:
The solid-state crown-like S8 ring is first electrochemically reduced into highly soluble through a solid–liquid two states reaction, exhibiting upper voltage plateau at ~2.3 V. Subsequently, the dissolved is further reduced into lower-order on the surface of cathode, accompanied with a series of chemical or electrochemical intermediates such as etc. (Barchasz et al., 2012b; Zhang and Read, 2012). This process causes rapid increase of electrolyte viscosity due to increase of the polysulfides (PS) anions concentration, and results in a steeply decline of voltage until a downward peak is observed when the solution reaches maximum viscosity as shown in region 2. The third process, which contributes the major capacity of Li–S cells, shows a long plateau at a lower potential of ~2.1 V, corresponding to the liquid–solid two phases reduction from dissolved low-order soluble PS to insoluble Li2S2 or Li2S as described in Eq. 4. The subsequent reduction from Li2S2 to Li2S is through a solid–solid single phase reaction. This process suffers poor kinetic and high polarization due to the sluggishness of ion diffusion in solid-state bulk and the electronic insulation natures of Li2S2 and Li2S (Yamin and Peled, 1983; Yamaki et al., 1998).
Despite the considerable advantages mentioned-above, Li–S batteries still suffer tough challenges for their practical applications: (1) the electronic and ionic insulation nature of sulfur and its discharge products deteriorate the utilization of active sulfur material. (2) The dissolution of polysulfide – intermediates of cathode reaction in conventional organic liquid electrolyte – results in the so-called “shuttle” effect and leads to a severe active material loss in the cathode and lithium corrosion in the anode. (3) The remarkable 76% volume change from S to Li2S leads to the instability of cathode structure. (4) The adoption of metallic lithium anode results in the potential security liability due to the lithium dendrite formation and flammability in the organic liquid electrolyte.
A significant amount of effort and expertise have been invested to overcome the challenges mentioned-above, among which the novel design of sulfur cathode has received the maximum concentration in the purpose of elevating the electronic conductivity and suppressing the dissolution of PS (Ji and Nazar, 2010; Barghamadi et al., 2013; Bresser et al., 2013; Evers and Nazar, 2013; Manthiram et al., 2013, 2014; Song et al., 2013; Yin et al., 2013; Chen and Shaw, 2014; Xu et al., 2014). These works usually focused on constructing a conductive porous matrix, such as nanostructured carbons and conducting polymers, as holder for active sulfur species as well as to physically or chemically restrain the dissolution and diffusion of PS to alleviate active material loss and suppress the shuttle effect.
Except for the thriving cathode development in Li–S batteries, the research on Li–S electrolytes, has also been accelerated recently due to its especial and critical role. The primary function of electrolyte for Li–S batteries is to efficiently transport Li+ ions between the electrodes. It generally requires adequately high Li+ conductivity in the premise of physical, chemical, and electrochemical stabilities under operating conditions such as temperature, pressure, as well as the working voltage window. Moreover, the electrolyte has additionally critical influence on electrode reaction mechanisms and the behavior of active sulfur and its discharge products. In this review, we herein mainly aim to introduce some critical and instructive researches on different types of electrolytes presently applied in Li–S batteries, including liquid electrolytes such as ether-based, carbonate-based and ionic liquid (IL)-based electrolytes, and solid electrolytes such as polymer and non-polymer electrolytes. We also suggest some ways to rationally design novel electrolytes for future applications in Li–S batteries, to enhance its electrochemical performance for longevity of Li–S cells.
Liquid electrolyte is the most commonly used in not only Li–S batteries, but also most of other electrochemical cells, due to its low surface tensions and low viscosities. These properties provide electrolyte with good wettability to obtain favorable contact between electrolyte and active materials along with low interface resistance (Scheers et al., 2014). Meanwhile they also provide easier access to achieve large-scale applicable electrolytes with considerable ion conductivity, due to the easier ion diffusion as well as preparation of homogeneous solution. As for Li–S cells, special requirements need to be proposed for electrolyte, due to high chemical reactivity of PS and metallic lithium (Gao et al., 2011; Zhang, 2013). Moreover, taking the poor electrochemical kinetics of sulfur and lithium sulfide into consideration, more beneficial design of electronic and ionic paths should raise the difficulty in the electrolyte selection of Li–S cells (Scheers et al., 2014).
Ether Based Electrolytes
At present, ether-based electrolyte is adopted as the most commonly used electrolyte for Li–S batteries, which is typically composed of 1 M lithium bis-trifluoromethanesulfonimide (LiTFSI) in a binary ether solvent of 1,2-dimethoxyethane (DME) and 1,3-dioxolane (DOL) with a small amount of LiNO3 as additives (Gao et al., 2011; Kim and Jeong, 2011; Zhang, 2013; Xu et al., 2014). Ether solvents are chosen mainly because their general stability in the presence of PS (Aurbach et al., 1990a,b; Gofer et al., 1992) and high ion transmission and better electrolyte/electrode contact from the low-viscosity and excellent wettability (Zhang, 2013). In this section, we will discuss the ether-based electrolytes from the following three aspects: the solvents, the salts, and the additives.
Among many types of ether solvents, chain-ether such as DME, polyethylene glycol dimethyl ethers (PEGDME), and tetraethylene glycol dimethyl ether (TEGDME) dominated the use as a single solvent for Li–S battery due to its good dissolving capacity against PS (Tobishima et al., 1997; Marmorstein et al., 2000; Shim et al., 2002; Barchasz et al., 2013a). Table 1 shows the list of solvents used in the present Li–S cells and their characteristics. For example, Mikhaylik group of Sion Power Corporation studied single DME, single DOL, and a binary solvent of DME + DOL as the electrolyte for Li–S battery (Mikhaylik et al., 2010). DOL has relatively lower polysulfide solubility, but provides a more stable solid electrolyte interface (SEI) on the metallic lithium surface. DME, on the other hand, is more reactive with lithium, but provides higher polysulfide solubility for improved cathode reaction kinetics. These two electrolyte solvents exhibit some synergistic effect on improving the specific capacity and cycle life of lithium cells. Wang et al. (2010) used different electrolyte composition of DME: DOL = 4:1, 2:1, 1:1, 1:2, and 1:4 as solvents and LiClO4 as lithium salt. When using the optimal composition of DME:DOL = 2:1 (v/v), the cell exhibited the highest initial capacity of 1,200 mAh g−1 and best cycling capacity retention of 750 mAh g−1 after 20 cycles. A followed EIS analysis indicated that high content of DME in electrolyte raised the interfacial resistance due to the formation of an impermeable layer on the surface of the sulfur cathode, while the increase of DOL could ameliorate this phenomenon. Parallel works were also conducted by Jung’s group (Kim et al., 2014) and Lim’s group (Kim et al., 2004).
Tetraethylene glycol dimethyl ether, with a glyme structure and low dielectric constant (εr = 7.9), is another commonly used solvent for Li–S batteries. Barchasz et al. (2013b) carried out the study on the binary solvent consist of TEGDME and DOL in different volume ratio, as well as single TEGDME or DOL as solvent for Li–S cells. The best performance was obtained when TEGDME/DOL = 25/75 (v/v) solvent composition was used. The solvation ability of the electrolyte was considered as a key factor for high electrochemical performance. These cells exhibited better performance than those with TEGDME when combined with DOL in volume ratio of 1:1 as reported by Barchasz et al. (2013a).
Lithium salts require high chemical and electrochemical stability, considerable solubility, and high degree of dissociation in specific solvent to ensure good ion conductivity. Figure 3 shows the typical lithium salts already used in or of potential use for Li–S cells. Among them, the most commonly used lithium salts in Li–S system are LiTFSI and LiTf (Foropoulos and Desmarteau, 1984; Xu, 2004; Scheers et al., 2014) due to the high thermal stability, good compatibility with ether solvents, and high dissociation ability. It is worth noting that LiTFSI and particularly LiTf were suffering Al corrosion problem starting as ~2.8 V (Krause et al., 1997) and were not suggested to be used for most Li-ion battery. However, the lower cell voltage and less stringent condition on anodic stability of Li–S batteries liberates LiTFSI and LiTf from this problem as well as renewed the interest of some of other salts of intermediate anodic stability such as lithium bis(fluorosulfonyl)imide (Li[N(SO2F]2, LiFSI) (Guerfi et al., 2008) and lithium 4,5-dicyano-2-trifluoromethylimidazolide (LiTDI) (Dudley et al., 1991; Xu and Angell, 2002). Meanwhile lithium perchlorate (LiClO4) is also one of the alternatives by Wang et al. (2010). LiClO4 has also been studied by some other groups (Kim and Jeong, 2011), whose performance is usually inferior compared to LiTFSI or LiTf, presumably due to the inability to form a stable SEI on the lithium anode (Tarascon and Guyomard, 1994). As for LiPF6, a commonly used salt in Li-ion batteries, is rarely adopted in ether system due to the generation of Lewis acids, which decomposes the solvent (Armand, 1994). However, it is notable that until now there are few studies focusing on the influence of lithium salt on the performance of Li–S cells.
Figure 3. The typical lithium salts already used in or of potential use for Li–S cells (Scheers et al., 2014).
Most electrolytes for Li–S batteries contains small amount of additive in purpose of protecting lithium anode and enhancing the solubility and stability of PS. LiNO3 has become the most commonly used additive in Li–S battery since its first adoption in 2008. The functions of LiNO3 in Li–S system were investigated in detail by Aurbach et al. (2009). The results showed that LiNO3 lead to a smaller impedance of Li foil while its reduction products LixNOy contribute to the formation of suitable surface film, protecting Li from further reaction with PS. However, the LiNO3 study by Zhang indicated that the beneficial anode passivation was accompanied by a less desired effect at the cathode (Zhang, 2012). During the first discharge, LiNO3 was found to be irreversible reduced at the carbon surface and the reduction products adversely affect the redox reversibility of active sulfur, with a negative impact on the capacity and cycle performance of the Li–S battery. It was recommended not to discharge the cell lower than 1.6 V to avoid the reduction problem of LiNO3 (Mikhaylik et al., 2010).
Polysulfides were also used as additives for Li–S electrolyte due to its participation in the formation of anode SEI (Demir-Cakan et al., 2013; Xiong et al., 2013). The liquid Li–S battery or catholyte concept represents the extreme of this strategy while the majority of the related works still focuses on the PS as additives in Li–S cells together with mesoporous S/C cathodes (Barchasz et al., 2012a; Zhang and Read, 2012; Zhang and Tran, 2012; Demir-Cakan et al., 2013). Xiong et al. (2013) investigated the formation of a stable solid two layered interface on the surface of metallic lithium by cycling symmetric Li/Li and Li/S cells with 0.2 M Li2S6 as a co-salt in 0.8 M LiTFSI DOL:DME (1:1 v/v) electrolyte. The top layer was composed of the decomposition products of LiTFSI owing to the initial contact with lithium anode. The inner layer was consisted of the reduction product by the chemical reaction between lithium metal and PS in electrolyte. Xiong et al. suggested that the inner layer efficiently prevented continuous decomposition of LiTFSI, while the top layer cannot efficiently suppress the PS shuttle. Another novel additive, phosphorous pentasulfide (P2S5) was introduced by Liang’s group (Lin et al., 2013a). The function of P2S5 was introduced in two sides: (1) P2S5 promotes the dissolution of Li2S and alleviates the capacity loss caused by the precipitation of Li2S, and (2) P2S5 takes part in the formation of passivation layer on the surface of lithium metal, and therefore eliminates the polysulfide shuttle phenomenon. A Li–S test cell demonstrated a high reversible capacity of 900–1,350 mAh g−1 and a high coulombic efficiency of ≥90% for 40 stable cycles at C/10.
Carbonate-based electrolyte, typically composed of 1 M LiPF6 dissolved in binary solvent of ethylene carbonate (EC) and diethyl carbonate (DEC) in volume ratio of 1:1, is the most commonly used in Li-ion batteries. However, it was proposed inappropriate for Li–S batteries, due to the chemical reaction between nucleophilic sulfide anions and carbonates to form methylated thiolate and thioether during discharge (Gao et al., 2011). Similar results were also confirmed by other groups (Barchasz et al., 2013a; Yim et al., 2013).
In sharp contrast, several studies showed that carbonate-based electrolytes are possible for use in Li–S cells under certain conditions. Zhang et al. (2010) used 1 M LiPF6 in PC/EC/DEC (1:4:5, v/v/v) as electrolyte for sulfur/carbon spheres composite cathode. The corresponding Li–S cell showed only one lower discharge voltage plateau at around 1.8 V instead of two voltage plateaus at 2.3 and 2.1 V in conventional ether-based electrolyte. The authors attributed this potential hysteresis to the encapsulation of sulfur in the narrow micropores of carbon matrix. The composite contained 42 wt% sulfur presented a long cycle life of 500 cycles with high capacity retention over 80% due to constrained electrochemical reaction inside the micropores.
Another significant work by Xin et al. (2012) demonstrated a compatibility against carbonate electrolyte by using metastable small sulfur molecules of S2–4. S2–4 were synthesized in the confined space of a conductive microporous carbon (MPC) matrix in purpose of avoiding the generation of unfavorable long-chain PS, which is highly reactive against carbonates. These confined small S2–4 showed a single discharge plateau at ~1.9 V, with a high specific capacity of 1,670 mAh g−1 and an impressive cycling stability of 1,149 mAh g−1 after 200 cycles. On the basis of the above works, Li et al. (2013) investigated the lithiation/delithiation mechanism of S2–4 cathode by comparing the electrochemical performances of the S2–4 and S2–4/S8 electrodes in ether or carbonated electrolyte. Figure 4 shows the theoretically calculated dimensions of EC and DMC molecules as well as the lithiation processes of sulfur in different pore structures. If the micropores of carbon are small enough to prevent the penetration of the solvent molecules, the lithiation/delithiation of S2–4 occurs through a solid–solid process, which is in consist with the single plateau in discharge potential profile. In such condition, irreversible chemically reactions between the polysulfides are effectively avoided due to the steric hindrance, ensuring a high adaptability to the electrolytes of the confined S2–4. The corresponding cells can exhibit excellent rate capability and cycling stability. Similar results with S/porous carbon composite as cathodes in carbonate electrolyte were also obtained by some other groups with good electrochemical performances (Wang et al., 2002, 2012; Zheng et al., 2014). However, one of the obvious problems of this strategy is the low sulfur loading due to the small pore volume contributed by micropores.
Figure 4. Theoretically calculated dimensions of EC and DMC molecules (A) as well as the lithiation processes of sulfur in different pore structures (B,C) (Li et al., 2013).
Ionic Liquid Based Electrolytes
Ionic liquids have been considered as promising electrolytes for Li–S battery due to highly thermal and chemical stability with good ionic conductivity (Armand et al., 2009). These properties ensure Li–S batteries much greater security in terms of avoidance of leakage and gassing, large electrochemical stability window, and high solvent powers. Owing to the absence of highly solvable ethers, the PS dissolution and shuttle effect could be effectively suppressed to maintain a decreased active material loss and high columbic efficiency. However, the main drawbacks of ILs for Li–S battery are higher viscosities than organic liquids and higher cost compared to other conventional organic solvent.
The very first paper using pure ILs as the electrolyte matrix for Li–S cells was reported by Yang’s group (Yuan et al., 2006). A novel room temperature IL N-methyl-N-butyl-piperidinium bis(trifluoromethanesulfonyl) imide (PP14-RTIL), supported by 1 M LiTFSI, was used as electrolyte for Li–S battery. This cell exhibited the initial discharge capacity of 1,055 mAh g−1 with a single discharge plateau at ~1.9 V and over 750 mAh g−1 after 10 cycles. Park et al. (2013a) investigated a Li–S system with a 0.64 M LiTFSI IL electrolyte based on a quaternary ammonia cation N,N-diethyl-N-methyl-N-(2-methoxyethyl)ammonium (DEME) and TFSI compared with a 0.98 M LiTFSI dissolved in TEGDME electrolyte. The dissolution of PS was significantly suppressed owing to the weak donor ability of [TFSI]− anion. In this IL electrolyte, the electrochemical reduction of sulfur mainly occurred on the surface of electrode through solid phase process, resulting in an improved capacity decay of Li–S cells during cycling. Park et al. (2013b) further carried out an extensive work by focusing on the important roles of the IL anions in the electrolytes. The results indicated that the non-ionic sulfur possessed low solubility in all of the evaluated electrolytes, while the BF4− anion and [FS]− anion irreversibly reacts with PS on the surface of electrode. The low-viscosity [TFSI]− anion based ILs maintained considerable chemical and electrochemical stability with PS during cycling, allowing the best cell performance with a sustainable capacity up to >650 mAh g−1 and high coulombic efficiency of >98% during 50 cycles.
Wang et al. (2008) compared the behavior of S/mesoporous carbon composite cathode in Li–S cells in 1 M 1-ethyl-3- methylimidazolium bis(trifluoromethanesulfonyl)imide (EMIM TFSI)/LiTFSI-based electrolyte with 1 M LiTFSI/PEGDME electrolyte. The ILs electrolyte exhibited both better cyclability and discharge capacity due to the claimed less solubility of PS in the IL based electrolyte. More recently, Tachikawa et al. (2011) used a so-called “quasi-IL” [LiG4][NTf2] (G4 = tetraethylene glycol dimethyl ether, TEGDME), a glyme-Li salt molten complex electrolytes, where the [LiG4]+ cation is an equimolar complex of G4 and Li+. The corresponding cells with sulfur supported on 3D ordered macroporous carbon as cathode material showed good reversibility, large capacity, and high coulombic efficiency. Yan et al. (2013) reported on an expended selection for IL of [P1A3][TFSI] (P1A3 = n-Methyl-n-Allylpyrrolidinium) by using a Si/C anode instead of metallic lithium. Li–S cells gave a nominal voltage of 1.5 V and delivered a high initial discharge capacity of 1,457 mAh g−1 at C/10 and remained 670 mAh g−1 after 50 cycles.
Although cyclability of Li–S cells was improved obtained by the employment of IL electrolyte also led to low rate performance and low operation voltage (Shin and Cairns, 2008b). In order to alleviate the above problems, the IL-organic mixture electrolyte was the alternatives to the neat ILs. An early work on IL-organic mixture was conducted by Kim et al. (2005) by introducing different amount imidazolium salt of EMIMBETI and BMIMPF6 into 0.5 M LiTFSI or 0.5 M LiPF6 in DOL:DME (1:4 v/v). Best cell performance was obtained when 10% IL was used. Kim carried out an extended work by using a large number of other ILs as additives in the same DOL:DME (1:4 v/v)-based electrolytes (Kim et al., 2007). The EMI and BMI contained Li–S cells showed much higher capacity and cyclability compared to regular LiTFSI-based Li–S cells due to the lower charge transfer resistance at the electrodes, while DMPI showed poor cell performance probably due to the its irreversible reaction with PS to form a non-conductive coating on the cathode surface.
To sum up, the IL-organic mixture electrolyte combines the advantage of high conductivity in organic solvent and low PS dissolution in ILs. The existence of organic solvent was also designed for decrease of electrolyte viscosity, better wettability, and higher conductivity for better electrochemical kinetics of active sulfur. Based on these beneficial properties, the IL-organic mixture has been considered as a promising electrolyte for Li–S batteries (Shin and Cairns, 2008a; Dokko et al., 2013; Wang and Byon, 2013).
Though the organic liquid electrolytes dominate Li–S batteries, it is still necessary to search for other electrolytes because of the polysulfide shuttle and the lithium dendrite formation. Under this circumstance, solid electrolytes are considered highly effective in improving Li–S cells performance (Scheers et al., 2014). Figure 5 shows the typical discharge profile in all-solid Li–S batteries. Compared to the typical two plateaus in organic liquid electrolyte, all-solid Li–S cell demonstrates a single plateau at a relatively low potential of around 1.9 V, which is due to the solid–solid single phase reduction from S8 to Li2S with a deteriorated reaction kinetics and polarization.
Figure 5. The typical discharge profile in all-solid Li–S batteries (Scheers et al., 2014).
Solid Polymer Electrolytes
Solid polymer electrolyte is defined as the membrane that possess ion transporting ability compared with the dissociation of lithium salts in common liquid electrolytes (Manuel Stephan, 2006). Polymer electrolyte has received many attentions after first report by Fenton et al. (1973), mainly due to advantageous properties of no internal shorting, no leakage of electrolytes, non-flammability as well as its promising applications in electrochemical devices (Idris et al., 2012).
The solid polymer electrolyte (SPE) is usually composed of lithium salts dissolved in high molecular weight polymer host, which functionalized as solid solvents (Song et al., 1999). By employing an SPE to assemble all-solid Li–S cells, SPE can effectively suppress the dissolution and diffusion of PS as well as the shuttle phenomenon, greatly enhancing the cyclability of Li–S cells (Kim et al., 2006). Many polymers, including poly(ethylene oxide) (PEO), PPO, PAN, PMMA, PVC, poly(vinylidene fluoride) (PVDF), and poly(vinylidene fluoride)-hexafluoropropylene (PVDF-HFP) were adopted as the solid host due to high solvation power and considerable ion transport ability. Among which, PEO-based SPE emerged as possibly the best candidate because its great solvation power, complexation ability, and ion transport mechanism directly connected with the alkaline lithium salt (Zhao et al., 2012). Different lithium salts (e.g., LiClO4, LiTFSI, LiBF4, and LiPF6) were employed to combined with PEO, and their influence on electrolyte ion conductivity is listed in Table 2 (Weston and Steele, 1982).
The combination of PEO–LiClO4 was first studied by Jeon et al. (2003) as electrolyte for Li–S cells. However, the low ionic conductivity of PEO–LiX electrolyte at room temperature (10−7–10−6 S cm−1) is inadequate for the application in Li–S cells. Regarding to this problem, recently a promising strategy is to use inorganic ceramic filler such as SiO2, TiO2, ZrO2, Al2O3, and LiAlO2 in the host polymer matrix to enhance the ionic conductivity of SPEs (Appetecchi et al., 2000; Chung et al., 2001; Croce et al., 2001; Shin et al., 2002b; Ahn et al., 2003; Dissanayake et al., 2003; Lin et al., 2005; Zhu et al., 2005; Jeong et al., 2007). The nano-filler is beneficial to reduce the crystallinity of polymer solvent so as to the increase of ion conductivity due to the amorphous phase. Additionally, the filler surface groups interact with the PEO oxygen atoms and the crosslinking polymer chains retard the structural reorganizations and increase the Li-ion mobility (Przyluski et al., 1995).
One significant work was carried out by Hassoun et al. by using ZrO2 as an electrolyte additive for Li–S batteries (Hassoun and Scrosati, 2010b). With 10 wt% ZrO2, significant enhancements in ion conductivity, Li+ transference number, and electrode/electrolyte interface stability were obtained as well as the formation of finely dispersed layer on lithium surface (Croce et al., 2006a,b). The corresponding Li–S cells maintained a capacity up to 900 mAh g−1 and a sustained high coulombic efficiency close to 100% for 50 cycles. Liang et al. (2011) studied PEO18LiTFSI-10 wt% SiO2 as electrolyte with a mesoporous carbon sphere with uniform channels (OMCs) supported sulfur as the cathode. The Li–S cells exhibited excellent cycling performance with a reversible capacity up to 800 mAh g−1 after 25 cycles.
Though the SPE was successfully optimized by inorganic additives, the rate performance still remains poor (usually no higher than C/20), and a relatively high temperature is needed for adequate ion conductivity.
Gel Polymer Electrolytes
The gel polymer electrolyte (GPE), where the liquid component is tightly trapped in the polymer matrix, was developed as a compromise strategy against the low ionic conductivity of SPE (Xu and Ye, 2005). The bulk of the membrane was usually composed of connected micropores to ensure adequate absorption amount toward liquid electrolyte. The ion conductivity is largely depended on the property of liquid electrolyte or otherwise the transfer of Li+ mainly happens in the polymer membrane with insufficient liquid absorption (Li et al., 2008). Several types of polymer membranes, such as those based on PEO, PVDF, and PVDF-HFP, were developed and characterized for Li–S cells (Shin et al., 2002a; Wang et al., 2002, 2003; Ryu et al., 2006; Hassoun and Scrosati, 2010a; Zhang and Tran, 2013).
Ryu et al. (2006) used PVDF based polymer matrix combined with LiTf/tetraglyme as electrolyte for Li–S cells. Two plateaus were observed in the first discharge possessing a high capacity up to 1,268 mAh g−1. However, the upper plateau disappeared in the second discharge with a deceased capacity of 1,028 mAh g−1, indicating the hindering effect of GPE in the dissolution of long-chain PS. Hassoun and Scrosati (2010a) made in important progress by building a metallic lithium-free system using Sn/C anode and Li2S/C cathode. Gel-type polymer membrane formed by trapping LiPF6/EC + DMC in PEO/LiCF3SO3 polymer matrix was adopted as electrolyte with dispersed zirconia ceramic filer as additive to enhance the mechanical property. Impedance study indicated a low resistance and a high conductivity close to 10−2 S cm−1. The obtained polymer cell showed a high initial capacity of over 1,200 mAh g−1 and good capacity retention at C/20 rate along with cycling. The GPE functionalized as the barrier to prevent PS dissolution, and the Sn/C anode aimed to eliminate the risk of anode corrosion for liquid electrolyte.
Owing to the combination of SPE and liquid electrolyte, higher ion conductivity, and better reaction kinetics were obtained by GPE at the cost of the resurgence of PS dissolution and shuttle effect. However, more deep going and systematic research on how GPE and GPE composition affects the PS solvation characteristic as well as modification on pore structure and polymer crystallinity in purpose of improved Li+ transport remain to be carried out.
In virtue of the poor cell performance with solid polymer based electrolytes, non-polymer electrolytes provide a promising strategy for all-solid Li–S cells considering its inherent advantages of high thermal and chemical stability toward the Li anode under ambient atmosphere (Adachi et al., 1996; Robertson et al., 1997; Thangadurai and Weppner, 2006; Thangadurai et al., 2014). Since the first study on primary solid-state Li-ion batteries in 1972 (Scrosati, 1972), large number of inorganic solid-state electrolytes were investigated for Li–S cells as well as Li-ion batteries, including LiSICON-type phosphates, perovskite-type La(2/3)xLi3xTiO3 (LLT), Li3N, and Li4SiO4 (Hayashi et al., 2003b; Stramare et al., 2003; Kobayashi et al., 2008; Nagao et al., 2011, 2013). A list of non-polymer electrolytes, comparing with other electrolytes including polymer electrolytes, ionic liquids, and gel electrolytes, are shown in Figure 6.
Figure 6. Thermal evolution of ionic conductivity of the Li10GeP2S12 phase, together with those of other lithium solid electrolytes, polymer electrolytes, ionic liquids, and gel electrolytes (Kamaya et al., 2011).
The family of sulfide compounds that form amorphous solid electrolyte with high Li+ conductivity is one of the hotspot in inorganic solid-state electrolytes. The group of Hayashi and Tatsumisago carried out a series of significant works on Li2S-P2S5 glass electrolyte (Hayashi et al., 2001b, 2004, 2008; Nagao et al., 2012; Teragawa et al., 2014). In their early work, mechanical milled 80Li2S-20P2S5 (mol %) glass was demonstrated of an exceptionally high conductivity up to 10−3 S cm−1 at room temperature, due to the formation of Li7PS6 (Hayashi et al., 2001a), which was described as “superionic” and crystallographic analogs of thio-LISICON (Hayashi et al., 2003a). The Li2S–P2S5 glass–ceramic electrolyte was successfully applied in Li–S system. The corresponding cells with S/CuS cathode retained capacity of over 650 mAh g−1 for 20 cycles (Hayashi et al., 2003b). Further development was obtained by using sulfur–carbon composite electrode and Li2S–P2S5 glass–ceramic electrolyte. Excellent cell performance was maintained with reversible capacity over 850 mAh g−1 for 200 charge/discharge cycles under 1.3 mA cm−2 at room temperature, and even close to 500 mAh g−1 at 20 mA g−1 when temperature was raised to 80°C (Nagao et al., 2011). Recently, a related compound of Li10GeP2S12 developed by Kamaya et al. (2011) shows an ever highest ion conductivity of around 10−2 S cm−1 at room temperature with good potential of application in Li–S system, albeit that the relatively limited reversibility against metallic lithium remains to be overcome. Nagata el al. assembled cells using Li-In alloy as negative electrode and Li10GeP2S12 as solid electrolyte (Nagata and Chikusa, 2014). The cathode material was prepared by mechanochemical treatment on the mixture of Li1.5PS3.3, sulfur, and conductive carbon. The resulting cathode showed the reversible capacity of 1,600 mAh g−1 (based on sulfur) after 100 cycles under 1°C rate at 25°C, exhibiting a high power density of over 11,000 W kg−1 at 50% SOC.
Recently, the Liang’s group at Oak Ridge National Laboratory reported a nanoporous β-Li3PS4 with high conductivity up to 1.6 × 10−4 S cm−1 at room temperature through a liquid-state reaction (Liu et al., 2013). Reversible lithium deposition and excellent inhabitation against lithium dendrite were identified by CV and cells cycling at 25°C. In the subsequent development of this material, nano-sized Li2S particles coated by β-Li3PS4 were prepared as the active material for cathode (Lin et al., 2013b). With the thiophosphate also serving as the electrolyte, metallic lithium as anode, the assembled cells delivered a considerable capacity of 1,216 mAh g−1 (based on sulfur) in the first discharge, but also suffered about 30% capacity decay over 100 cycles at 60°C. It should be noted that the low surface area carbon used in this work may result in a lack of extensive interaction between sulfur/sulfide and functional substrate. Another application of this material is in the form of P2S5 additive toward the conventional liquid electrolyte by forming β-Li3PS4 on electrolyte surfaces, providing good ion transporting, protection anode from PS and raised solubility for all sulfides as mentioned in liquid electrolyte additive part. Lin et al. (2013c) made a significant progress by using a novel class of sulfur-rich lithium polysulfidophosphates as cathodes for Li–S battery. These compounds exhibited a high Li-ion conductivity of 10−4–10−5 S cm−1 at room temperature. Excellent performance was demonstrated when this cathode material was combined with the solid-state Li3PS4 electrolyte to display a reversible capacity of over 1,200 mAh g−1 at C/10 over 300 cycles at 60°C.
Conclusion and Prospects
Though promising, the tough challenges of the insulating properties of sulfur species, the polysulfide shuttle, and the dendrite formation/safety concerns have prevented the Li–S batteries from practical applications. In the past few years, significant efforts have been dedicated to the study of each component in the Li–S cells for improved cyclability. In this article, we have reviewed the most recent progresses in Li–S batteries in the field of electrolyte systems, including liquid electrolytes and solid electrolytes.
As the most commonly used electrolyte, liquid electrolytes are chosen because of its high ion conductivity, low-viscosity, and high compatibility with lithium and PS. There’s indeed a large variation in the properties of electrolytes with different solvents, salts, and additives. As the emergence of different cathode materials and designs, electrolyte should be uniquely defined for each system in purpose of better performance. In the future research, liquid electrolytes need to be compared and studied systematically in the following aspects: (1) understanding the cycling mechanisms when different electrolytes are used, (2) implementing alternative electrolytes in the same Li–S cell configuration to study the importance of each component, (3) having better understanding of PS behavior and anode SEI formation using different electrolytes, and (4) choosing the suitable liquid electrolyte for the Li–S battery system.
With the emergence of solid electrolytes with ionic conductivities comparable to that of liquid electrolytes, the all-solid Li–S batteries promise to be the next breakthrough for electric energy storage. The replacement of liquid electrolytes by solid electrolyte eliminates the polysulfide shuttle and enables the practical applications of high-energy and intrinsically safe Li–S batteries. For the future research, solid electrolytes need to be compared and studied systematically in the following aspects: (1) the ionic conductivities of SPEs and GPEs need to be enhanced for further applications, (2) the electrochemical mechanisms of the Li–S cells need to be studied further when solid electrolytes are used, (3) novel electrolyte compositions or good additives should be explored to improve stability and solve safety concerns when cycling metallic lithium anodes, and (4) interfacial resistance need to be solved for high-performance all-solid Li–S cells.
In summary, Li–S batteries can supply the theoretical energy density five times higher than that of Li-ion batteries, and they have been considered as the most promising candidate for the application in the electrification of vehicles. With great interest and extensive research in the Li–S cells, there have been significant progresses in improving cycling performance of both liquid and solid Li–S batteries. With more and more developments in this field, we believe that Li–S batteries could be a practical technology for the applications in transportation and large-scale grid energy storage in the near future.
Conflict of Interest Statement
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
This work is financially supported by the National Natural Science Foundation of China, Grant No. 21476200 and 21276229; the Zhejiang Provincial Natural Science Foundation of China, Grant No. Z4110126.
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Keywords: Li–S batteries, energy storage, polysulfide, electrolytes, review
Citation: Li G, Li Z, Zhang B and Lin Z (2015) Developments of electrolyte systems for lithium–sulfur batteries: a review. Front. Energy Res. 3:5. doi: 10.3389/fenrg.2015.00005
Received: 13 November 2014; Accepted: 22 January 2015;
Published online: 11 February 2015.
Edited by:Mariusz Walkowiak, Institute of Non-Ferrous Metals, Poland
Reviewed by:Angu N. Lakshmi, Mahatma Gandhi University, India
Oscar Tutusaus, Toyota Research Institute of North America, USA
Andrea Strakova Fedorkova, Pavol Jozef Safarik University in Kosice, Slovakia
Copyright: © 2015 Li, Li, Zhang and Lin. This is an open-access article distributed under the terms of the Creative Commons Attribution License (CC BY). The use, distribution or reproduction in other forums is permitted, provided the original author(s) or licensor are credited and that the original publication in this journal is cited, in accordance with accepted academic practice. No use, distribution or reproduction is permitted which does not comply with these terms.
*Correspondence: Zhan Lin, College of Chemical and Biological Engineering, Zhejiang University, Hangzhou, Zhejiang, China e-mail: firstname.lastname@example.org