Research Progress of the Solid State Lithium-Sulfur Batteries

Abstract

Lithium-sulfur batteries using lithium as the anode and sulfur as the cathode can achieve a theoretical energy density (2,600 Wh.g⁻¹) several times higher than that of Li ion batteries based on the chemical conversion reaction of 6Li + S₈ ↔ 8Li₂S. The cost effectiveness, together with the intrinsic high energy density of the Li-S batteries, enables it to be an important option for the next generation energy storage devices. However, lithium-sulfur batteries using the liquid electrolyte would lead to the dissolution and “shuttle effect” of polysulfides, which greatly decrease the cycle life and specific capacity. In order to realize long cycle life of the lithium-sulfur battery, it is crucial to address the uncontrolled diffusion of polysulfides. Replacing the liquid electrolyte with the solid electrolyte, which can address the polysulfide dissolution and diffusion problem, inhibit the growth of lithium dendrites on the anode side, and greatly improve the safety and the cycle stability of lithium-sulfur batteries. In spite of the above merits, the performance and application of solid state Li-S batteries are strongly constrained by their low discharge capacity, poor rate performance and unsatisfied cycle life, which need to be overcome by advances in both the materials and the battery design. In this mini-review, the recent research progress of solid-state lithium-sulfur batteries in several aspects, including the sulfur-cathode design, different types of solid electrolyte and Li-S batteries based on them is described/summarized. New insights and synthesis approaches for the stable lithium anode are also summarized. We particularly emphasize the role of the interface in impeding the battery reaction, as well as the construction of the “solid/solid/solid” three-phase reaction boundary. At last, the prospects and challenges in further advancing the scientific understanding and enabling the battery technology viable are presented to shed light on the upcoming research efforts.

Introduction

Lithium sulfur batteries use lithium metal as the negative electrode and sulfur elemental or sulfide as the positive electrode (Xu, 2004; Bruce et al., 2011; Chen R. et al., 2016). Among them,the lithium-sulfur battery using the elemental sulfur as the active cathode material has the highest theoretical specific energy density in gravimetric (2,600 Wh/kg) and capacity density (2,800 Wh/L), based barely on the mass of active materials. Prototype Li-S pouch cells can already deliver specific energy as high as 600 Wh/kg, which is much higher than that of the existing Li ion batteries (250 Wh/kg) and can meet the target of enabling the electric cars with >300 miles driving range. Lithium-sulfur batteries also have the advantages of high output power, abundant sulfur reserves and low cost, and have become one of the commanding heights of energy storage battery technology competition (Xu, 2004; Goodenough and Kim, 2010; Bruce et al., 2011; Chen R. et al., 2015).

Although the performance of lithium-sulfur batteries has been initially verified, the safety and the cycle performance are still standing out as the big barriers in the practical application of lithium-sulfur batteries (Kamyshny et al., 2007; Barchasz et al., 2012; Zhang, 2013). At present, lithium-sulfur batteries using the sulfur cathode usually employ the liquid electrolyte with LiTFSI dissolved in ether solvent, such as 1, 3 dioxane (DOL), dimethoxy-ethane (DME), etc. In general, lithium-sulfur batteries with the liquid electrolyte have achieved success in demonstrating the huge potential of this sulfur battery, but large scale deployment and application are still out of their capability due to the following aspects: (a) During the charging and discharging process of the battery, a long-chain lithium polysulfide intermediate can be formed, which is easily soluble in the liquid electrolyte. The continuous dissolution of the polysulfide increases the viscosity of the electrolyte, meanwhile it also destroys the structure of the cathode. In addition, the precipitation of polysulfides will turn into the insulating Li₂S on the surface of the cathode, which would hinder the electronic and ionic migration, and reduce the utilization of sulfur active substances (Xu et al., 2015; Peng et al., 2017). (b) The dissolved long-chain polysulfide diffuses from the cathode to the anode, and the long-chain polysulfide will be reduced to short-chain polysulfide on the anode surface, which then migrates back to the cathode and reconverts into the middle of the chain of lithium polysulfide. The infinite motion of the polysulfide between the cathode and the anode is known as the “shuttle effect” of the polysulfide. During the charging and discharging process, the shuttle effect of the polysulfide causes the low coulombic efficiency and corrosion of the lithium metal anode (Mikhaylik and Akridge, 2004; Bruce et al., 2011). (c) The electrolyte solvent becomes unstable with fresh and porous Li metal anode after corrosion with polysulfides. On which, the electrolyte is gradually consumed until it is exhausted, and the reaction generates gas which may cause the expansion of the battery,and even explosion (Zhang, 2013; Jozwiuk et al., 2016; Schneider et al., 2017; Hancock et al., 2018). When used under high temperature conditions, the organic solvent is also easily ignited which increases the safety hazard (Chen W. et al., 2018). (d) The uncontrolled lithium deposition in liquid electrolyte leads to the dendrite growth. The uncontrollable dendrite growth leads to the formation of “dead lithium” with low coulombic efficiency, and may even trigger the internal short circuit and catastrophic failure (Cao et al., 2015; Cheng et al., 2017).

In order to overcome the above problems and further improve the performance of lithium-sulfur batteries, researchers have studied a series of countermeasures, including the design of sulfur cathode (Song et al., 2013; Rosenman et al., 2015; Li et al., 2016; Pang et al., 2016; Ye et al., 2018), the protection of lithium anode (Wu et al., 2014, 2015; Cheng X. B. et al., 2016; Jiaqiang et al., 2017), and the optimization of electrolytes (Arumugam et al., 2014; Zhang S. et al., 2015). In terms of the electrolyte optimization, solid electrolytes including gels, solid polymers, inorganic ceramics and inorganic-organic composite electrolytes are gaining more and more attention (Figure 1). Solid electrolytes can cure many problems caused by liquid electrolytes. In the past few years, a growing body of researches have proved the advantages of solid electrolytes (Liu et al., 2016; Wang S. et al., 2016; Tao et al., 2017). This mini-review is intended to summarize the recent progress of Li-sulfur batteries based on the solid electrolytes, including the pros and cons of using gels, solid polymers, inorganic and organic-inorganic composites as solid electrolytes; and the progress of solid state Li-sulfur batteries based on either the sulfur cathode or lithium metal anode. The challenges to further advance this battery technology and progress it from laboratory interest to commercial feasibility are also presented, which might shine a light for the development and large-scale applications of the solid lithium battery.

Figure 1

Merits of Solid Electrolyte

As an important part of lithium-sulfur batteries, the electrolyte plays an important role in the transportation of ions. The liquid electrolyte can realize fast kinetics, but also brings about many concerns on the safety and the cycle life of the battery. The electrolytes currently used are all organic electrolytes of ethers or carbonates. Such electrolytes have poor thermal stability and are prone to leakage and cause safety accidents. Although ionic liquids are highly safe and non-flammable, they are expensive and have certain environmental hazards, and are not suitable for large-scale application in battery systems.

There is an urgent requirement to study the new electrolyte to avoid the “shuttle effect” of the polysulfide (Li₂S₆, Li₂S₄) formed during the charging and discharging process on the premise of ensuring high lithium ion conductivity, thereby improving the utilization of active sulfur species and the cycle life of lithium-sulfur batteries. Solid electrolytes are usually classified into four types: gels, solid polymers, inorganic and inorganic-organic composite electrolytes. Table 1 lists the composition and properties of the different electrolytes. In general, an ideal solid electrolyte should have the properties of higher ion conductivity, better electrical insulation, wider electrochemical window, stable chemical properties, and stable chemical reactivity with the positive and negative electrodes.

Gel Electrolyte

One of the main reasons hindering the commercialization of all solid-state batteries presently is the poor ionic conductivity of all solid electrolytes at room temperature, which mean the discharge specific capacity of all solid-state batteries is far from the requirement of practical application. In order to solve the problem of poor ionic conductivity of the solid electrolyte at room temperature, the gel electrolyte with a certain amount of liquid electrolyte was developed. The lithium ion transport of the gel electrolyte is basically the same as that of the liquid electrolyte. At the same time, due to the presence of the electrolyte, the adsorption capacity of the polyvinylidene fluoride is poor, and the shuttling effect of the lithium polysulfide intermediates cannot be effectively limited. In order to solve this problem, polar sites are introduced to entrap the dissolved lithium poly-sulfides. The polymer with oxygen-containing functional group and metal oxide particles have been added into the gel polymer electrolyte as fillers to blocks the diffusion effect in the gel electrolyte. By the adding of organic solvents [such as ethylene carbonate (EC), propylene carbonate (PC), dimethyl carbonate (DMC), dimethyl Carbonate (DEC)] and lithium salts in polymer matrices [such as polymethyl methacrylate (PMMA), polyethylene glycol (PEG), Polyethylene oxide (PEO), etc.], Gel polymer electrolyte (GPE) or Gel electrolyte can possess the advantages of the liquid electrolyte and the solid electrolyte (Zhang et al., 2013; Jeddi et al., 2014). It has high ion conductivity >10⁻⁴ S/cm at room temperature and low interface impedance. The GPE is capable of adsorbing a large amount of liquid electrolyte and isolating the contact between the liquid electrolyte and the sulfur electrode, thereby inhibiting the dissolution of the polysulfide and blocking the “shuttle effect” to some extent.

All-Solid-State Polymer Electrolytes

The all-solid polymer electrolyte does not contain the liquid electrolyte, which has benefits, such as good thermal stability, high mechanical strength and easy to form film, chemical and electrochemical stability, the ability to perform structural design at the molecular level, etc. It can effectively inhibit the dissolution of the polysulfide while the all-solid polymer electrolyte and the electrode are in close contact.

The all-solid polymer electrolyte is usually composed of a polymer matrix with a higher dielectric constant and a lithium salt with a lower lattice energy. Among them, the common polymers are PEO, PMMA, PVDF [Poly(vinylidene fluoride)], PAN (polyaniline) and the like. The ionic conductivity of PAN can reach 10⁻³ S/cm at a certain temperature, due to the higher Li⁺ migration number and electrochemical stability window of the PAN, but the disadvantage is that PAN can react with lithium metal anode (Abraham and Alamgir, 1991; Wang et al., 1996; Ryoo et al., 1998). Therefore, it is difficult to apply to lithium sulfur batteries on a large scale. The mechanical properties of PMMA are too low to inhibit the growth of lithium dendrites. PVDF has a high dielectric constant, which can fully ionize the lithium salt, thereby increasing the ionic migration number, but the interfacial stability between PVDF and lithium metal is poor, and the LiF is generated to cause safety problems (Choe et al., 1995). In the currently studied solid polymer electrolyte(SPE), poly(ethylene oxide) (PEO)-based SPE has good compatibility with electrode interface, excellent electrochemical stability and an acceptable Li⁺ migration number (Scrosati et al., 2001; Hovington et al., 2015). The problem of PEO-based polymer electrolytes remains to be the poor ionic conductivity (<10⁻⁵ S/cm) at room temperature. Therefore, a large number of studies are devoted to exploring the microscopic mechanism of the kinetic transport of the ions in polymers. For PEO-based polymer electrolyte, the dissociation of lithium salt with ether oxygen bonds in the PEO chain, while the chain end motion drives the transport of lithium ions. PEO is amorphous and has satisfactory ionic conductivity above the glass transition temperature but has a relatively low ionic conductivity (10⁻⁷ S cm⁻¹) at room temperature. This is because, at high temperatures (above 60°C), PEO has a similar molecular structure to the polyether liquid electrolyte. Thus, the conductivity can be improved. The Li+ conducting behavior of PEO-based Li-S cells at high temperatures may be similar to that of a typical liquid electrolyte Li-S battery, so it is not effective at inhibiting lithium polysulfide at higher temperatures. In contrast, at room temperature, since PEO has the rigidity of a solid polymer film, lithium dendrite and polysulfide dissolution can be effectively suppressed. Li/PEO/S cells were investigated by in-situ scanning electron microscopy (SEM) and UV-vis spectroscopy at higher temperatures. The results show that the polysulfide will dissolve in the SPE and diffuse into the anode. In addition, the type of polysulfide during discharge is different from the charging process. is formed during discharging, but is formed during charging. An insulating sulfur-rich layer is formed on the Li metal anode to increase internal resistance and limit capacity. In the past few years, researchers have focused on reducing the glass transition temperature and on increasing the ionic conductivity of PEO at room temperature to achieve high cycle performance of Li-S cells around room temperature.

Inorganic Solid Electrolytes

Compared with the GPE and the SPE, the inorganic solid electrolyte has excellent thermal stability, low flammability, wide electrochemical window, and can effectively block the shuttle of the polysulfide, and inhibit the growth of lithium dendrites. Moreover, the inorganic solid electrolyte can maintain a good chemical stability over a wide temperature range. The inorganic electrolyte includes the ceramic electrolyte (also referred to as a crystalline electrolyte) and the glass electrolyte (also referred to as an amorphous electrolyte). The ceramic electrolyte is a good conductor of lithium ion, which has high Li⁺ conductivity and Li⁺ migration number at room temperature, but the preparation process of it is complicated. The glass electrolyte has a large change in composition, so it is easy to obtain a high room temperature ionic conductivity. Therefore, compared to the ceramic electrolyte, the glass electrolyte has the advantages of higher ionic conductivity, conductive isotropic, smaller particle interfacial charge transfer resistance and a more simple preparation process (Lee et al., 2002; Tatsumisago, 2004; Xu and Wen, 2005).

Many inorganic ceramic solid electrolytes, such as NASICON type electrolytes, perovskite electrolytes and garnet type electrolytes have been studied. The perovskite electrolyte whose chemical formula can be described as ABO₃ has a high ionic conductivity (~10⁻³ S/cm, room temperature). The Li_3xLa_2/3−xTiO₃(LLTO) is a typical perovskite electrolyte. At the A site, Li⁺ and La³⁺ are disorderly distributed between the cubic phases and are sequentially placed between the two perovskite structures. The LLTO type electrolyte exhibits a high electrochemical stability at high potential (8–9 V) and excellent air stability (Bohnke, 2008). The NASICON type electrolyte has a stable structure and fast ion conductivity. Its chemical formula can be abbreviated as MA₂(BO₄)₃ where M, A, B represent metal ions and different vacancy states, respectively. The ionic conductivity of the typical NASICON such as Li_1.3Ti_1.7Al_0.3(PO₄)₃ can be as high as 7 × 10⁻⁴ S/cm at room temperature (Arbi et al., 2007). The basic chemical formula of the garnet-type lithium ion solid electrolyte is Li₅La₃M₂O₁₂ (M = Nb or Ta), wherein Li₆BaLa₂Ta₂O₁₂ has an ionic conductivity of 1.69 × 10⁻⁵ S/cm at 25°C, a poor ion conduction activation energy (0.40 eV) (Kokal et al., 2012). The ionic conductivity of Li_6.4La₃Zr_1.6Ta_0.6O₁₂ at room temperature is up to 10⁻³ S/cm (Li et al., 2012). In addition, garnet-type electrolytes have attracted much attention because of the wide electrochemical stability window and high stability relative to the Li anode. It has been reported that (Li Y. et al., 2017) reduced the interfacial impedance of the solid electrolyte with the lithium negative electrode by adding 2 wt% of LiF to Li_6.5La₃Zr_1.5Ta_0.5O₁₂. Han et al. (2017) prepared an ultra-thin Al₂O₃ film on the surface of Li₇La_2.75Ca_0.25Zr_1.75Nb_0.25O₁₇ electrolyte with the atomic layer deposition technique, which effectively decreased the interfacial resistance from 1,710 to 1 Ω/cm². In general, the advantages of inorganic ceramic solid electrolytes are outstanding, however, due to the complicated preparation process, the industrial development is greatly limited.

In order to overcome the shortcomings of ceramic solid electrolytes, researchers have turned their attention to inorganic glass electrolytes. Glass electrolytes have the advantages of anisotropic ionic conductivity, zero grain boundary impedance, easy to form the film, and low cost. Glass electrolytes can be divided into two major categories: the oxide-type amorphous electrolyte and the sulfide-type amorphous electrolyte. The former has good electrochemical and thermal stability but the room temperature ionic conductivity is extremely low (10⁻⁸~10⁻⁶ S/cm) (Jing et al., 2017). Conversely, the latter type at room temperature has a higher conductivity (10⁻³~10⁻⁴ S/cm) but it is very sensitive to the moisture and difficult to prepare. Sulfide glass electrolytes include Li₂S-P₂S₅, Li₂S-SiS₂, and Li₃PS₄ (Chen R. et al., 2016; Manthiram et al., 2017).

Inorganic-Organic Composite Solid Electrolytes

In order to compensate for the shortcomings of inorganic solid electrolytes, researchers have designed a series of inorganic-organic composite electrolytes in combination with the organic electrolytes. Composite electrolytes (CPE) are typically synthesized by chemical or physical methods from ceramic materials to polymers or organic materials such as organic fibers, cellulose, and organic electrolytes. The composite electrolyte contains inorganic and organic moieties that combine the advantages of each material, such as high Li ion conductivity, the good mechanical strength of the inorganic portion, and good interfacial contact of the organic portion. Therefore, the use of the composite electrolyte in the Li-S battery can not only solve the problems associated with the shuttling effect of polysulfide species but also solve the interface contact problem. The interfacial compatibility between the electrolyte and the electrode decreases the interfacial impedance; and the inorganic substance also has the ability to adsorb the polysulfide. Therefore, the inorganic-organic composite electrolyte is expected to simultaneously improve the battery safety and the electrochemical performance. Common composite electrolytes are: polymer-inorganic ceramics, organic liquid-inorganic ceramics, polymer-active fillers, and the like. Generally, complex electrolytes operate at higher temperatures to achieve high ionic conductivity. Among various composite solid electrolytes, PEO-based composite electrolyte is the research focus. Lithium-ion conductive nanoparticles, such as LLZO, Li_0.33La_0.557TiO₃ (LLTO), LiAlO₂ and Li₁₀SnP₂S₁₂ (LSPS), are embedded in the host PEO polymer matrix to reduce the crystallization of the PEO polymer chain and promote the amorphous region, thereby increasing the ionic conductance rate.

Advances in Solid State Li-Sulfur Batteries

Li-Sulfur Batteries Based on GPE

The PVDF-based GPE, prepared by solvent casting and swelling with a liquid electrolyte solution, can effectively stabilize the high-loading (e.g., 70% S) sulfur composite cathode, reduce the dissolution of sulfur, and slow the diffusion of polysulfide to the anode. And with the GPE based electrolyte, Li-sulfur batteries can achieve a capacity which is close to the theoretical limit of the Li-S battery (1,675 mA h g⁻¹) (Agostini et al., 2017). Composite gel electrolytes based on PEO and poly(vinylidene fluoride-co-hexafluoropropylene) (PVDF–HFP) have also improved the safety and cycle performance of lithium-sulfur batteries (Ho Park et al., 2010; Zhang and Tran, 2013). A novel small molecule of the GPE was prepared by mixing the 1,3-dioxolane, dimethyl ether and the lithium salt. When the mass fraction of small molecules was 8.3 wt%, the ionic conductivity was the highest, reaching 6.43 × 10⁻³ S/cm. The initial discharge specific capacity of the sulfur positive electrode at 0.1 C is 1,008 mAh g⁻¹ (Zhu et al., 2017). Wu et al. (2016) designed a novel sandwich layered polymer electrolyte, in which the PVDF layer absorbs a large amount of ether-based liquid electrolyte, thereby increasing the migration of Li ions, and the PMMA layer prevents the liquid electrolyte from reacting with the metal lithium. The initial capacity of the lithium-sulfur battery based on the GPE reaches 1711.8 mAh g⁻¹ and has a good cycle performance. This “sandwich” GPE provides a new idea for the design of the electrolyte structure of lithium-sulfur batteries. In addition to the PVDF, the PMMA is also a good candidate for gel polymer. The electrospun polypropylene eye (PAN)/PMMA film absorbing the polyethylene glycol dimethyl ether (PEGDME) and the lithium salt is used as the electrolyte, and the composite material of carbon nanotubes and sulfur is used as the positive electrode. The excellent chemical compatibility between the PAN/PMMA film and the sulfur cathode improves the conductivity of the positive electrode and suppresses the shuttle of the polysulfide, thereby improving the electrochemical performance (Rao et al., 2012). There is also a report on the preparation of a novel gel polymer consisting of an alkyl carbonate mixture solution and a lithium salt dispersed in PVDF-HFP/PMMA (Zhao et al., 2013; Zhang Y. et al., 2014). The poly(vinylidene fluoride) (PVDF)-based gel polymer electrolyte (GPE), with a dense morphology, was prepared using a simple solution casting method, incorporating the poly(ethylene oxide) and the nano-zirconia to improve the absorption of the liquid electrolyte and the Li⁺ mobility (Gao et al., 2017) (Figure 2A).

Figure 2

2012) Copyright 2017, Polymer. (E) Schematic illustration of coin cells incorporated with GPE and GPE/CNF membrane, respectively. (F) PP separator, GPE membrane, and GPE/CNF membrane before and after thermal treatment. (E,F) Reproduced with permission (Baloch et al., 2016). Copyright 2017, Chemistry—An Asian Journal.

The in-situ synthesis method has the characteristics of simple process and low cost, which provides the possibility of realizing the large-scale application of the solid electrolyte for high-performance lithium-sulfur battery. The in-situ synthesized pentaerythritol tetra-acrylate (PETEA)-based GPE has an ionic conductivity of 1.13 × 10–2 S/cm at room temperature, and the electrolyte/electrode interface is tightly bonded leading the good compatibility, which in turn decreases the impedance of the interface (Liu et al., 2016). At the same time, a flexible and stable passivation layer is formed on the surface of the sulfur electrode, which can limit the movement of the polysulfide (Figure 2B) and improve the cycle performance of the lithium-sulfur battery. The polysulfide can also be used as an additive for gel electrolytes (Agostini and Hassoun, 2015), resulting in a significant improvement in the performance of the electrolyte (Figure 2C). In order to improve the room temperature ionic conductivity of GPEs, some optimization of GPEs is conducted. For example, ball milling of GPEs can cause certain changes in microstructure and promote the ionic interactions, thereby improving the ionic conductivity (Shin et al., 2002a). In addition, decreasing the crystallinity of the gel polymer can also increase the ionic conductivity. The ionic conductivity of the crosslinked amorphous polyepichlorohydrin terpolymer-based GPE reached 10⁻³ S/cm at room temperature (Figure 2D; Choudhury et al., 2017). The nano-scale microfibrillated cellulose is prepared by a thermally induced polymerization method and can be used as the support for GPE electrolyte, which exhibits excellent ionic conductivity, thermal stability and interfacial stability (Nair et al., 2016). Based on the polyimide (PI)-based electrospun polymer film, a new type of GPE was prepared by activating the PVDF-HFP and further coating the nano-Al₂O₃. The specific capacity of the Li-S battery can still reach 820 mAh g⁻¹ after more than 100 cycles (Rao et al., 2015). A free-standing trimethylolpropane ethoxylate triacrylate gel polymer electrolyte was synthesized by the chemical crosslinking method, and the crosslinked gel polymer electrolyte (Figures 2E,F) exhibited an excellent thermal stability at a high temperature of 130°C. Moreover, the GPE combined with carbon nanofibers (CNFs) can effectively prevent the polysulfide dissolution and enhance the electrochemical properties, including the high capacity of 1,177 mAh g⁻¹ in the first cycle and the capacity retention of 64% after 300 cycles (Choi et al., 2017).

Although GPEs are physically able to block the transfer of the polysulfide, the dissolution of the polysulfide is still present due to the employment of the liquid electrolyte. Recently, ionic liquids (ILs) have been found to be an attractive addition for GPE because the combination of ILs and GPE can effectively control the polysulfide diffusion and protect the lithium metal from reacting with the dissolved polysulfides and electrolyte solvents (Shin and Cairns, 2008; Jin et al., 2012; Rao et al., 2012). Many studies have shown that this mixed electrolyte can also decrease the crystallinity of the polymer and improve the thermal/chemical stability of the electrolyte. 1-propyl-3-methylimidazolium bis(trifluoromethanesulfonyl)imide (PMImTFSI) was used for GPE (Kim, 2017), based on which the Li-S battery has an initial discharge capacity of 1,029 mAh/g at 0.1 C and 885 mAh g⁻¹ after 30 cycles. The gel polymer electrolyte (GPE), combining the porous membrane with the N-methyl-N-butyl pyrrolidine bis (trifluoromethanesulfonyl)imide ionic liquid, exhibited good thermal stability and excellent interfacial stability (Baloch et al., 2016). The corresponding lithium-sulfur battery provided an initial discharge capacity of 1217.7 mAh g⁻¹ and maintained a reversible capacity of 818 mAh g⁻¹ after 20 cycles at a current density of 50 mA g⁻¹ (Jin et al., 2012). Cheng et al. (2018) proposed a novel gel polymer electrolyte (GPE) in which a nanostructured ionic liquid (IL) was introduced into the gel polymer electrolyte matrix prepared by electrospinning. After bonding with the nanostructured IL, the new GPE exhibited good mechanical properties, improved the absorption of the electrolyte (552 wt%), and had an ionic conductivity up to 0.64 mS cm⁻¹ at room temperature, as well as a high lithium ion transfer number (t_Li+ = 0.60).

It can be seen from the above analyses that the GPE has high ionic conductivity at room temperature, good interfacial contact, and can significantly inhibit the shuttle of the polysulfide, which can significantly improve the cycle life of lithium-sulfur batteries. However, the GPE still contains a certain amount of liquid electrolyte, which is difficult to fundamentally solve various problems of liquid electrolyte, such as the polysulfide shuttle and poor thermal stability. It is necessary to further study the polymerization mechanism pf the precursor and the in-situ synthesis method, giving full play to the advantages of lower GPE interface impedance and higher ionic conductivity.

Li-S Batteries Based on Solid Polymer Electrolyte

At room temperature, the polymer electrolyte like PEO usually has the poor ionic conductivity due to the high crystallinity and the high glass transition temperature (Verma et al., 2014b). In order to decrease the crystallinity and the glass transition temperature to obtain PEO-based electrolytes with high ionic conductivity, researchers have conducted extensive researches and have found that adding certain inorganic fillers, such as oxides and sulfides to polymer electrolytes, can effectively enhance the ionic conductivity. The glass transition temperature decreases with the increase of the amorphous region, thereby increasing the ionic conductivity and the mechanical strength at room temperature (Croce et al., 1998). The (PEO)₂₀LiTFSI-10% (w) γ-LiAlO₂ type SPE was applied to a lithium-sulfur battery (Zhu et al., 2005), showing an initial discharge specific capacity of 450 mAh g⁻¹ at a current density of 0.1 C. Subsequently (PEO)₁₈LiTFSI-10% (w) SiO₂ type SPE was used in a lithium-sulfur battery whose positive electrode material was sulfur/mesoporous carbon sphere, and the first discharge specific capacity was 1,265 mAh g⁻¹ (Liang et al., 2011a).

Typical oxide fillers such as TiO₂, Al₂O₃, SiO₂ (Verma et al., 2014a) and ZrO₂ are widely used in all-solid-state polymer Li-S batteries, Liang (1973) added the A1₂O₃ to polycrystalline LiI to conduct ion without chemical reaction. To explain this phenomenon, Maier (1995) proposed a space charge effect, which is believed that can affect the ionic conductivity of the two-phase interface, so that the ionic conductivity can be improved by introducing an inert ceramic filler into the inorganic polymer. Bronstein et al. synthesized a novel hybrid solid polymer electrolyte consisting of organically modified aluminum silicon (OM-AlSi) formed in the PEO-LiTFSI phase, which was highly effective in increasing the dielectric constant and ionic conductivity (Bronstein et al., 2004). Shin et al. (2002b) added titanium oxide (TinO_2n−1, n = 1, 2) to PEO [lithium bis(fluorosulfonyl)-imide] (LiFSI) SPE, which could increase the ionic conductivity of PEO-based SPE and improve the interfacial stability between the Li metal anode and the SPE. The research group also prepared nano-Al₂O₃ as a filler of PEO(LiBF₄) SPE by ball milling. It was found that the addition of Al₂O₃ filler decreased the spherulite size and crystallinity of PEO, thus improving the ionic conductivity of the PEO-based electrolyte (Jeong et al., 2005). As well as that, the solid polymer electrolyte prepared with Al₂O₃ filler improved the cycle performance of lithium-sulfur batteries (Jeong et al., 2007). This is because the unique structure of PEO-Al₂O₃-based SPE allows the free transport of lithium ions and prevents the transport of polysulfide anions through the physical absorption and electrochemical deposition, which can effectively reduce the shuttle effect and the loss of active materials (Zhang Z. et al., 2014). Bing-joe Hwang et al. also added TiO₂ to the PEO-based solid electrolyte improving the performance of the battery effectively (Lee et al., 2017) (Figure 3A). The specific capacity of the polymer electrolyte with nano-sized TiO₂ is >1,450 mAh g⁻¹, and the capacity retention after 100 cycles is 87%. In contrast, the capacity retention using the pure PEO is 38%. Calculations and Raman measurements indicate that nano-sized TiO₂ particles can interact with and anchor to polysulfide species through adsorption mechanisms, preventing them from diffusing to the Li anode (Figures 3B,C). Besides, the incorporation of TiO₂ nanoparticles increases the amorphous phase of PEO and the ionic conductivity.

Figure 3

In addition to oxides, sulfides and other inorganic materials are often used as fillers for polymer electrolytes in all-solid lithium sulfur batteries. Hassoun and Scrosati (2010) prepared a SPE film by hot pressing PEO (LiFSI) with adding the nano ZrO₂ and Li₂S to stabilize the Li metal anode/electrolyte interface, while increasing the ionic conductivity and Li+ transfer number. Sheng et al. (2017) prepared novel poly(ethylene oxide) (PEO) solid polymer electrolytes (SSPEs) containing ionic liquid grafted oxide nanoparticles (IL@NPs) (Figure 3D), and the IL containing Cl⁻ increased the free lithium ion conductivity by weakening the interaction between the lithium ion and the PEO chain. At the same time, the ion-grafted oxide nanoparticles also increased the ion channel leading the high ionic conductivity at low temperatures. In addition, the difference between the IL@NPs based on ZrO₂, TiO₂, and SiO₂ was compared (Figure 3E). Among these modified electrolytes, the ZrO₂ filled electrolyte has the highest ionic conductivity. Similarly, the Lewis acidic metal-organic framework [MIL-53 (Al)] can be added to the polymer electrolyte to improve the cell performance (Zhu et al., 2014). MIL-53 (Al) was used as the filler for polyethylene oxide (PEO) based SPE. With the participation of MIL-53 (Al), the ionic conductivity of the solid electrolyte increased from 9.66 × 10⁻⁴ S/cm to 3.39 × 10⁻³ S/cm at 120°C, and the oxidation potential increased from 4.99 V to 5.10 V. Simultaneously, the addition of MIL-53 (Al) can effectively inhibit the dissolution and shuttle of the polysulfide in all-solid lithium-sulfur batteries. The discharge capacity at 0.2 and 80°C is 1,520 mA h/g, and the 1,000th cycle discharge capacity at 4C is still as high as 325 mA h g⁻¹, indicating that the battery has excellent rate performance and cycle life (Zhang C. et al., 2015). According to the EIS spectrum, there was no semicircle caused by the polysulfide shuttle and the electrolyte/Li interface reaction, demonstrating that the polysulfide did not dissolve. After 10 discharge/charge cycles, the XPS spectrum on the surface of the Li anode showed that the sulfur and polysulfide didn't transfer from the cathode to the anode. The group also used the natural halloysite nanotubes (HNT) as the solid electrolyte filler. Lithium ions were immobilized on the outer tube wall (negative electrode) of HNT with a 3D channel structure. The TFSI⁻ anion was adsorbed on the inner tube wall (positive electrode). Since the surface of the HNT particles has the charge opposite to that of the lithium salt, the dissociation of the lithium salt is promoted, and the 3D channel accelerates the transmission of Li⁺ (Lin et al., 2017). Zhang Y. et al. (2015) fabricated a solid polymer electrolyte using PEO, LiTFSI and montmorillonite (MMT). The PEO-based solid electrolyte containing 10 wt% of MMT exhibited an ion conductivity of 3.22 × 10⁻⁴ S/cm at 60°C, which satisfied the operational requirements of the all-solid lithium-sulfur battery. An initial discharge capacity of 998 mAh g⁻¹ was provided at 0.1 C, and a reversible specific discharge capacity of 634 mAh g⁻¹ was still available after 100 cycles.

Apart from adding inorganic fillers, the design of the molecular structure also has a great effect on the performance of the PEO-based SPE. The PEO forming the pleated structure by the cross-linking method improves the mechanical strength while decreasing the crystallinity. Ben Youcef et al. (2016) prepared a SPE with semi-interpenetrating network by UV-induced the cross-linking of poly(ethylene glycol) diacrylate (PEGDA) and divinylbenzene (DVB) in a PEO (LiTFSI) matrix. The addition of DVB crosslinker decreased the crystallinity of PEO from 34 to 23% and the melting temperature from 50 to 34°C. The SPE showed a high electrochemical stability of 4.3 V. The actual conductivity value exceeds 10⁻⁴ S/cm at 70°C.

In summary, all solid polymer electrolytes, such as PEO based electrolyte and its derivatives, have the disadvantage of poor ionic conductivity at room temperature, the battery based on which generally needs to operate at high temperatures. Such polymer electrolytes become viscoelastic at high temperatures and migrate through the polymer segments to drive their coordinated lithium ions. In addition, the mechanical strength of PEO-based polymer electrolytes at high temperatures is decreased, and the short circuits of the battery are likely to occur (Agrawal and Pandey, 2008). In order to realize the practical application of the polymer solid electrolyte, it is necessary to further increase the room temperature ionic conductivity of the polymer, develop a single ion conductor polymer electrolyte with ion mobility close to 1, and improve the mechanical properties of the polymer solid electrolyte.

Li-S Batteries Based on Inorganic Solid Electrolyte

Fu et al. (2017a) reported for the first time a 3D double-layer garnet electrolyte (Figure 4A). The thickness of the dense layer reduced to a few microns and still maintained good mechanical stability. The thicker porous layer acts as a mechanical support for the thin dense layer and a body for the high loading cathode material. The Li-S battery exhibited high initial coulombic efficiency (>99.8%) and high average coulombic efficiency (>99%) in subsequent cycles. Recently, Yu et al. (2016) applied another NASICON-type lithium ion conductor, Li_1+xY_xZr_2−x(PO₄)₃ (LYZP) as a solid-electrolyte (Figure 4B). The initial discharge capacity of the Li-S battery assembled with this oxide solid electrolyte reached 1,100 mAh g⁻¹ and retained ~90% of the initial capacity after 150 cycles at 0.2 C.

Figure 4

2004). Copyright 2016, Advanced Energy Materials. (C) Conductivity map for xLi₂S·(100 –x)P₂S₅ (x = 65, 67.5, 70, 72.5, 75) ball-milling glass, quenched glass and heat-treatment glass ceramic at room temperature. Reproduced with permission (Xu et al., 2017). Copyright 2017, Solid State Ionics. (D) Arrhenius conductivity plots of Li₇P₃S₁₁ and Li₇P_2.9S_10.85Mo_0.01 at temperatures from 298 to 388 K and the corresponding CV curves of Li metal cells show the electrochemical window. Reproduced with permission (Kobayashi et al., 2008). Copyright 2017, Journal of Materials Chemistry A.

Recently, Machida et al. (2004) studied the lithium-sulfur battery based on Cu₂S/S cathode and the solid electrolyte of Li₂S-SiS₂. The first cycle discharge had a specific capacity of 480 mAh g⁻¹, which was higher than the theoretical capacity of Cu₂S. Similarly, Hayashi et al. (2003) successfully prepared an all-solid-state battery using a sulfur-based cathode material and a Li₂S-P₂S₅ glass-ceramic electrolyte, which showed good cycle performance at room temperature. The battery maintained a high capacity of more than 650 mAh g⁻¹ after 20 cycles. Zhang et al. (2017) obtained a glass phase of xLi₂S-(100-x)P₂S₅(65 ≤ x ≤ 75, mol%) by the mechanical ball milling, followed by rapid quenching and tempering. Among them, the 70Li₂S·30P₂S₅ sample showed the ionic conductivity up to 1.58 × 10⁻³ S/cm (Figure 4C). The excellent performance is attributed to the precipitation and heat treatment of the high conductivity thio-LISICON III phase, which reduces the grain boundary and improves the grain morphology. The lithium-sulfur battery with 70Li₂S·30P₂S₅ glass ceramic as the solid electrolyte has the first discharge specific capacity of 1,055 mAh g⁻¹ and has excellent coulombic efficiency. Hayashi et al. (2008) constituted an all-solid battery adopting the Li₂S-Cu composite electrode prepared by the mechanical milling method and the Li₂S-P₂S₅ glass ceramic electrolyte. The first cycle showed a specific discharge capacity up to 490 mAh g⁻¹. Xu et al. (2017) studied the MoS₂-doped Li₂S-P₂S₅ glass ceramic electrolyte (Li₇P_2.9S_10.85Mo_0.01), which exhibited an ionic conductivity of 4.8 × 10⁻³ S/cm at room temperature and a wide electrochemical window as high as 5 V (relative to Li/Li⁺). In order to prove the high stability of the MoS₂-doped electrolyte with the lithium metal, the all-solid lithium-sulfur battery was assembled with Li₇P₃S₁₁ and Li₇P_2.9S_10.85Mo_0.01 as solid electrolytes, respectively. The Li-S battery with Li₇P_2.9S_10.85Mo_0.01 electrolyte showed a high discharge capacity of 1,020 mAh g⁻¹, which was superior to that of the Li₇P₃S₁₁ electrolyte (Figure 4D).

In order to improve the interface problem between the electrode and the electrolyte, and further improve the utilization of the active material simultaneously, the sulfide electrolyte is often used as the cathode additive to prepare the composite electrode (Kobayashi et al., 2008; Agostini et al., 2013). However, this type of electrolyte has a low ionic conductivity. In order to increase the ionic conductivity, Nagata and Chikusa (2016) added the LiI to the Li_1.5PS_3.3 solid electrolyte for the first time, which improved the ionic conductivity effectively. Kato et al. (2016) reported a new sulfide-type lithium ion fast conductor (LISICON) solid electrolyte Li_9.45Si_1.74P_1.44S_11.7C_l0.3 with ultra-high conductivity (2.5 × 10⁻² S/cm) and high electrochemical stability. The crystal structure of the Li₁₀GeP₂S₁₂ (LGPS) is shown in the figure, and its ionic conductivity is the highest among the existing LISICON solid electrolytes. In general, the inorganic solid electrolyte has the high transfer number of lithium ions higher than that of SPE and GPE, high ionic conductivity at room temperature and the ability of theoretically completely blocking the diffusion of (4 ≤ n ≤ 8) to the metal lithium negative electrode. However, the inorganic solid electrolyte also has many disadvantages, including a difficult preparation process, low mechanical strength, and large interface impedance with the electrode, which all limit the practical application of the inorganic solid electrolyte. Thus, we need to find a higher quality composite solid electrolyte to solve the above shortcomings.

Li-Sulfur Batteries Based on Composite Electrolyte

So far, researchers have found a large number of active inorganic fillers that can increase the ionic conductivity of solid electrolytes. The active filler itself has the ionic conductivity and can be used as the solid electrolyte alone. Typically, researchers add the active fillers to the all-solid polymer electrolyte to form a polymer-active filler composite electrolyte to further enhance the performance of all-solid-state batteries. Capuano (1991) firstly combined the spherical active filler γ-LiAlO₂ with a diameter of <1 μm with the PEO and the LiClO₄ to prepare a composite solid electrolyte, and found that the performance using this composite electrolyte was greatly improved. Choi et al. (2015) fabricated a composite electrolyte complexing the tetragonal phase of Li₇La₃Zr₂O₁₂ with a PEO matrix, which showed a ionic conductivity as high as 4.42 × 10⁻⁴ S/cm at 55°C.

The Li₁₀GeP₂S₁₂ with a very high ionic conductivity (10⁻² S/cm) is dispersed into the PEO-based electrolyte, which enables the electrolyte a high ionic conductivity of 1.21 × 10⁻³ S/cm at 80°C (Zhao et al., 2016). Blanga et al. (2016) prepared a composite Li₁₀SnP₂S₁₂ (LSPS)/polyethylene oxide (PEO) electrolyte containing 25–50 wt% polymer which could act as a good barrier to suppress the shuttle of the polysulfide in Li-S battery. Meanwhile, a new composite Li_10+xI_xSnP₂S₁₂ (LISPS)/P(EO)₃/LiI solid electrolyte was formed by adding the saturated LiI salt and annealing at 90°C. The solid electrolyte has an ionic conductivity of 0.1–0.3 mS/cm at room temperature, and the increase in polymer content or temperature can further improve the total ionic transport in the LISPS/PEO system (Figure 5A). Judez et al. (2017) studied a composite electrolyte of lithium bis(fluorosulfonyl)imide/poly(ethylene oxide) (LiFSI/PEO) containing lithium ion conductive glass ceramics (LICGC) and inorganic Al₂O₃ fillers. The CPE with Al₂O₃ filler improved the stability of the Li/electrolyte interface. The Li-S cells based on LICGC-based CPE provided a specific capacity of 1,111 mAh g-1 and an area capacity of 1.14 mAh/cm². Fu et al. (2016) reported a 3D lithium ion-conductive ceramic network based on the garnet-type Li_6.4La₃Zr₂Al_0.2O₁₂ (LLZO) lithium ion conductor, which provided a continuous Li⁺ transmission channel in a polyethylene oxide (PEO) based composite (Figure 5B). While increasing the mechanical properties, the ionic conductivity is also improved, and the ionic conductivity at room temperature is 2.5 × 10⁻⁴ S/cm. Wang Q. et al. (2016) newly designed a gel-ceramic multilayer electrolyte as shown in Figure 5C, which blocked the polysulfide shuttle, exhibiting excellent electrochemical performance and an initial discharge specific capacity up to 725 mAh g⁻¹ with almost no self-discharge, and maintained 700 mAh g⁻¹ after 300 cycles at C/2 (Figure 5D). Xia et al. (2017) prepared a PVDF-HFP/LAGP composite electrolyte by adding the nano-fast ion conductor filler to the gel electrolyte, which had a high lithium ion migration number (0.51) and exhibited the electrochemical stability compared with the commercial liquid electrolyte. The solid lithium-sulfur battery assembled with the composite electrolyte showed an initial capacity of 918 mAh g⁻¹ at 0.05 C, and good cycle performance. Zhou et al. (2016) fabricated a new SiO₂ hollow nanosphere electrolyte (SiSE) by the adsorption and in situ polymerization of tripropylbenzodiacrylate (TPGDA) monomer with the addition of the SiO₂ hollow nanosphere (Figure 5E). The silica layer not only enhanced the mechanical property of the electrolyte but also provided a high ionic conductivity (1.74 × 10⁻³ S/cm) at room temperature, which effectively inhibited the growth of lithium dendrites (Figure 5F).

Figure 5

2016). Copyright 2016, Journal of Solid State Electrochemistry. (B) Schematic of the hybrid solid-state composite electrolyte with 3D ceramic backbone. Reproduced with permission (Xia et al., 2017). Copyright 2016, Proc Natl Acad Sci. (C) Schematic illustration for the fabrication of the Li–S cell. (D) Long-term cycle life of the Li-S cell at 1/2C. (C,D) Reproduced with permission (Zhou et al., 2016). Copyright 2016, Chemical Communications. (E) Schematic illustration for the preparation route of SiSE. (F) The suppression mechanism for Li dendrite growth by capitalizing on SiSE as solid electrolyte. (E,F) Reproduced with permission (Wang Q. et al., 2017). Copyright 2016, Adv. Energy Mater.

Although the polymer-inorganic composite electrolyte can effectively inhibit the shuttle of the polysulfide and control the growth of lithium dendrites to prevent the internal short circuit of the battery, the lithium ion conductivity is still too low, compared with the organic liquid-inorganic composite electrolyte at room temperature. The poor conductivity and migration number of the Li ions greatly limit the application of polymer-inorganic composite electrolytes. Wang et al. (2014) successfully realized the development and utilization of the organic liquid-inorganic composite electrolyte. When used in lithium-sulfur battery, the initial discharge specific capacity reached 1,528, 1,386, and 1,341 mAh g⁻¹ at C/20, C/5, and C/2 rates, respectively, and remained 720 mAh g⁻¹ after 40 cycles at C/5 rate. However, the researchers found that the active material is inevitably lost during the cycle process, resulting in a rapidly decline in capacity. In order to make full use of the active material and improve the cycle life, the group (Wang Q. et al., 2017) coated a carbon layer on the one side of the Li1.5Al0.5Ge1.5(PO4)3 (LAGP) facing the sulfur cathode. The innovative configuration not only improved the electron transport capacity of the sulfur-containing active material, but also improved the wettability of the ceramic electrolyte to the liquid electrolyte, thereby improving the cycle performance of the sulfur-containing active material. The interracially modified hybrid Li-S battery had an initial discharge capacity of 1,409 mAh g⁻¹ and remained at 1,000 mAh g⁻¹ after 50 cycles at a rate of 0.2 C.

All in all, the overall performance of the inorganic-organic composite electrolyte has been improved compared to the single all-solid polymer or inorganic electrolyte; stability, interfacial compatibility, safety and mechanical properties, and the ability of inhibiting the polysulfide shuttle have all improved. Therefore, it demonstrates great potential for use as an electrolyte for lithium-sulfur batteries, but the ionic conductivity at room temperature is still too low to meet the practical application.

Sulfur Cathode Design for Solid State Li-S Batteries

For the sulfur cathode of the solid-state Li-S battery, the electrochemical reaction occurring in the “solid/solid/solid” three-phase boundary is more difficult to occur than “solid/liquid/solid” in the traditional liquid counterparts. Therefore, it is necessary to design the structure of the sulfur cathode elaborately and to develop the efficient preparation technology of the electrode to obtain the sulfur cathode with excellent ionic and electronic transport network. As well as that, it is necessary to maintain the relative stability of the electrode structure, eliminating the influence of volume expansion and contraction of the active material during discharge and charge cycles.

Other Types of Sulfur Cathode

Apart from choosing the elemental sulfur as the cathode material for Li-S batteries, the researchers have also studied the sulfide used as the cathode material instead of the sulfur. The common sulfides include the inorganic sulfides and the organic sulfides (Jing et al., 2017). The inorganic sulfides, such as FeS and CuS have an electronic conductivity of 2.1 × 10⁻² S/cm (Zeng et al., 2014) and 10⁻³ S/cm, respectively (Lai et al., 2011). Table 2 summarizes the electrochemical performance of some inorganic sulfides as the positive electrode for the all-solid cells (Machida and Shigematsu, 2004; Machida et al., 2004; Kim et al., 2005; Hayashi et al., 2008; Sakuda et al., 2010; Tomonari et al., 2010; Aso et al., 2011; Lin et al., 2013a; Matsuyama et al., 2013; Chen M. et al., 2015; Long et al., 2016). The same in-situ growth method as the method used in fabricating the sulfur elemental positive electrode can also reduce the impedance of the interface and improve the cycle performance of the solid lithium-sulfur battery. Yao et al. (2016) fabricated the CoS₂-Li₇P₃S₁₁ composite material using the in-situ liquid phase method fabricated (Figure 6A). The composite material maintained the nano-sheet structure of CoS₂, and the Li₇P₃S₁₁ particles with the diameter of about 10 nm were distributed uniformly on the surface of the CoS₂. The all solid-state lithium-sulfur battery was assembled with the CoS₂-Li₇P₃S₁₁ composite material prepared with w(CoS₂-Li₇P₃S₁₁):w(Li₇P₃S₁₁):w(super P) = 4:5:1 as the cathode, the Li₇P₃S₁₁ as the electrolyte, the lithium metal as the anode, exhibiting the specific capacity of 421 mAh g⁻¹ at 1.27 mA /cm at 25°C after 1,000 cycles. The Li₂S-Li₆PS₅Cl-C composite prepared by Han et al. (2016) (Figure 6B) exhibited an ionic conductivity of 10⁻⁵ S/cm at room temperature at 50 mA g⁻¹ and a high load of Li₂S (3.6 mg cm⁻²) in the next 60 cycles also show a large reversible capacity of 830 mAh g⁻¹ (Li₂S utilization reaches 71%). Lin et al. (2013b) synthesized the Li₃PS₄+n with adding the Li₃PS₄ and S to the THF, showing the ionic conductivity of 3 × 10⁻⁵ S/cm at room temperature. The assembled all-solid lithium-sulfur battery showed the specific capacity of 600 mAh g⁻¹ after 300 cycles at 0.1 C at 60°C.

Figure 6

2013a). Copyright 2016, Nano Letters. (B) Schematic illustration of the bottom-up synthesis of the mixed conducting Li₂S nanocomposite. Reproduced with permission (Yu et al., 2004). Copyright 2016, Nano Letters. (C) Cycling efficiency of lithium deposition/dissolution for Li-B alloy (30 wt% B) and metallic Li electrodes. Reproduced with permission (Bucur et al., 2016). Copyright 2014, Journal of Materials Chemistry A.

Like the inorganic sulfide, the organic sulfide is also a research hotspot for Li-S battery. The sulfurized polyacrylonitrile is the most commonly used organic sulfide among the organic sulfide cathode materials. Yu et al. (2004) fabricated the cathode materials using the sulfurized polyacrylonitrile as the active material of the positive electrode and a small amount of solid electrolyte and carbon black. The sulfur electrode was prepared by the mixing method, and the assembled all-solid lithium-sulfur battery was charged and discharged at a current density of 1 C at 70°C, which exhibited the specific capacity of 385 mAh g⁻¹ after 40 cycles. Zhang C. et al. (2015) assembled the all-solid lithium-sulfur battery with the PANI@C/S-280 as the cathode, the MIL-53 (Al) metal-organic framework modified solid electrolyte as the electrolyte, and the lithium metal as the anode. When charged and discharged at 0.2 C at 80°C, the battery showed a stable capacity of 876 mAh g⁻¹. After 1,000 cycles at 80°C, the battery exhibited the discharge capacity of 325 and 558 mAh g⁻¹ at 2 and 1 C-rates, respectively. These results indicate that the combination of the PANI@C/S-280 cathode and the solid polymer electrolyte is an effective way to prevent the polysulfide dissolution and shuttle effect, thereby improving the performance of the battery.

Add Conductive Agent and Binder

When preparing the sulfur positive electrodes, the selection of the conductive agent is also an important issue to consider. The sulfur positive electrode was prepared by the ball milling with the conductive carbon black acetylene black (AB), the Ketjenblack (KB) and the activated carbon (AC), and solid-state battery was assembled with solid electrolyte and Li-In alloy. It was found that the battery with AB as the conductive agent cannot be charged and discharged; the specific capacity of the battery, using KB and AC as the conductive agent at a current density of 0.64 mA cm⁻², was about 1,600 mAh g⁻¹; and the specific capacity of the electrode with AC as the conductive agent is higher than that using KB (Nagata and Chikusa, 2014a). This indicates that the conductive agent in the positive electrode can affect the electrochemical performance of the all-solid lithium-sulfur battery. Meanwhile, in order to further improve the contact between the sulfur positive electrode and the solid electrolyte, the sulfur and the porous carbon are generally prepared as a carbon-sulfur composite at high temperatures, and then mixed with the solid electrolyte. Liang et al. (2011b) prepared the carbon-sulfur composites (S-OMCs) with a sulfur content of 67% employing the carbon with a regular mesoporous structure as the carrier. An all-solid lithium-sulfur battery was assembled with a PEO-based solid electrolyte with the adding of 10% (mass fraction) of SiO₂ inorganic filler, a metallic lithium negative electrode, and a sulfur-based positive electrode prepared on the basis of the carbon-sulfur composite. The battery was charged and discharged at a current density of 0.1 mA cm⁻¹ at 70°C, which exhibited the specific capacity of sulfur of 800 mAh g⁻¹ after 25 cycles, and the capacity retention of 65%. The sulfur positive electrode, which does not use the regular mesoporous carbon, has the capacity retention of only 22% after 25 cycles. Nagao et al. (2016) developed a carbon-sulfur composite using the mesoporous carbon with a pore diameter of 8.6 nm as the carrier, which showed a specific capacity of 366 mAh g⁻¹ at a current density of 0.065 mA cm⁻² and at room temperature after 20 cycles. When the mesoporous carbon with the pore diameter of 42.2 and 117.2 nm were used as the carriers, the specific capacities under the same conditions were 126 and 57 mA h g⁻¹(S) after 20 cycles, respectively. In addition, many studies have shown that the temperature of the heat treatment of carbon-sulfur composites can also affect the electrochemical performance of the battery. For example, Nagao et al. (2013a) prepared a S-CMK3 composite cathode material with a sulfur content of 30% by the hot melt method. It was found that the temperature of the heat-treat of S-CMK3 increased from 170 to 230°C, and it was still reversible after 30 cycles under the same condition. The specific capacity was increased from 500 mA·h g⁻¹(S) to 1,300 mA·h/g(S). The result of the XRD test shows that (Nagao et al., 2013b), after heating to 230°C, the sulfur randomly disperses on the inner wall of CMK3, which improves the electrochemical performance and the cycle stability.

As described above, the electronic conductivity of S and lithiated S species is poor, and various conductive polymers are used as binders to overcome this limitation. In addition to the problem of electronic conductivity, the intermediate product Li₂S_x (2 < x < 8) can be dissolved in a common organic electrolyte. To prevent this dissolution that can lead to self-discharge, inefficiency, and poor cycle stability, the researchers designed adhesives and conductive carbon additives to capture polysulfides through precise chemical reactions (Pang et al., 2016; Hao et al., 2018). Strong coordination between polar functional groups containing N, O or S in the polymer binder, resulting in an interaction strength of ~ 1–2 eV with Li₂S_x, while Li-X (X = N, O, S or Other types) are stronger, which increases the retention of polysulfide (Li et al., 2013; Seh et al., 2013; Ma et al., 2014; Park et al., 2015). Due to the strong ionic character of polysulfide species, positively charged polyelectrolyte material is used as a binder to trap (Bucur et al., 2016; Li L. et al., 2017) and a negatively charged polymer is coated on the separator to Repel multi-sulfide to prevent crossover.

Interface Contact and Sulfur Cathode Preparation

While optimizing the sulfur positive electrode, the interface contact between the electrode and the solid electrolyte should also be considered. For the all-solid lithium-sulfur battery, the poor contact between the solid/solid interface enables a large interfacial impedance, which greatly decreases the cycle performance of the battery. The preparation of the sulfur cathode in lithium-sulfur batteries is crucial to achieve the high performance. At present, the preparation method of the sulfur positive electrode of the solid lithium-sulfur battery is mainly the physical mixing method (such as grinding, ball milling, etc.), heat treatment method and the like. For example, Zhu et al. (2005) prepared a sulfur positive electrode with w (single sulfur): w (PEO) = 3:7 by ball milling and heat treatment at 180°C in an inert atmosphere. The prepared sulfur positive electrode was assembled into an all-solid lithium-sulfur battery with a P(EO)20LiTFSI-10 wt% γ-LiAlO2 solid electrolyte and a metallic lithium anode. At room temperature, the first discharge specific capacity of the sulfur positive electrode using the ball milling process was 609 mAh g-1, which was higher than the sulfur positive electrode using the heat treatment process. Kinoshita et al. (2014) prepared the positive electrode with w (single sulfur): w (carbon fiber): w (Li3PS4) = 3:1:6 via a two-step ball milling method, wherein the sulfur loading was 4.29 mg cm⁻², the initial specific capacity was 1,320 mAh g⁻¹ at a current density of 0.1 mA cm⁻² at 25°C. The average operating voltage of the battery was 1.5 V and the capacity retention after 50 cycles was 90%. Further studies have shown that the conductivity of the solid electrolyte in the positive electrode is not the only factor affecting the electrochemical performance of the battery. For example, Nagata and Chikusa (2014b), Nagata and Chikusa (2014c) compared the effect of Li₂S-P₂S₅ solid electrolyte with different phosphorus-to-sulfur ratio (P/S) on the electrochemical performance of the battery. As the P/S value of the solid electrolyte in the electrode increases, the specific capacity of sulfur increases first,and then decreases to 7%.

The in-situ growth method can be used to decrease the impedance of the “solid/solid/solid” three-phase interface and improve the compatibility of the interface. The in-situ growth technique can effectively improve the contact between the solid electrolyte and the electrode, facilitate the rapid transfer of lithium ions, and improve the rate performance and cycle life, thereby improving the electrochemical performance. Nagata and Chikusa (2014b) assembled the solid battery with the sulfur positive electrode prepared by the ball milling method, and the solid electrolyte Li₁₀GeP₂S₁₂ prepared by the constant current and constant pressure electrolysis method in situ in a pole piece and with the lithium indium alloy (Li-In) negative electrode. The battery charged and discharged at a current density of 1.6 mA cm⁻² at 25°C exhibited the specific capacity of 1,200 mAh g⁻¹ after 10 cycles.

In summary, in order to improve the “solid/solid/solid” three-phase interface problem, a series of studies have been conducted on the sulfur positive electrode. From the loading of the sulfur element to the design and preparation of the sulfur positive electrode, these improvements have greatly improved the cycle performance of the solid lithium-sulfur battery. But for the purpose of reducing impedance, the in-situ growth of the positive electrode is performed to reduce impedance. In-situ synthesis can effectively improve the contact between interfaces. On the one hand, in-situ synthesis can simplify the process and facilitate the modification of the interface. On the other hand, through the analysis of the microstructure, it can be concluded that the in-situ synthesis enables the interface compatible. In addition, the interface can be constructed by adding a small molecule polymer and coating a small liquid molecule on the surface of the sulfur positive electrode to completely infiltrate the sulfur positive electrode, and polymerizing the small molecule through an initiator to improve the interface compatibility.

Stable Lithium Anode for Solid State Li-S Batteries

The use of lithium alloy can reduce the reducibility and activity of the metallic lithium. The Lithium alloy negative electrodes for all-solid lithium-sulfur batteries reported in the literature are mainly Li-In, Li-Ge, Li-Si and Li-Al. Among them, Li-In alloy (Li/In = 0.79, molar ratio) is the most widely used, and its redox potential is + 0.6 V (Li⁺/Li) (Wen and Huggins, 1980). Nagata and Chikusa (2014a) used the Li-In alloy as the negative electrode, and the sulfide Li₁₀GeP₂S₁₂ as the solid electrolyte assembling the all-solid Li-S battery. The charge and discharge were performed at a current density of 1 C, and the specific capacity was about 1,600 mAh , and the capacity retention was closed to 100%. Zhang X. et al. (2014) used the Li-B alloy as the negative electrode and formed a passivation film on the negative electrode, which effectively reduced the performance loss caused by the volume change of the alloy. The battery assembled with the Li-B alloy has a very stable cycle performance as shown in Figure 6C.

Nagao et al. (2012) deposited a lithium film by vacuum evaporation to increase the contact area between the lithium electrode and the Li₂S-P₂S₅ solid electrolyte. The effect of the insertion of lithium film on the reversibility of lithium dissolution and the deposition of all solid-state cells were also investigated. The electrochemical test showed that the charge and discharge were performed at a current density of 0.064 mA cm⁻², and the specific capacity was 920 mAh g⁻¹ (S) after 20 cycles, and the capacity retention was 97%. Wang et al. (2013) added a gel polymer electrolyte and a ceramic film on the surface of the lithium negative electrode. The ceramic film is a solid film of Li₂O-Al₂O₃-SiO₂-P₂O₅-TiO₂-GeO₂, which prevents the direct contact between the lithium negative electrode and the electrolyte, making the interface contact more compacter, decreasing the interfacial impedance, and greatly enabling the batter cycle performance. The energy density can reach 446 Wh kg⁻¹, which is about 80% higher than the traditional lithium-ion batteries, and its power efficiency can reach more than 95%. Han et al. (2017) demonstrated that the large interfacial resistance came from the physical and/or chemical instability between the solid electrolytes and the metallic Li. Hu et al. showed a strategy to deposit the ultrathin intermediates [such as alumina (Al₂O₃), zinc oxide (ZnO), germanium (Ge), silicon (Si), metal aluminum (Al)] on Garnets, forming a continuous and conformal interface [lithium aluminum, Li Zn alloy (Wang C. et al., 2017), Li Ge alloy (Luo et al., 2017), Li Si alloy (Kim et al., 2014), Li Al alloy (Fu et al., 2017b)], which can enhance the surface wettability of the stone toward Li metal. Compared to the pure LLZO particles, the LLZO coating with Al₂O₃ prepared by the atomic layer deposition (ALD) exhibits a much smaller interfacial impedance of 1 Ω cm⁻². The similar observations have been observed in the work of Ge-coated garnet and Al-coated garnet systems. The aluminum-coated garnet hybrid SSE system effectively prevented the migration/shuttle effect of LiPSs and successfully solved the wetting problem between the Garnet SSE and the Lithium metal (Fu et al., 2017b). It is worth noting that the layer formed in situ by chemical reaction is critical to improving the stability between the Li metal anode and the SSE. Hood et al. (2016) reported a self-limiting interfacial reaction between the Li₂OHCl solid electrolyte and the Li-metal anode to form an extremely stable interface. The Li/Li₂OHCl/Li battery circulated at 195°C showed that the stability between the solid electrolyte and the molten Li anode was achieved during the formation of the SEI, in which the interfacial resistance between the Li₂OHCl solid electrolyte and the Li metal was small.

In summary, the metallic lithium has strong reducibility, and it is necessary to study the interfacial compatibility of the lithium metal with the solid electrolyte, establish an interface modification method, and develop a metal lithium negative electrode with a highly stable three-dimensional structure.

Summary and Outlook

This review summarizes the concept and preparation technologies for solid-state Li-S batteries in recent years. The recent research progress on different kinds of solid-state electrolytes and their specific mechanical, charge transfer and chemical properties were discussed in detail, as well as the advantages and disadvantages of the solid-state electrolyte. The selection of the solid-state electrolyte and how to stabilize the solid/solid/solid three-phase interface both hold the key to the success of solid Li-sulfur batteries. As well, the technical challenges of solid-state lithium-sulfur batteries are also systematically described in the design and preparation of sulfur positive electrode and lithium negative electrode.

The stand out challenges facing the solid-state electrolyte materials includes the development of the fast lithium ion transport at room temperature, the establishment of a high-quality electrode/electrolyte architecture to improve the “solid/solid/solid” three-phase contact, the further stabilization of high-capacity electrodes. Prospective approaches to solving these problems can draw inspiration from the latest trends in polymer science, including the use of highly specific sequence control to obtain well-defined structures, the use of secondary structural modifications to extend control over material properties, and the materials with recyclable chemical design or bio-inspired molecular structures.

In short, all-solid lithium-sulfur batteries will play a pivotal role in the successful deployment of clean energy and achieve carbon neutral society, and the development prospects are worth looking forward to.

References

• 1

  AbrahamK. M.AlamgirM. (1991). Dimensionally stable MEEP-based polymer electrolytes and solid-state lithium batteries. Chem. Mater.3, 339–348. 10.1021/cm00014a027

  • CrossRef
  • Google Scholar
  • View reference in article

• 2

  AgostiniM.AiharaY.YamadaT.ScrosatiB.HassounJ. (2013). A lithium–sulfur battery using a solid, glass-type P2S5–Li2S electrolyte. Solid State Ionics244, 48–51. 10.1016/j.ssi.2013.04.024

  • CrossRef
  • Google Scholar
  • View reference in article

• 3

  AgostiniM.HassounJ. (2015). A lithium-ion sulfur battery using a polymer, polysulfide-added membrane. Sci. Rep.5:7591. 10.1038/srep07591

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 4

  AgostiniM.LimD. H.SaddM.FascianiC.NavarraM. A.PaneroS.et al. (2017). Stabilizing the performance of high-capacity sulfur composite electrodes by a new gel polymer electrolyte configuration. ChemSusChem10:1700977. 10.1002/cssc.201700977

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 5

  AgrawalR. C.PandeyG. P. (2008). Solid polymer electrolytes: materials designing and all-solid-state battery applications: an overview. J. Phys. D Appl. Phys.41:22. 10.1088/0022-3727/41/22/223001

  • CrossRef
  • Google Scholar
  • View reference in article

• 6

  ArbiK.RojoJ. M.SanzJ. (2007). Lithium mobility in titanium based Nasicon Li_1+xTi₂-xAl_x(PO₄)₃ and LiTi₂-x Zr_x(PO₄)₃ materials followed by NMR and impedance spectroscopy. J. Eur. Ceram. Soc.27, 4215–4218. 10.1016/j.jeurceramsoc.2007.02.118

  • CrossRef
  • Google Scholar
  • View reference in article

• 7

  ArumugamM. Y.Sheng-HengF.ChenxiC.Yu-ShengZ. (2014). Rechargeable lithium-sulfur batteries. Chem. Rev.114, 11751–11787. 10.1021/cr500062v

  • CrossRef
  • Google Scholar
  • View reference in article

• 8

  AsoK.HayashiA.TatsumisagoM. (2011). Synthesis of needlelike and platelike sns active materials in high-boiling solvents and their application to all-solid-state lithium secondary batteries. Crystal Growth Design11, 3900–3904. 10.1021/cg200459t

  • CrossRef
  • Google Scholar
  • View reference in article

• 9

  BalochM.VizintinA.ChellappanR. K.MoskonJ.ShanmukarajD.DedryvereR.et al. (2016). Application of gel polymer electrolytes based on ionic liquids in lithium-sulfur batteries. J. Electrochem. Soc.163, A2390–A2398. 10.1149/2.1151610jes

  • CrossRef
  • Google Scholar
  • View reference in article

• 10

  BarchaszC.LeprêtreJ. C.AlloinF.PatouxS. (2012). New insights into the limiting parameters of the Li/S rechargeable cell. J. Power Sources199, 322–330. 10.1016/j.jpowsour.2011.07.021

  • CrossRef
  • Google Scholar

• 11

  Ben YoucefH.Garcia-CalvoO.LagoN.DevarajS.ArmandM. (2016). Cross-linked solid polymer electrolyte for all-solid-state rechargeable lithium batteries. Electrochim. Acta220, 587–594. 10.1016/j.electacta.2016.10.122

  • CrossRef
  • Google Scholar
  • View reference in article

• 12

  BlangaR.GoorM.BursteinL.GladkichA.LogvinukD.ShechtmanI.et al. (2016). The search for a solid electrolyte, as a polysulfide barrier, for lithium/sulfur batteries. J. Solid State Electrochem.20, 3393–3404. 10.1007/s10008-016-3303-7

  • CrossRef
  • Google Scholar
  • View reference in article

• 13

  BohnkeO. (2008). The fast lithium-ion conducting oxides Li_3xLa_2/3-_xTiO₃ from fundamentals to application. Solid State Ionics179, 9–15. 10.1016/j.ssi.2007.12.022

  • CrossRef
  • Google Scholar
  • View reference in article

• 14

  BronsteinL. M.KarlinseyR. L.RitterK.JooC. G.SteinB.ZwanzigerJ. W. (2004). Design of organic-inorganic solid polymer electrolytes: synthesis, structure, and properties. J. Mater. Chem.14, 1812–1820. 10.1039/B401826E

  • CrossRef
  • Google Scholar
  • View reference in article

• 15

  BruceP. G.FreunbergerS. A.HardwickL. J.TarasconJ. M. (2011). Li–O₂ and Li–S batteries with high energy storage. Nat. Mater.11, 19–29. 10.1038/nmat3191

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 16

  BucurC. B.MuldoonJ.LitaA. (2016). A layer-by-layer supramolecular structure for a sulfur cathode. Energy and Environ. Sci.9, 992–998. 10.1039/C5EE02367J

  • CrossRef
  • Google Scholar
  • View reference in article

• 17

  CaoR.XuW.LvD.XiaoJ.ZhangJ. G. (2015). Anodes for rechargeable lithium-sulfur batteries. Adv. Energy Mater. 5:1402273. 10.1002/aenm.201402273

  • CrossRef
  • Google Scholar
  • View reference in article

• 18

  CapuanoF. (1991). Composite polymer electrolytes. J. Electrochem. Soc.138:1918. 10.1149/1.2085900

  • CrossRef
  • Google Scholar
  • View reference in article

• 19

  ChenM.YinX.ReddyM. V.AdamsS. (2015). All-solid-state MoS₂/Li₆PS5Br/In-Li batteries as a novel type of Li/S battery. J. Mater. Chem. A3, 10698–10702. 10.1039/C5TA02372F

  • CrossRef
  • Google Scholar
  • View reference in article

• 20

  ChenR.QuW.GuoX.LiL.WuF. (2016). The pursuit of solid-state electrolytes for lithium batteries: from comprehensive insight to emerging horizons. Materials Horizons3, 487–516. 10.1039/C6MH00218H

  • CrossRef
  • Google Scholar

• 21

  ChenR.ZhaoT.WuF. (2015). From a historic review to horizons beyond: lithium-sulphur batteries run on the wheels. Chem. Commun.51, 18–33. 10.1039/c4cc05109b

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 22

  ChenW.LeiT.WuC.DengM.GongC.HuK.et al. (2018). Designing safe electrolyte systems for a high-stability lithium–sulfur battery. Adv. Energy Mater. 8:1702348. 10.1002/aenm.201702348

  • CrossRef
  • Google Scholar

• 23

  ChengX. B.ZhangR.ZhaoC. Z.WeiF.ZhangJ. G.ZhangQ. (2016). A review of solid electrolyte interphases on lithium metal anode. Adv. Sci.3:1500213. 10.1002/advs.201500213

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 24

  ChengX. B.ZhangR.ZhaoC. Z.ZhangQ. (2017). Toward safe lithium metal anode in rechargeable batteries: a review. Chem. Rev.15, 10403–10473. 10.1021/acs.chemrev.7b00115

  • CrossRef
  • Google Scholar

• 25

  ChengY.ZhangL.XuS.ZhangH.RenB.LiT.et al. (2018). Ionic liquid functionalized electrospun gel polymer electrolyte for use in a high-performance lithium metal battery. J. Mater. Chem. A6, 18479–18487. 10.1039/C8TA06338A

  • CrossRef
  • Google Scholar

• 26

  ChoeH. S.GiaccaiJ.AlamgirM.AbrahamK. M. (1995). Preparation and characterization of poly(vinyl sulfone)- and poly(vinylidene fluoride)-based electrolytes. Electrochim. Acta40, 2289–2293. 10.1016/0013-4686(95)00180-M

  • CrossRef
  • Google Scholar
  • View reference in article

• 27

  ChoiJ. H.LeeC. H.YuJ. H.DohC. H.LeeS. M. (2015). Enhancement of ionic conductivity of composite membranes for all-solid-state lithium rechargeable batteries incorporating tetragonal Li₇La₃Zr₂O₁₂ into a polyethylene oxide matrix. J. Power Sources274, 458–463. 10.1016/j.jpowsour.2014.10.078

  • CrossRef
  • Google Scholar

• 28

  ChoiS.SongJ.WangC.ParkS.WangG. (2017). Multifunctional free-standing gel polymer electrolyte with carbon nanofiber interlayers for high-performance lithium-sulfur batteries. Chem. Asian J.12, 1470–1474. 10.1002/asia.201700402

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 29

  ChoudhuryS.SahaT.NaskarK.StammM.HeinrichG.DasA. (2017). A highly stretchable gel-polymer electrolyte for lithium-sulfur batteries. Polymer112, 447–456. 10.1016/j.polymer.2017.02.021

  • CrossRef
  • Google Scholar
  • View reference in article

• 30

  CroceF.AppetecchiG. B.PersiL.ScrosatiB. (1998). Nanocomposite polymer electrolytes for lithium batteries. Nature394, 456–458. 10.1038/28818

  • CrossRef
  • Google Scholar
  • View reference in article

• 31

  FuK. K.GongY.DaiJ.GongA.HanX.YaoY.et al. (2016). Flexible, solid-state, ion-conducting membrane with 3D garnet nanofiber networks for lithium batteries. Proc. Natl. Acad. Sci. U.S.A.113, 7094–7099. 10.1073/pnas.1600422113

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 32

  FuK. K.GongY.HitzG. T.McOwenD. W.LiY.XuS.et al. (2017a). Three-dimensional bilayer garnet solid electrolyte based high energy density lithium metal–sulfur batteries. Energy Environ. Sci.10, 1568–1575. 10.1039/C7EE01004D

  • CrossRef
  • Google Scholar
  • View reference in article

• 33

  FuK. K.GongY.LiuB.ZhuY.XuS.YaoY.et al. (2017b). Toward garnet electrolyte-based Li metal batteries: an ultrathin, highly effective, artificial solid-state electrolyte/metallic Li interface. Sci. Adv.3:4. 10.1126/sciadv.1601659

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 34

  GaoS.WangK.WangR.JiangM.HanJ.GuT.et al. (2017). Poly(vinylidene fluoride)-based hybrid gel polymer electrolytes for additive-free lithium sulfur batteries. J. Mater. Chem. A5, 17889–17895. 10.1039/C7TA05145J

  • CrossRef
  • Google Scholar
  • View reference in article

• 35

  GoodenoughJ. B.KimY. (2010). Challenges for rechargeable li batteries^†. Chem. Mater.22, 587–603. 10.1021/cm901452z

  • CrossRef
  • Google Scholar
  • View reference in article

• 36

  HanF.YueJ.FanX.GaoT.LuoC.MaZ.et al. (2016). High-performance all-solid-state lithium-sulfur battery enabled by a mixed-conductive Li2S nanocomposite. Nano Lett.16, 4521–4527. 10.1021/acs.nanolett.6b01754

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 37

  HanX.GongY.FuK. K.HeX.HitzG. T.DaiJ.et al. (2017). Negating interfacial impedance in garnet-based solid-state Li metal batteries. Nat. Mater.16, 572–579. 10.1038/nmat4821

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 38

  HancockK.BechererJ.HagenM.JoosM.AbertM.MuellerD.et al. (2018). Electrolyte decomposition and electrode thickness changes in Li-S cells with lithium metal anodes, prelithiated silicon anodes and hard carbon anodes. J. Electrochem. Soc.165, A6091–A6106. 10.1149/2.0161801jes

  • CrossRef
  • Google Scholar
  • View reference in article

• 39

  HaoC.MinL.LukeH.HanY. L.GaoranL.ZhanL.et al. (2018). Exploring chemical, mechanical, and electrical functionalities of binders for advanced energy-storage devices. Chem. Rev.118, 8936–8982. 10.1021/acs.chemrev.8b00241

  • CrossRef
  • Google Scholar
  • View reference in article

• 40

  HassounJ.ScrosatiB. (2010). Moving to a solid-state configuration: a valid approach to making lithium-sulfur batteries viable for practical applications. Adv. Mater. Weinheim.22, 5198–5201. 10.1002/adma.201002584

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 41

  HayashiA.OhtomoT.MizunoF.TadanagaK.TatsumisagoM. (2003). All-solid-state Li/S batteries with highly conductive glass–ceramic electrolytes. Electrochem. Commun.5, 701–705. 10.1016/S1388-2481(03)00167-X

  • CrossRef
  • Google Scholar
  • View reference in article

• 42

  HayashiA.OhtsuboR.OhtomoT.MizunoF.TatsumisagoM. (2008). All-solid-state rechargeable lithium batteries with Li2S as a positive electrode material. J. Power Sources183, 422–426. 10.1016/j.jpowsour.2008.05.031

  • CrossRef
  • Google Scholar
  • View reference in article

• 43

  Ho ParkJ.YeoS. Y.ParkJ. K.LeeY. M. (2010). Electrochemical performance of lithium sulfur batteries with plasticized polymer electrolytes based on P(VdF-co-HFP). J. Korean Electrochem. So13, 110–115. 10.5229/JKES.2010.13.2.110

  • CrossRef
  • Google Scholar
  • View reference in article

• 44

  HoodZ. D.WangH.Samuthira PandianA.KeumJ. K.LiangC. (2016). Li₂OHCl crystalline electrolyte for stable metallic lithium anodes. J. Am. Chem. Soc.138, 1768–1771. 10.1021/jacs.5b11851

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 45

  HovingtonP.LagacéM.GuerfiA.BouchardP.MaugerA.JulienC. M.et al. (2015). New lithium metal polymer solid state battery for an ultrahigh energy: nano C-LiFePO4 versus nano Li1.2V3O8. Nano Lett.15, 2671–2678. 10.1021/acs.nanolett.5b00326

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 46

  JeddiK.SarikhaniK.QazviniN. T.ChenP. (2014). Stabilizing lithium/sulfur batteries by a composite polymer electrolyte containing mesoporous silica particles. J. Power Sources245, 656–662. 10.1016/j.jpowsour.2013.06.147

  • CrossRef
  • Google Scholar
  • View reference in article

• 47

  JeongS. S.LimY. T.ChoiY. J.ChoG. B.KimK. W.AhnH. J.et al. (2007). Electrochemical properties of lithium sulfur cells using PEO polymer electrolytes prepared under three different mixing conditions. J. Power Sources174, 745–750. 10.1016/j.jpowsour.2007.06.108

  • CrossRef
  • Google Scholar
  • View reference in article

• 48

  JeongS. S.LimY. T.JungB. S.KimK. W. (2005). “Electrochemical characteristics of Li/S secondary battery with (PEO)(6)LiBF₄-Al₂O₃ composite polymer electrolyte prepared by ball milling,” in Eco-Materials Processing & Design Vi, Vol. 486–487, eds KimH. S.ParkS. Y.HurB. Y.594–597. 10.4028/0-87849-966-0.594

  • CrossRef
  • Google Scholar
  • View reference in article

• 49

  JiaqiangE.JinY.DengY.ZhaoX.HanD.PengQ.et al. (2017). Wetting models and working mechanisms of typical surfaces existing in nature and their application on superhydrophobic surfaces: a review. Adv. Mater. Interfaces2017:1701052. 10.1002/admi.201701052

  • CrossRef
  • Google Scholar
  • View reference in article

• 50

  JinJ.WenZ.LiangX.CuiY.WuX. (2012). Gel polymer electrolyte with ionic liquid for high performance lithium sulfur battery. Solid State Ionics Diffus. React.225, 604–607. 10.1016/j.ssi.2012.03.012

  • CrossRef
  • Google Scholar
  • View reference in article

• 51

  JingG.WenfengR.JianC. (2017). Research progress of all-solid lithium-sulfur battery. Energy Storage Sci.Technol. 2, 199–230. 10.1007/s41918-019-00029-3

  • CrossRef
  • Google Scholar
  • View reference in article

• 52

  JozwiukA.BerkesB. B.WeissT.SommerH.JanekJ.BrezesinskiT. (2016). The critical role of lithium nitrate in the gas evolution of lithium-sulfur batteries. Energy Environ. Sci.9, 2603–2608. 10.1039/C6EE00789A

  • CrossRef
  • Google Scholar
  • View reference in article

• 53

  JudezX.ZhangH.LiC.EshetuG. G.ZhangY.González-MarcosJ. A.et al. (2017). Polymer-rich composite electrolytes for all-solid-state Li-S cells. J. Phys. Chem. Lett.8, 3473–3477. 10.1021/acs.jpclett.7b01321

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 54

  KamyshnyA.GunJ.RizkovD.VoitsekovskiT.LevO. (2007). Equilibrium distribution of polysulfide ions in aqueous solutions at different temperatures by rapid single phase derivatization. Environ. Sci. Technol.41, 2395–2400. 10.1021/es062637+

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 55

  KatoY.HoriS.SaitoT.SuzukiK.HirayamaM.MitsuiA.et al. (2016). High-power all-solid-state batteries using sulfide superionic conductors. Nat. Energy1:16030. 10.1038/nenergy.2016.30

  • CrossRef
  • Google Scholar
  • View reference in article

• 56

  KimB. C.TakadaK.OhtaN.SeinoY.ZhangL.WadaH.et al. (2005). All solid state Li-ion secondary battery with FeS anode. Solid State Ionics, Diffusion and Reactions, 176, 2383–2387. 10.1016/j.ssi.2005.05.019

  • CrossRef
  • Google Scholar
  • View reference in article

• 57

  KimJ.-K. (2017). Hybrid gel polymer electrolyte for high-safety lithium-sulfur batteries. Mater. Lett.187, 40–43. 10.1016/j.matlet.2016.10.069

  • CrossRef
  • Google Scholar

• 58

  KimK. M.PoliquitB. Z.LeeY.-G.WonJ.KoJ. M.ChoW. I. (2014). Enhanced separator properties by thermal curing of poly(ethylene glycol)diacrylate-based gel polymer electrolytes for lithium-ion batteries. Electrochim. Acta120, 159–166. 10.1016/j.electacta.2013.12.077

  • CrossRef
  • Google Scholar
  • View reference in article

• 59

  KinoshitaS.OkudaK.MachidaN.NaitoM.SigematsuT. (2014). All-solid-state lithium battery with sulfur/carbon composites as positive electrode materials. Solid State Ionics256, 97–102. 10.1016/j.ssi.2013.12.045

  • CrossRef
  • Google Scholar
  • View reference in article

• 60

  KobayashiT.ImadeY.ShishiharaD.HommaK.NagaoM.WatanabeR.et al. (2008). All solid-state battery with sulfur electrode and thio-LISICON electrolyte. J. Power Sources182, 621–625. 10.1016/j.jpowsour.2008.03.030

  • CrossRef
  • Google Scholar
  • View reference in article

• 61

  KokalI.RamanujacharyK. V.NottenP. H. L.HintzenH. T. (2012). Sol–gel synthesis and lithium ion conduction properties of garnet-type Li₆BaLa₂Ta₂O₁₂. Mater. Res. Bull.47, 1932–1935. 10.1016/j.materresbull.2012.04.032

  • CrossRef
  • Google Scholar
  • View reference in article

• 62

  LaiC. H.LuM. Y.ChenL. J. (2011). Metal sulfide nanostructures: synthesis, properties and applications in energy conversion and storage. J. Mater. Chem.22, 19–10. 10.1039/C1JM13879K

  • CrossRef
  • Google Scholar
  • View reference in article

• 63

  LeeC. H.JooK. H.KimJ. H.WooS. G.SohnH. J.KangT.et al. (2002). Characterizations of a new lithium ion conducting Li₂O-SeO₂-B₂O₃ glass electrolyte. Solid State Ionics149, 59–65. 10.1016/S0167-2738(02)00137-6

  • CrossRef
  • Google Scholar
  • View reference in article

• 64

  LeeF.TsaiM.-C.LinM.-H.Ni'mahY. L.HyS.KuoC.-Y.et al. (2017). Capacity retention of lithium sulfur batteries enhanced with nano-sized TiO2-embedded polyethylene oxide. J. Mater. Chem. A5, 6708–6715. 10.1039/C6TA10755A

  • CrossRef
  • Google Scholar
  • View reference in article

• 65

  LiL.PascalT. A.ConnellJ. G.FanF. Y.MecklerS. M.MaL.et al. (2017). Molecular understanding of polyelectrolyte binders that actively regulate ion transport in sulfur cathodes. Nat. Commun.8:2277. 10.1038/s41467-017-02410-6

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 66

  LiW.ZhangQ.ZhengG.SehZ. W.YaoH.CuiY. (2013). Understanding the role of different conductive polymers in improving the nanostructured sulfur cathode performance. Nano Lett.13, 5534–5540. 10.1021/nl403130h

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 67

  LiY.HanJ. T.WangC. A.XieH.GoodenoughJ. B. (2012). Optimizing Li+ conductivity in a garnet framework. J. Mater. Chem.22, 15357–15361. 10.1039/c2jm31413d

  • CrossRef
  • Google Scholar
  • View reference in article

• 68

  LiY.XuB.XuH.DuanH.LüX.XinS.et al. (2017). Hybrid polymer/garnet electrolyte with a small interfacial resistance for lithium-ion batteries. Angewandte Chem. Int. Edn. 56, 753–756. 10.1002/anie.201608924

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 69

  LiZ.WuH. B.LouX. W. (2016). Rational designs and engineering of hollow micro-/nanostructures as sulfur hosts for advanced lithium–sulfur batteries. Energy Environ. Sci.9, 3061–3070. 10.1039/C6EE02364A

  • CrossRef
  • Google Scholar
  • View reference in article

• 70

  LiangC. C. (1973). Conduction characteristics of the lithium iodide-aluminum oxide solid electrolytes. J. Electrochem. Soc.120:1289. 10.1149/1.2403248

  • CrossRef
  • Google Scholar
  • View reference in article

• 71

  LiangX.WenZ.LiuY.WuM.JinJ.ZhangH.et al. (2011a). Improved cycling performances of lithium sulfur batteries with LiNO3-modified electrolyte. J. Power Sources196, 9839–9843. 10.1016/j.jpowsour.2011.08.027

  • CrossRef
  • Google Scholar
  • View reference in article

• 72

  LiangX.WenZ.LiuY.ZhangH.HuangL.JinJ. (2011b). Highly dispersed sulfur in ordered mesoporous carbon sphere as a composite cathode for rechargeable polymer Li/S battery. J. Power Sources196, 3655–3658. 10.1016/j.jpowsour.2010.12.052

  • CrossRef
  • Google Scholar

• 73

  LinY.WangX.LiuJ.MillerJ. D. (2017). Natural halloysite nano-clay electrolyte for advanced all-solid-state lithium-sulfur batteries. Nano Energy31, 478–485. 10.1016/j.nanoen.2016.11.045

  • CrossRef
  • Google Scholar

• 74

  LinZ.LiuZ.DudneyN. J.LiangC. (2013a). Lithium superionic sulfide cathode for all-solid lithium-sulfur batteries. Acs Nano7, 2829–2833. 10.1021/nn400391h

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 75

  LinZ.LiuZ.FuW.DudneyN. J.LiangC. (2013b). Lithium polysulfidophosphates: a family of lithium-conducting sulfur-rich compounds for lithium-sulfur batteries and angewandte chemie-international edition. Angew Chem Int Ed Engl.52, 7460–7463. 10.1002/anie.201300680

  • CrossRef
  • Google Scholar
  • View reference in article

• 76

  LiuM.ZhouD.HeY.-B.FuY.QinX.MiaoC.et al. (2016). Novel gel polymer electrolyte for high-performance lithium-sulfur batteries. Nano Energy22, 278–289. 10.1016/j.nanoen.2016.02.008

  • CrossRef
  • Google Scholar
  • View reference in article

• 77

  LongP.XuQ.PengG.YaoX.XuX. (2016). NiS nanorods as cathode materials for all-solid-state lithium batteries with excellent rate capability and cycling stability. Chemelectrochem3, 764–769. 10.1002/celc.201500570

  • CrossRef
  • Google Scholar
  • View reference in article

• 78

  LuoW.GongY.ZhuY.LiY.YaoY.ZhangY.et al. (2017). Reducing interfacial resistance between garnet-structured solid-state electrolyte and Li-metal anode by a germanium layer. Adv. Mater.29:22. 10.1002/adma.201606042

  • Pubmed Abstract
  • CrossRef
  • Google Scholar
  • View reference in article

• 79

  MaL.ZhuangH.LuY.MogantyS. S.HennigR. G.ArcherL. A. (2014). Tethered molecular sorbents: enabling metal-sulfur battery cathodes. Adv. Energy Mater. 4:1400390. 10.1002/aenm.201400390

  • CrossRef
  • Google Scholar
  • View reference in article

• 80

  MachidaN.KobayashiK.NishikawaY.ShigematsuT. (2004). Electrochemical properties of sulfur as cathode materials in a solid-state lithium battery with inorganic solid electrolytes. Solid State Ionics Diffus. React.175, 247–250. 10.1016/j.ssi.2003.11.033

  • CrossRef
  • Google Scholar
  • View reference in article

• 81

  MachidaN.ShigematsuT. (2004). An all-solid-state lithium battery with sulfur as positive electrode materials. Chem. Lett.33, 376–377. 10.1246/cl.2004.376

  • CrossRef
  • Google Scholar
  • View reference in article

• 82

  MaierJ. (1995). Ionic conduction in space charge regions. Progress Solid State Chem.23, 171–263. 10.1016/0079-6786(95)00004-E

  • CrossRef
  • Google Scholar
  • View reference in article

• 83

  ManthiramA.YuX.WangS. (2017). Lithium battery chemistries enabled by solid-state electrolytes. Nature Reviews Materials, 2, 16103. 10.1038/natrevmats.2016.103

  • CrossRef
  • Google Scholar
  • View reference in article

• 84

  MatsuyamaT.SakudaA.HayashiA.TogawaY.MoriS.TatsumisagoM. (2013). Electrochemical properties of all-solid-state lithium batteries with amorphous titanium sulfide electrodes prepared by mechanical milling. J. Solid State Electrochem.17, 2697–2701. 10.1007/s10008-013-2157-5

  • CrossRef
  • Google Scholar

• 85

  MikhaylikY. V.AkridgeJ. R. (2004). Polysulfide shuttle study in the Li/S battery system. J. Electrochem. Soc.151, A1969–A1976. 10.1149/1.1806394

  • CrossRef
  • Google Scholar
  • View reference in article

• 86

  NagaoM.HayashiA.TatsumisagoM. (2012). Fabrication of favorable interface between sulfide solid electrolyte and Li metal electrode for bulk-type solid-state Li/S battery. Electrochem. Commun.22, 177–180. 10.1016/j.elecom.2012.06.015

  • CrossRef
  • Google Scholar

• 87

  NagaoM.ImadeY.NarisawaH.KobayashiT.WatanabeR.YokoiT.et al. (2013a). All-solid-state Li-sulfur batteries with mesoporous electrode and thio-LISICON solid electrolyte. J. Power Sources222, 237–242. 10.1016/j.jpowsour.2012.08.041

  • CrossRef
  • Google Scholar

• 88

  NagaoM.ImadeY.NarisawaH.WatanabeR.YokoiT.TatsumiT.et al. (2013b). Reaction mechanism of all-solid-state lithium-sulfur battery with two-dimensional mesoporous carbon electrodes. J. Power Sources243, 60–64. 10.1016/j.jpowsour.2013.05.037

  • CrossRef
  • Google Scholar

• 89

  NagaoM.SuzukiK.ImadeY.TateishiM.WatanabeR.YokoiT.et al. (2016). All-solid-state lithium-sulfur batteries with three-dimensional mesoporous electrode structures. J. Power Sources330, 120–126. 10.1016/j.jpowsour.2016.09.009

  • CrossRef
  • Google Scholar

• 90

  NagataH.ChikusaY. (2014a). A lithium sulfur battery with high power density. J. Power Sources264, 206–210. 10.1016/j.jpowsour.2014.04.106

  • CrossRef
  • Google Scholar

• 91

  NagataH.ChikusaY. (2014b). Transformation of P2S5 into a solid electrolyte with ionic conductivity at the positive composite electrode of all-solid-state lithium-sulfur batteries. Energy Techn.2, 753–756. 10.1002/ente.201402040

  • CrossRef
  • Google Scholar

• 92

  NagataH.ChikusaY. (2014c). Activation of sulfur active material in an all-solid-state lithium-sulfur battery. J. Power Sources263, 141–144. 10.1016/j.jpowsour.2014.04.032

  • CrossRef
  • Google Scholar

• 93

  NagataH.ChikusaY. (2016). An all-solid-state lithium-sulfur battery using two solid electrolytes having different functions. J. Power Sources329, 268–272. 10.1016/j.jpowsour.2016.08.058

  • CrossRef
  • Google Scholar

• 94

  NairJ. R.BellaF.AngulakshmiN.StephanA. M.GerbaldiC. (2016). Nanocellulose-laden composite polymer electrolytes for high performing lithium–sulphur batteries. Energy Storage Mater.3:S2405829715300945. 10.1016/j.ensm.2016.01.008

  • CrossRef
  • Google Scholar

• 95

  PangQ.LiangX.KwokC. Y.NazarL. F. (2016). Advances in lithium–sulfur batteries based on multifunctional cathodes and electrolytes. Nat. Energy1:16132. 10.1038/nenergy.2016.132

  • CrossRef
  • Google Scholar

• 96

  ParkK.ChoJ. H.JangJ.-H.YuB.-C.De La HozA. T.MillerK. M.et al. (2015). Trapping lithium polysulfides of a Li–S battery by forming lithium bonds in a polymer matrix. Energy Environ. Sci.8, 2389–2395. 10.1039/C5EE01809A

  • CrossRef
  • Google Scholar

• 97

  PengH. P.HuangJ. Q.ChengX. B.ZhangQ. (2017). Review on high-loading and high-energy lithium-sulfur batteries. Adv. Energy Mater. 7:1700260. 10.1002/aenm.201700260

  • CrossRef
  • Google Scholar

• 98

  RaoM.GengX.LiX.HuS.LiW. (2012). Lithium-sulfur cell with combining carbon nanofibers–sulfur cathode and gel polymer electrolyte. J. Power Sources212, 179–185. 10.1016/j.jpowsour.2012.03.111

  • CrossRef
  • Google Scholar

• 99

  RaoR.liX.LiaoY.LiX. (2015). Preparation and performance of a composite polyimide/poly(vinylidene fluoride-co-hexafluoropropylene)/nano-Al2O3polymer electrolyte for lithium-sulfur cell. Ionics21, 1937–1943. 10.1007/s11581-014-1360-4

  • CrossRef
  • Google Scholar

• 100

  RosenmanA.MarkevichE.SalitraG.AurbachD.GarsuchA.ChesneauF. F. (2015). Review on li-sulfur battery systems: an integral perspective. Adv. Energy Mater. 5:1500212. 10.1002/aenm.201500212

  • CrossRef
  • Google Scholar

• 101

  RyooH. J.KimH. T.LeeY. G.ParkJ. K.MoonS. I. (1998). Thermal and electrochemical characteristics of plasticized polymer electrolytes based on poly(acrylonitrile-co-methyl methacrylate). J. Solid State Electrochem. 3, 1–6. 10.1007/s100080050123

  • CrossRef
  • Google Scholar

• 102

  SakudaA.HayashiA.TatsumisagoM. (2010). Interfacial observation between LiCoO2 electrode and Li2S–P2S5 solid electrolytes of all-solid-state lithium secondary batteries using transmission electron microscopy. Chem. Mater.22, 949–956. 10.1021/cm901819c

  • CrossRef
  • Google Scholar

• 103

  SchneiderH.Thomas Weiß, Scordilis-Kelley, C.MaeyerJ.LeitnerK.PengH. J.et al. (2017). Electrolyte decomposition and gas evolution in a lithium-sulfur cell upon long-term cycling. Electrochim. Acta243, 26–32. 10.1016/j.electacta.2017.05.034

  • CrossRef
  • Google Scholar

• 104

  ScrosatiB.CroceF.PaneroS. (2001). Progress in lithium polymer battery R&D. J. Power Sources100, 93–100. 10.1016/S0378-7753(01)00886-2

  • CrossRef
  • Google Scholar

• 105

  SehZ. W.ZhangQ.LiW.ZhengG.YaoH.CuiY. (2013). Stable cycling of lithium sulfide cathodes through strong affinity with a bifunctional binder. Chem. Sci.4:3673. 10.1039/c3sc51476e

  • CrossRef
  • Google Scholar

• 106

  ShengO.JinC.LuoJ.YuanH.FangC.HuangH.et al. (2017). Ionic conductivity promotion of polymer electrolyte with ionic liquid grafted oxides for all-solid-state lithium-sulfur batteries. J. Mater. Chem. A5, 12934–12942. 10.1039/C7TA03699J

  • CrossRef
  • Google Scholar

• 107

  ShinJ. H.CairnsE. J. (2008). N-Methyl-(n-butyl)pyrrolidinium bis(trifluoromethanesulfonyl)imide-LiTFSI-poly(ethylene glycol) dimethyl ether mixture as a Li/S cell electrolyte. J. Power Sources177, 537–545. 10.1016/j.jpowsour.2007.11.043

  • CrossRef
  • Google Scholar

• 108

  ShinJ. H.JungS. S.KimK. W.AhnH. J.AhnJ. H. (2002a). Preparation and characterization of plasticized polymer electrolytes based on the PVdF-HFP copolymer for lithium/sulfur battery. J. Mater. Sci. Mater. Electron.13, 727–733. 10.1023/A:1021521207247

  • CrossRef
  • Google Scholar

• 109

  ShinJ. H.KimK. W.AhnH. J.AhnJ. H. (2002b). Electrochemical properties and interfacial stability of (PEO)(10)LiCF3SO3-TinO2n-1 composite polymer electrolytes for lithium/sulfur battery. Mater. Sci. Eng. B Solid State Mater. Adv. Techn.95, 148–156. 10.1016/S0921-5107(02)00226-X

  • CrossRef
  • Google Scholar

• 110

  SongM. K.ZhangY.CairnsE. J. (2013). A long-life, high-rate lithium/sulfur cell: a multifaceted approach to enhancing cell performance. Nano Lett.13, 5891–5899. 10.1021/nl402793z

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 111

  TaoX.LiuY.LiuW.ZhouG.ZhaoJ.LinD.et al. (2017). Solid-state lithium-sulfur batteries operated at 37°c with composites of nanostructured Li7La3Zr2O12/Carbon foam and polymer. Nano Lett.17, 2967–2972. 10.1021/acs.nanolett.7b00221

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 112

  TatsumisagoM. (2004). Glassy materials based on Li2S for all-solid-state lithium secondary batteries. Solid State Ionics175, 13–18. 10.1016/j.ssi.2004.09.012

  • CrossRef
  • Google Scholar

• 113

  TomonariT.HiroyukK.NakanishibK.TabuchiM.SakaebeH.OhtaT.et al. (2010). All-Solid-State Lithium Secondary Battery with Li2S – C composite positive electrode prepared by spark-plasma-sintering process. J. Electrochem. Soc.157, A1196–A1201. 10.1149/1.3486083

  • CrossRef
  • Google Scholar

• 114

  VermaM. L.MinakshiM.SinghN. K. (2014a). Structural and electrochemical properties of nanocomposite polymer electrolyte for electrochemical devices. Indust. Eng. Chem. Res.53, 14993–15001. 10.1021/ie502615w

  • CrossRef
  • Google Scholar

• 115

  VermaM. L.MinakshiM.SinghN. K. (2014b). Synthesis and characterization of solid polymer electrolyte based on activated carbon for solid state capacitor. Electrochim. Acta137, 497–503. 10.1016/j.electacta.2014.06.039

  • CrossRef
  • Google Scholar

• 116

  WangC.GongY.LiuB.FuK.YaoY.HitzE.et al. (2017). Conformal, nanoscale ZnOSurface modification of garnet-based solid-state electrolyte for lithium metal anodes. Nano Lett.17, 565–571. 10.1021/acs.nanolett.6b04695

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 117

  WangQ.GuoJ.WuT.JinJ.YangJ.WenZ.et al. (2017). Improved performance of Li-S battery with hybrid electrolyte by interface modification. Solid State Ionics300, 67–72. 10.1016/j.ssi.2016.11.001

  • CrossRef
  • Google Scholar

• 118

  WangQ.JinJ.WuX.MaG.YangJ.WenZ. (2014). A shuttle effect free lithium sulfur battery based on a hybrid electrolyte. Phys. Chem. Chem. Phys.16, 21225–21229. 10.1039/C4CP03694H

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 119

  WangQ.WenZ.JinJ.GuoJ.HuangX.YangJ.et al. (2016). A gel-ceramic multi-layer electrolyte for long-life lithium sulfur batteries. Chem. Commun.52, 1637–1640. 10.1039/C5CC08279J

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 120

  WangS.DingY.ZhouG.YuG.ManthiramA. (2016). Durability of the Li_1+xTi_2−xAl_x(PO₄)₃ solid electrolyte in lithium sulfur batteries. Acs Energy Lett.1, 1080–1085. 10.1021/acsenergylett.6b00481

  • CrossRef
  • Google Scholar

• 121

  WangX.HouY.ZhuY.WuY.HolzeR. (2013). An aqueous rechargeable lithium battery using coated li metal as anode. Sci. Rep.3:1401. 10.1038/srep01401

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 122

  WangZ.HuangB.HuangH.ChenL.XueR.WangF. (1996). Investigation of the position of Li+ ions in a polyacrylonitrile-based electrolyte by Raman and infrared spectroscopy. Electrochim. Acta41, 1443–1446. 10.1016/0013-4686(95)00392-4

  • CrossRef
  • Google Scholar

• 123

  WenC. J.HugginsR. A. (1980). Thermodynamic and mass transport properties of “LiIn”. Mater. Res. Bull.15, 1225–1234. 10.1016/0025-5408(80)90024-0

  • CrossRef
  • Google Scholar

• 124

  WuF.LeeJ. T.NittaN.KimH.BorodinO.YushinG. (2015). Lithium iodide as a promising electrolyte additive for lithium-sulfur batteries: mechanisms of performance enhancement. Adv. Mater.27, 101–108. 10.1002/adma.201404194

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 125

  WuF.QianJ.ChenR.LuJ.LiL.WuH.et al. (2014). An effective approach to protect lithium anode and improve cycle performance for Li–S batteries. ACS Appl. Mater. Interfaces6:140822155118003. 10.1021/am504345s

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 126

  WuY.WangY.FengJ.MaZ.ShaoG. (2016). High capacity and cycle stability Rechargeable Lithium–Sulfur batteries by sandwiched gel polymer electrolyte. Electrochim. Acta210, 71–78. 10.1016/j.electacta.2016.05.087

  • CrossRef
  • Google Scholar

• 127

  XiaY.WangX.XiaX.XuR.ZhangS.WuJ.et al. (2017). A newly designed composite gel polymer electrolyte based on poly(vinylidene fluoride-hexafluoropropylene) (PVDF-HFP) for enhanced solid-state lithium-sulfur batteries. Chemistry23:60. 10.1002/chem.201703464

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 128

  XuK. (2004). Nonaqueous liquid electrolytes for lithium-based rechargeable batteries. Chem. Rev.104, 4303–4417. 10.1021/cr030203g

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 129

  XuR.LuJ.AmineK. (2015). Progress in mechanistic understanding and characterization techniques of li-s batteries. Adv. Energy Mater. 5:1500408. 10.1002/aenm.201500408

  • CrossRef
  • Google Scholar

• 130

  XuR. C.XiaX. H.WangX. L.XiaaY.TuJ. P. (2017). Tailored Li2S–P2S5 glass-ceramic electrolyte by MoS2 doping, possessing high ionic conductivity for all-solid-state lithium-sulfur batteries. J. Mater. Chem. A. 5, 2829–2834. 10.1039/C6TA10142A

  • CrossRef
  • Google Scholar

• 131

  XuX. X.WenZ. Y. (2005). Glass and glass-ceramics solid electrolytes for lithium-ion battery. J. Inorganic Mater.20, 21–26.

  • Google Scholar

• 132

  YaoX.LiuD.WangC.LongP.PengG.HuY. S.et al. (2016). High-energy all-solid-state lithium batteries with ultralong cycle life. Nano Lett.16, 7148–7154. 10.1021/acs.nanolett.6b03448

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 133

  YeY.WuF.XuS.QuW.LiL.ChenR. (2018). Designing realizable and scalable techniques for practical lithium sulfur batteries: a perspective. J. Phys. Chem. Lett.9, 1398–1414. 10.1021/acs.jpclett.7b03165

  • Pubmed Abstract
  • CrossRef
  • Google Scholar

• 134

  YuX.BiZ.ZhaoF.ManthiramA. (2016). Polysulfide–Shuttle control in Lithium–Sulfur batteries with a chemically/electrochemically compatible NaSICON–Type solid electrolyte. Adv. Energy Mater. 6:24. 10.1002/aenm.201601392

  • CrossRef
  • Google Scholar

• 135

  YuX. G.XieJ. Y.YangJ.WangK. (2004). All solid-state rechargeable lithium cells based on nano-sulfur composite cathodes. J. Power Sources132, 181–186. 10.1016/j.jpowsour.2004.01.034

  • CrossRef
  • Google Scholar

• 136

  ZengS.-L.WangH.-X.DongC. (2014). Synthesis and electrical conductivity of nanocrystalline tetragonal FeS. Chinese Phys. B23:8. 10.1088/1674-1056/23/8/087203

  • CrossRef
  • Google Scholar

• 137

  ZhangC.LinY.LiuJ. (2015). Sulfur double locked by a macro-structural cathode and a solid polymer electrolyte for lithium–sulfur batteries. J. Mater. Chem. A3, 10760–10766. 10.1039/C5TA01037C

  • CrossRef
  • Google Scholar

• 138

  ZhangS.UenoK.DokkoK.WatanabeM. (2015). Recent advances in electrolytes for lithium-sulfur batteries. Adv. Energy Mater. 5:1500117. 10.1002/aenm.201500117

  • CrossRef
  • Google Scholar

• 139

  ZhangS. S. (2013). Liquid electrolyte lithium/sulfur battery: Fundamental chemistry, problems, and solutions. J. Power Sources231, 153–162. 10.1016/j.jpowsour.2012.12.102

  • CrossRef
  • Google Scholar

• 140

  ZhangS. S.TranD. T. (2013). How a gel polymer electrolyte affects performance of lithium/sulfur batteries. Electrochim. Acta114, 296–302. 10.1016/j.electacta.2013.10.069

  • CrossRef
  • Google Scholar

• 141

  ZhangX.WangW.WangA.HuangY.YuanK.YuZ.et al. (2014). Improved cycle stability and high security of Li-B alloy anode for lithium-sulfur battery. J. Mater. Chem. A2, 11660–11665. 10.1039/C4TA01709A

  • CrossRef
  • Google Scholar

• 142

  ZhangY.ChenK.ShenY.LinY.NanC.-W. (2017). Synergistic effect of processing and composition x on conductivity of xLi₂S-(100-x)P₂S₅ electrolytes. Solid State Ionics305, 1–6. 10.1016/j.ssi.2017.03.024

  • CrossRef
  • Google Scholar

• 143

  ZhangY.ZhaoY.BakenovZ.BabaaM.-R.KonarovA.DingC.et al. (2013). Effect of graphene on sulfur/polyacrylonitrile nanocomposite cathode in high performance lithium/sulfur batteries. J. Electrochem. Soc.160, A1194–A1198. 10.1149/2.068308jes

  • CrossRef
  • Google Scholar

• 144

  ZhangY.ZhaoY.BakenovZ.ChenP. (2014). Poly(vinylidene fluoride-co-hexafluoropropylene)/poly(methylmethacrylate)/nanoclay composite gel polymer electrolyte for lithium/sulfur batteries. J. Solid State Electrochem.18, 1111–1116. 10.1007/s10008-013-2366-y

  • CrossRef
  • Google Scholar

• 145

  ZhangY.ZhaoY.GosselinkD.ChenP. (2015). Synthesis of poly(ethylene-oxide)/nanoclay solid polymer electrolyte for all solid-state lithium/sulfur battery. Ionics21, 381–385. 10.1007/s11581-014-1176-2

  • CrossRef
  • Google Scholar

• 146

  ZhangZ.LaiY.ZhangZ.ZhangK.LiJ. (2014). Al2O3-coated porous separator for enhanced electrochemical performance of lithium sulfur batteries. Electrochim. Acta129, 55–61. 10.1016/j.electacta.2014.02.077

  • CrossRef
  • Google Scholar

• 147

  ZhaoY.WuC.PengG.ChenX.YaoX.BaiY.et al. (2016). A new solid polymer electrolyte incorporating Li10GeP2S12 into a polyethylene oxide matrix for all-solid-state lithium batteries. J. Power Sources301, 47–53. 10.1016/j.jpowsour.2015.09.111

  • CrossRef
  • Google Scholar

• 148

  ZhaoY.ZhangY.BakenovZ. (2013). Electrochemical performance of lithium gel polymer battery with nanostructured sulfur/carbon composite cathode. Solid State Ionics234, 40–45. 10.1016/j.ssi.2013.01.002

  • CrossRef
  • Google Scholar

• 149

  ZhouD.LiuR.HeY. B.LiF.LiB.YangQ. H.et al. (2016). SiO₂ hollow nanosphere-based composite solid electrolyte for lithium metal batteries to suppress lithium dendrite growth and enhance cycle life. Adv. Energy Mater. 6:7. 10.1002/aenm.201502214

  • CrossRef
  • Google Scholar

• 150

  ZhuK.LiuY.LiuJ. (2014). A fast charging/discharging all-solid-state lithium ion battery based on PEO-MIL-53(Al)-LiTFSI thin film electrolyte. RSC Adv.4, 42278–42284. 10.1039/C4RA06208F

  • CrossRef
  • Google Scholar

• 151

  ZhuS.MaF.WangY.YanW.SunD.JinY. (2017). New small molecule gel electrolyte with high ionic conductivity for Li-S batteries. J. Mater. Sci.52, 4086–4095. 10.1007/s10853-016-0671-4

  • CrossRef
  • Google Scholar

• 152

  ZhuX. J.WenZ. Y.GuZ. H.LinZ. X. (2005). Electrochemical characterization and performance improvement of lithium/sulfur polymer batteries. J. Power Sources139, 269–273. 10.1016/j.jpowsour.2004.07.002

  • CrossRef
  • Google Scholar