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Aug 28, 2023

A reflection on polymer electrolytes for solid

Nature Communications volume 14, Article number: 4884 (2023) Cite this article 5629 Accesses 1 Altmetric Metrics details Before the debut of lithium-ion batteries (LIBs) in the commodity market,

Nature Communications volume 14, Article number: 4884 (2023) Cite this article

5629 Accesses

1 Altmetric

Metrics details

Before the debut of lithium-ion batteries (LIBs) in the commodity market, solid-state lithium metal batteries (SSLMBs) were considered promising high-energy electrochemical energy storage systems before being almost abandoned in the late 1980s because of safety concerns. However, after three decades of development, LIB technologies are now approaching their energy content and safety limits imposed by the rocking chair chemistry. These aspects are prompting the revival of research activities in SSLMB technologies at both academic and industrial levels. In this perspective article, we present a personal reflection on solid polymer electrolytes (SPEs), spanning from early development to their implementation in SSLMBs, highlighting key milestones. In particular, we discuss the SPEs’ characteristics taking into account the concept of coupled and decoupled SPEs proposed by C. Austen Angell in the early 1990s. Possible remedies to improve the physicochemical and electrochemical properties of SPEs are also examined. With this article, we also aim to highlight the missing blocks in building ideal SSLMBs and stimulate research towards innovative electrolyte materials for future rechargeable high-energy batteries.

In his 1870 novel “Twenty Thousand Leagues Under The Sea” Jules Verne describes the submarine Nautilus as powered by an advanced battery system, and Captain Nemo mentions that “…the cells with sodium must be regarded as most energetic, and that their electromotive force is double that of the zinc cells.”1 The concept of building high-energy batteries proposed by Jules Verne was undoubtedly ahead of its time in the late 19th century but in line with the then fascination for the wonders generated by the use of electricity. “All with electricity” was a dream for humanity living in the early 1900s, but it would come into reality in the late 20th century with the invention of lithium-ion batteries (LIBs) based on the rocking chair concept (i.e., batteries built with two intercalation-based electrodes with different potentials for storing/delivering electrochemical energy)2,3. Presently, the global production of LIBs has reached a large scale of >500-gigawatt hour (GWh), acting as power sources for more than 6 million electric vehicles (EVs)4. The success of LIBs testifies to the early hypothesis of “all with electricity” and opens up new avenues for more sustainable development of energy-consuming anthropogenic activities.

The production capacity of LIBs has risen tenfold over the past decade5, and this demand is expected to continue growing rapidly over the next 10–30 years, driven mainly by the fast-growing EV sector4. The need for high-performance (e.g., energy density, safety, cost, etc.) rechargeable batteries is also pressing, particularly considering the stringent requirements brought by contemporary practical applications (e.g., EVs for road and flying, drones, advanced robotics, etc.), including inherent safety and specific energy (>500 Wh kg−1) and energy density (>1000 Wh L−1)6. Unfortunately, the nonaqueous liquid electrolytes used in today’s LIBs are unstable and highly flammable due to the presence of organic carbonate solvents (e.g., dimethyl carbonate, ethylene carbonate, etc.); additionally, the graphite negative electrodes with a relatively low specific capacity of 372 mAh g−1 are also limiting factors for improving further the specific energy of the state-of-the-art LIBs6. In this regard, solid-state lithium metal batteries (SSLMBs) coupling high-energy electrode materials (e.g., lithium metal (Li°), lithium alloys, nickel-rich LiNi1−x−yCoxMnyO2 (1−x − y > 0.8), sulfur, etc.) with solid electrolytes are considered a viable approach to circumvent the specific energy density stumbling block of current LIB technology7,8,9.

Among all kinds of lithium-ion conductive solid-state electrolytes, solid polymer electrolytes (SPEs) have attracted significant attention owing to their physicochemical features (e.g., high flexibility, ease of thin-film processing)10,11,12. In particular, practical high-energy applications (>1 GWh) of SPE-based SSLMBs as power sources for EV and grid storage have been deployed by the Bolloré group since 201013. This is a relevant industrial example of SPE technology capable of providing support for the development of high-performance SSLMBs.

Since the historical development of solid solution electrodes in LIB technologies is well reported in recent perspective and review articles4,14,15,16,17, here, we focus our attention on the evolution of SPE materials and their physical chemistries, with particular reference to their applications in rechargeable secondary batteries, aiming to bridge the gaps between the earlier-developed solid-state batteries and contemporary high-performance SPE-based SSLMBs. In particular, the timeline rationale of SPE-based SSLMBs evolution is discussed considering the concept of coupled and decoupled SPE systems introduced by C. Austen Angell in the early 1990s18,19.

Before the first industrial revolution in the early 19th century, global energy consumption relied heavily on traditional biomass (e.g., wood) and coal, as shown in Fig. 1a20. In the 1930s, significant advances in the petroleum industry enabled the shift from coal to petroleum-based high-energy sources21. However, petroleum resources are unevenly distributed worldwide, with nearly half located in the Middle East. So the increasing demand for petroleum-based energy from those countries having fewer reserves led to the oil crisis of the 1970s. This geopolitical situation prompted countries in the global north to explore alternative and disruptive technologies, seeking to transform the energy landscape and decrease dependence on fossil fuels, particularly through advancement in high-energy rechargeable batteries22,23.

a Evolution of global energy consumption during the past two centuries. The dashed arrow notes a surge in oil consumption in the 1970s. b Brief outline of batteries developed before the 1970s, including the primary Voltaic pile, primary Daniell cell, secondary lead-acid battery, secondary nickel–iron alkaline battery, and secondary nickel-cadmium battery27. c Photographic picture of the first solid-state cell assembled in 1972, in which sodium metal and chromium oxide intercalated into graphite (CrO3@graphite) were utilized as negative and positive electrode active materials, respectively. The solid-state sodium-ion conductor β-alumina was adopted as the electrolyte for supporting the operation of solid-state cell at room temperature (25 °C) with moderate stacking pressure (ca. 10 MPa). The crystal structures of sodium metal, CrO3@graphite, and β-alumina are obtained from Materials Projects120 and re-constructed with VESTA software121.

Before the 1970s, the specific energy of rechargeable batteries remained lower than 50 Wh kg−1 at the pack level, significantly hindering their large-scale application in the automotive industry (Fig. 1b). The utilization of lithium or sodium metal (Na°) negative electrodes and other high-energy electrode materials was considered a straightforward and effective approach to improve the specific energy of rechargeable batteries. Before the early 1970s, several attempts had been made to recharge lithium metal-based high-energy batteries. However, the formation of electrically unstable lithium metal electrodeposition morphologies, such as dendrites formed during the cycling process, caused significant safety issues, including the risk of fire and explosion24.

It thus became clear that nonaqueous liquid electrolyte solutions with high volatility and flammability were incompatible with lithium metal negative electrodes. For using high-energy metal negative electrodes, a solid-state electrolyte was considered key to building high-energy rechargeable batteries operated in ambient temperature region (−40 to 40 °C)25. In 1972, the very first prototype of a sodium-based solid-state cell was assembled by M. Armand25 utilizing sodium metal as the negative electrode, β-alumina as the solid electrolyte, and a chromium oxide/graphite intercalation compound (CrO3@graphite) at the positive electrode. The physical image of the cell constructed 50 years ago is shown in Fig. 1c. Effectively, under room temperature (25 °C) and moderate stacking pressure (ca. 10 MPa), the all-solid-state Na°||CrO3@graphite cell would deliver a high theoretical specific energy of ca. 1000 Wh kg−1 at the material level (i.e., energy content calculated by the mass of CrO3@graphite), nearly three times higher than the nickel-cadmium batteries26.

The first conference dedicated to solid-state materials was held in Belgirate (Italy) in 197227, which greatly accelerated the development of solid-state batteries (e.g., silver metal|silver sulfide iodide|iodine cell)28,29. In addition to the already known sodium-ion conductors (e.g., β-alumina30), several kinds of inorganic electrolytes capable of transporting lithium ions were discovered before the mid-1970s, including lithium iodide (LiI)31 and lithium nitride (Li3N)32. However, the high mechanical stiffness of inorganic electrolytes (e.g., Young’s modulus of 150 GPa for Li3N32) results in inadequate physical contact between the electrodes and the inorganic electrolyte, as illustrated in Fig. 2a. A high Young’s modulus also makes inorganic electrolytes unable to accommodate the induced mechanical stresses resulting from volume changes during cycling, resulting in cracks/small gaps formation at the electrode|electrolyte interface and interphases, the evolution of parasitic side reactions and formation of unfavorable metallic electrodepositions (e.g., dendrites)33.

a Critical role of soft contact between the electrode and a solid electrolyte. Lithium nitride (Li3N) and poly(ethylene oxide) (PEO)-based electrolytes are shown as typical examples for elucidating the distinctions between inorganic and organic materials. The crystal structures of Li3N are obtained from Materials Projects120 and re-constructed with VESTA software121. The light green, dark blue, and pink spheres refer to lithium, nitrogen, and oxygen atoms, respectively; and the black sticks represent the carbon–carbon linkage between two oxygen atoms in PEO. b Electron leakage versus ionic conduction in SPEs. Polymers were treated as insulating materials due to their large band gaps between valence and conduction bands (e.g., >4 eV for PEO34). The two discs (light gray) on the top and bottom of the SPE membrane represent the blocking electrodes. DC: direct current. c Phase diagram of lithium trifluoromethyl sulfonate (LiCF3SO3)/PEO. The values are taken from ref. 38. The light green and pink areas represent the amorphous phase (abbreviated as AP) region and two-phase region in the PEO-based electrolytes, respectively. PEO(C) and (PEO)3LiCF3SO3(C) denote the crystalline phase of PEO and the salt/polymer complex (i.e., (PEO)3LiCF3SO3), respectively. d Microscopic views of PEO-based SPEs at room (25 °C) and high (>60 °C) temperatures above the melting transition of PEO phases. e Effect of temperature on the ionic conductivity of PEO-based SPEs [(PEO)20LiCF3SO3] and conventional liquid electrolyte solutions (e.g., 1.0 mol kg−1 lithium hexafluorophosphate (LiPF6) per kilogram propylene carbonate). The ionic conductivity values are taken from refs. 39,122.

To overcome the contact issues between two rigid materials, designing soft solid electrolytes is an intuitive solution. In the late 1960s, it was established that polymeric materials are good electronic insulators (i.e., materials with the capability of blocking the transport of electrons) with large band gaps (>4 eV34) for electron jumping between conduction and valence bands (Fig. 2b). Yet, it was not clear whether the transportation of ionic species would be possible at that time. In 1966, Lundberg et al.35 investigated the mixture of metal salts (e.g., potassium iodide) and poly(ethylene oxide) (PEO). They concluded that metal salts interact with PEO and reduce crystallinity. In 1971, M. Armand carried out several ionic conductivity tests with lithium bromide (LiBr)/PEO. From the analysis of the results, he concluded that because of the very high resistance (>1 MΩ) measured at room temperature (ca. 20–30 °C), the utilization of LiBr/PEO for battery applications was not recommended. Two years later, Fenton et al.36 discovered that the mixtures of PEO and low-lattice-energy metal salts (e.g., sodium iodide (NaI), sodium thiocyanate (NaSCN), potassium thiocyanate (KSCN), etc.) become ionically conductive upon warming up the samples (e.g., ionic conductivities for the (PEO)4KSCN complex: 10−7 (40 °C) vs. 10−2 S cm−1 (170 °C)). This key finding rapidly caught the attention of Armand, and he suggested the utilization of these polymeric ionic conductors as solid electrolytes for building solid-state batteries37. These pioneering research works ushered a new direction for developing soft solid electrolytes and circumventing the surface contact issue in solid-state batteries with inorganic solid electrolytes.

However, it was still unclear why the ionic conductivity of PEO-based SPEs was sensitive to temperature. To shed some light on this aspect, Vallée et al. and Robitaille et al.38,39 systematically studied the phase diagrams of a series of lithium salt/PEO binary mixtures and revealed that PEO forms crystalline complexes with various kinds of lithium salts (e.g., (PEO)3lithium trifluoromethanesulfonate (LiCF3SO3), (PEO)6lithium perchlorate (LiClO4)) and eutectic mixtures with low melting transitions from 40 to 60 °C depending on the type of salt anions (e.g., 55 °C for (PEO)32LiCF3SO3), as shown in Fig. 2c.

Using solid-state nuclear magnetic resonance spectroscopy, Berthier et al.40 demonstrated that the amorphous phases in the PEO-based SPEs are primarily responsible for the transport of ionic species within the SPE. Therefore, the presence of crystalline phases at room temperature (e.g., 20–30 °C, Fig. 2d) was indicated as the main reason for the low ionic conductivities of PEO-based SPEs. Figure 2e shows the comparison of ionic conductivities of LiCF3SO3/PEO and lithium hexafluorophosphate (LiPF6)/propylene carbonate, which are representative examples of SPEs, and conventional nonaqueous liquid electrolyte solutions, respectively. In particular, the LiCF3SO3/PEO electrolyte shows two different regions below and above the melting transition of the crystalline phases in the Arrhenius plot, which highlights the critical role of the testing temperature on the ionic conductivity of the PEO-based SPEs.

For early-developed PEO-based SPEs, the ion transport at the microscopic scale is illustrated in Fig. 3. Generally, in amorphous phases, the long-range transport of ionic species, particularly lithium ions, is mainly realized via a segmental motion of the polymer backbone (Fig. 3a), following the percolation model proposed by M. A. Ratner and co-workers41. In the mixture of amorphous and crystalline phases, the crystalline surface can assist ion transport through surface coordination (Fig. 3b)42. In contrast, the inner cores of crystalline phases do not allow the lithium-ion transport due to the immobilized polymer segments, like in the helical conformation of PEO in the crystalline structure of (PEO)3LiCF3SO343. It is accepted that most crystalline complexes are poor ionic conductors, and the presence of these crystalline spherulites (i.e., typical morphology of crystalline PEO) in PEO-based SPEs causes a significant drop in ionic conductivities by discontinuing the conduction pathways in the amorphous phases44. For a well-defined crystalline complex (e.g., (PEO)6lithium hexafluoroarsenate), ion transport becomes possible via the hopping of lithium ions to adjacent sites (Fig. 3c)45. It has to be stressed that the molecular weight of PEO and the type of lithium salts are crucial to guarantee the rapid transport of lithium ions since the ion-hopping pathways are strongly associated with the accessible defects within these crystalline polymers.

a Graphical representation of the microscopic transport of lithium ions in fully amorphous phases, in which lithium-ion migration is tightly correlated with the segmental dynamic of polymer backbones. b Graphical representation of the microscopic transport of lithium ions in the mixture of amorphous and crystalline phases, where the surface functional groups of crystalline phases favor the transport of ionic species. c Graphical representation of the microscopic transport of lithium ions in crystalline phases, in which the cationic species migrate via the ion-hopping mechanism.

Because in the two former cases (Fig. 3a, b) the lithium-ion transport is associated with the segmental motion of PEO, these systems are labeled as coupled SPEs. In these cases, the degree of lithium salt dissociation and the structural flexibility (i.e., ease in conformational change) of anions determine the ionic conductivities of SPEs. Before the 1980s, the salts employed for SPEs contained mainly inorganic anions (e.g., SCN−(see ref. 36) and ClO4−(see ref. 46)), which either bind too strongly to lithium ions or have poor structural flexibility. The available organic anions at the time, e.g., CF3SO3−, also bind tightly to lithium cations, as demonstrated by vibrational spectroscopic studies of PEO and LiCF3SO3 mixtures47. Thanks to the development of sulfur-nitrogen chemistry48, in 1972, Meussdorffer et al.49 reported the preparation of the bis(trifluoromethanesulfonyl)imide (TFSI−) anion with a highly delocalized negative charge and inherent structural flexibility. This molecule was then brought into the battery research field by Armand et al.50 in the early 1980s. As seen in Fig. 4a, replacing CF3SO3− with TFSI− in the salt anion leads to an order of magnitude increase in total ionic conductivity (i.e., the sum of cationic and anionic conductivities), reaching 10−3 S cm−1 above the melting transitions of PEO phases (e.g., ca. 2 × 10−3 at 100 °C)38. This ionic conductivity meets the minimum requirements (i.e., >10−3 S cm−1) for operating SPE-based SSLMBs at elevated temperatures (≥80 °C)51,52. In the last decade, the development of molecules with delocalized negative charges has further progressed53,54. For example, Ma et al.54 proposed a delocalized polyanion, i.e., poly[(4-styrenesulfonyl)(trifluoromethyl(S-trifluoromethylsulfonylimino) sulfonyl)imide] (PSsTFSI−), that demonstrates improved lithium-ion conductivity of SPEs for unipolar conduction (i.e., only positive charges are mobile) due only to lithium cation (e.g., at 80 °C, ca. 10−4 S cm−1 for LiPSsTFSI-based electrolyte and ca. 10−5 S cm−1 for lithium poly[(4-styrenesulfonyl)(trifluoromethanesulfonyl)imide] (LiPSTFSI)-based electrolyte54). The polyanion PSsTFSI− could be obtained through the replacement of an oxygen atom in a TFSI-like moiety (i.e., CF3SO2N(−)SO2—) with strong electron-withdrawing trifluoromethanesulfonylimino ( = NSO2CF3) group; thus, the negative charges are further delocalized via five oxygens and two nitrogen atoms. These research works demonstrate an effective strategy for improving the ionic conductivity in coupled SPEs by weakening the interaction between salt anion and lithium ions.

a Chemical formula of lithium bis(trifluoromethanesulfonyl)imide (LiTFSI) and lithium trifluoromethanesulfonate (LiTf) and their ionic conductive properties in poly(ethylene oxide) (PEO)-based solid electrolytes at various temperatures. The values are taken from ref. 38. b Graphical representation of the inclusion of inorganic fillers in polymer electrolytes. c Schematic representation of amorphous Jeffamine-based polymer electrolytes. d Graphical summary of the in situ ultraviolet photo-irradiated cross-linking strategy for the PEO-based electrolytes.

Alternatively, to further increase the conductivity of SPEs, Croce et al.55 suggested the utilization of nano-sized inorganic fillers as active sites for suppressing the crystallization of ethylene oxide (EO) chains and promoting the lithium-ion transport via surface mechanism (Fig. 4b). Inorganic fillers can be electrochemically non-active or active (e.g., garnet and lithium phosphorus oxynitride)56, in which the bulk phases of inorganic fillers could provide additional transport channels besides the polymer phases (Fig. 4b). In addition, to facilitate rapid lithium-ion transport, the morphology of inorganic fillers was expanded from nanoparticles (i.e., less than 100 nm for all three Cartesian dimensions of the nanoparticle) to nano-wires (i.e., less than 100 nm for the diameter of the nanowire)57,58. Functionalization of nanofiller was also suggested to improve the compatibility of organic and inorganic phases59. It has to be noted that experimental evidence for the transport of lithium ions between polymer and inorganic phases is not widely reported, and this mechanism is not fully understood. However, it is reported that the transport along inorganic bulk phases is likely to only occur in inorganic-rich (>50 vol%) SPEs or when particular morphologies (e.g., nanowire) of inorganic phases are used56.

Various modification strategies, including polymer blends and co-polymerization12, have been proposed in the last two decades to suppress the crystallization of PEO matrices. For example, the co-polymerization of EO-containing monomers with styrene-based monomers has been investigated by various researchers60,61,62. It has been concluded that incorporating styrene-based moieties effectively suppresses the crystallization of EO units and improves the mechanical properties of the as-formed membranes61,62. Yet, sophisticated synthetic procedures are needed to tailor the chemical structures of the polymer matrices, which hinders the practical deployment of such strategies.

Jeffamine® compounds are commercial amine-terminated polyether oligomers produced by Huntsman Corporation63, widely used as foam stabilizers and corrosion inhibitors in petroleum industries. In 1992, Benrabah et al.64 suggested the utilization of the Jeffamine moiety as a charge carrier region for SPEs. Systematic investigations were also carried out to optimize the Jeffamine moiety’s chemical structures. It was found that the Jeffamine-based comb-like polymers (i.e., polymers comprising a linear backbone grafted with multiple side chains65) remain amorphous at room temperature (e.g., 20–30 °C) due to the presence of structurally disordered propylene oxide (PO) units (Fig. 4c), allowing an order of magnitude increase in ionic conductivities at room temperatures (e.g., 20–30 °C) for the corresponding SPEs compared to the PEO-based solid electrolytes66. Replacing LiTFSI with lithium bis(fluorosulfonyl)imide (LiFSI) in Jeffamine-based electrolytes leads to improved chemical and electrochemical stabilities of the lithium metal negative electrode, enabling the operation of SPE-based SSLMBs close to room temperatures (e.g., 20–30 °C)67.

To enhance the mechanical strength of PEO-based SPEs, Kim et al.68 reported in situ ultraviolet photo-irradiated cross-linking of PEO-based electrolytes in the absence of volatile solvents (Fig. 4d). This SPE preparation strategy could also be considered for possible implementation during hot-pressing processes (i.e., pressing electrolyte materials between two hot plates) which are typical procedures for making thin SPE films69. The preparation of cross-linked polymers through other synthetic methods has also been reported, as well as crystallinity suppression, ionic conductivity increment below the PEO melting temperature, and improvement of the elastic properties of SPEs33,70. In the past decades, the structural optimizations of lithium salts and polymer matrices have improved the transport, mechanical, and interfacial properties of the coupled SPEs, endowing the SPE-based SSLMBs with stable and highly reversible battery cycling performances12.

The main shortcomings of a strongly coupled SPE system are the low ionic conductivity in response to high Tg and the low lithium-ion transference number (tLi+). Typically, the value of tLi+ represents the portion of total currents carried solely by lithium ions. For coupled SPEs, the lithium cations are highly coordinated by electron-donating groups (e.g., ether oxygens) and become less mobile than the corresponding free anionic species (i.e., uncoordinated anions), resulting in relatively low metal-ion transference number (i.e., tM+ <0.5). As discussed above, a straightforward approach to increasing the ionic conductivity of coupled SPE is mainly through decreasing glass transition temperatures (Tg) via structural manipulation. Another approach proposed in refs. 18,71 is to look for more fragile polymers, which can be assessed by C. Austen Angell’s plot (Fig. 5a). Here, the term fragile signifies a deviation from Arrhenius behavior. Glass-formers with a high fragility are called fragile, that is, experiencing a more rapid increase in viscosity (i.e., faster cooling process) as they approach the glass transition temperature Tg (Fig. 5a)18. At the same temperature above Tg, the higher fragility of polymer, the larger deviation from Arrhenius behavior18,71. This eventually leads to higher ionic conductivities for the SPE comprising “fragile” polymer vs. conventional polyethers. For example, poly(vinyl chloride) (PVC) tends to be more fragile than poly(isobutylene), and in principle, the use of PVC could increase ionic conductivity. Since the glass transition temperature of polymer also strongly affects the ionic conductivity in coupled SPEs, finding an SPE capable of simultaneously satisfying the low Tg and high-fragility requirements is challenging, which limits a broader application of this fragility concept in SPEs.

a Angell plot for strong and fragile solid materials. b Entanglement mechanism of polymeric materials. Adapted from ref. 71 with permission. Copyright 1998 Society of Chemical Industry. c Walden–Angell plot for ionic materials. The values are taken from ref. 18. d, e Schematic representation of the microscopic ionic transport in true (d) and pseudo (e) decoupled solid polymer electrolytes. For true decoupled systems, polymers (black lines) empower the as-formed electrolytes with certain mechanical strength without participating in the transport of lithium ions.

Nevertheless, given the solid nature of SPEs, the increment of the polymer segmental motion alone cannot enhance metal-ion diffusion enough unless the metal-ion motions are decoupled from the polymer dynamics (e.g., segmental diffusion, chain relaxation, etc). Some attempts to enhance the decoupled metal-ion motion included modifying the polymer chemistry in the backbone by incorporating functional groups that weakly coordinate with metal ions, such as poly(carbonates)72 and poly(tetrahydrofuran)73. However, this strategy has so far failed to significantly improve ion decoupling and ionic conductivities. Indeed, the ionic conductivity remained low due to the high rigidity of polymer backbones74.

In the 1990s, Angell et al.75 proposed a novel approach for achieving decoupled superionic systems (i.e., the ion transport which is decoupled from the apparent viscosity of system) via a so-called polymer-in-salt (PIS)-type SPEs. In this work, a high content (90 wt%) of a superionic four-salt melt (i.e., LiI/lithium acetate (LiOAc)/lithium chlorate (LiClO3)/LiClO4) was mixed with a small amount (10 wt%) of high-molecular-weight (4 × 103 g mol−1) poly(propylene oxide), achieving a room temperature (e.g., 20–30 °C) ionic conductivity of about 10−4 S cm−1. The salts provide ionic conductivity and the role of polymer here is to provide mechanical strength. According to ref. 76, the macroscopic viscosity (i.e., apparent viscosity which is experimentally measurable) of polymers increases significantly when the numbers of repeat units exceed a threshold value of 200, which is known as the entanglement effect (Fig. 5b). Such a distinctive feature allows the solidification of this superionic liquids system upon the addition of small amounts (<5 wt%) of high-molecular-weight polymers.

The concept of decoupling in such a system is formulated on a hypothesis that when the salt concentration keeps increasing to a threshold, Tg finally will reach a maximum, then further increasing salt concentration will enhance the ion movements and should simultaneously increase the decoupling of the small metal ions from the polymer backbone. Later in the early 2000s, research provided further insight into the PIS electrolytes. It was shown that excess salt in SPEs leads to the formation of salt aggregates in which metal ion can diffuse through anions. Those aggregates become more interconnected at high salt concentrations (>50 wt% of salt in SPEs)17, promoting the metal ions to diffuse through this second conduction path. This demonstrates the ability of PIS-type SPEs to decouple metal-ion motion from polymer dynamics77. Several criteria, such as polymer Tg, salt type, polymer/salt solubility, electrochemical stability, and ionic conductivity78, were also discussed in C. Austen Angell’s early works to understand the physicochemical properties of PIS electrolytes. Among these, the concept of the ionicity of lithium salt is of utter importance. Specifically, ionicity is a measure of the degree of ion dissociation, commonly referring to the effective fraction of ionic species being able to participate in ionic conduction18. Figure 5c displays the Walden-Angell plot for the dependence of equivalent conductivities on the viscosities of electrolytes. With 1.0 M potassium chloride/H2O solution as a reference electrolyte, the regime above the diagonal line refers to the electrolyte materials with super-ionic characters. For PIS-type SPE systems, the lithium salt should possess sufficient ionicity to ensure the high conductivity, i.e., be located in the super-ionic regime in Fig. 5c.

However, the superionic salt solution C. Austen Angell proposed is not applicable to lithium metal batteries due to the poor chemical and electrochemical stabilities of the as-prepared PIS-type SPEs. Starting from the late 1990s, several other PIS-type SPE systems having different polymer structures and salts were proposed and investigated, including poly(acrylonitrile) (PAN)-in-salt79, which incorporated a LiCF3SO3 salt with the PAN polymer. Unfortunately, this PIS electrolyte showed inadequate ionic conductivities, e.g., 2 × 10−6 S cm−1 at 50 °C and 10−5 S cm−1 at 75 °C79, which were increased to 10−4 S cm−1 at 30 °C by Wu et al.80 in 2016 used graphene oxide (GO) as a nanofiller. The authors claim that the GO nanosheets provide a fast three-dimensional ion transport network. In addition, recent research works reported various benefits of using PIS-type electrolytes for lithium metal batteries, including but not limited to stable interphase formation, improved cycling performance81, enhanced oxidation stability82, and increased compatibility with high-voltage positive electrodes83.

However, the proposed PIS electrolytes are still far from achieving true decoupling. Indeed, in a true decoupled system, metal ions should move independently of the polymer (Fig. 5d)18. In practical non-ideal systems (aka. pseudo-decoupled systems), true decoupling cannot be obtained because of the chemical interactions constantly occurring between ions and the repeat units (Fig. 5e). Therefore, in a decoupled superionic system, the influence of polymers on the motion of metal ions should be minimized, and the ionicity of salt should be maximized. Experimentally, one can measure decoupled motion by comparing time scales for polymer structural relaxation (i.e., cooperative reorientation of polymer segments78) with ionic conductivity relaxation using Tg-scaled Arrhenius plot84. So far, the search for superionic low melting-point salts for alkali metal ions is still ongoing and represents a great challenge for the electrolyte research community85. Nevertheless, the strategy of using salt mixtures to maintain their liquid state at room temperatures (e.g., 20–30 °C) to achieve high ionic conductivities was successful85. Clearly, C. Austen Angell’s research opened a new avenue for designing solid and liquid electrolyte materials86,87.

In the field of electrolytes, the equivalent conductivity of a given system is generally found to be inversely proportional to its viscosity, as defined by the Walden rule (Eq. (1))88

where Λ is equivalent conductivity, and η is viscosity. Effectively, an ideal decoupled electrolyte follows the Walden rule and shows a certain degree of derivation from the Arrhenius behavior in the ionic conductivity–temperature, provides significantly increased ionic conductivity as temperature elevates slightly above glass transition temperature (Fig. 6a, black line). However, due to the entanglement effect (i.e., transient cross-links between polymer chains), the Walden rule becomes unapplicable for decoupled SPEs, and the ionic conductivities remain at much higher values than expected (i.e., viscosity does not dominate the transport of the ions; Fig. 6a, red line). Therefore, the breakdown of the Walden rule (i.e., diminishing the impact of viscosity on ion transport) effectively favors the increase of ionic conductivity for SPEs.

a Comparison between ideal and experimental decoupled solid polymer electrolytes (SPEs) in a typical Arrhenius plot for ionic conductivities. Adapted from ref. 71 with permission. Copyright 1998 Society of Chemical Industry. b Dependence of decoupling exponent (ε) on fragility index (m) and glass transition temperature (Tg) for various kinds of polymers. pl-PVC plasticized poly(vinyl chloride), PC poly(carbonate), PEO poly(ethylene oxide), PMMA poly(methyl methacrylate), PVAc poly(vinyl acetate), PVC poly(vinyl chloride), PVDC poly(vinylidene chloride), P2ClSt poly(2-chlorostyrene), P2VP poly(2-vinylpyridine), P3ClSt poly(3-chlorostyrene), P4BrSt poly(4-bromostyrene), P4ClSt poly(4-chlorostyrene), P4VP poly(4-vinylpyridine). Adapted from ref. 90 with permission. Copyright 2011 American Chemical Society. c Ionic conductivities of poly(diallyldimethylammonium) (PDADMA)-based electrolytes vs. concentration of lithium salts at 30 °C (black line), 50 °C (red line), and 80 °C (blue line). Reproduced from ref. 95 with permission. Copyright 2019 Elsevier. d Interactions between lithium cations and anions in the P(DADMA+)-based electrolytes. The chemical structures are visualized with VESTA software122.

Agapov et al.89 systematically investigated the relations between the decoupling exponent (ε), fragility index (m), and Tg (see Fig. 6b). The decoupling exponent and fragility index are mathematically expressed below90,91:

Where ε is the decoupling exponent, τ is the characteristic relaxation time of the polymer segment, Tg is the glass transition temperature, σo is the ionic conductivity at temperatures close to Tg, and T is the temperature89. It has been demonstrated that ionic species might migrate in high-fragility polymers (fragility index m > 4089) via the loose structures (i.e., rigid polymer chains with low packing density), despite their low segmental relaxation rate; segmental motion is necessary for the less-fragile polymers with dense structures (i.e., compact packing of flexible polymer chains), including PEO and other polyethers.

In 2017 and 2019, Angell wrote two review articles to discuss the research directions to achieve decoupling ion motion18,84, namely, the side-chain solvation decoupling and the anion-trapping strategies. The concept of side-chain solvation decoupling is to allocate the cation-solvating groups on a pendant side chain of polymer matrices to decouple the transport of cations from the segmental relaxation of the polymer backbone. Unfortunately, the practical implementation of this strategy is challenging due to the absence of the secondary relaxation effect (e.g., the motion of side chains) before reaching sufficient relaxation time (e.g., 10−10 s) required by ion transport for battery use84. In comparison, anion-trapping strategies have shown some success in increasing tLi+ values in polymer electrolytes either by developing polymers that are more prone to solvate anions than lithium ions (such as including under-coordinated boron centers in polymer chains92) or designing new anion chemistries to increase its interaction with polymers and slow down anion motion93. A more direct method to trap anions can be using a cationic polymer electrolyte94. However, the recent progress in developing cationic polymer electrolytes is not only limited to providing anion-trapping functions.

For example, Wang et al.94 reported a type of PIS-type SPE based on cationic poly(ionic liquid) (PolyIL, Fig. 6c, d), in which ionic liquid cations are chemically bound to a polymer backbone, showing promising physicochemical and electrochemical results. This PolyIL, more precisely poly(diallyldimethylammonium) bis(fluorosulfonyl)imide (P(DADMA+)FSI−), presented a decreased Tg at elevated LiFSI salt concentrations from a low to a high concentration range ([Li+]/[polycation] increases from 0.5 to 4). The highest conductivity was obtained at a high salt concentration of [Li+]/[polycation] = 1.5 within the temperature range from 30 °C to 80 °C, which in fact, forms a PolyIL-in-salt (PolyIL-IS) electrolyte. Later, through molecular simulations, Chen et al.95 predicted the fast transport of sodium- and potassium- ions in the same PolyIL system. They also experimentally verified the sodium-ion conduction behavior for the PolyIL-IS [Na+]/[polycation] = 2 system. The PolyIL-IS system demonstrated an ionic conductivity of 1 × 10−3 S cm−1 at 80 °C without adding any plasticizers (i.e., compounds for improving polymer dynamics), and a high decoupling index with log (Rτ) close to 6.3, which is clear evidence to suggest the decoupled ion motion in this PolyIL-IS96. However, the ionic conductivities at room temperatures (20–30 °C) are still two orders of magnitudes lower than that of conventional nonaqueous electrolytes, e.g., at 30 °C, ca. 2 × 10−4 (PolyIL-IS) vs. 1 × 10−2 S cm−1 (1.0 M LiPF6/ethylene carbonate-ethyl methyl carbonate97).

Although various approaches have been proposed, tested, and developed, true decoupled SPEs is still unattainable today. As C. Austen Angell mentioned in his 2019 review article, “there is some fundamental problem in the original salt-in-polymer solvent (and anionic polymer) physics, due to the ion proximity to the mobility-limiting polymer chains”84. This aspect is true for PEO-type SPEs and the anionic single-ion conductors (anionic transference number >0.9). This is also a fact in most PIS-type electrolytes since only a small portion of metal ions can be decoupled from the polymer, whereas the rest are still bound to the polymer chains. In the case of the PolyIL-IS systems, the weak coupling between the metal ion and the polymer exists through the anion-bridging co-coordination. The highly coupled metal ion-anion motion also limits the metal-ion transference number to ca. 0.595. In this case, improving the ionicity of the salt could maximize the decoupling motion in PolyIL-IS, although not yet experimentally proved.

The development of SPE-based SSLMBs is closely associated with the discovery of positive electrode active materials. Lithium vanadium oxides (e.g., Li1+xV3O8, 0 <x < 2) have been long investigated as positive electrode active materials since the early 1970s due to their wide range of oxidation states enabling high specific capacities during reversible electrochemical reactions98. B. Scrosati and co-workers99 systematically studied the electrochemical performances of Li°|LiCF3SO3/PEO|Li1.2V3O8 cells and suggested that adequate cell rechargeability could be attained at relatively high temperatures (ca. 100 °C). With the optimization of SPEs and vanadium oxide-based positive electrodes, long-term (>1000 cycles) and stable cycling of these SPE-SSLMBs have been achieved by the research group at Hydro-Québec100. Yet, the main obstacle to large-scale implementation of batteries with vanadium-based positive electrodes lies, at the cell level, in the dissolution of vanadium species during continuous cycling, and at the raw material level, in the uneven geographical distribution of vanadium resources worldwide101.

In 1997, Padhi et al.102 reported an olivine-type positive electrode active material (Fig. 7a, left), i.e., lithium iron phosphate (LiFePO4), which shows a flat discharge/charge plateau at ca. 3.45 V vs. Li/Li+, and specific energy, at the material level, slightly higher than that of vanadium-based positive electrode active materials (Fig. 7a, right). However, the electronic conductivity of pristine LiFePO4 powder (e.g., 2 × 10−9 S cm−1 at 25 °C103) is lower compared to other layered oxide positive electrode active materials (e.g., 6 × 10−4 S cm−1 for lithium cobalt oxide (LiCoO2) at 25 °C104). This aspect favors sluggish electrode kinetics and poor rate-capability performance of the LiFePO4-based batteries. In 1998, Armand et al.105 attempted to increase the electrode kinetics by ball-milling LiFePO4 powder with conductive carbon in a poly(ethylene) jar. By accident, the ball-milling process was left for an unexpectedly long duration. The positive electrode formulated using the ball-milled LiFePO4 laminates showed improved enhanced rate-capabilities when tested in Li metal lab-scale cells using a nonaqueous electrolyte solution. Systematic investigations showed that ball-milled poly(ethylene) was converted into amorphous carbon during subsequent calcination and coated the surface of LiFePO4 particles. These results suggest that carbon-coating is an effective strategy to improve the reaction kinetics of positive electrode active materials with low electronic conductivity (Fig. 7b). Indeed, the deployment of carbon-coated LiFePO4 substantially increases the cycle life and attainable specific energy of SPE-based SSLMBs105. Moreover, the abundance of the elements in LiFePO4 suggests a higher sustainability of such technology than cobalt-based positive electrode active materials14. The rate performance of LiFePO4-based SSLMBs is further enhanced by decreasing the particle sizes of LiFePO4 powders into nanoscale prior to electrode formulation (Fig. 7b)106,107.

a (left) Schematic representation of the structural and chemical compositions of lithium vanadium oxide (LiV3O8) and lithium iron phosphate (LiFePO4, LFP). The crystal structures of LiV3O8 and LiFePO4 are obtained from Materials Projects121 and re-constructed with VESTA software122. (right) Comparison of voltage curves of Li metal cells with SPE comprising a Li1.2V3O8- and carbon-coated-LiFePO4- based positive electrodes cycled at 0.2 mA g−1. The values are taken from ref. 101. b Schematic representations of the LiFePO4 carbon-coating and nano-size reduction strategies c Photographic picture of the Bluebuses® developed by Bolloré group, in which SPE-based SSLMBs are utilized as the only power source. The photo is provided courtesy by the Bolloré Group. d Challenges for the contemporary SPEs and their batteries, in which conventional SPEs comprising polyethers are likely to be only suitable for low-voltage cathodes (e.g., sulfur (S), LFP), and improvement in the electrochemical window and ionic conductivities of SPEs are desired for future development.

Presently, the SSLMBs comprising LiTFSI-based SPEs and LiFePO4-based positive electrodes have been practically deployed as power sources for EVs and grid storage by the Bolloré group. Figure 7c shows the photographic pictures of Bluebuses® equipped with 120 kWh SPE-based SSLMBs. Up to 2020, more than 1000 Bluecars® and 500 Bluebuses® have been produced, reaching a cumulated driving experience of >6 × 108 km with a decent safety record (only two cases with unexplained runaway reactions). These industrially-relevant examples stimulated industrial and academic laboratories to restart the research activities in lithium metal rechargeable batteries after the initial abandonment of this technology as a consequence of the various fire accidents that occurred in AA-size Li°||molybdenum disulfide cells produced by Moly Energy in the late 1980s24.

It is important to highlight that a wider application of SPE-based SSLMBs is hindered by their low specific energy (<400 Wh kg−1) and rate-capability (< 2 C), stemming from the unsatisfactory anodic stability and ionic conductivities of the state-of-the-art SPEs (Fig. 7d). Besides, due to the low ionic conductivities of SPEs at room temperature (< 10−4 S cm−1 at 25 °C), the SPE-based SSLMBs need to be operated at elevated temperatures (60–80 °C), thus requiring additional accessories for thermal management108. To date, various types of solid electrolyte technologies have been proposed, e.g., structurally ordered organic/inorganic composite electrolytes109, in situ formed polymer electrolytes110, and localized high‐concentration electrolytes (i.e., with non-solvating diluents)111. Although these electrolyte concepts suggest plausible approaches to circumvent the obstacle to the development of solvent-free SPE-SSLMBs, further assessment of the long-term stability and scalability of these technologies are required to move toward technology readiness levels ≥5 (e.g., for practical application in large-format SSLMBs)5.

For the basic SPEs that simply contain a single lithium salt and a single polymer matrix, it is unclear if they could be used to boost the performances of SSLMBs. Although the anodic stability of the PEO-based SPEs is inadequate for coupling with high-voltage insertion-based positive electrode active materials (e.g., nickel-rich LiNixCoyMn1−x−yO2)60, it is possible to couple SPEs with high specific-energy positive electrode active materials that exploit conversion reactions for lithium-ion storage (e.g., sulfur/organosulfur and oxygen/lithium oxide). For example, Hu et al.112 proposed the utilization of iron fluoride (FeF3) as a conversion-type positive electrode to produce high-energy SPE-based SSLMBs. By introducing aluminum fluoride as an electrolyte additive, the tLi+ value of standard PEO-based SPEs was enhanced (ca. 0.6 at 60 °C), and the corresponding Li°||FeF3 lab-scale cell showed high initial capacities (ca. 600 mAh g−1 at 60 °C). In this context, it should also be pointed out that the multi-layer structure of electrolyte films could improve the stability of the interphases formed at the electrode|SPE interfaces. For instance, using a double-layer SPE comprising a polyether-based membrane for the lithium negative electrode and a polyester-based membrane for the high-voltage positive electrode could improve the cyclability of SSLMBs113. Moreover, the interdiffusion of lithium salt originating from the different activity coefficients (i.e., a measure for the difference between real and ideal solutions) in the two electrolytes in contact could be tailored by replacing discrete anions with polyanions114.

Looking at future development, to improve the rate-capability of SPE-based SSLMBs, it is essential to enchance the lithium-ion conductivities of SPEs by thinking out-of-the-box to deliver unconventional approaches for material development. For example, inheriting C. Austen Angell’s polymer-in-salt concept, would it be possible to prepare lithium salts with high ionicity in the liquid state at room temperatures (20–30 °C)? Starting from LiCF3SO3, the replacement of one oxygen atom ( = O) with =NSO2CF3 gives LiTFSI (i.e., Li[CF3SO2(NSO2CF3)]) with a lower melting point [i.e., Tm = 233 °C (LiTFSI) vs. >350 °C (LiCF3SO3)]115. A further homologation of the oxygen atom results in the formation of a super lithium sulfonimide salt (Li[CF3SO(NSO2CF3)2], LisTFSI) with a low melting transition approaching the ionic liquid domain (i.e., Tm ≤ 100 °C for typical ionic liquids88, and Tm = 118 °C for LisTFSI116). In this regard, we speculate that the concept of negative charge delocalization could be extended further to accessing liquid lithium salts. From another perspective, one may also replace typical neutral polyether/polyesters with charged polysalts (e.g., polycations, polyanions, or poly(zwitterions)), to regulate the ion-ion interactions and thereby achieving decoupled SPE systems117. For instance, the utilization of imidazole-type poly(zwitterions) could provide ordered subdomains with superionic nature, which allows rapid transport of ionic species even at temperatures close to their Tg values118.

In summary, we provided a reflection on SPEs and their application in SSLMBs focusing on the key milestones reached over the last five decades of research and development. The emergence of SPEs arises from the demand for soft solid electrolytes to circumvent the contact issues faced by SSLMBs using inorganic solid-state electrolytes. The utilization of SPEs stimulated the development of SSLMBs, making the long-term cycling of lithium metal negative electrodes possible. For future development, it is essential to bear in mind that designing high-performance SPE-based SSLMBs requires not only highly ionic conductive SPEs but also stable electrode|electrolyte interphases. As suggested by C. Austen Angell, decoupled SPE systems could be helpful in designing lithium salts and polymers with tailored structures and building lithium-ion conductive SPEs with high selectivity for cation transport. We advise that coupling high-energy conversion-type positive electrode active materials with SPEs could be an effective approach to enhance the energy content of the state-of-the-art SPE-based SSLMBs5, along with the improvement of inherent characteristics (e.g., suppressed volume changes, enhanced redox kinetics, high tap density, etc.) of conversion-type positive electrodes5. It has to be highlighted that SPEs with sufficient geometric flexibility are the key to confronting the solid-solid contact issues in SSLMBs119; and it could be anticipated that SPEs with improved electrochemical stabilities and ionic conductivities, particularly cation-only conductivities, will continue to be a desirable solution for developing more sustainable battery technologies.

Verne, J. Vingt mille lieues sous les mers (Hetzel Editor, Paris, 1870).

Armand, M. in Materials for Advanced Batteries (eds Murphy, D. W. Broadhead, J. & Steele, B. C. H.) 145–161 (Springer, 1980).

Zhang, H. et al. From solid-solution electrodes and the rocking-chair concept to today’s batteries. Angew. Chem. Int. Ed. 59, 534–538 (2020). This viewpoint provides a historical overview on the essential findings related to today’s lithium-ion batteries and solid-state batteries.

Article CAS Google Scholar

Bloomberg NEF group. Electric Vehicle Outlook 2022. https://about.bnef.com/electric-vehicle-outlook/ (2023).

Frith, J. T., Lacey, M. J. & Ulissi, U. A non-academic perspective on the future of lithium-based batteries. Nat. Commun. 14, 420 (2023).

Article ADS CAS PubMed PubMed Central Google Scholar

Armand, M. et al. Lithium-ion batteries—current state of the art and anticipated developments. J. Power Sources. 479, 228708 (2020).

Article CAS Google Scholar

Famprikis, T., Canepa, P., Dawson, J. A., Islam, M. S. & Masquelier, C. Fundamentals of inorganic solid-state electrolytes for batteries. Nat. Mater. 18, 1278–1291 (2019).

Article ADS CAS PubMed Google Scholar

Janek, J. & Zeier, W. G. A solid future for battery development. Nat. Energy 1, 16141 (2016).

Article ADS Google Scholar

Varzi, A., Raccichini, R., Passerini, S. & Scrosati, B. Challenges and prospects of the role of solid electrolytes in the revitalization of lithium metal batteries. J. Mater. Chem. A 4, 17251–17259 (2016).

Article CAS Google Scholar

Zhang, H. et al. Single lithium-ion conducting solid polymer electrolytes: advances and perspectives. Chem. Soc. Rev. 46, 797–815 (2017). This review presents the evolution of key progresses related to the polymer electrolyte with high lithium-ion transport number.

Article CAS PubMed Google Scholar

Lopez, J., Mackanic, D. G., Cui, Y. & Bao, Z. Designing polymers for advanced battery chemistries. Nat. Rev. Mater. 4, 312–330 (2019).

Article ADS CAS Google Scholar

Mindemark, J., Lacey, M. J., Bowden, T. & Brandell, D. Beyond PEO—alternative host materials for Li+-conducting solid polymer electrolytes. Prog. Polym. Sci. 81, 114–143 (2018).

Article CAS Google Scholar

https://www.blue-solutions.com/. Accessed 29 June 2023.

Manthiram, A. A reflection on lithium-ion battery cathode chemistry. Nat. Commun. 11, 1550 (2020).

Article ADS CAS PubMed PubMed Central Google Scholar

Xie, J. & Lu, Y. A retrospective on lithium-ion batteries. Nat. Commun. 11, 2499 (2020).

Article ADS CAS PubMed PubMed Central Google Scholar

Winter, M., Barnett, B. & Xu, K. Before Li ion batteries. Chem. Rev. 118, 11433–11456 (2018).

Article CAS PubMed Google Scholar

Zhang, H. & Armand, M. History of solid polymer electrolyte-based solid-state lithium metal batteries: a personal account. Isr. J. Chem. 61, 94–100 (2020).

Article ADS Google Scholar

Angell, C. A. Polymer electrolytes—some principles, cautions, and new practices. Electrochim. Acta 250, 368–375 (2017). This work outlines the fundamentals of desigining decoupled polymer electrolytes.

Article CAS Google Scholar

Angell, C. A. Dynamic processes in ionic glasses. Chem. Rev. 90, 523–542 (2002).

Article Google Scholar

Ritchie, H., Roser, M. & Rosado, P. Energy. https://ourworldindata.org/energy (2023).

History.com Editors. Oil industry. https://www.history.com/topics/industrial-revolution/oil-industry (2023).

Armand, M. & Tarascon, J. M. Building better batteries. Nature 451, 652–657 (2008).

Article ADS CAS PubMed Google Scholar

Goodenough, J. B. How we made the Li-ion rechargeable battery. Nat. Electron. 1, 204–204 (2018).

Article Google Scholar

Xu, K. A long journey of lithium: from the big bang to our smartphones. Energy Environ. Mater. 2, 229–233 (2019).

Article Google Scholar

Armand, M. in Fast Ion Transport in Solids (eds van Gool, W.) 665–672 (North Holland Publishing, 1972).

Omar, N. et al. Reference Module in Chemistry, Molecular Sciences and Chemical Engineering (Elsevier, 2014).

Owens, B. B. Solid state electrolytes: overview of materials and applications during the last third of the Twentieth Century. J. Power Sources. 90, 2–8 (2000).

Article ADS CAS Google Scholar

Scrosati, B. Recent advances in lithium solid state batteries. J. Appl. Electrochem. 2, 231–238 (1972).

Article CAS Google Scholar

Takahashi, T. & Yamamoto, O. The Ag/Ag3SI/I2 solid-electrolyte cell. Electrochim. Acta 11, 779–789 (1966).

Article CAS Google Scholar

Yu, Y. & Kummer, J. T. Ion exchange properties of and rates of ionic diffusion in beta-alumina. J. Inorg. Nucl. Chem. 29, 2453–2475 (1967).

Article Google Scholar

Haven, Y. The ionic conductivity of Li-halide crystals. Recl. Trav. Chim. Pays-Bas 69, 1471–1489 (1950).

Article CAS Google Scholar

Li, W., Chen, J. & Wang, T. Electronic and elastic properties of Li3N under different pressure. Phys. B Condens. Matter. 405, 400–403 (2010).

Article ADS CAS Google Scholar

Banerjee, A., Wang, X., Fang, C., Wu, E. & Meng, Y. Interfaces and interphases in all-solid-state batteries with inorganic solid electrolytes. Chem. Rev. 120, 6878–6933 (2020).

Article CAS PubMed Google Scholar

Mohan, V. M., Raja, V., Bhargav, P. B., Sharma, A. K. & Rao, V. V. R. N. Structural, electrical and optical properties of pure and NaLaF4 doped PEO polymer electrolyte films. J. Polym. Res. 14, 283–290 (2007).

Article CAS Google Scholar

Lundberg, R. D., Bailey, F. E. & Callard, R. W. Interactions of inorganic salts with poly(ethylene oxide). J. Polym. Sci. A Polym. Chem. 4, 1563–1577 (1966).

Article ADS CAS Google Scholar

Fenton, D. E., Parker, J. M. & Wright, P. V. Complexes of alkali metal ions with poly(ethylene oxide). Polymer 14, 589 (1973).

Article CAS Google Scholar

Armand, M., Chabagno, J. & Duclot, M. Second International Meeting on Solid Electrolytes (St Andrews, 1978).

Vallée, A., Besner, S. & Prud’Homme, J. Comparative study of poly(ethylene oxide) electrolytes made with LiN(CF3SO2)2, LiCF3SO3 and LiClO4: thermal properties and conductivity behaviour. Electrochim. Acta 37, 1579–1583 (1992).

Article Google Scholar

Robitaille, C. D. & Fauteux, D. Phase diagrams and conductivity characterization of some  PEO-LiX electrolytes. J. Electrochem. Soc. 133, 315–325 (1986).

Article ADS CAS Google Scholar

Berthier, C. et al. Microscopic investigation of ionic conductivity in alkali metal salts-poly(ethylene oxide) adducts. Solid State Ionics 11, 91–95 (1983).

Article CAS Google Scholar

Ratner, M. A. & Shriver, D. F. Ion transport in solvent-free polymers. Chem. Rev. 88, 109–124 (1988).

Article CAS Google Scholar

Marzantowicz, M., Dygas, J. R., Krok, F., Florjańczyk, Z. & Zygadło-Monikowska, E. Influence of crystalline complexes on electrical properties of PEO:LiTFSI electrolyte. Electrochim. Acta 53, 1518–1526 (2007).

Article CAS Google Scholar

Lightfoot, P., Mehta, M. A. & Bruce, P. G. Crystal structure of the polymer electrolyte poly(ethylene oxide)3:LiCF3SO3. Science 262, 883–885 (1993).

Article ADS CAS PubMed Google Scholar

Marzantowicz, M. et al. In situ microscope and impedance study of polymer electrolytes. Electrochim. Acta 51, 1713–1727 (2006).

Article CAS Google Scholar

Gadjourova, Z., Andreev, Y. G., Tunstall, D. P. & Bruce, P. G. Ionic conductivity in crystalline polymer electrolytes. Nature 412, 520–523 (2001).

Article ADS CAS PubMed Google Scholar

Gauthier, M. et al. Behavior of polymer electrolyte batteries at 80–100°C and near room temperature. J. Power Sour. 14, 23–26 (1985).

Article ADS CAS Google Scholar

Frech, R., Chintapalli, S., Bruce, P. G. & Vincent, C. A. Dual fluorination of polymer electrolyte and conversi in the poly(ethylene oxide)−LiCF3SO3 system. Macromolecules 32, 808–813 (1999).

Article ADS CAS Google Scholar

Becker, R. Gmelin Handbuch der Anorganischen Chemie (Springer, 1977).

Meussdorffer, J. N. N. Bisperfluorakansulfonylimide (RfSO2)2NH Chem. Ztg. 96, 582–583 (1972).

Google Scholar

Armand, M. & Moursli, F. E. K. C. Bis perhalogénoacyl-ou sulfonyl-imidures de metaux alcalins, leurs solutions solides avec des matières plastiques et leur application à la constitution d'éléments conducteurs pour des générateurs électrochimiques. FR patent 2527602A1 (1983).

Wang, Q. et al. Siloxane-based polymer electrolytes for solid-state lithium batteries. Energy Stor. Mater. 23, 466–490 (2019).

Google Scholar

Zhao, W., Yi, J., He, P. & Zhou, H. Solid-state electrolytes for lithium-ion batteries: fundamentals, challenges and perspectives. Electrochem. Energy Rev. 2, 574–605 (2019).

Article CAS Google Scholar

Meziane, R., Bonnet, J. P., Courty, M., Djellab, K. & Armand, M. Single-ion polymer electrolytes based on a delocalized polyanion for lithium batteries. Electrochim. Acta 57, 14–19 (2011).

Article CAS Google Scholar

Ma, Q. et al. Single lithium-ion conducting polymer electrolytes based on a super-delocalized polyanion. Angew. Chem. Int. Ed. 55, 2521–2525 (2016).

Article CAS Google Scholar

Croce, F., Appetecchi, G. B., Persi, L. & Scrosati, B. Nanocomposite polymer electrolytes for lithium batteries. Nature 394, 456–458 (1998).

Article ADS CAS Google Scholar

Keller, M., Varzi, A. & Passerini, S. Hybrid electrolytes for lithium metal batteries. J. Power Sour. 392, 206–225 (2018).

Article ADS CAS Google Scholar

Liu, W. et al. Ionic conductivity enhancement of polymer electrolytes with ceramic nanowire fillers. Nano Lett 15, 2740–2745 (2015).

Article ADS CAS PubMed Google Scholar

Liu, W. et al. Enhancing ionic conductivity in composite polymer electrolytes with well-aligned ceramic nanowires. Nat. Energy 2, 17035 (2017).

Article ADS CAS Google Scholar

Porcarelli, L. et al. Single-ion conducting polymer nanoparticles as functional fillers for solid electrolytes in lithium metal batteries. ACS Appl. Mater. Interfaces 13, 54354–54362 (2021).

Article CAS PubMed PubMed Central Google Scholar

Gomez, E. D. et al. Effect of ion distribution on conductivity of block copolymer electrolytes. Nano Lett. 9, 1212–1216 (2009).

Article ADS CAS PubMed Google Scholar

Jannasch, P. Ionic conductivity in physical networks of polyethylene-polyether-polyethylene triblock copolymers. Chem. Mater. 14, 2718–2724 (2002).

Article CAS Google Scholar

Stone, G. M. et al. Resolution of the modulus versus adhesion dilemma in solid polymer electrolytes for rechargeable lithium metal batteries. J. Electrochem. Soc. 159, A222–A227 (2012).

Article CAS Google Scholar

Aldalur, I., Armand, M. & Zhang, H. Jeffamine-based polymers for rechargeable batteries. Batteries Supercaps 3, 30–46 (2019).

Article Google Scholar

Benrabah, D., Sanchez, J. Y. & Armand, M. New polyamide-ether electrolytes. Electrochim. Acta 37, 1737–1741 (1992).

Article CAS Google Scholar

McKeen, L. in The Effect of Sterilization Methods on Plastics and Elastomers (eds Ebnesajjad, S.) 41–61 (Elsevier, 2018).

Aldalur, I. et al. Jeffamine® based polymers as highly conductive polymer electrolytes and cathode binder materials for battery application. J. Power Sources 347, 37–46 (2017).

Article ADS CAS Google Scholar

Aldalur, I. et al. Lowering the operational temperature of all-solid-state lithium polymer cell with highly conductive and interfacially robust solid polymer electrolytes. J. Power Sources 383, 144–149 (2018).

Article ADS CAS Google Scholar

Kim, G. T. et al. UV cross-linked, lithium-conducting ternary polymer electrolytes containing ionic liquids. J. Power Sources 195, 6130–6137 (2010).

Article ADS CAS Google Scholar

Aldalur, I. et al. Nanofiber-reinforced polymer electrolytes toward room temperature solid-state lithium batteries. J. Power Sources 448, 227424 (2020).

Article CAS Google Scholar

Tosa, M., Hashimoto, K., Kokubo, H., Ueno, K. & Watanabe, M. Effect of network homogeneity on mechanical, thermal and electrochemical properties of solid polymer electrolytes prepared by homogeneous 4-arm poly(ethylene glycols). Soft Matter 16, 4290–4298 (2020).

Article ADS CAS PubMed Google Scholar

Angell, C. A., Imrie, C. T. & Ingram, M. D. From simple electrolyte solutions through polymer electrolytes to superionic rubbers: some fundamental considerations. Polym. Int. 47, 9–15 (1998).

3.0.CO;2-1" data-track-action="article reference" href="https://doi.org/10.1002%2F%28SICI%291097-0126%28199809%2947%3A1%3C9%3A%3AAID-PI69%3E3.0.CO%3B2-1" aria-label="Article reference 71" data-doi="10.1002/(SICI)1097-0126(199809)47:13.0.CO;2-1">Article CAS Google Scholar

Kimura, K., Motomatsu, J. & Tominaga, Y. Correlation between solvation structure and ion-conductive behavior of concentrated poly(ethylene carbonate)-based electrolytes. J. Phys. Chem. C 120, 12385–12391 (2016).

Article CAS Google Scholar

Mackanic, D. G. et al. Crosslinked poly(tetrahydrofuran) as a loosely coordinating polymer electrolyte. Adv. Energy Mater. 8, 1800703 (2018).

Article Google Scholar

Hernández, G., TianKhoon, L., Erdelyi, M., Brandell, D. & Mindemark, J. Do non-coordinating polymers function as host materials for solid polymer electrolytes? The case of PVdF-HFP. J. Mater. Chem. A 11, 15329–15335 (2023).

Angell, C. A., Liu, C. & Sanchez, E. Rubbery solid electrolytes with dominant cationic transport and high ambient conductivity. Nature 362, 137–139 (1993). This work desmontreates the feasibility of decoupling ion transport from polymer dynamics in polymer electrolytes.

Article ADS CAS Google Scholar

de Gennes, P. G. Reptation of a polymer chain in the presence of fixed obstacles. J. Chem. Phys. 55, 572–579 (1971).

Article ADS Google Scholar

Forsyth, M., Sun, J., Macfarlane, D. R. & Hill, A. J. Compositional dependence of free volume in PAN/LiCF3SO3 polymer-in-salt electrolytes and the effect on ionic conductivity. J. Polym. Sci. B Polym. Phys. 38, 341–350 (2000).

3.0.CO;2-S" data-track-action="article reference" href="https://doi.org/10.1002%2F%28SICI%291099-0488%2820000115%2938%3A2%3C341%3A%3AAID-POLB6%3E3.0.CO%3B2-S" aria-label="Article reference 77" data-doi="10.1002/(SICI)1099-0488(20000115)38:23.0.CO;2-S">Article ADS CAS Google Scholar

Bailey, E. J. & Winey, K. I. Dynamics of polymer segments, polymer chains, and nanoparticles in polymer nanocomposite melts: a review. Prog. Polym. Sci. 105, 101242 (2020).

Article CAS Google Scholar

Forsyth, M., Sun, J. Z. & MacFarlane, D. R. Novel polymer-in-salt electrolytes based on polyacrylonitrile (PAN)-lithium triflate salt mixtures. Solid State Ionics 112, 161–163 (1998).

CAS Google Scholar

Wu, B. et al. Performance of “polymer-in-salt” electrolyte PAN-LiTFSI enhanced by graphene oxide filler. J. Electrochem. Soc. 163, A2248–A2252 (2016).

Article CAS Google Scholar

Gao, H., Grundish, N. S., Zhao, Y., Zhou, A. & Goodenough, J. B. Formation of stable interphase of polymer-in-salt electrolyte in all-solid-state lithium batteries. Energy Mater. Adv. 2021, 1932952 (2021).

Article ADS Google Scholar

Wu, H. et al. A polymer-in-salt electrolyte with enhanced oxidative stability for lithium metal polymer batteries. ACS Appl. Mater. Interfaces 13, 31583–31593 (2021).

Article CAS PubMed Google Scholar

Sun, M. et al. In situ prepared “polymer-in-salt” electrolytes enabling high-voltage lithium metal batteries. J. Mater. Chem. A 10, 11732–11741 (2022).

Article CAS Google Scholar

Angell, C. A. Concepts and conflicts in polymer electrolytes: the search for ion mobility. Electrochim. Acta 313, 205–210 (2019). This review summarizes the attempts related to the development of truely decoupled polymer electrolytes, and outlines the possible directions in this domain.

Article Google Scholar

Guzmán‐González, G. et al. Lithium borate ionic liquids as single-component electrolytes for batteries. Adv. Energy Mater. 13, 2202974 (2023).

Article Google Scholar

Li, M., Wang, C., Chen, Z., Xu, K. & Lu, J. New concepts in electrolytes. Chem. Rev. 120, 6783–6819 (2020).

Article CAS PubMed Google Scholar

Xu, K., Xu, W. & Zhang, S. Austen Angell’s legacy in electrolyte research. J. Non Cryst. Solids X 14, 100088 (2022).

Angell, C. A., Ansari, Y. & Zhao, Z. Ionic liquids: past, present and future. Faraday Discuss. 154, 9–27 (2012).

Article ADS PubMed Google Scholar

Agapov, A. L. & Sokolov, A. P. Decoupling ionic conductivity from structural relaxation: a way to solid polymer electrolytes? Macromolecules 44, 4410–4414 (2011).

Article ADS CAS Google Scholar

Angell, C. A. Relaxation in liquids, polymers and plastic crystals—strong/fragile patterns and problems. J. Non Cryst. Solids 131-133, 13–31 (1991).

Article ADS CAS Google Scholar

Sokolov, A. P. & Schweizer, K. S. Resolving the mystery of the chain friction mechanism in polymer liquids. Phys. Rev. Lett. 102, 248301 (2009).

Article ADS PubMed Google Scholar

Sun, X. & Angell, C. A. “Acid-in-chain” versus “base-in-chain” anionic polymer electrolytes for electrochemical devices. Electrochim. Acta 46, 1467–1473 (2001).

Article CAS Google Scholar

Zhang, H. et al. Enhanced lithium-ion conductivity of polymer electrolytes by selective introduction of hydrogen into the anion. Angew. Chem. Int. Ed. 58, 7829–7834 (2019).

Article CAS Google Scholar

Wang, X. et al. Poly(ionic liquid)s-in-salt electrolytes with co-coordination-assisted lithium-ion transport for safe batteries. Joule 3, 2687–2702 (2019).

Article CAS Google Scholar

Chen, F., Wang, X., Armand, M. & Forsyth, M. Cationic polymer-in-salt electrolytes for fast metal ion conduction and solid-state battery applications. Nat. Mater. 21, 1175–1182 (2022).

Article ADS CAS PubMed Google Scholar

Angell, C. A. Mobile ions in amorphous solids. Annu. Rev. Phys. Chem. 43, 693–717 (1992).

Article ADS CAS Google Scholar

Han, H. et al. Lithium bis(fluorosulfonyl)imide (LiFSI) as conducting salt for nonaqueous liquid electrolytes for lithium-ion batteries: physicochemical and electrochemical properties. J. Power Sources 196, 3623–3632 (2011).

Article ADS CAS Google Scholar

Eichinger, G. & Besenhard, J. O. High energy density lithium cells. J Electroanal. Chem. Interfacial Electrochem. 72, 1–31 (1976).

Article CAS Google Scholar

Bonino, F., Ottaviani, M., Scrosati, B. & Pistoia, G. Electrode kinetics in poly(ethylene oxide)-based electrolytes. J. Power Sources 20, 333–338 (1987).

Article ADS CAS Google Scholar

Hovington, P. et al. New lithium metal polymer solid state battery for an ultrahigh energy: nano C-LiFePO4 versus nano Li1.2V3O8. Nano Lett. 15, 2671–2678 (2015).

Article ADS CAS PubMed Google Scholar

Yang, B., He, J., Zhang, G. & Guo, J. in Vanadium: Extraction, Manufacturing and Applications (eds Jones, G.) 33–58 (Metallurgical Industry Press, 2021).

Padhi, A. K., Nanjundaswamy, K. S. & Goodenough, J. B. Phospho-olivines as positive-electrode materials for rechargeable lithium batteries. J. Electrochem. Soc. 144, 1188–1194 (1997).

Article ADS CAS Google Scholar

Shi, S. et al. Enhancement of electronic conductivity of LiFePO4 by Cr doping and its identification by first-principles calculations. Phys. Rev. B 68, 195108 (2003).

Article ADS Google Scholar

Tukamoto, H. & West, A. R. Electronic conductivity of LiCoO2 and Its enhancement by magnesium doping. J. Electrochem. Soc. 144, 3164–3168 (1997).

Article ADS CAS Google Scholar

Armand, M. et al. Electrode materials having high surface conductivity, CA patent 2270771A1 (2000). This patent discloses the significant improvement of redox kinetic for the LiFePO4 electrode via carbon coating technology.

Delacourt, C., Poizot, P., Levasseur, S. & Masquelier, C. Size effects on carbon-free LiFePO4 powders. Electrochem. Solid-State Lett 9, A352 (2006).

Article CAS Google Scholar

Gaberscek, M., Dominko, R. & Jamnik, J. Is small particle size more important than carbon coating? An example study on LiFePO4 cathodes. Electrochem. Commun. 9, 2778–2783 (2007).

Article CAS Google Scholar

Cabañero Martínez, M. A. et al. Are polymer–based electrolytes ready for high–voltage lithium battery applications? An overview of degradation mechanisms and battery performance. Adv. Energy Mater. 12, 2201264 (2022).

Article Google Scholar

Wan, J. et al. Ultrathin, flexible, solid polymer composite electrolyte enabled with aligned nanoporous host for lithium batteries. Nat. Nanotechnol. 14, 705–711 (2019).

Article ADS CAS PubMed Google Scholar

Zhao, Q., Liu, X., Stalin, S., Khan, K. & Archer, L. A. Solid-state polymer electrolytes with in-built fast interfacial transport for secondary lithium batteries. Nat. Energy 4, 365–373 (2019).

Article ADS CAS Google Scholar

Cao, X., Jia, H., Xu, W. & Zhang, J. Review—Localized high-concentration electrolytes for lithium batteries. J. Electrochem. Soc. 168, 010522 (2021).

Article ADS CAS Google Scholar

Hu, J. et al. Dual fluorination of polymer electrolyte and conversion-type cathode for high-capacity all-solid-state lithium metal batteries. Nat. Commun. 13, 7914 (2022).

Article ADS CAS PubMed PubMed Central Google Scholar

Zhou, W. et al. Double-layer polymer electrolyte for high-voltage all-solid-state rechargeable batteries. Adv. Mater. 31, e1805574 (2019).

Article PubMed Google Scholar

Arrese-Igor, M. et al. Toward high-voltage solid-state li-metal batteries with double-layer polymer electrolytes. ACS Energy Lett 7, 1473–1480 (2022).

Article CAS Google Scholar

Zhang, H., Feng, W., Nie, J. & Zhou, Z. Recent progresses on electrolytes of fluorosulfonimide anions for improving the performances of rechargeable Li and Li-ion battery. J. Fluor. Chem. 174, 49–61 (2015).

Article CAS Google Scholar

Zhang, H. et al. Lithium salt with a super-delocalized perfluorinated sulfonimide anion as conducting salt for lithium-ion cells: physicochemical and electrochemical properties. J. Power Sources 296, 142–149 (2015).

Article ADS CAS Google Scholar

Bresser, D., Lyonnard, S., Iojoiu, C., Picard, L. & Passerini, S. Decoupling segmental relaxation and ionic conductivity for lithium-ion polymer electrolytes. Mol. Syst. Des. Eng. 4, 779–792 (2019).

Article CAS Google Scholar

Jones, S. D. et al. Design of polymeric zwitterionic solid electrolytes with superionic lithium transport. ACS Cent. Sci. 8, 169–175 (2022).

Article CAS PubMed PubMed Central Google Scholar

Chen, C. et al. Interface aspects in all‐solid‐state Li‐based batteries reviewed. Adv. Energy Mater. 11, 2003939 (2021).

Article CAS Google Scholar

Jain, A. et al. Commentary: The Materials Project: a materials genome approach to accelerating materials innovation. APL Mater 1, 011002 (2013).

Article ADS Google Scholar

Momma, K. & Izumi, F. VESTA3 for three-dimensional visualization of crystal, volumetric and morphology data. J. Appl. Crystallogr. 44, 1272–1276 (2011).

Article CAS Google Scholar

Ding, M. S. & Jow, T. R. Conductivity and viscosity of PC-DEC and PC-EC solutions of LiPF6. J. Electrochem. Soc. 150, A620 (2003).

Article CAS Google Scholar

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This work is supported by the Fundamental Research Funds for the Central Universities, HUST (No. 2020kfyXJJS095), and the National Natural Science Foundation of China (Nos. 52203223 and 22279037). F.C. and M.F. acknowledge the Australian Research Council for funding support through the discovery project (DP210101172) and ARC Training Centre in Future Energy Storage Technologies (StorEnergy).

Key Laboratory of Material Chemistry for Energy Conversion and Storage (Ministry of Education), School of Chemistry and Chemical Engineering, Huazhong University of Science and Technology, Luoyu Road 1037, 430074, Wuhan, China

Ziyu Song, Wenfang Feng, Zhibin Zhou & Heng Zhang

Institute for Frontier Materials, Deakin University, Burwood, VIC, 3125, Australia

Fangfang Chen & Maria Forsyth

Centre for Cooperative Research on Alternative Energies (CIC energiGUNE), Basque Research and Technology Alliance (BRTA), 01510, Vitoria-Gasteiz, Spain

Maria Martinez-Ibañez & Michel Armand

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H.Z. and M.A. conceived the work. H.Z., W.F., and F.C. organized the content and prepared the draft manuscript. H.Z. and Z.S. designed and created all original and self-created figures. H.Z., F.C., Z.Z., and M.A. supervised the work. M.F. and F.C. carefully revised the manuscript, particularly the section related to “decoupled” polymer electrolytes. All authors contributed to the writing and revision of the manuscript.

Correspondence to Fangfang Chen, Zhibin Zhou, Michel Armand or Heng Zhang.

The authors declare no competing interests.

Nature Communications thanks Guinevere Giffin and the other, anonymous, reviewer(s) for their contribution to the peer review of this work.

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Song, Z., Chen, F., Martinez-Ibañez, M. et al. A reflection on polymer electrolytes for solid-state lithium metal batteries. Nat Commun 14, 4884 (2023). https://doi.org/10.1038/s41467-023-40609-y

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Received: 30 October 2022

Accepted: 02 August 2023

Published: 12 August 2023

DOI: https://doi.org/10.1038/s41467-023-40609-y

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