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# Copper-coordinated cellulose ion conductors for solid-state batteries

## Abstract

Although solid-state lithium (Li)-metal batteries promise both high energy density and safety, existing solid ion conductors fail to satisfy the rigorous requirements of battery operations. Inorganic ion conductors allow fast ion transport, but their rigid and brittle nature prevents good interfacial contact with electrodes. Conversely, polymer ion conductors that are Li-metal-stable usually provide better interfacial compatibility and mechanical tolerance, but typically suffer from inferior ionic conductivity owing to the coupling of the ion transport with the motion of the polymer chains1,2,3. Here we report a general strategy for achieving high-performance solid polymer ion conductors by engineering of molecular channels. Through the coordination of copper ions (Cu2+) with one-dimensional cellulose nanofibrils, we show that the opening of molecular channels within the normally ion-insulating cellulose enables rapid transport of Li+ ions along the polymer chains. In addition to high Li+ conductivity (1.5 × 10−3 siemens per centimetre at room temperature along the molecular chain direction), the Cu2+-coordinated cellulose ion conductor also exhibits a high transference number (0.78, compared with 0.2–0.5 in other polymers2) and a wide window of electrochemical stability (0–4.5 volts) that can accommodate both the Li-metal anode and high-voltage cathodes. This one-dimensional ion conductor also allows ion percolation in thick LiFePO4 solid-state cathodes for application in batteries with a high energy density. Furthermore, we have verified the universality of this molecular-channel engineering approach with other polymers and cations, achieving similarly high conductivities, with implications that could go beyond safe, high-performance solid-state batteries.

## Main

Solid-state batteries with lithium-metal anodes are attractive as next-generation energy-storage systems with high energy density and safety. The realization of such batteries will depend largely on the development of superior ion conductors for the solid-state electrolyte and of an ion-conducting network for the cathode materials. Solid polymer electrolytes (SPEs)—typically ether-based, such as poly(ethylene oxide) (PEO)3,4—are promising candidates, owing to their low density, ability to dissociate Li salts at elevated temperatures, facile processibility, and good interfacial contact with the electrodes5,6,7. However, Li+ transport in SPEs is highly coupled with the segmental motion of the polymer chains, resulting in limited ionic conductivities (generally less than 10−5 S cm−1 at room temperature2) and low Li+-transference numbers (usually 0.2–0.5)8,9.

To improve the conductivity of Li+ ions, SPEs are commonly used at elevated temperatures in order to promote the segmental motion of the polymer for faster ion movement. However, increasing the temperature deteriorates the mechanical strength of the SPE and compromises the safety of the battery. Other efforts to improve the Li+ conductivity, transference number and/or mechanical properties of SPEs include modifying the polymer matrix structure with crosslinked polymers10,11,12, block copolymers13 and single-ion-conducting polymers14, or incorporating inorganic fillers4,15,16. Despite these approaches, the tradeoff between the ion conduction, transference number and mechanical strength in SPEs has persisted for more than four decades, and the room-temperature ionic conductivity of SPEs barely approaches 10−4 S cm−1. Additionally, SPEs feature poor ionic percolation when used as ion-conducting additives in cathode materials, requiring a threshold content of roughly 25 wt% SPE17,18, which further reduces the energy density of the battery. Clearly, the conventional SPE structure and Li+-transport mechanism must be drastically transformed to meet future energy-storage needs.

Here, we explore a design strategy for polymer ion conductors that is based on expanding the intermolecular polymer structure and decoupling the Li+ transport from the polymer segmental relaxation, which leads to high ionic conductivity. We first demonstrate this approach using cellulose nanofibrils (CNFs, either as individual building blocks or as an integral component in the format of paper or delignified wood). CNFs are abundantly available from various biomass sources (for example, wood) and feature an aligned, one-dimensional (1D) hierarchical structure rich in oxygen-containing polar functional groups (for example, hydroxyl) in the form of repeating anhydroglucose units (AGUs) that make up the cellulose molecular chains (Fig. 1a). Such polar functionalities could solvate Li+ and aid in Li+ movement. However, the narrow spacing between the cellulose molecular chains does not naturally allow Li+ incorporation. As a result, CNFs have been used previously only as an inert supporting matrix for liquid/gel electrolytes (not a solid-state ion conductor) or other SPEs (with poor ionic conductivities)19,20,21. We show here that the coordination of copper ions (Cu2+) with CNFs (producing Cu–CNF) allows us to alter the crystalline structure of the cellulose by expanding the spacing between the polymer chains into molecular channels that enable the insertion and rapid transport of Li+ ions (Fig. 1a). In such 1D conduction passages, the abundant oxygen-containing functional groups of cellulose, along with a small amount of bound water, assist in the movement of Li+ in a manner that is decoupled from the segmental motion of the polymer.

As a result, the Li+-inserted Cu–CNF (Li–Cu–CNF) ion conductor features a high ionic conductivity of 1.5 × 10−3 S cm−1 (10–1000 times that of other Li-stable SPEs) and a high transference number of 0.78 at room temperature (Fig. 1b). Li–Cu–CNF also features a wide electrochemical stability window of 0–4.5 V (potentials in this work are all versus Li+/Li), in addition to low cost, scalability and flexibility (Fig. 1c). Besides serving as a thin and dense solid-state separator/electrolyte, the 1D structure of Li–Cu–CNF also makes it an effective ion-conducting binder for thick solid-state electrodes in which low ionic conductivity has been a key hurdle. Indeed, the effective ionic percolation of Li–Cu–CNF has allowed us to fabricate a thick LiFePO4 solid-state cathode (roughly 120 μm), suggesting the material’s potential for increasing battery energy density. This design principle—using facile coordination chemistry and expansion of the polymer molecular channels to provide fast diffusion pathways for uncoupled Li+ transport—can be applied to other polymers and cations, enabling high-performance solid-state ion conductors that may have applications far beyond high-energy-density and safe solid-state batteries.

## Synthesis and structure analysis

We fabricated the solid-state Li–Cu–CNF ion conductor using a simple ion-coordination and solvent-exchange process (Fig. 2a). We first immersed the CNF-containing materials (for example, CNF suspensions, cellulose paper, or aligned CNFs derived from wood, as specified in the Methods) in Cu2+-saturated alkaline solution (20% NaOH), in which Cu2+ gradually coordinates with the cellulose molecular chains, forming a blue-coloured Cu–CNF–NaOH complex filled with NaOH solution. After washing the NaOH from Cu–CNF–NaOH with water, displacing the water with dimethylformamide (DMF), and finally evaporating the DMF under vacuum, we obtained the solid-state Cu–CNF material. Li+ was then inserted into the Cu–CNF by soaking in an electrolyte consisting of LiPF6 in non-aqueous solvents, followed by evaporation of the solvents, producing the Li–Cu–CNF ion conductor (Fig. 2a and Supplementary Discussion 1 in the Supplementary Information).

We applied fibre X-ray diffraction (XRD; Fig. 2b–e and Extended Data Fig. 1a–d) and X-ray absorption spectroscopy (XAS; Extended Data Fig. 1e–h) to track the structural evolution during the fabrication process. We also constructed model structures of the materials through molecular dynamics (MD) simulations (Fig. 2f–i; for details, see Methods and Extended Data Fig. 2), using the fibre XRD results. The pristine CNFs feature a typical monoclinic diffraction pattern of cellulose Iβ, with diffraction peaks at (110), (200) and so on (Fig. 2b), showing a cellulose molecular spacing (d200) of 0.39 nm22. The corresponding MD simulation of the crystalline CNF (Fig. 2f) suggests that the material cannot accommodate the insertion of Li+ between the intermolecular spacing owing to the close packing of the cellulose chains. By contrast, the Cu–CNF–NaOH features a hexagonal crystal structure, with threefold symmetry along the direction of the cellulose chains (Fig. 2c)23. In the simulated structure of the Cu–CNF–NaOH (Fig. 2g), each cellulose chain has three neighbouring chains, with an interchain distance of 0.87 nm, which are bridged by Cu2+ via four coordinated Cu–O bonds, opening the close molecular packing of the CNFs. After removing NaOH and liquid water, the crystalline Cu–CNF–NaOH becomes amorphous Cu–CNF (Fig. 2d). This amorphous structure has a much lower density of cellulose packing (4.7 AGU nm−3; Fig. 2h) than do the pristine CNFs (6.1 AGU nm−3; Fig. 2f), with molecular channels opened between the cellulose chains. The final Li–Cu–CNF structure after Li+ is inserted into these channels maintains the amorphous state (Fig. 2e) with a low packing density (4.4 AGU nm−3; Fig. 2i). XAS (Extended Data Fig. 1e–h) further confirms that the Cu2+ ions are bonded with O atoms in the amorphous Cu–CNF and Li–Cu–CNF materials, with an average bonding distance of 1.97 Å. As a result of the coordination of Cu2+, the amorphous Li–Cu–CNF has expanded molecular channels that can accommodate Li+.

## Li+ conduction in Li–Cu–CNF

The Li–Cu–CNF material contains a small amount of bound water but still displays excellent electrochemical stability. 1H magic-angle spinning (MAS) nuclear magnetic resonance (NMR; Extended Data Fig. 3a, b) shows that the final Li–Cu–CNF product contains roughly 1.9 wt% of H2O (lower than the 4–6 wt% typically found in regular paper24). This small amount of water in Li–Cu–CNF does not aggregate as a condensed liquid phase, but instead exists as discrete H2O molecules bound to the cellulose through hydrogen bonding, as shown by Fourier-transform infrared spectra (FTIR), quasi-elastic neutron scattering (QENS) and differential scanning calorimetry (DSC), as well as model simulations (Extended Data Fig. 3c–h). The low content of bound water in Li–Cu–CNF does not compromise the material’s solid nature, but is essential for its flexibility (Fig. 1c) and high mechanical strength (29.2 MPa; Extended Data Fig. 3i). More importantly, Li–Cu–CNF containing bound water still has a wide electrochemical stability window of 0–4.5 V (Fig. 3a and Extended Data Fig. 4), which allows for the reversible operation of the Li-metal anode and high-voltage cathodes (for example, LiNi0.8Mn0.1Co0.1O2 (NMC811)) needed for high-energy-density solid-state batteries. This is substantially different from electrolytes that contain free liquid water25, where the water molecules exist as bulk liquid and hence are reactive with Li metal.

The Li–Cu–CNF material serves as an excellent Li+ conductor. At 25 °C, Li–Cu–CNF has a high Li+ conductivity of 1.5 × 10−3 S cm−1 along the direction of the cellulose molecular chains (that is, in the fibre direction; Extended Data Fig. 5a–d), which is higher by orders of magnitude than that of other reported SPEs (Fig. 3b)3,4,10,11,13,14,17,26. The conductivity–temperature relationship of Li–Cu–CNF (along the fibre direction) follows an Arrhenius-type behaviour (that is, logarithmic conductivity linear to 1/T). According to the Arrhenius equation, the activation energy is 0.19 eV, which is much lower than that of PEO (roughly 1 eV)3 and PEO–inorganic composite electrolytes (roughly 0.6 eV)4. Additionally, a Li–Cu–CNF paper electrolyte consisting of three-dimensionally, randomly distributed Li–Cu–CNF shows a through-plane ionic conductivity of 3.4 × 10−4 S cm−1 at room temperature—still much higher than that of all reported Li-stable SPEs (Fig. 3b)3,4,10,11,13,14,17,26. The through-plane conductivity–temperature relationship also follows the Arrhenius equation, without a transition point even at temperatures below 0 °C (Fig. 3b and Extended Data Fig. 5e–g). Li–Cu–CNF offers a similar ionic conductivity to oxide-based electrolytes (for example, Li7La3Zr2O12 (LLZO)) but at a much lower Li concentration (1.2 mol l−1 versus 41.3 mol l−1 in LLZO27; Fig. 3c), which is preferential for lower cost. The Li concentration is similar to that of PEO (roughly 1.1 mol l−1)27, but Li–Cu–CNF features a roughly 500 times higher Li+ diffusion coefficient at room temperature (DLi = 6.1 × 10−7 cm2 s−1, by 7Li pulsed field gradient (PFG) NMR; Supplementary Discussion 2).

The Cu2+ in Li–Cu–CNF is not mobile, as indicated by a negligible Cu2+ conductivity of 1.0 × 10−8 S cm−1 (Extended Data Fig. 5h), but it does have an indispensable role in opening the cellulose molecular channels to allow transport of Li+ in Li–Cu–CNF. Without Cu2+ coordination, the control sample Li–CNF (synthesized similarly to Li–Cu–CNF but in the absence of Cu2+) has closely packed cellulose chains that spatially prevent Li+ from accessing the interior of the nanofibrils (Extended Data Fig. 5n) and thus displays a much lower Li+ conductivity (Fig. 3b). In addition, Li–Cu–CNF shows a high Li+-transference number of 0.78 (Extended Data Fig. 5i, j), which is much higher than that of Li–CNF (0.35; Extended Data Fig. 5k–m) and other SPEs (0.2–0.5; Fig. 1b), except single-Li-ion conducting polymers13,14 (which feature a transference number of close to 1.0, although this is often achieved at the impractical expense of the overall ionic conductivity).

In the Li–Cu–CNF molecular channels, the Li+ can form multiple coordinations with the rich oxygen-containing functional groups (shown schematically in Fig. 3d), including hydroxyl (ROH), carboxylate (COO), alkoxide (RO), and ether (EO) moieties, in addition to bound H2O molecules and some residual PF6. Given the Li+ content (1.3 wt%) in Li–Cu–CNF measured by inductively coupled plasma (ICP) analysis, the number of oxygen atoms is roughly 20 times that of Li+. Solid-state 6Li NMR (Extended Data Fig. 6a–d) shows that the number of Li+ ions that are coordinated with oxygen atoms (RO···Li, COO···Li, and ROH/H2O···Li) in the Li–Cu–CNF material is substantially larger than that in Li-CNF. MD simulations also reveal that the Li–O coordination number in Li–Cu–CNF (4.2), due to Li+ insertion, is much larger than that in Li–CNF (3.0), due to surface adsorption (Fig. 3e). The multiple Li–O coordination is important for the diffusion of Li+. When Li+ moves, it can dissociate from just one to two bonded oxygen atoms while still coordinating with the others, resulting in a low hopping energy barrier28.

To investigate the Li+-transport pathways, we performed 6Li tracer-exchange NMR (Extended Data Fig. 6e–g)29. After 7Li in Li–Cu–CNF was exchanged with 6Li tracer by electrochemical cycling, the number of 6Li+ ions coordinated with COO, RO, ROH/H2O and PF6 in Li–Cu–CNF increased by 15, 20, 25 and 4.5 times, respectively, compared with Li–Cu–CNF before cycling (Fig. 3f and Extended Data Fig. 6g). Thus, the hopping sites of Li+ are mainly the counter-anions in the cellulose (COO and RO).

MD simulations further show that the Li+ in Li–Cu–CNF hops between the COO and RO sites instead of moving within a solvation sheath formed by the polymer chain segment (Extended Data Fig. 7a), with the assistance of H2O molecules (Extended Data Fig. 7b, c). The rich oxygen groups in Li–Cu–CNF (COO, RO, ROH, and EO) form a continuous Li+-hopping pathway, with a short hopping distance (roughly 3.0 Å; Extended Data Fig. 7d) close to that of fast inorganic ion conductors30, enabling high-mobility Li+ hopping. The counter-anions in the cellulose (COO and RO) move much less than Li+ (Extended Data Fig. 7e), while the only mobile counter-anion is the residual PF6, resulting in the high transference number of Li–Cu–CNF (0.78; see Supplementary Discussion 2 for more analysis). Figure 3g shows a simulated fast-moving Li+ ion travelling along or between the cellulose molecular chains, while the cellulose backbone moves very little, indicating that the Li+ hopping is decoupled from the motion of the polymer chain. This decoupled Li+-hopping mechanism—which is enabled jointly by the open molecular channels, multiple Li–O coordination and assistance of bound water molecules—contributes to the unprecedentedly high ionic conductivity and transference number of Li–Cu–CNF.

## Use of Li–Cu–CNF in batteries

The 1D, nanoscale Li–Cu–CNF ion conductor can be applied as both an independent solid-state electrolyte and an effective ion-conducting binder for constructing continuous Li+-transport networks in solid-state cathodes (Fig. 4a), both of which are crucial for building high-performance solid-state Li-metal batteries. We first show that Li–Cu–CNF can be assembled and pressed into a thin (roughly 50 μm) yet dense paper with three-dimensionally, randomly distributed fibrils (Fig. 4b and Extended Data Fig. 8a, b) as a solid-state electrolyte. The Li–Cu–CNF electrolyte enables stable Li-cycling performance at 0.5 mA cm−2 for 300 h in a Li-metal symmetric cell without dendrite-induced short-circuiting or Cu2+ reduction on Li (Extended Data Fig. 8c–e), indicating the compatibility of Li–Cu–CNF with a Li-metal anode.

We also applied individual Li–Cu–CNF fibrils as an effective ion-conducting binder for thick battery electrodes in order to overcome interfacial ion-transport challenges. As an ion-conducting binder, Li–Cu–CNF has the advantage of the high aspect ratio (roughly 200) of the CNFs, which should enable a low percolation threshold31. We selected LiFePO4 to demonstrate that the incorporation of 1D Li–Cu–CNF additive forms an ion-percolation network within the solid-state cathode (Fig. 4c). The resulting cathode featured a percolation threshold of 15 vol% to form an ion-conducting network (Fig. 4d), which corresponds to roughly 5 wt% of the Li–Cu–CNF additive in the composite (Supplementary Discussion 3). Moreover, the use of the Li–Cu–CNF ion-conducting binder is compatible with the traditional slurry-casting method for electrode preparation (Fig. 4e and Extended Data Fig. 9a), which allows large-scale, roll-to-roll manufacturing of solid-state batteries.

We further show the effective Li+ transport enabled by Li–Cu–CNF in a full battery featuring both the Li–Cu–CNF paper electrolyte and a thick (120 μm) solid-state LiFePO4 cathode containing the Li–Cu–CNF additive. The solid-state LiFePO4 cathode (Fig. 4f) demonstrated here is three to five times thicker than other reported solid-state LiFePO4 cathodes11,17,18,32. With the Li–Cu–CNF ion-conducting binder, this thick LiFePO4 cathode showed much smaller impedance (Extended Data Fig. 9b, c), reduced overpotential and higher capacity (Fig. 4g) compared with the cathode without the Li–Cu–CNF binder. The solid-state LiFePO4 battery with Li–Cu–CNF also showed good cycling performance with a capacity retention of 94% after 200 cycles at room temperature (Fig. 4h), which cannot be achieved with a PEO electrolyte (Supplementary Discussion 4). The disassembled cells after cycling showed that Li–Cu–CNF is stable against the Li metal and cathode, without Cu2+ reduction on the Li-metal anode (Supplementary Discussion 5, 6). The flexibility of the Li–Cu–CNF electrolyte also allowed us to fabricate a flexible solid-state battery that remained operational when folded (Fig. 4h, inset, and Extended Data Fig. 9d).

The stability of Li–Cu–CNF against the Li-metal anode and high-voltage cathode materials enables its use in high-energy-density solid-state batteries. As a proof-of-concept, we successfully demonstrated long-term cycling of solid-state batteries constructed using a Li-metal anode, Li–Cu–CNF electrolyte, and NMC811 or LiMn2O4 cathodes, without any liquid electrolyte (Extended Data Fig. 10). By contrast, widely studied PEO-based SPEs can barely function with high-voltage cathodes33, showing the substantial advance offered by the room-temperature performance and high-voltage stability of Li–Cu–CNF.

## Conclusions

As a 1D solid-state ion conductor, Li–Cu–CNF demonstrates an exceptionally high ionic conductivity (1.5 × 10−3 S cm−1) and high Li+-transference number (0.78) at room temperature, which is made possible by decoupling the Li+ transport from the local solvation environment. The Li+ transport follows a rapid ion-hopping mechanism via the polar functional groups and bound water molecules available in the cellulose molecular channels that have been opened by Cu2+-coordination chemistry. The Li–Cu–CNF ion conductor, made with a simple and reproducible synthesis procedure, provides exceptional conductivity, electrochemical stability, processibility, transference number and mechanical strength for high-energy-density batteries (Fig. 4i). This 1D ion conductor can also function as an ionic building block for forming solid-state ionic conducting networks, enabling it to be compatible with thick cathodes and thus high-energy-density solid-state batteries. The success of this design strategy creates a class of polymer ion conductors that enable fast conduction by various cations (for example, Na+) with high room-temperature ionic conductivities that have so far been challenging for traditional polymer electrolytes (Supplementary Discussion 8, 9). For example, we investigated this same Cu2+-coordination approach for the synthesis of polymer ion conductors made of chitosan, alginate acid, carboxymethyl cellulose (CMC) and xanthan gum (XG) (Fig. 4j), all of which showed high room-temperature ionic conductivities ($${\sigma }_{{\rm{Li}}}$$ = 3 × 10−4 S cm−1 for Li–Cu–chitosan; $${\sigma }_{{\rm{Na}}}$$ = 2 × 10−4 S cm−1 for Na–Cu–alginate; and $${\sigma }_{{\rm{Zn}}}$$ = 9 × 10−4 S cm−1 for Zn–Cu–XG/CNF). Our strategy provides both material and conceptual breakthroughs for the development of many other high-performance solid-state ion conductors that could have a broad impact beyond just safe solid-state batteries, examples of which could include electrochemical synaptic devices, solid-state sensors, and redox-controlled information processing and storage.

## Methods

### Preparation of CNFs

CNFs were produced by (2,2,6,6-tetramethylpiperidin-1-yl)oxidanyl (TEMPO) oxidation of commercial bleached eucalyptus Kraft pulp (International Paper) and mechanical treatment in a microfluidizer (M-110EH Microfluidizer Processor) as before34. The resulting CNF suspension (roughly 1 wt% solid content) was stored at 4 °C for further treatment. CNF paper was fabricated by vacuum filtration of the CNF suspension. The filtrated CNF paper was placed between sheets of filter paper and pressed at room temperature for 24 h at a pressure of roughly 2 MPa to obtain dense CNF paper. To achieve aligned CNFs, wood slices (cut along the longitudinal direction, that is, the growth direction of the tree) were delignified by immersing and boiling in a NaClO2 solution (5 wt%) with a pH of roughly 4.6 (adjusted by acetic acid) until the wood slices turned completely white (roughly 2 h). The delignified wood slices were then washed with deionized water three times to remove the residual chemicals and then hot-pressed at 60 °C for two days to obtain the aligned CNFs (that is, densified wood, different from the individual CNFs produced by TEMPO oxidation).

### Preparation of Cu2+-saturated alkaline solution

The Cu2+-saturated alkaline solution was made by immersing excess copper wire in NaOH solution (20 wt%), for example, 5 g of copper wire in 500 ml of NaOH solution. The solution was magnetically stirred until the NaOH solution turned blue after two to three days. Before use, this stock solution was stored with excess immersed copper wire. According to ICP analysis, the concentration of Cu2+ in the Cu2+-saturated NaOH solution was 2.8 wt%.

### Preparation of Li–Cu–CNF

We fabricated Li–Cu–CNF through the following three steps. (1) CNFs (generally referring to any format of cellulose consisting of CNFs, including CNF suspension, cellulose paper or aligned CNFs) were immersed in Cu2+-saturated alkaline solution (20% NaOH) for one to two weeks until the CNFs gradually turned blue (reaching saturated Cu2+ coordination with the CNFs), with the product referred to as Cu–CNF–NaOH. (2) The free water in the Cu–CNF–NaOH was then replaced by DMF solvent exchange, which was then evaporated to produce the Cu–CNF. (3) The Cu–CNF was soaked in a Li-salt solution (1 mol l−1 LiPF6 dissolved in ethylene carbonate/dimethyl carbonate (EC/DMC); 1:1 volumetric ratio) for two days in an argon-filled glovebox, followed by repeatedly pressing and wiping the absorbed liquid and evaporating the solvent in vacuum to obtain the Li–Cu–CNF solid-state ion conductor. For the Li–CNF control sample, the CNFs were treated using the same steps, except that the material was immersed in the NaOH solution without Cu2+ in step 1.

For different uses of Li–Cu–CNF, the materials or synthesis process described above was slightly changed. To obtain Li–Cu–CNF with aligned orientation for measuring the intrinsic conductivity, mechanical strength and fibre XRD along the fibre direction, the aligned CNFs (produced from wood as above) were used as the CNF source in step 1 to produce the aligned Li–Cu–CNF as above. To fabricate the Li–Cu–CNF paper electrolyte, the cellulose paper was used as the CNF source in step 1 and was treated as above.

### Preparation of other M–Cu–polymers

The Li–Cu–CNF system was extended to other M–Cu–polymer systems via slightly modified synthesis methods. Here, aqueous solutions of chitosan, sodium alginate and sodium CMC (all from Sigma Aldrich) were cast-dried and pressed into thin films. The XG (TCI) was mixed with the TEMPO-oxidized CNF material (XG/CNF; mass ratio 1:1) in solution, filtrated, and pressed into a thin film. The polymer films were coordinated with Cu2+ to form Cu–polymer via a similar method in step 1. The Cu–chitosan was further similarly treated via steps 2 and 3 for Li+ insertion. The Cu–CMC was soaked in a Na+-ion electrolyte (3 mol l−1 NaClO4 in DMF) for inserting Na+ and forming Na–Cu–CMC. The Cu–alginate was treated with a Na+-ion electrolyte (4 mol l−1 NaClO4 aqueous solution) to form Na–Cu–alginate for Na+ conduction. The Cu–XG/CNF was treated with a Zn2+ electrolyte (2 mol l−1 ZnSO4 aqueous solution) to form Zn–Cu–XG/CNF for Zn2+ conduction. All samples were dried in vacuum before electrochemical testing.

### Preparation of solid-state cathodes

To prepare the LiFePO4 (BTR New Material Group) cathode mixed with Li–Cu–CNF, the Cu–CNF–NaOH suspension obtained in step 1 was washed and mixed with the cathode material and CNT (Carbon Solutions) (typical mass ratio of LiFePO4:CNT:Cu–CNF = 9:1:1) in water solution using a vortex mixer for 5 min, followed by ultrasonication for 30 s (FS110D, Fisher Scientific). The mixture was then either filtrated as a free-standing thick cathode or cast on aluminium foil with the addition of 9 wt% sodium alginate binder, followed by the same treatment as in steps 2 and 3. To measure the ion-percolation behaviour of Li–Cu–CNF in the cathode, the LiFePO4 cathode was fabricated through the same filtration method using different ratios of Li–Cu–CNF (Li–CNF was used as the ‘zero’ Li–Cu–CNF control) and without CNTs. The solid-state NMC811 and LiMn2O4 cathodes were made by casting the cathode materials with carbon black and poly(vinylidene fluoride) (dissolved in N-methyl-2-pyrrolidone) with a mass ratio of 8:1:1 on aluminium foil, followed by drying at 100 °C.

### Assembly of solid-state batteries

The solid-state batteries were assembled in an argon-filled glovebox. The Li symmetric cells were assembled by sandwiching the Li–Cu–CNF paper electrolyte between two Li metals. The solid-state full cells were made with a Li-metal anode, the Li–Cu–CNF electrolyte, and a cathode (LiFePO4, NMC811 or LiMn2O4 cathodes made as described above). The solid-state flexible cell was assembled using a thin Li-metal anode, Li–Cu–CNF paper electrolyte, and LiFePO4 cathode in a paper pouch.

### Characterization

A Hitachi SU-70 field emission SEM coupled with an energy-dispersive X-ray (EDX) spectroscopy system was used for SEM and elemental analysis. The fibre XRD measurements were conducted on a Xenocs Xeuss SAXS/WAXS system with a Cu Kα (λ = 1.5418 Å) source and Detris Pilatus 300k detector. A home-made sample holder was used to bring samples close to the detector. The content of Li and Cu in Li–Cu–CNF was analysed by dissolving the metal ions in the samples in nitric acid (5%) and measuring the metal concentration using a multi-collector ICP mass spectrometer (Thermo-Finnigan Element 2). FTIR was conducted on a Nexus 670 made by Thermo Electron with a ‘Smart Endurance’ attenuated total reflectance accessory. Stress–strain measurements of Li–Cu–CNF (along the cellulose fibre direction) were carried out using a Tinius Olsen H5KT testing machine.

XAS measurements were carried out at the 8-ID Beamline of the National Synchrotron Light Source II at Brookhaven National Laboratory (BNL). X-ray absorption near-edge spectroscopy (XANES) and extended X-ray absorption fine structure (EXAFS) data were collected at the Cu K-edge in transmission mode. The samples were placed between two Kapton tapes, which allow for high transmissivity for X-ray measurements. The spectra of the standards were obtained from copper foil (provided by BNL), commercial Cu2O powder and CuO powder (Sigma Aldrich). XAS data were analysed using the IFEFFIT package, which included ATHENA and ARTEMIS35.

QENS spectra were measured at the high-flux backscattering spectrometer (HFBS) in elastic scan mode. In this mode, only elastically scattered neutrons are counted, and a drop in the intensity indicates the presence of the motions in the dynamic range accessible by the instrument. The HFBS has an instrument resolution of about 0.8 eV, which is equivalent to about 2 ns. The data are simultaneously collected for angular momentum transfer, Q, in the range 0.25 Å−1 to 1.75 Å−1. In this analysis, the entire Q range was used. All samples were loaded in the standard aluminium sample holders and sealed with indium. All samples were loaded at 296 K and cooled to 4 K at a ramp rate of 0.8 K min−1, followed by heating back to 296 K at the same ramp rate. The measured elastic intensity can be used to calculate the mean square displacement (MSD) of the sample using a classic Gaussian approximation:

$$\frac{I(T)}{I({T}_{{\rm{\min }}})}={\rm{e}}{\rm{x}}{\rm{p}}\left(-\frac{{Q}^{2} < {u}^{2} > }{3}\right)$$
(1)

where I(T) is the elastic intensity measured at temperature T; I(Tmin) is the intensity at the base temperature of 4 K; and <u2> is the MSD.

To measure the content of water and EC, we conducted 1D 1H MAS NMR analysis of Li–Cu–CNF, using a dry Cu–CNF sample as a control (without EC and dried at 30 °C under vacuum for three days to remove water), on a 300 MHz Varian NMR spectrometer with a 1.6-mm double-resonance-probe head (spun at 33 kHz MAS). The 1H chemical shifts were externally referenced to TMS.

7Li and 19F PFG NMR were conducted on a 300 MHz NMR spectrometer on a double-resonance probe equipped with a maximum gradient of 1,200 G cm−1. Double-stimulated echo or spin-echo pulse sequences were used to measure the diffusion coefficients. The signal was accumulated by using a minimum of 64, up to a maximum of 1,536, transients with a 2-s recycling delay. The gradient strength was varied from 2–50 G cm−1 or 2–700 G cm−1 over 16 increments. The diffusion time (Δ) and the diffusion pulse length (δ) were in the range of 50–400 ms and 2–9 ms, respectively. The diffusion coefficients (D) were calculated using the Stejskal–Tanner equation:

$$\frac{I}{{I}_{0}}=\exp \left[-{(G\gamma \delta )}^{2}\left(\varDelta -\frac{\delta }{3}\right)D\right]$$
(2)

in which γ is the gyromagnetic ratio and G is the gradient strength.

For isotope tracing, the tracer exchange (6Li→7Li) was driven by electrochemical cycling using 6Li-enriched metal (95 atom%; Sigma Aldrich) as electrode foils. The Li–Cu–CNF (or Li–CNF as a control) electrolyte was assembled between two 6Li foils to form a symmetric cell (6Li//Li–Cu–CNF//6Li). The cell was galvanically polarized for 50 cycles with a current density of 32 μA cm−2, and the current switched the direction every 30 min. After cycling, the electrolyte was removed from the cell for 6Li NMR measurements. 6Li magic-angle-spinning NMR experiments were performed on a Bruker Avance III-500 spectrometer with a 6Li Larmor frequency of 73.6 MHz. Samples were packed in 2.5-mm rotors and spun at a speed of 25 kHz. We used a single pulse to acquire the 6Li NMR spectra with a 90° pulse length of 2.5 μs and a recycle delay of 10 s. 6Li NMR chemical shifts were referenced to solid LiCl at −1.1 ppm. We fitted the 6Li NMR spectra (Extended Data Fig. 6) using Gaussian–Lorentzian functions29. The fitted peaks were assigned to different chemical environments of Li+ on the basis of experiments (reference NMR spectra in Extended Data Fig. 6c, d) or literature references36,37. The peak areal integrals were normalized on the basis of the mass of the samples and the number of signal averages.

### Electrochemical tests

Electrochemical tests (electrochemical impedance spectroscopy (EIS), d.c. polarization and LSV) were done on a Biologic electrochemical working station. EIS spectra were measured in a frequency range of 1 MHz to 1 Hz with a voltage amplitude of 20 mV. We used two Li//Li–Cu–CNF//SS cells to conduct separate cathodic (from OCV to 5.4 V) and anodic (from OCV to 0 V) scans at 0.1 mV s−1 to measure the electrochemical stability window of Li–Cu–CNF. Electrochemical stripping/plating for Li symmetric cells and galvanostatic cycling tests for solid-state full cells were conducted on a LAND electrochemical testing system with galvanostatic conditions.

For ionic conductivity tests, we first confirmed the Li+ transport along the fibre direction of the Li–Cu–CNF ion conductor through the galvanostatic Li plating/stripping cycling (Extended Data Fig. 5a) between two ends of the aligned Li–Cu–CNF (length 1 cm) at room temperature. To distinguish the resistances of the electrolyte and Li–electrolyte interface, we measured the EIS of the same aligned Li–Cu–CNF at different lengths (Extended Data Fig. 5b). The EIS spectra of the Li–Cu–CNF ion conductor show two semi-circles, which are attributed to the electrolyte and interface resistance. The semi-circle at the high-frequency region increases linearly as we increase the electrolyte length from 1 cm to 3 cm (Extended Data Fig. 5c). Thus, the high-frequency semi-circle is attributed to the resistance of the Li–Cu–CNF electrolyte. The calculated Li+ conductivity of Li–Cu–CNF at different temperatures (Extended Data Fig. 5d) is plotted in Fig. 3b, following an Arrhenius-type relationship.

We then tested the EIS of a Li–Cu–CNF paper electrolyte made up of randomly oriented fibres (sandwiched between two stainless-steel spacers) at different temperatures (60 °C to −20 °C; Extended Data Fig. 5e, f) to obtain the temperature-dependent through-plane ionic conductivity of the Li–Cu–CNF paper electrolyte (Extended Data Fig. 5g). The Li–Cu–CNF electrolyte shows a through-plane ionic conductivity of 3.4 × 10−4 S cm−1 at room temperature and an Arrhenius-type temperature-dependent ionic conductivity (60 °C to −20 °C) without an abrupt conductivity drop below 0 °C. We attribute this lack of transition to the H2O molecules in the material being bound rather than free, and therefore lacking a freezing point38.

We used d.c. polarization (Extended Data Fig. 5h) to measure the Cu2+ diffusion using a Cu//Cu–CNF//Cu cell, which allows only Cu2+ transport without Li+ conduction. Therefore, the Cu2+ in Li–Cu–CNF is considered immobile and the ionic conductivity of Li–Cu–CNF is contributed by the material’s Li+ rather than Cu2+.

We measured the Li+-transference numbers (tLi) in Li–Cu–CNF and Li–CNF (without Cu coordination) using the Bruce–Vincent method39. d.c. polarization measurements were conducted with a potential of ∆V = 10 mV in the Li//Li–Cu–CNF//Li and Li//Li–CNF//Li cells until the current reached a steady state, and corresponding EIS measurements were collected before and after the d.c. polarization (Extended Data Fig. 5i–l). tLi was calculated according to:

$${t}_{{\rm{Li}}}=\frac{{I}_{{\rm{ss}}}(\Delta V-{I}_{0}{R}_{0})}{{I}_{0}(\Delta V-{I}_{{\rm{ss}}}{R}_{{\rm{ss}}})}$$
(3)

where ∆V is the applied potential, I0 is the initial current, R0 is the initial resistance, Iss is the steady-state current, and Rss is the steady-state resistance. The measured results of these parameters are listed in Extended Data Fig. 5m.

### Density functional theory (DFT) calculations

To predict the oxidation/reduction voltage and binding energies, we carried out DFT calculations using the Gaussian 16 code (revision AVX2)40. We used the hybrid PBE0 functional41 and the basis set 6-311+G** for geometry optimizations, energy calculations and frequency calculations. We adopted the D3 version of Grimme’s dispersion with Becke–Johnson damping (GD3BJ)42 in order to correct for weak interactions.

### Molecular dynamics simulations

The crystalline Cu–CNF–NaOH was built using the Materials Studio (MS, version 7.0)43 Visualizer with experimental input for the lattice constant and crystal symmetry23. The Forcite module in MS was used to conduct classical molecular dynamics (MD) simulations. The COMPASS II forcefield44, which is extended for polymer systems, was adopted to account for both the bonded and the non-bonded interactions. The force-field type and charges listed in Extended Data Fig. 2a result in Li–O interactions for different functional groups comparing well with DFT calculations (Extended Data Fig. 2b). As the Cu2+ did not diffuse in experiments, an additional Harmonic potential with a force constant of 25,000 kcal mol−1 Å−2 was applied to the Cu–O bond term to keep the Cu–O distances at the values obtained from DFT calculations (Extended Data Fig. 2c). The Ewaldsummation method was used to calculate the Coulombic interactions with an accuracy of 0.001 kcal mol−1 and a cutoff distance of 12.5 Å. The Nosé method45 was used for constant temperature dynamics and the Berendsen method46 was used for NPT (constant particle number, pressure and temperature) dynamics. A total simulation time of 5.0 ns with a timestep of 1.0 fs was applied to typical production MD runs.

### Computational models and procedure

We started by building the atomic structure of the crystalline Cu–CNF–NaOH on the basis of the experimental inputs on the lattice parameters and crystal symmetry. The 2 × 2 supercell of the Cu–CNF backbone structure (Extended Data Fig. 2d) was assigned with lattice parameters of a = b = 15.0 Å with a hexagonal symmetry, which agrees with the experimental measurements. Every two nearby cellulose chains were connected by one Cu atom through the hydroxyl O atoms in the simulation cell. A long cell was built with c = 90.0 Å. In our MD simulations, the 2 × 2 supercell was used to avoid the interactions between periodic images. An appropriate number of H2O molecules were added by the Amorphous Cell module in MS (Extended Data Fig. 2e). Our simulated cell contained 144 AGUs, 1,600 water molecules and 12 Cu atoms. Twenty-four CH2OH groups were replaced by COOH groups. Room temperature (298 K) and a pressure of 1 bar were kept constant during NPT dynamics for 1.0 ns to obtain the density at this stage. Next, we removed most water molecules to model the drying process with only 144 H2O molecules left in the system. Although this is the structure used for most analysis (unless noted otherwise), additional systems with 96, 48 and 0 H2O molecules (H2O:AGU = 2:3, 1:3 and 0, respectively) were simulated to evaluate the effect of bound water concentration (Extended Data Fig. 7d). Li+ insertion was achieved by replacing the 24 −COOH groups with 24 −COOLi groups, and the 24 −CH2OH groups with 24 −CH2OLi groups (Extended Data Fig. 2g). There were 48 Li+ ions in the modelling system, and the Li:AGU ratio was set to 1:3, which is the value estimated in the ICP experiment. Then NPT dynamics simulations were performed to obtain the equilibrated amorphous Cu–CNF (Extended Data Fig. 2f) and Li–Cu–CNF (Extended Data Fig. 2g). A high temperature of 600 K was used to accelerate the dynamics; compared with room-temperature simulations, no change in mechanism was observed owing to the use of classical force field. Finally, production runs for 5.0 ns were carried out at 600 K under an NVT (constant particle number, volume and temperature) ensemble to investigate the Li-transport mechanism. Li–Cu–CNF without any H2O molecules was also simulated for comparison. Additional MD simulations on Li–Cu–CNF systems with EC and LiPF6 included were also conducted to investigate the effects of residual EC and PF6 and to calculate the transference number (see Supplementary Discussions 2, 10).

### XANES calculations

Cu K-edge theoretical XANES calculations for the Cu–(AGU)2 system (Extended Data Fig. 2c) were conducted in the framework of the real-space full multiple scattering scheme with the muffin-tin approximation for the potential as implemented in the FDMNES code47.

## Data availability

The data that support the findings of this study are available within this article and its Supplementary Information. Additional data are available from the corresponding authors upon reasonable request. Source data are provided with this paper.

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## Acknowledgements

L.H. and C.Y. acknowledge support from the University of Maryland A. James Clark School of Engineering. Q.W. and Y.Q. acknowledge support from the National Science Foundation (NSF) under grant DMR-2054438. Y.-Y.H. acknowledges support from the NSF under grant DMR-1847038. Solid-state NMR experiments were carried out at the National High Magnetic Field Laboratory, which is supported by the NSF through NSF/DMR-1644779 and the State of Florida. The NMR diffusion work at Hunter College was supported in part by the US Office of Naval Research, grant N00014-20-1-2186. This research used resources at the 8-ID Beamline of the National Synchrotron Light Source II, a US Department of Energy Office of Science User Facility operated by Brookhaven National Laboratory under contract no. DE-SC0012704. Access to the High Flux Backscattering Spectrometer was provided by the Center for High Resolution Neutron Scattering, a partnership between the National Institute of Standards and Technology (NIST) and the NSF under agreement DMR-1508249. Certain commercial equipment, instruments and materials are identified in this paper in order to specify the experimental procedure adequately. Such identification is not intended to imply recommendation or endorsement by the NIST. K.X. acknowledges support from the Joint Centre for Energy Security Research (JCESR), an energy hub funded by the US Department of Energy, Office of Science, Basic Energy Science under IAA SN2020957. We thank F. Lin, D. Hou and Z. Yang from Virginia Tech for providing the NMC811 cathode material.

## Author information

Authors

### Contributions

L.H. conceived the SPE concept and supervised the project. C.Y. and W.X. designed the experiments and conducted the material synthesis, characterization and electrochemical tests. S.H. and Y.G. also contributed to the material synthesis. Y.Q. and Q.W. carried out the DFT and MD simulations and XANES calculation. X.Z. and R.B. contributed to the structural analysis. M.N.G. and S.G. carried out the NMR analysis and determination of the ion diffusion coefficient. J.Z., P.W. and Y.-Y.H. carried out the 6Li NMR analysis. Y.M. and M.T. carried out the neutron-scattering characterization. B.H.K. and F.J. contributed to the XAS experiment. C.W. provided LiMn2O4 material and assisted with testing and evaluating the electrochemical stability window. L.H., C.Y., Y.Q., Q.W., A.B., C.W., A.I., P.A., K.X. and M.W. drafted the paper. All authors contributed to the final manuscript.

### Corresponding authors

Correspondence to Yue Qi or Liangbing Hu.

## Ethics declarations

### Competing interests

The authors declare no competing interests.

Peer review information Nature thanks Lynden Archer and the other, anonymous, reviewer(s) for their contribution to the peer review of this work.

Publisher’s note Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

## Extended data figures and tables

### Extended Data Fig. 1 Structural characterization during the synthesis of Li–Cu–CNF.

ad, Fibre XRD patterns of the CNFs (in the format of densified wood for high-resolution diffraction patterns) after the following treatment steps. a, Cu–CNF–NaOH obtained from Cu2+-saturated NaOH aqueous solution. Peaks are indexed on the basis of the literature23. The (003) reflection is observed with a spacing of 0.51 nm, while the (001) and (002) reflections are absent, indicating that the Cu–CNF–NaOH features a threefold symmetric structure along the direction of the cellulose molecular chain. b, Cu–CNF washed with water to remove NaOH, demonstrating an amorphous structure. c, Cu–CNF after removing water by DMF exchange and evaporating DMF. The fibre XRD pattern shows a mostly amorphous structure with a small angle peak at roughly 2 nm corresponding to cellulose II22, possibly because of a small number of cellulose chains without coordinated Cu that form cellulose II after NaOH is removed. A high q peak at roughly 0.4 nm in the equatorial direction indicates the average molecular chain-to-chain distance of cellulose II. The green arrow in the meridian direction shows a peak corresponding to 0.47 nm in real space. The yellow arrows are pointing to peaks indicating the repeating unit of the Cu–CNF is roughly 1 nm along the cellulose chain. The 0.47 nm and 1 nm repeating distances are absent in all known cellulose structures, and therefore we attribute them to the unique structure of the Cu–CNF. d, Li–Cu–CNF after inserting Li+ in Cu–CNF and evaporating the solvent. The amorphous cellulose structure is maintained with some weak diffraction peaks of cellulose II. The yellow and green arrows indicate the same peaks as in c. eh, XAS analysis of the Cu–CNF and Li–Cu–CNF samples. e, f, Cu K-edge X-ray absorption near edge structure (XANES) spectra of: e, Cu–CNF, Li–Cu–CNF and a CuO standard; f, Cu2O and Cu standard samples. The green dashed line shows the calculated XANES spectrum of Li–Cu–CNF, in good agreement with the experimentally measured spectrum. Cu–CNF and Li–Cu–CNF show similar yet broadened pre-edge peaks to CuO at 8,986 eV (1s → 3d transition), without the characteristic peaks of Cu2O or Cu metal, indicating that the Cu ions in Cu–CNF and Li–Cu–CNF are of +2 valency. g, h, Fourier-transformed Cu K-edge extended X-ray absorption fine structure (EXAFS) spectra of: g, Cu–CNF; h, Li–Cu–CNF. On the basis of the EXAFS spectra, in Cu–CNF and Li–Cu–CNF, the Cu2+ are bonded with O atoms with an average bonding distance of 1.97 Å, consistent with that in reported Cu–organic complexes48, indicating that the Cu2+ is coordinated with the hydroxyl groups of the cellulose molecules.

### Extended Data Fig. 2 DFT calculations and MD simulations of the Li–Cu–CNF structure.

a, Assigned COMPASS II force-field types and atomic charges in typical cellulose units for MD simulations. b, Optimized atomic structures of the representative systems of Li–Cu–CNF used to evaluate interactions between Li+ and different oxygen-containing functional groups and water molecules, and corresponding energy–distance relationships for different Li+-bonding environments given by molecular mechanics calculations using COMPASS II FF and DFT calculations. The difference between the total system energy at r = 10.0 Å and the minimum energy is taken as the Li+-dissociation energy. The Li+ is strongly bonded with both anionic COO and RO groups with dissociation energies of more than 5.0 eV. The dissociation energy of the Li+ is roughly 3.0 eV for ROH and EO groups, and 1.5 eV for H2O molecules. The strong interactions between the Li+ and one or two oxygen species in cellulose suggest slow Li+ movements in the absence of multiple Li–O coordination. In the H2O molecule, the O atom has an atom type of o2* and charge of −0.82 e, while the H atom has an atom type of h1o and a charge of +0.41 e for force-field calculations. c, To simulate Cu2+ coordination in cellulose, we optimized the atomic structure of two AGUs connected by one Cu2+ (Cu–(AGU)2 system) to serve as a structural building block. Two H atoms are deprotonated by the Cu. The average optimized Cu–O bond length (1.96 Å) is close to that observed in the experiment (1.97 Å), and the calculated XANES of the Cu–(AGU)2 system is also in good agreement with the experimental measurement (Extended Data Fig. 1e), showing that our computational model for the structure of the Cu–O complex is reasonable. Atom types and atomic charges in force-field calculations are given for Cu and its connected O atoms, which are categorized as ROH for statistics (Fig. 3d in the main text). d, Top view of a 2 × 2 supercell of the periodic Cu-coordinated CNF structure as a starting structure for the simulation, built with the most reasonable model that we proposed on the basis of the fibre XRD pattern (Fig. 2c). Every two nearby cellulose chains are connected by one Cu atom through the hydroxyl oxygen atoms. The unit cell is denoted by dashed blue lines. e, Top and side views of the Cu–CNF–NaOH. f, Top and side views of the amorphous Cu–CNF obtained by removing NaOH aqueous solution from Cu–CNF–NaOH and then equilibrating the system with NPT dynamics simulations. In Cu–CNF, we reserved 144 H2O molecules to keep an H2O:AGU ratio of 1:1. g, Schematic of the computational approach used to obtain the atomic structure of the final amorphous Li–Cu–CNF model (top and side views).

### Extended Data Fig. 3 Bound water analysis of Li–Cu–CNF.

a, 1H MAS NMR spectra of Li–Cu–CNF with peak deconvolution. b, 1H MAS NMR spectra of Cu–CNF (dried at 30 °C under vacuum for three days to remove water). c, FTIR of the pristine CNFs and solid-state Li–Cu–CNF. Both the pristine CNFs and Li–Cu–CNF show a broad –OH stretching peak at roughly 3,300 cm−1. d, The −OH stretching peak of Li–Cu–CNF deconvoluted into three bands at 3,464 cm−1, 3,235 cm−1 and 2,886 cm−1, which can be assigned to bound water molecules in different hydrogen-bonding states49,50. e, The atomic mean square displacement (MSD) change in CNF and Li–Cu–CNF as a function of temperature, as measured by QENS. The Cu–CNF sample after DMF solvent exchange with some residual DMF (Cu–CNF–DMF) is also shown for comparison. f, Elastic neutron-scattering intensity of free water plotted against temperature (60 μl H2O on Cu foil) upon cooling; data derived from ref. 51. g, DSC curve of Li–Cu–CNF in a cooling process from 30 °C to −30 °C. h, Plots of H2O–H2O radial distribution function (RDF) (solid lines) and coordination number (dashed lines) in liquid bulk water (red lines) and Li–Cu–CNF (blue lines). The first minimum of the RDF plot for the liquid bulk water system at 3.4 Å (indicated by the black dashed line) was applied to calculate the coordination numbers. The distance is defined as the distance between the O atoms of the H2O molecules. i, Stress–strain curve of Li–Cu–CNF along the direction of the CNF fibre. For more analysis, see Supplementary Discussion 11.

### Extended Data Fig. 4 Electrochemical stability of Li–Cu–CNF.

a, b, The electrochemical stability window of Li–Cu–CNF was measured by both anodic and cathodic LSV scans at 0.1 mV s−1. a, The first three anodic scans from OCV to 5.4 V. b, The first three cathodic scans from OCV to 0 V. c, Top, reduction and oxidation potentials (versus Li+/Li) obtained from DFT calculations for (bottom) different structures representative of the cellulose and Li–Cu–CNF systems, including: (1) glucose; (2) AGU dimer; (3) AGU–COOLi; (4, 5) two isomers of (AGU)2–COOLi; (6) AGU–CH2OLi; (7, 8) two isomers of (AGU)2–CH2OLi; (9) Cu– (AGU)2; (10) H2O dimer; and (11) (AGU)2–(H2O)2. C, H, O, Li and Cu atoms are represented by grey, white, red, purple and blue spheres, respectively. Water molecules are depicted with stick models. The experimental oxidation potential for Li–Cu–CNF (black) and the redox potentials for EC are denoted with dashed lines (blue for reduction and red for oxidation) for reference. See Supplementary Discussion 12 for more detailed analysis.

### Extended Data Fig. 5 Ionic conductivities and transference numbers of Li–Cu–CNF and Li–CNF.

a, Voltage profile of the galvanostatic Li plating and stripping between two ends of the Li–Cu–CNF with aligned cellulose fibres (length 1 cm) at 0.01 mA. b, EIS Nyquist plots of aligned Li–Cu–CNF materials of different lengths, ranging from 1 cm to 3 cm, for measuring the intrinsic conductivity of Li–Cu–CNF along the direction of the cellulose molecular chain. c, Resistance corresponding to the high-frequency semi-circle in b of the aligned Li–Cu–CNF with different lengths. d, EIS Nyquist plots of the aligned Li–Cu–CNF with a length of 3 cm and cross-sectional area of 0.03 cm2 at different temperatures, ranging from 10 °C to 60 °C. e, f, EIS Nyquist plots of the Li–Cu–CNF paper electrolyte (through-plane) at different temperatures (e, 60 °C to 0 °C; f, −2 °C to −20 °C); g, the corresponding temperature-dependent through-plane ionic conductivity of the Li–Cu–CNF paper electrolyte. h, d.c. polarization curve of the Cu2+ in the Li–Cu–CNF electrolyte in a Cu//Cu-CNF//Cu cell, showing that the Cu2+ conductivity is 1.0 × 10−8 S cm−1, much lower than the Li+ conductivity in Li–Cu–CNF. i, Simulated structure of Li–CNF by MD. The Li–CNF system consists of 16 cellulose chains surrounded by Li+ and water molecules. Different chains are denoted by different colours. Li+ ions are indicated by purple spheres and water molecules as stick models. The size of the Li–CNF system is given roughly. The simulations show that, without the participation of Cu2+, the Li+ and water molecules adsorb only on the surface of the cellulose structures. j, d.c. polarization curve, and k, EIS Nyquist plots before and after polarization of the Li//Li–Cu–CNF//Li cell. l, d.c. polarization curve, and m, EIS Nyquist plots before and after polarization of the Li//Li–CNF//Li cell. n, Table showing the parameters measured by d.c. polarization and EIS for calculating the Li+-transference number.

### Extended Data Fig. 6 NMR analysis of Li-coordination environments and diffusion pathways.

a, b, 6Li NMR spectra and simulations for: a, Li–Cu–CNF; b, Li–CNF. c, d, 6Li NMR spectra for: c, CH2COOLi∙2H2O, and d, LiPF6, as references for the COO∙∙∙Li and LiPF6 peak assignments in Li–Cu–CNF. e, f, 6Li NMR spectra and simulations for: e, Li–Cu–CNF, and f, Li–CNF after 6Li→7Li tracer exchange, which was performed by cycling either the Li–Cu–CNF or the Li–CNF electrolyte (natural abundance: 92.4% 7Li and 7.6% 6Li) between two 6Li-enriched metal electrodes (that is, symmetric 6Li//Li–Cu–CNF//6Li cells). g, Table showing the amount of Li+ in the different chemical environments of Li–Cu–CNF and Li–CNF before and after 6Li→7Li tracer exchange, derived from the relative spectral areal integrals of the 6Li resonances in the NMR spectra shown in a, b, e, f. The normalized peak area for each sample (Li–Cu–CNF and Li–CNF, before and after 6Li→7Li tracer exchange) can be quantitatively compared between different samples as the normalized peak area is proportional to the amount of 6Li in each individual product. We took the total number of 6Li in the pristine Li–Cu–CNF (before 6Li→7Li tracer exchange) to be 100%, and calculated the ‘relative 6Li number’ of each component by comparing the fitted peak area (Extended Data Fig. 6a, b, e, f) with the total area of 6Li in the pristine Li–Cu–CNF (Extended Data Fig. 6a).

### Extended Data Fig. 7 Numerical analyses of MD simulations for Li+ transport in Li–Cu–CNF.

a, Displacement plots for six Li+ ions that have displacements of more than 15.0 Å in the simulated Li–Cu–CNF system (Fig. 2i) with an H2O:AGU ratio of 1:1, and indexes of COO/RO atoms that are bonded to the six moving Li+ ions (Li–O distance less than 2.5 Å). The different colours of the COO/RO atoms indicate they are from different cellulose chains. b, Coordination numbers of Li+ ions coordinating with all available oxygen atoms (Li–O, including the oxygen atoms in cellulose and bound water molecules) and with just water molecules (Li–H2O) for the six fastest and six slowest Li+ ions in the Li–Cu–CNF system with an H2O:AGU ratio of 1:1. c, MSD plots for Li–Cu–CNF systems with different number of water molecules, and for the Li–CNF system with water molecules on the surface of the CNFs. d, Radial distribution functions (RDFs) for Li–Li and COO–RO pairs in Li–Cu–CNF with an H2O:AGU ratio of 1:1. The locations of the first peak of the Li–Li pair and the second peak of the COO-RO pair indicate the Li+ hopping distance (roughly 3.0 Å) between the residence sites. The first peak of the COO–RO pair indicates the distance between the two O atoms within the same COO group. e, MSD plots for Li+, COO and RO groups and Cu2+ in the simulated Li–Cu–CNF system with an H2O:AGU ratio of 1:1. The average MSD plots show that Li+ moves fast while COO, RO, and Cu2+ in the Li–Cu–CNF backbone move much more slowly. For further analysis, see Supplementary Discussion 13.

### Extended Data Fig. 8 The Li–Cu–CNF paper electrolyte and its electrochemical performance.

a, Top-view SEM image of the Li–Cu–CNF paper electrolyte. b, Digital photos (top and back) of a permeability test of the Li–Cu–CNF paper electrolyte to demonstrate the denseness. c, Li plating/stripping cycling performance of the Li–Cu–CNF paper electrolyte at 0.5 mA cm−2, with 2 h for each plating/stripping half cycle, for a total of 300 h at room temperature. d, SEM image and e, corresponding EDX spectrum of the Li-metal anode after long-term cycling with the Li–Cu–CNF paper electrolyte. The SEM image of the cycled Li anode shows a fairly smooth surface without Cu particles deposited on the surface. The EDX shows no detectable Cu element on the Li surface, and instead only C, O, F and P, indicating the formation of a solid electrolyte interphase (SEI) on the Li-metal anode.

### Extended Data Fig. 9 Demonstration using Li–Cu–CNF as a paper electrolyte and ion-conducting binder for solid-state LiFePO4 batteries.

a, Fabrication steps for incorporating the cathode material (LiFePO4 here) with the Li–Cu–CNF ion-conducting binder via the traditional slurry-casting method. The Cu–CNF suspension is first mixed with the cathode material, CNT additive and sodium alginate binder in an aqueous solution to obtain the cathode slurry. The slurry is then cast on aluminium foil using a doctor blade and vacuum dried at 35 °C. The cathode electrodes are then soaked in Li+ electrolyte to achieve the insertion of Li+ into the Cu–CNF, followed by vacuum drying to obtain solid electrodes containing the Li–Cu–CNF binder. b, c, EIS of the solid-state batteries using thick LiFePO4 cathodes (roughly 120 μm), made by filtration-pressing with the addition of: b, Li–Cu–CNF; c, Li–CNF. d, A pouch solid-state battery made using a Li anode, the Li–Cu–CNF paper SPE, and a LiFePO4 solid-state cathode containing the Li–Cu–CNF ion-conducting binder, which shows good flexibility while still powering an LED light.

### Extended Data Fig. 10 Electrochemical performances of high-voltage cathodes with the solid-state Li–Cu–CNF electrolyte.

a, b, Typical galvanostatic charge/discharge voltage profile of a solid-state NMC811 cathode with the Li–Cu–CNF electrolyte cycled at 100 mA g−1 and room temperature (a); and its discharge capacities during cycling (b). c, d, Typical galvanostatic charge/discharge voltage profile of the solid-state LiMn2O4 cathode with the Li–Cu–CNF electrolyte cycled at 50 mA g−1 and room temperature (c); and its discharge capacities during cycling (d).

## Supplementary information

### Supplementary Information

This file contains Supplementary Discussion, including Supplementary Figs. 1–21 and Supplementary Tables 1–8, and additional references.

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Yang, C., Wu, Q., Xie, W. et al. Copper-coordinated cellulose ion conductors for solid-state batteries. Nature 598, 590–596 (2021). https://doi.org/10.1038/s41586-021-03885-6

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• DOI: https://doi.org/10.1038/s41586-021-03885-6

• ### Expanding cellulose

• Sang-Young Lee

Nature Energy (2021)