## Introduction

Reversible electrodeposition of metals has recently reemerged as an area for fundamental and applications- oriented studies, reviving interest in rechargeable batteries that use metal anodes, such as Lithium (Li), sodium (Na), magnesium (Mg), calcium (Ca), zinc (Zn), and aluminum (Al)1,2,3,4. A large body of evidence now exists that uneven, mossy, and dendritic deposits, hinder reversibility in both expected (e.g., limiting battery lifetime through internal shorting) and un-expected (e.g., weakening the connections between deposits and the current collector to promote electronic isolation) ways. In either case, the result is that less of the active metal in the anode is available for charge storage, and consequently few, if any, of the metal anodes under consideration live up to their potential for achieving cost-effective and energy-dense storage5,6.

These findings have in turn renewed interest in understanding root causes and the fundamental transport and electrochemical processes that promote mossy deposition and dendrite formation over different ranges of current density, i7,8. In the low current density region—characterized as current densities well-below the classical diffusion-limited value, iL = 4FcD+/l—classical transport-based theories that invoke hydrodynamic instability8 are not relevant. Here iL is the limiting current; D+ is the cation diffusion coefficient; c the salt concentration in the electrolyte solution (assume to be dilute concentration: ≤0.05 M); l is the space between physically separated electrodes confined in the same cell; and F is Faraday constant. Thus, for i << iL, two processes are thought to be most responsible for non-uniform, wire-like and mossy deposition: (1) uneven electric field lines at irregular deposit features (e.g., bumps, edges, etc.), which promote growth of non-planar wire-like/mossy/dendritic structures9; and (2) uneven charge transport through interphases formed on the metal, leading to preferential nucleation and growth of metal deposits along particular directions. A serious consequence of the second process is that stripping of metal from underneath deposits coated by a non-uniform solid electrolyte interphase, can selectively remove portions of a non-planar deposit near its roots, which promotes breakage and electrochemical disconnection of the deposits (i.e., metal orphaning). This results in high anode irreversibility10,11, which typically means the reversible cycling of metal anodes is limited to a few cycles. All of these processes remain at high current density, iiL, and are augmented by the hydrodynamic instability termed electroconvection, which is driven by an ion-depleted, extended space charge layer that extends away from the electrode surface into the bulk12. For fundamental reasons discussed elsewhere13,14, electroconvection favors localized deposition on a spectrum of length scales and recent studies, including numerical simulation and experimental observation13,14,15, show that strong “electroconvection” accelerates growth of non-planar deposit morphologies formed by other processes (Fig. 1a). A consequence is that operation of metal anode batteries is generally limited to the regime i << iL4,16,17,18,19,20,21,22, which is a barrier to their use in electric grid and fast-charging electrified transportation applications where long-term stability at high current densities is demanded.

Aqueous zinc batteries have recently been reported to provide excellent model systems for understanding interfacial processes in all batteries that employ metal anodes23. They also promise cost and performance advantages that are attractive from an applications perspective24,25. We note however that, notwithstanding the very high D+ values in aqueous electrolytes, the highest current density achieved in state-of-the art Zn cells4 are still substantially below iL (≤40 mA cm−2). A number of strategies, including deployment of viscoelastic liquid electrolytes7 and field-induced crystallographic reorientation8 of Zn deposits have been reported to show potential for suppressing electroconvection and achieving primary smooth, uniform metal electrodeposition at high current densities. These effects are conventionally discussed in terms of coupling between electroconvection (which produces a spatially non-uniform cation flux at the electrode) and secondary flows produced by polymer elasticity or viscous fluid flow produced by electrode motion, either of which can produce counter flows that render the cation flux to the interface more uniform26,27. Local Joule heating has been reported as another important strategy to achieve smooth electrodeposition at high current density28. Results from linear stability analysis and direct numerical simulations from a number of groups, show that the Damkohler number Da ≡ i0/iL, the dimensionless ratio of exchange current i0 at the electrode to the diffusion-limited current iL in the electrolyte determines the propensity for metals to deposit in largely planar/compact or non-planar/non-compact morphologies14,26,27,29. Here we make specific reference to findings from recent direct numerical simulations of coupled electro-hydrodynamics, transport, and interfacial reaction of metals at planar interfaces14,27, which show that as Da decreases, the lateral gradient of the surface potential creates a lateral ion flux that drives cations away from high cation concentration regions, meaning that the ion velocity (Vx) parallel to the electrode surface increases, while the velocity perpendicular (Vy) decreases (Fig. 1b). This finding is in qualitative accord with reports from direct tracer particle visualization experiments15,30, and can be interpreted more simply in terms of a competition between kinetic processes in the following manner: by allowing arriving metal ions sufficient time to redistribute at the electrode surface before they are reduced, low Da values are advantageous for obtaining a smooth electrodeposition morphology, irrespective of the current density. The fast reaction kinetics of metal electroreduction and large volume change at a metal anode required for practical battery operation are fundamental, un-resolved barriers for creating interphases that support sufficiently low Da at metal anodes in liquid electrolytes, as well as for maintaining such low Da values over long cell lifetimes and under conditions where the anode volume changes significantly during cycles of charge and discharge (Fig. 1b).

Here we report that dynamic, nanometer-thick, ion-oligomer interphases in situ formed on a Zn metal anode inside a single-cell battery provide a powerful and versatile approach for suppressing non-planar deposition by suppressing the full set of instabilities (chemical, morphological, and hydrodynamic) (Fig. 1b). The approach is stable during long-term operation (>10,000 cycles) of an unusually long-time scale (>1000 h). We show further that the spontaneously formed nanolayers enable highly reversible Zn electrodes at current densities as high as 160 mA cm−2 in aqueous electrolytes, which is at the same order of magnitude of the limiting current density (iL ≈ 10^2 mA cm−2), and about four times higher than the highest values reported for aqueous Zn electrodes. When paired with conversion cathodes such as I2/activated carbon, we demonstrate that the dynamic ion-oligomer complexes enable battery cells, pseudocapacitor-like lifetimes (>12,000 charge/discharge cycles) at high active material utilization. In addition, fast-charge pouch cell batteries employing a 20-μm thin Zn anode are demonstrated to run for over 100 cycles at a charge current density of 56 mA cm−2. Even without efforts to optimize their performance, the pouch cells achieve specific energy as high as 555 Wh kg−1AC (151 Wh kg−1Zn+AC), illustrating the scalability of the ion-oligomer electrolyte concept. As an extended example, we investigate Zn||MnO2 aqueous cells and find that they also achieve long-term cycling performance (>1000 charge/discharge cycles) at a charge current density of 160 mA cm−2, meaning the reported ion-oligomer complexes are quite versatile for both anode and cathode sides (Fig. 1c). We also explore the possibility to apply the in situ formed ion-oligomer nanometric interphase strategy in a non-aqueous electrochemical energy storage system such as an Li||I2 cell where we demonstrate reversibly battery operation at a current density of 40 mA cm−2.

## Results

As a first step to identifying a general strategy for achieving high metal anode reversibility, we speculate that a conformal, interfacial nanolayer spontaneously formed on a metal electrode by reversible adsorption of poly-/oligo-ethers could simultaneously block electroreduction sites—lowering i0—and providing a “self-healing” (polymer layer can be spontaneously reformed during metal strip and deposit process) characteristic stemming from dynamic polymer adsorption/desorption processes at the electrolyte/electrode interface. To evaluate this hypothesis, we take advantage of the following three well-known effects to create and study adsorption of Zn2+-halide ion-oligomer complex at metal substrates: (i) high affinity of metal cations for the lone electron pairs on ether oxygens in poly-ethers; (ii) high surface affinity of halide ions for metal substrates, which has been attributed to their ability to form interfacial halide-metal covalent-like bonds31; and (iii) spontaneous dynamic adsorption/desorption of dissolved polyether ion complexes to the electrode surface. Thus, a well-designed halide ion-oligoether complex, provides a possible mechanism for reversibly drawing the oligomer out of solution and onto the metal surface, and anchoring it there using strong interfacial bonds between halide and metal. The bonding between Zn2+ and oligomer increases the de-solvation energy of Zn-ion at the electrode, lowering i0 for the interfacial reduction of Zn2+32,33. On this basis we speculate that an effective polymer adsorption layer requires a balance between two polymer solution effects: ion-oligomer complex formation and interfacial complex adsorption. The hydrated oligomer must first bond with the initial complexes of Zn2+-halide ions in the bulk electrolyte to create the complex, while remaining soluble. The second requirement is that the Zn2+-halide ion-oligomer complex dynamically adsorbs onto the surface by the process mentioned above.

### Zn2+-halide ion-oligomer design and adsorption

We designed and studied the structure of ion-oligomer complexes in aqueous electrolytes formed between Zn2+-halide ion complexes and a polyethylene oxide (PEO) oligomer of average molecular weight 300 Da. Aqueous electrolytes solutions based on three zinc halide salts (ZnX2 (X = Cl, Br, I)) were prepared and the results compared with an aqueous ZnSO4 reference electrolyte solution. The structure of the solvated Zn halide complexes deduced from Raman vibrational spectroscopy of the electrolytes (Supplementary Fig. 1) are consistent with previous reports34,35,36 and show that structure of the initial ion complexes formed by Zn salts in aqueous media varies substantially from salt to salt. For ZnSO4 electrolyte, octahedral [Zn(H2O)6]2+ is the dominant ionic complex in solution (Supplementary Fig. 2a); in ZnCl2 electrolyte, tetrahedral [ZnCl2(H2O)2], in which Zn ions bond with two water molecules and two chloride ions, are the main ionic states (Supplementary Fig. 2b); in ZnI2 electrolyte, in addition to the stable complexes [ZnI4]2− (in which Zn only bonds with iodide ions in aqueous media), several unstable complexes [ZnI3], [ZnI2] and [ZnI]+ are also present in large proportions (Supplementary Fig. 2c); in ZnBr2 electrolyte, the ion complexes states combine the structure of ZnCl2 and ZnI2 electrolyte, [ZnBr2(H2O)2], [ZnBr4]2−, [ZnBr3], [ZnBr2] and [ZnBr]+ coexist and the ratio of these ion complexes varies as the concentration of ZnBr2 change (Supplementary Fig. 2d). The different initial ion complex states result from the different anion steric structures (SO42− and halide ions) and electronegativity (Cl, Br, I). The LUMO potential of all solvation ions was given by simulation (Supplementary Fig. 3), which explains the different reaction kinetics (exchange current) in the following sections.

Long-chain PEO (MW > 3000) shows a great potential to regulate Zn electrodeposition due to several reasons37: (1) PEO can increase the viscosity of the electrolyte that has a great influence on the ion mobility; (2) due to the interfacial electrode adsorption of PEO, visualization experiments show that the ion velocity Vx highly suppressed while Vy increases (Fig. 1b) that may result from the relaxation and contraction of long polymer chain. On the basis of these results, we choose to study polyethylene glycol with a molecular weight of 300 g mol−1 (PEG300). This polymer is of interest because it is easily dissolved in aqueous Zn salt electrolytes to form ion-oligomer complexes. We observed different ion-oligomer complex structures when PEG300 is introduced to the four aqueous Zn salt-based electrolytes.

Nuclear magnetic resonance (NMR) was used to first understand the ion-oligomer complexes formation in aqueous electrolytes containing Zn salts and PEG300. It is known that the de-shielding effect results in the left shift of 1H peak in NMR spectra, therefore, the 1H peak in the PEG backbone (Supplementary Fig. 4) reflects the complexes’ stability of PEG300, Zn2+, and halide ions. In 5% PEG300 + ZnSO4 electrolyte, the 1H peaks of PEG300 shift to the far right, indicating the strong shielding effect here, which increases as the concentration of ZnSO4 increases (Fig. 2a). We assume that it’s the hydrogen bond between Zinc solvation ions, water molecules, and PEG300 that results in this kind of effect, and further predicts the bond model (Fig. 2a). To evaluate our hypothesis, Fourier-transform infrared spectroscopy (FTIR) and ab initio calculations are used to understand the hydrogen bonding effect. In FTIR (Supplementary Figs. 57), the ratio between the absorbance intensity of Peak c and Peak d can reflect the level of hydrogen bond cooperativity38,39. The value of Peak c/Peak d decreases as 5% PEG is added into the DI water, meaning that much higher hydrogen bonds cooperativity and the interaction between water molecules and PEG is stronger (Supplementary Fig. 6). 1 M ZnSO4 salts can further decrease the Peak c/Peak d value, which can be explained by the formation of Zn solvation ions (Supplementary Fig. 6). An intense decrease of Peak c/Peak d value is observed in the 5% PEG300 + 1 M ZnSO4 electrolyte, verifying that hydrogen bond is the main factor that facilitates the PEG300–H2O–[Zn(H2O)6]2+ complex (Supplementary Fig. 6). Ab initio calculations further confirms the complex formation model (Supplementary Table 1). However, a different shift trend of the PEG300 1H peak is observed in Zn halide electrolytes. For ZnCl2 + 5% PEG electrolytes (Fig. 2b), the shielding effect (peak shift) is not as strong as that of ZnSO4 electrolyte, indicating lower hydrogen bond cooperativity that can be further confirmed by the increase of Peak c/Peak d value (Supplementary Fig. 6). Nevertheless, the reverse shifting trend (de-shielding effect) in ZnI2 + 5% PEG electrolytes indicates a different bonding effect between PEG and the unstable complex [ZnI3]−, [ZnI2] and [ZnI]+, in which no water molecules take part in the ion-oligomer complex formation (Fig. 2c) and the Peak c/Peak d value highly increases (Supplementary Fig. 7). Such a behavior can be explained by the lower electronegativity and higher polarization of iodine atoms, resulting in a more uniform electron distribution and less partial charge at both Zn and I. Compared to the highly polarized Zn-Cl bond, the [ZnIx]2−x complex is less prone to bond with free water (a strong dipole), but prefers bonding with the oxygen atom on PEG, whose partial charge is stabilized by the carbon backbone. The above mechanism is verified in ab initio simulations (Supplementary Tables 2 and 3). For ZnBr2 + 5% PEG electrolytes, shielding effect is observed initially (shift to the right) and then overwhelmed by the de-shielding effect (shift back to the left), indicating the ion-oligomer formation effect changes as the concentration of ZnBr2 increases (Fig. 2d). Bromine has an intermediate electronegativity and polarization compared to chlorine or iodine, and thus demonstrates a mixed behavior of both. On the basis of the 1H spectrum of NMR results (Fig. 2), hydrogen bond peaks of FTIR (Supplementary Figs. 6 and 7), we deducted the complex structure for the Zn halide + PEG electrolytes: (1) PEG-H2O-[ZnCl2(H2O)2] complex in ZnCl2 electrolyte (Fig. 2b); (2) PEG-[ZnI3], [ZnI2] and [ZnI]+ complexes in ZnI2 electrolyte (Fig. 2c); (3) PEG- H2O-[ZnBr2(H2O)2], PEG-[ZnBr3]-, [ZnBr2] and [ZnBr]+ complexes in ZnBr2 electrolyte (Fig. 2d). All these models are consistent with the ab initio calculations (Supplementary Figs. 8a, b and 9).

The influence of the ion-oligomer complexes on interfacial polymer adsorption was studied using a quartz-crystal microbalance (QCM), ellipsometry, and electrochemical impedance spectroscopy (EIS). QCM (Fig. 3a, b and Supplementary Fig. 10a–d) is very sensitive to the interfacial polymer adsorption process and can be used to characterize the amount, thickness, reversibility, and interfacial physical properties of the adsorbed polymer layer. We employed three electrolyte flowing steps protocol. First, flowing the blank 1 M ZnSO4 aqueous electrolyte solution or Zn halide electrolyte solution to establish the effect of salts adsorption on the frequency shift. Second, 5% PEG300 + 1 M ZnSO4 or Zn halide electrolytes flow through QCM sensor, we can observe the frequency change (∆f) and dissipation change (∆D) (“dissipation” is the sum of all energy losses in the flowing system per oscillation cycle) which can be related to physical properties of the polymer adsorbate (including thickness, viscosity, and modulus) as well as the viscosity increment produced in the electrolyte bulk. Finally, after the stabilization of the second step, we re-flow the blank 1 M ZnSO4 aqueous electrolyte solution or Zn halide electrolyte solution. In this step, if the frequency returns to the value in the first step, the polymer adsorption in the second step is considered reversible.

Analysis of the QCM experiments revealed a number of important features of the interphases formed by polymer adsorption: (1) Ion-oligomer adsorption is a reversible process since the frequency and dissipation values plummet to zero when the flowing fluid is switched back to the initial solution (1 M ZnSO4 or 1 M ZnX2), not containing polymer; (2) as shown in Fig. 3b and Supplementary Fig. 10e, the average thickness is related to the interfacial coverage, meaning the thicker the adsorbate layer, the greater the coverage. The designed complex of Zn2+-halide ions-PEG300 shows larger interfacial coverage than PEG-[Zn(H2O)6]2− complex, which we believe reflects the strong interfacial specific adsorption of halide ions33; (3) however, the interfacial viscosity (Supplementary Fig. 10f) of these four kinds of complexes does not vary greatly, implying that the interfacial viscosity is not the main source of the change of interfacial properties, which disagrees with previous reports7; (4) the ion-oligomer adsorption layer is viscoelastic in nature since the shift in different harmonics do not overlap (F_1:3, F_1:5, F_1:7, the number 3, 5, 7 represent the third, fifth and seventh harmonics) and the dissipation values (D_1:3, D_1:5, D_1:7, the number 3, 5, 7 represent the dissipation change for different harmonics) are high (>1 × 10−6). Direct measurement of ion-oligomer complex layer features was performed using an ALPHA-SE Ellipsometer (Supplementary Fig. 11). These measurements confirm the strong interfacial adsorption of Zn2+-halide ions-oligomer complex (Fig. 3c, d). Based on the QCM and ellipsometer results, the adsorbate thickness of the designed ion-oligomer complex varies from 2 to 150 nm, depending on the anion chemistry and polymer concentration. Hence, we can conclude that the influence of the adsorption layer is concentrated in a nanometer-thick interphase zone near the electrode surface.

EIS experiments can also provide complementary insights into the dynamics of an interfacial nanolayer composed of the designed Zn2+-halide-PEG300 complex. Figure 4a–c, Supplementary Fig. 12a–d and Supplementary Table 4 show that much lower interfacial impedance are observed in electrolytes containing ZnI2 and that these values are reduced slightly in electrolytes containing PEG oligomer additives. These results are consistent with our previous report33, which showed the strong interfacial adsorption of unstable iodide and bromide ion complexes facilitate interfacial ion transport. Our earlier results showed further that these complexes are stabilized by adsorption to PEG oligomers, which we believe results in the reduced interfacial impedance observed (Fig. 4d).

### Effect of the ion-oligomer complex layer on the Zn electrodeposition

Figure 5 reports the effect of the ion-oligomer complex layer on the Zn electrodeposition process. First, we interrogate the effect of the adsorbed polymer on the exchange current density (Fig. 5a, b and Supplementary Fig. 13). In all electrolytes studied, the PEG is seen to markedly lower i0 (Fig. 5b), which we attribute to ion-oligomer adsorption, which can increase the de-solvation energy of Zn2+ by the aforementioned mechanism. Next, limiting current densities extracted from the current–voltage (i–v) curve (Supplementary Fig. 14) can further reflect the interfacial ion diffusion kinetics. Zn halide + PEG electrolytes show much higher limiting current densities than ZnSO4 + PEG electrolytes (Fig. 5c), which results from the strong interfacial adsorption of Zn-halide ion complexes (such as [ZnI3])33, further supporting the speculation that halide ions can improve the interfacial adsorption of ion-oligomer complex. Based on these results, we can combine the influence of reaction kinetics and diffusion kinetics by Da (Da ≡ i0/iL). Previous numerical simulations14,27 show that when Da reaches a critical low value of 0.0025, a uniform ion flux parallels (Vy) at the electrode surface can be achieved. As Shown in Fig. 5d, Da values below this theoretical threshold are observed in ZnBr2 + PEG300 (Da ≈ 0.0033) and ZnI2+ PEG300 (Da ≈ 0.0028) electrolytes. Chronoamperometry experiments were performed to more directly correlate the transient current response and electrodeposition morphology under conditions approaching the transport limiting current range. The inflection in the current versus time (i–t) plots for the pure Zn salt and ZnSO4 + PEG electrolytes is associated with the Sands time (Fig. 5e), indicative of the time-scale required for the space charge to develop and mixing due to formation of electroconvection rolls to begin8. The inflection disappears in ZnX2 (X = Cl, Br, I) + PEG electrolytes (Fig. 5f–h). Significantly, smooth and uniform Zinc deposits were observed in the ZnBr2+ PEG and ZnI2 + PEG electrolytes (Fig. 5i–l), even at current densities in the classical over-limiting electrokinetic regime region (–2.1 V vs AgCl/Ag). Our finding that the Zn electrodeposit morphology is uniform even at the high voltages used in the study implies that it should be possible to create stable Zn batteries able to operate at high current densities as discussed in the following section.

### Assembly and testing of aqueous Zn metal lab-scale cells

To evaluate the reversibility of Zn deposits in our designed ion-oligomer electrolytes at the high current density, we measured the electrochemical cycling performance of Zn anodes in Zn||carbon cloth half-cell. The plating/stripping Coulombic efficiency (CE %) of Zn deposits in each cycle reveals the ratio between the amount of metal that can be stripped and the amount that is plated in the previous cycle. Figure 6a and Supplementary Fig. 15a show the reversible Coulombic efficiency (CE %) for a long time cycling at current density 160 mA cm−2 and areal capacity 2.6 and 1.1 mAh cm−2. Compared with ZnI2 (Supplementary Fig. 15b), ZnSO4 + PEG300 (Supplementary Fig. 16a) and ZnCl2 + PEG300 electrolytes (Fig. 6a), ZnBr2 + PEG300 and ZnI2 + PEG300 electrolytes (Supplementary Figs. 16b, 17, and 18), show more stable and higher CE (99.2% for ZnBr2 + PEG and 99.5% for ZnI2 + PEG, respectively) and better reversible cycling performance (5000 cycles at 2.6 mAh cm−2 and 8000 cycles at 1.1 mAh cm−2). It is worth noting that the stable reversible cycling performance at a current density of 160 mA cm−2 was achieved on a Zn anode (Fig. 6).

Benefiting from the long cycle life of the Zn anode at high current density (160 mA cm−2), fast-charge aqueous batteries can be produced using ZnI2 + PEG electrolytes. For ZnI2 + PEG electrolyte, we choose active carbon (AC) as cathode, which can provide sufficient adsorption site33 for the oxidation product I3 (3I → I3 + 2e). Here, to compensate for the relatively low reaction rate at cathode side, we designed an intermittent charging method for Zn||I2(AC) full cell: charging 10 s at 160 mA cm−2, resting 10 s to enable the interfacial ion equilibrium and then charging another 10 s. As shown in Fig. 6c, voltage increase can be observed in both charging stages, while the voltage drop during the 10-s rest is minimal, demonstrating stable charging behavior. During the discharging process, a stable discharge plateau at 8 mA cm−2 proves the effectiveness of this charge process and the stability of the electrode at ZnI2 + PEG electrolytes. Significantly, Zn||I2(AC) full cell with 1 M ZnI2 + 5% PEG electrolytes shows stable cycle performance: at a charge current density of 160 mA cm−2 and discharge current density of 8 mA cm−2, we achieved an areal capacity of 0.88 mAh cm−2 over 12,000 cycles (Fig. 6d), benefiting from the stable Zn electrodeposition and intermittent charging method (Supplementary Fig. 19). Importantly, the designed 1 M ZnI2 + 5% PEG electrolytes and intermittent charging method can also be applied to pouch cells with 20-μm thick zinc foil (Supplementary Fig. 20). By using ZnI2 + 5% PEG electrolytes and 20 μm Zn foil, Zn||I2 (AC) pouch cell can be charged at a high current density of 56 mA cm−2 and run stably over 100 cycles. For pouch cell, we employed a similar intermittent charging method: charge the pouch cell for 1 min at 56 mA cm−2, then rest for 10 s, and repeat three times (Fig. 6e). Similar to coin cell, a distinct discharge plateau can be observed with discharge current density of 11 mA cm−2, proving the effectiveness of our ion-oligomer electrolyte system and intermittent charging method. Notably, a specific energy of 555 Wh kg−1AC at a current of 0.506 A can be achieved based on the mass of AC, and 151 Wh kg−1 can be retained considering the total mass of AC and 20 µm Zn anode (Fig. 6f).

### Investigation on the interfacial ion movement mechanism

On the basis of previous simulation results14,26,27 and our experimental results, we investigated the interfacial ion movement mechanism at the ion-oligomer nanolayer adsorbed on the electrode. Without the ion-oligomer adsorption layer, the high Da value leads to dendrite growth by physical and hydrodynamic instability at high current densities (Fig. 1a). Simulation results show that a viscoelastic polymer coating layer14,26,27 can regulate the interfacial ion movement by lowering Da (≤0.0025). With a small Da, the interfacial ion movement velocity (Vx and Vy) can be regulated as mentioned before and smooth electrodeposition can be achieved. However, considering the mechanical stability of the viscoelastic polymer coating layer, the stagnant coating layer is not suitable for long-term battery cycling. Here, the small Da of “self-healing” dynamic ion-oligomer adsorption layer in ZnBr2 + PEG300 (Da ≈ 0.0033) and ZnI2+ PEG300 (Da ≈ 0.0028) electrolytes indicate the interfacial ion movement regulation effect also exists here (Fig. 1b). To prove such an effect, we firstly obtained different i–v curves at different concentrations in these four Zn salts (Supplementary Fig. 14). The voltage stability window ΔV extracted from the i–v curve is consistent with the bonding effect and the intensity of the ion-oligomer adsorption layer, proving that the ion movement is influenced by the ion-oligomer adsorption layer (detailed explanation see Supplementary Note 1).

Furthermore, if the ion movement regulation effect can work well for the Zn anode, the same kind of influence can also work on the intercalation/ de-intercalation cathode at high current density (Fig. 1c). Generally, high current density leads to much more serious problems including electrochemical and hydrodynamic instability for intercalation/de-intercalation cathode materials. Hence, we choose layered MnO2 cathode40 (Supplementary Fig. 21) and ZnBr2 + PEG electrolyte here. The same intermittent charging method for Zn||MnO2 full cell is applied here: charging 10 s at 160 mA cm−2, resting 10 s, and then charging another 10 s. The voltage–capacity curve and X-ray diffraction experiments (Fig. 7a, b) show that without regulation of polymer, Zn2+ is hard to be extracted from MnO2 cathode at super high current density, which should be the main reason that the MnO2 is unable to discharge at blank ZnBr2 electrolyte. However, as shown in Fig. 7c, a slight voltage increase can be observed in both charging stages, demonstrating a potential voltage plateau, while the voltage drop during the 10-s rest is minimal, demonstrating stability. On the other hand, during the discharging process, a stable discharge plateau at 8 mA cm−2 proves the ion movement at cathode sides can also be regulated by the ion-oligomer adsorption layer (Supplementary Fig. 22 and Fig. 7d). Considering the simplicity and effectiveness of the approach, we wondered whether it could be used to enable fast charging of non-aqueous Li-based batteries. Supplementary Fig. 23 reports results showing that the concept is effective for lithium-iodine cells. Specifically, we find that Li||I2 cell that use LiI and 1% PEG300 in a DOL-based electrolyte, can be charged at current densities as high as 40 mA cm−2 (Supplementary Fig. 23a). Compared with the electrolyte systems without PEG300 additive (Supplementary Fig. 23b), the LiI + 1% PEG additive can well stabilize the lithium electrodeposition and lead to high Coulombic efficiency (93%) in Li||I2 cell over 200 cycles (Supplementary Fig. 23c). However, the results reported still need to be further optimized the ion-oligomer complex and electrolyte solvent for Li. Taken together with the more in-depth results for the Zn system, the Li results nonetheless lead us to conclude that the interfacial ion regulation mechanism achieved by the ion-oligomer nano-adsorption layer is quite versatile.

In summary, we report that controlling the Zn electrodeposition process at high current density (e.g., 160 mA cm−2) can be achieved by an interfacial ion-oligomer interphase with small Damkohler number Da. By designing the Zn2+-halide ion-PEG complex, reversible interfacial ion-oligomer adsorption can meet both the experimental and theoretical requirements (small Da). Small Da indicates that the ion-oligomer adsorption layer can effectively regulate the interfacial ion movement, and this kind of ion regulation effect can be applied to both anode and cathode sides. More importantly, a highly reversible Zn anode at a high current density of 160 mA cm−2 enables the fast-charge aqueous coin cell with noticeable stability (160 mA cm−2, 12,000 cycles) and fast-charge pouch cell with good cycling performance (56 mA cm−2, over 100 cycles) (Supplementary Fig. 24). Finally, we perform initial proof of concept studies to show that the findings are also relevant for achieving reversible, fast charge characteristics at reactive metal electrodes like Li tested in non-aqueous electrolyte environment.

## Methods

### Materials

ZnSO4·7H2O, ZnCl2, ZnBr2, ZnI2, Polyethylene glycol 300 (PEG300) and Deuterium oxide (D2O, ≥99.96%) were purchased from Sigma-Aldrich. In all, 0.25 mm Zn foil (99.994%) was bought from Alfa Aesar; 0.1 mm Zinc foil (99.999%), AC, DOL, LiNO3, LiTFSI and LiI were bought from Sigma. Chemicals are used as-is without any modifications. For 20-μm Zinc foil, 0.1 mm Zinc foil was rolled many times until reaching the desired thickness. Deionized water was obtained from Milli-Q water purification system. The resistivity of the deionized water is 18.2 MΩ cm−1 at room temperature. ZnSO4·7H2O, ZnCl2, ZnBr2 and ZnI2 were dissolved in deionized water to prepare 0.05 M, 0.5 M, 1 M electrolyte, respectively. Free-standing interwoven carbon fibers (Plain carbon cloth 1071 HCB) were purchased from Fuel Cell Store.

### Preparation of electrolytes

For electrodeposition and cell performance characterization, ZnSO4·7H2O, ZnCl2, ZnBr2 and ZnI2 were dissolved in deionized water to prepare 1 M electrolyte, respectively. 5 wt.% PEG300 was added to the 1 M ZnCl2, ZnBr2 and ZnI2 electrolyte, respectively to created ZnX2 (X = Cl, Br, I) polymer electrolyte.

For Li-containing non-aqueous electrolyte solution, 2 M LiTFSI, 0.5 M LiNO3 and 1 M LiI were added to the DOL solvent. For polymer-containing electrolyte, 1 wt% PEG400 was added.

### Electrochemical measurements

Galvanostatic charge/discharge performance of coin cells were tested on Neware battery test systems at room temperature (25 ± 1 °C). No climatic/environmental chamber was used. Electrochemical studies were performed using CR2032 coin cells. The area of electrodes in this study is 0.3175 cm2. Half cells were assembled with 0.25 mm Zn foil and carbon cloth and separated by a glass fiber (GF/A, WHA1821047, thickness 0.68 mm, pore size 1 μm). In each coil cell, ~100 μL electrolyte was added by pipette.

In the Zn||I2-AC coin cell, the electrolyte was 1 M ZnI2 with/without 5 wt.% PEG300. The cathode is prepared by mixing AC, Super P carbon and polyvinylidene fluoride at a weight ratio 8:1:1. The mass loading of AC is 5 mg cm−2. In the Zn||MnO2 coin cell, α-MnO2 was synthesized via a conventional hydrothermal route, in which a solution that contains 5 mM KMnO4 and 0.3 M HCl was kept at 140 °C for 18 h. All coin cells were assembled at the air.

For pouch cell, 20-μm zinc foil was assembled with cathode materials and separated by a Celgard 3501 membrane. Single-layer electrode was used in pouch cell. The area of the electrode is 9 cm2. The pouch cells were assembled in Ar-filled glovebox. The specific energy of pouch cell was calculated by:

$${{{{{{\rm{Specific}}}}}}}\,{{{{{{\rm{energy}}}}}}}\,\left({{{{{{\rm{Wh}}}}}}}\,{{{{{{{\rm{kg}}}}}}}}^{{{{{{\rm{-}}}}}}1}\right)=\frac{{{{{{{\rm{Average}}}}}}}\,{{{{{{\rm{discharge}}}}}}}\,{{{{{{\rm{voltage}}}}}}}\ \left(V\right)\times {{{{{{\rm{discharge}}}}}}}\,{{{{{{\rm{capacity}}}}}}}({Ah})}{{{{{{{\rm{Total}}}}}}}\,{{{{{{\rm{mass}}}}}}}\,({{{{{{\rm{kg}}}}}}},\,{{{{{{\rm{active}}}}}}}\,{{{{{{\rm{materials}}}}}}}\,{{{{{{\rm{on}}}}}}}\,{{{{{{\rm{cathode}}}}}}}\,{{{{{{\rm{side}}}}}}}+{{{{{{\rm{Zn}}}}}}}\,{{{{{{\rm{anode}}}}}}})}$$

For Li||I2-AC cell, all procedures are the same as Zn||I2-AC cell. The electrolyte is DOL + 2 M LiTFSI + 2 M LiI + 0.5 M LiNO3 + 1% PEG400 and the membrane is Celgard 2400. The cathode side is AC. The Li||I2-AC cell was assembled in Ar-filled glovebox.

EIS measurements was performed using a Solartron in a frequency range from 50 to 1 HZ with an AC polarization of 10 mV. The measurements used two-electrode zinc symmetric cells. Overall, 56 points were collected for each test. Before carrying out the EIS measurement, the open-circuit voltage–time applied was 2 h.

For i–v curve, a three-electrode system, including a working electrode made of glassy carbon, a counter electrode made of zinc foils and a reference electrode (AgCl/Ag), was used to measure the i–v curve of these four zinc salts electrolyte with various concentration (0.05 M, 0.5 M and 1 M). The glassy carbon electrode was purchased from Pine Research. The scan rate of all experiments is 5 mV s−1. Limiting current can be extracted from the i–v curve. During the scanning process, no bubbling is observable near the working electrode, which is attributable to the sluggish kinetics of the H2 evolution reaction in this system.

Exchange current: cyclic voltammetry was performed using a CHI 600E electrochemical workstation and symmetrical zinc cells, in which the glass fiber is used as a separator. Tafel plots of 1 M ZnSO4 and various ZnX2 aqueous electrolytes derived from cyclic voltammetry measurements with a scan rate of 0.2 V s−1. Exchange current density calculated from the Tafel plots.

### Characterization of materials

For 1H NMR sample preparation, 25 µL PEG300 was first diluted in 500 µL D2O, and then desired amount of ZnSO4·7H2O, ZnCl2, ZnBr2 and ZnI2 were slowly dissolved in this solution. Various amount of ZnSO4·7H2O, ZnCl2, ZnBr2 and ZnI2 were added in 500 µL D2O with 25 µL PEG300 solution to prepared 0.1 M, 0.5 M, 1 M, 1.5 M, 2 M and 4 M ZnI2 polymer electrolytes.

For Ellipsometer experiments, a silicon wafer with a 2 × 2 cm2 area was used. For each silicon wafer, we tested three points and get the average thickness. For each kind of electrolyte, we tested three samples (three silicon wafers), which means totally we tested nine times for the PEG adsorption thickness and then extracted the average value.

Field-emission scanning electron microscopy was carried out on Zeiss Gemini 500 Scanning Electron Microscope equipped with Bruker energy dispersive spectroscopy detector to study the electrodeposition morphology of Zn. NMR 1H spectra were collected on a Bruker AVIIIHD (H, 500 MHz) spectrometer with a broad band Prodigy cryoprobe and referenced to D2O solvent shifts (D2O = 4.78 ppm). Linear sweep voltammetry was performed using a CH 600E electrochemical workstation. Impedance measurements of all electrolytes were measured using frequency–domain dielectric relaxation measurements in the range 107–10−1 Hz using a Novocontrol Broadband dielectric spectrometer. ATR-FTIR spectra were conducted using a Thermo Scientific spectrometer. Renishaw inVia confocal Raman microscope is used for Raman tests of electrolytes (excitation wave-length: 785 nm).

QCM-D measurements were performed with Q-sense Explorer system (Biolin Scientific AB) at 25 °C. Fundamental frequency and three harmonics (third, fifth and seventh) were recorded simultaneously along with the corresponding dissipation factors. Gold coated AT-cut quartz crystal (fundamental frequency ~4.95 MHz) was purchased from Q-sense (QX301). Before the experiment, the crystal was cleaned by immersing in 5:1:1 solution of water, ammonia (25%) and hydrogen peroxide (30%) for 5 min at 75 °C, followed by thorough rinsing with deionized water. The crystal was subsequently dried with nitrogen gas and finally UV treated for 10 min in UV/Ozone ProcleanerTM (Bioforce, Nanosciences). 1 M ZnSO4 and Zn halide solution was used as the buffer solution and a stable baseline was obtained before switching to 1 M ZnSO4 and Zn halide solution + 5 wt% PEG300 solution. The data obtained from QCM-D was modeled using the Q-tools software (Q-sense). “Voigt” viscoelastic model was used to model third, fifth and seventh harmonics. This model assumes a homogeneous adsorbed layer. Fluid density and viscosity were taken to be 1638 kg m−3 and 0.001 kg ms−1, respectively. The density of the adsorbed layer was assumed to be 1125 kg m−3 (which is the density of the PEG300) for calculating viscoelastic properties. Descending incremental fitting was used. Direct measurement of ion-oligomer complex adsorption thickness was performed at ALPHA-SE ELLIPSOMETER. The data were collected through three angles (65°, 70°, 75°) and ten different adsorption sites of the silicon wafer, and then get the average adsorption thickness of different PEG300+ Zn salts electrolytes.

#### First-principles calculations

The bond formation of PEG-Zn-halide complexes was studied by ab initio quantum chemistry calculations using the General Atomic and Molecular Electronic Structure System (GAMESS-US), version 2019 R1 patch 1. All calculations were based on the restricted Hartree–Fork method, with a non-SMD solvation model of water (ε = 78.3553) and a gradient convergence tolerance of 0.0001 Hartree Bohr–1. An example of our GAMESS header can be found below. The initial geometries of the ZnXn (H2 O)m−n complexes were individually constructed in Avogadro ver1.2.0 and then optimized in GAMESS using a 6-31G** basis set assuming the atomic radius of Zn is 1.39 Å. Together with a linear PEG molecule and five free water molecules, each ZnXn (H2 O)m−n complex structure was further optimized in GAMESS using the same parameter settings. The degree of polymerization of PEG was chosen to be 5-unit to resemble the molecular weight used in the experiment (~300 g mol−1). After convergence, the bond lengths and bond angles were obtained from the equilibrium structure. HOMO and LUMO energy extracted from the ab initio model.

$SYSTEM MWORDS = 125$END

$PCMCAV RIN(1) = 1.39$END

$PCM SOLVNT = WATER$END

$BASIS GBASIS = N31 NGAUSS = 6 NDFUNC = 1 NPFUNC = 1$END

$CONTRL SCFTYP = RHF RUNTYP = OPTIMIZE ICHARG = −2 MAXIT = 100$END

$STATPT OPTTOL = 0.0001 NSTEP = 1000$END

$SCF DIRSCF = .T.$END