Aqueous zinc battery

Aqueous zinc battery DEFAULT

A chemically self-charging aqueous zinc-ion battery


Self-charging power systems integrating energy harvesting technologies and batteries are attracting extensive attention in energy technologies. However, the conventional integrated systems are highly dependent on the availability of the energy sources and generally possess complicated configuration. Herein, we develop chemically self-charging aqueous zinc-ion batteries with a simplified two-electrode configuration based on CaV6O16·3H2O electrode. Such system possesses the capability of energy harvesting, conversion and storage simultaneously. It can be chemically self-recharged by the spontaneous redox reaction between the discharged cathode and oxygen from the ambient environment. Chemically self-recharged zinc-ion batteries display an initial open-circuit voltage of about 1.05 V and a considerable discharge capacity of about 239 mAh g−1, indicating the excellent self-rechargeability. Impressively, such chemically self-charging zinc-ion batteries can also work well at chemical or/and galvanostatic charging hybrid modes. This work not only provides a route to design chemically self-charging energy storage, but also broadens the horizons of aqueous zinc-ion batteries.


Rechargeable batteries are widely used in many fields, such as electric devices and grid-scale energy storage systems1,2,3,4. In general, the commercial batteries are often charged by electrical grid. However, in the harsh environment or remote area, the electrical grid is unavailable, which limits the recharging and reuse of batteries. In order to solve this issue, various energy harvesting technologies, such as photovoltaic devices5,6,7,8,9,10,11, piezoelectric nanogenerators12,13, triboelectric nanogenerators14,15, and thermoelectrics16,17,18, were integrated with batteries into self-charging power systems. However, these systems are highly dependent on the energy resources, which are not always available in some environment or during a certain period of time. Furthermore, the configurations of these integrated systems are usually complicated and many extra components (e.g., photoelectrodes or temperature-sensitive redox couples) are required in comparison with the traditional batteries with two-electrode configuration. Therefore, self-charging power systems that possess simplified configuration and are available in various environments must be considered.

Chemical energy stored in molecules is an available energy source and can be converted into electrical energy through redox reaction19,20,21,22. In this regard, chemical energy of oxygen that is an abundant resource in air is attracting much more attention in the energy conversion and storage devices, such as metal–air batteries. Furthermore, the metal–air batteries can be further integrated with other energy storage devices and charge them23,24. However, in such integrated devices, the metal–air components cannot always compensate the energy consumption of energy storage devices, and they have to be recharged by external power supply to recover when both the metal–air and energy storage components are exhausted23. Therefore, they cannot meet the demand in some case, where the batteries are required to be charged directly by the successive chemical energy conversion of oxygen on their cathodes. Recently, a variety of vanadium-based compounds have been developed to serve as the cathode materials of aqueous zinc-ion batteries (ZIBs) due to their open-framework crystal structure and multiple oxidation states of vanadium25,26,27,28,29,30. During the discharge process, the insertion of Zn2+ ions and reduction of vanadium occur simultaneously in vanadium-based ZIBs. Furthermore, it is noted that vanadium-based compounds are also active redox materials and can be oxidized by oxygen in low valence state. Therefore, the discharged vanadium-based cathodes would be oxidized by oxygen in the ambient environment, like a charge process. As a result, self-charging ZIBs that simultaneously possess energy conversion and storage functions would be achieved.

Inspired by this, we develop a chemically self-charging aqueous ZIBs system, in which the chemical energy harvesting, conversion, and storage are integrated in a single CaV6O16·3H2O (CaVO) cathode. Such system possesses a similar two-electrode configuration with the conventional ZIBs. It can harvest energy from ambient environment through spontaneous redox reaction, and then convert chemical energy into electrical energy and store them in ZIBs. Therefore, the resultant ZIBs can be self recharged by directly exposing CaVO cathodes to air without any external power supply. This design would provide a promising research direction for the next-generation self-powered systems.


Preparation and characterization of CaVO nanoribbons

The CaVO nanoribbons were synthesized via a one-step hydrothermal method31. They display a size of several hundred micrometers in length and 200–500 nm in width (Fig. 1a, d). Their crystalline phase was further understood by X-ray diffraction (XRD) and the corresponding Rietveld refinement, as shown in Fig. 1b. The results show that the diffraction peaks can be well indexed to the monoclinic CaVO phase with space group of A2/m (JCPDS 33-317) and lattice parameters of a = 12.2533 Å, b = 3.5149 Å, c = 18.3874 Å, α = γ = 90.0°, and β = 118.642°. Thermogravimetric analysis (TGA) also confirms that three molecular waters exist in a formula unit (Supplementary Fig. 1, Supplementary Note 1). Furthermore, it is noted that the XRD pattern exhibits multiple (00l) reflections and the intensity of (002) reflection is extremely strong. It suggests that CaVO nanoribbons possess a typical layered structure, which is constructed by the stacking of V6O16 framework and the hydrated Ca atoms act as “pillars” between the V6O16 layers to stabilize the layered structure (Fig. 1c)32,33. In addition, the lattice fringes with d-spacing of 0.205 nm is observed in the high-resolution transmission electron microscopy (HRTEM) image, corresponding to the (008) plane of CaVO (Fig. 1e), which is in good agreement with the XRD result. Moreover, the transmission electron microscopy (TEM) elemental mapping images clearly show that Ca, V, and O element are homogeneously distributed in CaVO nanoribbons (Fig. 1f).

a SEM image. b Rietveld refinement of the XRD pattern. c Crystal structure. d TEM image. e HRTEM image. f TEM elemental mapping images. Scale bars: a 10 μm; d 1 μm; e 3 nm; and f 400 nm.

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Electrochemical performance of Zn/CaVO batteries

The favorable morphological features, open framework and expanded interlayer spacing (0.819 nm) would contribute to the fast kinetics of Zn2+ ions insertion/extraction in CaVO (refs. 26,34,35,36), thereby enhancing their electrochemical performance. The electrochemical performance of CaVO nanoribbons was investigated in coin cells. In their cyclic voltammetry (CV) curves, there are two pairs of reduction/oxidation peaks at 0.75/0.95 and 0.47/0.66 V (Fig. 2a). They can be ascribed to a two-step redox reaction associated with Zn2+ ion insertion/extraction (corresponding analysis see the following energy storage mechanism section), corresponding to the valence change of vanadium from V5+ to V4+ and V4+ to V3+, respectively26,37,38. Furthermore, the CV curves display similar shape after first cycle, suggesting the high reversibility of the charge/discharge process of Zn/CaVO batteries, which is further confirmed by the reversible galvanostatic charge/discharge (GCD) profiles (Fig. 2b). Besides, Zn/CaVO batteries deliver a high initial discharge capacity of 300 mA h g−1 at 0.1 A g−1 and an average operating voltage of ~0.7 V versus Zn2+/Zn, corresponding to an insertion of ~3.6 Zn per unit formula of CaVO. Impressively, even the current density is up to 30 A g−1, a capacity of 62 mAh g−1 is still achieved (Fig. 2c). When the current density recovers from 30 to 0.2 A g−1 after 70 cycles, the capacity is able to recover to the initial capacity of ~290 mAh g−1. Such excellent rate capability of Zn/CaVO batteries significantly depends on their electrochemical kinetics, as suggested by CV measurements at different scan rates (see Supplementary Fig. 2 and detailed calculation in Supplementary Note 2). The high surface-controlled capacity contributions result in the fast Zn2+ ion diffusion, enabling the high rate capability as well as outstanding cycling stability39,40,41,42. The capacity of Zn/CaVO batteries is still 263 mAh g−1 after 100 cycles at 0.5 A g−1 (Supplementary Fig. 3). Impressively, even after 10,000 cycles at a high current density of 10 A g−1, there is no degradation in their capacity, remaining stable at ~170 mA h g−1 (Fig. 2d). During initial 200 cycles, the capacity is gradually increased, which is attributed to the activation of CaVO at a high current density of 10 A g−1 (refs. 43,44).

a CV curves at 0.1 mV s−1. b GCD curves at 0.1 A g−1. c Rate capability at various current densities. d Cycling performance at 10 A g−1. e In situ XRD patterns of (002) reflection and corresponding GCD curves at 0.2 A g−1 during the first cycle. f XPS spectra of Zn 2p at initial, fully discharged, and charged states. g V K-edge XANES curves at initial, fully discharged, and charged states with reference to the standard V2O3, VO2, and V2O5.

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Energy storage mechanism of Zn/CaVO batteries

The fast reaction kinetics and excellent electrochemical performance depend on the energy storage mechanism of Zn/CaVO batteries. To further understand the energy storage mechanism of Zn/CaVO system, various measurements, including in situ/ex situ XRD, ex situ TEM, X-ray photoelectron spectrometry (XPS) and X-ray absorption near-edge spectroscopy (XANES) were utilized to characterize the CaVO cathodes at the selected states of charge/discharge process. It is noted that the XRD characteristic diffraction peaks of (002) and (004) plane shift slightly toward high degree during the discharge process, corresponding to the decrease of interlayer spacing (Fig. 2e, Supplementary Figs. 4 and 5). It is ascribed to the strong electrostatic interaction between intercalated Zn2+ ions and V6O16 layers38,45. In contrast, the (\(\bar{2}06\)) reflection shifts slightly toward low degree, corresponding to the expansion of the interlayer spacing of (\(\bar{2}06\)) plane, which could arise from the reduction of V5+/V4+ upon Zn2+ ion insertion and the resultant increase in the V–V bond distance between the layers43. Furthermore, the disorder in structure caused by Zn2+ ion insertion would result in the broadening of (\(\bar{2}06\)) and (006) reflections. Reversibly, during the subsequent charge process, these characteristic diffraction peaks gradually return to their original state with the extraction of Zn2+ ions. This reversible change of interlayer spacing is also confirmed by the HRTEM images (Supplementary Fig. 6). Therefore, the energy storage mechanism of Zn/CaVO batteries is the insertion/extraction of Zn2+ ions into/from the CaVO (Supplementary Fig. 7, Supplementary Note 3), which is similar to the case of conventional ZIBs (refs. 30,46). Moreover, this Zn2+ ion insertion/extraction mechanism is further substantiated by the XPS analysis of Zn 2p peaks (Fig. 2f). The peaks of Zn 2p are not detected in the initial CaVO cathode, whereas strong peaks are observed at the fully discharged state, corresponding to the intercalated Zn2+ ions. In contrast, at the fully charged state, the intensity of Zn 2p peaks is significantly weakened, suggesting that most of Zn2+ ions are extracted from the CaVO. It is also proved by TEM elemental mapping images, where Zn element is uniformly distributed in the nanoribbons at fully discharged state and then almost disappears at fully charged state (Supplementary Fig. 8). The insertion/extraction of Zn2+ ions is accompanied by the valence change of vanadium in CaVO, as illustrated in V K-edge XANES curves of CaVO cathodes at different charge/discharge states (Fig. 2g). Compared with the initial state, the main absorption edge slightly shifts toward lower binding energy at fully discharged state, suggesting that the average oxidation state of vanadium is reduced due to the insertion of Zn2+ ions47,48,49. Subsequently, the position of absorption edge reversibly shifts back toward higher energy at fully charged state, indicating the oxidation of vanadium caused by the extraction of Zn2+ ions from CaVO. The above insertion/extraction of Zn2+ ions during the charge/discharge process can also be reflected by the reversible intensity change of pre-edge peak in XANES (Fig. 2g), which is sensitive to the change of the local symmetry of V atoms50.

Based on the above results and discussion, the overall electrochemical reaction of the Zn/CaVO batteries can be described as follows:


$${\mathrm{CaV}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}} + 3.6{\mathrm{Zn}}^{2 +} + 7.2e^ - \leftrightarrow {\mathrm{CaZn}}_{3.6}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}}$$



$$3.6{\mathrm{Zn}} \leftrightarrow 3.6{\mathrm{Zn}}^{2 + } + 7.2e^ -$$



$${\mathrm{CaV}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}} + 3.6{\mathrm{Zn}} \leftrightarrow {\mathrm{CaZn}}_{3.6}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}}$$


Chemically self-charging mechanism

The CaVO cathodes exhibit excellent Zn2+ ion storage performance, and the reduction/oxidation of vanadium occurs during the Zn2+ ion insertion/extraction. In the galvanostatic charging process, electrons are released from the CaZn3.6V6O16·3H2O (CaZn3.6VO) cathode. As a result, vanadium in CaZn3.6VO is oxidized and the Zn2+ ions are extracted from the layered structure simultaneously. In this process, the driving force of the release of electron from CaZn3.6VO is generally the external power supply. In addition to above-mentioned electrochemical oxidation reaction, other strategies that can realize the electron transfer from CaZn3.6VO would be also promising to carry out the charging process of the ZIBs based on CaZn3.6VO cathode. It is well known that redox reaction is an effective and straightforward approach to realize the electron transfer, which is driven by the redox potential difference (ΔE) between reactants51,52. In the case of CaZn3.6VO, the redox potential in this system can be obtained from the CV curves of Zn/CaVO batteries (Fig. 2a)53, in which the minimum reduction peak potential of CaVO versus Zn2+/Zn is 0.47 V. According to the Nernst equation, the calculated redox potential of CaZn3.6VO is −0.27 V versus standard hydrogen electrode (SHE). Theoretically, CaZn3.6VO can be oxidized spontaneously by the oxidants with a higher potential than −0.27 V versus SHE. Among various oxidants, O2 is common and abundant in the air, the standard electrode potentials (Eθ) of which are ~0.40 V and ~1.23 V versus SHE in the neutral and acidic medium, respectively. Owing to the difference in redox potential between O2 and CaZn3.6VO, the CaZn3.6VO tends to release electrons to be oxidized and O2 can accept these electrons to be reduced simultaneously (Fig. 3a). Therefore, if the redox reaction between CaZn3.6VO and O2 could take place, the oxidation of vanadium in CaZn3.6VO would be realized, and the Zn2+ ions would be extracted from the layered structure to balance the charge at the same time. As a result, the fully discharged product CaZn3.6VO would recover to its charged states CaZn3.6−xV6O16·3H2O (CaZn3.6−xVO) without any external power supply. In the Zn/CaVO batteries, acidic 4 M Zn(CF3SO3)2 electrolyte was used. In an open device, O2 could be dissolved into such electrolyte and imported to the discharged product CaZn3.6VO, realizing the redox reaction between CaZn3.6VO and O2. In order to validate the spontaneity of the redox reactions between CaZn3.6VO and O2 in the acidic 4 M Zn(CF3SO3)2 electrolyte, we designed a galvanic cell54,55

$$( - ){\mathrm{CaZn}}_{3.6}{\mathrm{VO}}|{\mathrm{CaZn}}_{3.6 - {\mathrm{x}}}{\mathrm{VO}}||{\mathrm{H}}_2{\mathrm{O}}|{\mathrm{O}}_2|{\mathrm{Pt}}( + )$$

a Energy level transition diagram of CaZn3.6VO and O2. b Optical image of the designed galvanic cell. c V 2p XPS spectra of the CaVO electrodes at different states and the CaZn3.6VO electrodes after being oxidized by O2 in 4 M Zn (CF3SO3)2 solution for different times. d Comparison of XPS spectra of V 2p before and after oxidation. e XRD patterns and f calculational interlayer spacing of (002) plane of CaZn3.6VO electrodes after being oxidized by O2 for different times.

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As shown in Fig. 3b, the CaZn3.6VO electrode served as anode, which was in 4 M Zn(CF3SO3)2 electrolyte without the dissolved oxygen and sealed under Ar. The platinum wire was used as cathode, which was immersed in 4 M Zn(CF3SO3)2 solution containing dissolved oxygen. In this system, a cell voltage of 0.38 V was observed. According to the relationship between thermodynamic function and cell voltage:

where, ΔG, F, and E are the free energy change, Faraday constant, and cell voltage, respectively, the free energy change is less than zero in this case, suggesting that the redox reaction between CaZn3.6VO and O2 can take place spontaneously in 4 M zinc trifluoromethanesulfonate (Zn (CF3SO3)2) solution at ambient condition.

To gain insight into the process of such redox reaction, various ex situ characterizations were carried out to investigate the structure and composition evolution of CaZn3.6VO electrodes that were immersed in 4 M Zn (CF3SO3)2 to react with the dissolved oxygen for different times. With the extension of immersion time from 0 (fully discharged state) to 36 h, the V 2p peak in the XPS spectra gradually shifts toward higher binding energy (Fig. 3c), where the intensity of V5+ peak is significantly enhanced and V3+ peak disappears in comparison with those of initial CaZn3.6VO (Fig. 3d), suggesting the oxidation of vanadium in CaZn3.6VO during the redox reaction process. Simultaneously, to balance the charge of CaZn3.6VO, the intercalated Zn2+ ions are extracted from the layered structure, resulting in the increase of the interlayer spacing of CaZn3.6VO, as proved by the XRD pattern. Furthermore, it is worth noting that the amount of extracted Zn2+ ions of CaZn3.6VO can be effectively controlled by varying the oxidation time in this system. The (002) reflection of oxidized CaZn3.6VO gradually shifts toward lower degree with the extension of oxidation time (Fig. 3e, Supplementary Figs. 5 and 9, Supplementary Note 4). According to the Bragg equation (2dsinθ = , n = 1, λ = 0.154 nm), the interlayer spacing of (002) plane is calculated and increases from 7.75 to 8.10 Å after oxidation for 42 h (Fig. 3f). In addition, it is noted that V 2p XPS spectra and the (002) reflection will not further shifts when the oxidation time exceeds 36 h (Fig. 3c, e), suggesting the oxidation of vanadium in CaZn3.6VO and the extraction of Zn2+ ions would be finished within 36 h.

In addition to O2, it is noted that H2O also plays an important role in the redox reaction process. In order to demonstrate this, the CaZn3.6VO electrodes were immersed in acetonitrile containing dissolved oxygen. In the absence of H2O, the oxidation of vanadium is not detected in the resultant CaZn3.6VO, as reflected by the V 2p XPS spectra, where V 2p region remains unchanged in comparison with that of the initial CaZn3.6VO (Supplementary Fig. 10). Furthermore, there is no shift in the XRD characteristic peak of the resultant CaZn3.6VO (Supplementary Fig. 11), indicating that the Zn2+ ions are not extracted from the CaZn3.6VO. Clearly, the redox reaction between CaZn3.6VO and O2 cannot take place in the absence of H2O. In case of the neutral aqueous solution, the redox reaction between CaZn3.6VO and O2 can also occur (Supplementary Figs. 12–16, Supplementary Notes 5 and 6), where O2 accepts the electrons from CaZn3.6VO and reacts with H2O to form OH. The generated OH and extracted Zn2+ ions combine with the adsorbed electrolyte ions (Zn2+ and CF3SO3) to form amorphous triflate containing layered double hydroxide Znx+y(CF3SO3)2y(OH) (see Supplementary Figs. 17–22 and discussion in Supplementary Notes 7–10)37,44,56,57. Based on the above discussion, in the neutral deionized water, the redox reaction between CaZn3.6VO and O2 can be summarized as below:

$$\begin{array}{l}{\mathrm{CaZn}}_{3.6}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}} + x/2{\mathrm{O}}_2 + x{\mathrm{H}}_2{\mathrm{O}} + y{\mathrm{Zn}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_2 \to \\ {\mathrm{CaZn}}_{3.6 - {\mathrm{x}}}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot {\mathrm{3}}{\mathrm{H}}_2{\mathrm{O}} + {\mathrm{Zn}}_{{\mathrm{x}} + {\mathrm{y}}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_{{\mathrm{2y}}}{\mathrm{(OH)}}_{2{\mathrm{x}}}\end{array}$$


Different from the case in neutral deionized water, in the acidic 4 M Zn(CF3SO3)2 electrolyte, O2 is reduced to H2O in the presence of H+ ions, and the CaZn3.6VO is oxidized along with the extraction of Zn2+ ions. The redox reaction mechanism can be expressed by the following half-cell reactions:

$${\mathrm{CaZn}}_{3.6}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot {\mathrm{3}}{\mathrm{H}}_2{\mathrm{O}} \to {\mathrm{CaZn}}_{3.6 - {\mathrm{x}}}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}}\\ + x{\mathrm{Zn}}^{2 + } + 2xe^ -$$


$$x/2{\mathrm{O}}_2 + 2x{\mathrm{H}}^ + + 2xe^ - \to x{\mathrm{H}}_2{\mathrm{O}}$$


The continuous consumption of H+ ions promotes the water dissociation, thus producing additional H+ ions and OH ions:

$$2x{\mathrm{H}}_2{\mathrm{O}} \to 2x{\mathrm{H}}^ + + 2{\it{x}}{\mathrm{OH}}^ -$$


The additional H+ ions also participate in the oxygen reduction reaction (O2 + 4 H+ + 4e → 2H2O). The generated OH ions react with electrolyte ions (Zn2+ and CF3SO3) and Zn2+ ions that are extracted from the oxidation reaction of CaZn3.6VO to form Znx+y(CF3SO3)2y(OH)2x on the surface of electrode (Supplementary Figs. 23 and 24):

$$x{\mathrm{Zn}}^{2 + } + y{\mathrm{Zn}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_2 + 2x{\mathrm{OH}}^ - \to {\mathrm{Zn}}_{{\mathrm{x}} + {\mathrm{y}}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_{2{\mathrm{y}}}({\mathrm{OH}})_{2{\mathrm{x}}}$$


The overall reaction can be expressed as:

$${\mathrm{CaZn}}_{3.6}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}} + x/2{\mathrm{O}}_2 + x{\mathrm{H}}_2{\mathrm{O}} + y{\mathrm{Zn}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_2 \to$$

$${\mathrm{CaZn}}_{3.6 - {\mathrm{x}}}{\mathrm{V}}_6{\mathrm{O}}_{16} \cdot 3{\mathrm{H}}_2{\mathrm{O}} + {\mathrm{Zn}}_{{\mathrm{x}} + {\mathrm{y}}}({\mathrm{CF}}_3{\mathrm{SO}}_3)_{2{\mathrm{y}}}{\mathrm{(OH)}}_{2{\mathrm{x}}}$$


Self-charging performance of ZIBs

The oxidation of vanadium and extraction of Zn2+ ions in CaZn3.6VO can spontaneously occur in the 4 M Zn(CF3SO3)2 electrolyte containing dissolved oxygen. Consequently, the fully discharged product CaZn3.6VO can recover to its charged states CaZn3.6−xVO through spontaneous redox reaction, which could be considered as a chemical self-charging process (Fig. 4a). When the oxidized product CaZn3.6−xVO electrode directly act as the cathode of ZIBs, the discharge process will take place due to the Zn2+ ion chemical potential difference between CaZn3.6−xVO cathode and Zn anode, where anodic Zn is dissolved to form Zn2+ ions and then intercalate into the CaZn3.6−xVO cathode (Fig. 4b)51. Simultaneously, electrons flow out of the anode to cathode through the external circuit to maintain electrical neutrality. In order to investigate the electrochemical performance of aqueous ZIBs based on CaZn3.6−xVO cathodes, their galvanostatic discharge curves were measured. The open-circuit voltage (OCV) of the Zn/CaZn3.6−xVO batteries rises continually along with extending the oxidation time of CaZn3.6VO (Fig. 4c, d). It is ascribed to the enhanced electrode potential of CaZn3.6−xVO cathode as a result of the deeper oxidation of vanadium and the extraction of more Zn2+ ions, with the extension of oxidation time. When the CaZn3.6VO is oxidized for 36 and 42 h, the OCV of Zn/CaZn3.6−xVO batteries reaches up to 1.05 and 1.08 V, respectively, which nearly reach to the initial OCV (~1.2 V) of the Zn/CaVO battery. In addition to OCV, the discharge capacity of Zn/CaZn3.6-xVO batteries also depends on the oxidation time of CaZn3.6VO. When the oxidation time is <36 h, the discharge capacity gradually increases with the prolongation of oxidation time and a discharge capacity of 239 mAh g−1 is achieved at 36 h. It is much higher than the case of chemical charging in neutral deionized water (Supplementary Figs. 25 and 26, Supplementary Note 11). However, it is noted that the discharge capacity of Zn/CaZn3.6−xVO batteries degrades when the oxidation time exceeds 36 h, since the increasing Znx+y(CF3SO3)2y(OH)2x would hinder the subsequent insertion of Zn2+ ions. In addition, Zn/CaZn3.6−xVO batteries display high reversibility of such chemical charging/galvanostatic discharging process even at different chemically self-charged states. When the chemical charging time is extended stepwise from 6 to 30 h and then abruptly switched back to 6 h, the corresponding discharge capacity increases from 105.1 to 221.4 mAh g−1 and then returns to 96.4 mAh g−1 (Fig. 4e). During the repeated chemical charging/galvanostatic discharging cycles, CaZn3.6−xVO can be reversibly converted with CaZn3.6VO (Supplementary Fig. 5). Different from CaZn3.6−xVO, the Znx+y(CF3SO3)2y(OH)2x is progressively generated and aggregated on the electrode, which will inevitably increase electrochemical impedance and hinder the insertion of Zn2+ ions during subsequent cycles, resulting in the capacity degradation (Fig. 4f). Importantly, after the electrochemical charging process, most Znx+y(CF3SO3)2y(OH)2x would be decomposed and disappear from the electrode (Supplementary Fig. 27, Supplementary Note 12). Therefore, the chemical-charging ability and capacity will recover to a large extent after the electrochemical charging process. However, it is noted that there is still a capacity decay even after several chemical-recharging/galvanostatic-recharging cycling (Fig. 4f). It could be ascribed to the structural stress generated from continuous extraction/insertion of Zn2+ ions, during the repeated chemical charging/galvanostatic discharging cycles25,34.

Working mechanism of chemically self-charging ZIBs during a chemical charging and b galvanostatic discharging process. c The galvanostatic discharge curves of Zn/CaZn3.6−xVO batteries at 0.1 A g−1 after the CaZn3.6VO electrodes were oxidized for different times. d Effect of the oxidation time on OCV and discharge capacity of Zn/CaZn3.6−xVO batteries. e Voltage–time curves of the Zn/CaZn3.6−xVO batteries after being chemically charged to different states (dotted lines: chemical charging for different times. Solid lines: galvanostatic discharging at 0.1 A g−1). f Chemical charging/galvanostatic discharging cycling stability of the Zn/CaZn3.6−xVO battery in a voltage window from 0.3 to ~1.05 V.

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According to the redox reaction mechanism, O2 and H2O are essential in the chemical charging process. Considering that water-based electrolyte was utilized in aqueous ZIBs and the Zn anode was stable in ambient air58,59,60, we designed “open” coin-type aqueous ZIBs, where the cathode caps were predrilled with holes to import O2 into electrolyte and then reacted with CaZn3.6VO to realize the chemical charging process in situ. In such chemically self-charging ZIBs, the CaVO cathode simultaneously serves as an electrode for energy conversion and storage. After the batteries were fully discharged, the gas diffusion window was opened to ensure that O2 could continuously diffuse into electrolyte and react with CaZn3.6VO cathode. These “open” coin-type ZIBs still exhibit superior self-rechargeability, as reflected by the repeated chemical charging/galvanostatic discharging cycles (Fig. 5a). Furthermore, the chemical charging/galvanostatic discharging process is also reversible. In addition, such chemically self-charging ZIBs can work at multiple charge/discharge modes. When they are chemically charged, the OCV slowly reaches ~0.77 V (Fig. 5b, Supplementary Fig. 28). After the batteries are exhausted, they can be chemically recharged again. Impressively, when the external power supply is available, the batteries can be galvanostatically recharged from self-charged state (0.77 V) to the fully charged state (1.5 V). Furthermore, it is worth mentioning that the operation of chemical charging process has almost no effect on the subsequent galvanostatic charging/discharging process. Similar GCD behavior is observed after several chemical charging cycles (Fig. 5b, Supplementary Fig. 29), indicating the excellent reusability of these chemically self-charging ZIBs. To demonstrate the feasibility of the resultant chemically self-charging ZIBs via a simple visual cue, two “open” coin-type batteries were connected in series to power a timer. After the batteries were exhausted and then exposed to the air, they could be chemically recharged to light up the liquid crystal display from the timer (Fig. 5c), suggesting their availability as chemically self-charging energy storage devices.

a Repeated chemical charging/galvanostatic discharging cycles of the ZIBs. b Charging/discharging behavior of the ZIBs at chemical or/and galvanostatic charging hybrid modes. c A timer powered by two self-charging ZIBs in series at (left) exhausted and (right) chemically charged states.

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The recharging and reuse of commercial batteries is often limited in the harsh environment or remote area, where electrical grid is unavailable. Therefore, self-charging power systems that integrate energy harvesting devices and batteries together must be considered. The rational design of self-charging power systems mainly depends on the fabrication of innovative electrodes and the construction of simplified device configurations. In our case, the favorable nanoribbon morphology, open framework and expanded interlayer spacing endow CaVO with the fast kinetics of Zn2+ ion insertion/extraction in the layered structure. As a result, Zn/CaVO batteries exhibit a high initial discharge capacity (300 mAh g−1 at 0.1 A g−1), excellent rate performance (62 mAh g−1 at 30 A g−1) and outstanding cycling stability (100% capacity retention after 10,000 cycles). Owing to the redox potential difference between the fully discharged product CaZn3.6VO and O2, the redox reaction between them will occur, where CaZn3.6VO releases electrons to be oxidized and O2 accepts these electrons to be reduced simultaneously. Meanwhile, the Zn2+ ions are extracted from CaZn3.6VO to balance the charge. As a result, the oxidation of vanadium and extraction of the Zn2+ ions take place in CaZn3.6VO during above redox process at ambient condition. Clearly, the fully discharged product CaZn3.6VO recovers to its charged states in such redox process instead of external power. Therefore, Zn/CaZn3.6−xVO system can harvest chemical energy from the ambient environment and convert it to electrical energy stored in batteries through the chemical charging process. They can be self-charged to ~1.05 V without any external power supply and deliver a considerable discharge capacity of ~239 mAh g−1. Furthermore, the chemical charging/galvanostatic discharging process is also reversible in such open battery design. More importantly, chemically self-charging ZIBs are compatible with different chemical or/and galvanostatic charging hybrid modes. Chemically self-charging ability ensures that Zn/CaVO batteries are available at various conditions. It is different from the conventional ZIBs and zinc–air batteries, which are only charged by external power supply. In the case of rechargeable zinc–air battery61, O2 is an oxidant and reduced to OH ions via a reduction reaction at the air electrode during the discharge process. The generated OH ions then migrate to the zinc electrode, forming insoluble zinc oxide (ZnO) at supersaturated Zn(OH)2- 4 concentrations. In its charge process, the OH ions are oxidized to generate O2, which is driven by external power supply. However, in our case, during the discharge process, Zn2+ ions insert into the CaVO, which is a characteristic behavior. In this process, O2 does not participate in the reaction. During the self-charging process, the discharge product CaZn3.6VO will be oxidized by O2 due to the difference in redox potential between O2 and CaZn3.6VO, replacing the electric energy to make the oxidization of discharged product and realizing the self-charging. However, during the chemical charging process, the Zn2+ ions will not be redeposited on the Zn anode and the formation of byproduct Znx+y(CF3SO3)2y(OH)2x will consume Zn2+ ions from the anode irreversibly, limiting the long-term chemical charging/galvanostatic discharging cycling. Significantly, the Znx+y(CF3SO3)2y(OH)2x can be decomposed by a electrochemical charging process and Zn2+ ions could be also redeposited on the Zn anode. This work paves the way for the potential application of ZIBs in self-charging systems, and the chemical charging strategy provides a promising research direction for the self-powered systems.



Ammonium metavanadate (NH4VO3, 99%) and N-methyl-2-pyrrolidone (NMP, 99.5%) were purchased from Aladdin. Sodium dodecyl sulfate (SDS, 99%), and polyvinylidene fluoride (PVDF) were purchased from Sinopharm Chemical Reagent Co., Ltd. Single-walled carbon nanotubes (SWCNTs, P3) were purchased from Carbon Solutions Inc. Zn foil (99.9%) was purchased from Alfa Aesar. Glass fiber (Grade GF/A) was from Whatman. Zn (CF3SO3)2, 97.5% was from J&K Scientific Ltd. The prepared electrolyte was purified before using.

Preparation of CaVO nanoribbons

CaVO nanoribbons were fabricated by a simple hydrothermal method. A total of 117 mg of NH4VO3 was added into 30 mL deionized water and stirred at 80 °C for 20 min to obtain a clear yellowish solution. Meanwhile, 666 mg of CaCl2 and 100 mg SDS were dissolved in another 30 mL deionized water, and stirred at 60 °C for 10 min to achieve a transparent solution. Subsequently, the CaCl2/SDS solution was added into NH4VO3 solution under stirring. Finally, the above mixture solution was transferred into a 100 mL Teflon-lined autoclave and heated at 160 °C for 10 h. After cooling to room temperature, the brownish-red precipitates were washed with deionized water and freeze-dried.

Electrochemical measurement

Electrochemical performance of CaVO nanoribbons was measured in CR2032 coin cells. The cathode was prepared by mixing the CaVO nanoribbons, SWCNTs, and PVDF in a weight ratio of 7:2:1 by NMP. Then, the slurry was coated on stainless-steel meshes and dried at 60 °C for 12 h under vacuum. The mass loading of CaVO in the cathode is ~1 mg cm−2. Commercial glass fiber and zinc foil with a thickness of 30 μm were employed as the separator and anode, respectively. Aqueous 4 M Zn (CF3SO3)2 solution was used as electrolyte since the high-concentration electrolyte would not only alter the solvation and transporting behaviors of cations/anions to enhance stability and kinetics, but also reduce the water activity and water-induced side reactions48,62,63,64. They were assembled into CR2032 coin cells by a traditional method. The GCD tests were performed on a battery test system (LAND CT2001A) with a voltage window of 0.3–1.5 V. CV were measured using an electrochemical workstation (CHI660E) in a voltage window from 0.3 to 1.5 V.

To understand the mechanism of redox reaction between CaZn3.6VO and O2, the Zn/CaVO batteries were discharged to 0.3 V at a current density of 0.1 A g−1. Subsequently, the fully discharged cathodes (CaZn3.6VO) were washed by deionized water and then immersed in 4 M Zn(CF3SO3)2 solution or water for different times to react with the dissolved oxygen. After that, the treated CaZn3.6-xVO cathodes were assembled into coin cells again for the electrochemical performance measurement. In the in situ chemical charging process, the cathode cap was predrilled with a hole to import oxygen. The cell was first sealed with a Kapton membrane, which was subsequently wiped off to enable O2 to pass through the hole. Furthermore, to avoid the excessive volatilization of water from the electrolyte, the chemical charging process was carried out under a high humidity condition (>60%). After self-charging, the cell was sealed again. The specific capacities were calculated based on the mass of the active material CaVO of cathodes.


The morphologies of CaVO nanoribbons and cathodes were characterized via field-emission scanning electron microscopy (SEM, JEOL JSM7500F, 5 kV and Phenom XL, 15 kV). The SEM–energy dispersive spectroscopy (EDS) of the samples are collected with Phenom XL at an acceleration voltage of 15 kV. The microstructure was characterized by TEM (FEI Talos F200X and FEI Talos F200X G2) equipped with EDS mapping at an acceleration voltage of 200 kV. The crystalline structure of samples was determined by XRD (Rigaku SmartLab) with Cu Kα radiation (λ = 0.15405 nm). TGA (Netzsch STA 449 F3 Jupiter analyzer) was carried out in an Ar flow from room temperature to 600 °C at a heating rate of 10 °C min−1. In situ XRD experiments were performed using home-made cells that were designed with Be window for X-ray penetration. XPS (PerkinElmer PHI 1600 ESCA) was used to characterize the composition and surface oxidation state of the electrodes. V K-edge XANES spectra were collected at the beamline 14W1 in Shanghai Synchrotron Radiation Facility. The solid state 1H nuclear magnetic resonance (1H NMR) was taken from a 400 MHz superconducting NMR spectrometer (AVANCE ||| 400).

Data availability

The authors declare that all the relevant data are available within the paper and its Supplementary Information file or from the corresponding author upon reasonable request.


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This work was supported by National Natural Science Foundation of China (51822205, 21573116, and 21875121), Ministry of Science and Technology of China (2017YFA0206701), Ministry of Education of China (B12015), and the Young Thousand Talents Program and Natural Science Foundation of Tianjin (18JCJQJC46300). The authors thank Professor Jun Luo (Center for Electron Microscopy, Institute for New Energy Materials and Low-Carbon Technologies, Tianjin University of Technology) for TEM measurements and Professor Li Song (National Synchrotron Radiation Laboratory, CAS Center for Excellence in Nanoscience University of Science and Technology of China) for help in XANES characterizations. Dedicated to the 100th anniversary of Nankai University.

Author information


  1. Key Laboratory of Advanced Energy Materials Chemistry (Ministry of Education), Renewable Energy Conversion and Storage Center, College of Chemistry, Nankai University, Tianjin, 300071, People’s Republic of China

    Yan Zhang, Fang Wan, Shuo Huang, Shuai Wang, Zhiqiang Niu & Jun Chen


Zinc-ion battery

Battery that uses zinc ions as the charge carriers

A zinc-ion battery or Zn-ion battery (abbreviated as ZIB) uses zincions (Zn2+) as the charge carriers.[1] Specifically, ZIBs utilize Zn as the anode, Zn-intercalating materials as the cathode, and a Zn-containing electrolyte. Generally, the term zinc-ion battery is reserved for rechargeable (secondary) batteries, which are sometimes also referred to as rechargeable zinc metal batteries (RZMB).[2] Thus, ZIBs are different than non-rechargeable (primary) batteries which use zinc, such as alkaline or zinc-carbon batteries.


In 2011, Feiyu Kang's group showcased for the first time the reversible Zn-ion insertion into the tunnel structure of alpha-type manganese dioxide (MnO2) host used as the cathode in a ZIB.[3][4]

The University of Waterloo in Canada owns patent rights to zinc-ion battery technology developed in its laboratories.[5][6]

The Canadian company Salient Energy is commercialising the zinc-ion battery technology. [7]

Eos Energy Storage is producing 1.5GWh of ‘Made in America’ zinc batteries to be used in the Texas and California electric grids.[8][9]


Motivation and issues[edit]

Compared to lithium metal, a zinc negative electrode holds a higher theoretical volumetric capacity and natural abundance. Depending on the ZIB positive electrode, such theoretical advantages may also be present when comparing to lithium-ion batteries (LIBs). Moreover, zinc is more compatible with aqueous electrolytes. However, ZIBs generally show lower Coulombic (charge) efficiency than state of the art LIBs, larger overpotentials for plating and striping on the negative electrode, and the possibility of dendritic failure.[2][10]


Both aqueous and non-aqueous electrolytes are being investigates as candidates for ZIBs. Zinc salts using the TFSI or triflate anions have been considered for both aqueous and non-aqueous electrolytes. Zinc sulfate and alkaline KOH-based aqueous electrolytes have also been considered.[2][10]

Until now, several cathode materials have been explored for ZIBs, including gamma-, delta-type MnO2, copper hexacyanoferrate, bismuth oxide, layer sulfides and Prussian blue analogues.[2][11][12][13] For example, in 2017, researchers reported a prototype zinc-ion battery that has high reversibility, rate, and capacity without dendrite formation.[14] The device used a zinc metal anode, a vanadium oxide cathode (Zn0.25V2O5⋅nH2O) and an aqueous electrolyte, all non-toxic materials. After 1,000 cycles it retained 80% of its capacity. The cell achieved a capacity up to 300  mAh g−1 and an energy density of ∼450  Wh l−1.

See also[edit]


  1. ^"A cheap, long-lasting, sustainable battery for grid energy storage | KurzweilAI". 2016-09-16. Retrieved 2017-02-02.
  2. ^ abcdMa, Lin; Schroeder, Marshall A.; Borodin, Oleg; Pollard, Travis P.; Ding, Michael S.; Wang, Chunsheng; Xu, Kang (2020). "Realizing high zinc reversibility in rechargeable batteries". Nature Energy. 5 (10): 743–749. Bibcode:2020NatEn...5..743M. doi:10.1038/s41560-020-0674-x. ISSN 2058-7546. S2CID 221118342.
  3. ^US 20120034515, Kang, Feiyu; XU, Chengjun & Li, Baohua, "Rechargeable zinc ion battery", published Feb 9, 2012 
  4. ^Xu, Chengjun; Li, Baohua; Du, Hongda; Kang, Feiyu (2012-01-23). "Energetic Zinc Ion Chemistry: The Rechargeable Zinc Ion Battery". Angewandte Chemie International Edition. 51 (4): 933–935. doi:10.1002/anie.201106307. ISSN 1521-3773. PMID 22170816.
  5. ^Kundu, Dipan; Vajargah, Shahrzad Hosseini; Wan, Liwen; Adams, Brian; Prendergast, David; Nazar, Linda F. (April 18, 2018). "Aqueous vs. nonaqueous Zn-ion batteries: consequences of the desolvation penalty at the interface". Energy & Environmental Science. 11 (4): 881–892. doi:10.1039/C8EE00378E. OSTI 1469689 – via
  6. ^
  7. ^"Power up: Halifax's thriving battery scene attracts Ontario startup". Dalhousie News.
  8. ^"Home". Eos Energy Enterprises.
  9. ^"1.5GWh of 'Made in America' zinc batteries joining Texas, California grids from Eos Energy Storage". Energy Storage News. 1 Sep 2020.
  10. ^ abMa, Lin; Schroeder, Marshall A.; Pollard, Travis P.; Borodin, Oleg; Ding, Michael S.; Sun, Ruimin; Cao, Longsheng; Ho, Janet; Baker, David R.; Wang, Chunsheng; Xu, Kang (2020). "Critical Factors Dictating Reversibility of the Zinc Metal Anode". Energy & Environmental Materials. 3 (4): 516–521. doi:10.1002/eem2.12077. ISSN 2575-0356.
  11. ^Alfaruqi, Muhammad H.; Mathew, Vinod; Gim, Jihyeon; Kim, Sungjin; Song, Jinju; Baboo, Joseph P.; Choi, Sun H.; Kim, Jaekook (2015-05-26). "Electrochemically Induced Structural Transformation in a γ-MnO2 Cathode of a High Capacity Zinc-Ion Battery System". Chemistry of Materials. 27 (10): 3609–3620. doi:10.1021/cm504717p. ISSN 0897-4756.
  12. ^Alfaruqi, Muhammad Hilmy; Gim, Jihyeon; Kim, Sungjin; Song, Jinju; Pham, Duong Tung; Jo, Jeonggeun; Xiu, Zhiliang; Mathew, Vinod; Kim, Jaekook (2015). "A layered δ-MnO 2 nanoflake cathode with high zinc-storage capacities for eco-friendly battery applications". Electrochemistry Communications. 60: 121–125. doi:10.1016/j.elecom.2015.08.019.
  13. ^Trócoli, Rafael; La Mantia, Fabio (2015-02-01). "An Aqueous Zinc-Ion Battery Based on Copper Hexacyanoferrate". ChemSusChem. 8 (3): 481–485. doi:10.1002/cssc.201403143. ISSN 1864-564X. PMID 25510850.
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Aqueous zinc ion batteries: focus on zinc metal anodes

J. Shin, J. Lee, Y. Park and J. W. Choi, Chem. Sci., 2020, 11, 2028 DOI: 10.1039/D0SC00022A

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Zinc Ion Battery

Aqueous vs. nonaqueous Zn-ion batteries: consequences of the desolvation penalty at the interface†

Author affiliations

* Corresponding authors

a Department of Chemistry, Waterloo Institute for Nanotechnology, University of Waterloo, 200 University Ave W, Waterloo, Ontario N2L 3G1, Canada
E-mail:[email protected]

b The Molecular Foundry, Lawrence Berkeley National Laboratory, Berkeley, CA 94720, USA

c Joint Center for Energy Storage Research (JCESR), USA


Zinc ion batteries using metallic zinc as the negative electrode have gained considerable interest for electrochemical energy storage, whose development is crucial for the adoption of renewable energy technologies, as zinc has a very high volumetric capacity (5845 mA h cm−3), is inexpensive and compatible with aqueous electrolytes. However, the divalent charge of zinc ions, which restricts the choice of host material due to hindered solid-state diffusion, can also pose a problem for interfacial charge transfer. Here, we report our findings on reversible intercalation of up to two Zn2+ ions in layered V3O7·H2O. This material exhibits very high capacity and power (375 mA h g−1 at a 1C rate, and 275 mA h g−1 at an 8C rate) in an aqueous electrolyte compared to a very low capacity and slow rate capabilities in a nonaqueous medium. Operando XRD studies, together with impedance analysis, reveal solid solution behavior associated with Zn2+-ion diffusion within a water monolayer in the interlayer gap in both systems, but very sluggish interfacial charge transfer in the nonaqueous electrolyte. This points to desolvation at the interface as a major factor in dictating the kinetics. Temperature dependent impedance studies show high activation energies associated with the nonaqueous charge transfer process, identifying the origin of poor electrochemical performance.

Graphical abstract: Aqueous vs. nonaqueous Zn-ion batteries: consequences of the desolvation penalty at the interface

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Article type

04 Feb 2018

19 Feb 2018

First published
19 Feb 2018

Energy Environ. Sci., 2018,11, 881-892

Aqueous vs. nonaqueous Zn-ion batteries: consequences of the desolvation penalty at the interface

D. Kundu, S. Hosseini Vajargah, L. Wan, B. Adams, D. Prendergast and L. F. Nazar, Energy Environ. Sci., 2018, 11, 881 DOI: 10.1039/C8EE00378E

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