Source: https://pubs.rsc.org/en/content/articlehtml/2019/cc/c8cc07243d
Timestamp: 2019-04-19 00:26:23+00:00

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For the first time, CaV6O16·3H2O (CVO), synthesized via a highly efficient and fast microwave reaction, is used as a cathode material for aqueous zinc-ion batteries. Ex situ X-ray diffraction confirms the structure of this material to be stable upon reversible Zn2+ intercalation, due to its large interlayer distance (8.08 Å). The pillaring effect of calcium makes the as-prepared CVO an excellent Zn2+ cation host.
Although rechargeable AZBs are appealing, they are still in their infancy and their development is hindered by the restricted choice of cathode materials that often display limited cycle life, poor rate capability, and structural instability upon multivalent cation insertion. Polyanionic compounds and Prussian blue analogues suffer from low specific capacity, while manganese-based oxides have a short lifespan due to severe manganese dissolution.6 Nazar et al. reported a high-capacity and long-life rechargeable AZB based on Zn0.25V2O5·nH2O.7 Since then, a series of layered vanadium-based oxides and sulfides have been investigated.8 In general, these compounds deliver high specific capacity (>300 mA h g−1) when the composition and morphology are carefully designed. For example, as reported by Pang et al., H2V3O8 nanowires (diameter is 50–100 nm) anchored on the surface of graphene sheets exhibit a high capacity of 394 mA h g−1 at 100 mA g−1.9 The high specific capacity of vanadium oxides compensates for their relatively low operating voltage (around 0.8 V vs. Zn2+/Zn). However, although displaying a better cycling stability than manganese oxides, vanadium oxides still need further improvement to meet the standard of practical use. Previous studies have shown that adopting a suitable metal cation as a pillaring agent can effectively stabilize the vanadium slab, reducing, or even fully avoiding the structural collapse upon Li+ and Na+ intercalation/de-intercalation.10 This strategy was extended to AZBs and, so far, focused on the effect of alkali metal cations (e.g., LiV3O8, Na0.25V2O5, Na2V6O16, KV3O8, K0.25V2O5, K2V6O16, and K2V8O21),11 while the effect of alkaline-earth metal cations was less investigated.
Fig. 1 Summary of the Rietveld refinement of the as-prepared CVO. The experimental data, calculated pattern, difference curve, and Bragg position are shown in red, black, blue, and olive, respectively. The inset shows the crystal structure model projected along .
As seen in Fig. 2a, the as-prepared CVO was composed of uniform fibers longer than 100 μm and with a diameter in the range of hundreds of nanometers. The latter sub-micrometric dimension is certainly beneficial for shortening the solid-state diffusion path of Zn2+.16 Nevertheless, the diameter of the as-prepared CVO is still larger than those of other vanadium oxides reported for AZBs,10 which, as discussed in the following, may affect its electrochemical performance. Additionally, the valence state of vanadium in CVO is 5+, which could result in a high electronic resistance within a single wire.17Fig. 2b shows the EDX elemental mapping of the CVO micro-wires. The distribution of the three elements (Ca, V, and O) in the CVO material was found to be uniform and in good agreement with the secondary electron image taken on the same region. The transmission electron microscopy (TEM) image shown in Fig. 2c further reveals that the fiber is not uniform. Furthermore, the parallel boundaries along the edge indicate that it consists of slabs. The inset displays a typical [0 0] electron diffraction pattern, demonstrating that the fiber is a single crystal with the slabs stacking along the same direction. Finally, the high-resolution TEM (HRTEM) image (Fig. 2d) shows well-developed lattice fringes with an interplanar spacing of 1.08 nm, which is identical to that of the (100) plane of CVO.
Fig. 2 (a) SEM images of the as-prepared CVO. (b) SEM image and the corresponding EDX elemental mapping images of Ca, V, and O. (c) TEM image of the as-prepared CVO and the corresponding electron diffraction pattern. (d) HRTEM image of the as-prepared CVO.
where i is the current, v is the scan rate, and a and b are the adjustable parameters,17 the b values of peaks 1–4 are calculated to be 0.72, 0.75, 0.5 and 0.7, respectively.
Fig. 3 Electrochemical performance of the as-fabricated CVO electrode. (a) CV curve at 0.05 mV s−1. (b) Specific capacity and coulombic efficiency obtained at different current densities. (c) Charge–discharge profiles at different current densities. (d) Specific capacity and coulombic efficiency upon extensive cycling at 500 mA g−1. The first two activation cycles were performed at 50 mA g−1.
Galvanostatic discharge/charge cycles at different current densities are reported in Fig. 3b. In the first cycle at 50 mA g−1, the discharge capacity reached 367 mA h g−1, while the coulombic efficiency was 93.69% and gradually increased upon cycling. Since the size of the microwave synthesized CVO wires was rather large, the diffusion-controlled process is expected to be predominant. Thus, the resulting high specific capacity must result from the large interlayer distance in CVO. The irreversible capacity observed in the first cycle could arise from two possible parasitic reactions involving the reduction of dissolved O2 and the salt anion (CF3SO3−). In fact, although the electrolyte was de-aereated by bubbling N2 in it for one hour, the cell was assembled in an ambient atmosphere, leading to some inevitable O2 in the cell. The reduction of oxygen during the discharge process could consume some electrons and contribute to the irreversible capacity.20 Regarding the salt anion, CF3SO3−, its reduction in concentrated NaCF3SO3 electrolytes has been reported.21 However, the efficiency rapidly increased to 99.72% at the 4th cycle, demonstrating, overall, a good reversibility of the multivalent cation intercalation process. Because of the larger grain size and, possibly, lower electronic conductivity, the specific capacity at high specific current is not superior to those of other reported vanadium oxides, leaving considerable room for optimization. Nevertheless, at a specific current of 1 A g−1, a specific capacity higher than 125 mA h g−1 was achieved. The corresponding charge–discharge curves are shown in Fig. 3c. The plateaus matched well with the redox peaks in Fig. 3a. When the specific current was brought back to 500 mA g−1, the cell recovered its capacity without any loss, implying the integrity of the CVO structure. The evaluation of the long-term cycling is displayed in Fig. 3d. At the 4th cycle, the discharge capacity was 160 mA h g−1, gradually increasing to 170 mA h g−1 and then remaining stable for the whole duration of the test (i.e., 300 cycles). The cell voltage vs. capacity during a few, selected charge–discharge cycles is displayed in Fig. S4 (ESI†).
The electrochemical properties of several cathode materials for AZBs are compared in Table S3 (ESI†). The specific capacity of the as-prepared CVO is much higher than that of polyanionic compounds, Prussian blue analogues, and manganese-based oxides, and it exceeds that of a series of other vanadium-based oxides as well as sulfides. Furthermore, CVO displays excellent capacity retention, e.g., better than most of the reported cathode materials for AZBs.
To investigate the Zn-cation storage mechanism, the ex situ XRD characterization of CVO electrodes was performed. Fig. 4a displays the diffractograms obtained at different states of charge and discharge during the first cycle. The corresponding charge/discharge profile is shown in Fig. 4b. Notably, the initial interlayer distance (7.4 Å) was smaller than that of the pristine powder. This can be attributed to the partial loss of the water molecules intercalated in the interlayer due to the extensive drying process after electrode fabrication. Upon Zn2+ intercalation, the (002) peak gradually shifted to higher degrees, suggesting the decrease of the interlayer distance from the initial value (7.4 Å) to 6.8 Å at the fully intercalated state. This is due to the intercalated Zn2+ cations attracting the adjacent, negatively charged V–O slabs. When Zn2+ was extracted, the (002) peak shifted back to lower degrees. The final interlayer distance was very close to the initial value. This reveals the excellent reversibility of Zn2+ (de-)intercalation in the layered structure of CVO. Interestingly, a set of new peaks, marked by grey boxes in Fig. 4a, appeared during Zn2+ intercalation and disappeared upon Zn2+ release.16 No other peaks evolved at higher angles (Fig. S5, ESI†). It is reasonable to think that these peaks originated from the intercalated Zn2+. To gain more information about the intercalated CVO, SEM and TEM were applied to the fully discharged sample. As shown in Fig. 4c, the fiber-like morphology is retained. The distribution of zinc element matches well with the secondary electron image, indicating the presence of zinc in the intercalated fiber, i.e., confirming the proposed intercalation mechanism. Observing the electron diffraction pattern, one can conclude that the zinc intercalated CVO fiber is a single crystal. The calculated interlayer spacings and the HRTEM image (see Fig. S6, ESI†) imply that the lattice constants have quite large difference after the intercalation of zinc. Considering the regular and reversible shift of the (002) peak during the charge/discharge process, one can infer that the intercalated compound still retains some structural features of pristine CVO. A deep analysis is ongoing to clarify the structural evolutions occurring in the CVO electrode during cell cycling.
Fig. 4 (a) Ex situ XRD patterns of the as-fabricated CVO electrodes at various states of the first cycle, and (b) the corresponding voltage profile. (c) SEM image and the corresponding EDX elemental mapping images of the CVO fiber discharged to 0.2 V. (d) Electron diffraction pattern of the CVO fiber discharged to 0.2 V and the corresponding TEM image of the fiber.
In conclusion, ultra-long CVO micro-wires were obtained with a highly efficient and very fast microwave reaction. Owing to the large interlayer distance and pillaring effect of calcium, the electrode material reversibly intercalated up to 4.5 equivalents of Zn2+ per mole of CVO, delivering high specific capacity with excellent capacity retention. Ex situ XRD measurement confirmed the reversibility of the process, the high structural stability of CVO. Although we can already foresee further optimization of the synthesis conditions (e.g., a decrease of CVO wire diameter, introduce mixed vanadium valence states or electronically conductive materials), CVO prepared by the microwave reaction is a promising cathode for aqueous zinc-ion batteries and a potential host for other multivalent cations.
X. L., H. Z., and J. H. gratefully acknowledge financial support from the China Scholarship Council (CSC). Financial support from the Helmholtz Association is also acknowledged.
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