ORIGINAL RESEARCH article
Volume 7 - 2019 | https://doi.org/10.3389/fchem.2019.00437
Facile Controlled Synthesis of Spinel LiMn2O4 Porous Microspheres as Cathode Material for Lithium Ion Batteries
- 1Beijing Key Laboratory of Materials Utilization of Nonmetallic Minerals and Solid Wastes, School of Materials Science and Technology, China University of Geosciences, Beijing, China
- 2School of Science, China University of Geosciences, Beijing, China
Although the electrochemical properties of porous LiMn2O4 microspheres are usually improved compared to those of irregular LiMn2O4 particles, the effects of the different synthesis conditions on the preparation of the porous LiMn2O4 microspheres are rarely discussed in detail. In the present work, porous LiMn2O4 microspheres were successfully synthesized by using molten LiOH and porous Mn2O3 spheres as a template. Multiple factors were considered in the preparation process, including reagent concentration, pH, adding mode, heating time, etc. The morphology of the MnCO3 template was crucial for the preparation of porous LiMn2O4 microspheres and it was mainly affected by the concentration of reactants and the pH value of the solution during the precipitation process. During the lithiation of Mn2O3 microspheres, the heating temperature and the ratio between Mn2O3 and lithium salt were the most significant variables in terms of control over the morphology and purity of the LiMn2O4 microspheres. Furthermore, we demonstrated that the porous LiMn2O4 microspheres presented better rate capability and cyclability compared to commercial LiMn2O4 powder as cathode materials for lithium-ion batteries (LIBs). This study not only highlights the shape-controllable synthesis of LiMn2O4 microspheres as promising cathode materials, but also provides some useful guidance for the synthesis of porous LiMn2O4 microspheres and other LIB' electrode materials.
With the development of science and technology, lithium-ion batteries (LIBs) have been widely used in various portable energy storage devices (Wakihara, 2001; Etacheri et al., 2011; Chen D. et al., 2018; Chen H. et al., 2018) such as tablets, smartphones, cameras, etc. Further applications in electric vehicles, hybrid vehicles, military, and aerospace have also been developed and explored (Smart et al., 2004; Park et al., 2010; Lu et al., 2013; Lipu et al., 2018). Among various cathode materials for LIBs, LiMn2O4 cathode material with a spinel structure—which is cheap, safe and rich in resources—has become a research hotspot (Lee et al., 2010; Qu et al., 2011; Lai et al., 2016; Zhu et al., 2016; Wang et al., 2018). In long-term charging and discharging, the dissolution of Mn into electrolytes causes capacity degradation and poor cycle performance of cathode materials, which severely restricts the commercial application of LiMn2O4. Various methods have been tried to improve the electrochemical performance of spinel LiMn2O4 cathode materials, including surface coating, bulk doping, and morphology control (Iqbal et al., 2012; Tang et al., 2013; Jeong et al., 2015; Xu et al., 2018). Among these improvements, down-sizing of LiMn2O4 particles can significantly shorten the transport distance of lithium ions in solid, thus helping to improve their rate performance. Therefore, nanostructured LiMn2O4 with various morphologies has been extensively prepared in recent years (Lee et al., 2010; Tang et al., 2012, 2013). Tang et al. (2012) synthesized a nanochain of LiMn2O4 by a sol-gel method with a very good rate capability. The result showed a reversible capacity of 100 mAhg−1 at rate of about 1 C and 58 mAh g−1 at rate of 20 C. Lee et al. (2010) synthesized ultrathin LiMn2O4 nanowires with diameters <10 nm and lengths of several micrometers, which displayed 100 and 78 mAh g−1 at very high rates of 60 and 150 C. Nevertheless, the tap density of the above nanostructured LiMn2O4 is generally low due to its irregular shape, high surface area, and high porosity (Guo et al., 2014), resulting in low volumetric energy density of the LIBs' electrodes. In contrast, the LIBs' electrodes made of sub-micron-sized spherical active materials usually show higher volumetric energy density (Aurbach et al., 1999; Levi et al., 1999; He et al., 2006), which is caused by the compact packing of spherical particles. Additionally, an ideal structure would be a porous microsphere which consists of nanocrystallites tightly compacted with three-dimensional channels for ion diffusion in consideration of electron transportation distance (Qian et al., 2010; Ren et al., 2014; Yin et al., 2019). This structured LiMn2O4 can have both high volumetric energy density and high rate capability simultaneously. For example, Liu et al. (2018) reported the synthesis of the porous LiMn2O4 micro-/nano-hollow spheres from the globe precursor MnCO3 via a facile precipitation route. The obtained LiMn2O4 delivered excellent cycle stability and almost no capacity loss after 200 cycles. Wang et al. (2013) synthesized porous LiMn2O4 spheres with pores at an average size of 45 nm. The discharge capacity of the porous sphere LiMn2O4 was 83 mAh g −1 at a rate of 20 C, which showed stable high-rate capability. Although the previous work has reported the preparation of porous LiMn2O4 microspheres and improvement of their electrochemical properties, the effects of the different synthesis conditions on the LiMn2O4 morphology and size have been rarely discussed in detail.
Herein, we reported the synthesis of spinel LiMn2O4 porous microspheres by lithiation of porous Mn2O3 microspheres. The effects of a series of preparation conditions, including reagent concentration, pH, adding mode, heating time, etc., on the morphology of the LiMn2O4 microspheres were investigated in detail. Moreover, we compared the electrochemical performance of synthesized LiMn2O4 microspheres with that of commercial LiMn2O4 powder. Significantly, without cation doping or surface coating, the porous LiMn2O4 microspheres present better rate capability and cyclability.
Preparation of MnCO3 Microsphere
LiOH·H2O (99.0%, AR) and ethanol (99.7%, AR) were purchased from Aladdin. MnSO4·H2O (99.0%, AR), NH4HCO3 (21.0%, AR), NH3·H2O (25%, AR), and H2SO4 (98.0 wt.%) were supplied by XiLong Chemical Co. Ltd. All reagents were used without further purification. The spherical MnCO3 was first prepared by a general chemical precipitation method. In a typical synthesis, 0.3042 g MnSO4·H2O and 1.4231 g NH4HCO3 were dissolved in 45 mL deionized water and 5 mL ethanol, respectively, to form a transparent solution. After the complete dispersion of the MnSO4 and NH4HCO3 solutions, the NH4HCO3 solution was added to the MnSO4 solution rapidly with vigorous stirring. A certain amount of NH3·H2O (10.0% v/v.) or H2SO4 (10.0% v/v.) was then added dropwise to adjust the pH value of the suspension to 7.5. The milky white suspension was stirred for 3 h at room temperature and maintained for 5 h. The powder was obtained by filtrating, washing, and drying in the air at 80°C for 24 h to obtain spherical MnCO3 precursors.
Preparation of Mn2O3 and LiMn2O4
The as-obtained MnCO3 powders were heated in air at 700°C for 10 h at a heating rate of 10°C·min−1 to synthesize porous Mn2O3 spheres. The porous Mn2O3 spheres were grounded thoroughly with LiOH·H2O in a molar ratio of Mn2O3:LiOH = 1:1.1 using ethanol as a dispersal agent. Finally, the mixtures were calcined at 650°C for 10 h with a heating rate of 5°C·min−1 in the air to achieve porous LiMn2O4 spheres.
X-ray diffraction (XRD) characterization was conducted to identify the crystal structure of the samples on an X-ray powder diffractometer (D8 Advance, Bruker, Germany) with a Cu Kα (λ = 0.15406 Å) radiation. The micro-morphologies of MnCO3, Mn2O3, and LiMn2O4 were observed using scanning electron microscopy (FESEM, MERLIN VP Compact, ZEISS, Germany).
The electrochemical performance was evaluated using CR2032 coin cells assembled in a high-purity argon-filled glove box with the moisture and oxygen content maintained below 0.1 ppm. The working electrode consisted of 70 wt.% LiMn2O4 spheres, 20 wt.% acetylene black and 10 wt.% polyvinylidene fluoride (PVDF) as a binder. Pure lithium foil was used as the counter electrode. The separator was Celgard 2400. The electrolyte was 1.0 M LiPF6 in ethylene carbonate/ethyl methyl carbonate/dimethyl carbonate solvent (1:1:1 v/v/v, Shenzhen Keijing Star Tech. Co.). The cells were aged for 12 h before measurement. All cyclic voltammogram tests were performed on an electrochemical workstation (Ivium-Vertex, Ivium Technologies, Holland). The galvanostatic charge/discharge tests were carried out using a Battery Testing system (CT-4008, NEWARE, China) with a voltage window of 3.0–4.5 V vs. Li+/Li at room temperature.
Results and Discussion
The Synthesis Principle and Process of LiMn2O4 Microspheres
Figure 1 shows the schematic of the preparation of the spinel LiMn2O4 porous microspheres. First, MnCO3 microspheres as precursors are synthesized based on a precipitation method through the reaction of the MnSO4 solution with the NH4HCO3 solution. Secondly, MnCO3 microspheres are subsequently transformed into Mn2O3 microspheres through the decomposition by heating treatment in tube furnace. Finally, LiMn2O4 microspheres are obtained by the lithiation reaction of Mn2O3 porous microspheres with LiOH at high temperature. The influences of the key parameters in each of the above processes on the microstructures and crystallinities of the products are further discussed in detail.
The Effects of Main Preparation Conditions on the Morphology of MnCO3
The first step is to synthesize MnCO3 microspheres successfully, which is a key for the preparation of LiMn2O4 microspheres. We have successfully prepared the MnCO3 microspheres using precipitation. Powder X-ray diffraction analysis of spherical products after the precipitation reaction was employed to identify the crystallographic phase. Figure 2a shows the XRD pattern of the obtained products and the standard pattern of MnCO3. All the diffraction peaks can be indexed to the well-crystallized hexagonal MnCO3 (JCPDS#44-1472). No other impurities can be observed in the XRD pattern. Figures 2b,c displays the SEM images of spherical MnCO3. It is evident that MnCO3 spheres are uniform and monodispersed with rough surface with an average diameter of about 1.0 μm. In addition, we found that the morphology of the MnCO3 was greatly influenced by the preparation conditions during the precipitation. Therefore, we have studied the effects of the main preparation conditions in the precipitation process of the synthesis of MnCO3.
Figure 2. (a) XRD pattern of MnCO3 and the standard pattern of MnCO3 (PDF#44-1472) is shown as reference; (b,c) SEM images of MnCO3 at different magnification. The inset shows the size distribution of these particles.
The Effects of MnSO4 Concentration on the Morphology of MnCO3
The SEM images of MnCO3 prepared at the different concentrations of the MnSO4 solution are shown in Figure 3. During the preparation, the concentration of NH4HCO3 was 0.36 M, and other synthesis conditions were maintained. When the concentration of MnSO4 solution is 0.02 M, the morphology of MnCO3 tends to form more cubes than spheres (Figure 3a). With the increase of the MnSO4 concentration to 0.036 M, their morphology gradually transforms from cubical to spherical shapes (Figure 3b). When the concentration of the MnSO4 solution is higher than 0.10 M, the morphology of MnCO3 becomes an irregular granular shape (Figures 3c,d).
Figure 3. SEM images of MnCO3 prepared at different concentrations of MnSO4 solution. (a) 0.02 M; (b) 0.036 M; (c) 0.10 M; (d) 0.20 M.
The Effects of NH4HCO3 Concentration on the Morphology of MnCO3
Figure 4 shows the SEM images of MnCO3 prepared at different concentrations of the NH4HCO3 solution. During the preparation, the concentration of the MnCO3 solution was 0.036 M, and the other synthesis conditions were maintained. When the NH4HCO3 concentration is 0.09 M, the morphology of MnCO3 is irregular. With the increase of the NH4HCO3 concentration to 0.18 M, the morphology of MnCO3 tends to form spheres. When the concentration of NH4HCO3 is 0.36 M, the MnCO3 spheres own uniform size and good dispersion. The particle size varies from 0.5 to 1.8 μm, mainly in the range of 1.1–1.4 μm, and the average particle size is about 1.0 μm. When the concentration of NH4HCO3 goes higher as 0.54 M, the spherical MnCO3 becomes larger and has a clear agglomeration.
Figure 4. SEM images of MnCO3 prepared at different concentrations of NH4HCO3 solution. (a) 0.09 M; (b) 0.18 M; (c) 0.36 M; (d) 0.54 M. The inset shows the size distribution of these particles.
The Effects of Solution pH on the Morphology of MnCO3
Solution pH proved to be a crucial factor in the controlled formation of the final products (Hong et al., 2003; Kloprogge et al., 2004; Kong et al., 2019; Simon et al., 2019). Herein, the synthesis process in different pH of the above solution was investigated. Figure 5 shows the SEM images of MnCO3 prepared at different pH. When the pH is 6.5 and 7.0, MnCO3 displays morphologies that are a mixture of cubes and irregular shapes (Figures 5a,b). With the increase of pH value to 7.5, the spherical morphology forms (Figure 5c). When the pH value reaches to 8.0, the size of the microspheres becomes uneven and seriously agglomerated (Figure 5d). This can be explained by the relationship between the pH of the solution and the hydrolysis process of the reactants. An increase in pH can lead to an increase in the hydrolysis rate (Nagao et al., 2004; Hussain et al., 2017). In the reaction process, when the pH value is higher, the hydrolysis of NH4HCO3 and MnSO4 are more complete, which accelerates the formation of MnCO3 microspheres, but a hydrolysis speed that is too fast is not conducive to controlling the properties of particles, which will widen the particle size distribution. Instead, the low pH will cause incomplete hydrolysis and irregular appearance of final products.
Figure 5. SEM images of MnCO3 prepared at different solution pH of 6.5 (a), 7.0 (b), 7.5 (c), and 8.0 (d).
The Effects of Addition Mode on the Morphology of MnCO3
In addition to the effect of reagent ratio and pH, the addition mode of NH4HCO3 also has a significant impact on the size and morphology of the synthesized samples. Two synthetic methods—adding the NH4HCO3 dropwise and pouring it directly into the MnSO4 solution—were employed in our experiment. The SEM results of corresponding products are displayed in Figure 6. As shown in Figure 6a, drop-by-drop addition of NH4HCO3 solution into the MnSO4 solution leads to large differences in the size of the MnCO3 microspheres, with the average size being 1.95 μm. On the contrary, the size of the MnCO3 microspheres is more uniform and the average size reduces to 0.99 μm (Figure 6b) in the later method. This is probably because the nucleation of MnCO3 was continuously formed in the solution during the drop-by-drop addition of NH4HCO3, leading the small microspheres that were formed to be accompanied by the growth of existing microspheres in the solution. In contrast, when the NH4HCO3 solution was directly poured into the MnSO4 solution, the nucleation of MnCO3 was formed in a short time and grew up simultaneously. Therefore, the size of the MnCO3 microspheres is more uniform.
Figure 6. SEM images of MnCO3 prepared at different adding mode of NH4HCO3 solution. (a) Added dropwise, (b) poured directly. The inset shows the size distribution of these particles.
The Effects of Heating Temperature and Time on the Morphology of Mn2O3
The second step is to synthesize Mn2O3 porous microspheres through the decomposition of the MnCO3 microspheres by heating treatment. The porous structure of Mn2O3 microspheres is important for the synthesis of LiMn2O4 microspheres without structural collapse because this structure can provide more grain shrinkage space during the lithiation process of Mn2O3 microspheres. We have investigated the influences of the heating temperature and heating time on the morphology of Mn2O3. The XRD result and SEM images of the corresponding samples are shown in Figure 7. During the decomposition process, the solid phase changes from MnCO3 to Mn2O3 with the release of CO2. Reversible oxidation and formation of various manganese oxides occur in the range of 350–560°C (Biernacki and Pokrzywnicki, 1999; Wang et al., 2013), and ultimately, pure phase of Mn2O3 is formed at above 600°C. Figure 7a shows the XRD pattern of Mn2O3 heated at 600°C for 5 h. All the peaks are identical to the pure phase of Mn2O3 (JCPDS#71-0636), which is consistent with the phase transition process in the literature (Wang et al., 2013). On the other hand, a porous microsphere structure consisting of small Mn2O3 nanocrystals are formed after heating for 5 h (Figure 7b). Furthermore, the EDS result (Figure 7c) also proves that MnCO3 has been fully reacted. When the heating time is increased to 10 and 20 h, the spherical shape of the Mn2O3 porous microspheres is well-maintained, but the sizes of the nanocrystallites increase slightly (Figures 7d,e). As the heating temperature increases to 700°C for 10 h, the nanocrystallites of the Mn2O3 porous microspheres increase obviously in size and partial microspheres show large holes in the surface (Figure 7f). The above results indicate that both extension of heating time and increase of heating temperature leads the Mn2O3 crystallites to grow into larger ones by adsorbing surrounding primary particles.
Figure 7. (a) XRD pattern of Mn2O3 heated at 600°C for 5 h, (b,c) SEM image and EDS result of Mn2O3 heated at 600°C for 5 h, (d–f) SEM images of Mn2O3 heated at different temperature and time, (d) 600°C, 10 h (e) 600°C, 20 h (f) 700°C, 10 h.
The Effects of Calcination Temperature, Calcination Time, and Mn2O3:LiOH Molar Ratio on the Synthesis of LiMn2O4
The last step for the synthesis of the LiMn2O4 spheres is the lithiation reaction of Mn2O3 porous microspheres with LiOH at high temperature. There are influences of the calcination temperature, calcination time and Mn2O3:LiOH molar ratio on the synthesis of LiMn2O4 microspheres. At first, the calcination temperature was adjusted in the range of 600–750°C, and the calcination time and molar ratio of Mn2O3:LiOH were set as 5 h and 1:1.05, respectively. Figure 8 shows the XRD patterns and SEM images of the corresponding samples. In Figure 8a1, for all the samples, the main characteristic peaks can be indexed as spinel LiMn2O4 (JCPDS#35-0782), but there is also a small weak peak at 32.9° originating from unreacted Mn2O3, indicating a slight deficiency in the amount of lithium. It is apparent in Figures 8a3,a4 that the porous spherical structure is well-preserved. It is also clear that LiMn2O4 spheres are composed of aggregated nanocrystallites with pores existing among them. Compared with the samples heated at 650 and 700°C, a small fraction of broken spheres can be observed in the products under 600°C (Figure 8a2). In Figure 8a5, the samples are piled up by irregular particles, and the holes disappeared. This is due to the structural collapse caused by excessive sintering temperature.
Figure 8. (a1) XRD patterns of LiMn2O4 heated at different temperature. (a2–a5) SEM images of LiMn2O4 heated at different temperature for 5 h. (a2) 600°C (a3) 650°C (a4) 700°C (a5) 750°C. (b1) XRD patterns of LiMn2O4 heated at different Mn2O3: LiOH and calcination times. (b2–b5) SEM images of LiMn2O4 heated at different Mn2O3:LiOH and calcination times. (b2) 1:1.1, 5 h (b3) 1:1.1, 10 h (b4) 1:1.5, 5 h (b5) 1:1.5, 10 h.
Next, we attempted to increase the molar ratio of Mn2O3:LiOH to 1.10 and 1.50 to obtain pure spinel LiMn2O4. Figure 8b1 shows the XRD patterns of the samples synthesized at 650°C with different time. When the molar ratio of Mn2O3:LiOH reaches 1:1.1 and the calcination time is 5 h, the lithiation reaction is incomplete, remaining as unreacted Mn2O3. With the extension of calcination time to 10 h, all the diffraction characteristic peaks in the XRD patterns can be identified with standard LiMn2O4 (JCPDS#35-0782), indicating good crystallinity and high purity for the products. Nevertheless, when the molar ratio of Mn2O3:LiOH further increases to 1.50, a new characteristic peak appears at 44.8°, which is indexed as Li2MnO3 (JCPDS#27-1252) phase, indicating that the lithium is excessive in this molar ratio. The above results suggest that the synthesis of pure LiMn2O4 requires an appropriate range for the molar ratio of Mn2O3:LiOH, and it is easy to produce byproducts beyond or under the critical values. The morphology and particle size of the products are observed by SEM. As can be seen from Figure 8b2 through Figure 8b5, LiMn2O4 is composed of uniform microspheres with a rough surface. The diameter of the microspheres is in the range of 0.8–1.0 μm.
Electrochemical Properties of LiMn2O4 Microspheres
The electrochemical performance of synthetic porous LiMn2O4 spheres was discussed as a cathode material for a lithium-ion battery. The cyclic voltammogram (CV) of the synthesized LiMn2O4 is shown in Figure 9a. Two pairs of separate redox peaks were observed form the CV curves of the synthesized sample, which correspond to the two-step insertion/deinsertion of lithium ion (Thackeray et al., 1983). Figure 9b reveals the current charge/discharge measurement by different rates over a voltage range of 3.0–4.5 V. The discharge capacities at rates of 0.1, 0.2, 0.5, 1.0, and 2.0 C were 103.18, 102.33, 101.50, 100.51, and 94.23 mAh g−1, respectively. The rate performance is shown in Figure 9c. As can be seen, the rate performance of LiMn2O4 synthesized at 650°C is quite good, which demonstrates clearly slower capacity decay with increasing discharge rates. For example, the porous LiMn2O4 microspheres retain a capacity of 94.23 mAh g−1, which is 91.3% of the initial capacity at rate of 0.1 C. This is much higher than that (76%) of the commercial LiMn2O4 powders at the same rate. When the current went back to a rate of 0.1 C, a capacity of 102.27 mAh g−1 was resumed. The cycle stability of LiMn2O4 synthesized at 650°C at 1.0 C is shown in Figure 9d. The capacity of synthesized LiMn2O4 remains at 96.42 mAh g−1 after 100 cycles and drops by only 3.24% compared to that of the first cycle. For comparison, the commercial LiMn2O4 exhibits a discharge capacity of 85.15 mAh g−1 after 100 cycles, which is much lower than that of the synthesized porous LiMn2O4 microspheres sample. The good rate and cycling performance of the samples prepared are ascribed to a well-defined structure such as uniform size and high porosity, which is effective in increasing contact area, shortening the transport distance of lithium ions and enhancing the structural stability of electrode material.
Figure 9. Electrochemical performances of the synthetic porous LiMn2O4 spheres. (a) CV curves at a scan rate of 0.1 mV s −1 in the voltage range of 3.0–4.5 V (vs. Li/Li+); (b) discharge-charge curves at different rate from 0.1 to 2.0 C (c) variation of discharge capacity vs. cycle number of synthetic porous LiMn2O4 electrodes at 0.1–2.0 C rate; (d) cycle performance of synthetic porous LiMn2O4 at 1.0 C rate.
In summary, porous LiMn2O4 microspheres with an average diameter of about 1 μm have been successfully synthesized by using molten LiOH and porous Mn2O3 spheres as templates. The morphology and particle size of the products could be conveniently controlled by changing the reactant ratio, pH, adding mode, heating time, etc. The morphology of MnCO3 was crucial for the preparation of porous LiMn2O4 microspheres and was mainly affected by the concentration of reactants and pH value of the solution during the chemical precipitation process. The optimum concentrations of MnSO4 and NH4HCO3 were 0.036 and 0.36 M, respectively, with appropriate pH of 7.5. During the lithiation of Mn2O3 microspheres, the heating temperature and the ratio between Mn2O3 and lithium salt were the most significant variables in terms of control over the morphology and purity of the LiMn2O4 microspheres. Excessive or low temperature would cause the collapse or agglomeration of the prepared LiMn2O4 microspheres. In addition, unreacted Mn2O3 can be found in the final products when the amount of lithium salt was deficient. Instead, the byproduct of Li2MnO3 was easy to generate when there was too much lithium salt. Our work suggested that the uniform porous LiMn2O4 microspheres were synthesized with the optimum molar ratio of Mn2O3:LiOH = 1: 1.1 and heated at 650°C for 10 h. Compared with the commercial LiMn2O4 powder, the synthesized LiMn2O4 microspheres present better rate capability and cyclability. This work can provide some guidance for the design and synthesis of porous LiMn2O4 microspheres or other LIBs' electrode materials.
The raw data supporting the conclusions of this manuscript will be made available by the authors, without undue reservation, to any qualified researcher. Requests to access the datasets should be directed to email@example.com.
YH and ZZ carried out the experiment and wrote the manuscript. PF and YW participated in the experiment. GL and LM contributed to the discussion. HL and LL supervised the experiment and proofread the manuscript.
This work is supported by the National Natural Science Foundation of China (No. 21875223) and the Fundamental Research Funds for the Central Universities (No. 649911023).
Conflict of Interest Statement
The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.
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Keywords: lithium manganese oxide, microsphere, cathode, lithium ion battery, percipitation, calcination
Citation: Hai Y, Zhang Z, Liu H, Liao L, Fan P, Wu Y, Lv G and Mei L (2019) Facile Controlled Synthesis of Spinel LiMn2O4 Porous Microspheres as Cathode Material for Lithium Ion Batteries. Front. Chem. 7:437. doi: 10.3389/fchem.2019.00437
Received: 30 April 2019; Accepted: 28 May 2019;
Published: 14 June 2019.
Edited by:Juchen Guo, University of California, Riverside, United States
Reviewed by:Liang Shi, University of Science and Technology of China, China
Jingbing Liu, Beijing University of Technology, China
Copyright © 2019 Hai, Zhang, Liu, Liao, Fan, Wu, Lv and Mei. This is an open-access article distributed under the terms of the Creative Commons Attribution License (CC BY). The use, distribution or reproduction in other forums is permitted, provided the original author(s) and the copyright owner(s) are credited and that the original publication in this journal is cited, in accordance with accepted academic practice. No use, distribution or reproduction is permitted which does not comply with these terms.