Research Article | Open Access
Daichi Fujimoto, Yu Lei, Zheng-Hong Huang, Feiyu Kang, Junichi Kawamura, "Synthesis and Electrochemical Performance of LiMnPO4 by Hydrothermal Method", International Journal of Electrochemistry, vol. 2014, Article ID 768912, 9 pages, 2014. https://doi.org/10.1155/2014/768912
Synthesis and Electrochemical Performance of LiMnPO4 by Hydrothermal Method
LiMnPO4 with olivinestructure which is the promising candidate for high voltage cathode material was synthesized by hydrothermal method. In order to synthesize high purity and well-defined LiMnPO4, several precursors for Li, Mn, and P sources and hydrothermal reaction parameters including temperature and [H2O]/[Mn] value are optimized. By analyzing the structure, Mn valence, morphology, and chemical ratio via XRD, XPS, Raman, SEM, and ICP LiMnPO4 synthesized from manganese acetate tetrahydrate have single phase of LiMnPO4 without impurity and showed charge and discharge reaction caused by Mn2+/Mn3+ redox. Specific capacity of synthesized LiMnPO4 grew up during cycling. Moreover, when hydrothermal temperature was set at 150°C and [H2O]/[Mn] value was set at 15, discharge capacity as high as 70 mAh/g was obtained at rate.
Lithium-ion batteries are used widely as mobile devices like cellphone and notebook. Recently, researchers are actively devoted into the lithium-ion battery research for high energy conversion system, such as electric vehicle. Most of present lithium-ion batteries have used LiCoO2 as cathode which was discovered in 1980 . However, LiCoO2 which includes rare-metal Co has irreversible structure shift at discharging over 0.6 Li from LiCoO2 that cause discharge capacity limited to 120~130 mAh/g instead of theoretical capacity of 270 mAh/g . Several alternative materials are proposed as cathode materials. In 1997, Padhi et al. reported that phospho-olivine can work as promising cathode materials for lithium-ion battery [3, 4]. Among phospho-olivine LiFePO4, LiMnPO4, LiCoPO4, and LiNiPO4 are considered to be possible candidates for lithium-ion battery. Compared to LiFePO4 and LiCoPO4, LiMnPO4 is a cathode material with high redox potential which can be used with presently available liquid electrolyte so that LiMnPO4 exceeds the energy density of LiFePO4 which is the most investigated electrode among LiMPO4 family . The characteristic of this olivine structure is an inductive effect which appears due to a strong covalent bond of to rise up redox potential . However, the strong covalent bond causes poor conductivity, decelerating the charge and discharge processes. So far, several approaches have been used to solve this problem, such as controlling the particle size, morphology, and carbon coating . Solid state reaction is generally used to prepare LiMnPO4 [7, 8]. Besides this, other approaches such as sol-gel method [9, 10], precipitation [11–13], hydrothermal [10, 14–19], solvothermal method [14, 20–22], spray pyrolysis , and polyol process [24, 25] are also used. The hydrothermal method is a simple synthesis method in which precursors are put into autoclave with water and seal and heat at around 200°C. The advantages of hydrothermal method are the capability of synthesizing at low temperature, obtaining high crystallinity, high purity material, and controlling particle size and morphology. Therefore, in this work, we further optimized synthesis parameters of hydrothermal method for LiMnPO4 synthesis and investigated their electrochemical performance.
2.1. Preparation of LiMnPO4
The hydrothermal reaction of LiMnPO4 was carried out under various conditions at 150°C or 190°C for 12 hours after Li, Mn, and P source with stoichiometric ratio were dispersed uniformly with distilled water. Lithium acetate dihydrate (denoted as LiAc) and lithium hydroxide monohydrate (LiOH) were the candidates for Li source, manganese acetate tetrahydrate (MnAc) and manganese sulfate monohydrate (MnSO4) worked as Mn source, and ammonium dihydrogen phosphate (NH4H2PO4) was P source. The amount of water was set as [H2O]/[Mn] = 15 or 30. Herein, samples are denoted as A, B, C, D, E, F, and G depending on synthesis conditions. The samples preparation conditions are listed in Table 1. These precursors were put into autoclave with quantitative distilled water and stirred by magnetic stirrer. This solution was put into oven with 2.5°C/min heating rate. After keeping 12 hours, the autoclave was naturally cooled down to room temperature. Finally, the powder was washed with distilled water and ethanol several times by centrifugation and dried out at 100°C for about 12 hours.
The crystalline phases were identified by X-ray diffraction (XRD, D/max-2500, Rigaku) with Cu-K radiation. The oxidation state of manganese was confirmed by the X-ray photoelectron spectroscopy (XPS, ESCALAB 250Xi, Thermo Scientific). The composition analysis of Li, Mn, and P was carried out using inductively coupled plasma (ICP-OES, VISTA-MPX) by dissolving LiMnPO4 powder into aqua regia. The morphology and particle size were observed by scanning electron microscope (SEM, LEO-1530). The existence of impurity was confirmed by Raman spectroscopy (Lab RAMHR800, HORIBA Jobin Yvon Ltd., USA) with 488 nm wavelength laser.
2.3. Electrochemical Measurement
The synthesized LiMnPO4 by hydrothermal reaction was mixed and smashed with carbon black (weight was set to 1/8 of LiMnPO4) by wet ball milling with ethanol for 3 hours. After evaporating ethanol, this mixture was followed by dry ball milling for 3 hours to obtain well-mixed LiMnPO4/C compound.
The electrochemical measurement was performed by constant current cyclic voltammetry using 2032 coin-cell battery for evaluation of specific capacity. LiMnPO4/C compound was mixed with PVDF (polyvinyliden fluoride: Shenzhen Kejing Star Technology Company) and carbon black (Shenzhen Kejing Star Technology Company) and then dispersed in NMP (N-methylpyrrolidone: Shenzhen Kejing Star Technology Company). Then, the slurry was stirred by magnet stirrer for several hours. The final weight ratio of LiMnPO4 : carbon black : PDVF was set as 70 : 20 : 10. The solution was then pasted on aluminum foil followed by drying at 80°C for 2 hours and then 120°C in vacuum for 12 hours. After vacuum for half day, this foil was naturally cooled down to room temperature in vacuum and cut to disc with 10 mm of diameter. Lithium disc was used as counter electrode, and EC:DMC (1 mol/L LiPF6) was used as electrolyte and a celgard 2400 was used as separator. 2032 coin-cell battery (CR-2032) was assembled in glove box filled by Ar gas. After 1 day, galvanostatic charge and discharge were carried out at 1/20 C rate for 50 cycles using LAND battery test (Wuhan Jinnuo Electronics Co., Ltd.).
3. Results and Discussion
3.1. Effect of Different Precursors on Hydrothermal Synthesis of LiMnPO4
XRD pattern of all the samples is shown in Figure 1. Samples synthesized from MnAc as Mn source (samples A and B) have LiMnPO4 crystal structure. All peaks come from LiMnPO4 diffraction pattern, and no impurity was observed. However, diffraction pattern corresponding to Mn2P2O7 rather than LiMnPO4 was observed in the XRD patterns of samples synthesized from MnSO4 (samples C and D).
XPS measurement was performed to evaluate Mn valence in LiMnPO4. The narrow scan XPS spectra in Figure 2(b) suggest that the binding energy of Mn2p3/2 is around 641.6 eV in samples A and B synthesized from MnAc. On the other hand, the binding energy of Mn2p3/2 is around 642.0 eV in samples C and D synthesized from MnSO4 (Table 2). Since the Mn2+ has lower oxidation state than Mn3+, therefore larger amount of Mn2+ might exist in samples A and B. Lee et al.  previously reported that the binding energy of Mn2p3/2 for Mn2+ and Mn3+ is 641.1 eV and 642.3 eV, which is consistent with the present data.
In order to further investigate the gap between atomic ratio of Li : Mn : P for as-prepared LiMnPO4 and stoichiometric ratio, inductively coupled plasma (ICP-OES) was carried out. As shown in Table 3, samples synthesized from MnSO4 (samples C and D) contain very small amount of Li. However, samples synthesized from MnAc (samples A and B) contain large amount of Li. This Li deficiency is corresponding to Li vacancy which is termed on Li defects in this paper. It is also found that sample B contains smaller Li deficiency than that of sample A. The difference in the Li deficiency is probably due to the difference in basic strength of LiOH (strong basic) and LiAc (weak basic). It was previously reported that hydrothermal reaction using basic solution is suitable for the synthesis of LiMnPO4 . In addition, as the amount of Li increases, the amount of P also increases.
Cycling performance and galvanostatic charge and discharge curves at 1st, 10th, 30th, and 50th cycle are shown in Figures 4(a)–4(e). Galvanostatic charge and discharge curves of samples synthesized from MnAc (samples A and B) indicate coexistence of plateau of LiMnPO4 and MnPO4 near 4 V with 40 mAh/g discharge capacity at rate. However, no obvious redox plateau is observed from samples synthesized from MnSO4 (samples C and D) whose capacity is less than 10 mAh/g. These results are consistent with XRD results and Li content information obtained from ICP data that the sample prepared from MnAC and LiOH contains higher quality olivine structure and less impurity. Besides, discharge capacity increases as a function of cycle number for all samples. The discharge capacity of sample A and sample B reached 40.6 mAh/g at the 50th cycle from 26.7 mAh/g of the 1st cycle and 45.9 mAh/g at the 50th cycle from 12.8 mAh/g of the 1st cycle, respectively. Referring to ICP data, this phenomenon may be due to the gradual insertion of Li ion into the Li defect as the cycle number increases.
3.2. Various Parameters for Hydrothermal Synthesis
Since LiMnPO4 using LiOH and MnAc shows larger discharge capacity, therefore hydrothermal parameters including temperature and [H2O]/[Mn] value were further investigated by using LiOH, MnAc, and NH4H2PO4 as precursors. The hydrothermal temperature was set from 150°C to 190°C for 12 hours, and [H2O]/[Mn] value was set as 15 or 30 (Table 4). After hydrothermal, reaction as-prepared powder was rinsed by distilled water and ethanol as the same as the above.
The XRD patterns for all LiMnPO4 samples shown in Figure 5 indicate olivine structure derived from LiMnPO4 without any impurity. No significant difference was detected among the sample prepared between various conditions.
The XPS spectra and binding energy of Mn2p shown in Figures 6(a) and 6(b) display similar spectra and binding energy of Mn2p3/2 around 641.6 eV. Therefore, Mn oxidation state is mainly influenced by Mn source rather than the hydrothermal condition, temperature, and [H2O]/[Mn] value.
ICP results listed in Table 5 indicate that Li and P defects are observed in all LiMnPO4 samples and the amounts of Li and P defects are about 13% and 9%, respectively. It is easy to lose Li and P during the hydrothermal reaction. Therefore, it is suggested that excess Li and P are used as precursors, which is consistent with the previously reported results [10, 14–19].
Since no impurity is detected by XRD, Raman spectroscopy is used to detect excess Li, Mn, and P compounds which might exist in LiMnPO4 as impurity. It is previously reported [13, 27] that LiMnPO4 sample contained Mn2P2O7 and Li3PO4 as impurity. However, no such impurity is detected in our sample. Figure 7 shows that the Raman spectra of as-prepared LiMnPO4 are consistent with the previously reported data . The Raman data suggests that the as-prepared sample only contains single phase LiMnPO4 without impurities such as Mn2P2O7 or Li3PO4.
The SEM images of each LiMnPO4 particle are presented in Figures 8(a)–8(d). As-prepared LiMnPO4 powder of sample B shows a particle size over 1 . Grain growth was restricted as reducing hydrothermal temperature and [H2O]/[Mn] value. Sample G has the smallest particle size among them. Moreover, particle morphology changes from prismatic shape to thin plate shape.
The electrochemical performances were summarized in Figures 9(a)–9(e). Sample G shows the largest discharge capacities, which was as high as 39.0 mAh/g at the 1st cycle and 68.7 mAh/g at the 50th cycle. Other samples do not show large discharge capacities. However, each sample shows different discharge capacities in the 1st cycle. In addition, discharge capacity in each cycle becomes large as a function of cycle number. The presence of Li defect in the samples might be responsible for increasing discharge capacity.
High purity LiMnPO4 was synthesized by hydrothermal method with different precursors and conditions. Different synthesis condition results in different characteristics. In case of precursors, samples synthesized from MnSO4 hardly contain lithium and do not have olivine structure, and they do not show charge and discharge reaction between Mn2+ and Mn3+. However, samples synthesized from MnAc have olivine structure without impurity and show charge and discharge reaction of Mn2+/Mn3+ although these LiMnPO4 synthesized from MnAc contain some Li and P defects. For Li source, the sample synthesized from LiOH shows better discharge capacity than that of LiAc. In the case of hydrothermal condition, as the temperature and the [H2O]/[Mn] values are decreased, smaller particle size and larger capacity were obtained. The precursor molar ratio of Li : Mn : P was set at 1 : 1 : 1 to synthesize LiMnPO4 by hydrothermal reaction, which results in a slight deficiency of Li and P. Therefore, it is important to adjust Li and P precursor molar ratios for synthesizing stoichiometric LiMnPO4.
Conflict of Interests
The authors declare that there is no conflict of interests regarding the publication of this paper.
This research work was carried out under a Joint Education Program between Tsinghua University and Tohoku University. The authors wish to thank Mr. Naoaki Kuwata and Mr. M. T. Chowdhury for the valuable suggestions.
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