Lithium ion battery (LIB) has become the most widely used power supply for electronics. Safer electrode material has been pursued by researchers for years [1] . Spinel lithium manganese oxide (LiMn₂O₄), with the advantages of abundant, nontoxic, and inexpensive, is a promising cathode material for power lithium ion battery mainly [2] . Especially, the good stability may ensure its large-scale usage in the batteries for electric vehicle or energy storage [3] . However, LiMn₂O₄ shows obvious capacity fade when high-temperature working condition is applied (50˚C - 60˚C) [4] . The cause for the capacity degradation of LiMn₂O₄ is Jahn-Teller distortion and accepted as electrolyte decomposition, Mn²⁺ ions dissolution [5] , oxygen deficiency [6] [7] . In order to solve this problem, earlier studies have been focused on a chemical modification of LiMn₂O₄ by a partial substitution of Mn with some metal ions to obtain LiM_xMn_2−xO₄ (M = Co, Mg, Cr, Ni, Fe, Al, Ti and Zn) [8] - [12] . Another effective way is surface coating on LiMn₂O₄ by oxide with high thermal and structural stability. ZrO₂, SiO₂, Al₂O₃ and MgO [13] - [16] have been used to coat LiMn₂O₄ by some chemical processes. LiCoO₂ coating may suppress the dissolution of Mn and with de-intercalation and intercalation of Li ions, which will enhance the capacity of LiMn₂O₄. Therefore, it is expected that the LiMn₂O₄ by coating LiCoO₂ will show an excellent cycle performance at high-temperature. In this study, the effect of LiCoO₂ layer on the morphology and electrochemical performances of LiMn₂O₄ cathode materials were examined in detail.

LiMn₂O₄ powder was purchased from Hebei Strong-Power Li-ion Battery Technology Co. Ltd. (D98, China). LiCH₃COO∙2H₂O (1.03 g), Co (CH₃COO)₂∙4H₂O (2.53 g) with a stoichiometric ratio (1:1) were dissolved in distilled water. An aqueous solution of ethylene glycol and citric acid (1:4) as a chelating agent was added to the mixtures. pH value at 7.0 - 7.5 was achieved by Ammonium hydroxide. Then slowly add the LiMn₂O₄ powders (50 g) to the sol and vigorously stirred at 85˚C for 5 h. As the evaporation of water proceeding, the sol was turned into a viscous transparent gel. After drying and sieving, the powder was sintering in air at 350˚C for 3 h and 650˚C for 3 h to obtain LiCoO₂-coated LiMn₂O₄. For a comparison, pristine LiMn₂O₄ was also heat-treated in the same condition.

Figure 1 shows the XRD patterns. The peaks of both samples could be indexed to a cubic spinel structure with the space group Fd3m. There is no substantial difference between XRD patterns for LiMn₂O₄ and modified sample. The crystal lattice parameters were calculated by using the software of Jade, are 8.245 and 8.246 Å for the pristine and LiCoO₂-coated LiMn₂O₄, indicating that the bulk structure of LiMn₂O₄ unchange after surface modification. The characteristic peaks corresponding to LiCoO₂ are not observed because of low content (about 2.0 wt%).

Scanning electron microscopy has been shown in Figure 2 which reveals the pristine and modified samples

present a uniform particle distribution, ranging from 3 to 6 μm. The pristine spinel crystals are smooth with well-defined facets, as observed in Figure 2(a). It can be seen that the morphology and particle diameter of the LiCoO₂-coated LiMn₂O₄ powders in Figure 2(b), are similar to the pristine sample. No LiCoO₂ agglomerations and obscured facets of spinel LiMn₂O₄ are observed.

The further investment of the surface of LiMn₂O₄ by transmission electron microscope is displayed in Figure 3. Compared to the pristine sample (Figure 3(a)), about 3 - 5 nm thick layer of LiCoO₂ is uniformly formed on the surface of the LiMn₂O₄ (Figure 3(b)). The coating layer is clearly distinguishable from the crystalline LiMn₂O₄. This result demonstrates that sol-gel method is an effective way to coat the LiCoO₂ layer on the surface of LiMn₂O₄.

To further identify the homogeneity of coating layer, the element distribution is determined by EDS mapping, which is displayed in Figure 4. The dense accumulation of Mn element is attributed to the host material of LiMn₂O₄ and there is no significant agglomeration of Co. These results indicate that LiCoO₂ is homogeneously dispersed on the surface of the LiMn₂O₄ particles.

The XPS is shown in Figure 5, for pristine LiMn₂O₄ sample, there is no Co2p peaks. For LiCoO₂-coated LiMn₂O₄ sample, the Co2p region shows a Co2p_3/2 main peak at 780.4 eV with satellite peak at 796.8 eV. It is concluded that Co³⁺ have deposited on the surface of LiMn₂O₄. This result is in good agreement with the

observation in TEM and EDS element mapping.

The structure of pristine LiMn₂O₄ and LiCoO₂-coated LiMn₂O₄ cathodes after cycling 100 times (55˚C) was examined. The results are given in Figure 6. It can be seen that, the diffraction peaks of cycled LiMn₂O₄ cathode are widened and the peak intensity declined compared with the pristine LiMn₂O₄ cathode. In addition, some extra peaks appear in LiMn₂O₄ cathode XRD pattern after cycling, which should be assigned to Li₂Mn₂O₄. Usually, tetrahedral Li₂Mn₂O₄ can be generated at the final discharge stage of LiMn₂O₄ because of more Mn³⁺ and more significant Jahn-Teller effect. However, for the LiCoO₂-coated LiMn₂O₄ cathode, the diffraction peak width changed insignificantly before and after cycling. Comparing with cycled LiMn₂O₄ cathode, in the XRD

pattern of the cycled LiCoO₂-coated LiMn₂O₄, the peak intensity declines a polarization, we still should ascribe them to the LiCoO₂ on the surface of LiMn₂O₄.

In Figure 7, the galvanostatic charge-discharge curves under a current rate of 2C were conducted at (a) room temperature and (b) elevated temperatures in drying oven. They shows two discharge plateaus, which should be attributed to orderly intercalating of lithium ions in the tetrahedral (8a) sites at 4.1 V and disorderly intercalating lithium ions at 3.9 V which substantially maintains the intercalation feature of LiMn₂O₄ substrate [17] , indicating LiCoO₂ surface layer rather than Ni-doped LiMn₂O₄ because LiMn₂O₄ with Ni-doped spinel surface showed two ambiguously resolved discharging plateaus [18] . LiCoO₂-coated LiMn₂O₄ shows a higher discharge capacity compares to the pristine sample. The reason of high initial discharge capacity is that LiCoO₂ has capacity at this voltage range.

Figure 8 shows the cycling performance of electrodes with and without LiCoO₂ coating at (a) room temperature and (b) elevated temperatures. After 100 cycles at room temperature, the capacity retention of pristine sample (94.3%) is similar to that of modified sample (94.4%), as shown in Figure 8(a). However, after 100 cycles at elevated temperature, the discharge capacity of the pristine LiMn₂O₄ drops from 115.3 to 100.6 mAh/g. In contrast, the discharge capacity of modified sample changes from 117.2 to 110.1 mAh/g. The capacity retention increases from 87.5% to 93.6% after LiCoO₂ coating. Compared with other coating materials such as Al₂O₃ [19] , La₂O₃ [20] , AlPO₄ [21] , In these paper, surface modification by sol-gel method can improve the high-tempera- ture cycling stability of LiMn₂O₄, because oxide layer can reduce the contact area of LiMn₂O₄ and electrolyte. However, the covering layer is not very uniform, the highest capacity retention is about 89%, coupled with the oxide itself do not have de-intercalation and intercalation of Li ions, it will result in a decrease in initial capacity.

To further verify the effects of surface coating on manganese ions dissolution, the quality of the manganese element was directly determined by using ICP-AES. Li metal anode was washed by dilute hydrochloric acid after 100th cycle at 55˚C ± 2˚C. It can be seen in Table 1, the dissolved quality of Mn²⁺ ions of the pristine and LiCoO₂-coated LiMn₂O₄ electrode was 22.54 and 10.17 μg/cm², respectively. It can be concluded that after coating by LiCoO₂ layer, the dissolution of the manganese ions was significantly reduced. Therefore, LiCoO₂- coated LiMn₂O₄ electrode had better cycle stability at elevated temperature. The reason is that the coating material will reduce the contact area of LiMn₂O₄ and electrolyte, which may decrease the dissolution of Mn. The reactivity between LiCoO₂ and electrolyte has not yet clear, which need further research in future.

In summary, the surface of LiMn₂O₄ sample was modified by LiCoO₂ using a sol-gel method. TEM and XPS results confirm the existence of LiCoO₂ layer. A uniform and dense layer about 3 - 5 nm was coating on the

surface of pristine LiMn₂O₄. The LiCoO₂-coated LiMn₂O₄ sample exhibits much better cycling stability at elevated temperature (55˚C) compared with the pristine sample. These results demonstrated that this is an effective way to improve the high-temperature cyclic performance of spinel LiMn₂O₄.

This work was supported by National Science Foundation of China (No. 50672026). This work was also supported by Shanghai Nano Technology Promotion (No. 12ZR1448800).