MnO2 prepared by hydrothermal method and electrochemical performance as anode for lithium-ion battery
© Feng et al.; licensee Springer. 2014
Received: 29 April 2014
Accepted: 1 June 2014
Published: 10 June 2014
Two α-MnO2 crystals with caddice-clew-like and urchin-like morphologies are prepared by the hydrothermal method, and their structure and electrochemical performance are characterized by scanning electron microscope (SEM), X-ray diffraction (XRD), galvanostatic cell cycling, cyclic voltammetry, and electrochemical impedance spectroscopy (EIS). The morphology of the MnO2 prepared under acidic condition is urchin-like, while the one prepared under neutral condition is caddice-clew-like. The identical crystalline phase of MnO2 crystals is essential to evaluate the relationship between electrochemical performances and morphologies for lithium-ion battery application. In this study, urchin-like α-MnO2 crystals with compact structure have better electrochemical performance due to the higher specific capacity and lower impedance. We find that the relationship between electrochemical performance and morphology is different when MnO2 material used as electrochemical supercapacitor or as anode of lithium-ion battery. For lithium-ion battery application, urchin-like MnO2 material has better electrochemical performance.
Manganese dioxides with diverse crystal morphologies are attracting a lot of attention because of their physical and chemical properties and wide applications in catalysis , biosensors , water treatment [3, 4], electrochemical supercapacitors [5–9], and so on. Up to now, various MnO2 crystals with different morphologies such as nanosphere [10, 11], nanorod [12, 13], nanowire , nanoflower [13, 14], nanotube , pillow-shape , urchin-like [10, 16], hollow nanosphere, hollow nanocube , and hollow cone  have been synthesized. MnO2 crystals were already used in water treatment, gas sensors, electrochemical supercapacitors, and so on. For example, hollow spherical and cubic MnO2 nanostructures prepared by Kirkendall effect showed good ability to remove organic pollutants in waste water . Cao et al. had prepared pillow-shaped MnO2 crystals which could remove about 85% of the Cd2+ in waste water . Zhang et al. had prepared MnO2 hollow nanospheres and nanowires used for ammonia gas sensor . MnO2 hollow nanospheres were found to exhibit enhanced sensing performance to ammonia gas at room temperature compared with MnO2 nanowires. Ma et al. had prepared urchin-shaped MnO2 and clew-like-shaped MnO2 used for electrochemical supercapacitors . They found the electrochemical performances differed with various morphologies, and clew-like MnO2 nanospheres had higher capacitance and lower charge-transfer resistance due to their incompact structure. However, the application researches of MnO2 as anode for lithium-ion battery were relatively few.
MnO2 nanomaterials are recognized as anode materials since three-dimensional (3d) transition metal oxides (MO, where M is Fe, Co, Ni, and Cu) were proposed to serve as high theoretic capacity anodes for lithium-ion battery by Poizot et al. . Before that, MnO2 nanomaterials were usually used to prepare LiMn2O4 crystals as cathode for lithium-ion battery [19, 20]. Chen's research group has made great contributions on the research of anode for lithium-ion battery [21, 22]. Nevertheless, compared to the intensive investigation on Fe2O3, Fe3O4, SnO2, CoO, and so on [23–28], the application investigation of MnO2 nanomaterials on anodes for lithium-ion battery is still immature, although the investigations on their preparation are plentiful.
The research on MnO2 anode is relatively complex because MnO2 exists in several crystallographic forms such as α-, β-, γ-, and δ-type. For example, Zhao et al.  reported γ-MnO2 crystals with hollow interior had high discharge capacity as 602.1 mAh g−1 after 20 cycles. Li et al.  found α-MnO2 with nanotube morphology exhibited high reversible capacity of 512 mAh g−1 at a high current density of 800 mA g−1 after 300 cycles. Thus, from the above two examples, we could summarize that the electrochemical performance of MnO2 crystals has relationship both with the crystallographic forms and with the morphologies. Therefore, the researches on the relationship of electrochemical performance with the morphologies and the relationship of electrochemical performance with the crystallographic forms are very essential.
In the present work, to enrich the relationship between electrochemical performances and morphologies, two α-MnO2 crystals with caddice-clew-like and urchin-like morphologies were prepared by hydrothermal method. For lithium-ion battery application, urchin-like α-MnO2 crystal with compact structure was found to have better electrochemical performance.
Synthesis and characterization of MnO2 micromaterials prepared by hydrothermal method
All reagents purchased from the Shanghai Chemical Company (Shanghai, China) were of analytical grade and used without further purification. The MnO2 micromaterials were prepared using the similar method described by Yu et al.  with some modifications. To prepare caddice-clew-like MnO2 micromaterial, 1.70 g MnSO4 · H2O was dissolved in 15-mL distilled water with vigorous stirring. When the solution was clear, 20-mL aqueous solution containing 2.72 g K2S2O8 was added to the above solution under continuous stirring. Then, the resulting transparent solution was transferred into a Teflon-lined stainless steel autoclave (50 mL) of 80% capacity of the total volume. The autoclave was sealed and maintained at 110°C for 6 h. After the reaction was completed, the autoclave was allowed to cool to room temperature naturally. The solid black precipitate was filtered, washed several times with distilled water to remove impurities, and then dried at 80°C in air for 3 h. The obtained caddice-clew-like MnO2 micromaterial was collected for the following characterization.
Urchin-like MnO2 micromaterial was prepared by the similar method, while after adding 1.70 g MnSO4 · H2O and 2.72 g K2S2O8 into 35-mL distilled water, 2 mL H2SO4 was then added. Subsequently, the solution was transferred into a Teflon-lined stainless steel autoclave (50 mL), and the autoclave was sealed and maintained at 110°C for 6 h as well. After the reaction was completed, the autoclave was allowed to cool to room temperature naturally. The solid black precipitate was filtered, washed several times with distilled water to remove impurities, and then dried at 80°C in air for 3 h.
The crystallographic structures of the products were determined with X-ray diffraction (XRD) which were recorded on a Rigaku D/max-2200/PC (Rigaku, Beijing, China) with Cu target at a scanning rate of 7°/min with 2θ ranging from 10° to 70°. The morphological investigations of scanning electron microscope (SEM) images were taken on a field emission scanning electron microscope (FESEM; Zeiss Ultra, Oberkochen, Germany).
Electrochemical studies of MnO2 micromaterials
Electrochemical performances of the samples were measured using CR2025 coin-type cells assembled in a dry argon-filled glove box. To fabricate the working electrode, a slurry consisting of 60 wt.% active materials, 10 wt.% acetylene black, and 30 wt.% polyvinylidene fluoride (PVDF) dissolved in N-methyl pyrrolidinone was casted on a copper foil and dried at 80°C under vacuum for 5 h. Lithium sheet was served as counter and reference electrode, while a Celgard 2320 membrane (Shenzhen, China) was employed as a separator. The electrolyte was a solution of 1 M LiPF6 in ethylene carbonate (EC)-1,2-dimethyl carbonate (DMC) (1:1 in volume). Galvanostatical charge-discharge experiments were performed by Land electric test system CT2001A (Wuhan LAND Electronics Co., Ltd., Wuhan, China) at a current density of 0.2 C between 0.01 and 3.60 V (versus Li/Li+). Cyclic voltammogram (CV) tests were carried out on an electrochemical workstation (CHI604D, Chenhua, Shanghai, China) from 0.01 to 3.60 V (versus Li/Li+). Electrochemical impedance spectroscopy (EIS) measurements were performed on an electrochemical workstation (CHI604D, Chenhua, Shanghai, China), and the frequency ranged from 0.1 Hz to 100 kHz with an applied alternating current (AC) signal amplitude of 5 mV.
Results and discussion
Structure and morphology
As can be seen in Reaction (1), the reaction rate is pH dependent. Therefore, sulfuric acid is added to decrease the reaction rate, and the morphology can be modulated. When no sulfuric acid is used, these primary nanoparticles form quickly (shown in Figure 2(a)). Then, the tiny nanoparticles spontaneously aggregate into long nanowires. With minimizing interfacial energies, the nanowires wrap with each other incompactly to form caddice-clew-shaped MnO2 micromaterials. When sulfuric acid is added as morphology modulation agent, the nucleation process in Reaction (1) is suppressed. In this situation, it is not easy to form nanowires. Alternatively, short nanorods are formed (shown in Figure 2(b)). With minimizing interfacial energies, the nanorods self-assemble compactly to urchin morphology with a hollow interior. Thus, urchin-like MnO2 micromaterials are prepared. Therefore, sulfuric acid plays a crucial role in the morphology evolution due to its control of the nucleation rate of MnO2.
In addition, a discharge plateau with wide and flat shape appears in all the discharge voltage curves. Urchin-like MnO2 micromaterial has a plateau at about 0.32 V from 120 to 1,100 mAh g−1 during the first discharging process and has a plateau from 50 to 360 mAh g−1 in the second cycling. The caddice-clew-like MnO2 micromaterial has similar discharge plateau. The discharge plateau may bring stable discharge current to the battery prepared by MnO2 micromaterials. According to the results of discharge specific capacity, urchin-like MnO2 micromaterial was better than caddice-clew-like MnO2 micromaterial.
The current intensity of oxidation peak is much lower than that of reduction peak. The current intensity of reduction peak and oxidation peak for the urchin-like MnO2 material is 0.7828 and 0.1202 mA mg−1, respectively. The current intensity attenuation of oxidation peak indicates that Mn element could not completely convert to MnO2 during the charging process. The shapes of the CV curves for the MnO2 samples are similar, while urchin-like MnO2 material has higher peak intensity. The current intensity of reduction peak and oxidation peak for the caddice-clew-like MnO2 material is 0.3333 and 0.0712 mA mg−1, respectively. The asymmetry cyclic voltammogram curves in Figure 5 indicate that the discharging/charging process is irreversible.
To exclude the influence of the MnO2 micromaterial density on the electrode, we have normalized the CV curve in Figure 5. According to the results of galvanostatical charge-discharge experiments and CV tests, the urchin-like MnO2 micromaterial is more superior than caddice-clew-like MnO2 micromaterial. We presume the difference on electrochemical performance results from the morphology as both the MnO2 micromaterials have identical crystalline phase. Theoretically, nanomaterials with incompact structure are beneficial to improve the transmission rate and transfer ability of lithium ion. However, the discharge cycling stability of caddice-clew-like MnO2 micromaterial is poor. We guess the incompact structure may lead to easy electrode pulverization and loss of inter-particle contact during the repeated charging-discharging processes. A hollow structure which is another effective strategy to improve the cycling stability could provide extra free space for alleviating the structural strain and accommodating the large volume variation associated with repeated Li+ insertion/extraction processes. So, the relatively better discharge cycling stability may result from the hollow structure. In addition, the surface of urchin-like MnO2 is an arrangement of compact needle-like nanorods, which could improve the transmission rate and transfer ability of lithium ion. Therefore, the electrochemical performances of the MnO2 micromaterials indeed have relationship on their morphologies. The results suggest that the urchin-like MnO2 micromaterial is more promising for the anode of lithium-ion battery.
Compared to the literature , when MnO2 materials were used for electrochemical supercapacitors, caddice-clew-like MnO2 material had higher specific capacitance of 120 F g−1 and lower charge-transfer resistance, while the specific capacitance of urchin-like MnO2 material was about 48 F g−1. Moreover, they found the unique capacitance of caddice-clew-like MnO2 was mainly due to the incompact structure. Therefore, the relationship between electrochemical performance and morphology is different when MnO2 material is used as electrochemical supercapacitor or as anode of lithium-ion battery. For the application on lithium-ion battery, urchin-like MnO2 material is better.
R s , R sf , and R ct calculated from Nyquist plots for the MnO 2 materials
In summary, two MnO2 micromaterials with urchin-like and caddice-clew-like morphologies are prepared by hydrothermal method. Both the crystalline phases are α-MnO2, which is essential to evaluate the relationship between electrochemical performances and morphologies of MnO2 crystals as anodes for lithium-ion battery application. Both the as-prepared α-MnO2 exhibit high initial specific capacity, but the discharge cycling stability is poor. Just in case of this research, the urchin-like MnO2 material has better electrochemical performance. The results suggest that different morphologies indeed have influence on electrochemical performances of MnO2 micromaterials in the application of lithium-ion battery. This study also gives us advice to make shell coating on the as-prepared MnO2 micromaterials to improve the cycling stability.
This work was financially supported by the Program for Innovative Research Team (in Science and Technology) in the University of Yunnan Province (2010UY08, 2011UY09), Yunnan Provincial Innovation Team (2011HC008), the General Program of the Application and Basic Research Foundation of Yunnan Province (2013FZ080), the Youth Fund Research Project of Yunnan Minzu University (2012QN01), the Key Project of Scientific Research Foundation of the Educational Bureau of Yunnan Province (2013Z039), and the Graduate Program of Scientific Research Foundation of the Educational Bureau of Yunnan Province (2013J120C).
- Sui N, Duan Y, Jiao X, Chen D: Large-scale preparation and catalytic properties of one-dimensional MnO2 nanostructures. J Phys Chem C 2009, 113: 8560–8565.View ArticleGoogle Scholar
- Zhang W, Zeng C, Kong M, Pan Y, Yang Z: Water-evaporation-induced self-assembly of α-MnO2 hierarchical hollow nanospheres and their applications in ammonia gas sensing. Sens Actuators B 2012, 162: 292–299. 10.1016/j.snb.2011.12.080View ArticleGoogle Scholar
- Fei J, Cu Y, Yan X, Qi W, Yang Y, Wang K, He Q, Li J: Controlled preparation of MnO2 hierarchical hollow nanostructures and their application in water treatment. Adv Mater 2008, 20: 452–456. 10.1002/adma.200701231View ArticleGoogle Scholar
- Cao J, Mao Q, Shi L, Qian Y: Fabrication of g-MnO2/α-MnO2 hollow core/shell structures and their application to water treatment. J Mater Chem 2011, 21: 16210–16215. 10.1039/c1jm10862jView ArticleGoogle Scholar
- Wei W, Cui X, Chen W, Ivey DG: Manganese oxide-based materials as electrochemical supercapacitor electrodes. Chem Soc Rev 2011, 40: 1697–1721. 10.1039/c0cs00127aView ArticleGoogle Scholar
- Yu P, Zhang X, Wang D, Wang L, Ma Y: Shape-controlled synthesis of 3D hierarchical MnO2 nanostructures for electrochemical supercapacitors. Cryst Growth Des 2009, 9: 528–533. 10.1021/cg800834gView ArticleGoogle Scholar
- Subramanian V, Zhu H, Wei B: Nanostructured MnO2: hydrothermal synthesis and electrochemical properties as a supercapacitor electrode material. J Power Sources 2006, 159: 361–364. 10.1016/j.jpowsour.2006.04.012View ArticleGoogle Scholar
- Jiang R, Huang T, Liu J, Zhuang J, Yu A: A novel method to prepare nanostructured manganese dioxide and its electrochemical properties as a supercapacitor electrode. Electrochim Acta 2009, 54: 3047–3052. 10.1016/j.electacta.2008.12.007View ArticleGoogle Scholar
- Subramanian V, Zhu H, Vajtai R, Ajayan PM, Wei B: Hydrothermal synthesis and pseudocapacitance properties of MnO2 nanostructures. J Phys Chem B 2005, 109: 20207–20214. 10.1021/jp0543330View ArticleGoogle Scholar
- Xu M, Kong L, Zhou W, Li H: Hydrothermal synthesis and pseudocapacitance properties of γ-MnO2 hollow spheres and hollow urchins. J Phys Chem C 2007, 111: 19141–19147. 10.1021/jp076730bView ArticleGoogle Scholar
- Li Z, Ding Y, Xiong Y, Xie Y: Rational growth of various γ-MnO2hierarchical structures and α-MnO2 nanorods via a homogeneous catalytic route. Cryst Growth Des 2005, 5: 1953–1958. 10.1021/cg050221mView ArticleGoogle Scholar
- Wang X, Li Y: Rational synthesis of α-MnO2 single-crystal nanorods. Chem Commun 2002, 764–765.Google Scholar
- Duan X, Yang J, Gao H, Ma J, Jiao L, Zheng W: Controllable hydrothermal synthesis of manganese dioxide nanostructures: shape evolution, growth mechanism and electrochemical properties. Cryst Eng Comm 2012, 14: 4196–4204. 10.1039/c2ce06587hView ArticleGoogle Scholar
- Li WN, Yuan J, Shen XF, Gomez-Mower S, Xu LP, Sithambaram S, Aindow M, Suib SL: Hydrothermal synthesis of structure- and shape-controlled manganese oxide octahedral molecular sieve nanomaterials. Adv Funct Mater 2006, 16: 1247–1253. 10.1002/adfm.200500504View ArticleGoogle Scholar
- Li L, Nan C, Lu J, Peng Q, Li Y: α-MnO2 nanotubes: high surface area and enhanced lithium battery properties. Chem Commun 2012, 48: 6945–6947. 10.1039/c2cc32306kView ArticleGoogle Scholar
- Song XC, Zhao Y, Zheng YF: Synthesis of MnO2 nanostructures with sea urchin shapes by a sodium dodecyl sulfate-assisted hydrothermal process. Cryst Growth Des 2007, 7: 159–162. 10.1021/cg060536hView ArticleGoogle Scholar
- Portehault D, Cassaignon S, Baudrin E, Jolivet JP: Twinning driven growth of manganese oxide hollow cones through self-assembly of nanorods in water. Cryst Growth Des 2009, 9: 2562–2565. 10.1021/cg9002862View ArticleGoogle Scholar
- Poizot P, Laruelle S, Grugeon S, Dupont L, Tarascon JM: Nano-sized transition-metal oxides as negative-electrode materials for lithium-ion batteries. Nature 2000, 407: 496–499. 10.1038/35035045View ArticleGoogle Scholar
- Kim DK, Muralidharan P, Lee HW, Ruffo R, Yang Y, Chan CK, Peng H, Huggins RA, Cui Y: Spinel LiMn2O4 nanorods as lithium ion battery cathodes. Nano Lett 2008, 8: 3948–3952. 10.1021/nl8024328View ArticleGoogle Scholar
- Luo J, Cheng L, Xia Y: LiMn2O4 hollow nanosphere electrode material with excellent cycling reversibility and rate capability. Electrochem Commun 2007, 9: 1404–1409. 10.1016/j.elecom.2007.01.058View ArticleGoogle Scholar
- Cheng F, Zhao J, Song W, Li C, Ma H, Chen J, Shen P: Facile controlled synthesis of MnO2 nanostructures of novel shapes and their application in batteries. Inorg Chem 2006, 45: 2038–2044. 10.1021/ic051715bView ArticleGoogle Scholar
- Zhao J, Tao Z, Liang J, Chen J: Facile synthesis of nanoporous γ-MnO2 structures and their application in rechargeable Li-ion batteries. Cryst Growth Des 2008, 8: 2799–2805. 10.1021/cg701044bView ArticleGoogle Scholar
- Wu HB, Chen JS, Hng HH, Lou XWD: Nanostructured metal oxide-based materials as advanced anodes for lithium-ion batteries. Nanoscale 2012, 4: 2526–2542. 10.1039/c2nr11966hView ArticleGoogle Scholar
- Zhang WM, Wu XL, Hu JS, Guo YG, Wan LJ: Carbon coated Fe3O4 nanospindles as a superior anode material for lithium-ion batteries. Adv Funct Mater 2008, 18: 3941–3946. 10.1002/adfm.200801386View ArticleGoogle Scholar
- Barreca D, Cruz-Yusta M, Gasparotto A, Maccato C, Morales J, Pozza A, Sada C, Sánchez L, Tondello E: Cobalt oxide nanomaterials by vapor-phase synthesis for fast and reversible lithium storage. J Phys Chem C 2010, 114: 10054–10060. 10.1021/jp102380eView ArticleGoogle Scholar
- Barreca D, Carraro G, Gasparotto A, Maccato C, Cruz-Yusta M, Gómez-Camer JL, Morales J, Sada C, Sánchez L: On the performances of CuxO-TiO2(x = 1, 2) nanomaterials as innovative anodes for thin film lithium batteries. ACS Appl Mater Interfaces 2012, 4: 3610–3619. 10.1021/am300678tView ArticleGoogle Scholar
- Zhang L, Wu HB, Madhavi S, Hng HH, Lou XW: Formation of Fe2O3 microboxes with hierarchical shell structures from metal-organic frameworks and their lithium storage properties. J Am Chem Soc 2012, 134: 17388–17391. 10.1021/ja307475cView ArticleGoogle Scholar
- Wang C, Zhou Y, Ge M, Xu X, Zhang Z, Jiang JZ: Large-scale synthesis of SnO2 nanosheets with high lithium storage capacity. J Am Chem Soc 2012, 132: 46–47.View ArticleGoogle Scholar
- Xiang JY, Tu JP, Zhang L, Zhou Y, Wang XL, Shi SJ: Self-assembled synthesis of hierarchical nanostructured CuO with various morphologies and their application as anodes for lithium ion batteries. J Power Sources 2010, 195: 313–319. 10.1016/j.jpowsour.2009.07.022View ArticleGoogle Scholar
- Chen J: Recent progress in advanced materials for lithium ion batteries. Materials 2013, 6: 156–183. 10.3390/ma6010156View ArticleGoogle Scholar
- Wan W, Wang C, Zhang W, Chen J, Zhou H, Zhang X: Superior performance of nanoscaled Fe3O4 as anode material promoted by mosaicking into porous carbon framework. Funct Mater Lett 2014, 7: 1450005–4. 10.1142/S1793604714500052View ArticleGoogle Scholar
- Gao XW, Feng CQ, Chou SL, Wang JZ, Sun JZ, Forsyth M, MacFarlane DR, Liu HK: LiNi0.5Mn1.5O4 spinel cathode using room temperature ionic liquid as electrolyte. Electrochim Acta 2013, 101: 151–157.View ArticleGoogle Scholar
- Feng L, Xuan Z, Bai Y, Zhao H, Li L, Chen Y, Yang X, Su C, Guo J, Chen X: Preparation of octahedral CuO micro/nanocrystals and electrochemical performance as anode for lithium-ion battery. J Alloys Compd 2014, 600: 162–167.View ArticleGoogle Scholar
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