- About this Journal ·
- Abstracting and Indexing ·
- Aims and Scope ·
- Annual Issues ·
- Article Processing Charges ·
- Articles in Press ·
- Author Guidelines ·
- Bibliographic Information ·
- Citations to this Journal ·
- Contact Information ·
- Editorial Board ·
- Editorial Workflow ·
- Free eTOC Alerts ·
- Publication Ethics ·
- Reviewers Acknowledgment ·
- Submit a Manuscript ·
- Subscription Information ·
- Table of Contents
Journal of Nanomaterials
Volume 2011 (2011), Article ID 961389, 4 pages
Fabrication of VO2 (B) Nanobelts and Their Application in Lithium Ion Batteries
1College of Mechanical and Material Engineering, China Three Gorges University, Yichang 443002, China
2Key Laboratory for Intelligent Nanomaterials and Devices (MOE), Institute of Nanoscience and Department of Material Science, Nanjing University of Aeronautics and Astronautics, Yudao Road 29, Nanjing 210016, China
Received 5 June 2011; Accepted 11 July 2011
Academic Editor: Renzhi Ma
Copyright © 2011 Shibing Ni et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.
VO2 (B) nanobelts have been successfully synthesized via a simple hydrothermal route. The products were characterized by X-ray diffraction (XRD), field emission scanning electron microscopy (FE-SEM), and Raman spectrum. These nanobelts are of rectangular cross-section with mean length about 1 μm, mean width about 80 nm, and mean thickness about 50 nm. The as-synthesized VO2 nanobelts were assembled as the cathode electrodes of lithium ion batteries. Their electrochemical properties were studied by conventional charge/discharge tests, which show an initial discharge capacity of 321 mAh g−1 with voltage plateau near 2.5 V. These results indicated that such hydrothermally synthesized VO2 (B) nanobelts could be an ideal candidate of cathode material for lithium ion battery.
During the past few years, vanadium-oxides-based materials have attracted much attention due to their fascinating structures and electronic, optical, and magnetic properties, which are relevant to such diverse areas as lubrication, chemical sensor, catalysis, cathode materials in batteries, and minerals [1–7].
Metastable phase oxide VO2 (B) is built up of distorted VO6 octahedra sharing edges and corners  and has been found to be of interesting cathode properties in lithium ion batteries . However, VO2 (B) is very difficult to synthesize by conventional high temperature procedures because the phase change from metastable VO2 (B) to thermodynamically more stable rutile VO2 will occur at and the latter shows no attractive electrochemical properties . The synthesis of VO2 (B) hierarchical structures is generally achieved via low-temperature chemical methods [8, 11–13], which can hardly be separated from toxic reducing agent and usually need long reaction time. So we are interested in developing simple methods to synthesize VO2 (B) nanostructures using nontoxic reducing agent and exploring its morphology-related electrochemical properties. Among different nanostructures, one-dimensional (1D) nanostructured VO2 (B) has attracted special attention due to its high surface-to-volume ratio, which is strongly relevant to its electrochemical performances. VO2 (B) nanowires, nanobelts, nanoribbons, nanoneedles, and nanorods were respectively synthesized [14–18]. To the best of our knowledge, the synthesis of 1D nanostructured VO2 (B) with rectangular cross-section is rarely achieved due to the intrinsic growth habit of VO2 (B) crystal . Here, we report a simple hydrothermal approach to synthesize VO2 (B) nanobelts with rectangular cross-section using nontoxic glucose as reducing agent, and its electrochemical properties are studied by conventional charge/discharge tests.
All the chemicals were of analytical grade and purchased from Shanghai Chemical Reagents. In a typical procedure, 1 mmol V2O5 and 0.5 mmol glucose were dissolved in 30 mL distilled water, and then 0.5 g sodium sulfate was put into the solution. After stirring for 20 minutes, the obtained homogeneous yellowy suspension was transferred into a 50 mL teflon-lined autoclave, and distilled water was subsequently added up to 80% of its capacity. The autoclave was at last sealed and placed in an oven, heated at 160°C for 24 h. The precipitate was centrifuged with distilled water and ethanol both for 4 times and dried in an oven at 60°C for 24 h.
The morphology and structure of the resulting products were characterized by field-emission scanning electron microscopy (FE-SEM S-4800, Hitachi), X-ray powder diffraction (Rigaku RINT2400 with Cu Kα radiation), and micro-Raman spectrometer (Jobin Yvon LabRAM HR800 UV, YGA 532 nm). For fabricating of lithium ion batteries, a mixture of 80 wt% of active material, 10 wt% of acetylene black, and 10 wt% of polyvinylidene fluoride (PVDF) dissolved in N-methylpyrrolidone (NMP) solution (0.02 g mL−1) was coated on aluminum foil and cut into disc electrodes with a diameter of 14 mm using a punch. Coin-type cells (2025) of Li/1 M LiPF6 in ethylene carbonate, dimethyl carbonate and diethyl carbonate (EC/DMC/DEC, 1 : 1 : 1 v/v/v + VC)/VO2 were assembled in an argon-filled glove box. A Celgard 2400 microporous polypropylene was used as the separator membrane. The cells were tested in the voltage region between 1.5 V and 3.75 V with a multichannel batteries test system (LAND CT2001A).
3. Results and Discussion
Typical XRD pattern of the as-synthesized products is shown in Figure 1. All diffraction peaks can be indexed as monoclinic cell of VO2 (B) with cell parameters Å, Å, and Å, which is in good agreement with the JCPDS, no. 31-1438, indicating the formation of pure phase VO2 (B). The strong and sharp diffraction peaks suggest that the as-synthesized products are well crystallized.
Figure 2(a) is a low magnification SEM image of the as-synthesized VO2 (B), showing a large quantity of nanobelts. For further clarification of the morphology and size of those nanobelts, an SEM image with high magnification is shown in Figure 2(b). It can be found that those nanobelts are of rectangular cross-section with mean length about 1 μm, mean width about 80 nm, and mean thickness about 50 nm, respectively.
As shown in Figure 3, Raman spectrum in the wavelength range of 150 cm−1 ~ 1500 cm−1 is dominated by the peaks at 170 cm−1, 271 cm−1, 438 cm−1, 519 cm−1, 705 cm−1, and 985 cm−1, and these peaks are the vibration bands of VO2 (B) . The peaks at 170 cm−1 and 271 cm−1 can be assigned to V–O–V bending modes and external mode (bending/wagging), respectively. The peaks at 438 cm−1 and 519 cm−1 are attributed to V–O–V stretching mode. The peak at 705 cm−1 is due to coordination of vanadium atoms with three oxygen atoms, while the peak at 985 cm−1 is attributed to V=O stretching of distorted octahedral and distorted square-pyramids [19–22]. These Raman results are highly accordant with above XRD pattern and further confirm the formation of monoclinic VO2 (B).
Figure 4 is the 1st and 2nd discharge and charge curves of VO2 (B) nanobelts electrode at a current density of 214 mA g−1. It shows a high initial discharge capacity of 316 mAh g−1 with clear voltage plateau near 2.5 V, while the first charge capacity is 321 mAh g−1 with distinct voltage plateau near 2.62 V. The charge and discharge capacities show little attenuation, which indicates a highly reversible intercalation and extraction of Lithium ions. In the 2nd discharge and charge curve, the discharge and charge capacities are 323 mAh g−1 and 319 mAh g−1 and the voltage plateaus locate at near 2.52 V and 2.64 V, respectively. The charge and discharge behavior of our VO2 (B) nanobelts is similar to that reported in the literature [13, 17, 18], but with smaller capacity attenuation. We propose that the unique synthesis environment in hydrothermal method and the special morphology of the as-synthesized VO2 (B) nanobelts are the causations of its good electrochemical performance.
In conclusion, VO2 (B) nanobelts with rectangular cross-section are synthesized via a simple hydrothermal route. Electrochemical properties of the as-synthesized VO2 nanobelts as cathode electrode of lithium ion batteries are studied by conventional charge/discharge tests, which show high discharge/charge capacity and steady voltage plateaus, indicating that it is suitable for the application in lithium ion batteries as cathode electrode material.
The authors gratefully acknowledge the financial support from Natural Science Foundation of China (NSFC, 50972075), key projects of Chinese Ministry of Education (D209083) and Education Office of Hubei Province (Q20111209, D20081304, and CXY2009A004). Moreover, the authors are grateful to Dr. Jianlin Li at China Three Gorges University for his kind support to their research.
- E. Lugscheider, O. Knotek, S. Bärwulf, and K. Bobzin, “Characteristic curves of voltage and current, phase generation and properties of tungsten- and vanadium-oxides deposited by reactive d.c.-MSIP-PVD-process for self-lubricating applications,” Surface and Coatings Technology, vol. 142–144, pp. 137–142, 2001.
- A. Lavacchi, B. Cortigiani, G. Rovida, et al., “Composition and structure of tin/vanadium oxide surfaces for chemical sensing applications,” Sensors and Actuators B, vol. 71, no. 1-2, pp. 123–126, 2000.
- W. P. Griffith, “Polyoxometallates as homogeneous cataysts for organic oxidations,” Transition Metal Chemistry, vol. 16, no. 5, pp. 548–552, 1991.
- I. V. Kozhevnikov, “Advances in catalysis by heteropolyacids,” Russian Chemical Reviews, vol. 56, no. 9, pp. 811–825, 1987.
- A. R. Armstrong, C. Lyness, P. M. Panchmatia, M. S. Islam, and P. G. Bruce, “The lithium intercalation process in the low-voltage lithium battery anode Li1+x V1-x O2,” Nature Materials, vol. 10, no. 3, pp. 223–229, 2011.
- L. Mai, L. Xu, C. Han et al., “Electrospun ultralong hierarchical vanadium oxide nanowires with high performance for lithium ion batteries,” Nano Letters, vol. 10, no. 11, pp. 4750–4755, 2010.
- H. T. Evans and J. A. Konnert, “The crystal chemistry of sherwoodite, a calcium 14-vanadoaluminate heteropoly complex,” American Mineralogist, vol. 63, no. 9-10, pp. 863–868, 1978.
- G. Grymonprez, L. Fiermans, and J. Vennik, “Structural properties of vanadium oxides,” Acta Crystallographica, vol. A33, no. 5, pp. 834–837, 1977.
- A. M. Kannan and A. Manthiram, “Synthesis and electrochemical evaluation of high capacity nanostructured VO2 cathodes,” Solid State Ionics, vol. 159, no. 3-4, pp. 265–271, 2003.
- C. Tsang and A. Manthiram, “Synthesis of nanocrystalline VO2 and its electrochemical behavior in lithium batteries,” Journal of the Electrochemical Society, vol. 144, no. 2, pp. 520–524, 1997.
- K. F. Zhang, S. J. Bao, X. Liu, J. Shi, Z. X. Su, and H. L. Li, “Hydrothermal synthesis of single-crystal VO2(B) nanobelts,” Materials Research Bulletin, vol. 41, no. 11, pp. 1985–1989, 2006.
- X. Wu, Y. Tao, L. Dong, Z. Wang, and Z. Hu, “Preparation of VO2 nanowires and their electric characterization,” Materials Research Bulletin, vol. 40, no. 2, pp. 315–321, 2005.
- Z. Chen, S. Gao, L. Jiang, M. Wei, and K. Wei, “Crystalline VO2 (B) nanorods with a rectangular cross-section,” Materials Chemistry and Physics, vol. 121, no. 1-2, pp. 254–258, 2010.
- G. Armstrong, J. Canales, A. R. Armstrong, and P. G. Bruce, “The synthesis and lithium intercalation electrochemistry of VO2(B) ultra-thin nanowires,” Journal of Power Sources, vol. 178, no. 2, pp. 723–728, 2008.
- X. Liu, G. Xie, C. Huang, Q. Xu, Y. Zhang, and Y. Luo, “A facile method for preparing VO2 nanobelts,” Materials Letters, vol. 62, no. 12-13, pp. 1878–1880, 2008.
- L. Mao and C. Liu, “A new route for synthesizing VO2(B) nanoribbons and 1D vanadium-based nanostructures,” Materials Research Bulletin, vol. 43, no. 6, pp. 1384–1392, 2008.
- F. Sediri, F. Touati, and N. Gharbi, “From V2O5 foam to VO2(B) nanoneedles,” Materials Science and Engineering B, vol. 129, no. 1–3, pp. 251–255, 2006.
- C. V. S. Reddy, E. H. Walker Jr., S. A. Wicker Sr., Q. L. Williams, and R. R. Kalluru, “Synthesis of VO2 (B) nanorods for Li battery application,” Current Applied Physics, vol. 9, no. 6, pp. 1195–1198, 2009.
- J. Twu, C. F. Shih, T. H. Guo, and K. H. Chen, “Raman spectroscopic studies of the thermal decomposition mechanism of ammonium metavanadate,” Journal of Materials Chemistry, vol. 7, no. 11, pp. 2273–2277, 1997.
- F. D. Hardcastle and I. E. Wachs, “Determination of vanadium-oxygen bond distances and bond orders by Raman spectroscopy,” Journal of Physical Chemistry, vol. 95, no. 13, pp. 5031–5041, 1991.
- J. Twu and P. K. Dutta, “Structure and reactivity of oxovanadate anions in layered lithium aluminate materials,” Journal of Physical Chemistry, vol. 93, no. 23, pp. 7863–7868, 1989.
- S. Onodera and Y. Ikegami, “Synthesis and properties of chlorine(I) and bromine(I) trifluoromethanesulfonates and Raman spectra of CF3SO2X (X=fluorine, hydroxyl, hypochlorite),” Inorganic Chemistry, vol. 19, no. 3, pp. 615–618, 1980.