Open Access

A simple additive-free approach for the synthesis of uniform manganese monoxide nanorods with large specific surface area

  • Mingtao Zheng1,
  • Haoran Zhang1,
  • Xuebin Gong1,
  • Ruchun Xu1,
  • Yong Xiao1,
  • Hanwu Dong1,
  • Xiaotang Liu1 and
  • Yingliang Liu1Email author
Nanoscale Research Letters20138:166

DOI: 10.1186/1556-276X-8-166

Received: 17 January 2013

Accepted: 13 March 2013

Published: 11 April 2013


A simple additive-free approach is developed to synthesize uniform manganese monoxide (MnO) one-dimensional nanorods, in which only manganese acetate and ethanol were used as reactants. The as-synthesized MnO nanorods were characterized in detail by X-ray diffraction, scanning and transmission electron microscopy (TEM) including high-resolution TEM and selected-area electron diffraction, Fourier transform infrared spectrum, and nitrogen adsorption isotherm measurements. The results indicate that the as-synthesized MnO nanorods present a mesoporous characteristic with large specific surface area (153 m2 g−1), indicating promising applications in catalysis, energy storage, and biomedical image. On the basis of experimental results, the formation mechanism of MnO one-dimensional nanorods in the absence of polymer additives was also discussed.


Manganese monoxide Nanorods Additive-free synthesis Formation mechanism


During the past decade, manganese oxides have attracted considerable research interest due to their distinctive physical and chemical properties and potential applications in catalysis, ion exchange, molecular adsorption, biosensor, and energy storage [112]. Particularly, nanometer-sized manganese oxides are of great significance in that their large specific surface areas and small sizes may bring some novel electrical, magnetic, and catalytic properties different from that of bulky materials. A wide variety of manganese oxides (e.g., MnO2, Mn2O3, and Mn3O4) have been synthesized through various methods [1324]. Among them, manganese monoxide (MnO) is a model system for theoretical study of the electronic and magnetic properties of rock salt oxides [25], and its nanoclusters interestingly exhibit ferromagnetic characteristics [26]. On the other hand, MnO is very interesting for its lower charge potential (1.0 V vs. Li/Li+) compared to other transition metal oxides [27]. It has been reported that a relatively high voltage and energy density can be obtained when it was coupled with a certain cathode material to construct a full lithium ion cell [28].

In terms of the synthesis methods of MnO, several approaches have been developed to prepare nanostructured MnO with different morphologies [2842], such as hydrothermal reactions and subsequent annealing [28], thermal decomposition of Mn-containing organometallic compounds [2932], thermal decomposition of MnCO3 precursor [33, 34], vapor-phase deposition [37], etc. More recently, Lin et al. reported a simple one-pot synthesis of monodispersed MnO nanoparticles (NPs) using bulk MnO as the starting material and oleic acid as solvent [38]. Sun et al. reported a microwave-polyol process to synthesize disk-like Mn complex precursor that was topotactically converted into porous C-modified MnO disks by post-heating treatment [41]. However, these methods are often associated with the use of high-toxicity, environmentally harmful, and high-cost organic additives. Moreover, the by-products may have a detrimental effect on the size, shape, and phase purity of the MnO NPs obtained. It still remains a major challenge to prepare high-quality monophase MnO NPs due to the uncontrollable phase transformation of multivalent manganese oxides (MnO2, Mn2O3, and Mn3O4).

In the present work, we report a simple, cost-effective, and additive-free method for the synthesis of uniform MnO nanorods with large specific surface area, in which cheap manganese acetate and ethanol were used as starting materials. The microstructures of the as-synthesized products were investigated using scanning electron microscopy (SEM) and transmission electron microscope (TEM). The as-synthesized MnO nanorods present a mesoporous characteristic and large specific surface area. More importantly, we have avoided the use of expensive polymer or surfactant additives during the synthesis process. The possible formation mechanism for MnO nanorods in the absence of polymer additives was also discussed.


Preparation of MnO nanorods

In a typical synthesis, 1.0 g of manganese acetate was put into 30 mL of anhydrous ethanol distilled freshly to form a homogeneous solution under stirring. The solution was transferred to a 40-mL Teflon-lined stainless steel autoclave. These manipulations were operated in a glove box under N2 atmosphere. The autoclave was heated at 200°C for 24 h in an electric oven. After cooling to room temperature, the final products were washed with deionized water and ethanol several times and subsequently dried at 80°C for 6 h in vacuum.

Instruments and characterization

The phase purity of the obtained samples was examined by X-ray diffraction (XRD) using an MSAL-XD2 X-ray diffractometer with CuKα radiation (λ = 0.15406 nm) operating at 40 kV and 20 mA. Morphologies of the samples were characterized by field emission scanning electron microscopy (JSM6700F). The morphology and structure of the MnO nanorods were further investigated by TEM and high-resolution transmission electron microscopy (HRTEM; JEM-2010, 200 kV) with energy-dispersive X-ray spectroscopy (EDS; INCA X200). X-ray photoelectron spectroscopy (XPS) was carried out by means of a Shimadzu AXIS UTLTRADLD spectrometer (Shimadzu, Kyoto, Japan). Nitrogen adsorption-desorption measurements were performed using a Micromeritics Tristar 3000 gas adsorption analyzer (Micromeritics Instrument Co., Norcross, GA, USA). Fourier transform infrared (FTIR) spectrum was measured by an Equinox 55 (Bruker, Ettlingen, Germany) spectrometer ranging from 400 to 4,000 cm−1.

Results and discussion

Figure 1 shows the XRD patterns of the product synthesized at 200°C for 24 h. The diffraction peaks were observed at 2θ = 34.9°, 40.6°, 58.8°, 70.3°, and 73.8°, which could be assigned to (111), (200), (220), (311), and (222) reflections, respectively. These reflections could be readily indexed to cubic MnO with a lattice constant of 4.443 Å, in good accordance with the literature values (JCPDS 89–4835). No other phases of manganese oxide could be seen, indicating the monophase of cubic MnO.
Figure 1

XRD pattern of as-prepared MnO nanorods synthesized at 200°C for 24 h.

The morphology of the as-prepared sample was examined by SEM and TEM. Figure 2a shows a typical SEM image of MnO nanorods synthesized at 200°C for 24 h, revealing that the product displays a uniform nanorod-like morphology. It can be observed that the nanorod is composed of small NPs, and the coarse surface of the nanorod can also be seen, as shown in Figure 2b. Figure 2c,d presents the TEM images of the unique MnO nanorods, showing that the lengths and diameters of the nanorods were ca. 100 to 200 nm and 20 to 30 nm, respectively. Figure 2e shows an enlarged TEM image, revealing the porous character of the nanorods. Figure 2f depicts an HRTEM image of one single nanorod, revealing that the obtained nanorod consists of small nanoparticle subunits. As shown in the inset of Figure 2f, the selected-area electron diffraction (SAED) pattern with polycrystalline-like diffraction also indicates that the nanorod is an ordered assembly of small nanocrystal subunits without crystallographic orientation, well consistent with the HRTEM results.
Figure 2

Morphology of the cubic MnO nanorods obtained at 200°C for 24 h. (a) Low-magnification and (b) high-magnification SEM images, (c, d, and e) TEM, and (f) HRTEM images. The inset in (e) is an enlarged TEM image, and the inset in (f) shows the SAED pattern of one single MnO nanorods.

The chemical composition of the as-prepared MnO nanorods was further confirmed by EDS analysis. The spectrum, taken from the center area of the nanorod, shows four strong signals of Mn, C, O, and Cu (Figure 3). The atomic ratio of Mn and O is about 1.02, indicating that the as-prepared nanorods are consist of high-purity MnO rather than other manganese oxides (e.g., Mn2O3, Mn3O4, and MnO2), in good agreement with the XRD results. The Cu and O may have resulted from the Cu gridding and C support membrane in the TEM observation.
Figure 3

EDS spectroscopy of the as-prepared MnO nanorods.

The FTIR spectrum was further performed to substantiate the formation of MnO and the organic residue on the surface of MnO nanorods. As shown in Figure 4, two strong peaks at about 630 and 525 cm−1 arise from the stretching vibration of the Mn-O and Mn-O-Mn bonds [43], indicating the formation of MnO in the present work. In addition, strong absorptions at 3,442 cm−1 and weak absorptions around 2,800 to 3,000 cm−1 reveal the stretching vibrations of O-H and C-H, respectively. The absorption peak at 1,112 cm−1 corresponds to the C-OH stretching and OH bending vibrations, whereas the bands at 1,385, 1,580, and 1,636 cm−1 correspond to C-O (hydroxyl, ester, or ether) stretching and O-H bending vibrations [44, 45]. These results indicate that some organic residues such as hydroxyl and carboxyl groups are present on the surface of the as-prepared MnO nanorods.
Figure 4

FTIR spectroscopy of the as-synthesized MnO nanorods.

The presence of the residue functionalities on the surface of the as-synthesize MnO nanorods was further characterized by XPS measurements. As shown in Figure 5, the survey spectrum shows the signals of Mn 2p, O 1s, and C 1s, indicating the presence of carbon element on the surface the nanorods. The presence of the organic groups was further confirmed by the C 1s spectrum. The inset in Figure 5 presents the C 1s core-level spectrum and the peak fitting of the C 1s envelope. Four signals at 284.8, 286.4, 287.6, and 288.8 eV were identified, which were attributed to carbon group (C = C/C-C, CH x ), hydroxyl groups or ethers (−C-OR), carbonyl or quinone groups (>C = O), and carboxylic groups, esters, or lactones (−COOR), respectively. These results also reveal the presence of organic functional groups on the surface of the nanorods, in good agreement with the FTIR results.
Figure 5

XPS survey spectrum of the as-prepared MnO nanorods. The inset shows the C 1s core-level spectrum and the peak fitting of the C 1s envelope.

The porous characteristic of the as-synthesized MnO nanorods was examined by nitrogen adsorption isotherm measurements. The specific surface area and pore size distribution (PSD) of the MnO nanorods were obtained from an analysis of the desorption branch of the isotherms using the density function theory. As shown in Figure 6, an isotherm is typical for a mesoporous material with a hysteresis loop at high partial pressures. According to the Brunauer-Emmett-Teller analysis, the as-synthesized MnO nanorods exhibited large specific surface area of ca. 153 m2 g−1 and pore volume of ca. 0.22 cm3 g−1. The inset in Figure 6 shows the Barrett-Joyner-Halenda PSD curve that was centered at ca. 3.9 nm, suggesting that the MnO nanorods possess uniform mesoporous structures.
Figure 6

N 2 adsorption-desorption isotherms and pore size distribution curve of the MnO nanorods.

To investigate the formation mechanism of the MnO nanorods, a series of time-dependent experiments were carried out. As shown in Figure 7a, numerous amorphous manganese precursor NPs with size of ca. 5 to 6 nm were observed when the reaction was executed for 1 h. Figure 7b shows that larger NPs with size of ca. 20 to 30 nm were formed when the reaction time was increased to 3 h. The inset in Figure 7b reveals that the lattice fringe is ca. 0.36 nm, consistent with the d012 spacing for rhodochrosite MnCO3, indicating that the transformation from manganese precursor to MnCO3 happened in the earlier stage. When the reaction time was increased to 6 h, many nanorod-like particles could be obtained besides dispersed NPs (Figure 7c). It can also be seen that the nanorod-like products were formed by the self-assembly of small NPs. Figure 7d shows an HRTEM image taken from two adjacent NPs. The lattice fringes were found to be ca. 0.36 and 0.26 nm, corresponding to the d102 spacing for rhodochrosite MnCO3 and the d111 spacing for cubic MnO, respectively, suggesting that the transformation from MnCO3 to cubic MnO was incomplete within a short time. When the reaction time was further increased to 12 h, a large number of nanorods were formed (Figure 7e). Figure 7f shows an HRTEM image of one nanorod aggregated by small nanocrystals, and the boundary can be observed among the NPs. The SAED pattern in the inset of Figure 7f presents a polycrystalline character of the nanorods, indicating that the nanorod is of an ordered assembly of nanocrystals without crystallographic orientation.
Figure 7

TEM images of the as-prepared products at 200°C for different reaction times. (a) 1 h, (b) 3 h, (c and d) 6 h, and (e and f) 12 h.

On the basis of the above experimental results, the possible formation mechanism of the MnO one-dimensional nanorods in the present work was proposed, as schematically illustrated in Figure 8. Firstly, the reaction between manganese acetate and ethanol results in the formation of certain alcohol acetate complexes, e.g., CH3COOMnOC2H5, accompanied with the nucleation and growth of amorphous precursor NPs, which are then transformed into MnCO3 nanocrystals (step 1). Secondly, with the increase of reaction time, the MnCO3 precursor is decomposed into MnO nanocrystallites (step 2). Meanwhile, the generated MnO nanocrystallites are capped by the short C-chain molecules forming oxide-organic hybrids, which act as build blocks to form novel MnO nanostructures. When two MnO building blocks come together, the capillary force between them facilitates the solvent removal and strengthens the agglomerate by van der Waals forces. Finally, with the increase of reaction time, directed self-assemblies of the oriented nanocrystallites and subsequent fusion lead to the formation of the MnO one-dimensional nanorods (step 3).
Figure 8

The possible formation mechanism of the MnO one-dimensional nanorods.


In summary, uniform mesocrystalline MnO nanorods were prepared successfully by using manganese acetate and ethanol as starting materials. The as-synthesized MnO nanorods exhibited uniform morphology, large specific surface area, and narrow pore size distribution. The simple, cost-effective, and environmentally friendly synthesis can be scaled up to produce large quantities of porous MnO one-dimensional nanorods. Owing to their large specific surface area, the as-prepared MnO nanorods may have promising applications in energy storage, catalysis, and biomedical image. This method may also open a new avenue for the simple synthesis of porous functional materials with applications in the fields of energy and environment.



This work was financially supported by the National Natural Science Foundation of China (21201065 and 21031001), the Natural Science Foundation of Guangdong Province (s2012040007836), the Key Program of Science Technology Innovation Foundation of Higher Education Institutions of Guangdong Province (cxzd1014), and the Minister Funds of South China Agricultural University.

Authors’ Affiliations

Department of Applied Chemistry, College of Science, South China Agricultural University


  1. Wang X, Li YD: Selected-control hydrothermal synthesis of alpha- and beta-MnO2 single crystal. J Am Chem Soc 2002, 124: 2880–2881.View ArticleGoogle Scholar
  2. Li ZQ, Ding Y, Xiong YJ, Yang Q, Xie Y: One-step solution-based catalytic route to fabricate novel alpha-MnO2 hierarchical structures on a large scale. Chem Commun 2005, 7: 918–920.Google Scholar
  3. Wang LZ, Sakai N, Ebina Y, Takada K, Sasaki T: Inorganic multilayer films of manganese oxide nanosheets and aluminum polyoxocations: fabrication, structure, and electrochemical behavior. Chem Mater 2005, 17: 1352–1357.View ArticleGoogle Scholar
  4. El-Deab MS, Ohsaka T: Manganese oxide nanoparticles electrodeposited on platinum are superior to platinum for oxygen reduction. Angew Chem Int Ed 2006, 45: 5963–5966.View ArticleGoogle Scholar
  5. Li WN, Yuan JK, 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.View ArticleGoogle Scholar
  6. Zhang WX, Yang ZH, Wang X, Zhang YC, Wen XG, Yang SH: Large-scale synthesis of beta-MnO2 nanorods and their rapid and efficient catalytic oxidation of methylene blue dye. Catal Commun 2006, 7: 408–412.View ArticleGoogle Scholar
  7. Liu DW, Zhang QF, Xiao P, Garcia BB, Guo Q, Champion R, Cao GZ: Hydrous manganese dioxide nanowall arrays growth and their Li+ ions intercalation electrochemical properties. Chem Mater 2008, 20: 1376–1380.View ArticleGoogle Scholar
  8. Fei JB, Cui Y, Yan XH, Qi W, Yang Y, Wang KW, He Q, Li JB: Controlled preparation of MnO2 hierarchical hollow nanostructures and their application in water treatment. Adv Mater 2008, 20: 452–456.View ArticleGoogle Scholar
  9. Xu CL, Zhao YQ, Yang GW, Li FS, Li HL: Mesoporous nanowire array architecture of manganese dioxide for electrochemical capacitor applications. Chem Commun 2009, 48: 7575–7577.View ArticleGoogle Scholar
  10. Yan JA, Khoo E, Sumboja A, Lee PS: Simple coating of manganese oxide on tin oxide nanowires with high-performance capacitive behavior. ACS Nano 2010, 4: 4247–4255.View ArticleGoogle Scholar
  11. Park JH, Kim JM, Jin M, Jeon JK, Kim SS, Park SH, Kim SC, Park YK: Catalytic ozone oxidation of benzene at low temperature over MnOx/Al-SBA-16 catalyst. Nanoscale Res Lett 2012, 7: 1–5.View ArticleGoogle Scholar
  12. Xia H, Wang Y, Lin J, Lu L: Hydrothermal synthesis of MnO2/CNT nanocomposite with a CNT core/porous MnO2 sheath hierarchy architecture for supercapacitors. Nanoscale Res Lett 2012, 7: 1–10.View ArticleGoogle Scholar
  13. Ma RZ, Bando YS, Zhang LQ, Sasaki T: Layered MnO2 nanobelts: hydrothermal synthesis and electrochemical measurement. Adv Mater 2004, 16: 918–922.View ArticleGoogle Scholar
  14. Wang LZ, Ebina Y, Takada K, Sasaki T: Ultrathin hollow nanoshells of manganese oxide. Chem Commun 2004, 9: 1074–1075.View ArticleGoogle Scholar
  15. Yu CC, Zhang LX, Shi JL, Zhao JJ, Cao JH, Yan DS: A simple template-free strategy to synthesize nanoporous manganese and nickel oxides with narrow pore size distribution, and their electrochemical properties. Adv Funct Mater 2008, 18: 1544–1554.View ArticleGoogle Scholar
  16. Wei WF, Cui XW, Chen WX, Ivey DG: Phase-controlled synthesis of MnO2 nanocrystals by anodic electrodeposition: implications for high-rate capability electrochemical supercapacitors. J Phy Chem C 2008, 112: 15075–15083.View ArticleGoogle Scholar
  17. Ni JP, Lu WC, Zhang LM, Yue BH, Shang XF, Lv Y: Low-temperature synthesis of monodisperse 3D manganese oxide nanoflowers and their pseudocapacitance properties. J Phys Chem C 2009, 113: 54–60.View ArticleGoogle Scholar
  18. Chen S, Zhu JW, Han QF, Zheng ZJ, Yang Y, Wang X: Shape-controlled synthesis of one-dimensional MnO2 via a simple quick-precipitation procedure and its electrochemical properties. Cryst Growth Des 2009, 9: 4356–4361.View ArticleGoogle Scholar
  19. Gui Z, Fan R, Chen XH, Wu YC: A simple direct preparation of nanocrystalline γ-Mn2O3 at ambient temperature. Inorg Chem Commun 2001, 4: 294–296.View ArticleGoogle Scholar
  20. Lei SJ, Tang KB, Fang Z, Liu QC, Zheng HG: Preparation of α-Mn2O3 and MnO from thermal decomposition of MnCO3 and control of morphology. Mater Lett 2006, 60: 53–56.View ArticleGoogle Scholar
  21. Cao J, Zhu Y, Bao K, Shi L, Liu S, Qian Y: Microscale Mn2O3 hollow structures: sphere, cube, ellipsoid, dumbbell, and their phenol adsorption properties. J Phys Chem C 2009, 113: 17755–17760.View ArticleGoogle Scholar
  22. Cheney MA, Hanifehpour Y, Joo SW, Min BK: A simple and fast preparation of neodymium-substituted nanocrystalline Mn2O3. Mater Res Bull 2013, 48: 912–915.View ArticleGoogle Scholar
  23. Sambasivam S, Li GJ, Jeong JH, Choi BC, Lim KT, Kim SS, Song TK: Structural, optical, and magnetic properties of single-crystalline Mn3O4 nanowires. J Nanop Res 2012, 14: 1138/1–1138/9.Google Scholar
  24. Li J, Li L, Wu F, Zhang L, Liu X: Dispersion-precipitation synthesis of nanorod Mn3O4 with high reducibility and the catalytic complete oxidation of air pollutants. Catal Commun 2013, 31: 52–56.View ArticleGoogle Scholar
  25. Nayak SK, Jena P: Equilibrium geometry, stability and magnetic properties of small MnO clusters. J Am Chem Soc 1999, 121: 644–652.View ArticleGoogle Scholar
  26. Lee GH, Huh SH, Jeong JW, Choi BJ, Kim SK, Ri HC: Anomalous magnetic properties of MnO nanoclusters. J Am Chem Soc 2002, 124: 12094–12095.View ArticleGoogle Scholar
  27. Poizot P, Laruelle S, Grugeon S, Tarascon JM: Rationalization of the low-potential reactivity of 3d-metal-based inorganic compounds toward Li. J Electrochem Soc 2002, 149: A1212-A1217.View ArticleGoogle Scholar
  28. Fang XP, Lu X, Guo XW, Mao Y, Hu YS, Wang JZ, Wang ZX, Wu F, Liu HK, Chen LQ: Electrode reactions of manganese oxides for secondary lithium batteries. Electrochem Commun 2010, 12: 1520–1523.View ArticleGoogle Scholar
  29. Park J, Kang EA, Bae CJ, Park JG, Noh HJ, Kim JY, Park JH, Park JH, Hyeon T: Synthesis, characterization, and magnetic properties of uniform-sized MnO nanospheres and nanorods. J Phys Chem B 2004, 108: 13594–13598.View ArticleGoogle Scholar
  30. Zitoun D, Pinna N, Frolet N, Belin C: Single crystal manganese oxide multipods by oriented attachment. J Am Chem Soc 2005, 127: 15034–15035.View ArticleGoogle Scholar
  31. Shanmugam S, Gedanken A: MnO octahedral nanocrystals and MnO@C core-shell composites: synthesis, characterization, and electrocatalytic properties. J Phys Chem B 2006, 110: 24486–24491.View ArticleGoogle Scholar
  32. Ghosh M, Biswas K, Sundaresan A, Rao CNR: MnO and NiO nanoparticles: synthesis and magnetic properties. J Mater Chem 2006, 16: 106–111.View ArticleGoogle Scholar
  33. Lei S, Tang K, Fang Z, Liu Q, Zheng H: Preparation of α-Mn2O3 and MnO from thermal decomposition of MnCO3 and control of morphology. Mater Lett 2006, 60: 53–56.View ArticleGoogle Scholar
  34. Liu Y, Zhao X, Li F, Xia D: Facile synthesis of MnO/C anode materials for lithium-ion batteries. Electrochim Acta 2011, 56: 6448–6452.View ArticleGoogle Scholar
  35. Chen YF, Johnson E, Peng XG: Formation of monodisperse and shape-controlled MnO nanocrystals in non-injection synthesis: Self-focusing via ripening. J Am Chem Soc 2007, 129: 10937–10947.View ArticleGoogle Scholar
  36. Zhong KF, Zhang B, Luo SH, Wen W, Li H, Huang XJ, Chen LQ: Investigation on porous MnO microsphere anode for lithium ion batteries. J Power Sources 2011, 196: 6802–6808.View ArticleGoogle Scholar
  37. Banis MN, Zhang Y, Banis HN, Li R, Sun X, Jiang X, Nikanpour D: Controlled synthesis and characterization of single crystalline MnO nanowires and Mn-Si oxide heterostructures by vapor phase deposition. Chem Phys Lett 2011, 501: 470–474.View ArticleGoogle Scholar
  38. Li SR, Sun Y, Ge SY, Qiao Y, Chen YM, Lieberwirth I, Yu Y, Chen CH: A facile route to synthesize nano-MnO/C composites and their application in lithium ion batteries. Chem Eng J 2012, 192: 226–231.View ArticleGoogle Scholar
  39. Lin CC, Chen CJ, Chiang RK: Facile synthesis of monodisperse MnO nanoparticles from bulk MnO. J Crystal Growth 2012, 338: 152–156.View ArticleGoogle Scholar
  40. Nam KM, Kim , Kim YI, Jo Y, Lee SM, Kim BG, Choi R, Choi SI, Song H, Park JT: New crystal structure: synthesis and characterization of hexagonal wurtzite MnO. J Am Chem Soc 2012, 134: 8392–8395.View ArticleGoogle Scholar
  41. Sun YM, Hu XL, Luo W, Huang YH: Porous carbon-modified MnO disks prepared by a microwave-polyol process and their superior lithium-ion storage properties. J Mater Chem 2012, 22: 19190–19195.View ArticleGoogle Scholar
  42. Xu G, Zhang L, Guo C, Gu L, Wang X, Han P, Zhang K, Zhang C, Cui G: Manganese monoxide/titanium nitride composite as high performance anode material for rechargeable Li-ion batteries. Electrochim Acta 2012, 85: 345–351.View ArticleGoogle Scholar
  43. Chen H, He J: Facile synthesis of monodisperse manganese oxide nanostructures and their application in water Treatment. J Phys Chem C 2008, 112: 17540–17545.View ArticleGoogle Scholar
  44. Zheng M, Liu Y, Jiang K, Xiao Y, Yuan D: Alcohol-assisted hydrothermal carbonization to fabricate spheroidal carbons with a tunable shape and aspect ratio. Carbon 2010, 48: 1224–1233.View ArticleGoogle Scholar
  45. Sevilla M, Fuertes AB: Chemical and structural properties of carbonaceous products obtained by hydrothermal carbonization of saccharides. Chem Eur J 2009, 15: 4195–4203.View ArticleGoogle Scholar


© Zheng et al.; licensee Springer. 2013

This article is published under license to BioMed Central Ltd. This is an Open Access article distributed under the terms of the Creative Commons Attribution License (, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.