Open Access

Hydrothermal Synthesis and Photocatalytic Property of β-Ga2O3 Nanorods

Nanoscale Research Letters201510:364

Received: 9 June 2015

Accepted: 6 September 2015

Published: 16 September 2015


Gallium oxide (Ga2O3) nanorods were facilely prepared by a simple hydrothermal synthesis, and their morphology and photocatalytic property were studied. The gallium oxide hydroxide (GaOOH) nanorods were formed in aqueous growth solution containing gallium nitrate and ammonium hydroxide at 95 °C of growth temperature. Through the calcination treatment at 500 and 1000 °C for 3 h, the GaOOH nanorods were converted into single crystalline α-Ga2O3 and β-Ga2O3 phases. From X-ray diffraction analysis, it could be confirmed that a high crystalline quality of β-Ga2O3 nanorods was achieved by calcinating at 1000 °C. The thermal behavior of the Ga2O3 nanorods was also investigated by differential thermal analysis, and their vibrational bands were identified by Fourier transform infrared spectroscopy. In order to examine the photocatalytic activity of samples, the photodegradation of Rhodamine B solution was observed under UV light irradiation. As a result, the α-Ga2O3 and β-Ga2O3 nanorods exhibited high photodegeneration efficiencies of 62 and 79 %, respectively, for 180 min of UV irradiation time.


Gallium oxides Nanostructures Chemical synthesis Photocatalytic properties


In recent years, various fabrication methods of photocatalytic products have been developed for the photodegradation of organic and inorganic pollutants in the environment [1, 2]. Particularly, inorganic semiconductor nanomaterials have been considered to be promising for photocatalyst applications because they provide good physical and chemical properties with large surface area, and a variety of morphologies, such as nanorods, cubes, spheres, and flowers, could be achieved by the chemical synthesis [38]. In addition to the morphology and surface area of particles, the other factors which can influence the catalytic activity are pore volume, pore size, crystallinity, defect sites, exposed facets, etc. The electron transport mechanism and the exposed facets are related to the morphology of particles. In the one-dimensional (1D) morphology, the generation of electron charge carriers is higher along the elongated nanostructures and gives rise to fast transport of charge carriers, due to the hampering of recombination of charge carriers. Hence, 1D nanostructures are gaining more importance for their use in different applications as seen by latest reports [9, 10]. For example, Liu et al. studied the morphology-dependent photocatalytic properties of bare zinc oxide nanocrystals [11], which indicated that the rod-shaped ZnO nanostructures have higher photocatalytic activity than the multi-layer disks or truncated hexagonal cones. Similarly, Han et al. also studied the morphology-related properties of nano/microstructured ZnO crystallites [12]. Gallium oxide (Ga2O3) nanostructures have been recognized as an important material for several applications including catalysts, gas sensors, solar cells, and photodetectors due to their wide bandgap energy (E g = 4.2 to 4.7 eV) and good luminescence properties [1316]. Typically, the Ga2O3 nanostructures could be obtained by calcination of gallium oxide hydroxide (GaOOH) which has been synthesized via various fabrication routes including thermal evaporation, hydrothermal, sol-gel, and microwave-assisted methods [1719].

In order to obtain such GaOOH nanostructures by using a facile hydrothermal method, gallium nitrate was chemically reacted with various alkalis such as NaOH, NH4OH, KOH, and Na2CO3 [20, 21]. Then, the phase of the GaOOH nanostructures was changed into the rhombohedral crystal structure (α-Ga2O3) and monoclinic crystal structure (β-Ga2O3) after calcination [22, 23]. The crystal structures of Ga2O3 nanostructures strongly affect the chemical property and photocatalytic activity, but they still have not been completely studied. In this work, we prepared and characterized two kinds of Ga2O3 nanorods (α- and β-crystal structures) via a facile hydrothermal synthesis and proper calcination. By changing the temperature of the growth solution, the morphological properties of GaOOH nanostructures were investigated. Previously, there are so many reports on the preparation of Ga2O3 nanorods by hydrothermal and solvothermal methods which include complex instruments, making it an expensive approach. Girija et al. synthesized Ga2O3 nanostructures by the reflux method [24], Li et al. and Wang et al. used hydrothermal synthesis (autoclave) [25, 26], and Zhang et al. used the solvothermal method (autoclave) to obtain the Ga2O3 nanostructures [27]. However, in this work, we chose a simple and cost-effective process in which a beaker on a hotplate is used to produce crystalline Ga2O3 nanostructures. To characterize the structural property and functional group of the prepared samples, field-emission scanning electron microscopy (FE-SEM), X-ray diffraction (XRD), transmission electron microscopy (TEM), and Fourier transform infrared spectroscopy (FT-IR) analyses were employed. Also, the photocatalytic feasibility of Ga2O3 nanorods was evaluated by measuring the UV-vis absorption spectrum with a Rhodamine B (RhB) solution for environmental applications.


The GaOOH nanorods were synthesized by the hydrothermal synthesis method using analytical pure grade chemicals. To make the growth solution, 0.1 M of gallium(III) nitrate hydrate (Ga(NO3)3·nH2O) was dissolved in 100 ml of de-ionized (DI) water. Then, the aqueous solution was heated on a hot plate at different temperatures from room temperature to 95 °C. While the temperature of the growth solution was maintained, ammonium hydroxide (NH4OH) was slowly added into the solution until a pH of 9 is reached. The final solution was then heated for 5 h to get a white precipitate of GaOOH nanorods. After the solution was naturally cooled down to room temperature, the precipitate was filtered and washed with DI water. Then, the sample was dried in an oven at 70 °C for 5 h under ambient atmosphere. Further, the as-prepared GaOOH nanorods were calcinated at different temperatures of 500, 800, and 1000 °C for 3 h to obtain the α- and β-Ga2O3 powders.

For the morphological and structural analysis, FE-SEM (LEO SUPRA 55, Carl Zeiss), TEM (JEM-2100F, JEOL), and XRD (M18XHF-SRA, Mac Science) measurements were utilized. The thermal behavior of the GaOOH nanorods was investigated by thermogravimetric analysis-differential scanning calorimetry (TGA-DSC: SDT Q600 V8.3 Build 101). The FT-IR spectrum was scanned and analyzed in the wavenumber range of 4000–400 cm−1 by using a FT-IR measurement system (Spectrum 100, PerkinElmer). The photocatalytic properties of α- and β-Ga2O3 nanorods for the degradation of Rhodamine B (RhB) aqueous solution were characterized by measuring the absorbance of the irradiated solution. For UV irradiation, the 100-W UV lamp (SXT-20-M, UVitec) was used as a light source. To prepare the suspension of the photocatalyst, 50 mg of Ga2O3 nanorod powders was mixed with 50 ml of RhB aqueous solution (2 × 10−4 M), which was continuously stirred at room temperature in the dark for 30 min. Then, the suspension was irradiated at different illumination times from 30 to 180 min. After that, the aliquot was separated from Ga2O3 nanorod powders by using a filter paper and then the absorbance of RhB solution was obtained using a UV-vis spectrophotometer (CARY 300 Bio, Varian).

Results and Discussion

Figure 1 shows the FE-SEM images of GaOOH nanostructures synthesized via the hydrothermal method with different growth temperatures of (a) room temperature, (b) 50 °C, (c) 75 °C, and (d) 95 °C for 5 h. In general, the growth temperature plays an important role in controlling the size and shape of GaOOH nanostructures during the hydrothermal process. As shown in Fig. 1a, the cocoon-shaped GaOOH nanostructures were formed at room temperature and their size was approximately 100 nm. These cocoon-shaped structures were formed by multi-layers of small nanoplates. As the growth temperature was increased to 50 °C, the nanoplates merge together with the increase in thickness and width of each nanoplate due to Ostwald’s ripening as seen in Fig. 1b. Ostwald’s ripening continues further when the growth temperature is up to 75 °C and the multi-layered stacked structures were converted to a rod-shaped structure (Fig. 1c). With further increase of the growth solution temperature (95 °C), nanorods grow lengthwise and the width of the rods decreases as can be seen in Fig. 1d. The inset of Fig. 1d shows a single nanorod with lengths of a few micrometers and widths of approximately 1 μm. From the inset, we can also observe that the nanorod is ready to split into two rods of smaller size if the temperature of the growth solution is further increased.
Fig. 1

Effect of reaction temperature on the morphology of GaOOH nanostructures. FE-SEM images of the grown GaOOH nanostructures via hydrothermal method with different growth temperatures of a room temperature, b 50 °C, c 75 °C, and d 95 °C for 5 h

Figure 2 shows the 2θ scanned XRD patterns of (a) the as-prepared GaOOH nanorods and α-Ga2O3 calcined at 500 °C and (b) the β-Ga2O3 calcined at 800 and 1000 °C for 3 h. Here, the GaOOH nanorods were hydrothermally grown at 95 °C. As shown in Fig. 2a, the measured XRD peaks of the as-prepared GaOOH material well agreed with the crystallized orthorhombic structure (JCPDS no. 06-0180). The sharp dominant peak of the crystal planes (110), (130), (111), and (240) were observed at 2θ = 21.5, 33.7, 37.2, and 54.02°, respectively. For the calcined sample at 500 °C, it was observed that the as-prepared GaOOH nanorods were converted into α-Ga2O3 of the orthorhombic structure (JCPDS no. 06-0503) with dominant XRD peaks of (104) and (110) planes. When the calcination temperature was increased above 500 °C, as shown in Fig. 2b, the samples were changed into a monoclinic β-Ga2O3 (JCPDS no. 76-0573) without any impurity peaks. As the calcination temperature was increased to 1000 °C, the XRD patterns were clearly enhanced with sharp peaks owing to the improved crystallinity at relatively high calcination temperature. The sharp dominant peaks of the (\( \overline{4}01 \)), (002), (111), and (512) planes were observed at 2θ = 30.4, 31.8, 35.3, and 64.71°, respectively.
Fig. 2

XRD of samples calcinated at different temperatures. 2θ scanned XRD patterns of a the as-prepared GaOOH nanorods and α-Ga2O3 calcined at 500 °C for 3 h and b the β-Ga2O3 calcined at 800 and 1000 °C for 3 h. Here, the GaOOH nanorods were hydrothermally grown at 95 °C

Figure 3a shows the measured TGA-DSC curves of the as-prepared GaOOH nanorods by heating from room temperature to 1000 °C with a fixed rate of 10 °C/min in a nitrogen atmosphere. In the TGA curve of GaOOH, the total weight loss was 12.07 % from 200 to 800 °C from the weight loss step process due to the physical removal of the absorbed water on the surface of GaOOH. For the endothermic peaks at 413.2 °C in the DSC curve, the phase transformation of GaOOH into α-Ga2O3 is well consistent with the measured XRD patterns of Fig. 2a. The weak endothermic peak was also observed at the temperature between 750 and 830 °C with a weight loss of 2 % for the conversion from α-Ga2O3 to β-Ga2O3 phase in the DSC curve. With further prolonged heating up to 1000 °C, there is no weight loss. Figure 3b shows the measured FT-IR spectra in the range of 4000 to 400 cm−1 for the as-prepared GaOOH, α-Ga2O3, and β-Ga2O3 nanorods. The as-prepared GaOOH exhibited two broad band peaks around 3252.17 and 1932.62 cm−1 which are assigned to the stretching vibration of H-O-H bands. Also, the stretching vibration bond of the O-H group is also observed around 1314 cm−1 owing to the absorption of water molecules. The constitutional bending vibration of Ga-OH bands was observed at 1014 and 941 cm−1. As the sample was calcined above 500 °C, the peaks disappeared in the range of 4000–700 cm−1 due to the dehydration of water molecules. For the α-Ga2O3 nanorods calcined at 500 °C, the weak stretching peaks of the Ga-O band were observed at 687, 577, and 468 cm−1, respectively. In contrast, the β-Ga2O3 nanorods calcined at 1000 °C clearly revealed the strong and narrow peaks at 659 and 441 cm−1, respectively. These FT-IR results well agreed with the trend of crystallinity for the Ga2O3 nanorods with different calcination temperatures from the XRD data (Fig. 2).
Fig. 3

TGA-DSC curve and FT-IR spectra. a Measured TGA-DSC curves of the as-prepared GaOOH nanorods by heating from room temperature to 1000 °C with a fixed rate of 10 °C/min in a nitrogen atmosphere and b measured FT-IR spectra in the range of 4000 to 400 cm−1 for the as-prepared GaOOH, α-Ga2O3, and β-Ga2O3 nanorods

Figure 4 shows the TEM images and selected area electron diffraction (SAED) patterns of β-Ga2O3 nanorods calcined at 1000 °C. As can be seen in the perspective view of the TEM image (Fig. 4a), the single β-Ga2O3 nanorod exhibited a length of ~3 μm and a diameter of ~280–400 nm with many nanoholes. The porous structure of β-Ga2O3 nanorods was also previously reported by Liu et al. and Prakasham et al. [28, 29]. This pore surface of β-Ga2O2 nanorods was formed during the decomposition since water molecules were eliminated, thus leading to the creation of a lot of vacancies. In Fig. 4b, the many holes had a size of ~20 nm, as clearly observed in the high-magnification view of the TEM image. From the high-resolution TEM (HRTEM) images in Fig. 4c, the line array of lattice fringes (\( \overline{3}11 \)) was measured with a spacing of d = 0.235 nm, which is reasonable in comparison with the measured crystal plane of the corresponding XRD peak. From the SAED pattern of β-Ga2O3 nanorods, it was also supported that the GaOOH nanorods could be well converted into the β-Ga2O3 phase with good crystallinity by calcinating at 1000 °C.
Fig. 4

TEM images of β-Ga2O3 nanorods. a, b TEM images and c HRTEM image of the calcined β-Ga2O3 nanorods at 1000 °C. The SAED pattern of the corresponding sample is shown in d

To examine the photocatalytic activity of α-Ga2O3 and β-Ga2O3 nanorods, the photodegradation of RhB solution containing each sample was characterized. Figure 5 shows the measured absorbance spectra of the RhB solution at different UV irradiation times in the presence of (a) (i) α-Ga2O3 and (ii) β-Ga2O3 nanorods. From both the absorbance spectra, it is commonly observed that the absorption maximum of RhB occurred at 553 nm. As the UV irradiation time was increased from 0 to 60 min, the α-Ga2O3 and β-Ga2O3 nanorods exhibited a similar degradation of the absorption maximum. However, the absorbance peak of α-Ga2O3 nanorods was slowly reduced for longer UV irradiation time than 90 min. Meanwhile, the RhB solution shows the steady photodegradation up to 180 min of UV irradiation time by the photocatalyst of β-Ga2O3 nanorods. In general, the photocatalytic adsorption and desorption equilibrium are followed by a well-known Langmuir-Hinshelwood mechanism [30]. When the photon was absorbed into the photocatalyst, the photogenerated electron-hole separation contributed to the degradation of the RhB dye. Herein, this photocatalytic activity closely depends on the crystallinity and surface area [3133]. The good crystallinity and porous surface of β-Ga2O3 nanorods, from the XRD and TEM analyses (Figs. 2 and 4), led to the stable photocatalytic property compared to the α-Ga2O3 nanorods. Figure 5b shows the calculated constant reaction rate of the photodegradation of RhB solution (C/C 0) as a function of UV irradiation time for α-Ga2O3 and β-Ga2O3 nanorods. Here, C 0 is the initial concentration of the RhB dye and C is the concentration of the UV-irradiated RhB solution. For comparison, the self-degradation rate of RhB solution was also shown by obtaining the C/C 0 without photocatalyst. When the UV irradiation time was increased, the β-Ga2O3 nanorods provided a more efficient constant reaction rate. At 180 min of UV irradiation time, the photodegradation efficiency reached to 62 and 79 % for the α-Ga2O3 and β-Ga2O3 nanorods, respectively. The inset of Fig. 5b shows the photographic images of the RhB solution with β-Ga2O3 nanorods at different UV irradiation times. As the UV irradiation time was increased, it is clearly observed that the initial pink color of the RhB solution gradually disappeared, exhibiting a colorless solution. These fabrication methods and characterizations suggest that hydrothermally synthesized β-Ga2O3 nanorods can be expected to be a promising alternative for photocatalysts in the environmental remediation process.
Fig. 5

Photocatalytic activity of α-Ga2O3 and β-Ga2O3 under UV irradiation. Measured absorbance spectra of the RhB solution at different UV irradiation times in the presence of a (i) α-Ga2O3 and (ii) β-Ga2O3 nanorods. b Calculated constant reaction rate of the photodegradation of RhB solution (C/C 0) as a function of UV irradiation time for α-Ga2O3 and β-Ga2O3 nanorods. The photographic images of the RhB solution with β-Ga2O3 nanorods at different UV irradiation times are also shown in the inset of b


The GaOOH nanorods with a length of ~1 μm and a width of ~300–400 nm were successfully prepared by a simple hydrothermal synthesis at 95 °C of growth temperature. Then, the as-prepared GaOOH nanorods were calcined at different temperatures of 500–1000 °C for converting into single crystalline α-Ga2O3 and β-Ga2O3 nanorods, and their crystal structures were confirmed by the XRD analysis. Also, the dehydration processes were studied by thermal analysis with consideration of the phase changes of the as-prepared GaOOH precursors. At 1000 °C of calcination temperature, the β-Ga2O3 nanorods with good crystallinity and porous surface were formed by the removal of water molecules during the dehydration. Additionally, these β-Ga2O3 nanorods provided a relatively stable and high photocatalytic activity, compared with the α-Ga2O3 nanorods. Under UV irradiation for 180 min, the β-Ga2O3 nanorods exhibited a relatively high photodegradation efficiency of 79 % compared to the α-Ga2O3 nanorods (62 %). This fabrication process and analysis can be useful to produce a good inorganic semiconductor nanomaterial-based photocatalyst.



This work was supported by the National Research Foundation of Korea (NRF) grant funded by the Korea government (MSIP) (No. 2015-023255).

Open AccessThis article is distributed under the terms of the Creative Commons Attribution 4.0 International License (, which permits unrestricted use, distribution, and reproduction in any medium, provided you give appropriate credit to the original author(s) and the source, provide a link to the Creative Commons license, and indicate if changes were made.

Authors’ Affiliations

Department of Electronics and Radio Engineering, Institute for Wearable Convergence Electronics, Kyung Hee University


  1. Benjwal P, Kar KK. Simultaneous photocatalysis and adsorption based removal of inorganic and organic impurities from water by titania/activated carbon/carbonized epoxy nanocomposite. J Environ Chem Eng. 2015;3(3):2076–83.View ArticleGoogle Scholar
  2. Dong H, Zeng G, Tang L, Fan C, Zhang C, He X, et al. An overview on limitations of TiO2-based particles for photocatalytic degradation of organic pollutants and the corresponding countermeasures. Water Res. 2015;79:128–46.View ArticleGoogle Scholar
  3. Rajeshwar K, Thomas A, Janáky C. Photocatalytic activity of inorganic semiconductor surfaces: myths, hype, and reality. J Phys Chem Lett. 2015;6(1):139–47.View ArticleGoogle Scholar
  4. Ramanathan R, Bansal V. Ionic liquid mediated synthesis of nitrogen, carbon and fluorine-codoped rutile TiO2 nanorods for improved UV and visible light photocatalysis. RSC Adv. 2015;5(2):1424–9.View ArticleGoogle Scholar
  5. Yu H, Jin B, Feng C, Bi Y, Jiao Z, Lu G. Facile synthesis of Ag3PO4 nanospheres with enhanced photocatalytic properties for the degradation of methylene blue under visible light irradiation. Nanosci Nanotechnol Lett. 2015;7(7):565–70.View ArticleGoogle Scholar
  6. Cao Y, Xu Y, Hao H, Zhang G. Room temperature additive-free synthesis of uniform Cu2O nanocubes with tunable size from 20 nm to 500 nm and photocatalytic property. Mater Lett. 2014;114:88–91.View ArticleGoogle Scholar
  7. Cao F, Lv X, Ren J, Miao L, Wang J, Li S et al. Preparation of uniform BiOI nanoflowers with visible light-induced photocatalytic activity. Aust J Chem. 2015.
  8. Kang BK, Lim HD, Mang SR, Song KM, Jung MK, Kim S-W, et al. Synthesis and characterization of monodispersed β-Ga2O3 nanospheres via morphology controlled Ga4(OH)10SO4 precursors. Langmuir. 2015;31(2):833–8.View ArticleGoogle Scholar
  9. Tachikawa T, Majima T. Metal oxide mesocrystals with tailored structures and properties for energy conversion and storage applications. NPG Asia Mater. 2014;6:e100.View ArticleGoogle Scholar
  10. Veres A, Menesi J, Janaky C, Samu GF, Scheyer MK, Xu Q, et al. New insights into the relationship between structure and photocatalytic properties of TiO2 catalysts. RSC Adv. 2015;5(4):2421–8.View ArticleGoogle Scholar
  11. Liu T-J, Wang Q, Jiang P. Morphology-dependent photo-catalysis of bare zinc oxide nanocrystals. RSC Adv. 2013;3(31):12662–70.View ArticleGoogle Scholar
  12. Han X-G, He H-Z, Kuang Q, Zhou X, Zhang X-H, Xu T, et al. Controlling morphologies and tuning the related properties of nano/microstructured ZnO crystallites. J Phys Chem C. 2009;113(2):584–9.View ArticleGoogle Scholar
  13. Muruganandham M, Amutha R, Wahed MSMA, Ahmmad B, Kuroda Y, Suri RPS, et al. Controlled fabrication of α-GaOOH and α-Ga2O3 self-assembly and its superior photocatalytic activity. J Phys Chem C. 2012;116(1):44–53.View ArticleGoogle Scholar
  14. Jin C, Park S, Kim H, Lee C. Ultrasensitive multiple networked Ga2O3-core/ZnO-shell nanorod gas sensors. Sens Actuators, B. 2012;161(1):223–8.View ArticleGoogle Scholar
  15. Sheng T, Liu X-Z, Qian L-X, Xu B, Zhang Y-Y. Photoelectric properties of β-Ga2O3 thin films annealed at different conditions. Rare Met. 2015:1–5Google Scholar
  16. Zhao W, Xi H, Zhang M, Li Y, Chen J, Zhang J, et al. Enhanced quantum yield of nitrogen fixation for hydrogen storage with in situ-formed carbonaceous radicals. Chem Commun. 2015;51(23):4785–8.View ArticleGoogle Scholar
  17. Xu X, Bi K, Huang K, Liang C, Lin S, Wang WJ, et al. Controlled fabrication of α-GaOOH with a novel needle-like submicron tubular structure and its enhanced photocatalytic performance. J Alloys Compd. 2015;644:485–90.View ArticleGoogle Scholar
  18. Meng S, Danzhen L, Wenjuan Z, Xianzhi F, Yu S, Wenjuan L, et al. Rapid microwave hydrothermal synthesis of GaOOH nanorods with photocatalytic activity toward aromatic compounds. Nanotechnology. 2010;21(35):355601.View ArticleGoogle Scholar
  19. Li G, Peng C, Li C, Yang P, Hou Z, Fan Y, et al. Shape-controllable synthesis and morphology-dependent luminescence properties of GaOOH:Dy3+ and β-Ga2O3:Dy3+. Inorg Chem. 2010;49(4):1449–57.View ArticleGoogle Scholar
  20. Zhao Y, Frost RL, Yang J, Martens WN. Size and morphology control of gallium oxide hydroxide GaO(OH), nano- to micro-sized particles by soft-chemistry route without surfactant. J Phys Chem C. 2008;112(10):3568–79.View ArticleGoogle Scholar
  21. Qian H-S, Gunawan P, Zhang Y-X, Lin G-F, Zheng J-W, Xu R. Template-free synthesis of highly uniform α-GaOOH spindles and conversion to α-Ga2O3 and β-Ga2O3. Cryst Growth Des. 2008;8(4):1282–7.View ArticleGoogle Scholar
  22. Chai X, Liu Z, Huang Y. Influence of PEG 6000 on gallium oxide (Ga2O3) polymorphs and photocatalytic properties. Sci China Chem. 2015;58(3):532–8.View ArticleGoogle Scholar
  23. Pandey RM, Naidu BS, Sudarsan V, Pandey M, Kshirsagar RJ, Vatsa RK. Synthesis and characterization of Ga2O3:Eu nanorods. AIP Conference Proceedings. 2015;1665(1):140053.View ArticleGoogle Scholar
  24. Girija K, Thirumalairajan S, Mangalaraj D. Morphology controllable synthesis of parallely arranged single-crystalline β-Ga2O3 nanorods for photocatalytic and antimicrobial activities. Chem Eng J. 2014;236:181–90.View ArticleGoogle Scholar
  25. Li D, Duan X, Qin Q, Fan H, Zheng W. Ionic liquid-assisted synthesis of mesoporous α-Ga2O3 hierarchical structures with enhanced photocatalytic activity. Journal of Materials Chemistry A. 2013;1(40):12417–21.View ArticleGoogle Scholar
  26. Wang Y, Li N, Duan P, Sun X, Chu B, He Q. Properties and photocatalytic activity of β-Ga2O3 nanorods under simulated solar irradiation. J Nanomater. 2015;2015:5.Google Scholar
  27. Zhang W, Naidu BS, Ou JZ, O’Mullane AP, Chrimes AF, Carey BJ, et al. Liquid metal/metal oxide frameworks with incorporated Ga2O3 for photocatalysis. ACS Appl Mater Interfaces. 2015;7(3):1943–8.View ArticleGoogle Scholar
  28. Liu J, Zhang G. Mesoporous mixed-phase Ga2O3: green synthesis and enhanced photocatalytic activity. Mater Res Bull. 2015;68:254–9.View ArticleGoogle Scholar
  29. Arul Prakasam B, Lahtinen M, Muruganandham M, Sillanpää M. Synthesis of self-assembled α-GaOOH microrods and 3D hierarchical architectures with flower like morphology and their conversion to α-Ga2O3. Mater Lett. 2015;158:370–2.View ArticleGoogle Scholar
  30. Dong S, Zhang X, He F, Dong S, Zhou D, Wang B. Visible-light photocatalytic degradation of methyl orange over spherical activated carbon-supported and Er3+:YAlO3-doped TiO2 in a fluidized bed. J Chem Technol Biotechnol. 2015;90(5):880–7.View ArticleGoogle Scholar
  31. Cheng H, Wang J, Zhao Y, Han X. Effect of phase composition, morphology, and specific surface area on the photocatalytic activity of TiO2 nanomaterials. RSC Adv. 2014;4(87):47031–8.View ArticleGoogle Scholar
  32. Zhao Z, Wang Y, Xu J, Shang C, Wang Y. AgCl-loaded mesoporous anatase TiO2 with large specific surface area for enhancing photocatalysis. Appl Surf Sci. 2015;351:416–24.View ArticleGoogle Scholar
  33. Liu H, Joo JB, Dahl M, Fu L, Zeng Z, Yin Y. Crystallinity control of TiO2 hollow shells through resin-protected calcination for enhanced photocatalytic activity. Energy Environ Sci. 2015;8(1):286–96.View ArticleGoogle Scholar


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