- Nano Express
- Open Access
Monodisperse α-Fe2O3 Mesoporous Microspheres: One-Step NaCl-Assisted Microwave-Solvothermal Preparation, Size Control and Photocatalytic Property
Nanoscale Res Lett volume 6, Article number: 1 (2010)
A simple one-step NaCl-assisted microwave-solvothermal method has been developed for the preparation of monodisperse α-Fe2O3 mesoporous microspheres. In this approach, Fe(NO3)3 · 9H2O is used as the iron source, and polyvinylpyrrolidone (PVP) acts as a surfactant in the presence of NaCl in mixed solvents of H2O and ethanol. Under the present experimental conditions, monodisperse α-Fe2O3 mesoporous microspheres can form via oriented attachment of α-Fe2O3 nanocrystals. One of the advantages of this method is that the size of α-Fe2O3 mesoporous microspheres can be adjusted in the range from ca. 170 to ca. 260 nm by changing the experimental parameters. High photocatalytic activities in the degradation of salicylic acid are observed for α-Fe2O3 mesoporous microspheres with different specific surface areas.
The fabrication of mesoporous materials of transition metal oxides has attracted more and more attention in recent years for their unique catalytic, electrochemical, magnetic and adsorptive properties [1–4]. Among them, α-Fe2O3 mesoporous materials are of particular interest, because α-Fe2O3 is widely used in catalysis , photoelectrodes , sensors , the anode material for Li-ion batteries  and so on. As an important n-type semiconductor, α-Fe2O3 is also used as a photocatalyst [9, 10], especially in the degradation of salicylic acid [11–13]. Salicylic acid is a complexing agent that forms stable complexes with iron ions, and it is one of pollutants in waste effluent . Mesoporous structures will benefit the photocatalytic activity of α-Fe2O3 due to the high specific surface area and the redox activity of the surfaces and nanopores.
Although the preparation of mesoporous silica, aluminosilicates, aluminophosphates and related materials is already well established [15–18], however, the synthesis of mesoporous materials of transition metal oxides is much more difficult and less reported [19, 20]. Several mesoporous materials of transition metal oxides such as TiO2, ZrO2, Nb2O5, WO3 and MnOx [21–27] have been prepared owing to researchers' unremitting effort. α-Fe2O3 mesoporous structures were prepared using soft templating methods [1, 28–31], as well as using mesoporous silica as hard template . However, such methods suffer from some disadvantages. Soft templating methods usually lead to the formation of mesoporous α-Fe2O3 with amorphous walls, while the hard templating methods usually involve multistep processes and sometimes lead to the damage of pore structures during the removal of hard templates.
Monodisperse nanocrystals display novel properties thus to stimulate intensive researches on the synthesis of monodisperse nanocrystals for their fundamental and technological importance . However, challenges still arise, how to combine the mesoporous structure with monodisperse microspheres, for the enhancement of the structural stability and photocatalytic property of α-Fe2O3. Herein, we report a simple one-step NaCl-assisted microwave-solvothermal method for the preparation of monodisperse α-Fe2O3 mesoporous microspheres. In the present approach, monodisperse α-Fe2O3 mesoporous microspheres can form via oriented attachment of α-Fe2O3 nanocrystals in the presence of NaCl. One of the advantages of this method is that the size of α-Fe2O3 mesoporous microspheres can be adjusted in the range from ca. 170 to ca. 260 nm by changing the experimental parameters. High photocatalytic activities in the degradation of salicylic acid are observed for typical samples of α-Fe2O3 mesoporous microspheres with different specific surface areas.
Materials and Methods
Preparation of Monodisperse α-Fe2O3 Mesoporous Microspheres
In a typical synthetic procedure, 0.404 g Fe(NO3)3 · 9H2O, 0.117 g NaCl and 0.111 g PVP (K-30) were dissolved in mixed solvents of 15 ml H2O and 15 ml ethanol under magnetic stirring. The resultant solution was loaded into a 60-ml Teflon autoclave, sealed, microwave-heated to 120°C and kept at this temperature for 30 min. The microwave oven used for sample preparation was microwave-solvothermal synthesis system (MDS-6, Sineo, Shanghai, China). After cooled to room temperature, the products were collected and washed by centrifugation–redispersion cycles with deionized water and alcohol three times, respectively. Please refer to Table 1 for the detailed preparation conditions for typical samples.
Photocatalytic Activity Measurements
The photocatalytic reactor consisted of two parts: a 70-ml quartz tube and a high-pressure Hg lamp. The Hg lamp was positioned parallel to the quartz tube. In all experiments, the photocatalytic reaction temperature was kept at about 35°C. The reaction suspension was prepared by adding the sample (20 mg) into 50 ml of salicylic acid solution with a concentration of 20 mg l-1. The suspension was sonicated for 15 min and then stirred in the dark for 30 min to ensure an adsorption/desorption equilibrium prior to UV irradiation. The suspension was then irradiated using UV light under continuous stirring. Analytical samples were withdrawn from the reaction suspension after various reaction times and centrifuged at 10,000 rpm for 5 min to remove the particles for analysis.
Characterization of Samples
The as-prepared samples were characterized using X-ray powder diffraction (XRD) (Rigaku D/max 2550V, Cu Kα radiation, λ = 1.54178 Å), scanning electron microscopy (SEM) (JEOL JSM-6700F) and transmission electron microscopy (TEM) (JEOL JEM-2100F). The Brunauer–Emmett–Teller (BET) surface area and pore size distribution were measured with an accelerated surface area and porosimetry system (ASAP 2010, USA). The photocatalytic reactions were carried out under irradiation of a 300-W high-pressure Hg lamp (GGZ300, Shanghai Yaming Lighting) with a maximum emission at about 365 nm. The salicylic acid concentrations were analyzed using a UV–vis spectrophotometer (UV-2300, Techcomp) at a wavelength of 297 nm.
Results and Discussion
The detailed preparation procedures for the samples are described in the experimental section, and the preparation conditions for typical samples are listed in Table 1.
Figure 1a shows the XRD pattern of sample 1 prepared using 0.404 g Fe(NO3)3 · 9H2O, 0.117 g NaCl and 0.111 g PVP in mixed solvents of 15 ml H2O and 15 ml ethanol by microwave-solvothermal method at 120°C for 30 min. Based on the analysis of the XRD pattern in Figure 1a, the product is α-Fe2O3 with a hexagonal structure (JCPDS No. 80-2377).
TEM micrographs were recorded to investigate the morphology and structure of sample 1, as shown in Figure 2a–c. One can see that sample 1 is composed of monodisperse microspheres with a diameter of ca. 170 nm. However, dispersed nanocrystals are also observed around the microspheres. Figure 2d is the selected area electron diffraction (SAED) pattern of a single microsphere, revealing the single-crystal-like feature of the microsphere, indicating the oriented assembly of nanocrystals in each single microsphere. The SAED patterns of the individual aggregate constructed by the oriented organization of nanocrystals exhibiting single-crystal-like diffraction dots have been reported in the literature [11, 33, 34]. The energy dispersive spectroscopies (EDS) of microspheres (Figure 2e) and dispersed nanocrystals (Figure 2f) confirm that they both consist of Fe and O elements. The Cu peak is originated from the copper sample holder. The above information indicates that α-Fe2O3 microspheres are formed by the self-assembly of nanocrystals with diameters of several nanometers via an oriented aggregation mechanism. Since the microsphere is formed by oriented assembly of very small nanocrystals, the microsphere is characterized with a mesoporous structure, which is confirmed by nitrogen adsorption–desorption isotherm and the pore size distribution measurements, and this will be discussed below.
We have found that sodium chloride (NaCl) plays an important role in the formation of monodisperse α-Fe2O3 mesoporous microspheres. Sample 2 was prepared in the absence of NaCl for comparison, and TEM micrographs of this sample are shown in Figure 3a, b. One can see that sample 2 prepared without NaCl consists mainly of very small dispersed nanocrystals with diameters of several nanometers and that particles formed by aggregation of nanocrystals are observed as a minor morphology, as shown in Figure 3a. The HRTEM image (Figure 3b) reveals that the average size of the nanocrystals is smaller than 5 nm. We propose that NaCl in the present synthesis acts as a promoter for the oriented assembly of α-Fe2O3 nanocrystals to form monodisperse mesoporous microspheres. It was reported that NaAc was used in the synthesis of Fe3O4 microspheres , and Ru, Pt and Rh particles [35–37]. In the present reaction system, NaCl may assist the complexation of PVP and iron ions, forming the monodisperse microspheres. We have also prepared sample 3 without using PVP, and the TEM micrograph is shown in Figure 3c. It can be seen that although α-Fe2O3 microspheres can be obtained without using PVP, the sizes of microspheres in sample 3 are not as uniform as those in sample 1 prepared in the presence of PVP. This result indicates that the addition of PVP is favorable for the formation of α-Fe2O3 monodisperse microspheres. Moreover, the concentration of PVP also influences the size of α-Fe2O3 monodispersed microspheres, which will be discussed below.
In order to control the size of mesoporous microspheres, comparative experiments were performed by changing the experimental parameters. Sample 4 was obtained with increased PVP concentration (0.222 g), while the other conditions were unchanged. One can see that sample 4 is also composed of α-Fe2O3 microspheres with an average diameter of ca. 205 nm, as shown in Figure 3d, e. Although sample 4 has a similar morphology to that of sample 1, the average diameter of microspheres in sample 4 is larger than that of sample 1, indicating that the concentration of PVP has an effect on the size of as-prepared α-Fe2O3 microspheres.
Figure 3f, g shows TEM micrographs of sample 5 prepared when the microwave-solvothermal time was increased from 30 to 60 min, and the average diameter of α-Fe2O3 mesoporous microspheres increases from ca. 170 to ca. 225 nm. This experimental result indicates that longer microwave-solvothermal time results in larger mesoporous microspheres. Thus, the size of α-Fe2O3 mesoporous microspheres can be controlled by adjusting microwave-solvothermal time.
Sample 6 was prepared at a higher microwave-solvothermal temperature of 140°C instead of 120°C, while the other conditions were kept unchanged. Figure 1b shows the XRD pattern of sample 6, from which one can see that the product is a single phase of α-Fe2O3 with a hexagonal structure (JCPDS No. 80–2377). The higher intensities of the XRD peaks of sample 6 compared with those of sample 1 (Figure 1a) indicate that the crystallinity of sample 6 is improved. Figure 4a–e shows the SEM and TEM micrographs of sample 6. One can see that almost exclusive α-Fe2O3 mesoporous microspheres assembled with nanocrystals are obtained and that dispersed nanocrystals are hardly observed compared with sample 1. However, the average diameter of α-Fe2O3 microspheres in sample 6 increases to ca. 260 nm, higher than that of sample 1 (170 nm), implying that higher microwave-hydrothermal temperature will produce α-Fe2O3 microspheres with larger size. Figure 4f shows the SAED pattern of a single microsphere, revealing the single-crystal-like feature of the mesoporous microsphere formed via an oriented aggregation of α-Fe2O3 nanocrystals. The above experimental results indicate that the size of α-Fe2O3 mesoporous microspheres can be controlled (in the range from ca. 170 to ca. 260 nm under the present experimental conditions used) by changing the experimental parameters such as the microwave-solvothermal time and concentration of PVP.
We have measured the BET-specific surface areas and the pore size distributions of samples 1 and 6. Figure 5a, b shows the nitrogen adsorption–desorption isotherms and the pore size distributions of samples 1 and 6, which indicate that the BJH (Barrett–Joyner–Halenda) desorption average pore size and the BET-specific surface area are 4.3 nm and 114 m2/g for sample 1, and 7.9 nm and 37 m2/g for sample 6, respectively. Figure 5 indicates that there exist mesoporous structures in the α-Fe2O3 mesoporous microspheres. Sample 1 prepared at a lower temperature (120°C) has a much higher specific surface area and narrower pore size distribution than those of sample 6 prepared at a higher temperature (140°C). From the comparison of TEM micrographs of samples 1 and 6 (Figures 2, 4), one can see that the nanocrystals self-assembled in α-Fe2O3 mesoporous microspheres of sample 1 are smaller than those of sample 6. The oriented organization of smaller nanocrystals in α-Fe2O3 microspheres of sample 1 leads to smaller average pore size (4.3 nm); in contrast, the bigger nanocrystals in α-Fe2O3 microspheres of sample 6 result in larger average pore size (7.9 nm). On the other hand, the mesoporous microspheres constructed by the oriented organization of nanocrystals in sample 1 are much smaller (170 nm) than those of sample 6 (260 nm). These factors have effects on the BET-specific surface area, leading to the significant difference in BET-specific surface area between samples 1 and 6. These properties of α-Fe2O3 mesoporous microspheres will directly affect their photocatalytic activity, which will be discussed below.
To evaluate the photocatalytic activity of α-Fe2O3 monodisperse mesoporous microspheres, the comparison experiments were performed. Figure 6a shows the UV–vis absorption spectra of salicylic acid solution in the presence of sample 1 at different UV-irradiation times, from which one can see that the concentration of salicylic acid decreases rapidly after UV irradiation. Figure 6b shows the degradation percentage of salicylic acid in the presence of sample 1, from which one can see that the degradation percentage of salicylic acid increases rapidly with increasing time and nearly complete in a time period of 120 min. The photocatalytic activity of sample 1 is much higher than that obtained in our previous work [11, 12]. It can be found that the combination of the mesoporous structure with monodisperse microspheres is beneficial for the enhancement of the photocatalytic property of α-Fe2O3. We also investigated the photocatalytic activity of sample 6 as a reference. Sample 6 shows much weaker photocatalytic activity than sample 1, as illustrated in Figure 6c. It is obvious that α-Fe2O3 monodisperse mesoporous microspheres with higher specific surface area and narrower pore size distribution exhibit superior photocatalytic activity.
We have developed a simple one-step NaCl-assisted microwave-solvothermal method for the preparation of α-Fe2O3 monodisperse mesoporous microspheres formed by oriented assembly of nanocrystals. In this approach, Fe(NO3)3 · 9H2O is used as the iron source, and PVP acts as a surfactant in the presence of NaCl in mixed solvents of H2O and ethanol. NaCl is found to play an important role in the formation of α-Fe2O3 monodisperse mesoporous microspheres. One of the advantages of this method is that the size of α-Fe2O3 mesoporous microspheres can be adjusted in the range from ca. 170 to ca. 260 nm by changing the experimental parameters. High photocatalytic activities in the degradation of salicylic acid are observed for α-Fe2O3 mesoporous microspheres. The combination of the mesoporous structure with monodisperse microspheres is beneficial for the enhancement of the photocatalytic property of α-Fe2O3 in the degradation of salicylic acid by giving α-Fe2O3 mesoporous microspheres higher specific surface area and narrower pore size distribution.
Srivastava DN, Perkas N, Gedanken A, Felner I: J Phys Chem B. 2002, 106: 1878. 10.1021/jp015532w
Chen HR, Dong XP, Shi JL, Zhao JJ, Hua ZL, Gao JH, Ruan ML, Yan DS: J Mater Chem. 2007, 17: 855. 10.1039/b615972a
He X, Trudeau M, Antonelli D: J Mater Chem. 2003, 13: 75. 10.1039/b206951m
Izumi Y, Masih D, Aika K, Seida Y: Microporous Mesoporous Mater. 2006, 94: 243. 10.1016/j.micromeso.2006.04.002
Brown ASC, Hargreaves JSJ, Rijniersce B: Catal Lett. 1998, 53: 7. 10.1023/A:1019016830208
Ohmori T, Takahashi H, Mametsuka H, Suzuki E: Phys Chem Chem Phys. 2000, 2: 3519. 10.1039/b003977m
Sun HT, Cantalini C, Faccio M, Pelino M, Catalano M, Tapfer L: J Am Ceram Soc. 1996, 79: 927. 10.1111/j.1151-2916.1996.tb08527.x
Reddy MV, Yu T, Sow CH, Shen ZX, Lim CT, Rao GVS, Chowdari BVR: Adv Funct Mater. 2007, 17: 2792. 10.1002/adfm.200601186
Li X, Yu X, He JH, Xu Z: J Phys Chem C. 2009, 113: 2837. 10.1021/jp8079217
Miyauchi M, Nakajima A, Watanabe T, Hashimoto K: Chem Mater. 2002, 14: 2812. 10.1021/cm020076p
Cao SW, Zhu YJ: Acta Mater. 2009, 57: 2154. 10.1016/j.actamat.2009.01.009
Cao SW, Zhu YJ: J Phys Chem C. 2008, 112: 6253. 10.1021/jp8000465
Li LL, Chu Y, Liu Y, Dong LH: J Phys Chem C. 2007, 111: 2123. 10.1021/jp066664y
Pal B, Sharon M: J Chem Technol Biotechnol. 1998, 73: 269. 10.1002/(SICI)1097-4660(1998110)73:3<269::AID-JCTB944>3.0.CO;2-3
Corma A: Chem Rev. 1997, 97: 2373. 10.1021/cr960406n
Stein A, Melde BJ, Schroden RC: Adv Mater. 2000, 12: 1403. 10.1002/1521-4095(200010)12:19<1403::AID-ADMA1403>3.0.CO;2-X
Soler-illia GJD, Sanchez C, Lebeau B, Patarin J: Chem Rev. 2002, 102: 4093. 10.1021/cr0200062
Cundy CS, Cox PA: Chem Rev. 2003, 103: 663. 10.1021/cr020060i
Jiao F, Harrison A, Jumas J-C, Chadwick AV, Kockelmann W, Bruce PG: J Am Chem Soc. 2006, 128: 5468. 10.1021/ja0584774
Yu CC, Dong XP, Guo LM, Li JY, Qin F, Zhang LX, Shi JL, Yan DS: J Phys Chem C. 2008, 112: 13378. 10.1021/jp8044466
Yang PD, Zhao DY, Margolese DI, Chmelka BF, Stucky GD: Nature. 1998, 396: 152. 10.1038/24132
Tian ZR, Tong W, Wang JY, Duan NG, Krishnan VV, Suib SL: Science. 1997, 276: 926. 10.1126/science.276.5314.926
Tian BZ, Yang HF, Liu XY, Xie SH, Yu CZ, Fan J, Tu B, Zhao DY: Chem Commun. 2002, 1824.
Crepaldi EL, de GJ, Soler-Illia AA, Grosso D, Cagnol F, Ribot F, Sanchez C: J Am Chem Soc. 2003, 125: 9770.
Ulagappan N, Rao CNR: Chem Commun. 1996, 1685.
Xu X, Tian BZ, Kong JL, Zhang S, Liu BH, Zhao DY: Adv Mater. 2003, 15: 1932. 10.1002/adma.200305424
Antonelli DM, Nakahira A, Ying JY: Inorg Chem. 1996, 35: 3126. 10.1021/ic951533p
Malik AS, Duncan MJ, Bruce PG: J Mater Chem. 2003, 13: 2123. 10.1039/b303551d
Long JW, Logan MS, Rhodes CP, Carpenter EE, Stroud RM, Rolison DR: J Am Chem Soc. 2004, 126: 16879. 10.1021/ja046044f
Jiao F, Bruce PG: Angew Chem Int Ed. 2004, 43: 5958. 10.1002/anie.200460826
Lezau A, Trudeau M, Tsoi GM, Wenger LE, Antonelli D: J Phys Chem B. 2004, 108: 5211. 10.1021/jp031259h
Deng H, Li XL, Peng Q, Wang X, Chen JP, Li YD: Angew Chem Int Ed. 2005, 44: 2782. 10.1002/anie.200462551
Yang LX, Zhu YJ, Tong H, Wang WW: Ultrason Sonochem. 2007, 14: 259. 10.1016/j.ultsonch.2006.05.006
Ma MG, Zhu YJ, Cheng GF, Huang YH: Mater Lett. 2008, 62: 507. 10.1016/j.matlet.2007.05.072
Viau G, Toneguzzo P, Pierrard A, Acher O, Fiévet-Vincent F, Fiévet F: Scripta Mater. 2001, 44: 2263. 10.1016/S1359-6462(01)00752-7
Viau G, Brayner R, Poul L, Chakroune N, Lacaze E, Fiévet-Vincent F, Fiévet F: Chem Mater. 2003, 15: 486. 10.1021/cm0212109
Brown KR, Walter DG, Natan MJ: Chem Mater. 2000, 12: 306. 10.1021/cm980065p
Financial support from Science and Technology Commission of Shanghai (0852nm05800, 1052nm06200) and National Natural Science Foundation of China (50772124, 50821004) is gratefully acknowledged.