Preparation of Highly Crystalline TiO2 Nanostructures by Acid-assisted Hydrothermal Treatment of Hexagonal-structured Nanocrystalline Titania/Cetyltrimethyammonium Bromide Nanoskeleton
© The Author(s) 2010
Received: 28 May 2010
Accepted: 26 July 2010
Published: 11 August 2010
Highly crystalline TiO2 nanostructures were prepared through a facile inorganic acid-assisted hydrothermal treatment of hexagonal-structured assemblies of nanocrystalline titiania templated by cetyltrimethylammonium bromide (Hex-ncTiO2/CTAB Nanoskeleton) as starting materials. All samples were characterized by X-ray diffraction (XRD) and transmission electron microscopy (TEM). The influence of hydrochloric acid concentration on the morphology, crystalline and the formation of the nanostructures were investigated. We found that the morphology and crystalline phase strongly depended on the hydrochloric acid concentrations. More importantly, crystalline phase was closely related to the morphology of TiO2 nanostructure. Nanoparticles were polycrystalline anatase phase, and aligned nanorods were single crystalline rutile phase. Possible formation mechanisms of TiO2 nanostructures with various crystalline phases and morphologies were proposed.
KeywordsHydrothermal treatment Nanocrystalline titania Nanoskeleton
Titanium oxide (TiO2) is an important semiconductor material for use in a wide range of applications, including photocatalysis, environmental pollution control and solar energy conversion [1–4]. It is well known that titanium dioxide exists in three crystalline polymorphs, namely rutile (tetragonal), anatase (tetragonal), and brookite (orthorhombic). Rutile is the most stable phase, whereas anatase and brookite are metastable phase and transform to rutile upon heating [5, 7]. The rutile phase has been widely used for pigment materials because of its chemical stability. However, the anatase phase has been widely used in photodegradation due to its high photoactivity [1, 4, 6–8]. The majority of the applications of TiO2 are strongly influenced by the crystalline phase . In order to obtain highly crystalline TiO2 at low temperature, a long time is necessary to get pure anatase or anatase–rutile phase mixture, and days or even longer time for the formation of rutile phase in traditional sol–gel process [10–12]. Anatase or the mixture of anatase and rutile can be produced by calcination within several hours with use of amorphous TiO2 as starting materials. However, obtaining pure anatase requires calcinations at 500°C, and pure rutile needs higher temperature , which often resulted in the collapse of the unique nanostructures, such as nanotube, nanorods, and formation of a conglomeration influencing the applications of TiO2. How to synthesize highly crystalline TiO2 at a relative lower temperature is still a difficult and hot topic in recent years [13, 14].
In comparison with sol–gel method [15, 16], hydrothermal synthesis is an easy route to prepare a well-crystalline oxide under the moderate reaction condition, i.e. low temperature and short reaction time . Hydrothermal media provides an effective reaction environment for the synthesis of nanocrystalline TiO2 with high purity, good dispersion and well-controlled crystalline. The reactivity of a precursor system can be judged only by optimizing the processing variables such as starting materials, pH, and temperature . To take advantage of the opportunities offered by hydrothermal synthesis, it is important to select a proper precursor system that is both reactive and cost effective. Recently, nanocrystalline TiO2 particles with different structures and morphologies have been synthesized in hydrothermal media using different starting materials such as TiCl4[13, 18], TiCl3[7, 19, 20], amorphous TiO2, P25 , and titanate hydrates . However, the preparation process of such starting materials is relatively complicated and the precursors are usually expensive and unstable.
In our previous work , we chose titanium oxysulfate sulfuric acid hydrate (TiOSO4 · x H2SO4 · x H2O) as a titania precursor and cetyltrimethylammonium bromide (CTAB) as a structure-directing agent for the preparation of titania. Both TiOSO4 and CTAB are cheap and common materials for industries. After simply mixed together at a lower range of temperatures (30–60°C), hexagonal-structured assemblies of nanocrystalline titania were formed through hydrolysis of TiOSO4 promoted by CTAB spherical micelles and condensation process (named as Hex-ncTiO2/CTAB nanoskeleton) [22, 23]. This system had some unique features and advantages, for example, a facile preparation, crystallization of titania in aqueous solution in mild conditions and formation of hexagonal-structured anatase titania framework. Then, we were successful to prepare mesoporous titania particles with honeycomb structure and anatase crystalline framework after the calcinations of the Hex-ncTiO2/CTAB nanoskeleton at 723 K for 2 h [16, 23].
In this paper, we examined the preparation of highly crystalline titanium dioxide nanostructures from the acid-assisted hydrothermal treatment of the Hex-ncTiO2/CTAB nanoskeleton as a starting material. Nanostructured TiO2 with different crystalline phases, crystallinity, and morphologies were obtained. In addition, the effect of hydrochloric acid concentration on the evolution of crystalline structure and morphologies of nanostructural TiO2 products were investigated.
Cetyltrimethylammonium bromide (CTAB) (Sigma, USA) was used as template material. Titanium oxysulfate sulfuric acid complex hydrate (TiOSO4 · x H2SO4 · x H2O) (Aldrich USA) was used as titania precursor. Hydrochloric acid (HCl) (Luoyang Chemical Reagents Factory, China) aqueous solutions were used as solvents in the hydrothermal procedure.
CTAB/TiO2 hexagonal structures were prepared in the following procedures [16, 22, 23].A concentration of 2.4 g TiOSO4 was mixed with 25 mL H2O under constant magnetic stirring until the mixed solution turned into colorless solution at 50°C, and then 25 mL CTAB (60 mM) was added into the colorless solution and hold statically for 12 h at 50°C. The product obtained was filtered, washed with distilled water for several times, and dried at 120°C overnight.
Hydrochloric acid aqueous solutions with different concentrations were initially prepared from concentrated HCl with distilled H2O, including 0.1–8 M. Subsequently, 0.5 g Hex-ncTiO2/CTAB nanoskeleton was dispersed in 30 mL of the HCl aqueous solutions with stirring for 0.5 h, and then transferred into 50-mL container of a Teflon-lined stainless steel autoclave. The autoclave was heated and maintained at 150°C for 24 h and then cooled to room temperature. The precipitate was collected, centrifuged, washed with distilled water for several times, and then dried in a vacuum oven overnight at 60°C.
XRD patterns of the samples were collected with a Philips X’ Pert Pro MPD X-ray diffraction system (XRD, Cu-Kα radiation, λ = 0.154056 nm). All the samples were measured in the continuous scan mode in the 2θ range of 10–90°, using a scan rate of 0.02 deg/s. The crystallite size was calculated using the Scherrer equation []. The morphology and structure of the products were observed with transmission electron microscopy (TEM) by JEM-2010 (JEOL Corporation, Japan), operating at 200 kV. The optical absorption spectra were obtained with Lambda 35 UV–vis spectrometer (Perkin-Elmer Inc., USA). BaSO4 was used as a reflectance standard in the UV–visible diffuse reflectance experiment.
Results and Discussion
Figure 6b–6e shows the TiO2 nanostructures composed of aligned nanorods and irregular nanoparticles obtained with further increase in the HCl concentration from 2 to 7 M. The TEM results show that the TiO2 nanoparticles are of irregular shape with an average size of 18 nm. The aligned nanorods maintained the analogous morphology with a width of around 50 nm and lengths of up to 300 nm in the concentration range from 2 to 7 M. Figure 6h presents the HRTEM investigations into the irregular nanoparticles and aligned nanorods. The lattice images of nanoparticles and nanorods were clearly observed, which indicated that these nanoparticles and nanorods had high degrees of crystallinity and phase purity. From the distance between the adjacent lattice fringes, we can assign the lattice plane on the nanoparticles and nanorods. The nanoparticles showed lattice spacing of d = 0.354 nm for the (101) plane of the anatase phase. The distance between the lattice fringes (d = 0.325 nm) in the aligned nanorods can be assigned to the interplanar distance of rutile phase (110) plane, which is well consistent with XRD results. Further observation by SAED (inset image in Fig. 6d) confirmed that the nanoparticles had a polycrystalline anatase structure, and the aligned nanorods were single crystalline TiO2 with rutile structure.
Figure 6f shows that nearly monodispersed diamond-shaped nanocrystals with an average size of about 14 nm are formed as increasing the HCl concentration to 8 M. Further HRTEM analysis in Fig. 6i shows that the lattice fringes with an in interlayer distance of 0.356 nm is close to the 0.352 nm lattice spacing of the (101) planes in anatase TiO2, which is in accordance with XRD results. From the TEM and SAED analysis, it can be concluded that different HCl concentrations affect not only the crystalline phase and crystallinity but also the morphologies of TiO2 nanostructures. In addition, it can be noticed that the ratio of the rutile to anatase in the products increases with increasing HCl concentration range from 1 M to 5 M, and reach a maximum at 5 M, and decreases to zero with further increasing HCl concentration from 6 to 8 M, which corresponds to the XRD results in Fig. 3 and Fig. 4.
From the above results, the formation of TiO2 nanostructures with various crystalline phases and morphology from the starting materials involved different nucleation and growth processes under the hydrothermal conditions. Two formation mechanisms have been proposed for the hydrothermal reaction [26–28]. One is the dissolution and recrystallization mechanism and the other is the in situ transformation mechanism. XRD analysis in Fig. 2 presented that the Hex-ncTiO2/CTAB nanoskeletons as starting materials were mixture of poorly crystallized anatase and amorphous titania. It is expected that the reaction progresses through in situ transformation mechanism for the TiO2 samples obtained in HCl solutions ranged from 0.1 to 7 M. The anatase nanocrystals in Hex-ncTiO2/CTAB nanoskeletons may act as “seeds” for the growth of larger anatase nanoparticles. The transformation of amorphous TiO2 in the Hex-ncTiO2/CTAB nanoskeleton exists a competition between the two growth units of rutile and anatase. Both anatase and rutile can grow from the [TiO6] octahedra, and the phase formation proceeds by the structural rearrangement of the octahedral [13, 26–28]. During the process of TiO2 crystal growth, HCl worked like a chemical catalyst to cause a change in the crystallization mechanism and decreased the activation energy for the rutile formation . The growth of existed anatase nanocrystals and transformation of amorphous titania to anatase at low HCl concentration results in the formation of irregular nanoparticles with anatase phase in the 0.1 to 1 M HCl solutions. The increased HCl concentration ranged from 2 to 7 M, Cl−1 can affect the O–Ti–O bonding structure and favor formation of the rutile nanorods structure from amorphous titania, which is consistent with some reports of rutile nanorods fabrications in acidic solution [24, 28]. Moreover, our hydrothermal experiments processed in higher concentration HCl solutions were gradually inclined to the dissolution and recrystallization mechanism. The rutile content decreased and the crystallite size of anatase decreased with the increasing HCl concentration ranging from 5 to 8 M as shown in Fig. 4 and Fig. 5. The solubility of titania oxides increased in the high acid solutions with the HCl concentration increasing steadily. The amorphous titania and anatase nanocrystals in the starting materials decomposed and recrystallized to form anatase nuclei according to the dissolution recrystallization mechanism. The observation of smaller uniform diamond-shaped nanoparticles with high quality single-crystal anatase structure in 8 M HCl solution clearly showed that dissolution–recrystallization process occurred with the high HCl concentration.
Anatase and rutile are two primary crystalline phases of TiO2. The absorption onsets of anatase and rutile are located at about 387 nm and 413 nm, corresponding to band energy of 3.2 and 3.0 eV, respectively . The valance band of anatase and rutile is mainly composed of O2p states, while the conduction band is mainly formed of Ti3d states. The band gap of TiO2 is determined by the positions of conduction band and valance band, which is strongly related with its crystal structure, phase composition, grain size, and morphology. Therefore, the band gap of the mixture of anatase and rutile is between the values of pure anatase and rutile.
Highly crystalline TiO2 nanostructures were prepared through an acid-assisted hydrothermal process of the Hex-ncTiO2/CTAB nanoskeleton. The HCl concentrations affected not only the crystalline phase but also the morphologies of TiO2 nanostructures. Pure anatase nanoparticles were obtained in the lower HCl concentration range (0.1–1 M) and 8 M HCl, while a mixture of rutile nanorods and anatase nanoparticles were obtained for a broader concentration range of 2 M to 7 M. Different mechanisms were proposed for the phase formation and morphology changes of TiO2 nanostructures with various HCl concentrations.
The authors Shuxi Dai and Yanqiang Wu contributed equally to this work.
This work was supported by the National Natural Science Foundation of China (Grant No. 20903034, 10874040) and the Cultivation Fund of the Key Scientific and Technical Innovation Project, Ministry of Education of China (Grant No. 708062).
This article is distributed under the terms of the Creative Commons Attribution Noncommercial License which permits any noncommercial use, distribution, and reproduction in any medium, provided the original author(s) and source are credited.
- Shen LM, Bao NZ, Zheng YN, Gupta A, An TC, Yanagisawa K: J. Phys. Chem. C.. 2008, 112: 8809. COI number [1:CAS:528:DC%2BD1cXmt1ynsLk%3D] 10.1021/jp711369eView ArticleGoogle Scholar
- Tsai CC, Teng HS: Chem. Mater.. 2006, 18: 367. COI number [1:CAS:528:DC%2BD2MXht12lsr7E] 10.1021/cm0518527View ArticleGoogle Scholar
- Huang JQ, Huang Z, Guo W, Cao YG, Hong MC: Cryst. Growth Des.. 2008, 8: 2444. COI number [1:CAS:528:DC%2BD1cXmvVGrtr8%3D] 10.1021/cg800030yView ArticleGoogle Scholar
- Kim H.W., Kim H.S., Na H.G., Yang J.C., Kim D.Y.: J. Alloys Compd. 10.1016/j.jallcom.2010.05.094
- Kolenko YV, Burukhin AA, Churagulov BR, Oleynikov NN: Mater. Lett.. 2003, 57: 1124. COI number [1:CAS:528:DC%2BD38Xpslagtr8%3D] 10.1016/S0167-577X(02)00943-6View ArticleGoogle Scholar
- Fahmi A, Minot C, Silvi B, Causa M: Phys. Rev. B.. 1993, 47: 11717. COI number [1:CAS:528:DyaK3sXks1Siurk%3D]; Bibcode number [1993PhRvB..4711717F] 10.1103/PhysRevB.47.11717View ArticleGoogle Scholar
- Hosono E, Fujihara S, Kakiuchi K, Imai H: J. Am. Chem. Soc.. 2004, 126: 7790. COI number [1:CAS:528:DC%2BD2cXks1arurc%3D] 10.1021/ja048820pView ArticleGoogle Scholar
- Fujishima A, Rao TN, Tryk DA: J. Photochem. Photobiol. C.. 2000, 1: 1. COI number [1:CAS:528:DC%2BD3cXkslOjtrc%3D] 10.1016/S1389-5567(00)00002-2View ArticleGoogle Scholar
- Chung CC, Chung TW, Yang TK: Ind. Eng. Chem. Res.. 2008, 47: 2301. COI number [1:CAS:528:DC%2BD1cXisFyjtLY%3D] 10.1021/ie0713644View ArticleGoogle Scholar
- Kanie K, Sugimoto T: Chem. Commun.. 2004, 14: 1584. 10.1039/b404220dView ArticleGoogle Scholar
- Xu N, Shi Z, Fan Y, Dong J, Shi J, Hu M: Ind. Eng. Chem. Res.. 1999, 38: 373. COI number [1:CAS:528:DyaK1MXjtFSnsQ%3D%3D] 10.1021/ie980378uView ArticleGoogle Scholar
- Wang C, Ying JY: Chem. Mater.. 1999, 11: 3113. COI number [1:CAS:528:DyaK1MXmvFWlu7k%3D] 10.1021/cm990180fView ArticleGoogle Scholar
- Li S, Ye G, Chen G: J. Phys. Chem. C.. 2009, 113: 4031. COI number [1:CAS:528:DC%2BD1MXitVOmtr0%3D] 10.1021/jp8076936View ArticleGoogle Scholar
- Wu W, Chang Y, Ting J: Cryst. Growth Des.. 2010, 10: 1646. COI number [1:CAS:528:DC%2BC3cXjtFCmtLY%3D] 10.1021/cg901210cView ArticleGoogle Scholar
- Joo J, Kwon SG, Yu TY, Cho M, Lee JW, Yoon JY, Hyeon TW: J. Phys. Chem. B.. 2005, 109: 15297. COI number [1:CAS:528:DC%2BD2MXmsFWntLc%3D] 10.1021/jp052458zView ArticleGoogle Scholar
- Shibata H, Ogura T, Mukai T, Ohkubo T, Sakai H, Abe M: J. Am. Chem. Soc.. 2005, 127: 16396. COI number [1:CAS:528:DC%2BD2MXhtFOisLzK] 10.1021/ja0552601View ArticleGoogle Scholar
- Lencka MM, Riman RE: Chem. Mater.. 1995, 7: 18. COI number [1:CAS:528:DyaK2MXjt1Clsrg%3D] 10.1021/cm00049a006View ArticleGoogle Scholar
- Wu D, Liu J, Zhao XN, Li AD, Chen YF, Ming NB: Chem. Mater.. 2006, 18: 547. COI number [1:CAS:528:DC%2BD2MXhtlagu73F] 10.1021/cm0519075View ArticleGoogle Scholar
- Liu SJ, Gong JY, Hu B, Yu SH: Cryst. Growth Des.. 2009, 9: 203. COI number [1:CAS:528:DC%2BD1cXhsVWrurzM] 10.1021/cg800227xView ArticleGoogle Scholar
- Hosono E, Fujihara S, Lmai H, Honma I, Masaki I, Zhou HS: ACS Nano.. 2007, 4: 273. 10.1021/nn700136nView ArticleGoogle Scholar
- Wang Q, Wen ZH, Li JH: Inorg. Chem.. 2006, 45: 6944. COI number [1:CAS:528:DC%2BD28XmvF2ntLs%3D] 10.1021/ic060477xView ArticleGoogle Scholar
- Sakai T, Yano H, Ohno M, Shibata H, Torigoe K, Utsumi S, Sakamoto K, Koshikawa N, Adachi S, Sakai H, Abe M: J. Oleo Sci.. 2008, 57: 629. COI number [1:CAS:528:DC%2BD1cXhtlWntbzO]View ArticleGoogle Scholar
- Shibata H, Mihara H, Mukai T, Ogura T, Kohno H, Ohkubo T, Sakai H, Abe M: Chem. Mater.. 2006, 18: 2256. COI number [1:CAS:528:DC%2BD28XivVynsb4%3D] 10.1021/cm0524042View ArticleGoogle Scholar
- Kim SJ, Park S: Jpn. J. Appl. Phys.. 2001, 40: 6797. COI number [1:CAS:528:DC%2BD38XlvVSn]; Bibcode number [2001JaJAP..40.6797K] 10.1143/JJAP.40.6797View ArticleGoogle Scholar
- Patterson A: Phys. Rev.. 1939, 56: 978. COI number [1:CAS:528:DyaH3cXlvV2n]; Bibcode number [1939PhRv...56..978P] 10.1103/PhysRev.56.978View ArticleGoogle Scholar
- Wang ZY, Xia DG, Chen G, Yang T, Chen Y: Mater. Chem. Phys.. 2008, 111: 313. COI number [1:CAS:528:DC%2BD1cXptVWrt7o%3D] 10.1016/j.matchemphys.2008.04.015View ArticleGoogle Scholar
- Yang K, Zhu JM, Zhu JJ, Huang SS, Zhu XH, Ma GB: Mater. Lett.. 2003, 57: 4639. COI number [1:CAS:528:DC%2BD3sXosVCrsLY%3D] 10.1016/S0167-577X(03)00376-8View ArticleGoogle Scholar
- Sugimoto T, Zhou X, Muramatsu A: J. Coll. Inter. Sci.. 2002, 252: 339. COI number [1:CAS:528:DC%2BD38XmtV2gsb0%3D] 10.1006/jcis.2002.8454View ArticleGoogle Scholar
- Yanagisawa K, Ovenstone J: J. Phys. Chem. B.. 1999, 103: 7781. COI number [1:CAS:528:DyaK1MXlsFSmtro%3D] 10.1021/jp990521cView ArticleGoogle Scholar