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www.elsevier.com/locate/apsusc
Available online at www.sciencedirect.com
Applied Surface Science 254 (2008) 3033–3038
Low-temperature preparation of F-doped TiO2 film and its
photocatalytic activity under solar light
Jingjing Xu a,b, Yanhui Ao a,b, Degang Fu a,b,*, Chunwei Yuan a
a State Key Laboratory of Bioelectronics, Southeast University, Nanjing 210096, Chinab School of Chemistry and Chemical Engineering, Southeast University, Nanjing 210096, China
Received 20 September 2007; received in revised form 21 October 2007; accepted 21 October 2007
Available online 4 November 2007
Abstract
A novel and simple method for preparing F-doped anatase TiO2 (defined as FTO) film with high photocatalytic activity was developed using
titanium-n-butoxide and NH4F as TiO2 and fluorine precursors under mild condition, i.e. low temperature (lower than 373 K) and ambient pressure.
The prepared samples were characterized by XRD, SEM, X-ray photoelectron spectroscopy (XPS), diffuse reflectance spectrum (DRS),
photoluminescence spectrum (PL) and TG–DSC analysis. The photocatalytic activity was evaluated by decomposing X-3B under artificial
solar light. The results showed that the crystallinity of TiO2 was improved by F-doping. F� ions can prevent the grain growth, and the
transformation of anatase to rutile phase was also inhibited. The doped fluorine atoms existed in two chemical forms, and the ones incorporated into
TiO2 lattice might take a positive role in photocatalysis. Compared with surface fluorination samples, FTO film exhibited better photocatalytic
activity. The high photocatalytic activity of FTO may due to extrinsic absorption through the creation of oxygen vacancies rather than the excitation
of the intrinsic absorption band of bulk TiO2. Furthermore, the FTO can be recycled with little photocatalytic activity depression. Without any
further treatment besides rinsing, after 6 recycle utilization, the photocatalytic activity of FTO film was still higher than 79%.
# 2007 Elsevier B.V. All rights reserved.
PACS : 81.07.�b
Keywords: Fluorine-doped; Photocatalysis; Low-temperature; Recycle
1. Introduction
Recently, many efforts have been devoted to developing
TiO2 heterogeneous photocatalyst since it was approved to be a
high efficient catalyst for environmental remediation and
energy conversion purpose [1]. However, its technological
application seems limited by several factors, among which the
most restrictive one is the need of using an ultraviolet (UV),
wavelength (l) <387 nm, as excitation source due to its wide
band gap (3.2 eV for anatase) [2], and can only capture less than
5% of the solar irradiance at the Earth’s surface. For the sake of
efficient use of sunlight, or use of the visible region of the
spectrum, the technology of enlarging the absorption scope of
* Corresponding author at: School of Chemistry and Chemical Engineering,
Southeast University, Nanjing 210096, China. Tel.: +86 25 83794310;
fax: +86 25 83793091.
E-mail address: [email protected] (D. Fu).
0169-4332/$ – see front matter # 2007 Elsevier B.V. All rights reserved.
doi:10.1016/j.apsusc.2007.10.065
TiO2 may then appear as an appealing challenge for developing
the future generation of photocatalysts.
Several works reported that doping TiO2 with nonmetallic
elements, such as nitrogen, sulphur, carbon, shift the optical
absorption edge of TiO2 toward lower energy, thereby increasing
the photocatalytic activity in visible region [3–5]. It was also
demonstrated that F-doped TiO2 is effective for enhancing
photocatalytic activity. [6–8] Yu et al. [6] proposed that F-doping
converts Ti4+ to Ti3+ by charge compensation, and the existence
of Ti3+ can reduce the electron–hole recombination rate, and
subsequently enhances the photocatalytic activity. Li et al. [7]
confirmed that F-doping in TiO2 can induce visible-light-driven
photocatalysis by the creation of oxygenvacancies. However, the
methods of preparing F-doped samples usually need special
equipments or high temperature treatment. A few researchers
have revealed that fluorination of TiO2 powders in room
temperature can improve photocatalytic activity [9–13]. Minero
et al. claimed that surface fluorination of TiO2 improves the
photocatalytic oxidation rate of phenol and tetramethylammo-
Fig. 1. XRD patterns of FTO and TIO nanoparticles, (a) FTO and (b) TIO.
J. Xu et al. / Applied Surface Science 254 (2008) 3033–30383034
nium [10–12]. And they ascribed the phenomena to the enhanced
generation of mobile free OH radicals. However, this surface
fluorination calls for special pH range of the contaminated
solution, and that F� ions are easy to run off in recycle reactions.
In this article, a simple method is carried out for producing F-
doped TiO2 under low temperature (about 348 K) and ambient
pressure. The photocatalytic activity and the recycle ability of F-
doped TiO2 (defined as FTO) film are compared with pure TiO2
(defined as TIO) film, P25 film and surface fluorination sample
(defined as Surf-FTO) film under artificial solar light.
2. Experimental
2.1. Photocatalysts preparation
Ti(OBu)4 was chosen as a Ti precursor, and NH4F was
employed as F source for FTO samples. Firstly, NH4F was added
in the distilled water under vigorous stirring, the mixture of
Ti(OBu)4 and i-PrOH was then dropwise gradually into above
water whose pH value was adjusted by nitric acid at 2.0, until
Ti(OBu)4 was hydrolyzed completely. The molar ratio of F and Ti
were 1:100. Secondly, the solution was keep refluxing at 348 K
for 24 h to obtain the FTO sol. The sol was further dried in the
oven at 333 K, and finally, the uniform FTO powders were
available for analysis. TIO sample was prepared by the same
method mentioned above without adding NH4F. The surface
fluorination sample, Surf-FTO, was prepared following literature
[12] by adding NaF into the mixture of P25 and water, with the pH
value of 3.0. Glass plates, 70 mm � 20 mm, used as substrates
were dipped in the obtained FTO sol, Surf-FTO solution, TIO sol
and P25 solution for 30 min, respectively, and then dried in the
vacuum oven at 333 K for 2 h, then cooled in the atmosphere.
2.2. Characterization
The crystalline structure of TiO2 samples was measured by
X-ray diffractometer (XRD, XD-3A, Shimadazu Corporation,
Japan) using graphite monochromatic copper radiation (Cu Ka)
at 40 kV, 30 mA over the 2u range of 20–808. The morphology
and size of FTO and Surf-FTO films and particles were
observed by scanning electron microscope (SEM, Sirion, FEI),
and TEM (JEOL-2000EX), respectively. The binding energy
was identified by X-ray photoelectron spectroscopy (XPS) with
Mg Ka radiation (ESCALB MK-II). To investigate the
recombination and lifespan of photogenerated electrons/holes
in the photocatalysts, the photoluminescence (PL) emission
spectra of the samples were measured at room temperature by
LS-55 (Perkin-Elmer) illuminated with a 325-nm He–Cd laser.
A UV–vis spectrophotometer (Shimadzu UV-2100) was used to
record the diffuse reflectance spectra of samples. The crystal-
lization behavior of FTO was also monitored using a TG–DSC
instrument (TG 2000/2960, TA Instruments).
2.3. Photocatalysts characterization
The photocatalytic activity of FTO film was studied in the
photocatalytic degradation of Reactive Brilliant Red, X-3B in
aqueous solution, while Surf-FTO, TIO and P25 films were
used for comparison. A batch photoreactor system was used in
experiments. It consists of a cylindrical silica reactor with glass
plate at the bottom, and an external light source with vertical
irradiation. A 250 W halogen lamp of artificial solar light was
used as light source with average radiation intensity of
11.3 mW cm�2. A set of photocatalytic degradation experi-
ments were performed with the following procedure: a piece of
glass plate with sample film was dipped into 10 ml of X-3B
solution with an initial concentration of 50 mg l�1. Prior to
photoreaction, air was pumped into reactor in the dark for
30 min to reach adsorption–desorption equilibrium. Then, with
continuous pump, the reaction was irradiated by artificial solar
light from the top vertically. During the photoreaction, samples
were collected at a time interval of every 20 min for analysis.
As for many TiO2 samples, the active sites may occupied by
absorbed contaminated molecules or their by-product after
some time usage, moreover, the modified element may run off
from sample film. Accordingly, the recycle experiments were
designed to examine photoactivity on both FTO and Surf-FTO
films. After finishing a cycle, the film was rinsed and dried in
the atmosphere, without any other treatments. The recycle
experiment was carried on for 6 cycles.
3. Results and discussion
3.1. Characterization of F-TiO2 particles
The XRD behaviors of FTO and TIO are shown in Fig. 1. It
can be noted that both FTO and TIO have significant diffraction
peaks (25.528, 37.98, 48.28, 54.48, 62.48) representing the
characteristic of anatase phase [14], and a small amount of
brookite is existing. Moreover, the doping F atoms do not cause
any shift in peak position of that of TiO2 phase. This could be
understood that the ion radius of fluorine atom (0.133 nm) is
virtually the same as the replaced oxygen atom (0.132 nm) [15].
The average crystallite sizes of FTO and TIO, calculated from
the (1 0 1) peak of the XRD patterns are 3.78 and 5.54 nm,
Fig. 2. SEM images of FTO and Surf-FTO films, (a) FTO and (b) Surf-FTO. Fig. 3. TEM images of FTO and Surf-FTO particles, (a) FTO and (b) Surf-FTO.
Fig. 4. XPS spectra of F 1s region in both FTO and Surf-FTO samples (a) Surf-
FTO, (b) FTO, and the inset is the survey XPS spectrum of FTO.
J. Xu et al. / Applied Surface Science 254 (2008) 3033–3038 3035
respectively. It can be concluded that F-doping inhibits the
grain growth. And the increasing intensity of FTO sample
indicates that the crystallinity is improved upon F-doping.
The SEM and TEM images of FTO and Surf-FTO films and
nanoparticles are shown in Figs. 2 and 3, respectively. In SEM
images of FTO film, the surface is smoother than that of Surf-
FTO film, a probable explanation is that the morphologies of
the particles depended on the TiO2 precursors as well as
fluorine incorporation in TiO2 matrix. As for FTO, the existing
F-ions are not the same as that of Surf-TIO. As shown in the
TEM images, FTO possesses spherical particles with an
average particle diameter of about 5 nm, which is in good
agreement with XRD analysis. There exists some agglomera-
tion in Surf-FTO particles, while such phenomenon cannot be
detected in FTO image. This is probably due to the fact that F-
ions suppress the agglomeration by electrostatic repulsion.
The XPS survey spectrum of FTO indicates that the peak
related to Ti, O, F, and C elements. The C element can be
ascribed to the residual carbon from precursor solution, as our
samples are all prepared at low temperature. Fig. 4 gives the
high-resolution XPS spectra of the F 1s region of FTO and Surf-
FTO. An unsymmetrical F 1s peak was observed, especially for
FTO sample, which means that there exist two chemical forms
of F-atoms in FTO. Using Gaussian distributions, the F 1s peak
of FTO was divided into two separated peaks as shown in Fig. 4.
The peak 1 located at 684.3 eV corresponding to that of F atoms
adsorbed on TiO2 [16]. While the peak 2 located at 688.4 eV is
the F atoms in solid solution TiO2�xFx, which is probably
formed by nucleophilic substitution reaction of F� ions and
titanium alkoxide during the hydrolysis process [6,11]. As for
Surf-FTO, the F 1s peak is originated from the surface fluoride
formed by ligand exchange between F� and surface hydroxyl
group on TiO2. The F 1s peak only located at 684.3 eV, and no
Fig. 5. PL spectra of P25, Surf-F, and FTO samples.Fig. 6. The diffuse reflectance UV–vis spectra of P25, TIO, Surf-FTO, and FTO
samples.
Fig. 7. TG–DSC curve of FTO particles.
J. Xu et al. / Applied Surface Science 254 (2008) 3033–30383036
sign of F� ions in the lattice was detected, which is in
agreement with that of literature [16]. This means, in our
preparation, the fluorine atoms can incorporate in the TiO2
lattice, even at very low synthesized temperature, which takes a
positive role in photocatalysis [6].
PL emission spectra have been widely used to investigate the
efficiency of charge carrier trapping, immigration, transfer, and
to understand the fate of electron–hole pairs in semiconductor
particles [17]. Fig. 5 shows the PL spectra of FTO, Surf-FTO,
and P25. The excitonic PL intensity of these samples decreases
obeyed the following order: FTO < Surf-FTO < P25. This
indicates that an appropriate amount of F� doping may slow the
radiative recombination process of photogenerated electrons
and hole in TiO2, which may confirm that the lower the
intensity of PL spectra, the higher the photocatalytic activity.
Diffuse reflectance spectroscopy gives information about the
electronic absorption of the photocatalysts. In Fig. 6, the UV–
vis reflectance of P25, TIO and Surf-FTO are compared with
FTO. It is indicates that F-doping dose not cause any significant
red-shift in the fundamental absorption edge of TiO2. This
conclusion is consistent with Asahi, Yamaki, Ho and Li et al.
[3,15,18,19]. When doping with fluorine atoms in TiO2,
localized levels with high density appear below the VB of TiO2.
These levels consist of the F 2p state without any mixing with
VB or CB of TiO2. Accordingly, it is not expected to show high
photocatalytic activity under visible-light-region.
The thermal behavior of FTO was investigated with a TG/
DSC technique at temperature rang from room temperature to
1200 8C, and the TG–DSC patterns of the typical FTO is shown
in Fig. 7. It is well known that the thermal behavior of TiO2
usually depends on the chemical composition, preparation
condition and existing phases [20–22]. The endothermic peak at
about 100 8C is due to the desorption of the physically adsorbed
water and alcohol [21]. A small exothermal peak appeared at
about 180 8C is assigned to the decomposition of organic
substances in the powder. The relative broad exothermal peak at
790 8C observed is owning to the phase transformation from
anatase to rutile, while the usually transformation temperature is
around 600 8C. The TG curve can be divided into three stages.
The first stage is range from room temperature to 200 8C with a
moss loss of 14%, which represents the dehydration and loss of
residual solvent. In the temperature range of 200–400 8C, the
weight loss is about 5%, which is attributed to the loss of organic
substances, corresponding to a sharp exothermal process from
DSC curve. The third mass loss of 1.0% in the range of 400–
1200 8C is owning to the gradual removal of the organic residues.
It can be concluded from TG–DSC results that the phase of
sample FTO is mainly anatase, and the doping of fluorine atoms
can inhibit the transformation from anatase to rutile.
3.2. Photocatalytic activity
In order to investigate the photocatalytic activity of FTO,
degradation experiments of X-3B dye were studied under
artificial solar light and results are shown in Fig. 8. The blank
experiment without catalysts indicated that the merely photolysis
can be ignored as it is about 0.9% after illuminated for 80 min.
Concerning the catalysts, the degradation percent of X-3B
obeyed the following order: P25 < TIO < Surf-FTO < FTO.
Fig. 8. Kinetic of X-3B degradation for different samples.
Fig. 9. Variations in ln(C0/C) as a function of irradiation time and linear fits of
different samples.
Table 1
kapp and R data for each sample
kappa (min�1) Rb
P25 9.63 � 10�4 0.993
TIO 0.0060 0.997
Surf-FTO 0.011 0.997
FTO 0.022 0.999
a kapp is the apparent rate constant.b R is regression relative coefficient.
Fig. 10. Recycle photocatalytic experiments on FTO film for 6 cycles.
J. Xu et al. / Applied Surface Science 254 (2008) 3033–3038 3037
Both Surf-FTO and FTO showed better photodegradation effects
than pure TiO2. The apparent rate constant (kapp) has been chosen
as the basic kinetic parameter for the different photocatalysts,
since it enables one to determine photocatalytic activity
independent of the previous adsorption period in the dark and
the concentration of X-3B remaining in the solution. The
apparent first order kinetic equation:
ln
�C0
C
�¼ kapp � t (1)
was used to fit experimental data in Fig. 8. Where C is the
concentration of X-3B remaining in the solution at t, and C0 is
the initial concentration at t = 0 [23]. The variations in ln(C0/C)
as a function of irradiation time are given in Fig. 9. And kapp
data for FTO, Surf-FTO, TIO and P25 are exhibited in Table 1.
It shows that the kapp of FTO is obviously increases, about 2
times higher than that of Surf-FTO. It has been discussed above
that the FTO does not absorb in the visible spectrum by DRS
analysis. But according to recent study, it can also induce
visible-light-driven photocatalysis by extrinsic absorption
through the creation of oxygen vacancies [7]. Thus, the high
photocatalytic activity of FTO may due to that reason rather
than the excitation of the intrinsic absorption band of bulk TiO2.
The result is also in agreement with that of PL spectra analysis.
The regeneration of TiO2 photocatalyst was one of key steps
to making heterogeneous photocatalysis technology for
practical applications. The results of recycling of FTO and
Surf-FTO films are shown in Fig. 10 and Table 2. Fig. 10
exhibits the variation of X-3B concentration on FTO film of
every cycle. The photocatalytic activity of FTO almost kept the
same after three times reusing, and a little decline after six
cycles, and the decomposing rate was still above 79% after
recycle for 6 times. While for surf-FTO, after 6 cycles, the
photocatalytic activity decreased by 34%, as most F� ions were
absorbed on the surface of TiO2 physically [6], they were easy
to run off with the solution in repeated using. These results
mean that FTO can act as a useful photocatalyst to drive
photodegradation reaction. More importantly, FTO, as a novel
Table 2
Data for recycle photocatalytic experiments
Sample Decomposed rate (%)
Cycle 1 Cycle 2 Cycle 3 Cycle 4 Cycle 5 Cycle 6
FTO 82.7 81.7 82.0 80.6 79.2 80.8
Surf-FTO 56.6 38.4 31.5 26.8 22.6 22.4
J. Xu et al. / Applied Surface Science 254 (2008) 3033–30383038
photocatalyst, can be reused for several times without great
decrease in photocatalytic activity during the reactions, exhibits
potential application in continual and long-time reactions.
4. Conclusion
F-doped TiO2 was prepared under mild condition by
hydrolysis of titanium-n-butoxide in abundant NH4F-H2O
acidic solution. The doped fluorine atoms existed in two
chemical forms, and the ones incorporated into TiO2 lattice
might take a positive role in photocatalysis. The FTO film
exhibited the highest photocatalytic activity for degradation of
X-3B in aqueous solution under artificial solar light, and it was
higher than that of P25. The high photocatalytic activity of FTO
may due to extrinsic absorption through the creation of oxygen
vacancies rather than the excitation of the intrinsic absorption
band of bulk TiO2. Without any special treatments, FTO film
can be applied to recycle use in photocatalytic reactions while
keeping high activity. Thus, the as-prepared FTO exhibits
potential application on industrial area.
Acknowledgment
This work is financially supported by the National Natural
Science Foundation of China (No. 60121101).
References
[1] J.T. Chang, Y.F. Lai, J.L. He, Surf. Coat. Technol. 200 (2005) 1640.
[2] T. Yang, M. Yang, C. Shiu, W. Chang, M. Wong, Appl. Surf. Sci. 252
(2006) 3729.
[3] R. Asahi, T. Morikawa, T. Ohwaki, Science 293 (2001) 269.
[4] J.C. Yu, W. Ho, J.G. Yu, H. Yip, P.K. Wong, J.C. Zhao, Environ. Sci.
Technol. 39 (2005) 1175.
[5] S.U.M. Khan, M. Al-shahry, W.B.Jr. Ingler, Science 297 (2002)
2243.
[6] J.C. Yu, J.G. Yu, W.K. Ho, Z.T. Jiang, L.Z. Zhang, Chem. Mater. 14 (2002)
3808.
[7] D. Li, H. Haneda, N.K. Labhsetwar, S. Hishita, N. Ohashi, Chem. Phys.
Lett. 401 (2005) 579.
[8] A. Hattori, K. Shimota, H. Tada, S. Ito, Langmuir 15 (1999) 5422.
[9] C.M. Wang, T.E. Mallouk, J. Am. Chem. Soc. 112 (1990) 2016.
[10] C. Minero, G. Mariella, V. Maurino, E. Pelizzatti, Langmuir 16 (2000)
2632.
[11] C. Minero, G. Mariella, V. Maurino, D. Vione, E. Pelizzetti, Langmuir 16
(2000) 8964.
[12] M.S. Vohra, S. Kim, W. Choi, J. Photochem. Photobiol. A 160 (2003) 55.
[13] A. Hattori, M. Yamamoto, H. Tada, S. Ito, Chem. Lett. 8 (1998)
707.
[14] C.K. Xu, R. Killmeyer, M.L. Gray, S.U.M. Khan, Appl. Catal. B 64 (2006)
312.
[15] D. Li, H. Haneda, S. Hishita, N. Ohashi, N.K. Labhsetwar, J. Fluorine
Chem. 126 (2005) 69.
[16] H. Park, W. Choi, J. Phys. Chem. B 108 (2004) 4086.
[17] H. Yamashita, Y. Ichihashi, S.G. Zhang, Y. Matsumura, Y. Souma, T.
Tatsumi, M. Anpo, Appl. Surf. Sci. 121 (1997) 305.
[18] T. Yamaki, T. Umebayashi, T. Sumita, S. Yamamoto, M. Maekawa, A.
Kawasuso, H. Itoh, Nucl. Instrum. Methods Phys. Res. B 306 (2003)
254.
[19] W. Ho, J.C. Yu, S. Lee, Chem. Commun. (2006) 1115.
[20] X.P. Zhao, J.B. Yin, Chem. Mater. 14 (2002) 2258.
[21] J.G. Yu, Z. Xiujian, Z. Qingnan, Thin Solids Films 379 (2000) 7.
[22] X.Y. Li, X. Quan, C. kutal, Scripta Mater. 50 (2004) 499.
[23] J. Matos, J. Laine, J.M. Herrmann, Appl. Catal. B 18 (1998) 281.