comparison of the effect of hydrogen incorporation and oxygen vacancies on the properties of anatase...
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Artic le Materials Science
Comparison of the effect of hydrogen incorporation and oxygenvacancies on the properties of anatase TiO2: electronics, opticalabsorption, and interaction with water
Hui Jin • Lianzhou Wang • Debra J. Searles •
Chenghua Sun
Received: 3 September 2013 / Accepted: 18 October 2013 / Published online: 11 March 2014
� Science China Press and Springer-Verlag Berlin Heidelberg 2014
Abstract Hydrogenation has been recently developed as
an approach to improve the visible-light response of titanium
dioxide (TiO2); however, the effect of hydrogenation on the
electronics and optical absorption of anatase TiO2 has been
widely debated. In this work, the electronic structures and
optical properties of hydrogenated TiO2 and its interaction
with water have been studied using the density functional
theory plus Hubbard model. A comparison of the effect of
hydrogenation and introduction of oxygen vacancies (OVs)
to TiO2 is presented. It is found that both hydrogenation and
OVs can promote the absorption of visible light and
strengthen the adsorption of water. Compared with OVs,
hydrogen incorporation can lead to local distortion and even
amorphous structures when it is heavily doped.
Keywords Titanium dioxide � Hydrogenation �Oxygen vacancy � Density functional theory �Photocatalysis
1 Introduction
Fabricating photocatalysts with visible light activity is a
major challenge for solar hydrogen production [1]. Gen-
erally, the band structures of photocatalysts need to be
tuned to satisfy several requirements, including narrowed
band gaps to absorb visible light, and proper positions of
the valence band (VB), and conduction band (CB) [2].
A typical example is titanium dioxide (TiO2), which can
only work under ultraviolet (UV) light as determined by its
wide band gap (e.g. 3.20 eV for anatase TiO2) [3–6]. To
improve its response to visible (Vis) light, extensive efforts
have been made to narrow the band gap, such as doping
with metals or nonmetals [7–14]. Typically, dopants are
introduced to replace Ti or O, and thus change the positions
of the VB and/or CB, leading to smaller band gaps [15].
In recent years, hydrogen-incorporated TiO2, denoted as
H@TiO2, has attracted much attention in the band-gap
engineering of TiO2 [16–26]. A unique feature of H-dopants
is that H can be incorporated at the interstitial sites. For
instance, by high-pressure hydrogenation at 200 oC, Chen
et al. [16] obtained black H@TiO2 and achieved a narrowed
gap of 1.54 eV, in which case most visible light and even a
part of the near infrared (NIR) light can be absorbed. Dis-
ordered layers with a thickness of around 1 nm have been
observed, which was believed to account for the observed
Vis–NIR absorption [16]. Wang et al. [17] prepared black
TiO2 (rutile) nanowires via annealing in H2 steam at
200–550 �C, and their samples are highly crystalline. As
revealed by X-ray photoelectron spectroscopy (XPS),
hydrogenation leads to the formation of oxygen vacancies
(OVs) but has little effect on the location of the VB edge,
and thus, it was concluded that OVs account for the dark
color of H@TiO2 [17]. Under high pressure and high tem-
perature (450 �C), our team also obtained highly crystalline
SPECIAL ISSUE: Advanced Materials for Clean Energy
H. Jin � L. Wang � D. J. Searles � C. Sun (&)
Australian Institute for Bioengineering and Nanotechnology,
The University of Queensland, Brisbane, Qld 4072, Australia
e-mail: [email protected]
H. Jin � L. Wang
ARC Centre of Excellence for Functional Nanomaterials, School
of Chemical Engineering, The University of Queensland,
Brisbane, Qld 4072, Australia
D. J. Searles
School of Chemistry and Molecular Biosciences, The University
of Queensland, Brisbane, Qld 4072, Australia
C. Sun
School of Chemistry, Monash University, Melbourne,
VIC 3800, Australia
123
Chin. Sci. Bull. (2014) 59(18):2175–2180 csb.scichina.com
DOI 10.1007/s11434-014-0229-2 www.springer.com/scp
H@TiO2 (anatase), and it is found that the sample colors
strongly depend on the hydrogenation degree, varying from
gray, blue to black [18]. Hoang et al. [19] treated rutile TiO2
arrays at 500 �C under H2/Ar atmosphere, and interestingly,
the TiO2 film remains crystalline and white after the
hydrogenation treatment. Starting from amorphous TiO2,
Naldoni et al. [20] obtained black TiO2 nanoparticles via
heating under H2 stream at 400–500 �C. Both OVs and
disordered structures are presented in their H@TiO2 sam-
ples, and the black color was attributed to the co-existence
of OVs and surface disorder [20].
Although hydrogenated TiO2 has been prepared and
tested by several groups, the effect of hydrogen incorpo-
ration on the electronics and the optical properties of TiO2
hve not been fully understood yet [27–32]. Currently, it is
widely accepted that hydrogen can pass through the TiO2
surface and diffuse into the lattice, and the diffusion barrier
depends on the surface and the diffusion paths [18, 27–30].
As to the origin of the visible light adsorption, two struc-
tural reasons are proposed. Zhao et al. [32] found that
hydrogenation on oxygen is more favorable than that on
titanium; as a result, Ti3? is generated, and mid-gap states
are introduced, which they determine is the origin of the
Vis light absorption. In contrast, Chen et al. [31] suggested
that the mid-gap states actually origin from the disordered
structures, rather than Ti3?, and amorphous layers can
promote the hydrogen diffusion. Therefore, it is desirable
to further discuss the role of hydrogenation on the prop-
erties of TiO2.
In this work, density functional theory (DFT) calcula-
tions have been carried out to examine the electronics,
optical properties, and interaction of hydrogenated TiO2
with water. Given OV can lead to the formation of Ti3?, all
results are compared with TiO2 containing OVs.
2 Computational methods
Anatase TiO2 is modeled by a periodic (1 9 2) slab of (101)
surface with three Ti–O layers, as shown in Fig. 1. As a
reference, OV is generated by removing one oxygen atom
randomly, and labeled as OV@TiO2, as shown in Fig. 1a.
For H@TiO2, four hydrogen atoms are incorporated through
(101) into the lattice and located at the interstitial sites to
represent the H@TiO2, as shown in Fig. 1a. This above
model is based on two considerations: (1) (101) is the most
stable facet for clean TiO2 crystals [33], and although TiO2
with high percentage of minority surface (001) has been
synthesized in recent years [34–38], most crystals of TiO2
using in reports on H@TiO2 have not used that synthesis and
(2) hydrogen incorporation through the (001) surface is more
difficult (barrier: 1.49 eV) than that through (101) (barrier:
0.88 eV) [18]. Moreover, TiO2(001) containing H-dopants
and OVs has been tested. It is found that the conclusion
regarding the difference between OVs and H-doping
obtained with the (101) slab models and presented in this
work has no change if (001) model is employed. Over the
surface, a vacuum space of 15 A has been introduced to
eliminate the interaction between neighboring slabs.
Spin-polarized DFT has been carried out to optimize the
geometry and calculate the electronic structures within the
generalized-gradient approximation (GGA) [39], together
with the exchange–correlation functional of Perdew-Burke-
Ernzerhof (PBE) [40, 41], as implemented in the Vienna
ab initio simulation package (VASP) [42, 43]. The reci-
procal space has been spanned with a plane-wave basis
with a kinetic energy cutoff of 350 eV. The k-space is
sampled by a Monkhorst–Pack mesh of 7 9 7 9 1. Given
that OV is involved, the on-site electron correlation is
essential, and thus DFT plus Hubbard model (DFT ? U)
[44–48] has been employed in our calculations. In our case
U = 4.0 eV has been selected based on early publications
[49]. From the optimized geometries, the imaginary
dielectric function, labeled as Im, has been obtained by
calculating the frequency-dependent dielectric matrix with
a large number of empty bands, using the formula descri-
bed by Gajdos et al. [50].
3 Results and discussion
3.1 Electronic structures
The effect of H-dopants and OVs on the electronic struc-
tures of TiO2 has been firstly studied, and the spin-polar-
ized band structures are plotted in Fig. 2. For undoped
TiO2, the calculated band-gap (Eg) is 2.75 eV, which
agrees well with published results with U = 4.0 eV [49].
When an OV is introduced, four local states (LS), with two
occupied (dotted lines) and two unoccupied states (thick
Fig. 1 (Color online) Slab models for a OV@TiO2 and b H@TiO2.
H atoms have been labeled directly, and O is denoted as a sphere with
a circle, with the rest as Ti atoms. OV is indicated by the bigger
sphere in (a)
2176 Chin. Sci. Bull. (2014) 59(18):2175–2180
123
black lines), are generated, as shown in Fig. 2a, but there is
almost no change in the band gap. With insertion of four
H-atoms at interstitial sites, H-atoms directly bond with
oxygen, leading to the breakage of Ti–O bonds, as shown
in Fig. 1b. Electronically, four local occupied states
between Fermi energy (dashed thin line) and VB are gen-
erated, and these are shown as dotted green lines in Fig. 2b.
This is not surprising since each hydrogen can contribute
one electron to the system. In addition, the Eg has increased
from 2.75 to 2.97 eV, indicating that such hydrogen
incorporation does not narrow but enlarge the Eg.
Similarly, it was recently reported that interstitial boron
also has no effect on the Eg narrowing of TiO2 [51]. For
sunlight harvest, both OV@TiO2 and H@TiO2 may offer
the capacity to adsorb visible light due to the existence of
local states, which will be further explored below.
3.2 Optical adsorption
For hydrogenated TiO2, it has been widely observed that
the color can change from white to gray, blue, and even
black, depending on the hydrogenation conditions [18].
–2
–1
0
FQΓ Z Γ
En
erg
y (e
V)
(a)
Spin up
Eg
–2
–1
0
En
erg
y (e
V)
Spin down
FQΓ Z Γ
–3
–2
–1
0
En
erg
y (e
V)
(b)
Spin up
Eg
FQΓ Z Γ–3
–2
–1
0
En
erg
y (e
V)
Spin down
FQΓ Z Γ
Fig. 2 Calculated band structures for a OV@TiO2 and b H@TiO2. Fermi energy, occupied, and unoccupied local states are indicated by red,
green, and blue dashed lines, respectively
0 1 2 3 4 5 60
1
2
3
4
5<010>
Im <001>
<100>
Energy (eV)
(a)
0 1 2 3 4 5 60
1
2
3
4
5
<010>
Im <001>
<100>
Energy (eV)
(b)
Fig. 3 Calculated imaginary part of the dielectric function for a OV@TiO2 and b OV @TiO2
Chin. Sci. Bull. (2014) 59(18):2175–2180 2177
123
To understand the effect of hydrogenation on optical
adsorption, the imaginary part of the dielectric functions of
OV@TiO2 and H@TiO2 (labeled as Im) has been calcu-
lated. To depict the anisotropy, the value of Im along the
\100[,\010[, and\001[directions are shown in Fig. 3.
For both OV@TiO2 and H@TiO2, two adsorption peaks
are observed, located at 1.0–2.0 eV and 3.0–5.0 eV, which
can be assigned to the LS ? CB and VB ? CB excita-
tions based on the calculated band structures. In principle,
the excitations from occupied LS to unoccupied LS can
also contribute to the adsorption in the range of 1.0–2.0 eV,
depending on the mobility of electrons in these states.
The effect of adding more H-atoms to H@TiO2 can be
considered, and it is found that heavy hydrogenation may
lead to significant distortion, resulting in the formation of
defects and even amorphous layers. Chen et al. [16]
reported that long-term hydrogenation can lead to the for-
mation of amorphous layers and TiO2 samples become
black. Combining the calculated band structures and opti-
cal profiles, it is speculated that heavy hydrogenation
introduces a large number of local states, which are
involved in the optical adsorption, and thus, result in the
color change of the TiO2 crystals. In terms of optical
adsorption, OV@TiO2 and H@TiO2 show similar features,
except that the first adsorption peak of H@TiO2 is dis-
tributed over a wider range, which may be related to the
local distortion associated with the hydrogenation. Exper-
imentally, blue TiO2 containing -1.0 wt% hydrogen
becomes gray after the dehydrogenation, supporting the
above conclusion that H-dopants can effectively extend the
distribution of local states and strengthen the adsorption
of visible lights. Therefore, with respect to OV@TiO2,
H@TiO2 offers a more flexible approach to adjust the
optical adsorption of TiO2 photocatalysts.
3.3 Interaction with water
As well as sunlight absorption, the charge transfer between
TiO2 and water is another critical factor for photocatalytic
water-splitting, which is determined by the interaction
between water and TiO2. Over a clean (101) surface, it is
widely accepted that water is adsorbed molecularly, and
the calculated adsorption energy is 0.77 eV by standard
DFT (using PBE functional) [52, 53]. In this work, it is
×DO
S (
a.u
.)
Energy (eV)
(b)
H2O
Total
×
100
10
–12 –9 –6 –3 0 3
–9 –6 –3 0 3
DO
S (
a.u
.)
Energy (eV)
(d)
(a)
(c)
H2O
Total
×10
Fig. 4 (Color online) Adsorption of single water (as circled). a Optimized geometries and b DOS for water on OV@TiO2, and c optimized
geometries and d DOS for water on H@TiO2
2178 Chin. Sci. Bull. (2014) 59(18):2175–2180
123
found that the energy is 0.64 eV for single water adsorp-
tion, with a deviation of 0.13 eV due to the Hubbard cor-
rection. With OV in the sub-layer, as shown in Fig. 4a, the
adsorption energy is slightly increased to 0.91 eV. From
the calculated density of states (DOS) profile shown in
Fig. 4b, it is observed that a small fraction of the local DOS
of water has the same energy levels as the occupied LSs
introduced by OVs (indicated by the blue dashed lines).
Those occupied LSs mainly locate at unsaturated Ti-atoms,
and the water-TiO2 interaction can promote the electron
transfer through the Ti–O bonding.
As to water adsorption, several starting geometries are
tested with single water being introduced on the surfaces of
H@TiO2 and OV@TiO2. Figure 4c shows the most pre-
ferred geometry on H@TiO2, and the corresponding DOS
profile is present in Fig. 4d. With respect to water on
OV@TiO2, the adsorption energy is much higher, being up
to 1.52 eV, which is close to that by typical chemical
adsorption. From the optimized geometry, however, there
is no water dissociation, and such high adsorption energy is
still obtainable when the second water is introduced
(averaged Eads = 1.37 eV). If four and eight water mole-
cules are introduced on the surface, the averaged Eads will
decrease to 0.4–0.8 eV, corresponding to typical physical
adsorption. From the DOS profile, the local DOS of water
has almost no overlap with the LSs associated with
H-dopants, which is another difference from water on the
surface of OV@TiO2. Interestingly, a new distribution of
the local DOS of water appears in the VB range, as labeled
by the arrow in Fig. 4d. Given the VB is dominated by O2p
states, the above result may indicate stronger interaction
between water and surface oxygen, which may explain the
increase of adsorption energy. Another possibility is that
water can stabilize the surface layers of H@TiO2: as
revealed in Sect. 3.1, heavy hydrogenation may lead to
strong local distortion and strain energy, while the Ti–Ow
and H–O2c (two-coordinated oxygen on TiO2 surface)
bonding can effectively stabilize those surface atoms and
release local strain energy.
4 Conclusion
Using the DFT ? U approach, the geometries, electronic
structures, optical absorption, and water adsorption have
been discussed and compared for OV@TiO2 and H@TiO2.
Both OV and H-dopants can introduce LS between VB and
CB, which promote the adsorption of visible light, and such
promotion is achieved through the LS ? CB excitation,
rather than narrowing the band-gap. In addition, stronger
water-TiO2 interactions can be achieved through the
introduction of an OV and hydrogenation because both OV
and H-dopants can lead to more lowly saturated surface
atoms, which can actively interact with water. To clarify
whether these mid-gap states can promote water-splitting
or just serve as a recombination center of the electron–hole
pairs, the excited states of water-TiO2 system, and the
charge transfer should be further examined.
Acknowledgments This work was supported by Australian
Research Council through Discovery Project and Future Fellowship
(CHS). The authors also appreciate the generous grants of CPU time
from both the University of Queensland and the Australian National
Computational Infrastructure Facility.
References
1. Fujishima A, Honda K (1972) Electrochemical photolysis of
water at a semiconductor electrode. Nature 238:37–38
2. Wu Y, Lazic P, Hautier G et al (2013) First principles high
throughput screening of oxynitrides for water-splitting photo-
catalysts. Energy Environ Sci 6:157–168
3. Diebold U (2003) The surface science of titanium dioxide. Surf
Sci Rep 48:53–229
4. Chen X, Mao SS (2007) Titanium dioxide nanomaterials: syn-
thesis, properties, modifications, and applications. Chem Rev
107:2891–2959
5. Fujishima A, Zhang X, Tryk DA (2008) TiO2 photocatalysis and
related surface phenomena. Surf Sci Rep 63:515–582
6. Chen X, Shen S, Guo L et al (2010) Semiconductor-based pho-
tocatalytic hydrogen generation. Chem Rev 110:6503–6570
7. Asahi A, Morikawa T, Ohwaki T et al (2001) Visible-light photo-
catalysis in nitrogen-doped titanium oxides. Science 293:269–271
8. Khan SUM, Al-Shahry M, Ingler WB (2002) Efficient photo-
chemical water splitting by a chemically modified n-TiO2. Sci-
ence 297:2243–2245
9. Zaleska A (2008) Doped-TiO2: a review. Recent Patents Eng
2:157–164
10. Liu G, Zhao YN, Sun CH et al (2008) Synergistic effects of B, N
co-doping on the visible light photocatalytic activity of meso-
porous TiO2. Angew Chem Int Ed 47:4516–4520
11. Liu G, Wang L, Sun CH et al (2009) Nitrogen-doped titania
nanosheets towards visible light response. Chem Commun
11:1383–1385
12. Liu G, Wang LZ, Sun CH et al (2009) Band-to-band visible-light
photon excitation and photoactivity induced by homogeneous
nitrogen doping in layered titanates. Chem Mater 21:1266–1274
13. Diwald O, Thompson TL, Zubkov T et al (2004) Photochemical
activity of nitrogen-doped rutile TiO2 (110) in visible light.
J Phys Chem B 108:6004–6008
14. Burda C, Lou Y, Chen X et al (2003) Enhanced nitrogen doping
in TiO2 nanoparticles. Nano Lett 3:1049–1051
15. Liu G, Wang L, Yang HG et al (2010) Titania-based photocat-
alysts—crystal growth, doping and heterostructuring. J Mater
Chem 20:831–843
16. Chen X, Yu PY, Mao SS (2011) Increasing solar absorption for
photocatalysis with black hydrogenated titanium dioxide nano-
crystals. Science 331:746–750
17. Wang G, Wang H, Ling Y et al (2011) Hydrogen-treated TiO2
nanowire arrays for photoelectrochemical water splitting. Nano
Lett 11:3026–3033
18. Sun CH, Jia Y, Yang XH et al (2011) Hydrogen incorporation
and storage in well-defined nanocrystals of anatase titanium
dioxide. J Phys Chem C 115:25590–25594
19. Hoang S, Berglund SP, Hahn NT et al (2012) Enhancing visible
light photo-oxidation of water with TiO2 nanowire arrays via
Chin. Sci. Bull. (2014) 59(18):2175–2180 2179
123
cotreatment with H2 and NH3: synergistic effects between Ti3?
and N. J Am Chem Soc 134:3659–3662
20. Naldoni A, Allieta M, Santangelo S et al (2012) Effect of nature
and location of defects on bandgap narrowing in black TiO2
nanoparticles. J Am Chem Soc 134:7600–7603
21. Lu X, Wang G, Zhai T et al (2012) Hydrogenated TiO2 nanotube
arrays for supercapacitors. Nano Lett 12:1690–1696
22. Pan H, Zhang YW, Shenoy VB et al (2011) Effects of H-, N-, and
(H, N)-doping on the photocatalytic activity of TiO2. J Phys
Chem C 115:12224–12231
23. Leshuk T, Parviz R, Everett P et al (2013) Photocatalytic activity
of hydrogenated TiO2. ACS Appl Mater Interfaces 5:1892–1895
24. Zheng Z, Huang B, Lu J et al (2012) Hydrogenated titania: syn-
ergy of surface modification and morphology improvement for
enhanced photocatalytic activity. Chem Commun 48:5733–5735
25. Lu J, Dai Y, Jin H et al (2011) Effective increasing of optical
absorption and energy conversion efficiency of anatase TiO2 nano-
crystals by hydrogenation. Phys Chem Chem Phys 13:18063–18068
26. Jiang X, Zhang Y, Jiang J et al (2012) Characterization of oxygen
vacancies associates within the hydrogenated TiO2: a positron
annihilation study. J Phys Chem C 116:22619–22624
27. Bavykin DV, Lapkin AA, Plucinski PK et al (2005) Reversible
storage of molecular hydrogen by sorption into multilayered TiO2
nanotubes. J Phys Chem B 109:19422–19427
28. Hu X, Skadtchenko BO, Trudeau M et al (2006) Hydrogen
storage in chemically reducible mesoporous and microporous Ti
oxides. J Am Chem Soc 128:11740–11741
29. Kunat M, Burghaus U, Woll C (2004) The adsorption of hydrogen on
the rutile TiO2(110) surface. Phys Chem Chem Phys 6:4203–4207
30. Yin XL, Calatayud M, Qiu H et al (2008) Diffusion versus
desorption: complex behavior of H atoms on an oxide surface.
ChemPhysChem 9:253–256
31. Chen X, Liu L, Liu Z et al (2013) Properties of disorder-engi-
neered black titanium dioxide nanoparticles through hydrogena-
tion. Sci Rep 3:1510
32. Zhao Y, Hou T, Li Y et al (2013) Effective increasing of optical
absorption of TiO2 by introducing trivalent titanium. Appl Phys
Lett 102:171902
33. Lazzeri M, Vittadini A, Selloni A (2001) Structure and energetics
of stoichiometric TiO2 anatase surfaces. Phys Rev B 63:155409
34. Yang HG, Sun CH, Qiao SZ et al (2008) Anatase TiO2 single
crystals with a large percentage of 001 facets. Nature 453:638–641
35. Yang HG, Liu G, Qiao SZ et al (2009) Solvothermal synthesis
and photoreactivity of anatase TiO2 nanosheets with dominant
001 facets. J Am Chem Soc 131:4078–4083
36. Han X, Kuang Q, Jin M et al (2009) Synthesis of titania nano-
sheets with a gigh percentage of exposed (001) facets and related
photocatalytic properties. J Am Chem Soc 131:3152–3153
37. Liu G, Sun CH, Yang HG et al (2010) Nanosized anatase TiO2
with preferential 001 facets for drastically enhanced photocatal-
ysis. Chem Commun 46:755–757
38. Yang XH, Li Z, Sun CH et al (2011) Hydrothermal stability of
001 faceted anatase TiO2. Chem Mater 23:3486–3494
39. Kohn W, Sham LJ (1965) Self-consistent equations including
exchange and correlation effects. Phys Rev 140:A1133–A1138
40. Perdew JP, Burke K, Ernzerhof M (1996) Generalized gradient
approximation made simple. Phys Rev Lett 77:3865–3868
41. Kresse G, Joubert D (1999) From ultrasoft pseudopotentials to the
projector augmented-wave method. Phys Rev B 59:1758–1775
42. Kresse G, Furthmuller J (1996) Efficient iterative schemes for
ab initio total-energy calculations using a plane-wave basis set.
Phys Rev B 54:11169–11186
43. Kresse G, Furthmuller J (1996) Efficiency of ab initio total
energy calculations for metals and semiconductors using a plane-
wave basis set. Comput Mater Sci 6:15–50
44. Anisimov VI, Zaanen J, Andersen OK (1991) Band theory and
Mott insulators: Hubbard U instead of Stoner I. Phys Rev B
44:943–954
45. Anisimov VI, Aryasetiawan F, Liechtenstein AI (1997) First-
principles calculations of the electronic structure and spectra of
strongly correlated systems: the LDA ? U Method. J Phys:
Condens Matter 9:767–808
46. Rohrbach A, Hafner J, Kresse G (2003) Electronic correlation
effects in transition-metal sulfides. J Phys: Condens Matter
15:979–996
47. Solovyev IV, Deterichs PH, Anisimov VI (1994) Corrected
atomic limit in the local-density approximation and the electronic
structure of d impurities in Rb. Phys Rev B 50:16861–16871
48. Pickett WE, Erwin SC, Ethridge EC (1998) Reformulation of the
LDA ? U method for a local-orbital basis. Phys Rev B
58:1201–1209
49. Finazzi E, Di Valentin C, Pacchioni G et al (2008) Excess
electron states in reduced bulk anatase TiO2: comparison of
standard GGA, GGA ? U, and hybrid DFT calculations. J Chem
Phys 129:154113
50. Gajdos M, Hummer K, Kresse G et al (2006) Linear optical
properties in the PAW methodology. Phys Rev B 73:045112
51. Liu G, Yin LC, Wang J et al (2012) A red anatase TiO2 photocat-
alyst for solar energy conversion. Energy Environ Sci 5:9603–9610
52. Sun CH, Liu LM, Selloni A et al (2010) Titania-water interactions:
a review of theoretical studies. J Mater Chem 20:10319–10334
53. Posternak M, Baldereschi A, Delley B (2009) Dissociation of
water on anatase TiO2 nanoparticles: the role of undercoordinated
Ti atoms at edges. J Phys Chem C 113:15862–15867
2180 Chin. Sci. Bull. (2014) 59(18):2175–2180
123