Hybrids of Two-Dimensional Ti C and TiO Exposing {001
-
Upload
others
-
View
0
-
Download
0
Embed Size (px)
Citation preview
am5b11973 1..10Hybrids of Two-Dimensional Ti3C2 and TiO2 Exposing
{001} Facets toward Enhanced Photocatalytic Activity Chao Peng,†
Xianfeng Yang,‡ Yuhang Li,† Hao Yu,*,† Hongjuan Wang,† and Feng
Peng†
†School of Chemistry and Chemical Engineering, South China
University of Technology, Guangzhou, 510640, China ‡Analytical and
Testing Center, South China University of Technology, Guangzhou,
Guangdong 510640, P. R. China
*S Supporting Information
ABSTRACT: Effectively harvesting light to generate long-lived
charge carriers to suppress the recombination of electrons and
holes is crucial for photocatalytic reactions. Exposing the highly
active facets has been regarded as a powerful approach to high-
performance photocatalysts. Herein, a hybrid comprised of {001}
facets of TiO2 nanosheets and layered Ti3C2, an emerging 2D
material, was synthesized by a facile hydrothermal partial
oxidation of Ti3C2. The in situ growth of TiO2 nanosheets on Ti3C2
allows for the interface with minimized defects, which was
demonstrated by high-resolution transmission electron microscopy
and density functional theory calculations. The highly active {001}
facets of TiO2 afford high-efficiency photogeneration of
electron−hole pairs, meanwhile the carrier separation is
substantially promoted by the hole trapping effect by the
interfacial Schottky junction with 2D Ti3C2 acting as a reservoir
of holes. The improved charge separation and exposed active facets
dramatically boost the photocatalytic degradation of methyl orange
dye, showing the promise of 2D transition metal carbide for
fabricating functional catalytic materials.
KEYWORDS: MXenes, layered Ti3C2, (001) TiO2, Schottky junction,
hole trapping
1. INTRODUCTION
In response to the increasing environmental and energy-related
concerns, photocatalysis is considered as a promising approach to
clean environment and sustainable energy. As an enabling material,
titania plays a central role in a variety of photo/
photoelectrocatalytic processes across a wide spectrum from
pollutant cleanup1 to water splitting2 and artificial photosyn-
thesis,3 because of its high activity, low cost, environmental
benignity, and good chemical stability. However, so far, the
practical application of TiO2-based photocatalytic processes is
still hindered by the low-efficiency caused by the rapid
recombination of photogenerated electrons and holes. Cou- pling
TiO2 with foreign metals or semiconductors to form heterojunctions
can effectively separate the photogenerated electron−hole pairs and
thereby increase the lifetime of charge carriers, through electron
trapping,4 proper band alignment,5
and plasmonic effect.6 To this end, the interface between two
components has to be rationally designed to facilitate the transfer
of charge carriers and their spatial separation. In principle, an
interfacial engineering should be exerted to select appropriate
components,7,8 maximize the contacting area,7,8
and minimize the interfacial defects,7,8 where the recombina- tion
usually occurs. Besides, special attention should be paid to the
morphology and contacting pattern of two components. On one hand,
the electronic property of low-dimensional materials strongly
depends on their configuration. For example, a 2- dimensional (2D)
form of carbon, graphene, could display superior performance to its
1D and 0D allotropes, carbon nanotube and fullerene, as constructed
composites with TiO2
due to the intimate contact.9,10 On the other hand, the
photoexcitation is structurally sensitive because of the different
surface energy and atomic configuration of different crystalline
facets, which have been proved on the (001) surface of TiO2
11−13 and the (111) surface of Cu2O. 14 Taking TiO2 as an
example, the charge separation could be quite different when a
heterojunction formed on different surfaces, because (i) the
photogeneration rate of electron−hole pairs is different;15 and
(ii) the different work functions (Φ) of TiO2 facets16 may
Received: December 8, 2015 Accepted: February 9, 2016 Published:
February 9, 2016
Research Article
© 2016 American Chemical Society 6051 DOI: 10.1021/acsami.5b11973
ACS Appl. Mater. Interfaces 2016, 8, 6051−6060
D ow
nl oa
de d
vi a
C H
O N
G Q
IN G
U N
IV o
n Ja
nu ar
y 13
, 2 01
9 at
1 2:
33 :3
5 (U
T C
19,20 and MoS2-(001) TiO2. 21
MXenes, a new family of 2D materials composed of transition metal
carbides and carbonitrides, have attracted intensive interest since
their discovery in 2011,22 because of their excellent structural
stability, high electrical conductivity, and hydrophilicity.23,24
Ti3C2Tx (T = OH, F, or O) nanosheets are currently the most studied
MXene, which can be readily obtained by selectively etching and
exfoliating Ti3AlC2 ceramics with HF.22 Benefiting from their high
electrical conductivity and 2D structure, Ti3C2Tx has been regarded
as an energy storage material for anodes of Li-ion batteries
(LIBs),25,26
lithium−sulfur batteries,27,28 and electrochemical capaci-
tors.29−31 The unique morphology, dispersibility, and stability
also make Ti3C2Tx attractive as adsorbents for heavy metal ions or
dyes32−34 and as supports for catalysts.35,36 Moreover, a recent
computational study showed that the huge difference between the
hole and electron mobility in a Ti2CO2 bilayer makes it promising
for separating holes and electrons in photocatalysis.37
As a compound of titanium and carbon, Ti3C2Tx affords a natural
platform to construct composites of TiO2 and carbonaceous
materials, which have been widely recognized as a class of
high-performance photocatalyst,9 in which carbonaceous materials
may prolong the lifetime of electron− hole pairs, tune the band
gap, and adsorb reactants.9,10 More importantly, the titanium atoms
on Ti3C2Tx may act as nucleating sites to allow the growth of TiO2
photocatalysts; thereby, an atomic scale interfacial heterojunction
between 2D Ti3C2 and TiO2 could be facilely formed to minimize the
defect-induced recombination. Hitherto, few reports have been
devoted to this topic.38,39 Naguib et al. have reported that an
oxidation of laminar Ti3C2Tx resulted in TiO2 nanocrystals
decorated on disordered carbon sheets, as a good LIB anode
material.38 By a hydrothermal deposition of TiO2, a TiO2/ Ti3C2
composite was fabricated for photocatalytic application but with a
limited improvement.39 In these preliminary works, the interfaces
between the TiO2−Ti3C2 heterojunction have not been properly
designed to optimize the photocatalytic activity. Herein, the
layered Ti3C2 was used to fabricate a hybrid of
TiO2 nanosheets selectively exposing {001} facets and 2D Ti3C2
((001)TiO2/Ti3C2) through a facile hydrothermal oxidation route
without any additional Ti source (Scheme 1). In this design,
electrons and holes are photogenerated on the (001) surfaces of
TiO2, the most active surface for photo- catalysis. 2D Ti3C2(OH)x
sheets act as a reservoir of the charge carriers to prolong their
lifetime, because of the high mobility of charge carriers,
especially holes.37 The interfacial bonding was guaranteed under
hydrothermal conditions utilizing Ti atoms in Ti3C2 sheets as Ti
sources and nucleating centers, which may minimize the interfacial
defects. Through this design, the photogenerated charge carriers
were effectively separated, and the reaction rate of methyl orange
(MO) dye decomposition was improved, showing the promise of MXene
as an excellent charge separator for photocatalysis.
2. EXPERIMENTAL SECTION 2.1. Synthesis of layered Ti3C2. The
layered Ti3C2 was fabricated
by selectively exfoliating the Al layers from Ti3AlC2 with HF (49
wt %) at 60 °C for 12 h with stirring. Then the solids were
centrifuged, thoroughly rinsed with DI water, and dried.
2.2. Synthesis of (001)TiO2/Ti3C2 and p-TiO2/Ti3C2. Typically, 100
mg of the layered Ti3C2 was suspended in 15 mL of 1.0 M HCl
containing 0.165 g of NaBF4. After stirring for 30 min and
ultrasonication for 10 min, the suspension was transferred into a
100 mL Teflon-lined stainless steel autoclave for a hydrothermal
oxidation at 120−220 °C for 4−32 h (see the Supporting Information
for more details). With the morphology-directing reagent NaBF4, the
(001)TiO2/Ti3C2 can be grown, as illustrated in Scheme 1.
The particulate TiO2/Ti3C2 (p-TiO2/Ti3C2) was synthesized through a
facile hydrothermal method. 100 mg of Ti3C2 powder was added to 15
mL deionized water, and was stirred for 30 min followed by
additional ultrasonication for 10 min. Thereafter, the suspension
was transferred into a 100 mL Teflon-lined stainless steel
autoclave for a hydrothermal reaction at 160 °C for appropriate
durations.
2.3. Characterizations. Electron probe microanalysis (EPMA- 1600,
Shimadzu) was used to analyze the contents of various elements. The
structure of the materials were investigated by X-ray diffraction
analysis (XRD, Bruker D8 Advance, Germany) at 40 kV and 40 mA using
Cu Ka radiation, and performed in an angle range of 5−70°. The
Brunauer−Emmett−Teller (BET) specific surface areas (SBET) of the
samples were measured by N2 adsorption at liquid N2 temperature in
an ASAP 2010 analyzer. The surface morphology and the micro-
structure of the as-prepared samples were characterized by field
emission scanning electron microscopy (FESEM, Zeiss Merlin) at an
acceleration voltage of 5 kV. The STEM image, EDX elemental
mapping, TEM image and HRTEM images were all taken in a JEOL
JEM-2100F at an operating voltage of 200 kV. X-ray photoelectron
spectroscopy (XPS) was carried out in a Kratos Axis ultra (DLD)
spectrometer equipped with an Al Ka X-ray source. Binding energies
were referenced to the C 1s peak of (C−C) bond which set at 284.8
eV. The optical properties of all samples were obtained using a UV−
vis diffuse reflectance spectroscope (DRS, Hitachi-U3010) with an
integrated sphere attachment. FT-IR spectrometer (Nicolet 6700,
USA) of all samples was examined with a slice of powered potassium
bromide and sorbent in 400−4000 cm−1.
2.4. Photocatalytic reaction. Methyl orange (MO) was selected as a
probe chemical to evaluate the photocatalytic activity of the
photocatalysts. The photocatalytic reaction was conducted in a
cylindrical glass vessel fixed in the XPA-II photochemical
reactor
Scheme 1. Schematic Illustration of the Ti3AlC2 Exfoliation Process
and the Subsequent Formation of (001)TiO2/Ti3C2 Hybrids
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
(Nanjing Xujiang Machine-electronic Plant). Ten mg catalysts were
dispersed in 200 mL MO aqueous solution (20 mg L−1) in the dark
with strong stirring for 1 h to achieve adsorption equilibrium. Air
was bubbled into the reaction solution at a constant rate.
Thereafter it was irradiated by the ultraviolet (UV) light
generated from a 300 W mercury lamp. Five mL solution was taken out
every 10 min, centrifuged to remove the catalyst, and then measured
on a UV−vis spectrophotometer (Shimadzu UV 2550). In recycling
experiments, the used catalysts were washed with deionized water
for several times and dried at ambient temperature under vacuum
before each test. Isopropanol (IPA), ammonium oxalate (AO), and
p-benzoquinone (BQ) were used as scavenger of •OH, h+, and
•O2
−, respectively, to identify the active species in the
photocatlytic reaction. The trapping experiments were carried out
under the same conditions as those for photocatalytic reaction,
except for adding 1 mM of the trapping reagent. 2.5. Preparation of
photoelectrodes and Photoelectrochem-
ical measurement. For the photoelectrochemical measurement studies,
the electrodes were prepared by an electrophoretic deposition
method. The electrophoretic deposition was carried out by
dispersing 40 mg of samples and 10 mg iodine powder in 50 mL of
acetone. In this process, acetone reacts with iodine generating H+,
so that the photocatalyst particles were positively charged. Under
magnetic stirring, two parallel FTO (fluorine doped tin oxide)
glasses were immersed in the solution with a 10−15 mm separation,
and a 50 V bias was applied using a DC power supply for 10 min.
With the DC voltage was applied, the particles were deposited on
the cathode. The coated area was about 1.5 cm × 1 cm and then
dried. Photoelectrochemical measurements were measured in a
standard
three-electrode cell with a quartz window by electrochemical
workstation (CHI 660D Instruments Inc., Shanghai). The as-prepared
electrode was used as the working electrode, and a platinum net and
an Ag/AgCl electrode were used as the counter and reference
electrodes, respectively. The photocurrents were measured on a CHI
660D electrochemical station (Shanghai Chenhua, China), a 300 W Xe
arc lamp (Beijing Changtuo, China) equipped with a visible cut off
filter to provide ultraviolet light. 0.1 M Na2SO4 aqueous solution
(pH ≈ 6) was used as the electrolyte for photocurrent measurement.
1.0 M NaOH aqueous solution (pH = 13.6) was used as electrolyte
for
transient open-circuit voltage decay (OCVD) (i.e., photovoltage−
time) curves.
2.6. Computational Methods. To assess the interaction in the
TiO2/Ti3C2 interface layer, density functional theory (DFT)
calculations were performed with DMol3 Package in Materials Studio.
Because the Ti3C2 layer can be regarded as substrate, we fixed the
atomic position of Ti3C2 and only relaxed the atoms in TiO2.
Exchange-correlation functions were described by generalize
gradient approximation (GGA) with Perdew-Burke-Emzerhof (PBE). DFT
Semicore Pseudopots (DSPPs) was adopt as core treatment. Double
numerical plus polarization (DNP) was employed as the basis set,
which is comparable to 6-31G** in Gaussian. The orbital cutoff of
5.5 Å was assigned to global atoms. In addition, Grimme method for
the long-range interaction correction was applied throughout
calculations. The convergence tolerance of self-consistent field
(SCF) calculations was 1.0 × 10−5 Ha and the energy convergence for
geometry optimizations was 1.0 × 10−5 Ha. The k-point in the first
Brillouin zone was set to 12 × 12 × 1, which kept same to density
of states (DOS) and partial density of states (PDOS)
calculations.
Ti3C2 is one of hexagonal cells and we extracted one layer to
investigate the interface properties. The exposed titanium atoms on
the monolayer surface were saturated with hydroxyls. The optimized
lattice parameters are 3.0712 × 3.0712 × c, where c represents the
direction of vacuum layer. The TiO2-anatase cell belongs to
tetragonal system and we directly used the structure file in
Materials Studio library. In order to fit the Ti3C2 substrate, the
following operations were prepared for the calculation system. We
converted the imported TiO2-anatase cell into primitive cell, and
cleaved (001) surface. Then adjust γ-angle to 120° and the lattice
length to 6.1424 Å, which is equal to the twice length of Ti3C2
lattice. During the adjustment of parameters, fractional
coordinates of atoms should be kept fixed. Eventually, make a (2 ×
2 × 1) supercell of Ti3C2 and combine two modified structures as
the TiO2/Ti3C2 interface layer.
3. RESULTS AND DISCUSSION
X-ray diffraction (XRD) patterns of the materials are shown in
Figure 1a. After Ti3AlC2 was etched by HF, a (002) reflection of
Ti3C2 at 8.84° can be clearly observed. The (002) at 9.58°
Figure 1. (a) XRD patterns of Ti3AlC2, Ti3C2, and (001)TiO2/Ti3C2.
FESEM images of (b) Ti3C2 with layered structure and (c)
(001)TiO2/Ti3C2 hybrid hydrothermally prepared at 160 °C and for 12
h. The inset images of (c) show the enlarged HRSEM image of the
TiO2−Ti3C2 heterojunctions in the area highlighted by the green
square, and a schematic diagram of an anatase TiO2 crystal exposing
{001} and {101} facets. (d) STEM image and EDX elemental mapping of
the (001)TiO2/Ti3C2.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
and (004) at 19.17° of Ti3AlC2 were broadened and shifted toward
lower angle side, indicating the removal of interlayer Al and the
formation of Ti3C2 nanosheets, as shown in Figure 1b. After the
hydrothermal oxidation, the anatase TiO2 (JCPDS No. 21−1272) phase
emerged, meanwhile, the further shift of (002) peak of Ti3C2 to the
low angle side suggested the further delamination of Ti3C2
nanosheets. Figure 1c displays a typical SEM image of the
TiO2/Ti3C2
hybrid. Square nanosheets in width of ∼400 nm and thickness of ∼50
nm were sideling inserted across the stack of layered Ti3C2 to form
heterostructures (see Supporting Information for more details). The
HRSEM observations show that the interfacial angle between the
{001} and {101} facets of anatase is 68.3° on average, agreeing
well with the anatase TiO2
crystallite exposing a large proportion of {001} planes.11
According to the width and thickness of (001)TiO2 naosheets
observed by SEM, the proportion of {001} facets can be estimated as
about 77.5% from a geometric model of anatase TiO2.
40 The formation of TiO2 was further verified by STEM and EDS
mapping of Ti, O, and C. As shown in Figure 1d, by spotlighting the
area containing a square thin sheet on a large 2D substrate, it was
clearly revealed that the large 2D substrate can be attributed to
titanium carbide and the oxygen-containing small sheet is TiO2. It
should be noted that the carbide sheet contains considerable oxygen
because of hydroxyl groups terminating the surfaces. The formation
of −OH terminated
Ti3C2 can be supported by FTIR spectroscopy, showing the broad
bands at 3431 and 1628 cm−1 (see Figure S7), owing to the
stretching vibration of −OH. In our previous work, the {001}
surface exposed TiO2 can be formed by the hydro- thermal conversion
of TiN powders in the presence of NaBF4,
41 producing random aggregates of TiO2 sheets. In this work, by
controlling the oxidation extent through reaction duration and
temperature, the TiO2 nanosheets can be homogeneously distributed
around the layered Ti3C2 to provide improved accessibility to light
and reactants (see Supporting Information for the effects of
temperature and duration). More importantly, at an appropriate
extent of oxidation, the formation of TiO2/Ti3C2 heterojunctions
would be maximized, where 2D Ti3C2 sheets traverse TiO2 nano-
crystals at the most active {001} facets, as shown in Figure 1c.
The intimate contact between these two phases might facilitate the
separation of charge carriers photogenerated on the {001} surfaces,
thereby improving the photocatalytic activity. The detailed
crystallographic relationship between TiO2 and
Ti3C2 was revealed by HRTEM. Figure 2a clearly shows the growth of
TiO2 between two layers of Ti3C2, whose interfaces can be
distinguished in Figures 2b and c. In Figure 2b, the dashed line
represents the interface between TiO2 and Ti3C2. The typical
layered structure of Ti3C2 can be observed above the interface. The
FFT pattern in Figure 2c confirms that the crystal between two
Ti3C2 sheets is an anatase TiO2 (space
Figure 2. (a) TEM image of TiO2/Ti3C2. (b−e) show the close
observations of the areas highlighted by yellow boxes in (a). (b)
and (c) show the intimate contact of layered Ti3C2 with a TiO2
crystal. (e) shows a growth of TiO2 perpendicular to the [001]
direction of the Ti3C2 sheet. (f) shows a tiny TiO2 crystal formed
near the edge of Ti3C2. The insets (f1) and (f2) show the lattice
fringes of TiO2 and Ti3C2, respectively. The inset of (c) shows the
indexed FFT image of TiO2. The interface structure is shown in (d).
(g) The initial and the final optimized interface structures
simulated by DFT. The black, red, cyan, and green balls stand for
C, O, Ti, and H elements, respectively. Two Ti−O−Ti bonds are
labeled as Ti1−O1−Ti2 and Ti3−O2−Ti4, whose PDOS analyses are shown
in (h) and (i), respectively.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
group I41/amd, a = b = 0.378 nm, c = 0.951 nm) projected along its
[001] direction, namely, exposing {001} facets. A close observation
of the interface is shown in Figure 2d and compared with a
structure optimized by density functional theory (DFT) calculations
with the DMol3 Package in Materials Studio. In this heterojunction,
the lattice of Ti3C2 agrees well with the unit cell parameters of
Ti3C2 provided by Naguib et al.22 The interlayer distance, 0.55 nm,
can be ascribed as the two adjacent −OH groups terminating Ti3C2
sheets. At the interface, the Ti3C2 and TiO2 joint seamlessly on
the atomic level, benefiting from the small mismatch between {103}
of Ti3C2 and {11−1} of TiO2, despite their different crystallo-
graphic form. A DFT calculation suggested that chemical bonding can
be generated at the interface through Ti−O−Ti. Depending on whether
the oxygen atom originates from TiO2 or −OH, two Ti−O−Ti bonds
could be formed, both of which contribute to the interface
formation via overlapping of the Ti d-orbital and the O p-orbital
(Figures 2h,i). The structures in Figures 2e and 2f may help to
rationalize
the growth mechanism of the heterojunction. Figure 2e shows a case
of TiO2 embedded in a Ti3C2 nanosheet, which might represent the
initial stage of TiO2 crystallization without forming a special
orientation. Figure 2f displays a small TiO2 crystal embedded in a
crack of Ti3C2 nanosheets, implying the nucleation of TiO2 may
occur at the defective sites of Ti3C2.
These results may rationalize a plausible growth mechanism of
(001)TiO2/Ti3C2 hybrids. Under the acidic hydrothermal conditions,
the titanium atom of Ti3C2 may transform to hydrated Ti3+ ions42
that can be oxidized to TiO2 at the defects of Ti3C2. Assisted by
the directing reagent NaBF4, the formation of high-energy {001}
facets was enhanced during the sequential crystal growth, because
of the lower energy of {001} planes adsorbing F−.43
The formation of (001)TiO2/Ti3C2 heterojunctions was further
confirmed by XPS. As shown in Figure 3a, The Ti 2p core level is
fitted with four doublets (Ti 2p3/2−Ti 2p1/2) with a fixed area
ratio 2:1 and doublet separation of 5.7 eV.44
The Ti 2p3/2 components centered at 454.8, 455.7, 457.2, and 459 eV
can be assigned as Ti−C bond, Ti−X from substoichiometric TiCx (x
< 1) or titanium oxycarbides, Ti ions with reduced charge state
(TixOy), and Ti ions in valence 4+ (TiO2), respectively.
11,44,45 Obviously, as the hydrothermal reaction proceeds, the TiO2
increases while the other species decreased, indicating that Ti3C2
is consumed and transformed to (001)TiO2 nanosheets. The C 1s
spectrum of layered Ti3C2 is fitted by five components located at
281.7, 282.2, 284.8, 286.2, and 288.6 eV, corresponding to C−Ti,
C−Ti−Oa, C− C/C−H, C−O, and C−F bonds, respectively (Figure
3b).44
The C−Ti−Oa origins from the adsorbed −OH on the surfaces of Ti3C2.
Interestingly, a new peak emerges at 283.5 eV after
Figure 3. (a) Ti 2p, (b) C 1s, and (c) O 1s XPS spectra for Ti3C2
and (001)TiO2/Ti3C2 prepared for different reaction times. CHCl = 1
M, CNaBF4 = 0.1 M, T = 160 °C.
Figure 4. (a) DRS and (b) plots of [F(R∞)hv] 1/2 vs photon energy
of (001)TiO2/Ti3C2 prepared for different reaction times. CHCl = 1
M, CNaBF4 =
0.1 M, T = 160 °C.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
the hydrothermal oxidation, which could be attributed to the
C−Ti−Ob bonding at the interfaces of TiO2−Ti3C2 hetero- junctions.
This component reaches a maximum at 12 h, indicating the maximized
number of heterojunctions at the appropriate oxidation extent. With
respect to the O 1s XPS spectra, four peaks at 529.4, 530.4, 531.8,
and 533.3 eV have been deconvoluted (Figure 3c), which are ascribed
to surface adsorbed O species,46 Ti−O−Ti (lattice O),47 Ti−OH,47
and C−OH species,47 respectively. The Ti−OH species at 531.8 eV
unambiguously demonstrate the presence of −OH groups on the surface
of Ti3C2. The optical absorption property of the
(001)TiO2/Ti3C2
hybrids was characterized by UV−vis DRS (Figure 4a). The hybrids of
(001)TiO2/Ti3C2 synthesized for 4 to 16 h exhibit a broad
absorption. The light absorption above 400 nm reduces with the
increasing reaction time, namely the higher content of TiO2. It
could be attributed to the distinct adsorption of carbonaceous
materials.48 The band gap energies of two
representative (001)TiO2/Ti3C2 samples, for 12 and 14 h, were
determined through the [F(R∞)hv]
1/2 vs photon energy plots (Figure 4b),40 as 1.60 and 2.87 eV,
respectively. This result indicates that the band gap widens with
increasing the hydrothermal reaction time and the content of
(001)TiO2. The band gaps of (001)TiO2/Ti3C2 are narrower compared
with TiO2 nanosheets with dominant (001) facets (3.22 eV),40
due to the existence of metallic Ti3C2. 22,25 The narrow band
gap of (001)TiO2/Ti3C2 hybrids may favor optical absorption and
photocatalytic reactions. The photocatalytic activity of the
(001)TiO2/Ti3C2 hetero-
junction was evaluated by a probe reaction of MO dye elimination
under ultraviolet irradiation. As shown in Figure 5a, the
degradation rate of MO is maximized at the hydrothermal temperature
of 160 °C. This could be explained by the increasing formation rate
of TiO2 nanosheets at higher temperatures, which causes the
increasing number of heterojunctions at lower temperatures, while a
reduction of
Figure 5. (a) The photocatalytic degradation of MO over
(001)TiO2/Ti3C2 prepared at different hydrothermal temperatures.
The inset of (a) shows the photocatalytic degradation rate
constants of (001)TiO2/Ti3C2 prepared at different hydrothermal
temperatures. (b) The photocatalytic degradation rate constant (k)
of (001)TiO2/Ti3C2 and particulate TiO2/Ti3C2 (p-TiO2/Ti3C2)
prepared for different hydrothermal times. The photocatalytic
degradation rate constants are normalized by mass of TiO2 (k′) and
compared with Degussa P25.
Figure 6. (a) The transient photocurrent of (001)TiO2/Ti3C2
prepared for different hydrothermal times. (b) The partial
photocurrent decay of curve (a). (c) Transient open-circuit voltage
decay (OCVD) over Degussa P25 TiO2 and the (001) TiO2/Ti3C2
prepared for different reaction times. (d) Average electron
lifetimes (τn) of Degussa P25 TiO2 and the (001)TiO2/Ti3C2 reacted
for 4 h, 12 h, and 24 h.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
heterojunctions at higher temperatures is seen because of the
depletion of Ti3C2 (Figure S4). Analogously, the activity is
maximized at hydrothermal treatment for 12 h for a similar reason
(Figure 5b). The superior activity of TiO2 exposing {001} surfaces
to conventional particulate TiO2 is shown in Figure 5b (see Figures
S8 and S9 for more details of p-TiO2/ Ti3C2). The two materials
have the highest activities at hydrothermal reaction for 12 and 30
h, respectively. The (001)TiO2/Ti3C2 shows about 2.3-fold higher
degradation rate constant than p-TiO2/Ti3C2 at their respective
maximums, demonstrating the enhanced activity of {001} TiO2, and
this agrees with our previous study on the high-activity facets of
TiO2.
43 The excellent activity of hybrids can be further demonstrated by
the rate constant normalized by the mass of TiO2 (k′), which can be
determined through the elemental analysis by EPMA (see Tables S1
and S2 in the Supporting Information for details). As seen in
Figure 5b, the maximum k′ value of (001)TiO2/Ti3C2, 18.8 min−1 g−1,
exceeds that of Degussa P25 TiO2, 15.7 min−1 g−1. In addition, the
k′ values of (001)TiO2/Ti3C2 are also higher than that of pure TiO2
with exposed {001} and {101} facets reported in our previous work
obtained under similar conditions (1.86 min−1 gTiO2
−1),43
confirming that the 2D Ti3C2 can improve the photocatalytic
property of TiO2. Figure 6a shows the photocurrent test of the
samples
synthesized at 160 °C for different times under ultraviolet light
irradiation (<400 nm, 100 mW/cm2) by electrodepositing the
catalysts on a FTO (fluorine doped tin oxide) substrate (see Figure
S11 for the photoelectrochemical tests of samples at different
reaction temperatures). The photocurrent shows a similar tendency
with the MO degradation test. The (001)TiO2/Ti3C2 sample for 12 h
of hydrothermal oxidation has the highest photocurrent, even
comparable with that of Degussa P25 TiO2 (Figure S12), because of
the good compromise between the content of active TiO2 and the
number of (001)TiO2/Ti3C2 heterojunctions (see Table S2). It should
be noted that the photocurrent decays are very different among the
heterojunctions with different hydrothermal durations, suggesting
the different separation and recombina- tion of photogenerated
electron−hole pairs.49,50 As shown in Figure 6b, the samples for 4,
8, and 12 h display much slower photocurrent decays featured by the
long tails, while the samples for 16, 24, and 32 h display rapid
decay as the irradiation was turned off . The slow reversible
photoresponse is indicative of long charge carrier lifetimes and
metastable donor states,51,52 which have been observed in a variety
of elaborate heterojunction structures, e.g. tunable
bulk/surface
defects of TiO2, 49,51 Ti3+ doped TiO2,
52 TiO2/CNTs, 53 TiO2/
GR,54 and TiO2−Pd@Pt hybrid structures.55
= * −
=
0 (1)
where q is the unsigned charge of an electron (1.6 × 10−19 C), kB
is the Boltzmann constant (1.38 × 10−23 J/K), T is the temperature
in K of the three-electrode system, and n and n0 are the
photocarrier density in the semiconductor nanostruc- ture under
nonequilibrium state and equilibrium state, respectively.18,56−58
The temporal profiles of VOC of three representative samples were
monitored in the three-electrode system under UV (λ < 400 nm)
light to examine the dynamics of electrons within the TiO2 CB. As
shown in Figure 6c, the steady photovoltages of the (001)TiO2/Ti3C2
samples for different hydrothermal durations are in the same order
with the transient photocurrent, i.e. 12 h > 24 h > 4 h.
After turning off the light, the (001)TiO2/Ti3C2 samples at
hydrothermal durations for 4 and 12 h exhibit extended VOC
transient lasting more than 500 s, indicating the slow
recombination of electrons and holes and prolonged charge carrier
lifetime. While increasing the hydrothermal reaction to 24 h, it
was observed that the photovoltage was promptly established and
faded back to the equilibrium value in the dark, as the irradiation
was turned on/off. This behavior can be rationalized by the reduced
number of Ti3C2/TiO2 heterojunctions, as afore-described. The
average electron lifetime (τn) can be quantitatively
calculated through the VOC decay by the equation:18,56−58
τ = − −
(2)
where τn represents the average electron lifetime and Voc is the
open-circuit voltage at time t.18,56−58 As shown in Figure 6d, the
electron lifetime in TiO2 CB is in the range from 100 s to 104 s.
The (001)TiO2/Ti3C2 for 4 h hydrothermal oxidation shows the
longest short-lived distribution of τn at ca. 100 s, which appeared
at the moment lighting was turned off. The short-lived τn decreases
with the hydrothermal reaction
Figure 7. (a) The effects of scavengers on the degradation of MO
with (001)TiO2/Ti3C2-160 °C-12h under UV light irradiation. (b) The
recycling test of (001)TiO2/Ti3C2-160 °C-12h for the degradation of
MO under UV light irradiation.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
duration to ca. 50 and 2 s for the samples at 12 and 24 h,
respectively. It is widely accepted that the relatively short-lived
distribution of τn is an important signal of the rapid
recombination of photoexcited electrons and holes.18,55−58
The almost 2 orders of magnitude change of electron lifetime
strongly suggests that the recombination rate can be significantly
reduced by forming heterojunctions between TiO2 nanosheets and
layered Ti3C2. Additionally, it should be noted that the
(001)TiO2/Ti3C2 for 4 and 12 h display slower OCVD and longer
electron lifetimes than Degussa P25 TiO2, as shown in Figure 6c,d,
suggesting the improved charge separation over the hybrids of
(001)TiO2 and 2D Ti3C2. To understand the photocatalytic mechanism
of (001)TiO2/
Ti3C2, the effects of reactive oxygen species (ROS), including •OH
and •O2
−, and h+ were investigated by introducing isopropanol (IPA),
ammonium oxalate (AO), and benzoqui- none (BQ) as the scavengers,
respectively.59,60 As shown in Figure 7a, the degradation
efficiency significantly decreases with N2 bubbling, indicating
that the degradation of MO is a photocatalytic oxidation (PCO)
process. Three scavengers can quench the reaction in the order: IPA
> AO > BQ, indicating that the ROS contributes more than h+
in the MO degradation. According to these results, it can be
concluded that •OH is the most important reactive species in the
TiO2-catalyzed PCO process of MO, being consistent with Hirakawa T.
et al.61
The stability and reusability of (001)TiO2/Ti3C2 hybrid
photocatalyst were tested to degrade MO for four runs under UV
light (Figure 7b). The photocatalytic activity of
(001)TiO2/Ti3C2-160 °C-12h for MO degradation was well maintained
after 4 runs with 4.9% decrease of MO degradation from 97.4% to
92.5%, suggesting that (001)TiO2/Ti3C2 hybrids can be used as a
stable catalyst for the photodegradation process. On the basis of
the above experimental results, a possible
photocatalytic mechanism for the degradation reaction with
(001)TiO2/Ti3C2 was proposed. As Scheme 2a shows, the −OH
terminated Ti3C2 sheets are considered metallic because of its very
narrow band gap and high carrier mobility.22,25
Under ultraviolet irradiation, the exposed {001} facets of TiO2 are
excited to produce electrons (e−) and holes (h+). The transfer of
electrons is forbidden at the interfaces between TiO2 {001}
surfaces and Ti3C2, because of the more negative Fermi level of
Ti3C2 than the CB of TiO2.
37 The −OH terminated Ti3C2 sheets have recently been discovered as
an ultralow work function material with a work function ca. 1.8 eV
by theoretical calculations.62 This work function is much lower
than that of TiO2 (4.924 eV for (001) surface, 6.578 eV for
(101)
surface).16 From the viewpoint of work function, a Schottky barrier
may be established through their interfaces. Because the work
function of Ti3C2−OH is lower than that of the TiO2(001) surface,
the photogenerated holes, instead of electrons, could be injected
from TiO2 to Ti3C2−OH. The 2D structure and high mobility of the
hole make Ti3C2−OH a huge reservoir of holes. The Schottky barrier
at Ti3C2−TiO2 interfaces could effectively prevent the holes from
flowing back to TiO2 (Scheme 2b); thereby, a spatial separation of
photogenerated electron−hole pairs is achieved, as revealed by the
substantially prolonged electron lifetimes. In this interpretation,
the enriched electrons on TiO2(001) may react with the dissolved
oxygen to yield superoxide radical anions (•O2
−), which further react with H+ and e− to generate highly reactive
hydroxyl radicals (•OH).
4. CONCLUSIONS In summary, we have achieved the synergetic
utilization of Schottky-junction trapping holes and active facets
exposed to enhance the photocatalytic performance by fabricating an
atomic scale interfacial heterojunction composed of (001) TiO2
nanosheets inserted in the layered Ti3C2. The heterostructure was
synthesized by a hydrothermal oxidation of layered Ti3C2 assisted
by NaBF4. Ti3C2 not only afforded the Ti source of the
heterojunction; more importantly, it also form a Schottky- junction
with the {001} surfaces of n-type semiconductor TiO2. Under UV
irradiation, the ultralow-work-function −OH terminated Ti3C2 acts
as a reservoir of holes through the hole trapping by the
Schottky-junction, whereby the spatial separation of photogenerated
electrons and holes was achieved. The (001) TiO2−Ti3C2 hybrid
simultaneously overcomes the problems of fast recombination of
photogenerated electrons and holes, and the utilization of the
highly active {001} facets of TiO2, therefore, enabled the
significantly improved photo- catalytic degradation of MO. This
work opens a new window exploiting the MXenes for high-performance
photocatalysts.
ASSOCIATED CONTENT *S Supporting Information The Supporting
Information is available free of charge on the ACS Publications
website at DOI: 10.1021/acsami.5b11973.
More experimental results on the effects of NaBF4 concentration,
temperature, and reduction duration on the synthesis of
(001)TiO2/Ti3C2; characterizations of p- TiO2/Ti3C2; method
determining the content of TiO2 in heterojunction samples;
photocatalytic degradation
Scheme 2. (a) The charge-transfer process over (001)TiO2/Ti3C2. (b)
Schematic band alignments and charge flows at {001} TiO2−Ti3C2
interfaces
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
AUTHOR INFORMATION
ACKNOWLEDGMENTS
This work was financially supported by the National Natural Science
Foundation of China (No. 21273079), the Guangdong Provincial
Natural Science Foundation (Nos. S20120011275, 2014A030312007),
Program for New Century Excellent Talents in University
(NCET-12-0190), and the Fundamental Research Funds for the Central
Universities of China (No. 2015PT012). We also acknowledge the
high-performance computing support by the Information and Network
Engineer- ing and Research Center, SCUT.
REFERENCES (1) Zhang, H.; Lv, X.; Li, Y.; Wang, Y.; Li, J.
P25-Graphene Composite as a High Performance Photocatalyst. ACS
Nano 2010, 4, 380−386. (2) Xiang, Q.; Yu, J.; Jaroniec, M.
Synergetic Effect of MoS2 and Graphene as Cocatalysts for Enhanced
Photocatalytic H2 Production Activity of TiO2 Nanoparticles. J. Am.
Chem. Soc. 2012, 134, 6575− 6578. (3) Ryu, J.; Lee, S. H.; Nam, D.
H.; Park, C. B. Rational Design and Engineering of
Quantum-Dot-Sensitized TiO2 Nanotube Arrays for Artificial
Photosynthesis. Adv. Mater. 2011, 23, 1883−1888. (4) Subramanian,
V.; Wolf, E. E.; Kamat, P. V. Catalysis with TiO2/ Gold
Nanocomposites. Effect of Metal Particle Size on the Fermi Level
Equilibration. J. Am. Chem. Soc. 2004, 126, 4943−4950. (5) Baker,
D. R.; Kamat, P. V. Photosensitization of TiO2 Nanostructures with
CdS Quantum Dots: Particulate versus Tubular Support Architectures.
Adv. Funct. Mater. 2009, 19, 805−811. (6) Seh, Z. W.; Liu, S.; Low,
M.; Zhang, S. Y.; Liu, Z.; Mlayah, A.; Han, M. Y. Janus Au-TiO2
Photocatalysts with Strong Localization of Plasmonic Near-Fields
for Efficient Visible-Light Hydrogen Gener- ation. Adv. Mater.
2012, 24, 2310−2314. (7) Marschall, R. Semiconductor Composites:
Strategies for Enhancing Charge Carrier Separation to Improve
Photocatalytic Activity. Adv. Funct. Mater. 2014, 24, 2421−2440.
(8) Li, H.; Zhou, Y.; Tu, W.; Ye, J.; Zou, Z. State-of-the-Art
Progress in Diverse Heterostructured Photocatalysts toward
Promoting Photo- catalytic Performance. Adv. Funct. Mater. 2015,
25, 998−1013. (9) Leary, R.; Westwood, A. Carbonaceous
Nanomaterials for the Enhancement of TiO2 Photocatalysis. Carbon
2011, 49, 741−772. (10) Tan, L. L.; Chai, S. P.; Mohamed, A. R.
Synthesis and Applications of Graphene-Based TiO2 Photocatalysts.
ChemSusChem 2012, 5, 1868−1882. (11) Yang, H. G.; Sun, C. H.; Qiao,
S. Z.; Zou, J.; Liu, G.; Smith, S. C.; Cheng, H. M.; Lu, G. Q.
Anatase TiO2 Single Crystals with a Large Percentage of Reactive
Facets. Nature 2008, 453, 638−641. (12) Yang, X. H.; Yang, H. G.;
Li, C. Controllable Nanocarving of Anatase TiO2 Single Crystals
with Reactive {001} Facets. Chem. - Eur. J. 2011, 17, 6615−6619.
(13) Yang, X. H.; Li, Z.; Sun, C.; Yang, H. G.; Li, C. Hydrothermal
Stability of {001} Faceted Anatase TiO2. Chem. Mater. 2011, 23,
3486−3494.
(14) Kuo, C. H.; Chen, C. H.; Huang, M. H. Seed-Mediated Synthesis
of Monodispersed Cu2O Nanocubes with Five Different Size Ranges
from 40 to 420 nm. Adv. Funct. Mater. 2007, 17, 3773−3780. (15)
D'Arienzo, M.; Carbajo, J.; Bahamonde, A.; Crippa, M.; Polizzi, S.;
Scotti, R.; Wahba, L.; Morazzoni, F. Photogenerated Defects in
Shape-Controlled TiO2 Anatase Nanocrystals: A Probe to Evaluate the
Role of Crystal Facets in Photocatalytic Processes. J. Am. Chem.
Soc. 2011, 133, 17652−17661. (16) Zhao, Z.; Li, Z.; Zou, Z. Surface
Properties and Electronic Structure of Low-Index Stoichiometric
Anatase TiO2 Surfaces. J. Phys.: Condens. Matter 2010, 22, 175008.
(17) Linsebigler, A. L.; Lu, G.; Yates, J. T. Photocatalysis on
TiO2
Surfaces: Principles, Mechanisms, and Selected Results. Chem. Rev.
1995, 95, 735−758. (18) Bai, S.; Jiang, J.; Zhang, Q.; Xiong, Y.
Steering Charge Kinetics in Photocatalysis: Intersection of
Materials Syntheses, Characterization Techniques and Theoretical
Simulations. Chem. Soc. Rev. 2015, 44, 2893−2939. (19) Wang, W.-S.;
Wang, D.-H.; Qu, W.-G.; Lu, L.-Q.; Xu, A.-W. Large Ultrathin
Anatase TiO2 Nanosheets with Exposed {001} Facets on Graphene for
Enhanced Visible Light Photocatalytic Activity. J. Phys. Chem. C
2012, 116, 19893−19901. (20) Gu, L.; Wang, J.; Cheng, H.; Zhao, Y.;
Liu, L.; Han, X. One-Step Preparation of Graphene-Supported Anatase
TiO2 with Exposed {001} Facets and Mechanism of Enhanced
Photocatalytic Properties. ACS Appl. Mater. Interfaces 2013, 5,
3085−93. (21) Yuan, Y.-J.; Ye, Z.-J.; Lu, H.-W.; Hu, B.; Li, Y.-H.;
Chen, D.-Q.; Zhong, J.-S.; Yu, Z.-T.; Zou, Z.-G. Constructing
Anatase TiO2
Nanosheets with Exposed (001) Facets/Layered MoS2 Two-Dimen- sional
Nanojunctions for Enhanced Solar Hydrogen Generation. ACS Catal.
2016, 6, 532−541. (22) Naguib, M.; Kurtoglu, M.; Presser, V.; Lu,
J.; Niu, J.; Heon, M.; Hultman, L.; Gogotsi, Y.; Barsoum, M. W.
Two-Dimensional Nanocrystals Produced by Exfoliation of Ti3AlC2.
Adv. Mater. 2011, 23, 4248−4253. (23) Naguib, M.; Mochalin, V. N.;
Barsoum, M. W.; Gogotsi, Y. MXenes: A New Family of Two-Dimensional
Materials. Adv. Mater. 2014, 26, 992−1005. (24) Naguib, M.;
Gogotsi, Y. Synthesis of Two-Dimensional Materials by Selective
Extraction. Acc. Chem. Res. 2015, 48, 128−135. (25) Tang, Q.; Zhou,
Z.; Shen, P. Are MXenes Promising Anode Materials for Li Ion
Batteries? Computational Studies on Electronic Properties and Li
Storage Capability of Ti3C2 and Ti3C2X2 (X = F, OH) Monolayer. J.
Am. Chem. Soc. 2012, 134, 16909−16916. (26) Sun, D.; Wang, M.; Li,
Z.; Fan, G.; Fan, L.-Z.; Zhou, A. Two- Dimensional Ti3C2 as Anode
Material for Li-Ion Batteries. Electrochem. Commun. 2014, 47,
80−83. (27) Liang, X.; Garsuch, A.; Nazar, L. F. Sulfur Cathodes
Based on Conductive MXene Nanosheets for High-Performance
Lithium-Sulfur Batteries. Angew. Chem., Int. Ed. 2015, 54,
3907−3911. (28) Zhao, X.; Liu, M.; Chen, Y.; Hou, B.; Zhang, N.;
Chen, B.; Yang, N.; Chen, K.; Li, J.; An, L. Fabrication of Layered
Ti3C2 with an Accordion-Like Structure as a Potential Cathode
Material for High Performance Lithium−Sulfur Batteries. J. Mater.
Chem. A 2015, 3, 7870−7876. (29) Lukatskaya, M. R.; Mashtalir, O.;
Ren, C. E.; Dall'Agnese, Y.; Rozier, P.; Taberna, P. L.; Naguib,
M.; Simon, P.; Barsoum, M. W.; Gogotsi, Y. Cation Intercalation and
High Volumetric Capacitance of Two-Dimensional Titanium Carbide.
Science 2013, 341, 1502−1505. (30) Ghidiu, M.; Lukatskaya, M. R.;
Zhao, M. Q.; Gogotsi, Y.; Barsoum, M. W. Conductive Two-Dimensional
Titanium Carbide ’Clay’ with High Volumetric Capacitance. Nature
2014, 516, 78−81. (31) Ling, Z.; Ren, C. E.; Zhao, M. Q.; Yang, J.;
Giammarco, J. M.; Qiu, J.; Barsoum, M. W.; Gogotsi, Y. Flexible and
Conductive MXene Films and Nanocomposites with High Capacitance.
Proc. Natl. Acad. Sci. U. S. A. 2014, 111, 16676−16681. (32) Peng,
Q.; Guo, J.; Zhang, Q.; Xiang, J.; Liu, B.; Zhou, A.; Liu, R.;
Tian, Y. Unique Lead Adsorption Behavior of Activated
Hydroxyl
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060
Group in Two-Dimensional Titanium Carbide. J. Am. Chem. Soc. 2014,
136, 4113−4116. (33) Mashtalir, O.; Cook, K. M.; Mochalin, V. N.;
Crowe, M.; Barsoum, M. W.; Gogotsi, Y. Dye Adsorption and
Decomposition on Two-Dimensional Titanium Carbide in Aqueous Media.
J. Mater. Chem. A 2014, 2, 14334−14338. (34) Ying, Y.; Liu, Y.;
Wang, X.; Mao, Y.; Cao, W.; Hu, P.; Peng, X. Two-Dimensional
Titanium Carbide for Efficiently Reductive Removal of Highly Toxic
Chromium(VI) from Water. ACS Appl. Mater. Interfaces 2015, 7,
1795−1803. (35) Xie, X.; Chen, S.; Ding, W.; Nie, Y.; Wei, Z. An
Extraordinarily Stable Catalyst: Pt NPs Supported on
Two-Dimensional Ti3C2X2 (X = OH, F) Nanosheets for Oxygen Reduction
Reaction. Chem. Commun. 2013, 49, 10112−10114. (36) Li, X.; Fan,
G.; Zeng, C. Synthesis of Ruthenium Nanoparticles Deposited on
Graphene-Like Transition Metal Carbide as an Effective Catalyst for
the Hydrolysis of Sodium Borohydride. Int. J. Hydrogen Energy 2014,
39, 14927−14934. (37) Zhang, X.; Zhao, X.; Wu, D.; Jing, Y.; Zhou,
Z. High and Anisotropic Carrier Mobility in Experimentally Possible
Ti2CO2 (MXene) Monolayer and Nanoribbons. Nanoscale 2015, 7, 16020−
16025. (38) Naguib, M.; Mashtalir, O.; Lukatskaya, M. R.; Dyatkin,
B.; Zhang, C.; Presser, V.; Gogotsi, Y.; Barsoum, M. W. One-Step
Synthesis of Nanocrystalline Transition Metal Oxides on Thin Sheets
of Disordered Graphitic Carbon by Oxidation of MXenes. Chem.
Commun. 2014, 50, 7420−7423. (39) Gao, Y.; Wang, L.; Zhou, A.; Li,
Z.; Chen, J.; Bala, H.; Hu, Q.; Cao, X. Hydrothermal Synthesis of
TiO2/Ti3C2 Nanocomposites with Enhanced Photocatalytic Activity.
Mater. Lett. 2015, 150, 62−64. (40) Zhang, J.; Xi, J.; Ji, Z. Mo +
N Codoped TiO2 Sheets with Dominant {001} Facets for Enhancing
Visible-Light Photocatalytic Activity. J. Mater. Chem. 2012, 22,
17700. (41) Zhou, X.; Peng, F.; Wang, H.; Yu, H.; Fang, Y. A Simple
Preparation of Nitrogen Doped Titanium Dioxide Nanocrystals with
Exposed (001) Facets with High Visible Light Activity. Chem.
Commun. 2012, 48, 600−2. (42) Yang, X.; Zhuang, J.; Li, X.; Chen,
D.; Ouyang, G.; Mao, Z.; Han, Y.; He, Z.; Liang, C.; Wu, M.; Yu, J.
C. Hierarchically Nanostructured Rutile Arrays: Acid Vapor
Oxidation Growth and Tunable Morphologies. ACS Nano 2009, 3,
1212−1218. (43) Lai, Z.; Peng, F.; Wang, Y.; Wang, H.; Yu, H.; Liu,
P.; Zhao, H. Low Temperature Solvothermal Synthesis of Anatase TiO2
Single Crystals with Wholly {100} and {001} Faceted Surfaces. J.
Mater. Chem. 2012, 22, 23906−23912. (44) Rakhi, R. B.; Ahmed, B.;
Hedhili, M. N.; Anjum, D. H.; Alshareef, H. N. Effect of Postetch
Annealing Gas Composition on the Structural and Electrochemical
Properties of Ti2CTx MXene Electro- des for Supercapacitor
Applications. Chem. Mater. 2015, 27, 5314− 5323. (45) Dang, B. H.
Q.; Rahman, M.; MacElroy, D.; Dowling, D. P. Evaluation of
Microwave Plasma Oxidation Treatments for the Fabrication of
Photoactive Un-Doped and Carbon-Doped TiO2
Coatings. Surf. Coat. Technol. 2012, 206, 4113−4118. (46) Chen, L.;
He, B.-Y.; He, S.; Wang, T.-J.; Su, C.-L.; Jin, Y. Fe-Ti Oxide
Nano-Adsorbent Synthesized by Co-Precipitation for Fluoride Removal
From Drinking Water and its Adsorption Mechanism. Powder Technol.
2012, 227, 3−8. (47) Li, B.; Zhao, Z.; Gao, F.; Wang, X.; Qiu, J.
Mesoporous Microspheres Composed of Carbon-Coated TiO2 Nanocrystals
with Exposed {001} Facets for Improved Visible Light Photocatalytic
Activity. Appl. Catal., B 2014, 147, 958−964. (48) Shi, H.; Chen,
J.; Li, G.; Nie, X.; Zhao, H.; Wong, P. K.; An, T. Synthesis and
Characterization of Novel Plasmonic Ag/AgX-CNTs (X= Cl, Br, I)
Nanocomposite Photocatalysts and Synergetic Degradation of Organic
Pollutant under Visible Light. ACS Appl. Mater. Interfaces 2013, 5,
6959−67. (49) Kong, M.; Li, Y.; Chen, X.; Tian, T.; Fang, P.;
Zheng, F.; Zhao, X. Tuning the Relative Concentration Ratio of Bulk
Defects to Surface
Defects in TiO2 Nanocrystals Leads to High Photocatalytic
Efficiency. J. Am. Chem. Soc. 2011, 133, 16414−16417. (50) Yu, J.;
Dai, G.; Huang, B. Fabrication and Characterization of
Visible-Light-Driven Plasmonic Photocatalyst Ag/AgCl/TiO2 Nano-
tube Arrays. J. Phys. Chem. C 2009, 113, 16394−16401. (51) Zhuang,
J.; Weng, S.; Dai, W.; Liu, P.; Liu, Q. Effects of Interface
Defects on Charge Transfer and Photoinduced Properties of TiO2
Bilayer Films. J. Phys. Chem. C 2012, 116, 25354−25361. (52) Xin,
X.; Xu, T.; Yin, J.; Wang, L.; Wang, C. Management on the Location
and Concentration of Ti
3+ in Anatase TiO2 for Defects- Induced Visible-Light
Photocatalysis. Appl. Catal., B 2015, 176−177, 354−362. (53) Yu,
H.; Quan, X.; Chen, S.; Zhao, H. TiO2-Multiwalled Carbon Nanotube
Heterojunction Arrays and Their Charge Separation Capability. J.
Phys. Chem. C 2007, 111, 12987−12991. (54) Lee, J. S.; You, K. H.;
Park, C. B. Highly Photoactive, Low Bandgap TiO2 Nanoparticles
Wrapped by Graphene. Adv. Mater. 2012, 24, 1084−1088. (55) Bai, S.;
Yang, L.; Wang, C.; Lin, Y.; Lu, J.; Jiang, J.; Xiong, Y. Boosting
Photocatalytic Water Splitting: Interfacial Charge Polar- ization
in Atomically Controlled Core-Shell Cocatalysts. Angew. Chem., Int.
Ed. 2015, 54, 14810−14814. (56) Zaban, A.; Greenshtein, M.;
Bisquert, J. Determination of the Electron Lifetime in
Nanocrystalline Dye Solar Cells by Open-Circuit Voltage Decay
Measurements. ChemPhysChem 2003, 4, 859−864. (57) Meekins, B. H.;
Kamat, P. V. Got TiO2 Nanotubes? Lithium Ion Intercalation Can
Boost Their Photoelectrochemical Performance. ACS Nano 2009, 3,
3437−3446. (58) DuChene, J. S.; Sweeny, B. C.; Johnston-Peck, A.
C.; Su, D.; Stach, E. A.; Wei, W. D. Prolonged Hot Electron
Dynamics in Plasmonic-Metal/Semiconductor Heterostructures with
Implications for Solar Photocatalysis. Angew. Chem., Int. Ed. 2014,
53, 7887−7891. (59) Yi, J.; Huang, L.; Wang, H.; Yu, H.; Peng, F.
AgI/TiO2 Nanobelts Monolithic Catalyst with Enhanced Visible Light
Photo- catalytic Activity. J. Hazard. Mater. 2015, 284, 207−214.
(60) Chen, Z.; Wang, W.; Zhang, Z.; Fang, X. High-Efficiency
Visible-Light-Driven Ag3PO4/AgI Photocatalysts: Z-Scheme Photo-
catalytic Mechanism for Their Enhanced Photocatalytic Activity. J.
Phys. Chem. C 2013, 117, 19346−19352. (61) Hirakawa, T.; Nosaka,
Y.; Hirakawa, T.; Nosaka, Y. Properties of •O2
−and •OH Formed in TiO2 Aqueous Suspensions by Photo- catalytic
Reaction and the Influence of H2O2 and Some Ions. Langmuir 2002,
18, 3247−3254. (62) Khazaei, M.; Arai, M.; Sasaki, T.; Ranjbar, A.;
Liang, Y.; Yunoki, S. OH-Terminated Two-Dimensional Transition
Metal Carbides and Nitrides as Ultralow Work Function Materials.
Phys. Rev. B: Condens. Matter Mater. Phys. 2015, 92, 075411.
ACS Applied Materials & Interfaces Research Article
DOI: 10.1021/acsami.5b11973 ACS Appl. Mater. Interfaces 2016, 8,
6051−6060