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Black Titania for Superior Photocatalytic Hydrogen Production and Photoelectrochemical Water Splitting Guilian Zhu,[a] Hao Yin,[a] Chongyin Yang,[a] Houlei Cui,[a] Zhou Wang,[a] Jijian Xu,[a, c] Tianquan Lin,*[a] and Fuqiang Huang*[a, b] Introduction Photocatalytic water splitting has attracted enormous attention in recent decades for low-cost, environmentally friendly solar- hydrogen production to support the future hydrogen econo- my.[1] As perhaps the most important material in photocataly- sis, TiO2 is the most attractive d-block transition metal func- tional oxide for photocatalysis.[2] However, the light absorption ratio and solar-to-hydrogen energy conversion efficiency is too low for the technology to be economically sound. The main barriers are the rapid recombination of photogenerated elec- tron–hole pairs as well as the backward reaction and the poor activation of TiO2 by visible light. Recently, some hydrogena- tion methods were demonstrated to enable efficient visible- light absorption, which result in the formation of black TiO2 and improved photocatalytic activity.[3] The improved solar ab- sorption attributed to additional intermediate electronic states induced by hydrogen insertion into the lattice of TiO2. [3a] If we consider the danger and difficulty to control a typical hydroge- nation process (high temperature, high pressure, pure hydro- gen, etc.), an alternative facile and effective method should be developed.[4] Most previous studies have explored applications in photocatalytic degradation,[3a–d, 5] and some materials exhibit significantly worse photocatalytic activity because of their pro- pensity to form bulk vacancy defects.[6] The photocatalytic ac- tivities of black TiO2 reported previously are highly controver- sial, especially in water decontamination. Herein, we demonstrate a facile CaH2 reduction method to synthesize uniform black TiO2 with improved photocatalytic water decontamination and water-splitting performances at low temperatures. The reducing agent, CaH2, has been used to reduce TiO2-based materials to obtain TiAl alloy or Ti2O3. [7] It is active at considerably lower temperatures than that required by conventional techniques. A reduction of transition metal oxides by metal hydride at low temperatures has become more useful to generate oxygen deficiencies than that ach- ieved by standard methods.[8] CaH2 decomposes and releases highly active hydrogen atoms at a low temperature. The re- duced nanoparticles have crystalline-core/amorphous-shell structures and exhibit a 2.4 times higher efficiency in photoca- talytic water decontamination and a 4.5 times higher H2 pro- duction rate in photoelectrochemical (PEC) water splitting than commercial P25 TiO2. Results and Discussion The morphologies of reduced TiO2 were verified by TEM. The pristine TiO2 nanocrystals are highly crystallized as illustrated by the well-resolved lattice features shown in the high-resolu- To utilize visible-light solar energy to meet environmental and energy crises, black TiO2 as a photocatalyst is an excellent solu- tion to clean polluted air and water and to produce H2. Herein, black TiO2 with a crystalline core–amorphous shell structure re- duced easily by CaH2 at 400 8C is demonstrated to harvest over 80 % solar absorption, whereas white TiO2 harvests only 7 %, and possesses superior photocatalytic performances in the degradation of organics and H2 production. Its water decon- tamination is 2.4 times faster and its H2 production was 1.7 times higher than that of pristine TiO2. Photoelectrochemi- cal measurements reveal that the reduced samples exhibit greatly improved carrier densities, charge separation, and pho- tocurrent (a 4.5-fold increase) compared with the original TiO2. Consequently, this facile and versatile method could provide a promising and cost-effective approach to improve the visi- ble-light absorption and performance of TiO2 in photocatalysis. [a] G. Zhu,+ Dr. H. Yin,+ Dr. C. Yang, H. Cui, Dr. Z. Wang, J. Xu, Dr. T. Lin, Prof. Dr. F. Huang CAS Key Laboratory of Materials for Energy Conversion and State Key Laboratory of High Performance Ceramics and Superfine Microstructure Shanghai Institute of Ceramics, Chinese Academy of Sciences 1295 Dingxi Road, Shanghai, 200050 (P.R. China) E-mail : huangfq@mail.sic.ac.cn [b] Prof. Dr. F. Huang National Laboratory for Molecular Sciences and State Key Laboratory of Rare Earth Materials Chemistry and Applications College of Chemistry and Molecular Engineering Peking University Beijing 100871 (P.R. China) [c] J. Xu Key Laboratory of Silicon Materials School of Materials Science and Engineering Zhejiang University Hangzhou 310027 (P.R. China) [++] These authors contributed equally to this work. Supporting Information for this article is available on the WWW under http://dx.doi.org/10.1002/cctc.201500488. ChemCatChem 2015, 7, 2614 – 2619 Ó 2015 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim2614 Full PapersDOI: 10.1002/cctc.201500488 http://dx.doi.org/10.1002/cctc.201500488 tion transmission electron microscopy (HRTEM) image (Fig- ure S1). The lattice distances of pristine and reduced TiO2 are both 0.35 nm, which is typical for anatase (1 0 1). However, after CaH2 reduction, the titania nanocrystal (TiO2¢x) consist of a crystalline TiO2 as a core and a highly disordered surface layer (�2 nm thick) as shown in Figure 1 a. As the unique crystalline core–disordered shell structure was formed, the TiO2¢x samples were gray colored after reduction at 300 8C (denoted as T300) and black colored after reduction at 400 8C (denoted as T400). Diffusive reflectance and absorb- ance spectroscopy (Figure 1 b) reveal that the band gap of the unmodified pristine TiO2 nanocrystals was approximately 3.2 eV. After CaH2 reduction, the TiO2¢x samples exhibit signifi- cantly enhanced absorption of visible and near-infrared light. The absorption edge of black TiO2¢x near l= 406 nm is derived from the core of crystalline TiO2 that corresponds to �3.05 eV (Figure S2). We calculated the solar absorption ratios from the standard AM 1.5G solar spectrum and the absorption spectra of our samples (Table S1). The solar absorption of T400 is �81 % of the solar energy, much larger than that reported for black TiO2 (<30 %) [3a] and pristine TiO2 (�7 %).[9] The solar ab- sorption of black TiO2 reduced at 500 8C (T500) is further im- proved up to �90 % (Figure S3). These results demonstrate that the reduced samples capture much more sunlight than pristine P25 and a higher annealing temperature results in the higher absorption of sunlight. Interestingly, CaH2 can effectively reduce the rutile phase of Degussa P25 samples that are mixed anatase and rutile phases, which is confirmed by XRD. The ratio of the intensity of the rutile (11 0) peak and the anatase (1 0 1) peak, IR(110)/IA(101), decreases after CaH2 reduction (Figure 1 c). The ratios of the rutile phase in pristine P25, T300, and T400, calculated by a nor- malized RIR (Reference Intensity Ratio) method, are 15, 13, and 8 %, respectively. If the reduction temperature further increases to 500 8C, the reduced sample consists of anatase TiO2 and Magneli Ti4O7 without the rutile phase (Figure S4 a), which was confirmed by HRTEM. Two sets of lattice fringes with spacings of 0.28 and 0.37 nm are observed (Figure S4b), which corre- spond to the (0 2 2) and (0¢1 3) atomic planes, respectively, with an angle 89.48 for Magneli Ti4O7. Furthermore, there is no amorphous layer on the surface of the crystalline particle of T500. In other words, the samples maintain the mixed phase of anatase and rutile below 500 8C, although the ratio of rutile de- creases. However, if the reduction temperature reaches 500 8C, the sample becomes a mixture of anatase and Ti4O7, which means that Ti3++ appears as a result of the reduction. Black TiO2 with a similar crystalline core–amorphous shell structure has been synthesized by annealing TiO2 in H2 or by H-plasma enhanced chemical vapor deposition(CVD) previous- ly.[7c, 10] It was confirmed that the coloration and strong sunlight absorption result from the presence of amorphous layers. Ad- ditionally, the theoretical calculations and experimental studies reported previously indicate that Ti¢H bonds that exist in the amorphous layers could form the intermediate states in the band gap.[4c, 10] To realize the transformation of the surface chemical states during the CaH2 reduction process, X-ray pho- toelectron spectroscopy (XPS) was conducted. No impurities (such as Ca) are observed, except for the adventitious carbon contaminant. The XPS Ti 2p spec- tra of the three samples are shown in Figure 1 d. There are no Ti3++ signals observed on the surface of the T300 and T400 samples. This is similar to black TiO2 reduced by H2, which showed no detectable signal of Ti3++.[4a, b] Clearly, the coloration and strong sunlight absorption of the reduced samples are not attributed to the Ti3++ on the sur- face. EPR spectra were recorded to investigate the change of the crystal lattice structure. The three samples show different EPR signals (Figure 2 a). Pristine P25 does not show a distinct EPR signal. In contrast, the re- duced titania nanocrystals dis- play a single symmetrical signal with g = 2.003, which could be assigned to superoxide radicals (O2 ¢) attached to the oxygen va- cancies on the TiO2 surface. [11] It is well known that many oxygen vacancies are introduced by an- Figure 1. a) HRTEM images of T400 and b) UV/Vis absorption spectra, c) XRD patterns, and d) Ti 2p XPS spectra of P25, T300, and T400. The insets in (b) are the standard AM 1.5G solar spectrum (ASTM G173-03) and a photograph of the samples. ChemCatChem 2015, 7, 2614 – 2619 www.chemcatchem.org Ó 2015 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim2615 Full Papers http://www.chemcatchem.org nealing with ultra-high purity H2. [12] The EPR signal increases with elevated annealing temperature, which means that the oxygen vacancies become denser as the annealing tempera- ture increases. The superoxide radicals attached to the oxygen vacancies form Ti4++¢O2¢ species, which facilitate the oxidative processes and stabilize the separated e¢ and h++.[13] This sug- gests that T400 has more Ti4++¢O2¢ species and is more strong- ly oxidizing than T300. Raman scattering was explored to further examine the struc- tural properties of P25 and the reduced samples. All samples exhibit similar peaks of typical anatase TiO2 (Figure 2 b). The anatase structure is tetragonal and belongs to the space group of I41/amd. Its six active Raman transitions (1A1g, 2B1g, and 3Eg) lead to five peaks in the Raman spectra because the peaks of the Alg (n1) and B1g (n2) modes located at approximately ñ= 519 cm¢1 are not distinguishable at room temperature. The in- tensities and locations of the different Raman vibrational modes are summarized in Table S2. Clearly, the Eg (n6) peak lo- cated at ñ= 147 cm¢1 (Figure 2 b inset and Table S2) blueshifts to ñ= 148, 152, and 157 cm¢1 in T300, T400, and T500, respec- tively. The full width at half maximum intensity (FWHM) of the Eg (n6) peaks broaden from 12 to 13, 17, and 22 cm ¢1. As is well known, the blueshift and broadening of the Eg peak are either because of nano-sized grains (<10 nm) or the shorten- ing of the correlation length because of the presence of de- fects.[14] In this case, the size of the crystallites from TEM analy- sis are 20–30 nm, which rules out the occurrence of finite-size effects and indicates the formation of defects. It is easy to un- derstand that T500 possesses Ti3++ defects because of the pres- ence of Ti4O7. With regard to T300 and T400, the amorphous layers with an enormous number of oxygen vacancies lose lattice periodicity and break the octahedral symmetry of TiO6 to result in the blueshift and broadening in the Raman spec- tra. This is consistent with the conclusion drawn from the EPR investigation. The role of hydrogenation was examined by NMR spectroscopy (Figure 2 c). Both the reduced and pristine P25 show a large peak at d=++5.1 ppm, which corresponds to the main type of bridging proton.[15] The larger line width in reduced samples may be caused by the incorpora- tion of hydrogen atoms at bridg- ing sites produced in the amor- phous layer during the reduction process.[15, 16] Additionally, the stronger peak at d=++5.1 ppm suggests stronger hydrogen- bonded bridging hydroxyl groups in the reduced TiO2. In contrast to pristine P25, T300 and T400 show an additional sharp resonance at d = ++0.74 ppm on top of a broad base. This peak corresponds to dynamic exchange between 1H (fast motion) in different envi- ronments, which means rapid isotropic diffusion and rapid ex- change.[4c, 17] The rapid exchange may enhance the transport of photogenerated electrons, which reduces recombination in the nanocrystal. The measurement of photoluminescence (PL) emission was performed to understand the efficiency of charge carrier trap- ping, migration, transfer, and separation in the semiconductor as PL emission results from the recombination of free carri- ers.[18] A trend in the PL emission intensity is observed in the following order: P25>T300>T400, which indicates that the re- combination rate of photogenerated electrons and holes is suppressed in the reduced samples. The hydrogenation of TiO2 can improve their conductivity and carrier density,[19] which fa- cilitates the carrier transfer and separation and is the reason why the PL intensities of the reduced samples decrease drasti- cally. Generally, a low recombination rate of electrons and holes is a prerequisite for high photocatalytic activity. The photocatalytic activities of the reduced TiO2 were first evaluated by the decomposition of a standard model contami- nant methyl orange (MO) under simulated solar-light irradia- tion in an aqueous solution. The direct decomposition of MO in the absence of photocatalysts is not detected under light ir- radiation in a control experiment. The degradation curves of MO catalyzed by pristine and reduced TiO2 under simulated Figure 2. a) EPR spectra, b) Raman spectra, c) 1H NMR spectra and d) PL spectra of the reference P25 and the re- duced samples. The insets in (b) and (c) are partial magnifications of the region marked with a red border. ChemCatChem 2015, 7, 2614 – 2619 www.chemcatchem.org Ó 2015 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim2616 Full Papers http://www.chemcatchem.org solar-light irradiation are shown in Figure 3 a. For the T400 sample, the photodegradation is complete after 6 min. A trend in the photocatalytic activity was observed in the following order: T400>T300>P25, which is consistent with the trend of enhanced solar absorption. The photodegradation rate con- stants, calculated by a pseudo-first-order kinetics model, are 0.28, 0.33, and 0.68 min¢1 for P25, T300, and T400, respectively (Figure S5 a). Correspondingly, the rates of T300 and T400 are 1.2 and 2.4 times higher than that of P25, respectively. The visi- ble-light catalytic activity was further investigated to evaluate the visible-light photocatalysis of the reduced samples. T400 is demonstrated to deliver a greatly enhanced visible-light pho- tocatalytic performance compared with pristine P25; and T300 also shows an increased activity in MO degradation under visi- ble light (Figure S5 b). These results coincide well with the characterization. Compared with the photocatalytic activity of pristine TiO2, T500 demonstrates a slightly reduced activity be- cause of the absence of the amorphous layer and the exis- tence of the Ti4O7 phase (Figure S6 a). The photocatalytic activities of our samples were further evaluated by monitoring H2 evolution from water splitting (Fig- ure 3 b). The H2 generation of T300 (5.2 mmol h ¢1 g¢1) is 1.7 times higher than that of pristine TiO2 (3.0 mmol h ¢1 g¢1) and is in the group of the best semiconductors (5– 10 mmol h¢1 g¢1) for the photogeneration of H2. For the sample reducedat an increased reduction temperature of 500 8C (T500), the H2 generation decreases to nearly that of P25 be- cause of its poor crystallinity and the absence of the amor- phous layer (Figure S6 b). Clearly, low-temperature reduction by CaH2 is an efficient way to improve the photocatalytic per- formance of TiO2. T300 is the best catalyst for water splitting, whereas T400 is the best for the photocatalytic degradation of MO. H2 production is derived from the reducibility of the pho- togenerated electrons in the conduction band of black TiO2, whereas the degradation of MO is based on the oxidative effect of the photogenerated holes in the valence band. From our EPR spectroscopy results, it is clear that T400 has more Ti4++¢O2¢ species, which facilitate the trapping of holes for oxi- dation reactions on the surface. Combined with its better sun- light absorption and low recombination, T400 presents a higher efficiency in photocata- lytic degradation than T300 and P25. However, the formation of molecular H2 and H2O are com- petitive on the TiO2 surface. [20] H2 production on T400 is less effi- cient than H2O production as O2 ¢ on the surface can react with H++ to form H2O. H2 produc- tion is the result of a compromise between the amount of O2 ¢ spe- cies and photogenerated elec- trons, which is why T300 is better than T400 and P25 for H2 production. The excellent photocatalytic activities of the CaH2-reduced samples were further demonstrated by H2 generation by using a PEC cell (Figure 4). To investigate the PEC properties, the pris- tine and reduced TiO2 films were prepared by a spin-coating method. The photocurrents of these films were recorded in the dark and under illumination from a Xe lamp. The potential was swept linearly at a scan rate of 10 mV s¢1 between ¢1.3 and 0.6 V vs. Ag/AgCl for a full scan and between ¢0.7 and 0.6 VAg/AgCl for visible light in 1 m NaOH electrolyte. Both photo- electrodes show significantly low dark currents with respect to their photocurrents (Figure 4 a), which indicates that no drastic electrocatalytic water splitting occurs. Apparently, the photo- current of T400 under illumination is 4.5 times higher than that of pristine P25. Furthermore, the onset potential of the photo- current shifts from ¢1.05 VAg/AgCl for P25 to ¢1.12 VAg/AgCl for T400. The higher photocurrent density and the lower onset po- tential for T400 indicate a more efficient charge separation and transport compared to that of pristine P25. The efficiencies of T300 and T500 in PEC H2 production are lower than that of T400 because T400 possesses a higher crystallinity and a thicker amorphous layer outside the nanoparticle (Figure S7). The im- provement of the photocurrent density of T400 is shown in linear-sweep voltammograms under visible light (Figure 4 b). This enhancement is attributed to the improved visible-light absorption of T400 and contributes to its overall photoelectro- chemical performance. To further investigate the photoresponses of our samples, the PEC measurement was performed under illumination for several 40 s light on/off cycles at 0.23 VAg/AgCl (Figure 4 c). Both samples exhibit excellent photoresponses in chopped light cycles for several on/off cycles. The observed steady-state pho- tocurrent of T400 (1.99 mA cm¢2) is 4.6 times higher than that of P25 (0.43 mA cm¢2), which indicates the higher amount of photoinduced carriers and more efficient electron–hole separa- tion in T400. Electrochemical impedance spectroscopy (EIS) was conduct- ed for P25 and T400. Mott–Schottky plots of both samples show positive slopes characteristic of n-type semiconductor behavior (Figure 4 d). T400 displays a smaller slope than P25, which implies a much higher free charge carrier density in T400. The carrier density can be calculated from the slope of Figure 3. a) Photocatalytic decolorization of aqueous MO and b) photocatalytic water splitting in an aqueous solu- tion of 20 % methanol in the presence of P25, T300, and T400 under simulated sunlight. ChemCatChem 2015, 7, 2614 – 2619 www.chemcatchem.org Ó 2015 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim2617 Full Papers http://www.chemcatchem.org Mott–Schottky plots using Equation (1). Nd ¼ ð2=e0ee0Þ½dð1=C2Þ=dV¤¢1 ð1Þ in which e0, e, e0, Nd, and d(1/C 2)/dV represent the electron charge, the dielectric constant of TiO2 (31 for anatase), [21] the permittivity of a vacuum, the donor density, and the straight slope, respectively. The calculated electron concentrations of T400 and P25 are 1.54 Õ 1021 and 1.38 Õ 1019, respectively, which indicates an exponential increase of the electron density and, consequently, a large upward shift of the Fermi level in T400. This shift can result in a significant bending of the band edge at the surface of T400, which facilitates charge separation at the shell–electrolyte interface. The improved charge transport combined with the facilitated charge separation is responsible for the much more efficient PEC water splitting and the greatly enhanced H2 production of T400. Conclusions We reported a low-temperature reduction route by CaH2 to im- prove the photocatalytic performance of TiO2. The treatment decreases the ratio of rutile and induces defects and an amor- phous shell in reduced TiO2, which enables it to exhibit differ- ent colors and absorb more sunlight. The photocatalytic organ- ic degradation and water-splitting performances of the low- temperature reduced samples are both superior to those of P25. In addition, the electron concentration and photoelectro- chemical water-splitting proper- ties are improved greatly after CaH2 reduction. Through the al- teration of the reduction tem- perature, photocatalysts for spe- cific applications (pollutant deg- radation and water splitting, etc.) can be produced controlla- bly and easily. The low-tempera- ture reduction method is prom- ising for other oxide catalysts to enhance their photocatalytic ac- tivity. Experimental Section Synthesis The preparation of the catalysts was performed using CaH2 as a re- ducing reagent and commercial P25 TiO2 (Degussa) as precursor. P25 (0.2 g) and CaH2 (0.4 g) were ground finely in an Ar-filled glove- box, sealed in an evacuated Pyrex tube, and then reacted at 300– 500 8C for 5 h. After cooling to RT, the obtained powders were washed with 0.1 m HCl to remove the residual CaH2 and the CaO by- product. Photocatalysis H2 production by photocatalytic water splitting was performed by using a top-irradiation Pyrex reaction cell. Photocatalyst powder (100 mg) was dispersed by ultrasonication for 2 min into an aque- ous solution (200 mL) that contained methanol (40 mL) as the sac- rificial reagent. Pt (0.5 wt %) was loaded in situ by the impregna- tion of H2PtCl6 (0.05 mL, 10 g L ¢1) in the suspension. Then the sus- pension was degassed thoroughly with pure N2 and irradiated by a 300 W Xe lamp. The temperature of the reaction solution was maintained at RT by a flow of water. The amount of H2 evolved was determined by GC (Shanghai, GC-7900, thermal conductivity detector (TCD), N2 carrier). The photocatalytic activities were com- pared based on the average H2 evolution rate in the first 5 h. The photodegradation of MO was performed in an aqueous solu- tion under irradiation from a 300 W iodine gallium lamp. Typically, the as-prepared samples (100 mg) were dispersed in a Pyrex glass reactor that contained MO solution (100 mL, 10 mg L¢1). Before irra- diation, the suspensions were stirred in the dark for 30 min to reach the adsorption/desorption equilibrium. At given time inter- vals, portions of the suspension (�5 mL) were taken for analysis after centrifugation. The visible-light-driven photodegradation of MO was conducted under the same condition but using a 420 nm filter to cut off the UV light and allow only visible light (>420 nm) to pass through. PEC measurements were performed by using a conventional three- electrode electrochemical workstation (CHI600B, CH Instruments), in whichthe TiO2 film on an fluorine-doped tin oxide (FTO) sub- Figure 4. a) Linear-sweep voltammograms collected under AM 1.5 solar spectrum simulation using a three-elec- trode setup (P25 or T400 working, Pt counter, Ag/AgCl reference electrodes, scan rate of 10 mV s¢1) in 1 m NaOH electrolyte (pH 13.6). b) Linear-sweep voltammograms collected under visible light, the UV light was eliminated by a 420 nm cutoff glass light filter. c) Transient photocurrent responses of P25 or T400 samples at 0.23 V vs. Ag/ AgCl. d) Mott–Schottky plots collected at a frequency of 1 kHz in dark. ChemCatChem 2015, 7, 2614 – 2619 www.chemcatchem.org Ó 2015 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim2618 Full Papers http://www.chemcatchem.org strate, a Pt wire, and an Ag/AgCl (KCl saturated) electrode were used as the working, counter, and reference electrodes, respective- ly. A 1.0 m NaOH aqueous solution (pH 13.6) was used as the sup- porting electrolyte to maintain the stability of the film. A 150 W Xe lamp was used as the light source to simulate the sunlight irradia- tion. A set of linear sweeps and transient photocurrent responses were recorded in the dark and under illumination. Mott–Schottky plots were derived from impedance–potential tests conducted at a frequency of 100 Hz in the dark. Characterization UV/Vis diffuse reflectance spectra were obtained by using a UV/Vis spectrometer (Hitachi U-4100) using BaSO4 as a reference. XRD patterns were recorded by using a Bruker D8 advanced diffractom- eter with CuKa radiation. The morphology was characterized by TEM (JEOL JEM-2100). XPS experiments were performed by using a RBD upgraded PHI-5000C ESCA system (PerkinElmer) with MgKa radiation (hn= 1253.6 eV). EPR spectra were collected by using a Bruker EMX-8 spectrometer at 9.0 GHz and at 300 K. Raman spec- tra were collected by using a Thermal Dispersive Spectrometer using a laser with an excitation wavelength of 532 nm at a laser power of 10 mW. Solid-state 1H magic-angle spinning (MAS) NMR spectra were acquired by using a 600 MHz Bruker spectrometer. PL spectra were measured at RT by using a fluorescence spectropho- tometer (F-4600, Hitachi, Japan) with an excitation wavelength of 320 nm. Acknowledgements This work was financially supported by NSF of China (Grant Nos. 91122034, 51125006, 61376056, and 51402336), and Science and Technology Commission of Shanghai (Grants 13JC1405700 and 14YF1406500). Keywords: electrochemistry · hydrogen · photochemistry · titanium · water splitting [1] a) M. R. Hoffmann, S. T. Martin, W. Y. Choi, D. W. Bahnemann, Chem. Rev. 1995, 95, 69 – 96; b) A. L. Linsebigler, G. Q. Lu, J. T. Yates, Chem. Rev. 1995, 95, 735 – 758; c) Z. Y. Yin, Z. Wang, Y. P. Du, X. Y. Qi, Y. Z. Huang, C. Xue, H. Zhang, Adv. Mater. 2012, 24, 5374 – 5378. [2] a) P. V. 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