Chemical Engineering Journal 431 (2022) 134072 Contents lists available at ScienceDirect Chemical Engineering Journal journal homepage: www.elsevier.com/locate/cej Defective RuO2/TiO2 nano-heterostructure advances hydrogen production by electrochemical water splitting Wenqiang Li a, 1, Heng Zhang a, b, 1, Manzhou Hong a, b, Lilei Zhang a, Xun Feng a, *, Mengfei Shi a, Wenxuan Hu a, Shichun Mu c, d, * a College of Chemistry and Chemical Engineering, Luoyang Normal University, Luoyang 471934, PR China College of Chemistry, Zhengzhou University, Zhengzhou 450001, PR China State Key Laboratory of Advanced Technology for Materials Synthesis and Processing, Wuhan University of Technology, Wuhan 430070, PR China d Foshan Xianhu Laboratory, Foshan 528200, PR China b c A R T I C L E I N F O A B S T R A C T Keywords: Defective RuO2 TiO2 Hydrogen evolution reaction Oxygen evolution reaction DFT calculation Exploring highly active and stable catalysts toward hydrogen evolution reactions and oxygen evolution reactions (HER/OER) is the key for electrochemical water splitting. Herein, density functional theory (DFT) calculation results forecast that the defect-rich RuO2 and TiO2 nano-heterostructures can effectively adjust the electron structure of RuO2, and accelerate the water electrocatalysis, consequently reinforcing the intrinsic activity of the catalyst. Experimentally, to form an integrated nano-heterostructure, a facile approach is designed for in situ fabrication of TiO2 on Ti mesh (TM), simultaneously combined with defective RuO2 (D-RuO2) nanoparticles. Benefiting from the rich active sites, the D-RuO2/TiO2/TM nano-heterostructure formed provides current den­ sities of 50 mA/cm2 at 71 mV for HER and 10 mA/cm2 at 296 mV for OER in alkaline media. For overall water splitting, the electrolyzer assembled with D-RuO2/TiO2/TM electrode can reach 10 mA/cm2 with a voltage of only 1.59 V. Moreover, under a fixed current density, such an electrolyzer also achieves an outstanding stability. 1. Introduction Hydrogen is a promising energy carrier due to its superior calorific value and environmental friendliness. Among the different methods of hydrogen production, electrochemical water splitting, consisting of hydrogen evolution reaction (HER) and oxygen evolution reaction (OER), is an effective and green approach for producing hydrogen [1–5]. Hitherto, precious platinum (Pt)- and iridium (Ir)-based electrocatalysts exhibit the best HER and OER performance separately for water split­ ting. However, they undergo high cost, scarcity, and only single catalytic activity for large-scaled H2 generation [6–8]. Compared to Pt and Ir metals, Ru possesses lower cost, but it lags far behind in the activity and stability. Hence, in order to accelerate the practical applications of hydrogen production by full water splitting, it is important to explore a new and simple approach to prepare bifunctional Ru-based electro­ catalysts with excellent OER and HER activity and stability on a large scale. Due to advantages of the interfacial effect in adjusting the electronic structure of electrode materials, setting up a heterointerface structure becomes one of valid methods to enhance the catalytic activity of cat­ alysts toward water splitting [9–12]. In addition, through the strong interaction between metal with supports, the active noble metal could be evenly dispersed on the supports, achieving outstanding catalytic efficiency and stability [13–16]. For example, Mu’s group reported that ultralow Ru nanoparticles loaded on transition metal phosphides only required a low overpotential for HER [17]. And Ru/reduced TiO2 pre­ pared by Chen et al., exhibited a relatively low overpotential because of the weak OH adsorption of reduced TiO2 in the HER process [18]. Moreover, compared to use organic additives to fasten catalysts on electrode surfaces, if active components are directly grown on substrates with the high conductivity, it also can show the fast electron transport and reaction kinetics [19–21]. For example, Ni/NiMoN nanowire arrays and Co@NC/Ti exhibit vectorial electron transport characteristics and high electrochemical surface areas [22–24]. Metal doping of transition-metal oxides and defects/vacancies in ultrasmall nanoparticles are considered as effective strategy to improve the electrocatalytic activity due to the upsurge of active sites [25]. In comparison with RuO2/ non-defective CeO2, the mass activity of RuO2/ * Corresponding authors. E-mail addresses: fengx@lynu.edu.cn (X. Feng), msc@whut.edu.cn (S. Mu). 1 These authors contributed equally. https://doi.org/10.1016/j.cej.2021.134072 Received 23 October 2021; Received in revised form 29 November 2021; Accepted 6 December 2021 Available online 16 December 2021 1385-8947/© 2021 Elsevier B.V. All rights reserved. W. Li et al. Chemical Engineering Journal 431 (2022) 134072 defective CeO2 increased to 2.45 times at an overpotential of 0.4 V [26]. Ultrafine defective RuO2 nanoparticles on carbon cloth presented a lower overpotential in 0.5 M H2SO4 [27]. Herein, TiO2 as supports in Ru/TiO2-based nanomaterials can promote the water dissociation and weaken OH adsorption, which promote the conversion of water to H2 [28–30]. Toward this end, to form the heterostructure the combination of TiO2 and defective RuO2 would be a high efficient catalyst for water splitting. Here, we first predict the total water splitting activity of the defective RuO2/TiO2 heterostructure catalyst through density functional theory (DFT) calculations, which shows that setting up heterostructures be­ tween TiO2 and defective RuO2 is conducive to the OER and HER pro­ cess. With the encouragement of theoretical predictions, we then design and prepare a defective RuO2/TiO2 nano-heterostructure catalyst on Ti mesh (D-RuO2/TiO2/TM) by impregnating the Ru-containing precursor over Ti mesh, followed by a thermal-oxidative treatment at high tem­ peratures. Due to the rich active sites and the excellent intrinsic activity created by defective RuO2, the resultant defective RuO2/TiO2/TM nanoheterostructure reveals superior catalytic activity for both OER, HER and overall water splitting in 1 M KOH solutions. experiments. 2.2. Synthesis of D-RuO2/TiO2/TM catalysts 1.20 g RuCl3⋅xH2O and 0.5 g MgCl2 were dissolved in 10 mL of deionized water under magnetic stirring. The precursor solution was stored in the dark for further use. A piece of Ti mesh (2 cm × 3 cm) was immersed in the precursor solution and sonicated for about 30 s. After drying at 60 ℃ in oven, the Ti mesh containing precursor was annealed at 450 ◦ C for 3 h in the air to obtained Mg-RuO2/TiO2/TM. After cooled to room temperature, Mg-RuO2/TiO2/TM was collected. Last, the final product D-RuO2/TiO2/TM can be obtained by removing the Mg element in Mg-RuO2/TiO2/TM through acid tread for 18 h. RuO2/TiO2/TM and TiO2/TM can be obtained as the same process as D-RuO2/TiO2/TM except the absence of MgCl2 or RuCl3⋅xH2O in the precursor solutions. To explore the effect of interaction between TiO2 and RuO2 on activity, two other control samples were also prepared using the same synthetic method of D-RuO2/TiO2/TM apart from the pyrolysis temperature. The pyrolysis temperature of samples was 350 ◦ C and 550 ◦ C, which were named D-RuO2/TiO2/TM-350 and D-RuO2/ TiO2/TM-550, respectively. The related Material characterization, Electrochemical measurements and Theoretical calculation details are present in Support Information. 2. Experimental section 2.1. Materials and reagent 3. 3.Results and discussion Ruthenium chloride hydrate (RuCl3⋅xH2O), magnesium chloride (MgCl2) were purchased from Aladdin Ltd (Shanghai, China). Com­ mercial IrO2 was purchased from Sigma-Aldrich. Hydrochloric acid (36% wt) and sulfuric acid (68% wt) were purchased from Sinopharm Ltd (Shanghai, China). The Ti mesh (2 cm × 3 cm) was carefully soni­ cated in 0.5 M H2SO4 and acetone for 20 min to remove impurity of surface. Then the surface was cleaned for several times by deionized water and ethanol. Deionized water was used throughout all 3.1. Theoretical prediction DFT calculations were first performed to understand the catalytic activity of defect-rich RuO2 and TiO2 heterogenous nanoparticles to water splitting (Fig. 1A) [27]. As shown in Figure S1, electrons are transferred from the bottom TiO2(1 1 1) layer to the upper RuO2 layer, and cause a charge-rich state on the Ru, beneficial to the formation of Fig. 1. Atomic and electronic structures of D-RuO2/TiO2 nano-heterostructure and the corresponding free energy profiles for HER. (A) Side views of D-RuO2/TiO2. (B) Electron localization function analysis mapped for the first atomic layer in D-RuO2/TiO2 slab. (C)ΔGH profiles for the HER of TiO2, RuO2/TiO2, Pt/C and D-RuO2/ TiO2, (D) Density of states of Ti in TiO2, RuO2/TiO2 and D-RuO2/TiO2. (E) Partial electronic density of states of Ru d orbital in RuO2, RuO2/TiO2 and D-RuO2/TiO2. 2 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 abundant surface catalytic active centers. In Fig. 1B, the defect is created by removing one Ru atom in the first layer in RuO2/TiO2. Based on the electron localization function analysis map, we can find that the sur­ rounding Ru atom has more positive electrons due to the vacancy caused by Ru defects, conducive to water splitting [17]. To unveil how the interface between defects RuO2 and TiO2 influences the free energy profile of HER, the hydrogen adsorption Gibbs free energies (ΔGH) of pure TiO2, RuO2, RuO2/TiO2, D-RuO2/TiO2 were calculated (Fig. 1C). The ΔGH value of TiO2 is 0.32 eV, suggesting that hydrogen absorption on TiO2 is suppressed. When the RuO2 and TiO2 surface is combined to form the RuO2/TiO2 heterostructure, hydrogen atoms trend to be adsorbed on Ru sites. And the ΔGH of RuO2/TiO2 is − 0.17 eV, unsuitable for HER, due to the strong binding energy will restrains the desorption of H2. With introduction of defects, the ΔGH is − 0.12 eV, very close to the Pt (-0.1 eV), indicating that D-RuO2/TiO2 has a Pt-like adsorption en­ ergy and a fast hydrogen release rates in the HER process. Furthermore, the significant decreased ΔGH* value demonstrates that the hetero­ interface effect between defective RuO2 and TiO2 not only decreases the hydrogen adsorption energy, but also speeds up the hydrogen release rates in the HER process, allowing the D-RuO2/TiO2 catalyst with highest HER activity [31]. Unlike TiO2 with a wide band gap (Fig. 1D), RuO2/TiO2 and D-RuO2/ TiO2 are metallic in nature, indicating a high electrical conductivity. As a result, constructing the RuO2/TiO2 hybrid interface and introducing defects in RuO2 could modulate the electronic structure of Ru. There­ fore, compared with RuO2, the d-band center (εd) of Ru d orbital in defective RuO2/TiO2 moves to low energy level (Fig. 1E), indicating that the interaction between adsorbed oxygen species and Ru sites is weak­ ened, conducive to the OER performances [15,32,33]. Generally, the defective RuO2/TiO2 hybrid interface constructed can adjust the elec­ tronic state of RuO2, and then optimize the adsorption energy of in­ termediates in the HER key steps, speeding up the whole OER kinetic process, advantageous to the whole water splitting. atomic radius of Mg (1.6 Å) than that of Ru (1.89 Å), Mg atoms can be easily inserted into the RuO2 nanoparticles, creating some oxygen va­ cancies and reducing the crystallinity of RuO2. After removing Mg atoms in Mg-RuO2/TiO2 by acid etching, D-RuO2/TiO2/TM with some metal defects can be achieved. The XRD pattern (Figure S2) displays the diffraction peaks at 38.4◦ ,40.2◦ , 53.0◦ , 63.0◦ , 70.7◦ , 76.2◦ and 77.4◦ , which correspond to (0 0 2), (1 0 1), (1 0 2), (1 1 0), (1 0 3), (1 1 2) and (2 0 1) lattice planes of Ti substrate (JCPDF #44–1294), respectively. Except for the Ti peaks, only two diffraction peaks at 37.3◦ and 35.1◦ appear due to the poor crys­ tallinity of samples, corresponding to the (1 0 1) crystal plane of RuO2 (JCPDF #02–1365) and the (3 0 1) plane of TiO2 (JCPDF #34–0180). As displayed in the scanning electron microscopy (SEM) images (Fig. 3A-B), lots of defective RuO2/TiO2 nanoparticles were distributed on Ti mesh, quite different from the pure Ti mesh (Figure S3). The transmission electron microscopy (TEM) image displays (Fig. 3C) that the average grain size of D-RuO2/TiO2 is about 11.5 nm. Such small nanoparticles are beneficial for exposing more catalytically active sites for water splitting. The high-resolution TEM (HRTEM) image (Fig. 3D) display a clear interface structure. The lattice fringe is 0.347 nm, assigning to the (1 0 1) crystal plane of TiO2. At the same time, the lattice fringe spacing of 0.255 and 0.316 nm, in good consistence with (1 0 1) and (1 1 0) planes of RuO2, respectively, [35] basically consistent with the XRD results. Additionally, the elemental mapping images (Fig. 3E-H) make clear that the Ru, Ti and O elements in D-RuO2/TiO2 is uniform distribution. Based on the content of Ru, Ti, O elements (Figure S4), the atom ratio of Ru + Ti: O is about 1:2, indicating the successful synthesis of D-RuO2/TiO2 nano-heterostructure catalysts. X-ray photoelectron spectroscopy (XPS) spectrum was used to investigate the binding states and quantitative chemical compositions of the TiO2/TM, TiO2/RuO2/TM and D-RuO2/TiO2/TM. As exhibited in Fig. 4A, the Ru, Ti, O elements can be observed in samples. In Fig. 4B, the binding energies of 464.2 and 458.6 eV in Ti4+ region of D-RuO2/ TiO2/TM samples correspond to Ti 2p1/2 and Ti 2p3/2, respectively. And the spin–orbit splitting is 5.6 eV(464.2–458.6 = 5.6), which is very consistent with the value of the Ti4+ oxidation state in TiO2-based nanocomposites [36]. Between Ti 2p3/2 and Ti 2p1/2 (Fig. 4B), the peak at about 462.0 eV is attributed to the Ru 3p3/2, while Ru 3p3/2 is absent in TiO2/TM (Figure S5). Two peaks of Ru in D-RuO2/TiO2/TM at 280.6 and 284.3 eV are coincident with the Ru 3d5/2 and Ru 3d3/2 of RuO2 (Fig. 4C), confirming the presence of Ru (IV) in RuO2 in the composite [35]. While the peak located at 284.8 eV can be attributed to C 1 s [15,37]. Compared to TiO2, the Ti peaks in RuO2/TiO2 shift more 3.2. Structure of D-RuO2/TiO2/TM The synthetic route of D-RuO2/TiO2/TM is shown in Fig. 2. First, a piece of Ti mesh was immersed into an aqueous solution including magnesium chloride (MgCl2) and ruthenium chloride hydrate (RuCl3⋅H2O). After drying in the oven, the Ti precursor was annealed in air at high temperatures for a certain time, then Mg-RuO2/TiO2/TM can be obtained. At high temperatures (above 450℃) in the air atmosphere, the surface Ti in Ti mesh was oxidized to TiO2 [34]. Owing to the smaller Fig. 2. Schematic fabrication of D-RuO2/TiO2 nano-heterostructures on Ti mesh (D-RuO2/TiO2/TM). 3 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 Fig. 3. (A,B) SEM images of D-RuO2/TiO2 on Ti mesh. (C,D) TEM and HRTEM image of D-RuO2/TiO2. (E-H) EDS elemental mapping images for D-RuO2/TiO2. The sample was stripped from D-RuO2/TiO2/TM using ultrasonic treatment. negatively due to a stronger electron transfer from TiO2 to Ru (Figure S5). Compared to RuO2/TiO2/TM, the Ti peaks in D-RuO2/TiO2/ TM shift positively, indicates the significant electron transfer between TiO2 and defective RuO2 due to the strong metal-support interaction, resulting in the decreasing the chemical state of Ru. Thus, the Ru 3p peaks for D-RuO2/TiO2 shift negatively (Figure S6), also confirming that oxygen defects were successfully introduced into RuO2 [18,29]. For D-RuO2/TiO2/TM, the O 1 s spectra is composed of three oxygen peaks (Fig. 4E). Among them, the O1(529.5 eV), O2 (531.1 eV) and O3 (532.5 eV) are assigned to the metal–oxygen bonds, the surface chemisorbed oxygen such as O22– or O-(belonging to defectoxide and hydroxyl-like group), and water molecules, respectively [38,39]. Meanwhile, the ratio of O2/O1 (peak area) of D-RuO2/TiO2 is 1.4, larger than that of RuO2/TiO2 (0.43) (Fig. 4F), proving a larger amount of surface oxygen vacancies on the D-RuO2/TiO2 [40–42]. Furthermore, electron spin resonance (ESR) spectrum was performed to directly evidence the presence of vacancies in RuO2/TiO2/TM and D-RuO2/TiO2/TM (Fig. 4F). D-RuO2/TiO2/TM reveals a much stronger oxygen vacancy related ESR signal than RuO2/TiO2/TM, indicating that extensive oxy­ gen vacancies formed on the surface of D-RuO2/TiO2 [43,44]. The ox­ ygen vacancies on the surface of RuO2 can form more electrochemically active sites, thereby improving the electrocatalytic activity of catalysts [45,46]. has big influences on the RuO2 activity. At current densities of 10, 100, 150, and 200 mA/cm2, the overpotentials are 10, 114, 147, and 165 mV, respectively, proving the extremely high HER activity of D-RuO2/TiO2/ TM in alkaline media. In addition, it is worth noting that at high current densities above 150 mA/cm2, the HER activity of D-RuO2/TiO2/TM even surpasses that of commercial Pt/C on TM (Fig. 5A). Noting that, the excellent HER performance of D-RuO2/TiO2/TM in alkaline media is far ahead of the reported RuO2-based materials, and can be compared with the best Ru-based electrocatalysts as reported, such as RuO2/N-C(Ƞ10 = 40 mV) [47], RuO2-300Ar(Ƞ10 = 17 mV) [48], CoOx-RuO2(Ƞ10 = 24 mV) [49] as well as Pd3Ru /C (Ƞ10 = 42 mV) [50] (Table S1). In addition, to study the reaction kinetics during HER processes, the Tafel curves of different catalysts were measured (Fig. 5C). Obviously, the Tafel slopes of D-RuO2/TiO2/TM is 73.5 mV dec-1, close to the Tafel slopes (97.5 mV/dec) obtaining from the true steady-state polarization curve (Figure S7) [51], smaller than that of RuO2/TiO2/TM (105.3 mV dec-1), TiO2/TM (206.6 mV dec-1) and Bare TM (237.5 mV dec-1). Ac­ cording to the obtained Tafel value, the HER process on the D-RuO2/ TiO2/TM electrode should be the Volmer- Heyrovsky pathway [25]. Moreover, the Nyquist plots demonstrate that the D-RuO2/TiO2/TM electrode has the smallest charge transfer resistance (Rct) (Fig. 5D), suggesting it has an excellent electron transfer. Above all, the higher HER activity of the D-RuO2/TiO2/TM electrode can be explained by the smallest Tafel slope and minimal Rct. Furthermore, the exchange cur­ rent densities (j0) of D-RuO2/TiO2/TM, Pt/C on TM, RuO2/TiO2/TM and TiO2/TM are 6.9, 5.4, 5.01 and 0.38 mA cm− 2, respectively (Figure S8), manifesting that D-RuO2/TiO2/TM holds better intrinsic catalytic ac­ tivity than RuO2/TiO2/TM and TiO2/TM. Durability is another important factor in assessing the practical ap­ plications of an HER catalyst. After 1000 CV cycles, the LSV curves (Fig. 5E) show a negligible change. Furthermore, to further evaluate the durability, we performed the electrolysis measurement under the fixed current continuously for 18 h. As shown in Fig. 5F, D-RuO2/TiO2 only emerges nearly unchanged in the overpotential after electrolysis, proving the high catalytic durability. After the durability test, from the XRD (Figure.S9A), it shows the presence of RuO2 and TiO2 in the composite, and no significant change 3.3. Electrochemical evaluation for HER To understand the effect of constructing defect-rich nano-heter­ structures on the electrochemical activity, the HER activity of D-RuO2/ TiO2/TM was explored in 1 M KOH solutions at 5 mV s− 1. As depicted in Fig. 5A, we applied the solution resistance to achieve the iR compen­ sated polarization curves for TM, TiO2/TM, RuO2/TiO2/TM and DRuO2/TiO2/TM. Obviously, it can be seen that the performance was enhanced after generating defects and integrating TiO2 with RuO2. This can also be observed from the comparison of overpotentials (Fig. 5B), in which the overpotentials at 50 mA/ cm2 (Ƞ50) of TiO2/TM and RuO2/ TiO2/TM are 407 mV and 114 mV, respectively. While D-RuO2/TiO2/ TM shows a low Ƞ50 of 71 mV, suggesting the defect-rich heterogenous 4 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 Fig. 4. (A) XPS spectra for TiO2/TM, RuO2/TiO2/TM and D-RuO2/TiO2/TM; Ti 2p (B) and Ru 3d spectra(C)for D-RuO2/TiO2/TM; O1S spectra of RuO2/TiO2/TM(D) and D-RuO2/TiO2 /TM(E), respectively; (F) ESR spectra of RuO2/TiO2/TM and D-RuO2/TiO2/TM. can be observed in the chemical state with initial one, indicating the outstanding durability of D-RuO2-TiO2/TM for HER. In addition, the XPS spectra also illustrate that the composition of D-RuO2-TiO2/TM does not change significantly (Figure. S9B-D). Moreover, the HRTEM image of D-RuO2/TiO2 after long-term HER in 1 M KOH certifies the crystal structure without distinct change (Figure. S10). In general, in alkaline media, the performance of D-RuO2-TiO2/TM is better than most HER catalysts as previously reported. TM were obtained. As shown in Fig. 6A, the OER performance of bare TM is limited, while D-RuO2/TiO2/TM exhibits relatively high OER activities. It is worth noting that the LSV curves show the order for OER activities: D-RuO2/TiO2/TM < IrO2 on TM < RuO2/TiO2/TM < TiO2/ TM. As presented in Fig. 6B, the Ƞ10 of D-RuO2/TiO2/TM (296 mV) is 54, 75 and 226 mV, smaller than that of IrO2 on TM (350 mV), RuO2/ TiO2/TM (371 mV) and TiO2/TM (522 mV), respectively. Overall, the DRuO2/TiO2/TM electrode displays the highest OER catalytic activity, representing that the defects and interfaces can create more active sites to promote the catalytic performance. Furthermore, as shown in Table S2, it also confirms that the activity of D-RuO2/TiO2/TM is su­ perior to some reported Ru-based anode electrocatalysts in alkaline media. In order to further understand the OER kinetics, the Tafel curves of 3.4. Electrochemical evaluation for OER Next, we further probed the OER catalytic activity of D-RuO2/TiO2 in 1 M KOH solutions. The polarization curves with iR 100% compensated for bare TM, TiO2/TM, RuO2/TiO2/TM, D-RuO2/TiO2/TM and IrO2 on 5 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 Fig. 5. HER polarization curves for bare TM, Pt/C on TM, TiO2/TM, RuO2/TiO2/TM and D-RuO2/TiO2/TM in 1 M KOH recorded at 5 mV s− 1. (B) Corresponding overpotentials at j = 50 mA/cm2. (C) Corresponding Tafel plots. (D) Nyquist plots of TiO2/TM, RuO2/TiO2/TM and D-RuO2/TiO2/TM measured at overpotential of 120 mV. (E) Polarization curves recorded initial and after 1000 CV cycles for D-RuO2/TiO2/TM. (F) Time-dependent overpotentials curve for D-RuO2/TiO2/TM under a static current density for 18 h. the catalysts were plotted. The Tafel slopes of D-RuO2/TiO2TM, IrO2 on TM, RuO2/TiO2/TM and TiO2/TM were measured to be 40.6, 70.6, 71.7 and 171.6 mV dec-1, respectively (Fig. 6C). Especially, the Tafel slope of D-RuO2/TiO2TM obtained from the OER polarization curves with 100% IR drop is 40.6 mV/dec, close to that (72.2 mV/dec) of D-RuO2/TiO2TM from the true steady-state polarization curve (Figure S11). The smallest Tafel slope of D-RuO2/TiO2/TM in all control samples suggests it per­ forms the best OER catalyst in all catalysts. Electrochemical impedance spectroscopy (EIS) of samples (Fig. 6D) exhibits that compared with RuO2/TiO2/TM, both TiO2/TM and D-RuO2/TiO2/TM possess remark­ ably low charge-transfer resistance, suggesting an expeditious charge transfer. After 1000 CV cycles, the OER polarization curve of D-RuO2/TiO2/ TM nearly overlaps with the initial one, demonstrating it almost keeps unchanged the OER activity (Fig. 6E). In addition, electrolytic mea­ surements were performed continuously for 20 h at a fixed current density to further evaluate durability. As displayed in Fig. 6F, for DRuO2/TiO2 it changes slightly in overpotentials with time, also proving the excellent catalytic stability. In addition, the XRD spectra of D-RuO2/ TiO2 after durability tests show that its physical structure is well pre­ served (Figure. S12A). XPS analysis of the samples after OER durability tests demonstrates that the intensity of Ru 3p test decreases slightly compared with the initial one, indicating the surface passivation during the OER process (Figure. S12 B-D). 6 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 Fig. 6. (A) OER polarization curves for Bare TM, Pt/C on TM, TiO2/TM, RuO2/TiO2/TM and D-RuO2/TiO2/TM in 1 M KOH recorded at 5 mV s− 1. (B) Corresponding overpotentials at j = 10 mA/cm2. (C) Corresponding Tafel plots. (D) Nyquist plots of the Bare TM, Pt/C on TM, TiO2/TM, RuO2/TiO2/TM and D-RuO2/TiO2/TM measured at overpotential of 350 mV. (E) Polarization curves recorded initial and after 1000 CV cycles for D-RuO2/TiO2/TM. (F) Time-dependent overpotential curve for D-RuO2/TiO2/TM under a static current density for 20 h. 3.5. Electrochemical evaluation for water splitting shown in Fig. 7C, the LSV after 1000 CV cycles remains almost the same as the initial one. Figure S13 displays that the D-RuO2/TiO2/TM||DRuO2/TiO2/TM electrolyzer has outstanding durability and almost negligible decay of current densities after long-time stability test for 20 h under the fixed potential 1.8 V. What’s more, the chronopotentiometry curve of D-RuO2/TiO2/TM||D-RuO2/TiO2/TM were conducted under 250 mA/cm2 for 72 h (Fig. 7D). The real-time potential displays a slight change, also confirming the high durability of D-RuO2/TiO2/TM for water splitting. The H2 and O2 gases generated from the alkaline electrolyzer were quantitatively collected by the water drainage method. The vol­ ume–time curve (Figure S14) reveals a volume ratio of 2.1:1 for the collected H2 to O2, approaching to the theoretical 2:1 for water Inspired by the outstanding OER and HER catalytic performances of D-RuO2/TiO2/TM in alkaline solutions, an electrolyzer was assembled by employing D-RuO2/TiO2/TM as bifunctional catalyst for overall water splitting. Fig. 7A-B manifest that to reach 10 mA/cm2 the assembled device only needs a cell voltage of 1.59 V, significantly less than those of Pt/C||IrO2 (1.63 V at 10 mA/cm2) and RuO2/TiO2/|| RuO2/TiO2 couples (1.64 V at 10 mA/cm2). This activity even exceeds than those reported rare precious metal materials in 1.0 M KOH (Table S3), for instance Ni@Ru/CNS-10% (1.612 V at 10 mA/cm2), [52] Ru1Co2 NP (1.59 V at 10 mA/cm2), [53] CoFeRu@C (1.62 V at 10 mA/ cm2), [54] and PdP2@CB (1.72 V at 10 mA/cm2) [55]. In addition, as 7 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 Fig. 7. Polarization curves without iR-compensation of RuO2/TiO2/TM|| RuO2/TiO2/TM, Pt/C on TM||IrO2 on TM and D- RuO2/TiO2/TM||D- RuO2/TiO2/TM toward overall water splitting in 1 M KOH recorded at 5 mV s− 1. (B) Corresponding overpotentials at j = 10 mA/cm2. (C) Polarization curves recorded initial and after 1000 CV cycles for D-RuO2/TiO2/TM||D-RuO2/TiO2/TM (D) Potential–time response curve of D-RuO2/TiO2/TM||D-RuO2/TiO2/TM at 250 mA/cm2 in 1 M KOH for 72 h. electrolysis. This demonstrate the almost 100% faradic efficiency for full water splitting. In conclusion, D-RuO2/TiO2/TM has an high efficiency and durability for hydrogen production from electrochemical water splitting. be drawn that the pyrolysis at 350 ◦ C is not enough to obtain the TiO2 phase, while it is the optimal at 450 ◦ C. As demonstrated by the more electrochemical tests (Figures S19-S20), the superior OER and HER activity of D-RuO2/TiO2/TM is derived from the lowest charge transfer resistance and the highest ECSA. In short, the appropriate pyrolyzed temperature can optimize the interfacial synergistic effects and the overall catalytic activity of materials. Based on the above experimental and analytic results, the perfect activities of the D-RuO2/TiO2/TM heterogeneous materials toward overall water splitting could be attributable to the following aspects: (i) DFT calculation reveals that setting up a hybrid interface between defective RuO2 and TiO2 can optimize the adsorption energy of in­ termediates in HER, speeding up the OER overall kinetic process, conducive to the whole water splitting. (ii) The defects in D-RuO2/TiO2/ TM change the electronic structures of existing Ru, and generate more active sites, promoting the intrinsic catalytic activity. (iii) The doublelayer capacitance tests demonstrate that the D-RuO2/TiO2/TM has large electrocatalytic active surface area and more catalytic active sites, thereby speeding up the electrochemical process. (IV) The synergistic effect between defective RuO2 and TiO2 phases can significantly enhance the electrocatalytic activity toward OER together. (V) The Nyquist plots indicate that defective D-RuO2/TiO2 has a faster charge transfer capacity during water splitting processes than other contrast samples, owing to the synergistic effects between TiO2 and defective RuO2. 3.6. Mechanism analysis The double-layer capacitance (Cdl) used to estimate the electro­ catalytic active surface area (ECSA) (Figure S15A–C) can effectively explain the inherent activities of the catalytic materials [56]. Figure S15D reveals the Cdl value of D-RuO2/TiO2/TM is 48.8 mF cm− 2, about 1.35 and 25.6-fold larger than that of RuO2/TiO2/TM (36.1 mF cm− 2) and TiO2/TM (1.9 mF cm− 2), respectively. Such a Cdl value cer­ tifies that D-RuO2/TiO2/TM represents a larger ECSA (813 cm2) than RuO2/TiO2/TM (601 cm2) TiO2/TM (31.6 cm2). Obviously, CV mea­ surements reveal that D-RuO2/TiO2/TM owns a larger ECSA, exposing extensive active sites, and leading to superior activity than control samples. As shown in Figure S16, the superior ECSA normalized OER and HER activities further reveal that D-RuO2/TiO2/TM possesses higher intrinsic catalytic activity than TiO2/TM and RuO2/TiO2/TM. To explore the effect of interaction between TiO2 and defective RuO2 on activity, another two materials (namely D-RuO2/TiO2/TM/TM-350 and D-RuO2/TiO2/ TM-550) were further synthesized by changing the pyrolysis temperature to 350 ◦ C and 550 ◦ C. As illustrated by the XRD patterns (Figure S17) and polarization curves (Figure S18), the pyro­ lyzed temperature of precursors shows an important influence on the crystal structure and electrocatalytic performance. One conclusion can 8 W. Li et al. Chemical Engineering Journal 431 (2022) 134072 4. Conclusion [10] Y. Hu, X. Luo, G. Wu, T. Chao, Z. Li, Y. Qu, H. Li, Y. Wu, B. Jiang, X. 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Edit. 59 (23) (2020) 8982–8990, https://doi. org/10.1002/anie.201908760. In summary, we reported a simple but effective strategy to synthesize the bi-functional defective RuO2/TiO2 nano-heterostructure catalyst. Importantly, as predicted by DFT calculations, the Ru d-band center in defective RuO2/TiO2 can shift to a low-energy level due to the strong interface interaction, and weakens the interaction between adsorbed oxygen species on Ru sites, benefiting for the water splitting. As ex­ pected, the D-RuO2/TiO2/TM catalyst exhibited excellent performance for both OER and HER in 1 M KOH. For overall water splitting device assembled here, it merely required 1.59 V to achieve a current density of 10 mA/cm2. The defective RuO2/TiO2/TM also reveals superior dura­ bility. Overall, owing to low-cost, facile syntheses and outstanding cat­ alytic activity, the defect-rich RuO2/TiO2/TM is a promising electrode toward high-efficiency hydrogen production via electrocatalytic water splitting. 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