Electrocatalytic water oxidation is a rate-determining step in the water splitting reaction. Here, we report one single atom W6+ doped Ni(OH)2 nanosheet sample (w-Ni(OH)2) with an outstanding oxygen evolution reaction (OER) performance that is, in a 1 M KOH medium, an overpotential of 237 mV is obtained reaching a current density of 10 mA/cm2. Moreover, at high current density of 80 mA/cm2, the overpotential value is 267 mV. The corresponding Tafel slope is measured to be 33 mV/dec. The d0 W6+ atom with a low spin-state has more outermost vacant orbitals, resulting in more water and OH− groups being adsorbed on the exposed W sites of the Ni(OH)2 nanosheet. Density functional theory (DFT) calculations confirm that the O radical and O-O coupling are both generated at the same site of W6+. This work demonstrates that W6+ doping can promote the electrocatalytic water oxidation activity of Ni(OH)2 with the highest performance.
Electrocatalytic water splitting for hydrogen and oxygen generation provides an attractive path to obtain clean energy via the conversion and storage of intermittent solar and wind energies; however, the half reaction of oxygen evolution remains the bottleneck for such progress1,2,3,4,5. The oxygen evolution reaction (OER) is kinetically sluggish and needs the necessary two steps of O–H bond breaking and attendant O–O bond formation, which includes the transfer of four electrons4,5,6,7,8,9,10,11,12,13,14,15,16,17,18,19. The design of a considerable OER electrocatalyst is needed. In this case, the noble metal-based catalysts, for example IrO2 and RuO2, exhibit attractive OER activity, but their rare nature hinders their large-scale application. A great many non-noble metal-based alternative OER catalysts using abundant 3d metals (Fe, Co, Mn, and Ni) have been studied with increasing activity and stability in recent years9,10,20,21,22,23,24,25,26. In particular, Ni(OH)2-based samples have garnered a great interest with studies showing their encouraging water oxidation potential4,9. In addition, the doping of elemental Fe with Ni(OH)2 at low content levels has been shown to greatly increase the OER performance27. However, substantial progress in the development of Ni(OH)2-based OER catalysts with enhanced activity is still needed.
For the Fe-doped Ni(OH)2 sample, the detailed OER pathways have been shown through several manners of occurrence. In the preliminary works, Fe doping is considered to improve the electrical conductivity27 and change the electronic structure, anodically shifting the Ni redox potential28,29. Boettcher confirmed that Fe exerted a partial-charge transfer activation effect and then promoted the OER of the Ni sample30. By using operando X-ray absorption spectroscopy and computational methods, Bell et al. proposed that the Fe doping in NiOOH produced short Fe–O bonds. These active bond sites were said to have resulted in the high OER performance with low overpotentials and optimal adsorption energies of OER intermediates being observed31. Stahl et al. first detected the formation of Fe4+ during the OER process by Mössbauer Spectroscopy and reported that the species was not kinetically competent to serve as the active site in water oxidation32. Strasser concluded that Fe could suppress the oxidation process of Ni species from + 2 to + 3/ + 4 and help the lower-valent states of the Ni centers have a higher OER activity33. The Fe sites in Ni-based hydroxides are almost accepted to be the critical component of the record activity of water oxidation. To further confirm that reactive Fe sites were responsible for the exceptional OER, the introduction of Fe into the NiOxHy from solution was performed with the unaltered conclusion that its precise role remains unclear34. Although the replacement of Fe3+ to Ni2+ in the Ni(OH)2 sample has been shown to enhance oxygen evolution through extensive study, the core part of the water oxidation on the surface of the Ni(OH)2-based sample, that is, the reaction behavior on the exposed/contacted Ni(OH)2 surface is rarely studied and reported28,34,35,36,37. Moreover, the OER performance of Ni(OH)2-based electrocatalysts still needs improvement by doping, and the finding of a suitable element remains to be developed.
On the electrocatalytic process, there is an electric double layer (Helmholtz layer, HL) at the catalyst|solution interface as shown in Supplementary Fig. 1. The electrical circuit is completed through three resistance measures i.e., the catalyst, catalyst|solution interface, and the solution. The HL is important and determinative for the final electrocatalytic efficiency owing to the induced capacitive and resistive characteristics resultant from the changing of a solid to solution38,39,40. In the case of water splitting, the adsorption and desorption behaviors of H2O molecules and OH− groups in the HL will directly influence the hydrogen or oxygen generation41,42. Therefore, the specifics of the coordination of the exposed elements (such as Ni or Fe) should be studied further to potentially improve the performance35. The appropriate chemical environment, the strength of the bond between the electrode and intermediates and the electron migration resistance are the key factors in leading to a significant OER enhancement43. Recently, Shin et al. found that both Ni4+ and Fe4+ played essential roles in the OER. The high spin d4 Fe4+ site was favorable for stable O· radical formation with the low spin Ni4+ more favorable for O–O bond coupling44. In addition, Zhang et al. reported that the W doping can provide the near-optimal adsorption energies for OER intermediates in FeCo oxy-hydroxide samples14, and single-atom doping has been reported to be useful for assisting suitable sites for intermediates formation45,46,47,48. It is still then necessary to find one suitable reaction site for achieving both the formation and migration of intermediates.
Herein, we report that W6+ doping can boost the OER performance of Ni(OH)2 greatly. Owing to the d0 characteristic, the W6+ doping sites exhibit exothermic H2O adsorption and O radical formation reactions, differing from the endothermic reactions otherwise reported. Furthermore, the formation of the O radical and O–O coupling both happen at the W6+ sites. In conjunction, the W-doped sample exhibits low reaction potentials at high current densities.
Insight into the water oxidation on Ni(OH)2
At first, the electrocatalytic processes of Ni(OH)2 were studied to check the interfacial effect on the OER. On the electrocatalytic water oxidation by Ni(OH)2, one obvious process attributable to the Ni2+ ↔ Ni3/4+ peak (ca. 1.45 V in Fig. 1a) in the cyclic voltammetry plots was detected30,31,32,33,34,35,36,37. This process happened together with the formation of the O*, which is an essential intermediate (which couples with one OH− group to generate *OOH) for oxygen evolution44. Figure 1a gives the CV curve of Ni(OH)2, and the inset shows the corresponding oxygen evolution intermediate pathways: at the low potential (region ➀), *OH generation; in the mid potential (region ➁), the above-mentioned process occurs; and then the O2 will generate under high potential (region ➂). The three simplified processes of water oxidation involve the HL and include *OH species adsorption, *O radical formation, and *OOH transformation and desorption45. To detect the interfacial resistance of the corresponding process, three potentials of 1.2, 1.45, and 1.6 V were applied for the electrochemical impedance spectroscopy (EIS) measurement as shown in Fig. 1b. Supplementary Table 1 shows the fitted values based on the equivalent electric circuit (Fig. 1c). Clearly, RΩ, the resistance of the solution and electrode, presented a slightly increasing trend from 10.8 to 17.5 Ω/cm2 under the potential of 1.2 to 1.6 V; meanwhile, the Rct, the charge transfer resistance, gave a decreasing trend from 277.4 to 168.6 Ω/cm2. The above increasing and decreasing trends suggested the change (Ni2+ → Ni3/4+) of the electrode surface. To obtain further information, the change rate of fitted resistance values were carried out as shown in Fig. 1d. The increasing and decreasing rates of 1.45 V compared with 1.2 V are 0.55 and 0.14, respectively, meanwhile, the rates for the 1.6 V condition compared with 1.45 V are 0.05 and 0.29, respectively. The slight change confirms that the process of Ni2+ → Ni3/4+ at the lower potential is the decisive step for the overall water oxidation. Based on the above experimental results and analysis, an excellent OER Ni(OH)2-based catalyst should have the suitable outermost orbits for *OH species adsorption and for stabilization of the *O radical49,50. Moreover, if it has the preferred O–O coupling ability, then high water oxidation efficiency will be expected.
Synthesis of W single-atom doped Ni(OH)2. Bare Ni(OH)2 and doped samples were synthesized through the alcohothermal method using an NiCl2–ethanol and WCl6–ethanol solution (Experimental section and Supplementary Fig. 2). Figure 2a shows the XRD patterns of the obtained samples. For bare Ni(OH)2, (Ni(OH)2-r), all peaks were assigned to the α-Ni(OH)2 phase (PDF: 38-0715). The tungsten-doped sample (w-Ni(OH)2-e) also gave the typical α-Ni(OH)2 XRD signals with the obvious difference: the peaks of (101) and (110) loaded at 2 theta of 33.4 and 59.9 degree maintained their location, but the peaks of (003) and (006) showed a left shift compared with the Ni(OH)2-r sample. As we know, for the layered Ni(OH)2 sample, the shift of the (003) peak to the low diffraction angle suggested that the interlayer spacing between the signal from the octahedral Ni(OH)6 layer had been broadened. The W element has a more unoccupied outermost electron orbital than Ni, and the replacement of one Ni by one W in the layered Ni(OH)2 structure was expected to generate some additional adsorption sites on W. In our present work, the ethanol or other relative groups would adsorb on the exposed W sites and then widen the layered structure. When the w-Ni(OH)2-e sample was treated by ultrasound in the ethanol solution, the final w-Ni(OH)2 sample was obtained. As shown in Fig. 2a, only three XRD peaks with low intensity were detected, and the (003) peak exhibited a right shift when compared with the w-Ni(OH)2-e sample. The results confirmed that the ethanol exfoliation is serviceable for obtaining the thin layered W-doped Ni(OH)2 sample. We also tested the effect of ultrasound time on the final layered result (Supplementary Fig. 3). Supplementary Fig. 4a gives the FTIR spectra of the studied samples. Three peaks relative to the OH group loaded at 484, 1631, and 3440 cm−1 were detected51,52. Supplementary Fig. 4b shows the Raman spectra of the samples. The relative peaks for the three main OH groups at 1283, 2930, and 3645 cm−1 can be found with a decreasing intensity from Ni(OH)2-r to w-Ni(OH)251. Supplementary Fig. 5 shows the X-ray photoelectron spectroscopy (XPS) results. No obvious difference can be detected53.
Figure 2b shows the typical UV–Vis absorption spectrum. No obvious main peak shifts or WO3-based signals could be detected, confirming that the W doping did not change the electronic structure of the Ni(OH)2 sample. Moreover, the above UV–Vis spectra results suggested the low W content doping or lattice doping, which was thought to have occurred. To further confirm this, the UV–Vis signals of WO3, 1%, 2 and 3% WO3 loaded Ni(OH)2 samples were tested as shown in Supplementary Fig. 6. Obviously, the WO3-loaded Ni(OH)2 samples show the red-shift optical absorption even at a low content (1%), suggesting that W doping of the w-Ni(OH)2 sample was indeed lattice doping via single- or multi-atomic doping. The X-ray absorption spectroscopy (XAS) measurements were carried out to further confirm the atomic doping of W element. WO3 and W powder were used as the reference samples. As shown in Fig. 2c, the normalized X-ray absorption near-edge structure (XANES) spectra of W K-edge, the intensity of prominent peak of w-Ni(OH)2 or WO3 is higher than W powder, suggesting the oxidized electronic structure of W element in w-Ni(OH)2. Moreover, the position of the prominent peak of w-Ni(OH)2 was close to that of WO3 (10208.07 eV), revealing the dominance of W6+ in w-Ni(OH)2. The above observation coincides well with the XPS results (Supplementary Fig. 5). Further structural information about W atoms can be obtained from the extended X-ray absorption fine structure (EXAFS). The K2-weighted Fourier transform spectra of w-Ni(OH)2 and the reference samples in R space are shown in Fig. 2d. Typically, the EXAFS curve of W power shows a dominant peak at 2.6 Å, corresponding to the W–W coordination. In clear contrast with this common observation, the sample of w-Ni(OH)2 and WO3 only show the one peak located at ca. 1.3 Å, which can be assigned to W–O coordination. Importantly, in comparison with WO3 (1.31 Å), some appreciable shift of W–O peak (1.39 Å) for w-Ni(OH)2 can be detected, confirming the different W–O environment. Supplementary Fig. 7 shows the corresponding atomic force microscope (AFM) images of the studied samples, in which Ni(OH)2-r, w-Ni(OH)2-e, and w-Ni(OH)2 show the thickness of 8, 12, and 8 nm, respectively.
Figure 3 gives the electron microscope analysis of the w-Ni(OH)2 sample. According to the SEM image (Fig. 3a), the layered structure of w-Ni(OH)2 was found to be clearly evident. The reference samples i.e., Ni(OH)2-r and w-Ni(OH)2-e also gave the typical layered image (Supplementary Fig. 8). Figure 3b shows the corresponding TEM result of the w-Ni(OH)2 sample, the thin layered structure was here further confirmed. The inset shows the typical electronic diffraction spots with the hexagonal structure of α-Ni(OH)2 clearly present. The TEM images of reference samples can be found in Supplementary Fig. 9, Fig. 3c gives the HADDF image and the corresponding element mapping. Clearly, the Ni(OH)2 structure was doped by the W element uniformly. To directly find the W in the Ni(OH)2 lattice, HAADF-STEM was further carried out. As shown in Fig. 3d, the light spots originated from the W element, which had been doped into the lattice and did not change the elements hexahedral arrangement (Fig. 3e). Supplementary Fig. 10a shows the local enlarged HADDF–STEM image and the corresponding mode of the signal by the W-doped Ni(OH)2 hexagon structural unit, clearly suggesting that the signal by W doping has been obtained based on our present synthesized process. Moreover, according to the model of the atomically doped W atoms in the Ni(OH)2 structure in Supplementary Fig. 10b, the above XAS results confirm the atomic doping of W atoms into Ni(OH)2. Supplementary Fig. 11 gives the contrastive HADDF–STEM images of pristine and doped Ni(OH)2 samples. Clearly, the W-doped sample gives many disordered sites in comparison with the typical symmetric hexagon structure of the pristine Ni(OH)2 sample, further exemplifying that the W doping can change the lattice structure of Ni(OH)2. For determining the mass ratio of W to Ni, Inductively Coupled Plasma-Mass Spectrometry (ICP–MS, aurora M90) was used. The atomic ratio was detected to be 2.985: 99.55, near the theoretical value (Supplementary Table 2).
Electrocatalytic water oxidation performance
The electrocatalytic activity of the Ni(OH)2-r, w-Ni(OH)2-e, and w-Ni(OH)2 samples toward OER in a 1 M KOH aqueous solution was measured as shown in Fig. 4. As expected, the polarization curve of the w-Ni(OH)2 sample gave the best catalytic activity among the three electrodes, delivering a much higher current density than the others at the same overpotential (Fig. 4a). Typically, all the Ni(OH)2 samples showed the obvious Ni2+ ↔ Ni3/4+ peak at the potential of ca. 1.45 V. Furthering the anodic potential, the control material pure Ni(OH)2-r sample presented a slowly climbing line, indicating a gradual increase in current density. This was in contrast to the W-doped sample which showed a significantly steeper response at a lower potential. We next compared the overpotentials at three catalytic current density values of 10, 50, and 80 mA/cm2 as shown in Fig. 4b. The w-Ni(OH)2 electrode required an overpotential of 237 mV for reaching the current density of 10 mA/cm2, where the reference samples of Ni(OH)2-r and w-Ni(OH)2-e required 351 and 264 mV, respectively. Note that the potential value of the control Ni(OH)2-r sample at the current density of 10 mA/cm2 was 351 mV, which is lower than those reported15,17,18,19. At a higher current density i.e., 80 mA/cm2, the two samples of w-Ni(OH)2-e and w-Ni(OH)2 gave overpotential values of 290 and 257 mV, respectively. Please note that the W-doped thin layered Ni(OH)2 i.e., w-Ni(OH)2 showed the lowest overpotential at current densities of 50 and 80 mA/cm2 amongst reported literature values of Ni(OH)2-based OER catalysts (Supplementary Table 3). The kinetic parameters of the studied electrodes were further calculated from the corresponding polarization curves by plotting overpotential against log (j). As shown in Fig. 4c, Ni(OH)2-r, w-Ni(OH)2-e, and w-Ni(OH)2 showed Tafel slopes of 111, 58, and 33 mV/dec, respectively. To get a direct comparison, commercial RuO2, a commonly used electrocatalyst for OER, was prepared and tested as shown in Supplementary Fig. 12, the overpotentials recorded were 350 and 470 mV at the current density values of 10 and 50 mA/cm2, respectively. Moreover, the RuO2 electrode gave a Tafel slope of 92 mV/dec.
It was thought that the higher intrinsic catalytic activity of w-Ni(OH)2 may have been due to its higher conductivity over w-Ni(OH)2-e or Ni(OH)2-r. To confirm this hypothesis, EIS plots of the three samples were carried out as given in Fig. 4d. According to the above detailed analysis of the EIS measurements (Fig. 1), the bias voltage was set to be 1.48 V. Clearly, the sample of Ni(OH)2-r gave the biggest circular arc, followed by w-Ni(OH)2-e and then w-Ni(OH)2, suggesting that the W element doping improved the electrical conductivity which was then further improved by the exfoliation strategy. Supplementary Table 4 gives the corresponding fitted results based on the same equivalent electric circuit in Fig. 1c. Clearly, the Rct values show the rapid decrease from Ni(OH)2-r to w-Ni(OH)2, further confirming that the thin-layered W-doped sample had a relatively higher carrier mobility across the HL i.e., the catalyst|solution interface. Furthermore, chronopotentiometry experiments with multiple current steps were carried out to examine the rapid response of the carrier migration as shown in Fig. 4e. Attention was only paid to the relative high current density, which was increased from 50 to 100 mA/cm2. The response change of applied potentials was answered by corresponding stable current values consistently, confirming the excellent carrier migration across the interface of the electrode and solution. Supplementary Fig. 13a gives the comparison of the activity between the initial surface and of the surface after 1000 cycles, where no obvious change was detected. The XRD result also exhibited similar patterns (Supplementary Fig. 13b), and indistinguishable SEM images in Supplementary Fig. 13c of the samples can further be found for additional confirmation of structural similarity before and after 1000 cycles. Furthermore, XPS was carried out to confirm the stability of the w-Ni(OH)2 structure. As shown in Supplementary Fig. 14, no obvious change in the wide survey spectra was found. Moreover, the W 4 f XPS spectra of the initial, after 10 h sonication and after long-time stability test was also unchanged. To further confirm the stability of the surface W atoms in the Ni(OH)2 lattice, the concentration of W in the solutions under the different reaction time at 30 mA/cm2 was studied using ICP–MS. As shown in Supplementary Fig. 15, the W signals almost keep the same, suggesting its remarkable stability. The corresponding element mapping and the STEM images have also been given as shown in Supplementary Figs 16 and 17. No obvious change could be detected.
We also tested the relationship between elemental W content in the Ni(OH)2 and the final OER activity. According to the polarization curves in Supplementary Fig. 18, the W content played an essential role for the water oxidation in this study and it was concluded that the 3% W content (atomic ratio, W/Ni) was the optimal doping level. It was also shown that an increase or decrease of as little as 1% W dopant will decrease the catalytic performances (Supplementary Fig. 18a). The corresponding Tafel slopes in Supplementary Fig. 18b clearly show the change. Furthermore, we observed that the pH of the solution used for water oxidation was also crucial. The four pH solutions i.e., pH = 13.6, 12, 11, and 10 were prepared, and Supplementary Fig. 19 describes the resultant OER characteristics. The water oxidation activity decreased sharply from high-to-low pH solution, suggesting that the concentration of OH− groups around the electrode surface was very important for OER.
More analysis is needed to clarify the reaction sites of the single-atom W-doped material, w-Ni(OH)2. According to Fig. 4a, the oxidation peaks of Ni2+ to Ni3/4+ at ca. 1.45 V show a slight positive shift for the W-doped samples. These results suggest that single-atom W doping can promote carrier migration across the catalyst|solution interface and weaken the oxidation step of Ni2+. The EIS plots (Fig. 4d) support this as the charge transfer resistance, Rct is significantly lower for w-Ni(OH)2, see Table S4. The in situ Raman spectra of pristine and W-doped Ni(OH)2 was carried out to further verify this. As shown in Supplementary Fig. 20, the Raman shift peaks at ca. 440 and 493 cm−1 can be assigned to Ni(OH)2 signals, meanwhile, the peaks at ca. 477 and 550 cm−1 belong to the NiOOH18. It was deduced that the Ni(OH)2 was being oxidized to NiOOH, and the W-doped sample retained part of the Ni(OH)2 phase. This directly correlates with our previous assertion, that the doped W can assist in the migration of carriers from the catalyst to solution and weaken the oxidation effect of the electrocatalyst Ni(OH)2.
To better understand the effect of surface W sites on migrating carriers, the OER performance of the reference sample, i.e., WO3/Ni(OH)2 was also carried out. The STEM image (Supplementary Fig. 21a) clearly showed that the WO3 nanoparticles were only loaded on the Ni(OH)2 surface, not dispersed through it. Although the OER activity was a little enhanced by WO3 loading (Supplementary Fig. 21b), the oxidation potential of the peak of Ni2+ to Ni3/4+ was almost the same. This indirectly suggests that the W doping could weaken the carriers stay on Ni(OH)2. To further verify the advantage of our nanosheet sample, we also synthesized a nanoparticles sample of pure Ni(OH)2. As shown in Supplementary Fig. 22, the nanosheet sample shows a better OER performance at high current density than the reference nanoparticle material. We also tried other element doping using Nb, Mo, and Ta, and the corresponding OER performance was shown in Supplementary Fig. 23. The doped samples all exhibited enhanced activity compared with the pure Ni(OH)2 sample. However, their improved performance is limited in comparison with W element doping, suggesting that its unique electronic structure may be the reason for the enhanced performance. The specific activity of the samples is also an important parameter to suggest the intrinsic activity. The unit specific surface area values of the three catalysts (Ni(OH)2-r, w-Ni(OH)2-e, and w-Ni(OH)2) were tested to be 45, 46, and 58 m2/g, respectively. Supplementary Fig. 24 shows the corresponding specific activity. Clearly, the w-Ni(OH)2 sample still gives the best performance.
To obtain more information regarding the water oxidation process, an electrochemically active surface area (ECSA) investigation of w-Ni(OH)2 was carried out under the three pH values (pH = 13.6, 11, and 10). The characteristic CV curves of w-Ni(OH)2 with different scan rates are shown in Supplementary Fig. 25a–c. By plotting the ∆j at a certain potential against the scan rate, a linear slope that is twice the double-layer capacitance (Cdl) can be obtained, and the Cdl can be used to determine the corresponding ECSA18,19,53. For our experiment, we used a potential of 1.45 V (vs. RHE) to obtain the ECSA, the results of which are given in Supplementary Fig. 23d. The slopes at pH = 13.6, 11, and 10 are 0.01, 0.0058, and 0.0042 mF cm−2, respectively. This suggested that the Cdl at a high pH was responsible for a more electroactive surface. EIS plots of the w-Ni(OH)2 sample under the three different pH conditions were further carried out. The corresponding Nyquist plot of the pH = 13.6 solution displayed the smallest semicircular arc (Supplementary Fig. 26), followed by pH = 11 and 10, suggesting that the resistance of the HL here in a high-pH solution will return a relatively small impedance value. Moreover, the fast carriers adsorption–desorption and migration properties in the HL could also be obtained from the EIS result. To get the detailed information about the W element promoting the carriers migration in the HL of Ni(OH)2, CV curves of the reference Ni(OH)2-r and bulk w-Ni(OH)2-e samples were carried out under a pH of 13.6. As shown in Supplementary Fig. 27a and b, both of them gave typical closed curves under the different scan rates. We further calculated the Cdl, as shown in Supplementary Fig. 27c. The samples of Ni(OH)2-r and w-Ni(OH)2-e gave the slopes of 0.006 and 0.002, both of them were smaller than that of the w-Ni(OH)2 sample. This clearly suggested that the efficient property of the W-doped sample was the boosting of carrier migration across the electrode|solution interface. The turnover frequency (TOF) of Ni(OH)2-r and w-Ni(OH)2 were calculated to be 0.006 and 0.74 s−1, respectively. The W-doped sample shows a TOF 100 times higher than the pristine Ni(OH)2, seen in Supplementary Table 3, further confirming that the W doping can boost the OER activity. We also tried the practical water-splitting devices of the two-cell electrolyzer as shown in Supplementary Fig. 28. The corresponding OER performance shows the similar curves in the LSV plots, but a little high current response in the high potentials.
W-doped Ni(OH)2 OER mechanism
After the experimental characterization, density functional theory (DFT) calculations were implemented to unfold the microscopic mechanism of OER enhancement on W-doped Ni(OH)2. The six main sequential steps of water oxidation were explored:
where * represents the element of the surface reaction sites. The OER computational model (shown in Supplementary Fig. 29) adopted two layered α-Ni(OH)2 intercalated with Cl− and H2O molecules and then an edge Ni atom was substituted by a W atom. Complete OER processes on the W-doped Ni(OH)2 and Ni(OH)2 were shown in Fig. 5, in which the six reaction steps involved four electron–proton combinations43. In the case of w-Ni(OH)2 (Fig. 5a), one water molecule was adsorbed on the exposed W6+ site (State 1), and then proceeded through two deprotonation steps (State 2 and State 3) releasing energies of 0.76 eV and 0.34 eV, respectively. The adsorbed O radical then attracted one water molecule (State 4) and required 1.31 eV reaction free energy to proceed. After that, the adsorbed H2O molecule participated in O–O coupling to form *OOH (State 5) with a near-zero free uphill energy requirement. Please note that this step was different from the case of Fe-doped Ni oxyhydroxides (Ni1−xFexOOH), which are considered as the current most active non-noble electrocatalysts for OER under alkaline conditions and prefer the O–O coupling to occur at the low spin d6 Ni4+ rather than at high spin d4 Fe4+54. Whereas the low spin d0 W6+ stabilized the unpaired electron of the O and then assisted in the formation of O–O coupling. The above adjacent two steps did not then need to change their reactive sites and thereby the energy requirement was reduced. For the last step, the *OOH had to overcome a 1.67 -eV free energy barrier to achieve deprotonation into the O2 molecule (State 6), and consequently, the last step in the W-doped system is the Potential Determining Step (PDS) for OER. The overpotential was obtained based on the above results by subtracting the thermodynamic equilibrium potential (1.23 V for OER) from the highest free energy (1.67 eV) required for OER: ≅η = 1.67 eV/e −1.23 V = 0.44 V. Moreover, the spin states were also examined for the different states of the metal and intermediates as given in Table S6. Clearly, when compared with the high spin population (1.434) of Ni atom, a lower spin state of W atom was responsible for the stabilization of O–O bonding formation as discussed by Shin, Xiao, and Goddard54. As a contrast, in the case of pure Ni(OH)2, the first four states are all a result of endothermic reactions as shown in Fig. 5b, and step 4, the formation of *OOH2, is the PDS, which requires an uphill energy of 2.32 eV with a corresponding ƞ of 1.09 V. Furthermore, the O radical on Ni4+ was hard to form from State 3 to State 4, which induced an instability of O radical adsorption. The O–O–H formation (State 5) was an exothermic step and the final O–O coupling step needed an energy of 0.66 eV. The W-doped configurations, compared with bare Ni(OH)2, with a low spin population of 0.05 for the W atom showed it could stabilize the subsequent O–O coupling. As a result, the potential determining step of O radical formation on bare Ni(OH)2 is transferred to the deprotonation of *OOH. Also, the W element doped Ni(OH)2 sample gave the smallest overpotential at a relatively high current density of 80 mA/cm2 over all the Ni(OH)2-based OER catalysts in the literature. We also tried other dopant sites for W as shown in Supplementary Fig. 30. It was found that at the edge site, the dopant W is more energetically favorable than that of the interior W configuration. Note that although the PBE results cannot reproduce the exact experimental redox potentials due to the effect of the exchange-correlation functional in Ni oxyhydroxides systems, previous work showed that it has little influence on the knowledge of the concrete OER, especially at the PDS55. The K-point test of w-Ni(OH)2 systems for DFT calculations were carried out as shown in Supplementary Fig. 31. Meanwhile, we compared the dynamic processes of the PDS on w-Ni(OH)2 and Ni(OH)2 as shown in Supplementary Fig. 32. It was found that a lower kinetic energy barrier (2.05 eV) of the PDS on w-Ni(OH)2 was needed to be overcome when compared with that of PDS on pristine Ni(OH)2 (2.29 eV), meaning a faster electron transfer occurrence at this elementary step of OER. It agreed well with the steeper current response at low potential observed in the experiment.
In summary, single-atom W-doped Ni(OH)2 nanosheets were reported for the electrocatalytic water oxidation reaction. The w-Ni(OH)2 was synthesized from long-time ultrasonic exfoliation of w-Ni(OH)2-e, which was obtained via an alcohothermal method. Compared with the reference sample of pure layered Ni(OH)2, w-Ni(OH)2 gave an obvious enhanced OER performance: it only required an overpotential of 237 mV for reaching the current density of 10 mA/cm2. Moreover, at a high current density of 80 mA/cm2, the sample of w-Ni(OH)2 only needed a overpotential value of 267 mV with the corresponding Tafel slope measured to be 33 mV/dec. All the values were the best/highest level with respect to the current reported samples in the literatures. Based on DFT calculations, the w-Ni(OH)2 showed exothermic reactions for the first three steps of water oxidation: water adsorption, the formations of adsorbed OH− group and the O radical. The site of d0 W6+ stabilized the O radical owing to the low spin population of 0.05. Most significantly, the following O–O coupling step was also generated at the W6+ site, and almost-zero eV of the Gibbs free energy was further required. This effect helped the W6+ ions boost the final water oxidation reaction of Ni(OH)2. This work can help us understand the effect of the HL on the water oxidation and provide a new direction to design doped OER catalysts.
Synthesis of pure Ni(OH)2-r
The Ni(OH)2 was prepared through an alcohothermal method. Typically, 0.4 g of NiCl2 was added into a 40 -mL ethanol solution. The mixture was stirred until a transparent solution was observed. The solution was then moved into a 50 -mL autoclave. The autoclave was then placed into an oven and treated in flowing air and heated at 150 °C for 12 h. Green powder of Ni(OH)2 was treated by 24 h ultrasound in an ethanol solution and then was collected by centrifuging the reaction mixture at a speed of 9000 r.p.m. for 10 min. The product was washed by water and ethanol four times and then was dried at 80 °C overnight. The obtained pure Ni(OH)2 was used as the reference sample and named as Ni(OH)2-r.
Synthesis of w-Ni(OH)2-e
The w-Ni(OH)2-e was prepared through an alcohothermal method. At first, 1 g of WCl6 was added into 100 mL of ethanol to form a transparent solution. Then a certain amount of WCl6–ethanol solution was added into the NiCl2–ethanol solution (0.4g–40mL) by a pipette. After stirring for 15 min, the mixture was moved into a 50 -mL autoclave, which was then treated at 150 °C for 12 h in an oven. The product was collected by centrifuging the reaction mixture at a speed of 9000 r.p.m. for 10 min. After that, the powder was washed by water and ethanol four times and then dried at 80 °C overnight. The obtained W-doped Ni(OH)2 sample was named as w-Ni(OH)2-e.
Synthesis of w-Ni(OH)2
The w-Ni(OH)2 was prepared through the exfoliation of the w-Ni(OH)2-e sample. Typically, 0.1 g of w-Ni(OH)2-e was added into 40 mL of ethanol and then the mixture was treated by ultrasound for 24 h. After that, the product was collected by centrifuging at a speed of 9000 r.p.m. for 10 min. The powder was washed by water and ethanol four times and then dried at 80 °C overnight. The obtained sample was named as w-Ni(OH)2.
Transmission electron microscopy (TEM) was performed on a FEI Tecnai G2 F20 electron microscope at an acceleration voltage of 200 kV. Spherical aberration-corrected electron microscopy was carried out on a JEM-ARM200F electron microscope. The field-emission scanning electron microscopy (FESEM) was observed under a SU8020 electron microscopy. X-ray diffraction (XRD) patterns of the samples were recorded on a Rigaku Smartlab-9kW instrument using Cu Kα X-ray (λ = 1.54186 Å) radiation at a scanning rate of 4 o/min in the region of 2θ = 10–80o. X-ray photoelectron spectra (XPS) was acquired on a Kratos Axis Ultra DLD spectrometer with Al Kα (hυ = 1486.6 eV) as the excitation source. Fourier transform infrared reflectance (FTIR) and the Quasi FTIR spectra of samples were carried out on a Bruker V70 spectrometer. Diffuse reflectance ultraviolet–visible (UV–Vis) spectra of the studied samples were recorded in the air against BaSO4 in the region of 200–800 nm on a Perkin–Elmer Lambda 950 spectrophotometer. Raman analysis was carried out on a Renishaw InVia Raman spectrometer with a green line of an Ar-ion laser (514.53 nm) in micro-Raman configuration. XAFS experiments were performed at the 1W1B beamline of the Beijing Synchrotron Radiation Facility (BSRF). The storage ring runs at 2.0 GeV with a maximum electron current of about 450 mA. The energy range of the incident X-ray is tunable from 4 to 25 keV by fix-exit Si (111) double-crystal monochromator. The absorption edge of standard metal foils was used to calibrate the X-ray energy. Samples were ground into fine powers and then pressed into thin disks of 10 mm in diameter. W L3-edge XANES/EXAFS spectra were collected at room temperature in transmission mode. The data were processed using the IFEFFIT package56.
OER electrode preparation
For the three samples studied and the reference RuO2, the preparation method was the same. Typically, 10 mg of the sample was added into a 50 μL of isopropanol and then 50 μL of nafion (Nafion 117 solution, Sigma-Aldrich) was dispersed into the solution. The mixture was first treated by the strenuous vibration of an oscillator. After that, the mixture was treated by ultrasound ca. 10 h to form the uniform ink, which was then dropwise applied onto glassy carbon electrodes with a mass loading of 0.2 mg cm−2. The prepared electrodes were naturally dried in air. For all the samples, four electrodes were prepared and the near results were used in our paper.
All of the electrochemical tests were performed at room temperature with the use of a typical three-electrode setup. The Pt (1 cm2) and Hg/HgO (1 M KOH) electrodes were used as the counter and reference electrodes, respectively. In all, 1 M KOH solution was used as the electrolyte. The electrocatalytic measurements were carried out on a Zennium Zahner electrochemical workstation. The measured potentials versus Hg/HgO were converted to the reversible hydrogen electrode (RHE) scale according to the following Nernst equation: ERHE = EHg/HgO + 0.059 pH + EoHg/HgO, where ERHE is the converted potential versus RHE, EoHg/HgO = 0.098 at 25 °C, and EHg/HgO is the experimentally measured potential against the Hg/HgO reference. Before the test, the as-prepared anodes were activated by a chronopotentiometry scan with the 30 mA cm−2 current density for 2 h. The Tafel slopes were obtained from the polarization curves by plotting overpotential against log(current density). The steady-state activity was evaluated by chronopotentiometry measurements under different potentials. The ECSA was determined by measuring the capacitive current associated with double-layer charging from the scan rate CV-dependence. In our present work, the CV potential window was chosen to be 1.35 to 1.55 vs. RHE. The scan rates were 20, 40, 60, 80, and 100 mV s–1. The double-layer capacitance (Cdl) was estimated Δj = (jcharge–joff charge) at 1.45 V vs. RHE against the scan rate. The linear slope is twice of the double-layer capacitance Cdl. EIS measurements were carried out after the OER tests under the different potentials. The ZSim Demo software was used to fit the EIS results. The TOF was calculated using the below equation:17,18
where J (A cm−2) is the current density at a given overpotential (e.g., η = 250 mV), S is the surface area of the electrode (0.072 cm2), F is the Faraday constant (96,485 C mol−1), and n is the number of moles of reactive metal on the electrode. The μ is the Faradaic efficiency, which was determined from the total amount of charge Q (C) passed through the cell and the total amount of the produced O2, nO2 (mol): Faradaic efficiency = 4 F*nO2/Q, assuming the four electrons are needed to produce one oxygen molecule. Please note, we calculated the μ value to be ca. 100%. The metal content of Ni(OH)2 (55 wt.% Ni) and w-Ni(OH)2 (60 wt.% Ni and 5.5 wt.% W) was quantified by ICP–MS33. For the TOF calculation, the Ni and W are supposed to be the active sites for pure Ni(OH)2 and W-doped Ni(OH)2 samples, respectively.
All density functional theory calculations were realized by the Vienna ab initio simulation package (VASP)57. The exchange-correlation functional adopted the expression of Perdew–Burke–Ernzerhof (PBE) in the generalized gradient approximation (GGA) method58. Meanwhile, the Grimme method (DFT-D2)59 was introduced to consider the weak van der Waals’ interaction. The self-consistent calculations of single-electron wavefunction at ground state were terminated when the iterative convergence of energy and force fulfilled 10–5 eV and 0.01 eV/Å, respectively. Overall, 1 × 1 × 5 K-points mesh with a Gamma-centred Monkhorst-Pack scheme was sampled in the corresponding Brillouin zone on the reciprocal space (Fig. S28). A 15 Å lattice constant along the z-axis was set to avoid the layer image coupling caused by the periodic model. The detailed calculation results i.e., atomic Cartesian positions can be found in Table S5. Based on the standard hydrogen electrode model proposed by J. K Nørskov60, the Gibbs free energy change ΔG of oxygen evolution reaction (OER) on Ni(OH)2 and w-Ni(OH)2 were evaluated by the formula:
where ΔE is the adsorption energy of OER intermediates and ΔZPE is their corresponding zero-point energy. The entropy contribution is simplified into its vibrational entropy of OER intermediates. Herein, although the PBE results cannot reproduce the exact experimental redox potentials due to the effect of the exchange-correlation functional in Ni oxyhydroxides systems, previous work showed that it has little influence on the knowledge of the concrete OER, especially at the PDS55. In order to determine the dynamic processes at the potential determining step, the climbing image nudged elastic band (CI-NEB)61 method was adopted to calculate the energy barriers of the transition state.
The data that support the findings of this study are available on request from the corresponding authors.
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We thank the support from National Key Research Program of China (2017YFA0204800, 2016YFA0202403), Natural Science Foundation of China (No. 21603136), the National Science Basic Research Plan in Shaanxi Province of China (2017JM2007), the Changjiang Scholar and Innovative Research Team (IRT_14R33). The 111 Project (B14041), the Fundamental Research Funds for the Central Universities (GK201602007, 2018CSLZ011), Thousand Talents Program of China, Pan Deng Scholars Program of Liaoning Province, Science and Technology Innovative Talents Support Program of Shenyang (RC180166), Australian Research Council (ARC) through Discovery Early Career Researcher Award (DE150101306), and Linkage Project (LP160100927). The XAFS beam time was granted by the 1W1B beamline of Beijing Synchrotron Radiation Facility, Institute of High Energy Physics, Chinese Academy of Sciences. The authors would like to thank the staff of 1W1B for their technical support in XAFS measurement and guidance for the data analysis.
The authors declare no competing interests.
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Yan, J., Kong, L., Ji, Y. et al. Single atom tungsten doped ultrathin α-Ni(OH)2 for enhanced electrocatalytic water oxidation. Nat Commun 10, 2149 (2019). https://doi.org/10.1038/s41467-019-09845-z
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