Ternary nickel–tungsten–copper alloy rivals platinum for catalyzing alkaline hydrogen oxidation

Operating fuel cells in alkaline environments permits the use of platinum-group-metal-free (PGM-free) catalysts and inexpensive bipolar plates, leading to significant cost reduction. Of the PGM-free catalysts explored, however, only a few nickel-based materials are active for catalyzing the hydrogen oxidation reaction (HOR) in alkali; moreover, these catalysts deactivate rapidly at high anode potentials owing to nickel hydroxide formation. Here we describe that a nickel–tungsten–copper (Ni5.2WCu2.2) ternary alloy showing HOR activity rivals Pt/C benchmark in alkaline electrolyte. Importantly, we achieved a high anode potential up to 0.3 V versus reversible hydrogen electrode on this catalyst with good operational stability over 20 h. The catalyst also displays excellent CO-tolerant ability that Pt/C catalyst lacks. Experimental and theoretical studies uncover that nickel, tungsten, and copper play in synergy to create a favorable alloying surface for optimized hydrogen and hydroxyl bindings, as well as for the improved oxidation resistance, which result in the HOR enhancement. The lack of efficient and cost-effective catalysts for H2 oxidation reaction (HOR) hinders the application of anion exchange membrane fuel cells. Here, authors report a ternary nickel-tungsten-copper nanoalloy with marked HOR activity and stability that rivals the benchmark platinum catalyst.

O ver the past 30 years, the proton exchange membrane fuel cell (PEMFC) technology has developed rapidly, resulting in the first commercial sales of fuel-cell powered cars in 2015 (ref. 1 ). Although great success, the mass market penetration by such zero-emission vehicles is currently hindered by the absence of inexpensive materials to replace costly platinum (Pt)based catalysts, which are responsible for~46% of the stack cost 2 . Extensive research has been conducted using various strategies to reduce the Pt loading [3][4][5] , but the acidic environment largely constrains the choice of catalytic materials that perform stably in PEMFCs. This shortcoming can be overcome by switching the operating environment from an acid to alkaline one-the resultant anion exchange membrane fuel cells (AEMFCs) allow for the use of platinum group metal-free (PGM-free) catalysts, thus enabling significant cost reduction 6 . Indeed, some PGM-free materials have been observed to catalyze the oxygen reduction reaction (ORR) comparable to Pt for the AEMFC cathode [7][8][9][10] . However, at the AEMFC anode, the activity of the hydrogen oxidation reaction (HOR) on Pt is inherently slower by~100 times than that in acidic environment 11,12 , which demands much higher Pt loadings (0.4 mg Pt cm −2 at AEMFC anode versus 0.03 mg Pt cm −2 at PEMFC anode) to reach similar fuel cell performance 13 . At present, the lack of highly active and stable PGM-free HOR catalysts in alkaline environments hampers the progress towards the AEMFC implementation 14 .
Substantial effort has been devoted to searching HOR catalysts composed solely of earth-abundant elements, whereas PGM-free catalysts that show HOR activity in alkali are rather rare 15 . Nickel (Ni)-based compounds are currently the materials with the most promise as catalysts that drive the HOR in alkaline environments 16 . In 1960s, Raney Ni was first explored as HOR catalyst in liquid alkaline fuel cells under extreme alkalinity (6M KOH), but its activity was very low [17][18][19] . Since then, the HOR performance of Ni-based catalysts has been gradually improved via diverse methods, yielding catalysts such as CoNiMo 20 , MoNi 4 and WNi 4 21 , NiMo/C 22 , Ni/NiO/C 23 , Ni/N-doped carbon nanotubes 13 , CeO 2 /Ni heterostructures 24 , Cr-modified Ni 25 , and Ni 3 N nanoparticles 26,27 . Despite marked progress, many of these Ni-based HOR catalysts deactivate quickly above 0.1 V versus reversible hydrogen electrode (RHE) owing to the formation of surface hydroxides 28 . To generate adequate power density, however, HOR catalysts should remain stable to at least 0.3 V versus RHE 2 , which could also largely mitigate the risk of passivation of the stack under transient conditions. Unfortunately, there is no PGM-free HOR catalyst with operating stability up to 0.3 V versus RHE has been reported thus far.
Here we report that Ni 5.2 WCu 2.2 nanotubes (NTs)-a ternary nickel-tungsten-copper alloy-can catalyze the HOR in alkaline electrolyte highly efficient and stable. We find that the Ni 5.2 WCu 2.2 catalyst achieves higher HOR activity than a commercial Pt/C counterpart. Importantly, stability window up to 0.3 V versus RHE was realized on this catalyst. At this potential, a considerable current density of 16.5 mA cm −2 could be held over 20 hours without notable decay. Moreover, this alloyed catalyst also exhibits high tolerance to 20,000 ppm CO impurity. The extraordinary efficiency of Ni 5.2 WCu 2.2 exceeds that of previously reported PGM-free HOR catalysts.

Results
Synthesis and characterization of catalyst. Very recently, our group has reported bimetallic MoNi 4 and WNi 4 nanoalloys with notable activity toward the alkaline HOR, but such binary alloys lose activity above 0.2 V versus RHE owing to the surface oxidation 21 . Previous studies suggested an alloying-based approach for improved stability of catalysts by tuning the microstructures of the host metals [29][30][31][32] . For examples, alloying Mo with Pt 3 Ni (111) can mitigate the Ni leaching during electrochemical process, enabling greatly enhanced ORR stability 31 . Chorkendorff et al. identified that alloys of Pt and rare earths are stable ORR catalysts because of their very negative alloying energy E a that limits dissolution 32 . We thus seek to widen the stability window of binary Ni-W catalyst through alloying with additional element to form new structure that resists surface oxidation during HOR operation. Prior studies have shown that HOR activity and stability can be improved largely in alkaline electrolytes when using Cu to partially replace noble metals (e.g., PdCu nanoparticles 33 and Pt/Cu nanowires 34 ). Moreover, Dekel et al. reported that Cu in alloys often dissolves at higher anode potentials as compared to other metals such as Mo 28 . We thus speculate that Cu may play an important role in enhancing the HOR activity and stability. Hence, we decide to introduce Cu to form ternary Ni-W-Cu alloy and explore its alkaline HOR property.
To synthesize the catalyst, Cu foam was immersed in 1M KOH for an anodization process to grow Cu(OH) 2 (Fig. 1a). This simple synthetic approach provides good scalability. We synthesized a 3 cm × 10 cm Ni-W-Cu alloy foam by using scaled-up reactors, which shows good fidelity of the product, implying a potential industry-level use ( Fig. 1b and Supplementary Fig. 5).
The achieved electrode consists of numerous uniform Ni-W-Cu alloy nanofibers with length up to 10 μm when imaged by scanning electron microscopy (SEM) ( Fig. 2a and Supplementary  Fig. 6). Each fiber possesses a very rough surface that is made up of whiskerette particles. Low-resolution transmission electron microscopy (TEM) unveils that the center of a representative fiber appears brighter, demonstrating that it is hollow (Fig. 2b). The formation of hollow-fibers was caused by the outward diffusion of Cu in the NiW-Cu(OH) 2 precursor to produce Ni-W-Cu alloy during annealing process. Selected-area electron diffraction (SAED) analysis of a whisker reveals its high-crystalline structure (Up inset in Fig. 2b), which agrees with our atomic-resolution high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) result that shows continuous lattice fringes without surface defects (Down inset in Fig. 2b). In Fig. 2c, the STEM measurements reveal that alloyed whiskerette particles bounded closely to form distinct grain boundaries. Energydispersive X-ray (EDX) spectrum elemental mapping displays a uniform, uncorrelated spatial distribution of Ni, W, and Cu ( Fig. 2c and Supplementary Fig. 7). The weak O signal could originate from the adsorbed O and slight surface oxidation when exposing the sample in the air ( Supplementary Fig. 8).
We performed X-ray diffraction (XRD) measurements of the collected Ni-W-Cu alloy powder and observed a high-crystallinity face-centred cubic structure (Fig. 2d). Compared to (111), (200), and (220) reflections of Ni nanoparticles, the diffraction peaks are shifted to lower angles in Ni-W-Cu alloy, indicating a higher lattice parameter caused by the addition of atoms with larger radius. Using similar synthetic method, we also prepared Ni-W alloy with cubic Ni 17 W 3 phase ( Fig. 2d and Supplementary  Fig. 9), whose diffraction peaks sit between those of Ni nanoparticles ( Fig. 2d and Supplementary Fig. 10) and Ni-W-Cu alloy. Given that the atomic radius follows the sequence of Ni < Cu < W, we predict more W atoms in Ni-W-Cu than in Ni 17 W 3 . Our inductively coupled plasma atomic emission spectroscopy (ICP-AES) analysis gives a Ni:W:Cu ratio of 5.2:1:2.2 for Ni-W-Cu alloy, which agrees well with EDX measurements and confirms our speculation. Thereafter, we assign the obtained ternary alloy as Ni 5.2 WCu 2.2 .
Alloying-based design has been demonstrated to alter catalytic properties by modulating the electronic structures of host and alloyed metals, leading to a cooperative interplay that tunes the adsorption energies of critical intermediates for enhanced catalytic reactivity [35][36][37] . We probed the work function of Ni 5.2 WCu 2.2 , Ni 17 W 3 and Ni catalysts by Kelvin probe force microscopy 38,39 (KPFM; Supplementary Fig. 11). A clean highly oriented pyrolytic graphite (HOPG) with work function value of 4.6 eV was used as a reference 39 . Figure 2e presents the measured surface potentials for the studied samples, which correspond to a work function value of 4.54 for Ni 5 Fig. 2e), consistent with our calculated results ( Supplementary Fig. 12). The lower work function of Ni 5.2 WCu 2.2 suggests its modified electronic structure that allows for a faster electron transfer and thus enhanced catalytic ability 40 . To reveal the impact of ternary alloy effect on the chemical and structural environments of Ni, we performed the X-ray absorption spectroscopy. Figure 2f shows the X-ray absorption near-edge spectroscopy measurements of the Ni Kedge from Ni 5.2 WCu 2.2 , Ni 17 W 3 , and freshly-prepared Ni samples, as well as that from a Ni foil used for comparison. Adsorption features that are present in the spectra of our freshlyprepared Ni and Ni foil reference are similar. By contrast, a substantial increase in the white lines was observed for Ni 5.2 WCu 2.2 and Ni 17 W 3 , indicating electron donation from Ni to W and Cu upon alloying 41 . We probed the radial structure function around Ni by Fourier transform (FT) of extended X-ray absorption fine-structure (EXAFS) spectra (Fig. 2g Table 1). We surmise the lower coordination number attributable to the highly nanostructured hollow structure of Ni 5.2 WCu 2.2 , and estimate that more active sites exist on the ternary alloy that would modify the adsorption ability of HOR intermediates.
Evaluation of HOR performance. We evaluated HOR activity and stability of the ternary Ni 5.2 WCu 2.2 alloy in a standard threeelectrode setup ( Supplementary Fig. 15), using H 2 -saturated 0.1 M aqueous KOH as the electrolyte. The working electrode cuts from large-area Ni 5.2 WCu 2.2 monolith with a geometric surface area of 1 cm 2 (catalyst loading:~9.2 mg cm −2 ). Reference measurements of Ni 17 W 3 , Ni, and commercial Pt/C (20 wt%) catalysts were similarly performed for comparison. We used a slow sweep rate of 1 mV s −1 to minimize the capacitive contribution and to guarantee a steady-state measurement. Unless otherwise stated, all electrochemical data were measured without electrode rotation and were iR-corrected (i, current; R, resistance) for the uncompensated Ohmic drop.
As shown by the linear sweep voltammetry (LSV) curve of Ni 5.2 WCu 2.2 in 0.1 M KOH, the onset potential for generating HOR current is as low as 0 V versus RHE, beyond which a sharp increase in anodic current was observed, demonstrating its exceptional energetics for HOR (Fig. 3a). By contrast, Ni 5.2 WCu 2.2 gives almost no current-voltage feature in 0.1 M KOH saturated by Ar ( Supplementary Fig. 16), further confirming that HOR catalysis occurs on this alloy catalyst. Figure 3a also shows that Ni 5.2 WCu 2.2 can reach a diffusion-limiting HOR current density of~20 mA cm −2 , whereas Ni 17 W 3 exhibits much inferior HOR activity and the single Ni is almost HOR inactive. Remarkably, the Ni 5.2 WCu 2.2 catalyst even surpasses the commercial Pt/C catalyst from the kinetic to diffusion-limiting regions. We note that no rotation was applied to our bulky electrodes, suggesting that the Levich equation would not take effect 43 . As a result, the measured diffusion-limiting HOR currents on different catalysts deviate from the theoretical value. We measured a half-wave potential of 39 mV for Ni 5  impedance spectroscopy measurements that yield a small charge transfer resistance of~3.0 Ohms at 30 mV overpotential ( Supplementary Fig. 17).
In Fig. 3a Fig. 3a), which correspond to the formation of Ni(OH) 2 (ref. 44 ). The limited tolerance to anode overpotentials poses significant risk of passivation under high current operation, leading to unsatisfied power output 2 . The stability window up to 0.3 V versus RHE for our Ni 5.2 WCu 2.2 catalyst has not yet been achieved on previous PGM-free HOR catalysts (Fig. 3b), which would largely mitigate the risk of passivation under transient conditions.
We now extract the exchange current density (j 0 )-the most inherent measure of HOR activity-of various catalysts from linear fitting of micro-polarization regions (−5 to 5 mV; Supplementary  Fig. 18). The geometric j 0 of 11.36 mA cm −2 for Ni 5 Table 2 and Methods). To further quantify the intrinsic HOR activity, the j 0 is renormalized by the electrochemical active surface area (ECSA; see "Methods", Supplementary Fig. 19 and Table 3 for  details), yielding a value of 0.014 mA cm −2 for Ni 5.2 WCu 2.2 , which is 1.96 times higher than Ni 17 W 3 and 4.31 times higher than Pt/C catalyst (Fig. 3c). We also carried out the feed ratio-, temperature-, and time-dependent control experiments and unveiled that the optimized HOR activity was obtained on Ni-W-Cu alloy that was synthesized with Ni:W atomic ratio of 4:1 and then annealed at 500°C for 1 h (Supplementary Figs. 20-24). We next report that our ternary Ni 5.2 WCu 2.2 alloy shows good resistance to CO poisoning. It is well known that PGM catalysts (such as Pt) are poisoned very rapidly in the presence of CO because of its preferential adsorption on Pt that blocks the active sites 45 . In Fig. 3e, we find that the Pt/C catalyst loses HOR activity completely with 20,000 ppm CO in the H 2 fuel. By stark contrast, the Ni 5.2 WCu 2.2 catalyst can retain high HOR activity with the same level of CO contamination, exhibiting its remarkable COtolerant ability. Besides, our results further show that the HOR activity decreases on both Ni 5.2 WCu 2.2 and Pt/C catalysts when having 20,000 ppm CO 2 in the H 2 fuel (Supplementary Fig. 25). The detailed poison mechanism is unclear and needs further investigations.
Apart from activity and CO tolerance, another critical metric for the application of Ni 5.2 WCu 2.2 alloy as a PGM-free anode is the long-term stability-especially the stability at high anode potentials. To assess this, we performed two sets of stability tests on our Ni 5.2 WCu 2.2 alloy catalyst. We first performed accelerated durability tests (ADT) by applying linear potential sweeps between −0.2 and Fig. 3 (Fig. 3f), implying that Ni 5.2 WCu 2.2 alloy has stability better than Pt/C catalyst. Then, we evaluated the ability of Ni 5.2 WCu 2.2 alloy to continuously catalyze the HOR using chronoamperometry (j~t) at a high anode potential of 0.3 V versus RHE. As shown in Fig. 3g, the current density (~20 mA cm −2 ) generated from Ni 5.2 WCu 2.2 decreases to 16.5 mA cm −2 after 2 h, followed by slow degradation over the next 18 h. This degradation was likely caused by selective W leaching (Supplementary Fig. 26). By contrast, Pt/C catalyst delivers a current density of mere 10 mA cm −2 at the beginning, which decreases progressively to about 4.3 mA cm −2 over a 20 h of operation. After aggressive stability tests, the crystal phase, structure and composition of the Ni 5.2 WCu 2.2 alloy remained almost unchanged ( Supplementary Figs. 27-29), whereas Pt/C catalyst suffered from agglomeration and even detachment of Pt nanoparticles ( Supplementary Fig. 30). These results reveal superior HOR stability of Ni 5.2 WCu 2.2 alloy compared with Pt/C catalyst.
Surface structure and chemistry of catalyst. The formation of a ternary Ni 5.2 WCu 2.2 alloy enables a HOR catalyst that shows high activity and stability at large anode potential, as well as good resistance to CO poisoning. In this section, we study the structural and chemical characters that affect and determine these performances. X-ray photoelectron spectroscopy (XPS) analysis of the studied samples showed that Ni, Ni 17 W 3 , and Ni 5.2 WCu 2.2 are all metallic in nature with certain surface oxidation ( Fig. 4a  and b). We note that some degree of surface oxidation is nearly inevitable when these Ni-based compounds are exposed to air, analogous to our previous observation 21 . XPS measurements also revealed that the Ni 2p binding energies of Ni 5.2 WCu 2.2 shifted 0.3 eV to higher energy with respect to Ni 17 W 3 (Fig. 4a). Meanwhile, the W 4f XPS of Ni 5.2 WCu 2.2 showed a shift of the W core levels to lower binding energies compared with Ni 17 W 3 (Fig. 4b).
These results indicated electron donation from Ni to W once Cu participate in the alloy, leading to modulated electronic structure. Our Bader analyses further confirm such charge redistribution after incorporating Cu into the alloy structure ( Supplementary  Fig. 31).
To further probe the surface features, we conducted COstripping (CO electrooxidation) experiments on Ni 17 W 3 and Ni 5.2 WCu 2.2 with Pt/C catalyst as a reference. Results shown in Fig. 4c display that the oxidation of adsorbed CO (CO * ) occurs at 0.69 V for Pt/C catalyst, which is in agreement with prior reports 46 . By contrast, Ni 17 W 3 oxidizes CO * at a much lower potential of 0.48 V, and Ni 5.2 WCu 2.2 has a CO-stripping peak located in the middle (0.62 V). These results indicate that both Ni 17 W 3 and Ni 5.2 WCu 2.2 have a much lower CO adsorption ability compared with the Pt/C catalyst, leading to the good COtolerance property observed in Fig. 3e. Moreover, in alkaline electrolytes, because the OH adsorption can facilitate the removal of the CO * (ref. 47 ), our CO-stripping results thus offer additional surface information that Ni 17 W 3 and Ni 5.2 WCu 2.2 possess stronger OH adsorption than Pt/C catalysts following the order of Ni 17 W 3 > Ni 5.2 WCu 2.2 > Pt/C. Surface analysis of the studied samples was also carried out using cyclic voltammetry in 0.1 M KOH electrolyte that saturated by Ar and H 2 , respectively. At a large sweep rate of 50 mV s −1 , the oxidation curve of Ni 5.2 WCu 2.2 appears at higher anode potential than that of Ni and Ni 17 W 3 (Fig. 4d), suggesting its superior oxidation-tolerant ability 27 . Intriguingly, we find that the oxidation peak of Ni 5.2 WCu 2.2 in H 2 -saturated 0.1 M KOH exhibits a 58 mV positive shift relative to that in Ar-saturated 0.1 M KOH (Fig. 4d). Similar positive shifts were also observed on Ni (45 mV) and Ni 17  Computational studies. With these experimental information in hand, we now turn to perform density functional theory (DFT) to gain fundamental insight into mechanisms responsible for the excellent activity and stability, as well as the good CO-tolerance property (see Methods). We constructed and optimized crystal models of Ni 5.2 WCu 2.2 (111), Ni 17 (Fig. 5a). These results predict that the oxidation of Ni 5.2 WCu 2.2 is more difficult to occur as compared to Ni and Ni 17 W 3 (refs. 48,49 ), consistent with our experimentally observed HOR stability at higher anode potential. Additionally, our DFT simulations reveal that Pt possesses a much higher CO adsorption strength (−1.78 eV) than that of Ni 17 W 3 (−1.42 eV) and Ni 5.2 WCu 2.2 (−1.55 eV) (Fig. 5b), which explain the marked COtolerance ability of Ni 5.2 WCu 2.2 and agree well with above COstripping trend (Fig. 4c).
Although the HOR mechanism in alkaline electrolytes is still debated 6,50-52 , recent research has gradually led to agreement that hydrogen binding energy (HBE) and OH binding energy (OHBE)/oxophilicity both serve as descriptor for HOR performance 27,50,53 . With DFT calculations (Fig. 5c), we revealed that although the HBE of Pt(111) is optimum, whereas the adsorption energy of OH is too weak on Pt(111). As to Ni(111) facet, the HBE value is −0.58 eV, which means a too strong Hbinding that hampers HOR catalysis, agreeing with previous study 23  promote the HOR kinetics. We also computed the HBE and OHBE of Ni 17 W 3 for comparison (Fig. 5c). Despite this catalyst exhibits stronger OHBE than Pt(111), its HBE is unfortunately strong, thus showing inferior HOR activity. The optimized HBE and OHBE that enabled by the synergy of Ni, W, and Cu in the ternary alloy can be further verified by our projected density of states (PDOS) analyses ( Supplementary Fig. 37).
We note that our theoretically predicted trend of OH adsorption and CO adsorption perfectly match with COstripping results (Fig. 4c). Moreover, the free energy diagrams that we computed for the reaction pathways on various catalysts are presented in Fig. 5d contributes to its exceptional HOR performance. Altogether, our experimental and computational studies reveal that the synergy among Ni, W, and Cu-a multiple-element alloying effect-enables the optimized HBE and OHBE that improve the energetics for HOR, as well as the wide stability window up to 0.3 V versus RHE.

Discussion
To conclude, this work demonstrates a multiple-element Nibased alloy strategy for creating HOR catalyst that makes use of earth-abundant elements, showing exceptional activity and stability in alkaline electrolyte. This notable HOR performance can be explained by the alloying effect among nickel, tungsten and copper, which work in synergy to enable optimized hydrogen and hydroxyl bindings, as well as the improved resistance against surface oxidation. Our study calls for further exploration of multiple-element alloys composed of other cheap metals, thereby aiding the development of more efficient HOR catalysts for AEMFC anodes.

Methods
Synthesis of Cu(OH) 2 nanowires on Cu foam. The Cu(OH) 2 NWs were grown on commercial Cu foam via a simple anodization method. Prior to the growth of nanowires, a piece of Cu foam (1 cm × 3 cm) was ultrasonically cleaned by hydrochloric acid solution, ethanol and deionized water, respectively, which was then immersed into a two-electrode system using Pt foil as the counter electrode in 1 M NaOH solution. The anodization was carried out at a constant current of 60 mA for 20 min to obtain Cu(OH) 2 nanowires on Cu foam. Material characterizations. The obtained samples were examined by multiple analytic techniques. Optical microscope images were obtained with a polarizing microscope (Leica DM2700P, Germany) equipped with a Leica MC190 HD camera. The morphology of the samples was determined by SEM (Zersss Supra 40) and TEM (JEOL 2010F(s)). The STEM and HRTEM images, and EDX elemental mappings were taken on JEMARM 200 F Atomic Resolution Analytical Microscope with an acceleration voltage of 200 kV. The KPFM characterization was carried out with Atom Force Microscope (Dimension Icon). ICP-AES data was obtained by an Optima 7300 DV instrument. XRD was performed on a Japan Rigaku DMax-γA X-ray diffractometer with Cu Kα radiation (λ = 1.54178 Å). XPS was taken on an X-ray photoelectron spectrometer (ESCALab MKII) with an X-ray source (Mg Kα hυ = 1253.6 eV).
XAFS measurements. The XAFS spectra (Ni K-edge) were collected at 1W1B station in Beijing Synchrotron Radiation Facility (BSRF). The storage rings of BSRF were operated at 2.5 GeV with an average current of 250 mA. Using Si(111) double-crystal monochromator, the data collection was carried out in transmission/fluorescence mode using ionization chamber. All spectra were collected in ambient conditions. The k 3 -weighted EXAFS spectra were obtained by subtracting the post-edge background from the overall absorption and then normalizing with respect to the edge-jump step. Subsequently, k 3 -weighted χ(k) data of Ni K-edge were Fourier transformed to real (R) space using a hanning windows (dk = 1.0 Å −1 ) to separate the EXAFS contributions from different coordination shells. To obtain the quantitative structural parameters around central atoms, least-squares curve parameter fitting was performed using the ARTEMIS module of IFEFFIT software packages 54 .
Electrochemical measurements. A standard three-electrode set-up was applied to perform the HOR electrochemical measurements on the VSP-300 Potentiostat (Bio-Logic, France). Carbon rod was used as the counter electrode and all potentials were measured against an Ag/AgCl reference electrode (saturated in 3.0 M KCl) and converted to the RHE reference scale using following equation: Eðvs: RHEÞ ¼ Eðvs: Ag=AgClÞ þ 0:197 þ ð0:059 pHÞ ð 1Þ The as-synthesized Ni 5.2 WCu 2.2 , Ni 17 W 3 and Ni catalysts on Cu foam were directly used as working electrodes. After the annealing process, they were cut into 1 cm × 1 cm pieces for electrochemical tests. The commercial Pt/C was coated on a pure Cu foam (1 cm × 1 cm) with optimized loading of 1.5 mg cm −2 (Supplementary Fig. 38). Before HOR measurements, the electrolyte (0.1 M KOH) was bubbled with H 2 gas for at least 30 min. The EIS measurement was performed at 30 mV overpotential and an amplitude of the sinusoidal voltage of 5 mV (frequency range: 100 kHz to 40 mHz). All the linear sweep voltammetry (LSV), cyclic voltammetry (CV), and chronoamperometry (CA) curves were iR-corrected.
The exchange current density (j 0 ) can be obtained by fitting kinetic current density (j k ) versus the overpotential (η) using the following Butler-Volmer equation: where α is the charge transfer coefficient, η is the overpotential, R is the ideal gas constant (8.314 J mol −1 K −1 ), T is the experimental temperature (298 K), and F is the Faraday's constant (96,485 C mol −1 ). CO stripping was performed by holding the electrode potential at 0.1 V versus RHE for 10 min in the purged CO to adsorb CO on the metal surface, followed by Ar purging for another 30 min to remove residual CO in the electrolyte. The CO stripping current was obtained via cyclic voltammetry in a potential region from 0 to 1.2 V at a sweep rate of 20 mV s −1 .
DFT calculations. We carried out DFT calculations using the Vienna ab initio simulation package (VASP) 55,56 program with projector augmented wave (PAW) 57,58 method. The Perdew-Burke-Ernzerhof (PBE) 59 generalized gradient approximation (GGA) exchange-correlation functional was used throughout. A 500 eV plane-wave kinetic energy cutoff was chosen, and a 5 × 5 × 1 Monhorst-Pack k-point sampling was adopted for the structure relaxation. The convergence criterion for the electronic self-consistent iteration was set to be 10 −4 eV. A residual force threshold of 0.02 eV Å −1 was set for geometry optimizations. The calculations were conducted on (111) surface of Ni, Ni 17 W 3 , Ni 5.2 WCu 2.2 , and Pt models. Hubbard U corrections were applied to transition metal d-electrons and the values of U-J parameters for Ni (3.80), W (6.20) and Cu (3.08) atoms were taken from the references [60][61][62] . The vacuum layer was set to be 15 Å to ensure the separation between slabs.
The key reaction steps in alkaline HOR: *H þ OH À ! *H þ *OH þ e À ð4Þ The Gibbs free energy changes are calculated as follows: ΔG 1 ¼ Gð*HÞ þ GðH 2 OÞ À Gð*Þ À GðOH À Þ À GðH 2 Þ ð 7Þ The G values are calculated by: E DFT is the total energy from the DFT calculation. E ZPE is the zero-point energy, S is the entropy and T is the temperature (298 K).
The adsorption energies (ΔE ad ) for O and CO were calculated by the following equations: The O adsorption energies were calculated by: The CO adsorption energies were calculated by: The HBE and OHBE can be calculated by following equations: The HBE were calculated by: The OHBE were calculated by: Note: E O@cat. , E CO@cat. , E H@cat. , and E OH@cat. represent the energies of metals or alloy slabs with the adsorbed O, CO, H, and OH species; the E cat. , E O , E CO , E H , and E OH represent the energies of the metals or alloys slabs, the O atoms, the CO species, the H atoms, and OH species, respectively. Since the ground state of O 2 molecule is poorly described by DFT calculations, we thus used gas-phase H 2 O and H 2 as references to calculate the E O (E O = E H2O -E H2 ). As to the E OH , it can be obtained by E OH = E H2O -1/2 E H2 . We calculated the Gibbs free energy changes of G(OH − ), G(H 2 ) and G(H 2 O) according to a recent literature 63 .

Data availability
All experimental data within the article and its Supplementary Information are available from the corresponding author upon reasonable request.