Hydrogen (H₂) has been considered as an ideal energy carrier due to its high energy density (120–140 MJ/kg), clean, and sustainability [1-3]. Widespread use of hydrogen is partially hampered by its distribution since storage and transportation typically requires high pressure and cryogenic conditions. Materials-based hydrogen storage, viz. storing hydrogen in compounds such as ammonia borane [4], formic acid [5], formaldehyde [6-8], and hydrides [9], avoids high pressures and low temperatures and more importantly, features higher capacity. Among those potential carriers, inexpensive formaldehyde (HCHO) has many outstanding advantages for it generate hydrogen by spontaneous reforming at room temperature [10]. Although some noble-metal complex catalysts hold amazing formaldehyde reforming performance, the high cost limits their industrial application. Therefore, it is important to synthesize non-precious metal catalysts for reforming formaldehyde under ambient conditions.

Among numerous non-precious metal catalysts, Cu-based nanomaterials are considered as an attractive candidate due to their unique electronic structure and the capability for efficient catalytic dehydrogenation [11,12]. In the past decades, they were developed and used to catalyze formaldehyde conversion in electrochemistry [13,14], gas-phase [12,15], and liquid-phase [2,16,17]. To achieve highly-efficient catalysts, geometry and local electronic structure of active centers are tailored based on structure-property relationships, forming various fabrication strategies to control the particle size and composition [18,19], exposing facets [19], chemical ordering [20], and metal-support interfaces [21,22]. Previous study indicated that formaldehyde was a structure-sensitive molecule, and the conversion temperature on the nanofiber octahedral molecular sieve surface was significantly lower than that on the nanoparticle structure [7]. Therefore, the preparation of nanowire-structured catalyst is a good strategy for formaldehyde dehydrogenation. Recently, the oxide-derived Cu catalysts have attracted much attention due to their finer grains, higher grain boundary density, and superior catalytic performance compared to direct synthesized Cu catalysts [23-26]. Some reports suggest that Cu⁺ and residual subsurface oxygen in oxide-derived Cu may tune the surface binding energy, alter reaction pathway, which can significantly improve the catalytic performance [27]. Based on the above studies, it would be a feasible strategy to design an oxide-derived Cu catalyst with nanowire structure for boosting hydrogen production from formaldehyde aqueous reforming.

Herein, we successfully prepare high-density Cu nanowires (NWs) by the electrochemical reduction of CuO NWs, which generate from the oxidation of Cu wire mesh. The oxide-derived Cu NWs is firstly applied to produce hydrogen from formaldehyde/water at ambient conditions (Fig. S1 in Supporting information). High-density nanowire structure and finer grains are beneficial to the conversion of reactants and diffusion of products, while such self-supported Cu mesh provides convenience for the subsequent separation of catalyst and product. We demonstrate that the catalytic activity of Cu could be significantly enhanced with presence of oxygen. The rate of hydrogen generation is increased by purging oxygen into the reaction. We reveal that the gaseous oxygen activates copper surface via forming positively charged Cu sites. This research demonstrates a simple and effective strategy to tune catalytic activities of metal catalysts by dynamic activation.

The SEM morphologies of samples before and after electro-reduction are presented in Figs. 1a-f. The Cu mesh surface is completely covered by high density of CuO NW arrays after thermal oxidation at 600 ℃ in air. Typical diameter of the prepared CuO NWs is about 230 nm, with the length of about 40 µm. TEM observations confirm that the NWs are predominately CuO (Figs. 1g and h). Minor Cu₂O phase exists between the CuO NWs and the Cu woven mesh, which agrees well with the XRD results (Fig. S2 in Supporting information) and follows the Gibbs' phase rule. The high compressive stress in the Cu₂O overlayer drives the NWs growth on Cu surface [28,29]. The lattice fringes with an interplanar lattice spacing of 0.23 nm correspond to the CuO (111) atomic planes (Fig. 1h). Then the oxide NWs are electro-reduced to metallic Cu NWs at −0.4 V (vs. RHE). Due to the volume shrinkage during the conversion, the resulting Cu NWs tend to curve [30], as shown in Figs. 1d-f. The magnified TEM image (Fig. 1i) shows that the NWs are rougher after redox and composed of fine Cu nanocrystals, which explains the broadening of the diffraction peaks of the NW arrays (Fig. S2 in Supporting information). In Fig. 1j, many step structures appear at the edge of NW and the crystal lattice distances of 0.2 nm correspond to Cu (111) plane. In addition, monolithic catalysts attached to Cu meshes can be advantageous to trigger or stop reactions by simply inserting or taking out the mesh, allowing for an "on-off" feature [31].

X-ray photoelectron spectroscopy (XPS) is performed to further analyze Cu NWs and CuO NWs samples. As shown in Fig. 2a, the Cu 2p_3/2 and Cu 2p_1/2 peaks of CuO NWs around 933.69 eV and 953.55 eV are assigned to Cu²⁺ [32]. Additionally, there are two typical satellite peaks of Cu²⁺ at 942.43 eV and 962.22 eV, indicating the surface of CuO NWs has been completely oxidized. On the electro-reduced Cu NWs sample, two weak peaks at 932.63 eV and 952.47 eV can be assigned to Cu⁰ or Cu⁺ [33]. Therefore, Cu LMM Auger spectra surface state analysis is performed in Fig. 2b. The peak at 917.12 eV can be assigned to Cu⁰ [34]. Combining with the XRD results, CuO is reduced to metallic Cu after electrochemical reduction.

Then, the H₂ production performance on Cu mesh and Cu NWs with and without the presence of oxygen is studied in HCHO (2 mol/L) and KOH (1 mol/L) aqueous solution at ambient conditions. As shown in Fig. 3a, the Cu NWs outperforms the bare Cu mesh in catalytic activity. Hydrogen production is proportional to time with the use of Cu mesh and CuNWs, indicating a uniform hydrogen production rate. Interestingly, it is found that the introduction of different gasses into solution have a great effect on the hydrogen production. The H₂ production performance is improved when O₂ is introduced into the solution, while almost no H₂ is detected under the Ar condition. More importantly, the H₂ yield over Cu NW catalyst is 10 mL in 60 min, nearly 12 times higher than that of pure Cu mesh in the presence of oxygen injection. The large specific surface area of the NW nanostructure and its abundant grain boundaries contribute to the activity by providing more active sites [30]. The H₂ generation rate increases almost linearly with the amounts of the CuNWs mesh (Fig. 3b). As shown in Table S1 (Supporting information), the TOF of Cu NWs is higher than some precious metal catalysts. Considering that the metallic wire of ~50 µm diameter contributes most of the mass, the activity of the Cu NWs monolith in this work is good.

It is well known that the solution can have significant effect on the kinetics of catalytic performance [10]. We investigate the H₂ production of Cu NWs with the presence of oxygen under different concentrations of HCHO and KOH, respectively, and the results are shown in Figs. 3c and d. Negligible change in the H₂ generation rates is observed when the HCHO concentrations are varied between 1.0 mol/L and 2.5 mol/L (Fig. 3c), and the highest rate is obtained in 2.0 mol/L. While, the H₂ generation rate has an obviously vibration under different KOH concentrations (Fig. 3d). The reaction rate increases as the concentrations of KOH change from 0.1 mol/L to 1 mol/L, and then decreases in a more basic solution. Highly alkaline condition promotes Cannizzaro reaction that reforms aldehyde and water into methanol and formic acid (HCHO + H₂O → CH₃OH + COOH) as competing process [35]. Thus the rates of H₂ generation are decreased at KOH concentration higher than 1.0 mol/L. From the above results, 2 mol/L HCHO and 1 mol/L KOH are viewed as the best reaction conditions.

The above experimental results indicate that the introduction of different gasses into the solution have a large effect on the H₂ production. Therefore, we investigate the role of O₂ partial pressure on the H₂ production performance of HCHO reforming, and the results are summarized in Fig. 4a. The curve displays that the amount of H₂ production increases with increasing oxygen concentration, and the H₂ generation rate is 0.005 mL/min at Ar saturated solution. In other words, negligible amount of H₂ evolved on Cu NWs surface in absence of oxygen. In addition, the rate of hydrogen generation (Fig. 4b) clearly shows the correlation between oxygen and hydrogen evolution, i.e., higher partial pressure of oxygen leads to faster H₂ production, suggesting that O₂ enhances the catalytic activity of Cu NWs. The maximum rate of H₂ in oxygen-rich condition is 0.18 mL/min, which is nearly 36 times larger than that without oxygen. Next, the hydrogen evolution rate over Cu NWs obeys a parabolic correlation with oxygen concentration, and a fitting linear dependency with slope of 1.84 is obtained from double logarithmic plots of the initial reaction rate vs. oxygen concentration (Fig. 4b, insert). A positive slope indicates that the activation of oxygen and conversion to reactive oxygen species are the key step limiting the reaction rate. The reactivity of Cu catalyst highly depends on valency and local electronic structure because adsorption of reactive intermediates proceeds via electron hybridization. For example, metallic Cu is highly active for catalyzing propylene epoxidation, but its activity is normally suppressed by the oxide layer formed at the catalyst surface in oxidative environment. By illuminating visible light, Linic et al. found a steady activity and selectivity of Cu nanoparticles for epoxidation due to light-induced reduction [36]. Also, metallic Cu showed higher catalytic activity than Cu₂O in hydrogen production from N,N-dimethylformamide (DMF) and water [37]. It has been previously shown that the reforming of HCHO/H₂O over d¹⁰ elements can only proceed via the oxidized state rather than the corresponding metal [8,10,38], but maintaining the oxidized state is difficult because copper oxide can be easily reduced by formaldehyde. In this work, we deduce that purging oxygen into the reaction creates an electron-deficient state for Cu by extracting electrons from Cu surface and in turn forms an oxide layer [39]. Based upon the correlation between oxygen concentration and rate of H₂ generation (Fig. 4b), these in-situ oxidized Cu atoms are catalytically active for the formation of H₂. In-situ surface modification has also been found effective in enhancing catalytic performance in different systems. For example, the catalytic activity of Ru/TiO₂ for converting p-cresol to toluene was promoted by introducing molecular N₂ into the reaction, and the positive effect was attributed to the formation of hydrogenated nitrogen species on the ruthenium metal surface [40]. The catalytic oxidation of methane into CH₃OH is promoted by introducing water that favors formation of methoxy groups (^*CH₃O) [41].

To elucidate the crucial role of oxygen on activating Cu, we further compared the catalytic performance of CuO NWs and Cu NWs under Ar saturate (Fig. 5a) and oxygen saturated (Fig. 5b) conditions, respectively. As shown in Fig. 5a, in the initial 20 min, H₂ generation rate over CuO is much higher than Cu NWs in the absence of O₂. The reactivity over CuO then drops quickly after 20 min and nearly stops after 40 min, and the color of the CuO mesh simultaneously turns from dark brown to red. XRD analysis (Fig. 5c) shows that both CuO and Cu₂O are completely reduced to metallic Cu. And the newly formed Cu is comprised of fine crystal grains, revealed by broader diffraction peaks. These findings indicate that copper oxides are highly active but not stable over the course of hydrogen evolution due to reduction by formaldehyde [42]. For metallic Cu NWs, the reactivity also declines and diminishes quickly, which is associated with the thin copper oxide layer on NWs being quickly reduced to Cu which has no catalytic effect.

The performance of Cu NWs and CuO NWs for H₂ production with the presence of O₂ is shown in Fig. 5b. An induction period exists for both of CuO NWs and Cu NWs to start the hydrogen production. For metallic Cu NWs, the H₂ generation rate peaks after 20 min. In contrast, the oxide catalyst exhibits a longer induction period before reaching a maximum and then diminishes rapidly. We thus infer that the active sites are metallic Cu with adsorbed oxygen. Since copper oxide must be reduced first to Cu, a longer silent period is therefore required. To verify the reasoning, the time taken to reach the highest H₂ generating rate is recorded as a function of oxygen partial pressure (Fig. S3 in Supporting information). It is found that the period increases linearly with the oxygen partial pressure after 40% for the reduction process to Cu is delayed by the dioxygen. The higher O₂ partial pressure, the more time is needed to obtain the clean surface of metallic Cu with adsorbed oxygen. The H₂ generation rate over CuO NWs catalyst decreases to the same to metallic Cu after 70 min when CuO is entirely reduced to Cu, confirmed by that the two starting materials reach same level of activity. In each case, O₂ plays a role in activating inert Cu for hydrogen production from the formaldehyde/water system. To further prove the promoting role of oxygen, the rate of H₂ generation and changes of O₂ flow rate are monitored under an oxygen partial pressure of 0.4 (Ar as equilibrium gas) using Cu NWs as the catalyst (Fig. 5d). A decrease in oxygen concentration at the initial stage, due to oxygen absorption by Cu forming surface oxides, is observed along with an abrupt increase in H₂ generation. After that period, the O₂ flow rate remains almost steady, indicating that O₂ is not consumed during the dehydrogenation reaction. To evaluate the cyclic stability of Cu NWs, 4 cm² of Cu NWs mesh are taken for H₂ production reaction under optimal conditions for 1 h, and then, the sample is recovered for repeating the above experiment. Fig. S4 (Supporting information) shows that H₂ production experiment is repeated for 8 cycles, and the rate of H₂ production remains a steady state, indicating a good cyclic stability of Cu NWs.

Density functional theory (DFT) calculations are carried out to elucidate the mechanism of activating inert Cu by oxygen adsorption. The (111) surface is of highest percentage in the polycrystals of IB metals and the most thermodynamically stable under the reaction process [42,43]. As shown in Fig. 6a, the distance between pure Cu (111) surface and formaldehyde is 3.55 Å, meaning that formaldehyde could not be adsorbed on the Cu surface [44]. In another word, pure Cu surface is inert for the formaldehyde, making the formaldehyde adsorption the rate determining step of the hydrogen generation reaction.

In aqueous solution, formaldehyde is transformed to hydroxymethanolate (CH₂(OH)₂) (Fig. 6b) [38]. After oxygen is chemisorbed on the surface, Cu is activated to capture formaldehyde derivatives and the chemisorption is exothermic (Fig. 6c). The reaction starts with the chemisorption of oxygen on the Cu (111) surface at the bridge site, forming O₂^•− radicals by one electron transfer process from the Cu 3d orbital to the empty π^* orbital of O₂ [45]. As a consequence, the chemisorption of oxygen changes the valence of Cu from Cu⁰ to Cu⁺ (Fig. 6d). In a previous study on the activation of C=O bonds in formaldehyde by Cu⁺ in zeolites, electron pair donation from carbonyl oxygen to the metal cation was suggested to be responsible for bonding between the C=O and the cation [46]. Therefore, formaldehyde molecules are difficult to land on surface of metallic Cu due to the lack of empty orbit to accept the pair. Extracting electrons by oxygen endows Cu with the capability of capturing the formaldehyde. The O—H bond in the HOCH₂OH intermediate is cleaved into H⁺ and HOCH₂O¯ by the activated Cu surface (Fig. 6e). The cleaved H⁺ is coupled to adsorbed ^*O₂^•− forming ^*OOH, and the HOCH₂O¯ is adsorbed on the adjacent Cu⁺ site via the C=O bond that is not possible for bare metallic Cu (Fig. 6f). Subsequently, OHCHO¯ is formed by cleaving C—H bond and releasing H˙ to Cu site with an estimated activation energy of 27.87 kJ/mol, making it the rate-determining step of the reforming reaction (Fig. 6g). Since the interaction of ^*OOH and H˙ can react easily, H₂ is generated easily (−17.18 kJ/mol) (Fig. 6h) [8,10,45]. Finally, formic acid is desorbed from the Cu surface, and the active Cu site is recovered. Chemisorption of oxygen on Cu surface provides conducive conditions to reforming formaldehyde and water [47]. As we know, the solvation influences catalytic process by a field effect on dipolar reaction intermediate, changing the proton donor for the electron transferred during the reaction. Especially, alkali metal cations (K⁺) can stabilize reaction intermediates and decease the kinetic barrier by electrostatic interactions with dipolar intermediates, thereby increasing the formaldehyde reforming process.

Both of experiments and calculations prove that introducing oxygen is necessary because the O₂^•− species activate Cu sites. Similar promotion effect of dioxygen was previously observed on MgO supported Ag, where synergistic effect between the metal and the oxide support was attributed to [8,10]. However, in this work, all the cycling steps of oxygen occur only on the Cu surface. The special promotion effect of dioxygen for activating Cu may shed lights on tuning selectivity and activity of other transition metal catalysts.

In summary, we demonstrate oxygen-modulated catalytic performance of Cu nanowires for hydrogen evolution from aqueous solution of formaldehyde. The results show that pure metallic Cu is almost inert for formaldehyde due to the weak adsorption. Interestingly, the adsorption is strengthened by introducing oxygen during the spontaneous reaction. The main reason is that the Cu⁺ and O₂^•− are formed on Cu surface after the oxygen injection. As a result, the molecular O₂ greatly enhances the reforming reaction rate without consumption. This hydrogen evolution reaction not only brings opportunities to the development of pure H₂ source for fuel cell, but also shines light on the special effect of oxygen in catalytic reaction.

The authors declare that they have no known competing financial interests or personal relationships that could have appeared to influence the work reported in this paper.

This work is supported by the China BaoWu Low Carbon Metallurgical Innovation Foundation (No. BWLCF202113), the Fundamental Research Funds for the Central Universities (Nos. N2202012, N180206004) and the National Natural Science Foundation of China (No. 51971059).

Supplementary material associated with this article can be found, in the online version, at doi:10.1016/j.cclet.2022.107905.