**1. Introduction**

Due to the excessive consumption of fossil fuels, the resulting environmental pollution and global energy crisis have aroused widespread concern. It is essential to develop clean, environmental friendly and renewable energy sources to reduce our dependence on fossil fuels and benefit the environment by reducing greenhouse gas emissions [1–7]. Among variable alternatives, hydrogen has been considered as an ideal energy carrier due to its environmental friendliness and high energy density. Electrochemical water splitting is one of the most simple and promising strategies to create high-purity hydrogen in an economic way [8–14]. However, the production efficiency is low without the use of electrocatalysts, which can significantly reduce the large overpotential for the hydrogen evolution reaction (HER). It is well known that Pt, Ru-based and Ir-based catalysts are regarded as the most promising electrocatalysts for the HER and OER, because of their high electrocatalytic performance [15–23], whereas their widespread application is restricted by their high costs and low abundance on Earth. Therefore, the major challenge in hydrogen production is to reduce the use of noble metals or replace them with inexpensive nonprecious metal catalysts.

In recent years, a lot of effort in the field of highly active, Earth-abundant catalysts has been dedicated to various types of alternative materials, such as transition metal sulfides [24–26], metal carbides [27–29], metal nitrides [30–32], metal phosphides [33–36] and even metal-free materials [37,38]. Transition-metal phosphides (TMPs) are an important class of compounds with metalloid characteristics and good electrical conductivity. In the structure of metal phosphides, negatively charged P atoms can act as ideal active centers for proton adsorption, bringing about the dynamical optimization of the HER [39–41]. To date, various metal phosphides have been adopted for electrochemical hydrogen evolution, such as cobalt phosphide nanoparticles (CoP NPs [42]), nickel phosphide nanoparticles (Ni2P NPs [43]), molybdenum phosphide nanoparticles (MoP NPs [44]) and Ni–Fe phosphide nanohybrids [45], which have attracted attention for their excellent electrocatalytic activities

for the HER. However, the relatively low electrical conductivity of most phosphide catalysts remains a problem, leading to limited charge transfer and passivated electrocatalytic activity. Furthermore, these electrocatalysts are prone to agglomeration under high current density or long-term tests in practical application in the HER. these electrocatalysts are prone to agglomeration under high current density or long-term tests in practical application in the HER. To overcome the above-mentioned issues, alternative architectural arrays grown on conductive substrates have been explored due to the large surface area, abundant active

electrochemical hydrogen evolution, such as cobalt phosphide nanoparticles (CoP NPs [42]), nickel phosphide nanoparticles (Ni2P NPs [43]), molybdenum phosphide nanoparticles (MoP NPs [44]) and Ni–Fe phosphide nanohybrids [45], which have attracted attention for their excellent electrocatalytic activities for the HER. However, the relatively low electrical conductivity of most phosphide catalysts remains a problem, leading to limited charge transfer and passivated electrocatalytic activity. Furthermore,

*Catalysts* **2022**, *12*, 762 2 of 12

To overcome the above-mentioned issues, alternative architectural arrays grown on conductive substrates have been explored due to the large surface area, abundant active sites, and synergistic effects between the electrocatalysts and the conductive substrates. Recently, Sun and co-workers [46] reported on porous urchin-like Ni2P microsphere superstructures anchored on nickel foam, which afforded a current density of 10 mA cm−<sup>2</sup> at a low overpotential of only −98 mV for the HER. Tan and co-workers [47] reported on flower-like structures consisting of NiCoP-CoP nanowires grown directly on porous nickel frameworks to achieve a highly efficient HER in an alkaline solution. For the HER, a binder-free NiCoP-CoP/Ni/NF electrode can reach 10 mA cm−<sup>2</sup> current density at a quite low overpotential of 49 mV. Despite extensive progress in nanoarray architectures, self-supporting nanoarray structures on conductive materials are still a key challenge. sites, and synergistic effects between the electrocatalysts and the conductive substrates. Recently, Sun and co-workers [46] reported on porous urchin-like Ni2P microsphere superstructures anchored on nickel foam, which afforded a current density of 10 mA cm−<sup>2</sup> at a low overpotential of only −98 mV for the HER. Tan and co-workers [47] reported on flower-like structures consisting of NiCoP-CoP nanowires grown directly on porous nickel frameworks to achieve a highly efficient HER in an alkaline solution. For the HER, a binder-free NiCoP-CoP/Ni/NF electrode can reach 10 mA cm−2 current density at a quite low overpotential of 49 mV. Despite extensive progress in nanoarray architectures, self-supporting nanoarray structures on conductive materials are still a key challenge. Over the past decade, Fe, Co and Ni as electrocatalysts have exhibited excellent catalytic performance for the HER. Nevertheless, as an Earth-abundant transition metal,

Over the past decade, Fe, Co and Ni as electrocatalysts have exhibited excellent catalytic performance for the HER. Nevertheless, as an Earth-abundant transition metal, Cu-based catalysts have been relatively less studied in terms of the HER. Therefore, it is significant to design Cu-based materials with special structures for developing high-efficiency electrocatalysts. Recent studies have shown that Cu3P is an excellent electrocatalyst for use in the HER [48,49]. Herein, self-supported Cu/Cu3P nanoarrays were successfully grown on the surfaces of Cu nanosheets from Cu/CuO nanoarrays precursor by a low-temperature phosphidation process. The Cu/Cu3P nanoarray-270, as an electrocatalyst, displays excellent catalytic performance and durability for electrochemical hydrogen generation, and exhibits a low onset overpotential (96 mV) and a small Tafel slope (131 mV dec−<sup>1</sup> ). The morphology and nanostructure of the self-supported Cu/Cu3P nanoarray catalyst affect the electrocatalytic efficiency significantly. The nanoarrays possess large surface areas and a great number of active sites, which is immensely beneficial for electrocatalysis capacity enhancement. At the same time, copper-based catalysts can also be used in other types of organic reactions [50]. It is expected that this innovative approach will become a new concept to synthesize highly efficient catalysts. Cu-based catalysts have been relatively less studied in terms of the HER. Therefore, it is significant to design Cu-based materials with special structures for developing high-efficiency electrocatalysts. Recent studies have shown that Cu3P is an excellent electrocatalyst for use in the HER [48,49]. Herein, self-supported Cu/Cu3P nanoarrays were successfully grown on the surfaces of Cu nanosheets from Cu/CuO nanoarrays precursor by a low-temperature phosphidation process. The Cu/Cu3P nanoarray-270, as an electrocatalyst, displays excellent catalytic performance and durability for electrochemical hydrogen generation, and exhibits a low onset overpotential (96 mV) and a small Tafel slope (131 mV dec−1). The morphology and nanostructure of the self-supported Cu/Cu3P nanoarray catalyst affect the electrocatalytic efficiency significantly. The nanoarrays possess large surface areas and a great number of active sites, which is immensely beneficial for electrocatalysis capacity enhancement. At the same time, copper-based catalysts can also be used in other types of organic reactions [50]. It is expected that this innovative approach will become a new concept to synthesize highly efficient catalysts.

#### **2. Results 2. Results**

The typical procedure for the synthesis of Cu/Cu3P nanoarrays is summarized in Figure 1. In brief, Cu nanosheets are firstly synthesized according to hydrothermal method. Then, Cu nanosheets, as both a self-template and nano-conductive substrate, are immersed in a solution of NaOH/H2O<sup>2</sup> for the formation of Cu/CuO nanoarrays. Cu/CuO nanoarrays and NaH2PO<sup>2</sup> are calcinated under an Ar gas flow; the original black color of the Cu/CuO turns gray after the phosphorization process, thus suggesting that the copper oxides on the surfaces of Cu nanosheets are converted into cuprous phosphide. The typical procedure for the synthesis of Cu/Cu3P nanoarrays is summarized in Figure 1. In brief, Cu nanosheets are firstly synthesized according to hydrothermal method. Then, Cu nanosheets, as both a self-template and nano-conductive substrate, are immersed in a solution of NaOH/H2O2 for the formation of Cu/CuO nanoarrays. Cu/CuO nanoarrays and NaH2PO2 are calcinated under an Ar gas flow; the original black color of the Cu/CuO turns gray after the phosphorization process, thus suggesting that the copper oxides on the surfaces of Cu nanosheets are converted into cuprous phosphide.

**Figure 1.** Illustration of the preparation of Cu/Cu3P nanoarrays. **Figure 1.** Illustration of the preparation of Cu/Cu3P nanoarrays.

The X-ray diffraction (XRD) patterns of the Cu/CuO nanoarrays before and after phosphidation are shown in Supplemaentery Figures S1c and 2a. The precursor shows diffraction peaks characteristic of CuO (JCPDS No. 04-1548). In contrast, only peaks corresponding to Cu3P can be observed for the resulting copper phosphide. Figure 2a shows that all diffraction peaks are in accordance with the hexagonal structure of Cu3P (JCPDS No. 02-1623), and the strong peaks at 43.4◦ , 50.4◦ and 74.1◦ originate from the Cu nanosheets (JCPDS No. 04-0836), indicating that all copper oxides are completely trans-

formed into cuprous phosphides in the phosphating process, while the copper nanosheets, as a conductive template, have not been completely consumed. transformed into cuprous phosphides in the phosphating process, while the copper nanosheets, as a conductive template, have not been completely consumed.

The X-ray diffraction (XRD) patterns of the Cu/CuO nanoarrays before and after phosphidation are shown in Supplemaentery Figures S1c and 2a. The precursor shows diffraction peaks characteristic of CuO (JCPDS No. 04-1548). In contrast, only peaks corresponding to Cu3P can be observed for the resulting copper phosphide. Figure 2a shows that all diffraction peaks are in accordance with the hexagonal structure of Cu3P (JCPDS No. 02-1623), and the strong peaks at 43.4°, 50.4° and 74.1° originate from the Cu nanosheets (JCPDS No. 04-0836), indicating that all copper oxides are completely

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**Figure 2.** Characterization of the morphology and structure of sample: (**a**) XRD pattern of Cu/Cu3P nanoarrays. (**b**) SEM image of Cu nanosheets. (**c**,**d**) SEM images of Cu/CuO nanoarrays. (**e**,**f**) SEM images of Cu/Cu3P nanoarrays; inset shows the HRTEM of Cu3P. **Figure 2.** Characterization of the morphology and structure of sample: (**a**) XRD pattern of Cu/Cu3P nanoarrays. (**b**) SEM image of Cu nanosheets. (**c**,**d**) SEM images of Cu/CuO nanoarrays. (**e**,**f**) SEM images of Cu/Cu3P nanoarrays; inset shows the HRTEM of Cu3P.

The morphologies of products were characterized by scanning electron microscopy (SEM). Figures 2b and S1a show the SEM images of Cu nanosheets as the self-template and conductive substrate, which had a large area of 30–100 μm in diameter with smooth surface. The SEM images of the Cu/CuO nanoarrays at different magnification are shown in Figures 2c,d and S2. The CuO nanoarrays are uniformly distributed on the surface of the Cu nanosheet, consisting of uniform nanoplates with a width ranging from 30 nm to 80 nm and are 3–5 μm in length. After phosphidation, the nanoarray morphology is still preserved, as shown in Figure 2e,f. The plate Cu3P nanoarrays grown on the Cu nanosheet substrate and the surfaces of the nanoarrays become rough. The high-magnification SEM image of the Cu3P nanoplate is shown in Figure S3, and close observation reveals that the thickness of an individual Cu3P nanoplate increases from 60 nm to 120 nm in the phosphating process. The nanoarray structure helps to expose more The morphologies of products were characterized by scanning electron microscopy (SEM). Figures 2b and S1a show the SEM images of Cu nanosheets as the self-template and conductive substrate, which had a large area of 30–100 µm in diameter with smooth surface. The SEM images of the Cu/CuO nanoarrays at different magnification are shown in Figures 2c,d and S2. The CuO nanoarrays are uniformly distributed on the surface of the Cu nanosheet, consisting of uniform nanoplates with a width ranging from 30 nm to 80 nm and are 3–5 µm in length. After phosphidation, the nanoarray morphology is still preserved, as shown in Figure 2e,f. The plate Cu3P nanoarrays grown on the Cu nanosheet substrate and the surfaces of the nanoarrays become rough. The high-magnification SEM image of the Cu3P nanoplate is shown in Figure S3, and close observation reveals that the thickness of an individual Cu3P nanoplate increases from 60 nm to 120 nm in the phosphating process. The nanoarray structure helps to expose more active sites in the catalytic reaction, and the interspace between the nanoarrays can favor the diffusion of electrolytes. The high-resolution transmission electron microscopy (HRTEM) image (inset f) shows clear lattice fringes with an interplane distance of 0.31 nm, corresponding to the

(111) of the Cu3P. All these results clearly confirm the successful synthesis of Cu/Cu3P nanoarrays by low-temperature phosphidation from the Cu/CuO nanoarray precursor. The fabrication process of the Cu/Cu3P nanoarray is illustrated in Figure 4a. The morphology of the products was found to strongly depend on the distance between

hydride-acceptor center and P may act as the proton-acceptor center [55].

that charge transfer occurs between Cu and P, in which Cu may serve as the

elemental P (130.2 eV), indicating that P carries a negative charge (δ-

*Catalysts* **2022**, *12*, 762 4 of 12

Cu/CuO nanoarray precursor.

active sites in the catalytic reaction, and the interspace between the nanoarrays can favor the diffusion of electrolytes. The high-resolution transmission electron microscopy (HRTEM) image (inset f) shows clear lattice fringes with an interplane distance of 0.31 nm, corresponding to the (111) of the Cu3P. All these results clearly confirm the successful synthesis of Cu/Cu3P nanoarrays by low-temperature phosphidation from the

The detailed elemental compositions and valence states of as-synthesized Cu/Cu3P were characterized by X-ray photoelectron spectroscopy (XPS), as shown in Figure 3. The full survey XPS spectrum (Figure S4) shows that the Cu/Cu3P comprises Cu, P, O and C elements. As shown in Figure 3a, two main peaks of Cu 2p are located at 934.6 eV and 954.4 eV, which represent the Cu 2p3/2 and Cu 2p1/2 peaks, respectively. The peaks at 933.1 eV and 935.1 eV are assigned to the Cuδ+ in the Cu3P and oxidized Cu for the Cu 2p3/2 energy level, while the peaks at 940.8 and 944.1 eV belong to the satellite peaks of Cu 2p3/2. The three peaks appearing at 952.8, 955.2 and 962.9 eV are indexed to the Cuδ<sup>+</sup> in the Cu3P, oxidized Cu and the satellite for Cu 2p1/2, respectively [51,52]. In Figure 3b, the peak at 133.6 eV could be indexed to oxidized phosphate species, resulting from the exposure of the sample to air. The lower binding energy peaks situated at around 129.1 eV and 129.9 eV correspond to P 2p3/2 and P 2p1/2 of Cu/Cu3P nanoarrays, respectively [53,54]. Note that the binding energy of P 2p (129.9 eV) shows a negative shift from

). The results suggest

The detailed elemental compositions and valence states of as-synthesized Cu/Cu3P were characterized by X-ray photoelectron spectroscopy (XPS), as shown in Figure 3. The full survey XPS spectrum (Figure S4) shows that the Cu/Cu3P comprises Cu, P, O and C elements. As shown in Figure 3a, two main peaks of Cu 2p are located at 934.6 eV and 954.4 eV, which represent the Cu 2p3/2 and Cu 2p1/2 peaks, respectively. The peaks at 933.1 eV and 935.1 eV are assigned to the Cuδ<sup>+</sup> in the Cu3P and oxidized Cu for the Cu 2p3/2 energy level, while the peaks at 940.8 and 944.1 eV belong to the satellite peaks of Cu 2p3/2. The three peaks appearing at 952.8, 955.2 and 962.9 eV are indexed to the Cuδ<sup>+</sup> in the Cu3P, oxidized Cu and the satellite for Cu 2p1/2, respectively [51,52]. In Figure 3b, the peak at 133.6 eV could be indexed to oxidized phosphate species, resulting from the exposure of the sample to air. The lower binding energy peaks situated at around 129.1 eV and 129.9 eV correspond to P 2p3/2 and P 2p1/2 of Cu/Cu3P nanoarrays, respectively [53,54]. Note that the binding energy of P 2p (129.9 eV) shows a negative shift from elemental P (130.2 eV), indicating that P carries a negative charge (δ - ). The results suggest that charge transfer occurs between Cu and P, in which Cu may serve as the hydride-acceptor center and P may act as the proton-acceptor center [55]. Cu/CuO nanoarrays and sodium hypophosphite in the phosphating process. When the distance between the two precursors is less than 5 cm, the nanoarray structure on the surface of the Cu nanosheets disappears and its surface becomes rough, as shown in Figure 4b,c. Further increasing the phosphating distance to 16 cm, part of the array structure on the surface can be observed, as shown in Figure 4d. The nanoarrays are obviously thicker than the original CuO nanoplate, and agglomeration between the nanoarrays is more serious. When the phosphating distance was extended to 24 cm (in Figure 4e), the nanoarray structure composed of Cu3P nanoplates with a width of around 300–800 nm and lengths of up to several micrometers was vertically grown on the surface of the Cu nanosheets. The topotactic conversion of the Cu/CuO nanoarrays into the Cu/Cu3P nanoarray could be explained as follows: first, the thermal decomposition of NaH2PO2 generates PH3, and the CuO nanoarrays are reduced to Cu nanoarrays by PH3. Then, the resulting Cu subsequently catalyzes the decomposition of PH3 into elemental P. Finally, the elemental P further reacts with Cu to form Cu3P nanoarrays.

**Figure 3. Figure 3.**  Cu 2p ( Cu 2p ( **a**) and P 2p ( **a**) and P 2p ( **b**) core-level spectra of Cu/Cu **b**) core-level spectra of Cu/Cu <sup>3</sup>P nanoarrays. 3P nanoarrays.

The fabrication process of the Cu/Cu3P nanoarray is illustrated in Figure 4a. The morphology of the products was found to strongly depend on the distance between Cu/CuO nanoarrays and sodium hypophosphite in the phosphating process. When the distance between the two precursors is less than 5 cm, the nanoarray structure on the surface of the Cu nanosheets disappears and its surface becomes rough, as shown in Figure 4b,c. Further increasing the phosphating distance to 16 cm, part of the array structure on the surface can be observed, as shown in Figure 4d. The nanoarrays are obviously thicker than the original CuO nanoplate, and agglomeration between the nanoarrays is more serious. When the phosphating distance was extended to 24 cm (in Figure 4e), the nanoarray structure composed of Cu3P nanoplates with a width of around 300–800 nm and lengths of up to several micrometers was vertically grown on the surface of the Cu nanosheets. The topotactic conversion of the Cu/CuO nanoarrays into the Cu/Cu3P nanoarray could be explained as follows: first, the thermal decomposition of NaH2PO<sup>2</sup> generates PH3, and the CuO nanoarrays are reduced to Cu nanoarrays by PH3. Then, the resulting Cu subsequently catalyzes the decomposition of PH<sup>3</sup> into elemental P. Finally, the elemental P further reacts with Cu to form Cu3P nanoarrays.

The influence of different mass ratios of phosphorus precursor and the Cu/CuO nanoarrays on the morphology and crystal structure was investigated, as shown in Figure 5. When the mass ratio of NaH2PO<sup>2</sup> to CuO is 1, the morphology of Cu/Cu3P nanoarrays does not change significantly (Figure 5a), and the corresponding XRD pattern shows that only a small amount of Cu3P is formed in the product (Figure 5b), indicating that the CuO cannot be converted into Cu3P at this ratio. When the mass ratio of NaH2PO2/CuO increases to

2, the obtained array structure is thicker than that of the precursor (Figure 5c), and the corresponding XRD pattern reveals that CuO has been converted into Cu3P completely, but the amount of Cu3P in the product is small (Figure 5d). When the mass ratio of NaH2PO2/CuO further increases to 2.5, the morphology of the product still maintains the nanoarray structure (Figure 5e), and the corresponding XRD pattern shows that Cu3P is generated, while the peak intensity of the copper substrate does not change significantly (Figure 5f), indicating that the Cu nanosheet has not been converted. Until the mass ratio of NaH2PO2/CuO reached 3, the corresponding SEM image of this sample reveals that the Cu3P nanoarrays thickened and agglomerated together (Figure 5g). The intensity of the XRD pattern of Cu in the product is significantly weakened (Figure 5h), indicating that the Cu nanosheet substrate is partially converted into Cu3P during the phosphating reaction. *Catalysts* **2022**, *12*, 762 5 of 12

**Figure 4.** (**a**) Schematic of the preparation process of the Cu3P nanoarrays via the phosphorization of Cu/CuO. (**b**–**e**) SEM images of products at different distances between Cu/CuO and NaH2PO2: (**b**) d = 0 cm, (**c**) d = 5 cm, (**d**) d = 16 cm and (**e**) d = 24 cm. **Figure 4.** (**a**) Schematic of the preparation process of the Cu3P nanoarrays via the phosphorization of Cu/CuO. (**b**–**e**) SEM images of products at different distances between Cu/CuO and NaH2PO<sup>2</sup> : (**b**) d = 0 cm, (**c**) d = 5 cm, (**d**) d = 16 cm and (**e**) d = 24 cm.

The influence of different mass ratios of phosphorus precursor and the Cu/CuO nanoarrays on the morphology and crystal structure was investigated, as shown in Figure 5. When the mass ratio of NaH2PO2 to CuO is 1, the morphology of Cu/Cu3P nanoarrays does not change significantly (Figure 5a), and the corresponding XRD pattern shows that only a small amount of Cu3P is formed in the product (Figure 5b), indicating that the CuO cannot be converted into Cu3P at this ratio. When the mass ratio of NaH2PO2/CuO increases to 2, the obtained array structure is thicker than that of the precursor (Figure 5c), and the corresponding XRD pattern reveals that CuO has been converted into Cu3P completely, but the amount of Cu3P in the product is small (Figure The influence of the phosphating temperature on the nanostructures formed was investigated, as shown in Figure 6. Figure 6a,b show that CuO and Cu3P were simultaneously observed on the Cu nanosheets at 260 ◦C.With the increase in temperature, the thickness of nanoarrays composed of nanoplates was increased, while the CuO nanoarrays were completely converted to Cu3P nanoarrays at 290 ◦C, as shown in Figure 6c,d. Until the temperature reached 310 ◦C, the nanoarray structures grown on the surfaces of Cu nanosheets experienced obvious agglomeration and collapse, and the corresponding XRD pattern revealed that a part of the Cu nanosheets was converted to Cu3P in the phosphating reaction (Figure 6e,f). The effects of phosphating time on the morphology and phase of as-prepared nanostructures were likewise studied, as shown in Figure S5. When the calcination time was increased to 1.5 h, the morphology of the product obtained was as shown

5d). When the mass ratio of NaH2PO2/CuO further increases to 2.5, the morphology of the product still maintains the nanoarray structure (Figure 5e), and the corresponding XRD

does not change significantly (Figure 5f), indicating that the Cu nanosheet has not been converted. Until the mass ratio of NaH2PO2/CuO reached 3, the corresponding SEM image of this sample reveals that the Cu3P nanoarrays thickened and agglomerated together (Figure 5g). The intensity of the XRD pattern of Cu in the product is significantly weakened (Figure 5h), indicating that the Cu nanosheet substrate is partially converted

into Cu3P during the phosphating reaction.

in Figure S5c. The nanoarray structure composed of nanoplates is significantly thicker than that obtained at 1 h (Figure S5a). Moreover, the weak diffraction peak of Cu indicated that most of the Cu nanosheet substrates were transformed into Cu3P (Figure S5d). The above results reveal that the phosphating temperature and time had a great impact on the formation of the resultant Cu/Cu3P nanoarrays in the present study. *Catalysts* **2022**, *12*, 762 6 of 12

**Figure 5.** SEM images and XRD patterns of products at different mass ratios of NaH2PO2/CuO: (**a**,**b**) 1, (**c**,**d**) 2, (**e**,**f**) 2.5, (**g**,**h**) 3. **Figure 5.** SEM images and XRD patterns of products at different mass ratios of NaH2PO2/CuO: (**a**,**b**) 1, (**c**,**d**) 2, (**e**,**f**) 2.5, (**g**,**h**) 3.

The influence of the phosphating temperature on the nanostructures formed was investigated, as shown in Figure 6. Figure 6a,b show that CuO and Cu3P were simultaneously observed on the Cu nanosheets at 260 °C.With the increase in temperature, the thickness of nanoarrays composed of nanoplates was increased, while the CuO nanoarrays were completely converted to Cu3P nanoarrays at 290 °C, as shown in Figure 6c,d. Until the temperature reached 310 °C, the nanoarray structures grown on As a comparison, the pure Cu nanosheet was directly phosphated and calcined under the same conditions, while the morphology and crystal structure of the products were characterized. As shown in Figure S6a, the 2D nanosheet morphology was still preserved, and the smooth surface of the Cu nanosheets became rough after phosphating. At the same time, the corresponding XRD pattern confirmed that Cu3P was indeed generated (Figure S6b). The results indicate that the CuO nanoarray on the surface of the Cu nanosheet plays a very significant role in maintaining the morphology of Cu/Cu3P nanoarrays.

the surfaces of Cu nanosheets experienced obvious agglomeration and collapse, and the

Cu3P in the phosphating reaction (Figure 6e,f). The effects of phosphating time on the morphology and phase of as-prepared nanostructures were likewise studied, as shown in Figure S5. When the calcination time was increased to 1.5 h, the morphology of the product obtained was as shown in Figure S5c. The nanoarray structure composed of nanoplates is significantly thicker than that obtained at 1 h (Figure S5a). Moreover, the weak diffraction peak of Cu indicated that most of the Cu nanosheet substrates were transformed into Cu3P (Figure S5d). The above results reveal that the phosphating temperature and time had a great impact on the formation of the resultant Cu/Cu3P

nanoarrays in the present study.

**Figure 6.** SEM images and XRD patterns of products at different phosphating temperatures: (**a**,**b**) 260 °C, (**c**,**d**) 290 °C, (**e**,**f**) 310 °C. **Figure 6.** SEM images and XRD patterns of products at different phosphating temperatures: (**a**,**b**) 260 ◦C, (**c**,**d**) 290 ◦C, (**e**,**f**) 310 ◦C.

As a comparison, the pure Cu nanosheet was directly phosphated and calcined under the same conditions, while the morphology and crystal structure of the products were characterized. As shown in Figure S6a, the 2D nanosheet morphology was still preserved, and the smooth surface of the Cu nanosheets became rough after phosphating. At the same time, the corresponding XRD pattern confirmed that Cu3P was indeed generated (Figure S6b). The results indicate that the CuO nanoarray on the surface of the Cu nanosheet plays a very significant role in maintaining the morphology of Cu/Cu3P nanoarrays. The electrocatalytic activity of the Cu/Cu3P nanoarray for the HER was tested by using a standard three-electrode device in 0.5 M H2SO4 solution. Figure 7 shows the polarization curves of these electrodes obtained at different temperatures without iR The electrocatalytic activity of the Cu/Cu3P nanoarray for the HER was tested by using a standard three-electrode device in 0.5 M H2SO<sup>4</sup> solution. Figure 7 shows the polarization curves of these electrodes obtained at different temperatures without iR correction. The catalytic behavior of Cu/Cu3P NS obtained by the direct phosphating of the Cu nanosheet was also investigated for comparison. Obviously, the Cu/Cu3P NS showed poor electrocatalytic activity, with an onset overpotential value of 347 mV. In sharp contrast, Cu/Cu3P nanoarray-270 was significantly active for the HER, with an onset overpotential as low as 96 mV, and additional negative potential leads to a rapid rise in the cathodic current. It requires 253 mV of overpotential (η10) to reach a current density (*j*) of 10 mA cm−<sup>2</sup> , which is lower than that of Cu/Cu3P nanoarray-290 (η<sup>10</sup> = 342 mV) and Cu/Cu3P nanoarray-310 (η<sup>10</sup> = 395 mV). Moreover, an overpotential of 424 mV is required for Cu/Cu3P nanoarray-270 to reach the current density of 100 mA cm−<sup>2</sup> , which is much lower than that of Cu/Cu3P nanoarray-290 (η<sup>100</sup> = 589 mV) and Cu/Cu3P nanoarray-310 (η<sup>100</sup> = 635 mV).

correction. The catalytic behavior of Cu/Cu3P NS obtained by the direct phosphating of the Cu nanosheet was also investigated for comparison. Obviously, the Cu/Cu3P NS showed poor electrocatalytic activity, with an onset overpotential value of 347 mV. In sharp contrast, Cu/Cu3P nanoarray-270 was significantly active for the HER, with an onset overpotential as low as 96 mV, and additional negative potential leads to a rapid The Tafel slope is an effective means to assess the advantages of electrocatalysts. The Tafel plots in Figure 7b were obtained from the linear portion that conformed to the Tafel equation (η = a + b log *j*, where b is the Tafel slope and *j* is the current density). It can be seen that the Tafel slope for Cu/Cu3P nanoarray-270 is 131 mV dec−<sup>1</sup> , much lower than that of Cu/Cu3P nanoarray-290 (145 mV dec−<sup>1</sup> ) and Cu/Cu3P nanoarray-310 (156 mV dec−<sup>1</sup> ).

rise in the cathodic current. It requires 253 mV of overpotential (η10) to reach a current

mV) and Cu/Cu3P nanoarray-310 (η10 = 395 mV). Moreover, an overpotential of 424 mV is required for Cu/Cu3P nanoarray-270 to reach the current density of 100 mA cm−2, which is much lower than that of Cu/Cu3P nanoarray-290 (η100 = 589 mV) and Cu/Cu3P

nanoarray-310 (η100 = 635 mV).

These results indicate that Cu/Cu3P nanoarray-270 exhibits high electrocatalytic efficiency. A detailed comparison of Cu/Cu3P nanoarray-270 with other electrocatalysts is shown in Table S1, indicating its superior or comparable performance [56–59]. *Catalysts* **2022**, *12*, 762 8 of 12

**Figure 7.** Electrocatalytic activity of the as−prepared Cu/Cu3P nanoarray electrode for HER in 0.5 M H2SO4. (**a**) Polarization curves, (**b**) Tafel plots, (**c**) EIS Nyquist plots (inset: the equivalent circuit), (**d**) current density curve related to time at 23 mA cm<sup>−</sup>2. **Figure 7.** Electrocatalytic activity of the as−prepared Cu/Cu3P nanoarray electrode for HER in 0.5 M H2SO<sup>4</sup> . (**a**) Polarization curves, (**b**) Tafel plots, (**c**) EIS Nyquist plots (inset: the equivalent circuit), (**d**) current density curve related to time at 23 mA cm−<sup>2</sup> .

The Tafel slope is an effective means to assess the advantages of electrocatalysts. The Tafel plots in Figure 7b were obtained from the linear portion that conformed to the Tafel equation (η = a + b log *j*, where b is the Tafel slope and *j* is the current density). It can be seen that the Tafel slope for Cu/Cu3P nanoarray-270 is 131 mV dec−1, much lower than that of Cu/Cu3P nanoarray-290 (145 mV dec−1) and Cu/Cu3P nanoarray-310 (156 mV dec−1). These results indicate that Cu/Cu3P nanoarray-270 exhibits high electrocatalytic efficiency. A detailed comparison of Cu/Cu3P nanoarray-270 with other electrocatalysts is shown in Table S1, indicating its superior or comparable performance [56–59]. The long-term stability of an electrode is another important issue to consider for practical applications. The durability of Cu/Cu3P nanoarray-270 was examined at 23 mA cm−2 in H2SO4 solution, as shown in Figure 7c. The current density curve related to time reveals a minor increase after 15 h, indicating the high electrochemical stability of the Cu/Cu3P nanoarray catalysts for the HER in an acidic solution. Electrochemical impedance spectroscopy (EIS) was performed to identify the interfacial properties and catalytic kinetics of the as-synthesized Cu/Cu3P nanoarray catalyst in the HER process. The long-term stability of an electrode is another important issue to consider for practical applications. The durability of Cu/Cu3P nanoarray-270 was examined at 23 mA cm−<sup>2</sup> in H2SO<sup>4</sup> solution, as shown in Figure 7c. The current density curve related to time reveals a minor increase after 15 h, indicating the high electrochemical stability of the Cu/Cu3P nanoarray catalysts for the HER in an acidic solution. Electrochemical impedance spectroscopy (EIS) was performed to identify the interfacial properties and catalytic kinetics of the as-synthesized Cu/Cu3P nanoarray catalyst in the HER process. As shown in Figure 7d (inset: the equivalent circuit), the series resistance values (*R*s) were obtained in the highfrequency zone, and the semicircle in the low-frequency range reflects the charge transfer resistance at the interface between the Cu/Cu3P and the electrolyte (*R*ct). The Nyquist plots reveal that Cu/Cu3P nanoarray-270 (4.1Ω) exhibits a much smaller semicircle than Cu/Cu3P nanoarray-310 (49.6 Ω), suggesting that it has fast charge transfer kinetics for the HER. This result validates that the introduced Cu nanosheet, as a conductive substrate and nano-template, can improve the charge transport and electrochemical activity of the Cu/Cu3P nanoarray electrode.

#### As shown in Figure 7d (inset: the equivalent circuit), the series resistance values (*R*s) were obtained in the high-frequency zone, and the semicircle in the low-frequency range **3. Materials and Methods**

#### reflects the charge transfer resistance at the interface between the Cu/Cu3P and the *3.1. Chemicals and Materials*

electrolyte (*R*ct). The Nyquist plots reveal that Cu/Cu3P nanoarray-270 (4.1Ω) exhibits a much smaller semicircle than Cu/Cu3P nanoarray-310 (49.6 Ω), suggesting that it has fast charge transfer kinetics for the HER. This result validates that the introduced Cu nanosheet, as a conductive substrate and nano-template, can improve the charge Copper(II) sulfate (CuSO4·5H2O), glucose (C6H12O6), polyvinylpyrrolidone (PVP, M<sup>w</sup> = 30,000), hydrogen peroxide (H2O2, wt% = 30%), Nafion solution and sodium hypophosphite (NaH2PO2) were purchased from Sigma-Aldrich. All chemicals were used without further purification.

#### transport and electrochemical activity of the Cu/Cu3P nanoarray electrode. *3.2. Synthesis of Cu Nanosheets*

without further purification.

**3. Materials and Methods**  *3.1. Chemicals and Materials*  All chemicals in the experiment were analytical grade and used without purification. The well-defined Cu nanosheets were prepared according to the procedures in our previous

Copper(II) sulfate (CuSO4·5H2O), glucose (C6H12O6), polyvinylpyrrolidone (PVP, Mw = 30,000), hydrogen peroxide (H2O2, wt% = 30%), Nafion solution and sodium

report [60]. In brief, 1.0 g C6H12O6·H2O, 0.5 g polyvinyl pyrrolidone (PVP) and CuSO<sup>4</sup> were dissolved in 25 mL of deionized water with vigorous magnetic stirring, and then the mixture was transferred into a Teflon-lined autoclave and heated at 180 ◦C for 3 h. The brown-red products were collected, washed three times with deionized water and ethanol, respectively, and then dried in a vacuum at 60 ◦C.

#### *3.3. Synthesis of Cu/CuO Nanoarrays*

The hierarchical Cu nanosheet@CuO nanorods were synthesized by a simple hydrothermal process. In a typical synthesis procedure, an amount of Cu nanosheets and 22 mL of NaOH (0.55 mol/L) were added into a Teflon-lined vessel with vigorous magnetic stirring, and then 2 mL H2O<sup>2</sup> (30%) was injected rapidly into the mixture solution under stirring. Afterward, the vessel was sealed and then hydrothermally heated at 130 ◦C for 9 h; the as-prepared products were collected and washed three times with deionized water, and then dried in a vacuum at 60 ◦C.
