Borate Anion Dopant Inducing Oxygen Vacancies over Co3O4 Nanocages for Enhanced Oxygen Evolution

The rational design of cost effective and highly efficient oxygen evolution reaction (OER) catalysts plays an extremely important role in promoting the commercial applications of electrochemical water splitting. Herein we reported a sacrificial template strategy for the preparation of borate anion doped Co3O4@ZIF-67 nanocages assembled with nanosheets (B-Co3O4@ZIF-67) by hydrothermal boronation of zeolitic imidazolate framework-67 (ZIF-67). During the preparation process, two different kinds of borate anion sources were found to regulate the morphological structures by tuning the etching rate between ZIF precursors and the borate anion. Moreover, borate anion doping was also found to induce oxygen vacancy defects, which is beneficial for modulating the electronic structure and accelerating electron transport. Meanwhile, the resultant B-Co3O4@ZIF-67 nanocages possess a large specific surface area, which is beneficial for the mass transfer of the electrolyte and exposing more catalytic active sites. Benefiting from the advantages above, the resultant B-Co3O4@ZIF-67 nanocages exhibit impressive OER performance with a small overpotential of 334 mV, a current density of 10 mA cm−2, a small Tafel slope of 73.88 mV dec−1, as well as long-term durability in an alkaline electrolyte.


Introduction
Hydrogen as a clean energy carrier with high energy density (282 kJ·mol −1 ) is considered most promising for replacing traditional fossil fuels to cope with the increasing global energy demand and environmental issues [1][2][3][4]. Electrochemical water splitting (2H 2 O → 2H 2 + O 2 ), consisting of two half reactions of the oxygen evolution reaction (OER) and the hydrogen evolution reaction (HER), provides a green technology for hydrogen production through the use of renewable energy (such as wind energy, solar energy, tidal energy, etc.) [5][6][7]. Relative to the HER, the OER is a four-electron proton coupled transfer process, and possesses sluggish kinetics, severely limiting the efficiency of overall water splitting [8][9][10]. To date, the state-of-the-art OER catalysts mainly focus on precious metal catalysts (such as RuO 2 and IrO 2 ), but their scarcity and high cost limit their implementation in practical commercial applications [11,12]. Therefore, it is essential, yet remains a huge challenge for development of cost effective and highly efficient oxygen evolution reaction (OER) catalysts.
Recently, various transition-metal-based materials, including transition metal oxides [13], phosphides [14,15], sulfides [16], borides [17], (oxy) hydroxides [18], and layered double hydroxides (LDHs) [19,20], have been widely studied as a promising substitute to precious metal OER catalysts. Particularly, Co 3 O 4 -based materials have received increasing attention as promising alternatives due to their good OER catalytic activity in alkaline solution [21,22]. Nevertheless, the poor electronic conductivity of Co 3 O 4 is the main bottleneck hindering the improvement of its OER activity [23,24]. In this regard, the regulation in morphologic and electronic structure has been reported as an effective way to improve the electrochemical performances of Co 3 O 4 -based materials [25][26][27]. On one hand, the unique nanostructures, such as nanosheets and nanocages, usually possess large specific surface area, which are beneficial to the mass transport and exposure of catalytically active sites, and the release of the generated gas during the water splitting process [24,[27][28][29][30]. On the other hand, recent studies have shown that the introduction of dopants can induce the formation of a large number of oxygen vacancy defects, increasing electronic conductivity and promoting the improvement of electrochemical OER performance [31,32]. For instance, the introduction of boron into transition metal compounds was reported to induce vacancy defects and result in the generation of large numbers of catalytically active sites, promoting the improvement of electrochemical performances [24,31,33]. Based on the above considerations, it can be reasonable to conclude that high OER catalytic activity can be expected for heteroatom-doped Co 3 O 4 -based materials with nanocages structures composed of ultrathin nanosheets.
Metal-organic frameworks (MOFs), consisting of inorganic metal ions/clusters coordinated with organic ligands, are distinctive organic-inorganic hybrid porous materials with controllable porous structures, high specific surface areas and well-tunable structures [34,35]. Because of these unique structural merits, MOFs and their derivatives have been widely applied in energy storage and conversion [36,37], gas adsorption and separation [38,39] and other research fields. Generally, MOFs are used as sacrificial templates for the fabrication of various nanostructured materials that inherit the advantages of their precursors [8]. The large specific surface area of MOFs-derived nanostructured materials is conducive to exposing more catalytically active sites and promoting charge and mass transfer during the OER process [40]. Inspired by this, herein we propose an easy and effective strategy for the synthesis of MOF-derived borate anion doped cobalt oxide (B-Co 3 O 4 @ZIF-67) nanocages assembled with nanosheets by hydrothermal boronation. Meanwhile, the type of boron source and solvent system were also optimized, and boratebuffered methanol was found to be the optimal condition for the formation of unique nanocage structures composed of nanosheets. The unique nanocage structures create the large specific surface area (705.77 m 2 g −1 ), thus facilitating the exposure of catalytically active sites and accelerating mass transfer and gas release during the OER process. Moreover, borate anion doping is also conducive to the formation of oxygen vacancy defects, thus modulating the electronic structure of atoms and promoting improvement in catalytic OER activity. As expected, the resultant B-Co 3 O 4 @ZIF-67 exhibited superior OER activity in alkaline solution.

Results and Discussion
The schematic illustration for the preparation of the B-Co 3 O 4 -2@ZIF-67 nanocages is shown in Figure 1. Briefly, the uniform ZIF-67 nanocubes were first synthesized by the reaction of Co(NO 3 ) 2 ·6H 2 O with 2-methylimidazole under the assistance of CTAB. Subsequently, B-Co 3 O 4 -2@ZIF-67 nanocages were successfully obtained through the hydrothermal reaction of ZIF-67 with borate buffers solution (BBS). The pH value of the BBS solution, containing a large amount of borate ion (B 4 O 7 2− ), was measured to be 9.5. During the hydrothermal reaction process, hydroxyl ions (OH − ) were produced through the hydrolysis of B 4 O 7 2− , which then replaced 2-methylimidazole within ZIF-67 precursor to form Co(OH) 2 , which were finally transformed into B-doped Co 3 O 4 under high temperatures due to the existence of dissolved oxygen and a lot of borate ions (B 4 O 7 2− ) in the reaction system [41]. The morphological structures of the resultant ZIF-67 precursors and their derivatives were investigated by FESEM and TEM. As shown, uniform cubic morphology was observed for the resultant ZIF-67 precursor with an average size of 1 μm ( Figures S1 and S2), which is in accordance with the previously reported results [42,43]. After the hydrothermal reaction of ZIF-67 precursor with BBS in methanol, the resultant ZIF-67 nanocubes were transformed into B-Co3O4-2@ZIF-67 nanocubes assembled with nanosheets ( Figure  2a Interestingly, when we only used K2B4O7·4H2O as a boron source, nanosheets-assembled core-shell structured B-Co3O4-1@ZIF-67 can be obtained ( Figure S4a,b), which could be further confirmed by TEM images (Figure S4c-e). Similarly, HRTEM images and SAED patterns also proved the amorphous nature of the resultant B-Co3O4-1@ZIF-67 ( Figure  S4f,g). In the contrast, CoBi/ZIF-67 is composed of the residual ZIF-67 and cobalt borate (Co-Bi) nanosheets in the presence of H3BO3 as a boron source ( Figure S4h,i). We inferred that the formation of core-shell structure may be attributed to the incomplete etching process due to the insufficient amount of B4O7 2− only in the presence of K2B4O7. Differently, boric acid used as a boron source can produce protons (H + ) for the protonation of 2-methylimidazole, resulting in the release of Co 2+ and then reacting with the borate ions (B4O7 2− ) to form cobalt borate (Co-Bi) nanosheets. In addition, the effect of the solvent in the reaction system on the morphology of the resultant catalysts was also investigated. Under the same reaction conditions, the introduction of water resulted in the complete destruction of morphology from the nanocubes into irregular structures (nanowires and nanoparticles) ( Figure S5), which may be attributed to the fast etching rate. These results demonstrate that the morphologic structures of the resultant catalysts can be regulated through tuning the boron source and solvent during the preparation process. Besides, potassium hydroxide was selected as a substitute of K2B4O7·4H2O to provide an alkaline environment. Only a small number of nanosheets were formed on the surface of ZIF-67 precursor, but the cubic morphology of ZIF-67 precursor was still well-retained ( Figure S6). These results demonstrate that the presence of borate ion is essential for the formation of nanocages. The morphological structures of the resultant ZIF-67 precursors and their derivatives were investigated by FESEM and TEM. As shown, uniform cubic morphology was observed for the resultant ZIF-67 precursor with an average size of 1 µm ( Figures S1 and S2), which is in accordance with the previously reported results [42,43]. After the hydrothermal reaction of ZIF-67 precursor with BBS in methanol, the resultant ZIF-67 nanocubes were transformed into B-Co 3 O 4 -2@ZIF-67 nanocubes assembled with nanosheets ( Figure 2a Figure S4h,i). We inferred that the formation of core-shell structure may be attributed to the incomplete etching process due to the insufficient amount of B 4 O 7 2− only in the presence of K 2 B 4 O 7 . Differently, boric acid used as a boron source can produce protons (H + ) for the protonation of 2-methylimidazole, resulting in the release of Co 2+ and then reacting with the borate ions (B 4 O 7 2− ) to form cobalt borate (Co-Bi) nanosheets. In addition, the effect of the solvent in the reaction system on the morphology of the resultant catalysts was also investigated. Under the same reaction conditions, the introduction of water resulted in the complete destruction of morphology from the nanocubes into irregular structures (nanowires and nanoparticles) ( Figure S5), which may be attributed to the fast etching rate. These results demonstrate that the morphologic structures of the resultant catalysts can be regulated through tuning the boron source and solvent during the preparation process. Besides, potassium hydroxide was selected as a substitute of K 2 B 4 O 7 ·4H 2 O to provide an alkaline environment. Only a small number of nanosheets were formed on the surface of ZIF-67 precursor, but the cubic morphology of ZIF-67 precursor was still well-retained ( Figure S6). These results demonstrate that the presence of borate ion is essential for the formation of nanocages. The phase composition and crystal structure of the resultant materials were characterized by XRD. As observed, there are residual ZIF-67 precursors in the resultant B-Co3O4-2@ZIF-67, B-Co3O4-1@ZIF-67, and CoBi/ZIF-67 regardless of the type of boron source ( Figure S7), which could be clearly observed from TEM images ( Figure S4). Nevertheless, the diffraction peak intensity assigned to ZIF-67 obviously decreases for the resultant B-Co3O4-2@ZIF-67, implying the more thorough etching of ZIF-67 precursor when reacting with the BBS solution compared to K2B4O7 and H3BO3. Besides, there are not any crystal diffraction peaks except for those assigned to ZIF-67, demonstrating the amorphous nature of the newly formed nanosheets after reacting with different boron sources. Unexpectedly, all of the diffraction peaks assigned to ZIF-67 disappeared completely whereas new diffraction peaks indexed to the Co3O4 (JCPDS No. 74-2120) could be observed after the introduction of water in the reaction system ( Figure S8a) [44]. Moreover, the diffraction peak intensity increased as the addition of water increased, which may explain why there is poor crystallinity for the resultant B-Co3O4-2@ZIF-67 nanocages despite the introduction of a very small amount of water from K2B4O7·4H2O. It should be noted that no peaks assigned to cobalt borate were detected for all of the above XRD patterns, indicating that there was no formation of a new crystalline phase after the addition of a boron source. Careful observation demonstrates the appearance of the diffraction peak assigned to the (511) crystal plane of Co3O4 in the XRD patterns of the resultant B-Co3O4-1, B-Co3O4-2 and B-Co3O4-2@ZIF-67 ( Figure S8b), which all shifted the lower Bragg angle relative to standard diffraction peak (59.35°) of the (511) crystal plane of Co3O4. The negative shift of the Bragg angle indicates the expansion of the crystal lattice at the same incident wavelength [45], indicating that boron as dopant may be incorporated into the crystal structure Co3O4. Based on the XRD results, we inferred that B-doped cobalt oxide  Figure S7), which could be clearly observed from TEM images ( Figure S4). Nevertheless, the diffraction peak intensity assigned to ZIF-67 obviously decreases for the resultant B-Co 3 O 4 -2@ZIF-67, implying the more thorough etching of ZIF-67 precursor when reacting with the BBS solution compared to K 2 B 4 O 7 and H 3 BO 3 . Besides, there are not any crystal diffraction peaks except for those assigned to ZIF-67, demonstrating the amorphous nature of the newly formed nanosheets after reacting with different boron sources. Unexpectedly, all of the diffraction peaks assigned to ZIF-67 disappeared completely whereas new diffraction peaks indexed to the Co 3 O 4 (JCPDS No. 74-2120) could be observed after the introduction of water in the reaction system ( Figure S8a) [44]. Moreover, the diffraction peak intensity increased as the addition of water increased, which may explain why there is poor crystallinity for the resultant B-Co 3 O 4 -2@ZIF-67 nanocages despite the introduction of a very small amount of water from K 2 B 4 O 7 ·4H 2 O. It should be noted that no peaks assigned to cobalt borate were detected for all of the above XRD patterns, indicating that there was no formation of a new crystalline phase after the addition of a boron source. Careful observation demonstrates the appearance of the diffraction peak assigned to the (511) crystal plane of Co 3 O 4 in the XRD patterns of the resultant B-Co 3 O 4 -1, B-Co 3 O 4 -2 and B-Co 3 O 4 -2@ZIF-67 ( Figure S8b), which all shifted the lower Bragg angle relative to standard diffraction peak (59.35 • ) of the (511) crystal plane of Co 3 O 4 . The negative shift of the Bragg angle indicates the expansion of the crystal lattice at the same incident wavelength [45], indicating that boron as dopant may be incorporated into the crystal structure Co 3 O 4 . Based on the XRD results, we inferred that B-doped cobalt oxide (denoted as B-Co 3 O 4 ) was successfully formed by replacing oxygen ions (140 pm) in cobalt oxide with borate ions (191 pm) [2]. In order to further confirm the successful synthesis of B-Co 3 O 4 , the resultant B-Co 3 O 4 -2@ZIF-67 samples were further annealed at 700 • C for 1 h in air atmosphere. As shown in Figure S8c, eight diffraction peaks at 19 Figure S9 and Table S2), further confirming the successful doping of B into the Co 3 O 4 .
FT-IR spectra were also performed to investigate the surface functional groups and the skeleton changes of the resultant catalysts [46]. For ZIF-67 precursor, there is the apparent stretching vibration at 425 cm −1 related to the characteristic peak of Co-N ( Figure S10), which confirms the bonding between the cobalt atom and the N atom in the 2-methylimidazole linker in ZIF-67 [47]. The peaks in the region of 600-1500 cm −1 contribute to the bending and stretching modes of the imidazole ring in ZIF-67 [48]. The characteristic peaks at 693 cm −1 and 756 cm −1 can be ascribed to the out-of-plane bending vibration mode of the imidazole ring [49], while the in-plane bending vibration of the imidazole ring can be observed at 900-1350 cm −1 [50]. Additionally, the obvious characteristic peaks in the range 1350-1500 cm −1 can be attributed to the stretching vibration mode of the ring [51]. The peak at 1580 cm −1 can be associated with the stretching vibration of the C=N bond in 2-methylimidazole ligand [52]. Moreover, the peak at 2929 cm −1 and 3134 cm −1 are caused by the C-H stretching vibration of the aromatic ring and the aliphatic methyl group in 2-methylimidazole, respectively [47]. The above results demonstrate the successful synthesis of the ZIF-67 precursor. After the reaction of ZIF-67 precursor with different boron sources, there is new peak vibration in the range 480-660 cm −1 corresponding to the formation of a metal-oxygen bond (M-O) [53]. Meanwhile, the intensity of the vibration peak assigned to the ZIF-67 precursor decreases with the amount of boron source added, indicating the transformation of ZIF-67 into other components. Some characteristic peaks related to ZIF-67 precursor almost disappear after the introduction of water ( Figure S11), indicating that the material skeleton on the surface of ZIF-67 collapsed [46]. Meanwhile, there are two sharp characteristic peaks at 575 cm −1 and 667 cm −1 in the spectra, which contributed to the stretching vibration mode of octahedral coordinated Co 3+ -O bonding and tetrahedral coordinated Co 2+ -O bonding in Co 3 O 4 , respectively [54,55]. The broad absorption peak at 3440 cm −1 is due to the vibration of O-H from surface water molecules [51,56]. These results demonstrate that the main component was Co 3 O 4 after the introduction of water, which is consistent with the XRD results. Combined with the appearance of metal-oxygen bonds after the introduction of different boron sources, we can infer that we successfully synthesized B-Co 3 O 4 .
In addition, UV-Vis absorption spectra were also carried out by dispersing the resultant catalysts into ethanol with a constant concentration in the range of 400 to 700 nm. As displayed in Figure S12, the ZIF-67 precursor has characteristic transitions of tetrahedral Co 2+ at 539 nm and 596 nm, respectively [47]. Moreover, the characteristic transition peak can be well-retained after reaction with different boron sources and potassium hydroxide, and the intensity of the B-Co 3 O 4 -2@ZIF-67 peak is much lower than that of the ZIF-67 precursor, indicating that there remain ZIF-67 residues in the resultant B-Co 3 O 4 -2@ZIF-67, which is consistent with the above mentioned FESEM and TEM analysis results.
Nitrogen adsorption-desorption isotherms were performed to investigate the specific surface area of the resultant B- mesopores, with their average pore diameters being 2.97 and 7.98 nm, respectively [59]. The large specific surface area and microporous structure of the resultant B-Co 3 O 4 -2@ZIF-67 are beneficial for exposing more active sites and accelerating mass transfer, which can improve the catalytic activity of OER [60].  [59]. The large specific surface area and microporous structure of the resultant B-Co3O4-2@ZIF-67 are beneficial for exposing more active sites and accelerating mass transfer, which can improve the catalytic activity of OER [60].  Figure  S12b), there are two strong peaks at binding energies of 781.57 eV and 797.16 eV corresponding to Co 2+ species whereas the other two peaks at 780.10 eV and 795.80 eV can be attributed to Co 3+ species [8,56,61]. In addition, the other two peaks at 785.06 eV and 801.71 eV are shakeup satellite peaks. Specifically, by calculating the integrated peak area, the atomic ratio of Co 3+ /Co 2+ is 1.13 in the resultant Co(OH)2@ZIF-67, implying the partial oxidization of Co 2+ in alkaline solution during the hydrothermal process. Compared with Co(OH)2@ZIF-67, the binding energy of Co 2+ (781.89 eV) and Co 3+ (780.48 eV) has a significant positive shift in the resultant B-Co3O4-1@ZIF-67, demonstrating that doping with electron negativity borate anions induced the formation of a higher oxidation state [33]. This phenomenon may be attributed to the electron transfer from Co atoms to the borate anion dopant due to the large electron negativity of the borate anion relative to that of the metal Co [62]. In addition, the integrated peak area ratio of Co 3+ /Co 2+ was calculated to be 0.961 in the resultant B-Co3O4-1@ZIF-67, which is lower than the theoretical value of Co 3+ /Co 2+ (2:1) in Co3O4. It should be here noted that a certain amount of Co 2+ in the resultant B-Co3O4-1@ZIF-67 comes from the coordinated Co atoms of the ZIF-67 residues. Similarly, the more positive shift in binding energy of Co 2+ (782.20 eV) and Co 3+ (780.80 eV) in the resultant B-Co3O4-2@ZIF-67 was observed compared to the resultant B-Co3O4-1@ZIF-67 (Figure 4b), and the intensity of Co 3+ /Co 2+ was 1.15. The obvious change in binding energy may be attributed to the introduction of more borate anions when reacting the ZIF-67 precursor with the BBS solution (Table S3), which can be further confirmed by the highresolution B 1s XPS spectra of B-Co3O4-2@ZIF-67 ( Figure 4c). As shown, the peak at 192.3 eV, which is assigned to three-coordinated borate species (B-O), proved that boron atoms in the form of borate were incorporated into the crystal structure of Co3O4 [63,64]. In this process, B4O7 2− partially replaced the oxygen anions (O 2− ) in the Co3O4 lattice, thereby destroying the original crystalline structure and producing a large number of oxygen vacancy defects [27,65]. Therefore, we used electron paramagnetic resonance (EPR) spectra to analyze and detect the content of unpaired electronic species (oxygen vacancy defects) in the resultant B-Co3O4-1@ZIF-67 and B-Co3O4-2@ZIF-67 [27]. As shown in Figure S14, the resultant B-Co3O4-2@ZIF-67 produces more high-energy dangling bonds than B-  (Figure 2g), while the resultant Co(OH) 2 @ZIF-67 contains C, N, O, and Co elements. In the high-resolution Co XPS 2p spectra of Co(OH) 2 @ZIF-67 samples ( Figure S12b), there are two strong peaks at binding energies of 781.57 eV and 797.16 eV corresponding to Co 2+ species whereas the other two peaks at 780.10 eV and 795.80 eV can be attributed to Co 3+ species [8,56,61]. In addition, the other two peaks at 785.06 eV and 801.71 eV are shakeup satellite peaks. Specifically, by calculating the integrated peak area, the atomic ratio of Co 3+ /Co 2+ is 1.13 in the resultant Co(OH) 2 @ZIF-67, implying the partial oxidization of Co 2+ in alkaline solution during the hydrothermal process. Compared with Co(OH) 2 @ZIF-67, the binding energy of Co 2+ (781.89 eV) and Co 3+ (780.48 eV) has a significant positive shift in the resultant B-Co 3 O 4 -1@ZIF-67, demonstrating that doping with electron negativity borate anions induced the formation of a higher oxidation state [33]. This phenomenon may be attributed to the electron transfer from Co atoms to the borate anion dopant due to the large electron negativity of the borate anion relative to that of the metal Co [62]. In addition, the integrated peak area ratio of Co 3+ /Co 2+ was calculated to be 0.961 in the resultant B-Co 3 O 4 -1@ZIF-67, which is lower than the theoretical value of Co 3+ /Co 2+  (Table S3), which can be further confirmed by the high-resolution B 1s XPS spectra of B-Co 3 O 4 -2@ZIF-67 ( Figure 4c). As shown, the peak at 192.3 eV, which is assigned to three-coordinated borate species (B-O), proved that boron atoms in the form of borate were incorporated into the crystal structure of Co 3 O 4 [63,64]. In this process, B 4 O 7 2− partially replaced the oxygen anions (O 2− ) in the Co 3 O 4 lattice, thereby destroying the original crystalline structure and producing a large number of oxygen vacancy defects [27,65]. Therefore, we used electron paramagnetic resonance (EPR) spectra to analyze and detect the content of unpaired electronic species (oxygen vacancy defects) in the resultant B-Co 3 O 4 -1@ZIF-67 and B-Co 3 O 4 -2@ZIF-67 [27]. As shown in Figure S14, the resultant B-Co 3 O 4 -2@ZIF-67 produces more high-energy dangling bonds than B-Co 3 O 4 -1@ZIF-67, indicating that the resultant B-Co 3 O 4 -2@ZIF-67 possesses higher concentrations of oxygen vacancy defects [32]. It has been reported that the introduction of defects is beneficial for exposing more catalytically active sites. Co3O4-1@ZIF-67, indicating that the resultant B-Co3O4-2@ZIF-67 possesses higher concentrations of oxygen vacancy defects [32]. It has been reported that the introduction of defects is beneficial for exposing more catalytically active sites. In the high-resolution C 1s spectra of B-Co3O4-2@ZIF-67 (Figure 4d), there are three distinct characteristic peaks at 284.8, 285.9, and 289.0 eV, which are attributed to sp 2 bonded carbon (C-C), sp 2 hybrid C-N bonds, and the bond between carbon and surface oxygen (O-C=O), respectively [66,67]. The high-resolution N 1s XPS spectra (Figure 4e) can be deconvoluted into three peaks corresponding to the pyridine-N (399.0 eV) and pyrrolic-N (399.8 eV) [68]. As shown in Figure 4f, the high-resolution O 1s XPS spectra can be divided into four characteristic peaks, where the binding energy at 530.9 contributes to the lattice oxygen (M-O, OI), and the binding energy at 531.36 eV can be assigned to the oxygen vacancy (Vo, OII) [31]. The resultant B-Co3O4-1@ZIF-67 and B-Co3O4-2@ZIF-67 both have vacant oxygen (Vo, OII) peaks whereas Co(OH)2@ZIF-67 only contains two oxygen species of lattice oxygen (M-O, 530.74 eV) and adsorbed oxygen (OIII, 531.53 eV) ( Figure  S12f), proving that the introduction of boron leads to the formation of oxygen vacancy defects. The existence of oxygen vacancy defects has been reported to facilitate the adsorption of water molecules and OHanions during the OER process, thus promoting the water oxidation process [69]. Additionally, the binding energy at 532.2 and 533.1 eV were associated with the adsorbed oxygen species (OIII) and surface water molecules (OIV) on the catalysts' surface, respectively [70].
The electrocatalytic OER performances of the resultant catalysts were investigated in a typical three-electrode system with a rotating disk electrode (RDE) at the rotating speed of 1600 rpm in 1.0 MKOH. The catalyst loading amount was fixed at 0.5 mg/cm 2 , and all electrochemical data has been corrected by iRs compensation to eliminate the influence of ohmic voltage drop [71]. As shown in Figure 5a and Table S4, the resultant B-Co3O4-2@ZIF-67 exhibits the best OER performance with the largest current density among the investigated catalysts. Moreover, the overpotential at a current density of 10 mA cm −2 is 334 mV for the resultant B-Co3O4-2@ZIF-67, which is significantly lower than that of B-Co3O4-1@ZIF-67 (349 mV) and CoBi/ZIF-67 (341 mV). Besides, the lower OER performances of the resultant B-Co3O4-1 (351 mV) and B-Co3O4-2 (346 mV) prepared by the introduction of water were observed compared to the B-Co3O4-2@ZIF-67 (Figure S15a and In the high-resolution C 1s spectra of B-Co 3 O 4 -2@ZIF-67 (Figure 4d), there are three distinct characteristic peaks at 284.8, 285.9, and 289.0 eV, which are attributed to sp 2 bonded carbon (C-C), sp 2 hybrid C-N bonds, and the bond between carbon and surface oxygen (O-C=O), respectively [66,67]. The high-resolution N 1s XPS spectra (Figure 4e) can be deconvoluted into three peaks corresponding to the pyridine-N (399.0 eV) and pyrrolic-N (399.8 eV) [68]. As shown in Figure 4f Figure S12f), proving that the introduction of boron leads to the formation of oxygen vacancy defects. The existence of oxygen vacancy defects has been reported to facilitate the adsorption of water molecules and OH − anions during the OER process, thus promoting the water oxidation process [69]. Additionally, the binding energy at 532.2 and 533.1 eV were associated with the adsorbed oxygen species (O III ) and surface water molecules (O IV ) on the catalysts' surface, respectively [70].
The electrocatalytic OER performances of the resultant catalysts were investigated in a typical three-electrode system with a rotating disk electrode (RDE) at the rotating speed of 1600 rpm in 1.0 MKOH. The catalyst loading amount was fixed at 0.5 mg/cm 2 , and all electrochemical data has been corrected by iR s compensation to eliminate the influence of ohmic voltage drop [71]. As shown in Figure 5a and Table S4, the resultant B-Co 3 O 4 -2@ZIF-67 exhibits the best OER performance with the largest current density among the investigated catalysts. Moreover, the overpotential at a current density of 10 mA cm −2 is 334 mV for the resultant B-Co 3 O 4 -2@ZIF-67, which is significantly lower than that of B-Co 3 O 4 -1@ZIF-67 (349 mV) and CoBi/ZIF-67 (341 mV). Besides, the lower OER performances of the resultant B-Co 3 O 4 -1 (351 mV) and B-Co 3 O 4 -2 (346 mV) prepared by the introduction of water were observed compared to the B-Co 3 O 4 -2@ZIF-67 ( Figure S15a and Table S4). In addition, the OER performance of the resultant B-Co 3 O 4 -2@ZIF-67 was also superior to that of the resultant Co(OH) 2 @ZIF-67 (343 mV) and ZIF-67 precursor (371 mV) ( Figure S16a and Table S4). The catalytic kinetics parameter is generally used to evaluate the catalytic performances of the resultant catalysts. In order to get insight into the OER kinetics, a Tafel plot was obtained from the polarization curve according to the Tafel equation [59]: η = blogj + α, where η is the overpotential, j is the current density, b is the Tafel slope, and α is the constant. The resultant B-Co 3 O 4 -2@ZIF-67 presents a smaller Tafel slope (73.88 mVdec −1 ) than the resultant B-Co 3 O 4 -1@ZIF-67 (122.8 mVdec −1 ) and B-Co 3 O 4 /ZIF-67 (99.28 mV dec −1 ) (Figure 5b and Table S4), indicating more favorable OER catalytic kinetics for the resultant B-Co 3 O 4 -2@ZIF-67. The information of the rate determination step during the OER process can be acquired from the Tafel slope [2,72]. When the Tafel slope is less than 40 mVdec −1 and greater than 120 mVdec −1 , the formation of * OOH (O * + OH − → * OOH + e − , where * represents the catalytic active site on the catalysts surface) and * OH (* + OH − → * OH + e − ) are the rate-determining steps, whereas the Tafel slope located between the above two values, the formation of O * (* OH + OH − → * O + H 2 O + e − ) is the rate-determining step. Therefore, the formation of O * is the rate-determining step during the OER process over the resultant B-Co 3 O 4 -2@ZIF-67.
tween the above two values, the formation of O * (* OH + OH − → * O + H2O + e − ) is the rate-determining step. Therefore, the formation of O * is the rate-determining step during the OER process over the resultant B-Co3O4-2@ZIF-67.
It is well known that a highly electrochemically active surface area (ECSA) is beneficial for improving catalytic activity. Cyclic voltammetry (CV) was carried out at different scan rates in the non-faradaic potential region from 1.2 to 1.3 V vs. RHE due to the proportional relationship between ECSA and electrochemical double-layer capacitance (Cdl) [73]. As expected, the resultant B-Co3O4-2@ZIF-67 exhibited the high Cdl value of 65.78 mFcm −2 , which is much higher than that of the resultant B-Co3O4-1@ZIF-67 (35.10 mFcm −2 ) and CoBi/ZIF-67 (48.20 mFcm −2 ), and the other resultant catalysts (Figure 5c, Figures S17 and S18; Table S4). The large ECSA of the resultant B-Co3O4-2@ZIF-67 may be due to its unique nanosheets-assembled nanocage structure, thus exposing more catalytic active sites during the OER process [74]. Electrochemical impedance spectroscopy (EIS) measurements were also performed to explore the interfacial charge transport properties of these catalyst modified electrodes [75]. Unexpectedly, the resultant B-Co3O4-2@ZIF-67 exhibited a larger charge transfer resistance (Rct) than the resultant CoBi/ZIF-67, B-Co3O4-1@ZIF-67 (Figure 5d). In addition, the resultant B-Co3O4-1 and B-Co3O4-2 also exhibited a similar Rct with the resultant B-Co3O4-2@ZIF-67 ( Figure S15d). However, the Rct of the resultant B-Co3O4-2@ZIF-67 was smaller than that of the resultant ZIF-67 precursor and Co(OH)2@ZIF-67 ( Figure S16c). These results show that the Rct of the resultant ZIF-67 can be significantly reduced by one-step hydrothermal boronation treatment, but it is not the dominant factor affecting the catalytic performance of the resultant catalysts. It is well known that a highly electrochemically active surface area (ECSA) is beneficial for improving catalytic activity. Cyclic voltammetry (CV) was carried out at different scan rates in the non-faradaic potential region from 1.2 to 1.3 V vs. RHE due to the proportional relationship between ECSA and electrochemical double-layer capacitance (C dl ) [73]. As expected, the resultant B-Co 3 O 4 -2@ZIF-67 exhibited the high C dl value of 65.78 mFcm −2 , which is much higher than that of the resultant B-Co 3 O 4 -1@ZIF-67 (35.10 mFcm −2 ) and CoBi/ZIF-67 (48.20 mFcm −2 ), and the other resultant catalysts (Figure 5c, Figures S17 and S18; Table S4). The large ECSA of the resultant B-Co 3 O 4 -2@ZIF-67 may be due to its unique nanosheets-assembled nanocage structure, thus exposing more catalytic active sites during the OER process [74]. Electrochemical impedance spectroscopy (EIS) measurements were also performed to explore the interfacial charge transport properties of these catalyst modified electrodes [75]. Unexpectedly, the resultant B-Co 3 O 4 -2@ZIF-67 exhibited a larger charge transfer resistance (R ct ) than the resultant CoBi/ZIF-67, B-Co 3 O 4 -1@ZIF-67 (Figure 5d). In addition, the resultant B-Co 3 O 4 -1 and B-Co 3 O 4 -2 also exhibited a similar R ct with the resultant B-Co 3 O 4 -2@ZIF-67 ( Figure S15d). However, the R ct of the resultant B-Co 3 O 4 -2@ZIF-67 was smaller than that of the resultant ZIF-67 precursor and Co(OH) 2 @ZIF-67 ( Figure S16c). These results show that the R ct of the resultant ZIF-67 can be significantly reduced by one-step hydrothermal boronation treatment, but it is not the dominant factor affecting the catalytic performance of the resultant catalysts.
Long-term stability is another important parameter for evaluating the practical applications of the resultant catalyst [11]. In this regard, continuous CV cycles were conducted over the resultant B-Co 3 O 4 -2@ZIF-67 in the potential range from 1.2 to 1.5 V at the scan rate of 100 mVs −1 in 1.0 M KOH. No obvious decay in the current density was observed after 2000 CV cycles over the resultant B-Co 3 O 4 -2@ZIF-67 (Figure 5e). Meanwhile, the durability was also evaluated by chronopotentiometry at a current density of 10 mAcm −2 for 24 h, and chronoamperometry at the constant of potential corresponding to a current density of 10 mAcm −2 for 15 h. No obvious changes in potential and current density were observed after continuous operation (Figure 5f). These results suggest the excellent long-term durability of the resultant B-Co 3 O 4 -2@ZIF-67 in alkaline media. We also found that the morphologic structure of the resultant B-Co 3 O 4 -2@ZIF-67 can be well-retained after a long-term OER durability test ( Figure S19). The composition and chemical state of the resultant B-Co 3 O 4 -2@ZIF-67 was further investigated by XPS after the long-term OER durability test ( Figure S20). High-resolution Co 2p XPS spectra revealed that the intensity of the Co 3+ (795.22 eV) peak is significantly higher than that of Co 2+ (780.12 eV), and the ratio of Co 3+ /Co 2+ increased from 1.15 to 1.22, indicating that the low-valence Co 2+ is irreversibly oxidized to the high-valence Co 3+ during the OER process ( Figure S20a and Table S3). Differently, B 1's signal peak completely disappeared after the OER (Figure S20b), which may be due to the fact that the B element on the catalyst surface dissolved into the electrolyte during the OER process under the high potential [31]. As shown in Figure S20d

Materials Synthesis
ZIF-67 cubes were firstly prepared according to the previously reported method with slight modification [42] and maintained at 150 • C for 10 h in an electric oven. After being naturally cooled to room temperature, the product was collected via centrifugation (5000 rpm for 5 min), washed with ethanol three times, and finally dried for 30 h at −60 • C in a freeze dryer (SCIENTZ, SCIENCE-10N,Ningbo, China) for further use, which was denoted as B-Co 3 O 4 -2@ZIF-67 (2 represents the number of boron sources). As comparisons, CoBi/ZIF-67 and B-Co 3 O 4 -1@ZIF-67 were also prepared through the same method except for the use of different boron sources: H 3 BO 3 and K 2 B 4 O 7 ·4H 2 O, respectively. B-Co 3 O 4 was also prepared using 30 mL of deionized water and the mixture of water and methanol (v/v = 1:1) instead of methanol, and the resultant products were denoted B-Co 3 O 4 -1 and B-Co 3 O 4 -2, respectively. Meanwhile, Co(OH) 2 @ZIF-67 was also prepared replacing K 2 B 4 O 7 ·4H 2 O with KOH.

Physicochemical Characterization
Powder X-ray diffraction (XRD) patterns were recorded on a Bruker D8 Advance X-ray diffractometer (Karlsruhe, Germany) with Cu-Kα radiation (λ = 1.5406 Å; scan rate: 5 • /min). The morphologic structures were characterized by field-emission scanning electron microscopy (FESEM) on a MIRA3 TESCAN scanning electron microscope operating at 15.0 kV with transmission electron microscopy (TEM, FEI Tecnai G2 F20, Hillsboro, OR, USA) and equipped with an OXFORD X-max 80T energy-dispersive X-ray (EDX) system. Chemical valence and element analysis were conducted by X-ray photoelectron spectroscopy (XPS) on a Thermo Scientific K-Alpha+ instrument (Waltham, MA, USA) operating at 12 kV. All spectra took the C1's peak at binding energy of 284.80 eV as the energy standard. Fourier transform infrared spectroscopy (FT-IR) spectra (4000-400 cm −1 ) were measured using KBr as the reference sample on a Thermo Scientific Nicolet iS10 FTIR spectrophotometer (Waltham, MA, USA). UV-Vis absorption spectra were recorded on a UV-Vis spectrophotometer (YOKE INSTRUMENT T2600, Shanghai, China) with a certain concentration (0.5 mg/mL) of catalyst samples in ethanol solution. The specific surface area and pore volume were measured using an AUTOSORB IQ analyzer and analyzed via nitrogen adsorption-desorption isotherm. The pore-size distributions were calculated from the nitrogen desorption isotherms via the Horvaih-Kawazoe (HK) and Barrett-Joyner-Halenda (BJH) methods. The electron paramagnetic resonance (EPR) spectra were recorded on a Bruker EMXplus spectrometer (Karlsruhe, Germany) operated at X-band 9.5 GHz at room temperature.

Electrochemical Measurements
The electrochemical performances were investigated using a CHI 760E electrochemical workstation (CH Instruments, Inc., Shanghai, China) in a typical three-electrode system at room temperature. The catalyst-modified glassy carbon electrode (GCE, diameter: 5 mm) was used as a working electrode, and the GCE was polished with alumina slurry followed by cleaning in water and ethanol successively with ultrasonication prior to use. A carbon rod (Yueci Electronics, Shanghai) and an Ag/AgCl with saturated KCl solution electrode (Pine Research Instrumentation, Durham, NC, USA) were used as the counter electrode and reference electrode, respectively. The catalyst inks were prepared through dispersing 5 mg of the resultant catalyst into a mixture of 980 µL ethanol and 20 µL Nafion (5 wt.%, DuPont, Shenzhen, China) under ultrasonication for 40 min. Then 20 µL of the obtained ink was dropped on the surface of the polished GCE and dried in ambient conditions to form a uniform thin catalyst layer (we calculated the amount of catalyst loading to be 0.50 mg cm −2 ). For the durability test, the electrode was also fabricated using carbon paper (CP, 1 cm 2 in area, Comston Technology, Shenzhen, China). All the measured potentials were converted to the reversible hydrogen electrode (RHE) according the equation: E RHE = E Ag/AgCl + 0.215 + 0.059 pH. The 1.0 M KOH aqueous solution was used as the electrolyte for OER performance measurements. The rotation speed of the rotating disk electrode (RDE) was fixed at 1600 rpm for all the measurements. Prior to the linear sweep voltammetry (LSV) test, the working electrode was activated by applying continuous cyclic voltammetry (CV) several times between 1.2 and 1.5 V in 1.0 M KOH with a scan rate of 100 mVs −1 until the stable CV curves were obtained. The LSV curves were measured by sweeping the potential from 1.2 to 1.8 V vs. RHE with a scan rate of 5 mVs −1 . The electrochemical impedance spectroscopy (EIS) measurements were carried out in a frequency range from 100 KHz to 0.01 Hz at 1.5 V by applying an alternating current (AC) voltage with 5 mV amplitude. The electrochemical double layer capacitance (C dl ) of different catalysts were measured using cyclic voltammetry in a non-faradaic region from 1.2 to 1.3 V vs. RHE with different scan rates of 5, 10, 15, 20, and 25 mVs −1 . The durability of the catalyst was evaluated according to the following methods: a polarization curve after 2000 CV cycles, chronopotentiometry at the fixed current density of 10 mAcm −2 , and chronoamperometry at the fixed potential corresponding to the current density of 10 mAcm −2 . All electrochemical potentials were corrected by iR s compensation except for the chronopotential curve. The equivalent circuit of electrochemical impedance spectroscopy (EIS) was fitted by ZView software (Southern Pines, NC, USA).

Conclusions
In summary, B-Co 3 O 4 @ZIF-67 nanocages composed of nanosheets have been successfully prepared by hydrothermal boronation, and investigated as OER catalysts. The optimal B-Co 3 O 4 @ZIF-67 nanocages exhibited superior OER activity with a small overpotential of 330 mV at the current density of 10 mAcm −2 and excellent long-term durability in 1.0 M KOH. The excellent OER performance of B-Co 3 O 4 @ZIF-67 can be attributed to the two following qualities: (1) large specific surface area from unique its nanocages structure assembled with nanosheets, which is helpful in promoting mass transfer and exposing more catalytically active sites; (2) the formation of oxygen vacancy defects induced by borate anion doping, which is beneficial for modulating the electronic structure and improving the conductivity of the catalyst.  1 (a,b), B-Co 3 O 4 -2 (c,d), Co(OH) 2 (e,f) and ZIF-67 (g,h) in 1.0 M KOH solution, Figure S19: Low-magnification (a) and high-magnification (b) FESEM images of the resultant B-Co 3 O 4 -2@ZIF-67 after OER durability test, Figure S20: High-resolution XPS Co 2p spectra (a), B 1s spectra (b), C 1s spectra (c), O 1s spectra (d) of the resultant B-Co 3 O 4 -2@ZIF-67 before and after the stability test, Table S1: Summary of nitrogen adsorption-desorption isotherm data of the resultant B-Co 3 O 4 -1@ZIF-67 and B-Co 3 O 4 -2@ZIF-67,

Institutional Review Board Statement: Not application.
Informed Consent Statement: Not application.

Data Availability Statement:
The data presented in this study are available on request from the corresponding author.

Conflicts of Interest:
The authors declare no conflict of interest.