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Electrochemical Energy Reviews

, Volume 2, Issue 3, pp 373–394 | Cite as

Engineering Two-Dimensional Materials and Their Heterostructures as High-Performance Electrocatalysts

  • Qiangmin Yu
  • Yuting Luo
  • Azhar Mahmood
  • Bilu LiuEmail author
  • Hui-Ming ChengEmail author
Review article
  • 773 Downloads

Abstract

Electrochemical energy conversion between electricity and chemicals through electrocatalysis is a promising strategy for the development of clean and sustainable energy sources. This is because efficient electrocatalysts can greatly reduce energy loss during the conversion process. However, poor catalytic performances and a shortage in catalyst material resources have greatly restricted the widespread applications of electrocatalysts in these energy conversion processes. To address this issue, earth-abundant two-dimensional (2D) materials with large specific surface areas and easily tunable electronic structures have emerged in recent years as promising high-performance electrocatalysts in various reactions, and because of this, this review will comprehensively discuss the engineering of these novel 2D material-based electrocatalysts and their associated heterostructures. In this review, the fundamental principles of electrocatalysis and important electrocatalytic reactions are introduced. Following this, the unique advantages of 2D material-based electrocatalysts are discussed and catalytic performance enhancement strategies are presented, including the tuning of electronic structures through various methods such as heteroatom doping, defect engineering, strain engineering, phase conversion and ion intercalation, as well as the construction of heterostructures based on 2D materials to capitalize on individual advantages. Finally, key challenges and opportunities for the future development of these electrocatalysts in practical energy conversion applications are presented.

Graphical Abstract

Keywords

2D materials Electrocatalysts Heterostructures Hydrogen evolution reaction Oxygen reduction reaction Oxygen evolution reaction 

1 Introduction

The start of the second industrial revolution in the nineteenth century led to the invention and widespread use of the steam engine and as a result produced unprecedented demands for energy. Initially, this demand was met by thermal energy (heat) generated from wood or coal, but these resources suffered from low energy conversion and harvesting efficiencies. Later, fossil fuels were used to produce mechanical energy in the pursuit of higher energy conversion efficiencies. But efficiencies remain unsatisfactory. In addition, the excess use of fossil fuels has led to fossil fuel shortages and serious environmental problems. As a result, the development of sustainable and renewable energy resources is urgently needed [1, 2]. And because traditional energy conversion methods are unsatisfactory due to their low conversion efficiencies, the development of efficient, clean energy storage and conversion technologies is also crucial. Based on this, great efforts have been made in recent years to develop sustainable energy sources such as solar and hydrogen energy. Moreover, numerous efforts have been made in the efficient conversion of these sustainable energy sources to electrical energy [3, 4, 5] via energy conversion devices such as water electrolysis, fuel cells, and metal-air batteries [5, 6, 7]. And because these efficient energy conversion processes require electrocatalytic reactions, electrocatalysis is the key in the successful application of these energy conversion technologies [8]. One obvious advantage of electrocatalysis is that electrocatalysts can lower reaction energy barriers to allow chemical reactions to occur under smaller electric fields (overpotential), leading to lower energy consumption during the conversion process. In addition, the use of electrocatalysts can allow for the easy control of reaction pathways and rates to produce products.

Overall, electrochemical reactions occur at the interface between electrocatalysts and reactants in solution in which the surface of electrocatalysts interacts with dissolved reactants. Here, the performance of electrocatalysts is mainly determined by factors such as chemical composition, crystal structure, microstructure, and macromorphology, and these parameters have a direct influence on catalytic performance, meaning that catalytically active interfaces are vital for high-efficiency electrocatalysis [9]. A key consideration of interfacial catalysis is the adsorption and desorption ability of reaction intermediates by the catalyst in which desirable catalysts must possess suitable adsorption and desorption energy for intermediates to facilitate electrocatalytic reactions. Other considerations include good electron conductivity, rapid mass transfer, high durability, and environmental benignity [10, 11, 12]. Because of this, not only the intrinsic activity of catalysts is important, but the structure of catalysts is also critical to achieve efficient catalytic processes in which a major goal of electrocatalysis research is the design and synthesis of materials with high activity, high selectivity, and good durability. Therefore, investigations into the relationship between catalyst structure and catalytic performance are important because interfacial structures have direct influences on efficiency and selectivity.

Currently, noble metals (e.g., Pt) and noble metal oxides (e.g., RuO2 and IrO2) are being widely used as electrocatalysts due to their high performances in electrochemical reactions; however, limited resources restrict widespread application. To address this, increasing attention has been paid in recent years to the exploration of abundant low-dimensional materials, especially 2D materials, for electrocatalysis due to their tunable electronic structures, large specific surface areas, and scalable production capabilities [13, 14]. All of them are desirable properties for promising large-scale electrocatalyst applications. Therefore, this review will mainly focus on the rational engineering of 2D materials and corresponding heterostructures in the production of highly efficient electrocatalysts. In addition, current enhancement strategies for the catalytic performance of 2D materials, including heteroatom doping, defect engineering, strain engineering, phase conversion, and ion intercalation, are discussed. Furthermore, the fabrication of heterostructures based on 2D materials and their advantages in electrocatalysis are also discussed, and the challenges of future 2D material-based electrocatalyst development are presented.

2 Key Electrocatalysis Processes and the Potential of 2D Materials

Energy-related electrocatalysis processes are required in energy conversion applications such as water electrolysis, fuel cells, and metal-air batteries, and involve electrochemical reactions such as the hydrogen evolution reaction (HER), the oxygen reduction reaction (ORR), and the oxygen evolution reaction (OER). Because of this, these reactions (Fig. 1) are major topics of this review and are explained in detail.
Fig. 1

The electrocatalytic reaction processes of HER, ORR, and OER along with corresponding reaction steps and mechanisms

HER is the cathode reaction in water electrolysis and can be divided into two steps in acidic media [15] in which the first step is the Volmer step involving electrochemical hydrogen adsorption and the second step can be further divided into two types including the Heyrovsky step and the Tafel step [16]. Here, the rate of HER depends on the hydrogen adsorption free energy (∆GH*) [17] in which if hydrogen adsorption on the catalytic surface is weak, hydrogen adsorption becomes the rate-determining step of the overall reaction. Alternatively, if hydrogen adsorption is too strong, the desorption step becomes the rate-determining step of the overall reaction. Based on this, efficient HER catalysts should possess a ∆GH* close to 0 eV, allowing for both the adsorption of reactants and the desorption of products to occur easily [18, 19, 20]. Furthermore, the Volmer step varies depending on the electrolyte used (acidic or alkaline) in which in acidic media, electrocatalysts can directly adsorb H+ from the solution, whereas in alkaline media, electrocatalysts need to dissociate H2O before being able to adsorb H+, which is more difficult to realize than the subsequent H+ reduction in HER for many electrocatalysts. Overall, there are several key parameters that can be used to evaluate the performance of HER electrocatalysts. These parameters include: (i) the electrochemical active surface area (ECSA), which is defined as the number of catalytically active sites on the catalyst; (ii) the onset potential, which is defined as the potential at which cathodic currents are observed; (iii) the overpotential (η), which is the additional potential required to drive a reaction to reach a certain current density (j); (iv) the Tafel slope, which is the slope between η and log |j| and can be used to analyze the rate-determining step; (v) the exchange current density (j0), which is a key descriptor to evaluate the catalytic efficiency; (vi) the turnover frequency (TOF), which is defined as the numbers of reactant molecules transformed per active site per second; (vii) the Faradic efficiency, which describes the efficiency of charge transfer in an electrochemical reaction system; and (viii) stability, which is a key parameter to evaluate long-term catalyst performance [21].

The ORR is also a cathode reaction that is important in fuel cells and metal-air batteries. ORR possesses two types of reaction mechanisms in which one is a dissociative mechanism and the other is an associative mechanism [19, 22]. Here, reaction mechanisms depend on the oxygen dissociation barrier of catalyst surfaces and the binding energy of oxygenated species on catalyst surfaces determines catalytic activity. Based on this, optimal ORR catalysts should possess moderate binding to intermediates (i.e., O* and OOH*) in which weak binding can limit electron or proton transfer to adsorbed oxygen and strong binding can lead to difficulties in H2O desorption, which in turn can block active site for further oxygen adsorption. Here, the underlying mechanism behind the different binding energies of intermediates and catalyst surfaces is related to their electronic structures [23], and catalysts with optimal binding energies can provide enhanced catalytic properties for ORR, similar to HER. In addition, other factors such as mass transfer and gas diffusion at the catalyst interface also influence the catalytic properties for ORR. Based on this, the engineering and optimization of the geometric structure of catalysts are effective strategies to develop desirable ORR electrocatalysts [24]. As for the evaluation of ORR catalysts, the onset potential (Eonset) and the half-wave potential (E1/2, which is the potential corresponding to half of the limited current density) are generally used to provide quantitative evaluations of the ORR activity of electrocatalysts in which more positive Eonset and E1/2 values represent better catalytic performances. Other criteria used in the evaluation of ORR activity in catalysts include the kinetic current density (Jk), which can be obtained from the Levich–Koutecky equation [25], the electron transfer numbers and the amount of intermediate H2O2 produced, all of which can be obtained from rotating disk electrode (RDE) and rotating ring-disk electrode (RRDE) characterizations.

The OER is the anode reaction in water electrolysis and metal-air batteries and is the inverse of the ORR. OER also includes two reaction mechanisms based on the pH of the electrolyte [19, 26]. In acidic media, the first step of OER is the formation of water intermediates in which water molecules are adsorbed on the surface of the catalyst. These water intermediates subsequently release two electrons and two protons to form an O* intermediate. Following this, two different pathways can occur for the transformation of the O* intermediate to O2 in which one involves the direct combination of two O* to produce O2, whereas the other involves the formation of an OOH* intermediate through the combination of O* and H2O, leading to the formation of O2. Alternatively, the first step of OER in the alkaline media is the formation of OH intermediates with the subsequent steps being similar to those in acidic media. And based on the analysis of the OER process, appropriate catalytic interfaces for the association and dissociation of intermediates are prerequisites for optimal OER electrocatalysts. A summary of the key reaction steps in HER, ORR, and OER is listed in Fig. 1.

In the initial phases of electrocatalysis research, noble metals were the most widely studied with Pt being one of the most active electrocatalysts for HER and ORR [27, 28] based on the fact that Pt-based catalysts possess low overpotentials for both HER (\(\leqslant\) 50 mV to achieve a current density of 10 mA cm−2) and ORR (~ 300 mV with limited current density) [29]. However, unlike HER and ORR, OER requires large positive potentials; because metals are susceptible to oxidation at higher potentials, they are unsuitable. Alternatively, metal oxides and metal hydroxides generally possess decent OER performances [30, 31] and the use of noble metals and corresponding oxides for high-performance electrocatalysis is an active research area with significant progress being made in recent years [32, 33]. For example, despite large overpotentials (~ 300 mV to achieve a current density of 10 mA cm−2), iridium oxide (IrO2) and ruthenium oxide (RuO2) have become dominant OER catalysts in recent years [34]. However, noble metals suffer from the disadvantages such as high costs and limited availability, which restrict their large-scale commercialization. Therefore, the development of high-performance catalysts composed of earth-abundant and cheap elements is needed to achieve breakthroughs in the field of electrochemical energy conversion. And in recent years, scientists have investigated electrocatalysts based on noble metals, non-noble metals and even novel metal-free electrocatalysts, including metal oxides (CoxOy, FexOy, MnxOy, NixOy) [24, 26, 35, 36], metal hydroxides (NiFe LDH, FeCo LDH) [37, 38], metal phosphides or nitrides (CoxPy, NixPy, MoxPy, MoxNy) [39, 40, 41, 42], and carbon-based materials (carbon nanotubes, graphene, graphdiyne) [43, 44, 45]. Here, researchers have demonstrated that non-noble metal and metal-free electrocatalysts can provide catalytic activities for different catalytic reactions; however, most possess poorer catalytic performances than noble metal-based catalysts. Therefore, alternative noble metal-free catalysts with high catalytic performances need to be developed for large-scale implementation.

Overall, many materials have been demonstrated to be active for electrocatalysis, and the design of ideal electrocatalysts with high activities and long stability includes many factors. First, ideal electrocatalysts should possess large specific surface areas with abundant exposed pores to maximize active sites. Second, the active sites of ideal electrocatalysts should possess suitable binding strengths to both reactants and products to optimize corresponding electrocatalytic reactions in which binding strengths can be tuned through the modulation of catalyst electronic structures. Third, ideal electrocatalysts should be able to conduct electrons to external circuits and accelerate electrode kinetics. Fourth, ideal electrocatalysts should be porous to promote mass transfer and gas diffusion in electrolytes. Lastly, ideal electrocatalytic materials should be earth-abundant and inexpensive as compared with noble metal catalysts.

Since the successful isolation of single-atom-thick graphene from graphite by Geim et al. [46] in 2004, 2D materials have attracted tremendous attention as electrocatalysts. Aside from graphene, there is also a large family of 2D materials including hexagonal boron nitride (h-BN), transition metal dichalcogenides (TMDCs), black phosphorus (BP), MXenes, layered double hydroxides (LDHs) and many others [47, 48, 49, 50] that have shown outstanding properties [51, 52, 53], ranging from insulators, semiconductors, metals to superconductors [54]. 2D materials possess strong in-plane covalent bonding and weak interactions such as van der Waals forces between layers, allowing these materials to be applicable in electrochemical energy storage and conversion applications. In addition, 2D materials with varying exposed edge sites can be obtained by tuning lateral sizes, allowing for the tuning of catalytic performances [24, 55]. Other advantages of 2D materials include their lateral size and thickness as well as their extremely large specific surface areas. These features impart obvious advantages in electrocatalytic reactions in which 2D materials with large specific surface areas can form more active sites and atomic thicknesses can facilitate electron transfer. Furthermore, the electronic and interfacial structure of 2D materials can be tuned through different physical or chemical methods, which can provide active sites with proper adsorption/desorption abilities for intermediates in electrocatalytic reactions. Moreover, porous structures can be created through the enlargement of interlayer spacing in 2D materials, allowing for the formation of surface pores and the construction of heterostructures, which can accelerate mass transfer and gas diffusion, leading to increased catalytic performances. Lastly, as previously mentioned, there is a large family of 2D materials that contain many earth-abundant elements such as graphene and MoS2, making them promising for large-scale electrocatalysis applications. 2D materials are also ideal model electrocatalysts in the study of electrocatalytic processes because they possess clear and well-defined structures that are different from and simpler than nanoparticle catalysts, allowing for better investigations of electrocatalysis mechanisms. Furthermore, significant time and costs can be saved in computational studies for experimental investigations because 2D materials are easier to simulate as electrocatalysts for electrochemical reactions.

3 Rational Design of 2D Material-Based High-Performance Electrocatalysts

Most 2D materials possess little or no electrocatalytic activity, making them less desirable for catalytic reactions. However, various approaches including heteroatom doping, defects formation and engineering, strain engineering, ion intercalation and interfacial interaction (Fig. 2) have been demonstrated to be able to improve the catalytic performance of 2D materials through different mechanisms.
Fig. 2

Tuning the properties and catalytic activity of 2D materials by different methods, including heteroatom doping, defect engineering, strain, ion intercalation, and the construction of heterostructures based on them

3.1 Individual 2D Materials for Electrocatalysis

3.1.1 Graphene and Their Derivates

Graphene possesses no electrocatalytic activity due to its inert surface. However, catalytically inert electrons can be activated through defects that disturb the stable electronic structure [56] in which defects in electrocatalytic interfaces can alter the electronic structures and interfacial properties and enhance activity for electrocatalysis [57, 58]. 2D materials possess two types of defects, including in-plane defects (vacancies) and edge defects, and in graphene, vacancies can break the electron-hole symmetry, alter the local density of π-electrons and increase surface chemical reactivity. For example, Jia et al. [59] assembled a graphene material possessing different types of defects (defective graphene, DG) through the removal of nitrogen from N-doped graphene (Fig. 3a) to evaluate the role of these defects on the electrocatalysis through measurements of HER, OER, and ORR (Fig. 3d–g). Here, the researchers reported that the ORR activity of the DG was comparable to most previously reported metal-free ORR catalysts with a positive onset potential of 0.91 V and a half-wave potential of 0.76 V and that the OER activity of the DG was high with a potential of 1.57 V at a current density of 10 mA cm−2. Furthermore, the researchers reported that the DG showed significantly improved HER activities in both alkaline and acidic media with an operating potential at a current density of 10 mA cm−2 of − 0.15 V in acidic media. These results were further validated by using density function theory (DFT) calculations, and the defects in the graphene were observed directly by using aberration-corrected high-resolution transmission electron microscopy (HRTEM) and atomic force microscopy (AFM) (Fig. 3b–c), with the various defects on the edge of the graphene being directly observed by using high-angle annular dark-field scanning TEM (HAADF-STEM). And as a result of the satisfactory half-cell performance for ORR and OER, the researchers in this study used the DG material as a cathode catalyst to construct a Zn-air battery and reported a peak power density of ~ 154 mW mg−1 at a current density of 195 mA mg−1, which is comparable to that of Pt/C counterparts. Despite defects being able to greatly improve the electrocatalytic performance of graphene, however, they cannot be generated in a controlled manner. To address this, Tao et al. [60] recently developed a plasma technique to etch the surface of graphene and prepare defect-rich graphene in a controlled manner to be used as an excellent metal-free ORR electrocatalyst in which the defects were controlled by altering the treatment time and power of the plasma. Overall, the use of defective graphene in recent years as electrocatalysts has been widely reported by researchers [61, 62, 63], and new methods to create defects in a controlled manner, and advanced techniques to identify these defects are required to advance future development.
Fig. 3

a Schematic of the structure and formation of DG. b HAADF-STEM image of DG. Hexagons, pentagons, heptagons, and octagons are labeled in orange, green, blue, and red, respectively. c AFM image of DG. dg LSV curves of pristine graphene, NG and DG in different media. d ORR in 0.1 M KOH, e OER in 0.1 M KOH, f HER in 0.5 M H2SO4 and g HER in 0.1 M KOH. Here, G represents graphene, NG represents nitrogen-doped graphene, and DG represents defective graphene. Reprinted by permission from Ref. [59]. Copyright 2016, Wiley-VCH

Analogous to defects, heteroatom doping can also alter the inert electronic structure of graphene and heteroatom-doped graphene has attracted major interest as a promising substitute for noble metals in various electrocatalytic reactions. Dai et al. [64] were the first to report the heteroatom doping of carbon materials for electrocatalytic reactions in 2009, and Qu et al. [65] conducted a ground-breaking study of 2D materials with heteroatom doping through the synthesis of nitrogen-doped graphene (NG) using chemical vapor deposition (CVD) in 2010 in which the resulting NG as a cathode provided significantly enhanced electrocatalytic activities, long-term operational stability, and high tolerances to the crossover effect as compared with commercial Pt/C catalysts for ORR. Here, theoretical calculations indicate that the incorporation of nitrogen with higher electronegativity can generate substantial positive charge densities on adjacent carbon atoms, which can enhance the chemisorption of O2 at the interface with lower ORR overpotentials. Following this study, similar results for ORR were obtained for graphene doped with heteroatoms such as boron (B) [66], sulfur (S) [67], and phosphorus (P) [68]. Here, sulfur- and phosphorus-doped graphene possesses similar effects to nitrogen-doped graphene because sulfur, phosphorus, and nitrogen all possess higher electronegativity than carbon. As for boron, although it possesses lower electronegativity than carbon, a similar principle can be used to explain the increased activity for boron-doped graphene as compared with pure graphene in which the carbon–boron bonds in boron-doped graphene can undergo slight polarizations to form local positive charges on boron sites, allowing boron sites to become the preferred sites for O2 adsorption for subsequent reactions [69]. Furthermore, researchers have also developed dual-doped [70] and tri-doped [71] graphene as electrocatalysts with even better ORR performances due to synergistic effects. For example, Liang et al. [70] prepared N and S dual-doped graphene as an ORR catalyst and reported excellent catalytic activities with a high positive onset potential of −0.06 V and a large kinetic limiting current of 52 mA cm−2 at − 0.8 V (V vs. Ag/AgCl). Here, DFT calculations revealed that the synergistic performance improvements can be attributed to the redistribution of spin and charge densities caused by the dual doping of S and N atoms, which generated large numbers of C active sites. In another study, Zhang et al. [71] prepared a N, P and fluorine (F) tri-doped graphene as a multifunctional electrocatalyst and reported satisfactory electrocatalytic performances for ORR, OER, HER, and in a Zn-air battery.

Many studies have reported that doped graphene can possess multifunctional electrocatalytic activities [43, 67, 71]. However, the nature of the active sites used in the catalytic reactions is unclear. To address this, Lai et al. [72] proposed a method to determine the nature of active sites through the synthesis of different types of N in NG electrocatalysts in which NG samples were synthesized by the annealing of graphene oxide (GO) under ammonia (N-RGO) and by annealing polyaniline/reduced GO (PANi/RGO), polypyrrole/RGO (Ppy/RGO) and H3BO3/N-RGO (BN-RGO) (Fig. 4a). Here, N doping states were changed by modifying annealing temperatures and types of N precursors in which PANi/RGO and Ppy/RGO were found to possess the highest atomic N/C ratios. In addition, N-RGO was found to possess a larger number of graphitic N atoms, and the N atoms in the BN-RGO sample were found to be in the form of pyridinic N with most being covalently bonded to B, which may prevent the transformation of pyridinic N to graphitic N in graphene. The researchers in this study subsequently conducted electrochemical measurements on all samples and revealed that N-RGO demonstrated the largest limited current density (Fig. 4b) and that the ORR onset potential possessed a linear relationship with the number of pyridinic N species in the sample. Furthermore, the researchers reported that PANi/RGO and Ppy/RGO possessed lower activities as compared with the N-RGO-based catalyst, indicating that the total N atom content was not the determining factor in electrocatalytic reactions. And although these results demonstrate the influence of N species on catalytic activity, the nature of the catalytic active sites remains unclear. In order to identify this site, Nakamura et al. [73] synthesized four-model ORR catalysts with well-defined π conjugations based on highly oriented pyrolytic graphite (HOPG), including pyridinic N-dominated HOPG (pyri-HOPG), graphitic N-dominated HOPG (grap-HOPG) and for comparison, edges patterned onto the surface without N (edge-HOPG) and clean-HOPG. Here, the N 1 s XPS spectra for the four samples revealed that the non-doped edge-HOPG and clean-HOPG samples were free of N, whereas the N concentrations of grap-HOPG and pyri-HOPG were 0.73 at% (82% grap-N, 5% pyri-N, 13% other types) and 0.60 at% (95% pyri-N, 5% grap-N), respectively (Fig. 4c), suggesting that pyri-HOPG possessed outstanding catalytic activities toward ORR as compared with the other samples (Fig. 4d). Further characterization in this study revealed that carbon atoms next to pyridinic N can react with OH species with a consequent transformation of pyridinic N to pyridonic N (Fig. 4e), suggesting that the carbon atoms next to pyridinic N rather than pyridinic N atoms themselves actually act as the catalytically active sites.
Fig. 4

Doping of graphene for electrocatalysis. a Schematic of the preparation of N-doped graphene with different N states. b LSV curves of electrodes made from N-RGO 1000 °C, bare GC, PANi/RGO Ppy/RGO, BN-RGO, bare Pt and 20% Pt/C. Reprinted by permission from Ref. [72]. Copyright 2012, Royal Society of Chemistry. c N 1 s XPS spectra of model catalysts. d ORR results for the model catalysts in (c). The nitrogen content of these model catalysts is shown in the inset. e Schematic of the formation of pyridonic N by attaching OH to the carbon atom next to pyridinic N. Reprinted by permission from Ref. [73]. Copyright 2016, American Association for the Advancement of Science

As graphene derivates, 2D graphdiyne and g-C3N4 materials have also shown promising catalytic performances for electrocatalysis [74, 75]. Graphdiyne, possessing sp- and sp2-hybridized carbon atoms, a nano-porous structure [76], and good charge transport properties, has attracted development as high-performance electrocatalysts, and as a result, graphdiyne as metal-free electrocatalysts has shown excellent performances for both HER and ORR [77, 78, 79]. As another graphene derivates, g-C3N4, possessing a similar structure to graphene but with the higher N content, has also shown promising application in high-performance electrocatalysis. However, the conductivity of g-C3N4 is inferior to graphene, which hinders application. Therefore, scientists have made great efforts to improve the conductivity of g-C3N4 through combination with conductive materials such as graphene and carbon nanotubes [80, 81, 82, 83].

3.1.2 Transition Metal Dichalcogenides (TMDCs)

Although defects or dopants in graphene have shown great promise for electrocatalysis, they are generally difficult to control. Unlike graphene, however, other 2D materials such as TMDCs have been shown to be catalytically active toward HER even without modification despite weak activities [3, 31]. And in terms of catalytic properties, TMDCs possess many advantages as compared with graphene. First, TMDCs possess intrinsic activities for electrocatalytic reactions, whereas graphene is inert. Second, TMDCs possess different phases that are semiconducting or metallic and that can display different performances. Third, both transition metal atoms and nonmetal atoms can be substitutionally doped into TMDC lattices to provide more doping options as compared with graphene. And as a result of these advantages, significant efforts have been focused on TMDC catalysts in recent years [84, 85, 86].

Semiconducting TMDCs such as 2H-MoS2 have been shown to be active toward HER even though their bulk counterparts are not very active. Electrochemical hydrogen production by using MoS2 can be traced back to the 1970s [87]. And after several decades of technological developments, MoS2 has become a potential substitute for commercial Pt/C catalysts in HER. The identification of active sites is essential to properly study catalytic activity. Based on this, Jaramillo et al. [88] systematically explored the surface sites of MoS2 nanoparticles both experimentally and theoretically in which MoS2 samples were synthesized by using physical vapor deposition, and the ratio of basal-plane sites to edge sites was controlled through sintering without changing the nature of the edges. Here, electrochemical tests revealed that the rate of the reaction was directly proportional to the number of edge sites for all samples rather than to the particle size of samples. To gain further insights into the catalytic nature of MoS2, the researchers in this study also conducted DFT calculations to identify the activity differences between basal planes and edge sites. Here, the ∆GH* of the edge sites was calculated to be + 0.08 eV, which was closer to 0 eV than that of the basal plan sites. These results also showed that the electrocatalytic activity of hydrogen evolution possessed a linear relationship with the number of edge sites of the MoS2 catalyst. And based on these results, a series of methods was developed to obtain large numbers of edge sites on MoS2 in which the most effective method is to create defects [89, 90, 91]. For example, Xie et al. [92] developed a scalable method to produce large numbers of defects in MoS2 surfaces to expose active edge sites and reported that the resulting MoS2 nanosheets possessed excellent HER activities with a small onset overpotential of 120 mV, a large cathodic current density, and a small Tafel slope of 50 mV dec−1, which is one of the best comprehensive performances reported for individual MoS2 electrocatalysts.

In addition to defect engineering, the heteroatom doping of TMDCs is another effective method to obtain high-performance electrocatalysts because doping can change hydrogen absorption properties. For examples, Deng et al. [93] demonstrated that the doping of single Pt atoms into the inert MoS2 plane (Pt-MoS2) can triggered HER activities in which Pt can not only serves as electrocatalytic active sites but also as an agent to improve MoS2 performance. In this study, the replacement of Mo atoms by atomically dispersed Pt atoms in the MoS2 plane was confirmed by HADDF-STEM (Fig. 5a) and DFT calculations revealed that the doped Pt atoms can change the adsorption behavior of H atoms on neighboring S atoms, consequently improving HER activities. Here, the researchers reported that although few-layer MoS2 (FL-MoS2) showed high activities, it was far inferior to commercial Pt/C catalysts. Alternatively, the obtained Pt-MoS2 demonstrated significantly increased activities compared with FL-MoS2, decreasing the overpotential to ~ 60 mV at a current density of 10 mA cm−2 (Fig. 5b). Inspired by the successful increase in MoS2 activity through Pt single-atom doping, the researchers in this study further investigated the HER activity of MoS2 doped with various single-metal atoms using theoretical calculations and reported two types of metal atom-doped MoS2 in which one type (e.g., Fe, Mn, Cr) tended to possess metal dopants in the middle of a hexagon of S atoms, whereas the other (e.g., Pt, Ag, Ni) possessed dopant atoms shifted to one side and bonded with 4 S atoms, leaving the other 2 S atoms unsaturated (Fig. 5c). These two different doping types inevitably lead to different hydrogen adsorption energies, resulting in different HER performances. And based on this, these results can provide guidance to stimulate the inert surface activity of TMDCs in HER.
Fig. 5

Doping and straining of TMDCs for electrocatalysis. a TEM image of Pt-MoS2. The inset shows the simulated configuration of Pt-MoS2. b LSV curves of Pt-MoS2 compared with different samples. c The volcano-shaped relationship between current (log (i0)) and ΔGH*. Two different scales on the left and right of the plot provide better visibility. The inserted figures show the different configurations of doped MoS2 with the dopant atom coordinated with 4 (left) and 6 (right) S atoms. The adsorption sites for H atoms are marked with red dashed circles. Reprinted by permission from Ref. [93]. Copyright 2015, Royal Society of Chemistry. Atomic structure of monolayer MoS2 on gold ligaments of NPG. d Cross-sectional HAADF-STEM image of monolayer MoS2@NPG. e STEM images of monolayer MoS2@NPG from the flat region of a gold ligament. The inset shows the simulated STEM image based on the standard structural model of 2H MoS2 in (f). g STEM image of monolayer MoS2@NPG taken from the curved region of the NPG substrate. h The different S-Mo-S bonding angles (α) in the curved region shown in (g). The dashed line indicates the S-Mo-S bonding angle (120°) of perfect 2H MoS2. i LSV curves and j corresponding Tafel slopes of MoS2@NPG. Scale bars: 1 nm in (d), (e), and (g). Reprinted by permission from Ref. [95]. Copyright 2014, Wiley-VCH

Enormous efforts have been made to expose more active sites in TMDCs to increase catalytic performance; however, these efforts are usually accompanied by losses of stability and electrical conductivity. In one study, Voiry et al. [94] reported that strain-induced local lattice distortions of WS2 resulted in the phase conversion of WS2 from a 2H to 1T enriched phase, which led to enhanced catalytic activities. The researchers in this study also performed first-principles calculations to reveal the mechanisms responsible for the high activity of 1T WS2 in which calculations suggested that strain can significantly increase the density of states near the Fermi energy and facilitate the binding of hydrogen to the surface of distorted 1T WS2. To further understand the role of strain, Tan et al. [95] prepared monolayer MoS2 on the internal surface of curved 3D nano-porous gold (NPG) in which side-view STEM images clearly indicated significant lattice distortions (Fig. 5d–g) and different S-Mo-S bonding angles (α) (Fig. 5h). Here, the researchers reported that the distorted MoS2 film with the out-of-plane strain demonstrated good electrocatalytic performances toward HER and that the activity of the MoS2 film decreased as sample thicknesses increased from monolayer to three layers (Fig. 5i) with the corresponding Tafel slopes increasing from 46 to 55 mV dec−1 (Fig. 5j). The researchers suggested that this difference in performance can be attributed to the change of S-Mo-S angles (α) in which if α is larger than 140°, the band gap of monolayer 2H MoS2 is close to 0 eV, indicating that local semiconductor-to-metal transition was caused by out-of-plane lattice bending. Furthermore, the calculations conducted in this study showed that the free energy is also related to α and that lattice bending can cause smaller binding free energy, explaining the better performance of curved monolayer MoS2. A similar result was obtained by Putungan et al. [96] who used biaxial tensile strain to study the effects of distortion in 1T phase group-VI TMDCs on the free energy of hydrogen adsorption. Here, the researchers found that the density of states near the Fermi level increases as strain is introduced, which causes a decrease in hydrogen adsorption energy. Furthermore, Li et al. [97] systematically investigated the effects of S-vacancies combined with strain on HER performance and concluded that this combination can lead to even higher HER activities. In addition, the researchers in this study also suggested that strain can effectively stabilize adsorbed hydrogen on the surface of basal planes. Overall, these experiments and theoretical calculations demonstrate that strain engineering can enhance the activity of TMDC catalysts.

As one of the most well-studied TMDCs, semiconducting MoS2 with an inert plane possesses reasonable HER performances and researchers report that further modifications of the MoS2 structure can significantly increase electrocatalytic activities, with Li intercalation being especially successful [98, 99, 100]. For example, Wang et al. [101] developed a novel method to modify the MoS2 phase from a 2H semiconducting phase to a 1T metallic phase through the electrochemical intercalation of Li+ in which the Li content can be controlled by using the voltage of the LixMoS2 versus Li+/Li in the electrochemical process (Fig. 6a). Here, electrochemical intercalation is used because it is more controllable as compared with chemical intercalation. And as a result, the interlayer spacing expanded significantly to 0.72 nm (Fig. 6b) from 0.64 nm of pristine MoS2 after intercalation, with the MoS2 phase gradually changing from semiconducting 2H to metallic 1T as Li content increased (Fig. 6c). And as compared with pristine MoS2, the lithiated 1T-MoS2 nanosheets showed dramatically improved HER performances, with an overpotential of 110 mV versus RHE at a current density of 0.1 mA cm−2 and a Tafel slope of 44 mV dec−1 (Fig. 6d). Furthermore, the researchers in this study conducted electrochemical stability tests and reported that the lithiated sample maintained high catalytic activities with negligible degradation after 1000 cyclic voltammetry (CV) cycles (Fig. 6e). Similar enhancement in the HER activity was also observed in chemically intercalated 1T WS2 nanoflowers as synthesized by Lukowski et al. [102] in which structural characterizations revealed that the intercalated WS2 nanosheets possessed a metallic 1T phase superstructure, resulting in a low overpotential of 142 mV versus RHE at 10 mA cm−2 and a Tafel slope of 70 mV dec−1 for the 1T-WS2 catalyst. Recently, our group [103] also investigated a Co(OH)2-intercalated MoS2 material that achieved high HER performances in alkaline media in which Li+ was first intercalated into MoS2 and subsequently exchanged with Co2+ to form Co2+-intercalated MoS2. Following this, Co2+ was converted to Co(OH)2 through heating to produce Co(OH)2-intercalated MoS2 and the resulting catalyst exhibited a low overpotential of 89 mV at a current density of 10 mA cm−2. Here, these enhanced performances can be attributed to the ability of Co(OH)2 to dissociate water efficiently [104]. Overall, the ion intercalation method can produce TMDCs with better activities than pristine TMDCs, However, this method is difficult to scale up, which limits large-scale application.
Fig. 6

Metallic TMDCs for electrocatalysis. a Schematic of a battery testing system in which the cathode is a MoS2 nanofilm with layers perpendicular to the substrate and the anode is Li foil. b TEM image of MoS2 with Li electrochemical intercalation. Scale bar: 10 nm. c Galvanostatic discharge curve representing the lithiation process. The atomic structure changes from trigonal prismatic to octahedral along with electronic semiconducting to metallic transition. d LSV curves of pristine and lithiated MoS2. e Electrochemical stability test of lithiated MoS2. Scale bar: 2 μm. Reprinted by permission from Ref. [101]. Copyright 2013, National Academy of Sciences, USA. f Computed values of εLUS for MX2 materials. g Schematic of the proposed mechanism for morphology change in which hydrogen evolution at the basal-plane sites of stacked layers causes perforation and exfoliation of MX2. h LSV curves (iR-corrected) of H-TaS2, H-NbS2, H-MoS2, T-MoS2 and T-TaS2 measured in Ar-bubbled 0.5 M H2SO4. H-TaS2 and H-MoS2 were cycled for 5000 cycles, whereas H-NbS2 was cycled for 12000 cycles. i Corresponding Tafel plots for the catalysts in (h). Reprinted by permission from Ref. [106]. Copyright 2017, Nature Publishing Group

Both strain and ion intercalation results show that the activities of metallic TMDCs are higher than those of semiconducting ones. Moreover, metallic TMDCs possess better conductivity than semiconducting TMDCs, allowing for faster electrode kinetics and electron transport, demonstrating their potential as electrocatalysts. An effective method to obtain metallic TMDC-based electrocatalysts is through direct synthesis using simple methods. For example, Yin et al. [105] synthesized partially crystallized 1T-MoSe2 nanosheets using a modified one-pot hydrothermal strategy in which 1T-MoSe2 nanosheets can be obtained as abundant NaBH4 reductants are consumed during the hydrothermal process. Here, the researchers reported that by increasing the reductant, the conversion of MoSe2 nanosheets from the 2H phase to the 1T phase can be enhanced, leading to improved HER activities. And as a result, the optimized MoSe2 possessed an η of 152 mV at a j of −10 mA cm−2. Despite these performances, however, this method cannot obtain fully crystallized metallic nanosheets, leading to low catalyst utilization. To address this, Liu et al. [106] recently conducted a significant study to investigate the active sites of 2D metallic group-5 MX2 (H-TaS2 and H-NbS2) electrocatalysts, which possess high basal-plane activities for HER as demonstrated through theoretical calculations and experiments. In this study, first-principles calculations were used to reveal the underlying electronic factors controlling basal-plane activity in which the researchers reported that the populated state of electrons near the lowest unoccupied state (εLUS) was the key parameter determining the hydrogen adsorption strength of MX2 surfaces and that εLUS values between −  6.4 eV and − 5.5 eV were usual, corresponding to − 0.5 eV H* < Ea < + 0.5 eV H*. Furthermore, the researchers suggested that among viable candidates, group-5 metal disulfides (H-VS2, H-NbS2 and H-TaS2) were the most promising for catalysts due to suitable εLUS (<− 5.8 eV) (Fig. 6f). In experiments, both H-NbS2 and H-TaS2 demonstrated predictably high performances toward HER with overpotentials of 50–60 mV at a current density of 10 mA cm−2 (Fig. 6h) and Tafel slopes close to 30 mV dec−1 (Fig. 6i), surpassing the performance of all other TMDCs. The researchers in this study also found that these materials exhibited unusual self-optimizing properties as they catalyzed hydrogen evolution. Here, the researchers suggested that this unusual self-optimization was caused by beneficial morphological changes that improved charge transfer and the accessibility of active sites in which H-NbS2 and H-TaS2 were both weakly bounded layered materials and hydrogen gas produced at the sites between the layers can cause exfoliation and fracture, resulting in the thinning and exposure of more active sites during HER (Fig. 6g). At the same time, Shi et al. [107] also reported that metallic 2H-TaS2 grown on gold foil was an efficient HER electrocatalyst in which the catalyst displayed thickness-dependent electrocatalytic performances. Here, a ~ 150-nm-thick 2H-TaS2 catalyst provided a Tafel slope of ~ 33 mV dec−1 that was similar to that of Pt (~ 31 mV dec−1), indicating a Volmer–Tafel mechanism for HER. However, although the catalytic activity of metallic TaS2 was superior to those of other 2D materials, its activity in the basal plane needs to be further improved to satisfy practical applications. Furthermore, metallic TMDCs are sensitive to air and water, and therefore, special attention needs to be paid to their stability. And overall, having only been applied in electrocatalysis recently, metallic TMDCs possessing abundant active sites on both edges and basal planes need to be developed further to gain optimized electrocatalytic performances.

3.1.3 Other 2D Materials

Transition metal-based TMDCs possess excellent HER performances but poor OER performances. Alternatively, layered double hydroxides (LDHs) are 2D materials that are composed of positively charged metallic layers and anionic interlayers and are promising candidates for OER because of their natural abundance and lower costs [108]. However, the inferior electrical conductivity and lack of active sites in LDHs make them unsuitable for electrocatalysis, and researchers have devoted much effort in recent years to improve the performance of LDH-based electrocatalysts. For example, Gong et al. [109] reported that the poor electrical conductivity of LDHs can be improved through combination with conductive supports. In their study, the researchers prepared Ni-Fe LDHs electrocatalysts and reported that by supporting them on carbon nanotubes (CNTs), better OER activities can be obtained, highlighting the importance of conductive substrates. In addition, Song et al. [37] reported that the catalytic activity of LDHs was greatly affected by their thickness in which bulk materials usually exhibit poorer activity due to the limited number of active sites. In their study, the researchers developed an efficient approach to improve the OER activity of LDHs by reducing material thickness through the liquid-phase exfoliation of bulk LDHs (Fig. 7a). Here, the interlayer spacing of pristine LDHs was increased through anion exchange to accelerate the exfoliation of the bulk sample to monolayer nanosheets in which AFM revealed the formation of single layers with a thickness of ~ 0.8 nm (Fig. 8b, c), resulting in significantly higher OER activities as compared with bulk counterparts (Fig. 7d), with results being similar for NiFe, NiCo, and CoCo LDHs. Furthermore, Tafel slopes also decreased with reduced LDH thicknesses from bulk to monolayers. Further characterizations also revealed that exfoliation can not only form monolayer LDHs but also reduce LDH lateral sizes in which smaller lateral sizes can result in increased edge sites that can act as active sites for water oxidation. And overall, the researchers in this study concluded that the improved OER performances are a result of the increased number of exposed active sites in monolayer LDHs after exfoliation.
Fig. 7

LDHs for electrocatalysis. a Schematic showing the exfoliation of LDHs. b AFM image of monolayer nanosheets of NiCo LDHs. c Height profiles of four monolayer NiCo LDHs. d Electrochemical behaviors of LDHs and IrO2 nanoparticles. Inset shows the Tafel plots of the different catalysts. Reprinted by permission from Ref. [37]. Copyright 2014, Nature Publishing Group. e Schematic of the water-plasma-enabled exfoliation of CoFe LDH nanosheets. f TEM and g HRTEM images of water-plasma-exfoliated CoFe LDH nanosheets. h LSV curves for OER and i the corresponding Tafel plots of pristine CoFe LDHs and water-plasma-exfoliated CoFe LDH nanosheets. Reprinted by permission from Ref. [110]. Copyright 2017, Wiley-VCH

Fig. 8

0D/2D heterostructures for electrocatalysis. a Schematic showing ALD growth of Pt on NGNs. b HER LSV curves of ALD Pt/NGNs and Pt/C catalysts. Reprinted by permission from Ref. [136]. Copyright 2016, Nature Publishing Group. c Schematic showing the solvothermal synthesis of MoS2/RGO heterostructures in which MoS2 is supported on RGO. d SEM and (inset) TEM images of MoS2/RGO heterostructures. e LSV curves and f corresponding Tafel plots of the different catalysts. g Durability test for the MoS2/RGO catalyst. Reprinted by permission from Ref. [142]. Copyright 2011, American Chemical Society

Although the exfoliation of LDHs can create more active sites to improve electrocatalytic activity, the intrinsic activity of each site remains unchanged and the improvement of individual site activity is of great interest. In one study, Liu et al. [110] reported a water-plasma-enabled exfoliation process that increased the number of active sites and improved intrinsic activity involving the treatment of pristine CoFe LDHs with water plasma to obtain ultrathin CoFe LDH nanosheets (Fig. 7e) in which TEM revealed the formation of a relatively rough surface with small irregular pores (Fig. 7f) and atomic-size vacancies after the plasma exfoliation process (Fig. 7g). And as a result, the ultrathin CoFe LDH nanosheet catalyst with a large number of vacancies exhibited excellent OER performances with a lower overpotential of 290 mV and a smaller Tafel slope of 36 mV dec−1 as compared with pristine CoFe LDHs (331 mV and 52 mV dec−1) at a current density of 10 mA cm−2 (Fig. 7h–i). Here, the researchers suggested that the vacancies in the ultrathin CoFe LDH nanosheets were responsible for the higher electrocatalytic activity as compared with perfect LDH nanosheets with no vacancies. In another study, Yang et al. [111] synthesized ultrathin CoFe LDH nanosheets with large numbers of defects as a bifunctional electrocatalyst for overall water splitting and reported high electrocatalytic activities for both OER and HER in alkaline media, demonstrating that the density of catalytic active sites in LDHs can be increased through defect engineering. A significant problem with LDHs is the limited number of active sites on their edges. In addition, the electrocatalytic mechanisms of LDHs remain unclear despite extensive efforts. And because of the limited number of active sites and the poor intrinsic activity of LDH-based electrocatalysts, widespread application is hindered in which novel and effective strategies such as cation doping or layer spacing modification need to be developed to resolve these issues.

Another interesting family of 2D materials are MXenes, which possess the general formula of Mn+1AXn in which M is an early transition metal (e.g., Mo and Ti), A is C and/or N, and Xn is surface functional groups [112, 113, 114]. MXenes possess a wide range of components and structures, and some are competitive with other 2D materials. MXenes are also promising as electrocatalysts due to good hydrophilic surfaces, easily modified structures, excellent electrical conductivities, and superb chemical stability [115, 116]. And as a result, Vojvodic et al. [114] predicted and validated that Mo2CTx catalysts are active toward HER through experimental results and found that unlike MoS2 in which only edge sites are active, the basal planes of Mo2CTx are also active catalytic sites for HER. In general, the HER performance of MXenes largely depends on oxygen terminations on the surface due to their strong interaction with H intermediates [117], and Gao et al. [118] demonstrated that as compared with MXenes without oxygen terminations, those with oxygen terminations possess lower hydrogen absorption free energy, resulting in a high exchange current density for HER. In addition, MXenes have also been found to be active for ORR and OER after suitable modifications [119, 120], allowing these newly developed 2D materials to not only act as catalysts and co-catalysts, but also as supporting substrates in electrocatalysis [115]. Overall, the multifunctionality of MXenes makes them promising candidates for catalytic applications.

BP is another representative 2D material that has attracted increasing attention because of its unique structures and properties [121, 122]. BP nanosheets possess large surface areas, lone-pairs of electrons on the surface, and anisotropic electrical and optical properties, making them promising electrocatalysts for water electrolysis [123, 124]. The first study of BP electrocatalysts was reported by Jiang et al. [125] in which synthesis was carried out by using a thermal-vaporization transformation method, resulting in an OER performance with an overpotential of 0.37 V to achieve a current density of 10 mA cm−2, comparable to commercial RuO2 electrocatalysts. However, similar to LDHs, the OER performance of bulk BP is also limited by insufficient active sites and the most effective method to improve the performance is the exfoliation of bulk BP to few-layer nanosheets. For example, Ren et al. [126] developed a simple liquid exfoliation method to obtain few-layer BP nanosheets and reported OER performances that were significantly better than those of bulk BP. In addition, because BP is a new nonmetal layer material, methods used to improve the catalytic performance of graphene and TMDCs may also be applicable. Another issue with BP is that it is unstable in water and its layers gradually cleave and generate defects on the edges and surfaces, which may cause issues for electrocatalytic applications in aqueous media. To address this, Wang et al. [127] developed an effective method to protect BP through the synthesis of Co2P on the defects/edges of BP nanosheets. Here, the researchers reported that Co2P on the edges not only occupied defect sites to improve stability, but also increased electrocatalytic performances. Overall, the use of BP in electrocatalysis has only been recently studied, and it is expected that the research on BP-based high-performance electrocatalysts will continue to expand.

2D metal nanosheets (e.g., Ru, Ir, or Pt nanosheets) have also been widely studied in electrocatalysis due to their high intrinsic activities, high specific surface areas, good charge transfer properties, and abundant active sites, making them promising as high-performance electrocatalysts [128, 129, 130]. In addition, 2D metal alloy nanosheets are potential substitutes for precious metal-based electrocatalysts because they can reduce the amount of precious metals used [131, 132]. Researchers report that the maximization of atom exposure is necessary to achieve high catalytic activity in 2D metal nanosheets. Based on this, Kong et al. [133] synthesized free-standing 2D Ru nanosheets with large portions of atom exposure and reported that the resulting 2D Ru nanosheets demonstrated improved HER activities with an overpotential of 20 mV at 10 mA mg−1, which is lower than that of commercial Ru powder (30 mV). Furthermore, Ir-based electrocatalysts have also been widely applied for OER. For example, Pi et al. [134] investigated 2D Ir nanosheets with large surface areas and accessible active sites and reported greatly improved catalytic activities toward OER in which onset potentials of 1.45 V and 1.43 V versus RHE in acidic and basic media were obtained, respectively. Moreover, catalytic properties of 2D metal nanosheets can be greatly enhanced through the introduction of transition metals to optimize electronic structures and adsorptive behaviors. And overall, these results highlight that the rational construction of 2D structures can enhance the electrocatalytic performance of 2D metal-based catalysts.

3.2 2D Material-Based Heterostructures for Electrocatalysis

Interfacial structures such as heterostructures are key in determining the catalytic performance of 2D materials and can not only overcome the intrinsic shortcomings of each material, but also produce novel properties due to interfacial effects. Based on this, the design and fabrication of heterostructures composed of 0D, 1D, and 2D materials is an effective method to achieve high electrocatalytic performances. In recent years, there has been growing interest in the synthesis of 2D material-based heterostructures to produce high-performance electrocatalysts. The following sections of this review will discuss the fabrication and performance of heterostructures based on 2D materials, including 0D/2D, 1D/2D, and 2D/2D heterostructures.

3.2.1 0D/2D Heterostructures

0D materials are materials possessing sizes in all three dimensions of less than 100 nm and include single atoms, clusters, quantum dots, and nanoparticles. These materials have been widely used as catalysts due to the exposure of abundant active sites with high catalytic activities. However, 0D materials possess low electrical conductivities, making them unsuitable for electrocatalysis if used alone. To resolve this, an effective method is to disperse 0D materials on supports with large surface areas and good conductivity. For example, based on the fact that single-metal atoms can be prepared on high surface area 2D materials to make 0D/2D heterostructures for electrocatalysis, Fei et al. [135] prepared an HER electrocatalyst based on small numbers of individual cobalt atoms dispersed on NG (Co-NG) in which the resulting Co-NG demonstrated good electrocatalytic performances for hydrogen production with a low overpotential of ~ 170 mV at a current density of 10 mA cm−2. In another example, Cheng et al. [136] developed a 0D/2D heterostructure composed of individual Pt atoms and clusters on an N-doped graphene nanosheets (Pt/NGNs) in which the size and the dispersion of the Pt atom clusters were accurately controlled through atom layer deposition (ALD) (Fig. 8a). Here, the researchers conducted both experimental and theoretical studies to reveal that Pt atoms preferred to adsorb onto nitrogen sites in NG and possessed strong interactions with NG, thus promoting electron transfer between them. And as a result, Pt/NGNs in this study provided exceptionally high catalytic activities and good stability for HER as compared with commercial Pt/C catalysts (Fig. 8b) as well as the Co-NG electrocatalysts. Other 2D materials such as TMDCs have also been used as supports to improve the catalytic performance of 0D/2D heterostructures. For example, Cheng et al. [137] used Rh nanoparticles and MoS2 nanosheets, as strong H-adsorbing and quick H2-desorbing components, respectively, in which the resulting Rh/MoS2 heterostructures demonstrated a low overpotential of 47 mV at a current density of 10 mA cm−2, a small Tafel slope of 24 mV dec−1, and decent stability. Here, the excellent performances of the catalysts were attributed to the Rh atoms and their fast capture of hydronium ions as a result of their strong H-adsorbing ability in which the adsorbed H atoms can migrate to the surface of MoS2 with strong H2-desorbing ability, demonstrating the mechanism in which 0D Rh nanoparticles and MoS2 nanosheets together can improve the electrocatalytic activity of heterostructured catalysts. Despite this, the large-scale synthesis of single atom or nanoparticle catalysts dispersed on 2D materials is difficult.

Like metal atom catalysts, 0D compounds can also serve as excellent active sites for electrocatalytic reactions [138, 139, 140, 141]. For example, Li et al. [142] in situ grew MoS2 nanoparticles onto RGO using a one-step solvothermal method (Fig. 8c–d) and reported that because 0D MoS2 nanoparticles possess more abundant S edge sites than 2D MoS2 nanosheets, their combination with RGO can significantly promote catalytic activities, leading to a small onset potential of ~ 0.1 V (Fig. 8e) and a low Tafel slope of 41 mV dec−1 (Fig. 8f). In addition, the researchers cycled the resulting MoS2/RGO catalyst for 1000 cycles and reported negligible cathodic current losses from the initial value (Fig. 8g), demonstrating good durability. Aside from small onset potentials and overpotentials, large current density is another important parameter for high-performance electrocatalysts that is often ignored. Based on this, our group recently designed and constructed a 0D/2D heterostructure electrocatalyst based on Mo2C nanoparticles and MoS2 nanosheets (MoS2/Mo2C) through the in situ carbonization of MoS2 [143]. Here, the resulting MoS2/Mo2C heterostructure was found to possess highly exposed active sites and rough surfaces both at the micro- and nanoscale and demonstrated a low overpotential of 227 mV in acidic media and 220 mV in alkaline media at a large current density of 1000 mA cm−2. In addition, the MoS2/Mo2C catalyst also provided good durability during a 24-h test in both media. Here, the super performance of this MoS2/Mo2C heterostructure was attributed to the enhanced interfacial mass transfer and the surface oxygen formed on Mo2C during HER. And based on these results, further studies into practical industrial use should be conducted. Overall, 0D/2D heterostructures are promising for electrocatalysis; however, poor long-term durability prevents practical application and further improvements are necessary.

3.2.2 1D/2D Heterostructures

1D materials are materials that possess sizes smaller than 100 nm in two out of three dimensions and include nanotubes, nanofibers, nanowires, etc. Different from 0D materials, 1D materials usually possess good conductivities and can act not only as catalytic sites, but also as conductive substrates. In addition, the construction of 1D/2D heterostructures can create optimally sized pores for mass transfer or gas diffusion, and in order to prepare high-performance electrocatalysts, a wide range of 1D/2D heterostructures have been assembled to optimize their microstructures and properties [144, 145]. For example, Li et al. [146] synthesized an ORR catalyst based on CNT/graphene (CNT/G) heterostructures through the oxidation of few-walled CNTs. Here, the outer walls of the CNTs were exfoliated under oxidation to form a nano-sized graphene and the resulting graphene with large numbers of defects was found to be able to facilitate the formation of ORR catalytic sites after annealing in ammonia. In addition, the inner walls of the CNTs remained intact and acted as conductors for charge transfer. And as a result, the CNT/G catalyst provided pronounced ORR catalytic activities with an onset overpotential of ~ 0.89 V and a half-wave potential of ~ 0.76 V. Similarly, Kim et al. [147] developed a 1D/2D heterostructure composed of MoS2 directly grown onto CNTs through the low-temperature decomposition of amorphous MoSx (Fig. 9a) in which HRTEM revealed that the aligned CNT forest retained its structure without collapse after MoS2 deposition (Fig. 9b) with MoS2 catalysts growing along CNT strands (Fig. 9c). As a result, this forest hybrid provided a low overpotential of ~ 110 mV at 10 mA cm−2 and a small Tafel slope of 40 mV dec−1 (Fig. 9d–f). The researchers in this study further investigated the stability of this forest hybrid using continuous CV and reported negligible reductions in cathodic current after 1000 cycles and attributed this to the strong interactions between the active materials and the support. Furthermore, 1D/2D heterostructures with two active materials rather than one are also attractive. Based on this, Chen et al. [148] synthesized a metal-free NG with N-doped CNT (NG-NCNT) heterostructured catalyst that possessed a near-four-electron pathway for ORR and suggested that both of the components in this catalyst can provide active sites to increase the electrochemical activities and the use of CNTs to separate graphene layers can produce gaps or pores to enhance gas diffusion, thus demonstrating that 1D/2D heterostructures can improve catalytic performances through synergistic effects. Despite this, however, these 1D/2D heterostructured catalysts cannot be directly used as self-supporting electrodes.
Fig. 9

1D/2D heterostructures for electrocatalysis. a Schematic showing the synthesis of the 3D MoSx/NCNT forest-based hybrid catalyst. b SEM image and c TEM image of the MoSx/NCNT forest-based hybrid catalyst and the corresponding Fourier transform (FFT) pattern (inset). d HER schematic of the MoSx/NCNT forest hybrid catalyst. e LSV curves and f Tafel plots for different catalysts. g Stability of the MoSx/NCNT forest hybrid catalyst. Reprinted by permission from Ref. [147]. Copyright 2014, American Chemical Society. h Schematic of a hydrogel film electrode based on NG-CNT. i SEM image of NG-CNT. j Contact angles of NG-CNT and dry NG-CNT. k LSV curves of G-CNT, NG-CNT and dry NG-CNT. l LSV plots collected at different scan rates with the inset showing the corresponding data re-plotted as current density versus scan rate. m Chronoamperometric response. The inset in (m) shows the LSV plots for the 1st and 800th cycles. Reprinted by permission from Ref. [149]. Copyright 2014, Wiley-VCH

Different from substrate-supported electrodes, self-supporting electrodes are more suitable for practical applications. And to optimize the electrocatalytic interfacial structure of self-supporting electrodes, Chen et al. [149] fabricated a graphene-CNT hydrogel film electrocatalyst doped with both N and O (NG-CNT) through the layer-by-layer assembly of graphene and CNTs that can be used as a self-supporting electrode for electrocatalysis (Fig. 9h). Here, graphene and CNTs were assembled in a relatively ordered fashion in the hydrogel film due to their strong interactions (Fig. 9i), which the researchers suggested may facilitate charge transport and improve durability during catalytic processes. In addition, the resulting NG-CNT was found to be highly hydrophilic with a small contact angle of ~ 1.6º as compared with 74.2º for dry NG-CNT (Fig. 9j), indicating that the reactants in the electrolyte have easy access to the surface of the film. And as a result, the NG-CNT film directly used as a working electrode for OER provided high catalytic activities with a small onset potential of 315 mV (Fig. 9k), which was less than that of other samples such as dry NG-CNT (410 mV) and G-CNT (322 mV). Furthermore, this NG-CNT hydrogel film with its unique structural features also provided surprisingly high performances that were even better than noble metal oxides (IrO2) and some transition-metal complex catalysts [150, 151, 152, 153]. The researchers in this study also reported that NG-CNT provided similar catalytic currents as scan rates increased from 10 to 100 mV s−1, suggesting highly efficient transports and favorable catalytic kinetics within the electrodes (Fig. 9l). More importantly, NG-CNT also demonstrated excellent durability and stability with little performance loss (Fig. 9m). Overall, self-supporting electrodes based on 1D/2D heterostructures have been demonstrated to possess decent performances and can be directly used in energy conversion devices in which performance improvements will come from better coordination between 1D and 2D materials in terms of nanostructures, chemical components, and the interactions between them.

3.2.3 2D/2D Heterostructures

Individual 2D materials can show decent catalytic performances due to their unique properties; however, these catalytic activities cannot compete with noble metal-based catalysts because of the severe restacking issues. Here, the emergence of van der Waals heterostructures may provide new methods to achieve the full potential of 2D materials in which 2D/2D heterostructures can be constructed by using two different 2D materials to compensate for individual weaknesses and decrease interfacial contact resistances, leading to improved catalytic performances [154, 155, 156, 157, 158]. For example, Yang et al. [159] synthesized a 2D WS2 and 2D RGO heterostructure using a hydrothermal reaction and reported good performances for HER, which the researchers attributed to improved charge transfer kinetics due to the intimate contact between the two components despite being synthesized in solution with little control over their porosity and structure. Inspired by these results, Tang et al. [160] recently used mesoporous magnesia as a template to construct a van der Waals heterostructure composed of graphene- and nitrogen-doped MoS2 in which a porous graphene skeleton was first synthesized by using CVD and followed by the introduction of Mo/S/N sources to grow nitrogen-doped MoS2 nanosheets onto the graphene skeleton (G@N-MoS2, Fig. 10a, b). Here, the researchers reported that the design and synthesis process of the material not only allowed for the effective regulation of the physical and electronic structures of each component, but also allowed the hybrid material to possess strong interfacial interactions. Furthermore, HRTEM clearly showed the presence of N-MoS2 with an interlayer spacing of 0.62 nm (Fig. 10c) and micrographs revealed that the N-MoS2 nanosheets were spread over graphene to form a face-to-face van der Waals heterostructures (Fig. 10d) in which due to the special structural and electronic properties, resulting in efficient multifunctional electrocatalytic performances. The researchers in this study also investigated HER performances and reported that N-MoS2 possessed higher activities than pure MoS2 in which the G@N-MoS2 catalyst provided optimal HER activities with a low overpotential of 243 mV at a current density of 10 mA cm−2 in acidic media (Fig. 10e) and an onset potential of 100 mV greater than corresponding counterparts in alkaline media (Fig. 10f). Furthermore, the G@N-MoS2 catalyst exhibited excellent ORR (Fig. 10g) and OER activities (Fig. 10h) in alkaline media despite few studies referring to these applications. The researchers in this study also reported that the limited current density of the G@N-MoS2 catalysts was close to that of Pt/C for ORR and that the half-wave potential was much smaller than that of other catalysts in which the overpotential of the G@N-MoS2 catalyst at a current density of 10 mA cm−2 was 20 mV lower than that of Ir/C catalysts. Here, the improved electrocatalytic activities were attributed to several factors, including the fact that nitrogen doping can effectively regulate the electronic structures of MoS2 to provide higher spin densities [161] and lower band gaps [162], which can strengthen interfacial charge transfer. Another factor is that the interfacial interaction between graphene and MoS2 can optimize adsorption energy and the last factor is that the resulting 3D mesoporous structures can enhance active site exposure and proton transport. Despite the decent trifunctional performances of this catalyst, however, underlying mechanisms remain unclear and further theoretical and experimental studies are required.
Fig. 10

2D/2D heterostructures for electrocatalysis. a Schematic of the synthesis of 3D mesoporous G@N-MoS2 heterostructures. b Schematic of G@N-MoS2 with a van der Waals heterostructure with nitrogen doping and topological curvature. c HRTEM image of G@N-MoS2. d Micrograph confirming the van der Waals heterostructure of graphene and N-MoS2. eh Multifunctional electrocatalytic activities of 3D mesoporous G@N-MoS2 heterostructures. HER polarization curves of different samples obtained in e H2SO4 and f KOH solutions. g ORR and h OER polarization curves of different samples obtained in a KOH solution. Reprinted by permission from Ref. [160]. Copyright 2018, Wiley-VCH

Similar to 1D/2D heterostructures, 2D/2D heterostructures can also serve as self-supporting electrodes for direct energy conversion devices. For example, Duan et al. [163] constructed a flexible film by integrating porous C3N4 (PCN) nanosheets with nitrogen-doped graphene (PCN@-N-graphene) using a simple vacuum filtration method in which the large numbers of in-plane and out-of-plane pores in the PCN nanosheets can generate highly exposed active sites. Here, the flexible film with a hierarchical porous structure allowed for enhanced mass transport during catalytic processes and the layer-on-layer structure of C3N4 and graphene possessed strong interactions to enhance charge transfer. And as a result, the self-supporting PCN@-N-graphene electrode produced superior HER performances with a small onset potential (− 0.008 V) that was close to that of commercial Pt, a high exchange current density of 0.43 mA cm−2 and excellent durability with negligible activity losses after 5000 cycles, allowing this 2D/2D heterostructure with good conductivity, flexibility, and catalytic performance to be promising for practical electrocatalysis applications. Beyond 2D/2D heterostructures, 2D materials can also possess electronic coupling with substrates in a face-to-face fashion. For example, Voiry et al. [164] reported that the electronic coupling between MoS2 and a gold substrate can greatly reduce the contact resistance of systems and improve electron injection from the substrate to the catalyst active sites. Here, the basal plane of 2H MoS2 is generally less active than 1T MoS2 for HER due to its worse conductivities and poorer charge transfer kinetics. Therefore, the facilitation of charge transfer is an effective method to increase the activity of basal planes in 2H MoS2 [165]. And because gold substrates possess excess d electrons, they can improve the charge transfer of 2H MoS2 if the two are coupled together. And as a result, the electrons injected from the gold substrate to the basal plane of 2H MoS2 can not only accelerate charge transfer but also enhance the adsorption of hydrogen reactants onto the basal planes of 2H MoS2, resulting in improved electrocatalytic performances of 2H MoS2. Overall, this study provided new insights into the role of contact resistance and charge transport on the catalytic performance of 2D materials, and the research discussed in this section indicated that the catalytic performance of 2D materials can be substantially improved through the construction of 2D/2D heterostructures, laying the foundation for 2D materials development in electrocatalytic applications.

4 Conclusions and Outlook

Considerable efforts have been made in recent years to improve the catalytic performance of 2D materials in different electrochemical reactions. And as a result, many breakthroughs have been achieved that clearly demonstrate the advantages of 2D materials in electrocatalysis in which the interfacial structure of 2D materials clearly plays a decisive role in their electrocatalytic performance. However, although 2D materials possess a bright future in electrocatalysis, they face many challenges in which the vast majority of studies report mixed results. These challenges include the unclear origin of the electrocatalytic activity of 2D materials, and the inability to directly observe the electrocatalytic process, which prevents the observation of the reaction stages involved in the mechanisms, and the complexities, inefficiencies and high costs associated with the synthesis of most 2D materials, preventing commercialization. To overcome these challenges, attention needs to be paid to the following research topics.
  1. 1.

    The exploration of novel 2D materials with intrinsically high catalytic activities. Here, the control and engineering of both the chemical and structural composition of these 2D materials need to be considered to achieve this goal, and these explorations will not only assist in the understanding of the origins of active sites, but also provide insights into the effects of doping, defects and strain on catalytic properties. In addition, model electrocatalysts based on 2D materials need to be built to enable simple and more reliable theoretical calculations.

     
  2. 2.

    The elucidation of electrocatalytic mechanisms of 2D materials with the help of advanced in situ characterization techniques. Electrochemical reactions involve multiple electron transfer processes in which each electron transfer is accompanied by the formation of different intermediates. The identification of these intermediates is key to understanding the catalytic mechanisms. Here, in situ characterization techniques such as in situ X-ray absorption fine structure spectroscopy are helpful in analyzing the structural and valence state of intermediates.

     
  3. 3.

    The high-efficiency and energy-saving synthesis of 2D material-based electrocatalysts in large quantity is a prerequisite for practical applications. Currently, most studies only focus on enhancements in catalytic performance and often ignore the costs of individual components and the complexity of the synthesis process. Therefore, the development of efficient strategies for the large-scale production of high-quality 2D materials is urgently needed.

     
  4. 4.

    The durability and the stability of 2D material-based electrocatalysts need to be taken into consideration because they are important parameters in the evaluation of electrocatalysts. The durability of an electrocatalyst mainly depends on its chemical stability in solution, its aggregation between layers and its connection with supporting electrodes in which the structure and components of electrocatalysts must remain stable to maintain activity during long catalytic processes.

     
  5. 5.

    The electrocatalytic activity of 2D materials based solely on laboratory data is often inaccurate, and it is difficult to fairly compare the catalytic performance of 2D materials with other nanomaterials for any given reaction. Therefore, a standardized evaluation system such as large current density and stability for the analysis of electrocatalytic performance needs to be established to meet practical requirements.

     

By following these suggestions, the study of 2D materials that started just ten years ago can potentially lead to important practical applications.

Notes

Acknowledgements

We acknowledge the financial support from the National Natural Science Foundation of China (Nos. 51521091 and 51722206), the Youth 1000-Talent Program of China, the Shenzhen Basic Research Project (No. JCYJ20170307140956657), the China Postdoctoral Science Foundation (No. 2018M641346), the Economic, Trade and Information Commission of Shenzhen Municipality for the “2017 Graphene Manufacturing Innovation Center Project” (No. 201901171523), and the Development and Reform Commission of Shenzhen Municipality for the development of “Low-Dimensional Materials and Devices” disciplines.

References

  1. 1.
    Singh, S., Jain, S., Venkateswaran, P.S., et al.: Hydrogen: a sustainable fuel for future of the transport sector. Renew. Sust. Energy Rev. 51, 623–633 (2015)CrossRefGoogle Scholar
  2. 2.
    Chu, S., Majumdar, A.: Opportunities and challenges for a sustainable energy future. Nature 488, 294–303 (2012)CrossRefPubMedGoogle Scholar
  3. 3.
    Lu, Q.P., Yu, Y.F., Ma, Q.L., et al.: 2D transition-metal-dichalcogenide nanosheet-based composites for photocatalytic and electrocatalytic hydrogen evolution reactions. Adv. Mater. 28, 1917–1933 (2016)CrossRefPubMedGoogle Scholar
  4. 4.
    Dresselhaus, M.S., Thomas, I.L.: Alternative energy technologies. Nature 414, 332–337 (2001)CrossRefPubMedGoogle Scholar
  5. 5.
    Khan, M.A., Zhao, H., Zou, W., et al.: Recent progresses in electrocatalysts for water electrolysis. Electrochem. Energy Rev. 1, 483–530 (2018)CrossRefGoogle Scholar
  6. 6.
    Wang, Y.J., Fang, B., Zhang, D., et al.: A review of carbon-composited materials as air-electrode bifunctional electrocatalysts for metal–air batteries. Electrochem. Energy Rev. 1, 1–34 (2018)CrossRefGoogle Scholar
  7. 7.
    Steele, B.C.H., Heinzel, A.: Materials for fuel-cell technologies. Nature 414, 345–352 (2001)CrossRefPubMedGoogle Scholar
  8. 8.
    Electrocatalysis for the generation and consumption of fuels. Nat. Rev. Chem. 2, 0125 (2018).  https://doi.org/10.1038/s41570-018-0125
  9. 9.
    Stamenkovic, V.R., Strmcnik, D., Lopes, P.P., et al.: Energy and fuels from electrochemical interfaces. Nat. Mater. 16, 57–69 (2017)CrossRefGoogle Scholar
  10. 10.
    Birss, V.I.: Oxygen evolution at platinum electrodes in alkaline solutions. J. Electrochem. Soc. 134, 113–117 (1987)CrossRefGoogle Scholar
  11. 11.
    Anson, A.C.: Double-layer and electrode kinetics (Delahay, Paul). J. Chem. Educ. 43, 54–55 (1966)CrossRefGoogle Scholar
  12. 12.
    Schultze, J.W., Vetter, K.J.: The influence of the tunnel probability on the anodic oxygen evolution and other redox reactions at oxide covered platinum electrodes. Electrochim. Acta 18, 889–896 (1974)CrossRefGoogle Scholar
  13. 13.
    Cai, Z.Y., Liu, B.L., Zou, X.L., et al.: Chemical vapor deposition growth and applications of two-dimensional materials and their heterostructures. Chem. Rev. 118, 6091–6133 (2018)CrossRefGoogle Scholar
  14. 14.
    Cai, X., Luo, Y., Liu, B., et al.: Preparation of 2D material dispersions and their applications. Chem. Soc. Rev. 47, 6224–6266 (2018)CrossRefPubMedGoogle Scholar
  15. 15.
    Benck, J.D., Hellstern, T.R., Kibsgaard, J., et al.: Catalyzing the hydrogen evolution reaction (HER) with molybdenum sulfide nanomaterials. ACS Catal. 4, 3957–3971 (2014)CrossRefGoogle Scholar
  16. 16.
    Laursen, A.B., Kegnaes, S., Dahl, S., et al.: Molybdenum sulfides-efficient and viable materials for electro- and photoelectrocatalytic hydrogen evolution. Energy Environ. Sci. 5, 5577–5591 (2012)CrossRefGoogle Scholar
  17. 17.
    Norskov, J.K., Bligaard, T., Logadottir, A., et al.: Trends in the exchange current for hydrogen evolution. J. Electrochem. Soc. 152, J23–J26 (2005)CrossRefGoogle Scholar
  18. 18.
    Zheng, Y., Jiao, Y., Jaroniec, M., et al.: Advancing the electrochemistry of the hydrogen-evolution reaction through combining experiment and theory. Angew. Chem. Int. Ed. 5, 52–65 (2015)Google Scholar
  19. 19.
    Seh, Z.W., Kibsgaard, J., Dickens, C.F., et al.: Combining theory and experiment in electrocatalysis: insights into materials design. Science 355, eaad4998 (2017)CrossRefPubMedGoogle Scholar
  20. 20.
    Parsons, R.: The rate of electrolytic hydrogen evolution and the heat of adsorption of hydrogen. Trans. Faraday Soc. 54, 1053–1063 (1958)CrossRefGoogle Scholar
  21. 21.
    Wang, J., Xu, F., Jin, H.Y., et al.: Non-noble metal-based carbon composites in hydrogen evolution reaction: fundamentals to applications. Adv. Mater. 29, 1605838 (2017)CrossRefGoogle Scholar
  22. 22.
    Norskov, J.K., Rossmeisl, J., Logadottir, A., et al.: Origin of the overpotential for oxygen reduction at a fuel-cell cathode. J. Phys. Chem. B 108, 17886–17892 (2004)CrossRefGoogle Scholar
  23. 23.
    Zinola, C.F., Arvia, A.J., Estiu, G.L., et al.: A quantum-chemical approach to the influence of platinum surface-structure on the oxygen electroreduction reaction. J. Phys. Chem. 98, 7566–7576 (1994)CrossRefGoogle Scholar
  24. 24.
    Zhou, X.J., Qiao, J.L., Yang, L., et al.: A review of graphene-based nanostructural materials for both catalyst supports and metal-free catalysts in PEM fuel cell oxygen reduction reactions. Adv. Energy Mater. 4, 1301523 (2014)CrossRefGoogle Scholar
  25. 25.
    Ge, X.M., Sumboja, A., Wuu, D., et al.: Oxygen reduction in alkaline media: from mechanisms to recent advances of catalysts. ACS Catal. 5, 4643–4667 (2015)CrossRefGoogle Scholar
  26. 26.
    Man, I.C., Su, H.Y., Calle-Vallejo, F., et al.: Universality in oxygen evolution electrocatalysis on oxide surfaces. ChemCatChem 3, 1159–1165 (2011)CrossRefGoogle Scholar
  27. 27.
    Yu, W.T., Porosoff, M.D., Chen, J.G.G.: Review of Pt-based bimetallic catalysis: from model surfaces to supported catalysts. Chem. Rev. 112, 5780–5817 (2012)CrossRefPubMedGoogle Scholar
  28. 28.
    Debe, M.K.: Electrocatalyst approaches and challenges for automotive fuel cells. Nature 486, 43–51 (2012)CrossRefPubMedGoogle Scholar
  29. 29.
    Nie, Y., Li, L., Wei, Z.: Recent advancements in Pt and Pt-free catalysts for oxygen reduction reaction. Chem. Soc. Rev. 44, 2168–2201 (2015)CrossRefPubMedGoogle Scholar
  30. 30.
    Suen, N.T., Hung, S.F., Quan, Q., et al.: Electrocatalysis for the oxygen evolution reaction: recent development and future perspectives. Chem. Soc. Rev. 46, 337–365 (2017)CrossRefPubMedGoogle Scholar
  31. 31.
    Gong, M., Dai, H.J.: A mini review of NiFe-based materials as highly active oxygen evolution reaction electrocatalysts. Nano Res. 8, 23–39 (2015)CrossRefGoogle Scholar
  32. 32.
    Han, L., Dong, S.J., Wang, E.K.: Transition-metal (Co, Ni, and Fe)-based electrocatalysts for the water oxidation reaction. Adv. Mater. 28, 9266–9291 (2016)CrossRefPubMedGoogle Scholar
  33. 33.
    Suntivich, J., May, K.J., Gasteiger, H.A., et al.: A perovskite oxide optimized for oxygen evolution catalysis from molecular orbital principles. Science 334, 1383–1385 (2011)CrossRefPubMedGoogle Scholar
  34. 34.
    Lee, Y., Suntivich, J., May, K.J., et al.: Synthesis and activities of rutile IrO2 and RuO2 nanoparticles for oxygen evolution in acid and alkaline solutions. J. Phys. Chem. Lett. 3, 399–404 (2012)CrossRefPubMedGoogle Scholar
  35. 35.
    Smith, R.D.L., Prevot, M.S., Fagan, R.D., et al.: Water oxidation catalysis: electrocatalytic response to metal stoichiometry in amorphous metal oxide films containing iron, cobalt, and nickel. J. Am. Chem. Soc. 135, 11580–11586 (2013)CrossRefPubMedGoogle Scholar
  36. 36.
    Zhang, Z.H., Liu, J., Gu, J.J., et al.: An overview of metal oxide materials as electrocatalysts and supports for polymer electrolyte fuel cells. Energy Environ. Sci. 7, 2535–2558 (2014)CrossRefGoogle Scholar
  37. 37.
    Song, F., Hu, X.L.: Exfoliation of layered double hydroxides for enhanced oxygen evolution catalysis. Nat. Commun. 5, 4477 (2014)CrossRefPubMedGoogle Scholar
  38. 38.
    Diaz-Morales, O., Ledezma-Yanez, I., Koper, M.T.M., et al.: Guidelines for the rational design of Ni-based double hydroxide electrocatalysts for the oxygen evolution reaction. ACS Catal. 5, 5380–5387 (2015)CrossRefGoogle Scholar
  39. 39.
    Zhang, Z., Hao, J.H., Yang, W.S., et al.: Modifying candle soot with FeP nanoparticles into high-performance and cost-effective catalysts for the electrocatalytic hydrogen evolution reaction. Nanoscale 7, 4400–4405 (2015)CrossRefPubMedGoogle Scholar
  40. 40.
    Wang, C.D., Jiang, J., Zhou, X.L., et al.: Alternative synthesis of cobalt monophosphide@C core-shell nanocables for electrochemical hydrogen production. J. Power Sources 286, 464–469 (2015)CrossRefGoogle Scholar
  41. 41.
    Liu, Q., Pu, Z.H., Asiri, A.M., et al.: Nitrogen-doped carbon nanotube supported iron phosphide nanocomposites for highly active electrocatalysis of the hydrogen evolution reaction. Electrochim. Acta 149, 324–329 (2014)CrossRefGoogle Scholar
  42. 42.
    Jin, H., Liu, X., Vasileff, A., et al.: Single-crystal nitrogen-rich 2D Mo5N6 nanosheets for efficient and stable seawater splitting. ACS Nano 12, 12761–12769 (2018)CrossRefPubMedGoogle Scholar
  43. 43.
    Dai, L., Xue, Y., Qu, L., et al.: Metal-free catalysts for oxygen reduction reaction. Chem. Rev. 115, 4823–4892 (2015)CrossRefPubMedGoogle Scholar
  44. 44.
    Hu, C.G., Dai, L.M.: Carbon-based metal-free catalysts for electrocatalysis beyond the ORR. Angew. Chem. Int. Ed. 55, 11736–11758 (2016)CrossRefGoogle Scholar
  45. 45.
    Liu, B.L., Ren, W.C., Gao, L.B., et al.: Metal-catalyst-free growth of single-walled carbon nanotubes. J. Am. Chem. Soc. 131, 2082–2083 (2009)CrossRefPubMedGoogle Scholar
  46. 46.
    Novoselov, K.S., Geim, A.K., Morozov, S.V., et al.: Electric field effect in atomically thin carbon films. Science 306(5696), 666–669 (2004)CrossRefGoogle Scholar
  47. 47.
    Novoselov, K.S., Jiang, D., Schedin, F., et al.: Two-dimensional atomic crystals. Proc. Natl. Acad. Sci. USA 102, 10451–10453 (2005)CrossRefPubMedGoogle Scholar
  48. 48.
    Novoselov, K.S., Mishchenko, A., Carvalho, A., et al.: 2D materials and van der Waals heterostructures. Science 353, aac9439 (2016)CrossRefPubMedGoogle Scholar
  49. 49.
    Jin, H., Guo, C., Liu, X., et al.: Emerging two-dimensional nanomaterials for electrocatalysis. Chem. Rev. 118, 6337–6408 (2018)CrossRefPubMedGoogle Scholar
  50. 50.
    Chen, S., Xu, R., Liu, J., et al.: Simultaneous production and functionalization of boron nitride nanosheets by sugar-assisted mechanochemical exfoliation. Adv. Mater. 31, 1804810 (2019)CrossRefGoogle Scholar
  51. 51.
    Roldan, R., Chirolli, L., Prada, E., et al.: Theory of 2D crystals: graphene and beyond. Chem. Soc. Rev. 46, 4387–4399 (2017)CrossRefPubMedGoogle Scholar
  52. 52.
    Wang, Q.H., Kalantar-Zadeh, K., Kis, A., et al.: Electronics and optoelectronics of two-dimensional transition metal dichalcogenides. Nat. Nanotechnol. 7, 699–712 (2012)CrossRefPubMedGoogle Scholar
  53. 53.
    Wang, H., Yu, L.L., Lee, Y.H., et al.: Integrated circuits based on bilayer MoS2 transistors. Nano Lett. 12, 4674–4680 (2012)CrossRefPubMedGoogle Scholar
  54. 54.
    Gupta, A., Sakthivel, T., Seal, S.: Recent development in 2D materials beyond graphene. Prog. Mater. Sci. 73, 44–126 (2015)CrossRefGoogle Scholar
  55. 55.
    Wang, H., Feng, H.B., Li, J.H.: Graphene and graphene-like layered transition metal dichalcogenides in energy conversion and storage. Small 10, 2165–2181 (2014)CrossRefPubMedGoogle Scholar
  56. 56.
    Yan, D.F., Li, Y.X., Huo, J., et al.: Defect chemistry of nonprecious-metal electrocatalysts for oxygen reactions. Adv. Mater. 29, 1606459 (2017)CrossRefGoogle Scholar
  57. 57.
    Tang, C., Wang, H.F., Chen, X., et al.: Topological defects in metal-free nanocarbon for oxygen electrocatalysis. Adv. Mater. 28, 6845–6851 (2016)CrossRefPubMedGoogle Scholar
  58. 58.
    Xu, Y., Kraft, M., Xu, R.: Metal-free carbonaceous electrocatalysts and photocatalysts for water splitting. Chem. Soc. Rev. 45, 3039–3052 (2016)CrossRefPubMedGoogle Scholar
  59. 59.
    Jia, Y., Zhang, L.Z., Du, A.J., et al.: Defect graphene as a trifunctional catalyst for electrochemical reactions. Adv. Mater. 28, 9532–9538 (2016)CrossRefPubMedGoogle Scholar
  60. 60.
    Tao, L., Wang, Q., Dou, S., et al.: Edge-rich and dopant-free graphene as a highly efficient metal-free electrocatalyst for the oxygen reduction reaction. Chem. Commun. 52, 2764–2767 (2016)CrossRefGoogle Scholar
  61. 61.
    Liu, Z.J., Zhao, Z.H., Wang, Y.Y., et al.: In situ exfoliated, edge-rich, oxygen-functionalized graphene from carbon fibers for oxygen electrocatalysis. Adv. Mater. 29, 1606207 (2017)CrossRefGoogle Scholar
  62. 62.
    Lim, D.H., Wilcox, J.: Mechanisms of the oxygen reduction reaction on defective graphene-supported Pt nanoparticles from first-principles. J. Phys. Chem. C 116, 3653–3660 (2012)CrossRefGoogle Scholar
  63. 63.
    Jia, Y., Zhang, L.Z., Gao, G.P., et al.: A heterostructure coupling of exfoliated Ni-Fe hydroxide nanosheet and defective graphene as a bifunctional electrocatalyst for overall water splitting. Adv. Mater. 29, 1700017 (2017)CrossRefGoogle Scholar
  64. 64.
    Gong, K.P., Du, F., Xia, Z.H., et al.: Nitrogen-doped carbon nanotube arrays with high electrocatalytic activity for oxygen reduction. Science 323, 760–764 (2009)CrossRefGoogle Scholar
  65. 65.
    Qu, L.T., Liu, Y., Baek, J.B., et al.: Nitrogen-doped graphene as efficient metal-free electrocatalyst for oxygen reduction in fuel cells. ACS Nano 4, 1321–1326 (2010)CrossRefPubMedGoogle Scholar
  66. 66.
    Sheng, Z.H., Gao, H.L., Bao, W.J., et al.: Synthesis of boron doped graphene for oxygen reduction reaction in fuel cells. J. Mater. Chem. 22, 390–395 (2012)CrossRefGoogle Scholar
  67. 67.
    Yang, Z., Yao, Z., Li, G.F., et al.: Sulfur-doped graphene as an efficient metal-free cathode catalyst for oxygen reduction. ACS Nano 6, 205–211 (2012)CrossRefPubMedGoogle Scholar
  68. 68.
    Liu, Z.W., Peng, F., Wang, H.J., et al.: Phosphorus-doped graphite layers with high electrocatalytic activity for the O2 reduction in an alkaline medium. Angew. Chem. Int. Ed. 50, 3257–3261 (2011)CrossRefGoogle Scholar
  69. 69.
    Agnoli, S., Favaro, M.: Doping graphene with boron: a review of synthesis methods, physicochemical characterization, and emerging applications. J. Mater. Chem. A 4, 5002–5025 (2016)CrossRefGoogle Scholar
  70. 70.
    Liang, J., Jiao, Y., Jaroniec, M., et al.: Sulfur and nitrogen dual-doped mesoporous graphene electrocatalyst for oxygen reduction with synergistically enhanced performance. Angew. Chem. Int. Ed. 51, 11496–11500 (2012)CrossRefGoogle Scholar
  71. 71.
    Zhang, J.T., Dai, L.M.: Nitrogen, Phosphorus, and fluorine tri-doped graphene as a multifunctional catalyst for self-powered electrochemical water splitting. Angew. Chem. Int. Ed. 55, 13296–13300 (2016)CrossRefGoogle Scholar
  72. 72.
    Lai, L., Potts, J.R., Zhan, D., et al.: Exploration of the active center structure of nitrogen-doped graphene-based catalysts for oxygen reduction reaction. Energy Environ. Sci. 5, 7936 (2012)CrossRefGoogle Scholar
  73. 73.
    Guo, D.H., Shibuya, R., Akiba, C., et al.: Active sites of nitrogen-doped carbon materials for oxygen reduction reaction clarified using model catalysts. Science 351, 361–365 (2016)CrossRefPubMedGoogle Scholar
  74. 74.
    Jia, Z., Li, Y., Zuo, Z., et al.: Synthesis and properties of 2D carbon-graphdiyne. Acc. Chem. Res. 50, 2470–2478 (2017)CrossRefPubMedGoogle Scholar
  75. 75.
    Liang, J., Zheng, Y., Chen, J., et al.: Facile oxygen reduction on a three-dimensionally ordered macroporous graphitic C3N4/carbon composite electrocatalyst. Angew. Chem. Int. Ed. 51, 3892–3896 (2012)CrossRefGoogle Scholar
  76. 76.
    Li, Y., Xu, L., Liu, H., et al.: Graphdiyne and graphyne: from theoretical predictions to practical construction. Chem. Soc. Rev. 43, 2572–2586 (2014)CrossRefPubMedGoogle Scholar
  77. 77.
    Liu, R., Liu, H., Li, Y., et al.: Nitrogen-doped graphdiyne as a metal-free catalyst for high-performance oxygen reduction reactions. Nanoscale 6, 11336–11343 (2014)CrossRefPubMedGoogle Scholar
  78. 78.
    Xue, Y., Guo, Y., Yi, Y., et al.: Self-catalyzed growth of Cu@graphdiyne core–shell nanowires array for high efficient hydrogen evolution cathode. Nano Energy 30, 858–866 (2016)CrossRefGoogle Scholar
  79. 79.
    Zhao, Y., Wan, J., Yao, H., et al.: Few-layer graphdiyne doped with sp-hybridized nitrogen atoms at acetylenic sites for oxygen reduction electrocatalysis. Nat Chem 10, 924–931 (2018)CrossRefPubMedGoogle Scholar
  80. 80.
    Zheng, Y., Jiao, Y., Chen, J., et al.: Nanoporous graphitic-C3N4@carbon metal-free electrocatalysts for highly efficient oxygen reduction. J. Am. Chem. Soc. 133, 20116–20119 (2011)CrossRefGoogle Scholar
  81. 81.
    Zheng, Y., Jiao, Y., Zhu, Y., et al.: Molecule-level g-C3N4 coordinated transition metals as a new class of electrocatalysts for oxygen electrode reactions. J. Am. Chem. Soc. 139, 3336–3339 (2017)CrossRefPubMedGoogle Scholar
  82. 82.
    Ma, T.Y., Dai, S., Jaroniec, M., et al.: Graphitic carbon nitride nanosheet-carbon nanotube three-dimensional porous composites as high-performance oxygen evolution electrocatalysts. Angew. Chem. Int. Ed. 53, 7281–7285 (2014)CrossRefGoogle Scholar
  83. 83.
    Jin, H., Liu, X., Jiao, Y., et al.: Constructing tunable dual active sites on two-dimensional C3N4@MoN hybrid for electrocatalytic hydrogen evolution. Nano Energy 53, 690–697 (2018)CrossRefGoogle Scholar
  84. 84.
    Li, H.N., Shi, Y.M., Chiu, M.H., et al.: Emerging energy applications of two-dimensional layered transition metal dichalcogenides. Nano Energy 18, 293–305 (2015)CrossRefGoogle Scholar
  85. 85.
    Zhang, G., Liu, H.J., Qu, J.H., et al.: Two-dimensional layered MoS2: rational design, properties and electrochemical applications. Energy Environ. Sci. 9, 1190–1209 (2016)CrossRefGoogle Scholar
  86. 86.
    Li, H.Y., Jia, X.F., Zhang, Q., et al.: Metallic transition-metal dichalcogenide nanocatalysts for energy conversion. Chem 4, 1510–1537 (2018)CrossRefGoogle Scholar
  87. 87.
    Tributsch, H., Bennett, J.C.: Electrochemistry and photochemistry of MoS2 layer crystals. J. Electroanal. Chem. 81, 97–111 (1977)CrossRefGoogle Scholar
  88. 88.
    Jaramillo, T.F., Jorgensen, K.P., Bonde, J., et al.: Identification of active edge sites for electrochemical H2 evolution from MoS2 nanocatalysts. Science 317, 100–102 (2007)CrossRefPubMedGoogle Scholar
  89. 89.
    Kibsgaard, J., Chen, Z.B., Reinecke, B.N., et al.: Engineering the surface structure of MoS2 to preferentially expose active edge sites for electrocatalysis. Nat. Mater. 11, 963–969 (2012)CrossRefGoogle Scholar
  90. 90.
    Yin, Y., Han, J., Zhang, Y., et al.: Contributions of phase, sulfur vacancies, and edges to the hydrogen evolution reaction catalytic activity of porous molybdenum disulfide nanosheets. J. Am. Chem. Soc. 138, 7965–7972 (2016)CrossRefPubMedGoogle Scholar
  91. 91.
    Hong, J.H., Hu, Z.X., Probert, M., et al.: Exploring atomic defects in molybdenum disulphide monolayers. Nat. Commun. 6, 6293 (2015)CrossRefPubMedPubMedCentralGoogle Scholar
  92. 92.
    Xie, J.F., Zhang, H., Li, S., et al.: Defect-rich MoS2 ultrathin nanosheets with additional active edge sites for enhanced electrocatalytic hydrogen evolution. Adv. Mater. 25, 5807–5813 (2013)CrossRefPubMedGoogle Scholar
  93. 93.
    Deng, J., Li, H.B., Xiao, J.P., et al.: Triggering the electrocatalytic hydrogen evolution activity of the inert two-dimensional MoS2 surface via single-atom metal doping. Energy Environ. Sci. 8, 1594–1601 (2015)CrossRefGoogle Scholar
  94. 94.
    Voiry, D., Yamaguchi, H., Li, J., et al.: Enhanced catalytic activity in strained chemically exfoliated WS2 nanosheets for hydrogen evolution. Nat. Mater. 12, 850–855 (2013)CrossRefPubMedGoogle Scholar
  95. 95.
    Tan, Y.W., Liu, P., Chen, L.Y., et al.: Monolayer MoS2 films supported by 3D nanoporous metals for high-efficiency electrocatalytic hydrogen production. Adv. Mater. 26, 8023–8028 (2014)CrossRefPubMedGoogle Scholar
  96. 96.
    Putungan, D.B., Lin, S.H., Kuo, J.L.: A first-principles examination of conducting monolayer 1T’-MX2 (M = Mo, W; X = S, Se, Te): promising catalysts for hydrogen evolution reaction and its enhancement by strain. Phys. Chem. Chem. Phys. 17, 21702–21708 (2015)CrossRefPubMedGoogle Scholar
  97. 97.
    Li, H., Tsai, C., Koh, A.L., et al.: Activating and optimizing MoS2 basal planes for hydrogen evolution through the formation of strained sulphur vacancies. Nat. Mater. 15, 48–53 (2016)CrossRefPubMedGoogle Scholar
  98. 98.
    Eda, G., Yamaguchi, H., Voiry, D., et al.: Photoluminescence from chemically exfoliated MoS2. Nano Lett. 11, 5111–5116 (2011)CrossRefPubMedGoogle Scholar
  99. 99.
    Zeng, Z.Y., Yin, Z.Y., Huang, X., et al.: Single-layer semiconducting nanosheets: high-yield preparation and device fabrication. Angew. Chem. Int. Ed. 50, 11093–11097 (2011)CrossRefGoogle Scholar
  100. 100.
    Acerce, M., Voiry, D., Chhowalla, M.: Metallic 1T phase MoS2 nanosheets as supercapacitor electrode materials. Nat. Nanotechnol. 10, 313–318 (2015)CrossRefPubMedGoogle Scholar
  101. 101.
    Wang, H., Lu, Z., Xu, S., et al.: Electrochemical tuning of vertically aligned MoS2 nanofilms and its application in improving hydrogen evolution reaction. Proc. Natl. Acad. Sci. USA 110, 19701–19706 (2013)CrossRefPubMedGoogle Scholar
  102. 102.
    Lukowski, M.A., Daniel, A.S., English, C.R., et al.: Highly active hydrogen evolution catalysis from metallic WS2 nanosheets. Energy Environ. Sci. 7, 2608–2613 (2014)CrossRefGoogle Scholar
  103. 103.
    Luo, Y., Li, X., Cai, X., et al.: Two-dimensional MoS2 confined Co(OH)2 electrocatalysts for hydrogen evolution in alkaline electrolytes. ACS Nano 12, 4565–4573 (2018)CrossRefPubMedGoogle Scholar
  104. 104.
    Subbaraman, R., Tripkovic, D., Chang, K.C., et al.: Trends in activity for the water electrolyser reactions on 3d M(Ni Co, Fe, Mn) hydr(oxy)oxide catalysts. Nat. Mater. 11, 550–557 (2012)CrossRefPubMedGoogle Scholar
  105. 105.
    Yin, Y., Zhang, Y., Gao, T., et al.: Synergistic phase and disorder engineering in 1T-MoSe2 nanosheets for enhanced hydrogen-evolution reaction. Adv. Mater. 29, 1700311 (2017)CrossRefGoogle Scholar
  106. 106.
    Liu, Y., Wu, J., Hackenberg, K.P., et al.: Self-optimizing, highly surface-active layered metal dichalcogenide catalysts for hydrogen evolution. Nat. Energy 2, 17127 (2017)CrossRefGoogle Scholar
  107. 107.
    Shi, J., Wang, X., Zhang, S., et al.: Two-dimensional metallic tantalum disulfide as a hydrogen evolution catalyst. Nat. Commun. 8, 958 (2017)CrossRefPubMedPubMedCentralGoogle Scholar
  108. 108.
    Fan, G., Li, F., Evans, D.G., et al.: Catalytic applications of layered double hydroxides: recent advances and perspectives. Chem. Soc. Rev. 43, 7040–7066 (2014)CrossRefPubMedGoogle Scholar
  109. 109.
    Gong, M., Li, Y.G., Wang, H.L., et al.: An advanced Ni-Fe layered double hydroxide electrocatalyst for water oxidation. J. Am. Chem. Soc. 135, 8452–8455 (2013)CrossRefPubMedGoogle Scholar
  110. 110.
    Liu, R., Wang, Y.Y., Liu, D.D., et al.: Water-plasma-enabled exfoliation of ultrathin layered double hydroxide nanosheets with multivacancies for water oxidation. Adv. Mater. 29, 1701546 (2017)CrossRefGoogle Scholar
  111. 111.
    Liu, P.F., Yang, S., Zhang, B., et al.: Defect-rich ultrathin cobalt-iron layered double hydroxide for electrochemical overall water splitting. ACS Appl. Mater. Interfaces. 8, 34474–34481 (2016)CrossRefPubMedGoogle Scholar
  112. 112.
    Naguib, M., Mashtalir, O., Carle, J., et al.: Two-dimensional transition metal carbides. ACS Nano 6, 1322–1331 (2012)CrossRefPubMedGoogle Scholar
  113. 113.
    Naguib, M., Kurtoglu, M., Presser, V., et al.: Two-dimensional nanocrystals produced by exfoliation of Ti3AlC2. Adv. Mater. 23, 4248–4253 (2011)CrossRefPubMedGoogle Scholar
  114. 114.
    Seh, Z.W., Fredrickson, K.D., Anasori, B., et al.: Two-dimensional molybdenum carbide (MXene) as an efficient electrocatalyst for hydrogen evolution. ACS Energy Lett. 1, 589–594 (2016)CrossRefGoogle Scholar
  115. 115.
    Zhu, J., Ha, E.N., Zhao, G.L., et al.: Recent advance in MXenes: a promising 2D material for catalysis, sensor and chemical adsorption. Coord. Chem. Rev. 352, 306–327 (2017)CrossRefGoogle Scholar
  116. 116.
    Chaudhari, N.K., Jin, H., Kim, B., et al.: MXene: an emerging two-dimensional material for future energy conversion and storage applications. J. Mater. Chem. A 5, 24564–24579 (2017)CrossRefGoogle Scholar
  117. 117.
    Pang, J., Mendes, R.G., Bachmatiuk, A., et al.: Applications of 2D MXenes in energy conversion and storage systems. Chem. Soc. Rev. 48, 72–133 (2018)CrossRefGoogle Scholar
  118. 118.
    Gao, G., O’Mullane, A.P., Du, A.: 2D MXenes: a new family of promising catalysts for the hydrogen evolution reaction. ACS Catal. 7, 494–500 (2016)CrossRefGoogle Scholar
  119. 119.
    Zhang, Z.W., Li, H.N., Zou, G.D., et al.: Self-reduction synthesis of new MXene/Ag composites with unexpected electrocatalytic activity. ACS Sustain Chem. Eng. 4, 6763–6771 (2016)CrossRefGoogle Scholar
  120. 120.
    Xie, X.H., Chen, S.G., Ding, W., et al.: An extraordinarily stable catalyst: Pt NPs supported on two-dimensional Ti3C2X2 (X = OH, F) nanosheets for oxygen reduction reaction. Chem. Commun. 49, 10112–10114 (2013)CrossRefGoogle Scholar
  121. 121.
    Lei, W., Liu, G., Zhang, J., et al.: Black phosphorus nanostructures: recent advances in hybridization, doping and functionalization. Chem. Soc. Rev. 46, 3492–3509 (2017)CrossRefPubMedGoogle Scholar
  122. 122.
    Ling, X., Wang, H., Huang, S., et al.: The renaissance of black phosphorus. Proc. Natl. Acad. Sci. USA 112, 4523–4530 (2015)CrossRefPubMedGoogle Scholar
  123. 123.
    Sofer, Z., Sedmidubsky, D., Huber, S., et al.: Layered black phosphorus: strongly anisotropic magnetic, electronic, and electron-transfer properties. Angew. Chem. Int. Ed. 55, 3382–3386 (2016)CrossRefGoogle Scholar
  124. 124.
    Liu, B.L., Kopf, M., Abbas, A.N., et al.: Black arsenic-phosphorus: layered anisotropic infrared semiconductors with highly tunable compositions and properties. Adv. Mater. 27, 4423–4429 (2015)CrossRefPubMedGoogle Scholar
  125. 125.
    Jiang, Q., Xu, L., Chen, N., et al.: Facile synthesis of black phosphorus: an efficient electrocatalyst for the oxygen evolving reaction. Angew. Chem. Int. Ed. 55, 13849–13853 (2016)CrossRefGoogle Scholar
  126. 126.
    Ren, X., Zhou, J., Qi, X., et al.: Few-layer black phosphorus nanosheets as electrocatalysts for highly efficient oxygen evolution reaction. Adv. Energy Mater. 7, 1700396 (2017)CrossRefGoogle Scholar
  127. 127.
    Wang, J., Liu, D., Huang, H., et al.: In-plane black phosphorus/dicobalt phosphide heterostructure for efficient electrocatalysis. Angew. Chem. 130, 2630–2634 (2018)CrossRefGoogle Scholar
  128. 128.
    Zhao, Y.F., Jia, X.D., Chen, G.B., et al.: Ultrafine NiO nanosheets stabilized by TiO2 from monolayer NiTi-LDH precursors: an active water oxidation electrocatalyst. J. Am. Chem. Soc. 138, 6517–6524 (2016)CrossRefPubMedGoogle Scholar
  129. 129.
    Mahata, A., Garg, P., Rawat, K.S., et al.: A free-standing platinum monolayer as an efficient and selective catalyst for the oxygen reduction reaction. J. Mater. Chem. A 5, 5303–5313 (2017)CrossRefGoogle Scholar
  130. 130.
    Lai, J., Chao, Y., Zhou, P., et al.: One-pot seedless aqueous design of metal nanostructures for energy electrocatalytic applications. Electrochem. Energy Rev. 1, 531–547 (2018)CrossRefGoogle Scholar
  131. 131.
    Mahmood, A., Lin, H., Xie, N., et al.: Surface confinement etching and polarization matter: a new approach to prepare ultrathin PtAgCo nanosheets for hydrogen-evolution reactions. Chem. Mater. 29, 6329–6335 (2017)CrossRefGoogle Scholar
  132. 132.
    Luo, M., Yang, Y., Sun, Y., et al.: Ultrathin two-dimensional metallic nanocrystals for renewable energy electrocatalysis. Mater. Today 23, 45–56 (2019)CrossRefGoogle Scholar
  133. 133.
    Kong, X., Xu, K., Zhang, C., et al.: Free-standing two-dimensional Ru nanosheets with high activity toward water splitting. ACS Catal. 6, 1487–1492 (2016)CrossRefGoogle Scholar
  134. 134.
    Pi, Y.C., Zhang, N., Guo, S.J., et al.: Ultrathin laminar Ir superstructure as highly efficient oxygen evolution electrocatalyst in broad pH range. Nano Lett. 16, 4424–4430 (2016)CrossRefPubMedGoogle Scholar
  135. 135.
    Fei, H., Dong, J., Arellano-Jimenez, M.J., et al.: Atomic cobalt on nitrogen-doped graphene for hydrogen generation. Nat. Commun. 6, 8668 (2015)CrossRefPubMedPubMedCentralGoogle Scholar
  136. 136.
    Cheng, N.C., Stambula, S., Wang, D., et al.: Platinum single-atom and cluster catalysis of the hydrogen evolution reaction. Nat. Commun. 7, 13628 (2016)CrossRefGoogle Scholar
  137. 137.
    Cheng, Y.F., Lu, S.K., Liao, F., et al.: Rh-MoS2 nanocomposite catalysts with Pt-like activity for hydrogen evolution reaction. Adv. Funct. Mater. 27, 1700359 (2017)CrossRefGoogle Scholar
  138. 138.
    Wang, X.P., Wang, L.X., Zhao, F., et al.: Monoatomic-thick graphitic carbon nitride dots on graphene sheets as an efficient catalyst in the oxygen reduction reaction. Nanoscale 7, 3035–3042 (2015)CrossRefPubMedGoogle Scholar
  139. 139.
    Liang, Y.Y., Li, Y.G., Wang, H.L., et al.: Co3O4 nanocrystals on graphene as a synergistic catalyst for oxygen reduction reaction. Nat. Mater. 10, 780–786 (2011)CrossRefPubMedGoogle Scholar
  140. 140.
    Dou, S., Tao, L., Huo, J., et al.: Etched and doped Co9S8/graphene hybrid for oxygen electrocatalysis. Energy Environ. Sci. 9, 1320–1326 (2016)CrossRefGoogle Scholar
  141. 141.
    Cui, X., Ren, P., Deng, D., et al.: Single layer graphene encapsulating non-precious metals as high-performance electrocatalysts for water oxidation. Energy Environ. Sci. 9, 123–129 (2016)CrossRefGoogle Scholar
  142. 142.
    Li, Y.G., Wang, H.L., Xie, L.M., et al.: MoS2 nanoparticles grown on graphene: an advanced catalyst for the hydrogen evolution reaction. J. Am. Chem. Soc. 133, 7296–7299 (2011)CrossRefGoogle Scholar
  143. 143.
    Luo, Y.T., Tang, L., Khan, U., et al.: Morphology and surface chemistry engineering for pH-universal catalysts toward hydrogen evolution at large current density. Nat. Commun. 10, 269 (2019)CrossRefPubMedPubMedCentralGoogle Scholar
  144. 144.
    Ma, T.Y., Dai, S., Jaroniec, M., et al.: Graphitic carbon nitride nanosheet-carbon nanotube three-dimensional porous composites as high-performance oxygen evolution electrocatalysts. Angew. Chem. Int. Ed. 53, 7281–7285 (2014)CrossRefGoogle Scholar
  145. 145.
    Ma, T.Y., Dai, S., Qiao, S.Z.: Self-supported electrocatalysts for advanced energy conversion processes. Mater. Today 19, 265–273 (2016)CrossRefGoogle Scholar
  146. 146.
    Li, Y., Zhou, W., Wang, H., et al.: An oxygen reduction electrocatalyst based on carbon nanotube–graphene complexes. Nat. Nanotechnol. 7, 394–400 (2012)CrossRefPubMedGoogle Scholar
  147. 147.
    Li, D.J., Maiti, U.N., Lim, J., et al.: Molybdenum sulfide/N-doped CNT forest hybrid catalysts for high-performance hydrogen evolution reaction. Nano Lett. 14, 1228–1233 (2014)CrossRefPubMedGoogle Scholar
  148. 148.
    Chen, P., Xiao, T.Y., Qian, Y.H., et al.: A nitrogen-doped graphene/carbon nanotube nanocomposite with synergistically enhanced electrochemical activity. Adv. Mater. 25, 3192–3196 (2013)CrossRefPubMedGoogle Scholar
  149. 149.
    Chen, S., Duan, J.J., Jaroniec, M., et al.: Nitrogen and oxygen dual-doped carbon hydrogel film as a substrate-free electrode for highly efficient oxygen evolution reaction. Adv. Mater. 26, 2925–2930 (2014)CrossRefPubMedGoogle Scholar
  150. 150.
    Cherevko, S., Geiger, S., Kasian, O., et al.: Oxygen and hydrogen evolution reactions on Ru, RuO2, Ir, and IrO2 thin film electrodes in acidic and alkaline electrolytes: a comparative study on activity and stability. Catal. Today 262, 170–180 (2016)CrossRefGoogle Scholar
  151. 151.
    Tian, J.Q., Liu, Q., Asiri, A.M., et al.: Ultrathin graphitic C3N4 nanosheets/graphene composites: efficient organic electrocatalyst for oxygen evolution reaction. Chemsuschem 7, 2125–2130 (2014)CrossRefPubMedGoogle Scholar
  152. 152.
    Lei, H.T., Liu, C.Y., Wang, Z.J., et al.: Noncovalent immobilization of a pyrene-modified cobalt corrole on carbon supports for enhanced electrocatalytic oxygen reduction and oxygen evolution in aqueous solutions. ACS Catal 6, 6429–6437 (2016)CrossRefGoogle Scholar
  153. 153.
    Wurster, B., Grumelli, D., Hotger, D., et al.: Driving the oxygen evolution reaction by nonlinear cooperativity in bimetallic coordination catalysts. J. Am. Chem. Soc. 138, 3623–3626 (2016)CrossRefPubMedGoogle Scholar
  154. 154.
    Lei, Y., Pakhira, S., Fujisawa, K., et al.: Low-temperature synthesis of heterostructures of transition metal dichalcogenide alloys (WxMo1−xS2) and graphene with superior catalytic performance for hydrogen evolution. ACS Nano 11, 5103–5112 (2017)CrossRefPubMedGoogle Scholar
  155. 155.
    Geim, A.K., Grigorieva, I.V.: Van der Waals heterostructures. Nature 499, 419 (2013)CrossRefPubMedGoogle Scholar
  156. 156.
    Jia, Y., Zhang, L., Gao, G., et al.: A heterostructure coupling of exfoliated Ni-Fe hydroxide nanosheet and defective graphene as a bifunctional electrocatalyst for overall water splitting. Adv. Mater. 29, 1700017 (2017)CrossRefGoogle Scholar
  157. 157.
    Li, H., Yu, K., Li, C., et al.: Charge-transfer induced high efficient hydrogen evolution of MoS2/graphene cocatalyst. Sci. Rep. 5, 18730 (2015)CrossRefPubMedPubMedCentralGoogle Scholar
  158. 158.
    Ma, T.Y., Cao, J.L., Jaroniec, M., et al.: Interacting carbon nitride and titanium carbide nanosheets for high-performance oxygen evolution. Angew. Chem. Int. Ed. 55, 1138–1142 (2016)CrossRefGoogle Scholar
  159. 159.
    Yang, J., Voiry, D., Ahn, S.J., et al.: Two-dimensional hybrid nanosheets of tungsten disulfide and reduced graphene oxide as catalysts for enhanced hydrogen evolution. Angew. Chem. Int. Ed. 52, 13751–13754 (2013)CrossRefGoogle Scholar
  160. 160.
    Tang, C., Zhong, L., Zhang, B., et al.: 3D mesoporous van der Waals heterostructures for trifunctional energy electrocatalysis. Adv. Mater. 30, 1705110 (2018)CrossRefGoogle Scholar
  161. 161.
    Zhang, H.Y., Tian, Y., Zhao, J.X., et al.: Small dopants make big differences: enhanced electrocatalytic performance of MoS2 monolayer for oxygen reduction reaction (ORR) by N- and P-doping. Electrochim. Acta 225, 543–550 (2017)CrossRefGoogle Scholar
  162. 162.
    Xiao, W., Liu, P.T., Zhang, J.Y., et al.: Dual-functional N dopants in edges and basal plane of MoS2 nanosheets toward efficient and durable hydrogen evolution. Adv. Energy Mater. 7, 1602086 (2017)CrossRefGoogle Scholar
  163. 163.
    Duan, J.J., Chen, S., Jaroniec, M., et al.: Porous C3N4 nanolayers@N-graphene films as catalyst electrodes for highly efficient hydrogen evolution. ACS Nano 9, 931–940 (2015)CrossRefGoogle Scholar
  164. 164.
    Voiry, D., Fullon, R., Yang, J.E., et al.: The role of electronic coupling between substrate and 2D MoS2 nanosheets in electrocatalytic production of hydrogen. Nat. Mater. 15, 1003–1009 (2016)CrossRefPubMedGoogle Scholar
  165. 165.
    Conway, B.E., Tilak, B.V.: Interfacial processes involving electrocatalytic evolution and oxidation of H2 and the role of chemisorbed H. Electrochim. Acta 47, 3571–3594 (2002)CrossRefGoogle Scholar

Copyright information

© Shanghai University and Periodicals Agency of Shanghai University 2019

Authors and Affiliations

  1. 1.Shenzhen Geim Graphene Center (SGC), Tsinghua-Berkeley Shenzhen Institute (TBSI)Tsinghua UniversityShenzhenChina
  2. 2.Shenyang National Laboratory for Materials Science, Institute of Metal ResearchChinese Academy of SciencesShenyangChina

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