Recent Progress on Transition Metal Based Layered Double Hydroxides Tailored for Oxygen Electrode Reactions

Abstract

The oxygen reduction reaction (ORR) and oxygen evolution reaction (OER), namely, so-called oxygen electrode reactions, are two fundamental half-cell reactions in the energy storage and conversion devices, e.g., zinc–air batteries and fuel cells. However, the oxygen electrode reactions suffer from sluggish kinetics, large overpotential and complicated reaction paths, and thus require efficient and stable electrocatalysts. Transition-metal-based layered double hydroxides (LDHs) and their derivatives have displayed excellent catalytic performance, suggesting a major contribution to accelerate electrochemical reactions. The rational regulation of electronic structure, defects, and coordination environment of active sites via various functionalized strategies, including tuning the chemical composition, structural architecture, and topotactic transformation process of LDHs precursors, has a great influence on the resulting electrocatalytic behavior. In addition, an in-depth understanding of the structural performance and chemical-composition-performance relationships of LDHs-based electrocatalysts can promote further rational design and optimization of high-performance electrocatalysts. Finally, prospects for the design of efficient and stable LDHs-based materials, for mass-production and large-scale application in practice, are discussed.

1. Introduction

The excessive consumption of fossil fuels and accompanying environmental issues, e.g., greenhouse effect and NO_x/SO_x pollutants emission, have caused serious effect on the development of global society. Under the “new policies” or “current policies” scenarios from the International Energy Agency (IEA), the world’s energy demand will increase from 12 TW in 2009 to 17 or 18 TW by 2035, respectively, accompanied by CO₂ emissions soaring from 29 Gt yr⁻¹ in 2009 to 36 or 43 Gt yr⁻¹ in 2035 [1]. Consequently, the exploitation and use of renewable, and sustainable energy sources, such as solar, wind, biomass, and tide, are of vital importance in reducing the dependence on fossil fuels [2,3,4,5].

Hydrogen (H₂), an ideal and zero-carbon energy carrier with high heat value (142 MJ kg⁻¹) and energy conversion efficiency has been considered as the most promising candidate to replace fossil fuels in the twenty-first century [6,7,8]. Recently, electrochemical water splitting is regarded as a highly efficient and sustainable H₂ production technology, in which the generated electricity from renewable energy sources is stored in the form of chemical energy: 2H₂O + energy → 2H_2(g) + O_2(g) [9]. The produced H₂ can be further converted into electricity: 2H_2(g) + O_2(g) → 2H₂O + electricity, in fuel cells (FCs) system. The pivotal processes of energy storage and conversion devices like fuel cells, and metal-air batteries (MABs) are four electrochemical “half-reactions”, namely, hydrogen evolution reaction (HER), hydrogen oxidation reaction (HOR), oxygen reduction reaction (ORR), and oxygen evolution reaction (OER) [10,11,12]. Alkaline HER process involves, in alkaline electrolyte, the water dissociation, namely, the two-electron transfer HER (2H₂O + 2e⁻ → H₂ + 2OH⁻) at the cathode of electrochemical water splitting device, whereas the anodic OER shows a more complex reaction mechanism involving four-electron-OH⁻-coupling processes (4OH⁻ → O₂ + 2H₂O + 4e⁻). The formation of various OER intermediates (O_ad, OH_ad, and OOH_ad), as well as adsorption/desorption of oxygen molecules, which leads to a sluggish kinetics and high overpotential (η) [13]. The OER mechanism depends mainly on the surface property of the catalyst. There are several proposed possible mechanisms for OER, i.e., traditional adsorption evolution mechanism (AEM) and a lattice-oxygen-mediated mechanism (LOM) [14]. For example, the traditional adsorption evolution process, in alkaline environment, can be described by the following steps (“*” denotes an active site): (i) OH⁻ species is adsorbed on the electrode surface, and form the *OH intermediate (OH⁻ + * → *OH + e⁻); (ii) generated *OH intermediate interacts with OH⁻ to produce *O specie (*OH + OH⁻ → *O + H₂O + e⁻); (iii) the *O specie is combined with OH⁻, forming *OOH intermediate; (iv) the above *OOH intermediate is further oxidized to O₂ molecule (*OOH + OH⁻ → O₂ + H₂O + e⁻ + *) [14]. In comparison with the AEM, the existence of lattice oxygen is found in the LOM process. Initially, the OH⁻ species on two neighboring metal sites undergo deprotonation and form metal–oxo intermediates. Next, the metal–oxo intermediates directly couple to form O-O bond instead of producing *OOH species. Finally, the molecular oxygen (O₂) is released with the generation of two oxygen vacancies, which are subsequently occupied by OH⁻ for a continuous OER process [14]. To achieve low overpotentials, extensive efforts have been devoted to developing highly efficient electrocatalysts with optimal binding energy for OER intermediates to reduce the reaction energy barrier, and thus accelerate the reaction rate [15].

Until now, the benchmark electrocatalysts towards OER are precious metal materials, such as ruthenium oxides (RuO₂) and iridium oxides (IrO₂) [16,17,18], but their high cost and scarcity hinder their industrial use [19,20,21]. Therefore, the development of non-precious electrocatalysts towards OER, with high efficiency, excellent electrical conductivity, abundant active surface, as well as structural stability, is crucially important to achieve large-scale commercial application of clean energy infrastructures. The first 3d transition metals such as Mn, Fe, Co, and Ni oxides [22,23,24,25,26,27,28,29]; hydroxides [30,31,32,33,34,35]; phosphides [36,37,38,39,40,41,42]; chalcogenides [43,44,45,46,47,48]; and layered double hydroxides (LDHs) [49,50,51,52,53,54,55,56] have aroused great interest in the OER as potential alternatives to precious metals due to their intriguing intrinsic activity and stability. It is worth mentioning that one of the first reports, in 1983, on the electrocatalytic performance of metal hydroxides, revealed a good OER activity of α-Ni(OH)₂ [57], and it was further confirmed that the Fe impurities in the α-Ni(OH)₂ greatly lower the OER overpotential [58,59]. Since then, the LDHs of 3d iron group metals (Fe, Co and Ni)—such as Ni-Fe [60,61,62,63,64], Ni-Co [65,66,67,68], Co-Ni [69,70,71], Fe-Ni [72,73,74], Fe-Co [75,76,77,78], and Co-Co [79,80,81,82]—and the corresponding derivatives—e.g., NiFe₂O₄ [83,84,85,86], CoFe₂O₄ [87], NiCo₂O₄ [88,89], and Co₃O₄ [90,91,92]—have been employed as OER or bifunctional ORR/OER electrocatalysts with high kinetics in alkaline solution.

Several review articles have summarized the multidimensional applications of LDHs including energy storage and conversion [21,93,94]. For example, Gong’s group [95] published a mini review in 2014, which was focused on the early discovery and recent progress on NiFe-LDHs for OER electrocatalysis in terms of chemical properties, synthetic methodologies, as well as catalytic performances. Kundu and co-workers [93] provided a detailed review with insights on the structure, activity, and mechanism of LDHs and layered-oxide materials in the electrochemical and photoelectrochemical water oxidation. Recently, a review by Sun’s group [50] covered the identification of active sites in LDHs materials at the atomic level for the OER, the superaerophobic nanoarray electrode assembly as well as the current optimization strategies of active sites. However, there is still a lack of a comprehensive review on the functionalization strategies of LDHs and their derivatives as OER or ORR/OER bifunctional electrocatalysts.

Herein, we summarize the most recent advances in the functionalization strategies, structural performance and chemical-composition-performance relationships of transition metal based LDHs and corresponding derivatives served as catalysts in the OER electrocatalysis in alkaline medium. Specifically, common functionalization strategies involving LDHs are designed into the following major categories, in Figure 1, namely: (1) layer composition tuning; (2) intercalation; (3) vacancy engineering; (4) ultrathin nanosheets; (5) nanostructuring; and (6) hybridization. In addition, the application of LDHs-based materials used as bifunctional ORR/OER electrocatalysts is also shown. Finally, we briefly point out the remaining challenges to achieve large-scale commercial applications of renewable energy storage and conversion devices, as well as opportunities in developing advanced, efficient, and stable transition metal-based LDHs materials towards ORR and OER processes.

2. Fundamental Characteristics of LDHs

Layered double hydroxides (LDHs) or hydrotalcite-like compounds, are a typical kind of two-dimensional (2D) layered anionic clay materials [96,97], which can be described by a generic formula [M^II_1−xM^III_x(OH)₂(Aⁿ⁻)_x/n • yH₂O], where M^II and M^III represent the divalent (e.g., Mg²⁺, Co²⁺, Ni²⁺, Cu²⁺ or Zn²⁺) and trivalent (e.g., Al³⁺, Fe³⁺, or Cr³⁺) metal cations, respectively; Aⁿ⁻ is the interlayer anion (e.g., CO₃²⁻, NO₃⁻, Cl⁻, SO₄²⁻ or HPO₄²⁻) compensating the positive charge of the host-sheet; x is the molar ratio of M^II/(M^II + M^III) and generally ranges from 0.20 to 0.33; y is the amount of molecular H₂O [98,99]. Within the 2D structure, LDHs consist of the positively charged host sheets and the interlayer guests containing negatively charged anions and water molecules (Figure 2) [100]. Due to various host–guest assemblies and nanoarchitectures with versatile physico-chemical properties, LDHs have been proved to be promising candidates for a wide range of applications like flame retardant [101], anticorrosive coating [102,103], catalysis [104,105,106], and energy storage and conversion [107,108,109]. Particularly, in the OER electrocatalysis, LDHs offer a number of advantages: (i) the tunable chemical composition, including the type of metal cations and molar ratio of M^II/(M^II + M^III), favors to improve the intrinsic catalytic activity or introduce the extra active sites; (ii) the exchangeable interlayer anions (Aⁿ⁻) with large sizes can enlarge the interlayer region, resulting in the exposure of more inner active sites; (iii) the synergistic interaction between the highly dispersed M^II and M^III cations, in the host sheets, favors the enhancement of the electrocatalytic activity; (iv) the geometric morphology, coordination environment and surface defects of LDHs can be modulated by precisely designing and controlling the chemical compositions of LDHs, which not only provide unsaturated active centers, such as low-coordinated metal cations, corner or edge sites, but also improve the porosity and electronic conductivity; and (v) a series of mixed metal oxides (MMOs) with high electrocatalytic performance can be acquired from LDHs via topological structure transformation process.

2.1. Binary LDHs

In mono-metallic hydroxides of divalent cations, the activity trend is directly correlated with the d-electron configuration. The decrease in the OER activity of 3d mono-metallic (oxy)hydroxides that followed the order: Ni > Co > Fe > Mn, was first reported by Subbaraman et al. [110], along with the increase in the oxophilicity of the 3d-M elements. Based on the interaction between 3d metal (oxy)hydroxides and OH_ad, the authors concluded that the OER reactivity trend was determined by the strength of OH_ad–M^2+δ (δ: valence state), with M (Ni < Co < Fe < Mn), and δ variation (0 ≤ δ ≤ 1.5). When the interaction between OH_ad and metals was too strong, the reaction intermediates were stabilized, leading to a lower turnover frequency (defined as the number of complete reaction events per site per second). This was called “poisoning” effect of catalytic sites by preventing them from coordinating with hydroxide/oxyhydroxide ligands. Thus, among these 3d metals, Ni, with an optimal interaction strength with OH_ad, satisfied the Sabatier principle for OER catalyst design.

In addition, when other metal elements are incorporated in the mono-metallic hydroxides, the formed binary hydroxides possess near-optimal binding energies of O* intermediates that facilitate the absorption/desorption for OER process, which is ascribed to the modulation of the local coordination environment and electronic structure [111]. In this context, Chen et al. [112] prepared Cu-doped cobalt hydroxide (Cu-Co(OH)₂) nanosheets with an excellent performance for OER. Interestingly, the Cu-doping favored the increase of the positive charge in the matrix of Co ions. The valence states of Co ions in Cu-Co(OH)₂ were 2 + δ (0 < δ < 1), higher than 2+ as in Co(OH)₂, which tended to absorb OH⁻ and facilitates the formation of Co⁽⁺⁾-OH_ad and Co-OOH species. Similarly, Qiao et al. [113] developed porous ZnCo-LDH nanosheets as an efficient OER electrocatalyst delivering a current density of ~15.06 mA cm⁻² at η = 0.54 V. It explained that the inactive Zn element, in the alternately distributed binary LDH host-sheets, played a key role in overlapping of e_g orbital of active sites and O-2p_σ orbital of reactant OH⁻, which facilitated the formation of M=O bonds, thus reducing the OER kinetic energy barrier. Similarly, an ultrathin amorphous cobalt-vanadium hydr(oxy)oxide (CoV-hydr(oxy)oxide) for water oxidation was synthesized by Liu et al. [114]. They suggested that the Co active sites with near-optimal energetics for OER in CoV-hydr(oxy)oxides could be attributed to the modification of the coordination environment of Co atoms caused by lattice mismatch, originating from the V-doping.

The NiFe-LDHs have recently documented to possess the highest OER catalytic activity and stability among the binary LDHs, especially when the Ni/Fe ratio is 3:1 [115]; which was firstly developed for OER electrocatalysis in 2013, thanks to the work of Gong and co-workers [116]. The active site for OER process in alkaline conditions on NiFe-LDHs has been studied and reported in many publications over the years. In the early 21st century, the so-called “Ni active site” mechanism was proposed, and then turned out to be that the Fe element was the active site (“Fe active site” mechanism); while some recent findings propose that the synergistic effect of Ni and Fe sites are responsible for the high OER activity. A pioneering study carried out by Bell’s group [117], probed the active sites of Ni-Fe films on the OER activity. They found that the Ni-Fe film, with a surface composition of 40% Fe, exhibited an enhanced OER activity that was roughly 2 orders of magnitude higher than that of a fresh Ni film. In addition, the in situ Raman spectra results demonstrated that the local environment of Ni-O, modified by Fe correlated with the increasing OER activity. These observations suggested that the OER was catalyzed by Ni in Ni-Fe films, and the incorporation of Fe gave rise to an increase in the potential at which Ni(OH)₂/NiOOH redox took place. Additionally, Trotochaud et al. [118] proposed that in a Ni_1−xFe_xOOH OER electrocatalyst, Fe played an activated effect on Ni active centers via a partial-charge-transfer mechanism, which leaded to a lower dependence of thickness for Ni_1−xFe_xOOH than NiOOH. This work showed that the incorporation of Fe-impurities was responsible for the dramatic increase in OER activity of aged Ni(OH)₂/NiOOH and held a view that β-NiOOH was less active for OER than the disordered γ-NiOOH.

Some research groups argued that, although iron ion existed in OER catalysts (NiFe oxides/(oxy)hydroxides) in the form of +3 oxidation state, it still acted as the main active site of the catalytic reaction [58,118,119]. Bell et al. [120] probed the short-range structure at Fe and Ni sites in electrodeposited (Ni,Fe) oxyhydroxide catalysts through operando X-ray absorption spectroscopy (XAS), using high energy resolution fluorescence detection (HERFD). They showed that a 500-fold increase in the OER activity originated from Ni_1−xFe_xOOH as compared with NiOOH and FeOOH. The in situ HERFD and XAS data revealed that Fe³⁺, located in the octahedral sites with short Fe-O bond distances, was triggered by the edge-sharing with the surrounding [NiO₆] octahedra. This explanation was reinforced by the density function theory with Hubbard U (DFT+U) calculations. More importantly, DFT+U calculations established that the active sites in Ni_1−xFe_xOOH for the oxidation of water were Fe³⁺ ions. These species presented an extremely lower overpotential than Ni³⁺ cations in either γ-Ni_1−xFe_xOOH or γ-NiOOH.

To elucidate the role of Fe cation in NiFe-LDHs with a metal molar ratio of 3:1, Chen et al. [121] carried out an operando Mössbauer spectroscopy study. Figure 3A displays the dynamic CV curves recorded in the operando cell, as well as the Mössbauer spectrum collected initially at the open-circuit potential (OCP), and then at 1.49 V, 1.62 V and 1.72 V, respectively. In Figure 3B, under the OCP, the Mössbauer spectrum showed a doublet with an isomer shift (δ) of 0.34 mm/s and quadrupole splitting (Δ) of 0.46 mm/s, which remained unchanged until 1.49 V, cf. Figure 3C. When the applied potential increased to 1.62 V, in Figure 3D, there was a new singlet at δ = −0.27 mm/s, and the intensity reflected the oxidation of approximately 12% of the Fe sites in the material, which was conferred to the oxidized Fe species as Fe⁴⁺. With an applied electrode potential of 1.76 V, a growth of this oxidized Fe peak with ~21% of the total Fe (Figure 3E) was observed. When the potential was returned to 1.49 V, the oxidized Fe peak was still evident in the Mössbauer spectrum (~20% of total Fe, Figure 3F). This work provides the obvious evidence for the formation of Fe⁴⁺ in NiFe oxides during the OER process, suggesting that more attention is needed to be paid on the role of reactive Fe⁴⁺ species generated at edge, corner, or defect sites within Fe-doped NiOOH lattice. Bard et al. [122] reported the direct measurement of surface OER kinetics of Ni⁴⁺ and Fe⁴⁺ in NiOOH, FeOOH, and Ni_1−xFe_xOOH (0 < x < 0.27) by performing surface interrogation scanning electrochemical microscopy (SI-SECM). Two types of surface sites showing “fast” and “slow” OER kinetics were found in FeOOH and Ni_1−xFe_xOOH electrodes, where the fraction of “fast” sites in Ni_1−xFe_xOOH coincided well with the Fe atom content in the film, suggesting that the dispersed Fe atoms, in a NiOOH matrix, were indeed the active sites for OER process.

Many reports have shown that the Fe ion that exist in the form of +3 oxidation state in the OER process, assist to accelerate the OER process, and improve the electrocatalytic performance [123,124,125,126]. Strasser et al. [123] explored the active metal redox states of Fe and Ni in amorphous NiFe oxyhydroxide by means of operando differential electrochemical mass spectrometry (DEMS) and XAS (Figure 4A,B). Under OER conditions in 0.1 M KOH, Ni centers were present in the +4 oxidation states at Fe content <4 at%. However, Ni atoms were stabilized in low-valent +2 oxidation states at >4 at% Fe contents, while the faradaic efficiency of O₂ was increased, suggesting that the OER active state could be designated as Ni⁺²Fe⁺³OOH. Nocera et al. [124] suggested that the incorporation of Fe³⁺, as a superior Lewis acid into Ni oxide matrix, helped to increase the acidity of OH_x moieties and then engendered a greater population of Ni⁴⁺, which in turn led to an increase in the oxyl character along with an enhanced activity of the catalyst in promoting OER. Based on in situ Raman spectro-electrochemistry, Edvinsson et al. [127] proposed that the synergistic electronic interplay between Fe and Ni is crucial for alkaline water splitting. As shown in Figure 4C–E, with increased overpotentials, on the NiFe LDHs, the Ni(OH)₂ gradually converts to γ-NiOOH with a high OER reactivity. Compared with single Ni(OH)₂ in Figure 4C, the binary NiFe-LDHs showed a sluggish transition period from Ni(OH)₂ to γ-NiOOH at high overpotentials, indicating that the presence of Fe in the NiFe-LDHs inhibited the electrochemical oxidation of Ni(OH)₂ to γ-NiOOH. The authors suggested that at low overpotentials OH_ad was adsorbed at Fe sites to form FeOOH species whereas at high potentials it tended to be anchored at (or migrated to) Ni sites. It was explained that the electronic effect of Fe³⁺ could induce the formation of γ-NiOOH phase with a higher Ni valence state, and thus the OH_ad selectively adsorbed on Ni site to form O_Had-Ni^δ+ intermediate to accelerate the water dissociation (Figure 4E).

Although in recent decades, numerous advanced ex- and in situ technologies as well as theory calculation have been employed to get an insight of the roles of Ni and Fe elements in determining the OER activity of NiFe-LDHs electrocatalysts, it still remains a matter of controversy as to the true active centers for OER electrocatalysis. Thus far, regarding to the roles of Ni and Fe in NiFe-LDHs system, there are several possibilities: (1) Ni is the active site and Fe plays an activated effect on it; (2) Fe is the active site and Ni provides a conductive support for OER process; and (3) Ni works with Fe to boost the OER activity.

3. Strategies to Functionalize LDHs

Although LDHs materials with unique properties have been proved to be promising candidates for OER catalysis, they still suffer from intrinsic drawbacks, e.g., low electrical conductivity (10⁻¹³–10⁻¹⁷ S cm⁻¹), poor intrinsic activity of active sites, and structural collapsibility. These factors limit the electrocatalytic performance improvement of LDHs materials. To overcome these constraints, various functionalization strategies were proposed, namely: (1) increasing the number of active sites (e.g., through increased mass loading or improved catalyst structuring to expose more active sites per gram) and (2) improving the intrinsic activity of each active site. For example, by regulating the layer composition, through changing the metal components, relative molar ratio and oxidation state, the electronic structure can be optimized to improve the intrinsic active sites. The exfoliated LDHs nanosheets are prone to expose more active sites on the surface than the LDHs bulk, leading to a fast electron transfer process coupled to protons and rapid diffusion of reactants, thus accelerating the rate of the redox reaction. The construction of three-dimensional (3D) hierarchical nano-architecture of LDHs can remarkably facilitate the electron/charge transfer and the diffusion of reactants during the water oxidation.

3.1. Regulation of Layer Composition

The layer composition of LDHs is adjustable, i.e., the metal components, the relative molar ratio, and the chemical valence state can be modulated in the host-sheets, which can be achieved by adding reducing metal element(s) or replacing the metal element(s) with different metals. As mentioned in Section 2.1, the incorporation of additional cations into the metal hydroxides causes the lattice mismatch, modifying the coordination environment and the electronic structure of active sites. Taking NiFe-LDHs as a benchmark for OER catalysis, in which Fe³⁺ centers are atomically surrounded and isolated by Ni²⁺ sites to form Ni-O-Fe motifs; there are several representative studies involving doping with a third metal cation selected from M^II = Co²⁺, Mn²⁺, Fe²⁺ and M^III = Fe³⁺, Co³⁺, Cr³⁺, V³⁺.

According to a well-known “adsorbate evolution mechanism” (AEM), the metal sites with electron-rich structure are more easily oxidized, thus possessing higher reactivity for OER catalysis. Zhou et al. [128] reported that the doping of Mn cations with a weaker electronegativity than Ni and Fe leaded to activation of basal plane in NiFe-LDHs. Compared to pristine NiFe-LDHs, Mn²⁺-doped NiFe-LDHs showed increased electron densities on Ni and Fe sites in the basal plane (initial: Ni²⁺ (8.92), Fe³⁺ (6.72); after doping: Ni²⁺ (8.96), Fe³⁺ (6.83)), as revealed by the DFT+U calculation, cf. Figure 5. Such surface electronic structure modification of Ni and Fe sites encountered in Mn²⁺-doped NiFe-LDHs led to an overpotential of 230 mV at 100 mA cm⁻² and a Tafel slope of 68 mV dec⁻¹ in 1 M KOH solution. Such data were much lower than those of pristine NiFe-LDHs. Apart from Mn cation with an oxidation state of +2, the Mn⁴⁺ was also chosen to dope the laminate of NiFe-LDHs to improve the intrinsic electric conductivity, which displayed a narrower bandgap than that of NiFe-LDHs [129]. Moreover, Cai et al. [130] modified the local atomic structure of NiFe-LDHs by partially replacing Ni²⁺ with Fe²⁺, forming Fe-O-Fe motifs in Ni²⁺Fe²⁺Fe³⁺-LDHs system. The in situ spectroscopic characterization results combined with DFT study demonstrated that the Fe-O-Fe sites could stabilize the high-valent Fe sites (i.e., Fe^(3+δ)+, where δ > 0), decreasing the energy barrier of the deprotonation step and resulting in an ultralow overpotential of 195 mV at 10 mA cm⁻² for OER.

Additionally, the Co-doped NiFe-LDHs also exhibited an enhanced OER activity relative to pristine NiFe-LDHs. Strongin et al. [131] found that the doping amount of Co cations into NiFe-LDHs was strongly associated with their corresponding OER performance. The Ni₁₅Fe₅Co_2.5-LDHs with cobalt substitution of ~12% showed an improvement in catalysis while a higher degree of substitution resulted in a slight decrease in OER activity. Such phenomenon was attributed to the modified energetics of OER reaction intermediates (O*, *OH, and *OOH), which led to the improvement in OER catalysis. In another case, Co²⁺ and Co³⁺ were doped into NiFe-LDHs to substitute Ni²⁺ and Fe³⁺, forming Co²⁺-doped NiFe-LDHs and Co³⁺-doped NiFe-LDHs, respectively [132]. The authors considered that Fe³⁺ in Co²⁺-doped NiFe-LDHs and Co³⁺ in Co³⁺-doped NiFe-LDHs were responsible for the high OER activity. In particular, the DFT+U simulation found that Co³⁺ with an optimal electronic structure could easily accept electrons from H₂O molecules, and thus accelerated the deprotonation step (*OH → *O). The Co³⁺-doped NiFe-LDHs and Co²⁺-doped NiFe-LDHs exhibited onset overpotentials of 249 mV and 264 mV, respectively, lower than those of pristine NiFe-LDHs (282 mV). The results evidenced that the modification of electronic structure of the active sites by doping extra metal cations (Co²⁺ or Co³⁺) could successfully overcome the disadvantage of insufficient active sites of pristine NiFe-LDHs.

The vanadium (V) doping had also been recognized as an efficient strategy to improve the intrinsic OER activity of pristine NiFe-LDHs [133]. Li et al. [134] reported that V-doping could modify the electronic structure of Fe sites in NiFeV-LDHs, and the strong electronic interaction in NiFeV-LDHs resulted in an unprecedented OER activity, which only required an overpotential of 195 mV to achieve a current density of 20 mA cm⁻² and a Tafel slope of 42 mV dec⁻¹ (Figure 6A–D). Due to the different electronegativity between Fe and V, a charge compensation in NiFeV-LDHs was generated, leading to the oxidation of V³⁺ to V⁴⁺ and V⁵⁺, accompanied by the reduction of Fe³⁺. The DFT calculation results showed that V-doping into NiFe-LDHs decreased the free energy difference from *OH to *O, and thus resulted in a fast water oxidation reaction rate at the low overpotential. The total density of states (TDOS) spectrum further confirmed that V-doping could change the conduction band sate of LDHs, and narrow its bandgap to provide a more conductive electronic structure for OER catalysis, which was in agreement with the results of the decreased resistivity from (2.4 ± 0.3) × 10³ Ω sq⁻¹ to (1.3 ± 0.2) × 10³ Ω sq⁻¹ in (NiFe-LDHs), and (NiFeV-LDHs), respectively. On the other hand, a study carried by Jiang et al. [111] suggested that the V-doping with distorted geometric and disturbed electronic structures made a crucial contribution to high activity of the Ni/Fe/V trimetallic catalysts. The XANES and XPS results revealed that the partial electron transfer from Ni²⁺ to Fe³⁺ in NiFe-LDHs or V⁴⁺ and V⁵⁺ in NiV-LDHs, or Fe³⁺ in NiFeV-LDH took place from Ni²⁺ through the oxygen bridges (O²⁻) between metal cations via π-donation. After that, the electron-rich t_2g d-orbital of Fe³⁺ transferred electrons to the strongly electron-deficient t_2g d-orbitals of V⁴⁺ and V⁵⁺ through the bridging O²⁻ ions, which led to a better π-symmetry electron delocalization among Ni, Fe, and V cations in the host matrix, as shown in Figure 6E. The optimized Ni₃Fe_0.5V_0.5 catalyst exhibited an outstanding OER performance with a low overpotential of 200 mV at 10 mA cm⁻².

Moreover, the dopants could serve as new active sites in the resultant metal-doped LDHs, thus improving the reactivity of the active sites. Wang’s group [135] reported a highly active ORR electrocatalyst: Cr-doped CoFe-LDHs, which only demanded an overpotential of 238 mV to obtain a current density of 10 mA cm⁻² in 1 M KOH electrolyte. The experimental and theoretical simulation studies demonstrated that the engineered electronic modulation aroused from the Cr-doping effect in Cr-doped CoFe-LDHs, and the Cr dopants as new active sites donated more electrons to the reactants thanks to the smaller electronegativity of Cr in comparison with Fe and Co. Consequently, the larger charge transfers of Cr–O resulted in the larger binding energy relative to Co–O bonds, which assisted to break the scaling relation between ΔG_*OOH and ΔG_*OH and boosted the OER activity. A similar phenomenon was also observed for Cr³⁺-doped CoFe-LDHs with partial-oxidized Cr⁶⁺ cations [136]. By virtue of the strong electron-withdrawing ability for Cr⁶⁺ cations, the electronic structure of active sites was modified, forming new Co-active sites with high oxidation state for H₂O absorption in the OER process. Enhanced OER activity was achieved by partially oxidized Cr⁶⁺ in Cr³⁺-doped CoFe-LDHs with an overpotential of 202 mV at 10 mA cm⁻².

It is noteworthy that the doping of non-metallic atoms (i.e., Se, S, B, F, and P) is another efficient protocol to modify the electronic structure to boost the intrinsic conductivity of LDHs materials. For example, an active S-doped NiFe-LDH electrocatalyst was synthesized through a one-step hydrothermal process [137]. Herein, S introduced in trace amount in Ni_4/5Fe_1/5-LDHs played a vital role in boosting its catalytic activity towards OER. When the S doping amount was ~0.43 at%, the sample Ni_4/5Fe_1/5-LDHs-S-2 demonstrated the best OER activity in alkaline media, featuring an overpotential of 257 mV at 10 mA cm⁻² lower than that of Ni_4/5Fe_1/5-LDHs without S doping (325 mV). Such enhanced OER activity of S-doped NiFe-LDHs was the result of the synergistic effect between S and the Fe sites to reduce the energy barriers for the formation of the OER intermediates on Fe sites, and thus enhancing the OER activity. Inspired by amorphous boron-based catalysts, with a mass of percolation pathways and a fast-diffusion rate, amorphous boron-modified LDHs (B-Co₂Fe-LDHs) material decorated by numerous nanosheet-nanoflakes, was prepared [78]. The defective interfaces in the crystalline-amorphous phase boundaries allowed for enhanced electronic kinetics with an overpotential of 309 mV at 100 mA cm⁻² and high corrosion resistance of more than 100 h both in fresh and saltwater. This work provides a simple and scalable strategy to develop efficient and stable LDHs materials for highly selective seawater oxidation. Zhang et al. [138] fabricated a surface reconstructed NiFe-OH-F-SR catalyst derived from fluoride-incorporated NiFe hydroxide nanosheets (NiFe-OH-F) as an excellent OER catalyst. The OER activity of the NiFe-OH-F-SR electrode was increased by ~58 folds compared with the original NiFe-OH-F. This phenomenon could be attributed to: (i) the reconstructed amorphous surface layer, with defect-rich and the high defect concentration, played an important role in improving the conductivity of the NiFe-OH-F-SR; (ii) the increased surface area, desirable nanostructure, as well as enhanced charge-transfer ability helped to improve the electrocatalytic activity of NiFe-OH-F-SR; and (iii) the hierarchical framework with three levels of porosity of NiFe-OH-F-SR, was beneficial for exposing catalytic active sites and making them completely in contact with the electrolyte, promoting the electrochemical reaction.

Moreover, the intrinsic activity of LDHs can be fine-tuned by adjusting the molar ratio of the metal components. For example, Liu et al. [139] found that the molar ratio of Co/Fe greatly affected the OER electrocatalytic performance of CoFe-LDHs by controlling the ratio of CoO₆ octahedrons and CoO₄ tetrahedrons. With increasing Fe content, there were fewer CoO₄ tetrahedra when the ratio reached a certain degree (Co/Fe = 5:1), resulting in higher OER performance than the other with a Co/Fe ratio of 3:1. The appropriate Fe content could activate the inactive octahedral coordinated Co²⁺, giving rise to an enhanced reactivity. When the Fe content was further increased, there was a loss of catalytic activity of tetrahedrally coordinated Co²⁺. Moreover, a series of CoMo-LDHs with different Co/Mo weight ratios (1:4, 2:3, 3:2, and 4:1) were synthesized by Lee’s group [140]. Among these catalysts, the Co₃Mo₂-LDHs showed the highest OER activity due to the synergic effect between Co and Mo, and compositional merits with adequate number of active Co and Mo species.

3.2. Intercalation

The intercalation of LDHs, with a layer-by-layer structure, is a process of inserting a foreign species between the edge-shared metal hydroxide layers of the LDHs. The host-guest interaction in LDHs can be modulated by controlling the properties of interlayer guests, e.g., the radii, redox activity, acid and/or base. In many reported works, it has been proposed that the intercalation can lead to remarkably improved OER performance for LDHs materials.

An early study revealed that the divalent anions possessed higher ion selectivity than monovalent ones, and the ion-exchange equilibrium constants followed the sequence: CO₃²⁻ > SO₄²⁻ > OH⁻ > F⁻ > Cl⁻ > I⁻ [141]. Later, Müller’s group [142] further studied the effect of the anions (A^m−) with different valence states on water oxidation activity for NiFe-LDHs. Based on the Gaussian fits of the (003) peaks results, the calculated basal spacings of NiFe-A^m−-LDHs materials with different intercalated anions, were depicted in Figure 7A. It was worth noting that this analysis was limited to the spherical halogen anions. It obviously showed that there was a linear correlation of the calculated basal spacings with anionic radii. However, the measured overpotentials were not dependent on the basal spacings. On the other hand, they discovered that the water oxidation activity was strongly correlated with the pK_a of the conjugate acid of the interlayer anions, e.g., the larger pK_a value, the higher OER activity of the intercalated LDHs (Figure 7B). This result suggested that the anions’ Brønsted or Lewis basicity played a role in the water oxidation mechanism of transition metals-based LDHs. In the same context, Sun’s group correlated the intercalated phosphorus oxo-anions (e.g., phosphate, phosphite, and hypophosphite) and the OER performance of NiFe-LDHs [143]. They found that the intercalation of phosphorus oxo-anions dramatically enhanced the OER activity and durability over the carbonate-intercalated NiFe-LDHs in an alkaline solution. Specifically, the optimal performance (e.g., a low onset potential of 215 mV and a small Tafel slope of 37.7 mV dec⁻¹) was achieved by the hypophosphite-intercalated NiFe-LDHs, which was attributed to its stronger donor-electron ability than phosphate and phosphite. Later, Zhou and Sun [144] proposed a universal relationship between sixteen anions-intercalated NiFe-LDHs and their OER activity from a different viewpoint. The authors deemed that the OER performance was not completely relevant to the pK_a of the conjugate acid of the interlayer anions, but a linear relationship between the redox potential of the intercalated anions and the corresponding OER activity, as shown in Figure 7C. For example, the intercalated hypophosphite anions with a high reducing ability led to the formation of electron-rich metal sites, which could be easily oxidized to higher-valence states then acted as active sites in the OER process, providing a higher OER activity. DFT+U calculations and XPS analysis demonstrated the introduced anions modified the electronic structure of the exposed metal atoms, increasing the electron density of the laminate metal sites and stabilizing the high-valence states, which was beneficial to lower the activation energy and improve the OER performance.

The intercalated anions, with larger basal spacing, benefit the OER performance of the LDHs by providing more space for mass diffusion during the oxygen evolution. Xu and Hao [145] fabricated two intercalated NiFe-NO₃⁻-LDHs and NiFe-CO₃²⁻-LDHs catalysts and compared their OER activity differences. The NiFe-NO₃⁻-LDHs with an interlayer spacing of 7.69 Å displayed a higher OER activity than NiFe-CO₃²⁻-LDHs (interlayer spacing of 8.04 Å), as a result of more exposed active sites and a low charge transferring resistance. Zhong et al. [60] intercalated dodecyl sulfonate (DS⁻) into the interlayer spaces of NiFe-LDHs through a one-step hydrothermal method, which increased the basal spacing (Figure 7D) from 7.6 Å to 24.9 Å. As a result, the overpotential for OER to reach the current density of 10 mA cm⁻² reduced from 333 mV to 289 mV. Li et al. [146] developed an in situ intercalation method to prepare formamide intercalated NiFe-LDHs electrodes, and the corresponding interlayer spacing increased from 7.8 Å to 9.5 Å. More importantly, compared with ex situ intercalation/exfoliation approach, the in situ intercalation method largely maintained the good interfacial connection and long-term stability of LDHs materials, which provided an overpotential of 203 mV at 10 mA cm⁻² and a stability of up to 16 h. Komarneni et al. [147] intercalated several dicarboxylic acids of different alkyl chain lengths (suberic acid, adipic acid and succinic acid) into the interlayer spaces of NiFe-LDHs and studied the effect of basal spacing on the OER activity. It was discovered that suberic acid, intercalated in NiFe-LDH, exhibited a remarkable activity for OER in a pH-near-neutral K-B_i electrolyte (pH = 9.2), which was mainly ascribed to the “structural instability” induced “in situ” anion exchange” process in which borate anions entered the interlayer and activated inner Ni sites. This work further proved that the pillaring of NiFe-LDHs with large organic anions was a promising method to create LDH-type high-performance catalysts for the OER in a pH-near-neutral K-B_i electrolyte.

The intercalation of homogeneous species (i.e., inorganic anions, organic acid/base, and organic complexes) favors improving the electrocatalytic performance for LDHs in three different aspects: (i) the enlarged basal spacing with more exposed inner active sites can facilitate the electron/charge transfer and the mass diffusion to bring about a more favorable OER kinetics; (ii) the intercalation could induce structural changes, such as lattice expansion or phase change, providing novel physicochemical properties; and (iii) due to the different redox ability between the metal sites and intercalated anions, the intercalation significantly modulates the electronic structure of metal sites in the laminate, endowing them with optimal binding of reaction intermediates and enhanced chemical reactivity.

3.3. Vacancy Engineering

Recently, the vacancy engineering has emerged as an interesting strategy to improve the OER electrocatalytic performance of LDHs materials. Many studies manifested that the oxygen vacancies could decrease the absorption energies of OER intermediates, and the metal vacancies would lead to the formation of unsaturated-coordination metal centers which can serve as active sites and subsequently improve OER activity. What is more, the vacancy can also act as new active sites, narrowing the bandgap to increase the conductivity [148]. It is noteworthy that the different types of the vacancy (oxygen vacancies and metal vacancies) make different contribution to the OER performance of LDHs due to the different working mechanisms and functions. To be specific, the creation of metal vacancies leads to “positive holes”, to facilitate the adsorption of *O intermediates on the surface, which renders the conversion of *O to *OH energetically quite favorable and results in a small overpotential [149]. The oxygen vacancies can induce the bonding interaction between the exposed oxygen-coordination-deficient metal atoms/centers and *OH intermediates to promote the uptake and conversion of *OH [150].

There are various post-synthesis methodologies for introducing vacancies, such as thermal treatment [151], acidic/alkaline etching [152], ball mill [153], and laser ablation [154]. Especially, the aqueous chemical reduction by strong reducing agents (NaBH₄/N₂H₄) [155] or high-temperature (e.g., >600 °C) annealing under H₂ atmosphere [148] can selectively create the oxygen vacancies. Xiong et al. [155] introduced the oxygen vacancies into NiFe-LDH nanosheets by a simple immersion in NaBH₄ solution at room temperature (Figure 8A). The role of oxygen vacancies in NiFe-LDHs during the OER process was investigated by DFT+U calculations. Taking the bridge sites between Ni and Fe (Ni-O-Fe) as the active sites, the calculation results elucidated that the potential determining step (PDS) of pristine NiFe-LDHs was the deprotonation step with a high overpotential of 0.86 V, and after introducing oxygen vacancies, the potential determining step (PDS) of defective NiFe-LDHs tuned to be the *OOH formation step with a lower overpotential (0.65 V), showing a higher intrinsic activity. In another case, Zhou et al. [151] synthesized oxygen vacancies-rich NiFe-LDH nanosheets through a fast (30 s) and facile (operated at room temperature) flame-engraving method. In Figure 8B, the inner core of a burner flame was typically deficient in oxygen, yielding a reducing and high-temperature environment to rapidly create oxygen vacancies in NiFe-LDHs structure. After flame treatment, the thickness of NiFe-LDH nanosheets decreased from 4.5 to 3.5 nm, while many well-defined hexagonal cavities with (110) edges appeared. Abundant oxygen vacancies, lower coordination numbers, and electron-rich structures of Ni and Fe sites emerged in the flame-engraved NiFe-LDHs array electrode, leading to its onset potential as low as 1.40 V.

In addition to oxygen vacancies, introduction of metal vacancies via etching could selectively create M^II or M^III metal vacancies in LDH nanosheets. Xie et al. [156] reported a novel method of ionic reductive complexation extraction (IRCE) to etch the target Cu(II) ions and create atomically dispersed cation vacancies in SAV-NiCu_x-LDHs. In a typical procedure, based on the different equilibrium constant (K) of transition metal ions, SCN⁻ was used as the extractant because of the large log K of Cu(I)-SCN (12.11), which was more than six-folds higher than that of Cu(II)-SCN (1.9) and Ni(II)-SCN (1.18). To achieve selective extraction of Cu from NiCu-LDHs, Na₂SO₃ was added to in situ reduce the Cu(II) to Cu(I). The overpotential at 100 mA cm⁻² and Tafel slope of SAV-NiCu_x-LDHs were evaluated to be as low as 355 mV and 45 mV dec⁻¹. This work provides a promising direction for engineering atomically dispersed vacancies and alleviating the mechanical collapse of LDHs, greatly guaranteeing the superior OER activity of the electrocatalysts. Besides, the alkaline etching treatment in 1 M KOH solution, was also employed to manufacture Fe³⁺ (Ni²⁺) vacancies in NiFeAl-LDHs (NiZnFe-LDHs) to prepare NiFe-LDHs-V_Fe (NiFe-LDHs-V_Ni) electrocatalysts, respectively (Figure 8C) [49]. The NiFe-LDHs-V_Fe and NiFe-LDH-V_Ni nanosheets exhibited faster OER kinetics and smaller charge transfer resistance compared with NiFe-LDHs, which could be ascribed to the following reasons: (i) the edge and corner sites with numerous coordinated unsaturated sites helped to enhance the catalytic activity of defective LDHs; (ii) the redistributed electronic structure of reactive sites surrounding Fe or Ni vacancies led to form more Ni³⁺ with an optimal orbital distribution of $t_{2\mathrm{g}}^6{e}_{\mathrm{g}}^1$ (the e_g orbital occupancy of surface metal ion is 1, being regarded as the optimal electronic configuration for OER) [157], facilitating the adsorption of OER intermediates; and (iii) the defective states that appeared in the conduction and valence bands could hybridize with 2p states of *O resulted in a strong *O adsorption, which essentially enhanced the OER activity.

Both of the oxygen and cation vacancies engineering in one NiFe-LDHs system was reported by Zhang et al. [158], through a fast, one-step synthetic strategy in the presence of formamide. The defective-LDHs showed excellent OER performance with a low overpotential of 230 mV at 10 mA cm⁻², and a Tafel slope of 47 mV dec⁻¹. The synergistic effect between the oxygen vacancies and metal vacancies increased the electro-positivity of the LDH nanosheets, and thus facilitated the adsorption of H₂O and increased the *OH bonding energy. In the same context, Zhou et al. [159] prepared multiple vacancy-rich (Co, Fe, and O vacancies) CoFe-LDHs nanosheets, via an HNO₃-etched reaction (labeled E-CoFe-LDHs). Since the solubility of Co (OH)₂ was greater than Fe(OH)₃, the former was more active to react with HNO₃, leaving more Co vacancies in LDHs. Benefiting from modified electronic structure and more active sites, the E-CoFe-LDHs showed better OER performance than the pristine LDHs.

In summary, vacancies can offer the following advantages to electrocatalysts: (i) it can build atomic defects and influence the chemical environment on the catalyst surface; (ii) it can form a porous structure, increase specific surface area, and expose more edge sites and active sites to expend the electrochemical area; and (iii) it can also reduce the electron transfer resistance and speed up the mass transfer to accelerate the reaction kinetics. Consequently, etching layered double hydroxides is an alternative strategy to get highly efficient catalysts.

3.4. Ultrathin Nanosheets

The exposure and accessibility of active sites and the surface adsorption capability of the reactants are strongly associated with the morphology of the catalysts, which plays a crucial role in the electrocatalytic performance. Usually, the pristine LDHs with several self-stacking layers display inferior electrocatalytic activity. In contrast, ultrathin LDHs nanosheets with single-or few-atoms thickness and large lateral size show excellent electrocatalytic performance due to their ultrahigh specific surface area and highly intrinsic activity of active sites [160]. The layer modification/engineering methods generally include the “top-down” exfoliation and the “bottom-up” direct synthesis. The former is in virtue of strongly physical shear force or chemical intercalation to break interlayers bonding forces, and then exfoliate the bulk into single or few-layered nanosheets, while the latter tends to directly prepare ultrathin 2D LDHs nanosheets based on the chemical reaction.

The chemical exfoliation is recognized as a “top-down” route, through which ultrathin LDHs nanosheets were prepared. The chemical exfoliation usually involves multi-chemical processes, including anion-exchange, osmotic swelling, and exfoliation [161]. Typically, the anion-exchange initializes the process by enlarging the interlayer spacing and weakening the interaction between host layers, which is conducive to the following osmotic swelling. The swelling is triggered by intercalating organo-ammonium anions into the interlayer region, and the corresponding degree can be adjusted by the balance of osmotic pressure between the interlayer region and the solvent. The pristine LDHs can be exfoliated into unilamellar nanosheets with a molecular-level thickness of about 1 nm versus 2D lateral size in submicrometer or micrometer scale.

The liquid exfoliation of LDHs nanosheets in the presence of various anionic surfactants has motivated a strong interest since Adachi-Pagano et al. [162] reported, in 2000, the successful delamination of layered double hydroxide structure [Zn₂Al(OH)₆][C₁₂H₂₅SO₄•nH₂O] in butanol solution. The authors pointed out that the van der Waals interlayer interactions were introduced by the intercalation of dodecyl sulfate anions in Zn₂Al(OH)₆Cl•2H₂O, which weakened the stacking of the layers and favored interactions with butanol solvent. Later in 2014, inspired by the topochemical transformation, Song and Hu [160] conducted a pioneering study to prepare NiFe-LDHs, NiCo-LDHs, and CoCo-LDHs with single-layer nanosheets via an anion-exchange process and a formamide-exfoliation process. After anion exchange, the increased inter-layer distance allowed the delamination of the bulk LDHs to monolayer nanosheets in the purged formamide. In Figure 9A, the exfoliated LDHs nanosheets showed remarkably enhanced OER activity with a decrease (40~54 mV) of the overpotential at the current density of 10 mA cm⁻² compared with its original bulk one. They suggested that the higher intrinsic activity of exfoliated nanosheets was mainly due to the increased active site density, rather than the higher electrochemically active surface area (ECSA). Additionally, the edges in the exfoliated nanosheets, with open coordination sites, could serve as active sites for water oxidation. Zhang’s group [163] synthesized ultrathin and ultrafine monolayer ZnCo-LDHs with abundant oxygen vacancies and unsaturated coordination edge-sites through a simple ultrasonic exfoliation procedure in formamide. On the one hand, the ultrathin and ultrafine nanostructure provided numerous accessible and coordinately unsaturated active sites for H₂O adsorption. On the other hand, the ultrafine monolayer nanosheets offered short diffusion paths for charge transfer to the current collector. As a result, the monolayer ZnCo-LDHs exhibited an enhanced OER activity with an overpotential of 340 mV at 5 mA cm⁻¹, which was smaller than that of the bulk counterpart (530 mV) in 1 M KOH electrolyte.

Nevertheless, the liquid-phase exfoliation is typically time-consuming and expensive, and the exfoliating solvent molecules, e.g., formamide and surfactants, are easily adsorbed on the exfoliated nanosheets, thus blocking the exposed active sites and reducing the catalytic activity. Recently, Yong et al. [164] reported a novel Ostwald ripening driven exfoliation (ORDE) of NiFe-LDHs on Cu mesh without the assistance of any exfoliating reagent or surfactant, which efficiently realized the in situ exfoliation of LDHs bulk into stable ultrathin nanosheets with significantly improved OER performance (Figure 9C). In the thermodynamic process, the tiny stacked layers on each bulk LDH surface tended to dissolve in solution and redeposited on the edge sites of relatively large layers to reach a more stable equilibrium state with lower overall energy, resulting in the larger lateral dimension (X and Y directions) and thinner thickness of each bulk bundle, and creating abundant active edge-sites at the same time. This ultrathin NiFe-LDHs/Cu with increased surface area exhibited a competitive OER activity with an overpotential of 292 mV at 10 mA cm⁻², and a superior stability for 60 h at the fixed current density. The plasma etching is also a highly efficient strategy for exfoliation of LDHs into stable and clean ultrathin nanosheets. Compared with liquid-phase exfoliation, plasma-induced exfoliation process only involved solid powders and plasma, which avoids the adsorption of solvent molecules and prevents the re-stacking of LDHs nanosheets. For example, Wang et al. [165] exfoliated bulk CoFe-LDHs into ultrathin LDH nanosheets by Ar plasma etching, which also caused the formation of multiple vacancies (V_Co, V_Fe, and V_O), cf. Figure 9B. The XRD spectra and atomic force microscopy (AFM) images confirmed the successful exfoliation of the LDHs into monolayer nanosheets because of the disappearance of the (003) and (006) diffraction peaks and the decreased layer thickness from 20.6 nm to 0.6 nm. The multiple vacancies effectively modulated the surface electronic structure and decreased the coordination numbers of catalytic sites, which in turn improved the intrinsic activity of ultrathin LDH nanosheets. Upon exfoliation, the ultrathin CoFe-LDHs-Ar catalyst only acquired a small overpotential of 266 mV to reach the current density of 10 mA cm⁻² in 1 M KOH, whereas it was 321 mV for bulk CoFe-LDHs. With the same strategy, Liu et al. [166] applied the CHF₃-plasma etching technique to exfoliate the Co₃Fe-LDHs and obtain F-doped Co₃Fe-LDH ultrathin nanosheets. Interestingly, during the CHF₃-plasma treatment process, F⁻ ions selectively filled oxygen vacancies, and tuning the electronic structure with a high electronegativity. The previous literature reported that the F-doping can enhance the electronic conductivity of electrocatalysts, and then facilitate the electron transfer and the formation of active sites to decrease the Gibbs reaction energy barrier [167]. As expected, the OER activity of CoFe-LDHs supported on Ni foam was optimized, which only needed a small overpotential of 276 mV to reach 10 mA cm⁻².

The “bottom-up” chemical methods including microemulsion method and layer growth inhibitors, can realize the direct synthesis of ultrathin 2D LDHs nanostructures by creating a “microreactor” environment or inhibiting the growth of the layers by a layer growth inhibitor (e.g., formamide, acetylacetone, and ethylene glycol) [168,169]. For example, Gao et al. [168] constructed a series of ultrathin atomic-thick LDH nanosheets through a facile and rapid precipitation method with both formamide and water as solvents (Figure 10A). The AFM image manifested that the individual nanosheet had an average thickness of ca. 1.3 nm and width of 40 nm. The height was very close to the single-unit-cell spacing in the (00l) direction (~0.8 nm) for CO³⁻/LDHs, confirming the successful synthesis of ultrathin single-unit-cell LDHs nanosheets. The overpotential at 10 mA cm⁻² of the ultrathin LDH NSs was 72 mV lower than the bulk counterpart, which mainly originated from the increase in active site density and C_dl values in the ultrathin single-unit-cell-thick LDHs (Figure 10B). Very recently, Zhao et al. [170] synthesized sub-3 nm monolayer LDHs (LDH-UF), namely, the lateral size less than 3 nm, by means of the pulsed ultrasonication of monolayer LDHs nanosheet precursors in formamide, cf. Figure 10C. EXAFS studies and DFT calculations revealed that the sub-3 nm monolayer LDHs possessed a higher concentration of metal and oxygen vacancies compared with the monolayer NiFe-LDHs precursor or bulk NiFe-LDHs, which gave the former semi-metallic character. The high conductivity of LDH-UF, along with an abundance of exposed surface sites (especially sheet edges), all contributed to the ultrafine nanosheets displaying enhanced performance for electrocatalytic water oxidation relative to monolayer LDH nanosheets. (Figure 10D). Kuai and Du [171] developed an alcohol intercalation method to prepare ultrathin NiFe-LDHs with a 1/3 unit-cell thickness. Operando synchrotron X-ray analysis indicated that the metallic ions in ultrathin Ni-Fe LDHs were fully oxidized into tetravalence states at low applied potentials and that the OER occurred on the tetravalent Ni and Fe ions following a decoupled proton/electron mechanism. Furthermore, it was found that a full oxidization of metal ions played a vital role in highly active NiFe LDHs and that it can be accomplished by engineering ultrathin nanostructures.

3.5. Nanostructuring

The controllable synthesis of the electrocatalysts with well-defined nanostructure, morphology, size, and crystallinity provides solid foundation for the development of LDHs. Among many nanostructures, the hierarchical porous structures received particular attention due to their better electrolyte permeability, shorten mass and electron transport paths. There are several common strategies to prepare the porous electrocatalysts as follows: (i) in situ growing on a porous substrate (carbon paper, carbon cloth, Ni foam, etc.); (ii) external-template methods: the hard templates including SiO₂, MgO, and Al₂O₃, which need to be removed using etching agents such as HF and NaOH; the soft templates usually used in the preparation of organic compounds are not eco-friendly; and (iii) self-template methods utilizing a porous precursor, e.g., metal organic frameworks (MOFs). For instance, Zhong et al. [172] fabricated a series of 3D flower-like NiFe-LDH hollow microspheres (3D NiFe-LDHs HMS) by adjusting the concentration of NH₄F and reaction time during the hydrothermal treatment. This fluoride-mediated self-transformation process or Ostwald ripening for the preparation of hollow microspheres, was beneficial for the exposure of more inner-active sites and improvement of the hydrophilicity, which can reduce the ions-transport resistance and thus enhance the OER dynamics. The optimized NiFe-LDH-0.4M HMS showed an excellent OER performance with η = 290 mV@10 mA cm⁻² and a Tafel slope of 51 mV dec⁻¹ in 1 M KOH solution. A similar phenomenon was also observed for NiFe-LDHs hollow microspheres (HMS) with a shell thickness of 50 nm synthesized by [173] in situ grew NiFe-LDHs on the SiO₂ surface as a self-sacrificial template, which was subsequently etched, as displayed in Figure 11A. The NiFe-LDHs HMS showed highly efficient OER electrocatalytic activity with a preferable current density (71.69 mA cm⁻² at η = 300 mV) and a small onset overpotential (239 mV at 10 mA cm⁻²), which outperformed the 20 wt.% commercial Ir/C catalyst. Moreover, it exhibited a low Tafel slope (53 mV dec⁻¹) as well as a desirable long-time stability. Such outstanding OER performance was ascribed to its high specific surface area, flourishing pore structure, and excellent hydrophilicity, which facilitated a full exposure of active sites and facile ion transport kinetics. Similarly, Lou’s group prepared hierarchical NiFe-LDHs hollow nanoprisms via a facile self-templated strategy by using nickel tetragonal nanoprism precursors as the self-sacrificial template [174]. It was found that, the NiFe-LDHs hollow nanoprisms had a higher OER activity, larger double-layer capacitance (C_dl), and more stable than the NiFe-LDHs nanocluster, suggesting that the open and porous structure was responsible for the enhanced OER performance.

Metal organic frameworks (MOFs), a self-assembly porous material, links organic and inorganic moieties through covalent coordination linkages, possessing tunable structures and versatile functionalities that render catalytic materials with large surface areas and pore sizes. As an example, Xu et al. [175] prepared a uniform and hollow 3D NiFeCe-LDHs microcapsule electrocatalyst by a facile one-step solvothermal reaction with the help of Ce-doping. As shown in Figure 11B, in the early stage, the formed MIL-88A templates became more stable after coordinating with Ce³⁺ ions; as the reaction progressed, urea gradually released more OH⁻ ions, which prompted the dissolution of the inner core and the precipitation of Fe³⁺, Ni²⁺ and extra Ce³⁺ to construct a hierarchical shell with vertical and interconnected NiFeCe-LDHs nanosheets on the surface of MOF precursors. By precisely controlling the concentration of Ce³⁺ ion, well-defined hierarchical hollow NiFeCe-LDHs microcapsules with a high specific surface area of 286.33 m² g⁻¹ were obtained. The NiFeCe-LDHs microcapsules displayed a superior OER performance with a low overpotential of 242 mV at 10 mA cm⁻² and good stability over 24 h. Zhu et al. [176] prepared the hollow Rh-doped CoFe-LDHs derived from the zeolitic imidazolate framework-67 (ZIF-67) nanotriangles by an efficient simultaneous etching-doping sedimentation equilibrium (EDSE) strategy. During the EDSE process, urea dissolved in aqueous solution and converted to ammonium cyanate, and the latter rapidly hydrolyzed to produce NH₄⁺ and CO₃²⁻. Then, the ammonium decomposed and formed an alkaline environment when temperature rose above 60 °C. The outer ZIF-67 nano-triangles were gradually etched, while the generated Co²⁺ coprecipitated with the metal cations and form more stable CoFe-LDHs nanosheets, along with the simultaneous doping of Ru. The double-layer capacitance results demonstrated that the hollow Rh-doped CoFe-LDHs catalyst exhibited higher active area and more active sites than solid LDHs, which originated from the typical hollow hierarchical structure.

3.6. Hybridization

The combination of two or more distinct properties into an integrated composite is a fascinating direction to develop multi-functional materials. Construction of LDH-based hybrids, especially one with a nanostructure, by interacting LDHs with other materials (e.g., carbon materials, metal/metal oxides, and 3D conductive substrate), has attracted extensive attention in the field of energy conversion and storage.

Coupling catalysts with conductive carbonaceous materials, e.g., graphene, carbon black, carbon nanotubes (CNTs), graphene quantum dots (GQDs) and carbon fiber papers (CFPs), is an extremely effective and reliable approach to promote their electrocatalytic performance by exposing more active sites and facilitating electron transfer [177]. Dai et al. [116] synthesized a novel hybrid of NiFe-LDHs/CNTs, in which mildly oxidized multiwalled CNTs served as the support; the electrostatic force between negatively charged functional groups on the CNTs can adsorb positively charged metal cation precursors. The NiFe-LDHs/CNTs exhibited outstanding OER performance due to more exposed active sites and the faster electron transfer. In a similar process, Guo et al. [178] hybridized Ni-based LDHs (NiM-LDHs, M=Fe, Co, Mn) and GQDs with the help of electrostatic-adsorption effect, and successfully fabricated a series of LDHs/GQDs hybrids, cf. Figure 12A. Due to the electron absorption/donation effects, electrons transferred from LDHs to GQDs, leading to the of new Ni³⁺ species, which were favorable for enhancing the electrocatalytic activity of OER (Figure 12B). Interestingly, they found, compared with NiMn-LDHs/GQDs, that NiFe-LDHs/GQDs and NiCo-LDH/GQDs with higher activity had a higher shift degree in Ni 2p_3/2 binding energy, further attesting that Ni with high oxidation states has a positive effect on the OER activity. The NiFe-LDHs/GDQs with a strong interfacial electronic coupling exhibited a conspicuous catalytic performance with an overpotential of only 189 mV at 10 mA cm⁻². Further, Li et al. [179] reported an enhanced OER performance of superhydrophilic CoAl layered double hydroxides/graphdiyne (CoAl-LDHs/GDY) hybrid. They suggested that superhydrophilic GDY had strong interaction with CoAl-LDHs catalysts and attracted H₂O molecules around the catalysts’ sites, thus facilitating interfacial mass/electron transportation. By comparison, a lower overpotential of ~258 mV to reach 10 mA cm⁻² and higher turnover frequency (TOF) of ~0.60 s⁻¹ at η = 300 mV were observed on CoAl-LDHs/GDY than that of pure CoAl-LDHs.

Metal-based materials (i.e., metal single atom, metal compounds, and 3D metal scaffolds) have been recognized as a sort of robust candidates for the enhanced electrocatalytic performance of LDHs due to their good conductivity, abundant active sites and large surface area. In particular, the integration of LDHs and 3D conductive substrates not only provides a conductive framework with numerous internal electron transport channels, but also can prevent the aggregation of catalysts and increase the effective ECSA for electrocatalytic process. For example, Zhang et al. [180] reported that single-atom Au supported on NiFe-LDHs (^sAu/NiFe-LDHs) showed a 6-fold enhancement of OER performance by 0.4 wt.% ^sAu decoration. Such behavior was ascribed to the charge redistribution of active Fe atoms in NiFe oxyhydroxide supported by LDHs and stabilized by interlayer CO₃²⁻ anions and H₂O molecules, resulting from the electron-donation effect of Au atoms. Generally, the core–shell nanostructure is well-known for a better stability, for being able to protect the core material from the surrounding environment. The properties of the “core” and “shell”, and their synergistic effect, play an important role in the functions of core–shell catalysts [97]. Therefore, the construction of core–shell nanostructure has become an intriguing avenue to functionalize LDHs for OER catalysis. For instance, self-standing Cu@NiFe-LDHs/CuF (CuF stands for Cu foams) with a core–shell nanostructure: NiFe-LDHs were the “shells” and Cu nanowires were the “cores”, are shown in Figure 13A [181]. Clearly, this 3D core–shell nanostructures can provide large surface areas with increased exposure of active sites, efficient electron transport from the inner Cu NWs to the surrounding NiFe-LDHs, and a fast release of gaseous products. Additionally, the core–shell Cu@NiFe-LDHs/CuF had a good mechanical structure since the Cu NWs were directly grown on the Cu foam, and the Cu NWs firmly grasped the shell of NiFe-LDHs NSs, ensuring a good electronic transport. Summing up, the Cu@NiFe-LDHs/CuF catalyst displayed a high OER activity with an overpotential of 199 mV at 10 mA cm⁻², and good stability of more than 48 h at fixed current densities of 10 and 100 mA cm⁻² in 1 M KOH solution. A similar phenomenon was also observed for NiCo₂O₄@FeNi-LDHs electrode [182]. It was found that, the core NiCo₂O₄ nanocones acted as scaffolds to offer more reactive sites and accelerate charge transfer to the shell FeNi-LDHs. Enhanced OER activity was achieved by hybridizing the conductive NiCo₂O₄ building blocks with active FeNi-LDHs into a compact structure. The authors further suggested that the electrocatalytic performance of NiCo₂O₄@FeNi-LDHs was governed by a synergy between electronic effects (core–shell) and morphological effects.

To break the scaling relationship, namely, the adsorption energies of OER intermediates, a NiO/NiFe LDHs hybrid was prepared through laser ablation of urea solution and subsequent electrochemical oxidation [184]. The synchrotron radiation soft X-ray absorption spectroscopy (sXAS) analysis and spin-polarized DFT+U calculations verified that Ni⁴⁺ at the NiO/NiFe LDHs intersection was an active site for OER, and one or two additional chemical bonds assisted it to adsorb intermediates, forming the dynamic tridimensional adsorption. In particular, the configuration of tridimensional adsorption varied with the type of intermediate, hence, the linear correlation among the adsorption energies of intermediates was broken. As a result, the scaling relationship was successfully circumvented by the NiO/NiFe LDHs composite. Liu et al. [185] constructed a NiCo₂S₄@NiFe-LDHs heterostructure by directly growing NiFe-LDHs nanosheets on NiCo₂S₄/NF precursors. This NiCo₂S₄@NiFe-LDHs/NF catalyst exhibited the improved OER performance with a low overpotential of 201 mV at the current density of 60 mA cm⁻² and low Tafel slope of 46.3 mV dec⁻¹ due to the strong interaction and electron transfer. Qiu et al. [186] synthesized hierarchically porous and hydrophilic 3D NiFe-LDHs/MXene composites through electrodeposition. Due to the strong interfacial coupling, rapid charge transfer at the interface, and high hydrophilicity of Mxene, the complex showed improved electrical conductivity and fast OER process compared to the individual part, which only required a low overpotential of 300 mV to reach 500 mA cm⁻².

As is well-known, the formation of semiconductor junction can reach a state of thermal equilibrium and, especially, constitute two regions with opposite charged, and strong built-in fields at the interface can change the electron densities of the atoms around the interfaces. The NiFe-LDHs, is a typical n-type semiconductor. Once it is in contact with a p-type semiconductor forming a p-n junction, energy levels of E_F of n- and p-type semiconductors shift until the two are aligned in a thermal equilibrium state. Inspired by this view, He et al. [183] constructed a 3D free-standing NiFe-LDHs/CoP/carbon cloth (CC) with three-level hierarchical p-n junction structure. The 3D NiFe-LDHs/CoP/CC electrode only required an overpotential of 231.1 mV to deliver the current density of 20 mA cm⁻² in 1 M KOH solution. Notably, the current density at 1.485 V of NiFe-LDHs/CoP/CC achieved ~10-fold and ~100-fold increase compared to those of n-type NiFe-LDHs/CC and p-type CoP/CC, respectively, in Figure 13B. The energy-level diagrams illustrated that in the intimate- contact interface, the electrons flowed from p-type CoP to n-type NiFe-LDHs until the E_F of CoP and NiFe-LDHs turned to be aligned, which lead to opposite space-charge region at the p-n junction interface and further resulted in energy level shifting and band edge bending. As a result, positively charged active centers at the surface of NiFe-LDHs can effectively adsorb the OH⁻ ions, while the electrons of OH⁻ transferred to the valence band (VB) of NiFe-LDHs, and then recombined with the holes at the VB of NiFe-LDHs. The redundant electrons at the conduction band (CB) of NiFe-LDHs further recombined with the holes at VB of CoP to keep the charge balance. The above representative LDHs electrocatalysts for the OER process, modulated by various strategies, are summarized in Table 1.

4. Applications of LDHs-Based Bifunctional Electrocatalysts

Bifunctional electrocatalysts with both brilliant ORR and OER, or HER and OER performance are essential for energy conversion and storage devices, such as rechargeable zinc-air batteries (ZABs), unitized regenerative fuel cells (URFCs), electrolyzers, and so on. In such closed-loop systems, the essential component is the desired bifunctional oxygen electrode catalysts with high catalytic activity, long-term durability, and strongly resistance to anodic corrosion. Although the LDHs show a promising OER activity, the intrinsically poor electrical conductivity, and easily degradable active sites due to stacking of the material greatly prevent them from serving as bifunctional ORR/OER catalysts. It is fascinating to design and build a bifunctional oxygen electrode catalyst based on the combination of highly OER-active LDHs and highly ORR-active materials like conductive metals, carbon materials, and M-N-C compounds.

The hierarchical structure design and novel material chemistry endow high activity propelling O₂ redox. Inspired by the excellent electrical conductivity of Ag, Hwang’s group [215] developed a hierarchical 3D core–shell architecture, where the shell NiMn-LDHs nanosheets, was grown on the Ag nanowires (NWs) core, labeled as Ag NWs@NiMn-LDHs. This latter exhibited a preeminent bifunctional activity with onset potentials of 0.19 V and 0.27 V for OER and ORR, respectively. Furthermore, the Ag NWs@NiMn-LDHs had an outstanding overvoltage difference (ΔE) of 0.75 V between the OER overpotential at the current density of 10 mA cm⁻² and the ORR half-wave overpotential at the current density of −3 mA cm⁻². Analogously, Ag nanoparticles decorated NiRu-LDHs nanosheets (Ag NPs/NiRu-LDHs) were reported as bifunctional catalysts (Figure 14A) [216]. The Ag NPs/NiRu-LDHs revealed significantly higher ORR/OER bifunctional activity than pristine NiRu-LDHs in alkaline conditions, cf. Figure 14B. They inferred that the enhanced ORR activity of Ag NPs/NiRu-LDHs was mainly attributed to the increased Ag sites and accessible Ag site populations; the increase in the OER activity was due to intrinsically active Ni sites with multiple vacancies (oxygen vacancy, V_O and metal vacancies, V_M) after decoration strategy. The extraordinary low overpotential for ORR/OER was ascribed to the synergetic effects between Ag NPs and NiRu-LDHs.

Wang et al. [217] designed a hierarchical structure constructed a MnO₂-NiFe Janus electrode by selectively electrodepositing MnO₂ and NiFe-LDH on two sides of a porous nickel foam (MnO₂-NiFe/NF), in which the MnO₂ nanoflakes and NiFe-LDHs nanosheets served as the ORR and OER active centers, respectively (Figure 14C). Such a Janus MnO₂-NiFe air electrode endowed the zinc–air battery with better cycling stability and energy efficiency than the bare MnO₂ and NiFe-LDHs electrodes, as illustrated in Figure 14D. In another interesting example, a bifunctional electrocatalyst: Fe₃O₄/Au/CoFe-LDH with sandwich structured, was used for the hydrogen evolution reaction and the electrocatalytic glucose oxidation reaction (GOR) [219]. The combination of structural characterizations with electrochemical characterizations revealed that Fe₃O₄ and CoFe-LDHs played key roles in catalyzing the HER, whereas metallic Au was responsible for the GOR, Figure 14E. In a self-assembled asymmetrical electrolyzer-cell, in which the two-electrode electrolysis test was carried out using an AA battery (1.5 V rated voltage), the current density could achieve 20.9 mA cm⁻², cf. Figure 14F. During the test, bubbles were only observed on the cathode, while the solution in the anode compartment gradually turned yellow, indicating the formation of gluconate. These results manifested that this bifunctional electrocatalyst, built in a two-electrode cell system, achieved the replacement for OER with organic molecules oxidation reaction.

Nitrogen-doped graphene oxides (N-doped GO), as one of conductive carbon materials, with numerous functional oxygen groups (–OH⁻, –CO, –COO⁻) and defects, not only can provide catalysts with good hydrophilicity, but also provide ideal sites for metal sites to anchor by electrostatic force. Hence, the combination of ORR-active N-doped GO and LDHs materials have also been considered as an effective method for designing highly bifunctional electrocatalysts towards ORR and OER [218,221,222,223,224,225,226]. For example, a ternary NiCo^IIIFe-LDHs electrode with Co³⁺ grafted on nitrogen-doped graphene oxide (N-GO) was fabricated by an in situ growth route, and used as a bifunctional catalyst for ORR and OER (Figure 14G,H) [218]. The NiCo^IIIFe-LDHs/N-GO had a low overvoltage difference of 0.77 V between ORR and OER, which can be attributed to the following key factors: (i) the high valence state Co, i.e., Co³⁺, possessed a positive effect on the electrocatalytic performance of ORR and OER; (ii) the pyridinic-N and graphitic-N in N-GO could alter the electron density of carbon atoms so as to facilitate the adsorption of O₂ and break of O–O bonds in the ORR process; (iii) the enlarged surface area (SA) led to a highly exposure of Ni and Fe active sites; and (iv) the intimate contact between N-GO and LDHs brought out a high conductivity. Hou’s group [224] prepared NiFe-LDHs supported in reduced graphene oxides (NiFe-LDHs/rGO) nanohybrid as an efficient bifunctional electrocatalyst towards ORR and OER in alkaline medium. The NiFe-LDHs/rGO nanohybrid exhibited a better bifunctional performance than NiFe-LDHs and NiFe-LDH/GO counterparts, which can be credited to the fast electron/charge transfer and the synergistic effect of NiFe-LDHs and rGO in NiFe-LDHs/rGO system.

Recently, the zeolitic imidazolate frameworks (ZIFs), a subclass of metal-organic frameworks, consisted of metal cations (e.g., Zn²⁺, Co²⁺, etc.) and N-containing organic linkers (e.g., 2-methyl imidazole), are used as a precursor to controllably synthesize metal, N-codoped carbon nanoframes (metal, N-CNFs), which possesses a high surface area, excellent conductivity, and metal, N-codoped active sites. In addition, the metal, N-CNFs show excellent electrocatalytic performance for ORR [227,228,229]. Consequently, combining LDHs with metal, N-CNFs becomes an up-to-date strategy for the development of efficient bifunctional catalysts. Zhang et al. [220] reported a NiFe-LDHs/Co,N-CNF hybrid electrocatalyst, in which NiFe-LDH nanoparticles with the particle sizes of 3–5 nm were anchored on the Co,N-co-doped carbon supports. The high conductivity and homogeneously distribution of N-doped defects for Co,N-CNF support endowed the NiFe-LDHs/Co,N-CNF with an excellent bifunctional activity, demonstrating an OER overpotential of 0.31 V at 10 mA cm⁻² and an ORR half-wave potential of 0.79 V. Moreover, the self-assembly rechargeable zinc-air battery with NiFe-LDHs/Co,N-CNF electrocatalyst delivered a narrow discharge-charge voltage gap (1.0 V at 25 mA cm⁻²) over 80 h operation, which outperformed the rechargeable zinc-air batteries constructed using Co, N-CNF, NiFe-LDHs, and Pt/C + IrO₂ catalysts, respectively, cf. Figure 14I,J.

In order to alleviate the competition of the active sites for occupying the efficient positions, it is necessary to rationally design and arrange the active sites on the specific positions and ensure fully exposure to the dual-pathway of electron conduction and ion transportation in the multiphase electrocatalysis. As an example, Zhang et al. [230] proposed a multi-scale construction strategy to rationally integrate various active sites into a composite electrocatalyst (LDH-POF) to achieve superb bifunctional electrocatalytic performances for long-lifespan rechargeable zinc–air batteries. Here, the carbon nanotubes (CNTs) were employed as the scaffolds to anchor the active sites thanks to their high conductivity to construct electron conduction path-ways and the wearability to form porous structures to strengthen ion transportation. Second, cobalt coordinated porphyrin and NiFe-LDHs were selected as ORR and OER active sites, respectively. In Figure 15A–C, the resulting LDH-POF composite exhibited remarkable bifunctional performances with a small voltage gap of 0.68 V and enabled the rechargeable zinc-air batteries with a low discharge/charge voltage gap, a power density of 185.0 mW cm⁻², and an ultralong lifespan of more than 2400 cycles at the current density of 5.0 mA cm⁻². Later, this group further fabricated CoNC@LDHs composite for both ORR and OER through a two-step synthesis route. Specifically, the cobalt coordinated framework porphyrin was in situ coaxially coated on the CNT network surface to introduce atomic-level Co-N-C ORR sites, followed by the coprecipitation of hydrophilic NiFe-LDHs nano particles as OER active sites (Figure 15D) [231]. Owing to the increased hydrophilicity and strengthened ion/electron pathway, the CoNC@LDHs composite electrocatalyst delivered a ΔE of 0.63 V, significantly outperforming the noble-metal-based electrocatalyst (ΔE = 0.77 V), cf. Figure 15E. Additionally, the constructed rechargeable zinc-air battery achieved a power density of 173 mW cm⁻², and an ultralong lifespan (over 3600 cycles @10 mA cm⁻²) with a stable charge/discharge voltage difference of 0.76 V. It also exhibited excellent cycling current density (100 mA cm⁻²), surpassing that of the noble-metal catalysts (Figure 15F). This work highlights the integration of hydrophilic and conductive synergy in the search of efficient, durable, and bifunctional catalysts for ORR and OER processes. Yang et al. [232] developed a novel CoFe-LDHs coupled with NiFe-LDHs nanosheet array supported on nickel foam (denoted as CoFe@NiFe/NF) through a facile hydrothermal and electrodeposition method. Benefiting from strong synergistic effect between CoFe-LDHs and NiFe-LDHs and the 3D interconnected architectures, the resulting CoFe@NiFe/NF catalyst exhibited excellent activities and stabilities for both OER and HER. Furthermore, an efficient and stable alkali-electrolyzer using CoFe@NiFe/NF, as cathode and anode, achieved a voltage of 1.59 V at the current density of 10 mA cm⁻².

Apart from the combination of LDHs with other ORR-active nanomaterials, a variety of LDHs-derived catalysts are also employed as bifunctional electrocatalysts to catalyze oxygen electrode reactions (ORR/OER). Compared with traditional transition- metals catalysts, multifunctional catalysts derived from LDHs precursors via the topological structure transformation, show unique nano-size effect, high dispersion, and synergistic interaction, which are conducive to the improvement of electrocatalytic performances. The abundant interfaces are obtained simultaneously that may be beneficial for the electrocatalysis. Moreover, the in situ preparation of heterogeneous catalysts from LDHs is considered to be more chemically stable in comparison with the LDHs. The LDHs’ derivatives are usually prepared by a simple heat-treatment, viz. confinement synthesis strategy based on transformation. Zhong and Feng [233] fabricated a CoN_y/NiFeO_x/C electrocatalyst by annealing the phthalocyanine cobalt tetrasulfonate (CoPcTs) intercalated Ni₂Fe-LDHs precursor under N₂ atmosphere. The key aspects of this bifunctional electrocatalyst, for the reversible oxygen electrodes, was the mutual incorporation of the ORR-active sites (CoN_y), and OER-active ones (spinel NiFeO_x), respectively, derived from the interlayer CoPcTs²⁻ anions and the nickel-iron host sheet in the same LDHs system. The CoN_y/NiFeO_x/C composite afforded an excellent bifunctional activity with a ΔE of 0.84 V in alkaline media, and a remarkable stability in alternating modes (fuel cell mode/electrolyzer mode) in a H₂-O₂ laminar flow unitized regenerative micro-cell (LFURMC). Similarly, based on the host-guest transformation of LDHs, the organic molecule-intercalated CoAl-LDHs as precursors were subjected to the calcination and acid etching treatment, producing cobalt (Co) single atoms catalysts (denoted as IE-SACs), as demonstrated in Figure 16A [234]. The metanilic acid (MA) was selected as intercalation molecules to provide highly N species to form Co-N active sites, whereas the p-toluenesulfonic acid (PA) served as the other co-intercalation molecules and can promote the exposure of Co single atoms. As a result, the IE-SACs(PA+MA) catalyst had a small potential gap (ΔE) of 0.72 V for ORR/OER processes. Moreover, the self-assembled liquid ZAB with the IE-SACs(PA+MA) displayed an open circuit voltage of 1.42 V and a peak power density of 65 mW cm⁻², which were higher than those of IE-SACs(PA)- and IE-SACs(MA)-assembled liquid ZABs (Figure 16B). At a discharge density of 5 mA cm⁻², in Figure 16C, the IE-SAC(PA+MA)-assembled liquid ZAB delivered a high discharge voltage of 1.2 V with a specific capacity of 690.3 mAh g⁻¹ and an energy density of 963.3 Wh kg⁻¹.

Moreover, on account of the unique electronic property and high intrinsic reactivity, the transition-metals nitrides (TMNs) and chalcogenides (TMCs) derived from LDHs precursor have also been investigated as bifunctional catalysts capable of driving both OER and ORR. For example, Fu et al. [235] reported a highly efficient bifunctional ORR/OER electrocatalyst: Ni₃FeN microspheres with porous structure, synthesized by the thermal ammonolysis of NiFe-LDHs microspheres. As compared with the Ni₃Fe alloy and NiFeO_x catalysts prepared by calcination of the NiFe-LDHs precursor under H₂ and N₂ atmospheres, respectively, the Ni₃FeN catalyst exhibited better bifunctional electrocatalytic activity and stability, which was mainly attributed to the high electrical conductivity rooted in its typical metallic characteristic. In addition, Ni₃N electrocatalysts have also shown remarkable HER activity because of its small ΔG_H* due to the Ni–N co-effect [236], but the HER activity of nickel nitrides in alkaline media is still unsatisfactory for practical applications due to their sluggish water dissociation kinetics. Recently, metal hydroxides or oxides are selected as water cleavage “promoters” for cleaving HO–H bonds to produce hydrogen species to increase the alkaline HER activity [237]. As an example, Wang et al. designed and fabricated a bifunctional electrocatalyst, 3D hierarchical heterostructure NiFe-LDHs@Ni₃N nano/microsheet arrays on Ni foam (NiFe-LDHs@Ni₃N/NF), showing a low cell voltage of 1.80 V at a current density of 500 mA cm⁻² with a remarkable durability of 100 h in an alkaline aqueous electrolyzer [238]. Such bifunctional OER/HER performance was ascribed to the strong coupling and synergistic effects between the NiFe-LDHs nanosheets and the Ni₃N micro-sheet arrays, which provides a robust integrated structure and fast electron transfer.

Considering the high ORR-active activity of Co,N-CNF derived from Zn,Co-ZIFs, a novel Ni₃FeN/Co,N-CNF hybrid was fabricated by Wang et al. [239], which delivered an improved bifunctional activity with a ΔE of 0.69 V, lower than those of Ni₃FeN (1.00 V) and Co,N-CNF (0.86 V). The constructed rechargeable zinc–air battery using the Ni₃FeN/Co,N-CNF hybrid displayed a steady operation over 540 h at 6 mA cm⁻² with a small initial discharge-charge voltage gap of 0.79 V. In another case, cobalt-based hydroxysulfides (CoMS_x(OH)_y, M = Fe, Al) with high intrinsic activity and electrical conductivity were presented as bifunctional ORR/OER electrocatalysts for ZABs device [240]. In a typical procedure, the CoAl-LDHs were immersed in a high-concentration S²⁻ solution at room temperature, and then the S²⁻ ions continuously replaced the OH⁻ in the solid phase according to the solubility equilibrium (K_sp[Co(OH)₂] = 1.6 × 10⁻¹⁵, K_sp[CoS] = 4 × 10⁻²¹ at 25 °C). The electron structure of the active transition-metals sites was adjusted by S²⁻ anions modulation. The Co₃FeS_1.5(OH)₆ hydroxysulfides were assembled in the air electrode for a rechargeable ZAB with a small overpotential of 0.86 V at 20.0 mA cm⁻², a high specific capacity of 898 mAh g⁻¹, and a long cycling life, which was much better than Pt and Ir-based electrocatalysts in the same systems. Dai’s group designed 2D rhenium disulfide (ReS₂)/NiFe-LDHs materials grown on the carbon fiber paper (CFP) for a “one device-two functions” system by integrated cascade Zn-air battery/electrolyzer, which can be efficiently switched between electricity storage (of Zn-air battery) and power-to-gas conversion (of electrolyzer) modes [241]. It was pointed out that the edge and surface sites of NiFe-LDHs were responsible for both OER and ORR activities, while the unprecedented activity of the ReS₂/NiFe-LDHs for HER emerged from the S–O bonds at the heterointerfaces, together with the strong coupling effect of NiFe-LDHs and ReS₂. As shown in Figure 17A, a voltage of 1.60 V was obtained at 10 mA cm⁻², indicating an overpotential of only 370 mV for the overall water electrolysis when ReS₂/NiFe-LDHs hetero-nanosheets electrocatalyst served as both the anode and cathode. The ReS₂/NiFe-LDHs hybrids exhibited a robust durability for water electrolysis upon a long-term operation at different current densities of 10, 20, 50, 100, and 200 mA cm⁻², respectively, Figure 17B. The total Faraday efficiency (FE) for the self-powered system was calculated to be ~32%, Figure 17C. The integrated system, when used as cascade electrolyzers, can produce H₂ continuously with a high FE of ~96%, while working as cascade Zn–air batteries, featuring a round-trip efficiency of ~61%. In short, using the ReS₂/NiFe-LDHs hetero-nanosheets electrocatalyst as shared electrodes, the newly developed integrated cascade system can be readily and efficiently switched between the battery and electrolyzer modes, realizing “one device-two functions”, Figure 17D. Additionally, some typical bifunctional LDHs-based ORR/OER electrocatalysts are summarized in Table 2.

5. Conclusions and Perspectives

LDHs-based materials have shown great potential in the alkaline electrocatalytic ORR and OER. This review summarizes the latest developments in transition metal-based LDHs electrocatalysts, focusing on NiFe-, CoFe-, CoNiFe-, and other transition metals-based electrocatalysts. The design and synthesis of electrocatalysts, activity origin analysis, functionalization strategies for boosting OER performance, catalytic mechanism as well as structure-performance and chemical-composition-performance relationships are discussed from the experimental and theoretical perspectives. The key issues for developing highly efficient LDHs-based electrocatalysts are (i) the regulation of layer composition, to modify the coordination environment and electronic structure of active sites, improving the intrinsic activity; (ii) the interlayer–guest intercalation to enlarge basal spacing and expose more inner active sites, facilitating the electron/charge transfer and the mass diffusion; (iii) vacancy engineering (e.g., oxygen vacancy and metal vacancy) to facilitate the adsorption of reaction intermediates and improve the reaction kinetics; (iv) ultrathin nanostructure to increase the exposed numbers of active edge-sites; (v) structural/morphologic design, to achieve a desirable stability and durability; and (vi) the hybridization to enhance the electronic conductivity and provide multifunctional properties. The remarkable performances endow functionalized LDHs and their derivatives with great potential application as bifunctional ORR/OER electrocatalysts in the rechargeable zinc-air batteries, and unitized regenerative fuel cells.

Although some achievements have been made on electrocatalysts based on functionalized LDHs in oxygen electrode reactions, there are still some critical challenges to overcome, and there is much room for improving the catalytic performance, precise regulation of catalyst structure, as well as revealing the structure-performance correlation. The first challenge is to develop a scalable synthetic method. Although there are plenty of well-established synthetic methods developed in the laboratory, a facile and controllable synthesis route of LDHs-based electrocatalysts with satisfactory activity/structure-stability and performance is still limited. This is a restriction to achieve their mass-production and large-scale application. Secondly, it is difficult to identify the real active sites and explore the reaction mechanism due to the complexity of reaction intermediates and paths, as well as the evolution of active sites under real reaction conditions. The atomically resolved electron microscopy (4D-EM, STM, and HAADF-STEM) can allow the direct observation of transient morphology and structure of active sites during the reaction process. The combination of in situ/operando techniques, such as operando Raman, XRD, XPS, XAS, XANES, as well as theoretical study, e.g., DFT and DFT+U, can help deeply study the real catalytic process, the structural evolution, and the structure-performance relationship of the LDHs. The third key challenge is how to maintain the chemical and mechanical stability of LDHs-based electrodes under the industrial conditions, such as strong alkali electrolyte, high operating-temperature, and high current density. The in situ grown nanoarray electrode based on LDHs materials or their derivatives is significantly superior over the corresponding electrode prepared by the traditional spraying or dip-coating method. The nanoarray electrode, without the addition of the binder, shows a strong interaction between the conductive substrate (current collector) and active species, which can protect the active materials from falling off from the current collector. Moreover, the electro-deposition method would be feasible for preparing large scale nanoarray electrodes. Finally, integrating the ORR-active materials and OER-active LDHs, or designing the derivatives from LDHs precursors for bifunctional ORR/OER catalysts, is essential to the development of the URFCs and ZABs in the future. How to precisely control the composition and hierarchical structure of the bifunctional electrocatalysts? The key aspects are to rationally design and arrange the different active sites on the specific positions to avoid the competition of the ORR/OER active sites; and the occupation of the efficient positions, in a bifunctional electrocatalyst, might ensure fully the exposure to the dual-pathway of electron conduction and ion transportation in the ORR/OER multiphase electrocatalysis.

Author Contributions

J.W. searched the literature and wrote the manuscript; H.K. contributed with the data analysis; Y.J. wrote part of this work; F.G. redacted and corrected the references; N.A.-V. reviewed the work; H.Z. and Y.F. organized, supervised, and reviewed the work. All authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Acknowledgments

This work is supported by National Key R&D Program of China (No. 2016YFB0301600), the National Natural Science Foundation of China (No. 21571015, 21627813), Program for Changjiang Scholars and Innovative Research Team in University (No. IRT1205), Fundamental Research Funds for the Central Universities (No. ZY2117).

Conflicts of Interest

The authors declare no conflict of interest.

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Figures and Tables

Figure 1. The design of the different modification strategies for LDHs materials.

Figure 2. Schematic representation of the typical LDHs structure [100]. Copyright 2017, MDPI.

Figure 3. (A) CV curves of NiFe layered oxyhydroxide electrocatalysts used for the operando experiments with (B,G) Mössbauer spectra collected at open circuit (gray), at (C,F) 1.49 V (purple), (D) 1.62 V (yellow), and (E) 1.76 V (red). CV data were recorded in the Mössbauer-electrochemical cell with a scan rate of 25 mV/s prior to Mössbauer measurements [121]. Copyright © 2015 American Chemical Society.

Figure 4. (A) Faradaic O2 efficiencies of NiFe oxyhydroxide catalysts as a function of Fe-content (Ni100−xFex) given as atomic%. The hatched bar represented the O2 efficiency excluding the charge associated with QF,Ni+2/+3, corresponding to the Ni(OH)2/NiOOH redox process. The Faradaic O2 efficiency was derived from FEO2 (%) = QF,O2DEMS/QFtot; (B) X-ray absorption spectra of the NiFe catalysts with varying catalyst composition (Ni100−xFex) freeze-quenched under application of catalytic potential after conditioning at 1.63 V for 30 min in 0.1 M KOH [123]. Copyright © 2016 American Chemical Society. (C) In situ Raman spectra collected in a large wavenumber region from NiFe-LDHs during OER process in 1 M KOH at various overpotentials vs. RHE; (D) In situ Raman spectra collected in 1 M KOH with different applied overpotentials vs. RHE from −100 mV to 300 mV for Ni(OH)2 on Ni foam. The peaks appeared at ~478 ± 1 and ~557 ± 1 cm−1, indicating the transformation of Ni(OH)2 to NiOOH during oxygen evolution reaction in alkaline media; (E) the OER mechanism of NiFe LDH: OH− from the aqueous electrolyte was adsorbed on the Ni2+ center at modest overpotentials (η~200–300 mV), forming OHad intermediate on the Ni site [127]. Copyright © The Royal Society of Chemistry 2019.

Figure 5. (A) Schematic structure of pristine NiFe-LDH and Mn2+-doped NiFe-LDH. (B) Electronic structure of Ni and Fe sites in pristine NiFe-LDH and Mn2+-doped NiFe-LDH in (A), respectively. (C) CV curves at a scan rate of 1 mV s−1; (D) Tafel slopes of pristine NiFe-LDH, Mn2+-doped NiFe-LDH and RuO2 in 1 M KOH solution [128]. Copyright © The Royal Society of Chemistry 2018.

Figure 6. (A) The schematic diagram of NiFeV-LDHs structure. (B) Polarization curves of the non-noble metal catalysts (NiFeV-LDHs, NiFe-LDHs, Ni-(OH)2, and NiV-LDHs) and the commercial RuO2/C catalyst (C) Gibbs free energy diagram for the four steps of OER on NiFe LDHs (black line) and NiFeV LDHs (red line). (D) Total density of states (TDOS) curves of NiFeV LDHs and NiFe LDHs [134]. Copyright © 2018 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim. (E) Schematic representations of the electronic coupling among Ni, Fe, and V in Ni3Fe, Ni3V, and Ni3Fe0.5V0.5 [111]. Copyright © 2018 Nature Publishing Group.

Figure 7. (A) Basal spacings of NiFe-LDHs nanosheets with different interlayer anions as synthesized (blue) and after suspension in 1 M KOH in ambient air (red). (B) Overpotentials η of NiFe-LDHs materials with different interlayer anions Am− derived from constant current electrolysis at 1 mA cm−2 in virtually carbonate-free electrolyte as a function of anion basicity [142]. Copyright © The Royal Society of Chemistry 2016. (C) Relationship between onset potentials with the standard redox potentials of the examined anions [144]. Copyright © Tsinghua University Press and Springer-Verlag GmbH Germany 2017. (D) Schematic illustration of the fabrication process of Ni2Fe-CO32−-LDH/CFP and Ni2Fe-SDS2−-LDH/CFP [60]. Copyright © 2017 Elsevier Ltd.

Figure 8. (A) Schematic illustration of introducing oxygen vacancy defects to NiFe-LDHs nanoarray electrode and the corresponding OER performance [155]. Copyright © Science China Press and Springer-Verlag GmbH Germany 2018. (B) Schematic illustration of defective NiFe-LDH with oxygen vacancies prepared by fast reducing flame treatment for different periods of time and the corresponding OER performance [151]. Copyright © 2018 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim. (C) The synthesis of NiFe LDHs-VFe and NiFe LDHs-VNi by strong alkali etching LDHs and the corresponding OER performance [49]. Copyright © 2018 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim.

Figure 9. (A) Schematic representation of materials structures, the corresponding polarization curves at 1600 rpm in 1 M KOH and the AFM image of exfoliated single-layer nanosheets of NiCo LDH [160]. Copyright © 2014 Macmillan Publishers Limited. (B) Schematic illustration for pristine bulk NiFe-LDHs transformed to exfoliated ultrathin nanosheets via the ORDE process, and the SEM characterizations of the pristine bulk (left) and exfoliated NiFe LDHs (right) [164]. Copyright © 2018 American Chemical Society. (C) CoFe-LDH nanosheets by Ar plasma exfoliation, the corresponding OER performance at 1600 rpm in 1 M KOH and the TEM image of the ultrathin CoFe LDHs-Ar nanosheets [165]. Copyright © 2017 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim.

Figure 10. (A) Schematic illustration for the formation of ultrathin single-unit-cell-thick LDH NSs; (B) LSV curves for the ultrathin single-unit-cell NiFe-LDH NSs, bulk NiFe-LDHs, IrO2 nanoparticles at 1600 rpm in 0.1 M KOH solution [168]. Copyright © Tsinghua University Press and Springer-Verlag GmbH Germany 2017. (C) Synthetic strategy used for the synthesis of ultrafine monolayer LDH nanosheets; (D) OER polarization curves for LDH-Bulk, LDH-Monolayer, LDH-UF, IrO2, and graphite, respectively at 1600 rpm in 1 M KOH solution [170]. Copyright © 2018 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim.

Figure 11. (A) Scheme of the Synthesis of NiFe-LDH HMS; (B) LSV curves of the catalysts at 1600 rpm in 1 M KOH [173]. Copyright © 2016 American Chemical Society. (C) Schematic illustration of the fabrication of hollow Ni-Fe-Ce-LDH microcapsules mediated by cerium doping in MIL-88A; (D) polarization curves of Ni-Fe-Ce-LDH with different Ce/Fe ratios at 1600 rpm in 1 M KOH solution [175]. Copyright © The Royal Society of Chemistry 2020.

Figure 12. (A) Schematic illustration of the fabrication and synthesis principle of the Ni-based LDH/GQDs nanosheet arrays; (B) XPS spectra of the NiFe-LDHs/GQD (left), NiCo-LDHs/GQD (middle), NiMn-LDHs/GQD (right) electrocatalysts, respectively; (C) Reduced LSV overpotentials at 10 mA cm−2 vs. shift degree of Ni 2p3/2 binding energy center for Ni-based LDHs/GQDs; (D) Reduced LSV overpotentials at 10 mA cm−2 vs. reduced DFT overpotentials of Ni-based LDHs/GQDs; (E) Charge density difference of NiFe/G when O‒CH bonds with Ni/Fe (iso-surface levels are 0.0036 eÅ−3, cyan and yellow represented electron depletion and accumulation, respectively) [178]. Copyright © 2021 Elsevier Ltd.

Figure 13. (A) Schematic illustration of the fabrication procedure of the self-standing 3D core–shell Cu@NiFe-LDH electrocatalysts; (B) OER performance of Cu@NiFe-LDH conducted in 1 M KOH [181]. Copyright © The Royal Society of Chemistry 2017. (C) The energy diagrams of CoP and FeNi-LDH and the proposed mechanism for electrocatalyzing OER in the FeNi-LDH/CoP/CC p-n junction under the condition of applying enough potential via the external circuit; (D) LSV curves toward OER in 1 M KOH electrolyte at a scan rate of 5 mV s−1 [183]. Copyright © 2019 Wiley-VCH Verlag GmbH & Co. KGaA, Weinheim.

Figure 14. (A) Formation of metal/oxygen vacancies (VM, VO) in LDHs; (B) Bifunctional catalytic activity of Ag NP/NiRu-LDHs and commercial Pt/C catalysts toward ORR/OER activities at 1600 rpm in 0.1 M KOH electrolyte [216]. Copyright © 2018 American Chemical Society. (C) Schematic illustration of the selective growth for the fabrication of Janus MnO2-NiFe/Ni with the assistance of Vaseline. (D) OER and ORR polarization curves of air electrodes at 1600 rpm in 1 M KOH solution [217]. Copyright © 2019 American Chemical Society. (E) Structural representation of the asymmetrical electrolytic cell (AEC). (F) Electrolysis test with AA battery (1.5 V rated voltage) as the power source [218]. Copyright © 2021 Wiley-VCH GmbH. (G) Schematic of the in situ growth of LDH nanosheets on nitrogen doped GO (N-GO); (H) Individual ORR and OER, and total overpotentials for Ni2CoIIIFe-LDH/N-GO of this study in comparison to the published literature [219]. Copyright © 2017 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim. (I) Charge and discharge polarization curves of rechargeable zinc-air batteries in 6 M KOH and 0.2 M zinc acetate. (J) Charge and discharge cycling curves of rechargeable zinc-air batteries at a current density of 25 mA cm−2 [220]. Copyright © 2017 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim.

Figure 15. (A) Charge and discharge polarization profiles and discharge power density, the electrolyte was 6.0 M KOH aqueous solution containing 0.20 M Zn(CH3COO)2; (B) Rate performances of the LDH-POF and Pt/C+Ir/C cathodes; (C) Galvanostatic cycling curves at 5.0 mA cm−2 of the LDH-POF and Pt/C+Ir/C cathodes [230]. Copyright © 2020 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim. (D) Schematic diagram of the synergy between each component in the CoNC@LDH electrocatalyst; (E) Bifunctional performance evaluation and comparison, the inset is the corresponding Tafel plots for ORR and OER, respectively at 1600 rpm in 0.1 M KOH alkaline electrolyte; (F) Long-term durability evaluations on rechargeable ZABs [231]. Copyright © 2021 Wiley-VCH GmbH.

Figure 16. (A) Schematic representation of IE-SACs obtained via confinement synthesis strategy. (B) Polarization curves and corresponding power density plots of the liquid ZABs, 6 M KOH + 0.2 M zinc acetate as the electrolyte. (C) Galvanostatic discharge curves of the IE-SAC(PA+MA)-assembled liquid ZAB at 5 mA cm−2 [234]. Copyright © 2020 Wiley-VCH GmbH.

Figure 17. (A) Overall water electrolysis LSV curves of the ReS2/NiFe-LDH‖ReS2/NiFe-LDHs and 20% Pt/C‖IrO2 in 1 M KOH solution. Insets show the digital photograph of the two-electrode configuration. (B) Chronopotentiometry curves at various current densities. (C) Faraday efficiencies of the Zn–air batteries-powered water electrolysis and the power supply directly driven four-cascade water electrolysis at different charging current. (D) Schematic illustration and digital photographs of the integrated cascade battery/electrolyzer systems for electrolyzer (H2 production) and batteries (mobile charging) operations [241]. Copyright © 2021 American Chemical Society.

Table 1

Representative LDHs electrocatalysts for the OER process in 1 M KOH electrolyte.

Catalysts	Modification Method	Overpotential/mV	Tafel Slope/mV dec−1	Stability	Ref.
Co2+-doped NiFe-LDHs	Cation-doping	264@10 mA cm−2	58.1	10 h	[132]
Co3+-doped NiFe-LDHs	-	249@10 mA cm−2	50.5	10 h	[132]
Ni6Fe2Cr1-LDHs	-	225@25 mA cm−2	69	At 10 mA cm−2 for 6 h	[187]
NiFeZr-LDHs	-	198@10 mA cm−2	53.1	At 1.47 V for 12 h	[188]
Mn2+-doped NiFe-LDHs	-	190@10 mA cm−2	68.6	At 50 mA cm−2 for 40 h; 750 cycles at 5 mV s−1	[128]
NiFeV-LDHs	-	195@20 mA cm−2	42	At 1.48 V for 18 h	[134]
NiVRu-LDHs	-	190@10 mA cm−2	83	2000 cycles; at 50 mA cm−2 for 600 h; at 200 mA cm−2 for 400 h	[189]
NiFeMn4+-LDHs	-	289@20 mA cm−2	47	At η = 310 mV for 15 h; at 10 mA cm−2 for 15 h	[129]
NiVIr-LDHs	-	203@10 mA cm−2	55.3	At 10 mA cm−2 for 15 h	[190]
NiCoRu-LDHs	-	270@100 mA cm−2	40	At 100 mA cm−2 for 55 h	[191]
CoFeV-LDHs	-	242@10 mA cm−2	57	At η = 250 mV for 32 h	[192]
CoFeCr-LDHs	-	270@100 mA cm−2	32	At 1.58 V for 24 h	[193]
Cr-CoFe LDHs	-	238@10 mA cm−2	107	1000, 3000, and 5000 cycles at 50 mV s−1; at 20 mA cm−2 for 20 h	[135]
W0.5Co0.4Fe0.1-LDHs	-	310@100 mA cm−2	32	3000 cycles at 5 mV s−1; at 20 mA cm−2 for 50 h	[194]
CoMoV-LDHs	-	270	106	At η = 300 mV for 20 h	[195]
ZnFe-VO4-LDHs	Anion- intercalation	250@10 mA cm−2	26	At 2.4 V for 4000 s; 200 cycles at 200 100 mV s−1	[196]
NiFe-WO4-LDHs	-	290@10 mA cm−2	41.5	At 10 mA cm−2 for 20 h	[197]
Ni2Fe-SDS-LDHs/CFP	-	289@10 mA cm−2	39	At 50 mV s−1 for 10 h	[60]
H2PO2−/NiFe-LDHs	-	250@10 mA cm−2	37.7	30,000 s	[143]
Formamide intercalated NiFe-LDHs/CR	-	210@10 mA cm−2	39	At 0.5 V for 18 h	[146]
NiFe-LDHs (POM)	-	287@10 mA cm−2	43	At 50 mA cm−2 for 35 h; at 10 mA cm−2 for 40 h	[198]
0.05-SB-Ni0.8Fe0.2(OH)2	-	301@10 mA cm−2	42	250, 500, 750 and 1000 cycles at 100 mA s−1; at η = 300 mV for 20 h	[199]
R-NiFe-LDHs	Defect engineering	200@10 mA cm−2	59.3	at 1.43 V for 10 h	[155]
CoFe-LDHs-Ar	-	266@10 mA cm−2	37.85	2000 CV cycles at 5 mV s−1	[165]
PM-LDHs	-	230@10 mA cm−2	47	At η = 230 mV for 100 h	[158]
N-CoFe-LDHs	-	310@10 mA cm−2	74	10 h
NiFe-LDHs-VFe	-	255@10 mA cm−2	70	2000 cycles at 10 mA cm−2	[49]
NiFe-LDHs-VNi	-	229@10 mA cm−2	62.9	2000 CV cycles at10 mA cm−2	[49]
D-NiFeZn-LDHs	-	200@20 mA cm−2	34.9	At 30 mA cm−2 for 10 h	[200]
ZnCo-UF	ultrathin nanosheets	360@10 mA cm−2	66		[163]
NiFe-LDHs	-	254@10 mA cm−2	32	At η = 254 mV for 12 h	[170]
E-CoFe-LDHs	-	302@10 mA cm−2	41	At 10 mA cm−2 for 10 h	[159]
DH-CoFe-LDHs	-	276@10 mA cm−2	40.3	At η = 276 mV for 10 h	[169]
N-CoFe–LDHs	-	233@10 mA cm−2	40.03	2000 cycles at 5 mV s−1	[201]
Ni3FeAl0.91-LDHs/NF	-	304@10 mA cm−2	50	18 h
NiFe-LDHs	-	300@10 mA cm−2	40	At 10 mA cm−2 for 13 h	[160]
FeNi-GO	LDH/carbon composites	206@10 mA cm−2	39	At 10 mA cm−2 for 8 h	[202]
NiFe-LDHs-NS@DG10	-	210@10 mA cm−2	52	At 5 mA cm−1 for 10 h; at 10 mA cm−1 for 10 h	[203]
NiFe LDHs/GQDs	-	189@10 mA cm−2	52.1	At 10 mA cm−2 for 15 h	[178]
CoFe-LDHs/TEG	-	301@10 mA cm−2	80	At 1.50 V for 25 h	[179]
NiFe-LDHs/CNT	-	290@10 mA cm−2	31	At 10 and 20 mA cm−2 for 1 h	[116]
Ce-NiFe-LDHs/CNT	-	227@10 mA cm−2	33	At 10 mA cm−2 for 30,000 s	[204]
Ag NWs/Ni0.95Fe0.05-LDHs	LDHs/Metal Compounds	330@10 mA cm−2	89	At 10 mA cm−2 for 12 h	[205]
FeNi-LDHs/FeNi foil	-	130@10 mA cm−2	39.8	At 1.5 V for 10 h	[206]
FeNi-LDHs@NWSSF	-	210@10 mA cm−2	56	At 10 mA cm−2 for 18 h	[207]
FeOOH/NiFe-LDHs	-	174@10 mA cm−2	27	1000 cycles at 300 mV s−1; at 10 mA cm−2 for 25 h; at 50 mA cm−2 for 15 h	[208]
NiO/NiFe-LDHs	-	205@30 mA cm−2	30	At 20 mA cm−2 for 10 h	[184]
NiMn- LDHs/NiCo2O4	-	310@10 mA cm−2	99	1000 cycles at 10 mA cm−2; at 1.65 V for 8 h	[209]
Ni3S2/NiFe-LDHs	-	200@10 mA cm−2	29.71	1000 cycles at 2 mV s−1; at 10 mA cm−2 for 45,000 s	[210]
NiFe-LDHs/(NiFe)Sx/CMT	-	210@10 mA cm−2	31	1000 cycles at 10 mA cm−2; at 10 mA cm−2 for 15 h	[211]
FeNi-LDHs/CoP	-	254@350 mA cm−2	33.5	18.5 h	[183]
Ni5P4/NiP2/NiFe-LDHs	-	197@10 mA cm−2	46.6	At 10, 100, and 200 mA cm−2 for 24 h	[212]
FeNi-LDHs/Ti3C2-MXene	-	240@10 mA cm−2	43	At 10 mA cm−2 for 12 h	[213]
FeCo-LDHs/MXene	-	268@10 mA cm−2	85	At 10 mA cm−2 for 30,000 s	[214]

Table 2

The bifunctional performances of LDHs-based materials in alkaline medium.

Catalysts	E1/2/V@ORR	Ej=10/V@OER	Specific Capacity/mAh g−1	PowerDensity	Open Circuit Potential	Charge/DischargeVoltage Gap	Cycling Time	Ref.
O-NiCoFe-LDHs	0.63	260	-	-	-	-	40 h	[242]
Ag NW@NiMn-LDHs	0.75	270	-	-	-	0.77 V @ 10 mA cm−2	-	[215]
Ag NP/NiRu-LDHs	0.8	210	-	-	-	-	25 h	[216]
NiFe-LDHs/NrGO	0.75	250	-	-	-	-	9.5 h	[225]
CoNi-NS/rGO	0.85	330	746	300 mW cm−2	1.37 V	0.8 V @ 10 mA cm−2	6 h	[221]
NiFe-LDHs/Fe-N-C	0.8	300	-	-	-	-	24 h	[243]
CoNiMn-LDHs/PPy/RGO	0.77	369	-	-	-	-	5 h	[244]
NiCoIIIFe-LDHs/N-GO	0.82	320	-	-	-	-	-	[218]
LDHs-POF	0.8	250	807	185mW cm−2	-	0.74 V @ 5 mA cm−2	2400cycles	[230]
NiFe-LDHs/Co,N-CNF	0.79	312	-	-	-	1 V @ 25 mA cm−2	80 h	[220]
CoNC@LDHs	0.84	240	743	173mW cm−2	1.22 V	0.67 V @ 10 mA cm−2	3600cycles	[231]
Co3O4@NiFe-LDHs	-	226	667.5	798Wh kg−1	1.38 V	0.8 V @ 15 mA cm−2	2000 h	[245]
MnO2-NiFe/Ni	0.81	226	-	94mW cm−2	-	0.98 V @ 50 mA cm−2	25 h	[217]
CoFe@NC/CC	0.75	254	-	154 mW cm−2	1.469 V	0.77 V @ 10 mA cm−2	42 h	[246]
IE-SAC(PA+MA)	0.851	349	690.3	963 Wh kg−1	1.38 V	0.57 V @ 1 mA cm−2	12 h	[234]
Ni3FeN	0.78	355	-	-	1.547 V	0.7 V @ 10 mA cm−2	100 h	[235]
Ni3FeN/Co,N-CNF	0.81	270	-	200 mW cm−2	1.43 V	0.79 V @ 6 mA cm−2	540 h	[239]
Co3FeS1.5(OH)6	0.721	358	898	113 mW cm−2	-	0.86 V @ 20 mA cm−2	36 h	[240]
Co3O4-doped Co/CoFe	0.82	370	757	942 Wh kg−1	1.43 V	0.65 V @ 5 mA cm−2	65 h	[90]
Co-CoOx/N-C	0.75	278	-	21 mW cm−2	1.32 V	-	11 h	[247]

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