Zesheng
Li
*,
Bolin
Li
,
Yifan
Hu
,
Shaoyu
Wang
and
Changlin
Yu
*
College of Chemistry, Guangdong University of Petrochemical Technology, Maoming, 525000, China. E-mail: lzs212@163.com; yuchanglinjx@163.com
First published on 1st December 2021
Electrocatalysts for the oxygen reduction reaction (ORR) are crucial for a variety of renewable energy applications (e.g., proton exchange membrane fuel cells, PEMFCs). The synthesis of highly-dispersed and high-metal-density ORR electrocatalysts (e.g., nanoscale and atomic-level structures) on carbon supports with strong durability is extremely desirable but remains challenging. Carbon-supported high-loading noble metal catalysts with nanoscale structures (e.g., Pt-based nanoparticles) are the most widely used catalysts with the best catalytic performances. Single atom catalysts (SACs) that integrate the merits of homogeneous and heterogeneous catalysts have attracted considerable attention in recent years. Aside from the manipulation of the geometric and electronic structures of active metal sites, another key challenge in this field is the development of strategies for preparing high-metal-density SACs, thus rendering atomic-level ORR electrocatalysts dramatically reactive, selective, and stable compared to their nanoscale counterparts. This review summarizes the recent advancements in carbon-supported nanoscale and atomic-level ORR electrocatalysts with high metal density (namely high loading) for fuel cells. Special emphasis is placed on the basic principles, preparation strategies and catalytic applications of these highly-dispersed and high-metal-density ORR electrocatalysts on carbon supports from nanoparticles to atomic-level architectures.
The oxygen reduction reaction (ORR), that is, the electrochemical reduction of oxygen molecules, is a relatively complex process in fuel cells or metal–oxygen cells.4 The oxygen reduction reaction of cathodes has many possible reaction mechanisms; the main reaction pathways are as follows:
(i) Oxygen molecules can be reduced to form water through a direct “four-electron mechanism” (taking metal Pt as an example):
2Pt + O2 → 2Pt–O | (1) |
2Pt–O + 2H+ + 2e− → 2Pt–OH | (2) |
2Pt–OH + 2H+ + 2e− → Pt + 2H2O | (3) |
O2 + 4H+ + 4e− → 2H2O E = 1.23 V vs. SHE (25 °C) | (4) |
(ii) Oxygen molecules can also be reduced by a “two-electron mechanism”; that is, two electrons can be obtained to be reduced to hydrogen peroxide:
O2 + 2H+ + 2e− → H2O2 E = 0.69 V vs. SHE (25 °C) | (5) |
The intermediate product H2O2 can be further reduced to water:
H2O2 + 2H+ + 2e− → 2H2O E = 1.77 V vs. SHE (25 °C) | (6) |
The development of ORR electrocatalysts with high performance and low cost is of great strategic significance in the development of advanced energy conversion devices. In essence, platinum (Pt) is still the most effective ORR electrocatalyst.6 However, its high price has restricted the development of PEMFCs. At present, effective countermeasures include: (i) reducing the use of Pt by optimizing the utilization of Pt catalyst, (ii) reducing the use of Pt by improving the performance of Pt catalyst, and (iii) developing other catalysts that can replace Pt metal.7 At present, the design direction of ORR electrocatalysts mainly includes “low-Pt electrocatalysts”, “Pt-free electrocatalysts” and “non-noble-metal electrocatalysts”. According to their action mechanism, low-Pt electrocatalysts can be divided into three types: (i) core–shell structure low-Pt electrocatalysts, (ii) alloy structure low-Pt electrocatalysts, and (iii) synergistic-effect low-Pt electrocatalysts (facilitated using co-catalysts).8 Pt-free electrocatalysts refer to other lower-price noble-metal electrocatalysts such as palladium (Pd), iridium (Ir) and silver (Ag).9 Non-noble-metal electrocatalysts refer to transition metal catalysts especially those of iron (Fe) and cobalt (Co), which are alternative electrocatalysts with rich resources and low price.10 These noble-metal or non-noble-metal ORR electrocatalysts have their own characteristics and advantages, and they are related to each other, and even complement each other in specific dimensions and environments.
Recently, several reviews have summarized the preparation methods and structural modification of noble-metal11,12 and non-noble-metal13,14 ORR electrocatalysts. They all are very much concerned with the relationship between the nanostructures, crystal structures, and electronic structures of metals and their electrochemical performances. Some of them only focus on the design of individual nano-morphologies and ignore the interaction with carbon supports. However, electrocatalysts for the actual application in PEMFCs are typically composed of highly dispersed active metal nanoparticles (NPs) on a variety of carbon supports, often with a high metal content (40–50 wt%), to guarantee the formation of thin catalyst layers along with metallically conducting interfaces.15–17 Therefore, it is necessary to pay attention to summarizing the synthetic strategies and structural properties of high-metal-loading ORR electrocatalysts, to meet the demands of practical applications of PEMFCs.
On the other hand, the dimensions and distribution of these high-loading active metal components on carbon supports have a great impact on the catalytic activity, product selectivity (i.e., two electron or four electron mechanism), and electrochemical stability of ORR electrocatalysts.18–20 In recent years, in order to improve the catalytic activity and selectivity and increase the utilization of active metals, ORR electrocatalysts have been developed from nanosize to sub-nanosize21 and even atomic-level22 architectures. Therefore, the development of highly-dispersed and high-metal-content (or high-metal-density) electrocatalysts with reduced dimensions (or atomic level structures) on carbon supports is very critical for the ORR in the practical application of fuel cells.
Single atom catalysts (SACs) usually consist of dispersed metal atoms and appropriate support materials, where the supports are employed to anchor onto, confine to, and/or coordinate with isolated metal atoms.23 Therefore, the features of SACs allow achieving maximum atom utilization (∼100%), which is of particular significance for the development of carbon-supported SACs for ORR electrocatalysis. In recent years, several reviews have discussed the synthesis strategies, coordination regulation, electrocatalytic applications, and structure–property relationships of carbon-supported SACs.24–26 However, these reviews to some extent have not addressed the regulation of metal density and site distance effects of SACs, or the synergistic effects of high-density single atoms, dual atoms, or atom clusters in ORR electrocatalysis. So, in order to deeply understand the ORR mechanisms and structure–property relationship of high-density SACs, a relevant review study is very necessary.
In this review, the preparation methods and ORR performances of carbon-supported high-metal-density ORR electrocatalysts (including nanosize NPs and atomic-level structures) are systematically summarized (see Scheme 1 for an overview of the topics covered here). The promising carbon supports for ORR electrocatalysts are introduced. The basic principles and applications of highly-dispersed and high-metal-density ORR electrocatalysts on different carbon supports are reviewed and analyzed. Particularly, the development process of carbon-supported SACs, the synthetic strategies of high-density SACs, and the synergistic effect of high-density SACs on carbon supports for the ORR are discussed. The fundamental understanding of the synthesis–construction–performance correlations for carbon-supported high-metal-density ORR electrocatalysts is preliminarily demonstrated. Finally, the challenges and prospects for the development of high-metal-density ORR electrocatalysts on carbon supports are highlighted.
When preparing high-metal-density ORR electrocatalysts, nano-scale carbon materials with high specific surface area are preferentially selected as supports, so that the active sites of metal NPs (or metal atoms) are fully exposed and participate in the catalytic reaction to maximize the mass activity.34 Because of the high metal loading, the metal components can very easily agglomerate, so the high dispersion of the catalyst is particularly critical. The pore structure (defects and nanopores) and surface state (doped N, P, and S atoms) of carbon materials play important roles in anchoring metal nanoparticles and dispersing metal atoms by coordination.35 Therefore, it is demonstrated that carbon supports with favorable porous structures, optimized surface defects and suitable functional groups should be considered to fabricate high-metal-density ORR electrocatalysts for PEMFCs.
In recent years, single-atom catalysts (SACs) have been widely studied because of their nearly 100% utilization of metal active sites and accurate and controllable coordination structures.43 However, due to the lack of multiple-atom connected group sites, monatomic sites are not competent in some multi-step complex catalytic reactions. For example, in the ORR catalytic process, monatomic Pt catalyst often cannot effectively catalyze the fracture of the O–O bond, so it is difficult to effectively catalyze the ORR in the four-electron mechanism.44 Due to the inability of isolated Pt single atoms to break the O–O bond through lateral adsorption, the ORR tends to form the two-electron product (H2O2) rather than the four-electron product (H2O) required by fuel cells.45 High-metal density (high loading) Pt SACs show much better ORR performance (with much higher mass activity) than low-metal density (low loading) Pt SACs and Pt NPs, in which the selectivity of high-metal density Pt SACs can be greatly inclined to the four-electron path.46 Therefore, for atomically-dispersed ORR electrocatalysts, the high-metal density strategy appears to be particularly important in the design of high-efficiency catalytic systems, in view of their distance-tunable metal sites and variable coordination environments.
Fig. 1 A series of carbon-supported Pt nanoparticles (reprinted with permission from ref. 50): (A) TEM images, (B) particle size distribution histograms of Pt, and (C–F) electrochemical performances; and typical carbon-supported Pt nanodendrites (reprinted with permission from ref. 54): (G and H) TEM images and (I and J) electrochemical performances. |
Fig. 1A and B show the TEM images of a variety of carbon-supported Pt catalysts (40 wt% Pt) and the corresponding particle size distribution histograms of Pt. The Pt NPs are uniformly dispersed on Vulcan, OMC and GNP500 supports, while some particle agglomerates are observed on HSAG300 and GNP10 supports. The highly graphitized structure and lack of oxygen functional groups in HSAG300 and GNP10 are not conducive to the uniform nucleation and dispersion of Pt NPs on their surfaces. The average particle sizes of Pt NPs were as follows: 3.11 nm (Pt/OMC) < 4.20 nm (Pt/GNP10) < 4.22 nm (Pt/Vulcan) < 4.41 nm (Pt/GNP500) < 6.57 nm (Pt/HSAG300). The ordered mesoporous carbon (OMC) with an internal porosity can offer a high surface area (1000 m2 g−1) for accommodating a large number of small Pt NPs compared with the solid carbon black (Vulcan) and graphitized carbons (HSAG300). The mesoporous graphitized nanoparticle (GNP500) support has favorable mesoporous structures (5–10 nm), moderately graphitized structures (namely moderate oxygen content), and small nanoparticle structures (∼50 nm), and should be a better support for Pt NPs than the OMC with amorphous structures and larger nanoscale structures (>500 nm). In addition, two commercial Pt/C catalysts (Pt/CJM and Pt/CHeraeus with 40 wt% Pt) also showed larger Pt NPs and poorer dispersion.
Fig. 1C shows the cyclic voltammograms (CVs) of the seven carbon-supported Pt catalysts (with 40 wt% Pt). In all these CVs, typical electrochemical potential sweep responses for Pt metal, such as Hads/des (0–300 mV), double-layer capacitance (300–750 mV) and oxide formation (750–1200 mV) regions, are clearly presented. The electrochemically active surface areas (ECSAs) of all these catalysts were evaluated by integrating Hdes peaks. This showed that Pt/OMC had the highest ECSA (34.3 m2 gPt−1) and the widest double-layer capacitance region. These are attributed to the smallest Pt NPs and the largest specific BET surface area of the carbon support for Pt/OMC. Fig. 1D shows the linear sweep voltammograms (LSVs) of the catalysts for the ORR in oxygen-saturated 0.5 M H2SO4 electrolyte. In the kinetic regime, the ORR activity was evaluated at a half-wave potential (2.5 mA cm−2), in which the two GNP-supported catalysts (Pt/GNP10 and Pt/GNP500) obviously showed better performance than the other catalysts. About 85 mV less overpotential for the ORR was obtained at Pt/GNP500 compared with that at Pt/Vulcan. Obviously, Pt/GNP500 showed the highest mass activity (Fig. 1E) and desirable stability (Fig. 1F) for the ORR. The results of this study demonstrated that the moderate graphitization level (namely moderate oxygen content and specific surface area), suitable mesoporous structure (5–10 nm), and interconnected small spherical morphology (∼50 nm) of carbon were found to be ideal properties for designing well-performing and highly-stable Pt NPs on carbon ORR electrocatalysts.50
On the other hand, three-dimensional (3-D) Pt-based nanostructures with a dendritic morphology have received much attention as ORR electrocatalysts.51–53 These unique Pt-based nanodendrites (NDs) generally have the advantages of high surface area and enhanced performances due to their dominant crystal planes and highly branched shapes.53 Previously, Li et al. reported carbon-supported Pt-on-Co NDs with high-Pt-content (37.52 wt% Pt) as an efficient ORR electrocatalyst for the first time (see Fig. 1G–J).54 These Pt-based NDs were spontaneously generated and deposited on polymer-derived carbon by a simple cobalt-induced and carbon-mediated galvanic cell reaction approach. The TEM images clearly reveal that the carbon-supported Pt NDs have distinct 3-D flower-like structures and an average diameter of 20 nm (with individual Pt nanoparticles of 3 nm) (Fig. 1G and H). The ORR LSV curves of the catalysts were recorded in oxygen-saturated 0.1 M HClO4 (Fig. 1I), and the mass activities at 0.9 V were calculated to be 122, 163 and 251 mA mg−1 Pt for commercial Pt/C (47.60 wt% Pt), supported 3-D Pt NDs (37.52 wt% Pt) and supported 3-D Pt-on-Co NDs (18.34 wt% Pt), respectively. More recently, Feng and co-workers synthesized branched Pt–Pd NDs supported on reduced graphene oxide (rGO), which exhibited enhanced ORR activity (onset potential of 0.05 V, half-wave potential of −0.15 V, electron transfer number >3.99) and good stability in alkaline medium (0.1 M KOH).55 Besides, high-density Au ND-loaded GO (Au ND-GO) also exhibited high electrocatalytic activity (in a near four-electron pathway) and superior stability toward the ORR in alkaline medium (0.1 M KOH).56 Overall, the results of these studies indicated that the construction of 3-D dendritic nanostructures is an attractive strategy for designing high-metal-density ORR catalysts with remarkable catalytic activity and durability.
The development of carbon-supported PtM (where M = Fe, Co, Ni, etc.) alloys with high dispersion and high metal density is an important research direction for high-performance ORR electrocatalysts.62–64 Achieving the homogeneous formation of ultrasmall PtM alloy NPs directly on carbon supports, with high catalyst loading, promises a facile and scalable production of alloy ORR electrocatalysts. However, the precise control of nucleation and alloying of two different metals on carbon supports is still a great challenge. Recently, Sung and co-workers63 reported a novel synthetic strategy to directly grow highly-dispersed MPt (where M = Fe, Co, and Ni) alloy NPs on various carbon supports with high catalyst loading, from a unique bimetallic compound composed of [M(bpy)3]2+ cations (bpy = 2,2′-bipyridine) and [PtCl6]2− anions. Thereinto, the representative rGO-supported FePt catalyst (37 wt%-FePt/rGO) with high homogeneity and narrow size distribution (5–6 nm) exhibited 18.8 times higher specific activity and 11.5 times higher mass specific activity than commercial Pt/C catalyst at 0.9 V (see Fig. 2A–C). It is noteworthy that the high metal loading catalyst (37 wt%-FePt/rGO) showed better electrocatalytic activity than the low metal loading catalyst (24 wt%-FePt/rGO), due to its high uniformity and high utilization efficiency. The high metal loading catalyst (37 wt%-FePt/rGO) also demonstrated excellent electrochemical stability without degradation over 20000 cycles.63
Fig. 2 The rGO-supported FePt alloy catalyst (reprinted with permission from ref. 63): (A and B) TEM images and (C) electrochemical performances. The 3-D MGS-supported PtAg alloy catalyst (reprinted with permission from ref. 70): (D–F) TEM images, (G) XRD patterns, and (H and I) electrochemical performances. |
Fu and co-workers64 also demonstrated a general hydrogel-freeze drying and annealing joint strategy for the synthesis of rGO-supported Pt3M (where M = Mn, Cr, Fe and Co) alloy NPs (Pt3M/rGO) with ultrafine particle size (about 3 nm) and dramatic monodispersity. With Pt3Mn/rGO as an example, after the annealing process at high temperature (700 °C) for 12 h, ultrasmall Pt3Mn ordered intermetallic NPs can be formed due to the confinement effect of the porous structure of rGO. The catalytic performance of Pt3Mn/rGO (∼3 nm, 22.5 wt%) for the ORR was evaluated and compared with that of commercial Pt/C (∼3.3 nm, 20 wt%). The Pt3Mn/rGO catalyst exhibited greatly improved kinetic activity (1.37 times) compared to the commercial Pt/C at 0.9 V potential. The improved catalytic activity can be due to three factors: (i) the ultrafine particle size of Pt3Mn NPs affords rich active sites, (ii) the ordered intermetallic phase promotes the shift of the d-band of Pt3Mn NPs, and (iii) the high graphitization degree of rGO improves the conductivity of the catalyst.64
For traditional PtM (where M is transition metal) alloy ORR electrocatalysts, their electrochemical stability is far from meeting the requirements of practical applications, and the dissolution of transition metal is always a key problem affecting fuel cell systems.65 In order to design stable alloy electrocatalysts, the use of acid-soluble transition metals should be avoided or reduced as much as possible. Some noble metals with relatively low price or rich reserves, such as Ag, Pd and even Au, can be selected to prepare newly Pt-based alloy electrocatalysts.66–68 As a cheap noble metal with the highest conductivity, Ag can be used to design cost-effective AgPt alloy ORR electrocatalysts. In addition to the “structural adjustment” of alloys to improve their stability, the “support enhancement” of alloys can also be considered. For example, one can develop highly-stable support materials (e.g., 3-D porous graphene) to improve the stability of catalysts in terms of support enhancement.
Previously, Shen and co-workers prepared a new type of 3-D mesoporous graphene nanosheet conductive network (3-D MGS) material by an efficient synchronous graphitization-activation technology.69 The 3-D MGS material has highly mesoporous structures with high permeability and well graphitized structures with high conductivity. Recently, Li et al. further synthesized a high-metal-content AgPt alloy ORR electrocatalyst based on this novel 3-D MGS as a support material (see Fig. 2D–I).70 Typically, when the total metal content is 49.6 wt% (24.7 wt% Pt + 24.9 wt% Ag), highly-dispersed and highly-dense AgPt alloy NPs with ultrafine size (2.4–2.7 nm) are loaded onto the surface of the 3-D MGS support without any agglomeration (see Fig. 2D–F). The uniformity of the particle size distribution of PtAg/3DMGS (49.6 wt%) is much better than that of PtAg/Vulcan XC-72 (25.7 wt%),71 indicating that the 3DMGS with small mesoporous structures (2–10 nm) is more beneficial for the preparation of catalysts with high metal content. The average crystal sizes of Pt/3DMGS (2) (46.1 wt%), PtAg/3DMGS-1# (3) (45.3 wt%), and PtAg/3DMGS-2# (4) (49.6 wt%) are estimated to be 2.3, 2.4, and 2.5 nm based on (220) planes in XRD patterns (see Fig. 2G).
The ORR electrocatalytic activities of the series of catalysts were evaluated using the RRDE in oxygen-saturated 0.1 M HClO4 aqueous solution. The PtAg/3DMGS-2# catalyst exhibits better ORR performance; it shows 43 mV higher half-wave potential (3.0 mA cm−2) than commercial Pt/C catalyst (47.6 wt%, TKK) based on the same Pt loading (10 mgPt) on the electrode (see Fig. 2H). This promising PtAg/3DMGS-2# catalyst exhibits an ultrahigh mass activity (at 0.9 V) of 392 mA mgPt−1, which is nearly 4 times that of commercial Pt/C catalyst (102 mA mgPt−1) (see Fig. 2I). The PtAg/Vulcan XC-72 (25.7 wt%) catalyst shows a lower mass activity (at 0.9 V) of 316 mA mgPt−1 under the same test conditions.71 Moreover, comparable electrocatalytic stability (81.6% of the initial activity) is also obtained for PtAg/3DMGS-2# through an accelerated durability test with 1000 CV cycles. The excellent electrocatalytic performances of the PtAg/3DMGS catalysts are mainly attributed to the structural advantages and electronic effects of the ultrafine PtAg alloy NPs. Meanwhile, the convenient binary channels for both electron transport and ion diffusion of 3DMGS conductive networks are also supposed to be beneficial for their performance improvement.70
The M@Pt core–shell structure can be generally prepared by a seed-mediated galvanic replacement strategy by in situ displaced growth of a Pt shell on a M core (seed).74–76 Galvanic replacement usually takes place between a noble metal salt (high standard reduction potential) and transition metal (low standard reduction potential), which can be inhibited during the growth of Co@Pt NPs by using carbon monoxide as a stabilizing ligand and a reducing agent.75 However, these Co@Pt NPs need to be further loaded onto a carbon support before the measurement of electrochemical performances. Recently, Jia and co-workers developed a facile galvanic replacement method to achieve gradient Pt–Ni alloys (with Pt-rich surfaces), followed by a partial dealloying approach for the construction of core–shell (Pt–Ni alloy core with defective (D) Pt shell (≈3 monolayers)) NPs directly on a graphene carbon support (Pt–Ni@PtD/G) as a high-performance ORR electrocatalyst (see Fig. 3A–D).76
Fig. 3 The Pt–Ni@PtD/G core–shell catalyst (reprinted with permission from ref. 76): (A) structural schematic diagram, (B) TEM image, and (C and D) electrochemical performances. The Pt-skin Pd10Pt1/AGN catalyst (reprinted with permission from ref. 79): (E) structural schematic diagram, (F–H) TEM images, (I) XRD patterns, and (J and K) electrochemical performances. The Pd9Au1@Pt/C core–shell catalyst (reprinted with permission from ref. 81): (L) TEM images and (M and N) electrochemical performances. |
The graphene (G)-supported Ni NPs were directly reacted in chloroplatinic acid to form gradient Pt–Ni alloys on G by galvanic replacement reaction. Then, the Pt–Ni@PtD/G core–shell catalyst was obtained by an acid leaching process to gradually etch surface Ni atoms in the Pt–Ni alloys (see Fig. 3A). The high-density Pt–Ni@PtD/G NPs were homogeneously dispersed on the graphene surface with particle sizes of around 5 nm (see Fig. 3B). The Pt–Ni@PtD/G core–shell NPs performed as a promising catalyst for the ORR in 0.1 M HClO4 electrolyte with a mass activity threefold higher than that of the Pt/C counterpart (see Fig. 3C and D), which is mainly due to the optimized electronic structure of Pt because of the synergetic effect between the Pt–Ni core and defective Pt shell. More importantly, the Pt–Ni@PtD/G core–shell NPs showed extremely enhanced stability arising from the Pt shell preventing the dissolution of the Ni core, which solve a long-standing issue of unstable Pt–Ni alloy in an acidic ORR.76
On the other hand, PtM (where M = Fe, Co, Ni, etc.) alloys with Pt-skin surfaces can be produced by thermally-induced surface segregation in specific atmospheres (CO, NO, O2, H2, etc.).77 Different PtM alloys require different atmospheres for the surface segregation of Pt atoms. For example, PtCo alloy NPs can be transformed into PtCo@Pt-skin NPs by heat treatment in a CO atmosphere.78 Recently, Li et al. successfully constructed an ultra-low-Pt Pd10Pt1 bimetallic catalyst (with a Pt-skin surface) by heat treatment in a H2 atmosphere for the ORR (see Fig. 3E–K).79 Particularly, a novel active graphene-like nanosheet (AGN) material with high specific surface area and high conductivity was developed as an efficient support to form a high-metal-density Pt-skin Pd10Pt1/AGN catalyst (the total metal content was 32.04 wt% (29.19 wt% Pd + 2.85 wt% Pt)) (see Fig. 3F–I). The Pd10Pt1/AGN catalyst exhibited excellent catalytic activity and superb durability for the ORR, giving a high mass activity of 1930 mA mgPt−1 (equal to 1185 mA mgPt−1 when the activity of Pd is taken into account) at 0.9 V in 0.1 M HClO4 electrolyte (see Fig. 3J and K). Relying on the remarkable supporting effect of AGNs and the favorable Pt-skin core–shell structure, a highly active and stable ORR electrocatalyst was demonstrated in this study.79
Previously, Adzic et al. reported a novel core-catalyzed coating strategy for epitaxial growth of Pt atomic layers on the surfaces of Pd NPs, inspired by aerobic alcohol oxidation catalyzed by Pd cores (where alcohol is employed as both a reducing agent and solvent).80 In addition, noble metal Au-incorporation is a promising strategy to retard composition-loss and boost the catalytic durability for Au-core/Pt-based-shell structured catalysts (via outward diffusion of Au atoms in the subsurface).61 More recently, inspired by the above-mentioned two design strategies, Qin and co-workers developed a Pd9Au1@Pt/C core–shell catalyst via a Pd9Au1-catalyzed coating route in ethanol solution with carbon black (Vulcan XC-72) as support for the ORR (see Fig. 3L–N).81 The as-synthesized Pd9Au1@Pt NP catalyst presents well-defined core–shell structures superposed on a carbon support (see Fig. 3L), and the thickness of the Pt layers can be controlled by tuning the amount of Pt precursor during synthesis. The Pd9Au1@Pt/C catalyst with 2 atomic Pt layers exhibits the best mass activity for the ORR (see Fig. 3M and N), and excellent stability as evidenced by its even increased half-wave potential after 10000 CV cycles in oxygen-saturated 0.1 M HClO4 electrolyte. This greatly enhanced ORR stability can be attributed to the compressive strain and stabilizing effect of the Pd9Au1 core on the Pt shell.81
Fig. 4 The Co3O4/N-rmGO catalyst (reprinted with permission from ref. 84): (A and B) SEM and TEM images, and (C and D) electrochemical performances. The Co9S8/NHCS-900 catalyst (reprinted with permission from ref. 85): (E and F) TEM images and (G and H) electrochemical performances. The Co3W3C/NPG catalyst (reprinted with permission from ref. 88): (I–L) TEM images and (M–P) electrochemical performances. |
To achieve both high catalytic efficiency and outstanding stability, Wang et al. designedly synthesized monodispersed Co9S8 NPs embedded in N-doped hierarchical carbon nanoflakes (denoted Co9S8/NHCS) as an ORR catalyst, by direct carbonization of metanilic anion-confined 2-D cobalt–aluminum layered double hydroxides (CoAl-LDHs) (see Fig. 4E–H).85 The electrochemical results showed that the Co9S8/NHCS material prepared at 900 °C exhibited superior ORR catalytic activity in both alkaline (0.1 M KOH) and acidic (0.1 M HClO4) electrolytes (see Fig. 4G and H). High onset and half-wave potentials of 0.97 and 0.86 V were obtained in 0.1 M KOH electrolyte, which are comparable to those of commercial Pt/C (1.00 V and 0.85 V). And in 0.1 M HClO4 electrolyte, the Co9S8/NHCS-900 catalyst showed only a 76 mV difference in half-wave potential when compared with commercial Pt/C. The average value of the electron number (n) is 3.95 and 3.65 for alkaline and acidic electrolytes respectively. The durability of Co9S8/NHCS-900 is much better than that of Pt/C in both electrolytes. The high-density Co9S8 NPs with small particle size provide abundant active sites and high catalytic activity. The synchronous carbonization of CoAl-LDHs makes the Co9S8 NPs embedded within the carbon nanoflakes, leading to strong anchoring force and outstanding stability.85
Carbide-based electrocatalysts (e.g., tungsten carbide, WC) have been intensively studied because of their Pt-like behavior and intrinsic catalytic activity for chemical catalysis.86 Especially, bimetallic carbides showed more enhanced electrocatalytic activity for the ORR due to their special electronic structure and the synergistic effect of the dual metal species.87 Recently, Li and co-workers proposed a composite of cobalt–tungsten bimetallic carbide NPs and N/P co-doped graphitized carbon (Co3W3C/NPG) as a highly active and stable non-noble-metal catalyst for the acidic ORR (see Fig. 4I–P).88 Obviously, extremely high-density Co3W3C NPs of about 20 nm size were loaded onto the graphitized carbon support (see Fig. 4I–L). The carbon content of Co3W3C/NPG was determined to be 39.8% by TGA; in other words, the Co3W3C loading onto the NPG support was up to 60.2%. The newly Co3W3C/NPG catalyst presented a high onset potential of 0.92 V, a large limiting current (5.3 mA cm−2) and an especially high half-wave potential (0.79 V) in 0.1 M HClO4 electrolyte (see Fig. 4M–P). The slightly decreased half-wave potential of 5 mV and the high electron transfer number of 3.95 after 8000 cycles indicated that the catalyst undergoes a steady four-electron process in acidic medium. The excellent performances can be attributed to two factors: (i) the Co element in the carbide endows it with Co/N/C and Co/P/C double active sites; and (ii) the W species in the carbide is a synergistic component that boosts the activity of the hybrid catalyst system.88
Recently, He et al. utilized large-surface-area graphene as a support to load high-density WC and Pt NPs, which showed high activity and high stability for the ORR in 0.1 M HClO4 (see Fig. 5A–C).93 A microwave-assisted method was used to synthesize truncated hexagonal pyramid (THP) WC with 5 nm in size on graphene (WCTHP/G) first, then Pt NPs on the WCTHP/G composite with close-contact Pt–WC interfaces were prepared by a chemical adsorption/reduction method (see Fig. 5A). Pt–WCTHP/G showed much higher ORR onset potential (1.052 vs. 0.993 V), half-wave potential (0.942 vs. 0.900 V) and mass activity (528 vs. 137 mA mgPt−1) values compared with commercial Pt/C (see Fig. 5B and C). The enhancement of ORR activity on Pt–WCTHP/G is mainly due to the synergistic effect of Pt and WC, which correlates with the change in the Pt surface d-band center caused by the EMSI on the Pt–WC interfaces. Furthermore, the EMSI can also increase the binding energy of oxygen on Pt–WCTHP/G, thereby enhancing its catalytic activity toward the ORR.93
Fig. 5 The Pt–WCTHP/G catalyst (reprinted with permission from ref. 93): (A) HAADF-STEM images and (B and C) electrochemical performances. The WC/FeS/FePt/NC catalyst (reprinted with permission from ref. 94): (D) TEM images and (E and F) electrochemical performances. The Pd/Co3W3C/GC catalyst (reprinted with permission from ref. 95): (G–J) TEM images and (K–N) electrochemical performances. |
The development of multi-component hybrid catalysts offers great promise to enhance catalytic performance for the ORR. Li and co-workers reported a quaternary hybrid material composed of WC, FeS, FePt alloy and N-doped carbon (NC), i.e. WC/FeS/FePt/NC hybrid architecture, as a high-performance electrocatalyst for the ORR (see Fig. 5D–F).94 Due to the efficient ternary promoting effects from WC, FeS and NC, the FePt alloy electrocatalyst exhibits an excellent mass activity of 317 mA mgPt−1, which is much higher than that of Pt/C catalyst (125 mA mgPt−1) (see Fig. 5E and F). Moreover, superior durability of the WC/FeS/FePt/NC is also demonstrated for the ORR in acidic electrolyte (0.1 M HClO4). This hybrid catalyst has three structural advantages over previous reports:89–91 (i) ultrafine 1-D WC nanorods are prepared by an FeS-regulated strategy; (ii) FePt alloy is formed by in situ transformation on FeS without an external Fe source; and (iii) multiple synergistic effects on the FePt alloy might be in operation relying on the WC, FeS and NC components.
Recently, Pt-free electrocatalysts based on Pd have been proposed as promising candidates for the ORR in acidic electrolyte, due to the inherent catalytic activity and lower cost of Pd compared to Pt. For example, Li and co-workers synthesized a high-performance Pd electrocatalyst (Pd/Co3W3C/GC) for the ORR, which was synergistically enhanced using Co3W3C and graphitic carbon (GC) (see Fig. 5G–N).95 The GC nanosheet was uniformly decorated with the ultrahigh-density and well-proportioned Co3W3C NPs (∼20 nm) and Pd NPs (∼3 nm) (see Fig. 5A and B). The Pd NPs were deposited not only onto the carbon substrate but also onto Co3W3C, indicating a strong interaction between the Co3W3C and Pd NPs (see Fig. 5C and D). It was estimated that more than 30% of the Pd NPs were deposited onto or closely around the Co3W3C, which provided necessary conditions for interface synergistic effects.91 Due to the synergistic effects of Co3W3C and acceleration by GC, the Pd/Co3W3C/GC electrocatalyst showed much higher activity than Pd/GC and Pd/C in a 0.1 M HClO4 electrolyte, and the mass activity of Pd/Co3W3C/GC (110 mA mgPd−1) was comparable to that of commercial Pt/C (107 mA mgPt−1) (see Fig. 5K and L). After the 1000th cycle, a high activity retention of 93% was achieved for Pd/Co3W3C/GC, which was higher than that of commercial Pt/C (82%) (see Fig. 5M and N). These excellent properties make it a highly active and stable Pt-free acidic ORR electrocatalyst. For the sake of convenience, the comparison parameters of different nanoscale ORR electrocatalysts are summarized in Table 1.
Ref. | Name of the catalyst | Type of catalyst | Content of metals | Electrolyte | Onset potential | Half-wave potential | Limited diffusion current density | Specific activity/electron transfer number (n)/H2O2 yield/Tafel slope |
---|---|---|---|---|---|---|---|---|
[50] | Pt/GNP500 | Single metal NPs | 39.2 wt% Pt | 0.5 M H2SO4 | 0.91 V | 0.80 V | 5.9 mA cm−1 | 80 mA mg−1 Pt@0.8 V |
[54] | Pt dendrites/C | Single metal NPs | 37.5 wt% Pt | 0.1 M HClO4 | 1.02 V | 0.92 V | 6.0 mA cm−1 | 251 mA mg−1 Pt@0.9 V |
[63] | FePt/rGO | Metal alloy NPs | 37.0 wt% Pt | 0.5 M H2SO4 | 1.00 V | 0.93 V | 5.6 mA cm−1 | 1960 mA mg−1 Pt@0.9 V |
[70] | PtAg/3DMGS | Metal alloy NPs | 49.6 wt% PtAg | 0.1 M HClO4 | 1.02 V | 0.93 V | 6.0 mA cm−1 | 392 mA mg−1 Pt@0.9 V |
[76] | Pt–Ni@PtD/G | Metal core–shell NPs | — | 0.1 M HClO4 | 0.94 V | 0.83 V | 6.3 mA cm−1 | 610 mA mg−1 Pt@0.9 V |
[79] | Pd10Pt1/AGNs | Metal core–shell NPs | 32.0 wt% PdPt | 0.1 M HClO4 | 1.00 V | 0.89 V | 5.7 mA cm−1 | 1185 mA mg−1 Pt@0.9 V |
[81] | Pd9Au1@Pt/C | Metal core–shell NPs | 19.6 wt% PdAuPt | 0.1 M HClO4 | 0.94 V | 0.89 V | 6.1 mA cm−1 | 239 mA mg−1 Pt@0.9 V |
[84] | Co3O4/N-rmGO | Metal compound NPs | 70.0 wt% Co3O4 | 0.1 M KOH | 0.93 V | 0.83 V | 5.0 mA cm−1 | n = 3.90 |
[85] | Co9S8/NHCS | Metal compound NPs | 19.6 wt% Co9S8 | 0.1 M KOH/0.1 M HClO4 | 0.97 V/0.78 V | 0.86 V/0.63 V | 6.0 mA cm−1/5.0 mA cm−1 | n = 3.95/n = 3.65 |
[88] | Co3W3C/NPG | Metal compound NPs | 60.2 wt% Co3W3C | 0.1 M HClO4 | 0.92 V | 0.79 V | 5.3 mA cm−1 | n = 3.95 |
[93] | Pt-WCTHP/G | Synergistic hybrid NPs | — | 0.1 M HClO4 | 1.05 V | 0.94 V | 6.0 mA cm−1 | 528 mA mg−1 Pt@0.9 V |
[94] | WC/FeS/FePt/NC | Synergistic hybrid NPs | 28.4 wt% Pt | 0.1 M HClO4 | 1.03 V | 0.92 V | 6.0 mA cm−1 | 317 mA mg−1 Pt@0.9 V |
[95] | Pd/Co3W3C/GC | Synergistic hybrid NPs | 30.0 wt% Pd | 0.1 M HClO4 | 0.98 V | 0.87 V | 5.6 mA cm−1 | 110 mA mg−1 Pd@0.9 V |
[118] | Fe–N–C/N-OMC | Single-atom catalysts | 2.9 wt% Fe | 0.1 M KOH | 1.08 V | 0.93 V | 8.1 mA cm−1 | n = 3.93 |
[120] | SA-Fe-NHPC | Single-atom catalysts | 1.25 wt% Fe | 0.1 M KOH | 1.04 V | 0.93 V | 5.9 mA cm−1 | n = 3.92 |
[121] | Commercial Fe–N–C | Single-atom catalysts | — | 0.1 M KOH | 0.97 V | 0.85 V | 7.1 mA cm−1 | n = 3.97 |
[123] | Fe–N4 SACs | Single-atom catalysts | 8.02 wt% Fe | 0.1 M KOH | 1.00 V | 0.84 V | 5.8 mA cm−1 | 1570 mA mg−1http://mailto:Fe@0.85 V |
[124] | Fe–N–C SACs | Single-atom catalysts | 1.5 at% Fe | 0.5 M H2SO4 | 1.03 V | 0.88 V | 4.0 mA cm−1 | H2O2 < 1% |
[125] | Fe–N–C SACs | Single-atom catalysts | 2.5 wt% Fe | 0.5 M H2SO4 | 0.94 V | 0.82 V | 5.4 mA cm−1 | 0.047 A cm−2 at 0.88 ViR-free |
[128] | Co–N4 SACs | Single-atom catalysts | 1.0 at% Co | 0.5 M H2SO4 | 0.93 V | 0.82 V | 4.0 mA cm−1 | H2O2 < 1.5% |
[129] | Fe2N6 DACs | Dual-atom catalysts | 4.9 wt% Fe | 0.5 M H2SO4 | 0.92 V | 0.82 V | 5.0 mA cm−1 | n = 3.96 |
[130] | Co2N5 DACs | Dual-atom catalysts | — | 0.1 M HClO4 | 0.90 V | 0.79 V | 6.0 mA cm−1 | n = 3.97; 7468 mA mgCo2−1 |
[131] | Fe,Co N–C DACs | Dual-atom catalysts | — | 0.1 M HClO4 | 1.06 V | 0.86 V | 6.0 mA cm−1 | n = 3.98 |
[132] | FeCoN6 DACs | Dual-atom catalysts | 10 wt% FeCo | 0.1 M KOH/0.1 M HClO4 | 0.95 V/0.91 V | 0.89 V/0.81 V | 5.7 mA cm−1/5.0 mA cm−1 | n = 3.97 |
[133] | Fe–N4|Co–N4 DACs | Dual-atom catalysts | 3.27 wt% FeCo | 0.1 M KOH/0.5 M H2SO4 | 0.98 V/0.91 V | 0.86 V/0.75 V | 5.7 mA cm−1/5.2 mA cm−1 | n = 3.97; 52 mV dec−1 |
[136] | Co/PC SCCs | Atom cluster catalysts | — | 0.1 M KOH | 1.00 V | 0.92 V | 6.0 mA cm−1 | 66 mV dec−1 |
[137] | CuZn/NC SCCs | Atom cluster catalysts | 0.77 wt% CuZn | 0.1 M KOH | 1.00 V | 0.89 V | 5.2 mA cm−1 | 45 mV dec−1 |
[138] | FeAC@FeSA–N–C | SACs + SCCs | 4.0 wt% Fe | 0.1 M KOH | 1.00 V | 0.91 V | 6.1 mA cm−1 | 61 mV dec−1 |
[139] | Fe–N–C | SACs + SCCs | 2.9 wt% Fe | 0.1 M KOH | 0.98 V | 0.90 V | 3.8 mA cm−1 | n = 3.85 |
[140] | FeSA/FeONC/NSC | SACs + SCCs | 0.25 wt% FeSA | 0.1 M KOH | 0.95 V | 0.85 V | 4.5 mA cm−1 | n = 3.87 |
[142] | Co-SAC/SNPs@NC | SACs + NPs | 5.8 wt% Co | 0.1 M KOH | 0.97 V | 0.90 V | 6.0 mA cm−1 | n = 3.96 |
[143] | CoNPs@Fe–N4–C | SACs + NPs | 0.1 wt% Co | 0.1 M KOH | 1.01 V | 0.92 V | 5.0 mA cm−1 | n = 3.95 |
[144] | FeCo–N–C | SACs + NPs | 6.6 wt% FeCo | 0.1 M KOH | 0.98 V | 0.85 V | 4.8 mA cm−1 | n = 3.97 |
The initially developed non-noble metal ORR electrocatalysts are Me/N/C catalysts (where Me includes transition metals, such as Fe, Co, Ni and Cu, N is chelating atomic nitrogen, and C is sp2 carbon).97 The earliest non-noble metal electrocatalysts were macrocyclic compounds containing nitrogen transition metals, such as phthalocyanines and porphyrins. The common structure of these macrocyclic compounds is their planar configuration MeN4 structure, which is also the most likely active site in the Me/N/C catalyst. Some of the studies have shown that the structures of MeN2 and MeN2+2 may also be the active sites for oxygen reduction. Therefore, the structure formula of the active sites of Me/N/C non-noble metal electrocatalysts can be expressed as: Me/Nx/C (x = 2 and 4, or 2 + 2).98 The early Me/N/C non-noble metal catalysts were usually in the form of composites with transition metal NPs and N-doped carbon, laying more emphasis on the pyrolytic synthesis of catalysts, as well as the effect of the size of metal NPs, the content of N, and the thickness of the graphited layer on ORR performances.
In recent years, since the original concept of “single-atom catalysts (SACs)” (noble metal Pt single atoms on oxide supports) was proposed by the Zhang group,23 numerous noble metal (Pt, Pd, Ag, Ir, etc.) and transition metal (Fe, Co, Ni, Cu, etc.) SACs on carbon supports have been discovered in different electrocatalytic fields.22,99 The formation of M–N4 active moieties (where M includes noble or transition metals) from atomically dispersed metal (M) atoms and the coordination N atoms doped onto carbon supports is the main reason for the stabilization and high ORR activity of these carbon-supported SACs.25,100 In general, the research priorities of carbon-supported SACs (M–N4) ORR electrocatalysts are as follows: (i) adjusting the coordination environment and electronic structures of M centers, (ii) optimizing the nanoscale morphology and pore structures of carbon supports, (iii) increasing the number of metal active centers by increasing the metal density, and (iv) investigating the atomic interaction and synergistic effect of single atoms with different metal densities.
However, some of the current carbon-supported SACs cannot provide enough reaction sites in ORR catalytic reactions due to their low metal loading.44–46 Generally, at least two adjacent metal atoms (i.e., two adjacent active centers) need to cooperate effectively to promote the efficient four-electron mechanism. Therefore, the existing noble metal SACs with low metal loading usually exhibit oxygen reduction by the two-electron mechanism because they cannot cooperate with each other.105 Many carbon nanocomposites with a M/N/C structure, especially those in atomically-dispersed M–N4 (where M = Fe, Co, Ni, etc.) moieties, exhibit ORR catalytic properties that are even comparable to commercial Pt based catalysts.25,99,100 The latest research shows that in M/N/C catalyst, when the dispersed M–N4 single sites are close enough (i.e., when the metal density is large enough), there will be strong interaction between two adjacent single atoms, so as to form the synergetic paired active centers of M–N4 and significantly improve the ORR catalytic performances.104,106 The specific reasons can be attributed to the following aspects: (i) adjacent metal atoms may change the adsorption energy and adsorption state of catalytic species; (ii) the synergistic effect may be conducive to the activation of chemical bonds and reduce the reaction energy barrier; and (iii) the adjacent paired active centers may also change the reaction route of the intermediate and lead to fast kinetics.
However, due to the easy migration and aggregation of active atoms in the preparation process, the high loading of SACs onto carbon supports is still a great challenge.25 Common synthesis methods of M–N–C (in M–N4 moieties) SACs include the process of high-temperature pyrolysis. Increasing the density of active sites only by increasing the concentration of metals usually leads to inevitable metal clusters and metal NPs.99Researchers have achieved some impressive results by using the following methods to achieve highly-dispersed and high-density SACs on carbon supports: (i) using a large number of complexing agents to form coordination bonds with metal ions to physically isolate the metal sources at the molecular scale, ensuring the formation of highly-dispersed single atom sites by subsequent pyrolysis;108 (ii) nanoscale carbon supports with high specific surface area and rich functional groups are used to realize the high-density loading of metal complexes relying on their high pore volume and rich coordinated groups;26 and (iii) high-density M–N4 moieties can be generated by the synchronous pyrolysis of N-containing precursors and metal complexing compounds, where a porous carbon network is generated as an effective cascaded anchoring carrier.99 N-Doped carbon (N–C) is an ideal support for the preparation of high-metal-density SACs, where the N with lone pair electrons can form a M–N4 coordination bond with metal species, which greatly improves the thermal and chemical stability of SACs. The synthetic strategies of N–C materials mainly include: use of (1) nitrogen-containing organic compounds (such as phenanthroline, porphyrin and phthalocyanine); (2) MOFs and their derivatives; (3) N-doped graphene and CNTs; (4) g-C3N4 with high nitrogen content; and (5) rich, cheap and renewable nitrogen-containing biomass.34
In the following, we will introduce the design strategies and preparation methods of high-density SACs on carbon supports through several typical cases according to the “physical synthesis” and “chemical synthesis” categories. For the physical synthesis, ALD and CVD synthetic strategies are analyzed contrastively. Recently, Yan et al. devised a reliable ozone-assisted multicycle ALD technique for the preparation of high-metal-loading Co1/G SACs, which allows the precise tuning of the density of isolated Co single atoms (Co1) on the graphene (G) support (see Fig. 6A–C).109 During ALD cycles, the self-limiting surface reaction ensures that each Co precursor molecule is anchored onto a single active site of the graphene, and the active site (epoxy groups) can be re-generated by the secondary reaction between ozone and the graphene surface (see Fig. 6A). The expected result is that the ALD in different cycles can be used to accurately control the synthesis of SACs with different metal loadings. A series of Co1/G catalysts with Co loadings of 0.4, 0.8, 1.3, 2.0, and 2.5 wt% (see Fig. 6B1–B5) were synthesized by performing 1, 2, 3, 4, and 5 cycles of ozone-assisted Co ALD respectively (see Fig. 5C). The density of Co single atoms loaded onto graphene is closely correlated with the amount of epoxy groups on the support, which further supports the idea that the epoxy groups act as anchor sites for the Co precursors. The ozone-assisted multicycle ALD not only completes a single cycle of ALD, but also regenerates the active sites of chelating single atoms, conducive to the precise tuning of the density of Co single atoms.109
Fig. 6 The Co1/G SACs prepared by ALD (reprinted with permission from ref. 109): (A) schematic diagram of the synthesis, (B) HAADF-STEM images and (C) ALD cycle relational graph. The Fe–N–C SACs prepared by CVD (reprinted with permission from ref. 110): (D) schematic diagram of the synthesis and (E and F) HAADF-STEM images. The Cu–N–C SACs prepared by CVD (reprinted with permission from ref. 112): (G) schematic diagram of the synthesis, (H) HAADF-STEM image and (I) EXAFS spectra. |
In order to increase active site density and site utilization, Jiao et al. proposed a metal-transferred CVD technique to synthesize Fe–N–C by flowing iron chloride (FeCl3) vapor over a Zn–N–C substrate at 750 °C, leading to in situ trans-metalation of Zn–N4 sites into Fe–N4 sites (see Fig. 6D–F).110 Zeolite imidazole framework (ZIF-8) nanocrystals with a uniform size of about 80 nm were first prepared to obtain a Zn–N–C substrate with high-density Zn–N4 sites (see Fig. 6D). After the in situ CVD trans-metalation, carbon-supported Fe-based SACs with high-density Fe–N4 sites were readily achieved (see Fig. 6E and F). These Fe–N4 sites formed by this transformation approach were in the gas-phase and electrochemically accessible, and the catalyst had a high active site density of Fe–N4 (1.92 × 1020 sites g−1) with 100% site utilization.110 Wang et al. lately reported Fe–N–C SACs (Fe–N4 sites) obtained by pyrolysis of ferric (Fe3+) ion-adsorbed porous N-doped carbon derived from ZIF-8, which also showed a high density of accessible surface Fe–N4 sites (2.63 × 1020 sites g−1).111 The high porosity of the ZIF-8-derived N-doped carbon support is a key factor in building Fe–N–C SACs with a high density of accessible-sites.
Because bulk copper can be changed into gaseous species of Cu(NH3)x at high temperature and in an ammonia environment, a thermal emitting and atom trapping strategy was developed to prepare Cu–N–C SACs (Cu–N4 sites) on a pyrolytic carbon support from ZIF-8 (see Fig. 6G–I) by the Li group.112 In the NH3 atmosphere, Cu(NH3)x species were trapped by Zn-vaporized defects in the N-doped carbon, forming isolated Cu sites, and then forming Cu–N4 catalysts (see Fig. 6G). Relatively high metal density and close atomic distance (∼1 nm) were demonstrated for these Cu–N4 catalysts (see Fig. 6H and I). Overall, this work developed an NH3-assisted gas migration strategy (i.e., facile CVD strategy) that enabled the direct conversion of bulk metal to M–N4 single atoms, bringing new hope for large-scale preparation and industrial applications of SACs on carbon supports.
For the chemical synthesis of carbon-supported SACs, the wet-chemistry and pyrolysis synthetic strategies are widely investigated.23 The wet-chemistry method usually includes impregnation, co-precipitation, and electrochemical deposition, and belongs to the “top-down approach” based on ready-made carbon supports with vacancy modification (see Fig. 7A-(1)). This synthetic approach can easily lead to inevitable metal clusters or metal NPs when increasing the concentration of metals, and the subsequent acid treatment is therefore a necessary step.113 On the other hand, the pyrolysis method belongs to the “bottom-up approach”, where SACs are directly prepared from metal node-containing nitrogen and carbon precursors (such as MOFs and COFs) by pyrolysis (see Fig. 7A-(2)). For example, Jiang and co-workers114 recently reported atomically-dispersed Ni metal on N-doped carbon nanotubes (CNTs) with a high Ni loading (20 wt%) via the direct pyrolysis “bottom-up approach” with Ni(acac)2 and C2H8N2 as precursors (see Fig. 7B). Wu and co-workers115 also reported high-density Fe SACs (<1 nm in distance) supported on N-doped carbon nanosheets by a Phen-molecule-confined pyrolysis “top-down approach” with FeCl2, polyetherimide (PI) and g-C3N4 as precursors (see Fig. 7C and D). Importantly, during pyrolysis, the closed Fe ions are directly reduced by carbonization of PEI to form isolated Fe atoms without additional acid treatment.
Fig. 7 (A) Schematic diagram of carbon-supported SACs by chemical synthesis; (B) HAADF-STEM images of Ni–N–C SACs prepared by pyrolysis (reprinted with permission from ref. 114); (C) schematic diagram and (D) HAADF-STEM images of Fe–N–C SACs obtained by pyrolysis (reprinted with permission from ref. 115); (E) XRD patterns, (F) atomic ratios, (G) XPS spectra, and (H) HAADF-STEM images of Fe–N–C SACs obtained by pyrolysis (see (A) for the schematic diagram) (reprinted with permission from ref. 116); (I) schematic diagram of the synthesis and (J and K) HAADF-STEM images of M-SA-NSFC (reprinted with permission from ref. 117). |
Noble metal SACs have high catalytic activity per metal site, but it is usually difficult to achieve a high density of SACs (usually less than 3 wt%), so the overall catalytic activity is limited. Therefore, developing a general synthesis strategy to greatly improve the atom density of noble metal SACs and make the metal loading close to or even exceed the commercial benchmark (e.g., 20 wt% Ir/C) will play a key role in the field of electrocatalysis. In view of this, Xia and co-workers116 developed a universal method lately for synthesizing record high-metal-loading (41.6 wt%) Ir SACs on graphene quantum dots (GQDs) (see Fig. 7A-(3) and E–H). Specifically, when functionalized with amine groups and mixed with IrCl3, GQDs can stably and uniformly diffuse and limit Ir3+ on their surfaces (Ir3+/GQDs-NH2) due to the strong chelation effect between Ir3+and amine groups (see Fig. 7A-(3)). This strong interaction helps GQDs connect with each other and crosslink into a 3-D network structure during the freeze-drying process (see Fig. 7H1). Then pyrolysis was carried out in an ammonia rich atmosphere to obtain a GQD-supported Ir SAC (3.84 at% or 41.6 wt%) with 8 ml of IrCl3 (see Fig. 7E–G). The GQD-supported Ir SAC (Ir–N4 sites) reveals an extremely-uniform and highly-dense distribution of Ir atoms (∼0.5 nm in distance) on GQDs (see Fig. 7H2–H4).
Starting from amine-group functional graphene quantum dots (GQDs-NH2), the authors had the following motives: (i) compared with the carbon support in the “top-down approach”, GQDs are small enough to provide many N-doped active sites for anchoring a large number of isolated metal atoms; and (ii) compared with the organic precursors in the “bottom-up approach”, GQDs, as an intermediate carbon support, do not undergo significant structural evolution during pyrolysis, providing stable and large spacings between metal atoms to avoid aggregation.116 The authors also obtained other noble metal (Pt) SACs or transition metal (Ni) SACs with similarly high metal loadings (32.3 wt% and 15.0 wt% respectively) on GQDs, demonstrating the favorable universality and generality of this GQD-NH2-guided synthetic strategy for high-loading metal single-atom architectures.
Furthermore, the design of tunable coordination environments (e.g., second coordination regulation) for carbon-supported SACs with high metal loading has special significance for catalytic performance regulation. Recently, Zhou et al. reported a multilayer stabilization strategy for constructing M–N4 (where M = Fe, Co, Ru, Ir and Pt) SACs with high metal loading (∼16 wt%) on N, S and F co-doped porous graphitized carbons (i.e., M-SA-NSFC) (see Fig. 7I–K).117 The metal precursors (ferrocene) are embedded into perfluorotetradecanoic acid (PFTA) multilayers and further coated with polypyrrole (Ppy) prior to hydrothermal reaction and pyrolysis (see Fig. 7I). The confinement by the PFTA and Ppy multilayers can efficiently prevent metal precursors from migrating during the pyrolysis process, resulting in the efficient coordination of high-density metal atoms (∼0.5 nm in distance) with N atoms in graphitized carbon (see Fig. 7J and K). This multilayer stabilization bottom-up strategy coupled with the N, S and F co-doping conception is very promising, in terms of abundant metal species, the control of metal loading and second coordination regulation by S (or long-range regulation by F), to explore the potential of high-loading M-SACs and their diversified catalytic applications.117
Because ORR activity is controlled by kinetics and mass transfer processes, in order to better mass diffusion, optimizing the pore structure of catalysts can effectively affect their ORR activity. The rapid transfer of O2 from bulk solution to active centers is a key step in providing high current density.70 The three types of pore structures that can promote the mass transfer of O2 in porous catalysts are macropores (>50 nm), mesopores (2–50 nm) and micropores (<2 nm).69 Each type of pore has a unique function to improve ORR activity: (i) macropores are designed to ensure that reactants quickly pass through the entire dense catalyst layer; (ii) mesopores ensure that electrolytes and reactants enter the active centers (e.g., FeN4 active sites) deeply buried under the surface of the catalyst; and (iii) micropores help in increasing the number of active sites and the total surface area of the catalyst.119
Recently, Feng and co-workers120 designed a novel N-doped hierarchical micro/meso-porous carbon (NHPC)-supported Fe–N–C SAC with densely available FeN4 species by a Zn-mediated silica-template strategy, and applied it to a high-performance alkaline ORR (see Fig. 8A–E). Firstly, the DAP/ZnFe/SiO2 composite was prepared by drying colloidal silica containing 2,6-diaminopyridine (DAP), zinc nitrate and iron nitrate. The obtained DAP/ZnFe/SiO2 was heat treated at 900 °C under nitrogen for 2 hours, then etched in HF followed by secondary pyrolysis in nitrogen to obtain the final SA-Fe-NHPC SAC (see Fig. 8A). There are many mesopores on the Fe-NHPC SAC, with an average diameter of about 12 nm, which is consistent with the size of the silica template (see Fig. 8B). In addition, the HAADF-STEM image of the Fe-NHPC SAC shows that the dense single Fe atoms are well dispersed on the carbon matrix with rich micropores by Zn vaporization (see Fig. 8C). The Fe-NHPC SAC showed unprecedentedly high ORR activity in 0.1 M KOH electrolyte, and the half wave potential was 0.93 V (see Fig. 8D and E), which is much better than those of Pt/C catalyst (0.82 V) and commercial Fe–N–C catalyst (0.85 V) (see Fig. 8F).121 This work opens a new way to improve the density and accessibility of FeN4 species and develop high-performance Fe–N–C ORR catalysts. In addition, Fe–N–C/N-OMC catalysts with N-doped ordered mesoporous carbon (N-OMC) can also provide highly accessible FeN4 active sites and reduce mass transfer resistance.118 Therefore, the Fe–N–C/N-OMC catalysts show extremely high ORR activity in 0.1 M KOH electrolyte, with a half wave potential of 0.93 V and a limited current density of 8.14 mA cm−2. To sum up, the design of mesoporous carbon and high metal loading provide double guarantee for high-performance SACs.
Fig. 8 The SA-Fe-NHPC catalyst (reprinted with permission from ref. 120): (A) schematic diagram of synthesis, (B and C) HAADF-STEM images and (D and E) electrochemical performances. (F) ORR curves of commercial Fe–N–C catalyst (reprinted with permission from ref. 121). The Fe–N4 SACs with various site distances (dsite) (reprinted with permission from ref. 123): (G) HAADF-STEM images, (H) EXAFS spectra, (I) Gibbs free energy, (J) ORR curves and (K) mass activity for various dsite values. |
When the density of single-atom active sites increases to a certain extent, the distance between single atoms will become very small, and the interaction between adjacent active sites becomes a key factor affecting intrinsic activity. And the adjacent single-atom active sites can cooperate to produce an optimized electronic structure, which affects the catalytic activity and catalytic path of SACs in heterogeneous catalysis.122 Previous studies have shown that adjusting the active site density of SACs can significantly improve the electrocatalytic performance of the ORR due to the synergistic effect.104–106 At the same time, the recent breakthrough in the synthesis method of SACs has helped the metal loading to exceed 10 wt%, which exceeds the performance of Pt/C (20 wt%).23 Although high-density SACs have better overall activity for the ORR, the catalytic behavior controlled by the distance between single active sites has not been deeply studied.
With that in mind, Yu and Xiao recently studied and revealed the origin of the enhancement of ORR activity (in 0.1 M KOH electrolyte) of isolated Fe–N4 SACs with the different intersite distances at the sub-nanometer level, by integrating the experimental and theoretical methods (see Fig. 8G–K).123 Atomically-dispersed Fe–N4 sites with controllable density and various site distances (dsite) were prepared on an N-doped carbon substrate via the hydrogel anchoring strategy (see Fig. 8G). When the dsite was controlled at 0.5–2.6 nm, favorable Fe–N4 moieties were obtained without Fe clusters or nanoparticles (see Fig. 8H). The theoretical and experimental results indicate that, when the dsite value is less than 1.2 nm, the strong interaction between adjacent Fe–N4 sites changes the electronic structure and improves the inherent activity of the ORR. This distance-dependent enhanced activity could be maintained until the dsite value was close to 0.7 nm; when the dsite was further reduced, the ORR activity decreased slightly (see Fig. 8I–K). This study determined in detail the kinetic behavior of a single active site and the site distance effect of adjacent single metal atoms, which provides an important opportunity to further understand the inherent catalytic behavior of carbon-supported SACs. And understanding the site distance effect of Fe–N4 catalyst is of great significance to the mechanism of the ORR, which is helpful to realize the full potential of densely distributed SACs in electrocatalysis.123
Platinum group metal-free (PGM-free) catalysts for the ORR with atomically-dispersed Fe–N4 sites have emerged as potential catalysts for acidic polymer electrolyte fuel cells (PEFCs).26 Therefore, it is very important to study the acidic ORR performance (in H2SO4 or HClO4) of carbon-supported Fe–N–C SACs with high Fe–N4 site density. Previously, polyaniline/cyanamide-based Fe–N–C SACs with rich Fe–N4 sites at graphene edges exhibited a half-wave potential of 0.80 V and a limited current density of 3 mA cm−2 in 0.5 M H2SO4 electrolyte.100 The Fe–N–C catalyst with the highest density of Fe–N4 active sites achieved from ZIF-8 precursors also showed respectable ORR activity with a half-wave potential of 0.88 and a limited current density of 4 mA cm−2 in 0.5 M H2SO4 electrolyte.124 Mesoporous silica coated ZIF-8 derived Fe–N–C with dense active sites and efficient mass transport exhibited a desirable half-wave potential of 0.82 V and a larger limited current density of 5.4 mA cm−2 in 0.5 M H2SO4 electrolyte.125 Compared with ZIF-8-derived Fe–N–C prepared via wet chemical synthesis, the CVD method can reduce the pore size of the Kat-Zn (MeIm)2 (Kat) phase to reduce the formation of inert metal aggregates, resulting in a much higher density of Fe–N4 active sites and excellent catalytic performance in 0.5 M H2SO4 electrolyte.126 Besides, previously mentioned high-density Fe SACs on porous carbon nanosheets presented a half-wave potential of 0.80 V and a larger limited current density of 5.5 mA cm−2 in 0.1 M HClO4 electrolyte.115 In general, it is difficult for the ORR half-wave potential of Fe–N–C in acidic electrolyte to reach 0.9 V as in alkaline electrolyte,118,121 so the development of acidic PEFCs with PGM-free catalysts is a challenging task.
On the other hand, carbon-supported Co–N–C SACs with a high-density of Co–N4 active sites are also promising candidates for PGM-free catalysts, by virtue of their high intrinsic activity and immunity to Fenton reactions (for Fe–N–C SACs) that occurred in the proton exchange membrane of fuel cells.26,96 The research on the relationship between the site density of Co–N4 moieties and the activity of Co–N–C SACs is also very necessary for achieving optimized performances in fuel cells. In view of this, the Shui team synthesized a series of Co–N–C SACs with different densities of Co–N4 active sites for a quantitative study of the structure–property relationship.127 It was found that in the low-density region, the battery power density increased slowly and linearly with the Co–N4 site density, while in the high-density region, an accelerated growth trend in terms of power density was observed. These results confirm the fact that M–N–C SACs with limited intrinsic activity can effectively improve the performance of batteries by increasing the density of M–N4 active sites.97,100
More recently, the Shao team synthesized a high-performance atomically-dispersed Co(mIm)-NC catalyst by means of a microporous encapsulation-ligand exchange strategy, where ZIF-8, Co(acac)3, and 2-methylimidazole (mIm) were used as precursors.128 This strategy greatly increases the density of Co–N4 sites and therefore greatly increases ORR catalytic activity in 0.5 M H2SO4 electrolyte. The mass activity of the catalyst increased with the increase of Co content (0.28–1.0 at%), in which the Eonset and E1/2 values of Co(mIm)–NC (1.0 at% Co) were 0.93 V and 0.82 V, which are only 25 mV and 35 mV lower than those of Pt/C catalyst, respectively. In addition, the catalytic activity of this Co–N–C SAC is comparable to that of the Fe–N–C SACs, but the durability is increased by four times. This study provides a promising method to develop high activity and durable Fe-free and PGM-free ORR electrocatalysts (i.e., high-density single atom Co–N4/C) for PEM fuel cells.128
Fig. 9 The Fe2N6 DACs (reprinted with permission from ref. 129): (A) structural schematic diagram, (B and C) HAADF-STEM images and (D–G) electrochemical performances; the FeCoN6 DAC (reprinted with permission from ref. 132): (H) structural schematic diagram, (I) HAADF-STEM image and (J and K) ORR curves in different electrolytes; and the FeN4|CoN4 DAC (reprinted with permission from ref. 133): (L) structural schematic diagram, (M) HAADF-STEM image and (N and O) ORR curves in different electrolytes. |
For example, Wu and co-workers unraveled planar-like Fe2N6 active sites (homonuclear DACs) as a highly efficient ORR catalyst, which showed greatly improved catalytic activity and excellent stability compared to isolated Fe–N4 sites (see Fig. 9A–G).129 The formation of planar-like Fe2N6 structures results from the thermal migration of isolated Fe–N4 sites in hemin molecules (see Fig. 9A). The planar-like Fe2N6 structure presents a high-density and homogeneous distribution of Fe atoms on the carbon framework (see Fig. 9B), and most of the Fe atoms get together to form many Fe2 dimer structures (see Fig. 9C). The planar-like Fe2N6 structure exhibits the highest catalytic activity with a high half-wave potential of 0.84 V (see Fig. 9D) and a small Tafel slope of 82 mV dec−1 (see Fig. 9E) in 0.5 M H2SO4 electrolyte. The Fe2N6 structure shows much enhanced mass activity and half-wave potential compared to single Fe–N4 and Fe NPs (see Fig. 9F). The electron transfer number of the Fe2N6 structure reaches 3.98 below 0.75 V, indicating an efficient four-electron reduction pathway (see Fig. 9G). The planar-like Fe2N6 follows a unique ORR redox transition from initial state Ox–Fe3+–Fe2+ to final state Fe2+–Fe2+, which triggers optimized oxygen intermediate adsorption and strong driving force for O–O bond breaking, thus promoting ORR kinetics and inhibiting side reactions.129
By tuning the Zn/Co ratio in a bimetallic MOF (ZnCo-ZIF8) and subsequent pyrolysis, non-planar binuclear Co2N5 sites with high density were also synthesized and identified (with a Co–Co distance of 0.212 nm and a protruding N between the two Co atoms).130 This homonuclear DAC shows optimized catalytic activity with a halfwave potential of 0.79 V, a limited current density of 6.0 mA cm−2, and an electron transfer number of 3.97 in 0.1 M HClO4 electrolyte. Excitingly, the intrinsic mass activity of Co2N5 sites is as high as 7468 mA mgCo2−1, which is about 12 times higher than that of isolated Co–N4 sites (560 mA mgCo1−1). Theoretical calculations reveal that this novel Co2N5 site exhibits a greatly reduced thermodynamic barrier towards the ORR, thus contributing to the much higher intrinsic activity. This finding opens up a new opportunity to design high-performance M–N–C catalysts, thus pushing the fuel cell industry one step ahead possibly.130
Recently, Wu and co-workers131 reported a host–guest synthesis of a high-density heteronuclear (Fe,Co)/N–C DAC (with FeCoN6 dual sites) on N-doped porous carbon from a Zn/Co bimetallic MOF (ZnCo-ZIF8) with adsorbed FeCl3 molecules. The bonding (Fe–Co) between the Co nodes (host) and adsorbed Fe ions (guest) can be precisely controlled within ZnCo-ZIF8 by a double-solvent method. Compared with Fe SAs/N–C, Co SAs/N–C, commercial Pt/C and those previously reported,129,130 this well-defined (Fe,Co)/N–C DAC exhibits a considerably high ORR activity with a record halfwave potential of 0.86 V, an onset potential of 1.06 V and a limited current density of 6.0 mA cm−2 in 0.1 M HClO4 electrolyte.131 Just like the catalytic behavior of Pt/C, the H2O2 yield of the (Fe,Co)/N–C DAC is below 1.17%, demonstrating the efficient four-electron mechanism (n = 3.98). Besides, excellent power density and long-term stability are also obtained in H2/air fuel cells, suggesting its great potential in shortening the gap between non-noble metal catalysts and commercial Pt/C catalyst.
Considering the high price of MOF-based precursors, it is of great significance to prepare bimetallic (Fe,Co)/N–C catalysts with cheap and extensive raw materials. Back in 2011, Wu et al.10 used commercial carbon black and polyaniline (PANI) as low-cost precursors for the high-temperature synthesis of (Fe,Co NPs)/N–C catalysts, which showed desirable activity with an onset potential of 0.93 V and a halfwave potential of 0.78 V in 0.5 M H2SO4 electrolyte. Recently, Zhang et al.132 reported an efficient synthesis of (Fe,Co)/N–C DACs (with FeCoN6 dual sites) based on a cost-effective route by condensation and carbonization of inexpensive formamide (FA) (see Fig. 9H–K). This general method can be used for mass production (16 g) of DACs with high-loading (∼10 wt% for Fe and Co) and atomically-dispersed FeCoN6 sites (see Fig. 9H and I). Under the same catalyst load, the ORR activity in alkaline (0.1 M KOH) and acidic (0.1 M HClO4) electrolytes is outstanding, and is better than that of commercial Pt/C (see Fig. 9J and K). The halfwave potential in alkaline and acidic electrolytes is 0.89 V and 0.81 V, respectively. More importantly, the extraordinary ORR activity was preserved when these FeCoN6 sites were deposited on inexpensive activated carbon (AC), presenting broad application prospects for implantable electrocatalysts or heterogeneous catalysts.132
The controllable preparation of adjacent dual active centers (M1–N4|M2–N4) is also a very promising approach to high-activity DACs for the ORR due to synergetic effects.134 More recently, Zhang et al.133 reported FeCo–N-doped hollow carbon nanocages (FeCo–N–HCN) with adjacent Fe–N4 and Co–N4 dual active centers as an efficient ORR electrocatalyst (see Fig. 9L–O). The theoretical calculations show that the Fe–Co distance in adjacent M1–N4|M2–N4 active centers is 0.49 nm, which is very close to the value (∼0.5 nm) obtained by experimental observation (see Fig. 9L and M). In 0.1 M KOH electrolyte, FeCo–N–HCN shows much higher ORR activity than Fe–N–HCN, even better than Pt/C, with halfwave potentials of 0.86 V, 0.76 V and 0.85 V, respectively. And the corresponding halfwave potentials are 0.75 V, 0.70 V and 0.84 V in 0.5 M H2SO4 electrolyte on FeCo–N–HCN, Fe–N–HCN and Pt/C. The synergistic effect of adjacent Fe–N4 and Co–N4 dual active centers reduces the energy barrier for the ORR by largely increasing the O–O bond on Fe–N4|Co–N4 DACs. This work provides new insights into and understandings about adjacent dual-active-centers at the atomic level.133
Recently, Zhou et al. devised porous carbon limited Co SCCs (Co/PC SCCs) as an efficient electrocatalyst for the ORR in alkaline electrolyte via a “top-down approach” from carbon black.136 Typically, Co(NO3)2 and phenanthroline were dissolved in ethanol and then a porous carbon black material (Ketjenblak) was added. Because this carbon black has a rich porous structure and Π–Π interaction with metal macrocyclic molecules, the Co-phenanthroline intermediate can be adsorbed in the nanopores. After sintering in an inert atmosphere at 750 °C for 2 h, Co clusters (0.5–1.0 nm) can be confined to the nanopores to form Co/PC SCCs (see Fig. 10A). The as-prepared Co/PC SCCs showed an extremely high initial potential (1.0 V), a half-wave potential (0.92 V), and a remarkable limited current density of 6.0 mA cm−2 in 0.1 M KOH electrolyte (see Fig. 10B). The Tafel slope of Co/PC was as low as 66 mV dec−1, indicating that the ORR kinetics was significantly enhanced, which was closely related to the rich active sites and higher O2 mass transfer effect (see Fig. 10C). In addition, the stability of Co/PC can be significantly improved by the nonporous confinement, where the attenuation of the half-wave potential and the limiting current density of the Co/PC catalyst can be ignored after 10000 CV cycles. Thanks to the water-resistance effect of the nanopores, the highly active Co clusters are confined in specific nanopores and have a stable gas–solid–liquid three-phase reaction region, which enhances the mass transfer capacity, makes full use of the active sites, and also has strong stability due to confinement.136
Fig. 10 The Co/PC SCCs (reprinted with permission from ref. 136): (A) HAADF-STEM image and (B and C) electrochemical performances; the CuZn/NC SCCs (reprinted with permission from ref. 137): (D) HAADF-STEM image and (E and F) electrochemical performances; and the FeAC@FeSA–N–C (reprinted with permission from ref. 138): (G) HAADF-STEM image and (H and I) electrochemical performances. |
Zhou et al. also reported a simple one-step pyrolysis method (so-called “bottom-up approach”) for the preparation of bimetallic CuZn sub-nanoclusters (0.8 nm in mean size) anchored onto N-doped carbon (denoted CuZn/NC SCCs) with rhamnose (C6H12O5) as a carbon source.137 The formation of abundant homogeneous Cu and Zn sub-nanoclusters and a spot of single Cu/Zn sites on carbon carriers can be clearly observed in HAADF-STEM images (see Fig. 10D). An X-ray absorption fine structure test showed that the M–N bond (M = Cu or Zn) and M–M bond existed simultaneously in the catalyst. These N-coordinated Cu and Zn bimetallic structures make CuZn/NC SCCs exhibit high ORR activity in alkaline solution (0.1 M KOH), showing a half wave potential of 0.89 V (see Fig. 10E) and a Tafel slope of 45 mV dec−1 (see Fig. 10F). The ORR activity of CuZn/NC SCCs is even higher than that of commercial Pt/C catalyst. After a 30000 s continuous electrolysis, CuZn/NC SCCs showed a smaller current drop of 12.3% than Pt/C (49.4%), indicating a very high durability of these SCCs. Comprehensive experiments and theoretical calculations approved that the excellent performances of this catalyst can be attributed to the collaboration of the Cu/Zn–N4 sites with CuZn moieties on N-doped carbons.137
For example, Ao et al. recently designed and fabricated a multi-scale Fe–N–C ORR electrocatalyst, where abundant Fe atomic clusters and Fe–N4 single-atom sites are both embedded in an N-doped carbon support (FeAC@FeSA–N–C), by using a covalent organic framework (COF) as the precursor.138 The coexistence of Fe single atoms and Fe nanoclusters was realized by a spatial isolation strategy based on COFs (see Fig. 10G). The FeAC@FeSA–N–C catalyst exhibits excellent electrocatalytic performance for the ORR with a half-wave potential of 0.912 V in 0.1 M KOH electrolyte, which is 68 and 15 mV higher than those of the single-atom Fe–N4 catalyst (FeSA–N–C) (0.844 V) and commercial Pt/C (0.897 V), respectively (see Fig. 10H). The Tafel slope of FeAC@FeSA–N–C was as low as 61 mV dec−1 (see Fig. 10I), which is slightly lower than that of Co/PC SCCs (see Fig. 10C). The DFT calculation showed that Fe–N4 sites are the main active sites, and Fe nanoclusters could further enhance its activity. In addition to the formation of Fe–N bonds, Fe nanoclusters also promote the conversion of pyrrole nitrogen and nitrogen oxide to graphitic nitrogen and pyridine nitrogen due to metal catalysis, which is beneficial for improving the performance of the ORR.138
Lee and Yang also reported an Fe–N–C ORR electrocatalyst with Fe single atoms and Fe nanoclusters co-embedded in N-doped porous carbon by pyrolysis of metal–organic precursors and NaCl.139 The geometric structures of catalytic sites in Fe–N–C are revealed, where the isolated distribution of Fe–N4 sites and Fe nanoclusters with sizes less than 0.5 nm are well deposited on NC. The synergistic enhancement effect of Fe single atoms and Fe nanoclusters results in excellent ORR performances with a half-wave potential of 0.895 V in 0.1 M KOH electrolyte. The DFT calculation showed that, compared with the Fe–N4 site with single structures, the coexistence of Fe nanoclusters on the carbon layer will supply electrons to the Fe–N4 system. Therefore, both the d-band center of the Fe active site and the Fermi level of the system are adjusted, and the neighboring Fe nanoclusters are shown to weaken the binding energies of the ORR intermediates on Fe–N4 sites, hence enhancing both catalytic kinetics and thermodynamics. This study provides new insights into the understanding of the synergies of single atoms and clusters on N-doped carbon ORR electrocatalysts.139
More recently, Lei and co-workers reported a hybrid catalyst (FeSA/FeONC/NSC) with Fe single atoms (Fe–N4 sites) and Fe2O3 clusters (only a few Fe atomic centers) on N,S-co-doped porous carbon, which was obtained by the in situ transformation of Fe-distributed biomass (Spirulina platensis) based on a small molecular nitrogen source-mediated co-pyrolysis strategy.140 Due to the coupling effect with ultra-small Fe2O3 clusters and the favorable reaction site provided by the ultra-thin N,S-co-doped porous carbon skeleton, the FeSA/FeONC/NSC catalyst showed excellent ORR activity and catalytic stability comparable to Pt/C and. FeSA/FeONC/NSC has high Eonset (0.99 V) and E1/2 (0.86 V) values, which are better than those of Pt/C (Eonset = 0.98 V; E1/2 = 0.85 V). The ultra-thin porous structure of FeSA/FeONC/NSC is rich in edge defects, which not only provides a favorable site for the ORR, but also contributes to enhancing ORR activity. Crucially, the high ORR activity is mainly caused by the interaction between the atomic-level dispersed Fe–N4 sites and Fe2O3 clusters embedded in the N,S-mediated porous carbon layers. In this study, a highly efficient catalyst coupled with metal single atoms and homologous oxide clusters was obtained directly from biomass by in situ conversion, which provided inspiration for the synthesis of newly non-noble metal electrocatalysts.140
Recently, Wang et al.142 reported a mixed ORR catalyst with atomically-dispersed Co–N4 sites (Co SAC) and small Co NPs (Co SNPs) co-anchored in N-doped porous carbon nanocages (denoted Co-SAC/SNPs@NC). Co SNPs promote the formation of a graphited layer, which also acts as the support of Co–N4 sites without affecting the highly porous structure of the carbon nanocages. The synergy between Co SAC and Co SNPs and the enhanced graphitization matrix of carbon endowed this mixed catalyst with a high half-wave potential of 0.898 V and a high dynamic current density (JK) of 60.7 mV cm−2 at 0.85 V in alkaline medium. After 20000 cycles, the negative shift in half-wave potential was only 7 mV, which was better than that of Co-SAC@NC with only Co–N4 sites and commercial Pt/C. It may be a feasible method to solve the stability problem, by appropriately introducing metal small NPs into carbon-supported SACs. The small NPs and SCAs can work together to not only improve the activity of the ORR, but also improve the graphitization (high stability) of carbon supports.142
Recently, Jiang et al.143 also reported an Fe–N–C ORR catalyst (with Fe–N4 sites) enhanced by heterogeneous Co NPs (denoted Co@Fe–N4–C) prepared by an auxiliary thermal loading method. The characteristics showed that the Co@Fe–N4–C catalyst had larger specific surface area and higher graphitic N content than single Fe–N4–C. The Co@Fe–N4–C catalyst showed strong ORR activity in 0.1 M KOH electrolyte, where the half-wave potential (E1/2) was 0.92 V, which was much higher than those of single Fe–N4–C (E1/2 = 0.85 V) and Pt/C (E1/2 = 0.90 V). In 0.1 M HClO4 electrolyte, the E1/2 of the catalyst was 0.79 V, which was only 30 mV lower than that of Pt/C (E1/2 = 0.82 V). The DFT calculations confirmed that the strong synergistic effect between Co NPs and Fe–N4 sites provided Co@Fe–N4–C with favorable electronic structures and a local coordination environment. The introduction of Co NPs onto the surfaces of Fe–N4–C materials plays a key role in improving the catalytic activity and stability of the ORR, which provides a new way to prepare efficient Fe–N–C ORR catalysts.143
More recently, Sun and co-workers144 developed a bimetallic FeCo–N–C catalyst with highly active M–NPs and MN4 composite sites (M = FeCo) on N-doped porous carbon (denoted M/FeCo–SA–N–C). This FeCo–N–C catalyst showed the coexistence of Fe/Co NPs and Fe/Co single atoms, indicating that M/MN4 composite sites were successfully constructed. The M/FeCo–SA–N–C catalyst exhibited superior catalytic activity in terms of superhigh onset potential (0.981 V) and half-wave potential (0.851 V) in 0.1 M HClO4 electrolyte, which surpassed those of most M–N–C electrocatalysts in an acidic ORR.88,115,130,132,143 It was also successfully proved that the M/MN4 composite sites provided excellent stability to the M/FeCo–SA–N–C catalyst in acidic electrolyte. The synergistic effect between M–NPs and MN4 may play a crucial role in the boosted ORR performance through the construction of M/MN4 composite sites. The DFT calculations indicated that the M–NPs can increase the local charge density of MN4, and subsequently enhance O2 adsorption and elongate O–O bonds, resulting in the facile cleavage of the O–O bond. This work may present new highly active M/MN4 composite sites for catalyzing the ORR in acidic medium.144
On the other hand, transition metal SACs with MN4 sites can synergistically promote single noble metal (or its alloy) NPs for the ORR in acidic medium.145,146 For example, He and Mu145 reported a Pt@Co SAs-ZIF-NC catalyst by isolation of Pt NPs with CoN4 sites on ZIF-based N-doped carbon. In 0.1 M HClO4 electrolyte, the Pt@Co SAs-ZIF-NC showed a half wave potential (0.917 V) that is better than that of commercial Pt/C (0.868 V), and its mass activity (480 mA mgPt−1) at 0.9 V is three times that of Pt/C (160 mA mgPt−1). More recently, Wu and co-workers146 also reported that Fe SACs with FeN4 sites on N-doped carbon can significantly promote the ORR activity of Pt NPs and Pt3Co alloy NPs. Pt/FeN4–C and Pt3Co/FeN4–C showed mass activities of 451 mA mgPt−1 and 720 mA mgPt−1 at 0.9 V, respectively. The DFT calculation predicted that the synergy between Pt NPs and the surrounding FeN4 sites can weaken the adsorption of O2 on the Pt plane, thus enhancing the intrinsic activity of the Pt catalyst. In general, transition metal single atoms can improve the activity of noble metal catalysts, and finally achieve the goal of reducing the use of noble metal. For the sake of convenience, the comparison parameters of different atomic-level ORR electrocatalysts are also summarized in Table 1.
Fig. 11 (A) The relative distance of metal particles or atomic sites, (B) the diffusion models of nanoparticle arrays at different potential sweep rates (reprinted with permission from ref. 147), and (C–E) schematic diagrams of atomic site electrostatic interaction (reprinted with permission from ref. 148). |
For nanoparticle catalysts, method (i) (relative distance method) is more objective and convenient to calculate or evaluate the metal density, due to their different particle diameters and easily distinguishable structures. Based on the previous case analysis, it can be found that when the relative distance is close to or less than 1, the distribution of nanoparticles on the carbon support is very close, and these catalysts also show high mass catalytic activity (see Fig. 2–5 for details). For atomic-level catalysts, both method (i) (relative distance method) and method (ii) (average number method) can be used under high resolution HAADF-STEM. Particularly, considering that the site sizes of metal atoms are very close, we can use the actual site distance to evaluate the metal density of atomic-level catalysts. In general, when the average distance of atomic sites is equal to or less than 1 nm, the distribution of metal atoms in the carbon carrier is very dense (see Fig. 7 for details) and the catalytic performance is obviously dependent on the site distance (see Fig. 8 for details).
For nanoparticle systems, high-metal-density electrocatalysts can lead to distinctive ion diffusion characteristics in extensive electrochemical processes. Fig. 11B shows the surface-density-dependent diffusion models of nanoparticle arrays at different potential sweep rates: (left) high sweep rate, (middle) medium sweep rate and (right) very low sweep rate.147 For the high sweep rate, the diffusion layer thickness is much smaller than the average distance between adjacent particles; for the medium sweep rate the diffusion layers of adjacent particles overlap for a high particle density; and for the very low sweep rate steady-state diffusion is reached for all density samples. These electrochemical characteristics have positive guiding significance in the design of high-performance electrocatalysis, where the overlap effect of the diffusion layer thickness of adjacent particles may induce unexpected electrocatalytic synergistic effects for high-metal-density electrocatalysts.
For atomic-level systems, high-metal-density electrocatalysts can also lead to distinctive electronic properties and catalytic activity. Fig. 11C–E show the structural model and surface-density-dependent atomic site electrostatic interaction of Pd1/CeO2 single atom catalyst.148 Due to the cumulative enhancement of CeO2 reducibility, the specific activity of a single Pd atom supported by CeO2 increases linearly with the increase of Pd atom density. With the increase of surface Pd density, the long-range electrostatic footprints (∼1.5 nm) around each Pd site overlap each other, resulting in a deviation from the constant specific activity observed. The results show that the specific catalytic activity of reducible oxide supported single atom catalysts can be adjusted by changing the surface density of a single metal atom. These theoretical models provide help with the development of high specific activity and high metal density atomic-level catalysts.
When the distance between two active metal atom centers is reduced to the subnanometer level, the catalytic behavior will be significantly affected because of the site interaction effect. High-density atomically-dispersed metal catalysts (including SACs, DACs, and SCCs) often exhibit more significant catalytic properties than the sparse counterparts due to the synergistic effect of dense atomic sites. M–N–C (where M includes transition metals and noble metals) ORR catalysts with high active site density can generate higher activity by exposing the inaccessible M–N4 active sites and strengthening the mass transport. In order to ensure the mass transport and high activity of high-metal-density SACs, it is very necessary to develop carbon supports with high surface area and mesoporous structure, which facilitates ion transfer and improves their catalytic performances. Besides, the high-density bimetal sites dispersed on N-doped carbon (M1M2Nx DACs) can form different adjacent active sites and improve the activity and stability of the catalyst through synergistic catalysis. The construction of dual active sites provides a new opportunity for high-performance ORR catalysts, which can not only develop more combinations of coordination environments, but also lead to the enhancement of two different metal sites of high-density atomically-dispersed catalysts. Preparation of cluster catalysts (SCCs) and the combination of SACs with SCCs/NPs are the significant complement strategies for the design of high-density ORR catalysts with improved catalytic performances.
The ORR performance of high-metal-density M–N–C (M = Fe, Co, Ni, etc.) catalysts (including SACs, DACs, and SCCs) in the kinetic region is very close to that of Pt-based catalysts, but there are still great challenges for these non-noble metal catalysts, especially under acidic conditions. Because of their sensitive physical and chemical properties, especially in acidic environments, these transition metal elements have poor corrosion resistance. Therefore, high-density transition metal M–N–C catalysts (especially Fe–N4 SACs) still face great challenges in the practical application of PEMFCs, due to their under-stable characteristic and potential Fenton oxidation. More catalytic systems with high activity, high stability and four-electron selectivity still need to be found. Rational design of metal cluster catalysts, including dimers, trimers, and larger metal clusters, is also an important research direction to overcome the defects of SACs. At present, the central metal atom of most high-density atomically-dispersed metal catalysts only coordinates with the N atom in the carbon substrates. In the subsequent research, the coordination effect of other elements such as S, P, B and O can be considered to adjust the electronic structure of the central metal atom, so as to obtain a more efficient and stable ORR electrocatalyst. Particularly, some reliable synthesis strategies (e.g., mechanochemistry and heat migration strategies) need to be explored to realize the batch production of SACs with high metal density and high stability on different supports.
Carbon-supported ORR electrocatalysts (including nanoparticles and atomic-level architectures) are always faced with problems of carbon corrosion of the support and the resultant catalyst instability in practical application. Especially under the catalysis of ultrafine metal species and high-potential or acidic oxidation conditions, the amorphous component in conventional carbon supports (e.g., porous carbon and acetylene black) shows a fast electrochemical corrosion rate in the operating state of fuel cells. Based on this, it is necessary to develop new-type high-crystallinity carbon with or without ceramic support materials (e.g., conducting metal oxides, carbides, and borides) with high electrochemical and thermodynamic stability, in order to accelerate the progress of both nano-structured and atomic-level ORR electrocatalysts in practical application of fuel cells.
This journal is © The Royal Society of Chemistry 2022 |