Thank you for visiting nature.com. You are using a browser version with limited support for CSS. To obtain the best experience, we recommend you use a more up to date browser (or turn off compatibility mode in Internet Explorer). In the meantime, to ensure continued support, we are displaying the site without styles and JavaScript.

# Exceptionally active iridium evolved from a pseudo-cubic perovskite for oxygen evolution in acid

## Abstract

Exploring robust catalysts for water oxidation in acidic electrolyte is challenging due to the limited material choice. Iridium (Ir) is the only active element with a high resistance to the acid corrosion during water electrolysis. However, Ir is rare, and its large-scale application could only be possible if the intrinsic activity of Ir could be greatly enhanced. Here, a pseudo-cubic SrCo0.9Ir0.1O3-δ perovskite, containing corner-shared IrO6 octahedrons, is designed. The Ir in the SrCo0.9Ir0.1O3-δ catalyst shows an extremely high intrinsic activity as reflected from its high turnover frequency, which is more than two orders of magnitude higher than that of IrO2. During the electrochemical cycling, a surface reconstruction, with Sr and Co leaching, over SrCo0.9Ir0.1O3-δ occurs. Such reconstructed surface region, likely contains a high amount of structural domains with corner-shared and under-coordinated IrOx octahedrons, is responsible for the observed high activity.

## Introduction

The electricity from renewable energy sources, such as wind and solar power, has been showing a gradual proportional increase in global energy infrastructure1. However, due to the intermittent availability, the storage of the electric energy by these sources becomes pivotal. The conversion of the electricity into hydrogen fuel is expected to be one of the most efficient storage ways due to the high energy density of hydrogen fuel. Water electrolysis is a promising strategy to realize such energy conversion. The alkaline condition has been popular for industrial water electrolysis, while the acidic electrolyte condition is not. This is mainly due to the limited choices of robust anode catalysts in acidic condition during the oxygen evolution reaction (OER). In fact, the acidic condition offers a high proton concentration and thus enables much faster reaction kinetics of hydrogen production2,3. An ideal anode catalyst in acid should exhibit both high catalytic activity and high tolerance to the severe acidic corrosion at a high anodic potential. To date, the iridium oxides have been found high in stability in harsh acidic environment4,5. Due to the high cost and scarcity of Ir, great efforts have been made to develop novel Ir-based materials for water oxidation with high efficiency, e.g., a high activity normalized to the material surface area (intrinsic activity) and, more importantly, a high turnover frequency (TOF) for Ir6,7,8,9,10,11.

Recently, several Ir-based perovskites were reported as highly active catalysts for OER12,13,14,15. The perovskite is a type of oxide with a general formula of ABO3, where A represents alkaline-earth-metal or lanthanide and B represents active transition metals. Among these perovskite catalysts, a SrIrO3 perovskite, with reconstructed surface was found with the highest intrinsic activity (normalized to its surface area) for catalyzing OER in acidic environment to date13. Nevertheless, the synthesis of such SrIrO3 catalysts requires special tools or conditions, such as a pulse laser deposition (PLD) equipment16 or a high pressure (~5 GP) for solid state synthesis17, which could hinder the practical application of such catalyst. In addition, the key surface reconstruction step in this PLD-SrIrO3 is likely time-consuming because a ~30 h electrochemical activation process is required.

Here, we design a pseudo-cubic SrCo0.9Ir0.1O3−δ material with an orthorhombic structure. In this design, the Ir and Co co-share the octahedral site and all octahedrons are corner shared. To form a comparison, we investigate a monoclinic SrIrO3 (m-SrIrO3) perovskite, which adopts a highly distorted 6H BaTiO3 structure with mixed corner-shared and face-shared IrO6 octahedrons18,19. We show that the intrinsic activity (TOF) of Ir from SrCo0.9Ir0.1O3−δ is approximately two orders of magnitude higher than the m-SrIrO3 and more than one order of magnitude higher than the benchmark PLD-SrIrO3. The Sr and Co leach from SrCo0.9Ir0.1O3−δ surface during electrochemical tests. As a result, a highly active surface IrOx layer likely contains a high amount of corner-shared and under-coordinated IrOx octahedrons without long-range ordering, and is responsible for the observed superior activity of SrCo0.9Ir0.1O3−δ.

## Results

### Structure characterization

Figure 1a–c shows the crystal structures of PLD-SrIrO3, pseudo-cubic SrCo0.9Ir0.1O3−δ, and m-SrIrO3. In PLD-SrIrO3 and pseudo-cubic SrCo0.9Ir0.1O3−δ, all IrO6 octahedrons are corner-shared. Nevertheless, in m-SrIrO3, corner-shared and face-shared IrO6 octahedrons are alternatively arranged. Both m-SrIrO3 and SrCo0.9Ir0.1O3−δ samples were synthesized with a classical solid state method, which is easily accessible for large scale preparation. Figure 1d includes the scanning electron microscope (SEM) images from m-SrIrO3 and SrCo0.9Ir0.1O3−δ samples. The corresponding Brunauer–Emmett–Teller (BET) surface area for these two samples are also presented. The SrCo0.9Ir0.1O3−δ has a lower BET surface area due to its relative large particles. A m-SrIrO3 with a space group (SG) of C 2/c and a SrCo0.9Ir0.1O3−δ with SG of P nma are confirmed based on their X-ray diffraction (XRD) patterns (the refined results are shown in Fig. 1e and Supplementary Table 1). Figure 1f, g presents HRTEM images taken from m-SrIrO3 and SrCo0.9Ir0.1O3−δ. The corresponding inverse fast Fourier transformed (FFT) images are taken from white square box regions. The measured interplanar distances from inverse FFT images correspond well with the results from XRD refinement, which are in brackets. Selected area electron diffraction (SAED) patterns are also presented. All patterns can be well indexed based on the XRD refinement results, indicating the formation of m-SrIrO3 and SrCo0.9Ir0.1O3−δ with high purity.

### Activity evaluation

The activities of SrCo0.9Ir0.1O3−δ, m-SrIrO3 and commercial IrO2 for the OER were then evaluated in a perchloric acid solution (0.1 M, pH = 1.08). The measured specific activity (mA cm−2 normalized to BET surface area), representing the intrinsic activity of a catalyst20, is shown in Fig. 1h. The activity for the PLD-SrIrO3 prepared with PLD method from literature is also presented for comparison13. The calculated specific activity of IrO2 is similar to the previously reported values7. A higher specific activity, approximately one order of magnitude higher than that of IrO2, is obtained from the m-SrIrO3. For instance, at a potential of 1.5 V (vs. RHE), a specific current density of ~1 × 10−2 mA cm−2 and ~0.2 mA cm−2 is recorded for IrO2 and m-SrIrO3, respectively. However, such activity is much inferior to that of the PLD-SrIrO3. Moreover, different from the reported PLD-SrIrO3 catalyst, the m-SrIrO3 did not show a gradually increased activity during the successive test (Supplementary Figure 1). As a result, the specific activity of the m-SrIrO3 is more than one order of magnitude lower than that from the PLD-SrIrO3 catalyst (stabilized activity at 2 h). This activity difference indicates that the pseudo-cubic structure is a key factor to determine the intrinsic activity of SrIrO3. On the other hand, regardless of the low Ir atom ratio in the lattice, the specific activity of SrCo0.9Ir0.1O3−δ is more than one order of magnitude higher than that from m-SrIrO3 and comparable with the reported initial activity of PLD-SrIrO3. Interestingly, such specific activity is just 2–4 times lower than the final specific activity of PLD-SrIrO3, which hints the intrinsic activity of Ir over the surface of SrCo0.9Ir0.1O3−δ is higher than that of Ir over the surface of PLD-SrIrO3. We caution that the Co in SrCo0.9Ir0.1O3−δ does not contribute to the observed superior activity of SrCo0.9Ir0.1O3−δ for its high solubility in the acidic electrolyte (Supplementary Figure 2). Additionally, as discussed in the following sections, a rapid dissolution of Sr and Co is expected in acidic electrolytes. The stable activity of SrCo0.9Ir0.1O3−δ during cycling test, shown in Supplementary Figure 2, also confirms that the measured OER current contributed by Sr and Co leaching is negligible. In addition, an estimated maximum current due to Sr and Co leaching in initial 5 cycles is more than two orders of magnitude lower than the measured OER current from SrCo0.9Ir0.1O3−δ (see the estimation of the current due to Sr and Co leaching in the Methods). Figure 1i presents the TOF of Ir from IrO2, m-SrIrO3, and SrCo0.9Ir0.1O3−δ. Three cases, including Ir at outermost surfaces (upper limit), of Ir from reconstructed surface regions (the surface reconstruction over catalysts will be discussed later) and all Ir from the bulk (lower limit), were considered for TOF calculations. Calculation details are presented in Methods. Among them, the TOF of Ir by considering the effect of surface reconstruction should be the most reliable for comparing the intrinsic activity of Ir from different materials. From Fig. 1i, at an overpotential of 270 mV (1.5 V vs. RHE), the Ir in SrCo0.9Ir0.1O3−δ is found with a high TOF of 2.56 ± 0.15 s−1, which is more than 10 times and ~75 times higher than PLD-SrIrO3 (~0.2 s−1) and m-SrIrO3 (0.034 ± 0.001 s−1), respectively. It confirmed that the observed superior activity of SrCo0.9Ir0.1O3−δ is attributed to the formation of highly active surface Ir species.

### Surface reconstruction

For IrO2, it has been reported with a high resistance to acidic corrosion21. However, it is unlikely that m-SrIrO3 and SrCo0.9Ir0.1O3−δ can keep their original structure in strong acidic condition due to the thermodynamic instability of Sr and Co. The surface structure evolution of m-SrIrO3 and SrCo0.9Ir0.1O3−δ is then evaluated by HRTEM. Moreover, since the performance of both SrCo0.9Ir0.1O3−δ and m-SrIrO3 become stable in a few cycles (within 5 cycles), the surface structures of these two materials after 5 cycles were also investigated. The HRTEM images from pristine and cycled m-SrIrO3 are presented in Fig. 2a. No apparent structural reconstruction can be observed from the surface of pristine m-SrIrO3, while a surface reconstruction from cycled m-SrIrO3 is observed with a depth of approximately 5 nm. By comparing the FFT images from bulk and surface, such reconstructed surface is likely amorphous with no long-range order. We caution that nanoparticles (~2 nm) emerge from the bulk of the m-SrIrO3 after a short-term electron beam illumination, and such nanoparticles were determined to be Ir (Fig. 2b). Similar behaviors have also been observed in a few other Ir-based oxides22,23. In spite of the formation of Ir nanoparticles, the crystallinity of the surfaces of m-SrIrO3 was not affected during the period of TEM analysis. Figure 2c presents the HRTEM images from pristine and cycled SrCo0.9Ir0.1O3−δ. The surface region from pristine SrCo0.9Ir0.1O3−δ with a depth of 1–3 nm is amorphous. Such slight surface amorphization in pristine SrCo0.9Ir0.1O3−δ likely occurs during the TEM sample preparation process, in which the sample is ultrasonically dispersed in ethanol solution. After electrochemical cycling, an apparent surface structure reconstruction is observed for SrCo0.9Ir0.1O3−δ with a depth of approximately 10 nm. Similar to the case in m-SrIrO3, such reconstructed surface of SrCo0.9Ir0.1O3−δ is also likely amorphous with no long range order. The FFT image from bulk of SrCo0.9Ir0.1O3−δ can be well indexed, indicating the bulk maintains its initial crystal structure. In combination with the observed reconstructed surface layers, the in situ reconstructed surface layers are responsible for the observed activities from the m-SrIrO3 and the SrCo0.9Ir0.1O3−δ.

The X-ray photoelectron spectroscopy (XPS) was then performed to study the surface chemical states in m-SrIrO3 and SrCo0.9Ir0.1O3−δ before and after 5 cyclic voltammetry (CV) cycles. The XPS of Sr_3d from the m-SrIrO3 are shown in Fig. 2d. The fitting parameters are listed in Supplementary Table 2. To compare the relative composition change, all Sr_3d spectra are normalized based on corresponding Ir contents. In Fig. 2d, an apparent decrease in Sr_3d signal is observed from cycled m-SrIrO3, indicating a Sr leaching during the test. Moreover, although the Sr_3d signal from pristine m-SrIrO3 and cycled m-SrIrO3 can both be fit with two doublets, their profile is totally different. Specifically, both doublets in the pristine m-SrIrO3 should be mainly related to the Sr from m-SrIrO3 lattice as two low binding energy of 130.55 and 131.81 eV for the 3d5/2 peak are obtained24. In addition, a relative larger full width at half maximum (FWHM) for the second doublet (marked in green) indicates it also includes a small amount of surface Sr components, such as SrO, SrCO3, and Sr(OH)2, with higher binding energies (above 133 eV)25. In the cycled m-SrIrO3, the first doublet (marked in yellow) with a low binding energy of 131.15 eV should still be related to lattice Sr. More surface Sr components seem formed because the second doublet shifts to a higher binding energy of 132.62 eV for the 3d5/2 peak. In combination with the HRTEM results, the increased amount of surface Sr components is likely related to the leached bulk Sr, which re-deposits on the electrode surface. Figure 2e shows the XPS of Sr_3d and Co_2p from pristine and cycled SrCo0.9Ir0.1O3−δ samples. The fitting parameters for Sr_3d spectra are listed in Supplementary Table 3. In the spectrum of Sr_3d from pristine SrCo0.9Ir0.1O3−δ sample, only one doublet at 131.83 eV for the 3d5/2 peak is observed, which should be mainly related to lattice Sr. Importantly, a severe Sr leaching is observed from the cycled SrCo0.9Ir0.1O3−δ sample as the Sr_3d signal is almost invisible just after 5 CV cycles (time of duration: ~10 min). Similarly, a fast cobalt leaching is observed from the surface of cycled SrCo0.9Ir0.1O3−δ because the XPS signal of Co_2p from cycled SrCo0.9Ir0.1O3−δ sample is almost invisible. As summarized in Fig. 2f, after 5 cycles, approximately 50% Sr dissolved from the surface of m-SrIrO3. In the reported PLD-SrIrO3 catalyst, approximately 75% Sr is expected to leach from its surface after 30 min of electrochemical OER testing13. Although the leaching degree of Sr from the surface of m-SrIrO3 is slightly lower than that in PLD-SrIrO3, considering the much inferior activity of m-SrIrO3, the initial pseudo-cubic structure with corner-shared IrO6 octahedron is critical for a highly active Ir site after the cation leaching. This corresponds well with the previous calculation results13, which found the reconstructed surface with a structure similar to IrO3 or anatase IrO2 is active to catalyze OER. Different from m- and PLD-SrIrO3, the surface region of SrCo0.9Ir0.1O3−δ loses approximately 92% Sr + Co after 5 CV cycles. This Sr and Co leaching in acid from SrCo0.9Ir0.1O3−δ likely causes the obvious surface reconstruction on SrCo0.9Ir0.1O3−δ. More importantly, we can confirm the formed amorphous surface Ir-related species after Sr and Co leaching are responsible for the measured activity of m-SrIrO3 and SrCo0.9Ir0.1O3−δ.

### Understanding Ir from reconstructed surfaces

Ir from IrO2, m-SrIrO3, and SrCo0.9Ir0.1O3−δ were investigated by XPS to gain more information about the Ir in reconstructed surfaces and the Ir_4f spectra from the three samples before and after electrochemical tests are given in Fig. 3a. The Ir_4f spectra from the IrO2 are studied first. Distinctive asymmetric tail can be observed from the peaks in the two spectra and is reported related to the screening response of 5d conduction electrons26. Based on the previous studies, both Ir_4f spectra can be fitted with two doublets and an additional single satellite peak. The fitting results are listed in Supplementary Table 4. The Ir_4f7/2 peak with a binding energy of 61.61 and 61.63 eV is found from the first doublet (marked in yellow) in the pristine IrO2 and the cycled IrO2, respectively. The observed binding energies are within the reported ranges for Ir_4f7/2 peak in IrO2 (61–62 eV). The second wide doublet (marked in green), with an energy shift of approximately 1 eV as compared with the first doublet, should be related to the shake-up satellites of the first doublet27. The spin–orbit splitting in both doublets is 2.98–2.99 eV, which is also close to the reported values27,28,29. The additional single satellite at 67.6 eV for pristine IrO2 or at 67.76 eV for the cycled IrO2 is related to the localized non-bonding states27,28. From the fitting results, the Ir 4f spectra from the IrO2 is almost unchanged after the electrochemical cycling, confirming a highly stable surface structure of IrO2 during OER in acidic environment.

The Ir_4f spectra from the m-SrIrO3 were also fit to explore the change of surface Ir after electrochemical cycling. The fitting parameters are listed in Supplementary Table 2. Both spectra can be fit with two doublets. In the pristine m-SrIrO3, the Ir_4f7/2 peak from the first doublet located at a low binding energy of 60.33 eV, which is generally considered as the signal of Ir metal30. However, Ir metal is unlikely to exist in the sample as a long-term high temperature calcination is required in the solid state method for sample preparation. Considering the Ir in the m-SrIrO3 is 4+ for charge neutrality, it is rational to define this first doublet comes from Ir4+. Moreover, in the previous studies, the Ir_4f7/2 peak of Ir4+ from PLD-SrIrO3 is found with a binding energy located in between 61.8 and 62.6 eV13. The much lower binding energy observed in the m-SrIrO3 indicates the XPS signal of Ir is strongly related to its local structural environment. The second doublet has a binding energy ~1.4 eV higher than that of the first doublet. This energy shift between two doublets is similar to the cases observed in rutile IrO2 and PLD-SrIrO3, indicating the second doublet should be shake-up satellites. After electrochemical cycling, apparent shifts of the two doublets in the Ir_4f spectra to higher binding energy are observed. The Ir_4f7/2 in the first doublet is at 61.2 eV, which is approximately 0.9 eV higher than that in pristine m-SrIrO3. This moderate energy shift is different from the case observed in PLD-SrIrO3, in which the Ir_4f7/2 in the first doublet is almost unchanged irrespective of the Sr leaching during electrochemical testing13. The Sr leaching in m-SrIrO3 probably influences the chemical state of Ir and thus certain SrxIrOyHz (x < 1) phase(s) may form, considering a high amount of Sr remains in the surface. The Ir_4f7/2 peak from the second doublet has a high binding energy of 63.35 eV, which, however, cannot be solely treated as the shake-up satellites because an energy shift of approximately 2.2 eV, relative to the first doublet, is observed. Such energy shift is much larger than those (1–1.6 eV) observed in rutile IrO2, PLD-SrIrO3 as well as the pristine m-SrIrO3. The unusual energy shift of this second doublet hints the formed surface is very complex and multiple phases can exist.

The profile of Ir_4f spectra from the pristine SrCo0.9Ir0.1O3−δ is different from those observed in rutile IrO2 or SrIrO3 phases. The fitting parameters are listed in Supplementary Table 3. The fitting results revealed an Ir_4f7/2 peak at approximately 59.7 eV for the first doublet. This Ir_4f7/2 peak with a large FWHM likely represents the mixed Ir4/5+ in SrCo0.9Ir0.1O3−δ since a low binding energy is also observed in the pristine m-SrIrO3 phase. The second doublet with a binding energy ~2 eV higher than the first doublet cannot be solely treated as the shake-up satellite. Certain Ir specie(s) from SrCo0.9Ir0.1O3−δ surface can exist, and its identification is beyond the scope of this study. After electrochemical cycling, the Ir_4f spectra from SrCo0.9Ir0.1O3−δ can be well fit with two doublets. A binding energy of 61.0 eV is observed for the Ir_4f7/2 peak in the first doublet. Such peak position is more than 1 eV higher than that in pristine SrCo0.9Ir0.1O3−δ, but ~0.6 eV lower than that in rutile IrO2. The second doublet in cycled SrCo0.9Ir0.1O3−δ shifts ~1.5 eV to higher binding energy, which then can be related to the shake-up satellites. As a result, certain IrOxHy phase may form over the SrCo0.9Ir0.1O3−δ surface as Sr and Co have leached out. Previously, some amorphous IrOx phases have also been prepared for a higher activity than crystallized rutile IrO222,31,32. However, the Ir_4f spectra from amorphous IrOx and crystalline rutile IrO2 always have similar peak positions and profiles27,31,32,33. Moreover, the influence of Sr on Ir_4f in XPS can be excluded since there is almost no Sr in the surface region after five cycles (Fig. 2e). In fact, the signals of Sr and Co in XPS from the surface region of SrCo0.9Ir0.1O3−δ disappeared completely after 10k cycles (Supplementary Figure 3a & b). That indicates only Ir remaining in the surface region. Therefore, the possibility that the residual Sr caused the difference (Fig. 3a and Supplementary Figure 3c) in Ir_4f between cycled SrCo0.9Ir0.1O3−δ and hydrous IrOx can be excluded. As a result, the formed IrOxHy phase in SrCo0.9Ir0.1O3−δ is different from previous amorphous IrOx phases.

For a better understanding of the formation and evolution of the surface in m-SrIrO3 and SrCo0.9Ir0.1O3−δ, we further studied the CV cycles measured from SrCo0.9Ir0.1O3−δ and m-SrIrO3. Since Ir hydrous oxide can be formed on metal Ir through electrochemical cycling, the CVs of Ir metal was also recorded for comparison34. As shown in Fig. 3b, different redox behaviors are observed for Ir from these three catalysts. For SrCo0.9Ir0.1O3−δ, three oxidation peaks, representing Ir3+/4+ (~1 V), Co2+/3+ (~1 V), and Ir4+/5+ (~1.2 V), can be observed at the first cycle35,36. In the following cycles, the Co peak disappeared and only the two peaks belonging to Ir become remarkable, which is probably due to the dissolution of Co as well as the formation of IrOxHy species in the surface region. The intensities of the two Ir-related oxidation peaks simultaneously increased, which should be related to the increased degree of surface reconstruction. Interestingly, the surface reconstruction process likely stopped after 5000 cycles since the 5,000th cycle almost overlapped with the 10,000th cycle. The peak at ~1.2 V indicates the oxidation of Ir4+ to Ir5+ is greatly facilitated over the SrCo0.9Ir0.1O3−δ surface. For m-SrIrO3, two oxidation peaks, representing Ir3+/4+ (~0.8 V) and Ir4+/5+ (~1.2 V), can be observed. However, unlike SrCo0.9Ir0.1O3−δ, the redox of Ir3+/Ir4+ is dominant on m-SrIrO3. As for Ir metal, one distinctive oxidation peak at ~1 V is observed after ~1000 cycles, indicating the formation of surface Ir hydrous oxide. Such broad oxidation peak likely due to successive oxidation of Ir3+ to Ir5+35. By comparing the CVs of these three catalysts, one can conclude that they give different Ir-based amorphous phase(s) by cycling. The formation of different Ir-related phase(s) over these catalysts is also indicated by corresponding XPS results (Supplementary Figure 3 and Supplementary Table 5). More importantly, the profiles of CVs (the 5000th/10,000th cycle) from cycled samples resemble those of 1st cycle, strongly suggest that the formed Ir-based amorphous phase(s) are strongly influenced by the initial lattice.

### Possible active phase after surface reconstruction

Till now, several facts have been put forward to explain the high activities measured from Ir-based complex oxides with perovskite or perovskite-related structures12,13,14,15. For example, derived from Sr-leached SrIrO3, it is revealed certain IrOx, with structure resemble cubic perovskite, is highly active towards OER13. A similar conclusion was obtained from Ir-based double perovskites, that is Ir is more active in 3D network of corner-shared octahedrons12. Although the surfaces of these double perovskites may also experience fast surface rearrangement, the initial cubic perovskite structure with corner-shared octahedrons seems to be a key factor that influence or even determine the activity of formed surface active phase(s). This may also explain the inferior activity of m-SrIrO3 in our study. In fact, for an amorphous IrOx, the strong correlation between activity and local structure (corner-shared vs. edge-shared IrO6 octahedrons) has also been highlighted by Willinger et al.23. Besides, it is reported that certain lattice oxygen atom can be activated in a La2LiIrO6 perovskite. Such activated lattice oxygen atom can participate in the OER and is proposed critical for the observed high activity15. However, as surface reconstruction is observed in our catalysts, the activated lattice oxygen atom from perovskite is unlikely. We hypothesized that the high activity of IrOxHy evolved from SrCo0.9Ir0.1O3−δ due to the strong correlation between the IrOxHy and the initial/bulk lattice of SrCo0.9Ir0.1O3−δ.

In the developed SrCo0.9Ir0.1O3−δ, first of all, its pseudo-cubic structure with initially corner-shared octahedrons can induce the formation of a local structure optimized IrOxHy phase, which still contains a high ratio of corner-shared IrO6 octahedrons. However, this is insufficient to explain the measured higher activity when compared with that from the reported PLD-SrIrO313. As compared with SrIrO3 and other reported Ir-based perovskites, the SrCo0.9Ir0.1O3−δ here is expected to possess a high amount of oxygen vacancies in the lattice since the SrCoO3−δ matrix is highly oxygen deficient37. Accordingly, the oxygen vacancy formation energies for m-SrIrO3, PLD-SrIrO3, and SrCo0.9Ir0.1O3 were calculated by density functional theory (DFT). Moreover, the O p-band centers of different materials were also calculated. This is because a perovskite with an O p-band center close to Fermi level was found easier to release oxygen, i.e., the formation of oxygen vacancies38 (computation details and discussions are shown in Supplementary Figure 4&5 and Supplementary Table 6). As compared with m-SrIrO3 and PLD-SrIrO3, the DFT calculations indicate that the SrCo0.9Ir0.1O3−δ could contain a higher amount of oxygen vacancies.

To further investigate the oxygen vacancies in SrCo0.9Ir0.1O3−δ, the X-ray adsorption spectroscopy (XAS) was performed to check the valence state and coordination environment of Co and Ir. As shown in Fig. 3c, the average valence state of Co in the SrCo0.9Ir0.1O3−δ is approximately 3+ by comparing with the Co K-edge from the standard LaCoO3, in which the Co is strictly trivalent state39,40. Considering the Ir-LIII edge positions from m-SrIrO3 and IrO2 are similar to each other (Fig. 3d), the oxidation state of Ir in m-SrIrO3 is approximately 4+, indicating almost no oxygen vacancy in m-SrIrO3. The valence state of Ir in SrCo0.9Ir0.1O3−δ is found slightly higher than 4+ as the Ir-LIII edge shifts to higher energy as compared with IrO2. For charge neutrality, the δ (oxygen nonstoichiometry) in SrCo0.9Ir0.1O3−δ can reach a minimum value of 0.4 if assuming all Ir is pentavalent state. Therefore, a high amount of oxygen vacancies should exist in SrCo0.9Ir0.1O3, and thus both Co and Ir in SrCo0.9Ir0.1O3−δ are highly under-coordinated. Accordingly, the Fourier transformed (FT) EXAFS spectra in R-space for Co and Ir in SrCo0.9Ir0.1O3−δ are compared with the spectra from standard LaCoO3, m-SrIrO3, and IrO2, in which Co and Ir are fully or almost fully coordinated. In FT EXAFS spectra, the peaks are related to the coordination shells of Ir and Co. Specifically, the first peak represents the first Ir/Co–O shell caused by the interference between the electronic back scatterings from Ir/Co to neighbor O. Figure 3e shows the FT EXAFS spectra of the Co K edge from SrCo0.9Ir0.1O3−δ. The first peak at a reduced distance of ~1.5 Å represents the first Co–O coordination shell in SrCo0.9Ir0.1O3−δ and it shows a much lower intensity as compared with the first peak from LaCoO3, indicating the highly under-coordinated Co. Additional evidence of such high oxygen-deficiency is obtained from the fitting of the first peaks, where the coordination number of Co in SrCo0.9Ir0.1O3−δ is approximately 4.1 (Supplementary Figure 6 and Supplementary Table 7). The comparison of FT EXAFS spectra at the Ir LIII-edge from IrO2, m-SrIrO3, and SrCo0.9Ir0.1O3−δ is shown in Fig. 3f. The first peak (at ~1.5 Å) from IrO2 and m-SrIrO3 overlaps to each other, while a shift to lower distance (shown in the inset of Fig. 3f) is found for SrCo0.9Ir0.1O3−δ, implying a shorter average Ir–O bond length in SrCo0.9Ir0.1O3−δ. The fitting of first Ir–O coordination shells also confirms this reduced bond length. (Supplementary Figure 7 and Supplementary Table 8). As expected, a first shell fitting indicates Ir in SrCo0.9Ir0.1O3−δ is also highly under-coordinated with a coordination number of ~4.9. Instead, the Ir in m-SrIrO3 is fully coordinated, which is consistent with the DFT result.

Based on the results shown in Figs. 2 and 3, a schematic in Fig. 4 is proposed to illustrate the possible surface reconstruction over the SrCo0.9Ir0.1O3−δ surface. In initial SrCo0.9Ir0.1O3−δ, the IrO6 octahedrons are corner-shared with surrounding (Co/Ir)O6 octahedrons. Due to the presence of oxygen vacancies, the Ir in the lattice is under-coordinated. During electrochemical cycling, fast leaching of Sr and Co leaves an Ir rich surface. The initial pseudo-cubic structure will collapse on the surface and the formed IrOxHy phase(s) is amorphous without long-range ordering. The formed IrOxHy phase(s) may contain a high amount of structural domains with corner-shared IrO6 octahedrons. Moreover, the Ir in the amorphous phase could be more under-coordinated as compared with those derived from SrIrO3 after Sr leaching. This deduction also explains why the activity of Ir from SrCo0.9Ir0.1O3−δ is higher than that of Ir from electrochemically cycled SrIrO3.

### Assessing the stability of SrCo0.9Ir0.1O3−δ

Most recently, Geiger et al. proposed a stability number (S-number), considering the dissolution of active sites, is a proper metric to evaluate the stability of catalysts41. Thus, in this study, we also calculate the S-number of Ir in SrCo0.9Ir0.1O3−δ. The dissolution of cations, including Sr, Co, and Ir, from SrCo0.9Ir0.1O3−δ during electrochemical tests are studied. The amount of dissolved cations during the cycling are shown in Fig. 5a. The corresponding overall dissolved Sr, Co, and Ir from SrCo0.9Ir0.1O3−δ during the cycling are shown in Supplementary Figure 8. The dissolution of Ir from Ir metal is also measured for comparison. At the early stage (0–100 cycles), fast Sr, Co, and Ir dissolution is observed from SrCo0.9Ir0.1O3−δ. The simultaneous dissolution of Sr and Co likely induces such high dissolution rate of Ir. In the following cycles, the dissolution rate of Ir from SrCo0.9Ir0.1O3−δ is found slowed down. Interestingly, the apparently reduced dissolution rates of Sr and Co suggests that the dissolution of Sr and Co from SrCo0.9Ir0.1O3−δ is kinetically hindered by the formed Ir-rich surface layer. Similarly, The Ir metal also showed a gradually decreased rate of Ir dissolution. That is the formation of active Ir hydrous oxide also causes a fast Ir dissolution at the early stage. Figure 5b shows the potential profiles of as-synthesized/purchased SrCo0.9Ir0.1O3−δ, Ir metal, and IrO2 by chronopotentiometry method. Regardless of potential fluctuations caused by intermittent O2 bubbles released from the electrode surface, fairly stable performance is observed for all samples. The stability for different catalysts is then compared using their S-numbers, which are calculated by dividing the amount of oxygen molecules evolved by the amount of Ir dissolved in the electrolyte41. Moreover, as the surface reconstruction with fast cation dissolution (Fig. 5a) may greatly affect the following S-number calculation, both SrCo0.9Ir0.1O3−δ and Ir metal electrodes are pre-treated at 10 mA cm−2 for 60 min (Supplementary Figure 9) for reaching the steady state. Figure 5c shows S-numbers for SrCo0.9Ir0.1O3−δ, Ir metal, and IrO2. Here, all S-numbers are calculated according to the amount of dissolved Ir measured during chronopotentiometry (Fig. 5b and Supplementary Figure 9). The S-numbers of different oxides reported by Geiger et al. are also presented41. Due to the initial surface reconstruction, much lower S-numbers (103–104) are observed from SrCo0.9Ir0.1O3−δ and Ir metal during the pre-treatment stage (initial 60 min). Interestingly, from the following 180 min test, the S-number of SrCo0.9Ir0.1O3−δ steeply increased to approximately 105, which is approximately one order of magnitude higher than the S-numbers of reported perovskites. In addition, the S-numbers of SrCo0.9Ir0.1O3−δ and Ir metal are comparable with the S-number of IrO2 (by Sigma-Aldrich). The S-number of IrO2 we measured, however, is much lower than that of reported IrO2 (by Alfa-Aesar)41. Such higher stability of reported IrO2 can be related to the improved stoichiometry on the surface after additional annealing step. It is likely the production or condition of raw materials may also affect the S-numbers. From these results, we can conclude that the eventually formed Ir-rich layer over SrCo0.910Ir0.1O3−δ is rather stable if neglecting the initial instability caused by surface reconstruction process.

## Discussion

In summary, we developed a pseudo-cubic SrCo0.9Ir0.1O3−δ perovskite. Such material can be easily prepared with a simple solid state method without high pressure condition. The Ir from pseudo-cubic SrCo0.9Ir0.1O3−δ showed an intrinsic activity (TOF) more than two orders of magnitude higher than that in IrO2, and approximately 10 times higher than that in the benchmark PLD-SrIrO3. The chemical state of surface Ir in SrCo0.9Ir0.1O3−δ is found changed after electrochemical cycling. The reconstructed surfaces are responsible for the observed activities. Although the initial bulk catalysts may not directly influence the OER, this study highlights that the chemical states of bulk catalysts, such as the crystal structure (pseudo-cubic structure with corner-shared IrO6 octahedrons) and the content of oxygen vacancy in the lattice (under-coordinated Ir), will affect the activity of the in-situ formed active sites (Ir-rich surface) for OER.

## Methods

### Synthesis of oxides

All composite oxides were synthesized with solid state method. Powders of SrCO3, IrO2, TiO2, and Co3O4 from Sigma-Aldrich Corporation were used as raw materials. Briefly, stoichiometry amount of raw materials were weighted and then mixed in mortar. The mixed precursors were finally calcined with box furnaces in ambient air. A sintering condition of 850 °C for 12 h, 1100 °C for 12° h, and 1200 °C for 12 h is applied for m-SrIrO3, SrCo0.9Ir0.1O3−δ, and SrCo0.9Ti0.1O3−δ respectively.

### Characterizations

The phase structures of m-SrIrO3 and SrCo0.9Ir0.1O3−δ were identified with X-ray Powder Diffractometer (D8 advance, Bruker Corporation). The phase structures were analyzed by the Rietveld method with GSAS program and EXPGUI interface42. The morphologies of the materials were studied by FESEM (JEOL 6340F). TEM images were collected on JEM-2010F (JEOL). The XPS tests were performed using a PHI-5400 equipment with Al Ka beam source (250 W) and position-sensitive detector. An XPSpeak41 software is applied for peak fitting. Considering the spin–orbit splitting, a relative area ratio of 2:3 and 3:4 is considered for the doublets in Sr_3d and in Ir_4f, respectively. A spin–orbit splitting of 3 eV is considered for the doublets in Ir_4f. A Shirley background was applied during the fitting. All peaks are described as convolution of Gaussian and Lorentzian function.

XAS experiments were performed at Singapore Synchrotron Light Source, XAFCA beamline. Data analysis were performed with the Athena software package. The surface areas were characterized by nitrogen adsorption–desorption tests (ASAP Tri-star II 3020) with the BET method.

### Electrochemical tests

The electrochemical experiments were carried out on a rotating electrode configuration from Pine Instrument at room temperature. The working electrode of glassy carbon (rotating disk) with an area of 0.196 cm−2 was applied. The catalyst ink with a concentration of 5 mg mL−1 was prepared by ultra-sonically dispersing 2.5 mg oxide and 1 mg acetylene black (Alfa Aesar) in an water (375 µL)–isopropanol (112.5 µL)–Nafion (12.5 µL) solution. 10 µL of well dispersed ink was dropped onto the glassy carbon and dried overnight. For ICP-MS tests, the amount of oxide increased to 5 mg for SrCo0.9Ir0.1O3−δ and Ir metal. As a higher stability is expected for IrO2, its amount further increase to 10 mg. An SP-150 workstation (Bio-Logic Science Instruments) was applied to perform cyclic voltammetry scanning and chronopotentiometric tests. The tests were performed in a 0.1 M HClO4 solution, which was purged with ultra-pure oxygen before each measurement for approximately 30 min. A rotation speed of 1600 rpm was used. A Pt wire was used as the counter electrode and a saturated calomel electrode (SCE) was used as the reference electrode.

### TOF calculation

The TOF is calculated from the equation:

$${\mathrm{TOF}} = \frac{{j \times A_{\rm OX}}}{{4 \times e \times N_{\mathrm A}}}$$
(1)

where j is the BET surface area normalized current density at an overpotential of 270 mV. AOX is the total surface area of the catalyst deposited on the GC electrode. e is the electric charge carried by a single electron. NA is the number of Ir atoms. While calculating the NA, three cases are considered.

In the first case, only the Ir atoms from the outermost surface are considered. For PLD-SrIrO3, the calculation is performed by assuming PLD-SrIrO3 with an ideal P m-3m structure and a perfect (100) surface. A lattice parameter of 4.024 Å reported in the literature is used13. For m-SrIrO3, the lattice parameters from XRD refinement are used and a (001) surface, with the highest Ir surface density, is chosen (thus the activity will not be overestimated). For SrCo0.9Ir0.1O3−δ, the lattice parameters from XRD refinement are used and a (010) surface, with the highest Ir surface density, is chosen (thus the activity will not be overestimated). For IrO2, lattice parameters of a = 4.505 Å and c = 3.159 Å are used and a (110) surface is considered43. In this case, the active Ir atoms in reconstructed surface region are not counted and thus the activity is over-estimated. Thus, this way cannot be used for comparing TOF.

In the second case, all Ir atoms for each catalyst loaded on the electrode are considered active for OER. Please note this case over-estimates the active Ir atoms and thus the activity will be significantly under-estimated. Therefore, this way does not make sense, too.

In the third case, to include the effect of surface reconstruction, all Ir atoms from reconstructed surface regions are considered. Based on the TEM results (Fig. 2a, c), we assume the depth of the reconstructed surface region in m-SrIrO3 and SrCo0.9Ir0.1O3−δ is 5 and 10 nm, respectively. In PLD-SrIrO3 film, it was reported that the root mean square roughness is <4 nm before OER and <20 nm after cycling13. Thus, we assume a surface reconstruction with a depth of 8 and 40 nm to normalize the initial activity and final activity (after 30 h test) of Ir in PLD-SrIrO3, respectively. For IrO2, the surface reconstruction effect is negligible, and thus is not considered.

### Estimation of the current due to Sr and Co leaching

Here, we estimate the maximum current contributed by Sr and Co leaching (possible leaching current). Several assumptions are made for the calculation/estimation:

1. (1)

The Sr2+ and Co3+ leached is compensated by electron lose from the catalyst, i.e., all leached Sr2+ and Co3+ cations will contribute to the current.

2. (2)

All Sr2+ and Co3+ from the surface region (10 nm depth, determined by TEM as shown in the manuscript) leached in 5 cycles at a constant speed. This is because we did not see steep current changes due to cation leaching.

Then, the current from cation leaching $$\left( {{I}_{{\mathrm{ox}}}^{{\mathrm{leach}}}} \right)$$ can be calculated by the equation:

$$I_{{\mathrm{ox}}}^{{\mathrm{leach}}} =\frac{{\left( {2 \times {n}_{{\mathrm{Sr}}^{2 + }} + 3 \times {n}_{{\mathrm{Co}}^{3 + }}} \right) \times {e}}}{{{t} \ast {S}_{{\mathrm{ox}}}}}$$
(2)

$${n}_{{\mathrm{Sr}}^{2 + }}$$ and $${n}_{{\mathrm{Co}}^{3 + }}$$ are the number of leached Sr2+ and Co3+ from the surface region (10 nm depth). e is the electric charge of an electron. t is the time used for 5 cycles. Our cycling test for SrCo0.9Ir0.1O3−δ is performed in the potential range (vs. RHE) from 1 to 1.7 V. The scan rate is 10 mV s−1. Sox is the surface area of the loaded catalyst.

Based on that, a maximum current of 0.0186 $${\mathrm{mA}}\;{\mathrm{cm}}_{{\mathrm{ox}}}^{ - 2}$$ is calculated, and which can contribute to the measured current in initial 5 cycles. This current value is more than two orders of magnitude lower than the measured OER current from SrCo0.9Ir0.1O3−δ. For example, at an overpotential of 270 and 320 mV, the measured OER current from SrCo0.9Ir0.1O3−δ can reach 2.8 and 16.3 $${\mathrm{mA}}\;{\mathrm{cm}}_{{\mathrm{ox}}}^{ - 2}$$, respectively.

### DFT calculation

Spin-polarized DFT calculations were performed using the Vienna ab initio simulation package (VASP)44,45 with the projector-augmented wave (PAW) approach46 and the Perdew–Burk–Ernzerhof (PBE) exchange-correlation functional47. To account for the strongly localized d-electrons of Co, a DFT+U approach was adopted and an effective Hubbard U parameter of 3.32 eV was used48,49. The electronic energy tolerance was set to 10−6 eV and the force tolerance for structural relaxation was 0.015 eV Å−1. The structural model for PLD-SrIrO3 is a 2 × 2 × 2 cubic supercell, for m-SrIrO3 is a conventional standard unit cell and for pc-SrCo0.875Ir0.125O3 is a 2 × 1 × 1 orthorhombic supercell. For all compositions, the lattice constants and ion positions were first fully relaxed. Then, the defect calculations were performed on the fully relaxed stoichiometric structures, and all the symmetry distinct oxygen sites in the corresponding model were explored to search for the most stable vacancy site. The oxygen vacancy concentration for PLD-SrIrO3 and pc-SrCo0.875Ir0.125O3 is 4.167% while for m-SrIrO3 is 3.125%. The total energy calculations of all structures were performed with the tetrahedron method with Blöchl corrections50 and an energy cutoff of 520 eV. And a 6 × 6 × 6 Monkhorst–Pack k-point mesh was employed for PLD-SrIrO3, a 4 × 6 × 8 mesh for pc-SrCo0.875Ir0.125O3 and a 10 × 6 × 4 mesh for m-SrIrO3. For all compositions, the bulk oxygen vacancy formation energy was calculated based on the most stable oxygen-deficient structure and with respect to H2O (g) and H2 (g) at standard condition. The oxygen vacancy formation enthalpy will be shifted around +2.33 eV larger if O2 (g) is used as the reference.

## Data availability

All relevant data are available from the authors upon request.

## References

1. 1.

Ginley, D., Green, M. A. & Collins, R. Solar energy conversion toward 1 terawatt. MRS Bull. 33, 355–364 (2008).

2. 2.

Strmcnik, D. et al. Improving the hydrogen oxidation reaction rate by promotion of hydroxyl adsorption. Nat. Chem. 5, 300–306 (2013).

3. 3.

Danilovic, N. et al. Enhancing the alkaline hydrogen evolution reaction activity through the bifunctionality of Ni(OH)2/metal catalysts. Angew. Chem. Int. Ed. 51, 12495–12498 (2012).

4. 4.

Reier, T., Oezaslan, M. & Strasser, P. Electrocatalytic oxygen evolution reaction (OER) on Ru, Ir, and Pt catalysts: a comparative study of nanoparticles and bulk materials. ACS Catal. 2, 1765–1772 (2012).

5. 5.

Antolini, E. Iridium as catalyst and cocatalyst for oxygen evolution/reduction in acidic polymer electrolyte membrane electrolyzers and fuel cells. ACS Catal. 4, 1426–1440 (2014).

6. 6.

Zhao, Y. X., Hernandez-Pagan, E. A., Vargas-Barbosa, N. M., Dysart, J. L. & Mallouk, T. E. A high yield synthesis of ligand-free iridium oxide nanoparticles with high electrocatalytic activity. J. Phys. Chem. Lett. 2, 402–406 (2011).

7. 7.

Lee, Y., Suntivich, J., May, K. J., Perry, E. E. & Shao-Horn, Y. Synthesis and activities of rutile IrO2 and RuO2 nanoparticles for oxygen evolution in acid and alkaline solutions. J. Phys. Chem. Lett. 3, 399–404 (2012).

8. 8.

Lim, J. et al. Ultrathin IrO2 nanoneedles for electrochemical water oxidation. Adv. Funct. Mater. 28, 1704796 (2018).

9. 9.

Pi, Y. C., Zhang, N., Guo, S. J., Guo, J. & Huang, X. Q. Ultrathin laminar Ir superstructure as highly efficient oxygen evolution electrocatalyst in broad pH range. Nano Lett. 16, 4424–4430 (2016).

10. 10.

Oh, H. S., Nong, H. N., Reier, T., Gliech, M. & Strasser, P. Oxide-supported Ir nanodendrites with high activity and durability for the oxygen evolution reaction in acid PEM water electrolyzers. Chem. Sci. 6, 3321–3328 (2015).

11. 11.

Nong, H. N. et al. Oxide-supported IrNiOx core–shell particles as efficient, cost-effective, and stable catalysts for electrochemical water splitting. Angew. Chem. Int. Ed. 54, 2975–2979 (2015).

12. 12.

Diaz-Morales, O. et al. Iridium-based double perovskites for efficient water oxidation in acid media. Nat. Commun. 7, 12363 (2016).

13. 13.

Seitz, L. C. et al. A highly active and stable IrOx/SrIrO3 catalyst for the oxygen evolution reaction. Science 353, 1011–1014 (2016).

14. 14.

Tang, R. B. et al. Oxygen evolution reaction electrocatalysis on SrIrO3 grown using molecular beam epitaxy. J. Mater. Chem. A 4, 6831–6836 (2016).

15. 15.

Grimaud, A. et al. Activation of surface oxygen sites on an iridium-based model catalyst for the oxygen evolution reaction. Nat. Energy 2, 16189 (2017).

16. 16.

Liu, Y. X., Masumoto, H. & Goto, T. Structural, electrical and optical characterization of SrIrO3 thin films prepared by laser-ablation. Mater. Trans. 46, 100–104 (2005).

17. 17.

Zhao, J. G. et al. High-pressure synthesis of orthorhombic SrIrO3 perovskite and its positive magnetoresistance. J. Appl. Phys. 103, 103706 (2008).

18. 18.

Longo, J. M., Kafalas, J. A. & Arnott, R. J. Structure and properties of high and low pressure forms of SrIrO3. J. Solid State Chem. 3, 174–179 (1971).

19. 19.

Qasim, I., Kennedy, B. J. & Avdeev, M. Synthesis, structures and properties of transition metal doped SrIrO3. J. Mater. Chem. A 1, 3127–3132 (2013).

20. 20.

Sun, S. N., Li, H. Y. & Xu, Z. C. J. Impact of surface area in evaluation of catalyst activity. Joule 2, 1024–1027 (2018).

21. 21.

Danilovic, N. et al. Using surface segregation to design stable Ru–Ir oxides for the oxygen evolution reaction in acidic environments. Angew. Chem. Int. Ed. 53, 14016–14021 (2014).

22. 22.

Massue, C. et al. Microwave-assisted synthesis of stable and highly active Ir oxohydroxides for electrochemical oxidation of water. ChemSusChem 10, 1958–1968 (2017).

23. 23.

Willinger, E., Massue, C., Schlogl, R. & Willinger, M. G. Identifying key structural features of IrOx water splitting catalysts. J. Am. Chem. Soc. 139, 12093–12101 (2017).

24. 24.

Mutoro, E., Crumlin, E. J., Biegalski, M. D., Christen, H. M. & Shao-Horn, Y. Enhanced oxygen reduction activity on surface-decorated perovskite thin films for solid oxide fuel cells. Energy Environ. Sci. 4, 3689–3696 (2011).

25. 25.

Vasquez, R. P. X-ray photoelectron-spectroscopy study of Sr and Ba compounds. J. Electron Spectrosc. 56, 217–240 (1991).

26. 26.

Wertheim, G. K. & Guggenheim, H. J. Conduction-electron screening in metallic oxides—IrO2. Phys. Rev. B 22, 4680–4683 (1980).

27. 27.

Pfeifer, V. et al. The electronic structure of iridium oxide electrodes active in water splitting. Phys. Chem. Chem. Phys. 18, 2292–2296 (2016).

28. 28.

Atanasoska, L., Atanasoski, R. & Trasatti, S. XPS and AES study of mixed layers of RuO2 and IrO2. Vacuum 40, 91–94 (1990).

29. 29.

Kodintsev, I. M., Trasatti, S., Rubel, M., Wieckowski, A. & Kaufher, N. X-ray photoelectron-spectroscopy and electrochemical surface characterization of IrO2 + RuO2 electrodes. Langmuir 8, 283–290 (1992).

30. 30.

Peuckert, M. XPS study on thermally and electrochemically prepared oxidic adlayers on iridium. Surf. Sci. 144, 451–464 (1984).

31. 31.

Minguzzi, A. et al. Easy accommodation of different oxidation states in iridium oxide nanoparticles with different hydration degree as water oxidation electrocatalysts. ACS Catal. 5, 5104–5115 (2015).

32. 32.

Smith, R. D. L., Sporinova, B., Fagan, R. D., Trudel, S. & Berlinguette, C. P. Facile photochemical preparation of amorphous iridium oxide films for water oxidation catalysis. Chem. Mater. 26, 1654–1659 (2014).

33. 33.

Pfeifer, V. et al. The electronic structure of iridium and its oxides. Surf. Interface Anal. 48, 261–273 (2016).

34. 34.

Li, T. et al. Atomic-scale insights into surface species of electrocatalysts in three dimensions. Nat. Catal. 1, 300–305 (2018).

35. 35.

Minguzzi, A. et al. Observing the oxidation state turnover in heterogeneous iridium-based water oxidation catalysts. Chem. Sci. 5, 3591–3597 (2014).

36. 36.

Wang, H. Y. et al. In operando identification of geometrical-site-dependent water oxidation activity of spinel Co3O4. J. Am. Chem. Soc. 138, 36–39 (2016).

37. 37.

Mefford, J. T. et al. Water electrolysis on La1−xSrxCoO3-delta perovskite electrocatalysts. Nat. Commun. 7, 11053 (2016).

38. 38.

Lee, Y. L., Kleis, J., Rossmeisl, J., Shao-Horn, Y. & Morgan, D. Prediction of solid oxide fuel cell cathode activity with first-principles descriptors. Energy Environ. Sci. 4, 3966–3970 (2011).

39. 39.

Tejuca, L. G., Bell, A. T., Fierro, J. L. G. & Pena, M. A. Surface behavior of reduced LaCoO3 as studied by TPD of CO, CO2 and H2 probes and by XPS. Appl. Surf. Sci. 31, 301–316 (1988).

40. 40.

Pishahang, M., Bakken, E., Stolen, S., Larring, Y. & Thomas, C. I. Oxygen non-stoichiometry and redox thermodynamics of LaMn1−xCoxO3-delta. Solid State Ion. 231, 49–57 (2013).

41. 41.

Geiger, S. et al. The stability number as a metric for electrocatalyst stability benchmarking. Nat. Catal. 1, 508–515 (2018).

42. 42.

Toby, B. H. EXPGUI, a graphical user interface for GSAS. J. Appl. Crystallogr. 34, 210–213 (2001).

43. 43.

Sen, F. G. et al. Towards accurate prediction of catalytic activity in IrO2 nanoclusters via first principles-based variable charge force field. J. Mater. Chem. A 3, 18970–18982 (2015).

44. 44.

Kresse, G. & Furthmuller, J. Efficient iterative schemes for ab initio total-energy calculations using a plane-wave basis set. Phys. Rev. B 54, 11169–11186 (1996).

45. 45.

Kresse, G. & Furthmuller, J. Efficiency of ab-initio total energy calculations for metals and semiconductors using a plane-wave basis set. Comput. Mater. Sci. 6, 15–50 (1996).

46. 46.

Blochl, P. E. Projector augmented-wave method. Phys. Rev. B 50, 17953–17979 (1994).

47. 47.

Perdew, J. P., Burke, K. & Ernzerhof, M. Generalized gradient approximation made simple. Phys. Rev. Lett. 77, 3865–3868 (1996).

48. 48.

Wang, L., Maxisch, T. & Ceder, G. Oxidation energies of transition metal oxides within the GGA+U framework. Phys. Rev. B 73, 195107 (2006).

49. 49.

Lee, Y. L., Kleis, J., Rossmeisl, J. & Morgan, D. Ab initio energetics of LaBO3(001) (B = Mn, Fe, Co, and Ni) for solid oxide fuel cell cathodes. Phys. Rev. B 80, 224101 (2009).

50. 50.

Blochl, P. E., Jepsen, O. & Andersen, O. K. Improved tetrahedron method for Brillouin-zone integrations. Phys. Rev. B 49, 16223–16233 (1994).

## Acknowledgements

This work is supported by the Singapore MOE Tier 2 (MOE2017-T2-1-009) and by the Singapore National Research Foundation under its Campus for Research Excellence And Technological Enterprise (CREATE) programme, through the Singapore Berkeley Research Initiative for Sustainable Energy (SinBeRISE), The Cambridge Center for Carbon Reduction in Chemical Technology (C4T), and eCO2EP programmes. The authors thank the Facility for Analysis, Characterisation, Testing and Simulation (FACTS) in Nanyang Technological University for materials characterization.

## Author information

Authors

### Contributions

Y.C. and Z.J.X. designed the experiments. Y.C. conducted material synthesis, performed XRD analysis, and electrochemical characterization and analysis. H.L. and Y.S. performed DFT calculations. J.W. and Y.C. performed TEM experiments and analysis. Y.D., S.X. and Y.C. carried out XAS experiment and analysis. Y.C. and Z.J.X. wrote the manuscript. M.S., J.W.A. and A.C.F. analyzed the data and polished the manuscript.

### Corresponding author

Correspondence to Zhichuan J. Xu.

## Ethics declarations

### Competing interests

The authors declare no competing interests.

Journal peer review information: Nature Communications thanks the anonymous reviewers for their contribution to the peer review of this work.

Publisher’s note: Springer Nature remains neutral with regard to jurisdictional claims in published maps and institutional affiliations.

## Rights and permissions

Reprints and Permissions

Chen, Y., Li, H., Wang, J. et al. Exceptionally active iridium evolved from a pseudo-cubic perovskite for oxygen evolution in acid. Nat Commun 10, 572 (2019). https://doi.org/10.1038/s41467-019-08532-3

• Accepted:

• Published:

• ### Spin-polarized oxygen evolution reaction under magnetic field

• Xiao Ren
• , Tianze Wu
• , Yuanmiao Sun
• , Yan Li
• , Guoyu Xian
• , Xianhu Liu
• , Chengmin Shen
• , Jose Gracia
• , Hong-Jun Gao
• , Haitao Yang
•  & Zhichuan J. Xu

Nature Communications (2021)

• ### Spin pinning effect to reconstructed oxyhydroxide layer on ferromagnetic oxides for enhanced water oxidation

• Tianze Wu
• , Xiao Ren
• , Yuanmiao Sun
• , Shengnan Sun
• , Guoyu Xian
• , Günther G. Scherer
• , Daniel Mandler
• , Joel W. Ager
• , Alexis Grimaud
• , Junling Wang
• , Chengmin Shen
• , Haitao Yang
• , Jose Gracia
• , Hong-Jun Gao
•  & Zhichuan J. Xu

Nature Communications (2021)

• ### Recent Advances in the Understanding of the Surface Reconstruction of Oxygen Evolution Electrocatalysts and Materials Development

• Junwei Chen
• , Haixin Chen
• , Tongwen Yu
• , Ruchun Li
• , Yi Wang
• , Zongping Shao
•  & Shuqin Song

Electrochemical Energy Reviews (2021)

• ### Praseodymium iridium oxide as a competitive electrocatalyst for oxygen evolution reaction in acid media

• Yimeng Wang
• , Shangguo Liu
• , Qing Qin
• , Huihui Liu
• , Lijie Zhang
• , Tao Wei
• , Haisen Li
•  & Xien Liu

Science China Materials (2021)

• ### Transition metal oxides for water oxidation: All about oxyhydroxides?

• Zhichuan J. Xu

Science China Materials (2020)