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Exceptional electrocatalytic oxygen evolution via tunable charge transfer interactions in La0.5Sr1.5Ni1−xFexOδ Ruddlesden-Popper oxides

Nature Communicationsvolume 9, Article number: 3150 (2018) | Download Citation


The electrolysis of water is of global importance to store renewable energy and the methodical design of next-generation oxygen evolution catalysts requires a greater understanding of the structural and electronic contributions that give rise to increased activities. Herein, we report a series of Ruddlesden–Popper La0.5Sr1.5Ni1−xFexOδ oxides that promote charge transfer via cross-gap hybridization to enhance electrocatalytic water splitting. Using selective substitution of lanthanum with strontium and nickel with iron to tune the extent to which transition metal and oxygen valence bands hybridize, we demonstrate remarkable catalytic activity of 10 mA cm−2 at a 360 mV overpotential and mass activity of 1930 mA mg−1ox at 1.63 V via a mechanism that utilizes lattice oxygen. This work demonstrates that Ruddlesden–Popper materials can be utilized as active catalysts for oxygen evolution through rational design of structural and electronic configurations that are unattainable in many other crystalline metal oxide phases.


Increasing global energy demand requires greater efficiency in water electrolyzers to generate hydrogen at a low cost as well as in other devices for energy storage such as rechargeable metal-air batteries. Given that the efficiencies of devices for these types of energy storage are limited largely by the slow kinetics of the oxygen evolution reaction (OER, 4OH → O2 + 2H2O + 4e), extensive work has been done to reduce the overpotential required to evolve oxygen in basic electrolytes using state-of-the-art catalysts1. While precious metals such as Ir and Ru have become standard OER catalysts when working at low pH, alkaline electrolytes allow for the use of abundant, less expensive metals. For example, Ni–M oxyhydroxides such as Ni1−xFexOOH are known to be very active for the OER; however, lack of long-range order and uncontrolled electronic structure stemming from different synthetic methods2 complicates elucidation of the mechanism(s) by which the OER activity is improved3,4,5. In fact, recent reports question whether Fe is part of the catalytic cycle or if it promotes partial charge transfer between Ni and Fe metal centers2,4,6. Additionally, recent work on Ni–Fe oxyhydroxides demonstrated that a significant portion of the measured OER current may be due to other processes and highlighted the need for careful electrochemical analysis of what reactions are contributing to the high activities reported7. Collectively this means that while Ni1−xFexOOH materials have been reported as highly active catalysts, the large variations in electronic configuration and the resulting catalytic activity in these studies complicate establishment of precise structure–property correlations for Ni–Fe oxyhydroxides2,5,8.

In contrast, perovskite oxides with the nominal formula ABOδ, in which A is a rare-earth or alkaline earth element and B is a transition metal, have recently been shown to promote OER catalysis through increased ionic and electronic conductivities, as well as good structural stability and synthetic versatility, all of which enable the development of rational catalyst design criteria9,10,11. Importantly, the ability to substitute elements of varying valence, electronegativity, or ionic size into A- and B-site directly influences the resultant properties of these catalysts1,12. An example of this was the substitution of Cu into the A-site of the quadruple perovskite CaCu3Fe4O12 to increase stability of the catalyst13. Recently, we demonstrated that highly covalent Co 3d–O 2p bonding in SrCoO2.7 improved OER activity via a more energetically favorable lattice oxygen mediated (LOM) reaction pathway, consistent with prior reports and theory14,15,16. This LOM mechanism does not require the redox switching of transition metal sites, but rather utilizes lattice oxygen in the OER when the Fermi level \((E_{\mathrm F}^0)\) crosses the transition metal 3d–O 2p hybridized bands. This results in ligand holes that activate lattice oxygen which may combine with chemisorbed OH to produce O2−. This mechanism has since been confirmed by others using isotopic labeling experiments to detect exchanged oxygen from the lattice of SrCoO317. In a separate report, SrNiO3 perovskite was predicted to be more covalent, even more prone to oxygen deficiency, and thus be more catalytically active than SrCoO318. Unfortunately, this prediction is hard to validate experimentally as SrNiO3 adopts a non-perovskite structure based on a hexagonal close packing of Sr and O atoms19. In addition, it is known that the substitution of Sr into LaNiO3 is limited to ~5–20% after which phase impurities appear that result in poor catalytic activity20,21.

To overcome this limitation, we investigate an alternative crystal structure to the perovskite-phase SrNiO3 that promotes high OER activity but does not suffer from limited Sr solubility and can stabilize highly oxidized, covalently bound Ni. The Ruddlesden–Popper (RP) crystal structure is represented as An+1BnO3n+1 or equivalently (AO)(ABO3±δ)n, wherein perovskite layers with a thickness of n (BO6) octahedra are separated by rocksalt (AO)(OA) double layers. This RP phase can accommodate all the elemental substitutions available to perovskites as well as additional compositions that are not stable in the perovskite structure22. While Ruddlesden–Popper materials have been explored as solid oxide fuel-cell cathodes owing to their chemical flexibility and labile lattice oxygen, they have not been fully examined for room temperature water oxidation23,24,25,26,27,28,29.

Herein, we report a series of La0.5Sr1.5Ni1−xFexOδ (LSNF, x = 0 to 1) OER catalysts that have enabled us to achieve exceptionally high catalytic activities at low overpotentials with small OER Tafel slopes. We show that Sr substitution promotes high catalytic activity by further oxidizing Ni via charge compensation, enhancing Ni–O covalency and electronic conductivity. Chemical substitution of Fe for Ni introduces and tunes the overlap between the Ni and Fe 3d bands and the O 2p band. Density functional theory (DFT) modeling confirms that cross-gap hybridization between eg(Ni), p(O) and eg(Fe) bands across the Fermi level enhances charge transfer interactions across Fe–O–Ni bridges and the bandwidth available for electrode-adsorbate electron transfer. The increased covalency and cross-gap hybridization30 of transition metal 3d states and O 2p orbitals are an effective new catalyst design criteria for improving OER activity that supports oxygen evolution taking place via the LOM mechanism, a mechanism which has already been demonstrated to apply to other catalyst materials as well. Furthermore, our work illustrates the remarkable catalytic activity of the RP LSNF series that encompasses a range of chemical substitutions and electronic configurations not accessible in other crystalline metal oxide phases and that enables the elucidation of crucial structural–chemical–electronic relationships and the OER mechanism that has not been possible with Ni–M oxyhydroxides and other reported metal oxide catalysts for OER.


Materials characterization

La0.5Sr1.5Ni1−xFexOδ (LSNF, x = 0 to 1) samples were synthesized using a modified Pechini method31 followed by crystallization and annealing, details of which are found in the Methods section. Electron diffraction and powder X-ray diffraction (PXRD) patterns correspond to a body-centered tetragonal unit cell with the I4/mmm space group, characteristic of the n = 1 Ruddlesden–Popper (RP) crystal structure (Figs. 1a, b and Supplementary Figure 1). No superlattice reflections were detected that could be attributed to the La/Sr or Fe/Ni ordering, ordering of hyperstoichiometric oxygen atoms, or lattice distortions. The a and c unit cell parameters (Fig. 1d) and unit cell volume (Supplementary Figure 2) increase almost linearly with Fe substitution reflecting that the La0.5Sr1.5Ni1−xFexOδ solid solution is homogeneous over the entire substitutional range. The I4/mmm structure has been confirmed with Rietveld refinement from PXRD data (Supplementary Table 1, Supplementary Figures 3 and 4). Unit cell volume increases with Fe substitution are in agreement with the increasing fraction of Fe cations that have larger ionic radii than Ni cations (r(Fe3+, HS) = 0.645 Å, r(Fe4+, HS) = 0.585 Å, r(Ni3+, LS) = 0.56 Å, r(Ni4+, LS) = 0.48 Å)32. The ratio of the apical to equatorial Ni/Fe–O distances increases from 1.038 in LSN to 1.073 in LSF, reflecting slight apical elongation of the (Ni/Fe)O6 octahedra. The I4/mmm crystal structure is also directly viewed with annular bright field scanning transmission electron microscopy (ABF-STEM, Fig. 1c), which visualizes heavier cations and lighter oxygen anions simultaneously. The ABF-STEM image shows perfect stacking of the perovskite (BO2) (B = Ni, Fe) layers and the rocksalt (AO)(OA) (A = La, Sr) layers without stacking faults and the crystal structure propagates to the surface without amorphization.

Fig. 1
Fig. 1

Crystallographic characterization of the La0.5Sr1.5Ni1−xFexO4+δ series. a PXRD patterns of La0.5Sr1.5Ni1−xFexO4+δ demonstrate all compositions have the tetragonal n = 1 Ruddlesden–Popper I4/mmm structure. b Electron diffraction patterns of LSNF30 confirm the absence of cation and/or anion ordering. c [100] ABF-STEM image of LSNF30 directly visualizes the stacking of the (BO2) octahedra (white arrowheads, B = Ni, Fe) and (AO)(OA) layers (black arrowheads, A = La, Sr) in the Ruddlesden–Popper structure. The scale bar is 2 nm. d Compositional dependence of a and c unit cell parameters showing 0 ≤ x ≤ 1 homogeneity range

The consistent morphology of catalysts is crucial to the analytical comparison of electrochemical OER activity. High-angle annular dark-field scanning TEM (HAADF-STEM) and Brunauer–Emmet–Teller (BET) surface area analysis were performed and the results, presented in Supplementary Figure 5, indicate similar morphology across the LSNF series regardless of Fe substitution. All compositions consist of 50–300 nm crystallites loosely sintered into agglomerates that are up to several microns in size. This morphological similarity is reinforced by BET surface area results which range from 3.3 to 8.0 m2 g−1 (Supplementary Figure 6).


The La0.5Sr1.5Ni1−xFexOδ (LNSF) series was supported on Vulcan carbon (VC) at 30 wt% and tested for the OER with the results presented in Fig. 2. Supporting the catalyst on VC increases the conductivity of the composite by facilitating increased electrical contact between the glassy carbon RDE and the catalyst particles as well as between catalyst particles themselves. While carbon has its limitations as a support for device-level applications, the issue of carbon corrosion is a matter of kinetics and for fundamental studies such as this one it is quite common to support metal oxide catalysts on carbon when doing OER studies at room temperature. A major reason for this is to eliminate possible contributions from other supports, such as Ni foam, that while more appropriate for device-level mass loadings and performance can contribute a great deal to the OER current generated or have their own redox features that can convolute the examination of the material of interest and the fundamental principles explored in this work. The carbon ratio used in this paper was chosen as a result of our past work in which we carefully studied the effect of the catalyst to carbon ratio to determine that a 30:70 weight ratio resulted in optimal catalyst utilization33.

Fig. 2
Fig. 2

Oxygen evolution results and catalytic activities for the LSNF series supported at 30 wt% on XC72 Vulcan carbon (VC). Activities measured in O2-saturated 0.1 M KOH at 10 mV s−1 and 1600 rpm. a Averaged (anodic and cathodic) OER polarization curves presented in geometric current density (5 mm GCE, A = 0.196 cm2). b Oxide mass activities of the LSNF series at 1.63 V vs RHE-iR compared to leading OER catalysts SrCoO2.7, LaNiO3, and IrO2 on VC, all tested in the same experimental setup and conditions. Error bars are the standard deviations of measurements performed in triplicate. c Tafel plots of the specific activity of each LSNF catalyst. Error bars are the standard deviations of measurements performed in triplicate d RRDE test to confirm that current is due to oxygen evolution. The disk has a thin layer of 30 wt% LSNF30/VC and the ring is Pt. O2 generated at the disk is then reduced back to OH at the ring which is poised at −0.4 V vs Hg/HgO (1 M). The collection efficiency of the RRDE at 1.63 V was found to be 34%. RRDE measurements were performed in Ar-saturated 0.1 M KOH

Representative polarization curves for all supported compositions are shown in Fig. 2a and Supplementary Figure 7. For all amounts of Fe substitution, except for 100% (LSF), the onset potential for the OER decreases and the corresponding catalytic activity increases significantly compared to LSN. Merely 15% replacement of Ni with Fe increases the specific activity (mA cm−2oxide) by over an order of magnitude at 1.63 V vs the reversible hydrogen electrode corrected for electrolyte resistance (RHE-iR) as seen in Fig. 2b. Further substitution of Fe for Ni yields a volcano-like catalytic trend with 30% Fe substitution in LSNF30 being the most active composition. LSNF30 displays exceptionally high catalytic activities of 32.7 mA cm−2oxide and 1930 mA mg−1oxide at 1.63 V, over 20 and 40 times higher than the respective values for LSN, with a Tafel slope of 44 mV dec−1 and achieves the common benchmark of 10 mA cm−2geo at only a 360 mV overpotential which is remarkable considering the relatively small mass loading used (Fig. 2c). Details regarding conversion of potentials from Hg/HgO to RHE can be found in the Methods and Supplementary Figure 8. Figure 2b and Supplementary Figure 9 demonstrate the significantly higher mass activity of LSNF30 compared to other leading metal oxide OER catalysts with LSNF30 being over five times more active than the recently reported SrCoO2.7 (1930 vs 332 mA mg−1oxide) and over an order of magnitude better than IrO2 (173 mA mg−1oxide), a leading precious metal oxide benchmark catalyst. The LSNF30 composition generates three times as much current per surface area as SrCoO2.7 (32.7 vs 9.2 mA cm−2oxide) and over an order of magnitude more than IrO2 (1.2 mA cm−2oxide) at 1.63 V (Supplementary Table 2). The catalytic activity of VC is negligible, contributing only 7 mA mg−1 (Supplementary Figures 7 and 9) at 1.63 V. Cyclic voltammetry (CV) experiments using a rotating ring disk electrode (RRDE) were performed to ensure the measured currents for LSNF30VC were due to oxygen evolution and not carbon oxidation or other reactions. As can be seen in Fig. 2d, at 1.63 V, the same potential at which we base our activity measurements, the measured collection efficiency of 34% closely matches the theoretical collection efficiency. While carbon corrosion may become a factor at much higher potentials where the VC support would oxidize, at the potentials we use to examine the catalyst in this fundamental context the only current measured is due to oxygen evolution, lending further validity to the trends we observe. Additional experimental details for RRDE experiments can be found in the Methods section and Supplementary Figure 10. In the absence of the VC support, much lower activities were observed (Supplementary Figure 11) due to the lack of a carbon matrix to increase conductivity, however, the same volcano trend in activities was observed across the LSNF series and LSNF30 exhibited catalytic activity comparable to IrO2. Supplementary Table 2 summarizes the catalytic activities of other promising catalysts to enable comparison with LSNF30 using multiple metrics. Examined in the context of both precious and non-precious metal OER catalysts, LSNF30 is one of the most active catalysts ever reported for the OER.

The stability of LSNF30 was investigated using multiple types of electrochemical tests. One such experiment was a galvanostatic current hold during which the supported catalyst sustained 10 A g−1ox for over 24 h without failure (Supplementary Figure 12). To further investigate the stability of the catalyst both supported and unsupported LSNF30 materials were drop cast at 1 mg cm−2 onto Ni foam electrodes and cycled 100 times in 0.1 M KOH. The currents measured at 1.63 V on the Ni foam that is capable of performing the OER on its own, both drop cast with VC and without, were subtracted out. As can be seen in Fig. 3 and Supplementary Figure 13 the OER current generated by the LSNF30VC composite stabilizes very quickly and displays a much higher mass activity than the unsupported catalyst due to the added conductivity of the composite that comes from the VC support. These activities are much lower than measured on RDE due to the inefficient catalyst utilization that comes from using higher mass loadings as well as mass transport limitations and the buildup of oxygen on the electrode without rotation. These stability experiments demonstrate that while a small amount of amorphization may occur at the surface during the first CV (Supplementary Figure 14) as a result of wetting or an initial restructuring such has been seen for other perovskite catalysts34 and as was seen for the bare Ni foam electrodes, the exceptionally high activities we observe are due to the covalency imparted by Sr substitution into the crystalline RP phase and the stability of the structure with repeated cycling. Were a transformation to amorphous oxyhydroxide phases taking place and governing the catalytic activity of the LSNF materials then we would expect much lower currents due to the decreased surface areas of active sites formed at high temperature as well as the majority of oxide mass that is made up of catalytically inactive La and Sr sites. The stability of LSNF materials was further studied using DFT and is discussed below.

Fig. 3
Fig. 3

Cyclic voltammetry stability tests of LSNF30 dropcast on Ni foam electrodes at 1 mg cm−2. a One hundred cycles of LSNF30 supported at 30 wt% on VC performed in O2-saturated 0.1 M KOH at 10 mV s−1. b Mass activities measured at 1.63 V for both LSNF30VC and unsupported LSNF30 at various points during the 100 cycle stability tests. Mass activities were calculated by subtracting the current at 1.63 V for an Ni foam electrode with or without carbon but without catalyst from the current measured from the catalyst on Ni foam with or without the VC support and then dividing by the mass of catalyst used

Chemical states and electronic structure

Upon exposure to alkaline electrolyte the surface of the catalyst is hydroxylated and reduced. The Ni2+/3+ redox couple in LSNF is observed to shift to more positive potentials with Fe substitution, indicating a direct modulation of Ni’s reactivity with Fe substitution. This redox couple exists in the incipient OER region, as indicated in the reversible CV peaks in Fig. 4a. The potential range over which the redox peaks are observed is consistent with prior studies of Ni-based electrocatalysts3,35,36 with Fe substitution shifting the peak potential (EP) of Ni2+/3+ oxidation as documented with Ni–Fe oxyhydroxides3,4,35. Integration of the oxidation waves (Supplementary Figures 15 and 16) reveals that the specific oxidative charge (µC cm−2oxide) transferred during oxidation/intercalation consistently decreases upon continued replacement of Ni with Fe, with the exception of the initial introduction of Fe in LSNF15 (Fig. 4b). Similar behavior was previously reported for 10% Fe substitution into NiOOH hydroxide electrodes3 and was speculated to be due to increased oxygen and electrolyte diffusivity. This interpretation is supported here by the increased electrochemical oxygen diffusion rate measured in LSNF15 as compared to LSN (1.04E−12 cm2 s−1 vs 8.03E−13 cm2 s−1; Supplementary Figure 17 and Supplementary Table 3) and confirms that along with the surface redox of Ni2+/3+, oxygen intercalation concomitant with Ni redox is likely given the labile nature of oxygen in La2NiOδ. The observation that the pH dependence of the Ni2+/3+ oxidation Ep in Supplementary Figure 14 behaves like a Nernstian pseudocapacitor using OH as the intercalating ion further indicates that the intercalation of oxygen is taking place14,33,37,38.

Fig. 4
Fig. 4

Cyclic voltammetry (CV) of LSNF catalysts in O2-saturated 0.1 M KOH. a CVs of LSNF at 100 mV s−1 revealing a systematic anodic shift in Ni2+/3+ oxidation/intercalation potentials with increasing Fe substitution. CVs at 100 mV s−1, taken after 3–4 cycles, are depicted to aid the reader in distinguishing peak potential shifts and relative areas, but at 100 mV s−1 contributions to EP from capacitance and mass transport resistance cannot be ignored. To address this, peak potentials reported in Supplementary Figure 8c were taken from stable CVs at 10 mV s−1. b Specific oxidative charge (µC cm−2oxide) resulting from the integration of oxidation waves. Integrations were performed using specific current density (µA cm−2oxide) to normalize differences in catalyst surface area (Supplementary Figure 8d). The OER baselines for stable CVs at 10 mV s−1 were fit and subtracted. Supplementary Figure 14 contains the CVs used for integration

It is known that over 50% Sr substitution for La induces metal-like conductivity25,39 in the charge transfer insulator La2NiOδ due to hole doping in the O 2p band40. Furthermore, the remarkable improvement of the catalytic activity of LSN upon Fe substitution for Ni may be explained by the impact of the Fe 3d states on the electronic structure of LSNF. Earlier studies of the electronic structure of La1.1Sr0.9Ni0.8Fe0.2Oδ with resonant photoemission spectroscopy suggest that the Fe 3d states make a substantial contribution to the valence band near the Fermi level (EF) by strongly hybridizing with the O 2p and Ni 3d states which facilitates cation oxidation and redox processes28. The mixed Fe 3d and Ni 3d bands pinned at EF in close proximity to the O 2p band should give rise to a mixture of Ni3+/4+ and Fe3+/4+ where the relative proportion of oxidation states changes with the amount of Fe substitution27,29,41. This was confirmed by ex situ room temperature Mössbauer spectroscopy (Supplementary Figures 18 and 19, Table 1) in conjunction with iodometric titrations. Knowing the average B-site oxidation state as well as the oxidation state of Fe allows for the calculation of the Ni oxidation state and Table 1 contains the results of this analysis. The average oxidation state of Ni increases with increasing Fe content from +3.54 in LSN to +3.95 in LSN85, as does the oxygen hyperstoichiometry (δ) and the average B-site oxidation state. The increase in the oxidation state of Ni is further demonstrated by the observation that the Ni 3p spectrum obtained by X-ray photoelectron spectroscopy (XPS) shifts to higher binding energies with increasing Fe content (Supplementary Figure 20), and again by the positive shift in potential of the Ni2+/3+ redox features upon Fe substitution (Fig. 4a). Fitting parameters for Mössbauer spectroscopy can be found in Supplementary Tables 4 and 5. Additional discussion of oxygen stoichiometry and LSNF oxidation states can be found in Supplementary Note 1.

Table 1 Oxygen hyperstoichiometry (δ) and B-site oxidation states in La0.5Sr1.5Ni1−xFexOδ

To further understand the electronic structure evolution across the LSNF series and its implications for the OER activity, as well as confirm the results of the Mössbauer spectroscopy and iodometric titrations, we model the bulk phase of LSNF and a simplified Sr2Ni1−xFexO4 (SNF) series by DFT. While the SNF system was not investigated experimentally, it was modeled to confirm that the same trends in electronic structure evolution that occur in LSNF also take place in a sample with a different A-site composition. Additionally, modeling the SNF series also eliminates a possible source of variation between the atomic arrangements of A-site elements in the modeled LSNF system vs the arrangements in the synthesized samples and verifies our results on a simplified catalyst system.

A series of LSNF compositions are modeled by 2 × 2 × 1 primitive unit cells, allowing for unit compositions of La0.5Sr1.5NiO4 (LSN), La0.5Sr1.5Ni0.75Fe0.25O4 (LSNF25), LSNF50, LSNF75, and LSF. The SNF series was modeled using the same Ni and Fe ratios, and details regarding cell formation and magnetic investigation are given in the Methods and Supplementary Note 2. Figure 5a, b shows the (001) atomic layers of the most stable LSNF structures based on our screening. First, we look at LSN (Fig. 4a) and we find a uniform, proportional distribution of La/Sr42. Using this La/Sr distribution we determine the minimum energy Ni/Fe ordering which results in two key features governing the Fe arrangement in LSNF (Fig. 5b). First, each of the two B(B′)O2 layers has an equal number of Fe cations in order to prevent an unbalanced charge distribution between them. Second, the Fe cations in each B(B′)O2 plane are distributed such that the number of Fe–O–Ni bridges is maximized2. This arrangement mitigates the effects of the induced O 2p electron hole at Ni–O–Ni bridges due to more effective electron donation by Fe at Fe–O–Ni bridges, which increases stability18. Compared with Fe–O–Fe bridges, the Fe–O–Ni bridges induce shorter Fe–O bond lengths and indicate higher Fe oxidation states, a trend that also occurs in the simplified SNF system. This observation agrees with the experimentally observed predominance of Fe4+ over Fe3+ at low Fe substitution as well as the increase in unit cell parameters as Fe content increases (Fig. 1d, Supplementary Table 1).

Fig. 5
Fig. 5

Density functional theory modeling of atomic and electronic structures of bulk LSNF in ferromagnetic configuration. a The ground state 2 × 2 × 1 cell of La0.5Sr1.5NiO4, with uniformly distributed La in each [001] AO layer. b Representations of the two B(B′)O2 layers for each ground state La0.5Sr1.5Ni1−xFexO4, with x at 0, 0.25, 0.5, 0.75, and 1; for each x, the ground state Fe arrangement is characterized by equal numbers of Fe in the two B(B′)O2 layers, with the Fe in each layer arranged to maximize the number of Fe–O–Ni bridges. c The corresponding spin polarized PDOS of eg (Ni: gray shaded area and Fe: blue line) and 2p (O: red line) with respect to Fermi level (\(E_{\mathrm {F}}^0\)) for the B–O–B′ bridges; the PDOS are the average of existing B–O–B′ bridges; the adapted Fermi level (\(E_{\mathrm {F}}^\delta\)) to oxygen hyperstoichiometry is estimated via the rigid band model, with \(E_{\mathrm {F}}^\delta = E_{\mathrm {F}}^0 - 2e^ - {\mathrm{\delta }}/{\mathrm{DOS}}(E_{\mathrm {F}}^0)\) (Eq. (1)), where \({\mathrm{DOS}}(E_{\mathrm {F}}^0)\) is the total density of states at \(E_{\mathrm {F}}^0\) per formula unit of LSNF. d Top: Computed values of the O–p band center (top panel), with La2NiO4 calculated as reference. Middle: The magnitude of band overlap, determined by the integration of maximum PDOS between eg(B) and eg(B′) from −2 to 2 eV, normalized to eg(Ni) in LSN. Bottom: The corresponding overlap center (centroid) of maximum PDOS between eg(B) and eg(B′). Additional details can be found in Supplementary Note 2

The computed projected density of states (PDOS) of the Fe–O–Ni bridges in both LSNF and SNF confirm that the Ni cations are in the low-spin state with fully occupied \(t_{2g}^ \downarrow\) states (Supplementary Figures 2123) while the Fe cations are in the high-spin state with mostly unoccupied \(t_{2g}^ \downarrow\) states for all LSNF and SNF43. These spin states lead to eg bands positioned around the Fermi level \((E_{\mathrm {F}}^0)\), thus becoming the most relevant for Fe–O–Ni interactions of interest and the focus of our study. Inspection of the Fe–O–Ni bridges reveals significant overlap of O 2p, Ni \(e_g^ \uparrow\) and Fe \(e_g^ \uparrow\) bands for all compositions in the LSNF series (Fig. 5c), in agreement with our predictions. The same overlap is observed in the SNF series with only a small downward shift in EF due to increased oxidation of the B-site elements to differentiate the two (Supplementary Figure 23). This overlap leads to two important observations. First, the unoccupied O 2\(p^ \uparrow\) states indicate oxygen electron holes with finite PDOS across \(E_{\mathrm {F}}^0\), thus bridging charge transfer between neighboring cations32,43. Second, the similar energies of the Ni and Fe \(e_g^ \uparrow\) states (denoted Band I and Band II in the following) open up the possibility of electron exchange through oxygen. These two factors govern the evolution of the PDOS from LSN to LSF and from SN to SF. On the one hand, the substitution of Ni by less electronegative Fe stabilizes O 2p electrons and increases the Ni–O distances, shifting the O 2p band center downwards relative to EF (Fig. 5d, Supplementary Figure 23) and decreasing the bandwidth43 which reduces electron hole concentration and charge transfer ability44. This condition is consistent with the experimentally observed increase in oxygen hyperstoichiometry going from LSN to LSF (Table 1, Supplementary Table 3). On the other hand, the partially filled Band II (Fe) significantly hybridizes with both O 2p and Band I (Ni), driving the latter towards \(E_{\mathrm {F}}^0\). Both Bands I and II make significant contributions to the occupied (valence) and unoccupied (conduction) states, respectively, and this dramatically increases the bandwidth of the triple band overlap going from LSN to LSNF50 and from SN to SNF50, with its center approaching \(E_{\mathrm {F}}^0\). As the eg states are relevant for surface chemisorption, the increasing bandwidth around \(E_{\mathrm {F}}^0\) would decrease the energetic cost to accept/donate electrons28 at the adsorbate-catalyst interface, and therefore should increase the rate of reaction according the Gerischer–Marcus model of charge transfer45. The increased Fe concentrations in LSNF75 and SNF75, however, drive Band I (Ni) into the similar distribution of Band II (Fe) and this reduces the bandwidth (Fig. 5d). This suggests that the optimal OER activity will occur for a composition between LSNF25 and LSNF50, consistent with experimental observations. Although these calculations are performed for the bulk structure of LSNF, the surface electronic structure is expected to be strongly correlated to that of bulk, similar to ABO3 perovskites as was demonstrated in previous work46, thus preserving the key feature of Ni–O–Fe hybridization and its evolution across LSNF and SNF compositions.


The computed band structure of LSNF is similar to that reported for other highly active OER catalysts, especially those compositions with mixed transition metal sites such as Ni–Fe layered double hydroxide catalysts2. Conesa calculated the DOS of one such polymorph, FeNi7O8(OH)8 in the 2HC structure with Fe in O4(OH)2 coordination, and their result is strikingly similar to that of LSNF in that Ni and Fe 3d bands are strongly hybridized just above EF. They concluded that Fe4+ is stabilized by induced charge transfer between Ni sites, which is also seen in Ni–Fe oxyhydroxides6, and this explanation agrees with our observation of Fe in the 4+ oxidation state in LSNF (Table 1). The shifting of the Ni2+/3+ redox couple upon Fe substitution that we observe (Fig. 4) has previously been reported in NiOOH upon incorporation of Fe and is further evidence of this partial charge transfer between Fe and/or Ni4,5,47. A change in covalency by the introduction of FeO6 units into LSN must have an inductive effect on Ni through next nearest neighbor interactions via Fe–O–Ni bridges48, which is consistent with the observation that our activity is maximized for the composition having the highest probability of Fe–O–Ni bridging interactions, LSNF30.

The band structure of LSNF also resembles the computed band structures of LaCo1−xFexO3(ref.49), Sr2−xLaxMOδ(ref.50), and Ba0.5Sr0.5Co0.75Fe0.25Oδ (BSCF)51. Merkle calculated the band diagram for BSCF and found a similar electronic configuration as in LSNF, and Schmidt and co-workers saw that the catalytic activity of Ba0.5Sr0.5Co0.8Fe0.2Oδ was much higher than that of Ba0.5Sr0.5CoOδ(ref.34). Thus it is possible that the high activity of BSCF, SrNb0.1Co0.7Fe0.2O3−δ34,52 as well as others with similar mixed transition metal sites may be rationalized not just by the covalent bonding, but also by triply-overlapping Co/Ni and Fe 3d states with O 2p near EF similar to the LSNF series, which has largely been overlooked up to now. Furthermore, the similarities between the band structures of LSNF materials and these other active catalysts of varying structures, some of them amorphous, reinforces how the principle of cross-gap hybridization may apply to many different metal oxide catalysts and applies to the LSNF series even in the event of surface restructuring.

As we have discussed in our previous work, the OER can proceed by the adsorbate exchange mechanism (AEM) or the LOM mechanism14,18. In the AEM, chemisorbed intermediates undergo a series of electrochemical oxidations as the transition metal active site undergoes oxidation and reduction, and these redox reactions are the most energetically intensive and thus rate limiting steps14. The LOM OER mechanism, on the other hand, does not require significant redox switching of transition metal sites but instead requires the participation of lattice oxygen in the OER. Ligand holes that arise when transition metal 3d bands are highly covalent with O 2p bands and exist around \(E_{\mathrm {F}}^0\) activate lattice oxygen that combines with chemisorbed OH to produce O2. In previous studies we found that the DFT-computed Ovac formation energy in bulk ABO3 perovskites (donated as \(\Delta E_{V_O}\)) served as an effective indicator of OER mechanism18. Highly covalent perovskites favor Ovac formation that results from an overall high-energy lying O 2p band relative to \(E_{\mathrm {F}}^0\) and the appearance of electron holes that facilitate reversible lattice oxygen participation under OER conditions. Employing \(\Delta E_{V_O}\), we showed that the mechanism for oxygen evolution switches from the AEM to the LOM with decreasing \(\Delta E_{V_O}\) for the LaxSr1−xCoO3−δ series when x > 0.4 (ref.14). The decrease in oxygen vacancy formation energy in these materials occurred in concert with an increase in oxygen diffusion rates and OER activity14. This proposed mechanistic switch was experimentally confirmed by a recent report from the Shao Horn group who used isotopic labeling of lattice oxygen to observe a transition from the AEM on LaCoO3 to the LOM on La0.5Sr0.5CoO3−δ and SrCoO3−δ17.

The same type of band overlap and resulting covalency that is a requirement of the LOM mechanism and that occurs in the previously reported materials discussed above also occurs in LSNF. The hybridization of eg(Ni) and eg(Fe) bands with the p(O) band across \(E_{\mathrm {F}}^0\) results in increased oxygen electron holes, and DFT computations reveal that \(\Delta E_{V_O}\) in LSN, LSNF25, and LSNF50 at Ni–O–Fe bridges is more negative than in LaNiO3 and La0.5Sr0.5CoO3−δ18 while \(\Delta E_{V_O}\) in LSNF75 and LSF is larger (Supplementary Table 6). Thus \(\Delta E_{V_O}\), a proven indicator of the LOM mechanism, works in conjunction with the experimentally measured increased oxygen diffusion rates from LSN to LSNF45 (Supplementary Figure 17, Supplementary Table 3), to suggest that the exchange of surface lattice O plays a key role in OER and that the highly active LSNF materials utilize a LOM-type mechanism. The catalytic effect from the LOM mechanism is further enhanced by the substitution of Fe that causes broadening of eg bandwidth through Ni–O–Fe cross-gap hybridization. Altogether this demonstrates how the LOM applies to a new series of materials and solidifies the importance of both increased covalency that results in oxygen electron holes, as well as the cross-gap hybridization that causes broadening of the overall bandwidth near EF in the design and optimization of oxide catalysts.

We have precisely synthesized a series of RP catalysts having highly oxidized and covalent Ni 3d–O 2p–Fe 3d bonds that give rise to exceptional OER activity. Sr substitution into the perovskite LaNiO3 has previously been proposed as an avenue to increase the oxidation state if Ni and Ni–O covalency but has not been fully realized. In this work we were able to avoid inactive secondary phases resulting from poor solubility of Sr in the perovskite phase through utilization of the RP crystal structure. Additionally, by using La0.5Sr1.5NiOδ as the host lattice we achieved complete substitution of Fe for Ni across the entire compositional range. The crystalline RP structure and the high degree of phase purity enabled precise study of the impact of Fe substitution on the chemical and electronic properties of the LSNF series, something that has not been possible up to this point with other, amorphous materials. Iodometric titrations coupled with Mössbauer spectroscopy indicate that the average Ni oxidation state in the LSNF series increases from +3.46 to +3.95 with increasing Fe substitution while the Ni2+/3+ redox peaks also shift to more positive potentials, consistent with Ni developing a more oxidized character. The influence of Fe substitution extends beyond increasing the oxidative strength of Ni, however, as the electrocatalytic activity increases by over an order of magnitude from LSN to LSNF30 despite possessing statistically equivalent Ni oxidation states. DFT calculations reveal that Fe substitution results in cross-gap hybridization where the Fe 3d eg band is hybridized with both the Ni 3d eg and the top of the O 2p density of states across the Fermi level. The increased covalency of the Ni–O bonds as well as facile charge transfer through Fe–O–Ni bridges due to incorporation of Fe explains the enhanced catalytic activity going from LSN to LSNF30. Furthermore, the increased covalency demonstrated via calculated partial density of states for LSNF and a simplified SNF that is a requirement for the OER to take place via a LOM mechanism resembles the band structure of other highly active OER catalysts with varying crystal or amorphous structures for which this mechanism has already been verified. Decreased oxygen vacancy formation energies and increased rates of oxygen diffusion, descriptors already accepted in the literature as indications of the LOM, are seen on LSNF and further support the hypothesis that the OER proceeds via a LOM mechanism on LSNF. This methodology of selective A- and B-site substitution to promote cross-gap hybridization in RP oxides reveals important fundamental aspects related to their structure and the exceptional electrocatalytic activities of these materials as well as other metal oxide catalysts.



All chemicals were used as they were received from manufacturers. Lanthanum(III) nitrate hexahydrate (99.995%), strontium(II) nitrate hexahydrate (99%), nickel(II) nitrate hexahydrate (99%), iron(III) nitrate non-ahydrate (99.99%), tetramethylammonium hydroxide pentahydrate (TMAOH, 99%), diethylene glycol (DEG, 99.99%), citric acid monohydrate, 2-propanol, ethylenediaminetetraacetic acid, and potassium hydroxide (KOH) were purchased from Fisher Scientific. Absolute 200 proof ethanol was obtained from Aaper Alcohol. 5 wt % Nafion solution in lower alcohols and IrO2 powder were obtained from Sigma-Aldrich. Millipore high-purity water (DI water, 18 MΩ) was used in all experiments and synthesis and research grade, 99.999% purity oxygen and argon gases were purchased from Praxair. Vulcan XC72 carbon (VC) was purchased from Cabot Corporation and ball-milled prior to use.

Catalyst synthesis

La0.5Sr1.5Ni1−xFexOδ (LSNF, x = 0 to 1) samples were synthesized using a modified Pechini method29 followed by crystallization and annealing. A- and B-site nitrate salts, in stoichiometric ratios, were dissolved in water to create a solution in which the total concentration of metal salts was 0.1 M. Citric acid and EDTA were added, each at a concentration of 0.1 M, and then 1 M TMAOH was added dropwise until the pH had reached 7.5 in order to deprotonate and dissolve the EDTA. DEG was then injected to reach a concentration of 0.067 M and the solution was heated to 85 °C while stirring. The EDTA and citric acid were both added to ensure complete chelation of the metal cations, preventing agglomerations or particle formations that may lead to catalyst inhomogeneity. DEG and heat were added to the solution to drive a dehydration reaction between the polyhydroxyl alcohol and the carboxylic acid groups of the chelates to form a polyester gel. Once all the water had been evaporated the gel was combusted on a hot plate at 350 °C to form mixed metal oxide precursor particles. This step was performed on a hot place and not in a sealed tube furnace to avoid possible explosions from rapid evolution of gasses upon combustion. Finally, precursor particles were crystallized at 950 °C (heated at 20 °C min−1) for 5 h, then cooled to 400 °C and left to anneal for 6 h in a tube furnace. The entire crystallization and annealing routine was done under pure O2 flowing at 200 mL min−1. Catalysts were recovered and immediately stored under Ar gas to prevent catalyst surface amorphization. Total catalyst yields per synthesis ranged from 500 to 750 mg. More details regarding the synthesis can be found in Kakihana et al.31

SrCoO2.7 and LaNiO3 were synthesized via a coprecipitation method previously reported elsewhere13,46 in which A and B-site nitrate salts in a 1:1 ratio were dissolved in a 1 wt% solution of TMAOH containing an equimolar amount of TPAB to the total moles of metal cations in order to form mixed metal hydroxide precursor particles. These solutions were flash-frozen on a rotating metal drum that had been cooled to cryogenic temperatures and was collected before lyophilization to remove water. The precursor particles were then calcined at 700 °C (LaNiO3) or 950 °C (SrCoO2.7) to form the perovskite phase.

Electrochemical characterization

To make catalyst inks 2 mg of catalyst powder were added to 2 mL of NaOH neutralized 0.05 wt% Nafion solution47 and bath sonicated for at least 1 h. Ten microliters of catalyst ink was drop cast onto 5 mm glassy carbon electrodes (GCE) from Pine Instruments and dried in air overnight. All GCEs were polished before drop casting via sonication in a solution of equal parts water and ethanol followed by polishing using 0.05 μm alumina powder after which they were again sonicated in a fresh solution of water and ethanol and dried in ambient air. This method was used to clean all GCEs prior to drop casting, after which a composite catalyst loading of 51 μgtotal cm−2geo, yielding 15.3 μgoxide cm−2geo was achieved for catalysis and intercalation tests.

CH Instruments CHI832a or Metrohm Autolab PGSTAT302N potentiostats were used to carry out all electrochemical testing. Potentiostats were equipped with high-speed rotators from Pine Instruments. Experiments were performed at room temperature in 0.1 M KOH (measured pH ≈ 12.8). Electrolyte resistance was measured using current interrupt and positive feedback methods (46 Ω) and iR compensation was applied to all electrochemical measurements after testing unless otherwise noted. A 3 electrode cell was used for all experiments. The reference electrode was a CH Instruments Hg/HgO (1 M KOH) reference electrode, a Au wire served as the counter electrode, and GCEs drop cast with catalyst ink and dried as described above were used as the working electrode. All potentials were measured vs Hg/HgO but were reported vs the reversible hydrogen electrode (RHE), which was determined experimentally to be +0.8976 V vs. Hg/HgO (1 M KOH). Supplementary Figure 8 contains the RHE calibration data.

All testing for OER activities was performed on newly dropcast electrodes which had not undergone previous testing, dropcast with 30 wt% catalyst on VC (15.3 μgoxide cm−2geo) or unsupported catalyst. CV scans were performed from 1 to 2 V vs RHE at a scan rate of 10 mV s−1 while rotating at 1600 rpm in O2-saturated 0.1 M KOH. The anodic and cathodic scans were averaged and iR corrected, and the current at 1.63 V vs RHE-iR was used for comparison of OER activities. Scatter in the data at high current densities is due to oxygen bubble formation and desorption on the electrode surface. Data presented in this report are the average of at least three tests on fresh electrodes. OER testing using Ni foam supports were performed under the same electrolyte conditions but dropcast at 1 mg cm−2 and held stationary.

All CVs were taken on fresh electrodes of 30 wt% oxide on VC. All catalysts were first conditioned by performing 20 cycles from 1.26 to 1.55 V vs RHE at 100 mV s−1. Immediately following, three cycles at 100, 50, 25, 10, and 5 mV s−1 were collected. Unless otherwise stated, all cycles shown are the third cycle at a given scan rate. For samples containing more than 50% Fe substitution, it was necessary to perform four cycles at each scan rate. Additionally, LSNF85 had to be cycled to 1.575 V before any oxidative features were observed.

For comparison of charge passed for all oxidative waves, the last cycle at 10 mV s−1 was used to compute specific current density. The baseline of each CV was fit and subtracted from the specific current density. The background subtracted CVs (Supplementary Figure 16) were then integrated to find the total charge transferred.

All RRDE tests were performed in argon-saturated, 0.1 M KOH on fresh 30 wt% oxide films. LSNF30 was cycled at 10 mV s−1 on the disk while the Pt ring was held at −0.4 V vs. RHE. One-fourth the normal geometric loading of catalyst was used (3.8 μgoxide cm−2geo) to limit the amount of oxygen generated a minimize bubble formation which reduces collection efficiency. Additional information regarding the RRDE calibration data can be found in Supplementary Figure 10.

All oxygen diffusion tests were performed in argon-saturated, 1 M KOH on fresh 85 wt% oxide films. Each LSNF composition was cycled at 20 mV s−1 until the oxidative peak potential did not change upon further cycling. Chronoamperometry was then performed at potentials 10 mV more anodic than Ep to ensure diffusion-limited intercalation. Linear regression was performed as described elsewhere48,49 to determine the diffusion rate. Particle sizes were estimated using the surface area calculated from BET measurements and densities determined by Rietveld analysis. All values reported are the average of at least three tests.

Iodometric titrations

Iodometric titrations were performed following the procedure referenced above13. In this procedure 3 mL of 2 M KI solution that had previously been deoxygenated were combined in a flask with 15–20 mg of perovskite and stirred for 3 min under argon, after which 25 mL of 1 M HCl was added to dissolve the perovskite. The solution was then titrated with a solution of ~26 mM solution of Na2S2O3 that had been pre-standardized with 0.1 N KIO3 until a faint golden color was reached, after which a starch indicator was injected and the titration was continued until the solution was clear, marking the end point.

Catalyst preparation and support

Fresh, Ar-sealed catalysts were ball milled for 3 min using a Wig-L-Bug spectroscopic grinding mill. To support the catalysts onto VC, the correct amounts of pre-ground catalyst and pre-ground VC were measured into the grinding mill’s vial and ball milled for 3 min.

Powder X-ray diffraction (PXRD)

Catalyst structure was examined by performing X-ray diffraction with a Rigaku MiniFlex600 Diffractometer. Measurements were performed at 298 K in ambient conditions while the instrument operated at 40 kV and 15 mA using Cu Kα radiation (1.54 Å wavelength). For all tests, argon-sealed catalyst powder was exposed to ambient air and scanned over 10–100° 2θ in 0.01° increments with a dwell time of 0.35 s per step. PXRD patterns for the Rietveld refinement were taken with a Huber G670 Guinier diffractometer (Cu Kα1 radiation; curved Ge(111) monochromator; image plate). The refinement was performed with the JANA2006 package50. As the electron diffraction patterns of all compositions revealed no deviation from the RP n = 1 I4/mmm structure, the La2NiO4 structure51 was used as a starting model. The La/Sr occupancy factors of the A positions were refined; the Fe/Ni occupancy factors for the B positions were assigned according to the results of the EDX analysis. The crystallographic data, positional and atomic displacement parameters, interatomic distances, and reliability factors are listed in Supplementary Table 1.

Surface area analysis

Catalyst surface areas were measured via nitrogen sorption analysis which was performed at a temperature of 77 K on a Quantachrome Instruments NOVA 2000 high-speed surface area BET analyzer. Before BET experiments were performed, all catalyst materials were ball milled for 3 min followed by degassing under vacuum at room temperature for at least 12 h. Only data in the relative pressure range (P/P0) of 0.05 to 0.30, with a minimum R2 of 0.995 and C value of 20 was used to calculate the specific surface area using the BET method.

Transmission electron microscopy

Preparation of TEM samples was performed by mixing the crystals with ethanol and crushing them in a mortar, after which drops of the suspension were deposited onto holey carbon grids. Electron diffraction patterns, TEM images, HAADF-STEM images, ABF-STEM images, and energy dispersive X-ray (EDX) spectra were collected using an aberration-corrected Titan G3 electron microscope equipped with a Super-X EDX system, operating at 200 kV using a convergence semi-angle of 21.6 mrad.

Mössbauer spectroscopy

57Fe Mössbauer spectra were collected using a constant acceleration spectrometer MS1104 (Rostov-na-Donu, RF) in transmission mode with a 57Co/Rh γ-ray source. Calibration of the spectrometer was performed using standard sodium nitroprusside absorbers. All isomer shift values (IS) are referred to α-Fe at room temperature and spectra evaluation was performed using “UnivemMS” (Rostov-na-Donu, RF) and custom least squares fitting software with Lorentzian–Gaussian line shapes. Details regarding the deconvolution of the spectra are found in the text accompanying Supplementary Figure 18.

DFT modeling

The Vienna Ab initio Simulation Package (VASP) was used to do spin polarized calculations52, using the PAW pseudopotentials and the exchange-correlation functional of Perdew–Burke–Ernzerhof (PBE), with the effective Hubbard Ueff of 5.3 (Fe) and 6.2 eV (Ni), respectively. The Ruddlesden–Popper bulk phase is modeled by fully relaxing a 2 × 2 × 1 primitive unit cell, La(Sr)16Ni(Fe)8O32, with a plane wave cutoff energy of 520 eV, Monkhorst-Pack k-point of 4 × 4 × 2, forces convergence criterion of 10–4 eV Å−1 and Gaussian smearing, where the smearing width is 0.1 eV. All models follow ferromagnetic ordering, as our calculations indicate its lower energy than those of nonmagnetic and antiferromagnetic orderings (A, C, and G type). Details regarding the determinations of effective Hubbard Ueff, atomic, magnetic and electronic structures, and oxygen hyperstoichiometry effects are provided Supplementary Note 2.

X-ray photoelectron spectroscopy

Characterization of the chemical states was done using a Kratos AXIS Ultra DLD XPS and a monochromatic Al X-ray source (Al α, 1.4866 eV), scanning in 0.1 eV steps with a dwell time of 4 s per step. Charge compensation was used for all samples. Binding energies were for all spectra were calibrated against the adventitious carbon peak at 285 eV. CasaXPS was used for all data analysis and deconvolution. Details regarding the deconvolution of the Ni 3p spectrum are found in the text accompanying Supplementary Figure 20.

Determination of Ni and Fe oxidation states

Together, the iodometric titrations and the Mössbauer spectroscopy enable the calculation of Ni’s average oxidation state and the relative percentage of Fe3+/4+. Supplementary Figure 18 contains the deconvolution method and Mössbauer spectra.

Data availability

The authors declare that all data collected and discussed in support of the findings of this study are available within the paper and its Supplementary Information.

Additional information

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  1. 1.

    Zhu, H., Zhang, P. & Dai, S. Recent advances of lanthanum-based perovskite oxides for catalysis. ACS Catal. 5, 6370–6385 (2015).

  2. 2.

    Conesa, J. C. Electronic structure of the (undoped and Fe-doped) NiOOH O2 evolution electrocatalyst. J. Phys. Chem. C 120, 18999–19010 (2016).

  3. 3.

    Corrigan, D. A. The catalysis of the oxygen evolution reaction by iron impurities in thin film nickel oxide electrodes. J. Electrochem. Soc. 134, 377–384 (1987).

  4. 4.

    Trotochaud, L., Young, S. L., Ranney, J. K. & Boettcher, S. W. Nickel–iron oxyhydroxide oxygen-evolution electrocatalysts: the role of intentional and incidental iron incorporation. J. Am. Chem. Soc. 136, 6744–6753 (2014).

  5. 5.

    Dionigi, F. & Strasser, P. NiFe-based (oxy)hydroxide catalysts for oxygen evolution reaction in non-acidic electrolytes. Adv. Energy Mater. 6, 1600621 (2016).

  6. 6.

    Chen, J. Y. C. et al. Operando analysis of NiFe and Fe oxyhydroxide electrocatalysts for water oxidation: detection of Fe4+ by Mössbauer spectroscopy. J. Am. Chem. Soc. 137, 15090–15093 (2015).

  7. 7.

    Görlin, M. et al. Tracking catalyst redox states and reaction dynamics in Ni–Fe oxyhydroxide oxygen evolution reaction electrocatalysts: the role of catalyst support and electrolyte pH. J. Am. Chem. Soc. 139, 2070–2082 (2017).

  8. 8.

    Hunter, B. M., Gray, H. B. & Müller, A. M. Earth-abundant heterogeneous water oxidation catalysts. Chem. Rev. 116, 14120–14136 (2016).

  9. 9.

    Bockris, J. O. & Otagawa, T. Mechanism of oxygen evolution on perovskites. J. Phys. Chem. 87, 2960–2971 (1983).

  10. 10.

    Suntivich, J., May, K. J., Gasteiger, H. A., Goodenough, J. B. & Shao-Horn, Y. A perovskite oxide optimized for oxygen evolution catalysis from molecular orbital principles. Science 334, 1383–1385 (2011).

  11. 11.

    Hardin, W. G. et al. Tuning the electrocatalytic activity of perovskites through active site variation and support interactions. Chem. Mater. 26, 3368–3376 (2014).

  12. 12.

    Galasso, F. S. Structure, Properties and Preparation of Perovskite-Type Compounds (Pergamon Press, Oxford, United Kingdom, 1969).

  13. 13.

    Yagi, S. et al. Covalency-reinforced oxygen evolution reaction catalyst. Nat. Commun. 6, 9249 (2015).

  14. 14.

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

  15. 15.

    Zhou, W., Zhao, M., Liang, F., Smith, S. C. & Zhu, Z. High activity and durability of novel perovskite electrocatalysts for water oxidation. Mater. Horiz. 2, 495–501 (2015).

  16. 16.

    Man, I. C. et al. Universality in oxygen evolution electrocatalysis on oxide surfaces. ChemCatChem 3, 1159–1165 (2011).

  17. 17.

    Grimaud, A. et al. Activating lattice oxygen redox reactions in metal oxides to catalyse oxygen evolution. Nat. Chem. 9, 457–465 (2017).

  18. 18.

    Rong, X., Parolin, J. & Kolpak, A. M. A fundamental relationship between reaction mechanism and stability in metal oxide catalysts for oxygen evolution. ACS Catal. 6, 1153–1158 (2016).

  19. 19.

    Takeda, Y. et al. Synthesis of SrNiO3 and related compound, Sr2Ni2O5. J. Inorg. Nucl. Chem. 34, 1599–1601 (1972).

  20. 20.

    Oliveira, F. S., Pimentel, P. M., Oliveira, R. M. P. B., Melo, D. M. A. & Melo, M. A. F. Effect of lanthanum replacement by strontium in lanthanum nickelate crystals synthetized using gelatin as organic precursor. Mater. Lett. 64, 2700–2703 (2010).

  21. 21.

    Seki, H., Saito, T. & Shimakawa, Y. High pressure synthesis of SrFe1−xNixO3. J. Jpn Soc. Powder Powder Metall. 63, 609–612 (2016).

  22. 22.

    Sharma, I. B. & Singh, D. Solid state chemistry of Ruddlesden-Popper type complex oxides. Bull. Mater. Sci. 21, 363–374 (1998).

  23. 23.

    Amow, G., Davidson, I. J. & Skinner, S. J. A comparative study of the Ruddlesden-Popper series, Lan+1NinO3n+1 (n=1, 2 and 3), for solid-oxide fuel-cell cathode applications. Solid State Ionics 177, 1205–1210 (2006).

  24. 24.

    Zhang, Z. & Greenblatt, M. Synthesis, structure, and properties of Ln4Ni3O10-δ (Ln=La, Pr, and Nd). J. Solid State Chem. 117, 236–246 (1995).

  25. 25.

    Takeda, Y. et al. Crystal chemistry and physical properties of La2−xSrxNiO4 (0≤x≤1.6). Mater. Res. Bull. 25, 293–306 (1990).

  26. 26.

    Benloucif, R., Nguyen, N., Greneche, J. M. & Raveau, B. La2−2xSr2xNi1−xFexO4−(x2)+δ: magnetic and electron transport properties. J. Phys. Chem. Solids 50, 435–440 (1989).

  27. 27.

    Rao, C. N. R., Ganguly, P., Singh, K. K. & Ram, R. A. M. A comparative study of the magnetic and electrical properties of perovskite oxides and the corresponding two-dimensional oxides of K2NiF4 structure. J. Solid State Chem. 72, 14–23 (1988).

  28. 28.

    F Howlett, J. et al. Electronic structure, reactivity and solid-state chemistry of La2 –xSrxNi1–yFeyO4+δ. Faraday Discuss. 105, 337–354 (1996).

  29. 29.

    Gilev, A. R., Kiselev, E. A. & Cherepanov, V. A. Homogeneity range, oxygen nonstoichiometry, thermal expansion and transport properties of La2−xSrxNi1−yFeyO4+δ. RSC Adv. 6, 72905–72917 (2016).

  30. 30.

    Cohen, R. E. Origin of ferroelectricity in perovskite oxides. Nature 358, 136–138 (1992).

  31. 31.

    Kakihana, M. & Yoshimura, M. Synthesis and characteristics of complex multicomponent oxides prepared by polymer complex method. Bull. Chem. Soc. Jpn. 72, 1427–1443 (1999).

  32. 32.

    Erat, S. et al. Entanglement of charge transfer, hole doping, exchange interaction, and octahedron tilting angle and their influence on the conductivity of La1-xSrxFe0.75Ni0.25O3-δ: a combination of x-ray spectroscopy and diffraction. J. Appl. Phys. 108, 124906 (2010).

  33. 33.

    Mefford, J. T., Hardin, W. G., Dai, S., Johnston, K. P. & Stevenson, K. J. Anion charge storage through oxygen intercalation in LaMnO3 perovskite pseudocapacitor electrodes. Nat. Mater. 13, 726–732 (2014).

  34. 34.

    Fabbri, E. et al. Dynamic surface self-reconstruction is the key of highly active perovskite nano-electrocatalysts for water splitting. Nat. Mater. 16, 925–931 (2017).

  35. 35.

    Louie, M. W. & Bell, A. T. An investigation of thin-film Ni–Fe oxide catalysts for the electrochemical evolution of oxygen. J. Am. Chem. Soc. 135, 12329–12337 (2013).

  36. 36.

    Forslund, R. P. et al. Nanostructured LaNiO3 perovskite electrocatalyst for enhanced urea oxidation. ACS Catal. 6, 5044–5051 (2016).

  37. 37.

    Bhavaraju, S., DiCarlo, J. F., Scarfe, D. P., Jacobson, A. J. & Buttrey, D. J. Electrochemical oxygen intercalation in La2NiO4+δ crystals. Solid State Ionics 86, 825–831 (1996).

  38. 38.

    Conway, B. E. Electrochemical Supercapacitors (Springer, New York, NY, United States of America, 1999).

  39. 39.

    Sreedhar, K. & Honig, J. M. Low-temperature electron transport properties of La2-xSrxNiO4 with 0.5≤x≤1.3. J. Solid State Chem. 111, 147–150 (1994).

  40. 40.

    Anisimov, V. I., Bukhvalov, D. & Rice, T. M. Electronic structure of possible nickelate analogs to the cuprates. Phys. Rev. B 59, 7901–7906 (1999).

  41. 41.

    Falcón, H., Carbonio, R. E. & Fierro, J. L. G. Correlation of oxidation states in LaFexNi1-xO3+δ oxides with catalytic activity for H2O2 decomposition. J. Catal. 203, 264–272 (2001).

  42. 42.

    Ritzmann, A. M., Muñoz-García, A. B., Pavone, M., Keith, J. A. & Carter, E. A. Ab initio DFT+U analysis of oxygen vacancy formation and migration in La1-xSrxFeO3-δ (x=0, 0.25, 0.50). Chem. Mater. 25, 3011–3019 (2013).

  43. 43.

    Mogni, L. et al. Synthesis, crystal chemistry and physical properties of the Ruddlesden–Popper phases Sr3Fe2−xNixO7−δ (0≤x≤1.0). J. Solid State Chem. 178, 1559–1568 (2005).

  44. 44.

    Torrance, J. B., Lacorre, P., Nazzal, A. I., Ansaldo, E. J. & Niedermayer, C. Systematic study of insulator-metal transitions in perovskites RNiO3 (R = Pr, Nd, Sm, Eu) due to closing of charge-transfer gap. Phys. Rev. B 45, 8209–8212 (1992).

  45. 45.

    Bard, A. J. & Faulkner, L. R. Electrochemical Methods: Fundamentals and Applications (Wiley, New York, NY, United States of America, 2000).

  46. 46.

    Akhade, S. A. & Kitchin, J. R. Effects of strain, d-band filling, and oxidation state on the surface electronic structure and reactivity of 3 d perovskite surfaces. J. Chem. Phys. 137, 084703 (2012).

  47. 47.

    Corrigan, D. A., Conell, R. S., Fierro, C. A. & Scherson, D. A. In-situ Moessbauer study of redox processes in a composite hydroxide of iron and nickel. J. Phys. Chem. 91, 5009–5011 (1987).

  48. 48.

    Goodenough, J. B. Magnetism and The Chemical Bond (John Wiley and Sons, WIley, New York, NY, United States, 1963).

  49. 49.

    Duan, Y. et al. Tailoring the Co 3d-O 2p covalency in LaCoO3 by Fe substitution to promote oxygen evolution reaction. Chem. Mater. 29, 10534–10541 (2017).

  50. 50.

    Lee, Y.-L. et al. Kinetics of oxygen surface exchange on epitaxial Ruddlesden–Popper phases and correlations to first-principles descriptors. J. Phys. Chem. Lett. 7, 244–249 (2016).

  51. 51.

    Merkle, R., Mastrikov, Y. A., Kotomin, E. A., Kuklja, M. M. & Maier, J. First principles calculations of oxygen vacancy formation and migration in Ba1−xSrxCo1−yFeyO3−δ Perovskites. J. Electrochem. Soc. 159, B219–B226 (2011).

  52. 52.

    Zhu, Y. et al. SrNb0.1Co0.7Fe0.2O3−δ perovskite as a next-generation electrocatalyst for oxygen evolution in alkaline solution. Angew. Chem. Int. Ed. Engl. 127, 3969–3973 (2015).

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Financial support for this work was provided by the R. A. Welch Foundation (grants F-1529 and F-1319). X.R. and A.M.K. acknowledge support from the Skoltech-MIT Center for Electrochemical Energy Storage. Computations were performed using computational resources from XSEDE and NERSC. The Kratos XPS was funded by the NSF under grant CHE-0618242.

Author information

Author notes

    • William G. Hardin

    Present address: Exponent Failure Analysis Associates, 9 Strathmore Rd, Natick, MA, 01760, USA

    • J. Tyler Mefford

    Present address: Department of Materials Science & Engineering, Stanford University, 496 Lomita Mall, Stanford, CA, 94305, USA

  1. These authors contributed equally: Robin P. Forslund, William G. Hardin.


  1. Department of Chemistry, The University of Texas at Austin, 1 University Station, Austin, TX, 78712, USA

    • Robin P. Forslund
    •  & J. Tyler Mefford
  2. Texas Materials Institute, The University of Texas at Austin, 1 University Station, Austin, TX, 78712, USA

    • William G. Hardin
  3. Department of Mechanical Engineering, Massachusetts Institute of Technology, Cambridge, MA, 02139, USA

    • Xi Rong
    •  & Alexie M. Kolpak
  4. Center for Electrochemical Energy Storage, Skolkovo Institute of Science and Technology, 3 Nobel Street, Moscow, 143026, Russia

    • Artem M. Abakumov
    •  & Keith J. Stevenson
  5. Department of Chemistry, Moscow State University, 1 Leninskiye Gory, Moscow, 119991, Russia

    • Dmitry Filimonov
  6. McKetta Department of Chemical Engineering, The University of Texas at Austin, 1 University Station, Austin, TX, 78712, USA

    • Caleb T. Alexander
    • , Hrishikesh Iyer
    •  & Keith P. Johnston


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R.P.F. and W.G.H. performed the synthesis, X-ray diffraction, iodometric titrations, and electrochemical characterization. A.M.A. performed HAADF-STEM, ABF-STEM, SAED, energy dispersive X-ray measurements, and crystallographic analysis. D.F. performed Mӧssbauer spectroscopy and provided analysis. X.R. and A.M.K. performed density functional theory computations. C.T.A. and J.T.M. provided reference electrochemical data and intellectual contributions to this work. H.I. assisted with materials synthesis. R.P.F., W.G.H., A.M.A., X.R., A.M.K., K.P.J., and K.J.S. planned the experiments and analyzed the data.

Competing interests

The authors declare no competing interests.

Corresponding author

Correspondence to Keith J. Stevenson.

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