Catalysis of the Oxygen Evolution Reaction by 4–10 nm Cobalt Nanoparticles

Open Access
Original Paper


Electrolysis of water is key technology, not only for clean energy production, but to ensure a continued supply of hydrogen beyond fossil resources, essential to the manufacture of many chemical goods other than fuels. Cobalt nanomaterials have been widely identified as a promising candidate for the anode (oxygen evolution) reaction in this process, but much work has focused on applied materials or electrode design. Given the importance of oxidation state changes Co(III) → Co(IV) in the accepted reaction mechanism, in this work we look at size effects in small (4–10 nm) cobalt nanoparticles, where the ease of oxidation for lower cobalt oxidation states is known to change with particle size. To discriminate between geometric and chemical effects we have compared the catalysts in this study to others in the literature by turnover frequency (widely used in other areas of catalysis), in addition to the more commonly employed performance metric of the overpotential required to produce a current density of 10 mA cm−2. Comparisons are drawn to key examples of using well defined nanomaterials (where the surface are of cobalt sites can be estimated). This has enabled an estimated intrinsic turnover rate of ~ 1 O2 molecule per surface Co atom per second at an overpotential of 500 mV in the oxygen evolution reaction under typical alkaline reaction conditions (pH 14.0) to be identified.


Cobalt Nanoparticles Water splitting Oxygen evolution reaction Particle size 

1 Introduction

Hydrogen, a molecule essential for the production of many major chemicals, is currently produced almost exclusively from methane. However, in the face of concerns about diminishing fossil fuel reserves and energy security, considerable effort has been made to identify renewable sources of hydrogen, and in particular in the area of electrochemical and photochemical water splitting [1, 2]. Electrochemical water splitting would provide a means to harness renewable electricity (wind, tidal, photovoltaic) to produce hydrogen, whereas photochemical water splitting would perform both capture of solar energy and subsequent water splitting [3]. In water splitting technology, the production of oxygen at the anode, known as the oxygen evolution reaction (OER), is generally the more energy demanding/inefficient step [4]. An effective catalyst to reduce the activation energy or overpotential (η) is therefore required. A great deal of work has been conducted to identify materials for this purpose, and while precious metal oxides such as iridium or ruthenium are effective catalysts, there has been a push to identify lower-cost, earth-abundant catalysts for widespread use [4]. Work on thin films of metal oxide catalyst materials based on first row transitions metal oxides found activity Ni > Co > Fe > Mn to follow the reverse order of M–OH bond strength [5, 6], but a plethora of reports have appeared based on low overpotentials for different alloyed first row transition metals, generally working under alkaline conditions [7, 8]. Of particular note for producing stable, active catalysts are cobalt oxides and spinels [9, 10, 11, 12], in a number of cases in combination with auxiliaries such as phosphate ions [13, 14, 15]. While not generally able to operate under the less alkaline or acidic conditions seen for Ir and Ru based materials because the transition metal oxides dissolve [16], cobalt may represent an acceptable compromise of cost and performance (prices per kg in May 2017: Co: $55, Ru $2090, Ir $29,100) [17]. The phosphate system, known as “Co–Pi” is of interest as electrolysis of Co2+ salts in phosphate buffer has been able to produce a single system active for both hydrogen evolution reaction (HER) and OER at lower pHs [14, 18]. Here it has been postulated that, for OER, the phosphate acts as a proton acceptor, favoring the Co(IV) oxidation state thought to be the active species in other cobalt OER catalysts [19]. More generally, a range of cobalt nanomaterials (usually under alkaline conditions, pH 13–14) have been studied, including thin films [6], nanoparticles deposited on Ni foams [20, 21] or carbon materials [9, 22, 23] and mesoporous cobalt oxides [24].

The above idea that Co(IV) is the key active component has been supported by density functional theory (DFT) calculations, showing Co(IV)-oxyl moieties to be key precursors to the oxygen–oxygen bond forming mechanism in the case of the Co–Pi (also known as CoCat) system. The mechanism for one of the lower energy pathways they identified is shown in Fig. 1, highlighting the changes in cobalt oxidation state at the active site [25]. Strikingly, electron paramagnetic resonance investigations to identify this widely postulated Co(IV) species found only small (< 10%) quantities of Co(IV) in films of the oxide electrocatalysts [26]. This suggests that if the Co(IV) is key for activating the reaction process, then the ease of cobalt oxidation may be of paramount importance in preparing effective catalysts. Nanoparticle size effects and especially particle size dependent redox behavior has been a recent focus of work in the group of Prof. Gabor Somorjai, in honor of whom it is pleasure to contribute a paper to this issue. It is well known from other types of catalysts that small nanoparticles in general may stabilize higher oxidation states of metals [27], or increase their rate of formation [28]. For cobalt specifically, small particles (less than about 6 nm in diameter) are less active in Fischer–Tropsch type chemistry, where larger Co particles to avoid adsorbate induced restructuring or oxidation of the active metallic Co(0) are needed [29, 30, 31]. Although particle size effects have been studied for OER, this was upwards from ~ 6 nm [21], so if a similar size threshold exists for the Co(III)/Co(IV) redox couple it would be valuable to extend this range to slightly smaller nanoparticles.

Fig. 1

Cobalt catalyzed OER mechanism showing the surface radical intermediates on the injection of holes from the external circuit into incomplete cubane units of cobalt oxide: a terminal Co–OH; b Co=O oxyl; c Co(OOH) hydroperoxo; d Co(OO) peroxo; e Co–OO superoxo; f solvated O2 molecule. Cobalt oxidation states are given in Roman numerals and oxidation state of oxygen atoms in Arabic numerals by each species.

Reproduced with permission from Mattioli et al. [25]

The benchmarking of electrocatalysts for OER using ‘the overpotential required to obtain an electrode current of 10 mA cm−2’ has been adopted on a widespread basis, representing the current density required for a 10% solar-to-fuels device [32]. Technologically speaking, this has clear advantages, but in understanding the atomic level chemistry this becomes problematic, as roughness and porosity of the electrode surface mask the intrinsic catalytic properties of the material. A better material could be better either because of improved active site behavior or because of structure supporting a greater number of active sites on the 1 cm2 geometric surface area of the electrode for which the current density is measured. Much as turnover frequency (TOF) has served to provide understanding of the chemistry underlying mass activities at a given temperature in conventional thermal catalysis, it can be suggested that their potential in better understanding electrochemical materials’ performance (current density at a given overpotential) is similar, yet only sometimes considered.

In the present work we have therefore studied the OER reaction catalyzed by cobalt nanoparticles in the size range 4–10 nm to identify if any changes in activity exist in this size range, where cobalt oxidation behavior at lower oxidation states is known to vary. Particular attention has been paid to identifying the best strategy to study particle size effects; both a conventional “Tafel plot” based measurements and a more direct surface area normalized method have been used. Furthermore, we have sought to identify an estimate for the intrinsic turnover rate per surface cobalt for these cobalt nanoparticles at a specific overpotential and compared it to that calculated for other recent cobalt nanomaterials in the literature.

2 Experimental

Co2(CO)8 (96% with hexane stabiliser) was obtained from Alfa Aesar, o-dichlorobenzene (99%) and Nafion perfluorinated resin solution (5 wt% in alcohol) were obtained from Sigma Aldrich. The o-dichlorobenzene was dried by refluxing with CaH2 for 3 h and distillation under nitrogen. Oleic acid (97%) was obtained from Acros Organics. All other reagents and solvents were obtained from Fisher Scientific and used without further purification. High purity water was obtained from a Purite Neptune purification system (18.2 MΩ). Synthesis was carried out using standard Schlenk techniques under a nitrogen atmosphere. The inert gas was dried by passing through a moisture trap consisting of indicating phosphorus pentoxide and calcium chloride drying agents. All glassware was washed in a base bath (1 M potassium hydroxide in 2-propanol and water) and then rinsed with water, washed in an acid bath (1 M nitric acid) and again thoroughly rinsed with water before being air dried and then dried in a 100 °C oven overnight before use. Glassware for use in electrochemical experiments was further cleaned as outlined below.

2.1 Nanoparticle Synthesis

Synthesis of 4–10 nm cobalt nanoparticles with narrow size distribution was conducted using a previously reported method [30]. All manipulations with Co2(CO)8 were carried out in a glove box prior to dissolving in o-dichlorobenzene under N2. After evacuation of oleic acid (210 mg, 0.743 mmol) for 10 min, anhydrous o-dichlorobenzene (20 mL) was added under N2. The flask was equipped with a long Liebig condenser and gas release line to accommodate the large volume of carbon monoxide gas which is produced upon decomposition of the carbonyl precursor. While vigorously stirring, the oleic acid solution was heated to the required temperature (as monitored by a submerged K-type thermocouple). Temperature was controlled (± 0.4 °C) using a Omega CN7500 PID controller connected to an isomantle heater. Once stabilized at the required temperature (168, 172, 178 or 183 °C), Co2(CO)8 in anhydrous o-dichlorobenzene (4 mL) was injected quickly into this solution. The solution immediately turned black indicating the formation of colloidal particles. This colloidal suspension was then aged for 20 min prior to stopping heating and cooling the flask in air. O-dichlorobenzene (10 mL) and 2-propanol (99.5%, ca. 100 mL) were added to this suspension, precipitating nanoparticles, which could then be extracted by centrifugation (5000 rpm). The solid was re-dispersed and stored in hexane (98.93%) until further use. The inductively coupled plasma optical emission spectroscopy (ICP-OES) derived cobalt yield was found to be 45, 54, 61 and 76% for 3.7, 4.4, 6.3 and 9.3 nm mean diameter nanoparticle samples.

2.2 Electrocatalysis

Electrochemical data were recorded on a Metrohm Autolab PGSTAT128N computer controlled potentiostat using NOVA 1.8 software. All measurements were performed in a one compartment cell using a standard three electrode configuration. It should be noted that care was taken in the placement of the working and counter electrodes to maximise the separation so as to prevent transfer of produced gases to the opposite electrodes. Catalytic runs were collected in rapidly stirred 1 mol dm−3 KOH electrolyte (~ 30 mL) at room temperature (20 °C) and referenced to a Ag/AgCl reference electrode (Mettler Toledo InLab). Coiled Pt wire (~ 8 cm long, 0.127 mm diameter, Alfa Aesar) served as the counter electrode. Working electrodes composed of a glassy carbon electrode (BAS instruments MF-2012 with a 3.0 mm working diameter) loaded with cobalt nanoparticles, as detailed below, completed the standard three-electrode configuration. Prior to electrolysis, the solution was saturated with N2 via a glass tube for at least 20 min to remove oxygen, enabling direct comparison with prior literature [21]. (Although it has been suggested O2 saturation is preferable as it maintains a constant oxygen concentration, even over the stability experiments of 2 h the electrodes produce only a limited number of bubbles compared to the gas flow required to saturate a solution and only minimal amounts are produced during cyclic voltammetry from which the results have been primarily derived). All cyclic voltammograms were obtained with a scan rate of 10 mV s−1. Current densities were obtained by dividing by the geometric area of the glassy carbon electrode (0.0707 cm2). Chrono-potentiometry was used to assess sample stability by maintaining the current density at the working electrode at 10 mA cm−1 showing reasonable stability over several hours for the most active electrode (smallest particle size). Further details of this are discussed in the supporting information along with additional experiments using Nafion stabilizer commonly used for catalysts that do not easily attach to the electrode [33], but which in our hands was found to inhibit activity, but not stabilise the samples significantly.

To thoroughly clean the glassware a weak solution of permanganic acid and manganese heptoxide (commonly known as ‘green acid’) was prepared by slowly adding KMnO4 (1–2 crystals) to H2SO4 (33%, 10 mL). Note: The concentration should not be increased as manganese heptoxide can decompose explosively. This was contacted with all internal glass surfaces and left to soak overnight, before washing thoroughly in high purity water to remove all traces of the cleaning agent.

The glassy carbon working electrode was first polished to a mirror like finish using a 0.05 µm alumina polishing disk (Blue Helix) moistened with high purity water. The electrode was then sonicated in high purity water, acetone and high purity water (5 min ea.) and dried in air. The Pt wire counter electrode was cleaned by immersion in nitric acid (70%) for ~ 10 s followed by rinsing in high purity water, sonicating in high purity water and drying in air. The Ag/AgCl reference electrode was cleaned by rinsing thoroughly in high purity water and air drying, and stored in 3 mol dm−1 KCl when not in use.

Cobalt nanoparticles were loaded onto the electrode by a simple drop casting method. A sample of the nanoparticle solution in hexane was diluted such that a 50 µL aliquot contained the desired mass of cobalt (based on a solution Co concentration known from ICP-OES). To ensure complete dispersion of the solution, the sample was mixed on a vortex mixer (2 min) and sonicated (10 min) prior to removal of a 50 µL aliquot, which was applied one drop at a time under a bright lamp to evaporate the solvent. Once all the solution had been applied, the electrode was dried at 80 °C for 1 h to cast the nanoparticles to the surface and remove all traces of solvent. Since the electrode is embedded in a plastic holder the mass loading was scaled to account for the fact the solution dries across the whole electrode assembly surface, not just the active electrode area. The experiment in the Electronic Supplementary Material in which a Nafion stabilizer was tested was prepared in a similar manner, but with 5 µL (0.1 wt%) Nafion solution deposited on top of the sample prior to drying. Nafion stabilizer was not used in any of the other experiments described.

For the OER reaction in a pH 14.0 solution and a reference electrode using 3 mol dm−3 KCl, E° = 0.404 V versus RHE, then offset 0.210 V to account for the Ag/AgCl reference electrode. Overpotential and current densities were calculated by obtaining a linear plot 10 points either side of the point of interest and using the linear equation of a least squares fit to determine the exact value. TOF per cobalt atom calculations assume 100% faradaic efficiency with 4 electrons per oxygen molecule produced and the amount of cobalt present is derived from ICP-OES analysis. TOF per surface cobalt atom was then obtained by estimating the geometric area, assuming the particles are spherical, of the surface of Co3O4 nanoparticles (density ratio Co:Co3O4 is 1.46:1) [34] and using the fact there are 3.1 × 1018 cobalt atoms m−2 in a typical Co3O4 surface [based on (100) facets] to obtain an estimate of the number of surface atoms. A sensitivity analysis for the assumptions that particles are spherical and (100) surfaces are exposed is provided in the Electronic Supplementary Material (Table S5), and confirms within the other errors of the experiment the differences obtained are relatively small for cubic or different low energy facets [(111) and (100) that likely dominate the surface]. Co3O4 is assumed to be present as the stable highest oxidation state form of the nanoparticles before the application of electrical potential. This approach has also been taken for calculation of values based on available literature data where the geometric nanoparticle surface area where possible, or the BET surface area for mesoporous materials, has been used, as tabulated in the supporting information.

2.3 Transmission Electron Microscopy (TEM)

The size of the as prepared nanoparticles was characterized by TEM by casting one droplet of nanoparticle solution (hexane) onto a holey carbon coated copper grid (Agar Scientific) and allowing to evaporate to dryness. TEM imaging was performed using a JEOL 2100F FEG TEM with a Schottky field emission source. The accelerating voltage was 200 kV. The obtained particle size distribution was obtained from imaging at least 6 different areas of the grid and measuring the diameter of over at least 120 individual nanoparticles. ImageJ software was used for manual size analysis of the images. Measurements were taken of the ~ 20 particles in the top right hand corner of each image to ensure consistency and each particle was measured horizontally on the image to avoid systematically measuring the longest axis. No measurable change in particle size was seen in different regions of the grid.


ICP-OES was performed on a Jobin Yvon Horiba Ultima-2, with a vertically orientated radial torch and a sequential monochromator. A cobalt in nitric acid ICP-OES standard (Sigma-Aldrich), and the Co emission line at 228.616 nm were used. ICP-OES samples were prepared by dissolving 1.0 mL aliquots of the nanoparticle samples in hexane in 3 mL of aqua regia (HNO3:HCl, 1:3 v/v by volume). These samples were then heated to near boiling for ~ 10–20 min to evaporate all the hexane and until it was seen any precipitated metal was seen to be fully dissolved. After cooling, the sample was made up to 25 mL in a volumetric flask using high purity water. The aliquots were calculated such that the concentrations of the 25 mL samples measured should be ~ 80 mg L−1, assuming a 60% yield.

3 Results and Discussion

Representative TEM images of the as synthesized cobalt nanoparticles (Fig. 2) show the formation of a size series (as expected from the literature) of nanoparticles with narrow size distributions as a result of varying the temperature during nanoparticle synthesis. It is notable that, by the time the samples are subjected to electron microscopy, a significant oxide shell forms on the surfaces of the nanoparticles; this can be clearly seen in the case of the largest nanoparticles, as shown in the inset in Fig. 2d. Because of previous findings under similar basic conditions showing there is a negligible difference in activity when starting with Co3O4, CoO and Co metal nanoparticle coated electrodes, and the ease of surface oxidation seen for nanoparticles of this type, it is expected that such an oxide surface layer will not be important in determining the state of the anode under working conditions once voltage is applied [20].

Fig. 2

Typical TEM images of each nanoparticle sample overlaid with the particle size distributions obtained from measuring > 120 nanoparticles (ad show particles synthesised at 183, 178, 172 and 168 °C producing particles with mean diameters of 3.7 ± 0.8, 4.4 ± 0.7, 6.3 ± 1.0 and 9.3 ± 1.2 nm, respectively). The inset in d shows more clearly the oxide layer that forms around the cobalt nanoparticles due to air handling

These four nanoparticle samples (based on the concentration of cobalt determined by ICP OES) were initially used to prepare working electrodes with a fixed cobalt concentration of 20 µg cm−2 by deposition on a glassy carbon electrode. This concentration was chosen to allow us to obtain a baseline activity, where most of the cobalt was accessible for reactants and products to absorb and desorb. This is confirmed by the overpotential required to obtain a current of 10 mA cm−2 decreasing from 485 to 454 mV between cobalt electrode loadings of 20 and 45 µg cm−2 (for the same sample), showing the active surface area to still be increasing substantially, whereas on increasing to higher loading the decrease in overpotential becomes much less (see Electronic Supplementary Material). Figure 3 shows the average overpotential required to obtain specified current densities of 10 and 50 mA cm−2 as a function of mean nanoparticle diameter (the average is based on repeats of the entire process including loading the electrode and catalyst testing). While the error bars are significant a clear trend of overpotential required decreasing with decreasing particle size is seen. This is consistent with the previous observation by Esswein et al. for larger cobalt particles, where it was found this change in overpotential was simply a result of the increased surface area [21]. In their work the linear nature of overpotential versus ln(surface area) plots based on the Tafel equation was used to confirm the decrease in overpotential for smaller particles was purely due to the increased surface area. In the present work the same approach was followed and the Tafel plots for the overpotential required to reach current densities of 10 and 50 mA cm−2 are shown in Fig. 4. The surface areas were estimated as the geometric surface area of the nanoparticles, which has been shown previously to be in reasonable agreement with other methods of surface area estimation [29]. It should be noted that due to the semi-logarithmic plot if a fraction of each nanoparticle is inaccessible because of deposition on the surface or contact with other nanoparticles, so long as that fraction is assumed to be constant for different sizes nanoparticles the Tafel slope will not vary. As can be seen, the Tafel slope obtained (59 ± 8 mV dec−1) is broadly similar to that reported when varying larger sized Co3O4 starting particles (47 ± 7 mV dec−1) [21]. However, consideration of the errors in measurement, even based on repetition of each point, makes asserting no-deviation from a linear relationship dubious. This can be seen more clearly in a simple thought experiment in which the smallest particles are deemed to have half or double the rate per surface site of the largest ones and vary linearly for intermediate sizes (Fig. 5, assumes the above Tafel slope to be otherwise correct—details of calculation are in the Electronic Supplementary Material). Clearly although the Tafel slope obtained is very different, the plots remain very linear in appearance. It is noteworthy that it has previously been suggested that the Tafel relation could be used to calculate a turnover frequency at zero overpotential as a measure of intrinsic activity for electro catalysed processes [35], but the use of the extrapolation of a ln(TOF) versus overpotential graph makes this method similar reliant on precise knowledge of the TOF (which is typically at best an estimate).

Fig. 3

Average overpotential as a function of cobalt nanoparticle size measured at 10 mA cm−2 (a) and 50 mA cm−2 (b) using a constant cobalt loading on the electrode of 20 µg cm−2. The error bars in the y-axis show standard deviation in the mean based on repeat measurements of each point, the error bars in the x-direction show the standard deviation value from the mean of the measured particle size distribution as described above (and not an error in the mean particle size that would be much smaller)

Fig. 4

Tafel plot of overpotential against ln(surface area per gram) based on the nanoparticle’s geometric surface area (assuming the nanoparticles to be roughly spherical). The error bars in the y-axis show standard deviation in the mean based on repeat measurements of each point, the error bars in the x-direction show error in the ln(surface area) based on propagation of the standard deviation of the measured particle size distribution

Fig. 5

Schematic showing the effect of recalculating the Tafel plot for 10 mA cm−2 current density based on the Tafel slope in Fig. 4, but assuming the smallest particles are deemed to have half (a) or double (b) the rate per surface site of the largest ones and vary linearly for intermediate sizes (details of calculation given in the Electronic Supplementary Material)

To overcome this problem, the working electrode was instead loaded with a differing amount of cobalt nanoparticles, such that each electrode contained the same geometric surface area of nanoparticles. The average overpotential required to obtain specified current densities of 10 and 50 mA cm−2 as a function of mean nanoparticle diameter for a constant surface area can be seen in Fig. 6. This provides definitive evidence that even for small (~ 3.5 nm) particles, which are known to exhibit different oxidation behaviour, there is no significant particle size effect.

Fig. 6

Average overpotential as a function of cobalt nanoparticle size measured at 10 mA cm−2 (a) and 50 mA cm−2 (b) using a surface area-normalized electrode loading. The error bars in the y-axis show standard deviation in the mean based on repeat measurements of each point, the error bars in the x-direction show the standard deviation value from the mean of the measured particle size distribution as described above (and not an error in the mean particle size that would be much smaller)

In addition to investigating whether a particle size effect exists for < 10 nm cobalt nanoparticles, a second aim of the present work was to investigate the intrinsic activity of cobalt nanoparticles—this is important because many previous studies have focussed on practical electrode designs (such as deposition within a conducting foam) [20, 21] or innovative porous cobalt materials [24], but it is not clear how much of the cobalt remains accessible for catalysis. In the present case the cobalt nanoparticles have instead been loaded directly on a flat working electrode surface and with a concentration at which most of the surface area of the nanoparticles is accessible (at most a few layers deep allowing diffusion between them). Knowledge of the intrinsic turnover frequency then allows for the efficiency of 3D electrode designs to be improved to eliminate diffusion restrictions and maximise the useful catalyst area. It is well known that comparison of electrocatalytic activities for different preparations and testing conditions is difficult [32], however it has previously been suggested some comparisons can be drawn for the TOF at a fixed overpotential [36]. In many systems this is difficult to do, because of the uncertainty in the number of accessible surface sites, as discussed in a study of electrodeposited Fe–Co films, where an electrochemical method based on the Co2+/Co3+ wave during a cyclic voltogram is used to estimate the number of accessible cobalt sites [37].1 Figure 7 attempts to compare estimates of the apparent TOF per Co atom and per Co surface atom at a fixed overpotential of 500 mV (for convenient comparison) for the present study and several similar literature studies using nanostructured cobalt. Unsurprisingly, it can be seen that normalising by surface area (Fig. 7b) substantially improves the commonality between the reported results. It can also be seen that for all the nanoparticulate structures the TOF is of a ball park figure a little under 1.5 O2 molecule per surface Co site per second. Notably the largest nanoparticle structures reported by Esswein et al. have a slightly larger TOF [21], but this could be the result of either a smaller fraction of the surface being in contact with the support or as result of surface roughening under reaction conditions (the calculation used assumed they are spherical and all of the mean size reported). It can also be seen the nanocast mesoporous Co3O4 structures have a slightly lower values, suggesting some inaccessibility of some surface sites. Nevertheless this analysis allows us to confirm a “typical” intrinsic TOF for cobalt catalysed OER under these typical conditions.

Fig. 7

Apparent TOF at η = 500 mV per Co atom (mass activity) (a), and per surface Co atom (b), for Co3O4 nanoparticles in Ni foam (surfactant method) [21], CoO nanoparticles in Ni foam (surfactant free) [20], nanocast mesoporous Co3O4 [24] and the cobalt nanoparticles in the present work. More details of the calculation are given in the Electronic Supplementary Material. All catalysts shown were tested in 1 mol dm−3 KOH electrolyte. The geometric area (assuming the particles are spherical) of all nanoparticle materials in their oxide form is used to calculate surface area, assuming (100) surface facets (containing 3.1 × 1018 Co atoms m−2). For the mesoporous Co3O4 the reported BET surface area is used as such a calculation is not possible

4 Conclusions

In summary, we have shown that small cobalt nanoparticles (4–10 nm) can be used in the OER and under typical alkaline conditions they do not exhibit any particle size effect, in spite of the known differences in oxidation behaviour for lower oxidation state redox couples across this size range. Two methods were used to evaluate this, firstly the standard electrochemical method based on the linearity of Tafel plots and secondly a direct method employing a surface-area normalised cobalt loading on the working electrode. Finally, the use in this study of small quantities of cobalt nanoparticles on a flat working electrode to maximise accessibility, and comparison to several literature studies using cobalt nanostructures, has allowed identification of an estimated intrinsic turnover rate for cobalt surface sites in Co3O4 catalysed OER under typical alkaline reaction conditions (ambient temperature, pH 14) of order 1 O2 molecule per surface Co site per second (η = 500 mV).


  1. 1.

    It should be noted that the TOFs calculated in this study were at an overpotential of 350 mV at which Co is not active, so no direct comparison can be made.



The authors gratefully acknowledge PW Dyer for access to a glovebox and the DU GJ Russell Microscopy Facility for access to TEM, SJ was funded by the UK Catalysis Hub, which is kindly thanked for resources and support provided via membership of the UK Catalysis Hub Consortium and funded by the UK Engineering and Physical Sciences Research Council (Grants EP/K014706/2, EP/K014668/1, EP/K014854/1, EP/K014714/1 and EP/M013219/1).

Supplementary material

11244_2018_923_MOESM1_ESM.pdf (295 kb)
Supplementary material 1 (PDF 294 KB)


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Authors and Affiliations

  1. 1.Department of ChemistryUniversity of DurhamDurhamUK

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