Article | Open | Published:

Dual properties of a hydrogen oxidation Ni-catalyst entrapped within a polymer promote self-defense against oxygen

Nature Communicationsvolume 9, Article number: 864 (2018) | Download Citation


The Ni(P2N2)2 catalysts are among the most efficient non-noble-metal based molecular catalysts for H2 cycling. However, these catalysts are O2 sensitive and lack long term stability under operating conditions. Here, we show that in a redox silent polymer matrix the catalyst is dispersed into two functionally different reaction layers. Close to the electrode surface is the “active” layer where the catalyst oxidizes H2 and exchanges electrons with the electrode generating a current. At the outer film boundary, insulation of the catalyst from the electrode forms a “protection” layer in which H2 is used by the catalyst to convert O2 to H2O, thereby providing the “active” layer with a barrier against O2. This simple but efficient polymer-based electrode design solves one of the biggest limitations of these otherwise very efficient catalysts enhancing its stability for catalytic H2 oxidation as well as O2 tolerance.


A major challenge of humankind is a future sustainable energy economy. Hydrogen has been proposed as an ideal target to store energy from renewable sources, e.g., solar-driven water splitting1,2,3,4. A hydrogen-powered fuel cell is then able to recover a major part of the energy in high yields on demand. An unsolved challenge in this endeavor is to design active, efficient and stable catalysts based on earth-abundant metals4.

Nature uses the highly active and efficient hydrogenase enzymes for hydrogen cycling in living systems. The enzymes are capable of achieving low overpotentials and high turnover frequencies in both hydrogen oxidation and proton reduction, bearing only the abundant metals Fe and/or Ni in their active sites5. Chemists have been inspired by these enzymes to design inexpensive molecular complexes capable of efficiently producing or oxidizing H2. Particularly noteworthy examples are the DuBois catalysts6,7, which are Ni-(bis)diphosphine based complexes equipped with a pendant amine that acts as a Lewis base, accepting the proton during H2 splitting, in a manner analogous to that proposed to occur at the active site of [FeFe] hydrogenases8,9.

Extension of the proton channel with a carboxylic acid moiety between the metal center and the solvent by attachment of an amino acid to the pendant amine, allows the DuBois catalyst to operate at very low overpotentials at low pH and at room temperature in aqueous systems10,11,12, or even reversibly13,14. Moreover, these catalysts show tolerance towards CO, a common contaminant of H2 feedstocks and a strong inhibitor of hydrogenases and of platinum used for catalysis5,15,16.

On the other hand, the DuBois catalyst undergoes rapid degradation under conditions relevant for technological applications, i.e., when immobilized on an electrode15,17,18 or on photoactive materials19. We demonstrated in a previous study that the electrocatalytic H2 oxidation activity of the DuBois catalyst CyGly (for Structure see Fig. 1) was lost irreversibly after 10 min when 2% O2 was added to the H2 gas feed15. Similarly, other studies with DuBois complexes in solution revealed that the H2 production activity was completely suppressed when O2 was present in the electrochemical cell16,20. Crystallographic and nuclear magnetic resonance (NMR) spectroscopic studies showed that the Ni-(bis)diphosphine complexes in low oxidation states react with O2 to oxidize the phosphine ligands, inactivating the complexes irreversibly21. Hence, under electrocatalytic conditions implying fast collection of electrons by the electrode, which is desired for current generation in fuel cells, exacerbates the O2 sensitivity of the Ni-catalyst. In contrast, in solution and in the presence of H2, the Ni-complex accumulates in a highly reduced doubly protonated Ni0 state, which can catalytically reduce O2 to water, slowing the formation of the oxidized inactive complex (Fig. 1)21.

Fig. 1
Fig. 1

Reactions of the CyGly complex with H2/O2 in solution. The Ni2+ complex, [NiII(PCy2NGly2)2]2+, undergoes slow and irreversible inactivation by O2 while the H2 reduced Ni0 complex, [Ni0(PCy2NGly2)2], is able to catalytically reduce O2 to H2O

In the present study, we take advantage of the dual catalytic nature of this complex: the electrocatalytic oxidation of H2 and the catalytic reduction of O2. We use here the properties of a redox-silent hydrophobic polymer to support the catalyst and obtain a polymer/catalyst film which creates two discrete reaction layers serving separate roles: a phase close to the electrode surface where electrons can directly tunnel between catalyst and electrode. This layer is responsible for electrocatalytic H2 oxidation. Near the interface between the polymer and the electrolyte, a second region which is electrically disconnected from the electrode surface, prevents anodic reoxidation of the catalyst, allowing the doubly protonated Ni0 complex to reduce incoming O2 to water. This results in a simple and efficient self-protecting, catalytically active matrix that serves to extend the limited lifetime of the Ni-catalyst when immobilized on an electrode surface.


Reactivity of the CyGly complex on electrode surfaces with O2

The catalyst was dispersed into a poly(glycidyl methacrylate-co-butyl acrylate-co-poly(ethylene glycol) methacrylate) (denoted as P(GMA-BA-PEGMA) in the following) polymer (See Methods section)). This polymer was chosen because of its rather hydrophobic nature that allows for the formation of stable films in aqueous electrolytes. Moreover, the polymer backbone consists of chemically inert and non-coordinating monomers. Thus, unintended interactions between the Ni-center and the polymer backbone that may affect the catalytic properties of the catalyst are prevented. Film formation was carried out by drop-casting of a homogenous solution of the polymer and the complex in acetonitrile on a glassy carbon electrode followed by drying under anaerobic conditions. Consecutive cyclic voltammograms of the modified electrodes at pH 3.0 revealed the appearance of a reversible signal with a mid-point potential of −12 mV vs. SHE (Fig. 2). This wave was previously assigned to two overlapping one electron processes, corresponding to the reduction of Ni2+ to Ni10,15. The intensity of the signal increases during the first 30 min as a result of the initial solvation of the polymer and/or penetration of counter ions into the film (see Supplementary Fig. 1). The peak intensity is proportional to the square root of the scan rate, indicating the diffusional nature of the electrochemical process. This is indicative of some mobility of the Ni-complex, and/or counter ion transport inside the polymer film (See Supplementary Fig. 2). When H2 is flushed through the electrochemical cell, a catalytic current appears starting at the redox potential of the complex (Fig. 2b). The catalytic current increases with the applied potential, indicating slow counter ion movement within the film or a distribution of the tunneling distance between the CyGly molecules and the electrode as a result of the non-conductive nature of the polymer. The latter is similar to what has been reported for complexes in solution with bulky dipeptides in the outer coordination sphere22.

Fig. 2
Fig. 2

Catalytic properties and tolerance of CyGly modified electrodes towards oxygen. a Electrode preparation schemes: (i) A monolayer of CyGly complex; (ii) a monolayer of CyGly complex coated with the pristine polymer and the PCy2NGly2 ligand, and (iii) CyGly/polymer film on glassy carbon electrodes. b Cyclic voltammograms of the polymer/catalyst film (iii) under N2 (black trace) and under H2 (red trace). Conditions: 20 mV s−1, pH = 3, 0.1 M MES/0.1 M HEPES + HClO4, 25 °C, 2000 rpm. c Chronoamperometry experiments under 90% H2/10% N2 with the addition of 5% O2 (90% H2, 5% N2) over 600 s (shaded area) for all three electrode preparations. Conditions: + 541 mV vs. SHE, 25 °C, 2000 rpm, pH = 3, 0.1 M MES/0.1 M HEPES + HClO4. The initial current drop corresponds to slow equilibration processes inside the polymer (establishment of H2 and Ni2+ gradients)

Addition of O2 to the gas mixture during H2 oxidation using a film of CyGly complex dispersed in the polymer, does not affect the catalytic current (Fig. 2c, black trace). This is in stark contrast to measurements with a monolayer of the immobilized catalyst, where the CyGly complex loses 75% of its catalytic H2 oxidation activity irreversibly over 10 min as 5% O2 is added to the gas feed (Fig. 2c, blue trace). On the other hand, when the catalyst in a DET configuration is exposed to O2 in the absence of H2, most of the catalytic activity is recovered when the gas is switched back to H2 (See Supplementary Fig. 3b, blue trace). This suggests a higher O2 sensitivity of the complex during electrocatalytic H2 oxidation. When the potential on the electrode was kept low enough to maintain the Ni-center in the reduced Ni0 state during O2 exposure, the catalytic current was completely recovered (see Supplementary Fig. 3b, red trace). In line with this result, electrodes prepared outside the glovebox did not show any catalytic activity (data not shown) suggesting that long exposure of the Ni-complex in the Ni2+ oxidation state to O2 without any applied potential on the electrode or in the absence of H2 damages the catalytic properties of the complex.

To evaluate if the observed protection is only based on a simple physical blocking of O2 by the polymer, cyclic voltammetry experiments with polymer-coated glassy carbon electrodes in the presence of O2 were conducted. Indeed, direct O2 reduction at glassy carbon electrodes is significantly hampered by the presence of the polymer film on the electrode surface (See Supplementary Fig. 4). However, when a monolayer of the catalyst on the electrode surface was further coated with a mixture of polymer and ligand (of similar thickness, with two equivalents of CyGly ligand but without Ni), the catalyst exhibits similar sensitivity to oxygen as the monolayer without a polymer top layer (Fig. 2c, red trace). This excludes on one hand the possibility that a physical barrier to oxygen is the sole explanation for the decreased oxygen sensitivity in catalyst-polymer films. On the other hand, since the CyGly ligand is also O2 sensitive, this experiment further demonstrates that the simple stoichiometric reaction of O2 with the catalyst during its oxidative degradation does not significantly participate in the protection mechanism. An active Ni-complex dispersed in the polymer film is required for effective protection.

The CyGly complex as an O2 reducing catalyst

The reactivity of the CyGly complex with O2 in solution was analyzed by means of 2H NMR spectroscopy. D2 was used as a reductant and the formation of D2O upon O2 addition to the gas feed was quantified. The TOF for O2 reduction to D2O was measured to be (20 ± 5) h−1 (see Supplementary Fig. 5). Formation of D2O under such conditions supports the mechanism proposed in Fig. 1 and is consistent with results described previously by Yang et al21. for a series of similar complexes containing a pendant base on the phosphine ligand (see Supplementary Note 1).

On the other hand, if the NMR tube contains mixtures of H2 and O2 in order to reproduce the conditions in the electrochemical cell, the 31P NMR spectrum of the catalyst in solution shows almost complete loss of the CyGly resonances after 3 h along with new resonances of its degradation products appearing (See Supplementary Figs 11 and 12).

To reduce O2 to water, two molecules of the Ni0 complex are needed to provide the required 4 electrons and protons (Fig. 1). This is possible with the freely diffusing catalyst in solution, but using a monolayer of catalyst immobilized on the electrode, the catalyst is cycling through different redox states and geometries under turnover conditions23. As a result, the immobilized doubly protonated Ni0 complex does not accumulate in the required concentrations to effectively reduce O2 to water, because of fast electron transfer to the electrode. Consequently, catalyst degradation and the observed drop in catalytic current results (Fig. 2c, red and blue traces).

A polymer matrix to separate reaction layers

The stability of the H2 oxidation currents under O2 observed in Fig. 2c for the CyGly/polymer films can be explained if we consider a layered structure for the CyGly complex/polymer film. The insulating polymer acts as a supporting matrix to immobilize the complex on the electrode surface, but also prevents electrical contact between the complexes in the remote regions of the film and the electrode. The formation of a sufficiently thick polymer film generates two distinct regions; with electrocatalytic H2 oxidation in the inner layer near the electrode surface and O2 reduction in the outer layer as shown in Fig. 3.

Fig. 3
Fig. 3

Proposed reactions inside the polymer/catalyst film. Schematic representation of the polymer film separating the immobilized CyGly complex into two functional layers where different reactions occur; colors are used to identify the different polymer layers and the boundary between polymer and electrolyte. In the electrocatalytic layer (yellow), H2 is oxidized to protons and electrons via the Ni-complex. Within the protection layer (green) the doubly reduced Ni0 complex catalyzes the reduction of incoming O2 to H2O by using the electrons supplied from H2

Under H2 in the absence of O2, the complex in the protection layer (Fig. 3, green region) is reduced to the protonated Ni0 state, but since it is electrically isolated from the electrode, electrons will not be shuttled to the electrode. However, when O2 reaches the film/electrolyte interface, it will encounter the reduced Ni-complexes, which will then reduce incoming O2 to water, thus protecting the electrocatalytic layer (Fig. 3, yellow region) from O2 damage.

Validation of the protection mechanism

The mechanism of O2 reduction to water requires two catalyst molecules per O2, which has implications for the film preparation. If films with low catalyst loading are used, oxidative damage of the catalyst is observed (See Supplementary Fig. 6). This is thought to be due to slow diffusion of the catalyst molecules within the film, thus allowing O2 to pass the protection layer and/or the accumulation of partially reduced oxygen species.

Conductive multi-walled carbon nanotubes (MWCNT) were used to extend the electrocatalytic region in the polymer film, connecting the electrode to catalyst molecules in the film further away from the electrode, i.e., in the previously defined protection layer. The resulting electrode showed higher H2 oxidation currents, but as expected, reduced the protection layer by increasing the number of catalyst molecules capable of H2 electrocatalysis rather than O2 reduction. Consequently, the result is a catalytic current decay when O2 is added to the gas feed (see Supplementary Fig. 7). Moreover, the thickness of the film is crucial for effective protection. While thinner films produced higher catalytic currents for H2 oxidation (substrate diffusion is not limiting), these films do not show protection against O2 and the H2 oxidation current decayed as soon as O2 was added to the gas feed (Fig. 4a). Similar O2 sensitivity as a function of film thickness was observed for an air sensitive enzyme, i.e., a NiFeSe hydrogenase, that was immobilized in an O2 quenching redox polymer24.

Fig. 4
Fig. 4

Catalytic H2 oxidation by CyGly/polymer films in the presence of O2. a Chronoamperometric experiments of glassy carbon electrodes (GCEs) modified with CyGly/polymer films of different thicknesses obtained by drop-casting 20 µL (black line), 10 µL (blue line) and 2.5 µL (red line) of the CyGly/polymer solution in acetonitrile onto the GCEs. Measurements conducted under 90% H2/10% N2 with addition of 5% O2 (90% H2/5% N2) over 10 min (shaded area). Conditions: + 541 mV vs. SHE, pH = 3, 0.1 MES/0.1 M HEPES + HClO4, 25 °C, 500 rpm. b Chronoamperometric experiment with a CyGly/polymer film under 5% O2/90% H2/5% N2 gas mixture over 24 h showing the high stability of the H2 oxidation process in this film even under aerobic conditions. Conditions: + 541 mV vs. SHE, pH = 3, 0.1 M MES/0.1 M HEPES + HClO4, 25 °C, 2000 rpm

To further investigate the catalytic nature of the O2 reduction reaction by the catalyst, we tested the stability of the catalytic current when the film was exposed to O2 in the absence of H2. This gas is required to regenerate the reduced Ni-complex in the protection layer once it is oxidized by an O2 molecule. Supplementary Fig. 8 shows that when the catalyst-polymer film is exposed to 5% O2 in the absence of H2 for 5 h, 35% of the catalytic activity is lost, while when H2 is present, 100% of the initial current is maintained for the same O2 exposure. Interestingly, while measuring the control experiment under N2 (See Supplementary Fig. 8, blue trace), without O2 to corroborate that N2 is not damaging the complex, we noticed that the oxidation current did not reach 0 A. The most likely explanation for this observation is that as we start the experiment under H2 to record the initial activity of the film, the catalyst in the polymer layer is completely reduced by H2. Since diffusion inside the polymer is extremely slow, its oxidation by the electrode surface is also very slow. Integration of the charge passed gives a value of 31 μC, which would correspond to 0.2 μmol of Ni-complex, 20% of the catalyst present in the film. This explains why only 35% of the catalytic activity is lost under a N2/O2 mixture. Under such conditions, the Ni-complex in the polymer film is still reduced, and therefore protecting the complex in the inner layer, but in the absence of H2 to regenerate the reduced complex, the inactive front advances more rapidly.

The polymer enhances catalyst stability

The catalytic current was remarkably stable over time. After 18 days of continuous measurement in a chronoamperometry experiment under turnover conditions in the absence of O2, the electrode still maintained 75% of the initial current (See Supplementary Fig. 9). This stability contrasts with what was reported previously for a monolayer of the same catalyst covalently attached to the electrode, where the activity was completely lost after 3 days15. The increased stability could be a result of the hydrophobic nature of the polymer film, which may stabilize the integrity of the complex during turnover. Moreover, within the polymer film, the Ni-catalyst can freely diffuse without any structural and/or conformational constraints, as it is the case for the surface confined Ni-catalyst (See Supplementary Note 2).

The H2 oxidation current remains completely unaffected by the presence of O2 in the gas feed for the first 7 hours (Fig. 4b). After this time, the current starts to decay slowly, maintaining 75% of the initial current after 24 h of continuous O2 exposure. As stated before, we cannot eliminate the undesired slow oxidation of the phosphines21 forming an inactive product and therefore eliminating the protective capacity of the protection layer over time. After 7 h the catalyst in the protection layer is most likely starting to get oxidized, which results in an advancement of the inactive front reaching the catalyst molecules in the electrocatalytic layer. At this point, catalyst molecules participating in the electrocatalytic H2 oxidation begin to decompose due to incoming O2, resulting in the slow decay of the catalytic current.


DuBois catalysts with modifications in the outer coordination sphere have already been proposed as good candidates for use in fuel cells10,14,23,25,26. They operate at very low overpotential and unlike noble metals or hydrogenases they are insensitive to CO,16,17 which allows for the use of inexpensive low purity H2 as fuel. The remaining limitations to be solved are the lack of stability and the oxygen sensitivity16. We demonstrate that the use of a redox silent polymer acting as a support for the fabrication of H2 oxidation may overcome these limitations. The polymer matrix provided several important advantages to the Ni-complex: the stability of the catalyst was extended dramatically, both in the absence and in the presence of O2. While previous strategies for protection of enzymes against oxidative damage were based on redox polymers with intrinsic O2 reducing capabilities24,27,28,29, here the polymer is redox silent and does not contribute directly to protection via a redox process. Instead, the polymer serves as a supporting matrix that imposes local redox states and confers local reactivity to the embedded catalysts. For sufficiently thick films, the polymer electrically isolates the catalyst in the outer layer (protection layer) from the electrode. As a result, when exposed to H2, this portion of the catalyst remains in the Ni0 state and is capable of reducing incoming O2. This allows the catalyst to effectively eliminate O2 in the outer layers of the polymer, preventing it from reaching the electrocatalytic H2 oxidation layer. Moreover, it is possible to achieve high catalyst concentrations inside the polymer film to favor fast interaction of O2 with two reduced Ni-complexes to ensure the complete reduction of O2 to water. It is the combination of these effects that makes the O2 protection mechanism possible.

This possibility to activate the catalyst for self-protection without the need for auxiliary functionalities greatly simplifies the protection concept. Importantly, the ability to maintain the metal complex in a highly reduced protonated state, which is essential for protection, scales with the activity for H2 oxidation, implying that future highly active catalysts, even if potentially highly oxygen sensitive, may still find technological application by exploiting this protection concept.


Electrochemical experiments

All electrochemical experiments, electrode modifications and handling of the CyGly were carried out inside a glovebox (MBRAUN) filled with nitrogen. A set of mass flow-controllers (Brooks Instruments) were used to control the gas composition flushed through the electrochemical cell. The total flow in all experiments was 1000 mL min−1, unless stated otherwise. An oxygen filter (Air Liquide) before the electrochemical cell avoids any undesired O2 contamination. The potential was controlled by a VersaSTAT 4-400 potentiostat. A standard three electrode water jacketed electrochemical cell was used for the measurements with a Pt wire as counter electrode and a saturated calomel electrode located in a side arm as reference electrode. All potentials were converted to the standard hydrogen electrode (SHE) by adding + 241 mV.

NMR experiments

A DPX200 NMR spectrometer from Bruker with a proton resonance frequency of 200.13 MHz was used for polymer characterization and a Bruker Avance500 (202.4 MHz 31P resonance frequency) for 31P NMR measurements. Solution state 2H NMR spectra were recorded on an Agilent VNMR spectrometer (500 MHz 1H resonance frequency). Direct detect dual-band or OneNMR probes were used. Typical 2H 90o pulses were 10 μs. The polymer was characterized in deuterated acetone-d6. The residual solvent peak was used as the internal standard.

Ni complex and polymer synthesis

The synthesis of the CyGly complex was described earlier10. All chemicals and solvents for polymer synthesis were purchased from Sigma-Aldrich, Alfa Aesar, Acros-Organics or J.T. Baker. The free radical initiator 2,2′-azobis(2-methylpropionitrile) (AIBN) was recrystallized from hot toluene prior to use. The co-monomers glycidyl methacrylate (GMA), butyl acrylate (BA) and poly(ethylene glycol methacrylate) (dissolved in isopropyl alcohol, 0.05 g mL−1) were passed through a short column filled with inhibitor remover prior to polymerization. The initiator and the co-monomers were stored at −20 °C or +4 °C.

Size exclusion chromatography (SEC)

SEC measurements were conducted against polystyrene standards in THF at 30 °C. Data were analyzed with the PSS WinGPC Unity software. Sample concentration was 15 mg mL−1.

The redox silent polymer matrix poly(glycidyl methacrylate-co-butyl acrylate-co-poly(ethylene glycol methacrylate)) (P(GMA-BA-PEGMA)) was synthesized following protocols described previously (see Supplementary Fig. 13)30. The co-monomers glycidyl methacrylate (GMA, 0.68 mL, 0.710 g, 5 mmol, 49.5 mol%), butyl acrylate (BA, 0.61 mL, 0.545 g, 4.3 mmol) and poly(ethylene glycol methacrylate) (PEGMA, Mn = 500 g mol−1, 8 mL of a 0.05 g mL−1 isopropyl alcohol solution, 0.4 g, 0.8 mmol, 8 mol%) were mixed in a Schlenk tube under argon atmosphere. Then, the free radical initiator AIBN (15 mg, 91 µmol) was added and the mixture was deaerated by bubbling argon through the solution. The reaction mixture was heated to 80 °C and stirred for ≈35 min at this temperature. The turbid solution was quenched with 40 mL of water. The colorless precipitate was separated by means of a centrifuge (4000 rpm, 20 min). The supernatant was decanted off and the residue was successively washed with water (40 mL), MeOH/water (40 mL, 1:1 vol%) and finally with diethyl ether (120 min) with centrifugation and separation after each step. The highly viscous colorless product was dried under reduced pressure. The dry foamy solid was dissolved in acetonitrile (14.5 mL) to obtain a polymer solution with a concentration of 0.1 g mL−1 (yield: 1.45 g, 88%). 1H-NMR (200.13 MHz, acetone-d6) δ/ppm: ≈1 (broad, -CH3 and -CH2- of backbone); 1.41 (m, -CH2-, BA); 1.62 (m, -CH2-, BA); 2.69, 2.84 and 3.26 (all s, epoxide, GMA), 3.60 (s, -CH2-, PEGMA), 3.82 and 4.37 (all broad, -CH2-O moiety, GMA), 4.02 (broad, -CH2-O moiety, BA) composition determined via the integral ratio extracted from the 1H-NMR spectrum: GMA = 60 mol%, BA = 36 mol%, PEGMA = 4 mol% (Supplementary Fig. 14); SEC (vs. poly(styrene) standard, THF): Mw = 39 kDa, PDI = 2.8.

Film formation

Glassy carbon electrodes (GC, Pine Research Instrumentation, 5 mm diameter) were drop-cast with a mixture of 1 mg of CyGly and polymer solution (20 μL, 20 mg ml−1 in acetonitrile) and left to dry for 1 h in the glove box. Immobilization of the catalyst on a monolayer was performed as described elsewhere15. The pH 3 electrolyte used in all experiments was a 0.1 M MES/0.1 M HEPES mixture where the pH was adjusted with the required amount of HClO4.

Data availability

All data are available from the authors upon reasonable request.

Additional information

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


  1. 1.

    Lewis, N. S. & Nocera, D. G. Powering the planet: chemical challenges in solar energy utilization. Proc. Natl Acad. Sci. USA 103, 15729–15735 (2006).

  2. 2.

    Concepcion, J. J., House, R. L., Papanikolas, J. M. & Meyer, T. J. Chemical approaches to artificial photosynthesis. Proc. Natl Acad. Sci. USA 109, 15560–15564 (2012).

  3. 3.

    Faunce, T. A. et al. Energy and environment policy case for a global project on artificial photosynthesis. Energy Environ. Sci. 6, 695–698 (2013).

  4. 4.

    McKone, J. R., Marinescu, S. C., Brunschwig, B. S., Winkler, J. R. & Gray, H. B. Earth-abundant hydrogen evolution electrocatalysts. Chem. Sci. 5, 865–878 (2014).

  5. 5.

    Lubitz, W., Ogata, H., Ruediger, O. & Reijerse, E. Hydrogenases. Chem. Rev. 114, 4081–4148 (2014).

  6. 6.

    Helm, M. L., Stewart, M. P., Bullock, R. M., Rakowski DuBois, M. & DuBois, D. L. A synthetic nickel electrocatalyst with a turnover frequency above 100,000 s−1 for H2 production. Science 333, 863–866 (2011).

  7. 7.

    DuBois, D. L. Development of molecular electrocatalysts for energy storage. Inorg. Chem. 53, 3935–3960 (2014).

  8. 8.

    Wilson, A. D. et al. Hydrogen oxidation and production using nickel-based molecular catalysts with positioned proton relays. J. Am. Chem. Soc. 128, 358–366 (2006).

  9. 9.

    Berggren, G. et al. Biomimetic assembly and activation of (FeFe)-hydrogenases. Nature 499, 66–69 (2013).

  10. 10.

    Dutta, A. et al. Minimal proton channel enables H2 oxidation and production with a water-soluble nickel-based catalyst. J. Am. Chem. Soc. 135, 18490–18496 (2013).

  11. 11.

    Boralugodage, N. P., Arachchige, R. J., Dutta, A., Buchko, G. W. & Shaw, W. J. Evaluating the role of acidic, basic, and polar amino acids and dipeptides on a molecular electrocatalyst for H2 oxidation. Catal. Sci. Technol. 7, 1108–1121 (2017).

  12. 12.

    Dutta, A., Roberts, J. A. S. & Shaw, W. J. Arginine-containing ligands enhance H2 oxidation catalyst performance. Angew. Chem. Int. Ed. 53, 6487–6491 (2014).

  13. 13.

    Priyadarshani, N. et al. Achieving reversible H2/H+ interconversion at room temperature with enzyme-inspired molecular complexes: a mechanistic study. ACS Catal. 6, 6037–6049 (2016).

  14. 14.

    Gentil, S. et al. Carbon-nanotube-supported bio-inspired nickel catalyst and its integration in hybrid hydrogen/air fuel cells. Angew. Chem. Int. Ed. 56, 1845–1849 (2017).

  15. 15.

    Rodriguez-Macia, P., Dutta, A., Lubitz, W., Shaw, W. J. & Rüdiger, O. Direct comparison of the performance of a bio-inspired synthetic nickel catalyst and a [NiFe]-hydrogenase, both covalently attached to electrodes. Angew. Chem. Int. Ed. Engl. 54, 12303–12307 (2015).

  16. 16.

    Wakerley, D. W., Gross, M. A. & Reisner, E. Proton reduction by molecular catalysts in water under demanding atmospheres. Chem. Commun. 50, 15995–15998 (2014).

  17. 17.

    Rodriguez-Macia, P. et al. Covalent attachment of the water-insoluble [Ni(PCy 2N Phe 2)2] electrocatalyst to electrodes showing reversible catalysis in aqueous solution. Electroanalysis 28, 2452–2458 (2016).

  18. 18.

    Das, A. K., Engelhard, M. H., Bullock, R. M. & Roberts, J. A. S. A hydrogen-evolving Ni(P2N2)(2) electrocatalyst covalently attached to a glassy carbon electrode: preparation, characterization, and catalysis. comparisons with the homogeneous analogue. Inorg. Chem. 53, 6875–6885 (2014).

  19. 19.

    Martindale, B. C. M., Joliat, E., Bachmann, C., Alberto, R. & Reisner, E. Clean donor oxidation enhances the H2 evolution activity of a carbon quantum dot–molecular catalyst photosystem. Angew. Chem. Int. Ed. 55, 9402–9406 (2016).

  20. 20.

    Wakerley, D. W. & Reisner, E. Oxygen-tolerant proton reduction catalysis: much O2 about nothing? Energy Environ. Sci. 8, 2283–2295 (2015).

  21. 21.

    Yang, J. Y. et al. Reduction of oxygen catalyzed by nickel diphosphine complexes with positioned pendant amines. Dalton Trans. 39, 3001–3010 (2010).

  22. 22.

    Reback, M. L. et al. The role of a dipeptide outer-coordination sphere on H2-production catalysts: influence on catalytic rates and electron transfer. Chem. Eur. J. 19, 1928–1941 (2013).

  23. 23.

    Dutta, A., DuBois, D. L., Roberts, J. A. & Shaw, W. J. Amino acid modified Ni catalyst exhibits reversible H2 oxidation/production over a broad pH range at elevated temperatures. Proc. Natl Acad. Sci. USA 111, 16286–16291 (2014).

  24. 24.

    Ruff, A. et al. Protection and reactivation of the [NiFeSe] Hydrogenase from Desulfovibrio vulgaris Hildenborough under oxidative conditions. ACS Energy Lett. 2, 964–968 (2017).

  25. 25.

    Lense, S., Dutta, A., Roberts, J. A. S. & Shaw, W. J. A proton channel allows a hydrogen oxidation catalyst to operate at a moderate overpotential with water acting as a base. Chem. Commun. 50, 792–795 (2014).

  26. 26.

    Ginovska-Pangovska, B., Dutta, A., Reback, M. L., Linehan, J. C. & Shaw, W. J. Beyond the active site: the impact of the outer coordination sphere on electrocatalysts for hydrogen production and oxidation. Acc. Chem. Res. 47, 2621–2630 (2014).

  27. 27.

    Fourmond, V. et al. Mechanism of protection of catalysts supported in redox hydrogel films. J. Am. Chem. Soc. 137, 5494–5505 (2015).

  28. 28.

    Oughli, A. A. et al. A redox hydrogel protects the O2-Sensitive FeFe -hydrogenase from Chlamydomonas reinhardtii from oxidative damage. Angew. Chem. Int. Ed. 54, 12329–12333 (2015).

  29. 29.

    Plumeré, N. et al. A redox hydrogel protects hydrogenase from high-potential deactivation and oxygen damage. Nat. Chem. 6, 822–827 (2014).

  30. 30.

    Pinyou, P. et al. Wiring of the aldehyde oxidoreductase PaoABC to electrode surfaces via entrapment in low potential phenothiazine-modified redox polymers. Bioelectrochemistry 109, 24–30 (2016).

Download references


We like to thank Birgit Nöring and Karolina Lewandowska for technical assistance in electrocatalytic measurements and Prof. S. Ludwigs and Dr. K. Dirnberger (both University of Stuttgart, IPOC) for size exclusion chromatography experiments. This work was funded by the Max Planck Society, the US Department of Energy (DOE, Office of Science Early Career Research Program), the Cluster of Excellence RESOLV (EXC1069) from the Deutsche Forschungsgemeinschaft (DFG) and the Deutsch-Israelische Projektkooperation (DIP) in the framework of the project “Nanoengineered optoelectronics with biomaterials and bioinspired assemblies” funded by the Deutsche Forschungsgemeinschaft (245916028). N. Plumeré acknowledges funding by the European Research Council (ERC Starting Grant 715900). Pacific Northwest National Laboratory is operated by Battelle for the US DOE.

Author information


  1. Max-Planck-Institut for Chemical Energy Conversion, Stiftstrasse 34–36, 45470, Mülheim an der Ruhr, Germany

    • Alaa A. Oughli
    • , Patricia Rodríguez-Maciá
    • , Wolfgang Lubitz
    •  & Olaf Rüdiger
  2. Department Analytical Chemistry, Center for Electrochemical Sciences (CES), Ruhr-Universität Bochum, Universitätsstrasse 150, 44780, Bochum, Germany

    • Adrian Ruff
    •  & Wolfgang Schuhmann
  3. Pacific Northwest National Laboratory, 902 Battelle Blvd, Richland, WA, 99352, USA

    • Nilusha Priyadarshani Boralugodage
    •  & Wendy J. Shaw
  4. Center for Electrochemical Sciences—Molecular Nanostructures, Ruhr-Universität Bochum, Universitätsstrasse 150, 44780, Bochum, Germany

    • Nicolas Plumeré


  1. Search for Alaa A. Oughli in:

  2. Search for Adrian Ruff in:

  3. Search for Nilusha Priyadarshani Boralugodage in:

  4. Search for Patricia Rodríguez-Maciá in:

  5. Search for Nicolas Plumeré in:

  6. Search for Wolfgang Lubitz in:

  7. Search for Wendy J. Shaw in:

  8. Search for Wolfgang Schuhmann in:

  9. Search for Olaf Rüdiger in:


A.A.O. performed all electrocatalytic experiments with the polymer and 31P NMR spectroscopy, P.R.-M. the electrocatalytic measurements with the catalyst-monolayer. A.R. designed, synthesized and characterized the polymer. N.P.B. synthesized the CyGly catalyst and performed 2H NMR spectroscopy to determine the O2 reduction TOF. All authors contributed to the manuscript writing, experiment design and discussion of the results.

Competing interests

The authors declare no competing financial interests.

Corresponding author

Correspondence to Olaf Rüdiger.

Electronic supplementary material

About this article

Publication history





Further reading


By submitting a comment you agree to abide by our Terms and Community Guidelines. If you find something abusive or that does not comply with our terms or guidelines please flag it as inappropriate.