Photoinduced Oxygen Evolution Catalysis Promoted by Polyoxometalate Salts of Cationic Photosensitizers.

The insoluble salt Cs15K[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3] (CsCo9) is tested as heterogeneous oxygen evolution catalyst in light-induced experiments, when combined with the homogeneous photosensitizer [Ru(bpy)3]2+ and the oxidant Na2S2O8 in neutral pH. Oxygen evolution occurs in parallel to a solid transformation. Post-catalytic essays indicate that the CsCo9 salt is transformed into the corresponding [Ru(bpy)3]2+ salt, upon cesium loss. Remarkably, analogous photoactivated oxygen evolution experiments starting with the [Ru(bpy)3](5+x)K(6-2x)[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·(39+x)H2O (RuCo9) salt demonstrate much higher efficiency and kinetics. The origin of this improved performance is at the cation-anion, photosensitizer-catalyst pairing in the solid state. This is beneficial for the electron transfer event, and for the long-term stability of the photosensitizer. The latter was confirmed as the limiting process during these oxygen evolution reactions, with the polyoxometalate catalyst exhibiting robust performance in multiple cycles, upon addition of photosensitizer, and/or oxidant to the reaction mixture.

Introduction

Sunlight is the preferred carbon-neutral energy source for competing with fossil fuels for energy production, because solar radiation is readily accessible at almost any location on the surface of the Earth (Cook et al., 2010). Artificial photosynthesis aims to mimic natural photosynthesis, where sunlight is stored in the form of chemical bonds through reduction of CO2 into sugars, employing H2O as the ultimate source of electrons (Mcevoy and Brudvig, 2006). Therefore, an artificial photosynthesis device would convert sunlight into spatially separated electron/hole pairs and store its energy subsequently into chemical bonds by means of water splitting, obtaining hydrogen as a clean fuel together with oxygen as the only side product (Lewis and Nocera, 2006; Balzani et al., 2008; Barber, 2009). Unfortunately, the market introduction of commercial artificial photosynthesis devices is still hampered by the lack of robust, inexpensive and efficient water oxidation catalysts (WOCs) (Dau et al., 2010; Seh et al., 2017).

Over the last decades, scientists have reported a wide variety of new WOCs. Homogeneous organometallic compounds work at fast oxygen evolution rates and offer good processability (Concepcion et al., 2008, 2009; Bozoglian et al., 2009; Blakemore et al., 2010; Xu et al., 2010; Lloret-Fillol et al., 2011; Mccool et al., 2011; Barnett et al., 2012; Duan et al., 2012; Liu and Wang, 2012; Zhang et al., 2013; Goberna-Ferrón et al., 2014). However, they often suffer from limited long-term stability due to oxidative degradation of the organic ligands in the harsh working conditions needed for water oxidation. Precious-metal-based WOCs, for instance Ir-, and Ru-based materials, have shown superior performance and stability for water oxidation catalysis (Pillai et al., 2000; Youngblood et al., 2009; Blakemore et al., 2010; Duan et al., 2012). Unfortunately, the high production price due to metal scarcity questions their viable implementation into commercial devices. Earth abundant transition metal oxides and perovskites are a robust alternative, but exclusively in alkaline media (Galán-Mascarós, 2015). Therefore, alternatives to the current state-of-the-art catalysts are needed.

Polyoxometalates (POMs) have recently appeared as a promising new catalyst class (Geletii et al., 2008; Sartorel et al., 2008). When employed as WOCs, they combine the most appealing features of homogeneous and heterogeneous materials, and many of them can be obtained from inexpensive raw materials. They are all-inorganic molecular clusters with high stability under strongly oxidizing conditions. At the same time, their molecular nature provides access to the tunability and superior processing capabilities of homogeneous catalysts for their easier implementation into devices (Pope, 1983; Pope and Müller, 2001). POMs have shown high catalytic activity in water oxidation over a remarkable pH range (0-10), and they retain their catalytic activity under heterogeneous conditions as their corresponding insoluble salts, or when anchored onto solid supports (Wu et al., 2012; Guo et al., 2013; Quintana et al., 2013; Soriano-López et al., 2013).

Among polyoxometalates, the cobalt-containing POMs (Co-POMs) have emerged as the most promising WOCs due to their high efficiency and kinetics (Goberna-Ferrón et al., 2012; Lv et al., 2012, 2014; Evangelisti et al., 2013). After Hill et al. reported the OER activity of the [Co4(H2O)2(PW9O34)2]10− polyanion (Yin et al., 2010; Huang et al., 2011; Stracke and Finke, 2011, 2013, 2014), we turned our attention to the high nuclearity [Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]16− (Goberna-Ferrón et al., 2012, 2015; Soriano-López et al., 2013; Co9, Figure 1). Co9 shows good activity for photo-assisted water oxidation in homogeneous conditions, exhibiting fast charge transfer kinetics with the model [Ru(bpy)3]2+ photosensitizer (bpy = 1,2-dipyridyl; Natali et al., 2017). It is also active in the solid state when processed as an insoluble salt with alkaline metal countercations (Soriano-López et al., 2013).

Figure 1

Polyhedral representation of the polyanion [Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]16− (Co); WO6, gray octahedra; PO4, orange tetrahedra; CoO6, pink octahedra.

In this work we report the next required step on the road to technological applications for Co in an artificial photosynthesis platform, namely its combination with a photosensitizer in a light-induced process in heterogeneous conditions. These essays have been very successful with other POMs and water oxidation catalysts to assess photo-induced catalytic performance, mechanistic considerations, and stability issues (Puntoriero et al., 2010; Gao et al., 2013; Sartorel et al., 2013; Al-Oweini et al., 2014; Xiang et al., 2014; Natali et al., 2017). Our experiments confirm the efficient electron transfer between catalyst and sensitizer, even when both species are combined into an insoluble salt. The latter opens up interesting possibilities for future combinations of cationic photosensitizers with polyanionic WOCs for the construction of compact functional photoelectrodes.

Experimental section

Materials and synthesis

Tris(2,2′-bipyridyl)dichlororuthenium(II) hexahydrate and sodium persulfate were purchased from TCI and Sigma-Aldrich (>99% purity) and used without further purification. The synthesis of Cs15K[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·39H2O (CsCo) was already reported (Soriano-López et al., 2013). [Ru(bpy)3](5+x)K(6−2x)[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·(39+x)H2O (RuCo) was prepared by metathesis: A stoichiometric excess of [Ru(bpy)3]Cl2 was added to a solution containing Na8K8[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·43H2O (KCo). RuCo immediately precipitated as an orange powder. It was filtered, washed with water and acetone, and air-dried.

Material characterizations

Elemental CHN analysis was performed with an Elemental Microanalyzer Flash model 1112. Detection of Co, Ru, and W was performed on an inductively coupled plasma atomic emission spectrometer iCap 6500 (Thermo Fisher Scientific), and K was detected on a 2,380 atomic absorption spectrophotometer (Perkin-Elmer), both by Mikroanalytisches Labor Pascher (Remagen/Germany). Thermogravimetric analyses were performed with powder samples using a TGA/SDTA851 Mettler Toledo with a MT1 microbalance. Dynamic light scattering was used to measure the particle size distribution employing a Malvern NanoZS analyzer. FT-IR spectra were collected in the 3600–400 cm−1 range with a Bruker Optics FTIR Alpha spectrometer equipped with a DTGS detector and a KBr beamsplitter at 4 cm−1 resolution. Raman measurements were acquired using a Renishaw inVia Reflex Raman confocal microscope (Gloucestershire, UK) equipped with a diode laser emitting at 785 nm at a nominal power of 300 mW, and a Peltier-cooled CCD detector (−70°C) coupled to a Leica DM-2500 microscope. X-ray photoelectron spectroscopy (XPS) (K-ALPHA, Thermo Scientific SSTTI at University of Alicante) was used to analyze the surface of the samples. All spectra were collected using Al-Kα radiation (1486.6 eV), monochromatized by a twin crystal monochromator, yielding a focused X-ray spot with a diameter of 400 μm, at 3 mA x 12 kV. The alpha hemispherical analyzer was operated in the whole energy band, and 50 eV in a narrow scan to selectively measure the particular elements.

Photoinduced water oxidation catalysis

Oxygen evolution experiments were performed in a 6.7 mL headspace Schlenk tube sealed with a rubber septum (PFTE). The Schlenk tube was covered with aluminum foil, in order to avoid an early light-induced reaction of the system, and filled with 1 mM (9.4 mg) [Ru(bpy)3]Cl2, 5 mM (14.9 mg) Na2S2O8, the desired amount of catalyst, and 12.5 mL of 40 mM KPi buffer solution at pH 7.0. Experiments employing the RuCo salt as catalyst were performed with and without addition of [Ru(bpy)3]Cl2, the former for comparison in the same conditions required for Co3O4 experiments. Suspensions were completely deaerated by purging with nitrogen. A baseline of 20 min was recorded to ensure that no oxygen leakage or side reactions took place. Next, the system was exposed to the light of a blue LED lamp (wavelength at peak emission = 465 nm; OSRAM Opto Semiconductors) working at 0.20 A and 11.4 V. The concentration of oxygen in the headspace was measured by employing a O2-sensor probe (Ocean Optics NeoFOX oxygen-sensing system equipped with a FOXY probe). Turnover number (TON) and turnover frequency (TOF) were estimated per Co content as obtained from chemical analyses on fresh compounds (see SI).

Results and discussion

Visible-light-driven water oxidation by CsCo9 in heterogeneous conditions

Water oxidation experiments were carried out with [Ru(bpy)3]2+ as a model photosensitizer and S2 as sacrificial electron acceptor, in a suspension of the insoluble salt Cs15K[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3] (CsCo). Light irradiation (λ > 400 nm) of this mixture promotes oxygen evolution, which was monitored using a fluorescence O2-sensor probe for increasing amounts of CsCo (1–50 mg). The proposed net reaction mechanism for light-driven water oxidation catalyzed by POMs is depicted in Scheme 1. No oxygen evolution was detected in the absence of any of the components.

Scheme 1

Schematic representation of the light-driven water oxidation catalysis reaction, employing [Ru(bpy)3]2+ as photosensitizer, S2 as sacrificial electron acceptor, and a polyoxometalate as water oxidation catalyst (further side reactions giving rise to sulfate radical anions were omitted for clarity).

The reaction starts with fast kinetics immediately after light irradiation, and slows down until oxygen evolution stops reaching a plateau after 2 h. We analyzed the oxygen production as a function of catalyst content (Figure 2 and Table 1). The highest values of turnover number (TON) and turnover frequency (TOF) obtained were 14.2 and 10.8 h−1, for the minimum quantity used (1 mg, ≈ 0.1 μmol). In terms of chemical yield (CY, see SI), a maximum 9.2% was reached for intermediate CsCo contents (10 mg, ≈ 1 μmol) in the investigated range. After oxygen evolution, CsCowas recovered from the reaction vessel to perform structural characterization. The FT-IR spectrum shows the typical Co bands within the 1,100-400 cm−1 range, identical to those observed with the freshly made CsCo. We also found additional bands in the region between 1,200 and 1,600 cm−1, which can be attributed to the bipyridyl (bpy) ligand (Figure S1). The same information is obtained from the Raman spectra (Figure S2). Moreover, comparison of the XPS spectra (Figure S3) showed the appearance of intense Ru peaks in the recovered CsCo, and disappearance of the expected Cs peak (Figure S4). The data in their entirety suggest that cation exchange occurred under turnover conditions, i.e., Cs+ cations are replaced by [Ru(bpy)3]2+ cations. Indeed, the Raman spectrum of the recovered CsCo is reminiscent of the corresponding Raman spectrum of the salt obtained by addition of an excess of [Ru(bpy)3]Cl2 to an aqueous K16Co solution (Figure S9).

Figure 2

Oxygen evolution profile of the CsCo salt in KPi (40 mM) buffer at pH 7, with [Ru(bpy)3]2+ (1 mM) and S2 (5 mM).

Table 1

Comparison of visible-light-driven oxygen evolution performance of CsCo and RuCo catalysts(.

POM	Catalyst (mg)	1	5	10	20	50
CsCo9 (first run)	TON	14.2	5.3	2.9	0.7	0.2
	TOF (h−1)	10.8	4.0	1.4	0.3	0.2
	CY (%)	4.4	8.4	9.2	4.0	3.6
RuCo9	TON	27.3	20.3	16.7	7.2	2.7
	TOF (h−1)	19.1	11.9	17.0	9.0	4.3
	CY (%)	7.6	28.4	47.6	42.4	36.4
POM	Catalyst (μm)	0.1	0.5	1	2	5

TON, total turnover number after completion of the reaction; TOF, slope of the oxygen evolution curve at the starting time; CY, total chemical yield after completion of the reaction.

Visible-light-driven water oxidation by RuCo9 in heterogeneous conditions

Addition of an excess of [Ru(bpy)3]Cl2 to an aqueous KCo solution forms immediately an insoluble precipitate. The presence of the [Ru(bpy)3]2+ cation and the [Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]16− anion were confirmed by FT-IR spectroscopy (Figure S8) with the signature bands for both molecular species. However, the exact stoichiometry was difficult to completely assess. We carried out elemental CHN analyses, and metal ICP analyses, along with thermogravimetry analyses, and they were not fully consistent (Table S1). It is worthy to note at this point that our attempts to crystallize this compound in order to accurately characterize its composition and structure failed, because slow diffusion between solutions of cation and anion produce insoluble single crystals of the compound [Ru(bpy)3]2K12[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·xH2O (Table S2, Figure S13). This Ru/POM stoichiometry is far too low in comparison with our RuCo analyses (Table S1), and thus it is not representative of the RuCo catalyst. The obtention of this crystalline phase, though, precludes the isolation of other salts with higher [Ru(bpy)3]2+ content, closer to the present RuCo solid. The most plausible explanation is that RuCo actually consists of a mixture of different [Ru(bpy)3]/Co salts, and their slightly different solubility and composition gives small deviations depending on the given analytical technique. With all the analytical data taken into account (Table S1), we assign an average stoichiometry [Ru(bpy)3](5+x)K(6−2x)[Co9(H2O)6(OH)3(HPO4)2(PW9O34)3]·(39+x)H2O (RuCo), where −1 < x < 1 (see Table S1 and Figure S5). This powder is insoluble in water at room temperature with an average particle size of 374 nm (Figure S6).

When a suspension of RuCo in a solution of S2 is irradiated (λ > 400 nm), oxygen evolution starts. In this case, the proposed reaction mechanism is analogous to that depicted in Scheme 1, but with photosensitizer and catalyst bound together in the solid state through electrostatic cation-anion interactions. Remarkably, the measured oxygen evolution in these conditions (Figure 3) is significantly superior to the first run starting from photosensitizer in solution (Table 1 and Figure 4). The maximum TON (27.3) and TOF (19.1 h−1) values are doubled, and the CY showed a remarkable increase up to 47.6%. Pulsed experiments confirmed that oxygen evolves exclusively when the light source is switched on (Figure S7).

Figure 3

Oxygen evolution profile for solid RuCo in KPi (40 mM) buffer at pH 7 with S2 (5 mM).

Figure 4

Comparison of TON, TOF, and chemical yield (CY) for RuCo (blue) and CsCo (red). Experiments were carried out in a KPi (40 mM) buffer at pH 7, with S2 (5 mM). [Ru(bpy)3]2+ (1 mM) was added to the suspension of CsCo, whereas no homogeneous photosensitizer was added for the RuCo catalyst.

Stability of the RuCo9 system

In order to determine the limiting agent in the photo-assisted oxygen evolution reaction, we carried out different tests. Successive additions of S2 to the as-used RuCo suspension indicate that oxygen evolution activity is severely affected after each cycle (Figure 5 and Table 2), i.e., the system can barely perform three cycles before reaching complete deactivation. After deactivation, addition of an aliquot containing the photosensitizer [Ru(bpy)3]2+ and S2 to the reaction vessel restarts oxygen evolution, with rates and yields comparable to those obtained with CsCo (Figure 5). This behavior can only be explained with deactivation of the photosensitizer in RuCo recycling experiments, probably due to oxidative degradation of the organic ligands, during the harsh working conditions. The catalytic POM appears to be robust, since its performance is maintained during successive cycles.

Figure 5

Top: Oxygen evolution with successive additions of oxidant S2 (5 mM) to a KPi (40 mM) buffered suspension of RuCo (10 mg, 0.9 μmol) at pH 7. Bottom: Oxygen evolution after addition of photosensitizer [Ru(bpy)3]2+ (1 mM) and oxidant S2 (5 mM) as solid reagents to a KPi (40 mM) buffered suspension of recycled RuCo at pH 7 compared with the same experiments starting from fresh CsCo.

Table 2

Comparison of the RuCo-catalyzed light-driven oxygen evolution performance obtained for successive addition of S2 (5 mM) to the reaction vessel.

	TON	TOF (h−1)	CY (%)
1st cycle	16.7	17.0	47.6
2nd cycle	6.4	2.7	17.6
3rd cycle	2.1	0.7	5.6

TON, total turnover number at the final reaction time; TOF, slope of the oxygen evolution curve at the starting time; CY, total chemical yield at the final reaction time.

Analysis of adventitious CoOx formation

In water oxidation with cobalt-based catalysts, it is fundamental to rule out the in situ formation of cobalt oxide CoOx, a competent heterogeneous WOC. This could occur through Co2+ leaching from the RuCo salt, and the subsequent formation of CoOx under oxidative conditions. Thus, we analyzed the as-used RuCo with different experimental techniques in the search for traces of CoOx.

RuCo was recovered from the reaction vessel after the visible-light-driven water oxidation experiments. The signature FT-IR and Raman bands of the Co cluster remain identical when compared with pristine RuCo, suggesting that the bulk POM structure is maintained during the experiments. Raman spectroscopy is particularly suited to detect even traces of CoOx due to its high surface sensitivity, but no bands that could be assigned to a CoOx species are present (Figures S8–S10).

As with fresh RuCo, the elemental and ICP analyses showed small deviations, making difficult to confirm final stoichiometry. The numbers are not too different from the original stoichiometry (Table S1). However, we need to point out that these analyses show a decrease for all elements, except for W that increases. We assign this surprising result to the deterioration of the compounds during working conditions [triggered by the [Ru(bpy)3]2+ decomposition], making them even more insoluble, and untractable.

Another powerful surface-sensitive technique is XPS. Pristine and recovered RuCo salts display analogous XPS spectra (Figure S11). The presence of CoOx should include the appearance of a typical Co3+ peak below 780 eV (Chuang et al., 1976; Tan et al., 1991; Hara et al., 2000). Close analysis of the Co and O edges in search of such features that could be assigned to the presence of an CoOx phase were negative. XPS spectra of RuCo before and after oxygen evolution show intense bands only in the 780-783 eV range, which differ from those expected for CoOx (Figure S12). This indicates that no cobalt oxide amounts are formed during turnover conditions within the detection limit of these techniques.

In order to gather additional indirect proof of the absence of the significant participation of cobalt oxide impurities, we compared the photo-induced oxygen evolution reaction starting from the RuCo salt to the Co3O4 catalyst (Figure 6 and Table 3). For equimolar conditions, RuCo displays an overall better performance, with faster onset kinetics and a higher efficiency. This is incompatible with the attribution of the catalytic activity observed for RuCo to very small traces of CoOx, which may be below the detection limit of Raman or XPS techniques.

Figure 6

Comparison of the measured oxygen evolution employing equimolar Co amounts for RuCo (blue) and Co3O4 (green). The experiments were performed in a KPi (40 mM) buffer at pH 7 with [Ru(bpy)3]2+ (1 mM) as photosensitizer and S2 (5 mM).

Table 3

Comparison of the light-driven oxygen evolution data catalyzed by RuCo and by Co3O4 under the same reaction conditions[a,b].

Catalyst	TON	TOF (h−1)	CY (%)
RuCo9	3.2	2.3	17.2
Co3O4	0.9	0.3	12.8

TON, total turnover number at the final reaction time; TOF, slope of the oxygen evolution curve at the starting time; CY, total chemical yield at the final reaction time.

The experiments were performed in a KP.

Conclusions

We compared the heterogeneous catalytic activity of two different Co starting materials under visible-light-driven water oxidation conditions at neutral pH. Direct combination of CsCo with a homogeneous photosensitizer yields a maximum turnover number (TON) of 14.2 and a maximum turnover frequency (TOF) of 10.8 h−1 with oxygen yields around 10%. Pre-catalytic incorporation of the cationic photosensitizer into the polyoxometalate salt through substitution of the alkali metal improves the oxygen evolution notably, affording chemical yields close to 50%. We associate this improvement to two beneficial effects of photosensitizer immobilization. On the one hand, the closer cation-anion (photosensitizer/catalyst) interaction in the solid state facilitates electron transfer, and therefore enhances the oxygen evolution kinetics. Additionally, the incorporation of the photosensitizer into the solid state partially improves its stability, an additional benefit to increase the efficiency of the overall process.

Our experimental data indicate that oxygen evolution eventually stops due to decomposition of the photosensitizer. Successive additions of photosensitizer re-start the water oxidation reaction at consistent rates, supporting the stable catalytic performance of Co. We carried out careful surface analyses on the as-used catalyst in the search of traces of cobalt oxide. Neither Raman nor XPS spectroscopy showed any feature that could be associated with CoOx species. Additionally, RuCo exhibits superior catalytic performance than Co3O4. Thus, the hypothetical presence of undetectable CoOx traces cannot be responsible for the observed catalytic activity. This supports the genuine catalytic activity of RuCo for photo-induced water oxidation as the first example, to the best of our knowledge, of an effective photosensitizer/catalyst electron transfer in an ionic salt. The superior performance of this ionic composite opens up interesting perspectives for the use of such materials in the development of compact photoanodes for artificial photosynthesis.

Author contributions

GP and JRG-M proposed the concept. GP, JRG-M, and JS-L designed the experiments. JS-L and FS carried out the experiments. All authors analyzed the data and contributed to the manuscript writing.

Conflict of interest statement

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.