(Invited) Development of Molecular Photocathodes Based on Metal Complex Photocatalyst and Their Application for Photoelectrochemical CO2 Reduction in Aqueous Electrolyte

Abstract

Metal complex photocatalysts are promising candidates in CO2 photo-reduction systems in terms of its high efficiency and selectivity under visible light even in aqueous solution.[1] These systems, however, need the sacrificial reductive additives as electron donor due to the low oxidation power of photosensitizer unit. In this study, we developed novel “molecular” photocathodes consisting of Ru(II)-Re(I) metal complex photocatalyst (RuRe) and p-type semiconductor electrodes for visible-light-driven CO2 reduction (Figure). The application of the molecular photocathodes for photoelectrochemical CO2 reduction in aqueous solution was also examined. RuRe consists of tris-diimine Ru(II) unit as a photosensitizer and tricarbonyl diimine Re(I) unit as a catalyst, and has methylphosphonate anchoring group to adsorb on the electrode surface. p-type NiO electrode was synthesized and hybridized with RuRe to obtain molecular photocathode (RuRe/NiO).[2] This RuRe/NiO photocathode displayed photocathodic responses under the visible light (λex > 460 nm), which selectively photoexcites Ru(II) photosensitizer in RuRe, in a CO2-purged aqueous electrolyte without the need for any sacrificial additives. It reflects that the photo-excited RuRe can receive electrons from an external circuit through the NiO electrode. The onset potential for cathodic photocurrent was approx. -0.1 V vs. Ag/AgCl in a CO2-purged 50 mM NaHCO3 aqueous solution. Photoelectrochemical CO2 reduction using the RuRe/NiO photocathode was examined under the continuous irradiation at the potential of -0.7 V vs. Ag/AgCl, resulting that the catalytic amount of CO was observed. Its turnover number for CO formation, which was based on the amount of RuRe on the NiO, was 32 for 12 h irradiation. These results clearly suggest that the immobilized metal complex photocatalyst (RuRe) functions to drive photoreduction of CO2 with using electrons supplied from the NiO electrode. We next developed p-type CuGaO2 electrode as an alternative of NiO for such molecular photocathode with RuRe.[3] The resulting RuRe/CuGaO2 photocathode also shows photoelectrochemical activity for CO2 reduction under visible light irradiation. The photocathodic responses was obtained from approx. +0.3 V vs. Ag/AgCl, which is equivalent to +0.9 V vs. RHE. This value of onset potential is around 0.4 V positive than that for RuRe/NiO, which means that the utilization of CuGaO2 as an electrode material enlarged the region of working potential for CO2 reduction to positive direction. This tendency agreed well to the flat band potentials of these semiconductor electrodes obtained from the electrochemical impedance spectroscopy. The turnover number of CO formation using the RuRe/CuGaO2 photocathode reached to 125 for 15 h irradiation, while H2 was also generated as byproduct. These results indicate the advantage of CuGaO2 for usage of an electrode material for molecular photocathode from the aspect of efficient interfacial electron injection. In addition, these photocathodes were investigated to combine with a CoO x /TaON photoanode for the oxidation of water.[4] The constructed photoelectrochemical cells consisting of these molecular photocathodes and the CoO x /TaON photoanode enabled the visible-light-driven catalytic reduction of CO2 with water oxidation to obtain CO and O2 as the products. These systems successfully demonstrated CO2 reduction using water as an electron donor by means of combined photocatalytic abilities of both the molecular metal complex (RuRe) and the semiconductor material (TaON). To the best of our knowledge, these are the sole examples of visible-light-driven CO2 reduction systems using water as the reductant, based on molecular photocatalysts with hybridizing semiconductor. [1] Y. Yamazaki, H. Takeda and O. Ishitani, J. Photochem. Photobiol. C, 2015, 25, 106–137.; A. Nakada, K. Koike, K. Maeda and O. Ishitani, Green Chem., 2016, 18, 139–143. [2] G. Sahara, R. Abe, M. Higashi, T. Morikawa, K. Maeda, Y. Ueda and O. Ishitani, Chem. Commun., 2015, 51, 10722–10725.; G. Sahara, H. Kumagai, K. Maeda, N. Kaeffer, V. Artero, M. Higashi, R. Abe and O. Ishitani, J. Am. Chem. Soc., 2016, 138, 14152–14158. [3] H. Kumagai, G. Sahara, K. Maeda, M. Higashi, R. Abe and O. Ishitani, Chem. Sci., 2017, 8, 4242–4249. [4] M. Higashi, K. Domen and R. Abe, J. Am. Chem. Soc., 2012, 134, 6968–6971. Figure 1