Shunichi Fukuzumi - Electron Transfer

10 Chapter 10Figure 10.1 Time profiles of formation of [Fe(C 5H 4Me) 2] +monitored at 650 ...Scheme 10.1 The catalytic cycle for the two‐electron reduction of O 2by Fe(C 5HFigure 10.2 Selected distance (Å) in Co 2(DPB), Co 2(DPA), Co 2(DPX), and Co 2(DPD...Scheme 10.2 The catalytic mechanism of the four‐electron reduction of O 2by fe...Figure 10.3 (a) Time profiles of formation of [Fe(C 5Me 5) 2] +monitored by a...Scheme 10.3 Catalytic dehydration vs. oxygenation of the R group of AcrHR with...Scheme 10.4 Mechanism of the catalytic oxygenation of the R group of AcrHR by ...

11 Chapter 11Scheme 11.1 Catalytic cycle for thermal water oxidation with CAN using [(L)Ru I...Scheme 11.2 Catalytic cycle for photodriven water oxidation by persulfate us...Scheme 11.3 Catalytic cycle for water oxidation by CAN with a Ru III‐aqua compl...Scheme 11.4 Catalytic cycle for photodriven water oxidation by persulfate with...Scheme 11.5 Catalytic cycle for photodriven water oxidation at pH 9.3 by per...

12 Chapter 12Figure 12.1 Structures of Co porphyrin catalysts for two‐electron reduction of...Scheme 12.1 Photocatalytic water oxidation by O 2to produce H 2O 2.Figure 12.2 (a) Time courses of H 2O 2production under visible light irradiatio...Figure 12.3 A schematic drawing of (Fe xCo 1−x) 3[Co(CN) 6] 2where x = 0, 0....Figure 12.4 Schematic representation of a two‐compartment cell employed in t...Figure 12.5 Production of H 2O 2under photoirradiation of a two‐compartment cel...Scheme 12.2 Photocatalytic water oxidation by O 2to H 2O by double photoexcitat...

13 Chapter 13Figure 13.1 Photocatalytic production of H 2O 2from water and O 2using m‐WO 3/FT...Figure 13.2 Time courses of H 2O 2production with m‐WO 3/FTO photoanode and Co IIFigure 13.3 I–V (light grey) and I–P (dark grey) curves of the one...

14 Chapter 14Figure 14.1 Time courses of O 2evolution by X‐Q [0.50 mM; DDQ (black), BQ (sec...Scheme 14.1 Proposed mechanism of the photodriven water oxidation by DDQ with ...

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2 Table of Contents

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Shunichi Fukuzumi

Author

Shunichi Fukuzumi

Department of Material & Life Science

Osaka University

2‐1 Yamada‐oka, Suita

Osaka University

565‐0871 Osaka

Japan

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© 2020 Wiley‐VCH Verlag GmbH & Co. KGaA, Boschstr. 12, 69469 Weinheim, Germany

All rights reserved (including those of translation into other languages). No part of this book may be reproduced in any form – by photoprinting, microfilm, or any other means – nor transmitted or translated into a machine language without written permission from the publishers. Registered names, trademarks, etc. used in this book, even when not specifically marked as such, are not to be considered unprotected by law.

Print ISBN:978‐3‐527‐32666‐2

ePDF ISBN:978‐3‐527‐65180‐1

ePub ISBN:978‐3‐527‐65179‐5

oBook ISBN:978‐3‐527‐65177‐1

The author gratefully acknowledges the contributions of his collaborators mentioned in the references. The author thanks Japan Science Technology Agency and the Ministry of Education, Culture, Sports, Science and Technology of Japan for the continuous support.

The rapid consumption of fossil fuel has already caused unacceptable environmental problems such as the greenhouse effect by CO 2emission, which is predicted to lead to disastrous climatic consequences [1]. Moreover, the consumption rate of fossil fuels is expected to increase further at least twofold relative to the present by midcentury because of population and economic growth, particularly in the developing countries. It is becoming more and more obvious that fossil fuels will run out eventually in the next century despite the recent shale gas revolution. Thus, renewable and clean energy resources are urgently required in order to solve global energy and environmental issues [2,3]. Among renewable energy resources, solar energy is by far the largest exploitable resource [1–3]. Nature harnesses solar energy for its production by photosynthesis, and fossil fuels are the product of photosynthesis [4]. Fossil fuels range from volatile materials with low carbon:hydrogen ratios such as methane, to liquids such as petroleum, and to nonvolatile materials composed of almost pure carbon, such as anthracite coal. The age of the organisms and their resulting fossil fuels is typically millions of years, and sometimes exceeds 650 million years. The consumption rate of fossil fuels is becoming much faster than the production rate by nature. Thus, it is quite important to develop artificial photosynthetic systems for production of solar fuels, which are hopefully simpler and more efficient than natural systems. The conversion of photon energy to chemical energy in photosynthesis is achieved by electron transfer from the excited state of an electron donor (D *: *denotes the excited state) to an electron acceptor (A) to produce the charge‐separated state (D ·+–A ·−). The high oxidizing power of D ·+in D ·+–A ·−is used for four‐electron oxidation of water to produce dioxygen, whereas the high reducing power of A ·−is used to reduce nicotinamide adenine dinucleotide phosphate (NADP +) coenzyme to NADPH [5]. NADPH reduces CO 2by multi‐electron reduction to produce sugar [4,5]. Thus, electron transfer plays essential roles in photosynthesis. In order to develop artificial photosynthesis systems, it is quite important to control electron‐transfer systems to maximize the energy conversion.