Chemoselective reduction and oxidation of ketones in water through control of the electron transfer pathway

The selective synthesis of different products from the same starting materials in water, which is the most abundant solvent in nature, is a crucial issue as it maximizes the utilization of materials. Realizing such reactions for ketones is of considerable importance because numerous organic functionalities can be obtained via nucleophilic addition reactions. Herein, we report chemoselective reduction and oxidation reactions of 1,2-diketones in water, which initiates anionic electron transfer from the inorganic electride [Ca24Al28O64]4+·4e−, through controlling the pathway of the electrons to substrates. The generation of different radical species for transient intermediates was the key process required to control the reaction selectivity, which was achieved by reacting the anionic electrons with either diketones or O2, leading to the formation of ketyl dianion and superoxide radicals in the reduction and oxidation reactions, respectively. This methodology that utilizes electrides may provide an alternative to the pulse radiolysis of water in synthetic chemistry.

Scientific RepoRts | 5:10366 | DOi: 10.1038/srep10366 The development of chemoselective organic transformations is one of the most fundamental tasks in synthetic chemistry because it reduces material consumption, superfluous trimming and re-functionalization steps in reactions 21,22 . In particular, achieving chemoselectivity in water-mediated reactions by controlling the electron transfer pathway enables a single reactant to be transformed into structurally diverse products with different functionalities. However, the chemoselectivity of fundamental reactions in water, such as oxidation and reduction, has not been previously explored. Herein, we report chemoselective reactions both reduction and oxidation of 1,2-diketones in water by controlling the intermolecular electron transfer pathway with inorganic [Ca 24 Al 28 O 64 ] 4+ •4e − electrides.
Electrides are ionic crystals with cavity-trapped electrons that act as anions 23 . The first electride was synthesized in 1983 using crown ethers and solvated electrons in alkali-ammonia solutions to provide precursors for anionic electrons 24 . Because the organic electrides were chemically and thermally unstable and decomposed in ambient conditions, their applications for synthetic chemistry were limited 25 . In 2003, the first electride stable at room temperature was synthesized using the inorganic complex oxide   27 and transformation to a molten state at 1873 K while maintaining the solvated electrons 28 . This inorganic electride has recently appeared in a new class of reagents that serves as electron generators in aqueous solutions, facilitating the pinacol coupling reaction of aldehydes 29 . One consequence of the reaction between the [Ca 24 Al 28 O 64 ] 4+ •4e − electride and water is that when electrides are dissolved in water, the anionic electrons that are loosely trapped in cavities can be released and directly transferred to the reactants, thus facilitating chemical reactions. Applying [Ca 24 Al 28 O 64 ] 4+ •4e − electrides to water-mediated chemoselective reactions of ketones, which are ubiquitous functional groups, can provide important insights into the fundamental roles of electrons in water-mediated synthetic organic reactions and a broad opportunity for producing diverse functional molecules. Figure 1 describes the strategy for realizing chemoselective oxidation and reduction reactions of ketones in water through controlling both the electron transfer pathway and the formation of different intermediates in each reaction. When the targeted electron acceptor is benzil 1a, which is the model substrate selected for incorporating an electron acceptor (such as a carbonyl moiety), the path of the reaction is primarily dependent on the type of catalysts and reagents being used [30][31][32][33][34][35][36][37] . In fact, either the oxidation or reduction reaction of benzil 1a can occur by using different reagents that completely alter the formation of intermediates to result in enediol 1aa" in reduction reactions and α -keto peroxide 1ab" in oxidation reactions (Fig. 1a). However, despite extensive research on the reaction of benzil with diverse electron transfer reagents and solvents, there was no success in utilizing both electron transfer pathways with one reagent in a highly selective manner. Furthermore, a selective reaction in the presence of water is difficult to achieve because of the vigorous water splitting reactions that occur between the excess electrons from the reagents and water. Nevertheless, as shown in Fig. 1b, it is hypothesized that the chemoselective reaction of benzil 1a in the presence of water is possible if the electrons are smoothly generated through a moderate cage-opening rate by the robustness of the [Ca 24 Al 28 O 64 ] 4+ •4e − electride in water, which diminishes the loss of electrons by water splitting. The solvated electrons would then react with different substances, such as benzil or O 2 , to selectively form the transient radicals (1aa' or I). To realize our hypothesis, the [Ca 24 Al 28 O 64 ] 4+ •4e − electride, which is an electron-donating reagent that possesses moderate reactivity in water, was used because of its smooth electron release and the possible solvation of anionic electrons by water molecules. Figure 1c shows the details of our approach of using the [Ca 24 Al 28 O 64 ] 4+ •4e − electride to realize chemoselective reactions of benzil in water. In water-mediated reactions with the [Ca 24 Al 28 O 64 ] 4+ •4e − electride, water has two important roles: 1) releasing anionic electrons from the electrides and 2) acting as the medium for transferring the anionic electrons to electron acceptors. The cage structure of the  4+ •4e − electride slowly decomposes in water and forms a Ca-Al-O-OH gel as aluminous cement, leading to the release of anionic electrons. The released electrons are transferred to the appropriate electron acceptors, most likely through electron solvation by water molecules, which are aptly referred to as solvated electrons. During the reaction, we observed the evolution of hydrogen gas as a result of water splitting by electrons, which indicates that electrons are in proximity to water molecules. Because the formation of transient radicals is critical in determining the course of reactions and producing an intermediate, controlling the electron transfer pathway is the major concern. In the reduction reaction, benzil 1a accepts two electrons and then transforms into the enediol dianion 1aa'. In postulating the oxidation reaction, we intentionally involved oxygen molecules in the reaction to facilitate the formation of the superoxide radicals I. Table 1 presents the results of the reduction reaction of benzil 1a, which was conducted under an inert argon atmosphere to prevent the incorporation of oxygen molecules in the reactions. Benzil 1a accepts two electrons from the [Ca 24 Al 28 O 64 ] 4+ •4e − electride and then transforms into the enediol dianion 1aa'. The resulting enediol dianion species may subsequently undergo protonation, affording an α -hydroxy ketone via keto-enol tautomerization. To identify the necessity of a proton source, we initially performed the reaction of benzil 1a with 1.0 equivalent of electride in water alone. However, no reaction occurred, most likely due to the poor solubility of benzil 1a in water (Table 1, entry 1), which prompted the use of co-solvent to improve the solubility of benzil 1a. We observed the reaction progress when deoxygenated THF-H 2 O (v/v = 1:1) was applied as a co-solvent to the reaction of benzil 1a with 1.0 equivalent of [Ca 24 Al 28 O 64 ] 4+ •4e − at 60 °C under an inert argon atmosphere. In this reaction, benzil 1a was reduced to benzoin 2a in low yield after 24 h (Table 1, entry 2). The use of an additional equivalent of electride led to a slight improvement in the reaction yield ( . This result is attributed to two reasons: 1) the difference in solvent polarity, which facilitates rapid electron transfer 38 , and 2) the difference in solvent acidity, which accelerates protonation of the products. A more polar solvent is expected to facilitate electron transfer because of the stronger coupling between molecules and the faster solvation response. Although the two solvents, MeOH and H 2 O, have similar pKa values (pKa of H 2 O = 15.7 and pKa of MeOH = 15.5), the more acidic MeOH molecule donates a proton and becomes a − OMe ion. Upon acid dissociation, the methoxide ion is stabilized by the solvation of H 2 O molecules, in which the positively charged H atoms move toward the methoxide ion solutes. This process makes MeOH more acidic than H 2 O, rendering MeOH a sufficient proton source in the reduction process.

Results and Discussion
When using alcohols in the co-solvent, the yield of product 2a increased in the following order of acidity and electron transfer rates 39 (methanol > ethanol > isopropanol > tert-butanol) ( Table 1, entries 4-7). Notably, the reaction time decreased as the MeOH-H 2 O volume ratio was changed from 1:1 to 1:3 ( Table 1, entry 8). It is hypothesized that the increased polarity from the greater amount of water contributed to the acceleration of cage opening and donation of electrons from the electrides. Finally, in contrast to deoxygenated THF-H 2 O (v/v = 1:1) ( Table 1, entry 3), the use of a partially oxygenated THF-H 2 O co-solvent yielded a small amount of benzoic acid 3a (Table 1, entry 9), which was identified by NMR spectroscopy. This result indicated that the oxidative cleavage reaction of benzil 1a should be investigated by introducing oxygen molecules as electron acceptors into the reaction. To verify the necessity of electrons in the reaction, we examined the reaction using [Ca 24  Following the identification of benzoic acid 3a after using the partially oxygenated THF-H 2 O co-solvent, we changed the reaction atmosphere from inert argon gas to molecular oxygen as a terminal oxidant, which enabled an increase in the amount of oxygen molecules that was dependent upon the different solubilities of oxygen molecules in each solvent system. We initially performed the reaction of benzil 1a with 2.0 equivalents of electride in MeOH-H 2 O (v/v = 1:3) at 60 °C under an oxygen atmosphere and obtained benzoic acid 3a in 36% yield ( Table 2, entry 1). The use of DMF, DMSO and MeCN solvent in water afforded benzoic acid 3a in moderate yields (up to 53%; Table 2, entries 2-4). The reaction was optimized using THF-H 2 O co-solvent, which provided the best yield (96%; Table 2, entries 5-7). Increasing the amount of THF in the co-solvent significantly improved the yield of benzoic acid 3a ( Table 2, entries 5-7), albeit with longer reaction times (20 h). This improvement may be explained by the following two reasons: i) due to the higher solubility of O 2 in THF (2.1 mM) compared to water (0.26 mM), the reaction is accomplished through an enhanced formation of superoxide radicals, or ii) decreasing the ratio of water in the co-solvent causes a reduction in polarity, which retards cage decomposition and electron release into the solvent. The slow generation of electrons and the reduced rate of molecular oxygen permeating into the co-solvent may minimize the probability of electron loss by reaction with O 2 rather than water.
Based on the chemoselective reactions established above, we expanded the reaction scope to the diverse set of 1,2-diketone molecules listed in Table 3. In the reactions of the unsubstituted aromatic 1,2-diketones, both the reduction and oxidation reactions afforded the corresponding products in high yields ( Table 3, entries 1 and 2). Additionally, both the reduction and oxidation reactions proceeded not only for the 1,2-diketones bearing electron-withdrawing substituents on the aryl ring (Table 3, entries 3 and 4) but also for other substrates bearing strong electron-donating substituents, such as -Me or -OMe groups (Table 3, entries 5, 6 and 7). This result indicates that this electride, which possesses a low work function, has great potential for use as a powerful reducing agent in chemical reactions.
We also examined the feasibility of large-scale reactions using the [Ca 24 Al 28 O 64 ] 4+ •4e − electride in water to address the potential limitations of utilizing the [Ca 24 Al 28 O 64 ] 4+ •4e − electride in organic synthesis. For both the reduction and oxidation reactions, benzil 1a was used as shown in Fig. 2 on a 2.5 mmol scale (525 mg of benzil), which was 12.5 times greater than the amount used for the optimization. Notably, benzoin 2a and benzoic acid 3a were obtained in yields of 84% and 98%, respectively.
Based on the experimental results, we propose mechanisms associated with electron transfer from the electrides in aqueous solutions. For the mechanism of the reduction process, two electrons from the [Ca 24 Al 28 O 64 ] 4+ •4e − electride are transferred to 1,2-diketone 1a. Consequently, two ketyl radical anions  of 1,2-diketone are generated and quickly converted to enediol dianion 1aa' via radical dimerization 40 . The use of a protic solvent allowed the enediol dianion to be protonated, thereby forming enediol intermediate 1aa" which undergoes tautomerization to form α -hydroxy ketone 2a.
In contrast to reduction, the oxidation reaction was a rather complex process. The oxidative cleavage reaction occurs in a two-step process. In contrast to the reduction reaction that occurs via direct electron transfer to benzil 1a, in the oxidation reaction, the electrons are firstly transferred to the oxygen molecule, generating superoxide radicals I 41 . These radical anions then react with benzil 1a, leading to the formation of α -peroxy ketone intermediate 1ab".
To obtain insight into the reaction mechanism for oxidation, we conducted 18 O isotopic labeling experiments using 18 O 2 gas, which provides an integral part of the electron transfer pathway for the formation of carboxylic acids, as shown in Fig. 3. The superoxide radicals I was initially generated by the reaction between 18 O 2 and a single electron from the electride and then most likely transferred to 1a, affording α -keto peroxy radical anion 1ab'. Then, hydrogen abstraction from water occurred almost simultaneously to form α -keto peroxide 1ab". Subsequently, two different 18 O-labeled anhydrides, 4 and 4', were formed via either epoxidation (pathway A) or the Baeyer-Villiger reaction with acyl group migration from α -keto peroxide 1ab", with simultaneous release of 18 O-labeled hydroxide ion 5 (pathway B). Presumably, the 18 OH − ions rapidly exchanged protons with an extremely large amount of water to produce hydroxide ion (OH − ) 6 according to Le Chatelier's principle (Eq. 1). The nucleophilic attack of a hydroxide ion on the carbonyl carbon of 18  To support the proposed mechanism, the resulting products (3a and 7) were subjected to gas chromatography-mass spectrometry (GC-MS) for isotopic analysis. The 16 O and 18 O compositions of the individual carboxylic acids were determined based on the relative abundances of mass peaks at m/z = 122 for 16 O and m/z = 124 for 18 O. As shown in Fig. 4, it is clear that the relative abundances of the isotopic masses for each product are identical to those of the isotopic masses. This result strongly suggests that oxygen molecules are incorporated into 1,2-diketone, producing carboxylic acids, which is initiated by the formation of superoxide radicals I.
To expand the synthetic application of this selective fashion, we then investigated the regioselectivity in the reaction of unsymmetrical 1,2-diketone 1h with the electride (Fig. 5). The most favourable  reduction site was the carbonyl adjacent to the electron-withdrawing substituted aromatic ring, showing the specific regioselectivity of the products in a > 99: 1 ratio of 2h : 2h′ .

Summary
The use of the [Ca 24 Al 28 O 64 ] 4+ •4e − electride, an exceptional electron source, allowed the first demonstration of chemoselective oxidation and reduction reactions with ketones in water. Transient radical formation was integral to the chemoselective success of the reactions, and the formed radical was dependent on either the presence of a proton source or an oxygen molecule in each electron transfer process. This proposed mechanism explains why the electron transfer process in water, which is omnipresent but often goes unnoticed, should be regarded as a critical mechanistic step for the formation of intermediate substances in chemical reactions. Additionally, this new methodology using the [Ca 24 Al 28 O 64 ] 4+ •4e − electride as a solid-state reducing agent in water may provide an alternative to the high-energy pulse radiolysis of water, in which it is not possible to realize these selective chemical reactions. Finally, the solvated electrons, which are extremely potent reducing agents, can be used for oxidation reactions when the electron pathway is controlled to form the proper transient intermediates according to the desired reaction conditions.