The oxidative cleavage of the C–C bonds in 1,2-diols is an important transformation in synthetic organic chemistry. The challenge for this reaction is to develop a recyclable catalyst and an efficient catalytic system that operates under mild conditions. Here we report an atomically dispersed cobalt (3.8 wt% Co) on N-doped carbon catalyst, which exhibits improved catalytic activity toward the oxidative cleavage of a variety of 1,2-diols into esters, ketones or aldehydes using molecular oxygen under mild conditions. For example, the oxidative cleavage of internal diols is achieved at ambient temperature and air pressure. The robust catalyst can be reused at least seven times without regeneration treatment. The formation of highly dispersed active Co-Nx sites is demonstrated by catalyst characterization and potassium thiocyanate poisoning experiment. Mechanistic insights into monosubstituted diols indicate a sequence reaction including stepwise oxidation/nucleophilic addition/C–C bond cleavage, and reveal two reaction pathways.
The oxidative cleavage of the C–C bonds in 1,2-diols to the corresponding carbonyl compounds is one of the most important transformation in synthetic organic chemistry1. The Malaprade reaction and the Criegee oxidation are classical methods for cleaving the C–C bond of 1,2-diols, which use stoichiometric or excess amount oxidants, such as periodic acid and its salts or lead tetraacetate (Fig. 1a)2,3. Up to now, these two methods remain the most widely used for vicinal diols cleavage. Other oxidants, such as chromium trioxide, manganese dioxide, and pyridinium chlorochromate have also been studied4. But these oxidants produce equimolar quantities of toxic waste and cannot meet the current environmental sustainable development needs. Therefore, the development of catalytic oxidation processes with a clean oxidant such as molecular oxygen is an alternative and promising protocol. A number of homogeneous transition-metal catalytic systems have been studied in the early time (Fig. 1b)5,6,7,8,9,10,11,12,13. Although these catalytic systems are capable of cleaving simple diols with molecular oxygen, most of them are still suffering from drawbacks such as low product selectivity, limited substrate range, the use of expensive noble metals (e.g., Pd, Ru), the required harsh conditions, activating sacrificial substrates, and no reusability of the catalyst. Very recently, Giulia Licini and co-workers reported vanadium-catalyzed aerobic C–C bond oxidative cleavage of vicinal diols under relatively mild conditions (80–100 °C) in different solvents, with a large variety of diols, affording the corresponding carbonyl derivatives14. Another recent example of mild silver(I)-catalyzed oxidative cleavage of 1,2-diols into carboxylic acids with wide adaptability was reported by Li and co-workers15. However, a critical drawback persists as these catalysts are homogeneous and suffer from the pervasive difficulty in recovery and reuse. Heterogeneous catalysis can address this limitation, but heterogeneous catalysts usually have the disadvantage of low activity. Some noble metal heterogeneous catalysts (such as Pt, Ru, and Au) were used for the oxidative cleavage of 1,2-diols16,17,18. Only one example was reported by Escande and co-workers for the oxidative cleavage of 1,2-diols using a heterogeneous catalyst based on non-noble metal manganese and sodium at 100 °C with a limited substrate rang (Fig. 1c)19,20. Hence, the development of sustainable and cost-efficient heterogeneous catalysts for the selective aerobic oxidative cleavage of 1,2-diolsunder mild reaction conditions still remains one of the most challenging issues.
Our recent investigations on the use of noble-metal-free nanoparticles deposited on nitrogen-doped carbon materials for various organic transformations led us to study the application of a promising heterogeneous catalyst for the oxidative cleavage of 1,2-diols21,22,23,24.
Herein, we report an atomically dispersed Co-based heterogeneous catalyst supported on nitrogen-doped carbon materials with improved catalytic performance in the aerobic oxidative cleavage of a variety of 1,2-diols into esters, aldehydes or ketones under mild conditions with O2 or air as the oxidant. The ability to cleave a variety of internal 1,2-diols at room temperature or 50 °C is a significant advantage compared to the previous reports (reaction temperature up to 100 °C)19,20. The robust catalyst can be recycled several times without loss of activity. The cobalt catalyst with well-dispersed Co–Nx sites on mesoporous N-doped carbon is synthesized by pyrolysis of well-defined natural vitamin B12 via hard template method. The studies of catalyst characterization and control experiments improve our understanding of the active species and the reaction process.
Supplementary Fig. 1 shows the simple preparation process for the cobalt catalyst according to our previous report with slight modification. The as-obtained catalysts are labeled as meso-Co-NC-X (meso: mesoporous; X: pyrolysis temperature).
Screening catalysts and optimizing the reaction conditions
Initially, the oxidative cleavage of 1-phenylethane-1,2-diol (1a) in MeOH to produce methyl benzoate (2a) was used as a model reaction to evaluate the abilities of the catalysts (Fig. 2). Firstly, the results from blank experiments indicated that the reaction did not proceed only in the presence of K2CO3 (Table 1, entry 1), and that the catalyst precursors gave no product 2a without the high temperature pyrolysis process (Table 1, entry 2). The pyrolysis temperature greatly affected the catalytic activity (Table 1, entries 3–7). Meso-Co-NC-800 showed the best catalytic performance to produce 2a in 96% yield (Table 1, entry 5). To unveil the underlying factors affecting the catalytic activity, the pore textural properties of the meso-Co-NC-X were analyzed by N2 adsorption/desorption. The surface areas, total pore volume and pore size of meso-Co-NC-X catalysts were shown in Supplementary Table 1. The results showed that the specific surface area was positively related to the catalytic efficiency of the prepared catalysts with different pyrolysis temperatures. Meso-Co-NC-800 with the highest specific surface area and total pore volume exhibited the best catalytic activity compared with the other four catalysts. Meso-Co-NC-600 showed a lower catalytic activity, which might not only be attribute to the lower specific surface area, but also the lower pore volume and the lower pore size. In order to prove the crucial role of the cobalt species surviving from the acid treatment in this reaction, the vitamin B12 analogue phthalocyanine is used as precursor to obtain the catalyst through the same preparation method. The resulting catalyst meso-Pc-800 has no activity in the reaction (Table 1, entry 8). No reactivity was observed under N2 atmosphere or in the absence of K2CO3 (Table 1, entries 9 and 10) indicating that O2 and K2CO3 were necessary to achieve this reaction. Other inorganic bases were also screened in Supplementary Table 2. K2CO3 was turned out to be the best additive. When template SiO2 was not removed, only 15% of 2a was obtained, suggesting the importance of mesoporous structure (Table 1, entry 11). Other reaction condition optimizations including catalyst loading, K2CO3 loading, air, and reaction temperature have been examined (Supplementary Table 2).
Stability study of catalyst
Encouraged by these promising results, we first need to confirm the heterogeneous nature of the catalyst. A leaching experiment was carried out by removing catalyst before the reaction was complete by simple hot-filtration test. The results showed that the yield of product did not increase further after the catalyst was filtered, suggesting that the catalytic process was truly heterogeneous (Supplementary Fig. 2). Then, the stability and recyclability of the meso-Co-NC-800 were examined. After reaction, the catalyst was filtrated off, washed with methanol and dried under vacuum. What is noteworthy is that the regeneration treatment of the used catalyst is not needed, when the next cycle is conducted. The catalyst was run for six consecutive times without any loss of activity (Supplementary Fig. 3).
N2 adsorption/desorption analysis showed the mesoporous structure of the as-obtained catalysts, and the Brunauer–Emmett–Teller (BET) surface area and the average pore size were 659.7 m2 g−1 and 12.5 nm, respectively (Supplementary Fig. 4). XRD diffractogram did not reveal anycobalt metal or its oxide peaks, indicating that the Co species in the sample are either highly dispersed or amorphous (Supplementary Fig. 5).The morphology of catalyst was characterized by electron microscopy techniques. SEM images under UED detector mode with 1.0 keV accelerating voltages showed honeycomb mesoporous structure of the meso-Co-NC-800 catalyst (Supplementary Fig. 6a, and more images see Supplementary Figure 7a–c). No cobalt-containing nanoparticles were detected on the surface of the meso-Co-NC-800, which is in good agreement with the XRD results. The result was confirmed under BED-C mode 15 keV accelerating voltages (Supplementary Fig. 6b, and more images see Supplementary Figure 7d, e, f). The same conclusion was reached from HRTEM and STEM images (Supplementary Fig. 6c-d, and more images see Supplementary Figure 8a–d). Nevertheless, from the STEM images, C, N, O, and Co elements were clearly observed on the surface of catalyst by energy-dispersive X-ray EDX analysis (Supplementary Fig. 9), and the corresponding element maps showed that these elements are evenly distributed throughout the structure (Supplementary Fig. 6e). Moreover, inductively coupled plasma atomic emission spectrometry (ICP-AES) and X-ray photoelectron spectroscopy (XPS) revealed approximately 3.8 wt% and 0.79 at% (corresponding to a weight percentage of 3.7 wt%) of cobalt survived the acid treatment, respectively. These results indicated that the cobalt species must be highly dispersed as subnanoscale level or single atoms that cannot be detected or visible by XRD, SEM, HRTEM, and STEM techniques. In order to obtain some information about the chemical state of cobalt at the atomic level, high angle annular dark field (HADDF) technique was per formed on an aberration-corrected JEM-ARM 200F microscope to observe the meso-Co-NC-800 catalyst (Supplementary Fig. 6f). It was observed that Co single atoms were uniformly dispersed on N-doped carbon materials. No agglomerated metallic cobalt or cobalt oxide are found in the whole detected region. Our previous investigation using Extended X-ray absorption fine-structure (EXAFS) indicated that at the Co K edge, the spectrum of meso-Co-NC-800 catalyst was different from the reference samples, Co foil, CoO, or Co3O4, further confirming that there exists no metallic cobalt or cobalt oxide particles in our catalyst22.
To gain more information on the elemental compositions and chemical states of as-obtained catalysts, X-ray photoelectron spectroscopy (XPS) analysis was conducted. The survey of meso-Co-NC-X (X = 600–1000 °C) catalysts was shown in Supplementary Fig. 10. C, N, O, and Co elements were detected, which is consistent with EDX results. The content of each element in a series of meso-Co-NC-X catalysts was summarized in Supplementary Table 3. The content of Co, N decreases with the pyrolysis temperature increasing, while the content of C tends to increase. The general trend of oxygen content is reduced. Especially, when the temperature reaches 800 °C, the content of O is minimum. The XPS detailed analysis of the best active catalyst (meso-Co-NC-800) was given as following. The C1s spectrum reveals four types of carbon species: C=C at 284.6 eV, C=N at 285.7 eV, C−N 286.6 eV, and O−C=O at 289.2 eV, which indicates N atoms successfully doped in the VB12 derived materials (Supplementary Fig. 11a)25. The high-resolution O1s spectrum shows the existence of carbon atoms bonded with oxygen atoms (Supplementary Fig. 11b). The high-resolution N1s spectrum was fitted into four peaks: pyridinic or N–Co (398.5 eV), pyrrolic (400.2 eV), graphitic (401.0 eV), and oxidized nitrogen (403.9 eV) (Supplementary Fig.11c)26,27. The proportion of pyridine nitrogen is greatest (accounting for 47.9% in total N species). It is important to note that the peak value of 398.6 eV should also include N–Co contribution, because the N–Co has a binding energy close to the pyridinic N. The Co XPS spectrum showed two main peaks at 780.9 eV and 795.9 eV, which are attributed to Co 2p3/2 and Co 2p1/2, respectively (Supplementary Fig. 11d). The low energy bands can be deconvoluted into two peaks: Co–O (780.0 eV), Co–N (781.7 eV)28,29. This type of Co–N was well in agreement with the N–Co species detected from N1s spectrum. These results demonstrated the existence of the coordination of Co species with N atoms in the graphitic layer (Co–Nx). This coordination environment not only resists against either aggregation during the subsequent heat treatment or leaching by acid treatment, but also plays a key role in improving the activity of catalyst30,31,32.
XPS measurements were also used to analyze the effect of pyrolysis temperature on the possible bonding between Co and N or O in catalysts. As shown in Supplementary Table 3, 800 °C affords the highest ratio of Co/N, which indicated that the density of Co–Nx active sites is the largest. In addition to Co–N, the peak Co–O was also detected in Co XPS spectrum. The cobalt coordination environment may also involve oxygen atoms33. Excessive oxygen atoms saturate the cobalt and may reduce the cobalt active sites. It should be noted that the ratio of Co/O at 800 °C is much higher than other pyrolysis temperature, indicating the existence of much more Co unsaturated sites. These results suggest that nitrogen-coordinated maximum atomic Co sites produced the largest density of Co–Nx active sites with the best activity.
Catalyst poisoning experiment
To further shed light on this viewpoint that Co–Nx species was the primary active sites in the target reactions, the poisoning experiment was performed with KSCN as binding molecule, which would interrupt the metal-centered active site and inhibit the catalyst toward the reaction. Amount of KSCN was mixed with catalyst in MeOH at 60 °C for 1 h, and then the reaction was conducted under standard conditions. The results indicated that the catalytic activity was significantly reduced (Supplementary Fig. 12).
Scope of the present reaction
With the optimal conditions in hand, we applied the catalytic method to other substrates (Fig. 3). The electron-deficient mono-substituted aromatic 1,2-diols (1a–1i) afforded the desirable products (2a–2i) in good to excellent yields. The electron-rich mono-substituted aromatic1,2-diols (1j–1n) gave the desirable products (2j–2n) in moderate to good yields. The corresponding major by-products were aldehydes. It seems that the position of the substitutes on the benzene ring has no obvious effect on cleavage of C–C bond under the optimized conditions. But the electron properties of substituents have a greater effect on the chemoselectivity of the reaction.
To further expand the substrate scope of this catalytic system, internal diols were also tested in this catalytic system. Firstly, we use (S,S)-hydrobenzoin (3a) to optimize the reaction temperature (Supplementary Table 4). It was found that the heterogeneous catalytic system can realize the oxidative cleavage of this kind of substrates at room temperature. The results are summarized in Fig. 4. Both meso- and (S,S) or (RR)-hydrobenzoin (3a–3c) were cleaved efficiently. When air replaces pure oxygen as the oxidant, the yield of 91% is still available. The substrates (3d–3e) containing an electron-withdrawing group at the aryl ring could be transformed to the desired products (2b, 2d) in excellent yields. However, 3f employed as substrate led to a low yield, and afforded 2-chlorobenzaldehyde in 64% yield. Substrates (3g–3i) with electron-rich aryl substituents gave the corresponding products (2k–2o) in good to excellent yield. The major products were the corresponding aldehydes, which might be due to the low reaction temperature (25 °C). The aldehyde is not easily converted to the corresponding ester at 25 °C. When the temperature was increased to 80 °C, 2h could be obtained in 84% yield with only 12% yield of o-chlorobenzaldehyde. The cleavage of heteroaryl 1,2-diol (3j) containing pyridine fragment, proceeded smoothly to generate heterocyclic esters 2p in 99% yield. But Furan 1,2-diol (3k) gave 61% yield of aldehyde. Several benzopinacol substrates (3l–3p) were subjected to the variable reaction conditions. The corresponding ketones (2r–2t) were obtained in excellent yield. One of the hydroxyl groups is protected by the methyl group (3q), giving 2a in 91% yield by raising the reaction temperature. It is noteworthy that the catalytic system is also effective for less activated internal diols (3r).
To further extend the range of application, this catalytic system was used to cleave C–C bonds of internal 1,2-diols to produce aldehydes, which could be used for further transformations (Fig. 5). The reaction conditions were optimized with (S,S)-hydrobenzoin (3a) as the model substrate (Supplementary Table 5). A variety of 1,2-diols with electron-donating and with drawing aromatic substituents, afforded the corresponding products in good to excellent yields (3a–3d, 3f–3j). Notably, the substrate 3f bearing o-chloro substituents underwent quantitative cleavage into the corresponding aldehyde 4f in quantitative yield. The catalytic system can also effectively oxidize the diols containing heteroatoms into the corresponding aldehyde (3j).
The synthetic utility of the present catalyst is further evaluated in multistep, one-pot reaction sequences. A variety of transformations of 1,2-diols are achieved in Fig. 6. All the desired products were obtained in good to excellent yields, suggesting that the catalyst is of high efficiency and multiple catalytic capacities.
The gram-scale experiment was performed using 1-phenylethane-1,2-diol as a test substrate. The target product was obtained in 85% yield even with the catalyst loading reduced to 2.5 mol%. The result indicates that the heterogeneous Co-based catalytic system shows high activity, selectivity, and practicability for the aerobic oxidative cleavage of 1,2-diols under mild reaction conditions.
To gain more insights into the mechanism of this transformation, several control experiments were carried out. First, a radical scavenger e.g., 2,2,6,6-tetramethyl-1-piperidinyloxy (TEMPO), 2,6-di-tert-butyl-4-methylphenol (BHT), or acrylamide is used to determine whether the reaction is a free radical process. When TEMPO, BHT, or acrylamide was added into the reaction mixture, the target product was obtained in 87%, 85%, and 80% yields, respectively, thus suggesting that this reaction might not involve free radicals.
Next, some compounds derived from 1,2-diols as potential intermediates were examined in the reaction system (Fig. 7a). In addition to benzoic acid, all possible derivatives gave excellent yield under standard reaction conditions, while different reaction results were given in terms of shortening the reaction time. It was found that when 2-hydroxy-1-phenylethanone (5a), phenylglyoxal monohydrate (5c), mandelic acid (5d), and benzoylformic acid (5e) were employed as the substrates, the reaction was much faster for the latter than for the former. These results suggest a stepwise oxidation of α-hydroxy group through the oxidation of 5a (or the tautomer 5b as well, which is a tautomer of 5a) to 5c (5d), and further to 5e.
When possible intermediates 5a and 5c were subjected to the standard conditions, ketoester (5f) was also obtained in 54% and 39% yield, respectively, and the yield of the 5f decreased gradually, thus implying that the formation of 5f was from the reaction of nucleophilic addition of the aldehyde group of 5c with MeOH. It’s worth noting that the reaction of 5a, 5c, 5e, and 5f under the standard conditions did not give aldehyde (4a).
When possible intermediate 5d was subjected to the standard conditions, 4a was obtained in 24% yield within 4 h. The result promoted us to investigate the reaction evolution of 5d with different reaction times (Fig. 7b). It was found that the quantitative aldehyde was obtained in 0.5 h. No 2a, 5e, and 5f were detected. These results demonstrated that 4a was from 5d. The yield of 2a increased with the extension of the reaction time, while the yield of 4a decreased gradually. These results suggested that the nucleophilic addition of 4a with MeOH formed the hemiacetal and that the hemiacetal was subsequently oxidized to the ester (2a). In addition, formic acid was obtained along with the C–C bond cleavage of 5d, and then the formic acid decomposed to CO234, which was detected by the lime-water-test (Supplementary Fig. 13). When possible intermediate 5e was subjected to the standard conditions, 2a was obtained in 90% yield within 4 h. Such a fast reaction rate leads to a further reduction reaction time, with 56% yield of 2a being achieved in just 0.5 h. These results demonstrated that compound 5e rapidly cleave C–C bonds without passing through intermediate 5f and that 5f was not from 5e but from 5c, which was different from the previous work35.
Then, the transformation of 5f to 2a was verified in Fig. 7c. Only 15 % of 2a was detected when the reaction was performed in n-heptane instead of MeOH. In order to further prove the necessity of alcohol, 5f was subjected to the standard conditions in d4-MeOH. The desired deuterated methyl benzoate was obtained in >99% yield. These results gave us a conclusion that the nucleophilic addition of the keto with MeOH took place in the conversion of 5f to 2a. The 2a was obtained along with the C–C bond cleavage of 5f. The methyl formate was hydrolyzed to MeOH and HCOOH. The resultant HCOOH was decomposed to CO2 and H234.
A kinetic study with time-dependent experiments on the oxidative cleavage of 1a revealed the presence of benzaldehyde (4a) and ketoester (5f) (Supplementary Fig. 14a). The kinetic data did not fit well with the first-order rate equation with respect to diol, while followed the pseudo-second-order-rate equation very well with a rate constant of 0.219 mol L−1 h−1 (Supplementary Fig. 14b). The apparent activation energy of this reaction determined by an Arrhe-nius plot (60–80 °C) was 14.9 kJ mol−1 (Supplementary Fig. 15).
On the basis of the control experiment results and pertinent literature reports, a possible reaction mechanism was proposed (Fig. 8). Firstly, with the assistance of K2CO3, 1- phenylethane-1,2-diol (1a) was oxidized to the 2-hydroxy-1-phenylethanone (5a) (or the tautomer 5b as well) by the active species generated from the activation of oxygen by the Co-based catalyst36,37,38,39,40. Then, there are two possible reaction pathways for this reaction. In pathway a, 5b was oxidized to mandelic acid (5d) and then the C–C bond cleavage occurs to produce benzaldehyde (4a) with release of a CO2. The addition of MeOH to 4a afforded the hemiacetal intermediate 5h. Subsequently, Co-catalyzed aerobic oxidation of the 5h takes place, leading to the formation of ester 2a. In pathway b, compound 5a was oxidized to phenylglyoxal (5c). The addition of MeOH to 5c formed the hemiacetal intermediate, and then hemiacetal intermediate underwent the oxidation to afford ketoester (5f) under standard conditions. The nucleophilic addition of the 5f with MeOH gave the intermediate 5g. Finally, the C–C bond cleavage of the 5g produced the ester 2a, along with the production of CO2. And, in pathway b, there is another alternative. The compound 5c is further oxidized to benzoylformic acid (5e), which rapidly cleaves the C–C bond to form the target product ester 2a with this release of a CO2.
To get more information about the reaction mechanism of the aerobic oxidative cleavage, isotope-labeling experiments were conducted with 18O2 as the sole oxidant. Under our experimental conditions, C18O16O (m/z = 46) was detected as by-products by mass spectrometry (Supplementary Fig. 16); Meanwhile, H2 (m/z = 2) was also detected (Supplementary Fig. 17). The above results proved the oxygen transfer from O2 to CO2, further affirming the existence of the proposed reaction pathways.
In order to obtain more information on the mechanism of the cleavage of internal diols, time-dependent experiments on the oxidation of (S,S)-hydrobenzoin was conducted to study this reaction Kinetic (Supplementary Fig. 14c). At the initial reaction time, the aldehyde was obtained, but the target product ester was not detected. In addition, it has to be noted that benzil was not detected by GC-MS during the whole reaction process, and that when benzil was subjected to the standard reaction conditions, ester was obtained only in 18% yield. These results indicated that this reaction process refused to undergo benzil compound, which is different from some previous reports15. It was very interesting to find that trans isomer, meso-hydrobenzoin was fast cleaved faster than the cis isomer, (S,S)-hydrobenzoin (Supplementary Fig. 14d). The results indicated that this reaction process may be classified as a type II mechanism41. Free radical capture experiments have ruled out free radical process of the reaction (Supplementary Fig. 18). So we can speculate on such a conclusion that this type II mechanism involves the formation of a monodentate complex between diol and active oxidant species, which then oxidatively collapses to the carbonyl product in a two-electron oxidation (Supplementary Fig. 19).
In conclusion, we have developed a single-atom dispersed meso-Co-NC-based heterogeneous catalytic system for the aerobic oxidative C−C bond cleavage of 1,2-diols with O2/air as the oxidants under mild reaction conditions. A series of diols could be efficiently cleaved and converted into the corresponding esters, ketones or aldehydes. Characterization results demonstrated that cobalt species are highly dispersed in the form of Co–Nx. The Co–Nx active site was further confirmed by the KSCN poisoning experiment. Mechanistic insights into the monosubstituted diol cleavage process reveal that two key intermediates introduce two different reaction pathways, and that a sequence reaction involves stepwise oxidation/nucleophilic addition/C–C bond cleavage. The reaction process of internal 1,2-diols followed a type II mechanism via two-electron oxidative fragmentation. Mild reaction conditions, non-noble metal catalyst, and excellent reusability of the catalyst make the present catalytic system much more competitive than the existing systems. This work also provides insights into the application of single atom catalyst (SAC) in C−C bond cleavage.
Synthesis and characterization
Preparation of meso-Co-NC-X catalyst
2.5 g of LUDOX® AS-40 colloidal silica and 1.0 g VB12 were dissolved in 50 mL water for 30 min at room temperature under vigorous stirring. Then, the mixture was dried at 100 °C. The obtained VB12@SiO2 was grinded into powder and pyrolyzed in a flow of ultrapure nitrogen at 800 °C (or 600, 700, 900, and 1000 °C) for 2 h with the heating rate of 5 °C min−1, then cooled naturally to room temperature. The samples were acid leached in HF (40 wt% hydrofluoric) for 24 h continuous agitation at room temperature to remove the silica template. Finally, the etched samples were thoroughly washed with de-ionized water until reaching a neutral pH and dried in vacuum at 100 °C overnight.
Procedures for the aerobic oxidative cleavage of monosubstituted 1,2-diols to esters
In a typical oxidation, 1-phenylethane-1,2-diol (0.25 mmol), meso-Co-NC-800 (5 mol%), K2CO3 (20 mol%) and MeOH (4 mL) were into a round-bottom flask (25 mL) with a magnetic bar. Then the resulting mixture was transferred to an autoclave. After the autoclave was closed, and purged with oxygen three times before it was finally pressurized for 24 h with an oxygen atmosphere, and stirred at 80 °C. After the reaction, the internal standard (biphenyl, 15 mg) and MeOH (1 mL) were added. The mixture analysis were performed on LC, GC and confirmed by GC-MS.
Procedures for the aerobic oxidative cleavage of internal 1,2-diols to esters
In a typical oxidation, (S,S)-hydrobenzoin (0.25 mmol) and meso-Co-NC-800 (5 mol%), K2CO3 (20 mol%) and MeOH (4 mL) were introduced into a round-bottom flask (25 mL) with a magnetic bar. Then the resulting mixture was transferred to an autoclave. After the autoclave was closed, and purged with oxygen three times before it was finally pressurized with an oxygen atmosphere. Subsequently, the tube was stirred at 25 °C for 24 h. After the reaction, the internal standard (biphenyl, 15 mg) and MeOH (1 mL) were added. The mixture were analyzed by LC, GC, and confirmed by GC-MS.
Procedures for the aerobic oxidative oxidation of internal 1,2-diols to aldehydes
In a typical oxidation, (S,S)-hydrobenzoin (0.25 mmol) and meso-Co-NC-800 (5 mol%), K2CO3 (20 mol%) and n-heptane (4 mL) were introduced into a round-bottom flask (25 mL) with a magnetic bar. Then the resulting mixture was transferred to an autoclave. After the autoclave was closed, and purged with oxygen three times before it was finally pressurized with an oxygen atmosphere. Subsequently, the flask was stirred at 50 °C. After the reaction, the internal standard (biphenyl, 15 mg) and n-heptane (1 mL) were added. The mixture were analyzed by LC, GC, and confirmed by GC-MS.
Large-scale and recycling test
1-phenylethane-1,2-diol (7.5 mmol), meso-Co-NC-800 (2.5 mol%), K2CO3 (20 mol%) and MeOH (15 mL) were added into a round-bottom flask (50 mL) with a magnetic bar. Then the resulting mixture was transferred to an autoclave. After the autoclave was closed, and purged with oxygen three times before it was finally pressurized with an oxygen atmosphere. Subsequently, the flask was stirred at 80 °C for 48 h. After completion of the reaction, the liquid mixture was analyzed by LC, GC, and confirmed by GC-MS.
The catalyst was recovered by filtration, washing with MeOH and drying under vacuum to remove the residual solvent, and reused for the next run.
All data that support the findings of this study are available within the paper and its Supplementary Information, or are available from the corresponding author upon reasonable request.
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We gratefully acknowledge financial support from the National Natural Science Foundation of China (No. 21773227, 21403219, and 21773232), and Shandong Province Major Science and Technology Innovation Project (2108CXGC1102).
The authors declare no competing interests.
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Luo, H., Wang, L., Shang, S. et al. Aerobic oxidative cleavage of 1,2-diols catalyzed by atomic-scale cobalt-based heterogeneous catalyst. Commun Chem 2, 17 (2019). https://doi.org/10.1038/s42004-019-0116-5
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