The development of new methods for the direct transformation of methanol into two or multi-carbon compounds via controlled carbon–carbon coupling is a highly attractive but challenging goal. Here, we report the first visible-light-driven dehydrogenative coupling of methanol into ethylene glycol, an important chemical currently produced from petroleum. Ethylene glycol is formed with 90% selectivity and high efficiency, together with hydrogen over a molybdenum disulfide nanofoam-modified cadmium sulfide nanorod catalyst. Mechanistic studies reveal a preferential activation of C−H bond instead of O−H bond in methanol by photoexcited holes on CdS via a concerted proton–electron transfer mechanism, forming a hydroxymethyl radical (⋅CH2OH) that can readily desorb from catalyst surfaces for subsequent coupling. This work not only offers an alternative nonpetroleum route for the synthesis of EG but also presents a unique visible-light-driven catalytic C−H activation with the hydroxyl group in the same molecule keeping intact.
Methanol can be derived from a variety of carbon resources, such as natural gas or shale gas, coal, biomass, and carbon dioxide, and is an abundant and renewable one-carbon (C1) building block1. Many types of chemicals can be produced from methanol, and the carbon–carbon (C–C) bond formation is the most attractive and challenging reaction in methanol chemistry. Current conversions of methanol involving C−C bond formation are restricted to dehydrative oligomerizations such as methanol-to-olefin and methanol-to-gasoline processes, which show limited selectivity to a specific product2, as well as methanol carbonylation3. The importance of methanol chemistry is increasing under the background of growing interest in the utilization of nonpetroleum carbon resources (in particular, shale gas) and carbon dioxide for sustainable production of chemicals. This trend has become a strong incentive to develop new methods or new routes for the transformation of methanol via C−C coupling with high selectivity.
Traditionally, the conversion of methanol usually involves the activation of its O−H or C−O bond. The system that can selectively activate the unreactive C–H bond of methanol with the hydroxyl group intact and form C–C bond is rare4. The preferential activation of inert sp3 α-C–H bond in an alcohol without affecting the hydroxyl group is highly challenging in synthetic chemistry and is of high academic significance5, 6.
Here, we present a visible-light-driven dehydrogenative coupling of methanol into ethylene glycol (EG) (Eq. 1), in which the hydroxyl group keeps intact. EG is an important chemical having a number of applications7. In particular, EG is widely used for the manufacture of polyesters, predominantly poly(ethylene terephthalate) (PET). The annual production of EG is >25 million metric tons and the demand for EG is expected to increase at a rate of 5% per year8. In the current industry, EG is primarily produced from petroleum-derived ethylene via epoxidation to ethylene oxide (EO) and the subsequent hydrolysis of EO. This multistep process suffers from low efficiency due to the low EO yield and high energy consumption7. The dehydrogenative coupling of methanol would offer a fascinating nonpetroleum route for sustainable production of EG.
We report that CdS is a unique catalyst for the conversion of methanol to EG under visible-light irradiation. The modification of CdS nanorods with MoS2 nanofoams further enhances the activity and EG selectivity. An EG selectivity of 90% can be obtained with a yield of 16% and a quantum yield of above 5.0%. We demonstrate that the preferential activation of C–H bond in methanol is driven by photoexcited holes via a concerted proton–electron transfer (CPET) mechanism on CdS surfaces, forming ⋅CH2OH radical as an intermediate for EG formation.
Photocatalysts Efficient for Methanol Coupling to EG
It is noteworthy that Eq. 1 cannot proceed via conventional thermocatalysis because of the thermodynamic limitation (Supplementary Fig. 1). Solar-energy-driven photocatalysis is a promising strategy to realize the C−C coupling under mild conditions9,10,11. However, so far, the photocatalytic C−C coupling has been mainly limited to larger molecules such as 2,5-dihydrofuran10. Basically, a semiconductor with the conduction-band edge higher (more negative) than the H2O/H2 redox potential and the valence-band edge lower (more positive) than the EG/CH3OH redox potential may photocatalyze Eq. 1 (Supplementary Fig. 2). However, over most semiconductors investigated, instead of EG, HCHO was formed as a major carbon-based product (Table 1), suggesting that the O−H bond is easier to be activated. EG was formed on ZnS, but ZnS only worked under ultraviolet (UV) irradiation12 due to its large bandgap energy (3.6 eV, corresponding to λ = 345 nm). We discovered that CdS, a semiconductor with a bandgap energy of 2.4 eV (corresponding to λ = 518 nm), catalyzed the formation of EG with better selectivity under visible light. The catalytic behavior of CdS depended on its morphology (Supplementary Table 1), and CdS nanorods exhibited the best performance for EG formation among CdS samples with different morphologies (Supplementary Fig. 3). HCHO was a major by-product along with EG and H2. We estimated the ratio of photogenerated electrons and holes consumed in product formation by assuming Eqs. 2–4, and the value was close to 1.0 for CdS. This confirms the occurrence of reactions of Eqs. 2–4.
Superior Performances of MoS2-Foam-Modified CdS Nanorods
We loaded some typical co-catalysts13 onto CdS nanorods to enhance the catalytic performance. Although all the co-catalysts investigated accelerated the formation of H2, the formation of HCHO was enhanced more significantly than that of EG, leading to lower EG selectivity in most cases (Supplementary Table 2). It is quite unique that the addition of MoS2 onto the CdS nanorod not only enhances the formation of H2 and EG but also significantly increases the EG selectivity (Table 1). Moreover, we found that MoS2 nanofoam is a better co-catalyst for EG formation than MoS2 nanosheet. The increase in the loading of MoS2 nanofoam from 1.0 to 5.0 wt% gradually increased the rates of H2 and EG formations, but did not significantly change the rate of HCHO formation (Supplementary Table 2). Thus, the EG selectivity increased upon increasing the MoS2 loading amount to 5.0 wt%. A too higher MoS2 loading (7.0 wt%) was unbeneficial to EG formation (Supplementary Table 2). The rates of EG and H2 formations over the 5 wt% MoS2 foam/CdS reached 11 and 12 mmol gcat−1 h−1, respectively, which were about 24 and 16 times higher than those for the CdS nanorod alone. Further, the rate of EG formation for our MoS2 foam/CdS catalyst under visible-light irradiation was about 1 order of magnitude higher than that for ZnS under UV-light irradiation. The EG selectivity was 90% over the MoS2 foam/CdS catalyst (Table 1), which was also significantly higher than that over CdS alone or ZnS.
We performed characterizations to understand the origin of the significant promoting effect of MoS2 nanofoam. The high-resolution transmission electron microscopy (HRTEM) and high-angle annular dark-field scanning TEM (HAADF-STEM) studies revealed that the MoS2 foam located on the CdS rod had more edge sites and more intimate contact with CdS than the MoS2 sheet on CdS (Fig. 1a–1d, Supplementary Figs. 4, 5, and 6). The extended X-ray absorption fine structure (EXAFS) studies clarified that the MoS2 foam on CdS possessed less Mo–Mo coordination than the corresponding MoS2 sheet (Fig. 1e), also suggesting that the catalyst with MoS2 foam had more edge sites. The MoS2 edge sites are believed to be active sites for H2 evolution14, 15. Actually, the MoS2 foam/CdS catalyst also displayed a higher H2 formation rate than CdS and MoS2 sheet/CdS when a hole scavenger (Na2S/Na2SO3 or lactic acid) was used instead of CH3OH (Supplementary Table 3). On the other hand, the intimate contact between the MoS2 foam and CdS rod may accelerate the transfer of photogenerated charge carriers, which is also a key parameter determining the performance. The photoluminescence (PL) intensity of the emission band at ~520 nm due to the recombination of photogenerated electrons and holes decreased in the following sequence: CdS >MoS2 sheet/CdS >MoS2 foam/CdS (Supplementary Fig. 7). The PL average lifetime (ave. τ) derived from the time-resolved PL (TRPL) spectroscopy16 decreased in the same order (Fig. 1f). These results confirm the enhancement in the separation and transfer of photogenerated excitons by the presence of MoS2, in particular, MoS2 foam. The photocurrent density and the cathodic current density of linear sweep voltammetry (LSV) measurements provided further evidence for this (Supplementary Figs. 8 and 9). Therefore, MoS2 accelerates the photocatalytic activity for EG formation by both providing H2-evolution active sites and enhancing the transfer of photogenerated electrons and holes (Fig. 1g).
Furthermore, it should be reminded that the increase in the loading of MoS2 foam from 1.0 to 5.0 wt% increased the EG formation rate but did not significantly change the HCHO formation rate. The average pore size of MoS2 nanofoam derived from N2 physisorption is 26 nm (Supplementary Fig. 10), while the size of ⋅CH2OH is only 0.29 nm. Thus, the ⋅CH2OH radicals can easily diffuse into the mesopores of MoS2 nanofoam. We speculate that the mesoporous structure of MoS2 nanofoam may provide more probability for the coupling of the reaction intermediate to form EG. Our kinetic measurements indicate that the formation of EG is a second-order reaction, whereas the formation of HCHO is a first-order reaction (Supplementary Fig. 11). The enrichment of the intermediate inside the mesopores of MoS2 foam may be a reason for the enhancement in EG selectivity.
We performed deep studies to understand the reaction mechanism for EG formation. The addition of an electron scavenger (nitrobenzene) into the system with either CdS or MoS2 foam/CdS catalyst stopped H2 formation, whereas EG formation ceased and HCHO formation rate decreased drastically after the addition of a hole scavenger (Na2S/Na2SO3) (Supplementary Table 4). These results provide further evidence for the reactions of Eqs. 2–4. The addition of a radical scavenger, 5,5-dimethyl-1-pyrroline-N-oxide (DMPO), also significantly suppressed the formation of EG and HCHO (Supplementary Table 4), suggesting that the formations of EG and HCHO proceed via radical intermediates. In situ electron spin resonance (ESR) spectroscopic studies using DMPO as a spin-trapping agent revealed the generation of the hydroxymethyl radical (⋅CH2OH) and methoxyl radical (CH3O⋅) on CdS and MoS2 foam/CdS catalysts (Supplementary Fig. 12 and Fig. 2a). The ⋅CH2OH radical should be an intermediate by C−H activation for the formation of EG, whereas the CH3O⋅ radical resulting from O−H activation may be responsible for HCHO formation.
What controls the preferential activation of C−H or O−H bond in methanol and the formation of intermediates over different catalysts is of paramount importance in mechanisms. To gain further insight into the reaction intermediate and the bond-activation mode, we performed density functional theory (DFT) calculations for methanol transformations on CdS and TiO2, two semiconductors with different product distributions; the former provided EG as a major product, while the latter predominantly catalyzed the formation of HCHO without EG (Table 1). Generally, the formation of radical intermediates through X−H (X = C or O) cleavage by accepting a hole may proceed via either a stepwise pathway, i.e., proton transfer followed by electron transfer (PT−ET) or a CPET pathway, in which proton/electron transfer takes place in a concerted manner (Fig. 2b, c). On TiO2 surfaces, the OH group of CH3OH has a moderate deprotonation energy due to the strong interaction with the ionic oxide surfaces consistent with previous studies17. It is therefore more likely to take a two-step PT−ET route via CH3O– to CH3O⋅, eventually leading to the formation of HCHO (Fig. 2d, TiO2). Such a route has been demonstrated in several previous studies18,19,20. On the other hand, CH3OH has a negligible adsorption energy (−0.1 eV) on CdS, in contrast to that on TiO2 (−1.4 eV). This indicates that the OH group of CH3OH on CdS is difficult to deprotonate. The direct deprotonation of the C−H bond of methanol is even more difficult. It is often believed that the CPET takes place to avoid high-energy or highly unstable intermediates (Fig. 2c)21, 22. Our DFT studies suggest that the cleavage of the C−H bond in methanol occurs preferentially on CdS surfaces because of the following reasons. First, the formation energy of ⋅CH2OH is about 0.5 eV lower than that of CH3O⋅ (Fig. 2d, CdS). Second, assuming the nearby surface sulfur atom as a proton acceptor, the CPET driven by a hole state for the production of ⋅CH2OH possesses a much smaller reaction barrier (0.8 eV) than that of CH3O⋅ (1.6 eV) (Fig. 2d, CdS). The formed ⋅CH2OH intermediate has a small adsorption energy of −0.2 eV on CdS, and thus can readily desorb from the CdS surface, undertaking a thermodynamically downhill coupling to produce EG. We also found that ZnS, showing 54% EG selectivity, weakly binds ⋅CH2OH with an adsorption energy of −0.5 eV (Supplementary Table 5). Hence, we believe that the weak adsorption of ⋅CH2OH on catalyst surfaces plays a key role in the formation of EG. The strong adsorption of ⋅CH2OH, even if produced, on TiO2 (adsorption energy, −1.3 eV) and CuS (adsorption energy, −1.0 eV) will keep the intermediate on the surfaces, which then undergoes consecutive oxidation to form products such as HCHO (Fig. 2d, TiO2 and Supplementary Table 5).
Process Intensification and Quantum Yield
Considering that EG may undergo consecutive oxidation in the reaction system, we have designed a process-intensified reactor that can perform simultaneous EG separation during the reaction (Fig. 3a, Supplementary Figs. 13 and 14). In this reactor with EG separation, the MoS2 foam/CdS catalyst could be easily recovered and used repeatedly without significant deactivation (Supplementary Fig. 15). As compared with the conventional reaction mode, the process-intensified mode demonstrated a high EG selectivity (90%) during the longtime reaction. On the contrary, EG selectivity decreased significantly with reaction time, and many by-products such as glycoaldehyde, oxalic acid, HCHO, and HCOOH were observed in the conventional reactor (Fig. 3b, Supplementary Table 6). Therefore, EG yield could reach as high as 16% after 100 h in the reactor with EG separation.
We have measured the apparent quantum yields of EG under irradiation with different wavelengths. The quantum yield of EG was above 5.0% at wavelengths not longer than 450 nm for the MoS2 foam/CdS catalyst, and decreased upon increasing the wavelength (Supplementary Fig. 16). The longest wavelength suitable for EG formation (~500 nm) was found to coincide with the absorption edge of the MoS2 foam/CdS catalyst, which was obtained from the diffuse reflectance UV-Vis measurement. This further indicates that the EG formation is indeed driven by light.
The present CdS-based photocatalytic system is quite unique in the preferential activation of the C−H bond in methanol without affecting the O−H group, forming EG via ⋅CH2OH radical intermediate. This is achieved by photoexcited holes via the CPET mechanism on CdS surfaces. The weak adsorption of CH3OH and ⋅CH2OH intermediate on CdS decreases the possibility of O−H bond activation, which is a case on TiO2, and enables the facile desorption of ⋅CH2OH from catalyst surfaces for subsequent C−C coupling. The loading of MoS2 nanofoam with abundant edge sites significantly improves the formation of H2 and the overall activity. The EG selectivity is also enhanced probably because of the enriching effect of mesoporous nanofoam. The high selectivity of EG (90%) can be sustained in the long-term reaction by using a process-intensified reactor with EG-separation capability. The present visible-light-driven methanol transformation not only offers an atom-efficient method for the synthesis of EG under mild conditions, but also opens up a new avenue for preferential C–H bond activation without affecting other functional groups in the same molecule.
Synthesis of CdS Nanorods
CdS nanorods were synthesized by a modified solvothermal method23. Typically, 4.62 g of CdCl2·2.5H2O and 4.62 g of CH4N2S were dissolved in 60 mL of ethylenediamine. Then, the mixture was transferred to a Teflon-lined autoclave and was maintained at 160 °C for >24 h. After cooling down to room temperature, the resulting yellow solid products were collected by centrifugation, and washed with distilled water and ethanol three times. The product was then dried at 60 °C.
Synthesis of MoS2 Nanofoam and Nanosheet
MoS2 nanofoam and nanosheet were synthesized by procedures reported previously15. For the synthesis of nanofoam, 0.4 g of (NH4)6Mo7O24·4H2O and 1.6 g of SiO2 nanospheres (30 wt% SiO2 in EG, Alfa Aesar) were first dispersed in 20 mL of deionized water. After removing the solvent, the obtained powder reacted with 0.8 g of CH4N2S at 400 °C for 4 h. The obtained product was treated in hydrofluoric acid aqueous solution under room temperature, followed by washing with deionized water and drying. For the synthesis of the nanosheet, 0.9 g of (NH4)6Mo7O24·4H2O was dissolved in 20 mL of deionized water and was then reacted with 10 mL of carbon disulfide at 400 °C for 4 h. The final product was obtained by treating in saturated NaOH aqueous solution at 60 °C, followed by washing with deionized water and drying.
Preparation of MoS2 Foam/CdS and MoS2 Sheet/CdS Catalysts
A series of MoS2/CdS nanocomposites were prepared by an ultrasonic method24. For example, for the preparation of the MoS2 foam/CdS catalyst, MoS2 nanofoam (5.0 mg) was first ultrasonically dispersed in N,N-dimethylformamide (DMF,10 mL) in a flask for 3 h at room temperature. Then, CdS nanorods (100 mg) were added to the suspension. The mixture was further subjected to ultrasonic treatment for another 2 h to achieve close contact between MoS2 and CdS. The MoS2/CdS nanocomposite was collected by centrifugation and washed with deionized water and ethanol, followed by drying at 60 °C.
Photocatalytic reactions were carried out in a sealed quartz-tube reactor (volume, 20 mL). The visible (Vis) light source was a 300-W Xe lamp with a UV cutoff filter (420–780 nm). The UV-Vis light (320–780 nm) irradiation without using the UV cutoff filter was also applied to some catalysts. The solid catalyst powder (10 mg) was ultrasonically dispersed in 5.0 mL of mixed solution containing 76 wt% CH3OH and 24 wt% H2O. Then, the reactor was evacuated and filled with high-purity (99.999%) nitrogen. The photocatalytic reaction was carried out at room temperature typically for 12 h. After the reaction, the liquid products were analyzed by high-performance liquid chromatography (HPLC, Shimadzu LC-20A) with refractive index and UV detectors together with a Shodex SUGARSH-1011 column (8 × 300 mm) using a dilute H2SO4 aqueous solution as the mobile phase. H2, CH4, CO, and CO2 were analyzed by an Agilent Micro GC3000 equipped with a molecular sieve 5A column and a high-sensitivity thermal conductivity detector. The relative deviation of detection was 4% for gas chromatography and 3% for liquid chromatography.
We measured the apparent quantum yields by using light at different wavelengths for the photocatalytic conversion of CH3OH to EG over the 5% MoS2 foam/CdS catalyst. The apparent quantum yield (η) for the formation of EG was calculated using the following equation:
where n(EG), NA, I, S, and t represent the molar amount of EG, Avogadro’s constant, light intensity, irradiation area, and reaction time, respectively. E λ can be calculated using hc/λ (λ = 380, 420, 450, 475, 500, 550, or 600 nm).
Photocatalytic reactions with EG-separation mode (Supplementary Fig. 13) were carried out in the reactor shown in Supplementary Fig. 14. The light source was a 300-W Xe lamp with a UV cutoff filter (420–780 nm). The solid catalyst (20 mg) was ultrasonically dispersed in 10 mL of mixed solution containing 76 wt% CH3OH and 24 wt% H2O. Then, the reactor was evacuated and filled with nitrogen. The photocatalytic reaction was performed at room temperature. After the reaction, the liquid and gaseous products were also analyzed by HPLC and Micro GC.
The photocatalysts or photocatalytic systems were characterized by scanning electron microscopy, TEM, high-resolution HAADF-STEM, energy-dispersive X-ray spectroscopy mapping, three-dimensional tomography, steady-state and TRPL spectroscopy, EXAFS spectroscopy, ESR spectroscopy, LSV, N2 physisorption, diffuse reflectance UV-Vis spectroscopy, and photoelectrochemical measurements. The details of these techniques were described in Supplementary Information.
The other experimental and computational methods are displayed in Supplementary Information.
The data that support the findings of this study are available from the corresponding authors upon a reasonable request.
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This work was supported by the National Key Research and Development Program of the Ministry of Science and Technology of China (nos. 2017YFB0602201, 2016YFA0204100, and 2016YFA0200200), and the National Natural Science Foundation of China (nos. 21690082, 91545203, 21373166, and 21503176), the Key Research Program of Frontier Sciences of the Chinese Academy of Sciences (no. QYZDB-SSW-JSC020). We thank staffs at the BL14W1 beamline of the Shanghai Synchrotron Radiation Facilities (SSRF) for assistance with the EXAFS measurements.
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