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Article

Immobilization of Peroxo-Heteropoly Compound and Palladium on Hydroxyapatite for the Epoxidation of Propylene by Molecular Oxygen in Methanol

by
Yanyong Liu
Research Institute of Energy Process, National Institute of Advanced Industrial Science and Technology (AIST), AIST Tsukuba West, 16-1 Onogawa, Tsukuba 305-8569, Japan
Molecules 2023, 28(1), 24; https://doi.org/10.3390/molecules28010024
Submission received: 31 October 2022 / Revised: 2 December 2022 / Accepted: 16 December 2022 / Published: 20 December 2022
(This article belongs to the Special Issue Catalysis by Hybrid Materials)
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Abstract

:
Peroxo-heteropoly compound PO4[W(O)(O2)2] was synthesized on calcium-deficient hydroxyapatite using a reaction of surface [HPO4]2− groups on hydroxyapatite with a Na2[W2O3(O2)4] aqueous solution. The vibration of [HPO4]2− at 875 cm−1 became very weak, and the vibration of the peroxo-oxygen bond [O–O]2− at 845 cm−1 appeared in the FT-IR spectrum of the solid product, indicating that PO4[W(O)(O2)2] was formed on the surface of hydroxyapatite. The formed solid sample was further reacted with PdCl2(PhCN)2 in an acetone solution to fix PdCl2 between the O sites on the hydroxyapatite. Elemental analyses proved that the resultant solid contained 1.2 wt.% Pd, implying that PdCl2 molecules were immobilized on the surface of hydroxyapatite. The hydroxyapatite-based hybrid compound containing Pd and PO4[W(O)(O2)2] was used as a heterogeneous catalyst in a methanol solvent for propylene epoxidation by molecular oxygen in an autoclave batch reaction system. A propylene conversion of 53.4% and a selectivity for propylene oxide of 88.7% were obtained over the solid catalyst after reaction at 363 K for 8 h. The novel catalyst could be reused by a simple centrifugal separation, and the yield of propylene oxide did not decrease after the reaction for five runs. By prolonging the reaction time to 13 h, the highest yield of propylene oxide at 363 K over the solid catalyst was obtained as 53.8%, which was almost the same as that of the homogeneous catalyst containing PdCl2(PhCN)2 and [(C6H13)4N]2{HPO4[W(O)(O2)2]2} for the propylene epoxidation. Methanol was used as a solvent as well as a reducing agent in the propylene epoxidation by molecular oxygen. Small particles of Pd metal were formed on the surface of the hybrid solid catalyst during the reaction, and acted as active species to achieve the catalytic turnover of PO4[W(O)(O2)2] in the propylene epoxidation by molecular oxygen in methanol.

Graphical Abstract

1. Introduction

Propylene oxide (denoted as PO), obtained from the epoxidation of propylene, is an important industrial intermediate to produce polyurethanes, unsaturated resins, and other products. The chlorohydrin process and hydroperoxide process are conventional industrial methods for producing PO from propylene. However, they are not environmentally benign methods due to the formation of a large amount of co-product CaCl2 or t-butyl alcohol. Hydrogen peroxide (H2O2) is an environmentally benign oxidant and exhibits a high selectivity for PO in propylene epoxidation [1]. However, H2O2 is too expensive to achieve an economically viable process. Molecular oxygen (O2) is the best oxidant from views of cost and environment. The catalytic oxidation of propylene by O2 mainly forms acrolein, and the selectivity for PO is very low due to the high activity of allylic C−H bonds of propylene molecules [2,3]. The selectivity for PO, in the propylene oxidation by O2, greatly increased in the presence of a reducing agent, such as H2 [4] and N2O [5]. In an industrial process, it is hard to handle the gaseous reducing agent H2 or N2O in the presence of O2. We developed a homogeneous catalytic system containing Pd and peroxo-heteropoly compound for the propylene epoxidation by O2 in methanol [6]. Methanol was used as a solvent as well as a reducing agent in the reaction. The catalytic system is promising in the industry because methanol is a tractable and reusable liquid-reducing agent [7]. Compared to homogeneous catalysts, heterogeneous catalysts are desirable in the industry because they are easily separated and reused [8,9,10]. We have designed two kinds of heterogeneous catalysts containing Pd and peroxo-heteropoly compound for the propylene epoxidation by O2 in methanol [11,12].
Heteropoly compounds are attractive catalysts for acid-catalytic and oxidation reactions in homogeneous and heterogeneous systems [13,14,15]. Moreover, the bifunctional catalysts, containing heteropoly compounds and noble metals, are effective catalysts for many industrially important reactions [16,17,18,19,20,21,22,23,24]. H3PW12O40 is an excellent catalyst for olefin epoxidation using H2O2 as an oxidant [15]. Peroxo-heteropoly compounds formed in situ from H3PW12O40 and H2O2 are the real active species in the catalytic systems [25]. It is important to effectively utilize peroxo-heteropoly compounds for catalytic oxidation reactions in industrial processes [26,27,28]. The immobilization of peroxo-heteropoly compounds, on solid supports by chemical bonds, has been used to develop heterogeneous catalysts [29,30,31,32,33]. The reaction of surface P−OH groups with peroxo-isopoly compound [W(O)(O2)2]2 to form peroxo-heteropoly compounds is an efficient method to immobilize peroxo-heteropoly compounds on the supports [11,29].
Hydroxyapatite (denoted as HAP) has been used as a kind of useful material in various fields [34]. HAP attracts considerable attention as an effective catalyst and support in organic synthesis [35]. HAP-supported heteropolyacids have been reported as excellent catalysts in the epoxidation of olefin using H2O2 as an oxidant [36,37,38]. Stoichiometric HAP has a formula of Ca10(PO4)6(OH)2, giving a Ca/P molar ratio of 1.67 [34]. Nonstoichiometric HAP is a kind of calcium-deficient HAP with a formula of Ca10−x(HPO4)x(PO4)6−x(OH)2−x, where x ranges from 0 to 2, giving a Ca/P molar ratio ranging from 1.67 to 1.33 [39,40,41,42]. The surface of calcium-deficient HAP contains the groups of HPO4, which can be used for surface modification [43]. On the other hand, PdCl2 can be immobilized on the HAP surface and the PdCl2-immobilized HAP has been used as a highly effective catalyst in alcohol oxidation by O2 [44,45,46,47,48].
This study reported a kind of novel hybrid compound prepared by immobilizing peroxo-heteropoly compound and PdCl2 on the HPA surface at the same time. The hybrid compound showed high catalytic ability and reusability in the epoxidation of propylene by O2 in methanol.

2. Results

2.1. FT-IR Spectra

Figure 1 shows the FT-IR spectra of various samples. HAP showed main peaks at around 1060, 875, 680, and 630 cm−1 in the FT-IR spectrum. These peaks coincided with the FT-IR spectrum of HAP in the literature [49]. The large peak at around 1060 cm−1 and its shoulder peaks were assigned to the vibrations of tetrahedral [PO4]3– groups, and the peak at 875 cm−1 was assigned to the vibrations of [HPO4]2− groups in the calcium-deficient hydroxyapatite HAP [50,51,52]. The FT-IR spectrum of K2[W2O3(O2)4] showed peaks at around 980, 960, 845, 775, and 615 cm−1, coinciding with the literature data [53]. The peak at 845 cm−1 was assigned to the stretching vibration of the peroxy-oxygen bond [O–O]2− [54]. In the FT-IR spectrum of [(C6H13)4N]2{HPO4[W(O)(O2)2]2} (denoted as THA-PW2), the big peak at around 1070 cm−1, and its shoulder peaks, were assigned to the stretching vibration of P−O, and the peak at 930 cm−1 was assigned to the stretching vibration of W=O nearby P−O bonds [53]. Moreover, the peak at 845 cm−1 due to the stretching vibration of [O–O]2− was observed in the FT-IR of THA-PW2. The sample of PO4[W(O)(O2)2]-immobilized HAP (denoted as PW-HAP) exhibited the main peaks of HAP and THA-PW2 in the FT-IR spectrum. However, the vibrations of the HPO4 units at 875 cm−1 almost disappeared, and the vibration of W=O nearby P−O bonds appeared at 930 cm−1 in the IR spectrum of PW-HAP. The stretching vibration of the peroxy-oxygen bond [O–O]2− could be observed in the spectrum in the PW-HAP. The FT-IR spectrum of PdCl2 did not show an obvious peak in the range from 600 to 1400 cm−1. On the contrary, PdCl2(PhCN)2 showed many peaks correlating with the organic PhCN groups in the FT-IR spectrum. The IR spectrum of PdCl2-immobilized PW-HAP (denoted as Pd-PW-HAP) was almost the same as the IR spectrum of PW-HAP. The peaks of PhCN groups could not be observed in the IR spectrum of Pd-PW-HAP.

2.2. Elemental Analyses

Table 1 shows the results of elemental analyses of various HAP-containing samples. HAP contained 34.3 wt.% of Ca, and 19.8 wt.% of P, with a Ca/P molar ratio of 1.34. PW-HAP contained 26.8 wt.% of Ca, 15.6 wt.% of P, and 13.6 wt.% of W by element analyses. This indicated that W was successfully introduced in PW-HAP by stirring HAP powders in the Na2[W2O3(O2)4] aqueous solution. On the other hand, Pd-PW-HAP contained 26.1 wt.% of Ca, 15.2 wt.% of P, 13.2 wt.% of W, and 1.2 wt.% of Pd. This indicated that Pd was fixed on the surface of the Pd-PW-HAP sample. The molar ratio of Ca/P in each sample was almost the same as the designed Ca/P molar ratio (1.33) in the synthesis step.

2.3. Epoxidation of Propylene by O2 in Methanol over Various Catalysts

Figure S1 shows the GC charts of gas and liquid products after reaction at 363 K for 8 h over Pd-PW-HAP.
Table 2 shows the results of propylene epoxidation by O2 in methanol over various catalysts. PW-HAP showed high selectivity for PO of 90.3%, but the C3H6 conversion was low (2.3%) after reaction at 363 K for 8 h. PW groups in PW-HAP contain peroxy-oxygen bonds [O–O]2− which can stoichiometrically epoxidize olefin to olefin oxide [25]. However, the catalytic turnover of peroxy-oxygen bonds in PW-HAP could not be achieved by O2. PdCl2(PhCN)2 showed a very low C3H6 conversion of 2.1%, and a low selectivity for PO of 9.5% for the oxidation of propylene by O2. The solid catalyst Pd-PW-HAP showed a propylene conversion of 53.4% and a selectivity for PO of 88.7%, after reaction at 363 K for 8 h. The by-products were acrolein, propionaldehyde, acetone, propane, and other products (mainly ring-opened compounds of PO). The homogeneous catalyst Pd+PW2 (with 0.24 g [(C6H13)4N]2{HPO4[W(O)(O2)2]2} and 0.02 g PdCl2(PhCN)2) was designed to contain the same amounts of W and Pd as the heterogeneous Pd-PW-HAP catalyst. Pd+PW2 showed a propylene conversion of 57.2% and a selectivity for PO of 88.5% for the reaction. Pd-HMS-PW2 and PdMgAl-PW4 are two kinds of solid catalysts we reported previously for the propylene epoxidation by O2 in methanol [11,12]. As shown in Table 2, Pd-HMS-PW2 showed a propylene conversion of 44.6% and a selectivity for PO of 89.6%, and PdMgAl-PW4 showed a propylene conversion of 48.3% and a selectivity for PO of 87.1% after reaction at 363 K for 8 h. The turnover number (TON) of the catalyst was defined as the number of formed PO molecules per peroxy-oxygen bond [O–O]2− in the catalyst. The number of the peroxy-oxygen bond [O–O]2− was calculated using the catalyst’s W amounts, assuming one W molecule was bonding with two [O–O]2− groups. The simultaneous existence of the peroxo-heteropoly compound and Pd is very important for improving the PO yield in the propylene epoxidation by O2 in methanol. As shown in Table 2, the PO yield and TON over the catalysts containing Pd and the peroxo-heteropoly compound decreased in an order of Pd+PW2 > Pd-PW-HAP > PdMgAl-PW4 > Pd-HMS-PW2 for the propylene epoxidation by O2 in methanol at 363 K. The homogeneous catalyst Pd+PW2 showed a higher PO yield and TON of [O–O]2− than the heterogeneous catalysts. On the other hand, Pd-PW-HAP obtained the highest PO yield and TON of [O–O]2− among various heterogeneous catalysts with the same loadings of Pd and W (1.2 wt.% of Pd and 13.2 wt.% of W).

2.4. Comparison of Catalytic Performance between Pd-PW-HAP and Pd+PW2

Figure 2 shows the effect of reaction time on the propylene epoxidation by O2 in methanol at 363 K over Pd-PW-HAP and Pd+PW2. The homogeneous catalyst Pd+PW2 exhibited a C3H6 conversion higher than that of the heterogeneous catalyst Pd-PW-HAP at the same reaction time. On the other hand, the PO selectivity over Pd+PW2 was higher than that over Pd-PW-HAP from 1 to 7 h, but became lower than that over Pd-PW-HAP when the reaction time was more than 8 h. The increase in by-products from the open-ring and over-oxidation decreased the PO selectivity in a long-time reaction. Pd+PW obtained the highest PO yield after the reaction for 10 h, and then the PO yield decreased with increasing reaction time. On the other hand, the highest PO yield over Pd-PW-HAP was obtained after the reaction for 13 h. The highest PO yield over Pd-PW-HAP (53.8%) was almost the same as that of Pd+PW2 for the propylene epoxidation at 363 K by O2 in methanol.

2.5. Stability of Solid Catalyst Pd-PW-HAP

Figure 3 shows the stability of the solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol. The experiment was carried out using a method reported previously [11]. A portion of 0.5 g fresh Pd-PW-HAP catalyst was used in the first run for catalyzing the propylene epoxidation at 363 K for 8 h. After the reaction, the autoclave reactor was cooled down to room temperature. The used solid catalyst was obtained by centrifugal separation, and was then put into another reactor containing reactants and solvent. The second run was started by heating the reactor containing the used Pd-PW-HAP to 363 K. In the meantime, the liquid after the first run, by eliminating out Pd-PW-HAP, was charged with reaction gases for a further reaction at 363 K for 8 h. As shown in Figure 3, the PO yield over the used Pd-PW-HAP in the second run did not decrease in comparison with that over the fresh catalyst in the first run. On the contrary, the liquid without Pd-PW-HAP did not show a further reaction at 363 K, and the PO yield slightly decreased with reaction time due to the increase in ring-opened products.

2.6. Reusability of Solid Catalyst Pd-PW-HAP

Figure 4 shows the time courses of solid catalyst Pd-PW-HAP in the propylene epoxidation by O2 in methanol for five runs. The used catalyst was obtained through centrifugal separation, and then dried under vacuum at room temperature for 3 h. When the amount of the used catalyst after drying was less than 0.5 g, due to loss in the operation, a small amount of fresh catalyst was added to the used catalyst to keep the catalyst amount at 0.5 g for the next run. The propylene conversion greatly increased, but the selectivity for PO slightly decreased with reaction time in each run. The catalytic activity of Pd-PW-HAP was almost kept in the reaction for five runs.
Table 3 shows the reusability of solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol. The fresh catalyst showed a C3H6 conversion of 53.4% and a selectivity for PO of 88.7% after the reaction at 363 K for 8 h. The used catalysts showed very similar C3H6 conversion and selectivity for PO to the fresh catalyst after reaction at 363 K for 8 h. The PO yield obtained in the fifth run was 47.3%, which was the same as those obtained in the first run.

2.7. XRD Patterns of Various Samples

Figure S2 shows XRD patterns of HAP and Pd-PW-HAP before reaction. In the range from 5 to 70 degrees, the samples showed characteristic reflections of the HAP phase according to the Rigaku PDXL2 database (No 1011242). The strong reflections of HAP and Pd-PW-HAP existed in the range of 25–45 degrees in the XRD patterns [55,56].
Figure 5 shows the XRD patterns of Pd-PW-HAP and Pd+PW2 before and after reaction. The sample of Pd+PW2 before reaction showed the reflections of the peroxo-heteropoly compound in the XRD pattern. For the sample of Pd+PW2 after reaction at 363 K for 8 h, a weak peak at 40.1 degrees corresponding to the reflection of (1 1 1) for Pd0 metal species could be observed in the XRD pattern. The XRD pattern of Pd-PW-HAP, after reaction at 363 K for 8 h, was almost the same as that of Pd-PW-HAP before reaction. Because a peak at 39.9 degrees corresponding to the (3 1 0) reflection of HAP appeared in the XRD pattern, the reflection of Pd (1 1 1) at 40.1 degrees could not be ensured in the XRD pattern of Pd-PW-HAP after reaction, due to overlapping by the (3 1 0) reflection of HAP.

2.8. TEM Images of Pd-PW-HAP before and after Reaction

Figure 6 shows the TEM images of Pd-PW-HAP before reaction and after reaction. For the sample of Pd-PW-HAP before reaction, the metal particles could not be observed in the TEM image. On the hand, for the sample of Pd-PW-HAP after reaction at 363 K for 8 h, the metal particles were observed as small black spots in the TEM image. The diameter of metal particles ranged from 1 to 2 nm in the TEM image of Pd-PW-HAP after reaction, and the size distribution of metal particles was uniform. Moreover, the particle size of Pd metal did not increase after reaction at 363 K for 8 h for five runs.
Table S1 shows the results of elemental analyses of Pd-PW-HAP before reaction by ICP and EDS. Three points on the Pd-PW-HAP particle in the TEM image of Pd-PW-HAP before reaction (Figure 6A) were analyzed using the EDS instrument attached to the electron microscope. The three points by EDS analyses gave a similar composition of each element, indicating that PW and Pd were uniformly distributed on the surface of Pd-PW-HAP before reaction. Because EDS mainly analyzed the solid surface of Pd-PW-HAP, but ICP analyzed the HNO3 aqueous solution of Pd-PW-HAP, the EDS analyses gave lower values of Ca and P and higher values of W and Pd in comparison with the results of ICP analyses.

2.9. EXAFS Functions of Pd-PW-HAP before and after Reaction

Figure 7 shows the EXAFS functions of various samples. The sample of Pd-PW-HAP before reaction showed a Pd–Cl interaction peak at 1.85 Å, coinciding with the Pd–Cl interaction peak in the PdCl2 sample. As for the sample of Pd-PW-HAP after reaction at 363 K for 8 h, the Pd–Cl interaction peak disappeared and an interaction peak at 2.3 Å was observed in the EXAFS function. In comparison with the EXAFS function of Pd foil, the interaction peak at 2.3 Å was assigned to the interaction of the Pd–Pd bond in the Pd metal. The PdCl2 molecules immobilized on the Pd-PW-HAP were reduced to the Pd0 metal species during the reaction.

2.10. XPS Spectra of Pd-PW-HAP before and after Reaction

Figure 8 shows the XPS spectra of Pd-PW-HAP before and after reaction. The binding energy of the Pd(3d5/2) peak was 338.2 eV in the XPS spectrum of Pd-PW-HAP before reaction, indicating that the Pd species remained in the oxidation state of +2 in the sample. On the other hand, the sample of Pd-PW-HAP after reaction showed the binding energy of the metallic Pd0 species with 3d5/2 of 334.9 eV and 3d3/2 of 340.2 eV in the XPS spectrum. These results proved that all Pd2+ species in the sample of Pd-PW-HAP before reaction were reduced into the metallic Pd0 species during the epoxidation of propylene by O2 in methanol at 363 K for 8 h.

2.11. Solvent Effect in the Epoxidation of Propylene by O2 over Pd-PW-HAP

Table 4 shows the results of catalytic propylene epoxidation by O2 over Pd-PW-HAP in various solvents. Pd-PW-HAP obtained a propylene conversion of 53.4%, and a selectivity for PO of 88.7% after reaction at 363 K for 8 h in the methanol solvent. On the other hand, in the chloroform solvent, Pd-PW-HAP showed a low propylene conversion of 2.2% although the selectivity for PO was high (91.5%) after reaction at 363 K for 8 h. Hence, the peroxo-heteropoly compound in Pd-PW-HAP stoichiometrically epoxidizes propylene to PO using the peroxy-oxygen bonds, but the catalyst turnover could not be achieved in the chloroform solvent. Methanol is a necessary solvent for the epoxidation of propylene by O2 over Pd-PW-HAP.

2.12. Co-Products from Methanol in the Epoxidation of Propylene by O2

Table 5 shows the consumed amounts, and formed amounts, in the propylene epoxidation in methanol over various catalysts at 363 K for 8 h. PW-HAP consumed a small number of C3H6 (0.7 mmol) and selectively converted them to PO (0.6 mmol). The methanol medium was not consumed over PW-HAP during the reaction. These results indicated that PW-HAP stoichiometrically converted C3H6 to PO using the peroxy-oxygen bonds in PW, but the peroxy-oxygen bonds were not recovered to achieve a catalytic turnover. On the other hand, Pd-PW-HAP consumed 18.8 mmol of C3H6 to form 17.0 mmol of PO after reaction at 363 K for 8 h. Hence, Pd is a necessary component in the catalysts containing peroxo-heteropoly compounds for the epoxidation of propylene by O2 in methanol. As shown in Table 5, an amount of 10.1 mmol of methanol was consumed to form co-products (mainly CO and CO2) over Pd-PW-HAP after reaction at 363 K for 8 h. O2 was consumed for both oxidizing propylene and oxidizing methanol during the reaction. The consumed methanol was almost converted to the co-products involving CO, CO2, and small amounts of HCHO and HCH(OH)2.

3. Discussion

3.1. Synthesis Route of Pd-PW-HAP

Figure 9 shows the route in the synthesis of the hybrid compound Pd-PW-HAP.
The first step in the synthesis route is grafting peroxotungstic ions on the HAP surface to form PW-HAP by using the reaction of surface HPO42− groups. Calcium-deficient HAP has a structure of stoichiometric HAP (Ca/P = 1.67), but involves Ca and OH defects and HPO42− groups [44,45,46,47]. The surface HPO42− groups have activity for some chemical reactions, and thus have been used for surface modification to graft other groups [38]. On the other hand, the HPO42− groups on the solid surface have a reaction activity with peroxotungstic ions to form peroxo-heteropoly ions in an aqueous solution [11,27,28]. As shown in the FT-IR spectra (Figure 1), HAP showed the vibrations of HPO4 groups at 875 cm−1, which proved the existence of the HPO4 group in the calcium-deficient HAP. Moreover, the vibrations at 875 cm−1 became weak and the vibrations of the peroxo-bond O–O at 845 cm−1 appeared in the FT-IR spectrum of PW-HAP. This indicated the number of HPO4 groups on HAP greatly decreased by reacting with [W2O3(O2)4]. In comparison with the IR spectra of PW-HAP and K2[W2O3(O2)4], the vibration of W=O nearby P−O bonds at 940 cm−1 appeared in the IR spectra of PW2-HAP. This implied that the HPO4 groups reacted with [W2O3(O2)4] ions to form peroxo-heteropoly compounds on the PW-HAP.
The second step in the synthesis route is fixing PdCl2 molecules between the O atoms of PO43– groups on the HAP surface. It has been reported that PdCl2 molecules can be fixed on the HAP surface, and the resultant compounds are excellent catalysts for alcohol oxidation by O2 [44,47,48]. As shown in the FT-IR spectra (Figure 1), the peaks of PhCN groups disappeared in the FT-IR spectrum of Pd-PW-HAP, indicating that the organic PhCN groups dropped out from Pd-PW-HAP during the synthesis process. Because the IR spectrum of Pd-PW-HAP was almost the same as that of PW-HAP, the peroxo-heteropoly compound PW remained on the surface of HAP during the PdCl2 immobilization. Using the two steps of surface modification, both peroxo-heteropoly compounds and PdCl2 molecules were immobilized on the HAP surface in Pd-PW-HAP simultaneously.
The molecular formulas of the samples in Table 1 can be obtained using the elemental compositions and the general formulas. At first, the total molecular weight of each compound was calculated using the content of Ca from elemental analysis, and the chemical stoichiometry of Ca in the general formula. Then, the chemical stoichiometries of various groups were calculated using their proportions in the sample, total molecular weight, and the general formula. The deficiency between the summed percentages of various elements and 100% was calculated as adsorbed water. By calculation using the method described above, the formulas of HPA, PW-HAP, and Pd-PW-HAP were Ca4(HPO4)(PO4)2·1.1H2O, Ca4(HPO4)0.56{HPO4[W(O)(O2)]0.44}(PO4)2·1.9H2O, and Ca4(HPO4)0.56{HPO4[W(O)(O2)2}0.44(PO4)2(PdCl2)0.07·2.1H2O, respectively. It can be supposed that the HPO4 groups on the HAP surface almost converted to the PW groups in PW-HAP because a large excessive amount of Na2[W2O3(O2)4] was used in the synthesis step by reacting HAP with Na2[W2O3(O2)4]. However, the HPO4 groups in the inner structure of HAP remained in the PW-HAP. On the other hand, the actual Pd amount in Pd-PW-HAP (as shown in Table 1) was 1.2 wt.%, which was lower than the designed Pd amount in Pd-PW-HAP (2 wt.%) in the synthesis step. This implied that a suitable distance and angle between two PO4 groups were needed to fix PdCl2 molecules on the HAP surface.

3.2. Strong Points of Pd-PW-HAP

As shown in the XRD pattern Pd-PW-HAP before reaction (in Figure 5), the reflections of palladium and peroxo-heteropoly compounds did not appear. The crystals of PW and PdCl2 did not form on the Pd-PW-HAP, implying that PW and PdCl2 were uniformly immobilized on the surface of HAP. Because palladium and peroxo-heteropoly compounds were fixed on the surface of HAP by chemical bonds, the active components (PW and Pd) did not leach from Pd-PW-HAP in the solvent during the reaction (results in Figure 3). Not only the Pd2+ complex could be fixed on the surface of HAP [44], but also the Pd0 nanocluster formed from the reduction of Pd2+ during the reaction had a strong interaction with the surface of HAP [48]. This is the reason why Pd-PW-HAP could be used for five runs without a decrease in the catalytic activity (as shown in Table 3). Because the homogeneous catalyst Pd+PW2 easily diffuses in the methanol solvent, Pd+PW2 showed a higher C3H6 conversion than that of Pd-PW-HAP (as shown in Table 2). However, the only possible method for recovering the homogeneous catalysts was vacuum distillation of the mixture after the reaction. The vacuum distillation consumed a larger amount of energy compared with the centrifugal separation. On the contrary, the solid catalyst Pd-PW-HAP can be reused by simple centrifugal separation in the propylene epoxidation by O2 in methanol. Hence, Pd-PW-HAP is desirable in industry manufacture because of its ease of separation and renewability. As shown in Figure 2, there was only a small difference in the PO yield between Pd-PW-HAP and Pd+PW2 because PW and PdCl2 were uniformly distributed on the HAP surface. Moreover, the highest PO yield over Pd-PW-HAP, obtained by increasing reaction time, was equal to the highest PO yield over Pd+PW2 for the reaction at 363 K (as shown in Figure 2b). HAP-immobilized Pd is a kind of highly efficient catalyst for oxidation reactions using O2 as an oxidant [44,47,48]. This is the reason that Pd-PW-HAP showed a catalytic activity higher than those of PdMgAl-PW4 and Pd-HMS-PW2 for the propylene epoxidation by O2 in methanol (as shown in Table 2).

3.3. Active Pd Species in Pd-PW-HAP

As shown in the XRD pattern of Pd+PW2 after reaction (Figure 5), the peak at 40.1 degrees, corresponding to Pd0 species, could be observed. The metal Pd0 species was the active species in the propylene epoxidation by O2 in methanol over the homogenous catalyst Pd+PW2 [7]. On the other hand, the peak of Pd0 species at 40.1 degrees could not be confirmed in the XRD pattern of Pd-PW-HAP after reaction (as shown in Figure 4). It is necessary to confirm the active Pd species in the propylene epoxidation by O2 in methanol over the heterogeneous catalyst Pd-PW-HAP. The EXAFS function confirmed that the PdCl2 species were converted to Pd0 metal species after the reaction (as shown in Figure 7). Furthermore, the Pd metal particles were observed in the TEM image of Pd-PW-HAP after the reaction (as shown in Figure 6). The size of Pd0 metal particles ranged from 1–2 nm in the TEM image of Pd-PW-HAP after the reaction. The metal particle with a size lower than 3 nm hardly exhibited their reflections in the XRD pattern [57]. Hence, the reflections of Pd0 metal did not appear in the XRD pattern of Pd-PW-HAP after reaction because the size of the formed Pd0 metal particles was too small. The small Pd0 particles were formed after reaction because the precursor PdCl2 molecules were uniformly fixed on the surface of Pd-PW-HAP before reaction. As a result, Pd0 metal was the species for the propylene epoxidation by O2 in methanol over the solid catalyst Pd-PW-HAP.

3.4. Roles of Methanol in the Reaction

Scheme 1 shows the co-oxidation of methanol in the system containing Pd and O2. HAP-immobilized palladium is a kind of highly efficient catalyst for the oxidation of alcohols by O2 [44,45,46,47,48]. Methanol has the highest reducibility among various alcohols, and thus can be oxidized to a peroxy intermediate HOCH2OOH by O2 in the presence of a Pd catalyst [58,59]. The aliphatic organic peroxide HOCH2OOH can achieve the catalytic turnover of the peroxo-heteropoly compound in propylene epoxidation [15,25]. Some HOCH2OOH molecules turn back to HCH(OH)2 for the next catalytic cycle after giving their peroxo-bonds to heteropoly compounds. On the other hand, some HOCH2OOH molecules decompose to COx and H2O in the catalytic system because HOCH2OOH is not stable [60]. Hence, methanol was not only a solvent but also a co-reactant or reducing agent in the propylene epoxidation by O2 in methanol, over Pd-PW-HAP. Because the reaction temperature was low (mainly at 363 K) in this study, only a small amount of methanol underwent co-oxidation by O2 during the reaction.

3.5. Reaction Mechanism for the Reaction

Scheme 2 shows the reaction mechanism for propylene epoxidation by O2 in methanol. The peroxo-heteropoly compounds in PW-HAP stoichiometrically epoxidize propylene to PO by O–O peroxo-bonds in methanol, but the O–O peroxo-bonds cannot be recovered by O2 (results in Table 2). Moreover, the O–O peroxo-bonds in the peroxo-heteropoly compounds on Pd-PW-HAP cannot be recovered in a chloroform solvent (results in Table 4). Hence, Pd on HAP oxidizes CH3OH to the peroxy intermediate HOCH2OOH by O2, and the formed HOCH2OOH acts to recover the O–O peroxo-bonds of peroxo-heteropoly compounds. Pd and methanol convert the weak oxidant O2 to the strong oxidant HOCH2OOH in situ during the reaction. As shown in Table 2, PdCl2(PhCN)2 showed a very low PO yield (0.2%) for the propylene epoxidation in methanol. This indicates that the concentration of HOCH2OOH formed in the system was low, and could not directly result in epoxidation of propylene to PO. The peroxo-heteropoly compounds are necessary for the catalytic system to convert propylene to PO using their peroxy-oxygen bonds. As a result, peroxo-heteropoly compounds achieve the catalytic conversion of propylene to PO, and Pd achieves the catalytic conversion of methanol and O2 to peroxy intermediate HOCH2OOH, which are used for recovering peroxo-heteropoly compounds in situ.
Although the aliphatic organic peroxide HOCH2OOH formed in situ was used as an oxidant for propylene epoxidation, the catalytic system in propylene epoxidation by O2 in methanol, over Pd-PW-HAP, is different from the conventional hydroperoxide process. In comparison with the t-butyl alcohol co-product formed in the conventional hydroperoxide process, the co-product COx can be used to synthesize methanol in the industrial process over Cu-based catalysts, which achieves the recycling of methanol solvent in the catalytic system. Pd-PW-HAP is a kind of heterogeneous catalyst that can be reused by simple centrifugal separation after the reaction. Because Pd-PW-HAP fixed Pd and PW on the HAP surface by chemical bonds, Pd-PW-HAP did not leach the active components to the solvent during the reaction.

4. Materials and Methods

4.1. Reagents

Inorganic reagents were purchased from Wako Pure Chemical Industries Ltd. (Tokyo, Japan) with purities higher than 99%. Organic reagents were purchased from Tokyo Chemical Industry Co., Ltd. (Tokyo, Japan) with purities higher than 99.5%. Gas cylinders were purchased from Sumitomo Seika Chemicals Co., Ltd. (Tokyo, Japan) with purities higher than 99.995%.

4.2. Catalyst Preparation

According to the literature, calcium-deficient HAP was prepared using a wet method [41]. A 1.0 M Ca(NO3)2 aqueous solution and a 0.6 M (NH4)2HPO4 aqueous solution were simultaneously added to 500 mL distilled water in a three-necked flask while stirring. The pH was kept at around 11 during the process by adding an ammonia solution. The resultant milky solution was further stirred at 353 K for 1 h. Then, the precipitate was filtered and washed with distilled water. The resulting solid was dried at 383 K for 24 h and calcined at 773 K for 3 h. The designed Ca/P molar ratio was 1.33.
Na2[W2O3(O2)4] aqueous solution was prepared by dissolving solid Na2WO4 in 30% H2O2 [53]. A portion of 15 g Na2WO4 powder was gradually added to 60 mL of 30% H2O2 at 323 K while stirring to form a clear solution. The solution was stored in a refrigerator at 278 K.
K2[W2O3(O2)4] was obtained by adding an excessive amount of KCl to an aqueous solution of Na2[W2O3(O2)4] to form a K2[W2O3(O2)4] precipitate [54]. The precipitate was filtered, dried in the air at room temperature, and stored in a refrigerator at 278 K.
PW-HAP was prepared using a surface reaction, according to the method in the literature [11,29]. Two grams of HAP powder were added to 20 mL of Na2[W2O3(O2)4] solution with vigorous stirring at room temperature for 6 h. Then, the solid was isolated by filtration, dried in the air at room temperature, and stored in a refrigerator at 278 K.
Pd-PW-HAP was synthesized by fixing PdCl2 molecules on PW-HAP, according to the method in the literature [44]. Two grams of PW-HAP were stirred in a 150 mL acetone solution of PdCl2(PhCN)2 (2.5×10−3 M) at room temperature for 3 h. The solid product Pd-PW-HAP was isolated by filtration, dried in the air at room temperature, and stored in a refrigerator at 278 K. The designed Pd loading was 2 wt.%.
THA-PW2, with a molecular formula of [(C6H13)4N]2{HPO4[W(O)(O2)2]2}, was prepared according to the method in the literature [54]. A portion of 2.5 g H2WO4 was added to 7 mL 30% H2O2. After stirring at 323 K for 40 min, 0.85 mL of 6 M H3PO4 was added to the supernatant. After further stirring for 5 min, 7.8 g of tetrahexylammonium chloride dissolved in 10 mL of water was added to the clear solution. Further stirring was carried out at room temperature for 10 min. Then, the solid product was filtered, dried in the air at room temperature, and stored in a refrigerator at 278 K.
Pd-HMS-PW2, a mesoporous silica containing peroxo-heteropoly compound and Pd, was prepared according to the literature [11]. The peroxo-heteropoly compound {HPO4[W(O)(O2)2]2} was synthesized on the surface of HMS by reacting HMS-PrNH(PO3H2) with H2[W2O3(O2)4] aqueous solution, and then palladium ions were exchanged into the channels of mesoporous silica HMS.
PdMgAl-PW4 was prepared by treating PdMgAl-[PW11O39] with 30% H2O2 according to the literature [12]. PdMgAl-[PW11O39] was synthesized using an ion exchange method to introduce heteropoly anion [PW11O39]7− in the interlayer zone of Pd-containing MgAl-type hydrotalcite. The molar ratio of Mg/Al was three in the hydrotalcite.

4.3. Catalyst Characterization

The elemental analyses were measured by a method of inductively coupled plasma (ICP) using a Thermo Jarrel Ash IRIS/AP instrument. The samples for the ICP analyses were obtained by dissolving HAP-based samples in the HNO3 aqueous solution.
The X-ray diffraction (XRD) patterns were measured by a RINT-2500HLR diffractometer (Rigaku Corp.) with Cu Kα radiation (λ = 0.154 nm). The operation voltage was 40 kV, and the operation current was 50 mA in the XRD analyses.
Fourier transform infrared (FT-IR) spectra were carried out using a KBr pellet method by a JASCO FT/IR-7000 spectrometer. The KBr pellet, containing 0.5 wt.% of each sample, was measured at room temperature under atmospheric conditions.
Transmission electron microscopy (TEM) images were taken using a JEOL JEM 2010FX electron microscope equipped with a Hitachi/Keves H-8100/Delta IV EDS at 200 kV. The samples were supported on carbon-coated copper grids before the TEM measurement.
X-ray absorption fine structure (XAFS) of Pd K-edges was measured at the beamline 10B of the Photon Factory in the National Laboratory for High-Energy Physics, Tsukuba, Japan. Extended X-ray Absorption Fine Structure (EXAFS) data were examined using the Rigaku EXAFS analysis program. Fourier transformation of k3-weighted normalized EXAFS data was carried out in the range of 3.5 Å < k/Å−1 < 11 Å.
X-ray photoelectron spectra (XPS) were carried out using a Phi-5500 ESCA spectrometer equipped with Mg Kα radiation (1253.6 eV). The chamber pressure was 10−9 Torr. The binding energy of Pd was calibrated by the C1s of 284.6 eV.

4.4. Reaction Procedure and Analyses

The reaction was performed in a 100 mL stainless steel autoclave reactor. In a typical reaction, 0.5 g Pd-PW-Hap and 20 mL methanol were added to the autoclave. A nitrogen gas with a pressure of 0.4 MPa was charged in the autoclave, and then charged out from the autoclave to change the air. After purging with nitrogen five times, the autoclave contained 0.1 MPa of nitrogen at room temperature. Then, 1.0 MPa of propylene and 1.0 MPa of oxygen were sequentially charged in the autoclave at room temperature. Then, the autoclave was immersed in an oil bath with temperature control. The reaction started with vigorous stirring (500 revolutions per minute) after the autoclave reactor was heated to the reaction temperature.
After the reaction, the autoclave was cooled down to room temperature. The gas in the autoclave was collected in a plastic gas bag. Then, a certain amount of 1,4-dioxane was added to the autoclave as an internal standard [61]. Inorganic gases (CO2, CO, O2, and N2) were analyzed by a Shimadzu 2014 TCD-GC equipped with a Shincarbon-ST packed column in He carrier gas. Organic gaseous compounds were analyzed by a Shimadzu 2014 FID-GC equipped with an RT-QPLOT capillary column. The factors of various gaseous compounds were obtained using a standard mixed gas (with a known concentration for each component) from a cylinder. On the other hand, the liquid and the solid were separated using a centrifuge. The liquid compounds were analyzed by an Agilent 6890 N FID-GC equipped with a PoraPLOT U capillary column.
The propylene conversion was calculated from the difference in its molar amounts before and after reactions using Equation (1):
XC3H6 = (MC3H6, before − MC3H6, after)/MC3H6, before × 100
The selectivity for each product was expressed in terms of carbon efficiency and was calculated using Equation (2):
S = ni Ci/Σ(ni Ci) × 100
Herein, ni denotes the number of carbon atoms in each product.

5. Conclusions

The novel hybrid compound Pd-PW-HAP was synthesized by immobilizing PdCl2 molecules and peroxo-heteropoly compounds on the surface of calcium-deficient hydroxyapatite. Pd-PW-HAP was an effective heterogeneous catalyst for propylene epoxidation by O2 in methanol. The propylene conversion over Pd-PW-HAP was slightly lower than that over the homogeneous catalyst in the epoxidation of propylene by O2 in methanol. By increasing the reaction time, Pd-PW-HAP could obtain the highest PO yield, comparable to that of the homogeneous catalyst at 363 K. Pd-PW-HAP could be used five times, without a decrease in the catalytic performance in the epoxidation of propylene. During the reaction, the immobilized PdCl2 formed small particles of Pd0 metal species on the Pd-PW-HAP surface by the reduction of methanol. During the reaction, a small part of the methanol solvent was oxidized to the peroxy intermediates HOCH2OOH by O2 in the presence of Pd. The peroxy intermediates recovered the peroxy-oxygen bonds, and achieved the catalytic turnover of peroxo-heteropoly compounds for the epoxidation of propylene.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules28010024/s1, Table S1: Results of elemental analyses of Pd-PW-HAP before reaction by ICP and EDS; Figure S1: GC charts of products after reaction at 363 K for 8 h over Pd-PW-HAP; Figure S2: XRD patterns of HAP and Pd-PW-HAP before reaction.

Funding

This research received no external funding.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Acknowledgments

The author appreciates Kazuhisa Murata, and Megumu Inaba at the National Institute of Advanced Industrial Science and Technology (AIST, Japan) for their cooperation and discussion.

Conflicts of Interest

The authors declare no conflict of interest.

Sample Availability

Samples of the HAP-based catalysts are available from the author.

References

  1. Clerici, M.G.; Bellussi, C.; Romano, U. Synthesis of propylene oxide from propylene and hydrogen peroxide catalyzed by titanium silicalite. J. Catal. 1991, 129, 159–167. [Google Scholar] [CrossRef]
  2. Liu, Y.; Murata, M.; Inaba, M.; Mimura, N. Selective oxidation of propylene to propylene oxide by molecular oxygen over Ti-Al-HMS catalysts. Catal. Lett. 2003, 89, 49–53. [Google Scholar] [CrossRef]
  3. Liu, Y.; Murata, M.; Inaba, M.; Mimura, N. Syntheses of Ti- and Al-containing hexagonal mesoporous silicas for gas-phase epoxidation of propylene by molecular oxygen. Appl. Catal. A Gen. 2006, 309, 91–105. [Google Scholar] [CrossRef]
  4. Qi, C.; Okumura, M.; Akita, T.; Haruta, M. Vapor-phase epoxidation of propylene using H2/O2 mixture over gold catalysts supported on non-porous and mesoporous titania-silica: Effect of preparation conditions and pretreatments before reaction. Appl. Catal. A Gen. 2004, 263, 19–26. [Google Scholar] [CrossRef]
  5. Wang, X.; Zhang, Q.; Guo, Q.; Luo, Y.; Yang, L.; Wang, Y. Iron-catalysed propylene epoxidation by nitrous oxide: Dramatic shift of allylic oxidation to epoxidation by the modification with alkali metal salts. Chem. Commun. 2004, 1396–1397. [Google Scholar] [CrossRef] [PubMed]
  6. Liu, Y.; Murata, K.; Inaba, M. Direct epoxidation of propylene by molecular oxygen over catalyst system containing palladium and peroxo-heteropoly compound in methanol. Chem. Commun. 2004, 582–583. [Google Scholar] [CrossRef] [PubMed]
  7. Liu, Y.; Murata, K.; Inaba, M.; Mimura, N. Direct epoxidation of propylene by molecular oxygen over Pd(OAc)2-[(C6H13)4N]3{PO4[W(O)(O2)2]4}-CH3OH catalytic system. Appl. Catal. B Environ. 2005, 58, 51–59. [Google Scholar] [CrossRef]
  8. Zheng, Z.; Wu, Q.; Zhong, S. HPW/PAM catalyst for oxidative desulfurization-synthesis, characterization and mechanism study. Processes 2022, 10, 402. [Google Scholar] [CrossRef]
  9. Sedghi, R.; Heidari, B.; Shahmohamadi, H.; Zarshenas, P.; Varma, R.S. Pd nanocatalyst adorned on magnetic Chitosan@N-Heterocyclic carbene: Eco-compatible Suzuki cross-coupling reaction. Molecules 2019, 24, 3048. [Google Scholar] [CrossRef] [Green Version]
  10. Kuniyil, M.; Kumar, J.V.S.; Adil, S.F.; Shaik, M.R.; Khan, M.; Assal, M.E.; Siddiqui, M.R.H.; Al-Warthan, A. One-pot synthesized Pd@N-doped graphene: An efficient catalyst for Suzuki–Miyaura couplings. Catalysts 2019, 9, 469. [Google Scholar] [CrossRef]
  11. Liu, Y.; Murata, K.; Inaba, M. Epoxidation of propylene with molecular oxygen in methanol over a peroxo-heteropoly compound immobilized on palladium exchanged HMS. Green Chem. 2004, 6, 510–515. [Google Scholar] [CrossRef]
  12. Liu, Y.; Murata, K.; Hanaoka, T.; Inaba, M.; Sakanishi, K. Syntheses of new peroxopolyoxometalates intercalated layered double hydroxides for propene epoxidation by molecular oxygen in methanol. J. Catal. 2007, 248, 277–287. [Google Scholar] [CrossRef]
  13. Okuhara, T.; Mizuno, N.; Misono, M. Catalytic chemistry of heteropoly compounds. Adv. Catal. 1996, 41, 113–252. [Google Scholar]
  14. Misono, M. Unique acid catalysis of heteropoly compounds (heteropolyoxometalates) in the solid state. Chem. Commun. 2001, 13, 1141–1152. [Google Scholar] [CrossRef]
  15. Mizuno, N.; Yamaguchi, K.; Kamata, K. Epoxidation of olefins with hydrogen peroxide catalyzed by polyoxometalates. Coord. Chem. Rev. 2005, 249, 1944–1956. [Google Scholar] [CrossRef]
  16. Liu, Y.; Misono, M. Hydroisomerization of n-butane over platinum-promoted cesium hydrogen salt of 12-tungstophosphoric acid. Materials 2009, 2, 2319–2336. [Google Scholar] [CrossRef]
  17. Liu, Y.; Koyano, G.; Misono, M. Hydroisomerization of n-hexane and n-heptane over platinum promoted Cs2.5H0.5PW12O40 (Cs2.5) studied in comparison with several other solid acids. Top. Catal. 2000, 11, 239–246. [Google Scholar] [CrossRef]
  18. Liu, Y.; Na, K.; Misono, M. Skeletal isomerization of n-pentane over Pt-promoted cesium hydrogen salts of 12-tungstophosphoric acid. J. Mol. Catal. A Chem. 1999, 141, 145–153. [Google Scholar] [CrossRef]
  19. Liu, Y.; Koyano, G.; Na, K.; Misono, M. Isomerization of n-pentane and n-hexane over cesium hydrogen salt of 12-tungstophosphoric acid promoted by platinum. Appl. Catal. A Gen. 1998, 166, L263–L265. [Google Scholar] [CrossRef]
  20. Liu, Y.; Murata, K.; Inaba, M. Direct oxidation of benzene to phenol by molecular oxygen over catalytic systems containing Pd(OAc)2 and heteropolyacid immobilized on HMS or PIM. J. Mol. Catal. A Chem. 2006, 256, 247–255. [Google Scholar] [CrossRef]
  21. Liu, Y.; Murata, K.; Inaba, M. Liquid-phase oxidation of benzene to phenol by molecular oxygen over transition metal substituted polyoxometalate compounds. Catal. Commun. 2005, 6, 679–683. [Google Scholar] [CrossRef]
  22. Liu, Y.; Murata, K.; Inaba, M.; Mimura, N. Selective oxidation of propylene to acetone by molecular oxygen over Mx/2H5-x[PMo10V2O40]/HMS (M = Cu2+, Co2+, Ni2+). Catal. Commun. 2003, 4, 281–285. [Google Scholar] [CrossRef]
  23. Liu, Y.; Murata, K.; Inaba, M. Heterogeneous carbonylation of dimethyl ether to methyl acetate over bifunctional catalysts containing Rh and heteropoly acids. React. Kinet. Mech. Catal. 2016, 117, 223–238. [Google Scholar] [CrossRef]
  24. Liu, Y.; Murata, K.; Inaba, M.; Nakajima, H.; Koya, M.; Tomokuni, K. Catalytic oxidation of cyclohexene by molecular oxygen over isopolyoxometalates. Chem. Lett. 2004, 33, 200–201. [Google Scholar] [CrossRef]
  25. Venturello, C.; D’Aloisio, R.; Bart, J.C.; Ricci, M. A new peroxotungsten heteropoly anion with special oxidizing properties: Synthesis and structure of tetrahexylammonium tetra(diperoxotungsto)phosphate(3–). J. Mol. Catal. 1985, 32, 107–110. [Google Scholar] [CrossRef]
  26. Gao, Y.; Juliao, D.; Silva, D.F.; Castro, B.; Zhao, J.; Balula, S.S. A simple desulfurization process to achieve high efficiency, sustainability and cost-effectivity via peroxotungstate catalyst. Mol. Catal. 2021, 505, 111515. [Google Scholar] [CrossRef]
  27. Kruse, J.H.; Langer, M.; Romanenko, I.; Trentin, I.; Hernández-Castillo, D.; González, L.; Schacher, F.H.; Streb, C. Polyoxometalate-soft matter composite materials: Design strategies, applications, and future directions. Adv. Funct. Mater. 2022, 2208428. [Google Scholar] [CrossRef]
  28. Buru, C.T.; Farha, O.K. Strategies for incorporating catalytically active polyoxometalates in metal−organic frameworks for organic transformations. ACS Appl. Mater. Interfaces 2020, 12, 5345–5360. [Google Scholar] [CrossRef]
  29. Gelbard, G.; Gauducheau, T.; Vidal, E.; Parvulescu, V.I.; Crosman, A.; Pop, V.M. Epoxidation with peroxotungstic acid immobilized onto silica-grafted phosphoramides. J. Mol. Catal. A Chem. 2002, 182–183, 257–266. [Google Scholar] [CrossRef]
  30. Gelbard, G.; Raison, F.; Roditi-Lachter, E.; Thouvenot, R.; Ouahab, L.; Grandjean, D. Epoxidation of allylic alcohols by hydrogen peroxide in the presence of complexed peroxotungstic species. J. Mol. Catal. A Chem. 1996, 114, 77–85. [Google Scholar] [CrossRef]
  31. Gao, Y.; Mirante, F.; de Castro, B.; Zhao, J.; Cunha-Silva, L.; Balula, S.S. An effective hybrid heterogeneous catalyst to desulfurize diesel: Peroxotungstate@Metal–organic framework. Molecules 2020, 25, 5494. [Google Scholar] [CrossRef] [PubMed]
  32. Chilivery, R.; Chaitanya, V.; Nayak, J.; Seth, S.; Rana, R.K. Heterogenization of phosphotungstate clusters into magnetic microspheres: Catalyst for selective oxidation of alcohol in water. ACS Sustain. Chem. Eng. 2022, 10, 6925–6933. [Google Scholar] [CrossRef]
  33. Leng, Y.; Wu, J.; Jiang, P.; Wang, J. Amphiphilic phosphotungstate-paired ionic copolymer as a highly efficient catalyst for triphase epoxidation of alkenes with H2O2. Catal. Sci. Technol. 2014, 4, 1293–1300. [Google Scholar] [CrossRef]
  34. Ibrahim, M.; Labaki, M.; Giraudon, J.M.; Lamonier, J.F. Hydroxyapatite, a multifunctional material for air, water and soil pollution control: A review. J. Hazard. Mater. 2020, 383, 121139. [Google Scholar] [CrossRef] [PubMed]
  35. Gruselle, M. Apatites: A new family of catalysts in organic synthesis. J. Organomet. Chem. 2015, 793, 93–101. [Google Scholar] [CrossRef]
  36. Ichihara, J.; Yamaguchi, S.; Nomoto, T.; Nakayama, H.; Iteya, K.; Naitoh, N.; Sasaki, Y. Keggin-type polyacid cluster on apatite: Characteristic catalytic activities in solvent-free oxidation. Tetrahedron Lett. 2002, 43, 8231–8234. [Google Scholar] [CrossRef]
  37. Ichihara, J.; Kambara, A.; Iteya, K.; Sugimoto, E.; Shinkawa, T.; Takaoka, A.; Yamaguchi, S.; Sasaki, Y. Cetylpyridinium dodecatungstate on fluorapatite: Efficient and reusable solid catalyst for solvent-free epoxidation. Green Chem. 2003, 5, 491–493. [Google Scholar] [CrossRef]
  38. Crosman, A.; Gelbard, G.; Poncelet, G.; Parvulescu, V.I. Epoxidation of cyclohexene and indene with hydrogen peroxide in the presence of WO5 onto hydroxyapatite as a catalyst. Appl. Catal. A Gen. 2004, 264, 23–32. [Google Scholar] [CrossRef]
  39. Ishikawa, K.; Ducheyne, P.; Radin, S. Determination of the Ca/P ratio in calcium-deficient hydroxyapatite using X-ray diffraction analysis. J. Mater. Sci.-Mater. Med. 1993, 4, 165–168. [Google Scholar] [CrossRef]
  40. Bulina, N.V.; Makarova, S.V.; Baev, S.G.; Matvienko, A.A.; Gerasimov, K.B.; Logutenko, O.A.; Bystrov, V.S. A Study of Thermal Stability of Hydroxyapatite. Minerals 2021, 11, 1310. [Google Scholar] [CrossRef]
  41. Mortier, A.; Lemaitre, J.; Rodrique, L.; Rouxhet, P.G. Synthesis and thermal behavior of well-crystallized calcium-deficient phosphate apatite. J. Solid State Chem. 1989, 78, 215–219. [Google Scholar] [CrossRef]
  42. Matsumura, Y.; Kanai, H.; Moffat, J.B. Catalytic oxidation of carbon monoxide over stoichiometric and non-stoichiometric hydroxyapatites. J. Chem Soc. Faraday Trans. 1997, 93, 4283–4387. [Google Scholar] [CrossRef]
  43. Tanaka, H.; Futaoka, M.; Hino, R. Surface modification of calcium hydroxyapatite with pyrophosphoric acid. J. Colloid Interface Sci. 2004, 269, 358–363. [Google Scholar] [CrossRef]
  44. Mori, K.; Hara, T.; Oshiba, M.; Mizugaki, T.; Ebitani, K.; Kaneda, K. Catalytic investigations of carbon-carbon bond-forming reactions by a hydroxyapatite-bound palladium complex. New J. Chem. 2005, 29, 1174–1181. [Google Scholar] [CrossRef]
  45. Kaur, J.; Kozhevnikov, I.V. Polyoxometalate-catalysed epoxidation of propylene with hydrogen peroxide: Microemulsion versus biphasic process. Catal. Commun. 2004, 5, 709–713. [Google Scholar] [CrossRef]
  46. Yamaguchi, K.; Mori, K.; Mizugaki, T.; Ebitani, K.; Kaneda, K. Creation of a monomeric Ru species on the surface of hydroxyapatite as an efficient heterogeneous catalyst for aerobic alcohol oxidation. J. Am. Chem. Soc. 2000, 122, 7144–7145. [Google Scholar] [CrossRef]
  47. Mori, K.; Yamaguchi, K.; Hara, T.; Mizugaki, T.; Ebitani, K.; Kaneda, K. Controlled synthesis of hydroxyapatite-supported palladium complexes as highly efficient heterogeneous catalyst. J. Am. Chem. Soc. 2002, 124, 11572–11573. [Google Scholar] [CrossRef]
  48. Hara, T.; Mori, K.; Oshiba, M.; Mizugaki, T.; Ebitani, K.; Kaneda, K. Highly efficient dehalogenation using hydroxyapatite-supported palladium nanocluster catalyst with molecular hydrogen. Green Chem. 2004, 6, 507–509. [Google Scholar] [CrossRef]
  49. Zhou, J.; Zhang, X.; Chen, J.; Zeng, S.; DE Groot, K. High temperature characteristics of synthetic hydroxyapatite. J. Mater. Sci.-Mater. Med. 1993, 4, 83–85. [Google Scholar] [CrossRef]
  50. Li, Y.; De Groot, K.; De Wijn, J.; Klein, C.P.A.T.; Meer, S.V.D. Morphology and composition of nanograde calcium phosphate needle-like crystals formed by simple hydrothermal treatment. J. Mater. Sci.-Mater. Med. 1994, 5, 326–331. [Google Scholar]
  51. Tamai, M.; Nakamura, M.; Isshiki, T.; Nishio, K.; Endoh, H.; Nakahira, A. A metastable phase in thermal decomposition of Ca-deficient hydroxyapatite. J. Mater. Sci.-Mater. Med. 2003, 14, 617–622. [Google Scholar] [CrossRef]
  52. Tanaka, H.; Cjikazawa, M.; Kandori, K.; Ishikawa, T. FTIR and TPD studies on the adsorption of pyridine, n-butylamine and acetic acid on calcium hydroxyapatite. Phys. Chem. Chem. Phys. 2000, 2, 2647–2650. [Google Scholar] [CrossRef]
  53. Aubry, C.; Chottard, G.; Platzer, N.; Bregeault, J.M.; Thouvenot, R.; Chauveau, F.; Huet, C.; Ledon, H. Reinvestigation of epoxidation using tungsten-based precursors and hydrogen peroxide in a biphase medium. Inorg. Chem. 1991, 30, 4409–4415. [Google Scholar] [CrossRef]
  54. Dengel, A.C.; Griffith, W.P.; Parkin, B.C. Studies on polyoxo- and polyperoxo-metalates. Part 1 Tetrameric heteropolyperoxotungstates and heteropolyperoxomolybdates. J. Chem. Soc. Dalton Trans. 1993, 2683–2688. [Google Scholar] [CrossRef]
  55. Bulina, N.V.; Eremina, N.V.; Vinokurova, O.B.; Ishchenko, A.V.; Chaikina, M.V. Diffusion of copper ions in the lattice of substituted hydroxyapatite during heat treatment. Materials 2022, 15, 5759. [Google Scholar] [CrossRef] [PubMed]
  56. Bulina, N.V.; Rybin, D.K.; Makarova, S.V.; Dudina, D.V.; Batraev, I.S.; Utkin, A.V.; Prosanov, I.Y.; Khvostov, M.V.; Ulianitsky, V.Y. Detonation Spraying of Hydroxyapatite on a Titanium Alloy Implant. Materials 2021, 14, 4852. [Google Scholar] [CrossRef]
  57. Liu, Y.; Hayakawa, T.; Suzuki, K.; Hamakawa, S.; Tsunoda, T.; Ishii, T.; Kumagai, M. Highly active copper/ceria catalysts for steam reforming of methanol. Appl. Catal. A-Gen. 2002, 223, 137–145. [Google Scholar] [CrossRef]
  58. Jacob, P.; Wehling, B.; Hill, W.; Klockow, D. Feasibility study of Raman spectroscopy as a tool to investigate the liquid-phase chemistry of aliphatic organic peroxides. Appl. Spectrosc. 1997, 51, 74–80. [Google Scholar] [CrossRef]
  59. Yeom, Y.H.; Ulagappan, N.; Frei, H. Mechanistic Study of CH3OH + O2 photoredox reaction in a FeAlPO4 sieve by time-resolved FT-IR spectroscopy. J. Phys. Chem. A 2002, 106, 3350–3355. [Google Scholar] [CrossRef]
  60. Bauerl, S.; Moortgat, G.K. Absorption cross-sections of HOCHOOH vapor between 205 and 360 nm at 298 K. Chem. Phys. Lett. 1999, 309, 43–48. [Google Scholar] [CrossRef]
  61. Liu, Y.; Sotelo-Boyas, Y.; Murata, K.; Minowa, T.; Sakanishi, K. Hydrotreatment of vegetable oils to produce bio-hydrogenated diesel and liquefied petroleum gas fuel over catalysts containing sulfided Ni-Mo and solid acids. Energy Fuels 2011, 25, 4675–4685. [Google Scholar] [CrossRef]
Molecules 28 00024 g001 550
Figure 1. FT-IR spectra of various samples. (A): HAP; (B): PW-HAP; (C): Pd-PW-HAP; (D): PdCl2; (E): PdCl2(PhCN)2; (F): THA-PW2; (G): K2[W2O3(O2)4].
Figure 1. FT-IR spectra of various samples. (A): HAP; (B): PW-HAP; (C): Pd-PW-HAP; (D): PdCl2; (E): PdCl2(PhCN)2; (F): THA-PW2; (G): K2[W2O3(O2)4].
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Figure 2. Effect of reaction time in the propylene epoxidation by O2 in methanol at 363 K over Pd-PW-HAP and Pd+PW2. (●): Pd-PW-HAP; (▲): Pd+PW2. (a) Effects of C3H6 conversion and PO selectivity; (b) effect of PO yield. Reaction conditions: same as those in Table 2.
Figure 2. Effect of reaction time in the propylene epoxidation by O2 in methanol at 363 K over Pd-PW-HAP and Pd+PW2. (●): Pd-PW-HAP; (▲): Pd+PW2. (a) Effects of C3H6 conversion and PO selectivity; (b) effect of PO yield. Reaction conditions: same as those in Table 2.
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Figure 3. Stability of the solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol. (a) The first run with a fresh catalyst; (b) the second run with the used solid catalyst (♦) and the liquid without a solid catalyst (▲).
Figure 3. Stability of the solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol. (a) The first run with a fresh catalyst; (b) the second run with the used solid catalyst (♦) and the liquid without a solid catalyst (▲).
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Figure 4. Time courses of solid catalyst Pd-PW-HAP in the propylene epoxidation by O2 in methanol for 5 runs. (●): Propylene conversion; (■): selectivity for PO. Reaction conditions: same as those in Table 2.
Figure 4. Time courses of solid catalyst Pd-PW-HAP in the propylene epoxidation by O2 in methanol for 5 runs. (●): Propylene conversion; (■): selectivity for PO. Reaction conditions: same as those in Table 2.
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Figure 5. XRD patterns of Pd-PW-HAP and Pd+PW2 before and after reaction. (A): Pd-PW-HAP before reaction; (B): Pd-PW-HAP after reaction at 363 K for 8 h; (C): Pd+PW2 before reaction; (D): Pd+PW2 after reaction at 363 K for 8 h.
Figure 5. XRD patterns of Pd-PW-HAP and Pd+PW2 before and after reaction. (A): Pd-PW-HAP before reaction; (B): Pd-PW-HAP after reaction at 363 K for 8 h; (C): Pd+PW2 before reaction; (D): Pd+PW2 after reaction at 363 K for 8 h.
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Figure 6. TEM images of Pd-PW-HAP before reaction and after reaction. (A): Before reaction; (B): after reaction at 363 K for 8 h; (C): after reaction at 363 K for 8 h for 5 runs.
Figure 6. TEM images of Pd-PW-HAP before reaction and after reaction. (A): Before reaction; (B): after reaction at 363 K for 8 h; (C): after reaction at 363 K for 8 h for 5 runs.
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Figure 7. EXAFS functions of various samples. (a) Pd K-edge k3-weighted EXAFS spectra and (b) magnitude of Fourier transforms in the r-space. (A): Pd-PW-HAP before reaction; (B): PdCl2; (C): Pd-PW-HAP after reaction at 363 K for 8 h; (D): Pd foil. A reduced factor of 0.5 was applied for Pd foil.
Figure 7. EXAFS functions of various samples. (a) Pd K-edge k3-weighted EXAFS spectra and (b) magnitude of Fourier transforms in the r-space. (A): Pd-PW-HAP before reaction; (B): PdCl2; (C): Pd-PW-HAP after reaction at 363 K for 8 h; (D): Pd foil. A reduced factor of 0.5 was applied for Pd foil.
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Figure 8. XPS spectra of Pd-PW-HAP before and after reaction. (A): Pd-PW-HAP before reaction; (B): Pd-PW-HAP after reaction at 363 K for 8 h.
Figure 8. XPS spectra of Pd-PW-HAP before and after reaction. (A): Pd-PW-HAP before reaction; (B): Pd-PW-HAP after reaction at 363 K for 8 h.
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Figure 9. The route in the synthesis of the hybrid compound Pd-PW-HAP.
Figure 9. The route in the synthesis of the hybrid compound Pd-PW-HAP.
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Scheme 1. Co-oxidation of methanol in the system containing Pd and O2.
Scheme 1. Co-oxidation of methanol in the system containing Pd and O2.
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Scheme 2. Reaction mechanism for propylene epoxidation by O2 in methanol.
Scheme 2. Reaction mechanism for propylene epoxidation by O2 in methanol.
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Table
Table 1. Results of elemental analyses of various HAP-containing samples 1.
Table 1. Results of elemental analyses of various HAP-containing samples 1.
CompoundChemical Composition (wt.%)Molar Ratio of Ca/P
CaPWPd
HAP34.319.8001.34
PW-HAP26.815.613.601.33
Pd-PW-HAP26.115.213.21.21.33
1 Obtained by inductively coupled plasma (ICP) analyses.
Table
Table 2. Results of propylene epoxidation by O2 in methanol over various catalysts 1.
Table 2. Results of propylene epoxidation by O2 in methanol over various catalysts 1.
Catalyst 2C3H6 Conv. (%)Selectivity (%)PO Yield (%)TON of [O–O] 2−
POAcroleinPA 3AcetoneC3H8Others 4
PW-HAP2.390.33.42.5003.82.11.1
PdCl2(PhCN)22.19.551.66.47.320.74.50.2–
Pd-PW-HAP 53.488.73.62.30.80.93.747.423.6
Pd+PW257.288.53.52.40.81.03.850.625.2
Pd-HMS-PW244.689.62.31.81.31.13.940.019.9
PdMgAl-PW448.387.13.82.91.20.94.142.121.0
1 Reaction temperature: 363 K; reaction time: 8 h. Autoclave reactor size: 100 mL; methanol: 20 mL. Charged gas in room temperature: C3H6: 1.0 MPa; O2: 1.0 MPa; N2: 0.1 MPa. 2 Catalyst amount: 0.5 g for solid catalysts; 0.02 g for PdCl2(PhCN)2; and 0.24 g THA-PW2 and 0.02 g PdCl2(PhCN)2 for homogeneous catalyst Pd+PW2. 3 PA: propionaldehyde. 4 Other products containing ring-opened compounds and C1–C6 hydrocarbons except for C3H8.
Table
Table 3. Reusability of solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol 1.
Table 3. Reusability of solid catalyst Pd-PW-HAP for the propylene epoxidation by O2 in methanol 1.
CatalystRun No.C3H6 Conv. (%)Select. for PO (%)PO Yield (%)
Fresh153.488.747.3
Used253.488.847.4
353.388.747.3
453.488.647.3
553.388.847.3
1 Reaction conditions: same as those in Table 2.
Table
Table 4. Results of catalytic propylene epoxidation by O2 over Pd-PW-HAP in various solvents 1.
Table 4. Results of catalytic propylene epoxidation by O2 over Pd-PW-HAP in various solvents 1.
SolventC3H6 Conversion (%)Selectivity for PO (%)PO Yield (%)TON of [O–O]2−
Methanol53.488.747.423.6
Chloroform2.291.52.01.0
1 Reaction conditions: same as those in Table 2.
Table
Table 5. Consumed amounts and formed amounts in the propylene epoxidation in methanol over various catalysts at 363 K for 8 h 1.
Table 5. Consumed amounts and formed amounts in the propylene epoxidation in methanol over various catalysts at 363 K for 8 h 1.
CatalystAmounts of Consumption (mmol)Amounts of Formation (mmol)
C3H6 (mmol)O2
(mmol)		CH3OH (mmol)PO (mmol)By-Product (mmol) 2Co-Product (mmol) 3
PW-HAP0.70.400.60.10
Pd-PW-HAP18.820.310.117.01.810.1
1 Reaction conditions: same as those in Table 2. 2 By-products: formed from propylene oxidation, including acetone, acrolein, propionaldehyde, propane, hydrocarbons, and ring-opened compounds. 3 Co-products: formed from methanol oxidation, mainly CO and CO2 (denoted as COx), with a small amount of HCHO.
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Liu, Y. Immobilization of Peroxo-Heteropoly Compound and Palladium on Hydroxyapatite for the Epoxidation of Propylene by Molecular Oxygen in Methanol. Molecules 2023, 28, 24. https://doi.org/10.3390/molecules28010024

AMA Style

Liu Y. Immobilization of Peroxo-Heteropoly Compound and Palladium on Hydroxyapatite for the Epoxidation of Propylene by Molecular Oxygen in Methanol. Molecules. 2023; 28(1):24. https://doi.org/10.3390/molecules28010024

Chicago/Turabian Style

Liu, Yanyong. 2023. "Immobilization of Peroxo-Heteropoly Compound and Palladium on Hydroxyapatite for the Epoxidation of Propylene by Molecular Oxygen in Methanol" Molecules 28, no. 1: 24. https://doi.org/10.3390/molecules28010024

APA Style

Liu, Y. (2023). Immobilization of Peroxo-Heteropoly Compound and Palladium on Hydroxyapatite for the Epoxidation of Propylene by Molecular Oxygen in Methanol. Molecules, 28(1), 24. https://doi.org/10.3390/molecules28010024

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