Next Article in Journal
A Critical Review on Artificial Intelligence for Fuel Cell Diagnosis
Next Article in Special Issue
Mechanistic Details of the Sharpless Epoxidation of Allylic Alcohols—A Combined URVA and Local Mode Study
Previous Article in Journal
Application of Nanocatalysts in Advanced Oxidation Processes for Wastewater Purification: Challenges and Future Prospects
Previous Article in Special Issue
Influence of the Support on Propene Oxidation over Gold Catalysts
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Catalysts
Volume 12
Issue 7
10.3390/catal12070742
catalysts-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Alkene Epoxidation and Thioether Oxidation with Hydrogen Peroxide Catalyzed by Mesoporous Zirconium-Silicates

by
Irina D. Ivanchikova
1,
Olga V. Zalomaeva
1,
Nataliya V. Maksimchuk
1,
Olga A. Stonkus
1,
Tatiana S. Glazneva
1,
Yurii A. Chesalov
1,
Alexander N. Shmakov
1,
Matteo Guidotti
2 and
Oxana A. Kholdeeva
1,*
1
Boreskov Institute of Catalysis, Lavrentieva Ave. 5, Novosibirsk 630090, Russia
2
CNR-SCITEC, Via C. Golgi 19, 20133 Milano, Italy
*
Author to whom correspondence should be addressed.
Catalysts 2022, 12(7), 742; https://doi.org/10.3390/catal12070742
Submission received: 14 June 2022 / Revised: 1 July 2022 / Accepted: 3 July 2022 / Published: 5 July 2022
(This article belongs to the Special Issue Catalytic Epoxidation Reaction)
Browse Figures
Versions Notes

Abstract

:
Mesoporous zirconium-silicates have been prepared using two different methodologies, evaporation-induced self-assembly and solventless organometallic precursor dry impregnation of commercial SiO2. The samples were characterized by elemental analysis, XRD, N2 adsorption, TEM, DRS UV–vis and Raman spectroscopic techniques. The catalytic performance of the Zr-Si catalysts was assessed in the epoxidation of three representative alkenes, cyclohexene, cyclooctene and caryophyllene, as well as in the oxidation of methyl phenyl sulfide using aqueous hydrogen peroxide as a green oxidant, with special attention drawn to the structure/activity relationship and catalyst stability issues. The key factors which affect substrate conversion and epoxide selectivity have been defined. The catalysts with larger contents of oligomeric ZrO2 species revealed higher activity. The nature of alkene and, in particular, its molecular hindrance is crucial, since the adsorption of the epoxide product is the main factor leading to fast catalyst deactivation. In fact, bulky epoxides do not show this effect. After optimization, the oxidation of caryophyllene gave endocyclic monoepoxide with 77% selectivity at 87% alkene conversion. Methyl phenyl sulfoxide afforded 37% of sulfoxide and 63% of sulfone at 57% sulfide conversion. The nature of catalysis was truly heterogeneous and no Zr leaching was observed.

Graphical Abstract

1. Introduction

Epoxides are key intermediates in the production of a wide variety of valuable products [1]. The selective epoxidation of alkenes with the green oxidant hydrogen peroxide using heterogeneous catalysts is an environmentally benign and economically sound route for the synthesis of epoxides and their derivatives [2,3,4,5,6]. Impressive progress has been made in this area due to the development of titanium silicalite-1 (TS-1) by the Eni group and its implementation for propene epoxidation [7,8]. However, the small pore size of TS-1 (ca. 5.5 Å) does not allow for transformation of bulky alkene substrates. Such limitation stimulated further research activity in the synthesis of mesoporous metal-silicates and the assessment of their catalytic performance started in the mid-1990s [9,10,11,12].
Significant advances have been achieved in the incorporation of Ti, Zr, Nb, W and some other transition metals into mesoporous silica matrixes using various synthetic methodologies [13,14,15,16,17,18]. Following the noteworthy success of TS-1, mesoporous titanium-silicates have received the greatest attention [9,10,11,12,13,14,19,20,21,22,23,24,25,26,27]. However, several research groups demonstrated that Nb-silicates can be more efficient than Ti-ones in the epoxidation of bulky alkenes with H2O2 and, moreover, possess better stability than the latter [28,29,30,31,32,33,34]. Some success has been recorded in the preparation of tungsten-containing silicates and their use in oxidation catalysis; however, partial tungsten leaching under the conditions of liquid-phase oxidation with H2O2 still remains an unresolved problem [35,36,37,38,39,40,41].
Although first attempts to insert zirconium into silica matrixes date back to the late 1990s [42,43,44], oxidation catalysis over Zr-silicates remains largely underexplored [42,43,45,46,47,48,49,50]. Oxidation of aniline and alkylphenols/naphthols were among the most studied reactions, while oxidation of alkenes and thioethers was less investigated, especially from the viewpoint of the oxidation mechanism. Strukul and co-workers revealed that ZrO2-SiO2 mixed oxides prepared by sol-gel method could accomplish oxidation of cyclooctene and cyclohexene to give corresponding diols as the main oxidation products [45,46]. In turn, Maksimchuk et al. demonstrated that Zr-MCF prepared by impregnation of the mesostructured silica support with Zr(IV) isopropoxide is an efficient catalyst for the allylic oxidation of α-pinene [47]. On the other hand, Zr-SiO2 made through a molecular precursor method showed very low activity in both alkene and thioether oxidation [33,51]. Meanwhile, more recent works on Zr-substituted polyoxometalates (Zr-POM) [52] and Zr-based metal-organic frameworks (Zr-MOF) [53,54] proved that Zr-catalysts can serve as highly effective epoxidation catalysts. These recent findings have stimulated our interest in oxidation catalysis with Zr(IV).
In the present work, we developed unprecedented protocols for the synthesis of leaching-resistant mesoporous Zr-silicates and investigated their catalytic performance in H2O2-based oxidation of a few representative olefins and thioethers. Two different methodologies were employed for the catalyst synthesis, namely, evaporation-induced self-assembly (EISA) and solventless dry impregnation of an organometallic Zr precursor onto a commercial mesoporous SiO2 (OM-DI). Previously, the EISA approach was successfully used for insertion of Ti [27], Nb [32], and W [40] into silicate materials while the OM-DI strategy found application in the preparation of solid oxidic catalysts containing Mo [55,56], Ti and Nb [30,57]. Our present work demonstrated that, regardless of the catalyst preparation method, mesoporous Zr-silicates enable fairly good substrate conversions and product selectivity in the oxidation of bulky alkenes and thioethers. Their common drawback is a fast deactivation caused by the strong adsorption of the epoxide product on Zr active sites. This problem does not exist if bulky alkene molecules are involved in the oxidation process.

2. Results and Discussion

2.1. Synthesis and characterization of Zr-Si-Catalysts

Zirconium is an oxophilic transition metal highly prone to the formation of di(oligo)meric forms [58]. Acetylacetone has been widely employed as a hydrolysis/oligomerization-retarding additive in the sol–gel and template syntheses of mesoporous metal-silicates [13,14,59]. Use of this chelating agent in the EISA-based synthesis of Ti-MMM-E catalysts not only prevented the formation of anatase-like aggregates, but also assisted the generation of a specific, di(oligo)meric state of Ti centers within the silica matrix [27]. The same chelating ligand was successfully employed for the stabilization of Nb and W precursors in the synthesis of Nb-MMM-E and W-MMM-E, respectively, using the EISA methodology [32,40]. In this work, we have extended this approach to the synthesis of mesoporous zirconium-silicates, hereinafter designated as Zr-MMM-E (see Experimental section for details).
Sample A was, therefore, prepared by a procedure similar to the one reported earlier for the synthesis of Ti-MMM-E [27], Nb-MMM-E [32] and W-MMM-E [40]. Zr(acac)4 was taken as a zirconium source. The molar ratio of Zr/Si was 0.9/50. For the preparation of samples B, C, and D we used an increased amount of HCl, corresponding to 1, 2 and 7 equiv of acid to Zr, respectively.
Upon evaporation of ethanol, the critical micelle concentration was achieved and self–assembly of a silica–Zr–surfactant mesophase occurred, resulting in the formation of transparent monoliths. After calcination and grounding, the solids gave a fine white powder. According to the EISA methodology, the composition of the starting mixtures is replicated in the composition of the resulting materials, as confirmed by the elemental analysis data reported in Table 1.
The textural properties of all Zr-MMM-E samples acquired from the nitrogen adsorption measurements are presented in Table 1, while the nitrogen adsorption-desorption isotherms for samples A and D are presented in Figure 1. All solids possess mostly mesopores. The increase in the HCl amount added during the synthesis led to the increase in specific BET surface area from 995 m2/g for sample A to 1404 m2/g for sample D. At the same time, the average pore diameter diminished from 3.8 nm for sample A to 3.1 nm for sample D. Moreover, the mesopore volume did not change significantly and remained in the interval of 0.58–0.62 cm3/g.
In Table 1, elemental analysis and textural data are also reported for a Zr/SiO2 catalyst that was prepared for the sake of comparison following the organometallic dry impregnation technique (OM-DI). In fact, analogous Ti(IV) and Nb(V) catalysts obtained by impregnating titanocene or niobocene dichloride, respectively, over a commercial non-ordered mesoporous silica support, under solventless conditions, proved to be efficient epoxidation catalysts in the liquid-phase epoxidation of unsaturated terpenes and fatty acid methyl esters [30,57].
While the Zr/SiO2 catalyst is fully amorphous and non-ordered to X-ray analysis, small angle XRD patterns of Zr-MMM-E exhibit a broad diffraction peak around 1.9 and 2.9 2θ° for samples A and D, respectively (Figure 2), indicating a long–range structural order of cylindrical mesopores typical of EISA-prepared metal-silicates [27,32,40]. No peaks were detected in the wide-angle range, which implies the absence of a zirconium oxide phase in the samples.
DR UV–vis spectra of the Zr-MMM-E and Zr/SiO2 catalysts are shown in Figure 3. Sample A synthesized without additional HCl revealed a sharp band with a maximum at 205–210 nm, that is usually attributed in the literature to the ligand-to-metal charge transfer from O2− to Zr4+ ion isolated in a silica matrix [44,60,61,62,63,64]. On the contrary, the spectrum of sample D prepared with additional 7 equiv of HCl displays a broad absorption in the range of 240–280 nm with a maximum centered at 250–270 nm, which can be assigned to nanoscopic regions of Zr-O-Zr linkages (ZrO2-like domains) [44,61,64]. The other two materials obtained with 1 and 2 equiv of HCl exhibit both adsorptions, although at a different ratio. It is also worth noting a small shoulder at 220 nm in the spectra of samples B and C, which can be attributed to small Zr-O-Zr clusters (oligomers) [44,62]. In general, the more amount of HCl added during the synthesis, the higher contribution of oligo(poly)meric ZrO2 species and their size. The Zr/SiO2 sample prepared by dry impregnation of silica exhibited a DRS-UV band with a maximum at ca. 210 nm and a shoulder around 240–270 nm (Figure 3), indicating the large occurrence of quasi isolated Zr(IV) species on the silica surface.
Raman spectroscopy was also used to investigate the nature of Zr species formed on the catalyst surface. The spectra of samples A and D are shown in Figure 4 in comparison with the spectra of the zirconium-free silicate matrix. Despite the pronounced difference observed in the DR–UV spectra, all Raman spectra look quite similar. Although the spectra are not well defined, we may conclude that ZrO2 is present in amorphous and/or clusterized forms rather than in crystalline domains, as no characteristic bands typically attributed to monoclinic, tetragonal, or cubic modifications of ZrO2 can be distinguished in the Raman spectra of the Zr-MMM-E samples [65,66].
Figure 5 shows TEM and HAADF-STEM images of silicate particles in A and D samples. The particle size varies over a wide range, from tens of nanometers to several micrometers. According to the EDX-mapping data, a homogeneous distribution of Si and Zr is observed in both samples regardless of the silicate particle size. Quantification gives an atomic ratio Si/Zr ≈ 98.5/1.5 in the studied areas which agrees well with the elemental analysis data.
The study of the Zr-catalysts in the HAADF-STEM mode allowed us to identify the location of Zr atoms, thanks to their high contrast (Z-contrast). On the HAADF-STEM image of sample A (Figure 6a) one can clearly see the individual bright dots and groups of bright dots with a higher contrast against the background of silicate. These data indicate the presence of Zr in a highly dispersed state. No periodic structures are observed in these areas, indicating the absence of nanoparticles with a defined structure of zirconium oxides. Thus, the zirconium species have a disordered or amorphous structure. A similar state of zirconium was observed in sample D. The HRTEM image of this solid (Figure 6b) shows only the amorphous structure of the silicate, while the HAADF-STEM image (inset of Figure 6b) exhibits inhomogeneous contrast indicating the presence of highly dispersed Zr-species.
The acidic and basic properties of the samples were studied using FTIR spectroscopy of the adsorbed probe molecules: carbon monoxide and deuterochloroform. FTIR spectra of calcined samples show a broad high-intensity band with a maximum at 3740 cm−1 in the absorption region of OH groups (Figure 7a). This band is usually observed for silicon oxide and indicates isolated Si-OH groups with stretching vibrations at 3740 cm−1 [67,68]. In addition, various types of Zr-OH groups with characteristic bands at 3670–3680 and 3760–3780 cm−1, usually observed for ZrO2, can contribute to such absorption band [69,70,71]. In this case, the absorption band at 3740 cm−1 cannot be separated into contributions from OH groups of various types. However, the presence of different types of OH groups is manifested in differential FTIR spectra by shifts in the absorption bands of the hydroxyl groups during CO adsorption (Figure 7b).
When CO is adsorbed (Figure 7b), the bands at 3725 and 3760 cm−1, characterizing various OH groups, disappear, and broad absorption bands at 3515 and 3600 cm−1 are formed, corresponding to hydrogen-bonded complexes of OH groups with CO molecules. Thus, the formation of various types of CO complexes with OH groups differing in strength is clearly seen. The strength of the OH groups (Brønsted acid sites, BAS) was characterized by proton affinity calculated from FTIR spectra using the values of the band shifts [72]. The OH groups characterized by the absorption band at 3760 cm−1 belong to Zr4+–OH and do not have pronounced acidic properties [70]. The band at 3725 cm−1 is formed by OH groups of two types with a band shift of 125 and 210 cm−1, which corresponds to proton affinities of 1330 and 1230 kJ/mol, respectively. The BAS of silicon dioxide and titanium silicates are known to have very low acidity—the characteristic shifts of the OH group bands are 90–120 cm−1 [72,73,74]. In our case, the BAS strength is much higher, which may be due to the formation of Si-O-Zr bonds and an increase in the electron density on the bridging oxygen. Yamaguchi et al. [75] studied ZrO2/SiO2 samples prepared by impregnating SiO2 with a Zr(n-OC3H7) solution and also showed an increase in Brønsted acidity due to charge transfer from the ZrO4 tetrahedron to SiO4 and strengthening of the Si–O bond. A rise in Brønsted acidity was previously shown for a number of mesoporous silicates modified with zirconium [76,77,78,79], which was associated with the introduction of Zr4+ ion into the silicate framework resulting in weakening the Si-OZrO–H bond and increasing the acidity of these OH groups.
CO adsorption on two types of BAS can also be observed in the range of carbonyl vibrations (Figure 8): at low CO pressures, there is a band at 2162 cm−1, and with increasing CO pressure, an additional band appears at 2155 cm−1, characterizing CO adsorbed on SiOH groups [53,72,80]. In addition, a band at 2182 cm−1 is observed in the spectra, which refers to the adsorption of CO on zirconium cations Zr4+ (Lewis acid sites, LAS) [53,70]. The absorption band at 2135 cm−1 characterizes the vibrations of physically adsorbed CO [72]. The BAS and LAS concentrations were determined from the integral intensities of the absorption bands at 2162 and 2182 cm−1 with integral absorption coefficients of 2.6 cm/µmol [72,80] and 2.2 cm/µmol [53,81], respectively. The number of BAS (OH groups with CO adsorption band at 2162 cm−1) is 2 µmol/g and 8 µmol/g, the number of LAS is 18 and 35 µmol/g for the samples A and D, respectively. The calculated LAS strength in units of CO adsorption heat [72] is 30 kJ/mol, which is close to that evaluated for Zr-MOFs (27–29 kJ/mol) [53,82] and slightly lower than the one acquired previously for Ti- and Nb-silicates (32 and 36 kJ/mol, respectively) [80]. The number of LAS estimated for Zr-silicates by the IR technique is also close to that found for Ti- and Nb-silicates, thereby indicating similar accessibility to active sites in all the metal-silicates prepared by the same EISA methodology.
Basic properties of the samples were studied using FTIR spectroscopy of adsorbed deuterochloroform. Figure 9 shows the FTIR spectra of samples A and D after adsorption of CDCl3. The spectra show an absorption band in the region of 2200–2300 cm−1, which can be deconvoluted into two individual Gaussian components with maxima at 2262 and 2268 cm−1 corresponding to hydrogen-bonded complexes of CDCl3 with the basic sites of the samples and CDCl3 in the gas phase, respectively [53,80,83]. The concentration of the basic sites determined from the integrated intensity of the absorption band at 2262 cm−1 is 1403 μmol/g and 1918 μmol/g, for the samples A and D, respectively. The strength of the basic sites characterized by the proton affinity [53,72,80] is 780 kJ/mol, which corresponds to weak basic sites. This value is similar to the one previously reported for the niobium-silicates prepared by EISA [80] and lower than the values of this parameter evaluated for various Zr-MOFs (840–860 kJ/mol) [53,82] and zirconium oxide (900 kJ/mol) [84]. Most likely, the basic sites are represented by oxygen of the surface ZrOH groups [82].

2.2. Catalytic Activity of Zr-Silicates in H2O2-Based Oxidation of Alkenes

Catalytic performance of Zr-MMM-E (samples A–D) and Zr/SiO2 was assessed in the oxidation of three representative alkenes, cyclohexene (CyH), cyclooctene (CyOct), and trans-caryophyllene (CP) with 30% aqueous H2O2 using acetonitrile as a solvent. The main results are summarized in Table 2, Table 3 and Table 4.
Cyclohexene was chosen because it serves as a conventional test substrate to evaluate contributions of homo- and heterolytic oxidation pathways by analysis of the composition of the reaction products (Scheme 1) [85]. Regardless of the method of their synthesis, all samples of Zr-MMM-E and Zr/SiO2 exhibited similar activity (Table 2). With equimolar amount of the oxidant, CyH conversions practically did not exceed the one obtained in a ‘blank’ experiment with no catalyst (Table 2, entry 1). However, the amount of the two-electron oxidation product epoxide increased in comparison to the amount of one-electron (allylic) oxidation products, cyclohexenyl hydroperoxide (HP), 2-cyclohexene-1-ol (enol), and 2-cyclohexene-1-one (enone) (compare entry 1 with entries 3, 7, 9, 11 and 13).
Recently, it has been reported that in situ addition of a source of protons to various Zr-MOF catalysts is a useful tool to increase the oxidation rate and reduce of the yield of allylic oxidation products in the CyH oxidation with H2O2 [53,86]. Indeed, the addition of 1 mol equiv (relative to Zr atoms in the silicate) of HClO4 increased significantly the attainable CyH conversion, reduced the reaction time and altered the composition of products, favoring the formation of epoxide along with diol, with total selectivity toward heterolytic oxidation products up to 94% (Table 2, entries 4, 8, 10, 12 and 14). In the absence of a Zr catalyst, the impact of the acid was much lower (Table 2, entry 2). The use of concentrated H2O2 (77%) instead of the dilute one (30%) led to a slight increase in the yield of epoxide with respect to the one of diol (Table 2, entry 5). The addition of 1 mol equiv of NaOAc to a Zr catalyst produced a negative effect on the catalytic activity (Table 2, entry 6).
Therefore, in this case too, acid additives favor the formation of active Zr peroxo species (most likely, hydroperoxo ones [52]). This seems to be a general phenomenon that operates with different types of Zr-catalysts, including Zr-silicates and Zr-MOFs.
Surprisingly, Zr-silicates exhibited rather low activity and selectivity in the epoxidation of cyclooctene (Table 3), the alkene substrate that often features good yields of epoxides with most of the known catalysts [80,87,88]. Higher conversion and epoxide selectivity were attained over sample D with a high fraction of oligomeric ZrO2 species, but, even in this case, a maximum 40% substrate conversion and 50% epoxide selectivity could be achieved using a two-fold excess of the oxidant. It is noteworthy that about 70% of H2O2 remained unused. The epoxide selectivity decreased with the reaction time (increased conversion), which is also atypical for CyOct, whose epoxide is generally considered ring-opening resistant. Indeed, independent experiments, in which CyOct epoxide was used as a substrate, showed no significant conversion of this compound under the reaction conditions. These observations suggest that some unidentifiable, probably, polymeric products are accumulated during the reaction course. As in the case of the CyH oxidation, acid additives accelerated CyOct oxidation and led to higher conversions. However, CyOct epoxide yield decreased markedly (see Table 3).
On the contrary, the oxidation of caryophyllene, a bulky natural terpene, with 2 equiv of H2O2 in the presence of Zr-MMM-E catalysts (samples A and D) as well as Zr/SiO2 produced endocyclic monoepoxide (Scheme 2) with fairly good substrate conversions and product yields (Table 4). Note that CP epoxide is a valuable product approved by FDA as a food and cosmetic stabilizer [89] and used as a flavoring substance with the scent of cloves too [90]. In contrast with CyH and CyOct oxidation, epoxidation of CP easily proceeds without acid additives too. As in the case of CyOct oxidation, sample D displayed the highest activity among the catalysts studied. Conversion of CP attained 87% after 5 h, whereas it reached only 69% over sample A. The selectivity to monoepoxide for all Zr-silicates reached 78–80%. It is noteworthy that CP was practically the only alkene substrate that revealed good epoxide yields in H2O2-based oxidations over Zr-MOFs [53]. Interestingly, other electron-rich alkenes, e.g., 3-carene and limonene, as well as tetramethylethylene gave significantly lower conversions and epoxide yields, indicating that nucleophilicity of the C=C double bond is not the main factor affecting the epoxidation efficiency. For instance, Zr/SiO2 was able to convert limonene into 1,2-limonene epoxide with an epoxide yield of 23% in 1 h [91], whereas Nb/SiO2, obtained via OM-DI from niobocene dichloride, was able to attain an epoxide yield of 46% in 1 h under the same conditions [30]. Therefore, we may suggest that some other factors, in particular alkene (epoxide) bulkiness, has a strong impact on the epoxidation over Zr-catalysts.
Figure 10 shows comparison of the catalytic performance of Zr-MMM-E in CP oxidation with that of Ti- and Nb-silicates prepared by the same EISA methodology. While the highest activity was observed over Nb-MMM-E, Zr-MMM-E proved to be more active than Ti-MMM-E. Selectivity to CP epoxide attained 77%, 80% and 74% for Zr-, Nb- and Ti-MMM-E, respectively.

2.3. Catalytic Activity of Zr-silicates in H2O2-Based Oxidation of Methyl Phenyl Sulfide

The oxidation of a representative thioether, methyl phenyl sulfide, over Zr-Si catalysts was investigated as well. In this reaction, the primary oxidation product is sulfoxide (MPSO) that is oxidized further to produce sulfone (MPSO2) (Scheme 3).
The product distribution in thioether oxidation with equimolar amount of oxidant allows one to suggest the nature of the oxidizing species, electrophilic or nucleophilic. While sulfoxides are products of electrophilic oxidation of sulfides, which are strong nucleophiles, sulfones can be produced via both electrophilic and nucleophilic oxidation of sulfoxides, which possess a biphilic nature [92]. Earlier, we have found that H2O2-based oxidation of MPS and other thioethers in the presence of Zr-MOFs, in particular UiO-66, occurs via predominantly nucleophilic mechanism, leading to the formation of sulfone with selectivity up to 99% at ca. 50% MPS conversion [53,82].
The main results on the MPS oxidation with 1 equiv of H2O2 over Zr-Si catalysts are presented in Table 5. For all Zr-MMM-E samples and the OM-DI-derived catalyst Zr/SiO2, sulfone was the prevailing product formed with selectivity 62–74% at 51–57% MPS conversion. Catalyst A, having mostly ‘isolated’ zirconium centers, was less active and gave more sulfone than the other catalysts that possess oligomeric ZrO2 species. Again, sample D was the most active one among the series of Zr-MMM-E catalysts. The Zr/SiO2 sample showed a higher initial oxidation rate than all Zr-MMM-E solids, but MPS conversion and products yields were similar to the ones obtained with samples B, C and D (Table 5). The oxidant utilization efficiency values were as high as 89–93% for Zr-MMM-E samples and 86% for the Zr/SiO2 catalyst.

2.4. Mechanism of Alkene and Thioether Oxidation with H2O2 over Zr-Silicate Catalysts

The prevalent formation of sulfone over sulfoxide in the MPS oxidation with one equivalent of the oxidant clearly indicates predomination of nucleophilic oxidizing species over electrophilic ones in the presence of Zr-catalyst and H2O2 [82] and references cited therein. Given that di(oligo)nuclear species certainly prevail in the most active Zr-silicate catalysts, we may suggest a hydrogen peroxide activation mechanism similar to the one we proposed earlier for Zr-MOFs (Scheme 4). In this mechanism, the first step is the formation of an electrophilic Zr hydroperoxo species ‘ZrOOH’, which is responsible for the oxygen transfer to a C=C bond in the alkene and nucleophilic S atom in the thioether. The presence of weak basic sites (most probably ZrOH) favors the transformation of ‘ZrOOH’ to a nucleophilic peroxo Zr species, ‘ZrOO–‘, which acts as the oxidant toward the sulfoxide bound to the neighboring Zr site.

2.5. The reasons for Zr-Si Catalyst Deactivation

Zr-silicate-catalyzed epoxidation is typically characterized by relatively low alkene conversion values. Thus, with 1 equiv of oxidant, the maximal CyH conversion attained 23–29%, without a significant alteration in the product selectivity (Table 2). The incomplete substrate conversion might be caused by competitive decomposition of H2O2 with evolution of molecular oxygen. However, we have found that the rate of unproductive H2O2 decomposition over Zr-MMM-E was rather low in comparison with Nb- and Ti-silicates (Figure 11a), for which significantly higher CyH conversions could be achieved [32] (Figure 11b). Indeed, H2O2 utilization efficiency in the presence of Zr-MMM-E (sample A) and 1 equiv of H+ attained 90%, indicating that the reaction stopped before all H2O2 was consumed. Therefore, unproductive degradation of the oxidant cannot be the main reason for low alkene conversions in the presence of Zr-silicates.
Another reason for fast catalyst deactivation could be the accumulation of the reaction products inside the pores and/or their strong binding to zirconium active sites. However, physical adsorption of the product could hardly be the reason for catalyst deactivation, otherwise the same phenomenon would be observed for Nb- and Ti-catalysts as well, which is not the fact. This means that a specific chemical binding of products to oxophilic Zr(IV) sites can play a critical role. Previously, we have shown that oxidation products (epoxide/diol and water) caused the catalyst deactivation in the CyH oxidation over UiO-66 [86]. Interestingly, in the case of Zr-MMM-E, only epoxide additives dramatically slowed down the CyH oxidation process, without reaching the expected substrate conversion, while the addition of CyH diol or H2O into the reaction mixture produced no effect at all (Figure 12).
In sharp contrast, the addition of CP epoxide produced no rate-retarding effect on the oxidation of CP itself (Figure 13). Given that CP epoxide is a large molecule, we may assume that, because of its bulkiness, it likely prevents the coordination of the epoxide oxygen atom to Zr(IV) sites. This specific feature enables high epoxidation yields in CP oxidation over Zr-catalysts.
Specific adsorption study (see Section 3.5 for details) revealed some adsorption of sulfoxide (about 10% from a 0.1 M solution in CH3CN) and no adsorption of sulfide and sulfone on Zr-MMM-E (sample D). However, the addition of sulfoxide to the reaction mixture produced minor effect on the MPS oxidation over Zr-MMM-E (Figure 14), which is due to fast oxidation of sulfoxide to sulfone.

2.6. Catalyst Stability and Reusability

The stability of the structure of Zr-Si catalysts in the presence of aqueous H2O2 was checked by means of XRD technique. XRD patterns of both sample A and sample D remained intact after treatment with an aqueous-acetonitrile solution of H2O2 (Figure 15).
The nature of the catalysis over Zr-MMM-E was verified for both alkene and MPS oxidation by hot filtration tests. Practically no further substrate conversion was observed after removal of the catalyst, indicating the truly heterogeneous nature of the observed catalysis (Figure 16). The solid and filtrate were also studied by elemental analysis using ICP-AES. It was found that Zr content in the sample remains intact while the amount of Zr in the filtrates is below 1 ppm, which confirms the absence of metal leaching under the conditions employed.
The recycling behavior of the most active catalysts, sample D, was studied in several consecutive runs in the oxidation of CP and MPS with 30% H2O2 (Figure 17a,b), respectively). The catalyst was regenerated by calcination at 550 °C between the runs. The catalyst revealed a rather stable recycling performance in the CP epoxidation (Figure 17a) and MPS oxidation (Figure 17b). Although some reduction of the turnover frequency (TOF) could be observed after the first use in MPS oxidation, the TOF remained constant and even increased during the subsequent runs.

3. Materials and Methods

3.1. Materials

Cetyltrimethylammonium bromide (CTAB, 99+%), tetraethyl orthosilicate (TEOS, 98+%), zirconium(IV) acetylacetonate (Zr(C5H7O2)4) (97%), 98.5% (-)-trans-caryophyllene, were purchased from Sigma-Aldrich. Methyl phenyl sulfide (99%) was purchased from Acros. CyH and CyOct were purchased from Sigma-Aldrich and purified prior to use by passing through a column filled with neutral alumina to remove traces of possible oxidation products. Acetonitrile (HPLC–grade, Panreac) was dried and stored over activated 4 Å molecular sieves. Ethanol (95%), ethylacetate and other reactants were obtained commercially and used without any additional purification. The concentration of H2O2 (30 or 77 wt.% in water) was determined iodometrically prior to use. Deionized water (EASY pure, RF, Barnsted) was used for the preparation of catalysts.

3.2. Catalyst Preparation and Characterization

Preparation of Zr(acac)4 solution. A typical procedure was as follows: 0.44 g (0.9 mmol) Zr(acac)4 were dissolved in 8 mL of ethanol (95%) and mixed for 1 h at room temperature with periodical heating at 40 °C until complete dissolution.
Synthesis of Zr-MMM-E by EISA. In a standard procedure, surfactant, CTAB (2.75 g, 7.5 mmol) was dissolved in ethanol (95%, 73 mL) under vigorous stirring for 2 h at room temperature. Then TEOS (11.2 mL, 0.05 mol), deionized H2O (6 mL), 36.5% HCl (6 µL, 0.07 mmol) and the solution of the Zr(acac)4 in ethanol (see above) were added under vigorous stirring. The reaction mixture was stirred (750 rpm) for 30 s and then the resulting clear sol was left in an open Petri dish under ambient conditions until full evaporation of the solvent. The as–made solid was calcined at 550 °C for 5 h in the air with a temperature ramp of 1 °C/min to remove the organic species. The solid was designated as sample A. For the preparation of samples B, C and D, the amount of HCl was increased to 77 (0.9 mmol, 1 equiv to Zr), 154 (1.8 mmol, 2 equiv to Zr), and 532 µL (6.3 mmol, 7 equiv to Zr), respectively.
Synthesis of Ti-MMM-E and Nb-MMM-E by EISA. For comparison, mesoporous titanium and niobium silicates with oligomeric Ti(IV) and Nb(V) sites were prepared by the same EISA approach following the protocols reported earlier [27] and [32], respectively. Textural properties for Ti-MMM-E (Ti 2.5 wt.%): SBET = 1040 m2/g, Vp = 0.68 cm3/g, Dp = 2.6 nm; for Nb-MMM-E (Nb 1.85 wt.%): SBET = 1138 m2/g, Vp = 0.59 cm3/g, Dp = 2.9 nm.
Synthesis of Zr/SiO2. The Zr/SiO2 catalyst was obtained via solventless organometallic precursor dry impregnation of commercial SiO2 (Grace Davison, LC60A; S BET 529 m2/g, pore volume 0.88 cm3/g, mean pore diameter 2.0–8.0 nm (very broad distribution with a maximum at 5.4 nm). The silica support was rehydrated with high purity deionized (18 MΩ cm) water (MilliQ Academic, Millipore) for 2 h and then dried at the rotary evaporator. The sample was calcined at 300 °C for 1 h in air and overnight under dynamic vacuum. Bis(cyclopentadienyl)zirconium(IV) dichloride (98% Sigma-Aldrich) was finely milled and added under inert atmosphere in solid phase to the silica. The solid mixture was stirred overnight under static vacuum at 150 °C. The mixture was calcined under oxygen at 500 °C for 2 h to obtain the final catalyst.
The freshly calcined samples were characterized by elemental analysis, N2 adsorption, X–ray diffraction, TEM, Raman, and diffusion reflectance UV–vis techniques and used for catalytic tests.

3.3. Catalytic Oxidations

Catalytic reactions were performed under vigorous stirring (500 rpm) in thermostated glass vessels. Typical reaction conditions for CyH oxidation were as follows: CyH 0.1 M, H2O2 0.1 M, Zr-Si catalyst 10 mg (0.003 mmol Zr), CH3CN, 1 mL, 50 °C, 2 h. Typical reaction conditions for CyOct and CP oxidations were as follows: CyOct or CP 0.1 M, H2O2 0.1–0.2 M, Zr-Si catalysts 20 mg (0.005 mmol Zr), CH3CN, 1 mL, 50 °C, 2–5 h. Typical reaction conditions for MPS oxidation: MPS 0.1 M, H2O2 0.1 M, Zr-MMM-E 5 mg (0.0014 mmol Zr), CH3CN, 1 mL, 60 °C, 0.5–2 h. Reactions were started by the addition of H2O2 to the reaction mixture. Samples of the reaction mixture were withdrawn periodically during the reaction course by a syringe through a septum. Each experiment was reproduced 2–4 times. The oxidation products were identified by the comparison of gas chromatography (GC) retention time with the retention time of the authentic samples. Product yields and substrate conversions were quantified by GC using biphenyl as an internal standard.

3.4. Hydrogen Peroxide Decomposition

Decomposition of H2O2 (0.4 M) was studied in the absence of organic substrate at 70 °C in CH3CN (5 mL) in the presence of M-MMM-E catalysts (M = Ti, Nb or Zr, 0.016 mmol). Aliquots of 0.2 mL were taken during the reaction course, and H2O2 concentration was determined by iodometric titration. Each experiment was reproduced 2–3 times.

3.5. Sorption Studies

MPS, MPSO and MPSO sorption studies were performed in thermostated glass vessels under vigorous stirring (500 rpm). 1 mL of 0.1 M solution of MPS, MPSO or MPSO2 in CH3CN were added to 10 mg of Zr-MMM-E (sample A) and stirred during 1 h at 27 °C. The aliquots were taken from solution by syringe and analyzed by GC using biphenyl as an internal standard to quantify the concentration.

3.6. Hydrothermal Stability and Stability towards Aqueous H2O2

To estimate the stability toward aqueous H2O2, samples A and D was treated with aqueous 30% H2O2 for 1 h (100 mg of catalyst, 0.11 M H2O2, 20 mL MeCN, 25 °C), dried in air and calcined at 550 °C before physicochemical measurements.

3.7. Instrumentation

GC analyses were performed using a gas chromatograph Tsvet-500 or Chromos GH-1000 equipped with a flame ionization detector and a quartz capillary column (30 m × 0.25 mm) filled with Agilent DB-5MS.
XRD measurements were performed on a high precision X–ray diffractometer mounted on beamline No.2 of the VEPP–3 storage ring at Siberian Synchrotron Radiation Center (SSRC). The radiation wavelength was 0.15393 nm. A high natural collimation of the synchrotron radiation beam, a flat perfect crystal analyzer, and a parallel Soller slit on the diffracted beam limiting its azimuthal divergence provided an extremely high instrumental resolution in a small angle region of 2θ = 0.5 ÷ 10° and higher.
Nitrogen adsorption measurements were carried out at 77 K using a NOVA 1200 instrument (Quantachrome) within the partial pressure range 10−4–1.0. The catalysts were degassed at 150 °C for 24 h before the measurements. Surface areas of the Zr-MMM-E samples were determined by the BET analysis of low–temperature N2 adsorption data. Pore size distributions were calculated from the adsorption branches of the nitrogen isotherms by means of the regularization procedure, using reference local isotherms calculated in a cylindrical silica pore model in the framework of the density functional theory (DFT) approach. Special software provided by Quantachrome Corp. was used for this purpose. Mean pore diameters were calculated as mathematical expectation values from these distributions.
Zirconium content in the solids and in the filtrate, which remained after separation of the catalysts from the reaction mixture, was determined by ICP–OES using a Perkin-Elmer Optima-430 DV instrument.
The state of zirconium in the catalysts was studied by DR UV–vis spectroscopy under ambient conditions using a Shimadzu UV–VIS 2501PC spectrophotometer. FT–Raman spectra (3600–100 cm−1, 300 scans, resolution 4 cm−1, 180° geometry) were recorded using a RFS 100/S spectrometer (Bruker). Excitation of the 1064 nm line was provided by an Nd–YAG laser (100 mW power output). Infrared spectra of adsorbed CO and CDCl3 were recorded on a Shimadzu IRTracer-100 spectrometer in the range of 400–6000 cm−1 with a resolution of 4 cm−1 and acquisition of 200 scans. Before adsorption of probe molecules, the samples pressed into thin pellets (20–25 mg/cm2) were evacuated in an IR cell at 500 °C for 1 h. CO adsorption was performed at −196 °C and CO pressure from 0.1 to 10 Torr. CDCl3 was adsorbed at 20 °C. Transmission electron microscopy (TEM) data were obtained using a Thermo Fisher Scientific Themis Z (Netherlands) electron microscope operated at 200 kV. Images with a high atomic number contrast were acquired using a high angle annular dark field (HAADF) detector in scanning-TEM (STEM) mode. The local composition of the samples was studied using EDX spectroscopy. The samples for the TEM study were prepared on a perforated carbon film mounted on a copper grid.

4. Conclusions

In this work, we demonstrated that mesoporous zirconium-silicates with fairly good dispersion and accessibility of active Zr(IV) sites can be prepared by two different methodologies, evaporation-induced self-assembly and solventless organometallic precursor dry impregnation of commercial SiO2. These two kinds of materials revealed similar catalytic performances in alkene and thioether oxidation with aqueous H2O2 that differed significantly from the catalytic behavior of Ti- and Nb-silicates prepared by the same methodologies, indicating that the nature of the transition metal plays a critical role in the oxidation scenario. In contrast to Ti- and Nb-catalysts, Zr-ones are highly prone to fast deactivation caused by strong adsorption of the epoxide product on Zr sites. However, high epoxide yields can be achieved if bulky electron-rich alkenes, e.g., caryophyllene, are used as substrates. In the thioether oxidation, sulfone predominates over sulfoxide, indicating a nucleophilic oxidation mechanism. These features are also typical of other types of Zr-catalysts, e.g., Zr-MOFs. Therefore, we may suggest that Zr-containing materials deserve a further investigation as heterogeneous catalysts to be potentially applied in the selective oxidation of bulky organic molecules for the production of high added-value products.

Author Contributions

Conceptualization, I.D.I., O.V.Z. and O.A.K.; formal analysis, I.D.I., O.V.Z., N.V.M., O.A.S., T.S.G., Y.A.C., A.N.S. and M.G.; investigation, I.D.I., O.V.Z., N.V.M., O.A.S., T.S.G., Y.A.C., A.N.S. and M.G.; methodology, I.D.I., O.V.Z., N.V.M., O.A.S., T.S.G., Y.A.C., A.N.S., M.G. and O.A.K.; visualization, I.D.I., O.V.Z., N.V.M., O.A.S. and T.S.G.; writing—original draft, O.V.Z.; writing—review & editing, I.D.I., O.V.Z., N.V.M., O.A.S., T.S.G., M.G. and O.A.K.; funding acquisition, N.V.M. and O.A.K.; project administration, O.A.K.; supervision, O.A.K. All authors have read and agreed to the published version of the manuscript.

Funding

This research was partially funded by the Ministry of Science and Higher Education of the Russian Federation within the governmental order for the Boreskov Institute of Catalysis (project AAAA-A21-121011390008-4) and the Russian Foundation for Basic Research (grant 21-53-15010).

Data Availability Statement

Not applicable.

Acknowledgments

The authors thank A.A. Leonova for the N2 adsorption measurements.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Sienel, G.; Rieth, R.; Rowbottom, K.T. Epoxides. In Ullmann’s Encyclopedia of Industrial Chemistry; Wiley-VCH Verlag GmbH & Co. KGaA: Weinheim, Germany, 2000. [Google Scholar] [CrossRef]
  2. Clerici, M.G.; Kholdeeva, O.A. (Eds.) Liquid Phase Oxidation via Heterogeneous Catalysis: Organic Synthesis and Industrial Applications; John Wiley & Sons: Hoboken, NJ, USA, 2013; 546p. [Google Scholar] [CrossRef]
  3. Duprez, D.; Cavani, F. (Eds.) Handbook of Advanced Methods and Processes in Oxidation Catalysis; Imperial College Press: London, UK, 2014; 1036p. [Google Scholar] [CrossRef]
  4. Sheldon, R.A.; van Bekkum, H. Fine Chemicals through Heterogeneous Catalysis; Wiley: Weinheim, Germany, 2001; pp. 473–551. [Google Scholar] [CrossRef]
  5. Mizuno, N. (Ed.) Modern Heterogeneous Oxidation Catalysis: Design, Reactions and Characterization; Wiley-VCH: Weinheim, Germany, 2009; 356p. [Google Scholar] [CrossRef]
  6. Sheldon, R.A. E factors, green chemistry and catalysis: An odyssey. Chem. Comm. 2008, 10, 3352–3365. [Google Scholar] [CrossRef]
  7. Clerici, M.G.; Bellussi, G.; Romano, U. Synthesis of propylene oxide from propylene and hydrogen peroxide catalyzed by titanium silicalite. J. Catal. 1991, 129, 159–167. [Google Scholar] [CrossRef]
  8. Forlin, A.; Bergamo, M.; Lindner, J. Production of Propylene Oxide. In Liquid Phase Oxidation via Heterogeneous Catalysis: Organic Synthesis and Industrial Applications; Clerici, M.G., Kholdeeva, O.A., Eds.; John Wiley & Sons: Hoboken, NJ, USA, 2013; Chapter 10.3; pp. 474–495. ISBN 978-0-470-94552-3. [Google Scholar] [CrossRef]
  9. Tanev, P.T.; Chibwe, M.; Pinnavaia, T. Titanium-Containing Mesoporous Molecular Sieves for Catalytic Oxidation of Aromatic Compounds. Nature 1994, 368, 321–323. [Google Scholar] [CrossRef]
  10. Sayari, A. Catalysis by Crystalline Mesoporous Molecular Sieves. Chem. Mater. 1996, 8, 1840–1852. [Google Scholar] [CrossRef]
  11. Corma, A. From microporous to mesoporous molecular sieve materials and their use in catalysis. Chem. Rev. 1997, 97, 2373–2420. [Google Scholar] [CrossRef]
  12. Tuel, A. Modification of mesoporous silicas by incorporation of heteroelements in the framework. Micropor. Mesopor. Mater. 1999, 27, 151–169. [Google Scholar] [CrossRef]
  13. Kholdeeva, O.A. Selective Oxidations Catalyzed by Mesoporous Metal-Silicates. In Liquid Phase Oxidation via Heterogeneous Catalysis: Organic Synthesis and Industrial Applications; Clerici, M.G., Kholdeeva, O.A., Eds.; John Wiley & Sons: Hoboken, NJ, USA, 2013; Chapter 4; pp. 127–219. [Google Scholar] [CrossRef]
  14. Kholdeeva, O.A. Recent Developments in Liquid-Phase Selective Oxidation Using Environmentally Benign Oxidants and Mesoporous Metal-Silicates. Catal. Sci. Technol. 2014, 4, 1869–1889. [Google Scholar] [CrossRef]
  15. Dal Santo, V.; Guidotti, M.; Psaro, R.; Marchese, L.; Carniato, F.; Bisio, C. Rational Design of Single-Site Heterogeneous Catalysts: Towards High Chemo-, Regio-and Stereoselectivity. Proceed. Royal Soc. A 2012, 468, 1904–1926. [Google Scholar] [CrossRef]
  16. Cui, X.; Li, W.; Ryabchuk, P.; Junge, K.; Beller, M. Bridging homogeneous and heterogeneous catalysis by heterogeneous single-metal-site catalysts. Nat. Catal. 2018, 1, 385–397. [Google Scholar] [CrossRef]
  17. Liang, J.; Liang, Z.; Zou, R.; Zhao, Y. Heterogeneous Catalysis in Zeolites, Mesoporous Silica, and Metal–Organic Frameworks. Adv. Mater. 2017, 29, 1701139. [Google Scholar] [CrossRef]
  18. Samantaray, M.K.; Pump, E.; Bendjeriou-Sedjerari, A.; D’Elia, A.; Pelletier, J.D.A.; Guidotti, M.; Psaro, R.; Basset, J.M. Surface organometallic chemistry in heterogeneous catalysis. Chem. Soc. Rev. 2018, 47, 8403–8437. [Google Scholar] [CrossRef] [PubMed]
  19. Kholdeeva, O.A.; Melgunov, M.S.; Shmakov, A.N.; Trukhan, N.N.; Kriventsov, V.V.; Zaikovskii, V.I.; Malishev, M.E.; Romannikov, V.N. A New Mesoporous Titanium-Silicate Ti-MMM-2: A Highly Active and Hydrothermally Stable Catalyst for H2O2-Based Selective Oxidations. Catal. Today 2004, 91–92, 205–209. [Google Scholar] [CrossRef]
  20. Xiao, F.-S. Ordered Mesoporous Materials with Improved Stability and Catalytic Activity. Topics Catal. 2005, 35, 9–24. [Google Scholar] [CrossRef]
  21. Sorokin, A.B.; Tuel, A. Metallophthalocyanine Functionalized Silicas: Catalysts for the Selective Oxidation of Aromatic Compounds. Catal. Today 2000, 57, 45–59. [Google Scholar] [CrossRef]
  22. Xiao, F.S.; Han, Y.; Yu, Y.; Meng, X.; Yang, M.; Wu, S. Hydrothermally Stable Ordered Mesoporous Titanosilicates with Highly Active Catalytic Sites. J. Am. Chem. Soc. 2002, 124, 888–889. [Google Scholar] [CrossRef]
  23. Wu, P.; Tatsumi, T.; Komatsu, T.; Yashima, T. Postsynthesis, Characterization, and Catalytic Properties in Alkene Epoxidation of Hydrothermally Stable Mesoporous Ti-SBA-15. Chem. Mater. 2002, 14, 1657–1664. [Google Scholar] [CrossRef]
  24. Moliner, M.; Corma, A. Advances in the Synthesis of Titanosilicates: From the Medium Pore TS-1 Zeolite to Highly-Accessible Ordered Materials. Micropor. Mesopor. Mater. 2014, 189, 31–40. [Google Scholar] [CrossRef] [Green Version]
  25. Guidotti, M.; Gavrilova, E.; Galarneau, A.; Coq, B.; Psaro, R.; Ravasio, N. Epoxidation of Methyl Oleate with Hydrogen Peroxide. The Use of Ti-Containing Silica Solids as Efficient Heterogeneous Catalysts. Green Chem. 2011, 13, 1806–1811. [Google Scholar] [CrossRef]
  26. Guidotti, M.; Pirovano, C.; Ravasio, N.; Lázaro, B.; Fraile, J.M.; Mayoral, J.A.; Coq, B.; Galarneau, A. The Use of H2O2 over Titanium-Grafted Mesoporous Silica Catalysts: A Step Further towards Sustainable Epoxidation. Green Chem. 2009, 11, 1421–1427. [Google Scholar] [CrossRef]
  27. Ivanchikova, I.D.; Kovalev, M.K.; Mel’gunov, M.S.; Shmakov, A.N.; Kholdeeva, O.A. User-Friendly Synthesis of Highly Selective and Recyclable Mesostructured Titanium-Silicate Catalysts for the Production of Bulky Benzoquinones. Catal. Sci. Technol. 2014, 4, 200–207. [Google Scholar] [CrossRef]
  28. Ziolek, M. Niobium-Containing Catalysts—The State of the Art. Catal. Today 2003, 78, 47–64. [Google Scholar] [CrossRef]
  29. Aronne, A.; Turco, M.; Bagnasco, G.; Ramis, G.; Santacesaria, E.; Di Serio, M.; Marenna, E.; Bevilacqua, M.; Cammarano, C.; Fanelli, E. Gel Derived Niobium–Silicon Mixed Oxides: Characterization and Catalytic Activity for Cyclooctene Epoxidation. Appl. Catal. A General 2008, 347, 179–185. [Google Scholar] [CrossRef]
  30. Gallo, A.; Tiozzo, C.; Psaro, R.; Carniato, F.; Guidotti, M. Niobium Metallocenes Deposited onto Mesoporous Silica via Dry Impregnation as Catalysts for Selective Epoxidation of Alkenes. J. Catal. 2013, 298, 77–83. [Google Scholar] [CrossRef]
  31. Ramanathan, A.; Maheswari, R.; Subramaniam, B. Facile Styrene Epoxidation with H2O2 over Novel Niobium Containing Cage Type Mesoporous Silicate, Nb-KIT-5. Top. Catal. 2015, 58, 314–324. [Google Scholar] [CrossRef]
  32. Ivanchikova, I.D.; Maksimchuk, N.V.; Skobelev, I.Y.; Kaichev, V.V.; Kholdeeva, O.A. Mesoporous Niobium–Silicates Prepared by Evaporation–Induced Self–Assembly as Catalysts for Selective Oxidations with Aqueous H2O2. J. Catal. 2015, 332, 138–148. [Google Scholar] [CrossRef]
  33. Hajjami, N.E.; Thompson, A.B.; Notestein, J.M. Periodic Trends in Highly Dispersed Groups IV and V Supported Metal Oxide Catalysts for Alkene Epoxidation with H2O2. ACS Catal. 2015, 5, 5077–5088. [Google Scholar] [CrossRef]
  34. Kholdeeva, O.A.; Ivanchikova, I.D.; Maksimchuk, N.V.; Skobelev, I.Y. H2O2-Based Selective Oxidations: Nb(V) versus Ti(IV). Catal. Today 2019, 333, 63–70. [Google Scholar] [CrossRef]
  35. Zhang, Z.; Suo, J.; Zhang, X.; Li, S. Synthesis of Highly Active Tungsten-Containing MCM-41 Mesoporous Molecular, Sieve Catalyst. Chem. Commun. 1998, 2, 241–242. [Google Scholar] [CrossRef]
  36. Brégeault, J.-M.; Piquemal, J.-Y.; Briot, E.; Duprey, E.; Launay, F.; Salles, L.; Vennat, M.; Legrand, A.-P. New Approaches to Anchoring or Inserting Highly Dispersed Tungsten Oxo (Peroxo) Species in Mesoporous Silicates. Micropor. Mesopor. Mater. 2001, 44–45, 409–417. [Google Scholar] [CrossRef]
  37. Dai, W.-L.; Chen, H.; Cao, Y.; Li, H.; Xie, S.; Fan, K. Novel Economic and Green Approach to the Synthesis of Highly Active W-MCM41 Catalyst in Oxidative Cleavage of Cyclopentene. Chem. Commun. 2003, 7, 892–893. [Google Scholar] [CrossRef]
  38. Gao, R.; Yanga, X.; Dai, W.-L.; Le, Y.; Li, H.; Fan, K. High-Activity, Single-Site Mesoporous WO3-MCF Materials for the Catalytic Epoxidation of Cycloocta-1,5-diene with Aqueous Hydrogen Peroxide. J. Catal. 2008, 256, 259–267. [Google Scholar] [CrossRef]
  39. Yan, W.; Ramanathan, A.; Ghanta, M.; Subramaniam, B. Towards Highly Selective Ethylene Epoxidation Catalysts Using Hydrogen Peroxide and Tungsten- or Niobium-Incorporated Mesoporous Silicate (KIT-6). Catal. Sci. Technol. 2014, 4, 4433–4439. [Google Scholar] [CrossRef] [Green Version]
  40. Maksimchuk, N.V.; Ivanchikova, I.D.; Zalomaeva, O.V.; Skobelev, I.Y.; Chesalov, Y.A.; Shmakov, A.A.; Kholdeeva, O.A. Tungsten-Incorporated Mesoporous Silicate W-MMM-E as Heterogeneous Catalyst for Liquid-Phase Oxidations with Aqueous H2O2. Catalysts 2018, 8, 95. [Google Scholar] [CrossRef] [Green Version]
  41. Ten Dam, J.; Badloe, D.; Ramanathan, A.; Djanashvili, K.; Kapteijn, F.; Hanefeld, U. Synthesis, Characterisation and Catalytic Performance of a Mesoporous Tungsten Silicate: W-TUD-1. Appl. Catal. A General 2013, 468, 150–159. [Google Scholar] [CrossRef]
  42. Gontier, S.; Tuel, A. Novel Zirconium Containing Mesoporous SIlicas for Oxidation Reactions in the liquid Phase. Appl. Catal. A Gen. 1996, 143, 125–135. [Google Scholar] [CrossRef]
  43. Besson, M.; Bonnet, M.C.; Gallezot, P.; Tkatchenko, I.; Tuel, A. Catalysis for Fine Chemicals: Towards Specificity with Polyphasic Media. Catal. Today 1999, 51, 547–560. [Google Scholar] [CrossRef]
  44. Morey, M.S.; Stucky, G.D.; Schwarz, S.; Fröba, M. Isomorphic Substitution and Postsynthesis Incorporation of Zirconium into MCM-48 Mesoporous Silica. J. Phys. Chem. B 1999, 103, 2037–2041. [Google Scholar] [CrossRef]
  45. Palazzi, C.; Oliva, L.; Signoretto, M.; Strukul, G. Microporous Zirconia–Silica Mixed Oxides Made by Sol–Gel as Catalysts for the Liquid-Phase Oxidation of Olefins with Hydrogen Peroxide. J. Catal. 2000, 194, 286–293. [Google Scholar] [CrossRef]
  46. Morandin, M.; Gavagnin, R.; Pinna, F.; Strukul, G. Oxidation of Cyclohexene with Hydrogen Peroxide Using Zirconia–Silica Mixed Oxides: Control of the Surface Hydrophilicity and Influence on the Activity of the Catalyst and Hydrogen Peroxide Efficiency. J. Catal. 2002, 212, 193–200. [Google Scholar] [CrossRef]
  47. Maksimchuk, N.V.; Melgunov, M.S.; Mrowiec-Białoń, J.; Jarzębski, A.B.; Kholdeeva, O.A. H2O2-Based Allylic Oxidation of α-Pinene over Different Single Site Catalysts. J. Catal. 2005, 235, 175–183. [Google Scholar] [CrossRef]
  48. Chaudhari, K.; Bal, R.; Srinivas, D.; Chandwadkar, A.J.; Sivasanker, S. Redox Behavior and Selective Oxidation Properties of Mesoporous Titano- and Zirconosilicate MCM-41 Molecular Sieves. Microporous Mesoporous Mater. 2001, 50, 209–218. [Google Scholar] [CrossRef]
  49. Liu, J.M.; Liao, S.J.; Jiang, G.D.; Zhang, X.L.; Petrik, L. Preparation, Characterization and Catalytic Activity of Zr Embedded MSU-V with High Thermal and Hydrothermal Stability. Microporous Mesoporous Mater. 2006, 95, 306–311. [Google Scholar] [CrossRef]
  50. Quignard, F.; Choplin, A.; Teissier, R. A Molecular Route Towards Silica Supported Zirconium Catalysts Active for the Mild Oxidation of Olefins with H2O2. J. Mol. Catal. A Chem. 1997, 120, L27–L31. [Google Scholar] [CrossRef]
  51. Thornburg, N.E.; Notestein, J.M. Rate and Selectivity Control in Thioether and Alkene Oxidation with H2O2 over Phosphonate-Modified Niobium(V)–Silica Catalysts. ChemCatChem 2017, 9, 3714–3724. [Google Scholar] [CrossRef]
  52. Maksimchuk, N.V.; Evtushok, V.Y.; Zalomaeva, O.V.; Maksimov, G.M.; Ivanchikova, I.D.; Chesalov, Y.A.; Eltsov, I.V.; Abramov, P.A.; Glazneva, T.S.; Yanshole, V.V.; et al. Activation of H2O2 over Zr(IV). Insights from Model Studies on Zr-Monosubstituted Lindqvist Tungstates. ACS Catal. 2021, 11, 10589–10603. [Google Scholar] [CrossRef]
  53. Maksimchuk, N.V.; Ivanchikova, I.D.; Cho, K.H.; Zalomaeva, O.V.; Evtushok, V.Y.; Larionov, K.P.; Glazneva, T.S.; Chang, J.-S.; Kholdeeva, O.A. Catalytic Performance of Zr-Based Metal-Organic Frameworks Zr-abtc and MIP-200 in Selective Oxidations with H2O2. Chem. Eur. J. 2021, 27, 6985–6992. [Google Scholar] [CrossRef]
  54. Kholdeeva, O.A.; Maksimchuk, N.V. Metal-Organic Frameworks in Oxidation Catalysis with H2O2. Catalysts 2021, 11, 283. [Google Scholar] [CrossRef]
  55. Jaenicke, S.; Loh, W.L. Preparation of highly dispersed molybdenum on alumina by thermal decomposition of Mo(CO)6. Catal. Today 1999, 49, 123–130. [Google Scholar] [CrossRef]
  56. Debecker, D.P.; Stoyanova, M.; Rodemerck, U.; Eloy, P.; Leonard, A.; Su, B.L.; Gaigneaux, E.M. Thermal Spreading As an Alternative for the Wet Impregnation Method: Advantages and Downsides in the Preparation of MoO3/SiO2–Al2O3 Metathesis Catalysts. J. Phys. Chem. C 2010, 114, 18664–18673. [Google Scholar] [CrossRef]
  57. Tiozzo, C.; Bisio, C.; Carniato, F.; Marchese, L.; Gallo, A.; Ravasio, N.; Psaro, R.; Guidotti, M. Epoxidation with Hydrogen Peroxide of Unsaturated Fatty Acid Methyl Esters over Nb(V)-Silica Catalysts. Eur. J. Lipid Sci. Technol. 2013, 115, 86–93. [Google Scholar] [CrossRef]
  58. Nielsen, R.H.; Schlewitz, J.H.; Nielsen, H. Zirconium and Zirconium Compounds. In Kirk-Othmer Encyclopedia of Chemical Technology; John Wiley & Sons, Inc.: Hoboken, NJ, USA, 2013. [Google Scholar] [CrossRef]
  59. Schubert, U. Chemical Modification of Titanium Alkoxides for Sol–Gel Processing. J. Mater. Chem. 2005, 15, 3701–3715. [Google Scholar] [CrossRef]
  60. Tuel, A.; Gontier, S.; Teissier, R. Zirconium Containing Mesoporous Silicas: New Catalysts for Oxidation Reactions in the Liquid Phase. Chem. Commun. 1996, 651–652. [Google Scholar] [CrossRef]
  61. El Haskouri, J.; Cabrera, S.; Guillem, C.; Latorre, J.; Beltrán, A.; Beltrán, D.; Marcos, M.D.; Amorós, P. Atrane Precursors in the One-Pot Surfactant-Assisted Synthesis of High Zirconium Content Porous Silicas. Chem. Mater. 2002, 14, 5015–5022. [Google Scholar] [CrossRef]
  62. Newalkar, B.L.; Olanrewaju, J.; Komarneni, S. Microwave-Hydrothermal Synthesis and Characterization of Zirconium Substituted SBA-15 Mesoporous Silica. J. Phys. Chem. B 2001, 105, 8356–8360. [Google Scholar] [CrossRef]
  63. Ramanathan, A.; Castro Villalobos, M.; Kwakernaak, C.; Telalovic, S.; Hanefeld, U. Zr-TUD-1: A Lewis Acidic, Three-Dimensional, Mesoporous, Zirconium-Containing Catalyst. Chem. Eur. J. 2008, 14, 961–972. [Google Scholar] [CrossRef] [PubMed]
  64. Zhu, H.; Maheswari, R.; Ramanathan, A.; Subramaniam, B. Evaporation-Induced Self-Assembly of Mesoporous Zirconium Silicates with Tunable Acidity and Facile Catalytic Dehydration Activity. Microporous Mesoporous Mater. 2016, 223, 46–52. [Google Scholar] [CrossRef]
  65. Barberis, P.; Merle-Méjean, T.; Quintard, P. On Raman Spectroscopy of Zirconium Oxide Films. J. Nucl. Mater. 1997, 246, 232–243. [Google Scholar] [CrossRef]
  66. Kontoyannis, C.G.; Orkoula, M. Quantitative Determination of the Cubic, Tetragonal and Monoclinic Phases in Partially Stabilized Zirconias by Raman Spectroscopy. J. Mater. Sci. 1994, 29, 5316–5320. [Google Scholar] [CrossRef]
  67. Morrow, B.A.; McFarlan, A.J. Infrared and Gravimetric Study of an Aerosil and a Precipitated Silica using Chemical and Hydrogen/Deuterium Exchange Probes. Langmuir 1991, 7, 1695–1701. [Google Scholar] [CrossRef]
  68. Miller, J.B.; Ko, E.I. Acidic Properties of Silica-Containing Mixed Oxide Aerogels: Preparation and Characterization of Zirconia–Silica and Comparison to Titania–Silica. J. Catal. 1996, 159, 58–68. [Google Scholar] [CrossRef]
  69. Flego, C.; Carluccio, L.; Rizzo, C.; Perego, C. Synthesis of Mesoporous SiO2–ZrO2 Mixed Oxides by Sol–Gel Method. Catal. Commun. 2001, 2, 43–48. [Google Scholar] [CrossRef]
  70. Hadjiivanov, K.; Lavalley, J.C. FT–IR Spectroscopic Study of CO Adsorption on Monoclinic Zirconia of Different Hydroxylation Degrees. Catal. Commun. 2001, 2, 129–133. [Google Scholar] [CrossRef]
  71. Morterra, C.; Cerrato, G.; Di Ciero, S. IR Study of the Low Temperature Adsorption of CO on Tetragonal Zirconia and Sulfated Tetragonal Zirconia. Appl. Surf. Sci. 1998, 126, 107–128. [Google Scholar] [CrossRef]
  72. Paukshtis, E.A.; Yurchenko, E.N. Study of the Acid–Base Properties of Heterogeneous Catalysts by Infrared Spectroscopy. Russ. Chem. Rev. 1983, 52, 242–258. [Google Scholar] [CrossRef]
  73. Trukhan, N.N.; Panchenko, A.A.; Roduner, E.; Melgunov, M.S.; Kholdeeva, O.A.; Mrowiec-Bialon, J.; Jarzebski, A.B. FTIR Spectroscopic Study of Titanium-Containing Mesoporous Silicate Materials. Langmuir 2005, 21, 10545–10554. [Google Scholar] [CrossRef]
  74. Zecchina, A.; Bordiga, S.; Spoto, G.; Marchese, I.; Petrini, G.; Leofanti, G.; Padovan, M. Silicalite Characterization. 2. IR Spectroscopy of the Interaction of Carbon Monoxide with Internal and External Hydroxyl Groups. J. Phys. Chem. 1992, 96, 4991–4997. [Google Scholar] [CrossRef]
  75. Yamaguchi, T.; Morita, T.; Salama, T.M.; Tanabe, K. Surface properties of ZrO2 dispersed on SiO2. Catal. Lett. 1990, 4, 1–6. [Google Scholar] [CrossRef]
  76. Chen, L.F.; Zhou, X.L.; Norena, L.E.; Wang, J.A.; Navarrete, J.; Salas, P.; Montoya, A.; Del Angel, P.; Llanos, M.E. Comparative Studies of Zr-Based MCM-41 and MCM-48 Mesoporous Molecular Sieves: Synthesis and Physicochemical Properties. Appl. Surf. Sci. 2006, 253, 2443–2451. [Google Scholar] [CrossRef]
  77. Ramanathan, A.; Subramaniam, B.; Maheswari, R.; Hanefeld, U. Synthesis and Characterization of Zirconium Incorporated Ultra Large Pore Mesoporous Silicate, Zr–KIT-6. Micropor. Mesopor. Mater. 2013, 167, 207–212. [Google Scholar] [CrossRef]
  78. Vasudevan, S.V.; Cai, J.; Bu, Q.; Mao, H. Ordered Mesoporous Zirconium Silicates as a Catalyst for Biofuel Precursors Synthesis. Mol. Catal. 2021, 516, 112003. [Google Scholar] [CrossRef]
  79. Nash, C.P.; Ramanathan, A.; Ruddy, D.A.; Behl, M.; Gjersing, E.; Griffin, M.; Zhu, H.; Subramaniam, B.; Schaidle, J.A.; Hensley, J.E. Mixed Alcohol Dehydration over Brønsted and Lewis Acidic Catalysts. Appl. Catal. A Gen. 2016, 510, 110–124. [Google Scholar] [CrossRef] [Green Version]
  80. Ivanchikova, I.D.; Skobelev, I.Y.; Maksimchuk, N.V.; Paukshtis, E.A.; Shashkov, M.V.; Kholdeeva, O.A. Toward Understanding the Unusual Reactivity of Mesoporous Niobium Silicates in Epoxidation of C=C Bonds with Hydrogen Peroxide. J. Catal. 2017, 356, 85–99. [Google Scholar] [CrossRef]
  81. Soltanov, R.I.; Paukshtis, E.A.; Yurchenko, E.N. IK-Study of Thermodynamic Characteristics of Carbon Monoxide Interaction with the Surface of Some Oxide Adsorbents. Kinet. Catal. 1982, 23, 164–170. [Google Scholar]
  82. Zalomaeva, O.V.; Evtushok, V.Y.; Ivanchikova, I.D.; Glazneva, T.S.; Chesalov, Y.A.; Larionov, K.P.; Skobelev, I.Y.; Kholdeeva, O.A. Nucleophilic versus Electrophilic Activation of Hydrogen Peroxide over Zr-Based Metal–Organic Frameworks. Inorg. Chem. 2020, 59, 10634–10649. [Google Scholar] [CrossRef] [PubMed]
  83. Paukshtis, E.A.; Kotsarenko, N.S.; Karakchiev, L.G. Investigation of Proton-Acceptor Properties of Oxide Surfaces by IR Spectroscopy of Hydrogen-Bonded Complexes. React. Kinet. Catal. Lett. 1979, 12, 315–319. [Google Scholar] [CrossRef]
  84. Paukshtis, E.A. Infrared Spectroscopy in Heterogeneous Acid–Base Catalysis; Novosibirsk: Nauka, Russia, 1992; 253p. (In Russian) [Google Scholar]
  85. Sheldon, R.A.; Kochi, J.K. Metal–Catalyzed Oxidations of Organic Compounds; Academic Press: New York, NY, USA, 1981; 446p. [Google Scholar] [CrossRef]
  86. Maksimchuk, N.V.; Lee, J.S.; Solovyeva, M.V.; Cho, K.H.; Shmakov, A.N.; Chesalov, Y.A.; Chang, J.-S.; Kholdeeva, O.A. Protons Make Possible Heterolytic Activation of Hydrogen Peroxide over Zr-Based Metal-Organic Frameworks. ACS Catal. 2019, 9, 9699–9704. [Google Scholar] [CrossRef]
  87. Van Sickle, D.E.; Mayo, F.R.; Arluck, R.M. Liquid-Phase Oxidations of Cyclic Alkenes. J. Amer. Chem. Soc. 1965, 87, 4824–4832. [Google Scholar] [CrossRef]
  88. Botar, B.; Geletii, Y.V.; Kögerler, P.; Musaev, D.G.; Morokuma, K.; Weinstock, I.A.; Hill, C.L. The True Nature of the Di-iron(III) γ-Keggin Structure in Water: Catalytic Aerobic Oxidation and Chemistry of an Unsymmetrical Trimer. J. Amer. Chem. Soc. 2006, 128, 11268–11277. [Google Scholar] [CrossRef]
  89. Food Drug Administration. Rules and Regulations: Title 21—Food and Drugs, Food Additives, Synthetic Flavoring Substances and Adjuvants. Fed Regist 1973, 95, 12913. [Google Scholar]
  90. Bauer, K.; Garbe, D.; Surburg, H. Common Fragrance and Flavor Materials; Wiley-VCH: New York, NY, USA, 1997; 278p. [Google Scholar]
  91. Guidotti, M. Institute CNR-ISTM Internal Report; CNR-ISTM: Milan, Italy, 2018. [Google Scholar]
  92. Di Furia, F.; Modena, G. Mechanism of Oxygen Transfer from Peroxo Species. Pure Appl. Chem. 1982, 54, 1853–1866. [Google Scholar] [CrossRef]
Catalysts 12 00742 g001 550
Figure 1. Nitrogen adsorption–desorption isotherm and pore size distribution (inset) for Zr-EISA (a) sample A and (b) sample D.
Figure 1. Nitrogen adsorption–desorption isotherm and pore size distribution (inset) for Zr-EISA (a) sample A and (b) sample D.
Catalysts 12 00742 g001
Catalysts 12 00742 g002 550
Figure 2. Representative XRD patterns of calcined Zr-MMM-E (samples A and D).
Figure 2. Representative XRD patterns of calcined Zr-MMM-E (samples A and D).
Catalysts 12 00742 g002
Catalysts 12 00742 g003 550
Figure 3. DR UV–vis spectra of Zr-MMM-E (samples A–D) and Zr/SiO2.
Figure 3. DR UV–vis spectra of Zr-MMM-E (samples A–D) and Zr/SiO2.
Catalysts 12 00742 g003
Catalysts 12 00742 g004 550
Figure 4. Raman spectra of Zr-EISA samples A and D in comparison with the Zr-free SiO2-EISA matrix.
Figure 4. Raman spectra of Zr-EISA samples A and D in comparison with the Zr-free SiO2-EISA matrix.
Catalysts 12 00742 g004
Catalysts 12 00742 g005 550
Figure 5. TEM data for samples A (a) and D (b): TEM-images, HAADF-STEM images and corresponding EDX-mapping patterns showing distribution of Si (blue) and Zr (red) in selected regions.
Figure 5. TEM data for samples A (a) and D (b): TEM-images, HAADF-STEM images and corresponding EDX-mapping patterns showing distribution of Si (blue) and Zr (red) in selected regions.
Catalysts 12 00742 g005
Catalysts 12 00742 g006 550
Figure 6. (a) HAADF-STEM image of sample A; (b) HRTEM image of sample D and HAADF-STEM image of the marked region shown in inset. The marks on HAADF-STEM images indicate the location of highly dispersed Zr-species.
Figure 6. (a) HAADF-STEM image of sample A; (b) HRTEM image of sample D and HAADF-STEM image of the marked region shown in inset. The marks on HAADF-STEM images indicate the location of highly dispersed Zr-species.
Catalysts 12 00742 g006
Catalysts 12 00742 g007 550
Figure 7. (a) FTIR spectra of samples A and D at room temperature in the absorption region of hydroxyl groups and (b) differential FTIR spectra of OH groups after CO adsorption on samples A and D.
Figure 7. (a) FTIR spectra of samples A and D at room temperature in the absorption region of hydroxyl groups and (b) differential FTIR spectra of OH groups after CO adsorption on samples A and D.
Catalysts 12 00742 g007
Catalysts 12 00742 g008 550
Figure 8. Differential FTIR spectra of CO adsorbed on (a) sample A and (b) sample D at −196 °C and a pressure of 0.1–3 Torr.
Figure 8. Differential FTIR spectra of CO adsorbed on (a) sample A and (b) sample D at −196 °C and a pressure of 0.1–3 Torr.
Catalysts 12 00742 g008
Catalysts 12 00742 g009 550
Figure 9. FTIR spectra of deuterochloroform adsorbed on samples A and D.
Figure 9. FTIR spectra of deuterochloroform adsorbed on samples A and D.
Catalysts 12 00742 g009
Catalysts 12 00742 sch001 550
Scheme 1. Cyclohexene oxidation pathways: (A) heterolytic (with metal-peroxo species) giving primarily epoxide-relevant products and (B) homolytic (radical-mediated) with mostly allylic oxidation products.
Scheme 1. Cyclohexene oxidation pathways: (A) heterolytic (with metal-peroxo species) giving primarily epoxide-relevant products and (B) homolytic (radical-mediated) with mostly allylic oxidation products.
Catalysts 12 00742 sch001
Catalysts 12 00742 sch002 550
Scheme 2. Oxidation of trans-caryophyllene with H2O2 over Zr-silicates.
Scheme 2. Oxidation of trans-caryophyllene with H2O2 over Zr-silicates.
Catalysts 12 00742 sch002
Catalysts 12 00742 g010 550
Figure 10. Comparison of catalytic performances of Zr-MMM-E, Nb-MMM-E and Ti-MMM-E in CP epoxidation with H2O2: kinetic curves for (a) CP consumption and (b) CP epoxide yield. Reaction conditions: CP 0.1 mmol, H2O2 0.2 mmol, catalyst (0.005 mmol Zr, Nb or Ti), CH3CN 1 mL, 50 °C.
Figure 10. Comparison of catalytic performances of Zr-MMM-E, Nb-MMM-E and Ti-MMM-E in CP epoxidation with H2O2: kinetic curves for (a) CP consumption and (b) CP epoxide yield. Reaction conditions: CP 0.1 mmol, H2O2 0.2 mmol, catalyst (0.005 mmol Zr, Nb or Ti), CH3CN 1 mL, 50 °C.
Catalysts 12 00742 g010
Catalysts 12 00742 sch003 550
Scheme 3. Oxidation of methyl phenyl sulfide with H2O2 over Zr-silicates.
Scheme 3. Oxidation of methyl phenyl sulfide with H2O2 over Zr-silicates.
Catalysts 12 00742 sch003
Catalysts 12 00742 sch004 550
Scheme 4. Tentative mechanism of CP and MPS oxidation with H2O2 over Zr-silicate.
Scheme 4. Tentative mechanism of CP and MPS oxidation with H2O2 over Zr-silicate.
Catalysts 12 00742 sch004
Catalysts 12 00742 g011 550
Figure 11. Comparison of catalytic activity of Zr-MMM-E, Nb-MMM-E and Ti-MMM-E in (a) H2O2 decomposition (reaction conditions: H2O2 0.4 M, catalyst 0.016 mmol of Zr, Nb or Ti, 70 °C, CH3CN 5 mL) and (b) CyH oxidation (reaction conditions as in Table 2, catalyst 0.003 mmol of Zr, Nb or Ti).
Figure 11. Comparison of catalytic activity of Zr-MMM-E, Nb-MMM-E and Ti-MMM-E in (a) H2O2 decomposition (reaction conditions: H2O2 0.4 M, catalyst 0.016 mmol of Zr, Nb or Ti, 70 °C, CH3CN 5 mL) and (b) CyH oxidation (reaction conditions as in Table 2, catalyst 0.003 mmol of Zr, Nb or Ti).
Catalysts 12 00742 g011
Catalysts 12 00742 g012 550
Figure 12. Effect of reaction products on CyH oxidation with H2O2 over Zr-MMM-E (sample A) and 1 equiv of HClO4. Reaction conditions: CyH 0.1 mmol, catalyst 10 mg (0.003 mmol Zr), H2O2 (30% aq.) 0.1 mmol, HClO4 0.003 mmol, CH3CN 1 mL, 50 °C. Additives: 0.02 mmol of CyH-epoxide or 0.015 mmol of CyH-diol or 0.3 mmol of H2O (added in the beginning of the reaction).
Figure 12. Effect of reaction products on CyH oxidation with H2O2 over Zr-MMM-E (sample A) and 1 equiv of HClO4. Reaction conditions: CyH 0.1 mmol, catalyst 10 mg (0.003 mmol Zr), H2O2 (30% aq.) 0.1 mmol, HClO4 0.003 mmol, CH3CN 1 mL, 50 °C. Additives: 0.02 mmol of CyH-epoxide or 0.015 mmol of CyH-diol or 0.3 mmol of H2O (added in the beginning of the reaction).
Catalysts 12 00742 g012
Catalysts 12 00742 g013 550
Figure 13. Effect of reaction products on CP oxidation with H2O2 over Zr-MMM-E (samples A and D). Reaction conditions: CP 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), H2O2 (30% aq.) 0.2 mmol, CH3CN 1 mL, 50 °C. Additive: 0.02 mmol of CP epoxide (added in the beginning of the reaction).
Figure 13. Effect of reaction products on CP oxidation with H2O2 over Zr-MMM-E (samples A and D). Reaction conditions: CP 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), H2O2 (30% aq.) 0.2 mmol, CH3CN 1 mL, 50 °C. Additive: 0.02 mmol of CP epoxide (added in the beginning of the reaction).
Catalysts 12 00742 g013
Catalysts 12 00742 g014 550
Figure 14. Effect of reaction products on MPS oxidation with H2O2 over Zr-MMM-E (sample D). Reaction conditions: MPS 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), H2O2 (30% aq.) 0.1 mmol, CH3CN 1 mL, 60 °C. Additives: 0.02 mmol of MPSO or MPSO2 (added in the beginning of the reaction).
Figure 14. Effect of reaction products on MPS oxidation with H2O2 over Zr-MMM-E (sample D). Reaction conditions: MPS 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), H2O2 (30% aq.) 0.1 mmol, CH3CN 1 mL, 60 °C. Additives: 0.02 mmol of MPSO or MPSO2 (added in the beginning of the reaction).
Catalysts 12 00742 g014
Catalysts 12 00742 g015 550
Figure 15. XRD patterns of samples (a) A and (b) D: initial and after treatment with H2O2 in MeCN.
Figure 15. XRD patterns of samples (a) A and (b) D: initial and after treatment with H2O2 in MeCN.
Catalysts 12 00742 g015
Catalysts 12 00742 g016 550
Figure 16. Hot catalyst filtration test for (a) CP and (b) MPS oxidation with H2O2 in the presence of Zr-MMM-E (sample D). Reaction conditions: MPS 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), H2O2 (30% aq.) 0.22 mmol, CH3CN 1 mL, 60 °C.
Figure 16. Hot catalyst filtration test for (a) CP and (b) MPS oxidation with H2O2 in the presence of Zr-MMM-E (sample D). Reaction conditions: MPS 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), H2O2 (30% aq.) 0.22 mmol, CH3CN 1 mL, 60 °C.
Catalysts 12 00742 g016
Catalysts 12 00742 g017 550
Figure 17. Reuse of sample D in (a) CP and (b) MPS oxidation with H2O2. Reaction conditions: (a) CP 0.1 mmol, H2O2 (30% aq.) 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), CH3CN 1 mL, 50 °C; (b) MPS 0.1 mmol, H2O2 (30% aq.) 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), CH3CN 1 mL, 60 °C. TOF = (moles of substrate consumed)/(moles of Zr × time).
Figure 17. Reuse of sample D in (a) CP and (b) MPS oxidation with H2O2. Reaction conditions: (a) CP 0.1 mmol, H2O2 (30% aq.) 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), CH3CN 1 mL, 50 °C; (b) MPS 0.1 mmol, H2O2 (30% aq.) 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), CH3CN 1 mL, 60 °C. TOF = (moles of substrate consumed)/(moles of Zr × time).
Catalysts 12 00742 g017
Table
Table 1. Elemental analysis data and textural characteristics of Zr-silicates.
Table 1. Elemental analysis data and textural characteristics of Zr-silicates.
CatalystZr, a wt%Zr(acac)4:HCl bSBET, m2/gVp, c cm3/gDp, d nm
A2.461:09950.623.8
B2.331:113180.613.6
C2.431:213760.583.5
D2.501:714040.623.1
Zr/SiO21.91- e4080.662.0–8.0 f
a Based on elemental analysis data for calcined samples. b Molar ratio of Zr(acac)4 and extra HCl. c Mesopore volume. d Average pore diameter. e Zirconium was introduced as Zr(Cp)2Cl2 precursor. f Broad distribution of mesopores with a maximum at 4.9 nm.
Table
Table 2. Cyclohexene oxidation with H2O2 in the presence of various Zr-Si catalysts a.
Table 2. Cyclohexene oxidation with H2O2 in the presence of various Zr-Si catalysts a.
EntryCatalystTime, b hCyH conv., %Product Selectivity, c %
EpoxideDiolAllylic d
1 e-1.56161665
2 fH+1.59432128
3A1.57311539
4A + H+0.32774194
5 gA + H+0.32778154
6 hA + NaOAc14252526
7B37311531
8B + H+0.52370226
9C4633934
10C + H+0.32566284
11D28311326
12D + H+0.32973174
13Zr/SiO21.58251938
14Zr/SiO2 + H+0.32167245
a Reaction conditions: CyH 0.1 mmol, catalyst 10 mg (0.003 mmol Zr), H2O2 (30% aq.) 0.1 mmol, HClO4 0.003 mmol (if added), CH3CN 1 mL, 50 °C. b Optimal reaction time to reach the maximum selectivity and conversion. c Based on substrate consumed. d Sum of allylic oxidation products (HP + enol + enone). e No catalyst was present. f 0.003 mmol HClO4. g 77% aq. H2O2 was used as oxidant. h 0.003 mmol of NaOAc was added.
Table
Table 3. Cyclooctene oxidation with H2O2 in the presence of Zr-Si catalysts a.
Table 3. Cyclooctene oxidation with H2O2 in the presence of Zr-Si catalysts a.
CatalystTime, hCyOct conv., %Selectivity to Epoxide, b %
A21331
52719
A + H+ c22814
D22050
54038
Zr/SiO221839
53928
a Reaction conditions: CyOct 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), H2O2 (30% aq.) 0.2 mmol, CH3CN 1 mL, 50 °C. b Based on substrate consumed. c HClO4 0.005 mmol.
Table
Table 4. Caryophyllene oxidation with H2O2 in the presence of Zr-Si catalysts a.
Table 4. Caryophyllene oxidation with H2O2 in the presence of Zr-Si catalysts a.
CatalystTime, hCP conv, %Selectivity to Epoxide, b %
A24078
56978
D26376
58777
Dc,d24575
56470
Zr/SiO223778
56580
UiO-67 e44492
a Reaction conditions: CP 0.1 mmol, catalyst 20 mg (0.005 mmol Zr), H2O2 (30% aq.) 0.2 mmol, CH3CN 1 mL, 50 °C. b Yield of endocyclic monoepoxide based on substrate consumed. c H2O2 0.1 mmol. d H2O2 efficiency 90%. e catalyst 2 mg (0.007 mmol Zr), H2O2 0.1 mmol, CH3CN 1 mL, 50 °C (data taken from ref. [53]).
Table
Table 5. Methyl phenyl sulfide oxidation with H2O2 in the presence of Zr-Si catalysts a.
Table 5. Methyl phenyl sulfide oxidation with H2O2 in the presence of Zr-Si catalysts a.
CatalystTime, b hMPS conv, %Product Selectivity, c %H2O2 Efficiency, d %
MPSOMPSO2
A251267489
B1.555366490
C1.555366490
D157376393
Zr/SiO20.553386286
a Reaction conditions: MPS 0.1 mmol, catalyst 5 mg (0.0013 mmol Zr), H2O2 (30% aq.) 0.1 mmol, CH3CN 1 mL, 60 °C. b Optimal reaction time to reach the maximum selectivity and conversion. c Based on substrate consumed. d H2O2 utilization efficiency = total yield of products based on the oxidant consumed.
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Ivanchikova, I.D.; Zalomaeva, O.V.; Maksimchuk, N.V.; Stonkus, O.A.; Glazneva, T.S.; Chesalov, Y.A.; Shmakov, A.N.; Guidotti, M.; Kholdeeva, O.A. Alkene Epoxidation and Thioether Oxidation with Hydrogen Peroxide Catalyzed by Mesoporous Zirconium-Silicates. Catalysts 2022, 12, 742. https://doi.org/10.3390/catal12070742

AMA Style

Ivanchikova ID, Zalomaeva OV, Maksimchuk NV, Stonkus OA, Glazneva TS, Chesalov YA, Shmakov AN, Guidotti M, Kholdeeva OA. Alkene Epoxidation and Thioether Oxidation with Hydrogen Peroxide Catalyzed by Mesoporous Zirconium-Silicates. Catalysts. 2022; 12(7):742. https://doi.org/10.3390/catal12070742

Chicago/Turabian Style

Ivanchikova, Irina D., Olga V. Zalomaeva, Nataliya V. Maksimchuk, Olga A. Stonkus, Tatiana S. Glazneva, Yurii A. Chesalov, Alexander N. Shmakov, Matteo Guidotti, and Oxana A. Kholdeeva. 2022. "Alkene Epoxidation and Thioether Oxidation with Hydrogen Peroxide Catalyzed by Mesoporous Zirconium-Silicates" Catalysts 12, no. 7: 742. https://doi.org/10.3390/catal12070742

APA Style

Ivanchikova, I. D., Zalomaeva, O. V., Maksimchuk, N. V., Stonkus, O. A., Glazneva, T. S., Chesalov, Y. A., Shmakov, A. N., Guidotti, M., & Kholdeeva, O. A. (2022). Alkene Epoxidation and Thioether Oxidation with Hydrogen Peroxide Catalyzed by Mesoporous Zirconium-Silicates. Catalysts, 12(7), 742. https://doi.org/10.3390/catal12070742

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop