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Article

Three-Dimensional Hierarchical Hydrotalcite–Silica Sphere Composites as Catalysts for Baeyer–Villiger Oxidation Reactions Using Hydrogen Peroxide

by
Daniel Cosano
*,
Dolores Esquivel
,
Francisco J. Romero-Salguero
,
César Jiménez-Sanchidrián
and
José Rafael Ruiz
*
Departamento de Química Orgánica, Facultad de Ciencias, Campus de Rabanales, Instituto Universitario de Investigación en Química Fina y Nanoquímica IUNAN, Universidad de Córdoba, Edificio Marie Curie, 14071 Córdoba, Spain
*
Authors to whom correspondence should be addressed.
Catalysts 2022, 12(6), 629; https://doi.org/10.3390/catal12060629
Submission received: 16 May 2022 / Revised: 2 June 2022 / Accepted: 7 June 2022 / Published: 8 June 2022
(This article belongs to the Special Issue Nano-Porous Materials for Catalytic Systems in Green Chemistry Processes)
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Abstract

:
The development of effective, environmentally friendly catalysts for the Baeyer–Villiger reaction is becoming increasingly important in applied catalysis. In this work, we synthesized a 3D composite consisting of silica spheres coated with Mg/Al hydrotalcite with much better textural properties than its 2D counterparts. In fact, the 3D solid outperformed a 2D-layered hydrotalcite as catalyst in the Baeyer–Villiger reaction of cyclic ketones with H2O2/benzonitrile as oxidant. The 3D catalyst provided excellent conversion and selectivity; it was also readily filtered off the reaction mixture. The proposed reaction mechanism, which involves adsorption of the reactants on the hydrotalcite surface, is consistent with the catalytic activity results.

1. Introduction

One of the major aims of Green Chemistry is successfully combining the use of environmentally friendly reagents and heterogeneous catalysts [1] and one of the processes that has been successfully adapted to its requirements is the Baeyer–Villiger reaction, by which a ketone is oxidized to an ester with an organic peroxide. The original reaction developed by Baeyer and Villiger [2] involved treating menthone and carvomenthone with a mixture of potassium monopersulfate and sulfuric acid (see Scheme 1a). Since then, the reaction has been the subject of much research and conducted with a variety of reagents and catalysts [3,4,5,6,7]. The reaction takes place in two steps (Scheme 1b), the first involving a nucleophilic attack of the oxygen atom in the peracid on the carbonyl group of the ketone to form a Criegee adduct. In the second step, the adduct rearranges to the corresponding ester and a carboxylic acid is formed as a by-product. Hazardous reagents, which additionally lead to unwanted by-products, can be avoided by using hydrogen peroxide in the presence of a solid catalyst as oxidant. A variety of catalysts have been used for this purpose [6,7] including layered double hydroxides (LDHs), also known as hydrotalcite-like compounds or, simply, “hydrotalcites” (HTs) [8,9,10,11,12]. Our group has ample experience in the use of HTs [13,14,15] and structurally similar solids [16,17].
Hydrotalcites are a family of natural and synthetic products structurally consisting of brucite-like layers (viz., Mg(OH)6 octahedra) and exchangeable anions in their interlayer region. Their general formula is M(II)1−xM(III)x[(OH)2]x+[Xn/x]n−·mH2O, where M(II) is a divalent metal, M(III) a trivalent metal and X the interlayer anion [18,19]. Replacing M(II) with M(III) in brucite-like layers produces a charge deficiency that is offset by interlayer anions, whether inorganic or organic [20]. So, a widely variable chemical composition also results in variable physicochemical properties that have promoted extensive use HTs in a number of scientific fields [21,22,23,24,25].
Although hydrotalcites are easily prepared, the methods typically used to obtain them (viz., coprecipitation and hydrothermal synthesis) produce poorly crystalline two-dimensional solids. Hydrotalcites used as catalysts in the Baeyer–Villiger reaction usually require a nitrile to combine with hydrogen peroxide on their surface to form a peroxycarboximidic acid—the actual oxidant [13,14]. In this form, however, the catalytic process only occurs on the outer surface of the hydrotalcite. Therefore, improving HT activity entails increasing the active surface.
New synthetic methods have allowed hierarchical three-dimensional (3D) hydrotalcites to be developed for a number of uses such as nanotechnological applications [26,27,28]. The new family of materials includes hydrotalcite–silica composites [29,30,31,32]. Silica nanostructures consist of orderly frameworks [33] that allow the position of silicon atoms to be changed in order to obtain specific forms such as nanospheres, nanotubes or nanowires [34]. Silica has a nonporous surface with a 3D network of silanol (Si–OH) and siloxane (Si–O) groups. Silica particles aggregate through interaction between their silanol groups and create negative surface charge [35]; as a result, they can in theory be used as nucleation sites for HT growth. SiO2@HT hierarchical structures are usually prepared layer-by-layer or by in situ growth [36]; the latter method involves coprecipitation from a suspension of structured silica. In previous work [37], our group reported the synthesis and structural characterization of silica microspheres coated with Mg/Al hydrotalcite layers. In this work, we used them as catalysts in the Baeyer–Villiger oxidation of cyclic ketones with hydrogen peroxide.

2. Results and Discussion

2.1. Characterization of Catalysts

Table 1 shows the mole ratios of the SiO2@HT. As can be seen, the Mg/Al ratio was close to its theoretical value of 2, and so were the Si/Mg and Si/Al ratios to theirs. The table additionally shows the surface Mg/Al ratio as determined by XPS (entry 4). This ratio was lower than the total value, which is consistent with previous results of our group for hydrotalcites containing Mg and Al in variable proportions [38]. The elemental analysis and thermogravimetric results (Figure S5) were used to determine the formula of the resulting hydrotalcite, which was Mg0.657Al0.343(OH)2(A)0.172·0.58H2O (where (A) is the interlaminar anion), and also that the catalysts consisted of 57.1 wt% hydrotalcite and 32.9 wt% SiO2.
As noted earlier, similar solids were examined structurally in previous work. However, Figures S1–S4 show the results for the synthetic processes conducted here. As can be seen, the catalyst was successfully synthesized here as well.
SiO2@HT was for the first time characterized in textural terms in this work. The specific surface area, cumulative pore volume and pore size distribution of a catalyst are highly influential on its activity. Nitrogen adsorption–desorption measurements were made in two solids. Figure 1a shows the resulting isotherm and the textural parameters derived from it. The surface area of SiO2@HT was much higher than that of 2D layered hydrotalcites (Figure S5), which is typically around 70 m2/g; also, it clearly exceeded that of silica microspheres (ca. 20 m2/g). The isotherm was type IV in IUPAC’s classification [39] and exhibited a well-defined hysteresis cycle over the range 0.4 < P/P0 < 1, suggesting the presence of mesopores. This was confirmed by the average pore diameter (ca. 10 nm) and the fact that it spanned a narrow range (i.e., that the pore size distribution was rather uniform). Furthermore, the hysteresis cycle was H2 type [39]. This is usually the case with porous sorbents such as inorganic oxide gels and porous glasses, which, however, have a more poorly defined pore size and shape. In fact, H2 cycles are especially difficult to interpret. Until a few decades ago, they were ascribed to a difference in mechanism between condensation and evaporation in pores with wide bodies but thin necks—often referred to as “ink-bottle pores”; at present, however, this is regarded as an oversimplified interpretation that ignores lattice effects.

2.2. Baeyer–Villiger Reaction

2.2.1. Kinetics of the Process

The Baeyer–Villiger reaction studied here was the oxidation of cyclohexanone to ε-caprolactone with hydrogen peroxide and benzonitrile at different temperatures. The optimum working conditions were established by following a kinetic procedure involving plotting the natural logarithm of the lactone concentration as a function of time. The plot was a straight line, which suggests first-order kinetics in the cyclohexanone concentration obeying the following law:
ln (c0/c) = k·t,
where c0 and c are the cyclohexanone concentrations at times zero and t, respectively; k is the rate constant and t time. A plot of ln (c0/c) versus t thus gave the rate constant.
The influence of temperature on the reaction was examined over the range 40–90 °C. The results are shown in Table 2, entries 1–4, and the corresponding Arrhenius plot in Figure 2. As can be seen from the figure, a straight line was obtained, the slope of which allowed an activation energy of 19.40 kcal/mol to be calculated. Based on these results, we chose 90 °C as the optimum reaction temperature.
This determination was followed by blank tests intended to confirm that the reaction developed to no appreciable extent in the absence of catalyst and also that a nitrile was absolutely necessary for it to occur. The reaction also failed to develop (entries 5–7 in Table 2) in the absence of catalyst or nitrile, or in the presence of uncoated silica (SP-SiO2). Therefore, the catalyst was indispensable. Finally, the catalyst (SiO2@HT) was confirmed to be more active than a conventional 2D hydrotalcite by using one with an Mg/Al ratio of 2 similar to those used in previous studies [13,14,15]. Based on the results (Table 2, entry 8), the rate constant was four times higher with the 3D catalyst than with the 2D hydrotalcite.
To evaluate the catalytic performance of the 3D catalyst, comparisons with different materials were also made and the results are shown in Table S1. It was found that the catalyst had comparable or even better performance, indicating that it has a good catalytic performance.

2.2.2. Reaction Mechanism

The Baeyer–Villiger reaction of a cyclic ketone with a nitrile on a catalyst consisting of hydrotalcite-coated silica microspheres should take place through a mechanism similar to that observed with 2D layered hydrotalcites [13] (i.e., on the surface of the catalyst as shown in Scheme 2). Thus, the SiO2@HT catalyst initially adsorbs hydrogen peroxide at surface basic sites to form an unstable hydroperoxide species that attacks nitrile molecules to form a peroxycarboximidic acid—the actual oxidant. Then, the nucleophilic oxygen in the carbonyl group of the ketone is adsorbed on an electrophilic metal site of the catalyst for attack by the acid to form a Criegee-like adduct similar to those forming in homogeneous catalysis processes. Finally, the adduct rearranges to the lactone. Therefore, the improving textural properties of 3D hydrotalcite involved an increase of Brønsted basic centers (surface hydroxyl groups), which favor the formation of unstable hydroperoxide species [8,9,40,41,42,43].

2.2.3. Baeyer–Villiger Oxidation of Cyclic Lactones

Once the optimum working conditions were established, the reaction was extended to other cyclic ketones (Table 3). Most were converted to their lactones with high selectivity and conversion. Ring size was very strongly influential on conversion and reaction rate. If only the ketone adsorption step is considered, then there should be little difference between the lactones with five to seven rings (Scheme 3a). By contrast, adsorption of cyclooctanone should be more markedly hindered and its reaction slower as a result—which was indeed the case, judging from entry 4 in Table 3. In addition, the reaction rate decreased with increasing ring size from five to seven carbon atoms (Table 3, entries 1–3). Based on adsorption provisions alone, the differences should not be too large, however. Therefore, they must depend on the ease with which a five-membered ring can be expanded to a six-membered ring (e.g., from cyclopentanone to cyclohexanone). Cyclohexanone is less easily expanded to a seven-membered lactone ring, so its reaction rate should also be lower. This is especially so with cycloheptanone. In fact, the seven-membered ring was difficult to cleave and reacted at a lower rate. Expanding cyclooctanone to a nine-membered ring is even more difficult, which, together with its more sterically hindered adsorption, led to its reaction being much slower than with the previous ketones.
The influence of the ease of ketone adsorption onto the catalyst on the reaction rate was examined by using cyclohexanones bearing a methyl substituent at position 2, 3 or 4 (Scheme 3b; Table 3, entries 5–7). The substituent at 2 strongly hindered adsorption of the substrate and considerably reduced the reaction rate as a result. Steric hindrance was less marked with the substituent at 3, so the reaction rate was higher than with 2-methylcyclohexanone. Finally, there was virtually no steric hindrance from the substituent at position 4 and the resulting reaction rate was similar to that with cyclohexanone. A bulkier substituent again reduced the reaction rate by hindering adsorption of the cyclohexanone ring. Furthermore, 2- and 3-methylcyclohexanone have an asymmetric structure that can lead to two different products (see Scheme 4), thereby detracting from selectivity. In addition, the reaction rate of cyclohexanones bearing a substituent is more markedly influenced by their ease of ring expansion than by that of adsorption. This is immediately apparent if one compares the conversion and rate values for cycloheptanone and cyclooctanone (entries 3 and 4 in Table 3 with those for 2-methylcyclohexanome (entry 5), for example.
This section may be divided by subheadings. It should provide a concise and precise description of the experimental results, their interpretation, as well as the experimental conclusions that can be drawn.

3. Materials and Methods

3.1. Materials

3.1.1. Silica Microspheres

Silica microspheres were obtained according to Stöber [44]. A volume of 3.7 mL of tetraethyl orthosilicate (TEOS) was added to a solution containing 88 mL of ethanol and 12 mL of ammonia, the mixture being vigorously stirred at room temperature for 24 h. Then, the solid formed (SP-SiO2) was isolated by centrifugation, washed with 300 mL of ethanol and dried in a stove at 70 °C overnight.

3.1.2. Hydrotalcite-Coated Microspheres

Three-dimensional materials were obtained as described elsewhere [37]. A volume of 200 mL of an aqueous solution containing 10 mmol of Mg(NO3)2·6H2O and 5 mmol of Al(NO3)3·9H2O was added to 500 mL of an also aqueous suspension containing 0.5 g of silica microspheres that was previously sonicated for 90 min to facilitate dispersion. The addition time was 2 h and pH 9, kept constant by adding 1 M NaOH as required. Then, the composite formed (SiO2@HT) was filtered off and washed with bidistilled, de-ionized water.

3.1.3. Two-Dimensional Hydrotalcite

The 2D hydrotalcite used was prepared from solutions of Mg(NO3)2·6H2O and Al(NO3)3·9H2O in Mg (II)/Al(III) ratio of 2, using a coprecipitation method described elsewhere (ref). Typically, the mixture was slowly dropped over 500 mL of a solution of NaOH at pH 9 at 60 °C under vigorous stirring. Then, the material formed (HT-2D) was filtered off and washed with bidistilled, de-ionized water.

3.2. Characterization

The solids used were previously characterized in structural terms elsewhere [37]. However, the fact that the silica spheres were coated by hydrotalcite layers was confirmed with new analyses here. The results are shown in Figures S1–S4, Supplementary Materials. Those analyses were supplemented with others of texture including the determination of the Mg/Al, Si/Mg and Si/Al ratios by inductively coupled plasma mass spectrometry (ICP-MS). Samples were prepared on DigiPrep equipment, using Teflon vessels and a nitric acid medium at a programmed temperature for 90 min. The digestates thus obtained were diluted in 10% nitric acid for ICP-MS measurement. Elemental analyses were performed on a Perkin–Elmer NexION 350X ICP-MS instrument. Surface metal ratios were determined with a SPECS Phoibos HAS 3500 150 MCD X-ray photoelectron spectrometer (XPS) using a monochromatic Al anode (1486.7 eV). Accurate binding energies were determined relative to the position of Si 2p at 103.4 eV. Finally, moisture contents were determined by thermogravimetric analysis (TGA) on a Mettler Toledo balance. An air stream at 100 mL min−1 and a heating rate of 10 °C min−1 were used. The catalysts were characterized for texture by nitrogen adsorption–desorption porosimetry. Specific surface areas and pore size distributions were established with the Brunauer–Emmett–Teller (BET) and Barrett–Joyner–Halenda (BJH) methods, respectively. Nitrogen adsorption–desorption isotherms at −196 °C were obtained with an Autosorb-iQ MP/MP-XR instrument. All samples were outgassed at 60 °C overnight prior to measurement.

3.3. Reaction

Baeyer–Villiger reaction runs were performed at different temperatures in a two-neck flask containing 0.006 mol of cyclohexanone, 0.049 mol of nitrile, 0.05 mol of hydrogen peroxide and 0.1 g of catalyst. One of the neck’s mouths was fitted with a reflux condenser and the other was used for sampling at regular intervals. The reaction mixture was stirred throughout. Identical conditions were used in the reactions of the other cyclic ketones. Reaction products were identified from their retention times as measured with a Varian gas chromatograph equipped with a capillary column (VF-1MS, 15 m × 0.25 mm ID) and a flame ionization detector (FID).

4. Conclusions

A spherical hydrotalcite was obtained by coating silica microspheres with a layered double hydroxide. The resulting hierarchical 3D solid proved an excellent catalyst for the Baeyer–Villiger reaction of cyclic ketones with hydrogen peroxide and benzonitrile, which developed at a much higher rate than with a 2D hydrotalcite catalyst. As shown by the results, the reaction is strongly influenced by the adsorption of the ketone on the catalyst and the ease with which the ketone can undergo ring expansion. Thus, cyclopentanone exhibited the highest reaction rate because its adsorption was not being sterically hindered and its expansion to a six-membered lactone ring was quite easy. The reaction rate decreased with increasing ring size due to the increasing steric hindrance and decreasing ring expansion ability. The effect of steric hindrance was also apparent in cyclohexanones bearing a methyl substituent at position 2 or 3.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/catal12060629/s1, Figure S1: TG profiles for SiO2@HT (solid line) and SP-SiO2 (dashed line). Figure S2: XRD patterns for synthetized solids: HT-2D (a); SiO2 microspheres; (b) and SiO2@HT (c). Figure S3: µ-Raman spectra for synthetized solids: HT-2D (a); SiO2 microspheres (b) and SiO2@HT (c). Figure S4: TEM images for synthetized solids: (a) HT-2D; (b) SiO2 microspheres and (c) SiO2@HT. Figure S5: Nitrogen adsorption–desorption isotherm for (a) HT-2D and (b) SP-SiO2. Table S1: Comparison of the prepared catalysts with those reported recently [17,28,44,45,46,47,48,49,50,51,52].

Author Contributions

D.C. and J.R.R. carried out the research sampling and processing. D.C. and J.R.R. performed the data analysis and interpretation. Critical review of the manuscript was realised by D.E., F.J.R.-S. and C.J.-S. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by Spanish Ministry of Education and Science (Project RTI2018-101611-B-100).

Data Availability Statement

The authors declare that the manuscript is original and has not been submitted or published in any other journal, and the data in the manuscript is real.

Acknowledgments

The authors gratefully acknowledge funding by the Spanish Ministry of Education and Science (Project RTI2018-101611-B-100), D.C. acknowledges to 2014–2020 Social European Fund program of Andalusia (DOC_01376, FEDER).

Conflicts of Interest

The authors declare no conflict of interest.

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Catalysts 12 00629 sch001 550
Scheme 1. Baeyer-Villiger reaction (a) original reaction and (b) generally accepted mechanism [6].
Scheme 1. Baeyer-Villiger reaction (a) original reaction and (b) generally accepted mechanism [6].
Catalysts 12 00629 sch001
Catalysts 12 00629 g001 550
Figure 1. Nitrogen adsorption–desorption isotherm (a) and pore size distribution function (b) for the catalyst (SiO2@HT). SBET specific surface area; Vp cumulative pore volume; Dp average pore diameter.
Figure 1. Nitrogen adsorption–desorption isotherm (a) and pore size distribution function (b) for the catalyst (SiO2@HT). SBET specific surface area; Vp cumulative pore volume; Dp average pore diameter.
Catalysts 12 00629 g001
Catalysts 12 00629 g002 550
Figure 2. Arrhenius plot for the Baeyer–Villiger reaction of cyclohexanone on SiO2@HT.
Figure 2. Arrhenius plot for the Baeyer–Villiger reaction of cyclohexanone on SiO2@HT.
Catalysts 12 00629 g002
Catalysts 12 00629 sch002 550
Scheme 2. Reaction of Baeyer-Villiger catalyzed by SiO2@HT (a) Catalyst structure. (b) Mechanism for the Baeyer–Villiger reaction of cyclohexanone with benzonitrile and hydrogen peroxide on an HT layer in the catalyst.
Scheme 2. Reaction of Baeyer-Villiger catalyzed by SiO2@HT (a) Catalyst structure. (b) Mechanism for the Baeyer–Villiger reaction of cyclohexanone with benzonitrile and hydrogen peroxide on an HT layer in the catalyst.
Catalysts 12 00629 sch002
Catalysts 12 00629 sch003 550
Scheme 3. Structure of the cyclic ketones studied. (a) Difference between the cyclic ketones with five to seven rings (b) Difference between the cyclohexanones bearing a methyl substituent at position 2, 3 or 4.
Scheme 3. Structure of the cyclic ketones studied. (a) Difference between the cyclic ketones with five to seven rings (b) Difference between the cyclohexanones bearing a methyl substituent at position 2, 3 or 4.
Catalysts 12 00629 sch003
Catalysts 12 00629 sch004 550
Scheme 4. Intermediate adducts in the Baeyer–Villiger reaction of 2-, 3- and 4-methylcyclohexanone.
Scheme 4. Intermediate adducts in the Baeyer–Villiger reaction of 2-, 3- and 4-methylcyclohexanone.
Catalysts 12 00629 sch004
Table
Table 1. Theoretical and experimental element ratios for the catalyst (SiO2@HT) as determined by ICP-MS.
Table 1. Theoretical and experimental element ratios for the catalyst (SiO2@HT) as determined by ICP-MS.
EntryMolar RatioTheoreticalExperimental
1Mg/Al2.001.97
2Si/Mg0.830.85
3Si/Al1.671.67
4Mg/Al a-1.46
a Determined by XPS.
Table
Table 2. Influence of temperature on the Baeyer–Villiger oxidation of cyclohexanone with hydrogen peroxide a.
Table 2. Influence of temperature on the Baeyer–Villiger oxidation of cyclohexanone with hydrogen peroxide a.
Catalysts 12 00629 i001
EntryT (°C)Conversion (%) bk (min−1·gcat)·10−4 c
1907812.6
270557.7
355365
440222.7
5 d90301.9
6 e9000
7 f90281.7
8 g90393.1
a Reaction conditions: catalyst: 0.1 g; cyclohexanone = 6 mmol; hydrogen peroxide = 49 mmol; benzonitrile = 50 mmol; catalyst: 100 mg. b Conversion to ε-caprolactone (6 h); c rate constant; d reaction without catalyst; e reaction without nitrile; f reaction using SP-SiO2 as catalyst; g reaction using layered HT-2D as catalyst.
Table
Table 3. Structure, conversion, rate constant and selectivity in selected Baeyer–Villiger reactions.
Table 3. Structure, conversion, rate constant and selectivity in selected Baeyer–Villiger reactions.
EntryNamePubchem I.D.Formuleφ (%) ak (10−3) (min−1) bS (%) c
1Cyclohexanone108-94-1 Catalysts 12 00629 i0027812.6100
2Cycloheptanone502-42-1 Catalysts 12 00629 i003508.3100
3Cyclooctanone502-49-8 Catalysts 12 00629 i004423.199
42-Methylcyclohexanone583-60-8 Catalysts 12 00629 i005599.967
53-Methylcyclohexanone591-24-2 Catalysts 12 00629 i0066010.852
64-Methylcyclohexanone589-92-4 Catalysts 12 00629 i0077812.399
74-Ethylcyclohexanone5441-51-0 Catalysts 12 00629 i008548.7100
82-terc-butylcyclohexanone98-53-3 Catalysts 12 00629 i009526.4100
a Conversion to lactone (6 h); b rate constant; c selectivity to lactone (6 h).
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Cosano, D.; Esquivel, D.; Romero-Salguero, F.J.; Jiménez-Sanchidrián, C.; Ruiz, J.R. Three-Dimensional Hierarchical Hydrotalcite–Silica Sphere Composites as Catalysts for Baeyer–Villiger Oxidation Reactions Using Hydrogen Peroxide. Catalysts 2022, 12, 629. https://doi.org/10.3390/catal12060629

AMA Style

Cosano D, Esquivel D, Romero-Salguero FJ, Jiménez-Sanchidrián C, Ruiz JR. Three-Dimensional Hierarchical Hydrotalcite–Silica Sphere Composites as Catalysts for Baeyer–Villiger Oxidation Reactions Using Hydrogen Peroxide. Catalysts. 2022; 12(6):629. https://doi.org/10.3390/catal12060629

Chicago/Turabian Style

Cosano, Daniel, Dolores Esquivel, Francisco J. Romero-Salguero, César Jiménez-Sanchidrián, and José Rafael Ruiz. 2022. "Three-Dimensional Hierarchical Hydrotalcite–Silica Sphere Composites as Catalysts for Baeyer–Villiger Oxidation Reactions Using Hydrogen Peroxide" Catalysts 12, no. 6: 629. https://doi.org/10.3390/catal12060629

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