Thangaraj Baskarana,
Raju Kumaravela,
Jayaraj Christopherb and
Ayyamperumal Sakthivel*a
aDepartment of Chemistry, Inorganic Materials and Catalysis Laboratory, University of Delhi, India. E-mail: sakthiveldu@gmail.com; Tel: +91-8527103259
bIndian Oil Corporation Ltd, R&D Centre, Faridabad-121007, India
First published on 6th February 2014
Silicate intercalated CoAl hydrotalcite materials were synthesized (CoAl-HT-Si) and systematically characterized. The intercalated hydrotalcite materials lead to the formation of solid solutions of cobalt silicate and cobalt spinel structures, which have higher surface area and pore volume than pure CoAl-HT. The XPS studies revealed the presence of cobalt in divalent and trivalent oxidation states on the surface. The resultant materials were found to be promising catalysts for oxidation of various alcohols.
Here we report the synthesis of silicate anion intercalated cobalt-aluminium hydrotalcite as stable, effective heterogeneous catalysts for the oxidation of alcohols into aldehydes–ketones under mild conditions as green processes. A series of CoAl-HT and silicate anion intercalated samples were prepared according to modified literature and systematically characterized (Scheme 1).
Silicate anion intercalated HT was produced by introducing various concentrations of sodium silicate into pre-prepared HT. Silicate solutions of appropriate concentrations were added slowly to the HT gel at room temperature and stirred for 48 h. The silicate intercalated HT materials were then filtered and washed with deionized H2O. The intercalated HT samples prepared by using 1.42 and 2.03 M sodium silicate solutions are represented by CA-Si4 and CA-Si6, respectively and these samples calcined at 400 °C for 6 h in air. Further, attempts were made to retain the layered structure on silicate anion intercalated CoAl-HT by crystallizing the interlayer silicate anion species using a dry gel method. Approximately 1.5 g of as-synthesized CA-Si6 was wetted with the help of a calculated amount of 40% tetrapropylammonium hydroxide (TPAOH) solution. The resultant solid cake was allowed to crystallize at 175 °C for 72 h. The TPAOH was removed by calcination at 550 °C in air for 6 h. The interlayer silicate anion crystallized sample synthesized using CA-Si6 with TPAOH is represented as CA-Si6S. For the reference, CoAl2O4 prepared by solid state mixing of corresponding salts followed by calcination at 600 °C in air for 6 h.
X-ray photoelectron spectra (XPS) of the catalysts were recorded with custom built ambient pressure photoelectron spectrometer (APPES) (Prevac, Poland), equipped with VG Scienta's R3000HP analyzer and MX650 monochromator.27 Monochromatic Al Kα X-ray was generated at 450 W and used for measuring X-ray photoelectron spectrum (XPS) of the above samples. Base pressure in the analysis chamber was maintained in the range of 2 × 10−10 Torr. The energy resolution of the spectrometer was set at 0.7 eV at a pass energy of 50 eV. Binding energy (BE) was calibrated with respect to Au 4f7/2 core level at 84.0 eV. The error in the reported BE values is within 0.1 eV. The acidity of materials were studied as per the literature procedure28 by pyridine vapour adsorption, which was carried out in a Harrick Scientific HVC-DR2 reaction chamber with a detachable ZnSe window. About 100 mg (10% of sample was mixed with KBr) of sample was placed in the sample cup and was pre-activated at 350 °C for 6 h. Pyridine adsorption was done at 150 °C for 1 h under flowing helium. After attaining saturation desorption was done at different temperature. The amount of soluble basic sites was determined by acid–base titration method.29 In this method 100 mg of pure and silicate intercalated HT samples were vigorously shaken with 10 ml water about 24 h in room temperature and catalyst was separated. The filtrate was neutralized with 0.05 M of HCl. The remaining acid was titrated with 0.1 M of standard NaOH. Elemental composition present in the final materials were determined using Wavelength Dispersive X-ray Fluorescence spectrometer (WDXRF; ZSX PRIMUS Primus, Rigaku). Calibration of the equipment was carried out using standards containing Co, Al & Si in different proportions. Net intensity (peak–background) of standards was used for calibration and Co, Al & Si contents in the catalyst samples were obtained from the calibration curve.
These results indicate that silicate anions were successfully intercalated between the brucite-like layers.26 After calcination, the FT-IR spectrum of CoAl-HT shows that a strong and sharp peak around 670 and 560 cm−1 indicates Co–O bonds of cobalt spinel (Co3O4).23,25,30 In silicate anion intercalated hydrotalcite, the relative intensity for the band 670 and 560 cm−1 was reduced and showed an intense peak around 1000 cm−1 corresponding to silicate anion, which supports the formation of layered cobalt hydrotalcite and cobalt silicate solid solution upon calcination. Further, the band at 470 cm−1 corresponding to Co–O–Si bending vibration indicates the presence of cobalt silicate species.31,32
Powder X-ray diffraction patterns of as-synthesized hydrotalcite and silicate intercalated hydrotalcite samples are shown in Fig. 2. CoAl-HT shows that sharp and symmetrical reflections of (003) and (006) planes around 2θ ranges 11 and 23, respectively, are typical of layered HT structure.7,25,26,30,31 The silicate anion intercalated hydrotalcite CA-Si4 and CA-Si6 showed broad peak evidence that the silicates are stuffed in the interlayer spaces of the brucite structure. Unlike earlier report, the current study it was not observed much shift in XRD d-spacing upon silicate intercalation. However, it is known that the peak position and broadening of X-ray reflection is directly reflects the orientation of anions present in the interlayer of HT.17 The broadening of X-ray reflection (Fig. 2b) evidently supports the orientation of the silicate anion in the interlayer as a layered silicate.17 Pure CoAl-HT (CA-Si0) shows an XRD pattern characteristic of cobalt spinel (Co3O4 and CoAl2O4) structure (Fig. 2b) upon calcination,25 whereas silicate anion intercalated CoAl-HT (CA-Si) resulted solid solution of cobalt silicates and cobalt spinel structure, which is in agreement with FT-IR studies. The stabilization of silicate anions by TPAOH results in a mesoporous solid solution of cobalt silicate and cobalt spinel structures.
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Fig. 2 XRD patterns of (a) as-synthesized and (b) calcined silicate free HT and silicate intercalated materials. |
The elemental composition of CoAl-HT and silicate intercalated HT were estimated using WDXRF and results are shown in Table S1 (ESI†). It was evident that slight decrease in cobalt content in final materials is noticed as compared to synthesis gel composition. This might be due to an incomplete condensation of cobalt species, which remain as soluble cobalt species during the synthesis washed while filtering.
Nitrogen sorption isotherms of CoAl-HT and silicate intercalated HT correspond to multilayer adsorption followed by capillary condensation typically of type IV isotherms (Fig. 3) according to the IUPAC.33,34 Textural properties of various cobalt hydrotalcite samples are summarized in Table 1. The BET surface area and pore volume of the silicate-intercalated HT samples were found to be higher than those of the pure HT sample. The observed increase in surface area in CA-Si samples are owing to intercalation of silicate anion by replacing carbonate anions is in agreement with the FT-IR spectra (Fig. 1).
Sample code | Calcination temp.(°C) | Surface area (m2 g−1) | Pore volume (cm3 g−1) | Basicity (mmol g−1) | ||
---|---|---|---|---|---|---|
BET | Micropore (t-plot) | Total | Micropore | |||
CA-Si0 | 400 | 142 | 0 | 0.35 | 0 | 2.85 |
CA-Si4 | 400 | 342 | 29.0 | 1.20 | 0.012 | 2.94 |
CA-Si6 | 400 | 317 | 33.5 | 1.11 | 0.015 | 4.0 |
CA-Si6S | 550 | 361 | 54.5 | 1.40 | 0.026 | — |
A further increase in the anion concentration (2.03 M; CA-Si6) resulted in a slight decrease in the surface area (317 m2 g−1) and the pore volume. These reductions were a result of the filling of the HT interlayers by condensed polymeric silicates in distorted environment.17 Treatment with TPAOH followed by calcination at 550 °C resulted in an increase in porous nature of silicate anion present on interlayer, which enhances surface area and micropore volume, support the formation of porous layered pillars between the HT layers, as the results are in agreement with powder XRD. The surface acidity of HT and silicate intercalated HT were followed by pyridine-FTIR spectroscopy and the results are shown in Fig. S1 (ESI†). The pure cobalt HT show absorption bands at 1449 cm−1 which can be attributed to pyridine coordinated to Al3+ ions.35 As the desorption temperature increases from 200 to 500 °C, the vibrational band corresponding to Lewis acid sites remains accountable indicate that presence of Al3+ in the surface and has strong interaction with pyridine. In contrast, in the silicate anion intercalated HT (CA-Si6) the peak at 1449 cm−1 decreases drastically with desorption temperature evident the presence of weak Lewis acidity on the surface. Further, an additional broad absorption band around 1596 cm−1 was evident due to presence of surface hydroxyl group attached to cobalt and silica species.35
The amount of soluble basic sites was measured by acid–base titration method,29 after the samples were treated with 0.05 M HCl and results are shown in Table 1. It was evident from the above results, the amount of surface basic sites increases with increase in silicate anion concentration. The increase in surface basicity on silicate anion intercalated sample is due to exposed more oxide species (Co2+ and Co3+) present on the surface compared to silicate anion free HT.36 The TEM images of pure HT and silicate intercalated HT samples are shown in Fig. 4. In pure HT (CA-Si0) sample shows non-uniform elongated spherical shape morphology with clear lattice fringes typical of spinel structure25e (further supported from ED pattern Fig. S2a†), which is in agreement with XRD. The introduction of silicate anion into the interlayer of HT resulted to formation of crumbled hexagonal plates. The ED pattern of calcined CoAl-HT-Si (Fig. S2b†) showed characteristic lattice feature of hexagonal cobalt silicate31 and spinel structure.25c It supports the intercalation of silicate anion in the interlayer and formed the solid solution of cobalt silicate and cobalt spinel as evident in XRD. The coordination and oxidation status of cobalt species present in the structure were followed with the help of DR UV-Vis spectra (Fig. 5). All the as-synthesised samples show (Fig. 5a) broad band near to 530 nm related to 4T1g (F) → 4T1g (P) corresponds to Co2+ in octahedral (Oh) environment.30b The absorption band in the range of around 350–400 nm region are assigned to typical of Co3+ (HT; 1A1g → 1T1g).32 Further, the presence of band around 430 nm could be assigned to d–d transitions (1A1g → 1T2g) of Co3+ (Oh) species incorporated in the octahedral sites of Al2O3 matrix.30b,32 After calcination (see Fig. 5b) the broadening of band around 680 nm on typical of Co2+ in tetrahedral environment in CoAl2O4.32 In addition, the silicate anion stabilized HT (CA-Si6S) exhibit broad triplet absorption bands (540, 580, and 626 nm) are assigned to the 4A2(F) → 4T1(P) transition of Co(II) in the tetrahedral silicate environment,32c further support the formation solid solution of cobalt silicate and spinel structure (Fig. 5).
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Fig. 5 DR UV-Vis spectra of as-synthesized (a) and calcined (b) HT and silicate intercalated materials. |
In order to understand the nature of the active species present on the surface, XPS has been carried out for silicate free cobalt hydrotalcite (CA-Si0) and silicate intercalated hydrotalcite (CA-Si4, CA-Si6) and spent catalyst (CA-Si6R). The important features of the XPS data are summarized in Table 2 and Co 2p core level spectra of these samples are shown in Fig. 6. XPS of Co 2p shows two components appearing due to spin–orbital splitting of Co 2p3/2 and Co 2p1/2 peaks with binding energies around 782 and 797 eV along with satellites indicating cobalt is predominantly in mixed oxidation state on the surface.25b The binding energy difference between Co 2p1/2 and Co 2p3/2 is about 15.2 ± 0.1 eV for pure hydrotalcite further support the presence of Co3+ on the surface.25b Due to strong interaction of Co3+ on the surface in the form of CoO(OH) species (Fig. 6).25b
Catalysts | Co 2p3/2 (eV) | Co 2p1/2 (eV) | Spin orbital splitting (eV) | Difference between main and satellite peaks for | O1s (eV) | Al 2p (eV) | Si 2p (eV) | Si/Co ratio | ||||
---|---|---|---|---|---|---|---|---|---|---|---|---|
Main | Satellite | Main | Satellite | Co 2p3/2 (eV) | Co 2p1/2 (eV) | Surface XPS | Bulk XRF | |||||
CA-Si0 | 782.2 | 788.5 | 797.3 | 804.9 | 15.1 | 6.3 | 7.6 | 533.0 | 75.9 | — | — | — |
CA-Si4 | 781.8 | 787.8 | 797.1 | 804.2 | 15.3 | 6.0 | 7.1 | 532.5 | 74.6 | 103.5 | 0.18 | 0.51 |
CA-Si6 | 781.3 | 788.5 | 796.9 | 804.3 | 15.6 | 7.2 | 7.4 | 532.5 | 74.3 | 103.4 | 0.36 | 0.71 |
CA-Si6R | 781.5 | 787.2 | 797.0 | 803.7 | 15.5 | 5.7 | 6.7 | 532.7 | 74.6 | 103.5 | — | — |
On silicate intercalation, there is a broadening observed, especially, on the lower binding energy side and it is indicated by solid arrows on CA-Si0 and CA-Si6. Above broadening is accompanied with an increase in spin-orbit splitting from 15.3 to 15.5 eV in the silicate anion intercalated species and regenerated catalysts indicates the presence of Co2+ ions with possible formation of cobalt aluminates and silicates species.38 This is also supported by the satellite lines which are located at about 6–7 eV above the photoline corresponds to presence of high-spin Co2+ compounds such as CoO, CoAl2O4 and CoSi2O5 species.39 The XPS core level spectra of Co 2p3/2 were further deconvoluted using XPS Peak 4.1 software with Shirley background and using Gaussian–Lorentzian fitting to quantify the various oxidation state present in the materials and the results are shown in Table 3. The deconvoluted XPS CA-Si0 spectrum showed a major peak at 781.9 and less intense peak at 780.7 are typical of cobalt in Co2+ and Co3+ oxidation state with cobalt aluminate (CoAl2O4) species.40 In the case of silicate intercalated samples peaks are broader (indicated by solid line); the deconvolution shows two major peaks at 781.9 eV and 780.7 eV which are typical of Co2+ in oxides in the form of Cobalt oxides, cobalt silicates, cobalt aluminates and cobalt in a cobalt oxides, where cobalt has an oxidation state of Co3+.40 The relative ratio Co3+/Co2+ species increases on silicate intercalated samples to about 0.55–0.65 indicating the silicate intercalated (CoAl-HTSi) samples exposes mixed oxidation states of Co by nearly equivalent amount.
The surface composition obtained from the XPS studies showed Si/Co ratio of 0.36 and 0.18 respectively. However the bulk composition of Si/Co on silicate intercalated samples calculated using XRF found to be 0.71 and 0.51 respectively for CA-Si6 and CA-Si4 samples. The presence of less silica concentration on the surface supports that most of the silicate anions are intercalated between the layers of HT and formed solid solution.
The O 1s spectrum of CA-Si0 (see Fig. 7) exhibit a peak around 533 eV and the corresponding silicate anion intercalated cobalt aluminium HT (CA-Si4, CA-Si6 and CA-Si6R) exhibits (Fig. 7) lower binding energy values around 532.5 eV. As in Co 2p core level, there is a clear broadening observed on the lower binding energy side and it is attributed to the presence of more than one kind of oxygen present on the surface. Especially, oxygen from silicate and hydroxyl are known to be observed between 532 and 533 eV. The Al 2p and Si 2p core level peak (figure shown in S3a and S3b (ESI†)) for silicate anion intercalated HT showed at 74 and 103–104 eV, respectively, which is significantly higher than that of pure Al2O3 and SiO2 support, indicate the presence of strong interaction between cobalt with alumina and silicate species. Further the observed shift in Al 2p XPS value on silicate intercalated HT revealed that Al present in distorted Td environment.37
The catalytic activities of CoAl-HT (CA-Si0), CoAl-HTSi (CA-Si4, CA-Si6), and silicate-anion-stabilized CoAl-HTSi (CA-Si6S) in the oxidation of benzhydrol to benzophenone at 70 °C for 6 h were investigated; the results are summarized in Table 4. Although CoAl-HT intercalated with silicate ions had lower cobalt content than pure CoAl-HT, it gave a higher yield of benzophenone. The higher yield obtained on CA-Si6 was the result of the presence of active cobalt species (Co2+ and Co3+) exposed on the surface of the hydrotalcite layer. These results are in agreement with the basicity and XPS results. The high turn over number (TON) on CA-Si6 compared with that on silicate-free CoAl-HT further supports the presence of exposed cobalt species on the surface. In all cases, benzophenone was obtained as the major product, along with a small amount of a peroxo intermediate. To understand the mechanistic pathway, the reaction was carried out in the presence of a radical scavenger, i.e. 2, 6-di-tert-butyl-p-cresol (BHT). It was found that in the presence of BHT, the conversion decreased to 45%. It is therefore clear that reaction proceeds through a free-radical mechanism. The proposed mechanism, based on surface-active species identified in XPS studies, is shown in Scheme 2.41 First, tert-butyl hydro peroxide (TBHP) interacts with surface-active Co3+ and Co2+ species, yielding peroxo and alkoxo radicals. The peroxo radical interacts with the alcohol, with abstraction of the proton present at the benzylic position, and forms the corresponding radical. The resultant radical interacts with the already-formed alkoxo radical, resulting in production of a ketone or aldehyde, along with tert-butyl alcohol as a by-product. The CA-Si6 catalyst was re-used after separation from the reaction mixture; it was found that the catalytic activity was intact. However, the silicate-intercalated CA-Si6 was regenerated by recalcination at 550 °C in order to remove any chemisorbed organic compounds, and the reaction over the regenerated catalyst was studied. It was again found that the catalytic conversion remain constant with decrease in benzophenone selectivity.
S. No | Catalyst | Co contentb (Wt%) | Conv. (%) | Sel. (%) | Yield (%) | TONc |
---|---|---|---|---|---|---|
a Reaction conditions: alcohol![]() ![]() ![]() ![]() |
||||||
1 | Without catalyst | 0.0 | 18.0 | 100 | 18.0 | — |
2 | CA-Si0 | 38 | 73.2 | 100 | 73.2 | 1144 |
3 | CA-Si4 | 24 | 83.8 | 100 | 83.8 | 2095 |
4 | CA-Si6 | 18 | 85.7 | 99.6 | 85.3 | 2856 |
5 | CA-Si6d | 18 | 81.5 | 100 | 81.5 | — |
6 | CA-Si6e | 18 | 87.5 | 70.0 | 61.2 | 2766 |
7 | CA-Si6f | 18 | 45.2 | 100 | 45.2 | — |
8 | CA-Si6S | — | 82.7 | 96.8 | 80.0 | — |
9 | Co/Al2O3 | 18 | 23.0 | 100 | 23.0 | — |
10 | Co/SiO2 | 18 | 11.7 | 100 | 11.7 | — |
The XPS core cobalt 2p level spectrum of the regenerated catalyst was found to be very similar to that of the fresh catalyst, showing that the catalytic activity was stable. The catalytic activity was also compared with those of samples prepared by physical mixing, i.e. Co/SiO2 and Co/Al2O3. The activities of the physical mixtures were much lower than that of the silicate-anion-intercalated CA-Si6 sample; this is because active cobalt species are uniformly distributed on the catalyst surface (Table 4). The highly active CA-Si6 catalyst was further studied in oxidation of a series of substituted aromatic and aliphatic alcohols; the results are shown in Table 5. The catalyst gave very good yields in all cases. The catalyst also gave very good conversion in the oxidation of aliphatic alcohols, clearly supporting the presence of large numbers of exposed active sites. However, alcohol conversion was lower in the presence of electron-withdrawing groups such as NO2− and Br− at the para position; this might be the result of stabilization of free radicals formed on the surface during the reaction. In contrast, the conversion decreased slightly in the presence of an electron-withdrawing group at the meta position and a methoxy group at the ortho position. Overall, the catalyst was found to be promising for several alcohol oxidations under ambient conditions.
Footnote |
† Electronic supplementary information (ESI) available: Fig. S1 pyridine FT-IR spectra of CA-HT and CA-Si6 at different desorption temperature. Fig. S2 TEM and ED pattern of CA-HT and CA-Si4. Fig. S3 Al 2p and Si 2p XPS spectra of HT and silicate anion intercalated HT materials. Table S1. Elemental composition of HT and silicate anion intercalated materials calculated using XRF spectrometer. See DOI: 10.1039/c3ra46703a |
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