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International Journal of Spectroscopy
Volume 2013 (2013), Article ID 961404, 7 pages
http://dx.doi.org/10.1155/2013/961404
Research Article

Infrared Spectroscopic Characterization of CIT-6 and a Family of *BEA Zeolites

1Department of Chemical Engineering, Kansas State University, 1005 Durland Hall, Manhattan, KS 66506-5102, USA
2Burns & McDonnell, 9400 Ward Parkway, Kansas City, MO 64114, USA

Received 26 June 2013; Accepted 9 September 2013

Academic Editor: Akihide Wada

Copyright © 2013 Sean R. Tomlinson et al. This is an open access article distributed under the Creative Commons Attribution License, which permits unrestricted use, distribution, and reproduction in any medium, provided the original work is properly cited.

Abstract

Infrared spectroscopy is known to be a useful tool for identifying local structure changes in zeolites. Infrared spectroscopy is often employed to complement X-ray diffraction data. Local structure changes in zeolite CIT-6 and its zeolite beta (*BEA) analogs caused by calcination, altering framework composition, and ion exchange have been identified with mid- and far-infrared spectroscopy. Differences in the local structures of the samples were observed in mid- and far-infrared spectra, including changes in the intratetrahedral asymmetric stretch, the double-ring mode, and the intratetrahedral bending mode regions. The infrared spectra indicate that calcination or acetic acid extraction changed the structure of CIT-6 to that of zeolite beta (*BEA). Zinc ion exchange or the substitution of aluminum into the framework structure of acetic acid extracted samples retained the CIT-6 structure.

1. Introduction

Microporous molecular sieves are employed in catalytic, ion exchange and adsorption/separation processes and are, therefore, of scientific and commercial interest [1]. While “zeolite” specifically refers to aluminosilicate microporous molecular sieves, the term is often applied to compounds with similar crystalline structures. Zeolites are remarkable because of their uniform pores (which are less than 2 nm), their channel configuration, and their void space organization.

Because of zeolites’ vast application potential, the characterization of chemical composition, structure, and bonding are important, leading to the use of various analytical techniques to obtain such data. Chemical composition of zeolites can be obtained with atomic absorption spectroscopy (AAS), atomic emission spectrometry (ICP-AES), and X-ray fluorescence spectrometry (XRF) [2]. Both 29Si and 27Al nuclear magnetic resonance (NMR) spectroscopies have proven to be valuable tools in understanding local environments surrounding atoms in the lattice. When NMR data are coupled with density functional theory (DFT) calculations, valuable insights into the crystalline structure of zeolites result [3]. X-ray diffraction (XRD) is also widely used to determine crystalline structure of zeolitic materials, and these data permit identification of samples by comparison with XRD results of known samples [46].

Vibrational spectroscopy, including both Raman and infrared (IR), is often employed to investigate the chemistry (with probe molecules) and short-range order in zeolites [715]. In the 1970s, Flanigen et al. proposed zeolite functional group assignments for the absorption bands between 1250 and 300 cm−1 [14, 15]. Assignments divided spectra into regions classified with respect to intra- or intertetrahedral vibrations. Intratetrahedral vibrations are stretches associated with movements within the TO4 tetrahedra that comprise the zeolite’s structure. These movements can be O–T–O bending modes or symmetric or asymmetric stretches of O–T–O bonds. Intertetrahedral (between adjacent tetrahedra) vibrations include pore-opening (also known as breathing) modes. These guidelines have become the primary tool for absorption assignments in the infrared spectra of zeolites [13, 16]. Far-infrared spectroscopy (FIR) (wavenumbers less than 400 cm−1) has been used to probe the local cation environment [17], provide structural information such as pore-breathing and intratetrahedral bending modes on the zeolite network [14], and examine the local environment of zeolites through cation probes [1720].

The present study examines the infrared spectra of the zincosilicate molecular sieve CIT-6. CIT-6 was first synthesized and characterized in 1999 [21] and has since been examined with respect to chemical properties [6], mechanism of crystallization [22], and ability to catalyze propane dehydrogenation [4]. CIT-6 is of interest in this study as it can be transformed from the original zincosilicate to a pure silicate without changing the XRD spectra of the sample [21]. This pure silicate can subsequently be modified, without visibly altering the XRD spectra to an aluminosilicate through the insertion of aluminum into T-atom locations formerly occupied by zinc [21]. However, no investigation has been done as to how these chemical changes affect short-range structure, that is, structure changes that may occur and affect zeolite performance, but are not visible using XRD.

CIT-6 has the framework structure of zeolite beta (International Zeolite Association designation *BEA), which is particularly appealing for study because it is an ingrowth of two polymorphs [21, 23]. Zeolite *BEA is also useful in industrial applications such as gas separation and reforming of industrial naphtha [24, 25]. Zeolite *BEA has been analyzed for long-range order in development of its polymorphs [26], short-range order with 29Si NMR chemical shifts to identify structure [3], effects of partial replacement of silicon with tin or titanium atoms [27], and development of connectivity-defect-free zeolite *BEA [28]. Structural [7, 29, 30] and chemical properties [31, 32] of pure silica zeolite *BEA have been investigated using infrared spectroscopy. However, no reported attempts have been made to analyze structure or chemical properties of CIT-6 and modified versions using infrared spectroscopy. Of particular interest is whether IR, especially FIR, can be employed to view local changes to the structure that are otherwise difficult to see using only XRD.

In this work, vibrational spectra of CIT-6 and its derivatives are reported over the spectral range from 1500 cm−1 to 200 cm−1. Seven samples are included in this report: (1) as synthesized, prior to any treatments (As-made CIT-6); (2) as-synthesized after calcination (Calcined); (3) low-temperature (60°C) acetic acid structural-zinc extracted (Low- Si *BEA); (4) high-temperature (135°C) acetic acid structural-zinc extracted (High- Si *BEA); (5) low-temperature acetic acid with aluminum inserted into the T-atoms structural locations from which zinc had been extracted (Aluminum); (6) as synthesized that has been ion-exchanged to substitute zinc for the original lithium cation (Zn CIT-6); and (7) pure silica *BEA (Pure Si *BEA) [4, 6, 28].

2. Experimental Section

CIT-6 was synthesized following the procedure described by Takewaki et al. [21] Reactants were mixed at a molar composition of 0.05 moles LiOH : 0.03 moles Zn(OAc)2 (zinc acetate) : 0.65 moles TEAOH (tetraethylammonium hydroxide) : 1 mole SiO2 : 30 moles H2O and heated for four days at 150°C in a Teflon-lined autoclave. The product was recovered via filtration, washed with water, and dried at 100°C overnight in air. This “As-made CIT-6” is a zincosilicate zeolite with lithium cations to balance the framework charge. It also contains residual TEAOH in pores that serve as the structure-directing agent (SDA). Postsynthesis structure analysis was performed with either a Bruker AXS D8 Advance X-ray diffractometer or a Rigaku MiniFlex II X-ray diffractometer, using copper Kα radiation.

The As-made CIT-6 was then exposed to five treatments to modify framework composition while maintaining the *BEA structure visible with XRD [6]. Figure 1 shows these treatments and the resulting samples. The “Calcined” sample was obtained by heating As-made CIT-6 at 550°C for ten hours to remove remaining SDA [4]. The “Zn CIT-6” was prepared by ion-exchanging lithium cations in the As-made CIT-6 with zinc cations through exposure to a 1 molar Zn solution for ten hours at 80°C [4]. In both the “High- Si *BEA” and “Low- Si *BEA,” intratetrahedral zinc atoms were extracted from the As-made CIT-6 zincosilicate framework with acetic acid, leaving behind a pure silica zeolite with the *BEA framework [6]. The High- Si *BEA resulted from exposing As-made CIT-6 to acetic acid at 135°C for two days, where the higher temperature is expected to anneal extracted zinc sites [6]. The Low- Si *BEA was made by exposing As-made CIT-6 to acetic acid at 60°C for three days, resulting in exposed silanol groups at the sites of extracted zinc [6, 21]. Mixing the Low- Si *BEA with aluminum nitrate nonahydrate at a 1 : 2.50 weight ratio of zeolite to Al ·9H2O at 80°C for one day resulted in the insertion of an aluminum atom into the tetrahedral framework [6], thus creating the aluminosilicate form of zeolite *BEA, referred to here as “Aluminum.”

961404.fig.001
Figure 1: Flow chart of synthesis procedures from Andy and Davis [4], Takewaki et al. [6, 21], and Camblor et al. [28].

The “Pure Si *BEA,” a pure silica zeolite *BEA, was synthesized following the procedure described by Camblor et al. [28]. This is the only sample studied in this work that did not originate from postsynthesis treatments of As-made CIT-6. Pure Si *BEA was synthesized using hydrofluoric acid, resulting in formation of zeolite *BEA with enhanced crystallinity and no connectivity defects [28]. This is an excellent model for comparison of *BEA structure with other samples in this study [28].

Infrared spectroscopic data were obtained with a Mattson Instruments Cygnus 100 FTIR spectrometer. All data were obtained via diffuse reflection utilizing a Spectra Tech “COLLECTOR” diffuse reflection accessory. Collected data were obtained in Kubelka-Munk units, the preferred units of diffuse reflectance IR, and then normalized to account for variations in spectral intensity arising from the dilution occurring during sample preparation [33, 34].

In the mid-infrared (MIR) region, a high-temperature ceramic source and a germanium-coated potassium bromide (KBr) beam splitter were employed. The detector was a deuterated triglyceride sulfate (DTGS) detector with a KBr window. The mirror velocity was 0.6 cm/sec, and the resolution was set at two cm−1. The iris setting was 50%. One thousand twenty-four scans were coadded for each spectrum.

In the far-infrared (FIR) region, a high-temperature ceramic source was employed. The beam splitter was a three-micron thick Mylar film, and the detector was a DTGS detector with a polyethylene window. The mirror velocity was 0.3 cm/sec, and the resolution was two cm−1. The iris was 50% open. Each spectrum was the result of coadding 1,024 scans.

Due to requirements of the diffuse reflection technique, all samples were mixed with cesium iodide powder at an approximate ratio of 1 : 5 (zeolite : CsI). A mortar and pestle were used to reduce the particle size of the solids and to mix cesium iodide powder and sample. CsI powder was used for the background spectra.

3. Results and Discussion

As reported in the literature, XRD patterns of the samples did not change significantly upon treatment [4]. Figure 2 shows similarities between the As-made CIT-6, Calcined, and Aluminum samples; the XRD pattern of the defect-free Pure Si *BEA is included for comparison [4]. All patterns exhibit strong similarities, with the only difference between spectra being the appearance of peaks at 13.4° and 14.4° 2θ in the Calcined sample versus the Aluminum and As-made samples. These differences are consistent with results reported in the literature and are similar to peaks seen in the XRD of the Pure Si *BEA sample [21].

961404.fig.002
Figure 2: XRD results for Pure Si *BEA, Aluminum, Calcined, and As-made CIT-6 samples.

The mid-infrared peak assignments from 1500 to 700 cm−1 are given in Table 1, and MIR spectra for all samples can be seen in Figure 3. The As-made CIT-6 and Pure Si *BEA sample spectra match spectra reported in the literature [22, 35].

tab1
Table 1: Mid-IR peaks for CIT-6 and its derivatives. The notations are as follows: w is weak intensity, m is medium intensity, s is strong intensity, and sh is shoulder.
961404.fig.003
Figure 3: Mid-infrared spectra of samples with sample labels and peaks of interest labeled.

In Figure 3 all the samples (except Pure Si *BEA) show absorptions in the aliphatic C–H bending mode region between 1500 and 1350 cm−1, characteristic of either leftover SDA or its decomposition products [4, 36, 37]. The presence of residual SDA is consistent with a previous report that 24% of SDA remains after acetic acid extraction [4]. The Aluminum sample is unique, having a more complex spectrum in the region from 1500 to 1250 cm−1. The additional, medium intensity, broad peaks in the Aluminum sample between 1500 and 1250 cm−1 are due to nitrate anions from the aluminum insertion process [36, 37]. Additionally, the High- and Low- Si *BEA and Aluminum samples have small peaks at approximately 950 cm−1, indicative of residual acetic acid [37].

Differences in the spectra in Figure 3 show changes in the intratetrahedral asymmetric O–T–O region, between 1230 and 990 cm−1, indicating a change in the intratetrahedral environment. The As-made CIT-6 structure is retained during zinc ion exchange (sample Zn CIT-6), as shown by the similarity in the peaks at 1165 and 998 cm−1. But these peaks are absent in the Calcined, High- , and Low- samples. Either calcination or acetic acid extraction results in spectra more similar to the Pure Si *BEA sample, particularly with regard to disappearance of the peak at 1165 cm−1. However, the Aluminum sample, which inserted aluminum into vacant zinc locations (caused by acetic acid extraction), apparently has a small peak at 1165 cm−1, indicating a return to an intratetrahedral environment similar to the original CIT-6. All spectra show a broad region between two primary peaks at ~1220 and ~1070 cm−1, but only the Pure Si *BEA sample shows an additional broad peak at 1103 cm−1. The structural changes shown in Figure 3 for the samples are not seen in the XRD of the samples (Figure 2). The differences between the spectra shown in Figure 3 indicate the usefulness of IR to show short-range differences in zeolite structure as opposed to the long-range structure identification ability of XRD.

All samples have a peak at approximately 800 cm−1 and a smaller peak or shoulder at approximately 735 cm−1, identified by Flanigen as symmetric intertetrahedral O–T–O stretches [14, 15]. This similarity indicates little change in intertetrahedral O–T–O bonding of the samples, in spite of the intratetrahedral changes discussed above.

Far-infrared peak assignments are given in Table 2, and the FIR spectra are provided in Figure 4.

tab2
Table 2: Far-IR peaks for CIT-6 and its derivatives. The notations are as follows: w is weak intensity, m is medium intensity, s is strong intensity, and sh is shoulder.
961404.fig.004
Figure 4: Far-infrared spectra of samples with sample labels and peaks of interest labeled.

The Pure Si *BEA sample has an FIR spectrum consistent with previous reports in the literature [35]. Far-IR spectra for CIT-6 and its derivatives have not been previously reported. Figure 4 shows a change in the double-ring mode region (from 650 to 500 cm−1) for the Calcined and High- and Low- Si *BEA samples with the addition of the extra peak at 640 cm−1, compared to the original As-made CIT-6 [14, 15]. The region from 500 to 420 cm−1 also shows changes in the intratetrahedral T–O bending region for High- and Low- Si *BEA and Calcined samples with an additional peak or shoulder at approximately 473 cm−1, compared to As-made CIT-6 [14, 15]. The 473 cm−1 peak is clearly resolved in the Pure Si *BEA spectrum. Similar to changes in the MIR shown in Figure 3, calcination and acetic acid extraction result in a change in the FIR and together indicate a change in the structure of the zeolite.

As in the MIR shown in Figure 3, the similarity of Aluminum’s FIR structure to that of As-made CIT-6 is interesting because the Aluminum sample is prepared from the Low- Si *BEA. As the Low- Si *BEA sample shows changes from the original As-made CIT-6, the return to the original structure is an interesting outcome of the aluminum insertion process. This change shows that inserting aluminum atoms into T-atom locations once occupied by zinc results in reversion of the framework structure from Low- Si *BEA to the original As-made CIT-6 sample. This structural reversibility is of note because changes are visible with IR, even though zinc T-atom locations are only 3% of total T-atom sites available [4].

The region from 420 to 300 cm−1 shows the pore-opening modes of the zeolites [14, 15]. The Pure Si *BEA sample has three clear peaks, and the High- Si *BEA exhibits three weak peaks at the same wavenumbers. Other samples show little difference from As-made CIT-6. Similarities of As-made CIT-6 and its derivatives in this region suggest that these samples lack long-range order at the level of pore-breathing modes observed with the Pure Si *BEA sample. Lack of change in the pore-opening region corroborates what is seen in XRD results where samples maintain similar patterns even after treatment [21].

The synthesis method for Pure Si *BEA results in defect-free material, and a lack of defects contributes to resolution narrowing of absorption bands in this spectrum [28]. A narrowing of line widths for CIT-6 upon calcination is expected. Both Aluminum and Zn CIT-6 samples exhibit peak broadening in the FIR. The Aluminum sample’s broader absorbances in the FIR are indicative of distortions of tetrahedral bond angles due to the extraction and insertion process. Despite the fact that only about 3% of the tetrahedral sites are impacted by replacing zinc with aluminum, the process of extraction and then reinsertion of the T-atoms creates a disruption in the long-range structure as evidenced by the broadening of both the mid- (Figure 3) and far-IR (Figure 4) spectra. The Zn CIT-6 samples show that limited ion exchange has the distorted local order of the samples even without disordering the overall structure.

Figure 4 demonstrates that the chemical or thermal treatments studied herein affect the structure of the sample by modifying both the intratetrahedral T–O bending modes and the intertetrahedral double-ring modes. These changes can be seen in the FIR spectra of the sample. These changes in both the double-ring and intratetrahedral regions verify that chemical or thermal treatment converted As-made CIT-6 to the *BEA structure, while ion-exchanged Zn CIT-6 does not exhibit a structural change [32].

4. Conclusions

The mid- and far-infrared spectra of CIT-6 and related framework structures have been reported and band assignments have been made. Calcination or acetic acid extraction of CIT-6 results in a structure different from the original As-made CIT-6 and very similar to Pure Si *BEA in both MIR and FIR. Pure Si *BEA, Calcined, and Low- and High- Si *BEA samples all have two peaks in the MIR intratetrahedral asymmetric stretch region, compared to four peaks seen in the As-made CIT-6, Aluminum, and Zn CIT-6 samples. The changes in the FIR from the As-made CIT-6 result in an additional intratetrahedral bending mode and a new double-ring mode. The zinc ion-exchange process did not alter the As-made CIT-6 structure. Broadening of Aluminum and Zn CIT-6 samples in the FIR shows that chemical treatments and ion exchange disrupt the local order of the structure. The changes in the local order are difficult to see using XRD but are visible with FIR.

This work demonstrates the utility of IR, for qualitative analysis of chemical effects on zeolite structures as a complement to XRD. In particular, FIR provides information regarding how short- and long-range structures of the samples are modified by thermal or chemical treatment. Significant changes in the FIR of the samples are easier to identify than changes visible using XRD.

Acknowledgments

The authors thank Dr. Mark Davis (California Institute of Technology) and Dr. John McKeen (formerly at California Institute of Technology) for providing the original CIT-6 sample. This project was funded by Kansas State University. Support for SRT was provided through the National Science Foundation (CBET-0943087).

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