Zeolites are typically a class of crystalline microporous aluminosilicates that are constructed by SiO4 and AlO4 tetrahedra. Because of their unique porous structures, strong Brönsted acidity, molecular-level shape selectivity, exchangeable cations, and high thermal/hydrothermal stability, zeolites are widely used as catalysts, adsorbents, and ion-exchangers in industry. The activity, selectivity, and stability/durability of zeolites in applications are closely related to their Si/Al ratios and Al distributions in the framework. In this review, we discussed the basic principles and the state-of-the-art methodologies for regulating the Si/Al ratios and Al distributions of zeolites, including seed-assisted recipe modification, interzeolite transformation, fluoride media, and usage of organic structure-directing agents (OSDAs), etc. The conventional and newly developed characterization methods for determining the Si/Al ratios and Al distributions were summarized, which include X-ray fluorescence spectroscopy (XRF), solid state 29Si/27Al magic-angle-spinning nuclear magnetic resonance spectroscopy (29Si/27Al MAS NMR), Fourier-transform infrared spectroscopy (FT-IR), etc. The impact of Si/Al ratios and Al distributions on the catalysis, adsorption/separation, and ion-exchange performance of zeolites were subsequently demonstrated. Finally, we presented a perspective on the precise control of the Si/Al ratios and Al distributions of zeolites and the corresponding challenges. 沸石是一类典型的由SiO4和AlO4四面体构成的结晶微孔铝硅酸盐。由于其独特的多孔结构、强的布朗斯台德酸性、分子水平的形状选择性、可交换的阳离子和高的热/水热稳定性，沸石在工业中被广泛用作催化剂、吸附剂和离子交换剂。沸石在应用中的活性、选择性和稳定性/耐久性与其Si/Al比和Al在骨架中的分布密切相关。本文综述了分子筛硅铝比和铝分布调控的基本原理和方法，包括晶种法、分子筛间转化法、氟化物介质法和有机结构导向剂法等。 综述了测定Si/Al比和Al分布的常规和新发展的表征方法，包括X射线荧光光谱（XRF）、固态29Si/27Al魔角旋转核磁共振（29Si/27Al MAS NMR）、傅里叶变换红外光谱（FT-IR）等。研究了硅铝比和铝分布对沸石催化、吸附分离和离子交换性能的影响。最后，我们展望了沸石分子筛硅铝比和铝分布的精确控制以及相应的挑战。
This review highlights the basic principles and the state-of-the-art methodologies for regulating the Si/Al ratios and Al distributions as well as their impact on performances. A perspective on their precise control is presented.
Zeolites are crystalline microporous solids in which the frameworks are composed of corner-sharing tetrahedral TO4 units (T = Si, Al, etc.), forming periodic one-dimensional (1D) to three-dimensional (3D) channels with an aperture size of typically <2 nm or inter-connected nano-cages.1,2 Because of their unique porous structures, large specific surface area, molecular-level shape selectivity, tuneable active sites, and high thermal/hydrothermal stability, zeolites are widely used as catalysts,3–5 adsorbents,6,7 and detergents.8,9 The global zeolite market size was valued at USD 12.6 billion in 2021 and is expected to expand at a compound annual growth rate (CAGR) of 6.2% from 2022 to 2030.10 To date, over 250 types of zeolitic structures have been recognized by the Structure Commission of the International Zeolite Association (IZA-SC).11 Each three-letter code is assigned to a confirmed zeolite structure. There are about 20 types of industrialized zeolites including MFI, MOR, FAU, *BEA, MWW, LTA, FER, CHA, etc.12 沸石是结晶微孔固体，其中骨架由共角四面体TO4单元（T = Si、Al等）组成。），形成周期性的一维（1D）至三维（3D）通道，其孔径尺寸通常为1/3 ~ 2nm或相互连接的纳米笼。1，2由于其独特的多孔结构、大的比表面积、分子水平的形状选择性、可调节的活性位点和高热/水热稳定性，沸石被广泛用作催化剂、3-5吸附剂、6，7和洗涤剂。2021年全球沸石市场规模为126亿美元，预计从2022年到2030年将以6.2%的复合年增长率（CAGR）扩张。10迄今为止，国际沸石协会结构委员会（IZA-SC）已确认了250多种沸石结构。11每个三个字母的代码被分配给一个确认的沸石结构。目前已工业化的沸石有MFI、莫尔、FAU、* 沸石、MWW、LTA、FER、CHA等20余种。12
The pure siliceous zeolite structure built of only SiO4 tetrahedra possesses a neutral framework. The isomorphous substitution of a Si4+ by an Al3+ generates a negative charge which needs to be compensated by a cation adjacent to the connected oxygen.3,13,14 Brönsted acidity is thus obtained when the compensating cation is the proton. The strength of Brönsted acidity mainly depends on first the concentration and then the local environment of the AlO4 tetrahedron, corresponding to the Si/Al ratios and the Al distributions of the framework, respectively. Because of the intrinsic affinity of protons to water and the non-negligible difference in the stabilities between Si–O and Al–O bonds, the concentration and distribution of Al atoms will affect the hydrophilicity/hydrophobicity and stability of zeolites.15–20 Typically, Y zeolite (FAU-type) synthesized with a conventional template-free route usually has Si/Al ratios of <3 and suffers from poor hydrothermal stability during catalysis.21,22 Therefore, high-silica Y zeolite was either synthesized via utilization of organic structure-directing agents (OSDAs)23,24 or prepared by dealumination of low silica Y zeolite via steam treatment.25 The dealuminated Y zeolite (denoted as ultra-stable Y, USY) exhibited higher hydrothermal stability and good catalytic performance in fluid catalytic cracking (FCC). As for the impacts of Al distributions, for example, the preferential location of Al atoms in the narrow straight/sinusoidal channels of ZSM-5 catalysts would suppress the aromatic-based cycle and facilitate the olefin-based cycle in the methanol-to-olefins (MTO) reaction, which would increase the olefin selectivity (e.g., propylene) and the catalyst lifetime.26–29 Furthermore, the distributions of Al atoms of zeolites refer to three aspects: (i) the location of Al atoms at/within the individual crystallographically distinguishable framework T sites; (ii) the relation of two or more Al atoms in the framework, including their distances and the possibility of cooperation; and (iii) the location of Al atoms at specific positions such as the intersections of the channels. 纯硅沸石结构仅由SiO4四面体构成，具有中性骨架. Si4+被Al3+类质同晶取代产生负电荷，该负电荷需要由与连接的氧相邻的阳离子补偿。3，13，14因此，当补偿阳离子是质子时，就得到了布朗斯台德酸度。Brönsted酸性的强弱主要取决于AlO 4四面体的浓度和局部环境，分别对应于骨架的Si/Al比和Al分布。由于质子对水的固有亲和力以及Si-O键和Al-O键之间稳定性的不可忽略的差异，Al原子的浓度和分布将影响沸石的亲水/疏水性和稳定性。通常，用常规无模板路线合成的Y沸石（FAU型）通常具有<3的Si/Al比，并且在催化期间具有差的水热稳定性。21，22因此，高硅Y沸石或者通过利用有机结构导向剂（OSDA）23，24合成，或者通过经由蒸汽处理的低硅Y沸石的脱铝制备。25脱铝Y型分子筛（简称超稳Y，USY）具有较高的水热稳定性和良好的催化裂化性能。 至于Al分布的影响，例如，Al原子在ZSM-5催化剂的窄直/正弦通道中的优先位置将抑制甲醇制烯烃（MTO）反应中的芳族基循环并促进烯烃基循环，这将增加烯烃选择性（例如，丙烯）和催化剂寿命。此外，沸石的Al原子的分布涉及三个方面：（i）Al原子在各个晶体学上可区分的骨架T位点处/内的位置;（ii）骨架中两个或更多个Al原子的关系，包括它们的距离和协作的可能性;和（iii）Al原子在特定位置如通道的交叉点处的位置。
To get an appropriate Brönsted acidity, it is often necessary to break the limitation of the current Si/Al ratios of zeolites, which is much more difficult for specific zeotype frameworks such as Y zeolite.23,30 Meanwhile, regulating the Al distributions of zeolites is very challenging because of the randomly located Al atoms within the equivalent crystallographically distinguishable framework T sites in zeolites and the difficulty in determining their spatial distribution.31 Developing an ingenious strategy for the synthesis and new methods for analysing Si/Al ratios and Al distributions is crucially needed.
There have been several excellent reviews regarding the acid sites or Al distributions of zeolites.32–35 However, they tend to be organized on the basis of the generation of acidity and the corresponding applications. Therefore, a comprehensive review throughout the process of regulating and determining the Si/Al ratios and Al distributions of zeolites and on the corresponding impacts on the performance of zeolites is very helpful in establishing the relationship between the Si/Al ratios and Al distributions of zeolites and their functionalities.
In this review, we comprehensively surveyed the latest studies related to the regulation of the Si/Al ratios and Al distributions of zeolites including the synthetic strategies and methodologies, mechanisms, characterization techniques, and impacts on the catalysis, adsorption/separation, and ion-exchange performance. However, due to the unclear synthesis mechanism of zeolites, the precise control of the Si/Al ratios and Al distributions of zeolites remains challenging. In this review, the insights and keys for regulating Si/Al ratios and Al distributions are presented. We hope that this review will be helpful to the chemists in academic and industrial fields working on the synthesis, modification, characterization, and applications of zeolites.
2. Regulation of the Si/Al ratios of zeolites
During the formation of aluminosilicate zeolite, it is well accepted that the long-range ordering of the framework is formed by the assembly of aluminosilicate oligomers with specific structures and Si/Al ratios, which determine the Si/Al ratios of the framework of a zeolite.36–38
Basically, tuning the Si/Al ratios of zeolites can be achieved by modifying the gel chemistry (mostly Si/Al ratios) of the synthetic mixture and the “post-treatment” of synthesized zeolite crystals of zeolites, which correspond to the “bottom-up” and “top-down” strategies (Fig. 1), respectively. In the terminology of zeolites, “high-silica” and “Si-rich” usually refer to the high Si/Al ratios of a zeolite, while “low-silica” and “Al-rich” usually refer to the low Si/Al ratios of a zeolite. However, the classification of Si/Al ratios into “Si-rich” or “Al-rich” is just applicable to the given zeolite. For example, the typical Si/Al ratios of Beta zeolite synthesized without organic structure-directing agents (OSDAs) in a basic medium often range from 4 to 6.39–41 For Beta (*BEA) zeolite,” Al-rich” usually refers to Si/Al ratios of <5 and “high-silica” usually refers to Si/Al ratios of >10.42,43 For Y zeolite (FAU), “high-silica” corresponds to Si/Al ratios of >3, while “Al-rich” corresponds to Si/Al ratios of <3 but >1.5, which is a criterion for X and Y zeolites.21,22,44 For ZSM-5 (MFI) zeolite, “high-silica “usually refers to Si/Al ratios of >20 and the “Al-rich” usually refers to Si/Al ratios of <15.45,46 Thus, the difficulty in tuning the Si/Al ratios depends on zeotype structures. For example, the range of the Si/Al ratios for Y zeolite is narrow, while that for ZSM-5 is broad. Generally, the Si/Al ratios of a zeolite cannot be lower than 1 because of the limitation of the Löwenstein rule.43,47,48
Fig. 1. Principles and methodologies for regulating the Si/Al ratios of zeolites.
2.1. “Bottom-up” tuning of the Si/Al ratios of zeolites
The “bottom-up” strategy for tuning the Si/Al ratios of zeolites is mostly performed by changing the Si/Al ratios of the synthetic mixture. The Si/Al ratios of the oligomers can be modified by various methods which can be divided into two categories. One category is associated with altering the gel chemistry such as by altering the gel composition via modifying the recipe or dissolving the parent zeolites and introducing additives to promote the formation of Si–O or Al–O bonds.42,49,50 The other category is associated with the principle of charge balance. As mentioned above, the negative charges of the framework of zeolites originated from the substitution of Si4+ by Al3+, which have to be balanced by the positive charges. Hence, the number of Al atoms equals the number of compensated positive charges provided by inorganic and/or organic extra-framework cations. In the end, fluoride, organic structure-directing agents (OSDAs) and dry gel conversion (DGC) can alter the Si/Al ratios of zeolites by following the principle of charge balance in which defects with negative charges can be easily formed in the DGC process.
As mentioned above, directly changing the Si/Al ratios of the synthetic mixture can accordingly alter the Si/Al ratios of the oligomers, resulting in the corresponding modification of the Si/Al ratios of a zeolite framework. For example, ZSM-5 (MFI-type) with Si/Al ratios ranging from 20 to 220 can be obtained by directly tuning the Si/Al ratios of the synthetic mixture in the presence of the OSDA tetrapropylammonium ions (TPA).+51,52 However, an unusually high concentration of Al or Si in the synthetic mixture can slow down the crystallization process, which often requires a longer time to complete the crystallization.53–55 For example, *BEA-type zeolites with Si/Al ratios from 25 to ∞ can be synthesized from a synthetic mixture with the molar composition of 0.35Na2O : 4.5(TEA)2O : xAl2O3 : 25SiO2 : 295H2O, using a tetraethylammonium cation (TEA) as the template, where x is varied between 0 and 0.50.+54 The complete crystallization of the high-silica Beta zeolite needs a longer time compared to the Al-rich Beta zeolite. For example, three days are needed for the crystallization of Beta zeolite with Si/Al ratios of 25, 50, and 83 and five days are needed for the Beta zeolite with a Si/Al ratio of 250, while 11 days are needed for the pure silica Beta zeolite.
However, if the gel chemistry of the synthetic mixture deviates too far from the optimal one due to the modification of the Si/Al ratios of the synthetic mixture, the target zeolites will usually not be formed no matter how long the crystallization time is prolonged. In such cases, introducing the seed, which can promote the nucleation of the synthetic mixture, usually helps the formation of the target zeolites with desired Si/Al ratios.56–58 For example, if the Si/Al ratios of a synthetic mixture for the crystallization of *BEA zeolite are significantly decreased from their optimal value in order to synthesize Al-rich Beta, the competitive MOR zeolite becomes the main product, while introducing Beta seeds to the same synthetic mixture resulted in the crystallization of Al-rich Beta with Si/Al ratios of 4–6.42,55,59 By utilization of K-CHA seeds, phase pure Al-rich CHA (Si/Al = 1.6–2.0) can be synthesized from an Al-rich synthetic mixture, which produces CHA zeolite and an impurity in the absence of K-CHA seeds.58 Liu and co-workers reported for the first time the synthesis of high-silica ZSM-35 (Si/Al = 14.5) with high solid yield (65–85%) by using the as-synthesized MCM-49 (Si/Al = 9.55) as seeds, while an amorphous product and MOR zeolite were obtained in the absence of MCM-49 seeds after crystallization of the same initial reaction mixture for 16 and 40 h, respectively.60 The high-silica zeolite Y with a Si/Al ratio of up to 7.95 can be synthesized with the seed-assisted strategy, while only an amorphous product was obtained in the absence of seeds.61 Xiao and co-workers also successfully synthesized pure silica zeolites (MFI, MTT, TON, and *MRE) and ZSM-5 zeolites with Si/Al ratios ranging from 38 to 240 by using such a strategy (besides zeolite seeds, alcohol as the space filler was also used).62,63 Therefore, the successful assembly of oligomers with appropriate Si/Al ratios is the key to forming zeolites with desired Si/Al ratios.
Interzeolite transformation has been proven to be an efficient strategy for zeolite synthesis.64 Such a strategy can also be used to tune the Si/Al ratios of target zeolites because the released locally ordered aluminosilicate oligomers from parent zeolites might facilitate the formation of another zeolite with unusual Si/Al ratios under appropriate conditions.65 For example, high-silica OFF zeolites can be synthesized via interzeolite transformation in an aqueous solution containing benzyltrimethylammonium hydroxide (BTMAOH) and alkali metal hydroxide at 125 °C by solely tuning the Si/Al ratios of the parent FAU zeolites without introducing additional Si and Al sources (i.e., Si/Al = 23 (FAU) → 7.6 (OFF); 31 (FAU) → 8.0 (OFF)).66 Interestingly, high-silica CHA can be obtained after crystallization for 7–21 days (i.e., Si/Al = 16 (FAU) → 14.5 (CHA); 22 (FAU) → 18.2 (CHA); 30 (FAU) → 21.5 (CHA)) if the CHA seeds were introduced into the same synthesis system.67 Moreover, high-silica CHA (Si/Al = 10.5–11.4) zeolites can be transformed from FAU (Si/Al = 10.8) zeolite under a solvent-free system within 24 h in the presence of the OSDA N,N,N-dimethylethylcyclohexylammonium bromide (DMCHABr), CHA seeds, and NaOH.68 However, only amorphous products were obtained under identical conditions if the parent FAU zeolites were replaced by equivalent chemicals which demonstrated that the appropriate distribution of the oligomers with specific Si/Al ratios and specific structures in the synthetic mixture is critical for the formation of OFF or CHA zeolites with target Si/Al ratios.
In interzeolite transformation, sometimes additional Si and Al sources and seeds are needed to achieve a successful interzeolite transformation. For example, Li and co-workers synthesized high-silica CHA zeolite with higher Si/Al ratios (i.e., Si/Al > 30) via interzeolite transformation in the presence of the OSDA N,N,N-trimethyladamantammonium hydroxide (TMAdaOH), the seed of zeolite L with a Si/Al ratio of 3, and additional Si and Al sources, making a Si/Al ratio of 42.85 in the initial mixture.69 Besides high-silica CHA, Al-rich CHA (Si/Al = 1.5–1.7) zeolites can also be synthesized via interzeolite transformation from the FAU (Si/Al = 2.6) zeolite along with an additional Al(OH)3 source.70 In the synthesis of high-silica Beta zeolite viaFAU interzeolite transformation, it was found that the transformation was not successful if the Si/Al ratios of FAU were higher than 69.71 Considering that the MOR zeolite and Beta zeolite have similar building units, Wu and co-workers prepared the high-silica Beta zeolite with a Si/Al ratio of 146, 216, 254, 296, and 357 via interzeolite transformation of the high-silica MOR zeolite with a Si/Al ratio of 145, 213, 255, 298, and 353, respectively, in the presence of tetraethylammonium hydroxide (TEAOH) and fluoride ions (Fig. 2).49 These results clearly demonstrate that the right gel chemistry combined with the seeding strategy if necessary is of the utmost importance to regulate the Si/Al ratios of the resultant zeolites, which can be achieved via modifying the recipe of the initial reaction mixture or interzeolite transformation.
Fig. 2. Synthesis of high-silica Beta zeolite via interzeolite transformation of high-silica MOR zeolite. Reproduced from ref. 49 with permission from Elsevier, Copyright 2021.
Besides changing the Si/Al ratios of the initial mixture or dissolving the zeolites to modify the Si/Al ratios of the oligomers, introducing extra species to alter the condensation of Si–O–Si(Al) bonds, such as anions, metal ions, and hydroxyl radicals can also modify the Si/Al ratios of the oligomers and further regulate (mostly increase) the Si/Al ratios of the resultant zeolites. Guided by this principle, Yu and co-workers reported a general and facile strategy to improve the Si/Al ratios of MOR, FAU, and MFI zeolites by adding iodide ions into the initial mixture, which promoted the formation of Si–O–Si bonds and thus provided a high-silica oligomer.72,73 Shen and co-workers introduced Co2+ into the initial mixture for the OSDA-free crystallization of zeolite Y.44 The introduced Co2+ forms a 5-coordinated intermediate (Co–O–Si)* with the silicate species. Such intermediate interferes the formation of the Al–O–Si species but has less influence on the formation of Si–O–Si species, resulting in the high Si/Al ratios of aluminosilicate oligomers in the initial mixture and the increased SiO2/Al2O3 ratio of the produced zeolite Y to 6.15. Yu and co-workers discovered that hydroxyl radicals (˙OH) can facilitate the dissociation of the Si–O–Si bonds and promote the remaking of Si–O–Si bonds.74 In terms of such an effect of ˙OH, Yu and co-workers introduced ˙OHs via hydrogen peroxide into the initial mixture for the OSDA-free crystallization of zeolite Y with a SiO2/Al2O3 ratio of 6.35, overcoming the upper limit of 6.0 for synthetic zeolite Y by a one-step organic-free route.50 The condensation of Si(OH)3ONa and Al(OH)4Na monomers with Si(OH)3O˙ and Si(OH)2ONaO˙ radical species was studied using density-functional theory (DFT) calculations (Fig. 3). The calculated Gibbs free energies (Fig. 3c) indicated that the Si(OH)3O˙ radical preferentially accelerated the formation of Si–O–Si bonds. Furthermore, nanosized Beta zeolites with Si/Al ratios ranging from 6 to 300 were obtained by a facile l-lysine assisted method.75 In such a synthetic system, l-lysine can chelate the silica and aluminum precursors. Attachment of l-lysine to the oligomers inhibits the growth of zeolites and prevents the formation of impurities. These results demonstrate that the additionally introduced species possessing the ability to modify the Si/Al ratios of the oligomers can also regulate the Si/Al ratios of the resultant zeolites.
Fig. 3. Optimized geometries of the structures involved in the condensation of (a) Si(OH)3O˙ and (b) Si(OH)2ONaO˙ radical species with Si(OH)3ONa and Al(OH)4Na. Si, Al, O, H, and Na atoms are depicted as yellow, blue, red, white and purple spheres, respectively. (c) Corresponding Gibbs free energy profiles for condensation of radicals with Si(OH)3ONa (blue) and Al(OH)4Na (orange). Reproduced from ref. 50 with permission from Wiley, Copyright 2020.
The synthesis of zeolites usually involves a silicon source, an aluminum source, alkali hydroxide, and water. OH− from alkali hydroxide acts as a mineralizer that promotes the formation of Si–O–Si and Si–O–Al bonds resulting in negatively charged aluminosilicate oligomers, which are assembled around alkali cations to form long-range ordering structures of zeolites. As mentioned above, the number of compensated alkali cations equals the number of Al atoms in the framework of zeolites, and the zeolites directed by the alkali hydroxide are mostly Al-rich due to the high charge density of alkali cations.23,76 Therefore, replacing the high charge density cation with low charge density organic quaternaryammonium and/or the mineralizer OH− with another mineralizer F− in the form of hydrogen fluoride (HF) can decrease the incorporation of Al into the framework of zeolites, which can thus increase the Si/Al ratios of the resultant zeolites.77,78 Taking this principle into consideration, Liu and co-workers synthesized high-silica Beta zeolites with various Si/Al ratios (Si/Al = 130 to 340) in the presence of fluoride ions and TEAOH.79 Moreover, pure silica Beta zeolite can be obtained from a fluoride medium with TEAOH as OSDA under extremely low water content conditions.80
Zeolites directed by OSDAs usually have higher Si/Al ratios than those directed by inorganic cations such as Na and K because the charge density of an OSDA is usually lower than that of inorganic cations. Compared to OSDA cations, more inorganic cations can be accommodated in the same pore or cavity of the zeolite, which needs more Al atoms to be incorporated into the oligomers, finally resulting in lower Si/Al ratios.++23 Unlike inorganic cations possessing similar charge densities, organic cations' charge densities vary widely. Thus, the Si/Al ratios of zeolites can be tuned by varying the charge density of organic cations. Basically, the upper limit of the Si/Al ratio for Y zeolite synthesized by a one-step organic-free route is 3, which was broken by Yu and co-workers via introducing ˙OHs into the synthetic system.50 However, there are kinetic limitations for the synthesis of Y zeolite with high Si/Al ratios because the crystallization rate decreases with increasing Si/Al ratios of the Y zeolite.81 Y zeolite with a Si/Al ratio approaching 5 was synthesized by using crown-ether based supramolecules as OSDAs in 1990.82 Subsequently, high-silica Y zeolite with various Si/Al ratios had been reported by using N-methylpyridinium (NMP) iodide (Si/Al = 3.18–3.43),83 imidazolium-based ionic liquid (Si/Al = 3.2–3.4),84 TEAOH (Si/Al = 3.88),85 and choline (Ch, Si/Al = 3–6).30,86 Recently, Liu and co-workers reported that increasing the TBA/TEA (TBA: tetrabutylammonium cations) ratio from 1.3 to 4.0 results in an increase in the Si/Al ratio of Y zeolite from 5.1 to 7.8.+++23 Using the bulky organic cation of 4,4′-trimethylenebis(N-methyl, N-benzyl-piperidinium) (TMP) as the OSDA, purely siliceous *BEA can be synthesized in alkaline media with a molar composition of 1 SiO2 : x TMP(OH)2 : 25 H2O (x = 0.15–0.30) at 90–100 °C.87 Similarly, Corma and co-workers synthesized nanosized high-silica Beta zeolites with solid yields of over 95% by using alkyl-substituted flexible dicationic OSDAs such as 1,1′-(pentane-1,5-diyl)bis(1-butylpyrrolidin-1-ium) and 1,1′-(pentane-1,5-diyl)bis(1-butylazepan-1-ium).88
Besides high-silica zeolites, combining OSDAs and fluoride can result in the formation of pure-silica zeolites. Zeolite A (LTA) crystallized from an OSDA-free synthesis system is highly Al-rich and the typical Si/Al ratio is one.89 Using tetramethylammonium (TMA) and tetraethylammonium (TEA) as structure-directing agents (SDAs) instead of alkali cations increased the Si/Al ratio of zeolite A to 3.2.++90 Notably, pure-silica LTA (ITQ-29) zeolite can be obtained in the presence of fluoride and the combined OSDAs of methylated julolidine and TMA.91 Subsequently, high/pure-silica LTA zeolites were synthesized from an initial mixture containing fluoride and TMA/imidazolium-based OSDAs.92–94 In addition, Hong and co-workers successfully synthesized high-silica UFI zeolite (Si/Al = 11) and LTA zeolites (Si/Al = 8.3 to ∞) in fluoride media together with benzylimidazolium-based OSDAs.94
Besides hydrothermal synthesis, dry gel conversion (DGC) is another main method to synthesize zeolites, which was first reported by Xu and co-workers in 1990.95 Unlike the hydrothermal synthesis containing a large amount of water, the DGC method contains only a very limited amount of water, which may moderate the species transportation and thus leave abundant defects (e.g., Si–O−) with negative charges, which can balance the positive charge of the OSDA. Thus, high-silica and even pure-silica zeolites can usually be obtained by the DGC method even in the absence of fluoride.96 For example, the Si/Al ratios of SSZ-13 (CHA) typically range from 10 to 54. However, Miyake and co-workers increased the Si/Al ratios of SSZ-13 up to 182 by the DGC method.97 Recently, Fan and co-workers reported that the charge-balancing interactions between an inorganic cation, OSDA, and Si–O− defects by the DGC method are essential aspects for the synthesis of fluoride-free siliceous CHA, STT, *BEA, MFI, and *MRE.98 Very recently, pure-silica Beta was also fabricated by DGC with a dry gel composition of SiO2 : 0.16NaOH : 0.08TEAOH.99
Table 1 summarizes the representative examples of regulating the Si/Al ratio and their influence on the performance with “bottom-up” methods. “Bottom-up” methods provide a one-pot methodology to regulate the Si/Al ratios of zeolites which avoids destroying the framework but is not easily amenable to industrialization since they involve substantial amounts of costly templates, emissions of waste liquor, and complicated operating steps.32
Summary of the representative examples of regulating the Si/Al ratio and their influence on the performance with “bottom-up” methods
OSDAs (TMA and imidazolium-based OSDAs) and fluoride media
16 to ∞
The Cu2+ ion-exchanged high-silica (Si/Al ∼ 17) LTA hydrothermally aged at 900 °C showed better activity maintenance for selective catalytic reduction of nitrogen oxides with ammonia (NH3-SCR) than Cu-SSZ-13
92–94
a
SiO2/Al2O3 used in the original research is listed in parentheses.
2.2. “Top-down” tuning of the Si/Al ratios of zeolites
Regulating the Si/Al ratios of zeolites means tuning the Si/Al ratios of the zeolite crystals (i.e., the final products). “Top-down” means tuning the Si/Al ratios on the basis of already synthesized zeolite crystals, which is mostly realized by post-treatment methodologies. In addition, for the aluminosilicate framework of zeolites, the Al or Si within the framework can be selectively removed to modify the Si/Al ratios of a zeolite, which is also termed “post-synthesis” or “post-treatment”. Compared to the “bottom-up” strategy, the “top-down” strategy has the advantages of facile operation and easy scale-up, but it will inevitably cause a significant decrease in the crystallinity of zeolites, resulting in plenty of defects and silanol groups.
The foundation of the “top-down” strategy is that the tension of the tetrahedral sites (T-sites) in the framework of a zeolite is not uniform throughout the framework and depends on its position, which makes it possible to selectively remove Si (desilication) or Al (dealumination).100–103
The routes for the dealumination of zeolites via post-modification include acid, fluoride, steam, and salt treatment. During dealumination by acid treatment, Al species with high tension are dissolved using an acid. However, the framework of the zeolite may collapse in nitric acid if the Si/Al ratio is too low. The successful dealumination in nitric acid has been applied to *BEA, FAU, and MOR.104–109 In the dealumination of Beta zeolites, the Si/Al ratio was increased to over 200 if the starting Si/Al ratio was greater than 12, while the framework collapsed if the starting Si/Al ratio was less than 12.105 Besides nitric acid, many other acids and chelates can also be used in the dealumination of zeolites, such as oxalic acid,109–112 ethylene diamine tetraacetic acid (EDTA),103,107,113 and hydrochloric acid.103,107 For example, Valtchev and co-workers recently reported the mild dealumination of zeolites with chromic acid.114 The Si/Al ratio of 9.0 of the parent CHA zeolite was increased to 9.4 and further to 10.5, while the Si/Al ratio of the MFI zeolite was increased to 21 from 19. During mild dealumination, the framework was well preserved and Brönsted acid sites (BASs) were preserved and their accessibility was increased. Moreover, Fan103,115,116 and Yu117 developed a microwave-assisted dealumination method which can significantly reduce the treatment time from at least 6 h via conventional hydrothermal treatment to several minutes and generate mesoporous structures. However, sequential alkaline desilication was needed after the dealumination treatments to recover the zeolitic framework and generate mesopores in the treated zeolites.
As mentioned above, fluoride has been widely used in the synthesis of high- or pure-silica zeolites.77–80,93,94 Considering the strong affinity of fluorine with Si and Al, fluoride can also be used in tuning the Si/Al ratios of zeolites via desilication or dealumination. However, the pH of the solution needs to be carefully controlled to prevent framework collapse when hydrogen fluoride (HF) is used. Besides HF, NH4F,102,118,119 NaF,119,120 NaHF2,119,121 and NH4HF2102,119 have also been used as the sources of fluoride. Moreover, dealumination by F− or HF2− can also generate secondary porosity.102,119,120,122 (NH4)2SiF6 is also a widely used dealumination agent,123 which can not only extract aluminium from the framework but also serve as an extraneous source of silicon that can fill up the vacancies created in the framework by the extraction of aluminium.123–127 For example, Yokoi and co-workers tuned the Si/Al ratio of Al-rich Beta to 73 and removed more than 40% of the Al atoms of MCM-22 by treating it with (NH4)2SiF6 solution.126,128 Furthermore, (NH4)2SiF6 has also been used to increase the Si/Al ratios of MOR, FER, Y, ZSM-5, and SSZ-13 zeolites via dealumination with simultaneous silicon reinsertion.124,125,127,129
Similar to (NH4)2SiF6, SiCl4 vapour has the ability to extract the Al atoms from the framework of zeolites and simultaneously insert the Si atoms derived from SiCl4 into the vacancy due to the removal of Al, which results in an increase in Si/Al ratios.130 In the 1980s, Beyer and co-workers first developed such a method.131–133 With this method, highly siliceous Y zeolites (Si/Al = 3.3–63) were obtained.131,134,135 However, this method is not commonly used because of the harsh operating conditions.
In solution, Al2(SO4)3 can react with the framework Al of zeolites containing Na to form the mineral natroalunite (NaAl+3(SO4)2(OH)6), resulting in the extraction of the framework Al and thus an increase in Si/Al ratios.136 With this method, the Si/Al ratio of the framework of NaY can be increased to 4.2 from 2.4, while that of Beta zeolite can be increased up to 12.4 from 4.6.43,136
Besides reacting with the framework Al of zeolite, breaking the Al–O bonds can also lead to the removal of the framework Al. In fact, water in steam form can break the Al–O bonds via hydrolysis (Fig. 4).137 Based on this knowledge, steaming dealumination of zeolite has been developed, which has been commercialized for preparing ultra-stable Y zeolite (USY), a revolutionary fluid catalytic cracking (FCC) catalyst.138 Besides Y zeolite, Hutchings and co-workers dealuminated the MOR zeolite via steaming and increased the Si/Al ratio of the MOR zeolite to 16.6 from 7.5.139 At the same time, Morin and co-workers prepared a series of dealuminated EMT zeolites with Si/Al ratios of 5.5, 7.6, 13, 31, and 52 from the NH4 type EMT with a Si/Al ratio of 4.5 by steaming for various times (0.5–3 h) at various temperatures (450–650 °C).140 Recently, Yang and co-workers prepared dealuminated H-MOR (Si/Al = 15.26, 25.13, 40.65) and dealuminated Na-MOR (Si/Al = 9.96, 11.20, 12.61) by steaming H-MOR (Si/Al = 8.74) and Na-MOR, respectively, which increased the availability of acid sites in the side pockets of MOR zeolite.141
Fig. 4. Proposed mechanism of the dealumination process induced by hydrothermal-treatment of SSZ-13 zeolite. Reproduced from ref. 137 with permission from the Royal Society of Chemistry, Copyright 2022.
Dealumination of zeolites can increase their Si/Al ratios, while desilication can decrease their Si/Al ratios. It is well known that hydroxide ions (OH−) can effectively break the Si–O–Si bonds. Thus, alkaline solution treatment of zeolites can remove the Si atoms from the framework, which certainly reduces the Si/Al ratios142,143 and thus forms mesopores within the zeolite crystals.45,144–152 To date, the inorganic bases NaOH45,100,111,142,147–155 and Na2CO3145 have been used for the desilication of zeolites. For example, Bjørgen and co-workers produced ZSM-12 with Si/Al ratios of 13–34 by treating calcined ZSM-12 (Si/Al = 39) with 0.2–0.6 M NaOH solutions at temperatures of 35 °C, 65 °C, or 85 °C for durations of 15 to 60 min.156 Besides inorganic bases, organic bases, such as TBAOH,154,155 TEAOH,149,151 and TPAOH, can also be used for the desilication of zeolites and generation of intracrystalline mesopores in zeolites.146
2.3. Methods for determining the Si/Al ratios of zeolites
The commonly used analytical techniques for determining the Si/Al ratios of zeolites include X-ray fluorescence spectroscopy (XRF), atomic absorption spectroscopy (AAS), inductively coupled plasma atomic emission spectroscopy (ICP-AES), X-ray diffraction (XRD), solid state 29Si magic-angle-spinning nuclear magnetic resonance spectroscopy (29Si MAS NMR), X-ray photoelectron spectroscopy (XPS), energy-dispersive X-ray spectroscopy (EDS), electron probe micro-analysis (EPMA), and newly developed Fourier-transform infrared spectroscopy (FT-IR).157
Generally, chemical analyses such as ICP-AES and AAS determine bulk Si/Al ratios. However, the XRD, FT-IR, and NMR analyses can also be used to determine the framework Si/Al ratios. XPS as well as EDS and EPMA are used to determine the surface or local Si/Al ratios which have poor sampling depths or rely on the electron penetration of a beam.158,159
XRF has been widely used to determine the Si/Al ratios of zeolites.42,61,103 The features of XRF analysis are accuracy, rapidity, multielement capacity, and nondestructiveness.160 However, XRF analysis is a surface-sensitive method, and the penetration depth of the primary radiation is about μm or so for low-Z elements and about 100 μm or so for heavy elements.
AAS is a routine but widely and frequently used tool in determining the metal and metalloid concentrations dissolved in solution. It offers sufficient sensitivity and is relatively interference free, which has been used to determine the Si/Al ratios of zeolites.161–163 An ICP-AES is one of the most popular instruments in chemical laboratories, which can determine more than 70 elements with detection limits in the parts per billion (ppb) to parts per million (ppm) range and offers very high throughput and the capacity of multiple reportable results per run. Compared to AAS, ICP-AES is especially suitable for refractory elements, such as Si and Al, which are analysed poorly by flame AAS.52,112,164 However, analysis of Si and Al by AAS and ICP-AES requires the complete dissolution of zeolite samples into solution, which usually involves toxic hydrofluoric acid. This is the disadvantage of AAS and ICP-AES.
Due to the non-negligible difference in the bond lengths between Si–O and Al–O bonds, for Y zeolite for example, the change in Si/Al ratios may lead to the change of the specific crystal plane, which thus modifies the cell parameters and shifts the position of specific X-ray diffraction peaks. On the basis of this fact, X-ray diffraction analysis has been widely used as an important and convenient method to determine the Si/Al ratios of Y zeolites.50 With this method, Hajjar and co-workers reported that the d302 spacing of *BEA zeolites decreased along with an increase in the Si/Al ratio from 3.955 Å (Si/Al = 11; 2θ = 22.55°) to 3.939 Å (Si/Al = 46; 2θ = 22.57°), 3.929 Å (Si/Al = 87; 2θ = 22.63°), 3.922 Å (Si/Al = 135; 2θ = 22.69°), and finally to 3.920 Å (Si/Al = 1240; 2θ = 22.71°).165
Solid state 29Si MAS NMR spectroscopy plays an important role in probing various aspects of zeolite structures. In the framework of zeolites, Si is tetrahedrally coordinated. Considering all possibilities, there are five different environments for framework Si atoms depending on the number of adjacent O–Al atoms, which are denoted as Si(nAl) (n = 0, 1, 2, 3, 4). According to the 29Si MAS NMR spectrum, the Si/AI ratios in the zeolite framework can be calculated as follows:1where ISi( n Al) is the intensity of the NMR signal attributable to the Si(nAl) units, and the summation is from n = 0 to n = 4.166 The Si/Al ratios determined by solid state 29Si MAS NMR are consistent with those measured by elemental analysis.24,72,141 By comparing the (Si/Al)NMR values with those obtained by chemical analyses, the amount of extra-framework aluminium can be calculated. However, eqn (1) works well with materials that have framework Si/AI ratios of less than about 10. It cannot be directly applied to the spectra in which signals coming from Si(nAl) units of crystallographically nonequivalent Si atoms overlap, such as the spectrum of omega zeolite.166–168
Determining the Si/Al ratios of zeolites by FT-IR is a recently developed technique.157,169 In the FT-IR spectrum of zeolites, the vibrations associated with the framework structure are present in the mid IR region (200–1300 cm−1). The T–O–T asymmetric stretching band associated with the framework is sensitive to the Al content. As shown in Fig. 5, the skeletal stretching vibrations shift to higher frequencies along with an increase in Si/Al ratios.170,171 A recent study combined the chemometric methods of partial least squares (PLS), support vector machines (SVMs), and soft independent modelling of class analogy (SIMCA) to quantify the Si/Al ratio in zeolites based on FT-IR spectra.169 Before this tentative finding, Fichtner-Schmittler and co-workers found a linear relationship for FAU zeolite between the unit cell parameter a0 and the framework vibrations over the whole range of Si/Al ratios (Si/Al < 10) with an error of <10%:1722where
000000000
000000000
001111100
000000000
011000110
001100010
000100010
000100100
000101000
000110000
000100000
as is the wavenumber of an asymmetric stretching band. Later, Lohse and co-workers observed another linear relationship for Y zeolite between the Si/Al ratios and the vibrational band ν3 at 748–837 cm−1:3where Δν3 is the difference between the wavenumbers ν3 of the recorded sample and the standard Y zeolite (Si/Al = 2.4).170 Recently, Ng and co-workers developed an IR-based protocol to determine the Si/Al ratios of 19 kinds of zeolites.157 The authors proposed a linear equation of y = 0.0458x − 43.584, where y is the Si/Al ratio and x is the asymmetric stretching frequency of the Si–O–T band (cm−1). The equation is valid for Si/Al ratios between 1 and 5. Very recently, Sadrara and co-workers combined the FT-IR spectra, partial least squares, and support vector machines to quantify the Si/Al ratios of zeolites ZSM-5, MOR, and ZSM-48 with high accuracy.169
Fig. 5. FT-IR skeletal spectra of the ZSM-5 samples having different molar ratios of Si/Al (A, 18.5; B, 23.8; C, 43.0; D, 68.3). Reproduced from ref. 171 with permission from Elsevier, Copyright 2006.
XPS is an elemental analysis technique that is a surface-sensitive technique with a sampling depth of only a few nanometres.159 With this technique, Rimer and co-workers determined the shell thickness of core–shell MEL zeolites with ZSM-11 cores and passivated silicalite-2 shells (denoted as ZSM-11@silicalite-2) as shown in Fig. 6.173 The Si/Al ratio of the shell is much higher than that of the core. The depth with a sudden drop in the Si/Al ratio was treated as the thickness of the shell. Scanning electron microscopy with energy dispersive X-ray spectrometry (SEM/EDS) is an elemental microanalysis technique widely applied in the determination of Si/Al ratios of zeolites.174–176 However, high-reliability quantitative X-ray microanalysis by SEM-EDS needs a slim thickness (<50 nm) and standards.158
Fig. 6. Comparison of Si/Al ratios for a ZSM-11 core (C-30 with Si/Al = 30) and core–shell samples (CS-60, CS-91, and CS-133, and the corresponding Si/Al ratios of the shell are 60, 91, and 133) from XPS depth analysis (VKE-XPS) as a function of photon energy (bottom x-axis) and the corresponding information depth (top x-axis) where 95% of the signal is generated. Each sample was pre-coated with ca. 10 nm of carbon. Any uneven (or rough) surfaces of zeolite powders from VKE-XPS sample preparation increase the uncertainty in depth estimation for a single particle. This results in a diffuse transition between the shell and core that creates uncertainty in estimates of shell thickness. Reproduced from ref. 173 with permission from Elsevier, Copyright 2022.
EPMA is well known as an analytic method that can acquire high quality and reproducible compositional data on individual zeolite grains. But sample heating and element mobility caused by the interactions between the electron beam and the sample result in dehydration and underestimation of light extra-framework cations as well as problems in determining the framework Si and Al, leading to subsequent inaccurate calculations of Si/Al ratios.177,178
2.4. Impact of Si/Al ratios on the performance of zeolites
The isomorphous substitution of a Si4+ by an Al3+ introduces a negative charge (polarity) to the framework of zeolites and a Brönsted acid site is obtained if this negative charge is balanced by a proton. The strength of Brönsted acid sites is stronger if they are more isolated from each other.179 Thus, the content of Al3+ in the framework directly determines the amount (i.e., concentration) and the strength of Brönsted acid sites. Moreover, the Si/Al ratios of zeolites can also affect the hydrophilicity/hydrophobicity, stability, and performance of zeolites on catalysis, adsorption, and ion-exchange.18,23,164
2.4.1. Catalysis
Fluid catalytic cracking (FCC) is one of the most important catalytic processes, which converts heavy petroleum to gasoline, diesel, and light gases. USY zeolite is the most efficient and important catalyst in FCC. In the catalytic cracking process, the catalyst needs to be circulated continuously between the reactor and the regenerator at high temperatures in the presence of steam, which requires the ultra-stability of Y zeolite and thus higher Si/Al ratios of Y zeolite. To maximize the activity and selectivity, the Si/Al ratios of Y zeolites need to be optimized.100,180 Therefore, the precise control of Si/Al ratios of Y zeolite has been attracting the researcher's interest. Recently, a series of high-silica Y zeolites have been prepared in the laboratory for cracking and pyrolysis.24,61,100 Y zeolite with a Si/Al ratio of 8.0 exhibited higher conversion than two USY zeolites with Si/Al ratios of 5.3 and 6.9 in n-octane and 1,3,5-triisopropylbenzene (TIPB) cracking.24 Compared to the USY zeolite with lower Si/Al ratios, the USY zeolite with higher Si/Al ratios has fewer acid sites. However, the remaining acid sites are strengthened, which increases the activity and the selectivity of cracking. Very recently, Liu and co-workers investigated the catalytic activity of HS-SY14.3 (Y zeolite with a Si/Al ratio of 7.15) for TIPB cracking and cumene cracking.61 Their results indicated that HS-SY14.3 exhibited both high activity and high selectivity compared to the conventional Y zeolite because of the larger amount of acid sites and higher acid strength in HS-SY14.3. The same group reported that the Y zeolite with Si/Al ratios of up to 8.0 possessed more strong acid sites than commercial USY with Si/Al ratios of 5.3 and 6.9. The former Y zeolite exhibited higher conversion and cracking depth in TIPB cracking and several times higher conversion in n-dodecane cracking than the latter USY reference.23 In the co-pyrolysis of oil sludge and high density polyethylene (HDPE) catalysed by USY zeolites, Calderari and co-workers found that the catalytic cracking process followed a carbenium ion reaction mechanism, which was generated by the removal of a negative hydrogen ion from alkanes or the protonation of olefins.100,181 The species containing carbenium ions cracked to small hydrocarbons on the BASs and Lewis acid sites of USY zeolites and resulted in the formation of new carbonium ions.182,183 Recently, Shen and co-workers discovered that the dealuminated Beta zeolite generated more carbonium ions in the cracking of n-octane due to the enhanced strength of BASs, which is beneficial for hydrocarbon conversion.184 Thus, enhancing the strength of the Brönsted acid by dealumination of zeolites via steaming can improve their catalytic properties for hydrocarbon activation.
Besides enhancing the strength of the Brönsted acid, dealumination of zeolite via steaming can also generate new species that can promote their catalytic performance. For example, Khivantsev and co-workers very recently observed the small alumina clusters of Al1O5 in the micropores of steam dealuminated MFI zeolite, which facilitated the C–H bond breaking of alkane and thus promote the cracking of C–C bonds over BASs.185 Unlike the dealumination process that decreases the amount of BASs but enhances the strength of the remaining BASs, the desilication process generates more Lewis acid sites and mesopores thus increasing the total amount of acid sites and the accessibility of BASs but decreasing the strength of BASs.154 As expected, the dedicated Beta zeolite with low acid strength had low activity on low-density polyethylene (LDPE) and n-octane cracking.154,186
Isomerization, oligomerization, aromatization, and alkylation of the hydrocarbons catalysed by the BASs of zeolites also follow the classical carbenium ion mechanism.107,181 The performances of zeolite catalysts for these reactions strongly depend on the concentration and strength of BASs.107,187–189 The quantity/concentration of BASs determine the number of active sites and the strength of the BASs governs the type of reaction. For example, the dealuminated Beta zeolite can catalyse isobutyl alcohol oligomerization and the conversion of isobutyl alcohol increases with an increase in the Si/Al ratios of Beta zeolite, which is controlled by the dealumination time.107 However, the conversion of isobutyl alcohol decreases significantly if the Beta zeolite is treated by NaOH solution due to the significant loss of BASs. In the transformation of 2-butene, weak Lewis acid sites can result in double-bond migration, while the strong BASs can catalyse cis–trans and skeletal isomerization as well as oligomerization.108 The former reaction is affected by the quantity of the BASs, while the latter reaction is affected by the strength of the BASs. As a result, the chain growth capacities of the butene isomers in the oligomerization reaction catalysed by the untreated Beta zeolite are much higher than those catalysed by the dealuminated Beta zeolite.
Alkylation is catalysed by BASs and the distribution of products is affected by the strength of BASs. For example, lanthanum modified USY zeolite (LaFAU) with a high Si/Al (Si/Al = 6.7) ratio possesses enhanced acid strength, which results in higher cracking and self-alkylation activity. Compared to the LaFAU catalyst with a low Si/Al (Si/Al = 1.2) ratio, such high-silica LaFAU yielded a lower C8 production in isobutane alkylation.190 Naphthalene tert-butylation with tertiary butanol can be catalysed by various dealuminated and/or desilicated MOR zeolites. However, first alkaline-treated and then acid-treated zeolites exhibited enhanced activities because the alkaline-treatment increased the accessibility of the active sites and the acid-treatment reduced the concentration of the strong BASs and increased the strength of the remaining BASs.142 Palkovits and co-workers investigated the synthesis of oxymethylene dimethyl ethers (OMEx oligomers with a chain length of x) over the zeolites *BEA, FAU, MFI, and MOR with various Si/Al ratios and observed a high turnover frequency for the zeolites with high Si/Al ratios.191 As mentioned above, the Si/Al ratio of a zeolite not only determines the concentration/density but also the strength of the BASs. Thus, the optimal Si/Al ratio of a zeolite should be closely related to the specific reaction it catalysed. For example, Li and co-workers reported that ZSM-5 zeolites with lower Si/Al ratios have higher activity in the direct hydration of aromatic alkynes to ketones.192
Dimethyl ether (DME) is a reliable alternative fuel for compression ignition engines and can also be used as an intermediate to produce olefins and chemicals, which can be produced from the dehydration of methanol catalysed by the BASs of zeolites.193–195 However, the trade-off effect between the activity and the selectivity is observed in such a reaction, depending on the Si/Al ratios of the zeolite catalyst.196,197
Hydrogenation of methyl acetate (MeOAc) that is formed via DME carbonylation is a new, efficient route to produce ethanol from syngas.198 DME carbonylation can be catalysed by MOR zeolite in which BASs play an important role.199,200 Yang and co-workers observed that dealuminated MOR zeolites exhibited low catalytic activity but high MeOAc selectivity, indicating that the low BAS density of mordenite is beneficial for the formation of MeOAc.141 However, a trade-off effect was also observed in the DME carbonylation catalysed by the MOR zeolite, i.e., the conversion of DME increased before the Si/Al ratio reached 11.8 and then decreased with a further increase in the Si/Al ratio.201 More investigations revealed that the strength of the BASs in the 8MR side pockets of MOR zeolite decreased with an increase in Si/Al ratios202 and the catalytic performance of MOR zeolites on DME carbonylation is mainly determined by the BASs in the 8MR channels.141,201–203
The conversion of methanol to hydrocarbons (MTH) catalysed by zeolites including methanol to olefins (MTO), methanol to propane (MTP), methanol to gasoline (MTG), and methanol to aromatics (MTA) provides an alternative route for producing basic chemicals on a large scale from non-petroleum sources. However, there is a debate on the aromatic-based hydrocarbon pool (HCP) mechanism and the olefin methylation/cracking mechanism.204–206 Because MTH reactions are catalysed by BASs, the Si/Al ratios of zeolites will definitely affect their catalytic performance. For example, Guisnet and co-workers explained that a lower Si/Al ratio of a zeolite results in a higher density of acid sites; thus a larger number of successive chemical steps occurred along the diffusion path within the zeolite, which favours the condensation reactions and leads to a faster coking rate.207,208 In the MTH reaction catalysed by Beta zeolite, propylene selectivity increased from 50.2% to 60.8% and aromatic selectivity decreased from 3% to 0.3% when the Si/Al ratio was increased to 300 from 150.49 As expected, high-silica ZSM-5 (Si/Al = 181) with low acid density exhibited outstanding catalytic performance in the MTP reaction.77 Moreover, the low acid density due to the high Si/Al ratio prolongs the catalytic lifetime of zeolites in MTH. In the MTO reaction catalysed by H-ZSM-5 and H-ZSM-11 with different Si/Al ratios, the catalytic lifetime increases with increasing the Si/Al ratio due to the low acid density which reduces condensation reactions.209 Liu and co-workers reported that the hierarchical Beta zeolite with a low acid density (Si/Al = 277) showed a much longer catalytic lifetime and slower coking rate in the MTO reaction than the non-hierarchical Beta zeolite with conventional acid density (Si/Al = 228).80
Beta zeolite is a newly developed catalyst for converting aqueous lactic acid (LA) to lactide (LT), a key building block toward a biodegradable and renewable polylactic acid (PLA).210 Yu and co-workers synthesized nanosized Beta zeolites with a Si/Al ratio of 15.5 and nanosized hierarchical Beta zeolite with a Si/Al ratio of 10, which exhibited outstanding LT yields of 74.0% and 77.5%, respectively.75,211 These results suggest that the high density of Brönsted acid sites with better accessibility favours the conversion of LA to LT.
2.4.2. Adsorption/separation
Because of their well-defined microporous structures, BASs, and compensated cations, zeolites are widely employed for gas drying, air separation, hydrogen purification, separation of paraffin isomers, xylene isomers, inert gases, and light hydrocarbons, capture and separation of carbon dioxide, storage of methane and hydrogen, and removal of harmful gases.7 In the framework of zeolites, the proton attached to the O atom linking the Al and Si atoms has an intrinsic affinity to water.
Zeolites are one of the most commonly employed adsorbents in the temperature swing adsorption (TSA) process for natural gas drying. The affinity of protonic zeolites to water is mainly driven by the intrinsic attraction between the polar molecules and the BASs by dipole-field interaction. Furthermore, the presence of cations enhances the affinity of zeolites to polar adsorbate molecules. Thus, the Si/Al ratios of both cationic and protonic zeolites have a significant influence on water adsorption.164,212 The higher the content of Al in the framework, the more cations are required to balance the charge and thus higher water uptake is expected.164 For example, Na balanced CHA zeolite with a Si/Al ratio of 2 exhibited a significant adsorption capacity for water. However, dealuminated Y zeolite with a Si/Al ratio of >200 is highly hydrophobic.+113,164
Unlike the adsorption of polar H2O in zeolites, air separation by zeolites relies on the difference in the stronger quadrupole interaction between the cations and N2versus O2.213,214 Thus, a zeolite with a large capacity of cations would be beneficial for air separation. As expected, Al-rich zeolites were used for air separation such as low-silica X (LSX, Si/Al = 1)215–217 and ZSM-2 (Si/Al = 1.6).218 Recently, Al-rich CHA (Si/Al = 1.6–2.0) was prepared and exchanged with Li for N+2 adsorption.58
The strong local electric field and high basicity of the framework of zeolites cause a strong interaction with acidic CO2 molecules. Al-rich zeolite such as NaLSX with a Si/Al ratio of 1 is a typical CO2 adsorbent.219,220 The affinity to CO2 increases along with a decrease in Si/Al ratios.221 For example, Na-type ZSM-5 with lower Si/Al ratios exhibited a higher affinity to CO2.222 Corma and co-workers reported that the interaction between the adsorbed CO2 molecules and the framework of the LTA zeolite increased with the increase of the Al content.15 Wang and co-workers studied the CO2/CH4/N2 adsorptive separation by CHA zeolites with various Si/Al ratios and discovered that the higher Si/Al ratios result in weaker electrostatic fields and the separation performance for both CO2/CH4 and CO2/N2 decreases with an increase in Si/Al ratios, while the regeneration capacity of CO2 presented an opposite trend because the polarity of CO2 is higher than that of CH4 and N2, and thus the interaction between CO2 molecules and the CHA framework is more sensitive to the variation of the electrostatic field, i.e., the Si/Al ratio.223 However, the high content of Al with a large number of extra-framework cations near the windows of pores might lead to poor capacity for the adsorbates. For example, Na-type GIS zeolites with a Si/Al ratio under 2.2 showed less CO2 uptake (≤0.7 mmol g−1 at 25 °C and 1.0 bar) than those with a Si/Al ratio from 2.5 to 4.7 due to the large number of cations near the 8-ring windows.224
Coal bed methane (CBM) is an unconventional gas with a main composition of CH4, N2, and CO2. Separation of methane has important economic value and environmental significance, which requires the selective capture of CH4 from N2 and CO2. CH4 and N2 have very similar dynamic molecular diameters and thus the enrichment of CH4 from CBM mainly depends on their difference in polarizability. Compared to N2, CH4 has higher polarizability and thus a higher affinity towards polar surfaces. For example, FAU zeolite is a common and efficient adsorbent for the adsorption of CH4 from N2 due to its high polar surface, high specific surface area, and large pore volume.225,226 Azizpour and co-workers studied the influence of the Si/Al ratios in the FAU zeolite on the adsorption of CH4 and N2 and discovered that the adsorption capacity towards CH4 was improved by decreasing the Si/Al ratios because of the formation of more acid sites in the Al-rich FAU zeolite.227
As mentioned above, high-silica zeolite is hydrophobic and has the ability to adsorb organic compounds.228 For example, ZSM-5 zeolite has the ability to adsorb methyl tert-butyl ether (MTBE) from water and the distribution coefficient Kd is improved by increasing the Si/Al ratios.229 Because zeolites have a negative framework, only neutral or positive organic compounds in water can be adsorbed by zeolites. For example, ZSM-5 (Si/Al = 80) and MOR (Si/Al = 200) zeolites both showed high removal ability for neutral and positive nitrosamines in demineralized water.230 However, negative organic compounds can also be adsorbed by zeolites if they can be protonated in solution. For example, rhodamine B (RB) molecules can be protonated in the solution with a pH < 3 and can be adsorbed by Beta zeolite.231 If the pH of the solution is greater than 3, RB converts to a zwitterionic form which causes an electrostatic repulsion between the RB molecules and the Beta zeolite. By increasing the Si/Al ratios of Beta zeolite, the adsorption capacity for RB increases and reaches a maximum value of 4.808 mg g−1 at Si/Al = 9.2.231
In the adsorption of organic compounds from solution by zeolites, solvent molecules will be competitively adsorbed. For example, Jiang and co-workers studied the adsorption of 2,4,6-trichlorophenol (TCP) by high-silica FAU.232,233 It was observed that a supercage accommodated approximately 2 TCP molecules in an Al containing cage and 2.5 TCP molecules in a non-Al containing cage because Al-containing cages adsorbed more water molecules than the cages without Al (Fig. 7), illustrating an increase in the adsorption capacity of FAU zeolite for TCP along with an increase in the Si/Al ratios.232,233
Fig. 7. Arrangements of TCP and water molecules in the non-Al containing supercages of FAU250 (Si/Al ratio in the simulated box is 255) zeolites: (a) 1 TCP, (b) 2 TCP, and (c) 3 TCP molecule(s) per cage at TCP equilibrium concentrations equal to (a) 4.6, (b) 77.6 and (c) 77.6 μmol L−1. The characteristic distance between the center of mass of the benzene rings in the TCP molecules is shown as d1. Reproduced from ref. 232 with permission from Elsevier, Copyright 2020.
Zeolites can also be used for hydrogen storage because of their BASs and the electrostatic field within the channels or cages. In 1998, a study on H2 adsorption at 77 K on NaX zeolites with various Si/Al ratios indicated that the H2 adsorption capacity on NaX zeolite with low Si/Al ratios is larger than that on the NaX zeolite with high Si/Al ratios.234 Later, Chang and co-workers reported that the isosteric heat of H2 adsorption increased with a decrease in Si/Al ratios.235 As expected, the Al-rich CHA zeolite and low-silica X fully exchanged by alkali-metal cations also showed good potential for H2 adsorption.236,237
2.4.3. Ion-exchange
According to the origin of the negative charge of zeolites, the Si/Al ratio of a zeolite will certainly affect the cationic exchange capacity and the location as well as the state of the compensating cations. In principle, a low Si/Al ratio corresponds to a high ion-exchange capacity and the maximum ion-exchange capacity is achieved when the Si/Al ratio of a zeolite is 1.238 For example, the Ag exchange capacity of FAU zeolite with a Si/Al ratio of 2.5 is much higher than that of FAU zeolite with a Si/Al ratio of 40.+239 A zeolite with a low Si/Al ratio possesses a high ion-exchange capacity and therefore facilitates the application in water softening and heavy metal cation removal from water.240 Moreover, the Si/Al ratio of a zeolite can also affect the ion-exchange selectivity. For example, a zeolite with a high Si/Al ratio results in a low anionic field that gives rise to an enhanced selectivity towards monovalent cations,241 while zeolites with a Si/Al ratio of around 1 are highly selective for divalent cations.238 In zeolites with low Al content, the hydration energy is the major factor contributing to selectivity. An ion with higher (negative) hydration energy is preferentially ion-exchanged.242 The selectivity follows the order of Cs > Rb > K > Na > Li. As the Al content increases, the contribution of electrostatic attraction is the major factor for the selectivity and the selectivity is reversed to Na > Li > K > Rb > Cs. Furthermore, high-silica zeolites prefer univalent cations such as alkali ions and NH++++++++++4+.242,243
3. Regulation of Al distributions of zeolites
Because of the strong electromagnetic interaction between the positive charge of the cations and the negative charge of the O near Al, it is expected that the Al distributions of zeolites can be regulated during the synthesis by selecting organic or inorganic SDAs with a specific configuration.244–247 According to the formation process of zeolites, changing the Si/Al ratios of aluminosilicate oligomers can also regulate the Al distributions in the framework of a zeolite.248,249 In addition, the tension of the tetrahedral sites (T-sites) in the framework of a zeolite usually depends on its position. Thus, the removal of Si or Al with high tension via “post-synthesis” or “post-treatment” can also be used to regulate Al distributions.184
According to the origin of Brönsted acidity, the Al distributions in zeolites decide the strength and distributions of BASs and further affect their performance in catalysis, adsorption/separation, and ion-exchange. Basically, the distribution of Al in the framework of a zeolite has three situations: (i) the location of Al atoms at/within the individual crystallographically distinguishable framework T sites; (ii) the spatial correlation of two or more Al atoms, i.e., the distances and the possibility of neighbouring Al atoms cooperating in the formation of active sites; and (iii) the external surface, internal channels, or intersections, as shown in Fig. 8.248 Regulating and determining the distributions of Al atoms in the framework of a zeolite is extremely microscopic and challenging. In general, there are “bottom-up” and “up-bottom” strategies to approach the regulation of Al distributions.
Fig. 8. Three situations of Al distribution: (i) the location of Al atoms at/within the individual and crystallographically distinguishable framework T sites; (ii) the spatial correlation of two or more Al atoms, i.e., the distances and the possibility of neighbouring Al atoms cooperating in the formation of active sites; and (iii) the external surface, internal channels, or intersections.
3.1. “Bottom-up” tuning of the Al distributions of zeolites
The “bottom-up” strategy for tuning the Al distributions of zeolites is mostly performed by changing the components of the initial mixture or the synthesis conditions. The location of Al in the framework of zeolites is related to the intrinsic thermodynamic stability of Al at different T sites and the kinetic factors in gelation and crystallization processes, which include the coordination structure of Al species, Si/Al ratios, OSDAs, cations, and the nature of raw materials.
Al distributions are closely associated with the Si/Al ratios of the framework of a zeolite. For example, it was reported that the proportion of the Al atoms sitting at the intersections of H-MFI zeolite, especially for the Al pairs, increased with a decrease in the Si/Al ratios.250 As for zeolites, there are several types of Al distributions that have been identified: (i) Al–O–Si–O–Al sequences in low silica zeolites, for example in CHA zeolite with a Si/Al ratio below 7,251 in Beta zeolite with a Si/Al ratio of 4.5,252 and in A zeolite with a Si/Al ratio of 1/1; (ii) Al–O–(Si–O)2–Al or Al–O–(Si–O)3–Al sequences in the rings forming cationic sites for bare divalent cations such as Co2+ (denoted as Al pairs); (iii) Al–O–(Si–O)n ≥2–Al sequences accommodating Co2+ hexaaqua complexes in hydrated zeolites, but not bare Co2+ in dehydrated zeolites (denoted as close unpaired Al atoms); and (iv) Al–O–(Si–O)>3–Al sequences with far distant Al atoms located in different rings which are unable to accommodate both bare Co2+ and Co2+ hexaaqua complexes (denoted as single Al atoms).249,253 The close unpaired Al atoms have been identified in SSZ-13, Beta, and ZSM-5 zeolites now.252–254
As for the MFI zeolite, the Al atoms in Al-rich ZSM-5 with a Si/Al of < 10 are predominantly present in the form of Al–O–Si–O–Al sequences.248,255 When the Si/Al ratio of ZSM-5 increases, the relative concentration of Al pairs decreases, while the relative concentration of single Al atoms increases.256 As for silica-rich FER zeolites (Si/Al = 20, 27, 30), the framework contains only isolated Al atoms, while for Al-rich FER zeolites (Si/Al = 8.6 and 10.8), the framework contains Al–O–(Si–O)2–Al sequences.249 Unlike MFI and FER zeolites, Al atoms are more easily distributed in the diagonal position of the 4-ring of the FAU zeolite (Y zeolite, Si/Al = 15, 11, 8.6, 7, 5.8), as confirmed using the density functional theory (DFT) calculations. With the decrease of the Si/Al ratio from 15.0 to 5.8, the Al atoms are, prior to distribution, in the form of a trigonal symmetrical arrangement around the same Si atom.257 While Si-rich *BEA (Si/Al > 12) zeolites do not contain Al–O–Si–O–Al sequences, Al-rich *BEA (Si/Al = 4–5) zeolites contain Al atoms in the form of Al–O–Si–O–Al sequences with concentrations in the range from 40% to 100% of the total Al and the most populated (50–65%) Al atoms are the unpaired Al atoms located in different rings of the channel surface.252 However, regardless of the types of zeolites, the presence of Al–O–(Si–O)2–Al sequences in the zeolite framework is a key feature of high-silica zeolites even when Si/Al is relatively high (>25).249
SDAs including OSDAs and alkali metal cations (e.g., Na) have a great influence on the Al distribution in the framework of zeolites because the Al species are located near the SDAs to balance the positive charge (vice versa). In the ZSM-5 zeolite with a Si/Al of > 10, the Al pairs in close vicinity to quaternary N atoms of TPA are mostly located in β-type 6MRs at the intersection of straight and sinusoidal channels.++258 The pre-organized organic–inorganic composites around TPA (i.e., oligomers) control the distribution of Al atoms in the framework of ZSM-5; that is to say, SDAs, especially OSDAs with specific structures affect the numbers of Al atoms incorporating the framework of zeolites and thus the Al distributions of Al atoms in the framework of zeolites.+258 For example, the Al atoms in ZSM-5 zeolite synthesized with TPA in the absence of Na are predominantly located at channel intersections, while the Al atoms in the ZSM-5 zeolite synthesized with both TPA and Na are located not only at the intersections but also in narrow straight and sinusoidal channels because TPA is exclusively located at the intersections and Na is located within the channels.++++++259 In the synthesis of ZSM-11 zeolite, the addition of Na or Li to the initial synthesis mixture can increase the proportion of the Al atoms at the intersection cavity of ZSM-11.++246 Besides, the introduction of Na in the initial synthesis mixture can also induce the migration of Al atoms from the straight channel to the intersection cavity. In the absence of alkali metal ions, increasing the Si/Al ratios of the framework leads to a more prominent decrease of the Al atoms in the intersection cavity and a relative enrichment of the Al atoms in the straight channel. Introducing alcohols as a pore-filling agent in the synthesis of zeolites creates an Al free environment around the alcohol molecule because of the neutral nature of alcohol molecules. For example, the Al atoms in the ZSM-5 zeolite are preferentially located in the narrow straight and sinusoidal channels instead of at the intersections if the bulky and branched-chain alcohols, such as pentaerythritol (PET) and trimethylolethane (TME) are used as additives.+245,260,261
As mentioned above, an OSDA affects the Al distributions in the framework of zeolites via (1) a strong interaction between the organic cation and the framework oxygen atoms surrounding Al (SDA⋯OAl+−) and (2) occupying the well-defined positions within the void volume of the framework structure. Thus, it is expected that the Al distribution is determined by the location of the SDA species within the zeolite framework during synthesis.262 For example, Okubo and co-workers reported that the occupancy of Al atoms at different T sites in IFR zeolites can be tuned by selecting appropriate OSDAs.263 In the framework of MOR zeolite synthesized with hexamethyleneimine (HMI) and Na as the SDAs, the BASs are enriched in the 8MR channels even at a low Al content in the zeolite framework (i.e., a high Si/Al ratio) because the HMI molecule (kinetic diameter, 0.76 nm) can only be accommodated in the 12MR pores, driving Na into the 8MR channels and thus enriching the Al atoms in the 8MR channels.++201,264 Pinar and co-workers also regulated the Al distribution in FER zeolite directed by TMA by introducing the second OSDA, pyrrolidine, which has a stronger interaction with the framework than TMA and thus prohibits the incorporation of Al atoms into specific positions.++262 Tatsumi and co-workers synthesized RTH-type zeolites in the absence/presence of OSDAs.265 When large OSDA molecules such as 1,2,2,6,6-pentamethylpiperidine (PMP) and N-methyl-piperidine (MP) are used as OSDAs, they are preferentially located in the large non-distorted 8MR pores rather than the distorted 8MR ones, which makes the Al atoms preferentially incorporate into T1 and T2 sites but not the T3 site because the T3 site does not face any 8MR pores. In contrast, in the OSDA-free synthesis of RTH, the Al atoms could be uniformly distributed at the T1, T2, T3, and T4 sites because they are accompanied only by Na. When pyridine (Py) with a size smaller than PMP and MP but larger than Na was used as the OSDA, more Al atoms are incorporated into the T++4 site located at the distorted 8MR pores.265 Moreover, the size of the alkali metal ions may also affect the Al distributions. For example, Fan and co-workers discovered that the proportion of the paired Al atoms in the total Al species in SSZ-13 decreased to 44%, 28%, 16%, and 10% with increasing the radii of alkali metal ions Li, Na, K, and Cs, respectively.++++266 In this case, small rings such as double-six-membered rings (D6Rs) can accommodate only small alkali metal cations Li and Na instead of large alkali metal cations K and Cs. Thus, Li and Na directed more Al atoms into small D6Rs, which accounted for the high content of paired Al species in the resultant SSZ-13.++++++
Considering that the location of the Al atoms in the framework of zeolites can be affected by the size of both OSDAs and alkali metal ions, the Al atoms at specific positions of the framework thus can be regulated by combining OSDAs and alkali metal ions. For example, the SSZ-13 zeolites (Si/Al = 15–30) synthesized in the presence of TMAda cations did not contain any paired Al sites, while introducing Na promoted the formation of paired Al sites and a linear relationship between the number of paired Al sites and the Na/TMAda ratio (0–1) was observed.++++163 The proportion of paired Al reached the maximum at a Na/TMAda ratio of 1 and decreased as the Na/TMAda ratio was between 1 and 2.++++163 Schneider and co-workers reported that the CHA zeolite directed by (a) TMAda only; (b) the combination of TMAda and Na; and (c) the combination of TMAda and K contained (i) one TMAda in each cage; (ii) one TMAda in each cage and Na in the 6MR in an amount linearly proportional to the amount of the paired Al sites in 6MR; and (iii) one TMAda/K in each cage (Fig. 9), corresponding to isolated, paired, and isolated Al, respectively.++++++++++267 Moreover, the type of OSDA (i.e., HMI or cyclohexylamine) occluded in the MCM-49 zeolite also has a significant impact on Al distributions. When HMI was used as the OSDA, the Al distribution at the T sites in MCM-49 followed the ratio of T2 : (T1, T3, T4, T5, T8) : (T6, T7) = 19 : 69 : 12, while this ratio shifted to T2 : (T1, T3, T4, T5, T8) : (T6, T7) = 32 : 63 : 5 when cyclohexylamine was used as the OSDA.244
Fig. 9. Cooperation or competition between organic and inorganic SDAs for Al distributions of CHA zeolites. Reproduced from ref. 267 with permission from the American Chemical Society, Copyright 2020.
Introducing trivalent or tetravalent heteroatoms such as B and Sn into the framework of a zeolite to competitively occupy various T sites with Al atoms is also a feasible route for regulating Al distributions. For example, the Al distribution among the three types of pores in MCM-22 can be regulated by adjusting the content of B incorporated during the synthesis.268 With a proper content of B, BASs can be enriched in the sinusoidal channels rather than in the surface pockets and the supercages. When the B/Al ratio in the initial mixture (Si/Al = 200) reaches 7 or 9, the Al content in the narrow straight/sinusoidal channels is increased.26 In the framework of ZSM-5, B atoms preferentially occupy the positions at the intersections, which enriches the Al atoms in the 10MR channels.269 Moreover, introducing Sn into the framework of ZSM-5 leads to the preferential location of Al atoms in the straight channels rather than at the intersections.28 Recently, Shen and co-workers reported that introducing Mg into the framework of ZSM-5 results in a slight increase in the amount of Al pairs in both the straight channel (from 5% to 10%) and the sinusoidal channel (from 16% to 22%).270
Besides regulating the interaction between the SDA and oligomers, modifying the Al distributions in the oligomers can also alter the Al distributions of the resultant zeolites. For instance, changing the nature of the source materials can also modify the Al distributions in the framework of zeolites. Preferential Al distribution in the narrow straight/sinusoidal channels of ZSM-5 is observed when silica sol is the Si source, while the Al atoms are enriched in larger channel intersections when tetraethyl orthosilicate (TEOS) is used as the Si source.29 Compared to the Al source Al(NO3)3 and Al-tri-sec-butoxide, the Al source AlCl3 or Al(OH)3 resulted in a significant increase in the amount of Al–O–(Si–O)1,2-Al sequences in the same ring of ZSM-5 (<10% for Al(NO3)3 and Al-tri-sec-butoxide, 33% for AlCl3 and 27% for Al(OH)3).254,271 In the interzeolite transformation synthesis, the Al distribution in the resultant zeolite is usually different from that formed by the direct hydrothermal synthesis. For example, the CHA zeolite from the interzeolite conversion of FAU zeolite contains more Al pairs than the CHA zeolite from the direct hydrothermal synthesis.272,273 Recently, Yabushita and co-workers synthesized Al-pair-rich CHA zeolites by using lab-made Al-rich amorphous aluminosilicate containing a large quantity of Al–O–Si–O–Al sequences as the source material.274 Besides cations, halogen anions can also affect the Al location by interacting with SDAs and oligomers.275,276 For example, Cl− anions can induce more Al atoms to sit on the external surface of ZSM-11 crystals while larger Br− or I− anions lead to a uniform distribution of Al species in the inner straight channels.275 Furthermore, the crystallization temperature also has an impact on Al distributions. For example, ZSM-5 obtained at 230 °C exhibits a higher proportion of Al pairs at the intersections than ZSM-5 obtained at 120 °C because the Al substitution at the channel intersection, which competes with the substitution in the straight channel, becomes more feasible at elevated temperature.27
3.2. “Top-down” tuning of the Al distributions of zeolites
As mentioned above, dealumination can selectively remove the Al atoms at specific sites, which can tune the Al distributions in the framework of zeolite. For example, Lercher and co-workers investigated the Al distributions of Beta zeolites with Si/Al = 12.5 (HBEA25) and Si/Al = 75 (HBEA150) dealuminated via leaching with extended X-ray absorption fine structure (EXAFS) and 27Al MAS NMR.277 The results indicated that the distribution of Al T-sites in HBEA150 is significantly different from those in HBEA25. HBEA150 has a lack of population in T7 and T2 sites, which are highly populated in HBEA25. The resilience of the T5 and T6 sites toward the removal of Al is also observed. In the framework of ZSM-5, the Al atoms in straight and sinusoidal-shaped channels are more stable than those at the intersections toward steam treatment at high temperatures.278 Shen and co-workers reported a mild-acid-assisted thermal/hydrothermal dealumination method for Beta zeolite.184 In such a study, Beta zeolite was first steamed, which eliminated most of the framework Al, especially Al atoms at the T2, T5, T6, and T7 sites. In the subsequent acid-calcination treatment, the extra-framework Al (EFAL) and the framework Al in the defect sites, especially the Al at T5, T6, and T9 sites, are removed. Very recently, Liu and co-workers developed a low-pressure SiCl4 treatment (LPST) strategy to replace the framework Al atoms at the T1, T2, and T4 sites of the 12MR channels of MOR zeolite and discovered that the resultant AlCl3 species migrate into the 8MR channels and directly reinsert into the T3 sites as a new framework Al through the reaction between AlCl3 and silanol defects (Fig. 10).203
Fig. 10. (a) Schematic of a typical treatment process, showing the directional migration of framework Al into T3 sites of the MOR zeolite via LPST. (b) Topology of MOR and steric configuration of SiCl4 and AlCl3 molecules with a kinetic diameter of 7.0 and 6.7 Å, respectively. Reproduced from ref. 203 with permission from Wiley, Copyright 2022.
3.3. Methods for determining the Al distributions of zeolites
Chemical environments of Al atoms are diverse and complex which are affected by the topology of zeolites; therefore an unambiguous determination of the Al distributions in the framework of zeolites is challenging.
So far, solid-state 27Al MAS NMR has been the main technique to determine the Al distributions in the framework of high-silica zeolites, which is sensitive to the local environments of the Al atoms in the framework of zeolites and is in principle capable of distinguishing between 27Al species at different T sites.279 However, due to the strong quadrupolar interactions of 27Al (I = 5/2) nuclei and the inhomogeneous distributions of 27Al species, the resolution of the 27Al MAS NMR spectra is limited and can only show whether the Al site is in the framework (tetrahedral) or the extra-framework Al (octahedral).280,281 Several advanced 27Al MAS NMR techniques have been developed to improve the resolution of the NMR spectra, such as using higher magnetic fields (>18 T), multiple-quantum magic angle spinning (MQMAS), and multidimensional NMR.282 By applying these techniques, new information about the Al sites in the framework of zeolites has been obtained. For example, high-field 27Al MQMAS NMR analyses of different ZSM-5 zeolites allowed the identification and assignment of at least 12 different 27Al signals associated with different T sites.278,283 MQ NMR spectra collected at 18.8 T revealed four non-equivalent T-sites of MOR zeolites.203 Furthermore, the 2D (two-dimensional) 29Si–27Al D-HMQC (dipolar-mediated heteronuclear multiple-quantum coherence) spectrum was employed to investigate the Al incorporation in the crystallization of MCM-49 (MWW-type) and ZSM-5 zeolites.73,284 Moreover, the 27Al MAS NMR spectra acquired at 18.8 T and 13C{27Al}/1H{23Na} REAPDOR (rotational echo adiabatic passage double resonance) MAS NMR, 2D 27Al 3Q (triple quantum) MAS, 1H–13C HETCOR (heteronuclear correlation) MAS, and 1H–27Al/1H–23Na D-RINEPT (dipolar refocused-insensitive nuclei enhancement by polarization transfer, INEPT) MAS NMR experiments were employed to analyses the Al distributions in MCM-49 zeolite with different OSDAs.244 2D 27Al MQMAS NMR spectra were used to determine the Al sites in ZSM-11 zeolite and four signals were distinguished.246 2D 27Al 3QMAS NMR was used to analyse IFR zeolite and distinguished four resonances that presumably corresponded to the different Al locations at four T sites in IFR zeolite, which can suppress and correctly deal with the quadrupolar effect of 27Al.263
Recently, Bokhoven and co-workers exploited the resonant (anomalous) scattering near the Al K edge (1.56 keV or 7.95 Å) to obtain a quantitative assignment of Al to the T sites in a zeolite framework.285 By combining the conventional X-ray powder diffraction data collected at the Al K edge, the distribution of Al over the T sites in a zeolite framework structure can be determined quantitatively and unambiguously. This method can be applied even to zeolites with Si/Al ratios as high as 15.
Techniques such as XRD and NMR mainly offer bulk average of the information of a specific sample. Although a number of tomographic techniques have been developed to give 3D reconstructions, none of them currently offer sub-nanometer spatial resolution.286 These techniques also have difficulty differentiating the primary elements consisting of zeolites (i.e., Al, P, and Si) due to their close and light atomic masses. However, atom probe tomography (APT) can provide three-dimensional compositional mapping with sub-nanometre resolution and sensitivity in the range of parts per million (ppm) for all elements.287 For example, Weckhuysen and co-workers employed APT to determine the Al distributions of zeolites (Fig. 11).286,288,289 It is shown that Al atoms are non-randomly distributed within the ZSM-5 crystals with a most probable Al–Al neighbour distance of 18 ± 6 Å, an average Al density of 0.025 atoms per nm3, and a relative strength of non-randomness of 0.7. Because there are 12 and 24 crystallographically distinguishable framework T sites in the MFI structure with symmetry of Pnma and P21/n, respectively, the current results suggested that the Al atoms preferentially locate at some crystallographically distinguishable framework T sites in ZSM-5 crystals due to the preference of thermodynamics. In severely steam-treated ZSM-5 crystals, they found that the Al distribution is also non-random. However, such a technique can only provide local information, beyond the concept of distribution in topology.
Fig. 11. (a) Si and O and (b) Al atom distributions from within a steam-treated zeolite ZSM-5 crystal. The Cr and Pt layers serve as a fiducial marker to mark the position of the zeolite crystal surface. Bounding box dimensions are 46 × 45 × 126 nm3. (c) Si/Al ratio as a function of distance from the surface marked by a black dashed line. A least-squares polynomial fit is shown as a green dotted curve to guide the eye to the distribution. The Pt and Ga intensities as well as the Si/Al ratio values are averaged over each cross-section when moving from the top to the bottom of the analysed volume. (d) Al distribution of isolated subvolume (red dashed box) viewed normal to the arrow direction in (b). Bounding box dimensions 53 × 58 nm2. (e) Plane view of the isolated subvolume outlined by the dashed box in (d). Bounding box dimensions 26 × 67 nm2. (f) 1D composition profile with associated error bars taken across the arrowed black dashed line in (d). Reproduced from ref. 288 with permission from Springer Nature, Copyright 2015.
Labelling can be employed to determine Al distributions indirectly. Molecules such as carbon monoxide (CO), Py, and 2,6-di-tert-butylpyridine (DTBPy) can be used as probes of the acid site location.290,291 The probe molecules with different sizes could be adsorbed on different accessible acid sites, which can be further characterized by FT-IR or 13C NMR and thus reveal the Al distributions.291 Moreover, certain divalent cations such as Co2+ are practical experimental probes for paired Al in zeolites because single Al atoms cannot accommodate Co2+ while Al pairs can accommodate bare Co2+ and hydrated Co2+ and close unpaired Al can only accommodate hydrated Co2+. For example, with this method, the amount of single Al atoms, Al pairs, and close unpaired Al atoms in SSZ-13 can be calculated as follows:456where [Comax] is the Co concentration in the zeolite maximally exchanged by the Co2+ hexaaqua complex, [Cobare] is the concentration of bare Co2+ in the maximally bare Co2+ exchanged zeolite, and [CoD6R] is the concentration of bare Co2+ in the hexagonal prism.248,253,292 This method has been successfully used for determination of Al pairs in CHA, MFI, and MEL.27,245,246,267,292,293 Co2+-type zeolites can also be studied by UV-vis spectroscopy in which bands in the UV-vis spectra correspond to the Co2+ ions coordinated to the Al atoms at different positions.209 The role of ion-exchanged Cu2+ is similar to that of Co2+ but more sensitive to the conditions.248 Upon ion-exchange, the Cu2+ species compensate for the negative charge of the framework and the formation of Cu-complexes simply depends on the location of the Al atoms. Besides Co2+ and Cu2+, Mo species can also be used to distinguish Al atoms from Si atoms because the Mo species have strong interaction with Al atoms and the Mo species can be determined from the atomic-resolution transmission electron microscope (TEM) images (Fig. 12).294 In addition, CO2 can also be used to probe the location of Al atoms in the framework of zeolites.295 Recently, Chiesa and co-workers reported that paramagnetic ZnI is also a convenient spin label that can be used to determine the Al distributions within the framework of a zeolite by pulse dipolar spectroscopy (PDS).31
Fig. 12. (a) A representative integrated differential phase-contrast scanning transmission electron microscopy (iDPC-STEM) image of Mo/ZSM-5, showing the presence of off-center contrast in many 10MR channels. (b–d) Zoomed-in areas 1, 2, and 3 of (a), respectively, corresponding to three scenarios: an empty channel (b), and channels containing a MoO3H cluster bound at the T8 site (c) and at the T1 site (d). Each panel includes the raw image (top), the calculated structural model (middle), and the simulated projected electrostatic potential (bottom). Si: blue, O: red, Al: green, Mo: pink, and H: white. (e) Intensity line profiles of the images in (b)–(d), across the areas as represented by the red dashed rectangle. (f) Statistics of Al occupancy at different T sites, based on the results of one hundred channels. The labels “E” and “C” represent empty channels and channels with an on-center extra contrast, respectively. Reproduced from ref. 294 with permission from Wiley, Copyright 2019.
3.4. Impact of Al distributions on the performance of zeolites
For a given zeolite, the performance of catalysis, adsorption-separation, and ion-exchange is significantly affected not only by Si/Al ratios but also by Al distributions.
3.4.1. Catalysis
In catalytic cracking, BASs are the active sites. Thus, the activity and selectivity depend on the Al distributions in the framework of zeolites. For example, Beta zeolites with selectively removed Al atoms on T5, T6, and T9 sites show a higher gasoline yield, while those with selectively removed Al atoms at the T2, T5, T6, and T7 sites show a higher diesel yield in vacuum gas oil (VGO) catalytic cracking.184 In the catalytic cracking of 1-octene over ZSM-5 zeolite, the acid sites at the intersections have a positive contribution to the bimolecular reactions involving carbenium cations and olefins.296 Cracking of n-hexane over ZSM-5 exhibits a similar trend. The acid sites at the intersections and/or external surfaces enhance the formation of aromatics and coke.260 Alkylation of hydrocarbons catalysed by BASs of zeolites is similar to the cracking reaction. The acid sites at the intersections of ZSM-5 led to higher benzene conversion, xylene selectivity, and stability in the alkylation of benzene with methanol.245 Moreover, previous studies indicated that the relatively “close” Al atoms providing “close” protonic sites can enhance oligomerization and hydrogen transfer reactions leading to aromatics during the catalytic cracking of 1-butene, while “single” Al atoms prefer olefin cracking.271
DME carbonylation to MeOAc is catalysed by the BASs of zeolite (e.g., MOR). T3 Al sites located in the 4MRs of the 8 and 12MR channels of MOR zeolite are responsible for the activity and selectivity in DME carbonylation.297 Selectively coupled removal of T3 and T4 Al sites results in low activity and prolonged catalyst lifetime. Moreover, the rate of DME carbonylation exhibited a linear dependence on the amount of BASs located in the 8MR channels.201 The Al atoms at the T3 positions of the MOR 8MR channels are the active sites for DME carbonylation, which leads to the significantly prolonged catalytic lifetime and the higher selectivity of methylamine (MA), while the BASs at the 12MR channels result in coke formation and frequent deactivation.203,297 Stronger acid sites at the 8MR channels in MOR zeolite could reduce the activation barriers of CO insertion to form acetyl groups, thus promoting the activity of DME carbonylation.202
MTO is another important BAS catalysed reaction. The catalytic performance of the RUB-13 zeolite in MTO is closely related to Al distributions and the acid density.298 The Al atoms at the T1 and T2 sites are the effective acid sites that are accessible to the MTO reaction. The catalytic lifetime of H-RUB-13 increases almost linearly with an increase in the number of effective acid sites, although the selectivity to lower olefins may decrease considerably with an increase in the acid density (Fig. 13). As for ZSM-11 in the MTO reaction, increasing the proportion of Al atoms in the intersection cavity favours the aromatic cycle that preferably produces ethylene and aromatics, while the Al atoms in the straight channels favour the alkene cycle.246 A high proportion of Al–O–Si–O–Al sequences in the framework of zeolites showed a short catalytic life in the MTO reaction compared to that with a low proportion.273 Al atoms located across the 4MR in CHA zeolite generally result in weaker acids and higher activation barriers, whereas Al atoms located across the 6MR or at certain 8MR positions decrease activation barriers.299 Therefore, the alkanol dehydration rates are enhanced on the paired Al sites located in the 6MR of CHA.
Fig. 13. (I) Effect of the Si/B ratio (Si/Al ∼ 170) on the aluminium sitting in the framework and the catalytic lifetime of the H–Al–B-RUB-13-170-n series zeolites in MTO. (II) Effect of the Si/Al ratio (Si/B ≈ 17) on the aluminium sitting and the catalytic lifetime of the H–Al–B-RUB-13-m-17 series zeolites in MTO. (III) Relationship between the selectivity to propene and the catalytic lifetime of H–Al–B-RUB-13-m-n in MTO and the density of effective acid sites (represented as the number of aluminium atoms per unit cell sited at the T1 and T2 sites): (a) the H–Al–B-RUB-13-170-n series zeolites; (b) the H–Al–B-RUB-13-m-17 series zeolites. The MTO reactions were carried out at 400 °C with a methanol WHSV of 1.0 h−1; the lifetime was determined as the reaction time when the methanol conversion decreased to 95% and the steady state selectivity to propene was reported at about 90 min on stream. Reproduced from ref. 298 with permission from the Royal Society of Chemistry, Copyright 2020.
Selective catalytic reduction of nitrogen oxides with ammonia (NH3-SCR) is not an acid but a Cu2+ catalysed reaction in which the activity and durability of the catalyst are significantly affected by the ion-exchange sites, i.e., the Al location of the SSZ-13 zeolite.266,300,301 In Cu-SSZ-13, Cu(NH3)2+-pairs in CHA zeolite have been suggested to activate oxygen during low-temperature NH3-SCR. The Al-distributions in the zeolite are found to clearly affect the probability for Cu-pair formation, which is the most favourable with an intermediate Al–Al distance of about 7.5 Å.302 The amount of the Cu2+ species located in D6MRs increased linearly with the content of the paired Al species in the D6MRs of the CHA zeolite, which enhanced the catalytic activity for SCR of NO by NH3.266
3.4.2. Adsorption/separation
According to the equilibrium adsorption mechanism, it is expected that Al distributions will affect the adsorption energy. For example, Bulánek and co-workers investigated the influence of composition on the equilibrium CO2 adsorption in alkali metal exchanged NaY with a Si/Al ratio of ∼2.5 by combining spectroscopic, calorimetric, and theoretical studies, which yielded fine details on the CO2 adsorption complexes and corresponding gas–solid interaction energy.303 It was found that all CO2 molecules are adsorbed on the cations at sites II (centre of the 6MR) of NaY via dispersion interactions. At a Si/Al ratio of ∼2.5, the 6MR can hold only one or two Al atoms.304 The alkali metal cation in site II containing only one Al atom has a larger partial charge than the cation in the ring having two Al atoms, which therefore has a higher polarizing capability and adsorption heat (around 2–3 kJ mol−1) of CO2 on such a site confirmed by theoretical calculations. However, this influence is relatively mild compared to that caused by the change in the Si/Al ratio of a zeolite. Lin and co-workers investigated the effects of Si/Al ratios and Al distributions of Brönsted-acid zeolites on the adsorption selectivity of n-alkanes via configurational-bias Monte Carlo simulations.305 The adsorption selectivity in their studies is defined as the ratio of equilibrium adsorption constants for central C–C bonds relative to terminal bonds of n-alkanes. Their results revealed that Al distributions have a significant influence on adsorption selectivity, as much as 2-fold in the adsorption selectivity for n-hexane in ZSM-5. The sitting of Al atoms and their spatial proximity are two factors that substantially influence adsorption selectivity. Al atoms in close proximity have a synergistic effect on adsorbing the central C–C bonds of n-hexane, which results in a higher adsorption selectivity relative to isolated Al atoms. In the framework of ZSM-5, T1, T2, and T12 sites are the three most selective T-sites for the adsorption of n-hexane via interacting with the central C–C bond of n-hexane, while T4, T5, T6, and T7 sites are the four least selective T-sites. These results indicate that the adsorption selectivity can be controlled by regulating the Al distributions in the framework of zeolites.
3.4.3. Ion-exchange
The influence of Al distributions on the performance of the ion-exchange of zeolites is mainly reflected in the capture of divalent ions. Al pairs provide ion-exchange sites that can capture divalent cations in zeolites because of the two close negative charges. Single Al atoms are able to accommodate exclusively monovalent cationic species, while Al pairs can stabilize divalent cations and divalent species. In addition, the Al pairs can also create two close and cooperating monovalent centers.253CHA zeolite with enriched Al pairs exhibits better adsorption performance for the divalent cation Sr2+, a radioactive pollutant,274 and Fe ions, active sites of the partial oxidation of methane.272
4. Summary and outlook
This review summarized the strategies and methodologies for regulating the Si/Al ratios and Al distributions of zeolites, commonly used as well as newly developed characterization techniques for determining the Si/Al ratios and Al distributions of zeolites, and their impacts on applications involving catalysis, adsorption/separation, and ion-exchange. The “bottom-up” methodologies follow the principle of regulating the Si/Al ratios of aluminosilicate oligomers. “Top-down” methodologies including steam treatment and etching with acid and/or base are the straightforward approaches to removing Al atoms or Si atoms at a specific location in the framework. Although such processes would produce a large amount of acid/base wastewater, they are suitable for large-scale industrial production. The wet chemical method (i.e., ICP-AES) and XRF are the main methods for determining the Si/Al ratio in the laboratory and industry. In addition, FT-IR and XRD based methods are also developed even though their applications are limited to a specific zeolite and Si/Al ratio range. Regulating Al distributions such as sitting at a specific location and the formation of Al pairs is very challenging in the field of zeolites and is far from precise control at the present stage. Changing the Si/Al ratios and Al distributions of zeolites will undoubtedly affect their performance in catalysis, adsorption/separation, and ion-exchange. However, their correlations are far from being clarified yet.
For the synthesis of zeolites, broadening the Si/Al ratios and controlling the Al distributions are highly desired, which can tune the activity, selectivity, and durability of zeolites. Considering that zeolites are assembled by oligomers with specific Si/Al ratios and Al distributions, the efforts on regulating the Si/Al ratios and Al distributions of zeolites should focus on how to make specific oligomers with desired Si/Al ratios and Al distributions and achieve the successful assembly of such oligomers. New methodologies are desired to break the typical Si/Al limitation of zeolites and predict the Al distributions, which include high throughput techniques combined with computation predictions306–308 and machine learning.309 Moreover, developing new characterization techniques to unambiguously distinguish the Si and Al atoms in the framework of zeolites and the Al distributions is greatly important, which is the base to establish a clear relationship between the Al distribution and the performance of zeolites. Considering the fact that there does not exist any experimental technique to directly determine the location of aluminum or to distinguish the silicon and aluminum at framework T sites, especially within equivalent crystallographic framework T sites so far, there is an imminent and urgent need to combine theoretical calculations/simulations with in situ/operando characterization techniques at the molecular/atomic level.
In the end, the precise control of the Si/Al ratios and Al distribution of zeolites requires a molecular-level understanding of the formation mechanism of zeolites and the process of oligomer assembling, which can be achieved by combining the multi-scale simulation and the in situ characterization of the zeolite crystallization process.
Author contributions
Conceptualization: J. Yu and W. Yan; writing – original draft: J. Li; validation: M. Gao; writing – review & editing: J. Yu and W. Yan.
Conflicts of interest
The authors declare no conflicts of interest.
Acknowledgments
We thank the National Natural Science Foundation of China (Grants 22288101, 21920102005, U1967215, and 21835002), the National Key Research and Development Program of China (Grants 2021YFA1500401 and 2021YFA1501202), and the 111 Project (B17020) for supporting this work.
Zeolite Market Size, Share & Trends Analysis Report By Application (Catalyst, Adsorbent, Detergent Builder), By Product (Natural, Synthetic), By Region (North America, Europe, APAC, CSA, MEA), And Segment Forecasts, 2022–2030 , Report 978-1-68038-601-1, Grand View Research
A. Osatiashtiani, B. Puértolas, C. C. S. Oliveira, J. C. Manayil, B. Barbero, M. Isaacs, C. Michailof, E. Heracleous, J. Pérez-Ramírez, A. F. Lee, K. Wilson
C. Lei, Z. Dong, C. Martinez, J. Martinez-Triguero, W. Chen, Q. Wu, X. Meng, A. N. Parvulescu, T. De Baerdemaeker, U. Muller, A. Zheng, Y. Ma, W. Zhang, T. Yokoi, B. Marler, D. E. De Vos, U. Kolb, A. Corma, F. S. Xiao
Angew. Chem., Int. Ed., 59 (2020), pp. 15649-15655
X. Xiong, D. Yuan, Q. Wu, F. Chen, X. Meng, R. Lv, D. Dai, S. Maurer, R. McGuire, M. Feyen, U. Müller, W. Zhang, T. Yokoi, X. Bao, H. Gies, B. Marler, D. E. De Vos, U. Kolb, A. Moini, F.-S. Xiao
P. A. S. Moura, E. Rodríguez-Aguado, D. A. S. Maia, D. C. Melo, R. Singh, S. Valencia, P. A. Webley, F. Rey, M. Bastos-Neto, E. Rodríguez-Castellón, D. C. S. Azevedo
Because of its great efficiency and widespread application, reverse osmosis (RO) is a popular tool for water desalination and purification. However, traditional RO membranes have a short lifespan due to membrane fouling, deterioration, decreased salt rejection rate, and the low water flux with aging. As a result, membrane modification has received a lot of attention recently, with nanomaterials being extensively researched to improve membrane efficacy and lifespan. Herein, we present an in-depth analysis of recent advances of RO membranes modification utilizing nanomaterials. An overview of the various nanomaterials used for membrane modification, including metal oxides, zeolites, and carbon nanomaterials, is provided. The synthesis techniques and methods of integrating these nanomaterials into RO membranes are also discussed. The impacts of nanomaterial change on the performance of RO membranes are addressed. The underlying mechanisms responsible for RO membrane enhancements by nanomaterials, such as improved surface hydrophilicity, reduced membrane fouling via surface repulsion and anti-adhesion properties, and enhanced structural stability, are discussed. Furthermore, the review provides a critical analysis of the challenges and limitations associated with the use of nanomaterials to modify RO membranes. Overall, this review provides valuable insights into the modification of RO membranes with nanomaterials, providing a full grasp of the benefits, challenges, and future prospects of this challenging topic.
Ni catalysts supported on 4A, 5A, 13X, ZSM-5, and BEA zeolites were prepared using the vacuum-heating method for CO2 methanation. These support materials play a pivotal role in shaping the catalysts' properties and their catalytic performance. High-resolution high-angle annular dark-field scanning transmission electron microscopy (HAADF-STEM) and energy-dispersive X-ray spectroscopy (EDS) mappings suggest a significant concentration of Ni nanoparticles situated on the external surfaces of catalysts with low Si/Al ratios zeolites (Ni-4A, Ni-5A, and Ni-13X). These Ni nanoparticles exhibit characteristics of weaker metal-support interaction, lower metal reduction temperatures, and moderate H2 adsorption activity. Moreover, these low Si/Al ratio zeolites demonstrate robust CO2 adsorption activity. These properties endow Ni-5A and Ni-13X catalysts with heightened CO2 conversion (70.4–70.9%) and methane selectivity (92.4–96.4%). In contrast, high Si/Al ratio zeolite-based catalysts (Ni-ZSM-5 and Ni-BEA) exhibit smaller Ni particles, strong metal-support interaction and weaker CO2 adsorption activity, resulting in reduced CO2 methanation activity and decreased methane selectivity (71.2–73.4%). The normalized CO2 conversion rate presents a correlation with the average Ni particle size.
Zeolites have become promising adsorbents for wastewater treatment due to their enhanced adsorption capacity, stability of crystalline structure, high porosity and surface area. One of the primary goals of our study was to assess the effectiveness of employing NaY zeolite as a sorbent and potential solid matrix for immobilizing radionuclides. In this study NaY faujasite zeolite was obtained by hydrothermal synthesis and characterized by X-Ray diffraction (XRD), N2 adsorption–desorption, scanning electron microscopy (SEM) and energy dispersive spectroscopy (EDS) methods. The prepared zeolite had NaY faujasite crystalline structure, characterized by developed surface area (370 m2/g) with micro-mesoporous structure, and spherical-like morphology with particles of 1–4 μm in diameter. The isotherms adsorption modeling on Cs, Sr+2+, Co2+, Pb2+ and La3+ ions was performed. The isotherm well described by Langmuir equation with maximum adsorption capacity of q(Cs) = 1,9 mmol/g, q(Sr+2+) = 3,75 mmol/g, q(Co2+) = 1,82 mmol/g, q(Pb2+) = 2,54 mmol/g, q(La3+) = 3,83 mmol/g. Thermal behavior of metal-saturated adsorbents by differential thermal analysis (DTA) and thermal gravimetric (TG) techniques was studied. Each metal examined in this paper is responsible for the stable formation of radionuclides (137Cs, 90Sr, 60Co, La - generally, the group of active lanthanides was modelled, Pb - uranium fission residues) that are generated during the operation of nuclear power plants. To optimize sintering regimes, it has been proposed to achieve sorption saturation of stable ions such as Cs, Sr, Co, La, and Pb and transfer them into solid matrices. It was shown that the consolidation temperature for the obtained samples varies in the range of 935–1040 °C.
In order to obtain extended storage life of food-grade materials and better barrier properties against environmental factors, a multilayer plastic packaging (MLP) is often used. The multilayer packaging plastics are labelled as “other” (SPI#7) category, and are manufactured with a combination of barrier plastics, rigid plastics and printing surface. Owing to their complex composition and difficulty in separating the layers of MLP, its mechanical recycling is challenging. In this study, MLP wastes (MLPWs) were collected from zero-waste garbage collection center of IIT Madras, India, and thoroughly characterized to determine their composition and plastic types. MLPWs were characterized using various physico-chemical methods such as thermogravimetric/differential scanning calorimetric analysis, Fourier transform infrared spectroscopy, bomb calorimetry, and proximate and ultimate analyses. The MLPWs were mainly made up of polyethylene (PE) and polyethylene terephthalate (PET). Further, the non-catalytic and zeolite-catalyzed fast pyrolysis of these MLPWs were studied using analytical pyrolysis coupled with gas chromatograph/mass spectrometer (Py-GC/MS). The non-catalytic fast pyrolysis of MLPWs primarily produced a mixture of aliphatic and alicyclic hydrocarbons, while zeolite catalyzed fast pyrolysis resulted in the formation of mono-aromatic hydrocarbons (MAHs). The activity of HZSM-5, zeolite Y (HY) and zeolite beta (Hβ) catalysts were evaluated, and the salient products were quantified. The yields of MAHs like benzene, toluene, ethylbenzene and xylene using the zeolites followed the trend: HZSM-5 (14.9 wt%) > HY (8.1 wt%) > Hβ (7.8 wt%), at 650 °C. The use of HZSM-5 resulted in highest yield of MAHs, viz. 16.1 wt%, at the optimum temperature of 550 °C and MLPW-to-catalyst ratio of 1:15 (w/w). The superior activity of HZSM-5 is due to its nominal acidity and larger pore size of 4.24 nm, as compared to HY and Hβ. The MAHs yield from three other types of MLPWs varied in the range of 9–16 wt%. The present study demonstrates a promising pathway for the catalytic upcycling of highly heterogeneous MLPWs in the context of circular economy.
New synthesis methods for selectively inserting heteroatoms into desired crystallographic sites, together with new experimental tools that determine their location, are more than needed. A recent review by Yu et al. summarises current state-of-the-art Al chemistry in zeolites, discussing our ability to incorporate Al into zeolite frameworks, modify Si/Al ratios in different zeolites, and highlight some examples of the impact on catalytic performance [40]. Template-free zeolite synthesis does not need to burn off organic structure-directing agents post-synthesis.
Zeolites today are a unique and highly successful class of catalytic materials, but their role in future low-carbon scenarios comes into question. This perspective article summarises the authors' joint view on zeolite chemistry's future direction for catalytic applications to stimulate discussion identifying pillars on which the scientific community should focus. Particular challenges discussed here include i) our view of the zeolite synthesis focused on new structures with optimised textural properties and design of zeolite catalysts with precise control of the location of active sites; ii) discussion of current, mostly new industrial, requests for zeolitic catalysts; iii) emerging catalytic applications in which zeolites should play a key role; and last but not least iv) opportunities for new types of microporous solids. Although some of these are rather challenging, with many barriers to overcome, we suggest fostering research on these directions as the key to maintaining the crucial role of zeolite as catalysts. Discussion on the future role of zeolite science and technology is organised in consideration of three possible future scenarios: (i) a low-carbon BAU (business-as-usual) scenario and (ii) two advanced scenarios, which differ in terms of the degree of circularity (low and high, LC and HC respectively), and (iii) level of substitution of fossil fuels with alternative energy and carbon sources. Trends characterising these scenarios and their impact on zeolite science and technology are discussed to provide the readers with the elements, tools and clues to identify priorities in research and application of zeolite catalysts.
