Methods of synthesizing chabazite zeolites with controlled aluminum distribution and structures made therefrom

Abstract

A method of synthesizing chabazite zeolites with controlled aluminum distribution. The method utilizes a source of an organic structure-directing agent, a source of an inorganic structure-directing agent, a source of aluminum and a source of silicon to form a synthesis gel which is subjected to a crystallization process to crystallize a chabazite zeolite with controlled aluminum distribution. A chabazite zeolite structure with controlled aluminum distribution. The structure contains zeolite crystal lattice framework containing silicon, aluminum, and oxygen; and extra-framework positions containing non-divalent chemical species such that each aluminum atom in the zeolite crystal lattice framework is in an isolated configuration. Another variant of this structure wherein a fraction of the aluminum atoms in the zeolite crystal lattice framework positions are not in an isolated configuration and hence oxygen atoms associated with aluminum atoms in the fraction can bind with the non-aluminum cations in the extra-framework positions.

Claims

1. A method of synthesizing chabazite zeolites with controlled aluminum distribution, the method comprising: determining a relationship between ratio of saturation Co.sup.2+/Al obtained from an ion exchange isotherm of a crystallized chabazite zeolite, and ratio (Na.sup.+/Al) of number of sodium ions to number of aluminum atoms in the crystallized chabazite zeolite obtained from elemental analysis of the crystallized chabazite zeolite; providing a desired value for ratio (Na.sup.+/Al) of number of sodium ions to number of aluminum atoms in a crystallized chabazite zeolite; adding a source of N,N,N-trimethyl-1-admantylammonium ions (TMAda.sup.+) and to water to form an aqueous solution and homogenizing the aqueous solution for a first time period; adding sodium aluminate to the homogenized aqueous solution to form an intermediate agent and homogenizing the intermediate agent for a second time period to form an aluminum-containing intermediate agent; adding a source of silicon to the aluminum-containing intermediate agent to form an aluminosilicate-containing intermediate agent and homogenizing the aluminosilicate-containing intermediate agent for a third time period to form a synthesis gel; wherein a correlation of Na.sup.+/ TMAda.sup.+to the saturation Co.sup.2+/Al and the relationship between ratio of saturation Co.sup.2+/Al obtained from an ion exchange isotherm of a crystallized chabazite zeolite, and ratio (Na.sup.+/Al) of number of sodium ions to number of aluminum atoms in the crystallized chabazite zeolite obtained from elemental analysis of the crystallized chabazite zeolite is utilized to determine the molar ion ratio Na.sup.+/TMAda.sup.+in the synthesis gel; and subjecting the synthesis gel to a crystallization process to crystallize a chabazite zeolite, wherein the determined molar ion ratio Na.sup.+/TMAda.sup.+results in the desired value for ratio (Na.sup.+/Al) of number of sodium ions to number of aluminum atoms in a crystallized chabazite zeolite.

2. The method of claim 1, wherein the amounts of N,N,N-trimethyl-1-adamantylammonium hydroxide and sodium hydroxide are such that the molar ratio of sodium cations to N,N,N-trimethyl-1-adamantylammonium cations are in a molar ratio in the range of 0.01 to 4.00.

3. The method of claim 2 wherein the source of silicon is one of colloidal silica, a silicon alkoxide compound, fumed silica, amorphous silica, and aluminosilicate.

4. The method of claim 1, wherein the source of silicon is sodium silicate such that the molar ratio of sodium cations to N,N,N-trimethyl-1-adamantylammonium cations is in the range of 0.01 to 4.00.

5. The method of claim 1, where in the first time period, the second time period and the third time period are each in the range of 1 second to 48 hours.

6. A method of synthesizing chabazite zeolites with controlled aluminum distribution, the method comprising: adding a source of N,N,N-trimethyl-1-admantylammonium ions (TMAda.sup.+) and a source of sodium ions (Na.sup.+) to water to form an aqueous solution and homogenizing the aqueous solution for a first time period; adding sodium aluminate to the homogenized aqueous solution to form an intermediate agent and homogenizing the intermediate agent for a second time period to form an aluminum-containing intermediate agent; adding a source of silicon to the aluminum-containing intermediate agent to form an aluminosilicate-containing intermediate agent and homogenizing the aluminosilicate-containing intermediate agent for a third time period to form a synthesis gel; and subjecting the synthesis gel to a crystallization process to crystallize a chabazite zeolite, wherein the determined molar ion ratio Na.sup.+/TMAda.sup.+results in the desired value for ratio (Na.sup.+/Al) of number of sodium ions to number of aluminum atoms in a crystallized chabazite zeolite.

7. The method of claim 6, wherein the source of the N,N,N-trimethyl-1-admantylammonium ions is an aqueous solution of N,N,N-trimethyl-1-adamantylammonium hydroxide and the source of the sodium ions is sodium hydroxide.

8. The method of claim 7, wherein the amounts of N,N,N-trimethyl-1-adamantylammonium hydroxide and sodium hydroxide are such that the molar ratio of sodium cations to N,N,N-trimethyl-1-adamantylammonium cations are in a molar ratio in the range of 0.01 to 4.00.

9. The method of claim 6, wherein the source of silicon is one of colloidal silica, a silicon alkoxide compound, fumed silica, amorphous silica, and aluminosilicate.

10. The method of claim 6, where in the source of silicon is one of colloidal silica, a silicon alkoxide compound, fumed silica, amorphous silica, and aluminosilicate.

11. The method of claim 6, where in the first time period, the second time period and the third time period are each in the range of 1 second to 48 hours.

Description

BRIEF DESCRIPTION OF DRAWINGS

(1) Some of the figures shown herein may include dimensions. Further, some of the figures shown herein may have been created from scaled drawings or from photographs that are scalable. It is understood that such dimensions or the relative scaling within a figure are by way of example, and not to be construed as limiting.

(2) FIG. 1A shows ion exchange isotherms for the sample SSZ-13(15, 0) (circles) and the sample SSZ-13(15, 1) (squares) at varying exchange molarities of Co(NO.sub.3).sub.2. The dashed line is a Langmuir isotherm for Co.sup.2+ exchange of SSZ-13(15, 0), and the dotted line is a Langmuir isotherm for Co.sup.2+ exchange of SSZ-13(15, 1).

(3) FIG. 1B shows ion exchange isotherms for the sample SSZ-13(15, 0) (circles) and the sample SSZ-13(15, 1) (squares) at varying exchange molarities of NaCl. The dashed line is a Langmuir isotherm for Co.sup.2+ exchange of SSZ-13(15, 0), and the dotted line is a Langmuir isotherm for Co.sup.2+ exchange of SSZ-13(15, 1).

(4) FIG. 2 shows the UV-Visible absorption spectra for the d-d transition of Co.sup.2+ (centered at 19,000 cm.sup.1) in Co.sup.2+-exchanged SSZ-13 zeolites with Co/Al values of 0.084 (black trace), 0.08 (dark grey trace), 0.047 (grey trace), 0.024 (light grey), and 0.021 (faint grey trace).

(5) FIG. 3 shows the fraction of paired Al atoms (measured by titration with Co.sup.2+) as a function of the synthesis gel charge density on SSZ-13(15) samples synthesized by fixing the total gel charge (circles) and by letting the total gel charge vary (squares).

(6) FIG. 4 shows the ordering of Si and Al atoms around the organic structure-directing agent N,N,N-trimethyl-1-admantylammonium (TMAda.sup.+), with and without Na.sup.+ present.

(7) FIG. 5 is a plot of the Co.sup.2+/Al ratio at saturation Co.sup.2+ exchange levels, versus the Na.sup.+/Al ratio in the crystallized chabazite product.

(8) FIG. 6 is an illustration of a zeolite structure showing all the framework aluminum atoms in an isolated configuration.

(9) FIG. 7 is an illustration of a zeolite structure wherein only a fraction of the framework aluminum atoms are an isolated configuration.

DETAILED DESCRIPTION

(10) For the purposes of promoting an understanding of the principles of the disclosure, reference will now be made to the embodiments illustrated in the drawings and specific language will be used to describe the same. It will nevertheless be understood that no limitation of the scope of the disclosure is thereby intended, such alterations and further modifications in the illustrated device, and such further applications of the principles of the disclosure as illustrated therein being contemplated as would normally occur to one skilled in the art to which the disclosure relates.

(11) In this disclosure, chabazite zeolite structures with controlled aluminum distribution and methods of making them are described. For purposes of this disclosure, a zeolite structure with controlled aluminum distribution is one in which the placement and arrangement (i.e. distribution) of aluminum atoms in its framework is controlled through method of preparation.

(12) Further, certain terms, abbreviations and designations are now defined to help understand this detailed description. CHA stands for Chabazite; SSZ-13 is a trade name familiar to those of ordinary skill in the art and refers to a chabazite structure containing primarily silicon, aluminum, and oxygen,

(13) In this disclosure, we focus on the synthesis of CHA zeolites (SSZ-13), which are used commercially as catalysts in their H-form for methanol-to-olefins (MTO) and after Cu or Fe exchange for the selective catalytic reduction of mobile-source NO.sub.x pollutants with ammonia. CHA zeolites contain one unique T-site and double 6-membered ring (D6R) building units that interconnect to form 8-MR windows (0.38 nm diameter) that limit transport into larger cages (0.82 nm diameter, 18 T-atoms per cage), and are typically synthesized in the presence of N,N,N-trimethyl-1-adamantylammonium cations (TMAda.sup.+) as organic SDAs that become occluded within CHA cages during crystallization. Each zeolite sample is denoted as H-SSZ-13(X,Y) where X is the Si/Al ratio in the solid and Y is the Na.sup.+/TMAda.sup.+ ratio in the synthesis gel. For purposes of this disclosure, a synthesis gel is a mixture of the aluminum and silicon sources and the structure-directing agents, which is converted to a zeolite when subjected to a crystallization process.

(14) Common approaches to synthesize high-silica SSZ-13 zeolites of varying Si/Al ratio (>10) involve preparing gels with equimolar amounts of Na.sup.+ and TMAda.sup.+ cations but with varying Al content, as was used here to synthesize. H-SSZ-13(15, 1) and H-SSZ-13(25, 1) and to compare with a low-silica H-SSZ-13(4.5) prepared using low-silica FAU zeolites as the Al source. These H-SSZ-13 samples were equilibrated with aqueous Cu(NO.sub.3).sub.2 or Co(NO.sub.3).sub.2 solutions of increasing molarity to obtain partially-metal-exchanged zeolites, with solid Cu/Al or Co/Al ratios measured by atomic absorption spectroscopy and residual H.sup.+ content measured by their selective titration with NH.sub.3 and subsequent temperature-programmed desorption. Cu exchanged predominantly as Cu.sup.2+ cations for two H.sup.+ sites until Cu/Al ratios of 0.21, 0.09 and 0.05 on H-SSZ-13(4.5), H-SSZ-13(15, 1) and H-SSZ-13(25, 1), respectively, and then as monovalent [CuOH].sup.+ complexes for one fr site. In contrast, Co exchanged exclusively as Co.sup.2+ cations with Langmuirian adsorption behavior until saturation, as shown in FIG. 1 of this specification. Sole presence of UV-Visible absorption bands for Co.sup.2+ d-d transitions (19,000 cm.sup.1) that increased linearly in area with Co content. FIG. 2 shows the UV-Visible absorption spectra for the d-d transition of Co.sup.2+ (19,000 cm.sup.1) in Co-exchanged SSZ-13 zeolites with Co/Al exchange values of 0.084 (black trace), 0.08 (dark grey trace), 0.047 (grey trace), 0.024 (light grey), and 0.021 (faint grey trace).

(15) Saturation Co.sup.2+/Al and Cu.sup.2+/Al values were identical on all three H-SSZ-13 zeolites, and similar to the fraction of Al pairs in double 6-MR locations of CHA that have been predicted from statistical simulations assuming a random Al distribution subject to Lowenstein's rule. These findings demonstrate that Co.sup.2+ cations can selectively titrate paired Al in zeolites, and that synthesis gels containing equimolar amounts of Na.sup.+ and TMAda.sup.+ crystallized SSZ-13 zeolites with a random framework Al distribution at different bulk compositions, which was surprising and unexpected considering the non-random siting of Al atoms reported for CHA and other zeolites.

(16) In experiments leading to this disclosure, SSZ-13 zeolites (Si/Al=15, 25) crystallized from gels comprising equimolar amounts of Na.sup.+ and TMAda.sup.+ contained a detectable fraction of paired Al atoms, defined here in function as two Al atoms separated by either one or two Si atoms in a 6-MR since both atomic configurations stabilize exchanged Co.sup.2+ and Cu.sup.2+ cations with similar energetic preferences according to density functional theory. The maximum concentration of Al atoms beyond which incorporation of additional Al causes unavoidable formation of next-nearest-neighbor Al arrangements (AlOSiOAl) can be calculated from the topological density of zeolite frameworks, and suggest that SSZ-13 zeolites with Si/Al>7 can be prepared (in theory) to contain exclusively isolated Al atoms. It has been demonstrated in the literature that one TMAda.sup.+ cation, which contains a large hydrophobic adamantyl moiety (0.70 nm in diam.) covalently bound to a singly-charged quaternary ammonium center, occupies the void space within one CHA cage. The synthesis of SSZ-13 in the presence of TMAda.sup.+ without Na.sup.+ has been demonstrated in fluoride media for Si/Al ratios between 20-400. However, no conclusions regarding the Al distribution or site isolation were made. Thus, in this disclosure, it is postulated that SSZ-13 crystallized solely in the presence of TMAda.sup.+, based on steric constraints and the minimization of electrostatic repulsion between anionic framework charges introduced by Al atoms, should enable the separation and isolation of one Al atom per CHA cage (Si/Al=17), on average.

(17) In experiments leading to this disclosure, the crystallization of SSZ-13 zeolites, in the absence of alkali cations, was attempted with varying gel Si/Al ratios (10-60) and all other synthesis variables held constant. Precursor gels with Si/Al ratios between 15 and 30 crystallized phase-pure CHA zeolites with solid Si/Al ratios between 14.5-26.1, with undetectable amounts of extra-framework Al. SSZ-13(15, 0), SSZ-13(20, 0), SSZ-13(25, 0), and SSZ-13(30, 0) samples (including 7 independent syntheses of SSZ-13(15, 0)) were measured by NH.sub.3 titration to have H.sup.+/Al ratios >0.9, yet these samples were unable to exchange detectable amounts of Co.sup.2+, reflecting the nearly complete incorporation of Al atoms within the framework, but in locations sufficiently isolated from each other so as to be incapable of divalent cation exchange. The Co.sup.2+ exchange isotherm measured on SSZ-13(15, 1) shows Langmuirian adsorption behavior reaching a saturation value of Co/Al=0.08 with a calculated fraction of paired Al sites from a fit Langmuir isotherm of 0.087, while SSZ-13(15, 0) showed negligible Co.sup.2+ exchange under identical exchange conditions, as shown in FIG. 1A. However, Na.sup.+ exchange isotherms on both SSZ-13(15, 0) and SSZ-13(15, 1) reach similar saturation values of Na/Al=0.90 and 0.95, respectively, as shown in FIG. 1B. .sup.29Si MAS NMR obtained on SSZ-13(15, 0) and SSZ-13(15, 1) look nearly identical and indicate high occupancies of Si(0Al), Si(1Al), and SiOH groups, but not of Si(2Al) groups, suggesting that AlOSiOAl linkages are preferentially avoided in favor of Al(OSi).sub.2OAl groups, as has been observed in FAU zeolites. However, even these Al(OSi).sub.2OAl linkages are not formed when only TMAda.sup.+ is used to synthesize SSZ-13. SSZ-13 zeolite gels with Si/Al<15 formed amorphous phases when only TMAda.sup.+ cations were present, yet formed phase-pure SSZ-13 (Si/Al=9) when additional amounts of Na.sup.+ cations were added, suggesting that such high concentrations of AlO.sub.4.sup. tetrahedra led to anionic gel charge densities higher than TMAda.sup.+ cations alone were capable of stabilizing, consistent with charge density mismatch theory. Additionally, attempts to crystallize SSZ-13 zeolites with Si/Al>30 in hydroxide media with only TMAda.sup.+ also resulted in amorphous phases, presumably because crystallization was frustrated by the requirement to form anionic framework vacancy defects to balance excess cationic charges in occluded TMAda.sup.+ cations (those not balanced by framework Al), in light of the ability of SSZ-13 to crystallize with low Al densities (Si/Al=60 to ) in the presence of fluoride anions.

(18) In the experiments of this disclosure, in the synthesis of SSZ-13(15, 0) and SSZ-13(15, 1) the charge density of the synthesis gel, which is defined here as the cationic charge density, has been manipulated by changing the ratio of two equally charged cations having different molecular (or atomic) volumes, i.e. Na.sup.+/TMAda.sup.+ ratio, while maintaining a constant total gel charge, (Na.sup.++TMAda.sup.+)/Al, constant Si/Al ratio, and constant gel pH. It has been reported in literature that modification of the Na.sup.+ cation concentration in the synthesis of ZSM-5 zeolites led to changes in the number of paired Al atoms, as measured by saturation with ion-exchanged Co.sup.2+ cations, but different anionic species (OH.sup., Cl.sup., NO.sub.3.sup.) and sources of Si and Al precursors were not controlled for, which also influence the Al distribution. In this disclosure, an important aspect is to systematically vary the ratio of Na.sup.+/TMAda.sup.+ (i.e., charge density) between 0-3 at a fixed composition (Si/Al=15), total synthesis gel charge ((Na.sup.++TMAda.sup.+)/Al=7.5) and pH (OH.sup./Al=7.5). On all samples synthesized at a constant gel charge density and a gel Si/Al ratio of 15, the final solids product Si/Al molar ratio was constant at a Si/Al=14.5. The number of TMAda.sup.+ molecules per CHA cage was measured by thermogravimetric analysis (TGA), and the amount of Na.sup.+ remaining on the as-synthesized SSZ-13 product was measured by atomic absorption spectroscopy (AAS). The total (TMAda.sup.++Na.sup.+)/Al ratio on the zeolite products was near unity on every sample, indicating that every Al atom is charge balanced by either a TMAda.sup.+ or a Na.sup.+ cation. FIG. 3 of this disclosure shows the Co/Al ratio at saturation Co.sup.2+ exchange levels, as a function of the synthesis gel cationic charge density.

(19) As the charge density in the gel increases (increasing Na.sup.+/TMAda.sup.+), the number of paired Al sites also increased to a maximum at Na.sup.+/TMAda.sup.+=1. Beyond this ratio, the number of paired Al sites begins to decrease towards zero, at which point a phase transition occurs from the CHA framework to the MOR framework between Na.sup.+/TMAda.sup.+=2.0 and 2.5. One possible explanation of this phenomenon is that the TMAda.sup.+ cation can position isolated Al in the framework, because its cationic charge is localized at one end of the molecule and the bulky organic adamantyl group prevents multiple TMAda.sup.+ from occupying the same void space. Na.sup.+ cations, which have a large charge density, are capable of being occluded within the D6R and occupying space near the cationic end of the TMAda.sup.+ molecule, their addition to the synthesis gel may position neighboring framework Al atoms while minimizing the overall electrostatic repulsion of the zeolite as shown in FIG. 4. As the concentration of Na.sup.+ increases towards a Na.sup.+/TMAda.sup.+=1, the distribution of Al in the framework becomes more random as the increasing number of Na.sup.+ atoms are arranged throughout the zeolite structure. FIG. 5 is a plot of the Co.sup.2+/Al ratio at saturation Co.sup.2+ exchange levels, versus the Na.sup.+/Al ratio in the crystallized chabazite product. Referring to FIG. 5, it can be seen that the Na.sup.+ retained on the final SSZ-13 products depends linearly with the amount of Co.sup.2+ exchanged, suggesting that in the regime bounded by Na.sup.+/TMAda.sup.+=0 and 1, every additional Na.sup.+ atom found on the SSZ-13 product is responsible for forming an Al pair. As the Na.sup.+/TMAda.sup.+ ratio increases further, the charge density reaches a critical point (Na.sup.+/TMAda.sup.+=1) at which the Al begins to become more isolated, which in this disclosure is proposed to be due to competition for Na.sup.+ with a separate phase forming in the synthesis gel containing Na and Al. As the concentration of Na.sup.+ further increases, it becomes increasingly favorable for Na.sup.+ to be incorporated into this second phase until the charge density of the synthesis gel eventually reaches a critical point where the CHA framework is no longer capable of outcompeting the second phase, during which a phase change occurs to form the MOR phase.

(20) Additionally, a second set of syntheses in which the total charge of the synthesis gel (i.e. (Na.sup.++TMAda.sup.+)/Al) was allowed to vary, in order to examine the influence of the total cationic charge on the Al isolation. The SSZ-13 solids crystallized from a gel Si/Al=15, in which the total cationic charge was allowed to vary, contain solid Si/Al ratios that systematically decreased with increasing total charge. This behavior contrasts the SSZ-13 samples of constant Si/Al ratio=15, prepared with synthesis gels containing fixed cationic charge. The fraction of paired Al, as measured by Co.sup.2+, showed a similar trend to the SSZ-13 samples synthesized at a constant total gel charge (FIG. 3) indicating that Al isolation is controlled by the cationic charge density of the synthesis gel, and not by the total cationic charge in the gel. A similar series of SSZ-13 syntheses was also repeated for a Si/Al=25 and trends similar to those shown by SSZ(15) are observed suggesting that the dependence of Al distribution (isolated vs. paired) on synthesis gel charge density occurs for other Si/Al ratios.

(21) In experiments leading to this disclosure, zeolites synthesized from different sources of aluminum were found to contain a fraction of aluminum atoms in an isolated configuration. The fraction varied between 0.5 to 1.0 in the samples studied. For purposes of this disclosure, an isolated configuration is a configuration in which each aluminum atom in the zeolite framework is separated from its next nearest aluminum atom neighbor in the framework, such that these two aluminum atoms are not able to behave as an exchange site for an extra framework divalent cation.

(22) Isolated Al atoms among different tetrahedral sites (T-sites) and zeolite topologies in periodic density functional theory models generate protons of equivalent ensemble-averaged deprotonation energy (DPE), a rigorous and probe-independent measure of Brnsted acid strength that influences reactivity in acid catalysis, while paired Al atoms generate weaker protons with higher DPE values (by 11-108 kJ mol.sup.1) according to quantum chemical calculations on embedded cluster models. Steam dealumination of faujasite zeolites (FAU; up to 1198 K for 2.5 h under steam) results in the formation of ultra-stable FAU that are increasingly resistant to further steam dealumination and .sup.29Si magic angle spinning nuclear magnetic resonance (MAS NMR) show the preferential removal of Al atoms in paired configurations, leading to FAU zeolites that contain solely isolated Al atoms. Increasing the fraction of isolated Al atoms in H-SSZ-13 zeolites, as monitored by .sup.29Si MAS NMR, caused by changing the Si/Al ratio (2.3-67) led to increasingly stable conversions as a function of time on stream for the MTO reaction (6.1 v % CH.sub.3OH, 548-598 K). Additionally, the arrangement of framework Al atoms controls the specification of extra framework cations that behave as catalytic active sites, as in the case of monovalent [CuOH].sup.+ complexes exchanged at isolated Al and divalent Cu.sup.2+ cations exchanged at paired Al in chabazite (CHA) zeolites for the selective catalytic reduction of NOx (x=1, 2) with NH.sub.3 in automotive emission control. Thus, synthetic methods to control the proximity of framework Al atoms can open new opportunities to tailor the structure, stability and catalytic behavior of a given zeolite, especially at fixed elemental composition.

(23) Based on the above detailed description, a method of synthesizing chabazite zeolites with controlled aluminum distribution can be described. The method begins by adding a source of an organic structure-directing agent and a source of an inorganic structure-directing agent to water to form an aqueous solution and homogenizing the aqueous solution for a first time period. The first time period can be in the range of 1 second to 48 hours. In a preferred embodiment, the source of the organic structure-directing agent can be an aqueous solution of N,N,N-trimethyl-1-adamantylammonium hydroxide and the source of the inorganic structure-directing agent can be sodium hydroxide. In one embodiment, the amounts of N,N,N-trimethyl-1-adamantylammonium hydroxide and sodium hydroxide are such that the molar ratio of sodium cations to N,N,N-trimethyl-1-adamantylammonium cations can be in a molar ratio in the range of 0.01 to 4.00.

(24) Next, a source of aluminum is added to the homogenized aqueous solution to form an intermediate agent and homogenizing the intermediate agent for a second time period to form an aluminum-containing intermediate agent. The second time period can be in the range of 1 second to 48 hours. There are several sources that can be used advantageously as a source of aluminum. These include, but not limited to sodium aluminate aluminum hydroxide, aluminum nitrate, aluminosilicate, aluminum chloride, aluminum phosphate and aluminum isopropoxide.

(25) Next, a source of silicon is added to the aluminum-containing intermediate agent to form an aluminosilicate-containing intermediate agent. The source of silicon can be one of colloidal silica, a silicon alkoxide compound, fumed silica, amorphous silica, and aluminosilicate.

(26) The aluminosilicate-containing intermediate agent formed is then homogenized for a third time period to form a synthesis gel. The third time period can be in the range of 1 second to 48 hours. The synthesis gel is then subjected to a crystallization process to crystallize a chabazite zeolite.

(27) It is another objective of this disclosure to describe a chabazite zeolite structure with controlled aluminum distribution. In such a chabazite zeolite structure, each aluminum atom in crystal lattice framework positions of the zeolite framework is in an isolated configuration, such that the zeolite cannot bind with a divalent cation in an extra-framework position. Such a structure is illustrated in FIG. 6. Referring to FIG. 6, Al atoms are in isolated configuration and can only bind with a monovalent cation, such as, but not limited to H.sup.+. For purposes of this disclosure, a lattice framework position is a crystallographic position for an atom (e.g., silicon, aluminum) that is tetrahedrally-bonded to four atoms in the crystalline zeolite lattice.

(28) Depending on the amount of inorganic structure-directing agent added during crystallization of zeolite as described in this disclosure, non-aluminum inorganic cations can be present in extra-framework positions of the zeolite. For purposes of this disclosure, an extra-framework position is to be understood to mean a position that is not covalently bonded to four atoms in the crystalline zeolite lattice. Atoms, ions and complexes located in extra-framework positions of a zeolite typically refer to those found in the pore spaces of the solid, and not those incorporated into the lattice framework itself.

(29) These non-aluminum inorganic cations can include, but not limited to sodium cations, calcium cations, potassium cations, magnesium cations, cobalt cations, copper cations, and lithium cations, and combinations thereof. In such a scenario, only a fraction of the aluminum atoms in the crystal lattice framework positions of the zeolite are in an isolated configuration and this fraction cannot exchange a divalent cation in an extra-framework position. Thus, it is yet another objective of this disclosure to describe a different class of chabazite zeolite structures with controlled aluminum distribution, wherein by virtue of non-aluminum inorganic cations being present in extra-framework positions of the zeolite, only a fraction of the aluminum atoms in the crystal lattice framework positions of the zeolite framework are in an isolated configuration and this fraction cannot bind with a divalent cation in an extra-framework position. Such a structure is illustrated in FIG. 7. Referring to FIG. 7, a fraction of the aluminum atoms in the zeolite structure are not in isolated configuration and can bind with a divalent cation, such as, but not limited to, Co.sup.2+. The fraction of such aluminum atoms in the zeolite lattice framework in an isolated configuration is in the range 0.0-1.0. In some embodiments, the range of this fraction can be 0.5-1.0.

(30) It should be noted that it is possible in some embodiments that the cations in the extra-framework positions can include aluminum cations.

(31) It should be noted that the method described here demonstrates synthetic procedures that directly and systematically control the Al distribution in chabazite zeolites at a fixed Si/Al ratio, by only manipulating the type and amount of structure-directing agents used.

(32) While the present disclosure has been described with reference to certain embodiments, it will be apparent to those of ordinary skill in the art that other embodiments and implementations are possible that are within the scope of the present disclosure without departing from the spirit and scope of the present disclosure. Thus, the implementations should not be limited to the particular limitations described. Other implementations may be possible. It is therefore intended that the foregoing detailed description be regarded as illustrative rather than limiting. Thus, this disclosure is limited only by the following claims.