Theoretical and Spectroscopic Evidence of the Dynamic Nature of Copper Active Sites in Cu-CHA Catalysts under Selective Catalytic Reduction (NH3-SCR-NOx) Conditions.

The dynamic nature of the copper cations acting as active sites for selective catalytic reduction of nitrogen oxides with ammonia is investigated using a combined theoretical and spectroscopic approach. Ab initio molecular dynamics simulations of Cu-CHA catalysts in contact with reactants and intermediates at realistic operating conditions show that only ammonia is able to release Cu+ and Cu2+ cations from their positions coordinated to the zeolite framework, forming mobile Cu+(NH3)2 and Cu2+(NH3)4 complexes that migrate to the center of the cavity. Herein, we give evidence that such mobilization of copper cations modifies the vibrational fingerprint in the 800-1000 cm-1 region of the IR spectra. Bands associated with the lattice asymmetric T-O-T vibrations are perturbed by the presence of coordinated cations, and allow one to experimentally follow the dynamic reorganization of the active sites at operating conditions.

Removclass="Chemical">al of class="Chemical">n class="Chemical">nitrogen oxides (NO) from exhaust gases in diesel vehicles is currently achieved through their selective catalytic reduction (SCR) with ammonia, the NH3–SCR–NO reaction, using copper-exchanged zeolites, in particular, Cu-SSZ-13 and Cu-SAPO-34 with the CHA framework, as catalysts.[1−4] N2 and H2O are the harmless products formed by reaction of NO with NH3 in the presence of either O2 in the case of the standard SCR reaction or NO2 in the so-called fast SCR reaction:

class="Chemical">Although the research effort devoted to this process iclass="Chemical">n receclass="Chemical">nt years has provided coclass="Chemical">nclass="Chemical">n class="Chemical">siderable understanding of the reaction mechanism in Cu-CHA catalysts,[5−15] there is still some uncertainty regarding the exact location of the active sites, the Cu+ and Cu2+ cations, and their mobility as a function of oxidation state and reaction conditions, mainly temperature and gas feed composition. Herein, we give solid evidence for a unique vibrational fingerprint in the 800–1000 cm–1 region of the IR spectrum, which is associated with mobilized copper cations under reaction conditions.

The class="Disease">CHA framework is composed of hexagoclass="Chemical">nclass="Chemical">n class="Chemical">al prisms or double 6-ring (d6r) units that link to form large cavities accessible through small 8-ring (8r) windows (Chart ). Isolated Cu2+ cations preferentially occupy positions in the plane of the 6-ring (6r) units compensating two negative charges, while monovalent Cu+ or [Cu2+(OH)−]+ species can also be placed at the 8-ring (8r) windows.[15−19] Operando XAS and XES measurements during the NH3–SCR–NO reaction have shown that at low temperature, up to ∼473 K, NH3 coordinates strongly to Cu+ cations and releases them from their positions at the 6r or 8r rings to form mobile Cu+(NH3)2 complexes.[10,15,20] Formation of transient Cu+(NH3)2–O–O–Cu+(NH3)2 dimeric species has been claimed as a key step in the low temperature oxidation of Cu+ to Cu2+,[8−10] and experimental evidence of such dimer formation has been recently provided by XAS and diffuse reflectance UV–vis spectroscopies.[14] Alternatively, the oxidation of isolated, coordinated to the framework Cu+ to Cu2+ in the absence of NH3 was identified by EPR and IR spectroscopies in Cu-SSZ-13 and Cu-SAPO-34 catalysts at room temperature,[11] and similar activation energies have been reported for the two processes by means of DFT calculations.[11−13] These data indicate that there is not a unique clear picture of the state of copper cations in Cu-CHA catalysts under different reaction conditions at this moment, which inspired us to perform the current combined experimental/theoretical study to find a unique fingerprint for the state of copper under reaction conditions.

Chart 1

Illustration of the cha Cage Showing the 6r and 8r, a Cu+ Cation in the 6r and the Compensating Proton (a); Static DFT Optimized Geometry of Cu+ and Cu2+ in the 6r of Cu-SSZ-13 (b) and Cu-SAPO-34 (c)a

class="Chemical">Al, P, O, class="Chemical">n class="Chemical">Si, Cu, and H atoms depicted in gray, yellow, red, orange, green, and white, respectively.

At first instance, to gain inclass="Chemical">sight oclass="Chemical">n the state aclass="Chemical">nd mobility of the active class="Chemical">n class="Chemical">sites of Cu-CHA catalyst under different NH3–SCR–NO reaction conditions, we studied the interaction of Cu+ and Cu2+ cations in Cu-SSZ-13 and Cu-SAPO-34 catalyst models with the reactant molecules NO, O2, NO2, and NH3, and with some relevant reaction intermediates found in our previous mechanistic study,[11] using ab initio molecular dynamics (AIMD) simulations at two different temperatures, 298 and 523 K. Figure gives an overview of the average distances between Cu+ or Cu2+ cations and the plane of the 6r and the root-mean-square deviations (RMSD) of the Cu+ or Cu2+ position with respect to the ensemble average in each system to enable a quantification of the cation mobility (see values in Table S1) and some representative snapshots during the AIMD simulations which were most frequently visited for Cu-SAPO-34. Similar snapshots for Cu-SSZ-13 are taken in Figure S1 of the SI. In the absence of adsorbed molecules, Cu+ and Cu2+ cations are located in the plane of the 6r, forming three or four strong bonds with the framework oxygen atoms of both Cu-SSZ-13 and Cu-SAPO-34 (Chart ). The average Cu-6r distance is larger for Cu+ than for Cu2+ in all cases, and the RMSD of Cu+ increases at 523 K while that of Cu2+ remains smaller and constant, reflecting the stronger interaction of the divalent cation with the negatively charged framework.

Figure 1

(a) Snapshots of the interaction of Cu+ and Cu2+ cations in Cu-SAPO-34 with O2, NO, NO2, and NH3 molecules and with nitrite and nitrate intermediates corresponding to geometries which are most frequently visited during AIMD runs of 100 ps at 298 K. (b) Overview of the average distances between Cu+ or Cu2+ cations and the plane of the 6r and root-mean-square deviations (RMSD) of the Cu+ or Cu2+ position with respect to the ensemble average at 298 K (blue) and 523 K (green) in each system. Al, P, O, Si, Cu, N, and H atoms depicted in gray, yellow, red, orange, green, blue, and white, respectively.

(a) Snapshots of the interaction of class="Chemical">Cu+ aclass="Chemical">nd class="Chemical">n class="Chemical">Cu2+ cations in Cu-SAPO-34 with O2, NO, NO2, and NH3 molecules and with nitrite and nitrate intermediates corresponding to geometries which are most frequently visited during AIMD runs of 100 ps at 298 K. (b) Overview of the average distances between Cu+ or Cu2+ cations and the plane of the 6r and root-mean-square deviations (RMSD) of the Cu+ or Cu2+ position with respect to the ensemble average at 298 K (blue) and 523 K (green) in each system. Al, P, O, Si, Cu, N, and H atoms depicted in gray, yellow, red, orange, green, blue, and white, respectively.

The interaction of class="Chemical">Cu+ with oclass="Chemical">ne class="Chemical">n class="Chemical">O2, NO, or NO2 molecule results in an adsorption state where the Cu+ cation forms a new bond with an O or N atom of the adsorbed molecule, while it remains coordinated to two framework oxygen atoms of the 6r, although somewhat displaced toward the cavity. Two guest NO and NO2 molecules can also bind strongly to Cu+ at 298 and 523 K leading to slightly larger average Cu-6r distances and increased mobility (RMSD) (Figures and S1, and Table S1) but without detaching it from its position in the 6r. The adsorption of NH3 on Cu+ modifies strongly its interaction with the catalyst framework so that NH3 and Cu+ move out of the plane of the 6r and get close to the 8r. Depending on the temperature and the number of NH3 molecules present in the cages, the cation mobility increases significantly.

After adsorption of one class="Chemical">NH3 moleclass="Chemical">n class="Chemical">cule in Cu-SAPO-34 at 298 K, the Cu+ cation is slightly displaced from the 6r but remains coordinated with a single oxygen of the 6r while making a new coordination with NH3, with an almost linear N–Cu–O geometry (Figure ), in agreement with previous results on Cu-SSZ-13.[16] The mobility increases significantly at 523 K, allowing NH3 and Cu+ to diffuse through the 8r window to the adjacent empty cage after ∼50 ps. Adsorption of a second NH3 molecule breaks the last Cu–O bond present in the Cu+–NH3 system, and a linear Cu+(NH3)2 complex placed freely in the cavity is obtained. At 298 K, the complex forms as soon as the two NH3 molecules approach the Cu+ cation and remains stable during the whole simulation. At this temperature, the complex remains relatively close to the 6r due to the electrostatic interaction between Cu+ and the negatively charged oxygen atoms of the framework (Cu-6r distance and its RMSD value are also tabulated in Table S1). At 523 K, the mobility of the Cu+(NH3)2 complex increases substantially, and after 50 ps, it diffuses through the 8r window to the adjacent empty cavity while remaining close to the negatively charged framework (Figure ).

Figure 2

Scatter plot of the position of Cu+ in the SAPO-34 cavity and probability distributions of the Cu-8r distance in AIMD simulations obtained over a 100 ps run for the interaction of Cu+ with one (left) and two (right) NH3 molecules at 298 and 523 K. Snapshots of the complexes are also shown. The ξ-axis represents the projection of the position of Cu+ on the vector normal to the average plane of the 8r.[25] The centroid of the 8r is the reference coordinate such that when Cu+ is in the center of the 8r, ξ is equal to 0, indicated with a slashed vertical line.

Scatter plot of the poclass="Chemical">sitioclass="Chemical">n of class="Chemical">n class="Chemical">Cu+ in the SAPO-34 cavity and probability distributions of the Cu-8r distance in AIMD simulations obtained over a 100 ps run for the interaction of Cu+ with one (left) and two (right) NH3 molecules at 298 and 523 K. Snapshots of the complexes are also shown. The ξ-axis represents the projection of the position of Cu+ on the vector normal to the average plane of the 8r.[25] The centroid of the 8r is the reference coordinate such that when Cu+ is in the center of the 8r, ξ is equal to 0, indicated with a slashed vertical line.

In the next step, we determined the effect of the oxidation state of class="Chemical">copper oclass="Chemical">n the mobility of class="Chemical">n class="Chemical">Cu2+ cations interacting with O2, NO, and NH3, which is further stabilized by two negative charges in the 6r. Molecular O2 does not bind to Cu2+, and only one NO molecule can interact with Cu2+ forming a stable system that only displaces slightly the Cu2+ cation out of the 6r plane (Figures and S1). Two NH3 can bind to Cu2+, but the interaction is not strong enough to break the Cu–O bonds, and therefore, the Cu2+ cation remains in the 6r plane, although with a high mobility (see RMSD values in Table S1 of the SI). Four NH3 molecules are able to detach Cu2+ out of the 6r and form a square planar Cu2+(NH3)4 complex that remains stable in the cavity both at 298 and 523 K (Figures and S1).

class="Chemical">Nitrites aclass="Chemical">nd class="Chemical">n class="Chemical">nitrates formed from NO and O2 following our previous proposal[11] could also modify the state of copper under NH3–SCR–NO reaction conditions, and therefore two additional systems containing a NO2 molecule and a nitrite anion NO2– attached to copper (Cu2+–NO2––NO2) and nitrate coadsorbed with NO (Cu2+–NO3––NO) were also considered (Figures and S1, and Table S1). The evolution of some of the Cu–O distances during the simulations indicates that both nitrite and NO2 interact strongly with Cu2+ and that the Cu–O bonds are quite dynamic, especially at 523 K. Thus, the original Cu–O1 bond in the nitrite anion is broken after some time and a new bond appears between Cu2+ and the equivalent O2 atom (Figure S2a). A similar dynamic behavior, with an interchange of the Cu–O1 and Cu–O2 bonds, was also observed for nitrate NO3– coadsorbed with NO (Figure S2b). In summary, the AIMD simulations indicate that Cu+ and Cu2+ usually reside close to the 6r plane interacting with framework oxygen atoms, and only NH3 is able to mobilize them by forming Cu+(NH3)2 or Cu2+(NH3)4 complexes.

Having obtained inclass="Chemical">sight iclass="Chemical">nto the mobility of class="Chemical">n class="Chemical">Cu+ and Cu2+ cations in contact with reactants and intermediates using AIMD simulations, we analyzed in a next step the IR spectrum of Cu-SAPO-34 exposed to different combinations of reactants and temperatures to investigate whether a vibrational fingerprint could be found for mobile copper cations under reaction conditions. As reported earlier, IR spectra of Cu-CHA and other Cu-containing zeolite catalysts exhibit some bands in the 800–1000 cm–1 region associated with the framework asymmetric T-O-T vibrations perturbed by the presence of coordinated cations.[21−24] Herein, the νasym(T-O-T) region of the IR spectra of Cu-SAPO-34 exposed to different reactant feeds and temperatures was analyzed in detail, assisted by theoretical vibrational spectra computed with both static and dynamic based approaches (see Table and Figures , S3, and S4).

Table 1

Vibrational Frequencies (in cm–1) between 800 and 1000 cm–1 Calculated for Cu-SAPO-34 with Static DFT and from AIMD Simulations at 298 K

	static DFT	AIMD
Cu+	983, 964, 877	910, 817
Cu2+	960, 900, 874, 835	888, 876, 833
Cu+–O2	985, 816	862, 850
Cu+–NO	972, 894	920, 888, 855
Cu+–2NO	953, 892	-
Cu+–NO2	961, 885	916, 840
Cu+–2NO2	935, 865, 808	888, 812
Cu+–NH3	969, 905	920, 835
Cu+–2NH3	984, 964	-
Cu2+–ONO–NO2	934, 875, 860	932, 895, 820
Cu2+–NO3–NO	993, 968, 873	930, 868, 815
Cu2+–NO3	946, 861	850
Cu2+–2NO	992, 984, 948, 883	900
Cu2+–2NH3	990, 921, 859	900, 868
Cu2+–4NH3	997	-

Figure 3

(a) Vibrational νasym(T-O-T) region of the FTIR spectra of H-SAPO-34 (black line) and Cu-SAPO-34 preactivated in vacuum at 723 K (redline) or in O2 at 623 K followed by vacuum at 523 K (blueline). (b) Simulated vibrational spectra in the same region obtained from static DFT (red lines) and AIMD calculations at 298 K (green lines).

(a) Vibrationclass="Chemical">al νasym(T-O-T) regioclass="Chemical">n of the FTIR spectra of class="Chemical">n class="Chemical">H-SAPO-34 (black line) and Cu-SAPO-34 preactivated in vacuum at 723 K (redline) or in O2 at 623 K followed by vacuum at 523 K (blueline). (b) Simulated vibrational spectra in the same region obtained from static DFT (red lines) and AIMD calculations at 298 K (green lines).

The IR spectra of the parent class="Chemical">H-SAPO-34 catclass="Chemical">n class="Chemical">alyst and of Cu-SAPO-34 activated either in vacuum at 723 K (containing predominantly Cu+) or in O2 at 623 K (containing predominantly Cu2+)[15−17] (Figure a) were used as reference to check the accuracy of the calculated spectra (see details in the Supporting Information). There is a very good agreement between the experimental and the simulated spectra for H-SAPO-34, with absence of peaks in both cases. For Cu2+ in Cu-SAPO-34, the experimental peak at ∼960 cm–1, the intense and broad band at ∼890 cm–1, and the less intense signal at ∼840 cm–1 are also well reproduced by the simulations (Table and Figure ). The higher mobility of Cu+ in the 6r of Cu-SAPO-34 discussed before makes the static DFT frequencies less reliable, and the band at ∼905 cm–1 in the IR spectrum of Figure a (redline) is only well reproduced by the AIMD simulations.

The interaction of class="Chemical">Cu+ aclass="Chemical">nd class="Chemical">n class="Chemical">Cu2+ cations with reactant and intermediate species modifies the calculated vibrational frequencies in the 800–1000 cm–1 region as a consequence of the displacement of the copper cations from the 6r plane and the rupture of some of the Cu–O bonds, and both the static DFT and the AIMD data indicate that bands around ∼850 and ∼890 cm–1 should be visible in the IR spectra when NO2, nitrite, or nitrate intermediates are adsorbed on the Cu+ or Cu2+ cations (Table and Figures and S4).

Regarding class="Chemical">NH3 adsorptioclass="Chemical">n, the high mobility of class="Chemical">n class="Chemical">Cu+–NH3 complexes makes the spectra obtained from static and dynamic approaches quite different (Figure b) with a big band at 835 cm–1 being predicted only by AIMD simulations. When two NH3 molecules adsorb simultaneously on Cu+, a linear Cu+(NH3)2 species is formed that moves to the center of the cage. In this situation, there are no direct bonds between Cu+ and the framework oxygen atoms, and therefore no bands in the 800–1000 cm–1 region associated with perturbations of the framework T-O-T vibrations are obtained. A similarly flat spectrum is obtained for the Cu2+(NH3)4 complex placed in the cavity. However, for the still coordinated to the 6r Cu2+–2NH3 structure, features at ∼900 and ∼860 cm–1 are observed in both spectra (see Table ). These data indicate that a direct assignation of each vibrational frequency to a particular species is not possible, but suggest that broad bands around ∼890 cm–1 could be associated with Cu2+ attached to NO2, nitrite or nitrate intermediates, and confirm that no bands in the 800–1000 cm–1 region should be observed when copper cations are not directly coordinated to the framework oxygen atoms.

Then, the class="Chemical">Cu-SAPO-34 sample was exposed to differeclass="Chemical">nt combiclass="Chemical">natioclass="Chemical">ns of reactaclass="Chemical">nts class="Chemical">n class="Chemical">NO, O2, and NH3 at increasing temperatures, and characterized by means of X-ray absorption and FTIR spectroscopies, as outlined in Scheme . The frequency region of the IR spectra between 800 and 1000 cm–1 was analyzed in detail taking into account the simulations described before, the XAS data (Tables , S2, Figures S5–S7, and detailed description in the SI) and the information provided by the bands observed simultaneously between 1300 and 2000 cm–1 (Figures and S8–S11).

Scheme 1

Summary of Copper Species Identified by EXAFS (in Red) and IR (in Blue) Spectroscopies in Cu-SAPO-34 Samples Exposed to Different Reaction Conditions, Indicating the Presence or Absence of T-O-T Vibrations in the 800–1000 cm–1 IR Region

Table 2

Oxidation State and Coordination Environment of Copper in Cu-SAPO-34 Catalyst Obtained from Linear Combination Fit (LCF) (Figure S6) and from Analysis of the k2-Weighted EXAFS Data (Table S2 and Figure S7) at Different Reaction Conditions

reaction condition	temperature (K)	Cu+ (%)	Cu2+ (%)	Na	rb (Å)
2NO + 0.5NH3	353	35	65	3.2	1.940
	423	92	8	1.7	1.882
	523	100	0	1.6	1.879
2NO + 5O2	353	0	100	3.9	1.915
	423	0	100	3.9	1.912
	523	0	100	3.9	1.913
2NO + 0.5NH3 + 5O2	353	0	100	3.6	1.926
	423	65	35	2.5	1.890
	523	45	55	2.9	1.902

Coordination number.

Average distance over the first coordination shell.

Figure 4

FTIR spectra of Cu-SAPO-34 before (black lines) and after adsorption of different reactant mixtures. (a) 2NH3/Cu at 298 K (blue line) and increasing temperature to 423 K (green line), 523 K (pink line), and 623 K (red line). (b) 2NO/5O2/Cu at 298 K (blue line). (c) 2NO/5O2/Cu at 423 K (green line) followed by addition of 1NH3/Cu (blue line) and 2NH3/Cu (pink line) at 423 K and further increasing temperature to 523 K (red line). (d) 2NO/2NH3/Cu at 523 K (gray line) followed by addition of 5O2/Cu at 523 K (blue line) and increasing temperature to 573 K (pink line) and 623 K (red line). Prior to adsorption, the sample was preactivated in vacuum at 723 K for 2 h (a) or in O2 at 623 K for 2 h, followed by vacuum at 423 K for 1 h (b, c, and d).

FTIR spectra of class="Chemical">Cu-SAPO-34 before (black liclass="Chemical">nes) aclass="Chemical">nd after adsorptioclass="Chemical">n of differeclass="Chemical">nt reactaclass="Chemical">nt mixtures. (a) class="Chemical">n class="Chemical">2NH3/Cu at 298 K (blue line) and increasing temperature to 423 K (green line), 523 K (pink line), and 623 K (red line). (b) 2NO/5O2/Cu at 298 K (blue line). (c) 2NO/5O2/Cu at 423 K (green line) followed by addition of 1NH3/Cu (blue line) and 2NH3/Cu (pink line) at 423 K and further increasing temperature to 523 K (red line). (d) 2NO/2NH3/Cu at 523 K (gray line) followed by addition of 5O2/Cu at 523 K (blue line) and increasing temperature to 573 K (pink line) and 623 K (red line). Prior to adsorption, the sample was preactivated in vacuum at 723 K for 2 h (a) or in O2 at 623 K for 2 h, followed by vacuum at 423 K for 1 h (b, c, and d).

To ensure the posclass="Chemical">sibility of migratioclass="Chemical">n of the class="Chemical">n class="Chemical">copper cations, a Cu-SAPO-34 sample preactivated in vacuum was used in the IR study of NH3 adsorption. IR bands at 850 and 910 cm–1 associated with Cu+ in the 6r are clearly observed before NH3 adsorption (Figures a and S8, black line), which completely disappear after addition of 2NH3/Cu at 298 K (Figures a and S8, blue line), confirming the migration of Cu+ to the cavity as proposed by the AIMD simulations. Raising temperature in the closed IR cell (green and pink lines in Figures a and S8) leads to a decrease in the intensity of the band at 1620 cm–1 attributed to NH3 adsorbed on Lewis acid sites, but only after vacuum at 623 K (red line) NH3 is detached from Cu+ ions and the bands at ∼910 and ∼850 cm–1 are recovered, indicating that copper cations have returned to their position in the 6r.

class="Chemical">Next, a class="Chemical">n class="Chemical">Cu-SAPO-34 sample preactivated in O2 and exhibiting lattice vibrational bands associated with Cu2+ (965 and 885 cm–1) and Cu+ (910 and 855 cm–1) (Figures b and S9a, black line) was exposed to 2NO/5O2/Cu at 298 K (Figures b and S9a, navy line). IR bands associated with NO, NO2, nitrites, and nitrates are observed in the high frequency region (see details in the Supporting Information); and simultaneously, in the lattice vibrations frequency region, the IR peak at 965 cm–1 disappears, the signals at ∼910 and 855 cm–1 decrease, and a broad band grows around 885 cm–1. Based on the simulated spectra previously discussed and the XAS data in Table indicating that only Cu2+ coordinated to the framework and directly bonded to four O atoms is present under these conditions, this broad band is assigned to Cu2+ in the 6r interacting with NO2, nitrites, and nitrates. These species are stable at 423 K and only start to desorb or decompose at higher temperatures (Figure S9b).

To study the mobilizing effect of class="Chemical">NH3, coclass="Chemical">ntrolled amouclass="Chemical">nts of class="Chemical">n class="Chemical">NH3 were added to a Cu-SAPO-34 sample previously exposed to 2NO/5O2 at 423 K (Figures c and S10, green line) that contains NO2, nitrites, and nitrates bonded to Cu2+. The XAS study indicates that the addition of a small amount of NH3 together with NO and O2 leads to a reduction of 65% of Cu2+ to Cu+ (see Table ). Addition of 1NH3/Cu at 423 K does not cause relevant changes in the IR spectrum, indicating that both Cu+ and Cu2+ cations remain coordinated to the framework oxygen atoms (blue line in Figures c and S10). In contrast, addition of 2NH3/Cu at 423 K (pink line in Figures c and S10) causes the disappearance of all IR signals in the 800–1000 cm–1 region, in agreement with the results from the AIMD simulations. At 523 K (red line), the adsorbed intermediates decompose and two bands centered at ∼900 and ∼850 cm–1 appear again, indicating the reallocation of copper cations in the 6r units of the SAPO-34 framework.

Finclass="Chemical">ally, the class="Chemical">n class="Chemical">Cu-SAPO-34 sample was first exposed to 2NO/2NH3/Cu at 523 K to ensure the reduction of all Cu2+ to Cu+ (see Table ) and the total migration of Cu+ cations to the cavity in the form of Cu+(NH3)2 complexes, as confirmed by the absence of IR bands in the 800–1000 cm–1 region (Figures d and S11, gray line). After addition of 5O2/Cu at 523 K (Figures d and S11, blue line) the NH4+ cations and NH3 bonded to Lewis sites are consumed, while the bands centered at ∼900 and ∼850 cm–1 appear, indicating a the return of copper cations to the 6r of the SAPO-34 framework.

To summarize, the dynamic behavior of class="Chemical">copper catioclass="Chemical">ns iclass="Chemical">n class="Chemical">n class="Chemical">Cu-SAPO-34 catalyst under NH3–SCR–NO reaction conditions has been investigated in detail by combining static DFT, AIMD simulations, and XAS and IR spectroscopies. The AIMD simulations show that only the interaction with NH3 is able to break the coordination of Cu+ and Cu2+ cations to the framework oxygen atoms, resulting in the formation of mobile Cu+(NH3)2 and Cu2+(NH3)4 complexes that migrate to the cha cavity. Computationally assisted analysis of the 800–1000 cm–1 region of the IR spectra of Cu-SAPO-34 exposed to different reactant mixtures and temperatures confirms that complete migration of copper cations from the 6r to the cavity only occurs when there is enough NH3 present in the reaction media, and that reaction of Cu+(NH3)2 complexes with added O2 leads to a fast recovering of the peaks in the 800–1000 cm–1 IR region, indicating the return of copper cations to the 6r of the SAPO-34 framework. The complementary experimental and computational approach allows one to observe the dynamic reorganization of the catalytic active sites for the SCR–NO reaction, and could be applied to follow in situ and operando whether the complete catalytic cycle of the SCR–NO reaction occurs in the cavity or if some elementary steps occur necessarily on copper cations coordinated to framework oxygens.