Computational characterization of halogen vapor attachment, diffusion and desorption processes in zeolitic imidazolate framework-8.

Computational simulation methods are used for characterizing the detailed attachment, diffusion and desorption of halogen vapor molecules in zeolitic imidazolate framework-8 (ZIF-8). The attachment energies of Cl2, Br2 and I2 are -55.2, -48.5 and -43.0 kJ mol-1, respectively. The framework of ZIF-8 is disrupted by Cl2, which bonds with Zn either on the surface or by freely diffusing into the cage. A framework deformation on the surface of ZIF-8 can be caused by the attachment of Br2, but only reorientation of the 2-methylimidazolate linkers (mIms) for I2. In diffusion, the halogen molecules have a tendency to vertically permeate the apertures of cages followed with swing effect implemented by the mIms. Larger rotation angles of mIms are caused by Br2 because of its stronger interaction with mIms than I2. A maximum of 7 Br2 or 5 I2 molecules can be accommodated in one cage. Br2 are clinging to the mIms and I2 are arranged as crystal layout in the cages, therefore in desorption processes molecules attached to the surface and free inside are desorbed while some remained. These results are beneficial for better understanding the adsorption and desorption processes of halogen vapors in the porous materials.

Introduction

The research subjects in the preparation, characterization and study, related to metal–organic frameworks (MOFs), have been explosive growth[1]. MOFs possess unique property among the various microporous and mesoporous materin class="Chemical">als, creating interest for an unprecedented range of applications[2]. As a new class of crystalline nanoporous materials, MOFs have been found extensively applied in the areas such as catalysis[3], biomedicine[4], separation[5], gas storage[6], chemical sensing[7], air purification[8], imaging agents[9], and so on.

One of the outstanding characteristics of MOFs are their highly diverse conformation, ideal porosity, and good chemicn class="Chemical">al properties[10], making them suitable for gas adsorption or separation and being a substitute for traditional adsorbents[11]. For example, Khan et al. used multinuclear solid-state NMR to study the adsorption of biologically important signaling molecule NO on two MOFs, indicating both physisorption and chemisorption of NO adsorbed on the open metal site[12]. Niu et al. successfully synthesized hierarchical UiO-66 and its amino-analog UiO-66-NH2 nanocrystals can enhance the adsorption capacity by introducing water into the conventional synthesis without the need for a chelating agent or surfactant[13].

To better understand the mechanism governing the gas molecules migration in adsorption processes or establish an investigation approach to promote the adsorption properties of the absorbents, detailed information on the gas adsorption and diffusion processes is crucial[14]. Therefore, nowadays more and more attention has been paid to the role of computationn class="Chemical">al simulation in the structure design and performance evaluation of MOFs[15]. Kitao et al. provided new and versatile MOFs by simulation that exhibit peculiar properties hard to realize with the individual components[16]. Farha et al. used computational modeling to design and characterize predictively MOFs with high surface areas[17].

Zeolitic imidazolate frameworks (n class="Chemical">ZIFs) are a sub-class of MOFs. Zeolitic imidazolate frameworks-8 (ZIF-8) is a compelling example because of its high thermal and chemical stability[18]. Bonding between 2-methylimidazolate linkers (mIms) and Zn2+ constituting the node is comparatively strong and the physical shielding of Zn2+ by four tetrahedrally coordinated mIms is effective[19]. The apertures in the framework lack polar groups and exclude liquid water effectively[20]. Therefore, ZIF-8 can bear prolonged soaking in 8 M NaOH solution at 100 °C[21]. It is suitable for gas separation/adsorption at temperatures below 300 °C in the presence of air/water and under inert gas over 400 °C[22]. Many researchers are attracted by the stability to study the application of ZIF-8 as a gas adsorbent[23].

Halogens are playing important roles in many aspects of industrin class="Chemical">al processes. Cl2 is used as disinfectant in water supply system and is an ingredient of plastic products[24]. Br2 and I2 are key elements in medicine, photography and dyes[25]. However, the safe handling, storage and transportation of halogens are great challenges because of their toxicity, corrosiveness and volatility. It is necessary to study the safe use or disposal of halogen gases such as adsorption. In the gas adsorption applications, ZIF-8 is usually chosen as the adsorbent[26]. The dynamic adsorption and desorption processes of Br2 and I2 on ZIF-8 film have also been monitored by electrodeless quartz crystal microbalance (EL-QCM) technique in our previous experiments[27,28].

In this work, for the purpose of supplying more detailed information and establishing a theoretical model to promote the adsorption properties of the adsorbents through modification, computationn class="Chemical">al simulation methods are used to investigate the Br2 and I2 adsorption/desorption processes in ZIF-8 on thermodynamics and dynamics. Additionally, the interaction of Cl2 and ZIF-8, which is scarcely discussed to our knowledge, is also included. Energy variations, charge distributions and structure parameters are explained and some of the results are confirmed by experiments. It is hopeful that the detailed characterization, could serve as an important stepping stone for understanding the adsorption/desorption processes during uptake action, illuminating the way of theoretical prediction or design on the porous material performances.

Methods

From the microscopic viewpoint, ZIF-8 crystn class="Chemical">al is characterized by the presence of square and hexagonal windows around the main pore. Calculation research performs on periodic system, which is uncharged compared to the fragments that Zn atoms at the vertices of square or hexagonal windows are fixed[29]. As previous research done[30], hexagonal window portion of the lattice was adopted in this work (Fig. S1, Supplementary Information). Previous research investigations[31,32], employed the density functional theory (DFT) method with B3LYP/lanl2dz basis set to obtain a much better energy description of the intermolecular interaction between ZIF-8 and vapors. The results are comparable with that calculated by Moller-Plesset correlation energy correction truncated at second-order and higher-level ab initio methods, but at a much lower computational effort[33]. Thus in this work, the simulation was performed by using the same basis set and all the results were zero-point corrected (ZPC) energies.

Stationary points calculated had been characterized as minima state or activation state by ann class="Chemical">alyzing the vibrational normal mode[32]. That point could be classified as minima if no imaginary frequency was obtained while an activation state if only one imaginary frequency was observed[33]. Atomic charges in the aperture structures were obtained by the natural population analysis (NPA) of Weinhold[34]. The attachment energy (ET) of halogen molecule at each adsorption site was calculated from the energy difference between the stable structure with adsorbed molecule [E (ZIF-8 + gas)] and the stable empty structure [E (ZIF-8)] corrected by the energy of the free molecule for the same volume [E (gas)]. That is, ET = E (ZIF-8 + gas) − E (ZIF-8) − E (gas). All the simulated work was performed with GAUSSIAN 09 suite of package[35].

Additionally, to gain more insights into the diffusion processes of n class="Gene">Cl2, Br2, and I2 in ZIF-8, the molecular dynamics (MD) simulation was also performed. The crystal structure of ZIF-8 was obtained from the previously published literature[36]. Due to large computational cost, geometric optimization was performed by Forcite module[37] based on the Universal Force Field (UFF)[38] in Materials Studio software. Equilibrium MD simulation was used to calculate self-diffusivities in ZIF-8 and it was also implemented in the Forcite module[39]. Independent simulation was performed for each process with NVT ensemble. The total simulation time was 2 ns with a time step of 1 fs. 1 ns was used for equilibrium, another 1 ns for statistics.

Results and Discussion

To describe more accurately, the whole processes can be divided into three processes: attachment (halogen molecule attaches to the aperture), diffusion (n class="Chemical">halogen passes through the aperture) and desorption (the opposite process of attachment and diffusion).

Selection of the aperture structures

Due to the size of the aperture windows (diameter, 3.40 Å) which connect the large pores (diameter, 11.60 Å), ZIF-8 is recognized as a molecular sieve[40,41]. In gas adsorption process, the high diffusivity implies the swing effect of mIms during the gas uptake experiments[42]. This structure variation is fundamentn class="Chemical">ally important because it promotes the diffusivity of gases through the porous networks[43]. Based on the flexibility stated above, 8 different aperture structures are designed to select the appropriate simulation model (Fig. S2), of which the methyl in the mIms (Me-m) point to different directions.

In the aperture (Fig. S2), structure of all Me-m oriented to Z-axis is named structure A, abbreviated S-A; structure B (S-B), Me-m 1 oriented to Z-axis; structure C (S-C), Me-m 1, 2 oriented to Z-axis; structure D (S-D), Me-m 1, 3 oriented to Z-axis; structure E (S-E), Me-m 1, 4 oriented to Z-axis; structure F (S-F), Me-m 1, 3, 5 oriented to Z-axis; structure G (S-G), n class="Chemical">all Me-m oriented to the center; structure H (S-H), all Me-m oriented against to the center. Other Me-m not mentioned oriented against the Z-axis. Structures simulated are originally composed of mIms groups, to show clearly, in figures the branched mIms are removed.

ZPC energies of S-A to S-H based on S-A (0 kJ mol−1) are listed in Table 1. The energies are 0 (S-A), 11.8 (S-B), 11.1 (S-C), 8.1 (S-D), 4.6 (S-E), −0.5 (S-F), 10.3 (S-G) and 20.2 (S-H), respectively. Therefore, S-F is the most stable structure. The vertical and side views of S-F is shown in Fig. 1. n class="Chemical">All the Zn form a plane represented by X and Y-axis. The mIms are numbered from 1 to 6 and mIm 1, 3, 5 follow by a 35.8° rotation, in good agreement with the previous research reported[44]. Detailed bond lengths (Å) and charge distributions (a.u.) are compiled in Tables S1 and S2.

Table 1

Zero-point corrected (ZPC) energies (kJ mol−1) of 8 aperture structures optimized.

Structures	S-A	S-B	S-C	S-D	S-E	S-F	S-G	S-H
Energy	0	11.8	11.1	8.1	4.6	−0.5	10.3	20.2

Figure 1

Vertical and side views about the most stable structure of the relevant hexagonal window aperture of ZIF-8. Zn, C and N atoms are shown in pink, gray and blue colors, respectively. H are omitted for clarity in the figure. All the six Zn form a surface which represented by X, Y-axis and the mIms are numbered from 1 to 6. Bond distances are in Å.

Vertical and side views about the most stable structure of the relevant hexagonn class="Chemical">al window aperture of ZIF-8. Zn, C and N atoms are shown in pink, gray and blue colors, respectively. H are omitted for clarity in the figure. All the six Zn form a surface which represented by X, Y-axis and the mIms are numbered from 1 to 6. Bond distances are in Å.

Attachment and diffusion processes of Cl2

Since the diatomic bond length of Cl2 is short (2.224 Å), optimized result reven class="Chemical">als that at the same time, several Cl2 molecules gather together on the top of the aperture (Fig. S3(a)). As the halogen gas getting closer and closer to the aperture, charges on each Cl are changing to negative. At some point in time at least up to two Cl2 molecules can be accommodated by the aperture, as shown in Fig. 2. Charge distributions on each Cl are −0.229 and −0.134, −0.183 and −0.263, respectively. Distance between two molecules is 2.964 Å. The attraction established between Cl2 and the aperture is 18.9 kJ mol−1 in average. Therefore, Cl2 are still on the way of approaching to the aperture at that time. As Cl2 getting closer to the aperture, a site on top of the aperture center where only one Cl2 molecule located can be identified. The stable structure is shown in Fig. 3. The diatomic bond of Cl2 is parallel to the plane of the aperture and the distance between Cl2 and the aperture is 2.490 Å. In general, the attachment energies of H2, CO2 and CH4 are −8.6, −20.0 and −20.9 kJ mol−1, respectively, and charges of the aperture change a little[28,29,45]. However, in this structure, the polarizability of Cl2 is increased and the charge distributions change to −0.240 and −0.257, respectively. The averaged charge on protons surrounding increases from 0.027 to 0.042. Charge variation in this structure is greater than that of other gases stated above. The attachment process of Cl2 releases more energy and ET is −55.2 kJ mol−1. It is indicated that the attachment of Cl2 vapor is a spontaneous process.

Figure 2

Vertical and side views about the stable structure of two Cl2 molecules attachment on the aperture. Bond distances are in Å and the charges are listed in parentheses.

Figure 3

Side views about the stable structures of halogens attachment on the aperture. Bond distances are in Å.

Vertical and side views about the stable structure of two n class="Gene">Cl2 molecules attachment on the aperture. Bond distances are in Å and the charges are listed in parentheses.

In the most stable aperture, charge distribution on C7 is 0.456. At the beginning of diffusion process, MD simulation reveals that there is an interaction between n class="Gene">Cl2 and C7 (Fig. S4). Related structures are further calculated by using the more precise DFT method. As shown in Fig. 4(a), Cl2 is close to the plane of the aperture in the initial. Then it is attracted to interact with C7 and the distance between them is 2.702 Å, as shown in Fig. 4(b). At that time, charge distributions on two Cl change to −0.482 and −0.449, respectively. Two Cl depart from each other and the distance is 2.768 Å. This distance keeps getting longer and longer. In Fig. 4(c), the positive part on the other side of the aperture, especially Zn which has a charge of 0.870, is attracted by the free Cl and the aperture is distorted. One Cl still interacts with C7 and the other interacts with Zn on the other side. Correspondingly, charge redistribution of the aperture is occurred. For example, charge distribution on N8 changes from −0.811 to 0.481. Bond lengths of N–Zn are dramatically elongated and bond strengths are greatly weakened. Finally, with structure adjustment, some bond lengths of N–Zn are extended more than 3.511 Å and the aperture is disrupted, as shown in Fig. 4(d).

Figure 4

The disruption profile of aperture in the diffusion process of Cl2. (a–d) are four typical structure change nodes. Bond distances are in Å.

The disruption profile of aperture in the diffusion process of Cl2. (a–d) are four typicn class="Chemical">al structure change nodes. Bond distances are in Å.

It is particularly noteworthy that there exists another type of interaction that can be regarded as an activation state in diffusion process of Cl2. In Fig. 5(a), structure with an imaginary frequency of 475 i cm−1 is accompanied by the rotation of n class="Gene">Cl2. The aperture plane separates Cl2 molecule into two parts: one Cl is pointing inside and the other pointing outside. Charge distribution on each Cl are −0.230 and −0.229, therefore, slight rotations of mIms are caused by the steric electric effect. However, distances between Cl2 and mIms 1, 3, 5 are 4.046, 3.776 and 4.129 Å, respectively, that are too long to cause an interaction between Cl2 and the aperture. There is a possibility that Cl2 can get through the apertures vertically and get inside the cages to bond with Zn. The disruption of ZIF-8 is confirmed by X-ray diffraction (XRD) and Fourier transform infrared spectroscopy (FTIR) investigations[46]. The spectrum in previous work reveals that structures of mIms are dramatically changed and vibrational modes of Zn–N bonds disappeared after interaction with Cl2 gas. Therefore, Cl2 can bond with Zn either on the surface or by freely diffusing into the cage, resulting in the disruption of ZIF-8.

Figure 5

Vertical views about the structures of halogens diffusion in the aperture. Bond distances are in Å. (a) Cl2 diffusion in the aperture, (b,c) different states of Br2 diffusion in the aperture, (d) I2 diffusion in the aperture.

Vertical views about the structures of n class="Chemical">halogens diffusion in the aperture. Bond distances are in Å. (a) Cl2 diffusion in the aperture, (b,c) different states of Br2 diffusion in the aperture, (d) I2 diffusion in the aperture.

Attachment, diffusion and desorption processes of Br2

As the gas getting closer to the aperture, MD simulation reveals that at some point in time three n class="Chemical">Br2 molecules can exist simultaneously close to the aperture. Charge distributions on each Br are −0.120 and −0.155, −0.107 and −0.178, −0.151 and −0.176, respectively (Fig. S3(b)). Br2 molecules are more polarized than that of Cl2. In the stable structure, because bond length of Br2 (2.510 Å) is longer than that of Cl2 (2.224 Å), space resistance does not allow two Br2 molecules to locate and only one on top of the aperture center is identified, as shown in Fig. 3. Charge distribution on Br close to protons is −0.399 and the other is −0.377, which induce all of the six mIms to rotate. Me-m 2, 4, 6 are rotated by 23.2° and correspondingly Me-m 1, 3, 5 are rotated by 43.0° to adapt to the new distribution of charges. The distance between Br2 and the aperture is 3.251 Å, which is 0.761 Å longer than that of Cl2. The interaction between Br2 and the aperture is reduced by charge redistribution and the long distance, although Br2 is strongly polarized. Correspondingly, the ET of Br2 is −48.5 kJ mol−1, exothermic 6.7 kJ mol−1 less than that of Cl2. Therefore, in the experiment, the adsorption rate of Br2 is slower than that of Cl2 in the initial stage (data for Cl2 are not shown because of the disruption of ZIF-8).

It is particularly noteworthy that there exist two activation states in the diffusion process of Br2. One state is that n class="Chemical">Br2 keeps diffusing accompanied by the aperture deformation. In Fig. 5(b), distances between each Br and the closest mIm are 3.164 and 3.112 Å, respectively. The diatomic bond length of Br2 is stretched to 3.480 Å. Correspondingly, deformation of the aperture is caused by the steric electric effect. The other state (446 i cm−1) is that Br2 is perpendicular to the aperture plane, as shown in Fig. 5(c). Distances between Br2 and mIms 1, 3, 5 are 3.953, 3.791 and 4.033 Å, respectively. Charge distributions on each Br are −0.385 and −0.361, respectively, which cause a large steric electric effect to the adjacent protons. Therefore, an averaged 40.0° reorientation of the mIms occurs, indicating a swing effect of the aperture. When the molecule gets inside the cage, charge distribution on each Br are −0.019 and −0.011, respectively. The steric electric effect of Br2 is dispersed due to more interaction to the framework.

The adsorption processes of Br2 vapor on n class="Chemical">ZIF-8 film is monitored by EL-QCM. The schematic drawing of experimental setups employed for equivalent circuit parameters and the measurements are illustrated in Fig. S5. The shifts of the resonant frequency (Δf) is recorded (Fig. S6) and the trend of adsorption/desorption can be directly reflected. As stated above, the ET of Br2 is greatly exothermic, thus it can be found in the experiment that the frequency drops rapidly in the initial 10 min, corresponding to the rapid increase in adsorption. In diffusion process, simulation result reveals that there exist adverse factors including the deformation of aperture and reorientation of mIms. Therefore, the adsorption takes a long time (100 min) to approach the stable level.

The released energies (ER) of Br2 molecules in one cage with the molecule number increasing from 0 n class="Species">to 7 are simulated. In Fig. 6, ER is increased with the increase of gas molecules at the beginning. When 4 molecules are congregated inside, there is a repulsion to the new one. As the diffusion proceeding, distances between Br2 molecules are decreased (Fig. S7) and the repulsive forces increased (less than 2.0 kJ mol−1), thus ER curve is descending. MD simulation shows that the framework of cage does not reveal any significant changes and most Br2 molecules are close to the cage walls. When the 8th molecule is diffused into the cage, there is an abnormal structure or energy interaction between Br2 and the cage. Additionally, the mass of Br2 inside the cages (g/g) can be obtained by Δf[27] in the experiment. Based on the molar mass of Br2 and cage unit, the molecular number ratio can be calculated. In the experiment, 7.3 Br2 can be obtained in each cage (0.87 g of Br2/g). Therefore, considering the results from simulation and experiment, it can be concluded that each cage can accommodate 7 Br2 molecules.

Figure 6

The released energies (ER) of Br2 placed in one cage with the molecule number of Br2 increasing from 0 to 7.

The released energies (ER) of Br2 placed in one cage with the molecule number of n class="Chemical">Br2 increasing from 0 to 7.

At the end of desorption process, approximately 21% of Br2 release is taken place and 79% left in the cages when the vacuum operation is carried out in the experiment (Fig. S6). Simulated result reven class="Chemical">als that there is an interaction between Br2 and mIms. In general, it needs to take in the energy of 5.5 kJ mol−1 at least for Br2 inside the cage to escape from the grasp of mIms, indicating that mIms play an important role in Br2 adsorption. The simulated result is supported by Δf measured in the experiment (Fig. S6). In the cage, the majority of Br2 interact with mIms and firmly attach to the cage walls; the minority are prone to move in the state of non-regular thermal motion. Therefore, in desorption process, the escaped vapor are the Br2 in the state of non-regular thermal motion in the cages and attached on the surface of ZIF-8 film before, while others stay inside.

Attachment, diffusion and desorption processes of I2

In attachment process, one molecule is close to the aperture (the distance less than 4.0 Å), while the distances of the others are all over 5.0 Å (Fig. S3(c)). Charge distributions on the closest I2 molecule are −0.141 and −0.177, respectively. The polarization of this I2 molecule, the attraction between this I2 and the aperture are both stronger than that of n class="Gene">Cl2 or Br2. In the stable state, only one I2 is located on top of the aperture center, as shown in Fig. 3. This is because that the bond length of I2 is 2.863 Å, much longer than that of Cl2 (2.490 Å) and Br2 (2.510 Å), taking up space upon the aperture. The shortest distance between I2 and the aperture is 3.221 Å, which is in good agreement with the experimental value of 3.210 Å obtained from difference Fourier analysis[46]. Charge distribution on I close to the aperture is changed to −0.240 and the other is −0.250, which are much less than that of Br2. Thus, the aperture has little variation. Me-m 1, 3, 5 are rotated by a slightly −0.9° in average, orienting to I2; Me-m 2, 4, 6 are rotated by 8.1°, orienting to Z-axis. Correspondingly, ET of I2 (−43.0 kJ mol−1, which is in good agreement with the previous research[47]) is the minimum of the three halogens. Therefore, the adsorption rate of I2 is the slowest in the initial adsorption stage of the experiment.

When the straight-line distance between I2 and the aperture shortens, the mIms gradually rotate from 35.1° to 0.64°, like a switch turned off. Only one state with an imaginary frequency of 391 i cm−1 which I2 is perpendicular to the aperture plane is found. As shown in Fig. 5(d), the distances between I2 molecule and n class="Gene">mIm 1, 3, 5 are 3.956, 4.001 and 3.999 Å, respectively. Charge distributions on each I are −0.219 and −0.219, which has less steric electric effect than Br2 to the protons. When I2 molecules get inside, simulated result reveals that a maximum of 5 I2 molecules can stabilize in the cage, which like a critical feature that retains I2 in ZIF-8 until the framework collapses. According to the experimental data (Fig. S8, 0.97 g I2/g), each cage contains 5.2 I2 molecules, which is in good agreement with the previous research determined by thermogravimetric analysis (5.4 I2 in each cage)[48]. MD simulation shows that each I2 molecule locates close to the center of the aperture (Fig. S9) and the molecules only move around the localized locations.

In desorption process, possible halogen bond interactions are further investigated. n class="Chemical">Although the halogen bonds are weakened under the influence of framework of cages, there is an interaction between Br2 or I2 aggregated molecules. For example, charge distributions reveal the slight influence of framework on I2 molecules (Fig. S9). A model of I2 − I2 interaction including bond distances, bond angles and charge distributions separated from the entire structure is shown in Fig. 7. The shortest distance between two molecules is 3.543 Å and the bond angle is 37.1°, which are in consistent with the values in polyiodide and metal iodide−iodine systems[47]. Without the influence of framework, I2 would be polarized and there would be an attraction between the two molecules, the energy of which is 9.1 kJ mol−1. Charge distributions on one I2 molecule would be −0.003 and 0.001, the other are −0.002 and 0.004. In the cage, charges of I2 molecules are changed to −0.084 and −0.015, −0.035 and −0.053, respectively. The attraction energy is reduced to about 3.0 kJ mol−1 but not disappeared. Therefore, halogen bonds can be considered as another factor to the overall stabilization.

Figure 7

The typical model of intermolecular I2 − I2 interaction separated from the entire optimized structure. Bond distances are in Å and the charges are listed in parentheses (the former is not affected by the framework of cages, while the latter is affected).

Based on the above analysis, it is quite possible that I2 in part of the upper layer of cages are regularly fixed and the diffusion rate is slowed down. That is why in the experiment, the amount of n class="Chemical">Br2 adsorbed increases slightly more than that of I2 in the initial 30 min. Also, the halogen bonds increase the overall stabilization. Thus in the desorption experiment (Fig. S8), the decreased amount of I2 (54%) is the vapor adsorbed on the surface of ZIF-8 film before. In addition, it has been proved by XRD and FTIR that interaction between I2 and mIms is the main influence factor of I2 fixation and after sorption, the cage does not reveal any significant changes[46,49,50].

Conclusions

In this work, the detailed attachment, diffusion and desorption processes of halogens in n class="Chemical">ZIF-8 have been explored by simulation on dynamics and thermodynamics. Deep interpretations including structure parameters, charge distributions and energy variations are discussed. The ET of Cl2, Br2 and I2 are −55.2, −48.5 and −43.0 kJ mol−1, respectively. The framework of ZIF-8 is disrupted with the interaction of Cl2 and Zn on the surface and in the cage. Framework deformation on the surface of ZIF-8 can be caused by the attachment of Br2 but not I2. In diffusion, vapor molecules tend to vertically pass through the aperture of cages and a maximum of 7 Br2 or 5 I2 molecules can be accommodated with different states in each cage. In desorption process, the decrease of Br2 or I2 is the molecules in the state of non-regular thermal motion in the cages or adsorbed on the surface of ZIF-8 before. Next, more ZIFs materials served as adsorbents will be investigated by simulation and some regularities will be summarized. It also hopes to design more MOFs materials with better adsorption properties and performances based on the simulation method.

Supplementary Information.