Effective capture of radioactive organic iodides from nuclear waste remains a significant challenge due to the drawbacks of current adsorbents such as low uptake capacity, high cost, and non-recyclability. We report here a general approach to overcome this challenge by creating radioactive organic iodide molecular traps through functionalization of metal-organic framework materials with tertiary amine-binding sites. The molecular trap exhibits a high CH3I saturation uptake capacity of 71 wt% at 150 °C, which is more than 340% higher than the industrial adsorbent Ag0@MOR under identical conditions. These functionalized metal-organic frameworks also serve as good adsorbents at low temperatures. Furthermore, the resulting adsorbent can be recycled multiple times without loss of capacity, making recyclability a reality. In combination with its chemical and thermal stability, high capture efficiency and low cost, the adsorbent demonstrates promise for industrial radioactive organic iodides capture from nuclear waste. The capture mechanism was investigated by experimental and theoretical methods.
Currently, nuclear power provides ~11% of the world’s electricity offering a cost-effective option compared to other energy sources1. Rapidly increasing global energy needs will likely increase the demand for nuclear energy in the future. Under normal operating conditions, fuel rods used in nuclear power plants need to be reprocessed. This procedure involves the production of complex off-gas mixtures consisting of HNO3, NO2, and N2O5 along with radioactive molecular iodine (I2) and organic iodides (ROIs, e.g., methyl iodide and ethyl iodide) at elevated temperatures (e.g., 150 °C)2,3,4. Radioactive I2 and ROI species must be selectively captured and sequestered to ensure safe nuclear energy usage. ROI species are known to be particularly difficult to capture, and a recent study has shown that the CH3I adsorption rate is only half of that for I2 in the case of Ag@MOR5. It thus tends to leak into the environment more easily6. Among various current capture technologies, solid sorbent-based fixed-bed methods have proven superior due to their simplicity and relatively low cost7. Examples of solid adsorbents for capturing ROIs from off-gas mixtures include triethylenediamine (TED) impregnated activated carbon (AC)8, 9, and silver impregnated/exchanged solid supports such as silica, alumina, and zeolites10,11,12,13,14. Typically the temperature of the off-gas is performed at high temperature (such as ~150 °C) in order to accelerate the chemical reactions and to remove adsorbed water from the narrow pores of the supports15. AC-based adsorbents, however, can only be used under 120 °C and are limited to specific applications absent of NOx16 because of low ignition temperatures and the risk of formation of explosive compounds. Silver functionalized porous materials are capable of performing at higher temperatures, but the high costs associated with the noble metal limits their widespread application. Additionally, much to their detriment, chemical adsorption of CH3I—necessary for its high uptake at high temperature in such systems—makes the silver-based adsorbents poorly recyclable. Based on these considerations, and the fact that the uptake capacity of all existing adsorbents remains insufficient, new types of adsorbent materials that are noble metal free, highly efficient, cost effective, recyclable, and safe to use, are much needed for ROIs capture.
To tackle the aforementioned challenges, a desired ROI adsorbent must possess the following features: extraordinarily high adsorption capacity at the reprocessing temperature; high tolerance toward nitrogen-based oxides, acidity, and humidity; high thermal stability (≥150 °C) that meets the required reprocessing conditions; high efficiency well above reprocessing facility regulatory requirements and low cost and excellent recyclability. To fulfill this goal, we investigate a different type of crystalline porous materials, metal-organic frameworks (MOFs)17,18,19,20,21,22,23,24,25,26,27, as tunable and recyclable solid adsorbents for ROIs capture. We reason that such materials can potentially offer the following advantages: large and adjustable surface area and pore size enable accommodation of a large amount of ROI molecules and thus result in high ROI capacity28,29,30,31,32,33,34,35,36,37,38; modular nature allows for rational design and tailoring of structural topology and functional sites39,40,41,42; multivariate syntheses offer possibilities for obtaining topologically identical yet functionally diverse crystalline frameworks43, 44; modifiable open metal sites (OMSs) that form reversible coordination bonds with tertiary amines provide an effective means for recyclability45,46,47. While numerous previous investigations have illustrated that MOFs serve as an excellent platform for capture of radioactive molecular iodine32,33,34,35, 48, their use as adsorbent materials to effectively trap ROI species remains unexploited to this date.
Here we demonstrate that highly efficient ROI molecular traps can be obtained via tertiary amine grafting to binding sites within a MOF framework. One such designed molecular trap, MIL-101-Cr-TED, exhibits an exceptionally high uptake capacity of 71 wt% for methyl iodide at 150 °C. Under identical capture conditions, this performance is more than 340% higher than that of the industrial adsorbent Ag0@MOR, a leading material in the United States for ROIs capture10, 49. Furthermore, the pristine MOF sample can be regenerated and reused multiple times without decrease in uptake capacity. This is a notable advancement as high-temperature recyclable adsorbent materials have been pursued since the 1980s but with very little success to this date. Coupled with its high chemical and thermal stability, relatively low cost, and high capture efficiency at both room and high temperatures, amine functionalized MIL-101-Cr-TED demonstrates a considerable potential for use as MOF-based adsorbent for the ROIs capture technology. Employing both experimental and theoretical methods, we further carried out an in-depth study to investigate and understand the mechanism of CH3I capture in the MIL-101-Cr-TED system. Our findings show that the construction and optimization of such molecular traps can be expanded to other MOFs by a suitable combination of robust frameworks with strong binding sites and tertiary amine molecules, which may lead to a large number of ROI capture materials. This strategy thus paves the way for further research and advancement on MOF-based molecular traps for their ultimate utility in ROIs capture from nuclear waste.
Synthesis and characterization
To construct high performance molecular traps (Fig. 1) that are highly stable, efficient, and recyclable for capturing organic iodides, we chose MIL-101-Cr as a model support material because of its large surface area (>3300 m2 g−1), high acid and moisture stability, thermal stability (~ 300 °C), and relatively low cost44. Two tertiary amines, triethylenediamine (TED) and hexamethylenetetramine (HMTA), were selected as functional molecules for post-synthetic modification of the MOF framework. Both species can use a single nitrogen to bind to the OMSs on the Cr trinuclear secondary building unit of MIL-101-Cr45, 47, 50, 51, with the remaining nitrogen atoms available as binding sites for organic iodides (Supplementary Fig. 1). MIL-101-Cr-TED and MIL-101-Cr-HMTA were obtained by stirring MIL-101-Cr with TED or HMTA in benzene or chloroform at 110 °C for 24 h in a resealed flask under nitrogen atmosphere. Transmission electron microscopy (TEM) images (Supplementary Fig. 2) of both functionalized MOFs show similar crystal morphology when compared to as-made MIL-101-Cr, suggesting retention of crystallinity and morphology after amine functionalization.
The successful grafting of tertiary amine groups onto MIL-101-Cr was confirmed by powder X-ray diffraction (PXRD), Fourier transform infrared (FT-IR) spectroscopy, X-ray photoelectron spectroscopy (XPS), solid-state 1H NMR, and elemental analysis. PXRD analysis shows that the diffraction profiles are unchanged after amine functionalization (Fig. 2a), indicating that the crystal structure of the functionalized material remains intact. The IR absorption spectra in Fig. 2b shows two additional peaks (at 1054 and 995 cm−1) associated with TED and HMTA that are not present in pristine MIL-101-Cr. This amine-associated mode (see inset of Fig. 2b) is attributed to the skeletal C-N stretching mode52, 53, confirming successful grafting. In addition, new features between 3000 and 2800 cm−1 are assigned to the aliphatic C-H stretching modes of TED and HMTA molecules (Fig. 2b)52, 53. XPS spectra (Supplementary Fig. 3) confirm that the N(1s) core level in MIL-101-Cr-TED and MIL-101-Cr-HMTA is at a binding energy (~400.0 eV) consistent with the nitrogen within tertiary amine groups54. Solid-state 1H NMR studies identify chemical shifts at 2.1 and 1.3 ppm for the hydrogen of –CH2– groups in TED and HMTA (Fig. 2c)55. These observations establish that TED and HMTA are chemically incorporated onto the OMSs. Elemental analysis reveals a nitrogen content of 6.38 and 12.15 wt% for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively. This is equivalent to ~2/3 TED or HMTA molecules grafted to each Cr, which is consistent with the previous report of two available open metal sites on each Cr3O cluster (2:3)45.
Nitrogen gas adsorption-desorption isotherms collected at 77 K indicate that the modification of TED and HMTA molecules onto MIL-101-Cr leads to a decrease in the Brunauer–Emmett–Teller surface area from 3342 to 2282 m2 g−1 and 2272 m2 g−1 for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively (Fig. 2d). Despite such decreases, the surface areas of the two amine-functionalized samples are significantly higher than any other benchmark porous materials, which usually exhibit moderate surface areas of ~300–1000 m2 g−110,11,12,13,14. Based on the pore size distribution (Supplementary Fig. 4), both MIL-101-Cr-TED and MIL-101-Cr-HMTA have pore diameters of about 16 and 21 Å, which are large enough for effective mass transfer during nuclear waste reprocessing. Thermogravimetric analysis (TGA) shows that MIL-101-Cr-TED and MIL-101-Cr-HMTA are stable up to 260 and 220 °C, respectively (Supplementary Note 1 and Supplementary Fig. 5). Isothermal TG analysis of amine grafted MIL-101-Cr samples clearly show that both TED and HMTA remain attached to the framework without losing mass upon prolonged heating at 150 °C for 12 h (Supplementary Fig. 6). The high thermal stability of the two compounds enables their use at the elevated working temperature (such as 150 °C) required for nuclear waste treatment. This result is consistent with the high binding energies of TED and HMTA to the OMSs (Supplementary Note 2, Supplementary Fig. 7, and Supplementary Table 1) obtained from ab initio theoretical calculations. The calculations also show that the TED and HMTA bind significantly more strongly to the OMSs compared to H2O molecules, further suggesting the feasibility of their application under humid conditions. In addition, two materials also show excellent stability in both CH3I gas stream and simulated off-gas mixture, as evident from the PXRD patterns collected after the experiments (Supplementary Fig. 8). The large surface area coupled with the high thermal and chemical stability of both MIL-101-Cr-TED and MIL-101-Cr-HMTA prompted us to evaluate their performance as molecular traps for the removal of ROIs from off-gas mixtures.
Radioactive organic iodides sorption studies
To evaluate the performance of MIL-101-Cr-TED and MIL-101-Cr-HMTA for ROIs capture, as-made samples (~20 mg of each) were placed in a thermogravimetric analyzer and a CH3I steam with partial pressure of 0.2 atm was passed through the sample cell using N2 as a carrier gas. The adsorption amount was monitored by recording sample mass as a function of time. As shown in Supplementary Fig. 9, MIL-101-Cr-TED and MIL-101-Cr-HMTA rapidly absorb 120 and 136 wt% CH3I within 10 min at 30 °C and reach their maximum uptake amount of 160 and 174 wt% by 120 min, respectively. The absorption amounts are significantly higher than all benchmark materials used for CH3I adsorption under the same conditions, such as TED- and HMTA-impregnated activated carbon (TED@AC and HMTA@AC) and silver functionalized zeolites (including ZSM-5, 13X, and mordenite (Ag+@ZSM-5, Ag+@13X, Ag+@MOR, and Ag0@MOR) with CH3I uptake amounts of 52, 54, 28, 45, 29, and 25 wt%, respectively (Supplementary Fig. 10)).
Since the capture of organic iodides from off-gas mixtures is usually performed at elevated temperatures (e.g., ~150 °C)15, we tested the CH3I uptake capacity at 150 °C for both samples and several benchmark materials. MIL-101-Cr-TED and MIL-101-Cr-HMTA can fast adsorb 48 and 39 wt% CH3I within 20 min (Fig. 3a). For the same time period, Ag0@MOR (the industrial zeolite material) only shows a CH3I uptake of 13 wt% under the same conditions. The fast adsorption rate of MIL-101-Cr-TED and MIL-101-Cr-HMTA is an important feature for practical applications of radioactive CH3I capture. The kinetic constants of MIL-101-Cr-TED and MIL-101-Cr-HMTA were calculated to be 0.30 and 0.36, respectively (Supplementary Note 3 and Supplementary Table 2), based on Lagergren’s pseudo first-order kinetic model. These values are similar as of other comparable materials, which have kinetic constant values between 0.19 and 0.62 (Supplementary Table 2 and Supplementary Fig. 11). At this temperature, the maximum uptake amounts at 0.2 atm are 71and 62 wt% for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively (Fig. 3a). These values are 4.4 and 3.9 times that of Ag0@MOR (16 wt%), a leading adsorbent material for capturing ROIs in the US nuclear fuel reprocessing industry48. We also compared the performance of MIL-101-Cr-TED with Ag+@13X, a zeolite with the highest silver content. Ag+@13X has a higher CH3I uptake amount (max. 48 wt%) compared to Ag0@MOR, but its low-acid resistance presents a serious drawback. MIL-101-Cr-TED adsorbs 1.5 times more CH3I than Ag+@13X under identical conditions. The capture capacity of MIL-101-Cr-TED is also much higher than the other benchmark materials, such as TED@AC, HMTA@AC, Ag+@ZSM-5, and Ag+@MOR, with uptake amounts of 17, 14, 24, and 16 wt%, respectively (Fig. 3b). Compared to the performance of pristine MIL-101-Cr (CH3I uptake: 13 wt%), TED functionalization leads to a remarkable increase of ~5.5 times. Based on these comparisons, MIL-101-Cr-TED clearly ranks as the top candidate for adsorbent-based capture and removal of ROIs during nuclear fuel reprocessing. The exceptionally high uptake capacity of tertiary amine functionalized MIL-101-Cr can be attributed to two main factors: (a) relatively high surface area of the adsorbent after functionalization, and more importantly, (b) effective grafting of TED and HMTA onto the MOF pore surface (via OMSs) creating molecular traps that offer greatly enhanced bonding interactions toward organic iodides. In addition, we performed adsorption experiments on two other organic iodides, CH3CH3I and CH3CH2CH2I. High uptake amounts were achieved for both species: 75 and 51 wt% of CH3CH3I and 74 and 54 wt% of CH3CH2CH3I in MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively (Supplementary Fig. 12).
To assess the influence of humidity on the organic iodide uptake capacity, a crucial aspect for a sorbent’s performance metrics in real-world applications, we performed column breakthrough tests at 150 °C under both dry and humid conditions (RH = 81% at 23 °C) (Supplementary Figs. 13–16 and Supplementary Table 3). For Ag+@13X, the zeolite with the best performance based on our parallel experimental results, the uptake drops from 41.3 to 16.1 wt%, a significant decrease of 61% (Fig. 3c, insert). We also observed a dramatic decrease of 63.7% for Ag0@MOR, with an uptake of 21.2 wt% under dry conditions and 7.7 wt% under humid conditions. For MIL-101-Cr-TED and MIL-101-Cr-HMTA, however, the extent of decrease is much smaller (42.4 and 40.8%, respectively). Based on the breakthrough data, the uptake capacities of MIL-101-Cr-TED and MIL-101-Cr-HMTA are 2.2 and 2.3 times higher than that of Ag+@13X, and 4.6 and 4.8 times greater than Ag0@MOR at 150 °C under humid conditions, underscoring the robustness of MIL-101-Cr-TED and MIL-101-Cr-HMTA adsorbents in humid environments. The higher hydrophilicity of zeolites compared to MOF materials may account for this difference, which makes MOFs are an advantageous platform for CH3I capture over conventional silver functionalized zeolites. As in the cases of previous studies8, moisture will affect the performance of capture materials. The decrease in the CH3I uptake capacity under humidity is likely due to the fact that a large amount of water molecules will take up the chemisorption sites and porous space, thereby reducing the overall loading amount.
Nuclear processing facilities’ regulatory standards require a “decontamination factor” (DF) of 3000 (99.967% of active species removed) for CH3I reprocessing, which is defined as the ratio of radioactivity before and after decontamination procedures56. To evaluate the efficiency of MIL-101-Cr-TED as a molecular trap for capturing CH3I from nuclear waste, we performed breakthrough experiments under conditions simulating the gas mixtures produced during CH3I reprocessing, which include H2O, HNO3, NO2, and NO at 150 °C56. As shown in Fig. 3d, for a very low CH3I concentration of 50 ppm that mimics real-world off-gas reprocessing conditions, very high DFs for MIL-101-Cr-TED are achieved, with the values range between 4800 and 6300, which are substantially higher than the reprocessing facility regulatory requirements57. This means that about 99.979–99.984% CH3I can be removed by MIL-101-Cr-TED under such conditions. The result further illustrates that the MOF-based molecular traps are highly suitable for ROIs capture from nuclear waste off-gas mixtures.
After CH3I adsorption, pristine MIL-101-Cr can be regenerated by washing with 3 M HCl followed by ethanol solution, resulting in complete recovery of the pristine MOF sample (Supplementary Figs. 17 and 18). The framework can then be re-functionalized to MIL-101-Cr-TED or MIL-101-Cr-HMTA following the initial procedure. The regenerated MIL-101-Cr-TED retains ~97–100% of the original loading capacity during the five full cycles (Fig. 3e). As silver-based adsorbents often suffer from a dramatic loss of adsorption capacity after only a few cycles (e.g., 50% loss for Ag+@13X after five cycles), our investigation thus established a recyclable system for ROIs capture from nuclear waste that is unattainable by any other known high-temperature adsorbents. We also estimated the CH3I capture cost for MIL-101-Cr-TED and Ag0@MOR. As shown in Supplementary Table 4, for each cycle the cost for the latter is 35 times of the former, a significant saving for MIL-101-Cr-TED.
To evaluate the material capability of capturing ROIs under the real-world conditions, we also conducted breakthrough experiments (Fig. 3f and Supplementary Fig. 19) at the conditions that mimic an off-gas mixture with high humidity (RH = 95%) and in the presence of HNO3 and NOx. The mixture also contains both radioactive species I2 (150 ppm) and CH3I (50 ppm). At 150 °C, the total iodine uptake amounts calculated based on unit weight and unit volume, as well as packing density of the sorbents (Supplementary Fig. 20) are summarized in Supplementary Table 5. The uptake are 38 and 33 wt% for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively, and high DF values (>5000) are obtained (Fig. 3f and Supplementary Table 5). These values are significant higher than those of Ag0@MOR (5 wt%)12 and pure silica zeolite HISL (16 wt%)15 under the same conditions (Fig. 3f and Supplementary Table 5). The results suggest that amine grafted MIL-101-Cr materials are capable of effectively capturing CH3I in off-gas mixtures containing I2. In addition, I2 adsorption isotherms were collected under similar experimental conditions (150 °C and 150 ppm) and its interaction with amine functionalized MIL-101-Cr were evaluated (Supplementary Note 4 and Supplementary Figs. 21–23). The possible adsorption mechanisms in simulated gas mixture were also investigated and binding energies were estimated by DFT calculations (Supplementary Note 2, Supplementary Fig. 24, and Supplementary Table 6). Similar experiments were also performed at room temperature, which gives the same trend (Supplementary Table 5). Furthermore, recyclability tests of MIL-101-Cr-TED under simulated off-gas conditions verified that the total iodine uptake remains the same after three cycles (Supplementary Fig. 25).
Investigation of CH3I-binding interactions mechanisms
The outstanding performance of MIL-101-Cr-TED and MIL-101-Cr-HMTA encouraged us to investigate the possible interaction mechanisms between CH3I molecules and the MOF host. Gas adsorption experiments carried out at 150 °C show evidence of both physisorption and chemisorption for CH3I (Supplementary Fig. 26), but chemisorption is the dominant mode of interaction (76 and 68% for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively) at that temperature, with most CH3I molecules being chemically trapped within the framework. The chemisorbed amounts are 54 and 43 wt%, respectively, for MIL-101-Cr-TED and MIL-101-Cr-HMTA, and physisorbed amounts, 17 and 19 wt%, respectively. The partial pressure of CH3I shows very little influence on the chemisorption capacity of the sorbents (Supplementary Fig. 27).
The strong interaction between CH3I molecules and MIL-101-Cr-TED and MIL-101-Cr-HMTA was verified by HRTEM-EDS, solid-state 1H NMR, XPS, and in situ FT-IR studies. Elemental mapping using HRTEM-EDS confirms uniformly dispersed iodine (CH3I) within the crystal samples of CH3I-loaded MIL-101-Cr-TED and MIL-101-Cr-HMTA (Fig. 4a, b). Solid-state 1H NMR spectra of CH3I-loaded MIL-101-Cr-TED and MIL-101-Cr-HMTA show a new peak at ~16 ppm (Fig. 4c, d), which can be assigned to the H atoms of CH3I58. The XPS data are consistent with this interpretation, as a good fraction of the N(1s) core level is shifted to higher binding energies upon CH3I loading (402.6 and 401.6 eV for MIL-101-Cr-TED and MIL-101-Cr-HMTA, respectively) as compared with the as-synthesized analogs. This shift indicates that the valence of N is increased by interacting with guest CH3I molecules (Fig. 4e, f). The N(1s) core level shifts more in CH3I@MIL-101-Cr-TED, 2.9 eV, compared to 1.8 eV in CH3I@MIL-101-Cr-HMTA, indicating less charge transfer in CH3I@MIL-101-Cr-HMTA. Consistent with this interaction, the I 3d5/2 peak of CH3I, positioned at 620.2 eV for the molecular adsorbed state, was red shifted to 618.7 ± 0.1 eV in MIL-101-Cr-TED and to 618.6 ± 0.1 eV in MIL-101-Cr-HMTA (Supplementary Fig. 28). This value is typical of CH3I dissociatively adsorbed on metal or metal oxide surfaces as previously observed (e.g., Ni(100), TiO2)59, 60. Similarly, a characteristic shift (~1 cm−1) of the signature ν(C-N) vibrational mode is observed with FT-IR upon CH3I loading of MIL-101-Cr-TED and MIL-101-Cr-HMTA (Fig. 4g, h). These results suggest the formation of strong chemical bonds between tertiary amines and CH3I, yielding ionic species (R3N-CH3)+ I− at high temperatures (Supplementary Fig. 29).
To test this hypothesis, we performed an ion-exchange experiment by using an anionic organic dye as a molecular probe. UV-vis measurements were used to monitor the adsorption efficiency of Orange G (OG) dye by the pristine MIL-101-Cr-TED and MIL-101-Cr-HMTA, as well as CH3I-loaded MIL-101-Cr-TED and MIL-101-Cr-HMTA (Fig. 4i and Supplementary Fig. 30). Fast anion-exchange kinetics were observed when using CH3I-loaded MIL-101-Cr-TED and MIL-101-Cr-HMTA as adsorbents, which adsorb over 95% of the anionic organic dye within 1 min and 30 s, respectively. In contrast, pristine MIL-101-Cr-TED and MIL-101-Cr-HMTA samples adsorb only 44 and 54% of the OG and over a much longer time period of 30 min. The fast kinetics of CH3I-loaded samples confirms the formation of (R3N-CH3)+ I− in high concentration when reacting CH3I with the free nitrogen atom of the amine molecules grafted on MIL-101-Cr-TED and MIL-101-Cr-HMTA at high temperature. In addition, the formation of I− ions after CH3I sorption was verified by AgNO3 titration of dye exchanged filtrates, which yielded AgI precipitate (Supplementary Fig. 31).
To better understand the relationship between the chemisorption and physisorption binding regime at different temperatures, we conducted simulations of the corresponding binding mechanisms (Supplementary Table 7). In particular, we performed an ab initio transition-state search to find the pathway that connects the two regimes and the energy barrier that separates them (see Supplementary Fig. 32). We find that an energy barrier of 459 meV separates the physisorption and chemisorption case while the energy difference for the products is 200 meV higher than that of the reactants (Supplementary Fig. 32). This energy difference is small enough at room temperature to allow some ionic I− to be present in the system, but large enough to prevent most CH3 from having covalently bonding to the nitrogen in TED. This finding is also consistent with our experimental results (Supplementary Figs. 33 and 34). Once the temperature increases to 150 °C, enough energy enters the system to overcome the energy barrier, resulting in the increased concentration of CH3 covalently bound to TED, which explains the experimentally observed higher amount of CH3I chemisorption (Supplementary Table 8).
Incorporating tertiary amine molecules within MIL-101-Cr gives rise to function-adjustable ROI molecular traps with record-high uptake capacities for ROIs capture from nuclear waste. In addition, these molecular traps exhibit excellent recyclability, which is not available for any currently known industrial adsorbents. Coupled with its exceptionally high chemical and thermal stability, high adsorption efficiency at a wide temperature range, and low cost, such molecular traps offer significant promise for ROIs capture from nuclear waste. We anticipate that such crystalline porous materials will become a new platform for effective capture of ROIs and that new molecular traps with optimized frameworks and improved performance will be developed in the near future.
Materials and measurements
Commercially available reagents were purchased in high purity and used without further purification. PXRD data were collected on a Rigaku Ultima-IV diffractometer or a Bruker AXS D8 Advance A25 Powder X-ray diffractometer. N2 gas sorption experiments were carried out on a Micromeritics 3Flex volumetric adsorption analyzer. Elemental analyses were performed on a Perkin-Elmer 2400 element analyzer. TGA was analyzed by a Q5000 thermogravimetric analyzer. The in situ infrared spectroscopic data were obtained using a Nicolet 6700 FTIR spectrometer (purchased from Thermo Scientific Inc, USA) equipped with a liquid N2-cooled mercury cadmium telluride MCT-A detector. A vacuum cell, purchased from Specac Ltd, UK (product number P/N 5850c), was placed in the sample compartment of the infrared spectrometer with the sample at the focal point of the beam (Supplementary Fig. 35). The MOFs (powder, ~2 mg) were gently pressed onto a KBr pellet (~1.3 cm diameter, 1–2 mm thick) and placed in the cell. The samples were first activated under atmospheric N2 flow at 150 °C for 3 h and then evacuated (base pressure <20 mtorr) for CH3I vapor exposure measurement. The infrared data were recorded during the vapor exposure. XPS measurements were performed on an ESCALAB 250 X-ray photoelectron spectroscopy, using Mg Kα X-ray as the excitation source. UV-Vis data were collected using a Shimadzu UV-3600 spectrophotometer. HRTEM-EDS analysis was performed in a FEI Tecnai G2 S-Twin with a field emission gun operating at 200 kV. Images were acquired digitally on a Gatan multiple CCD camera. The FEI Tecnai G2S-Twin is equipped with an EDS detector, which was used for elemental analysis of the nanocrystal composition. The 1H NMR data were collected on a Bruker AVANCE IIIHD console with 1.9 mm MAS probe. ICP was performed on a Perkin-Elmer Elan DRC II quadrupole inductively coupled plasma mass spectrometer (ICP-MS) analyzer. CH3I adsorption experiments were carried out on a homemade gravimetric adsorption analyzer modified from a thermogravimetric analyzer Q50 (TA Instruments).
Synthesis of MIL-101-Cr
MIL-101-Cr was synthesized according to the reported procedure with minor modifications61. Typically, a solution containing chromium(III) nitrate Cr(NO3)3·9H2O (800 mg, 2.0 mmol), HNO3 (2.0 mmol), benzene-1,4-dicarboxylic acid (328 mg, 2.0 mmol), and 10 mL H2O was transferred to the PTFE/Teflon liner in a hydrothermal autoclave, which is heated at 210 °C for 8 h and cooled afterwards slowly to room temperature. The solid product was isolated as a green powder by centrifugation and washed three times with DMF, water, ethanol for 12 h at 80 °C, respectively. The final product was dried under vacuum at 150 °C for 24 h.
Synthesis of MIL-101-Cr-TED
A resealable heavy-wall pressure flask was charged with MIL-101-Cr (1.0 g), TED (1.5 g), and benzene (50 mL). The flask was sealed and heated to 110 °C for 3 days. The green solid of MIL-101-Cr-TED was collected after washing the product with dry benzene, and then drying under vacuum at 200 °C for 3 h. Caution: the reaction was performed under high pressure with potential hazards. Elemental analysis: calculated: C: 47.63%; H: 3.97%, N: 6.17%; experimental: C: 47.58%; H: 4.14%; N: 6.38%. ICP: calculated: Cr 17.20%; experimental: Cr: 16.89%.
Synthesis of MIL-101-Cr-HMTA
A similar procedure was used to synthesize MIL-101-Cr-HMTA. MIL-101-Cr (1.0 g), HMTA (1.5 g), and chloroform (50 mL) were loaded in a resealable flask. The flask was sealed and heated to 110 °C for 3 days. The product was collected, washed with dry chloroform, and then dried under vacuum at 200 °C for 3 h to yield the green solid, MIL-101-Cr-HMTA. Caution: the reaction was performed under high pressure with potential hazards. Elemental analysis: calculated: C: 44.86%; H: 3.74%, N: 11.63%; experimental: C: 44.87%; H: 4.08%; N: 12.15%. ICP: calculated: Cr: 16.20%; experimental: Cr: 15.87%.
Synthesis of benchmark materials
The detail of synthesizing benchmark materials can be found in Supplementary Methods.
Organic iodide and I2 adsorption measurements
CH3I adsorption experiments were carried out on a homemade gravimetric adsorption analyzer modified from a thermogravimetric analyzer Q-50 (TA Instruments). In a typical adsorption experiment, ~20 mg adsorbent sample was loaded on the thermobalance and activated at 200 °C for 2 h under N2 flow to ensure complete removal of residue solvents in the sample. The temperature was then reduced to either 30 or 150 °C and the gas flow was switched from pure N2 to a combination of a pure N2 gas stream and another N2 gas stream passing through a CH3I bubbler. The flow rates of the two gas streams were controlled via two gas flow controllers to achieve certain partial pressures. The adsorption amount was monitored by recording the sample weight. The gas flow was switched back to pure N2 after a plateau was reached. The sorption data of CH3CH2I and CH3CH2CH2I were collected under the same experimental procedure at 150 °C with a partial pressure of 0.1 and 0.05 atm, respectively. I2 adsorption isotherms were also obtained following a similar procedure at 150 °C with the I2 concentration at 150 ppm.
Breakthrough experiment with or without humidity
The breakthrough experiment was conducted using a lab-scale fixed-bed reactor at 150 °C (Supplementary Fig. 36). In a typical experiment, the powder was activated at 150 °C for 3 h. Then 1.0 g of material was packed into a quartz column (5.8 mm I.D. × 150 mm) with silane-treated glass wool filling the void space. A helium flow (5 cm3 min−1) was used to purge the adsorbent. The flow of He was then turned off while dry N2 at a rate of 5 mL min−1 bubbled through CH3I and was allowed to flow into the column. The flow rate of CH3I was 8.872 mg min−1 (1.4 cm3 min−1), determined through trial and error. The effluent from the column was monitored using an online mass spectrometer (MS). Experiments in the presence of humidity were performed by injecting water into the gas mixture at a rate of 0.12 μL min−1 using a Fusion 100 syringe pump.
The absolute adsorbed amount of gas i(q i ) is calculated from the breakthrough curve by the equation:
where Fi is the influent flow rate of the specific gas (cm3 min−1); t0 is the adsorption time (min); Vdead is the dead volume of the system (cm3); Fe is the effluent flow rate of the specific gas (cm3 min−1); and m is the mass of the sorbent (g).
It should be mentioned that the loading amounts obtained from the breakthrough experiments are slightly different from those from adsorption isotherm measurements. This discrepancy is mainly due to small errors associated with factors such as sample particle size, packing length, and packing density.
Decontamination factor measurements
Decontamination factors (DFs) were measured using a similar system as breakthrough experiment. The concentration of CH3I was 50 ppm with or without I2 (150 ppm). 5 M nitric acid solution was introduced into a bubbler to allow the N2 (12 mL min−1) to carry the nitric acid and moisture vapors into the system, and the RH was 95% (23 °C). Heated lines temperature was kept at 150 °C to get in situ formation of NOx during heating. The residual CH3I and I2 were collected at interval time by NaOH bubbler and tested by ICP-MS. The DFs were calculated based on the ICP-MS data.
Ab initio calculations
Our ab initio calculations were performed at the density functional theory (DFT) level as implemented in the VASP62, 63 software, using the vdW-DF exchange-correlation function64, 65. We used PAW potentials with energy cutoff values of 600 eV and energies were converged to within 1×10−4 eV. Transition states were found with a common transition-state search algorithm.
A 10 mL aqueous solution of Orange G (0.073 mM) was added to a 20 mL vial, which was followed by addition of 30.0 mg of the respective MOF sample to form slurry at room temperature. During the stirring period, a small amount of mixture was drawn (~0.5 mL) and filtered immediately at selected time intervals through a 0.45 micron membrane filter, and the filtrates were analyzed using UV-vis spectroscopy to determine the concentration of the Orange G ions.
The data that support the findings of this study are available from the corresponding author on reasonable request.
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Financial support from the Materials Sciences and Engineering Division, Office of Basic Research Energy Sciences of the U.S. Department of Energy through Grant No. DE-FG02-08ER-46491 is gratefully acknowledged.
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