Microwave-Assisted Solvothermal Synthesis of UiO-66-NH 2 and Its Catalytic Performance toward the Hydrolysis of a Nerve Agent Simulant

: Zr-containing metal-organic frameworks (MOFs) exhibit a good performance of catalyzing the hydrolysis of chemical warfare agents, which is closely related to the size of MOF particles and its defects, but these two factors are often intertwined. In this article, we synthesized UiO-66-NH 2 nanoparticles using a microwave-assisted hydrothermal method. By using a new modulator 4-Fluoro-3-Formyl-Benzoic Acid (FFBA) in di ﬀ erent proportions, MOF particles with the same defect degree but di ﬀ erent scales and those with similar sizes but di ﬀ erent defect degrees can be obtained. The performance of the obtained MOF particles to catalyze the hydrolysis of the nerve agent simulant, dimethyl 4-nitrophenyl phosphate (DMNP), was investigated, and the e ﬀ ects of single factors of size or defect were compared for the ﬁrst time. As the size of the obtained MOF particles increased from 81 nm to 159 nm, the catalytic degradation e ﬃ ciency toward DMNP gradually decreased, and the half-life increased from 3.9 min to 11.1 min. For MOFs that have similar crystal sizes, the catalytic degradation half-life of MOF3 is only 5 min, which is much smaller than that of MOF5 due to the defects increase from 1.2 to 1.8 per Zr 6 cluster.


Introduction
Chemical warfare agents (CWAs) containing phosphonate ester bonds, which are named nerve agents, such as GA (Tabun), GB (Sarin), and GD (Soman), are among the most toxic chemicals known to mankind [1]. Recently, a series of world events [2][3][4][5] have made it necessary to continue to study the rapid destruction of these forbidden CWAs. Hydrolysis-based decontamination of CWAs remains an important way. The key is to find suitable catalysts to accelerate this process. Metal-organic frameworks (MOFs) are organic-inorganic hybrid materials, which have well-organized pore structures. With the help of coordination bonds, MOFs can be assembled by metal ions or metal-oxygen clusters and organic bridging ligands [6,7]. Recently, benefiting from their excellent properties such as ordered and tunable pore sizes, high surface areas, abundant metal sites, and controllable chemistry microenvironment, certain MOFs have been demonstrated to be promising catalysts, which can catalyze the degradation of toxic nerve agents and their simulants (hydrolysis). They can even detoxify such a deadly substance in just a few minutes [8][9][10][11] by providing people with new protection against the threat of CWA.
The typical effective MOFs usually contain Zr 6 clusters, such as UiO-66 (Universitet of Oslo), UiO-66-NH 2 , UiO-67, MOF-808, and NU-1000 [8][9][10]. They have multiple Zr-OH-Zr moieties, which can such as phosphotriesterase [5,12]. In addition, Zr-MOFs, like UiO-66-NH2, can be used as an active material for the sensor to identify a trace nerve agent [13]. Previous reports have revealed that most MOFs containing the small sizes of the pore structure, which hinder the reactants to go inside the interior pores of MOF and lead to the reaction, are diffusion-limited and their catalysis mainly occurred on the external surface of MOF particles [14,15]. Therefore, the size of MOFs has an important effect on catalysis, and the smaller the size of MOF crystals is, the more specific surface area/catalytic sites are available [16,17]. The defects in MOFs, such as missing linkers or nodes, is another important factor for the hydrolysis reaction of CWAs [18]. These two factors are often intertwined. For example, Peterson et al. [19] introduced more defects to the UiO-66-NH2. They found the high defect MOF (1.27 defects per node) has a reaction half-life by 20-fold shorter than that of a low defect MOF (0.55 defects per node). However, the high defect sample also have a significantly smaller crystal size than the smaller sample, which may contribute to enhance catalysis efficiency. Li et al. [17] reported the relationship between the catalytic hydrolysis of methyl paraoxon and the size of NU-1000 crystallites, and a remarkable increase in the rate was observed by reducing the crystal size. However, the defects in the MOFs were not discussed.
In this study, we try to synthesize UiO-66-NH2 nanoparticles with the same defective degree but different sizes. 4-Fluoro-3-Formyl-Benzoic Acid (FFBA) with a molecular structure similar to that of organic linker, 2-Aminoterephthalic acid (BDC-NH2), was used as a modulator, and a microwaveassisted solvothermal synthesis method was used to rapidly synthesize UiO-66-NH2 particles (Scheme 1). As the proportion of modifier FFBA increases from 0:10 to 1:9, 5:5 (molar ratio of FFBA to BDC-NH2), the size of MOF particles increases while keeping the defective degrees of the MOFs the same, which is equal to 1.2 per Zr6 cluster. However, when the ratio of FFBA to BDC-NH2 was fixed to 3:7, the defect of synthesized MOF (MOF3) increased to 1.8 per Zr6 cluster, while keeping the crystal size similar to that of MOF5 obtained when the molar ratio of FFBA to BDC-NH2 was 5:5. The performance of these obtained MOF particles to catalyze the hydrolysis of the nerve agent simulant, dimethyl 4-nitrophenyl phosphate (DMNP), was explored, and the effects of single factors of size or defect were discussed for the first time.

Synthesis and Characterization of UiO-66-NH2
UiO-66-NH 2 was prepared by a microwave-assisted solvothermal method with a varied molar ratio of FFBA to BDC-NH 2 and the obtained solid products with the ratio of 10:0, 9:1, 7:3, and 5:5 were labelled as MOF0, MOF1, MOF3, and MOF5, respectively. In order to confirm the success of the Catalysts 2020, 10, 1086 3 of 11 synthesis of UiO-66-NH 2 , Powder X-ray diffraction (PXRD), Fourier transform infrared spectra (FT-IR), scanning electron microscope (SEM), thermogravimetric analyses (TGA), Nitrogen physisorption, and nuclear magnetic resonance spectrometry (NMR) were used for characterization. As shown in Figure 1, the X-ray diffraction (XRD) patterns of all the four synthesized MOFs agree well with the simulated patterns from UiO-66 cif file [20]. There are three characteristic diffraction peaks at 7.4 • , 8.5 • , and 25.8 • corresponding to the (110), (200), and (600) planes of UiO-66-NH 2 . As the molar ratio of BDC-NH 2 and FFBA varied, the MOF products have the very similar patterns. PXRD results prove the success of the synthesis of UiO-66-NH 2 with high crystallinity with or without the modulator of FFBA.
Catalysts 2020, 10, x FOR PEER REVIEW 3 of 11 IR), scanning electron microscope (SEM), thermogravimetric analyses (TGA), Nitrogen physisorption, and nuclear magnetic resonance spectrometry (NMR) were used for characterization. As shown in Figure 1, the X-ray diffraction (XRD) patterns of all the four synthesized MOFs agree well with the simulated patterns from UiO-66 cif file [20]. There are three characteristic diffraction peaks at 7.4°, 8.5°, and 25.8° corresponding to the (110), (200), and (600) planes of UiO-66-NH2. As the molar ratio of BDC-NH2 and FFBA varied, the MOF products have the very similar patterns. PXRD results prove the success of the synthesis of UiO-66-NH2 with high crystallinity with or without the modulator of FFBA. The Fourier transform infrared (FT-IR) spectra of the produced MOFs and organic linker, NH2-BDC, are shown in Figure 2. In the spectrum of NH2-BDC, the vibrational bands around 3389 cm -1 and 3506 cm -1 correspond to (-NH2) group, the broad band around 2500-3000 cm -1 ascribes to the coupled -OH of COOH, and the strong peak at 1682 cm -1 is assigned to the C=O stretching of COOH [21]. The spectra of MOF0, MOF1, MOF3, and MOF5 are almost the same. The three strong peaks at 1567, 1427, and 1385 cm -1 originate from the carboxyl group on the organic linker, NH2-BDC. The triplet peaks at 767, 663, and 482 cm -1 spring from O-Zr-O vibrations in the metal-oxygen clusters [22]. The broad band around 2500-3000 cm -1 disappears and no band at around 1680 is observed, which indicates all the (-COOH) in NH2-BDC were coordinated with the Zr6 cluster and all modulators (BBFA) are rinsed out completely.  The Fourier transform infrared (FT-IR) spectra of the produced MOFs and organic linker, NH 2 -BDC, are shown in Figure 2. In the spectrum of NH 2 -BDC, the vibrational bands around 3389 cm −1 and 3506 cm −1 correspond to (-NH 2 ) group, the broad band around 2500-3000 cm −1 ascribes to the coupled -OH of COOH, and the strong peak at 1682 cm −1 is assigned to the C=O stretching of COOH [21]. The spectra of MOF0, MOF1, MOF3, and MOF5 are almost the same. The three strong peaks at 1567, 1427, and 1385 cm −1 originate from the carboxyl group on the organic linker, NH 2 -BDC. The triplet peaks at 767, 663, and 482 cm −1 spring from O-Zr-O vibrations in the metal-oxygen clusters [22]. The broad band around 2500-3000 cm −1 disappears and no band at around 1680 is observed, which indicates all the (-COOH) in NH 2 -BDC were coordinated with the Zr 6 cluster and all modulators (BBFA) are rinsed out completely.
Catalysts 2020, 10, x FOR PEER REVIEW 3 of 11 IR), scanning electron microscope (SEM), thermogravimetric analyses (TGA), Nitrogen physisorption, and nuclear magnetic resonance spectrometry (NMR) were used for characterization. As shown in Figure 1, the X-ray diffraction (XRD) patterns of all the four synthesized MOFs agree well with the simulated patterns from UiO-66 cif file [20]. There are three characteristic diffraction peaks at 7.4°, 8.5°, and 25.8° corresponding to the (110), (200), and (600) planes of UiO-66-NH2. As the molar ratio of BDC-NH2 and FFBA varied, the MOF products have the very similar patterns. PXRD results prove the success of the synthesis of UiO-66-NH2 with high crystallinity with or without the modulator of FFBA. The Fourier transform infrared (FT-IR) spectra of the produced MOFs and organic linker, NH2-BDC, are shown in Figure 2. In the spectrum of NH2-BDC, the vibrational bands around 3389 cm -1 and 3506 cm -1 correspond to (-NH2) group, the broad band around 2500-3000 cm -1 ascribes to the coupled -OH of COOH, and the strong peak at 1682 cm -1 is assigned to the C=O stretching of COOH [21]. The spectra of MOF0, MOF1, MOF3, and MOF5 are almost the same. The three strong peaks at 1567, 1427, and 1385 cm -1 originate from the carboxyl group on the organic linker, NH2-BDC. The triplet peaks at 767, 663, and 482 cm -1 spring from O-Zr-O vibrations in the metal-oxygen clusters [22]. The broad band around 2500-3000 cm -1 disappears and no band at around 1680 is observed, which indicates all the (-COOH) in NH2-BDC were coordinated with the Zr6 cluster and all modulators (BBFA) are rinsed out completely. Morphologies of produced MOFs were investigated by scanning electron microscopy (SEM) observation, and the results are shown in Figure 3. All samples exhibit well-shaped octahedral shapes, but the dispersion of their sizes using different amounts of the BBFA modulator is very broad. The size distribution of MOF0, MOF1, MOF3, and MOF5 in Figure 3 were analyzed, as shown in Figures S1-S4. When no BBFA is added, the obtained UiO-66-NH 2 nanocrystals (MOF0) are uniform and small. The average size is 81.2 nm. When the ratio of BBFA to BDC-NH 2 increases to 1:9, the obtained MOF1 nanocrystals are slightly agglomerated. The average size of MOF1 increases to 111.3 nm. When the ratio of BBFA to BDC-NH 2 further increases to 3:7, it can be observed that there are two different sizes of BDC-NH 2 particles generated. The smaller one is about 149.3 nm and the larger one is about 300 nm. When adding more modulator BBFA, up to one equivalent per BDC-NH 2 , the obtained UiO-66-NH 2 nanocrystals (MOF5) become uniform again and the average size is about 159.3 nm.
Catalysts 2020, 10, x FOR PEER REVIEW 4 of 11 Morphologies of produced MOFs were investigated by scanning electron microscopy (SEM) observation, and the results are shown in Figure 3. All samples exhibit well-shaped octahedral shapes, but the dispersion of their sizes using different amounts of the BBFA modulator is very broad. The size distribution of MOF0, MOF1, MOF3, and MOF5 in Figure 3 were analyzed, as shown in Figure S1-S4. When no BBFA is added, the obtained UiO-66-NH2 nanocrystals (MOF0) are uniform and small. The average size is 81.2 nm. When the ratio of BBFA to BDC-NH2 increases to 1:9, the obtained MOF1 nanocrystals are slightly agglomerated. The average size of MOF1 increases to 111.3 nm. When the ratio of BBFA to BDC-NH2 further increases to 3:7, it can be observed that there are two different sizes of BDC-NH2 particles generated. The smaller one is about 149.3 nm and the larger one is about 300 nm. When adding more modulator BBFA, up to one equivalent per BDC-NH2, the obtained UiO-66-NH2 nanocrystals (MOF5) become uniform again and the average size is about 159.3 nm. In addition, Lillerud's protocol [23] was used to confirm and evaluate the existence of defects from the thermogravimetric analysis (TGA) curves under air flow. The molecular weight of Zr6O6 (BDC-NH2)6, the dehydroxylated form of UiO-66-NH2 is 2.32 times of 6ZrO2, which is the only solid product after aerobic decomposition of UiO-66-NH2. Therefore, if the final weight of the aerobic TGAoperation is normalized to 100%, the plateau (representing the empty, solvent-free material) should ideally reach 232%. The normalized TGA curves of the obtained MOFs were plotted in Figure  4. The weight of MOF0, MOF1 and MOF5 at 297 °C is almost similar, which is 203.3% of 6ZrO2. The estimated density of missing-linker defects in MOF0, MOF1, and MOF5 per Zr6 cluster is only 1.2. Unexpectedly, the weight of MOF3 at 297 °C is only 189.8% of 6ZrO2, and the estimated defects of MOF3 reaches as high as 1.8 per Zr6 cluster. In addition, Lillerud's protocol [23] was used to confirm and evaluate the existence of defects from the thermogravimetric analysis (TGA) curves under air flow. The molecular weight of Zr 6 O 6 (BDC-NH 2 ) 6 , the dehydroxylated form of UiO-66-NH 2 is 2.32 times of 6ZrO 2 , which is the only solid product after aerobic decomposition of UiO-66-NH 2 . Therefore, if the final weight of the aerobic TGAoperation is normalized to 100%, the plateau (representing the empty, solvent-free material) should ideally reach 232%. The normalized TGA curves of the obtained MOFs were plotted in Figure 4. The weight of MOF0, MOF1 and MOF5 at 297 • C is almost similar, which is 203.3% of 6ZrO 2 . The estimated density of missing-linker defects in MOF0, MOF1, and MOF5 per Zr 6 cluster is only 1.2. Unexpectedly, the weight of MOF3 at 297 • C is only 189.8% of 6ZrO 2 , and the estimated defects of MOF3 reaches as high as 1.8 per Zr 6 cluster.  The specific surface areas and pore structures were determined by Nitrogen adsorptiondesorption isotherms, as shown in Figure 5. When p/p0 is less than 0.01, the adsorption capacity rises linearly, which indicates that the samples contain a large number of micropores. As the relative pressure increases, the adsorption isotherm bends into a plateau. When p/p0 increases to more than 0.9, the adsorption capacity increased significantly, which indicates that there is a certain macroporous structure in the sample. Combined with the SEM observation, it can be observed that the macropores are formed by accumulating MOF particles. The adsorption and desorption isotherm characteristics of the four samples are very similar, which indicates that their pore structure characteristics are almost the same. The Brunauer-Emmett-Teller (BET) specific surface areas of MOF0, MOF1, MOF3, and MOF5 are 642.9, 679.7, 691.3, and 741.2 m 2 /g, respectively, that is, with the increase of the modulator FFBA, the specific surface area slightly increases. Furthermore, the pore size distribution of the four were analyzed by Horvath-Kawazoe (HK) and Barrett-Joyner-Halenda (BJH) methods, and the results are presented in Figure S5-S8 and S9-S12, respectively. In the micropore range (< 2 nm), the most probable pore size distribution of the four samples is about 0.5 nm ( Figure S5-8), which is very close to the theoretical dynamic pore size of UiO-66-NH2. In the mesoporous range (2-50 nm) and macroporous range (> 50 nm) ( Figure S9-S12), the four samples have no clear pore distribution, which indicates that the defect degree is not high enough, and the defect-induced pores are not clear.  The specific surface areas and pore structures were determined by Nitrogen adsorption-desorption isotherms, as shown in Figure 5. When p/p 0 is less than 0.01, the adsorption capacity rises linearly, which indicates that the samples contain a large number of micropores. As the relative pressure increases, the adsorption isotherm bends into a plateau. When p/p 0 increases to more than 0.9, the adsorption capacity increased significantly, which indicates that there is a certain macroporous structure in the sample. Combined with the SEM observation, it can be observed that the macropores are formed by accumulating MOF particles. The adsorption and desorption isotherm characteristics of the four samples are very similar, which indicates that their pore structure characteristics are almost the same. The Brunauer-Emmett-Teller (BET) specific surface areas of MOF0, MOF1, MOF3, and MOF5 are 642.9, 679.7, 691.3, and 741.2 m 2 /g, respectively, that is, with the increase of the modulator FFBA, the specific surface area slightly increases. Furthermore, the pore size distribution of the four were analyzed by Horvath-Kawazoe (HK) and Barrett-Joyner-Halenda (BJH) methods, and the results are presented in Figures S5-S8 and S9-S12, respectively. In the micropore range (<2 nm), the most probable pore size distribution of the four samples is about 0.5 nm (Figures S5-S8), which is very close to the theoretical dynamic pore size of UiO-66-NH 2 . In the mesoporous range (2-50 nm) and macroporous range (>50 nm) ( Figures S9-S12), the four samples have no clear pore distribution, which indicates that the defect degree is not high enough, and the defect-induced pores are not clear.  The specific surface areas and pore structures were determined by Nitrogen adsorptiondesorption isotherms, as shown in Figure 5. When p/p0 is less than 0.01, the adsorption capacity rises linearly, which indicates that the samples contain a large number of micropores. As the relative pressure increases, the adsorption isotherm bends into a plateau. When p/p0 increases to more than 0.9, the adsorption capacity increased significantly, which indicates that there is a certain macroporous structure in the sample. Combined with the SEM observation, it can be observed that the macropores are formed by accumulating MOF particles. The adsorption and desorption isotherm characteristics of the four samples are very similar, which indicates that their pore structure characteristics are almost the same. The Brunauer-Emmett-Teller (BET) specific surface areas of MOF0, MOF1, MOF3, and MOF5 are 642.9, 679.7, 691.3, and 741.2 m 2 /g, respectively, that is, with the increase of the modulator FFBA, the specific surface area slightly increases. Furthermore, the pore size distribution of the four were analyzed by Horvath-Kawazoe (HK) and Barrett-Joyner-Halenda (BJH) methods, and the results are presented in Figure S5-S8 and S9-S12, respectively. In the micropore range (< 2 nm), the most probable pore size distribution of the four samples is about 0.5 nm ( Figure S5-8), which is very close to the theoretical dynamic pore size of UiO-66-NH2. In the mesoporous range (2-50 nm) and macroporous range (> 50 nm) ( Figure S9-S12), the four samples have no clear pore distribution, which indicates that the defect degree is not high enough, and the defect-induced pores are not clear.  As we know, in some cases, the modulator can coordinate to the cluster (especially in defective structures) in the synthesis process. In this case, we use NMR spectra to confirm if the new modulator FFBA would coordinate to the Zr 6 cluster. The 19 F, 1 H, and 13 C NMR spectra of four obtained MOF samples were performed and those spectra of FFBA, BDC-NH 2 , and DMF were also carried out for comparison. Figure S13 exhibits the chemical structures of DMF, BDC-NH 2 , and FFBA in the NMR test when NaOD/D 2 O (10 wt%) was used as the solvent. The 19 F spectra ( Figure S14) clearly show that the four MOF samples do not contain the FFBA modulator. The 1 H and 13 C spectra (Figures S15 and S16) further confirms this conclusion. They suggest that the four MOF samples contain only BDC-NH 2 ligands besides a small amount of residual DMF.

Catalysis Performance toward the Hydrolysis of DMNP
To determine the catalytic performance of obtained UiO-66-NH 2 toward the detoxification of CWAs, the catalysis on the hydrolysis of the CWA simulant, DMNP, was investigated for safety. DMNP has been widely used to simulate GA (Tabun), GB (Sarin), and GD (Soman) nerve agents [15,24] because they all contain similar phosphate ester bonds, but DMNP has much lower toxicity. Another advantage of using DMNP is that its decomposition product, 4-nitrophenol (Scheme 2) [6,7], has an absorption peak at around 407 nm, which makes it very easy to monitor the reaction process by Ultraviolet-visible (UV-Vis) spectroscopy.
Catalysts 2020, 10, x FOR PEER REVIEW 6 of 11 As we know, in some cases, the modulator can coordinate to the cluster (especially in defective structures) in the synthesis process. In this case, we use NMR spectra to confirm if the new modulator FFBA would coordinate to the Zr6 cluster. The 19 F, 1 H, and 13 C NMR spectra of four obtained MOF samples were performed and those spectra of FFBA, BDC-NH2, and DMF were also carried out for comparison. Figure S13 exhibits the chemical structures of DMF, BDC-NH2, and FFBA in the NMR test when NaOD/D2O (10 wt%) was used as the solvent. The 19 F spectra ( Figure S14) clearly show that the four MOF samples do not contain the FFBA modulator. The 1 H and 13 C spectra (Figure S15-S16) further confirms this conclusion. They suggest that the four MOF samples contain only BDC-NH2 ligands besides a small amount of residual DMF.

Catalysis Performance toward the Hydrolysis of DMNP
To determine the catalytic performance of obtained UiO-66-NH2 toward the detoxification of CWAs, the catalysis on the hydrolysis of the CWA simulant, DMNP, was investigated for safety. DMNP has been widely used to simulate GA (Tabun), GB (Sarin), and GD (Soman) nerve agents [15,24] because they all contain similar phosphate ester bonds, but DMNP has much lower toxicity. Another advantage of using DMNP is that its decomposition product, 4-nitrophenol (Scheme 2) [6,7], has an absorption peak at around 407 nm, which makes it very easy to monitor the reaction process by Ultraviolet-visible (UV-Vis) spectroscopy.

Scheme 2. Degradation of dimethyl 4-nitrophenyl phosphate (DMNP) to 4-nitrophenol.
The observed UV-vis spectra of hydrolysis reaction for DMNP using MOF0 as a catalyst were shown in Figure 6A, the intensity at 275 nm (corresponding to DMNP) decreases, and the peak at 407 nm (corresponding to 4-nitrophenol) increases along with time, which indicates that the DMNP can be effectively degraded and 4-nitrophenol can be released in the presence of MOF0. The monitor UVvis spectra of the hydrolysis reaction of DMNP in the presence of MOF1, MOF3, and MOF5 were shown in Figure S17-S19. The conversion profiles were further calculated and are given in Figure 6B. The half-lives of hydrolysis of DMNP were evaluated, according to first-order kinetics ( Figure S20-S23), and are presented in Table 1. The MOF0 shows high efficiency in hydrolyzing DMNP. The halflife of DMNP hydrolysis with MOF0 as a catalyst is 3.9 min, and, after 20 min, the hydrolysis rate can appear up to 90%. The half-lives of DMNP hydrolysis with MOF1, MOF3, and MOF5 as catalysts are 9.1, 5.0, and 11.1 min, respectively. The half-life of DMNP hydrolysis with no catalysts is as long as 1634 min, which suggests that all of the obtained UiO-66-NH2 can effectively catalyze DMNP to hydrolysis.

Scheme 2. Degradation of dimethyl 4-nitrophenyl phosphate (DMNP) to 4-nitrophenol.
The observed UV-vis spectra of hydrolysis reaction for DMNP using MOF0 as a catalyst were shown in Figure 6A, the intensity at 275 nm (corresponding to DMNP) decreases, and the peak at 407 nm (corresponding to 4-nitrophenol) increases along with time, which indicates that the DMNP can be effectively degraded and 4-nitrophenol can be released in the presence of MOF0. The monitor UV-vis spectra of the hydrolysis reaction of DMNP in the presence of MOF1, MOF3, and MOF5 were shown in Figures S17-S19. The conversion profiles were further calculated and are given in Figure 6B. The half-lives of hydrolysis of DMNP were evaluated, according to first-order kinetics ( Figures S20-S23), and are presented in Table 1. The MOF0 shows high efficiency in hydrolyzing DMNP. The half-life of DMNP hydrolysis with MOF0 as a catalyst is 3.9 min, and, after 20 min, the hydrolysis rate can appear up to 90%. The half-lives of DMNP hydrolysis with MOF1, MOF3, and MOF5 as catalysts are 9.1, 5.0, and 11.1 min, respectively. The half-life of DMNP hydrolysis with no catalysts is as long as 1634 min, which suggests that all of the obtained UiO-66-NH 2 can effectively catalyze DMNP to hydrolysis.
Catalysts 2020, 10, x FOR PEER REVIEW 6 of 11 As we know, in some cases, the modulator can coordinate to the cluster (especially in defective structures) in the synthesis process. In this case, we use NMR spectra to confirm if the new modulator FFBA would coordinate to the Zr6 cluster. The 19 F, 1 H, and 13 C NMR spectra of four obtained MOF samples were performed and those spectra of FFBA, BDC-NH2, and DMF were also carried out for comparison. Figure S13 exhibits the chemical structures of DMF, BDC-NH2, and FFBA in the NMR test when NaOD/D2O (10 wt%) was used as the solvent. The 19 F spectra ( Figure S14) clearly show that the four MOF samples do not contain the FFBA modulator. The 1 H and 13 C spectra (Figure S15-S16) further confirms this conclusion. They suggest that the four MOF samples contain only BDC-NH2 ligands besides a small amount of residual DMF.

Catalysis Performance toward the Hydrolysis of DMNP
To determine the catalytic performance of obtained UiO-66-NH2 toward the detoxification of CWAs, the catalysis on the hydrolysis of the CWA simulant, DMNP, was investigated for safety. DMNP has been widely used to simulate GA (Tabun), GB (Sarin), and GD (Soman) nerve agents [15,24] because they all contain similar phosphate ester bonds, but DMNP has much lower toxicity. Another advantage of using DMNP is that its decomposition product, 4-nitrophenol (Scheme 2) [6,7], has an absorption peak at around 407 nm, which makes it very easy to monitor the reaction process by Ultraviolet-visible (UV-Vis) spectroscopy.

Scheme 2. Degradation of dimethyl 4-nitrophenyl phosphate (DMNP) to 4-nitrophenol.
The observed UV-vis spectra of hydrolysis reaction for DMNP using MOF0 as a catalyst were shown in Figure 6A, the intensity at 275 nm (corresponding to DMNP) decreases, and the peak at 407 nm (corresponding to 4-nitrophenol) increases along with time, which indicates that the DMNP can be effectively degraded and 4-nitrophenol can be released in the presence of MOF0. The monitor UVvis spectra of the hydrolysis reaction of DMNP in the presence of MOF1, MOF3, and MOF5 were shown in Figure S17-S19. The conversion profiles were further calculated and are given in Figure 6B. The half-lives of hydrolysis of DMNP were evaluated, according to first-order kinetics ( Figure S20-S23), and are presented in Table 1. The MOF0 shows high efficiency in hydrolyzing DMNP. The halflife of DMNP hydrolysis with MOF0 as a catalyst is 3.9 min, and, after 20 min, the hydrolysis rate can appear up to 90%. The half-lives of DMNP hydrolysis with MOF1, MOF3, and MOF5 as catalysts are 9.1, 5.0, and 11.1 min, respectively. The half-life of DMNP hydrolysis with no catalysts is as long as 1634 min, which suggests that all of the obtained UiO-66-NH2 can effectively catalyze DMNP to hydrolysis.

Discussion
The three-dimensional relationship diagram of the first-order chemical reaction rate constant (k 1 ) with the sizes of the MOF catalysts and their defect degrees were shown in Figure 7. MOF0, MOF1, and MOF5 have a very similar defect degree estimated from the TGA curve, while they have different sizes. MOF0 is only about 81.2 nm, MOF1 increases to 111.3 nm, and MOF5 is as large as 159.3 nm. Accordingly, the calculated first-order chemical reaction rate constants (k 1 ) of the hydrolysis reaction of DMNP with MOF0, MOF1, or MOF5 as catalysts are 0.177, 0.076, and 0.062 min −1 , respectively. It indicates that the catalytic performance of MOF particles is inversely proportional to the size of MOF particles, when the defect density is equal. For MOF3, most of them are relatively small particles with a size of 149.3 nm, and a small number of particles at around 300 nm. Comparing MOF3 and MOF5, they have similar sizes, but their defect density is very different. MOF3 reaches 1.8 per Zr 6 unit, while MOF5 only has 1.2 per Zr 6 cluster. Comparing the catalytic performance of the two, it can be seen that the reaction rate constant of MOF3 is 122% higher than that of MOF5, and the half-life is only 45% of that of MOF5, which is as short as about 5 min. This is almost comparable to that of MOF0. The result testifies that the defects of MOFs play an important role in catalyzing the decomposition of DMNP. The greater the degree of MOF defects, the better the catalytic performance of MOF.

Discussion
The three-dimensional relationship diagram of the first-order chemical reaction rate constant (k1) with the sizes of the MOF catalysts and their defect degrees were shown in Figure 7. MOF0, MOF1, and MOF5 have a very similar defect degree estimated from the TGA curve, while they have different sizes. MOF0 is only about 81.2 nm, MOF1 increases to 111.3 nm, and MOF5 is as large as 159.3 nm. Accordingly, the calculated first-order chemical reaction rate constants (k1) of the hydrolysis reaction of DMNP with MOF0, MOF1, or MOF5 as catalysts are 0.177, 0.076, and 0.062 min -1 , respectively. It indicates that the catalytic performance of MOF particles is inversely proportional to the size of MOF particles, when the defect density is equal. For MOF3, most of them are relatively small particles with a size of 149.3 nm, and a small number of particles at around 300 nm. Comparing MOF3 and MOF5, they have similar sizes, but their defect density is very different. MOF3 reaches 1.8 per Zr6 unit, while MOF5 only has 1.2 per Zr6 cluster. Comparing the catalytic performance of the two, it can be seen that the reaction rate constant of MOF3 is 122% higher than that of MOF5, and the half-life is only 45% of that of MOF5, which is as short as about 5 min. This is almost comparable to that of MOF0. The result testifies that the defects of MOFs play an important role in catalyzing the decomposition of DMNP. The greater the degree of MOF defects, the better the catalytic performance of MOF. It is worth mentioning that there have been several reports concerning the degradation properties of UiO-66-NH2 powders [19,[25][26][27][28][29][30]. The shortest half-life of degradation of DMNP catalyzed by UiO-66-NH2 reported in the literature is less than 1 min [26] while the longest half-life reaches 495 min [19]. This difference is mainly due to the different sizes of MOF catalyst particles and the introduction of different defects. However, these two factors are often intertwined with each It is worth mentioning that there have been several reports concerning the degradation properties of UiO-66-NH 2 powders [19,[25][26][27][28][29][30]. The shortest half-life of degradation of DMNP catalyzed by UiO-66-NH 2 reported in the literature is less than 1 min [26] while the longest half-life reaches 495 min [19]. This difference is mainly due to the different sizes of MOF catalyst particles and the introduction of different defects. However, these two factors are often intertwined with each other, and there is no sufficient direct investigation of the influence of a single factor in the previous literature when the other factor is the same. Herein, the UiO-66-NH 2 nanoparticles with different sizes and the same defects were produced. The particles with different defects and similar sizes were also obtained in the same procedure with different ratios of modulator BBFA to BDC-NH 2 . The effect of a single factor of size or defect was discussed directly for the first time. The kinetic parameters of DMNP hydrolysis catalyzed different Zr-MOFs reported in the literatures are listed in Table S1. Besides UiO-66-NH 2 , other Zr-based MOFs, such as UiO-66 [15], UiO-67 [31], NU-1000 [12], and MOF-808 [32], were also explored for catalyzing the hydrolysis of nerve agent simulants. Typical half-lives of UiO-66 and NU-1000 are 35 min and 15 min, respectively, which were longer than that of those MOFs obtained in this scenario. In addition, the half-life of UiO-67 are about 3.5 min, which is comparable with those reported in this case. Furthermore, the half-lives of dehydrated NU-1000 and MOF-808 are only 1.5 min and 0.5 min, which are shorter than those reported in this work. Further optimization of the defect degree and particle size of UiO-66-NH 2 is expected to further improve its catalytic performance, reaching, or even exceeding, the catalytic activity of dehydrated NU-1000 and MOF-808.

Synthesis of UiO-66-NH 2
UiO-66-NH 2 was synthesized by microwave-assisted solvothermal method according to literature with modification [33][34][35]. Typically, ZrCl 4 (320 mg, 1.37 mmol) was dissolved in 50 mL DMF in a 200-mL beaker. Then 7-mL acetic acid (HAc) and 286-µl concentrated hydrochloric acid (HCl) were added into the solution. Afterward, a total of 1.38 mmol of BDC-NH 2 ligand and FFBA modulator were added into the mixture. The molar ratio of BDC-NH 2 and FFBA was varied to be 10:0, 9:1, 7:3, and 5:5, respectively. The mixture was transferred into a Teflon autoclave after 30 min of stirring. Furthermore, the autoclave was heated to 125 • C in a XH-300-A+ microwave reactor (Xianghu, Beijing) with an irradiation power of 300 W and kept there for 30 min. After cooling to room temperature, the synthesized products were obtained by centrifugation (12000 rpm), washing (2 times in DMF, soaking in acetone overnight), and drying (120 • C).

Catalytic Degration of DMNP
Catalytic hydrolysis of DMNP was performed according to the previous reports [29,30]. Typically, 10.4 mg of catalyst (MOF0, MOF1, MOF3, and MOF5, respectively) was added to 4.0 mL of N-EM solution (0.45 M, pH = 10) in a 50-mL vial at 25 • C. The resulting dispersion was vigorously sonicated for 5 min and stirred at 1100 rpm for 5 min. Then, 16 µL of DMNP was added to the suspension, and the stirring was kept at 1100 rpm. A 20-µL aliquot from the reaction mixture was taken out at a specific time, and diluted with 10 mL of N-EM solution (0.45 M). Catalytic efficiency was evaluated by observing the absorbance at 407 nm of 4-nitrophenoxide. For comparison, similar experiments were performed without a catalyst.

Characterization
PXRD patterns of the obtained MOFs were measured on a diffractometer (Bruker D8, Karlsruhe, Germany) with Cu Ka = 1.5418 Å. FT-IR were obtained using a spectrometer (Spectrum-Two, PerkinElmer, Waltham, MA, USA) equipped with an attenuated total reflectance (ATR) accessory. SEM images were observed on a Zeiss Sigma HD microscope (Jena, Japan). TGA were carried out on a thermal analyzer (STA6000, PerkinElmer, Waltham, MA, USA) under air flow at a heating rate of 10 • C/min. Nitrogen adsorption-desorption isotherms were recorded from a Quantachrome AUTOSORB IQ analyzer (Boynton Beach, FL, USA). NMR spectra were acquired on a Bruker 400M NMR spectrometer (Ettlingen, Germany). UV-Vis spectroscopy monitoring of DMNP hydrolysis in the range of 250-500 nm was performed using a spectrophotometer (LabTech BlueStarA, Beijing, China).

Conclusions
In this work, we have successfully prepared UiO-66-NH 2 using a rapid microwave-assisted solvothermal method. A new modulator of BBFA whose structure is similar to the ligand can effectively regulate the crystal size and defects of UiO-66-NH 2 . The UiO-66-NH 2 nanoparticles with different sizes and the same defects as well as particles with different defects and similar sizes can be produced in the same procedure with different ratios of modulator BBFA to BDC-NH 2 . Benefiting from this, the effect of a single factor of size or defect have been discussed directly for the first time. The catalytic performance of MOF particles is inversely proportional to the size of MOF particles when the defect density is equal. Furthermore, the greater the degree of MOF defects is, the better the catalytic performance of MOF is. Therefore, the preparation of MOF with both a small size and high defects is an important way to improve its catalytic performance.