ARTICLE pubs.acs.org/crystal Tuning the Formations of MetalOrganic Frameworks by Modification of Ratio of Reactant, Acidity of Reaction System, and Use of a Secondary Ligand Qian Gao,†,‡ Ya-Bo Xie,*,† Jian-Rong Li,‡ Da-Qiang Yuan,‡ Audrey A. Yakovenko,‡ Ji-Hong Sun,*,† and Hong-Cai Zhou*,‡ † ‡ College of Environmental and Energy Engineering, Beijing University of Technology, Beijing, 100124, P. R. China Department of Chemistry, Texas A&M University, P.O. Box 30012, College Station, Texas 77842, United States bS Supporting Information ABSTRACT: Four porous coordination networks (PCNs), {[Zn 3 O(H2O)3(adc)3] 3 2(C2H6NH2) 3 2(DMF) 3 3(H2O)}n (PCN-131), Zn2(DMA)2(adc)2] 3 2(DMA)}n (PCN-132), {[Zn3O(DMF)(adc)3(4,40 -bpy)] 3 2(C2H6 NH2) 3 S}n (PCN-1310 ), and {[Zn(adc)(4,40 -bpy)0.5] 3 S}n (PCN-1320 ), have been synthesized by the assembly of anthrancene-9,10-dicarboxylic acid (H2adc) with Zn(II) under different reaction conditions, including modifications of reactant ratio, acidity variations, and the use of a secondary ligand. Single-crystal X-ray diffraction studies reveal that PCN-131, obtained from the dimethylformamide (DMF) solution under acid condition, has a threedimentional (3D) framework structure with one-dimensional (1D) honeycomb channels. PCN-132 isolated from dimethylacetamide (DMA) solution without adding acid in synthesis is a two-dimensional (2D) layer compound. By employing 4,40 -bipyridyl (4,40 -bpy) as a secondary ligand, PCN-1310 and PCN-1320 were synchronously synthesized as a mixture outcome with more PCN-1310 than PCN-1320 . In PCN-1310 , 4,40 -bpy acting as a secondary ligand is arranged inside the honeycomb channel of the 3D PCN-131, resulting in an effective improvement of thermal stability of the network, while in PCN-1320 , 4,40 -bpy ligands link 2D layers of PCN-132 to form a pillared-layer 3D framework. Gas adsorption has been performed for selected materials. The results show that the framework of PCN-131 is thermally unstable after removing the solvent molecules coordinated to their metal sites. While PCN-1310 is stable for gas uptake, with an evaluated Langmuir surface area of 199.04 m2 g1, it shows a selective adsorption of CO2 over CH4. ’ INTRODUCTION Metalorganic frameworks (MOFs) or porous coordination networks (PCNs) have attracted much attention because of their intriguing structural architectures and topology,1 as well as their potential applications in many fields such as gas storage,2 gas separation,3 and drug delivery.4 These materials usually have a threedimensional (3D) open framework constructed from the combination of multidentate organic ligands with metal ions or clusters also known as secondary building units (SBUs). The approach of utilizing SBUs developed by Yaghi et al.5 has been proven to be a powerful strategy in designing functional MOFs. Inorganic building blocks, such as μ4-oxotetrametal basic carboxylate SBUs ([M4O(CO2)6]), are observed in several famous MOFs, including MOF-56 and MOF-177,7 μ3-oxotrimetal basic carboxylate SBUs ([M3O(CO2)6]) seen in MIL-1018 and other MOFs,9 and dimetal-paddle-wheel SBUs ([M2(CO)4]).10 Selecting the proper metal ions and ligands, one expects to synthesize the prospective SBUs and sequentially design and synthesize the prospective MOFs. However, some metal ions such as Zn(II) can form multiple possible SBUs with the same ligand; thus, it is difficult to predict both the SBUs and the structures of its MOFs. r 2011 American Chemical Society The formation of MOFs is highly influenced by various factors, such as the molar ratio of reactant reagents, solvent used, pH value of the solution, and the selection of a secondary ligand.11 In these factors, the secondary ligand plays a crucial role in extending and reconstructing the structure. On the other hand, 4,40 -bipyridyl (4,40 -bpy) is frequently introduced as a secondary ligand to extend two-dimensional (2D) sheets into threedimensional networks by displacing coordinated solvent molecules through the “pillar-and-layer” method.12,13 This kind of method has been proved to be a quite useful strategy. Additionally, 4,40 -bpy can also take part in channel modification to stabilize the structure and conveniently arrange the surface features of the channel in some MOFs.14 Gas adsorption selectivity is an important property of MOFs which has potential applications in gas separation and purification.3 Gas adsorption selectivity is determined not only by the pore size and shape, but also by the channel surface feature Received: August 14, 2011 Revised: October 23, 2011 Published: November 04, 2011 281 dx.doi.org/10.1021/cg201059d | Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE of MOFs. One effective way to increase the gas selectivity of MOFs is the modification of the inner channel, by changing the surface polarity and the acidbase property.15 Recent research has shown that ionic MOFs have a good behavior in selectively adsorbing high quadrupole moment molecules (for example CO2) through the electric field in the pores of MOFs.16 In previous works, our group successfully synthesized a 3D structural complex, PCN-13, and investigated its gas adsorption properties.9a As a continuing effort of our systematic investigation, we report herein the syntheses, crystal structures, and gas adsorption of four related MOFs, PCN-131, PCN-132, PCN1310 , and PCN-1320 . The effects of mole ratios of metal ion and ligand on the formation of SBU, as well as the function of the secondary ligand for extending and modifying the structures of these MOFs, are established. for 2 days, and then cooled to room temperature. Many yellow block crystals (PCN-1310 ) and a few colorless block crystals (PCN-1320 ) were obtained with a yield of 46% and 18% based on Zn, respectively. The two compounds were separated manually. FT-IR (cm1) for PCN-1310 : 3388 m, 3061 m, 2786w, 1617s, 1431w, 815s, 777s, 738w, 674s, 643s, 612s, 581s. FT-IR (cm1) for PCN-1320 : 3389 m, 3060 m, 2788w, 1618s, 1434w, 815s, 778s, 745w, 673s, 644s, 613s, 582s. X-ray Crystallography. Single crystal X-ray data were collected on an Apex-II diffractometer equipped with a low-temperature device. Single crystals were picked directly from the mother liquor, attached to a glass loop, and transferred to a cold stream of liquid nitrogen (163 °C) for data collection. Raw data collection and refinement was carried out using SMART. Data reduction was performed using SAINT and corrected for Lorentz and polarization effects.18 Adsorption corrections were applied using the SADABS routine. The structure was solved by direct methods and refined by full-matrix least-squares on F2 with anisotropic displacement using the SHELXTL software package.19 Nonhydrogen atoms (except some in coordinated solvents) were refined with anisotropic displacement parameters during the final cycles. Hydrogen atoms on carbon were calculated in ideal positions with isotropic displacement parameters. In PCN-1310 and PCN-1320 , free solvent molecules were highly disordered, and attempts to locate and refine the solvent peaks were unsuccessful. The diffused electron densities resulting from the these residual solvent molecules were removed from the data set using the SQUEEZE routine of PLATON and further refined using the data generated.20 The contents of the solvent region are not represented in the unit cell contents in crystal data. Attempts to determine the final formula of such compounds from the SQUEEZE results combined with elemental analysis and TGA data were not successful because the volatility of the crystallization solvents during measurements prevented accurate data from being obtained. Crystallographic data and experimental details for structural analyses are summarized in Table 1. The selected bond lengths and angles of all complexes are listed in Table S1 of the Supporting Information. ’ EXPERIMENTAL SECTION Materials and General Methods. Commercially available reagents were used as received without further purification. H2adc was synthesized according to a literature procedure.17 Elemental analyses (C, H, and N) were obtained by Canadian Microanalytical Service Ltd. 1 H NMR data were collected on a Mercury 300 spectrometer. FT-IR data were recorded on an IRAffinity-1 instrument. TGA data were obtained on a TGA-50 (Shimadzu) thermogravimetric analyzer with a heating rate of 2 °C min1 under N2 atmosphere. The powder X-ray diffraction patterns (PXRD) were recorded on a Bruker D8-Focus BraggBrentano X-ray powder diffractometer equipped with a Cu sealed tube (λ = 1.541 78 Å) at a scan rate of 0.2 s deg1. Simulation of the PXRD spectrum was carried out by the single-crystal data and diffraction-crystal module of the Mercury program available free of charge via Internet at http://www.iucr.org. ASAP 2020 surface area analyzer was used to measure gas adsorption. Syntheses of Complexes. {[Zn3O(H2O)3(adc)3] 3 2(C2H6NH2) 3 2(DMF) 3 3(H2O)}n (PCN-131). PCN-131 was prepared by the solvothermal reaction. N,N-Dimethylformamide (DMF, 1.5 mL) solution containing anthrancene-9,10-dicarboxylic acid (H2adc) (26.2 mg, 0.1 mmol) was mixed thoroughly with DMF (1.5 mL) solution containing Zn(NO3)2 3 6H2O (59.4 mg, 0.2 mmol), and then five drops of HBF4 were added. The mixture was sealed in a Pyrex tube, heated at 120 °C for 1 week, and then cooled to room temperature. The light-yellow block crystals were obtained with a yield of 56% based on Zn. FT-IR (cm1): 3273 m, 2920 m, 2779 m, 1609s, 1428s, 1381w, 1318s, 1280 m, 1091s, 815s, 777 m, 683s, 604s, 581s. Anal. Calcd for C60.5H73.5Zn3N4.5O25.5: C, 50.95; H, 4.87; N, 4.10. Found: C, 51.63; H, 4.78; N, 4.15. {[Zn2(DMA)2(adc)2] 3 2(DMA)}n (PCN-132). Complex PCN-132 was prepared by the solvothermal reaction. An N,N-dimethylacetamide (DMA, 1.5 mL) solution containing H2adc (26.6 mg, 0.1 mmol) was mixed thoroughly with a DMA (1.5 mL) solution containing Zn(NO3)2 3 6H2O (59.4 mg, 0.2 mmol). The mixture was sealed in a Pyrex tube, heated at 60 °C for 3 days, and then cooled to room temperature. Colorless block crystals were obtained with a yield of 32% based on Zn. FT-IR (cm1): 3278 m, 2921 m, 2781 m, 1607s, 1427s, 1381w, 1319s, 1282 m, 1091s, 816s, 778 m, 683s, 606s, 582s. Anal. Calcd for C48H52Zn2N4O12: C, 57.21; H, 5.20; N, 5.56. Found: C, 57.34; H, 5.18; N, 5.53. {[Zn3O(DMF)(adc)3(4,40 -bpy)] 3 2(C2H6NH2) 3 S}n (PCN-1310 ) and {[Zn(adc)(4,40 -bpy)0.5] 3 S}n (PCN-1320 ) (S = unassigned solvent molecule). By employing bpy as a secondary ligand, 3D metalorganic frameworks of PCN-1310 and PCN-1320 were obtained as a mixture. An N,N-dimethylformamide (DMF, 1.5 mL) solution containing H2adc (26.2 mg, 0.1 mmol) was mixed thoroughly with a DMF (1.5 mL) solution containing Zn(NO3)2 3 6H2O (59.4 mg, 0.2 mmol). 4,40 -bpy (15.6 mg, 0.1 mmol) and three drops of HBF4 were added to this solution to give an acid solution. The mixture was sealed in a Pyrex tube, heated at 120 °C ’ RESULTS AND DISCUSSION Syntheses and General Characterizations. Besides metal ions and ligands, the formation of MOFs is highly influenced by various factors, such as solvent used, pH value of solvent, ratio of reactants, reaction time, temperature, and so on.2125 In our case, we try to evaluate the most significant factors that drive the formation of three primary building units, μ4-oxo-tetrazinc basic carboxylate, μ3-oxo-trizinc basic carboxylate, and dizinc-paddlewheel carboxylate SBU. In the three SBUs, the ratios of metal and carboxylate ligand are 2:3, 1:2, and 1:2. In terms of a dicarboxylate ligand, such as adc2‑ herein (the mole ratios of metal and ligand in complexes are 4:3, 1:1, and 1:1), we can suppose that the ratio of metal and ligand may be the key factor to control the formation of different SBUs. In a previous report, a Zn-MOF named as PCN-139a was constructed with ligand adc2‑. In PCN13, a distorted Zn4O(COO)6 cluster as SBU was observed. Although this SBU is different from the regular μ4-oxo-tetrazinc basic carboxylate SBU observed in one of IRMOF series,26 it still has the same ratio of metal and ligand, 4:3. The unusually distorted SBU implies the possibility to get some new forms of Zn clusters with this ligand if the reaction condition changes. On the basis of the above assumption, we performed a systematic experiment in the syntheses of Zn(II)adc2‑ MOFs only by decreasing the mole ratio of metal salt and ligand from 5:1 to 1:1. Two new MOFs, PCN-131 and PCN-132, were obtained. The details are shown in the Supporting Information (Table S2 and Figures S1 and S2). As shown in Figure S1, when the mole ratio 282 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE Table 1. Crystal Data and Data Collection Parameters for PCN-131, PCN-132, PCN-1310 , and PCN-1320 PCN-131 PCN-132 PCN-1310 PCN-1320 formula C48H30Zn3O16 C48H52Zn2N4O12 C65H55Zn3N5O14 C21H12ZnNO5 formula weight 1058.83 1007.68 1326.25 423.69 crystal system trigonal monoclinic monoclinic tetragonal space group P31c P21/n P21/n I4/mcm a, Å 15.58(3) 15.28(11) 15.81 15.44(7) b, Å 15.58(3) 19.70(14) 26.42 15.44(7) c, Å 16.52(3) 15.59(11) 16.43 28.03(13) a, deg b, deg 90 90 90 90 90 90 90 90 g, deg 120 90 90 90 V, Å3 3472.0(12) 4692.1 6870.0 6680.0 Z 2 4 4 8 D, g/cm3 1.013 1.426 1.283 0.842 μ, mm1 1.076 1.089 1.102 0.752 independent reflections 2265 8693 11168 2451 Rint R [I/σ(I) > 2] 0.0862 0.0421 0.0696 0.0838 0 0.0635 0.0361 0.0614 Rw [I/σ(I) > 2] 0.1195 0.2162 0.1883 0.2529 goodness-of-fit on F2 1.063 1.050 0.970 1.114 no. of reflection used 2265 8693 11168 2451 no. of parameters refined 103 607 755 77 ΔFmax, e Å3 1.127 4.034 1.458 0.873 ΔFmin, e Å3 0.337 2.023 0.755 0.649 of metal salt and ligand is above 4:1, the PXRD patterns of the productions match well the simulated pattern (from single crystal data) of PCN-13. When the ratio reaches 3:1, in PXRD some new peaks are observed, which indicates a new compound (PCN-132), except PCN-13 starts to form in this condition. When the ratio reduced to 2:1, besides the above two compounds, a new compound (PCN-131) can also be obtained. However, when the ratio is less than 2:1, other unassigned new phases are formed. Because PCN-13, PCN-131, and PCN-132 were simultaneity produced at the same reaction conditions, additional experiments were carried out for clarifying the particular synthetic conditions of the three compounds. In this case, the mole ratio of metal/ligand is kept at 2:1 and just changes the acidity of the solvent system. The results showed that PCN-131 is the only product obtained in acid condition (by adding 48% HBF4 in water). Under low acidity conditions, the crystal size formed is too tiny to determine its structure by a single-crystal X-ray crystallographic study (the PXRD results showed that the product is still PCN-131), while in high acidity the crystal quality is very good. The results were confirmed by the PXRD patterns shown in Figure S2 (Supporting Information). The PXRD patterns show all samples have a slightly front shift of the peaks after 15° for 2θ that is probably due to the unstableness of PCN131 without solvent. It is interesting that when two drops of HBF4 acid were added to the system, some new peaks can be observed in the PXRD pattern (green) and the new shape crystals are found in the system. Those new shape crystals were manually picked up and their unit cell parameters were checked out several times by the single-crystal diffraction. The results show that they are all PCN-131. The new shape crystal is just a little bit of a twin crystal to the old one, which may cause the differences shown in PXRD patterns. However, pure phase of PCN-132 was found at the temperature of 60 °C without any HBF4 acid added. In order to extend layered PCN-132 into 3D networks, bpy acting as a secondary ligand was introduced in the synthesis process using the “layer and pillar” method. However, two new compounds, PCN-1310 and PCN-1320 , were found in the same reaction system. Pure PCN-1310 can be obtained under optimized conditions of metal salt mole ratio (6:5:3) of H2adc and 4,40 -bpy. Unfortunately, we could not get a pure phase of PCN-1320 either by changing the pH value of the solvent or by using different solvent systems or even by modifying the ratios of reagent. In the IR spectra of all complexes, the peaks at 29212787 cm1 belong to the CH3 stretching of solvent molecules. The Deacon Philips rule is helpful to determine the coordination mode between carboxylate groups and center metal ions, by calculating the frequency separation (Δν) between the asymmetric (νas) and symmetric stretching (νs) modes of the carboxylate unit.27 The Δν for PCN-131 provides an indication of the bridging coordination mode [Δν = 181 cm1 < 200 cm1, νas(COO) = 1609 cm1, νs(COO) = 1428 cm1]. Similar characteristics are also observed in PCN-132 [Δν = 180 cm1 < 200 cm1, νas(COO) = 1607 cm1, νs(COO) = 1427 cm1), PCN-1310 (Δν = 186 cm1 < 200 cm1, νas(COO) = 1617 cm1, νs(COO) = 1431 cm1] and PCN-1320 [Δν = 184 cm1 < 200 cm1, νas(COO) = 1618 cm1, νs(COO) = 1434 cm1]. For PCN-131, TGA studies show that a mass loss of 8.36% corresponds to the leaving of uncoordinated and coordinated water molecules (calcd 8.01%) in a temperature range of 6394 °C, while a mass loss of 13.17% corresponds to the leaving of uncoordinated DMF molecules (calcd 13.49%) in a temperature range of 157241 °C. 283 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE Figure 2. (a) SBU structure of PCN-132. (b) The 2D square-grid net structure of PCN-132. (c) The packing style of PCN-132. (d) The hydrogen bonds between adjacent layers. direction (Figure 1b). PLATON calculations indicate that the effective volume for solvent molecules is 1757.4 Å3 per unit cell, which is 50.6% of the crystal volume.28 {[Zn2(DMA)2(adc)2] 3 2(DMA)}n (PCN-132). PCN-132 crystallized in monoclinic space groups P21/n with two Zn ions, two adc ligands, two coordinated DMA solvent molecules, and two free DMA molecules in the asymmetric unit. Each Zn2+ ion is coordinated by five O atoms with four from the adc ligands and one from the coordinated DMA solvent molecule. Four carboxylate groups bridge two Zn2+ to form a distorted Zn2(CO2)4 paddle-wheel SBU as a square-planar four-connected node (Figure 2a). The distance of Zn 3 3 3 Zn in the paddle-wheel cluster is 2.979 Å, which is similar to those found in another dizinc paddle-wheel SBUs.29 The bond distance of ZnO (solvent) is 1.982 Å and ZnO (adc) bond distances range from 2.039 to 2.059 Å. The ligand adc bridges dizinc paddle-wheel SBUs to form a two-dimensional sheet (Figure 2b). There exist three kinds of CH 3 3 3 O hydrogen bonds between adjacent layers. The first one is formed between the methyl H atoms of the coordinated DMA solvent molecules and the carboxylic O atoms of ligands from adjacent layers. The second one is formed between H atoms of the anthrancene rings and O atoms of the free DMA solvent molecules. And the last one is formed between the methyl H atoms of free DMA solvent molecules and the carboxylic O atoms of ligands. These hydrogen bonds link the complex with an “ABAB” packing fashion, resulting in a nonporous structure (Figure 2c,d). The hydrogen-bond parameters are presented in Table S3 (Supporting Information). {[Zn(adc)(4,40 -bpy)0.5] 3 S}n (PCN-1320 ). PCN-1320 crystallized in tetragonal space group I4/mcm with one-half of a Zn2+ ion, one adc ligand, and one-quarter of a 4,40 -bpy in the asymmetric unit. The zinc ion adopts a similar coordination geometry to that of PCN-132 with 4,40 -bpy replacing the axial Figure 1. (a) SBU structure of PCN-131 and (b) 3D structure of PCN131 with 1D channels. This compound starts to decompose at ca. 310 °C (see Figure S3, Supporting Information). For PCN-132, TGA studies show that a mass loss of 17.18% corresponds to the loss of uncoordinated DMA molecules (calcd 17.27%) in a temperature range of 84151 °C, and the other mass loss of 17.79% corresponds to the leaving of coordinated DMA molecules (calcd 17.27%) in a temperature range of 262343 °C. The complex starts to decompose at ca. 350 °C (see Figure S4, Supporting Information). Crystal Structures. {[Zn3O(H2O)3(adc)3] 3 2(C2H6NH) 3 2 (DMF) 3 3(H2O)}n (PCN-131). X-ray single crystal diffraction analyses revealed that PCN-131 crystallizes in trigonal space group P31c. In the asymmetric unit of PCN-131, there are one-sixth of a μ3-O atom, one-half of a Zn2+ ion, a H2O molecule, the adc2‑ ligand and one third of C2H6NH2+. Uncoordinated C2H6NH2+ part is an NH2(CH3)2+ cation (dimethylammonium) which is formed by the decomposed DMF molecules during heated. For the whole framework structure, PCN-131 is built on a μ3-oxo-trizinc basic carboxylate SBU [Zn3O(COO)6] (Figure 1a) and the adc ligand, with a Znμ3O distance of 2.003 Å and adjacent Zn 3 3 3 Zn distance of 3.470 Å, which is isorecticular to PCN-19 (Ni-MOF).9c In this SBU, three Zn2+ ions and a μ3-O atom are on the same plane, forming a sixconnected node. Each pair of adjacent Zn2+ ions are bridged by two carboxylate groups from two different adc ligands, and the coordination geometry of each Zn2+ ion is octahedral with the ZnO (μ3-O) at a distance of 2.110 Å and ZnO (adc) bond distances ranging from 2.071 to 2.077 Å. Each trizinc SBU connects to six adc ligands and each adc ligand binds two SBUs to enclose a honeycomb one-dimensional channel along the c axis 284 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE Figure 3. (a) SBU structure of PCN-1320 , and (b) 3D structure of PCN-1320 . direction coordinated solvent molecules to form an octahedral sixconnected node instead of a square-planar four-connected node (Figure 3a). It is interesting that the attendance of 4,40 -bpy relieves the crowding among anthracene rings and breaks the weak intermolecule interactions, forming a typical dizinc paddle-wheel SBU with a ZnO (adc) bond distance of 2.046 Å, a ZnO (bpy) bond distance of 2.022 Å, and a Zn 3 3 3 Zn distance of 2.925 Å, which is shorter than that of PCN-132. With the linkage of 4,40 bpy PCN-1320 adopts a pillaredlayered structure with the formula of {[Zn(adc)(4,40 -bpy)0.5] 3 S}n (S = unknowable solvent molecule) (Figure 3b). However, 4,40 -bpy is disordered in this structure due to its rotation along the symmetry axis. Compared with PCN-132, the “layer” structure packs in an “AA” fashion, resulting in a “pillar” effect in PCN-1320 . Unfortunately, there are no pores in c direction because of the bulkiness of the anthracene rings, and finally only 2D channels form in PCN-1320 . PLATON calculations indicate that the effective volume for solvent molecules is 3575.3 Å3 per unit cell, which is 53.5% of the crystal volume.28 Figure 4. (a) SBU structure of PCN-1310 . (b) The structure of 1D channel and connection mode of decrated bpy. (c) The 3D packing style structure of PCN-1310 . {[Zn3O(DMF)(adc)3(4,40 -bpy)] 3 2(C2H6NH2) 3 S}n (PCN-1310 ). PCN-1310 crystallizes in monoclinic space group P21/n with three Zn2+ ions, one μ3-O atom, one 4,40 -bpy three adc ligands, one coordinated DMF molecule, and two C2H6NH2+ cations [C2H6NH2+ is an NH2(CH3)2+ cation (dimethylammonium) which is formed by the decomposed DMF molecules during heated.] in the crystallographically asymmetric unit. It is one of a 285 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE few cases of using 4,40 -bpy to “arrange” a channel in a MOF.14 The Zn(II) adopts a similar coordination geometry to that of PCN-131, with bpy replacing two coordinated water molecules, breaking the symmetry in the μ3-oxo-trizinc carboxylate SBU to form an eight-connected node instead of six-connected node (Figure 4a). In PCN-1310 , the honeycomb framework maintains the linking relationship while it exhibits significant expansion along the diagonal of two perpendicular directions a and b, as evidenced by the large variations in channel size parameters, from 1.66 1.66 1.66 nm to 1.74 1.59 1.56 nm (Figure 4b). This is also the reason why only two molecules of solvent can be replaced. The third one is just sitting along the expansion direction out of the reach of bpy. The “arrangement” of 4,40 -bpy not only changes the shape of the channel from honeycomb to rectanglular channel but also increases the stability of the whole framework (Figures 4c and 5). PLATON calculations indicate that the effective volume for solvent molecules is 2712.0 Å3 per unit cell, which is 39.5% of the crystal volume.28 Gas Adsorption. To characterize the porosity of PCN-131 and PCN-1310 , the samples were first soaked in MeOH for 3 days and then in CH2Cl2 for 3 days. However, the different stabilities of these compounds do not allow using the same activation conditions. Under high vacuum, PCN-131 has already been decomposed only by 3 h at room temperature, while the structure of PCN-1310 has remained stable even after heating to 80 °C for 10 h. This means that PCN-131 is unstable without the support of solvent molecules, and conversely, PCN-1310 is stable. It is also confirmed that the arrangement of 4,40 -bpy inside the channel can effectively increase the stability of the frameworks. Although PCN-131 is isorecticular to PCN-19, which is mentioned above, two MOFs have totally different stabilities after activation. The possible reason is that PCN-19 is a nickle-based MOF while PCN-131 is a zinc-based MOF, and the differences between the central metal ions cause different stabilities of their MOFs. Adsorption isotherms for N2, H2, O2, and Ar at 77 K and CO2 and CH4 at 195 and 273 K were measured. No adsorption was observed for PCN-131, which means that the framework collapsed after activation, as confirmed by PXRD pattern (Figure S5, Supporting Information). The N2 adsorption of PCN-1310 represents a typical type I isotherm (Figure 6). Its BET surface area is 442.20 m2 g1(Langmuir surface area is 496.85 m2 g1), and the total pore volume is 0.177 cm3 g1. The PXRD pattern after gas adsorption of PCN-1310 is still matches well with the simulated pattern, showing that the framework structure of this material is still stable (Figure S6, Supporting Information). Figure 5. The channel structures of PCN-131 and PCN-1310 . Figure 6. N2 adsorption isotherms of PCN-131 and PCN-1310 at 77 K (solid symbols stand for adsorption and open ones for desorption. Figure 7. (a) H2 adsorption isotherm of PCN-1310 measured at 77 K and (b) N2, O2 and Ar adsorption isotherm of PCN-1310 measured at 77 K. 286 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE Figure 8. (a) CO2 and CH4 adsorption isotherm of PCN-1310 measured at 195 K and (b) CO2 and CH4 adsorption isotherm of PCN-1310 measured at 273 K. The H2 sorption isotherm was measured at 77 K; as shown in Figure 7a, PCN-1310 can absorb 0.84 wt % (excess) without any hysteresis at 77 K and 800 Torr. Although the presence of bpy reduces the porous volume, it effectively enhances the stability of 1D channel compound, and its hydrogen uptake is still comparable to that of the similar complex (PCN-199c) without bpy. The O2 and Ar uptake was also carried out at 77 K (Figure 7b). In addition, PCN-1310 exhibits a selective gas adsorption to CO2 over CH4 both at 195 and 273 K, as shown in Figure 8, which is similar to several reported MOFs.16,30 ’ CONCLUSIONS Two porous coordination networks (PCNs), PCN-131 and PCN-132, were synthesized by solvothermal reactions of Zn(II) nitrate with anthrancene-9,10-dicarboxylic acid (H2adc) through tuning the mole ratio of mental salt and ligand from 5:1 to 1:1. The studies still show that PCN-131 is the only product under acid environment. By introducing 4,40 -bpy acting as secondary ligand, into reaction system, PCN-1310 and PCN-1320 were obtained. Pure PCN-1310 is the primary product and can be obtained with a mole ratio of metal salt, H2adcd, and 4,40 -bpy of 6:5:3. Through the smart synthetic design, the 1D honeycomb channel of PCN-131 was “rearranged” and modified by use of 4,40 -bpy, resulting in PCN-1310 , which is stable for gas adsorption. By use of 4,40 -bpy as secondary ligand, the 2D sheet of PCN-132 is pillared to form a 3D framework, PCN-1320 . In summary, judiciously tuning metalligand mole ratio could be an effective way to form different SBUs so as to affect the structural formation of complexes, and bpy as a good candidate of secondary ligand not only can extend structural dimension of complexes through the pillaredlayered method but also can modify the structures and enhance the stability of frameworks. ’ AUTHOR INFORMATION Corresponding Author *Y.-B.X.: fax, +86-10-67391983; tel, +86-10-67392130; e-mail: xieyabo@bjut.edu.cn (Y.-B.X.). H.C.Z.: e-mail: zhou@mail.chem. tamu.edu (H.-C.Z.). ’ ACKNOWLEDGMENT This work was supported by National Natural Science Foundation of China (No.21075114, 21076003, 20851002), the National Basic Research Program of China (973 Program 2009CB930200), the Special Environmental Protection Fund for Public Welfare project (201009015), the Funding Project for Academic Human Resources Development in Institutions of Higher Learning under the jurisdiction of the Beijing Municipality (PHR 201107104), the Ninth Technology Fund for Postgraduates of Beijing University of Technology (ykj-2011-5406), and U.S. Department of Energy (ARPA-E: AR0000073 and EFRC: DE-SC0001015). ’ REFERENCES (1) (a) Yaghi, O. M.; O’Keeffe, M.; Ockwig, N. W.; Chae, H. K.; Eddaoudi, M.; Kim, J. Nature 2003, 423, 705. (b) Huang, X.-C.; Lin, Y.-Y.; Zhang, J.-P.; Chen, X.-M. Angew. Chem. Int. Ed. 2006, 45, 1557. (c) Natarajan, S.; Mahata, P. Chem. Soc. Rev. 2009, 38, 2304. (d) Li, J.-R.; Timmons, D. J.; Zhou, H.-C. J. Am. Chem. Soc. 2009, 131, 6368. (e) Tranchemontagne, D. J.; Mendoza-Cortes, J. L.; O’Keeffe, M.; Yaghi, O. M. Chem. Soc. Rev. 2009, 38, 1257. (f) Deng, H.; Doonan, C. J.; Furukawa, H.; Ferreira, R. B.; Towne, J.; Knobler, C. B.; Wang, B.; Yaghi, O. M. Science 2010, 327, 846. (g) Zheng, S.-T.; Zuo, F.; Wu, T.; Irfanoglu, B.; Chou, C.; Nieto, R. A.; Feng, P.; Bu, X. Angew. Chem. Int. Ed. 2011, 50, 1849. (h) Meek, S. T.; Greathouse, J. A.; Allendorf, M. D. Adv. Mater. 2011, 23, 249. (2) (a) Eddaoudi, M.; Kim, J.; Rosi, N.; Vodak, D.; Wachter, J.; O’Keeffe, M.; Yaghi, O. M. Science 2002, 295, 469. (b) Rosi, N. L.; Eckert, J.; Eddaoudi, M.; Vodak, D. T.; Kim, J.; O’Keeffe, M.; Yaghi, O. M. Science 2003, 300, 1127. (c) Murray, L. J.; Dinca, M.; Long, J. R. Chem. Soc. Rev. 2009, 38, 1294. (d) Huang, S.-H.; Lin, C.-H.; Wu, W.-C.; Wang, S.-L. Angew. Chem. Int. Ed. 2009, 48, 6124. (e) Wang, Z.; Tanabe, K. K.; Cohen, S. M. Chem.—Eur. J. 2010, 16, 212. (f) Guo, Z.; Wu, H.; Srinivas, G.; Zhou, Y.; Xiang, S.; Chen, Z.; Yang, Y.; Zhou, W.; O’Keeffe, M.; Chen, B. Angew. Chem. Int. Ed. 2011, 50, 3178. (3) (a) Pan, L.; Parker, B.; Huang, X. Y.; Olson, D. H.; Lee, J. Y.; Li, J. J. Am. Chem. Soc. 2006, 128, 4180. (b) Ferey, G. Chem. Soc. Rev. 2008, 37, 191. (c) Li, J. R.; Kuppler, R. J.; Zhou, H. C. Chem. Soc. Rev. 2009, 38, 1477. (d) Li, Y. S.; Liang, F. Y.; Bux, H.; Feldhoff, A.; Yang, W. S.; ’ ASSOCIATED CONTENT bS Supporting Information. PXRD patterns of complexes prepared through changing the ratio of metal and ligand, PXRD patterns of PCN-131 obtained under different acidity in the synthesis, TGA results of PCN-131 and PCN-132, PXRD results of PCN-131 and PCN-1310 (after the gas adsorption), and complete crystallographic details (CIF file). This material is available free of charge via the Internet at http://pubs.acs.org. 287 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288 Crystal Growth & Design ARTICLE (27) Deacon, G. B.; Phillips., R. Coord. Chem. Rev. 1980, 33, 227. (28) Spek, A. L. PLATON, A Multipurpose Crystallographic Tool; Utrecht University: Utrecht, The Netherlands, 2001. (29) (a) Chun, H.; Moon, J. Inorg. Chem. 2007, 46, 4371. (b) Jiang, H.-L.; Liu, B.; Xu, Q. Cryst. Growth Des 2010, 10, 806. (30) (a) Kondo, A; Chinen, A.; Kajiro, H.; Nakagawa, T.; Kato, K.; Takata, M.; Hattori, Y.; Okino, F.; Ohba, T.; Kaneko, K.; Kanoh, H. Chem.—Eur. J. 2009, 15, 7549. (b) Botas, J. A.; Calleja, G.; SanchezSanchez, M.; Orcajo, M. G. Langmuir 2010, 26, 5300. (c) Babarao, R.; Eddaoudi, M.; Jiang, J. W. Langmuir 2010, 26, 11196. Caro, J. Angew. Chem., Int. Ed. 2010, 49, 548. (e) Li, J.-R.; Ma, Y.; McCarthy, M. C.; Sculley, J.; Yu, J.; Jeong, H.-K.; Balbuena, P. B.; Zhou, H.-C. Coord. Chem. Rev. 2011, 255, 1791. (f) Li, J.-R.; Tao, Y.; Yu, Q.; Bu, X.-H.; Sakamoto, H.; Kitagawa, S. Chem.—Eur. J. 2008, 14, 2771. (4) (a) Horcajada, P.; Serre, C.; Vallet-Regí, M.; Sebban, M.; Taulelle, F.; Ferey, G. Angew. Chem., Int. Ed. 2006, 45, 5974. (b) Horcajada, P.; Serre, C.; Maurin, G.; Ramsahye, N. A.; Balas, F.; Vallet-Regí, M.; Sebban, M.; Taulelle, F.; Ferey, G. J. Am. Chem. Soc. 2008, 130, 6774. (c) Horcajada, P.; Chalati, T.; Serre, C.; Gillet, B.; Sebrie, C.; Baati, T.; Eubank, J. F.; Heurtaux, D.; Clayette, P.; Kreuz, C.; Chang, J. S.; Hwang, Y. K.; Marsaud, V.; Bories, P. N.; Cynober, L. Nat. Mater. 2010, 9, 172. (5) Kim, J.; Chen, B.; Reineke, T. M.; Li, H.; Eddaoudi, M.; Moler, D. B.; O’Keeffe, M.; Yaghi, O. M. J. Am. Chem. Soc. 2001, 123, 8239. (6) Li, H.; Eddaoudi, M.; O’Keeffe, M.; Yaghi, M. O. Nature 1999, 402, 276. (7) Chae, H. K.; Siberio-Perez, D. Y.; Kim, J.; Go, Y. B.; Eddaoudi, M.; Matzger, A. J.; O’Keeffe, M.; Yaghi, O. M. Nature 2004, 427, 523. (8) Ferey, G.; Mellot-Draznieks, C.; Serre, C.; Millang, J. D.; Surble, S.; Margiolaki, I. Science 2005, 309, 2040. (9) (a) Ma, S.; Wang, X. S.; Manis, E. S.; Collier, C. D.; Zhou, H. C. Inorg. Chem. 2007, 46, 3432. (b) Jia, J.; Lin, X.; Wilson, C.; Blake, A. J.; Champness, N. R.; Hubberstey, P.; Walker, G.; Cussen, E. J.; Schr€oder, M. Chem. Commun. 2007, 840. (c) Ma, S.; Simmons, J. M.; Yuan, D.; Li, J.; Weng, W.; Liu, D. J.; Zhou, H. C. Chem. Commun. 2009, 4049. (10) (a) Dai, F.; He, H.; Gao, D.; Ye, F.; Qiu, X.; Sun, D. CrystEngComm 2009, 11, 2516. (b) Maniam, P.; Stock, N. Inorg. Chem. 2011, 50, 5085. (11) (a) Wang, J.; Hu, S.; Tong, M.-L. Eur. J. Inorg. Chem. 2006, 10, 2069. (b) Ma, L.; Lin, W. J. Am. Chem. Soc. 2008, 130, 13834. (c) Su, Z.; Fan, J.; Okamura, T.; Sun, W.-Y.; Ueyama, N. Cryst. Growth Des. 2010, 10, 3515. (d) Liu, J.-Q.; Wang, Y.-Y.; Zhang, Y.-N.; Liu, P.; Shi, Q.-Z.; Batten, R., St. Eur. J. Inorg. Chem. 2009, 1, 147. (12) (a) Maji, T. K.; Uemura, K.; Chang, H.-C.; Matsuda, R.; Kitagawa, S. Angew. Chem. Int. Ed. 2004, 43, 3269. (b) Pichon, A.; Fierro, C. M.; Nieuwenhuyzen, M.; James, S. L. CrystEngComm 2007, 9, 449. (13) (a) Bo, Q. B.; Sun, G. X.; Geng, D. L. Inorg. Chem. 2010, 49, 561. (b) Seo, J.; Matsude, R.; Sakamoto, H.; Bonneau, C.; Kitagawa, S. J. Am. Chem. Soc. 2009, 131, 12792. (14) (a) Tian, H; Jia, Q. X.; Gao, E. Q.; Wang, Q. L Chem. Commun. 2010, 46, 5349. (b) Park, H. J.; Cheon, Y. E.; Suh, M. P. Chem.—Eur. J. 2010, 16, 11662. (15) (a) Zhang, S.-M.; Chang, Z.; Hu, T.-L.; Bu, X.-H. Inorg. Chem. 2010, 49, 11581. (b) Chen, Z.; Xiang, S.; Arman, H. D.; Li, P.; Zhao, D.; Chen, B. Eur. J. Inorg. Chem. 2011, 14, 2227. (16) (a) Babarao, R.; Jiang, J.; Sandler, S. I. Langmuir 2009, 25, 5239. (b) Kondo, A.; Chinen, A.; Kajiro, H.; Nakagawa, T.; Kato, K.; Takata, M.; Hattori, Y.; Okino, F.; Ohba, T.; Kaneko, K.; Kanoh, Hi. Chem.— Eur. J. 2009, 15, 7549. (17) Jones, S.; Atherton, J. C. C.; Elsegood, M. R. J.; Clegg, W. Acta Crystallogr. Sect. C 2000, C56, 881. (18) Bruker-AXS SAINT Software Reference Manual, Bruker: Madison, WI, 1998. (19) Sheldrick, G. M. Acta Crystallogr., Sect. A 2008, 64, 112. (20) Spek, A. L. J. Appl. Crystallogr. 2003, 36, 7. (21) (a) Zhong, R. Q.; Zou, R. Q.; Du, M.; Yamada, T.; Maruta, G.; Takeda, S.; Xu, Q. Dalton Trans. 2008, 2346. (b) Ma, L. F.; Wang, L. Y.; Huo, X. K.; Wang, Y. Y.; Fan, Y. T.; Wang, J. G.; Chen, S. H. Cryst. Growth Des. 2008, 8, 620. (22) Zhang, J. J.; Wojtas, L.; Larsen, R. W.; Eddaoudi, M.; Zaworotko, M. J. J. Am. Chem. Soc. 2009, 131, 17040. (23) Khan, N. A.; Jun, J. W.; Jhung, S. H. Eur. J. Inorg. Chem. 2010, 1043. (24) Zhang, L.; Zhang, J.; Li, Z. J.; Qin, Y.-Y.; Lin, Q.-P.; Yao, Y. G. Chem.—Eur. J. 2009, 15, 989. (25) Urko, G.-C.; Oscar, C.; Javier, C.; Monica, L.; Antonio, L.; Sonia, P.-Y.; Pascual, R.; Daniel, V.-S. Inorg. Chem. 2010, 49, 11346. (26) Hausdorf, S.; Baitalow, F.; Boehle, T.; Rafaja, D.; Mertens, F. O. R. L. J. Am. Chem. Soc. 2010, 132, 10978. 288 dx.doi.org/10.1021/cg201059d |Cryst. Growth Des. 2012, 12, 281–288