English

• 0.   Introduction

  Detecting poisonous chemicals at a very low limit is crucial because leakage or loss of control of those can lead to widespread risks to the environment, even at very low concentrations^[1-3]. Evaluating the poisonous amines, one kind of the most hazardous and wide - spreading chemicals, is of great importance for pollution control. Additionally, there is another instant requirement for detection of amines in our daily life, like control of food quality, and management of some diseases^[4-6]. Various techniques have been developed and applied to detect poisonous amines, including classic gas and liquid chromatography, mass spectrometry, light - emitting sensing, and electrochemical sensing methods. Particularly, light - emitting sensing methods are gaining more attention attributed to their practical sensitivity, simple handling procedures, and rapid response time. Accordingly, most of the sensing methods are based on fluorescence changes due to the high selectivity and sensitivity of fluorescence sensing^[7-8]. Fluorescence quenching is the most common one in those sensing principles of probes, while probes of "turn - on"fluorescence enhancement for sensing of amines are more applicable than those of fluorescence quenching^[9-11]. Therefore, it is still attractive to construct a sensor with a"turn-on"property.

  Recently, metal-organic frameworks (MOFs) have been well - established as sensors owing to their fast, reversible, and recyclable sensing capacity^[12-17]. MOFs materials are superior to other porous materials because of their high/tunable porosity, pore functionality, various pore architectures/compositions, open metal sites, which control the molecular level interaction and selectivity between the framework and probe analytes^[18-20]. There are full of challenges to designing and synthesizing MOFs for distinguishable"turn-on"recognition of amines through interactions between ligand and amines, which can regulate the MOF photoluminescence (PL). Polycarboxylate ligands are good building blocks for the construction of luminescent MOFs networks because they can adopt a variety of coordination modes such as monodentate, chelating - bidentate, bridging-bidentate, and bridging-multidentate patterns^[21-23]. Meanwhile, compared with transition metal ions, alkaline earth metals generally have high and variable coordination numbers and can provide a flexible coordination environment because of their large ion radius, leading to a large number of MOFs with diverse structures^[24-27].

  Herein, we successfully synthesized a luminescent barium metal-organic framework [Ba(dna)(H₂O)₂]_n (1) using a π-conjugated, electron-deficient, carboxyl-functionalized ligand 1, 4, 5, 8-naphthalene tetracarboxylic acid (nta), which was further converted to 1, 8 naphthalic anhydride - 4, 5 - dicarboxylic (H₂dna) after the solvothermal reaction with BaCO₃. This novel Ba - MOF complex with high chemical stability can afford as a"turn - on"sensing probe for aromatic amines at a low detection limit. Based on direct calcination of complex 1, a simple method was further developed to produce micro-crystalline BaCO₃ particles.

  1.   Experimental

  1.1   Materials and methods

  1, 4, 5, 8 - Naphthalene tetracarboxylic acid (98%), BaCO₃, phenylamine, naphthylamine, and 1 - aminopyrene were purchased from J & K. Other reagents such as methanol and ethanol were purchased from Sinopharm Chemical Reagent Co., Ltd. All commercially available agents were of reagent grade and used as received without further purification. C and H analyses were made on a Perkin-Elmer 240C elemental analyzer. IR spectrum was recorded on Nicolet 6700 FT-IR spectrophotometer by using KBr pellet in a range of 4 000 - 400 cm^-1. Thermogravimetric analysis (TGA) was performed with a simultaneous SDT Q600 thermal analyzer under 100.0 mL·min^-1 flowing nitrogen with a heating rate of 20 ℃ ·min^-1 from room temperature to 800 ℃. The luminescent spectra for the samples were recorded at room temperature on CaryEclipse 300 spectrophotometer with a xenon arc lamp as the light source. In the measurements of the emission and excitation spectra, the pass width was 5.0 nm. Powder X - ray diffraction (PXRD) patterns were performed with a Bruker D8 ADVANCE X-ray diffractometer with Cu Kα radiation (λ =0.154 06 nm, U=45 kV, I=40 mA, 2θ =10° - 70°). The micro morphology of the synthesized material were observed by a JEOL JSM 5600LV at 20 kV.

  1.2   Synthesis of [Ba(dna)(H₂O)₂]_n (1)

  The mixture of nta (15.2 mg, 0.05 mmol) and BaCO₃ (7.9 mg, 0.04 mmol) in 4 mL distilled water and 12 mL ethanol was heated for about 20 h in a 25 mL Teflon - lined stainless - steel container at 160 ℃. The mixture was cooled to room temperature, and brown crystal 1 (5.6 mg, 48% yield based on Ba) were obtained by filtration and dried in air. Elements analyses Calcd. for C₁₄H₈BaO₉(%): C, 36.75; H, 1.76. Found: C, 36.72; H, 1.78. FT - IR spectrum (cm^-1): 3 405(bs), 1 776(s), 1 706(s), 1 605(s), 1 590(s), 1 440(m), 1 398 (m), 1 383(m), 1 337(m), 1 226(w), 1 190(w), 1 160(w), 1 128(w), 1 051(m), 1 016(w), 872(m), 828(m), 778(m), 745(w), 596(w).

  1.3   X-ray crystallography

  Data collection for complex 1 (0.33 mm×0.28 mm× 0.25 mm) was performed on a Bruker Smart APEX Ⅱ CCD diffractometer at 296 K by using a graphite monothematic Mo Kα radiation (λ =0.071 073 nm). A total of 9 136 reflections were collected, of which 3 049 (R_int=0.018 4) were independent in a θ range of 2.86°27.53°. The absorption corrections were applied using the SADABS program. Structural solutions were performed by direct methods using the SHELXS - 97 program and the structures were refined by full - matrix least - squares techniques with SHELXL - 97. All non hydrogen atoms were placed in successive difference Fourier syntheses and refined with anisotropic thermal parameters on F². The hydrogen atoms were geometrically generated and refined by a riding mode. The hydrogen atoms were generated geometrically.

  CCDC: 2026609.

  1.4   UV - Vis spectra, luminescence spectra, and detection of aromatic amines

  First, the luminescence emission spectra of 1 and ligand nta on solid states were recorded at room temperature. To determine the absorbance of aromatic amines, the UV - Vis spectra of all the samples were measured in water solution and ultrasonically dispersed before the test. Complex 1 was prepared into 1 mg·mL^-1 water solution in a homogeneous dispersion state using ultrasonic. The tested samples with aromatic amines were got first from the reaction of 1 mL above 1 solution (Calcd. 1 mg) with given amounts of the aqueous solution of amines (all in 0.1 mg·mL^-1) added, and reacted at 50 ℃ for 15 min. Then the solid was centrifuged and washed three times with 5 mL ethanol and 5 mL water separately, finally diluted and dispersed to 1 mL water solution. The samples for UV - Vis test and luminescence test in solution state were transferred 100 µL from as - prepared above solutions and diluted to 2 mL for the test.

  2.   Results and discussion

  2.1   Crystal structure of complex 1

  Single - crystal X - ray structure analysis reveals that complex 1 crystallizes in the triclinic P1 space group and the detailed crystallographic data are exhibited in Table 1. As shown in Fig. 1, the asymmetric unit of 1 consists of one unique Ba(Ⅱ) ion, one unique dna^2- ligand, and two coordinated water molecules. The Ba(Ⅱ) ion has a nine - coordinate configuration, consisting of seven carboxylate oxygen atoms from six different dna^2- ligands and two oxygen donors from two coordinated water molecules, which form a distorted mono-capped square geometry architecture. As listed in Table 2, the Ba—O distances range from 0.261 98(17) to 0.323 07(18) nm, which are similar to those observed in the reported complexes^[24-25]. The O—Ba—O bond angles fall in a range of 42.27(5)°-153.93(6)°.

  Table 1

  

  Table 1.  Crystallographic data of complex 1

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  Parameter	1
  Chemical formula	C14H8BaO9
  Formula weight	457.54
  crystal system	Triclinic
  Space group	P1
  a / nm	0.717 05(6)
  b /nm	0.828 50(7)
  c / nm	1.160 65(10)
  α / (°)	75.836(2)
  β / (°)	84.036(2)
  γ / (°)	87.866(2)
  V / nm3	0.664 88(10)
  Z	2 2
  Dc / (g·cm-3)	0.285
  μ (Mo Kα) / mm-1	3.041
  Unique reflection	3 049
  Observed reflection	2 918
  Rint	0.018 4
  F(000)	440
  R1, wR2 (all data)	0.019 1, 0.051 2
  R1, wR2 [I > 2σ(I)]a, b	0.017 9, 0.050 4
  GOF	1.002
  a R1=∑||Fo|-|Fc||/∑|Fo|; b wR2={∑[w(|Fo|2-|Fc|2)2]/∑[w(|Fo|2)2]}1/2.

  Figure 1

  

  Figure 1.  Coordination geometry of complex 1 drawn at 30% probability displacement ellipsoids

  Hydrogen atoms are omitted for clarity; Symmetry codes: #1: 1-x, -y, 1-z; #2: 1-x, -1-y, 1-z

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  Table 2

  

  Table 2.  Selected bond lengths (nm) and angles (°) for 1

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  Ba1—O1	0.282 21(17)	Ba1—O7	0.282 63(17)	Ba1—O6	0.277 60(17)
  Ba1—O8	0.277 7(2)	Ba1—O2#1	0.261 98(17)	Ba1—O9	0.276 9(2)
  Ba1—O3	0.293 11(19)	Ba1—O7#2	0.302 14(19)	Ba1—O2	0.323 07(18)
  O2#1—Ba1—O9	93.72(7)	O2#1—Ba1—O6	134.20(5)	O9—Ba1—O6	128.94(6)
  O2#1—Ba1—O8	70.04(6)	O9—Ba1—O8	122.37(7)	O6—Ba1—O8	72.61(6)
  O2#1—Ba1—O1	115.36(5)	O9—Ba1—O1	66.34(6)	O6—Ba1—O1	75.86(5)
  O8—Ba1—O1	72.05(6)	O2#1—Ba1—O7	133.24(5)	O9—Ba1—O7	81.78(7)
  O6—Ba1—O7	76.30(5)	O8—Ba1—O7	148.49(6)	O1—Ba1—O7	105.27(5)
  O2#1—Ba1—O3	78.67(6)	O9—Ba1—O3	137.44(7)	O6—Ba1—O3	78.83(6)
  O8—Ba1—O3	94.52(6)	O1—Ba1—O3	153.93(6)	O7—Ba1—O3	74.34(5)
  O2#1—Ba1—O7#2	65.03(5)	O9—Ba1—O7#2	66.92(6)	O6—Ba1—O7#2	140.52(5)
  O8—Ba1—O7#2	134.74(5)	O1—Ba1—O7#2	133.16(5)	O7—Ba1—O7#2	70.60(6)
  O3—Ba1—O7#2	72.07(5)	O2—Ba1—O2#1	73.47(5)	O9—Ba1—O2	62.37(6)
  O6—Ba1—O2	108.96(5)	O8—Ba1—O2	60.00(6)	O1—Ba1—O2	42.27(5)
  O7—Ba1—O2	138.14(5)	O7#2—Ba1—O2	109.99(5)	O3—Ba1—O2	147.22(5)
  Symmetry codes: #1: 1-x, -y, 1-z; #2: 1-x, -1-y, 1-z.

  In 1, ligand nta was deprotonated completely and converted to dna^2- as a μ₅ - bridge linking five Ba (Ⅱ) ions, in which two carboxylate groups adopt two μ₃-η¹∶η² and μ₂ - η²∶η¹ coordination fashions, respectively (Scheme 1). The dihedral angle between the center naphthalene ring and anhydride group (O₃, C13, O4, C14, O5) is 1.4°, indicating these two groups are almost coplanar. The dihedral angles between two carboxylate groups (O1—C11—O2, O6—C12—O7) and center naphthalene rings are 116.7° and 109.9°, respectively. The dihedral angle between two carboxylate groups (O1—C11—O2, O6—C12—O7) is 22.17°. If we consider two coordination models μ₃-η¹∶η² and μ₂-η²∶η¹ as μ¹-η¹∶η⁰ and μ¹-η¹∶η¹ temporarily, dna^2- acts as a μ₃-bridge to link three different Ba(Ⅱ) ions, which takes as three connection node, resulting in a 2D (6, 3) topology (Fig. 2a). Furthermore, the 2D layers are connected by μ₃-η¹∶η² and μ₂-η²∶η¹ carboxylate groups to give rise to 3D network structure as shown in Fig. 2b and Fig. 3. In the MOF lattice, the chromophoric naphthalene moieties are separated by a distance of 0.35 nm showing a strong π-π stacking interaction^[28].

  Scheme 1

  

  Scheme 1.  ORTEP view of coordination model of dna^2-

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  Figure 2

  

  Figure 2.  Infinite 2D structure in complex 1

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  Figure 3

  

  Figure 3.  Crystal packing diagram for 1

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  2.2   IR spectra of complex 1 and ligand nta

  As shown in the ligand nta structure, the anhydride group doesn't exist. This anhydride group was generated from nta after solvothermal reaction with BaCO₃. We proposed a possible reaction mechanism as outlined in Scheme 2^[29]. In the spectrum of complex 1, two characteristic absorption bands at 1 776 and 1 706 cm^-1 are ascribed to the anhydride group of dta^2- (Fig. 4). The absence of strong bands at 1 700 cm^-1 indicates the deprotonation of the ligand, which is in accordance with the structural analysis results of 1. The spectrum exhibited strong broad bands at 1 610 and 1 590 cm^-1, which are attributed to asymmetric COO stretching mode, while the peaks at 1 440 and 1 398 cm^-1 are corresponding to symmetric COO stretching vibration^[30]. The differences between the asymmetric and symmetric stretching of the carboxylate groups of 1, Δ=192 and 207 cm^-1, respectively, suggest a monodentate coordinating between the carboxylate group and barium ion^[30]. The difference between the asymmetric and symmetric stretching of the carboxylate groups of 1, Δ =150 cm^-1, indicates the presence of chelating —COO groups^[31]. Carboxylic acid anhydrides displayed symmetric and asymmetric carbonyl (C=O)₂ stretching vibration, respectively. For conjugation carboxylic acid anhydrides, the stronger absorption band of symmetric (C=O)₂ ranged from 1 770 to 1 780 cm^-1, while the weaker absorption band of asymmetric (C=O)₂ ranged from 1 715 to 1 725 cm^-1[31].

  Scheme 2

  

  Scheme 2.  Forming pathway of 1, 8-naphthalic anhydride-4, 5-dicarboxylic

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  Figure 4

  

  Figure 4.  FT-IR spectra of ligand nta and complex 1

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  2.3   Luminescence properties of complex 1

  MOFs have been reported to have the ability to adjust the emission wavelength of organic ligands through the incorporation of metal centers. Therefore, it is important to investigate the luminescence properties of MOFs given potential applications as light-emitting diodes (LEDs)^[32]. The luminescent behaviors of the ligand nta and complex 1 were investigated at room temperature using the same weight of powder in the solid - state, and the emission spectra are indicated in Fig. 5. Complex 1 exhibited photoluminescence with maximal emission at 520 nm upon excitation at 320 nm, which was about 100 nm red-shifting compared to ligand nta (maximal emission at 420 nm upon excitation at 290 nm). The observed emissions of complex 1 are probably contributed by the π-π^* intra-ligand fluorescence since similar emissions were also observed for the ligand itself^[33]. Nevertheless, the large red-shift of maximal emission is considerately attributed to the coordination or an excited state of a metal perturbing intra - ligand. The observed stronger emission intensity of 1 than free ligand implies the increased rigidity of the aromatic backbone of the ligand. This is also attributed to a strong π -π stacking resulting from the enhanced intra -/intermolecular interactions among the organic ligands due to the formation of MOFs, which can facilitate energy transfer^[33]. This is well known as aggregation - induced emission (AIE), which is caused by the coordination of organic ligands to metal ions that restricts the deformation of the ligand and induces nonradiative relaxation^[34-35].

  Figure 5

  

  Figure 5.  Emission spectra of complex 1 and ligand nta in the solid-state at room temperature

  λ_ex=320 nm (1), 290 nm (nta)

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  2.4   Detection of aromatic amines

  First, the UV-Vis spectra of complex 1 before and after the addition of aromatic amine are given in Fig. 6A and 6B. As shown in Fig. 6A, with the addition of 1-aminopyrene, the absorbance of the samples in a range of 200 to 400 nm increased gradually. As shown in Fig. 6B, 1 - aminopyrene itself had two maximal absorption peaks at 285 and 360 nm, and complex 1 had the maximum at 350 nm, which confirms the absorbance change of 1 - aminopyrene after 1 reacted with 1 - aminopyrene. Through analysis of the relationship between the absorbance at 350 nm and the added amount, the calculated regression equation and correlation coefficient were y=0.089 29+0.004 01x and 0.989 04, which shows that the enhancement of absorption peak is linearly related to the increase amount of 1-aminopyrene. The changes of the fluorescence intensity of 1 and 1 reacted with different amines are clearly shown in Fig. 6C, where it could be found that the highest enhancement was up to 1.7 - fold with maximum emission at 445 nm (excited at 320 nm) and the detection limit of 1-aminopyrene was calculated to be down to 0.01 mg·g^-1 (the ratio of 1-aminopyrene to complex 1). To explore the specificity of amines detection by complex 1, aniline and 1 - naphthylamine in the same ratios (0.01 mg·g^-1) were also tested. However, the intensity of their maximum emission increased less than that of 1 with 1-aminopyrene. The photographs of the samples with and without these amines under daylight were also recorded using a digital camera. The sample of 1 with 1-aminopyrene showed a visible color change from light brown to dark green. These results demonstrated that complex 1 exhibited an optimal enhanced fluorescent response to a low concentration of 1 - aminopyrene. Furthermore, the FT - IR spectra (Fig. 7) exhibited strong broadband at 1 560 cm^-1 owing to O=C—N_as stretching mode. This further confirms the absorbance change of 1 - aminopyrene is mainly related to the reaction of an amino group from aromatic amine and anhydride group from dta^2-[36].

  Figure 6

  

  Figure 6.  (A) UV-Vis spectra of complex 1 (1 mg) reacted with 1-aminopyrene of different masses ranging from 20 to 160 µg (a-g, respectively); (B) UV-Vis spectra of the samples: (a) 1, (b) 1 reacted with 20 µg 1-aminopyrene, (c) 1-aminopyrene; (C) Emission spectra of complex 1 before and after reacted with various aromatic amines of 10 µg: (a) 1, (b) 1 reacted with aniline, (c) 1 reacted with 1-naphthylamine, (d) 1 reacted with 1-aminopyrene

  Inset in (A): plot of absorbance at 350 nm vs mass of 1-aminopyrene; Inset in (C): photos of the powder samples

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  Figure 7

  

  Figure 7.  FT-IR spectra of complex 1 and 1 reacted with 1-aminopyrene at 50 ℃

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  2.5   Thermal stability and precursor for crystalline nano-BaCO₃

  TGA was used to examine the thermal stability of complex 1. The TG curve of 1 (Fig. 8) exhibited two main weight loss stages in a temperature ranges of 18187 ℃ (8.93%) and 307 - 554 ℃ (35.08%). This first and second weight loss are corresponding to the release of two coordinated water molecules (Calcd. 7.87%) and C₈H₁₀ (Calcd. 34.14%, caused by decomposition of the ligand), respectively. The final residue may be BaCO₃.

  Figure 8

  

  Figure 8.  TG curve of 1

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  In addition, dehydration and rehydration experiments were performed for 1, and PXRD was used to determine the phase reversibility. Complex 1 was heated at 300 ℃ for 10 min, to obtain complete loss of water. The powdered dehydrated phase had a PXRD pattern different from complex 1 (Fig. 9), which indicates that the framework probably shrank after the removal of water. The dehydrated phase was afterward exposed to water vapor at room temperature for another 24 h rehydration. The PXRD pattern of rehydrated sample was similar to that of 1 (see Fig. 9), which shows that the dehydration/rehydration process for 1 is reversible.

  Figure 9

  

  Figure 9.  PXRD patterns of simulation of 1 from single-crystal X-ray data and powder samples prepared by dehydration and rehydration process

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  The morphology of nano-sized BaCO₃ powder was studied by scanning electron microscopy (SEM) as shown in Fig. 10. SEM images of the particles obtained from the calcination of 1 in the air under different temperatures showed a size range of 0.1-0.41 µm. The PXRD patterns (Fig. 11) confirmed that single-crystalline BaCO₃ was formed by the thermal decomposition of 1 at different temperatures (a: 600 ℃, b: 650 ℃, c: 700 ℃) because all the d values (d is the distance between the lattice planes in the crystal) correspond to the reported values with no detectable peaks from impurity^[37]. The samples consist of a single phase of well-crystalline BaCO₃ with an orthorhombic structure (PDF No. 45 - 1471) and with lattice parameters of a= 0.643 3 nm, b=0.531 5 nm, c=0.890 4 nm. The strong and sharp diffraction peaks suggest that the prepared BaCO₃ is highly crystalline.

  Figure 10

  

  Figure 10.  SEM images of BaCO₃ obtained by thermolysis of 1 in the air at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  Figure 11

  

  Figure 11.  PXRD patterns of BaCO₃ obtained by thermolysis of 1 in the air at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  To further confirm the polymorphs of as-prepared products at different temperatures, they were characterized by FT - IR spectroscopy and the corresponding results are shown in Fig. 12. In general, isolated, planar CO₃^2- anion has a D_3h symmetry. The absorption bands attributed to the vibrations in CO₃^2- anion were located in the 2 000 -400 cm^-1 region. The vibrational spectra of carbonate minerals contain four normal modes: symmetric stretching (ν₁), out-of-plane bending (ν₂), antisymmetric stretching (ν₃), and in - plane bending (ν₄). The strong broad absorption centered at about 1 454 cm^-1 is ascribed to the asymmetric stretching vibration and two strong sharp absorption bands at about 856 and 694 cm^-1 can be assigned to out-of-plane bending vibrations and in - plane vibrations, respectively. The result agrees with the XRD analysis and further confirms the formation of BaCO₃^[38].

  Figure 12

  

  Figure 12.  FT-IR spectra of as-synthesized BaCO₃ at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  3.   Conclusions

  In summary, a new alkaline earth metal barium complex was synthesized and characterized. In complex 1, the central Ba²⁺ ion is nine - coordinate with a distorted mono-capped square geometry. Three carboxyl groups take three different coordination modes: μ¹-η¹ ∶η⁰, μ¹-η¹∶η¹, μ³-η²∶η². The whole dna^2- anion acts as a μ₃-bridge connecting three different Ba (Ⅱ) ions resulting in a 3D structure. The fluorescent and thermal stable properties of complex 1 were also investigated. In addition, it offers a"turn-on"sensing behavior for aromatic amines with a low detection limit. This polymer precursor was also thermally decomposed to prepare micro-crystal calcite particles.

  
  Acknowledgments: This work is supported by the National Natural Science Foundation of China (Grant No. 21671107), Science Research Starting Project of Chuzhou University (Grant No. 2014qd035), Foundation of Nanjing Xiaozhuang University (Grant No.2017NXY11), College Student Innovation and Entrepreneurship Training Program (Grants No. 202011460070Y, 2020XSKY089).
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• 

  Figure 1  Coordination geometry of complex 1 drawn at 30% probability displacement ellipsoids

  Hydrogen atoms are omitted for clarity; Symmetry codes: #1: 1-x, -y, 1-z; #2: 1-x, -1-y, 1-z

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  Scheme 1  ORTEP view of coordination model of dna^2-

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  Figure 2  Infinite 2D structure in complex 1

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  Figure 3  Crystal packing diagram for 1

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  Scheme 2  Forming pathway of 1, 8-naphthalic anhydride-4, 5-dicarboxylic

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  Figure 4  FT-IR spectra of ligand nta and complex 1

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  Figure 5  Emission spectra of complex 1 and ligand nta in the solid-state at room temperature

  λ_ex=320 nm (1), 290 nm (nta)

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  Figure 6  (A) UV-Vis spectra of complex 1 (1 mg) reacted with 1-aminopyrene of different masses ranging from 20 to 160 µg (a-g, respectively); (B) UV-Vis spectra of the samples: (a) 1, (b) 1 reacted with 20 µg 1-aminopyrene, (c) 1-aminopyrene; (C) Emission spectra of complex 1 before and after reacted with various aromatic amines of 10 µg: (a) 1, (b) 1 reacted with aniline, (c) 1 reacted with 1-naphthylamine, (d) 1 reacted with 1-aminopyrene

  Inset in (A): plot of absorbance at 350 nm vs mass of 1-aminopyrene; Inset in (C): photos of the powder samples

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  Figure 7  FT-IR spectra of complex 1 and 1 reacted with 1-aminopyrene at 50 ℃

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  Figure 8  TG curve of 1

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  Figure 9  PXRD patterns of simulation of 1 from single-crystal X-ray data and powder samples prepared by dehydration and rehydration process

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  Figure 10  SEM images of BaCO₃ obtained by thermolysis of 1 in the air at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  Figure 11  PXRD patterns of BaCO₃ obtained by thermolysis of 1 in the air at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  Figure 12  FT-IR spectra of as-synthesized BaCO₃ at different temperatures: (a) 600 ℃, (b) 650 ℃, (c) 700 ℃

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  Table 1.  Crystallographic data of complex 1

  Parameter	1
  Chemical formula	C14H8BaO9
  Formula weight	457.54
  crystal system	Triclinic
  Space group	P1
  a / nm	0.717 05(6)
  b /nm	0.828 50(7)
  c / nm	1.160 65(10)
  α / (°)	75.836(2)
  β / (°)	84.036(2)
  γ / (°)	87.866(2)
  V / nm3	0.664 88(10)
  Z	2 2
  Dc / (g·cm-3)	0.285
  μ (Mo Kα) / mm-1	3.041
  Unique reflection	3 049
  Observed reflection	2 918
  Rint	0.018 4
  F(000)	440
  R1, wR2 (all data)	0.019 1, 0.051 2
  R1, wR2 [I > 2σ(I)]a, b	0.017 9, 0.050 4
  GOF	1.002
  a R1=∑||Fo|-|Fc||/∑|Fo|; b wR2={∑[w(|Fo|2-|Fc|2)2]/∑[w(|Fo|2)2]}1/2.

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  Table 2.  Selected bond lengths (nm) and angles (°) for 1

  Ba1—O1	0.282 21(17)	Ba1—O7	0.282 63(17)	Ba1—O6	0.277 60(17)
  Ba1—O8	0.277 7(2)	Ba1—O2#1	0.261 98(17)	Ba1—O9	0.276 9(2)
  Ba1—O3	0.293 11(19)	Ba1—O7#2	0.302 14(19)	Ba1—O2	0.323 07(18)
  O2#1—Ba1—O9	93.72(7)	O2#1—Ba1—O6	134.20(5)	O9—Ba1—O6	128.94(6)
  O2#1—Ba1—O8	70.04(6)	O9—Ba1—O8	122.37(7)	O6—Ba1—O8	72.61(6)
  O2#1—Ba1—O1	115.36(5)	O9—Ba1—O1	66.34(6)	O6—Ba1—O1	75.86(5)
  O8—Ba1—O1	72.05(6)	O2#1—Ba1—O7	133.24(5)	O9—Ba1—O7	81.78(7)
  O6—Ba1—O7	76.30(5)	O8—Ba1—O7	148.49(6)	O1—Ba1—O7	105.27(5)
  O2#1—Ba1—O3	78.67(6)	O9—Ba1—O3	137.44(7)	O6—Ba1—O3	78.83(6)
  O8—Ba1—O3	94.52(6)	O1—Ba1—O3	153.93(6)	O7—Ba1—O3	74.34(5)
  O2#1—Ba1—O7#2	65.03(5)	O9—Ba1—O7#2	66.92(6)	O6—Ba1—O7#2	140.52(5)
  O8—Ba1—O7#2	134.74(5)	O1—Ba1—O7#2	133.16(5)	O7—Ba1—O7#2	70.60(6)
  O3—Ba1—O7#2	72.07(5)	O2—Ba1—O2#1	73.47(5)	O9—Ba1—O2	62.37(6)
  O6—Ba1—O2	108.96(5)	O8—Ba1—O2	60.00(6)	O1—Ba1—O2	42.27(5)
  O7—Ba1—O2	138.14(5)	O7#2—Ba1—O2	109.99(5)	O3—Ba1—O2	147.22(5)
  Symmetry codes: #1: 1-x, -y, 1-z; #2: 1-x, -1-y, 1-z.

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•