English

• 1. INTRODUCTION

  In recent years, lanthanide complexes have been extensively studied and reported in terms of luminescence^[1-3], catalysis^[4-6] and magnetism^[7-9]. As an important area in the coordination chemistry of lanthanide metals, complexes with phosphine oxides have attracted much attention^[10]. Anna G. Matveeva group have ever reported a series of lanthanide complexes by using hybrid scorpionate (OPPh₂)₂CHCH₂C(O)Me as ligand, and the coordination modes vary with the polyhedron of metals and the nature of solvent^[11]. Phosphonate has similar characteristics and properties to phosphine oxide groups (P=O), and correspon- ding complexes usually exhibit excellent properties and potential applications while rare work was carried out on lanthanide^[12-14]. In terms of hard acid, the lanthanide metal cation has very strong oxygen affinity and can easily interact with highly polar oxygen-containing groups to form a variety of complexes and coordination polymers. In this paper, following the Hard-Soft-Acid-Base (HSAB) theory, tetraethyl ethylenediphosphonate was adopted to coordinate with lanthanide ions. The ratio of Ln: L = 1:3, and the ligand chelating with the central ion satisfies the high coordination number of lanthanide ions. The mixed solvent of acetonitrile and water was found more conducive to the formation of high-quality, high-yield crystals. Besides, polyoxometalates (POMs) functionalized materials have broad application prospects in magnetic materials, catalysis, energy conversion and energy storage materials^[15-17]. So, POM-based organic- inorganic hybrids complexes have been an attractive topic^{[18, 19]}. In this work, the Keggin-type [PMo₁₂O₄₀]^3- was added to the system without coordinating with Ln(Ⅲ) but exists as an anion. According to Platon calculation and crystal structure analysis, there are hydrogen bonds between [PMo₁₂O₄₀]^3- anions and phosphonate, and [PMo₁₂O₄₀]^3- acts as a template in the entire complex structure.

  In addition, the terahertz time-domain spectra (THz-TDs) of the composite material at 0.2~2.8 THz (6.6~92.4 cm^-1) were measured at room temperature. This technique has been proven to detect free electron motion, molecular rotation modes, lattice vibration and dipole transitions, which can characterize the way of intermolecular interactions^[20-22]. According to our previous work, we have synthesized a number of lanthanide complexes with the bisphosphonate ligand and characterized them by terahertz time-domain spectroscopy^[23-25]. Herein, we first adopt THz-TDS to characterize lanthanide-bisphosphonate complexes based on POMs modification.

  2. EXPERIMENTAL

  2.1 Materials and measurements

  All commercially available initial reagents were used without furthermore treatment. FT-IR spectra (KBr pellets) were measured on a Perkin-Elmer Infrared spectrometer. C, H and N elemental analyses were carried out on an Elementar Vario MICRO CUBE (Germany) elemental analyzer. UV-Vis spectra were gained from a 2550 UV-Vis spectrophotometer (Shimadzu, Japan). The THz absorption spectra were recorded on a THz time domain device of Minzu University of China and carried out in a N₂ atmosphere to avoid the influence of water vapor, based on photoconductive switches for the generation and electro-optical crystal detection of the far-infrared light, effective frequency in the range of 0.2~2.8 THz.

  2.2 Syntheses of the complexes 1~3

  A mixture of 0.2 mmol Ln(NO₃)₃·6H₂O (Dy for 1, Ho for 2, Lu for 3), H₃PMo₁₂O₄₀·nH₂O (0.3651 g) and L (0.1813 g, 0.6 mmol) was dissolved in the mixed solvents of 8 mL CH₃CN and 2 mL H₂O, followed by stirring for 3 hours in an 80 ℃ water bath. The solution was filtered. Block-shaped crystals were obtained from the filtrate after standing at room temperature for several days. The crystals of complexes 1 and 3 were yellow and that of 2 was orange.

  [DyL₃(H₂O)]PMo₁₂O₄₀·C₂H₃N (1)    Yield: 60.19%. Element analysis calcd. for C₃₂H₇₆DyMo₁₂NO₅₉P₇ (%): C, 13.03; H, 2.60; N, 0.48. Found (%): C, 13.51; H, 2.52; N, 0.56. IR data (cm^-1, KBr pellets): 3469m, 2985m, 2926w, 1617w, 1476m, 1442m, 1395m, 1370w, 1304m, 1208s, 1162s, 1033s, 959s, 879s, 792s, 503s.

  [HoL₃(H₂O)]PMo₁₂O₄₀·C₂H₃N (2)    Yield: 63.67%. Element analysis calcd. for C₃₂H₇₄HoMo₁₂NO₅₉P₇ (%): C, 13.03; H, 2.53; N, 0.48. Found (%): C, 13.47; H, 2.44; N, 0.56. IR data (cm^-1, KBr pellets): 3469w, 2985w, 1637w, 1476w, 1442w, 1395w, 1371w, 1304w, 1209s, 1162m, 1063s, 1033s, 958s, 880s, 803s, 503m.

  [LuL₃(H₂O)]PMo₁₂O₄₀·C₂H₃N (3)    Yield: 55.52%. Element analysis Calcd. for C₃₂H₇₅LuMo₁₂NO₅₉P₇ (%): C, 12.98; H, 2.55; N, 0.48. Found (%): C, 13.57; H, 2.29; N, 0.55. IR data (cm^-1, KBr pellets): 3449w, 2985w, 1637w, 1467w, 1442w, 1396w, 1304w, 1211s, 1162m, 1063s, 1034s, 958s, 879s, 803s, 503w.

  2.3 Structure determination

  Single crystals of the title complexes were mounted on a Bruker Smart 1000 CCD diffractometer equipped with a graphite-monochromated MoKα (λ = 0.071073 nm) radiation at 298 K. Semi-empirical absorption corrections were applied using SADABS programs. All structures were solved by direct methods using SHELXS program of the SHELXTL-97 package and refined with SHELXL-97^{[26, 27]}. Metal atom centers were located from E-maps and other non-hydrogen atoms were located in successive difference Fourier syntheses. The final refinements were performed by full-matrix least-squares methods with anisotropic thermal parameters for non-hydrogen atoms on F². The hydrogen atoms were genera- ted geometrically and refined with displacement parameters riding on the concerned atoms.

  Crystallographic data and experimental details for struc- tural analysis are summarized in Table 1, and selected bond lengths and bond angles of complexes 1~3 are summarized in Table 2.

  Table 1

  

  Table 1.  Crystallographic Data for Complexes 1~3

  DownLoad: CSV

  Complex	1	2	3
  Formula	C32H76DyMo12NO59P7	C32H74HoMo12NO59P7	C32H75LuMo12NO59P7
  Formula weight	2949.51	2949.92	2960.970
  T/K	298(2)	298(2)	293(2)
  Crystal system	Monoclinic	Monoclinic	Monoclinic
  Space group	P21/c	P21/c	P21/c
  Crystal size/mm	0.20 × 0.20 × 0.20	0.20 × 0.20 × 0.20	0.20 × 0.20 × 0.20
  a (Å)	25.628(3)	25.633(2)	25.3493(3)
  b (Å)	14.5396(14)	14.5341(15)	14.4082(1)
  c (Å)	24.399(2)	24.391(2)	24.0864(3)
  α (°)	90.00	90.00	90
  β (°)	113.534(3)	113.456(2)	113.564(1)
  γ (°)	90.00	90.00	90
  V (Å3)	8335.2(14)	8335.9(14)	8063.69(16)
  Z	4	4	4
  F(000)	5688	5684.0	5704.0
  Goodness-of-fit on F2	1.096	1.077	1.076
  Rint	0.0891	0.0834	0.2238
  R (I > 2σ(I))a	0.0779	0.0674	0.1486
  wR (I > 2σ(I))b	0.1888	0.1575	0.3069
  R (all data)a	0.1523	0.1338	0.1587
  wR (all data)b	0.2231	0.1835	0.3156
  a R= ∑(||Fo| – |Fc||)/∑|Fo|, b wR=[∑w(|Fo|2 – |Fc|2)2/∑w(Fo2)]1/2

  Table 2

  

  Table 2.  Selected Bond Distances (Å) and Bond Angles (°) for Complexes 1~3

  DownLoad: CSV

  Complex 1
  Dy(1)–O(45)	2.293(11)		Dy(1)–O(48)	2.279(12)		Dy(1)–O(51)	2.268(12)
  Dy(1)–O(54)	2.300(11)		Dy(1)–O(57)	2.295(11)		Dy(1)–O(60)	2.261(12)
  Dy(1)–O(63)	2.396(13)
  O(48)–Dy(1)–O(45)	77.1(4)		O(51)–Dy(1)–O(54)	75.2(4)		O(60)–Dy(1)–O(57)	78.7(5)
  Complex 2
  Ho(1)–O(60)	2.240(10)		Ho(1)–O(54)	2.264(10)		Ho(1)–O(57)	2.272(10)
  Ho(1)–O(48)	2.278(10)		Ho(1)–O(51)	2.279(10)		Ho(1)–O(45)	2.281(9)
  Ho(1)–O(63)	2.428(10)
  O(48)–Ho(1)–O(45)	77.3(4)		O(54)–Ho(1)–O(51)	76.3(4)		O(60)–Ho(1)–O(57)	78.1(4)
  Complex 3
  Lu(1)–O(1)	2.199(16)		Lu(1)–O(3)	2.253(18)		Lu(1)–O(4)	2.184(18)
  Lu(1)–O(5)	2.366(17)		Lu(1)–O(7)	2.204(18)		Lu(1)–O(9)	2.236(19)
  Lu(1)–O(13)	2.259(17)
  O(1)–Lu(1)–O(13)	76.0(6)		O(4)–Lu(1)–O(3)	79.4(7)		O(7)–Lu(1)–O(9)	79.0(7)

  2.4 Dye adsorption experiment

  Rhodamine B aqueous solution was used as a wastewater simulation system to study the adsorption activity of this series of complexes. The dye powder was dissolved in distilled water to obtain a 20 mg/L solution. In a typical adsorption reaction, 50 mL of 20 mg/L dye solution was stirred with 50 mg of complex powder. Taking aliquots at different time intervals, the UV-visible absorbance in time after rapid centrifugation was measured. Formula (1) was applied to calculate the dye adsorption efficiency.

  $ \mathrm{H}=\left[\left(\mathrm{C}_0-\mathrm{C}\right) / \mathrm{C}_0\right] \times 100 \% $

  (1)

  In the formula, η is the adsorption efficiency and C₀ is the concentration before adsorption, mg/L; C is the concentration after adsorption, mg/L.

  3. RESULTS AND DISCUSSION

  3.1 Description of the crystal structures

  Single-crystal X-ray diffraction analysis reveals that each asymmetric unit contains a [LnL₄(H₂O)]³⁺, a [PMo₁₂O₄₀]^3- and a acetonitrile molecule. Complexes 1~3 crystallize in the monoclinic system with space group P2₁/c. They are all seven-coordinated by six oxygen atoms from three L ligands and one oxygen atom from a water molecule (Fig. 1). [PMo₁₂O₄₀]^3- exists only as an anion. It is not involved in coordination, and remains unchanged in structure. Herein, we discuss complex 1 deeply to demonstrate the general structural features. In 1, the Dy–O (P=O) bond lengths range from 2.261(12) to 2.300(11) Å. Compared with the similar complex [DyL₂(H₂O)₄]Cl₃·6H₂O (L = tetrakis(O-isopro- pyl)methylenediphosphonate)^[17], the average distance of Dy–O (P=O) bonds (2.299 Å) in complex 1 is shorter and the (P)O–Dy–O(P) bond angle (77.0°) is slightly increased. The coordination spheres of three crystals are all composed of Ln–O bonds but with different lengths. Detailed information about other complexes was put in ESI. By analyzing different complexes, it found that the Ln–O bond lengths depend on the radii of rare earth ions (rLu³⁺(0.861 Å) < rHo³⁺ (0.901 Å) < rDy³⁺ (0.912 Å)). The bond lengths of Ln–O increase as the radius of metal grows in the order of Dy–O > Ho–O > Lu–O (Table 2). At the same time, the comparison of average (P)O–Ln–O(P) bond angle formed by L ligands chelation results in the following order: complex 3 > complex 2 > complex 1.

  Figure 1

  

  Figure 1.  Molecular structure of complex 1. Hydrogen atoms were omitted for clarity

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  Complex 1 forms a three-dimensional structure through the action of abundant hydrogen bonds (Fig. 2). Wherein the hydrogen bonds are mainly C–H···O constructed by the hydrogen atoms from L ligands and oxygen atoms from [PMo₁₂O₄₀]^3-. Interestingly, despite all complexes have similar structures, the number of hydrogen bonds is different. In a basic unit, the number of hydrogen bonds in complexes 1~3 is 10, 9, and 11, respectively. Moreover, the angles and positions of hydrogen bonds vary with different complexes (Table 3). For 1, the nitrogen atom from the acetonitrile combines with the O–H group from coordination water to form hydrogen bonds O(63)–H(63D)···N(1). But in complexes 2 and 3, the C–H groups come from acetonitrile and the oxygen atoms from [PMo₁₂O₄₀]^3–, resulting in hydrogen bonds like C(32)–H(32C)···O(19) and C(15)– H(15A)···O(8).

  Figure 2

  

  Figure 2.  Three-dimensional stacking structure of complex 1. Hydrogen atoms and carbon chains not related to hydrogen bonding were omitted for clarity

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  Table 3

  

  Table 3.  Intermolecular Hydrogen Bonds in Complexes 1~3

  DownLoad: CSV

  Complex 1
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetry code
  O(63)–H(63C)···O(13)	0.85	2.08	2.906(19)	165
  O(63)–H(63D)···N(1)	0.85	2.02	2.85(3)	165	x, 1+y, z
  C(3)–H(3A)···O(37)	0.97	2.51	3.26(3)	134	2–x, 1/2+y, 3/2–z
  C(4)–H(4C)···O(43)	0.96	2.59	3.43(3)	148	2–x, 1–y, 2–z
  C(10)–H(10B)···O(18)	0.96	2.60	3.49(3)	155	1–x, 1–y, 1–z
  C(12)–H(12B)···O(42)	0.97	2.54	3.41(2)	160	1–x, 1/2+y, 3/2–z
  C(12)–H(12B)···O(46)	0.97	2.60	3.32(2)	138
  C(24)–H(24A)···O(17)	0.96	2.37	3.25(4)	152	x, 1+y, z
  C(27)–H(27A)···O(17)	0.97	2.49	3.43(4)	174	x, 3/2–y, 1/2+z
  C(28)–H(28C)···O(9)	0.96	2.53	3.33(4)	141	x, 1+y, z
  Complex 2
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetric code
  C(4)–H(4C)···O(43)	0.96	2.56	3.42(3)	150	2–x, 1–y, 2–z
  C(10)–H(10B)···O(18)	0.96	2.59	3.54(3)	171	1–x, 1–y, 1–z
  C(12)–H(12A)···O(22)	0.97	2.50	3.43(2)	160	1–x, 1/2+y, 3/2–z 333333333/2–z
  C(12)–H(12B)···O(42)	0.97	2.52	3.320(19)	140
  C(19)–H(19B) ···O(9)	0.97	2.60	3.53(3)	161
  C(23)–H(23B)···O(44)	0.97	2.57	3.53(3)	170	x, 3/2–y, –1/2+z
  C(24)–H(24B)···O(42)	0.96	2.42	3.37(3)	169	x, 3/2–y, –1/2+z
  C(27)–H(27A)···O(17)	0.97	2.46	3.43(3)	177	x, 3/2–y, 1/2+z
  C(32)–H(32C)···O(19)	0.96	2.53	3.44(2)	159	1–x, –y, 1–z
  Complex 3
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetric code
  C(2)–H(2A)···O(16)	0.97	2.44	3.27(4)	144
  C(3)–H(3A)···O(28)	0.96	2.43	3.36(4)	161	x, 1/2–y, –1/2+z
  C(3)–H(3B)···O(23)	0.98	2.43	3.23(4)	138
  C(5)–H(5B)···O(6)	0.97	2.60	3.41(5)	141
  C(9)–H(9A)···O(12)	0.97	2.59	3.47(5)	151	1–x, 1/2+y, 1/2–z 11111/21/2+z 1/2–z
  C(12)–H(12B)···O(11)	0.97	2.35	3.26(4)	155	x, 1/2–y, 1/2+z
  C(15)–H(15A)···O(8)	0.96	2.58	3.47(5)	155
  C(17)–H(17B)···O(42)	0.97	2.52	3.27(5)	134	x, 1+y, z
  C(19)–H(19A)···O(34)	0.97	2.54	3.50(5)	173	x, 1/2–y, –1/2+z
  C(19)–H(19B)···O(45)	0.98	2.59	3.28(5)	127	2–x, 1–y, 1–z
  C(25)–H(25B)···O(42)	0.96	2.40	3.31(5)	158

  3.2 IR, PXRD and TG curves of complexes

  The IR absorption spectra of complexes 1~3 were determined in the scope of 4000 to 400 cm^-1. Complexes 1~3 have very similar IR spectra, so only complex 1 is described in detail. For L ligands, the characteristic absorption band of ν(C−P−O) at 1035 cm^-1 shifts to 1034 cm^-1 and that of ν(P=O) at 1260 shifts to 1211 cm^-1[28]. All changes on the infrared absorption spectra are mainly caused by the coordination between P=O groups and rare earth ions. Besides, the bands at 958~803 cm^-1 are attributed to the Mo−O−Mo and Mo=O characteristic bands from POM^[29].

  Powder X-ray diffraction of complexes 1~3 shows that the samples have obvious crystal phase diffraction peaks in the range of 5~50º. The main peaks of the synthesized samples in the spectra are consistent well with the simulation results, indicating the high crystal phase purity of powder samples complexes 1~3 (Fig. 3).

  Figure 3

  

  Figure 3.  Powder PXRD patterns of complexes 1~3 compared with the simulation results

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  The thermal stability characterization of complexes 1~3 was carried out in nitrogen atmosphere from 30 to 850 ℃ at an average heating rate of 10 ℃/min. As shown in Fig. 4, the TG curves for complexes 1~3 display initial weight loss of 1.7% (calcd. 2.0%) for 1, 2.6% (calcd. 2.0%) for 2 and 3.2% (calcd. 2.0%) for 3 in the 30~240 ℃ region, which can be attributed to the loss of acetonitrile in crystal lattice and one coordinated water molecule. Then the dehydrated complexes 1~3 begin to decompose at 240 ℃ and the TG curve shows a maximum mass loss rate at 240~370 ℃.

  Figure 4

  

  Figure 4.  TG curves of complexes 1~3

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  3.3 Adsorption of dyes by complexes

  Adsorption is a simple and effective method during purification process of dye wastewater. Based on electrostatic interaction, RhB, as a cationic dye, can be effectively handled by large volume of [PMo₁₂O₄₀]^3- added to the complexes. During the adsorption experiment, 1.5 mL of sample solution was collected at certain intervals, and UV-vis spectroscopy was performed after centrifugation at 10000 r/min. The results show that complexes 1~3 have excellent dye adsorption performance and RhB was adsorbed significantly within 5 minutes (Fig. 5). It is worth noting that among the three complexes, 1 has the highest adsorption efficiency with the rate being 92.22% at 5 minutes, and reaching 93.54% after 30 minutes. In order to confirm that only adsorption but no degradation occurs, the samples after adsorption were soaked in ethanol, and the existence of RhB was proved by UV-vis spectroscopy. We also monitored the PXRD patterns after adsorption and desorption, indicating that the framework of 1 is stable and maintains during the processes.

  Figure 5

  

  Figure 5.  (a)-(c) UV-Vis spectra of RhB solutions under different adsorption time: (a) complex 1; (b) complex 2; (c) complex 3. (d) Adsorption efficiency of RhB by complexes 1~3

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  The effects of the different initial concentration on the adsorption of RhB for complex 1 are shown in Fig. 6. It is obvious that the adsorption capacity increased gradually from 35.95 to 113.93 mg/g with the increase of the initial concentration of RhB. Moreover, there was little increase for the adsorption capacity corresponding to the initial concentra- tion of RhB from 180 to 200 mg/L, which indicated that a saturated adsorption capacity has been attained. The adsorption capacity of complex 1 is better than that of the ordinary adsorbents such as Sago waste derived activated carbon, 16.1 mg/g^[30] and acid-functionalized multiwalled carbon nanotubes, 42.68 mg/g^[31].

  Figure 6

  

  Figure 6.  Effects of initial concentration on the adsorption of RhB in complex 1

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  The three complexes have similar structures but different intermolecular interactions, leading to a small gap in their adsorption performance. It is speculated that the slight difference can be attributed to the difference in hydrogen bonds between molecules, especially the hydrogen bonds on the surface of [PMo₁₂O₄₀]^3-, which may affect the diffusion of dye molecules.

  3.4 Terahertz time domain spectroscopy (THz-TDS)

  The terahertz time-domain spectroscopy (THz-TDS) of H₃PMo₁₂O₄₀·nH₂O and complexes 1~3 were measured in the range of 0.2~2.8 THz at room temperature. All the above compounds have characteristic resonance peaks, which may be explained by the factors of polar molecules and dipoles rotating and vibrating, resulting in strong absorption and chromatic dispersion. The peaks found for them are as follows: H₃PMo₁₂O₄₀·nH₂O (0.38, 0.53, 0.64, 0.73, 1.84, 1.96, 2.13, 2.22, 2.31, 2.40, 2.46, 2.55, 2.66, 2.75 THz) (Fig. 7); L ligand (0.90, 1.05, 1.20, 1.25, 1.46, 1.55, 1.76, 1.90, 2.10, 2.10, 2.31, 2.51, 2.57, 2.72 THz) (Fig. 8); complex 1 (0.32, 0.38, 0.44, 0.56, 0.64, 0.82, 0.91, 1.05, 1.20, 1.28, 1.37, 1.46, 1.55, 1.84, 1.99, 2.10, 2.19, 2.28, 2.37, 2.45, 2.52, 2.72 THz); complex 2 (0.32, 0.38, 0.44, 0.56, 0.70, 0.82, 0.93, 1.05, 1.20, 1.28, 1.37, 1.46, 1.55, 1.84, 1.90, 1.99, 2.04, 2.19, 2.31, 2.45, 2.52, 2.60, 2.72 THz) and complex 3 (0.38, 0.44, 0.53, 0.64, 0.73, 0.82, 0.91, 0.99, 1.20, 1.25, 1.37, 1.46, 1.55, 1.75, 1.84, 1.90, 1.99, 2.10, 2.19, 2.31, 2.44, 2.52, 2.60, 2.66, 2.75 THz) (Fig. 9). The THz absorption spectra of H₃PMo₁₂O₄₀·nH₂O show a rising trend in the range of 0.2~2.8 THz and have many obvious peaks in the range of 1.84~2.75 THz. The THz absorption spectra of L ligand show the first rise and fall, and have a lot of tiny peaks in the 0.9~2.8 THz region. Complexes 1~3 have almost consistent THz absorption spectra due to their similar structures. By comparing the THz absorption spectra of the products with L ligand and H₃PMo₁₂O₄₀·nH₂O, we can easily find that some peaks of the reactants disappear or move in the complexes, which can be attributed to the generation of new structures and intermole- cular interactions. The peak shapes of complexes 1~3 in 1.84~2.75 THz were different, which is likely to reflect the difference in the weak intermolecular forces that cause the different adsorption efficiency. Because of many hydrogen bonds in complexes, it is not easy to make tentative assignments of peaks in the terahertz region for the samples. However, it is worth noting that the construction of hydrogen bonds in complex 1 is different from that of complexes 2 and 3, so the peak of 1 at 1.75 THz may correspond to its unique hydrogen bond of O–H···N^[32]. The relationship between terahertz spectroscopy and the structure and properties of the complex needs further exploration. The results in this paper act as a supplement to the THz spectroscopic properties of lanthanide complexes containing phosphorous ligand.

  Figure 7

  

  Figure 7.  Terahertz spectrum of H₃PMo₁₂O₄₀·nH₂O

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  Figure 8

  

  Figure 8.  Terahertz spectrum of tetraethyl ethylenediphosphonate in the range of 0.2~2.8 THz in the range of 0.2~2.8 THz

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  Figure 9

  

  Figure 9.  Terahertz spectra of complexes 1~3 in the range 0.2~2.8 THz

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  4. CONCLUSION

  Three novel Ln(Ⅲ) complexes, namely [DyL₃(H₂O)]PMo₁₂O₄₀·CH₃CN (1), [HoL₃(H₂O)]PMo₁₂O₄₀·CH₃CN (2) and [LuL₃(H₂O)]PMo₁₂O₄₀·CH₃CN (3), have been synthesized and characterized by single-crystal X-ray diffraction, elemental analysis, PXRD, thermogravimetric analysis and THz time-domain spectroscopy (THz-TDS). All complexes are seven-coordinated mononuclear structures and the unit cells pack into a 3D structure by hydrogen bonds. PXRD and TG curves show good sample purity and thermal stability of the samples. Complex 1 has the highest adsorption performance for rhodamine B. Terahertz spectroscopy was used for the first time to characterize lanthanide phosphonate complexes based on [PMo₁₂O₄₀]^3- modified. The peak of complex 1 at 1.75 terahertz is related to hydrogen bond of O–H···N. Terahertz time-domain spectroscopy can act as a characterization method to analyze the changes of absorption peaks caused by intermolecular forces, which provide a spectroscopic basis for the rapid detection of weak intermolecular forces in complexes.

  
  
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• 

  Figure 1  Molecular structure of complex 1. Hydrogen atoms were omitted for clarity

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  Figure 2  Three-dimensional stacking structure of complex 1. Hydrogen atoms and carbon chains not related to hydrogen bonding were omitted for clarity

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  Figure 3  Powder PXRD patterns of complexes 1~3 compared with the simulation results

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  Figure 4  TG curves of complexes 1~3

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  Figure 5  (a)-(c) UV-Vis spectra of RhB solutions under different adsorption time: (a) complex 1; (b) complex 2; (c) complex 3. (d) Adsorption efficiency of RhB by complexes 1~3

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  Figure 6  Effects of initial concentration on the adsorption of RhB in complex 1

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  Figure 7  Terahertz spectrum of H₃PMo₁₂O₄₀·nH₂O

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  Figure 8  Terahertz spectrum of tetraethyl ethylenediphosphonate in the range of 0.2~2.8 THz in the range of 0.2~2.8 THz

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  Figure 9  Terahertz spectra of complexes 1~3 in the range 0.2~2.8 THz

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  Table 1.  Crystallographic Data for Complexes 1~3

  Complex	1	2	3
  Formula	C32H76DyMo12NO59P7	C32H74HoMo12NO59P7	C32H75LuMo12NO59P7
  Formula weight	2949.51	2949.92	2960.970
  T/K	298(2)	298(2)	293(2)
  Crystal system	Monoclinic	Monoclinic	Monoclinic
  Space group	P21/c	P21/c	P21/c
  Crystal size/mm	0.20 × 0.20 × 0.20	0.20 × 0.20 × 0.20	0.20 × 0.20 × 0.20
  a (Å)	25.628(3)	25.633(2)	25.3493(3)
  b (Å)	14.5396(14)	14.5341(15)	14.4082(1)
  c (Å)	24.399(2)	24.391(2)	24.0864(3)
  α (°)	90.00	90.00	90
  β (°)	113.534(3)	113.456(2)	113.564(1)
  γ (°)	90.00	90.00	90
  V (Å3)	8335.2(14)	8335.9(14)	8063.69(16)
  Z	4	4	4
  F(000)	5688	5684.0	5704.0
  Goodness-of-fit on F2	1.096	1.077	1.076
  Rint	0.0891	0.0834	0.2238
  R (I > 2σ(I))a	0.0779	0.0674	0.1486
  wR (I > 2σ(I))b	0.1888	0.1575	0.3069
  R (all data)a	0.1523	0.1338	0.1587
  wR (all data)b	0.2231	0.1835	0.3156
  a R= ∑(||Fo| – |Fc||)/∑|Fo|, b wR=[∑w(|Fo|2 – |Fc|2)2/∑w(Fo2)]1/2

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  Table 2.  Selected Bond Distances (Å) and Bond Angles (°) for Complexes 1~3

  Complex 1
  Dy(1)–O(45)	2.293(11)		Dy(1)–O(48)	2.279(12)		Dy(1)–O(51)	2.268(12)
  Dy(1)–O(54)	2.300(11)		Dy(1)–O(57)	2.295(11)		Dy(1)–O(60)	2.261(12)
  Dy(1)–O(63)	2.396(13)
  O(48)–Dy(1)–O(45)	77.1(4)		O(51)–Dy(1)–O(54)	75.2(4)		O(60)–Dy(1)–O(57)	78.7(5)
  Complex 2
  Ho(1)–O(60)	2.240(10)		Ho(1)–O(54)	2.264(10)		Ho(1)–O(57)	2.272(10)
  Ho(1)–O(48)	2.278(10)		Ho(1)–O(51)	2.279(10)		Ho(1)–O(45)	2.281(9)
  Ho(1)–O(63)	2.428(10)
  O(48)–Ho(1)–O(45)	77.3(4)		O(54)–Ho(1)–O(51)	76.3(4)		O(60)–Ho(1)–O(57)	78.1(4)
  Complex 3
  Lu(1)–O(1)	2.199(16)		Lu(1)–O(3)	2.253(18)		Lu(1)–O(4)	2.184(18)
  Lu(1)–O(5)	2.366(17)		Lu(1)–O(7)	2.204(18)		Lu(1)–O(9)	2.236(19)
  Lu(1)–O(13)	2.259(17)
  O(1)–Lu(1)–O(13)	76.0(6)		O(4)–Lu(1)–O(3)	79.4(7)		O(7)–Lu(1)–O(9)	79.0(7)

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  Table 3.  Intermolecular Hydrogen Bonds in Complexes 1~3

  Complex 1
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetry code
  O(63)–H(63C)···O(13)	0.85	2.08	2.906(19)	165
  O(63)–H(63D)···N(1)	0.85	2.02	2.85(3)	165	x, 1+y, z
  C(3)–H(3A)···O(37)	0.97	2.51	3.26(3)	134	2–x, 1/2+y, 3/2–z
  C(4)–H(4C)···O(43)	0.96	2.59	3.43(3)	148	2–x, 1–y, 2–z
  C(10)–H(10B)···O(18)	0.96	2.60	3.49(3)	155	1–x, 1–y, 1–z
  C(12)–H(12B)···O(42)	0.97	2.54	3.41(2)	160	1–x, 1/2+y, 3/2–z
  C(12)–H(12B)···O(46)	0.97	2.60	3.32(2)	138
  C(24)–H(24A)···O(17)	0.96	2.37	3.25(4)	152	x, 1+y, z
  C(27)–H(27A)···O(17)	0.97	2.49	3.43(4)	174	x, 3/2–y, 1/2+z
  C(28)–H(28C)···O(9)	0.96	2.53	3.33(4)	141	x, 1+y, z
  Complex 2
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetric code
  C(4)–H(4C)···O(43)	0.96	2.56	3.42(3)	150	2–x, 1–y, 2–z
  C(10)–H(10B)···O(18)	0.96	2.59	3.54(3)	171	1–x, 1–y, 1–z
  C(12)–H(12A)···O(22)	0.97	2.50	3.43(2)	160	1–x, 1/2+y, 3/2–z 333333333/2–z
  C(12)–H(12B)···O(42)	0.97	2.52	3.320(19)	140
  C(19)–H(19B) ···O(9)	0.97	2.60	3.53(3)	161
  C(23)–H(23B)···O(44)	0.97	2.57	3.53(3)	170	x, 3/2–y, –1/2+z
  C(24)–H(24B)···O(42)	0.96	2.42	3.37(3)	169	x, 3/2–y, –1/2+z
  C(27)–H(27A)···O(17)	0.97	2.46	3.43(3)	177	x, 3/2–y, 1/2+z
  C(32)–H(32C)···O(19)	0.96	2.53	3.44(2)	159	1–x, –y, 1–z
  Complex 3
  Donor-H···acceptor	D–H (Å)	H···A (Å)	D···A (Å)	D–H···A (°)	Symmetric code
  C(2)–H(2A)···O(16)	0.97	2.44	3.27(4)	144
  C(3)–H(3A)···O(28)	0.96	2.43	3.36(4)	161	x, 1/2–y, –1/2+z
  C(3)–H(3B)···O(23)	0.98	2.43	3.23(4)	138
  C(5)–H(5B)···O(6)	0.97	2.60	3.41(5)	141
  C(9)–H(9A)···O(12)	0.97	2.59	3.47(5)	151	1–x, 1/2+y, 1/2–z 11111/21/2+z 1/2–z
  C(12)–H(12B)···O(11)	0.97	2.35	3.26(4)	155	x, 1/2–y, 1/2+z
  C(15)–H(15A)···O(8)	0.96	2.58	3.47(5)	155
  C(17)–H(17B)···O(42)	0.97	2.52	3.27(5)	134	x, 1+y, z
  C(19)–H(19A)···O(34)	0.97	2.54	3.50(5)	173	x, 1/2–y, –1/2+z
  C(19)–H(19B)···O(45)	0.98	2.59	3.28(5)	127	2–x, 1–y, 1–z
  C(25)–H(25B)···O(42)	0.96	2.40	3.31(5)	158

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