Thermoanalytical, Spectroscopic and DFT Studies of Heavy Trivalent Lanthanides and Yttrium(III) with Oxamate as Ligand

Abstract

Solid-state LnL₃∙nH₂O complexes, where Ln stands for trivalent lanthanides (Tb to Lu) or yttrium(III) and L is oxamate (NH₂COCO₂^-), have been synthesized. The characterization of the complexes was performed by using elemental analysis (EA), complexometric titration with EDTA, thermoanalytical techniques such as simultaneous thermogravimetry and differential scanning calorimetry (TG-DSC), evolved gas analysis (TG-FTIR), infrared spectroscopy (IR) and powder X-ray diffraction (XRPD). The results provided information about thermal behavior, crystallinity, stoichiometry, coordination sites, as well as the products released during thermal degradation of the complexes studied. Theoretical calculation of yttrium oxamate, as representative of all complexes was performed using density functional theory (DFT) for studying the molecular structure and vibrational spectrum of the investigated molecule in the ground state. The optimized geometrical parameters and theoretical vibrational spectrum obtained by DFT calculations are in good agreement with the experimental results.

Keywords: Lanthanides; Oxamic acid; Thermal analysis; DFT calculations

1. Introduction

The oxamic acid is composed of carboxyl group and primary amide group and molecular formula C₂H₃NO₃. It has molar mass of 89.05 g mol^-1, odorless, sublimates and melts partly around 140 ºC and it is found as a white solid.

The oxamic acid is well known as a versatile ligand and can act as di, tri or tetradentate (bridging) regarding its coordination modes, or as mono or dianion, when the charge is taken into account. When treated as a monoanion, it can coordinate by two of its oxygen atoms, forming a five-membered chelate ring, or by one oxygen atom (from the carboxylate group) and the nitrogen (amide group). Still as a monoanion it can act as a monodentate ligand using one oxygen atom from the carboxylic group; or as a tridentate ligand using all of its oxygen atoms. In the dianion form, when it loses of its ionisable hydrogens, it can act as a chelate bidentate or bridging ligand, and also as bridging tetradentate ligand in binuclear complexes, which also can contain other multidentate chelate ligands¹.

A few studies about complexes involving lanthanides and oxamic acid are found in the literature. Two of them describe the synthesis, the determination of physical properties, spectroscopic studies and thermal behavior of lanthanide (III) oxamates^2,3. The others reported the crystal structure determination of the oxamate praseodymium, neodymium, and holmium^1,4,5.

The present paper reports the preparation of solid-state complexes of heavy trivalent lanthanides with oxamate and the investigation by means of complexometry, elemental analysis, simultaneous thermogravimetry and differential scanning calorimetry (TG-DSC), TG-DSC coupled to FTIR, powder X-ray diffraction (PXRD) and infrared spectroscopy (FTIR). DFT calculations were performed in order to compare and support the experimental results. This work is primarily a continuation and extension of the reported study on the thermal behavior of light trivalent lanthanide oxamates⁶.

2. Experimental

The oxamic acid, H₂NCOCOOH, with 99% purity was obtained from Sigma and used as received.

The basic carbonates of heavy trivalent lanthanides (Tb to Lu) and yttrium (III) were prepared following the procedure described in the literature⁶.

Solid-state heavy trivalent lanthanide and yttrium oxamates were prepared following the literature method⁶: Under stirring, slight excess of the corresponding metal basic carbonate was added to 50 mL of an aqueous suspension of oxamic acid 0.15 mol L^-1.

For the solid-state complexes, metal ions, hydration water, and oxamate contents were determined from TG curves. The metal ions were also determined by complexometry with standard EDTA solution after igniting the complexes to the respective oxides and their dissolution in hydrochloric acid solution⁶.

Carbon, hydrogen and nitrogen contents were determined by microanalytical procedures, with a CHN Elemental Analyzer from Perkin Elmer, model 2400.

Simultaneous TG-DSC curves were obtained in a Mettler Toledo TG-DSC 1 thermal analysis system. The purge gas was dry air with flow of 50 mL min^-1. Heating rate of 10 ºC min^-1 was used, with samples weighing about 7.0 mg. Alumina crucibles were used for recording the TG-DSC curves.

The evolved gas analysis (EGA) was performed using a Mettler TG-DSC thermogravimetric analyzer coupled to a Nicolet FTIR spectrophotometer with gas cell and DTGS KBr detector. The TG furnace and heated gas cell (250 ºC) were coupled through a heated (225 ºC) 120 cm stainless steel line transfer with diameter of 3.0 mm, both purged with dry air (50 mL min^-1). The FTIR spectra were recorded with 16 scans per spectrum at a resolution of 4 cm^-1.

X-ray powder diffraction (XRPD) data were obtained by using a Siemens D-5000 X-Ray Diffractometer employing CuKα radiation (λ = 1.541 Å) and setting of 40 kV and 20 mA.

The attenuate total reflectance infrared spectra of sodium oxamate as well as of its metal-ion complexes were recorded using a Nicolet iS10 FTIR spectrophotometer, using an ATR accessory with a Ge window. The FTIR spectra were recorded with 32 scans per spectrum at resolution of 4 cm^-1.

2.1. Computational strategy

In this study, the quantum chemical approach employed to determine the molecular structures was Becke's three parameter hybrid theory⁷ using the Lee-Yang-Par (LYP) correlation functional⁸, and the basis sets used for calculations were: 4s for H (²S)⁹, [5s4p] for C (³P), N (⁴S) and O (³P) (9), and [14s7p7d] for Y (²D)¹⁰. The diffuse functions for the yttrium atom (²D) were calculated according to the procedure described by Teu-Filho et al.⁹ and these values are: αs = 0.007007235, αp = 0.991840315, αd = 0.008880095. Full details about the wave function developed in this work are available upon request to the e-mail address: [e-mail].

In order to better describe the properties of the complex in the implementation of the calculations, it was necessary to include polarization functions ^9-11 for all atoms of the complex. The polarization functions are: αp = 0.33353749 for H (²S), αd = 0.72760279, αd = 0.35416230 αd = 0.36059494 for C (³P), N (⁴S) and O (³P), respectively, and αf = 0.394056689 for Y (²D) atoms. The role of a basis set is crucial in theoretical studies of metal complexes, since the description of the metal configuration in the complex differs from the neutral state. The performed molecular calculations in this study were made using the Gaussian 09 routine¹².

The theoretical infrared spectrum was calculated using a harmonic field¹³ based on C₁ symmetry (electronic state ¹A). Frequency values (not scaled), relative intensities, assignments, and description of vibrational modes are presented. The geometry optimization was computed using the optimized algorithm of Berny¹⁴ and the calculations of vibrational frequencies were also implemented to determine if the optimized geometry constitutes minimum or saddle points . The principal infrared active fundamental mode assignments and descriptions were done by the GaussView 5.0.2 W graphics routine¹⁵.

3. Results and Discussion

3.1. Analytical results

The analytical and thermoanalytical (TG) results for the synthesized complexes are shown in Table 1. The analytical results are in good agreement with the thermoanalytical ones, evidencing that the complexes were obtained in a high degree of purity. From the results, it was possible to establish the stoichiometry of the complexes, which is in agreement with the general formula: Ln(L)₃∙nH₂O, where Ln represents heavy trivalent lanthanides, L is oxamate and n = 1 (Dy, Ho, Y); 1.25 (Er); 1.5 (Tb and Lu); 2 (Tm) and 2.5 (Yb).

Table 1
Analytical and thermoanalytical (TG) data for Ln(L)₃∙nH₂O complexes.

Complexes	Ln (oxide)/ %		L (lost)/ %			H2O/ %		C/ %		H/ %		N/ %		Final Residue
	Calc.	EDTA	TG	Calc.	TG	Calc.	TG	Calc.	EA	Calc.	EA	Calc.	EA
Tb(L)3∙1.5H2O	39.77	39.50	39.77	52.21	52.64	6.01	5.57	16.01	16.01	2.02	2.02	9.34	9.34	Tb4O7
Dy(L)3∙1H2O	41.95	41.50	41.02	54.00	54.67	4.05	4.31	16.21	16.47	1.82	1.85	9.45	9.61	Dy2O3
Ho(L)3∙1H2O	42.26	42.06	42.31	53.71	53.81	4.03	3.88	16.12	16.10	1.81	1.81	9.40	9.39	Ho2O3
Er(L)3∙1.25H2O	42.14	41.87	41.36	52.90	53.52	5.90	5.12	15.88	16.09	1.89	1.92	9.26	9.38	Er2O3
Tm(L)3∙2H2O	41.13	40.97	41.18	51.19	51.53	7.68	7.29	15.36	15.35	2.15	2.15	8.96	8.95	Tm2O3
Yb(L)3∙2.5H2O	40.86	40.39	40.51	49.79	50.37	9.34	9.12	14.94	15.03	2.30	2.32	8.72	8.77	Yb2O3
Lu(L)3∙1.5H2O	42.69	42.40	42.83	51.52	51.39	5.80	5.78	15.46	15.42	1.95	1.95	9.02	8.99	Lu2O3
Y(L)3∙1H2O	30.43	30.20	30.46	64.71	64.64	4.86	4.90	19.42	19.41	2.18	2.18	11.33	11.32	Y2O3

• L: oxamate.

3.2. Thermal analysis (TG-DSC and EGA)

The simultaneous TG-DSC curves of the complexes are shown in Figure 1. In all complexes, the TG curves show mass losses in four consecutive and/or overlapping steps, although the DSC curves show that the thermal decomposition occurs with a large number of consecutive and/or simultaneous steps and through a more complex pathway than that observed in the TG curves. The mass losses corresponding to endothermic peaks are attributed to the dehydration or thermal decomposition and the exothermic ones to the oxidation of the organic matter and/or of the gaseous products evolved during the thermal decomposition.

Figure 1
Simultaneous TG-DSC curves of the complexes: (a) Tb(L)₃∙1.5H₂O, (b) Dy(L)₃∙1H₂O, (c) Ho(L)₃∙1H₂O, (d) Er(L)₃∙1.25H₂O, (e) Tm(L)₃∙2H₂O, (f) Yb(L)₃∙2.5H₂O, (g) Lu(L)₃∙1.5H₂O and (h) Y(L)₃∙1H₂O.

The thermal decomposition reaction interval (I) from anhydrous complexes and final temperature of thermal decomposition (II) as shown by the curves TG-DSC depends on the nature of the metal ion and they follow the order:

$\begin{array}{c}\left(I\right)\mathrm{Ho}\mathbf{>}Y\mathbf{=}\mathrm{Er}\mathbf{=}\mathrm{Dy}\mathbf{>}\mathrm{Lu}\mathbf{>}\mathrm{Tm}\mathbf{>}\mathrm{Yb}\mathbf{>}\mathrm{Tb}\hfill \\ \left(\mathrm{II}\right)\mathrm{Er}\mathbf{>}\mathrm{Ho}\mathbf{>}\mathrm{Lu}\mathbf{=}Y\mathbf{>}\mathrm{Dy}\mathbf{>}\mathrm{Tm}\mathbf{>}\mathrm{Yb}\mathbf{>}\mathrm{Tb}\hfill \end{array}$

A great similarity is observed in the profiles of the TG curves, except for the terbium complex. On the other hand, the profiles of the DSC curves show great similarity for two sets of complexes (Tb, Dy, Ho and Tm, Yb) and particular ones for the other complexes (Er, Lu and Y), as also observed in all DSC curves of the trivalent light lanthanide oxamates⁶. Thus, the features of each complex are discussed based on their similar thermal profiles from TG curves.

Terbium complex

The TG-DSC curves of the complex are shown in Figure 1 (a). These curves show mass losses in four steps and thermal events corresponding to these losses. The first mass loss that occurs through a slow process corresponding to an endothermic peak is attributed to dehydration.

The thermal decomposition of the anhydrous complexes occurs in three steps immediately after the dehydration and the first two mass losses corresponding to endothermic peaks are attributed to the thermal decomposition and an exothermic peak due to the oxidation of organic matter and/or of the gaseous products evolved in the thermal decomposition, with the formation of terbium oxide, Tb₄O₇. The last mass loss between 900 and 940 ºC corresponding to an endothermic peak at 910 ºC is attributed to reduction reaction of Tb₄O₇ to Tb₂O₃, as already observed in other studies^16,17.

Dysprosium to lutetium and yttrium

The TG-DSC curves of these complexes are shown in Figure 1 (b - h). These curves also show mass losses in four steps and thermal events corresponding to these losses. The first mass loss that occurs slowly corresponding to an endothermic peak (Ho, Tm, Y), and two (Dy) or three endothermic peak (Yb, Lu) is attributed to dehydration.

After the dehydration, the thermal decomposition of the anhydrous complexes occurs in three steps. The first two - corresponding to endothermic peaks - are attributed to the thermal decomposition, and the last - associated with an exothermic peak - is attributed to the oxidation of organic matter and/or of the gaseous products evolved in the thermal decomposition, with the formation of a mixture of carbonaceous residue and a derivative of carbonate. Tests with hydrochloric acid solution on samples heated up to the temperature of formation of this mixture, as indicated by the corresponding TG-DSC curves confirmed the formation of carbonate by the evolution of CO₂ and the presence of carbonaceous residue. The formation of carbonaceous residue and of derivative of carbonate had already been observed in the thermal decomposition of some light trivalent lanthanide oxamates⁶ and other lanthanide complexes^18,19.

The last mass loss corresponding to no thermal events (Dy, Lu), small endothermic peak (Ho) or exothermic peaks (Er, Tm, Yb, Y) is attributed to oxidation of carbonaceous residue (exo) and thermal decomposition of the derivative of carbonate (endo). Calculations based on the mass losses observed in the TG curves are in agreement with the formation of the respective oxides, Ln₂O₃ (Ln = Tb to Lu and Y) and confirmed by X-ray powder patterns.

In spite of the similarity in the TG profiles of these complexes, the temperature ranges (θ), mass losses (m) and temperature peaks (p) observed in each steps of the TG-DSC curves are characteristic of each complex, and for that reason this information is provided in Table 2.

Table 2
Temperature ranges (θ), mass losses (Δm) and peak temperatures (Tp) observed for each step of TG-DSC curves of the complexes.

Complexes	TG-DSC Steps					ΔmTotal
		First	Second	Third	Fourth
Tb(L)3∙1.5H2O	θ/ ºC	55 - 205	205 - 370	370 - 600	900 - 940	59.36
	Tp/ ºC	170↓	250↓, 340↓	450↑	910↓
	Δm/ %	5.57	27.06	25.36	1.37
Dy(L)3∙1H2O	θ/ ºC	55 - 190	190 - 360	360 - 530	530 - 670	58.98
	Tp/ ºC	120↓sm, 160↓sm, 175↓sm	285↓, 340↓	435↑	-
	Δm/ %	4.31	26.14	24.36	4.17
Ho(L)3∙1H2O	θ/ ºC	55 - 190	190 - 370	370 - 500	500 - 690	57.69
	Tp/ ºC	132↓, 155↓sh	250↓, 285↓sh, 340↓	415↓, 440↑	680↓
	Δm/ %	3.88	27.11	21.92	4.78
Er(L)3∙1.25H2O	θ/ ºC	55 - 220	220 - 385	385 - 530	530 - 700	58.64
	Tp/ ºC	-	340↓	410↓, 435↑	660↑
	Δm/ %	5.12	28.21	21.42	3.89
Tm(L)3∙2H2O	θ/ ºC	100 - 215	215 - 370	370 - 500	500 - 630	58.82
	Tp/ ºC	125↓, 162↓, 180↓sh	330↓	390↓, 435↑	605↑
	Δm/ %	7.29	26.95	20.52	4.06
Yb(L)3∙2.5H2O	θ/ ºC	100 - 210	210 - 365	365 - 470	470 - 620	59,49
	Tp/ ºC	140↓, 160↓, 205↓	290↓, 325↓	390↓, 425↑	580↑
	Δm/ %	9.12	27.08	19.38	3.91
Lu(L)3∙1.5H2O	θ/ ºC	55 - 220	220 - 385	385 - 470	470 - 680	57.17
	Tp/ ºC	145↓, 170↓, 185↓	262↓sh, 300↓, 330↓sh	400↓, 440↑	-
	Δm/ %	5.78	28.69	19.30	3.40
Y(L)3∙1H2O	θ/ ºC	50 - 200	200 - 370	370 - 510	510 - 680	69.54
	Tp/ ºC	130↓, 155↓ sh	260↓, 295↓sh, 340↓	420↓, 445↑	640↑
	Δm/ %	4.90	32.62	26.52	5.50

• L = oxamate; sm = small; sh = shoulder; ↓ = endothermic; ↑ = exothermic.

EGA

The Gram-Schmidt curves (GS) and the IR spectra of the gaseous products released during the thermal decomposition of the thulium complex, as representative of all the complexes, are presented in Figure 2. In general, GS curves are very similar to DTG curves (^{supplementary material}), and thus their profiles can be correlated to the number of mass loss steps. The differences that may arise between them are probably due to the fact that GS curve profile is related to the molar absorption coefficient of the molecules of gases while the DTG curve is related to mass variation. The GS curve shows four maximum-intensity regions, and the second consisting of two maximum values (two peaks). This suggests that the thermal decomposition takes place in at least four steps, and can be confirmed by inspecting the second mass loss in the TG curve, that is formed by at least two overlapping steps, as confirmed by the DTG curve. In addition, the GS curve shows that all steps are superposed, in agreement with the TG/DTG-DSC curves.

Figure 2
(a) Gram-Schmidt curve and (b) IR spectra of gaseous products evolved during the thermal decomposition of the yttrium complex.

The gases released during the thermal decomposition were identified based on FTIR reference spectra available in the spectrometer's software database and analysis of the frequencies of the vibrational modes. The spectra obtained up to approximately 200 ºC show characteristic bands of water vapor (ν O-H in the range 4000-3400 cm^-1 and δ O-H in the range of 2060 to 1260 cm^-1) attributed to dehydration of the complexes, as indicated by curves TG-DSC. Above 200 ºC, the main gas species identified were ammonia (characteristic bands at 3334 cm^-1 (νNH₃) and 1626, 966 cm^-1 (δNH₃), CO₂ (characteristic absorption bands at 2355 and 2311 cm^-1 ( νCO₂) and 669 cm^-1 (δ CO₂); CO (characteristic band at 2154 cm^-1 (ν CO)); N₂O (characteristic band at 2220 cm^-1), HCN (bands at 3300 cm-1 (ν C-H and 712 cm^-1 (δ HCN)).

Spectrum obtained at 600 ºC shows characteristic bands of CO₂ molecule, in accordance with the decomposition of the carbonate derivative with formation of thulium oxide.

3.3. Molecular modeling and vibrational spectroscopy in the infrared region

The calculated geometries are shown in Figure 3. Theoretical calculations showed that the structure in Fig 3a (isomer 1) is 10.90, 22.24 and 34.86 kcal mol^-1 more stable than the structures 3b (isomer 2), 3c (isomer 3) and 3d (isomer 4) respectively. These theoretical results suggest that the ligand oxamate coordinates to the metal center in a bidentate mode, by one of the oxygen atoms from the carboxylate group and the oxygen atom of the amide group forming a chelate five membered ring (Figure 3a), agreeing with the structure determined by single crystal X-ray diffraction¹. The structural parameters obtained from the most stable structure are shown in the supplemental material (Table S1).

Figure 3
Optimized geometric structure of the Y(L)3: (a) Isomer 1 (more stable), (b) isomer 2, (c) isomer 3 and (d) isomer 4.

The vibrational spectra in the infrared region of the oxamic acid, sodium oxamate, lanthanide complex and the calculated from the more stable structure of the yttrium complex are shown in Figure 4.

Figure 4
IR spectra of (a) oxamic acid, (b) sodium oxamate and of the complexes of: (c) Tb, (d) Dy, (e) Ho, (f) Er, (g) Tm, (h) Yb, (i) Lu, (j) Y and (l) Y theoretical.

The assignments were made based on theoretical calculations and also on the existing literature^20,21 and are presented in Table 3.

Table 3
Main vibrational frequencies in infrared of the oxamate complexes of lanthanides and yttrium.

Assignments	Frequencies
	Tb	Dy	Ho	Er	Tm	Yb	Lu	Y	Y*
ν O - H (H2O)	3394m,br	3390m,br	3213m,br	3307m,br	3208m,br	3208m,br	3220m,br	3226m, al
νas NH2	overlapped	overlapped	overlapped	overlapped	3443m	3442m	3442m	overlapped	3646, 3644, 3643
νs NH2	overlapped	overlapped	overlapped	overlapped	3372m	3376m	3381m	overlapped	3497, 3496, 3495
νas COO +δs NH2	1702sh	1701sh	overlapped	overlapped	overlapped	overlapped	overlapped	overlapped	1758, 1738, 1737
ν C = O (CONH2, Amide I band)	1638vs	1638vs	1639vs	1641vs	1633vs	1661vs	1653vs	1638vs	1699, 1686, 1683
δs NH2	overlapped	overlapped	overlapped	overlapped	overlapped	overlapped	overlapped	overlapped	1567, 1566
δs NH2 + ν C - N	1442w	1447w	1434w	1452w	1461w	1427w	1426w	1437w	1428, 1426, 1425
νs COO- +δs NH2	1318m	1320m	1317m	1342m	1341m, 1308m	1342m, 1310m	1351m, 1322m	1318m	1300, 1295, 1291
ρ NH2 + ν C = O (amide) + ν C - N	1092vw	1091vw	1093vw	1098vw	1110vw, 1091vw	1110vw, 1093vw	1094vw	1098vw	1105, 1104, 1102

• ^*
  theoretical; δ_s: symmetrical angular in plane deformation; ρ: asymmetric angular in plane deformation; L: oxamate; br: broad; vw: very week; w: week; m: medium; s: strong; vs: very strong.

Comparative analysis of some bands observed in the experimental and theoretical spectra shows: (i) a band at 1683 cm^-1, while the theoretical result shows the corresponding peak at 1744 cm^-1 with 3.62% discrepancy; (ii) a very strong band at 1638 cm^-1, while the theoretical spectrum shows the band corresponding to 1689 cm^-1, resulting in a 3.11% discrepancy; and (iii) a strong band at 1318 cm^-1, while the theoretical result shows the corresponding band in at 1295 cm^-1, a 1.75% discrepancy. The theoretical results are in very good agreement with the experimental data suggesting that the structure shown in Figure 3a can represent or be close to the real structure.

Furthermore, as shown in Table 3, the asymmetric stretching frequency of the carboxylate group (νas COO^-) and the stretching frequency of the amide carbonyl group (νC = O, amide band) are shifted to the lower energy region (lower frequency) compared to the oxamic acid. These data suggest that both the amide group and the carboxylate group participate in the coordination. These experimental results are in agreement with theoretical calculations (Figure 3a) and with results of structure determination¹. It is possible to observe that the frequency values are close to those observed for the sodium salt, which suggests a higher ionic character of the bonds in these complexes, a characteristic property of rare earth complexes²².

3.4. PXRD

The X-ray diffractograms are presented in supplementary material (Figure S1). These results show that holmium and yttrium complexes were obtained with low degree of crystallinity. On the other hand, the complexes of Tb and Lu were obtained with high degree of crystallinity and the diffractograms for the complexes Tm, Yb and Lu suggest the formation of an isomorphous series.

4. Conclusion

The oxamates of heavy trivalent lanthanides and yttrium were synthesized and characterized by TG-DSC, vibrational spectroscopy in the infrared region (IR), elemental analysis, powder X-ray diffraction and EDTA complexometric titrations.

Based on the TG curves, elemental analysis and complexometric titration results, a general empirical formula could be established for the synthesized complexes as Ln(L)₃∙nH₂O, in which Ln represents heavy trivalent lanthanides, L is oxamate and n = 1 (Dy, Ho, Y); 1.25 (Er); 1.5 (Tb and Lu); 2 (Tm) and 2.5 (Yb).

Simultaneous TG-DSC curves provided information about the thermal behavior of these complexes: dehydration, thermal stability and thermal decomposition steps.

The main gaseous products released during the thermal decomposition were identified as ammonia, hydrogen cyanide, nitrous oxides, CO₂ and CO.

The experimental and theoretical infrared spectroscopic data suggest that the oxamate acts as a chelating bidentate ligand to the metal ions through the oxygen of the amide and carboxylate groups. Furthermore, the great similarity between the experimental infrared spectra for all the complexes suggests that all are coordinated in the same way.

5. Acknowledgements

The authors thank FAPESP, CNPq and CAPES Foundations (Brazil) for financial support. This research was supported by resources supplied by the Center for Scientific Computing (NCC/Grid UNESP) of the São Paulo State University (UNESP), Instituto de Química de Araraquara, UNESP Campus de Araraquara and CENAPAD-UNICAMP.

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Supplementary material

The following online material is available for this article:

Table S1. Selected optimized geometrical parameters for the yttrium complex in the ground state calculated at B3LYP levels.

Figure S1. X-ray powder diffraction patterns of the compounds: (a) Tb(L)₃∙1.5H₂O, (b) Dy(L)₃∙1H₂O, (c) Ho(L)₃∙1H₂O, (d) Er(L)₃∙1.25H₂O, (e) Tm(L)₃∙2H₂O, (f) Yb(L)₃∙2.5H₂O, (g) Lu(L)₃∙1.5H₂O and (h) Y(L)₃∙1H₂O.

Publication Dates

• Publication in this collection
  22 June 2017
• Date of issue
  Jul-Aug 2017

History

• Received
  01 Sept 2016
• Reviewed
  18 Apr 2017
• Accepted
  21 May 2017