Synthesis, Crystal Structures, and Magnetic Properties of Lanthanide (III) Amino-Phosphonate Complexes

Two isostructural lanthanide amino-phosphonate complexes [Ln10(μ3-OH)3(μ-OH)(CO3)2 (O2CBu)15(O3PC6H10NH2)3(O3PC6H10NH3)2(H2O)2][Et2NH2] (Ln = Gd(III), 1 and Tb(III), 2) have been obtained through reflux reactions of lanthanide pivalates with, a functionalized phosphonate, (1-amino-1-cyclohexyl)phosphonic acid and diethylamine (Et2NH) in acetonitrile (MeCN) at 90 ◦C. Both compounds have been characterized with elemental analysis, single-crystal X-ray diffraction methods, and magnetic measurements. The molecular structure of compounds 1 and 2 reveal two highly unsymmetrical complexes comprising ten lanthanide metal centers, where the lanthanide metal ion centers in the cages are linked through pivalate units and further interconnected by CPO3 tetrahedra to build the crystal structure. The magnetic behavior of 1 and 2 was investigated between ambient temperature and ca. 2 K, the magnetic measurements for compound 1 suggests antiferromagnetic interactions between the Gd(III) metal ion centers at low temperatures. The large number of isotropic Gd(III) ions comprising 1 makes it a candidate for magnetocaloric applications, thus the magnetocaloric properties of this molecular cage were investigated indirectly through isothermal magnetisation curves. The magnetic entropy change was found to be 34.5 J kg−1K−1, making 1 a plausible candidate in magnetic cooling applications.


Introduction
In recent years, research involving metal phosphonates has been deeply explored because of the great variety of building blocks available for the preparation of functional materials useful in the field of structural chemistry and magnetic properties [1][2][3][4][5][6][7].Phosphonic acid and its derivatives are flexible coordination ligands towards a wide range of metal ions, with various ionic radii, including Ln(III) ions, resulting in some materials with promising magnetic properties [8][9][10][11].
4f-phosphonate molecular cages have been studied because of the magnetic anisotropies of the lanthanide ions and the weak coupling between the metal ions can produce interesting properties [12].When the isotropic Gd(III) metal ion is present, lanthanide phosphonate clusters display impressive magnetocaloric effects (MCE), which have been suggested for application in magnetic refrigeration [13].Lanthanide phosphonates with structural diversity and related physical and chemical properties could be obtained by modifying phosphonates with different functional organic groups, such as crown ether [14][15][16][17][18], carboxylate [19][20][21][22][23], pyridyl, amino and hydroxyl [24][25][26][27][28][29][30][31][32], etc.Much of recent work has so far focused on the exploration of metal phosphonate materials with new structural types, and a large number of metal phosphonates were prepared through designing and synthesizing phosphonic Magnetochemistry 2018, 4, 29; doi:10.3390/magnetochemistry4030029www.mdpi.com/journal/magnetochemistryacids with different functional organic groups [7,[33][34][35][36][37].More recently, a series of metal phosphonates, using phosphonic acids containing -NH 2 sub functional group were also isolated under solvothermal condition [38,39].So far, only few 4f-aminophosphonate molecular cages have been reported, the incorporation of the amino group into a phosphonate ligand could provide additional coordination sites for the metal ions and influence the packing of the structures through weak interactions such as hydrogen-bond interactions [8][9][10][11].The first lanthanide aminophosphonate, Lu(HO 3 PCH 2 CH 2 NH 3 ) 3 (ClO 4 ) 3 •3D 2 O was reported by Legendziwicz et al. in 1999 [40,41].Due to 4f-phosphonate low solubility in water and other organic solvents as well as their poor crystallinity, it is still a difficult task to obtain single crystals suitable for X-ray structural analysis [12,13].These problems can be solved by two methods: (1) introducing polar functional groups into the ligand, such as hydroxy, amino, carboxylate, or crown ether [42][43][44][45]; and (2) introducing a second ligand such as pivalic acid or oxalic acid [41,42].The introduction of the second ligand is to improve the crystallization of the products, to mediate the electronic effects between paramagnetic metal centers and to link the metal centers into various structures with dimensionalities extending from zero to three [46][47][48].
So far, only few 4f-aminophosphonate molecular cages have been reported, the incorporation of the amino group into a phosphonate ligand could provide additional coordination sites for the metal ions and influence the packing of the structures through weak interactions such as hydrogen-bond interactions [8][9][10][11].The first lanthanide aminophosphonate, Lu(HO3PCH2CH2NH3)3(ClO4)3•3D2O was reported by Legendziwicz et al. in 1999 [40,41].Due to 4f-phosphonate low solubility in water and other organic solvents as well as their poor crystallinity, it is still a difficult task to obtain single crystals suitable for X-ray structural analysis [12,13].These problems can be solved by two methods: (1) introducing polar functional groups into the ligand, such as hydroxy, amino, carboxylate, or crown ether [42][43][44][45]; and (2) introducing a second ligand such as pivalic acid or oxalic acid [41,42].The introduction of the second ligand is to improve the crystallization of the products, to mediate the electronic effects between paramagnetic metal centers and to link the metal centers into various structures with dimensionalities extending from zero to three [46][47][48].

Syntheses of the Complexes
Phosphonates of general formula RPO3 are well-known as binding groups for molecular metal clusters by using large R groups or co-ligands that inhibit formation of polymeric materials.Previous studies have shown that the phosphonate moiety is an efficient functional group for the construction of molecular cages [38,39].Winpenny and co-workers reported results using t-butylphosphonic acid (H2O3P t Bu) reacted with lanthanide salts Ln(NO3)3•nH2O or lanthanide pivalates (Ln = Gd(III), Tb(III), Dy(III), Ho(III), and Er(III) [12,13,39].Winpenny and coworkers have also synthesized a decanuclear 3d-4f phosphonate cage of [Co4Ln10(O2C t Bu)12(O3PC6H10NH2)8(PO4)2(O2CMe)2(O3PC6H10NH3)2] (Ln = Gd, Dy) [38].The molecule crystallizes in a triclinic space group and contains ten lanthanides, twelve phosphonates, and four cobalt metal ions.The {Ln10P12} core can be described as two centered 12vertex polyhedra sharing a face, the phosphonates present three different coordination modes of

Syntheses of the Complexes
Phosphonates of general formula RPO 3 are well-known as binding groups for molecular metal clusters by using large R groups or co-ligands that inhibit formation of polymeric materials.Previous studies have shown that the phosphonate moiety is an efficient functional group for the construction of molecular cages [38,39].Winpenny and co-workers reported results using t-butylphosphonic acid (H 2 O 3 P t Bu) reacted with lanthanide salts Ln(NO 3 ) 3 •nH 2 O or lanthanide pivalates (Ln = Gd(III), Tb(III), Dy(III), Ho(III), and Er(III) [12,13,39] (Ln = Gd, Dy) [38].The molecule crystallizes in a triclinic space group and contains ten lanthanides, twelve phosphonates, and four cobalt metal ions.The {Ln 10 P 12 } core can be described as two centered 12-vertex polyhedra sharing a face, the phosphonates present three different coordination modes of 6.222, 4.2111 (Ln = Dy, Gd).The compounds are isostructural and contain an anionic {Ln 10 } cage co-crystallized with a [Co 3 (µ 3 -O)(O 2 CtBu) 6 (py) 3 ] + cation, the anion of the compound contains nine Ln(III) metal ions in a ring and a tenth Ln(III) metal ion at the center of the structure, the ten metal sites are almost co-planar.Three of the six phosphonates lie below the plane of the {Ln 10 } disc and adopt the 4.221 binding mode, the remaining three phosphonates are above the plane of metal centers; two of them adopt the 3.111 binding mode, while the third adopts the 3.211 mode [52].Another frequently used ligand to the polynuclear 4f molecular cages is α-amino acids [42][43][44][45], thus 1-amino-1-cyclohexyl phosphonic acid is supposedly a good ligand to synthesize 4f molecular cages (Figure 2) [38,39].Herein the use of an aminophosphonic acid ligand to synthesize two 4f-phosphonate clusters is provided.The reactions have been performed by refluxing a mixture of lanthanide pivalate [Ln 2 (O 2 C t Bu) 6 (HO 2 C t Bu) 6 ] (Ln = Gd(III); Tb(III)), (1-amino-1-cyclohexyl) phosphonic acid (H 2 O 3 PC 6 H 10 NH 2 ), and a mild base, Et 2 NH in MeCN in the mole ratios 0.1:0.5:0.01.6.222, 4.2111, and 3.1111.More recently, Winpenny and co-workers also reported two cages of centered nine-metal rings of lanthanides [Co3(μ3-O)(O2C t Bu)6(py)3][Ln10(O2C t Bu)18(O3P t Bu)6(OH) (H2O)4] (Ln = Dy, Gd).The compounds are isostructural and contain an anionic {Ln10} cage cocrystallized with a [Co3(μ3-O)(O2CtBu)6(py)3] + cation, the anion of the compound contains nine Ln(III) metal ions in a ring and a tenth Ln(III) metal ion at the center of the structure, the ten metal sites are almost co-planar.Three of the six phosphonates lie below the plane of the {Ln10} disc and adopt the 4.221 binding mode, the remaining three phosphonates are above the plane of metal centers; two of them adopt the 3.111 binding mode, while the third adopts the 3.211 mode [52].Another frequently used ligand to the polynuclear 4f molecular cages is α-amino acids [42][43][44][45], thus 1-amino-1-cyclohexyl phosphonic acid is supposedly a good ligand to synthesize 4f molecular cages (Figure 2) [38,39].Herein the use of an aminophosphonic acid ligand to synthesize two 4f-phosphonate clusters is provided.The reactions have been performed by refluxing a mixture of lanthanide pivalate [Ln2(O2C t Bu)6(HO2C t Bu)6] (Ln = Gd(III); Tb(III)), (1-amino-1-cyclohexyl) phosphonic acid (H2O3PC6H10NH2), and a mild base, Et2NH in MeCN in the mole ratios 0.1:0.5:0.01.

Description of the Structures
Compounds 1 and 2 both crystallize in the monoclinic space group P21/n and are isostructural, allowing us to describe compound 1 as representative.The compounds contain an anionic {Ln 10 } cage co-crystallized with a [Et 2 NH 2 ] + cation.The metal ions are highly irregular and are best described as a square sandwiched between two triangles (Figure 1, Figures S1 and S2) Compound 1 contains ten lanthanide(III) metal ion centers and the compound is held together by fifteen pivalates, two carbonates, three µ 3 -OH, and five (1-amino-1-cyclohexyl) phosphonic acid ligands.P1 and P2 bind to five Gd(III) metal ion centers; adopting a [ 5.2221] coordination mode (as described using Harris notation [53], see Figure 3), P3 and P4 bind to three Gd(III) metal ion centers; adopting [3.1110] and [3.211] coordination modes, respectively.While, P5 binds to four Gd(III) metal ion centers using the [4.2211] binding mode.The carboxylates adopt three different coordination modes, 2.11, 1.11, and 1. 10.There are three µ 3 -hydroxide centered gadolinium triangles formed by (Gd1, Gd2, Gd3), (Gd4, Gd5, Gd6), and (Gd7, Gd8, Gd9), while the two µ 3 -hydroxide centered gadolinium triangles that are defined by (Gd4, Gd5, Gd6) and (Gd7, Gd8, Gd9) lie parallel to each other and share two edges (Gd5-Gd6) and (Gd8-Gd9) with the central distorted square.Whereas, Gd10 is in a bridging position between the vertices Gd4 and Gd7.The phosphonate, pivalate, and carbonate oxygen atoms are intensively coordinated to the edges and the vertexes of the three µ 3 -OH centered triangles, for example, six oxygen atoms of the two carbonates bind to three vertexes and three edges of the three µ 3 -OH centered triangles.The carbonates must arise from the atmospheric CO 2 fixation [54][55][56][57].Two different geometries are adopted by the Gd(III) ions in the cluster: whilst Gd2, Gd3 Gd5, Gd6, Gd8, Gd9, and Gd10 exhibit a triangular dodecahedron (D 2d ) and a Continuous Shape Measure value (CShM) of 1.750, 2.422, 0.804, 2.505, 0.715, 3.236, and 2.316 respectively; Gd1, Gd4, and Gd7 adopt a less regular coordination (muffin, Cs, with a CShM value of 2.776, 1.238 and 1.569) [58].(Figure S3 and Table S1).The Gd• • • Gd distance in the edges of the triangles is ca.3.9 Å and the three µ 3 -OH groups are displaced about 0.81 Å out of the plane of the metal ions.The Gd• • • Gd distances within the central distorted square are in the range 4.0749(7)-4.8390(8)Å, whereas the distances between Gd10 metal ion and each of the vertexes Gd4 and Gd7 are in the range 7.0318(9)-6.3986(9)Å, respectively (Table S2).In the crystal, four molecules reside in the unit cell, which are held together through hydrogen bonds between the non-coordinated water molecules residing in the pockets on the crystals and the NH 2 groups of the aminophosphonic groups.Likewise, hydrogen bonding is also observed between the nitrogen of the MeCN solvents molecules and some terminal H 2 O molecules coordinated to the lanthanide ions.
Magnetochemistry 2018, 4, x FOR PEER REVIEW 4 of 11 Gd10 metal ion and each of the vertexes Gd4 and Gd7 are in the range 7.0318(9)-6.3986(9)Å, respectively (Table S2).In the crystal, four molecules reside in the unit cell, which are held together through hydrogen bonds between the non-coordinated water molecules residing in the pockets on the crystals and the NH2 groups of the aminophosphonic groups.Likewise, hydrogen bonding is also observed between the nitrogen of the MeCN solvents molecules and some terminal H2O molecules coordinated to the lanthanide ions.

Magnetic Properties
The temperature dependence of the magnetic susceptibility of 1 and 2 were determined by employing a SQUID magnetometer.Microcrystalline samples were suspended in n-eicosane and measured under a DC field of 1000 Oe in the temperature range comprising 2-300 K.The temperature dependence of the χMT(T) (where χM is the molar magnetic susceptibility) for 1 was 78.3 emu mol −1 K at 300 K (Figure 4a), this value is slightly lower than expected (calcd.78.7 cm 3 K mol −1 for ten Gd(III): gJ = 2, J = 7/2).Upon cooling, the χMT remains constant to ca. 75 K before falling rapidly to 54 cm 3 K mol −1 at 2 K due to the depopulation of the ligand field levels and/or the antiferromagnetic interactions.The high temperature flat region of the χMT curve hints very weak magnetic interaction between Gd(III) metal ion centers.The room temperature χMT value for complex 2 (Figure S4) is 118.3 cm 3 K mol −1 , in agreement with the spin only value (calcd.118.1 cm 3 K mol −1 for ten Tb(III): gJ = 3/2; J = 6).The curve decreases slowly with decreasing temperature down to about 100 K, before decreasing more rapidly.The continuing fall of χMT at all temperatures for compound 2 proposes an effect from the combined action of the crystal-field effect of the Tb(III) and the possibly antiferromagnetic exchange interaction between the metal ion centers.In addition, alternating current magnetic susceptibilities studied were carried out for compound 2 to probe the Single Molecule Magnet character (SMM), revealing no out-of-phase component, thus 2 is not an SMM.
Magnetization (M) versus field (H) plots from 2 to 9 K (Figure 4b) for compound 1 shows a steady increase that reaches 68.3 μB at 7 T at 2 K.This value approaches the saturation value for ten paramagnetic S = 7/2, g = 2 Gd(III) metal ion centers, calculated from the Brillouin function.As

Magnetic Properties
The temperature dependence of the magnetic susceptibility of 1 and 2 were determined by employing a SQUID magnetometer.Microcrystalline samples were suspended in n-eicosane and measured under a DC field of 1000 Oe in the temperature range comprising 2-300 K.The temperature dependence of the χ M T(T) (where χ M is the molar magnetic susceptibility) for 1 was 78.3 emu mol −1 K at 300 K (Figure 4a), this value is slightly lower than expected (calcd.78.7 cm 3 K mol −1 for ten Gd(III): g J = 2, J = 7/2).Upon cooling, the χ M T remains constant to ca. 75 K before falling rapidly to 54 cm 3 K mol −1 at 2 K due to the depopulation of the ligand field levels and/or the antiferromagnetic interactions.The high temperature flat region of the χ M T curve hints very weak magnetic interaction between Gd(III) metal ion centers.The room temperature χ M T value for complex 2 (Figure S4) is 118.3 cm 3 K mol −1 , in agreement with the spin only value (calcd.118.1 cm 3 K mol −1 for ten Tb(III): g J = 3/2; J = 6).The curve decreases slowly with decreasing temperature down to about 100 K, before decreasing more rapidly.The continuing fall of χ M T at all temperatures for compound 2 proposes an effect from the combined action of the crystal-field effect of the Tb(III) and the possibly antiferromagnetic exchange interaction between the metal ion centers.In addition, alternating current magnetic susceptibilities studied were carried out for compound 2 to probe the Single Molecule Magnet character (SMM), revealing no out-of-phase component, thus 2 is not an SMM.
Magnetization (M) versus field (H) plots from 2 to 9 K (Figure 4b) for compound 1 shows a steady increase that reaches 68.3 µ B at 7 T at 2 K.This value approaches the saturation value for ten paramagnetic S = 7/2, g = 2 Gd(III) metal ion centers, calculated from the Brillouin function.As observed in Figure 4b, at low fields the M(H) at 2 K is significantly lower than the Brillouin function, indicating that antiferromagnetic interactions could be operative within the clusters.For 2, M vs. H curve increase with increasing field, the plots of 2 and 4 K show a linear increase after 3 T that reaches 41.8 µ B at 7 T at 2 K without reaching saturation (Figure S5), this is the typical shape of M versus H plot that indicates significant magnetic anisotropy.Studies of the entropy changes from the magnetization data suggest the gadolinium-containing compounds could be suitable for low-temperature magnetic cooling (MCE), In this context, the high magnetization value obtained for compound 1 and the magnetic entropy change was studied to examine whether compound 1 could be used for magnetic cooling applications.The MCE can be described as ΔS = ʃ[ (T,H)/ HdH [49][50][51].The calculated plot (Figure 5) gives peak value for a field change ΔH = 70 kG of 3 K of 34.5 J kg -1 K -1 .The maximum entropy value per mole given by nRln(2S + 1) [n = 10 Gd(III) spins s = 7/2], corresponding to the sum of the individual contributions from the Gd(III) metal ion spins, is 47.9 J kg −1 K −1 .These values are not reached experimentally mainly because of the antiferromagnetic interactions between the metal centers in compound 1, which are known to decrease the magnetic entropy.

Starting Materials
Unless stated otherwise, all reagents and solvents were purchased from Aldrich Chemicals and used without further purification.(1-amino-1-cyclohexyl) phosphonic acid synthesized according to the reported method [59].[Ln2(O2C t Bu)6(HO2C t Bu)6] (Ln = Gd(III); Tb(III)) were synthesized following Studies of the entropy changes from the magnetization data suggest the gadolinium-containing compounds could be suitable for low-temperature magnetic cooling (MCE), In this context, the high magnetization value obtained for compound 1 and the magnetic entropy change was studied to examine whether compound 1 could be used for magnetic cooling applications.The MCE can be described as ∆S = [∂M(T,H)/∂T] H dH [49][50][51].The calculated plot (Figure 5) gives peak value for a field change ∆H = 70 kG of 3 K of 34.5 J kg -1 K -1 .The maximum entropy value per mole given by nRln(2S + 1) [n = 10 Gd(III) spins s = 7/2], corresponding to the sum of the individual contributions from the Gd(III) metal ion spins, is 47.9 J kg −1 K −1 .These values are not reached experimentally mainly because of the antiferromagnetic interactions between the metal centers in compound 1, which are known to decrease the magnetic entropy.Studies of the entropy changes from the magnetization data suggest the gadolinium-containing compounds could be suitable for low-temperature magnetic cooling (MCE), In this context, the high magnetization value obtained for compound 1 and the magnetic entropy change was studied to examine whether compound 1 could be used for magnetic cooling applications.The MCE can be described as ΔS = ʃ[ (T,H)/ HdH [49][50][51].The calculated plot (Figure 5) gives peak value for a field change ΔH = 70 kG of 3 K of 34.5 J kg -1 K -1 .The maximum entropy value per mole given by nRln(2S + 1) [n = 10 Gd(III) spins s = 7/2], corresponding to the sum of the individual contributions from the Gd(III) metal ion spins, is 47.9 J kg −1 K −1 .These values are not reached experimentally mainly because of the antiferromagnetic interactions between the metal centers in compound 1, which are known to decrease the magnetic entropy.

Starting Materials
Unless stated otherwise, all reagents and solvents were purchased from Aldrich Chemicals and used without further purification.(1-amino-1-cyclohexyl) phosphonic acid synthesized according to

Starting Materials
Unless stated otherwise, all reagents and solvents were purchased from Aldrich Chemicals and used without further purification.(1-amino-1-cyclohexyl) phosphonic acid synthesized according to the reported method [59].[Ln 2 (O 2 C t Bu) 6 (HO 2 C t Bu) 6 ] (Ln = Gd(III); Tb(III)) were synthesized following the reported procedure [60,61].Analytical data were obtained by the microanalytical service of the University of Manchester.The data and yields are given in Table 1.S6). a Calculated based on the lanthanide pivalate starting material; b Both samples were filtered and dried at room temperature before conducting the Elemental Analysis (EA).Despite this, the EA clearly suggests the presence of some solvent molecules in the lattice.

Magnetic Measurements
Magnetic measurements were performed in temperature ranges of 2-300 K, using a Quantum Design MPMS-XL7 SQUID magnetometer equipped with a 7 T magnet.The samples were grounded and placed in a gel capsule.Small amounts of eicosane have been used to avoid movement of the sample during the measurement.The diamagnetic corrections for the compounds were estimated using Pascal's constants, and the magnetic data were corrected for diamagnetic contribution of the sample holder.AC magnetic measurements were conducted for compound 2 employing an oscillating magnetic field of 1.55 Oe and under diverse DC fields.

Crystallographic Data Collection and Refinement
Data collection was carried out on Agilent SUPERNOVA diffractometer using graphite-monochromator MoKα radiation (λ = 0.71073 Å).A hemisphere of data was collected using a narrow-frame method with scan widths of 0.30o in ω and an exposure time of 10 s per frame.Data reduction and unit cell refinement were performed with CrysAlisPro software.The structures were solved by direct method using SHELXS-97 [61] and were refined by full-matrix least-squares calculations on F2 using the program Olex2 [62].Suitable crystals of 1 and 2 were selected under microscope and mounted on a tip using crystallographic oil and placed in a cryostream and used for data collection.All non-hydrogen atoms were refined anisotropically, all H atoms were put in calculated positions using riding model, and were refined isotropically, with the isotropic vibration parameters related to the non-H atom to which they are bonded.Large solvent accessible voids were found for complexes 1 and 2, however, the location of discrete solvent molecules could not be determined by simple refinement, and therefore the contents of the large voids on the crystal structure were determined using the solvent masking procedure SQUEEZE using Platon [63].Table 2 contains the molecular formula for 1 and 2 considering all solvent molecules found; i.e., the ones localized in the lattice and those determined by the SQUEEZE analysis.The crystallographic data for 1 and 2 are listed in Table 2. Selected bond lengths are given in Table S2.CCDC 1584149-1584150 contain the supplementary crystallographic data for 1 and 2 for this paper.

Conclusions
In summary, two new lanthanide 4f-aminophosphonate with structure [Ln 10 (µ 3 -OH) 3 (µ-OH)(CO 3 ) 2 (O 2 C t Bu) 15 (O 3 PC 6 H 10 NH 2 ) 3 (O 3 PC 6 H 10 NH 3 ) 2 (H 2 O) 2 ][Et 2 NH 2 ] (Ln = Gd(III); Tb(III)) have been successfully synthesized by using (1-amino-1-cyclohexyl)phosphonic acid ligand and pivalic acid as the second metal linker under reflux conditions at 90 • C for 4 h, both compounds are structurally and magnetically characterized.Compounds 1 and 2 are isostructural crystallizing in a monoclinic unit cell.Three different amino-phosphonate binding modes are found in the compounds.Previous results from our group and others indicate that the alkyl groups attached to the aminophosphonic acid has a strong effect on the structures and properties of the lanthanide(III) phosphonates isolated [38,39].The aminophosphonic acids, H 2 NRPO 3 H 2 (R = alkyl or aryl group), have been proved to be very useful ligands for the synthesis of metal phosphonates with new structure types in which the organic part plays a controllable spacer role and the two inorganic-PO 3 groups chelate with metal ions to form one-, two-, and three-dimensional structures [64,65].The entropy value for Gadolinium containing complex is 34.5 J kg −1 K −1 , this value being larger than the value of 32.3 J kg −1 K −1 of a previously studied octametallic 4f-phosphonate horseshoes complex {Gd 8 P 6 } [13] for a field change ∆H = 7 T at 3 K.Our future research efforts will be devoted to the syntheses, crystal structures, and magnetic properties of lanthanide(III) compounds of other related amino-phosphonate ligands.

Figure 3 .
Figure 3. Scheme for binding modes by Harris notation of the phosphonates and acetates in the clusters 1 and 2. Scheme: Ln, purple; P, light green; O, red; C, grey; N, cyan; H omitted for clarity.

Figure 3 .
Figure 3. Scheme for binding modes by Harris notation of the phosphonates and acetates in the clusters 1 and 2. Scheme: Ln, purple; P, light green; O, red; C, grey; N, cyan; H omitted for clarity.

Figure 5 .
Figure 5. Magnetic entropy changes for compound 1 calculated from isothermal magnetization measurements.

Figure 4 .
Figure 4. (a) Variation of χ M T vs. T for 1 at 1 kOe from 2-300 K; (b) M β vs. H for 1 at different temperatures (2-9 K) in the field range comprising 0 to 7 T. Dotted line is the Brillouin function at 2 K for ten isolated Gd(III) (g J = 2.00 and S = 7/2).

Figure 5 .
Figure 5. Magnetic entropy changes for compound 1 calculated from isothermal magnetization measurements.

Figure 5 .
Figure 5. Magnetic entropy changes for compound 1 calculated from isothermal magnetization measurements.