1. Introduction

2. Short theoretical background

3. Lanthanide complexes with tripodal ligands

3.2. Complexes with the pyridyl bearing tripodal ligand

Pyridine containing tripodal ligands have earlier been described [1]. Moreover, a diversity of bridgehead atoms such as nitrogen, carbon, and phosphorus [106], as well as other elements: Si [107], As [108], Al and In [109], Sn [110,111], Pb [112] and B [113] have been included to alter the properties of the coordination metal complexes both in terms of polyhedral geometry and to tune the electronic structure.

Strangely enough, structurally characterized complexes of the tris(2-pyridyl)methane class for lanthanides have not yet been obtained. Only a small group of exotic organometallic complexes based on tris(2-pyridyl)metallates that are unstable under normal conditions has been obtained and structurally characterized. This family of Ln-complexes will be briefly discussed in the next subparagraph of the review.

3.2.1. Complexes of tris(2-pyridyl)metallates

The most numerous group of Ln-complexes including tris(2-pyridyl)metallates are the coordination compounds of anionic tris(pyridyl)stannate (TPS) [114,115,116,117].

Interaction of [Ln(η⁵-C₅Me₅)₂(OEt₂)] with the lithium [LiSn(2-Py-5-Me)₃(thf)] in THF solution using a 1:2 ratio gives the sandwich like [Ln{Sn(2-Py-5-Me)₃}₂] (11) complexes for divalent Ln = Eu and Yb [114]. The formation of 11 displays a more pronounced steric demand of the tripodal stannate ligand than C₅Me_5. This is comparable with similar reactions of tris(pyrazolyl)hydroborates [HB(R₂pz)₃]⁻ (R = H, Me; pz = pyrazolyl) with [Ln(η⁵-C₅Me₅)₂] species giving the analogous Ln^II-complexes [Ln(HB(R₂pz)₃)₂] [114].

Both compounds 11 crystallize in the same space group P2₁2₁2₁ and have very close cell parameters. The molecular structure for europium complex is shown in Figure 3(11).

The Ln atoms of 11 are in a distorted octahedral coordination environment formed by six pyridyl nitrogens with a staggered organization of the pyridine rings around the Ln center. The coordination sphere around Ln is strongly distorted and the large size of the Ln atom affords a slight twisting of one of the pyridine rings of each Sn(2-Py-5-Me)₃ ligand unit around its Sn—C_py bond. Besides, the non-central location of the Ln atom in the cage is reflected by a bending of the Sn⋅⋅⋅Ln⋅⋅⋅Sn axis with 165.50(1)° and 167.28(13)° for Yb and Eu ions respectively [114]. The Sn bridgehead atom of the tripod reveals a trigonal pyramidal coordination mode (Figure 3(11), left).

The reaction of [LiSn(2-Py-5-Me)₃(thf)] with [Ln(η⁵-C₅Me₅)₂] precursors resulted in formation of the first Ln^II sandwich complexes 12 involving the anionic TPS in a κ³N-coordinating manner and featuring “naked” Sn^II centers, which can be used for following κ¹Sn-metal coordination (Eu complex is shown as example in Figure 3(12)) [114].

Compound 12 crystallizes in the cubic space group Pa$\overline{3}$ with the Eu²⁺ lying on a special crystallographic position and four molecules in the unit cell. The longer Eu—N, (2.611(3) Å) and Eu⋅⋅⋅Sn (3.8874(4) Å) distances of are consistent with the larger size of the Eu²⁺ vs Yb²⁺ cation in 11. The most pertinent feature is the Sn—Li contact of 2.792(12) Å in 12 is shorter than the covalent Sn—Li bond lengths (2.831–2.897 Å) [118]. Encapsulation of the large Eu²⁺ ion and additional κ¹Sn coordination of the two inner TPS ligands originates an opening of the tripodal structure (C-Sn-C = 99.6(1)°) compared to both outer TPS frameworks with “naked” Sn centers (C-Sn-C = 93.6(1)°) [114]. Furthermore, the κ¹Sn binding gives a practically ideal octahedral environment of the Eu²⁺ ion with a linear Sn⋅⋅⋅Eu⋅⋅⋅Sn axis (180.0(1)°).

Figure 3. Molecular structures (left) and octahedral coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 11-16. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

Figure 3. Molecular structures (left) and octahedral coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 11-16. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

The room temperature reactions of a trialkylmetallates MAlk₃ (Alk = Me for Al, and Et for Ga and In) with complex [Ln{Sn(2-Py-n-Me)₃}₂] gave the following organometallic species: [Eu{Sn(2-Py-4-Me)₃}₂{GaEt₃}₂] (13), Eu{Sn(2-Py-4-Me)₃}₂{InEt₃}₂] (14) and [Yb{Sn(2-Py-3-Me)₃}₂{AlMe₃}₂] (15) [115].

The compounds 13 and 14 (Figure 3) have the similar crystal structures crystallizing in the same space group C2/c [115], the Eu ions being in a distorted octahedral geometry, characteristic for the compounds 11 described above. In contrast with the complexes 11, the non-central location of the Ln ion in the coordination octahedron 13 and 14 is much less expressed in the bending of the Sn⋅⋅⋅Eu⋅⋅⋅Sn axis by 176.40(5)° and 172.05(8)° for 13 and 14, respectively. In the solid state, complex 15 (Figure 3) reveals bonding characteristics similar to those for 13 and 14, but differs in that the Yb ion possesses almost perfect octahedral environment with a strictly linear Sn⋯Yb⋯Sn axis (180.0°) [115].

A few words about the only sandwich compound of a lanthanide complex comprising tris(2-pyridyl)plumbate. The compound [Eu{Pb(2-Py-6-OtBu)₃}₂] (16) have been isolated from a concentrated THF solution [117]. Like 12, the complex 16 (Figure 3) crystallized in Pa$\overline{3}$ space group. The Eu²⁺ ion is coordinated by six nitrogen donor atoms of two tripodal with Eu—N bond length of 2.699(2) Å Eu⋅⋅⋅O distance of 4.0215(1) Å, which is greater than those of 2.611(3) and 3.501(3) Å in 12. This is because of a larger radius of bridgehead ion in Pb(2-Py-6-OtBu)₃ tripod. Although the cavity of the tripodal ligand offers an almost ideal octahedral coordination sphere for the Eu²⁺ cation, which is well encapsulated and clearly separated from the formally negatively charged lead bridgehead atoms, compound 16 is not stable in THF solution [117].

The EPR solution studies at ambient conditions for 16 in presence of nitrosobenzene (NOB) suggested the generation of a radical entity. The X-band EPR spectrum exhibits one broad signal corresponding to a Eu^II 4f⁷ spin system with the value g₀=1.989±0.001 and a line width of ΔB_PP=(31.0±0.1) mT. An identical EPR spectrum was obtained and without spin trap. In addition to a broad signal, the spectrum shows a triplet of multiplets. The well-resolved hyperfine structure (hfs) is due to the coupling of the unpaired electron with the ¹⁴N (I=1) nucleus and three groups of nonequivalent protons of NOB. The spectrum has been well simulated giving the values g₀=2.0057±0.0005 and a₀^N=(1.097±0.005) mT, as well as a₀^H=(0.249±0.005) mT, a₀^H=(0.235±0.005) mT, and a₀^H=(0.089±0.005) mT, respectively. The trapped radical was stable over a period of few hours. However, no ²⁰⁷Pb hfs coupling could have been observed, indicating radical-adduct formation.

The complexes comprising tris(pyridyl)aluminate (TPAl) tripods are completed this section. As was shown by R. García-Rodríguez et al. [119,120], complexes of Ln²⁺ with TPAl are air unstable and can only be obtained employing sterically hindered tripods - [(Alkyl)Al(2-Py-6-R)₃]⁻, where Alkyl = Et and R = Me or Br. It means that the coordination ability of TPAl can be adjusted by the steric and electronic character of substituents at a 6-position of the pyridyls. While [EtAl(2-py-6-Me)₃]⁻ (17) coordinates strongly to Ln²⁺ ions, [EtAl(2-py-6-Br)₃]⁻ (18) forms much weaker complexes, and [EtAl(2-py-6-CF₃)₃]⁻ does not coordinate at all [120]. Synthetic and structural investigations were devoted essentially to the complexes of two anions [EtAl(2-Py-6-Me)₃]⁻ and [EtAl(2-Py-6-Br)₃]⁻. The 2 : 1 ratio reactions of the 17 with LnI₂ (Ln = Eu, Yb and Sm) in thf at room temperature gives deep-orange (Eu) or purple (Yb and Sm) solutions after 24 h, indicating of Ln coordination [119,120]. SC-XRD study confirmed a formation of the sandwich complexes: [{Ln(EtAl(2-py-6-Me)₃}₂] (Ln = Sm 18, Eu 19, Yb 20) and [{Eu(EtAl(2-py-6-Br)₃}₂] (21), Figure 4. The complexes 18 and 21 crystallizes in P Ī space group. The first contains one CH₃C₆H₅ molecule as a solvate since it was crystalized from toluene. The coordination environment formed about the Sm and Eu are slightly elongated octahedron and trigonal antiprism respectively, although the both compounds have strait line passing through the bridgehead atoms of the tripods (Al-Ln-Al the angle is 180°). The compounds 19 and 20 crystallize in P 4₃2₁2 and P 2₁/n space groups correspondingly. Molecules of 19 and 20 feature six-coordinate, distorted-octahedral lanthanide metal ions with the N–Ln–N angles being approximately 90° and slightly bent Al–Ln–Al axis (177.17° (19) and 178.23° (20))[120].

Figure 3. Molecular structures (left) and coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 18-21. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

Figure 3. Molecular structures (left) and coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 18-21. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

None of the Ln compounds comprising tris(2-pyridyl)metallates have been reported on their magnetic behavior. The next fairly representative group of lanthanide compounds with tripodal ligands are complexes with tris(2-pyridyl)amines.

3.2.2. Complexes of tris(2-pyridyl)amines

The interaction of tris(2-pyridylmethyl)amine (TPA) with the precursors LnHal₃(thf)₄ and Ln(OTf)₃ was investigated in anhydrous environment and in the presence of water [3,7]. In the absence of water, the succeeding formation of mono- and bis-(TPA) complexes were detected using Ln/ligand ratio of 1 and 2, respectively. The mono-TPA complexes [Ce(TPA)I₃] (22) [3], [Ln(TPA)Cl₃] (Ln(III) = Eu, Tb, Lu ([7]), and the bis(tpa) complexes [Ln(TPA)₂]X₃ (X = I, Ln³⁺ = La, Ce, Nd, Lu [3] and Sm [6]; X = OTf, bis(tpa) complexes [Ln(TPA)₂]X₃ (X = I, Ln³⁺ = La, Ce, Nd, Lu [3] and Sm [6]; X = OTf, Eu [3]) were obtained under anhydrous conditions and their crystal structures were determined.

Figure 4. Molecular structures (left) and coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 22-25. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

Figure 4. Molecular structures (left) and coordination polyhedra Ln-N₆, with colored faces forming the tripod bases (right) for the compounds 22-25. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

The complexes [Ln(TPA)Hal₃] (see as example Figure 4(22)) are isomorphous and crystalize in the space group P2₁/c without any solvent molecules per a crystal cell. Note that the tripod base and a plane passing through the halide ions are not parallel.The mono-tripod complexes [Ln(TPA)Cl₃(CH₃OH)]·CH₃OH (23) (Ln³⁺ = La, Nd. Sm) (Figure 4) were also obtained starting from the corresponding hydrated lanthanide halide [LnCl₃(H₂O)₆] [121]. Nonetheless, the compounds 23 are not of interest as high performance SMMs design because they do not have monoaxiality.

In contrast, a small group of heteroleptic complexes containing three nitrates and one tripodal tetradentate ligand tris((1H-pyrazol-1-yl)methyl)amine) (TPzMA) are enough axial, Figure 4(23a) [12]. The authors present the synthesis, structures, and photophysical and magnetic properties of a sequence complexes [Ln(TPzMA)(NO₃)₃]·nMeCN (Ln = Eu, Tb, Dy, Er, n = 0.5; Yb, n = 0). The SCXRD analysis reveals that, among the investigated compounds, the compounds of Eu, Tb, Dy, Er are isomorphous and crystallize in the triclinic P1̅ space group with a single complex molecule and 1/2 of an CH₃CN molecule in the asymmetric unit. Their structures includes a mononuclear complex in which the Ln³⁺ ion coordinated by four N-atoms from TPzMA and six oxygens atoms belonging to three bidentate nitrate anions, Figure 4(23a). The tripodal ligand coordinates to the central ion in a symmetrical manner frowning together with nitrates the Ln³⁺ coordination polyhedron, which is better described as a distorted spherocorona [12]. Contrary to their congeners, the Yb complex crystallizes in the monoclinic P2₁/c space group without solvates. Probably, due to the Ln contraction and the fall in intramolecular distances resulting in steric repulsions in the polyhedron, only two nitrate moieties are bidentate and the other one is monodentate, leading to a muffin geometry of the Yb site with Cs symmetry [12].

The europium, terbium, and dysprosium analogues exhibit a lanthanide-based luminescence, while the dysprosium, erbium, and ytterbium compounds show a field-induced slow relaxation of their magnetization involving Raman and direct processes.

The complexes [Ln(TPA)₂]I₃·CH₃CN (Ln = La, Ce, Nd, Sm) are isostructural to each other (see Figure 4(24)) [3,6]. The metal ions are eight coordinate by the two-tetradentate ligands that wrap around the metal in a pseudo-D₃-symmetric arrangement [3]. All the complexes crystallize as a single enantiomer in the non-centrosymmetric space group P2₁2₁2₁ [3]. The coordination polyhedra are best defined as distorted cubes with a less distorted geometry for Lu [3].

It was not possible to obtain the crystal structure of [Eu(TPA)₂]·3OTf under water-free conditions. The single crystals of [Eu(TPA)₂]·3OTf·CH₃CN·0.3H₂O (25) were obtained in the presence of ~0.5 equivalent of H₂O. The molecular structure of 25 (Figure 4(25)) is very close to those of the Ln-bis(tpa) iodides. Contrarily to the complexes 24, complex 25 crystallizes in a centro-symmetric space group P 2₁/c with two complex molecules per asymmetric unit and 0.15 molecule of H₂O, which apparently helps the crystallization [3].

Along with to the Ln³⁺ TPA complexes, their congeners for Ln²⁺ were also isolated. Starting from LnI₂ the stable mono- and bis-TPA complexes: [Yb(TPA)I₂(MeCN)]·MeCN (26, Figure 5(26)) and [Ln(TPA)I₂] (Ln²⁺ = Sm, Eu) (27), [Ln(TPA)₂]·2I·0.5MeCM (Ln²⁺ = Sm, Yb) (28, Figure 5(28)) were prepared and characterized [6]. When a bulk anion NaBPh₄ is added to the previous reaction mixture, a number of compounds with TPA and its analogs methylated, a family of Ln²⁺ complexes was also obtained in inert conditions [122]. The compounds [Ln(Me_nTPA)₂](BPh₄)₂ (n = 0–3 reliant to methylation degree of the 6-position of the pyridyl rings of Me_nTPA, when n = 0 — Ln²⁺ = Eu, Yb 29 (Figure 5(29)), n = 2 — Ln²⁺ = Eu, Yb (30) and n = 3 — Ln²⁺ = Eu (31, Figure 5(31))) have been synthesized and their structural, electrochemical and photophysical properties studied [122].

The complexes 27, [Ln(TPA)₂]·2I, crystallize in the monoclinic centrosymmetric P2₁/c space group while the complexes 28, [Ln(TPA)₂]·2I·0.5CH₃CN crystallize in the non-centrosymmetric monoclinic Cc space group [6].

Complexes 29 crystallize in the monoclinic P2₁/n space group, contrary to 30 and 31, which crystallize in the triclinic P1ˉ space group, with the lowering of symmetry attributed to the presence of the methyl substituents that result in crystallographic disorder [122]. The Ln²⁺ ion is 8-coordinate in all sandwich compounds. Continuous shape measures using the software SHAPE 2.1 were employed to determine the geometry of the Ln centers and suggest that the coordination geometry is closest to cubic in all cases [122]. The Shape distortion parameters are in the range 0.69–1.53 for the cubic geometry, the further the value being from zero, the greater the distortion from ideal geometry [122].

Unfortunately, for all the above compounds comprising TPA (both for sandwich and semisandwich), the magnetic properties have not been studied. Only two [Ln(TPA)(Anion)₃] compounds and four [Ln(TPzMA)(NO₃)₃]·complexes have been magnetically characterized [123]. The description of their magnetic behavior we conclude the current section of the review.

Two mononuclear seven-coordinate Dy³⁺ complexes [Dy(TPA)Cl₃] (32) and [Dy(TPA)(OPhCl₂NO₂)₃]·0.5CH₂Cl₂ (33) have been synthesized based on the neutral ligand TPA and either the strong strength ligand 2,6-dichloro-4-nitrophenol (Cl₂NO₂PhOH) or the weak ligand field donor Cl⁻ [123]. As in the tri-iodine compounds of type 22, mentioned above, the Dy³⁺ ions in complexes 32 and 33 have seven-coordinated capped octahedral and capped trigonal prismatic coordination geometries, respectively [123]. Magnetic studies showed that both Dy compounds possess field-induced slow magnetic relaxation. The energy barrier for 33 is higher than that of 32, which is due to the strong ligand field of Cl₂NO₂PhO⁻versus Cl⁻, resulting in a larger magnetic anisotropy of 33 as compared to 32 [123]. The direction of the magnetic anisotropy axes in both complexes deviate remarkably from the symmetry axis of the capped octahedron (C_3v) and the capped trigonal prismatic (C_2v), which explains the poor performance of SIM behavior for both complexes [123].

The room-temperature χT values of 12.97, 13.92, 11.54, and 3.20 emu/mol for 23a, respectively for [Ln(TPzMA)(NO₃)₃]·(Ln = Tb, Dy, Er, Yb), are in quite good accordance with the theoretical values of 11.82, 14.17, 11.48, and 2.57 emu/mol estimated for a unique Ln³⁺ ion [12]. Upon cooling, all compounds exhibit the typical decrease in χT caused by the thermal depopulation of the m_J levels reaching values at 1.8 K of 5.25, 7.35 [12]. For all complexes, the absence of saturation for the magnetization curves testifies to the existence of magnetic anisotropy, as expected for such lanthanide ions [12]. Under a zero-dc field, no strong out-of-phase susceptibility (χ″) components was observed for any of the samples pointing out the occurrence of fast QTM.

Excluding the Tb complex, for which the out-of-phase component remains weak, all other complexes show a strong χ″ component upon applying dc field. For the Er and Yb compounds, the appearance of a second low-frequency peak was detected at high magnetic fields. It might originate from different relaxation mechanisms actuated by large magnetic fields [12]. Appears therefore that the neutral tetradentate TPzMA ligand in association with nitrates and the resulting low-symmetry of the lanthanide site do not provide the requirements to maximize the anisotropy for either oblate or prolate lanthanide ions in zero dc field [12].

4.1. Complexes of the tripodal nitroxyl radicals

Metal-radical systems are recognized to display better SMM characteristics [124]. For example, an extra electron transforms (n-Bu)₄N[TbPc₂] (Pc is a dianion of phthalocyanine) into [TbPc₂] (Kramers system), guaranteeing twofold degeneracy of all electronic levels enforced by time reversal symmetry, irrespective to ligand field symmetry[125]. Park et al. [126] stated that the higher energy levels sturdily depend on the ligand type, molecular symmetry, and overall charge of the molecules. Additionally, ligand distortion and molecular symmetry play a key role in transverse CF parameters leading to tunnel splitting. The latter induces QTM. Compared to the anionic complex [TbPc₂]^–, for the neutral complex, no tunnel splitting was observed for the ground and excited state quasi-doublets [126]. For the anionic complex, the tunnel splittings of 0.007, 0.090, and 7.969 cm^–1 have been observed for the ground, first and second excited state quasi doublets. The perceived dissimilarity in the magnetic behavior was attributed to the significant an exchange interaction, J_ex of ~ 7 cm^–1, existing in the compound [TbPc₂] compared to the anionic one [126]. Moreover, the axial CF parameter (B₂⁰ = –5.93 vs –5.05 cm^–1) is larger, and the transverse CF parameter (B₂² = 0.3 to 0.4 cm^–1 vs. 0.8 to 3.6 cm^–1) is small for the latter [126].

Real influence of exchange coupling on magnetic relaxation dynamics was reported by Long et al., firstly reported very large T_B values [127]. They have obtained the binuclear Tb³⁺ complex [{[(Me₃Si)₂N]₂(THF)Tb}₂(µ-η₂:η₂-N₂)^–] (TbN₂Tb), in which the large magnetic interaction between Tb³⁺ and radical established to quench QTM in the absence of magnetic field. This SMM relaxes in the thermally activated direct process having (QTM probability B~10^–6) an U_eff=227 cm^–1 and T_B~14 K [127]. Later, the strong coupling of –27 cm^–1 was communicated for the Gd congener of TbN₂Tb [128]. For the GdN₂Gd the electronic structure calculations have been performed, which clearly evidence about the direct overlap between the Gd³⁺ 4f-orbitals and the π* orbital of the radical [129].

4.1.1. The functionalized by 2-pyridyl groups paramagnetic tripods and their complexes

Nitroxyl stable radicals a widely used in the field of molecular magnetism [130,131,132,133,134,135]. However, till now only three tripodal nitroxyl radical functionalized by pyridyl groups (Figure 6) are known [25,136]. The complexes of the 3d metal ions with the radical tripods 34-36 are most of a sandwich type [25,26,27,28,29,30,31,32,137]), while a number of semi-sandwich Ln-complexes were recently synthesized [138,139] (Figure 7(37)). In contrast to the tetradentate tripods of TPA described above, the tripodal oxazolidine radical (Rad) 35 is sterically rigid, forming a pyramid upon coordination with an almost right triangle at the face for both monoradical (37) and biradical complexes (38) (Figure 7) [138,140].

4.1.2. Structural features of the paramagnetic tripod complexes

According to PRXD study, the monoradical complexes [LnRad(NO₃)₃] (37) are isostructural. The crystal structures for the 37 complexes of Ln³⁺ = Dy, Tm, Y, Eu and Lu ascertained by SC-RXD experiments. Like their closest relatives, the nitrate complexes of Ln with diamagnetic tripod TPM (9), the compounds 37 crystallize in the non-centro symmetric P2₁/n space group [138]. In this complexes, Rad coordinates the Ln ion in a tridentate manner via two N atoms of the pyridyl substituents and an O atom of an NO group. The coordination sphere is further complemented by three bidentate nitrates to give an LnO₇N₂ polyhedron [138]. Consistent with the continuous symmetry measures method [104], the polyhedron is best described as a spherical tricapped trigonal prism. The radical donor atoms compose a triangular face of the prism. In addition, the coordinated oxygen atoms of the nitrate ligands, they also form triangular planes parallel to that of Rad (Figure 7(37), right). Moreover, the centers of all triangles lie on the same axis passing through the central Ln atom, which bears witness to with S₃ symmetry.

Figure 7. Molecular structures (left) and coordination Ln polyhedra with colored triangles forming the tripod bases (right) for the compounds 37-39. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

Figure 7. Molecular structures (left) and coordination Ln polyhedra with colored triangles forming the tripod bases (right) for the compounds 37-39. Hydrogen atoms are omitted. The picture was made using open crystallographic data.

The Ln–O bond distances related to the NO moiety vary in region of 2.34 – 2.38 Å. N – O bonds length of the nitroxyl group fluctuate in the 1.25–1.28 Å interval. Markedly, all bond lengths and angles of the complexes are in the expected range [138]. In biradical complexes 38, the mode of ligand coordination does not differ from that of monoradical complexes 37. The Ln environment is composed of three monodentate anions to give LnO₅N₄ polyhedron. Unlike nitrate ligands, triflates are bound to Ln by only one donor O atom and are located in the equatorial plane of the compounds 38. At first glance, the latter have D_3h pseudosymmetry, since both tripod bases are placed one above the other, and the donor atoms of the OTf ligands form a triangle (Figure 7(38)). However, due to the “sandwich” bending, all triangles are highly distorted. Though, the SHAPE analysis [104] gave the polyhedron geometry as a spherical capped square antiprism with the point symmetry close to C_4v [140]. The radical donor atoms and two OTf compose faces of the antiprism while oxygen of the third triflate arranges above the rectangular face [140].

Only two related compounds for the sandwich complex 38 are Ln³⁺ complexes with a quasi tripodal ligand 1,3,5-trimethyl-triazacyclohexane (Me₃tach) – [Pr(Me₃tach)₂(OTf)₃] [141] and HMe₃tach[La(Me₃tach)₂(OTf)₄] [142], Figure 8. The first is so bent that the three triflates are not evenly distributed in the equatorial plane, while the latter is capable to house even more triflates. Such a geometrical organization of the Ln coordination sphere is favorable to stabilize the highest m_J ground states for the prolate tripositive lanthanides ions (Pm, Sm, Er, Tm, and Yb). That is why the 38-Dy complex studied by us earlier does not exhibit slow magnetic relaxation. The most attractive geometry (for prolate type Ln³⁺) among compounds with this pseudotripodal ligand has the recently studied the only non-bent sandwich complex [La(Me₃tach)₂Cl₃] [142] having three chlorine anionic ligands in equatorial plane, Figure 9. However, chloride anions are bulky enough to enter threesome the inner sphere of smaller Ln³⁺ ion beginning from samarium. Nevertheless, two chlorides can fit quite well in the equatorial plane of the Ln coordination sphere. We did not find an example of such a specie for any [Ln(tripod)₂Cl₂]⁺. According to the CCDC, there are only a few examples of such compounds with bis-tripodal ligands. One of which is the Eu³⁺ complex [Eu^IIICl₂{R)-tppn}]ClO₄ (39) [143], Figure 7. The coordination geometry of 39 is best described as a distorted dodecahedron. The authors point out that the four coordinated pyridyl nitrogens and one from the two Cl-atoms are approximately on a plane and form a pentagon, the other Cl being coordinated almost perpendicular to this plane. However, from our point of view, it is better to choose a different description of the geometry of the compound 39 in order to predict the magnetic behavior. Both Cl anions are best placed in the same plane, as shown in Figure 8. In this case, the molecule have an axis, which could serve as an axis of anisotropy. Our preliminary studies have shown that sandwich-type complexes containing two chloride ligands in the equatorial plane of the cationic complex 40 (Figure 7) can also be obtained for the paramagnetic tripod 35 [144].

4.1.3. Magnetic properties of the paramagnetic tripod complexes

At 300 K, the χT product values are 7.814, 12.210, 14.366, 7.376 emu K/mol for the 37 type compounds of Gd, Tb, Dy, and Tm, respectively. These values are well consistent with the expected ones for the appropriate Ln^III ion plus a radical (8.255, 12.195, 14.545, 7.525 emu K/mol) [138]. With the temperature lowering, the χT value for all derivatives drops considerably, which can be ascribed to CFS and/or the antiferromagnetic metal-radical interaction. It could be assumed a dominance of the CFS for all Ln except Gd, which is magnetically isotropic at first order. It should be emphasized, that the 37-Tm complex, for which the nonmagnetic m_J = 0 ground state is stabilized (χT is equal to 0.375 emu K/mol corresponding to the value of a radical tripod). Furthermore, the important decrease in χT for 37-Gd bears witness to a strong antiferromagnetic (AFM) coupling between the Gd^III ion and the radical. The plot M(H) for the 37-Gd complex is very informative. Considering the low crystal field splitting typical of Gd³⁺, the saturation value of 6 μ_B is consistent with an AFM coupling between a spin S = 7/2 and a radical spin S = ½ (S_tot = 7/2-1/2 = 3) [138]. X band EPR has been performed on [GdRad(NO₃)₃] in order to obtain precise information about the electronic structure. The spectrum of Gd exhibits several broad transitions.

A satisfactory fitting of both the EPR and the static magnetic measurements can be obtained using the following Hamiltonian:

$$\mathcal{H}=b_2^0{\widehat{O}}_2^0+b_2^2{\widehat{O}}_2^2+b_4^0{\widehat{O}}_4^0+j{\widehat{S}}_{Gd}·{\widehat{S}}_{rad}+g_{Gd}{\mu }_B{\widehat{S}}_{Gd}·B+g_{rad}{\mu }_B{\widehat{S}}_{rad}·B$$

(1)

where the first three terms parametrize the CFS of the Gd^III ion, the fourth term is the isotropic magnetic coupling between Gd and the radical and the last two terms are the Zeeman splitting for Gd and the radical, respectively. The finest simulation result was achieved with the values b₂⁰ = 5.2 10^-2 cm^-1, b₂² = 1.1 10^-2 cm^-1, b₄⁰ = 3.8 10^-4 cm^-1, j = +23 cm^-1, g_Gd = 2.0023 and g_rad = 1.998. Notably, the value of +23 cm^-1 of the isotropic coupling constant is unusually large for gadolinium complexes of organic radicals. For example, for Gd³⁺ hexafluoroacetylacetonate complexes containing one acyclic nitroxyl radical [145,146,147] the |j| value of fluctuates between 9.6 and 12.5 cm^-1. For the similar compounds including one nitronyl nitroxyl radical [148,149,150,151,152,153], exchange coupling is also inferior (|j| = 0.77 ÷ 8.35 cm^-1). For the Gd-complex comprising congener of Rad TEMPO (TEMPO = 2,2,6,6-tetramethylpiperidin-1-oxyl) metal-radical interaction is very small (j = 2.43 cm^-1) [154]. For the mono-semiquinone complex [Gd(HBTp₃)₂SQ] j = 11.4 cm^-1 [155]. Moreover, the exchange interaction strength for Gd-radical in the [GdRad(NO₃)₃] species is comparable with for the binuclear Gd complex of the purely inorganic single radical N₂^3- obtained in the group of Long [128]. The origin of such a strong magnetic exchange interaction in 37 must be ascribed to a favorable metal-to-ligand orbital superposition. In contrast to the most studied complexes with nitronyl and imino-nitroxyl radicals, in which the spin density is mainly delocalized over four or three centers (O - N ... N – O [156], N ... N - O), in 37, an unpaired electron is shared by only two cites. Consequently, the spin density on the donor oxygen atom in Rad is two times higher than that in the nitronyl nitroxyl radical. Notably, the exchange interaction is directly related to magnetic orbital overlapping, which depends on the symmetry and donor strength of all ligands [138].

Dynamic magnetic studies were to get information on the magnetization dynamics at low temperatures. A frequency scan at various applied fields for 37 was performed at the temperature of 2 K. The only compound to display a relevant nonzero out of phase magnetic susceptibilities was 37-Tb. The latter displays slow relaxation both with and without an external applied field. In zero applied field the relaxation of 37-Tb at 2 K is at the upper edge of accessible frequencies with relaxation time ca. 16 μs, for this reason a temperature study was impossible. When an external magnetic field was applied, the slow relaxation of 37-Tb slows by several orders of magnitude [138]. The relaxation time best fit was obtained using a combination of quantum tunnelling and Orbach processes, giving τ_QT=12(1) ms, τ₀ = 0.9(3) ns and ΔE = 57 cm^-1 [138].

The magnetic studies on powder samples of the complexes 38 were also fulfilled. The χ_mT-value at 300 K for the 38-Dy compound (14.735 emu K/mol) is slightly smaller than theoretical one (14.92 emu K/mol) for the non-interacting two radicals and one Dy³⁺ ion (S = 1/2, g = 2.0023, 0.375 emu K/mol) (4f⁹, S = 5/2, L = 5, J = 15/2, g_J = 4/3, ⁶H_15/2, 14.17 emu K/mol). However, this value corresponds well to those of 14.365 emu K /mol, previously obtained for the monoradical complex 37-Dy [138] taking into account the fact that the experimental values for Dy³⁺ in a related coordination environment are somewhat lower than those for a free ion: 13.92–14.00 [12,157]. On cooling, the χ_mT value remains almost unchanged up to 90 K, and then steadily falls down to 10 emu K mol⁻¹ at 20 K and finely drops to 4.803 emu K mol⁻¹ at 2 K. The latter is considerably lower than that for the monoradical analogue (6.50 emu K/mol). Since significant intermolecular exchange interactions in 38-Dy can be excluded, the cause of such behavior could be attributed to the radical-radical coupling, which can reach high values (J_TEMPO1-_TEMPO2/k_B = −24.9 K) in [Y(hfac)₃(TEMPO)₂]) [158]. Moreover, the metal-to-radical coupling in the [Gd(hfac)₃(TEMPO)₂] has been reported to be either positive or negative for the different radicals of the same molecule (J_Gd–TEMPO/k_B = −6.45 and +4.0 K, obscuring the picture [158]. Therefore, for the very anisotropic Dy, it is difficult to obtain more information also due to the high mixing of the |J,m_j> levels favored by the relatively low-symmetry ligand field. In order to elucidate the nature of exchange interactions in 38-Dy [158].

The temperature dependence of χ_mT for Eu³⁺ compounds is determined by the thermal population of the ⁷F₁ level nearest to the ground nonmagnetic level ⁷F₀. The excited ⁷F₁ state, closely sited to the ground one, is partly populated already at room temperature. At 300 K, χ_mT for Eu³⁺ complexes with diamagnetic organic ligands can vary in the range of 1.032–1.386 emu K/mol¹ depending on the ligand field parameters [159]. Therefore, for the complex 38-Eu, the 300 K χ_mT value of 1.778 emu K/mol is reasonable for the two uncoupled radicals and one Eu³⁺ ion, but lower than the value of 1.93 emu K/mol found for the bis-nitronylnitroxide (NN) complex [Eu(NN)₂(NO₃)₃] with a different coordination environment (N₁₀ instead of N₄O₅) [160]. As the temperature pulls down, the χ_mT decreases gradually, and, starting from 9 K, drops to 0.348 emu K/mol, which is somewhat higher than that for [Eu(NN)₂(NO₃)₃] compound (0.24 emu K/mol). No ac signal was observed in either sample in the measurable interval of frequencies (0.1–10,000 Hz).

4.1.4. Rational design of the paramagnetic tripods and their complexes

As mentioned above, in the presence of anionic ligands in the equatorial plane, it is better to use prolate Ln ions: Pm, Sm, Er, Tm, and Yb. While for more "magnetic" dysprosium and terbium, the presence of anionic ligands at the equator is strictly contraindicated. Therefore, it is necessary to change the structure of the paramagnetic tripod so that there is no space for anionic ligands or solvent molecules in the Ln coordination sphere. An analysis of the molecular structure of sandwich complexes with diamagnetic tripods has showed that low-coordination compounds without anionic ligands are formed in the presence of steric hindrance in a position adjacent to donor tripod atoms giving propeller-like structures with ideal axiality (see compounds 1, 4, 16, 18, 21, 31). It should be noted that in most of the bis-tripodal complexes considered in this review, the ligands are symmetrical tripods, in contrast to the radical 35, which consists of two six- and one five-membered heterocycles. Moreover, the latter comprises a bridgehead carbon atom in ligand. While, other described tripods are more spatial ligands. In complexes with the radical 35, the average value for the side length of the triangular base is about 2.8 Å, while for other bridgeheads it is much larger: 2.9-3.1 for boron, 3.8-4.0 for nitrogen and metallic bridgehead. The larger dimensions allow to the tripods with hetero bridgehead atom “to more deeply set on the head” of the central Ln ion.

On the space filling image of the "burger" 38 (Figure 7), it is clearly seen that two pyridyl substituents of the different oxazolidine radicals 35 are in close proximity, and the shortest contact H…H between them is equal to 2.41 Å. In complex 40, there are also sufficiently close distances between the pyridine rings and the methyl groups of the radical (2.613 and 3.007 Å, Figure 10). Therefore, if an additional methyl group is located in the fourth position of the pyridyl rings (just near donor nitrogen atom), then most likely this will be enough for the paramagnetic tripods to turn relative to each other with the formation of a propeller-like structure in which there will be no place for additional molecules. In addition to increasing the steric load of the pyridyl substituents, it is necessary to make the paramagnetic tripod more symmetrical about the bridgehead carbon atom.

This can be done by going from a five-membered oxazolidine ring to a six-membered oxazinane (41), Figure 11a. The synthesis of such a tripodal radical becomes rather complicated due to commercially unavailable bis(6-methyl-2-pyridyl)methanone and 3-amino-3-methyl-butan-1-ol, the condensation of which yields its diamagnetic precursor.

Other way is a choice of 1-imidazole as a functional group (instead of pyridine) for oxazolidine nitroxide, Figure 11b. This is slightly easier root because the starting aminoalcohol is cheap, but corresponding bis-ketone must be prepared.

If the use of the hindered tripod 41 is intended to prevent coordination of hetero-ligands in the equatorial plane, which is favorable for complexes with oblate Ln-ions, then its unhindered congener is better to be used for heteroleptic complexes like 39 and 40 for the prolate series. The latter can also be chosen for heteroleptic complexes with tripod 42.

5. Conclusions

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