Structure and Properties of Heterometallics Based on Lanthanides and Transition Metals with Methoxy-β-Diketonates

Abstract

The possibility of obtaining volatile polynuclear heterometallic complexes containing lanthanides and transition metals bound by methoxy-β-diketonates was studied. New compounds were prepared by cocrystallization of monometallic complexes from organic solvents. Ln(tmhd)₃ were used as initial monometallic complexes (Ln = La, Pr, Sm, Gd, Tb, Dy, Lu; tmhd = 2,2,6,6-tetramethylheptane-3,5-dionate) in combination with TML₂ in various ratios (TM = Cu, Co, Ni, Mn; L: L¹ = 1,1,1-trifluoro-5,5-dimethoxypentane-2,4-dionate, L² = 1,1,1-trifluoro-5,5-dimethoxy-hexane-2,4-dionate, L³ = 1,1,1-trifluoro-5-methoxy-5-methylhexane-2,4-dionate). Heterometallic complexes of the composition [(LnL₂tmhd)₂TM(tmhd)₂] were isolated for light lanthanides Ln= La, Pr, Sm, Gd, and L= L¹ or L². By single crystal XRD, it has been established that heterometallic compounds containing La, Pr, Cu, Co, and Ni are isostructural linear coordination polymers of alternating mononuclear transition metal complexes and binuclear heteroleptic lanthanide complexes, connected by donor–acceptor interactions between oxygen atoms of the methoxy groups and transition metal atoms. A comparison of powder XRD patterns has shown that all heterometallic complexes obtained are isostructural. Havier lanthanides Ln = Tb, Dy, Lu did not form heterometallics. Instead, homometallic complexes Ln(L³)₃ were identified for Ln = Dy, Lu as well as for Ln = La. The thermal properties of the complexes were investigated by TG-DTA and vacuum sublimation tests. The heterometallic complexes were found to be not volatile and decomposed under heating to produce inorganic composites of TM oxides and Ln fluorides. In contrast, Ln(L³)₃ is volatile and may be sublimed in a vacuum. Results of magnetic measurements are discussed for several heterometallic and homometallic complexes.

1. Introduction

Ln-containing heterometallic complexes have attracted the attention of researchers due to their interesting magnetic, optical, and luminescent properties [1,2,3,4,5]. A significant number of works are devoted to the study of the magnetic properties of 4f–3d complexes. There are also works where 4f–3d heterometallic complexes exhibit several unusual properties simultaneously [1]. In addition, 4f–3d complexes are studied as precursors for mixed oxides of f-d metals [6,7,8]. The latter motivates the search for new volatile polynuclear complexes with organic ligands.

In particular, heterometallic β-diketonates usually consist of monometallic moieties sharing several chelating oxygen atoms between coordination centers and fluorinated ligands provide more volatile compounds [9]. The bridging function of oxygen atoms is limited by the steric action of the terminal substituents (R, R’) of the β-diketonate ligand R-CO-CH-CO-R’. To overcome this problem, one can use ligands with donor atoms at the terminal substituents that are more sterically accessible to form bridging bonds with neighboring metal atoms, which should be coordination unsaturated. Our systematic screening of mono- and di-methoxy-substituted diketones, including the ones presented in Figure 1 (R-CO-CH-CO-C(OCH₃)_x(CH₃)_3−x, x = 1, 2), allowed to prepare various heterometallic complexes by cocrystallization of monometallic complexes from organic solvents [10,11,12]. In the structure of such heterometallic complexes, the monometallic fragments are held together by bridging oxygen atoms, including those from methoxy groups. For example in Cu/Pb and Pd/Pb heterocomplexes, it was shown that the structure and reactivity depend on the composition and structure of ligands in the initial monometallic complexes [10,11]. First-row transition metals with methoxy-substituted diketones form a series of coordination saturated binuclear complexes that are rather stable in solution and, therefore, are inert to the formation of heterometallic products [12]. In the structure of copper (II) complexes with dimethoxy ligands and heterocomplexes based on them, usually, one of the adjacent methoxy groups does not form bridging bonds and remains free, creating only a steric effect. In order to involve two methoxy groups in one terminal substituent for bridging bonds, it is necessary to investigate the possibility of obtaining volatile heterometallic complexes with the participation of metal ions, which stand out for large coordination numbers, e.g., alkaline earth metals and lanthanides.

In this paper, we investigate the possibility of obtaining heterometallic complexes of lanthanides and first-row transition metals with mono- and dimethoxy-substituted diketonate ligands (Figure 1). We discuss here the preparation and purification methods, structure, thermal, and magnetic properties of new compounds using the example of typical representatives of a number of available lanthanides (III), namely La, Pr, Sm, Gd, Tb, Dy, Lu.

So far, for dimethoxy-substituted lanthanide diketonates, the structure of homometallic ([La(L²)₃]₂) and heterometallic complexes with alkali metals has been reported, where the coordination of metal cations is also stabilized due to bridging bonds involving methoxy groups, about half of which remain free [13,14,15,16]. The isolated compounds exhibit discrete and polymeric structures, but volatility was not reported.

2. Results and Discussion

2.1. Synthesis and Structure

Previously, it was shown that the monometallic complexes Cu(L¹)₂, Cu(L²)₂, and Cu(L³)₂ have the structure of coordination polymers and heterometallic complexes based on them can have both discrete and polymeric structures where the monometallic units are held together by bridging metal–oxygen bonds with the participation of methoxy groups [10]. For dimethoxy-substituted diketonate (L = L¹, L²), one of the adjacent methoxy groups in the terminal substituent remains free. To involve both methoxy groups in the formation of bridging bonds, the lanthanide complexes were used in which the central atoms can have large coordination numbers. We studied the crystalline reaction products of available Ln(tmhd)₃ (Ln = La, Pr, Sm, Gd, Tb, Dy, Lu) with transition metal bis-diketonates, TML₂, L = L¹, L², L³ (Figure 1), TM = Cu, Ni, Co, Mn. It was found that the ligand exchange reactions according to Scheme 1 occur in solution:

Heterometallic complexes were obtained only by reaction (A) in the series of light lanthanides and dimethoxy-substituted diketonates at a molar ratio of 1:1. Other molar ratios did not give new products. The cocrystallization product consists of two types of crystals easily distinguishable by color. Heterocomplexes of the [(LnL₂tmhd)₂TM(tmhd)₂] type are slightly colored depending on the TM. Crystals of the second component TM(tmhd)₂ could be separated either by extraction with heptane or by vacuum sublimation. For example, [(La(L¹)₂tmhd)₂Cu(tmhd)₂] is nonvolatile and non-soluble in heptane, while dark blue crystals of Cu(tmhd)₂ are well soluble in heptane and sublime at T_subl = 130 °C in dynamic vacuum ~10⁻² Torr. TM(tmhd)₂ can easily be identified by XRD, MP, and color. The remaining heterometallic product can be recrystallized from toluene. A series of copper–lanthanide complexes [(Ln(L¹)₂tmhd)₂Cu(tmhd)₂], where Ln = La (1), Pr (2), Sm (3), Gd (4), are apparently isostructural according to powder XRD data (Figure 2). To trace the sterical effect of the terminal bis-methoxy substituent, [(La(L²)₂tmhd)₂Cu(tmhd)₂] (8) was prepared. According to XRD, 8 is isostructural with the rest of the copper-containing heterocomplexes 1–4. Following the same approach, [(La(L¹)₂tmhd)₂Ni(tmhd)₂] (6), [(La(L¹)₂tmhd)₂Co(tmhd)₂] (5) were isolated. Crystals suitable for single crystal XRD were not obtained for 3 and 4 and for [(La(L¹)₂tmhd)₂Mn(tmhd)₂] (7) complexes, the manganese derivative turned out to be very unstable during recrystallization.

Crystals of 1, 2, 5, 6, and 8 are built of one-dimensional coordination polymers of alternating mononuclear transition metal complexes and binuclear heteroleptic lanthanide complexes, connected by donor–acceptor interactions between oxygen atoms of methoxy groups and transition metal atoms (Figure 3). In other words, the metal–organic chains are based on lanthanide binuclear fragments and transition metal fragments bridged by TM-O^O-La linkers when one of the adjacent methoxy-group is connected to Ln and another one is connected to TM atoms. As a result, the square planar coordination in TM(tmhd)₂ fragment is completed to square-bipyramidal by two oxygen atoms of OCH₃-groups. Key geometry parameters are summarized in Table 1.

In the binuclear heteroleptic fragment (Ln(L)₂tmhd)₂ for lanthanide atoms C.N. = 10. Distance Ln…Ln is ~3.8 Å. The lanthanide dimer itself is centrosymmetric and is bound by bridging bonds with the participation of oxygen atoms from both chelate and methoxy groups. However, for the two adjacent methoxy groups, only one is coordinated by the lanthanide atom. While the other methoxy-group remains free in one L, and, in the second L, is coordinated by a transition metal atom. Where both methoxy groups are coordinated the Ln-OCH₃ distance is shorter for L¹ in contrast to L². At the same time, the TM-OCH₃ bridging bond in 8 is longer than in 1, apparently due to the fact that the –CCH₃(OCH₃)₂ substituent in L² is bulkier than –CH(OCH₃)₂ in L¹. In turn, the chains of the coordination polymer do not form additional contact with each other. For example, in crystals of 2, the shortest distance between the nearest chains is F…H = 2.620 Å (Figure S1).

In route (B) for the heavier lanthanides (Ln = Tb-Lu), no heterometallic products formed. In this case, Cu(tmhd)₂ and a colorless glassy product, perhaps a mixed-ligand lanthanide complex, formed separately.

Thus, for ligands with two methoxy groups, the formation of two series of products is observed during cocrystallization. Light lanthanides (Ln = La-Gd) give isostructural heterometallic complexes with ligand exchange, while for heavier lanthanides (Ln = Tb-Lu) the ligand exchange occurs without the formation of a heterometallic complex.

In the case of the mono-methoxy-substituted ligand, the situation turned out to be quite different. It was assumed that the lanthanide dimer (Ln(L³)₂tmhd)₂ should contain two methoxy groups involved in bridging bonds and none free; no heterometallic complex would form. Indeed, the verification of systems with L³ according to route (C) of Scheme 1 has shown that the cocrystallization of Cu(L³)₂ and La(tmhd)₃ taken in an equimolar ratio does not yield a heterometallic complex, but rather a two-component system of individual complexes of lanthanum and transition metal was obtained in the result of ligand exchange. The resulting mixture was separated using gradient sublimation. There was only one lanthanum-containing fraction. ¹H NMR analysis of the lanthanum-containing fraction has shown the presence of signals for the ligands L³ and tmhd in a ratio of 2:1. It is difficult to say whether this is a mixed-ligand complex or a mixture of the lanthanum homoligand complexes. That is why this product is marked by an asterisk in Scheme 1. Further, it was assumed that in the result of the complete exchange of ligands, the lanthanum dimer should contain two free methoxy groups. However, the reaction (D) where reactants Ln(tmhd)₃ and TML₂ were taken in 2:3 ratio still did not give heterometallic complexes. As a result of complete exchange of ligands, homoleptic complexes of lanthanum and copper were obtained, which were also separated by vacuum sublimation. ¹H NMR analysis of the lanthanum-containing fraction have shown the presence of signals only for the L³ ligands at the same place, and again two sets of signals are visible in a ratio of 1:2. Moreover, in the ¹⁹F NMR spectra, two signals have been recorded in a ratio of 1:2. Thus, the NMR study supports the dimeric structure of the lanthanum complex in solution, with the broad lines indicating that dimer 9 has rather a fluctional structure. Structural data also confirm the dimeric structure, with 9 containing two free methoxy groups. The structure contains two crystallography-independent molecules differing in the orientation of the terminal methoxy groups (Figure 4). The coordination of lanthanum atoms in the homoleptic dimer is similar to that for the heteroleptic dimers described above in 1–6, 8. The main bond lengths and angles are given in Table 2. There are the same coordination manner, the same coordination polyhedron, C.N. = 10, number of bridging bonds is 4. La…La distance in dimer ~3.8 Å. A similar dimeric complex [La(L²)₃]₂ has been reported before [16]. For comparison, in La₂(tmhd)₆, the La…La distance is ~4 Å, and there are only two bridging oxygen atoms, C.N.(La) = 7 [17].

Thus, it has been established that under the cocrystallization of La(III) dipaloylmethanate with mono-methoxy-substituted transition metal(II) β-diketonates, the formation of heterometallic complexes does not occur. Instead, an exchange of ligands is observed with the isolation of the binuclear homoleptic lanthanum complex. In the structure of 9, the free methoxy groups are located as if along the dimer and steric conditions seem to be unfavorable for the formation of bridging bonds with square planar TM(tmhd)₂. Nevertheless, cocrystallization in such systems can be used as a simple way to obtain complexes of some lanthanides with fluorine-containing diketones by ligand exchange reaction. We believe that for other light lanthanides Ln = La-Gd complexes have dimeric structure [Ln(L³)₃]₂. As for the heavier lanthanides, the structure of Tb, Dy, and Lu derivatives were not determined because they were isolated as glassy substances. For example, the ¹H NMR spectrum of 11 is silent and the ¹⁹F NMR spectrum looks strange, indicating that this complex is paramagnetic. On the other hand, ¹H NMR of 12 shows broad lines but for one set of ligand signals, and an asymmetric multiplet is observed in the ¹⁹F NMR spectrum. Thus, it can be said that at least in solution the Ln(L³)₃ for Ln = Tb-Lu seem to be low-symmetry monomers. However, they are more volatile, since 11 and 12 can be re-sublimated at ~160 °C, and 9 already at ~200 °C. To determine the nuclearity of the resulting noncrystalline complexes, we additionally used data on magnetic properties, which are discussed in the corresponding section.

2.2. Thermal Properties

The sublimation test showed that the obtained heterometallic complexes 1–6, and 8 are not volatile and decompose when heated in a vacuum. A comparison of the TG-DTA data for 1, 2, 5, and 6 is shown in Figure 5. As can be seen, the heterometallic complexes exhibit similar thermal behavior, they decompose upon heating. XRD of the solid residues obtained in separate experiments on the calcination of heterocomplex samples in air showed that a composite containing CuO, LaF₃, and LaOF is obtained from [(La(L¹)₂tmhd)₂Cu(tmhd)₂] (1) (Figure S2). [(La(L¹)₂tmhd)₂Ni/Co(tmhd)₂] (5, 6) gives LaF₃, LaOF and probably metallic Ni or Co. Thermolysis of [(La(L¹)₂tmhd)₂Mn(tmhd)₂] (7) gives solid product containing LaMnO₃ and LaF₃ (Figures S3–S5). As already mentioned, Ln(L³)₃ complexes are volatile and can be re-sublimed in a vacuum.

TG-DTA results for homometallic 9 and 11 are compared to La(tmhd)₃ in Figure 6. Judging by the amount of nonvolatile residue, new homometallic complexes decompose when heated at atmospheric pressure.

2.3. Magnetic Properties

Among the studied complexes, the homometallic tris-diketonates 11 and 12 represent the simplest cases for discussing magnetic properties. As expected, 12 exhibits diamagnetic behavior owing to the non-magnetic (J = 0) state of Lu³⁺ ions, except for the low-temperature region (T < 30 K) where impurities of other rare-earth elements at the level of a few tenths of a percent provide a paramagnetic upturn of the magnetic susceptibility (Figure 7a). In its turn, 11 containing Dy³⁺ ions (S = 5/2, L = 5, J = 15/2) demonstrates paramagnetic behavior throughout the available temperature range of 1.77–300 K (Figure 7b). As can be seen in Figure 8a the 1/χ_p(T) curve deviates slightly from linearity and hence χ_p(T) deviates from the simple Curie–Weiss dependence ${\chi }_{\mathrm{p}}\left(T\right)=N_A{\mu }_{\mathrm{eff}}^2/3k_{\mathrm{B}}(T-\theta )$ (N_A and k_B are the Avogadro number and the Boltzmann constant) implying the effective magnetic moment µ_eff to be temperature dependent. Nevertheless, the Curie–Weiss fit can still be used in the lowest-temperature region to roughly estimate the Weiss constant θ that characterizes the interaction between Dy³⁺ ions. The evaluated θ has turned out to be less than 0.6 K in magnitude pointing to a very weak, if any, magnetic interaction between Dy³⁺ ions. The effective magnetic moment calculated for Dy(L³)₃ (11) under the assumption of non-interacting magnetic moments (θ = 0) gradually changes from µ_eff ≈ 10.45 μ_B at T = 300 K down to µ_eff ≈ 8.1 μ_B at T = 1.77 K (Figure 8a). Apparently, the high-temperature µ_eff value is close to the theoretical effective moment of a free Dy³⁺ ion µ_eff(Dy) ≈ 10.64 μ_B, while the gradual decrease in µ_eff upon cooling is predominantly caused by the crystal-field splitting of the ground state ⁶H_15/2 multiplet.

To clarify the magnetic state of the Dy³⁺ ions, one can examine the magnetic-field dependence of the magnetization that should follow the expression $M(H)=N_{A}g{\mu }_{B}J{B}_J(\frac{g{\mu }_B}{k_{B}T}JH)$, where B_J(x) is the Brillouin function. The shape of the M(H) dependence measured at T = 1.77 K turns out to be close to that expected for free Dy³⁺ ions with J = 15/2 and g = 4/3 [18], but the magnitude of the magnetization does not fit these parameters being less than half of the expected (Figure 8b). Indeed, as can be seen in Figure 8b the magnetization tends to saturate at a level below 5 μ_B per Dy³⁺ ion while the expected value equals 10 μ_B. This discrepancy can be naturally resolved by taking into account a strong anisotropy of the g factor that Dy³⁺ ions develop at low temperatures, especially when placed in a low-symmetry environment [18,19,20]. In the case of a strongly anisotropic g factor, the magnetization along the easy axis of Dy³⁺ ions mimics the behavior of free ions, while the transverse magnetization is drastically suppressed [19]. After averaging the crystallographic orientation for a powder sample, the behavior of M(H), shown in Figure 8b, is naturally obtained.

Having established that it is the crystal-field effects that cause µ_eff to decrease with cooling (Figure 8a), we can conclude that the actual Weiss constant is much less in magnitude than the apparent θ ≈ −0.6 K. Although the dipole–dipole mechanism that usually dominates the interaction of rare-earth Ln³⁺ ions is generally rather weak, a hypothetic dimer state of large-moment (J = 15/2) Dy³⁺ ions would exhibit a noticeably larger θ than the actual one; the small actual θ is indicative of a large distance between Dy³⁺ ions and speaks in favor of a monomer crystal structure of 11.

All the studied heterometallic complexes despite the presence of Ln³⁺ dimers in their structure were found to behave as almost ideal paramagnets over the available temperature range of 1.77–300 K without any sign of significant inter-ionic magnetic interactions (a detailed description is given in Supplementary Materials). The Gd-Cu complex was the only case when a very weak yet detectable inter-ionic interaction manifested in the Weiss constant θ ≈ −0.4 K was observed (Figure S6). Given its small magnitude, the Gd³⁺ -Gd³⁺ interaction in the binuclear structural fragment is most likely governed by the dipole–dipole mechanism rather than the exchange one.

In the cases of La-, Pr-, and Sm-based heterometallic complexes, the absence of noticeable inter-ionic magnetic interactions was caused by one and the same reason—a small or zero magnetic moment of the Ln³⁺ ion at low temperatures. Indeed, the µ_eff(T) data taken for the Pr-Cu complex (Figure S7) pointed to the singlet ground state of each Pr³⁺ ion—a state quite common for Pr³⁺ ions, for instance, in a hexagonal or cubic environment [21]. The data obtained for the Sm-Cu complex implied the doublet ±1/2 ground state of Sm³⁺ (J = 5/2) ions which is weakly magnetic due to the small g factor (Figure S8). In the available temperature range down to 1.77 K, all the inter-ionic magnetic interactions are much weaker than the thermal energy k_BT. Hence, from the point of view of magnetic properties, all the studied heterometallic complexes can be considered as a set of virtually non-interacting ions; all the observed magnetic peculiarities, if any, are associated exceptionally with specific properties of single ions in a particular structural environment. In this respect, the effective magnetic moments µ_eff of Pr- and Sm-based complexes were found to be small at low temperatures but increase considerably upon heating (up to µ_eff(300 K) ≈ 5.38 μ_B and 2.87 μ_B, respectively) owing to the excited levels of the Pr³⁺ and Sm³⁺ multiplets. The same is true for magnetic transition metal ions present in the studied heterometallic complexes. No sign of inter-ionic magnetic interactions was found for transition metal ions as well, yet the effective magnetic moments of Co²⁺ (S = 3/2) and Ni²⁺ (S = 1) changed significantly with temperature (Figures S9 and S10) due mostly to the zero-field spitting of their multiplets by the crystal-field [22].

3. Experimental

3.1. Synthesis

TML₂ complexes with L¹ and L² were courtesy of IOS UB RAS (www.iosuran.ru, accessed on 18 October 2022). The general procedures for the preparation of TML₂ have been described before [10,12,23,24,25]. For Ln(tmhd)₃, the general method was used [17]. For the synthesis of heterometallic complexes, 200 mg of Ln(tmhd)₃ (Ln = La, Pr, Sm, Gd) dissolved in 10 mL of toluene was mixed with an equimolar amount of TML₂ (L = L¹ or L²; TM = Cu, Co, Ni, Mn) dissolved in 10 mL of chloroform in a small cylindrical vessel covered with a paper cap and put into a small chamber with dry nitrogen flow. The cell was placed under a flow of dry nitrogen. When the volume of the solution was halved, an equal volume of heptane was added. As the solvent dries, a two-phase mixture of crystals is formed. The biphasic mixture was separated by vacuum sublimation or extraction (for Cu and Mn). For sublimation, the dried mixture was placed in a quartz boat and heated in a gradient tube furnace at T = 130 °C (P = 10⁻² Torr). A volatile TM complex was condensed at the walls of the glass tube. A nonvolatile residue was recrystallized from toluene giving crystals of a heterometallic complex. Cu or Mn diketonate well soluble in heptane was extracted from the reaction products mixture in the following way. After the addition of heptane, the mixture was filtered, and a residue was washed several times with small portions of heptane. TM diketonate was collected after removing the solvent. The residue from the filter was recrystallized from toluene giving crystals of the heterometallic complex. The composition of the obtained crystals was determined using elemental analysis and XRD. As a result, we have identified and characterized a series of new heterometallic complexes on the basis of dimethoxy-substituted β-diketonates [(La(L¹)₂tmhd)₂Cu(tmhd)₂] (1), [(Pr(L¹)₂tmhd)₂Cu(tmhd)₂] (2), [(Sm(L¹)₂tmhd)₂Cu(tmhd)₂] (3), [(Gd(L¹)₂tmhd)₂Cu(tmhd)₂] (4), [(La(L¹)₂tmhd)₂Co(tmhd)₂] (5), [(La(L¹)₂tmhd)₂Ni(tmhd)₂] (6), [(La(L¹)₂tmhd)₂Mn(tmhd)₂] (7), [(La(L₂)₂tmhd)₂Cu(tmhd)₂] (8). 1-[(La(L¹)₂tmhd)₂Cu(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂CuLa₂, (%): C, 44.9; H, 5.7; F, 11.8. Found: C, 44.2; H, 5.7; F, 12.1. MP(DTA) 216 °C. 2–[(Pr(L¹)₂tmhd)₂Cu(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂CuPr₂, (%): C, 44.8; H, 5.6; F, 11.8. Found: C, 44.5; H, 5.3; F, 11.2. MP(DTA) 201 °C. 3–[(Sm(L¹)₂tmhd)₂Cu(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂CuSm₂, (%): C, 44.8; H, 5.5; F, 11.7. Found: C, 44.1; H, 5.5; F, 11.5. MP(Kofler plate) 170 °C. 4-[(Gd(L¹)₂tmhd)₂Cu(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂CuGd₂, (%):C, 44.1; H, 5.5; F, 11.6. Found: C, 44.0; H, 5.4; F, 11.4. MP(Kofler plate) 138 °C. 5-[(La(L¹)₂tmhd)₂Co(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂CoLa₂, (%): C, 45.0; H, 5.6; F, 11.9. Found: C, 44.9; H, 5.7; F, 11.8; MP(Kofler plate) 185 °C. 6-[(La(L¹)₂tmhd)₂Ni(tmhd)₂] Anal. Calc. for C₇₂H₁₀₈O₂₄F₁₂NiLa₂, (%): C, 45.0; H, 5.6; F, 11.9. Found: C, 44.9; H, 5.7; F, 11.8; MP(Kofler plate) 178 °C. 8-[(La(L₂)₂tmhd)₂Cu(tmhd)₂] Anal. Calc. for C₇₆H₁₁₆O₂₄F₁₂CuLa₂, (%): C, 46.1; H, 5.9; F, 11.5. Found: C, 46.4; H, 5.7; F, 11.5; MP(Kofler plate) 225 °C.

New monometallic complexes [La(L³)₃]₂ (9), Tb(L³)₃ (10), Dy(L³)₃ (11), Lu(L³)₃ (12), were obtained by the same technique using a molar ratio of Ln(tmhd)₃ to TM(L³)₂ equal to 2:3. The obtained compounds are colorless solids; only 9 is crystalline. Anal. Calc. for C₂₄H₃₀O₉F₉La (9), (%):C, 37.3; H, 3.9; F, 22.1. Found: C, 36.5; H, 4.1; F, 22.5. ¹H NMR (500 MHz, CDCl₃, 25 °C): δ 6.10 (2H, w, γ-CH, peripheral), 5.51 (4H, w, γ-CH, internal), 3.61 (6H, w, -OCH₃, peripheral), 3.20 (12H, w, -OCH₃, internal), 1.31 (36H, s, -(CH3)2) ¹⁹F NMR (470 MHz, C₆D₆, 25 °C, CClF₃ as reference): δ 75.78 and 76.22 in 1:2 ratio for internal and peripheral -CF₃ groups. MP (Kofler plate/DTA) 225–229/224 °C. Anal. Calc. for C24H30O9F9Tb (10) (%):C, 36.4; H, 3.8; F, 21.6. Found: C, 35.6; H, 4.0; F, 21.5. Anal. Calc. for C24H30O9F9Dy (11) (%):C, 36.2; H, 3.8; F, 21.5. Found: C, 35.4; H, 4.1; F, 21.4. Anal. Calc. for C24H30O9F9Lu (12) (%):C, 35.7; H, 3.7; F, 21.2. Found: C, 35.5; H, 4.1; F, 21.5. ¹H NMR (500 MHz, CDCl₃, 25 °C): δ 6.3 (3H, w, γ-CH), 3.18 (9H, s, -OCH3), 1.19 (18H, s, -(CH₃)₂) ¹⁹F NMR (470 MHz, C₆D₆, 25 °C): δ 87.5–90.5 multiplets.

3.2. Physical Measurements

The elemental microanalysis (C, H, N) was performed with a Euro EA 3000 elemental analyzer; the content of fluorine was carried out at the laboratory of microanalysis of NIOCH SB RAS (http://web.nioch.nsc.ru/nioch/en/institute-nav/the-centers-of-collective-use accessed on 18 October 2022). To quickly verify the occurrence of both Ln and TM in the same phase, X-ray fluorescence (XRF) with a Bruker M1 Mistral was used. NMR was recorded with a Bruker Avance III/500. The thermal properties of the compounds in the condensed phase were investigated using thermogravimetric and differential thermal analyses (TG-DTA) on a TG 209 F1 Iris (NETZSCH) thermobalance in the standard open corundum crucible. The measurements were performed under atmospheric pressure in helium flow (30–40 cm³ min⁻¹) with a heating rate of 10 °C × min⁻¹ within the temperature range 25–500 °C. The sample weight was ~10 mg. For the XRD study of the solid residue after the compound thermolysis, a ~200 mg sample decomposed in a tube furnace at 600 °C in air.

Single crystals used to determine the structure of 1, 2, 5, 6, 8, and 9 were obtained directly from their solutions after slow evaporation of the solvent (toluene). The unit cell parameters and experimental intensities to solve the crystal structure were measured with a Bruker Kappa Apex II CCD diffractometer (MoKα radiation and graphite monochromator) using φ, ω scans of narrow (0.5°) frames. The structures of 1 and 2 were solved by direct methods by the SHELXS-97 program [26] and 5, 6, 8, and 9 by SHELXT 2014/5 [27]. 1 and 2 were refined in an anisotropic (isotropic for H and F in a minor part of disordered CF₃ groups) approximation using the SHELXL-2014 program [27] and 5, 6, 8, 9—with SHELXL2018/3 [28]. The hydrogens’ positions were calculated with the riding model. The CF₃ groups of both compounds 1 and 2 are disordered due to rotation approximately as 9:1 and ^tBu(C25) group–as 6:4. The ^tBu groups of tmhd in 5 are disordered in approximate ratios 3:1 and 3:2, and CF₃ groups of L¹ in ratios 9:1 and 3:2. In 8, methyl and methoxy groups of L² are disordered in ratio 1:1 for noncoordinated and 3:1 for coordinated methoxy-group. One of ^tBu group of tmhd in 8 is also disordered due to rotation in ratio 3:2. Compounds 1, 2 and 5, 6, 8 demonstrate the same space group, crystal packing and close geometry of the ligands. Asymmetry unit of 9 includes two independent molecules one of which demonstrate disordered due to rotation methoxy-group of L¹ in ratio 3:2. Another one has disordered CF₃ groups in ratio 9:1. Crystallographic data are summarized in Table S1. CCDC deposition numbers: 1534092 for 1, 1534091 for 2, 2175224 for 5, 2175225 for 6, 2175226 for 8, 2175227 for 9. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html, accessed on 18 October 2022 (or from the CCDC, 12 Union Road, Cambridge CB2 1 EZ, UK; Fax: [phone]; E-mail: [email protected]).

The X-ray powder diffraction (XRD) was carried out using a Shimadzu XRD-7000 diffractometer (CuKα radiation, Ni filter, 5 to 50° 2θ angle range and a step 0.03° 2θ) at room temperature and atmospheric pressure. The products were ground in an agate mortar; the powder was deposited onto the polished side of the standard quartz cuvette. A polycrystalline silicon sample prepared similarly was used as the external standard. Indexing of the diffraction patterns was carried out using data for compounds reported in the PDF-2 database [29] and by the results of the single crystal study.

Magnetic properties of polycrystalline samples were studied using a Quantum Design MPMS-XL SQUID magnetometer in the temperature range T = 1.77–300 K at magnetic fields H = 0–10 kOe. To determine the paramagnetic component of the molar magnetic susceptibility χ_p(T), the temperature-independent diamagnetic contribution χ_d and a possible contribution of ferromagnetic micro impurities χ_F were subtracted from the measured values of the total molar susceptibility χ = M/H: χ_p(T,H) = χ(T,H)–χ_d–χ_F(T,H). The value of χ_d was calculated according to the additive Pascal scheme. In its turn the ferromagnetic contribution χ_F, if any, was evaluated from the field dependences of the magnetization M(H) by decomposing the latter into a part changing linearly with a magnetic field (associated with diamagnetic and paramagnetic contributions), and a ferromagnetic part tending to saturate at magnetic fields of a few kOe.

4. Conclusions

This study has shown that the use of fluorinated methoxy-substituted diketones for the synthesis of volatile heterometallic complexes containing lanthanides and typical transition metals still requires a further search for methods and approaches to achieve the desired result. It has been found so far for these systems that during the cocrystallization of monometallic complexes there is the exchange of ligands by redistributing the latter following the principle of concentrating fluorine-containing ligands around lanthanide cations. Apparently, this is due to the fact that the electronegativity of lanthanides is lower than that of transition metals, and they tend to form complexes with a more polar coordination bond. In addition, large coordination numbers lead to the fact that the available methoxy groups are also coordinated by lanthanides without alternatives so that a homometallic aggregate is formed rather than a heterometallic one. The peculiarity of lanthanides is also manifested in that the set of products split into two series for La-Gd and Tb-Lu, which often occurs in their coordination chemistry. In particular, the former tend to form dimers in contrast to the latter. For dimethoxy diketonates L¹ and L² heterometallic complexes are formed for Ln = La-Gd, but not for Ln = Tb-Lu. For mono-methoxy diketonate L³ all Ln under discussion give no heterometallic products. At the same time, the effect of steric factors cannot be excluded, because even the presence of free methoxy groups does not guarantee the formation of heterometallic complexes as, e.g., for [La(L³)₃]₂ (9) or Lu(L³)₃ (12) in contrast to [Ln(L¹)₂tmhd]₂. In addition, the more rigid structure of TM complexes also does not allow them to adjust to it. Nevertheless, a number of unique heterocomplexes with interesting structures were obtained, which will be useful for the further design of polynuclear compounds with the required properties.

In addition, a reliable way to synthesize anhydrous lanthanide complexes with fluorinated diketonates has been found.

Author Contributions

Conceptualization, Methodology, Investigation, Writing—original draft, Supervision, Funding acquisition, V.V.K.; Investigation, Validation, Visualization, S.U.K.; Methodology, Investigation, Validation, Visualization, Writing—original draft, T.V.R.; Investigation, Validation, Visualization, I.V.K.; Methodology, Investigation, Validation, Visualization, Writing—original draft, A.N.L. and M.A.G. All authors have read and agreed to the published version of the manuscript.

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Not applicable.

Acknowledgments

Authors would like to acknowledge the Multi-Access Chemical Service Center SB RAS for spectral and analytical measurements at NIOC and NIIC SB RAS for rendered services. Special thanks are due to the team of the Postovsky Institute of Organic Synthesis, Ural Branch of RAS (IOS UB RAS, www.iosuran.ru (accessed on 18 October 2022)), including D. L. Chizhov, D. N. Bazhin, Y. S. Kudyakova et al. for kindly providing transition metal complexes with bis-methoxy-diketones.

Conflicts of Interest

The authors declare no conflict of interest.

Sample Availability

Samples of the compounds are not available from the authors.

Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Figures, Scheme and Tables

Figure 1. Graphical representation of the used β-diketonate ligands: L1 = 1,1,1-trifluoro-5,5-di-methoxypentane-2,4-dionate; L2 = 1,1,1-trifluoro-5,5-dimethoxyhexane-2,4-dionate; L3 = 1,1,1-tri-fluoro-5-methoxy-5-methylhexane-2,4-dionate; tmhd = 2,2,6,6-tetramethylheptane-3,5-dionate.

Scheme 1. Main reactions of Ln(tmhd)3 and TML2 in organic solvent.

Figure 2. Comparison of experimental powder X-ray diffraction patterns of several heterometallic diketonates.

Figure 3. A fragment of the chain in the structure of 1, 2, 5–6, and 8 (hydrogen atoms are omitted for clarity) with a detailed view of the TM coordination environment, respectively.

Figure 4. Binuclear structure of one of [La(L3)3]2 (9) molecules (a) and its coordination polyhedra representing the LaO10 coordination environment (b).

Figure 5. TG curves of heterometallics 1, 2, 5, and 6.

Figure 6. Comparison of TG data for homometallic tris-diketonates 9, 12 and La(tmhd)3 (He, 10 o/min).

Figure 7. Temperature dependences of the magnetic susceptibility χ measured for the 12 (a) and 11 (b) complexes at the magnetic fields H = 1; 10 kOe.

Figure 8. (a) Temperature dependences of μeff and 1/χp measured for the Dy(L3)3 (11) complex at the magnetic fields H = 1; 10 kOe. The depicted effective moment μeff is calculated for the case of non-interacting magnetic moments (θ = 0). (b) Magnetic-field dependence of the magnetization measured for complex 11 at T = 1.77 K.

Table 1

Comparison of geometry parameters for [(Ln(L¹)₂tmhd)₂TM(tmhd)₂], Ln = La, Pr, M= Cu, Ni, Co.

#-Ln	<Ln-Och>	<Ln-Ochb>	Ln-OCH3 *	Ln_Ln	TM	TM-Och	TM-OCH3	<Och-Ln-Ochb>	Och-TM-Och
1-La	2.46(8)	2.63(2)	2.765(3)2.759(3)	3.854(3)	Cu	1.915(3)1.941(3)	2.604(3)	65.4(4)	92.4(1)
2-Pr	2.42(8)	2.59(1)	2.752(3)2.739(3)	3.793(3)	Cu	1.915(3)1.941(3)	2.602(3)	66.2(4)	92.5(1)
5-La	2.50(8)	2.63(2)	2.767(3)2.747(3)	3.834(3)	Co	1.975(3)2.009(3)	2.370(3)	65.3(4)	70.3(1)
6-La	2.50(8)	2.63(2)	2.769(3)2.753(3)	3.838(3)	Ni	1.956(3)1.992(3)	2.306(3)	65.2(4)	70.5(1)
8-La	2.47(8)	2.65(2)	2.774(3)2.803(3)	3.838(3)	Cu	1.910(3)1.928(3)	2.685(3)	65.3(4)	92.4(1)

Bonds: ch—chelated; chb—chelato-bridged; *—first value is for L where both methoxy groups are coordinated. #—index number of the compound.

Table 2

Selected geometry parameters for 9.

Bond Length, Å			Angle, °
La2-O41	2.504(3)	O41-La2-O42	66.9(9)
La2-O42	2.613(3), 2.612 *	La2-O42-La2	93.1(9)
La2-O43	2.704(3)	O42-La2-O43	58.9(9)
La2-O51	2.505(3)	O51-La2-O52	65.7(9)
La2-O52	2.627(3), 2.622 *	La2-O52-La2	92.6(9)
La2-O53	2.702(3)	O52-La2-O53	56.1(9)
La2-O61	2.490(3)	O61-La2-O62	69.6(9)
La2-O62	2.454(3)

* bridging distance.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules27238400/s1, Table S1: XRD data for complexes 1, 2, 5, 6, 8, 9; Figure S1: A view of the cell packing along Z axis in crystals of 2; Figure S2: XRD data for solid residue after sintering [(La(L¹)₂tmhd)₂Cu(tmhd)₂] in comparison with appropriate PDF files; Figure S3: XRD data for solid residue after sintering [(La(L¹)₂tmhd)₂Co(tmhd)₂] in comparison with appropriate PDF files; Figure S4: XRD data for solid residue after sintering [(La(L¹)₂tmhd)₂Ni(tmhd)₂] in comparison with appropriate PDF files; Figure S5: XRD data for solid residue after sintering [(La(L¹)₂tmhd)₂Mn(tmhd)₂] in comparison with appropriate PDF files; Figure S6: (a) Temperature dependence of the magnetic susceptibility χ measured for the Gd-Cu complex at the magnetic-field H = 1 kOe. (b) Temperature dependences of μ_eff and 1/χp. The depicted effective moment μ_eff is calculated for the case of non-interacting magnetic moments (θ = 0). Pr-Cu complex (2); Figure S7: (a) Temperature dependence of the magnetic susceptibility χ measured for the Pr-Cu complex at the magnetic fields H = 1; 10 kOe. (b) Temperature dependences of μ_eff and 1/χp. The depicted effective moment μ_eff is calculated for the case of non-interacting magnetic moments (θ = 0). Sm-Cu complex (3); Figure S8: (a) Temperature dependence of the magnetic susceptibility χ measured for the Sm-Cu complex at the magnetic fields H = 1; 10 kOe. (b) Temperature dependences of μ_eff and 1/χp. The depicted effective moment μ_eff is calculated for the case of non-interacting magnetic moments (θ = 0). La-Co complex (5); Figure S9: (a) Temperature dependence of the magnetic susceptibility χ measured for the La-Co complex at the magnetic fields H = 1; 10 kOe. (b) Temperature dependences of μ_eff and 1/χp. The depicted effective moment μ_eff is calculated for the case of non-interacting magnetic moments (θ = 0). (b) Magnetic-field dependence of the magnetization measured at T = 1.77 K. La-Ni complex (6); Figure S10: (a) Temperature dependence of the magnetic susceptibility χ measured for the La-Ni complex at the magnetic fields H = 1; 10 kOe. (b) Temperature dependences of μ_eff and 1/χp. The depicted effective moment μ_eff is calculated for the case of non-interacting magnetic moments (θ = 0).

References

1. Long, J.; Guari, Y.; Ferreira, R.A.S.; Carlos, L.D.; Larionova, J. Recent Advances in Luminescent Lanthanide Based Single-Molecule Magnets. Coord. Chem. Rev.; 2018; 363, pp. 57-70. [DOI: https://dx.doi.org/10.1016/j.ccr.2018.02.019]

2. Jia, J.H.; Li, Q.W.; Chen, Y.C.; Liu, J.L.; Tong, M.L. Luminescent Single-molecule Magnets Based on Lanthanides: Design Strategies, Recent Advances and Magneto-luminescent Studies. Coord. Chem. Rev.; 2019; 378, pp. 365-381. [DOI: https://dx.doi.org/10.1016/j.ccr.2017.11.012]

3. Liu, C.M.; Zhang, D.Q.; Su, J.B.; Zhang, Y.Q.; Ben Zhu, D. Single-Molecule Magnet Behavior of 1D Coordination Polymers Based on DyZn₂(salen)₂ Units and Pyridin- N-Oxide-4-Carboxylate: Structural Divergence and Magnetic Regulation. Inorg. Chem.; 2018; 57, pp. 11077-11086. [DOI: https://dx.doi.org/10.1021/acs.inorgchem.8b01653] [PubMed: https://www.ncbi.nlm.nih.gov/pubmed/30137978]

4. Feltham, H.L.C.; Brooker, S. Review of Purely 4f and Mixed-metal nd-4f Single-molecule Magnets Containing Only One Lanthanide Ion. Coord. Chem. Rev.; 2014; 276, pp. 1-33. [DOI: https://dx.doi.org/10.1016/j.ccr.2014.05.011]

5. Liu, K.; Shi, W.; Cheng, P. Toward Heterometallic Single-Molecule Magnets: Synthetic Strategy, Structures and Properties of 3d-4f Discrete Complexes. Coord. Chem. Rev.; 2015; 289–290, pp. 74-122. [DOI: https://dx.doi.org/10.1016/j.ccr.2014.10.004]

6. Skaribas, S.P.; Pomonis, P.J.; Sdoukos, A.T. Low-Temperature Synthesis of Perovskite Solids LaMO₃ (M = Ni, Co, Mn) via Binuclear Complexes of Compartmental Ligand N,N′-bis(3-Carboxysalicylidene)ethylenediamine. J. Mater. Chem.; 1991; 1, pp. 781-784. [DOI: https://dx.doi.org/10.1039/JM9910100781]

7. Hasegawa, E.; Aono, H.; Igoshi, T.; Sakamoto, M.; Traversa, E.; Sadaoka, Y. Preparation of YBa₂Cu₃O₇. J. Alloys Compd.; 1999; 287, pp. 150-158. [DOI: https://dx.doi.org/10.1016/S0925-8388(99)00076-6]

8. Kuzmina, N.P.; Malkerova, I.P.; Alikhanyan, A.S.; Gleizes, A.N. The Use of 3d-Metal Complexes as Ligands to Prepare Volatile 4f-3d Heterobimetallic Complexes. J. Alloys Compd.; 2004; 374, pp. 315-319. [DOI: https://dx.doi.org/10.1016/j.jallcom.2003.11.098]

9. Mishra, S.; Daniele, S. Metal–Organic Derivatives with Fluorinated Ligands as Precursors for Inorganic Nanomaterials. Chem. Rev.; 2015; 115, 8379. [DOI: https://dx.doi.org/10.1021/cr400637c]

10. Krisyuk, V.V.; Urkasym Kyzy, S.; Rybalova, T.V.; Baidina, I.A.; Korolkov, I.V.; Chizhov, D.L.; Bazhin, D.N.; Kudyakova, Y.S. Isomerization as a Tool to Design Volatile Heterometallic Complexes with Methoxy-Substituted β-Diketonates. J. Coord. Chem.; 2018; 71, pp. 2194-2208. [DOI: https://dx.doi.org/10.1080/00958972.2018.1479746]

11. Krisyuk, V.V.; Tkachev, S.V.; Baidina, I.A.; Korolkov, I.V.; Turgambaeva, A.E.; Igumenov, I.K. Volatile Pd-Pb and Cu-Pb Heterometallic Complexes: Structure, Properties, and Trans-to-cis Isomerization under Cocrystallization of Pd and Cu β-Diketonates with Pb Hexafluoroacetylacetonate. J. Coord. Chem.; 2015; 68, pp. 1890-1902. [DOI: https://dx.doi.org/10.1080/00958972.2015.1035653]

12. Urkasym kyzy, S.; Krisyuk, V.V.; Turgambaeva, A.E.; Baidina, I.A.; Komarov, V.Y.; Korotaev, E.V.; Korolkov, I.V. Methoxy-Substituted Transition Metal β-Diketonates: Synthesis and Properties. J. Struct. Chem.; 2019; 60, pp. 1635-1647. [DOI: https://dx.doi.org/10.1134/S0022476619100093]

13. Kudyakova, Y.S.; Slepukhin, P.A.; Valov, M.S.; Burgart, Y.V.; Saloutin, V.I.; Bazhin, D.N. A Rare Example of Discrete Lanthanide–Lithium Tetrakis-β-Diketonates: Synthesis, Structures, and Luminescence Properties. Rus. J. Coord. Chem.; 2020; 46, pp. 545-552. [DOI: https://dx.doi.org/10.1134/S1070328420070027]

14. Kudyakova, Y.S.; Slepukhin, P.A.; Valova, M.S.; Burgart, Y.V.; Saloutin, V.I.; Bazhin, D.N. The Impact of the Alkali Metal Ion on the Crystal Structure and (Mechano)luminescence of Terbium(III) Tetrakis(β-diketonates). Eur. J. Inorg. Chem.; 2020; 2020, pp. 523-531. [DOI: https://dx.doi.org/10.1002/ejic.201901202]

15. Kudyakova, Y.S.; Slepukhin, P.A.; Valova, M.S.; Burgart, Y.V.; Saloutin, V.I.; Bazhin, D.N. Role of Alkyl Substituents in the Structure and Luminescence Properties of Discrete Terbium(III)-Lithium(I) β-Diketonates. J. Mol. Struct.; 2021; 1226, 129331. [DOI: https://dx.doi.org/10.1016/j.molstruc.2020.129331]

16. Kudyakova, Y.S.; Slepukhin, P.A.; Valova, M.S.; Burgart, Y.V.; Saloutin, V.I.; Bazhin, D.N. Functionalized Trifluoromethyl-Containing Lithium β-Diketonate in the Synthesis of Homo- and Heteronuclear Complexes of Rare-Earth Metals. Rus. J. Coord. Chem.; 2021; 47, pp. 280-295. [DOI: https://dx.doi.org/10.1134/S1070328421040059]

17. Yuikhan, L.; Mosyagina, S.A.; Stabnikov, P.A.; Alferova, N.I.; Korol‘kov, I.V.; Pervukhina, N.V.; Morozova, N.B. Structure of Lanthanum(III) tris-Dipivaloylmethanate. J. Struct. Chem.; 2017; 58, pp. 843-846. [DOI: https://dx.doi.org/10.1134/S0022476617040333]

18. Blundell, S. Magnetism in Condensed Matter; Oxford University Press: Oxford, UK, 2001; ISBN-10: 0198505914

19. Bernot, K.; Luzon, J.; Bogani, L.; Etienne, M.; Sangregorio, C.; Shanmugam, M.; Caneschi, A.; Sessoli, R.; Gatteschi, D. Magnetic Anisotropy of Dysprosium(III) in a Low-Symmetry Environment: A Theoretical and Experimental Investigation. J. Am. Chem. Soc.; 2009; 131, pp. 5573-5579. [DOI: https://dx.doi.org/10.1021/ja8100038]

20. Zhang, P.; Guo, Y.N.; Tang, J. Recent Advances in Dysprosium-Based Single Molecule Magnets: Structural Overview and Synthetic Strategies. Coord. Chem. Rev.; 2013; 257, pp. 1728-1763. [DOI: https://dx.doi.org/10.1016/j.ccr.2013.01.012]

21. Zvezdin, A.K.; Matveev, V.M.; Mukhin, A.A.; Popov, A.I. Rare Earth Ions in Magnetically Ordered Crystals; Nauka: Moscow, Russia, 1985.

22. Boča, R. Zero-field splitting in metal complexes. Coord. Chem. Rev.; 2004; 248, pp. 757-815. [DOI: https://dx.doi.org/10.1016/j.ccr.2004.03.001]

23. Chizhov, D.L.; Belyaev, D.V.; Yachevskii, D.S.; Rusinov, G.L.; Chupakhin, O.N.; Charushin, V.N. Efficient and Scalable Synthesis of 3-(polyfluoroacyl)pyruvaldehydes Dimethyl Acetals: A Novel Functionalized Fluorinated Building-Block. J. Fluor. Chem.; 2017; 199, pp. 39-45. [DOI: https://dx.doi.org/10.1016/j.jfluchem.2017.04.009]

24. Bazhin, D.N.; Chizhov, D.L.; Röschenthaler, G.V.; Kudyakova, Y.S.; Burgart, Y.V.; Slepukhin, P.A.; Saloutin, V.I.; Charushin, V.N. A Concise Approach to CF₃-Ccontaining Furan-3-ones, (Bis)pyrazoles from Novel Fluorinated Building Blocks Based on 2,3-Butanedione. Tetrahedron Lett.; 2014; 55, pp. 5714-5717. [DOI: https://dx.doi.org/10.1016/j.tetlet.2014.08.046]

25. Kudyakova, Y.S.; Onoprienko, A.Y.; Edilova, Y.O.; Burgart, Y.V.; Saloutin, V.I.; Bazhin, D.N. Effect of the Nature of a Fluorinated Substituent on the Synthesis of Functionalized 1,3-Diketones. Rus. Chem. Bull. Int. Ed.; 2021; 70, pp. 745-752. [DOI: https://dx.doi.org/10.1007/s11172-021-3145-z]

26. Sheldrick, G.M. A Short History of SHELX. Acta Crystallogr. Sect. A; 2008; 64, pp. 112-122. [DOI: https://dx.doi.org/10.1107/S0108767307043930] [PubMed: https://www.ncbi.nlm.nih.gov/pubmed/18156677]

27. Sheldrick, G.M. SHELXT—Integrated Space-Group and Crystal-Structure Determination. Acta Crystallogr. Sect. A; 2015; 71, pp. 3-8. [DOI: https://dx.doi.org/10.1107/S2053273314026370] [PubMed: https://www.ncbi.nlm.nih.gov/pubmed/25537383]

28. Sheldrick, G.M. Crystal Structure Refinement with SHELXL. Acta Crystallogr. Sect. C; 2015; 71, pp. 3-8. [DOI: https://dx.doi.org/10.1107/S2053229614024218]

29. Gates-Rector, S.; Blanton, T. The Powder Diffraction File: A Quality Materials Characterization Database. Powder Diffr.; 2019; 34, pp. 352-360. [DOI: https://dx.doi.org/10.1017/S0885715619000812]