High-Temperature Spin Crossover in Iron(II) Complexes with 2,6-Bis(1H-imidazol-2-yl)pyridine

Abstract

Novel iron(II) coordination compounds containing a ligand 2,6-bis(1H-imidazol-2-yl)pyridine (L), having such a composition as [FeL₂]SO₄·0.5H₂O, [FeL₂]Br₂·H₂O, [FeL₂](ReO₄)₂, [FeL₂]B₁₀H₁₀∙H₂O, [FeL₂]B₁₂H₁₂∙1.5H₂O had been synthesized and studied using UV-Vis (diffuse reflectance), infrared, extended X-ray absorption fine structure (EXAFS), and Mössbauer spectroscopy methods, as well as X-ray diffraction and static magnetic susceptibility methods. The analysis of the μ_eff(T) dependence in the temperature range of 80–600 K have shown that all the obtained complexes exhibit a high-temperature spin crossover ¹A₁ ↔ ⁵T₂.

1. Introduction

Searching for novel coordination compounds wherein the spin state of the central atom can be switched by an external action is an urgent problem. This is indicated by regularly appearing publications in the literature devoted to this topic [1,2,3,4,5,6,7,8]. These compounds include iron(II) complexes with spin crossover (SCO) ¹A₁ ↔ ⁵T₂. The change in spin multiplicity occurs owing to affecting temperature, pressure, irradiation with light of a certain wavelength (LIESST effect), high-frequency magnetic or electric field, and other factors. The transition from a low-spin (LS) to a high-spin (HS) state causes a change in the magnetic, optical, and vibrational properties of the complexes. An important property associated with the spin transition consists in changing metal–donor interatomic distance amounting to 0.2 Å in the case of Fe(II) complexes. Owing to the universal properties of complexes with SCO they have a wide range of potential applications in making optoelectronic, molecular electronic, and spintronic devices [9,10,11,12,13,14,15]. At present, polyfunctional materials combining SCO and other properties are under active study [16,17,18,19].

2,6-Bis(1H-imidazol-2-yl)pyridines represent a promising class of potential ligands for the synthesis of complexes with SCO [20]. Earlier, we have reported the studies on iron(II) complexes with 2,6-bis(benzimidazol-2-yl)- and 2,6-bis(4,5-dimethyl-1H-imidazol-2-yl)pyridine [21,22,23,24], wherein SCO is exhibited. It seemed worthwhile to continue these investigations into synthesizing and studying Fe(II) complexes with 2,6-bis(1H-imidazol-2-yl)pyridine (Scheme 1), which does not contain substituents at the imidazole fragment. Earlier, this ligand was used in order to synthesize complexes with Ru(II), and with a number of metals belonging to the first transition series [25,26,27,28,29]. The X-ray diffraction data have shown that L is coordinated to the metal ion in a tridentate-cyclic manner by two nitrogen atoms belonging to two imidazole rings and one nitrogen atom belonging to pyridine.

2. Materials and Methods

2.1. Materials

Commercial metal salts and solvents without further purification were used in the synthesis. 2,6-Bis(imidazol-2-yl)pyridine was synthesized as described in [30] (NMR spectra of ligand given in the Supplementary Materials, Figures S1–S4); K₂B₁₀H₁₀·2H₂O, K₂B₁₂H₁₂ were obtained according to the procedure [31].

2.2. Synthesis of [FeL₂]SO₄ 0.5H₂O (1·0.5H₂O)

A 0.28 g (1 mmol) sample of FeSO₄·7H₂O with the addition of 0.1 g of ascorbic acid was dissolved in 10 mL of water under heating; a 0.51 g (2 mmol) L was dissolved in 10 mL of ethanol, and the solutions were then heated and mixed. The resulting solution was evaporated until a red-violet precipitate began to form. After the solution with the precipitate was cooled in a crystallizer with ice, the precipitate was filtered off, washed twice with small portions of water, and dried in air. Yield: 55%. Anal. Calc. for C₂₂H₁₉FeN₁₀O_9/2S, (583.4): C, 45.3; H, 3.3; N, 24.0. Found: C, 46.2; H, 3.5; N, 23.4.

2.3. Synthesis of [FeL₂]Br₂·H₂O (2·H₂O) and [FeL₂](ReO₄)₂ (3)

A 0.28 g (1 mmol) sample of FeSO₄·7H₂O was dissolved in 5 mL of distilled water acidified with 0.1 g of ascorbic acid. An excess (0.43 g, 1.5 mmol) of KReO₄ or KBr (0.36 g, 3 mmol) in 10 mL of water and a solution of L (0.51 g, 2 mmol) in 10 mL of ethanol were successively added to the resulting solution under stirring. The resulting solution was evaporated until a red-violet precipitate began to form. After the solution with the precipitate was cooled in a crystallizer with ice, the precipitate was filtered off, washed twice with small portions of water, and dried in air. Yield: 70% (2·H₂O), 30% (3). Anal. Calc. for C₂₂H₂₀Br₂FeN₁₀O, (656.1): C, 40.3; H, 3.1; N, 21.3. Found: C, 41.3; H, 3.2; N, 21.0. Anal. Calc. for C₂₂H₁₈FeN₁₀O₈Re₂, (978.7): C, 27.0; H, 1.9; N, 14.3. Found: C, 27.5; H, 2.2; N, 14.6.

2.4. Synthesis of [FeL₂]B₁₀H₁₀∙H₂O (4∙H₂O) and [FeL₂]B₁₂H₁₂∙1.5H₂O (5·1.5H₂O)

A 0.14 g (0.5 mmol) sample of FeSO₄·7H₂O was dissolved in 3 mL of distilled water acidified with 0.05 g of ascorbic acid. An excess (0.23 g, 1 mmol) of K₂B₁₀H₁₀∙2H₂O or K₂B₁₂H₁₂ (0.22 g, 1 mmol) in 10 mL of water and a solution of L (0.21 g, 1 mmol) in 5 mL of ethanol were added to the resulting solution under stirring. Red-brown precipitates began to form immediately. Each precipitate was filtered off, washed twice with small portions of water and ethanol, and dried in air. Yield: 45% (4∙H₂O), 68% (5∙1.5H₂O). Anal. Calc. for C₂₂H₃₀B₁₀FeN₁₀O, (614.5): C, 43.0; H, 4.9; N, 22.8. Found: C, 42.5; H, 5.0; N, 22.1. Anal. Calc. for C₂₂H₃₃B₁₂FeN₁₀O_3/2, (647.1): C, 40.8; H, 5.1; N, 21.6. Found: C, 40.6; H, 5.3; N, 20.9.

2.5. Measurement and Characterization

The data for elemental analysis of the complexes was acquired on a EURO EA 3000 analyzer (EuroVector, Pavia, Italy).

X-ray absorption spectra (XAS) in the Fe K edge region (150 eV before and 800 eV after) were measured in the transmission mode with the use of synchrotron radiation on the 8 beamline, VEPP-3 storage ring at the Siberian Synchrotron and Terahertz Radiation Center (Budker Institute of Nuclear Physics, Siberian Branch, Russian Academy of Sciences, Novosibirsk, Russia) [32]. A Si(111) cut-off crystal was used as a two-crystal monochromator. The operating mode of the storage ring during measurement: energy—2 GeV; current—70–140 mA. For measurements, the samples were mixed with cellulose powder as a filler and pressed into tablets. The mass of the sample was calculated so that the absorption jump at the Fe K-edge was 0.8–1. The preprocessing of the absorption spectra (selection of the oscillating part—EXAFS spectra) was performed with the use of the VIPER 10.17 program [33]. The “radial pair distribution function” (Figure 1) was obtained by the Fourier transform of the k³-weighted EXAFS function in the range of wave vectors k = 2.0–11.0 Å⁻¹.

The local environment of the Fe ion [interatomic distances (R_i) and angles (Q_i), coordination numbers (N_i), and Debye–Waller factors (σ²)] was modeled using the EXCURVE 98 cod [34]. In this program phase and amplitude characteristics were calculated in the von-Bart and Hedin approximation. The amplitude suppression factor S₀² due to multielectron processes was determined for the crystallographically characterized compound (S₀² = 0.85) and fixed during further modeling of the studied compounds spectra. The Debye–Waller factor was the same separately for nitrogen and carbon atoms.

IR spectra were taken on a Scimitar FTS 2000 in the range of 4000–400 cm⁻¹ and a Vertex 80 in the range of 600–100 cm⁻¹. Compound samples were prepared as suspensions in vaseline and fluorinated oils and in polyethylene.

The Kubelka-Munk diffuse reflectance spectra were obtained on a Shimadzu UV-3101 PC scanning spectrometer.

The XRD investigation of polycrystalline samples was performed using a Shimadzu XRD 7000 diffractometer (CuK_α radiation).

The static magnetic susceptibility was measured using Faraday balance type setup equipped with electromagnetic compensating torsion quartz microbalance. The Delta DTB9696 temperature controller (Delta Electronics Inc., Taipei, Taiwan) was used for the investigated compounds temperature stabilization (~1 K) in the range of temperatures 80–600 K. The temperature scanning rate for the process of heating or cooling samples was ~1 K/min. The magnetic field strength (7300 Oe) stabilization precision was ~2%. The compounds studied were sealed in quartz cellules filled with atmospheric air at 760 Torr. In order to study the effect of crystallization water, the samples were placed in open quartz ampoules and vacuumed at 10⁻² Torr, after which the helium atmosphere at 5 Torr was formed.

The effective magnetic moment of studied compounds was calculated as:

$${\mu }_{eff}={\left(\frac{3k}{N_A{\mu }_B^2}\cdot \chi T\right)}^{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.}\approx {(8\chi T)}^{\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.},$$

k—Boltzmann constant, N_A—Avogadro constant, and µ_B—Bohr magneton. In the above formula, the diamagnetic contribution in total magnetic susceptibility (χ) was taken into account using the method of Pascal’s constants. The direct (T_c↑) and reverse (T_c↓) transitions temperatures were obtained using condition the magnetic moment second derivative zero value (d²(µ_eff(T))/dT² = 0).

The Mössbauer spectra were collected with a spectrometer NP-610 (KFKI, Budapest, Hungary), using ⁵⁷Co in a metal Rh matrix as a radioactive source. The spectra were measured at a room temperature. The spectra were processed to find the values of isomer shift δ and quadrupole splitting ε. The isomer shifts are given relative to metal iron.

3. Results and Discussion

Iron(II) complexes with 2,6-bis(1H-imidazol-2-yl)pyridine were isolated from aqueous-ethanol solutions. To maintain the oxidation state of iron(II), ascorbic acid was added to the solution.

Complex 1·0.5H₂O was synthesized by reacting stoichiometric amounts of FeSO₄ and L. Syntheses 2·H₂O, 3, 4∙H₂O, 5·1.5H₂O were carried out in two stages. At the first stage, the corresponding iron(II) salts were obtained by adding a 1.5- or 2-fold excess of KBr, KReO₄, K₂B₁₀H₁₀ or K₂B₁₂H₁₂ into a solution of FeSO₄ salt. At the second stage, a solution of the ligand in ethanol was added to the resulting salt solution. The obtained diffraction patterns show that the synthesized compounds are crystalline, while [FeL₂]SO₄·0.5H₂O and [FeL₂]Br₂·H₂O, as well as [FeL₂]B₁₀H₁₀∙H₂O and [FeL₂]B₁₂H₁₂∙1.5H₂O are isotypical.

The structure of the whole molecule for all complexes in the LS state (T = 297 °C) was established from the EXAFS data using the multiple scattering approximation within the software package EXCURV (except for [FeL₂](ReO₄)₂ (3)) excluding hydrogen atoms, and anions that exert only a weak effect on the shape of the EXAFS spectrum owing to their spatial separation from the central iron ion. For complex 3, the signal-to-noise ratio in the EXAFS spectrum is worse than that for the spectra of other complexes owing to the presence of a heavy anion ReO₄⁻. Simulation of the whole molecule in the multiple scattering approximation gives too large errors in determining the parameters. Therefore, the simulation of the EXAFS spectrum for complex 3 could be carried out only in a single scattering approximation. The structure of the complexes in the LS state (by the example of complex 4∙H₂O) obtained by means of EXAFS spectra simulation is presented in Figure 2.

Table 1. Microstructure parameters of the Fe coordination site for the complexes at T = 300 K (LS) obtained by EXAFS fitting with multiple scattering approximation (R_i—interatomic distance, 2σ_i²—Debye–Waller factor, F_i—the statistical error of the fitting).

Bonds	Ri, Å				Angles	Ω, Deg.
	1·0.5H2O	2·H2O	4∙H2O	5·1.5H2O		1·0.5H2O	2·H2O	4∙H2O	5·1.5H2O
Fe(1)-N(1)	1.96	1.97	1.98	1.94	N(1)Fe(1)N(8)	107.9	102.6	105.9	102.6
Fe(1)-N(3)	1.96	1.91	1.93	1.95	N(1)Fe(1)N(6)	95.3	92.5	95.1	100.1
Fe(1)-N(4)	1.95	1.97	1.98	1.93	N(1)Fe(1)N(9)	97.1	92.1	96.6	102.2
Fe(1)-N(6)	1.95	1.96	1.98	1.96	N(1)Fe(1)N(3)	75.2	79.8	75.6	85.3
Fe(1)-N(8)	1.86	1.88	1.90	1.86	N(3)Fe(1)N(9)	97.8	102.1	100.3	102.9
Fe(1)-N(9)	1.96	1.95	1.96	1.96	N(3)Fe(1)N(4)	75.8	81.2	80.6	73.7
2σ2 (Fe-N), Å2	0.014	0.013	0.013	0.012	Fi (*)	2.7	2.5	1.8	1.6

* The determination accuracy for parameters (interatomic distances and angles) based on the EXAFS data is ±1% (for the nearest sphere of the environment). $F_i={{\displaystyle \sum }}_i^N{w}_i^2{\left({\chi }_i^{exp}\left(k\right)-{\chi }_i^{th}\left(k\right)\right)}^2,w_i=\frac{k_i^n}{{{\displaystyle \sum }}_i^N{k}_i^n\vee {\chi }_j^{exp}\left(k\right)\vee }$.

lists the microstructure parameters of the coordination site for complexes 1·0.5H₂O, 2·H₂O, 4∙H₂O, 5·1.5H₂O.

The structure of the coordination site of complex [FeL₂](ReO₄)₂ (3) in the LS state was obtained from modeling the spectrum filtered in real space (ΔR = 0.9 to 3.0 Å). The simulation data are presented in

Table 2. Microstructure parameters for complex [FeL₂](ReO₄)₂ in the LS state obtained by single-scattering EXAFS data fitting.

Compound	Central Ion–Scattering Atom	Ni	Ri, Å	2σi2, Å2	Fi
[FeL2](ReO4)2	Fe–N	6	1.96	0.010	2.7
	Fe–C	8	2.78	0.014
	Fe–C	4	3.20

. The coordination numbers of the nearest spheres of the iron ion environment were fixed in accordance with the data obtained in the simulation of complexes in the LS state in the multiple scattering approximation.

Figure 3 illustrates a comparison of the experimental and simulated radial distribution function for [FeL₂]B₁₀H₁₀∙H₂O. The simulation was carried out using a multiple scattering approximation.

Table 3. The main vibrational frequencies (cm⁻¹) in the spectra of L and complexes.

L	1·0.5H2O	2·H2O	3	4·H2O	5·1.5H2O	Assignment
	3485	3433		3225	3269	ν(OH)
3100w	3020w	3147 3116	3050w	3151 3130	3148 3129	ν(NH)
3079 3035	3060 3021	3067	3067	2954 2924 2854	2988 2040 2849	ν(CH)
1598 1573 1552	1595 1570 1550	1569 1551 1479	1593 1566 1552	1622 1558 1490 1469	1622 1558 1490 1471	Rring
	1118 1085 1070					ν(SO4)
			903			ν(ReO4)
				2473	2493	ν(B-H)
				1086 1036	1105 1054	δ(BBH)
	496	491	485	485	484	Fe(3d6)–ligand (π) charge-transfer transition
	385 356 330	376 334	381 321	334	333	ν(M-N)

and Figures S5–S7 show the main vibration frequencies in the spectra of L and Fe(II) complexes. In the high-frequency spectral region for 1·0.5H₂O, 2·H₂O, 4∙H₂O, 5·1.5H₂O, ν(OH) vibrations are observed; in the wave number range of 3200–3050 cm⁻¹ for all the complexes there are stretching vibrations of NH-groups, and in the range of 3100–2850 cm^–1 there are vibrations of ν(CH). In the wave number range of 1650–1450 cm⁻¹, there are stretching and bending vibration bands inherent in heterocyclic rings. The spectra of the complexes in the range of ring vibrations exhibit a change in the number and position of the imidazole and pyridine bands in comparison with the spectrum of the ligand, which indicates the coordination of nitrogen atoms of the rings to Fe(II) ions. The presence of non-split bands inherent in stretching vibrations characteristic of the SO₄²⁻ and ReO₄⁻ anions indicates the fact that they are in outer-sphere position. The vibration bands of the B–H bonds of the outer-sphere anions B₁₀H₁₀²⁻ and B₁₂H₁₂²⁻ are centered at the wave numbers of 2470 (ν(BH)) and 1075 cm⁻¹ (δ(BBH)). In the case of the spectra for 4∙H₂O, 5·1.5H₂O they are shifted with respect to those observed in the spectra of the initial salts, which could be, to all appearance, caused by the formation of H₂O^{δ− … δ+}H–B bonds. In the far region of the spectra of all the complexes, Fe(3d⁶)–ligand(π) charge-transfer transition bands and vibration bands (M-N) are observed. The position of these bands is typical for the spectra of low-spin octahedral iron(II) complexes [35].

The diffuse reflectance spectra (DRS, Figures S8–S12) of all the obtained complexes exhibit intense metal-ligand charge transfer bands ν₁(e_g → ${\pi }_{\mathrm{L}}^{*}$) in the wavelength range of 300–350 nm (λ_max ≈ 324–326 nm). The DRS of 4∙H₂O and 5∙1.5H₂O exhibit three absorption bands, too, (see

Table 4. Parameters of diffuse reflectance spectra.

Complex	λ(1A1 → 1T2)	λ(1A1 → 1B2)	λ(1A1 → 1T1)	λ(1A1 → 1A2)	λ(1A1 → 1E)	Calculated Parameter
						B	C	∆LS
1·0.5H2O		454		613	536
2·H2O		454		624	539
3		432		603	503
4·H2O	475		518	620		109.3	482.0	1.97 × 104
5·1.5H2O	465		518	620		137.5	606.5	1.98 × 104

); they correspond to the ¹A₁ → ¹T₂, ¹A₁ → ¹T₁ and ¹A₁ → ¹A₂ transitions in the strong octahedral field of the ligands. For low-spin axially distorted octahedral iron(II) complexes, the term ¹T₁ is transformed according to the representation of ¹E + ¹A₂, whereas term ¹T₂ is transformed according to the representation of ¹E + ¹B₂ [36]. Therefore, the ¹A₁ → ¹B₂, ¹A₁ → ¹A₂ and ¹A₁ → ¹E wide transition bands (see Table 4) observed in the spectra of 1·0.5H₂O, 2·H₂O and 3, indicate the fact that an axial distortion of the octahedral coordination of these complexes occur. Low-intensity transitions and overlapping three wide bands do not make it possible to perform reliable quantitative calculations of crystal field parameters in this case. The spectra of all the complexes do not exhibit the ⁵T₂ → ⁵E band, which is caused by the HS state of iron(II). We were able to calculate the splitting parameters based on the difference between ¹A₁ → ¹T₂ and ¹A₁ → ¹T₁ absorption frequencies [36] for low-spin (LS) forms of complexes with closo-borate anions. The B values were computed using the formula 16B = [ν (¹A₁ → ¹T₂) − ν (¹A₁ → ¹T₁)]. The values C and Δ_LS (Table 4) were calculated using the equations: ν_LS = Δ_LS − C + 86B²/Δ_LS and C = 4.41·B [36,37,38]. The obtained data show that 2,6-bis(1H-imidazol-2-yl)pyridine is a strong field ligand. In addition, these data, as well as the values obtained for a number of previously synthesized Fe(II) complexes with 2,6-bis(benzimidazol-2-yl)pyridine and 2,6-bis(4,5-dimethyl-1H-imidazole) [22,23,24], obey the inequality that reflects the condition for the manifestation of SCO [37]: 19.000 cm⁻¹ ≤ Δ_LS ≤ 22.000 cm⁻¹.

The Mössbauer spectra of complexes 1·0.5H₂O, 2·H₂O, 3 and 5·1.5H₂O represent quadrupole doublets whose parameters correspond to the LS state of iron(II) (Figure 4). The spectrum of 4·H₂O also exhibits a broadened doublet related to the HS form of the complex (36%). The parameters of the Mössbauer spectra are presented in

Table 5. Mössbauer spectra parameters of the complexes.

Complex	δ, mm/s	ε, mm/s	Γ, mm/s
1·0.5H2O	0.269	0.364	0.33
2·H2O	0.266	0.342	0.25
3	0.288	0.464	0.28
4∙H2O	0.278 (64%) 0.925 (36%)	0.420 2.224	0.26 0.80
5·1.5H2O	0.282	0.465	0.25

.

The temperature dependences of the effective magnetic moment for the analyzed complexes are shown in Figure 5. Spin crossover (SCO) is observed for all the compounds under investigation. In the case of complexes 1·0.5H₂O, 2·H₂O, 3 the µ_eff values observed in the thermal stability range (2.35, 2.1 and 3.35 µ_Β, respectively), are significantly lower than the theoretical spin-only value of 4.9 µ_Β for the Fe(II) ion. The 4∙H₂O and 5∙1.5H₂O complexes are more stable and thus a temperature of 600 K could be reached. For these compounds, a complete spin-crossover is observed. However, the µ_eff values observed in the HS state of these compounds are also lower than the theoretical value for Fe(II). It should be noted that the experimental µ_eff values for 4∙H₂O and 5∙1.5H₂O complexes are in the range of 4.6–5.7 observed for Fe(II) compounds [39,40]. In the case of 1·0.5H₂O and 2·H₂O the residual effective magnetic moment in LS state (0.65 and 0.4 µ_Β, respectively), is presented by µ_eff(T) dependences. This fact could be connected with temperature-independent paramagnetism. Complexes 3_, 4∙H₂O and 5∙1.5H₂O in LS state exhibit diamagnetism with a zero µ_eff value. Despite the fact that low µ_eff values are achieved in the investigated temperature range for 1·0.5H₂O and 3, the condition of d²(µ_eff(T))/dT² = 0 could be satisfied and some values of SCO temperature could be determined.

Table 6. The temperatures of direct (T_c↑) and inverse (T_c↓) SCO for the studied complexes.

Complex	Tc↑, K	Tc↓, K
[FeL2]SO4·0.5H2O	>420	409
[FeL2]Br2·H2O	>420	>420
[FeL2](ReO4)2	340	340
[FeL2]B10H10·H2O	436	436
[FeL2]B12H12·1.5H2O	455	455
[FeL2]B10H10	447	440
[FeL2]B12H12	458	458

shows the temperature values of direct (T_c↑) and inverse (T_c↓) transitions. For the [FeL₂]Br₂·H₂O one could suggest that the SCO temperature is higher than 420 K. The determined temperature of the inverse transition increases in a series of [FeL₂](ReO₄)₂ → [FeL₂]SO₄·0.5H₂O → FeL₂]B₁₀H₁₀·H₂O → [FeL₂]B₁₂H₁₂·1.5H₂O.

The effect of the crystallization of water has been studied for 4·H₂O and 5·1.5H₂O complexes (Figure 6). It should be noted that in the case of rarefied atmosphere the decomposition of the dehydrated complexes occurs in a lower temperature range than it is observed for initial compounds. Nevertheless, the SCO has been observed in this case, too. The µ_eff value of 4.65 µ_Β achieved in HS state for 4 corresponds to the value observed for the initial complex. In the case of 5 complex, the µ_eff value (4.6 µ_Β) exhibits an increase after dehydration. Residual µ_eff values (~1–1.5 µ_Β) have been registered to occur for both complexes in the LS state. The SCO temperature increases after dehydration; however, the 5 complex demonstrates the highest SCO temperature values as it is observed in the case of the initial compound. Thus, the dehydration of 4·H₂O and 5·1.5H₂O complexes lead to appearing residual µ_eff value and to an increase in the temperature of SCO.

4. Conclusions

In this work, we have synthesized and investigated five novel coordination compounds of various iron(II) salts with 2,6-bis(1H-imidazol-2-yl)pyridine (L). The structure of the coordination core of the complexes has been determined by means of EXAFS spectra simulation. Two ligand molecules are coordinated to the iron(II) ion in a tridentate-cyclic fashion by the nitrogen atom belonging to pyridine and two nitrogen atoms belonging to imidazole rings. Thus, the complexes have the distorted-octahedral structure of the coordination polyhedron, the FeN₆ core. The studies on the µ_eff(T) dependence have shown that complexes having such a composition as [FeL₂]SO₄·0.5H₂O, [FeL₂]Br₂·H₂O, [FeL₂](ReO₄)₂, [FeL₂]B₁₀H₁₀·H₂O, [FeL₂]B₁₂H₁₂·1.5H₂O exhibit an ¹A₁ ↔ ⁵T₂ high-temperature spin crossover. A comparison of the data obtained for the synthesized compounds with those obtained by us earlier [21,22,23,24] shows that spin-crossover ¹A₁ ↔ ⁵T₂ is observed in all complexes of Fe(II) with 2,6-bis(imidazole-2-yl)pyridines. The temperatures of direct SCO, T_c↑, in most compounds are significantly higher than room temperature.