The transamination reaction used in the synthesis of ethyl-4H-1,2,4-triazol-4-yl-acetate and 4H-1,2,4-triazol-4-yl acetic acid [12] proved to be a good synthetic strategy to build a β-amino-acid triazole. The synthetic route, starting with β-Alanine ethyl ester hydrochloride and N,N-Dimethylformamide-azine, helped us to obtain a new molecule, βAlatrz, with a good yield. The synthesis time is relatively longer than the synthesis of previous ligands and the final product had to be purified by “flash” column chromatography.

A 1D coordination polymer was obtained as a white powder by reaction of the corresponding Fe^II inorganic precursor, prepared in air, [Fe(H₂O)₆](CF₃SO₃)₂ [17] with a methanolic solution of βAlatrz. This complex was successfully characterized by elemental analysis, TGA-DTA analyses, atomic absorption (AAS), X-Ray powder diffraction, IR, Raman, SEM, DSC, SQUID magnetometry and ⁵⁷Fe Mössbauer spectroscopy. The thermogravimetric and elemental analyses reveal the presence of guest water molecules, affording the following general formula [Fe(βAlatrz)₃](CF₃SO₃)₂·0.5H₂O (1·0.5H₂O). Compound 1·0.5H₂O was dehydrated by annealing, leading to a new compound, [Fe(βAlatrz)₃](CF₃SO₃)₂ (1), which was also characterized to reveal the influence of solvent molecules on the spin state. 1·0.5H₂O presents a rather crystalline character as revealed from X-ray powder diffraction (XRPD) patterns (Figure 1).

This result is also illustrated by the SEM analysis with blocks of hexagonal shape of about 2 μm widths (Figure 2). FT-IR and Raman analyses were performed: (i) to confirm the identity of the ligand framework before and upon complexation as the ester functionality is susceptible to hydrolysis; (ii) to ascertain the coordination mode of iron to the ligand and the presence of the trifluoromethane sulfonate in the crystal lattice (Figure 3).

Two sharp IR bands at 3,118(s) and 2,983(m) cm⁻¹ of βAlatrz, are assigned to the νCH₂ modes [18]. The carboxylic group of ester shows two stretching vibrations corresponding to (C=O) and (C–O) at 1,728(s) and 1,205(s) cm⁻¹, respectively, which are almost unchanged (1,732 and 1,212 cm⁻¹) in 1·0.5H₂O ruling out the possible ester hydrolysis and also confirming the non-involvement of carboxylic ester group in coordination. For βAlatrz, the band assigned to ring torsion of triazole at ν = 634(m) cm⁻¹, the ν_C=N stretching vibration at 1,535(m) cm⁻¹ and the N–N stretching band at ν = 1,022(s) cm⁻¹, are all shifted upon complexation in 1·0.5H₂O to 632 cm⁻¹, ν_C=N = 1,560 cm⁻¹, and ν_N-N = 1,028 cm⁻¹, respectively.

These values confirm the coordination of the iron to the 1,2,4-triazole ring [19,20]. Indeed, the characteristic bands of the ligand are not only present in the spectra of the complexes but are also shifted towards larger wave numbers, from 3 to 15 cm⁻¹, respectively. This energy increase is due to the deformation of the ligand upon coordination of the metal, the ligand molecule being indeed more constrained to perform vibration and twisting movements [19,21].

For a better understanding of the molecular structure of these ligands, Raman spectra were also collected (Figure 3). The band present at 1,728 cm⁻¹ for βAlatrz is assigned to a C=O vibration. In complexes this band is retained and appears around 1,732 cm⁻¹. The C–C stretching is also active in Raman as a medium band at 1,098 cm⁻¹ for βAlatrz and appears in the same wavenumber in 1·0.5H₂O. Presence of the monovalent counter-anion is also confirmed by IR and Raman: IR (cm⁻¹) υ(S–O)∼1,283(s), (1·0.5H₂O); Raman (cm⁻¹) υ_(S–O)∼1,034(s), 760(m) (1·0.5H₂O) [22]. ⁵⁷Fe Mössbauer spectroscopy confirm for 1·0.5H₂O the presence of one Fe^IIN₆ site, and exclude any oxidation product of iron. These spectroscopic data support a linear chain structure with Fe^II ions linked by triple N1,N2-1,2,4-triazole bridges [23,24].

1·0.5H₂O was prepared as a white powders and presents a reversible thermochromism on cooling to pink (Figure 4). These colors depend on the spin state of the Fe^II centers, as the ST involves a change in the electronic configuration which modifies the absorption spectrum of the complex.

The white color of 1·0.5H₂O, is due to the location of the spin-allowed lowest energy d-d transition, ⁵T_2g → ⁵E_g, for the HS sites in the near infrared region (∼11,500 cm⁻¹) [25,26]. Two supplementary bands, corresponding to the ¹A_1g → ¹T_1g and ¹A_1g → ¹T_2g d-d transitions of LS Fe^II sites are observed at ∼18,727 cm⁻¹ and ∼30,300 cm⁻¹, respectively suggesting that some proportion of Fe^II may be in the LS state at room temperature. The ligand field strengths for the HS and the LS state, given by equations 10D_q^HS = E(⁵E) − E(⁵T₂) and 10D_q^LS = E(¹T) − E(¹A₁) + (E(¹T₂) − E(¹T₁))/4, [25,26] allowed us to estimate 10D_q^HS and 10D_q^LS to be approximately 11,500 cm⁻¹ and 26,302 cm⁻¹, respectively. These values are characteristic for SCO complexes [25,26]. Presence of LS state at room temperature has been confirmed by ⁵⁷Fe Mössbauer spectroscopy (vide infra).

The reversibility of the rehydration/dehydration process within a given framework structure with the change of crystallinity can play an important role on the SCO properties [27]. This process was investigated for 1·0.5H₂O by thermogravimetric analysis, and the XRD powder pattern and SEM imaging recorded after annealing treatment. The sample was first deposited in a crucible and slowly heated at 1 K/min in air atmosphere (air flow 130 mL/min) to the temperature of complete dehydration (390 K) leading to 1. After a short standby period, the sample was cooled (1 K/min) slowly to reach room temperature revealing no rehydration. Thus the dehydration-rehydration process is irreversible and 1 is air stable which will ease any further physical studies on this compound. Comparison of the powder XRD patterns (Figure 1) and SEM images (Figure 2) of 1·0.5H₂O and 1 allow to exclude any framework rupture. Indeed, these two compounds are isostructural, 1 showing higher peak intensities indicating a better crystalline character. No deterioration is observed by SEM.

The temperature dependent magnetic properties of 1·0.5H₂O and 1 were determined by temperature-dependent susceptibility measurements using a SQUID magnetometer operating at 1000 Oe (Figure 5).

For complex 1·0.5H₂O, χ_MT is 3.10 cm³ K mol⁻¹ at 300 K, which is in the region expected for an Fe^II complex essentially in the HS state, with a small % of LS species. Upon cooling, χ_MT remains almost constant until 240 K where it drops sharply to T_c^↓ = 228 K down to ∼0.14 cm³ K mol⁻¹ at 77 K, which is typical for a diamagnetic Fe^II complex with possibly a few HS ions.

Upon warming, the χ_MT curve differs slightly revealing a small hysteresis width (4 K) at T_c^↑ = 232 K for this very sharp spin transition. An hysteretic behavior of width 4 K was observed too for 1 with a ST shifted upwards (T_c^↓ = 248 K and T_c^↑ = 252 K). The same curve shape is observed too which confirms the preservation of the 1D chain character [27] and does not support the appearance of a structural phase transition following the annealing process. The stabilization of the LS state upon water release is uncommon for this family of complexes [28] and was only observed for the 1D chain compounds [Fe(4-(2′-hydroxyethyl)-1,2,4-triazole)₃](anion)₂·nH₂O (anion = ClO₄⁻, n = 2, 0; anion = I⁻, n = 1, 0) [29], [Fe(4-amino-1,2,4-triazole)₃](anion)·nH₂O (anion = TiF₆²⁻, n = 1, 0.5; anion = ZrF₆²⁻, n = 0.5, 0) [23] as well as for [Fe(ethyl-4H-1,2,4-triazol-4-yl-acetate)₃](ClO₄)₂·nCH₃OH (n = 1,0) but with methanol as solvent [13]. The effect of the release of non-coordinated solvent molecules on the spin state can be translated here as an internal positive pressure effect [5,23].

An inspection of electronic and structural features for 1·0.5H₂O and 1 using ⁵⁷Fe Mössbauer spectroscopy was undertaken over the temperature range 77–300 K (Figure 6). At 77 K, the spectrum of 1·0.5H₂O consists of two quadrupole doublets of different resonance area fractions. The major quadrupole doublet with isomer shift δ^LS = 0.51(2) mm/s and quadrupole splitting, ΔE_Q^LS = 0.23(2) mm/s correspond to the LS state of Fe^II. The presence of an LS quadrupole splitting stems from a lattice contribution to the electric field gradient and therefore reveals a distorted character for the LS octahedron as expected within a chain, where constraints may not be negligible [30]. Another doublet, corresponding to HS Fe^II ions of weaker population (7%), with parameters (δ^HS = 1.14(1) mm/s and ΔE_Q^HS = 3.15(2) mm/s) confirms the incomplete nature of the ST at 77 K. Upon warming to 300 K, the intensity of the HS doublet slowly increases to 8% at 225 K, after which it increases dramatically to 87.5% at 300 K, confirming an incomplete thermally induced LS → HS conversion for a single Fe^II site. The presence of LS ions at room temperature could be related to crystal defects or end of chains. The hysteresis effect is clearly evidenced at 225 K (Figure 6a).

At 80 K, the spectrum of 1 shows a single LS quadrupole doublet (δ^LS = 0.52(1) mm/s and ΔE_Q^LS = 0.25(2) mm/s) indicating a complete spin transition. The compound remains mostly in the LS state on warming up to 250 K, after which a second quadrupole doublet attributed to HS Fe^II ions grows in intensity (e.g., at 297 K, δ^HS = 1.03(1) mm/s and ΔE_Q^HS = 2.75(1) mm/s). The asymmetry of the lines observed in the HS state is attributed to a texture effect. Upon cooling to low temperature, the reverse situation is observed with a clear hysteresis effect at 250 K (Figure 6b).

The isomer shift (δ^LS∼0.51(1) mm/s at 77–80 K and ΔE_Q^HS = 1.03(1) mm/s at 297–300 K) is not affected by the dehydration process which indicates that non coordinated water molecules are not H-bonded to the triazole ligand [31], but should be located at a remote position to the complex in the crystal lattice, either isolated or hydrogen bonded to the sulfonate group of the non coordinated anions. Their releases have no influence on the structural organization as demonstrated by the similarity in X-ray powder diffraction data. However, a clear influence on the transition temperatures, i.e., on the respective energy levels of the HS and LS states [25], has been detected.

Compound 1·0.5H₂O and 1 were investigated by differential scanning calorimetry over the temperature range 100–300 K, at 10 K/min for both cooling and heating modes (Figure 7).

An endothermic peak is observed on warming for 1·0.5H₂O at T_max^↑ = 235(1) K and an exothermic peak is recorded at T_max^↓ = 233(1) K, on cooling. These peaks correspond to a first-order phase transition in agreement with the transition temperatures determined by both SQUID and Mössbauer spectroscopy. The enthalpy and entropy variations associated to the active SCO centers are ΔH = 12(2) kJ/mol and ΔS = 51(2) J/mol/K. A similar profile, although with more abrupt peaks, was detected for 1 with phase transitions shifted upwards to T_max^↑ = 254(1) K and T_max^↓ = 247(1) K. The peaks are separated by a narrow temperature domain, which is indicative of the presence of a hysteresis loop. The enthalpy and entropy associated to the ST, considering only the switching sites, were derived as follows: ΔH = 13(1) kJ/mol and ΔS = 59(2) J/mol/K.

All reagents and solvents were used as received from commercial source: benzene (Fluka analytical), Methanol (VWR), SOCl₂ (Sigma-Aldrich), glycine ethyl ester hydrochloride (ACROS), CF₃SO₃H (ACROS), Fe powder (Merck). Ethyl 4H-1,2,4-triazol-4-yl-propionate (βAlatrz) were prepared by a similar method described in reference [12].

Elemental analyses were performed at University College London (UK) and at S.C.A. CNRS Solaize (France). ¹H and ¹³C NMR spectra were recorded at 300 MHz and 75 MHz, respectively, on a Bruker AC300 instrument. The residual solvent peak was used as internal reference. Mass spectral data were obtained on Thermo Finnigan LCQ Ion trap spectrometer (APCI mode). HRMS were carried out on a Micromass Q TOF 2 spectrometer in ESI mode, detecting positive mode. Raman spectra with 1,064 nm excitation were recorded between 2,300 to 400 cm⁻¹ with a Bruker RFS 100/s FT-Raman spectrometer (I = 200 mW) at r.t using a diode-pumped, air-cooled Nd:YAG laser as the excitation source. IR spectra were collected on a Shimadzu FTIR-84005 spectrometer using KBr pellets. Thermogravimetric analyses (TGA) were performed in air (100 mL/min) at the heating rate of 1 °C/min from 293 K to 400 K using a Mettler Toledo TGA/SDTA 851e analyzer. Diffuse reflectance spectra on solids were recorded with a CARY 5E spectrophotometer using polytetrafluoroethylene as a reference. Powder X-ray diffraction patterns were recorded on a Siemens D5000 counter diffractometer working with Cu-Kα radiation and operating at room temperature. The samples were mounted on the support with silicon grease. ⁵⁷Fe Mössbauer spectra were recorded in transmission geometry over the temperature range (78–300 K) with a conventional Mössbauer spectrometer equipped with a Cyclotron Ltd ⁵⁷Co(Rh) radioactive source operating at room temperature. The samples were sealed in aluminum foil and mounted on an Oxford nitrogen bath cryostat. The spectra were fitted to the sum of Lorentzians by a least-squares refinement using Recoil 1.05 Mössbauer Analysis Software [32]. All isomer shifts refer to α-Fe at room temperature. Magnetic susceptibilities were measured in the temperature range 4–390 K using a MPMS-XL (7T) SQUID magnetometer. Data were corrected for magnetization of the sample holder and diamagnetic contributions, which were estimated from the Pascal constants. Differential scanning calorimetry measurements were carried out in a He_(g) atmosphere using a Perkin-Elmer DSC Pyris 1 instrument equipped with a cryostat and operating down to 98 K. Aluminum capsules were loaded with 20–50 mg of sample and sealed. The heating and cooling rates were fixed at 10 K min⁻¹. Temperatures and enthalpies were calibrated over the temperature range of interest (298–400 K) using the solid-liquid transitions of pure In (99.99%) [33], and the crystal-crystal transitions of pure cyclopentane (≥99%) [34], over the range 78–298 K. Scanning electron microscopy (SEM) was performed using a Gemini Digital Scanning Microscope 982 with 1 kV accelerating voltage with an aluminum sample holder.