{'fraction_non_alphanumeric': 0.04610854580740146, 'fraction_numerical': 0.028642173592986684, 'mean_word_length': 4.9917802726543705, 'pattern_counts': {'":': 0, '<': 0, '<?xml version=': 0, '>': 0, 'https://': 0, 'lorem ipsum': 0, 'www.': 0, 'xml': 0}, 'pii_count': 0, 'substrings_counts': 0, 'word_list_counts': {'cursed_substrings.json': 1, 'profanity_word_list.json': 0, 'sexual_word_list.json': 0, 'zh_pornsignals.json': 0}}
Molecular Mobility and Stability Studies of Amorphous Imatinib Mesylate

The proposed study examined the characterization and stability of solid-state amorphous imatinib mesylate (IM) after 15 months under controlled relative humidity (60 ± 5%) and temperature (25 ± 2 °C) conditions. After 2 weeks, and 1, 3, 6, and 15 months, the samples were characterized using differential scanning calorimetry (DSC), thermogravimetric analysis (TGA), X-ray powder diffractometry (XRPD), attenuated total reflectance-Fourier transform infrared spectroscopy (ATR-FTIR) and scanning electron microscopy (SEM). Additionally, the amorphous form of imatinib mesylate was obtained via supercooling of the melt in a DSC apparatus, and aged at various temperatures (3, 15, 25 and 30 °C) and time periods (1–16 h). Glass transition and enthalpy relaxation were used to calculate molecular-relaxation-time parameters. The Kohlrausch–Williams–Watts (KWW) equation was applied to fit the experimental enthalpy-relaxation data. The mean molecular-relaxation-time constant (τ) increased with decreasing ageing temperature. The results showed a high stability of amorphous imatinib mesylate adequate to enable its use in solid dosage form.


Introduction
Amorphous substances form a separate class of solids, which are distinct from the more common and well-known crystalline solid. Crystalline materials consist of a three-dimensional long-range structure, which is not present in the amorphous state. Furthermore, compared to crystalline state, the positioning of amorphous state molecules are more irregular, as well as possessing high internal energy and specific volume, which improves dissolution and bioavailability [1][2][3]. The most common methods of amorphization include rapid precipitation from solution, quench-cooling, spray-drying, freeze-drying, and hot melt extrusion [4][5][6][7][8]. Mechanical stress associated with grinding and milling can also transform crystalline solids into amorphous form [9]. Amorphous substances are generally hygroscopic, with high solubility and bioavailability, and can possess superior compression characteristics than corresponding crystals [10,11]. The role of molecular mobility in time-dependent nucleation, chemical degradation, crystallization, and structural collapse of amorphous materials has been recognized in several studies [12][13][14]. In terms of stability, the amorphous state can unexpectedly transform into the crystalline state during production or storage [15,16]. Information regarding physicochemical stability of the amorphous state of drugs is invaluable in accurately determining pharmaceutical dosage [17,18]. To classify amorphous substances as stable, they must exhibit relaxation times comparable to their shelf life (3 years for pharmaceuticals) [19]. Therefore, Pharmaceutics 2019, 11 the objective of this study is to characterize the behavior and performance of imatinib mesylate (IM) in its amorphous state in order to predict its stability as a pharmaceutical raw material. IM (Figure 1), i.e., 4-(4-methyl-piperazin-1-ylmethyl)-N-u[4-methyl-3-(4-pyridin-3-yl)pyrimidine-2ylamino)phenyl]benzamide methanesulfonate, is a tyrosine-kinase inhibitor commonly used in the treatment of chronic myeloid leukemia [20][21][22] and gastrointestinal stromal tumors [23][24][25]. It can be useful in the treatment of atherosclerosis [26,27], thrombosis [28,29], and restenosis [30,31]. Imatinib therapy is a good option for unresectable, recurrent, or metastatic dermatofibrosarcoma protuberans [32][33][34][35][36][37]. IM is known to exist in various polymorphic forms, including hydrated and solvated forms, as well as hydrated and anhydrous amorphous forms [38][39][40][41][42][43][44]. The most extensively examined IM polymorphs are αand β-form. Grillo et al. showed that these forms transform into amorphous IM upon grinding, followed by conversion to the crystalline phase during aging or thermal treatment. Furthermore, recent studies have found that α and β-forms are enantiotropically related. Detailed reports have confirmed these solid forms based on crystallographic and spectroscopic techniques [45,46]. To the best of our knowledge, information related to the stability and characterization of IM amorphous form in the literature is non-excitant. However, there is a strong relationship between molecular mobility and stability of amorphous form in pharmaceutical substances. To predict the life expectancy of pure amorphous compounds in the study, we searched for correlations between crystallization tendency of glass formers with molecular mobility and thermodynamic properties of the amorphous state. It was recognized that storage well below T g prevents crystallization and ensures a physically stable drug during its shelf-life [13,47,48]. In this paper, the physical stability of IM was investigated using thermal methods by considering the onset temperature and enthalpy relaxation at the glass transition of the ageing time. The stability of IM in the amorphous state was estimated by the mean molecular relaxation-time constant "τ" and relaxation-time distribution parameter β using the Kohlrausch-Williams-Watts (KWW) equation. Moreover, the physicochemical characteristics of IM at time ageing were determined by thermal techniques X-ray powder diffractometry (XRPD), attenuated total reflectance-Fourier transform infrared spectroscopy (ATR-FTIR) and scanning electron microscopy (SEM). This is the first time such a study of amorphous IM was presented.
Pharmaceutics 2019, 11, x 2 of 14 state of drugs is invaluable in accurately determining pharmaceutical dosage [17,18]. To classify amorphous substances as stable, they must exhibit relaxation times comparable to their shelf life (3 years for pharmaceuticals) [19]. Therefore, the objective of this study is to characterize the behavior and performance of imatinib mesylate (IM) in its amorphous state in order to predict its stability as a pharmaceutical raw material. IM (Figure 1), i.e., 4-(4-methyl-piperazin-1-ylmethyl)-N-u[4-methyl-3-(4-pyridin-3-yl)pyrimidine-2-ylamino)phenyl]benzamide methanesulfonate, is a tyrosine-kinase inhibitor commonly used in the treatment of chronic myeloid leukemia [20][21][22] and gastrointestinal stromal tumors [23][24][25]. It can be useful in the treatment of atherosclerosis [26,27], thrombosis [28,29], and restenosis [30,31]. Imatinib therapy is a good option for unresectable, recurrent, or metastatic dermatofibrosarcoma protuberans [32][33][34][35][36][37]. IM is known to exist in various polymorphic forms, including hydrated and solvated forms, as well as hydrated and anhydrous amorphous forms [38][39][40][41][42][43][44]. The most extensively examined IM polymorphs are α-and β-form. Grillo et al. showed that these forms transform into amorphous IM upon grinding, followed by conversion to the crystalline phase during aging or thermal treatment. Furthermore, recent studies have found that α and β-forms are enantiotropically related. Detailed reports have confirmed these solid forms based on crystallographic and spectroscopic techniques [45,46]. To the best of our knowledge, information related to the stability and characterization of IM amorphous form in the literature is non-excitant. However, there is a strong relationship between molecular mobility and stability of amorphous form in pharmaceutical substances. To predict the life expectancy of pure amorphous compounds in the study, we searched for correlations between crystallization tendency of glass formers with molecular mobility and thermodynamic properties of the amorphous state. It was recognized that storage well below Tg prevents crystallization and ensures a physically stable drug during its shelf-life [13,47,48]. In this paper, the physical stability of IM was investigated using thermal methods by considering the onset temperature and enthalpy relaxation at the glass transition of the ageing time. The stability of IM in the amorphous state was estimated by the mean molecular relaxation-time constant "τ" and relaxation-time distribution parameter β using the Kohlrausch-Williams-Watts (KWW) equation. Moreover, the physicochemical characteristics of IM at time ageing were determined by thermal techniques X-ray powder diffractometry (XRPD), attenuated total reflectance-Fourier transform infrared spectroscopy (ATR-FTIR) and scanning electron microscopy (SEM). This is the first time such a study of amorphous IM was presented.

Materials
Crystalline imatinib mesylate  form used in this study was synthetized in a new continuousflow microwave reactor, described in [49] and donated by Silesian Catalysts Sp. z o.o (Wrocław, Poland). Residual solvents (below 0.5%) were determined using gas chromatography-mass spectrometry (GC-MS) method. Reference material: commercial IM of a grade useful for R&D was purchased from LC Laboratories (Woburn, MA, USA). According to the certificate attached by the manufacturer, the declared purity of the substance was 94.66% (by nuclear magnetic resonance

Materials
Crystalline imatinib mesylate α form used in this study was synthetized in a new continuous-flow microwave reactor, described in [49] and donated by Silesian Catalysts Sp. z o.o (Wrocław, Poland). Residual solvents (below 0.5%) were determined using gas chromatography-mass spectrometry (GC-MS) method. Reference material: commercial IM of a grade useful for R&D was purchased from LC Laboratories (Woburn, MA, USA). According to the certificate attached by the manufacturer, the declared purity of the substance was 94.66% (by nuclear magnetic resonance (NMR) method). The verification of purity by the method of differential scanning calorimetry (DSC) in our study confirmed 93.99% ± 0.08 purity. Our previous studies confirmed that both commercial and synthetized IM occur in crystalline α form [50].

Preparation of Amorphous Sample
Preparation of the amorphous form of a drug for physical stability studies was achieved by melting the drug in a stainless-steel beaker on a hot plate, followed by subsequent quenching by cooling the melt over crushed ice (method A). The quench-cooled product was ground, sieved using 315 µm sieve, and examined after 2 weeks, 1 month, 3 months, 6 months, and 15 months, respectively.
Additionally, the amorphous form of IM was obtained by supercooling the melt in a DSC apparatus (method B), and aged at various temperatures (3,15,25, and 30 • C) for periods of time between 1 and 16 h.

Physical Stability Studies
The physical stability of amorphous IM was monitored for fifteen months under controlled relative humidity (60 ± 5%) and temperature (25 ± 2 • C), which was the long-term stability condition, selected based on Guideline for Industry Q1A (R2) Stability Testing of new Drug Substances and Products [51]. Periodically (0 day, 2 weeks, 1 month, 3 months, 6 months, and 15 months), the samples were removed and examined for solid-state transitions using DSC, TGA, XRD, ATR-FTIR, and SEM methods.

Differential Scanning Calorimetry (DSC)
Differential scanning calorimeter DSC 214 Polyma instrument (Netzsch, Selb, Germany) equipped with an Intracooler IC70 (Netzsch, Selb, Germany) was used. Measurements of the amorphous samples were performed using the heat-flow measurement method at a heating rate of 10 • C per minute over a temperature range of 10-250 • C in a nitrogen dynamic atmosphere (25 mL/min). The samples of approx. 8.5 mg were placed in an aluminium pan (25 µL) with a pierced lid, and subsequently sealed. An empty pan of the same type was employed as reference. DSC peak area and transition temperatures were determined using Netzsch Proteus ® 7.1.0 analysis software (Netzsch, Selb, Germany). The apparatus was calibrated using standard samples from calibration set 6.239.2-91.3 supplied by Netzsch (Selb, Germany). All samples were weighed on a Sartorius CPA225D-0CE analytical balance (Sartorius AG, Gottingen, Germany) with a resolution of 0.01 mg.
In this study, the ageing experiments of IM crystals were also performed. The schematic representation of the entire temperature program is illustrated in Figure 2. The samples were melted in an aluminium pan at 175 • C and maintained for 5 min to avoid incomplete melting. The melt was quench-cooled at approx. 200 • C per minute cooling rate to different ageing temperatures (T a ) (3, 15, 25, and 30 • C) for a predetermined period of ageing time (t a ) (1, 2, 4, 8, and 16 h). Following the specified aging time, the glassy materials were heated at 10 • C per minute to 185 • C. A cycle for unaged sample was processed. This second heating determined the change heat capacity (∆C p ), the extrapolated onset glass transition temperature (T g ) and the enthalpy recovery (∆H t ).

Thermogravimetric Analysis (TGA)
The thermal stability of the samples was investigated by thermogravimetric analysis using TG 209 F1 Libra (Netzsch, Selb, Germany) thermobalance. The experiments were carried out in alumina crucibles (150 µL), under nitrogen atmosphere (25 mL/min) at a heating rate of 10 • C per minute. TGA/DTG curves were obtained in the temperature range of 25-600 • C. Netzsch Proteus ® 7.1.0 analysis software (Selb, Germany) was used to determine the mass change of the samples and DTG curves.

Thermogravimetric Analysis (TGA)
The thermal stability of the samples was investigated by thermogravimetric analysis using TG 209 F1 Libra (Netzsch, Selb, Germany) thermobalance. The experiments were carried out in alumina crucibles (150 μL), under nitrogen atmosphere (25 mL/min) at a heating rate of 10 °C per minute. TGA/DTG curves were obtained in the temperature range of 25-600 °C. Netzsch Proteus ® 7.1.0 analysis software (Selb, Germany) was used to determine the mass change of the samples and DTG curves.

Attenuated Total Reflectance-Fourier Transform Infrared Spectroscopy (ATR-FTIR)
A Nicolet 380 FTIR (Thermo Scientific, Waltham, MA, USA) analyzer equipped with OMNIC analysis software was used for FTIR spectra registration. Spectra were collected in attenuated total reflectance (ATR) mode. A small amount of each sample was placed on the diamond crystal and scanned over a wavelength of 400 cm −1 to 4000 cm −1 with a resolution of 4 cm −1 .

Scanning Electron Microscopy (SEM)
Scanning electron microscope (SEM) images were taken on Zeiss EVO MA25 (Carl Zeiss NTS GmbH, Oberkochen, Germany) apparatus at an accelerating voltage of 20 kV. The samples were covered with gold and palladium (60:40; sputter current, 40 mA; sputter time, 50 s) using a Quorum machine (Quorum International, Fort Worth, TX, USA).

Results and Discussion
DSC curves of amorphous IM samples stored at 25 °C under controlled relative humidity at different ageing times are presented in Figure 3. After 1 month (Figure 3c-f), it can be observed that the moisture is adsorbed by samples, which also corroborated with the results obtained from TGA. Water evaporation occurred between 40-130 °C, followed by recrystallization and melting of the sample. The glass transition temperature of amorphous IM with increasing ageing time at an ageing

Attenuated Total Reflectance-Fourier Transform Infrared Spectroscopy (ATR-FTIR)
A Nicolet 380 FTIR (Thermo Scientific, Waltham, MA, USA) analyzer equipped with OMNIC analysis software was used for FTIR spectra registration. Spectra were collected in attenuated total reflectance (ATR) mode. A small amount of each sample was placed on the diamond crystal and scanned over a wavelength of 400 cm −1 to 4000 cm −1 with a resolution of 4 cm −1 .

Scanning Electron Microscopy (SEM)
Scanning electron microscope (SEM) images were taken on Zeiss EVO MA25 (Carl Zeiss NTS GmbH, Oberkochen, Germany) apparatus at an accelerating voltage of 20 kV. The samples were covered with gold and palladium (60:40; sputter current, 40 mA; sputter time, 50 s) using a Quorum machine (Quorum International, Fort Worth, TX, USA).

Results and Discussion
DSC curves of amorphous IM samples stored at 25 • C under controlled relative humidity at different ageing times are presented in Figure 3. After 1 month (Figure 3c-f), it can be observed that the moisture is adsorbed by samples, which also corroborated with the results obtained from TGA. Water evaporation occurred between 40-130 • C, followed by recrystallization and melting of the sample. The glass transition temperature of amorphous IM with increasing ageing time at an ageing temperature of 25 • C was determined at approx. 100 • C. No significant changes were observed at the ageing temperature. In the case of samples stored longer than 6 and 15 months (Figure 3e,f), the glass transition was difficult to detect due to moisture absorption. Compared to DSC curves of IM amorphous form, only one thermal (endothermic) effect corresponding to the melting was visible for crystalline form (Figure 3g). DSC parameters of amorphous imatinib mesylate are presented in Table 1.
Based on DSC curves recorded at various temperatures (3, 15, 25, and 30 • C), enthalpy recovery (∆H t ) data for amorphous IM were obtained. Using the KWW equation, the average relaxation time constant τ and dimensionless relaxation time distribution parameter β were estimated (Table 2).  Figure 4 shows the best fits of the KWW equation to the experimental data (solid lines). The initial parameters were τ = 100 s and β = 0.5. The KWW equation is as follows: where ∅ t is the extent of impending relaxation at the annealing temperature, ∆H ∞ is the maximum enthalpy recovery, t is the ageing time, τ is the mean relaxation-time constant, and β is the non-exponential parameter, respectively. the ageing temperature. In the case of samples stored longer than 6 and 15 months (Figure 3e and 3f), the glass transition was difficult to detect due to moisture absorption. Compared to DSC curves of IM amorphous form, only one thermal (endothermic) effect corresponding to the melting was visible for crystalline form (Figure 3g). DSC parameters of amorphous imatinib mesylate are presented in Table 1. Tp -peak melting temperature; TOnset -onset melting temperature; TEndset -endset melting temperature; ΔHfenthalpy of fusion; Tgglass transition; ΔCp -heat capacity.  (Table 2). Figure 4 shows the best fits of the KWW equation to the experimental data (solid lines). The initial parameters were τ = 100 s and β = 0.5. The KWW equation is as follows: ∆H ∞ was calculated from the following equation: where ∆C p is the heat capacity change at T g and T a ageing temperature. Values of τ and β estimators presented in Table 3 were determined using two non-linear optimization algorithms: Levenberg-Marquardt and Quasi-Newton, which minimize the loss function L according to the equation: where RSS is the residual sum of squares, y i is the experimental values, and f (x i ) the values predicted by the estimated model. The statistical significance of τ and β estimators was evaluated using the t-test, assuming the confidence level p = 0.05, and 95% confidence interval (−95% CI/+95% CI). The quality of matching the KWW functions to the experimental data was determined by coefficients of determination R 2 (R-squared). The correctness of the entire model was additionally checked by residual analysis (Table 3). For each measurement point, the value predicted by the model f x i ,τ,β was determined as L(τ, β) = y i − f x i ,τ,β 2 . The values of residues were determined according to the formula L i = y i − f x i ,τ,β . A standard error, and 95% confidence interval for f x i ,τ,β and values of the entire model were also determined. The normality of the distribution of calculated L i residues was assessed using the Shapiro-Wilk W-test with the assumed confidence level p = 0.05. The distribution of standardized values L i is shown in Figure 4. The times t 50% listed in Table 3 are defined as the times required for half completion (50%) of the possible maximum enthalpy relaxation at a single relaxation temperature, which corresponds to the value of relaxation time τ in the KWW equation when ∅ t = 0.50. By comparing τΦ(t) = 50% values of each glass at each aging temperature, it was found that as aging temperature decreased, τΦ(t) = 50% values increased dramatically, hence, the rate of the aging process dramatically decreased at lower aging temperatures. A rapid decrease in t 50% values was observed with increasing aging temperatures from 4.91695 × 10 33 h at 3 • C to 8.21992 × 10 16 h at 30 • C, which again slowed the aging process at lower temperatures. Calculated mean molecular relaxation time constants for amorphous IM range from 3.609324 × 10 39 to 6.393168 × 10 21 s, which are comparable with values obtained for griseofulvin, tolbutamide, troglitazone, and simvastatin [52]. The width of relaxation-time distribution parameter β ranging from 0 to 1 were characterized. The smaller the β value, a greater distribution of molecular motion deviates from a single exponential behavior was obtained. Estimated values of β parameters were comparable at different ageing temperatures but vary significantly from the unit. Therefore, this indicates a distribution of time scale rather than one single relaxation time. Furthermore, with an increase in ageing temperature the mean relaxation-time constants τ decreased.
The statistical analysis presented in Table 3 was constructed using the following programs: Mathematica ver. 10.0 by Wolfram Research and Statistica ® ver. 13.1 from Dell. exponential behavior was obtained. Estimated values of β parameters were comparable at different ageing temperatures but vary significantly from the unit. Therefore, this indicates a distribution of time scale rather than one single relaxation time. Furthermore, with an increase in ageing temperature the mean relaxation-time constants τ decreased.
The statistical analysis presented in Table 3 was constructed using the following programs: Mathematica ver. 10.0 by Wolfram Research and Statistica ® ver. 13.1 from Dell.   Thermogravimetry and derivative thermogravimetry (DTG) was used to identify the thermal stability of amorphous IM. TGA and DTG curve of the substance at 0 time and after a specified time are presented in Figure 5. The thermal decomposition parameters are as follows: temperature of maximum weight loss rate (T m ); extrapolated onset temperature of decomposition (T Onset ); rate of mass loss, which corresponds to T m ; extrapolated temperature at which the degradation process ends  Table 4.
From the above results it can be extrapolated that the thermal degradation of the analyzed samples occurs in one step. The average temperature of maximum weight loss rate for the main effect was 371.57 • C, which corresponds to 5.42% min −1 , the rate of mass loss. As shown in Figure 6c-f, additional mass changes in the temperature range 25-140 • C was observed, possibly due to a loss of loosely bound water. The presence of water is evident from the DCS curves (Figure 3c-f). Moisture content fluctuates depending on ageing times from 1.16 % (1 month aging) to 3.95 % (15 months aging). A fall in the baseline above 270 • C was due to substance degradation. The average temperature at which 0.5 wt.% loss occurs was observed at approximately 274 • C, while the average extrapolated onset temperature of decomposition was 325 • C. The differentiation at c.a. 50 • C between T Onset and T 0.5 wt.% should be taken into consideration during thermal stability assessment.
According to TGA/DTG curve registered for the crystalline form of the substance, decomposition occurs in one step. The thermal decomposition parameters: T m = 376.0 • C, rate mass loss = 5.61 %·min −1 , T Onset = 325.6 • C, T Endset = 424.1 • C, T 0.5 wt.% = 278.6 • C, T 1.0 wt.% = 291.7 • C, and Res = 40.29% were determined. In the temperatures ranging between 25-140 • C no mass loss was observed related to moisture.  TEndset-extrapolated temperature at which the degradation process ends; T0.5 wt.%-temperature at which 0.5 wt.% loss occurs; T1.0 wt.%-temperature at which 1.0 wt.% loss occurs; Res-amount of residue at 600 °C XRPD pattern of crystalline IM confirms its crystalline nature (Figure 6a) [50]. The amorphous sample of the drug stored at 25 °C under controlled relative humidity at different ageing times is shown in Figure 6b-g. All diffractograms display a broad amorphous halo with the absence of sharp diffraction peaks signals characteristic for crystalline form. XRPD pattern of crystalline IM confirms its crystalline nature (Figure 6a) [50]. The amorphous sample of the drug stored at 25 • C under controlled relative humidity at different ageing times is shown in Figure 6b-g. All diffractograms display a broad amorphous halo with the absence of sharp diffraction peaks signals characteristic for crystalline form.  ATR-FTIR spectra of IM samples in the 4000-400 cm −1 region are presented in Figure 7. The obtained results correspond well with literature data [53]. ATR-FTIR showed characteristic bands at 3256 cm −1 (N-H stretching vibration), 1657 cm −1 (C=O band), 1570, 1525, and 1444 cm −1 (aromatic C=C, C=N stretching vibration), 1158 cm −1 (C-N stretching vibration), 1036 cm −1 (C-O stretching vibration), and 807 cm −1 (aromatic C-H deformations out of plane). ATR-FTIR spectra for crystalline and amorphous IM samples were qualitatively similar. The spectra of amorphous forms showed peak broadening attributed to the relative disorder of the molecules in the amorphous form, resulting in a broader distribution of bond lengths and energies with respect their crystalline counterparts. ATR-FTIR spectra of IM samples in the 4000-400 cm −1 region are presented in Figure 7. The obtained results correspond well with literature data [53]. ATR-FTIR showed characteristic bands at 3256 cm −1 (N-H stretching vibration), 1657 cm −1 (C=O band), 1570, 1525, and 1444 cm −1 (aromatic C=C, C=N stretching vibration), 1158 cm −1 (C-N stretching vibration), 1036 cm −1 (C-O stretching vibration), and 807 cm −1 (aromatic C-H deformations out of plane). ATR-FTIR spectra for crystalline and amorphous IM samples were qualitatively similar. The spectra of amorphous forms showed peak broadening attributed to the relative disorder of the molecules in the amorphous form, resulting in a broader distribution of bond lengths and energies with respect their crystalline counterparts.
In order to estimate the morphology of IM samples, scanning electron microscopy (SEM) analysis was performed. SEM images of crystalline and amorphous IM are shown in Figure 8. Synthetized IM exists as a needles-shape crystalline structure (Figure 8a). IM particles, observed on SEM images taken after 2 weeks (Figure 8b) and 1 month (Figure 8c) of storage, reveal an irregular spherical shape, characteristic for amorphous state. After 3, 6, and 15 months of storage (Figure 8d-f, respectively) the shape of IM particles become less compact, but remain irregular and do not resemble the needles.
ATR-FTIR spectra of IM samples in the 4000-400 cm −1 region are presented in Figure 7. The obtained results correspond well with literature data [53]. ATR-FTIR showed characteristic bands at 3256 cm −1 (N-H stretching vibration), 1657 cm −1 (C=O band), 1570, 1525, and 1444 cm −1 (aromatic C=C, C=N stretching vibration), 1158 cm −1 (C-N stretching vibration), 1036 cm −1 (C-O stretching vibration), and 807 cm −1 (aromatic C-H deformations out of plane). ATR-FTIR spectra for crystalline and amorphous IM samples were qualitatively similar. The spectra of amorphous forms showed peak broadening attributed to the relative disorder of the molecules in the amorphous form, resulting in a broader distribution of bond lengths and energies with respect their crystalline counterparts.  Synthetized IM exists as a needles-shape crystalline structure (Figure 8a). IM particles, observed on SEM images taken after 2 weeks ( Figure 8b) and 1 month (Figure 8c) of storage, reveal an irregular spherical shape, characteristic for amorphous state. After 3, 6, and 15 months of storage (Figure 8d, 8e, and 8f, respectively) the shape of IM particles become less compact, but remain irregular and do not resemble the needles.

Conclusions
A delicate balance exists among the chemical and physical properties of amorphous materials. Slight alterations or disturbances can have a major influence on stability, as well as future

Conclusions
A delicate balance exists among the chemical and physical properties of amorphous materials. Slight alterations or disturbances can have a major influence on stability, as well as future production and dissolution characteristics of the final product [54]. Unfortunately, the storage of such materials can promote unwanted transformation to their more stable crystalline form [55].
Herein, we showed efficient methodology for the preparation of amorphous IM via its crystalline form. The process eliminated unwanted chemical degradation and the presence of amorphous IM was confirmed using analytical techniques: DSC, ATR-FTIR, and XRPD. Glass transition and enthalpy relaxation were experimentally determined and used to calculate molecular relaxation-time parameters. The KWW equation fitted the experimental enthalpy relaxation data well. Two non-linear optimization algorithms: Levenberg-Marquardt and Quasi-Newton were applied to predict the long-term amorphous stability of IM. It was determined that the mean molecular relaxation time constant (τ) increased with decreasing ageing temperature.
By calculating the relaxation time of amorphous IM, it was possible to estimate the timescale of undesirable solid-state degradation or crystallization as a function of temperature. The calculated mean molecular-relaxation time constants for amorphous IM confirmed the long-term stability of the examined samples. This amorphous substance could be a potential candidate for the development of novel drug products.