New Data on Crystal Phases in the System MgSO 4 –OC(NH 2 ) 2 –H 2 O

: Urea complexes of magnesium sulfate have been intensively studied due to their application in many areas of life, including agricultural chemistry, pharmacy, medicine, etc. The aim of this study is to add new knowledge about the trends and consistencies in the preparation procedures of MgSO 4 · nOC(NH 2 ) 2 · mH 2 O phases. A set of analytical methods was used to characterize their structure, thermal and spectroscopic properties. The conditions for obtaining the three complexes in pure form were specified and the crystal structures of MgSO 4 · OC(NH 2 ) 2 · 2H 2 O and MgSO 4 · OC(NH 2 ) 2 · 3H 2 O were determined. The spectroscopic data of the considered compounds were analysed with respect to their structural and chemical properties. Thermal analyses showed that both the melting point and the urea decomposition temperature depend on the OC(NH 2 ) 2 : H 2 O ratio in the octahedral environment of the magnesium ion in the studied structures.


Introduction
Magnesium is one of the most abundant elements in nature.Magnesium makes up 2.4% of the Earth's crust as a component of a number of rock-forming minerals [1].The source of bioavailable magnesium is the hydrosphere, where the magnesium concentration is about 4.1 Clarke [2].Magnesium salts dissolve well in water and, as a result, a variety of magnesium sulfate hydrates and complexes, easily accessible to living organisms, are formed.Magnesium is one of the major biogenic elements and, as part of over 300 enzyme systems, magnesium ions are involved in a number of biochemical reactions [3][4][5].The essential role of magnesium determines the great research interest in its salts, hydrates and complexes.Magnesium compounds are widely used in almost all spheres of life, including agricultural chemistry, pharmacy, medicine, etc. [6][7][8][9].Particularly important and promising are studies on the interaction of magnesium salts with amide-type ligands, since a large proportion of the low molecular weight substances present in plants and animals are of the amide type.One of the common amide ligands in nature is urea (OC(NH 2 ) 2 ), which forms compounds with many of the magnesium salts.In such compounds, urea moieties displace water molecules from the magnesium coordination surrounding, thereby reducing the hygroscopicity of such salts as magnesium chlorides, iodides, bromides, nitrates, tetrafluoroborates, chlorates, formats, dihydrogen phosphates and perrhenates [10][11][12][13][14][15][16][17][18][19][20].Urea complexes of magnesium sulfate have been studied since the beginning of the last century.The phases reported so far are shown in Table 1.Some of the results in this field refers to studies of the MgSO 4 -OC(NH 2 ) 2 -H 2 O system and/or relationship between synthesis conditions and stoichiometry of the obtained MgSO 4 •nOC(NH 2 ) 2 •mH 2 O phases [21][22][23][24][25][26][27][28][29].Others relate to optimisation of the processes for preparation of products for the agrochemical industry, which include urea and magnesium sulfate composites [26][27][28][29][30][31][32][33].Among the results obtained, the following ones are relevant to the present study.Both starting reactants and final products of the studied system are very temperature sensitive and, even at the same ratio of starting reactants, a small difference in the temperature range leads to the formation of stoichiometrically different phases.For instance, when a solution of MgSO 4 and OC(NH 2 ) 2 in molar ratio 1: , whereas an evaporation at 30      [21,25].Diversity of magnesium sulfate sources and their pre-activation treatment are allowable, as presented in the patents WO 2013/098367, US 2014/0360239 A1, and US 2016/0046534 A1.The authors describe conditions for obtaining mixtures of some of the above mentioned compounds using MgSO 4 or MgSO 4 •7H 2 O as magnesium sources and reactivation temperatures varying in the range 40-95 • C. The main preparation methods are synthesis from solution and mechanoactivation, while US 2016/0046534 A1 reports procedures combining the features of both methods.All the compounds reported above have been obtained from solution, whereas only MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O has been obtained by mechanoactivation as a pure end product.The solvent type plays a key role for the run products, thus MgSO 4 have previously been obtained by evaporation from water solutions.However, in this case water is both a solvent and a reactant.In other cases, a methanol solution has been used as a medium e.g., [23].The latter compounds have been reported to be highly hygroscopic and unstable.
It should be noted that identification of the above-mentioned phases has been mainly based on chemical analysis and PXRD.Only have been identified by SCXRD [32,33].The presence of any crystalline substance in pure or mixed products can only be unambiguously evidenced by the knowledge of its crystal structure.Typically, this is obtained by comparing calculated and experimental diffraction data.Moreover, crystal structures provide a basis for precise interpretation of the physico-chemical characteristics of the studied substances, which in turn allows optimization of methods for their syntheses.
The aims of this study str: (i) to add new knowledge about the trends and consistencies in the preparation procedures of the products obtained in the system MgSO 4 -OC(NH 2 ) 2 -H 2 O; (ii) to determine the crystal structures of those MgSO 4 •nOC(NH 2 ) 2 •mH 2 O phases that have not been sufficiently studied before and to compare them to the already known ones; (iii) to evaluate the influence of water and urea molecules on certain physico-chemical properties of Crystals 2024, 14, 227 3 of 13 the studied compounds, e.g., solubility and thermal stability, directly related to their application as fertilizers or soil additives.

Syntheses Conditions
The reagents used for the syntheses were: MgSO 4 source-either MgSO 4 O has also been taken into account in calculations of the recipes.Both magnesium sources are comparatively stable under normal conditions evidence also by their existence as mineral species-epsomite and kieserite respectively (https://www.mindat.org, 2 January 2024).In a typical synthesis the appropriate ratio of the three initial reagents were mixed with or without grinding according to the chosen strategy and then placed in thermostat and heated at the desired temperature until complete evaporation of the excess water.

Syntheses Approaches
The studied compounds are highly water-soluble complex salts.They are easily formed under various conditions and within a wide range of the synthesis medium parameters such as temperature and ratio of the initial reactants.In laboratory conditions, methods such as crystallization from solution [24,25] and more recently mechanochemistry [27][28][29][30][31] are used for their preparation.Techniques combining features of both methods have also been used.The reason for this is the high reactivity of the reagents, in which usually urea molecules displace water ones from the magnesium coordination surrounding and water is released.As a result, even short-term grinding at room temperature in an agate mortar of an initial batch consisting of the three starting components leads to the formation of a homogeneous slurry.By appropriate heat treatment it is possible to obtain from it a single well-crystallized phase of magnesium urea sulfate hydrate as the final product.This prior knowledge allowed outlining of two synthesis strategies.
On one hand, based on the efforts of previous researchers to obtain new knowledge for some of the studied compounds prepared from aqueous solution, triangular diagrams of crystallization (mole %) were constructed (see next section, Figure 1).Analysis of the data directed attention to synthesis conditions favourable for achieving the set goals-obtaining solely a pure phase in the final product.The conduct of the new syntheses showed that in some cases the conditions often exceed the limits of crystallization from solution and acquire characteristics of preparation by mechanoactivation, especially where the intermediate product resembles a slurry.Without claiming to be exhaustive in terms of precise delineation of the phase boundaries and the amount of yield, the obtained results build on the previous ones.The diagram in Figure 2 also indicates those conditions under which the highest percentage yields of the tested compounds were obtained.The diagrams have been constructed on results obtained from PXRD studied materials processed with appropriate software programs.These data reveal certain important trends in the relationship between the initial synthesis conditions and the obtained phases and can be used in future to optimize the procedures for preparation of desired final products.The following features are observed in this synthesis approach: short synthesis duration (24-96 h); imperfect tiny crystals; more often mixtures of crystalline and amorphous phases as run products.
On the other hand, syntheses aiming to obtain crystals suitable for single crystal X-ray analyses were planned.In this case, crystallization from a solution was preferred and used, because this technique ensures the production of sufficiently large and high-quality crystals, although it requires a longer duration (1-2 weeks).The results are important for conducting proper phase identification by simulating powder X-ray diffraction patterns based on the single crystal studies and semi-quantitative phase analysis in cases where the run-product contains more than one phase.The materials used for the subsequent single crystal, thermal and spectroscopic analyses were obtained mainly in this way.
processed with appropriate software programs.These data reveal certain important trends in the relationship between the initial synthesis conditions and the obtained phases and can be used in future to optimize the procedures for preparation of desired final products.The following features are observed in this synthesis approach: short synthesis duration (24-96 h); imperfect tiny crystals; more often mixtures of crystalline and amorphous phases as run products.On the other hand, syntheses aiming to obtain crystals suitable for single crystal Xray analyses were planned.In this case, crystallization from a solution was preferred and used, because this technique ensures the production of sufficiently large and high-quality crystals, although it requires a longer duration (1-2 weeks).The results are important for conducting proper phase identification by simulating powder X-ray diffraction patterns diagrams have been constructed on results obtained from PXRD studied materials processed with appropriate software programs.These data reveal certain important trends in the relationship between the initial synthesis conditions and the obtained phases and can be used in future to optimize the procedures for preparation of desired final products.The following features are observed in this synthesis approach: short synthesis duration (24-96 h); imperfect tiny crystals; more often mixtures of crystalline and amorphous phases as run products.On the other hand, syntheses aiming to obtain crystals suitable for single crystal Xray analyses were planned.In this case, crystallization from a solution was preferred and used, because this technique ensures the production of sufficiently large and high-quality crystals, although it requires a longer duration (1-2 weeks).The results are important for conducting proper phase identification by simulating powder X-ray diffraction patterns

Powder X-ray Diffraction (PXRD)
Powder XRD patterns of the studied samples were recorded on Empyrean Powder X-ray diffractometer (Malvern Panalytical, Netherlands) in the 2 • -90 • 2θ range, overall scanning time 15 min, using Cu radiation (λ = 1.5406Å) and PIXcel3D detector.Phase identification was carried out using the HighScore Plus program [34] and/or through X-ray powder diffraction patterns simulated on the basis of the single-crystal studies for each of the studied complex salts using the PowderCell program [35].The semi-quantitative phase analysis was also conducted in the same environments.

Colourless crystals of MgSO
were mounted on a glass capillary and used for single crystal diffraction analyses.The data collection experiments were performed on Bruker D8 Venture diffractometer.The determination of unit cell parameters, data integration, scaling and absorption corrections were carried out using APEX4 program package.The crystal structures were solved by direct methods (SHELXS-97/2013) and refined by full-matrix least-square procedures on F 2 (SHELXL-97/2013).The hydrogens of the urea molecules were positioned geometrically, while the hydrogens of the water molecules were found by Fourier difference.All hydrogen atoms were refined by a riding model with U iso 1.2 times that of the attached nitrogen or oxygen atom.The experimental and structure refinement parameters are given in Table 1.Information about the structural data is available in the Cambridge Structural Database: CSD 2331202, CSD 2331203 for Mg(SO 4 )•OC(NH 2 ) 2 .2H 2 O and Mg(SO 4 )•OC(NH 2 ) 2 .3H 2 O, respectively.

Thermal Analyses
The differential scanning calorimetry (DSC) and thermogravimetry (TG) were carried out on the DSC-TG analyzer Setsys Evolution 2400, SETARAM at the following conditions: temperature range from 20 to 320 • C under Ar flow of 30 mL min −1 , with a heating rate of 10 • C min −1 and 10-12 mg sample mass in a corundum crucible.Such temperature range has been chosen for practical reasons and namely before the occurrence of complete urea decomposition.A calibration run with empty crucible was applied for all experiments to base line slope correction of both DSC and TG signal.Simultaneous analysis of the evolved gases (EGA) was performed via mass spectrometry using a quadrupole mass spectrometer (QMS) OmniStar connected to the TG apparatus.The mass/charge (m/z) values programmed for detection in QMS were for the following gases: CH 4 (16); NH 3 (17); H 2 O (18), NO 2 (28) and CO 2 (44).

IR and Raman Spectroscopy
Infrared spectra were measured using Tensor 37 (Bruker) FT-IR spectrometer with 4 cm −1 spectral resolution after averaging 128 scans on standard KBr pallets in the spectral region 400-4000 cm −1 at room temperature.Raman scattering experiments were performed using LabRam HR (Horiba) spectrometer equipped with an Olympus BH41 microscope.The measurements were conducted using the 633-nm line of He-Ne laser in a backscattering geometry with an objective ×50.The spectra were collected in the range 100-4000 cm −1 .Software package Origin 9 was used for spectral presentation.

Synthesis of Crystal Phases in the System
Figure 1 summarizes the results of previous synthesis [21][22][23][24] with respect to the experimental conditions and the type of phases obtained.In the diagram, we have not shown the products in the system at 25 • C because we could only find the abstract of the publication [25], which does not give any information about the ratio of the initial reagents.Figure 2 shows synthesis results of the present study.Symbols from the legend indicate the compounds obtained at 40 (blue color) and at 60 (red color) • C, respectively.Their positions in the diagrams correspond to the molar ratios of the reactants in the system.Figures showing the semi-quantitatively measured phase ratios (wt.%) are inserted immediately next to the symbols.In the studied system, maximum yields of urea complexes of magnesium sulfates are obtained under the following conditions: Such variety of products is due both to the high sensitivity of the studied system to the synthesis temperature and the ratio of the starting reagents, as well as to the high solubility of all considered phases.The latter allows easy structural arrangement and rearrangement of the primary and secondary building units with respect to the Mg polyhedral surrounding construction in the final products.Although the synthesis studies are not exhaustive, the achieved results clearly outline certain trends and consistencies.There is a direct dependence of the ratio of reactants and the chemical composition of the final products.Magnesium crystal hydrates crystallize as concomitant products in these parts of the system where there is an excess of SO 4  2− anions.An increase in temperature leads to expansion of the fields of crystallization of the resulting phases that are of interest in this study, in direction and at the expense of the starting reactants.
Suitable samples for structural, IR and DSC-TG-MS analyses were obtained by crystallization from water solution under the following syntheses conditions:

Single Crystal Analyses
The experimental and structure refinement parameters for MgSO 2. The molecular units of these compounds are shown in Figure 3 and their three-dimensional packing is shown in Figures S1 and S2.The crystal structures of MgSO 4 •4OC(NH 2 ) 2 •H 2 O and MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O have been published earlier [32,33].MgSO 4 •OC(NH 2 ) 2 •2H 2 O crystallizes in the triclinic crys- tal system, space group P-1.The magnesium ions in this compound form two types of octahedra.The octahedral units of the first type (MgO 4(SO4) O 2(H2O) ) are connected by Mg-O-S-O-Mg bridges to neighboring octahedra of the same type to build chains parallel to [100].The octahedral units of the second type (MgO 2(SO4) O 2(H2O) O 2(urea) ) connect the chains in [001] direction to form electroneutral layers parallel to (010).A schematic presentation of the described arrangement is shown in Figure 4.The water and urea molecules participate in a complex system of hydrogen bonding and stabilize the threedimensional packing of the layers (Figure S1 and Table S1).The hydrogen atoms of the water molecules are only involved in intra-layer hydrogen bonds of the type O-H. ..O, whereas the hydrogen atoms of the urea molecules are involved in both intra-layer and inter-layer hydrogen bonds.MgSO4•OC(NH2)2•3H2O crystalizes in a monoclinic crystal system, space group P21.In contrast to MgSO4•OC(NH2)2•2H2O, there is only one type of magnesium polyhedra (MgO2(SO4)O3(H2O)O1(Urea)) arranged in a folded electroneutral chain (Figure 4).The chains run parallel to [010] and their three-dimensional packing is stabilized by a network of hydrogen bonds in which all possible donors and acceptors are involved (Figure S2 and Table S2).Similar to the previously described compound, the water hydrogens stabilize the intra-chain arrangement, while the urea hydrogens participate in both intra-chain and inter-chain hydrogen bonding.MgSO4•4OC(NH2)2•H2O crystallizes in a monoclinic crystal

Thermal Data
DSC-TG(DTG)-MS data of the compounds under study are presented in Figure 5.In the set temperature interval, the four studied compounds exhibit similar features of thermal behavior manifested in the following sequence: compound melting, crystallization water release, and urea decomposition.The first endothermic peak observed on the DSC curves for all of the studied compounds refers to the occurrence of melting processes at 62.0 °C, 87.5 °C, 91.7 °C and 128.2 °C.As can be seen, the melting temperature increases with decreasing of the crystallization water content for the corresponding compound.It should be mentioned that data on the melting temperature of MgSO4•6OC(NH2)2•0.5H2O obtained by mechano-chemical synthesis have been previously reported [27].These authors stated that the melting effect occurs at 210 °C, although in the figure presented, a small endothermic peak could be detected at 127 °C (a temperature similar to that obtained in this study), which the authors did not attribute to any thermal process.The endoeffects positions and corresponding mass losses observed for MgSO4•OC(NH2)2•3H2O and MgSO4•OC(NH2)2•2H2O correlate well with those previously reported in US 2016/0046534 A1 patent data.The endothermal events occurring below 130 °C refer to the releasing of crystallization water molecules and their quantity per formula unit has been calculated on the basis of TG data.For MgSO4•OC(NH2)2•3H2O, one water molecule is released within the endothermal range, of which the maximum is at 116.6 °C.For MgSO4•4OC(NH2)2•H2O and MgSO4•6OC(NH2)2•0.5H2O, these effects occur at 124.4 °C and 128.2 °C and refer to the releasing of one or a half water molecules, respectively.All subsequent endothermal effects are related to the evolving of a variety of volatiles including CH4, NH3, H2O, NO2 and CO2.The results are indicative that, after 150 °C, the crystallization water release and urea decomposition occur simultaneously for all of the studied compounds.In general, the urea decomposition starts at various temperatures for each of the compounds:   In contrast to MgSO 4 •OC(NH 2 ) 2 •2H 2 O, there is only one type of magnesium polyhedra (MgO2 (SO4) O3 (H2O) O1 (Urea) ) arranged in a folded electroneutral chain (Figure 4).The chains run parallel to [010] and their three-dimensional packing is stabilized by a network of hydrogen bonds in which all possible donors and acceptors are involved (Figure S2 and Table S2).Similar to the previously described compound, the water hydrogens stabilize the intra-chain arrangement, while the urea hydrogens participate in both intra-chain and inter-chain hydrogen bonding.MgSO 4 •4OC(NH 2 ) 2 •H 2 O crystallizes in a monoclinic crystal system, space group P21/n, and exhibits structure where electroneutral magnesium octahedra (MgO4 (urea) O1 (H2O) O1 (SO4) ) occur as structure building units (Figure 4).MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O crystallizes in an orthorhombic crystal system, space group Pccn.Complex (MgO6 (urea) ) 2+ cations and (SO 4 ) 2− anions are packed in such a way as to form the 3D crystal structure involving water molecules in the interstitials (Figure 4).The coordination polyhedra of Mg atoms for the known MgSO 4 •nOC(NH 2 ) 2 •mH 2 O compounds are presented in Table S3.Similar to the magnesium sulfate hydrates' structures found in the available structural databases (Cambridge Structural Database, Crystallography Open Database and American Mineralogist Crystal Structure Database), in the compounds studied here, the magnesium atom is in octahedral coordination.When the ligands number is less than six, the magnesium octahedra exhibit a tendency to polymerize, forming electroneutral units such as layers and chains or remaining as insular moieties in the structure (Figure 4).With six or more ligands in the compound, isolated complex magnesium cations are formed, the relatively large sizes of which predetermine the specific 3D arrangement of the structural units.Typical of the latter type compounds is the ionic nature of the bonds between the complex units.As for the structures made of electroneutral units, their tri-dimensional arrangement is stabilized by only hydrogen bonds.

Thermal Data
DSC-TG(DTG)-MS data of the compounds under study are presented in Figure 5.In the set temperature interval, the four studied compounds exhibit similar features of thermal behavior manifested in the following sequence: compound melting, crystallization water release, and urea decomposition.The first endothermic peak observed on the DSC curves for all of the studied compounds refers to the occurrence of melting processes at 62.0 • C, 87.5 • C, 91.7 • C and 128.2 • C. As can be seen, the melting temperature increases with decreasing of the crystallization water content for the corresponding compound.It should be mentioned that data on the melting temperature of MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O obtained by mechano-chemical synthesis have been previously reported [27].These authors stated that the melting effect occurs at 210 • C, although in the figure presented, a small endothermic peak could be detected at 127 • C (a temperature similar to that obtained in this study), which the authors did not attribute to any Based on these data, it could be concluded that the number of water molecules in the crystal structure is of particular importance for their thermal behavior and stability.It is Based on these data, it could be concluded that the number of water molecules in the crystal structure is of particular importance for their thermal behavior and stability.It is evident that as the water content of the compound decreases, both melting point and urea decomposition temperature increase.The substitution of urea for water also plays a role in the structure stabilization, with the most stable structure being the one in which the magnesium surrounding involves solely urea moieties.Such a type of thermal stability trend also been observed for other crystal hydrate adducts of urea [12,20].

IR and Raman Spectra
The infrared spectra of magnesium sulfates are dominated by the absorption peaks of sulfate group and water molecules and their peak positions and assignments have already been reported [1,[36][37][38].Experimental IR spectra of the studied compounds are presented in Figure 6.The peaks in the range of O-H stretching of water molecules are overlapped by the peaks of NH 2 stretching of urea [20].The samples of the compounds with six and four urea molecules exhibit three distinguishable peaks at 3480, 3350 and 3210 cm −1 , whereas for the other two compounds with higher water contents these peaks merge into one broad band.In addition, the position of the peak arising from δ (CNH) is sensitive to the urea to water ratio.The position of this peak shifts from 1470 cm −1 in sample MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O to 1480 cm −1 in a sample with higher water content (MgSO 4 •OC(NH 2 ) 2 •3H 2 O).Another significant spectral difference can be detected in the region of ϱ(OH 2 ) rock + δ(OCN).Samples with high urea content reveal a peak at 783 cm −1 , whereas another peak at around 750 cm −1 appears with increasing water content.Within the range 900-1150 cm −1 , strong absorption of SO 4 and NH 2 groups dominates.It can be seen that the intensity ratio of the peaks at 1110 and 1150 cm −1 changes with the ratio of urea to water.The absorption near 1150 cm −1 is stronger for MgSO 4 •6OC(NH 2 ) 2 •0.5H 2 O, whereas with the increase of water molecules in the rest of the compounds, the intensity of the peak at 1110 cm −1 increases.Raman spectra of the studied compounds are presented in Figure 7.The spectra are dominated by the strong peaks at 980, 1012, 1020 and 1025 cm −1 in the range of ν(SO 4 ) and N-C-N stretching vibrations [39].There are peaks at 980, 1013 and a shoulder at 1022 cm −1 in the spectrum of MgSO  ready been reported [36][37][38][39].Experimental IR spectra of the studied compounds are presented in Figure 6.The peaks in the range of O-H stretching of water molecules are overlapped by the peaks of NH2 stretching of urea [20].The samples of the compounds with six and four urea molecules exhibit three distinguishable peaks at 3480, 3350 and 3210 cm −1 , whereas for the other two compounds with higher water contents these peaks merge into one broad band.In addition, the position of the peak arising from δ (CNH) is sensitive to the urea to water ratio.The position of this peak shifts from 1470 cm −1 in sample MgSO4•6OC(NH2)2•0.5H2O to 1480 cm −1 in a sample with higher water content (MgSO4•OC(NH2)2•3H2O).Another significant spectral difference can be detected in the region of ρ(OH2)rock + δ(OCN).Samples with high urea content reveal a peak at 783 cm −1 , whereas another peak at around 750 cm −1 appears with increasing water content.Within the range 900-1150 cm −1 , strong absorption of SO4 and NH2 groups dominates.It can be seen that the intensity ratio of the peaks at 1110 and 1150 cm −1 changes with the ratio of urea to water.The absorption near 1150 cm −1 is stronger for MgSO4•6OC(NH2)2•0.5H2O,whereas with the increase of water molecules in the rest of the compounds, the intensity of the peak at 1110 cm −1 increases.Raman spectra of the studied compounds are presented in

Figure 2 .
Figure 2. Diagram of crystallization of magnesium compounds prepared in the system MgSO4-OC(NH2)2-H2O at 40 and 60 °C based on the results from this study.

Figure 2 .
Figure 2. Diagram of crystallization of magnesium compounds prepared in the system MgSO4-OC(NH2)2-H2O at 40 and 60 °C based on the results from this study.

Figure 2 .
Figure 2. Diagram of crystallization of magnesium compounds prepared in the system MgSO 4 -OC(NH 2 ) 2 -H 2 O at 40 and 60 • C based on the results from this study.

Figure 5 .
Figure 5. DSC-TG(DTG)-MS data of the studied compounds.The numbers indicate molecular weight of the corresponding gas as follows: 16 for CH 4 ; 17 for NH 3 ; 18 for H 2 O; 28 for NO 2 , and 44 for CO 2 .

Figure 6 .
Figure 6.Infrared spectra of the studied compounds.

Figure 6 .
Figure 6.Infrared spectra of the studied compounds.

Table 2 .
Most important data collection and refinement parameters for the studied compounds.