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. 2023 May 8;8(20):17800–17808. doi: 10.1021/acsomega.3c00622

Synthesis, Thermal Analysis, Spectroscopic Properties, and Degradation Process of Tutton Salts Doped with AgNO3 or H3BO3

Tiago S Pacheco †,‡,*, Zélia M C Ludwig †, Victor H Oliveira †, Ingrid D Barcelos §, Rafael L de Souza ∥,⊥, Edinei C Paiva ∥,#, Maximiliano D Martins ∥, Flavia C Marques ∇, Gustavo F S Andrade ∇, Santunu Ghosh ○,*
PMCID: PMC10210023  PMID: 37251174

Abstract

graphic file with name ao3c00622_0006.jpg

In this work, we synthesized and studied the spectroscopic properties of (NH4)2(SO4)2Y(H2O)6 (Y = Ni, Mg) crystals doped with AgNO3 or H3BO3. These crystals constitute a series of hexahydrated salts known as Tutton salts. We investigated the influence of dopants on the vibrational modes of the tetrahedral ligands NH4 and SO4, octahedral complexes Mg(H2O)6 and Ni(H2O)6, and H2O molecules present in these crystals through Raman and infrared spectroscopies. We were able to identify bands that are attributed to the presence of Ag and B dopants, as well as band shifts caused by the presence of these dopants in the crystal lattice. A detailed study of the crystal degradation processes was performed by thermogravimetric measurements, where there was an increase in the initial temperature of crystal degradation due to the presence of dopants in the crystal lattice. Raman spectroscopy of the crystal residues after the thermogravimetric measurements helped us to elucidate the degradation processes occurring after the crystal pyrolysis process.

1. Introduction

A wide variety of complex inorganic materials composed of bimetallic sulfates are well known in the scientific community, for example, dehydrated A2B2(SO4)3 complexes are known as the langbeinite phase, dihydrated complexes constitute the A2B(SO4)2·2H2O krohnkite phase, and tetrahydrate complexes are leonites A2B(SO4)2·4H2O. In particular, hexahydrate complexes A2B(SO4)2·6H2O constitute the Tutton salt family, where A is a monovalent alkali metal or ammonium and B is a bivalent transition metal; S can be replaced by Se and H2O by D2O, as reported by Saha et al.1

Tutton salt crystals started to be studied by Alfred E. H. Tutton around 1890.2−4 This family of isostructural crystals can assume a broad range of compositions with different properties. Interestingly, regardless of their chemical composition, this family of salts crystallizes in the monoclinic system with the spatial group P21/c with two molecules occupying the unit cell Z = 2. The empirical formula that represents these crystals is A2B(YO4)2(H2O)6, where A = Cs+, K+, NH4+, Rb+, and Tl+; B = Co2+, Cu2+, Fe2+, Mn2+, Ni2+, V2+, and Zn2+; and Y = S, Se, and Cr, and can still be deuterated. These crystals can be used as optical filters to suppress transmission bands in the visible and allow passage in the UV region for wavelengths below 400 nm and IR for wavelengths between 700 and 1100 nm, mainly for transition metals Co, Cu, Fe, Mn, and Ni. Also, they can be used as radiation filters in UV/IR detectors used for military purposes in missile approach warning systems.3,5,6

The structure of Tutton salt is composed of SO42– tetrahedrons and M(H2O)62+ octahedrons through hydrogen bonds of H2O molecules and interconnected by monovalent cations K+, Rb+, Cs+, or NH4+. These above types of connections can be affected by agents such as dopants/impurities in the crystalline network of these materials. The presence of dopants can lead to changes in the normal vibrational modes of the molecular groups SO4, NH4, H2O, and M(H2O)6.7−9 In recent years, several studies have been reporting on the attempt of doping Tutton salt family crystals, in addition to theoretical–computational studies (density functional theory (DFT)) where band structures and calculations of vibrational frequencies were studied.10−12 Notably, our team synthesized K2M(SO4)2(H2O)6 mixed crystals, with M being a mixed composition of Ni/Co, to study the effects of a lithium dopant on the vibrational modes of the tetrahedral molecular groups SO4 and octahedral Ni(H2O)6 and Co(H2O)6, as reported by Pacheco et al.13

Other studies provide insights into doped crystals of the Tutton salt family with rare-earth ions, and the properties of the emission/luminescent absorption processes of rare-earth ions were investigated and possible applications in nonlinear optics were evaluated.7,14−17 Additionally, Abu El-Fadl et al.18 introduced doping with small fractions of iodide ions and verified subtle changes in powder X-ray diffraction patterns, transmittance properties, thermal behavior of their samples, and unexpected second harmonic generation behaviors. In that sense, researchers who developed studies on Tutton salts are increasingly seeking to combine the properties of bivalent ions such as Co2+, Ni2+, Mg2+, Mn2+, and Cu2+ in the crystalline structure of mixed or even doped salts in order to improve some of its properties or even discover new properties.

Neto et al.19 concluded in a new and interesting study that these crystals can be applied in thermochemical systems for thermal energy storage and also evaluated the empty spaces present in the unit cells of their crystals through electronic density isosurfaces, showing that high percentage of empty spaces can cause a decrease in the energy of interactions affecting physicochemical parameters such as solubility, dissolution, and hardness of crystalline structures. On the other hand, these empty spaces can be filled by dopants in order to strengthen these intermolecular interactions in order to increase, for example, the thermal stability of the crystals.

In the present study, we developed the synthesis of doped Tutton crystals using the crystal growth technique by slow isothermal evaporation. Moreover, we performed a study of the thermal and vibrational properties of silver-doped magnesium ammonium sulfate hexahydrate crystals (AMgSH:Ag), silver-doped nickel ammonium sulfate hexahydrate (ANiSH:Ag), and boron-doped nickel ammonium sulfate hexahydrate (ANiSH:B). Regarding the vibrational modes, our results were presented, discussed, and compared with the literature for pure crystals with similar compositions. In Raman spectra, we identified the vibrational modes of molecular groups SO4, M(H2O)6, and H2O. In addition, we were able to identify some bands that can be attributed to moieties containing Ag or B dopants, as well as band shifts caused by the presence of dopants in the crystal lattice. In thermogravimetric measurements, we verified that the crystals had significant gains in their initial dehydration temperatures caused by the presence of dopants. Furthermore, with Raman spectroscopy, the vibrational modes of the molecular groups that compose the structures of the oxide residues resulting from the thermogravimetric measurements were identified.

2. Materials and Methods

Our samples of crystals (NH4)2Mg(SO4)2·6H2O:AgNO3 (AMgSH:Ag), (NH4)2Ni(SO4)2·6H2O:AgNO3 (ANiSH:Ag), and (NH4)2Ni(SO4)2·6H2O:H3BO3 (ANiSH:B) were grown by the method of slow evaporation of the solvent in an aqueous solution with the temperature maintained at 40 °C. The precursor reagents for preparing the growth solutions were ammonium sulfate (NH4)2SO4, 99% purity; nickel sulfate hexahydrate Ni(SO4)2·6H2O, purity 98%; magnesium sulfate heptahydrate Mg(SO4)2·7H2O, 99% purity; silver nitrate AgNO3, 99.5% purity; and boric acid H3BO3, 99.5% purity.

The stoichiometric quantities of the starting materials are described in Table 1. After the reagent masses were measured, the solutions were prepared by dissolving the solids in 200 mL of deionized water with pH = 6 and R = 18.2 MΩ cm. To solubilize the reagents, the solution was heated up to a temperature of 50 °C and stirred for 1 h. Then, the solution was filtered on a filter paper (14 μm pores, 205 μm thickness, 80 g m–2) and taken to an oven with a temperature of 40 ± 1 °C, where the growth process took place in an average time of 20 days.

Table 1. Masses in Grams of Precursor Reagents Used to Crystallize the Samplesa.

reagents (NH4)2SO4 Mg(SO4)·7H2O Ni(SO4)·6H2O AgNO3 H3BO3
AMgSH:Ag 5.0003 9.3260   0.2004  
ANiSH:Ag 5.0030   9.9431 0.2014  
ANiSH:B 4.9988   9.9430   0.6142
molar mass (g mol–1) 132.14 246.47 262.85 169.87 61.83
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a

Molar masses are also given in the last line.

The thermogravimetry/differential thermal analysis (TG/DTA) thermogravimetric analysis was performed using a NETZSCH model STA 449 F3 Jupiter calorimeter. The samples were ground using a ceramic mortar, and the measurements were carried out at a heating rate of 10 °C min–1, covering the temperature range from 50 to 1000 °C, in an inert atmosphere of N2 and a flow of 20 mL min–1.

Raman spectra were acquired using a Bruker spectrometer, model SENTERRA, coupled to an Olympus microscope, with the excitation radiation at 632.8 nm from a HeNe laser and a laser power of 20 mW. For the acquisition of the Raman spectra, the sample at room temperature was placed on a rigorously cleaned glass slide. Data collection was performed using a 50× magnification objective lens (NA 0.51) and the acquisition time was 20 s.

Micro-FTIR measurements were performed using a Cary 620 FTIR spectromicroscopy from Agilent Technologies using a Globar source. Single-point reflectance spectra were collected in the mid-infrared range of 400–6000 cm–1, with a spectral resolution of 8 cm–1, signal reading by an MCT-100 μm detector, and a 25× objective lens with an approximately 400 × 400 μm2 spot size. The final spectrum is an accumulation of 64 scans normalized by the spectrum of a clean Au surface as a background reference.

3. Results and Discussion

Thermogravimetric analyses allowed a quantitative and qualitative study regarding all stages of the crystal degradation processes. In Figure 1, the TG/DTA curves of the obtained crystals are shown, where all stages of degradation of the crystals can be observed for each sample. The DTA curves in Figure 1a–c (samples AMgSH:Ag, ANiSH:Ag, and ANiSH:B) show two endothermic DTA peaks during dehydration in the temperature range of 100–270 °C. These crystals also acquire the anhydrous langbeinite crystalline phase (NH4)2M(SO4)2:X, where M = Mg and Ni and X = B and Ag. In the temperature range of 250–540 °C, four endothermic peaks appear in the DTA curves, referring to the decomposition of NH4+, H3BO3, or AgNO3 and of a SO42– moiety into SO and O2. In the last degradation step, in the temperature range of 745–890 °C, one may observe that an endothermic peak appears in the DTA curves of the samples ANiSH:Ag and ANiSH:B (Figure 1b,c), referring to the decomposition of one mol equivalent of SO42– into SO2 and (1/2)O2. However, for sample AMgSH:Ag (Figure 1a), the decomposition of the SO42– molecule seems to start around 890 °C going up to 1000 °C, decomposing one-third of the SO42– mol equivalent. Accompanying these figures, in Tables S1–S4, we present a detailed description of the theoretical values of the percentages of crystal mass losses in comparison with the values obtained experimentally for the chemical reactions that occur during each step of crystal degradation.

Figure 1.

Figure 1

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TG/DTA curves for the percentage of mass loss together with the endothermic peaks of temperature variation involved in each step of degradation of (a) AMgSH:Ag, (b) ANiSH:Ag, and (c) ANiSH:B crystals.

All degradation steps for each sample are described in detail in Tables S1–S4, where we presented the initial dehydration temperature and DTA peak position. The percentage values of ideal mass losses (%) were calculated from the empirical formula of each crystal, adding the atomic masses of the amounts of each chemical element present in that formula; then, the proportionality % is attributed to each element or molecule that the sample expels in gaseous form during its degradation process.

It can be seen from the DTA curve of Figure 1 that each mass loss is accompanied by endothermic peaks. Analyzing the degradation processes of samples AMgSH:Ag, ANiSH:Ag, and ANiSH:B, shown in Figure 1a–c, and the assignment of the mass in TG and peaks in DTA present in Tables S1–S4, one may observe that in the temperature range between 110 and 230 °C, the samples suffered a mass loss of approximately 17–26%, corresponding to the mass of six molecules of H2O, present in the crystal structure. For the other samples AMgSH:Ag, ANiSH:Ag, and ANiSH:B, the second degradation step is equivalent to approximately 16–23% and occurs between 240 and 506 °C; the decomposition sequence corresponds to the loss of 2 mol equiv of NH3, one H2O, and one SO2. The last degradation step occurs in the temperature range of 520–890 °C for ANiSH:Ag and ANiSH:B samples, resulting from the decomposition of the SO42–, equivalent to 17–19% mass loss. Conversely, sample AMgSH:Ag suffers a partial degradation of one SO42–, corresponding to approximately 6% mass loss. The final residues in samples AMgSH:Ag, ANiSH:Ag, and ANiSH:B after thermal treatment were Mg(1/2)SO2Ag(1/3)O2 and NiO3, respectively. The residual substances were confirmed through Raman spectroscopy because the vibrational modes of the oxides present in these residues were identified (a detailed discussion may be found below).

Comparing the initial degradation temperature, we observed an increase in the samples ANiSH:B and ANiSH:Ag, with temperature gains of 39 and 36 °C, respectively, while the dehydration temperature of the pure crystal (NH4)2Ni(SO4)2·6H2O was 96 °C, as reported by Pacheco et al.7 For sample AMgSH:Ag, the temperature gain was 24 °C compared to the similar pure crystal, which is 70 °C, as reported by Souamti et al.20

Raman measurements in the range of 100–3500 cm–1 were performed in all samples, as shown in Figure 2, using an excitation laser of 632.8 nm. These crystals have 234 normal vibrational modes, considering the structure of SO4, NH4, H2O, and M(H2O)6 groups, including three acoustic modes, being 1Au + 2Bu. According to the group theory, the irreducible representation for the optical phonons of these crystals is given by: Γ = 57Ag + 57Bg + 60Au + 60Bu, where only Ag and Bg modes are active in Raman, adding a total of 114 modes, and Au and Bu modes are active in IR, adding up to 120 modes.8−10,21,22

Figure 2.

Figure 2

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Raman spectra of samples ANiSH:B, ANiSH:Ag, and AMgSH:Ag (green, yellow and pink curves, respectively) in the ranges of (a) 70–900 cm–1, (b) 925–1040 cm–1, (c) 1040–2250 cm–1, and (d) 2700–3500 cm–1. We observed the bands related to the vibrational modes of molecular groups H2O, NH4+, (SO4)22–, and M(H2O)62+.

Specially doped crystals can present peculiar changes in the vibrational modes resulting from molecular interactions in the crystalline structure of these salts. In these crystalline structures, SO4 tetrahedral is present, which is linked to the M(H2O)6 octahedral by means of O–H···O hydrogen bonds between the hydrogen atoms belonging to the water molecules and the oxygen atoms of SO4; the NH4 tetrahedral is coordinated with the SO4 tetrahedral, forming the entire crystal lattice.10,21,23

Table 2 exhibits the position of Raman bands from Figure 2 and the assignment of the groups H2O, NH4+, (SO4)22–, and M(H2O)62+ to the samples ANiSH:B, ANiSH:Ag, and AMgSH:Ag. The results agree with the values presented in previous studies by Barashkov et al.8 and Ghosh et al.10

Table 2. Band Wavenumber (cm–1) and Vibrational Assignment for the Raman Spectra of ANiSH:B, ANiSH:Ag, and AMgSH:Aga.

band wavenumber (cm–1)
 literature
  
ANiSH:B ANiSH:Ag AMgSH:Ag (8) (10) assignment
112; 127 106; 127 112 110; 121 105; 113 SO4(L)
  145 145 131 122; 138
168 169   161 163 NH4(L)
188 188   170; 183 183 *(ν5)
207 207   196; 203 205 NH4(L)
230 231   218; 235   *(ν5)
261 262 251 253 241 *(ν2)
334 333 323 300; 313   H2O(Tw)
371 364 369     NH4(L)
399 398 402 384 393 *(ν1)(ss)
458 458 457 451, 457 455 (ν2) SO4(sb)
578 574 585 577 579 H2O(w)
617; 635 616; 633 623; 631 616; 627 610; 624 (ν4) SO4(ab)
  755 756     (sb)(ν4) AgNO324,25
743; 769 769   743; 807 839 H2O(r)
847; 880         (ss)H3BO326−28
  857; 890       AgNO324,25
985 991 989 983 981 (ν1) SO4(ss)
1023 1021 1022     (ν1) AgNO324,2526−28
1035 1038 1042     H3BO326−28
1073 1080 1172 1072 1068 (ν2 + ν4) SO4
1094 1100 1098 1093 1090 (ν3) SO4(as)
1137 1144 1139 1136 1136
1154 1159 1158 1152 1150
1430 1436 1433 1432 1426 (ν4) NH4(ab)
1472 1480   1467  
1675 1684 1680 1676 1670 (ν2) (NH4–H2O)(sb)
1707 1714 1712 1709 1707 NH4 (ν2)(sb)
2180 2194 2183     (ν2 + L) NH422
2850 2860 2845 2842 2845 (2ν4) NH4
2916 2923 2915 2918   (ν1) NH4
3038 3049 3026 3035 3035 (ν3) NH4
3102 3112 3091 3100 3109 (ν1) H2O
3141 3176 3150 3138   (ν3) H2O
3224 3232 3222 3232 3273
3280 3287 3300     (ν1) H2O
3336 3344 3370 3364   (ν3) H2O
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a

T = translation, L = libration, * = octahedral complex M(H2O)62+, tw = twisting, r = rocking, w = wagging, ss = symmetric stretching, sb = symmetric bending, ab = asymmetric bending, and as = asymmetric stretching.

The Raman measurements of the doped crystals in Figure 2 reveal changes compared to similar systems in the same crystal family that do not have any doping. These differences can be attributed to distortions in the bond lengths of the octahedral M(H2O)62+ and tetrahedral NH4+ and (SO4)22– caused by the influence of dopants introduced into the crystal lattice. According to Table 2, there was a marked difference for the ν1 mode of (SO4)22– in all samples, especially for samples ANiSH:B (with boron doping) and ANiSH:Ag (with silver doping) since these two are the samples with the closest composition to the nondoped crystal. One may notice that in the Raman spectrum of the crystal (NH4)2Ni(SO4)2·6H2O, there is a band at 981 cm–1 that may be assigned to the symmetrical mode of SO4 Ghosh et al.,10 while for ANiSH:B- and ANiSH:Ag-doped samples, this band appears centered at 985 and 991 cm–1, respectively. This band shift is caused by the presence of dopants that possibly change the local electron density in the vicinity of SO4, causing a higher vibrational frequency, that is, shifting the band to higher wavenumbers. In addition, the vibrational mode characteristics of the AgNO3 and H3BO3 dopants present in the crystalline structures of the crystals were also identified.

Complementary to the Raman spectroscopy results, spectroscopic measurements were performed in the mid- and near-infrared region, as shown in Figure 3. The analysis of spectra in the mid-infrared region is quite common for Tutton salts. However, for the near-infrared (NIR) region, no studies were found in the literature presenting results for this infrared range. The NIR spectra of the analyzed samples show two broad spectral bands, which arise from the presence of water, which present different coordination with the molecules in their vicinity.

Figure 3.

Figure 3

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Absorption spectra for samples ANiSH:B, ANiSH:Ag, and AMgSH:Ag obtained at (a) 400–2000 cm–1 in the mid-infrared region (400–4000 cm–1) and (b) 2000–6000 cm–1 in the initial near-infrared range (4000–6000 cm–1).

The wide bands appearing in this region of the infrared spectrum are assigned to M–OH vibrational modes and also to combinations of H–O and N–H modes, as described at the end of Table 3, according to the refs (29) and (30). The bands centered at 2340 and 2361 cm–1, visualized in the spectra shown in Figure 3, are characteristic of the asymmetric axial deformation of the O=C=O of the ambient atmosphere where the measurements were taken. The characteristic bands of deformations of the NH bond appear close to 2900 cm–1. For all samples, the frequencies of the two fundamental OH stretching vibrations, ν1 and ν3, and the bending vibration, 2ν2, of the H2O molecule are very close and cause an intermolecular coupling that occurs between similar vibrations of neighboring molecules; for these hydrated salts, this proximity causes strong broadening and general distortion of all forms of bands above 3200 cm–1. The same effect occurs in the region above 4000 cm–1 for fundamental vibrations associated with hydrogen–oxygen vibrations associated with water in the case of minerals and hydrated inorganic compounds such as Tutton salts.29,30

Table 3. Band Assignment for Near-Infrared Spectra of ANiSH:B, ANiSH:Ag, and AMgSH:Aga.

band wavenumber (cm–1)
 literature
  
ANiSH:B ANiSH:Ag AMgSH:Ag (8) (10) assignment
440; 447 440; 447 440; 455 438; 457 438; 450 (ν2) SO4(sb)
534; 568 534; 568 533; 568 544 549; 569 H2O(L)
642 646 651 615 614 (ν4) SO4(ab)
667 667 670 627; 690 625
728 761; 794 741; 759 725 744 H2O(r)
786 848 790; 815 743 769
848; 882 882 837; 882 807 770
987 987 983 983 980 (ν1) SO4(ss)
1036 1036 1036   1034 (ν2 + ν4) SO4
1099 1096 1099 1085 1094 (ν3) SO4(as)
1139 1127 1134 1144 1145
1203 1205 1199   1274
1453 1450 1454 1445 1432 (ν4) NH4(ab)
1494 1494 1494 1465 1468
1703 1703 1703 1709 1709 H2O–NH4 (ν2)(sb)
2449 2051 2047     (ν2 + L) NH4
    2117 2115   (ν2 + ν3) SO4
    2240 2240   (2ν3) SO4
2340 2340 2340     CO2 da atmosfera ambiente
2361 2361 2361    
2900 2900 2900     (2ν4) NH4
3108 3108 3108     (ν3) NH4(as)
      3364   (ν1) H2O(ss)
3445 3465       (ν3) H2O(as)
    3506     (ν1 + L) H2O
4166 4136 4150 4000 a 4400 Y–OH29,30
4227 4185 4226
4336 4342 4331
4499 4499 4499 4500 a 7000 H–O e N–H combinação de modos (sb + ss)29,30
4616 4611 4611
4916 4921 4906
5034 5085 5040
5341 5341 5341
5631 5631 5646
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a

T = translation, L = libration, * = octahedral complex M(H2O)62+, tw = twisting, r = rocking, w = wagging, ss = symmetric stretching, sb = symmetric bending, ab = asymmetric bending, and as = asymmetric stretching.

Supporting the information obtained previously through the thermogravimetric measurements, Raman measurements of the residues from the thermogravimetric measurements were obtained. This study confirms the composition of the oxide residues of the crystals after all degradation processes by identifying their characteristic vibrational modes. The Raman spectra for the thermal treatment residues are shown in Figure 4a, showing bands corresponding to the oxides Ni–O, O2–Ni–O2, and O–NiO–O.31−34 For the residues of the ANiSH:B and ANiSH:Ag samples, the band at 695 cm–1 is assigned to Ni–O–Ni bonds;33 the bands at 520 and 584 cm–1 are attributed to torsion and stretching of the Ni–O bonds, respectively. In addition, there is a broad band in the 900–1200 cm–1 range, which is attributed to Ni(O2)2; there are also two bands, one at 1096 cm–1 and another weak band at 1460 cm–1, both assignable to O–Ni–O–O.31

Figure 4.

Figure 4

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Raman spectra of sample oxide residues left over after thermogravimetric measurements: (a) 100–750 cm–1 and (b) 800–2600 cm–1.

It is clearly noted that ANiSH:B and ANiSH:Ag samples have NiO3 residues, as their compositions are very similar, and it was not possible to make a distinction in their spectra based on the effects of their dopants B and Ag. On the other hand, as expected, the Mg1/2SO2Ag1/3O2 residue has distinct Raman spectra, as it did not undergo complete degradation until reaching a temperature of 1000 °C, leaving SO2 molecules in its structure that did not wholly decompose during thermogravimetric measurements.

Residues containing boron and silver from ANiSH:B and ANiSH:Ag, respectively, present broad bands at 206, 458, and 486 cm–1, which may be associated with the translation of NiO in both. The bond at 724 cm–1 on the ANiSH:B residue, at 738 cm–1 on the ANiSH:Ag residue, and two bands at 905 and 1075 cm–1 on both residues were observed. In the region between 1250 and 1500 cm–1, we have two bands, one at 1310 cm–1 and one at 1450 cm–1, which corresponds to O–Ni–O–O.31

The Raman spectrum of the Mg1/2SO2Ag1/3O2 residue in Figure 4 has characteristic bands of the groups Mg–O, SO, Ag–O, and Ag–S, as described in Table 4. The bands assigned to SO and Mg–O bonds in the Mg1/2SO2Ag1/3O2 residue appear slightly shifted compared to the bands we had for the crystal before it underwent degradation in thermogravimetry. The bands between 650 and 900 cm–1 and 1900 and 2400 cm–1 are characteristic of water absorption from the ambient atmosphere since the residue has hygroscopic properties. In the region that goes from 1060 to 1400 cm–1, we have broad bands associated with SO, Mg–O, and Ag–O bonds, which are difficult to associate with any vibrational mode of the residue due to the widening caused by the absorption of water, resulting in a change in the structural environment.

Table 4. Vibrational Modes Observed Via Raman Spectroscopy of the Mg1/2SO2Ag1/3O2 Residuea.

Raman bands (cm–1) assignment to groups
205, 295 Ag–S(ss) 35
400 Mg–O
451 O–S–O(sb)
474 Ag–O
497 Ag–S35
510 Mg–O
607, 615 O–S–O(ab)
681, 699, 797 H2O (absorbed from the environment)
850 Ag–OH
964 S–O(ss)
1023, 1052 S–O
1060 a 1150 S–O(as), Mg–O, Ag–O
1180 a 1400 Mg–O e Ag–O
1501, 1612 Ag–O35
1772 S–O
1934, 2037, 2355 H2O (absorbed from the environment)
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a

ss = symmetric stretching, sb = symmetric bending, ab = asymmetric bending, and as = asymmetric stretching.

The results are consistent with the oxide residues proposed left over after all of the degradation steps of the samples in Tables S2–S4, in which all of the characteristic vibrational modes of these oxide residues were identified.

4. Conclusions

In this manuscript, we described the synthesis and characterization of Tutton crystals doped with H3BO3 and AgNO3, resulting in crystals of (NH4)2Ni(SO4)2·6H2O:B, (NH4)2Ni(SO4)2·6H2O:Ag, and (NH4)2Mg(SO4)2·6H2O:Ag. Thermogravimetric measurements allowed us to determine in detail the crystal degradation process up to 1000 °C, which allowed us to infer the chemical reactions that occur in each step of these processes, which are rarely reported in the literature on Tutton salts.

In addition, for these crystals, there were significant gains in dehydration temperature, which were 39, 36, and 24 °C in the crystals (NH4)2Ni(SO4)2·6H2O:B, (NH4)2Ni(SO4)2·6H2O:Ag, and (NH4)2Mg(SO4)2·6H2O:Ag, respectively, when compared with their equivalent crystals, without the influence of dopants on their structure. These considerable increases in the initial dehydration temperatures of the crystals are due to the effect of dopants on their crystal lattice, which makes them more thermally stable than conventional crystals without doping. In this sense, the Tutton salts with the doping investigated in this work may be promising materials for applications as windows for UV–IR radiation, as they are more thermally stable when compared to pure crystals of the Tutton salt family.

Concerning the Raman and infrared spectroscopic measurements, we identified the vibrational modes of H2O, NH4+, SO42–, and M(H2O)62+ groups from the crystalline structures of the synthesized crystals. Furthermore, we noted significant shifts in some bands related to these groups. The observed shifts were associated with the presence of dopants in the crystal lattice that cause distortions in the electronic densities of these molecular groups. Also, it was possible to identify characteristic bands related to the dopants. Moreover, complementary to the thermogravimetric measurements, Raman measurements of the residues confirmed that residues (NH4)2Ni(SO4)2·6H2O:B and (NH4)2Ni(SO4)2·6H2O:Ag were basically composed of NiO3 oxides. For residue (NH4)2Mg(SO4)2·6H2O:Ag, on the other hand, it was evident that samples did not completely decompose in the temperature range from 50 to 1000 °C. From the Raman results, it was possible to verify that the decomposition product was Mg1/2SO2Ag1/3O2.

The Raman results assigned the normal modes of vibration corresponding to chemical bonds Ni–O, Mg–O, Ag–O, Ag–S, and S–O, confirming the presence of dopants in the chemical composition of each residue of each crystal. It should be mentioned that some bands did not appear in the Raman spectra of the crystals before undergoing thermal degradation but appeared in the spectra of the residues. The study of residues of Tutton salts through spectroscopic techniques is still poorly explored in the literature. Therefore, our investigation opens the avenue to complement the understanding of the degradation processes of these materials.

Acknowledgments

The authors acknowledge the financial support from the Brazilian agencies Fundação de Amparo à Pesquisa do estado de Minas Gerais (FAPEMIG), Conselho Nacional de Desenvolvimento Cientifico e Tecnológico (CNPq), and Financiadora de Estudos e Projetos (FINEP) contrato CT-Infra 01.14.0015.00, referência 0633/13. The authors also would like to acknowledge the IMBUIA beamline at Brazilian Synchrotron Light Laboratory (LNLS) for providing the micro-FTIR facility. T.S.P., V.H.O., and F.C.M. thank the Coordenação de Aperfeiçoamento de Pessoal de Nível Superior (CAPES) for their doctoral scholarships. Santunu Ghosh acknowledges Prof. Alexandre Mello and PCI for the research scholarship and support.

Supporting Information Available

The Supporting Information is available free of charge at https://pubs.acs.org/doi/10.1021/acsomega.3c00622.

  • Initial dehydration temperatures and other degradation steps and description of the chemical reactions of each step of the sample degradation process: AMgSH:Ag, ANish:Ag, and AMgSH:B (PDF)

The authors declare no competing financial interest.

Supplementary Material

ao3c00622_si_001.pdf (116.8KB, pdf)

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Supplementary Materials

ao3c00622_si_001.pdf (116.8KB, pdf)

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