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Article

Synthesis and Characterization of High-Energy Anti-Perovskite Compounds Cs3X[B12H12] Based on Cesium Dodecahydro-Closo-Borate with Molecular Oxoanions (X− = [NO3]−, [ClO3]− and [ClO4]−)

by
Rouzbeh Aghaei Hakkak
,
Ioannis Tiritiris
and
Thomas Schleid
*
Institute for Inorganic Chemistry, University of Stuttgart, D-70569 Stuttgart, Germany
*
Author to whom correspondence should be addressed.
Molecules 2024, 29(2), 382; https://doi.org/10.3390/molecules29020382
Submission received: 19 December 2023 / Revised: 5 January 2024 / Accepted: 8 January 2024 / Published: 12 January 2024
(This article belongs to the Special Issue Research on the Crystal Structures and Properties of Energy Materials)
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Abstract

:
Three novel anti-perovskite compounds, formulated as Cs3X[B12H12] (X− = [NO3]−, [ClO3]−, and [ClO4]−), were successfully synthesized through the direct mixing of aqueous solutions containing Cs2[B12H12] and CsX (X−: [NO3]−, [ClO3]−, [ClO4]−), followed by isothermal evaporation. All three compounds crystallize in the orthorhombic space group Pnma, exhibiting relatively similar unit-cell parameters (e.g., Cs3[ClO3][B12H12]: a = 841.25(5) pm, b = 1070.31(6) pm, c = 1776.84(9) pm). The crystal structures were determined using single-crystal X-ray diffraction, revealing a distorted hexagonal anti-perovskite order for each. Thermal analysis indicated that the placing oxidizing anions X− into the 3 Cs+ + [B12H12]2− blend leads to a reduction in the thermal stability of the resulting anti-perovskites Cs3X[B12H12] as compared to pure Cs2[B12H12], so thermal decomposition commences at lower temperatures, ranging from 320 to 440 °C. Remarkably, the examination of the energy release through DSC studies revealed that these compounds are capable of setting free a substantial amount of energy, up to 2000 J/g, upon their structural collapse under an inert-gas atmosphere (N2). These three compounds represent pioneering members of the first ever anti-perovskite high-energy compounds based on hydro-closo-borates.

Graphical Abstract

1. Introduction

The perovskite crystal structure, with its distinctive ABX3 composition, has long been a focal point in materials science [1] owing to its diverse range of applications, spanning from photovoltaics [2] to superconductors [3]. In recent years, a counterintuitive class of materials, referred to as anti-perovskites, has emerged as a promising avenue for scientific exploration [4]. Unlike their traditional perovskite counterparts, anti-perovskite materials exhibit a unique crystallographic arrangement, characterized by an inverted cation–anion order. This unconventional configuration imparts distinct electronic, optical, and structural properties, sparking significant interest in harnessing their potential for groundbreaking advancements in various technological domains. The exploration of anti-perovskite materials has gained momentum due to their exceptional properties; these materials have demonstrated promise in diverse applications, such as having a high ionic conductivity [5], as well as opto-electronic [6], catalytic [7] and thermoelectric applications [8].
Boron (B) as a non-metal fuel has garnered considerable attention in advanced solid propellants. With a mass calorific value of up to 58.7 MJ/kg [9,10], boron surpasses another typical metal fuel, such as aluminum (Al), by almost two times, since aluminum has a calorific value of 30.8 MJ/kg. Moreover, the volumetric calorific value of boron reaches an impressive 135.2 kJ/cm3, significantly exceeding that of Al (83.3 kJ/cm3) by 51.9 kJ/cm3 [11,12]. Boron-based, fuel-rich propellants typically comprise the non-metal fuel boron, oxidants, binders, and additives. Serving as the pivotal component in propellants with a high mass ratio (usually ranging from 25 to 40%), the non-metal fuel boron continues to be a prominent focus in ongoing research [13,14].
On the other hand, hydroborates, notably with the dodecahydro-closo-dodecaborate anion [B12H12]2−, have been recognized since 1960 [15]. The alkyl-ammonium and alkali-metal compounds and derivatives originating from these hydroborates have captured the attention of numerous researchers owing to their distinctive properties [16]. Alkali- and alkaline-earth metal compounds containing the [B12H12]2− anion have exhibited outstanding stability over a wide temperature range. As an example, Cs2[B12H12] with an anti-fluorite structure arrangement remains in a solid and stable state up to temperatures of approximately 800 °C [17].
Anti-perovskites incorporating the dodecahydro-closo-dodecaborate anion [B12H12]2− have been previously synthesized, with a number of examples including Cs3Cl[B12H12], (NH4)3Br[B12H12] [18], K3I[B12H12] [19], Cs3[BH4][B12H12] [20], and luminescent Tl3Cl[B12H12] [21]. Among these compounds, only Tl3Cl[B12H12] exhibits a hexagonal and not a cubic anti-perovskite structure.
Energetic materials are one of the main topics in chemistry, because of their wide range of application as explosives [22], propellants [23] and pyrotechnic materials [24]. Boron-cluster compounds, specifically [B12H12]2−-containing ones, have become a remarkable subject of energetic research. The increased stability of these compounds compared to other borates, coupled with their substantial hydrogen and boron content, positions them at the forefront of energetic investigations. The amalgamation of the [B12H12]2− anion with energetic yet less stable cations has led to the creation of energetic salts, exemplified by diguanidinium [25] and dihydrazinium salts [26]. Under inert atmospheres like N2, dihydrazinium salts have demonstrated the capacity to release approximately 1650 J/g of heat next to elemental hydrogen (H2). Meanwhile, the combustion of diguanidinium salts has been shown to unleash an extraordinary amount of energy, reaching up to 34 kJ/g [27].
Perovskite chemistry recently advanced itself toward the synthesis of new types of energetic materials. A variety of different types of these energetic perovskites were syntheses with different compositions, such as compounds based on inorganic [28] and organic materials [29,30]. These compounds mostly use oxidizing anions, such as perchlorate, on their X-site in an ABX3 perovskite, but there is no record of energetic anti-perovskites to date.
In this research, we focused on the synthesis of the first ever high-energy anti-perovskite compounds and add new members to this family of high energetic materials. Three novel anti-perovskite compounds, namely Cs3[NO3][B12H12] (I), Cs3[ClO3][B12H12] (II) and Cs3[ClO4][B12H12] (III), were successfully synthesized and comprehensively characterized using various methods, include X-ray, single-crystal structure analysis, vibrational spectroscopy (Raman), thermogravimetry (TG), and differential scanning calorimetry (DSC).

2. Results and Discussion

2.1. Crystallography

The three new compounds Cs3X[B12H12] crystallize similarly in the orthorhombic space group Pnma with four formula units per unit cell and have similar cell parameters. Details of the crystallographic data and their determination are provided in Table 1 and an overall look at the unit cell of Cs3[ClO3][B12H12] (II), as an example, is depicted in Figure 1.
In these three compounds under consideration, four distinct molecular polyatomic anions are present: nitrate [NO3]−, chlorate [ClO3]−, perchlorate [ClO4]− and dodecahydro-closo-dodecaborate [B12H12]2−. Each of these species exhibits standard bond lengths and angles. Specifically, for nitrate, chlorate and perchlorate, the N–O and Cl–O distances and angles fall within the approximate ranges of 125–127 pm and 118–119°, 146–147 pm and 107–108°, and 141–145 pm and 109–110°, respectively [31,32,33]. Additionally, the B–B bond lengths within the [B12H12]2− anions typically range between 174 and 181 pm, and are consistently observed [25,26] for all three cases, and the same holds for the B–H distances (108–117 pm).
In all three compounds, the quasi-icosahedral [B12H12]2−-cluster units are bisected by both a mirror plane and a glide plane perpendicular to each other. All Cs+ cations exhibit a consistent placement on glide planes, while the (Cs1)+ cations, in addition to the glide planes, also reside on a mirror plane. Likewise, nitrogen and chlorine within these compounds undergo this bisection using a perpendicular mirror and glide planes.
As previously noted, these compounds exhibit a unique combination reminiscent of the anti-perovskite A3XB structure (A+ = Cs+, X− = [NO3]−, [ClO3]− and [ClO4]−, B2− = [B12H12]2−). However, it is noteworthy that, despite this association, the crystalline arrangement observed conforms to the hexagonal anti-perovskite pattern in all cases. In this specific configuration, the complex molecular oxoanions occupying the X− site are enveloped by six cations from the A+ site, forming infinite pillars in the present compounds by sharing trans-oriented faces. These pillars are parallel to the crystallographic [100] axis, as an example this arrangement in compound (I), as depicted in Figure 2, and are bundled like the hexagonal close packing of rods, as emphasized in Figure 1 for compound (II).
The monovalent molecular anions, nitrate, chlorate and perchlorate, exhibit a distinctive three-dimensional positioning within the octahedral coordination environment with Cs+ cations (two (Cs1)+ and four (Cs2)+), leading to their considerable structural resemblance. Our initial prediction for nitrate [NO3]−, based on its triangular planar two-dimensional shape, differed from that for chlorate and perchlorate, both featuring three-dimensional shapes (trigonal pyramidal and tetrahedral, respectively). However, the key to their similarity lies within the octahedral Cs+-cation arrangement. As illustrated in Figure 3, the nitrate anion is not centrally located within this octahedron, neither parallel nor perpendicular to the square. Instead, it assumes an oblique position. The standard deviation percentages (SDP) for compounds (I), (II) and (III) are 4.52, 1.13 and 1.12, respectively. These values suggest that chlorate and perchlorate can realize nearly ideal (Cs+)6 octahedra around them. In contrast, nitrate introduces a subtle distortion to the octahedral geometry. This nuanced distortion emphasizes the intricacies associated with the positioning of the nitrate anion within the crystal structure, contributing to the slight structural variations observed among the three compounds.
The coordination sphere around the Cs+ cations for both Cs1 and Cs2 in all three compounds consists of twelve (or even more) atoms, which is similar to the “normal” coordination numbers for the A site in cubic or hexagonal ABX3 perovskites. The cesium cations (1 and 2) are surrounded by two monovalent oxoanions (nitrate, chlorate and perchlorate) and four divalent anions ([B12H12]2−) with a cis-orientation, so the cesium cations are connected with two bonds and one bond to the oxygen atoms of the monovalent anions, and with one triple contact and three double contacts to surrounding boron cluster anions [B12H12]2−.
The coordination environment around both Cs+ cations (Cs1 and Cs2) in all three compounds is consistent with a coordination number of 12 and aligns well with the typical coordination numbers for perovskites (Figure 4 and Figure 5).
For compound (III), each of the cesium cations is connected again to two perchlorate anions and four boron-cluster anions, but in this compound each anion has two instances of contact with each cesium cation to add up to the coordination number of 12 (Figure 5).
Both kinds of cesium cations establish two bidentate Cs–O contacts to two monovalent perchlorate oxoanions, while (Cs1)+ is connected to four boron-cluster anions with different numbers of Cs–H contacts to each, with one monodentate, two bidentate and one tridentate contact and, for (Cs2)+, the number of Cs–H contacts to the four neighboring boron-cluster anions is ordered differently. Two monodentate and two bidentate contacts are used to complete the anti-perovskite twelvefold coordination for this position too. The interatomic distances for Cs–H and Cs–O bonds are listed in Table 2.
Figure 6 illustrates the anti-cuboctahedron {[B12H12](Cs1)4(Cs2)8}10+, which is formed by the mixed hexagonal close packing of Cs+ cations and [B12H12]2− anions. This arrangement follows the ∞ 3 {([B12H12]Cs12/4)+} structure, which is suitable for hosting X−-anion chains along [100], embedded into ∞ 1 {[XCs6/2]2+} pillars.
Despite its structure description and the cubic close packing of [B12H12]2− anions with Cs+ cations in all tetrahedral voids, the anti-fluorite arrangement of Cs2[B12H12] (Vm = 216.15 cm3/mol) appears rather fluffy. Therefore, the formation of double salts with the composition Cs3X[B12H12] is regarded as having derived from the pseudo-binaries CsX and Cs2[B12H12], and always occurs under densification when compared to the sum of their molar volumes (Σ = Vm(Cs2[B12H12]) + Vm(CsX); see Table 3). Even the formation of the dihydrate Cs2[B12H12] · 2 H2O matches this scheme.
The Goldschmidt tolerance factor is a widely employed tool to assess the stability of perovskites, calculated using the formula tG = (rB + rA)/√2(rX + rA), where rA, rB, and rX represent the ionic radii of A, B, and X, respectively, and an ideal perovskite ABX3 has a tolerance factor of 1 [21]. Calculating the Goldschmidt tolerance factors (tG) with r([B12H12]2−) = 322 pm, r(Cs+) = 177 [21], and r([NO3]−), r([ClO3]−) and r([ClO4]−) as 200, 208 and 225 [42], respectively, yields values of 0.936, 0.917 and 0.878 for compounds (I)–(III), respectively. These values fall within a narrow range, indicating a trend that aligns with predictions for the same perovskite-type structure, but not the hexagonal one. This seems to be often the case for anti-perovskite-type cesium compounds and was previously stated for Cs3OCl [43], Cs3OBr, Cs3OI [44] and Cs3OAu [45], where O2− plays the role of X− and Cl− takes the [B12H12]2− part.

2.2. Raman Spectroscopy

Raman spectroscopy was executed on powder samples of the compounds (I), (II) and (III). All three compounds exhibit similarities in four distinct regions associated with the vibrational characteristics of the dianionic boron cluster [B12H12]2−. In the spectral range spanning from 2500 to 2400 cm−1, a distinct manifestation of the symmetric breathing vibration of the boron cage becomes apparent. This phenomenon is predominantly influenced by the stretching mode of B–H bonds. Notably, the cubic Cs2[B12H12] crystals in the space group Fm 3 - [46] show only one peak in the specified region. Intriguingly, when the compound symmetry is diminished to orthorhombic in the space group Pnma, an unique outcome emerges—the region undergoes splitting, introducing a distinctive spectral pattern [21]. Accordingly, the anticipated finding is the observation of just two discernible peaks. Another marked region, spanning from 950 to 920 cm−1, corresponds to B–B stretching vibrations. At 750 cm−1, the most intense peak signifies the symmetric breathing mode of the B12 cage, while the interval from 570 to 560 cm−1 can be ascribed to more B–B stretching vibrations, culminating in lattice vibrations at approximately 200 cm−1.
In the case of compound (I), a subtle peak at 1350 cm−1 is discernible, which is attributable to the asymmetric stretch of the nitrate group. Notably, an intense symmetric stretching mode of the nitrate anion can be observed around 1050 cm−1, accompanied by a less pronounced peak at 700 cm−1, corresponding to its in-plane deformation mode. For compounds (II) and (III), distinctive features emerge, including three regions at 950 cm−1 associated with symmetric Cl–O stretching (overlapping with B–B skeleton vibrations), and wavenumbers of 620 and 470 cm−1, indicative of the active and inactive deformations of the Cl–O bonds, respectively [47]. As an example, the Raman spectrum of compound (II) is depicted in Figure 7, and the Raman spectra of compounds (I) and (III) are available as Figures S1 and S2 in the Supplementary Material.

2.3. Thermal Analysis

Two distinct methods of thermal analyses, namely TG/DTA and DSC, were conducted for the three compounds under investigation. The TG analysis revealed that the thermal decomposition of these compounds occurs at significantly lower temperatures when compared to the pure cesium salt of [B12H12]2−, namely cubic Cs2[B12H12]. In terms of mass loss, compound (I) exhibits a single-step thermal decomposition with an onset point at approximately 440 °C, resulting in a 3% mass loss (Figure 8). Conversely, compounds (II) and (III) undergo thermal decomposition in two closely spaced steps, each with less than 1% mass loss for both. The onset points for these steps are 360 °C for compound (II) and 320 °C for compound (III). The mass loss for these compounds initiates at substantially lower temperatures compared to Cs2[B12H12], which decomposes at around 800 °C.
The thermal study of these compounds also revealed intriguing energetic properties, particularly through their DSC analyses. Compound (I) exhibits a small endothermic peak around 180 °C, likely associated with a phase transition due to there being no observable mass change at this temperature. Subsequently, a substantial exothermic peak emerges at around 440 °C with an area of −1175 J/g. For compound (II), an endothermic peak appears at a remarkably low temperature of around 90 °C, followed by two consecutive exothermic peaks. The first exothermic peak has an area of approximately 800 J/g. Unfortunately, the DSC analysis could not be extended beyond 550 °C due to the crucible limitations. However, by comparing DTA and DSC numbers for the first peak, the area of the second peak was estimated to be approximately −360 J/g. Collectively, compound (II) exhibits an energy release of around 1150 J/g in two steps. In the case of compound (III), two endothermic peaks without a change in mass are observed at around 206 and 306 °C, followed by one substantial and one small exothermic peak. The first exothermic peak is observable in both DSC and DTA analyses with an energy release of around 1750 J/g. The second peak, detectable only in the DTA analysis, has an estimated energy release of around 200 J/g, resulting in a total energy release of approximately 1950 J/g (Figure 9). The observed phase transitions at lower temperatures align with findings from prior thermal studies on similar [B12H12]2−-containing compounds [10,11]. Earlier investigations into Cs2[B12H12] [17] demonstrated the remarkable stability of the cesium salt, maintaining its structural integrity up to approximately 800 °C, and, during the thermal decomposition, a singular endothermic peak was identified. However, the addition of oxidizing anions into the compound induced a notable shift, causing decomposition to initiate at far lower temperatures. This deviation from the behavior of simple salts was marked by the emergence of strongly exothermic decomposition reactions.
The decomposition temperatures of these three compounds exceed those of traditional energetic materials by far, rendering them exceptionally thermally stable. Notably, the heat release of compound (III) is nearly equivalent to that one of 1,3,5,7-tetranitro-1,3,5,7-tetrazocane (HMX, 1987 J/g). Refer to Table 4 for a comprehensive depiction of the decomposition temperatures of compounds (I)–(III) alongside the traditional high-energy materials and their density [48]. Density is a pivotal parameter in the high-energy materials domain and a higher density always favors these materials due to their lower space consumption and increased ratio of energy per volumetric space. The density of compounds (I) to (III) are relatively equal, ranging from 2.56 to 2.69 g·cm−3, respectively, due to their similarity in both unit-cell parameter and molar masses, and they always show a denser packing in comparison to pure Cs2[B12H12], as mentioned in a previous section.

3. Materials and Methods

3.1. Synthesis

The three anti-perovskite compounds featuring dodecahydro-closo-dodecaborate anions were synthesized by dissolving Cs2[B12H12] (ABCR (Karlsruhe, Germany)) in a minimal amount of distilled water. Subsequently, a 1:1 ratio of appropriate cesium salts (cesium nitrate: Sigma Aldrich (St. Louis, MO, USA), cesium chlorate: mixture of sodium chlorate (Fluka (Buchs, Switzerland)) and cesium hydroxide (Sigma Aldrich) and cesium perchlorate: prepared by mixing freshly obtained cesium hydroxide (Sigma Aldrich) with perchloric acid (70%, Fisher Scientific (Hampton, NH, USA))) was added to portions of this solution. The resulting clear brine was subjected to isothermal evaporation at room temperature, yielding transparent and colorless single crystals of the respective salts Cs3X[B12H12] (X− = [NO3]−, [ClO3]− and [ClO4]−).

3.2. Devices

3.2.1. X-ray Crystallography

Single-crystal X-ray diffraction data were acquired utilizing a Nonius κ-CCD diffractometer with Mo-Kα radiation graphite-monochromatized to a wavelength of λ = 71.07 pm. The entire process, spanning initial structure solutions via direct methods to subsequent structure refinements, was conducted using the SHELX-97 program package [49,50]. Atomic positions were accurately determined through difference Fourier maps based on the collected data, facilitating the anisotropic refinement of all non-hydrogen atoms. Detailed information regarding the data collection and the outcomes of the final structure refinements is provided in Table 1. Supplementary data related to the structure refinements can be accessed through the Fachinformationszentrum (FIZ) Karlsruhe (D-73644 Eggenstein-Leopoldshafen, E-mail: [email protected]) and are referenced with the numbers outlined in Table 1. Fractional atomic positions are additionally available in Tables S1–S3 of the Supplementary Material. It is noteworthy that, in this study, hydrogen atom positions were ascertained through electron-density maps generated by difference Fourier syntheses utilizing the X-ray diffraction data. No further calculations or corrections were deemed necessary, given that the positions of these hydrogen atoms are well-defined based on their precise angles and distances in relation to other atoms.

3.2.2. Thermal Analysis

Two distinct instruments were employed for thermal analyses in this study. The first device, STA 449 C Jupiter by Netzsch (Selb, Germany) with alumina crucibles, played a crucial role in the investigation. TG analysis was carried out in alumina crucibles with a heat rate of 5 K min−1 under an argon atmosphere. The second device, DSC 201, also from Netzsch, operated as a differential scanning calorimeter with a heating rate of 5 K min−1 and a nitrogen flow of 20 mL min−1 and samples prepared in aluminum crucibles with a maximum temperature of 600 °C. This instrument was essential in the research, providing precise measurements of the various thermal properties of the samples. These properties encompassed heat capacity, energy changes and activation energies, all of which were indispensable for the comprehensive analysis conducted in the study.

3.2.3. Raman Spectroscopy

We performed Raman spectroscopic analyses with the DXR Smart Raman system, a product developed by Thermo Fisher (Waltham, MA, USA), which operates at an excitation wavelength of λ = 740 nm. The spectroscopic data collected during these analyses were meticulously scrutinized.

4. Conclusions

The synthesis of three novel anti-perovskite compounds, Cs3X[B12H12] (X− = [NO3]−, [ClO3]−, [ClO4]−), is presented in this research. These compounds exhibit orthorhombic crystal structures in the space group Pnma, with comparable unit-cell parameters. Single-crystal X-ray diffraction has unveiled a hexagonal anti-perovskite order for each compound, characterized by pillars   ∞ 1 {[XCs6/2]2+} of trans-faced connected [XCs6]5+ octahedra, which are bundled like a hexagonal close rod packing, held together by quasi-icosahedral [B12H12]2− anions with a counter-intuitive Goldschmidt tolerance factor far below 1. Thermal analyses have revealed a reduction in thermal stability as compared to Cs2[B12H12], with decomposition processes commencing at lower temperatures (from 320 to 440 °C) upon the introduction of oxidizing anions. Additionally, differential scanning calorimetry (DSC) has indicated that the presence of molecular oxoanions in the compounds leads to an exceptional energy release potential, reaching up to 2000 J/g, as the compounds undergo structural collapse in an inert-gas atmosphere (N2). The substantial energy release and elevated decomposition characteristics render these compounds promising candidates for thermally stable energetic materials. This pioneering advancement solidifies their significance in the domain of energetic anti-perovskite materials.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules29020382/s1, Table S1. Atomic coordinates and coefficients of the equivalent isotropic displacement parameters for Cs3[NO3][B12H12] (I); Table S2. Atomic coordinates and coefficients of the equivalent isotropic displacement parameters for Cs3[ClO3][B12H12] (II); Table S3. Atomic coordinates and coefficients of the equivalent isotropic displacement parameters for Cs3[ClO4][B12H12] (III); Figure S1. Raman spectrum of Cs3[NO3][B12H12] (I); Figure S2. Raman spectrum of Cs3[ClO4][B12H12] (III).

Author Contributions

Research, analysis: R.A.H. and I.T.; writing: R.A.H.; supervision, correction: T.S. All authors have read and agreed to the published version of the manuscript.

Funding

The Federal State of Baden-Württemberg.

Data Availability Statement

CIF files are available at the CSD database. Other raw files are not necessary, and all the diagram and picture represent in article file and the Supplementary Material.

Acknowledgments

We would also like to express our gratitude to Falk Lissner from the academic staff of the University of Stuttgart for measuring single crystals and to Christof Schneck, chemical technical assistant at the Institute of Inorganic Chemistry of University of Stuttgart, for helping and providing us with insights to obtain better and more accurate thermal analysis results.

Conflicts of Interest

The authors declare no conflicts of interest.

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Molecules 29 00382 g001
Figure 1. Extended unit cell content of the crystal structure of Cs3[ClO3][B12H12] (II) as viewed along [100].
Figure 1. Extended unit cell content of the crystal structure of Cs3[ClO3][B12H12] (II) as viewed along [100].
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Molecules 29 00382 g002
Figure 2. Hexagonal anti-perovskite ordering of Cs3[NO3][B12H12] (I) as viewed along [010].
Figure 2. Hexagonal anti-perovskite ordering of Cs3[NO3][B12H12] (I) as viewed along [010].
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Molecules 29 00382 g003
Figure 3. Orientation of the monovalent oxoanions in compounds (I), (II) and (III).
Figure 3. Orientation of the monovalent oxoanions in compounds (I), (II) and (III).
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Molecules 29 00382 g004
Figure 4. Anionic coordination spheres around (Cs1)+ and (Cs2)+ in Cs3[NO3][B12H12] (I).
Figure 4. Anionic coordination spheres around (Cs1)+ and (Cs2)+ in Cs3[NO3][B12H12] (I).
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Molecules 29 00382 g005
Figure 5. Anionic coordination spheres around (Cs1)+ and (Cs2)+ in Cs3[ClO4][B12H12] (III).
Figure 5. Anionic coordination spheres around (Cs1)+ and (Cs2)+ in Cs3[ClO4][B12H12] (III).
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Molecules 29 00382 g006
Figure 6. Anti-cuboctahedron {[B12H12](Cs1)4(Cs2)8}10+ as result of the mixed hexagonal close packing of Cs+ cations and [B12H12]2− anions.
Figure 6. Anti-cuboctahedron {[B12H12](Cs1)4(Cs2)8}10+ as result of the mixed hexagonal close packing of Cs+ cations and [B12H12]2− anions.
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Molecules 29 00382 g007
Figure 7. Raman spectrum of Cs3[ClO3][B12H12] (II) recorded at an excitation wavelength of λ = 740 nm.
Figure 7. Raman spectrum of Cs3[ClO3][B12H12] (II) recorded at an excitation wavelength of λ = 740 nm.
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Molecules 29 00382 g008
Figure 8. Thermoanalytical TG/DTA and DSC diagram of Cs3[NO3][B12H12] (I).
Figure 8. Thermoanalytical TG/DTA and DSC diagram of Cs3[NO3][B12H12] (I).
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Molecules 29 00382 g009
Figure 9. Thermoanalytical TG/DTA and DSC diagrams of Cs3[ClO3][B12H12] (II) (top) and Cs3[ClO4][B12H12] (III) (bottom).
Figure 9. Thermoanalytical TG/DTA and DSC diagrams of Cs3[ClO3][B12H12] (II) (top) and Cs3[ClO4][B12H12] (III) (bottom).
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Table 1. Crystallographic data for the crystal structures of Cs3[NO3][B12H12] (I), Cs3[ClO3][B12H12] (II) and Cs3[ClO4][B12H12] (III).
Table 1. Crystallographic data for the crystal structures of Cs3[NO3][B12H12] (I), Cs3[ClO3][B12H12] (II) and Cs3[ClO4][B12H12] (III).
CompoundCs3[NO3][B12H12] (I)Cs3[ClO3][B12H12] (II)Cs3[ClO4][B12H12] (III)
temperature, K293293293
crystal systemorthorhombicorthorhombicorthorhombic
space groupPnmaPnmaPnma
a, pm848.51(5)841.25(5)892.46(5)
b, pm1045.62(6)1070.31(6)1054.89(6)
c, pm1761.38(9)1776.84(9)1718.53(9)
Dcal, g cm−32.5612.5912.627
μ(MoKα), mm−16.956.956.88
F(000), e−107211121144
hkl range12, 15, 2510, 13, 2211, 13, 22
2θmax, deg31.5127.4827.48
refl. measured31,74227,43629,173
refl. unique273019291956
Rint/Rσ0.064, 0.0260.117, 0.0420.055, 0.021
R1/wR20.042, 0.1160.050, 0.0950.022, 0.048
GooF1.0851.0611.088
CSD number231412823138822313868
Table 2. Cs–O and Cs–H bond lengths in compounds (I), (II) and (III).
Table 2. Cs–O and Cs–H bond lengths in compounds (I), (II) and (III).
CompoundCs–O Bond Lengths (d/pm)Cs–H Bond Lengths (d/pm)
Cs3[NO3][B12H12] (I)310–320313–359
Cs3[ClO3][B12H12] (II)318–327307–355
Cs3[ClO4][B12H12] (III)316–330311–357
Table 3. Molar volumes (Vm in cm3·mol−1) of compounds (I) to (III), their precursor materials, and similar hydro-borate perovskites, with a comparison of the calculated sum of the components and the real values. Vm(B) represents Vm(Cs2[B12H12]), and Vm(C) represents Vm(CsX) or Vm (ice-I), respectively.
Table 3. Molar volumes (Vm in cm3·mol−1) of compounds (I) to (III), their precursor materials, and similar hydro-borate perovskites, with a comparison of the calculated sum of the components and the real values. Vm(B) represents Vm(Cs2[B12H12]), and Vm(C) represents Vm(CsX) or Vm (ice-I), respectively.
Compound AVm(A)Vm(B) + Vm(C)Vm(B or C)Component B and C
–––216.2Cs2[B12H12] [19] (B)
Cs3[NO3][B12H12]235.3270.454.2Cs[NO3] [34] (C)
Cs3[ClO3][B12H12]240.9273.156.9Cs[ClO3] [35] (C)
Cs3[ClO4][B12H12]243.6275.569.3Cs[ClO4] [36] (C)
Cs3Cl[B12H12] [18]220.8258.342.1CsCl [37] (C)
Cs3Br[B12H12] [18]224.8263.247.0CsBr [38] (C)
Cs3I[B12H12] [18]236.9273.457.2CsI [39] (C)
Cs2[B12H12] · 2 H2O [40]202.0254.219.0H2O (ice-I) [41] (C)
Table 4. Decomposition temperatures of compounds (I)–(III) as compared to some traditional energetic materials and a compilation of their densities.
Table 4. Decomposition temperatures of compounds (I)–(III) as compared to some traditional energetic materials and a compilation of their densities.
CompoundDecomposition Peak (°C)Density (g·cm−3)
Cs2[B12H12]8001.43
Cs3[NO3][B12H12] (I)440–480–5142.56
Cs3[ClO3][B12H12] (II)3932.59
Cs3[ClO4][B12H12] (III)4052.63
Hexahydro-1,3,5-trinitro-1,3,5-triazine (RDX)2101.82
1,3,5,7-Tetranitro-1,3,5,7-tetrazocane (HMX)2831.91
2,4,6-Trinitrotoluene (TNT)2901.65
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Aghaei Hakkak, R.; Tiritiris, I.; Schleid, T. Synthesis and Characterization of High-Energy Anti-Perovskite Compounds Cs3X[B12H12] Based on Cesium Dodecahydro-Closo-Borate with Molecular Oxoanions (X− = [NO3]−, [ClO3]− and [ClO4]−). Molecules 2024, 29, 382. https://doi.org/10.3390/molecules29020382

AMA Style

Aghaei Hakkak R, Tiritiris I, Schleid T. Synthesis and Characterization of High-Energy Anti-Perovskite Compounds Cs3X[B12H12] Based on Cesium Dodecahydro-Closo-Borate with Molecular Oxoanions (X− = [NO3]−, [ClO3]− and [ClO4]−). Molecules. 2024; 29(2):382. https://doi.org/10.3390/molecules29020382

Chicago/Turabian Style

Aghaei Hakkak, Rouzbeh, Ioannis Tiritiris, and Thomas Schleid. 2024. "Synthesis and Characterization of High-Energy Anti-Perovskite Compounds Cs3X[B12H12] Based on Cesium Dodecahydro-Closo-Borate with Molecular Oxoanions (X− = [NO3]−, [ClO3]− and [ClO4]−)" Molecules 29, no. 2: 382. https://doi.org/10.3390/molecules29020382

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