Next Article in Journal
Chemical/Instrumental Approaches to the Evaluation of Wine Chemistry
Next Article in Special Issue
Exploring the Polymorphism of Drostanolone Propionate
Previous Article in Journal
Analytical Technology in Nutrition Analysis
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Molecules
Volume 25
Issue 6
10.3390/molecules25061361
molecules-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles thumb_up
...
Endorse textsms
...
Comment
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Isostructural Inorganic–Organic Piperazine-1,4-diium Chlorido- and Bromidoantimonate(III) Monohydrates: Octahedral Distortions and Hydrogen Bonds

by
Maciej Bujak
* and
Dawid Siodłak
Faculty of Chemistry, University of Opole, Oleska 48, 45-052 Opole, Poland
*
Author to whom correspondence should be addressed.
Molecules 2020, 25(6), 1361; https://doi.org/10.3390/molecules25061361
Submission received: 27 February 2020 / Revised: 11 March 2020 / Accepted: 13 March 2020 / Published: 17 March 2020
(This article belongs to the Special Issue Non-Covalent Interaction in Solids and Large Clusters)
Browse Figures
Versions Notes

Abstract

:
Halogenidoantimonate(III) monohydrates of the (C4H12N2)[SbX5]·H2O (X = Cl, 1 or Br, 2) formula, crystallizing in the same monoclinic space group of P21/n, are isostructural, with an isostructurality index close to 99%. The single crystal X-ray diffraction data do not show any indication of phase transition in cooling these crystals from room temperature to 85 K. Both hybrid crystals are built up from [SbX6]3– octahedra that are joined together by a common edge forming isolated bioctahedral [Sb2X10]4– units, piperazine-1,4-diium (C4H12N2)2+ cations and water of crystallization molecules. These structural components are joined together by related but somewhat different O/N/C–H···X and N–H···O hydrogen bonded systems. The evolution of structural parameters, notably the secondary Sb–X bonds along with the associated X/Sb–Sb/X–X/Sb angles and O/N/C–H···X hydrogen bonds, as a function of ligand exchange and temperature, along with their influence on the irregularity of [SbX6]3– octahedra, was determined. The comparison of packing features and hydrogen bond parameters, additionally supported by the Hirshfeld surface analysis and data retrieved from the Cambridge Structural Database, demonstrates the hierarchy and importance of hydrogen bond interactions that influence the irregularity of single [SbX6]3– units.

Graphical Abstract

1. Introduction

The crystal structures of mixed inorganic–organic halogenidoantimonates(III) with organic cations are mainly based upon [SbX6]3– and [SbX5]2– polyhedra (X = Cl, Br or/and I) forming various types of inorganic substructures, and organic cations that are located between and/or within inorganic frameworks [1,2,3,4]. The isolated as well as involved in more complicated [SbX6]3–, and [SbX5]2– units are usually distorted from regularity showing differences in their Sb–X bond lengths and X–Sb–X angles. The distortions are a consequence of the presence of the 5s2 lone electron pair of the SbIII atom [5,6,7] and can be described in terms of the valence shell electron pair repulsion (VSEPR) model that is supplemented by the ligand close packing (LCP) model [8,9] and further supported by the electronic distortion approach [10,11]. It was also found that the geometrical irregularities of antimony(III) polyhedra are related to interactions of these single inorganic units with both inorganic and organic components of the structure: (i) inorganic polyhedra may be joined together by bridging X atoms forming polyhedral infinitive or isolated units—primary deformation and (ii) organic cations may be hydrogen bonded to halogen ligands, changing their geometry relative to the central SbIII atom—secondary deformation [12,13,14,15].
Halogenidoantimonates(III) as the perovskite-like hybrid materials are also of interest because of their physicochemical properties such as luminescent, thermochromic and ferroic, particularly since they can be modified relatively easily by the replacement of halogen or organic structural components [3,16,17,18,19,20,21]. However, it is noteworthy that the ferroic properties, in these compounds, have been limited to particular chemical stoichiometries, e.g., R3Sb2X9 (R—organic cation) [3,18,22,23,24,25,26,27,28,29].
Recently, the structures along with the molecular motions study of two piperazine-1,4-diium halogenidoantimonate(III) monohydrates, (C4H12N2)[SbCl5]·H2O (1) and (C4H12N2)[SbBr5]·H2O (2), were reported. In addition, the phase transition behavior of both compounds was investigated [30,31].
We found that the isostructural crystals of 1 and 2 could serve as a convenient system for investigating the structural consequences of the effect of halogen exchange on the polyhedral distortion in the group of antimony(III) compounds, because of their close relationship and simple inorganic substructure. The introduction into the structure of 2 the heavier, more polarizable and less electronegative Br compared to Cl atoms, opens the possibility of the formation of weaker organic–inorganic N/C–H···X hydrogen bonds and thus weakens the secondary octahedral distortion factor. Further, the piperazine-1,4-diium cations due to their tendency to formation of hydrogen bonds and the relatively large spatial dimensions that create a pattern with appropriate cavities for inclusion of water of crystallization molecules [32,33] provide an opportunity to explore the occurrence, hierarchy and competition of N/C–H···X and O–H···X hydrogen bonds on the distortions of inorganic polyhedra. Moreover, the temperature effect, using the same single crystal samples in order to rationalize the contribution of different factors on the structural changes of crystals of 1 and 2, was studied.

2. Results and Discussion

2.1. Structures of 1 and 2

The title monohydrates of piperazine-1,4-diium pentachloridoantimonate(III) and pentabromidoantimonate(III) were found to be isostructural—they crystallize in the same monoclinic system with the P21/n space group and they are characterized by similar unit–cell parameters. Moreover, the positions of corresponding atoms and the crystal packing of both 1 and 2 are similar too (Table 1, Figure 1). The close relationship of these crystals is demonstrated by the calculated unit–cell identity parameters Π of 0.0294 and 0.0313 for the structures determined at 295 and 85 K, respectively, as well as by the very close to 100%, average for 295 and 85 K, isostructurality indexes of 98.8% [34,35,36].
It is also interesting to note that both crystals 1 and 2 show a similar degree of contraction with decreasing temperature from 295 to 85 K. All the a, b and c unit–cell parameters decrease, whereas the monoclinic β angles slightly increase. As a result, the unit–cell volumes at 85 K are 2.8% and 2.3% less than those at 295 K for 1 and 2, respectively. The structural relationship between 1 and 2 is also manifested in somewhat analogous patterns of voids (the empty spaces in a crystal structure) [37], however the smaller volume of the free spaces and related higher density for 2 should be noted (Table 1, Figure 1).
In both crystals, consisting of the same and fully ordered components, the simple inorganic [Sb2X10]4– units and organic cations (C4H12N2)2+ that are joined together by N/C–H···X hydrogen bonds were found. In addition, the water of crystallization molecules participates in the hydrogen bonded systems, competing for the same X acceptors, through the O–H···X interactions and also as the acceptors for N–H···O hydrogen bonds. Furthermore, the O···O contacts joining the water of crystallization molecules, with an average distance of ca. 2.94 Å, were found. It is noteworthy that the central SbIII atoms occupy general positions and therefore their coordination geometries are not constrained by symmetry. Consequently, the structural changes, induced by halogen atom replacement as well as those occurring by decreasing temperature, are associated with the particular properties of inorganic/organic substructures and changes in the non-covalent interactions. The single crystal X-ray diffraction data do not show any indication of phase transition/symmetry change, in the temperature range 295 to 85 K. This makes it possible to follow continuous changes in the interatomic parameters including those for non-covalent interactions. It was found that temperature does not significantly affect the bond lengths and angles of the organic cations, but it influences the inorganic substructures and the hydrogen bond interactions.
There is one SbIII atom that is surrounded by five X atoms, one piperazine-1,4-diium cation and one water of crystallization molecule in the asymmetric unit of both 1 and 2. The inorganic substructures are built up from [SbX6]3– octahedra connected by one edge forming bioctahedral isolated [Sb2X10]4– units. Therefore, in the coordination sphere of the central SbIII, two X atoms are bridging and four are terminal. At 295 K the shortest are two Sb1–X1/X3 terminal bond lengths, while the longest are located trans to them Sb1–X2I/X2 bridging distances. The third pairs of Sb–X involving two terminal mutually trans Sb1–X4/X5 bonds have intermediate lengths. The X–Sb–X angles for X atoms that are located cis to each another clearly deviate from the ideal 90°. In contrast to cis, the trans X–Sb–X angles are somewhat closer to an ideal 180° and are more similar to each other for both crystals (Table 2). The interoctahedral X–Sb–X angles were found to be one of the smallest (82.247(14)° for 1 and 87.723(11)° for 2) for both studied halogenidoantimonates(III) and other crystals possessing the [Sb2X10]4– bioctahedral units [37,38,39].
At 85 K, the Sb–X terminal distances involving X1, X3 and X4 are elongated, whereas the longest—both bridging Sb1–X2/X2I, as well as terminal Sb1—X5 are shortened in comparison to the corresponding parameters determined at room temperature. The largest changes were noted for bridging Sb1–X2 bonds that are shortened by 0.0237(7) and 0.0210(6) for 1 and 2, respectively. The X–Sb–X angles are also both smaller and larger than at 295 K. The largest average change of 1.19° of increase and decrease, respectively, with a decreasing temperature was found for the X2–Sb1–X2I and Sb1–X2–Sb1I angles involving the bridging X atoms (Table 2).
The geometry of the bioctahedral [Sb2X10]4– anions described above in 1 and 2 is comparable to that seen for the same units in other compounds [20,30,31,40]. Moreover, the geometrical parameters of the piperazine-1,4-diium cations in both crystals, adopting the energetically preferred chair conformation [41,42], are consistent with those reported for the structure of piperazine and other analogous compounds containing this cation [30,31,32,43,44,45,46,47,48].

2.2. Octahedral Distortions in 1 and 2

The detailed analysis of the first and the second coordination sphere of the basic inorganic [SbX6]3– octahedra and their centrosymmetric bioctahedral [Sb2X10]4– units together with the environment of organic piperazine-1,4-diium cations in 1 and 2 clarifies the understanding of the interactions in the studied crystals. Furthermore, the comparison to analogous halogenidoantimonates(III) reveals the hierarchy of interactions and elucidate the changes that occur with decreasing temperature and the halogen atom replacement.
As mentioned above, the distortion of polyhedra in the halogenidoantimonate(III) crystals is associated with the presence of the 5s2 lone electron pair of the SbIII atom and is considered to be a non-bonding effect that occurs for the post-transition metal compounds, in which the central metal shows an oxidation state of two lower than that one resulting from its periodic table group number. It was also found that the elongation of Sb–X bonds is consistent with the structural trans effect [14,49,50,51,52] and is associated with the shortening of oppositely located Sb–X distances.
The comparison of Sb–X bond lengths as well as X–Sb–X angles in 1 and 2 with corresponding geometrical parameters found for the ‘non-distorted’ isolated octahedra (in which all X atoms are engaged in hydrogen bonds) [SbCl6]3– [53] and [SbBr6]3– [54] demonstrates that the distortion of the single [SbX6]3– units is mainly associated with the primary distortion factor, i.e., is the consequence of the formation of [Sb2X10]4– units. Clearly, while all the Sb–Cl bonds in the ‘non-distorted’ [SbCl6]3– octahedron are 2.6552(4) Å [53] the average Sb–Cl distance, in 1, is 2.7159 and 2.7123 Å at 295 and 85 K, respectively. Only the average bond length of the two terminal trans located ligands of 2.6298 Å at 295 K and the corresponding, slightly shorter distance of 2.6259 Å at 85 K were found to be comparable to the reference distance. A similar behavior is observed for 2. The similar average Sb–Br distances of two oppositely located terminal bonds are 2.7890 and 2.7889 Å at 295 and 85 K, respectively, and they were found to be the closest to the reference 2.8022(5) Å distance of the ‘non-distorted’ [SbBr6]3– octahedron [54]. The cis X–Sb–X angles, in the case of 1 and 2 at 295 and 85 K, for both bridging X atoms are clearly above 90° (average of ca. 96°), whereas the average values of the remaining angles are close to the ideal 90°. The trans angles (average of ca. 176°) also deviate from 180°, whereas the average interoctahedral Sb–X–Sb angle of ca. 84° is evidently smaller than the theoretically expected 90° (Table 2).
The less pronounced secondary distortion results from the differences in geometry and strength of the hydrogen bond interactions between [Sb2X10]4– units and their environment. The hydrogen bonded to the [Sb2X10]4– units through N/C–H···X and O–H···X piperazine-1,4-diium cations and water of crystallization molecules, respectively, participate in the distortion of octahedral SbIII coordination, both in terms of differences between equivalent Sb–X bond lengths and X–Sb–X angles. The influence of these non-covalent interactions is seen in the geometrical parameters involving the longest Sb–X distances (Table 2 and Table 3, Figure 2). Comparing Sb–X bond lengths to X4 and X5, which are neither bridging nor opposite to bridging, we found a difference of ca. 0.2 Å for both 1 and 2, that implies the shift of the electron cloud in the direction of X5. This inequality can be explained by the presence of relatively strong hydrogen bonds in which X5, in contrast to X4, is involved.
The largest change in the D···A distances with cooling was found for O1–H12···X3 interactions that are shortened by 0.063(3) and 0.072(4) Å for 1 and 2, respectively. The shortening is associated with the elongation of the Sb1–X3 distances by 0.0090(7) for 1 and 0.0157(6) Å for 2. At the same time, in line with the structural trans effect, the largest shortening with decreasing temperature (by 0.0237(7) and 0.0210(6) Å for 1 and 2, respectively) was found for the oppositely located Sb1–X2 distances. It is also of interest to note that with a temperature decrease of 210 K, a decreasing of Sb1···Sb1I distances and interoctahedral Sb1–X2–Sb1I angles that are in relation to shortening of N–H···X2 hydrogen bonds is observed (Table 2 and Table 3, Figure 2).
The preferences for the formation of hydrogen bonds to the specific X atoms correspond well to the calculations of apparent residual δ charge carried by a particular halogen atom, which is related to the sum of the bond order n, in which the atom is involved (δ = –(1 – Σn); D(n) = 2.32 – 1.00 log n for 1 and D(n) = 2.46 – 1.10 log n for 2, D(n)—observed bond length) [55,56]. These calculations show that the largest negative residual charges were found for the longest bridging X2 and X2I as well as for the terminal X5 atoms that are all involved in the N/O–H···X hydrogen bonds belonging to the strongest interactions in the studied 1 and 2 (Table 2, Table 3 and Table 4, Figure 2).
The irregularity of [SbX6]3– octahedra can be also described by the bond length Δ ( Δ = 1 6 ∑ i = 1 6 [ ( R i − R ¯ ) / R ¯ ] 2 , R ¯ —average Sb–X bond length within the octahedron and Ri —individual Sb–X bond length of the octahedron) and the bond angle σ2 ( σ 2 = 1 11 ∑ i = 1 12 ( α i − 90 ) 2 , αi—individual cis-X–Sb–X bond angle of the octahedron) distortion parameters [57,58]. The distortion parameters for 1 and 2 at 295 and 85 K are displayed in Table 5.
By analysing the Δ and σ2 parameters, it is clear that in the case of 1 the distortion is revealed by both the bond length and the bond angle parameters. In the case of 2, both the Δ and σ2 are lower, confirming the less distorted [SbX6]3– units in the crystal. Such behavior corresponding to the energy requirements (i.e., it is easier to move the Cl atoms and change the Sb–Cl and Cl–Sb–Cl parameters than the heavier Br atoms) is further confirmed by the distortion parameters found for the isolated [SbX6]3– octahedra [15,53,54,59,60,61]. The observation, in both 1 and 2, that the linear distortions of the [SbX6]3– octahedra decrease and at the same time the angular distortions increase with decreasing temperature, is related to the strengthening of hydrogen bond interactions with decreasing temperature. Furthermore, the changes in bond angles with retaining the bond distances are energetically preferred than the elongation of bond distances for the asymmetrically distributed non-bonding interactions.
To further demonstrate, as well as compare and understand the influence of non-covalent interactions, the Hirshfeld surface analysis for 1 and 2 was carried out [62,63,64,65] (Figure 2b and Figure 3). The analysis highlights and additionally proves the aforementioned observations, i.e., there are some slight differences in the O/N/C–H···X hydrogen bonds in 1 and 2 which reflects the strength of the interactions in which the different acceptors of Cl and Br atoms are engaged.

3. Materials and Methods

3.1. Preparation of 1 and 2

The commercially available antimony(III) chloride, SbCl3 (>99%), antimony(III) oxide, Sb2O3 (pure), piperazine anhydrous, C4H10N2 (for synthesis), hydrochloric acid, HCl (35%–38%, pure p. a.) and hydrobromic acid, HBr (ACS reagent, 48%) was used, without further purification, for the synthesis and crystallization of (C4H12N2)[SbCl5]·H2O (1) and (C4H12N2)[SbBr5]·H2O (2).
1 and 2 were prepared according to a general, previously reported procedure, but the preheated and diluted HCl/HBr acids were used [3,14,30,31]. The molar ratio of starting materials, for both 1 and 2, was 1:2. C4H10N2 was dissolved in HCl/HBr acid and the resulting solution was used to treat SbCl3 and Sb2O3 solutions in HCl and HBr for 1 and 2, respectively. The appeared precipitates, in both cases, were dissolved by further addition of the minimum amount of HCl or HBr, stirring and heating up to ca. 325 K. Then the solutions were allowed to stand in a desiccator (P4O10 was used as a desiccant), at room temperature, forming the single crystals suitable for the X-ray diffraction studies.

3.2. X-ray Structure Determination

The intensity data for both 1 and 2, at 295(2) and 85.0(5) K, were collected on an Xcalibur single crystal diffractometer that was equipped with an Oxford Cryosystems cooler. All the data were subjected to Lorentz, polarization and analytical absorption corrections. The Oxford Diffraction CrysAlis CCD and CrysAlisPro programs were used during the data collection, cell refinement and data reduction [66,67]. SHELX software was used for the structure solutions and refinements [68,69]. The crystal structures were solved by the Patterson method. All hydrogen atoms were located in the subsequent difference Fourier maps, refined restraining to the similar distances (DFIX command of SHELXL [68,69]) for the >CH2, >NH2 and –OH groups. The hydrogen atom displacement parameters were taken with a coefficient 1.2 and 1.5 times larger than the respective parameters of the carrier carbon/nitrogen and oxygen atoms, respectively. The asymmetric units of the unit cells and the labelling schemes of atoms for both 1 and 2 at 295(2) and 85.0(5) K were chosen to show the structural relationship between the positions of corresponding atoms.
The room-temperature structure of 1 and the structure of 2 at 80(2) K was reported by Sghaier et al. and by Moskwa et al., respectively [30,31], but the low-temperature structure of 1 and room-temperature structure of 2 have not been investigated yet. The present results are basically consistent with the previous reports, Table 1 and Table 2 (cf. Tables S1 and S2), but to avoid biases in the analysis of the structural parameters resulting from comparison of the crystal data obtained for different crystal samples using different instruments, only the data presented in this paper are discussed. Furthermore, in contrast to previous studies, we were able to refine the hydrogen atom positions and discuss, in detail, the octahedral distortions along with the importance of hydrogen bond interactions. Table 3, for the sake of comparison, presents the same set of interactions for 1 and 2 at both the studied temperatures of 295(2) and 85.0(5) K.
The structure drawings were prepared using Mercury [37]. The results of the X-ray diffraction studies were further supported by the Hirshfeld surface analysis provided by CrystalExplorer 2.0 [62,63,64,65] along with the analysis of the data retrieved from the Cambridge Structural Database [37,38,39].

4. Conclusions

The structural chemistry of halogenidoantimonates(III) and other technologically important materials, in which central metals show lower oxidation states, is quite intriguing, since the presence of the lone electron pair affects the different degrees of distorted polyhedral coordination. Thus, it is not easy to find the perfectly non-distorted square pyramid or octahedron in the whole group of these compounds. Furthermore, the geometrical parameters within the inorganic substructures of halogenidoantimonates(III) are crucial for their properties, e.g., the Sb–Br bond length variances within [Sb2Br10]4– influence the thermochromic changes of (C16H20N2)[SbBr5] [20].
Two isostructural piperazine-1,4-diium halogenidoantimonate(III) monohydrates (C4H12N2)[SbX5]·H2O (X = Cl, 1 or Br, 2) were obtained, in a similar way, from its acidic HCl and HBr solutions, respectively. Both crystals are characterized by an inorganic substructure that is built up from isolated [Sb2X10]4– bioctahedra, as well as organic piperazine-1,4-diium cations and water of crystallization molecules. It was demonstrated that when two [SbX6]3– octahedra are joined together by a common edge forming [Sb2X10]4– units, the Sb–X bonds show different lengths and the X–Sb–X angles deviate from the ideal 90° and 180°. These deviations are associated with the requirements of the inorganic substructure formation as well as with the strength and distribution of non-covalent interactions.
No phase transition was detected, in both 1 and 2, within the studied temperature range, i.e., upon cooling from 295 to 85 K. This allows us to monitor the changes occurring, particularly in the case of the longest secondary Sb–X bonds and associated X–Sb–X angles as well as rationalizing the contribution of the hydrogen bonds to the distortion of inorganic polyhedra.
Both studied halogenidoantimonates(III) show unique structural behavior represented by evidently small X–Sb–X interoctahedral angles and related short Sb···Sb separation distances. These parameters are associated with relatively long Sb–X bridging distances and also with the hydrogen bond interactions, in which the bridging X atoms are involved. Such behavior demonstrates the stereochemical activity of the antimony(III) lone electron pair as well as the attractive character of hydrogen bond interactions. The Cl by Br replacement results in less distorted octahedra with regard to bond lengths and bond angles, whereas decreasing temperature leads to the more pronounced changes of bond angles than bond lengths. This could be explained in terms of the size and polarizability of halogen atoms and the energy required to move the X atoms along the Sb–X bonds.

Supplementary Materials

Supplementary Materials are available online. Tables S1 and S2. The set of supplementary crystallographic data for 1 and 2, at both 295(2) and 85.0(5) K, in the CIF format, is available from the Cambridge Crystallographic Data Centre nos. CCDC 1957876–1957879. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html, or from the Cambridge Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: +44 1223 336 033; e-mail: [email protected] or http://www.ccdc.cam.ac.uk.

Author Contributions

Conceptualization, M.B.; Methodology, M.B. and D.S.; Formal Analysis, M.B.; Investigation, D.S. (crystallization) and M.B.; Writing-Original Draft Preparation, M.B.; Writing-Review and Editing, M.B. and D.S.; Visualization, M.B. Both authors have read and agreed to the published version of the manuscript.

Funding

This research received no external funding.

Acknowledgments

The authors are grateful to A. Niemira and M. Bulanda for the preliminary studies of 1 and 2, respectively.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Fischer, G.A.; Norman, N.C. The structures of the group 15 element(III) halides and halogenoanions. Adv. Inorg. Chem. 1994, 41, 233–271. [Google Scholar]
  2. Sobczyk, L.; Jakubas, R.; Zaleski, J. Self-Assembly of Sb(III) and Bi(III) Halo-Coordinated Octahedra in Salts of Organic Cations. Structure, Properties and Phase Transitions. Pol. J. Chem. 1997, 71, 265–330. [Google Scholar]
  3. Bujak, M.; Zaleski, J. Synthesis of chloroantimonates(III) with selected organic cations. X-ray studies of phase transition in ferroelectric tris(trimethylammonium) nonachlorodiantimonate(III) at 125 K. J. Solid State Chem. 2004, 177, 3202–3211. [Google Scholar] [CrossRef]
  4. Rhaiem, T.B.; Elleuch, S.; Boughzala, H.; Abid, Y. Synthesis, crystal structure, vibrational and optical properties of chlorometalate hybrids incorporating (DABCOH2)2+ cations. Inorg. Chem. Commun. 2019, 105, 230–239. [Google Scholar] [CrossRef]
  5. Olivier-Fourcade, J.; Lbanez, A.; Jumas, J.C.; Maurin, M.; Lefebvre, I.; Lippens, P.; Lannoo, M.; Allan, G. Chemical Bonding and Electronic Properties in Antimony Chalcogenides. J. Solid State Chem. 1990, 87, 366–377. [Google Scholar] [CrossRef]
  6. Wang, X.; Liebau, F. Influence of polyhedron distortions on calculated bond-valence sums for cations with one lone electron pair. Acta Crystallogr. B 2007, 63, 216–228. [Google Scholar] [CrossRef]
  7. Wheeler, R.A.; Kumar, P.N.V.P. Stereochemically Active or Inactive Lone Pair Electrons in Some Six-Coordinate, Group 15 Halides. J. Am. Chem. Soc. 1992, 114, 4776–4784. [Google Scholar] [CrossRef]
  8. Gillespie, R.J.; Nyholm, R.S. Inorganic stereochemistry. Q. Rev. Chem. Soc. 1957, 11, 339–380. [Google Scholar] [CrossRef]
  9. Gillespie, R.J. Fifty years of the VSEPR model. Coord. Chem. Rev. 2008, 252, 1315–1327. [Google Scholar] [CrossRef]
  10. Brown, I.D. The Chemical Bond in Inorganic Chemistry: The Bond Valence Model; Oxford University Press: New York, NY, USA, 2002; pp. 90–98. [Google Scholar]
  11. Brown, I.D. Recent Developments in the Methods and Applications of the Bond Valence Model. Chem. Rev. 2009, 109, 6858–6919. [Google Scholar] [CrossRef] [Green Version]
  12. Bujak, M.; Zaleski, J. Dependence of the Distortion of the Square Pyramids in N,N-Dimethylethylenediammonium Pentachloroantimonate(III) on the Geometry of Hydrogen Bonds. Z. Naturforsch. 2001, 56, 521–525. [Google Scholar] [CrossRef]
  13. Bujak, M.; Osadczuk, P.; Zaleski, J. Aminoguanidinium(2+) aminoguanidinium(1+) hexachloroantimonate(III) at 295 and 92 K. Acta Crystallogr. C 2001, 57, 388–391. [Google Scholar] [CrossRef] [PubMed]
  14. Bujak, M. Primary- and secondary-octahedral distortion factors in bis(1,4-H2-1,2,4-triazolium) pentabromidoantimonate(III)–1,4-H2-1,2,4-triazolium bromide. Polyhedron 2015, 85, 499–505. [Google Scholar] [CrossRef]
  15. Bujak, M. Formation and distortion of iodidoantimonates(III): The first isolated [SbI6]3– octahedron. Acta Crystallogr. B 2017, 73, 432–442. [Google Scholar] [CrossRef] [PubMed]
  16. Bator, G.; Jakubas, R.; Zaleski, J.; Mróz, J. Crystal structure and dielectric relaxation studies of the [N(CH3)3H]3Sb2(1–x)Bi2xCl9 mixed crystals. J. Appl. Phys. 2000, 88, 1015–1023. [Google Scholar] [CrossRef]
  17. Wojtaś, M.; Bator, G.; Jakubas, R.; Zaleski, J. Crystal structure, phase transition and ferroelectric properties of the [(CH3)3NH]3[Sb2Cl9(1−x)Br9x] (TMACBA) mixed crystals. J. Phys. Condens. Matter 2003, 15, 5765–5781. [Google Scholar] [CrossRef]
  18. Bujak, M.; Angel, R.J. Single crystal X-ray diffraction studies on [(CH3)nNH4–n]3[Sb2Cl9] (n = 2, 3) chloroantimonates(III) in their low-temperature ferroelectric phases—structures and phase transitions. J. Solid State Chem. 2005, 178, 2237–2246. [Google Scholar] [CrossRef]
  19. Saparov, B.; Mitzi, D.B. Organic−Inorganic Perovskites: Structural Versatility for Functional Materials Design. Chem. Rev. 2016, 116, 4558–4596. [Google Scholar] [CrossRef]
  20. Zhang, W.; Sun, Z.; Zhang, J.; Han, S.; Ji, C.; Li, L.; Hong, M.; Luo, J. Thermochromism to tune the optical bandgap of a lead-free perovskite-type hybrid semiconductor for efficiently enhancing photocurrent generation. J. Mater. Chem. C 2017, 5, 9967–9971. [Google Scholar] [CrossRef]
  21. Wang, Z.; Zhang, Z.; Tao, L.; Shen, N.; Hu, B.; Gong, L.; Li, J.; Chen, X.; Huang, X. Hybrid Chloroantimonates(III): Thermally Induced Triple-Mode Reversible Luminescent Switching and Laser-Printable Rewritable Luminescent Paper. Angew. Chem. Int. Ed. 2019, 58, 9974–9978. [Google Scholar] [CrossRef]
  22. Jakubas, R. Ferroelectric phase transition in tris(dimethylammonium) nonachlorodiantimonate (III), [NH2(CH3)2]3Sb2Cl9. Solid State Commun. 1986, 60, 389–391. [Google Scholar] [CrossRef]
  23. Gdaniec, M.; Kostrukiewicz, Z.; Jakubas, R.; Sobczyk, L. Structure and mechanism of ferroelectric phase transition in tris(dimethylammonium) nonachlorodiantimonate (III). Ferroelectrics 1988, 77, 31–37. [Google Scholar] [CrossRef]
  24. Zaleski, J.; Pietraszko, A. Structure at 200 and 298 K and X-ray Investigations of the Phase Transition at 242 K of [NH2(CH3)2]3Sb2Cl9 (DMACA). Acta Crystallogr. B 1996, 52, 287–295. [Google Scholar] [CrossRef]
  25. Jakubas, R.; Czapla, Z.; Galewski, Z.; Sobczyk, L. Ferroelectric phase transition in [(CH3)3NH]3Sb2Cl9 (TMACA). Ferroelectr. Lett. 1986, 5, 143–148. [Google Scholar] [CrossRef]
  26. Kruger, F.-J.; Zettler, F.; Schmidt, A. Tri- und TetraMethylammonium-chloroantimonate(III). Z. Anorg. Allg. Chem. 1979, 449, 135–144. [Google Scholar] [CrossRef]
  27. Kallel, A.; Bats, J.W. Tris(trimethylammonium) Nonachlorodiantimonate(III), [NH(CH3)3]3[Sb2Cl9]. Acta Crystallogr. C 1985, 41, 1022–1024. [Google Scholar] [CrossRef]
  28. Tomaszewski, P.E. X-ray study of ferroelectric phase transition in (NH(CH3)3)3Sb2Cl9. Acta Phys. Pol. A 1995, 87, 631–634. [Google Scholar] [CrossRef]
  29. Bujak, M.; Zaleski, J. High temperature ferro-paraelectric phase transition in tris(trimethylammonium) nonachlorodiantimonate(III) (TMACA) studied by X-ray diffraction method. Cryst. Eng. 2001, 4, 241–252. [Google Scholar] [CrossRef]
  30. Sghaier, M.O.M.; Holderna-Natkaniec, K.; Czarnecki, P.; Wozniak-Braszak, A.; Chaabouni, S. Structure and internal dynamics of bis(piperazine-1,4-diium) pentachloroantimonate (III) monohydrate. Polyhedron 2014, 79, 37–42. [Google Scholar] [CrossRef]
  31. Moskwa, M.; Bator, G.; Piecha-Bisiorek, A.; Jakubas, R.; Medycki, W.; Ciżman, A.; Baran, J. X-ray structure and investigation of molecular motions by dielectric, vibrational and 1H NMR methods for two organic-inorganic hybrid piperazinium compounds: (C4H12N2)2[Sb2Cl10]·2H2O and (C4H12N2)2[Sb2Br10]·2H2O. Mater. Res. Bull. 2018, 104, 202–211. [Google Scholar] [CrossRef]
  32. Bujak, M. Efficient Diffusion-Controlled Ligand Exchange Crystal Growth of Isostructural Inorganic−Organic Halogenidorhodates(III): The Missing Hexaiodidorhodate(III) Anion. Cryst. Growth Des. 2015, 15, 1295–1302. [Google Scholar] [CrossRef]
  33. Bajpai, A.; Scott, H.S.; Pham, T.; Chen, K.-J.; Space, B.; Lusi, M.; Perry, M.L.; Zaworotko, M.J. Towards an understanding of the propensity for crystalline hydrate formation by molecular compounds. IUCrJ 2016, 3, 430–439. [Google Scholar] [CrossRef]
  34. Kálmán, A.; Argay, G.; Scharfenberg-Pfeiffer, D.; Höhne, E.; Ribár, B. ‘Main-Part’ Isostructuralism of Several Cardenolides and Bufadienolides. Structures of Three Cardenolides: (21S)-Methyldigitoxigenin, Uzarigenin and Sarmentogenin Methanol Solvate. Acta Crystallogr. B 1991, 47, 68–77. [Google Scholar] [CrossRef]
  35. Fábián, L.; Kálmán, A. Volumetric measure of isostructurality. Acta Crystallogr. B 1999, 55, 1099–1108. [Google Scholar] [CrossRef]
  36. Kubicki, M.; Szafrański, M. Hydrogen bonding in two isomorphous bis-guanidinium salts: Tetrachlorozincate(II) and tetrabromozincate(II). J. Mol. Struct. 1998, 446, 1–9. [Google Scholar] [CrossRef]
  37. Macrae, C.F.; Bruno, I.J.; Chisholm, J.A.; Edgington, P.R.; McCabe, P.; Pidcock, E.; Rodriguez-Monge, L.; Taylor, R.; van de Streek, J.; Wood, P.A. Mercury CSD 2.0—New features for the visualization and investigation of crystal structures. J. Appl. Crystallogr. 2008, 41, 466–470. [Google Scholar] [CrossRef]
  38. Bruno, I.J.; Cole, J.C.; Edgington, P.R.; Kessler, M.; Macrae, C.F.; McCabe, P.; Pearson, J.; Taylor, R. New software for searching the Cambridge Structural Database and visualizing crystal structures. Acta Crystallogr. B 2002, 58, 389–397. [Google Scholar] [CrossRef] [PubMed]
  39. Groom, C.R.; Bruno, I.J.; Lightfoot, M.P.; Ward, S.C. The Cambridge Structural Database. Acta Crystallogr. B 2016, 72, 171–179. [Google Scholar] [CrossRef] [PubMed]
  40. Bujak, M.; Zaleski, J. The Crystal Structure of Bis(ethylammonium) Pentachloroantimonate(III)-ethylammonium Chloride (C2H5NH3)2SbCl5·(C2H5NH3)Cl at 295 and 90 K. On the Deformation of the Octahedral Coordination of SbIII. Pol. J. Chem. 1999, 73, 773–782. [Google Scholar]
  41. Harris, R.K.; Spragg, R.A. Nuclear Magnetic Resonance Studies of Six-membered Rings. Part I. Ring Inversion in Heterocyclic Compounds. J. Chem. Soc. B 1968, 684–691. [Google Scholar] [CrossRef]
  42. Krueger, P.J.; Jan, J. Conformational equilibria in some cyclic imines: NH and CH stretching vibrations and the axial lone pair. Can. J. Chem. 1970, 48, 3236–3248. [Google Scholar] [CrossRef]
  43. Parkin, A.; Oswald, I.D.H.; Parsons, S. Structures of piperazine, piperidine and morpholine. Acta Crystallogr. B 2004, 60, 219–227. [Google Scholar] [CrossRef] [PubMed]
  44. Rérat, C. Structure Cristalline du Bichlorhydrate de Pipérazine Monohydraté. Acta Crystallogr. 1960, 13, 459–468. [Google Scholar] [CrossRef]
  45. Dehghanpour, S.; Mahmoudkhani, A.H.; Langer, V. Redetermination of piperazine dihydrochloride monohydrate. Acta Crystallogr. E 2001, 57, o610–o611. [Google Scholar] [CrossRef]
  46. Baisch, U.; Rubini, K.; Braga, D. Remarkable structural similarities between organic co-crystals and a metal–organic coordination network—insights into hydrogen bonded aliphatic ammonium chlorides. CrystEngComm 2008, 10, 1939–1947. [Google Scholar] [CrossRef]
  47. Reiss, G.J.; Bajorat, S. CSD Communication (Private Communication, CCDC 769156, Refcode: UJONEN); The Cambridge Crystallographic Data Centre: Cambridge, UK, 2010. [Google Scholar]
  48. Flatken, M.A.; Huber, M.J.; Reiss, G.J. The layered crystal structure of piperazine-1,4-diium diiodide–diiodine (1:1), C4H12I4N2. Z. Kristallogr. NCS 2014, 229, 423–424. [Google Scholar] [CrossRef]
  49. Landrum, G.A.; Hoffmann, R. Secondary Bonding between Chalcogens or Pnicogens and Halogens. Angew. Chem. Int. Ed. 1998, 37, 1887–1890. [Google Scholar] [CrossRef]
  50. Anderson, K.M.; Orpen, A.G. On the relative magnitudes of cis and trans influences in metal complexes. Chem. Commun. 2001, 2682–2683. [Google Scholar] [CrossRef]
  51. Bujak, M.; Zaleski, J. Crystal and Molecular Structure of 1,2,4-Triazolium Chloride and its Salt with Antimony Trichloride-Bis(1,2,4-triazolium) pentachloroantimonate(III)-1,2,4-triazolium Chloride. Z. Naturforsch. 2002, 57, 157–164. [Google Scholar] [CrossRef]
  52. Sheu, H.-L.; Laane, J. Trans. Effect in Halobismuthates and Haloantimonates Revisited. Molecular Structures and Vibrations from Theoretical Calculations. Inorg. Chem. 2013, 52, 4244–4249. [Google Scholar] [CrossRef]
  53. Podesta, T.J.; Orpen, A.G. Tris(Pyridinium)Triazine in Crystal Synthesis of 3-Fold Symmetric Structures. Cryst. Growth Des. 2005, 5, 681–693. [Google Scholar] [CrossRef]
  54. Mirochnik, A.G.; Udovenko, A.A.; Storozhuk, T.V.; Karasev, V.E.; Bukvetskii, B.V. Synthesis and Luminescence of Arsenic(III) and Antimony(III) Halide Complexes with N,N’-Diphenylguanidine. Crystal Structures of Tris(N,N’-diphenylguanidinium) Hexachloro- and Hexabromoarsenates(III) and -Antimonates(III). Russ. J. Inorg. Chem. 2003, 48, 961–971. [Google Scholar]
  55. Pauling, L. The Nature of the Chemical Bond, 3rd ed.; Cornell University Press: Ithaca, NY, USA, 1960; pp. 255–256. [Google Scholar]
  56. Hall, M.; Nunn, M.; Beglev, M.J.; Sowerby, D.B. Nonahalogenodiantimon(III)ates; Their Preparation and the Crystal Structures of [Hpy]3[Sb2Cl9], [NMe4]3[Sb2Br9], and [NMe4]3[Sb2Br3Cl6]. J. Chem. Soc. Dalton Trans. 1986, 1231–1238. [Google Scholar] [CrossRef]
  57. Robinson, K.; Gibbs, G.V.; Ribbe, P.H. Quadratic Elongation: A Quantitative Measure of Distortion in Coordination Polyhedra. Science 1971, 172, 567–570. [Google Scholar] [CrossRef] [PubMed]
  58. Brown, I.D.; Shannon, R.D. Empirical Bond-Strength-Bond-Length Curves for Oxides. Acta Crystallogr. A 1973, 29, 266–282. [Google Scholar] [CrossRef]
  59. Vezzosi, I.M.; Battaglia, L.P.; Corradi, A.B. The Crystal and Molecular Structure of Diethylenetriammonium Hexachloroantimonate(III). Inorg. Chim. Acta 1984, 89, 151–155. [Google Scholar] [CrossRef]
  60. Knödler, F.; Ensinger, U.; Schwarz, W.; Schmidt, A. Dimethylammonium-chloroantimonate. Struktur und Schwingungsspektren. Z. Anorg. Allg. Chem. 1988, 557, 208–218. [Google Scholar] [CrossRef]
  61. Piecha, A.; Gągor, A.; Pietraszko, A.; Jakubas, R. Unprecedented solid-state chemical reaction—from (C3N2H5)3SbBr6·H2O to (C3N2H5)5Sb2Br11. From centrosymmetric to non-centrosymmetric crystal structure. J. Solid State Chem. 2010, 183, 3058–3066. [Google Scholar] [CrossRef]
  62. Wolff, S.K.; Grimwood, D.J.; McKinnon, J.J.; Jayatilaka, D.; Spackman, M.A. CrystalExplorer 2.0.; University of Western Australia: Perth, Australia, 2007. [Google Scholar]
  63. McKinnon, J.J.; Spackman, M.A.; Mitchell, A.S. Novel tools for visualizing and exploring intermolecular interactions in molecular crystals. Acta Crystallogr. B 2004, 60, 627–668. [Google Scholar] [CrossRef]
  64. Spackman, M.A.; McKinnon, J.J.; Jayatilaka, D. Electrostatic potentials mapped on Hirshfeld surfaces provide direct insight into intermolecular interactions in crystals. CrystEngComm 2008, 10, 377–388. [Google Scholar] [CrossRef]
  65. Spackman, M.A.; Jayatilaka, D. Hirshfeld surface analysis. CrystEngComm 2009, 11, 19–32. [Google Scholar] [CrossRef]
  66. CrysAlis CCD, Version 171.33.57; Oxford Diffraction Ltd.: Yarnton, UK, 2010.
  67. CrysAlisPro, Version 1.171.39.15e; Rigaku Oxford Diffraction, Rigaku Corporation: The Woodlands, TX, USA, 2015.
  68. Sheldrick, G.M. A short history of SHELX. Acta Crystallogr. A 2008, 64, 112–122. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  69. Sheldrick, G.M. Crystal structure refinement with SHELXL. Acta Crystallogr. C 2015, 71, 3–8. [Google Scholar] [CrossRef] [PubMed]
Sample Availability: Samples of the compounds are not available from the authors.
Molecules 25 01361 g001 550
Figure 1. Packing diagrams of 1 (a) and 2 (b), along the c-axes, at 85 K. The intermolecular space accessible to the probing sphere of radius 0.70 Å and the grid spacing of 0.58 Å is indicated in yellow. The void volume is: 1.3%, 16.66 Å3 and 0.5%, 7.85 Å3 for 1 and 2, respectively.
Figure 1. Packing diagrams of 1 (a) and 2 (b), along the c-axes, at 85 K. The intermolecular space accessible to the probing sphere of radius 0.70 Å and the grid spacing of 0.58 Å is indicated in yellow. The void volume is: 1.3%, 16.66 Å3 and 0.5%, 7.85 Å3 for 1 and 2, respectively.
Molecules 25 01361 g001
Molecules 25 01361 g002 550
Figure 2. The N/O–H···Cl hydrogen bonds represented by the broken red lines to Cl2 and Cl5 atoms (a) along with the corresponding Hirshfeld surface mapped with dnorm for the [Sb2Cl10]4− bioctahedral unit (b) in 1 at 85 K. The overlapping surfaces are marked in red, touching in white, whereas separated in navy blue (b). Symmetry codes: (I) –x + 1, –y + 1, –z; (II) x – 1/2, –y + 3/2, z – 1/2; (III) x – 1/2, –y + 1/2, z – 1/2; (IV) –x + 1/2, y – 1/2, –z + 1/2.
Figure 2. The N/O–H···Cl hydrogen bonds represented by the broken red lines to Cl2 and Cl5 atoms (a) along with the corresponding Hirshfeld surface mapped with dnorm for the [Sb2Cl10]4− bioctahedral unit (b) in 1 at 85 K. The overlapping surfaces are marked in red, touching in white, whereas separated in navy blue (b). Symmetry codes: (I) –x + 1, –y + 1, –z; (II) x – 1/2, –y + 3/2, z – 1/2; (III) x – 1/2, –y + 1/2, z – 1/2; (IV) –x + 1/2, y – 1/2, –z + 1/2.
Molecules 25 01361 g002
Molecules 25 01361 g003 550
Figure 3. Hirshfeld surfaces mapped with dnorm for the piperazine-1,4-diium cations in 1 and 2 at 295 (a,c) and 85 K (b,d), respectively. The overlapping surfaces are marked in red, touching in white, whereas separated in navy blue.
Figure 3. Hirshfeld surfaces mapped with dnorm for the piperazine-1,4-diium cations in 1 and 2 at 295 (a,c) and 85 K (b,d), respectively. The overlapping surfaces are marked in red, touching in white, whereas separated in navy blue.
Molecules 25 01361 g003
Table
Table 1. Selected crystal data for 1 and 2 at 295 and 85 K.
Table 1. Selected crystal data for 1 and 2 at 295 and 85 K.
Compound1122
T (K)295(2)85.0(5)295(2)85.0(5)
FormulaC4H14Cl5N2OSbC4H14Cl5N2OSbC4H14Br5N2OSbC4H14Br5N2OSb
Mr405.18405.18627.43627.43
Crystal systemmonoclinicmonoclinicmonoclinicmonoclinic
Space group, ZP21/n, 4P21/n, 4P21/n, 4P21/n, 4
a (Å)9.54078(13)9.45434(13)9.9162(3)9.82225(15)
b (Å)14.14260(19)14.05399(19)14.4090(4)14.34740(19)
c (Å)10.03963(14)9.91376(13)10.3898(3)10.29729(16)
β (°)99.1119(13)99.2085(13)99.432(3)99.7664(15)
V (Å3)1337.57(3)1300.28(3)1464.45(7)1430.10(4)
ρcalc (g/cm3)2.0122.0702.8462.914
R1, I > 2σ(I)0.02120.01400.02520.0183
wR2, all data0.05250.03270.05000.0368
Table
Table 2. Selected bond lengths (Å) and angles (°) for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
Table 2. Selected bond lengths (Å) and angles (°) for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
Compound1122
T (K)2958529585
Sb1–X12.3914(5)2.3936(4)2.5687(5)2.5732(3)
Sb1–X22.9705(6)2.9468(4)3.0884(5)3.0674(3)
Sb1–X2I3.2308(6)3.2291(4)3.2537(5)3.2528(3)
Sb1–X32.4433(6)2.4523(4)2.6090(5)2.6247(3)
Sb1–X42.5246(6)2.5247(4)2.7049(5)2.7080(3)
Sb1–X52.7350(6)2.7270(4)2.8731(5)2.8697(3)
Sb1···Sb1I4.0832(2)4.0099(2)4.3962(5)4.3428(3)
X1–Sb1–X285.66(2)85.073(12)87.479(14)87.133(9)
X1–Sb1–X2I175.28(2)174.247(12)176.077(16)175.030(11)
X1–Sb1–X391.13(3)91.066(14)92.652(17)92.467(11)
X1–Sb1–X490.50(2)90.290(13)91.154(15)91.122(10)
X1–Sb1–X585.66(2)84.948(12)86.920(14)86.227(10)
X2–Sb1–X2I97.753(14)99.165(9)92.277(11)93.245(8)
X2–Sb1–X3176.70(2)176.075(12)177.960(15)177.964(11)
X2–Sb1–X489.783(15)89.840(11)90.061(12)90.183(9)
X2–Sb1–X589.695(15)89.388(10)87.614(12)87.392(8)
X2I–Sb1–X385.42(2)84.640(12)87.453(14)86.981(9)
X2I–Sb1–X492.771(17)93.596(11)92.762(12)93.832(9)
X2I–Sb1–X591.083(15)91.180(10)89.157(12)88.839(8)
X3–Sb1–X490.981(18)90.886(12)91.971(14)91.820(10)
X3–Sb1–X589.329(18)89.570(12)90.360(14)90.591(10)
X4–Sb1–X5176.147(17)175.224(12)177.043(13)176.492(10)
Sb1–X2–Sb1I82.247(14)80.835(9)87.723(11)86.755(8)
Symmetry code: (I) –x + 1, –y + 1, –z.
Table
Table 3. Hydrogen bonds geometries (Å, °) for 1 and 2 at 295 and 85 K.
Table 3. Hydrogen bonds geometries (Å, °) for 1 and 2 at 295 and 85 K.
AtomsD–HH∙∙∙AD∙∙∙AD–H∙∙∙A
1, 295 K
O1–H11···Cl1I0.85(1)2.95(3)3.449(2)119(3)
O1–H12···Cl30.85(1)2.71(3)3.414(3)140(4)
O1–H11···Cl5II0.85(1)2.70(2)3.399(3)141(3)
N11–H112···Cl20.89(1)2.35(2)3.201(2)163(2)
N11–H111···Cl5III0.89(1)2.76(2)3.3444(19)125(2)
N12–H122···Cl2IV0.90(1)2.38(2)3.256(2)165(2)
N12–H121···Cl5V0.89(1)2.51(2)3.2606(19)143(2)
C13–H132···Cl40.96(1)2.90(2)3.555(2)126(2)
C14–H141···Cl3V0.97(1)2.79(2)3.659(2)150(2)
C14–H142···Cl3VI0.96(1)2.84(2)3.675(3)146(2)
N11–H111···O1VII0.89(1)2.19(2)2.943(3)143(2)
1, 85 K
O1–H11···Cl1I0.85(1)2.80(2)3.4198(14)131(2)
O1–H12···Cl30.85(1)2.57(1)3.3512(15)155(2)
O1–H11···Cl5II0.85(1)2.67(2)3.3493(14)138(2)
N11–H112···Cl20.89(1)2.34(1)3.1859(14)160(2)
N11–H111···Cl5III0.90(1)2.76(2)3.3024(14)121(1)
N12–H122···Cl2IV0.90(1)2.38(1)3.2316(14)158(2)
N12–H121···Cl5V0.89(1)2.49(1)3.2287(13)140(2)
C13–H132···Cl40.96(1)2.86(2)3.5277(15)128(1)
C14–H141···Cl3V0.96(1)2.77(1)3.6256(16)148(1)
C14–H142···Cl3VI0.96(1)2.80(1)3.6358(16)145(1)
N11–H111···O1VII0.90(1)2.09(1)2.8926(19)148(2)
2, 295 K
O1–H11···Br1I0.85(1)2.92(3)3.592(4)137(4)
O1–H12···Br30.85(1)2.67(2)3.505(4)169(4)
O1–H11···Br5II0.85(1)3.07(2)3.543(4)117(2)
N11–H112···Br20.90(1)2.56(2)3.374(4)151(3)
N11–H111···Br5III0.90(1)2.90(3)3.480(3)124(3)
N12–H122···Br2IV0.90(1)2.61(2)3.473(3)159(3)
N12–H121···Br5V0.90(1)2.78(3)3.441(3)132(3)
C13–H132···Br40.97(1)2.94(3)3.685(4)134(3)
C14–H141···Br3V0.97(1)2.87(2)3.779(4)157(3)
C14–H142···Br3VI0.97(1)2.95(2)3.787(4)146(3)
N11–H111···O1VII0.90(1)2.17(3)2.939(5)142(3)
2, 85 K
O1–H11···Br1I0.85(1)2.93(2)3.551(2)132(3)
O1–H12···Br30.85(1)2.61(2)3.433(2)165(4)
O1–H11···Br5II0.85(1)2.99(2)3.502(3)121(2)
N11–H112···Br20.90(1)2.51(2)3.358(2)157(3)
N11–H111···Br5III0.90(1)2.96(3)3.443(2)115(2)
N12–H122···Br2IV0.91(1)2.58(2)3.437(2)158(3)
N12–H121···Br5V0.90(1)2.75(2)3.410(2)131(2)
C13–H132···Br40.98(1)2.93(2)3.657(3)133(2)
C14–H141···Br3V0.97(1)2.87(2)3.746(3)152(2)
C14–H142···Br3VI0.97(1)2.92(2)3.743(3)143(2)
N11–H111···O1VII0.90(1)2.08(2)2.896(3)151(3)
Symmetry codes: (I) –x + 1/2, y – 1/2, –z + 1/2; (II) x + 1/2, –y + 1/2, z + 1/2; (III) –x + 1, –y + 1, –z; (IV) x + 1/2, –y + 3/2, z + 1/2; (V) –x + 1/2, y + 1/2, –z + 1/2; (VI) –x + 1, –y + 1, –z + 1; (VII) –x + 3/2, y + 1/2, –z + 1/2.
Table
Table 4. Residual δ charges on the X atoms for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
Table 4. Residual δ charges on the X atoms for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
Compound1122
Atoms/T (K)2958529585
X1–0.15–0.16–0.20–0.21
X2–0.65–0.64–0.54–0.53
X2I–0.65–0.64–0.54–0.53
X3–0.25–0.26–0.27–0.29
X4–0.38–0.38–0.40–0.40
X5–0.62–0.61–0.58–0.58
Symmetry code: (I) –x + 1, –y + 1, –z.
Table
Table 5. Distortion Δ and σ2 parameters for [SbX6]3– octahedra for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
Table 5. Distortion Δ and σ2 parameters for [SbX6]3– octahedra for 1 (X = Cl) and 2 (X = Br) at 295 and 85 K.
ParameterBond Length Distortion, Δ × 103Bond Angle Distortion, σ2
Compound/T (K)2958529585
112.3511.9311.8816.31
27.777.344.906.91

Share and Cite

MDPI and ACS Style

Bujak, M.; Siodłak, D. Isostructural Inorganic–Organic Piperazine-1,4-diium Chlorido- and Bromidoantimonate(III) Monohydrates: Octahedral Distortions and Hydrogen Bonds. Molecules 2020, 25, 1361. https://doi.org/10.3390/molecules25061361

AMA Style

Bujak M, Siodłak D. Isostructural Inorganic–Organic Piperazine-1,4-diium Chlorido- and Bromidoantimonate(III) Monohydrates: Octahedral Distortions and Hydrogen Bonds. Molecules. 2020; 25(6):1361. https://doi.org/10.3390/molecules25061361

Chicago/Turabian Style

Bujak, Maciej, and Dawid Siodłak. 2020. "Isostructural Inorganic–Organic Piperazine-1,4-diium Chlorido- and Bromidoantimonate(III) Monohydrates: Octahedral Distortions and Hydrogen Bonds" Molecules 25, no. 6: 1361. https://doi.org/10.3390/molecules25061361

APA Style

Bujak, M., & Siodłak, D. (2020). Isostructural Inorganic–Organic Piperazine-1,4-diium Chlorido- and Bromidoantimonate(III) Monohydrates: Octahedral Distortions and Hydrogen Bonds. Molecules, 25(6), 1361. https://doi.org/10.3390/molecules25061361

Article Metrics

Back to TopTop