Open access peer-reviewed chapter

Structural Diversity in Substituted Pyridinium Halocuprates(II)

Written By

Marcus R. Bond

Submitted: 23 July 2022 Reviewed: 16 August 2022 Published: 30 September 2022

DOI: 10.5772/intechopen.107124

From the Edited Volume

Exploring Chemistry with Pyridine Derivatives

Edited by Satyanarayan Pal

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Abstract

The flexible coordination sphere of the Jahn-Teller active Cu(II) ion provides access to a full spectrum of coordination geometries from 4-coordinate (tetrahedral or square planar) to 6-coordinate elongated octahedral. This is further enhanced in anionic halide complexes by the ability of the halide ligand to bridge between Cu(II) centers to generate extended oligomeric or polymeric complexes. Coordination geometry and extended structure of the anionic complex is very sensitive to the nature of the organic counterion. This is especially true for planar substituted pyridinium cations in which minor changes in the nature or position of the substituted group can generate completely different halocuprate(II) structures. Early work focused on reducing ligand-ligand repulsion through strong hydrogen bonding with the organic cation in order to manipulate the Cu(II) coordination sphere. However, many unique structures have been found in which quaternary pyridinium cations were employed-including the remarkable thermochromic compound (1,2,6-trimethylpyridinium)2CuCl4- in which strong hydrogen bonding is absent. More recently aminopyridinium cations, which further increase structural diversity not only through the possibility of having mono- or di-protonated cations but also the ability of monoprotonated cations to coordinate to the Cu(II) center through the amino group, have been investigated.

Keywords

  • substituted pyridinium compounds
  • structural chemistry
  • copper(II) complexes
  • Jahn-Teller effect

1. Introduction

The d9 Cu2+ ion is, perhaps, the best known example of a Jahn-Teller active ion with an extremely flexible coordination sphere—to the extent that it has been referred to as “a chameleon of coordination chemistry” [1]. To summarize standard arguments [2]: in octahedral coordination the degenerate electronic ground state of d9 Cu2+ is further stabilized by distortion (typically by elongation of one octahedral axis) to yield a non-degenerate electronic ground state (Figure 1). (In tetrahedral coordination a flattening distortion toward the square planar limit serves a similar purpose).

Figure 1.

Schematic diagram of the d-orbital splitting of an octahedral CuCl64− complex undergoing an elongated axis Jahn-Teller distortion.

The elongated octahedral geometry can be described as 4 + 2 coordinate with four short coordinate covalent bonds (typical Cu-Cl bond lengths in the 2.2–2.4 Å range) and two longer semicoordinate bonds (typical Cu⋅⋅⋅Cl bond lengths ranging from 2.7 to well over 3 Å). The two semicoordinate bonds can be of different lengths leading to 4 + 1 + 1′ coordination. Further elongation of the longer bond eventually leads (conceptually) to removal of that ligand and results in 4 + 1 coordination. In some situations the semicoordinate bond of a 4 + 1 complex is short enough (Cu-Cl distance of 2.6 Å or less) to become a coordinate bond and yielding a five coordinate geometry that is usually found somewhere on the continuum between trigonal bipyramidal and square pyramidal due to a second order Jahn-Teller distortion [3]. Removal of the other semicoordinate ligand yields a 4-coordinate complex that is usually found in a flattened tetrahedral geometry with trans Cl-Cu-Cl angles between 130 and 140°. However, these angles are found with a range of values, including 180° in the square planar limit. Square planar CuCl42− complexes are rare, and square planar CuBr42− complexes are almost completely unknown—a fact attributed to the stronger ligand-ligand repulsion between the larger bromide ions. Thus a wide range of coordination numbers and geometries is available to a copper(II) complex, as depicted in Figure 2.

Figure 2.

Coordination numbers and geometries available to a Cu2+ complex.

The focus of this chapter is on copper(II) halide complexes—ergo the bond length and angle examples previously given. Chloride complexes have been more thoroughly investigated than bromide complexes [4]. This may be due to the wide variety of colors exhibited by chloride complexes of differing geometries and coordination numbers: ranging from reds to orange to yellow to greens. The author has found in some situations crystals of three or four different colors growing in the same beaker as identifiably distinct compounds. In contrast, the visible spectra of bromide complexes is dominated by ligand-to-metal charge transfer to give an intensely dark purple color with little variation across compounds [5, 6]. In both cases, however, the chloride and bromide ligands can bridge between copper(II) centers, as shown in Figure 3, to increase structural complexity by forming oligomeric or polymeric species.

Figure 3.

Bridging modes available to halocuprate(II) complexes.

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2. The utility of pyridinium cations

2.1 Anionic halocupreates(II)

Halocuprate(II) complexes, whether isolated monocopper(II) or oligomeric or polymeric, are anionic and in crystalline solids are always accompanied by a cationic species. Earliest studied compounds used highly symmetric alkali metal or ammonium cations [7, 8, 9, 10] but a wide variety of conterions have been used, including cationic inorganic or organometallic complexes. A broad array of organic cations, often readily and commercially available, have been most frequently employed [2].

2.2 Structures with organoammonium cations

Organoammonium cations can quickly become bulky with larger groups and higher degrees of substitution which prevents formation of polymeric complexes. Consider, for example, the (Et)x(Me)4−x series of chlorocuprates with an approximate 1:1 ratio of organic cation to CuCl2. For tetramethylammonium (x = 0) a tribridged chain of face sharing CuCl6 octahedra is found in (Me4N)CuCl3 [11]. For x = 1, in EtMe3N)4Cu5Cl14 a linear chain is also found, but with a mix of bi- and tribridging that “stretches” the chain in order to accommodate the bulkier organic cation [12]. For x = 2, a (Cu4Cl113−)n with even more frequent bibridging is found [13]. Organic cations with x = 3 and 4 are so bulky that a continuous chain is no longer possible, and isolated Cu3Cl93− [2, 14] and Cu4Cl124− [15] oligomers are found. Primary alkylammonium cations favor formation of layer perovskite A2CuX4 (A = monopositive cation and X = Cl, Br) compounds in which layers of corner sharing CuX6 octahedra are separated by bilayers of organic cations with NH3 head groups directed toward the inorganic layer to form multiple N-H…X hydrogen bonds [16].

2.3 Structures with anilinium versus structures with pyridinium cations

Substituted planar aromatic cations, i.e. anilinium or pyridinium, provide a wealth of counterion possibilities while avoiding the bulkiness found with organoammonium ions. With a protonated NH3+ head group, an anilinium cation can function structurally as a primary ammonium cation. Indeed, (anilinium)2CuCl4 exists as a layer perovskite system [17]. With pyridinium cations, however, the ring nitrogen acts as a single hydrogen bond donor (when protonated) that generally forms a single direct or a bifurcated hydrogen bond to halide(s) on a neighboring complex. The ring nitrogen can also be readily quaternized to examine halocuprate(II) structures in the absence of N-H hydrogen bonding. Pyridinium compounds have been more heavily studied than anilinium compounds: a Cambridge Structural Database (CSD) substructure search [18] on the anilinium core versus the pyridinium core with tetrachlorocuprate(II) complexes yields 24 compounds (14 of which are layer perovskites) and 120 compounds, respectively. This difference might be due to the tendency for anilinium cations to decompose in the presence of Cu(II) (presumably acting as a one-electron oxidation catalyst). In the author’s experience, crystal growth under ambient conditions of anilinium chlorocuprate(II) compounds often yields brown or black residues. Indeed, there are no reported structures of ring substituted methyl or dimethylanilinium chlrocuprate(II) compounds in the CSD, whereas there are a handful of chlorozincate(II) compounds (where Zn(II) with a d10 configuration does not have access to a + 1 oxidation state) and numerous ring substituted methyl or dimethylpyridinium chlorocuprate(II) compounds.

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3. A2CuX4 compounds containing isolated CuX42− complexes

3.1 General properties

Compounds containing isolated CuX42− complexes are readily prepared by slow evaporation of a solution, e.g. hydrohalic acid or alcoholic, containing a stoichiometric amount of organic cation halide and copper(II) halide, and examples are regularly reported. These most commonly contain flattened tetrahedral complexes with trans X-Cu-X angles in the range 130–140°. Strong hydrogen bonding between the organic cation and the halide ions of the inorganic complex is thought to reduce ligand-ligand repulsion and allow for larger trans X-Cu-X angles. Examples of these complexes are more rare, especially those with larger trans angles, Crystals containing chloro complexes with the commonly found trans angle are yellow/orange in color and become progressively more green in coloras the trans angle increases to reach an intensely dark green color at the square planar limit (180°) [19].

3.2 Square planar complexes

A recent example of square planar CuCl42− is in the isonicotinamidium (H-INAc) salt where strong bifurcated hydrogen bonds from the protonated ring nitrogen stabilize the sp geometry (Figure 4). This particular compound is also interesting since there is a companion compound in which neutral isonicotinamide molecules coordinate to the copper(II) center as terminal ligands in di-μ2-chloro polymeric chains. Exposure of these chains to moist HCl vapor protonates the pyridine and generates the sp complex in a reversible process [20]. In some cases green sp complexes undergo abrupt (green to yellow) thermochromic phase transitions to tet complexes on heating as increased thermal motion weakens the hydrogen bonding that stabilizes the sp geometry [19]. While no such transition is reported for the H-INAc salt, it is possible that heating might result in deprotonation of the pyridine before a transition occurs.

Figure 4.

Ball-and-stick model of the formula unit of bis(isonicotinadium) tetrachlorocuprate(II) showing the strong, bifurcated hydrogen bonds that stabilize the sp geometry.

3.3 Polymorphism and supramolecular interactions

Polymorphic crystalline forms of these systems can be obtained and studied with different polymorphs possible upon crystallization from different solvents or using different methods. An example occurs with 2,6-dimethylpyridinium in which a monoclinic structure (C2/c) is obtained from acidic aqueous solution [21] and an orthorhombic (Pbcn) polymorph is obtained from ethanol [22]. Supramolecular interactions were examined in both polymorphs, which illustrates a common application of A2CuX4 systems. Since they are readily prepared, it is convenient to use them to study supramolecular interactions with variations in pyridinium ring substitution, e.g. a recent study of halogen bonding in (chloromethyl)pyridinium salts [23].

3.4 Catalytic ring substitution

Willett et al. provided a classic series of papers detailing Cu(II) as a catalytically active species in serendipitous ring substitution reactions of pyridines. For example, recrystallization of 2-amino, 3-methylpyridine with CuBr2 in a slightly acidic solution yielded partial bromination of the pyridine to give (2-amino, 5-bromo, 3-methylpyridinium)(2-amino, 3-methylpyridinium) tetrabromocuprate(II) [24]. Likewise, recrystallization of 2,6-diaminopyridine with CuCl2⋅2H2O in slightly acidic solution yields (2,6-diamino, 3,5-dichlropyridinium) tetrachlorocuprate(II) [25] (the bromo analog more recently reported [26]).

3.5 Structural complexity

A2CuX4 systems can also provide examples of structural complexity, e.g. through complex packing arrangements or symmetrically inequivalent CuX42− complexes with different degrees of flattening. Well known older examples, the incommensurate phase of [(CH3)4N]CuCl4 [27] and the thermochromic compound [CH3CH2NH3]2CuCl4 (which contains three distinctly different CuCl42− complexes with one unit cell axis length ~ 45 Å) [28], do not contain pyridinium cations but there are more recent examples that do. The compound [bis(pyridinium-3-ylmethyl)ammonium]4(CuCl4)5Cl2 contains four distinct CuCl42− complexes with trans Cl-Cu-Cl angles ranging from 128 to 155° [29]. The high symmetry compound (1,3,4-trimethylpyridinium)2CuCl4 crystallizes in orthorhombic Fdd2 with complex anions found between layers of organic cations. The diamond glide symmetry generates a four organic cation layer repeat sequence and leads to a ~ 35 Å b-axis length. The corresponding bromide compound is in lower symmetry monoclinic P21/c with symmetrically inequivalent organic cations that are segregated into separate layers, as another form of structural complexity [30].

This Fdd2 structure is found across a range of (1,3,4-trimethylpyridinium)2MCl4 compounds (M = Co, Ni, Zn [31, 32, 33]) but larger metal ions (Mn, Cd [34, 35]) crystallize in monoclinic C2/c. A CSD search shows that C2/c is the second most commonly reported space group for pyridinium A2CuCl4 compounds (~40 structures) and slightly exceeds the number of compounds reported in the most commonly reported space group for all compounds, monoclinic P21/c. (The most commonly reported space group from pyridinium A2CuCl4 structures is triclinic P1¯ with ~60 structures.) Since in the C2/c structure both organic cations are symmetrically equivalent, this suggests a strategy in pursuing structurally complex compounds by mixing different organic cations to give AACuCl4 structures. A few examples are known, such as the 2-amino-3-methylpyridinium example cited above in which organic cations are similar, or the (dimethylammonium)(3,5-dimethylpyridinium)CuCl4 structure [36] where the organic cations are quite different. A systematic study could be conducted by redissolving existing stocks of A2CuCl4 compounds in a 1:1 molar ratio and recrystallizing.

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4. Quasi-planar oligomers

4.1 Overview

Halocuprate(II) complexes can form linear multicopper complexes through edge sharing of neighboring CuX4 complexes. At the simplest level this is a dicopper(II) complex which, with a monopositive organic cation, has the typical formulation A2Cu2X6 for a 1:1 organic cation:Cu(II) stoichiometry More copper rich stoichiometries are needed for longer CunX2n + 22− oligomers. Crystallization of a particular type of oligomer is not predictable, unlike the 2:1 stoichiometry A2CuX4 compounds which are readily formed. Thus it is common when exploring the halocuprate(II) structural landscape to prepare solutions of different stoichiometries, e.g. 2:1, 1:1, and 1:2. The stoichiometry of the crystals obtained from solution is not necessarily the same as starting stoichiometry. These compounds require crystallographic analysis to establish their identities as dissolution destroys the compounds.

4.2 Stacking of quasiplanar oligomers

With bulky organic cations the oligomers are isolated and are formed from edge-sharing CuX4 flattened tetrahedra. For planar or less bulky cations, the oligomers are now quasi planar, formed from edge sharing of CuX4 square planes, and are no longer isolated with halide ions from one oligomer form semicoordinate bonds with Cu(II) centers on neighboring oligomers to aggregate into stacks [4]. Neighboring oligomers are offset from each other by a half-integral multiple of a CuX4 edge length with the pattern simply communicated by a bracketed pair. For example, 2[1/2,1/2] indicates that neighboring dicopper oligomers are offset from one another by ½ an edge length parallel to the long axis of the oligomer and ½ an edge length perpendicular (the 2 in front of the bracket identifies these as dicopper(II) complexes). These stacking patterns vary by compound, and can become more complicated with different oligomers in the stack having different stacking environments [37]. A selection of different oligomer structures with associated stacking patterns are shown in Figure 5.

Figure 5.

(a) 2[1/2,1/2] stacking in (2-amino-4-bromo-3-hydroxopyridinium)2Cu2Br6⋅2H2O (water molecules omitted for clarity) [38], (b) 3[1/2,1/2] stacking in (4-chloropyridinium)2Cu3Cl8 [39], and (c) 4[5/2,1/2] stacking in (1-methylpyridinium)2Cu4Br10 [40].

4.3 Pyridinium cation interactions in oligomer stacking

While many different kinds of cations generate oligomer stacks, distinctions can be observed for pyridinium cations. Where hydrogen bonding is present, the oligomer is often terminated with a bifurcated hydrogen bond which mimics the bibridged structure within the oligomer, as shown in Figure 6.

Figure 6.

Hydrogen bonding scheme in (4,4′-diazenediyldipyridinium) Cu2Cl6 [41].

Oligomer stacks can often be visualized as sections of a layer from the CuX2 parent structure. This is particularly true for situations where hydrogen bonding is not possible and the structures can be described as CuX2 layers in which organic cation pairs replace (CunX2n-2)2+ fragments, as illustrated in Figure 7 for (1-methylpyridiniuim)2Cu4Br10 [40]. In this case the shape of the organic cation may have more to do with templating the inorganic structure rather than directed intermolecular interactions.

Figure 7.

Layer structure of (1-methylpyridinium)2Cu4Br10.

4.4 High-nuclearity oligomers

Oligomers containing more than four Cu(II) centers are rare. Only one example of a Cu5X122− oligomer is known (in 2-chloro-1-methylpyridinium)2Cu5Br10 [40]) in which oligomers are still found in isolated stacks (the neutral pentacopper oligomer Cu5Cl10(n-CH3CH2CH2OH)2 has long been known [42]). 1,2 dimethylpyridinium crystallizes with a hexacopper oligomer (Cu6Cl142−) and a heptacopper oligomer (Cu7Br162−) [43]. For these longer oligomers the stacks are no longer isolated, but overlap one another to form layers with the organic cations sandwiched between layers, as illustrated in Figure 8.

Figure 8.

Overlapping of oligomer stacks to form a layer with one organic cation shown for the compound (1,2-dimethylpyrdinium)2Cu7Br16.

2-Chloro-1-methylpyridinium also crystallizes with a Cu7Br162− oligomer in a structure that is almost identical to that of 1,2-dimethylpyridinium. The chloro and methyl groups are disordered, indicating no directed intermolecular interaction with the oligomer and templating of the oligomer on the cation shape may be more important [40].

The longest reported oligomer is found in (3,5-dibromopyridinium)Cu10Br22. The authors rationalize formation of the decacopper(II) oligiomer in terms of halogen bonding contacts with the organic cation [44]. This laboratory has obtained also a Cu10Br222− for 2,6-dimethylpyridinium shown in Figure 9 [45]. In spite of similarity in shape of the cation and similar unit cell parameters, the two structures are not superimposable. Longer oligomers are certainly possible, but these high copper(II) stoichiometries are rarely investigated so that further discoveries are likely to be serendipitous.

Figure 9.

Thermal ellipsoid plot (at the 50% level) of the formula unit of (2,6-dimethylpyridinium)2Cu10Br22 at 295 K. H-atoms are drawn as circles of arbitrary radii.

4.5 Asymmetrically bridged dicopper(II) oligomers

An exception to the symmetrically bridged oligomers discussed above are situations where two CuX4 square planes stack offset from each other to form long semicoordinate bonds between halide ligands of one complex and the Cu(II) center of the other. This leads to two asymmetric bridges with one short Cu-X bond and one long Cu⋅⋅⋅X bond, as shown in Figure 10. Stacks of CuX4 square planes are not known, but such stacking would lend itself to formation of linear chain structures—which are known.

Figure 10.

Asymmetric dicopper(II) oligomer in 4,4′-((cyclohexane-1,2-diylbis(ammoniumdiyl))bis(methylene))bis(pyridin-1-ium Cu2Cl8⋅H2O [46]. Hydrogen atoms and water molecule are omitted for clarity. Bond distances in the dimer bridge are shown in units of Å.

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5. ACuX3 linear chains

The CsNiCl3 structure consisting of chains of face-sharing NiCl6 octahedra separated by monopositive cations is the parent structure for ACuX3 linear chains. In the parent structure each Ni(II) ion is linked to its neighbor by three symmetric bridges. However, due to the axial Jahn-Teller distortion of the CuCl6 octahedron, in ACuX3 chains each Cu(II) is linked to its neighbor by two asymmetric bridges and only one symmetric bridge. In the absence of hydrogen bonding interactions from the counterion, in the case of Cs, (CH3)4N+, or the quaternary4-methyl-1-(4′-nitrobenzyl)-4-methylpyridinium (shown in Figure 11a [47]) cations, the tribridged chain is observed. Hydrogen bonding from the cation to the halides of the chain provides charge compensation to the halides that permits lengthening of the Jahn-Teller elongated Cu-Cl bond. For strong enough hydrogen bonding the semicoordinate bond is broken and the chain is converted into a symmetrically bibridged chain of CuCl5 square pyramids. This is illustrated by the (cyclohexylammonium)CuCl3 structure where hydrogen bonding from the ammonium head group leads to elongation of the Jahn-Teller axial bond to a distance of 3.48 Å (as compared to elongated distances of 2.76 and 2.96 Å in the chain shown in 11(a)). At this distance the chloride ligand is, at best, weakly interacting with the neighboring Cu(II) center and a nascent CuCl5 square pyramid has formed with two symmetric bridges now connecting Cu(II) centers with the apical Cu-Cl bond still canted at an acute angle relative to the chain axis (see Figure 11b [48]). In 2-amino-6-methylpyridinium CuCl3 both the pyridine nitrogen and amino group serve as hydrogen bond donors forming multiple hydrogen bonds to the apical chloride and providing sufficient charge compensation that the apical Cu-Cl bond is perpendicular to the chain axis and no longer involved in bridging (see Figure 11c [49]).

Figure 11.

(a) The tribridged chain in 1-(4′-nitrobenzyl)-4-methylpyridinium CuCl3, (b) the bibridged chain in cyclohexylammonium CuCl3 showing the ammonium head group in postion to hydrogen bond to canted apical chloride ligands, and (c) the bibridged chain in 2-amino-6-methylpyridinium CuCl3 showing hydrogen bonds from the pyridine and amino N atoms that stabilize the apical chloride ligand as non-bridging.

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6. Quaternary pyridinium cations

6.1 Overview

While hydrogen bonding has traditionally been seen as a means to control halocuprate(II) geometry, quaternary pyridinium cations provide a means of examining the effect of a lack of N-H hydrogen bonding on structure. Common methods used (in this laboratory) for preparation of quaternary pyridinium cations are (1) reaction of a substituted pyridine with an excess of iodomethane, then anion exchange with an excess of the appropriate silver halide in H2O or (2) direct combination of condensed chloro- or bromomethane (in excess) with chilled substituted pyridine in a pressure vessel that is then sealed and allowed to warm to room temperature for 24 hr. Examples of structures containing quaternary pyridinium cations have been mentioned in passing already. Here two particularly interesting systems are discussed.

6.2 “Knobby” chains in (1,4-dimethylpyridinium)4Cu5Cl14

The quaternary 1,4-dimethylpyridinium cation might be expected to crystallize with a tribridged (CuCl3)n chain due to the lack of hydrogen bonding—just as the quaternary cation example cited in the previous section and as is, notably, the case for (1,4-dimethylyrdinium) PbBr3 [50]. Instead it templates a highly unusual (Cu5Cl14)n “knobby” chains in which CuCl4 flattened tetrahedral “knobs” edge-share so as to bridge adjacent Cu(II) ions in the central chain [12]. The chain structure is distinctive since it exhibits the three major coordination numbers of Cu(II). Besides the flattened tetrahedral “knobs” on the outside of the chain, the central Cu(II) ion of the Cu5Cl14 repeat unit has the elongated octahedral 4 + 2 coordination. This bibridges on either side to 5-coordinated Cu(II) complexes with the intermediate sqp/tbp geometry. These 5-coordinate complexes then bibridge to 5-coordinate complexes on neighboring Cu5Cl14 units to complete the chain (Figure 12). With the lack of directed intermolecular interactions, the inorganic structure must template on the cation shape, although it is difficult to discern specifically the driving force behind formation of the structure. The knobs on the chain are found between stacks of organic cations with bridging chlorides close to the pyridinium N atoms as the most prominent point of interaction. There has been no reported attempt to prepare the bromide analog.

Figure 12.

A section of the “knobby” chains found for (1,4-dimethylpyridinium)Cu5Cl15.

6.3 sp to tet phase transitions in (1,2,6-trimethylpyridinium)2CuX4

The second interesting case is the (1,2,6-trimethylpyridinium)2CuX4 system [51]. Both the chloride and the bromide salts contain square planar CuX42− in a low temperature phase (below 60°C for the chloride and below −48°C for the bromide). Both compounds undergo a solid-solid phase transition on heating to a high temperature phase in which CuX42− is flattened tetrahedral, resulting in a thermochromic transition for the chloride salt (from dark green to yellow). As previously described, these sp to tet transitions are thought to occur due to a weakening of hydrogen bonding. Furthermore sp CuBr42− is not expected, even with strong hydrogen bonding, due to the greater ligand-ligand repulsion of the larger bromide. So the occurrence of sp complexes and sp to tet transitions in systems without strong hydrogen bonding is highly unusual, if not unprecedented. (It is also worth mentioning that the transitions go from higher symmetry (monoclinic C2/m) to lower symmetry (triclinic P1¯), which is also quite unusual.)

The quaternary ammonium cations in the low temperature structures form zipper-like ribbons with sp CuCl42− complexes between the ribbons, as shown in Figure 13, that act to template the sp geometry. Crystallographic mirror planes are perpendicular to this layer and bisect both the organic cation and the CuCl42− complex. The three dimensional structure is built up by stacking these layers so that organic cations of one layer sit above or below CuCl42− complexes in another so that the complexes are truly isolated. The structural transformation that occurs on heating disrupts this ribbon structure and results in two symmetrically inequivalent organic cations with aromatic planes tilted with respect to each other.

Figure 13.

Layer structure of (1,2,6-trimethylpyridinium)2CuCl4 showing the zipper-like ribbons of organic cations with methyl groups directed toward the center of the ribbon and with isolated sp CuCl42− between the ribbons. Mirror plane symmetry is perpendicular to the layer and bisects the organic cations and CuCl42− complexes.

The 1,2,3-trimethylpyridinium cation has a similar shape as 1,2,6-trimethylpyridinium, and also crystallizes as zipper-like ribbons with chlorocuprate(II) complexes between the ribbons to from layers. However the complexes formed are not isolated CuCl42− but asymmetrically bridged [CuCl3(H2O)]2 dicopper complexes [52]. Figure 14 illustrates the similar layer structure, right down to similar symmetry: monoclinic C2/m. As before, the mirror plane is perpendicular to the layer and bisects the organic cation. In this case, however, the N-atom lies off the mirror plane resulting in two-fold positional disorder that is not present in the 1,2,6-trimethylpyridinium analog. Does positional disorder stabilize a different structure? That is a difficult question to answer. Nevertheless, the sp CuX4 complex appears to be inaccessible with the 1,2,3-trimethylpyridinium cation. While (1,2,3-trimethylpyridinium)2CuBr4 is known, it is a conventional flattened tetrahedral complex that is isostructural to (1,2,3-trimethylpyridinium)2CoCl4 (both in monoclinic C2/c). Preliminary work from this laboratory indicates that mixed crystals of (1,2,6-trimethylpyridinium)x(1,2,3-trimethylpyridinium)2−xCuCl4 do contain sp complexes in a situation where positional disorder is reduced [53]. In any case, these two examples indicate how minor changes in cation can produce major differences in halocuprate(II) structure. It would be interesting to study structures produced by the shape-similar 2,3,4- and 3,4,5-trimethylpyridinium cations which would now also introduce N-H hydrogen bonding interactions. Since these pyridines are not commercially available, a collaboration with a synthetic organic chemist is underway to prepare them.

Figure 14.

Layer structure in (1,2,3-trimethylpyridinium) CuCl3(H2O) showing the zipper-like ribbons of organic cations separating inorganic complexes. Another layer stacks with offset inorganic complexes to form asymmetrically bridged dimers. Mirror plane symmetry is perpendicular to the layer and bisects the organic cations and the inorganic complex to produce two-fold positional disorder of the organic cation.

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7. Systems with 3-aminopyridines

Aminopyridines of various types have been prominent in the preparation of halocuprate(II) compounds, with some examples cited already. 3-Aminopyridines, in contrast to 2- or 4-aminooyridines, are capable of protonating both the pyridine and amino N-atoms. Typically the pyridine N-atom protonates first, and if a monoprotonated cation is desired care must be taken to crystallize compounds from solutions that are weakly acidic to avoid diprotonation. At the same time, the monoprotonated cation is capable of coordinating Cu(II) through the amino N-atom—which enables even further structural diversity. Willett et al. reported the earliest compounds with 3-aminopyridine and copper(II) halides. The 3-ammoniumpyridinium cation is found in CuX4 layer perovskite structures for both the chloride and bromide by virtue of the NH3 head group [54]. Other reported compounds have coordinated 3-aminopyridinium ligands: a symmetrically and asymmetrically bridged dicopper(II) complex for the chloride and the bromide (as a monohydrate in the latter case), respectively, as shown in Figure 15 [55].

Figure 15.

(a) The symmetrically bridged [CuCl3(3-aminopyridinium]2 dicopper complex and, (b) the asymmetrically bridged [CuBr3(3-aminopyridinium)]2 dicopper(II) complex as a monohydrate.

A structure for (3-aminopyridinium)2CuCl4 has been reported as a typical compound containing flattened tetrahedral CuCl42−. This reported structure, however, is almost identical to that of (2-aminopyridinium)2CuCl4, in both unit cell constants and atom positions, and is, in all likelihood, misreported [56]. In order to check this structure, this laboratory undertook crystal growth from acidic aqueous solution and managed to obtain crystals of (3-aminopyridinium)2CuCl4 by means that can only be described as serendipitous. These crystals gave completely different unit cell constants than the, likely, misreported structure.

In an effort to rationally synthesize crystals of this compound, crystals were grown from various organic solvents (1-proponal, acetonitrile, and tetrahydrofuran) by a thermal gradient technique in sealed, screwcap test tubes placed in a heater block with wells maintained at 40°C. Green crystals of (3-ammoniumpyridinium)CuCl4 were loaded into individual test tubes containing each organic solvent and crystal growth commenced. Another portion of these green crystals were ground together with a stoichiometric amount of 3-aminopyridine and a red-orange solid obtained. Portions of this solid were similarly loaded for crystal growth.

Two new compounds (Figure 16) have been obtained in crystal growth from 1-proponal: (1) green crystals of an asymmetrically bridged dicopper complex isomeric to the symmetrically bridged dimer reported by Willett el al.; and (2) red crystals of a monocopper complex with a coordinated 3-aminopyridinium ligand and a 3-aminopyridinium lattice cation. The latter compound, [3-aminopyridinium][(3-aminopyridinium)tetrachlorocuprate(II)], is identical in formulation to (3-aminopyridinium)2CuCl4 but with one organic cation moved to the inner coordination sphere. (Crystal growth from acetonitrile yields the known compounds (3-ammoniumpyridinium)CuCl4 and (3-aminopyridinium)2CuCl4) [57]. So far five different compounds have been obtained from the 3-aminopyridine:CuCl2 system just by varying crystal growth conditions. Studies are underway to investigate compounds of the corresponding bromides and of substituted 3-aminopyridines such as 3-amino-2-methylpyridine.

Figure 16.

Thermal ellipsoid plots of (a) the asymmetrically bridged dicopper(II) complex [CuCl3(3-aminopyridine]2 and (b) the formula unit of (3-aminopyridinium) [CuCl4(3-aminopyridinium)].

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8. Conclusion

The use of pyridinium cations as counterions for halocuprate(II) complexes has provided a wealth of unusual structures due, in part, to the thin profile of the cation, the variety of possible substituent groups, and the easy ability to form a quaternary cation. Previous work has relied heavily on pyridines that are commercially available, but future advances may greatly benefit from targeted pursuit of synthetically prepared pyridines. Mixed cation structures, particularly of A2CuX4 systems, have been rarely studied and offer the potential for discovery of new compounds with structural complexity. Different crystallization conditions and solvents have been used in the past to prepare different polymorphs, but now find use in preparation of diverse 3-aminopyridinium halocuprate(II) compounds. While pyridinium halocuprate(II) compounds have been widely studied and dispayed an amazing range of structural diversity, recent discoveries show that they still have the capacity to surprise.

Notes

Structure graphics software used

Ball-and-stick diagrams were plotted using Mercury 4.0 [58]. Thermal ellipsoid plots were drawn using ORTEP-3 for Windows [59].

Crystal data for (2,6-dimethylpyridinium)2Cu10Br22

Triclinic, P1¯, 295 K, a = 9.4862(5) Å, b = 10.0507(5) Å, c = 13.0217(5) Å, α = 104.108(3)°, β = 90.442(3)°, γ = 92.708(3)°, V = 1202.5(1) Å3, Z = 2. Reflections total/observed = 10,393/3691. θ(max) = 35.139°. Number of least squares parameters = 218. Rovserved = 0.0926, wRobserved = 0.2117, goodness of fit = 1.001, Δρ(max/min) = 2.181/−2.585 e3.

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Written By

Marcus R. Bond

Submitted: 23 July 2022 Reviewed: 16 August 2022 Published: 30 September 2022