A New Approach to the Synthesis of Nanocrystalline Cobalt Boride in the Course of the Thermal Decomposition of Cobalt Complexes [Co(DMF)6]2+ with Boron Cluster Anions

In the course of the study, nanocrystalline cobalt monoboride was prepared by thermal decomposition of precursors [Co(DMF)6][An], where [An] = [B12H12]2− (1), [trans-B20H18]2− (2) or [B10Cl10]2− (3) in an argon atmosphere. Three new salt-like compounds 1–3 were prepared when Co(NO3)2 was allowed to react with (Et3NH)2[An]. Compound 1 is new; the structures of compounds 2 and 3 have been previously reported. Samples 1–3 were annealed at 900 °C in argon to form samples 1a–3a, which were characterized by single crystal XRD for 1 and powder XRD for 1–3. Powder XRD on the products showed the formation of BN and CoB for 1a in a 1:1 ratio; 2a gave a higher CoB:BN ratio but an overall decreased crystallinity. For 3a, only CoB was found. IR spectra of samples 1a–3a as well as X-ray spectral fluorescence analysis for 3a confirmed these results. The nanoparticular character of the decomposition products 1a–3a was shown using TEM; quite small particle sizes of about 10–15 nm and a quite normal size distribution were found for 1a and 2a, while the decomposition of 3 gave large particles with 200–350 nm and a broad distribution.


Introduction
The preparation of high purity nanocrystalline metal borides has attracted the attention of many material chemists due to the remarkable physicochemical properties of these compounds, such as high strength, refractoriness, resistance to oxidation, corrosion, wear, etc. [1][2][3][4]. Cobalt borides are compounds with the general formula Co x B y ; two main representatives are CoB and Co 2 B. It is known that cobalt(II) borides exhibit excellent catalytic activity in the production of hydrogen [5][6][7][8][9] and oxygen [7,[10][11][12][13], in the liquid phase hydrogenation of citral [14,15], and can be used as anode materials in batteries [16,17].
To date, transition metal borides are obtained, as a rule, in the form of amorphous powders, which can lead to the presence of impurities and defects in the final material. Among the known methods for the preparation of nanoparticles of cobalt(II) borides Co x B, the most common is the chemical reduction of cobalt(II) chloride with alkali metal tetrahydroborate [5,9,13,[17][18][19][20]. In addition, cobalt(II) borides Co 2 B, CoB can be prepared by the interaction of cobalt(II) chloride or metal with elemental boron [21]. Moreover, preparation of mesoporous nanocrystalline α-CoB x was synthesized by chemical reduction of cobalt acetate with dimethylamine borane [20].
One of the possible ways to stabilize nanoparticles is the use of cages capable of encapsulating metal borides. In particular, a framework of hexagonal boron nitride is capable of encapsulating cobalt borides [10,22,23]. One of the possible ways to obtain metal boride nanoparticles in a similar way is based on the use of thermal plasma [24]. It should be noted that this method is a multi-stage process and requires high costs, both economic

Synthesis of Precursors [Co(DMF) 6 ][An]
In this work, we used cobalt(II) complexes with coordinated molecules of N,Ndimethylformamide, which are easily evaporating groups, as precursors [Co(DMF) 6 ][An]. The starting complexes were obtained by reacting cobalt(II) nitrate with the corresponding triethylammonium salts of boron cluster anions in DMF; the final compounds precipitated from the reaction mixture as purple crystals (Scheme 1).
Molecules 2023, 28 The coordinated state of DMF molecules by the oxygen atom of the carbonyl gro is evidenced by the shift of band ν(C=O) (1651, 1664, and 1652 cm -1 in the IR spectra o 2•3H2O and 3, respectively) into a lower frequency interval compared to that in the sp trum of free DMF (ν(C=O) is 1679 cm -1 ). It should be noted that the IR spectrum of 2•3H contains ν(OH) at about 3425 cm -1 , which is characteristic of associated water molecu The resulting compounds 1, 2·3H 2 O, and 3 were identified by elemental analysis, IR spectroscopy, and X-ray diffraction. The structures of [Co(DMF) 6 ][B 10 Cl 10 ] (1) [37] and [Co(DMF) 6 ][B 20 H 18 ] (2) [38] are known: water-free compound 2 was obtained when anhydrous CoCl 2 was allowed to react with [B 20 H 18 ] 2− ; for 1 and 3, water-free samples were isolated when using cobalt nitrate crystal hydrate. The structure of [Co(DMF) 6 ][B 12 H 12 ] (1) was determined by X-ray diffraction in this paper.
The IR spectra of 1 and 2·3H 2 O contain an intense absorption band in the region of 2550-2400 cm −1 , which is related to ν(BH) of the boron cluster anions [B 12 (Figures S1a,b). In the IR spectrum of 3, bands ν(BCl) are observed at 1157, 1002 cm −1 ; a band of stretching and bending vibrations of the B-B groups in boron cage is observed near 843 cm −1 ( Figure S1c).
The coordinated state of DMF molecules by the oxygen atom of the carbonyl group is evidenced by the shift of band ν(C=O) (1651, 1664, and 1652 cm −1 in the IR spectra of 1, 2·3H 2 O and 3, respectively) into a lower frequency interval compared to that in the spectrum of free DMF (ν(C=O) is 1679 cm −1 ). It should be noted that the IR spectrum of 2·3H 2 O contains ν(OH) at about 3425 cm −1 , which is characteristic of associated water molecules. The IR spectra of 1 and 3 contain no bands in this region, thus indicating the formation of water-free compounds.
According to single-crystal X-ray diffraction data, crystal 1 is built of cobalt(II) complexes [Co(DMF) 6 ] 2+ and anions [B 12 H 12 ] 2− (Figure 1a). The triclinic unit cell (space group P-1) of compound 1 contains four 1 2 complex cations located at the inversion centers and two anions occupying a common position. The coordination environment of Co(II) atoms includes six oxygen atoms from six DMF molecules.  6 ] 2+ form three-dimensional networks with square channels directed along axis a ( Figure S2). The [B 12 H 12 ] 2− anions are located in the center of these channels.

Scheme 1. Synthesis of precursors 1-3.
The coordinated state of DMF molecules by the oxygen atom of the carbonyl group is evidenced by the shift of band ν(C=O) (1651, 1664, and 1652 cm -1 in the IR spectra of 1, 2•3H2O and 3, respectively) into a lower frequency interval compared to that in the spectrum of free DMF (ν(C=O) is 1679 cm -1 ). It should be noted that the IR spectrum of 2•3H2O contains ν(OH) at about 3425 cm -1 , which is characteristic of associated water molecules. The IR spectra of 1 and 3 contain no bands in this region, thus indicating the formation of water-free compounds.
According to single-crystal X-ray diffraction data, crystal 1 is built of cobalt(II) complexes [Co(DMF)6] 2+ and anions [B12H12] 2- (Figure 1a). The triclinic unit cell (space group P-1) of compound 1 contains four ½ complex cations located at the inversion centers and two anions occupying a common position. The coordination environment of Co(II) atoms includes six oxygen atoms from six DMF molecules. The octahedra of metal atoms are slightly distorted. The Co-O bond lengths are in the range of 2.067-2.102 Å in 1. The O-Co-O bond angles are in the range of 87.2-92.8˚ and 87.6-92.4˚, respectively. In the packing of the structure of 1, complex cations [Co(DMF)6] 2+ form three-dimensional networks with square channels directed along axis a ( Figure S2). The [В12Н12] 2-anions are located in the center of these channels.
The structures of samples 2 [38] and 3 [37] were determined early; they are structurally similar and are shown in Figure 1b-c. Note that water-free sample 2 was isolated when anhydrous CoCl2 was allowed to react with (Et3NH)2[B20H18]; here we used sample 2•3H2O.  The structures of samples 2 [38] and 3 [37] were determined early; they are structurally similar and are shown in Figure 1b,c. Note that water-free sample 2 was isolated when anhydrous CoCl 2 was allowed to react with (Et 3 NH) 2  ons and anions are observed (in Figure 2a, dotted green lines show the B…H contacts, dotted red lines show the H…H contacts, the distances between atoms in which are less than the sum of the van der Waals radii). The strongest CH…BH interactions are represented on the Hirschfeld surface of the anion as red spots. Analysis of the full two-dimensional fingerprint plot shows that the H…H contacts of the anion account for 99.3% of the surface. X-ray powder diffraction data revealed that samples 1, 2•3H2O, and 3 are individual compounds and contain no impurities ( Figure S3). Experimental X-ray diffraction patterns for 1, 2•3H2O, and 3 were compared to calculated data found from single-crystal Xray diffraction studies of compounds 1-3. Some discrepancy in the X-ray diffraction pattern of 2 and 2•3H2O can be explained by the presence of associated water molecules in sample 2•3H2O.
TGA studies of samples [Co(DMF)6][An] (1-3) were performed in argon. Sample 1 is stable up to 156.47 °С (Figure 3). At this temperature, an endothermic effect appears on the thermogram, accompanied by a loss of sample weight of 34.11% which corresponds to loss of three DMF molecules and corresponding to the first stage of the removal of the organic part of the complex. With an increase in temperature to 241 °С, the second endothermic effect is observed on the thermogram, accompanied by a weight loss of the sample of 15.36% which corresponds to one DMF molecule. A further increase in temperature leads to an exothermic effects at 241.09 °С, which is accompanied with a weight loss of 51.47% and corresponds to loss of two remaining DMF molecules. An exothermic effect at 269.94 °С is accompanied with no weight loss and can be assigned to the opening of the closo-structure of the boron cluster to form nido-structures; an effect near 460 °С without weight loss can be assigned to rearrangement of nido-system and further destruction of the boron cage. X-ray powder diffraction data revealed that samples 1, 2·3H 2 O, and 3 are individual compounds and contain no impurities ( Figure S3). Experimental X-ray diffraction patterns for 1, 2·3H 2 O, and 3 were compared to calculated data found from single-crystal X-ray diffraction studies of compounds 1-3. Some discrepancy in the X-ray diffraction pattern of 2 and 2·3H 2 O can be explained by the presence of associated water molecules in sample TGA studies of samples [Co(DMF) 6 ][An] (1-3) were performed in argon. Sample 1 is stable up to 156.47 • C (Figure 3). At this temperature, an endothermic effect appears on the thermogram, accompanied by a loss of sample weight of 34.11% which corresponds to loss of three DMF molecules and corresponding to the first stage of the removal of the organic part of the complex. With an increase in temperature to 241 • C, the second endothermic effect is observed on the thermogram, accompanied by a weight loss of the sample of 15.36% which corresponds to one DMF molecule. A further increase in temperature leads to an exothermic effects at 241.09 • C, which is accompanied with a weight loss of 51.47% and corresponds to loss of two remaining DMF molecules. An exothermic effect at 269.94 • C is accompanied with no weight loss and can be assigned to the opening of the closo-structure of the boron cluster to form nido-structures; an effect near 460 • C without weight loss can be assigned to rearrangement of nido-system and further destruction of the boron cage. Molecules 2023, 28, 453 5 of 17 For 2•3H2O, a gradual weight loss of 7.489% is observed in the temperature range of 20-160 °C, which is accompanied by a broadened endothermic effect with a final value of 143.5 °C (Figure 4). These processes correspond to the removal of three associated water molecules, which is consistent with the data of the IR spectrum of 2•3H2O, where the ν(OH) stretching vibration band characteristic of associated water molecules is observed at 3450 cm -1 .
In the range of 155-220 °С, an exothermic effect is observed with a maximum at 204 °С, which is accompanied by a weight loss of 18.37% and corresponds to the removal of two coordinated DMF molecules. With a further increase in temperature, an exothermic effect is observed at 326 °C with sample weight loss of 8.257%, which corresponds to the removal of another DMF molecule. The broadened exothermic effects at 357 °C without weight loss corresponds to the opening of the closo-system of the boron cage; an effect at 470 °C can be assigned to rearrangement of the nido-system of the boron cage. Further heating results in gradual destruction of the boron cage accompanied by a weight loss of 7.815 °C of the sample which corresponds to release of one DMF molecule. For 2·3H 2 O, a gradual weight loss of 7.489% is observed in the temperature range of 20-160 • C, which is accompanied by a broadened endothermic effect with a final value of 143.5 • C ( Figure 4). These processes correspond to the removal of three associated water molecules, which is consistent with the data of the IR spectrum of 2·3H 2 O, where the ν(OH) stretching vibration band characteristic of associated water molecules is observed at 3450 cm −1 . For 2•3H2O, a gradual weight loss of 7.489% is observed in the temperature range of 20-160 °C, which is accompanied by a broadened endothermic effect with a final value of 143.5 °C (Figure 4). These processes correspond to the removal of three associated water molecules, which is consistent with the data of the IR spectrum of 2•3H2O, where the ν(OH) stretching vibration band characteristic of associated water molecules is observed at 3450 cm -1 .
In the range of 155-220 °С, an exothermic effect is observed with a maximum at 204 °С, which is accompanied by a weight loss of 18.37% and corresponds to the removal of two coordinated DMF molecules. With a further increase in temperature, an exothermic effect is observed at 326 °C with sample weight loss of 8.257%, which corresponds to the removal of another DMF molecule. The broadened exothermic effects at 357 °C without weight loss corresponds to the opening of the closo-system of the boron cage; an effect at 470 °C can be assigned to rearrangement of the nido-system of the boron cage. Further heating results in gradual destruction of the boron cage accompanied by a weight loss of 7.815 °C of the sample which corresponds to release of one DMF molecule. In the range of 155-220 • C, an exothermic effect is observed with a maximum at 204 • C, which is accompanied by a weight loss of 18.37% and corresponds to the removal of two coordinated DMF molecules. With a further increase in temperature, an exothermic effect is observed at 326 • C with sample weight loss of 8.257%, which corresponds to the removal of another DMF molecule. The broadened exothermic effects at 357 • C without weight loss corresponds to the opening of the closo-system of the boron cage; an effect at 470 • C can be assigned to rearrangement of the nido-system of the boron cage. Further heating results in gradual destruction of the boron cage accompanied by a weight loss of 7.815 • C of the sample which corresponds to release of one DMF molecule.
Three pronounced thermal effects are observed on the thermogram of sample 3 (Figure 5). The endothermic effect with a maximum at 203 • C, accompanied by a loss of sample weight 15.43%, corresponds to the removal of two DMF molecules. Two exothermic effects at 361.61 and 413.99 • C, accompanied by a weight loss of 16.68 and 14.34%, respectively, indicate the stepwise removal of four DMF molecules with simultaneous destruction of the closo-system of the boron cage. With further heating of the sample above 500 • C, no thermal effects are observed on the differential curve; however, the TG curve shows a mass loss of 9.803%, corresponding to the partial removal of exopolyhedral chlorine atoms with the formation of a Cl 2 molecule.  Three pronounced thermal effects are observed on the thermogram of sample 3 (Figure 5). The endothermic effect with a maximum at 203 °C, accompanied by a loss of sample weight 15.43%, corresponds to the removal of two DMF molecules. Two exothermic effects at 361.61 and 413.99 °C, accompanied by a weight loss of 16.68 and 14.34%, respectively, indicate the stepwise removal of four DMF molecules with simultaneous destruction of the closo-system of the boron cage. With further heating of the sample above 500 °C, no thermal effects are observed on the differential curve; however, the TG curve shows a mass loss of 9.803%, corresponding to the partial removal of exopolyhedral chlorine atoms with the formation of a Cl2 molecule. Based on the results obtained, the annealing temperature needed to prepare boride phases was determined to be 900 °C in order to achieve maximum structuration of samples. When heated 1, 2•3H2O, and 3 at 900 °C in argon, products 1a, 2a, and 3a, respectively, were prepared.

Thermal Decomposition of 1-3
The completeness of annealing of precursors 1-3 and the phase composition of samples 1a-3a were determined based on X-ray powder diffraction and IR spectroscopy data. On the X-ray powder diffraction patterns of the annealed samples, visually distinguishable reflections of the observed crystalline phases are noted and the corresponding Miller indices are marked ( Figure 6). The card numbers of the PDF-2 X-ray powder database used in this work are shown.
According to X-ray powder diffraction data, the annealing product 1a is a two-phase mixture (Figure 6a). The diffraction pattern contains reflections corresponding to boron nitride BN in the hexagonal modification, as well as reflections of cobalt monoboride CoB. Based on the results obtained, the annealing temperature needed to prepare boride phases was determined to be 900 • C in order to achieve maximum structuration of samples. When heated 1, 2·3H 2 O, and 3 at 900 • C in argon, products 1a, 2a, and 3a, respectively, were prepared.

Thermal Decomposition of 1-3
The completeness of annealing of precursors 1-3 and the phase composition of samples 1a-3a were determined based on X-ray powder diffraction and IR spectroscopy data. On the X-ray powder diffraction patterns of the annealed samples, visually distinguishable reflections of the observed crystalline phases are noted and the corresponding Miller indices are marked (Figure 6). The card numbers of the PDF-2 X-ray powder database used in this work are shown. In the case of sample 2a, boron nitride reflections (hexagonal modification) are also observed in the diffraction pattern ( Figure 6b). However, in contrast to 1a, the relative intensity of the reflections is lower, which can be caused by a decrease in the particle size of the CoB phase. Apparently, the increase in the size of CoB crystallites is hindered by their dilution in the nitride matrix due to an increase in the ratio of the number of boron atoms in the cluster (12 versus 20 boron atoms) to the number of nitrogen atoms in DMF molecules (compared with sample 1a).
The diffraction pattern of sample 3a shows reflections of the CoB crystalline phase (Figure 7) without other reflections. The formation of cobalt monoboride CoB in the tetragonal modification is observed for all samples; for 1a and 2a, it is better described by the space group Pbnm, the annealing product 3a has a crystal lattice with the space group Pnma.
In the case of all studied annealed compounds, the formation of other phases of the Co-B system (other cobalt borides, metallic cobalt, or crystalline boron) was not detected According to X-ray powder diffraction data, the annealing product 1a is a two-phase mixture (Figure 6a). The diffraction pattern contains reflections corresponding to boron nitride BN in the hexagonal modification, as well as reflections of cobalt monoboride CoB.
In the case of sample 2a, boron nitride reflections (hexagonal modification) are also observed in the diffraction pattern (Figure 6b). However, in contrast to 1a, the relative intensity of the reflections is lower, which can be caused by a decrease in the particle size of the CoB phase. Apparently, the increase in the size of CoB crystallites is hindered by their dilution in the nitride matrix due to an increase in the ratio of the number of boron atoms in the cluster (12 versus 20 boron atoms) to the number of nitrogen atoms in DMF molecules (compared with sample 1a).
The diffraction pattern of sample 3a shows reflections of the CoB crystalline phase (Figure 7) without other reflections. In the case of sample 2a, boron nitride reflections (hexagonal modification) are also observed in the diffraction pattern (Figure 6b). However, in contrast to 1a, the relative intensity of the reflections is lower, which can be caused by a decrease in the particle size of the CoB phase. Apparently, the increase in the size of CoB crystallites is hindered by their dilution in the nitride matrix due to an increase in the ratio of the number of boron atoms in the cluster (12 versus 20 boron atoms) to the number of nitrogen atoms in DMF molecules (compared with sample 1a).
The diffraction pattern of sample 3a shows reflections of the CoB crystalline phase (Figure 7) without other reflections. The formation of cobalt monoboride CoB in the tetragonal modification is observed for all samples; for 1a and 2a, it is better described by the space group Pbnm, the annealing product 3a has a crystal lattice with the space group Pnma.
In the case of all studied annealed compounds, the formation of other phases of the Co-B system (other cobalt borides, metallic cobalt, or crystalline boron) was not detected The formation of cobalt monoboride CoB in the tetragonal modification is observed for all samples; for 1a and 2a, it is better described by the space group Pbnm, the annealing product 3a has a crystal lattice with the space group Pnma.
In the case of all studied annealed compounds, the formation of other phases of the Co-B system (other cobalt borides, metallic cobalt, or crystalline boron) was not detected by X-ray powder diffraction. However, the presence of some amorphous components is expected.
The absence of absorption bands of stretching vibrations ν(BH) at 2466 cm −1 and 2532, 2497 cm −1 in the IR spectra of samples 1a and 2a, respectively, or ν(BCl) at 1157, 1002, and ν + δ(BB) at 843 cm −1 in the IR spectrum of 3a, as well as ν(C=O) at 1651, 1664, and 1652 cm −1 indicates complete destruction of boron cluster anions and coordinated dimethylformamide molecules, respectively (Figures S4-S6). The absorption band at 780 cm −1 in the IR spectrum of 1a and 781 cm −1 in the IR spectrum of 2a, which, according to the literature data [39], refers to stretching vibrations of the ν(BN) bond, indicates the formation of a boron nitride phase in annealed samples 1a and 2a. It should be noted that this absorption band is not observed in the IR spectrum of the annealed sample 3a ( Figure S6). In addition, the presence of absorption bands at~1100 and~798 cm −1 , as well as the correlation with the IR spectrum of amorphous boron, suggests the presence of an amorphous boron phase in annealed samples 1a-3a. It seems logical because using the started samples, the Co:B ratio is 1:12, 1:20, and 1:10 for 1, 2·3H 2 O, and 3, respectively. In the products, CoB and BN are observed (note that Co:N ratio is 1:6 for all the starting samples). Therefore, formation of amorphous boron is expected for all three samples.
Analyzing the data obtained from TGA studies, we can discuss the composition of compounds formed in samples 1a-3a. Note

Morphology of Samples 1a-3a
According to the presented TEM images (Figure 8), sample 1 is an inhomogeneous two-component system, which consists of large blocks and nanosized particles of cobalt monoboride crystallized on its surface, which have isometric shape. As can be seen from the distribution curve, the sizes of isometric particles are in the range of 2-35 nm. The average nanoparticle size is 11 nm (Figure 8d).
However, sample 2a is characterized by a higher degree of destruction of the matrix and the formation of nanosized particles of cobalt monoboride in both agglomerated and non-agglomerated forms (Figure 9b,c). Cobalt monoboride particles in sample 2a have a spherical shape. The particle sizes are in the range of 2-26 nm, with an average value of 10 nm. According to the size distribution curve, the nanosized particles of sample 2a are characterized by a smaller size spread. Heating of 2, as in the case of 1, leads to the destruction of its crystal structure and the formation of a two-component system consisting of large blocks and nanosized particles crystallized on their surface (Figure 9).  Heating of 2, as in the case of 1, leads to the destruction of its crystal structure and the formation of a two-component system consisting of large blocks and nanosized particles crystallized on their surface (Figure 9). Heating of 2, as in the case of 1, leads to the destruction of its crystal structure and the formation of a two-component system consisting of large blocks and nanosized particles crystallized on their surface (Figure 9).  Heating of 3, as in the case of 1 and 2, leads to the destruction of the crystal structure. However, it should be noted that, in all cases, an aqueous suspension was prepared for the study of samples by the TEM method, which was then sprayed onto carbon-coated copper grids. When preparing an aqueous suspension of sample 3a, a sharp odor was present. The process of dissolution is indirectly confirmed by the observed process of sample recrystallization on a carbon film in the form of separate branches ( Figure 10).
However, sample 2a is characterized by a higher degree of destruction of the matrix and the formation of nanosized particles of cobalt monoboride in both agglomerated and non-agglomerated forms (Figure 9b, 9c). Cobalt monoboride particles in sample 2a have a spherical shape. The particle sizes are in the range of 2-26 nm, with an average value of 10 nm. According to the size distribution curve, the nanosized particles of sample 2a are characterized by a smaller size spread.
Heating of 3, as in the case of 1 and 2, leads to the destruction of the crystal structure. However, it should be noted that, in all cases, an aqueous suspension was prepared for the study of samples by the TEM method, which was then sprayed onto carbon-coated copper grids. When preparing an aqueous suspension of sample 3a, a sharp odor was present. The process of dissolution is indirectly confirmed by the observed process of sample recrystallization on a carbon film in the form of separate branches (Figure 10). The crystals of sample 3a have the shape of regular hexagons (Figure 11a-c). It should be noted that sample 3a is characterized by the formation of crystals with well-defined faces, which indicates the perfection of the structure of the synthesized particles. The crystals of sample 3a have the shape of regular hexagons (Figure 11a-c). It should be noted that sample 3a is characterized by the formation of crystals with well-defined faces, which indicates the perfection of the structure of the synthesized particles. At the same time, an intermediate stage of the formation of faces of future crystals with a disordered defect structure is fixed (Figure 11a-11c), as evidenced by the inhomogeneity of the structure of the synthesized particles. Figure 11d shows the particle size Figure 11. (a-c) TEM images and (d) particle size distribution curve of sample 3a.
At the same time, an intermediate stage of the formation of faces of future crystals with a disordered defect structure is fixed (Figure 11a-c), as evidenced by the inhomogeneity of the structure of the synthesized particles. Figure 11d shows the particle size distribution curve: the particle size is in the range of 25-400 nm with an average size of about 250 nm.
Analyzing the results obtained, the process of formation of nanocrystalline cobalt monoboride in the course of thermal decomposition of cobalt(II) coordination compounds with boron clusters can be represented as follows (Scheme 2). The absence of BN in 3a is explained by the fact that the thermolysis of 3 conta [B10Cl10] 2-is accompanied by the destruction of the boron cluster and release of chl atoms. The latter, in turn, are a strong oxidizing agent, which leads to the oxidation o amide nitrogen atom N 3-, which is formed as a result of the destruction of dimethy mamide molecules, to a neutral N2 molecule followed by its removal from the syste addition, the released chlorine interacts with the boron atoms formed as a result o destruction of the boron cluster, which leads to the formation of a chlorine-boron pound. It should be noted that chlorine in the composition of annealing product 3a as a mineralizer, which improves the structure of cobalt monoboride particles (Figur The presence of chlorine in the annealing product 3a was qualitatively confirme X-ray fluorescence analysis. Note that this method qualitatively demonstrated the ence of Co in the thermolysis product 3a. The presence of analytical lines ClKα, ClKβ, C and CoKβ was revealed with a value many times higher than the background compo ( Figure S7). The absence of BN in 3a is explained by the fact that the thermolysis of 3 containing [B 10 Cl 10 ] 2− is accompanied by the destruction of the boron cluster and release of chlorine atoms. The latter, in turn, are a strong oxidizing agent, which leads to the oxidation of the amide nitrogen atom N 3-, which is formed as a result of the destruction of dimethylformamide molecules, to a neutral N 2 molecule followed by its removal from the system. In addition, the released chlorine interacts with the boron atoms formed as a result of the destruction of the boron cluster, which leads to the formation of a chlorine-boron compound. It should be noted that chlorine in the composition of annealing product 3a acts as a mineralizer, which improves the structure of cobalt monoboride particles ( Figure 11).

Synthesis of Compounds
The presence of chlorine in the annealing product 3a was qualitatively confirmed by X-ray fluorescence analysis. Note that this method qualitatively demonstrated the presence of Co in the thermolysis product 3a. The presence of analytical lines ClK α , ClK β , CoK α , and CoK β was revealed with a value many times higher than the background component ( Figure S7).

Preparation of Compounds 1a-3a
Compounds 1-3 were annealed in a quartz tube-reactor heated by a resistance furnace and sealed hermetically with tapered silica glass ground joints. The studied samples were placed in corundum crucibles. Annealing was carried out in a high purity argon (5-7 ppm O 2 , 10 ppm H 2 O) flow at a gas flow rate of 300 mL/min and heating at 10 • C/min. The annealing time for each sample was 120 min (in a flow of high purity argon) at 900 • C; the sample was cooled down to room temperature in an Ar flow. Note that with a longer exposure, the phase composition (qualitative and quantitative) did not change. Visually, the thermolysis products 1a-3a are black powders remained stable when treated in air.

Methods of Investigation
Elemental analysis of compounds 1-3 for carbon, hydrogen, and nitrogen was performed using a Carlo ErbaCHNS-3 FA 1108 automated elemental analyzer. Boron and metal content was determined on an iCAP 6300 Duo ICP emission spectrometer with inductively coupled plasma. Before the measurements, samples were dried in vacuum to constant weight; for 2·3H 2 O, solvent-free sample 2 was obtained.
IR spectra of complexes 1, 2·3H 2 O, 3 and annealed products 1a-3a and amorphous boron were recorded on a Lumex Infralum FT-02 Fourier-transform spectrophotometer in the range of 4000-600 cm −1 at a resolution of 1 cm −1 . Samples were prepared as Nujol mulls; NaCl pellets were used.
X-ray diffraction study. The single-crystal X-ray diffraction data for 1 performed with a Bruker APEX-II CCD and a Bruker D8 Venture (Centre of Joint Equipment of Kurnakov Institute of General and Inorganic Chemistry, Russian Academy of Sciences) using ϕ and ω-scan mode. The data were indexed and integrated using the SAINT program [44]. Absorption correction based on measurements of equivalent reflections (SADABS) were applied [45]. The structures were determined by direct methods and refined by full-matrix least squares technique on F 2 with anisotropic displacement parameters for non-hydrogen atoms. The hydrogen atoms were placed in calculated positions and refined within riding model with fixed isotropic displacement parameters [U iso (H) = 1.5U eq (C) for the CH 3groups and 1.2U eq (C) for the other groups]. All calculations were carried out using the SHELXTL program [46] and OLEX2 program package [47]. For details, see Table S1 (Electronic Supporting Information).
The crystallographic data were deposited with the Cambridge Crystallographic Data Center, CCDC no. 2159665. Copies of this information may be obtained free of charge from the Director, CCDC, 12 Union Road, Cambridge CHB2 1EZ, UK (Fax: +44 1223 336033; e-mail: deposit@ccdc.cam.ac.uk or www.ccdc.cam.ac.uk (accessed on 24 November 2022)).
X-ray powder diffraction studies of started samples 1-3 and annealed products 1a-3a were performed on a Bruker D8 ADVANCE diffractometer (CuK α radiation, Ni filter, LYNXEYE detector, reflection geometry) in low-background cuvettes with an oriented silicon single crystal substrate in the angle range 2θ = 5 • -80 • with a step 0.01125 • .
X-ray spectral fluorescence analysis of sample 3a was performed on a wave-dispersive X-ray fluorescence spectrometer SPECTROSCAN MAX (Russia) (voltage 40 kV, current 0.5 mA, X-ray tube anode material Pd, analyzer crystals: LiF(200) and COO 2 . Individual particles were placed between two layers of a polyethylene terephthalate film of thickness 5 µm.
Thermogravimetric analysis (TG-DSC) of samples 1-3 was carried out using an SDT Q600 synchronous thermal analyzer in alundum crucibles (40-100 µL) in a flow of high purity argon (100 mL/min) at a sample heating rate of 10 • C/min and within the range temperatures from room temperature to 900 • C. Samples 1-3 were annealed in a Nabertherm R 30/200/11 tube furnace in an inert gas flow to form samples 1a-3a. Before annealing, samples were ground in an agate mortar and transferred into thin-walled quartz test tubes, which were then placed in a quartz flow tube at the level of the furnace hot zone.
Transmission electron microscopy (TEM) studies of samples 1a-3a were carried out on a Jem-1011 instrument at an accelerating voltage of 80 kV. Samples were applied to copper grids by ultrasonic sputtering.
Hirshfeld surface analysis. The Crystal Explorer 17.5 [48] program was used to analyze the interactions within crystal 1. The donor-acceptor groups are visualized using a standard (high) surface resolution and d norm surfaces are mapped over a fixed color scale of −0.640 (red) to 0.986 (blue) a.u.

Conclusions
Nanocrystalline cobalt boride in the tetragonal modification was prepared by thermal decomposition (900 • C) of preliminarily synthesized cobalt precursors [Co(DMF) 6 (3) in an argon atmosphere. Thermolysis products 1a-3a were identified and characterized by X-ray powder diffraction and IR spectroscopy; X-ray fluorescence data were obtained for 3a. The average particle size of cobalt monoboride was determined using transmission electron microscopy (TEM). It has been found that the nature of the boron cluster anion affects the phase composition of the thermolysis products (presence of a boron nitride phase during the thermolysis of 1 and 2), as well as the structural features of the resulting cobalt monoboride (space groups Pbnm or Pnma). Thermolysis of 1 and 2 afforded CoB particles up to 35 nm in size with a narrow size distribution curve, which is an important task in catalysis; 3 gave CoB with 200-350 nm in size.