Hydrogen-bonded supramolecular structures in copper(II) nitrobenzoates with N-methylnicotinamide: synthesis, supramolecular structure, Hirshfeld surface analysis, spectral and DFT study

The synthesis of six new copper(II) nitrobenzoate complexes with N-methylnicotinamide, used as an auxiliary ligand for a supramolecular interaction study, is reported. Crystal structures of six novel compounds [Cu(2-NO2bz)2(mna)2(H2O)2] (1), [Cu(2-NO2bz)2(mna)2(H2O)2]∙2H2O (2), [Cu(3-NO2bz)2(mna)2(H2O)2] (3), [Cu(3,5-(NO2)2bz)2(mna)2(H2O)2]∙2H2O (4), [Cu(4-NO2bz)2(mna)2(H2O)2]∙2(4-NO2bzH) (5) and [Cu(3,5-(NO2)2bz)2(mna)(H2O)3] (6) (mna = N-methylnicotinamide, 2-NO2bz = 2-nitrobenzoate, 3-NO2bz = 3-nitrobenzoate, 4-NO2bz = 4-nitrobenzoate, 3,5-(NO2)2bz = 3,5-dinitrobenzoate) were determined by X-ray analysis. Compounds 1–6 are mononuclear with a tetragonal-bipyramidal geometry around the Cu2+ ion. The molecules of the studied complexes are mostly linked by a combination of N–H…O and O–H…O hydrogen bonds between N-methylnicotinamide and water molecules into supramolecular hydrogen-bonded coordination chains and networks. Intermolecular interactions in the supramolecular structures were also studied using Hirshfeld surface analysis. In addition, the complexes 1–6 have been characterised by elemental analysis, IR, UV–Vis and EPR spectroscopy. Density functional theory calculations were performed in order to reproduce the EPR magnetic parameters. DFT calculations of the EPR parameters show a good agreement with the experimental results.


Introduction
The field of structural and supramolecular chemistry has developed rapidly in the study of metal-organic supramolecular systems, partly because of the intellectual challenge of controlling the self-assembly processes and partly because of the potential applications of such novel materials in magnetic devices, nonlinear optical materials, heterogeneous catalysis, microporous and zeolite-like materials [1][2][3][4][5].The formation of various metal-organic supramolecular frameworks is caused by a spontaneous self-assembly process of metal cations and ligands via metal-ligand coordination in combination with other noncovalent interactions such as hydrogen bonding, π-π interactions or dispersive interactions [6].
Excellent examples of ligands for the construction of supramolecular architectures in the metal complexes are pyridincarboxamides such as nicotinamide and its derivatives [7].Nicotinamide is one of the most extensively studied pyridine derivatives.It is a component of the vitamin B complex and also forms part of the vital coenzyme NAD (nicotinamide adenine dinucleotide) [8].It is also a typical N-donor ligand, widely used in crystal engineering and supramolecular chemistry [9][10][11][12][13].Moreover, copper(II) carboxylate complexes with nicotinamide or isonicotinamide could have a potential utilization in supramolecular medicinal chemistry [14,15].Nicotinamide as a ligand in the transition metal complexes creates the hydrogen-bonded coordination networks through the carboxamide group [7,9].The hydrogen-bonded metal-organic supramolecular systems based on nicotinamide have been extensively studied in other papers [16][17][18][19][20][21][22][23].On the other hand, only a few papers report on transition metal complexes with N-methylnicotinamide as a hydrogen-bonded linking agent for the construction of different supramolecular architectures [24][25][26][27][28][29][30].

[Cu(2-NO 2 bz) 2 (mna) 2 (H 2 O) 2 ]•2H 2 O (2)
The complex 2 was prepared as described above for 1, except that the synthesis was carried out in aqueous solution.Yield: 0.15 g (41%  The complex 3 was prepared by the reaction of an aqueous solution (100 ml) of copper(II) acetate (0.5 mmol, 0.100 g) with N-methylnicotinamide (1 mmol, 0.136 g) followed by addition of the 3-nitrobenzoic acid (1 mmol, 0.167 g).The reaction mixture was stirred until the reaction finished and the color of the product remained unchanged.The blue microcrystals were filtered off, washed with small portion of water and dried at ambient temperature.The resulting solution obtained from filtration was kept for evaporation at ambient temperature.The blue crystals suitable for X-ray structure determination were separated after a several days.Yield: 0.20 g (57% The complex 4 was prepared in similar manner as 3 except that 3,5-dinitrobenzoic acid (1 mmol, 0.212 g) was used.Yield: 0.28 g (68%).Anal.calc.for C 28  The complex 5 was prepared as described for 3 except that 4-nitrobenzoic acid (2 mmol, 0.234 g) was used and the molar ratio copper(II) acetate: N-methylnicotinamide has been changed from 1: 2 to 1: 1 (1 mmol, 0.136 g of N-methylnicotinamide).Yield: 0.45 g (43%).Anal.calc.for  The complex 6 was prepared as described for 5 except that 3,5-dinitrobenzoic acid (2 mmol, 0.424 g) was used.Yield: 0.57 g (84%

Physical measurements
Carbon, hydrogen and nitrogen analyses were carried out on a CHNSO FlashEA™ 1112 Automatic Elemental Analyzer.The electronic spectra (190-1100 nm) of the complexes in the solid state were measured in nujol suspension with a SPECORD 250 Plus (Carl Zeiss Jena) spectrophotometer at room temperature.The infrared solid state spectra (ATR technique, 4000-400 cm −1 ) were recorded on a Nicolet 5700 FT-IR spectrophotometers at room temperature.Room-temperature EPR spectra of the powdered samples were recorded on an EMX Plus series EPR spectrometer (Bruker, Germany) operating at X-band (≈ 9.4 GHz) and simulated using Spin.exesoftware developed by Dr. Ozarowski [31].

X-ray crystallography
Data collection and cell refinement for complexes under study were measured on a Bruker-Nonius Kappa CCD diffractometer with an APEX-II CCD detector using graphite monochromated Mo-Kα radiation.Absorption correction was applied by multi-scan method using SADABS program [32].The structures were solved by a direct method with ShelXS-2013 [33] or SIR-2011 [34] and refined by the fullmatrix least squares procedure with either ShelXL [35] or Olex2.refine[36].Geometrical analysis was performed using ShelXL and the structures were drawn using the OLEX2 (ver.1.5) [37] or MERCURY (ver.3.8) [38] programs.ORTEP-like representations of the molecular structure of all complexes with descriptions of all non-hydrogen atoms are presented in the supplementary material as Figs.S1-S6.Table 1 shows the final crystal data and structure refinement parameters.
Nitro groups in crystal structures: 3 (nitro group of the 3-nitrobenzoate ligand), 4 (two nitro groups of the 3,5-dinitrobenzoate ligand) and 6 (two nitro groups of a 3,5-dinitrobenzoate ligand) are disordered in two positions with occupation factors 0.25/0.75;0.15/0.85;0.77/0.23;0.77/0.23;0.20/0.80,respectively.Hydrogen atoms of water molecules were found from the difference map or added and refined using a utility in OLEX2.They were then fixed at the refined ideal distances.Hydrogen atoms of other groups were added at standard distances.

Hirshfeld surface analyses
CrystalExplorer [39] was used to calculate Hirshfeld surfaces [40,41] and associated fingerprint plots [42,43].The Hirshfeld surfaces have been calculated including all orientations of the disordered methyl groups with their partial occupancies.Hirshfeld surfaces for disordered structures (3, 4 and 6) have been calculated for both disordered parts.

DFT calculations and computational details
The theoretical DFT calculation of g factors and A tensors were done with ORCA (version 4.0.0.2) program package [44] using methods developed and implemented into ORCA by Neese [45,46].Geometry optimization was done with the BP86 functional with Grimme dispersion correction method D3BJ on the experimental geometries obtained directly from the X-ray analysis.Tight convergence criteria and increased integration grids (final grid 5) were applied throughout.The def2-TZVP basis set together with corresponding auxilliary basis set was employed in the calculation.Two different functional have been used in the calculation: one hybrid functional, B3LYP and one hybrid meta-GGA functional, TPSSh.Relativistic effects were included using the Douglas-Kroll-Hess transformation to second order.The aug-cc-pVTZ-J basis set was employed for Cu [47] in the computation of spin hamiltonian parameters using enhanced grid for copper (SpecialGridIntAcc 7).All other atoms utilized relativistically recontracted Ahlrich's dkh-def2-TZVP basis set [48,49].Spin-orbit mean field approach SOMF(1X) with one-center approximation to the exchange term were also applied.To speed up the calculation the chain-of-spheres approximation (RIJCOSX) was set on using an automatically generated auxiliary basis set [50].In order to increase convergence tolerances and integration accuracy, TightSCF and Grid5 options were used.All our calculation of molecular g and A tensors have been done in the gas phase and we have made no attempt to simulate environmental effects on the computed values.

Synthesis
The reaction between copper acetate dihydrate, N-methylnicotinamide and the corresponding nitrobenzoic acid in appropriate molar ratios in acetonitrile (1) or aqueous solution (2-6) leads to the formation of complexes of the . A schematic representation of the preparation procedure is summarised in Scheme 1.All six complexes were isolated in a good yields (41-84%) and are stable in the air.The composition of the complexes was verified by the results of elemental analysis and IR spectroscopy and finally fully confirmed by single crystal X-ray diffraction analysis.

FT-IR and electronic spectroscopy
The IR spectra of the complexes 1-6 were measured in the range of 4000-400 cm −1 in the solid state by ATR technique (Figs.S7-S12) and a tentative band assignment of the main functional groups of the bound ligands (water, nitrobenzoates and N-methylnicotinamide) was done based on the literature [51].In general, the observed main features of the IR spectra were clearly consistent with the composition and structural features of the prepared complexes.Some selected IR bands of complexes 1-6 are collected in Table 2.The IR spectra of all studied complexes showed broad peaks of medium intensity in the region 3500-3100 cm −1 , which can be attributed to O-H (broader peaks at 3501-3444 cm −1 ) and N-H (sharper peaks at 3368-3305 cm −1 ) stretching vibrations of coordinated water and N-methylnicotinamide.Moreover, the complexes containing a lattice water molecules (2,4) or an additional water molecule (6) in addition to the coordinated axial water molecules also showed another broad band in this region (Figs.S8, S10, S12).The weak absorption bands observed in the region 3100-2600 cm −1 were attributed to C-H stretching vibrations of the coordinated nitrobenzoate and N-methylnicotinamide ligands.
The carboxylate coordination mode of nitrobenzoates can be verified by the observation of antisymmetric and symmetric stretching vibrations of the carboxyl group, found in the region 1585-1544 cm −1 and 1388-1374 cm −1 for the studied complexes.The parameter ∆ (ῦ a (COO)-ῦ s (COO)) which is used in this context shows values from 184 cm −1 for 1 to 210 for 5 cm −1 , except for complex 3 (∆ = 157 cm −1 ).These values indicate a monodentate type of coordination of the nitrobenzoate ligand, in agreement with literature data [19,52].The lower observed value of the ∆ parameter for complex 3 does not imply a different coordination mode of the 3-nitrobenzoate ligand, but can be explained by the presence of a combination band (mixed asymmetric NO 2 and COO − vibration) in the IR spectrum, which hinders the more accurate wavenumber determination of ῦ a (COO).Furthermore, the IR spectrum of 5 contains bands at 1707 and 1242 cm −1 respectively, which can be attributed to C=O and C-O stretching frequencies of 4-nitrobenzoic acid, which is bound by strong hydrogen bonds in the second coordination sphere of the complex.The most intense absorption bands in the IR spectra of all complexes were bands found between 1544-1515 cm −1 and 1376-1317 cm −1 which can be assigned to asymmetric and symmetric stretching vibrations of the nitro group [53].
The most characteristic absorption bands of secondary amides, such as N-methylnicotinamide, are the stretching vibration bands attributed to the N-H vibration and the mixed vibration called amide I, corresponding mainly to the C=O vibration, which could be easily identified in the IR spectra [26].These bands are found at 3329 cm −1 for N-H and 1640 cm −1 for amide I in the IR spectrum of solid N-methylnicotinamide.Both bands are strongly involved in the hydrogen bonding, as shown by the crystal structure of the solid ligand [26].In this respect, the involvement of the amide group in the hydrogen bonding in the studied complexes can be followed from the position of the amide I band.The carbonyl group in amides acts as an acceptor of hydrogen in hydrogen bonding.In complexes 1 and 3, the carbonyl group is not involved in the hydrogen bonding (Table 4), hence the observed position of the amide I band (1662 and 1666 cm −1 ) is found at a higher wavenumber compared to the solid N-methylnicotinamide ligand (1640 cm −1 ).However, for complexes 5 and 6 with the strongest involvement of the carbonyl group in hydrogen bonding, the position of the amide I band is found at 1645 and 1622 cm −1 , respectively.A very similar conclusion can be drawn for the position and shape of the N-H band (Table 2).Finally, the IR spectra of all complexes showed C=N and C=C vibrations Scheme 1 Schematic representation of the synthesis of complexes 1-6 within the aromatic moiety of the pyridine and benzene rings in the relatively narrow region 1590-1622 cm −1 .Since these vibrations are relatively insensitive to the coordination to the metal centre, it is better to follow the shift of the bands corresponding to the in-plane pyridine ring deformation γ(CN) (619/633 cm −1 in N-methylnicotinamide), which are found in the range 647-652 cm −1 in our complexes, suggesting the coordination of the ligand to the copper atom through the pyridine nitrogen atom [51].
The solid state UV-Vis spectra of the studied monomeric complexes 1-6 exhibit a very similar pattern.The electronic spectra are shown in Fig. S13.As can be clearly seen (Fig. S13 right), these spectra show a broad asymmetric band with a maximum ranging from 618 nm (16,180 cm −1 ) for 3 to 690 nm (14,490 cm −1 ) for 6 in the visible region.This band corresponds to a spectroscopically forbidden electronic d-d transition from the predominantly d xy orbital to the d x 2 −y 2 orbital (Fig. S13).Such a d-d transition is typical for complexes with the CuO 4 N 2 (1)(2)(3)(4)(5) or CuO 5 N (6) chromophore with a tetragonally distorted octahedral environment around the copper(II) centre [54,55].Based on the position of the d-d peak in the spectrum, the complexes can be arranged as follows according to the observed tetragonal distortion around the copper atom: 3 (618 nm) > 5 (623 nm) > 1 (631 nm) > 2 (638 nm) > 4 (643 nm) > 6 (690 nm).The maximum of the d-d band in the case of complex 6 is found at the longest wavelength (690 nm) in this series of complexes, reflecting the presence of a lower ligand field around the copper ion as a result of a different chromophore (CuO 5 N) compared to the other complexes 1-5 (CuO 4 N 2 ).
In addition, the spectra also contain two bands at around 200-400 nm which could be considered as an intraligand transition (262-274 nm) and a ligand-to-metal charge transfer transition (shoulder at around 315-330 nm) between the π-electron cloud of an aromatic ligand moiety and a central copper atom [53,55].95-1.97Å and by a pair of neutral N-methylnicotinamide molecules that coordinates to the central atoms using pyridine ring nitrogen atom with Cu-N eq distances 2.02-2.04Å in trans positions (Table 3).Two water molecules with Cu-OW ax distances 2.49-2.57Å occupy axial positions.As a result of the presence of water molecules, the molecular structures of 1-5 are stabilised by intramolecular hydrogen bonds O1W-H1W•••O2 (the distances O1W•••O2 are in the range 2.66-2.74Å) (Table 4).The molecular structure of the molecular complex [Cu(2-NO 2 bz) 2 (mna) 2 (H 2 O) 2 ] in 1 and 2 is similar but differs in conformation and can therefore be considered as pseudopolymorphs.The angle between the plane of the nitro group and the plane of the carboxylate group of the 2-nitrobenzoate ligands in two pseudopolymorphs is 88.4° for 1 and 66.9° for 2 [56,57].

Molecular and crystal structures
The crystal structures of 1 and 3 are very similar, which simplifies the discussion of them.In the crystal structures of 1 and 3 (Fig. 2) are the molecules of [Cu(X-NO 2 bz) 2 (mna) 2 (H 2 O) 2 ] (X = 2 or 3) arranged into the layers, which are connected through a system of N2-H2N    8) supramolecular synthons (Fig. 2) [58].On the other hand, the two complex molecules of 1 or 3, linked by N2-H2N•••O1W ii hydrogen bonds, create R 2 2 (16) supramolecular synthons (Fig. 2) [58].The crystal structures of zinc(II) complexes of the formula [Zn(X-sal) 2 (mna) 2 (H 2 O) 2 ] (X-sal = 4-bromosalicylate, Fig. 1 Perspective views of 1-6 with the atom numbering scheme.Disordered parts are deleted for clarity 4-chlorosalicylate or 5-chlorosalicylate) exhibit similar hydrogen bonding systems [59], except for the fact that the nitrogen carboxamide atoms are not involved in hydrogen bonding.The stronger hydrogen bonding system involving water molecules and carboxylato oxygen atoms gave the shortest Cu•••Cu distances of 7.390(2) Å, and 7.307(3) Å for 1 and 3 respectively.The slightly weaker system with carboxamide groups resulted in the shortest Cu•••Cu distances of 8.890(2) Å, and 8.805(3) Å for 1 and 3 respectively, forming a rhombohedral grid of copper(II) atoms within the layers.These layers are held together by weak van der Waals forces in a zipper-like manner with weak π-π stacking interactions [60] between two benzene rings of 2-nitrobenzoate ligands in 1 (Fig. S14) and 3-nitrobenzoate ligands in 3 (Fig. S15), that are significantly stronger in the case of 1.The centroid-to centroid distance c g •••c g is 3.58 Å, and 4.16 Å for 1 and 3, respectively.
Symmetry codes: The crystal structure of 1 and 3 also shows π-π stacking interactions [60] between two pyridine rings of N-methylnicotinamide ligands with a centroid-to centroid distance c g •••c g of 3.94 Å (Fig. S16) and 3.84 Å (Fig. S17), respectively.The shortest interplanar Cu•••Cu distances are 12.082(2) Å, and 12.957(4) Å for 1 and 2, respectively.The crystal structures of pseudopolymorphs 1 and 2 differ in that 2 contains uncoordinated lattice water molecules which are involved in hydrogen bonding.As a result, the hydrogen-bonding networks in the complex 2 (Fig. 2) are enriched.The same situation applies to complex 4 (Fig. 2).Squeezing the uncoordinated water molecules into hydrogen-bonding networks increases the number of O-H•••O hydrogen bonds connected to the rings, but there is a big difference in the involvement of the water molecules.Both complexes 2 and 4 create R 2 2 (16) supramolecular synthons held by hydrogen bonding between coordinated water molecules and N-methylnicotinamide ligands (Fig. 2), but in two different ways.In complex 2, the supramolecular synthons R 2 2 (16) are formed between hydrogen atoms H2W of coordinated water molecules O1W and oxygen O2 acceptors of N-methylnicotinamide    12) supramolecular synthons [58].But again there is a big difference between the two complexes and the connections of uncoordinated and coordinated water represent two alternatives of R 6 4 (12) ring formation.The R 6 4 (12) rings of 2 (Fig. 2) are created through O2W-H3W (6); 2.726(7) and 2.738(7) Å, respectively; symmetry code: (iv) − x + 2, − y + 1, − z + 1].The R 6 4 (12) rings of 4 (Fig. 2) are formed through O1W-H2W (7); 2.762(7) and 2.730(7) Å, respectively; symmetry code: (i) − x, − y + 1, − z + 1].Consequently, the uncoordinated water molecules O2W and complex molecules of both complexes 2 and 4 are connected to R 2 2 (10) rings (Fig. 2) through two different alternatives of hydrogen bonds N2-H2N and R 2 2 (10) patterns of 2 and 4 (Fig. 2) represent two alternatives of hydrogen bonding network formation resembling supramolecular isomerism [61].The involvement of uncoordinated water molecules in the formation hydrogen bonds together with coordinated water molecules resulted in the weakening of the shortest Cu•••Cu distance to 8.276(2) Å for 2 and to 8.722(5) Å for 4 compared to the previous pair of complexes.On the other hand, the Cu•••Cu distances of the copper atoms connected via R 2 2 (16) supramolecular synthons remain quite similar (8.762(2)Å for 2 and 8.780(5) Å for 4, respectively).The formation of these hydrogen bonded rhombohedra grids of copper(II) atoms has resulted in the layers being close together.Moreover, those grid layers are similar in that their nitrobenzoate rings protrude from the layers, thus limiting interlayer contacts.The π-π stacking contacts between two benzene rings of 2-nitrobenzoate ligands in 2 (Fig. S18) are also weaker due to the distances mentioned, and the shortest centroid-to centroid distance c g •••c g is 3.75 Å [60].The crystal structures of 2 and 4 also show weaker π-π stacking interactions between two pyridine rings of N-methylnicotinamide ligands with centroid-to centroid distances c g •••c g of 3.87 Å (Fig. S19), and 3.76 Å (Fig. S20).

Hirshfeld surface analyses
Hirshfeld surface analysis was used to further study the intermolecular interactions of the crystal structures of all compounds.For the illustration, Fig. 5 shows the 3D Hirshfeld surface of 5.The 3D Hirshfeld surface of other complexes are illustrated in supplementary material (Figs.S24-S28).The 3D Hirshfeld surfaces have been mapped over d norm shape index (Fig. 5

EPR spectroscopy
Experimental room temperature powder EPR spectra of studied complexes exhibit features typical of an S = ½ system with axial symmetry (Fig. 6).Furthermore, the EPR spectra of 5-6 contain well resolved hyperfine splitting in a parallel part of the signal, whereas the EPR spectra of 1-4 show only the axial type of EPR line without significant hyperfine splitting.The EPR spectra were analysed using the spin Hamiltonian in an axial form [65] and the resulting simulated spin Hamiltonian parameters are summarised in Table 5.
As can be seen from Table 5, the data obtained (g ⊥ , g || and A || ) are typical for copper in the tetragonal bipyramidal arrangement [66].In addition, the values of the g factors satisfy the relation g || > g ⊥ > 2.0023, which is consistent with the d x 2 − y 2 ground electronic state.The main difference in the EPR spectra is the observation of hyperfine splitting in 5-6 in contrast with 1-4.This observation could be explained by the presence of a different structural arrangement of the paramagnetic centres in accordance with the X-ray data.The complex molecules of 1-4 are arranged in such a way that allows the copper atoms to come closer together resulting in higher half-width of the EPR signal and poorer resolution.Unlike the crystal packing in complexes 5-6 separates well the individual paramagnetic centers, allowing hyperfine splitting to be observed.Eventually, some other EPR parameters derived from the spin Hamiltonian parameters such as the average g factor g ave , the geometrical parameter, G [66] and the empirical f factor [67] were also calculated and collected in the Table 5.If the value of the G parameter is G > 4 (2-5), then a negligible interaction between the Cu(II) centers is assumed [66].On the contrary, in the case of 1 and 6 there is some exchange interaction between the copper   centers as can be clearly seen from the larger half-width of the EPR signal (Fig. 6).Values of the f factor which characterises a degree of tetrahedral distortion of the tetragonal plane have been calculated for the complexes with resolved parallel hyperfine splitting (5)(6) The values obtained (142 and 134 cm) support the suggestion of a square planar geometry around the copper ions with elongated tetragonal distortion [67].

Calculation of g and A constant
The EPR parameters of complexes 5-6 were further studied and analysed by means of DFT calculations.The geometry of the studied complexes (5-6) was at first optimised with the BP86 functional with Grimme dispersion correction D3BJ on the experimental geometries.Since the obtained optimised geometries show a good agreement when compared with single-crystal X-ray diffraction data, we can expect the geometry optimisation to be reasonable accurate for predicting the EPR spin Hamiltonian parameters.Using the optimised structures a molecular g and copper A tensors were computed using two different density functionals: B3LYP and TPSSh.In any case, the DFT calculated g values are still in good qualitative agreement with the parameters obtained from the simulation of the experimental EPR spectra.This can be clearly seen by comparing the average g ave values between experiment and calculation (Table 6).The underestimation of the DFT computed g values in copper (II) complexes with tetragonal symmetry has also been observed by the other authors [68,69].Examination of the calculated copper A || values (Table 6) revealed very good agreement with experimental values, especially for the B3LYP functional.
In this case, we obtain the value of hyperfine splitting constant |A || |= 477 and 543 MHz for 5 and 6 and experimentally extracted values are |A || |= 487 and 522 MHz.The hyperfine interaction tensor A || is calculated as the sum of three different energy contributions: a) the contribution from the isotropic Fermi contact interaction A FC , b) the contribution from the spin-dipole interaction A SD , c) the contribution from the spin-orbital interaction A SO [44,45].The theoretical calculation therefore allows us to get a detailed view of how each member contributes to the resulting value of the hyperfine constant (Table 6) [70].In the case of the 5 (B3LYP), the individual contributions were as follows: A FC = − 220 MHz, A SD = − 528 MHz and A SO = 271 MHz.Thus, the dominant contribution to the hyperfine interaction in the studied tetragonal copper(II) complexes is the contribution from the spin-dipole interaction.

Conclusion
In conclusion, we have synthesised and fully characterised six copper(II)nitrobenzoate complexes with N-methylnicotinamide.The crystal structures of the studied complexes show tetragonal bipyramidal stereochemistry around the Cu(II) ions with monodentate coordinated nitrobenzoate, N-methylnicotinamide and water ligands.The crystal packing in the crystal structures of the studied complexes shows several hydrogen-bonded supramolecular arrangements mostly due to the presence of coordinated and uncoordinated lattice water and N-methylnicotinamide molecules.In addition, Hirshfeld surface and the fingerprint plot analysis were used to quantify the contributions of each noncovalent interaction in the supramolecular structures and the final results confirm the assertion that the hydrogen bonding interactions are the most important noncovalent interactions in stabilising the net supramolecular assemblies.EPR spectra of polycrystalline samples show a monomeric signal of axial symmetry either without (1-4) or with resolved copper hyperfine splitting (5-6) for all studied complexes.The simulated spin Hamiltonian parameters are consistent with a distorted tetragonal geometry around the copper centre as was confirmed by X-ray structural data.DFT calculations of the values of the molecular g tensor and hyperfine constant A || using B3LYP density functional show a good accordance with the experimental parameters.
a part of the Slovak Infrastructure of High Performance Computing (SIVVP project, ITMS code 26230120002, funded by the European region development funds, ERDF), for the computational time and resources made available.This publication was also created on the basis of the major project "Advancing University Capacity and Competence in Research, Development and Innovation" (ITMS project code: 313021X329) supported by Operational Programme Integrated Infrastructure and funded by the European Regional Development Fund.

T h e c 1 .
e n t r o s y m m e t r i c m o l e c u l e s [ C u ( X-NO 2 bz) 2 (mna) 2 (H 2 O) 2 ] of compounds 1-5 are very similar.The molecular structures of complexes 1-5 are depicted in Fig.The coordination environment around Cu(II) atoms in the 1-5 adopts tetragonal-bipyramidal (4+2) stereochemistry.The tetragonal plane in the complexes is formed by a pair of monodentately coordinated carboxylate anions with Cu-O eq distances 1.

Fig. 3 5 Fig. 4
Fig. 3 Hydrogen bonding network in crystal structure of 5 and Figs.S24-S28).The surfaces are shown in a transparent manner to allow visualization of the molecular moiety around which they were calculated.As shown in the Fig. 5 as well as in Figs.S24-S28, the deep red spots on the d norm Hirshfeld surfaces indicate the close-contact interactions, which are mainly responsible for the significant intermolecular hydrogen bonding interactions.The 3D Hirshfeld surface illustration of 5 (Fig. 5) and the others (Fig. S24-S28) show the deep red areas representing O-H•••O and N-H•••O hydrogen bonds and also weaker C-H•••O hydrogen bonding interactions.The Hirshfeld 2D fingerprint of all compounds are illustrated in supplementary material (Figs.S29-S34).The Hirshfeld 2D fingerprint plots allow a quick and easy identification of the significant intermolecular interactions map on the molecular surface[63,64].As shown in Figs.S29-S34, the strong and medium H•••O/O•••H hydrogen bonding interactions cover the 33.5-41.6%range of the total Hirshfeld surface with two distinct spikes in the 2D fingerprint plots, indicating that the hydrogen bonding interactions are the most significant noncovalent interactions in the crystal.In addition, in the middle of scattered points in the 2D fingerplots, H•••H interactions cover 16.8-41.2%range of the total Hirshfeld surface.In scattered points of the 2D fingerplots, H•••C/C•••H interactions cover in the range 9.3-18.3% of the total Hirshfeld surface.

Fig. 5
Fig. 5 View of the three-dimensional Hirshfeld surface of 5 plotted over d norm (top) in the range − 0.7486 to 1.3577 a. u. and plotted over the shape index (bottom) showing π-π stacking interactions

Table 3
Selected geometric parameters

Table 4
Selected hydrogen-bond parameters

Table 5
Selected EPR spectra parameters Table 6 shows the experimental and calculated values of g ⊥ , g || , g ave and A || .Although the calculations of the EPR parameters are done in vacuo, the calculated molecular values of g ⊥ and g || well reproduce the experimentally observed relation of g || > g ⊥ > 2.0023 in case of both functionals used.Analyzing the data in Table 6 we can see, that both functionals underestimate the values of g factors either g || or g ⊥ whereby the trend is higher in the case of g || .A better estimate is obtained for the B3LYP functional.