The Methylene Spacer Matters: The Structural and Luminescent Effects of Positional Isomerism of n-Methylpyridyltriazole Carboxylate Semi-Rigid Ligands in the Structure of Zn(II) Based Coordination Polymers

Two Zn(II) coordination polymers (CPs) based on n-methylpyridyltriazole carboxylate semi-rigid organic ligands (n-MPTC), with n = 3 (L1) and 4 (L2), have been prepared at the water n-butanol interphase by reacting Zn(NO3)2·4H2O with NaL1 and NaL2. This allows us to systematically investigate the influence of the isomeric positional effect on their structures. The organic ligands were obtained by saponification from their respective ester precursors ethyl-5-methyl-1-(pyridin-3-ylmethyl)-1H-1,2,3-triazole-4-carboxylate (P1) and ethyl-5-methyl-1-(pyridin-4-ylmethyl)-1H-1,2,3-triazole-4-carboxylate (P2), resulting in their corresponding sodium salt forms, 3-MPTC, and 4-MPTC. The structure of the Zn(II) CPs determined by single-crystal X-ray diffraction reveals that both CPs have 2D supramolecular hydrogen bond networks. The 2D supramolecular network of [Zn(L1)]n (1) is built up by hydrogen bond interactions between oxygen and hydrogen atoms between neighboring n-methylpyridyltriazole molecules, whereas in [Zn(L2)·4H2O]n (2) the water molecules link 1D polymeric chains forming a 2D supramolecular aggregate. The structures of 1 and 2 clearly show that the isomeric effect in the semi-rigid ligands plays a vital role in constructing the Zn(II) coordination polymers, helped by the presence of the methylene spacer group, in the final structural conformation. The structures of 1 and 2 significantly affect their luminescent properties. Thus, while 2 shows strong emission at room temperature centered at 367 nm, the emission of 1 is quenched substantially.

On the other hand, the CPs with general formulae, [Zn(L1)]n (1) and [Zn(L2)•4H2O]n (2), were obtained following a similar process to that which has been previously described in the literature [45] (The slow diffusion of the solution of the reactants, NaL and Zn(NO3)2•4H2O, in immiscible solvents (n-BuOH/H2O), resulted in the formation at the interphase of single crystals of 1 and 2 suitable for SC-XRD analysis (Scheme 2)). In general, both compounds were obtained with a moderate yield (30 and 40%, respectively). On the other hand, the CPs with general formulae, [Zn(L1)] n (1) and [Zn(L2)·4H 2 O] n (2), were obtained following a similar process to that which has been previously described in the literature [45] (The slow diffusion of the solution of the reactants, NaL and Zn(NO 3 ) 2 ·4H 2 O, in immiscible solvents (n-BuOH/H 2 O), resulted in the formation at the interphase of single crystals of 1 and 2 suitable for SC-XRD analysis (Scheme 2)). In general, both compounds were obtained with a moderate yield (30 and 40%, respectively). Moreover, both compounds are stable to moisture and common atmospheric conditions and exhibit good thermal stability until 350 • C (Figure 8). Both CPs are insoluble in common organic solvents and water at room temperature. Scheme 1. General synthetic route of ligands NaL1 and NaL2.
On the other hand, the CPs with general formulae, [Zn(L1)]n (1) and [Zn(L2)•4H2O]n (2), were obtained following a similar process to that which has been previously described in the literature [45] (The slow diffusion of the solution of the reactants, NaL and Zn(NO3)2•4H2O, in immiscible solvents (n-BuOH/H2O), resulted in the formation at the interphase of single crystals of 1 and 2 suitable for SC-XRD analysis (Scheme 2)). In general, both compounds were obtained with a moderate yield (30 and 40%, respectively). Moreover, both compounds are stable to moisture and common atmospheric conditions and exhibit good thermal stability until 350 °C (Figure 8). Both CPs are insoluble in common organic solvents and water at room temperature. Scheme 2. General synthetic route of compounds 1 and 2.

Crystallographic Studies
The powder X-ray patterns of 1 and 2 were indexed in monoclinic cells, which were corroborated by the X-ray single-crystal results. For each compound, a Rietveld refinement [46] was carried out using the Fullprof program [47] to check the structural parameters. Figure S1 shows the perfect fit between the observed and calculated patterns. These results verify the phase purity of the crystalline samples and that the single crystals studied are representative of the bulk samples.
The single-crystal X-ray diffraction method established the crystal structures and chemical compositions of all compounds. The molecular structures of L1 and L2 are shown in their ester forms P1 and P2 ( Figure 1). P1 crystallizes in the monoclinic system with space group P21/c, and P2 crystallizes in an orthorhombic system with space group P212121, with both compounds having four molecular entities per unit cell with centrosymmetric and non-centrosymmetric settings, respectively. All the bond lengths and angles fall in the expected range for related compounds [48]. The C1-C6-N2 torsion angle for P1 and P2, 112.80 (19) and 113.1(2)°, respectively, shows a loss of coplanarity from the related heterocycles (n-pyridyl and 1,2,3-triazole moieties), 66.72 (11) and 97.99(11)°, respectively. This is because the presence of the CH2 group allows a significant torsion angle between Scheme 2. General synthetic route of compounds 1 and 2.

Crystallographic Studies
The powder X-ray patterns of 1 and 2 were indexed in monoclinic cells, which were corroborated by the X-ray single-crystal results. For each compound, a Rietveld refinement [46] was carried out using the Fullprof program [47] to check the structural parameters. Figure S1 shows the perfect fit between the observed and calculated patterns. These results verify the phase purity of the crystalline samples and that the single crystals studied are representative of the bulk samples.
The single-crystal X-ray diffraction method established the crystal structures and chemical compositions of all compounds. The molecular structures of L1 and L2 are shown in their ester forms P1 and P2 ( Figure 1). P1 crystallizes in the monoclinic system with space group P2 1 /c, and P2 crystallizes in an orthorhombic system with space group P2 1 2 1 2 1 , with both compounds having four molecular entities per unit cell with centrosymmetric and non-centrosymmetric settings, respectively. All the bond lengths and angles fall in the expected range for related compounds [48]. The C1-C6-N2 torsion angle for P1 and P2, 112.80 (19) and 113.1(2) • , respectively, shows a loss of coplanarity from the related heterocycles (n-pyridyl and 1,2,3-triazole moieties), 66.72 (11) and 97.99(11) • , respectively. This is because the presence of the CH 2 group allows a significant torsion angle between their heterocycles concerning similar compounds previously reported with the same moieties [49]. The main difference between both compounds is the orientation of the pyridyl fragment relative to the triazole-carboxylate moiety. The torsion angles C2/C1/C6/N2 are 75.7(2) and 22.2(4) • for P1 and P2, respectively. Another significant difference between them is the position of the carbonyl group relative to a methyl group, cis in P1, and trans in P2, which in P1 is stabilized by a C-H···O intramolecular hydrogen bond interaction with graph-set notation S(6) [50]. their heterocycles concerning similar compounds previously reported with the same moieties [49]. The main difference between both compounds is the orientation of the pyridyl fragment relative to the triazole-carboxylate moiety. The torsion angles C2/C1/C6/N2 are 75.7(2) and 22.2(4)° for P1 and P2, respectively. Another significant difference between them is the position of the carbonyl group relative to a methyl group, cis in P1, and trans in P2, which in P1 is stabilized by a C-H‧•‧O intramolecular hydrogen bond interaction with graph-set notation S(6) [50].   In the crystal structure of P2 (Figure 3), the molecules are linked by C11-H11CN1 i hydrogen bonds forming a zig-zag chain along the [001] direction with graph-set notation C (13). Further, these chains are linked to neighbor chains through C(  . Thermal ellipsoids represent a 30% probability. Hydrogen atoms were omitted for the sake of clarity. Figure 2 shows intermolecular C(4)-H(4)···O(1) i hydrogen bond interactions that give rise to centrosymmetric dimers with a graph-set notation [50] along the crystal structure of P1.
their heterocycles concerning similar compounds previously reported with the same moieties [49]. The main difference between both compounds is the orientation of the pyridyl fragment relative to the triazole-carboxylate moiety. The torsion angles C2/C1/C6/N2 are 75.7(2) and 22.2(4)° for P1 and P2, respectively. Another significant difference between them is the position of the carbonyl group relative to a methyl group, cis in P1, and trans in P2, which in P1 is stabilized by a C-H‧•‧O intramolecular hydrogen bond interaction with graph-set notation S(6) [50].   In the crystal structure of P2 (Figure 3), the molecules are linked by C11-H11CN1 i hydrogen bonds forming a zig-zag chain along the [001] direction with graph-set notation C (13). Further, these chains are linked to neighbor chains through C(  In the crystal structure of P2 (Figure 3), the molecules are linked by C11-H11C···N1 i hydrogen bonds forming a zig-zag chain along the [001] direction with graph-set notation C (13). Further, these chains are linked to neighbor chains through C (12) The molecular structure of 1 and 2 with the coordination environment of the Zn(II) atom was confirmed by single-crystal X-ray diffraction ( Figure 4). In detail, for 1, the Zn(II) ion is set on inversion centers that were chelated by one triazole-carboxylate ligand. Two nitrogen symmetry-related atoms of the triazole and pyridyl fragments build the equatorial plane around the Zn(II) ions for 1 (Zn1−N4 2.151(3) Å, Zn1−N1 2.297 (3) Å). Meanwhile, the central Zn(II) ion also was coordinated by two oxygen symmetry-related atoms from carboxylate fragments at the equatorial axial positions (Zn1−O1 2.044(2) Å), giving rise to its octahedral geometry, with the trans-N4O2 configuration. For compound 2, the Zn (II) ion is located on a two-fold-axis, that was chelated by one triazole-carboxylate ligand. Two nitrogen symmetry-related atoms of the triazole and pyridyl fragment build the equatorial plane around the Zn(II) ions (Zn1−N4 2.166(3) Å, Zn1−N1 2.142 (3) Å). Meanwhile, the central Zn(II) ion also was coordinated by two oxygen symmetry-related atoms from carboxylate fragments at the axial positions (Zn1−O1 2.151(2) Å), giving rise to its octahedral geometry, with the cis-N4O2 configuration. The N-Zn-N and O-Zn-O bond angles are in the ranges 83.00(9)-97.00(9)/88.70(16)-163.94(12)°;180/174.64(12)° for 1 and 2, respectively. The bond distances and angles of 1 and 2 (Tables S1 and S2) are similar to showing the crystal packing. The hydrogen atoms not involved in hydrogen bond interaction were removed. Thermal ellipsoids were drawn with a 30% probability (symmetry code: The molecular structure of 1 and 2 with the coordination environment of the Zn(II) atom was confirmed by single-crystal X-ray diffraction ( Figure 4). In detail, for 1, the Zn(II) ion is set on inversion centers that were chelated by one triazole-carboxylate ligand. Two nitrogen symmetry-related atoms of the triazole and pyridyl fragments build the equatorial plane around the Zn(II) ions for 1 (Zn1−N4 2.151(3) Å, Zn1−N1 2.297 (3) Å). Meanwhile, the central Zn(II) ion also was coordinated by two oxygen symmetry-related atoms from carboxylate fragments at the equatorial axial positions (Zn1−O1 2.044(2) Å), giving rise to its octahedral geometry, with the trans-N 4 O 2 configuration. For compound 2, the Zn (II) ion is located on a two-fold-axis, that was chelated by one triazole-carboxylate ligand. Two nitrogen symmetry-related atoms of the triazole and pyridyl fragment build the equatorial plane around the Zn(II) ions (Zn1−  . The hydrogen atoms were omitted. Thermal ellipsoids were drawn with a 30% probability. In 1 and 2, the structural analysis also revealed the presence of [2+2] polymeric metallocycle complexes with two ligand molecules coordinated to a pair of symmetry-related Zn(II) ions, resulting in the formation of 16-membered metallo-cyclic rings, and then forming a rhomboid fashion, with a cross-sectional area of 30.68 and 38.77 Å 2 ( Figure 5). The so-formed metallocycles show different coordination modes due to the isomeric effect of the ligand over the metal center (cis and trans for 1 and 2, respectively). This effect is also reflected in the orientation of the triazole and n-pyridyl rings, concerning the rhomboid shape, meaning the plane generated by Zn1 and C6 atoms and their symmetry-related homologs atoms in each compound. The dihedral angles between the metallacycle mean plane and the triazole ring are 65.34 (10) and 84.79(12)°, respectively. Likewise, the dihedral angles between the metallacycle mean plane and the n-pyridyl rings are 68.73 (18)   The hydrogen atoms were omitted. Thermal ellipsoids were drawn with a 30% probability.
In 1 and 2, the structural analysis also revealed the presence of [2+2] polymeric metallocycle complexes with two ligand molecules coordinated to a pair of symmetryrelated Zn(II) ions, resulting in the formation of 16-membered metallo-cyclic rings, and then forming a rhomboid fashion, with a cross-sectional area of 30.68 and 38.77 Å 2 ( Figure 5). The so-formed metallocycles show different coordination modes due to the isomeric effect of the ligand over the metal center (cis and trans for 1 and 2, respectively). This effect is also reflected in the orientation of the triazole and n-pyridyl rings, concerning the rhomboid shape, meaning the plane generated by Zn1 and C6 atoms and their symmetry-related homologs atoms in each compound. The dihedral angles between the metallacycle mean plane and the triazole ring are 65.34 (10)

Luminescent Properties
The room temperature solid-state emission spectra, emission data, and electronic absorption of NaL1, NaL2, 1, and 2 are shown in Figure 7 and Table 1. These crystalline solids have interesting luminescent properties, with significant differences in their spectra.
Thus, compounds NaL1 and NaL2 show significant differences in their emission intensity and a large redshift, Δλ = 41 nm, between NaL1 and NaL2. These differences are attributable to their isomerism and the bonding mode with the Na(I) counterion. It is wellknown that the ionic strength in the luminescent ionic compounds can quench the emission response [51]. Therefore, it can be assumed that the difference in the intensity and the shift in the emission band between NaL1 and NaL2 is due to the interaction between the sodium counterion and the ligand. On the other hand, as the emission bands for the NaL1 and NaL2 are around 420-450 nm, the involved transitions are mainly π-π*. Moreover, at about 630 nm, a small band is observed in NaL2, which can be attributable to counterionligand charge transfer (XLCT), supporting the hypothesis of the decrease of the intensity emission maximum between NaL1 and NaL2 [31]. (2), the water molecules link a 1D polymeric chain forming a 2D supramolecular aggregate. A 1D polymeric chain is linked to the neighboring chain by O1S-H1SB···O1 and O1S-H1SB···O2, generating (4) non-centrosymmetric rings (labeled A); O1S-H1SB···O1 and O1S-H1SA···O1, generating (8) centrosymmetric rings (labeled B); O1S-H1SB···O1; and O1S-H1SB···O2 and O2S-H2SB···O1S, generating (19) centrosymmetric rings (labeled C) ( Figure 6). The water molecules are linked to form a tetrameric aggregate by O2S-H2SB···O1S and O2S-H2SA···O1S hydrogen bond interactions, generating a (8) centrosymmetric ring (labeled D) ( Figure 5). These four types of rings alternate in an ABACDC fashion to form a two-dimensional supramolecular aggregate ( Figure 6 and Table S5).

Luminescent Properties
The room temperature solid-state emission spectra, emission data, and electronic absorption of NaL1, NaL2, 1, and 2 are shown in Figure 7 and Table 1. These crystalline solids have interesting luminescent properties, with significant differences in their spectra. ergy loss by the nonradiative decay of the intra-ligands excited states [52]. The structures 1 and 2 show emission bands centered at 367 and 366 nm, respectively (Figure 7). However, 2 has a more significant luminescent response (~1000 times greater). As explained above, the difference in intensities is due to the rigidity that the metal ion contributes to the formation of these systems. The presence of electronically saturated d 10 ions, such as Zn(II), are appropriate, because they impose conformational rigidity to the ligand prevent energy loss via bond vibration or electron transfer processes [53,54]. Although both ligands are relatively similar, the isomeric positional effect can generate the difference in the coordination modes over the metal center (cis versus trans) that may contribute to a loss of intensity. The centrosymmetric setting 1 may be less favorable in the luminescent response than 2, due to the Zn(II) ion bond distances being smaller in 1 than in 2 (Table S1), generating a possible quenching by the concentration in the solid state of the different distances between Zn (II) ions that could effect this [55,56].

Thermogravimetry (TG) Analyses
The thermogravimetric analyses of NaL1, NaL2, 1, and 2 were recorded with a heating rate of β = 10 °C•min −1 under a dynamic nitrogen atmosphere at 20-700 °C. All curves are shifted to a higher temperature at a constant heating rate. NaL1 and NaL2 are stable up to ca. 322 and 306 °C, respectively. After these temperatures, the progressive decomposition of the ligands occurred. The organic fragments completely decompose at 462 °C with a loss of 49% weight for NaL1, and 630 °C with a  Thus, compounds NaL1 and NaL2 show significant differences in their emission intensity and a large redshift, ∆λ = 41 nm, between NaL1 and NaL2. These differences are attributable to their isomerism and the bonding mode with the Na(I) counterion. It is wellknown that the ionic strength in the luminescent ionic compounds can quench the emission response [51]. Therefore, it can be assumed that the difference in the intensity and the shift in the emission band between NaL1 and NaL2 is due to the interaction between the sodium counterion and the ligand. On the other hand, as the emission bands for the NaL1 and NaL2 are around 420-450 nm, the involved transitions are mainly π-π*. Moreover, at about 630 nm, a small band is observed in NaL2, which can be attributable to counterion-ligand charge transfer (XLCT), supporting the hypothesis of the decrease of the intensity emission maximum between NaL1 and NaL2 [31].
In 1 and 2, a different situation is observed compared with their respective ligands. For instance, the metal coordination clearly produces red shifting and intensity changes. These changes are due to the chelation of the metal center that generates an increase in the rigidity of the respective coordination polymers. These structural constraints avoid energy loss by the nonradiative decay of the intra-ligands excited states [52]. The structures 1 and 2 show emission bands centered at 367 and 366 nm, respectively (Figure 7). However, 2 has a more significant luminescent response (~1000 times greater). As explained above, the difference in intensities is due to the rigidity that the metal ion contributes to the formation of these systems. The presence of electronically saturated d 10 ions, such as Zn(II), are appropriate, because they impose conformational rigidity to the ligand prevent energy loss via bond vibration or electron transfer processes [53,54]. Although both ligands are relatively similar, the isomeric positional effect can generate the difference in the coordination modes over the metal center (cis versus trans) that may contribute to a loss of intensity. The centrosymmetric setting 1 may be less favorable in the luminescent response than 2, due to the Zn(II) ion bond distances being smaller in 1 than in 2 (Table S1), generating a possible quenching by the concentration in the solid state of the different distances between Zn (II) ions that could effect this [55,56].

Thermogravimetry (TG) Analyses
The thermogravimetric analyses of NaL1, NaL2, 1, and 2 were recorded with a heating rate of β = 10 • C·min −1 under a dynamic nitrogen atmosphere at 20-700 • C. All curves are shifted to a higher temperature at a constant heating rate.
NaL1 and NaL2 are stable up to ca. 322 and 306 • C, respectively. After these temperatures, the progressive decomposition of the ligands occurred. The organic fragments completely decompose at 462 • C with a loss of 49% weight for NaL1, and 630 • C with a loss of 57% for NaL2. The black color residue remains at the end of the heating process and contains Na 2 O and carbonaceous matter (Figure 8).
Polymers 2023, 15, x FOR PEER REVIEW 10 of 17 loss of 57% for NaL2. The black color residue remains at the end of the heating process and contains Na2O and carbonaceous matter (Figure 8).
In the case of 1, the TG curves show a four-step weight loss until total decomposition, starting at ca. 30 °C, with a total deterioration of over 500 °C. The first step corresponds to the loss of two water molecules due to moisture in the sample (~6%). In the second step at 300 °C, the decarboxylation from the ligand was found (~8%). The two following steps correspond to the progressive decomposition of the compound. The TG of 2 shows a twostep decomposition curve. The first one at ~110 °C represents a weight loss of 5% (two water molecules). The second step at ca. 290 °C corresponds to the progressive decomposition of the organic ligand. After the total disintegration of both CPs, the final compounds correspond to ZnO and carbonaceous material (Figure 8 and see Figure S2, for more details).

Materials and General Procedures
All reagents used were purchased from Sigma-Aldrich (Sigma-Aldrich, St. Louis, MO, USA) and used without further purification.

Characterization
FT-IR spectra in the range 400-4000 cm −1 were recorded on a Nicolet Avatar 300 spectrometer (Thermo Scientific,Waltman, MA, USA) using KBr pellets. NMR spectra were recorded at 298 K with a Bruker Avance III-HD Nanobay 300 MHz (Bruker Co.; Billerica, MA, USA). All NMR spectra are reported in parts per million (ppm, d) relative to tetramethylsilane (Me4Si) for 1H and 13C NMR spectra, with the residual solvent proton and carbon resonances used as internal standards, depicted in Figures S1 and S2, respectively. Coupling constants (J) are reported in hertz (Hz), and integrations are reported as the number of protons. The following abbreviations are used to describe peak patterns: s = singlet, d = doublet, t = triplet, m = multiplet, br = broad. High-resolution electrospray ionization mass spectra (ESI-MS) were obtained on a Thermo Fisher scientific ultimate 3000 y Q exactive focus mass spectrometer (Thermo Scientific, Waltman, MA, USA) and the results are expressed in a mass/charge ratio (m/z) in a positive mode and depicted in In the case of 1, the TG curves show a four-step weight loss until total decomposition, starting at ca. 30 • C, with a total deterioration of over 500 • C. The first step corresponds to the loss of two water molecules due to moisture in the sample (~6%). In the second step at 300 • C, the decarboxylation from the ligand was found (~8%). The two following steps correspond to the progressive decomposition of the compound. The TG of 2 shows a two-step decomposition curve. The first one at~110 • C represents a weight loss of 5% (two water molecules). The second step at ca. 290 • C corresponds to the progressive decomposition of the organic ligand. After the total disintegration of both CPs, the final compounds correspond to ZnO and carbonaceous material (Figure 8 and see Figure S2, for more details).

Materials and General Procedures
All reagents used were purchased from Sigma-Aldrich (Sigma-Aldrich, St. Louis, MO, USA) and used without further purification.

Characterization
FT-IR spectra in the range 400-4000 cm −1 were recorded on a Nicolet Avatar 300 spectrometer (Thermo Scientific,Waltman, MA, USA) using KBr pellets. NMR spectra were recorded at 298 K with a Bruker Avance III-HD Nanobay 300 MHz (Bruker Co.; Billerica, MA, USA). All NMR spectra are reported in parts per million (ppm, d) relative to tetramethylsilane (Me4Si) for 1H and 13C NMR spectra, with the residual solvent proton and carbon resonances used as internal standards. Coupling constants (J) are reported in hertz (Hz), and integrations are reported as the number of protons. The following abbreviations are used to describe peak patterns: s = singlet, d = doublet, t = triplet, m = multiplet, br = broad. High-resolution electrospray ionization mass spectra (ESI-MS) were obtained on a Thermo Fisher scientific ultimate 3000 y Q exactive focus mass spectrometer (Thermo Scientific, Waltman, MA, USA) and the results are expressed in a mass/charge ratio (m/z) in a positive mode. The thermogravimetry (TG) analyses were carried out on a STA 448 Jupiter F3 type simultaneous thermal analyzer (Netzsch, MA, USA). For TG, 6 mg of the samples were used as microcrystalline powders. The used sample cells were aluminum oxides pans. The parent reagents were heated up to 700 • C at a heating rate of 10 • C min −1 under a flow of nitrogen at 20 mL min −1 . Excitation (PLE) and emission (PL) spectra were measured at room temperature using a Jasco FP-8500 spectrofluorometer with a 150 W xenon lamp as the excitation. The luminescence spectra were recorded on a JASCO FP-8500 spectrofluorometer JASCO Co.; Kyoto, Japan) in the solid-state at room temperature. The excitation was performed with λex = 250-400 nm, and the emission was recorded at λem = 400-750 nm. All spectra were measured with 0.05 mmol of each compound.

X-ray Powder Diffraction
The X-ray powder diffraction diffractograms of complexes 1 and 2 were collected at room temperature, in a Panalytical X'Pert Pro automated diffractometer (Malvern Panalytical, Moreira, Portugal) equipped with an X'celerator detector by using CuKα radiation (λ = 1.54177 Å). The diffractometer was operated at 40 kV and 40 mA in θ/θ reflection mode. The powder patterns were scanned in the range of 2θ = 5-50 • , with a step size of 0.02 • and a counting time of 20 s per step ( Figure S1).

Single-Crystal X-ray Diffraction
Some suitable single crystals of each compound were measured. Their diffraction data were collected at 293-295 K on a Bruker D8 Venture diffractometer equipped with a bidimensional CMOS Photon 100 detector, using graphite monochromated Cu-Kα (λ = 1.54178 Å) radiation. The diffraction frames were integrated using the APEX3 package [57] and were corrected for absorptions with SADABS. The structures of all compounds were solved by intrinsic phasing [58] using the OLEX 2 program [59]. The structures were then refined with full-matrix least-squares methods based on F 2 (SHELXL-2014) [58]. For the four compounds, non-hydrogen atoms were refined with anisotropic displacement parameters. All hydrogen atoms were included in their calculated positions, assigned fixed isotropic thermal parameters, and constrained to ride on their parent atoms. A summary of the details about crystal data, collection parameters, and refinement are documented in Table 2, and additional crystallographic details are provided in the CIF files. ORTEP views were drawn using OLEX2 software [59].

General Procedure Syntheses for 1D CPs [Zn(L1)]n (1) and [Zn(L2)·4H 2 O]n (2)
A solution of Zn(NO 3 ) 2 ·4H 2 O (34 mg, 0.115 mmol) in n-butanol (5 mL) was slowly added over an aqueous solution of NaL (NaL1 or NaL2) (5 mL, 5 mg, 0.230 mmol). The resulting mixture was stored at room temperature for two weeks. Then, the formation of crystals suitable for SC-XRD analysis from the interphase occurred. The crystals were collected by hand and air dried.  ). The X-ray powder diffractions of 1 and 2 confirm that the powders and single crystals have the same structural phase ( Figure S1).

Conclusions
In summary, two new CPs with the semi-rigid n-methylpyridyltriazole carboxylate ligands, with n = 3 (L1) and 4 (L2), have been prepared at the water/n-butanol interphase by reacting Zn(NO 3 ) 2 ·4H 2 O with NaL1 and NaL2. Their X-ray structures confirm the formation of two 1D coordination polymers in which the flexibility of the methyl group and the change in the N-donor portion of the pyridyl entity n-methylpyridyltriazole carboxylate ligands coordinate to the metal center in a cis versus trans conformation, giving rise to the formation of rather different H-bond supramolecular networks. Remarkably, 2 shows a strong emission centered at 367 nm at room temperature. The structural differences result in the centrosymmetric setting 1 being less favorable in the luminescent response than 2, due to the different distances between Zn (II) ions that could cause a quenching by concentration in the solid state.