Sorption and Magnetic Properties of Oxalato-Based Trimetallic Open Framework Stabilized by Charge-Assisted Hydrogen Bonds

We report a new structure of {[Co(bpy)2(ox)][{Cu2(bpy)2(ox)}Fe(ox)3]}n·8.5nH2O NCU-1 presenting a rare ladder topology among oxalate-based coordination polymers with anionic chains composed of alternately arranged [Cu2(bpy)2(ox)]2+ and [Fe(ox)3]3− moieties. Along the a axis, they are separated by Co(III) units to give porous material with voids of 963.7 Å3 (16.9% of cell volume). The stability of this structure is assured by a network of stacking interactions and charge-assisted C-H…O hydrogen bonds formed between adjacent chains, adjacent cobalt(III) units, and alternately arranged cobalt(III) and chain motifs. The soaking experiment with acetonitrile and bromobenzene showed that water molecules (8.5 water molecules dispersed over 15 positions) are bonded tightly, despite partial occupancy. Water adsorption experiments are described by a D’arcy and Watt model being the sum of Langmuir and Dubinin–Serpinski isotherms. The amount of primary adsorption sites calculated from this model is equal 8.2 mol H2O/mol, being very close to the value obtained from the XRD experiments and indicates that water was adsorbed mainly on the primary sites. The antiferromagnetic properties could be only approximately described with the simple CuII-ox-CuII dimer using H = −J·S1·S2, thus, considering non-trivial topology of the whole Cu-Fe chain, we developed our own general approach, based on the semiclassical model (SC) and molecular field (MF) model, to describe precisely the magnetic superexchange interactions in NCU-1. We established that Cu(II)-Cu(II) coupling dominates over multiple Cu(II)-Fe(III) interactions, with JCuCu = −275(29) and JCuFe = −3.8(1.6) cm−1 and discussed the obtained values against the literature data.


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Formation of 2D and 3D frameworks can be achieved using different templates (e.g., quaternary amine cations and [M(AA) 3 ] 2+ cations with D 3 symmetry) [3]. To limit dimensions of the formed compounds, additional auxiliary capping ligands are used [30,31] as well as crown ethers [10]. Ladder chain was detected in [Cu 2 (bpy) 2 (ox)Cr/Fe(ox) 3 ] − 1D compounds [4,32] and the interactions were described using 0D model and a single exchange parameter because of the dominating antiferromagnetic interactions in the copper dimer over other couplings. For the description of the magnetic properties of homo-and heterometallic oxalato-based chains, the Heisenberg model was often used with a single exchange parameter [30,33]. A more complex description was proposed for a chain with two copper(II) ions in the asymmetric unit [1]. To properly model χT vs. T curve, the chain was split into ferromagnetic trimers which were subsequently antiferromagnetically coupled. Five exchange parameters were proposed for a trimetallic MnCuCr system showing a highly complex topology with three different ligands acting as bridges [8]. In modeling of the exchange pathways via oxalate anion connecting clusters into a chain, a classical spin approach useful for the description of systems with high spin (in this case S = 5) and relatively weak coupling between them was applied.
Parallel to the above mentioned works of Kanizaj et al. [4,32] we aimed to prepare a trimetallic (Co-Fe-Cu) compound with oxalate anions acting as bridges starting with tris(oxalato)ferrate unit and bpy as a capping ligand. Oxalate anions also offer an opportunity to create a robust hydrogen bond network. Hence, we intended to exploit these properties for the preparation of 1D chains forming 3D network. As the result, we have obtained new oxalato-based trimetallic open framework {[Co(bpy) 2 (ox)][{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ]} n ·8.5nH 2 O NCU-1 (NCU-Nicolaus Copernicus University). In NCU-1, the [{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ] − 1D oxalate-bridged chains [32] are spontaneously co-crystallized with [Co(bpy) 2 (ox)] 3+ cations, exploiting charge-assisted hydrogen bonds and π-π interactions, to establish the new coordination secondary building unit (SBU) for rigid porous architectures providing a new generation of magnets with predesigned and controllable structures susceptible for postsynthetic modifications [34]. The global approach for the more complete description of 1D magnetic properties was applied and water sorption/desorption properties were studied in detail, to provide the new quality born by this 1D modular form.

Synthesis
According to our procedure, two products were formed. First, the salmon crystals of NCU-1 are formed, and then green rods of [Cu(NCS) 2 (bpy)] [35] emerged. Nevertheless, owing to the time gap in crystallization of both complexes, they can be separately collected, and pure {[Co(bpy) 2 (ox)][{Cu 2 (bpy) 2 ox}Fe(ox) 3 ]} n ·8.5nH 2 O can be afforded. The composition of NCU-1 indicates significant changes to the substrates, beginning with the partial decomposition of [Fe(ox) 3 ] 3− and dissociation of [Cu(bpy) 2 NCS] + . These processes were accompanied by coordination of ox 2− to Cu(II), and uptake of both ox 2− and bpy by Co(II) centers, the latter followed by oxidation of Co(II) to Co(III) in the air during the crystallization process. Finally, new forms were self-assembled with the remaining [Fe(ox) 3 ] 3− metaloligands. It should be noted that the final compound was obtained solely according to the procedure described in the experimental part. The starting point was [Cu(bpy) 2 (NCS)](NO 3 ). Although, theoretically more appropriate direct strategies failed; an attempt of synthesis from simple salts and bpy or using the building blocks approach with [Cu 2 (bpy) 2 (ox)(H 2 O) 2 ] [36] did not yield any salmon crystals. We also tried to use K 3 [Cr(ox) 3 ]·3H 2 O but the chromium analog was not synthesized probably because of its inertness.

Structure Description
{[Co(bpy) 2 (ox)][{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ]} n ·8.5nH 2 O crystallizes in the monoclinic P2 1 /c space group with all atoms found in the general positions and with the whole formula motif composing the asymmetric unit ( Figure S1). There are 8.5 crystallization water molecules dispersed over 15 sites. The structure is composed of anionic chains [{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ] − and complex cations intercalated between them, whereas water molecules are found in large channels (11.6 × 9.0 Å) of the network. The chain is composed of alternately arranged copper dimers and tris(oxalato)ferrate anions connected via bidentate/monodentate and bidentate/bismonodentate oxalate bridges ( Figure 1). The bridging oxalate anions are coordinated bidentately to iron(III) cations and monodentately to copper(II) cations either by the outer oxygen atoms (mode 1) or via the inner oxygen atoms (mode 2) ( Figure S2). Because of chain topology and manner of coordination binding between tris(oxalato)ferrate blocks and copper(II) dimers, four different Fe-Cu distances (4.018-5.325 Å) are formed. These are the shortest intermetallic distances in this compound and they fall in the range found for structures with identical topology [32]. In the dimer copper(II), cations are coupled via bisbidentately coordinated oxalate anion (mode 3) ( Figure S2) with the Cu-Cu distance (5.132 Å) falling in the range found for dimers with two copper(II) ions bridged by bisbidentately coordinated oxalate anion with four short Cu-O ox distances [4,32] (Table S2, Figure S3). This indicates that there are many pathways of possible coupling between paramagnetic metal cations and hence, an extremely complex model of exchange interactions is expected.
space group with all atoms found in the general positions and with the who motif composing the asymmetric unit ( Figure S1). There are 8.5 crystalliza molecules dispersed over 15 sites. The structure is composed of anio [{Cu2(bpy)2(ox)}Fe(ox)3] -and complex cations intercalated between them, whe molecules are found in large channels (11.6 × 9.0 Å) of the network. The chain is of alternately arranged copper dimers and tris(oxalato)ferrate anions con bidentate/monodentate and bidentate/bismonodentate oxalate bridges (Figu bridging oxalate anions are coordinated bidentately to iron(III) ca monodentately to copper(II) cations either by the outer oxygen atoms (mode 1 inner oxygen atoms (mode 2) ( Figure S2). Because of chain topology and coordination binding between tris(oxalato)ferrate blocks and copper(II) di different Fe-Cu distances (4.018-5.325 Å) are formed. These are the shortest in distances in this compound and they fall in the range found for structures wi topology [32]. In the dimer copper(II), cations are coupled via bisbidentately c oxalate anion (mode 3) ( Figure S2) with the Cu-Cu distance (5.132 Å) falling i found for dimers with two copper(II) ions bridged by bisbidentately coordina anion with four short Cu-Oox distances [4,32] (Table S2, Figure S3). This indicate are many pathways of possible coupling between paramagnetic metal cations an extremely complex model of exchange interactions is expected. Both copper(II) cations show elongated octahedral (SOC = 1.325 for Cu1 and for Cu2) environments, with different deviation from planarity in the equat (SSP-4 = 0.412 for Cu1 and SSP-4 = 1.405 for Cu2) [37]. The coordination sphere is of two nitrogen atoms from bpy molecules and four oxygen atoms from oxala the coordination sphere. The equatorial plane is formed by two oxygen atoms to 1.9787(19) Å) and two nitrogen atoms (1.965(3) to 1.983(2) Å), whereas oxyg axial positions form very long Cu-O bonds ranging from 2.434(3) to 2.712 (2) longest value corresponding to a semi-coordination (Table S3). These distances to those found in ammonium and potassium compounds [32] apart from Cu Cu2-O61 which are significantly shorter than the bond lengths found in the a and potassium complexes ( Figure S4). In the reported structure, the two equa Cu-O distances are similar and we can anticipate significant antiferromagn couplings, whereas substantial differences in those bonds result in the reduc exchange integral value [12]. Iron(III) is found in a trigonally distorted environment formed by six oxygen atoms from oxalate anions. The Fe-O b Both copper(II) cations show elongated octahedral (S OC = 1.325 for Cu1 and S OC = 2.771 for Cu2) environments, with different deviation from planarity in the equatorial plane (S SP-4 = 0.412 for Cu1 and S SP-4 = 1.405 for Cu2) [37]. The coordination sphere is composed of two nitrogen atoms from bpy molecules and four oxygen atoms from oxalate anions in the coordination sphere. The equatorial plane is formed by two oxygen atoms (1.9691 (19) to 1.9787(19) Å) and two nitrogen atoms (1.965(3) to 1.983(2) Å), whereas oxygen atoms in axial positions form very long Cu-O bonds ranging from 2.434(3) to 2.712(2) Å with the longest value corresponding to a semi-coordination (Table S3). These distances are similar to those found in ammonium and potassium compounds [32] apart from Cu1-O54 and Cu2-O61 which are significantly shorter than the bond lengths found in the ammonium and potassium complexes ( Figure S4). In the reported structure, the two equatorial short Cu-O distances are similar and we can anticipate significant antiferromagnetic Cu-Cu couplings, whereas substantial differences in those bonds result in the reduction of the exchange integral value [12]. Iron(III) is found in a trigonally distorted octahedral environment formed by six oxygen atoms from oxalate anions. The Fe-O bonds range from 2.005(2) to 2.023(2) Å and are in the range observed for bridging and terminal oxalate anions [38][39][40]. The cobalt(III) cations coordination sphere consists of two oxygen atoms from bidentately coordinated oxalate anion (mode 4, 1.893(2)-1.900(2) Å) ( Figure S2) and four nitrogen atoms coming from bpy (1.947(3)-1.954(3) Å) ligands. The latter bonds fall in the range found for Co-N ar bonds, clearly indicating the low spin configuration by both experimental (XRD) and theoretical methods [41][42][43] and +3 (3.12) oxidation number by bond valence sum calculation [44].
Up to the best of our knowledge, such a ladder represents a very rare topology [4,32] with oxalate anions connecting iron(III) and copper(II) and rungs made of bisbidentately coordinated oxalate anions joining both copper(II) cations. Their superposition showed differences in O41/O5 oxalate position and bpy position due to the significant twist observed in NCU-1 ( Figure S5). The already published structures are much more tightly packed due to small ions (potassium or ammonium) connecting adjacent chains either via coordination bonds (potassium) or by hydrogen bonds (ammonium). In these compounds there is only one water molecule (ammonium compound) or the crystallization water molecule is absent (potassium compound). Therefore, for the models with removed solvent molecules, the packing indices are 68.1 and 75.1%, respectively [45]. The voids accessible for solvent are present only for ammonium compound and account for only 1.0% of the cell volume and 16.4 Å 3 per cell. In the reported structure we exploited the ability of oxalate anions for creation of non-covalent interactions. The packing shows channels running along the c axis filled with crystallization water molecules ( Figure 2a). Hence, the additional coordination unit introduces significant changes in symmetry and even more importantly in the network-large and stable channels are formed with cobalt units separating the chains along the a axis. It results in a much lower packing index of the backbone being 61.6% and the volume accessible for the solvent is 963.7 Å 3 (16.9%) which is sufficient for sorption of gases and/or solvents. relatively weak C-H…O bonds are sufficient for structure stabilization and permanent porosity of this system. We can hypothesize that the channels do not collapse for several reasons. First, these interactions are charged assisted according to the definition given by Lopes Jesus and Redinha [50] ("H-bonds wherein the donor group has a positive charge or the acceptor group a negative one are called charge-assisted (CAHBs), ionic, or lowbarrier hydrogen bonds"). In our case, oxygen atoms of the oxalate ligand are negatively charged. Moreover, it is proved that weak and labile C-H…N interactions are capable of forming a very complex porous structure [51]. Secondly, multipoint hydrogen bonds are a key factor for the stabilization of MOFs [21]. The presented interactions (Figure 2b-d) clearly indicate that our compound can complete this requirement. Finally, for HOFs stability, additional interactions reinforcing hydrogen bonds and assuring better rigidity are required [46]. Such interactions are driving forces for the preparation of covalent organic frameworks (COFs). In NCU-1, we found multiple π-π interactions forming zippers ( Figure 2b,c) In the channels formed by such a crystal network, there are water molecules dispersed over 15 sites. In the final model, their hydrogen atoms are missing and hence, detailed interaction analysis cannot be performed and must be limited to oxygen atoms acting as acceptors of hydrogen bonds. There is only one such interaction, C21-H21…O93[1 + x, y, z]. Taking into account the partial occupancy found for many of the water positions and the lack of efficient bonding, we can expect that they could be easily The crucial problem is the stability of such an open framework which is located between a classical covalently bonded 3D coordination MOF and a hydrogen-bonded organic framework (HOF), which relies on weak (mainly hydrogen bonds) interactions [46]. In the reported case, an additional moiety generates voids and we exploited oxalate ability for non-covalent interactions which were able to maintain the permanent porosity [47][48][49]. In NCU-1, the covalent bonds are formed only along the chain between copper and iron moieties, whereas in two other directions weak intermolecular interactions (between cobalt units as well as cobalt units and chains) are present. The crystal network is maintained by numerous C-H . . . O hydrogen bonds with hydrogen atoms coming from bpy molecules and acceptor atoms from all oxalate anions as well as by π-π interactions between bpy ligands. The observed hydrogen bonds can be split into three groups according to the unit type involved in the interaction (Table S4). Adjacent chains form strong interactions along the b axis due to hydrogen bonds between N1 bpy ligand and O52 and O54 outer oxygen atoms as well as N11 bpy molecules and outer O42 and O62 oxygen atoms (Figure 2b). Apart from that, there are two zipper motifs formed by stacking interactions between solely N1 as well as solely N11 bpy molecules. Along the c axis, each cobalt unit is involved in four hydrogen bonds with two adjacent [Co(bpy) 2 (ox)] + moieties ( Figure 2c). They are created between both outer oxygen atoms (O82 and O84) and N21 and N31 bpy molecules. This pattern is completed by a zipper formed by O81 oxalate anions and two stacking interactions between bpy ligands (N21-N21 and N31-N31). Along the a axis there is a robust set of hydrogen bonds between alternately arranged cobalt units and chains (Figure 2d). The cobalt units limit the channel size and stabilize the crystal network connecting chains translated along this direction. The hydrogen bonds are created between all ligands of Co(III) units and N1 bpy ligand as well as O61 and O71 oxalate anions from chains and they are reinforced by π-π interactions formed between strongly inclined N1, N31 bpy ligands. In HOF chemistry, usually strong hydrogen bonds are required to stabilize the open frameworks, whereas weak interactions usually are not able to maintain porosity [46]. Therefore, it is worth noting that in the reported case the relatively weak C-H . . . O bonds are sufficient for structure stabilization and permanent porosity of this system. We can hypothesize that the channels do not collapse for several reasons. First, these interactions are charged assisted according to the definition given by Lopes Jesus and Redinha [50] ("H-bonds wherein the donor group has a positive charge or the acceptor group a negative one are called charge-assisted (CAHBs), ionic, or low-barrier hydrogen bonds"). In our case, oxygen atoms of the oxalate ligand are negatively charged. Moreover, it is proved that weak and labile C-H . . . N interactions are capable of forming a very complex porous structure [51]. Secondly, multipoint hydrogen bonds are a key factor for the stabilization of MOFs [21]. The presented interactions (Figure 2b-d) clearly indicate that our compound can complete this requirement. Finally, for HOFs stability, additional interactions reinforcing hydrogen bonds and assuring better rigidity are required [46]. Such interactions are driving forces for the preparation of covalent organic frameworks (COFs). In NCU-1, we found multiple π-π interactions forming zippers (Figure 2b,c) In the channels formed by such a crystal network, there are water molecules dispersed over 15 sites. In the final model, their hydrogen atoms are missing and hence, detailed interaction analysis cannot be performed and must be limited to oxygen atoms acting as acceptors of hydrogen bonds. There is only one such interaction, C21-H21 . . . O93[1 + x, y, z]. Taking into account the partial occupancy found for many of the water positions and the lack of efficient bonding, we can expect that they could be easily removed. However, the performed EDX and single crystal experiments showed that the water molecules could not be easily substituted by other solvents (e.g., acetonitrile and bromobenzene).

Thermal Analysis
Thermal decomposition studied by the combined TGA-DTA techniques proceeds in two steps ( Figure S6). Loss of crystallization water molecules starts at room temperature (experimental: 8.68%, calculated: 10.48%), and is accomplished at ca. 120 • C. This behavior indicates that the quantity of solvent in the channels may vary and the initial loss of 1.5 water molecules at RT (resulting in 7 water molecules remaining in the system) matches the experimental value ideally. Subsequently, one exothermic and complex step related to a continuous mass loss (67.49%) of oxalate and bipyridine is observed and completed at ca. 400 • C. Finally, a small mass loss occurs and the mass residue corresponds to a mixture of oxides (CuO and Co x Fe y O 4 ; the experimental value is 23.79%, whereas for 7 crystallization water molecules the calculated value is 22.00%). Their presence was confirmed by the powder XRD method registered for products of thermal decomposition. Similar behavior and discrepancy were found for other porous structures indicating that the amount of water in side channels might vary in the broad range [52].

Powder Experiments
The PXRD patterns for the dehydrated (3 h in 120 • C) and rehydrated samples (RT) of NCU-1 show diffraction peaks identical to those observed in the pattern calculated using the single crystal model (Figure 3 and Figure S7). It was shown that careful analysis of certain peak positions could be useful for the determination of the framework stability [52]. The position of the (020) (ca. 3.6 • 2θ) and (100) (ca. 5.8 • 2θ) reflections can be considered as markers of the channel stability as they are parallel to the c direction. We observed a small shift (ca. 0.1 • ) of the former peak towards lower angles and to the higher angles (ca. 0.05 • ) for the latter one. After the heating and cooling cycle, both peaks are present approximately at their starting positions, indicating that this framework is robust and stabilized by charge-assisted hydrogen bonds resulting in the permanent porosity.
(experimental: 8.68%, calculated: 10.48%), and is accomplished at ca. 120 °C. This b indicates that the quantity of solvent in the channels may vary and the initial lo water molecules at RT (resulting in 7 water molecules remaining in the system) the experimental value ideally. Subsequently, one exothermic and complex step r a continuous mass loss (67.49%) of oxalate and bipyridine is observed and comp ca. 400 °C. Finally, a small mass loss occurs and the mass residue corresponds to a of oxides (CuO and CoxFeyO4; the experimental value is 23.79%, wherea crystallization water molecules the calculated value is 22.00%). Their prese confirmed by the powder XRD method registered for products of thermal decomp Similar behavior and discrepancy were found for other porous structures indica the amount of water in side channels might vary in the broad range [52].

Powder Experiments
The PXRD patterns for the dehydrated (3 h in 120 °C) and rehydrated samp of NCU-1 show diffraction peaks identical to those observed in the pattern ca using the single crystal model (Figure 3 and S7). It was shown that careful an certain peak positions could be useful for the determination of the framework [52]. The position of the (020) (ca. 3.6° 2θ) and (100) (ca. 5.8° 2θ) reflections considered as markers of the channel stability as they are parallel to the c direc observed a small shift (ca. 0.1°) of the former peak towards lower angles and to th angles (ca. 0.05°) for the latter one. After the heating and cooling cycle, both p present approximately at their starting positions, indicating that this framework and stabilized by charge-assisted hydrogen bonds resulting in the permanent po

Sorption Properties
When water is adsorbed on hydrophilic surfaces, the D'Arcy and Wa adsorption isotherm can be taken into account [53]. The model assumes adsorption of water occurs quite independently, on strong-high-energy and on low-energy sites. The former binding primary centers consist mainly of hyd groups. In the model, it is simplified that there is only one type of secondary which, for the adsorbed water, two-or three-dimensional hydrogen-bonded clus begin to build up even before all the primary sites are occupied. The simplest a popular form of the original DW equation is the sum of Langmuir (adsorption on sites) and DS1 isotherms (describing adsorption on secondary sites available f molecules): where amL is the total surface concentration of all Langmuir-type (high-energy) si . Powder diffractograms for NCU-1: calculated pattern (red), pristine sample at room temperature (blue), sample after heating at 120 • C during 3 h (green), and sample after cooling to room temperature (violet). Only the low angle part is presented (3-22.5 • ).

Sorption Properties
When water is adsorbed on hydrophilic surfaces, the D'Arcy and Watt (DW) adsorption isotherm can be taken into account [53]. The model assumes that the adsorption of water occurs quite independently, on strong-high-energy and on weak-low-energy sites. The former binding primary centers consist mainly of hydrophilic groups. In the model, it is simplified that there is only one type of secondary sites on which, for the adsorbed water, two-or three-dimensional hydrogen-bonded clusters can begin to build up even before all the primary sites are occupied. The simplest and most popular form of the original DW equation is the sum of Langmuir (adsorption on primary sites) and DS1 isotherms (describing adsorption on secondary sites available for water molecules): (experimental: 8.68%, calculated: 10.48%), and is accomplished at ca. 120 °C. This behavior indicates that the quantity of solvent in the channels may vary and the initial loss of 1.5 water molecules at RT (resulting in 7 water molecules remaining in the system) matches the experimental value ideally. Subsequently, one exothermic and complex step related to a continuous mass loss (67.49%) of oxalate and bipyridine is observed and completed at ca. 400 °C. Finally, a small mass loss occurs and the mass residue corresponds to a mixture of oxides (CuO and CoxFeyO4; the experimental value is 23.79%, whereas for 7 crystallization water molecules the calculated value is 22.00%). Their presence was confirmed by the powder XRD method registered for products of thermal decomposition. Similar behavior and discrepancy were found for other porous structures indicating that the amount of water in side channels might vary in the broad range [52].

Powder Experiments
The PXRD patterns for the dehydrated (3 h in 120 °C) and rehydrated samples (RT) of NCU-1 show diffraction peaks identical to those observed in the pattern calculated using the single crystal model (Figure 3 and S7). It was shown that careful analysis of certain peak positions could be useful for the determination of the framework stability [52]. The position of the (020) (ca. 3.6° 2θ) and (100) (ca. 5.8° 2θ) reflections can be considered as markers of the channel stability as they are parallel to the c direction. We observed a small shift (ca. 0.1°) of the former peak towards lower angles and to the higher angles (ca. 0.05°) for the latter one. After the heating and cooling cycle, both peaks are present approximately at their starting positions, indicating that this framework is robust and stabilized by charge-assisted hydrogen bonds resulting in the permanent porosity. Powder diffractograms for NCU-1: calculated pattern (red), pristine sample at room temperature (blue), sample after heating at 120 °C during 3 h (green), and sample after cooling to room temperature (violet). Only the low angle part is presented (3-22.5°).

Sorption Properties
When water is adsorbed on hydrophilic surfaces, the D'Arcy and Watt (DW) adsorption isotherm can be taken into account [53]. The model assumes that the adsorption of water occurs quite independently, on strong-high-energy and on weaklow-energy sites. The former binding primary centers consist mainly of hydrophilic groups. In the model, it is simplified that there is only one type of secondary sites on which, for the adsorbed water, two-or three-dimensional hydrogen-bonded clusters can begin to build up even before all the primary sites are occupied. The simplest and most popular form of the original DW equation is the sum of Langmuir (adsorption on primary sites) and DS1 isotherms (describing adsorption on secondary sites available for water molecules): where amL is the total surface concentration of all Langmuir-type (high-energy) sites, KL is the Langmuir constant, and h = p/ps, a0 and c are the number of adsorption centers and (experimental: 8.68%, calculated: 10.48%), and is accomplished at ca. 120 °C. This behavior indicates that the quantity of solvent in the channels may vary and the initial loss of 1.5 water molecules at RT (resulting in 7 water molecules remaining in the system) matches the experimental value ideally. Subsequently, one exothermic and complex step related to a continuous mass loss (67.49%) of oxalate and bipyridine is observed and completed at ca. 400 °C. Finally, a small mass loss occurs and the mass residue corresponds to a mixture of oxides (CuO and CoxFeyO4; the experimental value is 23.79%, whereas for 7 crystallization water molecules the calculated value is 22.00%). Their presence was confirmed by the powder XRD method registered for products of thermal decomposition. Similar behavior and discrepancy were found for other porous structures indicating that the amount of water in side channels might vary in the broad range [52].

Powder Experiments
The PXRD patterns for the dehydrated (3 h in 120 °C) and rehydrated samples (RT) of NCU-1 show diffraction peaks identical to those observed in the pattern calculated using the single crystal model (Figure 3 and S7). It was shown that careful analysis of certain peak positions could be useful for the determination of the framework stability [52]. The position of the (020) (ca. 3.6° 2θ) and (100) (ca. 5.8° 2θ) reflections can be considered as markers of the channel stability as they are parallel to the c direction. We observed a small shift (ca. 0.1°) of the former peak towards lower angles and to the higher angles (ca. 0.05°) for the latter one. After the heating and cooling cycle, both peaks are present approximately at their starting positions, indicating that this framework is robust and stabilized by charge-assisted hydrogen bonds resulting in the permanent porosity.

Sorption Properties
When water is adsorbed on hydrophilic surfaces, the D'Arcy and Watt (DW) adsorption isotherm can be taken into account [53]. The model assumes that the adsorption of water occurs quite independently, on strong-high-energy and on weaklow-energy sites. The former binding primary centers consist mainly of hydrophilic groups. In the model, it is simplified that there is only one type of secondary sites on which, for the adsorbed water, two-or three-dimensional hydrogen-bonded clusters can begin to build up even before all the primary sites are occupied. The simplest and most popular form of the original DW equation is the sum of Langmuir (adsorption on primary sites) and DS1 isotherms (describing adsorption on secondary sites available for water molecules): a ch a a a p K h ch where amL is the total surface concentration of all Langmuir-type (high-energy) sites, KL is the Langmuir constant, and h = p/ps, a0 and c are the number of adsorption centers and

DS1
(1) where a mL is the total surface concentration of all Langmuir-type (high-energy) sites, K L is the Langmuir constant, and h = p/p s , a 0 and c are the number of adsorption centers and the kinetic constant related to the adsorption on secondary sites (of Dubinin-Serpinsky type), respectively. It is well-known that the difference in the shape of water isotherms is caused by the combined effects of surface hydrophobicity (low-energy centers) and hydrophilicity (high-energy centers). Water is known to have an extremely low affinity toward the "pure" benzene ring and a high affinity toward polar sites leading even to chemisorption. Subsequently, those adsorbed molecules on primary sites (both mentioned above types of centers should be considered) can become secondary ones and adsorption on them occurs following the original Dubinin-Serpinsky mechanism. Thus, the total adsorption is the sum of the adsorption on all available for water molecules, primary (a prim ) and secondary sites (a sec ). This simple model was presented as applicable to the description of different adsorption data (see, e.g., [54,55]).
As NCU-1 possesses a high amount of high-energy adsorptive centers for the fitting of experimental adsorption data ( Figure 4) we have chosen the D-W Equation (1). It is seen that it fits the experimental data satisfactorily-the determination coefficient is 0.9997, the standard error of estimates is low, only in the case of a 0 it exceeds 10% of the estimated value. The fitted values of K L , c and a x (x = L or 0) are summarized in Table 1. The Langmuir constant K L is related to the affinity between the adsorbate and the adsorbent, while the parameter c is the ratio of adsorption and desorption constants; value of c = 1 suggests non-interacting sites. the kinetic constant related to the adsorption on secondary sites (of Dubinin-Serpinsky type), respectively. It is well-known that the difference in the shape of water isotherms is caused by the combined effects of surface hydrophobicity (low-energy centers) and hydrophilicity (high-energy centers). Water is known to have an extremely low affinity toward the "pure" benzene ring and a high affinity toward polar sites leading even to chemisorption. Subsequently, those adsorbed molecules on primary sites (both mentioned above types of centers should be considered) can become secondary ones and adsorption on them occurs following the original Dubinin-Serpinsky mechanism. Thus, the total adsorption is the sum of the adsorption on all available for water molecules, primary (aprim) and secondary sites (asec). This simple model was presented as applicable to the description of different adsorption data (see, e.g., [54,55]).
As NCU-1 possesses a high amount of high-energy adsorptive centers for the fitting of experimental adsorption data ( Figure 4) we have chosen the D-W Equation (1). It is seen that it fits the experimental data satisfactorily-the determination coefficient is 0.9997, the standard error of estimates is low, only in the case of a0 it exceeds 10% of the estimated value. The fitted values of KL, c and ax (x = L or 0) are summarized in Table 1. The Langmuir constant KL is related to the affinity between the adsorbate and the adsorbent, while the parameter c is the ratio of adsorption and desorption constants; value of c = 1 suggests non-interacting sites.  It is seen that practically in the p/ps range 0-0.85 the Langmuir term is sufficient to fit the data properly, the DS1 term is needed only for p/ps > 0.85 (Figure 4). Taking the molar  It is seen that practically in the p/p s range 0-0.85 the Langmuir term is sufficient to fit the data properly, the DS1 term is needed only for p/p s > 0.85 (Figure 4) To confirm the H 2 O adsorption on primary sites the DRIFT measurements were performed. The IR spectrum of NCU-1 ( Figure 5) shows the characteristic bands of all ligands. Crystallization water molecules can be detected due to the broad intense band with the maximum at 3424 cm -1 related to O-H stretching vibrations. The presence of bisbidentately coordinated 2,2 -bipyridine molecules can be confirmed by intense bands at 1600 and 1580 cm −1 assigned to ν(C=C) and ν(C=N), respectively, as well as δ(C-H) vibrations in the aromatic ring, whereas medium intensity bands at 3068, 1180, and 1033 cm −1 correspond to CH vibrations of aromatic rings [56][57][58][59]. There are four coordination modes of oxalate anions and hence, several bands corresponding to different vibrations of this fivemembered ring were registered. Intense bands in the region of 1720-1620 cm −1 are related to asymmetric ν CO vibrations, whereas those at 1400-1340 cm -1 come from symmetric ν CO vibrations [38,60]. Another bands occurred at 1274, 1246 (ν(CO) + δ(OCO)) cm −1 .  The increase in temperature causes a gradual removal of H 2 O from the structureobserved mainly as the decrease in the intensity of ν(OH) band (3700-2800 cm -1 ). The band shape being very broad indicates that H-bonding occurs to a great extent. Interestingly, simultaneously to the H 2 O removal from the structure, the ν(CH) bands of bpy ligands become more intense. It proves the strong interactions (through H-bonding) of H bpy with O (from H 2 O). Moreover, these interactions are much stronger than H-bonds between two H 2 O molecules. This observation explains (i) the complete lack of hysteresis loop, (ii) the Langmuir-shape in the low and middle pressure range, and (iii) the drastic rise during pore filling (high pressure range) in H 2 O adsorption isotherm.
Oxalate binds to a metal ion, forming five-membered chelating rings [61,62]. Coordination of oxalate to metal (Me) ions drastically changes its structural and electronic environment, thereby leading to the appearance of more complex IR spectra compared to the free oxalate spectrum [63]. As can be seen from Figure 5C

XAS Experiments
The energy ranges for iron, cobalt, and copper were carefully selected to avoid the edge regions of other elements, which is crucial for proper spectra normalization. It is especially important for iron which has to be truncated relatively early because of the presence of cobalt. These spectra show a more intense band corresponding to L 3 edge followed by much smaller L 2 peaks and the former one is discussed in detail in the Supplementary Materials (Table S5). For iron(III) and copper(II) the observed spectra are similar to those registered for the identical building blocks reported in the literature [64,65] (Figure S9). Hence, we can suppose that the electron structure of those units and the metal oxidation states are also similar (see discussion in Supplementary Materials). For cobalt, the multiplet is complicated and consists of four bands (Table S5). The first two components occurs at 777.2 and 779.0 eV, whereas the main peak is found at 781.0 eV (Figure 7) with a small postedge feature at 783.7 eV. This pattern is similar to [Co(bpy) 3 ] 3+ complex [41]. However, in NCU-1 one of these ligands is substituted by oxalate anion producing a much weaker ligand field and hence, impairing the direct comparison of multiplets in both complexes. Nevertheless, some observations are useful. In [Co(bpy) 3 ] 3+ , the main feature is attributed to the low spin configuration and the weak high energy peak to MLCT transition, whereas two low energy peaks can be ascribed mainly to high spin configuration. Therefore, in the reported compounds it is conceivable that the ligand substitution with oxalate reducing ligand field splitting can result in some admixture of this configuration. However, the magnetic data clearly indicate the diamagnetic low spin state of [Co(bpy) 2 (ox)] + accompanying the active exchange interactions along the [{Cu 2 (bpy) 2 ox}Fe(ox) 3 ] − chain counterions.

XAS Experiments
The energy ranges for iron, cobalt, and copper were carefully selected to avoid th edge regions of other elements, which is crucial for proper spectra normalization. It i especially important for iron which has to be truncated relatively early because of th presence of cobalt. These spectra show a more intense band corresponding to L3 edg followed by much smaller L2 peaks and the former one is discussed in detail in th Supplementary Materials (Table S5). For iron(III) and copper(II) the observed spectra ar similar to those registered for the identical building blocks reported in the literatur [64,65] (Figure S9). Hence, we can suppose that the electron structure of those units and the metal oxidation states are also similar (see discussion in Supplementary Materials) For cobalt, the multiplet is complicated and consists of four bands (Table S5). The first two components occurs at 777.2 and 779.0 eV, whereas the main peak is found at 781.0 eV ( Figure 7) with a small postedge feature at 783.7 eV. This pattern is similar to [Co(bpy)3] 3 complex [41]. However, in NCU-1 one of these ligands is substituted by oxalate anion producing a much weaker ligand field and hence, impairing the direct comparison o multiplets in both complexes. Nevertheless, some observations are useful. In [Co(bpy)3] 3+ the main feature is attributed to the low spin configuration and the weak high energy peak to MLCT transition, whereas two low energy peaks can be ascribed mainly to high spin configuration. Therefore, in the reported compounds it is conceivable that the ligand substitution with oxalate reducing ligand field splitting can result in some admixture o this configuration. However, the magnetic data clearly indicate the diamagnetic low spin state of [Co(bpy)2(ox)] + accompanying the active exchange interactions along th [{Cu2(bpy)2ox}Fe(ox)3] -chain counterions.  Figure 8a shows the plot of the molar magnetic susceptibility in the form of the χT product against temperature T for the powder sample of NCU-1 (black symbols). The χT values decrease on lowering the temperature from 5.33 cm 3 ·K·mol −1 at 300 K first steadily and next below 10 K abruptly displaying at the lowest temperatures an upturned kink with the value of 4.44 cm 3 ·K·mol −1 at 1.98 K and 4.48 cm 3 ·K·mol −1 at 1.80 K. The high temperature value of χT is slightly higher than the value of 5.13 cm 3 ·K·mol −1 expected fo combined contributions from one Fe(III) ion (SFe = 5/2, gFe = 2.0) and two Cu(II) ions (SCu 1/2, gCu = 2.0). Figure 8b shows the inverse susceptibility of the studied system (symbols) On lowering the temperature, it displays an almost linear decrease meeting the origin o  Figure 8a shows the plot of the molar magnetic susceptibility in the form of the χT product against temperature T for the powder sample of NCU-1 (black symbols). The χT values decrease on lowering the temperature from 5.33 cm 3 ·K·mol −1 at 300 K first steadily and next below 10 K abruptly displaying at the lowest temperatures an upturned kink with the value of 4.44 cm 3 ·K·mol −1 at 1.98 K and 4.48 cm 3 ·K·mol −1 at 1.80 K. The high temperature value of χT is slightly higher than the value of 5.13 cm 3 ·K·mol −1 expected for combined contributions from one Fe(III) ion (S Fe = 5/2, g Fe = 2.0) and two Cu(II) ions (S Cu = 1/2, g Cu = 2.0). Figure 8b shows the inverse susceptibility of the studied system (symbols). On lowering the temperature, it displays an almost linear decrease meeting the origin of the coordinate system (T, χ −1 ). The measurements of the isothermal magnetization demonstrated the lack of opening magnetic hysteresis (not shown) implying a soft magnetic material with negligible anisotropy. In Figure 8c, the experimental data for the field dependence of the magnetization at 1.8 K (symbols) are shown. The curve displays a monotonic increase with an increasing field value, not exceeding the maximal field value level of 5.13 N A µ B , which points to the strongly antiferromagnetic character of the coupling between the Cu(II) ions leaving effectively the sole contribution from the Fe(III) ion (S Fe = 5/2 with g Fe ≈ 2.065). the coordinate system (T, χ −1 ). The measurements of the isothermal magnetization demonstrated the lack of opening magnetic hysteresis (not shown) implying a soft magnetic material with negligible anisotropy. In Figure 8c, the experimental data for the field dependence of the magnetization at 1.8 K (symbols) are shown. The curve displays a monotonic increase with an increasing field value, not exceeding the maximal field value level of 5.13 NAμB, which points to the strongly antiferromagnetic character of the coupling between the Cu(II) ions leaving effectively the sole contribution from the Fe(III) ion (SFe = 5/2 with gFe ≈ 2.065). In what follows we make an effort to extract the magnetic interactions present in the studied system from the magnetic measurements. Unlike in [4,32], where similar ladderlike topologies have been reported, we attempt, here, to go beyond a simple zerodimensional (0D) spin Hamiltonian, developed in the next section for the sake of comparison, and reflect the genuine topology of NCU-1 taking duly into account all interaction pathways (see sections; Molecular field prediction and Semiclassical model).

Simple Dimer Model
The structural analysis of NCU-1 exhibited the dinuclear "Cu1-ox-Cu2" cations, with an almost symmetrical oxalate bridge forming a ladder due to the connection through tris(oxalato)ferrate(III) ions (Figure 1). To explain the magnetic properties, a simple model involving only copper(II)-copper(II) interaction was first used and copper(II)-iron(III) interactions were ignored. We applied Hamiltonian in the form H = −JCu-Cu(SCu1SCu2). We used the PHI program [66] in the fitting procedure, which allows for the simultaneous fitting of χT(T) and M(H) dependences. In this simple model, temperature-independent In what follows we make an effort to extract the magnetic interactions present in the studied system from the magnetic measurements. Unlike in [4,32], where similar ladder-like topologies have been reported, we attempt, here, to go beyond a simple zero-dimensional (0D) spin Hamiltonian, developed in the next section for the sake of comparison, and reflect the genuine topology of NCU-1 taking duly into account all interaction pathways (see sections; Molecular field prediction and Semiclassical model).

Simple Dimer Model
The structural analysis of NCU-1 exhibited the dinuclear "Cu1-ox-Cu2" cations, with an almost symmetrical oxalate bridge forming a ladder due to the connection through tris(oxalato)ferrate(III) ions (Figure 1). To explain the magnetic properties, a simple model involving only copper(II)-copper(II) interaction was first used and copper(II)-iron(III) interactions were ignored. We applied Hamiltonian in the form H = −J Cu-Cu (S Cu1 S Cu2 ). We used the PHI program [66] in the fitting procedure, which allows for the simultaneous fitting of χT(T) and M(H) dependences. In this simple model, temperature-independent magnetism (χ 0 ) and molecular field corrections term (zJ') were also introduced. Two different approaches to g-factors were used. In the first, only one g-factor was used. The best reasonable fit parameters were g Cu = g Fe = 2.068, J Cu-Cu = −324.4 cm −1 , χ 0 = +0.00089 cm 3 ·mol −1 , zJ' = +0.007 cm −1 and with good values of the test functions R χT = Σ (χT obs − χT calc ) 2 /Σ (χT obs ) 2 = 3.66·10 −5 for χT(T) data and R M = Σ (M obs − M calc ) 2 /Σ (M obs ) 2 = 4.54·10 −4 for M(H) data. In the second, g-factors, g Cu = 2.00 and g Fe = 2.065, were taken from SC model (see below) and fixed. In this case, the best reasonable fit parameters were J Cu-Cu = −327.0 cm −1 , χ 0 = +0.00095 cm 3 ·mol −1 , zJ' = -0.006 cm −1 and with following values of the test functions R defined as above, R χT = 3.17·10 −5 for χT(T) data and R M = 4.31·10 −4 for M(H) data. As we can see, in both cases, the key parameter, i.e., the Cu-Cu exchange integral, has shown almost identical values.

Molecular Field (MF) Prediction
Let us consider a chain with A 1 A 2 B topology, as depicted in Figure 9, where single centers of spin S B with the spectroscopic factor g B alternate with a couple of spins S A with the spectroscopic factor g A . Centers A 1 , A 2 and B are exchange coupled with J 1 , J 2 , J 3 , J 4 , and J 5 being the exchange coupling constants. The chain is of length N in terms of the A 1 A 2 B units. The pertinent Hamiltonian has the following form where µ B is the Bohr magneton, → H denotes the external magnetic field, and the periodic boundary conditions are imposed, i.e.,Ŝ BN+1 ≡Ŝ B1 . The molecular field theory is expressed in terms of net magnetization → S Bi (molar quantities are considered here and angle brackets denote thermodynamical averaging) corresponding to the i-th subsystem of A-type and B-type, respectively, rather than the subsequent spin variables. magnetism (χ0) and molecular field corrections term (zJ') were also introduced. Two different approaches to g-factors were used. In the first, only one g-factor was used. The best reasonable fit parameters were gCu = gFe = 2.068, JCu-Cu = −324.4 cm −1 , χ0 = +0.00089 cm 3 ·mol −1 , zJ' = +0.007 cm −1 and with good values of the test functions RχT = Σ (χTobs − χTcalc) 2 /Σ (χTobs) 2 = 3.66·10 −5 for χT(T) data and RM = Σ (Mobs − Mcalc) 2 /Σ (Mobs) 2 = 4.54·10 −4 for M(H) data. In the second, g-factors, gCu = 2.00 and gFe = 2.065, were taken from SC model (see below) and fixed. In this case, the best reasonable fit parameters were JCu-Cu = −327.0 cm −1 , χ0 = +0.00095 cm 3 ·mol −1 , zJ' = -0.006 cm −1 and with following values of the test functions R defined as above, RχT = 3.17·10 −5 for χT(T) data and RM = 4.31·10 −4 for M(H) data. As we can see, in both cases, the key parameter, i.e., the Cu-Cu exchange integral, has shown almost identical values.

Molecular Field (MF) Prediction
Let us consider a chain with A1A2B topology, as depicted in Figure 9, where single centers of spin SB with the spectroscopic factor gB alternate with a couple of spins SA with the spectroscopic factor gA. Centers A1, A2 and B are exchange coupled with J1, J2, J3, J4, and J5 being the exchange coupling constants. The chain is of length N in terms of the A1A2B units. The pertinent Hamiltonian has the following form where B μ is the Bohr magneton, H  denotes the external magnetic field, and the periodic boundary conditions are imposed, i.e., The molecular field theory is expressed in terms of net magnetization  Applying the procedure described in Supplementary Information, and identifying sublattices A1 and A2 with the Cu(II) subsystem (SCu = 1/2) and sublattice B with the Fe(III) subsystem (SFe = 5/2), one arrives at the following practical formula for the MF molar susceptibility of the studied system χMF = P/Q, where Applying the procedure described in Supplementary Information, and identifying sublattices A 1 and A 2 with the Cu(II) subsystem (S Cu = 1/2) and sublattice B with the Fe(III) subsystem (S Fe = 5/2), one arrives at the following practical formula for the MF molar susceptibility of the studied system χ MF = P/Q, where where k B -the Boltzmann constant, J 24 = J 2 + J 4 , and J 35 = J 3 + J 5 . The above formula will be used in what follows to obtain a preliminary estimate of the exchange interactions in the system under study.

Semiclassical (SC) Model
There is no available exact model to treat such a complex system with a knotted arrangement of spins within the chain. Nevertheless, even a necessarily approximate approach aimed at rationalizing the magnetic behavior may shed some light on the nature of magnetic interactions in this system. To obtain the zero-field susceptibility of the chain segment, a semiclassical analytical approach [67] is employed. In this scheme, the relatively large spin of the Fe(III) ion of the FeCu 2 unit (S Fe = 5/2) is treated as a classical commuting variable, while the remaining two Cu(II) spins (S Cu = 1/2) are given a rigorous quantum mechanical treatment. Unfortunately, the ensuing calculation cannot be performed analytically for the configuration of exchange couplings depicted in Figure 9, representing one of the pathological situations mentioned by the authors of [67]. Only by accepting the further restriction of J 2 = J 3 ≡ J 23 and J 4 = J 5 ≡ J 45 the calculation can be brought to its final explicit conclusion. The Hamiltonian of the finite chain involving N trimer units in Equation (2) may be rewritten as the sum of partial Hamiltonianŝ where Ψ i denotes the quantum subsystem of the two Cu(II) ions within the i-th trimer, → S i denotes the classical spin of the Fe(III) ion of that trimer, and → H is the external magnetic field, and the partial Hamiltonians real where isotropic Heisenberg exchange interactions between the constituent ions are assumed and the Zeeman terms introduced. In addition to the coupling constant J 1 , describing the superexchange interaction between the two Cu(II) ions of the trimer unit, two different superexchange coupling constants J 23 (= J 2 = J 3 ) and J 45 (= J 4 = J 5 ) alternating along the chain are assumed. The corresponding partition function may be written as where  [67], if only the exchange couplings in the system are isotropic, the calculation can be performed rigorously. Taking in the final step the thermodynamic limit ( N → ∞ ) one obtains the following expression for the zero-field susceptibility of the FeCu 2 chain unit where the quantities ρ, ρ α ', and ρ α " (α = 0, 1) are dimensionless functions of J 1 , J 23 , J 45 , and β, and their definitions are provided in the Supporting Information. There is no rigorous way one can introduce the interchain interactions into the model. Therefore, we decide here to employ the molecular field approximation, which yields the molar susceptibility of the interacting FeCu 2 chain unit χ CCU (CCU stands for Coupled Chain Unit) in the following form where zJ is the effective interchain coupling constant, and g = 3 g 2 Cu g Fe is the average spectroscopic factor of the FeCu 2 chain unit.

MS and SC Results
Let us start the presentation of the results with the analysis of the high-temperature behavior of the χ −1 signal by employing the molecular field theory. The MF theory was demonstrated above to give rise to the specific prediction for the high-temperature regime quoted in Equation (3a,b). The function (χ MF + χ 0 ) −1 was fitted to the experimental data of the inverse susceptibility above 80 K. All parameters g Cu , g Fe , J 1 , J 24 , J 35 , and χ 0 were relaxed during the fitting run. The best fit shown in Figure 8b by the solid line yielded the agreement quotient of  [68] and in oligonuclear Fe(III)-Co(III) compound with oxido-, sulfato-, and cyanido-bridging ligands (~0.000985 cm 3 ·mol −1 ) [69]. Preliminary calculations of the χT signal using the SC chain model with an additive temperature-independent susceptibility correction χ 0 showed a large discrepancy between the experimental and calculated values (the calculated signal was substantially larger in the low temperature regime). This indicated the need to take into account the interchain interactions. They originate from the system of hydrogen bonding, π-π stacking contacts, and finally from the through-space dipole-dipole coupling of the constituent magnetic moments. The reality-faithful introduction of the interchain coupling into the procedure would pose a cumbersome and complex computational problem, therefore we decided to conduct it within the simple and well-known molecular field approximation, where the resultant susceptibility signal is calculated according to the formula in Equation (8). The trials to relax the whole set of parameters, g Cu , g Fe , J 1 , J 23 (= J 2 = J 3 ), J 45 (= J 4 = J 5 ), χ 0 , and zJ' were all unsuccessful failing to reproduce the low-temperature end of the χT signal, although the values of the coupling constants J 23 and J 45 fell very close. Therefore, we decided to reduce the number of fitted parameters by setting these coupling constants equal. Just thereon we observed an instant improvement of the fit quality resulting in an excellent agreement of the model with the experimental data, however it involved an unphysical prediction of g Cu = 1.28 (4), and, therefore, must be dismissed. In the next and final step, we carried out the fitting procedure with the Landé factor of the Cu(II) ions fixed at the value of g Cu = 2.0. The ensuing fit is shown in Figure 8a by the solid line and yielded the satisfactory agreement quotient of  [68,69]. And finally, the interchain coupling constant is of plausible magnitude and negative, which implies an antiferromagnetic arrangement of magnetic moments originating in adjacent chains. The solid line in Figure 8c shows the shape of the Brillouin function corresponding to a single Fe(III) ion (S Fe = 5/2) with the Landé factor equal to the best fit value g Fe = 2.065. A good agreement is consistent with the strong antiferromagnetic coupling between the Cu(II) ions. A small discrepancy is observed at intermediate field values, most probably due to the state of weak frustration, which is the case with all coupling constants J 1 to J 5 being negative.

Magnetostructural Comparison
In the reported structure, copper(II) cations are close to each other (5.132 Å) and the bridge geometry given by coplanar arrangement of Cu1 and Cu2 basal planes (12.57 • ) as well as angles between basal planes and bridging oxalate (3.40 and 9.54 • ) result in strong antiferromagnetic Cu-Cu coupling (−275 cm −1 ). Table S2 shows a list of compounds containing the oxalate-bridged Cu(II) dimer units together with the corresponding values of the Cu(II)-Cu(II) exchange coupling constant. It can be seen that the magnetic coupling ranges from −400 cm −1 to weak antiferromagnetic or ferromagnetic coupling. The studied compound falls onto the weaker side of the strong antiferromagnetic coupling, being most close to compounds 3 or 38. It is well established for oxalate-bridged Cu(II) complexes [70][71][72] that the value and type of the exchange coupling is essentially determined by the magnitude of the overlap between the symmetry-adapted highest occupied molecular orbitals of the oxalate ligand and the metal-centered magnetic orbitals. If the four oxalate oxygen atoms are coordinated with short bond distances to each Cu(II) center in a way that is coplanar with the singly occupied molecular orbitals (SOMOs) of the copper atoms (coplanar topology) the strong antiferromagnetic coupling arises. On the other hand, if the oxalate ligand behaves as an asymmetric bis-bidentate bridging ligand and the two metal-centered magnetic orbitals are parallel to each other and perpendicular to the oxalate ligand (perpendicular topology), a weak ferromagnetic (accidental orthogonality) or antiferromagnetic coupling is implied. The full discussion of the geometric parameters affecting the bridge geometry, and hence, possibly influencing magnetic properties is given in the Supplementary Materials (Figures S10-S14, Table S2).

Materials and General Procedure
The starting K 3 [Fe(ox) 3 ]·3H 2 O [73] and [Cu(bpy) 2 (NCS)](NO 3 ) [74] complexes were prepared according to the literature procedures. Other reagents used in the synthesis were of analytical grade and used without further purification. Elemental analysis (C, H, N) was carried out with a Vario MACRO analyser. IR spectrum was recorded on a Perkin Elmer FT-IR 2000 spectrophotometer in the 4000-400 cm −1 region using KBr discs. Thermal behavior was studied on an SDT 2600 TA Instruments by simultaneous thermogravimetric analysis (TGA) and differential thermal analysis (DTA) in a stream of synthetic air up to 1000 • C. The powder diffraction patterns were collected using a Phillips X'Pert Pro diffractometer equipped with an X'Celerator Scientific RTMS detector using CuK α radiation. The diffractograms were registered with step of 0.017 • 2θ and exposure time 300 s in the range 3 < 2θ < 50 • for NCU-1 and 180 s in the range 5 < 2θ < 120 • for the products of the thermal analysis. X-ray absorption spectra were recorded at the National Synchrotron Radiation Centre SOLARIS at the bending magnet PEEM/XAS beamline for Fe (680-770 eV), Co (750-920 eV) and Cu (900-1050 eV) L 2,3 -edges. The sample was finely ground and attached to double-sided adhesive conductive graphite tape. The measurements were performed with the step size of 0.2 eV for the pre-edge region, 0.1 eV for the edge regions, and 0.5 eV for the high energy part. The data sets were collected at room temperature in ultra-high vacuum (UHV) using total electron yield mode (TEY). The measurements were repeated at least five-fold. The data were processed using the ATHENA program from Demeter package [75]. Magnetic measurements in the temperature range 1.8-300 K (µ 0 H = 0.1 T) and in the magnetic field range 0-7 T (T = 1.8 K) were performed using a SQUID MPMS-3 magnetometer, in a sample holder made from a small plastic envelope with very well estimated diamagnetic characteristics. The raw data have been corrected for the diamagnetic contribution of the sample holder measured in a separate run. The diamagnetic susceptibility of the studied compound estimated using Pascal constants was found to amount to −660 × 10 −6 cm 3 ·mol −1 , however, it was not subtracted from the measured susceptibility. Instead, it will be taken into account within the following fitting procedures in the form of an additive correction χ 0 together with the expected positive temperature-independent contribution (TIP, the second-order Zeeman contribution) from the off-chain Co(III) diamagnetic ion and two Cu(II) ions.

Single Crystal X-ray Diffraction Measurements
The preliminary experiments were carried out at room temperature using an Oxford Diffraction Sapphire CCD diffractometer, MoKα radiation λ = 0.71073 Å. However, due to the large b value, a significant spot overlapping was observed, and hence, the symmetry and this cell parameter were erroneously identified as P2/c and 24.682(4) Å, respectively. The final diffraction data of the studied compound were collected at 100 K on MX14-2 beamline (Helmholtz Zentrum Berlin, Bessy II). First, the data were processed in xdsapp software [76,77], and subsequently CrysAlis Pro [78] was used to apply the numerical absorption correction. The structure was solved by the direct methods and refined with the full-matrix least-squares procedure on F 2 (SHELX 2013/4) [79]. All heavy atoms were refined with anisotropic displacement parameters. Positions of hydrogen atoms were assigned at the calculated positions with thermal displacement parameters fixed to a value of 20% higher than those of the corresponding carbon atoms. There are 15 water positions accounting for 8.5 water molecules given in the formula. ISOR restraints were applied for some atoms, mainly partially occupied water molecules to assure stable refinement. All figures were prepared in DIAMOND and ORTEP-3 [80,81]. The results of the data collection and refinement have been summarized in Table S1. Additional single crystal experiments were performed also at MX14-2 beamline for crystals soaked over 48-72 h in acetonitrile and bromobenzene.

Water Adsorption-Desorption Measurements
The detailed specification of the implemented procedure, was described elsewhere [82][83][84]. Briefly, water adsorption-desorption measurements were performed at the temperature of 25 • C using a typical gravimetric adsorption apparatus equipped with the Baratron pressure transducers (MKS Instruments, München, Germany). Before the measurements, each sample was thermally desorbed under a high vacuum until a constant mass was obtained (usually after 3 days).

In-Situ DRIFT Investigations
Water adsorption was performed under isobaric conditions (p = 4 kPa by flowing He gas through H 2 O scrubber at 25 • C). By changing the temperature of the chamber (A Praying Mantis in-situ cell from Harrick Scientific Corporation) up to 120 • C (with the ramp 1 • C/min), the adsorption isobars were obtained. The construction of this cell enables the thermal treatment of the powdered sample up to 600 • C in any controlled atmosphere or in vacuum. The IR spectra of the samples were recorded (using Nicollet S10, Thermo Scientific, Waltham, MA, USA) with a period of 2 min.

Conclusions
Tending to develop new multimetallic coordination complexes [85,86], we report the original architecture {[Co(bpy) 2 (ox)][{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ]} n ·8.5nH 2 O NCU-1, as a product of the self-assembly between the complex building block originating from the recombination of [Co(H 2 O) 6 ]Cl 2 , [Cu(bpy) 2 NCS](NO 3 ) and K 3 [Fe(ox) 3 ] in aqueous solution. The molecular recognition led to the occurrence of oxalate-bridged 1D [{Cu 2 (bpy) 2 (ox)}Fe(ox) 3 ] − ∞ ladders of very rare topology, shown only very recently to crystallize with simple alkali metal cations. In NCU-1, however, these molecular 1D modules co-crystallize with much larger in situ formed [Co(bpy) 2 (ox)] + cations to produce a new robust porous architecture stabilized by charge-assisted hydrogen bonds and π-π interactions. The sorption studies coupled with the IR studies indicated the full reversibility of quantitative sorption/desorption of H 2 O over the hydrophilic surface within the porous space 963.7 Å 3 per one cell (16.9% of cell volume). Thus, NCU-1 exhibits an interesting hybrid porous molecular system combining the structural features of MOFs and HOFs. Finally, considering a relatively complicated 1D ladder topology of NCU-1, we developed our own general approach to optimize the description of super-exchange magnetic interactions in the like systems. The presented studies could be important from the viewpoint of a still developing field of multicomponent modular systems.
The presented studies could be important from the viewpoint of the still developing field of multicomponent modular systems. While the individual molecular architecture of NCU-1 seemed to be unavailable using the direct self-assembly method from the building blocks, we conclude that its overall scheme may be advantageous towards the creative design through the systematic modular structure-property modification approach. Each of the NCU-1 components, namely anionic bimetallic chain, monometallic cationic complex, and crystallization solvent molecules creates its own specific zone ( Figure 10). It is quite easy to imagine that other cationic species of the functional potential, e.g., the spin-crossover complexes (switchability) or non-innocent organic cations (electronic conductance) may be arranged in the dedicated 1-dimensional space (orange zone in Figure 10) to shape the separate functional subnetwork. The implementation of the building blocks of diverse size or/and electronic charge should implicate, on the other hand, the tuning of solvent accessible space zone, to reinforce the sorption potential (green zone in Figure 10). This functionality might be also built up by a systematic use of accessible oxalato ligands analogues, e.g., broad family of anilato ligands, through the formation of analogous (or modified) coordination arrangement (blue zone in Figure 10).
is quite easy to imagine that other cationic species of the functional potential, e.g., the spincrossover complexes (switchability) or non-innocent organic cations (electronic conductance) may be arranged in the dedicated 1-dimensional space (orange zone in Figure 10) to shape the separate functional subnetwork. The implementation of the building blocks of diverse size or/and electronic charge should implicate, on the other hand, the tuning of solvent accessible space zone, to reinforce the sorption potential (green zone in Figure 10). This functionality might be also built up by a systematic use of accessible oxalato ligands analogues, e.g., broad family of anilato ligands, through the formation of analogous (or modified) coordination arrangement (blue zone in Figure 10).  Supplementary Materials: The supporting information can be downloaded at: https://www.mdpi. com/article/10.3390/ijms23031556/s1.