Selective Formation, Reactivity, Redox and Magnetic Properties of MnIII and FeIII Dinuclear Complexes with Shortened Salen-Type Schiff Base Ligands.

The reactivity of the shortened salen-type ligands H3salmp, H2salmen and H2sal(p-X)ben with variable para-substituent on the central aromatic ring (X = tBu, Me, H, F, Cl, CF3, NO2) towards the trivalent metal ions manganese(III) and iron(III) is presented. The selective formation of the dinuclear complexes [M2(μ-salmp)2], M = Mn (1a), Fe (2a), [M2(μ-salmen)2(μ-OR)2)], R = Et, Me, H and M = Mn (3a-c) or Fe (4a-c), and (M2(μ-sal[p-X]ben)2(μ-OMe)2), X = tBu, Me, H, F, Cl, CF3, NO2 and M = Mn (5a-g) or Fe (6a-g), could be identified by reaction of the Schiff bases with metal salts and the base NEt3, and their characterization through elemental analysis, infrared spectroscopy, mass spectrometry and single-crystal X-ray diffraction of 2a·2AcOEt, 2a·2CH3CN and 3c·2DMF was performed. In the case of iron(III) and H3salmp, when using NaOH as a base instead of NEt3, the dinuclear complexes [Fe2(μ-salmp)(μ-OR)(salim)2], R = Me, H (2b,c) could be isolated and spectroscopically characterized, including the crystal structure of 2b·1.5H2O, which showed that rupture of one salmp3- to two coordinated salim- ligands and release of one salH molecule occurred. The same hydrolytic tendency could be identified with sal(p-X)ben ligands in the case of iron(III) also by using NEt3 or upon standing in solution, while manganese(III) did not promote such a C-N bond breakage. Cyclic voltammetry studies were performed for 3b, 4b, 5a and 6a, revealing that the iron(III) complexes can be irreversibly reduced to the mixed-valence FeIIFeIII and FeII2 dinuclear species, while the manganese(III) derivatives can be reversibly oxidized to either the mixed-valence MnIIIMnIV or to the MnIV2 dinuclear species. The super-exchange interaction between the metal centers, mediated by the bridging ligands, resulted in being antiferromagnetic (AFM) for the selected dinuclear compounds 3b, 4b, 5a, 5e,5f, 6a and 6e. The coupling constants J (-2JŜ1·Ŝ2 formalism) had values around -13 cm-1 for manganese(III) compounds, among the largest AFM coupling constants reported so far for dinuclear MnIII2 derivatives, while values between -3 and -10 cm-1 were obtained for iron(III) compounds.

1. Introduction

n class="Chemical">Salenpan>-related [1] pan> class="Chemical">Schiff bases bearing only one carbon atom between the two iminic C=N bonds of the condensed salicylaldehyde (salH) moieties are known as H3salmp (N,N′-bis(salicylidene)-2-hydroxyphenylmethanediamine), H2salmen (N,N′-bis(salicylidene)methanediamine) and H2salben (N,N′-bis(salicylidene)phenylmethanediamine) (Figure 1). H3salmp can be easily obtained by the reaction of three moles of salH and two moles of ammonia [2], and there are reports of its synthesis since the beginning of the 20th century [3]. H2salben’s derive from H3salmp via substitution of the central salH moiety by reaction with variably substituted benzaldehydes [4], while H2salmen can be obtained by reaction of salH with either methanediamine [5], formaldehyde and ammonia [6] or hexamethylenetetramine [7]. Even if some reports indicate mononuclear complexes with a metal:ligand (M:L) 1:1 ratio [8,9,10,11,12,13,14,15,16,17] as H2salen [18], such shortened ligands preferentially form oligonuclear metal complexes [19,20] due to the tension of the four-membered MNCN metallacycle in a hypothetic mononuclear compound. To the best of our knowledge, there is only one reported X-ray structure in which the two iminic nitrogen atoms coordinate to the same metal ion, (Zr(Hsalmp)2) [21]. However, in this compound the M:L ratio is 1:2 and the zirconium(IV) ion is octacoordinated with rather long bond distances (2.1–2.4 Å), which lowers the tension given by the four-membered metallacycle.

Figure 1

Pentadentate N2O3 (H3salmp), tetradentate N2O2 (H2salen, H2salmen and H2sal(p-X)ben, X = tBu, Me, H, F, Cl, CF3, NO2) and bidentate NO (Hsalim) Schiff bases.

With the exn class="Chemical">ceppan> class="Chemical">tion of H3salmp, for which quite a few complexes have been synthesized and structurally characterized up to date [10,21,22,23,24,25,26,27,28,29,30], less is known about the other two classes of shortened Schiff base derivatives [7,11,19,20,31]. Nevertheless, it is undeniable the usefulness of all these ligands for the synthesis of efficient catalysts [15,16,17], their use for metal sequestration in solution [32], synthesis of biomimetic systems [24] and the fascinating magnetic properties of the corresponding oligonuclear clusters [19,20,23,24,26,27,28,31,33]. Within this last topic, at the beginning of the new Millennium we started a systematic study on the coordination ability of H2salmen and H2salben with divalent metal ions [11] like copper(II) [19] and cobalt(II) [20,31], and the possibility to oxidize the latter to cobalt(III) and additionally form mixed-valence oligonuclear clusters [20,31]. In this work we aim to describe in detail the reactivity of these ligands toward manganese(III) and iron(III) in order to enrich the scenario with the coordination ability of H3salmp [26,27,28,34], H2salmen and H2salben towards these two trivalent ions. In particular, the formation of dinuclear complexes is confirmed by single-crystal X-ray diffraction structural studies on several derivatives. Furthermore, cyclic voltammetry (CV) measurements on selected so-obtained dinuclear complexes (Table 1) are presented in order to understand the redox properties of the metal ions conferred by the ligands, together with the temperature dependence of their magnetic moment, providing quantitative insight into the super exchange interaction between the bridged metal ions.

Table 1

Formulae and codes of dinuclear compounds object of study in this paper.

Formula	Compound Code
[M2(μ-salmp)2]	1a (M = Mn), 2a (M = Fe)
[Fe2(μ-salmp)(μ-OR)(salim)2]	2b–c (R = Me, H)
[Mn2(μ-salmen)2(μ-OR)2]	3a–c (R = Et, Me, H)
[Fe2(μ-salmen)2(μ-OR)2]	4a–c (R = Et, Me, H)
[Mn2(μ-sal(p-X)ben)2(μ-OMe)2]	5a–g (X = tBu, Me, H, F, Cl, CF3, NO2)
[Fe2(μ-sal(p-X)ben)2(μ-OMe)2]	6a–g (X = tBu, Me, H, F, Cl, CF3, NO2) 1

1 only 6a, 6c and 6e could be isolated in the solid state.

2. Results and Discussion

2.1. Synthesis of the Shortened Schiff Bases and Crystal Structures of H2sal(p-X)ben (X = tBu, CF3)

The n class="Chemical">Schiff bases pan> class="Chemical">H3salmp [2], H2salmen [5] and H2sal(p-X)ben (X = tBu, Me, H, F, Cl, CF3, NO2) [4,11,19,20,31] (Figure 1), used in this paper as ligands for manganese(III) and iron(III) (Table 1), were obtained following the synthetic procedures reported in the literature. Some of them have been structurally characterized and previously described in the literature; in particular, the X-ray crystal structures of H2sal(p-NO2)ben [31], H2salmen [6] and H3salmp [35] are available. We could obtain good crystals suitable for X-ray diffraction of the compounds H2sal(p-tBu)ben and H2sal(p-CF3)ben by slow evaporation of their chloroform solutions. The crystal structures could be solved, and the perspective views of these molecules are shown in Figure 2. Bond lengths and angles are compatible with Schiff base structures derived from salH and diamines where the enolimine tautomer is favored over the ketoamine form [6,31,35].

Figure 2

Crystal structures of (a) H2sal(p-tBu)ben and (b) H2sal(p-CF3)ben with atom numbering; color code: O = red, N = blue, C = grey, H = white, F = turquoise, intramolecular H-bond = dashed black line. Molecule (a) is located on a crystallographic mirror plane passing through atoms C8, C9, C12 and C13, and the tBu group is disordered (only one conformation is shown).

The n class="Chemical">H2sal(pan> class="Chemical">p-tBu)ben molecule is located on a crystallographic mirror plane, passing through atoms C8, C9, C12 and C13. This leads the tBu group to be disordered with two different conformations having occupancy of 0.5 each. No relevant intermolecular interactions below the sum of the van der Waals radii were observed in the crystal packing. The H2sal(p-CF3)ben molecule instead showed significant C–H···F intermolecular interactions as depicted in Figure S1 in Supplementary Materials, where a portion of the crystal packing is reported. In both cases, the molecules adopted a conformation mainly determined by the presence of strong intramolecular O–H···N hydrogen bonds (H-bonds) involving the phenolic groups and the iminic nitrogen atoms of the same sal moiety of the molecule (O1–HO1···N1, rO···N = 2.608(2) Å, OH···N angle = 138° in H2sal(p-tBu)ben, and O1–HO1···N1 and O2–HO2···N2, rO···N = 2.612(9) and 2.608(9) Å, respectively, with an average OH···N angle = 147° in H2sal(p-CF3)ben).

2.2. Synthesis, Isolation and Reactivity of Dinuclear Complexes with H3salmp

As stated above, the most studied ligand for n class="Chemical">complexapan> class="Chemical">tion of iron(III) and manganese(III) is H3salmp, where MIII2 complexes have been isolated, M = Mn (1a) and Fe (1b), together with their mixed-valence MIIMIII and reduced MII2 dinuclear species [26,27,28,34]. Oxidation to MnIIIMnIV and MnIV2 has also been achieved through cyclic voltammetry [27]. Due to the rich chemistry and the range of accessible oxidation states, we then decided to start our synthetic and reactivity studies by obtaining 1a and 2a while modifying the reaction conditions.

Instead of using n class="Chemical">MnCl2, pan> class="Chemical">salH and NH3 in boiling EtOH with ligand assembly directly in the reaction mixture followed by metal oxidation in air [27], H3salmp was first isolated, suspended in MeOH and NEt3 as a deprotonating agent and reacted with Mn(AcO)3·2H2O, Equation (1). After a few hours at room temperature (RT), 1a was isolated as a dark brown powder with two cocrystallized water molecules, whose elemental analysis, infrared and mass spectra confirmed the intactness of the ligand and the dinuclear nature of the complex. Substitution of MeOH with DMF as solvent caused a lowering in the yield of isolated product, together with cocrystallized DMF in substitution of water. This was confirmed by both elemental analysis and infrared spectroscopy, where the C=O stretching band of DMF at 1663 cm−1 was present [36,37,38]. Furthermore, the synthesis was also tested without the addition of NEt3, thanks to the role of the acetate anion as base, and the dinuclear species 1a was also suitably isolated, even if in lower yields. 2 H

The same results were obtained in the n class="Chemical">case of pan> class="Chemical">iron(III) (either chloride or nitrate salt) with the isolation of 2a as red-brown solid, Equation (1), similar to what has been reported in the literature using boiling EtOH [34]. 2a also cocrystallized with H2O or DMF molecules, and especially in the latter case this was clearly detected from the infrared spectrum with the C=O stretching of DMF at 1668 cm−1. Use of CH3CN as solvent was also tested in this case, causing the undesired coprecipitation of Et3NHCl salt together with the product, which forced extensive washing of the obtained solid with a MeOH:H2O 1:1 mixture. Nevertheless, all isolated compounds showed m/z signals at 799, 821 and 1618, attributable to [M + 1]+, [M + Na]+ and [2M + Na]+ ions, respectively, diagnostic of the intact dinuclear species [Fe2(μ-salmp)2]. Crystallization of the reaction mixtures in DMF and CH3CN with AcOEt and iPr2O, respectively, yielded crystals of 2a·2AcOEt and 2a·2CH3CN suitable for single-crystal X-ray diffraction studies (see below), further confirming the invariability of the obtained dinuclear species.

The use of n class="Chemical">NaOH inpan> subspan> class="Chemical">titution of NEt3 as a base in the reaction did not alter the isolation of the dinuclear manganese(III) 1a, while it invariably caused the rupture of one salmp3− to two salim− (Figure 1) fragments with iron(III), and substitution of the central phenoxido bridging oxygen atom with a methoxido or hydroxido bridging ligand, depending whether the reaction was conducted in MeOH or DMF, respectively, obtaining 2b or 2c, Equation (2). The reaction was not tested in CH3CN due to the concomitant precipitation of Et3NHCl. The coordinated salim− ligands were immediately recognized by infrared spectroscopy, with the presence of N–H stretching in the spectrum as a narrow band at 3302 cm−1. The C=N stretching also shifted to 1615 cm−1, probably due to the change in the coordination environment (see below) and the presence of two different C=N bonds (salmp3− and salim−). Mass spectra of both 2b and 2c showed the main peaks at m/z 749 and 606 ascribable to [Fe2(salmp)(salim)2(OMe) + Na]+ and [Fe2(salmp)(salim)(OMe)]+ ions, which undoubtedly proved the new dinuclear species obtained. The absence of any difference between the two compounds was safely ascribed by the fact that the mass spectra were registered in MeOH, which caused a rapid OH ↔ OMe scrambling in solution. We also obtained single crystals of 2b·1.5H2O suitable for X-ray diffraction by diffusion of iPr2O into the methanolic reaction mixture, confirming the structure of the dinuclear compound (see below). 2 H

2.3. Dinuclear Complexes with Tetradentate Ligands and Reactivity in Solution

Moving to the tetradentate ligands, rean class="Chemical">cpan> class="Chemical">tion of manganese(III) acetate and iron(III) chloride with H2salmen was performed in three different solvents, EtOH, MeOH or DMF. In the absence of the central phenoxido unit provided by salmp3−, the dinuclear species [M2(μ-salmen)2(μ-OR)2], M = Mn, 3a–c, and Fe, 4a–c, with R = Et, Me and H, respectively, were obtained, Equation (3). The fifth coordinating oxygen atom of the pentadentate salmp3− was here replaced by the bridging alkoxido/hydroxido groups, while maintaining the same dinuclear structure. The bridging OH− groups in 3c and 4c should be provided either by the crystallization water molecules of Mn(AcO)3·2H2O or by the amount of water present in the solvent when operating in DMF, especially in the case of the iron(III) derivative. This was also confirmed by the crystallization of 3b from DMF-iPr2O, which yielded crystals of 3c·2DMF, where the OMe ↔ OH scrambling occurred within the crystallization time (see below). Together with the elemental analyses, the composition of these complexes was confirmed by mass spectrometry; for example, peaks at m/z 727 and 729, even if weak, due to [Mn2(salmen)2(OEt)2 + Na]+ and [Fe2(salmen)2(OEt)2 + Na]+ ions, were observed in the case of 3a and 4a, respectively, together with signals of species obtained by the OEt ↔ OMe scrambling in methanolic solutions, such as [M2(salmen)2(OMe)]+ at m/z 645 and 647 for M = Fe and Mn, respectively. 2 H

Rean class="Chemical">cpan> class="Chemical">tivity of H2sal(p-X)ben with manganese(III) acetate in MeOH and Et3N revealed to be superimposable with the case of H2salmen, and the series [Mn2(sal(p-X)ben)2(OMe)2], 5a–g, with X = tBu, Me, H, F, Cl, CF3, NO2, respectively, was obtained in acceptable yields, Equation (4). Infrared spectra showed the C=N stretching around 1620 cm−1, with no modulating effect by the para substituent X, as expected for the absence of conjugation with the C=N bonds. Mass spectra displayed the most intense peaks at m/z corresponding to [M – OMe]+ species, together with [M + 1]+ and [M + Na]+ signals at variable intensities, which guaranteed the integrity of the dinuclear complexes. 2 H

In the n class="Chemical">case of the reapan> class="Chemical">ction of iron(III) salts (mostly nitrate due to the easier handling compared to FeCl3) with H2sal(p-X)ben, as already shown by reaction with H3salmp in the presence of NaOH, the tendency of the dinuclear complexes [Fe2(sal(p-X)ben)2(OMe)2], 6a–g, to hydrolyze directly in the reaction mixture, even working with NEt3, was enhanced. In fact, we isolated solid phases with good purity of only 6a (tBu), 6c (H) and 6e (Cl) by adjusting the reaction time to about 1 h, Equation (4). The mass spectra of freshly prepared methanolic solutions of the three compounds showed mass peaks attributable to [M – OMe]+, [M + 1]+ and [M + Na]+ positive ions, as sign of the structural integrity. Furthermore, no N–H stretching at about 3300 cm−1 of salim− ligands could be detected in their infrared spectra, which would have been hint of hydrolyzed sal(p-X)ben2−, and stretching of the iminic C=N bond appeared at 1614 cm−1 in all cases.

The mass spen class="Chemical">ctrum of 6a inpan> a methanpan>ol solupan> class="Chemical">tion aged for 1 day, instead, completely changed, and new peaks at m/z 678, 767 and 821 appeared, assigned to [Fe2(sal(p-tBu)ben)(salim)(OMe)2]+, ([Fe2(sal(p-tBu)ben)(salim)2(OMe)]+ and [Fe2(sal(p-tBu)ben)(salim)2(OMe)2 + Na]+, respectively, while the intensity of the peak at m/z 911 [M – OMe]+, which was the most intense one in the fresh solution, almost disappeared, with a relative intensity of only 5%. Similar results were also obtained with 6e, and this hints at the hydrolytic tendency of these iron(III) compounds also in the absence of other reagents, such as the base, Equation (5). [Fe

In the n class="Chemical">case of 6b (Me), 6d (F), 6f (pan> class="Chemical">CF3) and 6g (NO2), after 1 h of stirring the reaction mixture, or in the case of 6c (H) after a longer reaction time, no or very little solid was left and only deep red solutions were formed. Precipitation upon addition of water or iPr2O (followed by washing with water in order to eliminate residual salts) yielded brown-red solids, whose infrared spectra invariably showed the N–H stretching of salim− ligands as a sharp band in the 3296–3316 cm−1 range, together with the C=O stretching bands of the released p-X-benzaldehyde at 1700–1720 cm−1, Equation (5). Surprisingly, in the case of 6c and 6d, we detected the same mass peaks at m/z 606 and 749, also corresponding to the signals present in the mass spectrum of 2b. This suggests that, when the hydrolysis takes place on both sal(p-X)ben2− ligands, probably accelerated by the addition of water, formation of the stable dinuclear unit [Fe2(μ-salmp)(μ-OMe)(salim)2] occurs with rearrangement of the salim− fragments to recompose the coordinated salmp3− ligand, promoted by the stabilizing effect of the bridging phenoxido oxygen atom.

2.4. Molecular Structures of ·2AcOEt, ·2CH3CN, ·1.5H2O and ·2DMF

As reported above, we n class="Chemical">could obtainpan> crystals suitable for single-crystal X-ray diffraction studies of 2a·2AcOEt, 2a·2CH3CN and 2b·1.5H2O by slow diffusion of AcOEt, iPr2O and again iPr2O into the DMF, CH3CN and MeOH reaction mixtures, respectively. This was necessary especially for 2a, which is practically insoluble in all solvents but DMF, as also stated in the literature [34]. The same poor solubility in almost all common solvents was observed for the other four series 3–6 with tetradentate ligands, and only in the case of 3b we obtained a DMF solution with a sufficiently high concentration to allow the crystallization of 3c·2DMF through liquid diffusion of iPr2O, with concomitant OMe ↔ OH scrambling. The strong tendency of these complexes to cocrystallize with several solvent molecules was already reported [23,27] and here was clearly confirmed.

Details of the n class="Chemical">crystal strupan> class="Chemical">cture solution and refinement are listed in Table S1 in Supplementary Materials, while selected bond lengths and angles are summarized in Table 2 and Table 3. Data collection was performed at room temperature for all crystals, and structural parameters of 2a·2CH3CN and 2a·2AcOEt can be compared with both 2a·2DMF [34] and the manganese(III) derivative 1a·2CH3CN [27] in order to show the changes caused by solvent and metal ion. Comparison of the structure of 2a·2CH3CN at room temperature with the one previously reported at low temperature (153 K) [23] revealed little modification.

Table 2

Selected bond distances (Å) and angles (°) of 2a·2AcOEt, 2a·2CH3CN, 2a·2DMF [34], 1a·2CH3CN [27] and 3c·2DMF, all collected at room temperature 1,2.

Parameter	2a·2AcOEt 3	2a·2CH3CN 3	2a·2DMF 3	1a·2CH3CN 4	3c·2DMF 4
M–O1	1.897(2)	1.896(2)	1.894(3)	1.857(3)	1.9025(7)
M–O2’	1.917(2)	1.905(2)	1.921(3)	1.952(3)	1.9123(6)
M–N1	2.142(2)	2.164(2)	2.156(3)	2.088(3)	2.0018(7)
M–N2’	2.149(2)	2.144(2)	2.138(3)	2.196(3)	2.0027(7)
M–O3	2.033(2)	2.028(2)	2.023(2)	2.239(3)	1.8006(6)
M–O3’	2.059(2)	2.057(2)	2.064(2)	1.900(3)	1.7973(6)
M···M’	3.071(1)	3.091(2)	3.063(1)	3.111(1)	2.6357(4)
M–O3–M’	97.24(9)	98.32(7)	97.06(9)	97.1(1)	94.20(2)
O3–M–O3’	82.76(9)	81.68(7)	82.94(9)	82.9(1)	85.80(2)
O1–M–O2’	94.17(12)	94.24(8)	93.6(1)	93.3(1)	88.79(3)
O2’–M–O3	91.78(10)	92.07(8)	91.6(1)	93.0(1)	91.89(3)
O1–M–O3’	92.68(10)	93.69(7)	93.4(1)	91.0(1)	93.54(3)
O2’–M–N2’	87.04(10)	86.97(7)	88.3(1)	86.5(1)	90.82(3)
O2’–M–N1	107.03(10)	107.62(8)	101.3(1)	113.2(1)	95.02(3)
O1–M–N2’	102.91(9)	102.64(7)	108.4(1)	95.4(2)	91.82(3)
O1–M–N1	88.42(10)	87.86(7)	87.0(1)	90.9(1)	91.78(3)
O3–M–N2’	85.07(9)	86.42(7)	86.9(1)	79.9(1)	88.50(3)
O3–M–N1	82.47(9)	81.89(7)	82.5(1)	80.1(1)	87.83(3)
O3’–M–N2’	82.37(9)	81.75(7)	81.8(1)	85.2(1)	86.87(3)
O3’–M–N1	82.44(9)	82.44(7)	81.8(1)	86.4(1)	87.15(3)
O2’–M–O3’	168.44(9)	167.40(6)	170.5(1)	166.0(1)	176.76(3)
O1–M–O3	170.27(9)	169.21(6)	167.8(1)	173.6(1)	179.25(3)
N1–M–N2’	161.42(9)	161.53(7)	161.4(1)	159.1(1)	173.20(3)

1 Primed atoms are related to the unprimed atoms by an inversion center; 2 literature data were adapted in order to maintain the same atom numbering applied in this work; 3 M = Fe; 4 M = Mn.

Table 3

Selected bond distances (Å) and angles (°) of 2b·1.5H2O 1.

Molecule A	Value	Molecule B	Value
Fe1–O1	1.917(3)	Fe2–O5	1.908(4)
Fe1–O2	2.069(3)	Fe2–O6	2.065(3)
Fe1–O3	1.940(3)	Fe2–O7	1.935(4)
Fe1–O4	1.985(2)	Fe2–O8	1.990(3)
Fe1–N1	2.175(3)	Fe2–N3	2.163(4)
Fe1–N2	2.086(4)	Fe2–N4	2.081(4)
Fe1···Fe1’ 1	3.149(1)	Fe2···Fe2” 2	3.151(1)
Fe1–O2–Fe1’ 1	99.1(2)	Fe2–O6–Fe2” 2	99.4(2)
Fe1–O4–Fe1’ 1	105.0(2)	Fe2–O8–Fe2” 2	104.7(2)
O1–Fe1–N2	95.05(15)	O5–Fe2–N4	93.42(18)
N2–Fe1–O2	89.20(14)	N4–Fe2–O6	87.43(17)
O2–Fe1–O4	77.17(12)	O6–Fe2–O8	77.20(15)
O4–Fe1–O1	98.27(15)	O8–Fe2–O5	101.20(18)
O1–Fe1–N1	86.93(14)	O5–Fe2–N3	86.42(16)
O1–Fe1–O3	98.41(13)	O5–Fe2–O7	97.23(15)
N2–Fe1–N1	88.33(15)	N4–Fe2–N3	85.93(19)
N2–Fe1–O3	86.05(14)	N4–Fe2–O7	86.84(18)
O2–Fe1–N1	83.15(15)	O6–Fe2–N3	83.68(19)
O2–Fe1–O3	91.89(15)	O6–Fe2–O7	92.79(19)
O4–Fe1–N1	89.41(15)	O8–Fe2–N3	89.42(18)
O4–Fe1–O3	94.91(15)	O8–Fe2–O7	96.72(18)
O1–Fe1–O2	169.10(15)	O5–Fe2–O6	169.98(19)
N2–Fe1–O4	166.35(14)	N4–Fe2–O8	164.35(17)
N1–Fe1–O3	172.56(14)	N3–Fe2–O7	172.08(18)

1 symmetry code: 1–x, y, z; 2 symmetry code: –x, y, z

2a·2An class="Chemical">cOEt, 3pan> class="Chemical">c·2DMF and 2a·2CH3CN (Figure 3 and Figure S2 in Supplementary Materials, respectively) crystallize in the triclinic P–1 space group with the complex molecule located about a crystallographic inversion center. In contrast, 2b·1.5H2O (Figure 4) crystallizes in the orthorhombic Pmc2 space group and the asymmetric unit consists of two independent molecules A and B, located about a crystallographic mirror plane. Besides minor conformational differences of the phenyl groups, the main difference between the two complex molecules is the presence of one (B) or two (A) H-bonded water molecules.

Figure 3

Perspective views of the dinuclear complexes in (a) 2a·2AcOEt and (b) 3c·2DMF with main atom numbering; color code: Fe = black, Mn = violet, O = red, N = blue, C = grey, H = white.

Figure 4

Crystal structures of (a) molecule A and (b) molecule B of 2b·1.5H2O with main atom numbering; color code: Fe = black, O = red, N = blue, C = grey, H = white, H-bond = dashed black line.

In the n class="Chemical">crystal strupan> class="Chemical">ctures of 2a·2AcOEt and 2a·2CH3CN the two iron(III) ions are bridged by two deprotonated pentadentate Schiff base ligands through the iminic nitrogen atoms connected by one carbon atom and the central phenoxido oxygen atom directly bound to both metal centers. Each iron atom is hexa-coordinate (N2O4) with a pronounced distorted octahedral geometry where, given by the bond distances, the equatorial plane is formed by four oxygen atoms, O1/O2 from the lateral sal moieties and O3/O3’ from the bridging phenoxido group of salmp3−, while the elongated axial positions are occupied by the two iminic nitrogen atoms. The greatest deviation from the octahedron is the nonlinearity of the N1–Fe–N2’ system, whose angle is smaller than the ideal value of 180° (161.42(9) and 161.53(7)° for 2a·2AcOEt and 2a·2CH3CN, respectively). The four equatorial oxygen atoms deviate from the O4 least squares (l.s.) plane of about 0.15–0.16 Å in 2a·2AcOEt and 0.16–0.17 Å in 2a·2CH3CN, while the iron(III) ions resides in this plane (deviations of 0.01 Å, in both cases). In fact, analyzing the structures, it is possible to identify a twist angle between O1FeO2 and O3FeO3’ l.s. planes of 13.0 and 14.3° for 2a·2AcOEt and 2a·2CH3CN, respectively. The phenoxido bridge forms an angle Fe–O3–Fe = 97.24(9) and 98.32(7)° in the two complexes, with concomitant Fe···Fe distance of 3.071(1) and 3.091(2) Å.

The An class="Chemical">cOEt molecules in 2a·2AcOEt interact with the dinuclear species through two C–H···O H-bonds between the carbonyl group and the central and one iminic C–H units of the salmp3− ligand (C8–H8···O4, rC···O = 3.332(7) Å, CH···O angle = 170.8°; C7–H7···O4, rC···O = 3.553(8) Å, CH···O angle = 156.3°). A picture of the crystal packing is shown in Figure S3 in Supplementary Materials. The CH3CN molecules in 2a·2CH3CN, instead, occupy voids within the [Fe2(μ-salmp)2] units. Comparing the two complexes here described with 2a·2DMF [34], the latter is more similar to 2a·2AcOEt regarding both the internal distortion of the octahedral coordination of the iron(III) ions and the solvent interaction. In fact, the DMF molecules also interact with the dinuclear complex through similar C–H···O H-bonds (C8–H13···O4, rC···O = 3.457(9) Å, CH···O angle = 159.5°; C7B–H15B···O4, rC···O = 3.50(1) Å, CH···O angle = 153.2°) as in the case of the AcOEt molecules. The shortest Fe⋯Fe intermolecular distances are 8.309(2), 9.233(2) and 10.179(3) Å for 2a·2AcOEt, 2a·2CH3CN and 2a·2DMF, respectively, which reflect the steric and electronic features of the solvent molecules and the different crystal packing in the three crystal structures.

In 2b·n class="Chemical">1.5H2O, the inpan>tapan> class="Chemical">ct salmp3− binds both iron(III) centers as in 2a·2solvent, i.e. through the three phenoxido oxygen atoms and the two iminic nitrogen atoms, behaving as pentadentate ligand. The two metal centers are bridged by three different connections: (i) the iminic nitrogen atoms, which are connected by one carbon atom, Fe1–N1–C8–N1’–Fe1’ and Fe2–N3–C29–N3”–Fe2” in molecules A and B, respectively (symmetry codes: ‘ = 1–x, y, z; “ = –x, y, z); (ii) the central phenoxido oxygen atoms of salmp3−, Fe1–O2–Fe1’ and Fe2–O6–Fe2”; (iii) the methoxido ions, Fe1–O4–Fe1’ and Fe2–O8–Fe2”. The two salim−, instead, derived from the hydrolysis of one salmp3−, behave as bidentate ligands for the same iron(III) ion, N2/O3 in molecule A and N4/O7 in molecule B; they invert the coordinative positions so that the nitrogen atom of salmp3− N1/N3 is in trans to the phenoxido oxygen atom of salim− O3/O7. Each iron is hexa-coordinate with a less pronounced octahedral distortion with respect to [Fe2(μ-salmp)2] (angle N1–Fe1–O3 = 172.6(1), N3–Fe2–O7 = 172.1(1)°). The Fe···Fe distance in this compound is 3.149(1) and 3.150(1) Å in molecules A and B, respectively. Unlike 2a·2solvent, the l.s. O3N equatorial planes in which the two iron ions reside are no longer coplanar, but there is an angle of 19.1(1) (A) and 21.1(1)° (B) between the two. The shortest Fe1⋯Fe2 intermolecular distance is 6.002 Å (Figure S5 in Supplementary Materials).

In the A moiety there are two n class="Chemical">water molecules OW1 and OW2 that interact via H-bonds with the oxygen atoms of salim− and MeO−, with distances OW1···O3 = 2.905(5), OW1···O4 = 3.001(6) and OW1···OW2 = 2.785(11) Å. In B instead only one OW3 water molecule interacts with the dinuclear complex with similar contacts (OW3···O7 = 2.932(6) and OW3···O8= 3.118(8) Å) (Figure 4).

In 3n class="Chemical">c·2pan> class="Chemical">DMF, each salmen2− acts as tetradentate ligand toward both manganese(III) ions, leading to Mn–N1–C8–N2–Mn’ bridges. In addition, there are two bridging hydroxido groups between the metal ions. The manganese(III) ion is hexa-coordinate (N2O4) with a slightly distorted octahedral geometry, where the four oxygen atoms with the shortest coordination distances form an almost flat equatorial plane (deviation of atoms of about 0.020 Å from the O4 l.s. plane, and manganese resides at 0.015 Å from it), and the highest deviation consists of the nonlinearity of the N1–Mn–N2’ system, 173.20(3)°, smaller than the ideal value (180°). The metal–N/O distances range from 2.0018(7)/ 2.0027(7) Å for Mn–N1/N2’ to 1.9025(7)/1.9123(6) Å for the phenoxido oxygen atoms O1/O2’ and 1.8006(6)/1.7973(6) Å of the hydroxido bridge O3/O3’. These last distances are quite short leading to a very compact Mn2O2 core where the two manganese(III) ions are very close each other (Mn···Mn’ = 2.6356(6) Å), if compared with 1a·2CH3CN (Mn···Mn’ = 3.111(1) Å) [27]. This is ascribable to the presence of the bridging phenoxido on the central ring in [Mn2(μ-salmp)2] that imparts further strain to the structure, as also evident by the strong asymmetry of the coordination sites of the two manganese(III) ions. This tension contribution is relieved in 3c·2DMF with the bridging salmen2− and OH− ligands, and in fact the two coordination sites are similar and, most important, the N1–Mn–N2 angle is closer to 180° (173.20(3)°) than in 1a·2CH3CN (159.1(1)°).

As observed in 2a·2n class="Chemical">DMF, the solvenpan>t molecule interacts with the dinuclear complex through two C–H···O H-bonds (C8–H8A···O4, rC···O = 3.328(1) Å, CH···O angle = 163.2°; C7–H7···O4, rC···O = 3.286(1) Å, CH···O angle = 160.6°). The overall crystal packing (Figure S4 in Supplementary Materials) leads to the shortest Mn⋯Mn intermolecular distance of 7.957(1) Å.

2.5. Cyclic Voltammetry Studies

n class="Chemical">CV measuremenpan>ts were pan> class="Chemical">conducted on four selected derivatives, two of them with manganese, 3b and 5a, and two with iron, 4b and 6a. Furthermore, 3b and 4b have salmen as Schiff base ligands, while 5a and 6a have sal(p-tBu)ben. Though they are scarcely soluble, their cyclic voltammograms were recorded in DMF solutions with 0.1 M tetrabuthylammonium hexafluorophosphate (TBAPF6) as a supporting electrolyte (Figure 5 and Figures S6–S8 in Supplementary Materials) and the obtained electrochemical parameters are summarized in Table 4.

Figure 5

CV scans of 5a in the oxidation region recorded in DMF 0.1 M TBAPF6 at 50 mV/s scan rate; potentials measured vs. Ag/AgCl, 3 M KCl reference electrode.

Table 4

Electrochemical data (V) for 3b, 4b, 5a and 6a recorded in DMF 0.1 M TBAPF6 at 50 mV/s scan rate; potentials measured vs. Ag/AgCl, 3 M KCl reference electrode.

Compound	Redox Couple	E pa	E pc	ΔE	E ½
3b	MnIV/MnIII	+0.68	+0.63	0.05	+0.66
	MnIII/MnII	−0.00	−0.30	0.30	−0.15
		– 1	−0.90	–	–
4b	FeIII/FeII	– 1	−0.77	–	–
5a	MnIV/MnIII	+0.75	+0.60	0.15	+0.68
		+1.11	+0.98	0.13	+1.05
	MnIII/MnII	– 1	−0.41	–	–
		– 1	−0.97	–	–
6a	FeIII/FeII	– 1	−0.70	–	–
		– 1	−0.84	–	–

1 irreversible.

As n class="Chemical">canpan> be observed, the pan> class="Chemical">manganese(III) derivatives were both reduced and oxidized, as reported for [Mn2(μ-salmp)2] in the literature [27]. In 5a, two subsequent oxidation steps could be clearly detected at +0.75 and +1.11 V (Figure 5), which imply the formation of the mixed-state species [MnIIIMnIV(sal(p-tBu)ben)2(OMe)2]+ followed by [MnIV2(sal(p-tBu)ben)2(OMe)2]2+. Both anodic peaks in the forward scan presented relative cathodic signals in the backward scan, with ΔE indicating quasi reversibility of the oxidation processes. In the case of 3b, instead, one oxidation step at +0.68 V was observed, still fully reversible at +0.63 V (Figure S6 in Supplementary Materials), and this, due to the similarity of the potential with 5a, seems to suggest the electrochemical formation of [MnIIIMnIV(salmen)2(OMe)2]+. When moving to the negative region of potentials, 5a showed two peaks at –0.41 and –0.97 V until the final formation of the MnII2, as observed for the iron derivatives, and with no evident backward signals. Interestingly, after exploring the negative potential region, a change of the position of the peaks in the positive potential region was visible shifted to +0.84/+0.56 V (Figure S7 in Supplementary Materials). 3b, instead, showed two subsequent cathodic peaks at negative potentials, while one of them clearly showing a related anodic signal in the backward scan; in this case the oxidation resulted in not being affected by the negative potential scan (Figure S6 in Supplementary Materials).

The n class="Chemical">iron(III) complexes, differently from the manganese(III) ones, were characterized only by the electrochemical reduction to the FeII2 species, either in two close but separated steps (6a) or in one unique step at a mean potential value (4b) (Figure S8 in Supplementary Materials). Compared to [Fe2(μ-salmp)2] [34], instead, the reduction is irreversible, and this might be attributed to the formation of the neutral species [FeII2(μ-salmen)2] and [FeII2(μ-sal(p-tBu)ben)2] due to the loss of the methoxido bridging ligands, with a concomitant rearrangement of the coordination environment of the metal ions, which are more stable than those in the anionic [FeII2(μ-salmp)2]2− derivatives [34], where the iron(II) ions are still trapped by the octahedral embrace of the two bridging pentadentate salmp ligands.

2.6. Magnetic Properties

The magnen class="Chemical">tipan> class="Chemical">c susceptibility of selected polycrystalline samples of 3b, 4b, 5a, 5e, 5f, 6a and 6e was measured in the T = 5−300 K range under an applied magnetic field of 1 kOe. The molar susceptibility, χM, was referred to a dinuclear Mn2 or Fe2 unit, and data are shown in Figure 6 as temperature dependence of the product χMT. The curves of all the analyzed manganese(III) compounds 3b, 5a, 5e and 5f were very similar, regardless of the Schiff base ligand. As for the iron(III) derivatives, the magnetic behavior of 4b, bearing the salmen ligand, was quite different from those of 6a and 6e, which possessed sal(p-X)ben ligands (see Figure S9 in Supplementary Materials for individual plots).

Figure 6

Temperature dependence of the molar susceptibility of (a) manganese(III) (3b, black circles; 5a, red triangles; 5e, blue triangles; 5f, green triangles) and (b) iron(III) (4b, black circles; 6a, red triangles; 6e, blue triangles) dinuclear compounds; the solid lines are the best-fit curves (see text).

For the n class="Chemical">iron(III) complexes, χMT at 300 K was about 8 emu K mol−1 Oe−1, which was slightly lower than the expected value for two uncoupled iron(III) ions (8.77 emu K mol−1 Oe−1, g = 2.00). It then decreased upon cooling, reaching values close to zero at 5 K in all cases. Such behavior suggests that the iron(III) ions are antiferromagnetically (AFM) coupled in the dinuclear species, which have an S = 0 ground state. The χMT decrease of 6a and 6e was already evident at room temperature, while that of 4b occurred at a lower temperature, thus suggesting a weaker exchange coupling in 4b with respect to 6a and 6e. For the manganese(III) derivatives 3b, 5a, 5e and 5f, at 300 K χMT ≈ 5 emu K mol−1 Oe−1, lower than the expected value for two uncoupled manganese(III) ions (6.02 emu K mol−1 Oe−1, g = 2.00). Then the χMT product quickly decreased upon cooling, suggesting that the manganese(III) ions strongly interacted through AFM super-exchange coupling in all compounds.

The fitn class="Chemical">ting of χM of polynpan>upan> class="Chemical">clear magnetic compounds was a nontrivial issue, especially for manganese [39], in view of the overparameterization problem. We then decided to use an in-house software, based on full Hamiltonian diagonalization and Levenberg-Marquardt optimization, by first fitting χMT data to the sum of two terms: (i) a Hamiltonian containing the isotropic exchange and Zeeman terms for the coupled dinuclear species, as reported in Equation (6), and (ii) the Zeeman term for the molar uncoupled fraction f [40], further augmented with a TIP component fixed at 600 × 10−6 emu mol−1, value typical for manganese(III) ions [41]. The best-fit parameters revealed to be relatively insensitive to the TIP value.

Additionpan> of the zero-field splitpan> class="Chemical">ting and mean-field inter-dinuclear interaction to the Hamiltonian did not improve the fit quality nor significantly change the best fit values of the J, g and f parameters. The obtained results were confirmed by independently fitting the χMT data using the PHI 3.1.5 software [42]. The best fit J, g and f parameters are collected in Table 5. The fraction of uncoupled impurity f ranged from 0.8% in 5f to 3.4% in 5e, which can be considered acceptable for these poorly soluble complexes.

Table 5

Best fit values of the magnetic coupling constants J, g factors and uncoupled fractions f for 3b, 4b, 5a, 5e, 5f, 6a and 6e.

Compound	J (cm−1)	g 1	f 2
3b	–13.64(6)	2.05	2.8%
4b	–2.88(2)	2.02	1.0%
5a	–12.95(4)	1.98	1.2%
5e	–12.25(5)	1.97	3.4%
5f	–13.61(8)	2.07	0.8%
6a	–9.517(8)	2.20	1.6%
6e	–10.71(3)	2.21	2.9%

1 The estimated accuracy of g values is ± 0.01; 2 the estimated accuracy of the fractions f is ±0.1%.

All J n class="Chemical">constanpan>ts are negapan> class="Chemical">tive, showing that the metal-metal super-exchange coupling is AFM. Despite the significant variation going from 4b to 6a and 6e, the values fall in the −2.2 to −16.4 cm−1 range expected for bis(μ-alkoxido)diiron(III) complexes [23]. On the other hand, the two 2a·solvent derivatives are reported to possess a weak ferromagnetic (FM) coupling between the two iron(III) ions, in particular 2a·2DMF [34]: J = +1.21 cm− 1, zJ’ = –0.018 cm−1 (g probably assumed equal to 2.00 by the Authors) and Fe–O–Fe = 97.06(9)°; 2a·2CH3CN [23]: J = +0.48(1) cm−1, g = 2.02(1), zJ′ = −0.03(1) cm−1, TIP = 0.0016(2) cm3 mol−1 and Fe–O–Fe = 98.01(6)°. It is immediately clear that salmen2− and sal(p-X)ben2− ligands, even if strictly related to salmp3−, produce a super-exchange Fe–O(Me)–Fe pathway with a wider angle, probably caused by the absence of the bridging phenoxido atom on the central ring. Taking into account the suggested magneto-structural relationship [23], the Fe–O–Fe angle should be close to 101° for 4b and around 103° for 6a and 6e, even if this remains just a speculation in the absence of their crystal structures. Regardless, the small difference between 6a (X = tBu) and 6e (X = Cl) is most probably not related to the substituent X, which is far and in an unfavorable position for inducing any electronic effect on the coupling constant, differently from what we observed in trinuclear copper(II) hydroxido propellers with electronically-modulated tridentate Schiff base ligands [43].

In 4b the AFM n class="Chemical">couplinpan>g betweenpan> the pan> class="Chemical">iron(III) centers is much weaker that in the manganese(III) counterpart 3b, while the difference is less marked when comparing [M2(μ-sal(p-X)ben)2(μ-OMe)2] complexes, where the manganese(III) derivatives are slightly more AFM coupled compared to the iron(III) ones. 3b, 5a, 5e and 5f displayed coupling constants J in the range −12.3 to −13.6 cm−1, which, to the best of our knowledge, are the most negative (AFM) values reported so far.

Most n class="Chemical">manganese(III) dinpan>upan> class="Chemical">clear compounds feature FM coupling, especially those classified as out-of-plane dimers [39]. In these complexes, the plane defined by the N and O donor atoms of the Schiff base ligands is perpendicular to the plane defined by the two Mn–O–Mn bridges, leading to alignment of the individual Jahn–Teller axes. For instance, the out-of-plane [Mn(salmen)(μ-N3)]2 complex (salmen2− ligand is in this case a salen ligand with a methyl group on the ethylene bridge) has J = +0.58 or +0.85 cm−1, when either the ZFS or inter-dimer zJ’ interaction, respectively, is included in the fit [44]. The rare AFM-coupled out-of-plane dimers have J in the range −0.45 to −3.25 cm−1 but the significance of these values has been questioned [39]. On the other hand, 1a·2DMF is reported to have J = −3.3(2) cm−1 and g = 1.96(8) [27], getting closer to the values observed in 3b, 5a, 5e and 5f.

The family of dimerin class="Chemical">c species [Mn2O(R-sao)(tpa)2](ClO4)]2 (R-saoH2 = R-salicylaldoxime, with R = H, Et and Ph, and tpa = tris(2-pyridylmethyl)amine) have been recently reported, where the manganese(III) ions are linked by a Mn–N–O–Mn oxime and an Mn–O–Mn oxido bridge leading to AFM coupling with J = −4.94, −3.87, −5.17 cm−1 for R = H, Et, Ph, respectively [45]. The related complexes (Mn2(R-sao)2(dpa)2)(ClO4)2 (R = H, Me, Et and Ph, and dpa = di(2-picolyl)amine), having two Mn–N–O–Mn oxime bridges, display AFM coupling with J = −5.73, −3.63, −5.63, –2.05 cm−1 for R = H, Me. Et, Ph, respectively [46]. According to DFT calculations, these complexes can be classified as out-of-plane dimers since the manganese(III) Jahn–Teller axes are parallel. However, we note that in these complexes the core is a six-membered ring with chair conformation instead of the Mn2O2 planar core of conventional out-of-plane dimeric species.

The n class="Chemical">coordinpan>apan> class="Chemical">tion pattern in the present manganese(III) dinuclear complexes substantially differ from that of previously reported examples in that each Schiff base coordinates both metal ions instead of a single one, realizing an unusual N2O4 pattern with trans N atoms and two trans Mn–O(Me)–Mn bridges. This pattern does not in principle prevent that our complexes are out-of-plane dimers. However, the short bridge between the imino N atoms (i) causes a distortion of the N–Mn–N axis (N–Mn–N angle < 180°) and (ii) may provide an exchange pathway additional to the methoxido bridges. On the other hand, as outlined in the structural section, the absence of the central phenoxido bridging unit on going from 1a to 3c, but also to 3b, 5a, 5e and 5f, relieves part of the internal strain allowing closer manganese(III) ions, shorter Mn–O distances and smaller Mn–O–Mn angles, which are probably responsible for the stronger AFM coupling. As also discussed in the case of the iron(III) derivatives, especially in these manganese(III) complexes the small differences between 3b, 5a (X = tBu), 5e (Cl) and 5f (CF3) are not related to the substituent X, especially considering that the central aromatic ring is completely absent in 3b.

3. Materials and Methods

3.1. General Procedures

All used n class="Chemical">chemipan> class="Chemical">cals were reagent grade. Solvents were used as received. Elemental analyses were performed at the Microanalytical Laboratory at the Università degli Studi di Milano. ESI-MS spectra were recorded on MeOH or MeCN solutions with an LCQ Advantage Thermofluxional instrument. Infrared spectra were recorded using a JASCO FT-IR 410 spectrophotometer as KBr disks with a 2 cm−1 resolution. H3salmp [2], H2salmen [5] and H2sal(p-X)ben (X = tBu, Me, H, F, Cl, CF3, NO2) [4,11,19,20,31] were synthesised following the synthetic procedure reported in the literature.

3.2. Synthesis of [Mn2(μ-salmp)2] ()

This n class="Chemical">compounpan>d was obtainpan>ed by the modifipan> class="Chemical">cation of a literature procedure [27]. Solid Mn(AcO)3·2H2O (110.2 mg, 0.41 mmol) was added to a yellow solution of H3salmp (142.4 mg, 0.41 mmol) in MeOH (15 mL) and Et3N (1.5 mL) and the mixture was stirred at room temperature for 6 h. The dark brown solid formed was filtered, washed with MeOH, iPr2O and dried under vacuum. Yield: 113.9 mg (65%). Elemental analysis calcd (%) for C42H30Mn2N4O6·2H2O (832.62): C 60.59, H 4.12, N 6.73. Found: C 60.66, H 4.36, N 6.52. MS-ESI+ (MeOH): m/z 797 ([M + H]+, 20%), 819 ([M + Na]+, 100), 1614 ([2M + Na]+, 40). IR (KBr): 1608 (ν C=N) cm−1. The synthesis was also conducted in DMF as solvent under similar conditions, obtaining a very dark solid, washed with DMF and iPr2O and dried under vacuum. Yield: 22%. Elemental analysis calcd (%) for C42H30Mn2N4O6·1.5DMF (927.76): C 60.19, H 4.40, N 8.30. Found: C 60.20, H 4.19, N 8.44. IR (KBr): 1663 (ν C=ODMF), 1608 (ν C=N) cm−1.

3.3. Synthesis of [Fe2(μ-salmp)2] ()

This n class="Chemical">compounpan>d was obtainpan>ed by modifipan> class="Chemical">cation of a literature procedures [3,8,23,28]. Solid FeCl3 (168.8 mg, 1.04 mmol) was added to a solution of H3salmp (358.2 mg, 1.03 mmol) in MeOH (15 mL) and Et3N (1.5 mL) and the mixture was stirred at room temperature for 6 h. The brown-red solid formed was filtered, washed with MeOH, iPr2O and dried under vacuum. Yield: 370.2 mg (86%). Elemental analysis calcd (%) for C42H30Fe2N4O6·2H2O (834.45): C 60.45, H 4.11, N 6.71. Found: C 60.69, H 4.35, N 6.81. MS-ESI+ (MeOH): m/z 821 ([M + Na]+, 100%), 1618 ([2M + Na]+, 50). IR (KBr): 1609 (ν C=N) cm−1. The synthesis was also conducted in CH3CN or DMF as solvent under similar conditions, with final lower yields for co-precipitation of Et3NHCl in the former case, which needed extensive washing with a H2O:MeOH 1:1 solvent mixture (yield: 37%), or high solubility in the latter one (yield: 25%), as also observed in the case of the manganese(III) derivative 1a. Elemental analysis calcd (%) for C42H30Fe2N4O6·1.5DMF·5H2O (998.13): C 54.41, H 5.64, N 8.71. Found: C 54.50, H 5.52, N 8.90. IR (KBr): 1668 (ν C=O DMF), 1610 (ν C=N) cm−1. Single crystals suitable for X-ray diffraction were obtained by slow diffusion either of AcOEt into the DMF reaction mixture (2a·2AcOEt) or iPr2O into the MeCN reaction mixture (2a·2MeCN). Substitution of FeCl3 with Fe(NO3)3·9H2O yielded similar results.

3.4. Synthesis of [Fe2(μ-salmp)(μ-OMe)(salim)2] ()

Solid n class="Chemical">FeCl3 (146.4 mg, 0.90 mmol) was added to a solupan> class="Chemical">tion of H3salmp (314.4 mg, 0.91 mmol) in MeOH (15 mL) and NaOH (4.1 mL of a 0.66 mol L−1 aqueous solution, 2.71 mmol) and the mixture was stirred at room temperature for 6 h. The formed vivid red solid was filtered, washed with MeOH and iPr2O and dried under vacuum. Yield: 185.4 mg (50%). Elemental analysis calcd (%) for C36H30Fe2N4O6·1.5H2O·2MeOH (817.45): C 55.83, H 5.06, N 6.85. Found: C 55.57, H 4.50, N 6.74. MS-ESI+ (MeOH): m/z 606 ([M – salim]+, 80%), 749 ([M + Na]+, 100). IR (KBr): 3302 (ν N–H salim), 1615 (ν C=N) cm−1. Single crystals of 2b·1.5H2O suitable for X-ray diffraction were obtained from slow diffusion of iPr2O into the methanolic reaction mixture.

3.5. Synthesis of [Fe2(μ-salmp)(μ-OH)(salim)2] ()

Solid n class="Chemical">FeCl3 (158.6 mg, 0.98 mmol) was added to a solupan> class="Chemical">tion of H3salmp (313.2 mg, 0.90 mmol) in DMF (20 mL) and NaOH (4.4 mL of a 0.66 mol L−1 aqueous solution, 2.70 mmol) and the mixture was stirred at room temperature for 6 h. The formed dark red solid was filtered, washed with DMF and iPr2O and dried under vacuum. Yield: 285.6 mg (70%). Elemental analysis calcd (%) for C35H28Fe2N4O6·1.5DMF·H2O (839.98): C 57.16, H 5.36, N 9.15. Found: C 56.73, H 5.20, N 9.14. MS-ESI+ (MeOH): m/z 605 ([M – salim – OH + OMe]+, 100%), 749 ([M – OH + OMe + Na]+, 30) (OH/OMe exchange in MeOH solution). IR (KBr): 3302 (ν N–H salim), 1660 (ν C=O DMF), 1615 (ν C=N) cm−1.

3.6. Synthesis of [Mn2(μ-salmen)2(μ-OEt)2] ()

Solid Mn(An class="Chemical">cO)3·2pan> class="Chemical">H2O (54.1 mg, 0.20 mmol) was added to a solution of H2salmen (50.2 mg, 0.20 mmol) in EtOH (15 mL) and Et3N (3 mL) and the mixture was left under stirring at room temperature for 6 h. The obtained dark green solid was filtered, washed with EtOH and iPr2O and dried under vacuum. Yield: 52.3 mg (75%). Elemental analysis calcd (%) for C34H34Mn2N4O6 (704.53): C 57.96, H 4.86, N 7.95. Found: C 58.37, H 4.77, N 8.36. MS-ESI+ (MeOH): m/z 645 ([M – 2OEt + OMe]+, 100%), 727 [M + Na]+, 10) (OEt/OMe exchange in MeOH solution). IR (KBr): 1623 (ν C=N) cm−1. For the synthesis of 3b and 3c see Supplementary Materials.

3.7. Synthesis of [Fe2(μ-salmen)2(μ-OEt)2] ()

Solid n class="Chemical">FeCl3 (32.6 mg, 0.20 mmol) anpan>d pan> class="Chemical">Et3N (3 mL) were added to a solution of H2salmen (50.4 mg, 0.20 mmol) in EtOH (15 mL) and the mixture was left under stirring at room temperature for 6 h. The obtained dark brown solid was filtered, washed with EtOH, iPr2O and dried under vacuum. Yield: 37.1 mg (53%). Elemental analysis calcd (%) for C34H34Fe2N4O6 (706.39): C 57.81, H 4.85, N 7.93. Found: C 57.50, H 4.71, N 8.13. MS-ESI+ (MeOH): m/z 647 ([M – 2OEt + OMe]+, 100%), 701 ([M – 2OEt + 2OMe + Na]+, 75), 729 [M + Na]+, 20) (OEt/OMe exchange in MeOH solution). IR (KBr): 1618 (ν C=N) cm−1. For the synthesis of 4b and 4c see Supplementary Materials.

3.8. Synthesis of [Mn2(μ-sal(p-tBu)ben)2(μ-OMe)2] ()

Solid Mn(An class="Chemical">cO)3·2pan> class="Chemical">H2O (71.9 mg, 0.42 mmol) was added to a yellow suspension of H2sal(p-tBu)ben (155.5 mg, 0.40 mmol) in MeOH (3 mL) with a colour change to brown-green. Et3N (1.5 mL) was added yielding to the precipitation of a dark brown solid. The reaction mixture was left under stirring for 4 h at room temperature, and then the solid was filtered, washed with MeOH and iPr2O and dried under vacuum. Yield: 78.9 mg (41%). Elemental analysis calcd (%) for C52H54Mn2N4O6·1/3H2O (946.91): C 65.95, H 5.86, N 5.92. Found: C 65.95, H 5.85, N 5.77. MS-ESI+ (MeOH): m/z 909 ([M – OMe]+, 100%), 941 ([M + H]+, 70). IR (KBr): 1621 (ν C=N) cm−1. For the synthesis of 5b–g see Supplementary Materials.

3.9. Synthesis of [Fe2(μ-sal(p-tBu)ben)2(μ-OMe)2] ()

Solid n class="Chemical">FeCl3 (88.7 mg, 0.55 mmol) was added to a suspenpan>sionpan> of pan> class="Chemical">H2sal(p-tBu)ben (167.0 mg, 0.43 mmol) in MeOH (3 mL) and then Et3N (1.5 mL) was added, with a concomitant colour change from blue/violet to dark red and the formation of a precipitate. The reaction mixture was then left under stirring at room temperature for 1 h, after that the solid was collected by filtration, washed with MeOH and iPr2O and dried under vacuum. Yield: 145.1 mg (65%). Elemental analysis calcd (%) for C52H54Fe2N4O6·2.5H2O (987.76): C 63.23, H 6.02, N 5.67. Found: C 63.30, H 6.23, N 5.64. IR (KBr): 1614 (ν C=N) cm−1. MS-ESI+ (MeOH) on freshly-prepared solution: m/z 911 ([M – OMe]+, 100%), 965 ([M + Na]+, 40). MS-ESI+ (MeOH) on aged solution for 1 day: m/z 678 ([Fe2(sal(p-tBu)ben)(salim)(OMe)2]+, 20%), 767 ([Fe2(sal(p-tBu)ben)(salim)2(OMe)]+, 15), 821 ([Fe2(sal(p-tBu)ben)(salim)2(OMe)2 + Na]+, 100), 911 ([M – OMe]+, 5). Substitution of FeCl3 with Fe(NO3)3·9H2O yielded similar results. For the synthesis of 6b–g see Supplementary Materials.

3.10. X-ray Data Collection and Structure Determination

n class="Chemical">Crystals of pan> class="Chemical">H2sal(p-tBu)ben and H2sal(p-CF3)ben suitable for X-ray diffraction studies were obtained from slow evaporation of chloroform solutions, crystals of 2a·2AcOEt were obtained from slow diffusion of AcOEt into DMF, crystals of 2a·2CH3CN were obtained from slow diffusion of iPr2O into CH3CN, crystals of 2b·1.5H2O were obtained from slow diffusion of iPr2O into MeOH, while crystals of 3c·2DMF were obtained by slow diffusion of iPr2O into a DMF solution of 3b. Intensity data were collected at room temperature on a Bruker Apex II CCD diffractometer, using graphite-monochromatized Mo-Kα radiation (λ = 0.71073 Å). Intensity data were corrected for Lorentz-polarization effects and for absorption (SADABS [47]). The structures were solved by direct methods (SIR-97 [48]) and completed by iterative cycles of full-matrix least squares refinement on Fo2 and ΔF synthesis using SHELXL program [49] (WinGX suite [50]). Hydrogen atoms, located on the ∆F maps, were allowed to ride on their carbon atoms. A summary of the crystal data and refinement details for all compounds is given in Table S1 in Supplementary Materials.

n class="Chemical">Cpan> class="Chemical">CDC 2030845–2030850 contains the supplementary crystallographic data for 2a·2CH3CN, H2sal(p-CF3)ben, 3c·2DMF, H2sal(p-tBu)ben, 2b·1.5H2O and 2a·2AcOEt, respectively. These data can be obtained free of charge via http://www.ccdc.cam.ac.uk/conts/retrieving.html, or from the Cambridge Crystallographic Data Centre, 12 Union Road, Cambridge CB2 1EZ, UK; fax: (+44) 1223-336-033, or e-mail: deposit@ccdc.cam.ac.uk.

3.11. Cyclic Voltammetry

Elen class="Chemical">ctropan> class="Chemical">chemical tests were carried out with an Autolab PGSTAT 12 electrochemical instrument (Ecochemie). The experiments were performed in a single-compartment three-electrode cell at room temperature under Ar atmosphere. Pt was used as working electrode, a glassy carbon rod served as auxiliary electrode and an aqueous Ag/AgCl, KCl 3 M electrode (Metrohm) was the reference electrode; all the potential values given are referred to such an electrode. The solutions were prepared dissolving a small amount of 3b, 4b, 5a and 6a in a solution of DMF containing 0.1 M TBAPF6 as supporting electrolyte.

3.12. Magnetic Measurements

The magnen class="Chemical">tipan> class="Chemical">c moment μ of powder samples of 3b, 4b, 5a, 5e, 5f, 6a, and 6e was measured between 5 and 300 K using a Quantum Design MPMS XL-5 SQUID magnetometer. Weighed amounts (about 15 mg) of the compounds were sealed in polycarbonate capsules and μ was measured under an applied magnetic field of 1 kOe from 300 K down to 5 K. The molar susceptibility was obtained as χM = (μ/H) × (MW/m), where MW is the molecular weight of the complex, m is the sample mass, and H is the applied magnetic field. Diamagnetic contributions were subtracted from μ before calculating χM. The ligand diamagnetism was estimated using Pascal’s constants [51].

4. Conclusions

The present paper aimed to show a new pien class="Chemical">ce of pan> class="Chemical">chemistry, i.e. the reactivity of the shortened salen-type analogues H3salmp, H2salmen and H2sal(p-X)ben (X = tBu, Me, H, F, Cl, CF3, NO2) with manganese(III) and iron(III), which invariably formed dinuclear complexes with bridging Schiff base ligands and alkoxido ions of general formula [M2(μ-salmp)2], [M2(μ-salmen)2(μ-OR)2] and [M2(μ-sal(p-X)ben)2(μ-OMe)2] (M = Mn, Fe; R = H, Me, Et). Complexes of iron(III) with sal(p-X)ben2− showed the tendency to hydrolyse to salim− in solution and in some cases rearrange to salmp3−, while complexes of manganese(III) are more stable with no hints of C–N bond breakage. A similar ligand rupture was evidenced by reaction of H3salmp with iron(III) salts in the presence of NaOH as a stronger base than NEt3, leading to the dinuclear compound [Fe2(μ-salmp)2(μ-OMe)(salim)2], where part of the tension created by two salmp3− bridging ligands in [Fe2(μ-salmp)2] is relieved by one methoxido bridging ion. Infrared spectroscopy, mass spectrometry and structural characterization by single-crystal X-ray diffraction were used in combination to follow the reactivity.

n class="Chemical">CV measuremenpan>ts highlight the possibility to modulate the oxidapan> class="Chemical">tion state of the complexes analysed with the formation of mixed-state MnIIIMnIV and MnIIMnIII species. The electrochemical behaviour of the iron(III) derivatives, which reveal to be irreversibly reduced and suggest the formation of stable [FeII2(μ-L)2] complexes, is peculiar and certainly aim of our future efforts. Magnetic studies showed the presence of AFM super-exchange among the two metal ions within selected dinuclear complexes, with negligible effect of the substituent X, too far and in an unfavorable position for inducing any electronic effect on the coupling constants, which are then dominated by the structural distortion caused by the shortened salen-type ligands. In particular, the manganese(III) complexes show, to the best of our knowledge, the strongest AFM coupling reported so far, and this consolidates the usefulness of these ligands in different fields and the profit doing research with them.

Very little is known but so much needs to be discovered on these shortened Schiff bases, their behavior as ligands and the properties of the related metal complexes, and as the Italian poet Giacomo Leopardi wrote at the end of his famous poem ‘L’infinito’ [52] (The infinity), ‘e il naufragar m’è dolce in questo mar’ (and foundering in this sea is sweet to me), a sea of exciting chemistry.