# Synthesis, Characterization, and Catalytic Studies of Mn(III)-Schiff Base-Dicyanamide Complexes: Checking the Rhombicity Effect in Peroxidase Studies

Authors: Manuel R. Bermejo; Rocío Carballido; M. Isabel Fernández-García; Ana M. González-Noya; Gustavo González-Riopedre; Marcelino Maneiro; Laura Rodríguez-Silva
Journal: Journal of Chemistry
 (2017)

---

## Abstract

The condensation of 3-methoxy-2-hydroxybenzaldehyde and the diamines 1,2-diphenylendiamine, 1,2-diamine-2-methylpropane and 1,3-propanediamine yielded the dianionic tetradentate Schiff base ligands N,N′-bis(2-hydroxy-4-methoxybenzylidene)-1,2-diphenylendiimine (H2L1), N,N′-bis(2-hydroxy-4-methoxybenzylidene)-1,2-diamino-2-methylpropane (H2L2) and N,N′-bis(2-hydroxy-4-methoxybenzylidene)-1,3-diaminopropane (H2L3) respectively. The organic compounds H2L1 and H2L2 have been characterized by elemental analysis, IR, 1H and 13C NMR spectroscopies and mass spectrometry electrospray (ES). The crystal structure of H2L2 in solid state, solved by X-ray crystallography, is highly conditioned in the solid state by two N-H•••N intramolecular interactions. The synthesis of three new manganese(III) complexes1–3, incorporating these ligands, H2L1–H2L3, and dicyanamide (DCA), is reported. The complexes1–3 have been physicochemically characterized by elemental analysis, IR and paramagnetic 1H NMR spectroscopy, ESI mass spectrometry, magnetic moment at room temperature and conductivity measurements. Complex1 has been crystallographically characterized. The X-ray structure shows the self-assembly of the Mn(III)-Schiff base-DCA complex through µ-aquo bridges between neighbouring axial water molecules and also by π-π stacking interactions, establishing a dimeric structure. The manganese complexes were also tested as peroxidase mimics for the H2O2-mediated reaction with the water-soluble trap ABTS, showing complexes1-2 relevant peroxidase activity in contrast with3. The rhombicity around the metal ion can explain this catalytic behaviour.


---

## Body

## 1. Introduction

Schiff base ligands stabilize different metal ions in solution to yield metal complexes with a variety of properties and applications. For instance, one of these ligands, the chelatingsalen, is known by the ability to significantly decrease the Mn(III)/Mn(II) redox potentials, and the resulting complexes constitute suitable systems to catalyse multiple redox reactions such as asymmetric epoxidation of unfunctionalized olefins, catalase reaction, water photolysis, Diels-Alder cycloaddition, enantioselective cyclopropanation of styrenes and ring opening of epoxides [1–8]. Over the past years, a variety of applications of this type of complexes has also been reported, including a broad range of biological activities (antibacterial, antifungal, anticancer, antioxidant, anti-inflammatory, etc.) [9–13].During our search for new metal catalysts containing salen-type ligands, we have observed a better catalytic behaviour when the substrate molecule can be easily coordinated by the complex and this is favoured when the catalyst has either a vacancy in the coordination sphere or a labile ligand [14–17]. To achieve this, a careful design of the environment around the metal ion is necessary.In this article, we report the synthesis and characterization of three new complexes containing both salen-type ligands and ancillary dicyanamide ligands (see Figure1). The two imine nitrogen and two phenol oxygen atoms of the tetradentate Schiff bases H2L1–H2L3 constitute an inner ONNO site. The presence of the outer methoxy groups facilitates the extension of the supramolecular network through hydrogen-bond interactions [18, 19]. Our scheme consists of inducing tetragonal elongation around the manganese ion with the combination of the H2Ln and dicyanamide ligands.Figure 1
Structures of the Schiff base ligands H2L1–H2L3.These complexes may behave like enzyme mimics, and their peroxidase activity is reported in this work. Peroxidases catalyse oxidation of a broad range of substrates by hydrogen hydroxide, so they may be successfully used for different industrial processes since peroxidases are capable of degrading aromatic rings in lignin, dyes, and polycyclic aromatic hydrocarbons [15, 16, 20, 21]. In this sense, dyes are regarded as one of the most important contaminants to be removed from the industrial effluents, and peroxidases arise as a way to treat these pollutants. Here we check the peroxidase activity of Mn(III)-Schiff base complexes in function of the rhombicity (or tetragonal elongation) around the manganese ion.


## 2. Materials and Methods

### 2.1. Materials

All solvents, 3-methoxy-2-hydroxybenzaldehyde, 1,2-diphenylendiamine, 1,2-diamine-2-methylpropane, 1,3-propanediamine, manganese(II) acetate, sodium dicyanamide, hydrogen peroxide, and 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid, are commercially available and were used without further purification.


### 2.2. Physical Measurements

Elemental analyses of C, H, and N were performed on a Carlo Erba EA-1108. IR spectra were recorded as KBr discs on a Bio-Rad FTS135 spectrophotometer in the range 4000–400 cm−1. 1H NMR and 13C NMR spectra were recorded on a Bruker AC-300 spectrometer at 296 K using DMSO-d6 as deuterated solvent and tetramethylsilane as an internal reference. Positive electrospray-ionization (ESI) mass spectra of the ligands and complexes were recorded on a LC-MSD 1100 Hewlett-Packard instrument (positive-ion mode, 98 : 2 CH3OH/HCOOH as the mobile phase, 30–100 V). Magnetic susceptibilities were measured at room temperature using a Sherwood-Scientific MK1 balance, calibrated using mercury tetrakis(isothiocyanato)cobaltate(II), Hg[Co(NCS)4]. Measurements of conductivity were made with 10−3 M solutions of complexes in dimethylformamide using a Crison microCM 2200 conductivimeter.


### 2.3. Synthesis of H2L1

Schiff base ligand H2L1 was prepared according to the literature by condensation of 3-methoxy-2-hydroxybenzaldehyde (1.12 g, 10.35 mmol) with 1,2-phenylenediamine (0.54 mL, 5.18 mmol) in methanol [28]. The mixture of diamine and salicylaldehyde was refluxed in a round bottom flask fitted with a Dean-Stark apparatus. After heating for 3 h, the solution was concentrated to yield an orange solid. The product was collected by filtration, washed with diethyl ether, and dried in air. Yield was almost quantitative. M.p. 172.5°C. Anal. Calc. for C22H20N2O4: C, 70.2; H, 5.3; N, 7.4. Found: C, 70.1; H, 5.3, N, 7.5%. MS ES (m/z): 377 (L + H+)+; IR (KBr, cm−1): ν(O-H) 3461, ν(C=N) 1611, ν(C-O) 1253. 1H NMR (DMSO-d6, ppm): δ 12.95 (s, 2H), 8.88 (s, 2H), 7.42 (m, 4H), 7.36 (d, 2H), 7.13 (d, 2H), 6.88 (t, 2H), 3.79 (s, 6H). 13C NMR (DMSO-d6, ppm): δ 164.8 (C=N), 151.4 (C-OCH3), 142.8 (C-OH), 116-128.5 (Car), 40.2 (CH3).


### 2.4. Synthesis and Crystallization of H2L2

The tetradentate Schiff base H2L2 was prepared following the procedure already described for H2L1, using 3-methoxy-2-hydroxybenzaldehyde (2.00 g, 13.14 mmol) and 1,2-diamine-2-methylpropane (0.68 mL, 6.57 mmol) in methanol. The yellow product was collected by filtration, washed with diethyl ether, and dried in air. Yellow crystals of H2L2, suitable for single crystal X-ray diffraction studies, were obtained by slow evaporation of the methanol solution of the ligands. Yield was almost quantitative, 94%. M.p. 122.9°C. Anal. Calc. for C20H24N2O4: C, 67.4; H, 6.8; N, 7.9. Found: C, 67.3; H, 6.7, N, 7.8%. MS ES (m/z): 357 (L + H+)+, 379 (L + Na+)+; IR (KBr, cm−1): ν(O-H) 3441, ν(C=N) 1630, ν(C-O) 1256. 1H NMR (DMSO-d6, ppm): δ 8.53, 8.50 (s, 2H), 6.77–7.01 (m, 6H), 3.83 (m, 6H), 3.76 (t, 4H), 1.37 (t, 6H), 13C NMR (DMSO-d6, ppm): δ 163.3 (C=N), 148.9 (C-OCH3), 152.9 (C-OH), 25.7 (CH3).


### 2.5. Synthesis of H2L3

The synthesis and characterization of H2L3 have been already previously reported and they will not be discussed in this paper [22].


### 2.6. Complex Preparation

M
n
2
L
1
2
H
2
O
2
DCA
2
(
1
): to a methanolic solution of H2L1 (0.53 mmol, 0.20 g), 0.53 mmol (0.13 g) of Mn(CH3COO)2 was added and the stirred solution changed its initial yellow colour to brown. After 30 minutes of stirring with gentle heating, 0.53 mmol (0.05 g) of NaN(CN)2 in 10 mL of methanol was added. The solution was then concentrated by slow evaporation. The complex was obtained as brown crystals, which were isolated by filtration, washed with diethyl ether, and dried in air. Yield 60%. Anal. Calcd. for C48H40Mn2N10O10 (1026.8): C, 56.1; H, 3,9; N, 13.6. Found: C, 55.5; H, 3.9; N, 13.4%. MS ES (m/z): 429 [MnL]+; 496 [MnL(DCA)]+. IR (KBr, cm−1): ν(O-H) 3433 (m), ν(C=N) 1600 (vs), ν(C-O) 1258 (s), νsym(C≡N) 2151 (vs), νasym(C≡N) 2254 (m). 1H NMR (DMSO-d6, ppm): δ  −14.9 (H4), −20.0 (H5). μ = 4.8 BM. Conductivity (in DMF) ΛM = 45 μS.[
MnL
2
(
H
2
O)(DCA)](
H
2
O) (2) was obtained by the same procedure as1, using 0.46 mmol (0.16 g) of H2L2, 0.46 mmol (0.11 g) of Mn(CH3COO)2, and 0.46 mmol (0.04 g) of NaN(CN)2 in 10 mL of methanol which were added. Yield 58%. Anal. Calcd. for C22H26MnN5O6 (511.41): C, 51.6; H, 5.1; N, 13.7. Found: C, 52.1; H, 5.2; N, 13.5%. MS ES (m/z) 408.5 [MnL]+, 884.0 [Mn2L2(DCA)2]+; IR (KBr, cm−1): ν(O-H) 3425, ν(C=N) 1610, ν(C-O) 1260, νsym(C≡N) 2148, νasym(C≡N) 2266; 1H NMR (DMSO-d6, ppm): δ  −15.2 (H4), −16.8/−25.0 (H5). μ = 5.0 BM. Conductivity (in MeOH) ΛM = 46 μS.[
MnL
3
(
H
2
O)(DCA)](
H
2
O) (3) was obtained by the same procedure as1, using 0.58 mmol (0.20 g) of H2L3, 0.58 mmol (0.14 g) of Mn(CH3COO)2, and 0.58 mmol (0.05 g) of NaN(CN)2 in 10 mL of methanol which were added. Yield 65%. Anal. Calcd. for C21H24MnN5O6 (497.37): C, 50.7; H, 4.8; N, 14.1. Found: C, 49.8; H, 4.6; N, 13.8%. MS ES (m/z) 395.3 [MnL]+; IR (KBr, cm−1): ν(O-H) 3412, ν(C=N) 1612, ν(C-O) 1256, νsym(C≡N) 2144, νasym(C≡N) 2252; 1H NMR (DMSO-d6, ppm): δ  −16.4 (H4), −18.6 (H5). μ = 4.7 BM. Conductivity (in DMF) ΛM = 42 μS.


### 2.7. Peroxidase Probes

Peroxidase activity for complexes1–3 was tested according to the literature procedure [15, 16] by study of the oxidation of 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid (ABTS) with H2O2 atca. pH 6.8 in the presence of the complexes.


### 2.8. Crystallographic Studies

Single crystals of H2L2 and complex1, suitable for X-ray diffraction studies, were obtained by slow evaporation of the methanolic solution at room temperature.Table1 collects detailed crystal data collection and refinement for H2L2 and complex1. Measurements were made on a Bruker-Smart CCD-1000 diffractometer employing graphite-monochromatedMo-Kα radiation (λ = 0.71073 Å) at 100 K. The structures were solved by direct methods [29] and finally refined by full-matrix least-squares base on F2. An empirical absorption correction was applied using SADABS [30]. All nonhydrogen atoms were included in the model at geometrically calculated positions.Table 1
Crystal data and structure refinement for H2L2 and complex 1.
H2L2
Complex1
Chemical formula
C20H24N2O4
C24H20MnN5O5
Formula weight
356.41
513.39
Crystal system
Triclinic
Triclinic
Space group
P
1
-
P
1
-
Temperature (K)
100
100(2)
a (Å)
8.3632(6)
8.3157(4)
b (Å)
10.5626(7)
11.9711(6)
c (Å)
11.4846(7)
12.7633(10)
α (°)
108.689(2)
114.321(3)
β (°)
95.176(2)
102.633(3)
γ (°)
103.965(2)
97.626(2)
Volume (Å3)
917.00(11)
1093.74(11)
Z
2
2
Radiation type
MoKα
MoKα
μ (mm−1)
0.09
0.653
Crystal size (mm)
0.2 × 0.11 × 0.03
0.12 × 0.11 × 0.06
T
m
i
n, Tmax
0.942, 0.997
0.9619, 0.9858
F
(
000
)
380
528
Number of measured reflections
11933
20087
Number independent reflections
3607
4293
Reflections observed[I>2σ(I)]
2055
3209
R
i
n
t
0.054
0.0374
sin
⁡
θ
/
λ
m
a
x (Å−1)
0.617
0.0752
R
[
F
2
>
2
σ
(
F
2
)
]
0.049
0.0630
w
R
(
F
2
)
0.128
0.0816
Number of parameters
247
332
Δ
m
a
x, Δmin (e Å−3)
0.31, −0.28
0.338, −0.423Refinement ofF2 againstall reflections: the weighted R-factor wR is based on F2, and conventional R-factors R are based on F, with F set to zero for negative F2. The threshold expression of F2 > 2σ(F2) is used only for calculating R-factors(gt) and so forth and is not relevant to the choice of reflections for refinement. R-factors based on F2 are statistically about twice as large as those based on F, and R-factors based onall data will be even larger.


## 2.1. Materials

All solvents, 3-methoxy-2-hydroxybenzaldehyde, 1,2-diphenylendiamine, 1,2-diamine-2-methylpropane, 1,3-propanediamine, manganese(II) acetate, sodium dicyanamide, hydrogen peroxide, and 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid, are commercially available and were used without further purification.


## 2.2. Physical Measurements

Elemental analyses of C, H, and N were performed on a Carlo Erba EA-1108. IR spectra were recorded as KBr discs on a Bio-Rad FTS135 spectrophotometer in the range 4000–400 cm−1. 1H NMR and 13C NMR spectra were recorded on a Bruker AC-300 spectrometer at 296 K using DMSO-d6 as deuterated solvent and tetramethylsilane as an internal reference. Positive electrospray-ionization (ESI) mass spectra of the ligands and complexes were recorded on a LC-MSD 1100 Hewlett-Packard instrument (positive-ion mode, 98 : 2 CH3OH/HCOOH as the mobile phase, 30–100 V). Magnetic susceptibilities were measured at room temperature using a Sherwood-Scientific MK1 balance, calibrated using mercury tetrakis(isothiocyanato)cobaltate(II), Hg[Co(NCS)4]. Measurements of conductivity were made with 10−3 M solutions of complexes in dimethylformamide using a Crison microCM 2200 conductivimeter.


## 2.3. Synthesis of H2L1

Schiff base ligand H2L1 was prepared according to the literature by condensation of 3-methoxy-2-hydroxybenzaldehyde (1.12 g, 10.35 mmol) with 1,2-phenylenediamine (0.54 mL, 5.18 mmol) in methanol [28]. The mixture of diamine and salicylaldehyde was refluxed in a round bottom flask fitted with a Dean-Stark apparatus. After heating for 3 h, the solution was concentrated to yield an orange solid. The product was collected by filtration, washed with diethyl ether, and dried in air. Yield was almost quantitative. M.p. 172.5°C. Anal. Calc. for C22H20N2O4: C, 70.2; H, 5.3; N, 7.4. Found: C, 70.1; H, 5.3, N, 7.5%. MS ES (m/z): 377 (L + H+)+; IR (KBr, cm−1): ν(O-H) 3461, ν(C=N) 1611, ν(C-O) 1253. 1H NMR (DMSO-d6, ppm): δ 12.95 (s, 2H), 8.88 (s, 2H), 7.42 (m, 4H), 7.36 (d, 2H), 7.13 (d, 2H), 6.88 (t, 2H), 3.79 (s, 6H). 13C NMR (DMSO-d6, ppm): δ 164.8 (C=N), 151.4 (C-OCH3), 142.8 (C-OH), 116-128.5 (Car), 40.2 (CH3).


## 2.4. Synthesis and Crystallization of H2L2

The tetradentate Schiff base H2L2 was prepared following the procedure already described for H2L1, using 3-methoxy-2-hydroxybenzaldehyde (2.00 g, 13.14 mmol) and 1,2-diamine-2-methylpropane (0.68 mL, 6.57 mmol) in methanol. The yellow product was collected by filtration, washed with diethyl ether, and dried in air. Yellow crystals of H2L2, suitable for single crystal X-ray diffraction studies, were obtained by slow evaporation of the methanol solution of the ligands. Yield was almost quantitative, 94%. M.p. 122.9°C. Anal. Calc. for C20H24N2O4: C, 67.4; H, 6.8; N, 7.9. Found: C, 67.3; H, 6.7, N, 7.8%. MS ES (m/z): 357 (L + H+)+, 379 (L + Na+)+; IR (KBr, cm−1): ν(O-H) 3441, ν(C=N) 1630, ν(C-O) 1256. 1H NMR (DMSO-d6, ppm): δ 8.53, 8.50 (s, 2H), 6.77–7.01 (m, 6H), 3.83 (m, 6H), 3.76 (t, 4H), 1.37 (t, 6H), 13C NMR (DMSO-d6, ppm): δ 163.3 (C=N), 148.9 (C-OCH3), 152.9 (C-OH), 25.7 (CH3).


## 2.5. Synthesis of H2L3

The synthesis and characterization of H2L3 have been already previously reported and they will not be discussed in this paper [22].


## 2.6. Complex Preparation

M
n
2
L
1
2
H
2
O
2
DCA
2
(
1
): to a methanolic solution of H2L1 (0.53 mmol, 0.20 g), 0.53 mmol (0.13 g) of Mn(CH3COO)2 was added and the stirred solution changed its initial yellow colour to brown. After 30 minutes of stirring with gentle heating, 0.53 mmol (0.05 g) of NaN(CN)2 in 10 mL of methanol was added. The solution was then concentrated by slow evaporation. The complex was obtained as brown crystals, which were isolated by filtration, washed with diethyl ether, and dried in air. Yield 60%. Anal. Calcd. for C48H40Mn2N10O10 (1026.8): C, 56.1; H, 3,9; N, 13.6. Found: C, 55.5; H, 3.9; N, 13.4%. MS ES (m/z): 429 [MnL]+; 496 [MnL(DCA)]+. IR (KBr, cm−1): ν(O-H) 3433 (m), ν(C=N) 1600 (vs), ν(C-O) 1258 (s), νsym(C≡N) 2151 (vs), νasym(C≡N) 2254 (m). 1H NMR (DMSO-d6, ppm): δ  −14.9 (H4), −20.0 (H5). μ = 4.8 BM. Conductivity (in DMF) ΛM = 45 μS.[
MnL
2
(
H
2
O)(DCA)](
H
2
O) (2) was obtained by the same procedure as1, using 0.46 mmol (0.16 g) of H2L2, 0.46 mmol (0.11 g) of Mn(CH3COO)2, and 0.46 mmol (0.04 g) of NaN(CN)2 in 10 mL of methanol which were added. Yield 58%. Anal. Calcd. for C22H26MnN5O6 (511.41): C, 51.6; H, 5.1; N, 13.7. Found: C, 52.1; H, 5.2; N, 13.5%. MS ES (m/z) 408.5 [MnL]+, 884.0 [Mn2L2(DCA)2]+; IR (KBr, cm−1): ν(O-H) 3425, ν(C=N) 1610, ν(C-O) 1260, νsym(C≡N) 2148, νasym(C≡N) 2266; 1H NMR (DMSO-d6, ppm): δ  −15.2 (H4), −16.8/−25.0 (H5). μ = 5.0 BM. Conductivity (in MeOH) ΛM = 46 μS.[
MnL
3
(
H
2
O)(DCA)](
H
2
O) (3) was obtained by the same procedure as1, using 0.58 mmol (0.20 g) of H2L3, 0.58 mmol (0.14 g) of Mn(CH3COO)2, and 0.58 mmol (0.05 g) of NaN(CN)2 in 10 mL of methanol which were added. Yield 65%. Anal. Calcd. for C21H24MnN5O6 (497.37): C, 50.7; H, 4.8; N, 14.1. Found: C, 49.8; H, 4.6; N, 13.8%. MS ES (m/z) 395.3 [MnL]+; IR (KBr, cm−1): ν(O-H) 3412, ν(C=N) 1612, ν(C-O) 1256, νsym(C≡N) 2144, νasym(C≡N) 2252; 1H NMR (DMSO-d6, ppm): δ  −16.4 (H4), −18.6 (H5). μ = 4.7 BM. Conductivity (in DMF) ΛM = 42 μS.


## 2.7. Peroxidase Probes

Peroxidase activity for complexes1–3 was tested according to the literature procedure [15, 16] by study of the oxidation of 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid (ABTS) with H2O2 atca. pH 6.8 in the presence of the complexes.


## 2.8. Crystallographic Studies

Single crystals of H2L2 and complex1, suitable for X-ray diffraction studies, were obtained by slow evaporation of the methanolic solution at room temperature.Table1 collects detailed crystal data collection and refinement for H2L2 and complex1. Measurements were made on a Bruker-Smart CCD-1000 diffractometer employing graphite-monochromatedMo-Kα radiation (λ = 0.71073 Å) at 100 K. The structures were solved by direct methods [29] and finally refined by full-matrix least-squares base on F2. An empirical absorption correction was applied using SADABS [30]. All nonhydrogen atoms were included in the model at geometrically calculated positions.Table 1
Crystal data and structure refinement for H2L2 and complex 1.
H2L2
Complex1
Chemical formula
C20H24N2O4
C24H20MnN5O5
Formula weight
356.41
513.39
Crystal system
Triclinic
Triclinic
Space group
P
1
-
P
1
-
Temperature (K)
100
100(2)
a (Å)
8.3632(6)
8.3157(4)
b (Å)
10.5626(7)
11.9711(6)
c (Å)
11.4846(7)
12.7633(10)
α (°)
108.689(2)
114.321(3)
β (°)
95.176(2)
102.633(3)
γ (°)
103.965(2)
97.626(2)
Volume (Å3)
917.00(11)
1093.74(11)
Z
2
2
Radiation type
MoKα
MoKα
μ (mm−1)
0.09
0.653
Crystal size (mm)
0.2 × 0.11 × 0.03
0.12 × 0.11 × 0.06
T
m
i
n, Tmax
0.942, 0.997
0.9619, 0.9858
F
(
000
)
380
528
Number of measured reflections
11933
20087
Number independent reflections
3607
4293
Reflections observed[I>2σ(I)]
2055
3209
R
i
n
t
0.054
0.0374
sin
⁡
θ
/
λ
m
a
x (Å−1)
0.617
0.0752
R
[
F
2
>
2
σ
(
F
2
)
]
0.049
0.0630
w
R
(
F
2
)
0.128
0.0816
Number of parameters
247
332
Δ
m
a
x, Δmin (e Å−3)
0.31, −0.28
0.338, −0.423Refinement ofF2 againstall reflections: the weighted R-factor wR is based on F2, and conventional R-factors R are based on F, with F set to zero for negative F2. The threshold expression of F2 > 2σ(F2) is used only for calculating R-factors(gt) and so forth and is not relevant to the choice of reflections for refinement. R-factors based on F2 are statistically about twice as large as those based on F, and R-factors based onall data will be even larger.


## 3. Results and Discussion

Schiff bases H2L1-H2L2 have been obtained in almost quantitative yield and characterized by elemental analysis, IR, 1H, and 13C NMR spectroscopies, and mass spectrometry electrospray (ES). The synthesis and characterization of H2L3 have been already reported [22].Complexes1–3 were prepared in high yield as detailed in the Materials and Methods. Elemental analysis establishes the general formula [MnLn(H2O)(DCA)](H2O)x, with n = 1–3 and x = 0-1. Analytical and spectroscopic data are in accordance with this empirical formula. All the complexes seem to be stable in air and thermally stable, melting above 300°C without decomposition. They are insoluble or sparingly soluble in water but partially soluble in common organic solvents such as methanol and totally soluble in polar coordinating solvents such as pyridine, DMF, and DMSO.ESI (electrospray-ionization) mass spectra registered in methanol show, for complexes1–3, a peak corresponding to the fragment [MnL]+, indicating the coordination of the Schiff base ligand to the metal centre. Other minor signals, assigned to [MnL1(DCA)]+ and [Mn2L22DCA2]+ units, also confirm the coordination of the dicyanamide ion to the manganese ion and point to the formation of dimeric species (Figure 2).Figure 2
ESI mass spectrum for complex2.The values for the magnetic moment at room temperature are very close to the spin-only value of 4.89 BM, as expected for a high-spin magnetically diluted d4 manganese(III) ion.All the complexes show similar IR spectral features, exhibiting a strong band between 1600 and 1612 cm−1 attributable to ν(CNimine) band, which is shifted 3–7 cm−1 lower than in the free Schiff base ligand. There is also a positive shift (3–7 cm−1) of the ν(COphenol) mode with respect to the free ligand (Figure 3). These data suggest the coordination of the Schiff base in its dianionic form through the inner phenol oxygen and the imine nitrogen atoms [14, 15, 22]. Moreover, two new bands at about 2150 and 2260 cm−1 are assigned, respectively, to the symmetric and asymmetric dicyanamide modes [16, 31].Figure 3
Comparison between the spectra for the free ligand H2L2 (a) and complex2 (b).
(a)
(b)Paramagnetic1H NMR spectra of1–3 were registered using DMSO-d6 as solvent. The data interpretation, based on previous findings for manganese(III) complexes with related Schiff base ligands [24], indicates [32, 33] the formation of the manganese(III) complexes. The paramagnetic 1H NMR spectra of the complexes contain, for all cases, two upfield proton resonances, outside the diamagnetic region (δ = 0–14 ppm), due to the isotropic shifting of the ligand protons for high-spin manganese(III) complexes in an octahedral field. The signals must arise from the protons of the aromatic phenoxy rings. In the case of the symmetric complexes1 and3, the −20.0 (for1)/−18.6 (for3) signals arise from the protons in the orthopositions to the methoxy substituent, while the resonances from −14.9 (for1)/−16.4 (for3) ppm arise from protons in the metapositions to the methoxy substituent. For complex2 the signal from the protons in the orthopositions to the methoxy substituent appears split in two resonances at −16.8 and −25.0 ppm (Figure 4).Figure 4
Paramagnetic1H NMR spectrum for complex2.


### 3.1. Crystallographic Characterization of H2L2 and Complex1

#### 3.1.1. Crystal Structure of H2L2

The crystal structure reveals that H2L2 exists as discrete molecules, and it is composed of two identical 3-methoxy-2-hydrobenzylimine moieties twisted about the central aliphatic chain which acts as a spacer (Figure 5). The C12-N2 and C7-N1 distances of 1.272(3) and 1.279(3) Å, respectively, are practically identical and consistent with a C=N double bonding (Table 2), indicating both imine groups fully localized in the molecule [34]. The two oxygen O1 and O3 atoms are forming phenolic groups, and they present C-O distances of 1.354(3) Å and 1.351(3), respectively, corresponding to the expected single bonds. The C12-N2-C9 angle of 122.9(2)° confirms the sp2 character for N2 atom [32].Table 2
Selected geometric parameters (Å, °) for H2L2.
C12-N2
1.272(3)
C14-O3
1.351(3)
C12-N2-C9
122.9(2)
C7-N1
1.279(3)
C1-O1
1.354(3)
N2-C9-C8
106.65(19)Figure 5
ORTEP representation (50% probability) of H2L2.The disposition adopted by the free ligand in the solid state is conditioned by two strong intramolecular hydrogen-bond interactions which form two six-membered rings. These interactions arise from the contact between the hydroxy and the imine groups (see Table3). As expected, the O1-H1O•••N1 hydrogen bonding establishes an almost planar N1-C7-C6-C1-O1-H1 ring, the same for the O3-H3O•••N2 hydrogen bonding which establishes other almost planar N2-C12-C13-C14-O3-H3 rings.Table 3
Hydrogen bonds for H2L2.
D-H⋯A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O1-H1⋯N1
0.96
1.73
2.5839
146
O3-H3 ⋯N2
0.93
1.72
2.5891
154
C8-H8B⋯O1
0.99
2.55
3.4451
151Despite the mentioned intramolecular hydrogen interactions and a partial conjugation of the molecule, this one is not planar, probably due to the packing based on the intermolecular hydrogen bonds and theπ-stacking interactions between the salicyl residues of the neighbouring molecules (see Figure 6). The aromatic rings are arranged almost perpendicular to each other. Clearly, rotation about the C8-C9 bond to give a near-eclipsed or gauche conformation would achieve quasi-square-planar coordination environments using the inner ONNO site. According to this crystal structure study, this ligand should act as tetradentate donor in the equatorial plane about an octahedral metal centre. However, we cannot predict the role of the outer phenoxy oxygen atoms of each aldehyde residue during complexation as they could coordinate, for instance, with the metal centre by an axial position, but also their role could be limited to intermolecular hydrogen-bond interactions.Figure 6
View along theb-axis for H2L2.


#### 3.1.2. Crystal Structure of1

Single crystals of complex1, suitable for X-ray diffraction studies, were obtained as described in the Materials and Methods. The crystal structure is shown in Figure 7 and main bond distances and angles are shown in Table 4.Table 4
Selected bond lengths (Å) and angles (°) for complex1.
Mn(1)-O(830)
1.870(15)
Mn(1)-N(1)
1.9816(19)
Mn(1)-N(20)
2.257(2)
Mn1-O(130)
1.8705(15)
Mn1-N(8)
1.9940(19)
Mn1-O(30)
2.2859(18)
O(830)-Mn(1)-O(130)
91.03(7)
N(8)-Mn(1)-O(9)
86.02(6)
O(830)-Mn(1)-N(1)
176.10(7)
N(1)-Mn(1)-O(9)
84.56(6)
O(130)-Mn(1)-N(1)
92.72(7)
O(830)-Mn(1)-O(9)
90.13(6)Figure 7
ORTEP view of the environment around the manganese ion in complex1.The monomer is composed by an approximately octahedral [MnL1(H2O)(DCA)] unit. The planar tetradentate Schiff base L1 is tightly bound to the manganese ion through the inner N2O2 compartment by the Nimine and Ophenol atoms (Mn-Nimine bond lengths of 1.9816–1.9940 Å and Mn-Ophenol of 1.87 Å which are typical of such complexes [14–16]), occupying the equatorial positions. The geometry around the manganese ion can be described as distorted and octahedral with the axial positions of the octahedron occupied by a water molecule and a dicyanamide molecule. The axial distances of 2.2859 Å (for Mn-O(30)) and 2.257 Å (for Mn-N(20)) are considerably longer than the equatorial Mn-O bond lengths quoted earlier, resulting in a rhombicity factor, expressed as the ratio between the Mn-O axial and Mn-O equatorial distances in the crystal structure, of 1.22. The deviation from an ideal octahedral geometry is also revealed by the range of angles observed around the metal centre (from 82.93° to 95.13°), as well as by the interaxial angle O(30)-Mn-N(20) of 173.92°.The octahedral [MnL1(H2O)(DCA)] entities are linked in pairs by µ-aquo bridges between neighbouring axial water molecules and phenoxy and methoxy oxygen atoms and also by π-π stacking interactions to give [MnL1(DCA)(H2O)]2 dimeric structures (Figure 8, Table 5). As a result of these supramolecular interactions, the Mn⋯Mn distances of about 4.96 Å are short for monomeric compounds. These types of systems have been reported in literature [15, 16] as µ-acuo dimers.Table 5
Hydrogen bonds for complex1.
D-H···A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O(30)-H(30A)⋯O(130)∗
0.83(2)
2.43(2)
3.061(2)
134(2)
O(30)-H(30A)⋯O(141)∗
0.83(2)
2.12(2)
2.908(2)
158(2)
O(30)-H(30B)⋯O(830)∗
0.76(3)
2.40(2)
3.034(3)
141(2)
O(30)-H(30B)⋯O(840)∗
0.76(3)
2.23(3)
2.922(3)
152(2)
C(841)-H(84A)⋯N(24)∗∗
0.98
2.51
3.449(4)
160
∗ = -x, -y, and 2-z; ∗∗ = 1-x, 1-y, and 2-z.Figure 8
Stick diagram for the dimeric unit for complex1 (manganese ion in magenta, oxygen in red, nitrogen in blue, and carbon in grey).


### 3.2. Peroxidase Studies

The peroxidase-like activity of1–3 was followed by the oxidation of the diammonium salt of 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid (ABTS) at pH 6.8. During this reaction, ABTS is oxidized by hydrogen peroxide to the radical cation ABTS•+ [33] in the presence of the appropriate peroxidase mimic. While ABTS is colourless, its radical cation ABTS•+ is green, showing characteristic absorption bands that can be easily followed by UV-spectroscopy. The extent of the reaction can be measured quantitatively at λ = 650 nm since ε = 12000 M−1 cm−1 has been determined [35].In our experiments, an aqueous solution of ABTS (50µL; 0.009 M; 4.5 × 10−7 mol) and a methanolic solution of the corresponding complexes1–3 (10 µL; 10−3 M; 10−8 mol) were added to water. The intensity of the UV absorption bands of ABTS started to increase immediately after the addition of an aqueous solution of H2O2 (50 µL; 10 M; 5 × 10−4 mol). The extent of the reaction can be measured quantitatively at λ = 650 nm since ε = 12000 M−1 cm−1 has been determined. The peroxidase-like activity results are collected in Table 6, where peroxidase activity is expressed as the percentage of the starting ABTS oxidized to its radical cation measured 10 min after mixing the solutions. The rate of formation of ABTS•+ of about 33–53% indicates that1 and2 behave as efficient peroxidase mimics, while3 does not present significant catalytic activity. Figure 9 shows the UV spectrum of the ABTS•+ radical cation obtained after ABTS reaction with H2O2 in presence of complex2, with the characteristic absorption bands at 415, 650, 735, and 815 nm.Table 6
Peroxidase activity for complexes1–22, axial and equatorial crystal distances around the manganese ion for each complex with solved crystallographic structure, resulting tetragonal elongation, and corresponding reference.
Complex
Crystal distances
Tetragonal elongationa
Peroxidase activityb
Reference
Mn-Oax
Mn-Oeq
1
M
n
L
1
D
D
C
A
2
c
2.28
1.870
1.22
33 ± 2
This work
2[MnL2(D)(DCA)](D)
un.
un.
un.
53 ± 3
This work
3[MnL3(D)(DCA)]
un.
un.
un.
1.9 ± 0.4
This work
4[MnL4(D)2(DCA)2]
2.303
1.885
1.225
37 ± 2
[16]
5 [MnL5(D)2](NO3)(D)
2.326
1.872
1.243
34 ± 3
[22]
6 [MnL5(D)Cl](D)2.5
2.318
1.878
1.234
31 ± 2
[15]
7[MnL5(D)2](ClO4)
2.314
1.865
1.24
19 ± 2
[23]
8 [MnL6(D)2](NO3)(D)
2.373
1.862
1.27
50 ± 3
[15]
9 [MnL7(D)2](NO3)(D)
2.263
1.880
1.203
32 ± 1
[22]
10 [MnL8(D)2](NO3)(D)
2.271
1.870
1.214
33 ± 1
[24]
11 [MnL1(D)2](ClO4)
2.36
1.851
1.27
30 ± 3
[23]
12A [MnL2(D)2](NO3)(D)
2.246
1.871
1.200
29 ± 1
[15]
12B [MnL2(D)(D2)](NO3)
2.258
1.879
1.202
29 ± 1
[15]
13 [MnL2(D)(OAc)](D)
2.282
1.893
1.205
33 ± 1
[15]
14A [MnL2(D)(O2CEt)]
2.308
1.869
1.235
28 ± 2
[14]
14B [MnL2(D)(O2CEt)]
2.338
1.876
1.246
28 ± 2
[14]
15 [MnL2(D)(O2CPen)]
2.339
1.865
1.254
39 ± 2
[14]
16 [MnL9(D)2](NO3)(D)2
2.25
1.872
1.202
18 ± 1
[15]
17 [MnL10(D)2](NO3)(D)2
2.243
1.889
1.187
2.0 ± 0.4
[24]
18 [MnL11(D)(D2)](ClO4)
2.203
1.863
1.183
3.2 ± 0.4
[25]
19 [MnL12(D)2](ClO4)(D)
2.22
1.88
1.181
2.4 ± 0.4
[26]
20 [MnL13(D)2](ClO4)(D)
2.21
1.90
1.163
2.1 ± 0.4
[27]
21 [MnL14(D)2](NO3)(D)2
2.206
1.904
1.159
1.1 ± 0.3
[22]
22 [MnL15(D)2](NO3)(D)2
2.258
1.888
1.196
1.8 ± 0.3
[24]
aTetragonal elongation expressed as the ratio between the manganese-axial oxygen distances and the manganese-equatorial oxygen distances. bPeroxidase activity expressed as percentage of conversion of ABTS to ABTS•+ measured 10 min after mixing the solutions; cD = H2O or other solvent molecule (such as CH3OH); un.: unavailable (structure not solved).Figure 9
UV-Vis absorption spectrum of ABTS + H2O2 +2, recorded 10 min after mixing the solution.Our previous findings in this field indicate a better catalytic behaviour when the substrate molecule is easily coordinated by the manganese complex, and this is favoured if the peroxidase mimic has either a vacancy in the coordination sphere or a labile ligand [14, 15]. For the complexes used in this study, the high efficiency as peroxidase mimics found for complexes1 and2 can be explained in this sense. Complexes1 and2, derived from H2L1 and H2L2, respectively, have a short two-carbon chain between imine groups in the Schiff ligand. The short chain constricts the chelate ring once nitrogen atom coordinates with the metal and led to a tetragonally elongated octahedral geometry for the manganese complex. An axial water molecule in this class of distorted geometries constitutes a quite labile ligand, which would generate a vacant position in the coordination sphere to accommodate the substrate molecule. Besides, the two methyl groups located in the methylene spacer (bound to C9) in H2L1, or the aromatic phenyl ring in H2L2, increase the steric effect and probably increase the distortion of the octahedral symmetry. These structural factors, derived from these Schiff bases, provoke the high rates of peroxidase activity for the obtained manganese complexes1 and2. In the case of3, the Schiff base ligand with a flexible three-membered alkyl chain between the imine groups favours a better stabilization of a high-symmetry octahedral geometry, which subsequently makes generation of a coordination site difficult. This type of flexible chain for3 is similar for complexes17–22 of Table 6.In this way, a correlation between the factor of tetragonal elongation and peroxidase activity has been already reported [14, 15]. This tetragonal elongation may be calculated as the ratio between the manganese-axial oxygen distances and the manganese-equatorial oxygen distances of the complexes with known structures solved by X-ray crystallography (complex1 and complexes4–22). Table 6 gives the values for a number of complexes and Figure 10 shows the plot of the tetragonal elongation versus their peroxidase activity of this collection of complexes. The strength of this correlation is clearly checked in the present work using data from twenty-two solved crystallographic structures.Figure 10
Peroxidase activity, expressed as percentage of ABTS conversion into ABTS•+, in function of the tetragonal elongation of the catalyst, expressed as the ratio between the Mn-O axial and Mn-O equatorial distances in crystal structures1 and4–22.


## 3.1. Crystallographic Characterization of H2L2 and Complex1

### 3.1.1. Crystal Structure of H2L2

The crystal structure reveals that H2L2 exists as discrete molecules, and it is composed of two identical 3-methoxy-2-hydrobenzylimine moieties twisted about the central aliphatic chain which acts as a spacer (Figure 5). The C12-N2 and C7-N1 distances of 1.272(3) and 1.279(3) Å, respectively, are practically identical and consistent with a C=N double bonding (Table 2), indicating both imine groups fully localized in the molecule [34]. The two oxygen O1 and O3 atoms are forming phenolic groups, and they present C-O distances of 1.354(3) Å and 1.351(3), respectively, corresponding to the expected single bonds. The C12-N2-C9 angle of 122.9(2)° confirms the sp2 character for N2 atom [32].Table 2
Selected geometric parameters (Å, °) for H2L2.
C12-N2
1.272(3)
C14-O3
1.351(3)
C12-N2-C9
122.9(2)
C7-N1
1.279(3)
C1-O1
1.354(3)
N2-C9-C8
106.65(19)Figure 5
ORTEP representation (50% probability) of H2L2.The disposition adopted by the free ligand in the solid state is conditioned by two strong intramolecular hydrogen-bond interactions which form two six-membered rings. These interactions arise from the contact between the hydroxy and the imine groups (see Table3). As expected, the O1-H1O•••N1 hydrogen bonding establishes an almost planar N1-C7-C6-C1-O1-H1 ring, the same for the O3-H3O•••N2 hydrogen bonding which establishes other almost planar N2-C12-C13-C14-O3-H3 rings.Table 3
Hydrogen bonds for H2L2.
D-H⋯A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O1-H1⋯N1
0.96
1.73
2.5839
146
O3-H3 ⋯N2
0.93
1.72
2.5891
154
C8-H8B⋯O1
0.99
2.55
3.4451
151Despite the mentioned intramolecular hydrogen interactions and a partial conjugation of the molecule, this one is not planar, probably due to the packing based on the intermolecular hydrogen bonds and theπ-stacking interactions between the salicyl residues of the neighbouring molecules (see Figure 6). The aromatic rings are arranged almost perpendicular to each other. Clearly, rotation about the C8-C9 bond to give a near-eclipsed or gauche conformation would achieve quasi-square-planar coordination environments using the inner ONNO site. According to this crystal structure study, this ligand should act as tetradentate donor in the equatorial plane about an octahedral metal centre. However, we cannot predict the role of the outer phenoxy oxygen atoms of each aldehyde residue during complexation as they could coordinate, for instance, with the metal centre by an axial position, but also their role could be limited to intermolecular hydrogen-bond interactions.Figure 6
View along theb-axis for H2L2.


### 3.1.2. Crystal Structure of1

Single crystals of complex1, suitable for X-ray diffraction studies, were obtained as described in the Materials and Methods. The crystal structure is shown in Figure 7 and main bond distances and angles are shown in Table 4.Table 4
Selected bond lengths (Å) and angles (°) for complex1.
Mn(1)-O(830)
1.870(15)
Mn(1)-N(1)
1.9816(19)
Mn(1)-N(20)
2.257(2)
Mn1-O(130)
1.8705(15)
Mn1-N(8)
1.9940(19)
Mn1-O(30)
2.2859(18)
O(830)-Mn(1)-O(130)
91.03(7)
N(8)-Mn(1)-O(9)
86.02(6)
O(830)-Mn(1)-N(1)
176.10(7)
N(1)-Mn(1)-O(9)
84.56(6)
O(130)-Mn(1)-N(1)
92.72(7)
O(830)-Mn(1)-O(9)
90.13(6)Figure 7
ORTEP view of the environment around the manganese ion in complex1.The monomer is composed by an approximately octahedral [MnL1(H2O)(DCA)] unit. The planar tetradentate Schiff base L1 is tightly bound to the manganese ion through the inner N2O2 compartment by the Nimine and Ophenol atoms (Mn-Nimine bond lengths of 1.9816–1.9940 Å and Mn-Ophenol of 1.87 Å which are typical of such complexes [14–16]), occupying the equatorial positions. The geometry around the manganese ion can be described as distorted and octahedral with the axial positions of the octahedron occupied by a water molecule and a dicyanamide molecule. The axial distances of 2.2859 Å (for Mn-O(30)) and 2.257 Å (for Mn-N(20)) are considerably longer than the equatorial Mn-O bond lengths quoted earlier, resulting in a rhombicity factor, expressed as the ratio between the Mn-O axial and Mn-O equatorial distances in the crystal structure, of 1.22. The deviation from an ideal octahedral geometry is also revealed by the range of angles observed around the metal centre (from 82.93° to 95.13°), as well as by the interaxial angle O(30)-Mn-N(20) of 173.92°.The octahedral [MnL1(H2O)(DCA)] entities are linked in pairs by µ-aquo bridges between neighbouring axial water molecules and phenoxy and methoxy oxygen atoms and also by π-π stacking interactions to give [MnL1(DCA)(H2O)]2 dimeric structures (Figure 8, Table 5). As a result of these supramolecular interactions, the Mn⋯Mn distances of about 4.96 Å are short for monomeric compounds. These types of systems have been reported in literature [15, 16] as µ-acuo dimers.Table 5
Hydrogen bonds for complex1.
D-H···A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O(30)-H(30A)⋯O(130)∗
0.83(2)
2.43(2)
3.061(2)
134(2)
O(30)-H(30A)⋯O(141)∗
0.83(2)
2.12(2)
2.908(2)
158(2)
O(30)-H(30B)⋯O(830)∗
0.76(3)
2.40(2)
3.034(3)
141(2)
O(30)-H(30B)⋯O(840)∗
0.76(3)
2.23(3)
2.922(3)
152(2)
C(841)-H(84A)⋯N(24)∗∗
0.98
2.51
3.449(4)
160
∗ = -x, -y, and 2-z; ∗∗ = 1-x, 1-y, and 2-z.Figure 8
Stick diagram for the dimeric unit for complex1 (manganese ion in magenta, oxygen in red, nitrogen in blue, and carbon in grey).


## 3.1.1. Crystal Structure of H2L2

The crystal structure reveals that H2L2 exists as discrete molecules, and it is composed of two identical 3-methoxy-2-hydrobenzylimine moieties twisted about the central aliphatic chain which acts as a spacer (Figure 5). The C12-N2 and C7-N1 distances of 1.272(3) and 1.279(3) Å, respectively, are practically identical and consistent with a C=N double bonding (Table 2), indicating both imine groups fully localized in the molecule [34]. The two oxygen O1 and O3 atoms are forming phenolic groups, and they present C-O distances of 1.354(3) Å and 1.351(3), respectively, corresponding to the expected single bonds. The C12-N2-C9 angle of 122.9(2)° confirms the sp2 character for N2 atom [32].Table 2
Selected geometric parameters (Å, °) for H2L2.
C12-N2
1.272(3)
C14-O3
1.351(3)
C12-N2-C9
122.9(2)
C7-N1
1.279(3)
C1-O1
1.354(3)
N2-C9-C8
106.65(19)Figure 5
ORTEP representation (50% probability) of H2L2.The disposition adopted by the free ligand in the solid state is conditioned by two strong intramolecular hydrogen-bond interactions which form two six-membered rings. These interactions arise from the contact between the hydroxy and the imine groups (see Table3). As expected, the O1-H1O•••N1 hydrogen bonding establishes an almost planar N1-C7-C6-C1-O1-H1 ring, the same for the O3-H3O•••N2 hydrogen bonding which establishes other almost planar N2-C12-C13-C14-O3-H3 rings.Table 3
Hydrogen bonds for H2L2.
D-H⋯A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O1-H1⋯N1
0.96
1.73
2.5839
146
O3-H3 ⋯N2
0.93
1.72
2.5891
154
C8-H8B⋯O1
0.99
2.55
3.4451
151Despite the mentioned intramolecular hydrogen interactions and a partial conjugation of the molecule, this one is not planar, probably due to the packing based on the intermolecular hydrogen bonds and theπ-stacking interactions between the salicyl residues of the neighbouring molecules (see Figure 6). The aromatic rings are arranged almost perpendicular to each other. Clearly, rotation about the C8-C9 bond to give a near-eclipsed or gauche conformation would achieve quasi-square-planar coordination environments using the inner ONNO site. According to this crystal structure study, this ligand should act as tetradentate donor in the equatorial plane about an octahedral metal centre. However, we cannot predict the role of the outer phenoxy oxygen atoms of each aldehyde residue during complexation as they could coordinate, for instance, with the metal centre by an axial position, but also their role could be limited to intermolecular hydrogen-bond interactions.Figure 6
View along theb-axis for H2L2.


## 3.1.2. Crystal Structure of1

Single crystals of complex1, suitable for X-ray diffraction studies, were obtained as described in the Materials and Methods. The crystal structure is shown in Figure 7 and main bond distances and angles are shown in Table 4.Table 4
Selected bond lengths (Å) and angles (°) for complex1.
Mn(1)-O(830)
1.870(15)
Mn(1)-N(1)
1.9816(19)
Mn(1)-N(20)
2.257(2)
Mn1-O(130)
1.8705(15)
Mn1-N(8)
1.9940(19)
Mn1-O(30)
2.2859(18)
O(830)-Mn(1)-O(130)
91.03(7)
N(8)-Mn(1)-O(9)
86.02(6)
O(830)-Mn(1)-N(1)
176.10(7)
N(1)-Mn(1)-O(9)
84.56(6)
O(130)-Mn(1)-N(1)
92.72(7)
O(830)-Mn(1)-O(9)
90.13(6)Figure 7
ORTEP view of the environment around the manganese ion in complex1.The monomer is composed by an approximately octahedral [MnL1(H2O)(DCA)] unit. The planar tetradentate Schiff base L1 is tightly bound to the manganese ion through the inner N2O2 compartment by the Nimine and Ophenol atoms (Mn-Nimine bond lengths of 1.9816–1.9940 Å and Mn-Ophenol of 1.87 Å which are typical of such complexes [14–16]), occupying the equatorial positions. The geometry around the manganese ion can be described as distorted and octahedral with the axial positions of the octahedron occupied by a water molecule and a dicyanamide molecule. The axial distances of 2.2859 Å (for Mn-O(30)) and 2.257 Å (for Mn-N(20)) are considerably longer than the equatorial Mn-O bond lengths quoted earlier, resulting in a rhombicity factor, expressed as the ratio between the Mn-O axial and Mn-O equatorial distances in the crystal structure, of 1.22. The deviation from an ideal octahedral geometry is also revealed by the range of angles observed around the metal centre (from 82.93° to 95.13°), as well as by the interaxial angle O(30)-Mn-N(20) of 173.92°.The octahedral [MnL1(H2O)(DCA)] entities are linked in pairs by µ-aquo bridges between neighbouring axial water molecules and phenoxy and methoxy oxygen atoms and also by π-π stacking interactions to give [MnL1(DCA)(H2O)]2 dimeric structures (Figure 8, Table 5). As a result of these supramolecular interactions, the Mn⋯Mn distances of about 4.96 Å are short for monomeric compounds. These types of systems have been reported in literature [15, 16] as µ-acuo dimers.Table 5
Hydrogen bonds for complex1.
D-H···A (Å)
D-H (Å)
H⋯A (Å)
D⋯A (Å)
D-H⋯A (Å)
O(30)-H(30A)⋯O(130)∗
0.83(2)
2.43(2)
3.061(2)
134(2)
O(30)-H(30A)⋯O(141)∗
0.83(2)
2.12(2)
2.908(2)
158(2)
O(30)-H(30B)⋯O(830)∗
0.76(3)
2.40(2)
3.034(3)
141(2)
O(30)-H(30B)⋯O(840)∗
0.76(3)
2.23(3)
2.922(3)
152(2)
C(841)-H(84A)⋯N(24)∗∗
0.98
2.51
3.449(4)
160
∗ = -x, -y, and 2-z; ∗∗ = 1-x, 1-y, and 2-z.Figure 8
Stick diagram for the dimeric unit for complex1 (manganese ion in magenta, oxygen in red, nitrogen in blue, and carbon in grey).


## 3.2. Peroxidase Studies

The peroxidase-like activity of1–3 was followed by the oxidation of the diammonium salt of 2,2′-azinobis-(3-ethylbenzothiazoline)-6-sulfonic acid (ABTS) at pH 6.8. During this reaction, ABTS is oxidized by hydrogen peroxide to the radical cation ABTS•+ [33] in the presence of the appropriate peroxidase mimic. While ABTS is colourless, its radical cation ABTS•+ is green, showing characteristic absorption bands that can be easily followed by UV-spectroscopy. The extent of the reaction can be measured quantitatively at λ = 650 nm since ε = 12000 M−1 cm−1 has been determined [35].In our experiments, an aqueous solution of ABTS (50µL; 0.009 M; 4.5 × 10−7 mol) and a methanolic solution of the corresponding complexes1–3 (10 µL; 10−3 M; 10−8 mol) were added to water. The intensity of the UV absorption bands of ABTS started to increase immediately after the addition of an aqueous solution of H2O2 (50 µL; 10 M; 5 × 10−4 mol). The extent of the reaction can be measured quantitatively at λ = 650 nm since ε = 12000 M−1 cm−1 has been determined. The peroxidase-like activity results are collected in Table 6, where peroxidase activity is expressed as the percentage of the starting ABTS oxidized to its radical cation measured 10 min after mixing the solutions. The rate of formation of ABTS•+ of about 33–53% indicates that1 and2 behave as efficient peroxidase mimics, while3 does not present significant catalytic activity. Figure 9 shows the UV spectrum of the ABTS•+ radical cation obtained after ABTS reaction with H2O2 in presence of complex2, with the characteristic absorption bands at 415, 650, 735, and 815 nm.Table 6
Peroxidase activity for complexes1–22, axial and equatorial crystal distances around the manganese ion for each complex with solved crystallographic structure, resulting tetragonal elongation, and corresponding reference.
Complex
Crystal distances
Tetragonal elongationa
Peroxidase activityb
Reference
Mn-Oax
Mn-Oeq
1
M
n
L
1
D
D
C
A
2
c
2.28
1.870
1.22
33 ± 2
This work
2[MnL2(D)(DCA)](D)
un.
un.
un.
53 ± 3
This work
3[MnL3(D)(DCA)]
un.
un.
un.
1.9 ± 0.4
This work
4[MnL4(D)2(DCA)2]
2.303
1.885
1.225
37 ± 2
[16]
5 [MnL5(D)2](NO3)(D)
2.326
1.872
1.243
34 ± 3
[22]
6 [MnL5(D)Cl](D)2.5
2.318
1.878
1.234
31 ± 2
[15]
7[MnL5(D)2](ClO4)
2.314
1.865
1.24
19 ± 2
[23]
8 [MnL6(D)2](NO3)(D)
2.373
1.862
1.27
50 ± 3
[15]
9 [MnL7(D)2](NO3)(D)
2.263
1.880
1.203
32 ± 1
[22]
10 [MnL8(D)2](NO3)(D)
2.271
1.870
1.214
33 ± 1
[24]
11 [MnL1(D)2](ClO4)
2.36
1.851
1.27
30 ± 3
[23]
12A [MnL2(D)2](NO3)(D)
2.246
1.871
1.200
29 ± 1
[15]
12B [MnL2(D)(D2)](NO3)
2.258
1.879
1.202
29 ± 1
[15]
13 [MnL2(D)(OAc)](D)
2.282
1.893
1.205
33 ± 1
[15]
14A [MnL2(D)(O2CEt)]
2.308
1.869
1.235
28 ± 2
[14]
14B [MnL2(D)(O2CEt)]
2.338
1.876
1.246
28 ± 2
[14]
15 [MnL2(D)(O2CPen)]
2.339
1.865
1.254
39 ± 2
[14]
16 [MnL9(D)2](NO3)(D)2
2.25
1.872
1.202
18 ± 1
[15]
17 [MnL10(D)2](NO3)(D)2
2.243
1.889
1.187
2.0 ± 0.4
[24]
18 [MnL11(D)(D2)](ClO4)
2.203
1.863
1.183
3.2 ± 0.4
[25]
19 [MnL12(D)2](ClO4)(D)
2.22
1.88
1.181
2.4 ± 0.4
[26]
20 [MnL13(D)2](ClO4)(D)
2.21
1.90
1.163
2.1 ± 0.4
[27]
21 [MnL14(D)2](NO3)(D)2
2.206
1.904
1.159
1.1 ± 0.3
[22]
22 [MnL15(D)2](NO3)(D)2
2.258
1.888
1.196
1.8 ± 0.3
[24]
aTetragonal elongation expressed as the ratio between the manganese-axial oxygen distances and the manganese-equatorial oxygen distances. bPeroxidase activity expressed as percentage of conversion of ABTS to ABTS•+ measured 10 min after mixing the solutions; cD = H2O or other solvent molecule (such as CH3OH); un.: unavailable (structure not solved).Figure 9
UV-Vis absorption spectrum of ABTS + H2O2 +2, recorded 10 min after mixing the solution.Our previous findings in this field indicate a better catalytic behaviour when the substrate molecule is easily coordinated by the manganese complex, and this is favoured if the peroxidase mimic has either a vacancy in the coordination sphere or a labile ligand [14, 15]. For the complexes used in this study, the high efficiency as peroxidase mimics found for complexes1 and2 can be explained in this sense. Complexes1 and2, derived from H2L1 and H2L2, respectively, have a short two-carbon chain between imine groups in the Schiff ligand. The short chain constricts the chelate ring once nitrogen atom coordinates with the metal and led to a tetragonally elongated octahedral geometry for the manganese complex. An axial water molecule in this class of distorted geometries constitutes a quite labile ligand, which would generate a vacant position in the coordination sphere to accommodate the substrate molecule. Besides, the two methyl groups located in the methylene spacer (bound to C9) in H2L1, or the aromatic phenyl ring in H2L2, increase the steric effect and probably increase the distortion of the octahedral symmetry. These structural factors, derived from these Schiff bases, provoke the high rates of peroxidase activity for the obtained manganese complexes1 and2. In the case of3, the Schiff base ligand with a flexible three-membered alkyl chain between the imine groups favours a better stabilization of a high-symmetry octahedral geometry, which subsequently makes generation of a coordination site difficult. This type of flexible chain for3 is similar for complexes17–22 of Table 6.In this way, a correlation between the factor of tetragonal elongation and peroxidase activity has been already reported [14, 15]. This tetragonal elongation may be calculated as the ratio between the manganese-axial oxygen distances and the manganese-equatorial oxygen distances of the complexes with known structures solved by X-ray crystallography (complex1 and complexes4–22). Table 6 gives the values for a number of complexes and Figure 10 shows the plot of the tetragonal elongation versus their peroxidase activity of this collection of complexes. The strength of this correlation is clearly checked in the present work using data from twenty-two solved crystallographic structures.Figure 10
Peroxidase activity, expressed as percentage of ABTS conversion into ABTS•+, in function of the tetragonal elongation of the catalyst, expressed as the ratio between the Mn-O axial and Mn-O equatorial distances in crystal structures1 and4–22.


## 4. Conclusions

The synthesis and structural characterization of the Schiff base compounds N,N′-bis(2-hydroxy-4-methoxybenzylidene)-1,2-diphenylendiimine (H2L1) and N,N′-bis(2-hydroxy-4-methoxybenzylidene)-1,2-diamino-2-methylpropane (H2L2) have been reported. These two organic compounds behave as suitable ligands for coordination with metal ions, highly versatile due to different structural features: being tetradentate, ability to extend the hydrogen network using the outer methoxy groups, short and bulky spacer, etc. Three new manganese(III)-L-dicyanamide complexes have been obtained and characterized. The short two-carbon chain between imine groups in H2L1-H2L2 provokes tetragonally elongated octahedral geometries in the resulting complexes, which may increase their potential as catalysts for different applications. The correlation of peroxidase activity and the rhombicity caused by the short length of the Schiff base should be taken into account for designing new potential catalytic systems.



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*Source: 5465890-2017-08-16.xml*