# Synthesis, Spectroscopic, and Thermal Investigations of Metal Complexes with Mefenamic Acid

Authors: Karolina Kafarska; Michał Gacki; Wojciech M. Wolf
Journal: Journal of Chemistry
 (2017)

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## Abstract

The novel metal complexes with empirical formulae M(mef)2·nH2O (where M = Mn(II), Co(II), Ni(II), Cu(II), Zn(II), and Cd(II); mef is the mefenamic ligand) were synthesized and characterized by elemental analysis, molar conductance, FTIR-spectroscopy, and thermal decomposition techniques. All IR spectra revealed absorption bands related to the asymmetric (νas) and symmetric (νs) vibrations of carboxylate group. The Nakamoto criteria clearly indicate that this group is bonded in a bidentate chelate mode. The thermal behavior of complexes was studied by TGA methods under non-isothermal condition in air. Upon heating, all compounds decompose progressively to metal oxides, which are the final products of pyrolysis. Cu(II), Zn(II), and Cd(II) complexes were also characterized by the coupled TG-FTIR technique, which finally proved the path and gaseous products of thermal decomposition. Additionally, the coupled TG-MS system was used to determine the principal volatile products of thermolysis and fragmentation processes of Mn(mef)2·3H2O and Co(mef)2·2H2O.


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## Body

## 1. Introduction

Fenemates (N-arylated derivatives of anthranilic acid) are pharmaceutical compounds with distinct anti-inflammatory and analgesic, antipyretic activity. Their mode of biological action is based on inhibiting prostaglandin synthetase [1, 2]. In particular, 2-(2,3-dimethyl-phenyl) aminobenzoic acid (mefenamic acid: (CH3)2C5H3NHC5H4COOH (Figure 1)) is an effective nonsteroidal agent widely used for the treatment of mild to moderate pains, inflammation, ache, and fever [3–5]. Moreover mefenamic acid, as other anti-inflammatory drugs, is emerging as novel chemopreventive agents against cancer [6, 7]. It is an active ingredient of numerous drugs which are present on the pharmaceutical market [8, 9]. However, NSAID-induced side effects, particularly in the gastrointestinal tract and kidney, often limit their applications. For this reason, considerable efforts have been made to increase their activity while minimizing side effects [10].Figure 1
Chemical structure of mefenamic acid.It is well known that several transition metal complexes with nonsteroidal drugs are more effective and show significantly lower toxicity than that of their parent drugs [11, 12]. In particular, divalent metal complexes with several NSAID are better anti-inflammatory candidates then NSAIDs, because they have unique structures that could interact with the target enzymes more specifically. In addition, metal ions introduce extra antioxidant activity [13] and antiproliferative activity against cancer [14–16]. Furthermore gastrointestinal toxicities associated with the administration of complexes are much lower than those of the parent drug and improved safety of these drugs [17].Our studies were stimulated by the fact that majority of anti-inflammatory drugs are carboxylic acids with their carboxylate group prone to metal binding [11, 18–20]. Some of mefenamate complexes have been described in the literature. Brzyska and Ożga characterized complexes of rare earth metals with mefenamic ligand [21]. Tapacli and Ide described mefenamate compounds with Ca and Na ions [22]. Kovala-Demertzi et al.  investigated the compounds with the formulae: SnPh3(mef) and SnBu2(mef)2 [23].The aim of the present work was to obtain the mefenamate complexes of Mn(II), Co(II), Ni(II), Cu(II), Zn(II), and Cd(II), determine their chemical properties, and study their thermal decomposition patterns.


## 2. Materials and Methods

### 2.1. Materials

Pure mefenamic acid was obtained as a gift from Polfa Pabianice; metal chlorides MCl2·nH2O (where M = Mn, Co, Ni, Cu, Zn, and Cd), DMSO, DMF, and EtOH p.a. were purchased from Aldrich and MeOH from Lab-Scan; other chemicals were from POCh-Gliwice.


### 2.2. Synthesis

All complexes were obtained according to similar procedures. The first step of synthesis was preparation sodium salt of ligand by dissolution of mefenamic (1 mmol) acid in 50 mL fresh precipitated aqueous-ethanol solution (1 : 1) of NaOH (0,02 mol·L−1). The mixture was heated up to 60°C and added to aqueous solution of metal chlorides (0,5 mol in 25 mL). The reaction mixture was kept in 60°C for 2 hours. After several days the solid precipitates were isolated by filtration, washed with hot water, and dried on air.Complex Mn(mef)2·3H2O: color: pale pink; IR (KBr, ν): 3358 (OH), 3067 (NH), 2859 (CH), 1652 (NH), 1578 (OCO-), 1495 (NH), 1459 (CH3), 1394 (OCO-), 1283 (CH3), 1183 (CH3), 1159 (CH), 1093 (CH), 1043 (CH3), 852 (CH), 749 (CH3), 679 (MO) cm−1; Anal. Calc. C30H34MnN2O7 (%): C, 61.12; H, 5.81; N, 4.75; Mn, 9.32; Found (%): C, 61.00; H, 5.50; N, 4.76; Mn, 9.36.Complex Co(mef)2·2H2O: color: pink; IR (KBr, ν): 3315 (OH), 3069 (NH), 1651 (NH), 1578 (OCO-), 1504 (NH), 1454 (CH3), 1393 (OCO-), 1283 (CH3), 1188 (CH3), 1159 (CH), 1097 (CH), 1043 (CH3), 854 (CH), 748 (CH3), 675 (MO) cm−1; Anal. Calc. C30H32CoN2O6 (%): C, 62.61; H, 5.60; N, 4.87; Co, 10.24; Found (%): C, 62.67; H, 5.60; N, 4.88; Co, 10.22.Complex Ni(mef)2·2H2O: color: pale green; IR (KBr, ν): 3346 (OH), 3069 (NH), 2860 (CH), 1653 (NH), 1578 (OCO-), 1499 (NH), 1455 (CH3), 1391 (OCO-), 1285 (CH3), 1190 (CH3), 1159 (CH), 1097 (CH), 1043 (CH3), 851 (CH), 748 (CH3), 678 (MO) cm−1; Anal. Calc. C30H32NiN2O6 (%): C, 62.64; H, 5.60; N, 4.87; Ni, 10.20; Found (%): C, 62.70; H, 5.49; N, 4.98; Ni, 10.21.Complex Cu(mef)2·2H2O: color: green; IR (KBr, ν): 3321 (OH), 3077 (NH), 2910 (CH), 1647 (NH), 1578 (OCO-), 1506 (NH), 1458 (CH3), 1393 (OCO-), 1285 (CH3), 1188 (CH3), 1153 (CH), 1067 (CH), 1034 (CH3), 854 (CH), 746 (CH3), 680 (MO) cm−1; Anal. Calc. C30H32CuN2O6 (%): C, 62.11; H, 5.56; N, 4.83; Cu, 10.95; Found (%): C, 62.08; H, 5.59; N, 4.85; Cu, 10.44.Complex Zn(mef)2·2H2O: color: white; IR (KBr, ν): 3338 (OH), 3066 (NH), 2858 (CH), 1651 (NH), 1576 (OCO-), 1506 (NH), 1466 (CH3), 1388 (OCO-), 1283 (CH3), 1183 (CH3), 1155 (CH), 1069 (CH), 1043 (CH3), 856 (CH), 748 (CH3), 677 (MO) cm−1; Anal. Calc. C30H32ZnN2O6 (%): C, 61.92; H, 5.54; N, 4.81; Zn, 11.23; Found (%): C, 61.88; H, 5.50; N, 4.88; Zn, 11.25.Complex Cd(mef)2·2H2O: color: white; IR (KBr, ν): 3312 (OH), 3067 (NH), 2858 (CH), 1651 (NH), 1576 (OCO-), 1499 (NH), 1452 (CH3), 1396 (OCO-), 1283 (CH3), 1190 (CH3), 1159 (CH), 1043 (CH3), 862 (CH), 750 (CH3), 679 (MO) cm−1; Anal. Calc. C30H32CdN2O6 (%): C, 57.29; H, 5.13; N, 4.45; Cd, 17.86; Found (%): C, 57.30; H, 5.15; N, 4.53; Cd, 17.90.


### 2.3. Measurements

The chemical compositions of all complexes were defined by the elemental analysis followed by the atomic absorption spectrometry. Hydrogen, carbon, and nitrogen contents were measured with the Vario EL III Elemental Analyzer. The metal content was determined in samples mineralized using the Anton Paar Multiwave 3000 closed system instrument. The mixture of concentrated HNO3 (6 mL) and HCl (2 mL) was applied. Metal concentrations were measured by the FAAS with the GBC Scientific Equipment 932 plus spectrometer.IR spectra were recorded on FTIR-8501 Shimadzu spectrophotometer over 4000–400 cm−1 range using KBr pellets. The thermal stabilities of complexes were studied by means of TGA techniques. The measurements were made with the Netzsch, TG 209 apparatus, and Q-1500 Derivatograph. Samples (1·10−2 g) were heated (in ceramic crucibles) up to 1000°C, at a heating rate 10°C min−1 in air atmosphere. The analysis of solid decomposition products was performed using TG and DTG curves and supported by the X-ray diffractograms (Siemens D-5000 diffractometer, graphite monochromatized CuKα radiation) of sinters, obtained by heating the complex samples up to temperatures defined from TG curves. A coupled TG-MS system was applied for analysis of volatile products of thermal decomposition and fragmentation processes. Data were processed using online connected computer system with commercial software (Derivatograph TG/DTA-SETSYS-16/18, coupled to a Mass Spectrometer QMS-422 model ThermoStart from Balzers); platinum crucible, mass sample: 4–6 mg. Dynamic measurements were carried out in argon atmosphere (at a flow rate 20 mL·min−1) with a heating rate 10°C·min−1 and an ion source temperature ofca. 150°C using 70 eV electron impact ionization. The TG-FTIR measurements were carried out in ceramic crucibles at flowing argon atmosphere (20 mL·min−1) using the Netzsch TG 209 apparatus coupled with Bruker FTIR spectrophotometer. The samples were heated up to 1000°C at a heating rate 10°C·min−1. Molar conductivity (ΛM) of all synthesized compounds was measured in 1·10−3 mol·L−1 solutions of MeOH, DMSO, and DMF, according to procedure as described in [24].


## 2.1. Materials

Pure mefenamic acid was obtained as a gift from Polfa Pabianice; metal chlorides MCl2·nH2O (where M = Mn, Co, Ni, Cu, Zn, and Cd), DMSO, DMF, and EtOH p.a. were purchased from Aldrich and MeOH from Lab-Scan; other chemicals were from POCh-Gliwice.


## 2.2. Synthesis

All complexes were obtained according to similar procedures. The first step of synthesis was preparation sodium salt of ligand by dissolution of mefenamic (1 mmol) acid in 50 mL fresh precipitated aqueous-ethanol solution (1 : 1) of NaOH (0,02 mol·L−1). The mixture was heated up to 60°C and added to aqueous solution of metal chlorides (0,5 mol in 25 mL). The reaction mixture was kept in 60°C for 2 hours. After several days the solid precipitates were isolated by filtration, washed with hot water, and dried on air.Complex Mn(mef)2·3H2O: color: pale pink; IR (KBr, ν): 3358 (OH), 3067 (NH), 2859 (CH), 1652 (NH), 1578 (OCO-), 1495 (NH), 1459 (CH3), 1394 (OCO-), 1283 (CH3), 1183 (CH3), 1159 (CH), 1093 (CH), 1043 (CH3), 852 (CH), 749 (CH3), 679 (MO) cm−1; Anal. Calc. C30H34MnN2O7 (%): C, 61.12; H, 5.81; N, 4.75; Mn, 9.32; Found (%): C, 61.00; H, 5.50; N, 4.76; Mn, 9.36.Complex Co(mef)2·2H2O: color: pink; IR (KBr, ν): 3315 (OH), 3069 (NH), 1651 (NH), 1578 (OCO-), 1504 (NH), 1454 (CH3), 1393 (OCO-), 1283 (CH3), 1188 (CH3), 1159 (CH), 1097 (CH), 1043 (CH3), 854 (CH), 748 (CH3), 675 (MO) cm−1; Anal. Calc. C30H32CoN2O6 (%): C, 62.61; H, 5.60; N, 4.87; Co, 10.24; Found (%): C, 62.67; H, 5.60; N, 4.88; Co, 10.22.Complex Ni(mef)2·2H2O: color: pale green; IR (KBr, ν): 3346 (OH), 3069 (NH), 2860 (CH), 1653 (NH), 1578 (OCO-), 1499 (NH), 1455 (CH3), 1391 (OCO-), 1285 (CH3), 1190 (CH3), 1159 (CH), 1097 (CH), 1043 (CH3), 851 (CH), 748 (CH3), 678 (MO) cm−1; Anal. Calc. C30H32NiN2O6 (%): C, 62.64; H, 5.60; N, 4.87; Ni, 10.20; Found (%): C, 62.70; H, 5.49; N, 4.98; Ni, 10.21.Complex Cu(mef)2·2H2O: color: green; IR (KBr, ν): 3321 (OH), 3077 (NH), 2910 (CH), 1647 (NH), 1578 (OCO-), 1506 (NH), 1458 (CH3), 1393 (OCO-), 1285 (CH3), 1188 (CH3), 1153 (CH), 1067 (CH), 1034 (CH3), 854 (CH), 746 (CH3), 680 (MO) cm−1; Anal. Calc. C30H32CuN2O6 (%): C, 62.11; H, 5.56; N, 4.83; Cu, 10.95; Found (%): C, 62.08; H, 5.59; N, 4.85; Cu, 10.44.Complex Zn(mef)2·2H2O: color: white; IR (KBr, ν): 3338 (OH), 3066 (NH), 2858 (CH), 1651 (NH), 1576 (OCO-), 1506 (NH), 1466 (CH3), 1388 (OCO-), 1283 (CH3), 1183 (CH3), 1155 (CH), 1069 (CH), 1043 (CH3), 856 (CH), 748 (CH3), 677 (MO) cm−1; Anal. Calc. C30H32ZnN2O6 (%): C, 61.92; H, 5.54; N, 4.81; Zn, 11.23; Found (%): C, 61.88; H, 5.50; N, 4.88; Zn, 11.25.Complex Cd(mef)2·2H2O: color: white; IR (KBr, ν): 3312 (OH), 3067 (NH), 2858 (CH), 1651 (NH), 1576 (OCO-), 1499 (NH), 1452 (CH3), 1396 (OCO-), 1283 (CH3), 1190 (CH3), 1159 (CH), 1043 (CH3), 862 (CH), 750 (CH3), 679 (MO) cm−1; Anal. Calc. C30H32CdN2O6 (%): C, 57.29; H, 5.13; N, 4.45; Cd, 17.86; Found (%): C, 57.30; H, 5.15; N, 4.53; Cd, 17.90.


## 2.3. Measurements

The chemical compositions of all complexes were defined by the elemental analysis followed by the atomic absorption spectrometry. Hydrogen, carbon, and nitrogen contents were measured with the Vario EL III Elemental Analyzer. The metal content was determined in samples mineralized using the Anton Paar Multiwave 3000 closed system instrument. The mixture of concentrated HNO3 (6 mL) and HCl (2 mL) was applied. Metal concentrations were measured by the FAAS with the GBC Scientific Equipment 932 plus spectrometer.IR spectra were recorded on FTIR-8501 Shimadzu spectrophotometer over 4000–400 cm−1 range using KBr pellets. The thermal stabilities of complexes were studied by means of TGA techniques. The measurements were made with the Netzsch, TG 209 apparatus, and Q-1500 Derivatograph. Samples (1·10−2 g) were heated (in ceramic crucibles) up to 1000°C, at a heating rate 10°C min−1 in air atmosphere. The analysis of solid decomposition products was performed using TG and DTG curves and supported by the X-ray diffractograms (Siemens D-5000 diffractometer, graphite monochromatized CuKα radiation) of sinters, obtained by heating the complex samples up to temperatures defined from TG curves. A coupled TG-MS system was applied for analysis of volatile products of thermal decomposition and fragmentation processes. Data were processed using online connected computer system with commercial software (Derivatograph TG/DTA-SETSYS-16/18, coupled to a Mass Spectrometer QMS-422 model ThermoStart from Balzers); platinum crucible, mass sample: 4–6 mg. Dynamic measurements were carried out in argon atmosphere (at a flow rate 20 mL·min−1) with a heating rate 10°C·min−1 and an ion source temperature ofca. 150°C using 70 eV electron impact ionization. The TG-FTIR measurements were carried out in ceramic crucibles at flowing argon atmosphere (20 mL·min−1) using the Netzsch TG 209 apparatus coupled with Bruker FTIR spectrophotometer. The samples were heated up to 1000°C at a heating rate 10°C·min−1. Molar conductivity (ΛM) of all synthesized compounds was measured in 1·10−3 mol·L−1 solutions of MeOH, DMSO, and DMF, according to procedure as described in [24].


## 3. Results and Discussion

The empirical formulae of complexes showing number of water molecules and molar conductivities are presented in Table1. All synthesized solid complexes are stable in air. They are practically insoluble in water, but on the contrary quite soluble in polar organic solvents (e.g., EtOH, MeOH). Analysis of X-ray powder diffraction data reveals high level of crystallinity and proves that neither pair of investigated compounds is isostructural. The molar conductivity data clearly indicate that all complexes in MeOH and DMSO as well as Co(II), Ni(II), and Cu(II) compounds in DMF are non-electrolytes. On the other hand, molar conductivities for Mn(mef)2·3H2O in MeOH and DMF and Zn(mef)2·2H2O and Cd(mef)2·2H2O point out that solutions of these compounds according to the Geary criterion [25] are intermediates between those of nonelectrolytes and 1 : 1 electrolytes.Table 1
Molar conductivity of complexesΛM/Ω−1 cm2·mol−1 for 0,001 mol·L−1 solutions in MeOH, DMF, and DMSO at 25°C.
Complex
Λ
M
[Ω−1 cm2 mol−1]
MeOH
DMF
DMSO
Mn(mef)2·3H2O
45.20
35.70
16.90
Co(mef)2·2H2O
11.23
13.03
3.07
Ni(mef)2·2H2O
17.07
20.05
7.09
Cu(mef)2·2H2O
12.05
13.15
4.27
Zn(mef)2·2H2O
21.0
28.11
3.17
Cd(mef)2·2H2O
18.18
24.34
4.55


### 3.1. FTIR Spectra

The IR spectra of all complexes exhibit a broad absorption band in the water stretching region (3300–3600 cm−1). Additionally, bands related to the water bending vibrations are observed (1615–1620 cm−1). In all spectra the valence vibrations of monodissociated carboxylic group are not observed. On the contrary, asymmetric (1575–1578 cm−1) and symmetric (1386–1394 cm−1) vibration of dissociated OCO- group are clearly observed (Table 2). These bands are affected by the coordination of mefenamic ligand to metal ions. The separation Δν=νas(OCO)-νs(OCO) and the direction of the shifts of these bands in comparison to those values of sodium salt characterized the nature of the metal–carboxylate bonds. The bathochromic shifts of asymmetric (νas) and hypsochromic shifts of symmetric (νs) frequencies are also observed. The magnitude of separation and the bands direction show that carboxylate group of mefenamic ligand coordinated in bidentate chelate mode [26].Table 2
Principal IR bands (cm−1) for carboxylate group in investigated complexes.
Compound
ν
a
s
y
m
ν
s
y
m
Δ
ν
=
ν
a
s
y
m
-
ν
s
y
m
Na(mef)
1580,0
1380,0
200,0
Mn(mef)2·3H2O
1577,7
1393,6
184,1
Co(mef)2·2H2O
1577,7
1392,5
185,2
Ni(mef)2·2H2O
1577,7
1390,6
187,1
Cu(mef)2·2H2O
1577,7
1392,5
185,2
Zn(mef)2·2H2O
1575,7
1386,7
189,0
Cd(mef)2·2H2O
1575,7
1396,4
178,7Apart from carboxylate group the mefenamic anion has amine group, available for coordination. The NH deformation vibrations in the IR spectra of mefenamic acid are very close to those observed in the IR spectra of its complexes. That indicates that the NH group does not participate directly in coordination.


### 3.2. Thermal Analysis

The data obtained from TG, DTG, and DTA curves supported by chemical and X-ray diffraction pattern investigations are collected in Table3. The thermal decomposition curves of Cd(mef)2·2H2O are shown on Figure 2. The thermal decomposition of the complexes is a multistages process. All compounds started to decompose by dehydration accompanied by the endothermic effect. Majority of complexes lose their water molecules in one step. Only for Co(II) and Zn(II) complexes water elimination is two-stage transformation. Thermolyses of these complexes are quite similar. The two-stage dehydration (60–110°C, 130–240°C and 100–160°C, 160–190°C for Co(II) and Zn(II) compound, respectively) is followed by organic ligand thermodestruction and metal carbonate formation. Further heating leads to metal oxides: ZnO and CoO. The latter is obtained via Co3O4 intermediate. In the terminal step of pyrolysis the DTA curve exhibits exoeffects. Formation of oxides was confirmed by the powder X-ray diffraction technique (Figure 3).Table 3
Thermal decomposition data of complexes in air.
Compounds
Ranges of decomp., °C
DTA peaks, °C
Mass loss, %
Intermediate and final solid products
Found
Calc.
Mn(mef)2·3H2O
60–240
120 endo
9.0
9.17
Mn(mef)2
240–740
320,600 exo
78.0
77.68
Mn2O3
740–900
860 exo
1.0
1.80
Mn3O4
Co(mef)2·2H2O
60–110
100 endo
3.0
3.13
Co(mef)2·H2O
130–240
-
3.0
3.13
Co(mef)2
250–520
340 endo470 exo
73.0
73.07
CoCO3
530–660
570 exo
7.0
6.72
Co3O4
>900
920 exo
1.0
0.93
CoO
Ni(mef)2·2H2O
50–180
80 endo
6.5
6.30
Ni(mef)2
190–460
340, 430 exo
73.0
73.10
NiCO3
460–550
490 exo
8.5
9.0
NiO+Ni
550–750
570 exo
1.5[a]
1.39[a]
NiO
Cu(mef)2·2H2O
100–180
150 endo
6.5
6.66
Cu(mef)2
190–840
550, 640 exo
80.0
80.08
CuO
Zn(mef)2·2H2O
100–160
130 endo
3.0
3.10
Zn(mef)2·H2O
160–190
180 endo
3.0
3.10
Zn(mef)2
200–490
420 exo
72,0
72.26
ZnCO3
490–640
510 endo, 580 exo
8.0
7.56
ZnO
Cd(mef)2·2H2O
110–160
150 endo
6.0
5.73
Cd(mef)2
210–380
300 endo,340 exo
67.0
66.86
CdCO3
470–760
550 exo
7.0
6.59
CdO
[
a
] Mass increase on TG curve.Figure 2
Thermoanalytical curves of Cd(mef)2·2H2O in air, sample mass 7,407 mg.Figure 3
X-ray powder diffraction patterns of decomposition products of Co(mef)2·2H2O heated up to 660°C.Mn(mef)2·3H2O and Cu(mef)2·2H2O decompose in a similar way. One-step dehydration takes place at 60–240°C and 100–180°C for Mn(II) and Cu(II) complex, respectively. Further increase of temperature results in high mass loss (ca. 80%) caused by mefenamic ligand decomposition and Mn3O4 (via Mn2O3) and CuO formation. The lowest thermal stability was determined for Ni(II) complex. Its decomposition starts at 50°C with 6,5% mass loss related to water molecules elimination. In the following step, the anhydrous compound decomposes (190–460°C) to NiCO3. This step is represented as two distinct exothermic peaks at 340°C and 430°C on the DTA curve. Further heating leads to formation of intermediate equimolar mixture of NiO and Ni, which subsequently is fully oxided to nickel oxide (mass increase on the TG curve). Presence of NiO was confirmed by powder X-ray diffraction of sinters prepared by heating compound to 750°C. The highest thermal stability is shown by Cd(II) complex. Its pyrolysis pattern closely resembles that of Ni(II) complex. Dehydration is single-step process and started at 110°C. The next mass loss (210–380°C) as observed on TG curve corresponds to destruction of organic ligand and leads to formation of CdCO3. The latter is associated with endo- and exothermic effects as represented by two distinct DTA peaks at 300 and 340°C, respectively. Further weight loss is observed at 470–760°C and results from the CdO formation (maximum on DTA curves at 550°C).


### 3.3. TG-MS Measurement

Conventional thermoanalytic studies such as TG/DTA often do not allow for unequivocal identification of gaseous products. For this reason, the TG/MS techniques were employed to characterize products of dynamic decomposition and fragmentation of Mn(mef)2·3H2O and Co(mef)2·2H2O. The determination was carried out under an argon atmosphere. Them/z values are given for 1H, 12C, 14N, and 16O. Figure 4 presents some profiles of ion current detected by mass spectrometer as a function of time for Co(II) complex. MS peaks of ion fragments corresponding to H2+, C+, CH3+ OH+, H2O+, C2H2+, HCN+, N2+, C2H5+, NO+, CO2+, 13C16O2+, 13C16O18O+ (m/z = 1, 12, 15, 17, 18, 26, 27, 28, 29, 30, 44, 45, 46) are monitored. Recorded data clearly indicated that all investigated complexes decompose progressively. For Mn(II) complex maxima of ion current intensities were observed for temperature ranges 120–280°C, 270–450°C, and 600–900°C.Figure 4
TG and corresponding MS analysis of Co(mef)2·2H2O (where: (1)m/z = 12; (2)m/z = 15; (3)m/z = 18; (4)m/z = 44; (5) TG).The peaks from H2O+ and H2+ observed at 110 and 120°C are related to dehydration of complex. Subsequently, fragmentation of organic ligand occurred within the 120–180°C temperature range. The following molecular ions were detected (respective temperature maxima are given in parentheses): C3H7+ (160°C), CH3+ (150°C), C2H2+ (170°C), C2H5+ (165°C), C+ (210°C), CO2+ (215°C), 13C16O2+ (180°), (HCN+, N2+). Three major temperature ranges of gaseous products emissions 120–230°C, 230–400°C, and 500–900°C were recorded for Co(mef)2·2H2O. In the first area, CH3+, C2H5+, C2H2+ ions were detected (all maxima at 160°C). The second is related to C+, CO2+ including combination of isotopes (ca. 300°C) while the third range corresponds to C+, CH3+, C2H5+, and CO2+ ions.


### 3.4. TG-FTIR Measurement

The coupled TG-FTIR technique was applied to Cd(mef)2·2H2O, Cu(mef)2·2H2O, and Zn(mef)2·2H2O complexes. All experiments were performed in argon atmosphere. The IR spectra were recorded using the Gramm-Schmidt curves. The respective stacked plot as registered for Cd(mef)2·2H2O is given in Figure 5.Figure 5
The stacked plot TG-FTIR spectra of the evolved gases for Cd(mef)2·2H2O.Analysis of IR spectra of gases evolved during the thermal decomposition indicates that pyrolysis schemes of all investigated complexes are similar and closely related to those recorded in air atmosphere. All spectra clearly confirm that the thermal decomposition begins from the dehydration process. On the TG curve in range 100–160°C for Cd(mef)2·2H2O and Cu(mef)2·2H2O and 100–190°C for Zn(mef)2·2H2Oca.6% mass losses connected with water losing were observed. The IR spectra which recorded up to 120°C for Cd(II) and Cu(II) complexes and up to 150°C for Zn(II) complex show bands in the wavenumbers 3750–3500 and 1750–1400 cm−1 corresponding to stretching and deformation vibrations of liberating water molecules. Anhydrous complexes are stable up to about 170°C which is confirmed by the lack of IR spectra of gaseous products. Further heating leads to organic ligand degradation indicated by a significant mass loss observed on the TG curve. The spectra recorded at 260°C contain bands in frequencies ranging 3000–2600 cm−1 (assigned to the stretching vibrations of the CH bond from the CH3 and CH2 groups); 1450–1350 cm−1 (corresponding to bending vibrations of the CH in the CH3 and CH2 groups); 1225–1000 cm−1 and 900–720 cm−1 (from bending vibration of CH in aromatic ring). Additionally, this spectrum shows the trace of water molecules in split of organic ligand destruction (tied in with NH vibration). Spectra which recorded up to 290°C contain the same patterns as described above augmented by additional bands (in the range 2500–2250 cm−1 and 750–650 cm−1) corresponding to CO2 vibrations and trace CO oscillations (2250–2050 cm−1). Heating the sample above 450°C resulted in rising intensity of bands related to carbon oxides while in the same time decreasing those of water and complete absence of aromatic ring vibrations.


## 3.1. FTIR Spectra

The IR spectra of all complexes exhibit a broad absorption band in the water stretching region (3300–3600 cm−1). Additionally, bands related to the water bending vibrations are observed (1615–1620 cm−1). In all spectra the valence vibrations of monodissociated carboxylic group are not observed. On the contrary, asymmetric (1575–1578 cm−1) and symmetric (1386–1394 cm−1) vibration of dissociated OCO- group are clearly observed (Table 2). These bands are affected by the coordination of mefenamic ligand to metal ions. The separation Δν=νas(OCO)-νs(OCO) and the direction of the shifts of these bands in comparison to those values of sodium salt characterized the nature of the metal–carboxylate bonds. The bathochromic shifts of asymmetric (νas) and hypsochromic shifts of symmetric (νs) frequencies are also observed. The magnitude of separation and the bands direction show that carboxylate group of mefenamic ligand coordinated in bidentate chelate mode [26].Table 2
Principal IR bands (cm−1) for carboxylate group in investigated complexes.
Compound
ν
a
s
y
m
ν
s
y
m
Δ
ν
=
ν
a
s
y
m
-
ν
s
y
m
Na(mef)
1580,0
1380,0
200,0
Mn(mef)2·3H2O
1577,7
1393,6
184,1
Co(mef)2·2H2O
1577,7
1392,5
185,2
Ni(mef)2·2H2O
1577,7
1390,6
187,1
Cu(mef)2·2H2O
1577,7
1392,5
185,2
Zn(mef)2·2H2O
1575,7
1386,7
189,0
Cd(mef)2·2H2O
1575,7
1396,4
178,7Apart from carboxylate group the mefenamic anion has amine group, available for coordination. The NH deformation vibrations in the IR spectra of mefenamic acid are very close to those observed in the IR spectra of its complexes. That indicates that the NH group does not participate directly in coordination.


## 3.2. Thermal Analysis

The data obtained from TG, DTG, and DTA curves supported by chemical and X-ray diffraction pattern investigations are collected in Table3. The thermal decomposition curves of Cd(mef)2·2H2O are shown on Figure 2. The thermal decomposition of the complexes is a multistages process. All compounds started to decompose by dehydration accompanied by the endothermic effect. Majority of complexes lose their water molecules in one step. Only for Co(II) and Zn(II) complexes water elimination is two-stage transformation. Thermolyses of these complexes are quite similar. The two-stage dehydration (60–110°C, 130–240°C and 100–160°C, 160–190°C for Co(II) and Zn(II) compound, respectively) is followed by organic ligand thermodestruction and metal carbonate formation. Further heating leads to metal oxides: ZnO and CoO. The latter is obtained via Co3O4 intermediate. In the terminal step of pyrolysis the DTA curve exhibits exoeffects. Formation of oxides was confirmed by the powder X-ray diffraction technique (Figure 3).Table 3
Thermal decomposition data of complexes in air.
Compounds
Ranges of decomp., °C
DTA peaks, °C
Mass loss, %
Intermediate and final solid products
Found
Calc.
Mn(mef)2·3H2O
60–240
120 endo
9.0
9.17
Mn(mef)2
240–740
320,600 exo
78.0
77.68
Mn2O3
740–900
860 exo
1.0
1.80
Mn3O4
Co(mef)2·2H2O
60–110
100 endo
3.0
3.13
Co(mef)2·H2O
130–240
-
3.0
3.13
Co(mef)2
250–520
340 endo470 exo
73.0
73.07
CoCO3
530–660
570 exo
7.0
6.72
Co3O4
>900
920 exo
1.0
0.93
CoO
Ni(mef)2·2H2O
50–180
80 endo
6.5
6.30
Ni(mef)2
190–460
340, 430 exo
73.0
73.10
NiCO3
460–550
490 exo
8.5
9.0
NiO+Ni
550–750
570 exo
1.5[a]
1.39[a]
NiO
Cu(mef)2·2H2O
100–180
150 endo
6.5
6.66
Cu(mef)2
190–840
550, 640 exo
80.0
80.08
CuO
Zn(mef)2·2H2O
100–160
130 endo
3.0
3.10
Zn(mef)2·H2O
160–190
180 endo
3.0
3.10
Zn(mef)2
200–490
420 exo
72,0
72.26
ZnCO3
490–640
510 endo, 580 exo
8.0
7.56
ZnO
Cd(mef)2·2H2O
110–160
150 endo
6.0
5.73
Cd(mef)2
210–380
300 endo,340 exo
67.0
66.86
CdCO3
470–760
550 exo
7.0
6.59
CdO
[
a
] Mass increase on TG curve.Figure 2
Thermoanalytical curves of Cd(mef)2·2H2O in air, sample mass 7,407 mg.Figure 3
X-ray powder diffraction patterns of decomposition products of Co(mef)2·2H2O heated up to 660°C.Mn(mef)2·3H2O and Cu(mef)2·2H2O decompose in a similar way. One-step dehydration takes place at 60–240°C and 100–180°C for Mn(II) and Cu(II) complex, respectively. Further increase of temperature results in high mass loss (ca. 80%) caused by mefenamic ligand decomposition and Mn3O4 (via Mn2O3) and CuO formation. The lowest thermal stability was determined for Ni(II) complex. Its decomposition starts at 50°C with 6,5% mass loss related to water molecules elimination. In the following step, the anhydrous compound decomposes (190–460°C) to NiCO3. This step is represented as two distinct exothermic peaks at 340°C and 430°C on the DTA curve. Further heating leads to formation of intermediate equimolar mixture of NiO and Ni, which subsequently is fully oxided to nickel oxide (mass increase on the TG curve). Presence of NiO was confirmed by powder X-ray diffraction of sinters prepared by heating compound to 750°C. The highest thermal stability is shown by Cd(II) complex. Its pyrolysis pattern closely resembles that of Ni(II) complex. Dehydration is single-step process and started at 110°C. The next mass loss (210–380°C) as observed on TG curve corresponds to destruction of organic ligand and leads to formation of CdCO3. The latter is associated with endo- and exothermic effects as represented by two distinct DTA peaks at 300 and 340°C, respectively. Further weight loss is observed at 470–760°C and results from the CdO formation (maximum on DTA curves at 550°C).


## 3.3. TG-MS Measurement

Conventional thermoanalytic studies such as TG/DTA often do not allow for unequivocal identification of gaseous products. For this reason, the TG/MS techniques were employed to characterize products of dynamic decomposition and fragmentation of Mn(mef)2·3H2O and Co(mef)2·2H2O. The determination was carried out under an argon atmosphere. Them/z values are given for 1H, 12C, 14N, and 16O. Figure 4 presents some profiles of ion current detected by mass spectrometer as a function of time for Co(II) complex. MS peaks of ion fragments corresponding to H2+, C+, CH3+ OH+, H2O+, C2H2+, HCN+, N2+, C2H5+, NO+, CO2+, 13C16O2+, 13C16O18O+ (m/z = 1, 12, 15, 17, 18, 26, 27, 28, 29, 30, 44, 45, 46) are monitored. Recorded data clearly indicated that all investigated complexes decompose progressively. For Mn(II) complex maxima of ion current intensities were observed for temperature ranges 120–280°C, 270–450°C, and 600–900°C.Figure 4
TG and corresponding MS analysis of Co(mef)2·2H2O (where: (1)m/z = 12; (2)m/z = 15; (3)m/z = 18; (4)m/z = 44; (5) TG).The peaks from H2O+ and H2+ observed at 110 and 120°C are related to dehydration of complex. Subsequently, fragmentation of organic ligand occurred within the 120–180°C temperature range. The following molecular ions were detected (respective temperature maxima are given in parentheses): C3H7+ (160°C), CH3+ (150°C), C2H2+ (170°C), C2H5+ (165°C), C+ (210°C), CO2+ (215°C), 13C16O2+ (180°), (HCN+, N2+). Three major temperature ranges of gaseous products emissions 120–230°C, 230–400°C, and 500–900°C were recorded for Co(mef)2·2H2O. In the first area, CH3+, C2H5+, C2H2+ ions were detected (all maxima at 160°C). The second is related to C+, CO2+ including combination of isotopes (ca. 300°C) while the third range corresponds to C+, CH3+, C2H5+, and CO2+ ions.


## 3.4. TG-FTIR Measurement

The coupled TG-FTIR technique was applied to Cd(mef)2·2H2O, Cu(mef)2·2H2O, and Zn(mef)2·2H2O complexes. All experiments were performed in argon atmosphere. The IR spectra were recorded using the Gramm-Schmidt curves. The respective stacked plot as registered for Cd(mef)2·2H2O is given in Figure 5.Figure 5
The stacked plot TG-FTIR spectra of the evolved gases for Cd(mef)2·2H2O.Analysis of IR spectra of gases evolved during the thermal decomposition indicates that pyrolysis schemes of all investigated complexes are similar and closely related to those recorded in air atmosphere. All spectra clearly confirm that the thermal decomposition begins from the dehydration process. On the TG curve in range 100–160°C for Cd(mef)2·2H2O and Cu(mef)2·2H2O and 100–190°C for Zn(mef)2·2H2Oca.6% mass losses connected with water losing were observed. The IR spectra which recorded up to 120°C for Cd(II) and Cu(II) complexes and up to 150°C for Zn(II) complex show bands in the wavenumbers 3750–3500 and 1750–1400 cm−1 corresponding to stretching and deformation vibrations of liberating water molecules. Anhydrous complexes are stable up to about 170°C which is confirmed by the lack of IR spectra of gaseous products. Further heating leads to organic ligand degradation indicated by a significant mass loss observed on the TG curve. The spectra recorded at 260°C contain bands in frequencies ranging 3000–2600 cm−1 (assigned to the stretching vibrations of the CH bond from the CH3 and CH2 groups); 1450–1350 cm−1 (corresponding to bending vibrations of the CH in the CH3 and CH2 groups); 1225–1000 cm−1 and 900–720 cm−1 (from bending vibration of CH in aromatic ring). Additionally, this spectrum shows the trace of water molecules in split of organic ligand destruction (tied in with NH vibration). Spectra which recorded up to 290°C contain the same patterns as described above augmented by additional bands (in the range 2500–2250 cm−1 and 750–650 cm−1) corresponding to CO2 vibrations and trace CO oscillations (2250–2050 cm−1). Heating the sample above 450°C resulted in rising intensity of bands related to carbon oxides while in the same time decreasing those of water and complete absence of aromatic ring vibrations.


## 4. Conclusions

All investigated complexes have been obtained as crystalline hydrates. Majority of synthesized compounds in MeOH, DMSO, and DMF solutions do not dissociate or dissociate only in a very limited degree. IR spectra firmly confirmed that mefenamic ligands are directly coordinated to metal ions only through carboxylate group, in a bidentate chelate mode. According to the chemical, spectroscopic, and thermal data, we have proposed the formula of obtained complexes (Figure6).Figure 6
Proposed formula of the mefenamic-metal complexes.All compounds decompose progressively starting with dehydration at the temperature range 60–150°C. Anhydrous compounds are stable up to almost 170°C. The most temperature persistence is Cd(II) complex, while the least one is the Ni(II) compound. Results of the TG-MS and TG-FTIR investigations correlate closely with those obtained by the TG-DTG system. The differences are related to final products and paths of dehydration.



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*Source: 6172626-2017-12-18.xml*