# Thermal Degradation Behaviour of Ni(II) Complex of 3,4-Methylenedioxaphenylaminoglyoxime

Authors: Emin Karapınar; Ilkay Hilal Gubbuk; Bilge Taner; Pervin Deveci; Emine Ozcan
Journal: Journal of Chemistry
 (2013)

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## Abstract

Thermal degradation behaviour of the Ni(II) complex of 3,4-methylenedioxaphenylaminoglyoxime was investigated by TG, DTA, and DTG at a heating rate of 10°C min−1 under dinitrogen. The acquired experimental data shows that the complex is thermally stable up to 541 K. The pyrolytic decomposition process occurs by melting metal complex and metal oxide remains as final product. The energies of the reactions involved and the mechanism of decomposition at each stage have been examined. The values of kinetic parameters such as activation energy (E), preexponential factor (A) and thermodynamic parameters such as enthalpy (ΔH), entropy (ΔS), and Gibbs free energy (ΔG) are also evaluated.


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## Body

## 1. Introduction

vic-Dioximes have attracted extensive attention for many years due to their interesting structural diversity and various potential applications in different areas. Their synthesis, characterization, spectroscopic properties, and reactivity have been the subject of many papers because of their rich physicochemical properties, reactivity patterns, and potential applications in many important chemical processes in the areas such as medicine [1], bioorganic systems [2], catalysis [3], and liquid crystals [4]. Transition metal complexes of vic-dioxime ligands have been widely investigated as analytical reagents as models for biological systems like vitamin B12 [5, 6].Thermal behaviour of the transition metal derivatives with azomethines (Schiff bases, hydrazones, and oximes) is very important for the researcher in various branches of theoretical and technical chemistry [7–9]. The well-established thermogravimetric analysis (TG), derivative thermogravimetric analysis (DTG), differential thermal analysis (DTA), and derivative thermogravimetric scanning calorimetry (DSC) techniques have been reliably and widely used over many decades in studying thermal behaviour and properties of various types of materials and evaluating the thermal parameters for their degradation processes [10, 11]. The thermal analysis of the compound gives information about its stability and suggests a decomposition pathway. Therefore, kinetic studies have become a crucial point in thermal analysis, in which the main purpose is to determine the mechanism(s) of pyrolysis reaction and to calculate the parameters of the Arrhenius equation.The aims of this research are to study the chemical steps of the investigated degradation and the evaluation of the kinetic and thermodynamic parameters by using (Coats-Redfern) CR, (Horowitz-Metzger) HM, (Van Krevelen) VK, (Broido) B, and (Madhusudanan-Krishnan-Ninan) MKN methods for each step and to obtain degradation kinetics data.


## 2. Experimental

All the reagents purchased from Merck, Fluka, or Sigma and materials were chemically pure. Thevic-dioxime complex was synthesized from analytical pure reagents as described in the literature [12]. Elemental analysis (C, H, and N) was performed on a LECO-932 CHNSO apparatus. The IR spectra were recorded with a Perkin Elmer Model 1605 FT-IR spectrophotometer from KBr pellets. 1H NMR and 13C NMR spectra were recorded on Bruker GmbH Dpx-400 MHz high-performance digital FT-NMR spectrometers in DMSO-d6. The thermal measurements were carried out on a Perkin Elmer SII-Diamond TG-DTA Instruments thermal analysis system in dinitrogen atmospheres, applying a heating rate of 10°C min−1 in a temperature range of 313–1173 K. Sample mass was 2.675 mg.


## 3. Results and Discussion

### 3.1. Elemental Analysis, IR,1H NMR, and 13C NMR Spectra

The structure of 3,4 methylenedioxaphenylaminoglyoxime (HL) and Ni(II) complex of this ligand (Ni(HL)2) are shown in Figure 1.HL and Ni(HL)2 were characterized by elemental analysis, IR, 1H NMR, and 13C NMR spectra [11]. 1H NMR and 13C NMR spectra of Ni(HL)2 are given in Figures 2(a) and 2(b).Figure 1
Presentation ofHL,  Ni(HL)2.(a)1H NMR spectra of the Ni(HL)2; (b) 13C NMR spectra of Ni(HL)2.
(a)
(b)The elemental analyses ofHL and Ni(HL)2 were in agreement with theoretical expectations as given in the literature [12]. In the FTIR spectra of vic-dioxime complexes, the most important absorption bands that belong to the various vibration frequencies of the oxime groups are νOH: 3368–3398 cm−1 (broad band), νC=N: 1610–1640 cm−1, and νN–O: 960–970 cm−1 (a single band). The 1H and 13C NMR spectra were obtained in DMSO for the complex. In the 1H NMR spectra of Ni(HL)2, the proton resonance signal of the intermolecular hydrogen bridge appeared at 14.6 ppm, and the chemical shifts belonging to free OH protons (around 10 ppm) were not observed. In the 13C NMR spectra, quaternary carbon signals of hydroximino carbon atom (C=N–O) appeared at around 147 ppm (Figures 2(a) and 2(b)).


### 3.2. Thermal Behaviours of the Metal Complex

In the present study, thermal behaviour of theNi(HL)2 was studied with TG, DTA, and DTG techniques. Figure 3 shows TG, DTA, and DTG curves of the complex.Figure 3
TG/DTA/DTG plots forNi(HL)2 complex.From the thermogram, it can be observed that a three-step thermal degradation process exists forNi(HL)2. The thermal degradation for Ni(HL)2 is shown in Scheme 1.Scheme 1
The thermal degradation forNi(HL)2.For this complex, the first stage of degradation began at 541 K and terminated in 581 K, and the observed mass loss was 44.58%, which corresponds to the loss of CH2O2C6H3NHCN, and 2OH, NO molecules. The second stage of degradation, between 612 and 857 K, resulted in 29.98% weight loss. The third stage of degradation occurred in temperature range of 889–1078 K. In last two stages, CH2O2C6H3NCH and 2CHN molecules were lost from the complex, respectively. The stages of degradation were summarized in Table 1.Table 1
The temperature rangeT/K and weight loss values of the degradation stages for the Ni(HL)2.
Compound
Stage
T/K
Evolved moieties
Weight loss (%)
Found
Calc.
RE (%)
Ni(HL)2
1st
541–581
CH2O2C6H3NHCN, 2OH, NO
44.58
44.96
0.85
2nd
612–857
CH2O2C6H3NCH
29.98
29.44
1.83
3rd
889–1078
2CHN
9.97
10.74
7.1
Residue
>1079
NiO
15.42
14.72
4.75
RE(%): % relative error.It can be seen clearly (Table1) that the mass losses obtained from the TG curves and that calculated for the corresponding molecule or molecules and final decomposition product (i.e., final residue) are in good agreement for all of the decomposition steps. Thermal degradation studies of the Ni(HL)2 indicated that this complex was thermally stable up to 541 K and continues degrading up to 1079 K. The initial mass loss is seen to occur at 541 K, and decomposition is seen to end with 85.28% mass loss at 1078 K with a greenish-black coloured solid (NiO) in the TG curves. Degradation of this complex occurs in three stages and in harmony with the literature [13, 14].The inflation of the t.g.a. curves of the complex at a temperature below 900°C indicates the decomposition of the fully organic part of the chelate, leaving the metallic oxide at the final temperature [13, 14].


### 3.3. Kinetic Studies

In order to determine kinetic parameters in a solid-state degradation reaction, usually several equations [15–17] have been proposed as means of analyzing a TG curve. In the kinetic studies of the thermal systems, the mass-temperature relation, which can determine the behaviour of the degradation reactions, can be examined. In the present study, five equations such as HM [18], CR [19], VK [20], B [21], and MKN [22] were used for calculating the activation energy (E), preexponential factor (A), and thermodynamic parameters (ΔG, ΔH, and ΔS). The kinetics was studied for all the three stages of degradation of the complex. The degree of conversion, α, is defined as the ratio of actual weight loss to total weight loss. α is calculated according to
(1)α=W0-WW0-Wf,
where W0 is the initial mass of the sample (g), W is the mass of the sample (g) at a time and at temperature T (K), and Wf is the final mass of the sample (g). The rate of degradation process can be described as the product of two separate functions of temperature and fractional conversion [23]:
(2)dαdt=k(T)f(α),
where α is the fraction decomposed at time t, k(T) is the temperature dependent function, and f(α) is the conversion function dependent on the mechanism of degradation:
(3)k(T)=Aexp(-ERT),f(α)=(1-α)n.
Then,
(4)dαdt=Aexp(-ERT)(1-α)n.According toHorowitz-Metzger method [18] for n=1 (n is the reaction order),
(5)log[g(α)]=Eθ2.303RTm2.
Here, R is the gas constant and θ=T-Tm, where Tm is the temperature of maximum reaction rate and T is the temperature in Kelvin at any instant. A plot of log[g(α)] versus θ (Figure 4) should give a straight line whose slope is E/RTm2 [24]. g(α)=-ln(1-α) indicates random nucleation model for the degradation of the material. The preexponential factor (A) is calculated by using (6):
(6)A=ERTm2βexp(ERTm).
Here, β is the heating rate (K min−1).Figure 4
Graphical presentation of thelog[g(α)]-θ plot of HM equation Ni(HL)2.According toCoats-Redfern method [19],
(7)log[g(α)T2]=log[ARβE(1-2RTE)]-E2.303RT.
Plot of log[g(α)/T2] versus 1/T (Figure 5) gives the slope for evaluation of E and the intercept of A.Figure 5
Graphical presentation of thelog[g(α)/T2]-1/T plot of CR equation of Ni(HL)2.According to theVan Krevelen [20] method,
(8)ln[g(α)]=ln[Aβ(0.368Tm)E/RTm(ERTm+1)-1]+(ERTm+1)lnT.A typical curve oflog[g(α)] versus lnT for the nickel(II) complex is shown in Figure 6. The activation energies calculated from the slopes of degradation for metal complex are listed in Table 2.Table 2
Kinetic parameters of Ni(HL)2 determined using the CR, HM, B, MKN, and VK equations.
Complex
Stage
Method
Parameter
E (J mol−1)
A (s−1)
Δ
S (J mol−1 K−1)
Δ
H (kJ mol−1)
Δ
G (kJ mol−1)
Ni(HL)2
1st
CR
2.95 × 105
3.58 × 1026
2.58 × 102
2.90 × 105
1.43 × 105
HM
3.01 × 105
6.43 × 1026
2.62 × 102
2.96 × 105
1.47 × 105
B
3.04 × 105
1.54 × 1012
2.33
2.99 × 105
2.98 × 105
VK
3.03 × 105
5.48 × 1030
3.38 × 102
2.98 × 105
1.10 × 105
MKN
2.95 × 105
4.60 × 1028
2.98 × 102
2.90 × 105
1.24 × 105
2nd
CR
4.01 × 105
3.81 × 10
−2.40 × 102
3.42 × 104
1.72 × 105
HM
4.87 × 105
5.23 × 102
−2.19 × 102
4.23 × 104
1.58 × 105
B
5.22 × 104
4.12 × 10
−2.21 × 102
4.63 × 104
2.01 × 105
VK
5.06 × 104
3.73 × 105
−1.45 × 102
4.48 × 104
1.46 × 105
MKN
4.05 × 104
2.98 × 103
−1.85 × 102
3.47 × 104
1.65 × 105
3rd
CR
1.04 × 105
4.35 × 104
−1.66 × 102
9.57 × 104
1.76 × 105
HM
1.24 × 105
4.75 × 104
−1.65 × 102
1.16 × 105
1.77 × 105
B
1.20 × 105
6.32 × 102
−2.01 × 102
1.11 × 105
3.13 × 105
VK
1.24 × 105
7.23 × 108
−8.5 × 10
1.16 × 105
2.01 × 105
MKN
1.04 × 105
1.20 × 106
−1.39 × 102
9.62 × 104
2.35 × 105Figure 6
Graphical presentation of theln[g(α)]-lnT plot of VK equation of Ni(HL)2.The mathematical expression ofBroido’s  [21] method is
(9)ln[g(α)]=ln[Aβ(RE)Tm2]-(ER)x1T.E can be calculated from the plot of log[g(α)] versus 1/T (Figure 7).Figure 7
Graphical presentation of thelog[g(α)]-1/T plot of B equation of Ni(HL)2.The final method of calculation ofE is developed by Madhusudanan-Krishnan-Ninan. According to the MKNequation [22] method,
(10)ln[g(α)T1.921503]=[lnAEβR+0.3772050-1.921503lnE]-0.1200394(ET).According to this method, the plot ofln[g(α)/T1.921503] versus 1/T gives straight lines (Figure 8), and E and A can be calculated from the slope and intercept, respectively.Figure 8
Graphical presentation of theln[g(α)/T1.921503]-1/T plot of MKN equation of Ni(HL)2.The values obtained forE and A of Ni(HL)2 for each three stages have been calculated and are shown in Table 2.The entropy of activationΔS is calculated by using
(11)ΔS=Rln(AhkTm),
where k is the Boltzmann constant and h is the Planck constant. The activation enthalpy, ΔH, and Gibbs free energy, ΔG, are calculated from (12):
(12)ΔH=E-RT,ΔG=ΔH-TΔS.High activation energy values were calculated at the appropriate linear regions of the temperature range by using five methods and were given in Table2. The high E values indicate that the ligand is strongly bonded to the Ni(II) ions [25]. The activation energy is obtained at nearly the same value for three steps because of the structures of the evolved moieties.In the 1st stage, entropy was found to be positive. So, the activated complex can be thought to own less ordered structures than the reactant [10]. The negative values of entropy in the 2nd and 3rd steps indicate that the reactions were slower than normal. The negative values of ΔS are due to low A values and account for the nonspontaneous nature of the reaction [26]. The nonspontaneous nature of the degradation reactions of the complex was supported by the positive value of ΔG in the degradation steps [25]. The enthalpy was found to be positive value, and it was partially decreased with increase in temperature. The positive value of ΔH at a particular temperature indicated that the process was of endothermic nature. The high heat of degradation released during the processes might have masked the endothermicity of degradation reaction [17].In general, it can be concluded that it is possible to obtain Ni(HL)2  with in thermal stability and more applicable from the economic viewpoint.


## 3.1. Elemental Analysis, IR,1H NMR, and 13C NMR Spectra

The structure of 3,4 methylenedioxaphenylaminoglyoxime (HL) and Ni(II) complex of this ligand (Ni(HL)2) are shown in Figure 1.HL and Ni(HL)2 were characterized by elemental analysis, IR, 1H NMR, and 13C NMR spectra [11]. 1H NMR and 13C NMR spectra of Ni(HL)2 are given in Figures 2(a) and 2(b).Figure 1
Presentation ofHL,  Ni(HL)2.(a)1H NMR spectra of the Ni(HL)2; (b) 13C NMR spectra of Ni(HL)2.
(a)
(b)The elemental analyses ofHL and Ni(HL)2 were in agreement with theoretical expectations as given in the literature [12]. In the FTIR spectra of vic-dioxime complexes, the most important absorption bands that belong to the various vibration frequencies of the oxime groups are νOH: 3368–3398 cm−1 (broad band), νC=N: 1610–1640 cm−1, and νN–O: 960–970 cm−1 (a single band). The 1H and 13C NMR spectra were obtained in DMSO for the complex. In the 1H NMR spectra of Ni(HL)2, the proton resonance signal of the intermolecular hydrogen bridge appeared at 14.6 ppm, and the chemical shifts belonging to free OH protons (around 10 ppm) were not observed. In the 13C NMR spectra, quaternary carbon signals of hydroximino carbon atom (C=N–O) appeared at around 147 ppm (Figures 2(a) and 2(b)).


## 3.2. Thermal Behaviours of the Metal Complex

In the present study, thermal behaviour of theNi(HL)2 was studied with TG, DTA, and DTG techniques. Figure 3 shows TG, DTA, and DTG curves of the complex.Figure 3
TG/DTA/DTG plots forNi(HL)2 complex.From the thermogram, it can be observed that a three-step thermal degradation process exists forNi(HL)2. The thermal degradation for Ni(HL)2 is shown in Scheme 1.Scheme 1
The thermal degradation forNi(HL)2.For this complex, the first stage of degradation began at 541 K and terminated in 581 K, and the observed mass loss was 44.58%, which corresponds to the loss of CH2O2C6H3NHCN, and 2OH, NO molecules. The second stage of degradation, between 612 and 857 K, resulted in 29.98% weight loss. The third stage of degradation occurred in temperature range of 889–1078 K. In last two stages, CH2O2C6H3NCH and 2CHN molecules were lost from the complex, respectively. The stages of degradation were summarized in Table 1.Table 1
The temperature rangeT/K and weight loss values of the degradation stages for the Ni(HL)2.
Compound
Stage
T/K
Evolved moieties
Weight loss (%)
Found
Calc.
RE (%)
Ni(HL)2
1st
541–581
CH2O2C6H3NHCN, 2OH, NO
44.58
44.96
0.85
2nd
612–857
CH2O2C6H3NCH
29.98
29.44
1.83
3rd
889–1078
2CHN
9.97
10.74
7.1
Residue
>1079
NiO
15.42
14.72
4.75
RE(%): % relative error.It can be seen clearly (Table1) that the mass losses obtained from the TG curves and that calculated for the corresponding molecule or molecules and final decomposition product (i.e., final residue) are in good agreement for all of the decomposition steps. Thermal degradation studies of the Ni(HL)2 indicated that this complex was thermally stable up to 541 K and continues degrading up to 1079 K. The initial mass loss is seen to occur at 541 K, and decomposition is seen to end with 85.28% mass loss at 1078 K with a greenish-black coloured solid (NiO) in the TG curves. Degradation of this complex occurs in three stages and in harmony with the literature [13, 14].The inflation of the t.g.a. curves of the complex at a temperature below 900°C indicates the decomposition of the fully organic part of the chelate, leaving the metallic oxide at the final temperature [13, 14].


## 3.3. Kinetic Studies

In order to determine kinetic parameters in a solid-state degradation reaction, usually several equations [15–17] have been proposed as means of analyzing a TG curve. In the kinetic studies of the thermal systems, the mass-temperature relation, which can determine the behaviour of the degradation reactions, can be examined. In the present study, five equations such as HM [18], CR [19], VK [20], B [21], and MKN [22] were used for calculating the activation energy (E), preexponential factor (A), and thermodynamic parameters (ΔG, ΔH, and ΔS). The kinetics was studied for all the three stages of degradation of the complex. The degree of conversion, α, is defined as the ratio of actual weight loss to total weight loss. α is calculated according to
(1)α=W0-WW0-Wf,
where W0 is the initial mass of the sample (g), W is the mass of the sample (g) at a time and at temperature T (K), and Wf is the final mass of the sample (g). The rate of degradation process can be described as the product of two separate functions of temperature and fractional conversion [23]:
(2)dαdt=k(T)f(α),
where α is the fraction decomposed at time t, k(T) is the temperature dependent function, and f(α) is the conversion function dependent on the mechanism of degradation:
(3)k(T)=Aexp(-ERT),f(α)=(1-α)n.
Then,
(4)dαdt=Aexp(-ERT)(1-α)n.According toHorowitz-Metzger method [18] for n=1 (n is the reaction order),
(5)log[g(α)]=Eθ2.303RTm2.
Here, R is the gas constant and θ=T-Tm, where Tm is the temperature of maximum reaction rate and T is the temperature in Kelvin at any instant. A plot of log[g(α)] versus θ (Figure 4) should give a straight line whose slope is E/RTm2 [24]. g(α)=-ln(1-α) indicates random nucleation model for the degradation of the material. The preexponential factor (A) is calculated by using (6):
(6)A=ERTm2βexp(ERTm).
Here, β is the heating rate (K min−1).Figure 4
Graphical presentation of thelog[g(α)]-θ plot of HM equation Ni(HL)2.According toCoats-Redfern method [19],
(7)log[g(α)T2]=log[ARβE(1-2RTE)]-E2.303RT.
Plot of log[g(α)/T2] versus 1/T (Figure 5) gives the slope for evaluation of E and the intercept of A.Figure 5
Graphical presentation of thelog[g(α)/T2]-1/T plot of CR equation of Ni(HL)2.According to theVan Krevelen [20] method,
(8)ln[g(α)]=ln[Aβ(0.368Tm)E/RTm(ERTm+1)-1]+(ERTm+1)lnT.A typical curve oflog[g(α)] versus lnT for the nickel(II) complex is shown in Figure 6. The activation energies calculated from the slopes of degradation for metal complex are listed in Table 2.Table 2
Kinetic parameters of Ni(HL)2 determined using the CR, HM, B, MKN, and VK equations.
Complex
Stage
Method
Parameter
E (J mol−1)
A (s−1)
Δ
S (J mol−1 K−1)
Δ
H (kJ mol−1)
Δ
G (kJ mol−1)
Ni(HL)2
1st
CR
2.95 × 105
3.58 × 1026
2.58 × 102
2.90 × 105
1.43 × 105
HM
3.01 × 105
6.43 × 1026
2.62 × 102
2.96 × 105
1.47 × 105
B
3.04 × 105
1.54 × 1012
2.33
2.99 × 105
2.98 × 105
VK
3.03 × 105
5.48 × 1030
3.38 × 102
2.98 × 105
1.10 × 105
MKN
2.95 × 105
4.60 × 1028
2.98 × 102
2.90 × 105
1.24 × 105
2nd
CR
4.01 × 105
3.81 × 10
−2.40 × 102
3.42 × 104
1.72 × 105
HM
4.87 × 105
5.23 × 102
−2.19 × 102
4.23 × 104
1.58 × 105
B
5.22 × 104
4.12 × 10
−2.21 × 102
4.63 × 104
2.01 × 105
VK
5.06 × 104
3.73 × 105
−1.45 × 102
4.48 × 104
1.46 × 105
MKN
4.05 × 104
2.98 × 103
−1.85 × 102
3.47 × 104
1.65 × 105
3rd
CR
1.04 × 105
4.35 × 104
−1.66 × 102
9.57 × 104
1.76 × 105
HM
1.24 × 105
4.75 × 104
−1.65 × 102
1.16 × 105
1.77 × 105
B
1.20 × 105
6.32 × 102
−2.01 × 102
1.11 × 105
3.13 × 105
VK
1.24 × 105
7.23 × 108
−8.5 × 10
1.16 × 105
2.01 × 105
MKN
1.04 × 105
1.20 × 106
−1.39 × 102
9.62 × 104
2.35 × 105Figure 6
Graphical presentation of theln[g(α)]-lnT plot of VK equation of Ni(HL)2.The mathematical expression ofBroido’s  [21] method is
(9)ln[g(α)]=ln[Aβ(RE)Tm2]-(ER)x1T.E can be calculated from the plot of log[g(α)] versus 1/T (Figure 7).Figure 7
Graphical presentation of thelog[g(α)]-1/T plot of B equation of Ni(HL)2.The final method of calculation ofE is developed by Madhusudanan-Krishnan-Ninan. According to the MKNequation [22] method,
(10)ln[g(α)T1.921503]=[lnAEβR+0.3772050-1.921503lnE]-0.1200394(ET).According to this method, the plot ofln[g(α)/T1.921503] versus 1/T gives straight lines (Figure 8), and E and A can be calculated from the slope and intercept, respectively.Figure 8
Graphical presentation of theln[g(α)/T1.921503]-1/T plot of MKN equation of Ni(HL)2.The values obtained forE and A of Ni(HL)2 for each three stages have been calculated and are shown in Table 2.The entropy of activationΔS is calculated by using
(11)ΔS=Rln(AhkTm),
where k is the Boltzmann constant and h is the Planck constant. The activation enthalpy, ΔH, and Gibbs free energy, ΔG, are calculated from (12):
(12)ΔH=E-RT,ΔG=ΔH-TΔS.High activation energy values were calculated at the appropriate linear regions of the temperature range by using five methods and were given in Table2. The high E values indicate that the ligand is strongly bonded to the Ni(II) ions [25]. The activation energy is obtained at nearly the same value for three steps because of the structures of the evolved moieties.In the 1st stage, entropy was found to be positive. So, the activated complex can be thought to own less ordered structures than the reactant [10]. The negative values of entropy in the 2nd and 3rd steps indicate that the reactions were slower than normal. The negative values of ΔS are due to low A values and account for the nonspontaneous nature of the reaction [26]. The nonspontaneous nature of the degradation reactions of the complex was supported by the positive value of ΔG in the degradation steps [25]. The enthalpy was found to be positive value, and it was partially decreased with increase in temperature. The positive value of ΔH at a particular temperature indicated that the process was of endothermic nature. The high heat of degradation released during the processes might have masked the endothermicity of degradation reaction [17].In general, it can be concluded that it is possible to obtain Ni(HL)2  with in thermal stability and more applicable from the economic viewpoint.


## 4. Conclusions

The new complex,Ni(HL)2, was prepared for the first time, and it was presented in the literature [11]. The present work is the first ever report including the reaction mechanism of thermal decomposition and application of the theories, namely, CR, HM, VK, MKN, and B, for all the three stages of decomposition of the material. The TG curves show the mass decrease with the linear increase in temperature. The material released at each step of the decomposition was identified by attributing the mass loss (Δm) at a given step to the component of similar weight calculated from the molecular formula of the investigated complex by comparing that with works of literature of relevant compounds taking into account their temperature [15, 27]. The observed percentage of weight loss corresponding to various steps in the TG curves was compared with those calculated in the assumption of possible composition of the complex suggested from the elemental analysis and confirmed later from IR, 1H-NMR, and 13C-NMR spectral studies. This may assist by identifying the mechanism of reaction in the decomposition steps. Tables 1 and 2 give the characteristic thermal and kinetic parameters of each step in the decomposition sequence of the complex, determined or evaluated, from the TG curves.



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