Chromic Acid Oxidation of Methylaminopyrazole Formamidine in Sulfuric Acid Medium: A Kinetic and Mechanistic Approach
Ahmed Fawzy1, 2, *, Ismail Althagafi1, Fahd Tirkistani1, Mohamed Shaaban1, 3, Moataz Morad1
1Chemistry Department, Faculty of Applied Science, Umm Al-Qura University, Makkah, Saudi Arabia
2Chemistry Department, Faculty of Science, Assiut University, Assiut, Egypt
3Chemistry Department, Faculty of Science, Cairo University, Cairo, Egypt
To cite this article:
Ahmed Fawzy, Ismail Althagafi, Fahd Tirkistani, Mohamed Shaaban, Moataz Morad. Chromic Acid Oxidation of Methylaminopyrazole Formamidine in Sulfuric Acid Medium: A Kinetic and Mechanistic Approach. American Journal of Physical Chemistry. Vol. 5, No. 1, 2016, pp. 1-9. doi: 10.11648/j.ajpc.20160501.11
Abstract: The kinetics of chromic acid oxidation of one of aminopyrazole formamidine derivatives, namely N,N-dimethyl-N’-(5-methyl-1H-pyrazol-3-yl) formamidine (MAPF)in sulfuric acid solutions has been investigated at constant ionic strength and temperature. The progress of the reaction was followed spectrophotometrically. The reaction showed a first order dependence on [chromic acid] and fractional-first order dependences with respect to [MAPF] and [H+]. Increasing ionic strength and solvent polarity of the reaction medium had no significant effect on the oxidation rate. Addition of AgI, PdII and RuIII catalysts was found to enhance the reaction rate and the order of catalytic efficiency is: AgI > RuIII > PdII. The final oxidation products of MAPF are identified by spectral and elemental analysis as methylaminopyrazole, dimethylamine and carbon dioxide. A spectral evidence for the formation of chromium(III) product was obtained. A reaction mechanism adequately describing the observed kinetic behavior is proposed, and the reaction constants involved in the different steps of the mechanism have been evaluated. The activation parameters with respect to the rate-determining step of the reaction, along with thermodynamic quantities of the equilibrium constants, are presented and discussed.
Keywords: Kinetics, Mechanism, Oxidation, Chromic Acid, Methylaminopyrazole Formamidine
During the few last decades, formamidines have achieved considerable attention because they have a unique and fascinating biological activity including monoamine oxidase inhibitors [1, 2], adrenergic and neuro-chemical receptors [3, 4]. Extensive investigations of N,N-dialkyl derivatives of formamidines which are very effective acaricides leads to the discovery of the acaricide-insecticide chlordimeform. Furthermore, the oxidative cleavage of formamidine derivatives is important because it yields N,N-dialkyl formamidine group which has various biosynthetic applications.
Formamidines may play an important role in the chemistry of chromium, especially in the environment because of its mutagenic and carcinogenic activity. Chromium in aqueous solutions exists in both trivalent, CrIII, and hexavalent, CrVI, species. However, these two oxidation states are characterized by different physical/chemical behavior and toxicity. The compounds of chromium(VI) pose serious dangers to biological systems, whereas those of chromium(III) are relatively non-toxic . On the other hand, chromium(VI) is one of the most versatile available oxidizing agents for the oxidation of organic compounds. It can be reduced to lower oxidation states by various biological and chemical reductants . The chemistry of the intermediate oxidation states of chromium, CrV and CrIV, which observed during the oxidation of organic substrates by chromium(VI) was attracted many researchers because of their implication in the mechanism of chromium–induced cancers .
Although, a vast amount of literature is available on the kinetics of chromic acid oxidation of various inorganic [8-11] and organic [12-15] compounds, no reports are available on the oxidation of the biologically active formamidines by this oxidant. Therefore, the present work seek to study the kinetics of oxidation of one of the most important formamidine derivative, namely N,N-dimethyl-N’-(5-methyl-1H-pyrazol-3-yl) formamidine (MAPF) by chromic acid in aqueous sulfuric acid solution. The objectives of such study were to check the selectivity of MAPF towards chromic acid, to establish the optimum conditions affecting oxidation of MAPF, to identify the different chromium intermediate species in such medium as well as MAPF, and finally to elucidate a plausible oxidation reaction mechanism.
Reagent grade chemicals and doubly distilled water were used throughout the work. A stock solution of MAPF was prepared by dissolving the requisite amounts of the sample in doubly distilled water. Required solution of the chromic acid oxidant was freshly prepared before each experiment and it was standardized spectrophotometrically. Sodium sulfate and acetic acid was employed to vary the ionic strength and dielectric constant in the reaction medium, respectively.
2.2. Kinetic Measurements
The reactants were formulated such that the reaction was of pseudo-first order kinetics where the substrate (MAPF) was added in a large excess relative to chromic acid. The reaction was followed by tracing the decay in CrVI absorbance at λmax = 348 nm, its maximum absorption wavelength, whereas the other constituents of the reaction did not absorb significantly at this wavelength. The applicability of Beer’s law for CrIV at 348 nm has been verified giving ɛ = 2035±15 dm3 mol−1 cm−1. Shimadzu UV-VIS-NIR-3600 double-beam spectrophotometer was used for all absorbance measurements.
First order plots of ln(absorbance) versus time were found to be linear up to more than 80% of the reaction completion and the pseudo-first order rate constants were evaluated as the gradients of such plots. Average values of at least two independent kinetic runs of the rate constants were taken for the analysis. The kinetic runs were reproducible to within ±4%. A few kinetic runs were performed after bubbling purified nitrogen and compared with those taken under air, and the results were found to be the same. Thus the dissolved oxygen did not affect the oxidation rate. The order of reaction with respect to the reactants were determined from the slopes of the log kobs versus log(concentration) plots by varying the concentrations of substrate and acid, in turn, while keeping other conditions constant.
The stoichiometry was determined spectrophotometrically which indicates consumption of two moles of chromic acid for three mole of MAPF to yield the oxidation products as shown in the following equation,
where MAP refers to methylaminopyrazole. The above stoichiometric equation is consistent with the results of product characterization which carried out by spectral and elemental analysis as described elsewhere [16-18].
3.2. Time-Resolved Spectra
The spectral changes during the oxidation of MAPF by chromic acid in aqueous sulfuric acid solution are shown in Figures 1 and 2. The scanned spectra shown in Figure 1 indicated gradual decay of CrVI band with time at its absorption maximum, λ = 348 nm, as a result of its reduction by the organic substrate (MAPF). Also, there was a simultaneous growing of an absorption band located in the region 395 - 470 nm with appearance of two isosbestic points centered at l = 318 and 393 nm. Careful examination of the spectral scans (Figure 2) manifests simultaneous appearance of new bands located in the wavelength range 390 - 720 nm. These spectroscopic features are consistent with the formation of a chromium(III) product as reported earlier .
3.3. Effect of [Chromic Acid] on the Oxidation Rate
Chromic acid oxidant was varied in the concentration range of (3.0 – 8.0) x10-4 mol dm−3 at fixed [MAPF], [H+], ionic strength and temperature. Plots of ln(absorbance) versus time were linear for more than 80% of the reaction completion. Furthermore, the observed first order rate constant, kobs, was found to be independent of the initial chromic acid concentration as listed in Table 1. These results confirm first order dependence of the reaction with respect to chromic acid concentration.
3.4. Effect of [MAPF] on the Oxidation Rate
The observed rate constant was determined at different initial concentrations of the reductant MAPF keeping other reactants concentrations constant. A plot of kobs versus [MAPF] was found to be linear with a positive intercept (Figure not shown) indicating that the reaction order with respect to [MAPF] was less than unity. This was also confirmed by the constancy of the second-order rate constants obtained by dividing the kobs values by [MAPF] at fixed [CrVI].
3.5. Effect of [H+] on the Oxidation Rate
To explore the effect of hydrogen ion concentration on the reaction rate, kinetic runs were carried out by varying the hydrogen ion concentration (1.0 - 3.0 mol dm-3) at constant [MAPF], [CrVI], ionic strength and temperature. An increase in acid concentration was found to accelerate the oxidation rate (Table 1) indicating that the oxidation process is acid-catalyzed. A plot of kobs versus [H+] was found to be linear with a positive intercept on kobs axis suggesting that the reaction was fractional-first order (Figure not shown).
|104 [CrVI] (mol dm-3)||102 [MAPF] (mol dm-3)||[H+] (mol dm-3)||I (mol dm-3)||105 kobs (s-1)|
Experimental error ± 4%.
3.6. Effect of Ionic Strength and Solvent Polarity of the Medium
The ionic strength was varied from 3.0 to 4.5 mol dm-3 using sodium sulfate at constant concentrations of MAPF and CrVI and at constant pH and temperature. Increasing the ionic strength had a negligible effect on the reaction rate (Table 1).
To investigate the effect of the solvent polarity (ɛ) of the reaction medium on the rate, the reaction was studied at different solvent compositions of acetic acid and water by varying the acetic acid content from 0 to 40% (V/V) in the reaction medium at constant other variables. As for ionic strength, changing solvent polarity of the medium did not affect the reaction rate.
3.7. Effect of Manganous Ion on the Oxidation Rate
To examine the contribution of CrIV as an intermediate species of chromium in the oxidation reaction, various concentrations of manganous ion, MnII, were added to the reaction mixtures up to 0.01 mol dm-3. The rate of reaction was found to decrease linearly with increasing the added MnII as shown in Figure 3.
3.8. Effect of AgI, PdII and RuIIICatalysts
The reaction rate was measured at various AgI, PdII and RuIII concentrations (2.0 – 12.0 x 10-6 mol dm-3) at constant other variables. The results show that the rate was increased with increasing metal ion concentration and the order of catalytic efficiency was: AgI > RuIII > PdII as shown in Figure 4.
3.9. Effect of Temperature on the Oxidation Rate
The reaction was studied at five temperatures, 15, 20, 25, 30 and 35°C with varying both substrate and hydrogen ion concentration keeping other conditions constant. The reaction rate was found to increase with raising temperature. The activation and thermodynamic parameters were evaluated and were listed in Tables 2 and 3, respectively.
3.10. Polymerization Test
The possible intervention of free radicals in the reaction was examined as follows: the reaction mixtures, to which a known quantity of acrylonitrile monomer was initially added and was kept for 6 h in an inert atmosphere. On diluting the reaction mixture with methanol, no white precipitate was formed thus confirming the absence of free radical in the reaction.
Two reaction mechanisms for electron transfer were suggested  for redox reactions involving chromium(VI) as an oxidant in acid media. The first mechanism involves a successive one-electron transfer in two steps. The second one involves a simultaneous two-electron transfer in a single step. However, both successive one-electron and simultaneous two-electron changes may be considered during reduction of chromium(VI) leading to formation of either CrV or CrIV intermediate species, respectively [21-23]. In the present investigation, the negative result for free radical intervention ruled out the formation of CrV intermediate species. On the other hand, the contribution of CrIV as an intermediate species during the reaction can be proved by inhibition of the oxidation rates upon addition of MnII to the reaction medium. This is because MnII has been recognized as a frequently tool for trapping CrIV intermediate . Therefore, if CrIV intermediate is involved, addition of MnII to the reaction mixture will remove it from the oxidation reaction resulting in a decrease in the oxidation rate according to the equation, CrIV + MnII = CrIII + MnIII. The notable decrease in the oxidation rate upon addition of MnII (Figure 3) is considered as good evidence to the contribution of CrIV. The inhibition effect occurs due to the competition existing between the substrate and MnII to react with CrIV.
In aqueous acid media, chromium(VI) was suggested [25, 26] to exist mainly as acid chromate, H2CrO4, as represented by the first step in Figure 5. The enhancement of the oxidation rate upon increasing hydrogen ion concentration confirmed a protolytic process of the chromate ion, i.e. the protonated species of the chromate oxidant (H2CrO4) may be considered as the kinetically reactive species which play the main role in the oxidation kinetics.
The present reaction between chromic acid and MAPF in H2SO4solution showed a stoichiometry of 2:3 (CrVI: MAPF) with a first order dependence on [CrVI] and a fractional-first order kinetics with respect to [MAPF]. The fractional order dependence on MAPF concentration can be attributed to complex formation between MAPF and chromic acid in a pre-equilibrium step. The formation of the complex was also proved kinetically by a non-zero intercept of the plot of 1/kobs versus 1/[MAPF] as shown in Figure 6. Further evidence for complex formation was obtained from the UV-Vis spectra as shown in Figure 1. A similar spectrophotometric observation was reported earlier [27, 28]. The complex formation between chromium(VI) and different organic compounds in acid media was also reported [28, 29]. Furthermore, the negligible effects of ionic strength and solvent polarity of the medium were consistent with a reaction occurs between an ion and a neutral molecule or between two neutral molecules [30, 31] i.e. between MAPF and H2CrO4.
Hence, the most reasonable reaction mechanism which may be suggested (see Figure 5), involves a fast complexation between the reductant MAPF and chromic acid oxidant to give an intermediate complex (C). The latter was slowly decomposed in the rate-determining step followed by subsequent fast steps, to give rise to the final oxidation products.
The suggested mechanistic Figure 5 leads to the following rate law (see Appendix A),
Under pseudo-first order condition,
Comparison of Eqs. (1) and (2) gives,
and with rearrangement of Eq. (3) leads to the following equations,
Owing to Eqs. (4) and (5), plots of 1/kobs versus 1/[MAPF] at constant [H+] and plots of 1/kobs versus 1/[H+] at constant [MAPF] should give straight lines with positive intercepts on the 1/kobs axes, as were experimentally observed (Figures 6 and 7, respectively). Values of the rate constant of the slow step (k1) along with the equilibrium constants K1 and K2 at different temperatures were calculated from the slopes and intercepts of such plots and were listed in Tables 2 and 3, respectively. The obtained values of the protonation constant of mono hydrogen chromate (K1) are in agreement with those reported in the literature .
The activation parameters of the rate constants of the slow step (k1) are calculated using Arrhenius (Figure 8a) and Eyring (Figure 8b) plots, and were listed in Table 2. Furthermore, the thermodynamic parameters of the equilibrium constants were also determined using a van’t Hoff plots (Figure 9) and were also listed in Table 3.
The obtained large negative values of DS≠ are consistent with the formation of compacted intermediate complex and such activated complex is more ordered than the reactants due to loss of degree of freedom. The experimental values of DH≠ and DS≠ were both favorable for electron-transfer process . Again, the positive values of DH≠ and DG≠ indicate endothermic formation of the intermediate and its non-spontaneity, respectively.
On the other hand, the enhancement of oxidation rate upon addition of the metal cations AgI, PdII and RuIII may be interpreted by formation of complexes with the reactants and, hence, facilitate the electron transfer, or oxidation of the substrate itself [34-36].
Experimental error = ±4%.
Experimental error ± 5%.
The oxidation of methylaminopyrazole formamidine (MAPF) by chromic acid was studied in sulfuric acid solutions. H2CrO4 is suggested to be the kinetically active species of the oxidant which takes part in the oxidation reaction. The final oxidation products of MAPF were identified as methylaminopyrazole, dimethylamine and carbon dioxide.
A spectral evidence for the formation of chromium(III) product was obtained. A mechanism which proposed for the oxidation reaction is in conformity with the kinetic findings. The rate and equilibrium constants involved in the different steps of the proposed mechanism along with their activation and thermodynamic parameters are evaluated and discussed.
According to the suggested reaction mechanism, and regarding to steps (I) and (II) in Scheme 1,
and K2 = ,
[C] = K2[MAPF][H2CrO4] = K1K2[MAPF][HCrO4-][H+] (A.2)
From step (III) in Scheme 1, the rate law expression can be expressed by Eq. (A.3),
Substituting Eq. (A.2) into Eq. (A.3) leads to,
Rate = k1K1K2[MAPF][HCrO4-][H+] (A.4)
The total concentration of HCrO4- is given by,
[HCrO4-]T = [HCrO4-]F + [H2CrO4] + [C] (A.5)
where ‘T’ and ‘F’ stand for total and free.
Substituting Eq. (A.1) into Eq. (A.5) gives,
[HCrO4-]T = [HCrO4-]F + K1[HCrO4-][H+] +K1K2[MAPF][HCrO4-][H+] (A.6)
[HCrO4-]T = [HCrO4-]F(1+ K1[H+] + K1K2[MAPF][H+]) (A.7)
Also, the total concentration of MAPF is given by,
[MAPF]T = [MAPF]F + [C] (A.9)
Substituting Eq. (A.2) into Eq. (A.9) leads to,
[MAPF]T = [MAPF]F + K1K2[MAPF][HCrO4-][H+] (A.10)
[MAPF]T = [MAPF]F (1+ K1K2[HCrO4-][H+]) (A.11)
Because of low concentration of HCrO4- used, the term K1K2[HCrO4-][H+] in the denominator can be neglected. Hence,
[MAPF]F = [MAPF]T (A13)
In view of the high concentrations of [H+] we can write,
[H+]F = [H+]T (A.14)
Substituting Eqs. (A.8), (A.13) and (A.14) into Eq. (A.4) (and omitting ‘T’ and ‘F’ subscripts) gives,
Under pseudo-first order condition,
Comparing Eqs. (A.15) and (A.16), the following relationship is obtained,
and with rearrangement, the following equations are obtained,