Voltammetric Generation and Kinetic Stability of Nitro Anion Radical from Nitrofurazone in Ionic Liquids

Abstract

The nitrofurazone (NF) electrochemical reduction has been studied by cyclic voltammetry (CV) and square wave voltammetry (SWV) in non-aqueous medium using three different ionic liquids (IL): BMImTf₂N, BMImBF₄ and BMMImTf₂N, having a carbon fiber microelectrode as working electrode. In all of them, two reversible cathodic peaks were recorded for NF. Under higher frequency values, only one reversible cathodic peak was registered. The systems reversibility could also be observed by CV, since a reversible redox couple was registered for this reduction. The systems reversibility with product and reagent adsorptions on the electrode surface was confirmed and the electrons number involved in this reduction indicated the nitro-anion radical formation followed by its respective dianion. For the first reduction, the EC mechanism (an electrochemical step followed by a chemical one) was considered for the systems in aprotic medium, in which there was a probable second-order chemical reaction after the charge transfer process, being the kinetic constants calculated following the Olmstead and Nicholson model.

Keywords:
nitrofurazone; nitro-anion radical; ionic liquids; voltammetry; EC mechanism

Introduction

Nitrocompounds belong to a class of organic compounds widely used as solvents, pesticides, dyes, explosives and drugs.^1,2 The therapeutic use of nitrocompounds as drugs deserves to be highlighted due to their wide range of biological actions, being classified as antibacterial, antiprotozoal and anticancer agents.³ In general, these biological activities are a result of their interaction with the biological targets from the nitro group reduction by nonspecific nitroreductases, generating free radicals that cause toxic oxidative stress in bacteria and parasites.^3-5 The nitro-heterocyclic compound, nitrofurazone (Figure 1), is commonly used as a prototype for the new drugs development due to its antiprotozoal activity,^4,6,7 especially for Chagas disease, which is considered one of the most serious health problems in the Latin America for being an endemic disease.^7,8

Figure 1
Nitrofurazone (NF).

The nitro-heterocycles have a complex and well-known reduction mechanism in which the formation of the nitro-anion radical (R-NO₂^•-) and the hydroxylamine derivative (R-NHOH) are accepted as the main species responsible for the compounds cytotoxic action.^9,10 The nitro group is known to be capable of receiving up to six electrons in its complete reduction to amine derivative,^11-14 as shown in Scheme 1. Proton and electron transfers are involved in several steps of the nitro group reduction, which clearly suggests the use of electrochemical techniques as excellent tools to study this kind of drugs. In addition, nitroaromatic compounds are ideal candidates for electrochemical detection due to their easily reducible nitro groups which originates distinct current response even in low concentrations.^15-19 In this context, several studies^11,15,16 on the voltammetric behavior of nitro-heterocycles have been performed in order to comprehend the species which have biological performance to specific targets.

Scheme 1
Complete reduction mechanism of the nitro group.

The voltammetric reduction mechanism of nitro-heterocycles can be significantly affected by the medium in which the reaction is carried out. Classically, in acidic medium, two voltammetric waves are registered, being the hydroxylamine derivative formation detected at less negative potential values followed by the second reduction process due to the amine derivative formation.^11-14 Distinctly, in alkaline aqueous media or aprotic/non-aqueous media, the nitro-anion radical generation is facilitated in function of low concentration or absence of protons in solution. In this case, the reversible redox process corresponding to the R-NO₂/R-NO₂^•- couple, involving one electron, is registered before the hydroxylamine derivative formation.^11-14 Additionally, an irreversible chemical reaction can occur after the reversible charge transfer process, characterizing an EC mechanism (an electrochemical step followed by a chemical one), in which the R-NO₂^•- decay is promoted by means of a disproportionation reaction (protic/alkaline aqueous media) or dimerization reaction (aprotic/mixed solvents or non-aqueous media), determining the kinetic stability of nitro-anion radical electrochemically generated.^11-14

Among the non-aqueous media sometimes required in reason of the substrates low solubility in traditional aqueous electrolytes, the ionic liquids (IL) stand out due to their good dissolution capacity, wide electrochemical range and intrinsic conductivity.^20,21 In addition, electrochemical reaction mechanism occurring in IL can be entirely changed compared to that seen in conventional solvents,²² since the mass transport properties and stability of the generated species are modified in this ionic medium. Therefore, the evaluation of nitrocompounds in ionic liquids can be useful. In this sense, several works^23-27 can be quoted as examples by the IL application versatility in electrochemistry of nitrocompounds.

Zhang et al. ²³ proposed electrochemical reduction mechanism of nitrobenzene in 1-butyl-3-methylimidazolium acetate (BMImAc). The results showed that the electrochemical process could be controlled by diffusion and that the main product formed at -1.45 V was azobenzene. A probable reaction mechanism in ionic liquid was proposed, following the formation sequence nitrobenzene → nitrosobenzene → azobenzene → aniline.

Studies^24,25 involving the nitrobenzene reduction and 4-nitrophenol in 1-butyl-2,3-dimethylimidazole bis(trifluoromethanesulfonyl)imide (BMMImTf₂N) were reported using a gold microelectrode. The reduction mechanisms reported are similar to those in aprotic organic solvents, with differences in voltammetric results mainly due to the viscosities of the ionic liquids. Silvester and co-workers^26,27 developed mechanistic studies involving the 2,4,6-trinitrotoluene (TNT) and 2,4-dinitrotoluene (DNT) reductions in IL by cyclic voltammetry, in which two and three reduction peaks were observed corresponding, respectively, to the two and three nitro groups on the aromatic ring. The authors propose that a chemical step occurs after the charge transfer process registered by the first reduction peak, characterizing the EC mechanism for both cases when high concentrations of these compounds are used. Based on the TNT and DNT reductions described above, using a glassy carbon electrode, Zeng and co-workers²⁸ evaluated the reaction mechanisms for the nitro group as a function of the cation and anion composition of ionic liquids and their consequent variation in the physicochemical properties such as viscosity and conductivity as well as solvation forces involving hydrogen-bonding donation ability.

In this context, most studies about the reduction mechanism and electrochemical kinetic of nitro-heterocyclic compounds reaction are mainly performed in aqueous medium as well as conventional non-aqueous. Therefore, among the studies that include non-aqueous medium, there are a few^25-27 that use ionic liquids as an alternative, especially when square wave voltammetry is chosen as electrochemical investigative technique. Considering that, the present study carried out by square wave and cyclic voltammetries by using three different IL (Figure 2) brings a description of the nitrofurazone electrochemical reduction in order to understand both, the nitro-anion radical generation process and its kinetic stability in these media.

Figure 2
Ionic liquids: BMImTf₂N (a), BMImBF₄ (b) and BMMImTf₂N (c).

Experimental

Instrumentation

All the electrochemical measurements were performed with a pontenciostat/galvanostat Autolab PGSTAT302, Eco-Chimie, using an electrochemical cell with a three-electrode system. Carbon fiber microelectrode was used as working electrode, Pt as auxiliary and a silver wire (Ag) as pseudo-reference electrode, whose calibration was done in a 1.5 mmol L⁻¹ ferrocene solution in acetonitrile with oxidation peak at 0.625 V with a 0.225 V lagging to the reference electrode Ag/AgCl (3.0 mol L^-1 KCl) in the same condition.²⁹ The homemade carbon fiber microelectrode was manually polished with alumina suspension on metallographic velvet (Arotec). Its effective area (3.48 µm²) was determined following methodology already reported³⁰ by cyclic voltammetric data obtained for 0.010 mol L⁻¹ of K₃Fe(CN)₆ in 0.5 mol L⁻¹ KCl solution, being the diffusion coefficient 7.76 × 10⁻⁶ cm² s⁻¹.³¹ The electrochemical behavior of the nitrofurazone was studied in IL by cyclic voltammetry (CV) and square wave voltammetry (SWV).

Reagents, solutions and ionic liquids

The stock solutions of 10 mmol L⁻¹ of nitrofurazone (Avocado Company, Morecambe, United Kingdom) were prepared through direct dissolution in the ionic liquids. The solution was stocked in amber flasks, kept under refrigeration (4 °C) and light protected. It was used analytical-grade reagents and ultrapure water from Millipore system Milli-Q from Merck (Darmstadt, Germany) The ionic liquids BMImTf₂N, BMImBF₄ and BMMImTf₂N were synthesized following previous procedure³² and characterized by nuclear magnetic resonance (NMR) spectroscopy (Figures S1-S3, Supplementary Information (SI) section). The voltammetric blank of all ionic liquids was performed in order to ensure that there were no obvious voltammetric events within the available potential range from 0.5 to -1.5 V.

Peak current ratio calculations

The calculated ratio between anodic and cathodic peak currents obtained by cyclic voltammetry registered in IL followed the Olmstead et al. ³³ methodology:

(1) $\frac{\mathrm{Ipa}}{\mathrm{Ipa}}=\frac{{\left(\mathrm{Ipa}\right)}_0}{{\left(\mathrm{Ipc}\right)}_0}+{\left[\frac{{\left(\mathrm{Isp}\right)}_0}{{\left(\mathrm{Ipc}\right)}_0}\right]}^2\beta +\frac{{\left(\mathrm{Isp}\right)}_0}{{\left(\mathrm{Ipc}\right)}_0}\gamma +\xi$

Being (I_pa)₀ and (I_pc)₀ = anodic and cathodic peak currents, respectively, (I_sp)₀ = current measured in the inversion potential, β = 0.9678, γ = -0.5370, ξ = 0.3337.

Kinetic parameter calculations

For the kinetic constants calculation the Olmstead-Nicholson model³³ was adopted, considering that a dimer is formed after the electron transfer process at a fully spherical electrode, plotting a working curve with the fit equation, being the correlation coefficient (R) = 0.99998, described below:

(2) $y=0.60007+0.14894e^{\left(-x/0.41669\right)}+0.25042e^{\left(-x/1.70667\right)}$

being y = ω and x = I_pa/I_pc.

Taking into account the sphericity character for the microelectrode, the ω kinetic parameters were determined through interpolation the I_pa/I_pc values obtained from experimental voltammograms. The ω parameter incorporates the effects of the rate constant (k₂), drug concentration (C) and scan rate.

The plot obtained between ω and τ is a linear fit correlation, following the equation below.

(3) $\omega =k_{2}C\tau$

Considering k₂ = rate constant value for the second-order reaction for the nitro-anion radical decay (L mol^-1s^-1), C = nitrofurazone (NF) concentration (mol L^-1) and τ = (E_1/2 - Es)/n, being E_1/2 correspondent to the half-wave potential, Es corresponds to the initial potential of the reverse scan in CV, and n is the scan rate (V s^-1). From the calculated k₂ by the slope, the nitro-anion radical stability can be estimated by the half-life (t_1/2) equation, assuming [R-NO₂^•-] as drug concentration.

(4) $t_{1/2}=\frac{1}{k_2\left[R-{\mathrm{NO}}_2^{•-}\right]}$

Results and Discussion

Voltammetric behavior of NF reduction in ionic liquids

The IL used in this work were selected according to their electrochemical and physicochemical characteristics (Table S1, SI section), depending on their constituents (cations and anions).³² The ionic liquids containing 1-alkyl-3-methylimidazolium (BMIm⁺) and 1,2-dimethylimidazolium (BMMIm⁺) species were chosen in view of the fact that these cations confer high electrochemical stability and lower viscosity for the IL.²⁶ The difference between BMIm⁺ and BMMIm⁺ is that the former has an acidic hydrogen in the C-2, bringing a differential that can be determinant for the proposed study.^26,28,34 Tf₂N^- and BF₄^- based on ionic liquids were selected since both display excellent electrochemical stability, even having different viscosities.²⁶ Tf₂N^- has delocalized charge, being larger than BF₄^- anion, influencing the ion-pairing in these ionic liquids. It is known that ion-pairing interactions affect the stability of the anion-radical.^26,28

The 10 mmol L^-1 NF reduction was studied with SWV, using frequency (f) = 10 Hz; amplitude (a) = 50.0 mV and sweeping increase (ΔEs) = 2.0 mV, in the three different IL indicated above (Figure 3). All the voltammetric records were obtained by using a carbon fiber microelectrode considered as the best option for the electrochemical measurements, since the volumes obtained by the IL syntheses were significantly small (2 mL was the volume in electrochemical cell) in addition to the advantage of being a homemade microelectrode. Furthermore, microelectrodes have greater mass transport due to the spherical shape of the diffusion layer, facilitating the study of fast electrode reactions and the detection of reaction intermediates which lifetime is very short, such as the formation of radicals. Additionally, the currents measured with microelectrodes are small and do not significantly change the concentration of the electrolyzed species in the solution, so the responses are not so sensitive to errors due to the ohmic drop, therefore, the microelectrodes could be used in solutions with large resistance, such as IL, in the absence of supporting electrolytes.¹⁴ The voltammograms presented two cathodic peaks (E_p1 and E_p2) at -0.623 and -0.783 V, -0.742 and -0.901 V, -0.902 and -1.089 V for BMImBF₄, BMImTf₂N and BMMImTf₂N, respectively. From the current-components evaluation, it was possible to observe the existence of a reversible system, since the net currents (ΔI_p) were made up of direct (I_f) and reverse (I_b) components, as well as previously registered in aqueous media.¹⁴ Thus, for all IL shown in Figure 3, the peaks represented in the voltammograms as E_p1 and E_p2 had the current components I_f and I_b from the ΔI_p decomposition, demonstrating the existence of two reversible systems.^35-37

Figure 3
NF square wave voltammograms in BMImBF₄ (a), BMImTf₂N (b) and BMMImTf₂N (c) 10.0 mmol L^-1 (f = 10 Hz; ΔEs = 2.0 mV and a = 50.0 mV).

In order to obtain information related to the electrode processes, the previous procedure tested in aqueous media was followed,¹⁴ being the frequency variation study also performed in IL. The frequency varied from 10 to 250 Hz, in which a = 50.0 mV and ΔEs = 2.0 mV were maintained. The E_p2 was observed throughout the frequency range studied in BMMImTf₂N. However, in BMImBF₄ and BMImTf₂N, E_p2 was registered only at frequencies lower than 50 and 70 Hz, respectively (results not shown).

According to literature,^35,36 the reversibility of the system could be verified by the linear relationship between ΔI_p and f^1/2, which can be seen in Figure 4. For the NF reduction in the three IL, the linear relationship was found in 10 Hz ≤ f ≤ 100 Hz range. For f > 100 Hz, it can be observed in Figure 4 that the behavior was changed in all cases. It is known that the greater the reversibility of the reaction, the higher the reverse current contribution implying an increase of ΔI_p intensity, since the peak current value is the result of the difference between I_f and I_b.^35,36 In this case, the ΔI_p decrease at higher frequency values suggests a lower I_b contribution with consequent loss of reversibility. Possibly, in these specific reduction process, the systems were apparently reversible at lower and quasi-reversible to higher frequencies.^35,36 Similar behavior has also been recorded for the NF in aqueous media.¹⁴

Figure 4
Plots of ΔI_p1 (■) and ΔI_p2 (●) vs. f^½ for NF in BMImBF₄ (a), BMImTf₂N (b) and BMMImTf₂N (c).

The opposite occurred for ΔI_p2, in which there was practically no net current increase with the frequency variation, indicating that the system reversibility tends to decrease with the increased f, reason why at frequencies higher than 50 Hz in BMImBF₄ and 70 Hz in BMImTf₂N there was no second reduction process record since the charge transfer process occurred more slowly than the potential scan rate. It is worth recalling that the scan rate for SWV analysis is given as function of the potential sweep increment and the potential pulses application frequency (f × ΔEs).³⁴ Therefore, as the potential values increment remained constant during the analyses, the scan rate increased according to the frequency increase. In this sense, the charge transfer process may be associated with the viscosity of each IL, since the diffusion coefficients decreased as the IL viscosity increased and the charge transfer occurred more slowly.

Figure 5 shows the relationship between peak potential values (E_p1 and E_p2) and the log f. The potential values for both peaks were practically kept constant with the frequency variation correspondent to the range in which the NF reduction was considered reversible for all IL studied (Figure 4, f ≤ 100 Hz), suggesting that reagents and products were adsorbed on the electrode surface.³⁵ According to the SWV theoretical model^35,36 for reversible systems, it is possible to calculate the kinetic rate constants of the reaction (k_r) for each system applying the equation I_p= k_r f^1/2. Regarding the k_r values and considering the ratio of log k_r/2f as determinant to clarify the mass transport process in the system, this ratio was calculated for the frequency range in all cases. For f = 10 Hz, the values of 0.477, 0.507 and 0.538 were estimated in BMImBF₄, BMImTF₂N and BMMImTF₂N, respectively, being, in this way, approximated to the established ratio value of 0.5 for reagent and product adsorption on the electrode surface.^35,36 However, the increased frequency provoked a significant decrease in these values, indicating loss of product and reagent adsorptions, which could be inferred that the system was not completely controlled by adsorption but by diffusional process at higher frequencies. In this sense, the the equation E_p/2 = 97/n mV, being E_p/2 the width at half-height peak and n the electrons number in the processes, was applied for the lowest frequency value (10 Hz) for which the SWV theoretical model^35,36 was completely fitted. Based on this behavior, the electrons number for both reduction processes correspondent to E_p1 and E_p2 were estimated (Table S2, SI section), being the values found between 0.85 and 0.88 for E_p1 and between 0.93 and 1.20 for E_p2.

Figure 5
Plots of E_p1 (■) and E_p2 (●) vs. log f for NF in BMImBF₄ (a), BMImTf₂N (b) and BMMImTf₂N (c).

Considering previous results,^12-14 the reversible system observed at less negative potentials (E_p1) was associated to the nitro-anion radical generation from NF in the three IL studied, according to the reaction in Scheme 2. Additionally, the dianion formation has been identified as the correspondent product obtained at E_p2. Literature works^28,38 have shown that the nitrocompounds voltammetric reduction in IL presents the possibility of the dianion formation after the nitro-anion radical generation. This formation might be accompanied by a certain instability, since the dianion is a strong Lewis base capable of removing protons from species normally non-donors under normal conditions, as it occurs with BMIm⁺ which has an acidic proton available at the C-2 position. This difference between BMIm⁺ and BMMIm⁺ would explain why the latter registered a higher intensity for E_p2 than the former. Moreover, the dianion formation was registered throughout the frequency range for BMMImTf₂N (IL with lowest viscosities) and only at low frequencies for BMImBF₄ and BMImTf₂N (IL with highest viscosities).^39-42 The dianion formation occurred from a nitro-anion radical reversible reduction, involving one more electron as also shown in Scheme 2.

Scheme 2
Reduction mechanism for the nitro-anion radical generation followed by the corresponding dianion formed.

In a complementary manner, information on the electrode process involving the NF reduction has been provided by studying the variation of CV scan rate, considering the range from 0.1 to 1.0 V s^-1. Figure 6 shows the cyclic voltammograms of NF reduction registered in each IL, being only one reversible system registered. Following the same record obtained by using SWV, the voltammetric waves registered in all IL corresponding to the R-NO₂/R-NO₂^•- reversible couple, having the values of E_pc -0.620 V (BMImBF₄), -0.814 V (BMImTf₂N) and -0.970 V (BMMImTf₂N). Probably, in function of the sensibility differences in comparison to the voltammetric pulse techniques the dianion formation was not observed by CV. The relations between current cathodic values (I_pc) and scan rate (n) indicated that the process was predominantly controlled by diffusion. The linear relationships of I_pc vs. n^1/2 (Figures 6b) showed this NF voltammetric behavior in all IL studied. Moreover, the slopes of the log-log plots (Figures 6c) close to 0.5 is an empiric indication of the diffusional controlled process,⁴³ being the slope values: 0.51, 0.53 and 0.49 for BMImBF₄, BMImTf₂N and BMMImTf₂, respectively. It is worth mentioning that these results were obtained after the manual polishing of the working microelectrode among the measurements. These results complement and reinforce the NF voltammetric reduction behavior registered by using SWV, in which the registers were carried out at lower scan rates (< 200 mV s^-1) while by using CV the scan rate range was wider and presenting higher values.

Figure 6
(a) Cyclic voltammograms of NF 10 mmol L^-1, ν = 500 mV s^-1, (b) plots of I_pc vs. ν^1/2 and (c) log I_pc vs. log ν in BMImBF₄ (A); BMImTf₂N (B); BMMImTf₂N (C).

Effect of the variation of NF concentration

The knowledge on the electrochemical reduction of nitroheterocyclic compounds is consolidated in both, protic and aprotic media, normally having a conventional size electrode as working electrode.^10-13,44-46 It can be observed that the cyclic voltammograms in Figure 6 show a similar profile to that recorded by a macroelectrode. Probably, the high viscosity and low conductivity of the IL promoted a certain hysteresis with microelectrode. That way, this behavior made it possible to acquire kinetic information related to the reaction order associated to the chemical step which may have occurred after the charge transfer in the NF electrochemical reduction. Applying the methodology of Olmstead-Nicholson,³³ the current ratio (I_pa/I_pc) is the main parameter as diagnostic criteria for the EC mechanism. The evaluation of the NF concentration effect on I_pa/I_pc values can bring a kinetic response, because if the chemical reaction that occurs after the charge transfer process following first-order kinetics, the current ratio values are kept constant with the concentration increase.^11,13,44 On the contrary, as it can be seen in Figure 7, the I_pa/I_pc values decrease as the NF concentration increases when its voltammetric reduction was performed in BMImBF₄ and in BMImT_f2N, indicating that the chemical reaction which occurs after the charge transfer process is second-order.^11,33,44 Curiously, in BMMImTf₂N there was no radical formation record for NF concentrations higher than 10 mmol L^-1.

Figure 7
Variation of I_pa/I_pc as a function of the NF concentration in BMImBF₄ (■) and in BMImTf₂N (●), ν = 500 mV s^-1. Initial potential scan (E_i) = 0.4 V and final potential scan (E_f) = –1.2 V.

In a protic media, in which there are protons to donate to the radical, the disproportionation reaction is favored after the charge transfer process, because the protonation of the radical generates the intermediate R-NO₂H•, facilitating the fast reaction between the R-NO₂^•- and its neutral radical form,^11,44,45 as shown by the reaction above:

(5) $R-{\mathrm{NO}}_2{H}^{•}+{\mathrm{NO}}_2^{•-}\left(+H^{+}\right)R-{\mathrm{NO}}_2+R-\mathrm{NO}\left(+H^{+}\right)$

On the other hand, as the IL used do not have ionizable hydrogen, the reactional model in aprotic media is better suited for the cases in which the mechanism proposed involves the nitrocompounds reduction in IL. Kanget al.²⁶ suggest the azo-product electrogeneration from nitro-anion radical generated on the electrode surface. Thus, the dimerization reaction could be considered, as well as a reaction between the radical formed at the electrode surface and the drug at the edge of the diffusion layer, being possible for the nitro-anion radical abstract a proton from another NF molecule following as a father-son reaction.^11,26,27 In any case, it can be reaffirmed that a second-order chemical reaction is the one that should occur.

Kinetic parameter calculations

According to the information obtained about the reaction order, the rate constants (k₂) were determined from the plots obtained between the kinetic parameters ω and τ for each IL studied (Figure 8). As there was no record of the anodic peak in lower concentrations, 10 mmol L^-1 of NF have been chosen to work.

Figure 8
The kinetic parameters ω as a function of τ for NF 10.0 (■), 15.0 (●) and 20.0 mmol L^-1 (▲) for BMImBF₄ (a), BMImTf₂N (b) and BMMImTf₂N (c).

Considering the NF electrochemical reduction as an EC mechanism and complementing the results described above, a second-order chemical reaction was adopted, considering that the model for a dimerization reaction is the best fit to what occurred in the IL, similarly as already registered in aprotic media.^11,33

For the NF in BMImBF₄ and in BMImTf₂N, the k₂ values were calculated for the three different concentrations (10, 15 and 20 mmol L^-1), reaching order values of 10². These values were increased in function of the compound concentration increase (Table 1). By doubling the NF concentration, the k₂ values reach a difference of up to a magnitude order. Similar behaviors were observed for NF in both IL, in which the highest stabilities were found for the lowest concentrations and with the longest half-life times.

Table 1
k₂ and t_1/2 values for the second-order chemical reaction from nitro-anion radical in IL

IL	NF concentration / (mmol L-1)
	10			15			20
	k2 × 10-2 / (mol L-1 s-1)	t1/2 / s		k2 × 10-2 / (mol L-1 s-1)	t1/2 / s		k2 × 10-2 / (mol L-1 s-1)	t1/2 / s
BMImBF4	0.533	1.87		1.25	0.54		5.02	0.10
BMImTf2N	1.36	0.73		8.41	0.08		16.8	0.03
BMMImTf2N	2.22	0.45		-	-		-	-

• NF: nitrofurazone; IL: ionic liquids; k₂: rate constant value for the second-order reaction for the nitro-anion radical decay; t_1/2: half-life.

The NF kinetic constants were calculated in BMMImTf₂N in the same conditions mentioned above, although only one value was calculated for these IL having 10 mmol L^-1 as NF concentration. The values on Table 1 were similar to those found in BMImTf₂N and BMImBF₄. From the results for all IL, the radical stability was the highest in BMImBF₄ with NF concentration of 10 mmol L^-1, being the lowest k₂ value and the highest t_1/2 value in these conditions. This may be explained by the fact that the radical decay reaction occurred more slowly in BMImBF₄, since it was the one presenting the highest viscosity followed by BMImTf₂N and BMMImTf₂N. In addition, as already mentioned, the composition of cations and anions of IL also influences the radical stability. In this sense, larger stability was observed in liquids containing the BMIm⁺ cation, which can be explained by a stronger interaction in function of a lower distance between the radical anion charge center and the cation. This occurred due to the planar geometry of the imidazolium BMIm⁺ ring and by the imidazolium cation ability for hydrogen-bonding.³⁴ For BMMIm⁺ cation, the values calculated for the k₂ and t_1/2 showed smaller radical stability, inferring that due the bulky cation, a large steric hindrance occurred around the R-NO₂ group, which decreased the ion-pair interaction.^23,34 Regarding the anions BF₄^- and Tf₂N^-, this interaction is also affected by the anion size, being stronger when it comes to a small anion, as in the case of the BF₄^-, since its substitution by the radical anion is easier than when a larger anion as Tf₂N^- is used.⁴⁶ In this case, combining the BMIm⁺ cation with the BF₄^- anion, the best stability conditions for the radical formation in terms of viscosity and pairing interactions was obtained.

Conclusions

The NF voltammetric reduction in the three ionic liquids showed that the nitro-anion radical formation was recorded in all cases, followed by the formation of its respective dianion, being two processes characterized as reversible. Based on the SWV parameters variations, the reagent and product adsorption processes on electrode surface was demonstrated only for lower frequency values, being predominantly controlled by diffusion for the frequency range used. The number of electrons estimate showed that one electron is involved in each reduction step, confirming the radical and the dianion formations. The CV study showed the existence of an EC mechanism, in which a chemical reaction occurred after the charge transfer process corresponding to the nitro-anion radical generation, being a second-order chemical reaction. The kinetic constant values were calculated, having their values increased as function of the NF concentration increase. Consequently, the radical half-life time values indicate the largest stability in BMImBF₄. The introduction of IL as a reaction medium, using the microelectrode as a working electrode, proved to be a good alternative for kinetic and mechanistic studies of nitroheterocyclic compounds.

Supplementary Information

Supplementary information about characterization by ¹H NMR, elemental analysis and physicochemical parameters of the ionic liquids and the number of electrons involved in the NF voltammetric reduction are available free of charge at http://jbcs.sbq.org.br as PDF file.

Acknowledgments

The scholarship for L. D. Chiavassa by the Coordenação de Aperfeiçoamento de Pessoal de Nível Superior (CAPES) and the financial support from FAPESP (2018/20826-4) for Fernanda F. Camilo are aknowledged.

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Publication Dates

• Publication in this collection
  29 Mar 2021
• Date of issue
  Apr 2021

History

• Received
  10 Aug 2020
• Accepted
  07 Dec 2020