1 Background

The hydrazones are a group of compounds that contain the azomethine linkage. This linkage influences the majority of their reactions and properties [13]. The derivatives of hydrazone have been demonstrated to display diverse biological activities which include α-glucosidase inhibition [33, 41], antibacterial and anti-fungi [4, 14, 16, 32, 34], anticancer [18, 38], antitumor [32], anticonvulsant [11], anticholinesterase [20] and antioxidant [3, 7, 12, 15, 19, 23] activities. Recently, hydrazone derivatives have been employed as corrosion inhibitors for mild steel and iron [10, 21]. They have also been shown to possess photoprotective capacities [7].

The various metabolic processes that take place in the human system result in the production of free radicals which includes reactive oxygen species (ROS). Excessive and uncontrolled production of reactive oxygen species in the human system is the major cause of various disease conditions such as atherosclerosis, cancer, cardiovascular disorders and oxidative damage to proteins and DNA [3, 19]. This condition could be prevented by the application of antioxidant therapeutic agents such as hydrazone derivatives with potent antioxidant activities. Antioxidants are able to interact with free radicals and terminate the chain reactions that cause their damaging effects in the body.

Virtual screening employs computer-based methods in the design and identification of new chemical entities on the basis of their biological activities. Upon the application of virtual screening, a large collection of compounds can be analysed, and candidates with the best potency subjected to synthesis. The key advantages associated with virtual screening are its ability to control cost, time and wastage encountered when screening a large collection of compounds for a particular biological activity. Two broad categories of virtual screening have been distinguished, namely, docking and ligand-based virtual screening [43]. Docking is a structure-based screening method, while ligand-based virtual screening involves the use of active compounds as templates. The particular chosen screening method depends on the information available for the system. Ligand-based approaches employ pharmacophore or quantitative structure-activity relationship quantitative structure-activity relationship (QSAR) models to screen a broad range of ligands [24, 35].

The use of mathematical models such as those generated from QSAR studies, for screening new chemical compounds through the technique of ligand-based virtual screening is gaining popularity in the development of novel compounds with improved biological activities [5, 6, 26]. This research entails a systematic investigation of the free radical-scavenging mechanisms of newly designed hydrazone derivatives by thermodynamic studies. The earlier developed QSAR model for hydrazones [1] was employed in the design of a new set of hydrazone derivatives by ligand-based virtual screening. The antioxidant activities and applicability domain of these compounds were investigated with the aid of the model. The three basic mechanisms of free radical scavenge, namely, hydrogen atom transfer (HAT), single-electron transfer followed by proton transfer (SET-PT) and sequential proton loss electron transfer (SPLET), were investigated for the designed compounds with best antioxidant potentials via thermodynamic studies. This was accomplished by calculating the various antioxidant parameters such as bond dissociation enthalpy (BDE), adiabatic ionization potential (AIP), proton dissociation enthalpy (PDE), proton affinity (PA) and electron transfer enthalpy (ETE). Subsequently, the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital (LUMO) distributions of the compounds as well as their radical spin density were evaluated. The DFT method has been found to give an accurate evaluation of the above mentioned reaction enthalpies that characterize the various reaction mechanisms. Subsequently, geometry optimization of all molecular structures was conducted in the gas phase at the density functional theory (DFT) level with B3LYP functional and 6-311G* basis set. Also, the thermodynamically preferred mechanism of the reactions between the considered antioxidants and the two important peroxyl radicals (hydroperoxyl radical (HOO·) and methyl peroxyl radical (CH3OO)) were evaluated through the computation of their reaction Gibbs free energy.

2 Methods

2.1 Ligand-based virtual screening of new compounds

The results of the developed QSAR model for hydrazone antioxidants [1] were employed in the design of a new set of hydrazone compounds by ligand-based virtual screening. The applicability domain for the developed model has a leverage threshold h∗, value of 0.375.

This was performed by insertion, deletion and substitution of different substitutes on the template molecule as dictated by the developed hydrazone antioxidant model [6, 25, 28]. In the present research, compound M010 (Fig. 1) listed in Table 1 of [1], was chosen as a template based on its good antioxidant activity (pIC50 = 6.123). The chemical structures of the compounds were drawn using the Chem Draw Program [22]. With the aid of the Spartan 14 program [39], the resulting structures were minimized and further optimized at the density functional theory (DFT) level using the Becke’s three-parameter Lee-Yang-Parr hybrid functional (B3LYP) and 6-311G* basis set without symmetry constraints. This resulted in the generation of quantum chemical descriptors. The optimized structures were converted to Sdf files and submitted for the generation of molecular descriptors using the PADEL program package version 2.20 [46]. The effects of the structural modifications on the antioxidant activity of the resulting compounds were investigated. Subsequently, the applicability domain of the newly designed compounds was assessed by the leverage approach.

Fig. 1
figure 1

The parent hydrazone molecule used as a template (M010)

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Table 1 Designed hydrazone antioxidants, their predicted antioxidant activities and leverage values
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2.2 Calculation of antioxidant parameters

In order to evaluate the preferred mechanism of free radical scavenge, various antioxidant descriptors were calculated as presented below:

The homolytic bond dissociation enthalpy (BDE): This is the standard enthalpy change at a given temperature when a particular chemical bond is broken under standard conditions [37]. The stability of the corresponding hydroxyl group is determined by the value of the BDE. When the BDE value is low, the stability of the corresponding O–H bond is low and thus can easily be broken (Fuyu and Ruifa 2013). This gives rise to high antioxidant capacity for the considered compound. This parameter was calculated under standard conditions of 1 atm and 298.15 K as presented in Eq. 1.

$$ \mathrm{BDE}={H}_{\mathrm{radical}}+{H}_{\mathrm{H}}-{H}_{\mathrm{neutral}} $$
(1)

The adiabatic ionization potential (AIP): This potential describes the process of electron donation by the antioxidant. It represents the capacity of the antioxidant to transfer electrons to the free radical. The lower the AIP value for a given molecule, the easier is the capacity to transfer electrons and the higher the susceptibility of that molecule to undergo ionization. Molecules with high to low AIP values have been observed to possess very strong antioxidant properties.

This parameter was estimated according to Eq. 2;

$$ AIP={H}_{\mathrm{cation}\ \mathrm{radical}}+{H}_{\mathrm{electron}}-{H}_{\mathrm{neutral}} $$
(2)

The proton dissociation enthalpy (PDE): This was also calculated using Eq. 3. PDE is a useful physical parameter that describes the ability of the compounds to donate a proton. Antioxidants with lower values of PDE have been observed to be more susceptible to proton abstraction [27].

$$ \mathrm{PDE}={H}_{\mathrm{radical}}+{H}_{{\mathrm{H}}^{+}}-{H}_{\mathrm{cation}\ \mathrm{radical}} $$
(3)

The proton affinity (PA): This may be defined as the negative of the molar enthalpy change at 298.15 K. The lower the PA value, the higher the antioxidant activity.

This parameter was computed using Eq. (4)

$$ \mathrm{PA}={H}_{\mathrm{anion}}+{H}_{{\mathrm{H}}^{+}}-{H}_{\mathrm{neutral}} $$
(4)

The electron transfer enthalpy (ETE): Eq. 5 was employed in the calculation of ETE. The lower the ETE value, the more active is the resulting phenoxide anion for a given molecule.

$$ \mathrm{ETE}={H}_{\mathrm{radical}}+{H}_{\mathrm{electron}}-{H}_{\mathrm{anion}} $$
(5)

where

Hradical= Total enthalpy of phenoxyl radical.

HH= Total enthalpy of the hydrogen atom.

Hneutral= Total enthalpy of neutral compound.

\( {H}_{{\mathrm{H}}^{+}}= \) Total enthalpy of the proton.

Hcation radical= Total enthalpy of the cation radical.

Helectron= Total enthalpy of the electron.

Hanion= Total enthalpy of the anion.

In this research, the total enthalpies of the species were calculated as the sum of total electronic energy, zero-point energy and the translational, rotational and vibrational contributions to the total enthalpy (Eq. 6). The RT (PV-work) term was added to convert the energy to enthalpy [29].

$$ H={E}_0+\mathrm{ZPE}+{H}_{\mathrm{trans}}+{H}_{\mathrm{rot}}+{H}_{\mathrm{vib}}+\mathrm{RT} $$
(6)

where, Htrans, Hrot and Hvib are the translational, rotational, and vibrational contributions to the enthalpy, respectively. E0 is the total energy at 0 K, while ZPE is the zero-point vibrational energy.

Also, for the calculation of the antioxidant parameters, the following values were employed: H(H•)vacuum=− 1312.479673 kJ/mol, H(H+)vacuum= 6.1961805 kJ/mol, and H(e−)vacuum= 3.14534924 kJ/mol, [8, 9, 30, 36].

2.3 Investigation of the thermodynamically favoured mechanism

The thermodynamically favoured mechanism is estimated by the reaction Gibbs free energy (∆rG) [2, 47]. In this light, computation of the Gibbs free energy of the reactants and products for the studied mechanisms of the reactions between the antioxidants and the two important peroxyl radicals (HOO· and CH3 − OO·) were performed.

The reaction between a free radical and an antioxidant is said to be thermodynamically favourable if the reaction Gibbs free energy is negative (Eq. 7).

$$ {\Delta }_rG=\left[G\left(\mathrm{products}\right)-G\left(\mathrm{reactants}\right)\right]<0 $$
(7)

The reaction Gibbs free energy for the HAT mechanism is given by ∆rGBDE. This was calculated as presented in Eq. 8.

$$ {\Delta }_r{G}_{\mathrm{BDE}}=\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{\bullet}\right)+G(RH)\right]-\left[G\left({H}_n\mathrm{Antiox}\right)+G\left({R}^{\bullet}\right)\right] $$
(8)

The reaction Gibbs free energy for the SET-PT mechanism is given by ∆rGAIP (Eq. 9) and ∆rGPDE (Eq. 10).

$$ {\Delta }_r{G}_{\mathrm{AIP}}=\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{\bullet +}\right)+G\left({R}^{-}\right)\right]-\left[G\left({H}_n\mathrm{Antiox}\right)+G\left({R}^{\bullet}\right)\right] $$
(9)
$$ {\Delta }_r{G}_{\mathrm{PDE}}=\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{\bullet}\right)+G(RH)\right]-\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{\bullet +}\right)+G\left({R}^{-}\right)\right] $$
(10)

Also, the reaction Gibbs free energy for the SPLET mechanism is given by ∆rGPA (Eq. 11) and ∆rGETE (Eq. 12).

$$ {\Delta }_r{G}_{\mathrm{PA}}=\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{-}\right)+G(RH)\right]-\left[G\left({H}_n\mathrm{Antiox}\right)+G\left({R}^{-}\right)\right] $$
(11)
$$ {\Delta }_r{G}_{\mathrm{ETE}}=\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{\bullet}\right)+G\left({R}^{-}\right)\right]-\left[G\left({H}_{n-1}{\mathrm{Antiox}}^{-}\right)+G\left({R}^{\bullet}\right)\right] $$
(12)

where

G(HnAntiox) = Gibbs free energy of neutral antioxidant.

G(Hn − 1Antiox•) = Gibbs free energy of phenoxyl radical.

G(R•) = Gibbs free energy of free radical.

G(RH) = Gibbs free energy of product formed by hydrogen abstraction to free radical.

G(Hn − 1Antiox•+) = Gibbs free energy of cation radical.

G(H+) = Gibbs free energy of proton.

G(R−) = Gibbs free energy of free radical anion.

G(Hn − 1Antiox−) = Gibbs free energy of anion.

In the above calculations, the values of −3.72 kJ/mol and −26.28 kJ/mol were employed as the Gibbs free energy of the electron (e−) and proton (H+) respectively [17, 42].

3 Results

4 Discussions

4.1 Virtual screening results

The predicted activities and leverage values of the designed hydrazone antioxidants are presented in Table 1. The applicability domain of the hydrazone model has a leverage threshold, h∗ value of 0.375. All the developed molecules were found within the applicability domain of the model except MHD 06, MHD 15, MHD 24, and MHD 25. Also, majority of the molecules have improved antioxidant activities compared to MHD 10 with MHD 17, MHD 21 and MHD 22 having the best pIC50 values of 6.851, 6.610 and 6.783, respectively. These molecules were subsequently selected and subjected to quantum chemical calculations in order to investigate their preferred mechanism of free radical scavenge. The molecular structure and carbon atom numbering for these three compounds are presented in Fig. 2.

Fig. 2
figure 2

Molecular structure and carbon atom numbering of MHD 017, MHD 021 and MHD 022

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4.2 Analysis of the HAT mechanism

The computed BDE results for MHD 017, MHD 021 and MHD 022 are presented in Table 2. For MHD 017, the 8-NH position has the highest BDE value of 379.156 kJ/mol. This is closely followed by the 14-OH position with a value of 373.984 kJ/mol. These high values of BDE could be attributed to the tendency of the hydrogen atoms at these positions to form intramolecular hydrogen bonds with the adjacent carbonyl group of the parent molecule. For this reason, hydrogen atom abstraction is more difficult at these positions in comparison to the other positions. Also, HAT occurs more easily at the 10-OH position since it has the lowest BDE value of 255.968 kJ/mol. A similar trend is observed for MHD 021 where the 14-NH position has the highest BDE value of 387.742 kJ/mol due to the possible formation of an intramolecular hydrogen bond with the adjacent ketone group of the parent molecule. While the 10-OH position has the lowest BDE value of 296.506 kJ/mol. Therefore HAT occurs more readily at this position. An examination of the BDE results of MHD 022 reveals that apart from the 10-OH and 14-SH positions which have lower BDE values of 305.800 kJ/mol and 307.060 kJ/mol, the 2-OH, 4-NH, 8-NH and 12-OH positions have very close and higher BDE results of 348.097 kJ/mol, 356.551 kJ/mol, 365.609 kJ/mol and 341.244 kJ/mol, respectively. Based on this result, the preferred site of free radical scavenge for MHD 022 is the 10-OH and 14-SH positions. The lower BDE value of MHD 022 14-SH against the higher values observed for MHD 017 14-OH and MHD 021 14-NH could be attributed to the less electronegative nature of sulphur in comparison to oxygen or nitrogen which form stronger intramolecular hydrogen bonds with the adjacent carbonyl group of the parent molecule. From the ongoing discussions, we observe that for MHD 017, MHD 021 and MHD 022 the lowest values of BDE occurred at the 10-OH positions on the A ring for each of the molecules with values of 255.968 kJ/mol, 296.506 kJ/mol and 305.800 kJ/mol. These results are by far lower than the BDE of phenol (327.550 kJ/mol) at the same level of theory, which is generally chosen as the reference compound. This implies that the −OH group at this position is the possible set of free radical scavenge and contributes mainly to the antioxidant activities of hydrazone derivatives through the HAT mechanism. While the −OH and −NH groups at other positions in these molecules have relatively little influence on the HAT mechanism.

Table 2 Antioxidant properties of designed hydrazone derivatives calculated at the B3LYP/6-311G* level in a vacuum
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4.3 Analysis of the spin density distribution

Apart from the magnitude of the BDE, another important factor that influences the antioxidant activity of phenolic antioxidants is the stability of the radical. The radical spin density distribution is very useful in rationalizing the stability of a given radical species [44, 45, 47]. The spin density results on the radicals of MHD 017, MHD 021 and MHD 022 are also presented in Table 2. For a given radical, the lower the spin density, the higher the delocalisation of the spin density in the radical, the easier the radical is formed, the lower the BDE. For instance, among the MHD 017, MHD 021 and MHD 022 molecule, the 10-OH radicals for each of the considered compounds have the lowest spin density values of 0.000121, 0.000181 and 0.000219, respectively. These positions also possess the lowest BDE values (Table 2). Based on these results, the radicals produced at the 10-OH position for each of these antioxidants are the most stable. This position also represents the most favoured site for free radical attack based on the HAT mechanism.

4.4 Analysis of SET-PT mechanism

The adiabatic ionization potential (AIP) and proton dissociation enthalpy (PDE) values for MHD 017, MHD 021 and MHD 022 molecules and their radicals were calculated and presented in Table 2. The first step of SET-PT mechanism is characterized by AIP. Apart from MHD 022 12-OH with an AIP value of 595.379 kJ/mol, the other scavenging sites of the considered molecules have AIP values well below that of phenol (572.776 kJ/mol at the same level of theory), which is chosen as our reference molecule (Table 2). This is an indication that the electron-donating ability of these molecules at the various considered sites is stronger than that of phenol. Also, the trend of the AIP results is significantly different from those of BDE for the considered molecules. This discrepancy could be attributed to the fact that BDE is influenced by local phenomena resulting from the various substituents in the molecule, whereas AIP results are influenced by the structure of the entire molecule (extended delocalization and conjugation of the π- electrons) [44, 45]. For MHD 017, MHD 021 and MHD 022 the lowest value of AIP is found for MHD 017 14-OH (379.878 kJ/mol), MHD 021 14-NH (342.517 kJ/mol) and MHD 022 14-SH (384.184 kJ/mol), respectively. For each of these molecules, these sites possess stronger electron-donating ability in comparison to the other sites.

The PDE characterizes the second step of the SET-PT mechanism. For each of the molecules MHD 017, MHD 021 and MHD 022, the highest values of PDE occurred at the 8-NH, 14-NH and 8-NH positions, respectively. This trend is analogous to those of BDE where these sites also record the highest values. This could be attributed to the fact that the second step of the SET-PT mechanism results in the generation of free radicals as in the HAT mechanism.

From the thermodynamic point, the first step is the most important for reactions that involve multiple-step mechanisms. Consequently, the results of AIP determine the order and magnitude in which these molecules undergo the SET-PT mechanism.

4.5 Analysis of SPLET mechanism

The proton affinity (PA) and electron transfer enthalpy (ETE) values for MHD 017, MHD 021 and MHD 022 hydrazone antioxidant molecules are presented in Table 2. The PA value is the antioxidant parameter that characterizes the first step of SPLET mechanism. The second step is characterized by ETE. For MHD 017, MHD 021 and MHD 022, the lowest observed PA values are 1352.500 kJ/mol, 1347.354 kJ/mol and 1276.256 kJ/mol which occur at the 11-NH, 10-OH and 14-SH positions, respectively. For each of these molecules, these are the most favoured sites for deprotonation to generate highly stabilized anions. PA results at these sites are also more favourable when compared with that of phenol which has a value of 1462.892 kJ/mol.

The ETE results for MHD 017, MHD 021 and MHD 022 recorded lowest values at the 13-NH, 14-NH and 4NH respectively. These are the sites that are most favoured to undergo electron transfer in the second step of the SPLET mechanism in each of the considered molecules. When the ETE results are compared with those of AIP, the ETE values are found to be lower. Accordingly, the single-electron transfer from the neutral form of the hydrazone antioxidant to the free radical is less favourable to that from the anionic form.

4.6 Thermodynamically preferred mechanism

The results of the Gibbs free energy change of reactions of inactivation of HOO· and CH3OO· via HAT, SET-PT and SPLET mechanisms by MHD 017, MHD 021 and MHD 022 molecules are presented in Tables 3 and 4, respectively. The values of the reaction Gibbs free energy (∆rG) are quite helpful in the assignment of the free radical-scavenging potency of molecules, because more negative values indicate the thermodynamically more preferred reactions. The results presented in Table 3 reveal that MHD 017 (at the 10-OH, 11-NH and 12-OH), MHD 021 (at the 10-OH) and MHD 022 (at the 10-OH and 14-SH) sites could scavenge HOO· by HAT and SPLET mechanisms because these processes are exergonic. The results at the other positions are thermodynamically unfavourable due to their endergonic nature. In the SPLET pathway, we observe that the exergonicity of ∆rGPA results overwhelm the endergonicity of the ∆rGETE results. Since a thermodynamically unfavourable reaction could be driven by a thermodynamically favourable reaction that is coupled to it, the entire SPLET mechanism is exergonic. A similar result to the HOO· scavenge is observed for the CH3OO· scavenge except for the 11-NH position of MHD 017 molecule where the reaction is endergonic (Table 4). On the basis of the exergonicity of the calculated reaction Gibbs free energy for each considered hydrazone antioxidant molecule, the 10-OH position appears to be the most efficient site for the scavenge of HOO· and CH3OO· in the studied environment via HAT and SPLET mechanisms. The Gibbs free energy of these reactions also indicates that these molecules are more efficient in scavenging HOO· than CH3OO·. On the basis of the calculated reaction free energies, MHD 017 at the 10-OH site possessed the highest free radical-scavenging potency for HOO· than CH3OO· via HAT and SPLET mechanisms. Subsequently, the radical-scavenging mechanism of this molecule by HAT and SPLET mechanisms are presented in Scheme 1(a) and (b) respectively.

Table 3 The reaction Gibbs free energy (∆rG in kJ/mol) of scavenging HOO· radical by hydrazone antioxidants at the B3LYP/6-311G* level in a vacuum
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Table 4 The reaction Gibbs free energy (∆rG in kJ/mol) of scavenging CH3OO· radical by hydrazone antioxidants at the B3LYP/6-311G* level in a vacuum
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Scheme 1
scheme 1

a HAT mechanism of MHD 017 in vacuum. b SPLET mechanism of MHD 017 in vacuum

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4.7 Analysis of frontier molecular orbitals

The results of frontier orbital distribution and energy for MHDM 017, MHDM 021 and MHDM 022 calculated at the B3LYP/6-311G* level in the gas phase are presented in Fig. 3. From Fig. 3, we observe that the LUMO is localized on ring B and its associated oxygen and nitrogen atoms in its functional groups for the three molecules. While the HOMO is delocalised almost over the entire molecules, they are observed to be highly concentrated on the nitrogen atoms of the hydrazine group. For MHDM 022, this includes the sulphur atom to which the hydrogen atom is attached. For MHDM 021, this includes the conjugated carbon atoms of ring A, and the nitrogen atom of the amino group. In all the molecules, they are equally distributed on the oxygen atoms of the hydroxyl groups. These sites with a high concentration of the HOMO possess higher tendency to lose electrons [31, 40, 44, 45]. These are the sites for free radical scavenge for the associated molecules.

Fig. 3
figure 3

The orbital distribution and energy (in eV) of HOMO and LUMO for MHD 017, MHD 021 and MHD 022 computed at the B3LYP/6-311G* level in the gas phase

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MHDM 021 has the highest HOMO value of − 5.50 eV, followed by MHDM 017 with a value of − 5.94 eV. This is closely followed by MHDM 022 with a value of − 6.00 eV. Based on this result, MHD 021 has the greatest capacity to lose electrons, because the higher the HOMO energy, the easier the electron is excited. While MHDM 022 has the weakest electron-donating ability among the considered molecules, the sequence of predicted electron-donating ability of these molecules as predicted by the HOMO energies is in very good agreement with that of the predicted AIP results (Table 2).

5 Conclusion

In this research, virtual screening by the method of quantitative structure-activity relationship was employed in the design of new hydrazone antioxidants with the earlier proposed antioxidant model for hydrazones. The structure and antioxidant activity of these compounds were successfully predicted in this work with (E)-3,5-diamino-Nˈ-(2-amino-3-ethoxy-4-hydroxy-5-nitrobenzylidene)-2,4,6-trihydroxybenzohydrazone (MHD 017) having the best antioxidant activity (pIC50 = 6.851). This demonstrates the ability of the developed hydrazone antioxidant model to reduce the time and cost of synthesizing new hydrazone antioxidants in addition to the investigation of their antioxidant activities.

The thermodynamics of three of the best antioxidants (MHD 017, MHD 021 and MHD 022) were investigated by the DFT method in the gas phase. In order to evaluate the possible mechanism of free radical scavenge by these molecules, thermodynamic parameters such as BDE, PDE, AIP, PA and ETE were calculated. The radical spin density was also calculated in order to rationalize the observed differences in the BDE results. The sequence of hydrogen donation by these molecules is MHD 017 > MHD 022 > MHD 021 and is in line with their predicted antioxidant activities. The trend of the BDE results is significantly different from those of the AIP, but analogous to those of PDE. Also, from the generated results for AIP and ETE, the single-electron transfer from the neutral form of the hydrazone antioxidant to the free radical is less favourable to that from the anionic form.

The thermodynamically preferred mechanism of reaction was investigated by calculating the reaction Gibbs free energy for inactivating HOO· and CH3OO· at the various reaction sites in each molecule. The observed results indicate that HAT and SPLET mechanisms are thermodynamically feasible at various sites in each molecule with best results observed at the 10-OH site based on the negative values of their reaction Gibbs free energy. On the other hand, the SET-PT mechanism was thermodynamically unfeasible for all the molecules as their reaction processes were endergonic. Among the tested molecules, MHD 017 which was earlier proposed to have the best antioxidant activity exhibited the highest free radical-scavenging potential against HOO· than CH3OO· at the 10-OH site upon thermodynamic studies. The present research not only did succeed in the elucidation of the free radical-scavenging mechanism of the considered hydrazone derivatives, but also will stimulate subsequent exploitation of these compounds in the field of food chemistry and pharmacy.