# Free Radical Scavenging Potency of Dihydroxybenzoic Acids

Authors: Dejan Milenković; Jelena Đorović; Svetlana Jeremić; Jasmina M. Dimitrić Marković; Edina H. Avdović; Zoran Marković
Journal: Journal of Chemistry
 (2017)

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## Abstract

In order to evaluate the free radical scavenging potency of dihydroxybenzoic acids (DHBAs) the Density Functional Theory (DFT) was used. The M05-2X/6-311++G(d,p) and B3LYP-D2/6-311++G(d,p) theoretical models were applied. Three possible antioxidant mechanisms were examined: hydrogen atom transfer (HAT), single-electron transfer followed by proton transfer (SET-PT), and sequential proton loss electron transfer (SPLET) mechanisms. All of these mechanisms have been studied in nonpolar (benzene and pentylethanoate) and polar solvents (water) using an implicit solvation model (SMD). The following thermodynamic quantities related to these mechanisms were calculated: bond dissociation enthalpy (BDE), ionization potential (IP), and proton affinity (PA). The obtained results indicated the HAT mechanism as the most favourable reaction pathway for antioxidative action of DHBAs in benzene. On the other hand, SPLET is indicated as predominant reaction mechanism in polar solvent. The SET-PT mechanism was not favourable reaction path for antioxidative action in any of the solvents under investigation.


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## Body

## 1. Introduction

Oxidative stress plays an important role in the pathogenesis of many diseases [1–5]. To neutralize the damaging effect of free radicals, the organisms often use some external factors including the dietary substances, such as phenolics, which can help in prevention of free radical damage. These substances constitute complex antioxidant defence systems. Phenolic acids are the group of the naturally occurring compounds which, besides one carboxylic acid functionality, have the common structural features as all phenolics: an aromatic ring bearing one or more hydroxyl substituents. There are two types of the phenolic acids: hydroxycinnamic (HCA) and hydroxybenzoic acids (HBA) [6, 7]. They are constituents of almost all vegetables, fruits, and grains. They can be found in the free state, but most commonly they are occurring in plant materials linked through esters, ethers, or as structural components of the cellulose, proteins, and lignins [8–10]. There is some evidence affirming multiple roles and functions of the phenolic acids and indicating these compounds as involved in processes such as the protein synthesis, nutrient uptake, enzyme activity, photosynthesis, and allelopathy [11–13]. There are also a number of the epidemiological investigations [14–17] which confirm a possible connection between the consumption of food containing phenolics and the reduced risk of developing some disorders, including cancer and cardiovascular diseases. However their in vivo role is still unknown.It has been proposed that the antioxidant activity of HBA depends on the number of hydroxyl groups in a molecule [18] and that it increases following the order: monohydroxy, dihydroxy, and trihydroxy, respectively [19]. Dihydroxybenzoic acids (DHBA) are a subclass of hydroxybenzoic acids possessing two hydroxyl groups whose relative position determines the properties of molecules. There are some experimental evidences which generally confirm good antioxidant activity of DHBAs [20, 21], especially indicating good scavenging potency of 3,4-DHBA and 2,3-DHBA. Protocatechuic acid (3,4-DHBA) is a strong antiradical and antioxidant agent which inhibits the chemical carcinogenesis and show protection against the hydroperoxide-induced toxicity [22]. Also, a few positive health attributes of 3,4-DHBA such as antibacterial [23], antimutagenic [24], anti-inflammatory, anticoagulatory [25], and antihyperglycemic [26] actions have been reported. Although all these compounds can be found in natural products there are certain findings which implicate the nonenzymatic production of 2,3-DHBA (pyrocatehuic acid), which proceeds upon trapping the hydroxyl radical by salicylic acid [27]. Moreover, pyrocatehuic acid may act as a metabolite of dioxygenases [28].As mentioned, the antioxidant ability of the phenolic acids is greatly influenced by the number and the relative position of the hydroxyl groups in the ring. It has been also suggested that the proximity of the hydroxyl groups to the acid moiety promotes the hydrogen atom transfer from the phenolic acid (PhO-H) to the radical specie. In the radical scavenging mechanisms the reactive radical specie is inactivated by accepting a hydrogen atom from a hydroxyl group of the phenolic acid. Phenolic acids can scavenge free radicals through three competitive mechanisms, which are generally influenced by the reaction conditions. The suggested mechanisms are hydrogen atom transfer (HAT, (1)), single-electron transfer followed by proton transfer (SET-PT, (2a) and (2b)), and sequential proton loss electron transfer (SPLET, (3a) and (3b)) [29–36]: (1)Ph-OH⟶Ph-O•+H•(2a)Ph-OH⟶PhOH+•+e-(2b)Ph-OH+•⟶Ph-O•+H+(3a)Ph-OH⟶Ph-O-+H+(3b)Ph-O-⟶Ph-O•+e-From the presented equations, it is clear that all these mechanisms have the same net result: formation of the corresponding phenoxyl radical which is more stable and less reactive than the free radical specie. The antioxidative mechanisms mentioned above are characterized with the thermodynamic parameters: bond dissociation enthalpy (BDE) related to (1), ionization potential (IP) related to (2a), proton dissociation enthalpy (PDE) related to (2b), proton affinity (PA) related to (3a), and electron transfer enthalpy (ETE) related to (3b).In this paper, we aimed to provide thermodynamical parameters, related to the antiradical mechanism, that can implicate the antioxidant activity of six DHBAs: 2,3-dihydroxybenzoic acid (2-pyrocatechuic acid or hypogallic acid); 2,4-dihydroxybenzoic acid (β-resorcylic acid); 2,5-dihydroxybenzoic acid (gentisic acid); 2,6-dihydroxybenzoic acid (gamma-resorcylic acid or 2,6-resorcylic acid); 3,4-dihydroxybenzoic acid (protocatechuic acid), and 3,5-dihydroxybenzoic acid (α-resorcylic acid) (Figure 1).Figure 1
Structural formulas of the examined dihydroxybenzoic acids (1,2,3,4,5, and6) with atom labeling indicated and their trivial names.


## 2. Methodology Section

All calculations were performed using Gaussian 09 program package [37], and two levels of theory were applied. The optimized geometries of the investigated dihydroxybenzoic acids and the corresponding radicals, anions, and radical cations were obtained by M05-2X method, in combination with 6-311++G(d,p) basis set [38, 39]. This hybrid functional, initially developed by Truhlar group [38], gives satisfactory results in the thermochemical and kinetic calculations and has been used widely by numerous authors [40–44].The other applied method is B3LYP-D2, developed by Grimme [45, 46]. This functional can be efficiently coupled with any existing DFT method. It is proved that this method describes the interatomic interactions at short and medium distances (≤5 Å) reliably and more accurately than the traditional DFT methods. For including a long-range dispersion contributions to the computed DFT total energy and gradients at the B3LYP level of theory [47, 48], Grimme [46] and Bayach et al. [49] used an atom-atom additive damped empirical potential of the form -fRC6/R6:(4)EB3LYP-D2=EB3LYP-EDisp,where C6 is the dispersion coefficient for the pair of atoms, R is the interatomic distance between atoms, and EDisp is the empirical term. Both M05-2X and B3LYP-D2 methods were chosen, primarily because of being widely used and secondly because these methods describe very well the interatomic interactions at short and medium distances. These methods are more reliable and accurate than traditional density function methods.Potential energy minima for all the optimized species are verified by the absence of the imaginary frequencies. Influence of water, pentylethanoate, and benzene was estimated using SMD solvation model [50]. The SMD continuum model allows the quantum mechanical approach in studying the interactions of the solvated molecules. The selected solvents enable investigating the behaviour of the molecules in polar and nonpolar environment. The delocalization effects were assessed within the NBO analysis framework [51].The thermodynamical parameters relevant for the investigated antioxidative mechanisms (BDE, IP, PDE, PA, and ETE) were calculated from total enthalpies of the optimized species using the following equations:(5)BDE=HPh-O•+HH•-HPh-OH(6a)IP=HPh-OH•++He--HPh-OH(6b)PDE=HPh-O•+HH+-HPh-OH•+(7a)PA=HPh-O-+HH+-HPh-OH(7b)ETE=HPh-O•+He--HPh-O-The recommended values of the solvation enthalpies of the protons and electrons were taken from the literature [52]. The reaction enthalpies were calculated at 298.15 K, with the temperature effects not taken into the account.


## 3. Results and Discussion

The conformational analysis of DHBAs was carried out. For this purpose, different conformations were obtained in the following way. First, two structures of each DHBA were constructed by placing the carboxyl group into two extreme positions (rotation around the C-C bond by 180°). Then, each of these structures was analysed by different orientations of hydrogen atom (antiperiplanar and synperiplanar) of different hydroxyl groups. All the rotamers of DHBAs are presented in Supplementary Material available online athttps://doi.org/10.1155/2017/5936239 (Figures S1–S6). The tables shown in Supplementary Material (Tables S1–S6) indicate the energy differences between the investigated rotamers of all the compounds under investigation. The most stable structures are presented in Figure 2.Figure 2
The most stable structures of the examined DHBAs.The structures of the all DHBAs presented in Figure2 are planar and have at least one internal hydrogen bond (IHB). Namely, compounds which possess the hydroxyl group in position C2 have IHB between hydrogen atom of the hydroxyl group and carbonyl oxygen of the carboxyl group. Compounds1 and4form one more IHB that contribute to the stability of these molecules. The oxygen atoms of the carbonyl and hydroxyl groups possess the lone electrons located in the antibonding orbitals. These lone pair-antibonding orbital interactions, between the oxygen and the adjacent O-H bonds, are responsible, as revealed by the NBO analysis, for IHB formation. The energy values presented in Tables S1–S6 confirm that the most stable rotamers are those with the highest number of IHBs, especially the ones that include IHBs with carbonyl oxygen. Also it is evident from Figure 2 that compounds4 and6 are symmetrical molecules. In further discussion only the species generated from the most stable rotamers will be discussed.


### 3.1. Radicals and Anions of DHBAs

Investigation of the antioxidant activity of DHBs was conducted to the OH groups. This restriction to the OH groups is supported by the fact that the protons of hydroxyl groups are more acidic than the proton of carboxylic group [53, 54]. The homolytic breaking of the O-H bonds in DHBAs results in formation of the radicals (Figure 3). The stability of the formed radicals, in water, plays the main role in determining the antioxidant activity of the investigated molecules. The obtained values of BDE are given in Tables 1 and 2.Table 1
M052X/6-311++G(d,p) calculated parameters of the antioxidant mechanisms for DHBAs in kJ mol−1 in all solvents under investigation.
Compounds Water Benzene Pentylethanoate HAT SET-PT SPLET HAT SET-PT SPLET HAT SET-PT SPLET BDE IP PDE PA ETE BDE IP PDE PA ETE BDE IP PDE PA ETE 1   518     673     592 2-OH 369  32 132 419 377  120 423 370 374  46 262 376 3-OH 362  25 145 405 366  109 434 356 371  35 273 341 2   550     703     622 2-OH 408  39 146 442 420  133 452 384 415  58 290 390 4-OH 401  31 129 452 392  105 401 406 392  35 244 412 3   504     658     577 2-OH 373  49 153 400 389  147 461 343 383  71 298 349 5-OH 358  34 153 386 350  108 444 321 350  38 284 331 4   521     674     593 2-OH 391  51 149 423 403  145 448 371 399  70 286 378 6-OH 380  39 137 423 381  123 423 374 379  51 264 380 5   532     693     611 3-OH 361  9 130 411 346  69 401 361 347  1 244 368 4-OH 364  12 119 425 347  70 383 380 349  3 227 386 6   537     697     613 3-OH 383  27 144 419 375  93 429 362 374  26 269 371 5-OH 382  26 143 419 374  92 427 362 374  25 268 371Table 2
B3LYP-D2/6-311++G(d,p) calculated parameters of the antioxidant mechanisms for DHBAs in kJ mol−1 in all solvents under investigation.
Compounds Water Benzene Pentylethanoate HAT SET-PT SPLET HAT SET-PT SPLET HAT SET-PT SPLET BDE IP PDE PA ETE BDE IP PDE PA ETE BDE IP PDE PA ETE 1   462     643     559 2-OH 348  37 135 364 356  102 401 344 352  44 257 346 3-OH 341  30 147 345 345  91 426 309 341  34 278 314 2   492     670     586 2-OH 386  45 151 386 397  116 431 355 392  58 286 358 4-OH 376  35 131 396 367  87 380 377 367  33 239 379 3   448     627     542 2-OH 352  56 157 346 367  130 438 319 362  71 293 320 5-OH 337  40 155 333 330  92 420 299 329  39 276 304 4   461     646     562 2-OH 367  56 148 370 382  126 427 345 378  68 281 348 6-OH 356  46 137 370 363  106 405 348 360  50 261 350 5   474     660     575 3-OH 339  16 132 358 325  54 378 337 325  2 237 340 4-OH 341  18 120 371 325  54 359 355 326  3 221 357 6   480     665     577 3-OH 361  32 147 365 353  79 407 336 353  27 263 341 5-OH 360  31 146 365 352  77 406 336 352  26 263 341Figure 3
Spin density distribution in all DHBA’s radicals in water.The stability of the formed radicals in water is decreasing in the following order:3 >5 >1 >4 >6 >2, while the order in pentylethanoate and benzene is5 >3 >1 >6 >4 >2. This result implies the homolytic cleavage of the 5-OH bond, in the polar solvent, as the favoured one in compound3, meaning that the3-R5 radical is the most stable radical of the investigated compounds. On the other hand, the homolytic cleavage of the 3-OH bond, in nonpolar solvents, is the favoured one in compound5 (5-R3).In order to rationalise the differences in BDE and consequently the differences in the reactivity of the individual OH sites the assessment of the spin density distribution was undertaken on the DHBA’s radicals. The lower BDE values implicate easier formation of the radicals and more delocalized spin density [55]. The spin density values in water, obtained by the NBO analysis, as well as SOMOs of DHBAs are depicted in Figures 3 and S7. The results show that the radicals formed from compounds3,5, and1 are the most stable. This is consequence of delocalization of their unpaired electrons over oxygen and carbons (O5, C2, C4, and C6 in3-R5; O3, C2, C4, and C6 in5-R3; and O3, C2, C4, and C6 in1-R3). The unpaired electron of5-R3 can be additionally delocalized only over the one adjacent OH group, 4-OH (Figure 3). Also, the unpaired electrons are well delocalized in radicals obtained by the homolytic cleavage of the O-H bond in other compounds (2,4, and6).The heterolytic cleavage of the O-H bond results in forming the corresponding anions. The obtained PA values of all OH groups (in compounds1–6), as well as in all solvents under investigation, presented in Tables 1 and 2, follow the sequence5-A4 >2-A4 >1-A2 >4-A6 >6-A5 >3-A5. This result implicates the proton transfer from the 4-OH group of the compound5as easier than the transfer from the other OH groups. It should be noted that the obtained PA values are significantly lower in water (polar solvent) than the other two, nonpolar, solvents (benzene and pentylethanoate). The reason for this is change of the solvent polarity, which influences the increase of PA values as the solvent polarity increases. This is a consequence of the higher solvation enthalpy of protons.The natural charge distributions of all anions, formed by heterolytic cleavage of O-H bonds of the DHBAs, are presented in Figure4. Two, the most stable, anions are obtained by deprotonation of the O-H bonds of thepara phenolic groups of compounds2 and5. The negative charges, which contribute to the stability of these anions, are delocalized over O4, C1, C3, C5, and C6 atoms in2-A4 and over O4, C1, C2, C5, and C6 atoms in5-A4. The deprotonated oxygen atom in5-A4 forms, with the neighbouring 3OH group, one hydrogen bond, which causes lower PA value and additionally contributes to the stability of this anion.Figure 4
The natural charge distributions in the most stable anions formed from the investigated DHBAs in water.


### 3.2. Free Radical Scavenging Mechanisms

As mentioned above, three mechanisms of free radical scavenging activity of DHBAs (HAT, SET-PT, and SPLET) were the subject of this study. Reaction enthalpies related to these mechanisms are calculated using (5)–(7b) and by applying two DFT methods. The values of BDE, PA, and IP are used for the estimation of the preferred mechanisms of the antiradical activity of the investigated DHBAs [56–58]. The species needed to complete the thermodynamic calculations are generated from the most stable conformation of the investigated compounds.If the calculated values obtained by both theoretical methods (Tables1 and 2) are compared, it is clear that the thermodynamic parameters calculated using the B3LYP-D2 functional are mainly lower. Having that in mind, the further discussion will refer to both used methods.From Tables1 and 2, it is clear that the IP values for all DHBAs calculated at both theoretical levels, as well as in all solvents investigated, are highly implicating SET-PT as nonoperative mechanism. On the other hand, looking at the obtained results, it is evident that in water and pentylethanoate the PA values are significantly lower than the corresponding BDE values. However, it should be pointed out that PA values are much higher in pentylethanoate than in water which indicates the SPLET mechanism as the most probable reaction pathway in those solvents. Taking into the account BDE and PA values in benzene as classical nonpolar solvent it is evident that BDE values are significantly lower than the corresponding PA values, which proves that the reaction in benzene proceeds via HAT mechanism. Further analysis of the thermodynamic values (Tables 1 and 2) indicates that compounds5 and1 have the best antioxidant activity in all solvents under investigation.The BDE values obtained for the investigated DHBAs are lower than those for phenol (406.4 and 382.8 kJ mol−1), resveratrol (368.8 and 356.2 kJ mol−1), and caffeic acid (359.9 and 342.52 kJ mol−1) [59], obtained with B3LYP method in water and benzene, as solvents. Comparing examined dihydroxybenzoic acids with the other phenolic acids, such as hydroxybenzoic acids and gallic acid [40, 41], it is clear that dihydroxybenzoic acids show quite good antioxidative properties. Among all the mentioned acids gallic acid shows the best antioxidant activity proving the significance of the number of hydroxyl groups in such activity [41]. Our results are in good accordance with previous results [40, 41, 60].


## 3.1. Radicals and Anions of DHBAs

Investigation of the antioxidant activity of DHBs was conducted to the OH groups. This restriction to the OH groups is supported by the fact that the protons of hydroxyl groups are more acidic than the proton of carboxylic group [53, 54]. The homolytic breaking of the O-H bonds in DHBAs results in formation of the radicals (Figure 3). The stability of the formed radicals, in water, plays the main role in determining the antioxidant activity of the investigated molecules. The obtained values of BDE are given in Tables 1 and 2.Table 1
M052X/6-311++G(d,p) calculated parameters of the antioxidant mechanisms for DHBAs in kJ mol−1 in all solvents under investigation.
Compounds Water Benzene Pentylethanoate HAT SET-PT SPLET HAT SET-PT SPLET HAT SET-PT SPLET BDE IP PDE PA ETE BDE IP PDE PA ETE BDE IP PDE PA ETE 1   518     673     592 2-OH 369  32 132 419 377  120 423 370 374  46 262 376 3-OH 362  25 145 405 366  109 434 356 371  35 273 341 2   550     703     622 2-OH 408  39 146 442 420  133 452 384 415  58 290 390 4-OH 401  31 129 452 392  105 401 406 392  35 244 412 3   504     658     577 2-OH 373  49 153 400 389  147 461 343 383  71 298 349 5-OH 358  34 153 386 350  108 444 321 350  38 284 331 4   521     674     593 2-OH 391  51 149 423 403  145 448 371 399  70 286 378 6-OH 380  39 137 423 381  123 423 374 379  51 264 380 5   532     693     611 3-OH 361  9 130 411 346  69 401 361 347  1 244 368 4-OH 364  12 119 425 347  70 383 380 349  3 227 386 6   537     697     613 3-OH 383  27 144 419 375  93 429 362 374  26 269 371 5-OH 382  26 143 419 374  92 427 362 374  25 268 371Table 2
B3LYP-D2/6-311++G(d,p) calculated parameters of the antioxidant mechanisms for DHBAs in kJ mol−1 in all solvents under investigation.
Compounds Water Benzene Pentylethanoate HAT SET-PT SPLET HAT SET-PT SPLET HAT SET-PT SPLET BDE IP PDE PA ETE BDE IP PDE PA ETE BDE IP PDE PA ETE 1   462     643     559 2-OH 348  37 135 364 356  102 401 344 352  44 257 346 3-OH 341  30 147 345 345  91 426 309 341  34 278 314 2   492     670     586 2-OH 386  45 151 386 397  116 431 355 392  58 286 358 4-OH 376  35 131 396 367  87 380 377 367  33 239 379 3   448     627     542 2-OH 352  56 157 346 367  130 438 319 362  71 293 320 5-OH 337  40 155 333 330  92 420 299 329  39 276 304 4   461     646     562 2-OH 367  56 148 370 382  126 427 345 378  68 281 348 6-OH 356  46 137 370 363  106 405 348 360  50 261 350 5   474     660     575 3-OH 339  16 132 358 325  54 378 337 325  2 237 340 4-OH 341  18 120 371 325  54 359 355 326  3 221 357 6   480     665     577 3-OH 361  32 147 365 353  79 407 336 353  27 263 341 5-OH 360  31 146 365 352  77 406 336 352  26 263 341Figure 3
Spin density distribution in all DHBA’s radicals in water.The stability of the formed radicals in water is decreasing in the following order:3 >5 >1 >4 >6 >2, while the order in pentylethanoate and benzene is5 >3 >1 >6 >4 >2. This result implies the homolytic cleavage of the 5-OH bond, in the polar solvent, as the favoured one in compound3, meaning that the3-R5 radical is the most stable radical of the investigated compounds. On the other hand, the homolytic cleavage of the 3-OH bond, in nonpolar solvents, is the favoured one in compound5 (5-R3).In order to rationalise the differences in BDE and consequently the differences in the reactivity of the individual OH sites the assessment of the spin density distribution was undertaken on the DHBA’s radicals. The lower BDE values implicate easier formation of the radicals and more delocalized spin density [55]. The spin density values in water, obtained by the NBO analysis, as well as SOMOs of DHBAs are depicted in Figures 3 and S7. The results show that the radicals formed from compounds3,5, and1 are the most stable. This is consequence of delocalization of their unpaired electrons over oxygen and carbons (O5, C2, C4, and C6 in3-R5; O3, C2, C4, and C6 in5-R3; and O3, C2, C4, and C6 in1-R3). The unpaired electron of5-R3 can be additionally delocalized only over the one adjacent OH group, 4-OH (Figure 3). Also, the unpaired electrons are well delocalized in radicals obtained by the homolytic cleavage of the O-H bond in other compounds (2,4, and6).The heterolytic cleavage of the O-H bond results in forming the corresponding anions. The obtained PA values of all OH groups (in compounds1–6), as well as in all solvents under investigation, presented in Tables 1 and 2, follow the sequence5-A4 >2-A4 >1-A2 >4-A6 >6-A5 >3-A5. This result implicates the proton transfer from the 4-OH group of the compound5as easier than the transfer from the other OH groups. It should be noted that the obtained PA values are significantly lower in water (polar solvent) than the other two, nonpolar, solvents (benzene and pentylethanoate). The reason for this is change of the solvent polarity, which influences the increase of PA values as the solvent polarity increases. This is a consequence of the higher solvation enthalpy of protons.The natural charge distributions of all anions, formed by heterolytic cleavage of O-H bonds of the DHBAs, are presented in Figure4. Two, the most stable, anions are obtained by deprotonation of the O-H bonds of thepara phenolic groups of compounds2 and5. The negative charges, which contribute to the stability of these anions, are delocalized over O4, C1, C3, C5, and C6 atoms in2-A4 and over O4, C1, C2, C5, and C6 atoms in5-A4. The deprotonated oxygen atom in5-A4 forms, with the neighbouring 3OH group, one hydrogen bond, which causes lower PA value and additionally contributes to the stability of this anion.Figure 4
The natural charge distributions in the most stable anions formed from the investigated DHBAs in water.


## 3.2. Free Radical Scavenging Mechanisms

As mentioned above, three mechanisms of free radical scavenging activity of DHBAs (HAT, SET-PT, and SPLET) were the subject of this study. Reaction enthalpies related to these mechanisms are calculated using (5)–(7b) and by applying two DFT methods. The values of BDE, PA, and IP are used for the estimation of the preferred mechanisms of the antiradical activity of the investigated DHBAs [56–58]. The species needed to complete the thermodynamic calculations are generated from the most stable conformation of the investigated compounds.If the calculated values obtained by both theoretical methods (Tables1 and 2) are compared, it is clear that the thermodynamic parameters calculated using the B3LYP-D2 functional are mainly lower. Having that in mind, the further discussion will refer to both used methods.From Tables1 and 2, it is clear that the IP values for all DHBAs calculated at both theoretical levels, as well as in all solvents investigated, are highly implicating SET-PT as nonoperative mechanism. On the other hand, looking at the obtained results, it is evident that in water and pentylethanoate the PA values are significantly lower than the corresponding BDE values. However, it should be pointed out that PA values are much higher in pentylethanoate than in water which indicates the SPLET mechanism as the most probable reaction pathway in those solvents. Taking into the account BDE and PA values in benzene as classical nonpolar solvent it is evident that BDE values are significantly lower than the corresponding PA values, which proves that the reaction in benzene proceeds via HAT mechanism. Further analysis of the thermodynamic values (Tables 1 and 2) indicates that compounds5 and1 have the best antioxidant activity in all solvents under investigation.The BDE values obtained for the investigated DHBAs are lower than those for phenol (406.4 and 382.8 kJ mol−1), resveratrol (368.8 and 356.2 kJ mol−1), and caffeic acid (359.9 and 342.52 kJ mol−1) [59], obtained with B3LYP method in water and benzene, as solvents. Comparing examined dihydroxybenzoic acids with the other phenolic acids, such as hydroxybenzoic acids and gallic acid [40, 41], it is clear that dihydroxybenzoic acids show quite good antioxidative properties. Among all the mentioned acids gallic acid shows the best antioxidant activity proving the significance of the number of hydroxyl groups in such activity [41]. Our results are in good accordance with previous results [40, 41, 60].


## 4. Conclusions

The generally accepted approach based on the thermodynamic parameters (BDE, IP, and PA), related to the HAT, SPLET, and SET-PT mechanisms, was applied to six dihydroxybenzoic acids, their radicals, and the corresponding radical cations and anions. Calculated energy requirements indicate thermodynamically plausible radical scavenging mechanisms. The calculations performed with two theoretical models, B3LYP-D2 and M05-2X, in polar and nonpolar solvents, proved to be in good accordance.The obtained results indicate HAT as thermodynamically favourable mechanism in benzene and SPLET in water and pentylethanoate. Calculated energy requirements indicated that compounds5 and1have better radical scavenging properties than other DHBAs.



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