Studies of the Functionalized α-Hydroxy-p-Quinone Imine Derivatives Stabilized by Intramolecular Hydrogen Bond

In this work, reactions between 6,7-dichloropyrido[1,2-a]benzimidazole-8,9-diones with different benzohydrazides were studied. Nucleophilic substitution at C(6) was followed by isomerization and led to α-hydroxy-p-quinone imine derivatives. Synthesized compounds represent a combination of several structural motifs: a benzimidazole core fused with α-hydroxy-p-quinone imine, which contains a benzamide fragment. X-ray crystallography analysis revealed the formation of dimers linked through OH···O interactions and stabilization of the imine form by strong intramolecular NH···N hydrogen bonds. The protonation/deprotonation processes were investigated in a solution using UV–Vis spectroscopy and a 1H NMR titration experiment. Additionally, the electrochemical properties of 6,7-dichloropyrido[1,2-a]benzimidazole-8,9-dione and its α-hydroxy-p-quinone imine derivative as cathode materials were investigated in acidic and neutral environments using cyclic voltammetry measurements. Cathode material based on 6,7-dichloropyrido[1,2-a]benzimidazole-8,9-dione could act as a potentially effective active electrode in aqueous electrolyte batteries; however, further optimization is required.


Introduction
Quinones and quinone derivatives are well known due to the redox activity that is important in a wide range of biological processes, such as photosynthesis [1] and cellular respiration [2].Quinones represent a class of biologically active compounds with both cytotoxic and cytoprotective effects [3].Considerable attention to redox-active compounds in general and quinones in particular [4,5] can be explained by growing demands on energy storage devices for portable electronics and renewable energy-powered vehicles [6].Quinones can potentially be used in different applications connected with energy storage due to their remarkable redox activity: as organic cathode materials for different kinds of rechargeable batteries [7], including redox flow batteries [8] and Zn-ion batteries [9], or as redox mediators in lithium-sulfur batteries [10].Physical properties of quinones can be modulated by the introduction of heteroaromatics fused with quinone cores [8] and different substituents that affect solubility [11] or affect the form of quinone fragment [12] or can facilitate binding with metal cations [13].Additionally, redox properties may be tuned to some extent by intra-and intermolecular hydrogen bonding [14].
Redox potentials, solubility, and stability in the case of small quinones can be affected by modification with electron-donating or -withdrawing functional groups or in combination with a side chain that can form hydrogen bonds.Additionally, substituted o-quinones, besides their "classical" form, can also exist in various forms [15], like quinone methides, quinone imines, and zwitterions.This ability to adopt different structures allows modulation of their properties for different applications.Despite progress in the design of quinone derivatives and their wide application as redox-active materials, limited information on molecular-level insights into the bulk properties (e.g., solubility, stability, redox activity, etc.) is available.The investigation of quinone structure at the molecular level, self-assembly in solid state, and behavior in solution will help tune the performance of quinone-functionalized materials.
An approach to modulate the redox properties of quinones is an introduction of nitrogen-containing redox-active groups (e.g., C≡N, C=N, and N=N) or incorporation of unsaturated carbon-nitrogen bonds and π-conjugated aromatic fragments [16].
This work aimed to gain an understanding of the molecular structure and behavior of unsymmetrical heterocyclic o-quinones and their derivatives bearing imine moiety.Also, electrochemical studies of selected compounds were conducted to assess their potential applications.

Results and Discussion
2.1.Synthesis and Structural Studies of Quinone Derivatives 3a-g 6,7-Dichloropyrido[1,2-a]benzimidazole-8,9-dione (1a) is a representative of unsymmetrical heterocyclic o-quinones that contains a combination of two structural motifs, an o-quinone fragment and imidazo[1,2-a]pyridine core, that possess C=N bonds (Scheme 1).It can be obtained in one-step synthesis from commercially available tetrachloro-1,4benzoquinone and 2-aminopyridine [17].During earlier studies [17][18][19], it was proved that quinone 1a and some of its derivatives are electrochemically active compounds.Investigation of the reactivity of heterocyclic quinones 1 with Cand N-nucleophiles (primary amines) indicated that the attack of the nucleophile proceeds selectively at the C(6)-position of quinone.Interestingly, obtained compounds containing different acceptor groups at the C(6)-position can exist in an o-quinone form or as p-quinone methides, depending on the introduced substituent.To expand the scope of redox-active heterocyclic o-quinone derivatives, the modification of quinone 1a with different benzohydrazides was carried out, and structural studies in solid state and solution were conducted.

Synthesis of Quinone Derivatives 3a-g
Quinone derivatives 3a-g (Scheme 1a, atoms are numbered according to ORTEP diagram, vide infra) were obtained by the nucleophilic substitution of a chlorine atom of quinone 1a,b by benzohydrazides 2a-d.Isolated compounds 3a-g have a red-orange color in the solid state.Interestingly, in the case of aminoderivatives of quinone 1 (a merocyanine on the base of the o-quinone form), deep-blue colored crystals were obtained [17,19].In general, derivatives containing aroyl hydrazine fragments were expected as a result of such substitution [15,20], and a few tautomeric structures can be supposed for the products [21,22].For the compounds obtained (3a-g), the structure determination of the quinone/substituent fragments (Scheme 1b) can explain the observed difference in color of crystals 3a-g in comparison to aminosubstituted derivatives of quinone 1a.

Single-Crystal X-ray Analysis of Quinone Derivative 3a
The use of routine identification procedures (such as 1 H-NMR and FTIR) to establish the molecular structure of compounds 3a-g left some room for doubt.To clarify the situation, crystals of compound 3a were grown from dichloromethane (DCM) solution, and their molecular structure was established using single-crystal X-ray crystallography.Crystal data and refinement details for the studied crystal are presented in Table 1. Figure 1a shows a perspective view of molecule 3a with thermal ellipsoids and the atom-numbering scheme.The p-quinone imine form was confirmed by the inspection of the bond length: bonds between C(9)=O( 23 [23]).Also, an analysis of bond lengths shows that the structure of compound 3a can be represented as a superposition of mesomeric forms.The main forms are shown in Figure 1b; at that, the non-ionized form has the highest specific weight.The molecules of compound 3a are characterized by a flattened conformation; only the phenyl group is slightly out of the plane of the heterocyclic system (the angle between planes is 5.19°).In the structure of compound 3a, intramolecular hydrogen bonds NH•••N and OH•••O were found (Figure 2).The hydroxy group of compound 3a forms bifurcated hydrogen bonds where O( 22)-H•••O( 23) is an intramolecular bond (Figure 1a) and O( 22)-H•••O'( 23) is an intermolecular one (Figure 2a).By means of these intermolecular H-bonds, the centrosymmetric  10 molecular dimers are formed in the crystal structure.Additional intermolecular interactions were found: stacking interaction between the planes of the molecules and a short intermolecular contact between heterocycle (C(3)-H) and the amide group of the substituent 2b,c).23) is an intermolecular one (Figure 2a).By means of these intermolecular Hbonds, the centrosymmetric R 2 2 (10) molecular dimers are formed in the crystal structure.Additional intermolecular interactions were found: stacking interaction between the planes of the molecules and a short intermolecular contact between heterocycle (C(3)-H) and the amide group of the substituent 2b,c).
Hirshfeld surfaces and energy framework calculations (Figures S14 and S15) were obtained in a whole-of-molecule approach using the B3LYP/6-31G(d,p) energy model implemented in CrystalExplorer 21.5 software [24].The Hirshfeld surface (shown in Figure S14, mapped with d norm ) investigation is a useful approach to establishing close contacts in a crystal.Areas of close contact are highlighted with different colors (red, white, and blue spots) to show intermolecular contacts with distances less than, equal to, and larger than van der Waal radii.As seen from the Hirshfeld surface analysis of compound 3a, bright red areas of the same size indicate strong interactions, specifically hydrogen bonds OH•••O, between neighboring molecules.Fainter red or white areas suggest relatively weak interactions involving hydrogen atoms from heterocyclic and phenyl rings and chlorine Hirshfeld surfaces and energy framework calculations (Figures S14 and S15) were obtained in a whole-of-molecule approach using the B3LYP/6-31G(d,p) energy model implemented in CrystalExplorer 21.5 software [24].The Hirshfeld surface (shown in Figure S14, mapped with dnorm) investigation is a useful approach to establishing close contacts in a crystal.Areas of close contact are highlighted with different colors (red, white, and blue spots) to show intermolecular contacts with distances less than, equal to, and larger than van der Waal radii.As seen from the Hirshfeld surface analysis of compound Energy frameworks provide an opportunity to explore the cooperative effects of intermolecular interactions in the crystal, admitting the electrostatic, dispersion, and total energy between pairs of molecules [25].In the case of the crystal of compound 3a (Figure S15), a strong stabilizing interlayer electrostatic interaction was found between molecules involved in the formation of hydrogen-bonded (O-H⋯O) dimers.On the other hand, dispersion energy was more dominant for the intercolumn stacking motif.Overall, the energy framework analysis of the crystal revealed two distinct patterns of electrostatic and dispersion energies, with each contributing similarly.

1 H NMR Spectroscopy Analysis of Quinone Derivatives 3a-g
To determine the structure of obtained products in solution compounds 3a-g, 1 H NMR spectroscopy data were analyzed, and a set of two broad signals corresponding to NH and OH protons was observed (Figures S1-S7).In the DMSO-d6 solution, signals appeared at 14.36-14.90ppm and can be assigned to the NH proton, while signals of the OH group were observed at 10.89-11.41ppm.Additionally, the 1 H NMR spectrum of compound 3a was also recorded in CDCl3 solution (a solvent in which hydrogen-bonding interactions are expected to be weaker [26]) (Figure S8), where the NH proton was found at 14.68 ppm (versus 14.71 ppm in DMSO-d6 solution).It can be concluded that a strong intramolecular bond between the NH group proton of the substituent (benzamide group at imine bond) and the nitrogen of the heterocycle (N(12)-H•••N(5)) can be found in solution as well as in a solid state (vide supra).Energy frameworks provide an opportunity to explore the cooperative effects of intermolecular interactions in the crystal, admitting the electrostatic, dispersion, and total energy between pairs of molecules [25].In the case of the crystal of compound 3a (Figure S15), a strong stabilizing interlayer electrostatic interaction was found between molecules involved in the formation of hydrogen-bonded (O-H• • • O) dimers.On the other hand, dispersion energy was more dominant for the intercolumn stacking motif.Overall, the energy framework analysis of the crystal revealed two distinct patterns of electrostatic and dispersion energies, with each contributing similarly.

1 H NMR Spectroscopy Analysis of Quinone Derivatives 3a-g
To determine the structure of obtained products in solution compounds 3a-g, 1 H NMR spectroscopy data were analyzed, and a set of two broad signals corresponding to NH and OH protons was observed (Figures S1-S7).In the DMSO-d 6 solution, signals appeared at 14.36-14.90ppm and can be assigned to the NH proton, while signals of the OH group were observed at 10.89-11.41ppm.Additionally, the 1 H NMR spectrum of compound 3a was also recorded in CDCl 3 solution (a solvent in which hydrogen-bonding interactions are expected to be weaker [26]) (Figure S8), where the NH proton was found at 14.68 ppm (versus 14.71 ppm in DMSO-d 6 solution).It can be concluded that a strong intramolecular bond between the NH group proton of the substituent (benzamide group at imine bond) and the nitrogen of the heterocycle (N( 12)-H•••N( 5)) can be found in solution as well as in a solid state (vide supra).
It is known [27] that in the case of α-hydroxyquinone derivatives, an intramolecular hydrogen bond was observed, and an OH proton signal appears at 7.30 ppm in the CDCl 3 solution.For compound 3a, a distinguishable shift was observed for the OH proton signal in the CDCl 3 solution (7.20 ppm) in comparison to the DMSO-d 6 solution (10.99 ppm), which can indicate the formation of the additional intermolecular interactions between the OH group and a solvent (DMSO-d 6 ) with hydrogen bond acceptor abilities [28].
Moreover, the introduction of various substituents in the phenyl ring (benzamide fragment) showed the linear correlation (Figure S9) between the type of substituent group (represented by the Hammett constant [29] (Table S1)) and OH signal shift in the sets of compounds 3a-c (R 1 = H) and 3e-g (R 1 = NO 2 ).The shift of the OH signal correlates well (R 2 = 0.99) with the increasing electron-withdrawing character of the substituent group for both sets of compounds (Figure S9).The presence of an electron-withdrawing group (EWG) at the heterocyclic fragment (R 1 = NO 2 ) led to a downfield shift in the OH signal compared to molecules without any substituent (R 1 = H) on that ring (∆δ OH ≈ 0.3 ppm).
The most downfield signal of the NH proton (14.90 ppm in DMSO-d 6 solution) in the 1 H NMR spectra was observed for compound 3c with a NO 2 group at the phenyl ring (R 2 at benzamide fragment).The most upfield signal of the NH proton (14.36 ppm) was found for compound 3f with a NO 2 group at the heterocyclic fragment (R 1 ) and electron-donating group at the phenyl ring (R 2 = OMe).Well-defined linear correlations between the Hammett substituent constant and the NH signal are presented in Figure S9.The variation in the electronic character of the substituent in the para-position of the phenyl ring showed the same trend for compounds 3a-c (R 2 = 0.96) and 3e-g (R 2 = 0.99), leading to the downfield shift of the NH signal going from an electron-donating to electron-withdrawing group.Interestingly, the presence of EWG (R 1 = NO 2 ) at the heterocyclic ring caused the NH signal upfield shift (∆δ NH ≈ 0.3 ppm) compared to a molecule where the same position has a hydrogen atom (R 1 = H).In general, the more downfield shifted the NH proton signal, the stronger the intramolecular H-bond [30].Thus, EWG at the phenyl ring (R 2 = NO 2 ) increases the acidity of the NH proton and increases the intramolecular H-bond strength, but EWG at the heterocyclic fragment (R 1 = NO 2 ) influences the electron density at N(5), affecting intramolecular H-bond in turn.
In the case of compounds 3a-g, the moiety at the C(6) position can be described as a structural analog of aroyl hydrazone (a different approach [22] to the naming of quinone imine derivatives was observed).A well-known characteristic of compounds containing the carbon-nitrogen double bond is the ability to undergo E/Z isomerization in the solution activated by light and/or chemical inputs [31,32].
Compounds 3a and 3b were chosen for the investigation of the isomerization process.In general, in the case of E/Z isomerization, an additional set of signals [33,34] is expected to appear.No signals of the second form (isomerization products) were observed in the 1 H NMR spectra of compound 3a either in DMSO-d 6 or in CDCl 3 solution.Also, in the case of compound 3b, configurational switching was not induced by the addition of excess trifluoracetic acid (TFA) and following irradiation by UV light (365 nm; irradiation by a high-pressure mercury lamp at room temperature) judging from the 1 H NMR spectra of compound 3b in DMSO-d 6 solution (Figure S10).The formation of a strong intramolecular hydrogen bond N(12)-H•••N(5) can explain the existence of a single configuration of substituted imine that agrees with the stabilization of only one form in the presence of an intramolecular hydrogen bond.Additional stabilization of the molecule may be explained by excitation energy dissipation caused by zwitterionic structure.
It is known [35] that for redox properties tests (fabrication of electrodes), a mixture of an organic compound, a conductive additive, and a binder is often prepared using N-methyl-2-pyrrolidone (NMP) [36] as a solvent (strongly basic solvent) [37].This fact prompted us to investigate the influence of the base on the structure of the products 3a-g.
During preliminary solubility tests of compounds 3a-g, the color change (from yellow to green or blue) was observed in NMP solution or in the presence of a base.For a better understanding of the effect, a few 1 H NMR experiments were carried out.Upon addition of an excess of the base (1,8-diazabicyclo(5.4.0)undec-7-ene,DBU), the 1 H NMR spectrum of compound 3b in DMSO-d 6 solution showed some changes (Figure 3): the signal of OH proton completely disappeared; the sharpened signal of the NH proton (the sharp line can indicate a dynamically stable state) shifted upfield.Additionally, a new minor proton signal at 13.44 ppm was observed.Simultaneously, the yellow-colored solution of compound 3b became dark blue.It should be noted that the same deprotonation behavior was observed for compound 3a in CDCl 3 solution (Figure S11).After the excess TFA was added, the solution became yellow again, a minor signal at 13.44 ppm disappeared, and the signal of the OH proton was restored.It can be concluded that deprotonation provides the formation of an anionic polymethine dye structure [38] (blue), and protonation restores quinone imine form (yellow); consequently, the equilibrium between the two forms is reversible.deprotonation behavior was observed for compound 3a in CDCl3 solution (Figure S11).After the excess TFA was added, the solution became yellow again, a minor signal at 13.44 ppm disappeared, and the signal of the OH proton was restored.It can be concluded that deprotonation provides the formation of an anionic polymethine dye structure [38] (blue), and protonation restores quinone imine form (yellow); consequently, the equilibrium between the two forms is reversible.To gain more information about the deprotonation process of compound 3b, a 1 H NMR titration experiment was carried out.As shown in Figure 4, in the case of compound 3b deprotonation upon sequential addition of the base (DBU), the 1 H NMR spectra reveal several features.The broad signal of the OH proton vanished upon the addition of only 0.15 equivalents of the base, which can be explained by the dynamical process as well; color changes were immediate (Figure 4, highlighted in yellow).The signal of the NH proton (benzamide fragment) sharpens and undergoes an upfield shift from 14.70 to 14.51 ppm (Figure 4, highlighted in red).To gain more information about the deprotonation process of compound 3b, a 1 H NMR titration experiment was carried out.As shown in Figure 4, in the case of compound 3b deprotonation upon sequential addition of the base (DBU), the 1 H NMR spectra reveal several features.The broad signal of the OH proton vanished upon the addition of only 0.15 equivalents of the base, which can be explained by the dynamical process as well; color changes were immediate (Figure 4, highlighted in yellow).The signal of the NH proton (benzamide fragment) sharpens and undergoes an upfield shift from 14.70 to 14.51 ppm (Figure 4, highlighted in red).A new signal appeared at 9.58 ppm (+0.15 eqv. of DBU) (Figure 4, highlighted in green), which can be explained by the formation of a hydrogen-bonded complex of protonated DBU ( 1 H NMR spectrum of DBU and TFA mixture in DMSO-d6 solution was recorded; the NH + signal appears at 9.69 ppm (Figure S12)) with the deprotonated compound 3b.Upon further addition of the base, this signal was broadened and shifted downfield (9.86 ppm) due to the interaction of protonated DBU (DBUH + ) with the anionic compound 3b through the N-H bond [39].
Upon addition of more than 1.05 eqv. of the base, a second minor form of the compound appears (Figure 4, highlighted in blue); the ratio between major and minor forms is 0.95:0.05,taking into consideration the signals of all protons.Moreover, the addition of an excess amount of the base (4 and 8 eqv.) did not result in the change of the 1 H NMR spectra of compound 3b (additional processes as a function of the time and/or temperature in the solution should not be excluded as 1 H NMR titration experiment was carried out within an hour after addition of DBU to the compound 3b at room temperature (T = 294 K)).
Also, the presence of two different species (one major and one minor) was detected from the changes in the 1 H NMR spectra of compounds 3a and 3c upon deprotonation with DBU in DMSO-d6 solution (after mixed with more than 1 equivalent of DBU).For compound 3a, the 1 H NMR spectrum was also recorded in the presence of NaOH.As a result, the acquired spectrum was identical to the one with an excess of DBU (Figure S13).
Unfortunately, the low solubility of compounds 3a-g limited the possibility of obtaining qualitative 13 C NMR spectra.

Electronic Absorption
The UV-Vis absorption spectra of compound 3a were investigated in solution using A new signal appeared at 9.58 ppm (+0.15 eqv. of DBU) (Figure 4, highlighted in green), which can be explained by the formation of a hydrogen-bonded complex of protonated DBU ( 1 H NMR spectrum of DBU and TFA mixture in DMSO-d 6 solution was recorded; the NH + signal appears at 9.69 ppm (Figure S12)) with the deprotonated compound 3b.Upon further addition of the base, this signal was broadened and shifted downfield (9.86 ppm) due to the interaction of protonated DBU (DBUH + ) with the anionic compound 3b through the N-H bond [39].
Upon addition of more than 1.05 eqv. of the base, a second minor form of the compound appears (Figure 4, highlighted in blue); the ratio between major and minor forms is 0.95:0.05,taking into consideration the signals of all protons.Moreover, the addition of an excess amount of the base (4 and 8 eqv.) did not result in the change of the 1 H NMR spectra of compound 3b (additional processes as a function of the time and/or temperature in the solution should not be excluded as 1 H NMR titration experiment was carried out within an hour after addition of DBU to the compound 3b at room temperature (T = 294 K)).
Also, the presence of two different species (one major and one minor) was detected from the changes in the 1 H NMR spectra of compounds 3a and 3c upon deprotonation with DBU in DMSO-d 6 solution (after mixed with more than 1 equivalent of DBU).For compound 3a, the 1 H NMR spectrum was also recorded in the presence of NaOH.As a result, the acquired spectrum was identical to the one with an excess of DBU (Figure S13).
Unfortunately, the low solubility of compounds 3a-g limited the possibility of obtaining qualitative 13 C NMR spectra.

Electronic Absorption
The UV-Vis absorption spectra of compound 3a were investigated in solution using solvents of various polarities (DCM and DMSO).Two absorption maxima were found at 381 nm and at 446-449 nm in the absorption spectra of compound 3a in both solutions (Figure 5a), which can be attributed to the neutral form of the compound.Upon addition of the base (DBU) to the DCM solution of 3a, the solution instantaneously turned violet, and the absorption revealed a broad band centered at 556 nm.When a base was added to the DMSO solution of compound 3a, the bathochromic shift was observed with an absorption maxima at 607 nm accompanied by a blue coloration.The effect of substituents (R1 and R2) on the longwave absorption maximum was examined when DBU was added to the initial solution of compounds 3a-c (variable R2 while R1 = H) and 3e-g (variable R2 while R1 = NO2) in CHCl3 (Figure S16, Table S2).It was noticed that the longwave absorption band of deprotonated species of derivatives 3e-g was red-shifted (λ = 569-578 nm) in comparison to compounds 3a-c (λ = 556-563 nm).This observation can be explained by the influence of the electron-withdrawing substituent at C(2) on the electron distribution in the heterocyclic fragment.Moreover, a hyperchromic effect was caused by the introduction of the nitro group in the benzamide fragment (compound 3c in Figure 5b; compounds 3c and 3g in Figure S16).

Electrochemistry/Redox Chemistry Studies of Quinone Derivatives 1a and 3a
Quinone imines contain structural fragments with potentially high redox activity.It was shown by Almeida, R. et al. [40] that p-quinone imines are known to undergo a redox cycle through aminophenols [41].Compound 1a was previously proved to be electrochemically active [42] when dissolved in the MeCN solution.However, it has not been tested as a cathode material before.To analyze the redox properties of quinone imine 3a in comparison to initial o-quinone 1a, open-circuit potential (OCP) and cyclic voltammetry (CV) measurements in a solid state were carried out.Preliminary solubility tests showed limited solubility of compounds 1a and 3a in aqueous media; compound 1a was insoluble in water (whole pH range), and at the same time, compound 3a was insoluble in neutral and acidic environments.

Open-Circuit Potential Measurements
To analyze the electrochemical properties of the compounds, CV measurements and OCP measurements before and after CV were performed (Figure S17).Cathode materials CM-1a and CM-3a were prepared by combining compounds 1a and 3a with Vulcan XC72 CB, respectively (the detailed sample preparation is described in the Experimental section).The OCP of freshly assembled half-cells for cathode materials CM-1a and CM-3a in the acidic (0.5 M H2SO4) electrolyte was 0.44 V and 0.37 V vs. Ag/AgCl; however, in a neutral (0.5 M K2SO4) electrolyte, the potentials of both were 0.28 V vs. Ag/AgCl.After The effect of substituents (R 1 and R 2 ) on the longwave absorption maximum was examined when DBU was added to the initial solution of compounds 3a-c (variable R 2 while R 1 = H) and 3e-g (variable R 2 while R 1 = NO 2 ) in CHCl 3 (Figure S16, Table S2).It was noticed that the longwave absorption band of deprotonated species of derivatives 3e-g was red-shifted (λ = 569-578 nm) in comparison to compounds 3a-c (λ = 556-563 nm).This observation can be explained by the influence of the electron-withdrawing substituent at C(2) on the electron distribution in the heterocyclic fragment.Moreover, a hyperchromic effect was caused by the introduction of the nitro group in the benzamide fragment (compound 3c in Figure 5b; compounds 3c and 3g in Figure S16).

Electrochemistry/Redox Chemistry Studies of Quinone Derivatives 1a and 3a
Quinone imines contain structural fragments with potentially high redox activity.It was shown by Almeida, R. et al. [40] that p-quinone imines are known to undergo a redox cycle through aminophenols [41].Compound 1a was previously proved to be electrochemically active [42] when dissolved in the MeCN solution.However, it has not been tested as a cathode material before.To analyze the redox properties of quinone imine 3a in comparison to initial o-quinone 1a, open-circuit potential (OCP) and cyclic voltammetry (CV) measurements in a solid state were carried out.Preliminary solubility tests showed limited solubility of compounds 1a and 3a in aqueous media; compound 1a was insoluble in water (whole pH range), and at the same time, compound 3a was insoluble in neutral and acidic environments.

Open-Circuit Potential Measurements
To analyze the electrochemical properties of the compounds, CV measurements and OCP measurements before and after CV were performed (Figure S17).Cathode materials CM-1a and CM-3a were prepared by combining compounds 1a and 3a with Vulcan XC72 CB, respectively (the detailed sample preparation is described in the Experimental section).The OCP of freshly assembled half-cells for cathode materials CM-1a and CM-3a in the acidic (0.5 M H 2 SO 4 ) electrolyte was 0.44 V and 0.37 V vs. Ag/AgCl; however, in a neutral (0.5 M K 2 SO 4 ) electrolyte, the potentials of both were 0.28 V vs. Ag/AgCl.After the CV measurements, the OCP of sample half-cells stabilized.For both samples in the acidic electrolyte, they were 0.41 V vs. Ag/AgCl, and in the neutral electrolyte, they were 0.37 V vs. Ag/AgCl.The OCP for both samples is approximately the same, and with decreasing pH, there is a visible shift to higher potential values going from neutral to the acidic electrolyte.

Cyclic Voltammetry Measurements
CV results for samples CM-1a, CM-3a, and a sample without active material (substrate) in neutral and acidic electrolytes at varying scanning speeds are shown in Figure 6.For the substrate in neutral electrolyte, no visible redox processes were observed.In the acidic electrolyte, a hydrogen evolution reaction can be observed around the potential of −0.3 V vs. Ag/AgCl and one insignificant redox process at faster scan rates around 0.3 V vs. Ag/AgCl.However, when scanning samples with active materials, this substrate process cannot be observed and, therefore, has no electrochemical significance other than providing electrical conductivity.CV results for samples CM-1a, CM-3a, and a sample without active material (substrate) in neutral and acidic electrolytes at varying scanning speeds are shown in Figure 6.For the substrate in neutral electrolyte, no visible redox processes were observed.In the acidic electrolyte, a hydrogen evolution reaction can be observed around the potential of −0.3 V vs. Ag/AgCl and one insignificant redox process at faster scan rates around 0.3 V vs. Ag/AgCl.However, when scanning samples with active materials, this substrate process cannot be observed and, therefore, has no electrochemical significance other than providing electrical conductivity.For sample CM-3a in a neutral electrolyte (Figure 6), no significant redox processes can be observed.Also, in an acidic electrolyte for sample CM-3a (Figure 6), there are no significant processes; however, upon closer inspection (Figure S18), two reversible oxidation (at 0.40 V and 0.07 V vs. Ag/AgCl) and reduction processes (at 0.23 V and −0.06 V vs. Ag/AgCl) can be seen.
Sample CM-1a has two redox maxima in the scanned potential window from −0.4 V to 1.0 V vs. Ag/AgCl electrode in both neutral and acidic electrolytes (Figure 6).In a neutral electrolyte (Figure S19), oxidation peaks are at 0.27 V and 0.10 V vs. Ag/AgCl; however, reduction peaks are at 0.14 V and −0.32 V vs. Ag/AgCl.In addition, the oxidation peaks are found at 0.48 V and 0.26 V vs. Ag/AgCl and reduction peaks at 0.40 V and 0.23 V vs. Ag/AgCl in an acidic electrolyte (Figure S20).This indicates a shift in reaction potential to more positive values by increasing H + ion concentration and thus lowering the pH level of the electrolyte.Both redox processes for sample CM-1a correspond to the o-quinone fragment in the molecule.However, by comparing the electrochemical performance of both samples CM-1a and CM-3a, it can be concluded that by converting o-quinone 1a to α-hydroxy-p-quinone imine 3a accompanied by the additional stabilization by intra-and intermolecular hydrogen bonds, the electrochemical reactivity of the cathode material has been greatly suppressed.
All CV measurement result developments in time can be seen in Figure S21.At the For sample CM-3a in a neutral electrolyte (Figure 6), no significant redox processes can be observed.Also, in an acidic electrolyte for sample CM-3a (Figure 6), there are no significant processes; however, upon closer inspection (Figure S18), two reversible oxidation (at 0.40 V and 0.07 V vs. Ag/AgCl) and reduction processes (at 0.23 V and −0.06 V vs. Ag/AgCl) can be seen.
Sample CM-1a has two redox maxima in the scanned potential window from −0.4 V to 1.0 V vs. Ag/AgCl electrode in both neutral and acidic electrolytes (Figure 6).In a neutral electrolyte (Figure S19), oxidation peaks are at 0.27 V and 0.10 V vs. Ag/AgCl; however, reduction peaks are at 0.14 V and −0.32 V vs. Ag/AgCl.In addition, the oxidation peaks are found at 0.48 V and 0.26 V vs. Ag/AgCl and reduction peaks at 0.40 V and 0.23 V vs. Ag/AgCl in an acidic electrolyte (Figure S20).This indicates a shift in reaction potential to more positive values by increasing H + ion concentration and thus lowering the pH level of the electrolyte.Both redox processes for sample CM-1a correspond to the o-quinone fragment in the molecule.However, by comparing the electrochemical performance of both samples CM-1a and CM-3a, it can be concluded that by converting o-quinone 1a to α-hydroxy-p-quinone imine 3a accompanied by the additional stabilization by intra-and intermolecular hydrogen bonds, the electrochemical reactivity of the cathode material has been greatly suppressed.
All CV measurement result developments in time can be seen in Figure S21.At the start, samples were cycled at the potential window of −0.4 V to 1.0 V vs. Ag/AgCl reference electrode.Observations indicate that all samples go through the surface activation phase, where the sample-specific capacity increases with each subsequent cycle.During the measurements at different scanning speeds, the stabilization of the system is observed.However, sample CM-1a in neutral electrolyte goes through an irreversible oxidation process at 0.11 V vs. Ag/AgCl and a reduction process at −0.32 V vs. Ag/AgCl.This irreversible redox process can be observed during all scan speeds.At an increased potential window (from −1.0 V to 1.5 V), another irreversible process at a scan speed of 0.1 V/s for sample CM-1a in a neutral electrolyte can be observed during the oxidation at −0.31 V and reduction at −0.56 V vs. Ag/AgCl.A slight capacity decrease due to the possible dissolution of active materials can be observed for sample CM-3a in a neutral electrolyte and sample CM-1a in an acidic electrolyte.

Raman Measurements
Raman measurements were performed on pure compounds 1a and 3a, prepared cathodes (CM-1a and CM-3a), and after cycling them in acidic and neutral electrolytes (Figure 7).For sample CM-3a, the spectra for prepared and cycled cathodes remain as for pure compound 3a, where an amide band can be seen at 1600-1630 cm −1, as well as bands for aromatic/heteroaromatic rings at 1550 and 1470 cm −1 [43].This indicates that compound 3a was preserved in the cathode-forming process and did not go through any chemical changes.Also, after CV measurements, the active material is unchanged and present in the samples.For sample CM-1a, the spectra for the prepared and cycled cathode in an acidic electrolyte remain as for pure compound 1a (bands for aromatic/heteroaromatic rings at 1570 and 1450 cm −1 and band for carbonyl groups at 1650-1690 cm −1 ) [43].However, for cathode CM-1a cycled in neutral electrolyte, only C and D bands of carbon [44,45] can be seen.Since redox processes are visible for this sample in CV measurements (Figure 6), the active material could have dissolved from the electrode in the electrolyte and gone through the electrochemical reactions from the electrolyte.
Molecules 2024, 29, x FOR PEER REVIEW 12 of 20 irreversible redox process can be observed during all scan speeds.At an increased potential window (from −1.0 V to 1.5 V), another irreversible process at a scan speed of 0.1 V/s for sample CM-1a in a neutral electrolyte can be observed during the oxidation at −0.31 V and reduction at −0.56 V vs. Ag/AgCl.A slight capacity decrease due to the possible dissolution of active materials can be observed for sample CM-3a in a neutral electrolyte and sample CM-1a in an acidic electrolyte.

Raman Measurements
Raman measurements were performed on pure compounds 1a and 3a, prepared cathodes (CM-1a and CM-3a), and after cycling them in acidic and neutral electrolytes (Figure 7).For sample CM-3a, the spectra for prepared and cycled cathodes remain as for pure compound 3a, where an amide band can be seen at 1600-1630 cm −1, as well as bands for aromatic/heteroaromatic rings at 1550 and 1470 cm −1 [43].This indicates that compound 3a was preserved in the cathode-forming process and did not go through any chemical changes.Also, after CV measurements, the active material is unchanged and present in the samples.For sample CM-1a, the spectra for the prepared and cycled cathode in an acidic electrolyte remain as for pure compound 1a (bands for aromatic/heteroaromatic rings at 1570 and 1450 cm −1 and band for carbonyl groups at 1650-1690 cm −1 ) [43].However, for cathode CM-1a cycled in neutral electrolyte, only C and D bands of carbon [44,45] can be seen.Since redox processes are visible for this sample in CV measurements (Figure 6), the active material could have dissolved from the electrode in the electrolyte and gone through the electrochemical reactions from the electrolyte.

Scanning Electron Microscopy Measurements
Scanning electron microscopy examinations of compounds 1a and 3a (Figure S22) were performed to assess the morphology of the products.Compound 1a consists of needle-like particles with sizes ranging from 1 µm to 10 µm in diameter and 3 µm to 30 µm in length.Compound 3a has smaller particles with an overall size of 1 µm in diameter and 5-20 µm in length.
Also, the prepared cathode surfaces with and without active materials before and after cyclic voltammetry are shown in Figure 8.The resemblance of the structures of compounds 1a and 3a (as shown in Figure S22) can be seen in the images of cathode disks (samples CM-1a and CM-3a in Figure 8) before CV measurements.For sample CM-3a,

Scanning Electron Microscopy Measurements
Scanning electron microscopy examinations of compounds 1a and 3a (Figure S22) were performed to assess the morphology of the products.Compound 1a consists of needle-like particles with sizes ranging from 1 µm to 10 µm in diameter and 3 µm to 30 µm in length.
Compound 3a has smaller particles with an overall size of 1 µm in diameter and 5-20 µm in length.
Also, the prepared cathode surfaces with and without active materials before and after cyclic voltammetry are shown in Figure 8.The resemblance of the structures of compounds 1a and 3a (as shown in Figure S22) can be seen in the images of cathode disks (samples CM-1a and CM-3a in Figure 8) before CV measurements.For sample CM-3a, these structures can also be seen in images after CV in neutral and acidic electrolytes with some partial dissolution in an acidic electrolyte, as fewer structures can be seen.The formation of non-covalent interactions between compound 3a and substrate can probably explain the greater stability of CM-3a in comparison to CM-1a.However, for sample CM-1a cycled in neutral and acidic electrolytes, only a few original structures can be seen.This correlates with findings from Raman spectroscopy (Figure 7b) that the active material 1a dissolves in a neutral electrolyte and goes through electrochemical reactions from it.
Molecules 2024, 29, x FOR PEER REVIEW 13 of 20 explain the greater stability of CM-3a in comparison to CM-1a.However, for sample CM-1a cycled in neutral and acidic electrolytes, only a few original structures can be seen.This correlates with findings from Raman spectroscopy (Figure 7b) that the active material 1a dissolves in a neutral electrolyte and goes through electrochemical reactions from it.

Materials and Instrumentation
Polyvinylidene fluoride (PVDF) (MW ~530,000) and Dimethylformamide (DMF) were purchased from Merck; Vulcan XC72 Carbon Black (CB) was used, and 0.05 mm thick conductive graphite paper (RERAS, purchased from China and used as electrode substrate) was used to prepare cathode materials.
Melting points were measured on a Kruess KSP 11 Melting Point Analyzer. 1 H NMR spectra were recorded on a Brucker Avance spectrometer at 300 or 500, respectively, in DMSO-d6 or CDCl3 solutions.Chemical shifts were expressed in parts per million (δ, ppm) relative to solvent signal (DMSO-d6: 2.50 ppm CDCl3: 7.26 ppm for 1 H NMR) [46].Compounds 3a-g are too insoluble to record a qualitative 13 C NMR spectrum.Elemental CHN analysis was carried out on a Euro Vector EA 3000 analyzer.FTIR spectra were recorded on a Perkin-Elmer Spectrum 100 FTIR spectrometer.The UV-Vis absorption spectra were acquired with a Perkin-Elmer 35 UV/Vis spectrometer using 1 cm length quartz cuvettes with a concentration of compound c = 2.5 × 10 −5 M. Low-resolution mass spectra were acquired on a Waters EMD 1000MS mass detector (ESI + mode, voltage 30 V) with an Xterra MS C18 5 µm 2.1 × 100 mm column and gradient eluent mode using 0.1% HCOOH in deionized water and MeCN or MeOH.

Materials and Instrumentation
Polyvinylidene fluoride (PVDF) (MW ~530,000) and Dimethylformamide (DMF) were purchased from Merck; Vulcan XC72 Carbon Black (CB) was used, and 0.05 mm thick conductive graphite paper (RERAS, purchased from China and used as electrode substrate) was used to prepare cathode materials.
Melting points were measured on a Kruess KSP 11 Melting Point Analyzer. 1 H NMR spectra were recorded on a Brucker Avance spectrometer at 300 or 500, respectively, in DMSO-d 6 or CDCl 3 solutions.Chemical shifts were expressed in parts per million (δ, ppm) relative to solvent signal (DMSO-d 6 : 2.50 ppm CDCl 3 : 7.26 ppm for 1 H NMR) [46].Compounds 3a-g are too insoluble to record a qualitative 13 C NMR spectrum.Elemental CHN analysis was carried out on a Euro Vector EA 3000 analyzer.FTIR spectra were recorded on a Perkin-Elmer Spectrum 100 FTIR spectrometer.The UV-Vis absorption spectra were acquired with a Perkin-Elmer 35 UV/Vis spectrometer using 1 cm length quartz cuvettes with a concentration of compound c = 2.5 × 10 −5 M. Low-resolution mass spectra were acquired on a Waters EMD 1000MS mass detector (ESI + mode, voltage 30 V) with an Xterra MS C18 5 µm 2.1 × 100 mm column and gradient eluent mode using 0.1% HCOOH in deionized water and MeCN or MeOH.

X-ray Crystallography Analysis
For compound 3a, diffraction data were collected at a low temperature (T = 150.0(1)K) on Rigaku, XtaLAB Synergy, Dualflex, HyPix diffractometer using copper monochromated Cu-Kα radiation (λ = 1.54184Å).The crystal structure was solved with the help of the ShelXT structure solution program [47] using the Intrinsic Phasing solution method.The model was refined with version of the program olex2.refine using Levenberg-Marquardt minimization [48].All nonhydrogen atoms were refined in anisotropical approximation.For further details, see crystallographic data for compound 3a deposited at the Cambridge Crystallographic Data Centre as Supplementary Publications Numbers CCDC 2238663 (for compound 3a).These data can be obtained free of charge via https://www.ccdc.cam.ac.uk/structures/ (accessed on 1 April 2024) or from the CCDC, 12 Union Road, Cambridge CB2 1EZ, U.K.; Fax: +44 1223 336033; e-mail: deposit@ccdc.cam.ac.uk).For crystal packing visualization, the program Mercury [49] was used.

Cathode Material Preparation
Quinone derivatives 1a or 3a were combined with Vulcan XC72 CB at a mass ratio of 5:4.The resulting powder was dried overnight at 80 • C.Then, a binder solution of PVDF:DMF (mass ratio 1:9) was added so the quinone to PVDF mass ratio would be 5:1.Stirring and ultra-sonication were used to create the ink slurry.Extra DMF was added to the slurry to form homogeneous ink (the total weight ratio of DMF to quinone was approximately 12:1).A manual doctor blade coater (with a 25 µm gap size) was employed to apply the coating onto carbon paper that was pre-dried at 120 • C for an hour.Coated cathode substrates were then dried in air to evaporate DMF.For further material characterization, cathode disks were cut out using a hollow punch.

Cyclic Voltammetry
To analyze the electrochemical properties of the different sample compounds, cyclic voltammetry (CV) measurements were performed using a 3-electrode measuring cell "TSC Surface" (from rhd instruments).For different measurements, the prepared thinlayer electrodes on carbon paper (with or without compound 1a or 3a) were used as working electrodes placed in 1 mL of electrolyte with the platinum counter electrode and Ag/AgCl (3 M KCl) reference electrode.Two different pH electrolyte solutions were used for measurements: neutral 0.5 M K 2 SO 4 and acidic 0.5 M H 2 SO 4 solutions.The CV measurements were performed from −0.4 to +1.0 V with the following program: (1) opencircuit measurement (OCP) of freshly assembled half-cell before the CV measurements; (2) ten cycles with scan speed of 0.075 V/s to stabilize the half-cell; (3) 5 cycles of 5 scans with scan rates ranging from 0.005 V/s to 0.1 V/s; and (4) OCP measurement after CV.

Raman Spectroscopy
Raman measurements were performed using a Renishaw In-ViaV727 spectrometer in a backscattering geometry at room temperature at 100× magnification.For phonon excitation, a red laser (He-Ne, λ = 633 nm, grating-1200 mm −1 , 125 µW) was used, and the sample exposure time was 10 s.

Conclusions
To summarize, a set of heterocyclic α-hydroxy-p-quinone imine derivatives was obtained via one-step nucleophilic substitution of 6,7-dichloropyrido[1,2-a]benzimidazole-8,9-diones 1a,b with different benzohydrazides 2a-d followed by isomerization.The α-Hydroxy-p-quinone imine form of the synthesized products was proved by X-ray crystallography analysis of compound 3a.The formation of a strong intramolecular hydrogen bond N(12)-H•••N(5) in a solid state and in solution can explain the stabilization of only one configuration of the C=N bond of the substituted imine.The 1 H NMR acid-base titration experiment showed that deprotonation/protonation processes are reversible.Deprotonation led to the electronic delocalization in the molecule, which is accompanied by distinct changes in the UV-Vis spectra.
Sample CM-1a has a distinct maximum of two redox reactions.In an acidic environment, both peaks are stable, while in a neutral environment, only one of them is stable and remains unchanged after several CV cycles.Moreover, for the stable redox reactions, the potential difference is only up to 0.2 V.This indicates that the sample CM-1a could act as an effective active electrode in aqueous electrolyte batteries.However, the dissolution of the sample in the electrolyte was observed, so the potential application as cathode material for aqueous batteries would require compound 1a to be attached to the polymer backbone.
Attempts to modulate redox properties by incorporation of additional unsaturated carbon-nitrogen bonds to the heterocyclic quinone 1a structure led to changes in the redoxactive fragment and the formation of p-quinone imine 3a.As a result, the electrochemical behavior is changed, as it is no longer possible to observe pronounced redox peaks in CV measurements.Structural changes of the quinone fragment (probably induced by the formation of intramolecular H-bond) decreased the redox activity of the derivative despite the introduction of an additional C=N bond; at the same time, the introduced substituent enhanced the stability of the cathode material, which was confirmed by Raman spectroscopy measurements.Therefore, further structure optimizations for the elaboration of effective cathode material should include the analysis of the possible tautomerization, the formation of intramolecular H-bonds, the effect of substituents and interaction with basic solvents versus redox properties, and the stability of the compound.

Molecules 2024 ,
Scheme 1.(a) Synthesis of compounds 3a-g, atom numbering of heterocyclic p-quinone imine fragment of compounds 3a-g is shown in blue; (b) p-Quinone imine and benzamide fragments of obtained compounds 3a-g.2.1.1.Synthesis of Quinone Derivatives 3a-g Quinone derivatives 3a-g (Scheme 1a, atoms are numbered according to ORTEP diagram, vide infra) were obtained by the nucleophilic substitution of a chlorine atom of quinone 1a,b by benzohydrazides 2a-d.Isolated compounds 3a-g have a red-orange color in the solid state.Interestingly, in the case of aminoderivatives of quinone 1 (a Figure 1a shows a perspective view of molecule 3a with thermal ellipsoids and the atom-numbering scheme.The p-quinone imine form was confirmed by the inspection of the bond length: bonds between C(9)=O(23) and C(6)=N(11) have double-bond character, and O(22)-C(8) is a single bond (typical bond distances: d (Å) (C-O) = 1.34, (C=O) = 1.21, (C-N) = 1.38, (C=N) = 1.28[23]).Also, an analysis of bond lengths shows that the structure of compound 3a can be represented as a superposition of mesomeric forms.The main forms are shown in Figure1b; at that, the non-ionized form has the highest specific weight.

Molecules 2024 , 20 Figure 1 .
Figure 1.(a) ORTEP diagram of compound 3a showing thermal ellipsoids at the 50% probability level; (b) two mesomeric structures of compound 3a based on the bond distances in the crystal structure.

Figure 1 .
Figure 1.(a) ORTEP diagram of compound 3a showing thermal ellipsoids at the 50% probability level; (b) two mesomeric structures of compound 3a based on the bond distances in the crystal structure.The molecules of compound 3a are characterized by a flattened conformation; only the phenyl group is slightly out of the plane of the heterocyclic system (the angle between planes is 5.19 • ).In the structure of compound 3a, intramolecular hydrogen bonds NH•••N and OH•••O were found (Figure2).The hydroxy group of compound 3a forms bifurcated hydrogen bonds where O(22)-H•••O(23) is an intramolecular bond (Figure1a) and O(22)-H•••O'(23) is an intermolecular one (Figure2a).By means of these intermolecular Hbonds, the centrosymmetric R 2 2 (10) molecular dimers are formed in the crystal structure.Additional intermolecular interactions were found: stacking interaction between the planes of the molecules and a short intermolecular contact between heterocycle (C(3)-H) and the amide group of the substituent(d C(3)•••O(14) = 3.112 Å, d C(3)-H•••O(14) = 2.344 Å) (Figure2b,c).Hirshfeld surfaces and energy framework calculations (FiguresS14 and S15) were obtained in a whole-of-molecule approach using the B3LYP/6-31G(d,p) energy model implemented in CrystalExplorer 21.5 software[24].The Hirshfeld surface (shown in FigureS14, mapped with d norm ) investigation is a useful approach to establishing close contacts in a crystal.Areas of close contact are highlighted with different colors (red, white, and blue spots) to show intermolecular contacts with distances less than, equal to, and larger than van der Waal radii.As seen from the Hirshfeld surface analysis of compound 3a, bright red areas of the same size indicate strong interactions, specifically hydrogen bonds OH•••O, between neighboring molecules.Fainter red or white areas suggest relatively weak interactions involving hydrogen atoms from heterocyclic and phenyl rings and chlorine

20 Figure 2 .
Figure 2. (a) A dimer (highlighted) formed in the crystal structure of compound 3a.(b) Crystal packing of compound 3a along the a axis.(c) Crystal packing of compound 3a along the c axis.Color map: C, grey; N, blue; O, red; Cl, green; H, white.

Figure 2 .
Figure 2. (a) A dimer (highlighted) formed in the crystal structure of compound 3a.(b) Crystal packing of compound 3a along the a axis.(c) Crystal packing of compound 3a along the c axis.Color map: C, grey; N, blue; O, red; Cl, green; H, white.

Figure 3 .
Figure 3.An expansion of 1 H NMR spectra of compound 3b in DMSO-d6 solution upon sequential addition of base (DBU) and acid (TFA).

Figure 3 .
Figure 3.An expansion of 1 H NMR spectra of compound 3b in DMSO-d 6 solution upon sequential addition of base (DBU) and acid (TFA).

Molecules 2024 , 20 Figure 5 .
Figure 5. (a) UV-Vis absorption spectra of neutral (in DMSO or DCM solution) and deprotonated (upon addition base to the DMSO or DCM solution) forms of compound 3a.(b) UV-Vis absorption spectra neutral (in DMSO solution) and deprotonated (upon addition of a base to the DMSO solution) forms of compounds 3a and 3c.

Figure 5 .
Figure 5. (a) UV-Vis absorption spectra of neutral (in DMSO or DCM solution) and deprotonated (upon addition base to the DMSO or DCM solution) forms of compound 3a.(b) UV-Vis absorption spectra neutral (in DMSO solution) and deprotonated (upon addition of a base to the DMSO solution) forms of compounds 3a and 3c.

Figure 7 .
Figure 7. (a) Raman spectra of pure compound 3a (green line), prepared cathode CM-3a before (blue line) and after cycling in acidic (red line) and neutral (gray line) electrolytes.(b) Raman spectra of pure compound 1a (green line), prepared cathode CM-1a before (blue line) and after cycling in acidic (red line) and neutral (gray line) electrolytes.

Figure 7 .
Figure 7. (a) Raman spectra of pure compound 3a (green line), prepared cathode CM-3a before (blue line) and after cycling in acidic (red line) and neutral (gray line) electrolytes.(b) Raman spectra of pure compound 1a (green line), prepared cathode CM-1a before (blue line) and after cycling in acidic (red line) and neutral (gray line) electrolytes.

Figure 8 .
Figure 8. Scanning electron microscopy images of samples CM-1a, CM-3a, and substrate (coating without active material) before and after CV measurements in neutral and acidic electrolytes (magnification of ×2500).

Figure 8 .
Figure 8. Scanning electron microscopy images of samples CM-1a, CM-3a, and substrate (coating without active material) before and after CV measurements in neutral and acidic electrolytes (magnification of ×2500).

Table 1 .
Crystal data and structure refinement details for compound 3a.