A Family of Ethyl N-Salicylideneglycinate Dyes Stabilized by Intramolecular Hydrogen Bonding: Photophysical Properties and Computational Study

In this work we report solvatochromic and luminescent properties of ethyl N-salicylideneglycinate (1), ethyl N-(5-methoxysalicylidene)glycinate (2), ethyl N-(5-bromosalicylidene)glycinate (3), and ethyl N-(5-nitrosalicylidene)glycinate (4) dyes. 1–4 correspond to a class of N-salicylidene aniline derivatives, whose photophysical properties are dictated by the intramolecular proton transfer between the OH-function and the imine N-atom, affording tautomerization between the enol-imine and keto-enamine forms. Photophysical properties of 1–4 were studied in different pure non-polar and (a)protic polar solvents as well as upon gradual addition of NEt3, NaOH, and CH3SO3H. The DFT calculations were performed to verify the structures of 1–4 as well as their electronic and optical properties.


Introduction
Schiff base is a condensation product of aldehyde and primary amine. When salicylaldehyde derivative is used as an aldehyde and amine is a monoamine derivative, the condensation yields a NO-Schiff base compound that may produce complexes with a great variety of metal ions upon deprotonation. Thus, Schiff bases are still of great importance in coordination chemistry, although more than a century has passed since their discovery [1][2][3]. Schiff bases have been known to be the most actively used ligands thanks to their ease of synthesis, availability, structural versatility, and solubility in common solvents. Moreover, Schiff bases are not only efficient ligands to coordinate/chelate many elements but can stabilize elements in various and specific oxidation states. It is also noteworthy that Schiff bases, as well as their corresponding complexes, can possess pronounced bioactivity [4][5][6], including against coronavirus [7]. The latter is becoming even more important since these days humanity is in dire need of drugs for COVID-19 treatment.
Notably, due to the abovementioned tautomerization, N-salicylidene aniline derivatives can also possess the so-called ESIPT (excited state intramolecular proton transfer) [36], which can afford an equilibrium between the excited keto-enamine* and enol-imine* forms [29,30,37,38]. The keto-enamine form usually, emits at a lower energy than the enolimine tautomer leading to dual fluorescence, which can be observed as two (or more) emission bands [29,30,37,38]. The ratio of these bands can be influenced by the nature of a solvent, which allows tuning the resulting emission color.
It should be noticed that we have recently initiated comprehensive studies of closely related N-salicylidene aniline derivatives 1-4, derived from the ethyl ester of glycine (Chart 1) [17,18]. We found that 1-4 in the solid state each exhibits an enol-imine form. Notably, the electron-withdrawing NO2 substituent in 4 is mainly responsible for the formation of the cis-keto form isomer in EtOH, while dyes 1-3 adopt the enol-imine form in the same solvent. Additionally, only 4 is emissive under ambient conditions in the solid state, while 2 is emissive in EtOH. Intrigued by the obtained results, herein, we continue our comprehensive studies of the dyes 1-4. Particularly, to probe solvatochromism, we focused on the optical properties of these compounds in different solvents, as well as shedding more light on their crystal structures using the Hirshfeld surface analysis to examine in-depth the non-covalent interactions responsible for crystal packing, which might be responsible for the observed photophysical properties of 1-4 in the solid state. Intrigued by the obtained results, herein, we continue our comprehensive studies of the dyes 1-4. Particularly, to probe solvatochromism, we focused on the optical properties of these compounds in different solvents, as well as shedding more light on their crystal structures using the Hirshfeld surface analysis to examine in-depth the non-covalent interactions responsible for crystal packing, which might be responsible for the observed photophysical properties of 1-4 in the solid state.

Results and Discussion
Dyes 1-4 were produced according to the described synthetic procedure [18]. We first applied a Hirshfeld surface analysis [39] to study the intermolecular interactions in the reported crystal structures of 1-4 [17]. As a result, a set of 2D fingerprint plots [40] were generated using CrystalExplorer 3.1 [41]. In order to estimate the propensity of two chemical species being in contact, we also calculated the enrichment ratios (E) [42] of the intermolecular contacts.
The intermolecular H···H, H···C and H···O contacts occupy a majority of a molecular surface of 1 (Table 1). There is a barely observed splitting of the shortest H···H fingerprint at d e + d i ≈ 2.4 Å, which is due to the shortest contact being between three atoms, rather than for direct two-atom contact ( Figure S1 in Supplementary Materials) [40]. The H···C and H···O shortest contacts are shown at d e + d i ≈ 2.7 and 2.3 Å, respectively ( Figure S1). The latter contacts in the corresponding fingerprint plot are shown as two spikes and mainly correspond to the contacts formed by the carbonyl oxygen atom. The molecular surface of 1 is also characterized by a negligible proportion of the H···N, C···O and O···O contacts, ranging from 0.6% to 2.4% (Table 1). Table 1. Hirshfeld contact surfaces and derived "random contacts" and "enrichment ratios" for the crystal structures of 1-4.

Results and Discussion
Dyes 1-4 were produced according to the described synthetic procedure [18]. We first applied a Hirshfeld surface analysis [39] to study the intermolecular interactions in the reported crystal structures of 1-4 [17]. As a result, a set of 2D fingerprint plots [40] were generated using CrystalExplorer 3.1 [41]. In order to estimate the propensity of two chemical species being in contact, we also calculated the enrichment ratios (E) [42] of the intermolecular contacts.
The intermolecular H•••H, H•••C and H•••O contacts occupy a majority of a molecular surface of 1 (Table 1). There is a barely observed splitting of the shortest H•••H fingerprint at de + di ≈ 2.4 Å, which is due to the shortest contact being between three atoms, rather than for direct two-atom contact ( Figure S1 in Supplementary Materials) [40]. The H•••C and H•••O shortest contacts are shown at de + di ≈ 2.7 and 2.3 Å, respectively ( Figure S1). The latter contacts in the corresponding fingerprint plot are shown as two spikes and mainly correspond to the contacts formed by the carbonyl oxygen atom. The molecular surface of 1 is also characterized by a negligible proportion of the H•••N, C•••O and O•••O contacts, ranging from 0.6% to 2.4% (Table 1). Table 1. Hirshfeld contact surfaces and derived "random contacts" and "enrichment ratios" for the crystal structures of 1-4.  [41]. 2 The "enrichment ratios" were not computed when the "random contacts" were lower than 0.9%, as they are not meaningful [42].

Results and Discussion
Dyes 1-4 were produced according to the described synthetic procedure [18]. We first applied a Hirshfeld surface analysis [39] to study the intermolecular interactions in the reported crystal structures of 1-4 [17]. As a result, a set of 2D fingerprint plots [40] were generated using CrystalExplorer 3.1 [41]. In order to estimate the propensity of two chemical species being in contact, we also calculated the enrichment ratios (E) [42] of the intermolecular contacts.
The intermolecular H•••H, H•••C and H•••O contacts occupy a majority of a molecular surface of 1 (Table 1). There is a barely observed splitting of the shortest H•••H fingerprint at de + di ≈ 2.4 Å, which is due to the shortest contact being between three atoms, rather than for direct two-atom contact ( Figure S1 in Supplementary Materials) [40]. The H•••C and H•••O shortest contacts are shown at de + di ≈ 2.7 and 2.3 Å, respectively ( Figure S1). The latter contacts in the corresponding fingerprint plot are shown as two spikes and mainly correspond to the contacts formed by the carbonyl oxygen atom. The molecular surface of 1 is also characterized by a negligible proportion of the H•••N, C•••O and O•••O contacts, ranging from 0.6% to 2.4% (Table 1). Table 1. Hirshfeld contact surfaces and derived "random contacts" and "enrichment ratios" for the crystal structures of 1-4.

Results and Discussion
Dyes 1-4 were produced according to the described synthetic procedure [18]. We first applied a Hirshfeld surface analysis [39] to study the intermolecular interactions in the reported crystal structures of 1-4 [17]. As a result, a set of 2D fingerprint plots [40] were generated using CrystalExplorer 3.1 [41]. In order to estimate the propensity of two chemical species being in contact, we also calculated the enrichment ratios (E) [42] of the intermolecular contacts.
The intermolecular H•••H, H•••C and H•••O contacts occupy a majority of a molecular surface of 1 (Table 1). There is a barely observed splitting of the shortest H•••H fingerprint at de + di ≈ 2.4 Å, which is due to the shortest contact being between three atoms, rather than for direct two-atom contact ( Figure S1 in Supplementary Materials) [40]. The H•••C and H•••O shortest contacts are shown at de + di ≈ 2.7 and 2.3 Å, respectively ( Figure S1). The latter contacts in the corresponding fingerprint plot are shown as two spikes and mainly correspond to the contacts formed by the carbonyl oxygen atom. The molecular surface of 1 is also characterized by a negligible proportion of the H•••N, C•••O and O•••O contacts, ranging from 0.6% to 2.4% (Table 1). Table 1. Hirshfeld contact surfaces and derived "random contacts" and "enrichment ratios" for the crystal structures of 1-4.   [41]. 2 The "enrichment ratios" were not computed when the "random contacts" were lower than 0.9%, as they are not meaningful [42].

Results and Discussion
Dyes 1-4 were produced according to the described synthetic procedure [18]. We first applied a Hirshfeld surface analysis [39] to study the intermolecular interactions in the reported crystal structures of 1-4 [17]. As a result, a set of 2D fingerprint plots [40] were generated using CrystalExplorer 3.1 [41]. In order to estimate the propensity of two chemical species being in contact, we also calculated the enrichment ratios (E) [42] of the intermolecular contacts.
The intermolecular H•••H, H•••C and H•••O contacts occupy a majority of a molecular surface of 1 (Table 1). There is a barely observed splitting of the shortest H•••H fingerprint at de + di ≈ 2.4 Å, which is due to the shortest contact being between three atoms, rather than for direct two-atom contact ( Figure S1 in Supplementary Materials) [40]. The H•••C and H•••O shortest contacts are shown at de + di ≈ 2.7 and 2.3 Å, respectively ( Figure S1). The latter contacts in the corresponding fingerprint plot are shown as two spikes and mainly correspond to the contacts formed by the carbonyl oxygen atom. The molecular surface of 1 is also characterized by a negligible proportion of the H•••N, C•••O and O•••O contacts, ranging from 0.6% to 2.4% (Table 1). Table 1. Hirshfeld contact surfaces and derived "random contacts" and "enrichment ratios" for the crystal structures of 1-4.  Random contacts (R, %) Substitution of the 5-hydrogen atom by the MeO function in 2 decreases a proportion of the H···H and H···C contacts by 2.8 and 1.7%, respectively, with the simultaneous increase of a proportion of the H···O contacts up to 30.1% (Table 1). The H···H and H···C shortest contacts are now shown at d e + d i ≈ 2.2 and 2.9 Å, respectively ( Figure S2). The H···O contacts in the corresponding 2D fingerprint plot are also shown as two spikes with the shortest contacts at d e + d i ≈ 2.3 Å, also being formed by the carbonyl oxygen atom ( Figure S2). The Hirshfeld molecular surface of 2 is further described by a very minor proportion of the H···N, C···C, C···O and O···O contacts, varying from 0.3 to 2.4% (Table 1).
In 3, incorporation of the bromine instead of the hydrogen in 1 or the methoxy group in 2 significantly decreases a proportion of the H· · · H and H· · · C intermolecular contacts down to 35.4 and 13.7%, respectively. A proportion of the H· · · O contact remains almost the same as in 1 ( Table 1). The H···H, H···C and H···O shortest contacts are shown in the corresponding 2D fingerprint plots at d e + d i ≈ 2.2, 2.8, and 2.3 Å, respectively ( Figure S3). The molecular surface of 3 is additionally characterized by a remarkable proportion of the H···Br intermolecular contacts of 17.4%, with the shortest contacts at d e + d i ≈ 3.0 Å ( Figure S3). Notably, the molecular surface of 3 is further described by a distinct proportion of the C···C contacts of 4.1%, which is due to intermolecular π· · · π stacking interactions between the phenylene rings [17]. These contacts are shown on the 2D plot as a typical area at d e = d i ≈ 1.7-2.0 Å ( Figure S3). Insignificant contributions from H···N, C···N, C···O, C···Br, N···O, O···O, and Br···Br contacts in 3 have also been revealed (Table 1).
Dye 4 contains the NO 2 group in the same position as the corresponding substituent in 2 and 3 (Chart 1). The molecular surface of 4 is characterized by a dominant contribution from the H···O contacts of 44.1% with the shortest contacts, shown in the corresponding 2D fingerprint plot at d e + d i ≈ 2.3 Å mainly formed by both the NO 2 and carbonyl oxygen atoms ( Figure S4). The H···H and H···C contacts occupy 30.0 and 11.5%, respectively. Notably, the structure of 4, similar to 3, also exhibits a distinct proportion of the C···C contacts of 4.9% due to the formation of intermolecular π· · · π stacking interactions between the phenylene rings [17]. These contacts are also shown on the 2D plot as a typical area at d e = d i ≈ 1.7-2.0 Å ( Figure S4). Remaining contacts, namely H···N, C···N, C···O, N···O and O···O contacts, occupy a negligible proportion of the molecular surface of 4 ( Table 1).
All the H···X (X = C, N, O) contacts are highly favored in 1 and 2 since the corresponding enrichment ratios E HX are significantly higher than unity (Table 1). This is explained by a relatively higher proportion of these contacts on the total Hirshfeld surface area over a corresponding proportion of random contacts R HX (Table 1). However, only H· · · N and H· · · O intermolecular contacts are favored in 3 and 4, while the H· · · C contacts on the surface of molecules are much less favored, which is related to a remarkably high enrichment of C· · · C contacts in 3 and 4 (Table 1), formed in aromatic stacking. Notably, both 3 and 4 are additionally characterized by highly favored H· · · Br and N· · · O contacts, respectively, and 3 is also described by less favored Br· · · Br contacts ( Table 1). The H· · · H intermolecular contacts on the molecular surfaces of all compounds are less favored since the corresponding enrichment ratios E HH are less than unity ranging from 0.85 to 0.90 ( Table 1). The remaining contacts are significantly impoverished with the corresponding enrichment ratios less than 0.50 (Table 1).
We have also examined the optical properties of 1-4 in different solvents. We first probed such solvents as cyclohexane (non-polar), THF (polar aprotic), CH 3 CN (polar aprotic), and EtOH (polar protic) to study the enol-imine and keto-enamine tautomerization in the applied solvents. It is known that the dipole moments for the enol-imine isomers are smaller than those for the keto-enamine derivatives [43,44], which means that the keto-enamine tautomer is more prevalent in polar solvents.
The absorption spectra of 1-3 each contain bands corresponding to n→π* and π→π* transitions only in the UV region, regardless of the solvent (Figures S5-S7). Interestingly, the longest wavelength band in the spectra of 2 is remarkably red-shifted ( Figures S5-S7). This is due to the electron-donating properties of the MeO fragment in comparison to the H and Br substituents in 1 and 3, respectively. Furthermore, the spectra of 1-3 in EtOH exhibit an additional low-intense band, centered at about 400-420 nm ( Figures S5-S7), which corresponds to the traces of the cis-keto-enamine form.
The absorption spectra of 4 in the same solvents, except cyclohexane, contain an intense band in the visible region, which arises from the cis-keto-enamine form ( Figure 1). Notably, in 4, the electron-donating OH is involved in a through-resonance effect with the electron-withdrawing NO 2 fragment. This leads to nitro-aci-nitro tautomerization, yielding an additional quinoid form [45].
Molecules 2021, 26, x FOR PEER REVIEW 5 of 18 exhibit an additional low-intense band, centered at about 400-420 nm ( Figures S5-S7), which corresponds to the traces of the cis-keto-enamine form.
The absorption spectra of 4 in the same solvents, except cyclohexane, contain an intense band in the visible region, which arises from the cis-keto-enamine form ( Figure 1). Notably, in 4, the electron-donating OH is involved in a through-resonance effect with the electron-withdrawing NO2 fragment. This leads to nitro-aci-nitro tautomerization, yielding an additional quinoid form [45]. Optical properties of 4 were also studied in a series of alcohols, namely MeOH, EtOH, nPrOH, iPrOH, and nBuOH. Interestingly, in the absorption spectra of 4 in all alcohols, except nPrOH, the band of the cis-keto-enamine form was observed with the most remarkable one in MeOH (Figure 2), which is the most polar and acidic within the applied alcohols. The most striking observation is the absence of the band of the cis-keto-enamine form in the spectrum of 4 in nPrOH ( Figure 2). This might be explained by possible specific solute-solvent interactions.  Optical properties of 4 were also studied in a series of alcohols, namely MeOH, EtOH, nPrOH, iPrOH, and nBuOH. Interestingly, in the absorption spectra of 4 in all alcohols, except nPrOH, the band of the cis-keto-enamine form was observed with the most remarkable one in MeOH (Figure 2), which is the most polar and acidic within the applied alcohols. The most striking observation is the absence of the band of the cis-keto-enamine form in the spectrum of 4 in nPrOH ( Figure 2). This might be explained by possible specific solute-solvent interactions. exhibit an additional low-intense band, centered at about 400-420 nm ( Figures S5-S7), which corresponds to the traces of the cis-keto-enamine form.
The absorption spectra of 4 in the same solvents, except cyclohexane, contain an intense band in the visible region, which arises from the cis-keto-enamine form ( Figure 1). Notably, in 4, the electron-donating OH is involved in a through-resonance effect with the electron-withdrawing NO2 fragment. This leads to nitro-aci-nitro tautomerization, yielding an additional quinoid form [45]. Optical properties of 4 were also studied in a series of alcohols, namely MeOH, EtOH, nPrOH, iPrOH, and nBuOH. Interestingly, in the absorption spectra of 4 in all alcohols, except nPrOH, the band of the cis-keto-enamine form was observed with the most remarkable one in MeOH (Figure 2), which is the most polar and acidic within the applied alcohols. The most striking observation is the absence of the band of the cis-keto-enamine form in the spectrum of 4 in nPrOH ( Figure 2). This might be explained by possible specific solute-solvent interactions.  Recently, we established that 2 was emissive in EtOH [17]. The resulting emission of 2 in EtOH was due to two emission bands arising from two conformers of the cisketo-enamine* form. Herein we report the emission properties of 4 in different alcohols. Interestingly, 4 was found to be emissive in iPrOH and nPrOH, while almost no emission was found in EtOH and MeOH (Figure 3). Recently, we established that 2 was emissive in EtOH [17]. The resulting emission of 2 in EtOH was due to two emission bands arising from two conformers of the cis-ketoenamine* form. Herein we report the emission properties of 4 in different alcohols. Interestingly, 4 was found to be emissive in iPrOH and nPrOH, while almost no emission was found in EtOH and MeOH (Figure 3).  The emission spectra of 4 in iPrOH and nPrOH exhibit an intense band at 475 and 460 nm, respectively. Notably, the former band is accompanied with an intense low-energy shoulder (Figure 3). The deconvolution process of the spectrum in iPrOH has allowed revealing three single bands at 463, 493, and 526 nm, and a ratio of these bands is 26.4, 30.0, and 43.6%, respectively ( Figure S8). The same deconvolution of the emission spectrum of 4 in nPrOH also revealed three bands, but with the maxima remarkably shifted to higher energies (444, 466, and 496 nm) and with a ratio of 17.2, 46.2, and 36.6%, respectively ( Figure S8). Based on the absorption and excitation spectra of 4 in iPrOH we were able to conclude that these three emission bands corresponded to two cis-ketoenamine* and trans-keto-enamine* conformers [8][9][10][11][12][13][14][15][16][17][18]. Contrarily, all three bands in the emission spectrum of 4 in nPrOH arose exclusively from the emission of different cis-ketoenamine* conformers.
We next studied the solution of 4 upon the gradual addition of two different bases, namely NEt3 and NaOH, to probe the influence of the nature of bases (electronic properties and steric demands). Upon addition of both bases, the absorption band at 313 nm disappeared and two new bands, centered at about 360 and 390 nm, appeared ( Figure 4 and Figure S9). Notably, the ratio of intensities of the new bands was in favor of the lowenergy band when NaOH was used.
The gradual addition of the methanesulfonic acid into a solution of 4 in EtOH decreased the intensity of the band of the cis-keto-enamine form, which was due to protonation of the imine N-atom, while the NO2 group remained unchanged, as seen from the high-energy band, which remained constant during the titration process ( Figure 5). Protonation of the imine N-atom prevented the formation of the intramolecular O-H•••N bonding. The emission spectra of 4 in iPrOH and nPrOH exhibit an intense band at 475 and 460 nm, respectively. Notably, the former band is accompanied with an intense low-energy shoulder ( Figure 3). The deconvolution process of the spectrum in iPrOH has allowed revealing three single bands at 463, 493, and 526 nm, and a ratio of these bands is 26.4, 30.0, and 43.6%, respectively ( Figure S8). The same deconvolution of the emission spectrum of 4 in nPrOH also revealed three bands, but with the maxima remarkably shifted to higher energies (444, 466, and 496 nm) and with a ratio of 17.2, 46.2, and 36.6%, respectively ( Figure S8). Based on the absorption and excitation spectra of 4 in iPrOH we were able to conclude that these three emission bands corresponded to two cis-keto-enamine* and transketo-enamine* conformers [8][9][10][11][12][13][14][15][16][17][18]. Contrarily, all three bands in the emission spectrum of 4 in nPrOH arose exclusively from the emission of different cis-keto-enamine* conformers.
We next studied the solution of 4 upon the gradual addition of two different bases, namely NEt 3 and NaOH, to probe the influence of the nature of bases (electronic properties and steric demands). Upon addition of both bases, the absorption band at 313 nm disappeared and two new bands, centered at about 360 and 390 nm, appeared (Figure 4 and Figure S9). Notably, the ratio of intensities of the new bands was in favor of the low-energy band when NaOH was used.
The gradual addition of the methanesulfonic acid into a solution of 4 in EtOH decreased the intensity of the band of the cis-keto-enamine form, which was due to protonation of the imine N-atom, while the NO 2 group remained unchanged, as seen from the high-energy band, which remained constant during the titration process ( Figure 5). Protonation of the imine N-atom prevented the formation of the intramolecular O-H···N bonding.  Since compound 3 also tends to clearly exhibit the cis-keto-enamine form in EtOH ( Figure S7), although less pronounced than 4, but more pronounced that 1 and 2, its optical properties were further studied upon gradual addition of NaOH and CH3SO3H. In general, the behavior of a solution of 3 in EtOH in the presence of NaOH and CH3SO3H was similar to a solution of 4 but much less pronounced; however, emission spectra of 3 differed significantly from those of 4.
After the addition of NaOH, the absorption band at 330 nm disappeared with the simultaneous increase of a low-intense band in the visible region ( Figure 6). However, the addition of CH3SO3H to a solution of 3 in EtOH vanished the same band, arising from the cis-keto-enamine tautomer (Figure 7).  Since compound 3 also tends to clearly exhibit the cis-keto-enamine form in EtOH ( Figure S7), although less pronounced than 4, but more pronounced that 1 and 2, its optical properties were further studied upon gradual addition of NaOH and CH3SO3H. In general, the behavior of a solution of 3 in EtOH in the presence of NaOH and CH3SO3H was similar to a solution of 4 but much less pronounced; however, emission spectra of 3 differed significantly from those of 4.
After the addition of NaOH, the absorption band at 330 nm disappeared with the simultaneous increase of a low-intense band in the visible region ( Figure 6). However, the addition of CH3SO3H to a solution of 3 in EtOH vanished the same band, arising from the cis-keto-enamine tautomer (Figure 7). Since compound 3 also tends to clearly exhibit the cis-keto-enamine form in EtOH ( Figure S7), although less pronounced than 4, but more pronounced that 1 and 2, its optical properties were further studied upon gradual addition of NaOH and CH 3 SO 3 H. In general, the behavior of a solution of 3 in EtOH in the presence of NaOH and CH 3 SO 3 H was similar to a solution of 4 but much less pronounced; however, emission spectra of 3 differed significantly from those of 4.
After the addition of NaOH, the absorption band at 330 nm disappeared with the simultaneous increase of a low-intense band in the visible region ( Figure 6). However, the addition of CH 3 SO 3 H to a solution of 3 in EtOH vanished the same band, arising from the cis-keto-enamine tautomer (Figure 7). Upon the addition of NaOH to a solution of 3 in EtOH, an emission band appeared (Figure 8), which deconvolution revealed two bands at 480 and 505 nm and with an area ratio of 30.1 and 69.9%, respectively ( Figure S10). Based on the comparison of the absorption ( Figure 6) and excitation (Figure 8) spectra, the emission band was assigned to two conformers of the deprotonated form of 3. Solutions of 3 in EtOH were found to be nonemissive regardless of the added amount of CH3SO3H. Upon the addition of NaOH to a solution of 3 in EtOH, an emission band appeared (Figure 8), which deconvolution revealed two bands at 480 and 505 nm and with an area ratio of 30.1 and 69.9%, respectively ( Figure S10). Based on the comparison of the absorption ( Figure 6) and excitation (Figure 8) spectra, the emission band was assigned to two conformers of the deprotonated form of 3. Solutions of 3 in EtOH were found to be nonemissive regardless of the added amount of CH3SO3H. We have further applied the density functional theory (DFT) calculations to examine the fine features of 1-4. It was established that the calculated values of bond lengths, bond angles, and dihedral angles ( Table 2) were in good agreement with the values recently obtained from single-crystal X-ray diffraction [17]. The observed differences between the calculated and experimental geometrical parameters are obviously explained by the fact that the DFT computations were performed in the gas phase. According to the DFT calculations, the dipole moments of the fully optimized ground state geometry of the enol-imine forms were 3.279813 Debye for 1, 4.290475 Debye for 2, 4.070018 Debye for 3, and 6.97922 Debye for 4. Notably, the transformation from the enolimine to the trans-keto-enamine through the cis-keto-enamine tautomers was followed by We have further applied the density functional theory (DFT) calculations to examine the fine features of 1-4. It was established that the calculated values of bond lengths, bond angles, and dihedral angles ( Table 2) were in good agreement with the values recently obtained from single-crystal X-ray diffraction [17]. The observed differences between the calculated and experimental geometrical parameters are obviously explained by the fact that the DFT computations were performed in the gas phase. by a remarkable increase in the dipole moments for all the structures (Table 3). Significantly higher dipole moments of different tautomers of 4 in comparison to the corresponding values of tautomers of 1-3 were obviously explained by the presence of the highly polar NO 2 substituent. The energies of the frontier molecular orbitals for the highest occupied molecular orbital (HOMO) and lowest-lying unoccupied molecular orbital (LUMO) are shown in Table 3. Both orbitals were mainly delocalized over the 2-OH(5-X)C 6 H 3 CH=N-CH 2 C(=O) fragment for all the structures except for the LUMO of 4, where the orbital was mainly spread over the 2-OH(5-X)C 6 H 3 fragment (Figure 9).  The so-called ionization potential (I) and the electron affinity (A) value of the molecules were established as follows: I = −EHOMO and A = −ELUMO (Table 3) [46], which determined the electron-donating ability and the ability to accept an electron, respectively. As such, as lower values of I as better donation of an electron, while as higher values of A as better ability to accept electrons. Both the I and A values for all the tautomers of 1-4 are remarkably lower than unity (Table 3), indicating that the reported dyes each exhibit high electron-donating and low electron-accepting properties. Notably, the corresponding cis-  (Table 3) [46], which determined the electron-donating ability and the ability to accept an electron, respectively. As such, as lower values of I as better donation of an electron, while as higher values of A as better ability to accept electrons. Both the I and A values for all the tautomers of 1-4 are remarkably lower than unity (Table 3), indicating that the reported dyes each exhibit high electron-donating and low electron-accepting properties. Notably, the corresponding cisketo-enamine and trans-keto-enamine tautomers of 1-4 are slightly better electron donors and electron acceptors in comparison to their enol-imine derivatives (Table 3).
To estimate the relative reactivity of molecules of 1-4, we have further established values of the so-called global chemical reactivity descriptors derived from the HOMO-LUMO energy gap (Table 3). The values of chemical potential (µ) for 1-4 were in the range from −0.13135 eV to −0.18025 eV for all tautomers, indicating the poor electron-accepting ability and the strong donating ability, which was further supported with low values of electroneg-ativity, χ (Table 3). Notably, the values of electronegativity for all the cis-keto-enamine tautomers were lower than those for the enol-imine and trans-keto-enamine forms of 1-4 (Table 3). Chemical hardness (η) describes the resistance towards deformation/polarization of the electron cloud of the molecule upon a chemical reaction, while softness (S) is a reverse of chemical hardness [46]. Compounds 1-4 are characterized by low values of η and high values of S, respectively, indicating a remarkable tendency to exchange their electron clouds with the surrounding environment for all the structures (Table 3). It should be noted that the trans-keto-enamine tautomers are more pronounced to exchange their electron clouds with the surrounding environment in comparison to the corresponding cis-ketoenamine tautomers, and even much more pronounced in comparison to the enol-imine tautomers ( Table 3). The electrophilicity index (ω) describes the energy of stabilization to accept electrons [46]. The ω values for all forms of 1-4 were found in the range from about 0.12 eV to 0.25 eV (Table 3). These values are low, indicating the strong nucleophilic nature of 1-4. Finally, compounds 1-4 can accept about 1.77-2.24 electrons for the enol-imine forms, 2.12-2.52 electrons for the cis-keto-enamine forms, and 2.30-2.89 electrons for the trans-keto-enamine forms, respectively, as evidenced from the ∆N max values, of which the highest values correspond to 4 ( Table 3).
The electrophilic and nucleophilic sites in 1-4 were examined using the molecular electrostatic potential (MEP) analysis. The red and blue colors of the MEP surface correspond to electron-rich (nucleophilic) and electron-deficient (electrophilic) regions, respectively. On the MEP surfaces of the enol-imine tautomers of 1-4 the most pronounced nucleophilic centers are located on the carbonyl and hydroxyl oxygen atoms, while the other negative electrostatic potential sites in the enol-imine form of 4 are located on the oxygen atoms of the NO 2 group (Figure 10). In the cis-keto-enamine and trans-keto-enamine tautomers of 1-4 the carbonyl oxygen atom attached to the aromatic ring is the most remarkable nucleophilic center, alongside with both oxygen atoms of the NO 2 group in 4, while the carbonyl oxygen atom of the carboxyl group becomes a less pronounced nucleophilic center ( Figure 10). As the most electrophilic region the CH=N-CH 2 fragment for the enol-imine tautomers and the CH-NH-CH 2 fragment for the cis-keto-enamine and trans-keto-enamine tautomers can be highlighted for the structures of 1-4 ( Figure 10).
The calculated absorption spectra of the fully optimized ground state geometry of all the three tautomers of 1-4 (Figures S11-S13) are in agreement with experimental spectra. In particular, the experimental UV-vis spectra for the enol-imine tautomers exhibited bands at 215-260 and 331-353 nm, and the calculated spectra for the same tautomers contained bands at 225-250 and 302-351 nm (Table S1). The cis-keto-enamine tautomers are shown as a band centered at 382-418 nm in both the experimental and calculated absorption spectra (Table S1). The calculated UV-vis spectra for the trans-keto-enamine tautomers of 1-4 each exhibited a low-energy band at 407-428 nm, while no similar bands were observed in the corresponding experimental spectra (Table S1) The calculated UV-vis spectra of the enol-imine forms of 1-4 exhibit absorption bands with three (for 1) or two (for 2-4) maxima exclusively in the UV region centered at about 220-255 nm and 300-350 nm ( Figure S11). These bands mostly corresponded to the HOMO-1 → LUMO, HOMO → LUMO, and HOMO → LUMO+3 transitions (Table 4, Figure S11). The absorption bands in the spectra of 3 and 4 were additionally supported by the HOMO → LUMO+1 transition and further described by the HOMO-4 → LUMO transition in the spectrum of 3, and by the HOMO-3 → LUMO+1 and HOMO-1 → LUMO+1 transitions in the spectrum of 4, respectively (Table 4, Figure S11). As for the calculated UV-vis spectra of the cis-keto-enamine and trans-keto-enamine tautomers of 1-4, absorption bands are observed in both the UV and visible regions up to about 500-550 nm ( Figure S12) and 600 nm ( Figure S13), respectively. These bands are characterized by two maxima centered at about 250-290 nm and 380-430 nm (Figures S12 and S13). Notably, the calculated UV-vis spectrum of the cis-keto-enamine form of 4 contained an additional maxima at 320 nm ( Figure S12). The corresponding transitions, responsible for the observed bands in the calculated UV-vis spectra of the cis-keto-enamine and trans-ketoenamine tautomers of 1-4, are shown in Figures S14-S17 and collected in Tables S2 and S3. The calculated UV-vis spectra of the enol-imine forms of 1-4 exhibit absorption bands with three (for 1) or two (for 2-4) maxima exclusively in the UV region centered at about 220-255 nm and 300-350 nm ( Figure S11). These bands mostly corresponded to the HOMO-1 → LUMO, HOMO → LUMO, and HOMO → LUMO+3 transitions (Table 4, Figure S11). The absorption bands in the spectra of 3 and 4 were additionally supported by the HOMO → LUMO+1 transition and further described by the HOMO-4 → LUMO transition in the spectrum of 3, and by the HOMO-3 → LUMO+1 and HOMO-1 → LUMO+1 transitions in the spectrum of 4, respectively (Table 4, Figure S11). As for the calculated UV-vis spectra of the cis-keto-enamine and trans-keto-enamine tautomers of 1-4, absorption bands are observed in both the UV and visible regions up to about 500-550 nm ( Figure S12) and 600 nm ( Figure S13), respectively. These bands are characterized by two maxima centered at about 250-290 nm and 380-430 nm (Figures S12 and S13). Notably, the calculated UV-vis spectrum of the cis-keto-enamine form of 4 contained an additional maxima at 320 nm ( Figure S12). The corresponding transitions, responsible for the observed bands in the calculated UV-vis spectra of the cis-keto-enamine and trans-keto-enamine tautomers of 1-4, are shown in Figures S14-S17 and collected in Tables S2 and S3.

Materials
All reagents and solvents were commercially available and used without further purification. Dyes 1-4 were obtained according to the described synthetic procedure [18].

Physical Measurements
Absorption and fluorescent spectra from the freshly prepared solutions (10 −4 M) in freshly distilled solvents were recorded on an Agilent 8453 instrument.

Computational Details
The ground state geometry of 1-4 was fully optimized without symmetry restrictions. The calculations were performed by means of the GaussView 6.0 molecular visualization program [47] and Gaussian 09, Revision D.01 program package [48] using the density functional theory (DFT) method with Becke three-parameter Lee-Yang-Parr (B3LYP) hybrid functional [49,50] and 6-311++G(d,p) [49,51] basis set. The crystal structure geometry was used as a starting model for structural optimization. The vibration frequencies were calculated for the optimized structures in the gas phase and no imaginary frequencies were obtained. The Cartesian atomic coordinates for the optimized structures are gathered in Tables S4-S7. The electronic isosurfaces of the HOMO and LUMO orbitals and MEP surfaces of all tautomers of 1-4 were generated from the fully optimized ground state geometry obtained by using the B3LYP/6-311++G(d,p) method. The absorption spectra of the fully optimized ground state geometry of all the three tautomers of 1-4 were simulated at the TD-DFT/B3LYP/6-311++G(d,p) level.
The intermolecular H···H, H···C, and H···O contacts are the dominant contributors to the molecular surface of all the reported compounds. 3 is further described by a remarkable proportion of the intermolecular H···Br contacts. Furthermore, a distinct proportion of the C···C contacts was found in the molecular surface of 3 and 4, which is explained by intermolecular π· · · π stacking interactions between the phenylene rings.
The absorption spectra of 4 in THF and CH 3 CN exhibit a band for the cis-keto-enamine form, while only the enol-imine tautomer was found in the absorption spectrum of 4 in cyclohexane and in the absorption spectra of 1-3 in cyclohexane, THF, and CH 3 CN. Furthermore, in the absorption spectra of 4 in MeOH, EtOH, iPrOH, and nBuOH the cis-keto-enamine form is clearly observed, with the most remarkable one in MeOH, while the same band is absent in the spectrum of 4 in nPrOH, that might be explained by possible specific solute-solvent interactions. Dye 4 is emissive in iPrOH and nPrOH, arising from two conformers of the cis-keto-enamine* form and from the trans-keto-enamine* form, while the origin of emission in nPrOH is exclusively from different cis-keto-enamine* conformers. Titration of the solutions of 3 and 4 in EtOH by NaOH leads to the gradual increasing of the band in the visible region of the corresponding UV-vis spectra. The same band gradually decreases and finally vanishes upon titration of the solutions of 3 and 4 in EtOH by CH 3 SO 3 H due to the protonation of the imine N-atom. Notably, upon addition of NaOH to the solution of 3 in EtOH, an emission band appeared and increased with increasing NaOH concentration.
We have also demonstrated that photophysical properties of a reported series of closely related compounds 1-4 can efficiently be tuned not only by changing the corresponding substituent in the phenolic ring, thus changing electronic properties, but also by the nature of a solvent (non-polar vs. polar aprotic vs. polar protic) and pH (NEt 3 or NaOH, and CH 3 SO 3 H). All these factors allow to fine influence to the keto-enamine-enol-imine tautomerization both in the ground and excited states, yielding two or even three emission bands with a certain ratio and, as a result, different resulting emission color. No doubt, all these findings are of potential interest for molecular optics. Furthermore, the presence of the ethyl glycinate fragment in 1-4 might play a pivotal role for the application of these compounds, e.g., as luminescent sensors, in biological systems.
According to the DFT calculation results, it was established that all the tautomers of 1-4 each exhibit high electron-donating and low electron-accepting properties. The most pronounced nucleophilic centers of the enol-imine tautomers are located on the carbonyl and hydroxyl oxygen atoms, while the other negative electrostatic potential sites in the enol-imine form of 4 are located on the oxygen atoms of the NO 2 group. In the cis-ketoenamine and trans-keto-enamine tautomers of 1-4, the carbonyl oxygen atom attached to the aromatic ring is the most remarkable nucleophilic center, alongside both oxygen atoms of the NO 2 group in 4, while the carbonyl oxygen atom of the carboxyl group becomes a less pronounced nucleophilic center. As the most electrophilic region, the CH=N-CH 2 fragment for the enol-imine tautomers and the CH-NH-CH 2 fragment for the cis-ketoenamine and trans-keto-enamine tautomers are highlighted for the structures of 1-4. The calculated absorption spectra of the fully optimized ground state geometry of all the three tautomers of 1-4 are in good agreement with experimental spectra.
Supplementary Materials: The following are available online, Figures S1-S4: 2D and decomposed 2D fingerprint plots of observed contacts for the crystal structure of 1-4, Figures S5-S7: UV-vis spectra of 1-3 in the applied solvents, Figure S8: Emission and excitation spectra of 4 in nPrOH and iPrOH, Figure S9: UV-vis spectra of 4 in EtOH upon gradual addition of NEt 3 , Figure S10: Emission and excitation spectra of 3 in EtOH after addition of 5 eqv. of NaOH, Figure S11: The calculated UV-vis spectra of the ground states of the enol-imine tautomers of 1-4, Figure S12: The calculated UV-vis spectra of the ground states of the cis-keto-enamine tautomers of 1-4, Figure S13: The calculated UVvis spectra of the ground states of the trans-keto-enamine tautomers of 1-3, Figures S14-S17: Energy levels and views on the electronic isosurfaces of the selected molecular orbitals of the ground state of 1-4, Table S1: Values for the main maxima in the experimental UV-vis spectra of 1-4 in different solvents, and in the calculated UV-vis spectra for different tautomers of 1-4, Table S2: Values for the calculated UV-vis spectra of the ground state for the cis-keto-enamine tautomers of 1-4, Table S3: Values for the calculated UV-vis spectra of the ground state for the trans-keto-enamine tautomers of 1-4, Tables S4-S7: Cartesian atomic coordinates for optimized structures of 1-4, obtained by using the DFT/B3LYP/6-311++G(d,p) method.