The Synthesis, Crystal Structure, DFT Calculations and Optical Properties of Orcinolic Derivatives as OH − Indicators

: The structures of 2-(3-hydroxy-5-methylphenoxy)-N-(4-nitrophenyl)acetamide), B1, and 2-(3-hydroxy-5-methylphenoxy)-N-(4-(triﬂuoromethyl)phenyl)acetamide, B2, are crystallized in the crystal symmetry of the monoclinic structure and in the space group of P2 1 /c. For the different structures of B1 and B2, B1 displays an absolute planarity conformation with torsion angles of 172.2–179.1. The two molecules of B1 are linked by a hydrogen bond of N–H . . . O–N–O, where a hydrogen atom of amide is bound to an oxygen atom of the nitro-substituted group. In the case of B2, the molecules are connected to each other through the hydrogen bonding interaction of C=O . . . H–O. DFT calculations reveal that the transition from HOMO to LUMO of B1 and B2 shows the absorption bands B1 and B2 at 314 and 240 nm, respectively. Upon the addition of an OH − ion, the absorption bands of B1 and B2 shift to a longer wavelength than the original bands of B1 and B2. According to the 1 H-NMR results, the NH proton of B1 and B2 disappears due to the deprotonation process. The methylene group and aromatic region move to upﬁeld shift when adding an OH − ion.


Introduction
Orcinolic derivatives are vital for many applications, such as organic synthesis, chemical sensors, enzyme inhibitors and antifungal agents [1,2]. The hydroxide ion (OH − ) is an ion necessary for precipitation processes and environmental systems. Moreover, the degree strength of the hydroxide ion is used to deprotonate the NH-and OH-groups within molecules [3,4]. The nitro group (-NO 2 ) and trifluoromethyl group (-CF 3 ) within the compounds are used as electron-withdrawing substituents [5,6]. In many studies, the nitro group connecting to compounds displays antibacterial activity and is used in optical materials-for example, fluorescence probes, photonics and optoelectronics [7][8][9][10]. Compounds with trifluoromethyl groups play important roles as anticancer compounds and dye materials [11][12][13][14]. In relation to the photophysical properties, these substituents exist in polar solvents and basic conditions, leading to various mechanisms, such as internal charge transfer and pi-pi transition. The design and synthesis of compounds containing −NO 2 and −CF 3 groups are highly focused on their utilization in many applications. Nath et al. prepared a sulfadiazine derivative containing 4-nitroaniline that can be grown in the form of crystals. The crystals that were obtained were solvated by DMF, and the process of binding with anions, such as Cl − , F − , Br − and I − , was investigated by using UV-Vis and 1 H NMR techniques, resulting in the loosening of the NH proton when F − was added due to the deprotonation process [15]. Nakayama et al. synthesized and studied the asymmetric N-phenyl imide derivatives acting as triboluminescence materials-for example, N-(4-trifluoromethylphenyl)phthalimide exhibited a twisted structure, and the blue light emission was also observed [11]. Lobatto et al. studied the inclusion complexes of triflurin derivatives and β-cyclodextrin by crystal X-ray and spectroscopic techniques, and observed that the 1:1 complex conformation of the 4-trifluoromethyl aniline derivative and β-cyclodextrin produced increases in the absorption band at 238 and 430 nm, and they calculated the association constant as 18 M −1 [16]. In the present study, we report on the synthesis and crystals of orcinolic derivatives. Additionally, the behavior of crystals in DMSO was studied using DFT calculations. Moreover, the crystals were investigated as OH − indicators by 1 H-NMR and UV-Vis spectroscopy.

Materials
In the experiment, all the chemical reagents were purchased from RCI Labscan Limited and Sigma-Aldrich Co. All the reagents for synthesis were used without purification.

Equipment
The 1 H and 13 C NMR spectra were obtained on a 400 MHz NMR spectrometer. UV-Vis spectra were recorded on a Perkin Elmer lambda 365. HRMS was performed on a Bruker microtof-Q III. Infrared spectra (4000-400 cm −1 ) were obtained by a Perkin Elmer system 2000 Fourier transform infrared spectrometer.

Crystallographic Methods
The X-ray diffraction data of the compounds, such as lattice constants and diffraction intensities for the crystals of the title compounds, were collected at 273.15 and 296.15 K with a Bruker D8 Quest CMOS diffractometer equipped with graphite monochromatic MoKα radiation. The structures were solved using the dual space method [17] with the olex2.solve structure solution program using Charge Flipping and refined by successive differential Fourier syntheses performed by the least-squares minimization method using the SHELXL refinement package [18]. Anisotropic thermal parameters were refined for all non-hydrogen atoms. The hydrogen atoms were isotopically treated with a mixture of independent and constrained refinements. The disordered fluorine atoms of CF 3 − substituent groups in compound B2 were refined with half occupancy. OLEX2 and Mercury 3.10.3 [19] software were used for graphical illustrations related to single crystal X-ray data. The supplementary crystallographic data for the structures of the compounds reported in the current article have been deposited in CCDC 2075678 and 2075682. These data can be obtained via http://www.ccdc.cam.ac.uk/conts/retrieving.html (accessed on 30 June 2021).

Computational Details
In the present study, all the theoretical calculations were performed for the isolated B1 and B2 molecules using density functional theory (DFT) to obtain further information concerning the structural and electronic properties. The electronic geometries for all molecules in the ground (S0) and the first excited state (S1) were fully optimized at the PBE0 level of theory [20] using the 6-311G(d,p) basis set. The electronic transitions were performed by time-dependent DFT (TD-DFT) with the PBE0 method using the 6-311G(d,p) basis set. The results for the solvent effects were analyzed with a polarizable continuum model (PCM) [21] of dimethyl sulfoxide (DMSO). All the calculations were performed using the Gaussian 09 program [22].

Crystal Structures of Compounds B1 and B2
The crystals of compounds B1 and B2 were grown in the solvent as EtOAc:CH 2 Cl 2 = 1:9. The experimental parameters relating to the single-crystal X-ray analysis of compounds are presented in Table 1. Compound B1 was crystalized as a monoclinic structure with a P2 1 /c space group, and its molecular structure with the E configuration for the N-C(=O)-C-O bond is presented in Figure 1. The structure of the compound was observed to present an almost absolute planarity conformation with the torsion angles of C4-N2-C7-O3; 0.9(5), C4-N2-C7-C8; 179.1(3), C9-O4-C8-C7; 174.2(2) and N2-C7-C8-O4; 172.7(2), respectively. Additionally, the torsion angles involved in the substituted benzene ring, with respect to the amide functional group, were discovered to be C7-N2-C4-C3; −178.6(3) and C7-N2-C4-C5; 1.8 (5), which indicated a minor deviation from the planar of the structure. The packing images of compound B1 for the front and side views are presented in Figure 2. Moreover, the difference between each plane of the structure was 3.778(2) Å; however; the π-π interaction was not observed in such a compound.  phenol ring. Furthermore, the molecules were also connected by N-H…O-N-O, in which the hydrogen atom of amide is bound to the oxygen of the nitro-substituted group. For compound B2, the molecule was also crystalized as a monoclinic structure with a P21/c space group, and its Z configuration concerning the N-C(=O)-C-O bond is presented in Figure 4. Remarkably, the structure of compound B2 was observed to be disordered at the position of fluorine atoms of the -CF3 functional group; therefore, the formula was presented as a double of the literal structure. Unlike compound B1, compound B2 was observed to be more diverged from the planarity condition, with the torsion angles of C8-C9-O1-C10; 172.8(1), C5-N1-C8-O2; 0.7(2), C5-N1-C8-C9; −179.6(1) and N1-C8-C9-O1; 1.7 (2). Notably, the torsion angles of C8-N1-C5-C4 and C8-N1-C5-C6 related to the -CF3-substituted benzene ring aligned with the remaining structure were −142.3(2) and 38.2(2), respectively. The arrangement largely deviated in comparison to compound B1; accordingly, the packing images are exhibited as zigzag structures, as presented in Figure  5. According to this orientation, the intramolecular H-bonding of C=O…H was not observed in compound B2; however, the molecules were also linked to each other through C=O…H-O bonding, as presented in Figure 6. The H-bonding process according to the hetero atom of fluorine with N-H, including π-π interaction between each plane, was not observed; nonetheless, the difference between each centroid was detected with the value of 4.8447(15) Å.
In terms of the bond lengths, the comparison of bond distances involving the amide functional group demonstrated that N2-C7; 1.352(4) and C7-O3; 1.211(4) in compound B1 were relatively comparable to the bonds of N1-C8; 1.338(2) and C8-O2; 1.222(2) in compound B2. In addition, the bond that bound the nitrogen atom of the amide group and the phenyl ring was observed to be 1.408(4) and 1.419 (2) in compounds B1 and B2, respectively. This was attributed to the related equivalent strength of the -CF3 electron-withdrawing group related to -NO2 that created an almost equal electron density in the bond formation, leading to the similar bond lengths of such compounds. Some important bond lengths, bond angles and torsion angles are presented in Table 2.     For compound B2, the molecule was also crystalized as a monoclinic structure with a P2 1 /c space group, and its Z configuration concerning the N-C(=O)-C-O bond is presented in Figure 4. Remarkably, the structure of compound B2 was observed to be disordered at the position of fluorine atoms of the -CF 3 functional group; therefore, the formula was presented as a double of the literal structure. Unlike compound B1, compound B2 was observed to be more diverged from the planarity condition, with the torsion angles of C8-C9-O1-C10; 172.8(1), C5-N1-C8-O2; 0.7(2), C5-N1-C8-C9; −179.6(1) and N1-C8-C9-O1; 1.7 (2). Notably, the torsion angles of C8-N1-C5-C4 and C8-N1-C5-C6 related to the -CF 3 -substituted benzene ring aligned with the remaining structure were −142.3 (2) and 38.2(2), respectively. The arrangement largely deviated in comparison to compound B1; accordingly, the packing images are exhibited as zigzag structures, as presented in Figure 5. According to this orientation, the intramolecular H-bonding of C=O . . . H was not observed in compound B2; however, the molecules were also linked to each other through C=O . . . H-O bonding, as presented in Figure 6. The H-bonding process according to the hetero atom of fluorine with N-H, including π-π interaction between each plane, was not observed; nonetheless, the difference between each centroid was detected with the value of 4.8447(15) Å.       In terms of the bond lengths, the comparison of bond distances involving the amide functional group demonstrated that N2-C7; 1.352(4) and C7-O3; 1.211(4) in compound B1 were relatively comparable to the bonds of N1-C8; 1.338(2) and C8-O2; 1.222(2) in compound B2. In addition, the bond that bound the nitrogen atom of the amide group and the phenyl ring was observed to be 1.408(4) and 1.419 (2) in compounds B1 and B2, respectively. This was attributed to the related equivalent strength of the -CF 3 electron-withdrawing group related to -NO 2 that created an almost equal electron density in the bond formation, leading to the similar bond lengths of such compounds. Some important bond lengths, bond angles and torsion angles are presented in Table 2.

Theoretical Calculations
For the calculations, the structures of B1 and B2 were optimized, as illustrated in Figure 7. The bond lengths for the C-N, N-H and N-C distances of B1 and B2 were 1.396Å

Theoretical Calculations
For the calculations, the structures of B1 and B2 were optimized, as illustrated in Figure 7. The bond lengths for the C-N, N-H and N-C distances of B1 and B2 were 1.396Å and 1.402 Å; 1.013 Å and 1.013 Å; 1.361 Å and 1.357 Å, respectively. There were no significant differences in the bond lengths' values in the optimized geometries of B1 and B2. However, optimized structures of B1 and B2 exhibited the existence of a strong H-bond (1.013 Å) belonging to N-H. The excitation energies, oscillator strengths (f) and transition states obtained from the TD-DFT calculations at the PBE0/6-311G(d,p) level using optimized ground state geometries for B1 and B2 are listed in Table 3. The calculated wavelengths with the maximum absorption values of B1 and B2 were 314 and 240 nm, respectively, which were slightly lower than the experimental results at 327 and 258 nm. According to the TD-DFT calculations, these strong absorptions corresponded to HOMO-1→ LUMO (S0→S3 state) and HOMO-2→LUMO (S0 → S4 state) transitions for B1 and B2, respectively. The results clearly show that the electronic transition of B1 with substituted (-NO2) is more effective than that of B2 with the trifluoromethyl (-CF3) group.
The molecular orbitals were related to the electronic transitions for both compounds, as presented in Figure 8. The structures of compounds B1 and B2 explained the contributions of HOMO-1, HOMO-2 and LUMO excitations. The HOMO-1 to LUMO and HOMO-2 to LUMO excitations corresponded to the internal charge transfer (ICT) process for the electronic spectra of compounds B1 and B2.  The excitation energies, oscillator strengths (f) and transition states obtained from the TD-DFT calculations at the PBE0/6-311G(d,p) level using optimized ground state geometries for B1 and B2 are listed in Table 3. The calculated wavelengths with the maximum absorption values of B1 and B2 were 314 and 240 nm, respectively, which were slightly lower than the experimental results at 327 and 258 nm. According to the TD-DFT calculations, these strong absorptions corresponded to HOMO-1→LUMO (S0→S3 state) and HOMO-2→LUMO (S0→S4 state) transitions for B1 and B2, respectively. The results clearly show that the electronic transition of B1 with substituted (-NO 2 ) is more effective than that of B2 with the trifluoromethyl (-CF 3 ) group. The molecular orbitals were related to the electronic transitions for both compounds, as presented in Figure 8. The structures of compounds B1 and B2 explained the contributions of HOMO-1, HOMO-2 and LUMO excitations. The HOMO-1 to LUMO and HOMO-2 to LUMO excitations corresponded to the internal charge transfer (ICT) process for the electronic spectra of compounds B1 and B2.

The Optical Properties of Compounds B1 and B2 by UV-Visible Spectroscopy
The maximum wavelength absorptions of compounds B1 and B2 in DMSO were at 327 and 258 nm, respectively. Upon the addition of the OHion to the B1 solution, an absorption wavelength of 327 nm disappeared. This indicated that a new band at 466 nm corresponded to the deprotonated species in the solution, as presented in Figure 9A. This mechanism was under the internal charge transfer process [24]. This phenomenon occurred under the π-π* transition that produced the red shift of the absorption wavelength.

The Optical Properties of Compounds B1 and B2 by UV-Visible Spectroscopy
The maximum wavelength absorptions of compounds B1 and B2 in DMSO were at 327 and 258 nm, respectively. Upon the addition of the OH − ion to the B1 solution, an absorption wavelength of 327 nm disappeared. This indicated that a new band at 466 nm corresponded to the deprotonated species in the solution, as presented in Figure 9A. This mechanism was under the internal charge transfer process [24]. This phenomenon occurred under the π-π* transition that produced the red shift of the absorption wavelength. In the case of B2, the absorption wavelength at 258 nm decreased and presented a new absorption wavelength at 303 nm upon the addition of OH − , as presented in Figure 9B. The mechanism was similar to that of B1. An obvious change can be observed in B1, rather than B2, because of the NO 2 group performing as an electron-withdrawing group, resulting in the NH of the amide functional group being a more acidic proton; therefore, the addition of OH − to the B1 solution led to the loss of a proton in the amide group. For the B2 compound, the CF 3 moiety is less powerful than the NO 2 group in B1, but B2 can lose the proton of the amide group. For the color change when adding OH − , as presented in Figure 10, the B1 solution changed from being colorless to an intense yellow color, but B2 did not change color. The color changes of the B1 and B2 solutions were consistent with the UV-Vis experiments. The mechanism was similar to that of B1. An obvious change can be observed in B1, rather than B2, because of the NO2 group performing as an electron-withdrawing group, resulting in the NH of the amide functional group being a more acidic proton; therefore, the addition of OHto the B1 solution led to the loss of a proton in the amide group. For the B2 compound, the CF3 moiety is less powerful than the NO2 group in B1, but B2 can lose the proton of the amide group. For the color change when adding OH -, as presented in Figure 10, the B1 solution changed from being colorless to an intense yellow color, but B2 did not change color. The color changes of the B1 and B2 solutions were consistent with the UV-Vis experiments.

The Interactions between Compounds (B1 and B2) and OH -Ion by 1 H NMR Spectroscopy
Additionally, the NH proton signals of B1 and B2 were 10.64 and 10.39 ppm, respectively. The OH proton signals of B1 and B2 are 9.33 and 9.34 ppm, as presented in Figures  11 and 12. Upon addition of OHin 1 equivalent, the NH and OH protons of both compounds disappeared due to the deprotonation process [25]. The CH2 and ArH protons of B1 and B2 exhibited an upfield shift because these protons gained an enhanced electron density. By adding 2-4 equivalents of OHto the B1 and B2 solutions, the proton peaks The mechanism was similar to that of B1. An obvious change can be observed in B1, rather than B2, because of the NO2 group performing as an electron-withdrawing group, resulting in the NH of the amide functional group being a more acidic proton; therefore, the addition of OHto the B1 solution led to the loss of a proton in the amide group. For the B2 compound, the CF3 moiety is less powerful than the NO2 group in B1, but B2 can lose the proton of the amide group. For the color change when adding OH -, as presented in Figure 10, the B1 solution changed from being colorless to an intense yellow color, but B2 did not change color. The color changes of the B1 and B2 solutions were consistent with the UV-Vis experiments.

The Interactions between Compounds (B1 and B2) and OH -Ion by 1 H NMR Spectroscopy
Additionally, the NH proton signals of B1 and B2 were 10.64 and 10.39 ppm, respectively. The OH proton signals of B1 and B2 are 9.33 and 9.34 ppm, as presented in Figures  11 and 12. Upon addition of OHin 1 equivalent, the NH and OH protons of both compounds disappeared due to the deprotonation process [25]. The CH2 and ArH protons of B1 and B2 exhibited an upfield shift because these protons gained an enhanced electron density. By adding 2-4 equivalents of OHto the B1 and B2 solutions, the proton peaks

The Interactions between Compounds (B1 and B2) and OH − Ion by 1 H NMR Spectroscopy
Additionally, the NH proton signals of B1 and B2 were 10.64 and 10.39 ppm, respectively. The OH proton signals of B1 and B2 are 9.33 and 9.34 ppm, as presented in Figures 11  and 12. Upon addition of OH − in 1 equivalent, the NH and OH protons of both compounds disappeared due to the deprotonation process [25]. The CH 2 and ArH protons of B1 and B2 exhibited an upfield shift because these protons gained an enhanced electron density. By adding 2-4 equivalents of OH − to the B1 and B2 solutions, the proton peaks presented greater upfield shift when compared to one equivalent of the OH − ion. This evidence indicates that the structures of B1 and B2 are changeable to a deprotonated form under basic conditions.

Conclusions
The orcinolic derivatives (B1 and B2) were synthesized and crystallized in the present study. The crystal structures of B1 and B2 were also stabilized by the hydrogen-bonding interaction. The π-π stacking interaction did not occur within intermolecular crystals. The DFT results indicate that the HOMO and LUMO of B1 and B2 are consistent with that of the UV-Vis results. The 1 H-NMR results show that the structures of B1 and B2 changed the resonance signals of aromatic and methylene protons upon the addition of OHions. Therefore, B1 and B2 can be used as hydroxide indicators.

Conclusions
The orcinolic derivatives (B1 and B2) were synthesized and crystallized in the present study. The crystal structures of B1 and B2 were also stabilized by the hydrogen-bonding interaction. The π-π stacking interaction did not occur within intermolecular crystals. The DFT results indicate that the HOMO and LUMO of B1 and B2 are consistent with that of the UV-Vis results. The 1 H-NMR results show that the structures of B1 and B2 changed the resonance signals of aromatic and methylene protons upon the addition of OHions. Therefore, B1 and B2 can be used as hydroxide indicators.

Conclusions
The orcinolic derivatives (B1 and B2) were synthesized and crystallized in the present study. The crystal structures of B1 and B2 were also stabilized by the hydrogen-bonding interaction. The π-π stacking interaction did not occur within intermolecular crystals. The DFT results indicate that the HOMO and LUMO of B1 and B2 are consistent with that of the UV-Vis results. The 1 H-NMR results show that the structures of B1 and B2 changed the resonance signals of aromatic and methylene protons upon the addition of OH − ions. Therefore, B1 and B2 can be used as hydroxide indicators.