1. Introduction

GSC

Green and Sustainable Chemistry

2160-6951

Scientific Research Publishing

10.4236/gsc.2020.102004

GSC-98790

Articles

Chemistry&Materials Science

A Density Functional Theory (DFT) Investigation on the Structure and Spectroscopic Behavior of 2-Aminoterephthalic Acid and Its Sodium Salts

Mohammad

A. Matin

¹Samiran

Bhattacharjee

¹^*Md.

Aftab Ali Shaikh

²Tapas

Debnath

³Mohammed

Abdul Aziz

Department of Theoretical and Computational Chemistry, University of Dhaka, Dhaka, Bangladesh

Department of Chemistry, University of Dhaka, Dhaka, Bangladesh

Centre for Advanced Research in Sciences (CARS), University of Dhaka, Dhaka, Bangladesh

11032020

100239554, February 20208, March 2020 11, March 2020

2014

This work is licensed under the Creative Commons Attribution-NonCommercial International License (CC BY-NC).http://creativecommons.org/licenses/by-nc/4.0/

As a substitute for lithium ion batteries, Na chemistry for ion battery systems is promising materials for energy storage applications for the next genera tion. Herein, the structures, IR and UV-visible spectra of 2-aminoterephthalic acid (H₂ATA), disodium 2-aminoterephthalate (Na₂ATA), trisodium 2-aminotere-phthalate (Na₃ATA) and tetrasodium 2-aminoterephthalate (Na₄ATA) have been studied using density functional theory (DFT/B3LYP/6-311++G(d,p)). The theoretical geometric parameters and FTIR results showed very good agreement with the experimental results. Different conformers of Na₂ATA, Na₃ATA and Na₄ATA showed that the binding energy per sodium in Na₂ATA, Na₃ATA and Na₄ATA is -694.94, -543.44 and -407.46 kJ/mol, respectively. The Na₃ATA and Na₄ATA salts are higher in energy (151.46 and 287.48 kJ/mol, respectively) than Na₂ATA, indicating the higher stability of the Na₂ATA complex. The calculated binding energy, enthalpy and Gibbs free energy of Na₂ATA, Na₃ATA and Na₄ATA revealed that the compounds are thermodynamically stable. Natural bond orbital (NBO) analysis of Na₂ATA, Na₃ATA and Na₄ATA indicated that the major interaction occurs between the lone pair electrons of the oxygen atom and anti-bonding orbitals of carbon atoms of the two carboxylate ions. UV-visible spectrum of the free H₂ATA and its sodium salts Na₂ATA, Na₃ATA and Na₄ATA were performed using the time-dependent density functional theory (TD-DFT) method at the level of B3LYP/6-311++G(d,p). The frontier molecular orbital energetic parameters and global reactivity descriptors revealed that the Na₄ATA and Na₃ATA complexes exhibited a higher band gap (ΔE_gap) and electronegativity ( χ eV ) than Na₂ATA.

2-Aminoterephthalic Acid Sodium 2-Aminoterephthalate Trisodium 2-Aminoterephthalate Tetrasodium 2-Aminoterephthalate Density Functional Theory

1. Introduction

Much attention has recently been paid to the establishment of environmentally friendly more acceptable routes, including removal of toxic reagents, minimization of by-product formation, low cost, green and easy procedure. Batteries play an important role as a power source in our everyday life such as mobile phones, microgrids, satellites, etc. Among the various metal ion batteries, lithium-ion batteries are comparatively mature technology having high energy density, power density and good long cycle life [1],but the high cost and low availability of certain materials are its main disadvantages [2]. Due to low cost and high natural abundance of sodium, the sodium ion batteries (SIBs) have gained much attention in recent years as an economically interesting alternative to lithium ion batteries for the future exploration [2] [3]. Recently, various cathode materials for sodium ion batteries have been studied, viz., olivine-type sodium metal phosphates, prussian blue, Na₃V₂(PO₄)₃/carbon, Cu-doped P2-Na_0.5Ni_0.33Mn_0.67O₂ encapsulated with MgO and titanium substituted P2-Type Na_0.67Fe_0.5Mn_0.5O₂ [4] - [9]. For anode materials in SIBs, carbon-based materials (such as graphene, hard carbon, carbon nanosheet and hollow carbon nanospheres), Na⁺ intercalation pseudocapacitance in TiO₂/graphene nanocomposites, amorphous phosphorus/carbon, carbon coated K_0.8Ti_1.73Li_0.27O₄ and carbon-coated NaTi₂(PO₄)₃ have been investigated [10] - [17]. Nanostructured and nanocomposites of organic conducting polymers have been studied in energy storage areas due to their numerous active sites which can generate green batteries with large capacity, high energy and long cycle life [18] [19] [20] [21]. A group of researchers reported the electrochemical performance of organic tetralithium salts of 2, 5-dihydroxyterephthalic acid having different morphologies viz., nanosheets, nanoparticles and bulk, as both positive and negative electrode of rechargeable lithium-ion batteries [22]. They observed that nanosheets morphologies exhibited the best electrochemical performance with discharge capacities of 223 and 145 mAh∙g⁻¹ at 0.1 and 5 C rates, respectively. Other organic electrode materials, such as, sodium salt of terephthalate and its various derivatives have been used as anode materials in sodium-ion batteries, which were prepared using simple acid-base chemistry [23]. These materials showed outstanding electrochemical activity [24]. In addition, tin, antimony and phosphorus easily formed alloy with sodium, which exhibited excellent electrochemical performance as an anode material for Na-ion batteries [24] [25] [26] [27]. Very recently, Li et al. described the sodium-ion storage on CuS nanosheets anchored into reduced graphene oxide as anode for SIBs [28]. These materials showed high specific capacity, high initial Coulombic efficiency, superior rate performance and excellent long-term cycle stability, suggesting that Na chemistry for ion battery systems will be feasible for energy storage applications for the next generation. As derivatives of terephthalic acid, the 2-aminoterephthalic acid (H₂ATA) have been used for organic building block for assembly of metal-organic framework compounds (for example, isoreticular metal-organic framework-3, IRMOF-3), in which –NH₂ groups of organic linker do not involve in the construction of framework structure [29] [30]. Most importantly, this uncoordinated amine group can serve as an active catalyst site for a variety of organic reactions [31] [32] [33] [34] [35] and also show as a selective adsorbent for harmful gases [36]. Karabacak et al. described the experimental and theoretical vibrational and electronic analysis of 2-aminoterephthalic acid [37]. Recently, Renault et al. reported the application of dilithium 2-aminoterephthalate as organic Li-battery anode material [38]. The resulting electrodes showed stable capacities (ca. 180 mAh∙g⁻¹) and excellent rate capabilities with battery performance at 500 mA∙g⁻¹. The above results encouraged us to carry out the detailed theoretical calculations of 2-aminoterephthalate (H₂ATA) and its sodium salts, aim to find out a sustainable, green and low-cost route towards the construction of sodium ion batteries.

In this study, we report the theoretical calculations of H₂ATA, disodium 2-aminoterephthalate (Na₂ATA) and its sodium inserted complexes (trisodium 2-aminoterephthalate, Na₃ATA and tetrasodium 2-aminoterephthalate, Na₄ATA) using Density Functional Theory (DFT) with the hybrid B3LYP method to calculate a wide variety of molecular properties such as optimized structure, binding energy (ΔE) per sodium and spectroscopic properties. NBO (natural bond orbital) analysis and global reactivity descriptors of 2-aminoterephthalic acid, disodium 2-aminoterephthalate and its inserted sodium complexes (Na₃ATA and Na₄ATA) were also performed to evaluate the strength of donor-acceptor interaction energy and chemical reactivity of this compound. Electronic properties and UV-Visible spectra were also calculated. To our knowledge, there has been no systematic theoretical study of 2-aminoterephthalic acid and its sodium salts using Density Functional Theory (DFT).

2. Computational Details

The geometries of the model complexes were optimized at the hybrid B3LYP [39] method based on Becke’s three-parameter functional of density functional theory (DFT) calculations using 6-311++G(d,p) basis set. Several structural configurations were considered for comparison of their stability. Geometry optimization was taken to be converged if the maximal atomic force was smaller than 0.00045 hartree/Bohr. Geometries of individual species ligand, metal and metal-complexes were optimized. No geometric constraint was imposed in all the calculations. After optimizing the geometry of each coordination complex, the metal−ligand binding energy ΔE was calculated as [40].

Δ E = − ( E complex − E metal − E ligand ) n

where, E_complex, E_metal and E_ligand are the energies of the sodium terephthalate complex, the metal ion and terephthalate ligand, respectively. Therefore, states to the binding energy of the complex per sodium.

The vibrational frequency analyses were performed for all optimized structures (no imaginary frequencies), and indicating that the structures are stable minima on the potential energy surface. It is known that DFT potentials systematically overestimate the vibrational wavenumbers. These discrepancies are corrected either by computing anharmonic corrections explicitly or by introducing a scaled field or by directly scaling the calculated wavenumbers with a proper factor. The raw vibrational frequencies were scaled by a factor of 0.9580, which produced good agreement with the experiment for a wide range of systems. All calculations were performed using the Gaussian 16 program package [41]. Gauss View 6.0.16 was used for the visualization of the optimized structures and simulated vibrational spectra.

Electronically excited state calculations were performed to examine the UV-visible spectra of the H₂ATA molecule and its sodium salts. The vertical excitation energies were obtained using the time-dependent density functional theory (TD-DFT) at the level of B3LYP with the 6-311++G(d,p) basis set, after the ground-state optimization. Molecular orbital analysis was also done to calculate the HOMO-LUMO energy gap. Natural bond orbital analysis was performed to provide the appropriate scheme for the metal-ligand interactions. The global reactivity descriptors were also analyzed to describe the molecular reactivity.

3. Results and Discussions3.1. Geometry of H2ATA

The three different optimized conformers of H₂ATA together with their energy with respect to the most stable structure are illustrated in Figures 1(a)-(c). Figure 1(a) is the most stable structure with minimum energy conformer where the C=O groups are on the same side. The second (Figure 1(b)) and third (Figure 1(c)) conformers are more than 0.76 and 11.81 kJ/mol, respectively, higher in energy than conformer 1a. The optimized geometrical parameters in both gas phase and different solvents are listed in Table 1. The bond lengths of both C-COOH (1) and C-COOH (2) in gas phase are slightly shorter (ca. 0.02Å) than experimental results (Table 1) [37]. Due to solvent effects, this bond length decreases almost by 0.018 Å than experimental. The C-NH₂ bond lengths both in gas phase and different solvents are calculated about 0.005 Å shorter than experimental result. There are no significant effects of solvents. Due to Coulombic interaction between O and H of COOH bond, C-O bond was calculated larger than C=O bond. The C=O bond is 0.005Å larger than experimental results and no such significant difference was found in other solvents. The calculated bond angles of two carboxylates are found to be 1.83˚ and 1.68˚ shorter than experimental results [37]. It is also noticed that the calculated bond angles in different solvents varies by 1.50˚ and 1.44˚ respectively. These calculated values are good agreements with the experimental results [37] except the NH₂ bond angles which are predicted shorter by 1.78˚ in gas phase and almost 2.90˚ in different solvents.

Table 1 Comparison of the theoretical (optimized) and experimental geometric parameters of H2ATA in gas phase and different solvents

Medium^a	Molecular Geometry^b
Medium^a	d_(C-O) (Å)	d_(C=O) (Å)	d_(C-N) (Å)	d_(Cg-C) (Å)	θ_(COO) (deg.)	θ ( NH 2 ) (deg.)
Gas	1.356 1.355	1.208 1.221	1.361	1.469 1.492	120.47 122.12	120.22
DMF	1.351 1.348	1.213 1.223	1.361	1.471 1.493	120.80 122.36	119.10
DMSO	1.351 1.348	1.213 1.223	1.360	1.471 1.493	120.80 122.36	119.10
EtOH	1.352 1.349	1.212 1.223	1.360	1.471 1.492	120.75 122.31	119.38
EtSH	1.352 1.349	1.212 1.223	1.360	1.471 1.492	120.75 122.31	119.38
Pyridine	1.351 1.348	1.213 1.223	1.360	1.471 1.493	120.78 122.34	119.20
FA	1.351 1.347	1.213 1.223	1.361	1.471 1.493	120.81 122.36	119.07
NBA	1.353 1.349	1.212 1.222	1.360	1.471 1.492	120.72 122.29	119.43
ACN	1.351 1.347	1.213 1.223	1.361	1.471 1.493	120.80 122.36	119.11
Exper.	1.330 1.333	1.195 1.216	1.365	1.489 1.512	122.3 123.8	122.0

[a] DMF = dimethylformamide, DMSO = dimethyl sulfoxide, EtOH = ethanol, EtSH = ethanethiol, FA = formamide, NBA = n-butylamine, ACN = acetonitrile. [b]d = bond length, d(Cg-C) = d(C_ring-C), θ = bond angle.

3.2. Geometries of Sodium Salts

The three different optimized structures of disodium 2-aminoterephthalate (Na₂ATA), sodium inserted complexes trisodium (Na₃ATA) and tetrasodium (Na₄ATA) 2-aminoterephthalate were shown in Figures 2-4 and the results were summarized in Table 2. A significant change of bond lengths of C-N and C_ring-C were observed in disodium, trisodium and tetrasodium salts of H₂ATA. The C-N bond lengths of tetrasodium salt were 0.055 Å larger than disodium salt. A significant change of bond angle of NH₂ was observed in disodium and its sodium inserted complexes and about 8.18˚ larger in disodium complex compare to trisodium and tetrasodium complex.

Different conformers of the C₈H₅Na_xNO₄ (x = 2, 3 or 4) were investigated by DFT calculations (Figures 2-4). In the case of C₈H₅Na₂NO₄, there is a negligible

Table 2 Geometrical parameters of Na2ATA, Na3ATA and Na4ATA (optimized lowest energy structure)

Complex	d C-O , s (Å)	d ′ C-N s (Å)	d ′ C ring -C s (Å)	θ ′ COO s (deg.)	θ NH 2 (deg.)
Na₂ATA	1.276	1.379	1.502	122.32	118.30
Na₃ATA	1.268	1.438	1.509	123.17	108.32
Na₄ATA	1.290	1.426	1.511	122.90	108.73

energy difference for the rotation of the carboxylate group in the meta position as compared to the amino group, but a relative increase in energy of 1.06 kJ/mol and 50.68 kJ/mol if the sodium is placed between the ortho-carboxylate and the amino group (Figure 2(b) and Figure 2(c)). The sodium ion naturally found in the unreduced carboxylate group, whereas retaining the energetically favorable location for one sodium atom near to the amino group.

According to Table 3, the binding energy, enthalpy and Gibbs free energy of Na₂ATA complex exhibit value on −694.94, −543.44 and −407.46 kJ/mol respectively and this suggests the thermodynamically most stability of the complex. The binding energies of Na₃ATA and Na₄ATA in the range of −543.44 to −407.46 kJ/mol, also suggest the thermodynamical stability. The per sodium energy difference of Na₂ATA is smaller (151.46 and 287.48 kJ/mol) compare to Na₃ATA and Na₄ATA, indicating the higher stability of the Na₂ATA complex. The binding energies, enthalpies and Gibbs free energy of disodium inserted complexes (Na₃ATA and Na₄ATA) are also tabulated in Table 3.

3.3. FTIR Spectra

The calculated infrared (IR) absorption frequencies of the compound and its sodium complexes in gasphase are listed in Table 4 and the spectra are shown in Figure 5. The calculated wavenumbers are scaled by a factor of 0.9580. The strong bands at 3615 and 3611 cm⁻¹ of free H₂ATA assigned to O-H stretching

Table 3 Binding energy (ΔE), enthalpy (ΔH) and Gibbs free energy (ΔG) of Na2ATA, Na3ATA and Na4ATA (optimized lowest energy structure)

Complex	ΔE (kJ/mol)	ΔH (kJ/mol)	ΔG (kJ/mol)
Na₂ATA	−694.94	−690.96	−657.90
Na₃ATA	−543.44	−539.73	−507.15
Na₄ATA	−407.46	−404.35	−372.96

Table 4 Characteristic IR bands (cm−1) for H2ATA, Na2ATA, Na3ATa and Na4ATAa

Complex	ν(OH)	ν_asy(NH₂)	ν_sy(NH₂)	νC=O	ν_asy(C-O)	ν_sy(C-O)	ν(C=C)	ν(C-N)
H₂ATA	3615 3611	3555	3405	1711 1670	-	-	1493	1250
Na₂ATA	-	3562	3369	-	1491	1394	1584	1228
Na₃ATA		3534	3386		1574	1361	1591	1196
					1522	1342
Na₄ATA	-	3529	3392	-	1566 1536	1367 1336	1587	1225

[a] ν = stretching vibration, ν_asy = asymmetric and ν_sy = symmetric.

vibrations of carboxylic groups, were disappeared on metal carboxylate formation [42]. The strong bands at 1711 and 1670 cm⁻¹ of free H₂ATA in FT-IR due to C=O stretching vibration are shifted to 1491 and 1394 cm⁻¹ in the disodium 2-aminoterephthalate complex, Na₂ATA, correspond to asymmetric ν_asy(C-O) and symmetric ν_sy(C-O) vibrations, respectively [43]. On the other hand, both trisodium 2-aminoterephthalate (Na₃ATA) and the tetrasodium 2-aminoterephthalate, Na₄ATA, exhibited four bands at ca.1574 and ca.1522 cm⁻¹, and at ca.1361 andca.1342 cm⁻¹, due to asymmetric ν_asy(C-O) and symmetric ν_sy(C-O) vibrations, respectively (Table 4). The FTIR spectra of H₂ATA and its sodium salts exhibited two bands at ca. 3550 and ca. 3390 cm⁻¹ due to the amino group [44]. In addition, all compounds showed band at ca. 1230 cm⁻¹ which may be assigned to the C-N stretching vibrations [45].

3.4. Natural Bond Orbital (NBO) Analysis

The NBO analysis was known to be effective tools for chemical elucidation of hyperconjugative interaction and electron density transfer from the filled lone pair electron [46]. Density Functional Theory with the hybrid B3LYP method was used for NBO calculation to examine the various second-order interactions between the filled orbitals of one subsystem andunoccupied orbital of another subsystem. NBO analysis of disodium, trisodium and tetrasodium 2-aminoterephthalate was carried out to evaluate the strength of donor-acceptor interaction energy, E(2) of these complexes and the results are summarized (disodium and tetrasodium only) in Table 5. The results showed the most effective interaction between the anti-bonding electrons of carbon (C₄-C₅) and carbon (C₁-C₆) of the π-conjugated system of the benzene ring. The results showed that the major interaction energies of this compound appeared from the interaction between the lone pair electrons of the O atom and antibonding orbitals of carbon atoms of the two carboxylate ions as well as sodium ions. There is also a significant

Table 5 Second order perturbation theory analysis of Fock matrix in NBO for the Na2ATA and Na4ATA in gas phasea

Complex	Na₂ATA			Na₄ATA
Donor(i)-Acceptor(j) Interaction	E² (kJ/mol)	E_j-E_i (a.u.)	F_ij (a.u.)	Donor(i)-Acceptor(j) Interaction	E² (kJ/mol)	E_j-E_i (a.u.)	F_ij (a.u.)
LP O1 0 → LP C4-C5 ∗	65.65	0.72	0.096	LP O1 0 → BD C4-O11 ∗	83.55	0.75	0.111
LP O1 0 → LP C9 ∗	722.91	0.15	0.158	LP O11 → BD C9-O1 0 ∗	304.51	0.30	0.132
LP O11 → LP C9 ∗	617.35	0.15	0.152	LP O13 → BD C12-O14 ∗	283.55	0.31	0.130
LP O13 → LP C12 *	720.36	0.15	0.158	LP O14 → BD C12-O13 ∗	84.35	0.75	0.111
LP O14 → LP C12 *	710.61	0.15	0.158	LP N16 → BD C4-O5 ∗	69.16	0.38	0.077
LP O1 0 * → LP Na12 *	16.07	0.76	0.006	BD C4-C5 ∗ → BD C1-C6 ∗	1270.14	0.01	0.083
LP O11 → LP Na12 *	16.23	0.79	0.050	LP O13 → LP C12 ∗	648.02	0.16	0.158
LP O13 ∗ → LP Na2 0 ∗	15.10	0.76	0.047	LP O14 → LP C12 ∗	656.80	0.16	0.158
LP O14 ∗ → LP Na2 0 ∗	15.10	0.76	0.047	LP O1 0 ∗ → LP Na19 ∗	13.68	0.82	0.046
				LP O11 → LP Na21 ∗	19.33	0.84	0.056
				LP O13 ∗ → LP Na2 0 ∗	14.94	0.81	0.048
				LP O14 ∗ → LP Na22 ∗	13.56	0.83	0.046

[a] LP = lone pair, LP* = antibonding lone pair, BD = bonding pair, BD* = antibonding.

interaction noticed with the lone pair electrons of nitrogen (amino group) to the anti-bonding of C₄-O₅.

3.5. Electronic Properties and UV-Visible Spectrum of H2ATA, Na2ATA and Sodium Inserted Complexes

The time-dependent DFT (TD-DFT) on electronic absorption spectrum of H₂ATA, Na₂ATA, Na₃ATA and Na₄ATA in gas phase were calculated using B3LYP/6-311++G(d,p) method. The major possible transitions, calculated frontier orbital energies, oscillator strengths (ƒ), excitation energies (eV) and molecular orbital (MO) major contributions listed in Table 6 and Table 7 respectively. The energy gap between the orbitals demonstrated the molecular chemical stability which is critical parameters in determining the molecular electrical

Table 6 Calculated wavelengths (λ), oscillator strengths (ƒ) and excitation energies (E) of H2ATA, Na2ATA, Na3ATA and Na4ATA at gas phase using TD-DFT/B3LYP/6-311++G(d,p) level of theory

Complex	λ(nm)	E(eV)	ƒ(Oscillator Strengths)	MO Contributions	Assignments
H₂ATA	225	5.52	0.3977	H → L+1(56%), H−1 → L(16%)	LLCT(π→π*)
	255	4.87	0.1297	H−1 → L(73%), H → L+1(25%)	LLCT(π→π*)
	260	4.76	0.0000	H−3 → L(90%), H−2 → L(4%)	LLCT(π→π*)
	270	4.59	0.0000	H−2 → L(91%), H−3 → L(4%)	LLCT(π→π*)
	365	3.39	0.0869	H → L(98%), H−1 → L+1(2%)	LLCT(n→π*)
Na₂ATA	260	4.76	0.1396	H−3 → L+2(46%), H−3 → L+1(16%)	LLCT(π→π^*)
	267	4.64	0.2047	H−3 → L+1(55%), H−6 → L+1(32%)	LLCT(π→π^*)
	272	4.55	0.0030	H → L+5(55%), H → L+6(40%)	LLCT(π→π^*)
	278	4.46	0.0026	H → L+3(70%), H → L+4(24%)	LLCT(π→π^*)
	285	4.35	0.0029	H → L+3(21%), H → L+4(50%)	LLCT(π→π^*)
	340	3.65	0.0989	H → L+2(96)	LLCT(n→π*)
Na₃ATA	235	5.28	0.0716	H−5 → L+1(70%)	LLCT(π→π*)
	251	4.93	0.0091	H → L+3(73%)	LLCT(π→π*)
	255	4.87	0.2060	H−5 → L+1(10%), H−3 → L+1(41%)	LLCT(π→π*)
	265	4.68	0.0252	H−2 → L+1(71%), H → L+3(18%)	LLCT(π→π*)
	288	4.31	0.0416	H−1 → L+1(88%)	LLCT(π→π*)
	307	4.03	0.0066	H−1 → L(89%)	LLCT(π→π*)
Na₄ATA	185	6.71	0.1024	H−4 → L+1(20%), H−1 → L+5(10%)	LLCT(π→π*)
	193	6.43	0.2045	H−1 → L+5(52%)	LLCT(π→π*)
	199	6.22	0.4060	H−1 → L+1(13%), H → L+5(37%)	LLCT(π→π*)
	219	5.66	0.0829	H−3 → L(10%), H−3 → L+1(33%)	LLCT(π→π*)
	228	5.43	0.0824	H → L(51%), H−3 → L+1(10%)	LLCT(π→π*)
	245	5.07	0.1268	H−1 → L(17%), H−1 → L+1(47%)	LLCT(π→π*)
	267	4.65	0.0523	H → L(17%), H → L+1(64%)	LLCT(π→π*)

Table 7 Frontier molecular orbital energetic parameters of free H2ATA, Na2ATA, Na3ATA and Na4ATA at gaseous statea

Complex	E_HOMO(eV)	E_LUMO(eV)	ΔE_gap(eV)	I(eV)	A(eV)
H₂ATA	−6.24	−2.38	3.86	6.24	2.38
Na₂ATA	−4.79	−1.47	3.32	4.79	1.47
Na₃ATA	−8.90	−4.35	4.55	8.90	4.35
Na₄ATA	−12.02	−7.03	4.99	12.02	7.03

[a] ΔE_gap = Energy gap, I = ionization potential, A = electron affinity.

transport properties owing to electron conductivity [47]. The chemical and spectroscopic properties of the molecules are mainly depending on the energy gaps. The frontier molecular orbitals show the electron density for predicting the most reactive position in π-electron systems and also explain several types of reaction in conjugated system [48]. The frontier molecular orbitals (HOMO and LUMO) of free H₂ATA are shown in Figure 6. In free H₂ATA molecule, the LLCT (Ligand to ligand charge transfer) bands are mainly observed at 185 nm, 224 nm and 365 nm indicating π→π* and n→π* transitions. However, TD-DFT data demonstrated that LLCT bands appeared at 185 - 224 nm. The sharp band appeared at ~224 nm. The molecular orbital contribution (56%) at this band in the gas phase showed the major transitions occurred between the highest occupied molecular orbital (HOMO) to lowest unoccupied molecular orbital+1 (LUMO+1) and the energy gap between HOMO and LUMO+1 was 5.52 eV for H₂ATA. An electronic system with a larger HOMO-LUMO gap should be less reactive than one having a smaller gap. The HOMO-LUMO (ΔE_gap) gap of the present studied molecule H₂ATA is 3.86 eV (Figure 6), indicating the high reactivity. Whereas in the metal complexes, Na₂ATA and Na₄ATA, the major transitions occur at 267 nm and 199 nm, respectively, due to LLCT (π→π*) transition. The molecular contribution (55%) at 267 nm band for Na₂ATA exhibited the major transitions occurred between the highest molecular orbital-3 (HOMO-3) to lowest unoccupied molecular orbital+1 (LUMO+1).

3.6. Global Reactivity Descriptors of H2ATA, Na2ATA and Its Sodium Inserted Complexes (Na3ATA and Na4ATA)

The global reactivity descriptors, e.g. electronegativity (χ), chemical potential (μ), global hardness (η), global softness (s), electrophilicity index (ω) were determined by the conceptual density functional theory on the basis of Koopmans’s theorem [49]. The global reactivity descriptors of the titled molecule and its sodium salts were calculated. Global reactivity descriptors were calculated using the energies of frontier molecular orbitals E_HOMO and E_LUMO as χ = −1/2(E_LUMO + E_HOMO), μ = −χ = 1/2(E_LUMO + E_HOMO), η = 1/2(E_LUMO − E_HOMO), ѕ = 1/2η and ω = μ²/2η. The energies of frontier molecular orbitals, (E_LUMO and E_HOMO) and global reactivity descriptors of H₂ATA Na₂ATA, Na₃ATA and Na₄ATA are listed in Table 6 and Table 7. The studied molecules, H₂ATA and

Table 8 Quantum chemical descriptors of free H2ATA, Na2ATA, Na3ATA and Na4ATAa

Complex	χ(eV)	μ(eV)	η(eV)	ѕ(eV)	ω(eV)
H₂ATA	4.310	−4.310	1.930	0.259	4.81
Na₂ATA	3.130	−3.130	1.662	0.301	2.95
Na₃ATA	6.625	−6.625	2.275	0.219	9.65
Na₄ATA	9.525	−9.525	2.495	0.200	18.18

[a] χ = electronegativity, μ = chemical potential, η = global hardness, ѕ = global softness, ω = electrophilicity index.

Na₂ATA showed a higher HOMO-LUMO gap in gas phase signifying harder molecule. The free H₂ATA exhibited higher value for global electrophilicity index, hardnessand electronegativity than Na₂ATA (Table 8).

4. Conclusion

In summary, we investigated the structural and vibrational properties of 2-aminoterephthalic acid, disodium 2-aminoterephthalate and inserted sodium complexes using density functional theory (DFT/B3LYP) methods with 6-311++G(d,p) basis set. The calculated binding energy, enthalpy and Gibbs free energy of Na₂ATA revealed that this compound is thermodynamically more stable than other inserted sodium complexes such as Na₃ATA or Na₄ATA. NBO analysis of disodium 2-aminoterephthalate exhibited the major interaction energy of the O atom with the carbon atoms of the two carboxylate ions as well as its sodium ions. The UV-visible spectrum of the 2-aminoterephthalic acid indicated that molecular orbital contribution (56%) occurred between the highest occupied molecular orbital (HOMO) and the lowest unoccupied molecular orbital+1 (LUMO+1), whereas, in the case of disodium salt, molecular orbital contribution (55%) occurred between the highest molecular orbital-3 (HOMO-3) and lowest unoccupied molecular orbital+1 (LUMO+1). In terms of the global reactivity descriptors, H₂ATA showed higher electronegativity than Na₂ATA. The present computational study of the 2-aminoterephthalic acid and its sodium salts provide strong encouragement for future exploration of functionalized terephthalic acid derivatives as useful material for the safe, low cost, non-toxic, green and easy technology for the production of sodium ion batteries for industrial application.

Acknowledgements

Financial support of this work by the Centre for Advanced Research in Sciences (University of Dhaka, Dhaka, Bangladesh) is greatly appreciated.

Conflicts of Interest

The authors declare no conflicts of interest regarding the publication of this paper.

Cite this paper

Matin, M.A., Bhattacharjee, S., Shaikh, M.A.A., Debnath, T. and Aziz, M.A. (2020) A Density Functional Theory (DFT) Investigation on the Structure and Spectroscopic Behavior of 2-Aminoterephthalic Acid and Its Sodium Salts. Green and Sustainable Chemistry, 10, 39-55. https://doi.org/10.4236/gsc.2020.102004

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