Synthesis, Characterization and Preliminary Study on Acetylpyrazine N(4)Butylthiosemicarbazone as a Potential CDK2 Inhibitor Combined with DFT Calculations

Abstract

In this study, a new thiosemicarbazone ligand, namely acetylpyrazine N(4)butylthiosemicarbazone (APBT), was synthesized and characterized using ¹H and ¹³C nuclear magnetic resonance (NMR) and Fourier transform infrared (FTIR) spectroscopies. Quantum chemical calculations were performed using density functional theory at the B3LYP/6-311++G(d,p) basis set level. The optimized molecular geometry of APBT is discussed based on X-ray structural reports from the literature. The assignment of the vibrational frequencies was done based on a potential energy distribution analysis using the vibrational energy distribution analysis (VEDA) 4 software. The energy gap between the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) was evaluated to study the reactivity and stability of the compound. Global chemical reactivity and local reactivity descriptors of reactants and the product (APBT) were calculated to study the reaction mechanism. The region of interaction during the reaction to form APBT was determined using molecular electrostatic potential analysis. Finally, a preliminary study of the title compound as a cyclin-dependent kinase (CDK) inhibitor was further evaluated by performing a docking calculation.

Keywords:
thiosemicarbazone; DFT; global reactivity descriptors; CDK inhibitor

Introduction

Thiosemicarbazones and their derivatives have shown significant interest in areas of chemistry and biology.¹ The thiosemicarbazone ligand itself can be used for metal analysis,² for device applications related to telecommunications, optical computing, storage and information processing.³ Thiosemicarbazones are versatile compounds that exist as three structural isomers (E, E' and Z)⁴ and can coordinate to a metal either as a neutral ligand or as a deprotonated ligand.⁵ The common thiosemicarbazone ligand acts as a bidentate ligand through the azomethine nitrogen and thiocarbonyl sulfur atom. The ligand can bind in a multidentate fashion when the N1 position of the thiosemicarbazone moiety is substituted with a carbon a to an aldehyde or ketone group that has atoms of different electronegativity. The presence of a NH-C=S group results in tautomerism of the thiosemicarbazone to form a thione or thiol.⁶ Moreover, thiosemicarbazones have shown a wide spectrum of biological properties, including antibacterial,⁷ antifungal,⁸ and anticancer.⁹ Cancer still remains one of the most feared diseases and a major cause of death in the modern world. Cyclin-dependent kinases (CDKs) as controllers in the cell cycle are overexpressed and overactive in many cancer cells. Ongoing study is being undertaken to find effective CDK inhibitors to overcome this problem.

In this study, the potential of the title compound was used to study the cyclin-dependent kinase 2 (CDK2) protein receptor activity, which is one of the CDK family, by using in silico calculations. The CDK2 inhibitor is involved in anticancer treatment for lung cancer.¹⁰ The unique properties of thiosemicarbazone ligands as a potential CDK2 inhibitor led us to the aim of the present work: to characterize in detail the chemical properties of thiosemicarbazone ligands using the density functional theory (DFT) method. The DFT functions act in a semi-empirical fashion to account for the electron correlation and have been extended to include other corrections such as dispersion.¹¹ Using this method, the highest occupied molecular orbital (HOMO) and lowest unoccupied molecular orbital (LUMO) energies were calculated to characterize global chemical reactivity parameters such as the chemical potential (µ), hardness (η), softness (s), electronegativity (χ) and electrophilic index (ω). In addition, Fukui functions were used to explain the selectivity of each atom in the reaction to become an electrophile or a nucleophile in the reaction mechanism. The data from the calculation was used to evaluate the correlations between experiment and theory for the Fourier transform infrared (FTIR) spectroscopy. The optimized structure using DFT calculation was further used to study the potential of the title compound against the CDK2 macromolecule as anticancer therapeutic using a computational drug design approach.

Results and Discussions

¹H and ¹³C nuclear magnetic resonance (NMR) spectroscopies

Proton and carbon NMR spectroscopies are helpful and powerful tools for identification of organic compounds in conjunction with other spectrometric information, in addition to X-ray crystallography. Recrystallization from various solvents was attempted to produce single crystals. However, it was unsuccessful. Figure S1 (Supplementary Information (SI) section) shows the numbering used for assignment of ¹H and ¹³C NMR chemical shift signals for N(4)butylthiosemicarbazone (APBT). The characterization of APBT was carried out in deuterated dimethyl sulfoxide (DMSO-d₆) solution using tetramethylsilane (TMS) as an internal standard. The data collected is presented in Table 1. The two proton signals of N(20) and N(16) were observed at δ 10.13 and 9.79 ppm, respectively, confirming that the ligand form is a thione compound. The most shielded proton, appearing as a triplet signal at δ 0.54 ppm, corresponds to the methyl group from C(31). The signal of the protons from the methyl group C(11) was identified as a single signal at δ 2.50 ppm. In the ¹³C NMR spectrum, the most downfield signal, appearing at δ 170.38 ppm, corresponds to the C(18) atom, while the signal of carbon C(10) appeared at δ 145.88 ppm. The C(10) signal was shielded compared with the C(18) because C(18) are bonded to the two nitrogen and sulfur, while C(10) are bonded to the two carbon and nitrogen atoms, respectively. The signal of the most shielded carbon atom, appearing at δ 12.34 ppm, corresponds to the methyl group of C(31).

Table 1
¹H and ¹³C NMR data of APBT

APBT	Chemical shift / ppm
N(16)–H	10.13 (s, 1H)
N(20)–H	9.79 (s, 1H)
C(5)–H	9.65 (s, 1H)
C(2)–H	8.62 (d, 2H)
C(11)–H	2.50 (s, 3Hs)
C(22)–H	1.70 (t, 2H)
C(28)–H	1.48 (m, 2H)
C(25)–H	1.39 (m, 2H)
C(31)–H	0.54 (t, 3H)
C18	170.38
C4	150.99
C5	150.70
C10	145.88
C2	144.77
C1	143.95
C22	30.99
C25	19.88
C28	18.35
C11	13.11
C31	12.34

• APBT: N(4)butylthiosemicarbazone.

Molecular geometry

The optimized structure of APBT calculated using Becke, 3-parameter, Lee-Yang-Parr (B3LYP) 6-311++G(d,p) basis set is shown in Figure 1. Comparison between selected bond lengths and bond angles was made with the other X-ray crystallographic structure¹² (Cambridge Structural Database (CSD) No. 820252) from a similar system since the crystal structure of this compound is not available. The experimental and calculated geometric parameters of APBT are listed in Table S1 (SI section). The calculated bond length of C-S was 1.681 Å, while the experimental data provided 1.680 Å. The calculated and experimetal data showed the bond length was assigned to the double bond character of C-S in a thione compound.^13,14 For the thiosemicarbazone moiety, the bond length of C10-N15 was 1.296 Å, while the experimental data provided 1.284 Å, with differences assigned to the double bond character as well.¹⁵ Due to the tautomerization around S19-C18-N20, the calculated and experimetal bond length of C18-N20 is slightly shorter compared to the C18-N16 with values of 1.343 and 1.337, and 1.386 and 1.373 Å, respectively. The selected single bonds were C4-C10, C10-C11, N15-N16, and N20-C22, calculated as 1.481, 1.506, 1.349, and 1.409 Å, respectively; the experimental data provided 1.485, 1.500, 1.366, and 1.409 Å, respectively. The value of correlation coefficient (R² = 0.97639) shown in Figure S2 (SI section) also confirmed that there is a good agreement between experimental and calculated results. The slightly deviated geometric parameters between the calculated and experimental data are likely due to the fact that the theoretical calculations were made on the molecule in the gas state/in a vacuum while the experimental results were for the solid state.¹⁶

Figure 1
The optimized molecular structure of APBT.

Vibrational analysis

The experimental IR spectrum and the calculated data using B3LYP/6-311++G(d,p) are shown in Figure 2. For comparison, the scaled calculated harmonic vibrational frequencies at the B3LYP/6-311++G(d,p) level, the selected data between experimental and theoretical vibrational frequencies, and the details of the percentage of potential energy distribution (PED) assignment have been tabulated in Table 2.

Figure 2
Experimental and calculated IR spectra of APBT using B3LYP/6-311++G(d,p).

Table 2
Selected experimental and theoretical vibrational frequencies of APBT with B3LYP6-311++G(d,p)

Experimental frequency / cm-1	Calculated frequency / cm-1		Intensity	Vibrational assignment (PED ≥ 10 / %)
	Unscaled	Scaled
3363	3587	3453	53.59	n[(N20H21)] (99)
3219	3571	3438	35.78	n[(N16H17)] (99)
3096	3210	3090	4.30	n[(C5H9)] (96)
3080	3192	3073	48.20	n[(C1H7)] (93)
2929	3049	2935	40.63	n[(C22H23)] (85)
2867	3024	2911	25.51	n[(C28H29)] (13)
1630	1660	1598	63.95	n[(N15C11)] (63)
1599	1612	1552	29.64	n[(N15C10)] (52) + d[(H8C2N3)] (21)
1504	1582	1523	139.60	n[(N6C5)] (69)
1470	1541	1484	264.09	d[(H17N16N1)5] (53)
1464	1522	1465	3.67	d[(H32C31H33)] (68) +t[(H29C28C31H33)] (10)
1176	1217	1172	359.38	n[(N16C18)] (41) + t[(H29C28C25C22)] (10)
1113	1180	1136	33.01	n[(N15N160)] (17) + t[(H29C28C25C22)] (26)
1104	1171	1127	60.45	n[(N15N16)] (38)
1064	1096	1055	55.20	n[(C22C25)] (30) + n[(S19C18)] (30) + t[(H33C31C28C25)] (10)
1008	1055	1016	0.26	g[(H13C11H14)] (14) + t[(C11H12C10H13)] (72)
800	856	824	29.52	n[(S19C18)] (25) + d[(C1C2N3)] (14)
641	672	647	7.31	n[(S19C18)] (11) + d[(C11C10N15)] (46)
417	423	407	12.83	t[(C2C1N6C5)] (84)

• PED: potential energy distribution; n: stretching; d: in-plane bending; g: out-of-plane bending; t: torsion.²¹

N-H vibrations

The two N-H stretching vibrations observed occurred at 3363 and 3219 cm^-1,^17,18 while the calculated theoretical values were found to be 3453 and 3438 cm^-1.¹⁹ Based on the results of the PED analysis shown in Table 3, the N-H bending vibrations were found at 1529, 1484, 1341 and 1279 cm^-1.²⁰ In the experimental data, the only vibration found was at 1470 cm^-1.²¹

Table 3
Calculated HOMO and LUMO energies, energy gap, electronegativity, chemical potential, global hardness, global softness, global electrophilicity index and additional electronic charge for reactants A and B, and the title compound using B3LYP/6-311++G(d,p)

	EH / eV	EL / eV	EH – EL / eV	µ / eV	c / eV	h / eV	s / eV-1	w / eV	–µ / h	ECT
Reactant A	–7.0314	–5.5378	–1.4936	–6.2846	6.2846	0.7468	0.6695	26.4436	8.4154	–
Reactant B	–9.7863	–4.6483	–5.138	–7.2173	7.2173	2.5690	0.1946	10.1381	2.8094	5.6056
APBT	–7.5514	–5.4371	–2.1143	–6.4943	6.4943	1.0572	0.4729	19.947	–	–

• E_H and E_L: calculated HOMO and LUMO energies, respectively; µ: chemical potential; c: electronegativity; h: global hardness; s: global softness; w: global electrophilicity index; –µ / h: additional electronic charge; ECT: electrophilicity-based charge transfer; APBT: N(4)butylthiosemicarbazone.

C-H_pyrazine vibrations

C-H stretching for the pyrazine ring occurred at a higher wavenumber compared to the C-H stretching for CH₂ or CH₃ in this compound. The theoretical calculated C-H stretching vibrations for the pyrazine ring were found at 3090 and 3073 cm^-1;²⁰ these two peaks were assigned in the experimental spectrum at 3096 and 3080 cm^-1.²²

CH₂ and CH₃ vibrations

The observations show that CH₂ stretching peaks were found at 2935 and 2911 cm^-1.²³ The experimental only showed the two peaks at 2929 and 2867 cm^-1.²¹ The calculated in-plane and out-of-plane bending vibrations of methyl group were assigned at 1465 and 1016 cm^-1.^23,24 The experimental bending vibrations for methyl group were found at 1464²⁵ and 1008 cm^-1.²⁶

C=N and C-N vibrations

The highest wavenumber of C=N was observed in the recorded FTIR spectrum at 1630 cm^-1, assigned to the C=N stretching vibration in the thiosemicarbazone moiety.^27,28 The calculated value was 1598 cm^-1.²⁰ The ring C=N stretching vibrations in the pyrazine ring were observed in the region of 1599-1504 cm^-1;^16,29 these wavenumbers were found at 1552, 1529 and 1523 cm^-1 in the calculation computed by B3LYP/6-311++G(d,p).³⁰ The calculations also showed that the assymmetric and symmetric stretching vibration of N16-C18-N20 occured at 1529 and 1172 cm^-1, respectively. The C18-N16 stretching mode corresponding to experimental value was found at 1176 cm^-1.^30,31 The details of vibrational frequencies can be seen in Table S5 (SI section).

C=S vibrations

The calculated wavenumbers of C=S stretching were 1055, 824 and 647 cm^-1,^20,23 with PED contributions of 30, 25 and 11%, respectively. The experimental spectrum showed bands for C=S stretching at 1064, 800 and 641 cm^-1.^32-34 The absent band at 2500 cm^-1 in the recorded and calculated spectra indicates that in both the solid state and as a gas/in a vacuum, the ligand remains as a thione tautomer.

N-N vibrations

The calculated N-N stretching vibrations with PED contributions of 17 and 38% were found at 1136 and 1127 cm^-1.^23,34 In the recorded FTIR spectrum, these were observed at 1113 and 1104 cm^-1, as reported in the literature and assigned to N-N stretching vibrations.³⁵ The calculated in-plane bending vibration for H-N-N was found at 1484 cm^-1 and the experimental showed peak at 1470 cm^-1.²¹

Global reactivity descriptors

Global reactivity descriptors were evaluated to understand the relationship between structure, stability and global chemical reactivity. The energy levels of HOMO and LUMO play specific roles for all parameters. HOMO is the orbital that acts as an electron donor while LUMO is the orbital that acts as the electron acceptor. The 3D plots of selected molecular orbitals and the energy gap of each electronic transition are shown in Figure 3. As seen from Figure 3, the HOMO orbital is mainly localized over S19 while LUMO orbital is mainly delocalized over pyrazine ring. The Figure represents n-p* electronic transition of the title compound. The highest energy gap was found at -2.1143 eV, which indicated the most stable electronic transition of the title compound.

Figure 3
Energies of the molecular orbitals.

The global chemical reactivity parameters, such as chemical potential (µ), electronegativity (χ), chemical hardness (η), global softness (s), global electrophilicity index (ω)^36-40 and electrophilicity-based charge transfer (ECT)⁴¹ of reactant A, reactant B and APBT, were evaluated from the HOMO and LUMO energy levels using the following equations. The results are listed in Table 3.

(1) $\mathit{\mu }=\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.\left(\mathit{I}+\mathit{A}\right)=-\mathit{\chi }$

(2) $\mathit{\eta }=\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.\left(\mathit{A}-\mathit{I}\right)$

(3) $\mathit{s}=\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2\mathit{\eta }$}\right.$

(4) $\mathit{\omega }=\raisebox{1ex}{${\mathit{\mu }}^2$}\!\left/ \!\raisebox{-1ex}{$2\mathit{\eta }$}\right.$

(5) $\mathit{ECT}=\left(\Delta {\mathit{N}}_{\max }\right)\mathit{A}-\left(\Delta {\mathit{N}}_{\max }\right)\mathit{B},\mathit{where}\left(\Delta {\mathit{N}}_{\max }\right)=-\raisebox{1ex}{$\mathit{\mu }$}\!\left/ \!\raisebox{-1ex}{$\mathit{\eta }$}\right.$

Figure S3 (SI section) shows the optimized geometries of the reactants and product involved in the chemical reaction calculated at the B3LYP/6-311++G(d,p) level. The calculated energy gap of frontier molecular orbital of reactant A is -1.4936 eV, while reactant B is -5.138 eV, respectively. The value indicates that reactant B is more reactive than reactant A. The hard molecule has high value of hardness (reactant B) contributed from the large energy band gap, while soft molecule has high value of softness (reactant A) contributed from small energy gap.³⁸ The calculated data also show that reactant A has a high value of chemical potential (-6.2846 eV) and a high electrophilicity index (26.4436 eV), so it acts as the electrophile, while the high value of electronegativity (7.2173 eV) shows that reactant B acts as the nucleophile. The ECT value of 5.6056 (ECT > 0) also shows that charge flow from reactant B to reactant A indicates that reactant B acts as nucleophile while reactant A acts as electrophile.

Fukui function

The Fukui function is a method in quantum chemistry used by chemists to recognize and provide information on which atom in a molecule has a greater tendency to either lose or accept an electron. The function also defines which atom is more prone to nucleophilic or electrophilic attack, respectively. The Fukui function is a local reactivity descriptor that indicates the preferred regions where a chemical species will change its density when the number of electrons is modified. It is defined as⁴²

(6) $\mathit{f}\left(\mathit{r}\right)=\frac{\mathit{\delta }\mathit{\rho }\left(\mathit{r}\right)}{\partial \mathit{N}}\mathit{r}$

where r(r) is the electronic density, N is the number of electrons and r is the external potential exerted by the nucleus. (f_k⁺, f_k^-, f_k⁰) were calculated using the following equations:

(7) ${\mathit{f}}_{\mathit{k}}^{+}=\left[\mathit{q}\left(\mathit{N}+1\right)-\mathit{q}\left(\mathit{N}\right)\right]\mathit{for}\mathit{nucleophilic}\mathit{attack}$

(8) ${\mathit{f}}_{\mathit{k}}^{-}=\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.\left[\mathit{q}\left(\mathit{N}+1\right)-\mathit{q}\left(\mathit{N}-1\right)\right]\mathit{for}\mathit{electrophilic}\mathit{attack}$

(9) ${\mathit{f}}_{\mathit{k}}^0=\raisebox{1ex}{$1$}\!\left/ \!\raisebox{-1ex}{$2$}\right.\left[\mathit{q}\left(\mathit{N}+1\right)-\mathit{q}\left(\mathit{N}-1\right)\right]\mathit{for}\mathit{radical}\mathit{attack}$

where N, N - 1, N + 1 are the total electrons present in the neutral, cationic and anionic states of the molecule, respectively. The local softness (s_k⁺, s_k^-, s_k⁰) and local electrophilicity indices (ω_k⁺, ω_k^-, ω_k⁰) were also evaluated to determine the selectivity of active sites in the molecule. The calculations of the selected reactivity sites of the reactants A and B are given in Table 4. The maximum value of the local descriptor prone to nucleophilic attack (f_k⁺, s_k⁺, ω_k⁺) was found for the C18 atom (reactant A) which had values of (0.1972, 0.0736, 5.2149), while the N14 atom (reactant B) had the maximum (f_k^-, s_k^-, ω_k^-) values of (0.6822, 1.4811, 2.3286) and is prone to electrophilic attack.

Table 4
Selected electrophilic reactivity descriptors (fk+, sk+, ωk+) for reactant A and nucleophilic reactivity descriptors (fk–, sk–, ωk–) for reactant B using Mulliken charge analyses

Reactant A					Reactant B
Site	fk+	sk+	ωk+		Site	fk–	sk–	ωk–
C10	0.1875	0.07	4.9594		N14	0.6822	1.4811	2.3286
C18	0.1972	0.0736	5.2149

• f_k⁺, s_k⁺, w_k⁺: Fukui function, softness and electrophilicity indices, respectively, for electrophilic reactivity; f_k^–, s_k^–, w_k^–: Fukui function, softness and electrophilicity indices, respectively, for nucleophilic reactivity.

Atomic charge analysis

The charge distribution of the molecule was calculated on the basis of the Mulliken method using B3LYP/6-311++G(d,p) level calculations. This calculation depicts the charges of every atom in the molecule. Mulliken population analysis computes charges by dividing the orbital overlap evenly between the two atoms involved.⁴³ As shown in Figure 4, the atoms which exhibit a negative charge are N3, N6, C11, N15, N16, S19, N20, C22, C25, C28 and C31, while C1, C2, C4, C5, C10, and C18 exhibit positive charges. All hydrogen atoms possess positive charges. The maximum negatively charged atom (N20) is in the neighborhood of the maximum positively charged atom (C18).

Figure 4
Bar diagram representing the charge distribution of APBT.

Molecular electrostatic potential

The molecular electrostatic potentials (MEP) of the reactants and product in 3D plots are illustrated in Figure 5. Molecular electrostatic potential is widely used as a reactivity map displaying the regions for electrophilic and nucleophilic attack.^44-46 As can be seen, the region of the C18 atom of reactant A is in green, indicating that it experiences the strongest repulsion, while the region surrounding the N14 atom is in red, and therefore experiences the strongest attraction in the reaction mechanism. The region of N14 in reactant B acts as the nucleophile and has the strongest attraction for the region of C18 in reactant A, which acts as the electrophile to form the title compound.

Figure 5
Molecular electrostatic potential for the reactants and the title compound.

Molecular docking

The CDK2 complex data file was obtained from the Protein Data Bank. CDK as a protein receptor was prepared by removing the waters and cocrystallized ligand using Discovery Studio Visualizer.⁴⁷ Calculation of the interaction between the optimized title compound and the protein receptor CDK2 within the grid box size of 30 × 30 × 30 ų showed the formation of a stable complex with value -6.4 kcal mol^-1 (Table 5). As shown in Figure 6, the interaction of amino acid ASP 145 forms a π anion (3.58 Å) with the pyrazine ring, GLN 131 forms a hydrogen bond (2.07 Å) with N(16)H, ASN 132 forms a carbon hydrogen bond (3.59 Å) with C(5)pyrazine and PHE 80 forms a π-σ (3.56 Å) interaction with C(31). The preliminary results suggest that the title compound has potential as an inhibitor of the CDK2 protein.

Table 5
The binding affinity values of different poses of the title compound

Mode	Affinity / (kcal mol-1)	Distance from the best mode / Å
		RMSD 1b	RMSD ub
1	–6.4	0.000	0.000
2	–6.3	4.334	7.190
3	–6.2	2.099	3.182
4	–6.1	3.087	6.067
5	–6.1	2.830	6.546
6	–5.9	4.667	7.154
7	–5.9	3.837	6.408
8	–5.8	1.939	2.908
9	–5.8	3.789	6.727

• RMSD: root mean square deviation; lb: lower bound; ub: upper bound.

Figure 6
Two-dimensional interaction of APBT with amino acid residues shown as balls colored by the type of interaction.

Conclusions

A thiosemicarbazone ligand (APBT) was synthesized and characterized using elemental analysis, NMR and FTIR spectroscopies. The calculation using B3LYP/6-311++G(d,p) was used to compute the chemical properties of the new ligand. The optimized geometric parameters and vibrational frequencies were compared with the experimental data. The small energy gap frontier molecular orbital of reactant B indicates that the molecule is more reactive than reactant A. Reactant A has high value of softness (0.6695 eV^-1), chemical potential (-6.2846 eV) and electrophilicity index (26.4433 eV), and acts as electron acceptor or electrophile, while reactant B, which has high value of hardness (2.569 eV) and electronegativity (7.2173 eV), acts as electron donor or nucleophile, forming the title compound. The specific sites within the molecule that acted as the electrophile and nucleophile were identified using the Fukui function. The result shows atom C(18) from reactant A is prone to nucleophilic attack, while N(14) from reactant B is prone to electrophilic attack. The 3D MEP plots also helped to show the regions of the reaction active sites in reactants A and B. These results will be used to design and synthesize new potential inhibitors for the CDK2 protein, which is attractive for anticancer treatment.

Experimental

The melting point was obtained on an Electrothermal 9300 digital melting point apparatus. Elemental analysis of APBT was performed using CHN-S Fison EA 1108 and IR spectra was recorded using KBr on a Perkin Elmer FTIR GX spectrometer. The ¹H and ¹³C NMR spectra were recorded in parts per million (ppm) using JEOL ECP 400 MHz spectrometer in DMSO-d₆ and were referenced to the residual solvent peak.

Procedure for acetylpyrazine N(4)butylthiosemicarbazone (APBT)

All the chemicals used were of analytical grade. Methyl 3-[1-(2-pyrazyl)ethylenediene]hydrazinecarbodithiote (0.68 g, 3 mmol) was dissolved in hot butanol (300 mL), and butylamine (0.26 g, 3 mmol) was added, then the mixture was refluxed for 24 h.⁴⁸ A yellow precipitate formed after the solution was evaporated for 14 days. The product was filtered off and dried in a desiccator. The product yield was 59% and the melting point was 189-191 ºC. The elemental analysis showed C 53.20, H 6.73, N 28.40, S 11.67%, whereas the calculated formula was C₁₁H₁₇N₅S; C 52.56, H 6.82, N 27.86, S 12.76%; IR (KBr) ν / cm^-1 3363, 3219, 1630, 1064, 800 and 641, 1113, 1104, 1599, 1504, 3004, 2955, 2929, 2867; ¹H NMR (400 MHz, DMSO-d₆) δ 10.13 (s, 1H, NH), 9.79 (s, 1H, NH), 2.50 (s, 3H, CH), 9.65 (1H, CH_pyrazine), 8.62, (d, 2H, CH_pyrazine), 0.54, 1.39, 1.48, 1.70 (9H, C-H_aliphatic); ¹³C NMR (400 MHz, DMSO-d₆) δ 144.77, 143.95, 150.70, 150.99, 145.88, 13.11, 170.38, 30.99, 19.88, 18.35, 12.34.

Computational methods

In this study, the DFT calculations were carried out using the GAUSSIAN 09 program.⁴⁹ DFT/B3LYP at the 6-311++G(d,p) basis set level was adopted to optimize geometrical parameters in gas phase and the most stable conformation (lowest total energy) was taken from the final optimization step calculation for all theoretical considerations. The 6-311++G (d,p) with ‘d’ and ‘p’ polarization function on heavy atoms and hydrogen atoms, respectively, was chosen to get a better description of polar bonds of the title compound. The computed harmonic frequencies were scaled by 0.9627⁵⁰ (B3LYP) to improve the agreement between the predicted and observed frequencies. The characterization of vibration frequencies was clarified by means of the PED using vibrational energy distribution analysis (VEDA) 4 program.⁵¹ The GaussView 5.0 program⁵² was used to construct the optimized molecular geometry, HOMO and LUMO electron distributions and the HOMO-LUMO energy gap. The ADT 4.2 software^53,54 was used to calculate the binding affinity between CDK2 macromolecule and the title compound, and the ligand-substate interaction was analyzed using Discovery Studio Visualizer 2016.⁴⁷

Acknowledgments

The authors are thankful to International Islamic University Malaysia and the Ministry of Higher Education, Malaysia, for supporting this research through grant FRGS15-205-0446.

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Publication Dates

• Publication in this collection
  Oct 2018

History

• Received
  17 Jan 2018
• Accepted
  18 May 2018