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The computational study of some s-block metal nitrophenolate complexes, [Ca(THEEN)(PIC)]+ (1), [Ca(THPEN)(H2O)2]2+ (2), Ba(THPEN)(PIC)2 (3) [Na(THPEN)]22+ (4), [Sr(THPEN)(H2O)2]22+ (5) and [Ba(THPEN)(H2O)2]22+ (6) (where THEEN (N,N,N′,N′-Tetrakis(2-hydroxyethyl)ethylenediamine) and THPEN (N,N,N′,N′-Tetrakis(2-hydroxypropyl)ethylenediamine) are tetrapodal ligands and PIC− is 2,4,6-trinitrophenolate anion), is presented here using density functional theory (DFT) in its hybrid form B3LYP. The geometries of the title complexes are described by the quantum-chemical approach using input coordinates obtained from the previously synthesized and X-ray characterized diffraction data of [Ca(THEEN)(PIC)](PIC), [Ca(THPEN)(H2O)2](PIC)2, Ba(THPEN)(PIC)2, [Na(THPEN)]2(PIC)2, [Sr(THPEN)(H2O)2]2(DNP)4 and [Ba(THPEN)(H2O)2]2(DNP)4 (where DNP is 3,5-dinitrophenolate). Only the primary coordination sphere of complexes (1–6) is optimized in the gaseous phase. Calculations of the energy gaps of frontier orbitals (HOMO-LUMO), 13C-NMR shifts and vibrational bands are carried out using B3LYP/6-31 g + (d,p)/LANL2DZ level of theory. The calculated geometric and spectral parameters reproduced the experimental data with a well agreement.
Department of Chemistry, Dr. B.R. Ambedkar National Institute of Technology, India
*Address all correspondence to: rakesh_nitj@yahoo.co.in
1. Introduction
The alkali and alkaline earth metal cations have inert gas electronic structures and are not expected to show any stereochemical requirements in their complex formation as do transition metal cations. They may be considered spherical even in the complex state. Their complexation is thus treated as recognition of spherical cations by organic ligands [1]. Depending upon the nature of the organic ligand and the anion, the metal ions can be separated as solvated ions, solvent separate, loose and tight ion pairs.
Alkali and alkaline earth metal ions form a large number of solid complexes with podands [2, 3, 4, 5, 6]. The podands are inherently flexible because the two ends of the molecule are not tied simultaneously. Polypodal ligands are acyclic multidentate ligands containing more than three arms. They form an unlimited family of structures which finally give rise to dendrimers. A predominant 1:1 complexation has also been observed in alkali and alkaline earth metal complexes of the tetra- and pentapodands. The stability constants of the terapodands are generally lower than those of the corresponding tripodands because of more severe steric hindrance to complexation [7]. Vögtle and coworkers have indicated that the ligands resembling tetrapodands are capable of forming 1:1 complexes with s-block metal ions [8, 9].
The s-block elements present a usual challenge in the molecular modeling, because the metal-ligand interactions in both cases are principally electrostatic. The types of alkali and alkaline earth metal complexes subjected to molecular modeling can be divided into five categories: crown ethers [10, 11, 12, 13, 14, 15, 16], cryptands [17, 18], spherands [19, 20], podands and other biologically important ligands, such as ionophores and cyclic antibiotics [21, 22, 23, 24] . The present work has been undertaken with the aim to computationally characterize the structure and nature of complexes of s-block metal ions with the tetrapodands THEEN and THPEN. Recently the computational studies of these tetrapodal ligands with Cu(II), Ag(I) and La(III) have been reported. Recently, synthesis, crystal structure and biological properties of [Co(edtp)Cl]·NO3·H2O complex was also determined, where edtp is N,N,N′,N′-Tetrakis(2-hydroxypropyl) ethylenediamine in which Co2+ ion is coordinated by the N,N′,O,O′,O″-pentadentate edtp ligand and a chloride to generate a distorted CoClN2O3 octahedron [25, 26, 27, 28].
From the last 3 decades density functional theory has been the dominant method for the quantum mechanical simulation of periodic systems. In recent years it has also been adopted by quantum chemists and is now very widely used for the simulation of energy surfaces in molecules. The quantum-chemical calculations (DFT calculations) giving molecular geometries of minimum energies, molecular orbitals (HOMO-LUMO), 13C-NMR and vibrational spectra were performed using the Gaussian 09 [29]. Molecular orbitals were visualized using “Gauss view”. The method used was Becke’s three-parameter hybrid-exchange functional, the nonlocal correlation provided by the Lee, Yang and Parr expression, and the Vosko, Wilk, and Nuair 1980 local correlation functional (III) (B3LYP) [30, 31]. The 6-31 g + (d,p) basis set was used for C, N and O. The LANL2DZ basis set [32] and pseudopotentials of Hay and Wadt were used for Ca, Sr, Ba and Na metal atoms [33, 34]. DFT calculations were performed in the gaseous phase and the input coordinates were obtained from and then compared with crystal structure data of already reported complexes: [Ca(THEEN)(PIC)](PIC),[Ca(THPEN)(H2O)2](PIC)2, Ba(THPEN)(PIC)2, [Na(THPEN)]2(PIC)2, [Sr(THPEN)(H2O)2]2(DNP)4 and [Ba(THPEN)(H2O)2]2(DNP)4 (where DNP is 3,5-dinitrophenolate) [35]. The structural parameters were adjusted until an optimal agreement between calculated and experimental structure obtained throughout the entire range of available structures. HOMO-LUMO analyses and spectroscopic calculations were performed on the optimized geometries of the title complexes (1–6) using B3LYP/6-31 g + (d,p)/LANL2DZ level of theory.
Complexes (1–6) were successfully modeled by using the input coordinates of crystal data. Tables 1 and 2 represent comparison of calculated and experimental M-Ligand bond lengths (Å) of complexes (1–3) and (4–6), respectively. The picrates and dinitrophenolates that are excluded from the primary coordination spheres of metal atoms in the crystallographic determinations, are not optimized in the computed structures. Tables 3 and 4 represent comparison of calculated and experimental torsion angles of ligand in complexes (1–3) and (4–6) respectively.
Complex 1 (M = Ca)
Complex 2 (M = Ca)
Complex 3 (M = Ba)
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
M-O1
2.450
2.410
0.040
2.389
2.341
0.048
2.720
2.722
−0.002
M-O2
2.450
2.380
0.070
2.495
2.498
−0.003
2.807
2.812
−0.006
M-O3
2.410
2.480
0.070
2.753
2.753
0.000
M-O4
2.410
2.370
0.040
2.812
2.816
−0.004
M-O5
2.681
2.687
−0.006
M-O6
3.127
3.135
−0.008
M-O12
2.310
2.30
0.01
2.728
2.735
−0.007
M-O13
2.470
2.73
0.26
M-O18
2.977
2.990
−0.013
M-O1W
2.440
2.442
−0.002
M-O2W
M-N1
2.824
2.591
0.233
2.601
2.603
−0.002
3.038
3.042
0.004
M-N2
2.738
2.658
0.08
3.026
3.032
−0.006
Table 1.
Comparison of experimental and calculated M-ligand bond lengths (Å) of complexes (1–3).
Complex 4 (M = Na)
Complex 5 (M = Sr)
Complex 6 (M = Ba)
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
M-O1
2.412
2.416
−0.004
2.617
2.628
−0.011
2.736
2.743
−0.007
M-O2
2.393
2.396
−0.003
2.611
2.618
−0.007
2.763
2.767
−0.004
M-O3
2.505
2.508
−0.003
2.506
2.516
−0.010
2.756
2.762
−0.006
M-O4
2.628
2.632
−0.004
2.618
2.626
−0.008
2.658
2.668
−0.010
M-O1W
2.701
2.711
−0.010
2.880
2.884
−0.004
M-O2W
2.699
2.705
−0.006
2.988
2.995
−0.007
M-O2WA
2.726
2.732
−0.006
M-N1
2.835
2.842
−0.007
3.009
3.008
−0.001
M-N2
2.849
2.857
−0.008
3.010
3.010
0.000
Table 2.
Comparison of experimental and calculated M-ligand bond lengths (Å) of complexes (4–6).
Name of the
Complex (1)
Complex (2)
Complex (3)
Atoms
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
O1-C1-C2-N1
−55.1
−55.05
0.05
57.9
58.0
0.1
−32.3
−32.4
−0.1
C1-C2-N1-C5
165.1
165.1
0.0
82.8
82.7
0.1
161.9
162.0
0.1
C2-N1-C5-C6
−159.0
−159.0
0.0
−165.5
−165.5
0.0
−157.6
−157.8
−0.2
N1-C5-C6-N2
65.4
65.3
0.1
60.4
60.5
0.1
65.9
66.1
0.2
C5-C6-N2-C8
−159.1
−159.0
0.1
−159.3
−159.4
0.1
C6-N2-C8-C7
89.1
89.1
0.0
163.6
163.7
0.1
N2-C8-C7-O3
60.9
60.9
0.0
−34.1
−34.2
−0.1
O2-C3-C4-N1
36.5
36.7
0.2
55.5
55.6
0.1
46.8
46.9
−0.1
C3-C4-N1-C5
−121.6
−121.7
−0.1
−161.0
−161.0
0.0
−132.6
−132.7
−0.1
C4-N1-C5-C6
77.2
77.2
0.0
72.6
72.6
0.0
83.7
83.8
0.1
C5-C6-N2-C10
79.4
79.4
0.0
79.0
79.1
0.1
C6-N2-C10-C9
−151.8
−151.8
0.0
−134.9
−134.9
0.0
N2-C10-C9-O4
61.3
61.4
0.1
52.1
52.2
0.1
Table 3.
Comparison of calculated and experimental torsion angles (°) of ligand in the complexes (1–3).
Name of the
Complex (4)
Complex (5)
Complex (6)
Atoms
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
Theo.
Exp.
Dev.
Complex
−55.6
−55.7
−0.1
32.3
32.3
0.0
−43.4
−43.5
0.1
O1-C1-C2-N1
152.7
152.6
0.1
−143.9
−143.9
0.0
162.3
162.4
0.1
C1-C2-N1-C5
−80.2
−80.2
0.0
86.1
86.1
0.0
−92.7
−92.8
0.1
C2-N1-C5-C6
−64.0
−63.9
−0.1
43.6
43.6
0.0
−50.1
−50.1
0.0
N1-C5-C6-N2
165.5
165.4
0.1
−146.4
−146.4
0.0
156.5
156.7
0.2
C5-C6-N2-C8
−85.7
−85.7
0.0
156
155.9
0.1
−89.6
−89.9
0.3
C6-N2-C8-C7
−60.3
−60.4
−0.1
−44.7
−44.7
0.0
−30.4
−30.4
0.0
N2-C8-C7-O3
−59.7
−59.8
−0.1
−17.4
−17.4
0.0
47.8
48.1
0.3
O2-C3-C4-N1
−91.0
−91.1
−0.1
112.7
112.7
0.0
−135.1
−135.2
0.1
C3-C4-N1-C5
156.0
156.0
0.0
−159.1
−159.2
0.1
151.9
151.9
0.0
C4-N1-C5-C6
−72.4
−72.5
−0.1
97.4
97.4
0.0
−92.1
−92.4
0.3
C5-C6-N2-C10
156.6
156.6
0.0
−151.8
−151.8
0.0
143.4
143.9
0.5
C6-N2-C10-C9
−59.2
−59.3
−0.1
41.6
41.7
0.1
5.1
4.9
0.3
N2-C10-C9-O4
−55.6
−55.7
−0.1
32.3
32.3
0.0
−43.4
−43.5
0.1
Table 4.
Comparison of experimental and calculated and torsion angles (°) of ligand in the complexes (4–6).
3.1.1 [Ca(THEEN)(PIC)]+ (1)
The coordination number of Ca(II) ion is eight with distorted cube geometry in the optimized geometry of cationic complex (1) (Figure 1). THEEN is interacting with Ca(II) ion through all the six potential donor atoms. The seventh and eighth coordination sites of Ca(II) are occupied by picrate anion through phenolic oxygen and one of the o-nitro oxygen. The observed and calculated positions of calcium and donor atoms are in agreement. A comparison of bond lengths and bond angles provided a maximum tolerance of 0.27 Å and 16.33°Å, respectively (Table 1 and Table S1; Figure S1a,b) of computed title complex (1) and crystallographically determined complex [Ca(THEEN)(PIC)](PIC). The torsion angles of the ligand THEEN in theoretically determined and experimental complex are also in well consistency with each other (Table 3). The HOMO-LUMO analysis has indicated that there is maximum distribution of HOMO over the carbon atoms and to a lesser extent on the oxygen of the coordinated picrate. LUMO is mainly distributed or concentrated on all the atoms of coordinated picrate except p-nitro group. Neither HOMO nor LUMO distribution is found either on calcium ion or on any ligand atom. The HOMO-LUMO gap (ΔE) is found to be 0.852 eV (Figure S1c).
Ca(II) is eight coordinated in monomeric cationic complex with a distorted square-antiprismatic geometry in complex (2) as is observed in crystal structure of [Ca(THPEN)(H2O)2] (PIC)2. H2O (Figure 2). THPEN is acting as hexadentate ligand towards the metal ion. Two remaining sites around the metal ion are occupied by two water molecules. The observed and calculated positions of calcium and donor atoms are in agreement. All strain energy minimized structures reproduced the observed X-ray structures with almost no deviation in M-L bond length and torsion angle of the ligand (Table 3). The maximum tolerance of L-M-L bond angle is 15.8° (Tables 1 and Table S1, Figure S2a,b). Complex 2 is displaying the main distribution of HOMO as well as LUMO only on water molecules. There is slight distribution of HOMO and LUMO on hydroxyl oxygen of THPEN ligand also with HOMO-LUMO gap (HLG) of 0.419 eV (Figure S2c).
Ba(II) is ten-coordinate in its monomeric complex (3) (Figure 3). The ligand THPEN coordinates through both its nitrogen atoms and all the four hydroxyl oxygen. The two picrate ions are also directly coordinated to Ba2+ ion through the phenolic oxygen and one oxygen of the o-nitro group. Since both the picrates are directly interacting with the cation, the complex is termed as tight ion-paired complex as is found in the crystallographically determined complex. The observed and calculated positions of barium and donor atoms are in agreement. There is negligible deviation found in bond length, bond angle (0.11°) and torsion angle of ligand THPEN for calculated title complex (3) and experimental Ba(THPEN)(PIC)2 (Tables 1 and 3 and S1, Figure S3a,b). An analysis of HOMO-LUMO has illustrated that HOMO is mainly distributed on the ligand THPEN with a small distribution on coordinated picrates. In contrast to this LUMO is mainly distributed on coordinated picrates with no distribution over the ligand or metal atom. The complex is showing HLG of 0.118 eV (Figure S3c).
Figure 4a shows the optimized structure of the cationic complex of sodium (4). This structure is centrosymmetric dimer. The coordination number around each Na+ ion is seven. Each THPEN ligand coordinates to Na(I) ion in a heptadenate fashion (Figure 4). In other words, one hydroxyl group of the THPEN ligand acts as a bridge between two Na+ ions. The geometry of the complex is distorted monocapped octahedron. The Na…Na non bridging distance is 3.429 Å. Almost no deviation has been observed in bond length (M-L), torsion angle of ligand THPEN and bond angles (L-M-L) of computed title complex (4) and crystallographically determined complex [Na(THPEN)]2(PIC)2 (Tables 2 and 4 and Table S1, Figures S4a,b). The HOMO-LUMO study has revealed that in the title complex (4) HOMO is mainly concentrated on bridged hydroxyl oxygens and sodium metal but to a smaller extent on the other coordinated hydroxyl oxygens and amine nitrogens. LUMO is mainly concentrated on bridged hydroxyl oxygens and to a smaller extent on other coordinated oxygen atoms. The HOMO-LUMO gap is 0.261 eV (Figure S4c).
Sr(II) is nine-coordinated in its dimeric complex (5) (Figure 5). This cationic complex is having tricapped trigonal-prismatic geometry as is found in crystallographically determined complex [Sr(THPEN)(H2O)2]2(DNP)4. Each Sr2+ ion in the complex is coordinated by six potential donor sites of the ligand THPEN and four water molecules. Out of four water molecules, two are bridging and the third one is non-bridging. Sr…Sr non bridging distance is 4.346 Å indicating the existence of van der Waals contact. All strain energy minimized structures reproduced the observed X-ray structures to a maximum tolerance of 9.07° bond angle (Table 2 and Table S1, Figure S5a,b). Almost no deviation of M-L bond length and torsion angle of ligand THPEN has been observed for the title complex (5) and crystallographically determined complex (Tables 2 and 4). The HOMO-LUMO analysis has shown that the complex (5) is having maximum distribution of HOMO and LUMO on bridged coordinated water molecules and there is HLG of 0.0225 eV (Figure S5c).
Figure 5.
(a) Optimized geometric structure of [Sr(THPEN)(H2O)2]2(DNP)4 (b) Trigonal- prismatic geometry.
3.1.6 [Ba(THPEN)(H2O)2]22+ (6)
Ba(II) is ten-coordinate in the cationic title complex (6) as is found in the crystallographic determined complex [Ba(THPEN)(H2O)2](DNP)4. The geometry around Ba(II) is bicapped cubic. Each Ba(II) in dimer is interacting with THPEN through all its six potential donor sites and four water molecules. The latter are bridging in nature. The existence of van der Waals contact between non-bridging Ba…Ba is indicated by their larger distance (4.196 Å). The observed and calculated positions of the metal and donor atoms are in agreement as almost negligible deviation of M-L bond length and torsion angle of THPEN. A deviation of 0.14° of bond angle L-M-L has been observed for complex (6) [Ba(THPEN)(H2O)2](DNP)4 (Tables 2 and 4 and Table S1; Figures S6a,b and S7). The region of distribution of HOMO and LUMO is only over two of the bridged water molecules in complex (6) with a very small HOMO-LUMO gap (ΔE = 0.0375 eV) indicating the soft nature of complex (Figure 6).
Smaller is the HUMO-LUMO gap (HLG) softer is the complex [36, 37]. The frontier orbitals HOMO and LUMO are very important parameters for chemical reaction and take part in chemical stability [38, 39, 40]. It is predicted from the HOMO-LUMO gaps that the title complexes are soft as is obvious from their smaller HUMO-LUMO energy gaps (HLG) relative to the similar reported complexes of copper, silver and lanthanoid [25, 26, 27] (Table 5). It has been observed in the present computational study that the dinitrophenolate complexes are softer than trinitrophenolate and among the latter, [Ca(THEEN)(PIC)]+ (1) is displaying least softness. It is pertinent to mention here that the complex (1) is having THEEN ligand whereas THPEN is ligand in rest of the complexes (2–6).
HLG (eV)
Reported complexes
HLG (eV)
Reported complexes
HLG (eV)
[Ca(THEEN)(PIC)]+ (1)
0.852
[Cu(THEEN)(H2O)](PIC)2
3.537
[La(THEEN)(PIC) (H2O)2] (PIC)2.2H2O
3.428
[Ca(THPEN)(H2O)2]2+ (2)
0.419
[Cu(THPEN)](PIC)2.C3H8O
3.467
[La(TEAH3)(H2O)2] (PIC)3
3.673
Ba(THPEN)(PIC)2 (3)
0.118
[Cu(TEAH3)(PIC)](PIC).H2O
3.619
[Na(THPEN)]22+ (4)
0.261
[Ag (THEEN)]2 (PIC)2
2.530
[Sr(THPEN)(H2O)2]22+ (5)
0.0225
[Ag (THPEN)]2 (PIC)2
2.640
[Ba(THPEN)(H2O)2]22+ (6)
0.0375
[Ag(TEAH3)2] (PIC)
1.061
Table 5.
Comparison of HOMO-LUMO energy gaps of complexes (1–6) with earlier reported complexes [25, 26, 27].
3.3 Spectral data
Nuclear magnetic resonance spectra (NMR) and infrared (IR) spectroscopy can be useful for studying the coordination of various ligating sites. The 13C-NMR spectra were predicted for complexes (1–6) using DFT/B3LYP/6-31G** method and the spectral data was compared with experimental data reported in literature [35]. The computed NMR spectral data is fairly in agreement with experimental data (Tables 6 and 7). Small deviations are due to the fact that H-bonding interactions or any type of lattice interactions are not modeled in theoretically computed structures. The terminal methyl groups in theoretically predicted complexes (2–5) are displaying quiet high upfield shifts relative to the experimentally obtained due to more free movements in the gaseous phase than in solution or solid phase.
Assignments (δ)
[Ca(THEEN)(PIC)]+ (1)
Ba(THPEN)(PIC)2 (3)
Theo.
Exp.
Theo.
Exp.
▬CH3
*
*
4.22
19.61
▬CH3
4.49
19.89
▬NCH2
52.31
55.03
51.73
55.34
▬NCH2
43.35
55.20
▬OCH2, ▬OCH
59.03
57.47
50.75
63.00
▬ArCH
113.63
124.33
117.85
124.36
p-ArCN
134.75
123.60
122.06
123.68
o-ArCN
140.68
140.78
140.98
140.78
▬ArCO
161.57
160.20
150.21
160.20
Table 6.
Comparison of calculated and experimental 13C-NMR spectral data for complexes (1 and 3).
* Group absent.
Assignment (δ)
[Ca(THPEN)(H2O)2]2+ (2)
[Na(THPEN)]22+ (4)
[Sr(THPEN)(H2O)2]22+ (5)
[Ba(THPEN)(H2O)2]22+ (6)
Theo.
Exp.
Theo.
Exp.
Theo.
Exp.
Theo.
Exp.
▬CH3
11.35
18.79
4.01
20.30
3.77
18.31
27.02
18.35
▬CH3
11.38
19.02
5.63
20.36
3.85
18.59
27.69
18.63
▬NCH2
39.60
50.99
43.05
50.42
43.60
48.31
61.69
59.80
▬NCH2
39.61
51.76
44.05
52.90
57.81
59.68
61.69
60.59
▬OCH
*
*
50.73
55.73
41.85
60.62
60.37
60.66
▬OCH
69.24
61.74
57.90
55.95
51.91
61.08
60.38
62.53
Table 7.
Comparison of calculated and experimental 13C-NMR spectral data for complexes (2, 4–6).
* Group absent.
The computed IR spectral peaks that appear in the range of 1370–600 cm−1 are fairly in agreement with the experimental data (Tables 8 and 9). The absorption peaks due to the presence of hydroxyl groups were observed only for complexes (1) and (6) in the computed IR spectra. It is pertinent to mention here that both of these complexes possess the picrate anion in their coordination sphere. The less extent of H-bonding is reported in the crystallographic description of these complexes [35]. The theoretical absorption band appears at 3223 and 3235 cm−1 for both complexes (1) and (6) whereas the experimental band is reported at 3300 cm−1 for both of them [35].
Assignments (cm−1)
[Ca(THEEN)(PIC)]+ (1)
[Ca(THPEN)(H2O)2]2+ (2)
Ba(THPEN)(PIC)2 (3)
Theo.
Exp.
Theo.
Exp.
Theo.
Exp.
ν (NO2)
1363.56
1360 m
1320.81
1360 vs
1384.20
1370
δ (〓CH)
696.80
700 m
784.16
790 m
800
800
Table 8.
Comparison of calculated and experimental IR spectral data for complexes (1–3).
Assignments (cm−1)
[Na(THPEN)]22+ (4)
[Sr(THPEN)(H2O)2]22+ (5)
[Ba(THPEN)(H2O)2]22+ (6)
Theo.
Exp.
Theo.
Exp.
Theo.
Exp.
ν (NO2)
1366
1371.21
1330
1329.24
1340
1329.43
δ (〓CH)
790
784.54
760
762.52
790
787.17
Table 9.
Comparison of calculated and experimental IR spectral data for complexes (4–6).
The coordination number of the title s-block complexes is varying from 7 to 10 in the present work. As the size of the metal increases, coordination number of central metal ion also increases. Out of the six complexes presented, three are monomeric (1–3) and three are dimeric (4–6). The longer distances between two M…M distances in the dinuclear complexes indicate the existence of van der Waals contacts between the two s-block metal ions. All the title complexes are cationic except Ba(THPEN)(PIC)2 (3). The latter is tight ion-paired complex. All strain energy minimized structures obtained using quantum-chemical approach reproduced the observed X-ray structures with geometric parameters in well agreement. HOMO-LUMO studies suggest the softness of the title s-block complexes relative to the similar already reported copper, silver and lanthanoid complexes. The theoretical spectral data (13C-NMR and IR) computed using DFT and experimental data is fairly in agreement with each other. The accuracy of the results predicts that the DFT studies performed using B3LYP/6-31 g + (d,p)/LANL2DZ level of theory is the appropriate quantum-chemical method for reproducing the experimental results for the title s-block complexes. This quantum-chemical approach has potential for molecular modeling of other s-block complexes and exploring their chemistry.
Small deviations in geometric as well as spectral parameters may be attributed to the lack of H-bonding and packing interactions within lattice which were not modeled during the computational study of the entitled s-block complexes. Moreover, the quantum-chemical approach of DFT studies has been carried out in the gaseous phase whereas the already reported experimental crystal and IR spectral data is in the solid phase while 13C-NMR spectral data is in the solution phase.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (1) and (c) (HOMO-LUMO) of the complex (1) with energy gap.
Figure S2.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (2) (c) (HOMO-LUMO) of the complex (2) with energy gap.
Figure S3.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (3) (c) (HOMO-LUMO) of the complex (3) with energy gap.
Figure S4.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (4) (c) (HOMO-LUMO) of the complex (4) with energy gap.
Figure S5.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (5) (c) (HOMO-LUMO) of the complex (5) with energy gap.
Figure S6.
Plot showing the deviations of theoretical and experimental (a) bond lengths (Å) and (b) bond angles (°) for the complex (6) (c) (HOMO-LUMO) of the complex (6) with energy gap.
Figure S7.
R = H, THEEN; R = CH3, THPEN.
Bond distances (Å)
Theoretical
Experimental
Dev.
Bond angles (°)
Theoretical
Experimental
Dev.
Complex (1)
Ca-N1
2.600
2.600
0.000
N1-Ca-N1A
71.54
71.60
0.06
Ca-O1
2.387
2.388
0.001
N1-Ca-O2A
81.41
65.52
15.89
Ca-O2
2.495
2.496
0.001
N1-Ca-O1W
119.08
119.09
0.01
Ca-O1W
2.439
2.439
0.000
N1-Ca-O1WA
143.89
143.89
0.00
O1-Ca-O2
102.93
102.95
0.02
O1-Ca-N1
67.80
67.79
0.01
O1-Ca-O1W
79.82
79.85
0.03
O1-Ca-N1A
132.22
132.22
0.00
O1-Ca-O2A
84.37
84.36
0.01
O1-Ca-O1A
159.11
159.10
0.01
O1-Ca-O1WA
83.52
83.54
0.02
O2-Ca-N1
65.50
65.52
0.02
O2-Ca-O1W
74.11
74.10
0.01
O2-Ca-N1A
81.42
81.40
0.02
O2-Ca-O2A
139.33
139.89
0.56
O2A-Ca-O1W
145.88
145.90
0.02
Complex (2)
Ca-O1
2.45
2.41
0.04
O1-Ca-O2
94.43
102.08
7.65
Ca-O2
2.45
2.38
0.07
O1-Ca-O3
172.00
175.21
3.21
Ca-O3
2.41
2.48
0.07
O1-Ca-O4
85.56
74.35
11.21
Ca-O4
2.41
2.37
0.04
O1-Ca-O12
107.80
104.18
3.62
Ca-O12
2.31
2.30
0.01
O1-Ca-O13
61.91
64.85
2.94
Ca-O13
2.47
2.73
0.26
O1-Ca-N1
65.93
68.50
2.57
Ca-N1
2.74
2.59
0.15
O1-Ca-N2
104.33
115.49
11.16
Ca-N2
2.82
2.65
0.17
O2-Ca-O3
90.99
79.27
11.72
O2-Ca-O4
180.00
168.65
11.35
O2-Ca-O12
108.06
107.20
0.86
O2-Ca-O13
61.38
69.92
8.54
O2-Ca-N1
64.20
68.43
4.23
O2-Ca-N2
114.39
105.72
8.67
O3-Ca-O4
89.01
105.24
16.23
O3-Ca-O12
75.95
71.06
4.89
O3-Ca-O13
126.03
110.69
15.34
O3-Ca-N1
111.54
116.18
4.64
O3-Ca-N2
67.97
68.26
0.29
O4-Ca-O12
71.93
84.20
12.27
O4-Ca-O13
118.62
116.91
1.71
O4-Ca-N1
115.80
100.38
15.42
O4-Ca-N2
65.61
67.36
1.75
O12-Ca-O13
71.32
62.19
9.13
O12-Ca-N1
168.56
169.55
0.99
O12-Ca-N2
123.47
120.54
2.93
O13-Ca-N1
97.26
107.46
10.2
O13-Ca-N2
163.73
175.60
11.87
N1-Ca-N2
67.95
69.92
1.97
Complex (3)
Ba-O1
2.720
2.720
0.000
O1-Ba-O2
86.95
87.00
0.05
Ba-O2
2.807
2.801
0.006
O1-Ba-O3
172.87
173.00
0.13
Ba-O3
2.753
2.750
0.003
O1-Ba-O4
88.55
88.50
0.05
Ba-O4
2.812
2.812
0.000
O1-Ba-O6
72.90
72.90
0.00
Ba-O5
2.681
2.683
0.002
O1-Ba-O12
61.79
61.80
0.01
Ba-O6
3.127
3.128
0.001
O1-Ba-O18
109.63
109.70
0.07
Ba-O12
2.728
2.729
0.001
O1-Ba-N1
58.12
58.10
0.02
Ba-O18
2.977
2.979
0.002
O1-Ba-N2
114.85
114.80
0.05
Ba-N1
3.038
3.038
0.000
O2-Ba-O4
129.37
129.40
0.03
Ba-N2
3.026
3.028
0.002
O2-Ba-O6
64.79
64.80
0.01
O2-Ba-O18
161.62
160.60
0.02
O2-Ba-N2
79.36
79.40
0.03
O2-Ba-N1
57.03
57.12
0.05
O3-Ba-O2
92.08
92.10
0.02
O3-Ba-O4
86.61
86.70
0.09
O3-Ba-O6
113.02
113.10
0.08
O3-Ba-O18
72.70
72.80
0.10
O3-Ba-N1
115.63
115.60
0.03
O3-Ba-N2
58.06
58.20
0.14
O4-Ba-O6
156.82
156.80
0.02
O4-Ba-O18
63.13
63.20
0.07
O4-Ba-N1
78.20
78.20
0.00
O4-Ba-N2
57.43
57.40
0.03
O5-Ba-O1
123.12
123.20
0.08
O5-Ba-O2
85.94
85.90
0.04
O5-Ba-O3
63.80
63.90
0.10
O5-Ba-O4
135.92
135.90
0.02
O5-Ba-O6
53.26
53.30
0.03
O5-Ba-O12
84.0
84.00
0.00
O5-Ba-O18
76.67
76.90
0.13
O5-Ba-N1
142.90
142.90
0.00
O5-Ba-N2
118.97
118.90
0.07
O12-Ba-O2
133.15
133.20
0.05
O12-Ba-O3
123.02
123.00
0.02
O12-Ba-O4
86.45
86.40
0.05
O12-Ba-O6
72.69
72.70
0.01
O12-Ba-O18
54.05
54.00
0.05
O12-Ba-N1
117.95
117.96
0.01
O12-Ba-N2
143.78
143.80
0.02
O18-Ba-O6
109.54
109.60
0.06
O18-Ba-N1
140.27
140.40
0.13
O18-Ba-N2
101.49
101.50
0.01
N2-Ba-N1
61.27
61.30
0.03
N2-Ba-O6
143.21
143.20
0.01
N1-Ba-O6
102.39
102.40
0.01
Complex (4)
Na-N1
2.552
2.554
0.002
O1-Na-O2
99.56
99.50
0.06
Na-N2
2.565
2.566
0.001
O1-Na-O3
86.59
86.60
0.01
Na-O1
2.412
2.412
0.000
O1-Na-O4
174.34
174.30
0.04
Na-O2
2.393
2.393
0.000
O1-Na-O4A
90.18
9023
0.05
Na-O3
2.505
2.505
0.000
O1-Na-N1
69.82
69.82
0.00
Na-O4
2.628
2.629
0.001
O1-Na-N2
109.13
109.10
0.03
Na-O4A
2.442
2.443
0.001
O2-Na-O3
164.10
164.13
0.03
Na-NaA
3.429
3.430
0.001
O2-Na-O4
78.26
78.31
0.05
O2-Na-O4A
88.56
88.57
0.01
O2-Na-N1
70.69
70.70
0.01
O2-Na-N2
121.68
121.71
0.03
O3-Na-O4
96.86
96.87
0.01
O3-Na-N1
125.19
125.17
0.02
O3-Na-N2
68.93
68.91
0.02
O3-Na-O4A
76.69
76.72
0.03
O4-Na-O4A
94.96
95.00
0.03
O4-Na-N1
68.25
68.25
0.00
O4-Na-N2
68.25
68.25
0.00
N1-Na-N2
73.38
73.37
0.01
N1-Na-O4A
147.48
147.51
0.03
N2-Na-O4A
138.85
138.87
0.02
Complex(5)
Sr-O1
2.617
2.618
0.001
O3-Sr-O2
151.28
158.70
7.42
Sr-O2
2.611
2.610
0.001
O3-Sr-O1
73.24
77.20
3.96
Sr-O3
2.506
2.505
0.001
O2-Sr-O1
113.98
114.30
0.32
Sr-O4
2.618
2.618
0.000
O3-Sr-O4
87.91
88.20
0.29
Sr-O1W
2.701
2.702
0.001
O2-Sr-O4
77.89
73.50
4.39
Sr-O2W
2.699
2.699
0.000
O1-Sr-O4
158.36
151.60
6.76
Sr-O2WA
2.726
2.699
0.000
O3-Sr-N1
102.34
113.60
11.26
Sr-N1
2.835
2.835
0.000
O4-Sr-N1
113.34
102.50
10.84
Sr-N2
2.849
2.849
0.000
O3-Sr-N2
61.38
64.40
3.02
O2-Sr-N2
89.92
97.10
7.18
O1-Sr-N2
96.80
90.2
6.60
O4-Sr-N2
64.13
61.60
2.53
O3-Sr-O2W
106.07
106.40
0.33
O2-Sr-O2W
70.58
77.10
6.52
O1-Sr-O2W
129.35
140.50
11.15
O4-Sr-O2W
70.80
67.90
2.90
O2-Sr-O1W
79.52
65.40
14.12
O1-Sr-O1W
65.11
79.80
14.69
O4-Sr-O1W
136.42
127.40
9.02
O3’-Sr-O1W
126.14
127.90
1.76
O2W-Sr-O1W
70.75
71.00
0.25
O2W-Sr-N2
128.11
128.40
0.29
O1W-Sr-N2
152.06
152.40
0.34
N1-Sr-N2
64.77
65.00
0.23
O2W-Sr-N1
139.03
139.30
0.27
O1W-Sr-N1
87.52
87.80
0.28
Complex (6)
Ba-O1
2.736
2.738
0.002
O4-Ba-O1
162.70
162.90
0.20
Ba-O2
2.763
2.761
0.002
O4-Ba-O3
92.45
92.70
0.25
Ba-O3
2.756
2.757
0.001
O1-Ba-O3
79.69
80.00
0.31
Ba-O4
2.658
2.657
0.001
O4-Ba-O2
84.25
84.60
0.35
Ba-O1W
2.880
2.880
0.000
O1-Ba-O2
94.22
94.50
0.28
Ba-O2W
2.988
2.990
-0.002
O3-Ba-O2
148.19
148.40
0.21
Ba-N1
3.009
3.002
0.007
O4-Ba-N1
107.19
107.50
0.31
Ba-N2
3.010
3.004
0.006
O1-Ba-N1
58.19
58.40
0.21
O3-Ba-N1
91.90
92.00
0.01
O2-Ba-N1
59.43
59.60
0.17
O4-Ba-N2
59.95
61.10
1.15
O1-Ba-N2
103.03
103.20
0.17
O3-Ba-N2
58.68
58.80
0.12
O2-Ba-N2
93.2
93.40
0.20
N1-Ba-N2
61.84
62.00
0.16
O4-Ba-O1W
126.17
126.50
0.33
O1-Ba-O1W
66.29
66.50
0.23
O3-Ba-O1W
72.53
72.80
0.27
O2-Ba-O1W
133.50
133.80
0.30
O1-Ba-O2W
73.43
73.70
0.27
O3-Ba-O2W
131.18
131.50
0.32
O2-Ba-O2W
74.74
75.00
0.26
O2W-Ba-O1WA
59.36
59.50
0.14
N1-Ba-O1WA
137.03
137.20
0.17
N1-Ba-O1W
124.19
124.19
0.00
N1-Ba-O2W
106.68
106.90
0.22
N2-Ba-O1WA
123.73
124.00
0.27
N2-Ba-O1W
131.21
131.50
0.29
N2-Ba-O2W
166.91
167.00
0.10
N2-Ba-O2WA
100.84
100.87
0.03
Table S1.
Comparison of selected experimental and calculated geometric parameters bond lengths (Å) and bond angles (°) for complexes (1–6).
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Rakesh Kumar and Sangeeta Obrai
Submitted: September 14th, 2019Reviewed: November 17th, 2019Published: March 11th, 2020
Open access peer-reviewed chapter
