# Synthesis of New Zirconium(IV) Complexes with Amino Acid Schiff Bases: Spectral, Molecular Modeling, and Fluorescence Studies

Authors: Har Lal Singh; Jangbhadur Singh
Journal: International Journal of Inorganic Chemistry
 (2013)

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## Abstract

New zirconium(IV) complexes were synthesized with bidentate ligands and characterized by elemental analysis, molar conductance measurements, molecular weight determinations, IR, electronic, NMR (1H and 13C), fluorescence and molecular modeling studies. All the complexes are 1 : 2 electrolytes in nature and may be formulated as [Zr(L)2Cl2] (where L is Schiff bases of amino acids and substituted isatin). The analytical data showed that the Schiff-base ligand acts as bidentate toward zirconium ion via the azomethine nitrogen and carboxylate oxygen. The conductivity values between 8.5–12.6 Ω−1, mol−1, cm2 in DMF imply the presence of nonelectrolyte species. On the basis of spectral and molecular modeling studies, the resulting complexes are proposed to have octahedral geometries.


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## Body

## 1. Introduction

The coordination chemistry of Schiff bases has been widely explored, though its use in supramolecular coordination chemistry remains largely unexplored. The Schiff-base moiety is potentially ambidentate and can coordinate through nitrogen with either oxygen or sulfur atoms. The vast literature on structural studies of Schiff-base complexes reveals some interesting features of their coordination behavior [1–6]. Schiff-base metal chelates have played a central role in the development of coordination chemistry. Metal complexes with Schiff-base ligands have been receiving considerable attention due to the pharmacological properties of both ligands and complexes [7–10]. Schiff-base derivatives exhibit a great variety of biological activities, such as antitumor [11, 12], antifungal [13, 14], antibacterial [15, 16], anticonvulsant [17] and antiviral [18] properties. The interest in the construction of Schiff-base coordination complexes by reacting transition metal ions with bidentate has been constantly growing over the past years [19–21]. Within this understanding lies an increased knowledge of molecular self-assembly, metal-ligand complexation, and disposition of metal binding sites. By mastering these areas, new improved systems related to the fields of catalysis, supramolecular chemistry, and bioengineering can be achieved. Although the chemistry of zirconium complexes has been extensively studied, particularly in relation to their application as polymerization catalysts, the coordination chemistry of these oxophilic metals has concentrated on the use of oxygen donors. Many researchers have conducted on Schiff-base complexes; most of these complexes were found to be biologically active [22–25] as there has been considerable interest in the study of first-row transition metal Schiff-base complexes. However, relatively less work has appeared on the complexes of 2nd and 3rd rows transition metal ions. There is not much information on zirconium(IV) complexes from the available literature; therefore this paper reports the synthesis and characterization of zirconium(IV) complexes of Schiff bases derived from amino acids and isatins.


## 2. Experimental

### 2.1. Starting Materials

All chemicals used in the present work, 1H-indole-2,3-dione, 5-chloro-1H-indole-2,3-dione, amino acids (glycine, alanine, valine, methionine, phenylalanine, and tryptophan), and oxozirconium(IV) chloride, were of analytical grade. The ligands were prepared by the condensation of isatins with amino acids as described earlier [9, 26].


### 2.2. Analytical Procedures

Solvents used were dried and purified by standard methods and moisture was excluded from the glass apparatus using CaCl2 drying tubes. The melting points of the compounds were determined on a capillary melting point apparatus and were not corrected. The purity of the compounds was confirmed by thin layer chromatography using silica gel-G glass plates as the stationary phase and benzene and ethanol (9 : 1) as the mobile phase. Zirconium was determined gravimetrically as its oxide, ZrO2. Nitrogen and sulfur were determined by Kjeldahl’s and Messenger’s methods, respectively. Molecular weight determinations were carried out by the Rast camphor method.


### 2.3. Physical Measurements

The IR spectra of samples in KBr pellets were recorded on an FTIR spectrophotometer model SP-2, Perkin Elmer in the range of 4000–400 cm−1. The electronic spectra of the ligands and their metal complexes were recorded in dry DMSO, on a thermo-, double-beam spectrophotometer UV 1, in the range of 800–200 nm. The fluorescence studies of Schiff base and its metal complexes were recorded on Shimadzu RF-5301PC spectrophotometer. The molar conductance of the complexes was measured on 10−3 M DMF solutions using Systronics conductivity bride model 305. 1H and 13C NMR spectra were recorded on Bruker avance II (400 MHz) FTNMR spectrometer at the SAIF, Punjab University, Chandigarh, using DMSO-d6 as the solvent and tetramethylsilane (TMS) as an internal standard.


### 2.4. Molecular Modeling Studies

The molecular modeling of a representative compound is carried out on a CS Chem 3D ultramolecular modeling and analysis programme, interactive graphics programme that enables rapid structure building and geometry optimization with minimum energy and molecular display.


### 2.5. Preparation of Zirconium Complexes

The complexes were prepared by treating oxozirconium(IV) chloride (1.61 mmol) in methanol with the corresponding Schiff bases (3.22 mmol) in the same solvent. The mixture was refluxed for three hours on a water bath after which the crystals of the complex separate out on cooling; the mixture was concentrated on a steam bath until about one-third of the solution remained. The concentrated solution was cooled after which the crystals were filtered, washed with methanol, and then dried in vacuum at45±5°C after repeated washing with dry cyclohexane. The compounds were purified by recrystallization from the same solvent. The purity of the compounds was checked by TLC using silica gel G as adsorbent.Compound
Z
r
(
L
1
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L1H); colour, red; yield, 0.218 g; mp, 170°C (d) and elemental analysis (%), calcd. for C20H14Cl2N4O6Zr: C, 42.26; H, 2.48; N, 9.86; found, C: 42.33; H, 2.57; N, 9.81; molecular weight: found, 580.12, calcd. 568.48. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 10.8; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.28 (s, 2H, N–CH2–), 8.06 (s, 1H, NH), 7.18–7.78 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 186.3 (COO), 52.1 (–CH2–), 153.8 (C=N), 167.3 (C=O), 148.65, 131.2, 129.9, 125.3, 122.7, 119.5 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1610; ν(C=O), 1722; νasym(COO), 1595; νsym(COO), 1325; ν(Zr←N), 535; ν(Zr–O), 465.Compound
Z
r
(
L
2
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L2H); colour, reddish brown; yield, 0.317 g; mp, 200°C (d) and elemental analysis (%), calcd. for C22H18Cl2N4O6Zr: C, 44.30; H, 3.04; N, 9.39; found, C: 44.46; H, 3.10; N, 9.33; molecular weight: found, 590.68, calcd. 596.53. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 11.5; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.70 (q, 1H, N–CH–); 8.32 (s, 1H, NH); 1.50 (d, 3H, C-CH3); 7.00–7.86 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 180.7 (COO), 63.6 (–CH–), 150.2 (C=N), 159.6 (C=O), 1502.7, 138.3, 133.6, 131.7, 130.5, 129.3, 124.9, 121.1 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1617; ν(C=O), 1728; νasym(COO), 1585; νsym(COO), 1322; ν(Zr←N), 537; ν(Zr–O), 460.Compound
Z
r
(
L
3
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L3H); colour, brown; yield, 0.179 g; mp, 144°C (d) and elemental analysis (%), calcd. for C26H26Cl2N4O6Zr: C, 47.85; H, 4.02; N, 8.58; found, C: 47.89; H, 4.14; N, 8.54; molecular weight: found, 640.96, calcd. 652.64. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 8.5; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.26 (d, 1H, N–CH–); 8.40 (s, 1H, NH); 2.16–2.30 (m, 1H, –CH–); 1.22 (d, 3H, –CH3) 7.11–7.65 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 183.1 (COO), 67.5 (–CH–), 18.4 (–CH3), 152.5 (C=N), 161.2 (C=O), 150.68, 140.7, 132.85, 131.5, 131.3, 129.4, 123.7, 121.2 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1616; ν(C=O), 1725; νasym(COO), 1588; νsym(COO), 1322; (Zr←N), 530; ν(Zr–O), 462.Compound
Z
r
(
L
4
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L4H); colour, reddish brown; yield, 0.120 g; mp, 160°C (d) and elemental analysis (%), calcd. for C26H26Cl2N4O6S2Zr: C, 43.57; H, 3.66; N, 7.82; found, C: 43.15; H, 3.70; N, 7.70; molecular weight: found, 723.11, calcd. 716.77. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.2; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.62 (t, 1H, N–CH–), 2.20–2.30 (m, 4H, –CH2–), 1.56 (s, 3H, –CH3), 8.00 (s, 1H, NH), 7.10–7.72 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 185.6 (COO); 62.3 (CH); 26.8, 30.2 (CH2); 17.9 (CH3); 153.7 (C=N); 158.1 (C=O); 144.86, 136.2, 132.5, 128.24, 122.6, 117.3 (aromatic carbons); UV-visible (λmax, nm): 218, 260, 378; infrared (KBr, cm−1): ν(C=N), 1608; ν(C=O), 1722, ν(NH), 3130, νasym(COO), 1582; νsym(COO), 1310; ν(Zr←N), 542; ν(Zr–O), 468.Compound
Z
r
(
L
5
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L5H); colour, brown; yield, 0.194 g; mp, 254°C (d) and elemental analysis (%), calcd. for C22H16Cl4N4O6Zr: C, 39.71; H, 2.42; N, 8.42; found, C: 39.56; H, 2.40; N, 8.34; molecular weight: found, 660.29, calcd. 665.42. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 11.9; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.15 (q, 1H, N–CH–); 1.40 (d, 3H, –CH3); 8.00 (s, 1H, NH), 7.02–7.60 (m, 3H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1612; ν(C=O), 1720; νasym(COO), 1585; νsym(COO), 1315; ν(Zr←N), 530; ν(Zr–O), 460.Compound
Z
r
(
L
6
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L6H); colour, brown; yield, 0.203 g; mp, 180°C (d) and elemental analysis (%), calcd. for C26H24Cl4N4O6Zr: C, 43.28; H, 3.35; N, 7.77; found, C: 42.97; H, 3.41; N, 7.62; molecular weight: found, 708.58, calcd. 721.53. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 10.6; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.00 (t, 1H, N–CH–); 2.25–2.28 (m, 1H, –CH2–); 8.40 (s, 1H, NH), 7.01–7.70 (m, 3H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1615; ν(C=O), 1722; νasym(COO), 1590; νsym(COO), 1320; ν(Zr←N), 538; ν(Zr–O), 466.Compound
Z
r
(
L
7
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L7H); colour, brown; yield, 0.332 g; mp, 210°C (d) and elemental analysis (%) calcd. for C34H26Cl2N4O6Zr: C, 54.54; H, 3.50; N, 7.48; found, C: 54.44; H, 3.55; N, 7.54; molecular weight: found, 755.64, calcd. 748.72. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.6; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.26 (t, 1H, N–CH–CH2–), 3.06 (d, 2H, –CH2–Ph), 8.00 (s, 1H, NH), 7.12–7.80 (m, 9H, aromatic); 13C NMR (DMSO, δ ppm): 185.8 (COO), 66.7 (–CH–), 38.3 (–CH2–), 15.9 (C=N), 166.4 (C=O), 149.6, 135.7, 133.1, 128.5, 127.6, 126.3, 124.5, 122.7, 120.8 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1609; ν(C=O), 1725; νasym(COO), 1585; νsym(COO), 1320; ν(Zr←N), 540; ν(Zr–O), 460.Compound
Z
r
(
L
8
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L8H); colour, dark brown; yield, 0.127 g; mp, 218°C (d) and elemental analysis (%), calcd. for C38H28Cl2N6O6Zr: C, 55.20; H, 3.41; N, 10.16; found, C: 55.03; H, 3.36; N, 10.21; molecular weight: found, 821.15, calcd. 826.80. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.4; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.36 (t, 1H, N–CH–CH2–); 3.22 (d, 2H, –CH2–); 8.06 (s, 1H, NH), 6.98–7.76 (m, 9H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1614; ν(C=O), 1726; νasym(COO), 1594; νsym(COO), 1318; ν(Zr←N), 535; ν(Zr–O), 470.


## 2.1. Starting Materials

All chemicals used in the present work, 1H-indole-2,3-dione, 5-chloro-1H-indole-2,3-dione, amino acids (glycine, alanine, valine, methionine, phenylalanine, and tryptophan), and oxozirconium(IV) chloride, were of analytical grade. The ligands were prepared by the condensation of isatins with amino acids as described earlier [9, 26].


## 2.2. Analytical Procedures

Solvents used were dried and purified by standard methods and moisture was excluded from the glass apparatus using CaCl2 drying tubes. The melting points of the compounds were determined on a capillary melting point apparatus and were not corrected. The purity of the compounds was confirmed by thin layer chromatography using silica gel-G glass plates as the stationary phase and benzene and ethanol (9 : 1) as the mobile phase. Zirconium was determined gravimetrically as its oxide, ZrO2. Nitrogen and sulfur were determined by Kjeldahl’s and Messenger’s methods, respectively. Molecular weight determinations were carried out by the Rast camphor method.


## 2.3. Physical Measurements

The IR spectra of samples in KBr pellets were recorded on an FTIR spectrophotometer model SP-2, Perkin Elmer in the range of 4000–400 cm−1. The electronic spectra of the ligands and their metal complexes were recorded in dry DMSO, on a thermo-, double-beam spectrophotometer UV 1, in the range of 800–200 nm. The fluorescence studies of Schiff base and its metal complexes were recorded on Shimadzu RF-5301PC spectrophotometer. The molar conductance of the complexes was measured on 10−3 M DMF solutions using Systronics conductivity bride model 305. 1H and 13C NMR spectra were recorded on Bruker avance II (400 MHz) FTNMR spectrometer at the SAIF, Punjab University, Chandigarh, using DMSO-d6 as the solvent and tetramethylsilane (TMS) as an internal standard.


## 2.4. Molecular Modeling Studies

The molecular modeling of a representative compound is carried out on a CS Chem 3D ultramolecular modeling and analysis programme, interactive graphics programme that enables rapid structure building and geometry optimization with minimum energy and molecular display.


## 2.5. Preparation of Zirconium Complexes

The complexes were prepared by treating oxozirconium(IV) chloride (1.61 mmol) in methanol with the corresponding Schiff bases (3.22 mmol) in the same solvent. The mixture was refluxed for three hours on a water bath after which the crystals of the complex separate out on cooling; the mixture was concentrated on a steam bath until about one-third of the solution remained. The concentrated solution was cooled after which the crystals were filtered, washed with methanol, and then dried in vacuum at45±5°C after repeated washing with dry cyclohexane. The compounds were purified by recrystallization from the same solvent. The purity of the compounds was checked by TLC using silica gel G as adsorbent.Compound
Z
r
(
L
1
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L1H); colour, red; yield, 0.218 g; mp, 170°C (d) and elemental analysis (%), calcd. for C20H14Cl2N4O6Zr: C, 42.26; H, 2.48; N, 9.86; found, C: 42.33; H, 2.57; N, 9.81; molecular weight: found, 580.12, calcd. 568.48. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 10.8; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.28 (s, 2H, N–CH2–), 8.06 (s, 1H, NH), 7.18–7.78 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 186.3 (COO), 52.1 (–CH2–), 153.8 (C=N), 167.3 (C=O), 148.65, 131.2, 129.9, 125.3, 122.7, 119.5 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1610; ν(C=O), 1722; νasym(COO), 1595; νsym(COO), 1325; ν(Zr←N), 535; ν(Zr–O), 465.Compound
Z
r
(
L
2
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L2H); colour, reddish brown; yield, 0.317 g; mp, 200°C (d) and elemental analysis (%), calcd. for C22H18Cl2N4O6Zr: C, 44.30; H, 3.04; N, 9.39; found, C: 44.46; H, 3.10; N, 9.33; molecular weight: found, 590.68, calcd. 596.53. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 11.5; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.70 (q, 1H, N–CH–); 8.32 (s, 1H, NH); 1.50 (d, 3H, C-CH3); 7.00–7.86 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 180.7 (COO), 63.6 (–CH–), 150.2 (C=N), 159.6 (C=O), 1502.7, 138.3, 133.6, 131.7, 130.5, 129.3, 124.9, 121.1 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1617; ν(C=O), 1728; νasym(COO), 1585; νsym(COO), 1322; ν(Zr←N), 537; ν(Zr–O), 460.Compound
Z
r
(
L
3
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L3H); colour, brown; yield, 0.179 g; mp, 144°C (d) and elemental analysis (%), calcd. for C26H26Cl2N4O6Zr: C, 47.85; H, 4.02; N, 8.58; found, C: 47.89; H, 4.14; N, 8.54; molecular weight: found, 640.96, calcd. 652.64. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 8.5; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.26 (d, 1H, N–CH–); 8.40 (s, 1H, NH); 2.16–2.30 (m, 1H, –CH–); 1.22 (d, 3H, –CH3) 7.11–7.65 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 183.1 (COO), 67.5 (–CH–), 18.4 (–CH3), 152.5 (C=N), 161.2 (C=O), 150.68, 140.7, 132.85, 131.5, 131.3, 129.4, 123.7, 121.2 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1616; ν(C=O), 1725; νasym(COO), 1588; νsym(COO), 1322; (Zr←N), 530; ν(Zr–O), 462.Compound
Z
r
(
L
4
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L4H); colour, reddish brown; yield, 0.120 g; mp, 160°C (d) and elemental analysis (%), calcd. for C26H26Cl2N4O6S2Zr: C, 43.57; H, 3.66; N, 7.82; found, C: 43.15; H, 3.70; N, 7.70; molecular weight: found, 723.11, calcd. 716.77. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.2; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.62 (t, 1H, N–CH–), 2.20–2.30 (m, 4H, –CH2–), 1.56 (s, 3H, –CH3), 8.00 (s, 1H, NH), 7.10–7.72 (m, 4H, aromatic); 13C NMR (DMSO, δ ppm): 185.6 (COO); 62.3 (CH); 26.8, 30.2 (CH2); 17.9 (CH3); 153.7 (C=N); 158.1 (C=O); 144.86, 136.2, 132.5, 128.24, 122.6, 117.3 (aromatic carbons); UV-visible (λmax, nm): 218, 260, 378; infrared (KBr, cm−1): ν(C=N), 1608; ν(C=O), 1722, ν(NH), 3130, νasym(COO), 1582; νsym(COO), 1310; ν(Zr←N), 542; ν(Zr–O), 468.Compound
Z
r
(
L
5
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L5H); colour, brown; yield, 0.194 g; mp, 254°C (d) and elemental analysis (%), calcd. for C22H16Cl4N4O6Zr: C, 39.71; H, 2.42; N, 8.42; found, C: 39.56; H, 2.40; N, 8.34; molecular weight: found, 660.29, calcd. 665.42. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 11.9; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.15 (q, 1H, N–CH–); 1.40 (d, 3H, –CH3); 8.00 (s, 1H, NH), 7.02–7.60 (m, 3H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1612; ν(C=O), 1720; νasym(COO), 1585; νsym(COO), 1315; ν(Zr←N), 530; ν(Zr–O), 460.Compound
Z
r
(
L
6
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L6H); colour, brown; yield, 0.203 g; mp, 180°C (d) and elemental analysis (%), calcd. for C26H24Cl4N4O6Zr: C, 43.28; H, 3.35; N, 7.77; found, C: 42.97; H, 3.41; N, 7.62; molecular weight: found, 708.58, calcd. 721.53. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 10.6; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.00 (t, 1H, N–CH–); 2.25–2.28 (m, 1H, –CH2–); 8.40 (s, 1H, NH), 7.01–7.70 (m, 3H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1615; ν(C=O), 1722; νasym(COO), 1590; νsym(COO), 1320; ν(Zr←N), 538; ν(Zr–O), 466.Compound
Z
r
(
L
7
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L7H); colour, brown; yield, 0.332 g; mp, 210°C (d) and elemental analysis (%) calcd. for C34H26Cl2N4O6Zr: C, 54.54; H, 3.50; N, 7.48; found, C: 54.44; H, 3.55; N, 7.54; molecular weight: found, 755.64, calcd. 748.72. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.6; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.26 (t, 1H, N–CH–CH2–), 3.06 (d, 2H, –CH2–Ph), 8.00 (s, 1H, NH), 7.12–7.80 (m, 9H, aromatic); 13C NMR (DMSO, δ ppm): 185.8 (COO), 66.7 (–CH–), 38.3 (–CH2–), 15.9 (C=N), 166.4 (C=O), 149.6, 135.7, 133.1, 128.5, 127.6, 126.3, 124.5, 122.7, 120.8 (aromatic carbons); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1609; ν(C=O), 1725; νasym(COO), 1585; νsym(COO), 1320; ν(Zr←N), 540; ν(Zr–O), 460.Compound
Z
r
(
L
8
)
2
C
l
2 was prepared by reacting zirconium(IV) dichloride with ligand (L8H); colour, dark brown; yield, 0.127 g; mp, 218°C (d) and elemental analysis (%), calcd. for C38H28Cl2N6O6Zr: C, 55.20; H, 3.41; N, 10.16; found, C: 55.03; H, 3.36; N, 10.21; molecular weight: found, 821.15, calcd. 826.80. Molar conductance (DMF, 10−3, Ω−1, moL−1, cm2): 12.4; 1H NMR (DMSO-d6, δ ppm, 400 MHz): 4.36 (t, 1H, N–CH–CH2–); 3.22 (d, 2H, –CH2–); 8.06 (s, 1H, NH), 6.98–7.76 (m, 9H, aromatic); UV-visible (λmax, nm): 220, 260, 320, 370; infrared (KBr, cm−1): ν(C=N), 1614; ν(C=O), 1726; νasym(COO), 1594; νsym(COO), 1318; ν(Zr←N), 535; ν(Zr–O), 470.


## 3. Results and Discussion

The reactions of zirconium(IV) dichloride with the monofunctional bidentate Schiff bases were carried out in dry methanol in 1 : 2 stoichiometric ratios and can be represented by the equation in Scheme1.Scheme 1
Representative equation illustrating the formation of Schiff bases and their zirconium(IV) complexes.All these compounds are coloured solids, insoluble in common organic solvents and soluble in DMSO, DMF, CHCl3, MeOH, and so forth and insoluble in n-hexane and petroleum ether. The conductivity values for the Zr(L)2Cl2 complexes (in DMF, 10−3 moL, 25°C), ranging in the 8.5–12.6 Ω−1, moL−1, cm2 region, indicate that the nonelectrolytic nature of the compounds suggests that the anions are covalently bonded. The molecular weight determination by the Rast camphor method shows that the products are monomeric in nature.


### 3.1. IR Spectra

The IR absorption frequencies for the ligands and their zirconium complexes were recorded in the range 4000–400 cm−1. The assignment of important infrared data for ligand and complexes are listed in experimental section. A strong band (due to the azomethine group) at 1620–1635 cm−1 in the spectra of the free ligands [27, 28] is shifted to lower wavenumber in the complexes studied, showing the coordination of azomethine nitrogen to the metal atom [26, 29]. The coordination of azomethine nitrogen to the metal atom is supported by the appearance of a new absorption band at 535 cm−1, which may be assigned to ν(Zr←N) vibrations [30].The infrared spectra of all the zirconium complexes do not show the strong band in the region 3105–2740 cm−1 due to ν(COOH), indicating the deprotonation of the carboxylate group of the Schiff bases with zirconium metal as expected. It is further confirmed by the appearance of sharp band at 465 cm−1 in the spectra of all the complexes assignable to the ν(Zr–O) stretching vibrations [31]. In the spectra of the complexes two sharp bands are observed at 1590 and 1320 cm−1 and are assigned to the νasym(COO) and νsym(COO), respectively. Furthermore, the separation between asymmetric and symmetric vibrations is about 270 cm−1,  indicating the covalent nature of the metal-oxygen bond as unidentate manner. Ionic bonding and also bridging or chelation can therefore be excluded. Sandhu and Verma in their studies and reports have shown that the Δν value of complexes greater by 65–90 cm−1 than in their sodium salts indicates either asymmetric or monodentate bonding of the carboxylate group to metal atom [32]. Moreover, Δν values of complexes below 200 cm−1 would be expected for bridging or chelating carboxylates, but greater than 200 cm−1 for the monodentate bonding carboxylate anions [33]. The C=O band of the indole group appears in the range of 1720–1740 cm−1 in the ligands. However, a strong band at 1740 cm−1 due to the vibration of C=O group remains unchanged in the spectra of complexes showing thereby the noninvolvement of this group in coordination and  thus confirms that the C=O from indole is not involved in the complexation.


### 3.2. Electronic Spectra

The electronic spectra of Schiff bases and its zirconium complexes have been recorded in methanol. In spectrum of the ligand, three bands are observed at 280, 300, and 380 nm. The bands at 280 and 300 nm are due to theπ-π* transitions within the aromatic ring and remain almost unchanged in the spectra of zirconium complexes. Another band at 380 nm is due to the n-π* transitions within the >C=N– chromophore and shows a bathochromic shift in the spectra of zirconium complexes due to the coordination of azomethine nitrogen to the zirconium atom. This band shifts slightly to the higher-energy region in the spectra of zirconium complexes due to the polarization within the >C=N chromophore caused by the zirconium-ligand electron interaction.


### 3.3.1H NMR Spectra

The characteristic resonance peaks for the synthesized compounds have been recorded in DMSO-d6 and data are given in experimental section. The expected resonances are assigned by their peak multiplicity, intensity patterns, and integration. The 1H NMR spectral data of the ligands show single resonance at δ11.4±0.10 ppm, which is absent in the spectra of the metal complexes, indicating the replacement of the carboxylic acid proton by the Zr(IV) moiety. The ligands give a complex multiplet signal in the region δ 7.20–7.82 ppm for the aromatic protons and these remain almost at the same position in the spectra of the metal complexes. The appearance of signals due to NH protons at the same positions in the ligand and its complexes shows the non-involvement of this group in coordination.Schiff bases derived from glycine, alanine, valine, and methionine display four/three aromatic protons, as expected. In the spectrum of phenylalanine, the integral of the aromatic region corresponds to nine protons; five protons on the phenyl ring are recognizable at 7.4 ppm. Methylene (for glycine, alanine, valine, and methionine) protons on theα-carbon of the carboxylic acid moieties appear at 3.96–4.30 ppm. This signal is a singlet for (1), a doublet for (3) and (6), a triplet for (7) and (8), and a quartet for (2) and (5) all of which arise from the nonequivalent methylene protons in structures (1–8). In general, the complexes obtained were found to exhibit no additional resonances and thus reflect the purity of the complexes. The integration of peaks concurs with the number of protons postulated from the structures proposed for the complexes.


### 3.4.13C NMR Spectra

The13C NMR spectral data for ligands and their corresponding metal complexes have been recorded in experimental part. Evidence of the formation of the complexes is clearly displayed in the 13C NMR spectra. The 13C NMR spectra of complexes showed that the δ(COO) signal shifted to the downfield region which is lower compared to that of the ligand (176.1–178.5 ppm) indicating the carboxylate anion is bonded to zirconium atom upon complexation. The signals due to the carbon atom attached to the azomethine group in the ligands appear at δ162.3±0.90 ppm. However, in the spectra of the corresponding metal complexes, these appear at ~δ 154.2 ppm. The considerable shifts in the resonance of the carbon atom attached to nitrogen indicate the involvement of azomethine nitrogen atom of coordination. The occurrence of eight resonances in the range of δ 118.3–150.7 ppm in the 13C NMR spectra of the complexes and ligands is defined as aromatic carbons signals. Generally, the 13C NMR spectra of the complexes obtained were found to exhibit no additional resonances and thus reflected the purity of the complexes.Though, it is also possible that the shifting of azomethine carbon is due to the change in hybridization of nitrogen attached to carboxylate group, but in the light of IR, UV, and1H NMR spectral studies it seems more plausible that the shifting in these carbons is due to the involvement of carboxylate oxygen and azomethine nitrogen in bonding.


### 3.5. Fluorescence Spectral Studies

Metal-ligand coordination may lead to significant changes of the fluorescence properties of the ligand, including increase of the intensity, shift of the emission wavelength, appearance of new emissions, or quenching of the fluorescence. The fluorescence spectra of the Schiff base HL1 and HL3 and their metal complexes were recorded in DMF with excitation wavelength 380 nm at room temperature (298 K). The fluorescence emission spectrum of HL1 with its metal complexes is depicted in Figures 1 and 2. HL1 exhibits a strong fluorescence emission at 430 nm; in contrast with this partial fluorescence quenching phenomena are observed in its metal complexes with weak fluorescence emission at 432 nm for zirconium(IV). HL3 shows strong fluorescence band at 435 nm and its Zr(IV) complexes exhibit weak emission bands at 436 nm, respectively. The maximum emission wavelength of Schiff bases is red-shifted about 10–20 nm owing to the formation of complex, which may be tentatively assigned to the ligand to metal charge transfer (LMCT). It is evident from the fluorescence spectra that fluorescence emission intensity of Schiff bases decreased dramatically on complex formation with transition metal ions. The decrease in fluorescence intensity with formation of metal complexes is due to decrease in electron density on Schiff bases [34, 35]. All these fluorescent emissions may be assigned to the intraligand fluorescence since the free ligand exhibited a similar emission at 430 and 435 nm, respectively, under the same condition.Figure 1
Emission spectra of the ligand (L3H).Figure 2
Emission spectra of the Zr(L3)2Cl2 complex.


### 3.6. Molecular Modeling and Analysis

The ligand (L4H) has 50 filled molecular orbitals, and the orbitals of the HOMO and LUMO levels are shown in Figures 3(a) and 3(b). Notice that the HOMO orbitals are concentrated on the oxygen and nitrogen atoms while the LUMO orbitals are concentrated on the carbons of the indole rings. The HOMO and LUMO energy was found to be −8.268 eV and −4.368 eV. All the synthesized compounds have hexa-coordination and distorted octahedral geometry. Molecular modeling was performed for [ZrCl2(L4)2], as representative compound.  Tables 1 and 2 list selected interatomic distances and bond angles. The structure of the complex with atomic numbering scheme is shown in Figure 4. The complex consists of two units of ligand molecule with metal ion Zr(IV). The complex is of six coordinates with distorted octahedral environment around the metal ion. The metal ion Zr(IV) is coordinated to one azomethine nitrogen atom and one carboxylate oxygen atom of Schiff-base ligand and Cl ion. The Zr–O and Zr–N bond lengths are 2.092 Å and 2.138 Å, respectively, and the bond distance between Zr–Cl is 2.444 Å. The two chloride groups are equidistant from Zr (2.44 Å) and complete the coordination sphere of Zr. The Cl–Zr–Cl angles are 154.92°. The O–Zr–N, N–Zr–N, and O–Zr–O angles are 80.11, 149.08, and 148.23°, respectively, for both the Schiff-base ligands. These angles and distances are in good agreement with the X-ray structure of a similar zirconium complex [36]. The Zr–Cl distances for the metal bound chloride groups are also similar in both complexes and are comparable with reported zirconium compounds [37].Table 1
Various Bond Lengths of Compound [Zr(L4)2Cl2].
S. No.
Atoms
Actual (Å)
Optimal (Å)
1
Zr(4)-N(3)
2.1381
2
C(41)-H(66)
1.1131
1.113
3
C(41)-H(65)
1.1126
1.113
4
C(39)-H(64)
1.1137
1.113
5
C(39)-H(63)
1.1153
1.113
6
C(38)-H(62)
1.1125
1.113
7
C(38)-H(61)
1.1135
1.113
8
C(38)-H(60)
1.1127
1.113
9
C(36)-H(59)
1.1132
1.113
10
C(36)-H(58)
1.1141
1.113
11
C(35)-H(57)
1.1142
1.113
12
C(35)-H(56)
1.1132
1.113
13
C(34)-H(55)
1.0939
1.1
14
C(33)-H(54)
1.1023
1.1
15
C(32)-H(53)
1.1023
1.1
16
C(31)-H(52)
1.1016
1.1
17
N(27)-H(51)
1.0444
1.05
18
C(25)-H(50)
1.1159
1.113
19
C(25)-H(49)
1.1146
1.113
20
C(24)-H(48)
1.1012
1.1
21
C(23)-H(47)
1.1061
1.1
22
C(22)-H(46)
1.1049
1.1
23
C(21)-H(45)
1.1012
1.1
24
N(17)-H(44)
1.0446
1.05
25
C(8)-H(43)
1.1138
1.113
26
C(2)-H(42)
1.1165
1.113
27
S(40)-C(41)
1.8167
1.815
28
C(39)-S(40)
1.8236
1.815
29
C(25)-C(39)
1.5388
1.523
30
S(37)-C(38)
1.8142
1.815
31
C(36)-S(37)
1.8255
1.815
32
C(35)-C(36)
1.5393
1.523
33
N(9)-Zr(4)
2.1345
34
Zr(4)-O(5)
2.0916
35
C(2)-C(35)
1.5486
1.523
36
C(34)-C(29)
1.4014
1.42
37
C(33)-C(34)
1.3978
1.42
38
C(32)-C(33)
1.3994
1.42
39
C(31)-C(32)
1.3929
1.42
40
C(28)-C(31)
1.3971
1.42
41
C(26)-O(30)
1.2293
1.208
42
C(29)-C(15)
1.4774
1.503
43
C(28)-C(29)
1.4077
1.42
44
N(27)-C(28)
1.3928
1.462
45
C(26)-N(27)
1.3678
1.462
46
C(15)-C(26)
1.5141
1.517
47
C(8)-C(25)
1.5398
1.523
48
C(24)-C(19)
1.4832
1.42
49
C(23)-C(24)
1.5134
1.42
50
C(22)-C(23)
1.5149
1.42
51
C(21)-C(22)
1.5092
1.42
52
C(18)-C(21)
1.4845
1.42
53
C(16)-O(20)
1.3098
1.208
54
C(19)-C(14)
1.5193
1.503
55
C(18)-C(19)
1.374
1.42
56
N(17)-C(18)
1.3476
1.462
57
C(16)-N(17)
1.3903
1.462
58
C(14)-C(16)
1.5503
1.517
59
N(3)-C(15)
1.2988
1.26
60
N(9)-C(14)
2.1882
1.26
61
C(1)-O(13)
1.2142
1.208
62
C(7)-O(12)
1.2117
1.208
63
Zr(4)-Cl(11)
2.4423
64
Zr(4)-Cl(10)
2.4453
65
C(8)-N(9)
1.4968
1.47
66
C(7)-C(8)
1.5279
1.509
67
O(6)-C(7)
1.3594
1.338
68
C(41)-H(67)
1.1129
1.113
69
O(5)-C(1)
1.3551
1.338
70
Zr(4)-O(6)
2.0914
71
C(2)-N(3)
1.5032
1.47
72
C(1)-C(2)
1.5292
1.509Table 2
Various Bond Angles of Compound [Zr(L4)2Cl2].
S. No.
Atoms
Actual (°)
Optimal (°)
1
H(67)-C(41)-H(66)
109.418
109
2
H(67)-C(41)-H(65)
108.9614
109
3
H(67)-C(41)-S(40)
110.3566
109.3
4
H(66)-C(41)-H(65)
108.7912
109
5
H(66)-C(41)-S(40)
109.9408
109.3
6
H(65)-C(41)-S(40)
109.3437
109.3
7
C(41)-S(40)-C(39)
97.5564
96.3
8
H(64)-C(39)-H(63)
107.5686
109.4
9
H(64)-C(39)-S(40)
110.1883
112
10
H(64)-C(39)-C(25)
110.4229
109.41
11
H(63)-C(39)-S(40)
109.8119
112
12
H(63)-C(39)-C(25)
109.1207
109.41
13
S(40)-C(39)-C(25)
109.6938
106.5
14
H(62)-C(38)-H(61)
109.6623
109
15
H(62)-C(38)-H(60)
109.0937
109
16
H(62)-C(38)-S(37)
110.3571
109.3
17
H(61)-C(38)-H(60)
108.6879
109
18
H(61)-C(38)-S(37)
110.0128
109.3
19
H(60)-C(38)-S(37)
108.9946
109.3
20
C(38)-S(37)-C(36)
98.533
96.3
21
H(59)-C(36)-H(58)
107.1198
109.4
22
H(59)-C(36)-S(37)
110.417
112
23
H(59)-C(36)-C(35)
109.5515
109.41
24
H(58)-C(36)-S(37)
110.7645
112
25
H(58)-C(36)-C(35)
110.8347
109.41
26
S(37)-C(36)-C(35)
108.1586
106.5
27
H(57)-C(35)-H(56)
104.9845
109.4
28
H(57)-C(35)-C(36)
108.6578
109.41
29
H(57)-C(35)-C(2)
110.8409
109.41
30
H(56)-C(35)-C(36)
108.9072
109.41
31
H(56)-C(35)-C(2)
109.5018
109.41
32
C(36)-C(35)-C(2)
113.5779
109.5
33
H(55)-C(34)-C(29)
122.3033
120
34
H(55)-C(34)-C(33)
117.5306
120
35
C(29)-C(34)-C(33)
120.1661
36
H(54)-C(33)-C(34)
119.6447
120
37
H(54)-C(33)-C(32)
119.4129
120
38
C(34)-C(33)-C(32)
120.9424
39
H(53)-C(32)-C(33)
119.7786
120
40
H(53)-C(32)-C(31)
120.1954
120
41
C(33)-C(32)-C(31)
119.9868
42
H(52)-C(31)-C(32)
121.1904
120
43
H(52)-C(31)-C(28)
120.678
120
44
C(32)-C(31)-C(28)
118.1313
45
C(34)-C(29)-C(15)
134.3781
120
46
C(34)-C(29)-C(28)
117.1629
120
47
C(15)-C(29)-C(28)
108.4549
120
48
C(31)-C(28)-C(29)
123.0239
120
49
C(31)-C(28)-N(27)
126.8775
120
50
C(29)-C(28)-N(27)
110.0936
120
51
H(51)-N(27)-C(28)
126.0741
118
52
H(51)-N(27)-C(26)
125.3088
118
53
C(28)-N(27)-C(26)
108.5425
54
O(30)-C(26)-N(27)
120.8581
122.6
55
O(30)-C(26)-C(15)
129.2063
123
56
N(27)-C(26)-C(15)
109.9356
122
57
H(50)-C(25)-H(49)
106.678
109.4
58
H(50)-C(25)-C(39)
108.7135
109.41
59
H(50)-C(25)-C(8)
108.393
109.41
60
H(49)-C(25)-C(39)
111.2794
109.41
61
H(49)-C(25)-C(8)
109.454
109.41
62
C(39)-C(25)-C(8)
112.1296
109.5
63
H(48)-C(24)-C(19)
117.3341
120
64
H(48)-C(24)-C(23)
117.009
120
65
C(19)-C(24)-C(23)
119.9311
66
H(47)-C(23)-C(24)
113.9434
120
67
H(47)-C(23)-C(22)
114.0848
120
68
C(24)-C(23)-C(22)
118.3693
69
H(46)-C(22)-C(23)
115.8207
120
70
H(46)-C(22)-C(21)
115.0649
120
71
C(23)-C(22)-C(21)
118.1479
72
H(45)-C(21)-C(22)
119.4891
120
73
H(45)-C(21)-C(18)
118.9569
120
74
C(22)-C(21)-C(18)
118.0658
75
C(24)-C(19)-C(14)
124.1732
120
76
C(24)-C(19)-C(18)
120.434
120
77
C(14)-C(19)-C(18)
114.4563
120
78
C(21)-C(18)-C(19)
123.9331
120
79
C(21)-C(18)-N(17)
126.1831
120
80
C(19)-C(18)-N(17)
109.7946
120
81
H(44)-N(17)-C(18)
126.029
118
82
H(44)-N(17)-C(16)
126.0518
118
83
C(18)-N(17)-C(16)
107.8705
84
O(20)-C(16)-N(17)
122.4042
122.6
85
O(20)-C(16)-C(14)
123.6108
123
86
N(17)-C(16)-C(14)
113.7879
122
87
C(29)-C(15)-C(26)
101.2183
117.6
88
C(29)-C(15)-N(3)
129.5068
120
89
C(26)-C(15)-N(3)
129.128
120
90
C(19)-C(14)-C(16)
93.7144
117.6
91
C(19)-C(14)-N(9)
101.1826
120
92
C(16)-C(14)-N(9)
103.5499
120
93
Zr(4)-N(9)-C(14)
104.5285
94
Zr(4)-N(9)-C(8)
111.1129
95
C(14)-N(9)-C(8)
111.1476
96
H(43)-C(8)-C(25)
108.1727
109.39
97
H(43)-C(8)-N(9)
109.7641
107.5
98
H(43)-C(8)-C(7)
106.4941
107.9
99
C(25)-C(8)-N(9)
111.9987
100
C(25)-C(8)-C(7)
113.8847
109.9
101
N(9)-C(8)-C(7)
106.3523
102
O(12)-C(7)-C(8)
125.0648
122.5
103
O(12)-C(7)-O(6)
124.6366
122
104
C(8)-C(7)-O(6)
110.2827
107.1
105
Zr(4)-O(6)-C(7)
111.3282
106
Zr(4)-O(5)-C(1)
114.0377
107
N(3)-Zr(4)-O(5)
80.1135
108
N(3)-Zr(4)-O(6)
128.6218
109
N(3)-Zr(4)-N(9)
149.0865
110
N(3)-Zr(4)-Cl(11)
88.0663
111
N(3)-Zr(4)-Cl(10)
84.2757
112
O(5)-Zr(4)-O(6)
148.2304
113
O(5)-Zr(4)-N(9)
78.2701
114
O(5)-Zr(4)-Cl(11)
85.1672
115
O(5)-Zr(4)-Cl(10)
116.7647
116
O(6)-Zr(4)-N(9)
78.9572
117
O(6)-Zr(4)-Cl(11)
82.9908
118
O(6)-Zr(4)-Cl(10)
83.2655
119
N(9)-Zr(4)-Cl(11)
111.6987
120
N(9)-Zr(4)-Cl(10)
86.0092
121
Cl(11)-Zr(4)-Cl(10)
154.9219
122
Zr(4)-N(3)-C(15)
121.0647
123
Zr(4)-N(3)-C(2)
107.937
124
C(15)-N(3)-C(2)
120.234
125
H(42)-C(2)-C(35)
110.432
109.39
126
H(42)-C(2)-N(3)
106.5807
107.5
127
H(42)-C(2)-C(1)
102.9891
107.9
128
C(35)-C(2)-N(3)
118.1743
129
C(35)-C(2)-C(1)
109.8863
109.9
130
N(3)-C(2)-C(1)
107.6576
131
O(13)-C(1)-O(5)
124.3628
122
132
O(13)-C(1)-C(2)
123.8243
122.5
133
O(5)-C(1)-C(2)
111.734
107.1(a) HOMO orbitals of the MM2 geometry-optimized structure of the ligand (L4H). (b) LUMO orbitals of the MM2 geometry-optimized structure of the ligand (L4H).
(a)
(b)Figure 4
3D molecular structure of Zr(L4)2Cl2.In all, 205 measurements of the bond lengths (72 in numbers) plus the bond angles (133 in numbers) are listed. Except for a few cases, optimum values of both the bond lengths and the bond angles are given in the tables, with the actual values. The actual bond lengths/bond angles given in Tables1 and 2 are calculated values as a result of energy optimization in Chem3D Ultra, and the optimum bond length/bond angle values are the standard bond lengths/bond angles established by the builder unit of CHEM 3D. Some values of standard bond lengths/bond angles are missing, possibly because of limitations of the software; we have already noticed this when modeling other systems. In most cases, the actual bond lengths and bond angles are close to the optimum values, confirming the proposed structure of the compound [Zr(L4)2Cl].


## 3.1. IR Spectra

The IR absorption frequencies for the ligands and their zirconium complexes were recorded in the range 4000–400 cm−1. The assignment of important infrared data for ligand and complexes are listed in experimental section. A strong band (due to the azomethine group) at 1620–1635 cm−1 in the spectra of the free ligands [27, 28] is shifted to lower wavenumber in the complexes studied, showing the coordination of azomethine nitrogen to the metal atom [26, 29]. The coordination of azomethine nitrogen to the metal atom is supported by the appearance of a new absorption band at 535 cm−1, which may be assigned to ν(Zr←N) vibrations [30].The infrared spectra of all the zirconium complexes do not show the strong band in the region 3105–2740 cm−1 due to ν(COOH), indicating the deprotonation of the carboxylate group of the Schiff bases with zirconium metal as expected. It is further confirmed by the appearance of sharp band at 465 cm−1 in the spectra of all the complexes assignable to the ν(Zr–O) stretching vibrations [31]. In the spectra of the complexes two sharp bands are observed at 1590 and 1320 cm−1 and are assigned to the νasym(COO) and νsym(COO), respectively. Furthermore, the separation between asymmetric and symmetric vibrations is about 270 cm−1,  indicating the covalent nature of the metal-oxygen bond as unidentate manner. Ionic bonding and also bridging or chelation can therefore be excluded. Sandhu and Verma in their studies and reports have shown that the Δν value of complexes greater by 65–90 cm−1 than in their sodium salts indicates either asymmetric or monodentate bonding of the carboxylate group to metal atom [32]. Moreover, Δν values of complexes below 200 cm−1 would be expected for bridging or chelating carboxylates, but greater than 200 cm−1 for the monodentate bonding carboxylate anions [33]. The C=O band of the indole group appears in the range of 1720–1740 cm−1 in the ligands. However, a strong band at 1740 cm−1 due to the vibration of C=O group remains unchanged in the spectra of complexes showing thereby the noninvolvement of this group in coordination and  thus confirms that the C=O from indole is not involved in the complexation.


## 3.2. Electronic Spectra

The electronic spectra of Schiff bases and its zirconium complexes have been recorded in methanol. In spectrum of the ligand, three bands are observed at 280, 300, and 380 nm. The bands at 280 and 300 nm are due to theπ-π* transitions within the aromatic ring and remain almost unchanged in the spectra of zirconium complexes. Another band at 380 nm is due to the n-π* transitions within the >C=N– chromophore and shows a bathochromic shift in the spectra of zirconium complexes due to the coordination of azomethine nitrogen to the zirconium atom. This band shifts slightly to the higher-energy region in the spectra of zirconium complexes due to the polarization within the >C=N chromophore caused by the zirconium-ligand electron interaction.


## 3.3.1H NMR Spectra

The characteristic resonance peaks for the synthesized compounds have been recorded in DMSO-d6 and data are given in experimental section. The expected resonances are assigned by their peak multiplicity, intensity patterns, and integration. The 1H NMR spectral data of the ligands show single resonance at δ11.4±0.10 ppm, which is absent in the spectra of the metal complexes, indicating the replacement of the carboxylic acid proton by the Zr(IV) moiety. The ligands give a complex multiplet signal in the region δ 7.20–7.82 ppm for the aromatic protons and these remain almost at the same position in the spectra of the metal complexes. The appearance of signals due to NH protons at the same positions in the ligand and its complexes shows the non-involvement of this group in coordination.Schiff bases derived from glycine, alanine, valine, and methionine display four/three aromatic protons, as expected. In the spectrum of phenylalanine, the integral of the aromatic region corresponds to nine protons; five protons on the phenyl ring are recognizable at 7.4 ppm. Methylene (for glycine, alanine, valine, and methionine) protons on theα-carbon of the carboxylic acid moieties appear at 3.96–4.30 ppm. This signal is a singlet for (1), a doublet for (3) and (6), a triplet for (7) and (8), and a quartet for (2) and (5) all of which arise from the nonequivalent methylene protons in structures (1–8). In general, the complexes obtained were found to exhibit no additional resonances and thus reflect the purity of the complexes. The integration of peaks concurs with the number of protons postulated from the structures proposed for the complexes.


## 3.4.13C NMR Spectra

The13C NMR spectral data for ligands and their corresponding metal complexes have been recorded in experimental part. Evidence of the formation of the complexes is clearly displayed in the 13C NMR spectra. The 13C NMR spectra of complexes showed that the δ(COO) signal shifted to the downfield region which is lower compared to that of the ligand (176.1–178.5 ppm) indicating the carboxylate anion is bonded to zirconium atom upon complexation. The signals due to the carbon atom attached to the azomethine group in the ligands appear at δ162.3±0.90 ppm. However, in the spectra of the corresponding metal complexes, these appear at ~δ 154.2 ppm. The considerable shifts in the resonance of the carbon atom attached to nitrogen indicate the involvement of azomethine nitrogen atom of coordination. The occurrence of eight resonances in the range of δ 118.3–150.7 ppm in the 13C NMR spectra of the complexes and ligands is defined as aromatic carbons signals. Generally, the 13C NMR spectra of the complexes obtained were found to exhibit no additional resonances and thus reflected the purity of the complexes.Though, it is also possible that the shifting of azomethine carbon is due to the change in hybridization of nitrogen attached to carboxylate group, but in the light of IR, UV, and1H NMR spectral studies it seems more plausible that the shifting in these carbons is due to the involvement of carboxylate oxygen and azomethine nitrogen in bonding.


## 3.5. Fluorescence Spectral Studies

Metal-ligand coordination may lead to significant changes of the fluorescence properties of the ligand, including increase of the intensity, shift of the emission wavelength, appearance of new emissions, or quenching of the fluorescence. The fluorescence spectra of the Schiff base HL1 and HL3 and their metal complexes were recorded in DMF with excitation wavelength 380 nm at room temperature (298 K). The fluorescence emission spectrum of HL1 with its metal complexes is depicted in Figures 1 and 2. HL1 exhibits a strong fluorescence emission at 430 nm; in contrast with this partial fluorescence quenching phenomena are observed in its metal complexes with weak fluorescence emission at 432 nm for zirconium(IV). HL3 shows strong fluorescence band at 435 nm and its Zr(IV) complexes exhibit weak emission bands at 436 nm, respectively. The maximum emission wavelength of Schiff bases is red-shifted about 10–20 nm owing to the formation of complex, which may be tentatively assigned to the ligand to metal charge transfer (LMCT). It is evident from the fluorescence spectra that fluorescence emission intensity of Schiff bases decreased dramatically on complex formation with transition metal ions. The decrease in fluorescence intensity with formation of metal complexes is due to decrease in electron density on Schiff bases [34, 35]. All these fluorescent emissions may be assigned to the intraligand fluorescence since the free ligand exhibited a similar emission at 430 and 435 nm, respectively, under the same condition.Figure 1
Emission spectra of the ligand (L3H).Figure 2
Emission spectra of the Zr(L3)2Cl2 complex.


## 3.6. Molecular Modeling and Analysis

The ligand (L4H) has 50 filled molecular orbitals, and the orbitals of the HOMO and LUMO levels are shown in Figures 3(a) and 3(b). Notice that the HOMO orbitals are concentrated on the oxygen and nitrogen atoms while the LUMO orbitals are concentrated on the carbons of the indole rings. The HOMO and LUMO energy was found to be −8.268 eV and −4.368 eV. All the synthesized compounds have hexa-coordination and distorted octahedral geometry. Molecular modeling was performed for [ZrCl2(L4)2], as representative compound.  Tables 1 and 2 list selected interatomic distances and bond angles. The structure of the complex with atomic numbering scheme is shown in Figure 4. The complex consists of two units of ligand molecule with metal ion Zr(IV). The complex is of six coordinates with distorted octahedral environment around the metal ion. The metal ion Zr(IV) is coordinated to one azomethine nitrogen atom and one carboxylate oxygen atom of Schiff-base ligand and Cl ion. The Zr–O and Zr–N bond lengths are 2.092 Å and 2.138 Å, respectively, and the bond distance between Zr–Cl is 2.444 Å. The two chloride groups are equidistant from Zr (2.44 Å) and complete the coordination sphere of Zr. The Cl–Zr–Cl angles are 154.92°. The O–Zr–N, N–Zr–N, and O–Zr–O angles are 80.11, 149.08, and 148.23°, respectively, for both the Schiff-base ligands. These angles and distances are in good agreement with the X-ray structure of a similar zirconium complex [36]. The Zr–Cl distances for the metal bound chloride groups are also similar in both complexes and are comparable with reported zirconium compounds [37].Table 1
Various Bond Lengths of Compound [Zr(L4)2Cl2].
S. No.
Atoms
Actual (Å)
Optimal (Å)
1
Zr(4)-N(3)
2.1381
2
C(41)-H(66)
1.1131
1.113
3
C(41)-H(65)
1.1126
1.113
4
C(39)-H(64)
1.1137
1.113
5
C(39)-H(63)
1.1153
1.113
6
C(38)-H(62)
1.1125
1.113
7
C(38)-H(61)
1.1135
1.113
8
C(38)-H(60)
1.1127
1.113
9
C(36)-H(59)
1.1132
1.113
10
C(36)-H(58)
1.1141
1.113
11
C(35)-H(57)
1.1142
1.113
12
C(35)-H(56)
1.1132
1.113
13
C(34)-H(55)
1.0939
1.1
14
C(33)-H(54)
1.1023
1.1
15
C(32)-H(53)
1.1023
1.1
16
C(31)-H(52)
1.1016
1.1
17
N(27)-H(51)
1.0444
1.05
18
C(25)-H(50)
1.1159
1.113
19
C(25)-H(49)
1.1146
1.113
20
C(24)-H(48)
1.1012
1.1
21
C(23)-H(47)
1.1061
1.1
22
C(22)-H(46)
1.1049
1.1
23
C(21)-H(45)
1.1012
1.1
24
N(17)-H(44)
1.0446
1.05
25
C(8)-H(43)
1.1138
1.113
26
C(2)-H(42)
1.1165
1.113
27
S(40)-C(41)
1.8167
1.815
28
C(39)-S(40)
1.8236
1.815
29
C(25)-C(39)
1.5388
1.523
30
S(37)-C(38)
1.8142
1.815
31
C(36)-S(37)
1.8255
1.815
32
C(35)-C(36)
1.5393
1.523
33
N(9)-Zr(4)
2.1345
34
Zr(4)-O(5)
2.0916
35
C(2)-C(35)
1.5486
1.523
36
C(34)-C(29)
1.4014
1.42
37
C(33)-C(34)
1.3978
1.42
38
C(32)-C(33)
1.3994
1.42
39
C(31)-C(32)
1.3929
1.42
40
C(28)-C(31)
1.3971
1.42
41
C(26)-O(30)
1.2293
1.208
42
C(29)-C(15)
1.4774
1.503
43
C(28)-C(29)
1.4077
1.42
44
N(27)-C(28)
1.3928
1.462
45
C(26)-N(27)
1.3678
1.462
46
C(15)-C(26)
1.5141
1.517
47
C(8)-C(25)
1.5398
1.523
48
C(24)-C(19)
1.4832
1.42
49
C(23)-C(24)
1.5134
1.42
50
C(22)-C(23)
1.5149
1.42
51
C(21)-C(22)
1.5092
1.42
52
C(18)-C(21)
1.4845
1.42
53
C(16)-O(20)
1.3098
1.208
54
C(19)-C(14)
1.5193
1.503
55
C(18)-C(19)
1.374
1.42
56
N(17)-C(18)
1.3476
1.462
57
C(16)-N(17)
1.3903
1.462
58
C(14)-C(16)
1.5503
1.517
59
N(3)-C(15)
1.2988
1.26
60
N(9)-C(14)
2.1882
1.26
61
C(1)-O(13)
1.2142
1.208
62
C(7)-O(12)
1.2117
1.208
63
Zr(4)-Cl(11)
2.4423
64
Zr(4)-Cl(10)
2.4453
65
C(8)-N(9)
1.4968
1.47
66
C(7)-C(8)
1.5279
1.509
67
O(6)-C(7)
1.3594
1.338
68
C(41)-H(67)
1.1129
1.113
69
O(5)-C(1)
1.3551
1.338
70
Zr(4)-O(6)
2.0914
71
C(2)-N(3)
1.5032
1.47
72
C(1)-C(2)
1.5292
1.509Table 2
Various Bond Angles of Compound [Zr(L4)2Cl2].
S. No.
Atoms
Actual (°)
Optimal (°)
1
H(67)-C(41)-H(66)
109.418
109
2
H(67)-C(41)-H(65)
108.9614
109
3
H(67)-C(41)-S(40)
110.3566
109.3
4
H(66)-C(41)-H(65)
108.7912
109
5
H(66)-C(41)-S(40)
109.9408
109.3
6
H(65)-C(41)-S(40)
109.3437
109.3
7
C(41)-S(40)-C(39)
97.5564
96.3
8
H(64)-C(39)-H(63)
107.5686
109.4
9
H(64)-C(39)-S(40)
110.1883
112
10
H(64)-C(39)-C(25)
110.4229
109.41
11
H(63)-C(39)-S(40)
109.8119
112
12
H(63)-C(39)-C(25)
109.1207
109.41
13
S(40)-C(39)-C(25)
109.6938
106.5
14
H(62)-C(38)-H(61)
109.6623
109
15
H(62)-C(38)-H(60)
109.0937
109
16
H(62)-C(38)-S(37)
110.3571
109.3
17
H(61)-C(38)-H(60)
108.6879
109
18
H(61)-C(38)-S(37)
110.0128
109.3
19
H(60)-C(38)-S(37)
108.9946
109.3
20
C(38)-S(37)-C(36)
98.533
96.3
21
H(59)-C(36)-H(58)
107.1198
109.4
22
H(59)-C(36)-S(37)
110.417
112
23
H(59)-C(36)-C(35)
109.5515
109.41
24
H(58)-C(36)-S(37)
110.7645
112
25
H(58)-C(36)-C(35)
110.8347
109.41
26
S(37)-C(36)-C(35)
108.1586
106.5
27
H(57)-C(35)-H(56)
104.9845
109.4
28
H(57)-C(35)-C(36)
108.6578
109.41
29
H(57)-C(35)-C(2)
110.8409
109.41
30
H(56)-C(35)-C(36)
108.9072
109.41
31
H(56)-C(35)-C(2)
109.5018
109.41
32
C(36)-C(35)-C(2)
113.5779
109.5
33
H(55)-C(34)-C(29)
122.3033
120
34
H(55)-C(34)-C(33)
117.5306
120
35
C(29)-C(34)-C(33)
120.1661
36
H(54)-C(33)-C(34)
119.6447
120
37
H(54)-C(33)-C(32)
119.4129
120
38
C(34)-C(33)-C(32)
120.9424
39
H(53)-C(32)-C(33)
119.7786
120
40
H(53)-C(32)-C(31)
120.1954
120
41
C(33)-C(32)-C(31)
119.9868
42
H(52)-C(31)-C(32)
121.1904
120
43
H(52)-C(31)-C(28)
120.678
120
44
C(32)-C(31)-C(28)
118.1313
45
C(34)-C(29)-C(15)
134.3781
120
46
C(34)-C(29)-C(28)
117.1629
120
47
C(15)-C(29)-C(28)
108.4549
120
48
C(31)-C(28)-C(29)
123.0239
120
49
C(31)-C(28)-N(27)
126.8775
120
50
C(29)-C(28)-N(27)
110.0936
120
51
H(51)-N(27)-C(28)
126.0741
118
52
H(51)-N(27)-C(26)
125.3088
118
53
C(28)-N(27)-C(26)
108.5425
54
O(30)-C(26)-N(27)
120.8581
122.6
55
O(30)-C(26)-C(15)
129.2063
123
56
N(27)-C(26)-C(15)
109.9356
122
57
H(50)-C(25)-H(49)
106.678
109.4
58
H(50)-C(25)-C(39)
108.7135
109.41
59
H(50)-C(25)-C(8)
108.393
109.41
60
H(49)-C(25)-C(39)
111.2794
109.41
61
H(49)-C(25)-C(8)
109.454
109.41
62
C(39)-C(25)-C(8)
112.1296
109.5
63
H(48)-C(24)-C(19)
117.3341
120
64
H(48)-C(24)-C(23)
117.009
120
65
C(19)-C(24)-C(23)
119.9311
66
H(47)-C(23)-C(24)
113.9434
120
67
H(47)-C(23)-C(22)
114.0848
120
68
C(24)-C(23)-C(22)
118.3693
69
H(46)-C(22)-C(23)
115.8207
120
70
H(46)-C(22)-C(21)
115.0649
120
71
C(23)-C(22)-C(21)
118.1479
72
H(45)-C(21)-C(22)
119.4891
120
73
H(45)-C(21)-C(18)
118.9569
120
74
C(22)-C(21)-C(18)
118.0658
75
C(24)-C(19)-C(14)
124.1732
120
76
C(24)-C(19)-C(18)
120.434
120
77
C(14)-C(19)-C(18)
114.4563
120
78
C(21)-C(18)-C(19)
123.9331
120
79
C(21)-C(18)-N(17)
126.1831
120
80
C(19)-C(18)-N(17)
109.7946
120
81
H(44)-N(17)-C(18)
126.029
118
82
H(44)-N(17)-C(16)
126.0518
118
83
C(18)-N(17)-C(16)
107.8705
84
O(20)-C(16)-N(17)
122.4042
122.6
85
O(20)-C(16)-C(14)
123.6108
123
86
N(17)-C(16)-C(14)
113.7879
122
87
C(29)-C(15)-C(26)
101.2183
117.6
88
C(29)-C(15)-N(3)
129.5068
120
89
C(26)-C(15)-N(3)
129.128
120
90
C(19)-C(14)-C(16)
93.7144
117.6
91
C(19)-C(14)-N(9)
101.1826
120
92
C(16)-C(14)-N(9)
103.5499
120
93
Zr(4)-N(9)-C(14)
104.5285
94
Zr(4)-N(9)-C(8)
111.1129
95
C(14)-N(9)-C(8)
111.1476
96
H(43)-C(8)-C(25)
108.1727
109.39
97
H(43)-C(8)-N(9)
109.7641
107.5
98
H(43)-C(8)-C(7)
106.4941
107.9
99
C(25)-C(8)-N(9)
111.9987
100
C(25)-C(8)-C(7)
113.8847
109.9
101
N(9)-C(8)-C(7)
106.3523
102
O(12)-C(7)-C(8)
125.0648
122.5
103
O(12)-C(7)-O(6)
124.6366
122
104
C(8)-C(7)-O(6)
110.2827
107.1
105
Zr(4)-O(6)-C(7)
111.3282
106
Zr(4)-O(5)-C(1)
114.0377
107
N(3)-Zr(4)-O(5)
80.1135
108
N(3)-Zr(4)-O(6)
128.6218
109
N(3)-Zr(4)-N(9)
149.0865
110
N(3)-Zr(4)-Cl(11)
88.0663
111
N(3)-Zr(4)-Cl(10)
84.2757
112
O(5)-Zr(4)-O(6)
148.2304
113
O(5)-Zr(4)-N(9)
78.2701
114
O(5)-Zr(4)-Cl(11)
85.1672
115
O(5)-Zr(4)-Cl(10)
116.7647
116
O(6)-Zr(4)-N(9)
78.9572
117
O(6)-Zr(4)-Cl(11)
82.9908
118
O(6)-Zr(4)-Cl(10)
83.2655
119
N(9)-Zr(4)-Cl(11)
111.6987
120
N(9)-Zr(4)-Cl(10)
86.0092
121
Cl(11)-Zr(4)-Cl(10)
154.9219
122
Zr(4)-N(3)-C(15)
121.0647
123
Zr(4)-N(3)-C(2)
107.937
124
C(15)-N(3)-C(2)
120.234
125
H(42)-C(2)-C(35)
110.432
109.39
126
H(42)-C(2)-N(3)
106.5807
107.5
127
H(42)-C(2)-C(1)
102.9891
107.9
128
C(35)-C(2)-N(3)
118.1743
129
C(35)-C(2)-C(1)
109.8863
109.9
130
N(3)-C(2)-C(1)
107.6576
131
O(13)-C(1)-O(5)
124.3628
122
132
O(13)-C(1)-C(2)
123.8243
122.5
133
O(5)-C(1)-C(2)
111.734
107.1(a) HOMO orbitals of the MM2 geometry-optimized structure of the ligand (L4H). (b) LUMO orbitals of the MM2 geometry-optimized structure of the ligand (L4H).
(a)
(b)Figure 4
3D molecular structure of Zr(L4)2Cl2.In all, 205 measurements of the bond lengths (72 in numbers) plus the bond angles (133 in numbers) are listed. Except for a few cases, optimum values of both the bond lengths and the bond angles are given in the tables, with the actual values. The actual bond lengths/bond angles given in Tables1 and 2 are calculated values as a result of energy optimization in Chem3D Ultra, and the optimum bond length/bond angle values are the standard bond lengths/bond angles established by the builder unit of CHEM 3D. Some values of standard bond lengths/bond angles are missing, possibly because of limitations of the software; we have already noticed this when modeling other systems. In most cases, the actual bond lengths and bond angles are close to the optimum values, confirming the proposed structure of the compound [Zr(L4)2Cl].


## 4. Conclusion

New Schiff bases and their zirconium complexes have been successfully synthesized. Elemental analysis data obtained are in good agreement with the predicted formula. Distorted octahedral geometries have been proposed for Zr(IV) complexes with the help of various physicochemical studies. The infrared spectra of these complexes show the presence of monofunctional and bidentate ligands. The Schiff base exhibits a strong fluorescence emission; in contrast with this partial fluorescence quenching phenomena is observed in its metal complexes. The proposed structures of metal complexes are presented in Figure4. The 1H NMR spectra showed that the calculated number of protons for each functional group in the complexes is equal to the number predicted from the molecular formula. Moreover, the 1H and 13C NMR spectra of the complexes obtained were found to exhibit no additional resonances and thus reflected the purity of the metal complexes.



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*Source: 847071-2013-02-21.xml*